A DICTIONARY OF CHEMICAL SOLUBILITIES INORGANIC THE MACMILLAN COMPANY NEW YORK BOSTON CHICAGO DALLAS 'ATLANTA SAN "FRANCISCO MACMILLAN & CO., LIMITED LONDON BOMBAY CALCUTTA MELBOURNE THE MACMILLAN CO. OF CANADA, LTD TORONTO DICTIONARY OF CHEMICAL SOLUBILITIES INORGANIC FIRST EDITION BY ARTHUR MESSINGER COMEY, PH.D. // * SECOND EDITION ENLARGED AND REVISED BY ARTHUR MESSINGER COMEY, Pn.D. DIRECTOR, EASTERN LABORATORY, E. I. DU PONT DE NEMOURS AND CO. AND DOROTHY A. HAHN, PH.D. PROFESSOR OF CHEMISTRY, MT. HOLYOKE COLLEGE THE MACMILLAN COMPANY 1921 Att rights reserved /ii '*/ MIMINCt O.I"T ( ftTT COPYRIGHT, 1921 MACMILLAN COMPANY Set up and printed Published February, 1921 PREFACE TO FIRST EDITION FOE many years a need has been felt by chemists for a book which shall collect into convenient form for ready reference the various data concerning the solu- bility of chemical substances that have been published from time to time in chemical periodicals and elsewhere. The first mention that can be found of such a plan was made in 1731, when Peter Shaw delivered Chemical Lectures in London, as may be seen from the following: EXTRACTS from PETER SHAW'S Chemical Lectures, publickly read at London in 1731 and 1732. London. Second Edition, London 1755. 8vo. Page 97. Experiment I. That Water as a Menstruum dissolves more of one body and less of another. [He shows that two ounces of water dissolve two ounces of Epsom salt, five drachms of common salt, and eight grains of cream of tartar. Only in the latter case much remained undissolved until boiled.] "It might be proper for the further Improvement of Chemistry and Natural Phi- losophy to form a Table of the Time and Quantity wherein all the known Salts are dissolvable in Water. . . . Such a Table regularly formed might ease the Trouble of re- fining Salts, by shewing at once without future Trial or Loss of Time how much Water each Salt required to dissolve it for Clarification, Filtration, or Crystallization. It would likewise supply us with a ready and commodious Way of separating any Mixture of Salts, by shewing which would first shoot out of the Mixture upon Crystallization. . . . The same Table might also direct us to a ready and commodious Method of separating two Salts without waiting for Crystallization. . . ." It was many years, however, before the scheme suggested by Peter Shaw was put into execution. Professor F. H. Storer published the first work that undertook to carry out the idea in its entirety, in 1864, in a book, which he entitled " First Outlines of a Dictionary of Solubilities of Chemical Substances," and which contained a compilation of nearly all the data on the subject pub- lished before 1860. It was at once recognized as a most valuable contribution to chemical literature; but for many years it has been difficult to obtain this work, as the limited edition which was published was soon wholly exhausted. Since then nothing has appeared on the subject except the brief tabulations found in various reference books, and no attempt has been made to cover the whole subject. It is needless to state that the growth of chemical science since the publication of Professor Storer's book has been so enormous that that work has lost, at least to a great extent, the practical value it possessed thirty years ago. This growth has been indeed so great, and the data which have accumulated since 1860 so far surpass the earlier in volume, that a simple revision of Professor Storer's book was impracticable, and it therefore seemed best to start afresh. A o A rr *r tr vi PREFACE TO FIRST EDITION With the facilities offered by the various scientific libraries at Harvard University, the Massachusetts Institute of Technology, and other libraries in Boston, it has been possible to collect nearly all the data relating to the subject. For the work before 1860 Professor Storer's work has been found invaluable. | The method pursued has been to form a preliminary list of compounds with more or less data by consulting the two most complete works on inorganic chemistry Gmelin-Kraut's "Handbuch der anorganischen Chemie" and Graham-Otto-Michaelis's "Lehrbuch." These statements have been verified and elaborated by consulting the original memoirs in all the periodicals devoted to chemical literature which were obtainable. The ' ' Jahresbericht der Chemie ' ' also has been used extensively in tracing references, but the original memoirs have always been consulted and references given to them when possible. It has been found impracticable to draw any distinction as to reliability between the various data given by different observers. It was manifestly impossible to attempt to verify experimentally the statements of those who have carried on the researches, for the most assiduous labor of many could only cover a small portion of the attested facts. Therefore, even when two statements are directly contradictory, both have been given with the authority for each. The only exception to this has been made when more recent dis- coveries have shown beyond any reasonable doubt the falsity of previous work. In this way some of the older manifestly inaccurate work has been omitted. In a majority of cases the more recent work may be considered to be the more accurate, but this is not the invariable rule. A Synchronistic Table of the more common periodicals is given in the Appendix, whereby it is easy to determine the date of the publication of a research to which reference is made. It may be objected by the practical chemist that most of the work previous to 1850 might well have been omitted, but a great deal of this work possesses at least a historical -value, and often furnishes facts which have not since been verified. Much of the earlier work, when obviously of less importance, has been printed in smaller type. The aim has been to include in this volume all analyzed inorganic substances, that is, all substances which do not contain carbon, but exception has been made in the case of CO2, CO, C$2, the carbonates, cyanides, ferro-cyanides, etc., which are here included. The work has been brought up to March, 1894, when this volume went to press, and the results of researches published since that time are not included in the present edition. It is hoped that this book will fill to some extent the want that has been felt by chemists for a compilation of this nature. While it has been attempted to make the book as free from errors as possible, nevertheless it is naturally im- possible to avoid many mistakes, and the compiler will be very grateful to those who may call his attention to any errors or omissions. A. M. C. CAMBRIDGE, MASS., Aug., 1895. PREFACE TO SECOND EDITION DURING the twenty-five years which have elapsed since the publication of th< first edition of this dictionary, a very large amount of work has been publishe( in chemical periodicals, containing data concerning the solubility of inorgani chemical compounds. As it was impossible for the compiler of the first editioi to devote the time necessary for the collecting of the published data, it wa necessary to employ assistance, and Dr. Dorothy A. Hahn, Professor of Chem istry, Mt. Holyoke College, was engaged for this work. Dr. Hahn has collectec the larger part of the material in this book, which work in spite of its arduou and tedious nature, she has performed in a most painstaking manner. The compilation and arrangement of the data collected by Dr. Hahn, whicl devolved upon the original author, took much time. This, together with diffi culties in printing, caused by the general conditions after the war, has delaye( the publication until the present year, although the work was begun in 1916 and it has only been brought up to January 1st of that year. Since the publication of the first edition of this work, Dr. Atherton Seidell ha: brought out two editions of his book, entitled " Solubilities of Inorganic anc Organic Substances," which covers quite a different field, as he considers onb quantitative data and those only for the commoner substances. Dr. Seidell hai followed the plan in most cases where there are several available solubility determinations of a substance, of selecting and averaging the more reliabli results, and embodying them in tables. Although this undoubtedly facilitate ready reference, it has seemed better to adhere to the original plan of the firs edition, and to publish all the data in the form of the original authorities witl references and dates, so that the user may be at liberty to use his own judgmen in selection. Some few of the tables arranged by Dr. Seidell, however, hav< seemed to possess decided advantages over any other published data and the;; have been incorporated in the present volume. It is desired also to acknowledg< indebtedness to Dr. Seidell's work for certain other tables where the origina sources were not available to the present compilers. The same plan and arrangement used in the first edition has been followec with certain elaboration, however, of the arrangement of data on the solubility of two or more salts in a solvent, which is explained in the Explanatory Preface Data published since the first edition on the cobalt and chromium ammonh compounds and those of the platinum group have been omitted, as it seemec that solubility data on those compounds possessed very little general interest. As stated in the preface of the first edition, while every possible attempt hai been made to avoid errors, it is manifestly impossible to avoid many mistakes ii a work of this nature, and the compiler will be glad to have his attention callec to any errors or omissions. WILMINGTON, Del., Jan., 1921. A. M. C. EXPLANATORY PREFACE IN order to reduce this volume to a convenient size the subject-matter has been abbreviated and condensed as far as seemed compatible with clearness; but it has been the aim not to use any abbreviations which are not at once intelligible without consulting the explanatory table. The more common chemical for- mulae have been universally used, thereby saving a large amount of space without detracting from ready intelligibility to chemists. The solubility of the substance in water is first given, the data being arranged chronologically in the longer articles. Then follow the specific gravities of the aqueous solutions, and also any data obtainable regarding their boiling-points; other physical data concerning solutions are not included. Following this is the solubility of the substance in other solvents first the inorganic acids, then alkali and salt solutions, and finally organic substances. Owing to the great increase of data, published during the last twenty years, on the simultaneous solubility of two or more salts in a given solvent,' it has been found necessary to plan some arrangement, whereby such data can easily be found, and the plan adopted is as follows: The data for the solubility of two salts in a solvent is placed under the salt which comes first according to the alphabetical arrangement in this dictionary, and the order of the data on various salts under the same heading follows the alphabetical order of the salts consid- ered. Thus the data on the solubility of NH 4 Cl+BaCl 2 , NH 4 Cl+CuCl 2 , and NH 4 ClH-PbCl2, and NH^Cl-HNEU^SCX are placed under Ammonium Chloride and arranged in the given order. Certain exceptions have been made to this rule, where the data directly concerns the solubility of a salt in a solu- tion of another salt, in which case, it is placed under the former. Numerous cross references, however, are given, which it is hoped will avoid confusion. In many cases no definite distinction can be drawn between the phenomena of solution and decomposition. At present the theory of solution is in a confused state, and until what really takes place when a substance dissolves is thoroughly understood no distinct line can be drawn. The whole subject is unsettled at the present time; for while many chemists believe in the so-called "dissociation" theory, yet the "hydrate" theory is not without its supporters. It is not my intention to discuss the theoretical side of the question, which has been so well treated in many recent works. It is, however, obvious that the phenomena are essentially different, when, for example, sodium carbonate is dissolved in water, in which case the original salt is deposited on evaporation, and when iron is dissolved in sulphuric acid, and the solution deposits a sulphate of iron. Yet it is still the custom to speak of iron as soluble in sulphuric acid, although it would be much more accurate to say that the sulphuric acid was decomposed by the iron. It has thus been found impracticable to draw a sharp line between solu- EXPLANATORY PREFACE tion and decomposition, and the term " soluble " has in general been used where a solution of some sort is formed by the action of the solvent. The matter of alphabetical arrangement of chemical compounds, in the present somewhat confused state of chemical nomenclature, has been a difficult question to decide. The plan followed has been practically that of the standard Dictionaries of Chemistry, whereby the compounds of metals with one of the non-metallic elements have been classified under the metals, while the salts of the other acids (the oxygen acids so called and some few others) have been arranged alphabetically under the acids. Thus barium chloride is found under barium, while barium chlorate is found under chloric acid. No exception has been made in the case of the rare metals, as is usually the custom in Dictionaries of Chemistry. Double salts are to be found under the word which comes first alphabetically; thus, " common alum," potassium aluminum sulphate, is found under aluminum sulphate as aluminum potassium sulphate (under sulphuric acid), but ammonia chrome alum is found under ammonium sulphate as am- monium chromium sulphate. In the same way the double sulphate and chro- mate of potassium is found under potassium chromate (chromic acid), and not under potassium sulphate (sulphuric acid) . The double chloride of ammonium and magnesium is found under ammonium chloride (ammonium), while the double chloride of potassium and magnesium is found under magnesium chloride (magnesium). An exception is made, however, in the case of double compounds of salts of oxygen acids with salts containing a single non-metallic element, in which case they are always found under the oxygen acid. Thus the double sulphate and chloride of lead, PbSO 4 , PbC^, is found under lead sulphate (sulphuric acid), and not under lead chloride (lead). The above method in some cases widely separates analogous compounds, but it was found to be the only practical way to a strictly alphabetical arrange- ment, which is no necessary in a book containing so many very short articles. The ammonia addition-products furnished another. difficulty. While their nature is more or less definitely understood in the cobalt, platinum, etc., com- pounds, and a definite nomenclature is in general use, there is an absolute lack of anything of the kind in the less definite compounds. It is good usage to speak of cuprammonium compounds, but how shall we designate the analogous cadmium compounds? " Cadmammonium " has not 'yet received the sanction of chemists, and A1C1 3 , NH 3 is a still worse case for naming. I have, therefore, not attempted to name these compounds, but classified them all under the salts to which the ammonia is added, affixing the word ammonia, thus: aluminum chloride ammonia, cadmium chloride ammonia, and also cupric chloride am- monia for the salt now almost universally known as cuprammonium chloride. The ammonia compounds of cobalt, chromium, mercury, and the platinum metals are arranged alphabetically according to their universally accepted names, a list of which i,s given under each of those elements. It has further been necessary to settle arbitrarily the question whether a sub- stance should be considered as a double salt or a salt of a compound acid con- EXPLANATORY PREFACE xi taining one of the metals. For example, " fluosilicates " (or silicofluorides, as some may prefer) is the general name for the double fluorides of SiF 4 and a metal, but this unanimity in usage gradually disappears as the basic elements become more nearly alike, so that it is impossible to draw a line between such compounds and a compound such as the double chloride of magnesium and potassium, for which indeed the name "potassium chloromagnesate " has been proposed. The aim has been in all these cases to follow the best usage rather than make an absolutely homogeneous system of nomenclature out of the exist- ing confusion. In the matter of formulae no attempt at uniformity has been made. Thus in the case above some chemists write the formula of the double chloride of mag- nesium and potassium as KMgCl 3 , others as KC1, MgCl 3 . The form here used has been in most cases that of the author from whom the data are taken. The prefixes mono, di, tri, ortho, pyro, etc., have in general been disregarded in the alphabetical arrangement, and have been printed in italics. Exceptions to this have been made, however, in the cobalt, chromium, etc., ammonium compounds, and in a few others, as dithionic, perchloric, etc., acids. Cross references have been used, so as to prevent any confusion arising from lack of uniformity in this respect. In the Appendix will be found formulae and tables for the conversion of the degrees of various hydrometer scales into specific gravity, and a Synchronistic Table of the Periodicals to which references are most frequently made. ABBREVIATIONS abs . absolute . atmos . atmosphere . b.-pt. boiling-point. comp . compound. cone . concen trated . corr. corrected. cryst. crystallised, crystalline decomp. decompose, decomposes, decomposition, etc. dil. dilute, eutec. eutectic. insol . insoluble . M. a univalent Metal. M in . M ineral . mol. molecule. m.-pt. melting-point, ord. ordinary, n. normal. ppt., pptd., etc. precipitate, pre- cipitated, etc. pt. part, sat. saturated, si. slightly, sol. soluble, sp. gr. specific gravity, supersat. supersaturated. t = temperature in Centigrade degrees, temp. temperature, tr. pt. transition point, vol. volume. ABBREVIATIONS OF REFERENCES A. Annalen der Pharmacie, edited by Liebig and others, 1832-39; continued as Annalen der Chemie und Pharmacie, 1840-73; continued as Justus Liebig's Annalen der Chemie, A. ch. Annales de Chimie et de Physique. Paris. 1st series, 1789-1816, 96 vols ; 2nd series, 1817-40, 78 vols.; 3rd series, 1841-63, 69 vols.; 4th series, 1864-73, 30 vols.; 5th series, 1874-83, 30 vols.; 6th series, 1884-93, 30 vols.: 7th series, 1893-1903, 30 vols ; 8th series, 190^13, 30 vols.; 9th series, 1914 +, 3 vols. Acta Lund. Acta Universitatis Lundensis/or Lunds Universitets Ars-skrift. Lund 1864+ Am. Chemist. The American Chemist. New York, 1870-77. 7 vols. Am. Ch. J. The American Chemical Journal, edited by Remsen. Baltimore, 187&-1913 50 vols. Am. J. Sci. American Journal of Science and Arts, edited by Silliman, Dana, and others. New Haven. 1st series, 1818-45, 50 vols.; 2nd series, 1846-70, 50 vols.; 3rd series, 1871-95, 50 vols.; 4th series, 1896-1915 +, 40 vols. Also numbered consecutively, 190 vols. Analyst. The Analyst. London, 1876-19 15+. 45 vols. Ann. chim. farm. Annali di chimica e di farmacologia. Milan, 1886-90. 5 vols. Ann. des Mines. See Ann. Min. Ann. Min. Annales des Mines. Paris. Ann. Phil. Annals of Philosophy. London. 1st series, 1813-20, 16 vols.; new series, 1821-26, 12 vols. Ann. Phys. See Pogg. and W. Ann. Apoth. Z. Apotheker-Zeitung. Berlin. Arb. Kais. Gesundheitsamt. Arbeiten aus dem Kaiserlichen Gesundheitsamte. Arch. Ne'er. Sc. Archives Ne"erlandaises des Sciences exactes et naturelles. Arch. Pharm. Archiv der Pharmacie, continued from Archiv des Apothekervereins in Norddeutschland, which forms the 1st series. 1st series, 1822-34, 50 vols.; 2nd series, 1835-72, 150 vols.; 3rd series, 1873-94+, 32 vols. Also numbered consecutively, which system is exclusively used after 3rd series, vol. 253 (1915). Arch. sc. Phys. nat. Archives des sciences physiques et naturelles de la Bibliotheque universelle de Geneve. A. Suppl. Annalen der Chemie und Pharmacie. Supplement-Bande. Vol. i. 1861; vol. ii, 1862-63; vol. iii. 1864-65; vol. iv. 1865-66; vol. v. 1867; vol. vi. 1868; vol. vii. 1870; vol. viii. 1872. B Berichte der deutschen chemischen Gesellschaft. Berlin, 1868-1915+. 48 vols. Att. Ace. Line. Atti della reale accademia dei Lincei, rendconditi, etc. B. A. B. Sitzungsberichte der koniglichen preussischen Akademie der Wissenschaften zu Berlin. Belg. Acad. Bull. Bulletin de 1' Academic Royale des Sciences, des Lettres, et des Beaux- Arts de Belgique. Berz. J. B. Jahresbericht iiber die Fortschritte der physischen Wissenschaften, edited by Berzelius. 1822-47. 30 vols. Br. Arch. Archiv des Apothekervereins im nordlichen Teutschland, etc., edited by Brandes. 1st series, 1822-31, 39 vols., corresponds to 1st series of Arch. Pharm. Bull. A.cad. Crac. Bulletin international de I'Acad&nie des Sciences de Cracovie. Bull. Ac. St. Petersb. Bulletin de 1' Academic Impe"riale des Sciences de St. Pe"tersbourg. Bull. Soc. Bulletin des Stances de la Socie'te' chimique de Paris. 2nd series, 1864-88, 50 vols.: 3rd series, 1889-1906, 36 vols.; 4th series, 1907-15+, 18 vols. Bull. Soc. chim. Belg. Bulletin de la Socie"te" chimique Belgique. Bull. Soc. ind. Mulhouse. Bulletin de la Soci6t< industrielle de Mulhouse. 1828-49. 22 vols. Bull. Soc. Min. Bulletin de la socifte" franchise de Mine'ralogie. 1878-1915+. 37 vols. C. A. Chemical Abstracts. American Chemical Society. New York. C. C. Chemisches Centralblatt, continued from Pharmaceutisches Centralblatt. C. B. Miner. Centralblatt fur mineralogie, Geologic und Palseontologie. Berlin. Chem. Ind. Die Chemische Industrie, edited by Jacobsen. Berlin. Chem. Soc. Journal of the Chemical Society of London. 1st series, 1849-62, 15 vols.; 2nd series, 1863-78, 17 vols. ; new series, 1878-19 15+. The vols. are numbered consecutively from 1849. 1878 = vol. 32. Total, 108 vols. xvi ABBREVIATIONS OF REFERENCES Chem.-tech. Centr-Anz. Chemisch-technischer Central- Anzeiger. Chem. Weekbl. Chemiker Weekblad. Chem. Z. See Ch. Z. Chem. Zeitschr. Chemische Zeitschrift. Ch. Gaz. The Chemical Gazette. London, 1843-59. 17 vols. Ch. Kal. Chemiker Kalender, edited 'by Biedermann. Ch. Z. Chemiker Zeitung. Ch. Z. Repert Chemisches Repertorium Beiblatt zur Chemiker-Zeitung. Gothen. Cim. II Cimento. Turin, 1852-54. 6 vols. C. N. The Chemical News. London; 1860-1915 +. 112 vols. Comm. Commentar zur Pharmacopoea germanica by Hager. Berlhi, 1883. Compt. chim. Comptes-rendus mensuels des Travaux chimiques, edited by Laurent and Gerhardt. 1845-51. 7 vols. C. R. Comptes-rendus hebdomadaires des Seances de 1' Academic des Sciences. Paris, 1835-19 15+. 161 vols. Crell. Ann. Chemische Annalen fur die Freunde- der Naturlehre, etc., edited by Crell. 1784-1803. 40 vols. Dansk. Vid. For. Oversigt over det kgl. danske Videnskabernes Selskabs Forhandlinger. Copenhagen. Dingl. Dingler's Polytechnisches Journal, edited by Dingier and others. 1820-1915+ . 330 vols. Edinb. Trans. Transactions of the Royal Society of Edinburgh. 1788-1915+ . 51 vols. Ed. J. Sci. The Edinburgh Journal of Science. 1st series, 1824-29, 10 vols.; 2nd series, 1829-32, 6 vols. Continued as Phil. Mag. Electrochem. Ind. Electrochemical Industry (Oct., 1902, to Dec., 1904) later Electro- chemical and Metallurgical Industry. New York. Elektrochem Z. Elektrochemische Zeitschrift. Berlin. Eng. Min. J. The Engineering and Mining Journal. New York. Gazz. ch. it. Gazzeta chimica italiana. Palermo, 1871-1915+. 45 vols. Gilb. Ann. Annalen der Physik, edited by Gilbert. 1st series, 1799-1808, 30 vols.; 2nd series, 1809-18, 30 vols.; 3rd series., 1819-24, 26 vols. Also numbered consecutively. 76 vols. Continued as Pogg. Gm.-K. Gmelin-Kraut's Handbuch der anorganischen Chemie, 6te Auflage. 1877-1905. 7te Auflage, 1907-1915+. Gr.-Ot. Graham-Otto's ausfiihrliches Lehrbuch der anorganischen Chemie, 5te Auflage, by Michaelis. 1878-89. Jahrb. Miner. Jahrbuch fur Mineralogie, Geologic und Palseontologie. Heidelberg. 1830- 1832. Then. Neues Jahrbuch fur Minerologie. Stuttgart. Jahrb. d. Pharm. Jahresbericht der Pharmacie. J. Am. Chem. Soc. Journal of the American Chemical Society. New York, 1876-1915+. 37 vols. J. Anal. Appl. Ch. The Journal of Analytical and Applied Chemistry, edited by Hart. 1887-93. 7 vols. J. B. Jahresbericht iiber die Fortschritte der Chemie, u. s. w. J. Chim. me"d. Journal de Chimie medicale, de Pharmacie, et de Toxicologie. 1st series, 1825-34, 10 vols.; 2nd series, 1835-44, 10 vols.; 3rd series, 1845-54, 10 vols.; 4th series, 1855-64, 10 vols.; 5th series ; 1865-76. 12 vols. Jena. Zeit. Jenaische Zeitschrift fur Medicin und Naturwissenschaften. J. Pharm. Journal de Pharmacie et de Chimie. Paris. 2nd series, 1815-41, 27 vols.; 3rd series, 1842-64, 46 vols.; 4th series, 1865-79, 30 vols.; 5th series, 1879-94: 6th series, 1895-1909, 30 vols.; 7th series, 1910-15+, 10 vols. J. Phys: Journal der Physik, edited by Gren. 1790-98. 12 vols. Continued as Gilb Ann J. Phys. Ch. The Journal of Physical Chemistry. Ithaca, N. Y. J. pr. Journal fur praktische Chemie, edited by Erdmanix, Kolbe, and v. Meyer. Leipzig 1st series, 1834-69, 108 vols.; 2nd series, 1870-1915 + . 92 vols. J. russ. phys. Chem. Soc. Journal de la Societe" physico-chemique russe. St. Ptersbourg. J. Russ. Soc. Journal of the Russian Chemical Society. St. Petersburg, 1869-1315+. 47 vols. J. Soc. Chem. Ind. Journal of the Society of Chemical Industry. London, 1882-1915+ . 34 vols. J. S. C. I. See above. J. Tok. Chem. Soc. Journal of the Tokyo Chemical Society. Kastn. Arch. Archiv fur die gesammte Naturlehre, edited by Kastner. Nuremberg, 1824- 35. 25 vols. Listy Chemicke*. Listy Chemicke", edited by Preis and others. Prague Lond. R. Soc. Proc. See Roy. Soc. Proc. Lund. Univ . Arsk. Lunds Universitets Ars-skrift. Lund. ABBREVIATIONS OF REFERENCES xvii Dd VerWandter Theile der anderer Wissenschaften. Vienna, M ' A ' A B i;"^ Sit?lll i gsb ?^ chte mathematisch-physikalischen Classe der kgl. bayerischen Akademie der Wissenschaften zu Munchen. Mag. Pharm. Magazin der Pharmacie. 1823-31. 36 vols Mem. Acad. St. PStersb. M^moires de TAcad^mie Imp&iale des Sciences de Saint-Peters- M. Ch. See M. Mem CoUSci. Kyoto. Memoirs of the College of Science, Kvoto. Metall. Metallurgie. Halle. Miner. Jahrb. Neues Jahrbuch fnr Mineralogie, etc. 1833-73. 40 vols Miner. Mag. Mineralogical Magazine. London. Miner. Mitt Mineralogische und petrographische Mitteilungen Wien Momt. Scient. Le Moniteur Scientifique, edited by Quesnesville. Paris. N. Arch. Sc. ph. nat Nouvelles Archives des Sciences physiques et naturelles. Geneva. N. Cim. II nuovo Cimento. Pisa, 1855-61. 14 vols N. Edinb. Phil. J. New Edinburgh Philosophical Journal. 1819-64. 90 vols. N. Jahrb. Miner. Neues Jahrbuch fur Mineralogie. Stuttgart. N. Jahrb. Pharm. Neues Jahrbuch der Pharmacie. 1796-1840. 42 vols. N. J. Pharm. Neues Journal der Pharmacie fur Aerzte, etc., edited by Trommsdorff. 1817-34. 27 vols. N. Rep. Pharm. Neues Repertorium fur Pharmacie. 1852-76. 25 vols. Pharm. Centralbl. Pharmaceutisches Centralblatt. 1830-49. 20 vols. Continued as O. O. Pharm. Era. Pharmaceutical Era. Pharm. J. Trans. Pharmaceutical Journal and Transactions. Pharm. Post. Pharmaceutische Post. Wien. Pharm. Vierteljb. Pharmaceutische Vierteljahresberichte. Pharm. Weekbl. Pharmaceutisches Weekblad. Pharm. Ztg. Pharmaceutische Zeitung. Phil. Mag. The Philosophical Magazine. London. 1st series, 1814-26, 26 vols. ; 2nd series, 1827-32, 11 vols.; 3rd series, 1832-50, 37 vols.; 4th series, 1851-75, 50 vols.; 5th series, 1876-1900, 50 vols.; 6th series, 1901-1915 +, 30 vols. Phil. Mag. Ann. The Philosophical Magazine and Annals of Chemistry, etc. Corresponds to Phil. Mag. 2nd series. Phil. Trans. The Philosophical Transactions of the Royal Society of London. 1665-1915+ . Phys. Rev. The Physical Eeview. Pogg. Annalen der Physik und Chemie, edited by Poggendorf . 1st series, 1824-43, 60 vols. ; 2nd series, 1844-53, 30 vols.; 3rd series, 1854-63, 30 vols.; 4th series, 1864-73, 30 vols.; 5th series, 1874-77, 10 vols. Continued as W. Ann. Polyt. Centralbl. Poly technisches Centralblatt. 1st series, 1835-46, 12 vols.; 2nd series, 1847-73, 30 vols. Proc. Am. A. A. S. Proceedings of the American Association for the Advancement of Science. Proc. Am. Acad. Proceedings of the American Academy of Arts and Sciences. Boston, 1846-19 15+. 50 vols. Proc. Am. Phil. Soc. Proceedings of the American Philosophical Society. Philadelphia. Proc. Chem. Soc. Proceedings of the Chemical Society of London. Proc. K. Akad. Wet. See Ver. K. Akad. Wet. Proc. Soc. Manchester. Proceedings of the Literary and Philosophical Society of Manchester. Proc. Roy. Soc. See Roy. Soc. Proc. Q. J. Sci Quarterly Journal of Science. London, 1816-26. 22 vols. Rass. Min. Rassegna mineraria, metallurgica e chirnica. Real. Ac. Line. Atti,di Reale Accademia dei Lincei. Rome. Rend. Ac. Line. See Att. Ac. Line. Rep. anal. Ch. Repertorium der analytischen Chemie. 1881-87. 7 vols. Rep. Brit. Assn. Adv. Sci. Reports of the Meetings of the British Association for the Ad- vancement of Science. Repert. See Rep. Pharm. Repert. chim. appl. Repertoire de Chimie pure et applique*e. Paris, 1858-63. 9 vols. Rep. Pharm. Repertorium fiir die Pharmacie, edited by Buchner. 1st series, 1815-34, 50 vols.; 2nd series, 1835-48, 50 vols. ; 3rd series, 1849-51, 10 vols. Continued as N. Rep. Pharm. Rev. ge*n. chim. Revue generate de chimie pure et applique"e. Rev. Met. Revue de Metallurgie. Paris. Roy. Soc. Proc. Proceedings of the Royal Society of London. 1832-1915+. 92 vols. xviii . ABBREVIATIONS OF REFERENCES Roy. Soc. Trans. Abstracts of Philosophical Transactions of the Royal Society of London. 1832-54. 6 vols. Continued with Roy. Soc. Proc. R. t. c. Recueil des Travaux chimiques des Pays-Bas. Leiden, 1882-1915+. 34 vols. Russ. Zeit. Pharm. Pharmaceutische Zeitschrift fur Russland. Scheik Verhandel. Scheikundige Verhandelingen en Onderzoekingen, edited by Mulder. Rotterdam, 1857-64. 3 vols. Scher. J. Allgemeines Journal der Chemie, edited by Scherer. 1798-1810. 17 vols. Con- tinued as Schw. J. Schw. J. Journal fiir Chemie und Physik, edited by Schweigger. 1st series, 1811-20, 30 vols.; 2nd series, 1821-30, 30 vols.; 3rd series, 1831-33, 9 vols. Continued as J. pr. Sill. Am. J. American Journal of Science, edited by Silliman, etc. See Am. J. Sci. Sitzungsb. bohms. Gesell. Sitzungsberichte der koniglichen bohmschen Gesellschaft der Wissenschaften in Prag. Storer's Diet. First Outlines of a Dictionary of Solubilities of Chemical Substances, by F. H. Storer. Boston, 1864. Sv. V. A. F. Ofversigt af kongl. Svenska Vetenskaps-Akademien Forhandlingar. Stock- holm. Sv. V. A. H. Kongliga Svenska Vetenskaps-Akademiens Handlingar. Stockholm. Sv. V. A. H. Bih. Bihang till kongl. Svenska Vetenskaps-Akademiens Handlingar. Stock- holm. Techn. J. B. Jahresbericht iiber die Fortschritte der chemischen Technologie, edited by Wagner, Fischer, etc. Trans. Am. Electrochem. Soc. Transactions of the American Electrochemical Society. Philadelphia. Trans. Faraday Soc. Transactions of the Faraday Society. London. Trans. Roy. Soc. Philosophical Transactions of the Royal Society of London. Ver. K. Akad. Wet. Verslag Koninkle Akademie van Wettenschappen, Amsterdam. W. A. B. Sitzungsberichte der mathematisch-naturwissenschaftlichen Classe der kaiser- lichen Akademie der Wissenschaften zu Wien. W. Ann. Annalen der Physik und Chemie, edited by Wiedemann. Continuation of Pogg 1877-1899. 69 vols. 4th series, 1900-1915 +. 48 vols. W. Ann. Beibl. Beiblatter zu Wiedemann's Annalen. Leipzig. Z. anal. Zeitschrift fiir analytische Chemie, edited by Fresenius. Wiesbaden, 1862-1915 + . 54 vols. Z. anorg. Zeitschrift fiir anorganische Chemie, edited by Krtiss. 1892-1915+. 93 vols. Z. B. H. Sal. Zeitschrift fur das Berg, Hiitten, und Salinen-Wesen in dem preussischen Staate. Berlin. Zeit. angew. Ch. Zeitschrift fur angewandte Chemie. Berlin, 1887-19 15+. 29 vols. Zeit. Chem. Zeitschrift fiir Chemie und Pharmacie. 1st series, 1858-64, 6 vols.' 2nd series "N. F.," 1865-71, 7 vols. Zeit. d. allgem. oster. Apothekerv. Zeitschrift des allgemeinen osterreichischen Apotheker- vereins. Zeit. ges. Nat. Zeitschrift fiir die gesammten Naturwissenschaften. Zeit. Krist. Zeitschrift fiir Krystallographie und Mineralogie. 1877-1915+ . 51 vols. Zeit. Pharm. See Russ. Zeit. Pharm. Z. Elektrochem. Zeitschrift fiir Elektrochemie. Halle. Z. Phys. Ch. Zeitschrift fiir physikalische Chemie, edited by Oswald and van't Hoff 1887- 1915+. 90 vols. Z. physiol. Chem. Zeitschrift fiir physiologische Chemie. Strassburg. Z. Ver. Zuckerind. Zeitschrift des Verein der deutschen Zuckerindustrie. A DICTIONARY OF CHEMICAL SOLUBILITIES INORGANIC DICTIONARY OP CHEMICAL SOLUBILITIES INORGANIC Actinium emanation. Solubility coefficient of actinium emanation in H2O at room temp, is 2. If the solubility of actinium emanation in H2O is made = 1, the relative solubility of the emanation in sat. KCl+Aq = 0.9; in cone. H 2 SO 4 = 0.95; in ethyl alcohol = 1.1; in amyl alcohol = 1.6; in benzaldehyde = 1.7; in ben- zene = 1.8; in toluene = 1.8; in petroleum = 1.9; inCS 2 = 2.1 at 18. (Hevesy, Phys. Zeit. 1911, 12. 1221.) Air, Atmospheric. See also Nitrogen and Oxygen. 100 vols. H 2 O at 15 and 760 mm. absorb about 5 vols. atmospheric air. (Saussure.) 1 vol. H 2 O at t and 760 mm. pressure absorbs V vols. atmospheric air reduced to 760 mm. and 0. 0.02471 0.02406 0.02345 0.02287 0.02237 0.02179 0.02128 9 10 11 12 13 0.02080 0.02034 0.01192 0.01953 0.01916 0.01882 0.01851 14 15 16 17 18 19 20 0.01822 0.01795 0.01771 0.01750 0.01732 0.01717 0.01701 (Bunsen's Gasometry.) 1 1. H 2 O absorbs cc. N and O from air at t c and 760 mm. pressure. cc. cc. t N O N+O 16.09 8.62 24.71 5 14.18 7.60 21.78 10 12.70 6.79 19.49 15 11.67 6.25 17.92 20 11.08 5.93 17.01 (Bunsen, Gasometr. Methoden, 2te Aufl. 209, 220.) 1 1. H 2 O absorbs cc. N and O from air at t and 760 mm. pressure (dry). t cc. N cc. O N+O %o 10 15.47 7.87 23.34 33.74 15 13.83 7.09 20.92 33.86 20 12.76 6.44 19.20 ' 33.55 25 11.78 5.91 17.69 33.40 (Roscoe and Lunt, Chem. Soc 55. 568.) 1 1. H 2 O absorbs cc. N and O from air at t and 760 mm. 6.0 6.32 9.18 13.70 14.10 cc. N 19.53 16.34 16.60 15.58 14.16 14.16 cc. O 10.01 8.28 8.39 7.90 7.14 7.05 %o 33.88 33.60 33.35 33.60 33.51 33.24 (Pettersson and Sonde"n, B. 22. 1439.) 1 1. H 2 O absorbs cc. N (0 and 760 mm.) from atmospheric air at t and 760 mm. pressure (dry). cc. N 19.14 18.20 17.34 16.54 15.81 10 12 14 16 18 cc. N 15.14 14.53 13.98 13.48 13.03 20 22 24 25 cc. N 12.63 12.27 11.95 11.81 (Hamberg, J. pr. (2) 33. 447.) 1 1. H 2 O absorbs cc. N from air at t and 760 mm. pressure. cc. N 19.29 17.09 t 10 15 cc. N 15.36 13.95 20 25 cc. N 12.80 11.81 (Dittmar, Challenger Expedition, vol. 1. pt. 1.) AIR, ATMOSPHERIC 1 1. H 2 sat. with air at t c and 760 mm. con- j. -_ f\ f j ' j. _ "no _2iJ ,*/a/\' ^.' V .* . Solubility of atmos. etc. Continued tains cc. \J (.rec 1 .to y, auu fou imn.^. .; t ^T'&mn Nitrogen Temp Oxygen Nitrogen. t cc. O t cc. O t cc. O emp Uxygen (*(* PP CC. CC. 10.187 11 7.692 22 6.114 58 IfV* 3.39 \j\j 6.71 80 1.97 4.03 1 9.910 12 7.518 23 5.999 59 3.34 6.60 81 1.89 3.88 2 9.643 13 7.352 24 5.886 60 3.28 6.50 82 1.81 3.73 3 9.387 14 7.192 25 5.776 61 3.22 6.39 83 1.73 3.57 4 9.142 15 7.038 26 5.669 62 3.16 6.27 84 1.65 3.41 5 8.907 16 6.891 27 5.564 63 3.10 6.16 85 1.57 3.24 6 8.682 17 6.730 28 5.460 64 3.04 6.05 86 1.48 3.07 7 8.467 18 6.614 29 5.357 65 2.98 5.94 87 1.39 2.89 8 8.260 19 6.482 30 5.255 66 2.92 5.82 88 1.30 2.71 9 8.063 20 6.356 . . 67 2.85 5.70 89 1.21 2.52 10 7.873 21 6.233 ... 68 2.79 5.59 90 1.11 2.32 (Winkler, B. 22. 1773.) 69 70 2.73 2.66 5.47 5.35 91 92 1.02 0.92 2.12 1.91 1 vol. H 2 absorbs 0.01748 vol. air at 24.05 and 760 mm. pressure. (Winkler, B. 21. 71 72 73 2.60 2.53 2.47 5.23 5.10 4.98 93 94 95 0.81 0.71 0.60 1.70 1.48 1.25 Composition of the absorbed air between and 24 is 34.91% O and 65.09% N (Bunsen) ; between 15 and 16, 32.17% O and 67.83% N (Konig and Kranch, Z. anal. 19. 259); 32% and 68% N (Regnault); at 0, 35.1% O; 10, 34.8% 0; 20, 34.3% 0; 25, 33.7% O (Winkler, B. 21. 2483). See also Roscoe and 74 75 76 77 78 79 2.40 2.33 2.26 2.19 2.12 2.04 4.85 4.72 4.59 4.45 4.32 4.18 96 97 98 99 100 0.48 0.37 0.27 0.13 0.00 1.01 0.77 0.52 0.27 0.00 (Winkler, B. 1901, 34. 1440.) Lunt, and Pettersson and Sonden, page 1. Absorption of atmospheric air by H 2 O at t Solubility of atmos. oxygen and nitrogen in 1000 cc. H 2 O at 760 mm. pressure (calc.). and 760 mm. pressure. = coefficient of absorption. 1 = " Solubility." (See under oxygen.) Temp Oxygen Nitrogen Temp Oxygen Nitrogen t ft 0i t /3i 1 2 3 4 5 6 7 8 9 CC. 10.19 9.91 9.64 9.39 9.14 8.91 8.68 8.47 8.26 8.06 CC. 18.45 17.99 17.55 17.12 16.71 16.30 15.91 15.54 15.18 14.83 29 30 31 32 33 34 35 36 37 38 CC. 5.33 5.24 5.15 5.07 4.99 4.91 4.83 4.76 4.69 4.62 CC. 10.30 10.15 9.99 9.83 9.67 9.52 9.37 9.22 9.08 8.94 5 10 15 20 25 30 35 40 45 KA 3.02881 2543 2264 2045 1869 1724 1606 1503 1418 1351 19Q7 3.02864 2521 2237 2011 1826 1671 1539 1420 1315 1224 1 1 d.n 55 60 65 70 75 80 85 90 95 100 0.01253 1216 1182 1156 1137 1126 1119 1113 1109 1105 0.01059 0978 0892 0801 0705 0600 0481 0343 0185 0000 10 7.87 14.50 39 4.55 8.81 ou l.A\J 1 114:U 11 7.69 14.19 40 4.48 8.67 (Winkler, B. 1901, 34. 1409.) 12 7.52 13.8k } 41 4.42 8.55 13 7 35 1361 42 4.35 8.43 Sea-water absorbs less O and N from air 14 i. 19 13.33 43 4.28 8.31 than pure H 2 O, but the ratio between O and N 15 7.04 13.07 44 4.22 8.20 remains constant. In sea-water sat. with air 16 6.89 12.83 45 4.15 8.09 at 6.22 the oxygen was 33.50% of the total 17 6.75 12.57 46 4.09 7.97 gas absorbed. (Pettersson and Sonde"n.) 18 6.61 12.34 47 4.03 7.87 1 1. sea-water absorbs cc. N and O from air 19 6.48 12.12 48 3.97 7.76 at t and 760 mm. pressure. 20 6.35 11.91 49 3.91 7.65 21 6.23 11.71 50 3.85 7.55 t cc. N CC. O N+0 % o 00 fi in UX.r > 51 3.79 7 4V mm 23 U \\j 5.98 *O 3 . 9W0 3 +7H 2 0. Not sol. in acids when dry. Somewhat decomp. by boiling with cone. HC1, HNO 3 or aqua regia. (Daniels, J. Am. Chem. Soc. 1908, 30. 1848.) Copper aluminicotungstate, 2CuO, A1 2 3 , Sol. in large quantities of H 2 O. (Daniels, J. Am. Chem. Soc. 1908, 30. 1847.) Meicurous aluminicotungstate, 5Hg 2 O, A1 2 O 3 , 9WO 3 . SI. sol. in H 2 O. Sol. in HNO 3 (1:5). (Dan- iels, J. Am. Chem. Soc. 1908, 30. 1849.) Zinc aluminicotungstate, IJ^ZnO, A1 2 O 3 , 9WO 3 +8H 2 O. Insol. in H 2 O. (Daniels, J. Am. Chem. Soc. 1908, 30. 1850.) Znp, A1 2 3 , 9WO 3 +20H 2 O. Sol. in H 2 O. (Daniels.) Aluminum, Al. Less easily attacked than ordinary metals (iron, copper, lead, zinc, tin) by air, H 2 O, wine, beer, coffee, milk, oil, butter, fats, etc. Vinegar dissolves 0.349 g. from a sq. decimetre in 4 months, and 5 % NaCl+Aq, only 0.045 g. in the same time. (Ballaud, C. R. 114. 1536.) The action of various substances contained in foods and drinks on compact Al as it occurs in utensils is very slight. Hard or soft water, whether cold or hot, showed no action in 8 days; 1 % solutions of tartaric, tannic, and acetic acids had no action in same time, also 5 % boric, carbolic, and salicylic acids. 4 % and 10 % acetic acid dissolved only 0.4 mg. of Al, while 10 % acetic acid dissolved 2.1 mg. from a roughened piece of Al foil in 8 days. 1 % soda solution dissolved 15 mg. in 8 days. (Rupp, Dingl. 283. 119.) Similar results were obtained by Arche. (Dingl. 284. 255.) Liquids which are ordinarily contained in f GOG'S and drinks do not attack sheet Al ex- cept in a very small degree. The following losses in weight in mg. by the action of the given liquids on 100 sq. centimetres sheet aluminum for 6 days were obtained : Liquids Loss in mg. Claret Hock Brandy . 5 % alcohol 5 % tartaric acid+Aq . 1% 5 % acetic acid-|-Aq 1 07 " " l/c 2.84 3.27 1.08 0.61 1.69 2.58 3.58 4.38 ALUMINUM, Liquids Loss in mg. 5 % citric acid+Aq 2.15 1 % - 1.90 5 % lactic acid+Aq 4.77 5 % butyric acid+Aq . Coffee ' 1.31 0.50 Tea . Beer 4 % boric acid+Aq . . ' 1.77 5 % carbolic acid+Aq . 0.23 1 % - 0.49 ^/i % salicylic acid + Aq , . ( f . 6.35 (Lunge, C.N. 65. 110.) The apparent solubility of this metal in H 2 O is due to the presence of minute quan- tities of Is 1 a. Absolutely pure Al does not lose any weight to H 2 O and the H 2 O remains perfectly clear. Also dil. acids remain per- fectly clear. (Moissan, C. R. 1895, 121. 794-98; C. C. 1896, 1. 193.) SI. attacked by H 2 O at 80. (W. Smith, J. Soc. Chem. Ind. 1904, 23. 475.) Easily sol. in dil. or cone. HCl+Aq, whether hot or cold; also in HBr. HI, or HF+ Aq. Insol. in dil. H 2 S0 4 + Aq (de la Rive) ; si. attacked by cold, easily by hot cone. H 2 SO 4 . Not attacked by HNO 3 +Aq even when cone, and boiling (Wohler); easily sol. in dil. H 2 SO 4 , or HNO 3 +Aq in vacuo (Weeren, B. 24. 1798) ; slowly sol. in 27 % HNO 3 +Aq, 100 com. HNO 3 +Aq requiring 2 months to dissolve 2 g. Al (Montemartini, Gazz. ch. it. 22. 397); very si. sol. in most organic acids, but solubil- ity is increased by presence of NaCl. Not attacked by dil. or cone. HNO 3 at ord. temp, but attacked by hot HNO 3 . Attacked by H 3 PO 4 . (Smith, J. Soc. Chem. Ind. 1904, 23. 475.) Completely sol. at 100 in two hours in HNO 3 , sp. gr. 1.15-1.46. (Stillman, J. Am Chem. Soc. 1897, 19. 714.) Very easily sol. in HNO 3 (contrary to the usual statement in text-books). (Woy, C. C 190 , Jl.94.) Slowly attacked by HNO 3 +Aq (20-25 %) at 25-30. (Deventer, Chem. Weekbl. 1907, 4. 69.) Dil. HNO 3 or H 2 SO 4 does not attack Al on account of formation of layer of gas. Ac- tion is increased by vacuum. Solutions of metallic chlorides, the metal of which is insol. and attaches itself to the Al (Pt, Au, Cu, Hg) increase the solubility, but when metal is soluble in the acid (Fe, Zn, etc.), there is no increase of solubility. (Ditte, C. R. 1890, 110. 573.) Violently attacked by dil. or cone. H 3 PO 4 + Aq. (Winteler.) Not attacked by solution of HC1 in liquid HCN. (Kahlenberg, J. phvs. Chem. 1902, 6. 662.) Very easily sol. in cone, or dil. KOH, or NaOH+Aq. Slowly attacked by NH 4 OH + (Wohler); sol. in BaO 2 H 2 +Aq (Beck- mann, J. pr. (2) 26. 385) ; slowly sol. in CaO 2 H 2 +Aq. Sol. in excess of 10 % KOH+Aq and in NaOH and LiOH+Aq; sol. in hot cone. Ba(OH) 2 , Sr(OH) 2 and Ca(OH) 2 +Aq. (Allen, Am. Ch. J. 1900, 24. 304-331.) Attacked by hot cone. NH 4 OH+Aq. (Smith, J. SocfChem. Ind. 1904, 23. 475.) SI. attacked by sulphates, or nitrates +Aq, but all chlorides, bromides, and iodides, except those of the alkalies and alkaline earths, even AlCls+Aq, dissolve the metal. Insol. in alum, or in NaCl+Aq, but sol. in alum+ NaCl+Aq. (Tissier, C. R. 41. 362); sol. in NaCl+Aq (Deville, A. ch. (3) 43. 14); sol. in neutral FeCl 3 +Aq in vacuo. (Weeren, B. 24. 1798.) Violently attacked by CuCl 2 + Aq. (Tommasi, Bull. Soc. (2) 37. 443.) Rapidly sol. in K 2 S 2 O 8 +Aq, more slowly sol. in (NH 4 ),S,O 8 +Aq. (Levi, Gazz. ch. it. 1908, 38. (1) 583.) Attacked by (NH 4 ) 3 PO 4 +Aq. SI. attacked by NaNO 3 +Aq or KNO 3 +Aq at 100. (Smith, J. Soc. Chem. Ind. 1904, 23. 475.) Not affected by NH 4 NO 3 +Aq. (Hodgkin- son, C. N. 1904, 90. 142.) Attacked by POC1 3 at 100. (Renitzer, B. 13. 845.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 64. 674.) Attacked by NOC1. (Sudborough, Chem. Soc. 1891, 59. 659. 92 %alcohol attacks Al less than H 2 O. Pure Al is attacked less than commercial. (Hugou- nenq, J. Pharm. 1895, (6) 1. 537.) Sol. in organic acids containing chlorides. (Smith, J. Soc. Chem. Ind. 1904, 23. 475.) Acetic, tartaric and citric acids attack Al only at first. Metal is covered by layer of hydrox'de but on addition of haloid salts, gradual solution ensues. (Ditte, C. R. 1898, 127. 919.) Not attacked bv sugar+Aq. (Klein, C. R. 102. 1170.) Aluminum arsenide. Decomp. by H->O with evolution of AsH 3 . (Wohler, Pogg. 11. 160.) Decomp. by H 2 O. (Fonzes-Diacon, C. R. 1900, 130. 1315.) Aluminum boride, A1 2 B 4 . Very slowly sol. in hot cone. HCl+Aq, and hot NaOH+Aq, but easily in moderately strong warm HNO 3 +Aq. (Hampe, A. 183. A1 2 B 24 . Not attacked by HC1, or KOH + Aq. Scarcely attacked by boiling H 2 SO 4 . Hot cone. HNO 3 +Aq dissolves gradually but completely. (Hampe, 1. c.) Aluminum borocarbide, A1 3 C 2 B 48 . Insol. in H 2 O, HCl+Aq, H 2 SO 4 +Aq, or ALUMINUM CHLORIDE KOH+Aq; slowly sol. in hot cone. HNO 3 + Aq. (Hampe, 1. c.) Aluminum bromide, AlBr 3 . Anhydrous. Dissolved by H 2 O with great violence and evolution of much heat. Very sol. in alcohol. More sol. in CS 2 than A1I 3 . (Weber, Pogg. 103. 264.) Sol. in SOC1 2 . (Besson, C. R. 1896, 123. 884.) Sol. in C 2 H 5 Br. (Plotnikoff, G. C. 1902, II. 617.) Sol. in acetone. (Naumann, B. 1904, 37. 4328); (Eidmann, C. C. 1899, II. 1014.) Solubility of AlBr 3 in organic liquids. Aluminum perbromide carbon bisulphide, AlBr 3 , Br 4 , CS 2 . Sol. in ether, ethyl bromide, ethylene brom- ide and benzene; decomp. by H 2 O. (Plot- nikoff, J. Russ. phys. Chem. Soc. 1901, 33. 91; C. C. 1901, I. 1193.) 2AlBr 3 , Br 4 , CS 2 . Sol. in ether and benzene; insol. in petroleum ether. (Plotnikoff, I. c.) Aluminum bromochloride, AlCl 2 Br. Deliquescent . Somewhat less violently dis- solved by H 2 O than is AlBr 3 . (v. Bartal, Z. anorg. 1907, 55. 154.) +6H 2 O. Deliquescent. Sol. in H 2 with- out evolution of heat. (v. Bartal, Z. anorg. Solvent t ,8 o t |8 t ! JLJ7LM, UU. J.UU. ) Aluminum carbide, A1 4 C 3 . ^ ^ 3 Decomp. by fused KOH at 100; insol. in a a fuming HNO 3 in the cold; decomp. by H 2 O, and dil. acids. (Moissan, Bull. Soc. 1894, (3) 11. 1012; C. R. 1894, 119. 16-20.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) 48 45 42 8.5 13.8 130 140 142 43.2 48.4 50 50 38 50 66.0 67.2 70.7 38 18.3 140 52.1 60 74.2 50 21 130 54.5 70 78.3 Aluminum chloride, basic, Al 6 Oi 4 Hi , HC1. Benzo- 60 23.4 120 56.7 80 83.3 Easily sol. in H 2 O. (Schlumberger, Bull. phenone 70 25.7 110 58.6 85 86.7 Soc. 1895, (3) 13. 56.) 80 90 28.1 30.6 100 90 60.3 61.7 90 93 90.7 94.8 Aluminum chloride, A1C1 3 . 100 33.4 80 62.9 96 100 Anhydrous. Very deliquescent. Sol. in 110 36.3 70 64.1 H 2 O with a hissing noise and evolution of 120 39.6 60 65.1 heat. Solution of A1C1 3 in H 2 loses HC1 on evaporation, and A1C1 3 is finally wholly con- 10 o 20 33.9 70 72.7 verted into A1 2 O 3 . 6 8.4 30 40 1 80 82 3 Sol. in 1.432 pts. H 2 O at 15. (Gerlach.) Ethylene 2 40 47.2 90 92.2 AlCl 3 +Aq containing 19.15 % A1C1 3 boils bromide 2 10 22.9 28.4 50 60 55.1 63.6 96 100 at 103.4; AlCl 3 +Aq containing 38.3 % A1C1 3 boils at 112.8. (Gerlach.) Sp. gr. of AlCl 3 +Aq at 15. 0.5 85 47 40 72.6 c Sp. gr. C1 Sp. gr. 2 5 6 5 90 50 8 60 79.4 /o 5 13.0 80 52.8 70 83.9 1 1.0072 22 1 . 1709 Benzoyl 10 17.4 60 56 80 89.2 2 .0144 23 1 . 1795 chloride 30 24.6 40 59.5 90 95.8 3 .0216 24 1 . 1881 50 31.8 20 63.1 96 100 4 .0289 25 1 . 1968 70 40 7 65,5 5 .0361 26 1.2058 80 44.3 20 67.9 6 .0435 27 1.2149 (Menschutkin, Ann. Inst. Pol. P.-le-Gr., 7 8 .0510 .0585 28 29 1 . 2241 1.2331 13. 1.) 9 .0659 30 1.2422 +6H 2 O. Very sol. in H 2 O. W +15H 2 O. (Panfiloff, J. B. 1895. 785.) 10 11 12 .0734 .0812 .0890 31 32 33 1.2518 1.2615 1.2711 Aluminum antimony bromide, 2AlBr 3 , 5SbBr 5 +24H 2 O. 13 14 .0968 .1047 34 35 1.2808 1.2905 Hygroscopic. Decomp. by H 2 O. (Wein- land, B. 1903, 36. 258.) 15 16 17 .1125 .1207 1.1290 36 37 38 1.3007 1.3109 1.3211 Aluminum potassium bromide, AlBr 3 , KBr. 18 1.1372 39 1.3313 Sol. in H 2 O. (Weber, Pogg. 103. 267.) 19 1.1455 40 1.3415 Aluminum bromide ammonia, AlBr 3 , zNH 3 . 20 21 1 . 1537 1 . 1632 41 1.3522 Decomp. by H 2 O. (Weber, Pogg. 103. 267.) (Gerlach, Z. anal. 8. 281.) ALUMINUM AMMONIUM CHLORIDE Sp. gr. at 20 of AlCl 3 +Aq containing mg. mols. A1C1 3 per liter. M. Sp. gr. 0.01 1.00104 0.025 1.00282 0.05 1.00588 0.075 1.00870 0.10 1.01158 0.25 1.02911 0.55 1.05706 1.0 1.11054 1.5 1.16308 2.0 1.21378 (Jones & Pearce, Am. Ch. J. 1907, 38. 726.) Sol. in 1 pt. strong alcohol at 12.5 (Wen- zel); easily sol. in ether; si. sol. in CS 2 ; insol. in ligroine or benzene. Difficultly sol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 26.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) Insol. in CS 2 at ord. temp. (Arctowski, Z. anorg. 1894, 6. 257.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in methylal. (Eidmann, C. C. 1899, II. 1014.) Solubility of A1C1 3 in organic liquids. <* 1 |2 Solvent t i| t ^ t 48 44 8.5 130 125 43.2 48.4 130 140 66.0 67.2 39.5 13.8 120 50 150 70.7 50 18.3 110 52.1 160 74.2 60 21. 100 54.5 170 78.3 Benzo- 70 23.4 90 56.7 180 83.3 phenone 80 25.7 80 58.6 185 86.7 90 28.1 70 60.3 190 90.7 100 30.6 60 61.7 192 94.8 110 33.4 80 62.9 194 100 120 36.3 100 64.1 125 39.6 120 65.1 -0.5 60 33.0 80 52.9 -4 7.9 70 37.5 70 55.1 Benzoyl -7.5 12.7 80 42.2 60 57.2 chloride 14.1 90 47.1 40 61.0 20 18.8 93 48.7 40 25.0 90 50.6 (Menschutkin, Ann. Inst. Pol. P.-le-Gr.. 13. 1.) +6H 2 O. Very deliquescent; very sol. in H 2 O. Sol. in 0.25 pt. H 2 O. (Thomson.) Sol. in 2 pts. abs. alcohol at ordinary temp., and 1.5 pts. at b.-pt. (Thomson.) Completely insol. in a solution of ether in H 2 O sat. with HC1. (Havens, Am. J. Sci. 1898, (4) 6. 46. Aluminum ammonium chloride, Aids, NH4C1. (Baud, A. ch. 1904, (8) 1. 46.) Aluminum antimony chloride. See Chlorantimonate, aluminum. Aluminum barium chloride, 2A1C1 3 , BaCl 2 . (Baud, C. R. 1901, 133. 869.) Aluminum calcium chloride, basic. 3CaO, CaCl 2 , A1 2 3 +10H 2 0. (Steinmetz, Z. phys. Ch. 1905, 62. 466.) lOCaO, CaCl 2 , 6A1 2 O 3 . Slowly decomp. by boiling H 2 O. (Gorgeu, Bull. Soc. 1887, (2) 48. 51.) Aluminum calcium chloride, 4A1C1 3 , SCaCU (Baud, A. ch. 1904, (8) 1. 51.) Aluminum nitrosyl chloride, A1C1 3 , NOC1. Deliquescent, and decomp. by H 2 O. (Weber Fogg, 118. 471.) Aluminum palladium chloride, A1C1 3 , PdCl 2 + 10H 2 0. See Chlorbpalladite, aluminum. Aluminum phosphorus pentachloride, A1C1 3 , PC1 5 . Decomp. violently by H 2 O. (Baudrimont.) Aluminum phosphoryl chloride, A1C1 3 , POC1 3 . Deliquescent. Sol. in H 2 O with decomp. Sol. in warm POC1 3 , from which it separates on cooling. (Casselmann, A. 98. 220.) Aluminum platinum chloride, A1C1 3 , PtCl 2 + 15H 2 O. See Chloroplatmite, alumhium. Aluminum potassium chloride, A1C1 3 , KC1. Slowly deliquescent. Sol. in H 2 O with evolution of heat and decomp. (Degen, A. 18. 332.) Alumhium selenium chloride, 2A1C1 3 , SeCl*. Sol. in H 2 with evolution of heat 'and separation of traces of selenium. (Weber, Pogg. 104. 427.) Aluminum sodium chloride, A1C1 3 , NaCl. Much less deliquescent than A1C1 3 . Sol. in H 2 O with evolution of heat. Upon evaporat- ing, NaCl crystallises out. (Wohler.) Aluminum strontium chloride, 4A1C1 3 , 3SrCl 2 . (Baud, A. ch. 1909, (8) 1. 52.) Aluminum sulphur chloride, 2A1C1 3 , SC1 4 . Decomp. by H 2 O with evolution of much ALUMINUM MAGNESIUM FLUORIDE 9 heat and separation of some sulphur. (Weber Pogg, 104. 421.) A1C1 3 ,SC1 4 . Decomp. by H 2 O. (Ruff, B 1901, 34. 1757.) Aluminum tellurium chloride, 2A1C1 3 , TeCl 4 . Very sol. in dil. H 2 SO 4 + Aq. (Weber, J. pr 76. 313.) Aluminum chloride ammonia, A1C1 3 , NH 3 . Sol. in H 2 O. (Rose, Pogg, 24. 248.) Completely sol. in H,O. (Baud, C. R. 1901, 132. 135.) A1C1 3 , 2NH 3 . Very hygroscopic. (Still- man, Am. Ch. J. 1895, 17. 750.) A1C1 8 , 3NH 3 . Decomp. by H 2 O. AlClj, 5NH 3 . M. pt. 380. (Baud, C. R. 1901, 132. 135.) A1C1 3 , 6NH 3 . Decomp. by H 2 O. (Still- man, Am. Ch J. 1895, 17. 752.) Somewhat hygroscopic. (Baud, C. R. 1901, 132. 135.) Aluminum chloride nitric oxide, [2A1C1 3 , NO. Very hygroscopic. Decomp. rapidly in the air. Sol. in KOH+Aq. (Thomas, C. R. 1895, 121. 130.) Aluminum chloride phosphine, 3A1C1 3 , PH 3 . Decomp. by H 2 O or NH 4 OH+Aq. (Rose Pogg, 24. 2950 Aluminum chloride hydrogen sulphide. Deliquescent. Decomp. by H 2 O or NH 4 OH +Aq. (Wohler.) Aluminum chloride sulphur dioxide, A1C1 3 , SO 2 . Decomp. by H 2 O, alcohol, or benzene. (Adrianowski, B. 12. 688.) 2A1C1 3 , SO 2 . (Baud, A. ch. 1904, (8) 1. 32.) Aluminum cobalt, Co 3 Al 3 . Sol. in strong acids. (Brunck, B. 1901, 34. 2734.) Aluminum copper, Cu 4 Al 9 . Sol. in aqua regia; decomp. by HC1. (Brunck, B. 1901, 34. 2733.) Aluminum fluoride, A1F 3 . Anhydrous. Not attacked by H 2 O or acids, and only very slightly by boiling cone. H 2 SO 4 . Insol. in boiling KOH+Aq. (Deville, C. R. 42. 49.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) + ^H 2 O. Insol. in H 2 O. SI. sol. in HF. (Baud, C. R. 1902, 135. 1104.) -f-H 2 O. Completely but only sparingly sol. in H 2 O. (Mazzuchelli, Real. Ac. Line. 1907, (5) 16, I. 775; Chem. Soc. 1907, 92, (2). 549.) +3^H 2 O. Two modifications: (1) Easily sol. in H 2 O. Sol. in HF. (2) Insol. in H 2 O. SI. sol. in HF. (Baud, C. R. 1902, 135. 1104.) -f 7H 2 O. Sol. in H 2 O. (Deville, A. ch. (3) 61. 329.) Min. Fluellile. +83/2H 2 0. Very efflorescent. Sat. solu- tion contains 3.85 g. A1F 3 per 100 g. at 11 and 1.2 g. at - 0.2. (Mazzucchelli, Real. Ac. Line. 1907, (5) 16, I. 775; Chem. Soc. 1907, (2), 92. 549.) Aluminum hydrogen fluoride, 3A1F 3 , 2HF + 5H 2 O. Sol. in H 2 0; precipitated by alcohol. (Deville.) 2A1F 3 , HF+5H 2 O. (Deville, A. ch. (6) 61. o29.) Aluminum ammonium fluoride, A1F 3 , NH 4 F. Somewhat sol. in H 2 O; insol. in H 2 O con- taining NH 4 OH or NH 4 F. (Berzelius, Pogg. 1. 45.) A1F 3 , 2NH 4 F+1.5H 2 0. Sol. in 100 pts. H 2 O at 16. (Baud, C. R. 1902, 135. 1338 ) A1F 3 , 3NH 4 F. Nearly insol. in H 2 O; easily sol. in dil. acids. (Petersen, J. pr. (2) 40. 35.) Quite easily sol. in H 2 O, but insol. in NH 4 F+Aq. (Helmholt, Z. anorg. 3. 129.) Aluminum barium fluoride. Apparently not obtained in pure state. (Roder.) Aluminum calcium fluoride, A1F 3 , CaF 2 -f-H 2 O. Min. Evigtokite. Aluminum calcium sodium fluoride, A1F 3 , CaF 2 , NaF+H 2 0. Min. Pachnolite. Aluminum cobaltous fluoride, A1F 3 , CoF 2 + 7H 2 0. Sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 272.) Aluminum cupric fluoride, 2A1F 3 , CuF 2 . Very slowly but completely sol. in H 2 O. (Berzelius.) A1F 3 2CuF 2 + llH 2 O. Sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 272-76.) 2A1F 3 , 3CuF 2 + 18H 2 O. Sol. in dil. HF + Aq. (Weinland.) Aluminum cupric hydrogen fluoride, A1F 3 , CuF 2 , HF+8H 2 0. Efflorescent in the air. Sol. in dil. HF + Aq. (Weinland, Z. anorg. 1899, 22. 272.) Aluminum iron (ferrous) fluoride, A1F 3 , FeF 2 +7H 2 O. SI. sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 270.) Aluminum lithium fluoride. Insol. in H 2 O. (Berzelius.) Aluminum magnesium fluoride. 2A1F 3 , MgF 2 (?). (Roder.) 10 ALUMINUM NICKEL FLUORIDE Aluminum nickel fluoride, A1F 3 , NiF 2 +7H 2 O. SI. sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 271.) Aluminum potassium fluoride, A1F 3 , 3KF. Very si. sol. in acid solutions, and still less in H 2 O. (Gay-Lussac and Thenard.) A1F 3 , 2KF. As above. Aluminum silicon fluoride. See Fluosilicate, aluminum. Aluminum sodium fluoride. 2A1F 3 , 3NaF. Min. Chiolite. A1F 3 , 2NaF. Min. Chodneffite. A1F 3 , 3NaF. Min. Cryolite. SI. sol. in H 2 O. Insol. in HCl+Aq. Decomp. by H 2 SO 4 , or by boiling with NaOH+Aq. Aluminum strontium fluoride. As the Ba salt. (Roder.) Aluminum thallous fluoride, 2A1F 3 , 3T1F. Ppt. SI. sol. in H 2 O. (Ephraim, Z. anorg. 1909, 61. 243.) Aluminum zinc fluoride, A1F 3 , ZnF 2 +7H 2 O. Sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 272.) 2A1F 3 , ZnF 2 . Slowly but completely sol. in H 2 O. (Berzelius.) Aluminum hydroxide, A1 2 O 3 , H 2 O =A1 2 2 (OH) 2 . Dehydrated by cone, acids, without dissolv- ing. (Becquerel, C. R., 67. 108.) Min. Diaspore. Insol. in HCl+Aq, and not attacked by boiling cone. H 2 SO 4 , unless it has been ignited. A1 2 O 3 , 2H 2 O=A1 2 O(OH) 4 . Pptd. Al hy- droxide, when boiled twenty hours with H 2 O is insol. in acids and alkalies, and has the above composition. (St. Gilles, A. ch. (3) 46. 57.) Min. Bauxite. Soluble modifications -(a) M eta-aluminum hydroxide From basic Al acetate. Sol. in H 2 O and more readily in HC 2 H 3 O ? . The aqueous solution is coagulated by traces oi alkalies, many acids, and salts, while other acids and salts have no effect . Thus, 1 pt H 2 SO 4 in 1000 pts. H 2 O, added to 7000 pts. of above solution containing 20 pts. A1 2 O 3 , con- verts the liquid into a nearly solid mass Citric, tartaric, oxalic, chromic, molybdic racemic, suberic, salicylic, benzoic, gallic lactic, cinnamic, butyric, valeric, camphoric picric, uric, meconic, comenic, and hemipini< acids act in the same way. HC1 and HNO ; have far less action, 600 mols. being necessary to produce the same effect as 1 mol. H 2 SO 4 while acetic, formic, boric, arsenious, pyro- meconic, and opianic acids do not coagulate he solution, except when moderately cone. _ pt. KOH in 1000 pts. H 2 O coagulates 9000 pts. of the solution. NaOH, NH 4 OH, and Ua(OH) 2 have the same effect. The solution is not coagulated by acetates, unless added in large quantity, and even then the ppt. is redissolved when treated with 3 2 O Nitrates and chlorides coagulate with difficulty; Na 2 SO 4 , MgSO 4 , and CaSO 4 +Aq, lowever, have as strong an action as a liquid containing the same amount of H 2 SO 4 . A ;easpoonful of the solution introduced into ;he mouth solidifies at once from the action of the saliva. The ppt. formed by acids is not sol. in an ecessx of the acid, but by the ong continued action of cone. H 2 S0 4 , espe- cially if hot, the ppt. is dissolved; boiling cone. HCl+Aq also dissolves it, but less read- ily than H 2 S0 4 . The ppt. is sol. in boiling cone. KOH+Aq. The residue, when the solution is evaporated at 100, has composi- tion A1 2 O 3 , 2H 2 0, and is insol. in acids. (Crum, Chem. Soc. 6. 225.) (b) By Dialysis. Sol. in H 2 O, from which it is separated by extremely small amounts of various substances, as acids, ammonia, salts (especially K 2 S0 4 ), caramel, etc. An excess of acid dissolves the coagulum. If the solu- tion contains 0.5% A1 2 O 3 or less, it may be boiled without change, but the hydroxide separates out suddenly when it is reduced to ^2 its vol., and even very dil. solutions gela- tinise spontaneously in a few days. The solution is not coagulated by alcohol or sugar. (Graham, A. 121. 41.) A1 2 O 3 ,3H 2 O=A1(OH) 3 . Crystallised. Diffi- cultly sol. in acids and alkalies. (Cossa, N. Cim. (2) 3. 228.) Insol. in boiling HCl+Aq. (Wohler, A. 113. 249.) SI. sol. in KOH+Aq; nearly insol. in cold H 2 SO 4 , HC1, HNO 3 +Aq; verv slowly sol. in hot HCl+Aq, more readily in hot H 2 SO 4 . (v. Bonsdorff, Pogg. 27. 275.) a-modification. Unstable. Changes into jS-modification. Sol. in N-H 2 SO 4 at ord. temp. Sol. in N-NaOH and in hot NaOH of concentration 5Na 2 O, 100H 2 O. (Russ, Z. anorg. 1904, 41. 226.) /3-modification. Insol. in N-H 2 SO 4 at ord. temp. Difficulty sol. in warm N-NaOH, but easily sol. in hot NaOH of concentration 5Na 2 O, 100H 2 O. Its solubility in NaOH in- creases with increase in concentration of the hydroxyl ions. (Russ.) 5-modification. Easily sol. in cone. H 2 SO 4 ; only si. sol. in HC1, HNO 3 or acetic acids, or in alkali +Aq. (Tommasi, C. C. 1905, II. 605.) Min. Gibbsite. Sol. in HCl+Aq, and dil. H 2 SO 4 +Aq. Readily sol. in cone. KOH, and NaOH+Aq. Precipitated. Completely insol. in H 2 O or H 2 CO 3 +Aq. Easily sol. in acids when freshly pptd., but solubility diminishes on standing Easily sol. in KOH or NaOH+Aq. (Son- nenschein.) ALUMINUM MERCURIC IODIDE 11 Herz (Z. anorg. 25. 155) found that alum- inum hydroxide which has been dried in a vacuum dessicator requires for solution in NaOH-j-Aq. 3 atoms Na to 1 atom Al. Slade (Z. Elektrochem. 1911, 17. 261) was unable to obtain this result . Herz says Slade' s error is due to insufficient shaking of the solu- tion. (Herz, Z. Elektrochem. 1911, 17. 403.) New solubility determinations verify the statement of Herz (Z. anorg. 25, 155) that the solubility of A1(OH) 3 in NaOH+Aq is pro- portional to the concentration of NaOH. They do not, however, verify his statement that the ratio Na : Al in the solutions is al- ways 3 : 1, for the author finds that the ratio Na : Al varies from 2 : 1 to 10 : 1 depending on the conditions of precipitation and the method and duration of drying of the A1(OH) 3 . (Slade, Z. Elektrochem, 1912, 18. 1.) SI. sol. in NH 4 OH+Aq when freshly pptd., but presence of NH 4 salts diminish its solu- bility, and it separates out completely after long standing. (Fresenius.) Somewhat sol. in NH 4 OH+Aq, the more readily the larger the vol. of H 2 O. Somewhat sol. in (NH 4 ) 2 CO 3 +Aq, but less than in NH 4 OH+Aq. SI. sol. in dil. NH 4 Cl+Aq, unless that salt be in large excess. It is finally wholly pptd. if allowed to stand several days. 18752 pts. NH 4 OH+Aq (4 % NH 4 OH) dis- solve an amt. of A1(OH) 3 corresponding to one pt. A1 2 O 3 ; NH 4 C1 prevents this solubility al- most completely. (Hanamann, Pharm. Vier- telj. 12. 527.) r A1(OH) 3 , prepared by ppt. of a solution of A1(NO 8 ) 8 with NH 4 OH, filtered and washed, is insol. in NH 4 OH+Aq. A1(OH) 3 prepared by pptn. of a solution of potassium aluminate with NH 4 C1, is sol. in a large excess of NH 4 OH if this is added to the ppt. at once. This modification which is sol. in NH 4 OH is unstable and easily goes over into the modification which is insol. in NH 4 OH. (Renz, B. 1903, 36. 2751.) Cone. (NH 4 ) 2 CO 3 +Aq does not dissolve A1(OH) 3 , and not a trace is dissolved by boiling cone. NH 4 Cl+Aq. (Weeren, Pogg. 92. 97.) With NH 4 F+Aq, it forms a double salt, A1F 3 , 3NH 4 F, which is sol. in H 2 O, but not in NH 4 F+Aq. (Helmholt, Z. anorg. 3. 127.) Insol. in (NH 4 ) 2 S+Aq. (Malaguti and Durocher, A. ch. (3) 17. 421.) Fuchs found, on the contrary, that it is not wholly insol. in (NH 4 ) 2 S+Aq. (Fresenius, Quant.) Insol. in FeCl 3 +Aq. (Bechamp.) Determinations of the solubility of alum- inum hydroxide in AlCl 3 +Aq show that part goes into solution to form a compound, while the greater part is in the colloidal form. (Fischer, Z. anorg. 1904, 40. 46.) Only si. sol. in cone. Al 2 (SO 4 ) 3 +Aq, but solubility increases with decrease in concen- tration of A1 2 (SO 4 ) 3 until it reaches a maxi- mum at a concentration of 32 % A1 2 (SO 4 ) 3 at 20, 28 % at 40, and 38 % at 60. With further decrease in concentration of A1 2 (SO 4 ) 3 the solubility of A1(OH) 3 in A1 2 (SO 4 ) 3 dim- inishes. (Kremann, C. A. 1909. 2422.) Sol. in Ba(OH) 2 +Aq. (Rose.) Sol. in boiling Fe(NO 3 ) 3 , Cr(NO 3 ) 3 , Bi(N0 3 ) 3 , Hg(N0 3 ) 2 , HgN0 3 , SnCl 2 , and SbCl 3 +Aq. (Persoz.) Insol. in HCN or cold KCN+Aq; but si. sol. in hot KCN+Aq. (Rose.) Insol. in KC 2 H 3 O 2 +Aq. (Osann, 1821.) When moist, sol. in H 2 SO 3 +Aq, from which it is repptd. on boiling. (Berthier, A. ch. (3) 7. 76.) Somewhat sol. in NaC 2 H 3 O 2 +Aq. (Mer- cer.) Not pptd. by NH 4 OH+Aq in presence of Na citrate. (Spiller.) Sol. in ethyl amine, amyl amine, sinkaline, ethyl picoline hydroxide^ stibethylium hy- droxide, triethyltoluenyl ammonium hydrox- ide+Aq. (Friedlander.) Sol. in alkyl amines. (Renz, B. 1903, 36. Insol. in acetone. (Naumann, B. 1904, 37. 4328.) Sol. to a considerable extent in K.>C 4 H 4 Oe+ Aq. Very si. sol. in cane sugar +Aq. (Ramsey.) Solubility in glycerine +Aq containing about 60 % by vol. of glycerine. 100 cc. of the solution contain 0.25 g. A1 2 O 3 . (Miiller, Z. anorg. 1905, 43. 322.) A1 2 3 , 5H 2 O. Insol. in H 2 O, NH 4 OH + Aq and alcohol. Sol. in HC1 and HNO 3 + Aq. (Zunino, Gazz. ch. it. 1900, 30 (1). 194.) Al 6 Oi 4 Hio, " Trialuminum hydroxide." Not sol. in cone, acids in the cold; not sol. in KOH (cold) and only si. sol. in hot KOH. Characterized by its solubility in exactly one mol. dil. HC1. Dil. solutions do not gelatinize even on long standing. Cone, solution of NH 4 C1 and other salts cause ppt. which re- dissolves on addition of H 2 O. Alkalies and alkali carbonates decomp. the salt with HC1 and ppt. trialuminium hy- droxide. H 2 SO 4 and sol. sulphates give insol. compds. with the hydrate. HNO 3 like HC1 gives soluble compds. with the hydrate. (Structural formula given.) (Schlumberger, Bull. Soc. 1895, (5) 13. 41-65; C. C. 1895, I. 421.) Aluminum iodide, A1I 3 . Anhydrous. Fumes on air and deliquesces. Sol. in H 2 with evolution of much heat. Sol. in CS 2 and crystallizes from the hot sat. solu- tion on cooling. (Weber.) Sol. in alcohol (Weber) ; ether and tetrachlormethane. (Gus- tavson.) Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 26.) +6H 2 O. Very sol. in H 2 O. Aluminum mercuric iodide, A1I 3 , HgI 2 -f 8H 2 O. Very deliquescent; sol. in H 2 O without de- comp. (Duboin, C. R. 1908, 146. 1028.) 12 ALUMINUM POTASSIUM IODIDE Aluminum potassium iodide, A1I 3 , KI. Sol in H 2 O with evolution of much heat. (Weber, Pogg. 101. 469.) Aluminum iodide ammonia, A1I 3 , 3NH 3 . Decomp. by H 2 O. (Weber, Pogg. 103. 263.) Aluminum iodide mercuric oxyiodide, 2A1I 3 , HgO, 3HgI 2 +15H 2 0. (Duboin, C. R. 1907, 145. 714.) Aluminum iron, FeAl 3 . Readily sol. in strong HNO 3 . (Brunck, B. 1901, 34. 2734.) Aluminum manganese, Mn 2 Al 7 . Sol. in strong HC1. (Brunck, B. 1901, 34. 2735.) Aluminum molybdenum, Al 4 Mo. Easily sol. in hot HNO 3 or HC1. (Wohler, A. 1860, 115. 103.) Al 2 Mo. (Guillet, C. R. 1901, 133. 293.) AlMo. (Guillet.) AlMo 4 . Not attacked by dil. HCl+Aq. (Guillet.) AlMo 20 . Not attacked by HCl+Aq. (Guillet.) Aluminum nickel, Al 3 Ni. Sol. in strong acids. (Brunck, B. 1901, 34. 2734.) Aluminum nitride, A1 2 N 2 . Slowly attacked by hot or cold H 2 O. De- comp. by acids and aqueous solutions of the alkalies, especially when they are concen- trated. (Mallet, A. 186. 155.) Easily decomp. H 2 O when finely powdered. (Rossil, C. R. 1895, 121. 942.) Decomp. by moist air and bv boiling H 2 O and by alkalis+Aq. (Franck," Ch. Z. 1897, 21.263. Aluminum oxide, Al 2 Os. Crystalline. Min. Corundum, sapphire, ruby, emery. Insol. in acids. Amorphous. Ignited A1 2 O 3 is insol. in acids except that it dissolves slowly when heated with a mixture of 1 pt. H 2 S0 4 and 1 pt. H 2 O. (Berzelius.) Slowly sol. -in boiling HCl+Aq. ' (Rose, Pogg. 52. 595.) Sol. in 22 pts. of a mixture of 8 pts. H 2 SO 4 and 1 pt. H-jO. (Mitscherlich.) The lower the temperature at which A1 2 O 3 has been heated, the more sol. is it in acids and alkalies. Solubility in (calcium sucrate+ sugar) + Aq. 1 1. solution containing 418.6 g. sugar and 34.3 g. CaO dissolves 1.35 g. A1 2 O 3 ; 1 1. solu- tion containing 296.5 g. sugar and 24.2 g. CaO dissolves 0.32 g. A1 2 O 3 ; 1 1. solution con- taining 174.4 g. sugar and 14.1 g. CaO dis- solves 0.19 g. A1 2 O 3 . (Bodenbender, J. B. 1865. 600.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) See also Aluminum hydroxide. Aluminum peroxide, A1 2 O 3 , A1 2 O 4 + 10H 2 O. Ppt.; sol. in acids with decomp. (Terni, . A. 1912. 3068.) Aluminum oxybromide. Basic aluminum bromides containing three equivalents or less of A1 2 O 3 to one of AlBr 3 are sol. in H 2 0. Those containing more than three equivalents are insol. (Ordway, Am. J. Sci. (2) 26. 203.) Aluminum oxychloride. Sol. in dil. acids or alkalies. Decomp. by H 2 O. (Hautefeuille and Perrey, C. R. 100. 1220.) Basic aluminum chlorides containing two equivalents or less of A1 2 O 3 to one of A1C1 3 are sol. in H 2 0. Those containing more than two equivalents are insol. (Ordway.) A1 2 O 3 , 3A1C1 3 +3H 2 O. (Tommasi, Bull. Soc. (2) 37. 443.) A1 2 3 , 8A1C1 3 +3H 2 0. (Tommasi.) 3A1 2 O 3 , A1C1 3 +15H 2 O. (Tommasi.) Aluminum phosphide, A1 3 P. Unstable. (Franck, Ch. Z. 1898, 22. 240.) A1 2 P 2 . Decomp. by H 2 O. (Fonzes-Diacon, C. R. 1900, 130. 1315.) Unstable. (Franck, Ch. Z. 1898, 22. 240.) A1 3 P 7 . Decomp. by H 2 O and acids. (Franck.) A1 3 P 7 . Decomp. by H 2 O and acids. (Franck, Ch. Z. 1898," 22. 288.) A1 S P 3 . Unstable. (Franck, Ch. Z. 1898, 22. 240.) Aluminum platinum, Pt 3 Ali . The Al is dissolved out by HC1. (Brunck, B. 1901, 34. 2735.) Aluminum selenide, Al 2 Se 3 . Decomp. by H 2 O. (Fonzes-Diacon, C. R. 1900, 130. 1315.) Aluminum silicide, Al 2 Si 4 . More easily sol. in acids than Al. (Winkler, J. pr. 91. 193.) Aluminum chromium silicide, Al 2 Cr 4 Si 6 . Insol. in hot cone. HC1, HNO 3 , H 2 SO 4 and aquaregia. Sol. in cold HF or in HF+HNO 3 . Sol. in molten alkali. Insol. in NaOH+Aq, KOCl+AqorfusedKClO 3 orKHSO 4 . (Man- chot and Kieser, A. 1904, 337, 356.) Al 2 Cr 4 Si 8 . Insol. in hot cone. HC1, HNO 3 , H 2 SO 4 and aqua regia. Sol. in HF and in molten alkali. (Manchot and Kieser, A. 1904, 337. 358.) AMIDOPHOSPHATE, FERRIC 13 Aluminum tungsten silicide. Insol. in most acids and aqua regia. Easily sol. in HF, HNO 3 and in molten alkali. Not attacked by dil. NaOH+Aq. (Manchot and Kieser, A. 1904, 337. 360.) Aluminum vanadium silicide, Al 2 V 8 Sii 3 . Sol. in HF. Not attacked by hot cone. HC1, HN0 3 , H 2 SO 4 or aqua regia. Decomp. by fusing with NaOH. Stable toward fused KC10 3 . (Manchot, A. 1907, 357. 134.) Aluminum sulphide, A1S. Decomp. by H 2 O. Sol. in acids and alkalis. (Regelsberger, Z. Elektrochem, 1898, 4. 548.) A1 2 S 3 . Decomp. in moist air and by H 2 O. (Wohler.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) Aluminum chromium sulphide, Al 2 S 3 ,CrS. SI. attacked by HCl+Aq. Gradually de- comp. by HNO 3 . (Houdard, C. R. 1907, 144. 1115.) Aluminum magnesium sulphide, A1 2 S 3 , MgS. Decomp. by H 2 0, alcohol and acids. (Houdard, C. R. 1907, 144, 1116.) Aluminum potassium sulphide. Violently decomposed by H 2 0. (St. Claire Deville, J. pr. 71. 293.) Does not exist. (Gratama, R. t. c. 3. 4.) Aluminum silver sulphide, 5A1 2 S 3 , 4Ag 2 S. (Cambi, Real. Ac. Line. (5) 21, II. 838.) Aluminum telluride. Decomp. by H 2 O. (Wohler, Pogg. 11. 160.) Aluminum titanide, Al 4 Ti. Not attacked by H 2 O or by cold HN0 3 . SI. sol. in warm HNO 3 . Sol. in cold cone. H 2 SO 4 or HC1. Sol. in warm KOH+Aq. (Levy, A. ch. 1902, (6) 26. 449.) Sol. in HC1 and in aqua regia. (Guillet.) Al 3 Ti. Sol. in hot dil. H 2 S0 4 and in hot KOH+aq. Sol. in hot cone, acids. (Man- chot, A. 1907, 357. 142.) Al 3 Ti 2 . Aluminothermic product is sol. in HC1 and aqua regia. (Guillet.) Aluminosulphuric acid, A1 2 (SO4H) 6 + 7H 2 0. Sol. in H 2 O with decomp. into A1 2 (S0 4 ) 3 and H 2 SO 4 . (Silberberger, M. 1904, 25. 222.) ZH'amide, N 2 H 4 . See Hydrazine. Amidochromic acid. Amidochromates. Do not exist. Those described by Darm- stadter and Lowenthal are impure bichro- mates. (Wyrouboff, Bull. Soc. 1894, (3) 11. 3; C. C. 845-53; 1894, II. 610.) Ammonium amidochromate, (NH 4 )NH 2 CrO 3 . Very sol. in H 2 O. (Lowenthal, Z. anorg. 1894, 6. 363.) Is ammonium dichromate. (Wyrouboff, Bull. Soc. (3) 11. 845.) Lithium amidochromate, LiNH 2 CrO 3 . Very sol. in H 2 O and acids. (Lowenthal, Z. anorg. 1894, 6. 364.) Potassium amidochromate, KCrO 3 NH 2 . Sol. only in H 2 O. Sat. solution in H 2 O contains 13 % of the salt. (Heintze, J. pr. (2) 4. 214.) Amidophosphoric acid, HPO 3 (NH 2 ) = PO(NH 2 ) (OH) 2 . Sol. in H 2 O, but decomp. on standing or by heat. (Stokes, Am. Ch. J. 16. 198.) Aluminum amidophosphate. Ppt. Sol. in NH 4 OH+Aq. (Stokes.) Ammonium amidophosphate, NH 4 HP0 3 (NH 2 ). Very sol. in H 2 O. (Stokes.) Barium amidophosphate, BaPO 3 (NH 2 ) +H 2 O. Very si. sol. in H 2 O. (Stokes.) BaH 2 (PO 3 NH 2 ) 2 +2MH 2 O. Quite diffi- cultly sol. in H 2 O. (Stokes.) Calcium amidophosphate, CaP0 3 (NH 2 ). Much less sol. in H 2 O than Ba salt. (Stokes.) CaH 2 (PO 3 NH 2 ) 2 . Much less sol. in H 2 O than the Ba salt. (Stokes.) Chromic amidophosphate. Ppt. Sol.inwarmNH 4 OH+Aq. (Stokes.) Cobalt amidophosphate. Neutral. Ppt. Add. SI. sol. in H 2 0; sol. in NH 4 OH+Aq. Cupric amidophosphate. Neutral. SI. sol. in H 2 O. Acid. Nearly insol. in H 2 O. Ferrous amidophosphate. Neutral. Sol. in much H 2 0, and in HC 2 H 3 O 2 , or NH 4 OH+Aq. Acid. Nearly insol. in H 2 O or NH 4 Cl+Aq. Sol. in NH 4 OH+Aq. Ferric amidophosphate. Neutral. Ppt. Sol. in excess of alkali 14 AMIDOPHOSPHATE, HYDROXYLAMINE amidophosphate and in NH 4 OH + Aq. Insol. in HC 2 H 3 O 2 +Aq. Add. As the neutral salt. Hydroxylamine amidophosphate, (NH 3 0)HP0 3 (NH 2 ). SI. sol. in H 2 O. (Stokes.) Lithium amidophosphate, LiHPO 3 (NH 2 ). SI. sol. in H 2 O. (Stokes.) Magnesium amidophosphate, MgPO 3 (NH 2 ) +7H 2 0. Very si. sol. in H 2 O; quite easily sol. in dil. NH 4 Cl+Aq. Sol.inHC 2 H 3 O 2 +Aq. (Stokes.) MgH 2 (P0 3 NH 2 ) 2 + 3MH 2 O. Insol. in NH 4 Cl+Aq. (Stokes.) Manganese amidophosphate. Neutral. Ppt. Add. SI. sol. in H 2 O. Nickel amidophosphate. Neutral. Ppt. Sol. in HC 2 H 3 O 2 or NH 4 OH+Aq. Add. SI. sol. in H 2 0. Potassium amidophosphate, K 2 PO 3 (NH 2 ). Very sol. in H 2 O and not decomp. by boil- ing. (Stokes.) KHPO 3 (NH 2 ). Easily sol. in cold H 2 O; insol. in alcohol. (Stokes.) Silver amidophosphate, Ag 2 P0 3 (NH 2 ). Almost insol. in H 2 O. Sol. in HN0 3 or NH 4 OH+Aq. AgHPO 3 (NH 2 ). SI. sol. in H 2 0; easily sol. in dil. HNO 3 or HC 2 H 3 2 +Aq, also in NH 4 OH+Aq. Sodium amidophosphate, Na 2 P0 3 (NH 2 ). Not deliquescent; very sol. in H 2 O; pptd. from aqueous solution by alcohol. (Stokes.) NaHPO 8 (NH 2 )+M(?)H 2 O. Nearly insol. in cold, and decomp. by hot H 2 O. Insol. in alcohol. Zinc amidophosphate. Neutral. Perceptibly sol. in H 2 O. Add. SI. sol. in H 2 O; sol. in NH 4 OH or HC 2 H 3 2 +Aq. Diamidophosphoric acid, PO(NH 2 ) 2 OH. Sol. in cold H 2 O; ahnost insol. in alcohol; stable in the air but decomp. when heated and by boiling in aq. solution. (Stokes, Am. Ch. J. 1894, 16. 130.) Barium diamidophosphate, [PO(NH 2 ) 2 O] 2 Ba. Very sol. in H 2 O; insol. in alcohol; aq. solution decomp. slowly. (Stokes, Am. Ch. J. 1894, 16. 134.) Magnesium diamidophosphate, [PO(NH 2 ) 2 0] 2 Mg. Sol, in H 2 O; insol. in alcohol. (Stokes.) Potassium diamidophosphate, PO(NH 2 ) 2 OK. Sol. in H 2 O; not deliquescent; insol. in alcohol. (Stokes.) Silver diamidophosphate, PO(NH 2 ) 2 OAg. Very stable; insol. in H 2 O. Very sol. in NH 4 OH+Aq. (Stokes.) Sodium cfo'amidophosphate, PO(NH 2 ) 2 ONa. Sol. in H 2 0; not deliquescent; insol. in alcohol. (Stokes.) Diamidofnhydroxylphosphoric acid. Silver diamidofnhydroxylphosphate, (AgO) 3 P(NHAg) 2 . (Stokes, Am. Ch. J. 1894, 16. 147.) (AgO) 3 P(NH 2 )(NHAg). Insol. in cold H 2 O. (Stokes.) (AgO) 3 P(NH 2 ) 2 . Decomp. by cold H 2 0. (Stokes.) +2H 2 O. Decomp. by boiling H 2 O. (Stokes.) Amidoimidophosphoric acid. Amidoheximidoheptaphosphoric acid, OH . PO . (NH a ) [NH . PO(OH)] 5 .NH; . PO(OH) 2 = P 7 N 7 15 H 16 . Known only in solution in H 2 O. (Stokes, Am. Ch. J. 1898, 20. 758.) Silver diamidopi/rimidophosphate, NH(PO.NH 2 .OAg) 2 . Almost insol. inH 2 O; sol. in NH 4 OH+Aq. (Stokes, Am. Ch. J. 1894, 16. 136.) Silver amido^rimido pentaphosphate, P 6 N 5 OnH 3 Ag 9 . Ppt. (Stokes, Am. Ch. J. 1898, 20. 752.) Silver amido/ieximido^eptophosphate, P 7 N 7 15 H 9 Ag 7 . Ppt.; decomp. by acetic acid. (Stokes, Am. Ch. J. 1898, 20. 759.) Sodium amidodiimidoZnphosphate, PO oN a ^ NH - P ( Na ) 2 - G at P *_- G at 760 20 ^-- ~ Gat P -_- ^ G at 760 40 G at P - -"* ' -^ G at 760 100 . * ~- G at P *-* Gat 760 20 082 3 113 30 o!ii7 2.960 .... .... 40 0148 2.820 60 . J.^O 169 2 522 0.119 1 513 \J\J 80 0.240 2^280 1^337 0.052 0.497 100 280 2 127 158 1 200 0.064 490 \J\J 120 0^316 2^000 o!l73 li095 01076 0.483 140 0.346 1.880 0.187 1.017 0.088 0.476 .... 160 0.375 1.780 0.202 0.962 0.099 0.470 .... 180 0.398 1.684 0.207 0.918 0.109 0.462 .... 200 0.421 1.598 0.232 0.881 0.120 0.454 .... 250 0.472 .434 0.266 0.810 0.145 0.440 .... 300 0.519 .315 0.296 0.750 0.168 0.426 .... 350 0.563 .223 0.325 0.705 0.191 0.414 .... 400 0.606 .152 0.353 ,0.670 0.211 0.402 .... 450 0.650 .100 0.378 0.638 0.232 0.399 500 0.692 1.052 0.403 0.612 0.251 0.382 .... 550 ' 0.732 1.012 0.425 0.587 0.269 0.372 .... 600 0.770 0.975 0.447 0.566 0.287 0.363 .... 650 0.809 0.946 0.470 0.550 0.304 0.355 .... 700 0.850 0.923 0.492 0.534 0.320 0.347 6! 068 0.074 750 0.891 0.903 0.514 0.521 0.335 0.339 0.073 0.074 760 0.899 0.518 0.518 0.338 0.338 0.074 0.074 800 850 900 950 1000 1050 1100 1150 1200 1250 1300 1350 1400 0^937 0.980 1.029 1.077 1.126 1.177 1.230 1.283 1.336 1.338 1.442 1.496 1.549 0.888 0.876 0.869 0.862 0.855 0.852 0.850 0.848 0.846 0.844 0.843 0.842 0.841 0.535 0.556 0.574 0.594 0.613 0.632 0.651 0.669 0.685 0.704 0.722 0.741 0.761 0.504 0.497 0.485 0.475 0.466 0.457 0.450 0.442 433 0.428 0.422 0.417 0.413 0.349 0.363 0.378 0.391 0.404 0.414 0.425 0.434 0.445 0.454 0.463 0.472 0.479 0.332 0.325 0.319 0.313 0.307 0.300 0.294 0.287 0.282 0.276 0.271 0.266 0.260 0.078 0.083 0.088 0.092 0.096 0.101 0.106 0.110 0.115 0.120 0.125 0.130 0.135 0.074 0.074 0.074 0.073 0.073 0.073 0.073 0.073 0.073 0.073 0.073 0.073 0.073 1450 1.603 0.840 0.780 0.409 0.486 0.255 1500 1.656 0.839 0.801 0.406 0.493 0.250 1600 1.758 0.835 0.842 0.400 0.511 0.242 1700 1.861 0.832 0.881 0.394 0.530 0.237 1800 1.966 0.830 0.919 0.388 0.547 0.231 1900 2.070 0.828 0.955 0.382 0.565 0.226 .... 2000 992 377 579 0.220 2100 0.594 0.215 (Sims, A. 118. 346.) 18 AMMONIA Solubility of NH 3 in H 2 O at temps, below 0. One gram H 2 O dissolves Sp. gr. of NH 4 OH+Aq, according to lire in Diet, of Arts. grams NH 3 1 emp. 0.947 3.9 % NHs Sp. gr. %NHs Sp. gr. 1 . 115 10 1 768 20 27.940 0.8914 15.900 0.9363 2 781 30 27.633 0.8937 14.575 0.9410 2 946 40 27.038 0.8967 13.250 0.9455 (Mallet, Am. Ch. J. 1897, 19. 807. The solubility of NH 3 in H 2 O does not follow Dalton's law at ord. temp., but does at temp, near 100. (Konowaloff, J. Russ. Phys. Chem. Soc. 1894, 26. 48; Chem. Soc. 1896, 70 (2). 351. 26.751 26.500 25.175 23.850 22.525 21.200 19.875 0.8983 0.9000 0.9045 0.9090 0.9133 0.9177 0.9227 11.925 10.600 9.275 7.950 6.625 5.300 3.975 0.9510 0.9564 0.9614 0.9662 0.9716 0.9768 0.9828 Sp. gr. of NH 4 OH+ Aq. 18.550 0.9275 2.650 0.9887 17.225 0.9320 1.325 0.9945 cr TSJTT, ^ * Sp. gr., b.-pt., and vols. gas in NH 4 OH-f Aq. 32.3* OQ or 0.8750 OOOK'T 14.53 1 Q Aft 0.9435 26 25.37* .ooO/ 0.9000 0.9054 lo.^o 12.40 11.56 0.9513 0.9545 %NH, Sp. gr. B.-pt. Vols. gas in 1 vol. liquid 22.07 19.54 17.52 15.88 0.9166 0.9255 0.9326 0.9385 10.82 10.17 9.6 9.5* 0.9573 0.9597 0.9616 0.9632 35. 32. 29. 27. 3 6 9 3 0.85 0.86 0.87 0.88 3.3 +3.3 10 16.6 494 456 419 382 (H. Davy, Elements, 1. 241.) 24. 7 0.89 23.3 346 * By direct experiment. The other numbers were obtained by calculation, making no allowance for com- 22. 19. 2 8 0.90 0.91 30 36.6 311 277 pensation. 17. 4 0.92 43.3 244 15 I 9 9 50 211 Sp. gr. of NH 4 OH+Aq at 16, according to 12 8 94 56 6 180 Otto in his Lehrbuch. 10. 5 0.95 63 3 147 8. 3 S li 70 116 % NHs Sp. gr. % NH 3 Sp. gr. 6 2 0.97 78.3 87 12.000 0.9517 8.500 0.9650 4. 1 0.98 86.1 57 11.875 0.9521 8.375 0.9654 2. 0.99 91.1 28 11.750 11.625 0.9526 0.9531 8.250 8.125 0.9659 0.9664 (Dalton, in New System, 2 . 422.) 11.500 11.375 0.9536 0.9540 8.000 7.875 0.9669 0.9673 Sp. gr. of NH 4 OH+Aqsat . at t. 11.250 11.125 0.954i5 0.9550 7.750 7.625 0.9678 0.9683 t Sp. gr. t Sp. gr. t SP. gr. 11.000 10.950 10.875 10.750 10.625 10.500 10.375 10.250 10.125 0.9555 0.9536 0.9559 0.9564 0.9569 0.9574 0.9578 0.9583 0.9588 7.500 7.375 7.250 7.125 7.000 6.875 6.750 6.625 6.500 0.9688 0.9692 0.9697 0.9702 0.9707 0.9711 0.9716 0.9721 0.9726 1 2 3 4 5 6 7 8 0.8535 0.8561 0.8587 0.8611 0.8635 0.8658 0.8681 0.8703 8725 9 10 11 12 13 14 15 16 17 0.8746 0.8766 0.8785 0.8804 0.8823 0.8841 0.8858 0.8874 8889 18 19 20 21 22 23 24 25 0.8903 0.8916 0.8928 0.8940 0.8952 0.8963 0.8974 0.8984 10.000 0.9593 6.375 0.9730 9.875 0.9597 6.250 0.9735 (Carius, A. 99. 141.) 9.750 0.9602 6.125 0.9740 9.625 9.500 9.375 0.9607 0.9612 0.9616 6.000 5.875 5.750 0,9745 0.9749 0.9754 Sp. gr. of NH 4 OH+Aq at 14, Carius (A. 99. 148). according to 9.250 0.9621 5.625 0.9759 % NHs Sp. gr. % NH 3 Sp. gr 9 125 9626 e KAA OQ7fiA 9.000 0.9631 5.375 0.9768 36.0 0. 8844 35.2 8860 8.875 0.9636 5.250 0.9773 35.8 0. 8848 35.0 8864 8.750 0.9641 5.125 0.9778 35.6 0. 8852 34.8 8868 8.625 0.9645 5.000 0.9783 35.4 0. 8856 34.6 0.8872 AMMONIA 19 Sp. gr. of NH 4 OH+Aq at 14, etc; Cont. Sp. gr. of NH 4 OH+Aq at 14, etc. Cont. % NHs Sp. gr. % NH S Sp. gr. % NHs Sp. gr. %NH 3 Sp. gr. 34.4 0.8877 22.2 0.9185 10.0 0.9593 5.0 0.9790 34.2 0.8881 22.0 0.9191 9.8 0.9601 4.8 0.9799 34.0 0.8885 21.8 0.9197 9.6 0.9608 4 . 6 0.9807 33.8 0.8889 21.6 0.9203 9.4 0.9616 4.4 0.9815 33.6 0.8894 21.4 0.9209 9.2 0.9623 4.2 0.9823 33.4 0.8898 21.2 0.9215 9.0 0.9631 4.0 0.9831 33.2 0.8903 21.0 0.9221 8.8 0.9639 3.8 . 9^839 33.0 0.8907 20.8 0.9227 . 8.6 0.9647 .3.6 9847 32.8 0.8911 20.6 0.9233 8.4 0.9654 3.4 0.9855 32.6 0.8916 20.4 0.9239 8.2 0.9662 3.2 0.9863- 32.4 0.8920 20.2 0.9245 8.0 0.9670 3.0 0.9873 32.2 0.8925 20.0 0.9251 7.8 0.9677 2.8 0.9882 32.0 0.8929 19.8 0.9257 7.6 0.9685 2.6 0.9890 31.8 0.8934 19.6 0.9264 7.4 0.9693 2.4 0.9899 31.6 0.8938 19.4 0.9271 7.2 0.9701 2.2 0.9907 31.4 0.8944 19.2 O.P277 7.0 0.9709 2.0 0.9915 31.2 0.8948 19.0 0.9283 6.8 0.9717 1.8 0.9924 31.0 0.8953 18.8 0.9289 6.6 0.9725 1.6 0.9932 30.8 0.8957 18.6 0.9296 6.4 0.9733 1.4 0.9941 30.6 0.8962 18.4 0.9302 6.2 0.9741 1.2 0.9950 30.4 0.8967 18.2 0.9308 6.0 0.9749 1.0 0.9959 30.2 0.8971 18.0 0.9314 5.8 0.9757 0.8 0.9967 30.0 0.8976 17.8 0.9321 5.6 0.9765 0.6 0.9975 29.8 0.8981 17.6 0.9327 5.4 0.9773 0.4 0.9983 29.6 OA A 0.8986 OOQO1 17.4 1*7 O 0.9333 OAO A A 5.2 0.9781 0.2 0.9991 29.4 29.2 29.0 . oyyl 0.8996 0.9001 17.2 17.0 16 8 .yo4u 0.0347 9353 Hager also gives a table in his Commentar zur Pharmacopoea, which is practically iden- 28.8 0.9006 16.6 0.9360 tical with those here given. 28.6 0.9011 16.4 0.9366 28.4 28.2 0.9016 0.9021 16.2 16.0 0.9373 0.9380 Strength of NH 4 OH+Aq of certain sp. gr. at 12. 28 9026 1 K C 9386 ,O . w 27.8 0'9031 J.U . O 15.6 0^9393 1 kg. solu- 1 1. solu- 1 litre consists of 27.6 0.9036 15.4 0.9400 Sp. gr. tion con- tains e. tains g. H2O in liquid NHs 27.4 0.9041 15.2 -t ~ f\ 0.9407 Of\ A 1 A NH 8 NH 3 cc. in cc. 27.2 27.0 . 9047 0.9051 15.0 14.8 .9414 0.9420 0.870 384.4 334.5 535.5 464.5 26.8 0.9057 14.6 0.9427 0.880 347.2 305.5 574.5 .425.5 26.6 0.9063 14.4 0.9434 0.890 311.6 277.3 612.7 387.3 26.4 0.9068 14.2 0.9441 0.900 277.3 249.5 650.5 349.5 26.2 0.9073 14.0 0.9449 0.910 244.9 222.8 687.2 312.8 26.0 0.9078 13.8 0.9456 . 920 213.4 196.3 723.7 276.3 25.8 0.9083 13.6 0.9463 0.930 182.9 170.1 759.9 240.1 25.6 0.9089 13.4 0.9470 0.940 152.9 143.7 796.3 203 7 25.4 0.9094 13.2 0.9477 0.950 124.2 118.0 832.0 168.0 25.2 0.9100 13.0 0.9484 960 97.0 93.1 866.9 133 . 1 25.0 0.9106 12.8 0.9491 0.970 70.2 68.0 902.0 98.0 24.8 0.9111 - 12.6 0.9498 0.980 45.3 44.3 935.7 64.3 24.6 0.9116 12.4 0.9505 0.990 21.0 20.7 969.3 30.7 24.4 24.2 0.9122 0.9127 12.2 12.0 0.9512 0.9520 (Wachsmuth, Arch. Pharm; (3) 8. 510.) 24.0 23.8 23.6 0.9133 0.9139 0.9145 11.8 11.6 11.4 0.9527 0.9534 0:9542 Sp. gr. of NH 4 OH+Aqatl5. (Most careful experiments.) 23.4 23.2 0.9150 0.9156 11.2 11.0 0.9549 0.9556 Sp. gr. % NH 3 Sp. gr. %NH 3 23.0 22.8 22.6 22 4 0.9162 0.9168 0.9174 0.9180 10.8 10.6 10.4 10.2 0.9563 0.9571 0.9578 0.9586 0.990 0.974 0.950 2.15 6.10 13 54 0.926 0.916 0.910 19.50 22:50 24.40 20 AMMONIA Sp. gr. of NH 4 OH+Aq at 15 Continued Sp. gr. of NH 4 OH+Aq at 15, etc. Continued Sp. gr. % NH 3 Sp. gr. % NH 3 Sp. gr. % NH 3 1 1. contains g. NH 3 Correction for* 1 0.900 27.70 0.890 31.40 0885 33.5 0.882 0.880 34.8 35.5 0.966 0.964 0.962 0.960 0,958 0.956 0.954 0.952 0.950 0.948 0.946 0.944 0.942 0.940 0.938 0.936 0.934 0.932 0.930 0.928 0.926 0.924 0.922 0.920 0.918 0.916 0.914 0.912 0.910 0.908 0.906 0.904 0.902 0.900 0.898 0.896 0.894 0.892 0.890 0.888 0.886 0.884 0.882 8.33 8.84 9.35 9.91 10.47 11.03 11.60 12.17 12.74 13.31 13.88 14.46 15.04 15.63 16.22 16.82 17.42 18.03 18.64 19.25 19.87 20.49 21.12 21.75 22.39 23.03 23.68 24.33 24.99 25.65 26.31 26.98 27.65 28.33 29.01 29.69 30.37 31.05 31.75 32.50 33.25 34.10 34.95 80.5 85.2 89.9 95.1 100.3 105.4 110.7 115.9 121.0 126.2 * 131.3 136.5 141.7 146.9 152.1 157.4 162.7 168.1 173.4 178.6 184.2 189.3 194.7 200.1 205.6 210.9 216.3 221.9 227.4 232.9 238.3 243.9 249.4 255.0 260.5 266.0 271.5 277.0 282.6 288.6 294.6 301.4 308.3 0.00026 0.00027 0.00028 0.00029 0.00030 0.00031 0.00032 0.00033 0.00034 0.00035 0.00036 0.00037 0.00038 0.00039 0.00040 0.00041 0.00041 0.00042 0.00042 0.00043 0.00044 0.00045 0.00046 0.00047 0.00048 0.00049 0.00050 0.00051 0.00052 0.00053 0.00054 0.00055 0.00056 0.00057 0.00058 0.00059 0.00060 0.00060 0.00061 0.00062 0.00063 0.00064 0.00065 (Gruneberg, Chem. Ind. 12. 97.) The following table is calculated from the above by interpolation: Sp. gr. % NHs Sp. gr. % NH 3 0.995 1 05 0.990 2.15 0.985 3.30 0.980 4.50 0.975 5.75 0.970 7.05 0.965 8.40 0.960 9.80 0.955 11 20 0.950 12.60 0.945 14.00 0.940 15.45 0.935 0.930 0.925 0.920 915 0.910 0.905 0.900 0.895 0.890 0.885 0.880 16.90 18.35 19.80 21.30 22 85 24.40 26.00 27.70 29.50 31.40 33.40 35.50 (Gruneberg.) Sp. gr. of NH 4 OH+Aq at 14. %HN 3 Sp. gr. % NH 3 Sp. gr. 31 23.8 20 4 0.8933 0.9116 0.9246 15.6 11.7 5.1 0.9400 0.9536 0.9780 (Lunge and Smith, B. 17. 777.) Sp. gr. of NH 4 OH+Aq at 15, according to Lunge and Wiernik (Zeit. f. angew. Ch. 1889. 183). (Most carefully worked out and calculated.) Sp. gr. % NH 3 1 . contains g. NH 3 Correction for 1 1.000 0.998 0.996 0.994 0.992 0.990 0.988 0.986 0.984 0.982 0.980 0.978 0.976 0.974 0.972 0.970 0.968 0.00 0.45 0.91 1.37 1.84 2.31 2.80 3.30 3.80 4.30 4.80 5.30 5.80 6.30 6.80 7.31 7.82 0.0 4.5 9.1 13.6 18.2 22.9 27.7 32.5 37.4 42.2 47.0 51.8 56.6 61.4 66.1 70.9 75.7 0.00018 0.00018 0.00019 0.00019 0.00020 0.00020 0.00021 0.00021 0.00022 0.00022 00023 0.00023 0.00024 0.00024 0.00025 0.00025 0.00026 NH 3 is much less sol. in KOH, or NaOH+ Aq than in H 2 O. Solubility of NH 3 in H 2 O, and KOH-f-Aq of various strengths: 100 pts. solvent absorbs g. NH 3 at t. t H--0 KOH+Aq 1 11.25% KzO KOH+Aq 25.25% K 2 O 90.00 72 00 8 72.75 . 57.00 16 59.75 46.00 24 49.50 37.25 49.50 37.50 28.50- 21.75 (Raoult, A. ch. (5) 1. 262 } AMMONIA 21 100 pts. sat. KOH+Aq dissolve only 1 pt. NH 3 . Solubility in NaOH+Aq is the same as in KOH+Aq of the same strength. NH 4 Cl+Aq absorbs slightly less NH 3 than the same vol. H 2 O. NaNO 3 , and NH 4 NO 3 + Aq absorb almost the same amount NH 3 as the same vol. H 2 O. (Raoult, I.e.) Solubility of NH 3 in 100 pts. Ca(NO 3 ) 2 +Aq. Solubility in salts +Aq at 35 C. Salt Concentration of the aq. solution Mols. NHj soluble in 1 liter of solution KC1 NaCl CH 3 COOK H(COOK) 2 KOH NaOH HK 2 C0 3 ^Na 2 C0 8 . 5 normal 0.426 normal tt 0.923 0.966 0.902 0.902 0.870 0.896 0.914 0.932 t H 2 Ca(NO 3 )2+Aq 28.38%Ca(NOi)i Ca(NO 3 )2+Aq 59.03%Ca(NO 3 )2 (Riesenfeld, Z. phys. Ch. 1903, 45. 462.) The solubility of NH 3 in NaNO 3 , NH 4 NO 3 and in AgNO 3 ,2NH 3 +Aq is nearly the same as in pure H 2 O. (Konowaloff, C. C. 1898, II. 659). 8 16 90.00 72.75 59.75 96.25 78.50 65.00 104.50 84.75 70.50 (Raoult, I.e.) Solubility in salt solutions at 25C. Distribution-coefficient of NH 3 between water and CHC1 3 =26.3 at 20 C ; 24.9 at 25; 23.2 at 30. The distribution-coefficient of NH 3 be- tween CHC1 3 and a number of salt solutions has been determined for the purpose of study- ing the nature of metal-ammonia compounds in aqueous solution. (Dawson, Chem. Soc. 1900, 77. 1242.) Distribution of NH 3 between H 2 O and CHC1 3 at 18 C . Salt Mols. NHs soluble in 1 liter of 5-normal solution 1 -normal solution 1.5-nor- mal solution KC1 KBr KI KOH NaCl NaBr ' Nal NaOH LiCl LiBr Lil LiOH KF KNO, - KNOi KCN KCNS ^K 2 S0 4 ^K 2 S0 3 ^K 2 C0 3 ^K 2 C 2 4 ^K 2 Cr0 4 CH.COOK HCOOK KB0 2 KK 2 HPO 4 KNa 2 S KClO 3 0.25-norm. KBrO 3 0.25-norm. KI0 3 0.25-norm. 0.930 0.950 0.970 0.852 0.938 0.965 0.995 0.876 0.980 1.001 1.030 0.865 0.839 0.923 0.920 0.926 0.932 0.875 0.865 0.788 0.866 0.866 0.866 0.868 0.814 0.860 0.887 0.927 0.940 0.951 0.866 0.904 0.942 0.716 0.889 0.916 0.992 0.789 1.008 1.040 1.094 0.808 0.722 0.862 0.855 0.858 0.868 0.772 0.768 0.650 0.771 0.771 0.765 0.760 0.677 0.749 0.795 0.809 0.857 0.900 0.607 0.843 0.890 0.985 0.716 1 045 1.090 1.190 0.768 0.626 0.804 0.798 0.802 0.814 0.678 0.675 0.554 0.675 0.675 0.685 0.678 0.560 0.664 0.726 NHs concentration in aqueous solution, mo Is. /litre NHs concentration in CHCh solution, mols./ litre 0.9280 1.921 2.064 2.274 2.590 3.700 4.333 0.03506 0.07703 0.08350 0.09317 0.1083 0.1639 0.1996 (Dawson, Z. phys. Ch. 1909, 69. 120.) Distribution of NH 8 between hydroxides -f Aq and CHC1 3 at 18. Aqueous solution NHj concen- tration in the aqueous solution, mols. /litre NHj concen- tration in the CHCls solution, mols./litre. 0.2-N.KOH 0.5-N. KOH 0.2-N. NaOH 0.5-N. NaOH 0.2-N. i^Ba(OH) 2 0.5-N. KBa(OH) 2 1.949 1.978 2.016 1.944 2.076 3.397 0.0841 0.0951 0.0869 0.0907 0.08905 0.1560 (Abegg & Riesenfeld, Z. phys. Ch. 1902, 40. 100.) (Dawson, I.e.} 22 AMMONIA Distribution of NH 3 between Cu(QH) 2 +Aq and GHGls-at 18V -- Solubility of NH 3 in ethyl alcohol (absolute) at t. Cone, of Cu(OH) 2 equivalents/ litre NHs concentra- tion in aqueous solution, mols./ litre NHs concentra- tion in CHCls solution, mols./litre t %NH 3 Pts. NHs per 100 , pts. alcohol 6 11.7 14.7 17 , | 22 L .-28.4 ..... 19.7 17.1 14.1 13.2 12.6 10.9 .1. 9.2 24.5 20.6 16.4 15,2 14.7 12.2 10.1 0.041 0.0705 0,081 2.014 2.653 3.011 0.07968 0.1087 0.1247 Dawson, I.e.) (r\o Rrnvn P t n 11.119.^ Sol. in 3 pts. alcohol of 38. (Boullay.) 1 vol. alcohol of 0.829 sp. gr. absorbs about 50 vols. NHs. (Davy.) Much less sol. in ethyl, propyl, or amyl alcohol than in H 2 0. (Pagliano and Emo, Gazz. ch. it. 13. 278.) 1 vol. abs. alcohol at 20 and 760 mm. pressure absorbs 340 vols. NH 3 gas. (Miiller, W. Ann. 1891, 43. 567.) 1 1. methyl alcohol sat .-with NHs contains 218 g. NH 3 at 0; sp. gr. of solution = 0.770 ; coefficient of solubility = 425.0. (Delepine) . Solubility of NH 3 in alcohol at t: weight NH; 3 = weight NH 3 contained in a litre of solution sat. at 760 mm. and t; sp. gr. = sp. gr.; of solution; C = coefficient of solubility . Temp. Degree of Alcohol 100 90 80 70 60 50 Weight NH 3 . 130.5 782 146.0 783 206.5 808 246.0 830 304.5 835 Q 209.5 245 (^ 390 504 5 697 7 10 Weight NH 3 . Sp.gr. . . . 108.5 0.787 164 3 120.0 0.803 186 167.0 0.8DO 288 ..... 198.25 0.831 373 o 227.0 0.850 438 6 r Weight NH 3 . gp.gr. ... ...... 75.0 0.791 106 6 97.5 0.788 147 8 119.75 0.821 190 5 137.5 0.829 223 152.5 0.842 260 8 182.7 0.869 QQO o 30 Weight NH 3 Sp.gr. . . . 51.5 0.798 97 74.0 0.791 186 7 81.75 0.826 121 6 100.3 129.5 0.846 Oil A 152.0 0.883 OKO A (Detepine, J. Pharm. (5) 25. 496.) Solubility of NH 3 in methyl alcohol (absolute) att. t %NHs Pts. NHs per 100 pts. alcohol 6 11.7 14.7 17 22 28.4 29.3 26.0 23.5 21.8 20.8 18.3 14.8 41.5 35.2 30.7 27.9 26.3 22.4 17.4 (de Bruyn, Z.c.) Readily sol. in ether. Sol. in, 0.4 vol. petroleum from Amiano. (Saussure.) 1 vol. oil of turpentine absorbs 7.5 vols. NH 3 at 16. 1 vol.. oil of lemon absorbs 8.5 vols. NH 3 at 16. 1 vol. oil of rosemary absorbs 9.75 vols NH 3 at 29. 1 vol. oil of lavender absorbs 47 vols. NH 3 at 20. (Saussure.) 1 vol. caoutchine absorbs 3 vols. NH 3 (Himly.) Valerol absorbs much NH 3 . (Gerhardt, A ch. (3) 7. 278.) 1 vol. ether at 760 mm. pressure absorbs 17.13 vols. NH 3 at 0; 12.35 vols. at 10 and 10.27 vols. at 15. (Christoff, Z. phys. Ch. 1912, 79. 459.) -f H 2 O. Colorless crystals. + KH 2 O. Large transparent crystals (Rupert, J. Am. Chem. Soc. 1909, 31. 868.) Ammonia, with metal salts. For the ammonia addition-products of metal salts, see under the respective metal salts, except in the case of Co, Cr, Hg, and the Pt metals, for which see cobalt ammonium, chromium ammonium, etc., compounds, for AMMONIA 23 further reference. New data on Co and Cr ammonium compounds and those of the Pt metals, published since the first edition, has not been included in the present edition. Ammonium amalgam, NH 4 , a?Hg. Decomp. by H 2 0, but more easily in pres- ence of naphtha, alcohol, or ether. Ammonium azoimide, N4H 4 = NH 4 N 3 . Easily sol. in H 2 O; si. sol. in absolute alcohol, easily in 80% alcohol. Insol. in ether or benzene. (Curtius, B. 24. 3344.) Ammonium cobalt azoimide, NH 4 N 3 , CoN 6 . Rather sol. in H 2 O. (Curtius and Rissom, J. pr. 1898, (2) 68. 302.) Ammonium bromide, NH 4 Br. Sol. in liquid NH 3 at 50. (Moissan C. R. 1901, 133. 713.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) SI. sol. in alcohol. 1 pt. NH 4 Br dissolves in 32.3 pts. alcohol (0.806 sp. gr.) at 15; 9.5 pts. at 78. (Eder, I.e.} 100 pts. absolute methyl alcohol dissolve 12.5 pts. at 19; 100 pts. absolute ethyl al- cohol dissolve 3.22 pts. at 19. (de Bruyn, Z. phys. Ch. 10. 783.) Solubility in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the solvent. G = g. NH 4 Br in 10 cc. of the solution. S =sp. gr. of the sat. solution at 25/4. heat. 1 pt. NH 4 Br dissolves in pts. H 2 at t. P G S 0.00 4.37 10.40 41.02 80.69 84.77 91.25 100.00 0.255 0.299 0.321 0.506 0.813 0.847 0.934 0.983 0.8065 0.8083 0.8117 0.8252 0.8501 0.8508 0.8551 0.8605 t Pts. H 2 O t Pts. H 2 O t Pts. H 2 O 10 1.51 30 1.23 100 16 1.39 50 1.06 0.78 (Eder, W. A. B. 82. (2) 1284.) NH 4 Br+Aq containing 41.09% NH 4 Br is sat. at 15. (Gerlach.) Sp. gr. of NH 4 Br+Aq at 15. (Herz, Z. anorg. 1908, 60. 156.) Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. NH 4 Br in 10 cc. of the solution. S = Sp. gr. of the sat. solution at 25/4. % NH 4 Br Sp. gr. % NH 4 Br Sp. gr. 5 10 15 1 . 0326 1.0652 1.0960 20 30 41 09 1.1285 1.1921 1.2920 (Eder.) Sp. gr. of NH 4 Br+Aq at 16. p G S 11.11 23.8 65.2 91.8 93.75 100. 0.983 0.851 0.690 0.308 0.128 0.125 0.095 0.8605 0.8524 0.8426 0.8184 0.8097 , 0.8089 0.8059 % NEUBr Sp. gr. % NH 4 Br Sp. gr. 2 3 4 5 6 . 7 8 9 10 11 12 13 14 15 16 17 18 19 20 _'! 1.0119 1.0181 1.0242 1.0303 1.0364 1.0425 1.0486 1.0547 1.0609 1.0672 1 . 0735 1 . 0798 1 . 0862 1.0926 1.0988 1.1051 1.1115 1.1181 1.1246 1.1310 22 23 24 25 26 27 28 29 '30 31 32 33 34 35 36 37 38 39 40 41 1.1375 1.1440 1.1506 1.1573 1.1642 1.1713 1.1787 .1862 .1938 .2018 .2098 .2180 .2260 1.2342 1.2425 1.2509 1 2594 1.2679 1.2765 1.2850 (Herz, I.e.) Solubility in mixtures of propyl and ethyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. NH 4 Br in 10 cc. of the solution. S =Sp. gr. of the sat/ solution at 25/4. P G S 8.1 17.85 56.6 88.6 91.2 95.2 100 0.255 0.251 0.237 0.163 0.111 0.105 0.104 0.095 0.8065 0.8062 0.8052 0.8048 0.8042 0.8049 0.8059 0.8059 (Hager, Comm. 1883.) 25 g. NH 4 Br+50 g. H 2 O lower the temp, from 15.1 to 1.1. (Rudorff.) (Herz, I.e.) 24 AMMONIUM BROMIDE Sol. in 809 pts. ether (0.729 sp. gr.) . (Eder, Sol. in acetone. (Eidmann, C. C. 1899. II, 1014); (Naumann, B. 1904, 37. 4328.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethylacetate. (Naumann, B. 1910, 43. 314.) Ammonium fnbromide, NH 4 Br 3 . Gives off Br in air. Sol. in H 2 0. (Rooze- boom, B. 14. 2398.) Decomp. in the air. Very sol. in H 2 O. (Chattaway, Chem. Soc. 1915, 107. 106.) Ammonium antimony bromide, 3NH 4 Br, 2SbBr 8 . Easily sol. in abs. alcohol. (Caven, C. C. 1906. II, 293.) 7NH 4 Br, 3SbBr s . Easily sol. in abs. al- cohol. (Caven, C. C. 1905. II, 293.) See also Bromantimonate, ammonium. Ammonium bismuth bromide. NH 4 Br, BiBr 3 +H 2 0. Deliquescent. Decomp. by H 2 O. Sol. in alcohol. (Nickles, C. R. 61. 1097.) Ammonium cadmium bromide, NH 4 Br, Sol. in 0.73 pt. H 2 0, 5.3 pts. abs. alcohol, 280 pts. ether (sp. gr. 0.729), and 24 pts. alcohol ether (1 : 1). (Eder, Dingl. 221. 89.) Sol. in H 2 without decomp. between 1 and 110.1. 100 pts. of the solution contain at: 1 14.8 52.2 110.1 53.82 58.01 65.32 75.83 pts. of the salt. (Rimbach, B. 1905, 38. 1555.) 4NH 4 Br, CdBr 2 . Sol. in 0.96 pt. H 2 0, from which it is pptd. by alcohol or ether. (Eder.) Solubility in H 2 O at t. Below 160 the salt is decomp. by H 2 O; at 160 it is sol. in H 2 O without decomp. 100 pts. of the solution contain t Solid phase Pts. Pts. Pts. Cd Br NH 4 0.8 13.0 14.72 14.94 50.46 51.48 6.67 6.85 Double salt+NH 4 Br (i 44.5 15.01 53.85 7.35 (( 76.4 14.60 55.28 7.80 tration, mol. g. alcohol for 1000 g. H 2 O Solubility in 1000 g. H 2 O Molecular solubility 298.40 5.59 u % 297.35 5.57 (I 1 A 296.55 5.55 11 i 292.65 5.47 (( 3 283 . 15 5.30 25 395.10 7.40 y* 394.75 7.39 (i & 393 85 7 37 a i 392.90 7.36 (c 3 386.20 7.23 (Armstrong and Eyre, Proc. R. Soc. Lond. (A) 84. 127.) Alcohol concen- t tration, mol. g. alcohol for 1000 g. H 2 O Solubility in 1000 g. H 2 O Molecular solubility 298.46 5.59 ( M 295.40 5.53 I M 291.30 5.45 { 1 284.00 5.32 25 395.10 7.40 < H 393.50 7.37 ' 1 A 390.80 7.32 i i 384.80 7.21 Solubility of NH 4 C1 in ethyl alcohol at 0. Alcohol concentration, mol. g. alcohol for 1000 g. H 2 O Solubility in 1000 g. H 2 O Molecular solubility 298.40 5.59 M 295.50 5.53 /^ 291.95 5.47 i 286.40 5.37 3 266.25 4.99 (Armstrong and Eyre, I.e.) See also ammonium cupric chloride. Solubility of NH 4 C1 in propyl alcohol. (Armstrong and Eyre, I.e.) Solubility in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the solvent. G = g. NH 4 C1 in 10 cc. of the solution. S = sp. gr. of the sat. solution at 25/4. P G s 0.00 4.37 10.40 41.02 80.69 84.77 91.25 100.00 0.0533 0.0583 0.0658 0.118 0.217 0.227 0.247 0.276 0.7908 0.7909 0.7910 0.7957 0.8020 0.8026 0.8040 0.8062 (Herz, Z. anorg. 1908, 60. 155.) Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. NH 4 C1 in 10 cc. of the solution. S = Sp. gr. of the sat. solution at 25/4. p G S 11.11 23.8 65.2 91.8 93.75 100.00 0.276 0.231 0.182 0.071 0.026 0.023 0.018 0.&062 O.S035 0.8008 0.8005 0.8002 Or8000 0.8009(?) (Herz, Z. anorg. 1908, 60. 157.) AMMONIUM CADMIUM CHLORIDE 31 Solubility in mixtures of propyl and ethyl alcohol at 25. p = % propyl alcohol in the solvent. G = g. NH 4 C1 in 10 cc. of the solution. S = Sp. gr. of the sat, solution at 25/4. p G s 0.0533 0.7908 8.1 0.0505 0.7910 17.85 0.0455 0.7916 ' 56.6 0.0312 0.7963 88.6 0.0210 0.7996 91.2 0.0203 0.8001 95.2 0.0190 0.8003 . 100 0.0177 0.8009 (Herz, Z. anorg. 1908, 60. 160.) Insol. in ether and CS 2 . (Fordos and Gelis, A. ch. (3) 32. 393.) Very si. sol. in acetone. (Krug and M'El- roy, J. anal. appl. Ch. 6. 184.) Solubility of NH 4 C1 in acetone +Aq at 25. I A = cc. acetone in 100 cc. acetone +Aq. ; - NH 4 C1 =millimols. NH 4 C1 in 100 cc. of the solution. A NH 4 C1 Sp. gr. 585.1 1 . 0793 10 534.1 1.0618 20 464.6 1.0451 30 396.7 1 . 0263 40 328.5 0.99984 46.5) lower 283.7 0.97998 to 2 phases 85. 7J upper 18.9 0.8390 90 9.4 0.8274 (Herz, Z. anorg. 1905, 46. 263.) Solubility of NH 4 C1 in glycerine +Aq at 25 G = g. glycerine in 100 g. glycerine +Aq. NH 4 Cl = millimols. NH 4 C1 in 100 cc. of th solution. G 13.28 25.98 45.36 54.23 83.84 100 NHiCl 585.1 544.6 502.9 434.4 403.5 291.4 228.4 Sp. gr. .0793 .0947 .1127 .1452 .1606 .2225 1.2617 (Herz, I.e.) Insol. in acetone. (Naumann, B. 1904, 37 4328.); (Eidmann, C. C. 1899. II, 1014.) Insol. in anhydrous pyridine. Sol. in 97 / pyridine+Aq, 95% pyridine +Aq and in 93 < pyridine+Aq. (Kahlenberg, J. Am. Chem Soc. 1908, 30. 1107.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894 6. 257.) Very sol. in ethyl amine. (Shinn, J. phys Chem. 1907, 11. 538.) Insol. in methyl acetate. (Xaumann, B 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B 910, 43. 314.) Insol. in benzonitrile. (Naumann, B. 1914, 7. 1370.) Sol. in formic acid. (Zanninovich-Tessarin, . phys. Ch. 1896, 19. 251.) Ammonium antimony chloride, SbCl 6 (NH 4 ) 2 , SbCl 6 (NH 4 ) 3 . Ppt. Decomp. by H 2 O. (Weinland, B. 905, 38. 1085.) SbCl 6 (NH 4 ),SbCl 6 ,NH 4 OH. Very deli- mescent; si. sol. in H 2 O with decomp. (Wein- and, B. 1901, 34. 2635.) Ammonium antimonous chloride, NH 4 C1, SbCl 3 . Deliquescent. (Deherain, C. R. 52. 734.) 2NH 4 C1, SbCl 3 +2H 2 O. Permanent in dry lir; decomp. by much H 2 O. (Poggiale.) 3NH 4 C1, SbCl 3 +3H 2 O. As above. Ammonium antimonic chloride, 3NH 4 C1, SbCl 5 . Decomp. by H 2 O. (Deherain, C. R. 52. 734.) 4NH 4 C1, SbCl 5 . Decomp. by H 2 O. (D.) See also Chlorantimonate, ammonium. Ammonium antimony platinum chloride, (Sb, Pt)Cl 6 (NH 4 ) 2 . Ppt. (Weinland, B. 1905, 38. 1084.) Ammonium antimony tin chloride, (Sb,Sn)Cl 6 (NH 4 ) 2 . Ppt. (Weinland, B. 1905, 38. 1085.) Ammonium arsenyl chloride, 2NH 4 C1, AsOCl (Wallace, Phil. Mag. (4) 16. 358.) Ammonium bismuth chloride, NH 4 C1, 2BiCl 3 . Deliquescent. (Deherain, C. R. 54. 724.) 2NH 4 C1, BiCl 3 . Decomp. by H 2 O. (Arppe.) Pogg. 64. 237.) +2>^H 2 O. (Rammelsberg.) 3NH 4 C1, BiCl 3 . Decomp. by H 2 O. (Arppe.) 5NH 4 C1, 2BiCl 3 . (Rammelsberg.) Ammonium bismuth potassium chloride, 2NH 4 C1, BiCl 3 , KC1. (Deherain, C. R. 54. 724.) . Ammonium cadmium chloride, NH 4 C1, CdCl 2 . Solubilitv of NH 4 C1, CdCl 2 in H 2 O at t. H 0.2 ~. t Pts. by weight in 100 pts. of solution 51 gffl ^i* 28 "^S Cl Cd NH 4 O 1 "" 1 2.4 13.44 14.26 2.24 29.94 42.74 3.25 16.0 15 07 15.82 2.56 33.45 50.26 3.83 41.2 17 46 18.61 2.89 38.96 63.83 4.86 63.8 19.73 20.92 3.34 43.99 78.54 5.98 105.9 23.52 24.70 4.01 52.58 109 . 33 8.30 (Rimbach, B. 1897, 30. 3076.) 32 AMMONIUM CHLOROMOLYDENUM CHLORIDE SI. sol. in H 2 O, alcohol, and wood spirit, (v. Hauer, W. A. B. 13. 449.) 4NH 4 C1, CdCl 2 . Sol. inH 2 O. (v. Hauer.) Decomp. by H 2 O to NH 4 C1, CdCl 2 . De- comp. increases with decrease of temp. At 3.9 approximately wholly decomp. to NH 4 C1, CdCl 2 . At 113.9 very nearly all is 4NH 4 C1, CdCl 2 . (Rimbach, B. 1897, 30. 3077.) Solubility of 4NH 4 C1, CdCl 2 in H 2 O at t. t Pts. dissolved in 100 pts. by weight of solution. Cd Cl NH 4 3.9 16.1 40.2 58.5 112.9 113.9 5.75 6.93 9.91 12.50 16.66 16.51 18.17 20.26 23.84 26,53 31.79 32.71 7.37 7.97 8.92 9.35 10.78 11.30 Sol. without decomp. in 37.3% HCl(d = 1.19) and 24.8% HCl(d = 1.125). (Rimbach, B. 1905, 38. 1569.) Solubility of 4NH 4 Cl,CdCl 2 +NH 4 Cl in H 2 O at t. In 100 pts. by wt. of the solution Composition of the solid phase Hygroscopic. Decomp. by H 2 O and by alcohol. (Weinland, B. 1907, 40. 3770.) Ammonium cobaltous chloride, NH 4 C1, CoCl 2 +6H 2 O. Deliquescent in moist air. Very easily soi. in H 2 O. (Hautz, A. 66. 284.) Ammonium cobaltous chloride ammonia, NH 4 C1, CoGl 2 , NH 3 . (F. Rose.) Ammonium cuprous chloride, 4NH 4 Cl.Cu 2 Cl 2 . Decomp. in the air. 4NH 4 C1, 3Cu 2 Cl 2 . Decomp. by H 2 O, not by alcohol. (Ritthausen, J. pr. 59. 369.) Fairly stable in air. (Wells, Z. anorg. 1895, 10. 158.) Ammonium cupric chloride, NH 4 C1, CuCl 2 . Solubility of NH 4 C1, CuCl 2 in absolute alcohol at 25. 4.65NH 4.74 6.45 Solid phase 4 C1+NH 4 C1, CuCl 2 NH 4 C1+NH 4 C1, CuCl 2 NH 4 C1, CuCl 2 12.90 34.92 34.50 Solid phase NH 4 C1, CuCl 2 NH 4 Cl,CuCl 2 + CuCl 2 , C 2 H 5 OH Pts. by wt. Cd 1.0 13.2 40.1 58.2 2.82 2.76 3.16 3.51 Pts. by wt. Cl 17.11 18.84 22.56 25.21 Pts. by wt. NH 4 Mol. % NH4C1 7.82 8.71 10.49 11.72 59.0 74.0 71.0 69.0 Mol. % Tetra- salt 41.0 26.0 29.0 31.0 (Rimbach, B. 1902, 36. 1300.) Solubility of 4NH 4 C1, CdCl 2 +NH 4 Cl, CdCl 2 in H 2 O at t. (Foote and Walden, J. Am. Ch. Soc. 1911, 33. 1032.) +2H 2 O. Sol. in 2 pts. H 2 O. (Hautz, A. 66. 280.) Does not exis t, (Meerburg, C. C. 1904. II, 1362. 2NH 4 C1, CuClo +2H 2 O. Easily sol. in H 2 O, also in alcohol, even when absolute. (Cap and Henry, J. pr. 13. 184.) Solubility of 2NH 4 C1, CuCl 2 in H 2 O at t. In 100 pts. by wt. of the Composition of solution the solid phase t Pts. by wt. Cd Pts. by wt. Cl Pts. by wt. NH 4 Mol. % Mono- salt Mol. % Tetra- salt 1.1 5.34 17.62 7.27 49.6 50.4 14.0 7.12 19.86 7.84 47.0 53.0 40.7 10.24 23.82 8.85 77.0 23.0 58.5 12.50 26.53 9.35 (Rimbach, B. 1902, 36. 1300.) Sol. without decomp. in 50% LiCl-fAq, 33.3% CaCl 2 +Aq and 50% MgCl 2 +Aq. (Rimbach, B. 1905, 38. 1569.) Ammonium chloromolybdenum chloride, 2NH 4 C1, Cl 4 Mo 3 Cl 2 +2H 2 0. Decomp. by pure H 2 O; can be crystallized from HCl+Aq. (Blomstrand.) Ammonium chromium chloride, 2NH 4 C1 CrCl 3 +H 2 0. Sol. in H 2 O with decomp. (Neumann, A. ' +6H 2 5 = 2NH 4 C1, [CrCl 2 .4H 2 0]Cl+2H 2 O. g. 2NH^rl 2 O. Min. Kremersite. Deliquescent. Ammonium lead chloride, NH 4 C1, 2PbCl 2 + 3H 2 O. Sol. in H 2 O without decomp. (?). (Andre", C. R. 96. 1502.) 6NH 4 C1, PbCl 2 +H 2 O. 9NH 4 C1, PbCl 2 + 13^H 2 0. 9NH 4 C1, 2PbCl 2 +2^H 2 O. 10NH 4 C1, PbCl 2 +H 2 O. 11NH 4 C1, 2PbCl 2 +3^H 2 O. 18NH 4 C1, PbCl 2 +4H 2 O. All these salts are decomp. by H 2 O. (Andre" A. ch. (6) 3. 104.) Of the salts prepared by Andre", only one NH 4 C1, 2PbCl 2 exists. (Wells, Sill. Am. J. 146. 25.) Solubility determinations show that NH 4 C1, 2PbCl 2 is the only double salt formed at 25. (Foote, Am. Ch. J. 1907, 37. 121.) NH 4 C1, PbCl 2 + V 3 H 2 0. (Wells, Z.c.) Ammonium lead tefrachloride. See Chloroplumbate, ammonium. Ammonium magnesium chloride, NH 4 MgCl +6H 2 O = NH 4 C1, MgCl 2 +6H 2 0. Deliquescent. Very sol. in H 2 O. Sol. in 6 pts. cold H 2 O. (Fourcroy.) Solubility in NH 4 Cl+Aq at t. Per 1000 Mol. H 2 O t ' Mol. NH 4 C1 MoL MgCh 3.5 27.5 55.7 25 42.1 56.4 50.0 62.9 59.1 (Biltz, Z. anorg. 1911, 71. 170.) 4NH 4 Cl,5MgCl 2 +33H 2 0. Sol. in H 2 O. (Berthelot and Andre", A. ch. (6) 11. 294.) Ammonium manganous chloride, NH 4 C1, Sol. in 13^ pts. H 2 at ordinary temp. (Hautz, A. 66. 280); does not exist. (Saund- ers, Am. Ch. J. 14. 134.) 2NH 4 C1, MnCl 2 +H 2 O. Sol. in H 2 O (Ram- melsberg) ; does not exist. (Saunders.) +2H 2 O. Easily sol. in H 2 O, but with decomp. into NH 4 C1 and MnCl 2 . (Saunders.) Ammonium manganic chloride, 2NH 4 C1, MnCl 3 . Sol. in H 2 O; less sol. in NH 4 Cl+Aq. Un- stable. (Neuman, M. 1894, 16. 490.) +H 2 0. Decomp. by H 2 0. Sol. in HC1 apparently without decomp. (Rice, Chem. Soc. 1898, 73. 260.) Ammonium mercuric chloride, 2NH 4 C1, HgCl 2 +H 2 O (sal alembroth). Sol. in 0.66 pt. H 2 at 10, and in nearly every proportion of hot H 2 O. NH 4 C1, HgCl 2 . Easily sol. in H 2 0. + ^H 2 O. Easily sol. in H 2 O. (Kane.) 2NH 4 C1, 3HgCl 2 +4H 2 O. Easily sol. in H 2 O. (Holmes, C. N. 6. 351.) NH 4 C1, 2HgCl 2 . Very sol. in H 2 O. (Ray, Chem. Soc. 1902, 81. 648.) NH 4 C1, 5HgCl 2 . (Stromholm, J. pr. 1902, (2) 66. 441.) Ammonium mercuric sodium chloride, NH 4 C1, HgCl 2 , 4NaCl (?). Sol. in H 2 O. (Kossmann, A. ch. (3) 27. 243.) Ammonium molybdenum chloride, 2NH 4 C1, MoCl 3 +H 2 O. Very sol. in H 2 0. Nearly insol. in alcohol and ether. (Chilesotti, C. C. 1903. II, 652.) /See also Ammonium chloromolybdenum chloride. Ammonium molybdenum chloride iodide. See Ammonium chloromolybdenum iodide. 34 AMMONIUM MOLYBDENYL CHLORIDE -Ammonium molybdenyl chloride, 2NH 4 C1, Mo0 2 Cl 2 +2H 2 O. (Weinland, Z. anorg. 1905, 44. 98.) 2NH 4 C1, MoOCl 3 . Sol. in H 2 O; insol. in H 2 O sat. with HC1. (Klason, B. 1901, 34. 149. Ammonium nickel chloride, NH 4 C1, NiCl 2 + 6H 2 0. Deliquescent in moist air. Easily sol. in H 2 O. (Hautz.) 4NH 4 C1, NiCl 2 +7H 2 O (?). Ammonium osmium tetrachlonde. See Chlorosmate, ammonium. Ammonium osmium sesgm'chloride. See Chlorosmite, ammonium. Ammonium osmyl chloride, (NH 4 ) 2 OsO 2 Cl 4 . Sol. in H 2 O. Decomp. by HC1. (Wintre- bert, A. ch. 1903, (7) 28. 92.) Ammonium osmyl oxy chloride, (NH 4 ) 2 Os0 3 Cl 2 . Very si. sol. in H 2 0. Sol. in KOH+Aq with decomp. (Wintrebert, A. ch. 1903, (7) 28. 116.) Ammonium palladium chlorides. See Chloropalladate, ammonium and chloro- palladite, ammonium. Ammonium rhodium bichloride, 4NH 4 C1, RhCl 2 +3^H 2 O. Sol. in H 2 0, but decomp. slowly. (Willm. B. 16. 3033.) Does not exist. (Leidie, A. ch. (6) 17. 277.) Ammonium rhodium trichloride. See Chlororhodite, ammonium. Ammonium rhodium chloride ammonium nitrate, Rh 2 Cl 6 , 6NH 4 C1, 2NH 4 NO 3 . See Chlororhodite nitrate, ammonium. Ammonium ruthenium trichloride. See Chlororuthenite, ammonium. Ammonium ruthenium tefrachloride. See Chlororuthenate, ammonium. Ammonium tellurium chloride. See Chlorotellurate, ammonium. Ammonium thallic chloride, 3NH 4 C1, T1C1 3 . Easily sol. in H 2 O. (Wilhn.) +2H 2 O. Easily sol. in H 2 O and alcohol. (Nickles, J. Pharm. (4) 1. 28.) Ammonium thorium chloride, 8NH 4 C1, ThCL +8H 2 0. Sol. inH 2 0. (Chydenius.) Ammonium tin (stannous) chloride (ammon- ium chlorostannite), NH 4 C1, SnCl 2 +H 2 O. Decomp. by H 2 O. Resembles K salt (Richardson, Am. Ch. J. 14. 93.) 2NH 4 C1, SnCl 2 +H 2 O. Sol. in H 2 O, but decomp. by boiling. (Rammelsberg.) Contains 2H 2 O. (Richardson.) 4NH 4 C1, SnCl 2 +3H 2 O. Decomp. by H,O. (Poggiale, C. R. 20. 1182.) Does not exist. (Richardson.) Ammonium tin (stannic) chloride. See Chlorostannate, ammonium. Ammonium titanium chloride, 2NH 4 C1, TiCl 4 -t-2H 2 0. Ppt.; decomp. in moist air; sol. in fuming HC1; insol. in ether. (Rosenheim, Z. anorg. 1901, 26. 242.) Ammonium titanium chloride, 3NH 4 C1, TiCl 4 . Sol. in H 2 O. 6NH 4 C1, TiCl 4 . Sol. inH 2 O. (Rose.) Ammonium tungsten chloride, (NH 4 ) 3 W 2 C1 9 = 3NH 4 C1, 2WC1 3 . Easily sol. in H 2 O. Nearly insol. in most organic solvents. (Olsson, B. 1913, 46. 577.) Ammonium uranyl chloride. Very deliquescent, and sol. in H 2 O. (Peli- got.) 2NH 4 C1,(UO 2 )C1 2 +2H 2 O. Solution at 15 contains in 100 g. 3.51 g., NH 4 , 40.67 g. UO 2 and 19.15 g. Cl, hence there is considerable decomp. (Rimbach, B. 1904, 37. 466.) Ammonium vanadium chloride, 2NH 4 C1. VC1 3 +H 2 O. Difficulty sol. in H 2 O and alcohol. (Stabler, B. 1904, 37. 4412.) Ammonium zinc chloride, NH 4 C1, ZnCl 2 -f- 2H 2 O. Deliquescent. Very sol. in H 2 O. (Hautz, A. 66. 287.) 2NH 4 C1, ZnCl 2 . Sol. in H 2 O. (Rammels- berg, Pogg. 94. 507.) +H 2 O. Deliquescent in moist air. Sol. in 2 /a pt. cold H 2 O with absorption of heat. Sol. in 0.28 pt. hot H 2 O (Golfier-Bassayre, A. ch. 70. 344) ; sol. in 1 A pt. cold H 2 O. (Hautz, A. 66. 287.) 3NH 4 C1, ZnCl 2 . Sol. in H 2 O. (Marignac.) +H 2 O. (Berthelot, A. ch. (6) 11. 294.) 4NH 4 C1, ZnCl 2 . (Deh6rain.) 6NH 4 C1, ZnCl,+ViH,0. (Berthelot, I.e.) Ammonium chloride zinc oxychloride, 2ZnCl 2 , 8NH 4 C1, ZnO. Sol. in a little H 2 O, but decomp. by excess. (Andre.) 3ZnCl 2 , 10NH 4 C1, ZnO. As above. (Andre, A..ch. (6)3.88.) Ammonium chloride antimony fluoride. NH 4 C1, SbF 3 . Easily sol. in H 2 0. (de Haen, B. 21. 901 R.) Ammonium chloride arsenic inoxide. See Arsenite chloride, ammonium. AMMONIUM MANGANIC FLUORIDE 35 e, Ammonium chloride bismuth bromide. 3NH 4 C1, BiBr 3 +H 2 O. Deliquescent; decomp. by H 2 O. (Muir, Chem. Soc. 31. 148.) 2NH 4 C1, BiBr 3 +3H 2 O. Decomp. by H 2 O. (Muir.) 5NH 4 C1, 2BiBr 3 +H 2 O. Decomp. by H 2 O. (Muir.) Ammonium chloride chromic oxychloride. 2NH 4 C1, CrOCl 3 . Decomp. in the air. Sol. in cone. HC1 without decomp. (Weinland, B. 1906, 39. 4045.) Ammonium chloride cuprocupric thiosulphat 2NH 4 C1, Cu 2 O, CuO, 3S 2 O 2 . See Thiosulphate ammonium chloride, cuprocupric. Ammonium chloride lead iodide. 3NH 4 C1, PbI 2 . Decomp. with H->O. (Behrens, Pogg. 62. 252.) 4NH 4 C1, PbIo+2H 2 O. Decomp. with H 2 0. (Poggiale, C. R. 20. 1180.) Ammonium chloride mercuric bromide. NH 4 Ci, HgBr 2 . (Edhem-Bey, Dissert. 1885.) Ammonium chloride platinum sulphite. See Chloroplatosulphite, ammonium. Ammonium chloride tin (stannous) bromide, 2NH 4 C1, SnBr 2 +H 2 O. Sol. in H 2 O. (Raymann and Preis, A. 223. 323.) Ammonium cfo'chloroiodide, NH 4 Cl2l. Slowly decomp. when exposed to dry air at ord. temp. Very sol. in H 2 O. (Chattaway, Chem. Soc. 1915, 107. 107.) Ammonium tefrachloroiodide, NH 4 C1 4 I. Decomp. in the air. (Chattaway, Chem. Soc. 1915, 107. 107.) Ammonium lead chloroiodide, NH 4 PbClI 2 + 2H 2 and (NH 4 ) 2 PbCl 2 I 2 +2H 2 O. Sol. in KOH+Aq and in strong acids; de- comp. by H 2 O. (Fonzes-Diacon, Bull. Soc. 1897, (3) 17. 348.) Ammonium fluoride, NH 4 F. Abundantly sol. in H 2 O; si. sol. in alcohol. (Marignac, Ann. Min. (5) 15. 221.) Insol. in liquid NH 3 . (Ruff and Geisel, B. 1903, 36. 820.) Almost insol. in liquid NH at 50. (Mois- san, C. R. 1901, 133. 713.) Sol. in methyl alcohol. (Carrara, Gazz. ch. it. 1896, 26. 119.) Ammonium hydrogen fluoride, NH 4 F, HF. Deliquescent in moist air. Sol. in H 2 O. Ammonium antimony fluoride, 2NH 4 F, SbF 3 . Deliquescent; sol. in 0.9 pt. cold H 2 O. Insol. in alcohol or ether. (Fluckinger, A. 84. 248.) NH 4 F, 4SbF 3 . 3 pts. sol. in 2 pts. H 2 O. (Raad and Hauser, B. 1890, 23. R. 125.) NH 4 F, SbF 5 . Easily sol. in H 2 O. (Marig- nac, A. 145. 239.) Ammonium bismuth fluoride, 2NH 4 F, BiF 3 . Insol. in H 2 O. Rather difficultly sol. in acids. (Helmholt, Z. anorg. 3. 115.) Ammonium cadmium fluoride, NH 4 F, CdF 2 . Insol. in H 2 O. Sol. in acids on boiling. (Helmholt, Z. anorg. 3. 115.) Ammonium chromium fluoride, 3NH 4 F, CrF 3 . Easily sol. in H 2 O. SI. sol. in NH 4 F+Aq. (Petersen, J. pr. (2) 40. 52.) 2NH 4 F,CrF 3 +H 2 O. (Wagner, B. 19. 896.) Ammonium cobaltous fluoride, 2NH 4 F, CoF 2 +2H 2 0. SI. sol. in H 2 O. (Wagner, B. 19. 896.) Easily sol. in H-O. (Helmholt, Z. anorg. 3. 132.) Ammonium columbyl fluoride. See Fluoxycolumbate, ammonium. Ammonium columbium fluoride oxyfluoride, 3NH 4 F, CbF 6 , CbOF 3 . See Fluoxycolumbate columbium fluoride, ammonium. Ammonium copper fluoride, 2NH 4 F, CuF 2 + 2H 2 0. Insol. in H 2 O. (Helmholt, Z. anorg. 3. 115.) Nearly insol. in H 2 O but decomp. thereby. (Haas, Ch. Z. 1908, 32. 8.) Ammonium glucinum fluoride, 2NH 4 F, G1F 2 . Sol. in H 2 O. (Marignac, A. ch. (4) 30. 51.) Very sol. in H 2 O. (Helmholt, Z. anorg. 3. 130.) Ammonium iron (ferrous) fluoride, 2NH 4 F, FeF 2 . (Wagner, B. 19. 896.) NH 4 F, FeF 2 -f-2H 2 O. (W.) Ammonium iron (ferric) fluoride, 2NH 4 F, FeF 3 . More sol. in H 2 O than the corresponding K compound. Decomp. by boiling. (Nickles, J. Pharm. (4) 7. 15.) 3NH 4 F, FeF 8 . SI. sol. in H 2 0. (Marignac, A. ch. (3) 60. 306.) EasUy sol. in acids. (Helmholt, Z. anorg. 3. 124.) Ammonium manganic fluoride, 2NH 4 F, MnF 4 . More sol. than the K salt. (Nickles, C. R 65. 107.) 36 AMMONIUM MANGANYL FLUORIDE True Composition is 4NH 4 F, Mn 2 F 6 . (Chris- tensen, J. pr. (2) 34. 41.) See also Fluomanganate, ammonium. Ammonium manganyl fluoride. See Fluoxymanganate, ammonium. Ammonium molybdenum fluoride. Insol. in H 2 O. Sol. in HCl+Aq. (Berze- lius.) See also Fluomolybdate, ammonium. Ammonium molybdenyl fluoride. See Fluoxymolybdate, ammonium. Ammonium nickel fluoride, 2NH 4 F, NiF 2 + 2H 2 0. Sol. in H 2 O. (Wagner, B. 19. 896.) Easily sol. in H 2 O. (Helmholt, Z. anorg. 3. 143.) Ammonium scandium fluoride, (NH 4 ) 3 ScF 6 . Easily sol. in H2p. Aqueous solution is liot decomp. by boiling. Decomp. by acids. (R. I. Meyer, Z. anorg. 1914, 86. 275.) Ammonium silicon fluoride. See Fluosilicate, ammonium. . Ammonium silver fluoride, 2NH 4 F, AgF+ H 2 O. Not hydroscopic. Sol. in H 2 O; sol. in cone. NH 4 F+Aq. Sol. in alcohol. (Griitzner, Arch. Pharm. 1900, 238. 3.) 15NH 4 F, AgF+4H 2 O. More deliquescent than NH 4 F. (Bohm, Dissert. 1906.) Ammonium tantalum fluoride. See Fluotantalate, ammonium. Ammonium tantalyl fluoride. See Fluoxytantalate, ammonium. Ammonium tellurium fluoride, NH 4 F, TeF 4 . Decomp. by H 2 0. (Hogbom, Bull. Soc. (2) 35. 60.) Ammonium tin (stannous) fluoride, 2NH 4 F, SnF 2 +2H 2 O. Sol. in H 2 O. (Wagner, B. 19. 896.) Ammonium tin (stannic) fluoride, 2NH 4 F, SnF 4 . See Fluostannate, ammonium. Ammonium titanium sesquifiuonde. See Fluotitanate, ammonium. Ammonium titanyl fluoride. See Fluoxypertitanate, ammonium. Ammonium tungstyl fluoride. See Fluoxytungstate, ammonium. Ammonium uranyl fluoride. See Fluoxyuranate, ammonium. Ammonium vanadium ses^mfluoride. See Fluovanadate, ammonium. Ammonium vanadyl fluoride. See Fluoxyvanadate, ammonium. Ammonium zinc fluoride, 2NH 4 F, ZnF 2 . Sol. inH 2 0. (R. Wagner.) +2H 2 O. Very si. sol. in H 2 O. Easily sol. in dil. acids. (Helmholt.) Ammonium zirconium fluoride. See Fluozirconate, ammonium. Ammonium fluoride manganic oxyfluoride, 2NH 4 F, MnOF 2 . Precipitate. (Nickles.) See also Fluoxymanganate, ammonium. Ammonium fluoride molybdenum dioxide, 2NH 4 F, Mo0 3 . Decomp. by H 2 O. (Mauro. Gazz. ch. it. 18. 120.) Ammonium fluoride tungsten oxyfluoride. See Fluoxytungstate, ammonium. Ammonium fluoride tungsten oxyfluoride ammonium tungstate, 4NH 4 F, WO 2 F 2 , (NH 4 ) 2 W0 4 . See Fluoxytungstate tungstate, ammonium. Ammonium fluoride vanadium oxyfluoride. See Fluoxyvanadate, and fluoxyhypovana- date, ammonium. Ammonium hydroselenide, NH 4 HSe. Sol. in H 2 O with decomp. (Bineau, A. ch. (2) 67. 229.) Ammonium hydrosulphide, NH 4 SH. Sol. in H 2 and alcohol. Solutions decomp. on air. Ammonium hydroxide, NH 4 OH. See Ammonia, Ammonium imidosulphamide, (S 2 O 4 N 3 H 4 )NH 4 . (Hantzsch, B. 1905, 38. 1033.) Ammonium iodide, NH 4 I. Very deliquescent. Sol. in 0.60 pt. H 2 O. (Eder, Dingl. 221. 89.) Sp. gr. of aqueous solution of NH 4 I at 18 containing 10 20 30 40 50%NH 4 I. 1.0652 1.1397 1.2260 1.3260 1.4415 (Kohlrausch, W. Ann. 1879. 1.) NH 4 I+Aq containing 12.51% NHJ has sp.gr. 20/20 = 1.0846. NH 4 I+Aq containing 19.19% NHJ has sp. gr. 20/20 = 1.1359. (Le Blanc and Rohland, Z. phys. Ch. 1896, Very easily sol. in liquid NH 3 . (Franklin Am. Ch. J. 1898, 20. 826.) Very sol. in liquid NH 3 at 50. (Moissan, C. R. 1901, 133. 713.) AMMONIUM ZINC IODIDE 37 Sol. in SOC1 2 . (Walden, Z. anorg. 1900, 25. 216.) Sol. in liquid SO 2 . (Walden, Z. anore. 1902, 30. 160.) Sol. in 4.0 pts. abs. alcohol. (Eder, I.e.} " 210 " ether. (Eder, I.e.) " 20 " alcohol-ether (1 : 1). (Eder, l.c-.) Sol. in acetone. (Eidmann, C.C. 1899, II. 1014.); (Naumann, B. 1904, 37. 4328.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. "314.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Ammonium (Modide, NH 4 I 2 . Sol. in alcohol, ether, CS 2 , and KI+Aq; less sol. in chloroform. (Guthrie, Chem. Soc. (2) 1. 239.) Ammonium imodide, NHJs. SI. deliquescent. Sol. in little H 2 O, but decomp. by much H 2 O. (Johnson, Chem. Soc. 33. 397.) Ammonium antimony iodide, NH 4 I, SbI 3 + 2H 2 O. Decomp. by H 2 O. (Nickles, C. R. 51. 1097.) 3NHJ, 4SbI 3 +9H 2 O. Decomp. by H 2 0, with separation of SbOI. Sol. in HC 2 H 3 O 2 , HC1, and H 2 C 4 H 4 O6+Aq. Decomp. by CS 2 . (Schaffer, Pogg. 109. 611.) 3NH 4 I, SbI 3 +3H 2 O. As above. 4NHJ, SbI 3 +3H 2 O. As above. Ammonium bismuth iodide, NH 4 I, BiI 3 + H 2 0. Deliquescent; decomp. by H 2 O. (Nickles, C. R. 51. 1097.) 4NHJ, BiI 3 +3HoO. As above. (Linau, Pogg. 111. 240.) 2NHJ, BiI 3 +2KH 2 O. Decomp. by H 2 O, or MCI, MBr, or MI+Aq. (Nickles, J. pr (2) 39. 116.) Ammonium cadmium iodide, 2NH 4 I, CdI 2 + 2H 2 O. Deliquescent. (Croft.) Sol. at 15 in 0.58 pt. H 2 O, 0.70 pt. abs. alcohol., 8.9 pts. ether (sp. gr. 0.729), and 1.8 pts. alcohol-ether (1:1). (Eder, Dingl 221. 89.) 100 pts. of the solution in H 2 contain 85.91 pts. of the salt at 14.5. (Rimbach, B. 1905 38. 1563.) NH 4 I, CdI 2 +HH 2 0. Sol. at 15 in 0.90 pt. H 2 O, 0.88 pt. abs. alcohol, and 2.4 pts ether (sp. gr. 0.729). (Eder, l.c.) +H 2 O. (Grossmann, Z. anorg. 1902, 33 154.) Ammonium chloromolybdenum iodide, 2NH 4 I, Cl 4 Mo 3 I 2 +2H 2 0. Decomp. by H 2 O. Cryst. from HI+Aq. (Blomstrand.) Ammonium cuprous iodide, 2NH 4 I, Cu 2 I 2 + H 2 O. Decomp. on the air, or by H 2 O, or alcohol. Saglier, C. R. 104. 1440.) -J-KH2O. Decomp. by H 2 O with separa- tion of Cu 2 I 2 . (Gossner, Zeit. Kryst. 1903, 38. 501.) Ammonium cupric iodide ammonia, 2NH 4 I, CuI 2 , 2NH 3 +2H 2 0. Insol. in H 2 O or alcohol; si. sol. in NH 4 OH +Aq. +6H 2 O. Unstable. (Saglier, C. R. 104. 1440.) NH 4 I, 2CuI 2 , 3NH 3 . (Fleurent, C. R. 1891, 113. 1047.) Ammonium iridium (Modide, 2NH 4 I, IrI 2 . Insol. in cold or hot H 2 O, and in alcohol. Sol. in warm dil. acids. (Oppler.) Ammonium iridium sesgmiodide. See lodiridite, ammonium. Ammonium iridium tefraiodide. See lodiridate, ammonium. Ammonium lead iodide, NH 4 I, PbI 2 +2H 2 O. Decomp. by much H 2 0. (Wells, Sill. Am. J. 146. 25.) 4NHJ,3PbI 2 +6H 2 O. SI. sol. in H 2 0. (Mosnier, C. R. 1895, 120. 444.) Sol. in H 2 with decomp. Sol. in strong KOH+Aq and in strong acids. (Fonzes- Diacon, Bull. Soc. 1897, (3) 17. 347.) Ammonium magnesium iodide, NH 4 I, MgI 2 +6H 2 O. Very deliquescent. (Lerch, J. pr. (2) 28. 338.) Ammonium mercuric iodide, NHJ, HgI 2 + H 2 O. Decomp. into its constituents by H 2 O. (Boullay, A. ch. (2) 34. 345.) Sol. without decomp. in alcohol and ether. NHJ, 2HgI 2 . Decomp. by H 2 O. Sol. in KI+Aq. Very sol. in alcohol, ether and nitrobenzol. (Low, Zeit. Kryst, 51. 138.) Ammonium silver iodide, 2NH J, Agl. Deliquescent. Decomp. by H 2 O. (Pog- giale.) Ammonium thallic iodide, NHJ, T1I 3 . Sol. in H 2 O. (Nickles, J. Pharm. (4) 1. 32.) Ammonium tin (stannous) iodide, NHJ, SnI 2 . Decomp. by small amt. H 2 O but completely sol. in a large amt. (Boullay, A. ch. (2) 34. 376.) + 1KH 2 O. (Personne.) Ammonium zinc iodide, 2NH J, ZnI 2 . Extremely deliquescent, and sol. in H 2 O. (Rammelsberg, Pogg. 43. 665.) 38 AMMONIUM IODIDE ARSENIC OXIDE NHJ, ZnI 2 +4^H 2 O. Hydroscopic. (Ephraim, Z. anorg. 1910, 67. 384.) Ammonium iodide arsenic trioxide. See Arsenite iodide, ammonium. Ammonium cobalt nitride. See Ammonium cobalt azoimide. Ammonium ruthenium cfohydronitrosobrom- ide, NO.Ru 2 H 2 (NH 3 ) 6 Br 3 .2HBr. Ppt. (Brizard, A. ch. 1900, (7) 21. 363.) Ammonium ruthenium nitrosochloride, 3NH 4 C1.2HCl.NORu 2 H 2 Cl 3 . Ppt. (Brizard, A. ch. 1900, (7) 21. 354.) Ammonium ruthenium dihydronitrosochlor- ide, NO.Ru 2 H 2 (NH 3 ) 6 Cl 3 .2HCl. Ppt. (Brizard, A. ch. 1900, (7) 21. 358.; Ammonium peroxide, (NH 4 ) 2 O 2 . M.-pt. 2. SI. sol. in ether without decomp. (D'Ans, B. 1913, 46. 3076.) Sol. in alcohol; insol. in ether; decomp. slowly in aq. solution. (Melikoff, B. 1897, 30. 3145.) Ammonium hydrogen peroxide, (NH 4 ) 2 O 2 , H 2 O 2 . Decomp. at ordinary temp. (Melikoff, B. 1898, 31. 447.) -fH 2 O. Unstable; deliquesces at ordinary temp.; sol. in alcohol; insol. in light petroleum. (Melikoff, B. 1898, 31. 152.) Ammonium selenide, (NH 4 ) 2 Se. Sol. in H 2 O with decomp. (Bineau, A. ch. (2) 67. 229.) Stable in- the air. Sol. in H 2 O; aq. solution decomp. slowly. (Lenher and Smith, J. Am. Chem. Soc. 1898, 20. 277.) Ammonium hydrogen selenide, NH 4 HSe. Sol. in H 2 O. (Fabre, C. R. 103. 269.) Ammonium raonosulphide, (NH 4 ) 2 S. Decomp. on air. Sol. in H 2 O, but solution decomposes rapidly. Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) ' Ammonium disulphide, (NH 4 ) 2 S 2 . Sol. in H 2 O with decomp. Does not exist. (Bloxam, Chem. Soc. 1895, 67. 293.) Ammonium tefrasulphide, (NH 4 ) 2 S 4 . Easily sol. in H 2 O. Cone, solution is stable, dil. solution decomp. on air. Easily sol. in alcohol without decomp., but solution de- comp. on the air more rapidly than the aqueous solution. (Fritzsche, J. pr. 32. 313.) + KH 2 O. When dissolved in H 2 O, it is at once dissociated with deposition of S. (Blox- am, Chem. Soc. 1895, 67. 303.) Ammonium pen/asulphide, (NH 4 ) 2 S 5 . Decomp. on air. Sol. in H 2 with separa- tion of S. Sol. in alcohol without decomp., but solution decomposes quickly on standing. (Fritzsche, J. pr. 32. 313.) Rapidly decomp. by H 2 O with separation of S. (Bloxam, Chem. Soc. 1895, 67. 298.) +H 2 O. Decomp. by H<>O with separation of S. (Bloxam, Chem." Soc. 1895, 67. 298.) Ammonium fteptasulphide, (NH 4 ) 2 S 7 . More stable on air, and less easily decom- posed by H 2 O than (NH 4 ) 2 S 6 . + lVsH 2 O. Decomp. by H 2 O with separa- tion of S. Slowly attacked by dil. HCl+Aq. (Bloxam, Chem. Soc. 1895, 67. 307.) T^rammonium hepta sulphide, (NH 4 ) 4 S 7 + 4H 2 O. Sol. in H 2 O. Solution can be kept for a long time without depositing S. (Bloxam, Chem. Soc. 1895, 67. 298.) Diammonium ennea sulphide, (NH 4 ) 2 S 9 + Decomposed by H 2 O with separation of S. Not attacked by boiling dil. HCl+Aq on account of formation of a hard crust of S on the crystals. (Bloxam, Chem. Soc. 1895. 67. 306.) Teirammonium enneasulphide, (NH 4 ) 4 S9. Solution in H 2 O deposits crystals of (NH 4 ) 2 S 5 on standing. (Bloxam, Chem. Soc. 1895, 67. 302.) +3HH 2 O. Decomp. by H 2 O with separa- tion of S. (Bloxam, Chem. Soc. 1895, 67. 299.) Ammonium po^sulphides. Cone. NH 3 +Aq dissolves H 2 S to form (NH 4 ) 2 S,2NH 4 SH. On dilution more H 2 S is absorbed to form (NH 4 ) 2 S,4NH 4 SH, then (NH 4 ) 2 S,8NH 4 SH, then (NH 4 ) 2 S,18NH 4 SH and finally NH 4 SH. (Bloxam, Chem. Soc. 1895, 67. 284.) Ammonium copper sulphide, (NH 4 ) 2 S, 2CuS 3 (?). Sol. in warm H 2 O, but decomp. on standing. Warm KOH+Aq acts similarly; si. sol. in NH 4 OH+Aq, Na 2 CO 3 +Aq, or absolute al- cohol. Insol. in ether. Decomp. by dil acids riwoznik, B. 6. 1291.) Correct formula is NH 4 CuS 4 . SI. sol. in H 2 p. Decomp. by cone, and dil. acids. Easily sol. in NaOH. SI. sol. in alcohol Biltz, B. 1907, 40. 976.) Ammonium gold pofysulphide, AuS 3 NH 4 . Ppt. (Hofmann, B. 1903, 36. 3092- B 1904, 37. 245.) Ammonium iridium pentadecasulphide, IrS l5 (NH 4 ) 3 . Ppt. (Hofmann, B. 1904, 37. 247.) ANTIMONIC ACID 39 Ammonium palladium imrfecasulphide. Ppt. (Hofmann, B. 1904, 37. 248.) Ammonium platinum pentadecasulphide, PtS 16 (NH 4 ) 2 +2H 2 0. Can be washed with CS 2 without decomp. Sol. in alcohol. Insol. in ether. (Hofmann, B. 1903, 36. 3091.) Ammonium stannic sulphide. See Sulphostannate, ammonium. Ammonium telluride, NH 4 HTe. Easily sol. in H 2 O. (Bineau, A. ch. (2) 67. 229.)' Ammonium sulphide ammonia. (NH 4 ) 2 S, 2NH 3 . Very unstable. (Bloxam, Chem. Soc. 1895, 67. 294.) Ammonium acz'sulphomelid, (NSO.ONH 4 ) 3 (?) (Hantzsch and Stuer, B. 1905, 38. 1039.) AmmonplatinrJ/amine comps. See Platin^n'amine comps. Ammoncfa'sulphonic acid, NH 3 (S0 3 H) 2 . Known only in its salts. (Claus, A. 158. 52 and 194.) Contains 2 at. H less, and is identical with imidosulphonic acid NH(SOsH) 2 , which see. (Raschig, A. 241. 161.) Ammonin'sulphonic acid, NH 2 (S0 3 H) 3 . Known only in its salts. (Claus, A. 158. 52 and 194.) Contains 2 at. H less, and is nitrilosulphonic acid N(SO 3 H) 3 , which see. (Raschig, A. 241. 161.) Ammontoasulphonic acid, NH(SO 3 H) 4 . Known only in its salts. (Claus, A. 168. 52 and 194.) Does not exist, but was impure nitrilosul- phonic acid, which see. (Raschig, A. 241. 161.) Anhydroarseniotungstic acid, See under Arseniotungstic acid. Anhydrooxycobaltamine chloride, Co 2 (NH 3 ) 10 [ (OH)1 Easily sol. in H 2 O, but decomposes after a few minutes; can be recrystallized from dil. HCl+Aq. Precipitated from sat. H 2 O solu- tion by cone. HCl+Aq, or alcohol. (Vort- mann, M. Ch. 6. 404.) Co 2 (NH 3 ) 10 mann.) Anhydrooxycobaltamine chloride mercuric chloride, Co 2 (NH 3 ) 10 (C10 2 H)Cl 4 , 3HgCl 2 . Can be recryst. from very dil. hot HCl+Aq. chloroplatinate, Co 2 (NH 8 )io(ClO 2 H)Cl 4 , 2PtCl 4 . Can be recrystallized from H 2 O containing HC1. chloronitrate, Co 2 (NH 3 ) 10 Cl(O.OH)(N0 3 ) 4 +H 2 0. Can be recrystallized from dil. HCl+Aq. Co 2 (NH 3 ) 10 Cl(O.OH)Cl 2 (N0 3 ) 2 +H 2 O. More easily sol. in H 2 O than the preceding comp. chlorosulphate, Co 2 (NH 3 ) 10 Cl(O.OH)(S0 4 ) 2 . cftchromate, [Co 2 (NH 3 ) 10 O.OH] 2 (Cr 2 7 )5 +8H 2 O. SI. sol. in H 2 O. nitrate, Co 2 (NH 3 ) 10 (NO 3 )(O.OH)(NO 3 ) 4 +H 2 0. SI. sol. in pure H 2 O with immediate decomp. Can be recrystallized from H 2 O containing HNO 3 . sulphate, [Co 2 (NH 3 ) 10 O . OH] 2 (SO 4 ) 6 , 2H 2 SO 4 +2H 2 O. SI. sol. in cold H 2 O. When crystallized from dil. H 2 SO 4 +Aq, is converted into [Co 2 (NH 3 ) 10 O.OH] 2 (S0 4 ) 6 ,H 2 S0 4 +3H 2 0, which by further recrystallization from very dil. H 2 SO 4 +Aq becomes [Co 2 (NH 3 ) 10 O.OH] 2 (SO 4 )5+8H 2 O. SI. sol. in cold H 2 O. (Vortmann.) Anhydrophospholuteotungstic acid, H 3 PW 8 28 . See under Phosphotungstic acid. Antimonic Acid. Mefantimonic acid, HSb0 3 . Very si. sol. in H 2 O; sol. in cone. HCl+Aq; si. sol. in dil. HNO 3 +Aq; easily sol. in tar- taric acid+Aq; easily sol. in hot KOH, or NaOH+Aq; completely insol. in NH 4 OH+ Aq. (Fremy, A. ch. (3) 23. 407.) SI. sol. in H 2 O. Very si. sol. in KOH and K 2 C0 3 +Aq. Insol. in NH 4 OH+Aq. Insol. in HNO 3 +H 2 SO 4 . Slowly sol. in cold, quickly in hot HCl+Aq. SI. sol. in tartaric and oxalic acid and in KHC 2 O 4 + Aq. (Senderens, Bull. Soc. 1899, (3) 21. 48.) Insol. in acetone. (Naumajm, B. 1904, 37. 4329.) Pf/roantimonic acid, H 4 Sb 2 O7. More sol. in H 2 O and acids than H 3 SbO 4 . Sol. in cold NH 4 OH, or KOH+Aq. (Fremy.) Slowly sol. in cold H 2 O. 5.88 g. Sb 2 O 5 in 1 1. H 2 O at 15 8.55 " " " 1 1. " " 25 21.30 " " " 1 1. " " 60 (Delacroix, J. Pharm. 1897, 6. 337-41.) 40 ANTIMONIC ACID SI. sol. in H 2 O. Very si. sol. in KOH and K 2 CO 3 +Aq. Insol. in NH 4 OH+Aq, and in HNO 3 +H 2 SO 4 . Slowly sol. in cold, quickly in hot HCl+Aq. SI. sol. in tartaric acid, oxalic acid and KHC 2 O 4 +Aq. (Senderens, Bull. Soc. 1899, (3) 21. 48.) Or^oantimonic acid, H 3 Sb0 4 . SI. sol. in H 2 O. Insol. in NH 4 OH+Aq. Easily sol. in KOH+Aq. (Fremy.) Does not exist. (Raschig, B. 18. 2745.) Has, however, been prepared by Daubrawa (A. 186. 110), Conrad (C. N. 40. 198), and Beilstein and Blaese (Bull. Ac. St. Petersb. 33. 97). Very sol. in H 2 O. (Delacroix, Bull Soc. 1899 (3) 21. 1049.) Very si. sol. in H 2 0, in KOH and K 2 CO 3 + Aq. Slowly sol. in cold, quickly in hot HC1 + Aq. Insol. in NH 4 OH+Aq, and in HN0 3 + H 2 SO 4 . SI. sol. in tartaric acid, oxalic acid and KHC 2 O 4 +Aq. (Senderens, Bull. Soc. 1899, (3) 21. 52.) + HH 2 O. (Beilstein and Blaese.) According to Beilstein and Blaese only one antimonic acid, H 3 SbO 4 , exists. TWrantimonic acid, Sb 2 O 5 +4H 2 0=H 8 Sb 2 O 9 . Slowly sol. in cold H 2 0. Solution sat. at t contains g. Sb 2 O 5 per litre t 15 25 60 70 g. Sb 2 6 5.88 8.3-8.75 21.30 53.89 Decomp. in solution by heating to 100 or long standing in the cold to Sb 2 O 5 , 3H 2 O. (Delacroix, Bull. Soc. 1899, (3) 21. 1049.) Insol. in H 2 O. Very si. sol. in KOH and K 2 CO 3 +Aq. Slowly sol. in cold, quickly in hot HCl+Aq. Insol. in NH 4 OH+Aq. Insol. in HNO 3 +H 2 SO 4 . SI. sol. in tartaric acid, oxalic acid and in KHC 2 O 4 + Aq. (Senderens, Bull. Soc. 1899, (3) 21. 51.) #ezantimonic acid, Sb 2 O 5 +6H 2 O = Sol. in H 2 O to the extent of 22 g. Sb 2 O 6 per 1. but on standing becomes turbid and a white powder is pptd. until finally only 3 g. Sb 2 O 5 are dissolved per 1. (Senderens, Bull. Soc. 1899, (3) 21. 48-49.) Antimonates. a. Antimonates. From HSbO 3 . Some of the K and NH 4 salts are sol. in H 2 O, the others are slightly sol. or insol. ft. Pyroantimonates. From H 4 Sb 2 O7. As a class, insol. in H 2 O, but decomp. thereby ex- cept in presence of large excess of alkali (Fremy, A. ch. (3) 12. 499.) Probably do not exist. (Beilstein and Blaese.) Aluminum antimonate, A1 2 O 3 , 3Sb 2 O 5 (?). Ppt. Somewhat sol. in excess of Al salts +Aq. Insol. in K 4 Sb 2 O 7 +Aq. Al(Sb0 3 ) 3 +15H 2 = AlH 6 (Sb0 Ppt. (Beilstein and Blaese, Bull. Ac. St. Petersb. 33. 101.) Al(SbO 3 ) 3 + 7H 2 O = AlH 6 (SbO 4 ) 3 + 4H 2 O. Ppt. (B. and B.) A1 2 O 3 , Sb 2 O 5 +9H 2 O. Ppt. (Ebel, B. 22. 3043.) Ammonium antimonate, NH 4 SbO 3 +2H 2 O, Insol. in H 2 O. +2^H 2 0. Insol. in HoO. (Senderens, Bull. Soc. 1899, (3) 21. 56.) +6H 2 0. See (NH 4 ) 2 H 2 Sb 2 O 7 +5H 2 O. Ammonium pyroantimonate, (NH 4 ) 4 Sb 2 O 7 . Known only in solution. (NH 4 ) 2 H 2 Sb 2 O 7 +5H 2 O. Sol. in H 2 O, but decomp. by standing or boiling into insol. salt. Insol. in alcohol. (Fremy, J. pr. 45. 215). Composition is NH 4 SbO 3 +6H 2 O, according to Raschig (B. 18. 2743). Barium antimonate, Ba(SbO 3 ) 2 . Ppt. Scarcely sol. in H 2 O. Slowly sol. in BaCl 2 +Aq. +2H 2 G. Somewhat sol. in H 2 O. Easily sol. in HCl+Aq. (Delacroix, Bull. Soc. 1899, (3) 21. 1051.) +5, or 6H 2 O. Ppt. BaSb 4 O 7 +5H 2 O. Sol. in cone. HC1. (Dela- croix, Bull. Soc. 1899, (3) 21. 1051.) BaO, 3Sb 2 O 5 +5H 2 O. Insol. in H 2 O. In- completely sol. in HC1. (Delacroix, I.e.) BaO, 4SboO 5 +15H 2 O. (Delacroix, I.e.) 9BaO, 10Sb 2 5 + 18H 2 O. Insol. in HC1 + Aq. (Delacroix, I.e.) Bismuth antimonate, BiSbO 4 +H 2 O. Ppt. Insol. in H 2 O; sol. in HCl+Aq. (Cavazzi, Gazz. ch. it. 15. 37.) 3Bi 2 O 3 , Sb 2 O 6 +H 2 O. Insol. in H 2 O; sol. in HCl+Aq. (Cavazzi.) 2Bi 2 O 3 , Sb 2 O 5 . As above. (Cavazzi.) Cadmium antimonate, Cd(SbO 3 ) 2 +2H 2 O. Insol. in H 2 O. (Senderens, Bull. Soc. 1899. (3) 21. 56.) +3HH 2 O. Very sol. in H 2 O. Sol. in HC1 +Aq. (Ebel, Dissert. 1890.) +5H 2 O. Insol. in H 2 O. (Senderens, I.e.) +6H 2 O. Ppt. Insol. in H 2 0. (Ebel, B. 22. 3043.) Calcium antimonate, Ca(SbO 3 ) 2 . Ppt. +5H 2 O. Ppt. (Heffter, Pogg. 86. 418.) +6H 2 O. Insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 56.) 3CaO, 2Sb 2 O 6 +6H 2 O. Min. Ullmanite. Chromic antimonate, Cr(SbO 3 ) 3 +14H 2 O. Ppt. (Beilstein and Blaese.) Cobaltous antimonate, Co(SbO 3 ) 2 +5H 2 O. Insol. in H 2 O. Loses 3H 2 O in the presence of H 2 SO 4 and passes into Co(SbO 3 ) 2 +2H 2 O, ANTIMONATE, POTASSIUM 41 also insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 55.) +6H 2 O. Ppt. (Ebel, B. 22. 3043.) +7H 2 O. SI. sol. in H 2 O. SI. sol. in boiling solutions of cobalt salts. + 12H 2 O. Ppt. (Heffter, Pogg. 86. 448.) Cobaltous hydrogen antimonate, CoH 4 (SbO 4 ) 2 +H 2 0. (Gorgeul, Ann. Phys. Beibl. 1897, 21. 198.) Cupric antimonate, 3CuO, 2Sb 2 O 6 . Ppt. (Beilstein and Blaese.) Cu(SbO 3 ) 2 . Insol. in H 2 O, acids, or alkalies. (Berzelius.) +2H 2 O. Insol. in H 2 0. (Senderens, Bull. Soc. 1899, (3) 21. 55.) +5H 2 O. Ppt. (Ebel, B. 22. 3043.) Insol. in HoO. (Senderens, I.e.) CuO, 2Sb 2 O 6 +9H 2 O. Insol. in H 2 O. Sol. in Sb 2 O 6 , 4H 2 O+Aq. (Delacroix, Bull. Soc. 1899, (3) 21. 1054.) 2CuC, 3Sb 2 O 5 + 10H 2 O. Insol. in H 2 O. Sol. in NH 4 OH and in fn'antimonic acid-f-Aq. (Delacroix, I. c. CuO, 6Sb 2 O 5 + 16H 2 O. (Delacroix, I.e.) Cupric antimonate ammonia, Cu(SbO 3 ) 2 , 4NH 3 +4H 2 O. Insol. in HoO and NH 4 OH+Aq. (Schiff, A. 123. 39.) CuSb 2 N 3 H 21 O 12 = Cu(ONH 4 )OH, 2(NH 4 SbO 3 +2H 2 0). (Raschig, B. 18. 2743.) Cu(SbO 3 )o,3NH 3 +9H 2 O. (Delacroix, BuU. Soc. 1901, (3) 25. 289.) Glucinum antimonate, Gl(Sb0 3 ) 2 +6H 2 O. Somewhat sol. in hot H 2 O. Easily sol. in warm HC1. (Ebel, Dissert. 1890.) Iron (ferrous) antimonate. SI. sol. in H 2 O. (Berzelius.) Iron (ferric) antimonate. Insol. in H 2 O. (B.) Fe 2 O 8 , Sb 2 O 5 +7H 2 O. Ppt. (Ebel, B. 22 3043.) Fe 2 O 3 , 2Sb 2 O 5 + llH 2 O. Ppt. (Beilstein and Blaese.) Fe(SbO 3 ) 3 +6^H 2 O. Ppt. (B. and B.) Lead antimonate, basic, Pb 3 (SbO 3 ) 2 (OH) 4 + Pb 3 (SbO 4 ) 2 +4H 2 O. Min. Bleinerite, Bindheimite. 2Pb(SbO 3 ) 2 , PbO + llH 2 O. Ppt. (B. and B.) Lead antimonate, Pb(SbO 3 ) 2 . Insol. in H 2 O. Incompletely decomp. bj acids. (Berzelius.) Naples Yellow. Insol. in H 2 O. +2H 2 O. Insol. in H 2 O. (Senderens, Bull Soc. 1899, (3) 21. 57.) +5H 2 0. Ppt. (Ebel, B. 22. 3043.) +6H 2 O. Ppt. (Beilstein and Blaese.) +9H 2 O. Insol. in H 2 O. (Senderens, I.e.) Lead antimonate chloride, Pb(SbO 3 ) 2 , PbCl 2 . Min. Nadorite. Sol. in HC1, HNO 3 , and tartaric acid+Aq. Lithium antimonate, LiSbO 3 . SI. sol. in cold, sol. in hot H 2 0, and crys- tallizes on cooling. Much more sol. than NaSb0 3 . +3H 2 O. Ppt. SI. sol. in H 2 O. (Beilstein and Blaese.) Magnesium antimonate, Mg(SbO 3 ) 2 + 12H 2 O. Sol. in hot, less sol. in cold H 2 O. (Heffter.) Sol. in MgSO 4 +Aq; insol. in KSbO 3 +Aq. (Berzelius.) Manganous antimonate, Mn(SbO 3 ) 2 . Difficultly sol. in H 2 O. When heated, is sol. only in strong acids. +2H 2 O. Insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 56.) +5H 2 O. Ppt. (Ebel, B. 22. 3043.) +6H 2 O. Insol. in H 2 O. (Senderens, I.e.) -j-7H 2 O. Ppt. (Beilstein and Blaese.) Mercurous antimonate. Insol. in H 2 O. (Berzelius.) Mercuric antimonate, Hg(SbO 3 ) 2 . Insol. in H 2 O, alkalies, and most acids. SI. attacked by boiling H 2 SO 4 , and HC1+ Aq. +2H 2 O. Insol. in H,O. (Senderens, Bull. Soc. 1899, (3) 21. 55.) +5H-.O. Insol. in H 2 O. (Senderens.) +6H 2 O. Ppt. (Beilstein and Blaese.) Nickel antimonate, Ni(SbO 3 ) 2 +2H 2 O. Insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 54.) +5H 2 O. Insol. in H 2 O. (Senderens.) +6H 2 O. Ppt. Insol. in H 2 O. (Heffter, Pogg. 86. 446.) + 12H 2 O. SI. sol. in H 2 O. (Heffter.) Potassium antimonate, KSbO 3 . Insol. in H 2 O. Sol. in warm KOH+Aq, but separates nearly completely on cooling. By boiling with H 2 O, or by standing for a long time with cold H 2 O, it gradually dissolves as 2KSbO 3 +5H 2 O, or K 2 H 2 Sb 2 O 7 +4H 2 O, or 2KH 2 SbO 4 +3H 2 O. Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) +H 2 O. Insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 57.) +1^H 2 O (=2KSbO 3 +5H 2 O of Fremy). Easily sol. in H 2 O, especially if warm. Solu- tion is pptd. by NH 4 Cl+Aq. (Fremy, A. ch. (3) 12. 499.) +2^H 2 O. 100 pts. H 2 O at 20 dissolve 2.81 pts. anhydrous salt; sp. gr. of solution sat. at 18 = 1.0263. Composition is given as K 2 H 2 Sb 2 O 7 +4H 2 O. (Knorre and Olschewsky, B. 20. 3043.) . Insol. in H 2 O. (Senderens, I.e.) 42 ANTIMONATE, POTASSIUM +4^H 2 O. Sol. in H 2 O. (Delacroix, J Pharm. 1897, (6) 6. 533.) 2KoO, 3Sb 2 O 5 +10H 2 O. SI. sol. in H 2 O (Delacroix, J. Pharm. -1897, 6. 337.) + 10H 2 O. (Delacroix, I.e.) Potassium pT/roantimonate, K 4 Sb 2 O 7 . Deliquescent; decomp. by boiling with H 2 into KSb0 3 +5H 2 O, by cold H 2 O into K 2 H 2 Sb 2 O 7 +6H 2 O. (Fremy.) Does not exist. (Knorre and Olschewsky.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1904,37.3601.) Potassium hydrogen pf/roantimonate, K 2 H 2 Sb 2 O 7 . Insol. in acetone. (Eidmann, C. C. 1899, II. 1014.) +2^H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 57.) +3HH 2 O. Very difficultly sol. in hot or cold H 2 O. (Knorre and Olschewsky, B. 18. 2358.) +6H 2 O. Quite difficultly sol. in cold H 2 O. Not precipitated by NH 4 Cl+Aq. Aqueous solution gradually decomposes. (Fremy.) +4H 2 O. See 2KSbO 3 +5H 2 O. Potassium antimonate sulphantimonate, KSbO 3 , K 3 SbS 4 +5H 2 O. Decomp. on air, and with 'cold H 2 O. Sol. in hot H 2 O. (Rammelsberg.) Silver antimonate. Insol. in H 2 O. (Berzelius.) AgSbO 3 +3H 2 O=AgH 2 SbO 4 +2H 2 O. Eas- ily sol. in NH 4 OH+Aq, when freshly pptd. (Beilstein and Blaese.) +1>^H 2 O. Ppt. (Ebel, B. 22. 3043.) Silver antimonate ammonia, AgH 2 SbO 4 , 2NH 3 +H 2 0. (Beilstein and Blaese.) Sodium antimonate, NaSbO 3 . Sol. in much H 2 O, but soon becomes de- composed into Na 2 H 2 Sb 2 O 7 . +3HH 2 O, composition of Na 2 H 2 Sb 2 7 + 6H 2 O, according to Beilstein and Blaese. 1000 pts. H 2 O dissolve 0.31 pt. NaSbO 3 + 3HH 2 O at 12.3. 1000 pts. alcohol of 15.8% dissolve 0.13 pt. NaSbO 3 +3^H 2 O at 12.3. 1000 pts. alcohol of 25.6% dissolve 0.07 pt NaSb0 3 +3KH 2 at 12.3. Somewhat more sol. when freshly precipi- tated. Absolutely insol. in glacial HC 2 H 3 O 2 . Presence of NaOH or Na salts diminish sol- ubility, while NH 4 OH or K salts increase it slightly. (Beilstein and Blaese, Bull. Ac. St. Petersb. 33. 201.) +4^H 2 O. Sol. inH 2 0. (Delacroix, Bull. Soc. 1899, (3) 21. 1051.) 2Na 2 O, 3Sb 2 O 5 +10H 2 O. (Delacroix, I. c.) Na 2 O, 3Sb 2 O 6 +HH 2 O. (Delacroix, L c.) Sodium pvroantimonate, Na 2 H 2 Sb 2 O 7 + 6H 2 0. Boiling H 2 O dissolves yj^ pt. of this salt. (Fremy.) 1000 pts. H 2 O dissolve 2.5 pts. salt. (Ebel, B. 22. 3044.) See also NaSbO 3 + +5H 2 0. (Knorre and Olschewsky.) Strontium antimonate, Sr(Sb0 3 ) 2 +6H 2 0. Ppt. Less sol. in H 2 O than SrS0 4 . (Heff- ter, Pogg. 86. 418.) Thallous antimonate, TlSbO 3 +2HoO = TlH 2 SbO 4 +H 2 O. Somewhat sol. in H 2 O, when freshly precipi- tated; insol. when dried. (Beilstein and Blaese.) Tin (stannous) antimonate, 2SnO, Sb 2 O 5 . Ppt. (Lenssen, A. 114. 113.) Sn(SbO 3 ) 2 +2H 2 O. Attacked with difficulty by acids or alkalies, most easily by hot cone. H 2 SO 4 . (Schiff, A. 120. 55.) 2SnO, 3Sb 2 O 5 +4H 2 O. SnO, 2Sb 2 O 5 . Tin (stannic) antimonate. Insol. in H 2 O. (Levol, A. ch. (3) 1. 504.) Uranium antimonate, 5U0 2 , 3Sb 2 O 5 +15H 2 O. Ppt. Sol. in hot cone. HCl+Aq, and in UCl 3 +Aq. (Rammelsberg.) Zinc antimonate, Zn(SbO 3 ) 2 . Very slightly sol. in H 2 O (Berzelius); sol. in solutions of Zn salts. +2H 2 O. (Ebel, Dissert. 1890.) Insol. in H 2 O. (Senderens, Bull. Soc. 1899, (3) 21. 57.) +5H 2 O. Not wholly insol. in cold, mod- erately sol. in hot H 2 O. (Ebel, Dissert. 1890.) +6H 2 O. Insol. in H 2 O. (Senderens.) Antimoniomolybdic acid. Ammonium antimoniomolybdate, 5(NH 4 ) 2 O, 4Sb 2 O 5 , 7MoO 3 + 12H 2 O. Readily sol. in hot H 2 O. (Gibbs, Am. Ch. J. 7. 392.) Antimoniotungstic acid, 3Sb 2 O 6 , 4W0 3 + 11H 2 O. Sol. in H 2 O. (Hallopeau, C. R. 1896, 123. 1068.) Potassium antimoniotungstate, 3K 2 0. 3Sb 2 O 5 , 4W0 3 +4H 2 0. Much more sol. in hot than in cold H 2 O. Decomp. by HC1, H 2 SO 4 and HNO 3 . (Hallo- peau, C. R. 1896, 123. 1066.) ANTIMONY 43 + 16H 2 O. Much more easily sol. in ho than cold H 2 O. Decomp. by HC1, H 2 SO and HNO 3 . (Hallopeau, I.e.) 6K 2 O, 4Sb 2 O 5 , 12WO 3 +25H 2 O. SI. sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 392 Antimoniuretted hydrogen. See Antimony hydride. Antimonosomolybdic acid. Ammonium antimonosomolybdate, 6(NH 4 ) 2 C 3Sb 2 O 3 , 17MoC 3 +21H 2 O. Insol. in cold H 2 O. (Gibbs, Am. Ch. J. 7 313.) Antimonosophosphotungstic acid. Potassium antimonosophosphotungstate, 12K 2 O, 5Sb 2 O 3 , 6P 2 O 5 , 22W0 3 +48H 2 O. Nearly insol. in cold or warm H 2 O. (Gibbs Am. Ch. J. 7. 392.) Antimonosotungstic acid. Ammonium antimonosotungstate. Sol. in H 2 O. Barium antimonosotungstate, 4BaO, 6Sb 2 O 3 22W0 3 +36H 2 0. Precipitate; very si. sol. in hot HO. (Gibbs Am. Ch. J. 7. 313.) Antimonous acid, HSbO 2 . (Long, J. Am. Chem. Soc. 1895, 17. 87.) +1^H 2 0. Ppt. (Schaffner, A. 51. 182.) H 3 SbO 3 . Ppt. (Clarke and Stallo, B. 13. 1793.) Does not exist. (Guntz, C. R. 102. 1472.) H 4 Sb 2 O 6 . When freshly pptd., is sol. in dil KOH, and NaOH+Aq. Scarcely sol. in NH 4 OH+Aq, or in (NH 4 ) 2 CO 3 , or KHCO 3 + Aq. Completely sol. in K 2 CO 3 , and Na 2 CO 3 + Aq, especially if warm. When recently pptd. is si. sol. in succinic acid+Aq. Calcium antimonite, CaSb 2 O 4 (?). Min. Romeite. Insol. in acids. Cobaltous antimonite (?). SI. sol. in H 2 O. (Berzelius.) Cuprous antimonite, Cu 6 (SbO 3 ) 2 . Insol. in H 2 O. Sol. in acids; most easily in cone. HCl+Aq. (Hausmann and Stromeyer, Schw. J. 19. 241.) Cupric antimonite (?). Insol. in H 2 O. (Berzelius.) CuSb 2 O 5 . Min. Ammiolite. CuSb 2 O 4 . Sol. in HCl+Aq, tartaric and citric acids. (Harding, Z. anorg. 1899, 20. Iron (ferrous) antimonite (?). More sol. in H 2 O than the antimonate. (Dumas.) Potassium antimonite, K 2 O, 3Sb 2 O 3 . Easily decomp. by cold H 2 0. Not decomp by KOH+Aq containing over 20.9% K 2 O. (Corimimbceuf, C. R. 115. 1305.) +3H 2 O. As above. (C.) Potassium antimonite iodide, K 2 O, 8Sb 2 O 3 , 2KI. Insol. and not decomp. by cold or hot H 2 O. Not decomp. by acids or alkalies. Aqua regia decomp. slowly. Tartaric acid dissolves gradually. (Griihl, Dissert. 1897.) Sodium antimonite, NaSbO 2 +3H 2 O. Difficultly sol. in H 2 O. (Terreil, A. ch. (4) 7. 380.) 2Na 2 O, 3Sb 2 O 3 +H 2 O. Decomp. by H 2 O, but not by NaOH+Aq containing 94.3 g. NaOH per 1. (Corimimbceuf.) Na 2 O, 2Sb 2 O 3 . Decomp. by H 2 O but not by NaOH+Aq containing 188.6 g. NaOH per 1. (C.) Na 2 0, 3Sb 2 O 3 . Decomp. by H 2 O, but not by NaOH+Aq containing 113.2 g. NaOH per 1. (C.) +2H 2 = NaH 2 (Sb0 2 ) 3 . (Terreil.) Antimony, Sb. Does not decomp. H 2 O. Not attacked by HCl+Aq (Berzelius); slowly sol. in cone. HC1 +Aq (Debray) ; slowly sol. in cone, warm HC1 +Aq (Troost). Attacked by very cone. HC1 +Aq only when finely divided (Schutzen- berger, Willm); very si. attacked by dil. or cone, acid (Guntz). Not attacked by boiling HCl+Aq (Gmelin). By careful experiments, pure Sb is absolutely insol. in dil. or cone., hot >r cold HCl+Aq, except when in contact with >xygen. (Ditte and Metzner, A. ch. (6) 29. 889.) Insol. in dil. or cold cone., but sol. in hot one. H 2 SO 4 . Oxidized but not dissolved by HNO 3 +Aq. Easily and completely sol. in aqua regia. Very slowly attacked by pure HNO 3 +Aq of 51-1.42 sp. gr.; weaker acid has no marked action whether it contains NO 2 or not . HC1 + HNO 3 has no action if dil. or at low temp., but vhen even very dil. and KNO 2 is added, the ction will begin. (Millon, A. ch. (3) 6. 101.) Not attacked in 10 months by 2% HNOs +Aq. Sb is not dissolved by HNO 3 +Aq of ny concentration, a white powder being al- ways left, which is insol. in HNO 3 +Aq or T 2 O. (Montemartini, Gazz. ch. it. 22. 384.) Insol. in alkalies +Aq. Somewhat sol. in distilled H 2 O. More or ess sol. in solutions of acids, alkalies and salts nd in alcohol and ether. Only si. sol. in a mixture of alcohol and ether. (Ruff and Al- ert, B. 1905, 38. 54.) Alkaline H 2 O 2 converts Sb into antimonic cid, but neutral H 2 O 2 is without action. Hark, Chem. Soc. 1893, 63. 886.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 898, 20. 826.) 44 ANTIMONY ARSENIDE Easily attacked by pyrosul; (Heumann and Kochlin, B. li Sb is sol. in a mixture of HIS acid or other polybasic acids anal. 1906, 45. 507.) Not attacked by a mixture ether. (Cohen, Z. phys. Ch. 1 A cc. oleic acid dissolves 6 days. (Gates, J. phys. Ch There are three modificatio 1. Ordinary gray metallic. 2. Black amorphous. Ur temp. By boiling with H 2 C metallic Sb. 3. Yellow. Very unstable, over rapidly into the ordinary tion. Sol. in CS 2 at a littl (Stock, B. 1903, 37. 898.) Unstable above 90. (St< 3837.) Antimony arsenide, Sb 2 As. (Descamps, C. R. 86. 1065 Antimony ^n'bromide, SbBr 3 . Deliquescent; decomp. by Very sol. in liquid NH 3 . J. 1898, 20. 826.) Very sol. in warm liquid ^ solution with sp. gr. = 3.685 a Z. phys. Ch. 1893, 11. 339.) Sol. in S 2 C1 2 . (Walden, Z. 217.) Sol. in AlBr 3 . (Isbekow, 64. 27.) Easily sol. in PC1 3 and PB anorg. 1900, 25. 211.) Sol. in alcohol and CS 2 . Sol. in ether forming two la^ Chem. Soc. 1902, 24. 360.) Sol. in acetone. (Naumai 4328.) Solubility of SbBr 3 in org Data in parentheses indicat rium. 3hurvl chloride. J. 479.) r O 3 and tartaric (Czerwek, Z. of alcohol and 1904, 47. 12.) [).0007 g. Sb in 1911, 15. 143.) ns. istable at ord. > is changed to Solubility of SbBr 3 in organic liquids. Cont. Solvent t - jj8 S" ^^ t j38 1 - 1 sa t jig h. lod- benzene 28.6 30.5 32 20 10 4.0 8.7 13.5 17.5 21.7 10 20 30 40 50 60 26.3 31,5 37.3 43.7 50.7 58.5 70 80 90 94 67.0 78.2 91.9 100 68.9 85.2 100 Paradi- chlor- benzene 54.5 51.5 48.5 55 6.3 12.8 18.7 65 70 75 80 29.5 37.0 45.6 56.2 85 90 94 At 50 goes black modifica- e above 90. 3ck, B. 1905, 38. ) H 2 O. ;Gore, Am. Ch. .sBr 3 , forming a b47. (Retgers, anorg. 1900, 26. Z. anorg. 1913, r 3 . (Walden, Z. ^ers. (Hayes, J. in, B. 1904, 37. anic liquids, e labile equilib- Paradi- brom- benzene 88 85 80 75 70 '0 6.8 18.0 29.5 41.5 65 70 75 80 85 52.0 59.1 66.5 74.4 83.0 90 92 94 91.8 95.4 100 Nitro- benzene 6 1 , A 9 15 (17) 8.6 17.0 24.0 29.7 (31.9) 5 5 15 25 35 45 32.3 35.3 38.8 42.8 47.4 52.8 49.1 53.0 54.4 56.1 58.8 62.2 66.2 55 65 75 85 90 94 59.1 66.4 74.9 86.0 93.0 100 70.8 76.0 81.7 87.8 94.2 100 Metadi- nitro- benzene 90 85 80 75 70 65 60 8.1 16.2 24.2 31.8 38.5 44.3 55 50 47.5 50 55 60 65 70 75 80 85 90 94 Toluene 93 93.5 70 50 30 10 1 0.3 1.2 2.6 5.2 13.3 22.4 10 20 30 (34) 40 50 60 28.8 36.7 47.5 (54.0) 51.5 56.3 62.3 70 80 85 90 94 69.4 79.4 85.2 92.6 100 59.8 67.4 77.4 85 92.6 100 Ethyl- benzene 93 60 40 20 10 0.1 0.4 1.0 2.3 3.9 6.4 0.4 1.2 3.4 5.5 9.5 17.2 24.3 10 20 25 29 40 50 9.8 19.5 28.6 37.8 44.6 51.6 60 70 80 85 90 94 Propyl- benzene 80 60 40 30 20 (1.5) (-20, 10 20 30 40 (33.3) (23.3) 25.8 27.8 30.5 34.1 38.6 50 60 70 80 90 94 44.3 51.5 61.5 73.5 90 100 35.8 43.3 54.0 68.5 90 100 Solvent t f. ^ FH %& t * s l t ! a& 5 Isoamyl- benzene 70 50 40 30 20 17 (15) 1.9 3.6 5.1 7.1 13.4 16.4 (19.4) (13) 10 10 20 30 40 (24.9) 17 18.2 19.9 22.5 25.9 30.3 50 60 70 80 90 94 Benzene 5.6 4.5 15 25 35 45 55 1.9 3.0 4.3 6.0 8.6 12.1 1.7 2.2 3.2 4.3 5.6 2.6 4.4 6.9 9.9 13.4 65 75 80 85 90 91.5 92.5 10 20 30 40 50 17.1 24.9 30.7 38.4 48.2 58.1 66.6 91.5 90 85 90 92 94 73.7 76.7 84.9 91.4 94.8 100 (Menschutkin, Ann. Inst. Pol. P. le Gr. 13. 1.) Antimony bromide with MBr. See Bromantimonate, M. Also below. Antimony hydrogen bromide, SbBr 5 , HBr+ 3H 2 O. Very hygroscopic. Decomp. by H 2 O (Weinland and Feige, B. 1903, 36. 256.) See Metabromantimonic acid. Chlor- benzene -^5.2 47 40 30 20 10 7.2 9.2 11.8 15.4 20.8 28.1 60 70 80 90 94 37.6 50.0 66.6 89.6 100 Brom- benzene 31 32 25 1.5 5 15 25 35 45 55 65 17.4 22.2 22.7 34.4 42.6 52.6 75 85 90 94 65.2 81.1 90.0 100 ANTIMONY CHLORIDE 45 Antimony caesium bromide. 2SbBr 6 , 3CsBr+ 2H 2 0. Loses Bro in the air. (Weinland, B. 1903, 36. 257.) Antimony calcium bromide, SbBr 3 , CaBr 2 + 8H 2 O. Easily decomp. (Benedict, Proc. Am. Acad. 1895, 30. 9.) Antimony glucinum bromide, 3SbBr 5 , 2GlBr 2 + 18H 2 0. Hydroscopic. Easily decomp. (Weinland, B. 1903, 36. 258.) Solubility in H 2 O. 100 pts. SbCl 3 sol. in pts. H 2 at t. t Pts. H 2 O 15 20 25 30 35 40 50 60 16.6 12.3 10.9 10.1 9.4 8.7 7.3 5.2 2.2 f\/InrvvV*v,-tr V r.-n^T./v 1 OAQ O9 OOft 'V Antimony magnesium bromide, SbBr 3) MgBr 2 +8H 2 O. As Ca salt. (Benedict, Proc. Am. Acad. 1895, 30. 9.) Antimony potassium bromide, 10SbBr 3 , 23KBr+27H 2 0. (Herty, Am. Ch. J. 1894, 16. 496.) Antimony rubidium bromide, 2SbBr 3 , 3RbBr. Decomp. by H 2 O; can be recryst. from dil. HBr+Aq. (Wheeler, Z. anorg. 5. 258.) SbRb 2 Br 6 . Slowly loses Br 2 in the air. Decomp. by H 2 O. (Weinland, B. 1903, 36. 259.) 10SbBr 3 , 23RbBr (?). Cryst. from cone. HBr+Aq. (Wheeler.) The composition assigned to this salt by Wheeler (Z. anorg. 5. 253) is incorrect. (Ephraim, B. 1903, 36. 1817.) Antimony vanadium bromide, SbBr 3 , VBr 4 + 7H 2 O. Hydroscopic. Decomp. by H 2 0. Sol. in dil. HC1 and in tartaric acid. (Weinland, B. 1903, 36. 260.) Antimony bromide potassium chloride, SbBr 3 , Solubility in HCl+Aq. 100 mol. H 2 O dissolve mol. SbCl 3 in presence of mol. HC1 at 20. e po 2 0. Slowly deliquescent. Very sol. in H 2 0. Sat. solution contains 120.5 g. to 100 cc. H 2 O, and has sp. gr. = 1.9. Decomp. by much H 2 0. (Atkinson, Chem. Soc. 43. 200.) Does not exist. (Herty, Am. Ch. J. 1894, 16. 497.) See also Antimony chloride potassium bromide. Antimony bromofluoride, SbF 6 Br. Decomp. by H 2 O. (Ruff, B. 1906, 39. 4319.) Antimony trichloride, SbCl 3 . Deliquescent. Decomp. by H 2 O with pre- cipitation of SbOCl. This precipitation is pre- vented by tartaric, citric, or hydrochloric acid, or by cone, solutions of chlorides of alkalies and alkaline earths. Mol. HC1 Mol. SbCls 72.1-72.8 2.4 73.0 6.5 67.5 8.4 67.6 8.6 66.5 9.8 65.0 12.2 65.3 29.6 54.5 (Meerburg, Z. anorg. 1903, 33. 304.) Solubility in HCl+Aq. 100 mol. H 2 O dissolve at 20 Solid phase 1 2 3 4 Mol. Mol. Mol. Mol. SbCls HC1 SbOCl HC1 SbOCl 8.7 7.2 9.8 6.9 8.6 7 5 16.1 7.9 19.6 8.0 21.7 7.4 19.8 8.9 25.0 8.8 28.0 8.6 (SbOCl)x,(SbCl 3 )y 37.5 8.7 32.0 7.9 44.0 6.8 35.8 7.9 63.7 6.2 59.5 6.4 69.1 5.6 61.0 6.5 66.1 4.6 62.7 4.4 69.8 5.3 SbCl 3 and 69.3 4.3 (SbOCl) x ,(SbCl 8 )y 68.3 3.6 1 & 2. (Meerburg, Z. anorg. 1903, 33. 302.) 3 & 4. (Noodt, Z. anorg. 1903, 33. 302.) Somewhat sol. in liquid (CN) 2 . (Cent- nerszwer, Bull. Soc. 1901, (3) 28. 405.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) Easily sol. in PC1 3 and PBr s . (Walden, Z. anorg. 1900, 26. 211.) Sol. in S 2 ri 2 . (Walden, Z. anorg. 1900, 25. 217.) 46 ANTIMONY CHLORIDE Easily sol. in AsBr 3 . (Walden, Z. anorg 1902, 29. 374.) Sol. in afcohol without decomp. Very sol in hot CS 2 , but solubility diminishes rapidly on cooling. (Cooke. Proc. Am. Acad. 13 72.) 1 g. SbCls is sol. in 0.186 g. acetone at 18 Sp. gr. of sat. solution 18/4 = 2.216.. (Nau- mann, B. 1904, 37. 4332.) Sol. in ethyl acetate. (Naumann. B. 1904, 37. 3601.) 1 pt. sol. in 16.97 pts. of ethyl acetate at 18. Sp. gr. of sat. solution 18/4 = 1.7968. (Naumann, B. 1910, 43. 320.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in methylal. (Eidmann, C. C. 1899, II. 1014.) Solubility of SbCl 3 .in organic liquids. Data in parentheses indicate labile equilib- rium. Solubility of SbCl 3 in organic liquids Cont. Solvent t |l s| t o n t o j2 3* 15 40.7) 10.7 16.4 24.7 39.1 47.2) 44.5 48.7 25 35 45 55 65 70 73 Paradi- chlor- benzene Paradi-; brom- benzene 54.5 50 45 40 6.3 15.5 28.0 39.5 45 50 55 29.5 37.5 46.4 56.0 60 65 70 73 66.5 78.1 91.1 00 88 85 80 75 70 5.9 15.8 25.7 35.7 65 60 49.5 55 60 45.4 53.8 64.9 72.5 79.8 65 70 73 87.1 95.2 00 Nitro- benzene 6 2 2 6 10 14 (18) 16.5 7.0 12.1 16.5 20.3 23.5 26.2) 25.2 13.5 10.5 7.5 6.5 6 6.5 5 5 27.3 29.8 35.2 40.7 50.0 52.8 53.0 55.8 15 25 35 45 55 65 70 73 59.2 63.0 67.6 72.8 79.0 87.2 92.7 00 ANTIMONY POTASSIUM CHLORIDE 47 Antimony hydrogen pentachloride. SbCls, " A/etachlorantimonic acid" according to Weinland and Schmid, (Z. anorg. 1905, 44. 43.) Very easily sol. in H 2 0, alcohol, acetone and glacial acetic acid. Aqueous solution decomp. on standing with separation of Sb 2 O5 but remains clear in presence of 10% HC1. (Weinland and Schmid, Z. anorg. 1905, 44. 43.) SbCl 5 , 5HC1+10H 2 O. Not deliquescent. Decomp. by H 2 O. Melts in crystal H 2 at about 55. (Engel, C. R. 106. 1797.) Antimony antimonyl chloride, SbCl 3 , SbOCl. More easily attacked by H 2 O than SbOCl. (Bemmelen, Z. anorg. 1903, 33. 293.) Antimony antimonyl potassium chloride. SbCl 3 , SbOCl, 2KC1. Not deliquescent. Immediately decomp. by hot or cold H 2 O; sol. in hot glacial HC 2 H 3 2 , or in HC1, or tartaric acid+Aq. Insol. in KCl+Aq, hot or cold alcohol, CS 2 , or ligroine. (Benedikt, Proc. Am. Acad. 29. 217.) Antimony antimonyl rubidium chloride, SbCl 3 , SbOCl, 2RbCl. Sol. in very dil. HCl+Aq. . (Wells, Am. J. Sci. 1897, (4) 3. 463.) Antimony barium chloride, SbCl 3 , BaCl 2 + 3 / 2 H 2 0. Decomp. by H 2 O. Antimony caesium chloride, SbCl 3 , GCsCl. Decomp. by H 2 O. Cryst. from dil. HC1+ Aq. (Godeffroy, Arch. Pharm. (3) 12. 47.) 2SbCl 3 , 3CsCl. Decomp. by H 2 0; si. sol. in cold, easily in hot dil. HCl+Aq. This is identical with the above salt. (Saunders, Am. Ch. J. 14. 152.) SbCl 4 , 2CsCl. Sol. in boiling cone. HC1+ Aq without decomp. (Setterberg, Oef. Vet. Akad. 1882, 6. 23.) SbCl 6 , CsCl. Cryst. from HC1 + Aq without decomp. Decomp. by H 2 O. (Setterberg, Oef. Vet. Akad. 1882, 6. 27.) Antimony calcium chloride, SbCl 3 , CaCl 2 + 8H 2 O. Easily decomp. (Benedict, Proc. Am. Acad. 1895, 30. 9.) SbCl 6 CaSbCl 6 .OH+9H 2 0. Deliquescent; si. sol. in H 2 O. (Weinland, B. 1901, 34. 2635.) Antimony chromium chloride, CrCl 3 , 3SbCl 5 +13H 2 O. (Weinland.) should be [SbCl 6 ] 3 [Cr(OH 2 ) 6 ]+7H 2 O; and CrCl 3 , SbCl 5 + 10H 2 O should be [SbCl6][Cr(OH 2 ) 4 Cl 2 ]+6H 2 O. (Pfeiffer, Z. anorg. 1903, 36. 349.) Antimony glucinum chloride, SbCl 3 , G1C1-.+ 3H 2 0. Very hydroscopic. Decomp. by H 2 O. Very easily sol. in HC1. (Ephraim, B. 1903, 36. 1822.) +4H,O. Ppt. Decomp. by H 2 0. Sol. in HC1. (Ephraim, B. 1903, 36. 1822.) Antimony hydrazine chloride, SbCl 3 , 3N 2 H 5 C1. Sol. in cone. HCl+Aq; decomp. by H 2 O. (Ferratini, C. A. 1912, 1613.) Antimony lithium chloride, SbCl 3 , 2LiCl+ 5H 2 O. Hydroscopic. Decomp. by H 2 O. Very easily sol. in HC1. (Ephraim, B. 1903, 36. 1821.) +6H 2 O. Decomp. by H 2 O; easily sol. in HC1. (Ephraim, B. 1903, 36. 1822.) Antimony magnesium chloride, SbCl 3 , MgCl 2 +5H 2 0. Hydroscopic. Decomp. by H 2 O. Can be cryst. from HC1 without decomp. (Ephraim, B. 1903, 36. 1823.) 2SbCl 3 , MgCU- Hygroscopic. Decomp. by H 2 O. Very sol. in HC1. (Ephraim.) SbClrMeSbCleMgOH + 17H 2 O. Hydro- scopic. Sol. in H 2 O with decomp. (Weinland, B. 1901, 34. 2635.) Antimony nitrosyl chloride, SbCl 5 , NOC1. Very deliquescent; decomp. by pure H 2 O; sol. in H 2 containing tartaric acid. (Weber, Pogg. 123. 347.) 2SbCl 5 , 5NOC1. Decomp. by H 2 O. (Sud- borough, Chem. Soc. 59. 661.) Antimony phosphorus chloride, SbCl 5 , PC1 5 . Deliquescent. (Weber, Pogg. 125. 78.) Antimony phosphoryl chloride, SbCl 5 , POC1 3 . Deliquescent. (Weber.) Antimony platinum potassium chloride, (Sb, Pt)CUKi. Ppt. (Weinland, B. 1905, 38. 1086.) Antimony potassium chloride, SbCl 3 , 2KC1. Sol in H 2 O without decomp. (Jacquelain, A. ch. (2) 66. 128.) Not deliquescent. Immediately decomp. by hot or cold H 2 O. Sol. in HC1, or tartaric acid+Aq. (Benedikt, Proc. Am. Acad. 29. 219.) +2H 2 O. Very efflorescent. SbCls, 3KC1. " Deliquescent. Decomp. by hotH 2 0. (Poggiale.) _,-,-.., +2H 2 O. (Romanis, C. N. 49. 273.) Not obtained by Benedikt (I.e.) 10SbCl 3 ,23KCl. True composition of above salts. Sol. inH 2 O. (Herty, Am. Ch. J. 1894, 16. 495.) SbCl 3 , 2KC1 is the only true compound, all 48 ANTIMONY RUBIDIUM CHLORIDE others being isomorphous mixtures. (Jordis, B. 1903, 36. 2539.) 2SbCl 4 , 3KC1. Deliquescent. Decomp. by H 2 O. (Bosek, Chem. Soc. 1895, 67. 516.) SbCtebCleKOH. Hydroscopic. Sol. in H 2 O with decomp. (Weinland, B. 1901, 34. 2635.) See also Antimony antimonyl potassium chloride. Antimony rubidium chloride, SbCl 3 , RbCl. Decomp. on air or with H 2 0. (Saunders, Am. Ch. J. 14. 162.) 2SbCl 3 ,RbCl+H 2 O. Decomp. on air. (Wheeler, Z. anorg. 5. 253.) SbCl 3 , 6RbCl. Decomp. by H 2 O. (Godef- froy, Arch. Pharm. (3) 9. 343.) Formula is 10SbCl 3 , 23RbCl (?). (Saunders Am. Ch. J. 14. 159.) 10SbCl 3 , 23RbCl (?). Decomp. by H 2 O; sol. in HCl-fAq. (Saunders.) Formula is 3SbCl 8 ,7RbCl. (Wells and Foote, Am. J. Sci. 1897, (4) 3. 461.) Composition assigned to this salt by Saunders (Am. Ch. J. 14. 155) is incorrect. (Ephraim, B. 1903, 36. 1817.) 3SbCl 3 , 5RbCl. As above. (Saunders.) Formula is 2SbCl 3 , 3RbCl. (Wheeler.) Rb 2 SbCl 6 . Ppt. Decomp. by H 2 O. (Wein- land, B. 1905, 38. 1083.) Rb 2 SbCl 6 , 2Rb 3 SbCl 6 . Ppt. Decomp. by H 2 O. (Weinland, B, 1901, 34. 2635.) Antimony selenium chloride, SbCl 5 , SeCl 4 . Deliquescent. (Weber.) Antimony selenyl chloride, SbCl 6 , SeOCl 2 . Very deliquescent. (Weber, Pogg. 125. 325.) Antimony sodium chloride, SbCl 3 , 3NaCl (?). Decomp. by much H 2 0. (Poggiale.) Antimony sulphur chloride, 2SbCl 5 , 3SC1 2 . Decomp. by H 2 O. SbCl 6 , SC1 4 . Sol. in dil. HN0 3 +Aq. Mpt. 125-126 in an atmos. of chlorine. Violently decomp. by H 2 0. (Ruff, B. 1904, 37. 4515.) Antimony thallium chloride, SbCl 3 , 3T1C1. Ppt. (Ephraim, Z. anorg. 1909, 61. 249.) SbCl 4 , T1C1. (Ephraim and Barteczko, Z. anorg. 1909, 61. 251.) 2SbCl 4 , 2T1C1, T1C1 3 . Slowly decomp. by cold H 2 O. (Ephraim and Barteczko, Z. anorg. 1909, 61. 253.) Antimony trichloride ammonia, SbCl 3 , NH 3 . Not very deliquescent. Decomp. by H 2 O. Antimony pentochloride ammonia, SbCl 5 , 6NH 3 . Decomp. by H 2 O. (Persoz.) Antimony pewfachloride cyanhydric acid, SbCl 5 , 3HCN. Deliquescent; decomp. by H 2 0. (Klein, A. 74. 85.) Antimony pewtachloride nitric oxide, 2SbCl6, NO. Decomp. by H 2 O. (Besson, C. R. 108. 1012.) Antimony pewtochloride nitrogen peroxide, 3SbCl 5 , 2NO 2 . Decomp. by H 2 O. (Besson.) Antimony pentachloride nitrogen sulphide, SbCl 5 , N 4 S 4 . Easily decomp. (Davis, Chem. Soc. 1906, 89. 1577.) Decomp. by cold H 2 p, HC1, H 2 SO 4 and warm alcohol, also by boiling with KOH+Aq. Almost insol. in organic solvents. (Wolbling, Z. anorg. 1908, 57. 283.) Antimony chloride potassium bromide, SbCl 3 ,3KBr+lHH 2 O. Very deliquescent. Decomp. by much H 2 O. (Atkinson, Chem. Soc. 43. 289.) 2SbCl 3 ,3KBr+2H 2 O. (Atkinson.) SbCl 3 ,KBr+H 2 0. (Atkinson.) Above are mixtures. (Herty, Am. Ch. J. 1894, 16. 497.) See Antimony bromide potassium chloride. Antimony chlorofluoride, SbCl 3 F 2 . (Swarts, Z. anorg. 1896, 12. 71.) Antimony fluoiodide, SbF 6 I. Slowly decomp. by H 2 O. (Ruff, B. 1906, 39. 4321.) (SbF 5 ) 2 I. Sol. in H 2 O with pptn. of I 2 . (Ruff, B. 1906, 39. 4321.) Antimony Znfluoride, SbF 3 . Deliquescent. Sol. in H 2 O. Solubilitv in H 2 O at t. t 100 g. of the solution con- tain g. SbF 3 100 g. H 2 O contain g. SbFs 20 22.5 25 30 79. 81. 81. 83. 84. 37 64 91 12 93 384.7 444.7 452.8 492.4 563.6 (Rosenh'eim, Z. anorg. 1909, 61. 189.) Solubility in HF+Aq at 0. Normality of HF+Aq 100 g. H 2 O of the HF solu- tion dissolve g. SbFs 2 1 0.5 474.9 432.5 404.0 (Rosenheim, Z. anorg. 1909, 61. 192.) ANTIMONY FLUORIDE POTASSIUM CHLORIDE 49 Solubility of SbF 3 in salts +Aq at 0. Antimony lithium fluoride, SbF 3 , 2LiF. ' Sol. in more than 20 pts. H 2 O. (Fliickinger, Pogg. 87. 245.) SbF 3 , LiF. Easily sol. in H 2 0. "(Stein, Chem. Z. 13. 357.) Antimony potassium fluoride, SbF 8 , 2KF. Sol. in less than 2 pts. boiling, and in 9 pts. cold H 2 O. Insol. in alcohol or ether. SbF 3 ,KF. More sol. than SbF 3 , 2KF. Sol. in 2.8 pts. H 2 O. (Fliickinger, Pogg. 87. 245.) SbF 6 , KF. Easily sol. in H 2 O. SbF 6 , 2KF+2H 2 O. Easily sol. in H 2 O. (Marignac, A. 146. 239.) Antimony sodium fluoride, SbF 3 , 3NaF. Sol. in 14 pts. cold, and 4 pts. boiling H 2 O. Sol. in HF. (Fliickinger, Pogg. 87. 245.) SbF 3 , NaF. 100 pts. cold H 2 O dissolve 93 pts. 100 pts. hot H 2 O dissolve 166 pts. (Stein, Wagners' J. B. 1887. 1160.) 4SbF 3 , NaF. As NH 4 salt. (Raad and Hauser, B. 1890, 23. R. 125.) SbF 6 , 2NaF. Easily sol. in H 2 O. (Marig- nac, A. 145. 329.) Antimony thallium fluoride, TlF,SbF 3 . Sol. in H 2 without decomp. (Ephraim, B. 1909, 42. 4458.) TlF,2SbF 3 . Sol. in H 2 O without decomp. (Ephraim.) TlF,3SbF 8 . Sol. in H 2 O without decomp. Decomp. by cold cone. H 2 SO 4 . (Ephraim.) Antimony Znfluoride ammonia, SbF 3 , 2NH 8 . SI. sol. in liquid NH 3 . (Ruff, B. 1906, 39. 4326.) Salt Normality of salt solution 100 g. H 2 O of the salt solution dis- solve g. SbF 8 KC1 1 0.5 0.25 0.125 461.8 448.3 431.9 407.3 KBr 1 0.5 0.25 0.125 448.7 450.0 455.6 417.2 KNOi 1 0.5 0.25 0.125 458.2 451.9 418.3 401.4 ^K 2 S0 4 1 0.5 0.25 419.9 408.5 406.6 ^K 2 C 2 4 1 0.5 0.25 0.125 465.7 481.2 451.3 405.2 K(NH 4 ) 2 C 2 4 0.5 0.25 0.125 431.9 442 3 433.3 HK 2 C 4 H 4 6 1 0.5 0.25 0.125 461.4 430.5 430.8 435.2 (Rosenheim, Z. anorg. 1909, 61. 192.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) Antimony pentafluoride, SbF 6 . Sol. in H 2 O. (Marignac, A. 146. 239.) Very hydroscopic; bpt. 155. Sol. in H 2 O with hissing. (Ruff, B. 1904, 37. 678.) +2H 2 O. (Ruff, B. 1904, 37. 679.) Antimony pentafluoride diantimony trir fluoride, Sb 3 Fn=2SbF 3 , SbF 5 . Hydroscopic; bpt. 390. Easily sol. in H 2 O. (Ruff, B. 1904, 37. 680.) Antimony pentofluoride penfoantimony iri- fluoride, SbF 6 , 5SbF 3 . B pt. 384 (corr.). (Ruff, B. 1904, 37. 681.) Antimony caesium fluoride, CsF,2SbF 3 . CsF,3SbF 3 . 4CsF,7SbF 3 . CsF,SbF 3 . 2CsF,SbF 3 . (Wells, Am. J. Sci. 1901, (4) 11. 451.) Antimony Znfluoride ammonium chloride. SbF 3 , NH 4 C1. Easily sol. in H 2 O. (de Haen, B. 21. 901 R.) Antimony /nfluoride ammonium sulphate, SbF 3 , (NH 4 ) 2 S0 4 . More sol. than K or Na salt. 1 pt. H 2 O dissolves 1.4 pts. at 24 and 15 pts. at 100. (de Haen, B. 21. 902 R.) Antimony fluoride lithium chloride, SbFj, LiCl. Sol. in H 2 O. (Stein, Chem. Z. 13. 357.) Antimony pewtafluoride nitrosyl fluoride, SbF 5 , NOF. Hydroscopic. Decomp. by H 2 0. Sol. in liquid NH 3 with decomp. SI. sol. in NOC1, SiCl 4 , PC1 3 , AsCl 3 , SO 2 C1 2 and SOC1 2 . (Ruff, Z. anorg. 1908, 68. 334.) Antimony influoride potassium chloride, SbF 3 , KC1. 100 pts. H 2 O dissolve 51 pts. at 24, and 300 pts. at 100. (de Haen, B. 21. 901 R.) 50 ANTIMONY FLUORIDE POTASSIUM SULPHATE Antimony Znfluoride potassium sulphat SbF 3 , K 2 S0 4 . Sol. in H 2 O. (de Haen.) 2SbF 3 , K 2 S0 4 . Very sol. in H,0. (Mayer B. 1894, 27. R. 922.) Antimony fnfluoride sodium chloride, SbF ; NaCl. Easily sol. in H 2 O. (de Haen, B. 21. 90 Antimony influoride sodium sulphate, SbF 3 Na 2 S0 4 . Sol.-inH 2 0. (deHaen.) Antimony fluoiodide, SbF 5 I. Mpt. 80; slowly decomp. by H 2 0. (Ruff B. 1906, 39. 4321.) (SbF 6 ) 2 I. Mpt. 110-115: decomp. H 2 O. (Ruff.) Antimony fluosulphide, SbF 5 S. Very hygroscopic. Decomp. by H 2 O. Sol with decomp. in alcohol. Sol.inCCl 4 . (Ruff B. 1906, 39. 4332.) Antimony gold, Au 3 Sb. Insol. in equal pts. of HN0 3 and tartaric acids. (Roessler, Z. anorg. 1895, 9. 72.) Antimony hydride, SbH 3 . Scarcely sol. in H 2 O. 1000 ccm. H 2 O ab- sorb 4.12 cc. SbH 3 at 10.5. Decomp. by long contact with H 2 O; also by cone. H 2 SO 4 or KOH+Aq. (Jones, Chem. Soc. 29. 641.) Antimony ZnTiydroxide, SboO 3 , 2H 2 O = Sb 2 O(OH) 4 . (Schaffner, A. 51. 182.) Sb(OH) 3 . Ppt. (Clarke and Stolla, B. 13. Does not exist. (Guntz, C. R. 102. 1472.) See Antimonous acid and antimony tri- oxide. Antimony ^niodide, SbI 3 . Decomp. by H 2 O or 80% alcohol. Sol. in HI+Aq; sol. in boiling CS 2 , and in boiling benzene, but separates out on cooling. Al- most insol. in CHC1 3 . (Cooke, Proc. Am. Acad. (2) 5. 72.) Easily sol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Sol. in warm AsBr 3 . Sp. gr. of a solution sat. at 40, which solidifies at 37, =3.720. This dissolves further AsI 3 , whereby the mpt. sinks to 31 and sp. gr. rises to 3.801. By mixing the latter solution with a solution of AsI 3 in CH 2 I 2 , a liquid can be obtained with a sp. gr. of 3.702 at 20. (Retgers, Z. phys. Ch. 1893, 11. 340.) Sol. in PC1 3 . (Beckmann, Z. anorg. 1906, 51. 110.) Sol. in SO 2 C1 2 . (Walden, Z. anorg. 1900, Sol. in SOC1 2 and S 2 C1 2 . (Walden, Z. anorg. 1900, 25. 216.) Sol. in AsCl 3 . (Walden, Z. anorg. 1900, 25. 214.) Sol. in SnCl 4 . (Walden, Z. anorg. 1900, 25. 218.) Sol. in POC1 3 . (Walden, Z. anorg. 1900, 25. 212.) Easily sol. in PC1 3 and PBr 3 . (Walden, Z. anorg. 1900, 25. 211.) Partly sol. in, and partly decomp. by al- cohol or ether. (M'lvor, Chem. Soc. (2) 14, 328.) Insol. in oil of turpentine and CC1 4 . 100 pts. methylene iodide dissolve 11.3 pts. SbI 3 at 12; sp. gr. of solution = 3.453. (Ret- gers, Z. anorg. 3. 343.) Sol. in C 6 H 6 . (Retgers, Z. phys. Ch. 1893, 11. 334.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Antimony penfaiodide, SbI 5 . Very unstable. (Pendleton, C. N. 48. 97.) Antimony barium iodide, SbI 3 , BaI 2 +9H 2 O. Decomp. by H 2 O. Sol. in HC1, HC 2 H 3 2 , or H 2 C 4 H 4 O 6 +Aq. CS 2 dissolves out SbI 3 . (Schaffer, Pogg. 109. 611.) Antimony caesium iodide, 2SbI 3 ,3CsI. SI. sol. in HI+Aq. Exists in two distinct brms. (Wells, Am. J. Sci. 1901, (4) 11. 455.) Antimony potassium iodide, 2SbI 3 , 3KI + 3H 2 O. Decomp. by H 2 O. Sol. in HC1, HC 2 H 3 O 2 , or H 2 C 4 H 4 O 6 +Aq. CS 2 dissolves out SbI 3 . Schaffer, Pogg. 109. 611.) SbI 3 , 2KI+2MH 2 O. Decomp. by H 2 O. Nickles, J. Pharm. (3) 39. 116.) Antimony rubidium iodide, 2SbI 3 , 3RbI. Decomp. by H 2 O. (Wheeler, Z. anorg. 5. 59.) Antimony sodium iodide, 2SbI 3 , 3NaI + 12H 2 O. As 2SbI 3 , 3KI. (Schaffer, Pogg. 109. 611.) Antimony thallous iodide, 2SbI 3 , 3T1I. Decomp. by H 2 O and by HCl+Aq, also by Icohol. (Ephraim, Z. anorg. 1908, 58. 354.) Antimony nitride, SbN. Decomp. by heat. (Franz Fischer, B. 1910, 3. 1471.) Vntimony irioxide, Sb 2 O 3 . Very si. sol. in H 2 O. Sol. in 8900-10,000 ts. H 2 O at 100; 55,000-61,100 pts. at 15. Schulze, J. pr. (2) 27. 320.) Sol. in HCl+Aq. Insol. in HNO 3 +Aq, but ot as insol. as metastannic acid. Sol. in cold uming HNO 8 or H 2 SO 4 . Insol. in dil., but ol. in cone, alkalies, or alkali carbonates + ANTIMONY SULPHIDE 51 Aq. Sol. in cold NH 4 C1, or NH 4 NO 3 +Aq. Sol. in 15 pts. boiling SbCl 3 . (Schneider, Pogg. 108. 407.) Sol. in HC 2 H 3 O 2 , or HjCJ^O.+Aq, and not pptd. from these solutions by H 2 O. Eas- ily sol. in benzoic acid. Insol. in pyrotartaric acid. Very sol. in KHC 4 H 4 O 6 +Aq. Sol. in glycerine. Somewhat sol. in H 3 PO 4 +Aq. (Kohler, Dingl. 1885, 268. 520.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) Sol. in lactic acid. (Kretzschmar, Ch. Z. 1888, 12. 943.) Sol. in grape sugar solution to which Ca(OH) 2 has been added. (Vogel, B. 1885, 18, R. 38.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Sol. in glycerine in presence of alkalies. (Kohler, Dingl. 1885, 258. 520.) Exists in a sol. colloidal modification. (Spring, B. 16. 1142.) Min. Valentinite, Senarmontite. +H 2 O. See Antimonous acid. Antimony feiroxide, Sb 2 O 4 . Insol. in H 2 O. Slightly attacked by acids; hot cone. HCl+Aq acts only slightly. ,(Fre- senius.) Min. Cenantite. SI. sol. in HCl+Aq. Antimony peroxide, Sb 2 O 5 . Insol. in H 2 O. Easily sol. in HCl+Aq. SI. sol. in cone. KOH+Aq. " Antimonoxyd" is sol. in glycerine in pres- ence of alkalies. 100 g. glycerine, to which have been added 10 g. NaOH+Aq (1 : 1), dissolve 20.6 g. at b.-pt.; 20 g. NaOH+Aq (1 : 1), dissolve 36.0 g. at b.-pt.; 40 g. NaOH+Aq (1 : 1), dissolve 68.5 g. at b.-pt.; 80 g. NaOH+Aq (1:1), dissolve 93.0 g. at b.-pt.; 120 g. NaOH +Aq (1 : 1), dissolve 119.2 g. at b.-pt. (Kohler, Dingl. 258. 520.) See also Antimonic acid. Antimony nitrogen pentoxide, 2Sb 2 O 5 , N 2 O 5 . Not decomp. by H 2 O. (Thomas, C. R. 1895, 120. 1116.) Antimony oxybromide. See Antimonyl bromide. Antimony oxy chloride. See Antimonyl chloride. Antimony oxyfluoride. See Antimonyl fluoride. Antimony oxysulphide, Sb 2 OS 2 . Min. Antimony blende (kermesite) . Insol. in H 2 O or dil. acids, except HCl+Aq. (Schneider, Pogg. 110. 147.) Antimony palladium, Sb 2 Pd. SI. sol. in equal pts. of HNO 3 and tartaric acids. (Roessler, Z. anorg. 1895, 9. 69.) Antimony platinum, Sb 2 Pt. Insol. in equal pts. of HNO 3 and tartaric acids. (Roessler, Z. anorg. 1895, 9. 67.) Antimony phosphide, SbP. Insol. in benzene, ether, or CS 2 . (M'lvor, B. 6. 1362.) Antimony selenide, SbSe. (Chretien, C. R. 1906, 142. 1341.) Sb 3 Se 4 . (Chretien, I.e.) Sb 4 Se 5 . (Chretien, I.e.) Sb 2 Se 3 . Sol. in KOH+Aq. (Hof acker, A. 107. 6.) Sb 2 Se 6 . (Hofacker.) Antimony selenide, with M selenide. See Selenoantimonates, M. Antimony Znsulphide, Sb 2 S 3 (Kermes). Insol. in H 2 O and dil. acids. 1 1. H 2 O dissolves 5.2 x 10- 6 mols. pptd. Sb 2 S 3 at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Decomp. by cone. HNO 3 or H 2 SO 4 . Sol. in cone. HCl+Aq. Easily sol. in dil. KOH, NaOH, (NH 4 ) 2 S, and K 2 S+Aq. SI. sol. in NH 4 OH+Aq; very si. sol. in (NH 4 ) 2 CO 3 + Aq; insol. in KSH+Aq. (Fresenius.) Sol. in a mixture of 50 pts. H 2 O and 18 pts. HC1 (sp. gr. 1.16) even when completely sat. with H 2 S. (Lang and Carson, J. Soc. Chem. Ind. 1902, 21. 1018.) SI. sol. in H 2 SO 3 +Aq. (Guerout, C. R. 1872, 75. 1276.) Cryst. Sb 2 S 3 is only si. sol. in NH 4 OH+ Aq (1 pt. in about 2000 pts. NH 3 ). Pptd. amorphous Sb 2 S 3 is appreciably more sol. (1 pt. in 600 pts. NH 3 ). (Garot, J. pr. 1843, 29. 83.) SI. sol. in hot 2% Na 2 B 4 O 7 +Aq, still less sol. in cold. (Materne, C. C. 1906, II. 557.) Insol. in NH 4 Cl+Aq. Sol. in 14-15 pts. pure SbCl 3 . - (Schneider, Pogg. 108. 407.) Slowly sol. in H 2 C 4 H 4 O 6 +Aq. Sol. in boiling' Na 3 SbS 4 +Aq. Sol. in hot citric, tartaric and oxalic acids. SI. sol. in malic, benzoic, picric and pyrogallic acids. Insol. in formic and acetic acids. Es- pecially easily sol. in citric and oxalic acids with addition of KNO 3 , KNO 2 or KC1O 3 . (Bolton, C. N. 1878, 37. 86 and 99.) Sol. in ethylamine sulphydrate+Aq. Min Stibnite. Sol. in cold citric acid+ Aq. (Bolton, C. N. 37. 14.) Soluble modification. Sb 2 S 3 may be ob- tained in a colloidal state in aqueous solution containing 1 pt. Sb 2 S 3 to 200 pts. H 2 O. This can be boiled without decomp., but Sb 2 S 3 is pptd. by acids and salts. 52 ANTIMONY SULPHIDE Table of maximum dilution of solutions of Antimony sulphur dioxide, SbSO 2 . acids and salts which cause pptn. of Sb 2 S 3 . Ppt. (Faktor, C. C. 1900, I. 12J1.) HC1 . . 1 : 270 H 2 S0 4 . . : 140 Antimony telluride, SbTe. H 2 C 2 4 . :45 Insol. in H 2 O. K 2 SO 4 . (NH 4 ) 2 S0 4 :65 :130 Sb 2 Te 3 . Insol. in H 2 O. (Oppenheim, J. pr. 71. 277.) MgS0 4 . : 1720 MnSO 4 . :2060 Antimonyl bromide, SbOBr. NaCl . BaCl 2 . : 135 :2050 Insol. in CS 2 . (Cooke, Proc. Am. Acad. 13. 104. ^ MgCl 2 . CoCl 2 . : : :5800 L :2500 J.vr./ SI. sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) KNO 3 . Fe 2 Cl 6 . Ba(N0 3 ) 2 . 1 : id . 1 : 2500 . 1 : 1250 Sb 4 5 Br 2 . (M'lvor, C. N. 29. 179.) 10Sb 4 O 5 Br 2 , SbBr 3 . K 2 A1 2 (SO 4 ) 4 1 : 35,000 Antimonyl chloride. (NH 4 ) 2 Fe 2 (SO 4 ) 4 . . 1 : 800 K 2 Cr 2 (SO 4 ) 4 . . . 1 : 40,000 KSbOC 4 H 4 O fl . . 1 : 18 From SbCl 3 . SbOCl. Insol. in H 2 0. De- comp. by boiling with H 2 0; sol. in HCl+Aq. Tnsnl in alnnhnl or pfhpr' nl in f~!L nTTPl. (Schulze, J. pr. (2) 27. 320.) Antimony bisulphide with M 2 S. See Sulphantimonites, M. Antimony pentasulphide, Sb 2 S 6 . Insol. in H 2 0, or H 2 O containing H 2 S. Sol. in cone. HCl+Aq. Completely sol. in NH 4 OH+Aq; traces dissolve in (NH 4 ) 2 CO 3 + Aq. Easily sol. in KOH, or NaOH+Aq, or in alkali sulphides +Aq. Sol. in 50 pts. cold dil. NH 4 OH+Aq. (Geiger.) Insol. in (NH 4 ) 2 CO 3 +Aq. Insol. in cold, but sol. in hot alkali carbon- ates -fAq. (Berzelius.) Insol. in Na 3 SbS 4 +Aq. When boiled with alcohol, ether, CS 2 , oil of turpentine, etc., portion of the S is dis- solved out. (Berzelius.) CS 2 dissolves about 5% of the sulphur. (Rammelsberg.) Antimony pewtasulphide with M 2 S. See Sulphantimonates, M. Antunony sulphochloride, SbSCl 3 . Decomp. by moist air or H 2 O. (Cloez. A. ch. (3) 30. 374.) SbS 2 Cl. Easily attacked by acids; insol. in CS 2 . (Ouvrard, C. R. 116. 1516.) Sb 2 S 5 Cl. (Ouvrard.) 2SbSCl, 3Sb 2 S 3 . Decomp. by dil. HC1+ Aq. (Schneider.) SbSCl, 7SbCl 3 . Deliquescent; decomp. by H 2 O. (Schneider, Pogg. 108. 407.) Antimony sulphofluoride, SbF 6 S. See Antimony fluo sulphide. Antimony sulphoiodide, SbSI. Not attacked by H 2 O, and decomp. only by cone, acids. Insol. in CS 2 . (Schneider, Pogg. 110. 147.) Sb 2 S 3 Ie. (Henry and Garot.) Sb 2 S 2 I 3 . Sol. in dry CS 2 . Very easily de- comp. (Ouvrard, C. R. 117. 108.) or C 6 H 6 . (Sabanajew, Zeit. Ch. 1871. 204.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 826.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Sb 4 O s Cl 2 . Algaroth powder. Decomp. by H 2 O. Sol. in HCl+Aq (Cooke, Proc. Am. Acad. 13. 1); tartaric acid+Aq. (Schaffer. A. 152. 135.) Sb 8 O n Cl 2 . (Cooke.) Sb 8 OCl 22 . Sb 41 O 50 Cl 23 . From SbCl 5 . SbOCl 3 . Deliquescent. De- composed by H 2 O. Sol. in H 2 O. (Daubrawa, A. 184. 118.) Does not exist. (Anschutz and Evans. A. 239. 285.) Sb 3 OCli 3 . Deliquescent. Insol. in CS 2 ; easily sol. in tartaric acid+Aq. (Williams, C. N. 24. 224.) Sb 3 O 4 Cl 7 . (Williams.) SbO 2 Cl. Decomp. by hot H 2 O into HSbO 3 . Antimonyl fluoride. From SbF 3 . Sb 4 O 3 F 6 . Not deliquescent. (Fliickiger, Pogg. 87. 249.) Antimonyl caesium fluoride, SbF 4 OH, CsF. (Wells, Am. J. Sci. 1901, (4) 11. 456.) Antimonyl sodium fluoride, SbOF 3 , NaF+ H 2 O. Deliquescent. Easily sol. in HoO. (Marig- nac, A. 145. 239.) Antimonyl iodide, Sb 4 O 6 I 2 . Difficultly sol. in solution of tartaric acid or tartrates. Decomp. by HC1, HNO 3 , or H 2 SO 4 +Aq. Easily sol. in alkalies, or (NH 4 ) 2 S+Aq. SbOI. Insol. in CS 2 . (Cooke, Proc. Am. Acad. (2) 6. 72.) Antimonyl sulphide. See Antimony oxysulphide. ARSENIC CHLORIDE 53 Argon, A. 100 cc. H 2 O dissolve 4.05 cc. argon at 13.9. Critical t 121 .6 under 50.6 atmos. Bpt. - 186.9. Sp. gr. 19.9. (Rayleigh, C. N. 1895, 71. 51-62; 299-302; C. C. 1895. 467.) Coefficient of absorption in H 2 O at 12 = 0.0394; at 13.9 = 0.0405. (Ramsay, Phil. Trans. 1895, 186. A. 225.) Absorption by H 2 at t. t Coefficient of absorption 10 20 30 40 50 0.0561 0.0438 0.0379 0.0348 0.0338 0.0343 (Antropoff, Roy. Soc. Proc. 1910, 83. A. 480.) Absorption of argon by H 2 at t and 760 mm. pressure. t Coefficient of absorption 0.05780 1 0.05612 5 0.05080 10 0.04525 15 0.04099 20 0.03790 25 0.03470 30 0.03256 35 0.03053 40 0.02865 45 0.02731 50 0.02567 (Estreicher, Z. phys. Ch. 1899, 31. 184.) 1 1. H 2 at 38 absorbs 25.7 cc. A. 1 1. blood absorbs 25.3 cc. A. (Regnard and Schloesing, C. R. 1897, 124. 303.) Not absorbed by members of the fatty series of organic compounds; with members of the aromatic series absorption was ob- served varying from 8% of the volume em- ployed for benzene to 1 % for aniline. (Berth- elot, C. R. 1899, 129. 71.) Arsenamide, As(NH 2 )3. Insol. in liquid NH 3 . Decomp. by H 2 O. (Hugot, C. R. 1904, 139. 55.) Arsenic, As. Unaltered by pure H 2 O. Insol. in HC1 + Aq if air is excluded, but si. sol. in presence of air. Not attacked by dil. H 2 SO 4 +Aq. Oxi- dized by cone. H 2 SO 4 , HNO 3 , or aqua regia. Not attacked at 20 by HNO 3 , cone, or dll., or containing NO 2 ; nor by HN0 3 +HC1, as long as they do not act on each other; but if treated with the above mixture in extremely dilute state, and a few drops of KNO 2 +Aq are added, the As is attacked at once. (Mil- Ion, A. ch. (3) 6. 101.) Sol. in sea water; 0.009 mg. per liter off Brittany; 0.01 to 0.09 mg. per liter near Azores. (Gautier, C. R. 1903, 137. 232.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in liquid .NH 3 . (Hugot, A. ch. 1900, (7)21.31.) Insol. in NaOH, KOH, or NH 4 OH+Aq. Sol. in S 2 Br 2 . (Hannay, Chem. Soc. (2) 11. 823.) Insol. in alcohol and ether. Sol. in certain fatty oils. Insol. in methylene iodide. (Retgers, Z. anorg. 3. 343.) Yi ccm. oleic acid dissolves 0.0032 g. As in 6 days. (Gates, J. phys. Ch. 1911, 15. 143.) Yellow modification. Very unstable. (Mc- Leod, C. N. 1894, 70. 139.) Fairly stable in liquid air. (Thomson, Chem. Soc. 1906, 90. (2) 745.) 100 ccm. CS 2 dissolve at: 46 20 12 15 60 11 8 6 4 2.0-2.5 l.Og. As. Less sol. in benzene and ethyl acetate. (Erdmann, Z. anorg. 1902, 32. 448.) Arsenic acid. See page 59. Arsenic bromide, AsBr 3 . Decomp. by H 2 O. Completely sol. in about 3 pts. boiling H 2 O, and much less, in presence of HBr. (Wallace, Phil. Mag. (4) 17. 261.) Sol. inCS 2 . Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 26.) Easily sol. in PC1 3 and PBr 3 . (Walden, Z. anorg. 1900, 25. 211.) Sol. in S 2 C1 2 . (Walden, Z. anorg. 1900, 25. 217.) Arsenic caesium bromide, 2AsBr 3 , 3CsBr. Decomp. by H 2 O; can be recryst. from cone. HBr+Aq. (Wheeler, Z. anorg. 4. 451.) Arsenic rubidium bromide, 2AsBr 3 , 3RbCl. As the corresponding Cs comp. Arsenic bromide ammonia, AsBr 3 , 3NH 3 . Decomp. by H 2 O. (Besson, C. R. 110. 1258.) Arsenic bromide copper, 2AsBr 3 ,7Cu. Stable toward hot H 2 O. Decomp. by KOH. (Hilpert andHernnan, B. 1913, 46. 2224.) Arsenic bromide silver, AsBr 3 , 3Ag. Scarcely decomp. by cold H 2 O. (Hilpert and Herrmann.) Arsenic chloride, AsCl 3 . Miscible with little H 2 O, and with alcohol, ether, and volatile oils. Decomp. by much H 2 O, or by boiling. (Gmelin.) 54 ARSENIC CHLORIDE Miscible with oil of turpentine, and wit! olive oil. Somewhat sol. in HCl+Aq. Easily sol. in PC1 3 and PBr 3 . (Walden Z. anorg. 1900, 26. 211.) Sol. in liquid CN. (Centnerszwer, J. russ phys. Ges. 1901, 33. 545.) Sol. in SoCl 2 . (Walden, Z. anorg. 1900, 25 217.) Arsenic penta chloride, AsCl 5 . Fumes in the air with evolution of hydro gen chloride. Readily sol. in CS 2 , and ab solute ether cooled to 30. (Baskerville J. Am. Qhem. Soc. 1902, 24. 1070.) Arsenic caesium chloride, 2AsCl 3 , 3CsCl. Decomp. by H 2 O. 100 pts. HCl+Aq (1.2 sp. gr.) dissolve 0.429 pt. salt. (Wheeler Z. anorg. 4. 451.) Arsenic indium phosphorus chloride. See Iridium phosphorus chloride arsenic chloride. Arsenic rubidium chloride, 2AsCl 3 , 3RbCl. Decomp. by H 2 O. 100 pts. HCl+Aq (sp gr. 1.2) dissolve 2.935 pts. salt. (Wheeler, Z anorg. 4. 451.) Arsenic sulphur chloride, 2AsCl 3 , 3SC1 2 . Decomp. by H 2 O. (Rose.) Above compound is a mixture. (Nilson C. N. 81. 81.) Arsenic chloride ammonia, 2AsCl 3 , 7NH 3 . Decomp. by cold H 2 O, with evolution of NH 3 . From the solution crystallizes As 4 CL N 2 H 10 8 . Sol. in alcohol without decomp. (Rose, Pogg. 52. 62.) Composition is AsCl 3 , 4NH 3 . (Besson, C. R. 110. 1258.) Arsenic chloride copper, 2AsCl 3 ,7Cu. Somewhat decomp. by H 2 O. Decomp. by KOH, or hot HC1. (Hilpert and Herrman, B. 1913, 46. 2224.) Arsenic chloride silver, 2AsCl 3 , 7Ag. H 2 O, NH 4 OH and KOH split off Ag. (Hil- pert and Herrmann.) Arsenic influoride, AsF 3 . Sol. in H 2 O with evolution of heat and de- composition. (Berzelius.) Easily sol. in benzene. (Moissan, C. R. 99. 874.) Miscible with alcohol and ether. (M'lvor, C. N. 30. 169.) Arsenic pewtafluoride, AsF 6 . Sol. in H 2 O, alkalies +Aq and liquid AsF 3 with evolution of heat. Absorbed by ether, alcohol and benzene with evolution of heat (Ruff, B. 1906, 39. 67.) Arsenic potassium fluoride, AsF 5 , KF + AsF 5 , 2KF+H 2 O. AsF 5 , AsOF 3 , 4KF+3H 2 O. (Marignac, A. 145. 237.) Arsenic fluoride ammonia, 2AsF 3 , 5NH 3 . Easily decomp, by H 2 O. (Besson, C. R. 110. 1258.) Arsenic pewtofluoride nitrosyl fluoride, AsF 5 , NOF. Decomp. by H 2 O, fuming HC1, NaOH+Aq, dry ether and dry alcohol with evolution of NO. Sol. in cone. HNO 3 , hot cone. HoSO 4 , boiling NOC1 and AsF 3 . Insol. in CC1 4 and CS 2 . (Ruff, Z. anorg. 1908, 58. 327.) Arsenic ^fluoride sulphur 2AsF 3 , SC1 4 . Very hydroscopic. Decomp. by H 2 O and NaOH. Decomp. by thionyl chloride, CC1 4 , CS 2 , abs. alcohol and ether. Decomp. by ligroin, benzene and toluene. (Ruff, B. 1904, 37. 4520.) Arsenic hydride, AsH 3 . SI. sol. in H 2 O and alkali hydrates+Aq, with subsequent decomposition. H 2 O ab- sorbs Vs vol. AsH 3 . Decomp. by cone, acids. Absorbed rapidly by oil of turpentine, slightly by fixed oils, and not at all by alcohol, ether, orKOH+Aq. (Gmelin.) Insol. in KOH + Alcohol. (Meissner.) Not more sol. in alkaline solutions than in pure H 2 O. (Berzelius.) AsH. Solid. Insol. in H 2 O, alcohol, ether, and CS 2 . (Wiederhold, Pogg. 118. 615.) Insol. in H 2 O; sol. in methylene iodide, cylene, or in cone. KOH+Aq. (Retgers, Z. anorg. 4. 403.) Arsenic hydride boron bromide, AsH 3 , BBr 3 . Easily decomp. Decomp. by. H 2 O. Ap- preciably sol. in AsH 3 or BBr 3 . Insol. in CS 2 . Stock, B. 1901, 34. 949.) Arsenic (Modide, As 2 I 4 . Decomp. by H 2 O or alkalies; easily sol. in alcohol, ether, chloroform, or carbon disul- hide. (Bamberger and Phillip, B. 14. 2643.) Not attacked by cold cone. H 2 SO 4 or by sold fuming HNO 3 . The latter oxidizes on vanning. Decomp. by pyridine. Sol. in soiling acetic anhydride. (Hewitt and Win- mill, Chem. Soc. 1907, 91. 962.) Vrsenic friiodide, AsI 3 . Sol in 3.32 pts. boiling H 2 O, and solution boiled down deposits pure AsI 3 , but if left o cool slowly, deposits crystals of As 2 O 3 and LfiUl. SI. sol. in HCl+Aq. Sol. in POC1 S , PC1 3 and PBr 3 . (Walden, r. anorg. 1900, 25. 212.) ARSENIC OXIDE 55 Sol. in PC1 3 . (Beckmann, Z. anorg. 1906 61. 110.) Sol. in SOC1 2 , S 2 C1 2 and S0 2 C1 2 . (Walden Z. anorg. 1900, 25. 216.) Sol. in SnCl 4 . (Walden, I.e.} Easily sol. in AsBr 3 . (Walden, Z. anorg 1902, 29. 374.) Sol. in AsCl 3 . (Walden, Z. anorg. 1900 26. 214.) Sol. in alcohol without decomp. Sol. in ether, benzene, chloroform, and CS 2 100 pts. methylene iodide dissolve 17.4 pts AsI 3 at 12. (Retgers, Z. anorg. 3. 343.) Arsenic pentaiodide, AsI 5 . More or less sol. in H 2 O, alcohol, CHC1 3 ether and CS 2 . (Sloan, C. N. 1882, 46. 194.. Arsenic caesium iodide, 2AsI 3 , 3CsI. Decomp. by H 2 O; sol. in cone. HI+Aq (Wheeler, Z. anorg. 4. 451.) Arsenic rubidium iodide, 2AsI 3 , 3RbI. As the corresponding Cs comp. Arsenic sulphur iodide. See Arsenic sulphoiodide. Arsenic Zraodide ammonia, 2AsI 3 , 9NH 3 . Insol. in benzene. (Bamberger and Phillip B. 14. 2643.) Asl,, 4NH 3 . (Besson, C. R. 110. 1258.) Arsenic nitride, AsN. Easily decomp. into As and N. (Hugot, C, R. 1904, 139. 56.) Decomp. by heat. (Franz Fischer, B. 1910, 43. 1471.) Arsenic sw&oxide, As 2 O (?). Insol. in H 2 O; decomp. by dil. acids or NH 4 OH+Aq. Does not exist. (Geuther, A. 240. 208.) Arsenic fnoxide, As 2 O 3 . "White arsenic" exists in two modifica- tions: aAs 2 O 3 , crystalline, octahedral, opaque, porcelaneous, etc.; /3As 2 O 3 , amor- phous, vitreous, "arsenic glass." The data concerning the solubility of As 2 O 3 are very contradictory, the reasons being that (1) the solubility of the two modifications is different; (2) that the length of time necessary to effect solution differs in the two modifica- tions; and (3) that there is a tendency of the amorphous As 2 O 3 to go over into the crystal- line state during the process of solution. aAs 2 O 3 is also not easily moistened, especially when in a pulverulent condition, which is not the case with the p modification. (Winkler, J. pr. (2) 31. 247.) The older data are very unreliable, but pos- sess a certain historical interest. 1 pt. As 2 O 3 is sol. in 10.55 pts. (Wenzel); 11.34 pts. (Fischer); 11.86 pts. in % hour (Klaproth); 12.2 pts. (Bucholz); 15.0 pts. (Brandt; Bergman); 16.0 pts. (Vogel) ; 24 pts. (Lametherie) ; 40 pts. (Porner) ; 64 pts. (Baume) ; 80 pts. (Navier) ; 200 pts. (Aschof and Nasse, 1812) ; 640 pts. (Hagen, 1796) boiling H 2 O. 1 pt. As 2 Os is sol. in 7.72 pts. H 2 O if a, or 9.33 pts. if j8 (Guibort) ; in 24 pts. HjO if a, or 21 pts. if (Taylor). Sol. in 53.3 pts. H 2 O at 18.75. (Abl.) Sol. in 30 pts. H 2 O. (Nussembrock.) After the solution in H 2 O at 100 has been left stand- ing at ordinary temperatures 1 pt. As 2 O3 remains dissolved in 16 pts. H 2 O at 16, and 20 pts. H 2 O at 7 (Bucholz) ; in 33 pts. H 2 O at 7 (Klaproth) ; in 38.45 pts. H 2 O after 3 days, 55 pts. H 2 O after 8 days, 64.50 pts. H 2 O after 2.3 weeks at 10 (Fischer) ; in 33.52 pts. if aAs 2 O 3 was used, 55.06 pts. if jSAszOs was used (Guibort) ; in 38 pts. if aAs 2 Os after 6 months, 53.71 pts. if #As 2 O 3 after 48 hours (Taylor). When an excess of pulverized As 2 Os is left to digest for several days with cold H 2 Q 1 pt. dissolves in 50 pts. (Bucholz); in 66 pts. (Fischer) ; in 80 pts. at 15 (Bergman) ; in 80 pts. if a, and 103 pts. if /3 (Guibort) ; 96 pts. at 10 (Spelman) ; 96 pts. at 35.5 (Hahnemann); 320 pts. H 2 O at 20 (Aschof and Nasse, 1812.) H 2 O at 15.6 or below dissolves less than Y% AszOj. (Dalton.) To dissolve 1 pt. As 2 C>3 in 12 pts. H 2 0, it is necessary to boil an excess of As 2 O 3 with H 2 O; if 1 pt. As 2 Os is boiled with 12 pts. H 2 O, considerable remains undis- solved; and even with 1 pt. As 2 O 3 to 50-60 pts. H 2 O long continued boiling is necessary to effect solution. If a clear solution saturated by long boiling with an excess of As 2 O 3 is poured off and evaporated con- tinuously to % its original bulk, no As 2 O 3 separates out, and the solution contains 1 pt. As 2 O 3 to 6 pts. H 2 O. (Fischer.) 100 pts. aqueous solution of /3As 2 Os sat. at 15 con- tain 0.96 pt. AssOs, and 9.68 pts. when sat. at 100. (Guibort.) If 1 pt. pulverized As 2 O 3 be digested 10 days at 19-25 in 5-10 pts. H 2 O, the solution contains 1 pt. As 2 O 3 to 50 pts. H 2 O. A solution of same strength is obtained in 25 days by digesting 1 pt. As 2 O 3 in 40 pts. H 2 O. If 1 pt. As 2 O 3 be immersed in 80 pts. H 2 O, the resulting solution contains 1 pt. As 2 Os to 90 pts. H 2 O; if in 160 pts. H 2 O, 1 pt. As 2 O 3 to 180 pts. H 2 O; if in 240 pts. H 2 O, 1 pt. As 2 O 3 to 280 pts. H 2 O; if in 1000 pts. H 2 O, 1 pt. As 2 Os to 1200 pts. H 2 O; and even when 1 pt. As 2 Os is digested at ordinary temperatures for several days with 16,000-100,000 pts. H 2 O, a portion remains undissolved. Pulverized aAs 2 O iwas set aside with H 2 O in closed bottles for 18 years; when 1 pt. As 2 Os was present in 1000 pts. H 2 O, a perfect solution was obtained; when 1 pt. As 2 O 3 in 100 pts. H 2 O, 0.017% As 2 O 3 was undissolved; when 1 pt. As 2 Os in 35 pts. H 2 O, 0.35% As 2 Os was undissolved, so that the solution contained 1 pt. As 2 O 3 to 54 pts. H 2 O. (Gmelin.) Porcelaneous modification (aAs 2 O 3 ) is much more sol. in H 2 O than the vitreous (/3As 2 O 3 ). 100 pts. H 2 O at ordinary temperature dissolve 0.96 pt. BAs 2 O 3 and 1.25 pts. oAs 2 Os; 100 pts. boiling H 2 O dissolve 9.68 pts. ?As 2 Os and 11.47 pts. aAs 2 O 3 ; and when the tempera- ;ure of this solution has fallen to 15, the solution from /3As 2 Os retains 1.78 pts., and that from aAs 2 Oj retains 2.9 pts. (Berzelius [citing Guibort].) /8As 2 O 3 dissolves more quickly and abun- dantly than aAs 2 O 3 . The same amount H 2 O which will take up 36-38 pts. As 2 O 3 at 12- 3 will dissolve only 12-14 pts. aAs 2 O 3 , or 00 pts. H 2 O dissolve 4 pts. /3As 2 O 3 and .2-1.3 pts. aAs 2 O 3 . By long boiling with 5 2 O, aAs 2 O 3 is converted into /3As 2 O 3 , and hus acquires the solubility of the latter, so hat 100 pts. boiling H 2 O can take up 11 pts. Ls 2 O 3 . But at low temperature /3As 2 O 3 is onverted into aAs 2 3 when in contact with H 2 O, so that the solution becomes weaker fter a while, and retains only the proportion f As 2 O 3 corresponding to the solubility of As 2 3 . Comminution, which hastens the ate of solubility of aAs 2 O 3 without increasing he amount dissolved, diminishes the solubil- ;y of 0As 2 O 3 , as this is converted into aAs 2 O 3 56 ARSENIC OXIDE by the friction or contact with H 2 0. As 2 O 3 , which has been rendered opaque by NH 4 OH, and that which has been crystallized from an aqueous solution, are equally sol. in H 2 O. (Bussy, C. R. 24. 774; A. 64. 286.) 100 pts. H 2 O dissolve 1.707 pts. /3As 2 O 3 in 2H years; 100 pts. boiling H 2 O dissolve 11.46 Ets. 0As 2 O 3 in 3 hours, and 11.86 pts. in 12 ours; 10.14 pts. aAs 2 3 in 3 hours, and 10.18 pts. in 12 hours. (Rose, Ann. Phys. (1) 36. 494.) A cold sat. solution which stood over excess of As 2 O 3 for 10 months at 10-20 contains 1.2% As 2 3 ; hot sat. solution a few days after saturation contains 2.25-2.50% As 2 3 . If trace of HC1 is present, the solution contains 3.8% As 2 3 . Hot sat. solution of porcelain mod. of As 2 O 3 contains 4 days after satura- tion 2.4% As 2 3 at 24; after 82 days at 14, 1.5%; after 4 months at 12, 1.3% As 2 3 . (Bacaloglo, J. pr. 83. 111.) According to later experiments, 1 pt. aAs 2 O 3 dissolves in 355 pts. H 2 O in 1 day at 15, while 1 pt. j8As 2 O 3 dissolves in 108 pts. H 2 O under the same conditions. 1 pt. aAs 2 3 dis- solves in 46 pts. H 2 0, if solution is prepared at 100, and allowed to stand 24 hours at 15, while 1 pt. /SAs 2 O 3 dissolves in 30 pts. H 2 O under the same conditions. (Biichner, N. Rep. Pharm. 22. 265.) 100 pts. H 2 O dissolve pts. aAs 2 3 and /3As 2 O 3 at ordinary temperature: Ratios of t Pts. + Pts. amts. dis- jSAsaOs /3As 2 O 3 solved at 80 : 18.5 80 1.0195 18.5 0.5422 1.88 1 1.3664 0.7203 1.89 1 1 . 1933 .... 0.6522 1.84 1 In the solution of /3As 2 O 3 , octahedral crys- tals were deposited on the sides of the vessel after 12 hours, which continued to increase. There was no such deposit in the case of aAs 2 O 3 . From the maxima in the above table, 100 pts. H 2 O can dissolve 3.7 pts. As 2 O 3 and 1.7 pts. aAs 2 O 3 at ordinary temperature. 100 pts. boiling H 2 O dissolve 11.46 pts. /3As 2 O 3 and 10.140 pts. aAs 2 O 3 in 3 hours; 11.86 pts. /3As 2 O 8 and 10.176 pts. aAs 2 O in 12 hours. (Cl. Winkler, J. pr. (2) 31. 247.) 100 pts. H 2 O dissolve 1.75 pts. of a third modification (hexagonal crystalline) at or- dinary temperature, and 2.75 pts. at 100. (Claudet, Chem. Soc. (2) 6. 179.) |9As 2 3 dissolves more rapidly in HCl-f Aq than aAs 2 O 3 . (Schultz-Sellac, B. 4. 109.) While 100 ccm. H 2 O dissolve 0.8507 g. /3As 2 3 at 18.5, 100 ccm. H 2 O containing 1.3195 g. HC1 dissolve 1.1513 g. j3As 2 O 3 ; containing 6.09 g. HC1, 1.2724 g. /3As 2 O 3 . (Chodounsky, Listy Chemicke", 13. 114.) 100 ccm. H 2 O dissolve 1.495 g. As 2 O 3 at 15. (W?od, Chem. Soc. 1908, 93. 412.) Solubility of crystalline As 2 O 3 in H 2 O. 1 1. of the sat. solution contains at: 2 15 .25 39.8 bpt. 12.006 16.566 20.384 29.302 60+g. As 2 O 3 (Bruner, Z. anorg. 1903, 37. 456.) Much more easily sol. in many acids than in H 2 O. Easily sol. in fuming H 2 SO 4 . (Schultz-Sellac.) 100 pts. dilute H 2 S0 4 +Aq of various strengths dissolve at t. (Chodounsky, I.e.] Decomp. by HNO 3 or aqua regia into As 2 O 6 . Sol. in H 3 P0 4 +Aq. (Bergman.) More sol. in HCl+Aq than in H 2 SO 4 , or HNO 3 +Aq, and still less in HC 2 H 3 O 2 +Aq. Solubility in HCl+Aq. Time aAsiOs /3As 2 3 Cone, of HCl+Aq Grams of As 2 Os per 100 cc. of solution 1 hour 0.023 1.589 3 hours 0.088 2.356 46N 1 52 6 hours 0.353 3.666 98N 1 41 12 hours 0.364 3.361 2 03N 1 17 24 hours 0.956 3.306 3 13N 1 11 2 days 1.627 2.629 3 81N 1 13 4 days 1.814 2.429 5 32N 2 20 1 week 1.673 1.763 6 SON" 5 11 3 weeks 1.776 1.713 7.85N 12.28 2M years 1.712 1.707 9.17N 18.16 As the concentration of the acid increases, the solubility of the oxide decreases, a mini- mum being reached when the concentration of the solvent is about 3.2N. Beyond this point, an increase in the concentration of the solvent leads to a corresponding increase in the solubility. (Wood, Chem. Soc. 1908, 93. 413.) Insol. in liquid CO 2 . (B.uchner, Z. phys. Ch. 1906, 64. 674.) Easily sol. in cold H 2 C 2 4 +Aq. (Berg- man.) When pulverized, it dissolves in hot H 2 C 2 O 4 +Aq, but separates out on cooling. Easily sol. in hot benzoic acid+Aq. Sol. in tartaric acid+Aq. Easily sol. in alkali hydrates, or carbonates +Aq. ARSENIC OXIDE 57 Easily sol. in NH 4 arsenite+Aq at 70-80, crystallizing out on cooling. (Berzelius.) Sol. in hot K 2 C 2 O 4 +Aq. Sol. in AsCl 3 . (Penney and Wallace.) More sol. in Na 2 B 4 O 7 -|-Aq than in H 2 O. Very si. sol. in absolute alcohol. (Vogel.) Sol. in 80 pts. highly rectified spirit. (Wenzel.) When 1 pt. powdered As2Os is digested 30 days 10-40 pts. alcohol, a solution is formed containing 1 pt. As2Os to 60 pts. alcohol; when 1 pt. As2Oa is digestec with 60-150 pts. alcohol, a solution is formed containing 1 pt. AszOs to 124-140 pts. alcohol. (Fischer.) Sol. in 70-80 pts. alcohol. (Thompson.) Alcohol dissolves 0.446 pt. /3As 2 O 3 . (Rose, Arsenic trioxide pentoxide, 3As 2 O 3 , 2As 2 O 5 +3H 2 O. Decomp. by H 2 O. (Joly, C. R. 100. 1221.) 2As 2 O 3 , As->O 5 +H,O. Decomp. bv H 2 O. (Joly.) As 2 O 3 , As 2 5 +H 2 O. (Joly.) Arsenic tefroxide, As 2 4 . SI. sol. in H 2 O from which it is partially pptd. by alcohol. More easily sol. in alkali carbonates or HCl+Aq. Most easily sol. in NaOH or KOH+Aq. (Herbst, Dissert. 1894.) A. I'nys. (i) oz. loo.; Arsenic pewtoxide, As 2 O 5 . 100 pts . alcohol dissolve pts. As 2 O 3 : Deliquescent in moist air; slowly sol. in TT f~\ fnrt-mi-nrr TT A O f~\ TTrVkirtVi n^k^ TP^^.1-.,. ^^.1 Vol. % of alcohol aAsaOs at 15 b.-pt. of alcohol jSAsaOs at 15 -Cl 2 v J ', lOIIillllg Jl 3 rVSvy 4 , wniCIl See. -Ljaoj^y oui. in alcohol; much more sol. in alcohol than As 2 O 3 . Very si. sol. in the fatty oils, 100 pts. of oil dissolving 0.2 pt. As 2 O 5 in the cold, and 56 1.680 4.895 0.504 1 pt. with partial decomp. on boiling. (Ber- 79 84 86 88 1.430 0^715 4.551 3.' 197 0.540 0.565 0'717 zelius.) 1000 pts. boiling poppy-oil dissolve 27 pts. As 2 O 5 ; 1000 pts. boiling castor-oil dissolve 34 pts. As 2 O 5 . (Heimpel and Grundner.) 100 0^025 3. '402 1.060 +4H 2 O. Solubility in H 2 O at t. (Girardin, J. Pharm. (3) 46. 269.) t Pts. HaAsCU inlOO pts. t Pts. HjAsO4 in 100 pts. 100 pts absolute alcohol dissolve 0.446 pt. solution solution /3As 2 O 3 in 2M years. (Winkler, J. pr. (2) 31. 55 69.9 CO 80.0 347.) Nearly 100 pts insol. in ether. . ether dissolve 0.454 pt. |8As 2 3 . 50 45 40 70.9 71.9 72.9 +5 10 81.0 82.1 83.3 (Winkler.j Qfv 73 Q 15 84 7 Ether extracts 1 mg. As 2 O 3 from sat. As 2 O 3 +Aq for every 15 cc. ether used; less is extracted when the solution is acidified with HC1, and almost none if acidified with OLlZ"Ht> Ul JJcul OltyLlIIl t5ullt?lj LJUU lllUltJ sol. in methyl alcohol, ethyl alcohol, ether, t Pts. HaAsO 4 in 100 pts. or chloroform. (Selmi.) of solution 100 pts. USj dissolve 0.001 pt /3As 2 8 in 1 1 AO OO 2M years. (Winkler.) + 10 f\f\ 88. o f\ 81. sol. in the fatty oils. 20 on 89. QQ 1000 pts. castor-oil dissolve 1.33 pts. As 2 O 3 oO oy . f\r\ at ordinary temperature, and 9 pts. at boiling 40 K(\ 90. Q1 temperature. 1000 pts. other oils dissolve 0.6-0.8 pt. As 2 O 3 in the cold, and about 1.7 O(J 60 7rt 'I . _ 91.9 Q9 A pts. on boiling. (Berzelius.) Insol. in chinoline or aniline. (Hoffmann, /u 80 on y,<5.o 93.2 QO Q A. ch. (3) 9. 143. 169.1 . yu yj . o a A 4 Moderately sol. in chinolin. (Beckmann 100 94.4 f\K f\ and Gabel, Z. anorg. 1906, 51. 236.) 110 i f)f\ 95.0 Qr (\ Insol. in acetone. (Naumann, B. 1904, 37. LZO i QH yo.o Qfi 9 4329); (Eidmann, C. C. 1899, II. 1014.) Sol. in amyl alcohol and is divided between *j. _. J TT /~\ *i,^ J.1- _ ,- -.4. ~ 4. >4. Sol. in boiling alkali hydroxides +Aq. (Szarvasy,B. 1897, 30. 1245.) Arsenic tfnselenide, As 2 S 3 . Partially sol. in KOH+Aq if boiled with it for a long time. (Uelsmann, A. 116. 123.) Arsenic pentoselenide, As 2 Se 5 . Insol. in most solvents, as cone. HC1. Sol. in alkali hydrates and sulpho-hydrates+Aq. (Szarvasy, B. 1895, 28. 2655-2656.) Insol. in H 2 O, in dil. acids and in cone. HC1. SI. sol. in warm HNO 3 +Aq. Oxidized by cold fuming HNO 3 . Sol. in alkalies and in hot alkali carbonates +Aq. Insol. in alcohol, ether, CS 2 , etc. (Clever, Z. anorg; 1895, 10. 129.) Arsenic selenosulphide. See Arsenic sulphoselenide. Arsenic sulphide, As 3 S. Ppt. Insol. in NH 4 OH or in colorless (NH 4 ) 2 S+Aq. Sol. in yellow NH 4 SH+Aq. (Scott, Chem. Soc. 1900, 77. 652.) Arsenic cftsulphide, As 2 S 2 . Min. Realgar. Difficultly sol. in alkali sulphides +Aq. Partly dissolved by KOH+ Aq with decomposition. Sol. at 150 in a sealed tube in NaHCO 3 +Aq, and crystallizes out on cooling. (SenarmOnt, A. ch. (3) 32. 158.) Arsenic bisulphide, As 2 S 3 . Insol. in H 2 O when prepared in the dry way, but when prepared moist is very liable to go into the colloidal modification mentioned below. Insol. in H 2 O containing H 2 SO 4 HNO 3 , HC1, H 2 C 2 O 4 , HC 2 H 3 O 2 , H 2 C 4 H 4 O 6 , C0 2 , NH 4 C1, KN0 3 , (NH 4 ) 2 S0 4 , MgSO 4 . (Bontigny.) Insol. in H 2 O. Traces are dissolved by H 2 S+Aq. SI. decomp. by boiling with H 2 O, or long contact with cold H 2 O. (Fresenius.) 1 1. H 2 O dissolves 2.1 x 10- 6 mols. pptd. As 2 S 3 at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Insol. in dil. acids. Insol. in cold, and scarcely attacked by hot cone. HCl+Aq. Easily decomp. by HNO 3 or aqua regia. Easily sol. in cold KOH, NaOH, or NH 4 OH +Aq, also in alkali carbonates, or sulphates + Aq. Sol. in hot KHSO 3 +Aq. Sol. in citric acid, and alkali citrates +Aq. (Spiller.) Slowly sol. in cold 2% Na 2 B 4 O 7 +Aq. Easily sol. on heating. (Materne, C. C. 1906, II. 557.) Insol. in CS 2 . Min. Orpiment. As 2 S 3 may also be obtained in a colloidal form, sol. in H 2 O. Sat. solution contains 34.46% As 2 S 3 ; it is decomp. by standing, but may be boiled without undergoing decom- position; most acids and many salts ppt. As 2 S 3 (Schulze, J. pr. (2) 25. 431.) The following solutions cause pptn. of As 2 S 3 in a .solution of the colloidal modifica- tion, when added in the given state of dilu- tion: 1 : 555 1 :276 1 : 255 1 : 138 1 :65 1 :26 1 : 0.18 1 :76 1 : 129 : 188 :2780 : 2630 : 3330 :2860 :3440 :2380 52600 HCl+Aq HNO 3 +Aq . H 2 S0 4 +Aq . H 2 S0 3 +Aq . H 2 C 2 O 4 +Aq . H 3 P0 4 +Aq . HC 2 H 3 O 2 +Aq K 2 SO 4 +Aq . Na 2 S0 4 +Aq . (NH 4 ) 2 S0 4 +Aq CaSO 4 +Aq . MgSO 4 +Aq . ZnS0 4 +Aq . MnSO 4 +Aq . NiSO 4 +Aq . FeS0 4 +Aq . Al 2 (S0 4 ) 3 +Aq Tl 2 S0 4 +Aq . KCl+Aq KBr+Aq KI+Aq . Lil+Aq NaCl+Aq . NH 4 Cl+Aq . BaCl 2 +Aq . CaCl 2 +Aq . MgCl 2 +Aq . 799 137 103 55 127 212 207 2860 4370 10000 ARSENIC ACID 59 FeCls+Aq . AlCl 8 +Aq . CrCla+Aq . KNOa+Aq . NaNOs+Aq . NH 4 NO 3 +Aq Ba(NO 3 ) 2 +Aq KC10 3 +Aq . CaH 2 (C0 3 ) 2 +Aq . K 2 G 2 H 4 6 +A q . K 2 CoO 4 +Aq . "..-' NaC 2 H 3 O 2 +Aq . Urea+Aq (NH 4 ) 2 Fe(SO 4 ) 2 +Aq K 2 Al 2 (SO 4 ) 4 +Aq . K 2 Fe 2 (SO 4 ) 4 +Aq . K 2 Cr 2 (S0 4 ) 4 +Aq . K 4 Fe(CN) 6 +Aq . K 3 Fe(CN) G +Aq . 1 : 50000 1 : 83000 : 20000 :84 : 117 : 138 :2080 :88 : 3120 :85 1 :78 1 :25 1 : 1160 1 : 50000 1 : 55500 1 : 25000 1 :67 1 :81 Cold cone, solutions of boric, arsenious, tar- taric, benzoic, and salicylic acids, also cane sugar, or chloral hydrate cause no pptn. Ab- solute alcohol and glycerine may also be mixed with the solutions without causing pptn. (Schulze, J. pr. (2) 25. 442.) +6H 2 O; decomp. completely into As 2 S 3 under a pressure of 6000 to 7000 atmos. (Spring, Z. anorg. 1895, 10. 186.) Arsenic pewfa sulphide, As 2 S 5 . Insol. in H 2 O. Sol. in NH 4 OH, KOH, NaOH+Aq, and solutions of alkali sulphides and carbonates. Sol. in BaOoH 2 , and Ca0 2 H 2 +Aq. Sol. in citric acid, and alkali citrates +Aq. (Spiller.) Alcohol dissolves out S on boiling. (Ber- zelius.) Sol. in alkali arsenates+Aq. (Nilson, J. pr. (2) 14. 155.) +H 2 O. (Nilson, I.e.} Arsenic bisulphide, with M 2 S. See Sulpharsenites, M. Arsenic pentasulphide, with M 2 S. See Sulpharsenates, M. Arsenic sulphobromide, AsS 2 Br 3 =AsSBr+ SBr 2 . Decomp. by H 2 O. (Hannay, Chem. Soc. 33. 284.) Arsenic sulphochloride, As 2 S5Cl. Slowly decomp. by boiling H 2 O. Sol. in hot AsCl 3 without decomp. (Ouvrard, C. R. 116. 1516.) AsS 2 Cl. Decomp. by H 2 O. Sol. in NH 4 OH, and alkali carbonates +Aq. (Ouv- rard.) AsS 2 Cl. Slowly decomp. by boiling H 2 O. Sol. in alkali carbonates and in NH 4 OH+Aq. (Ouvrard, C. R. 1893, 116. 1517.) Arsenic sulphoiodide, AsSI. Insol. in alcohol, chloroform or carbon di- sulphide. (Schneider, J. pr. (2) 23. 486.) Formula is probably As 2 S 3 , AsI 3 . Slowly attacked by HCl+Aq; somewhat more easily by HNO 3 +Aq. Easily sol. in KOH, or NH 4 OH + Aq. (Schneider, J. pr. (2) 34.505.) 2AsIs, Sle. Decomp. on air. (Schneider, J. pr. (2) 36. 509.) As 4 S 5 I 2 . Less sol. in CS 2 than AsI 3 . (Ouv- rard, C. R. 117. 107.) As 2 SI 4 . (Ouvrard.) See also Arsenyl sulphoiodide. Arsenic sulphoselenide, As 2 SeS 2 . Easily sol. in cold NH 4 SH+Aq. Nearly completely sol. in (NH 4 ) 2 CO 3 + Aq. (v. Ge- richten, B. 7. 29.) As 2 SSe 2 . More difficultly sol. than the pre- ceding comp. in NH 4 SH+Aq. (v. Gerichten.) As 2 Se 2 S 3 . Sp. gr. = 6.402 at ca. 750. Insol. in most solvents. Easily sol. in al- kali hydroxides and sulphides +Aq. (Szar- vasy, B. 1895, 28. 2661.) As 2 Se 3 S 2 . Sp. gr. = 11.35 at 550-600. Insol. in most solvents. Easily sol. in alkali hydroxides and sulphides +Aq. (Szar- vasy, B. 1895, 28. 2659.) Arsenic telluride, As 2 Te 2 . Sol. in HNO 3 and HNO 3 +HCl+Aq. (Op- penheim, J. pr. 71. 266.) As 2 Te 3 . As above. (Oppenheim.) Arsenic acid, anhydrous, AsaOs. See Arsenic pentoxide. Metaarsemc acid, HAsO 3 . Slowly sol. in cold, quite easily sol. in hot H 2 O, with considerable evolution of heat, and conversion into H 3 AsO 4 . (Kopp, A. ch. (3) 48. 196.) OrthoSLTsemc acid, H 3 As0 4 . Sol. in H 2 O, with absorption of heat. 1 pt. As 2 O 5 dissolves in 0.405 pt. H 2 O at pts. pt. 1 12.5, or 100 pts. H 2 O dissolve 244.81 As 2 5 at 12.5. (Vogel.) Sol. in 0.5 pt. H 2 O. (Thenard.) Sol. in 6 pts. cold H 2 O, and more quickly in 2 pts. hot H 2 O. (Bucholz.) 100 pts. H 2 O at 15.56 dissolve 150 pts. As 2 O 6 . (lire's Diet.) H 3 AsO 4 +Aq sat. at 15 contains 15% As 2 O 5 . Sp. gr. of H 3 As0 4 +Aq at 15: a = sp. gr. if % is As 2 O 5 ; b = sp. gr. if % is H 3 AsO 4 . % a 6 % a b 5 10 15 20 25 30 35 40 1.042 1.085 1.134 1.187 1.245 1.306 1.378 1.453 1.0337 1.0690 1.1061 1.1457 1.1882 1.2342 1.2840 1.3382 45 50 55 60 65 70 75 1.540 1.635 1.742 1.3973 1.4617 1.5320 1.6086 1.6919 1.7827 (Schiff, A. 113. 183, calculated by Gerlach, Z. anal. 27. 303.) 60 ARSENIC .ACID Sp. gr. of H 3 AsO 4 +Aq at 15: a =sp. gr. if % is As 2 O 5 ; 6 = sp. gr. if % is H 3 AsO 4 . less sol. in HC 2 H 3 O 2 +Aq. The neutral al- kaline-earth arsenates are less sol. in NH 4 OH I A /-* -fVioTi in TTr^ Viiii" mnvp Qnl "in "NTTTjf^l- % a b % a b ^^.fV(_| Tjlldll ill XI 2^-'; LHIL lilU \\J J At* *J J 11 12 1.092 1.102 1.073 1.081 57 58 1.777 1.801 1 54 9 1.56 4 Aluminum potassium arsenate, 2A1 2 O 3 , 3K 2 0, 13 1.111 1.088 59 1.825 1.57 9 2 5- " 14 1.121 1.096 60 1.850 1.594 (Lefe"vre.) 15 1 130 1 103 61 1.880 1 A1 ft 16 l!l40 1.111 62 1.910 1.'62 6 Aluminum sodium arsenate, 2A1 2 O 3 , 3Na 2 O, 17 1.150 1.119 63 1.940 1.64 3 3As 2 O 5 . 18 1.160 1.126 64 1.970 1.65 9 (Lefevre.) 19 1.170 1.134 65 2.000 1.675 20 1.180 1.142 66 2.030 1.69 3 Ammonium arsenate, (NH 4 ) 3 AsO 4 +3H 2 O. 21 1.191 1.150 67 2.060 1.71o Difficultly sol. in H 2 O. Less sol. in H 2 O 22 1.203 1.158 68 2.090 1 73o than (NH 4 ) 2 HAsO 4 . (Mitscherlich.) 23 1.214 1.167 69 2.120 1.74 9 Insol. in liquid NH 3 . (Franklin, Am. Ch. 24 1.226 1.175 70 2.150 1.767 J. 1898, 20. 826.) 25 1.237 1.183 71 l-78g 26 1.249 1.192 72 1.80 9 Ammonium hydrogen arsenate, 27 1.261 1.201 73 1.83 (NH 4 ) 2 HAs0 4 . 28 29 30 1.274 1.286 1.298 1.210 1.219 1 228 74 75 76 1.85i 1.87 2 1 897 Effloresces, giving off NH 3 ; more sol. in H 2 O than (NH 4 ) 3 AsO 4 . (Salkowsky, J. pr. 4 f\Jt -I f\{\ \ 31 32 1.312 1.325 1.238 1.248 77 78 1.92i 1.94 6 104. 129.) Insol. in acetone. (Eidmann, C. C. 1899, 33 1.339 1.257 79 1.97n '^ 34 35 36 37 1.352 1.366 1.381 1.396 1.267 1.277 1.288 1.299 80 81 82 83 u 1.995 2.02 2.04 5 2.07 Ammonium ^"hydrogen arsenate, NH 4 H 2 As0 4 . Not efflorescent. Very sol. in H 2 0. 38 1.411 1.309 84 2 095 39 1.426 1.320 85 2.'l2 Ammonium barium arsenate, NH 4 BaAsO 4 + 40 1.441 1.331 86 2.14 9 J^H^. 41 42 1.458 1.475 1.342 1.353 87 88 2.17 8 2.20 7 Sol. by 10 days' contact in 1391 pts. H 2 O; m 18,832 pts. of a mixture of 1 pt. NH 4 OH + 43 1.492 1.366 89 2.23 6 Aq and 3 pts. H 2 O; in 227 pts. of a solution 44 1.509 1.376 90 2.26 5 of 1 pt. NH 4 C1 in 10 pts. H 2 O; and in 2169 45 1.526 1.387 91 2.29 5 )ts. of a solution of 1 pt. NH 4 C1 in 10 pts. 46 1.545 1.400 NH 4 OH+ Aq and 60 pts. H 2 O. (Lefevre, A s\V\ 1 Of\O /!\ rtfT 1 O \ (Kopp, calculated by Gerlach, Z. anal. 27. A. cn. 189J, (b) 27. 13.) (NH 4 ) 2 BaH 2 (AsO 4 ) 2 . Efflorescent. Insol. 316.) See also Arsenic pentoxide. n H 2 0; easily sol. in dil. HN0 3 +Aq. (Bau- mann, Arch. Pharm. 36. 36.) P/roarsenic acid, Very deliquescent; easily sol. in H 2 with evolution of much heat, and conversion into H 3 As0 4 . Arsenates. Arsenates of the alkali metals, and acid arsenates of the alkaline-earth metals are sol. in H 2 O. Neutral and basic arsenates are easily sol. in mineral acids, including H 3 AsO 4 ; Ammonium calcium arsenate, NH 4 CaAsO 4 + 1000 pts. pure H 2 O dissolve 0.20 pt. this alt; 1000 pts. NH 4 Cl+Aq (containing 50 pts. NH 4 C1) dissolve 4.15 pts. this salt; 900 pts. H 2 O + 100pts. NH 4 OH (sp. gr. =0.880) dis- olve 0.01 pt. this salt. (Field, Chem. Soc. 11. Soluble by 10 days' contact in 2167 pts. H 2 O at 15; in 381 pts. NH 4 Cl+Aq (1 :7); in ARSENATE TELLURATE, AMMONIUM 61 43478 pts. NH 4 OH+Aq (1 : 3); in 10570 pts. NH 4 Cl+NH 4 OH+Aq (1 : 10 : 60). (Lefevre, A. ch. 1892, (6) 27. 13.) +6H 2 O. Sol. in hot, very si. sol. in cold H 2 O; si. sol. in NH 4 C1, and NH 4 OH+Aq (Wach, Schw. J. 12. 285.) +7H 2 O. (Bloxam, C. N. 54. 163.) (NH 4 ) 2 CaH 2 (AsO 4 ) 2 . Efflorescent. Insol. in H 2 O; easily sol. in dil. HNO 3 +Aq. (Bau- mann, Arch. Pharm. 36. 36.) (NH 4 )Ca 3 H 2 (AsO 4 ) 3 +3H 2 O. (NH 4 )Ca 6 H 5 (AsO 4 ) 6 +3H 2 O. (Bloxam, C. N. 54. 163.) Ammonium glucinum arsenate, NH 4 GlAsO 4 More stable than the corresponding potas- sium salt. (Bleyer, Z. anorg. 1912, 75. 291.) Ammonium iron (ferric) dihydrogen arsenate. NH 4 H 2 AsO 4 , FeAsO 4 . Hydrolyzed by H 2 O. Sol. in cold cone. HC1, hot HNO 3 , hot dil. H 2 SO 4 , and in hot arsenic acid+Aq contain- ing 75% arsenic pentoxide. Sol. in hot cone. NH 4 OH+Aq. Completely hydrolyzed by caustic alkalies. Insol. in cone. NH 4 Cl+Aq and in 50% acetic acid. (Curtman, J. Am. Chem. Soc. 1910, 32. 628.) lesium arsenate, Ammonium maj NH 4 MgAs 4 . SI. sol. in H 2 O. Sol. in acids. Anhydrous salt is sol. in 2784 pts. H 2 O at 15; in 15,904 pts. NH 4 OH+ Aq (1 : 3) (0.96 sp. gr.); in 1386 pts. NH 4 Cl+Aq (1 : 70); in 886.7 pts. NH 4 Cl+Aq (1 :7); in 3014 pts. NH 4 C1 (1 pt.)+NH 4 OH (0.96 sp. gr.) (10 pts.)+Aq (60 pts.); in 32,827 pts. magnesia mixture. (Fresenius, Z. anal. 3. 206.) Anhydrous salt is sol. in 4389 pts. NH 4 NO 3 +Aq (1 :50); in 2561.5 pts. KCl+Aq (1 : 165); in 1422 pts. ammoniacal solution of 3.5 g. tartaric acid in 250 cc. H 2 O; in 933.5 pts. ammoniacal solution of 2.5 g. citric acid in 250 cc. H 2 O. (Puller, Z. anal. 10. 62.) Sol. in 2656 pts. H 2 O at 15; in 15,038 pts. NH 4 OH+Aq (1 : 3) (0.96 sp. gr.); in 844 pts. NH 4 Cl+Aq (1:7); in 1315 pts. NH 4 Cl+Aq (1 : 70); in 2871 pts. NH 4 C1 (1 pt.)+NH 4 OH (0.96 sp. gr.) (10 pts.)+Aq (60 pts.). (Fre- senius.) 1000 pts. pure H 2 O dissolve 0.14 pt. salt; 1000 pts. NH 4 Cl+Aq (containing 100 pts. NH 4 C1) dissolve 0.95 pt. salt; 900 pts. H 2 O + 100 pts. NH 4 OH (sp. gr. 0.880) dissolve 0.07 pt. salt. (Field, Chem. Soc. 11. 6.) +6H 2 O. SI. efflorescent. SI. sol. in H,O. Very si. sol. in NH 4 OH+Aq. Solubility of NH 4 MgAsO 4 +6H 2 O in H 2 O and NH 4 salts +Aq. Grams salt dissolved in 100 g. solvent. t H 2 O 5% NH 4 NOa+Aq 5% NH 4 Cl+Aq NH 4 OH-t-Aq 1 pt. NH 4 OH + Aq (0.96) +4 pts. H 2 O 4% NEUOH + Aq+5% NH 4 Cl+Aq 4% NH 4 OH + Aq +10% NH 4 Cl+Aq 0.03388 0.09216 0.08397 0.00874 20 30 0.02066 0.11358 11758 0. 12284 11204 0.00958 0.01331 0.03165 40 02746 13936 19016 01173 50 0.02^61 18945 18889 0.01005 60 70 0.02103 0.01564 0.21115 18880 0.21952 22092 0.00902 0.00949 0.04691 0.05353 80 0.02364 0. 18945 0.23144 0.00912 (Wenger, Dissert. 1911.) Ammonium manganous arsenate, NH 4 MnAsO 4 +6H 2 O. Nearly insol. in cold H 2 O; easily sol. in dil. acids; insol. in alcohol. (Otto, J. pr. 2. 414.) Ammonium sodium arsenate. NH 4 NaHAsO 4 +4H 2 0. Sol. in H 2 O. (Uelsmann, Zeit. f. ges. Nat. 23. 347.) Ammonium sodium hydrogen arsenate, (NH 4 ) 3 Na 3 H 6 (AsO 4 ) 4 +6H 2 O. Sol. in H 2 O. (Filhol and Senderens, C. R. 94. 649.) Ammonium strontium arsenate, NH 4 SrAsO 4 . Sol. by 10 days' contact in 3229 pts. H 2 O, in 11,586 pts. dil. NH 4 OH+Aq, in 199 pts. of a mixture of 1 pt. NH 4 C1 in 7 pts. H 2 O, and in 1519 pts. of a solution of 1 pt. NH 4 C1 in 10 pts. NH 4 OH+Aq and 60 pts. HoO. (Lefevre, A. ch. 1892, (6) 27. 13.) Ammonium uranyl arsenate, NH 4 (UO 2 )AsO 4 Insol. in H 2 O, HC 2 H 3 O 2 , and saline solu- tions as NH 4 Cl+Aq; sol. in mineral acids. (Puller, Z. anal. 10. 72.) Ammonium vanadium arsenate, NH 4 (V0 2 ) 2 As0 4 , and (NH 4 ) 2 HAsO 4 + 2(VO 2 ) 2 H 2 AsO 4 . See Arseniovanadate, ammonium. Ammonium arsenate tellurate. See Arseniotellurate, ammonium. 62 ARSENATE, ANTIMONY Antimony arsenate (?). Insol. in H 2 0; insol. in acids after ignition, but when fresh is sol. in cone, boiling HC1+ Aq, and si. sol. in HNO 3 +Aq. (Dumas.) Barium arsenate, Ba 3 (AsO 4 ) 2 . 1000 pts. pure H 2 O dissolve 0.55 pt. Ba 3 (AsO 4 ) 2 ; 1000 pts. NH 4 Cl+Aq (containing 50 pts. NH 4 C1) dissolve 1.95 pts. Ba 3 (AsO 4 ) 2 ; 900 pts. HoO + 100 pts. NH 4 OH+Aq (sp. gr. = 0.88) dissolve 0.03 pt. Ba 3 (AsO 4 ) 2 . (Field, Chem. Soc. 11. 6.) Sol. in cold HNO 3 , and HCl+Aq (Berze- lius); H 2 C 4 H 4 6 , and HC 2 H 3 2 +Aq. (An- thon.) Solubility in H 2 O is not increased by pres- ence of NH 4 , Na, or K salts. (Laugier.) Not pptd. in presence of Na citrate. (Spiller.) . (Salkowsky, J. pr. 104. 129.) Barium hydrogen arsenate, BaHAsO 4 + . Very si. sol. in H 2 O, but decomp. thereby into Ba 3 (As0 4 ) 2 and BaH 4 (AsO 4 ) 2 . (Berze- lius.) SI. sol. in cold acids. +H 2 O. SI. sol. in either BaCl 2 +Aq or Na 2 HAsO 4 +Aq. (Maumene, J. B. 1864. 237.) Barium tetrahyfaogen arsenate, BaH 4 (AsO 4 ) 2 +2H 2 0. Easily sol. in H 2 O. (Setterberg, Berz. J. B. 26. 206.) Difficultly sol. in little, but decomp. by much H 2 O. Easily sol in 'HCl+Aq, less easily in HC 2 H 3 2 +Aq (Hermann, Dissert, 1879.) Barium arsenate, acid, BaO, 2As 2 O 5 +4H 2 O. Very si. sol. in H 2 O. (Mitscherlich.) Barium p?/roarsenate, Ba 2 As 2 7 . Insol. in H 2 O, but decomp. thereby into BaHAsO 4 -f H 2 O. (Lefevre, C. R. 108/1058.) Barium potassium arsenate, BaKAsO 4 . SI. decomp. by cold H 2 O; rapidly sol. in dil. acids. (Lefevre, A. ch. (6) 27. 1.) Barium sodium arsenate, BaNaAsO 4 + (Joly, C. R. 1887, 104. 1702.) Barium arsenate chloride, 3Ba 3 (AsO 4 ) 2 , BaCl 2 . Insol. in H 2 0; sol. in .dil. HNO 3 -f Aq. (Lechartier, C. R. 65. 172.) Bismuth arsenate, basic, BiAsO 4 , 3Bi 2 O 3 . Insol. in H 2 O. Sol. in mineral acids. (Cavazzi, Gazz. ch. it. 14. 289 ) 5Bi 2 O 3 , 2As 2 O 5 +8H 2 O. Min. Rhagite Easily sol. in HCl+Aq; si. sol. in HN0 3 + Aq. Bismuth arsenate, Insol. in H 2 O. Insol. in HNO 3 +Aq in presence of H 3 AsO 4 , or alkali arsenates+Aq; sol. in HCl+Aq. (Salkowsky, J. pr. 104. 129.) Not wholly insol. in HNO 3 +Aq. (Schneider, J. pr. (2) 20. 418.) Very sol. in H 3 AsO 4 +Aq. (Dumas.) Insol. in Bi(NO 3 ) 3 +Aq. (Dumas.) Sol. in Bi(NO 3 ) 3 +Aq. (Salkowsky.) Insol. in cone. Bi(NO 3 ) 3 +Aq containing a small quantity of HNO 3 . (Schneider.) Bismuth copper arsenate, BioCu 2 oAs:oH 44 7 o = Bi 2 O 3 , 20CuO, 5As 2 O 5 +22H 2 O. Min. Mixite. Decomp. by dil. HNO 3 +Aq into insol. BiAsO 4 , and Cu 3 (AsO 4 ) 2 , which goes into solution. (Dana.) Bismuth uranyl arsenate, Bi 2 (As0 4 ) 2 , 8BiO 3 H 3 , (UO 2 ) 3 (AsO 4 ) 2 . Min. Walpurgite. Cadmium arsenate, Cd 3 (AsO 4 ) 2 . Ppt. (Salkowsky, J. pr. 104. 129.) 2CdO, As 2 O 5 . (Lefevre, C. R. 110. 405.) 5CdO, 2As 2 O 5 +5H 2 O. Ppt, (Salkowsky.) Ca\imium p?/r0arsenate, Cd 2 As 2 O 7 . (de Schulten.) Cadmium hydrogen arsenate, CdHAsO 4 + H 2 O. Decomp. by H 2 O. (Demel, B. 12. 1279.) CdH 4 (AsO 4 ) 2 +2H 2 O. Decomp. by excess of H 2 O. (de Schulten, Bull. Soc. (3) 1. 473.) Cadmium potassium arsenate, 2CdO, K 2 0, As 2 O 5 . (Lefevre, C. R. 110. 405.) Cadmium sodium arsenate, CdO, 2Na 2 0, As 2 O 5 . Slowly sol. in dil. acids. (Lefevre, C. R. 110. 405.) 2CdO, 4Na 2 O, 3As 2 O 6 . (Lefevre.) Cadmium arsenate bromide, 3Cd 3 (AsO 4 ) 2 , CdBr 2 . Sol. in very dil. HNO 3 +Aq. (de Schulten, Bull. Soc. (3) 1. 472.) Cadmium arsenate chloride, 3Cd 3 (AsO 4 ) 2 , CdCl 2 . Sol. in very dil. HNO 3 +Aq. (de Schulten.) Caesium arsenate, Cs 2 O, 2As 2 O 5 +5H 2 O. Ppt. (Ephraim, Z. anorg. 1910, 65. 246.) Calcium arsenate, Ca 3 (AsO 4 ) 2 +3H 2 O. Ppt. Insol. in H 2 O; sol. in H 3 AsO 4 +Aq. (Kotschoubey, J. pr. 49. 182.) Calcium p?/roarsenate, Ca 2 As 2 O 7 . Slowly decomp. by cold H 2 O into CaHAsO 4 . (Lefevre.) ARSENATE, BASIC, CUPRIC 63 Calcium hydrogen arsenate, CaHAsO 4 + ^H 2 0. Insol. in H 2 O. (Debray, A. ch. (3) 61. 419.) +H 2 O. Min. Haidingerite. Easily sol. in acids. +2;HjH 2 O. Nlui^Pharmacolite. Easily sol. in acids. +3H 2 O. Insol. in H,O ; sol. in HC1, HNO 3 , or H 3 AsO 4 +Aq; also in (NH 4 ) 2 S0 4 , NH 4 NO 8 , NH 4 C 2 H 3 O 2 , and NH 4 Cl-fAq. (Pfaff.) Calcium teJrahydrogen arsenate, CaH 4 (AsO 4 ) 2 . Sol. inH 2 O. (Graham.) +H 2 O. SI. sol. in H 2 O. Decomp. by much hot H 2 O into H 3 AsO 4 and Ca 3 (AsO 4 ) 2 . (Hermann, Dissert. 1879.) Calcium iron (ferric) arsenate, 6CaO, 4Fe 2 O 3 , 5As 2 O 5 + 15H 2 O (?). Min. Arseniosiderite. Sol. in acids. Calcium magnesium arsenate, Ca 5 H 2 (AsO 4 ) 4 , Mg 5 H 2 (AsO 4 ) 4 + 10H 2 O. Min. Picropharmacolite. Easily sol. in acids. Ca 3 (AsO 4 ) 2 , Mg 3 (As0 4 ) 2 . Sol. in HNO 3 + Aq. (Kiihn.) Min. Berzeliite. Sol. in HNO 8 +Aq. Ca 8 Mg 6 Hi 4 (AsO 4 )i 4 +49H 2 O. Min. Wap- plerite. Calcium potassium arsenate, CaKAs0 4 . (Lefevre, A. ch. (6) 27. 5.) Calcium sodium arsenate, CaNaAsO 4 . (Lefevre, A. ch. (6) 27. 1.) 4CaO, 2Na 2 O, 3As 2 O 5 . Not attacked by boiling H 2 O; easily sol. in dil. acids, (Le- fevre.) Calcium uranyl arsenate, Ca(UO 2 ) 2 (AsO 4 ) 2 + 8H 2 O. Min. Uranospinite. Calcium vanadium arsenate, CaHAs0 4 , 2(VO 2 )H 2 AsO 4 +8H 2 O. See Arseniovanadate, calcium. Calcium arsenate chloride, Ca 3 (As0 4 ) 2 , CaCl 2 Insol. in H 2 O; sol. in dil. HNO 3 +Aq (Lechartier. C. R. 65. 172.) 3Ca 3 (AsO 4 ) 2 , CaCl 2 . As above. (Le- chartier.) Cerous arsenate, CeHAsO 4 . Insol. in H 2 O. Sol. in arsenic acid+Aq (Berzelius.) Ceric hydrogen arsenate, Ce(HAs0 4 ) 2 + 6H 2 O. Ppt. Insol. in H 2 O and dil. acids. (Bar bieri, B. 1910, 43. 2216.) Ceric cfthydrogen arsenate. Ce(H 2 AsO 4 ) 4 + 4H 2 0. Sol. in cone. HNO 3 . (Barbieri I. c.) Chromic arsenate, 2Cr 2 O 3 , 3As 2 O 5 . Insol. in H 2 O and cone, boiling acids. (Le- evre, A. ch. (6) 27. 5.) !hromic potassium arsenate, 2Cr 2 O 3 , 3K 2 O, 3As 2 O 5 . (Lefevre.) Chromic sodium arsenate, 2Cr 2 O 3 , 3Na 2 O, 3As 2 O 5 . (Lefevre.) Cobaltous arsenate, basic, 4CoO, As 2 O 5 . Easily sol. in acids. (Gentele, J. B. 1851. 559.) Co(CoOH)AsO 4 . Insol. in H 2 O; difficultly sol. in acids. (Coloriano.) Cobaltous arsenate, Co 3 (AsO 4 ) 2 +8H 2 O. Ppt. Insol. even in boiling H 2 O; easilv sol. in HNO 3 , HC1, and NH 4 OH+Aq; sol. in H 3 As0 4 +Aq (Proust); sol. in dil. FeSO 4 +Aq. Karsten, Pogg. 60. 266.) Min. Cobalt bloom. Erythrite. Easily sol. in acids. 5CoO, 2As 2 O 5 +3H 2 O. Insol. in H 2 O; dif- ficultly sol. in acids. (Coloriano, C. R. 103. 273.) 2CoO, AsaOs. SI. attacked by boiling H 2 O; easily sol. in dil. acids. (Lefevre.) Cobaltous hydrogen arsenate, CoH 4 (AsO 4 ) 2 . Sol. in H 2 0. Cobaltous potassium arsenate, CoKAsO 4 . (Lefevre.) Cobaltous sodium arsenate, CoNaAsO 4 . (Lefevre.) 4CoO, 2Na 2 O, 3As 2 O 5 . (Lefevre.) Cobaltous vanadium arsenate, Co(V0 2 ) 2 H 2 (As0 4 ) 2 +8H 2 0. See Arseniovanadate, cobaltous. Cobaltous arsenate ammonia, Co 3 (AsO 4 ) 2 , NH 3 +7H 2 O. (Ducru, A. ch. 1901, (7) 22. 185.) Co 3 (AsO 4 ) 2 , 2NH 3 +6H 2 O. (Ducru, I c.) Co 3 (AsO 4 ) 2 , 3NH 3 +5H 2 O. (Ducru, I, c.) Cuprous arsenate, 2Cu 2 O, As 2 O 5 . (Hampe, Dissert. 1874.) 4Cu 2 O, As 2 O 6 . (Hampe, L c.) Cuprous p^/roarsenate, Cu 4 As 2 O 7 . Ppt. Sol. in NH 4 OH or KOH+Aq. (Reichard, B. 1898, 31. 2166.) Cupric arsenate, basic, 8CuO, As 2 O 5 -f 12H 2 O. Min. Chalcophyllite. Easily sol. in acids andNH 4 OH+Aq. 6CuO, As 2 O 5 +3H 2 O. Min. Aphanesite, Clioclasite. Sol. in acids and ammonia. 5CuO, As 2 O 5 +2H 2 O. Min. Erinite. Sol. in HNOs+Aq. 64 ARSENATE, CUPRIC +5H 2 O. Min. Cornwallite. Sol. in acids, andNH 4 OH+Aq. +9H 2 O. Min. Tirolite. 4CuO, As 2 O 5 +H 2 O. Insol. in H 2 O. (De- bray, A. ch. (3) 61. 423.) Min. Olivenite. Sol. in acids, and NH 4 OH +Aq; decomp. by hot KOH+Aq. +7H 2 O. Min. Euchrvite. Sol.inHNO 3 + Aq. +4^H 2 O. (Hirsch, C. C. 1891, I. 15.) Cupric arsenate, Cu 3 (AsO 4 ) 2 . Insol. in H 2 O. Easily sol. in HCl+Aq; si. sol. in other acids; sol. in NH 4 OH+Aq. (Coloriano, C. R. 103. 273.) Insol. in methyl acetate. 1909, 42. 3790.) (Naumann, B. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) +4H 2 O. Decomp. by hot H 2 O. (Debray.) +5HoO. Min. Trichalcite. Easily sol. in cold HCl+Aq. Cupric arsenate, acid, 5CuO, 2As 2 O 5 . Sol. in H 2 SO 3 +Aq. (Vogel.) +3H 2 O. (Salkowsky.) +8, 9M, and 12HH 2 O. (Hirsch.) CuHAsO 4 +H 2 O. Insol. in H 2 0. (Color- iano.) + 1^H 2 O. Insol. in H 2 O. (Debray, A. ch. (3) 61. 419.) 8CuO, 3As 2 O 5 +12H 2 O. (Hirsch.) Cupric lead arsenate, 3CuO, PbO, As 2 O 5 + 2H 2 O. M in . Bayldonite . Nearly insol . in HNO 3 + Aq. Cupric potassium arsenate, CuKAs0 4 . Slowly sol. in NH 4 OH+Aq; easily sol. in acids. (Lefevre, A. ch. (6) 27. 5.) 8CuO, K 2 O, As 2 O 6 . Easily sol. in dil. acids. (Lefevre.) Cupric sodium arsenate, CuNaAs0 4 . (Lefevre.) 3CuO, Na 2 O, 2As 2 O 5 . Very sol. in dil. acids. (Lefevre.) 2Cu 3 (AsO 4 ) 2 , NaH 2 AsO 4 +5H 2 O. Ppt. (Hirsch, C. C. 1891, I. 15.) 6Cu 3 (AsO 4 ) 2 , 2NaH 2 As0 4 , Na 2 HAsO 4 + 13y 2 H 2 O, or 16H 2 O. Ppt. (Hirsch.) 3Cu 3 (AsO 4 ) 2 , Na 2 HAsO 4 +9^H 2 O. Ppt. (Hirsch.) 4Cu 3 (AsO 4 ) 2 , Na 2 HAs0 4 +llH 2 O. (Hirsch.) Ppt. Cupric uranyl arsenate, Cu(UO 2 ) 2 (AsO 4 ) 2 + 8H 2 O. (Wither, A. 68. 312.) Min. Zeunerite. Cupric vanadium arsenate, Cu(V0 2 ) 2 H 2 (As0 4 ) 2 +3H 2 0. See Arseniovanadate, cupric. Cupric arsenate ammonia, Cu 3 (AsO 4 ) 2 , 3NH 3 +4H 2 O. Insol. in cold or hot H 2 O. (Damour, J. pr. 37. 485.) 2CuO, As 2 O 5 , 4NH 3 +3H 2 0. Decomp. by" H 2 O. (Schiff, A. 123. 42.), Cupric arsenate calcium carbonate, 5CuO, As 2 O 5 , CaCO 3 +4H 2 O, or 9H 2 O. Min. Tyrolite. Easily sol. in acids, and NH 4 OH+Aq. Cupric arsenate sodium chloride. 2Cu 3 (AsO 4 )->, NaCl+7^H 2 0. Decomp. by hot H 2 O. (Hirsch, Dissert. 1891.) 3Cu 3 (As0 4 ) 2 , 2NaCl + 13^H 2 O. + 17^H 2 O. (Hirsch, i.e.) 5Cu 3 (AsO 4 ) 2 , 3NaCl+23H 2 0. (Hirsch.) Didymium arsenate, Di 2 H 3 (As0 4 ) 3 . Ppt. Insol. in H 2 O; si. sol. in weak acids. (Marignac, A. ch. (3) 38. 164.) 5Di 2 (AsO 4 ) 2 , As 2 O 6 +3H 2 0. Ppt. Glucinum arsenate, Gl 3 (AsO 4 ) 2 . Insol. in H 2 O; sol. in H 3 As0 4 +Aq. (Ber- zelius.) Glucinum hydrogen arsenate, GlHAs0 4 . Obtained in impure state by heating As 2 O 6 with G1(OH) 2 in a sealed tube at 220. (Bleyer, Z. anorg. 1912, 76. 287.) Glucinum Ze/rahydrogen arsenate, GlH 4 (As0 4 ) 2 . Very hydroscopic. (Bleyer, Z. anorg. 1912, 75. 287.) Glucinum potassium arsenate. KGlAsO 4 , HG1O+5H 2 O. Unstable. Amorphous. Easily hydrolyzed, giving more basic salts. (Bleyer, Z. anorg. 1912, 76. 289.) Glucinum sodium arsenate, NaGlAsO 4 . Unstable. Easily hydrolyzed. (Bleyer, Z. anorg. 1912, 75. 290.) Iron (ferrous) arsenate, Fe 3 (AsO 4 ) 2 + 6H 2 O (?). Ppt. SI. sol. in NH 4 OH+Aq. Insol. in (NH 4 ) 3 As0 4 +Aq or other NH 4 salts+Aq. (Wittstein.) +8H 2 O. Min. Sympksite. Sol. in HC1 + Aq. Iron (ferric) arsenate, basic, 16Fe 2 3 , As 2 O 5 +24H 2 O. Insol. in NH 4 OH+Aq. (Berzelius.) 2Fe 2 O 3 , As 2 O 5 + 12H 2 O. Insol. in NH 4 OH +Aq. 3Fe 2 O 3 , 2As 2 O 5 . 3Fe 2 (AsO 4 ) 2 , Fe 2 O 6 H 6 +12H 2 O. Min. Pharmacosiderite. Easily sol. in acids' decomp. by KOH+Aq. ARSENATE, MAGNESIUM POTASSIUM HYDROGEN 65 Iron (ferric) arsenate, Fe 2 O 3 , As 2 O 6 . Ppt. Insol. in H 2 O. Decomp. by hot H 2 O. Sol. in HC1, H 2 SO 4 and HNO 3 . (Metzke, Z. anorg. 1898, 19. 473.) +4H 2 O. Min. Scorodite. Easily sol. in HCl+Aq; insol. in HNO 3 +Aq. +8H 2 O. Insol. in H 2 O. When freshly pptd., sol. in NH 4 OH+Aq. Sol. in HC1, or HNOs+Aq. Insol. in HC 2 H 3 2 , or NH 4 salts +Aq. (Wittstein.) Sol. in warm H 2 SO 3 +Aq or (NH 4 ) 2 SO 3 + Aq. (Berthier, A. ch. (3) 7. 79.) Iron (ferric) arsenate, acid, Fe 2 O 3 ,3As 2 O 6 + 16.7H 2 O. Ppt.; si. sol. in acids with a yellow color, and in NH 4 OH+Aq with a red color. (Metzke, Z. anorg. 1898, 19. 476.) 2Fe 2 O 3 , 3 As 2 O 5 + 12H 2 O . Insol . in H 2 O or HC 2 H 3 O 2 +Aq. Sol. in mineral acids. Sol. only in cone. H 3 AsO 4 +Aq. Sol. in (NH 4 ) 3 AsO 4 , and other NH 4 salts -f-Aq. (Wittstein.) lol. +22KH 2 0. Ppt. SI. sol. in acids with yellow color, and in NH 4 OH+Aq with a color. (Metzke, Z. anorg. 1898, 19. 475.) Iron (ferroferric) arsenate, 6FeO, 3Fe 2 3 , 4As 2 O 5 +32H 2 O. Insol. in H 2 O. Sol. in HCl+Aq. Decomp. by KOH+Aq. (Wittstein, J. B. 1866. 243.) Iron (ferric) lead arsenate, 5Fe 2 (As0 4 ) 2 , Pb 3 (As0 4 ) 2 . Min. Carmine Spar. Carminite. Sol. in acids; KOH+Aq dissolves out As 2 O 5 . (Sand- berger.) Iron (ferric) potassium arsenate, 2Fe 2 3 , 3K 2 O, 3As 2 O 5 . Not attacked by boiling H 2 0; easily sol. in dil. acids. (Lefevre.) Fe 2 C 3 , K 2 O, 2As 2 O 5 . (Lefevre.) Iron (ferric) sodium arsenate, Fe 2 3 , Na 2 O, 2As 2 5 . (Lefevre.) 2Fe 2 O 3 , 3Na 2 0, 3As 2 5 . (Lefevre.) Lanthanum arsenate, La 2 H 3 (As0 4 ) 3 . (Frerichs and Smith.) Doubtful. (Cleve, B. 11. 910.) Lead arsenate, basic, 15PbO,2As 2 O 6 (?). Ppt. (Stromholm, Z. anorg. 1904, 38. 446.) Lead arsenate, Pb 3 (AsO 4 ) 2 . Insol. in H 2 O, NH 4 OH, or NH 4 salts +Aq. (Wittstein.) Sol. in 2703.5 pts. HC 2 H 3 O 2 +Aq contain- ing 38.94% HC 2 H 3 O 2 . (Bertrand, Monit. Scient. (3) 10. 477.) Sol. in sat. NaCl+Aq. (Becquerel, C. R. 20. 1523.) Not pptd. in presence of Na citrate. (Spiller.) Lead pyroarsenate, Pb 2 As 2 O 7 . Insol. in H 2 O or HC 2 H 8 O 2 +Aq. Sol. in HC1, or HNOs+Aq. (Rose.) Decomp. by cold H 2 0. (Lefevre.) +H 2 O=PbHAsO 4 . Ppt. (Salkowsky, J. pr. 104. 109.) Lead potassium arsenate, PbKAsO 4 . (Lefevre, A. ch. (6) 27. 5.) Lead sodium arsenate, PbNaAsO 4 . (Lefevre.) 4PbO, 2Na 2 O, 3As 2 5 . Superficially de- comp. by cold H 2 O. (Lefevre.) Lead arsenate chloride, 3Pb 3 (AsO 4 ) 2 , PbCl 2 . Sol. in dil. HNO 3 +Aq. (Lechartier.) Min. Mimetite. Sol. in HNO 3 , and KOH+ Aq. Lithium arsenate, Li 3 AsO 4 . Ppt. Sol. in dil. acids and in HC 2 H 3 02+. Aq. (de Schulten, Bull. Soc. (3) 1. 479.) LiH 2 AsC 4 + 3 /2H 2 O. Decomp. by H 2 O into H 3 AsO 4 and Li 3 AsO 4 . (Rammelsberg, Pogg. 128. 311.) Magnesium arsenate, Mg 3 (AsO 4 ) 2 . Ppt. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +7H 2 O, +8H 2 0, +10H 2 0, and +22H 2 0. (Griihl, Dissert. 1897.) +8H 2 O. Min. Hvrnesite. Insol. in H 2 0; easily sol. in acids. Magnesium hydrogen arsenate, MgHAs0 4 . + KH 2 O. Insol. in H 2 O. (de Schulten, C. R. 100. 263.) +5H 2 O. (Schiefer.) +6^H 2 O. Insol. in H 2 O. 1000 pts. boiling H 2 O dissolve 1.5 pts. (Thompson.) Sol. in HNO 3 +Aq before ignition, but insol. in acids after ignition. (Graham, A. 29. 29.) +7H 2 0. Min. Roesslerite. Sol. in HC1+ Aq. Magnesium tefrahydrogen arsenate, MgH 4 (As0 4 ) 2 . Very deliquescent; sol. in H 2 O. (Schiefer.) Magnesium potassium arsenate, MgKAsO 4 . Insol. in, but decomp. by cold H 2 O. (Rose.) Easily sol. in dil. acids. (Lefevre.) +7H 2 O. (Kinkelin, Dissert, 1893.) 4MgO, 2K 2 O, 3As 2 6 . Not attacked by boiling H 2 0; slowly sol. in dil. acids. (Le- fevre.) Magnesium potassium hydrogen arsenate, KMgH(AsO 4 ) 2 +zH 2 O. Decomp. by H 2 0. (Kinkelin, D ssert. 1883.) 66 ARSENATE, MAGNESIUM^POTASSIUM SODIUM Mg 3 KH 2 (AsO 4 ) 3 +5H 2 O. (Chevron and Droixhe, J. B. 1888, 523.) Magnesium potassium sodium arsenate, Mg 2 KNa(As0 4 ) 2 +10H 2 O. (Kinkelin, Dissert. 1883.) Magnesium sodium arsenate, MgNaAsO 4 . Insol. in H 2 0. Very si. sol. in dil. acids. (Lefevre.) 4MgO, 2Na 2 O, 3As 2 6 . (Lefevre.) Magnesium vanadium arsenate, MgH 2 (VO 2 ) 2 (As04) 2 +9H 2 O and MgHAsO 4 , 2(VO 2 )H 2 As0 4 +9H 2 0. See Arseniovanadate, magnesium. Magnesium arsenate chloride, Mg 3 (AsO 4 ) 2 , MgCl 2 . Insol. in H 2 O: sol. in dil. HNO 3 +Aq. (Lechartier, C. R. 65. 172.) Magnesium arsenate fluoride, Mg 3 (As0 4 ) 2 , MgF 2 . Insol. in H 2 O; sol. in dil. HNO 3 +Aq. (Lechartier.) Manganous arsenate, basic, 6MnO, As 2 O 5 -f 3H 2 (?). Min. Chondroarsenite. Easily and com- pletely sol. in dil. HC1, and HNO 3 +Aq. Manganous arsenate, Mn 3 (As0 4 ) 2 +H 2 O. Insol. in H 2 O; si. sol. in acids. (Coloriano, C. R. 103. 273.) 5MnO, 2As 2 O 6 +5H 2 O. Insol. in H 2 0. (Coloriano.) 2MnO, As 2 O 5 . SI. decomp. by cold H 2 O, but rapidly on heating. (Lefevre.) MnHAsO 4 +H 2 O. Decomp. by boiling H 2 O into 5MnO, 2As 2 O 5 +5H 2 O. Sol. in HNO 3 , H 2 SO 4 , or H 3 AsO 4 +Aq. Manganous e/rahydrogen arsenate, MnH 4 (AsO 4 ) 2 . Deliquescent. Easily sol. in H 2 0. (Schiefer.) Manganous potassium arsenate, MnKAs0 4 . (Lefevre, A. ch. (6) 27. 5.) Manganous sodium arsenate, MnNaAsO 4 . Very sol. in dil. acids. (Lefevre.) 2MnO, 4Na 2 O, 3As 2 O 5 . Not attacked by boiling H 2 O; very sol. in dil. acids. (Lefevre.) Manganous arsenate chloride, Mn 3 (AsO 4 ) 2 , MnCl 2 . Insol. in H 2 O; sol. in dil. HNO 3 +Aq. (Lechartier, A. 68. 259.) Manganic arsenate, Mn 2 (As0 4 ) 2 +2H 2 O. Insol. in H 2 O; sol. in acids. Mercurous arsenate, (Hg 2 ) 3 (AsO 4 ) 2 . Insol. in H 2 O; difficultly sol. in acids. (Coloriano, C. R. 103. 273.) Ppt. (Haack, C. C. 1890, II. 736.) Hg 2 (AsO 3 ) 2 . Insol. in H 2 O, HC 2 H 3 O 2 , or alcohol. Decomp. by cold HCl+Aq. SI. sol. in cold HNO 3 -f Aq, from which it is precipi- tated by NH 4 OH as Hg 2 HAsO 4 . (Simon, Pogg. 41. 424.) Mercurous hydrogen arsenate, Hg 2 HAsO 4 . ' Insol. in H 2 0, HC 2 H 3 O 2 , or NH 4 OH+Aq. Decomp. by cold HCl+Aq; sol. in cold HNO 3 +Aq without decomp; very si. sol. without decomp. in NH 4 NO 3 -j-Aq. (Simon, Pogg. 41. Mercuric arsenate, Hg 3 (AsO 4 ) 2 . Ppt. Sol.inH 3 AsO 4 orHNO 3 +Aq. (Berg- man.) Very si. sol. in H 2 O. Easily sol. in HCl+Aq. SI. sol. in HNO 3 +Aq. Insol. in H 3 AsO 4 +Aq. (Haack, C. C. 189P, II. 736.) Mercurous silver arsenate, Hg 2 AgAsO 4 . Sol. in hot cone. HNO 3 . (Jacobsen, Bull. Soc. 1909, (4) 5. 948.) Mercurous arsenate nitrate, Hg 3 AsO 4 , HgNO 3 +H 2 O. Insol. in H 2 or HC 2 H 3 2 ; sol. in HNO 3 + Aq. (Simon, Pogg. 41. 424.) 3Hg 3 As0 4 ,2HgN0 3 ,2Hg 2 0. Ppt. (Haack.) Molybdenum arsenate. Ppt. Nickel arsenate, basic, 5NiO, As 2 O 5 . Min. (Bergemann.) Ni(NiOH)AsO 4 . Difficultly attacked by acids or alkalies. (Coloriano, Bull. Soc. (2) 45. 241.) 5NiO, 2As 2 6 +3H 2 0. As above. Nickel arsenate, Ni 3 (AsO 4 ) 2 . Min. (Bergemann.) +zH 2 O. Insol. in H 2 O. Sol. in H 3 AsO 4 , and cone, mineral acids. Easily sol. in NH 4 OH+Aq. +2H 2 0. Insol. in H 2 0; difficultly sol. in acids. (Coloriano, Bull. Soc. 45. 241.) +8H 2 O. Min. Nickel-bloom, Annabergite. Easily sol. in acids. NiHAsO 4 +H 2 O. Sol.inH 2 O. Difficultly attacked by acids. (Coloriano, C. R. 103. 274.) Nickel potassium arsenate, 12NiO, 3K 2 O, 5As 2 O 5 . (Lefevre.) 2NiO, K 2 O, As 2 O 5 . Rapidly sol. in dil. acids. (Lefevre.) Nickel sodium arsenate, NiNaAsO 4 . Very slowly sol. in dil. acids. (Lefevre.) 4NiO, 2Na 2 O, 3As 2 O 5 . (Lefevre.) Nickel arsenate ammonia, Ni 3 (As0 4 ) 2 ,NH 3 +7H 2 0. Ni 3 (AsO 4 ) 2 ,2NH 3 +6H 2 O. Ni 3 (AsO 4 ) 2 ,3NH 3 +5H 2 O. (Ducru, C. R. 1900, 131. 703.) ARSENATE, SODIUM 67 Palladium arsenate (?). Ppt. Platinum arsenate (?). Ppt, Sol. in HNO 3 +Aq. Potassium arsenate, K 3 AsO 4 . Deliquescent. Very sol. in H 2 O. (Graham, Pogg. 32. 47.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Potassium hydrogen arsenate, K 2 HAs0 4 . Sol. in H 2 O. Potassium efohydrogen arsenate, KH 2 AsO 4 . Sol. in 5.3 pts. H 2 O at 6, forming a solu- tion of sp. gr. 1.1134. Much more sol. in hot H 2 0. Insol. in alcohol. Sol. in 26,666 pts. boiling cone, alcohol. (Wenzel.) Potassium sodium hydrogen arsenate, KNaHAsO 4 + 16H 2 O. Sol. in H 2 0. K 3 Na 3 H 6 (As0 4 ) 4 +9H 2 O. Sol. in H 2 O, and not easily decomp. thereby into its constitu- ents. (Filhol and Senderens, C. R. 95. 343.) Potassium strontium arsenate, KSrAsO 4 . (Lefevre, C. R. 108. 1058.) Potassium vanadium arsenate, K(VO 2 ) 2 As0 4 See Arseniovanadate, potassium. Potassium zinc arsenate, KZnAsO 4 . (Lefevre.) Potassium arsenate sulphate. See Arseniosulphate, potassium. Rhodium arsenate (?). Ppt. Rubidium metaarsenate, RbAsO 3 . Sol. in H 2 O. (Bouchonnet, C. R. 1907, 144. 642.) Rubidium arsenate, Rb 3 As0 4 -f-2H 2 O. Very hydroscopic; sol. in H 2 O to give an alkaline solution. Absorbs C0 2 from the air. (Bouchonnet, I.e.) Rubidium pyroarsenate, Rb 4 As 2 O 7 . (Bouchonnet, I.e.) Rubidium hydrogen arsenate, Rb 2 HAsO 4 + +H 2 0. Absorbs CO 2 from the air. Very hydro- scopic; sol. in H 2 O. Insol. in alcohol. (Bou- chonnet, I.e.) Rubidium (^hydrogen arsenate, RbH 2 AsO 4 . Not hydroscopic. Very sol. in H 2 O; aq. solution is acid to litmus. (Bouchonnet, I.e.) Silver arsenate, Ag 3 AsO 4 . Insol. in H 2 O. Sol. in acids; easily sol. in H 3 AsO 4 +Aq. (Joly, C. R. 103. 1071.) 1 1. H 2 O dissolves 0.0085 g. Ag 3 AsO 4 at 20. (Whitby, Z. anorg. 1910, 67. 108.) Much less sol. in H 3 AsO 4 than Ag 3 PO 4 . (Graham.) Sol. in NH 4 OH+Aq. (Scheele ) Sol. in (NHOzCOs+Aq. Insol. in NH 4 sulphate, nitrate, or succinate+Aq. (Witt- stein.) Very si. sol. in NH 4 NO 3 +Aq, more easily in HC 2 H 3 O 2 +Aq. (Graham.) Sol. in Na 2 S 2 O 3 +Aq, but not so easily as Ag 3 PO 4 . Not pptd. in presence of Na citrate. (Spiller.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Silver hydrogen arsenate, Ag 2 HAsO 4 . Decomp. by H 2 O, with formation of Ag 3 AsO 4 . (Setterberg, Berz. J. B. 26. 208.) AgH 2 AsO 4 . Decomp. by H 2 O. (Joly, C. R. 103. 1071.) *Ag 2 O, 2As 2 O 5 . Decomp. by H 2 O. Rather si. sol. in HNO 3 +Aq. Very easily sol. in NH 4 OH+Aq. (Hurtzig and Geuther, A. 111. 168.) Silver arsenate ammonia, Ag 3 AsO 4 , 4NH 3 . Easily sol. in H 2 O. (Widmann, Bull. Soc. (2) 20. 64.) Silver arsenate sulphate, 3Ag 2 O, As 2 O 6 , SO 3 . Decomp. by H 2 O, with separation of Ag 3 As0 4 ; decomp. by dil. H 2 SO 4 +Aq. (Set- terberg, Berz. J. B. 26. 209.) Sodium arsenate, Na 3 AsO 4 +'12H 2 O. Permanent in dry air. Sol. in 3.57 pts. H 2 O at 15.5. (Graham.) 100 pts. H 2 O at 15.5 dissolve 28 pts. Na 3 AsO 4 + 12H 2 O. (Ber- zelius.) Sol. in 3.75 pts. H 2 O at 17; or 100 pts. H 2 O at 17 dissolve 26.7 pts.; or sat. Na 3 AsO 4 +Aq at 17 contains 21.1% Na 3 AsO 4 + 12H 2 O or 10.4% Na 3 AsO 4 , and has sp. gr. 1.1186. (Schiff, A. 113. 350.) Melts in crystal H 2 O at 85.5. Sp. gr. of Na 3 As0 4 +Aq at 17. 7o %Na 3 AsO 4 +12H 2 O. % Sp. gr.. % Sp. gr. % Sp. gr. 1 2 3 4 5 6 7 1.0053 1.0107 1.0161 1.0215 1.0270 1.0325 1 . 0380 9 10 11 12 13 14 15 1.0490 1.0547 1.0603 1.0659 1.0716 1.0773 1 . 0830 17 18 19 20 21 22 1.0945 1 . 1003 1.1061 1.1121 1.1179 1.1238 8 1.0435 16 1.0887 (Schiff, calculated by Gerlach, Z. anal. 8. 286.) "Arseniate of soda" dissolves in 60 pts. boiling alcohol. (Wenzel.) +4>^H 2 O. (Hall, Chem. Soc. 61. 93.) -f-10H 2 O. Efflorescent. (Hall.) 68 ARSENATE, SODIUM HYDROGEN Sodium hydrogen arsenate, Na 2 HAsO 4 - 7H 2 O. Not efflorescent. (Schiff.) Solubility in Pb(NO 3 ) 2 +Aq. A table given which records the g. of As 2 O 5 in 100 c of the nitrate. (Curry, J. Am. Chem. Soc 1915, 37. 1685.) +7^H 2 O. (Lescoeur, C. R. 104. 1171.) +12H 2 O. Efflorescent. Sol. in H 2 O; so in 1.79 pts. H 2 O at 14; or 100 pts. H 2 O a 14 dissolve 56 pts. Na 2 HAsO 4 +12H 2 O. Sat Na 2 HAsO 4 +Aq contains 35.9% Na 2 HAsO 4 + 12H 2 O, or 16.5% Na 2 HAsO 4 , and has sp. gr. = 1.1722. (Schiff, A. 113. 350.) 100 pts. H 2 O at 7.2 dissolve 22.268 pts. (Thomp son.) 100 pts. H 2 O dissolve 17.2 pts. Na 2 HAsO 4 + 12H 2 O at 0, and 140.7 pts. at 30. (Tilden Chem. Soc. 45. 409.) Melts in crystal H 2 O at 28. (Tilden.) Sp. gr. of Na 2 HAsO 4 +Aq at 14. % = %Na 2 HAsO 4 +12H 2 O. % Sp. gr. % Sp. gr. % Sp. gr. 1 1.0042 15 1.0665 29 1.1358 2 1.0084 16 1 . 0712 30 1.1410 3 1.0126 17 1 . 0759 31 1 . 1463 4 1.0168 18 1.0807 32 1.1516 5 1.0212 19 1.0855 33 1.1569 6 1.0256 20 1.0904 34 1 . 1623 7 1.0300 21 1 . 0953 35 1.1677 8 1.0344 22 1 . 1003 36 1.1731 9 1.0389 23 1 . 1052 37 1 . 1786 10 1.0434 24 1.1103 38 1.1841 11 1 . 0479 25 1.1153 39 1 . 1896 12 1.0525 26 1 . 1204 40 1 . 1952 13 1.0571 27 1.1255 14 1.0618 28 1.1306 (Schiff, calculated by Gerlach, Z. anal. 8. 280.) Insol. in alcohol. + 133^H 2 O. (Setterberg.) Sodium cfoliydrogen arsenate, NaH 2 AsO 4 + H 2 O. More sol. in H 2 O than Na 3 AsO 4 or Na 2 HAsO 4 . (Schiff.) +2H 2 O. Efflorescent. (Jolv and Duffet, C. R. 102. 1391.) Sodium frihydrogen diarsenate, Na 3 H 3 (AsO 4 ) 2 +3H 2 O. Sol. in H 2 0. (Filhol and Senderens, C. R. 95. 343.) Sodium strontium arsenate, NaSrAsO 4 . Not attacked by boiling H 2 O. (Lefevre.) +9H 2 O. Scarcely sol. in H 2 O. (Joly,C.R. 104. 905.) + 18H 2 O. (Joly.) Sodium uranyl arsenate, Na(U0 2 )As0 4 . Ppt. (Werther, A. 68. 312.) Sodium zinc arsenate, NaZnAsO 4 . Slowly sol. in dil. acids. (Lefevre.) Na 2 ZnAs 2 O 7 . As above. (Lefevre.) Sodium arsenate fluoride, Na 3 AsO 4 , NaF + 12H 2 O. Sol. in 9.5 pts. H 2 O at 25, and 2 pts. at 75. (Briegleb, A. 97. 95.) Sodium arsenate stannate, 6Na 2 O, 2As.>O 5 , SnO 2 +50H 2 O. More difficultly sol. than sodium stannate. (Haeffely, Phil. Mag. (4) 10. 290.) 5Na 3 AsO 4 , Na 2 SnO 3 +60H 2 O. (Prandtl, B. 1907, 40. 2133.) Sodium arsenate sulphate, Na 8 As 6 Oi 9 , 2Na 2 SO 4 . Sol. in H 2 O. (Mitscherlich.) Na 4 As 2 O 7 , Na 2 SO 4 . (Setterberg.) Sodium arsenate tungstate, Na 4 As 2 O 7 , Na 2 W 3 O 10 +20H 2 O. See Arseniotungstate, sodium. Strontium arsenate, Sr 3 (As0 4 ) 2 . Not attacked by boiling H 2 O; easilv sol. in dil. acids. (Lefevre, A. ch. (6) 27. 5.) Strontium pyroarsenate, Sr 2 As 2 7 . Decomp. by cold H 2 O into SrHAsO 4 -f- H 2 O. (Lefevre.) Strontium hydrogen arsenate, SrHAsO 4 4- Insol. in cold, but decomp. by hot H 2 O into a basic, and a sol. acid salt. 100 pts. H 2 O at 15.5 dissolve 0.284 pt. (Thompson, 1831.) Sol. in HC 2 H 3 O 2 , and very easily in HC1-+- q. (Kotschoubey, J. pr. 49. 182.) Sol. in HNO 3 +Aq. SrH 4 (AsO 4 ) 2 +2H 2 O. Partly sol. in H 2 O. Hermann, Dissert. 1879.) Strontium vanadium arsenate, SrHAs0 4 , 2(V0 2 )H 2 As0 4 +7^H 2 0. See Arseniovanadate, strontium. Strontium arsenate chloride, 3Sr 3 (AsO 4 ) 2 , SrCl 2 . Insol. in H 2 0; easily sol. in dil. HNO 3 +Aq. Lechartier, C. R. 65. 172.) Thallous arsenate, Tl 3 AsO 4 . Sol. inH 2 O. (Willm, A. ch. (4) 5. 5.) Thallous hydrogen arsenate, Tl 2 HAsO 4 . Very easily sol. in H 2 O. (Willm.) hallous dihydrogen arsenate, TlH 2 AsO 4 . Easily sol. in H 2 O. (Willm.) hallic arsenate, TlAsO 4 -f 2H 2 O. v/wr 1 ^ Sol< in HC1 + A q; decomp. y NH 4 OH, or KOH+Aq. (Willm.) ARSENIMIDE 69 Thorium hydrogen arsenate, Th(HAs0 4 ) 2 + 6H 2 O. Insol. in H 2 O or H 3 AsO 4 +Aq. (Berzelius.) Ppt.; insol. in H 2 O. (Barbieri, C. A. 1911. 3385.) Th(H 2 As0 4 ) 4 +4H 2 O. Decomp. by H 2 O. (Barbieri, I. c.) Tin (stannous) arsenate, Insol. in H 2 O. (Lenssen, A. 114. 113.) Tin (stannic) arsenate, 2SnO 2 , As 2 O 5 . Ppt. Insol. in H->O and dil. HNO 3 +Aq. (Haeffely, Phil. Mag. (4) 10. 290.) Sn 3 (AsO 4 )4+6H 2 O. Insol. in H 2 O; sol. in cone. HCl+Aq, and in aqua regia; insol. in HN0 3 + Aq or H 2 SO 4 . (Williams, Proc. Soc. Manchester, 15. 67.) Colloidal.. Very slowly sol. in H 2 O, from which it is pptd. by HC1, HNO 3 , or H 2 SO 4 + Aq; also by BaCl 2 , CaCl 2 , NH 4 C1, and FeCl 3 + Aq, and by AgNO 3 , or KI + Aq. Not pptd. by alcohol, HC 2 H 3 O 2 , HgCL, Na 2 CO 3 , K 2 CO 3 , or (NH 4 ) 2 CO 3 +Aq. The pptd. jelly is read- ily sol. in cone, acids, and KOH, or NaOH + Aq. (Williams, I.e.) Tin (stannous) arsenate chloride, Sn 3 (AsO 4 ) 2 , SnCl 2 +2H 2 0. Decomp. on air. (Lenssen, A. 114. 113.) Titanium arsenate (?). Insol. in H 2 O. Sol. in titanic acid, arsenic acid, or HCl+Aq. Sol. in Ti salts +Aq. (Rose.) Titanyl arsenate, 5TiO 2 , 2As 2 O 5 . Sol. in acids without decomp. Scarcely attacked by KOH or by NH 4 OH+Aq. (Reichard, B. 1894, 27. 1026.) Uranous arsenate, U 3 (AsO 4 ) 2 . Ppt. Uranous hydrogen arsenate, UH 2 (AsO 4 ) 2 + 3H 2 O. Ppt. Sol. in HCl+Aq. Uranyl arsenate, (UO 2 )HAsO 4 +4H 2 O. Insol. in H 2 O, HC 2 H 3 Q 2 , and saline solu- tions, as NH 4 Cl+Aq; sol. in the mineral acids; sol. in K 2 CO 3 +Aq. (Werther, A. 68. 313.) (UO 2 )H 4 (AsO 4 ) 2 +3H 2 O. (Werther.) (UO 2 )oAs 2 O 7 . Insol. in H 2 O; sol. in acids. (UO 2 ) 3 (AsO 4 ) 2 + 12H 2 O. Min. Trosgerite. Vanadium dihydrogen arsenate, (VO 2 )H 2 AsO 4 +4H 2 O. Easily sol. in H 2 0. (Friedheim, B. 23. 2600.) See Arseniovanadic acid. Vanadium zinc arsenate, (VO 2 ) 2 ZnH 2 (AsO 4 ) 2 2 O, and2(VO 2 )H 2 AsO 4 +6^H 2 O. See Arseniovanadate, zinc. Vanadyl arsenate, (VO) 2 HAsO 4 +H 2 O. Very slowly sol. in H 2 O; insol. in alcohol; easily sol. in HCl+Aq. (Berzelius.) Composition given by Friedheim (B. 23. 2600). Yttrium arsenate, YtHAs0 4 . Ppt. Insol. in acetic, easily sol. in mineral acids. Zinc arsenate, basic, 4ZnO, As 2 O5+H 2 O. (Friedel, J. B. 1866. 949.) Min. Adamite. Easily sol. in dil. HCl+Aq, and is attacked by HC 2 H 3 C>2. Zinc arsenate, Zn 3 (AsO 4 ) 2 . (deSchulten, Bull Soc. (3) 2. 300.) +3H 2 O. Ppt. Sol. in HNO 3 , and H 3 AsO 4 +Aq. (Kottig, J. pr. 48. 182.) +8H 2 O. Min. Kottigile. Zinc arsenate, acid, Zn 5 H 2 (AsO 4 ) 4 . Easily sol. in cold HCl+Aq, less easily in cold HNO 3 . Sol. in KOH, or NaOH+Aq (Gorguel, Dissert, 1894.) +3H 2 O. Insol. in H 2 O; sol. in H 3 As0 4 , or HNO 3 +Aq. (Mitscherlich.) +5H 2 O. Sol. in dil. HCl+Aq. (Demel, B. 12. 1279.) Could not be obtained, (Coloriano, Bull. Soc. (2) 45. 709.) 2ZnO, As 2 O 5 . Very slowly decomp. by cold, rapidly by boiling H 2 O. (Lef6vre.) ZnHAsO 4 +H 2 O. Insol. in H 2 O. (Debray, Bull. Soc. (2) 2. 14.) Decomp. by hot H 2 O into 4ZnO, As 2 O 5 + H 2 O. (Coloriano, C. R. 103. 273.) Zn(ZnOH) 2 As 2 O 7 +7H 2 O (Gorgeul.) Zinc arsenate ammonia, Zn 3 (AsO 4 ) 2 , 2NH 3 + 3H 2 0. Insol. in H 2 O; sol. in acids, NH 4 OH, or KOH+Aq. (Bette, A. 16. 141.) Zirconium arsenate, 2ZrO 2 , As 2 O 5 + 5 /2H 2 O = (ZrO)HAsO 4 +MH 2 O. Ppt. Insol. in HoO or HCl+Aq. (Paykull, B. 6. 1467.) Perarsenic acid. See Perarsenic acid. Arsenicotungstic Acid. Ammonium vanadium arsenicotungstate. See Arsenicovanadicotungstate, ammonium. Arsenicovanadicotungstic acid. Ammonium arsenicovanadicotungstate, 16(NH 4 )oO, 5As 2 O 3 , 15V 2 O 3 , 26WO 3 + 101H 2 O. SI. sol. in cold, readily sol. in hot H 2 O. (Rogers, J. Am. Chem. Soc. 1903, 26. 308.) Arsenimide, As 2 (NH) 3 . Decomp. by H,,O. (Hugot, C. R. 1904, 139. 56.) 70 ARSENIOARSENIC ACID Arsenioarsenic acid, 3As 2 O 3 , 2As 2 O 5 + 3H 2 O. Decomp. by H 2 O. (Joly, C. R. 100. 1221.) 3As 2 O 3 , As 2 O 8 +H 2 O. Decomp. by H 2 O. (Joly.) As 2 O 3 , As 2 O 5 +H 2 O. Decomp. by H 2 O. (Joly.) See also Arsenic dioxide pentoxide. Arseniochromic acid. Ammonium arseniochromate, 2(NH 4 ) 2 O, As 2 O 6 , 4CrO 3 +H 2 O. Insol. in H 2 O. (Friedheim and Mozkin, Z. anorg. 1894, 6. 280.) 3(NH 4 ) 2 O, As 2 O 5 , 8CrO 3 . Decomp. by recryst. from H 2 O. (Friedheim and Mozkin, Z. anorg. 1894, 6. 281.) Potassium arseniochromate, 2K 2 O, As 2 O5, 4CrO 3 . Decomp. by recryst. from H 2 O. (Friedheim and Mozkin, Z. anorg. 1894, 6. 275.) 2K 2 O, As 2 O 6 , 4Cr0 3 +H 2 O. Decomp. by recryst. from H 2 O. (Friedheim and Moz- kin, I. c.) Arseniomolybdic acid, As 2 6 , 6MoO 3 + 10H 2 O. By recryst. from H 2 O the comp. with 18H 2 O is formed. (Pufahl, Dissert. 1888.) + 16H 2 O. Sol. in H 2 O. (Debray.) + 18H 2 O. Completely sol. in H 2 O. Sp.gr. of sat. solution at 18.8 is 2.21. Easily sol. in abs. alcohol. Insol. in CS 2 , liq. hydrocarbons and CHC1 3 . (Pufahl, I.e.) As 2 O 5 , 7MoO 3 +14H 2 O. (Seyberth, B. 7. 391.) As 2 O. 6 , 18MoO 3 +28H 2 O. Very sol. in H 2 O. Sp. gr. of sat. solution at 18.3 = 2.45 and 1 cc. contains 2.16 g. acid. Easily sol. in absolute alcohol; insol. in CS 2 , liquid hydrocarbons and CHC1 3 . (Pufahl, I.e.) Sol. in ether with subsequent separation into two layers. See Phosphotungstic acid. (Drechsel, B. 20. 1452.) +38H 2 O. Efflorescent. When recryst. comp. with 28HoO is formed. (Pufahl, I.e.) As 2 O 5 , 20MoO 3 +27H 2 O. SI. sol. in HNO 3 +Aq. (Debray, C. R. 78. 1408.) Ammonium arseniomolybdate, (NH 4 ) 2 O, As 2 O 5 , 2MoO 3 +3H 2 O. (Friedheim, Z. anorg. 1894, 6. 28.) +4H 2 O. (Friedheim, I.e.) (NH 4 ) 2 O, As 2 O 5 , 6MoO 3 +2H 2 O. SI. sol. in cold H 2 O; sol. in acids. (Debray.) +4H 2 O. SI. sol. in cold, very easily sol. in hotH 2 O. (Pufahl, I.e.) 2(NH 4 ) 2 O, As 2 O 5 , 6MoO 3 +6H 2 O. SI. sol. in H 2 O. Cannot be recryst. therefrom. (Pufahl.) + 12H 2 O. (Friedheim, Z. anorg. 1894, 6. 31.) 3(NH 4 ) 2 O, As 2 O 5 , 6MoO 3 +4H 2 O. (Fried- heim, I.e.) +8H 2 O. (Friedheim, I.e.) (NH 4 ) 2 O, 2H 2 O, 7MoO 3 , As 2 O 5 +4H 2 O. Sol. in hot H 2 O. (Seyberth, B. 7. 391.) Not obtained. (Pufahl.) 7fNH 4 ) 2 O, 2As 2 O 6 , 14MoO 3 +28H 2 O. (Friedheim, I.e.) 5(NH 4 ) 2 O, As 2 O 6 , 16Mo0 3 +5H 2 0. (Fried- heim, Z. anorg. 1894, 6. 31.) 5(NH 4 ) 2 O, As 2 O 5 , 16MoO 3 +9H 2 O. Nearly insol. in cold, sol. in boiling H 2 O. Easily sol. in NH 4 OH+Aq. (Gibbs, Am. Ch. J. 3. 402.) + 12H 2 O. (Pufahl, I.e.) 2(NH 4 ) 2 0, As 2 6 , 18Mo0 3 +17H 2 0. (Pufahl, I.e.) 3(NH 4 ) 2 O,As 2 O 5 ,18MoO 3 +14H 2 0. Very sol. in H 2 and alcohol. (Kehrmann, Z. anorg. 1894, 7. 421.) 3(NH 4 ) 2 O, As 2 O 5 , 20MoO 3 . Easily sol. in H 2 O. (Debray, C. R. 78. 1408.) 3(NH 4 ) 2 O, As 2 O 5 , 24MoO 3 +12H 2 O. De- composed by H 2 O, especially when boiling. Easily sol. in NH 4 OH+Aq, less easily sol. in warm H 2 SO 4 and boiling H 3 AsO 4 +Aq. SI. sol. in molybdic acid+Aq, HNO 3 , and cone. NH 4 NO 3 +Aq. (Pufahl, I.e.) Barium arseniomolybdate, BaO, As 2 O 5 , 6MoO 3 + 10H 2 O. SI. sol. in H 2 O. Partially decomp. by boil- ing. (Pufahl, I.e.) 3BaO, As 2 O 5 , 6MoO 3 . SI. sol. in H 2 O. (Pufahl, I.e.) 3BaO, As 2 O 5 , 7MoO 3 . Ppt. (Seyberth.) 3BaO, As 2 O 5 , 18MoO 3 . Decomp. by H 2 O. (Pufahl, I.e.} Cadmium arseniomolybdate, CdO, 2H 2 O, As 2 O 5 , 6MoO 3 +llH 2 O. (Pufahl.) 3CdO, 3H 2 0, As 2 6 , 18Mo0 3 +33H 2 O. (Pufahl.) Caesium arseniomolybdate, Cs 2 O, As 2 O 5 , 6MoO 3 . SI. sol. in H 2 O. (Pufahl, I.e.) 4Cs 2 O, As 2 O 5 , 26MoO 3 + 15H 2 O. Ppt. (Ephraim, Z. anorg. 1910, 65. 246.) Calcium arseniomolybdate, CaO, As 2 O 5 , 6Mo0 3 + 10H 2 0. Rather difficultly sol. in cold H 2 O. (Pufahl, I.e.) 3CaO, As 2 O 5 , 6MoO 3 . As Ba salt. (Pu- fahl, l.c.) 3CaO, As 2 O 5 , 18MoO 3 +32H 2 O. Very sol. in H 2 O. Solution sat. at 18 has sp. gr = 2.163. (Pufahl, I.e.) Cobalt arseniomolybdate, CoO, 2H 2 0, As 2 O 5 , 6MoO 3 + llH 2 O. (Pufahl.) 3CoO, 3H 2 O, As 2 O 5 , 18MoO 3 +33H 2 O. (Pufahl.) Cupric arseniomolybdate, CuO, 2H 2 O, As 2 O 5 , 6MoO 3 + 15H 2 O. (Pufahl.) 3CuO, 3H 2 0, As 2 5 , 18MoO 3 +34H 2 O. (Pufahl.) ARSENIOSULPHATE, POTASSIUM 71 Lithium arseniomolybdate, Li 2 O, As 2 O 5 6MoO 3 +14H 2 O. Very sol. in H 2 O. (Pufahl, I.e.) 3Li 2 O, As 2 5 , 18MoO 3 +34H 2 O. Solution sat. at 15 has sp. gr. of 2.481. (Pufahl, I.e. Magnesium arseniomolybdate, MgO, As 2 O 5 6Mo0 3 + 13H 2 0. Very sol. in H 2 O. (Pufahl, I.e.) 3MgO, As 2 O 5 , 18MoO 3 +36H 2 O. Sol. ir H 2 O. (Pufahl, I.e.) Manganese arseniomolybdate, MnO, 2H 2 As 2 O 5 , 6MoO 3 + llH 2 O. (Pufahl.) 3MnO, 3H 2 O, As 2 O 5 , 18MoO 3 +33H 2 (Pufahl.) Nickel arseniomolybdate, NiO, 2H 2 O, As 2 O 5 6Mo0 3 + llH 2 0. (Pufahl.) 3NiO, 3H 2 O, As 2 O 5 , 18Mo0 3 +34H 2 O (Pufahl.) Potassium arseniomolybdate, K 2 O, As 2 O 6 . 2MoO 3 +5H 2 O. Sol. in H 2 O. (Friedheim, Z. anorg. 2. 314.) K 2 O, As 2 O 5 , 6MoO 3 +5H 2 O. Sol. in hot H 2 O without decomp. (Friedheim, Z. anorg 1892, 2. 330.) K 2 O, As 2 O 5 , 18MoO 3 +25H 2 O. Easily sol in cold H 2 O. Decomp. on dilution. (Pufahl, I.e.) 3K 2 O, As 2 O 5 , 18MoO 8 +26H 2 O. Easily sol. in H 2 O. (Pufahl, I.e.) 3K 2 0, As 2 O 5 , 20MoO 3 . Insol. in H 2 O. (Debray, C. R. 78. 1408.) 3K 2 0, As 2 O 5 , 24MoO 3 +12H 2 0. Somewhat sol. in H 2 acidified with HNO 3 . (Pufahl, I.e.) Rubidium arseniomolybdate, 3Rb 2 O, 3As 2 O 5 , 5MoO 3 +9H 2 O. Easily sol. in H 2 O. (Ephraim, Z. anorg. 1910, 65. 241.) Rb 2 O, As 2 O 5 , 6MoO 3 . SI. sol. in H 2 0. (Pufahl, I.e.) 4Rb 2 O, As 2 6 , 18MoO 3 +40H 2 O. Pptd. (Ephraim, Z. anorg. 1910, 65. 241-4.) Silver arseniomolybdate, 3Ag 2 O, As 2 O 5 , 6MoO 3 +zH 2 O. (Pufahl, Leipzig, 1888.) 6Ag 2 O, As 2 O 5 , 18MoO 3 +22H 2 O. SI. sol. in H 2 O. Very sol. in NH 4 OH and in dil. HNO 8 . (Pufahl, I.e.) 7Ag 2 O, 2As 2 O 5 , 36MoO 3 +30H 2 O. SI. sol. in cold, easily sol. in hot H 2 O strongly acidi- fied with HNO 3 . (Pufahl, I.e.) Sodium arseniomolybdate, Na 2 O, As 2 O 5 , 2MoO 3 +8H 2 O. (Friedheim, Z. anorg. 1892, 2. 357.) Na 2 O, As 2 O 5 , 6Mo0 3 +12H 2 O. Very sol. in H 2 0. Solution sat. at 19.8 has sp. gr. = 1.678. (Friedheim, I.e.) 3Na 2 O, As 2 O 5 , 6MoO 3 +llH 2 O, + 12H 2 O, and +13H 2 0. SI. sol. in cold H 2 O. (Pufahl, 3Na 2 O, As 2 O 6 , 18MoO 3 +24H 2 0. Easily sol. in H 2 O. (Pufahl, I.e.) +30H 2 O. SI. sol. in cold H 2 0. (Pufahl, Strontium arseniomolybdate, SrO, As 2 6 , 6Mo0 3 +10H 2 O. " As Ba salt. (Pufahl, I.e.) 3SrO, As 2 O 6 , 6MoO 3 . As Ba salt. (Pu- fahl, I.e.) 3SrO, As 2 O 5 , 18MoO 3 +32H 2 O. Very sol. in H 2 0. (Pufahl, l.c.) Thallium arseniomolybdate, 6T1 2 O, As 2 O 5 . 18Mo0 3 +zH 2 0. Ppt. (Pufahl.) 3T1 2 O, 3H 2 O, As 2 O 5 , 18MoO 3 +3H 2 O. Ppt. (Pufahl.) Zinc arseniomolybdate, ZnO, 2H 2 O, As 2 6 , 6Mo0 3 +llH 2 0. (Pufahl.) 3ZnO, As 2 O 5 , 18MoO 3 +37H 2 0. Very sol. inH 2 O. (Pufahl.) Arseniophosphovanadicotungstic acid. Ammonium arseniophosphovanadicotung- state, 88(NH 4 ) 2 O, 2.As 2 O 6 , 12P 2 O 6 , 69V 2 O 3 , 148WO 3 +484H 2 O. Sol. in H 2 O. Insol. in alcohol and ether. (Rogers, J. Am. Chem. Soc. 1903, 25. 313.) Arseniophosphovanadicovanadiotungstic acid. Ammonium arseniophosphovanadicovanadio- tungstate, 99(NH 4 ) 2 O, 2As 2 O 5 , 12P 2 O 6 , 6V 2 O 3 , 66V 2 O 5 , 191WO 3 +522H 2 O. SI. sol. in cold H 2 O. (Rogers, J. Am. Chem. Soc. 1903, 25. 314.) Arseniophosphovanadiotungstic acid. Ammonium arseniophosphovanadiotungstate, 82(NH 4 ) 2 O, 3As 2 O 6 , 12P 2 6 , 52V 2 O 6 , 201WO 3 +567H 2 O. Very sol. in warm H 2 O. Insol. in organic solvents. (Rogers, J. Am. Chem. Soc. 1903, 25. 312.) Arseniosulphuric acid. Ammonium arseniosulphate, 2(NH 4 ) 2 O, As 2 O 5 , 2SO 3 +3H 2 0. Can be recryst. from H 2 O. (Friedheim and VIozkin, Z. anorg. 1894, 6. 290.) Potassium arseniosulphate, 2K 2 O, As 2 O fi , 2SO 3 +3H 2 O. (Friedheim and Mozkin, Z. anorg. 1894, 6 89.) 5K 2 O, As 2 O 5 , SSO 3 +6H 2 O. (Friedheim nd Mozkin, Z. anorg. 1894, 6. 291.) 72 ARSENIOSULPHATE, SODIUM Sodium arseniosulphate, 2Na 2 O, As 2 O 6 , 2SO 3 +3H 2 O. (Friedheim and Mozkin, Z. anorg. 1894, 6. 290.) Arseniotelluric acid. Ammonium arseniotellurate, 2(NH 4 ) 2 O, As 2 O 6 , TeO 3 +4H 2 O. Sol. in H 2 O. (Weinland, Z. anorg. 1901, 28. 65.) 4(NH 4 ) 2 O, 3As 2 O 5 , 2TeO 3 + HH 2 O. Sol. inH 2 O. (Weinland.) Sodium arseniotellurate, 2Na 2 O, As 2 O 5 , 2TeO 3 -f9H 2 O. Ppt. (Weinland, I.e.) Arseniotungstic acid, 3H 2 O, As 2 O 6 , 16WO 3 +32H 2 O = H 3 AsW 8 O 28 +16H 2 O (o-an- hydroarsenioluteotungstic acid) . Sol. in H 2 O. (Kehrmann, A. 246. 45.) 3H 2 O, As 2 O 5 , 19WO 3 (?). Sp. gr. of sat. solution in H 2 O is 3.279. (Fremery, B. 17. 296.) Is a mixture containing principally H 8 AsW 8 O 28 + 16H 2 O. (Kehrmann.) As 2 O 6 , 18WO 3 +zH 2 O. Sol. in H 2 O. (Kehrmann, Z. anorg. 1899, 22. 292.) Aluminum ammonium arseniotungstate. See Aluminicoarseniotungstate, ammo- nium. Ammonium arseniotungstate, 4(NH 4 ) 2 O, 2H 2 O, As 2 O 5 , 6WO 3 +3H 2 0. SI. sol. in cold H 2 O or HNO 3 +Aq; easily sol. in boiling H 2 O. (Gibbs, Proc. Am. Acad. 16. 135.) 7(NH 4 ) 2 0, A S ;0 6 , 14W0 3 ,+lftl 2 0. Very si. sol. even in boiling H 2 O. (Fremery, I. c.) 3(NH 4 ) 2 O, As 2 O 5 , 16WO 3 +16H 2 O = (NH 4 ) 3 AsWV) 28 +8H 2 O. Sol. in H 2 O. (Kehrmann.) 5(NH 4 ) 2 O, As 2 O 6 , 17WO 3 +8H 2 O. Can be recryst. from H 2 O without decomp. Decomp. by long boiling with H 2 O. (Kehrmann, Z. anorg. 1899, 22. 294.) 3(NH 4 ) 2 O, As 2 O 5 , 18WO 3 + 14, or 18H 2 O. Very sol. in cold H 2 O. Can be recryst. from H 2 0. (Kehrmann, I.e.) 3(NH 4 ) 2 O, As 2 O 5 , 21W0 3 +zH 2 O. Easily sol. in H 2 O. Easily decomp. on recryst. (Kehrmann, I.e.) 3(NH 4 ) 2 O, As 2 O 5 , 24WO 3 +12H 2 O. More sol. in H 2 O than corresponding phosphotung- state. (Kehrmann, I.e.) Barium arseniotungstate, 2BaO, As 2 O 5 , 16WO 3 -f-zH 2 O. Sol. in H 2 0. (Pechard, A. ch. (6) 22. 262.) 7BaO, As 2 O 6 , 22WO 3 +54H 2 O. Sol. in H 2 O. Can be recryst. therefrom. (Kehr- mann, I.e.) Potassium arseniotungstate, 3K 2 O, 3H 2 O, Aso0 5 , 6WO 3 . Insol. in H 2 O. Readily sol. in alkali hy- droxides +Aq. (Gibbs.) 3K 2 O, As 2 O 5 , 16WO 3 + 16H 2 O = K 3 AsW 8 O 28 +8H 2 O. Sol. in H 2 O. (Kehrmann.) 5K 2 O, As 2 O 5 , 17WO 3 +22H 2 O. Scarcely sol. in cold H 2 O. (Kehrmann, Z. anorg. 1899, 22. 295.) 3K 2 O, As 2 O 6 , 18WO 3 + 14H 2 O. Efflorescent. (Kehrmann, I.e.) 3K 2 O, As 2 5 , 19WO 3 + 16H 2 O (?). Sol. in H 2 0. (Fremery.) Silver arseniotungstate, Ag 5 AsW 8 O 29 . Insol. in H 2 O (Kehrmann, A. 245. 55) ; per- haps identical with 6Ag 2 O, As 2 O 5 , 16WO 3 + 11H 2 O. Insol. in H 2 O. (Gibbs.) Sodium arseniotungstate, 3Na 2 O, As 2 O 6 , 3WO 3 +20H 2 O. Very sol. in H 2 O. (Lefort, C. R. 92. 1461.) Arsenious acid, HAsO 2 . Solubility of HAsO 2 in amyl alcohol +Aq. at 25. a w =mol. of HAs0 2 in 1 1. of H 2 O. aa =mol. of HAsO 2 in 1 1. of amyl alcohol, h = partition coefficient. aw a a h 0.0449 0.0446 0.0887 0.0892 0.1800 0.0082 0.0083 0.0164 0.0161 0.0324 5.48 5.38 5 41 5.53 5.55 (Auerbach, Z. anorg. 1903, 37. 356.) Solubility of HAs0 2 in sat. H 3 BO 3 +Aq and amyl alcohol. a w =mol. of HAsO 2 in 1 1. of H 2 0. a a =mol. of HAsO 2 in 1 1. of amyl alcohol. h= partition coefficient. a w a a h 0.0859 0.1720 0.0161 0.0321 5.33 5.35 (Auerbach, I.e.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) See Arsenic inoxide. Arsenites. All arsenites, except those of the alkali metals, are partially or wholly insol. in H 2 O, but easily sol. in acids; several are sol. in (NH 4 ) 2 S0 4 , NH 4 N0 3 , or NH 4 Cl+Aq. All basic arsenites are sol. in acids except those that give an insol. salt with the bases. Many are sol. in excess of As 2 O 3 +Aq. ARSENITE, BASIC, COBALTOUS 73 Aluminum arsenite, A1 2 O 3 , As 2 O 3 . SI. sol. in boiling H 2 O. Easily sol. in NaOH +Aq and in acids. (Reichard, B. 1894, 27. 1029.) Aluminum arsenite iodide, Alls, 6As 2 O 3 + 16H 2 O. (Griihl, Dissert. 1897.) Ammonium arsenite, NH 4 AsO 2 . Very sol. in H 2 O. (Luynes, J. pr. 72. 180.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014); (Naumann, B. 1904, 37. 4328.) (NH 4 ) 3 AsO 3 (?). Sol. in HoO. (Staven- hagen, J. pr. 1895, (2) 51. 11.) , (NH 4 ) 4 As 2 O 5 . Very sol. in H 2 O. Insol. in alcohol or ether. (Stein, A. 74. 218.) Could not be obtained. (Stavenhagen.) Ammonium arsenite bromide, 2As 2 O 3 , NH 4 Br. SI. sol. in H 2 O. (Riidorff, B. 19. 2679.) Ammonium arsenite chloride, As 2 O 3 , NH 4 C1. SI. sol. in H 2 O. Sol. in warm dil. NH 4 OH +Aq. (Rudorff.) Ammonium arsenite iodide, 2As 2 O 3 , NH 4 I. SI. sol. in boiling H 2 O. Sol. in warm dil. NH 4 OH+Aq. (Rudorff.) . Antimony arsenite (?). Ppt. Sol. in a small amount H 2 O, but insol. in a large quantity. (Berzelius.) Completely sol . in KOH + Aq. (Reynolds.) Barium arsenite, Ba(AsO 2 )2. Easily sol. in H 2 O when recently pptd., but insol. after being dried. Pptd. from aqueous solution by boiling. (Filhol, A. 68. 308.) Only si. sol. in H 2 O. (Stavenhagen, J. pr. 1895, (2) 51. 18.) Ba 3 (AsO 3 ) 2 . SI. sol. in cold H 2 O; sol. in hot H 2 O and dil. acids. (Stavenhagen, J. pr. 1895, (2) 51. 17.) BaH 4 (AsO 3 ) 2 . Ppt. (Bloxam, Chem. Soc. 15. 281.) +34H 2 O. Moderately sol. in cold, more easily sol. in hot H 2 O. Insol. in alcohol. (Perper, Dissert. 1894.) BaoAs 2 O 5 +2H 2 O. Easily sol. in H 2 O. (Stavenhagen, J. pr. 1895, (2) 51. 18.) +4H 2 O. SI. sol. in H 2 O; also somewhat sol. in alcohol. (Stein, A. 74. 218.) SI. sol. in H 3 As0 4 +Aq and BaO 2 H 2 +Aq. (Dumas.) Sol. in NH 4 Cl+Aq. (Wackenroder, A. 41. 316.) Not pptd. from solutions containing Na citrate. (Spiller.) B a As 4 O 7 . Sol . in H 2 O . Less sol . in alcohol . (Reichard, B. 1894, 27. 1033.) Bismuth arsenite, BiAsO 3 +5H 2 O (?). Easily sol. in HNO 3 +Aq. (Schneider, J. p. (2) 20. 419.) SI. sol. in H 2 O. (Stavenhagen, J. pr. 1895, (2) 51. 35.) Cadmium arsenite, Cd 3 (AsO 3 ) 2 . SI. sol. in H 2 O; easily sol. in NH 4 OH+Aq and dil. acids. (Stavenhagen, I.e.) Cd 2 As 2 O 5 . Ppt. (Reichard, B. 1898, 31. 2168.) Sol. in acids without decomp.; insol. in alkalis. (Reichard, B. 1894, 27. 1033.) 5CdO, As 2 O 3 + 12H 2 O. Not attacked by KOH, Ba(OH) 2 or alkali carbonates +Aq. Insol. in KCN+Aq. (Reichard, Ch. Z. 1902, 26. 1145.) Caesium arsenite bromide, As 2 O 3 , CsBr. Sol. in H 2 0. (Wheeler, Z. anorg. 4. 451.) Caesium arsenite chloride, As 2 O 3 , CsCl. As above. Caesium arsenite iodide, As 2 O 3 , Csl. As above. Calcium arsenite, Ca(AsO 2 ) 2 . Somewhat sol. in H 2 O; sol. in Ca(OH) 2 + Aq or As 2 O 3 +Aq. (Simon, Pogg. 47. 417.) Ca 3 (AsO 3 ) 2 . Ppt. (Kuhn, J. B. 1852. 379.) Only si. sol. H 2 O; readily sol. in dil. acids. (Stavenhagen, I.e.) Sol. in H 2 O, insol. in alcohol. (Reichard, B. 1894, 27. 1036.) 3CaO, 2As 2 O 3 +3H 2 O. SI. sol. in H 2 O; easily sol. in NH 4 Cl+Aq; sol. in As 2 O 3 -f Aq. (Stein.) CaH 4 (AsO 3 ) 2 +o;H 2 O. Moderately sol. in H 2 O. Insol. in abs. alcohol. (Perper, Dis- sert. 1894.) Ca 2 As 2 O 5 . SI. sol. in H 2 O; 1 pt. in 3000- 4000 pts. H 2 O. Alkali chlorides increase sol- ubility slightly. (Stavenhagen, I.e.) SI. sol. in H2O; insol. in H2O 3 . 4NH 3 . Insol. in H 2 O or alcohol. (Girard.) Sodium arsenites. Correspond to potassium arsenites, but have not been obtained in crystalline form. All are very sol. in H 2 0. (Pasteur, A. 68. 308. Na 3 As0 3 . Very sol. in H 2 O. (Staven- hagen, I.e.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3602.) Sodium arsenite bromide, 2As 2 O 3 , NaBr. Decomp. by warm H 2 O. (Riidorff, B. 21. 3052.) Sodium arsenite iodide, 2As 2 O 3 , Nal. Decomp. by hot H 2 O. (Riidorff.) Strontium arsenite, Sr 3 (AsO 3 ) 2 . Sol. in H 2 O. (Stavenhagen, I.e.) Sol. in H 2 O, insol. in alcohol (identical with Stein). (Reichard, B. 1894, 27. 1036.) Sr 2 As 2 O 5 +2H,O. Quite easily sol. in H 2 O. (Stein.) SI. sol. in H 2 0, SrO 2 H 2 -f Aq, or H 3 AsO 4 + Aq. (Dumas.) Very si. sol. in alcohol. (Stein.) Easily sol. in H 2 O and in acids. (Staven- hagen, J. pr. 1895, (2) 51. 17.) Sr 3 As 4 O9. Moderately sol. in H 2 O. (Reich- ard, B. 1894, 27. 1036.) Strontium arsenite iodide, SrI 2 , 3As 2 O 3 + 12H 2 O. As Ba comp. (Griihl, Dissert. 1897.) Thallium arsenite, Tl 3 AsG 3 . SI. sol. in H 2 O and alcohol; easily sol. in acids, especially in dil. H 2 SO 4 . (Stavenhager , I.e.) Tin (stannous) arsenite, Sn 3 (AsO 3 ) 2 . Ppt.; decomp. by acids and alkali. (Reich- ard, B. 1898, 31. 2169.) +2H 2 O. SI. sol. in H 2 O. Easily sol. in dil. acids and alkalies. (Stavenhagen, I.e.) Tin (stannic) arsenite, Sn 3 (AsO 3 ) 4 +5KH 2 O. SI. sol. in H 2 O. (Stavenhagen, I.e.) 5SnO 2 , 2As 2 O 3 . Ppt. Sol. in acids without decomp. (Reichard, B. 1894, 27. 1025.) Sn 7 As 2 On. Ppt. (Reichard, B. 1898, 31. 2169.) Uranium arsenite, UO 2 , As 2 O 3 . Insol. in NH 4 OH+Aq; only si. sol. KOH + Aq. Sol. in acids. (Reichard, B. 1894, 27. 1029.) Zinc arsenite, ZnO, As 2 O 3 . Ppt. (Avery, J. Am. Chem. Soc. 1906, 28. 1163.) 3ZnO,As 2 O 3 . Sol. in acids without decomp. Easily sol. in NH 4 OH+Aq. (Reichard, B. 1894, 27. 1033.) Arseniovanadic acid, As 2 O 5 , V 2 O 5 +2H 2 O. Easily sol. in H 2 0, but solution easily de- composes; crystallizes from H 2 O with 10H 2 O. Composition is vanadium dihydrogen arsen- ate (VO 2 )H 2 As0 4 . (Friedheim, B. 23. 2600.) +14, and +18H 2 O. (Ditte, C. R. 102. 757.) Could not be obtained. (Friedheim.) 3As 2 O 5 , 2V 2 O 5 . (Berzelius.) Correct for- mula is as above. (Friedheim.) 3H 2 O, 7As 2 O 5 , 6V 2 O 5 . (Gibbs, Am. Ch. J. 7. 209.) Could not be obtained. (Fried- heim.) 3H 2 O, 5As 2 O 5 , 8V 2 O 5 +24H 2 0. (Gibbs.) Could not be obtained. (Friedheim.) Ar s enio vanadate s . According to Friedheim (Z. anorg. 1892, 2. 319) the arseniovanadates are double ar- senates of VO 2 and NH 4 . Ammonium arsenio vanadate, (NH 4 ) 2 0, As 2 O 5 2V 2 O 5 ,+5H 2 O. Efflorescent in dry air; si. sol. in cold, decomp. by hot H 2 O. Composition is ammonium divanadium arsenate = (VO 2 ) 2 (NH 4 )AsO 4 +2^H 2 O. (Friedheim, B. 23. 2600.) SI. sol. in cold H 2 O. Somewhat more easily sol. in hot H 2 O with separation of V 2 O 5 . (Schmitz-Dumont, Dissert. 1891.) 2(NH 4 ) 2 O, 3As 2 O 5 2V 2 O 5 ,+4H 2 O. Can- not be crystallized from H 2 O. Composition is m (NH 4 ) 2 HAs0 4 +2(V0 2 ) 2 H 2 As0 4 . (Fried- heim.) Decomp. under H 2 O to (NH 4 ) 2 O, 2V 2 O 5 . As 2 O 5 +5H 2 O. (Schmitz-Dumont, I.e.) 5(NH 4 ) 2 O, 4As 2 O 5 , 2V 2 O 5 +18H 2 O. Sol. in H 2 O. (Ditte, C. R. 102. 1019.) Does not exist. (Friedheim, B. 23. 2605.) ARSENOSOMOLYBDATE, MANGANESE 77 Calcium arseniovanadate, 2CaO, 3As 2 O 3 , 2V 2 O 5 +21H 2 O = CaHAsO 4 +2(VO 2 ) H 2 AsO 4 +8H 2 O. Can be crystallized in presence of vanadic acid without decomp. (Friedheim.) Efflorescent. Sol. in H 2 O. (Schmitz- Dumont, I.e.) Cobalt arseniovanadate, CoO, As 2 O 5 , V 2 O 5 -f 9H 2 O = Co(VO 2 ) 2 H 2 (AsO 4 ) 2 +8H 2 O. Sol. in H 2 O. (Friedheim.) Copper arseniovanadate, CuO, As 2 O 5 , V 2 O 5 + 4H 2 O = Cu(V0 2 ) 2 H 2 (As0 4 ) 2 +3H 2 O. Sol. in H 2 O. (Friedheim.) Magnesium arseniovanadate, MgO, As 2 O 6 , V 2 5 + 10H 2 = (V0 2 ) 2 MgH 2 (As0 4 ) 2 + 9H 2 O. Sol. in H 2 O. (Friedheim.) Moderately sol. in H 2 O. Solution decomp. on standing. (Schmitz-Dumont, I.e.) 2MgO, 3As 2 O 6 2V 2 O 5 ,+23H 2 O =MgHAsO 4 +2(V0 2 )H 2 AsO 4 +9H 2 O. Sol. in H 2 O. (Fried- heim.) Sol. in H 2 but solution decomp. on evap- oration. (Schmitz-Dumont, I.e.) Potassium arseniovanadate, K 2 0, As 2 (>6, 2V 2 O 5 +5H 2 O = (VO 2 ) 2 KAsO 4 +2HH 2 O. Sol. in H 2 O. (Friedheim.) SI. sol. in cold H 2 O. Partially decomp. on heating. (Schmitz-Dumont.) Strontium arseniovanadate, 2SrO, 3As 2 O5, 2V 2 O 5 +20H 2 O =SrHAsO 4 +2(V0 2 ) 2 H 2 Sol. in H 2 O. (Friedheim.) +21H 2 O. Easily sol. in H 2 O. (Schmitz- Dumont.) Zinc arseniovanadate, ZnO. As 2 O 5 , V 2 O 6 Sol. in H 2 O. (Friedheim.) 2ZnO, 3As 2 O 5 , 2V 2 O 6 +5H 2 O, and+18H 2 = ZnHAsO 4 +2(VO 2 ) 2 H 2 AsO 4 , and+6^H 2 0. Sol. in H 2 O. (Friedheim.) Arseniovanadicotungstic acid. Ammonium arsenic vanadicotungstate, 17(NH 4 ) 2 O,2As 2 O 6 ,14i^V 2 O 3 ,20WO 8 + 98H 2 O. SI. sol. in cold H 2 O. Readily sol. in boiling H 2 O. Insol. in alcohol, ether, benzene, CS 2 , CHC1 3 , acetone, nitrobenzene, aniline and acetic anhydride. (Rogers, J. Am. Chem. Soc. 1903, 25. 307.) Arseniovanadicovanadic acid. Ammonium arseniovanadicovanadate, 5(NH 4 ) 2 O, 12As 2 O 6 , 12V0 2 , 6V 2 O 5 + 7H 2 0. SI. sol. in cold, sol. in hot H 2 O, from which crystallizes 4(NH 4 ) 2 O, 9As 2 O 5 , 9VO 2 , 8V 2 O 5 +HH 2 O. Sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 209.) Arseniovanadicovanadiotungstic acid. Ammonium arsenic vanadicovanadiotungstate , +73H 2 0. 17(NH 4 ) 2 O,2As 2 O 6 ,7V 2 O 5 ,4V 2 O 3 ,32l SI. sol. in cold, readily sol. in boiling H 2 0. (Rogers, J. Am. Chem. Soc. 1903, 25. 310.) Arseniovanadiotungstic acid. Ammonium arseniovanadiotungstate, 18(NH 4 ) 2 O, 2As 2 6 , 13V 2 O 6 , 39WO 3 + 88H 2 O. Sol. in H 2 O. Insol. in organic solvents. (Rogers, J. Am. Chem. Soc. 1903, 25. 306.) Arseniuretted hydrogen, AsH 3 . See Arsenic hydride. Arsenochromic acid. Potassium arsenochromate, K 4 Cr 2 As 2 Oi 6 + 12H 2 0. Sol. in moderately cone, mineral acids. (Tarugi, C. C. 1897, II. 724.) K7Cr 3 As 5 O 2 2+24H 2 O. Ppt. Sol. in dil. warm acids. (Tarugi.) Potassium hydrogen arsenochromate, K 4 H 6 Cr 3 As 2 O 16 . (Tarugi, C. C. 1897, II. 724.) Arsenosoarseniotungstic acid. Potassium arsenosoarseniotungstate, 10K 2 O, 4As 2 O 5 , As 2 O 3 , 21WO 3 +26H 2 O. - Precipitate. Sol. in a large amount of hot H 2 O. (Gibbs, Am. Ch.J. 7.313.) Arsenosomolybdic acid. Ammonium arsenosomolybdate, 3(NH 4 ) 2 O, 5As 2 3 , 12MoO 3 +24H 2 O. SI. sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 313.) Ammonium barium arsenosomolybdate, 3(NH 4 ) 2 O, 2BaO, 5As 2 O 3 , 10MoO s + 50H 2 O. Ppt. (Ephraim, Z. anorg. 1910, 66. 57.) Ammonium cupric arsenosomolybdate, (NH 4 ) 2 O, CuO, 2As 2 O 3 , 4MoO 3 +2H 2 O, and 2(NH 4 ) 2 0, CuO, 3As 2 3 , 6MoO 3 + 13H 2 O. Ppts. (Ephraim, Z. anorg. 1910, 66. 58.) Barium arsenosomolybdate, 3BaO, 2As 2 O 8 , 8Mo0 3 + 13H 2 O. Very si. sol. in H 2 O. (Gibbs.) Copper arsenosomolybdate, 2CuO, 3As 2 O 3 , 6MoO 3 . Sol. inH 2 O. (Gibbs.) Manganese arsenosomolybdate, 3As 2 O 3 , 6MoO 3 +6H 2 O, Insol. in H 2 O. (Gibbs.) 2MnO, 2 O. 78 ARSENOSOMOLYBDATE, POTASSIUM Potassium arsenosomolybdate, 3K 2 O, As 2 O 3 , 5MoO 3 +3H 2 O. Easily sol. in H 2 O. (Ephraim, Z. anorg. 1910, 66. 54.) 3K 2 O, As 2 O 3 , 8MoO 3 + 18H 2 O. Easily sol. in H 2 0. (Ephraim.) Sodium arsenosomolybdate, Na 2 O, As 2 O 3 , 2MoO 3 +6H 2 O. ' Easily sol. in H 2 O. (Ephraim, Z. anorg. 1910, 66. 56.) 2Na 2 O, As 2 3 , 4MoO 3 +13H 2 O. Ppt. (Ephraim.) Zinc arsenosomolybdate, 2ZnO, 3As 2 O 3 , 6MoO 3 +6H 2 O. Sol.inH 2 0. (Gibbs.) Arsenosophosphotungstic acid. Potassium arsenosophosphotungstate, 10K 2 O, 14As 2 O 3 , 3P 2 O 6 , 32WO 3 +28H 2 O. Moderately sol. in cold, very easily in hot H 2 O. (Gibbs.) 7K 2 O, 2As 2 O 3 , 4P 2 5 , 60WO 3 +55H 2 O. Sol. in hot H 2 O with decomp. (Gibbs.) Potassium sodium arsenosophosphotungstate, 5K 2 O, Na 2 O, 2As 2 O 3 , 2P 2 O 5 , 12WO 3 + 15H 2 O. (Gibbs, Am. Oh. J. 7. 313.) . Arsenosotungstic acid. Ammonium arsenosotungstate, 7(NH 4 ) 2 O, 18W0 3 +18H 2 O. Sol. inH 2 O. (Gibbs.) Barium arsenosotungstate, 4BaO, As 2 O 3 , 9W0 3 +21H 2 0. Precipitate. 'Nearly insol. in H 2 O. (Gibbs.) Sodium arsenosotungstate, 9Na 2 O, 8As 2 O 3 , 16WO 3 +55H 2 O. Very sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 313.) Arsenyl bromide, AsOBr. H 2 O dissolves out As 2 O 3 : insol. in alcohol. (Serullas.) +H 2 O. (Wallace, Phil. Mag. (4) 17. 122.) As 8 O 9 Br 6 = 2AsBr 3 , 3As 2 O 3 +12H 2 O. Arsenyl bromide with MBr. See Arsenite bromide, M. Arsenyl chloride, AsOCl. Sol. in H 2 O with decomp. +H 2 O. (Wallace, Phil. Mag. (4) 16. 358.) As 3 O 4 Cl. (WaUace.) Arsenyl chloride with MCI. See Arsenite chloride, M. Arsenyl potassium fluoride, AsOF 3 , KF + (Marignac, A. 146. 237.) Arsenyl iodide, As 8 I 2 On = 2AsOI, 3As 2 O 3 + 12H 2 0. Decomp. by H 2 O. (Wallace, Phil. Mag. (4) 17. 122.) SI. sol. in cold H 2 O, less sol. in alcohol. (Plisson, J. Pharm. 14. 46.) Arsenyl iodide with MI. See Arsenite iodide, M. Arsenyl sulphoiodide, AsiJgSeOa. Scarcely attacked by cold H 2 O. Boiling H 2 O extracts AsI 3 . Decomp. by hot HNO 3 or H 2 SO 4 . Easily sol. in KOH, or NH 4 OH + Aq. (Schneider, J. pr. (2) 36. 513.) Arsine. See Arsenic hydride. Atmospheric air. See Air, atmospheric. Auriamine, Au(OH) 2 NH 2 . (Jacobsen, C. R. 1908, 146. 1214.) Zhauriamine, Au 2 (OH) 4 NH. (Jacobsen, C. R. 1908, 146. 1214.) O^0?/2'L111*1III11I1G .N-A-Us. JNiis. Decomp. by H 2 O into NAu 3 . (Raschig, A. 235. 341.) Auric acid, HAu 2 O 4 . Sol. in HBr, or HCl+Aq. (Kruss, B. 19. 2546.) Ammonium aurate. See Auroamidoimide. Barium aurate, BaAu 2 4 +5H 2 O. SI. sol. in H 2 O. (Weigand, Zeit. angew. Ch. 1905, 19. 139.) +6H 2 O. Sl.sol.inH 2 O. Sol. in dil. H 2 SO 4 and in dil. HNO 3 . Sol. in HC1. Decomp. by alcohol. (Meyer, C. R. 1907, 145. 806.) Calcium aurate (?). Insol. in H 2 O; sol. in CaCl 2 +Aq. (Fremy, A. ch. (3) 31. 485.) CaAu 2 4 +6H 2 0. As Ba salt. (Meyer, C. R. 1907, 145. 806.) Magnesium aurate (?). Ppt. Insol. in H 2 O; sol. in MgCl 2 +Aq. (Pelletier.) Potassium aurate, KAuO 2 +3H 2 0. Very sol. in H 2 O, and easily decomp. (Fremy, A. ch. (3) 31. 483.) Sol. in alcohol; the solution in alcohol does not decomp. below 50. (Figuier, A. ch. (3) 11. 364.) . Potassium aurate sulphite, KAuO 2 , 2K 2 SO 3 + 5H 2 O. Sol. in H 2 O with decomp. Nearly insol. in alkaline solutions. (Fremy, A. ch. (3) 31. 485.) BARIUM AMMONIA 79 Sodium aurate, Na 2 Au 2 O4+2H 2 O. Sol. in H 2 O. Sol. in dil. H 2 SO 4 , dil. HNO 3 , and HC1 with decomp. Decomp. by alcohol. (Meyer, C. R. 1907, 146. 806.) Strontium aurate, SrAu 2 O 4 +6H 2 O. As Ba salt. (Meyer.) Auriimide chloride, Au(NH)Cl. (Raschig.) Auriimide nitrate, Au 2 N 2 H 2 O, 2HNO 3 , or AuN, HNO 3 +}^H 2 O, or Au 2 O(NH) 2 , 2HN0 3 . Not deliquescent. Decomp. by hot H 2 O into Au 2 O(NH) 2 . (Schottlander, J. B. 1884. 453.) Auroamidoimide, Au(HN)NH 2 +3H 2 O. (Fulminating gold.) Insol. in H 2 O; not attacked by dil. acids; sol. in cone, acids, and in moderately dil. acids, when freshly pre- cipitated. Insol. in alkalies or alcohol. Sol. inKCN+Aq. Tnauroamine, Au 3 N+5H 2 O. Not decomp. by boiling dil. acetic acid, HNO 3 , or H 2 SO 4 . (Raschig, A. 1886, 235. 349.) Auricyanhydric acid, HAu(CN) 4 +1^H 2 O. Easily sol. in H 2 O, alcohol, or ether. See also Bromauricyanides. Chlorauricyanides. lodauricyanides. Ammonium auricyani'de, NH 4 Au(CN) 4 . Easily sol. in H 2 O or alcohol. Insol. in ether. Cobaltous auricyanide, Co[Au(GN) 4 ] 2 +9H 2 O. SI. sol. in cold, easily in hot H 2 O. SI. sol. in alcohol. (Lindbom.) Potassium auricyanide, KAu(CN) 4 +l^H 2 0. Efflorescent. SI. sol. in cold, easily in hot H 2 O. Easily sol. in alcohol. Silver auricyanide, AgAuCN 4 . Insol. in H 2 O or HNO 3 +Aq. Sol. in NH 4 OH+Aq. DiGLUTodiaxnine nitrate. See Auriimide nitrate. Aurobromhydric acid. See Bromauric acid. Aurobromic acid. See Bromauric acid. Aurochlorhydric acid. See Chlorauric acid. Aurochloric acid. See Chlorauric acid. Aurocyanhydric acid. Aurocyanides with MCN. See Cyanide, aurous with MCN. Azinosulphonic acid. Ammonium azinosulphonate, N 3 SO 3 NH 4 . (Traube, B. 1914, 47. 944.) Barium azinosulphonate, (N 3 SO 3 ) 2 Ba. (Traube, B. 1914, 47. 944.) Potassium azinosulphonate, N 3 SO 3 K. Easily sol. in H 2 0. Can be cryst. from boiling abs. alcohol, (Traube, B. '1914, 47. 943.) Sodium azinosulphonate, N 3 SO 3 Na. (Traube, B. 1914, 47. 944.) Azoimide, HN 3 . Miscible with H 2 O and alcohol. (Curtius and Radershausen, J. pr. (2) 43. 207.) Stable in aq. solution ; decomp. slowly by dil. boiling HC1. (Curtius, J. pr. 1898, (2) 58. 265.) For salts of HN 3 , see azoimide of metal under metal. Azoimide, hydroxylamine, N 3 H,2NH 2 OH. Sol. in H 2 0. Gradually volatilizes at ord. temp. (Dennis, J. Am. Chem. Soc. 1907, 29. 22.) Azophosphoric acid. See Pf/rophosphamic acid. Dewtezophosphoric acid. See Pyropb.osphodia.ndc acid. Barium, Ba. Decomp. by H 2 O and abs. alcohol. (Guntz, C. R. 1901, 133. 874.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Barium amalgam, BaHg 13 . Stable in contact with liquid amalgam up to 30. Can be cryst. from Hg without de- comp. if temp, does not exceed 30. (Kerp, Z. anorg. 1900, 25. 68.) BaHg 12 . Stable in contact with liquid amalgam from 30- 100. Can be cryst. from Hg without decomp. at any temp, within these limits. (Kerp.) Barium amide, Ba(NH 2 ) 2 . B.-pt. 280. (Mentrel, C. C. 1903, 1. 276.) Decomp. by H 2 O. (Guntz and Mentrel, Bull. Soc. 1903, (3) 29. 578.) Barium potassium amide. See Potassium ammonobarate. Barium ammonia, Ba(NH 3 ) 6 . Takes fire in the air. Only si. sol. in liquid NH 3 . Violently decomp. by H 2 O. (Mentrel, C. R. 1902, 135. 740.) 80 BARIUM ARSENIDE Barium arsenide, Ba 3 As 2 . Decomp. by H 2 O. (Lebeau, C. R. 1899 129. 48.) Barium azoimide, Ba(N 3 ) 2 . Very si. hydroscopic; explosive. 12.5 pts. are sol. in 100 pts. H 2 O at 16.2 " " " " 100 " H 2 O "10.5 16.7 " " " " 100 " H 2 O " 15 17.3 " " " " 100 " H 2 O " 17 0.0172 pts. are sol. in 100 pts. abs. alcohol at 16. Insol. in ether. (Curtius, J. pr. 1898, (2. 58. 290.) See also Barium nitride. Barium boride, BaB 6 Sol. in fused oxidizing agents, not decomp by H 2 O; insol. in aq. acids; si. sol. in cone H 2 SC>4, sol. in dil. and cone. HNO 3 . (Moissan C. R. 1897, 125, 634.) Barium sw&bromide sodium bromide, BaBr, NaBr. Decomp. by H 2 O. (Guntz, C. R. 1903, 136. 750.) Barium bromide, BaBr 2 , and +2H 2 O. 100 pts. H 2 O dissolve at 20 40 60 80 100 98 104 114 123 135 149 pts. BaBr 2 . Sat. BaBr 2 +Aq contains at: 20 9 +7 16 19 40 45.7 46.5 48.5 48.8 49.3 50.9%BaBr 2 71 76 77 104 145 160 175 55.1 55.555.656.6 60.5 59.4 60.3%BaBr 2 (Etard, A. ch. 1894, (7) 2. 540.) Sp. gr. of BaBr 2 +Aq at 19.5 containing: 5 10 15 20 25 30%BaBr 2 1.045 1.092 1.114 1.201 1.262 1.329 35 1.405 40 1.485 45 1.580 50 55%BaBr 2 . 1.685 1.800 (Kremers, Pogg. 99. 444, calculated by Gerlach, Z. anal. 8. 285.) BaBr 2 +Aq containing 7.74% BaBr 2 has sp.gr. 20/20= 1.0716. BaBr 2 +Aq containing 16.76% BaBr 2 has sp. gr. 20/20 = 1.1674. (Le Blanc and Rohland. Z. phys. Ch. 1896, 19. 279.) Sat. BaBr 2 +Aq boils at 113. (Kremers, Pogg. 99. 43.) Solubility in BaI 2 +Aq at t. t Sat. solution contains % BaBr 2 % BaI 2 16 -16 +60 135 135 170 210 4.7 5.0 5.5 9.3 9.0 11.0 14.9 57.9 59.0 66.0 67.3 67.2 67.4 67.7 (Etard, A. ch. 1894, (7) 3. 287.) Very sol. in absolute alcohol. (Hiinefeld.) 100 pts. absolute methyl alcohol dissolve 50 pts. BaBr 2 at 22.5. 100 pts. absolute ethyl alcohol dissolve 3 pts. BaBr 2 at 22.5. (de Bruyn, Z. phys. Ch. 10. 783.) Sat. solution in 87% alcohol contains 6% BaBr 2 . (Richards, Z. anorg. 3. 455.) 100 pts. absolute methyl alcohol dissolve 45.8 pts. BaBr 2 +2H 2 O at 15. 100 pts. 93.5% methyl alcohol dissolve 27.3 pts. BaBr 2 +2H 2 O at 15. 100 pts. 50% methyl alcohol dissolve 4 pts. BaBr 2 +2H 2 O at 15. (de Bruyn, Z. phys. Ch. 10. 787.) 100 g. BaBr 2 +CH 3 OH contain 0.4 g. BaBr 2 at the critical temp. (Centnerszwer, Z. phys. Ch. 1910, 72. 437.) At 15, 1 pt. by weight is sol. in: 36 pts. methyl alcohol, sp. gr. 0.709 207 " ethyl " " " 0.8035 652 " propyl " " " 0.8085 (Rohland, Z. anorg. 1897, 15. 413.) Nearly insol. in boiling amyl alcohol, 10 ccm. dissolving only an amt. equal to 1.3 mg BaO. (Browning, Sill. Am. J. 144. 459.) Sol. in acetone. (Naumann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3789.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Barium cadmium bromide, BaBr^ CdBr 2 -f- Sol. in H 2 0. (v. Hauer, W. A. B. 20. 40.) Barium rhodium bromide. See Bromorhodite, barium. Barium bromide ammonia, BaBr 2 ,8NH 3 . Decomp. by H 2 O. (Joannis, C. R. 1905. 140. 1244.) Barium bromide hydrazine, BaBr 2 , 2N 2 H 4 . Hydroscopic. Very sol. in H 2 O. Insol. in alcohol. (Franzen, Z. anorg. 1908, 60. 291.) Barium bromofluoride, BaBr 2 ,BaF 2 . Insol. in and undecomp. by boiling alcohol. Sol. in HBr and in HNO 3 . Decomp. by H 2 O, hot H,S0 4 , dil. HC1, dil. HN0 3 , or dil. acetic icid. (Defacqz, C. R. 1904, 138. 199.) Barium carbide, BaC 2 . Decomp. by H 2 O. (Maquenne, C. R. 144. 60.) Sp. gr. 3.75. Easily decomp. by H 2 O and dil. acids. (Moissan, Bull. Soc. 1894, (3) 11. 008.) BARIUM CHLORIDE 81 Barium carbonyl, Ba(CO) 2 . Sol. in H 2 O. (Guntz and Mentrel, Bull. Soc. 1903, (3) 29. 586.) Barium sw&chloride, BaCl. Decomp. by H 2 O. (Guntz, C. R. 1903, 136. 751.) Barium sw&chloride sodium chloride, BaCl, NaCl. Decomp. by H 2 O. (Guntz, C. R. 1903, 136. 750.) Barium chloride, BaCl 2 , and +2H 2 O. Permanent in dry air. 100 pts. H 2 O at t dissolve (a) pts. BaCh and (6) pts. BaCh+2H 2 O. Solubility in 100 pts. H 2 O at t. t Pts. BaCh t Pts. BaCh t Pts. BaCh 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 30.9 31.2 31.5 31.7 31.9 32.2 32.4 32.6 32.8 33.1 33.3 33.5 33.8 34.0 34.2 34.5 34.7 35.0 35.2 35.5 35.7 36.0 36.2 36.5 36.7 37.0 37.2 37.5 37.7 38.0 38.2 38.5 38.7 39.0 39.2 39.5 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 39.7 40.0 40.2 40.5 40.7 41.0 41.3 41.6 41.9 42.2 42.5 42.7 43.0 43.3 43.6 43.9 44.2 44.4 44.7 45.0 45.3 45.6 45.9 46.2 46.4 46.7 47.0 47.3 47.6 47.9 48.2 48.5 48.8 49.1 49.4 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 87 88 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 104 104.1 49.7 50.0 50.3 50.6 50.9 51.2 51.5 51.8 52.1 52.4 52.7 53.0 53.3 53.6 54.0 54.3 54.6 55.0 55.3 55.6 55.9 56.2 56.6 56.9 57.2 57.6 57.9 58.2 58.5 58.8 59.2 59.5 59.8 60.2 60.3 t a b t a b 15.64 49.31 34.86 43.84 43.50 55.63 74.89 59.94 65.51 105.48 59.58 77.89. (Gay-Lussac, A. ch. (2) 11. 309.) 100 pts. H 2 O at t dissolve 32.62 +0.271U pts. BaCh. (Kopp.) 100 pts. H 2 O dissolve pts. BaCh +2H 2 O at t. t Pts. BaCl+2HiO ,o Pts. BaCh+2H 2 16.25 20.00 22.50 37.50 50.00 39 42 43 51 65 .66 .22 .7 .0 .0 62.50 48.0 75.00 63.0 87.00 65.0 100 72.0 (Brandes.) Sol. in 2.67 pts. H 2 O at 18.75. (Abl.) 1 pt. BaCh is sol. in 2.86 pts. H 2 O at 15.5, and 1.67 pts. at boiling temp. (M. R. and P.) 100 pts. H 2 O at 15.5 dissolve 20 pts. BaCh, and 43 pts. at 87.7. (Ure's Diet.) Solubility in 100 pts. H 2 O at t. (Mulder, calculated from his own and other observations. Scheik. Verhandel. 1864. 45.) The saturated solution contains 60.3 pts. BaCl 2 to 100 pts. H 2 O, and boils at 104.1. (Mulder.) 60.1 pts. BaCl 2 to 100 pts. H 2 0, and boils at 104.4. (Legrand.) 61.8 pts. BaCl 2 to 100 pts. H 2 O, and boils at 104.5. (Griffith.) 59.58 pts. BaCl 2 to 100 pts. H 2 O, and boila at 105.48 (Gay-Lussac); at 106 (Kremers). 54.1 pts. BaCl 2 to 100 pts. H 2 0, and forms crust at 104.4; highest temperature observed, 104.9. (Gerlach, Z. anal. 26. 426.) Sat. BaCl 2 -f-Aq contains at: t Pts. BaCh , PtS. i BaCh 12.2 38.4 62^75 31.1 33.9 41.2 47.7 77.5 51.9 95.65 57.7 102.5 58.9 105 59.7 (Nordenskiold, Pogg. 136. 316.) 100 pts. H 2 O dissolve pts. BaCh at t. t Pts. BaCh , Pts. BaCh 9 30 37 33.2 38.1 40.0 50 43.7 58 45.9 (Gerardin, A. ch. (4) 5. 143.) 1 pt. BaCl 2 +2H 2 O is sol. in 2.18 pts. H 2 at 21.5, and the solution has sp. gr. = 1.2878. (Schiff, A. 109. 326.) 1 pt. anhydrous BaClo is sol. in 2.86 pts. H 2 O at 15. (Gerlach.) 100 130 144 160 180 215 36 37.3 37.5 38.9 40.7 43.1%BaCl 2 (fitard, A. ch. 1894, (7) 2. 535.) Aq. solution contains 27.6% BaCl 2 at 30. (Shreinemakers, C. C. 1910, 1. 9.) 82 BABIUM CHLORIDE Solubility of BaCl 2 +2H 2 O in H 2 O equals 1.745 mol.-litre at 30. (Masson, Chem. Soc. 1911, 99. 1136.) BaCh+Aq sat. at 8 has sp. gr. 1.27. (Anthon.) BaCh+Aq sat. at 15 has sp. gr. 1.282. (Michel and Krafft.) BaCh+Aq sat. at 18.1 has sp. gr. 1.285, and con- tains 44.31 pts. BaCh+2H 2 O to 100 pts. H 2 O. (Kar- sten.) Sp. gr. of BaCh+Aq at 19.5. Sp. gr. of BaCl 2 +Aqat20. g. mols. BaCh per 1. Sp. gr. 0.01 0.025 0.05 0.075 0.10 0.25 0.40 1 1 1 1 1 1 1 .001878 .00475 .00929 .01369 . 01766 .0456 .0726 % BaCh Sp. gr. || % BaCh Sp. gr. (Jones and Pearce, Am. Ch. J. 1907, 38. 701.) BaCl 2 -fAq containing 6.94% BaCl 2 has sp. gr. 20/20 = 1.0640. BaCl 2 +Aq containing 11.38% BaCl 2 has sp. gr: 20/20 = 1.1086. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 279.) Sp. gr. of BaCl 2 -f-Aq at 25. 8.88 18.24 1.0760 27.53 1.1521 || 35.44 1.2245 1.2837 (Kremers, Fogg. 99. 444.) Sp. gr. of BaCl 2 -fAq at 15. % BaCh Sp. gr. % BaCh Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 .00917 .01834 .02750 .03667 .04584 .05569 .06554 .07538 .08523 .09508 . 10576 . 11643 .12711 14 15 16 17 18 19 20 21 22 23 24 25 1.13778 1.14846 1.15999 1.17152 1.18305 1.19458 1.20681 1.21892 1.23173 1.24455 1.25736 1.27017 BaCh+Aq Sp. gr. 1-normal Vt" " 1.0884 1.0441 1.0226 1.0114 (Wagner, Z. phys. Ch. 1890, 5. 35.) Sp. gr. of BaCl 2 +Aq. t | Concentration of BaCh 4-Aq Sp. gr. 25 1 pt. BaCl 2 in 3.684 pts. H 2 O 1.2194 22.8) 1 " " " 52.597 " " 1.0145 (Hittorf, Z Temp. phys. Ch. 1902, 39. 628.) of Maximum Density. (Gerlach, Z. anal. 8. 283.) Sp. gr. of BaCl 2 +Aq at 21.5. Weight of BaCh in 1000 grams J H 2 O ""emp. of maximum density Molecular reduc- tion of temp, of M. D. % m?o 2+ Sp. gr. % BaCh + 2H 2 O Sp. gr. 6.73 10.42 20.83 41.72 3.982 3.207 2.783 1.572 0.843 23.94 23.88 24.04 24.04 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 1.0073 1.0147 .0222 .0298 .0374 .0452 .0530 .0610 .0692 .0776 .0861 .0947 .1034 .1122 .1211 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 1.1302 1.1394 1.1488 .1584 .1683 .1783 .1884 .1986 .2090 1.2197 1.2304 1.2413 1.2523 1.2636 1.2750 (De Coppet, C. R. 1897, 126. 533.) BaCl 2 +Aq containing 10% BaCl 2 boils at 100.6. (Gerlach.) BaCl 2 +Aq containing 20% BaCl 2 boils at 101.9. (Gerlach.) B.-pt. of BaCl 2 +Aq containing pts. BaCl 2 to 100 pts. H 2 O. G = according to Gerlach (Z. anal. 26. 443) : L = according to Legrand (A. ch. (2)59.452). B.-pt. G L (Schiff, calculated by Gerlach, Z.c.) Sp. gr. of BaCl 2 +Aq at 18. 100.5 101.0 101.5 102.0 102.5 103.0 103.5 104.0 104.4 104.5 6.4 12.7 19.0 25.3 31.6 37.7 43.7 49.5 55'.2 11.0 19.6 26.2 32.5 38.6 44.5 50.3 56.0 60.1 % BaCh Sp. gr. % BaCh Sp. gr. 5 10 15 1.0445 1.0939 1.1473 20 24 1.2047 1.2559 (Kohlrausch, W. Ann. 1879. 1.) BARIUM CHLORIDE 83 Less sol. in H 2 O containing HC1 than in pure H 2 0, and scarcely sol. in cone. HCl+Aq. (Berzelius.) Solubility of BaCl 2 in HCl+Aq at 0. BaCl 2 =no. % mols. (in milligrammes) dis- solved in 10 cc. of the liquid ; HCl = no. mols. (in milligrammes) contained in the same quantity of liquid. Sp. gr. 1.250 1.242 BaCl 2 HCl Sum of mols. 29.45 29.45 27.8 1.1 28.9 26.075 2.8 28.875 23.4 5.0 28.4 14.0 14.36 28.36 10.2 18.775 28.975 6.67 22.75 29.42 2.74 32.0 34.74 0.29 50.5 50.79 228 210 143 118 099 079 1.088 (Engel, Bull. Soc. (2) 45. 653.) Sol. in about 8000 pts. cone. HCl+Aq. Sol. in about 20,000 pts. cone. HCl+Aq through which HCl gas was passed. Practically insol. in cone. HCl+Aq con- taining Ve vol. ether. (Mar, Sill. Am. J. 143. Solubility in HCl+Aq at 30. Composition of the solution Solid phase %by wt; HCI % by wt. BaCh 5.94 11.55 18.11 32.35 37.34 38.63 27.6 12.97 3.85 0.46 0.00 0.00 0.00 BaCl 2 , 2H 2 O it (t ii n BaCl 2 , 2H,O+BaCl 2 , H 2 O BaCl 2 , H 2 O (Schreinemakers, Z. phys. Ch. 1909, 68. 89.) Much less sol. in HNO 3 +Aq than in H 2 O, because Ba(NO 3 ) 2 is nearly insol. therein. (Wurtz.) BaCl 2 is sol. in about 4.00 pts. H 2 O. 5.00 pts. NH 4 OH+Aq (cone.). 5.33 pts. NH 4 OH+Aq (1 vol. cone.: 3 vols. H 2 0). 5.33 pts. HCl+Aq (1 vol. cone.: 4 vols. H 2 0). 8.00 pts. HC 2 H 3 O 2 +Aq (1 vol. commercial acid: 1 vol. H 2 O). 6.00 pts. NH 4 Cl+Aq (1 pt. NH 4 C1 : 10 pts. H 2 O). 6.00 pts. NH 4 C 2 H 3 O 2 +Aq (dil. NH 4 OH + Aq neutralized by dil. HC 2 H 3 O 2 +Aq.) 6.67 pts. NaC 2 H 3 O 2 +Aq (commercial HC 2 H 3 O 2 neutralized by Na 2 CO 3 , and dil. with 4 vols. H 2 O). ' 6.33 pts. Cu(C 2 H 3 O 2 ) 2 +Aq. See Stolba (Z. anal. 2. 390). 5.67 pts. grape sugar (1 pt. grape sugar: 10 pts. H 2 O). (Pearson, Zeit. Chem. 1869. 662.) BaCl 2 +NH 4 Cl. Solubility of BaCl 2 NH 4 Cl+Aq at 30. in Composition of the Solid phase solution % NEUC1 % BaCh 27.6 BaCl 2 .2H 2 O 5.71 22.16 n 10.06 18.36 (( 13.84 15.42 t( 20.00 10.89 tt 24.69 8.33 tc 25.79 7.95 BaCl 2 .2H 2 O+NH 4 Cl 26.06 7.99 tt 27.47 3.56 NH 4 C1 29.5 K (Schreinemakers, Z. phys. Ch. 1909, 66. 688.) See also under Ammonium chloride. BaCl 2 +Ba(OH) 2 . Solubility of BaCl BaO+Aqat30. 2 in Composition of Solid phase the solution %by %by wt. wt. BaO BaCh 27.6 BaCl 2 , 2H 2 O 1.78 27.42 1.79 27.31 BaCl 2 , 2H 2 0+BaCl(OH), 2H 2 1.75 27.41 a 2.33 24.98 BaCl(OH), 2H 2 2.50 24.20 3.27 21.46 4 67 19.18 4.86 18.97 BaCl(OH), 2H O+BaO, 9H 2 O 4.29 18.83 4.64 18.77 4.65 18.10 4.62 18.04 BaO, 9H 2 O 4.60 17.08 4.58 12.81 4.45 10.77 4.99 Sol. in CuCl 2 ,NH 4 Cl+Aq at 30. (Schreine- makers, Z. phys. Ch. 1909, 66. 688.) The solubility data for the system BaCl 2 + }uCl 2 +KC1 + Aq have been determined at 40 id 6ot (Schreinemakers, C. C. 1915, 1. 933.) BaCl 2 +HgCl 2 . Solubility of BaCl 2 + HgCl 2 in H 2 O. Cms. per 100 g. solution Solid phase BaCb HgCh 10.4 23.58 50.54 BaCl 2 ,2H 2 O+HgCl 2 10.4 23.44 50.74 10.4 10.4 22.58 22.48 51.23 51.41 BaCl 2 ,3HgCl 2 , 6H 2 10.4 22.10 51.66 10.4 25.0 21.64 23.02 51.74 54.83 BaCl 2 ,2H 2 O+HgCl 2 (Foote and Bristol, Am. Uh. J. 32. -24s.; 84 BARIUM CHLORIDE Solubility of BaCl 2 +HgCl 2 in H 2 0. Temp. =30 Temp. =0 % HgCh % BaCh Solid phase % HgCh % BaCh Solid phase 27.77 BaCl 2 .2H 2 O 23.70 BaCl 2 .2H 2 2.90 27.56 * 14.25 24.0 " 7.09 27.47 * 36.20 24.89 . " 12.98 26.99 < 46.12 24.07 BaCl 2 , 3HgCl 2 .6H 2 O + 22.61 26.89 ' 46.05 24.03 " BaCl 2 .2H 2 O 34.57 26.69 ' 46.07 24.05 M 46.50 25.22 ' 46.59 23.28 BaCl 2 , 3HgCl 2 .6H 2 55.16 23.46 HgCl 2 +BaCl 2 .2H 2 O 47.78 21.05 a 55.32 23.08 H 48.43 20.64- BaCl 2 , 3HgCl 2 .6H 2 0+HgCl 2 55.19 22.98 It 48.49 20.71 u 48.97 17.87 HgCl 2 44.33 18.50 HgCl 2 41.30 14.26 29.0 11.59 u 27.62 8.41 16.36 6.11 u 14.19 7**7 2.65 a ft 3.95 tt .67 Temp. =40 56.57 22.98 BaCl 2 .2H 2 O+HgCl 2 (Schreinemakers, Ch. Weekbl. 1911, 7. 202.) BaCl 2 +KCl. Sol.insat.KCl+Aq, at first 10 P ts - H 2 dissolve, when both salts are without pptn. The KC1 is pptd. after a time until a state of equilibrium is reached. 100 pts. H 2 O at 16.6 dissolve 33.8-27.2 pts. KC1 and 18.2-34.9 pts. BaCl 2 . (Kopp, A. 34. 267.) 100 g. sat. solution of BaCl 2 +KCl contain 13.83 g. BaCl 2 and 18.97 g. KC1 at 25. (Foote, Am. Ch. J. 32. 253.) in excess i 2 3 4 5 6 NaCl . BaCl, . . . 35.9 4.1 34.5 ss!6 40.4 35.3 19.4 60'.3 38.6 54.7 BaCl 2 +Ba(NO 3 ) 2 . Ba(NO 3 ) 2 +Aq. BaCl 2 is sol. in sat. Solubility of BaCl 2 +Ba(NO) 2 in H 2 0. Both salts present in solid phase. 1, 2, and 3 are at 17. ( Kopp, A. 34. 268.) 4, 5, and 6 are at b.-pt. (Mulder.) Solubility of BaCl 2 +NaCl. 100 pts. H 2 O dissolve pts. BaCl 2 and NaCl at t. t 20 40 60 Gms. per 100 gms. solution t Gms. per 100 gms. solution BaCh Ba(NO 3 )2 BaCh Ba(NO 3 ) 2 22.5 24.5 26.5 28.5 4.3 6.0 7.5 9.5 100 140 180 210 31 32 33 32 14 20 26 32 (Etard, A. Ch. (7) 2. 535.) Very slowly sol. in sat. NaNO 3 +Aq with separation of Ba(NO 3 ) 2 . Rapidly sol. in sat. KNO 3 +Aq, forming Ba(NO 3 ) 2 , which separates out. (Karsten.) BaCl 2 +NaCl. BaCl 2 is sol. in NaCl+Aq at first without separation of NaCl, which, however, finally separates. t< Pts. BaCl 2 Pts. NaCl t Pts. BaCh Pts. NaCl 10 20 30 40 50 4.1 4.1 5.0 6.3 7.9 33.9 33.8 33.7 33.6 33.5 60 70 80 90 100 9.7 11.7 13.9 15.9 17.9 33.5 33.6 33.6 33.6 33.6 (Precht and Wittgen, B. 14. 1667.) Solubility of BaCl 2 +NaCl in HCl+Aq at 30. Solid phase, NaCl Solid phase, BaCl2+2H 2 O Sp. gr. of sat. solution G. mol. litre Sp. gr. of sat. solution G. mol.-litre HC1 NaCl HC1 BaCh 1.2018 1.1906 1.1801 1.1633 1.1512 1 . 1427 1 . 1289 1.1188 1.1258 0.0000 0.4575 0.969 1.786 2.412 3.052 4.152 5.950 7.205 5.400 4.932 4.386 3.589 2.978 2.463 1.628 0.630 0.268 1.3056 1.2651 1.2147 1.1789 1.1419 1 . 1068 1.0880 1.0895 1.1024 1 . 1609 0.0000 0.4709 1.107 1.622 2.234 3.041 3.953 3.059 6.234 10.25 1.745 1.468 1.122 0.861 0.592 0.307 0.124 0.020 0.00 0.00 (Masson, Chem. Soc. 1911, 99. 1136.) BARIUM CHLORIDE 85 Solubility of BaCl 2 +NaClin HCl+Aq at 30. %HC1 %NaCl %BaCl 2 Solid phase 4.84 12.02 17.20 23.16 28.66 36.51 23.85 18.07 9.55 4.65 1.54 0.47 0.12 3.8 2.27 0.82 0.29 0.00 0.00 0.00 NaCl,BaCl 2 .2H 2 NaCl+BaCl 2 .H 2 (Schreinemakers, Arch. Neer. Sc. ex. nat. (2) 15. 91.) ,. (Franklin, Am. Ch. Insol in liquid J. 1898, 20. 827.) Solubility in alcohol: 100 pts. alcohol of given sp. gr. dissolve pts. of the anhydrous, and crystallized salt. Sp. gr. Pts. BaCh Pts. BaCl 2 4-2H 2 O 0.900 0.848 0.834 0.817 1.00 0.29 0.185 0.09 1.56 0.43 0.32 0.06 (Kirwan.) Insol. in abs. alcohol, or below 19 in al- cohol of over 91%. Dil. alcohol dissolves less BaCl 2 than corresponds to the amount of H 2 O present. (Gerardin, A. ch. (4) 5. 142.) Solubility in 100 pts. alcohol at t. D =sp. gr. of alcohol; S= solubility. D =0.9904 D =0.9848 D =0.9793 D =0.9726 t s t s t s t .s 14 25 32 47 60 29.1 32.0 33.5 37.4 39.8 14 32 39 50 63 25.0 29.1 30.9 33.2 37.6 11 15 20 35 45 19.6 20.4 21.7 24.6 26.8 15 23 33 50 15.6 17.0 19.1 22.0 D =0.9573 D =0.9390 D =0.8967 D =0.8429 t s t s t s t s 13 24 34 39 50 10 11.4 12.9 13.8 15.2 12 23 31 37 47 6.5 7.2 8.3 9.0 10.1 12 30 47 0.1 4.3 4.9 12 19 25 50 67 0.00 0.00 0.04 0.28 0.377 (Gerardin, A. ch. (4) 5. 142.) Solubility in dil. alcohol of x% by weight at 15. % alcohol 10 20 30 40 60 80 Pts. BaCU, 2H 2 O 30.25 23.7 18.0 12.8 9.3 3.4 0.5 (Schiff, A. 118. 365.) Sol. in 6885-8108 pts. 99.3% alcohol at 14.5, and in 1857 pts. at ebullition. (Frese- nius.) Solubility of BaCl 2 in alcohol +Aq. t alcohol Cr/ BaCb Solid phase 30 32.67 50.16 66.72 92.53 94.83 94.75 94.60 97.14 98.17 99.41 27.95 10.63 5.68 2.23 0.05 0.07 0.05 0.07 '6^08 BaCl 2 .2H 2 O ii ii ii BaCl 2 .2H 2 0+BaCl 2 .H 2 <( . t( BaCl 2 .H 2 O BaCl 2 .H 2 O+BaCl 2 BaCl 2 60 16.68 34.10 66.02 88.55 90.11 90.39 93.95 31.57 20.16 13.21 2.82 0.25 0.09 BaCl 2 .2H 2 O u II (t n BaCl 2 .2H 2 0+BaCl 2 .H 2 ti BaCl 2 .H 2 O ..... (Schreinemakers and Massink, Chem. Weekbl. 1910, 7. 213.) 100 pts. absolute methyl alcohol dissolve 2.18 pts. BaCl 2 at 15.5, and 7.3 pts. BaCl 2 , 2H 2 O at 6. (de Bruyn, Z. phys. Ch. 10. 783.) At 15 C. 1 pt. by weight is sol. in: 78 pts. methyl alcohol of sp. gr. 0.790 7,000 " ethyl " " " " 0.8035 100,000 " propyl " " " " 0.8085 (Rohland, Z. anorg. 1897, 15. 413.) Absolutely insol. in boiling amyl alcohol. (Browning, Sill. Am. J. 144. 459.) Absolutely insol. in acetic ether. (Cann. C. R. 102. 363.) Very si. sol. in acetone. (Krug and M'El- roy, J. Anal. Ch. 6. 184.) 100 pts. by weight of glycerine dissolve 10 pts. BaCl 2 at 15.5. (de Bruyn, Z. phys. Ch. 10. 783.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) (Eidmann, C. C. 1899, II. 1014.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in anhydrous pyridine, 97% pyri- dine +Aq. and 95% pyridine -f Aq. SI. sol. in 93% pyridine +Aq. (Kahlenberg, J. Am. Chem. Soc. 1908, 30. 1107.) +H2O. Solution of monohydrate sat. at 6 contains 31.57% BaCl 2 . (Schreinemakers, Chem. Weekbl. 1910, 7. 213.) 2.5 grams of the monohydrate are sol. in 100 cc. of methyl alcohol at 14. (Kirschner, Z. phys. Ch. 1911, 76. 176.) Exact solubility in methyl alcohol cannot be determined as BaCl 2 +H 2 O separates out from a sat. solution of the dihydrate. (Kirsch- ner, Z. phys. ch. 1911, 76. 177.) Barium cadmium chloride, BaCl 2 ,CdCl 2 + 4H 2 O. Easily sol. in H 2 O. (v. Hauer.) BARIUM MERCURIC CHLORIDE Solubility in H 2 O at t. t- 100 pts. solution contain pts. 100 g. of solution contain g. salt 100 g. H 2 O dissolve g. salt 100 mols. H 2 dissolve mols. of anhydrous salt Cl Ba Cd 22.5 15.19 14.71 11.98 41.88 72.06 3.32 32.9 16.18 16.09 12.40 44.59 80.73 3.72 41.4 16.95 16.81 13.05 46.87 88.01 4.06 53.4 18.21 18.13 13.95 50.30 101.21 4.66 62.0 18.81 18.74 14.73 52.28 109.56 5.05 97.8 22.48 22.00 17.57 62.05 163.50 7.53 108.3 23.51 22.79 18.53 64.83 184.33 8.49 109.2 23.69 29.95 18.67 65 .,31 188.27 8.67 (Rimbach, B. 1897, 30. 3083.) BaCl 2 .2CdCl 2 +5H 2 O. Quite difficultly sol. in H 2 O. (v. Hauer.) Solubility in H 2 at t. t 100 pts. by wt. of solution contain pts. by wt. 100 g. of solution contain g. salt 100 g. H 2 O dissolve g. salt 100 mols. H 2 dissolve mols. of anhydrous salt Cl Ba Cd 22.6 41.3 53.9 62.2 69.5 107.2 107.2 16.89 18.15 18.78 19.66 20.18 23.31 23.16 11.00 11.77 12.41 12.83 13.09 14.87 14.93 17.71 19.22 19.85 20.59 21.20 24.11 24.39 45.60 49.14 51.04 53.08 54.47 62.29 62.48 83.82 96.62 104.25 113.13 119.64 165.18 166.53 2.63 3.03 3.27 3.55 3.76 5.19 5.23 (Rimbach, B. 1897, 30. 3083.) Barium mercuric chloride, basic, BaCl 2 , HgO +6H 2 O. Decomp. by H 2 0. (Andre, C. R. 104. 431.) Barium mercuric chloride, BaCl 2 , 2HgCl 2 + 2H 2 O. Efflorescent in dry air; sol. in H 2 O. (v, Bonsdorff, Pogg. 17. 130.) The salt BaCl 2 , 2HgCl 2 +2H 2 O described by Bonsdorff does not form under the conditions which he gives. (Foote, Am. Ch. J. 1904, 32. 251.) BaCl 2 ,3HgCl 2 +6H 2 O. Solubility deter- minations with mixtures of BaCl 2 and HgCl show that these chlorides do not form a double salt at 25, but that a transition temp, exists at about 17.2 below which the salt BaCl 2 , 3HgCl 2 +6H 2 O forms. (Foote, Am. Ch. J. 1904, 32. 251.) +8H 2 O. Less sol. in H 2 than the Sr and Mg double salts. (Swan, Am. Ch. J. 1898, 20. 633.) Barium rhodium chloride, 3BaCl 2 , Rh 2 Cl 6 . See Chlororhodite, barium. Barium stannous chloride, BaCl 2 , SnCl 2 + 4H 2 0. Sol. in H 2 O. (Poggiale, C. R. 20. 1183.) Barium stannic chloride. See Chlorostannate, barium. Barium uranium chloride, BaCl 2 ,UCl 4 . Decomp. by H 2 O. (Aloy, Bull. Soc. 1899, (3) 21. 265.) Barium zinc chloride, BaCl 2 , ZnCl 2 +4H 2 O. Deliquescent, and sol. in H 2 O. (Warner, C. N. 27. 271.) Pptd. from warm solution only. (Ephraim, Z. anorg. 1910, 67. 381.) +2^H 2 O. Pptd. from cold solution. (Ephraim.) Barium chloride hydrazine, BaCl 2 , 2N 2 H 4 . Hydroscopic. (Franzen, Z. anorg. 1908, 60. 290.) Barium chloride hydroxylamine, BaCl 2 , 2NH 2 OH. Very sol. in H 2 O. (Crismer, Bull. Soc. (3) 3. 118.) Barium chloride sulphuric anhydride, BaCl 2 , 2S0 3 . Decomp. by H 2 O. (Schultz-Sellack, B. 4. 113.) Barium chlorofluoride, BaClF. Difficultly sol. in H 2 O, but much more sol. than BaF 2 . Decomp. by H 2 O, so that when washed on filter, the nitrate contains more BaCl 2 than BaF 2 . (Berzelius, Pogg. 1. 19.) Insol. in and undecomp. by boiling alcohol; sol. in cone. HC1 and HNOs. Decomp. by hot H 2 0, hot H 2 SO 4 , dil. acetic acid, dil. HC1 or dil. HNO 3 . (Defacqz, C. R. 1904, 138. Barium cyanamide, BaCN 2 . Decomp. by H 2 O. (Frank, C. C. 1902, II. 774.) BARIUM HYDROXIDE 87 Barium sw&fluoride sodium fluoride, BaF, NaF. Decomp. by H 2 O. (Guntz, C. R. 1903, 136. 750.) Barium fluoride, BaF 2 . Scarcely sol. in H 2 O (Berzelius) ; less sol. in H 2 O than CaF 2 . 1 liter H 2 O dissolves 1630 mg. BaF 2 at 18. (Kohlrausch, Z. phys. Ch. 1904, 60. 356.) 1605 mg. are contained in 1 1. of sat. solu- tion at 18. (KohJrausch, Z. phys. Ch. 1908, 64. 168.) Insol. in molten MnCl 2 , MnBr 2 , MnI 2 , MnCl 2 +BaCl 2 , MnBr 2 +BaBr 2 and MnI 2 + BaI 2 . (Defacqz, A. ch. 1904, (8) 1. 350.) Easily sol. in HC1, HNO 3 , or HF+Aq. (Gay-Lussac and Thenard.) SI. sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Sol. in an aqueous solutio'n of sodium cit- rate. (Spiller.) Barium tin (stannic) fluoride. See Fluostannate, barium. Barium tellurium fluoride, BaF 2 , 2TeF 4 . Decomp. by H 2 O. (Hogbom, Bull. Soc. (2) 35. 60.) Barium titanium fluoride. See Fluotitanate, barium. Barium titanyl fluoride, TiO 2 F 2 , BaF 2 . See Fluoxypertitanate and fluoxytitanate, barium. Barium uranyl fluoride. See Fluoxyuranate, barium. Barium vanadyl fluoride. See Fluoxyvanadate, barium. Barium zirconium fluoride, 3BaF 2 , 2ZrF 4 + 2H 2 O. Insoluble precipitate. (Marignac.) See also Fluozirconate, barium. Barium fluoiodide, BaF 2 , BaI 2 . Decomp. by H 2 O, dil. HC1, dil. HNO 3 or hot H 2 SO 4 . Sol. in HI and HNO 3 . Insol. in and undecomp. by boiling alcohol. De- comp. by dil. acetic acid. (Defacqz, C. R. 1904, 138. 199.) Barium hydride, BaH. Decomp. by H 2 O or HCl+Aq. (Winkler, B. 24. 1979.) Decomp. by H 2 0. (Guntz, C. R. 1901, 132. 964.) Barium hydrosulphide, BaS 2 H 2 . Easily sol. in H 2 O. Insol. in alcohol. +4H 2 O. Sol. in H 2 0, and the solution dis- solves S. (Veley, Chem. Soc. 49. 369.) 100 pts. H 2 O dissolve pts. BaO at t. "t Pts. BaO t Pts. BaO t Pts. BaO 5 10 15 20 25 1.5 1.75 2.22 2.89 3.48 4.19 30 35 40 45 50 55 5.0 6.17 7.36 9.12 11.75 14.71 60 65 70 75 80 18.76 24.67 31.9 56.85 90.77 Barium hydroxide, BaO 2 H 2 . 100 pts. cold H 2 O dissolve 5 pts. BaO 2 H 2 . boiling 50 (Davy.) 100 pts. H 2 O at 20 dissolve 3.45 pts. BaO. (Bineau, C. R. 41. 509.) 100 pts. H 2 O at 13 dissolve 2.86 pts. BaO. 47 " 13.3 70 " 17.9 (Osann.) (Rosenthiel and Ruhhnann, J. B. 1870. 314.) 100 pts. H 2 O dissolve at 25 55.08 millimols. Ba 2 2H2> (Herz and Knoch, Z. anorg. 1904, 41. 315.) Sp. gr. of BaO 2 H 2 +Aq. %BaO Sp. gr. %BaO Sp. gr. 30 19 2.6 1.6 1.3 1.03 1.8 0.9 1.02 1.01 (Dalton.) Sp. gr. of Ba0 2 H 2 -f Aq at 18 containing 1.25% BaO 2 H 2 = 1.0120; containing 2.5% = 1.0253. (Kohlrausch, W. Ann. 1879, 6. 41.) Sp. gr. of BaO 2 H 2 +Aq at 80. Sp. gr. % BaO 2 H 2 by volume BaOzHz by weight Sp. gr. % Ba0 2 H 2 by volume % BaO 2 H 8 by weight .514 58.22 38.45 1.219 24.53 20.12 .500 56.31 37.54 1.200 23.00 19.17 .479 54.14 36.60 1.195 22.15 18.53 .458 49.38 33.87 1.174 19.83 16.89 .450 48.90 33.72 1.152 17.78 15.43 .413 45.99 32.55 1.129 16.01 14.18 .400 45.00 32.14 1.125 15.80 14.04 .390 44.22 31.81 1.114 14.56 13.07 1.375 42.40 30.84 1.100 13.06 11.87 1.368 41.45 30.30 1.076 10.58 9.83 1.350 38.60 28.59 1.062 9.16 8.62 1.338 37.30 27.88 1.049 7.55 7.20 1.312 35.02 26.69 .040 6.51 6.26 1.301 34.02 26.13 .031 5.18 5.02 1.278 31.48 24.67 .022 4.78 4.67 1.249 28.14 22.52 .015 3.90 3.84 1.236 26.41 21.36 .009 3.37 3.34 (Haff, C. N. 1902, 86. 284.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) More sol. in NaCl+Aq, KNO 3 +Aq, or NaNO 3 +Aq than in H 2 O. (Karsten.) Not precipitated by alcohol. 88 BARIUM HYDROXIDE Sol. with combination in absolute alcoho J 1 -]_.,, J-l 1 -1--T--1 T 1 i_ B.-pt. of Ba0 2 H 2 .8H 2 O+Aq, etc. Continued. and anhydrous ether. meunyi aiuonoi. iiisoi. m Bpt. Time %BaO Insol. in acetone. (Naumann, B. 1904, 37. 108 19' e;7 40 4329; Eidmann, C. C. 1899, II. 1014.) JLUO 108.5 JL0 U i . Ttt7 58.74 SolubHity in acetone +Aq at 25. 109 13' 61.44 A = cc. acetone in 100 cc. acetone -f-Aq 109 17' 40" 63.65 Ba0 2 H 2 imols. Ba0 2 H 2 in 100 cc. of 108 105 17' 50" 18' 66.53 67.51 2 the solution. 100 18' 45" 68.17 S = sp. gr. of the solution. (Bauer, Z. anorg. 1905, 47. 407.) A BaO 2 H 2 s Solubility in Ba(N0 3 ) 2 +Aq at 25. 2 Solution sat. with respect to both Ba(NOa) 2 55.08 1.04790 and BaO 2 H 2 , 8H 2 O. 10 31.84 1.01677 _ _. 20 30 A f\ 17.79 9.10 0.99268 0.97630 Sp. gr. 25/25 g. .03,0 is Ba(OH) 2 in 100 g. H 2 O g. Ba (NOs)s in 100 g. H 2 O 40 50 4.75 1.54 0.95605 0.93980 1.1448 5.02 11.48 60 0.48 0.91790 1.1371 . 4.93 10.21 70 0.08 0.89562 1.1288 4.83 8.66 1 . 1220 4.72 7 55 (Herz, Z. anorg. 1904, 41. 321.) 1.1133 4>2 7^01 BaO 2 H 2 is sol. in an aqueous solution of cane sugar (Hunton, Phil. Mag. (3) 11. 156) ; also in an aqueous sol. of mannite (Favre, A. ch. (3) 11. 76); sorbine (Pelouze); hot solu- tion of quercite, separating on cooling (Des- 1.1062 1.1044 1.1010 1.0975 1.0949 1.0937 4.65 4.61 4.64 4.60 4.55 4.54 6.82 6.55 6.08 5.66 5.46 5.32 saignes) . +3H 2 O. Decomp. by H 2 O free from car- bonic acid. SI. sol. in alcohol and ether. (Bauer, Z. anorg. 1905, 47, 416.) Solubility in H 2 O the same as that of the comp. with 8H 2 O. Insol. in alcohol and ether. (Bauer, Zeit. angew. Ch. 1903, 17. 341.) Nearly insol. in alcohol and ether. (Bauer, Zeit. angew. Ch. 1903, 16. 349.) 1.0885 1.0864 1.0840 1.0790 1.0774 1.0731 1.0711 1.0651 1/~lSO/j 4.52 4.53 4.52 4.48 4.46 4.40 4.42 4.35 4.44 4.41 4.04 3.47 3.14 2.79 2.53 1.88 +8H 2 O. Sol. in 20 pts. cold, and 3 pts. boiling H 2 (Graham); 17.5 pts. H 2 O at 15.5, and in all proportions of hot H 2 O. (Hope.) Sol. in 19 pts. H 2 O at 15, and 2 pts. .UO.JD 1.0640 1.0538 1.0512 4!35 4.29 4.29 1A5 0.43 at 100. (Wittstein.) If Ba0 2 H 2 +8H 2 is heated it dissolves in the crystal H 2 O and the solution has the (Parsons and Corson, J. Am. Chem. Soc. 1910, 32. 1385.) following bpts. %BaO 49.05 B.-pt. 103 50.05 52.43 53.72 104 105 106 Solubility of Ba(OH) 2 +8H 2 O (solid phase) in MCl+Aq (mol. per litre of solution) at 25. %BaO 55.35 57.49 58.74 61.44 Solution of (cr) (OHO B.-pt. 107 i n i n 5 ina BaO 2 H 2 +3H 2 separates at 109. (Bauer, LiCl 0.555 Zeit. angew. Ch. 1903, 17. 345.) (( ff 0.75 0.745 B.-pt. of BaO 2 H 2 .8H 2 0+Aq at 732 mm. Bpt. Time %BaO 78 (mpt.) 78 103 104 105 106 107 4' 6' 30" 6' 45" 7' 30" 9' 25" 10' 45" 48.45 48.45 49.05 50.05 52.43 53.72 55.35 BARIUM OXIDE 89 Solubility of BaO in NaOH+Aq at 30. Barium iodide, basic, Ba(OH)I+9H 2 O. % Na 2 O %BaO Solid phase See Barium oxyiodide. 4.99 BaO. 9H 2 O Barium bismuth iodide, BaI 2 , 2BiI 3 + 18H 2 O. 4.78 64Q 1.29 OCQ (( Deliquescent; decomp. by H 2 O. (Linau, . TrO 9.63 . oy 0.57 u Pogg. 111. 240.) 11.62 0.53 a Barium cadmium iodide, BaI 2 , CdI 2 +5H 2 O. 17.87 23.28 0.47 1.06 a (t Deliquescent. (Croft.) 24.63 .87 BaO . 9H 2 O -fBaO . 4H 2 O Barium mercuric iodide, BaI 2 , 2HgI 2 . 26.14 27.72 OQ 4.0 .84 .75 KO BaO. 4H 2 O 14 (( Decomp. by much H 2 O. (Boullay.) BaI 2 , HgI 2 . Sol. in H 2 O. (Boullay.) o . 1C 29.24 32.12 34.72 41.09 . Oo .34 0.82 0.59 0.57 Ba0.4H 2 O+BaO.2H 2 O BaO.2H 2 O a BaO.2H 2 O+NaOH.H 2 O Sp. gr. of sat. solution = 3.575-3.588. (Rohrbach, W. Ann. 20. 169.) +5H 2 O. (Duboin, C. R. 1906, 143. 314.) 2BaI 2 , 3HgI 2 +16H 2 O. (Duboin, C. R. 1906, 142. 888.) 42 NaOH.H 2 BaI 2 , 5HgI 2 +8H 2 O. As the corresponding (Schreinemakers, Z. phys. Ch. 1909, 68. 84.) 50% alcohol dissolves less than 0.5% oJ Ca salt. (Duboin, C. R. 1906, 142. 888.) 3BaI 2 , 5HgI 2 +21H 2 0. Very deliquescent. (Duboin, C. R. 1906, 142. 889.) its wt. of BaO 2 H 2 +8H 2 O. (Beckmann, J pr. 1883, (2) 27. 138.) Barium sw&iodide sodium iodide, Bal, Nal, Decomp. by H 2 0. (Guntz, C. R. 1903, 136. 750.) Barium iodide, BaI 2 . Not deliquescent. Very sol. in H 2 O and alcohol. 100 pts. of anhydrous salt dissolve: atO 19.5 30 40 60 90 106 in 59 48 44 43 41 37 35 pts. H 2 O. (Kremers, Pogg. 103. 66.) Sp. gr. of BaI 2 +Aq containing: 5 10 15 20 25 30%BaI 2 1.045 1.091 1.143 1.201 1.265 1.333 35 40 45 50 55 60%BaI 2 . 1.412 1.495 1.596 1.704 1.825 1.970 (Kremers, Pogg. 111. 63, calculated by Ger- lach, Z. anal. 8. 279.) Easily sol. in alcohol. (Henry.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in acetone. (Naumann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) +2H 2 0. At 15 C., 1 pt. by weight in sol. in: 22 pts. methyl alcohol sp. gr. 0.790 93 " " " " " 0.8035 307 " " " " " 0.8085 (Rohland, Z. anorg. 1897, 15. 413.) +7H 2 O. (Thomson, B. 10. 1343.) The composition of the hydrates formed by BaI 2 at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by BaI 2 and of the conduc- tivity and sp. gr. of BaI 2 +Aq. (Jones, Am. Ch. J. 1905, 34. 306.) Barium stannous iodide. Very sol. in H 2 O. (Boullay.) Barium zinc iodide, BaI 2 , 2ZnI 2 . Deliquescent, and sol. in H 2 O. (Rammels- berg.) +4H 2 O. Very hydroscopic. (Ephraim, ery , 67. Z. anorg. 1910, 67. 385.) Barium nitride, Ba 3 N 2 . Decomp. H 2 O violently, not alcohol. (Ma- quenne, A. ch. (6) 29. 219.) BaN 6 . See Barium azoimide. Barium oxide, BaO. Sol. in H 2 O with evolution of heat. Easily sol. in dil. HNO 3 , or HCl+Aq. Solubility in NaOH+Aq. See Barium lydroxide. Solubility in Na 2 O, HC1, +H 2 O at 30. Schreinemakers, Z. phys. Ch. 1909, 68. 98.) Solubility in Na 2 O, NaCl, BaCl 2 +Aq at 50. (Schreinemakers.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 898, 20. 827.) Sol. with combination in absolute alcohol and anhydrous wood-spirit. Insol. in ether. Easily sol. in absolute methyl alcohol. 1 1. absolute ethyl alcohol sat. with BaO at 9 contains 213.8 g. BaO. (Berthelot, Bull. Soc. 8. 389.) Sol. in methyl alcohol. (Neuberg and STeimann, Biochem. Z. 1906, 1. 173.) Insol. in acetone. (Eidmann, C. C. 1899, I. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 909, 42. 3790.) See also Barium hydroxide. Jarium peroxide, BaO 2 . Insol. in H 2 O; decomp. by boiling H 2 0. 90 BARIUM OXYBROMIDE Sol. in acids with formation of hydrogen dioxide. Forms hydrate with 8H 2 O; also 10H 2 O (Berthelot, A. ch. (5) 21. 157); also a com- pound BaO 2 , H 2 O 2 , which is very unstable, si. sol. in cold H 2 O, and insol. in alcohol or ether. (Schone, A. 192. 257.) +8H 2 O. 100 cc. pure H 2 O dissolve 0.168 g. BaO 2 +8H 2 0; if H 2 O contains 0.3 g. Ba(OH) 2 +8H 2 O, only 0.102 g. BaO 2 +8H 2 are dissolved; if 0.6 g. Ba(OH) 2 +8H 2 only 0.019 g. BaO 2 +8H 2 O are dissolved. (Schone, A. 1878, 192. 266.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Barium oxybromide, Ba(OH)Br+2H 2 0. Decomp. by H 2 O. (Beckmann, J. pr. (2) 27. 132.) BaBr 2 ,BaO +5H 2 O. SI. sol. in H 2 O. (Tas- silly, C. R. 1895, 120. 1340.) Barium oxychloride, Ba(OH)Cl+2H 2 O. Decomp. by H 2 O. (Beckmann, J. pr. (2) 26. 388, 474.) Barium mercury oxychloride, BaCl 2 , HgO-f 6H 2 0. Decomp. by H 2 0. (Andre, C. R. 104. 431.) Barium oxyiodide, Ba(OH)I+9H 2 O. Decomp. by H 2 O and alcohol. (Beckmann, B. 14. 2154.) BaI 2 ,BaO+9H 2 O. SI. sol. in H 2 O. (Tas- silly, C. R. 1895, 120. 1340.) Barium oxysulphides, Ba;O 4 S3+58H 2 O, Ba 2 OS + 10H 2 O, Ba 4 OS 3 +28H 2 O. Very unstable; decomp. by recrystalliza- tion into BaS 2 H 2 and BaO 2 H 2 . Barium phosphide, BaP 2 . Decomp. by H 2 O. (Dumas, A. ch. 32. 364.) Ba 3 P 2 . Crystallized. Sol. in dil. acids; insol. in cone, acids; decomp. by H 2 O. Insol. in organic solvents at ord. temp. (Jaboin, C. R. 1899, 129. 765.) Barium selenide, BaSe. Sol. in H 2 O with decomp. SI. sol. in H 2 O. (Favre, C. R. 102. 1469.) Barium silicide, Ba 2 Si. (Jungst, C. C. 1906, I. 195.) BaSi 2 . Slowly decomp. by H 2 O, not by NH 4 OH+Aq. Rapidly decomp. by cone. NaOH. Sol. in HNO 3 , H 2 SO 4 and H 3 PO 4 with evolution of spontaneously inflammable gas. Sol. in HF and HC1. Sol. in acetic acid without evolution of gas. (Moissan, Traite ch. min. 1904, III. 680.) Decomp. rapidly in both hot and cold H 2 O. (Bradley, C. N. 1900, 82. 150.) Barium sulphide, BaS. Sol. in H 2 O with decomp. Crystallized. Decomp. by H 2 O. Attacked by cold cone. HNO 3 . (Mourlot, A. ch. 1899, (7) 17. 521.) Cryst. modification is less readily acted on by air and other reagents than the amorphous modification; sol. in fuse oxidizing agents. (Mourlot, C. R. 1898, 126. 645.) +H 2 O. (Neuberg and Neimann, Biochem. Z. 1906, 1. 174.) +6H 2 O. Slowly sol. in boiling H 2 O, with decomp.; insol. in, but decomp. by boiling alcohol. (Schone.) Barium sulphide, Ba 4 S 7 +25H 2 O (?). Sol. in H 2 O. (Schone, Pogg. 112. 215.) Barium bisulphide, BaS 3 . Sol. in large amount of boiling H 2 O. (Schone, Pogg. 112. 215.) Barium tefrasulphide, BaS 4 +H 2 O. Easily sol. in H 2 O, especially if hot; sol. in 2.42 pts. H 2 O at 15; insol. in CS 2 or alcohol. (Schone, Pogg. 112. 224.) +2H 2 O. (Veley, Chem. Soc. 49. 369.) Barium pentasulphide, BaS 6 . Known only in solution. Barium mercuric sulphide, BaS, HgS+5H 2 O. Sol. in H 2 O. (Wagner, J. pr. 98. 23.) Barium nickel sulphide, BaS, 4NiS. Sol. in warm cone. HC1. (Bellucci, C. A. 1909, 293.) Barium stannic sulphide. See Sulphostannate, barium. Barium uranyl sulphide, 6BaS, U0 2 S + Decomp. by HCl+Aq. (Remele", Pogg. 124. 159.) - Baryta. See Barium oxide, BaO. Beryllium, Be. For beryllium and its salts, see Glucinum and the corresponding salts. Bismuth, Bi. Not attacked by H 2 0. Very slowly at- tacked by HCl+Aq (Troost). Very si. sol. in cone. HCl+Aq (Schiitzenberger, Willm). Not attacked by dil. HCl+Aq (Naquet and Hanriot). Very slowly attacked by cold HC1 +Aq (Godeffroy). According to very careful experiments pure Bi is absolutely unattacked by hot or cold, dil. or cone. HCl+Aq except in presence of oxygen. (Ditte and Metzner, A. ch. (6) 29. 397.) Not attacked by dil. H 2 SO 4 +Aq. Decomp. BISMUTH POTASSIUM CHLORIDE 91 by hot cone. H2SO4. Easily sol. in dil. or cone. HNO 3 +Aq, or aqua regia. Not attacked by pure HNO 3 +Aq of 1.52 to 1.42 sp. gr. at 20; violently attacked by a more dil. acid, but the acid becomes concen- trated thereby. Cone. HNO 3 +Aq attacks only by heating or adding NO2. (Millon, A. ch. (3) 6. 95.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) l /2 ccm. oleic acid dissolves 0.0091 g. Bi in 6 days. (Gates, J. phys. Chem. 1911, 16. 143.) Bismuth arsenide, Bi 3 As 4 . (Descamp, C. R. 86. 1065.) Bismuth dibromide, Bi 2 Br 4 . Not known in a pure state. (Weber, Pogg. 107. 599.) Bismuth inbromide, BiBr 3 . Very deliquescent. Decomp. by H 2 O. Sol. in alcohol or ether. Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 27.) Bismuth hydrogen bromide, BiBr 3 , 2HBr+ 4H 2 O. Deliquescent. Decomp. in the air. (Aloy, Bull. Soc. 1906, (3) 35. 398.) Bismuth caesium bromide, 2BiBr 3 , 3CsBr. Ppt. Insol. in HBr. Sol. in HC1 and in HN0 3 . (Hutchins, J. Am. Chem. Soc. 1907, 29. 33.) Bismuth potassium bromide, BiBr 3 ,2KBr. Decomp. by H 2 O. (Aloy, Bull. Soc. 1906, (3) 35. 398.) Bismuth bromide ammonia, BiBr 3 , 3NH 3 . Sol. in HCl+Aq. BiBr s , 2NH 3 (?). 2BiBr 3 , 5NH 3 . Not deliquescent; not de- comp. by H 2 O; easily sol. in dil. acids. (Muir, Chem. Soc. 29. 144.) Bismuth bromide potassium chloride, Decomp. by H 2 O. (Atkinson, Chem. Soc. 43.289.) ,:;. Bismuth ^'chloride, Bi 2 Cl 4 . Very deliquescent. Decomp. by H 2 O, dil. acids, or cone. NH 4 Cl+Aq. (Weber, Pogg. 107. 596.) Bismuth trichloride, BiCl 3 . Deliquescent. Decomp. by H 2 O. Sol. in dil. HCl+Aq, and alcohol. Not decomp. by H 2 O in presence of citrates. (Spiller.) 0.08 g. sol. in 100 ccm. liquid H 2 S. (An- tony, C. C. 1905, I. 1692.) Moderately sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) 1 g. Bids is sol. in 5.59 g. acetone at 18. Sp. gr. of sat. solution 18/4 = 0.9194. (Nau- mann, B. 1904, 37. 4331.) Sol. in acetone and in methylal. (Eidmann, C. C. 1899, II. 1014.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in ethyl acetate. (Naumann, B. 1910. 43. 314.) 1 pt. is sol. in 60.36 pts. ethyl acetate at 18. Sp. gr at 18/40 = 0.9106. (Naumann, B. 1910, 43. 320.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Bismuth chloride, Bi 3 Cl 8 (?). Decomp. by H 2 O. (Dehe*rain, C. R. 54. 724.) Bismuth hydrogen chloride, 2BiCl 3 , HC1+ 3H 2 O. Not deliquescent. Decomp. by H 2 O. (Engel, C. R. 106. 1797.) Bids, 2HC1. (Jacquelain, A. ch. (2) 62. 363.) Bismuth caesium chloride, BiCl 3 , 3CsCl. Decomp. by H 2 O. SI. sol. in cold dil. HC1+ Aq, but easily sol. on warming. (Brigham, Am. Ch. J. 14. 181.) 2BiCl 3 , 3CsCl. As above. (Brigham.) BiCl 3 , 6CsCl. Easily sol. in H 2 O and dil. HCl+Aq. (Godeffroy, B. 8. 9.) Does not exist. (Brigham.) Bismuth hydrazine chloride, BiCl 3 , 3N 2 H 4 HC1. Sol. in acids, from which it is pptd. by H 2 O. (Ferratini, C. A. 1912. 1613.) Bismuth nitrosyl chloride, BiCl 3 , NOC1. Very deliquescent. Decomp. by H 2 O. (Sudborough, Chem. Soc. 50. 662.) Bismuth potassium chloride, BiCl 3 , KC1+ H 2 0. Decomp. by H 2 O. Cannot be recryst. ex- cept from cone. BiCl 3 +HCl. Decomp. by HCl+Aq into BiCl 3 , 2KC1+2H 2 O. (Brig- ham, Am. Ch. J. 14. 167.) BiCl 3 , 2KC1. Decomp. by H 2 O. (Arppe, Pogg. 64. 37.) Deliquescent. Sol. in H 2 O with decomp. into the oxy- chloride when excess H 2 O is used. (Aloy, Bull. Soc. 1906, (3) 35. 397.) +2H 2 O. Decomp. by H 2 O. (Jacquelain, J. pr. 14. 1.) Sol. in moderately cone. HCl+Aq. BiCl 3 , 3KC1. Decomp. by H 2 O. (Arppe.) Does not exist. (Brigham.) 92 BISMUTH RUBIDIUM CHLORIDE Bismuth rubidium chloride, BiCl 3 , RbCl+ H 2 0. Decomp. by H 2 O; sol. in dil. HCl+Aq, from which BiCl 3 , 3RbCl crystallizes. (Brig- ham, Am. Ch. J. 14. 174.) BiCl 3 , SRbCl. Decomp. by H 2 O ; sol. in dil. HCl+Aq without decomp. (Brigham.) BiCl 3 , 6RbCl. Decomp. by H 2 O*; sol. in HCl+Aq (Godeffroy, B. 8. 9); does not exist. (Brigham.) lOBiCls, 23RbCl (?). As above. (Brig- ham.) Bismuth sodium chloride, BiCl 3 , 2NaCl+ H 2 0. +3H 2 O. Decomp. by H 2 O. (Arppe, Pogg. 64. 237.) BiCl 3 , SNaCl. Bismuth thallous chloride, BiCl 3 , 3T1C1. Ppt. (Ephraim, Z. anorg. 1909, 61. 254.) BiCl 3 , 6T1C1. Ppt. (Ephraim.) . Bismuth chloride ammonia, 2BiCl 3 , NH 3 . Stable. (Dene-rain, C. R. 64. 724.) BiCl,, 2NH 3 . (D.) BiCl 3 , 3NH 3 . (D.) Bismuth chloride nitric oxide, BiCl 3 , NO. Very hygroscopic. (Thomas, C. R. 1895, 121. 129.) Solubility of freshly pptd. Bi(OH) 3 in NaOH+Aq. g. NaOH per 1. g. Bi dissolved per 1. at 20 g. Bi dissolved per 1. at 100 400 320 240 200 160 120 80 40 20 0.16 0.11 0.11 0.10 0.08 0.07 0.04 trace 1.70 1.20 0.5 0.5 6^35 0.2 0.15 (Moser, Z. anorg. 1909, 61. 386.) Solubility of freshly pptd. Bi(OH) 3 in KOH+Aq. KOH per 1. g. g. Bi dissolved per 1. at 20 g. Bi dissolved per 1. at 100 560 448 336 280 224 168 112 56 28 0.14 0.11 0.11 0.10 0.08 0.06 0.03 trace 1.65 1.20 0'.5 0.5 o!3' 0.2 0.15 (Moser, Z. anorg. 1909, 61. 386.) Bismuth chloride nitrogen peroxide, BiCl 3 , N0 2 . Decomp. by moist air, but stable in dry air. (Thomas, C. R. 1896, 122. 612.) Bismuth chloride selenide. See Bismuth selenochloride. Bismuth Zn'fluoride, BiF 3 . Insol. in H 2 or alcohol. (Gott and Muir, Chem. Soc. 53. 138.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Bismuth hydrogen fluoride, BiF 3 , 3HF. Deliquescent. Decomp. by boiling H 2 (Muir, Chem. Soc. 39. 21.) Bismuth gold, Au 3 Bi. Insol. in equal pts. of HNO 3 and tartaric acids. (Roessler, Z. anorg. 1895, 9. 71.) Bismuthous hydroxide, Bi(OH) 3 . Sol. in strong acids. Insol. in solutions of alkalies, alkali carbonates, (NH 4 ) 2 CO 3 , or NH 4 NO 3 ; or of amyl amine (Wurtz). When recently pptd. is sol. in NH 4 Cl+Aq, but insol. in NH 4 NO 3 +Aq (Brett, 1837). Not 'pptd. in presence of Na citrates (Spiller). Bi 2 O 3 , 2H 2 0. Bi 2 O 3 , H 2 O. (Muir, Chem. Soc. 32. 131.) See also Bismuth Znoxide. ;, Bi 2 O 4 , H 2 O. Bi 2 O 4 , 2H 2 O. (Wernicke, Pogg. 141. 109.) Bismuthic hydroxide (Bismuthic acid), Bi 2 O 5 , H 2 O. Insol. in H 2 O; easily decomp. by acids. (Fremy, A. ch. (3) 12. 495.) Decomp. by H 2 SO 4 ; not attacked by SO 2 +Aq; neither dissolved nor decomp. by dil. HNO 3 +Aq, but slowly converted into an allotropic modifica- tion (?). Partially decomp. by cone. HNO 3 . Slowly but wholly dissolved by hot cone. BNO 3 . SI. sol. in cone. KOH+Aq. (Arppe.) Sol. in about 100 pts. boiling KOH+Aq, so cone, that it solidifies on removing the lamp 'Muir, Chem. Soc. 51. 77.) 1 Bi-jO,,, 2H 2 O. (Bodeker, A. 123. 61.) Does not exist. (Hoffmann and Geuther.) Bismuth iodide, BiI 3 . Not attacked by cold H 2 O, but by boiling, BiOI is formed. 100 pts. absolute alcohol dissolve 3^ pts. salt at 20. (Gott and Muir, ~!hem. Soc. 57. 138.) Sol. in HNO 3 , and HI+Aq, from which it TT O or alcohol. S(- ' ~ (Rammelsberg.) 3 , q, rom wc s repptd. by H 2 O or alcohol. Sol. in KI+Aq or KOH+Aq. BISMUTH OXIDE 93 SI. sol. in liquid NH 3 . (Franklin, Am. Ch. Bismuth Zn'oxide, Bi 2 O 3 . J. 1898, 20. 827.) 100 g. absolute alcohol dissolve 3.5 g. BiI 3 at 20. (Gott and Muir, Chem. Soc. 57. 138.) Insol. in H 2 O. Sol. in cone, acids. Solubility of Bi 2 O 3 in HNO 3 +Aq at 20. Sol. in acetone. (Naumann, B. 1904, 37. In 100 g. of the 4328.) liquid p! 100 pts. methylene iodide dissolve 0.15 pt. BiI 3 at 12, and very little more at higher Solid phase g. Bi 2 3 g. N 2 5 temperatures. (Retgers, Z. anorg. 3. 343.) Sol. in methyl acetate. (Naumann, B. 0.321 0.337 0.963 Q82 Bi 2 O 3 .N 2 O 5 .2H 2 O u 1909, 42. 3790.) 3^54 \J . t/O^ 4.68 (I Bismuth hydrogen iodide, BiI 3 , HI+4H 2 O. 6.37 13.67 7.17 12.50 a (Arppe, Pogg. 44. 248.) 14.85 13.31 II 18.74 15.90 Bi 2 O 3 .N 2 O 5 .H 2 O Bismuth caesium iodide, 3CsI,2BiI 3 . 23.50 19.21 a Very si. sol. in H 2 O. (Wells, Am. J. Sci. 23.50 19.29 (( 1897, (4) 3. 464.) 27.15 20.96 ei 28.11 21 . 64 Bismuth calcium iodide, 2BiI 3 , CaI 2 + 18H 2 O. 29.50 22.53 a Deliquescent; decomp. by H 2 O. (Linau, 30.19 22.90 (1 Pogg. 111. 240.) 31.48 . 23.70 a 32.93 24.83 |Bi 2 O 3 .N 2 O 5 .H 2 O+ Bismuth magnesium iodide, 2BiI 3 , MgI 2 + 32.80 24.86 {Bi 2 3 .3N 2 6 .10H 2 0. 12H 2 O. 32.67 24.70 Bi 2 O 3 .3N 2 O 5 .10H 2 O. Deliquescent; decomp. by H 2 O. (Linau, 32.59 24.60 a Pogg. 111. 240.) 32.24 24.68 (i 30.74 25.13 u Bismuth potassium iodide, BiI 3 , 4KI. 29.83 25.30 (( Ppt. (Arppe, Pogg. 44. 237.) 24.16 28.25 n BiI 3 , SKI. (Astre, C. R. 110. 1137.) 16.62 35.40 (i BiI 3 , 2KI. Sol. in acetic ether. (Astre.) 12.17 43.37 ( +4H 2 O. Sol. in small amt. H 2 O without 11.66 46.62 i pptn., but decomp. by much H 2 O. 11.19 49.38 t BiI 3 , 2KI, HI. (Arppe.) 11.19 50.20 t 2BiI 3 , 3KI+2H 2 O. (Astre.) BiI 3 ,KI+H 2 O. Decomp. by H 2 O. (Nickles, C. R. 61. 1097.) 2BiI 3 , KI. Sol. in acetic ether. (Astre.) 15.20 20.76 27.85 54.66 53.75 51.02 i (Bi 2 O 3 .3N 2 O 5 .10H 2 O+ Bi 2 O 3 .3N 2 O 5 .3H 2 O. , 8.58 68.28 Bi 2 O 3 .3N 2 O 5 .3H 2 O. Bismuth sodium iodide, BiI 3 , NaI+H 2 Q. 4.05 74.90 a Deliquescent; decomp. by H 2 O. (Nickles, (Rutten, Z. anorg. 1902, 30. 386.) C. R. 51. 1097.) 2BiI 3 , 3NaI + 12H 2 O. As above. (Linau, T* -I 4 H O A f\ \ Solubility of Bi 2 O 3 in HNO 3 +Aq at t. Pogg. 111. 240.) t %Bi 2 Os %N 2 O5 Solid phase Bismuth zinc iodide, 2BiI 3 , ZnI 2 +12H 2 O. Very deliquescent. (Linau, Pogg. 111. 240.) IF 20.8 24.02 17.1 19.1 Bi 2 O 3 .N 2 O 5 .H 2 O n Bismuth iodide ammonia, BiI 3 , 3NH 3 . 31.09 31.2 23.8 23.9 jBi 2 3 .N 2 O 5 .H 2 O+ jBi 2 O 3 .3N 2 O 5 .10H 2 O Decomp. by H 2 O. (Rammelsberg.) 30 34.2 26.5 ii Bismuth iodide zinc bromide. 28.2 29.6 Bi 2 O 3 .3N 2 O 5 .10H 2 O Sol. in H 2 O. (Linau, Pogg. 111. 240.) 16.1 47.7 u Bismuth nitride. 65 5.55 7.44 Bi 2 O 3 .N 2 5 .H 2 O Explosive. (Fischer, B. 1910, 43. 1471.) BiN. Ppt. ' Decomp. by H 2 O or dil. acids. 27.62 40.80 22.46 31.60 u Bi 2 O 3 . N 2 O 5 . H 2 O+Bi 2 O 3 . (Franklin, J. Am. Chem. Soc. 1905, 27. 847.) 3N 2 O 5 .10H 2 O 37.82 35.80 Bi 2 O 3 .3N 2 O 5 .10H 2 O Bismuth dioxide, Bi 2 2 . QK 7<3 A *7 AO (Bi 2 O 3 .3N 2 O 5 .10H 2 O + Sol. in cone. HNO 3 +Aq. Decomp. by OO . 4 O 4/ . UJ |Bi 2 O 3 .3N 2 O 5 .3H 2 O strong acids, and boiling KOH+Aq. 4.59 77.90 Bi 2 O 3 .3N 2 O 5 .3H 2 O Decomp. by H 2 O. (Tanatar, Z-. anorg. 1901, 27. 438.) (Rutten.) 94 BISMUTH OXIDE Solubility of Bi 2 O 3 in HNO 3 +Aq at t. Bismuth phosphide, BiP. (Cavazzi.) Bismuth /nselenide, Bi 2 Se 3 . Insol. in H 2 O, alkalies, or alkali sulphides +Aq; si. attacked by HCl+Aq; oxidized by HNO 3 +Aq. (Schneider, Pogg. 94. 628.) Min. Frenzelite. Bismuth potassium selem'de. See Selenobismuthite, potassium. Bismuth selenochloride, BiSeCl. Not attacked by H 2 O; very si. sol. in HC1+ Aq; easily and completely sol. with decomp. in HNO 3 +Aq. (Schneider.) Bismuth ^sulphide, Bi 2 S 2 +2H 2 O (?). Insol. in H 2 O. Decomp. by HCl+Aq. Bismuth Znsulphide, Bi 2 S 3 . Insol. in H 2 O. 1 1. H 2 O dissolves 0.35 x ICh 8 moles Bi 2 S 3 at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Easily sol. in moderately dil. HNO 3 +Aq, and cone. HCl+Aq, with separation of S. Insol. in alkalies, alkali sulphides, Na 2 S 2 O 3 , or KCN+Aq; insol. in NH 4 C1, or NH 4 NO 3 + Aq (Brett). Insol. in potassium thiocarbon- ate+Aq. (Rosenbladt, Z. anal. 26. 15.) Insol. in alkali hydroxides or alkali hydro- sulphides. Insol. in 2N-(NH 4 ) 2 S+Aq. 0.0090 g. Bi 2 S 3 is sol. in 100 cc. N-Na 2 S 2 + Aq at 25. (Knox, Chem. Soc. 1909, 95. 1764.) Somewhat sol. in Na 2 S+Aq. 75 cc. of Na 2 S+Aq (sp. gr. 1.06) dissolve an amt. of Bi 2 S 3 corresponding to 0.031 g. Bi 2 O 3 . (Still- man, J. Am. Chem. Soc. 1896, 18. 683.) t %Bi 2 Os %N 2 O 6 Solid phase 72 75 80 37.23 36.74 39.75 47.76 47.91 45.16 Bi 2 O3.3N 2 O5.4H 2 O (( u 9 20 30 50 64 65 75.5 ,72 31.2 32.8 34.2 36.9 40.6 40.8 45.4 45.9 23.9 24.8 26.4 28.9 31.1 31.6 34.6 35.6 Bi 2 O3.3N 2 5 .10H 2 O + Bi 2 O3.N 2 5 .H 2 O 11.5 20 50 65 25.36 27.85 32.22 35.73 52.57 51.02 49.29 47.02 } Bi 2 Os.3N 2 O 5 .10H 2 O + J Bi 2 O3.3N 2 O 5 .3H 2 O (i c( n (Rutten.) Solubility in NaOH+Aq at 25. Cone, of NaOH g. Bi 2 Os in 100 cc. of solution. Mol/l. Mean result. 1.0 0.0013^0.0002 2.0 0.0026^0.0002 3.0 0.00490.0005 (Knox, Chem. Soc. 1909, 95. 1767.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Min. Bismite. Easily sol. in HNO 3 +Aq. See also Bismuthous hydroxide. Sol. in cone. HCl+Aq, with evolution of Cl; in oxygen acids with evolution of O. Less easily sol. in cone. H 2 SO 4 than in HNO 3 , or HCl+Aq. Bismuth oxide, Bi 4 O 9 (?). (Hoffmann and Geuther.) Bismuth peroxide, Bi 2 O 6 . Sol. in dil. acids. Combines with H 2 O to form bismuthic hydroxide, which see. (Hase- broek, B. 20. 213.) Bismuth oxybromide, etc. See Bismuthyl bromide, etc. Bismuth palladium, PdBi 2 . Insol. in equal pts. HNO 3 and tartaric acids (Roessler, Z. anorg. 1895, 9. 70.) Bismuth platinum, PtBi 2 . Insol. equal pts. HNO 3 and tartaric acids (Roessler, Z. anorg. 1895, 9. 69.) Solubility in Na 2 S+NaOH+Aq at 25. Cone, of Na 2 S Mol/l Cone, of NaOH Mol./l. g. Bi 2 Ss in 100 cc. of solution 0.5 1.0 1.0 1.0 0.0185 0.0838 (Knox, Chem. Soc. 1909, 95. 1763.) Bismuth sulphide pptd. from acid solution is not dissolved by subsequent treatment with K 2 S+Aq. (Stone, J. Am. Chem. Soc. 1896, 18. 1091.) Sol. in K 2 S+Aq. (Ditte, C. R. 1895, 120. 187.) Solubility in K 2 S+KOH+Aq at 25. Cone, of K 2 S Mol./l. Cone, of KOH Mol./l. g. Bi 2 S 3 in 100 cc. of solution 0.5 1.0 1.25 1.0 1.0 1.25 0.0240 0.1230 0.2354 (Knox, Chem. Soc. 1909, 95. 1763.) BISMUTHYL FLUORIDE 95 Solubility in alkali sulphides +Aq at 25 C Alkali sulphide Cone, of alkali sulphide Mol. /I. g. BizSs in 100 cc. of solution Na 2 S 0.5 1.0 1.5 0.0040 0.0238 0.1023 K 2 S 0.5 1.0 1.25 0.0042 0.0337 0.0639 (Knox, Chem. Soc. 1909, 95. 1762.) Decomp. by FeCl 3 +Aq. (Cammerer, C. C. 1891, II. 525.) Insol. in KCN+Aq. (Hoffmann, A. 1884, 223. 134.) Min. Bismuthiniie. Easily sol. in HNO 3 + Aq. Bismuth cuprous sulphide, Bi 2 S 3 , Cu 2 S. Insol. in H 2 O. Sol. with decomp. in HNO 3 +Aq. (Schneider, J. pr. (2) 40. 564.) Min. Emplectonite. Bismuth potassium sulphide, Bi 2 S 3 , K 2 S. (Schneider, Pogg. 136. 460.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Bi 2 S 3 ,4K 2 S+4H 2 O. Decomp. by H 2 O. Very sol. in K 2 S-j-Aq. Efflorescent in dry air. (Ditte, C. R. 1895, 120. 186.) See also Sulphobismuthite, potassium. Bismuth silver sulphide, Bi 2 S 3 , Ag 2 S. Insol. in cold HC1, or HNO 3 . Sol. in warm HNO 3 with separation of S, in boiling HC1 with separation of H 2 S. Min. Plenargyrite, Matildite. (Schneider, J. pr. 1890, (2) 41. 414.) Bismuth sodium sulphide, Bi 2 S 3 , Na 2 S. (Schneider.) Bismuth sulphide telluride, Bi 2 S 3 , 2Bi 2 Te 3 . Min. Tetradymite. Sol. in HNO 3 with sepa- ration of S. Bi 2 S 2 , 2Bi 2 Te. Min. Joseite. As above. Bismuth sulphobromide, BiSBr 2 . (Muir and Eagles, Chem. Soc. 1895, 67. 91.) Bismuth sulohochloride, BiSCl. Insol. in H 2 O or dil. HCl-j-Aq. Sol. in cone. HC1, or HNO 3 +Aq. Decomp. by alkalies +Aq. (Schneider, Pogg. 93. 464.) , Bismuth sulphoiodide, BiSI. Not attacked by boiling H 2 O, and dil. acids. Decomp. by hot cone. HCl+Aq, and HNO 3 + Aq. KOH+Aq dissolves out I 2 . (Schneider, Pogg. 110. 114.) Bismuth telluride, Bi 2 Te 3 . Min. Tetradymite. Sol. in HNO 3 +Aq. See also Bismuth sulphide telluride. Bismuthic acid, HBiOs. See Bismuthic hydroxide. Potassium bismuthate, KBi0 3 . Sol. in H 2 O. (Arppe.) KH(BiO 3 ) 2 . Insol. in H 2 O. Not decomp. by boiling H 2 0. (Andre, C. R. 113. 860.) No salts of HBiO 3 can exist. (Muir and Carnegie, Chem. Soc. 51. 77.) Bismuthicotungstic acid. Ammonium bismuthicotungstate, 3(NH 4 ) 2 O, 2Bi 2 O 3 , 11WO 3 +10H 2 O. A yellow oil which dries to a yellow glass. (E. F. Smith, J. Am. Chem. Soc. 1903, 25. 1232.) Potassium bismuthicotungstate, 3K 2 O, 2Bi 2 3 ,l 1WO 3 + 15H 2 O. A yellow oil which dried to a pale yellow glass. (E. F. Smith, J. Am. Chem. Soc. 1903, 26. 1233.) Strontium bismuthicotungstate, 3SrO, 2Bi 2 O 3 ,llWO 3 +llH 2 O. A yellow wax, insol. in pure H 2 O, but sol. in H 2 O containing a few drops HNO 3 . (E. F. Smith, J. Am. Chem. Soc. 1903, 25. 1233.) Bismuthyl bromide, BiOBr. Insol. in H 2 O; sol. in moderately cone. HBr+Aq. Insol. in H 2 0. (Herz, Z. anorg. 1903, 36. 348.) Bi 8 O 9 Br 6 . Insol. in H 2 O; easily sol. in cone. HC1, or HNO 3 +Aq; less sol. in dil. HNO 3 +Aq. Bi u Oi 3 Br 7 . As the preceding comp. (Muir.) Bismuthyl chloride, BiOCl. Insol. in H 2 O or dil. acids. Sol. in cone. HC1, orHNO 3 +Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +H 2 O. (Heintz, Pogg. 63. 55.) +3H 2 O. (Phillips, Br. Arch. (1) 39. 41.) Bi 7 O 9 Cl 3 . (Arppe.) Bi0 2 Cl 3 . Insol. in H 2 O; sol. in hot HC1, or HNO 3 +Aq. (Muir.) Bismuthyl fluoride, BiOF. Insol. in H 2 O; sol. in HC1, HBr, or HI-f-Aq. (Gott and Muir, Chem. Soc. 33. 139.) BiOF, 2HF. Insol. in H 2 O. 96 BISMUTHYL IODIDE Bisinuthyl iodide, BiOI. Not decomp. by HsO or alkaline solutions Sol. in HCl+Aq. Decomp. by HNO 3 +Aq (Schneider, J. pr. 79. 424.) Insol. in KC1, or KI+Aq. 3BiOI,7Bi 2 O 3 . Sol. in dil. HC1; decomp by HNO 3 ; insol. in boiling H 2 and alkali (Blyth, C. N. 1896, 74. 200.) BiI 3 , 5Bi 2 O 3 . Ppt. SI. sol. in HC 2 H 3 O 2 + Aq. Not decomp. by H 2 O. (Fletcher anc Cooper, Pharm. J. (3) 13. 254.) 4BiI 3 , 5Bi 2 O 3 . Easily sol. in HCl+Aq Decomp. by HNO 3 +Aq. SI. attacked by H 2 SO 4 ; somewhat sol. in H 2 C 4 H 4 O 6 , anc KHC 4 H 4 O 6 +Aq. Sol. in (NH 4 ) 2 S, and KOH+Aq. (Storer's Diet.) Bisinuthyl sulphide, Bi 6 O 3 S. (Hermann, J. pr. 76. 452.) Bi 2 O 3 S. Insol. in H 2 O. (Scherpenberg, C. C. 1889, II. 641.) Bi 4 3 S. Min. Karelinite. Boracic acid. See Boric acid. Borax. See TeZraborate, sodium. Or, sat. aqueous solution contains at 19 3.75%H 3 BO 3 . 25 6.27 " 37.5 7.32 ' 50 8.96 ' 62.5 14.04 ' 75 17.44 ' 87.5 21.95 ' 100 25.17 < (Brandes and Firnhaber, Arch. Pharm. 7. 50.) 1 litre H 2 O dissolves at 12 20 40 62 80 102^ 19.47g. H 3 BO 3 . 29.20 " 39.92" 69.91" 114.16" 168.15" 291.16" (Ditte, C. R. 85. 1069.) 1 1. H 2 O dissolves 0.901 mol. H 3 BO 3 at 25. (Herz, Z. anorg. 1910, 66. 359.) 1 1. H 2 dissolves 0.898 mol. H 3 BO 3 at 25. Sp. gr. of the solution = 1.0 168. (Miiller, Z. phys. Ch. 1907, 67. 529.) 1 1. H 2 O dissolves 0.887 mol. H 3 BO 3 at 25 and 1.025 mol. at 30. (Ageno and Valla, 1st. Ven. (VIII) 14. II, 331.) Solubility in H 2 O at t. Boric acid, anhydrous, B 2 0a. t g. HsBOs in 100 g. of the solution See Boron Znoxide. 2.59 Metabolic acid, HB0 2 . 12.2 21 3.69 4.90 Sol. in H 2 O. 31 6*44 SI. sol. in hot glacial acetic acid. (Holt, 40 8.02 Chem. Soc. 1911, 100. (2) 720.) 50 10.35 60 12.90 Orthobonc acid, H 3 B0 3 . 69.5 15^58 Sol. in 33 pts. H 2 O at 10. 80 19.11 25 " " 20. " 3 " " 100 90 23.30 (Berzelius.) 99.5 108 28.10 36.7 Sol. in 20 pts: H 2 O at 18.75. (Abl.) 100 pts. HsO at 100 dissolve 2 pts. (Ure's Diet.) 115 120 45.0 52.4 1 pt. crystallized acid dissolves in 25. 66 pts. H 2 at 19. 14.88 " 25. (Nasini and Ageno, Z. phys. Ch. 1909, 69. 483.) ' 12.66 " 37.5. Solubility curve for orthoboric acid in 10.16 " 50. 6.12 " 62.5. 4 73 " 75 I 2 O at various temp, up to 120. (Nasini and Ageno, Gazz. ch. it. 1911, 41. (1) 131. 3.55 " 87.5. Sp. gr. of H 3 BOs +Aq sat. at 8 = 1.014. (Anthon, A . 4. 241.) 2.97 " 100. Sp. gr. of H 3 BO 3 +Aq sat. at 15 = 1.024S. (Stolba. J. Or, 100 pts. H 2 O dissolve at pr. 90. 457.) 19 3. 9 pts. H 3 BO 3 . oc o i Sp. gr. of H 3 B0 3 +Aq at 15. Zo O.o 37.5 7.8 " '%H 3 BO 3 Sp. gr. %H 3 B0 3 Sp. gr. 50 9.8 " ' 62.5 16.0 " 75 21.0 " 1 2 Q 1.0034 4 1.0069 Sat. sol. 1.0147 1.015 87.5 28.0 " O 1 . U1UO . . . 100 34.0 " ' (Gerlach, Z. anal. 28. 473.) BORIC ACID 97 Sp. gr. of H 3 BO 3 +Aq at 18. %H 3 BO 3 0.776 1.92 2.88 3 612 Sp.gr. 1-0029 1.0073 1.0109 1.013 (Bock, W. Ann. 1887, 30. 638.) Volatile with steam. More sol. in dil. HCl+Aq than in H 2 O Sol. in warm cone. H 2 SO 4 , HC1, or HNO 3 + Aq. Solubility in HCl+Aq at 25. Solubility in KOH+Aq. See Berates, potassium. Solubility in NaOH+Aq. See Borates, sodium. Solubility in LiCl+Aq at 25. Millimols LiCI in 10 ccm. of the solution Millimols HaBOs in 10 ccm. of the sat. solution 7'l 10.3 22.3 37.2 9.01 8.13 7.65 6.42 5.02 Millimols HC1 in 1 10 ccm. of the solution Vlillimois H 3 BO 3 in 10 ccm of the sat. solution 7.'6 13.7 9.01 7.69 6.66 (Herz, Z. anorg. 1910, 66. 359.) Solubility in KCl+Aq at 25. (Herz, Z. anorg. 1910, 66. 359.) Solubility of H 3 BO 3 in HCl+Aq at 16. Millimols KC1 in 10 ccm. of the solution Millimols HaBOj in 10 ccm. of the sat. solution Normality of HC1 Normality of HsBOa "l.9 7.9 15.6 30.6 9.01 9.20 9.44 9.80 10.75 0. 0.130 0.260 0.390- 1.30 2.16 4.32 6.00 7.08 8.74 9.51 0.907 0.895 0.870 0.842 0.645 0.542 0.308 0.338 0.327 0.327 0.338 (Herz.) Solubility in RbCl+Aq at 25. Millimols RbCl in 10 ccm. of the solution Millimols HsBOa in 10 ccm. of the sat. solution ii'6 25.3 9.01 9.66 10.60 (Herz, Z. anorg. 1902, 33. 354.) Solubility in HF+Aa at 26. (Herz.) Solubility in NaCl+Aq at 25. (1) < 2 > Titerof Titer after wp saturation wit H 3 B0 3 at 26 (3) Titer after f%\ /2) addition equals free h mannitol b ric add Millimols NaCl in 10 ccm. of the solution Millimols H 3 BO 3 in 10 ccm. of the sat. solution 3.21n. 1.61 2.80n. 1.25(1.40?) 2.36 0.75 2.21 0.96(0.81?) '8.'2 15.2 29.4 9.01 8.49 8.25 8.20 The values 0.75 and 0.81 represent the fluorboric acid resulting from the original concentration of HF+Aq. (Abegg, Z. anorg. 1903, 35. 145.) Solubility of H 3 BO 3 in acids +Aq at 26. Acid Normality of the acid Normality of HsBOs H 2 S0 4 0.548 2.74 5.48 8.75 0.746 0.518 0.312 0.092 HNO 3 0.241 1.206 1.607 2.411 5.96 7.38 0.818 0.676 0.593 0.567 0.268 0.238 (Herz, Z. anorg. 1903, 34. 205.) (Herz.) Solubility in H 2 O is increased by presence of KC1, KNO 3 , K 2 SO 4 , NaNOa and Na 2 SO 4 . In general the solubility in H 2 O is increased >y the presence of both electrolytes and non- electrolytes. (Bogdan, C. C. 1903, II. 2.) Sol. in borax +Aq. (McLauchlan, Z. anorg. 903 37 371 ) SI.' soL in liquid NH 3 . (Franklin, Am. Ch. r. 1898, 20. 827.) Unattacked and undissolved by liquid N0 2 . Frankland, Chem. Soc. 1901, 79. 1362.) Sol. in 6 pts. alcohol (Wittstein), 5 pts. soiling alcohol (Wenzel). Only traces .dis- olve in anhydrous ether. (Schiff.) Sol. in 00 pts. ether. (Hager's Comm.) Sol. m everal essential oils. 1 1. H 2 O sat. with amyl alcohol dissolves 1.8952 mol. H 3 BO 3 at 25. (Auerbach, Z. Jiorg. 1903, 37. 357.) 98 BORIC ACID Solubility of H 3 BO 3 in amyl alcohol -{-Aq at t. Sp. gr. of amyl alcohol+Aq sat. with H 3 BO 3 . M =millimols H 3 BO 3 in 1 1. of H 2 O. A = millimols H 3 BO 3 in 1 1. of alcohol. g. water in 1 1. of alcohol + Aq d25/4 t M A 32.481 0.82229 15 607.2 589.3 176.4 177.4 35.465 37.339 42.479 . 82324 0.82321 0.82392 . 589.0 177.1 45 . 175 0.82447 586.0 427.4 425.8 173.4 127.6 127.0 45.636 47.883 51.461 0.82456 0.82454 0.82527 289.1 894.0 372.0 371.8 84.9 264.0 110.0 110.8 52.043 59.270 63.179 64.254 0.82585 0.82699 0.82739 0.82779 25 301.2 85.7 66.403 66.624 0.82701 0.82670 180.8 49.15 51.04 26.02 54.0 15.45 15.45 8.05 68.253 69.211 . 75.610 0.82856 0.82884 0. 82999 (?) (M tiller.) 35 146.3 44.27 (Mtiller, Z. phys. Ch. 1907, 67. 514.) Solubility of H 3 BO 3 in amyl alcohol and NaCl+Aq at 25 C Water phase Amyl alcohol phase NaCl normality mol. HsBOs Sp. gr. 25/4 1 1. contains mol. H 2 O mol. amyl alcohol mol. HaBOs 0.00 0.880 0.8296 4.10 8.39 0.2640 0.945 0.866 0.8277 3.55 8.49 0.2638 1.490 0.850 0.8268 3.27 8.54 0.2689 1.865 0.844 0.8259 3.03 8.56 0.2724 2.355 0.833 0.8254 2.86 8.59 0.2850 2.845 0.827 0.8247 2.62 8.62 0.2877 3.06 0.810 0.8241 2.39 8.66 0.2891 3.48 0.810 0.8240 2.32 8.69 0.3006 3.57 0.807 0.8236 2.15 8.70 0.3066 4.01 0.801 0.8233 . 1.99 8.72 0.3162 4.28 0.798 0.8229 1.78 8.75 0.3210 (Miiller) Solubility in hydroxy-compounds+Aq at 25. Organic substance added Mol. of organic sub- stance in 100 mol. of the mixture Mol. of boric acid sol. in 1 1. of solution Sp. gr. of the pure mixture Sp. gr. of the mixture sat. with boric acid Lactic acid 2.321 6.819 18.77 36.33 1.07 1.61 1.86 2.08 1.0252 1.0722 1 . 1405 1.2023 1.0444 1.0986 1 . 1635 1.2254 Glycerine 24.64 46.75 67.71 90.58 1.208 2.132 2.96 3.78 1 . 1574 1.2370 1.2531 1.1707 1.2260 1.2526 1.2710 BORIC ACID Solubility in hydroxy-compounds, etc. Continued Organic substance added Mol. of organic sub- stance in 100 mol. of the mixture Mol. of boric acid sol. in 1 1. of solution Sp. gr. of the pure mixture Sp. gr. of the mixture sat. with boric acid Mannitol 0.790 0.810 0.945 1.585 1.007 1.015 1.029 1.136 l'0244 1.0288 1.0475 1.0425 1.0433 Dulcitol 0.065 0.130 0.260 0.8876 0.9078 0.9360 0.9995 1.0018 1.0060 1.0686 1.0212 1.0260 (Miiller.) Solubility of H 3 BO 3 in alcohols +Aq at 25. M =Mol. of alcohol in 100 mol. of alcohol+Aq. H 3 BO 3 = Mol. of H 3 BO 3 in 1 1. of the solution. d 1= Sp. gr. of alcohol+Aq. d 2 =Sp. gr. of alcohol+Aq sat. with H 3 BO 3 . Alcohol added M HsBOs di da Methyl alcohol 11.74 0.895 28.64 1.012 36.02 1.098 43.95 1.161 52.31 1.307 100 ' 2.900 0.7924 0.8904 Ethyl alcohol 8.996 0.829 22.28 0.800 44.46 0.729 55.62 0.700 79.89 0.893 88.10 1.105 99.26 1.527 0.7860 0.8353 n-Propyl alcohol 23.66 53.63 0.6437 0.4569 0.9043 0.8231 0.9193 0.8570 83.65 0.5776 0.8133 0.8466 100 0.961 0.8010 0.8297 i-Butyl alcohol 0.70 2.15 0.884 0.857 0.9923 0.9853 1.0124 0.0038 2.18 0.857 0.9855 0.0046 71.4 0.323 0.8173 0.8351 77.1 0.347 0.8133 0.8220 85 6 0.4212 0.8081 0.8195 100 0.6927 0.7984 0.8172 i-Amyl alcohol 0.448 0.520 0.883 0.880 0.9943 0.9936 1.0132 1.0125 0.525 1 0.880 0.9931 1.0123 - 67. 26 2 0.2584 0.8232 0.829 . 75.54 0.2722 0.8183 0.8253 83.40 0.3190 0.8142 0.8223 100 0.5703 0.8068 0.8220 i Water sat. with alcohol. 2 Alcoh l sat " Wlth water ' (Miiller.) 100 BORIC ACID Easily sol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Solubility in acetone -}-Aq at 20. A = ccm. acetone in 100 ccm. acetone-fAq. H 3 BO 3 = millimols H 3 BO 3 in 100 ccm. of the solution. A 20 30 40 50 60 70 80 100 HaBO 79.15 81.71 83.35 82.74 81.61 76.40 67.62 55.05 8.06 (Herz, Z. anorg. 1904, 41. 319.) 100 g. pure anhydrous ether dissolve 0.00775 g. H 3 B0 3 . 100 g. ether sat. with HO dissolve 0.2391 g. H 3 BO 3 . (J. A. Rose, Dissert. 1902.) Sol. in 10 pts. glycerine. (Hager.) 100 pts. glycerine (sp. gr. 1.26 at 15.5) dissolve pts. H 3 BO 3 at t. t Pts. HaBOs t Pts. H 3 B0 3 t Pts. H 3 B0 3 10 20 30 20 24 28 33 40 50 60 70 38 44 50 56 80 90 100 61 67 72 (Hooper, Ph. J. Trans. (3) 13. 258.) Solubility of H 3 BO 3 in glycerine -f Aq at 25. G g. glycerine in 100 g. glycerine+Aq. H 3 BO 3 = Millimols H 3 BO 3 in 100 cc. of the solution. Solubility of H 3 BO 3 , etc. Continued. Acid Normality of the acid Normality of H 3 BO Tartaric 0.955 1 .909 2.51 3.316 0.890 0.923 0.962 1.07 ^Jier/i, u. aiiuig. xuo, **. A\J\J.J The solubility of H 3 BO 3 in H 2 O is increased by the presence of racemic acid. Millimols racemic acid in 10 ccm. of the solvent 6.3 12.6 24.7 Millimols boric acid in 10 ccm. of the solution 9.01 9.86 10.46 11.65 (Herz, Z. anorg. 1911, 70. 71.) Solubility of H 3 BO 3 in H 2 O is increased by the presence of tartaric acid. Millimols tartaric acid in 10 ccm. of the solvent 7.5 15 30 Millimols boric acid in 10 ccm. of the solution 9.01 10.00 10.70 12.07 (Herz, Z. anorg. 1911, 70. 71.) Solubility in oxalic acid+Aq at 25. Millimols oxalic acid in 10 ccm. of the solution 2.97 5.95 13.77 Millimols HsBOs in 10 ccm. of the sat. solution 9.01 9.95 10.80 11.98 (Herz, Z. anorg. 1910, 66. 93.) Solubility in H 2 O is increased by the pres- ence of urea, acetone or propyl alcohol. (Bog- dan, C. C. 1903, II. 2.) G H 3 BO 3 Sp. gr. Readily sol. in hot glacial acetic aci Chem. Soc. 1911, 100 (2). 720.) Sol. in 250 pts. benzene. (Hager. Solubility of H 3 BO 3 in mannite+A d. (Holt q at t, 7.15 20.44 31.55 40.95 48.7 69.2 100 90.1 90.1 90.6 92.9 97.0 103.0 140.2 390.3 1.0170 1.0379 1.0629 1.0897 1.1130 1 . 1328 1.1871 1.2719 Solid phase, H 3 BO 3 t Mg.-mols. in 1 1. t 30 Mg-mols in 1 1. Mannite H 3 BO 3 Mannite HsBOs 25 0.1 03 0.4 0.5 0.6 0.7 0.8 1.043 1.409 1.781 0.887 0.951 1.015 1.039 1.071 1.102 1.142 1.173 1.244 1.404 1.521 0.1 0.2 0.3 0.4 0.5 0.6 0.7 1.025 1.056 1.086 1.118 1.157 0.193 1.21.9 1,258 (Herz, Z. anorg. 1905, 46. 268.) Solubility of H 3 BO 3 in organic acids +Aq at 26. Acid Normality of the acid Normality of HsBO, Acetic 0.570 2.85 5.70 0.887 0.538 0.268 BORATE, AMMONIUM 101 Buferibuftori bel\ie8n-HF~-f Aq and amyl alcohol at 25. Solid phase, mannite Mg. mols .mil. c = HF concentration (millimols) . t a = H 3 BO 3 concentration in alcohol layer (expressed in millimols). Mannite H 3 B0 3 25 1.075 1 . 1424 0.2646 w = H 3 BO 3 concentration in water layer (expressed in millimols). .259 0.463 c a w ofic ^Q . ^u_ .354 \J . OOi7 0.794 500 14.3 71.2 .409 0.927 a 19.2 99.2 .536 1.243 a 25.3 144.2 .781 1.521 (t 114.3 979.0 OKfl on i 1 A A K (Ageno and Valla, 1st. Ven. (VIII) 14. 331.) ^OU (( oU . 1 37.0 L'f . O 194.8 H 56.8 321.5 U 108.0 652.0 125 39.0 170.5 Distribution between H 2 O and amyl alcohol a 47.2 214.0 at 25. a 52.8 240.5 w = concentration of expressed in millimols. H 3 BO 3 in H 2 O layer u 62.5 tt 96.0 30.4 on A 442.0 111.2 mo a = concentration of H 3 BO 3 in alcohol layer expressed in millimols. a OVJ . ' 65 (68?) 90.0 . O 272.8 362.2 w a (Abegg, Z. anorg. 1903, 35. 131.) 265 .8 76.6 See also Boron Zn'oxide. 196 .5 59.5 159 126 .6 47.5 37.1 Pyrobonc (tetrabonc) acid, H 2 B 4 O 7 . 87 q 33.2 Sol. in H 2 O. O 1 75 . O. Somewhat sol. in cold H 2 O. (Wohler, Pogg. 28. 525.) 3MgO, 2B 2 O 3 . Sol. in warm H 2 SO 4 or HNO 3 +Aq. (Ditte, C. R. 77. 893.) MgO, 6B 2 O 3 + 18H 2 = Mg(BO 2 ) 2 , 10HBO 2 + 13H 2 O. (Rammelsberg, Pogg. 49. 445.) 3MgO, 4B 2 O 3 . Sol. in hot dil. acids; insol. in acetic acid. (Ditte, C. R. 77. 893.) 5MgO, 2B 2 O 3 + 1K, and 3H 2 O. Min. Szzibelyite. Difficultly sol. in HCl+Aq. 9MgO, B 2 O 3 . (Mallard, C. R. 106. 260.) Magnesium manganous borate, 3Mg 2 B 2 O 5 , 4Mn 2 B 2 O 6 +7H 2 O. Min. Xussexite. Sol. in HCl+Aq. Magnesium potassium borate, KMg 2 BuOi 9 + 9H 2 0. Min. Kaliborite. Insol. in H 2 O. (Feit, Ch. Z. 1889, 13. 1188.) 2MgO, 2K 2 O, 11B 2 O 3 +20H 2 O. (van't Hoff and Lichtenstein, B. A. B. 1904, 936.) Magnesium sodium borate, Mg 2 B 6 On, Na 2 B 4 O 7 +30H 2 O. Efflorescent. About as sol. in cold H 2 O as borax; solution separates out a Mg borate on warming, which redissolves on cooling. Decomp. by boiling H 2 O. (Rammelsberg.) Magnesium strontium borate, 3MgO, 3SrO 4B 2 O 3 . Easily sol. in dil. acids. (Ditte, C. R. 77. .895.) Magnesium borate bromide, 2Mg 3 B 8 Oi 5 , MgBr 2 or 6MgO, 8B 2 O 3 , MgBr 2 . (Rousseau and Allaire, C. R. 1894, 119, 71.) Magnesium borate chloride, 2Mg 3 B 8 Oi 5 , MgCl 2 . Min. Boradte. Insol. in H 2 O; slowly sol. n acids. (Kraut.) Stassfurthite. Easily sol. in warm acids. ;Bischof.) Magnesium borate iodide, 6MgO, 8B 2 O 3 , MgI 2 . (Allaire, C. R. 1898, 127. 556.) Magnesium borate phosphate, Mg(BO 2 ) 2 , 2MgHPO 4 +7H 2 O. Min. Luneburgite. Magnesium borate sulphate, 2Mg 3 B 4 O 9 , 3MgSO 4 +12H 2 O. Min. Magnesium sulphoborite. Sol. in mineral acids when ground. (Nau- pert, B. 1893, 26. 874.) Manganous borate, MnB 4 O 7 (?). Insol. in H 2 O (Berzelius); very si. sol. in H 2 O (Thomas, Am. Ch. J. 4. 358); decomp. by warm, slowly by cold H 2 O. Sol. in MgSO \ +Aq (Berzelius). +3H 2 O. (Endemann and Paisley, Zeit. angew. Ch. 1903, 16. 176.) +5H 2 O. Ppt. (Endemann and Paisley.) Very hydroscopic. (Endemann, Am. Ch. J. 1903, 29. 72.) 3MnO, B 2 O 3 . (Mallard, C. R. 106. 1260.) Not attacked by H 2 O. Very sol. in acids. (Ouvrard, C. R. 1900, 130. 336.) 3MnO, 2B 2 O 3 . (Mallard.) MnH 4 (BO 3 ) 2 . Very si. sol. in H 2 O. Solubility in 2% Na 2 SO 4 +Aq. At 18.5, 0.77 g. MnH 4 (BO 3 ) 2 are dissolved per litre; at 40, 0.65 g.; at 60, 0.36 g.; at 80, 0.12 g. Solubility in 2% NaCl+Aq. 1 1. solution dissolves 1.31 g. salt at 18.2; 0.6 g. at 59; and 0.29 g. at 80. Solubility in 2% CaCl 2 +Aq. 1 1. CaCl 2 + Aq dissolves 2.91 g. salt at 17.6; 2.44 g. at 43.0; 2.25 g. at 61; and 1.35 g. at 80. (Hart- ley and Ramage, Chem. Soc. 63. 129.) Manganous borate bromide, 6MnO, 8B 2 O 3 , MnBr 2 . (Rousseau and Allaire, C. R. 1894, 119. 73.) Manganous borate chloride, 6MnO, 8B 2 O 3 , MnCl 2 . (Rousseau and Allaire, C. R. 1894, 118. 1257.) Molybdenum borate, MoO 2 , 2B 2 O 3 (?). Insol. in H 2 O; sol. in H 3 BO 3 +Aq. (Ber- zelius.) 106 BORATE, MOLYBDENUM Molybdenum borate, Mo 2 O 3 , B 2 O 3 . Precipitate. Insol. in H 2 O; si. sol. in a solution of boric acid. (Berzelius.) See Boromolybdic Acid. Nickel borate, Ni(BO 2 ) 2 +2H 2 O. Insol. in H 2 O. Easily sol. in acids. Easily sol. in warm NH 4 Cl+Aq. (Rose, Pogg. 88. 299.) 2NiO, B 2 O 3 +zH 2 O. Easily sol. in acids. (Rose.) 3NiO, 2B 2 O 3 +5H 2 O. Easily sol. in acids. (Rose.) 3NiO,B 2 O 3 . Not attacked by H 2 O; sol. in acids. (Ouvrard, C. R. 1900, 130. 337.) Nickel borate bromide, 6NiO, 8B 2 O 8 , NiBr 2 . (Rousseau, C. R. 1894, 119. 73.) Nickel borate chloride, 6NiO,8B 2 O 3 ,NiCl 2 . (Rousseau, C. R. 1894, 118. 1257.) Potassium borates. Solubility of B 2 O 3 in K 2 O+Aq at 30. Solution contains % by wt. K 2 % by wt. B 2 O Solid phase 47.50 KOH, 2H 2 O 46.45 ' 0.72 it 46.36 0.91 K 2 O, B 2 O 3 , 2.5H 2 O 40.51 1.25 36.82 1.80 a 36.72 1.85 u 32.74 3*51 n 29.63 6-98 u 26.89 12.12 11 24.84 17.63 " 23.30 18.19 K 2 O, 2B 2 O 3 , 4H 2 O 16.21 13.10 11.78 9.82 u 9.18 8.00 " 6.22 9.13 7.79 13.20 u 7.73 13.37 K 2 O, 2B 2 O 3 , 4H 2 O + K 2 O, 5B 2 O 3 , 8H 2 O 7.81 13.28 7.67 13.19 a 7.71 13.21 K 2 O, 5B 2 O 3 , 8H 2 O 7.63 13.28 3.42 7.59 1.80 4.15 0.80 3.05 n 0.51 3.19 a 0.33 4.58 K 2 O, 5B 2 O 3 , 8H 2 O + B(OH) 3 0.38 4.51 0.31 4.46 0.28 4.36 B(OH) 3 3.54 n At 30 only the three potassium borates K 2 O, B 2 O 3 +2.5H 2 O; K 2 O, 2B 2 O 3 +4H 2 O and K 2 O, 5B 2 O 3 +8H 2 O exist in stable form. (Dukelski, Z. anorg. 1906, 50. 42.) Potassium raetaborate, KBO^. Sol. in small amount of H 2 O. (Berzelius, Pogg. 34. 568.) + 1MH 2 O. Only stabile hydrate. (Dukel- ski, Z. anorg. 1906, 50. 42.) + 1HH 2 O. (Atterberg, Bull. Soc. (2) 22. 350.) Potassium /elaborate, K 2 B 4 O7. Very sol. in H 2 O. +4H 2 O. (Atterberg, Bull. Soc. (2) 22. 350.) Only stabile hydrate. (Dukelski, I c.) +5H 2 O. Very sol. in H 2 O; more sol. than K 2 B 6 Oio or K 2 B 12 Oi9. +6H 2 O. . (Atterberg, I. c.) Potassium Aezaborate, K 2 B 6 Oio4-5, and 8H 2 O. Easily sol. in H 2 O. Does not exist. (Dukelski, Z. c.) Potassium elaborate, K 2 Bi Oi6+8H 2 O. Sol. in H 2 O. (Rammelsberg*.) Only hydrate. (Dukelski.) Potassium dode/caborate, K 2 Bi 2 Oi 9 4-10H 2 O. 81. sol. in cold, very sol. in hot H 2 O. (Laurent, A. ch. 67. 215.) = K 2 BioOi 6 . (Rammelsberg.) Does not exist. (Dukelski.) Potassium borate fluoride, KBO 2 , KF. Sol. in H 2 O. (Schiff and Sestini, A. 228. 72.) KBO 2 , 2KF. Sol. in little, decomp. by much H 2 O. Insol. in H 2 O. (SchuT and Ses- tini, A. 228. 72.) Rubidium borate, Rb 2 B 4 O 7 . Anhydrous. (Reisehle, Z. anorg. 4. 166.) +6H 2 O. Not deliquescent or efflorescent. Sol. in H 2 O. (Reissig, A. 127. 33.) Samarium borate, SmBO 3 . Insol. in H 2 O; sol. in HCl+Aq. (Cleve, Bull. Soc. (2) 43. 1670.) Scandium borate, ScBO 3 . Sol. in dil. acids. (Crookes, Phil. Trans. 1910, 210. A. 364.) Silver borate, AgBO 2 . 81. sol. in H 2 O. By washing with H 2 O the boric acid is dissolved out. (Rose. Pharm. Centralbl. 1853. 205.) Sol. with decomp. in Na 2 S 2 O 3 +Aq (Her- schel); sol. in NH 4 NO 3 +Aq if pptd. cold. 1 1. H 2 O dissolves ca. 6 x 10~ 2 gram-atoms at 25. (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) Insol. in. ethyl acetate. (Naumann, B. 1910, 43. 314.) 3Ag 2 O, 4B 2 O 3 . (Rose, L c.) BORATE, SODIUM 107 Sodium borates. +8H 2 O. (Atterberg.) Solubility of B 2 O 3 in Na 2 O+Aq at 30 C . +4H 2 O and +8H 2 O are the only hydrates Solution contains iormed. (Dukelski.) System Na 2 O, B 2 O 3 , H 2 O at 60 investi- % by wt. % by wt. Solid phase gated by Sborgi. (Real. Ac. Line. 1915, (5) Na 2 O B 2 O:, 24. I, 443.) 42.00 40.85 2.7i NaOH, H 2 O u Sodjum tefraborate, Na 2 B 4 O 7 (Borax). 41.37 5.10 u 100 g. H 2 O dissolve at: 38.85 34.44 5.55 3.73 Na 2 O, B 2 O 3 , 4H 2 O 5 10 21.5 30 37.5 1.3 1.6 2.8 3.9 5.6 g. anhydrous salt. 29.39 2.51 " 45 50 54 55 56 57 28.61 2.38 tt 8.1 10.5 13.3 14.2 15.0 16.0 g. anhydrous salt. 27.78 26.13 2.44 2.75 u (Horn and van Wagener, Am. Ch. J. 1903, 25.08 OQ fin 2.98 tt Insol. in ethyl acetate. (Naumann, B. - > . \j\j 16.61 21.58 20.58 18.31 13.69 4.63 4.69 4.97 Na 2 O, B 2 O 3 , 4H 2 O + Na 2 O, B 2 O 3 , 8H 2 O Na 2 O, B 2 O 3 , 8H 2 O 1910, 43. 314.) Sol. in amyl alcohol in the presence of meta- arsenious acid and excess of H 3 BO 3 . (Auer- bach, Z. anorg. 1903, 37. 358.) +4H 2 0. i CTJ r\ 15.32 6.21 it 7^ Oil 2^ 100 g. H 2 O dissolve at: 13 . 25 8 18 12.39 9 12 tt 65 70 80 90 100 8^85 HK49 Na 2 O, 2B 2 O 3 , 10H 2 O 22.0 24.4 31.4 40.8 52.3 g. anhydrous salt. 5.81 6.94 (Horn and van Wagener, Am. Ch. J. 1903, 4.00 4.76 30. 347.) 1.88 2.41 +6H 2 O. Grows opaque in the air. (Bechi, 1.38 5.16 14 Sill. Am. J. (2) 17. 129.) 1.84 7.36 U + 10H 2 O. Only stabile hydrate. (Dukel- 2.02 7.79 tt ski, Z. anorg. 50. 30.) Efflorescent on surface 2.40 9.48 it in dry air. Not efflorescent when free from 4.08 17.20 Na 2 O, 2B 2 O 3 , 10H 2 O Na 2 CO 3 . (Sims.) +Na 2 O, 5B 2 O 3 , 10H 2 O Sol. in 12 pts. cold, and 2 pts. hot H 2 O. Sat. cold 3.79 15.84 Na 2 O, 5B 2 O 3 , 10H 2 O Na 2 B4O?+Aq contains 9.23%, and sat. hot Na-jB4O 7 + Aq contains 33.33% Na-^O-. (Gmelin.) 3.47 13.30 " Sol. in 20 pts. cold, and 6 pts. boiling H 2 O. (Wal- 9 9fi 19 14- K lerius.) - I ) 1.99 1 . J.TT 11.84 Na 2 O, 5B 2 O 3 , 10H 2 O Sol. in 15 pts. H 2 O at 18.75. (Abl.) 100 pts. H 2 O at 15.5 dissolve 5 pts.; at 65, 40 pts.; +B(OH) 3 at 100, 166 pts. Na 2 B4O 7 + 10H 2 O. (Ure's Dictionary.) 1.86 11.78 B(OH) 3 100 pts. sat. Na 2 B4O+Aq at 105.5 contain 52.5 pts. Na 2 B 4 O 7 , or 100 pts. H 6 O dissolve 110.54 pts. Na 2 B 4 O7, 1.81 11.18 or 1 pt. Na 2 B or CC1 4 . (Moissan, C. R. 113. 624.) BIP. Less hygroscopic than BI 2 P, but otherwise the properties are similar. (Mois- san.) BOROTUNGSTATE, AMMONIUM 111 Boron nitride, BN. Insol. in. H 2 O, cone. HNO 3 , cone. HC1 + Aq, or cone, solutions of alkalies. Decomp. by hot cone.. H 2 SO 4 or HF. (Wohler, A. 74. 70.) Boron /n'oxide, B 2 O 3 . Deliquescent. Sol. in H 2 O with a large in- crease in temp. (Ditte, C. R. 85. 1069.) 1 pt. dissolves at 18.75 in 47.01 pts. H 2 O. 27.75 18.73 15.13 9.29 7.28 5.58 4.74 ' 25 " 37.5 " 50 " 62.5 75 " 87.5 " 100 Or 100 pts. H 2 O dissolve at 18.75 2.13 pts. B 2 O 3 . " 25 3.60 " 37.5 4.24 " 50 6.61 " 62.5 10.76 " 75 13.73 " 87.5 17.92 " 100 21.09 (Brandes and Firnhaber, Arch. Pharm. 7. 50.) 1 litre H 2 O dissolves at ll.OOg. B 2 O 3 . 12 16.50 " 20 22.49' 40 39.50' 62 64.50' 80 95.00' 102 164.50' (Ditte, C. R. 85. 1069.) Sat. H 2 O solution boils at 100. (Brandes and Firnhaber.) Sat. H 2 O solution boils at 103.3. (Grif- fiths, Quar. J. Sci. 18. 90.) Sol. in acetic acid, hot cone. HCl+Aq, HNO 3 , and H 2 SO 4 . From the three latter it separates on cooling or dilution with H 2 O. Solubility in Na 2 O+Aq at 30. See Borates, sodium. Solubility in K 2 O+Aq at 30. See Borates, potassium. Insol. in hot glacial acetic acid. (Holt, Chem. Soc. 1911, 100. (2) 720.) Insol. in alcohol. (Graham.) Sol. in alcohol. (Berzelius, Ebelmen.) Sol. in oils. See also Boric acid. Boron dioxide potassium fluoride, B 2 O 3 , 2KF. Gradually sol. in H 2 O. Decomp. by much H 2 O. Insol. in alcohol. (Schiff and Sestini, A. 228. 82.) Boron oxychloride, BOC1. (Gustavson, Zeit. Chem. 1870. 521.) BOC1 3 . Slowly decomp. by H 2 O. (Coun- cler, J. pr. (2) 18. 399.) Oxychlorides of either the above formulae do not exist; the true formula for boron oxy- chloride is B 8 O U C1 2 . (Lorenz, A. 247. 226.) Boron phosphide, BP. Insol. in H 2 O. Sol. in cone, boiling alkalies +Aq with decomp. Decomp. by HNO 3 +Aq. (Besson, C. R. 113. 78.) Insol. in PC1 3 , AsCl 3 , SbCl 3 , CC1 4 , and in fact in all known solvents. Not attacked by boiling H 2 O, cone. HC1, or Hl-f Aq. Sol. in cone. HNO 3 with decomp. on heating. Not attacked by cold H 2 SO 4 . (Moissan, C. R. 113. 726.) B 5 P 3 . Not attacked by boiling cone. HNO 3 +Aq. Insol. in all solvents. (Moissan.) Boron phosphoiodide. See Boron iodophosphide. Boron selenide, B 2 Se 3 . Violently decomp. by H 2 O. (Sabatier, C. R. 112. 1000.) Boron bisulphide, B 2 S 3 . Decomp. with violence with H 2 O. Com- bines with alcohol and ether. (Fremy, A. ch. (3) 38. 312.) Insol. in most solvents, but si. sol. in PC1 3 without decomp.; more sol. in SC1 2 , but does not crystallize from the solution. (Moissan, C. R. 115. 203.) Boron Jn'sulphide ammonia, B 2 S 3 ,6NH 3 . Ppt. (Stock, B. 1901, 34. 3042.) Boron pentasulphide, B 2 S 5 . Decomp. by H 2 O and alcohol. (Moissan, C. R. 115. 271.) Borosulphuric acid, BOHSO 4 +SO 3 . Decomp. by H 2 O. (Schultz-Sellac, B. 4. 12.) B(HSO 4 ) 3 . Very deliquescent. Easily sol. in fuming H 2 SO 4 . (D'Arcy, Chem. Soc. 55. 155.) SO 2 (O.BO) 2 . Hydroscopic. Deliquescent. Sol. in H 2 O with decomp. Decomp. by cold alcohols. (Pictet, Bull. Soc. 1908, (4) 3. 1121.) (SO 3 ) 2 B 2 O 3 . Hydroscopic. Deliquescent. Sol. in H 2 O with decomp. Decomp. by cold alcohols. (Pictet, Bull. Soc. 1908, (4) 3. 1121.) Borononotungstic acid, H 4 B 2 W 9 O 3 2 + 22H 2 O=9WO 3 , B 2 O 3 , 2H 2 O+22H 2 O. Sol. in less than 1 / 9 pt. H 2 O, and as easily sol. in alcohol and ether. Sp. gr. of aqueous solution is somewhat under 3. (Klein, A. ch. (5) 28. 370.) Aluminum borononotungstate, A1 4 (B 2 W 9 O 32 )3 +65H 2 O. Extremely sol. in H 2 O. (Klein.) Ammonium , (NH 4 ) 4 B 2 W 9 O 32 + 18H 2 O. Quickly effloresces. (Klein.) 112 BOROTUNGSTATE, BARIUM Barium borowo;zotungstate, Ba2 19H 2 O. Sol. in 4 pts. cold, and less than Y<> pt. hot H 2 0. (Klein.) Cadmium , Cd 2 B 2 W 9 O 3 2 + 18H 2 O. Deliquescent. 100 pts. of salt dissolve in less than 8 pts. H 2 O at 19. Sp. gr. of solution is 3.28. (Klein.) Sp. gr. of sat. solution at 15.6/4 = 3.2887; at 16.2/4= 3.2868. (Kahlbaum, Z. anorg. 1902, 29. 229.) Calcium , Ca 2 B 2 W 9 O 32 +15H 2 O. Sol. in Vio pt. H 2 O. Solution has sp. gr. = 3.10. (Klein.) Cerium , Ce 4 (B 2 W 9 O 32 ) 3 +57H 2 O. Very sol. in H 2 O; sp. gr. of solution is over 3. Chromium , Cr 4 (B 2 W 9 O 32 )3+74H 2 O. Very sol. in H 2 O; sp. gr. of solution is 2.80. (Klein.) Cobalt , Co 2 B 2 W 9 O 32 + 18H 2 O. Very sol. in H 2 O; sp. gr. of solution sat. at 19 = 3.36. (Klein.) 100 pts. H 2 O dissolve 306.8 pts. anhydrous salt at 16.2; 288 pts. at 18.5; 299.7 pts. at 19.6; 286 pts. at 21.8. Sp. gr. of solution sat. at 19.2/4 = 3.1369. (Kahlbaum, Z. anorg. 1902, 29. 218.) Copper , Cu 2 B 2 W 9 O 32 + 19H 2 O. 25 pts. H 2 O dissolve 100 pts. salt. Sp. gr. of solution = 2. 6. (Klein.) Lead , Pb 2 B 2 W 9 O 32 +llH 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Klein.) Lithium , (?). Very sol. in H 2 O. Sp. gr. of solution is about 3. Magnesium , Mg 2 B 2 W 9 O 32 +22H 2 O. Very sol. in H 2 O. (Klein.) Manganous , Mn 2 B 2 W 9 O 32 + 17H 2 0. 100 pts. dissolve in 13 pts. H 2 O. Sp. gr. of solution at 19 = 3. 15. (Klein.) Mercurous , 3Hg 2 O, B 2 O 3 , 9WO 3 + 14H 2 O (?). ..."' Precipitate. Insol. in H 2 O. (Klein.) Sol. in 20,000 pts. dil. cold, and 1000 pts boiling HNO 3 +Aq of 1.42 sp. gr. Nickel , Ni 2 B 2 W 9 O 32 + 18H 2 O. Very sol. in H 2 O; sp. gr. of sat. solution at 19 = 3.32. 100 pts. H 2 O dissolve 261.6 pts. at 21.2. Sp. gr. 15.75/4 of solution =2.295 (Kahlbaum, Z. anorg. 1902, 29. 218.) Potassium boronorcotungstate, K 4 B>W 9 O 3 > + 13H 2 O. 5 pts. salt dissolve in 8 pts. H 2 O at 19 to form a solution of 1.38 sp. gr. The solution sat. at 100 has sp. gr. of over 2. (Klein.) Silver , Ag 4 B 2 W 9 O 32 + 14H 2 O. Very si. sol. in H 2 O. Sodium , Na 2 H 2 B 2 W 9 O 32 +23H 2 O. Very sol. in H 2 O. Solution sat. at 19 con- tains 84 pts. salt to 16 pts. H 2 O. (Klein.) Na 4 B 2 W 9 O 32 + 12H 2 O. Sol. in less than l / 3 pt. H 2 O. Thallium , T1 2 B 2 W 9 O 32 +5H 2 O. SI. sol. in hot H 2 O and nearly insol. in cold H 2 O. (Klein.) Uranyl , (UO 3 ) 3 (B 2 W 9 O 30 ) 2 +30H 2 O. Very sol. in H 2 O. (Klein.) Sp. gr. of solution = 3.1. Zinc , Zn 2 B 2 W 9 O 32 +2H 2 O. Very sol. in H 2 O. Sp. gr. of solution =3.15. (Klein.) Borodecitungstic acid. Barium borodecitungstate, Ba 2 B 2 Wi O 35 + 20H 2 O. M> Sol. in H 2 O. (Klein, C. R. 99. 35.) Boroduodecitungstic acid, H 8 B 2 Wi 2 O 43 = 4H 2 O, B 2 O 3 , 12 WO 3 . Known only in solution, which decomposes into borommotungstic acid and tungstic acid, when evaporated to a certain concentration. (Klein, C. R. 99. 35.) Barium potassium borodwodea'tungstate, 3BaO, K 2 O, B 2 O 3 , 12WO 3 +28H 2 O. Potassium , K 8 B 2 Wi 2 O 43 +21H 2 O. Sol. in H 2 O. (Klein.) 2K 2 0, 12WO 3 , B 2 O 3 + 18H 2 O. Sol. in H 2 O. (Klein.) RoToquatuordecitungstic acid, HioBoWi 4 O 5 i = 6H 2 O, B 2 O 3 , 14WO 3 . Has not been obtained in the free state. (Klein, A. ch. (5) 28. 353.) Barium TooToquatuordecitungstate, Ba 3 B 2 W 14 O 48 = 3BaO, B 2 O 3 , 14W0 3 + 5H 2 0. SI. sol. in H 2 O. (Klein.) arium sodium , S^BaO, 5H 2 O, B 2 O 3 , 14WO 3 +29H 2 O. Potassium , 3K 2 O, H 2 O, B 2 O 3 , 14WO 3 - 22H 2 O. Sol. inH 2 O. (Klein.) Silver , Ag 6 H 2 B 2 W 14 O 49 +7H 2 O. Nearly insol. in cold H 2 O. (Klein.) Sodium , Na 4 H 8 B 2 W 14 O 51 +29HoO. Sol. in H 2 O (Klein.) BROMAURATE, MANGANESE 113 Sodium strontium boToquatttordecitungstaie, 3HSrO, l^Na 2 O, B 2 O 3 , 14WO 3 +29H 2 O. Decomp. by H 2 O. (Klein.) BoTOundevigintitungstic acid. Barium boroundevigintitungstate, 4BaO, B 2 O 3 , 19WO 3 +30H 2 O. Can be cryst. from H 2 O. (Ebenhusen, Dissert. 1905.) BoToquattuoretvigintitungstic acid, B 2 O 3 , 24WO 3 +66H 2 O. Deliquescent. Somewhat more sol. in H 2 O than B 2 O 3 , 28WO 3 +62H 2 O. Also more stable. (Copaux, C. R. 1908, 147. 975.) Barium boToquattuoretrigintitungsta.te, 5BaO, B 2 O 3 , 24WO 3 +54H 2 O. 100 pts. H 2 O dissolve 50 pts. salt. (Copaux, A. ch. 1909, (8) 17. 217.) 6BaO, B 2 O 3 , 24WO 3 +58H 2 O. (Copaux, I.e.) Cadmium , 5CdO, B 2 O 3 , 24WO 3 + 51H 2 O. Extremely sol. in H 2 O. (Copaux, I. c.) Calcium , 5CaO, B 2 O 3 , 24WO 3 +44H 2 O. Very sol. in H 2 O. (Copaux, I. c.) Lithium , 15Li 2 O, B 2 O 3 , 24WO 3 +38H 2 O. (Copaux, /. c.) Magnesium 42H 2 O. 5MgO, B 2 O 3 , 24WO 3 + Very sol. in H 2 O. (Copaux, I. c.) 9Hg 2 O, B 2 O 3 , 24WO 3 + 5K 2 O, B 2 O 3 , 24WO 3 Mercurous 25H.O. (Copaux, I. c.) Potassium 36H 2 O. (Copaux, I. c.) Sodium , 5Na 2 O, B 2 O 3 , 24WO 3 +5H 2 O. As NH 4 salt. (Copaux, /. c.) BoToquinquetvigintitungstic acid. Potassium boroquinquetvigintitungstate, 5K 2 O, B 2 O 3 , 25WO 3 +34H 2 O. (Ebenhusen, Dissert. 1905.) Boroduodetrigintatungstic acid, B 2 O 3 , 28WO 3 +62H 2 O. Decomp. in boiling aqueous solution. (Co- paux, C. R. 1908, 147. 975.) Potassium boTodiiodetrigintatungstate, 6K 2 O, B 2 O 3 , 28WO 3 +42H 2 O. Decomp. by boiling alkalies. (Copaux, A. ch. 1909 (8) 17. 217.) Borovanadic acid. Sol. in H 2 O. Easily decomp. (Guyard, Bull. Soc. (2) 25. 354.) Afetabromantimonic acid, HSbBr 6 +3H 2 O. Very hydroscopic. Loses Br 2 in the air. Decomp. by H 2 O with separation of anti- monic acid. (Weinland, B. 1903, 36. 256.) Ammonium metobromantimonate, NH 4 SbBr 6 +H 2 O. Loses Br 2 in the air. Decomp. by H 2 O. (Weinland, I. c.) - Iron (ferric) wdabromantimonate, Fe(SbBr 6 ) 3 + 14H 2 O. Very hydroscopic. Decomp. by H 2 O. (Weinland", I. c.) Lithium wetabromantimonate, LiSbBre + 4H 2 O. Very hydroscopic. Loses Br 2 in the air, Decomp. by H 2 O. (Weinland, L c.) Nickel metobromantimonate, Ni(SbBr 6 ) 2 + 12H 2 O. Hydroscopic. Decomp. by H 2 O. (Wein- land, I. c.) ^ Potassium /^etobromantimonate, KSbBre-h H 2 O. Loses Br 2 in the air. Decomp. by H 2 O. (Weinland, I. c.) Bromarsenious acid. See Arsenyl bromide. Bromauric acid, HAuBr 4 +3H 2 O. (Lengfeld, Am. Ch. J. 1901, 26. 329.) +5H 2 O. Very sol. in H 2 O. (Thomsen, J. pr. (2) 13. 337.) -f 6H 2 O. Sol. in ether and CHC1 3 without decomp. (Lengfeld, Am. Ch. J. 1901, 26. 329.) Ammonium bromaurate, NH 4 AuBr 4 . Ppt. (Gutbier, Z. anorg. 1914, 85. 358.) Barium bromaurate. Not deliquescent. Sol. in H 2 O. (v. Bons- dorff, Pogg. 17.261.) Caesium bromaurate, CsAuBr 4 . SI. sol. in H 2 O or alcohol. Insol. in ether. (Wells and Wheeler, Sill. Am. J. 144. 157.) Ppt. (Gutbier, Z. anorg. 1914, 85. 360.) Cerium bromaurate, CeAuBr 6 +8H 2 O. Sol. in H 2 O. ( Jolin, Bull. Soc. (2) 21. 533.) Didymium bromaurate, DiAuBr 6 -f-9H 2 0. Very deliquescent. Sol. in H 2 O. (Cleve.) Lanthanum bromaurate, LaAuBr 6 +9H 2 O. Sol. in H 2 O. (Cleve.) Magnesium bromaurate. Deliquescent in moist air. (v. Bonsdorff.) Manganese bromaurate. Deliquescent, (v. Bonsdorff.) 114 BROMAURATE, POTASSIUM Potassium bromaurate, KAuBr 4 . SI. sol. in H 2 O. More sol. in cold alcohol than in H 2 O. (v. Bonsdorff.) +2H 2 O. Sol. in 5.12 pts. H 2 O at 15, 1.56 pts. at 40, and 0.48 pt. at 67. Decomp. by ether. SI. sol. in KBr+Aq. (Schottlander, A. 217. 314.) +5H 2 (X Efflorescent, (v. Bonsdorff.) Rubidium bromaurate, RbAuBr4. As caesium bromaurate. Ppt. (Gutbier, Z. anorg. 1914, 85. 359.) Samarium bromaurate, SmAuBr 6 +10H 2 O. Very deliquescent. (Cleve, Bull. Soc. (2) 43. 165.) Sodium bromaurate, NaAuBr 4 . Slowly sol. in H 2 O. (v. Bonsdorff.) Zinc bromaurate, Zn(AuBr 4 ) 2 . Very deliquescent, (v. Bonsdorff.) Bromauricyanhdric acid. Not known in free state. * Barium bromauricyanide, Ba[Au(CN) 2 Br 2 ] 2 + 10H 2 0. Very sol. in hot or cold H 2 O, also in alcohol. (Lindbom, Lund. Univ. Arsk. 12. No. 6.) Cadmium bromauricyanide, Cd[Au(CN) 2 Br 2 ] 2 +6H 2 0. Very sol. in hot or cold H 2 O, but solution is unstable. (Lindbom.) Calcium bromauricyanide, Ca[Au(CN) 2 Br 2 ] 2 + 10H 2 0. Extremely sol. in H 2 O and alcohol. (Lind- bom.) Cobalt bromauricyanide, Co[Au(CN) 2 Br 2 ] 2 + 9H 2 0. Moderately sol. in H 2 O. Less sol. than other bromauricyanides. (Lindbom.) Potassium bromauricyanide, KAu(CN) 2 Br +3H 2 O. Sol. in H 2 O and alcohol. Sodium bromauricyanide, NaAu(CN) 2 Br 2 + 2H 2 O. Very sol. in H 2 O or alcohol. ; IJ * Strontium bromauricyanide, Sr[Au(CN) 2 Br 2 +zH 2 0. Very sol. in H 2 O or alcohol. Zinc bromauricyanide, Zn[Au(CN) 2 Br 2 ] 2 + 8H 2 O. Easily sol. in cold or hot H 2 O. Bfomhydric acid, HBr. Very sol. in H 2 O. The most concentrated HBr+Aq has a sp. gr. of 1.78, and contains 82.02% HBr. (Cham- pion and Pellat, C. R. 70. 620.) This, or a weak acid on heating leaves a residue, which t Pts. HBr t Pts. HBr t Pts. HBr 25 20 15 10 2.550 2.473 2.390 2.335 5 + 10 +25 2.280 2.212 2.103 1.930 +50 +75 + 100 1 . 715 1.505 1.300 distils unchanged at 125-125.5 under 785 mm. pressure, and contains 48.17% HBr (Topsoe); at 126 under 758 mm. pressure, and contains 46.83% HBr (Bineau); and has sp. gr. = 1.486 at 20 (Bineau); sp. gr. = 1.48 at 20 (Champion and Pellat); sp. gr. = 1.49 at 20 (Topsoe)! According to Roscoe (A. 116. 214) an acid of constant composition, obtained by boiling a stronger or a weaker acid, if distilled under 752-762 mm. pressure, contains 47.38-47.86% HBr, and boils at 126 at 760 mm. pressure; but the composition is dependent on the pressure, as, for example, under 1952 mm. pressure, the residue boils at 153, and con- tains 46.3% HBr. (Roscoe.) By conducting dry air through HBr+Aq an acid is obtained containing 51.65% HBr if at 16, and 49.35% HBr if at 100 (Roscoe). 1 vol. H 2 O dissolves 600vols. HBr at 10. (Berthelot, C. R. 76. 679.) 1 pt. H 2 O at t and 760 mm. pressure dissolves pts. HBr. (Roozeboom, R. t. c. 4. 107.) Absorption by 1 pt. H 2 O at t and p pressure in mm. t= 25. P Pts. HBr P Pts. HBr 760 300 140 2.550 2.263 2.120 100 1 0.5 2.056 1.755 1.10 t= 20. p Pts. HBr P Pts. HBr 760 375 180 2.473 2 267 2.119 130 20 2.056 1.850 t= 15, P Pts. HBr p Pts. HBr 760 470 250 2.390 2.266 2.119 175 102 2.056 1.980 t= 11.3. p Pts. HBr P Pts. HBr 760 570 2.350 2.265 310 216 2.118 2.055 BROMATE, ALUMINUM 115 t= 5. Sp. gr. of HBr+Aq at 15. p Pts. HBr p Pts HBr 7 7 c/ HBr Sp. gr. HBr Sp. gr. HBr Sp. gr. 760 2.280 430 2.117 n. J5r 730 2.264 298 2.055 1 1.0082 18 1.145- 35 1.314 1 m ^^ 1 Q 1 1 ^4. OR 1 *^9A t = 0. 4fi 3 1^0230 20 M63 OvJ 37 1.338 4 1 0305 21 1.172 38 1.350 P Pts. HBr p Pts. HBr 5 22 M81 39 1^362 Io^rcr 760 2.212 380 2.054 6 7 1 .046 1.053 23 24 1 . 190 1.200 40 41 .375 1.388 540 2.116 5 1.085 8 1.061 25 1.209 42 1.401 (Roozeboom, R. t. c. 4. 107.) 9 10 1.069 1.077 26 27 1.219 1.229 43 44 1.415 1.429 Sp. gr. of HBr+Aq. 11 1.085 28 1.239 45 1.444 12 1 .093 OQ i 24Q 46 1 .459 Sp. gr. % HBr Temp. Sp. gr. % HBr Temp. 13 l'l02 30 -L . ^Tti7 1.260 47 1^474 1.055 7.67 14 1.335 36.67 13 14 15 1.110 1.119 31 32 1.270 1.281 48 49 1.490 1.496 1.075 10.19 14 1.349 37.86 13 16 1.127 33 1.292 50 1.513 1.089 11.94 14 1.368 39.13 13 17 1.136 34 1.303 1 097 1 2 96 14 1 419 ; 12 13 1.118 15^37 14 1.431 43.99 13 (Biel , C. C. 1882. 148.) 1.131 1 6 92 14 1 438 44 L 62 13 1.164 20^65 14 1.451 45.45 14 Absorbed by alcohol with .formation of 1.200 1.232 1.253 1.302 24.35 27.62 29.68 33 84 13 13 13 13 1.460 1.485 1.490 46.09 47.87 48.17 13 14 14 C 2 H 5 Br. The composition of the hydrates formed by HBr at different dilutions is calculated from determinations of the lowering of the fr. pt. T3rOQU. r>orl ITIT- T^ Rr Q nrl rf fVi p (\c\rtf iint.ivit.v (Topsoe, B. 3. 404.) and sp. gr. of HBr+Aq. (Jones, Am. Ch. J. 1905, 3d 39.fi 1 Sp. gr. of HBr+Aq at 14. +H 2 O. (Roozeboom, R. t. c. 5. 363.) % HBr Sp. gr. %HBr Sp. gr. %HBr Sp. gr. +2H 2 O. (Berthelot, A. ch. (5) 14. 369.) (Pickering Chem. Soc.1894, 64 (2) 232. 1 007 18 1.140 35 .314 Mpt. 11.2. (Pickering, I. c.) 2 .014 19 1.149 36 .326 +3H 2 O. Mpt. 48.0. (Pickering.) 3 .021 20 1.158 37 .338 +4H 2 O. Mpt. 55.8. (Pickering.) 4 .028 21 1.167 38 .351 +5H 2 O. (Pickering.) 5 6 .035 .043 22 23 1.176 1.186 39 40 .363 .376 Bromhydric cyanhydric acid, . 3HBr, 7 1 .050 24 1.196 41 .389 2HCN. 8 1 .058 25 1.206 42 .403 Decomp. by H 2 O and alcohol. 9 1 .065 26 .215 43 .417 Insol. in ether. (Gautier, A. ch (4) 17. 10 1 .073 27 .225 44 .431 141.) 11 12 13 14 15 16 17 1 1 1 1 1 i i .081 .089 .097 .106 .114 .122 .131 28 29 30 31 32 33 34 .235 .246 .257 .268 .279 1.290 1.302 45 46 47 48 49 .445 .459 .473 .487 .502 Bromic acid, HBrO 3 . Known only in aqueous solution. Solution evaporated on water bath decom- poses when it contains 4.26% HBrO 3 . In vacuo, an acid containing 50.59% HBrO 3 corresponding to formula HBrO 3 +7H 2 O can be ob hamed. (Topsoe, calculated by Gerlach, Z. anal. 27. Not decomp. by dil. HNO 3 , orH 2 SO 4 +Aq. 316.) Sp.gr. of HBr+Aq at 15. Cone. H 2 SO 4 decomposes. Alcohol and ether are quickly oxidized by HBrO 3 . % HBr Sp. gr. %HBr Sp. gr. %HBr Sp. gr. Bromates. 5 10 15 1 1 1 .038 .077 .177 25 30 35 1.204 1.252 1.305 45 50 1.435 1.515 Most of the bromates are very sol a few are si. sol., but none are insol., sol/being AgBrO 3 and Hg 2 (BrO 3 ) 2 . in H 2 O, the least 20 1 .159 40 1.365 Aluminum bromate, Al(BrO 3 ) 3 . Only i i "moderate degree of accuracy" is Deliquescent. (Rammelsberg, Pogg. 55. claimed 242.) for this table. (Wright, C. N. 23. 63.) +9H 2 O. Mpt. 62.3. Less hygroscopic 116 BROMATE, AMMONIUM than A1(C1O 3 ) 2 . (Dobrosserdow, C. C. 1907. I, 1723.) Ammonium bromate, NH solution nont.ain: Solubility of Br 2 in NaBr+Aq at 25. g. NaBr per 1. g.-atoms Bra per 1. Sp. gr. 92.6 2.479 1.213 160.5 4.345 1.372 205.8 6.195 1.515 255.8 8.575 1.678 319.7 13.65 1.997 359.0 16.04 2.137 19.23 2.327 408.3 20.85 2.420 (Bell, J. Am. Chem. Soc. 1912, 34. 14.) Solubility in salts -j-Aq. Solubility in 1 liter K 2 SO 4 +Aq at 25. K 2 SO 4 +Aq g. Bromine 1-N Vr-N V 4 -N Vs-N V:e-N 25.14 29.44 31.46 32.70 33.10 (Jakowkin, Z. phys. Ch. 1896, 20, 26.) Millimols. Br 2 Millimols. Hg 2.125 0. 2.204 0.0560 , 2.216 0.0793 2.226 0.1284 2.231 0.2120 (Herz and Paul, Z. anorg. 1914, 85. 215.) 1 1. N.NH 4 C 2 H 3 O 2 +Aq dissolves 340.5 g. Br 2 at 25. (McLauchlan, Z. phys. Ch. 1903, 44. 617.) Miscible in all proportions with liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) More sol. in alcohol than in H 2 O; miscible with ether, CS 2 , CHC1 3 . (Sestini, Zeit. Chem. 1868. 718.) Somewhat soluble in glycerine. - (Pelouze.) Sol. in benzene (Mansfield) ; insol. in benzene (Moride, A. ch. (3) 39. 452). Sol. in warm chloral, bromal, and iodal. (Lowig, Pogg. 14. 485.) Sol. in SC1 2 (Solly), and SBr 2 . Sol. in cone. HC 2 H 3 O 2 +Aq. (Balard.) Sol. in aqueous solution of potassium, sodium, or cal- cium acetates. (Cahours.) BROMINE 121 Solubility in CS 2 . 100 g. of the sat. solution contain at: 95 110.5 116 45.4 39.0 36. 9 g. Br 2 . (Arctowski, Z. anorg. 1896, 11. 274.) Cryst. from CS 2 at 90 in fine needles. (Arctowski, Z. anorg. 1895, 10. 25.) Sp. gr. of Br 2 +CCl 4 at 32.5. % Br 2 by weight Sp. gr. 1 . 5449 1 . 58014 1 . 6454 1 . 58060 1 . 7990 1 . 58168 2 . 6676 1 . 58812 3 . 5833 1 . 59526 (Joseph, Chem. Soc. 1915, 107. 3.) Sp. gr. of Br 2+ nitrobenzene at 32.5. % Br 2 by weight Sp. gr. 1.5643 1.20225 3.2323 1.21449 4.6462 1.22518 6 . 1826 1 . 23603 (Joseph, Chem. Soc. 1915, 107. 3.) Very sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol in acetone. (Eidmann, C. C. 1899, II, 1014; Naumann, B. 1904, 37. 4328.) Partition of Br 2 between water and other solvents. W = millimols Bromine in 10 ccm. of the aqueous layer. G=millimols Bromine in 10 ccm. of the A C N=C/A 7.545 691.9 91.71 4.109 338.6 82.41 2.660 217.4 81.72 2.544 207.7 81.66 1.740 140.38 80.67 1.2878 103.7 80.51 0.8073 64.44 79.83 0.5046 39.64 78.38 Partition of Br 2 , etc. Continued Other solvent CS 2 7.750 10.600 14.696 17.999 26.345 40.625 57.038 1015 1387 1910 2352 3467 5194 7160 G/w 76.35 76.44 76.98 76.54 75.99 78.21 79.66 (Herz, Z. Elektrochem, 1910, 16. 871.) Partition coefficient for bromine between CS 2 and H 2 O at 25C. A = concentration of the water layer. C = concentration of the CS 2 layer. Partition coefficient for bromine between CHBr 3 and H 2 O at 25C. A = concentration of the water layer. C = concentration of the CHBr 3 layer. other layer. A C N=C/A Other solvent G w G/W 5.424 3.838 2.368 1.348 0.766 0.366 373.6 264.7 161.5 90.17 50.49 23.62 68.88 68.80 68.19 66.90 65.84 64.85 CC1 4 1.949 7.008 12.171 39.880 54.574 0.0853 0.3085 0.5300 1.3132 1.5560 22.73 22.71 23.13 30.32 35.01 Partition coefficient for bromine between CC1 4 and H 2 O at 25C. A = concentration of the water layer. C = concentration of the CC1 4 layer. 75% by vol. CC1 4 +25% by vol. CS 2 3.567 7.304 10.833 13.922 17.230 25.637 40.625 54.035 0.0985 0.1910 0.200 0.3720 0.4580 0.6580 0.9940 1.2080 37.06 38.15 37.36 37.42 37.62 38.96 40.88 44.73 A C N -C/A 14.42 10.80 7.901 7.163 6.803 5.651 3.216 2.054 1.266 0.7711 0.5761 0.4476 0.3803 0.2478 545.2 372.2 252.8 225.8 218.5 172.6 94.84 58.36 35.92 21.53 15.72 12 09 10.27 6.691 37.82 34.44 32.01 31.52 32.12 30.54 29.48 28.41 28.37 27.92 27.26 27.02 27.00 27.00 50% by vol. CC1 4 + 50% by vol. CS 2 3.592 6.820 10.148 13.866 16.616 42.975 55.965 0.0784 0.1487 0.2206 0.3065 0.3688 0.8086 0.9960 45.82 46.85 46.01 45.24 45.05 53.15 56.19 65.05 64.82 65.65 65.26 65.17 25% by vol. CC1 4 +75% by vol. CS 2 5.753 10.902 26.724 41.314 55.526 0.0884 0.1682 0.4970 0.6331 0.8520 (Jakowkin, Z. phys. Ch. 1895, 18. 588;) 122 BROMINE CHLORIDE Partition of bromine between CC1 4 and salts +Aq. A = concentration of Br in H 2 O layer. C = concentration of Br in CC1 4 layer. Partition of Br 2 between CC1 4 and NaNO 3 Aq at 25. NaNO 3 +Aq A C 1-N V 2 -N Vr-N. Vs-N Vir-N 7.905 8.763 9.033 9.200 9.399 316.7 319.5 315.7 316.7 319.3 (Jakowkin, Z. phys. Ch. 1896, 20, 25.) Partition of Br 2 between CC1 4 and K 2 SO 4 + Aq at 25. K 2 S04+Aq A c 1-N V*-N Vr-N Vs-N Vie-N 5.982 6.843 7 354 7.585 7.498 255.4 253.4 252.8 250.3 242.3 (Jakowkin, /. c.) Partition of Br 2 between CC1 4 and Na 2 SO 4 + Aq at 25. Na 2 SO4 +Aq A C 1-N V 2 -N 1 /4-N Vs-N Vie-N 5.934 6.838 7.402 7.609 7.713 254.6 253.4 254.4 252.8 251.2 (Jakowkin, I. c.) Crystallizes at 4 with 10H 2 O. Bromine chloride, BrCl. Sol. in H 2 O, CS 2 , ether, etc. Bromine fluoride, BrF 3 . Fumes in the air. Decomp. by H 2 O. (Le- beau, C. R. 1905, 141. 1019.) Bromine oxides. No oxides of bromine are known in the free state. See hypobromous, bromic, and per- bromic acids. Bromiridic acid. Ammonium bromiridate, (NH 4 ) 2 IrBr 6 . Less sol. in cold H 2 O than the K salt. (Birnbaum, Zeit. Chem. 1865. 22.) Very sol. in cold H 2 O. (Gutbier, B. 1909, 42. 3910.) Caesium bromiridate, Cs 2 IrBr 6 . Sol. in H 2 O. (Gutbier, B. 1909, 42. 3911.) Potassium bromiridate, K 2 IrBr 6 . Moderately sol. in cold, more easily in hot H 2 O. Insol. in alcohol or ether. Sol. in cold H 2 O and in HBr+Aq. (Gut- bier, B. 1909, 42. 3910.) Rubidium bromiridate, Rb 2 IrBr 6 . Very sol. in cold H 2 O. Sol. in hot dil. HBr+Aq. (Gutbier, B. 1909, 42. 3911.) Sodium bromiridate. : ,; "') Deliquescent. Easily sol. in H 2 0, alcohol, or ether. Bromiridous acid, H 6 Ir 2 Bri 2 -f6H 2 O. Easily sol. in H 2 O, alcohol, or ether. (Birr- baum, 1864.) Ammonium bromiridite, (NH 4 ) 6 Ir 2 Bri 2 +H 2 O. Difficultly* sol. in H 2 O. (Birnbaum.) Potassium bromiridite, K 6 Ir 2 Bri 2 +6H 2 O. Efflorescent. Sol. in H 2 0. Silver bromiridite, Ag 6 Ir 2 Bri2. Ppt. Insol. in H 2 O or acids. Sodium bromiridite, Na 6 Ir 2 Bri 2 +24H 2 O. Efflorescent. Very sol. in H 2 O. Bromocarbonatoplatmdiamine carbon- ate, ^ 3 [Pt(N 2 H 6 ) 2 ] 2 (C0 3 ) 2 +4H 2 0. Ppt, Bromocarbonatoplatincfo'amine carbonate bromoplatinefo'amine nitrate, B 3 [Pt(N 2 H 6 ) 2 ] 2 (CC 3 ) 2 , 2Br 2 Pt(N 2 H 6 ) 2 (NO,),. BromocWoroplatincfo'amine chloride, g[ Pt(N 2 H 6 ) 2 Cl 2 . Very si. sol. in H 2 O. (Cleve.) - chlorobromide, Q Pt N 2 H6Br (?) ' Very si. sol. in H 2 O. Bromochlororoplatinic acid. Potassium bromochloroplatinate, K 2 PtCl 5 Br (Pitkin, J. Am. Chem. Soc. 2. 408.) Mixture. (Herty, J. Am. Chem. Soc. 1896, 18. 130.) K 2 PtCl 4 Br 2 . SI. sol. in cold H 2 0; much more sol. in hot H 2 O. (Pitkin.) Mixture. (Herty.) K 2 PtCl 3 Br 3 . As above. K 2 PtCl 2 Br 4 . (Pigeon, A. ch. 1894, (7) 2. 488.) K 2 PtClBr 5 . (Pitkin.) Bromochromic acid. Potassium bromochromate, KCrO 3 Br 2 = CrO 2 (Br)OK. Decomp. by H 2 O. (Heintze, J. pr. (2) 4. BROMONITRATOPLATINAMINE NITRATE 123 Dibromochromium chloride, [Cr(H 2 O) 4 Br 2 ]Cl+2H 2 O. Ppt. Nearly insol. in fuming HC1. (Bjer- rum, B. 1907, 40. 2918.) Bromohydroxyloplatincfo'amine bromide, Very si. sol. in H 2 O. (Cleve.) -- chloride, ^ Pt(N 2 H 6 Cl) 2 . Sol. inH 2 O (Cleve.) - nitrate, ^ Pt(N 2 H 6 NO 3 ) 2 . Very si. sol. in cold, moderately sol. in hot H 2 O. (Cleve.) Bromohydroxyloplatinwonoc&amine nitrate, >t<>> + H 2 O. Easily sol. in H 2 O. (Cleve.) Bromomercurosulphurous acid. Ammonium bromomercurosulphite, NH 4 SO 3 HgBr. Sol. in H 2 O. (Earth, Z. phys. Ch. 9. 215.) Potassium bromomercurosulphite, KSO 3 HgBr. As above. (B.) Bromomolybdenum bromide, Br 4 Mo 3 Br 2 = molybdenum efabromide, MoBr 2 . Insol. in H 2 O or acids, or even in boiling aqua regia. Easily sol. in dilute, decomp. by cone, alkalies +Aq. (Blomstrand, J. pr. 82. 436.) Bromomolybdenum chloride, Br 4 Mo 3 Cl 2 -|- 3H 2 O. Insol. in acids. (Blomstrand.) Bromomolybdenum chromate, Br 4 Mo 3 CrO 4 + 2H 2 O. Insol. in dil. acids. Sol. in hot cone. HC1 +Aq. Insol. in alkali chromates+Aq. (At- terberg.) Bromomolybdenum fluoride, Br 4 Mo 3 F 2 + 3H 2 O. Insol. in H 2 O. (Atterberg.) Bromomolybdenum hydroxide, Br 4 Mo 3 (OH) 2 . Completely sol. in alkalies if not heated over 90. (Atterberg.) -f 2H 2 O. +8H 2 O. Bromomolybdenum iodide hydroxide, 2Br 4 Mo 3 I 2 , Br 4 Mo 3 (OH) 2 +8H 2 O. Precipitate. (Blomstrand, J. pr. 77. 92.) Bromomolybdenum molybdate, Br 4 Mo 3 MoO Precipitate. (Atterberg.) Bromomolybdenum phosphate, Br 4 Mo 3 H 4 (PO 4 ) 2 . Precipitate. Insol. in H 2 O. (Atterberg.) Bromomolybdenum sulphate, Br 4 Mo 3 SO 4 + 3H 2 O. Precipitate. SI. sol. in boiling H 2 SO 4 . (Atterberg.) ZH'bromomolybdous acid, MoOBr 2 (OH) -f Sol. in H 2 O. Very hydroscopic. ' (Wein- land, Z. anorg. 1905, 44. 86.) !Teirabromomolybdous acid, MoBr 4 (OH) + 2H 2 O. Sol. in H 2 O. Hydroscopic. (Weinland, I.e.) D?'ammonium pewtobromomolybdite, MoBr 6 O(NH 4 ) 2 . Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) Dicsesium pe/abromomolybdite, MoBr 6 OCs 2 . Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) Calcium ^e/rabromomolybdite, (MoBr 4 O) 2 Ca +7H 2 O. Hydroscopic. Sol. in H 2 O. (Weinland, I. c. te^rabromomolybdite, MoBr 4 (OLi)+4H 2 O. Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) Magnesium pewtobromomolybdite, MoBr 5 (OMg)+7H 2 O. Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) M o wopotassium t efrabromomolybdite, MoBr 4 (OK)+2H 2 O. Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) Dipotassium pewtobromomolybdite, MoBr 6 OK 2 . Hydroscopic. Sol. in H 2 O. (Weinland, I.e.) Dirubidium pefabromomolybdite, MoBr 6 ORb 2 . Hydroscopic. Sol. in H 2 O 4 (Weinland, I.e.) Bromonitratoplatindi'amine nitrate, Br p ,N 2 H 6 N0 3 . NOg l N 2 H 6 NO 3 . Decomp. by H 2 O. (Cleve.) - sulphate, jj 3 Pt(N 2 H 6 ) 2 S0 4 +H 2 6. SI. sol. in H 2 O. ' 124 BROMONITRITOPLATINAM1NE NITRITE Bromonitritoplatinsermdi'amine nitrite, NO 2 Br 2 Pt(NH 3 ) 2 NO*, SI. sol. in H 2 O. (Blomstrand.) Bromonitrous acid. Platinum silver bromonitrite, PtAg 2 Br 2 (NO 2 ) 4 . Ppt. (Miolati, Gazz. ch. it. 1900, 30. 588.) Bromopalladic acid. Ammonium bromopalladate, (NH 4 ) 2 PdBr 6 . Difficultly sol. in cold H 2 O. Decomp. by hot H 2 O and by hot cone. H 2 SO 4 . (Gutbier, B. 1905, 38. 1907.) Caesium bromopalladate, Cs 2 PdBr 6 . Difficultly sol. in cold H 2 O. Decomp. by hot H 2 O or by hot cone. H 2 SO 4 . (Gutbier, I.e.] Potassium bromopalladate, K 2 PdBr 6 . Difficultly sol. in cold H 2 O. Decomp. by hot H 2 O or by hot cone. H 2 SO 4 . (Gutbier, I.e.) Rubidium bromopalladate, Rb 2 PdBr 6 . Insol. in cold H 2 O. Decomp. by hot H 2 or by hot cone. H 2 SO 4 . (Gutbier, I. c.) Bromopalladious acid. Ammonium bromopalladite, (NH 4 ) 2 PdBr 4 . Very stable. Sol. in H 2 O. (Smith, Z. anorg. 1894,6.381.) Very sol. in cold H 2 O. Can be cryst. from a very small amount of hot H 2 O. (Gutbier, B. 1905, 38. 2387.) Barium bromopalladite. Not deliquescent. Sol. in H 2 O. (v. Bons- dorff.) Caesium bromopalladite, Cs 2 PdBr 4 . Very sol. in H 2 O. (Gutbier, B. 1905, 38. 2388.) Manganese bromopalladite, MnPdBr 4 . Sol. in H 2 O and alcohol, (v. Bonsdorff.) +7H 2 O. Very sol. in H 2 O. (Smith, Z. anorg. 1894, 6. 382.) Potassium bromopalladite, K 2 PdBr 4 . Easily* sol. in H 2 0. (Joannis, C. R. 95. 295.) Very stable. Sol. in H 2 O. (Smith, Z. anorg. 1894, 6. 381.) +2H 2 O. Unstable in the air. (Smith, I. c.) Rubidium bromopalladite, Rb 2 PdBr 4 . Can be cryst. from a very small amount of hot H 2 O. (Gutbier, B. 1905, 38. 2388.) Sodium bromopalladite, Na 2 PdBr 4 +4^H 2 O. Very deliquescent. Sol, in H 2 O. (Smith, I.e.) Strontium bromopalladite, SrPdBr 4 +6H 2 O. Stable in the air. Very sol. in H 2 O. (Smith, I. c.) Zinc bromopalladite. Sol. in H 2 O. (v. Bonsdorff.) Bromophosphatoplatmcfa'amme phos- phate, BrPt(N 2 H 6 ) 2 +2H 2 O. \ / P0 4 SI. sol. in H 2 O. (Cleve.) Bromopho sphoric acid. Thorium bromophosphate, ThBr 4 , 3(3ThO 2 , 2P 2 O 5 ). Insol. in most acids and in fused alkali carbonates. Decomp. by long boiling with cone. H 2 SO 4 . (Colani, C. R. 1909, 149. 208.) Bromoplatinamine bromide, Br 2 Pt(NH 3 Br) 2 . SI. sol. in H 2 G. (Cleve, Sv. V. A. H. 10, 9. 31.) - nitrite, Br 2 Pt(NH 3 NO 2 ) 2 . Very si. sol. in H 2 O. (Cleve.) Bromoplatincfo'amine bromide, Br 2 Pt(N 2 H 6 ) 2 Br 2 . Only si. sol. in hot H 2 O. (Here.) - chloride, Br 2 Pt(N 2 H 6 ) 2 Cl 2 . Very si. sol. in H 2 O. (Cleve.) - dichromate, Br 2 Pt(N 2 H 6 ) 2 Cr 2 O;. SI. sol. in H 2 O. -- nitrate, Br 2 Pt(N 2 H 6 NO 3 ) 2 . SI. sol. in cold, rather easily sol. in hot H 2 O. (Cleve.) -- phosphate, Br 2 Pt[N 2 H 6 PO 2 (OH) 2 ] 2 + 2H 2 O. Rather easily sol. in hot H 2 O. (Cleve.) -- sulphate, Br 2 Pt(N 2 H 6 ) 2 S0 4 . Very si. sol. in H 2 O. Bromoplatinraonocfa'amine nitrate, Rr Pf (NH 3 ) 2 NO 3 BraPt NH 3 N0 3 . Easily sol. in H 2 O. -- sulphate, Br 2 Pt .i SO 4 +H 2 O. Moderately sol. in H 2 0. (Cleve.) Bromoplatinsemicfa'amine bromide. Br 3 Pt(NH 3 ) 2 Br. SI. sol. in cold H 2 O. (Cleve.) Bromodi'platincfo'amine anhydronitrate, Sol. in HNO 3 +Aq. BROMOPURPUREOCHROMIUM CHLORIDE 125 Bromocfa'platincfo'amine chloride, Br 2 Pt 2 (N 2 H ) 4 Cl 4 . Ppt. (Cleve.) nitrate, Br 2 Pt 2 (N 2 H 6 ) 4 (NO 3 ) 4 +2H 2 O. Moderately sol. in hot H 2 O. - sulphate, Br 2 Pt 2 (N 2 H 6 ) 4 (SO 4 ) 2 +2H 2 O. "Ppt. (Cleve.) Bromoplatinic acid, H 2 PtBr 6 +9H 2 O. Very deliquescent, and sol. in H 2 O, alcohol, ether, chloroform, or acetic acid. (Topsoe, J. B. 1868. 273.) Ammonium brcmoplatinate, (NH 4 ) 2 PtBr G . Sol. in 200 pts. H 2 O at 15. (Topsoe.) 100 pts. (NH 4 ) 2 PtBr 6 +Aq sat. at 20 con- tain 0.59 pt. dry salt. (Halberstadt, B. 17. 2965.) Barium bromoplatinate, BaPtBr 6 + 10H 2 O. SI. deliquescent. Very sol. in H 2 O. Caesium bromoplatinate, Cs 2 PtBr 6 . SI. sol. in dil. HBr+Aq. (Obermaier, Dissert.) Calcium bromoplatinate, CaPtBr 6 + 12H 2 O. SI. deliquescent. Very sol. in H 2 O. Cobalt bromoplatinate, CoPtBr 6 + 12H 2 O. Deliquescent. Copper bromoplatinate, CuPtBr 6 +8H 2 O. Very deliquescent; sol. in H 2 0. Lead bromoplatinate, PbPtBr 6 . Easily sol. in H 2 O, but decomp. by large amount. Lead te/rabromoplatinate, [PtBr 4 (OH) 2 ]Pb, PbOH. Insol. in H 2 O. (Miolati, C. C. 1900, II. 810.) Magnesium bromoplatinate, MgPtBr 6 + 12H 2 0. Not deliquescent. Manganese bromoplatinate, MnPtBr 6 + 6H 2 O. [lt. Rplff Arsfld Rnll 1905. (Hinrichsen, Z. phys. Ch. 1904, 60. 96.) 359.) . Insol. in anhydrous pyridine and in 97% Solubility of CsCl+HgCl 2 in H 2 O at 25. pyridine+Aq. SI. sol. in 95% pyridine+Aq and in 93% pyridine+Aq. (Kahlenberg, J. Solution contains Am. Chem. Soc. 1908, 30. 1107.) Q I- 1 1 % CsCl % HgCl-2 Caesium chromium chloride, 2CsCl,CrCl 3 + 65.61 65.78 62.36 57.01 52.35 0.00 0.215 0.32 0.64 1.23 CsCl CsCl+Cs 3 HgCl 5 Cs 3 HgCl 5 u H 2 O. Stable in the air. Sol. in H 2 O. (Wells, Z. anorg. 1895, 10. 182.) 2CsCl,CrCl 3 +4H 2 O; hydroscopic; very sol. in H 2 O. (Wells, I. c.) 51.08 49.30 45 95 1.44 1.49 1 69 Cs 3 HgCl 5 +Cs 2 HgCl 4 Cs 2 HgCl 4 Caesium tetra-aquochiomium chloride, CrCl 2 (OH 2 ) 4 .Cl, 2CsCl. 45.23 1.73 Cs 2 HgCl 4 +CsHgCl 3 Ppt. (Werner, B. 1901, 34. 1602.) 38.63 17.03 1.32 0.51 CsHgCl 3 Caesium cobalt chloride, CsCoCl 3 +2H 2 O. 1.53 0.42 " Decomp. by H 2 O and alcohol. (Campbell, 0.61 2.64 CsHgCl 3 +CsHg 2 Cl 5 Z. anorg. 1894, 8. 126.) 0.49 2.91 CsHg 2 Cl 5 Cs 2 CoCl 4 . Decomp. by H 2 O and by al- 0.40 3.78 CsHg.CU+CsHgsCln cohol. (Campbell, Z. anorg. 1894, 8. 126.) 0.44 4.63 u Cs 3 CoCl 5 . Decomp. by H 2 O and by al- 0.41 0.25 4.68 5.65 CsHg 5 Cl u cohol. (Campbell, Z. anorg. 1894, 8. 126.) 0.18 7.09 CsHg 5 Cln+HgCl 2 Caesium cuprous chloride, CsCl, Cu 2 Cl 2 . 0.00 6.90 HgCl 2 Decomp. by H 2 O into CuCl 2 , CsCl. (Wells, (Foote, Am. Ch. J. 1903, 30. 340.) Z. anorg. 5. 306.) 3CsCl, Cu 2 Cl 2 . (Wells.) 6CsCl, Cu 2 Cl 2 . (Wells.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) 100 g. solution in acetone sat. at 25 con- tain 0.032 g. CsCl. (Foote and Haigh, J. Am. Chem. Soc. 1911, 33. 461.) Caesium cupric chloride, 2CsCl, CuCl 2 . Easily sol. in H 2 O and dil. HCl+Aq; insol. in cone. HCl+Aq. (Godeffroy, B. CASIUM SAMARIUM CHLORIDE 141 Sol. in small amount H 2 O without decomp. (Wells and Dupee, Z. anorg. 6. 300.) +2H 2 O. Efflorescent. (W. and D.) 3CsCl, 2CuCl 2 +2H 2 O. CsCl, CuCl 2 . Sol. in H 2 O without decomp. (W. and D.) Caesium gold chloride. See Chloraurate, caesium. Caesium indium See Chloriridate, caesium. Caesium iron (ferric) chloride, CsFeCl 4 Sol. in H 2 O. Decomp. in the air. (Wai- den, Z. anorg. 1894, 7. 332.) <* Cs 2 FeCl 5 +H 2 O. Sol. in H 2 O. (Walden.) Cs 3 FeCl 6 +H 2 O. Sol. in H 2 O. (Walden.) Caesium lanthanum chloride, Cs 3 LaCl 6 + 4H 2 O. Very hydroscopic. Easily sol. in H 2 O. (R. J. Meyer, Z. anorg. 1914, 86. 273.) Caesium lead chloride, CsCl, 2PbCl 2 . Nearly stable in aqueous solution. (Camp- bell, Sill. Am. J. 145. 126.) CsCl, PbCl 2 . Decomp. by H 2 O. (Camp- bell.) 4CsCl, PbCl 2 . As above. (Campbell.) Caesium lead te/rachloride. See Chloroplumbate, caesium. Caesium magnesium chloride, CsCl, MgCl 2 + 6H 2 O. Sol. in H 2 0. anorg. 5. 275.) Caesium manganous chloride, CsCl, MnCl 2 + 2H 2 O. Not deliquescent; sol. in H 2 O. (Saunders, Am. Ch. J. 14. 143.) 2CsCl, MnCl 2 . (Godeffroy.) +2^H 2 0. (Godeffroy.) +3H 2 O. Sol. in H 2 O. Cone. HCl+Aq precipitates anhydrous salt from aqueous solution. (Godeffroy, B. 8. 9.) The only salt which exists contains 2H 2 O. (Saunders, Am. Ch. J. 14. 143.) Caesium manganic chloride, 2CsCl, MnCls. Easily decomp. (Meyer and Best, Z anorg. 1899, 22. 187.) (Wells and Campbell, Z. Caesium mercuric chloride, CsCl, HgCl 2 . 100 pts. solution sat. at 17 contain 1.406 pts. CsHgCl 3 . Not decomp. by H 2 O. Insol in absolute alcohol, but sol. on diluting witt Va vol. H 2 O. (Wells, Sill. Am. J. 144. 221.) 2CsCl, HgCl 2 . Easily sol. in H 2 O and dil HCl+Aq; insol. in cone. HCl+Aq. (Godef- froy.) 3CsCl, HgCl 2 . Decomp. by HoO; on re- crystallizing from H 2 O, CsCl, HgCl 2 is finally formed. (Wells, Sill. Am. J. 144. 221.) CsCl, 5HgCl 2 . Decomp. by H 2 O. (Wells.) Solubility determinations show that the only double salts of CsCl and HgCl 2 which exist at 25 are Cs 3 HgCl 5 , Cs 2 HgCl 4 , CsHgCl 3 , CsHg 2 Cl 5 , CsHg 5 Cl n . (Foote, Am. Ch. J. 1903, 30. 340.) Caesium molybdenum chloride, Cs 2 MoCl 5 + . H 2 G. Sol. in H 2 O. Nearly insol. in alcohol and ether. (Chilesotti, C. C. 1903, II. 652.) Caesium molybdenyl chloride, CsCl, MoO 2 Cl 2 +H 2 O. Hygroscopic. Decomp. by H 2 O. (Wein- and and Knoll, Z. anorg. 1905, 44. 93.) 2CsCl, MoO 2 Cl 2 . Hygroscopic. Decomp. 3y H 2 O. (Weinland and KnoH, Z. anorg. 1905, 44. 92.) 2CsCl, 6MoO 2 Cl 2 +22H 2 O. Very hygro- scopic. Decomp. by H 2 O. (Weinland and Knoll, Z. anorg. 1905, 44. 94.) 2CsCl, MoOCl 3 . Only si. sol. in H 2 O. :Nordenskjold, B. 1901, 34. 1573.) Caesium neodymium chloride, Cs 3 NdCl 6 + 5H 2 O. Very hydroscopic. Easily sol. in H 2 O. R. J. Meyer, Z. anorg. 1914, 86. 273.) ;sesium nickel chloride, 2CsCl, NiCl 2 . As the corresponding Cu salt. CsNiCl 3 . Decomp. by H 2 O and by alcohol. (Campbell, Am. J. Sci. 1894, (3) 48. 418.) Caesium palladium ^chloride. See Chloropallad ; te, caesium. Caesium palladium /drachloride. See Chloropalladate, caesium. Caesium praseodymium chloride, Cs 3 PrCl 6 + 5H 2 0. Very hydroscopic. Easily sol. in H 2 O. (R. J. Meyer, Z. anorg. 1914, 86. 273.) Caesium rhodium chloride. See Chlororhodite, caesium. Caesium ruthenium chloride. See Chlororuthenite, caesium and chloro- ruthenate, caesium. Caesium oa:?/ruthenium chloride, Cs 2 RuO 2 Cl 4 . Ppt.: decomp. by H 2 O; sol. in cold HC1. (Howe, J. Am. Chem. Soc. 1901, 23. 779.) Caesium samarium chloride, Cs 3 SmCl6+ 5H 2 0. Very hydroscopic. Easily sol. in H 2 O. (R. J. Meyer, Z. anorg. 1914, 86. 273.) 142 OfcSIUM SILVER CHLORIDE Caesium silver chloride, 2CsCl, AgCl. Easily decomp. by H 2 O. (Wells and Wheeler, Sill. Am. J. 144. 155.) Caesium tellurium chloride. See Chlorotellurate, caesium. Caesium thallic chloride, 2CsCl, T1C1 3 . By recryst. from H 2 O forms 3CsCl, 2T1C1 3 . (Pratt, Am. J. Sci. 1895, (3) 49. 398.) +H 2 O. Readily sol. in hot H 2 O but SCsCl, 2T1C1 3 cryst. from the solution. (Pratt, Am. J. Sci. 1895, (3) 49. 399.) SCsCl, 2T1C1 3 . Can be recryst. from H 2 O without change. (Pratt, Am. J. Sci. 1895, (3) 49. 401.) 3CsCl, T1C1 3 +2H 2 O. Sol. in 36.4 pts. H 2 O at 17 and 3 pts. at 100. (Godeffroy, Zeitsch. d. allgem. osterr. Apothekerv. 1880. No. 9.) Caesium tin (stannic) chloride. See Chlorostannate, caesium. Caesium titanium chloride, TiCl 3 , 2CsCl + H 2 0. Difficultly sol. in H 2 O. (Stabler, B. 1904, 37. 4409.) Caesium tungsten chloride, Cs 3 W 2 Cl 9 . Nearly insol. in cold H 2 O. Sol. in a hot mixture of equal pts. H 2 O and cone. HC1. Nearly insol. in cone. HC1. Sol. in very dil. NaOH+Aq. Nearly insol. in most organic solvents. (Olsson, B. 1913, 46. 574.) Caesium uranous chloride, Cs 2 UCl 6 . As K salt. (Aloy, Bull. Soc. 1899, (3) 21. 264.) Caesium uranyl chloride, 2CsCl, (UO 2 )C1 2 . Sol. in H 2 O. (Wells, Z. anorg. 1895, 10. 183.) 100 pts. of the solution contain at 29.75, 56.07 pts. UO 2 C1 2 , 2CsCl. (Rimbach, B. 1904, 37. 468.) Pptd. from aq. solution by gaseous HC1. (Wells, Am. J. Sci. 1894, (3) 60. 251.) Caesium vanadium chloride, Cs 2 VdCl 5 +H 2 O. Difficultly sol. in H 2 O and alcohol. (Stab- ler, B. 1904, 37. 4412.) Caesium zinc chloride, SCsCl, ZnCl 2 . Sol. in H 2 O. (Wells and Campbell, Z. anorg. 6. 275.) 2CsCl, ZnCl 2 . Easily sol. in HoO and dil. HCl+Aq. Insol. in cone. HCl+Aq. (Godef- froy.) Caesium chloride chromic oxychloride, 2CsCl, CrOCl 3 . Decomp. in the air. Sol. in cone. HC1 without decomp. (Wein- land, B. 1906, 39. 4045.) Caesium chloride columbium oxychloride, 2CsCl, CbOCl 3 . Decomp. by H 2 O. (Weinland, B. 1906, 39. 3057.) Caesium chloroiodide, CsCl 2 I. Properties as CsBrClI. (Wells.) CsClJ. Si. sol. in H 2 O, from which it can be recrystallized without decomp. (Wells and Wheeler.) Caesium mercuric chloroiodide, Cs 2 HgCl 2 I 2 . Decomp. instantly by H 2 O to HgI 2 . (Wells.) Caesium fluoride, CsF. Ppt. (Chabrie, C. R. 1901, 132. 680.) +1^H 2 0. 100 g. H 2 O dissolve 366.5 g CsF at 15. (de Forcrand, C. R. 1911, 162. 1210.) Caesium hydrogen fluoride, CsHF 2 . Ppt. (Chabrie, C. R. 1901, 132. 680.) Caesium tantalum fluoride. See Fluotantalate, caesium. Caesium tellurium fluoride, CsF,TeF 4 . Decomp. by H 2 O. (Wells, Am. J. Sci. 1901, (4) 12. 190.) Caesium titanium fluoride. See Fluotitanate, caesium. Caesium zirconium fluoride. See Fluozirconate, caesium. Caesium hydride, CsH. Decomp. by H 2 O with evolution of H 2 . (Moissan, C. R. 1903, 136. 589.) Caesium hydroxide, CsOH. Very deliquescent, and sol. in H 2 O. Sol. in alcohol. 79.41% CsOH is contained in a sat. aq. solu- tion at 15. (de Forcrand, C. R. 1909, 149. 1344.) 75.08% CsOH is contained in sat. aq. solu- tion at 30. (Schreinemakers, C. C. 1909, I. 11.) Caesium iodide, Csl. Sol. in H 2 O. 100 pts. H 2 O dissolve 44 pts. Csl at 0; 66.3 pts. at 14.5; 160 pts. at 61. Sp. gr. of CsI+Aq sat. at 14 = 1.393. (Betekoff, Bull. Soc. Petersb. (4) 2. 197.) CALCIUM AMALGAM 143 Caesium periodide. Solubility determinations show that CsI 3 and Csls are the only periodides of caesium existing between 4 and +73. (Foote, Am. Ch. J. 1903, 29. 203.) Caesium fniodide, CsI 3 . 1 com. sat. CsI+Aq dissolves 0.0097 g. CsI 3 , and sp. gr. of solution is 1.154. Only si. decomp. by solution in H 2 O. Much more sol. in alcohol than in H 2 O. Not immediately decomp. by ether. (Wells, Sill. Am. J. 143. 17.) Caesium pentaiodide, Csls. Caesium cobalt iodide, Cs 2 CoI 4 . Decomp. by H 2 O. (Campbell, Z. anorg. 1894, 8. 12.) Deliquescent; decomp. by H 2 O and by alcohol. (Campbell, Am. J. Sci. 1894, (3) 48. 418.) Caesium lead iodide, CsPbI 2 . SI. sol. in hot Csl -f Aq. (Wheeler, Sill. Am. J. 145. 129.) Caesium mercuric iodide, Csl, 2HgI 2 . Decomp. by H 2 O finally into HgI 2 . (Wells, Sill. Am. J. 144. 221.) 2CsI, 3HgI 2 . Decomp. by H 2 O finally into Hgl*. Csl, HgI 2 . As above. 2CsI, HgI 2 . Decomp. by H 2 O; insol. in alcohol. 3CsI, HgI 2 . As above. Caesium silver iodide, Csl, Agl. (Penfield, Z. anorg. 1. 100.) Csl, 2AgI. More sol. in hot than in cold acetone. (Marsh, Chem. Soc. 1913, 103. 782.) Caesium tellurium iodide. See lodotellurate, caesium. Caesium thallic iodide, Csl, T1I 3 . Decomp. by H 2 O. (Pratt, Am. J. Sci. 1895, (3) 49. 403.) Caesium zinc iodide, 3CsI, ZnI 2 . Sol. in H 2 O. (Wells and Campbell, Z. anorg. 5. 275.) 2CsI, ZnI 2 . As above. Caesium oxide, Cs 2 O. Absorbs H 2 O and CO 2 from the air. Decomp. by H 2 O and by liquid NH 3 . (Ren- gade, C. R. 1906, 143. 593.) Caesium dioxide, Cs 2 O 2 . Decomp. by H 2 O. (Rengade, C. R. 1905, 140. 1537.) Caesium In'oxide, Cs 2 Os. Decomp. by H 2 O. (Rengade, C. R. 1905, 140. 1537.) Caesium tefroxide, Cs 2 O 4 . Decomp. by H 2 O. (Rengade, C. R. 1905, 140. 1538.) Caesium sulphide, Cs 2 S+4H 2 O. Deliquescent; very sol. in H 2 O. (Biltz, Z. anorg. 1906, 48. 300.) Caesium bisulphide, Cs 2 S 2 . Anhydrous. Sol. in H 2 O. Hydroscopic. (Biltz, Z. anorg. 1906, 60. 72.) +H 2 O. From Cs 2 S 2 +Aq. Hydroscopic. (Biltz, Z. anorg. 1906, 50. 72.) Caesium /nsulphide, Cs 2 S 3 . Anhydrous. Sol. in H 2 O. Not hydroscopic. (Biltz, Z. anorg. 1906, 50. 75.) +H 2 O. From Cs 2 S 3 +Aq. (Biltz, Z. anorg. 1906, 50. 76.) Caesium te^rasulphide, Cs 2 S4. Sol. in H 2 O. Insol. in abs. alcohol. (Biltz, Z. anorg. 1906, 48. 305.) Caesium perctasulphide, Cs 2 S 6 . Mpt. 2. Not hydroscopic. Very sol. in cold 70% alcohol. (Biltz, B. 1905, 38. 129.) Caesium hydrogen sulphide, CsHS. Deliquescent; very sol. in H 2 O. (Biltz, Z. anorg. 1906, 48. 300.) Caesium copper tefrasulphide, CsCuS 4 . SI. sol. in cold H 2 O. Decomp. by cone, and dil. HC1, H 2 SO 4 and HNO 3 . SI. sol. in alcohol. (Biltz, B. 1907, 40. 978.) Calcium, Ca, Decomp. H 2 O violently. Slowly attacked by cold H 2 S0 4 . Dil. H 2 S0 4 +Aq or HCl+Aq attack violently and dissolve. Dil. HNO 3 + Aq oxidizes, but fuming HNO 3 scarcely at- tacks even on boiling. (Bunsen and Matthies- sen ) Not attacked by anhydrous alcohol. (Lies-Bodart and Jobin, A. ch. (3) 54. 364.) Pure Ca is only very slowly decomp. by H 2 O at ordinary temp.; sol. in HC1, HNO 3 , H 2 SO 4 . (Moissan, C. R. 1898, 129. 589.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) YL com. oleic acid dissolves 0.0334 g. Ca in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Calcium amalgam, Ca 3 Hg 4 . Decomp. H 2 O readily. (Fere, C. R. 1898, 127. 619.) CaHg 5 . Rapidly decomp. in moist air. (Schiirger, Z. anorg. 1900, 25. 425.) 144 CALCIUM AMIDE Calcium amide, Ca(NH 2 ) 2 . (Moissan, A. ch. 1899, (7) 18. 326.) Calcium ammonia, Ca, 4NH 3 . Decomp. at ordinary temp.; takes fire in contact with the air; si. sol. in liquid NH 3 . (Moissan, C. R. 1898, 127. 691.) Ca,6NH 3 . (Kraus, J. Am. Chem. Soc. 1908, 30. 665.) Calcium arsenide, Ca 3 As 2 . Decomp. by cold H 2 O; insol. in cold fuming HNO 3 ; very sol. in hot HNO 3 . (Lebeau, C. R. 1899, 128. 98.) Calcium azoimide, Ca(N 3 ) 2 . Hydroscopic; explosive. 38.1 pts. sol. in 100 pts. H 2 O at 45.0 " " " 100 " H 2 O " 15.2 0.211 " " " 100 " abs. alcohol " 16. Sol. in H 2 O; decomp. when heated and on standing in the air. (Dennis, Z. anorg. 1898, 17. 21.) Insol. in pure ether. (Curtius, J. pr. 1898, (2) 68. 286.) Calcium boride, CaB 6 . Not decomp. by H 2 O at 250; sol. in fused oxidizing agents. Insol. in aq. acids; si. sol. in cone. H 2 SO 4 ; sol. in dil. or cone. HNO 3 . (Moissan, C. R. 1897, 125. 631-32.) Calcium bromide, CaBr 2 . Very deliquescent. 100 pts. H 2 O dissolve at 20 40 C 60 C 105 125 143 213 -278 312 pts. CaBr 2 . (Kremers, Pogg. 103. 65.) Sat. CaBro+Aq contains at: 22 22 14 7 5 C 50.5 50.2 52.5 52.6 52.6% CaBr 2 +8 9 11 20 50 53.1 55.1 55.7 57.1 62.6% CaBr 2 (fitard, A. ch. 1894, (7) 2. 540.) Sp. gr. of CaBr 2 +Aq at 19.5 containing: 5 10 15 20 25 %CaBr 2 , 1.044 1.089 1.139 1.194 1.25? 30 35 40 45 50 % CaBr 2 . 1.315 1.385 1.461 1.549 1.641 (Kremers, Pogg. 99. 444, calculated by Ger- lach, Z. anal. 8. 285.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Very sol. in alcohol. (Henry.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Sol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) +4H 2 O. (Kuznetzov, C. A. 1911. 842.) +6H 2 O. Calcium manganous bromide, GaMnBr 4 + 4H 2 O. SI. hydroscopic. Unstable. (Ephraim, Z. anorg. 1910, 67. 377.) Calcium mercuric bromide. Decomp. by H 2 O. (v. Bonsdorff.) Calcium molybdenyl bromide, CaBr 2 , 2MoOBr 3 +7H 2 O. (Weinland and Knoll, Z. anorg. 1905, 44. 112.) Calcium stannic bromide. See Bromostannate, calcium. Calcium bromide ammonia, CaBr 2 , 6NH 3 . Sol. in H 2 O. (Rammelsberg, Pogg. 56. 239.) Calcium bromide hydrazine, CaBr 2 , 3N 2 H 4 . Easily sol. in H 2 O. (Franzen, Z. anorg. 1908, 60. 288.) Calcium bromofluoride, CaBr 2 , CaF 2 . Decomp. by H 2 O. (Defacqz, A. ch. 1904, (8) 1. 357.) Calcium carbide, CaC 2 . Sp. gr. 2.22 at 18. Insol. in fuming HNO 3 and cone. H 2 SO 4 but readily decomp. by dil. acids and H 2 O. (Moissan, Bull. Soc. 1894, (3) 11. 1005.) Insol. in HC1 in the cold, but decomp. at red heat. Strong min. acids do not act in the cold; sol. in glacial acetic in the cold; sol. in fused alkali. (Venable, J. Am. Chem. Soc. 1895, 17. 307-310.) Calcium chloride, CaCl 2 . Very deliquescent. Veiy sol. in H 2 O with evolution of heat. Anhydrous CaCh is sol. in 1.459 pts. H2O. (Gerlach.) Anhydrous CaCl 2 is sol. in 1.58 pts. H 2 O at 10.2. (Kremers, Pogg. 103. 65.) - Anhydrous CaCh is sol. in 1.35 pts. H 2 O at 20; O.S3 pt. H 2 at 40; 0.72 pt. H 2 O at 60. CaCh+6H s O is sol. in 0.5 pt. H 2 O at 0, and 2.05 pt. at 16. (Gmelin.) CaCl 2 is sol. in 1.5 pts. cold, and 0.8 pt. boiling H 2 O. (Fourcroy.) CaClz+Aq sat. in the cold contains 40.7% CaCK>. (Fourcroy.) CaCl 2 +Aq sat. at 12.5 contains 53.8% CaCl 2 . (Hassenfratz.) 100 pts. H 2 O dissolve 165.7 pts. CaCl 2 + 6H 2 O at 0; 7141 pts. at 40. (Tilden, Chem. Soc. 45. 409.) 100 pts. H 2 O dissolve 60.3 pts. CaCl 2 from CaCl 2 +6H 2 O at 0, and solution has sp. gr. = 1.367. (Engel, Bull. Soc. (2) 47. 318.) CALCIUM CHLORIDE 145 Solubility of CaCl 2 +6H 2 O in H 2 O at t. If so 100 pts to +6 (Etard, Acco] bility oi employ tained Solubili [ubility S=pts. anhydrous C . solution, S = 32+0.2148t fron ; S = 54.5+0.0755t from 50 t C. R. 98. 1432.) ding to Bakhuis Roozeboom, t CaCl 2 varies according to the ] 3d, and the following data w is the result of very exact exper ty of CaCl 2 +6H 2 O in 100 pt at t. aC! 2 in t Sat. solution contains % CaCh Sat. solution contains %CaCh+6H 2 i 18 o 120. le solu- lydrate ere ob- iments. s. H 2 22 + 7.39 13.86 19.35 23.46 24.47 27.71 29.53 32.24 36.91 ' 38.77 41.03 42.50 44.15 45.33 46.30 50.67 63.61 72.82 76.49 80.95 83.85 87.11 89.44 91.35 99.97 t Pts. CaCh t Pts. CaCh t Pts. CaCh (Hammerl, W.A.B. 72, 2. 287.) Solubility in 100 pts. H 2 O at t. 20.4 25.05 75.1 81.67 28.0 28.9 88.8 92.05 29.5 30.2 96.07 102.7 t Pts. CaCh t Pts. CaC h There are two modifications of CaCl 2 + 4H 2 O, a and/3. Solubility of CaCl 2 H-4H 2 O|8 in 100 pts. H 2 O at t. 59.39 5 64.83 7.88 66.20 13.86 69.49 19.35 73.91 21.89 79.77 (Hammerl, calculated by Bakhuis Rooze boom, R. t. c. 8. 5.) Solubility in 100 pts. H 2 O at t. t Pts. CaCh t Pts. CaCh t Pts. CaCh t Pts. CaCh t Pts. CaCh 18.4 25 30.0 103 3 108.8 114.1 35.0 122.74 38.4 127.50 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 49.6 50 51 52 53 54 55 56 57 58 60 61 62 63 65 66 68 69 71 127 128 129 129 130 131 131 132 133 133 134 135 135 136 136 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 72 74 75 77 79 80 82 84 87 89 91 93 96 98 100 103 104 105 107 137 138 138 139 139 140 141 141 142 142 143 143 144 144 145 38 39 40 41 '42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 87 88 89 90 91 92 93 94 95 96 97 98 99 179.5 108 109 110 111 112 113 114 115 116 117 118 119 120 121 122 123 124 125 126 145 146 147 147 148 149 150 150 151 152 152 153 154 325 Solubility of CaCl 2 +4H 2 Oa in 100 pts. H 2 O att. t 22.0 24 7 29 8 Pts. CaCh t Pts. CaCh 92 67 95.59 100.6 35.95 40.00 45.00 107.21 115 3 129.9 Solubility of CaCl 2 +2H 2 O in 100 pts. H 2 O att. t Pts. CaCh t Pts. CaCh t Pts. CaCh 40 45 50 1 59.5 1 80.5 ] [28.1 [29.9 [32.3 [36.5 [45.3 95.8 115 124 137 156.5 169.5 176.0 187.6 139 155 165 174 191.0 214.3 236.2 275.7 Solubility of CaCl 2 +H 2 O in 100 pt at t. s. H 2 O t Pts. CaCh 191 235 306 331 (Mulder, Scheik. Verhandel. 1864. 107.) (Bakhuis Roozeboom, R. t. c. 8.1.) 146 CALCIUM CHLORIDE Sp. gr. of CaCl 2 +Aq. CaCl 2 Sp. gr. c?h, Sp. gr. % CaCh Sp. gr. 3.95 7.66 11.23 14.42 17.60 1.03 1.06 1.09 1.12 1.15 20.85 23.93 26.86 29.67 32.35 .18 .21 .24 .27 .30 34.57 36.49 38.31 40.43 41.91 1 . 33 1.36 1.39 1.42 1.45 (Richter.) Sp. gr. of CaCU+Aq at 19.5 containing pts. CaCl 2 to 100 pts. H 2 O. Pts. CaCh Sp. gr. Pts. CaCl 2 Sp. gr. 6.97 12.58 23.33 1.0545 1.0954 1 . 1681 36.33 50.67 62.90 1 . 2469 1.3234 1 . 3806 (Kremers, Pogg. 99. 444.) Sp. gr. of CaCl 2 +Aq. G = sp. gr. at 15 if % is CaCl 2 , according to Gerlach; S = sp. gr. at 18.3 if % is CaCl 2 -f6H 2 O, according to Schiff. Sp. gr. of CaCl 2 +Aq : a = nb. of half molecules in grammes dissolved in 1000 g. H 2 O; b = sp. gr. at 24.3 when a = CaC! 2 + 6H 2 O (Y 2 mol. = 109.5 g.); c = sp. gr. at 24.3 when a = CaC! 2 (^ mol.=55.5 g.). a b c a ' b o 1 2 3 4 5 6 .041 .076 .106 .133 .157 1 . 179 1.043 1.084 1.122 1.159 1.193 1 227 7 8 9 10 11 1.198 1.214 1.229 1.242 1.255 1.25S (Favre and Valson, C. R. 79. 968.) Sp. gr. of CaCl 2 +Aq at 18. % CaCl 2 5 10 15 20 Sp. gr. 1 . 0409 1.0852 1.1311 1 . 1794 % CaCl 2 25 30 35 Sp. gr. 1.2305 1.2841 1.3420 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 G .00852 .01704 .02555 .03407 . 04259 .05146 .06033 .06921 .07808 .08695 .09628 .00561 . 10494 . 12427 . 13360 . 14332 . 15305 . 16277 . 17250 . 18222 . 19251 . 20279 .21308 .22336 .23365 . 24450 .25535 .26619 .27704 28789 .29917 .31045 . 32174 .33602 34430 8 1.0039 1.0079 1.0119 1.0159 1.0200 1.0241 1.0282 1.0323 1.0365 0407 0449 0491 0534 0577 0619 0663 1.0706 1.0750 1.0794 1.0838 1.0882 1 0927 0972 1017 1062 1107 1153 1199 1246 1292 1339 1386 1.1433 1.1480 1 . 1527 35610 36790 37970 39150 40330 1 . 1575 .1622 .1671 .1719 .1768 .1816 .1865 .1914 .1963 .2012 .2062 .2112 .2162 .2212 .2262 .2312 .2363 .2414 .2465 .2516 .2567 .2618 .2669 .2721 .2773 .2825 .2877 .2929 .2981 .3034 .3087 .3140 .3193 .3246 .3300 (Kohlrausch, W. Ann. 1879. 1.) CaCl 2 +Aq sat. at has sp. gr. = 1.367. (Engel, Bull. Soc. 1887, (2) 47. 318.) Sp. gr. of CaCl 2 +Aq at 9.5C. Mass of salt per unit mass of solution 0.00191 0.00381 0.00570 0.00759 0.00947 0.01320 Density of solution (g. per cc.) 1.00168 1.00317 1 . 00465 1.00615 1.00765 1.01050 (McGregor, C. N. 1887, 55. 6.) Sp. gr. of CaCl 2 +Aq at 25. Concentration of CaCl 2 +Aq. Sp. gr. 1-normal j/r- ;; Vs- " 1.0446 1.0218 1.0105 1.0050 (Calculated by Gerlach, Z. anal. 8, 283.) (Wagner, Z. phys. Ch. 1890, 5. 36.) Sp. gr. at 16/4 of CaCl 2 +Aq containing 12.1638% CaCl 2 = 1.10489. (Schonrock, Z. phys. Ch, 1893, 11. 768.) CALCIUM CHLORIDE 147 Sp. gr. of CaCl 2 +Aq at 17.925C. B.-pt. of CaCl 2 100 pts. H (Z. anal. 2 grand (A. -f-Aq containin 2 O G accord I pts. CaCl 2 to ing to Gerlach cording to Le- % CaCh Sp. gr. CaCU Sp. gr. % CaCl Sp. gr. 6. 440); L = ac 3h. (2) 39. 43). 0.0 0.1 0.2 0.3 0.4- 0.6 0.8 1.0 1.5 2 3 4 5 6 7 8 9 10 11 12 0.99869 0.99954 1.00037 1.00116 1.00201 1.00371 1.00539 1.00703 1.01127 1.01548 1 . 02386 1.03238 1.04089 1.04951 .05822 .06680 1.07569 .08467 1.09373 1 . 10288 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 .11206 . 12130 . 13067 . 14016 . 14960 . 15926 . 16920 . 17910 1.18897 1.19901 1.20901 1.21918 1 . 22941 1.23969 1.25030 1.26092 1.27182 1.28271 1.29360 1.30461 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 1.31562 .32689 .33821 .34956 .36100 .37242 1.38400 1.39489 1.40641 1.41770 .42882 .44007 .45124 . 46238 .47329 .48450 .49573 .50676 .51778 B.-pt G L B.-pt. G L 101 102 103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 119 120 121 122 123 124 125 126 128 130 130.4 132 6.0 11.5 16.5 21.0 25.0 29.0 32.5 35.5 38.5 41.5 55^0 69.0 ioi 102.67 10 16.5 21.6 25.8 29.4 32.6 35.6 38.5 41.3 44.0 46.8 49.7 52.6 55.6 58.6 61.6 64.6 67.6 70.6 73.6 76.7 79.8 82.9 86.0 89.1 92.2 98.4 104.6 110.9 134 135 136 138 140 142 144 145 146 148 150 152 154 155 156 158 160 162 164 165 166 168 170 172 174 175 176 178 179.5 119 137^5 157 178 200" 222 245 268 ' 292 305 117.2 123.5 129.9 136.3 142.8 149.4 156^2 163.2 170.5 178.1 186.0 194^3 203.0 212.1 221.6 231.5 241.9 252.8 264.2 276.1 285.5 301.4 314.8 325.0 (Pickering, B. 1894, 27. 1385.) Sp. gr. of CaCl 2 +Aq at t. t Concentration of CaCh +Aq Sp. gr. 20 20 1 pt. CaCl 2 in 7.1045 pts. H 2 O 1 " " " 164.25 " " 1.1062 1.0032 (Hittorf, Z. phys. Ch. 1902, 39. 628.) Sp. gr. of CaCl 2 +Aq at 20. B.-pt. of CaCl 2 +Aq. % CaCl 2 B.-pt. % CaCU B.-pt. g. mols. CaCh per 1. Sp. gr. 5.6 101 10.3 102 14.5 103 17.5 104 20.0 105 0.010 .000982 0.025 .002539 0.050 .004874 0.075 .006814 0.10 .008971 0.25 .02267 0.50 .04451 0.75 .06641 1.00 1.08744 (Skinner, Chem. Soc. 61. 340.) Less sol. in HCl+Aq than in H 2 O. HCl-h Aq sat. at 12 dissolves 27% CaCl 2 , which crystallizes out with 2H 2 O. (Ditte, C. R. 92. 242.) Solubility of CaCl 2 in HCl+Aq at 0. (Jones and Pearce, Am. Ch. J. 1907, 38. 606.) Sat. CaCl2+Aq forms a crust at 150, and contains 178 pts. CaCl 2 to 100 pts. H 2 O. (Gerlach.) Sat. CaCl 2 +Aq boils at 180. (Riidorff.) Sp. gr. of solutions g. per 100 cc. solution CaCIj HCl 1.367 1.344 1.326 1.310 1.283 1.250 1.238 51.45 46.45 42.80 36.77 29.84 20.12 11.29 0.0 3.32 5.83 10.66 15.84 23.05 34.62 (Engel, C. R. 1887, 104, 434.) 148 CALCIUM CHLORIDE CaCl 2 +CaO 2 H 2 . Solubility of CaCl 2 + CaO 2 H 2 in H 2 O at 25. Solubility of CaCl 2 , 4CH 3 OH in CH 3 OH. t % by weight of CaCh, 4CH 3 OH CaCh CaO 2 H 2 Solid phase 10 20 30 40 50 55 56 33.3 37.6 42.2 47.0 52.0 57.3 60.0 61.3 5.02 10.00 12.94 15.14 17.20 18.15 18.01 21.02 23.80 24.33 28.37 29.54 32.67 33.21 33.72 34.36 38.61 41.32 44.30 44.60 44.77 0.101 0.115 0.128 0.140 0.145 0.148 0.152 0/147 0.146 0.147 0.170 0.180 0.225 0.245 0.254 0.173 0.060 0.048 0.030 0.029 Ca0 2 H 2 CaChHz-fCaCh, 4CaO.14H 2 O CaCh, 4CaO.14H 2 O Ca0 2 H 2 (?) CaCh, 4CaO.14H 2 O CaCh, 4Ca0.14H 2 0+CaCh, Ca0.2H 2 CaCh, CaO.2H 2 CaCh, 6H 2 0+CaCl 2 , CaO.2H 2 O CaCl 2 .6H 2 Solubility of CaCl 2 , 3CH 3 OH in CH 3 OH. t % by weight of CaClz, 3CH 3 OH 55 75 95 115 135 155 165 170 174 177 (mpt.) 60.5 63.1 66.3 70.3 75.2 81.8 86.2 U 89.5 93.5 100 (Menschutkin, Z. anorg. 1907, 62. 21.) (Schreinemakers and Figee, Chem. Weekbl. 1911, 8. 685.) See also under Calcium hydroxide CaCl 2 +KC1. 100 pts. H 2 O dissolve 56 pts. CaCl 2 at 7; 100 pts. H 2 O dissolve 31 pts. KC1 at 7; 100 pts. H 2 O dissolve 63.5 pts. CaCl 2 +4.9 pts. KC1 at 7. (Mulder, J. B. 1866. 67.) CaCl 2 +NaCl. 100 pts. H 2 O dissolve 53 S,s. CaCl 2 at 4, and 56 pts. at 7; 100 pts. 2 O dissolve 35.7 pts. NaCl at 4, and 35.7 pts. at 7; IOC pts. H 2 O dissolve 57.6 pts. CaCl 2 +2.4 pts. NaCl at 4; 100 pts. H 2 O dis- solve 59.5 pts. CaCl 2 +4.6 pts. NaCl at 7. (Mulder, I. c.) 100 g. H 2 O dissolve 72.6 g. CaCl 2 + 16.0 g. NaCl at 15. (Riidorff.) Sol. in sat. KNO 3 +Aq. (Fourcroy.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Sol. in 1 pt. strong boiling alcohol. (Wen- zel.) Sol. in 8 pts. alcohol at 15, and in 1 pt. spirits of wine. (Bergman.) Sol. in 0.7 pt. boiling absolute alcohol. (Otto.) Sol. in 1.43 pts. boiling absolute alcohol at 78.3. (Graham.) Solubility of CaCl 2 in methyl alcohol. CaCl 2 forms with methyl alcohol two com- plexes: CaCl 2 .4CH 3 OH and CaCl 2 .3CH 3 OH. Solubility of CaCl 2 in ethyl alcohol. CaCl 2 forms with ethvl alcohol a complex, CaCl 2 .3C 2 H 5 OH. Solubility of CaCl 2 .3C 2 H 5 OH in C 2 H 5 OH att. t % by weight of CaCh.3C 2 H 5 OH t % by weight of CaCl' 2 .3C 2 HbOH 34.8 80 86.8 20 46.0 85 89.2 40 58.7 90 91.9 60 73.0 95 96.2 70 80.8 97 mpt. 100 (Menschutkin, Z. anorg. 1907, 52. 23.) Sp. gr. at 1674 of CaCl 2 +alcohol con- taining 5.668% CaCl 2 = 0.83636. (Schonrock, Z. phys. Ch. 1893, 11. 768.) B.-pt. of an alcoholic solution of CaCl 2 . % CaCh B.-pt. 2.4 5.39 8.01 9.93 15.94 78.43+ 0.70 78.43 + 2.15 78.32 + 4.18 78.43 + 5.55 78.43 +11.75 (Skinner, Chem. Soc. 61. 340.) SI. sol. in propyl alcohol. (Berthelot.) 100 g. propyl alcohol dissolve 10.75 g. CaCl 2 . (Schlamp, Z. phys. Ch. 1894, 14, 276.) SI. sol. in amyl alcohol. (Bouis.) Pptd. from alcoholic solution by ether. (Dobbereiner.) CALCIUM CHLORIDE 149 Sol. in wood-spirit; sol. in lignone (Liebig); insol. in lignone. (Gmelin.) Insol. in acetone; sol. in butyl alcohol. (Wurtz.) Very si. sol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Solubility in acetone +Aq at 20. Sol. in many compound ethers, as ethyl acetate (Liebig), ethyl lactate (Strecker). Sol. in considerable quantity in amyl sul- phocyanide. (Medlock, Chem. Soc. 1. 374.) Sol. in valyl. (Kolbe.) Very sol. in cone. HC 2 H 3 O 2 . (Liebig.) Solubility of CaCl 2 in acetic acid. CaCl 2 will salt out acetone from aqueous solution. The table shows the composi- V^CtV^J.2 1W1111O Wltll CVVVVIW dl/lvl Ct ljVlllJl. \7JVp CaCl 2 , 4CH 3 COOH. tion of the solutions at the points at which inhomogeneous solutions of CaCl 2 , acetone and H 2 O just become homogen- Solubility of CaCl 2 , 4CH 3 COOH in CH 3 COOH at t. eous at 20 . 1 00 g . of the solution c ontain : t % by wt. CaCh, 4CH 3 COOH g. CaCl 2 g. H 2 K. acetone 11.1 42.0 QA 47 fi 13.03 52.49 34.48 ou 35 TT / . U 50.0 . 8.5 45.37 46.15 40 54.7 6.38 39.51 54.11 45 63.0 5.35 35.95 58.70 50 69.5 4.11 31.8 64.09 60 79.5 3.58 29.88 66.54 65 84.5 3.31 28.59 68.10 70 91.2 3.04 27.03 69.93 *7f\ CT* 73 100.0 2.77 13.90 26.67 53.47 70.56 32.63 (Menschutkin , Z. anorg. 1907, 54. 95.) 10 12 48 86 41 02 -Ll_f . i 8.47 45 '.59 45 '.94 Insol. in benzonitrile. (Naumann, B. 1914, 6.92 6.31 41.24 39.15 51.84 54.54 47. 1370.) Insol. in ethyl acetate. (Naumann, B. 5.28 4.94 4.37 1.99 36.09 34.72 33.8 23.38 58.63 60.34 61.83 74.63 1910, 43. 314.) SI. sol. in anhydrous pyridine. Sol. in 97%, 95% and 93% pyridine +Aq. (Kahlenberg, J. Am. Chem. Soc. 1908, 30. 1.6 1.35 18.787 12.443 10 70 21.4 19.92 55.301 52.153 49 6i 77.00 78.73 25.913 35.404 39 69 1107.) 100 g. sat. solution of CaCl 2 in sat. sugar + Aq at 31.25 contain 42.84 g. sugar+25.25 g. CaCl 2 , or 100 g. H 2 O dissolve 135.1 g. sugar +79.9 g. CaCl 2 at 31.25. (Kohler, Z. Ver. 9^59 8.82 7.48 7 07 47 '.75 46.04 42.75 41 ^4 42.66 45.14 49.77 51 39 Zuckerind, 1907, 47. 447.) +H*O. (Bakhuis Roozeboom.) See above. 4-2H 2 O. (Bakhuis Roozeboom.) See above. +4H 2 O. Two modifications. (Bakfcuis . \j i 6.72 30.04 18.23 15.49 13.18 11.40 28.09 TCi . t^X 40.48 49.39 55.01 54.00 52.52 50.20 51.71 52^8 20.57 26.76 30.51 34.3 38.40 20.20 Roozeboom.) See above, a and /3 modifications (a = stable form.) (Kuznetzov, C. A. 1911, 842.) +6H 2 O. Very deliquescent. Sol. in H 2 O with absorption of much heat. 250 pts. CaCl 2 +6H 2 O with 100 pts. H 2 O at 10.8 lower the temp. 23.2. (Riidorff, B. 26.81 22.67 18.189 52.01 55.66 56.21 21.18 21.67 25.60 ' Melts in crystal H 2 O at 28 (Tilden, Chem. Soc. 45. 409); at 30.2 (Bakhuis Roozeboom.) 31.21 2.23 1.82 0.68 48.00 24.93 22.27 15.87 20.81 72.84 75.89 83.44 Sat. solution in H 2 O contains at: 22 17 5 5 +4 31.5 32.4 35.1 35.2 36.5% salt, 0.58 14.93 84.49 8 22 29 35 49 0.45 13.55 86.00 37.9 42.1 46.1 49.0 55.1% salt, 0.48 14.49 85 . 13 0.27. 12.31 87.42 63 80 104 115 0.20 9.95 89.85 55.9 57.5 58.5 58.6% salt. 0.15 9.05 90.81 (fitard, A ch. 1894, (7) 2. 532.) (Frankforter, J. Am. Chem. Soc. 1914, 36. 1125.) Sat. solution of CaCl 2 +6H 2 O contains 150 CALCIUM HYDROXYLAMINE CHLORIDE 44.77 g. CaCl 2 at 25. (Schreinemakers and Figee, Chem. Weekbl. 1911, 8. 685.) See also above. Solubility of CaCl 2 +6H 2 O in ethyl alcohol-f- Aq under addition of increasing amounts of CaCl 2 . Per cent of alcohol by volume G. CaCh added Grams CaCl 2 in 5 cc. of solution 92.3 1.430 97.3 .409 99.3 .429 1 1 .529 ( 2 .561 * t 3 .590 t 4 .641 1 5 .709 (Bodtker, Z. phys. Ch. 1897, 22. 510.) Calcium hydroxylamine chloride, CaCl 2 , 3NH 2 OH, HC1. (Antonow, J. Russ. Phys. Chem. Soc. 1905, 37. 479.) Calcium iodine bichloride, 2IC1 3 , CaCl 2 + 8H 2 O. Hydroscopic. (Weinland, Z. anorg. 1902, 30. 142.) Calcium mercuric chloride, CaCl 2 , 5HgCl 2 + 8H,0. Decomp. by cold H 2 O, which dissolves out CaCl 2 , but all dissolves on heating, (v. Bons- dorff, 1829.) CaCl 2 , 2HgCl 2 +6H 2 O. Deliquescent. Very sol. in H 2 O. (v. Bonsdorff.) CaCl 2 , 6HgCl 2 +6H 2 O. Very deliquescent. Decomp. by H 2 O. (Stromholm, J. pr. 1902, (2) 66. 521.) Calcium lead chloride, basic. See Calcium lead oxychloride. Calcium magnesium chloride, CaCL, 2MgCl 2 + 12H 2 0. Min. Tachhydrite. Deliquescent. 100 pts. H 2 O dissolve 160.3 pts. at 18.75. By dissolving 20 pts. in 80 pts. H 2 O the temp. is raised 7.75. (Bischof.) Calcium mercuric chloride, basic, CaCl 2 2HgO+4H 2 0. See Calcium mercuric oxychloride. Calcium thallic chloride, 2TlCl 3 ,CaCl 2 + 6H 2 O. Can be cryst. from H 2 O. (Gewecke A 1909, 366. 222.) Calcium tin (stannic) chloride. See Chlorostannate, calcium. Calcium uranium chloride, CaCl 2 ,UCl 4 . Decomp. by H 2 O. (Aloy, Bull. Soc. 1899, (3) 21. 265.) Calcium zinc chloride. CaZnCl 4 +5>fH 2 O, and Ca 2 ZnCl 6 +6H 2 O. Very hydroscopic. (Ephraim, Z. anorg. 1910, 67. 379.) Calcium chloride ammonia, CaCl 2 , 8NH 3 . Sol. in H 2 O with decomp. (Faraday.) Calcium chloride hydrazine, CaCl 2 , 2N 2 H 4 (?). Ppt. (Franzen, Z. anorg. 1908,. 60. 288.) Calcium chloride hydroxylamine, CaCl 2 , NH 2 OH+5H 2 O. Not hygroscopic. (Antonow, J. Russ. Phys. Chem. Soc. 1905, 37. 479.) CaCl 2 , 2NH 2 OH. -f-H 2 O. Aqueous solution sat. at 20 con- tains 56.6 pts. salt. +2H 2 O. (Antonow, I. c.) 2CaCl 2 , 3NH 2 OH+6H 2 O. (Antonow, I. c.) 2CaCl 2 , 5NH 2 OH +4H 2 O. (Antonow, 1. c.) Calcium chloride lead oxide, CaCl 2 , 3PbO + 3H 2 O. See Calcium lead oxychloride. Calcium chloroferrite, CaO, CaCl 2 , Fe 2 O 3 . Insol. in H 2 O. (le Chatelier, C. R. 99. 276.) Calcium chlorofluoride, CaF 2 , CaCl 2 . Decomp. by H 2 O, by very dil. HC1, HNO 3 or acetic acid, by hot dil. or cone. H 2 SO 4 . Sol. in cone. HC1 or HNO 3 . Insol. in, and not decomp. by cold or boiling alcohol. (Defacqz, A. ch. 1904, (8) 1. 355.) Calcium cyanamide, basic, CN 2 (CaOH) 2 -f 6H 2 O. SI. sol. in H 2 O. (Meyer, J. pr. 1878, (2) 18. 425.) Calcium cyanamide, CaCN 2 . Decomp. by H 2 O. (Meyer, J. pr. 1878, (2) 18. 425.) Calcium swbfluoride, CaF. Decomp. by H 2 O. Sol. in hot dil. HC1 and somewhat sol. in dil. acetic acid. Somewhat sol. in boiling abs( (Wohler, Z. anorg. 1909, 61. 81.) Calcium fluoride, CaF 2 . Sol. in 26,923 pts. H 2 O at 15.5. (Wilson, Ch. Gaz. 1850. 366.) 1 1. H 2 O dissolves 16 mg. CaF 2 at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 16.3 mg. in 1 1. of sat. solution at 18. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) CALCIUM HYDROXIDE 151 When pptd. not completely insol. in H 2 O; scarcely sol. in dil., more sol. in cone. HCl-f Aq; decomp. by cone. H 2 SO 4 ; not decomp. by dil. alkaline solutions. (Fresenius.) Not decomp. by cone. H 2 SO 4 below 40, but forms a transparent syrup. CaF 2 is pptd. from this solution by addition of H 2 O. Sol. in cone. HC1, and HNO 3 +Aq in the same way, but the liquid is not viscid. Very si. sol. in HF. Boiling HCl+Aq dissolves slightly. Decomp. by boiling HNO 3 +Aq. Sol. in NH 4 salts +Aq. (Rose.) Partly decomp. by boiling K 2 CO 3 , and Na 2 CO 3 +Aq. (Dulong, A. ch. 82. 278.) Insol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Min. Fluorite (Fluorspar). Calculated from electrical conductivity of CaF 2 +Aq, 1 1. H 2 O dissolves 14 mg. CaF 2 at 18. (Kohl- rausch and Rose, Z. phys. Ch. 12. 241.) Calcium hydrogen fluoride, CaH 2 F 4 +6H 2 O. Decomp. by boiling H 2 O. Sol. in HF+Aq. (Fremy, A. ch. (3) 47. 35.) Calcium tantalum fluoride. See Fluotantalate, calcium. Calcium stannic fluoride. See Fluostannate, calcium. Calcium titanium fluoride. See Fluotitanate, calcium. 4 : Calcium fluoiodide, CaF 2 ,CaI 2 . Very deliquescent. Decomp. by cold H 2 O, more rapidly by hot H 2 O, by dil. HC1, HNO 3 , H 2 SO 4 cone. H 2 SO 4 , and by alcohol and by ether if these reagents are not absolute. (De- facqz, A. ch. 1904, (8) 1. 358.) % Calcium hydride, CaH. Decomp. by HCl+Aq. (Winkler, B. 24. 1975. (Moldenhauer, Z. anorg. 1913, 82. 136.) CaH 2 . Readily decomp. by H 2 O and dil. acids, almost insol. in cone, acids. Insol. in benzene, turpentine and alkyl haloids. (Mois- san, C. R. 1898, 127. 30-31.) Decomp. H 2 O and ether; sol. in dil. H 2 SO and HNO 3 : almost insol. in cone. H 2 SO 4 and HNO 3 . (von Lengyll, C. C. 1898, II. 262.) Insol. in CC1 4 , CS 2 , alcohols and ethers. No known solvent. (Moissan, C. C. 1903, I. 863.) Calcium hydrosulphide, CaS 2 H 2 . Cry st. with 6H 2 O. Extremely sol. in H 2 O and alcohol. l /i of its weight of H 2 O at or- dinary temp, more than suffices to hold it in solution. (Divers and Shimidzu, Chem. Soc. 46. 271.) Sp. gr. of aqueous solution containing 32% anhydrous CaS 2 H 2 (64% CaS 2 H 2 +6H 2 O) = 1.255: 37.5% CaS 2 H 2 (75.5% CaS 2 H 2 + 6H 2 O) = 1 .310. (Divers and Shimidzu.) Calcium hydroxide, CaO 2 H 2 . See also Calcium oxide. SI. sol. in cold, and less in hot H 2 O. 1 pt. CaO dissolves at t in pts. H2O. t Pts. HzO Authority 20 450 Davy. 656 Phillips (A. Phil. 17.. 107) 700 Bei uni an (Essa VS. ( itC.). 13 785 Pavesi and Rotondi (B. 7. 817) 18 780 Bin eai (A. ch. (3) 51. 2< W), 19.5 806 P. and R. (I. c.). 23 814 P. ind R. (I. c. 18.75 960 Ab . 54.4 972 Dalton (Syst. 2. 231). 15.6 778 Da !toi I (I. C.). 15.6 752 Ph nip s (I. c..). 15.6 15.6 731 741 Wittstein (Repert. Pharm. 1. 182). Tichborne (Bull. Soc. (2) 17. 24). 100 1270 Dalton (I. c.). 100 1280 Ph Hip s (I. c.). 100 1330 Wi ttst ein (I. c. 100 1340 Tichborne (I. c.). 100 1500 Bir irill 1 (I. C.). ICO 1758 Tichborne (I. c.). Solubility in sat. H 2 O. 1000 pts. CaO 2 H 2 +Aq at t contain pts. CaO. t Pts. CaO T- From Nitrate Marble Hydrate 1.362 1.381 ] .430 10 1.311 1.342 ] .384 15 1.277 1.299 1 .344 30 1.142 1.162 ] .195 45 0.996 1.005 ; .033 60 0.884 0.868 0.885 100 0.562 0.576 0.584 (Lamy, C. R. 86. 333 ) Solubility of CaO 2 H 2 in H 2 O at t. Pts. H 2 Pts. CaO Pts H 2 O Pts. CaO t to 1 pt. CaO in 100 pts. H 2 O t to 1 pt. CaO in 100 pts. H 2 O 759 0.131 60 1136 0.088 10 770 0.129 70 1235 0.080 20 791 0.126 80 1362 0.073 30 862 0.116 90 1579 0.063 40 932 0.107 100 1650 0.060 50 1019 0.098 (Maben, Pharm. J. Trans. (3) 14. 505.) 1 pt. CaO 2 H 2 is sol. in 640 pts. H 2 O at 19, and 3081 pts. at 150. (Shenstone and Cun- dall, Chem. Soc. 63. 550.) 1000 g. H 2 O dissolve 1.251 g. CaO. (Carles, Arch. Pharm. (3) 4. 558.) 152 CALCIUM HYDROXIDE Solubility of CaO 2 H 2 in H 2 O. 100 pts. H 2 O dissolve pts. CaO at t. Sol. in H 3 BO 3 +Aq at 30. (Sborgi, Real. Ac. Line. 1913, (5) 22. I, 715 and 798.) Sol. in NH 4 Cl-|-Aq. Much more sol. in NaCl+Aq than in H 2 O. (Rose.) Solubility of CaO 2 H 2 in NH 4 Cl+Aq at 25. t Pts. CaO t Pts. CaO 20 40 60 0.1374 0.1162 0.1026 80 100 0.0845 0.0664 Concentration of NH4C1 +Aq in millimols per liter Sorubility of CaO 2 H 2 in millimols per liter (Zahorsky, Z. anorg. 3. 34.) 1 pt. CaO is sol. in pts. H 2 O at t. t 15 20 25 30 35 40 45 pts. H 2 O 776 813 848 885 924 962 1004 0.00 21.76 43.52 87.03 20.22 29.08 39.23 59.68 t 50 55 60 65 70 75 80 pts. H 2 O 1044 1108 1158 1244 1330 1410 1482 (Herzfeld, C. C. 1897, I, 932.) 100 g. sat. CaO 2 H 2 +Aq contain g. CaO at t: t 5 10 15 20 25 g. CaO 0.135 0.1342 0.132 0.1293 0.1254 t 30 35 40 50 60 g. CaO 0.1219 0.1161 0.1119 0.0981 0.0879 t 70 80 90 100 g. CaO 0.0781 0.074 0.0696 0.0597 (Guthrie, J. Soc. Chem. Ind. 1901, 20. 223.) Solubility in H 2 O at high temp. 1 litre of the solution contains at: 120 150 190 0.305 0.169 0.084 g. CaO. (Herold, Z. elektrochem. 1905, 11. 421.) Solubility in H 2 O at t. t 1 g. CaO is sol. in g. HzO at t 2 768.5 10 786.8 15 804.3 20 826.4 25 868.7 30 908.2 40 988.1 50 1083.0 60 1179.0 70 1274.8 80 1368.1 (Moody, Chem. Soc. 1908, 93. 1772.) Sat. CaO 2 H 2 +Aq contains at: 95 76 0.0580 0.0705% by wt. CaO. (Tschugaeff, Z. anorg. 1914, 86. 159.) 100 g. sat. solution of CaO 2 H 2 in H 2 O at 25 contain 0.117 g. CaO 2 H 2 . (Cameron and Potter, J. phys. Ch. 1911, 16. 70.) Reaaily sol. in most acids. - i || i '1 c*~ o* 2 at the ordinary temperature (the solution obtained being of 1.0018 sp. gr.) and pressure, and an additional vol. for the pressure of each additional atmosphere to which it is subjected. The power of H2O to absorb CO2 does not increase in precisely the same ratio as the pressure. (Soubeiran.) 5 vols. CO2 dissolve in 1 vol. EbO at 7 atmos. pressure, and much greater pressure is necessary in order to in- crease the amount of gas dissolved; but up to 4 or 5 atmospheres the amount of gas dissolved is very nearly proportional to the pressure. (Courbe, L Pharm. 26. 121.) 100 vols. H 2 O at 12.78 absorb 116 vols. CO 2 (Caven- dish); at 29.44, 84 vols. CO 2 (Henry); at 15.56, 106 vols. CO2 (Saussure) ; at 15.56, 108 vols. COa (Henry) ; at 15.56, 100 vols. CO2 (Dalton). 100 vols. H 2 O at t C. absorb V vols. of CO2 gas reduced to 60 F. and 30 in. pressure. 4.4 10 15.6 21.1 175.72 147 . 94 122.27 100.50 83.86 26.7 32.2 37.8 65.6 100 68.60 57.50 50.39 11.40 trace (Rogers, Am. J. Sci. (2) 6. 107.) 1 vol. H2 in organic solvents at low temperatures. Continued Solubility of Co2 in organic solvents at low temperatures. Continued t= 59;sp. gr. =0.856 t= 59; sp. gr. =0.994 Pressure Coefficient of absorption Solubility Pressure Coefficient of absorption Solubility 100 200 400 700 40.85 41.00 42.35 44.15 27.27 27.16- 27.65 28.10 100 200 - 400 700 85.3 86.3 91.6 101.5 65.6 65.3 66.7 69.7 Solvent. Methyl alcohol. Solvent. Methyl acetate. t= 78: So. er. =0.884 Pressure Coefficient of absorption Solubility t = 78; sp. gr. =1.056 Pressure Coefficient of absorption Solubility 50 100 200 400 500 740 194.0 195.0 202.9 221.5 226.4 260.0 120.5 119 6 120.1 122.2 126.' 8 50 100 200 400 650 304.9 315.0 337.4 389 3 498.1 224.1 224.3 223.1 225.6 231.2 t = 59;sp.gr.= 0.866 t 59 sp gr 1 ( )32 Pressure Coefficient of absorption Solubility Pressure Coefficient of absorption Solubility 100 200 400 700 63.0 64.2 66.3 69.0 42.5 ' 42.7 43.1 43.3 100 200 400 700 94.3 98.45 103.6 112.9 75.8 77.1 77.6 79.0 Solvent. Acetone. (Stern, Z. phys. Ch. 1912 Solubility of CO 2 in ether 10 =6.044; at 15 = 5.46. (Ch Ch. 1912. 79. 459.) Coefficient of absorption ii 0.20376 at 36.57 mm., and 4.4< pressure. (Woukoloff, C. R. 100 vols. of following liquids absor Ether 5, 81. 468.) at = 7.33; at iristoff, Z. phys. i chloroform is J757 at 762 mm. L09. 62.) ) vols. CO 2 at 18 Sp. gr. Vols. CO 2 0.727 217 0.784 169 0.860 166 0.880 191 0.890 188 0.940 156 0.915 151 1 . 092 75 1.104 72 t = 78; sp.gr. =0.900 Pressure Coefficient of absorption Solubility 50 100 200 400 640 700 311 322 344.5 400 487 545.5 196.6 198.1 201.5 208.8 215.7 t= 59; sp.gr. =0.879 Rectified napht Oil of turpentii Oil of lavender Oil of thyme ie . . . . . . (freshly distilled) . Pressure Coefficient of absorption Solubility Olive oil . . Gum-arabic +1 of the gum) Cane -sugar -f- A 100 200 460 700 .97.8 101.2 106.6 118.8 67.2 68.0 72.8 72.8 Iq (containing 25% q (containing 25% (de Saussure, I. c.) 1 vol. oil of turpentine absorbs 1.7-1.9 vols. COi 1 vol. spirit at 10 absorbs 2 vols. COz. (de Saussure.) 1 vol. olive oil at 10 absorbs 1 +vol. CO. (de Saus- 1 vol. oil of turpentine at 10 absorbs 2 vols. COz. "Tvo!. caoutchine absorbs 11 vols. COz. (Bergman.) Coefficient of absorption for petroleum is 1 17 at 20 and 1.31 at 10. (Gniewasz and Walfisz, Zeit. phys. Ch. 1. 70.) 100 vols. petroleum absorb 70 vols. CO 2 at 10. (Robinet, C. R. 58. 608.) Solvent. Ethyl acetate. t= 78; sp. gr. =1.017 Pressure Coefficient of absorption Solubility 50 100 200 400 650 250.2 255.6 271.8 310.9 386.9 177.5 177.1 179.2 183.2 191.2 170 CARBON OXIDE N Solubility of CO 2 in solutions of various organic substances at 20. Absorption of C0 2 by propyl alcohol. Amount of alcohol used = 0.103 ccm. V and Vi. See under absorption of CO 2 by ethyl alcohol. Substance Sp. gr. of solution ~ _ , cc. CO 2 Coeff. of dissolved absorp- m JQQO tion g . H 2 Pressure kg/sq.cm. t Gas volume ccm. v Vi 20 30 40 50 20 60.59 4.867 8.472 13.46 21.62 56.16 86.62 122.1 174.6 Dextrose Mannite Glycerine Pyrogallol Hydrochinon Resorcin Pyrocatechin Urethane Carbamide Thio carbamide Antipyrine Acetamide Acetic acid N . Propylic acid 1.0328 1.03031 1.01413 1.01718 1.00946 1.00958 1.0107 1.0037 1.00715 1.00917 1.01339 1.005 1.0026 0.9939 0.792 841 0.782 833 0.843 864 0.853 894 887 928 0.901 945 0.868 908 0.869 907 0.864 884 0.859 885 0.859 935 0.879 906 0.868 893 0.869 902 20 30 40 50 60 70 80 35 62.96 3.493 6.307 9.296 13.99 18.90 35.03 49.23 40.00 64.08 98.16 122.8 159.9 228.2 269.6 20 30 40 50 60 70 80 90 100 60 68.08 2.602 4.722 6.723 9.810 13.05 17.15 19.61 24.75 30 19 24.73 47.68 64.65 88.54 111.5 144.4 159.2 184.3 213 9 (Usher, Chem. Soc. 1910, 97. 73.) Absorption of CO 2 by ethyl alcohol. Amount of alcohol used =0.093 ccm. V = ccm. of CO 2 absorbed by the solvent at t, reduced to a pressure of 1 kg. per sq. cm. Vi = ccm. of CO 2 absorbed by 1 ccm. of the solvent. 40 50 60 70 80 90 100 110 120 100 76.27 2 592 5.669 8.025 10.44 13.13 15.72 17.10 20.95 23.55 26 50 54.19 74.51 92.17 107.7 132.3 144.7 163.5 175.4 Pressure kg/sq.cm. t Gas volume 1 ccm. V Vi 30 40 50 ' 20 57.31 9.462 15.15 23.04 104.8 149.7 188.8 30 40 50 60 70 35 60.05 7.114 10.52 14.73 19.63 27.39 77.87 113.1 144.5 173.0 210.8 (Sander.) Absorption of CO 2 by ether. Amount of ether used = 0.131 ccm. V and Vi. See under absorption of CO 2 by alcohol. 40 50 60 70 80 90 100 60 64.44 6.429 9.023 12.27 15.64 19.11 20.64 23.88 72.82 97.09 122.5 145.2 167.9 180.7 195.7 Pressure kg/sq.cm. t Gas volume ccm. v Vt 45 50 60 35 62.06 42.62 46.81 57.83 205.6 217.3 241.6 50 60 70 80 90 100 60 67.11 28.49 35.24 42.01 46.64 50.72 56.63 171.6 195.4 210.0 221 A 235.0 248.7 50 60 70 80 90 100 110 120 130 140 100 72.19 3.809 6.034 8.374 10.76 13.06 14.90 16.22 18.93 20.48 20.61 42 .49 66.05 88.67 111.2 129.0 145.7 155.0 174.6 182.6 186.0 60 70 80 90 100 100 71.03 12.57 20.00 26.34 32.16 35.70 101.0 134.6 142.8 166.4 175.4 (Sander, Z. phys. Ch. 1912, 78. 524.) (Sander.) CARBON OXIDE 171 Absorption of CO2 by benzene. Amount of benzene used = 0.080 ccm. V and Vi. See under absorption of CO 2 by ethyl alcohol. Absorption of CO 2 by chlorbenzene. Cont. Pressure kg/sq.cm. t Gas volume ccm. V Vi 50 60 70 80 90 110 11.16 13.74 16.65 19.50 22.23 31.64 99.06 118.1 134.5 149.3 165.5 204.4 Pressure kg/sq.cm. t Gas volume ccm. v Vi 15 20 30 40 50 20 55.14 2.728 4.845 9.618 18.70 30.10 46.89 71 16 125.3 192.4 264.3 30 40 50 60 70 80 90 100 110 120 130 100 77.73 3.562 5.008 7.106 8.701 10.37 12.05 13.88 14.89 16.35 17.77 18.54 33.65 48.16 63.78 77.24 91.02 103.00 121.2 121.5 130.7 140.7 146.8 15 20 30 40 50 60 70 35 58.17 2.225 3.373 6.879 11.56 17.09 25.73 35.80 39.94 48.65 94.39 138.3 186.6 243.1 269.0 20 30 40 50 60 70 80 90 100 60 61.86 2.140 3.880 6.699 10.28 13.57 17.71 22.50 28.09 33.76 34.57 55.97 88.71 128.5 156.6 1*84.6 215.0 246.6 284.4 (Sander.) Absorption of CO 2 by brombenzene. Amount of brombenzene used = 0.1 13 ccm. V and Vi. See under absorption of CO 2 by ethyl alcohol. Pressure kg/sq.cm- t Gas volume ccm. V V, 20 30 40 50 20 60.84 4.531 7.793 12.22 17.37 50.83 82.29 121.1 160.0 40 50 60 70 80 90 100 110 120 100 73.75 2.822 3.981 6.440 8.398 11.96 14.57 17.79 20.60 23.98 46.52 58.46 91.27 119.0 155.8 182.5 212.9 237.7 258.2 20 30 40 50 60 70 80 35 63.96 3.947 5.782 8.508 11.96 16.00 22.56 41.26 43.38 62.69 90.43 116.4 146.0 184.1 233.9 (Sander.) Absorption of CO2 by chlorbenzene. Amount of chlorbenzene used = 0.106 ccm. V and Vi. See under absorption of CO 2 by ethyl alcohol. 20 30 40 50 60 70 80 90 100 110 60 69.16 2.650 3.714 5.971 7.406 9.718 10.27 13.99 16.76 20.06 23.13 30.58 46.15 62.64 77.19 98.73 108.4 131.4 144.3 169.7 190.6 Pressure kg/sq.cm. t Gas volume ccm. v Vi 20 30 40 50 20 61.03 5.813 10.25 17.17 26.59 62.61 95.22 137.3 187.5 30 40 50 60 70 . 80 90 100 110 120 100 77.48 2.970 4.032 5.833 7 239 8.330 9.714 11.14 12.79 13.80 15.50 30.56 41.49 59.64 72.64 82.56 92.86 107.1 118.0 125.3 140.7 20 30 40 50 60 70 35 64.16 4.650 7.705 11.81 16.83 22.82 32.83 46.66 72.73 101.5 137.3 168.3 205.5 20 30 40 60 69.38 3.685 5.510 7.982 35.86 53.94 73.69 (Sander.) 172 CARBON OXIDE Absorption of CO 2 by nitrobenzene. Amount of nitrobenzene used =0.164 com. V and Vi. See under absorption of CO 2 by ethyl alcohol. Absorption of CO 2 by toluene. 'Continued Pressure kg/sq.cm. t Gas volume ccm. ' V Vi 30 40 50 60 70 80 90 100 110 120 130 100 76.37 3.356 5.945 8.703 11.18 13.72 16.30 18-. 88 21.85 24.86 26.80 28.21 28.68 49.25 67.93 85.98 101.7 117.6 132.6 149.0 161.9 171.8 178.7 Pressure kg/sq.cm. t Gas volume ccm. v Vi 15 20 30 40 50 20 57.65 5.459 7.354 12.14 15.93 21.71 41.60 57.12 92.50 115.9 155.9 20 30 40 50 60 70 80 35 59.86 5.644 8.658 11.98 15.59 19.94 25.57 34.95 44.48 68.23 94.39 113.4 145.1 179.6 227.0 (Sander Absorption of CO 2 bj Amount of ethyl acetat V and Vi. See under by ethyl alcohol. ) ' ethyl ace e used ~ tate. .155 ccm. n of CO 2 20 30 40 50 60 70 80 60 64.73 3.787 4.519 6.308 7.750 8.887 10.15 10.80 31.38 38.23 52.26 64.21 72.15 82.40 85.03 absorptio Pressure kg/sq.cm. t Gas volume ccm. V Vi 25* 30* 40 20 60.30 29.43 37.91 51.26 158.6 188.2 227.9 20 30 40 50 60 70 80 100 75.52 2.749 4.162 5.393 6.832 7.763 9.048 10.65 24.67 41.00 50.36 63.80 70.85 75.75 86.86 30 40 50 60 35 63.40 26.54 38.69 48.35 51.88 145.2 188.4 213.9 219.8 30 40 50 60 70 , 80 60 68.55 18.12 25.67 33.21 40.12 45.47 49.16 108.0 110.5 165.2 186.7 201.1 223.4 (Sander.) Absorption of CO 2 by toluene. Amount of toluene used =0.114 ccm. V and VL See under absorption of CO 2 by ethyl alcohol. 40 50 60 70 80 90 100 100 76.80 12.76 18.80 24.12 28.99 32.96 36.92 42.75 80.70 110.1 132.0 152.0 162.3 172.1 191.5 Pressure kg/sq.cm' t Gas volume ccm. V Vi 20 30 40 50 20 59.97 7.420 13.31 23.25 45.10 57.91 103.3 155.9 235.8 20 30 40 50 60 70 30 40 50 60 70 80 90 100 35 63.05 6.018 10.13 16.03 23.34 31.39 44.17 49.60 82.63 118.8 155.8 192.1 225.8 (Sander.) Absorption of CO 2 by CH 3 COOH+CC1 4 . Solvent cc. CO 2 absorbed 1 mol. CH 3 COOH 0.8 CH 3 COOH + 0.2 CC1 4 0.5 CH 3 COOH + 0.5 CC1 4 0.2 CH 3 COOH + 0.8 CC1 4 1 CC1 4 58.8 61.0 62.4 60.2 57.6 60 68.17 6.735 9,, 885 13,98 18.00 22.66 26.60 31.66 38.86 54.67 78.67 104.6- 128.1 150.1 171.9 191.5 210.0 (Christoff. J. phys. Ch. 1905, 53. 382.) CARBON OXIDE 173 Absorption of CO 2 byC 2 H 4 Cl 2 +CS 2 . Solvent cc. CO2 absorbed 1 0.8 0.2 0.5 0.5 0.2 0.8 mol. C 2 H 4 C1 2 " C 2 H 4 C1 2 + " CS 2 " C 2 H 4 C1 2 + 11 CS 2 " C 2 H 4 C1 2 + " CS 2 " CS 2 209.7 173.4 140.0 71.9 19.9 (Christoff.) Solubility of CO 2 in organic solvents -rr = change of solubility for 1 increase in temp. Solvent Sol- ubility at 25 C. Sol- ubility at 20 C. Sol- ubility at 15 C. ds "dt Glycerine 0.0302 Water 0.8256 Carbon bisulphide 0.8699 0^8888 0'9446 0. 00747 lodobenzene 1.301 .371 1.440 0.0139 Aniline 1.324 .434 1.531 0.0207 o-Toluidine 1.381 .473 1.539 0.0158 m-Toluidine 1.436 .581 1.730 0.0244 Eugenol 1.539 .653 1.762 0.0223 Benzotrichloride 1.643 Cumene 1.782 !S79 l!978 6!oi96 Carvene 1.802 .921 2.034 0.0232 Dichlorhydrin 1.810 .917 2.020 0.0210 Amyl alcohol 1.831 .941 2.058 0.0227 Brombenzene 1.842 .964 2.092 0.0250 Isobutyl alcohol 1.849 .964 2.088 . 0239 Benzyl chloride 1.938 2.072 2.180 0.0242 m-Xylene 2.090 2.216 2.346 0.0256 Ethylene bromide 2.157 2.294 2.424 0.0267 Chlorobenzene 2.265 2.420 2.581 0.0316 Carbon tetrachloride 2.294 2.502 2.603 0.0309 Propylene bromide 2.301 2.453 2.586 0.0281 Toluene 2.305 2.426 2.557 0.0256 Benzene 2.425 2.540 2.710 0.0285 Amyl bromide 2.455 2.638 2.803 0.0348 Nitrobenzene 2.456 2.655 2.845 0.0389 Propvl alcohol 2 498 Carvol 2.498 2.690 2.914 0.0416 Ethyl alcohol (97%) 2.706 2.923 3.130 0.0424 Benzaldehyde 2.841 3.057 3.304 0.0463 Amyl chloride 2.910 3.127 3.363 0.0453 Isobutyl chloride 3.105 3.388 3.659 0.0554 Chloroform 3.430 3.681 3.956 0.0526 Butyric acid 3.478 3.767 4.084 0.0606 Ethylene chloride 3 . 525 3.795 4.061 0.0536 Pyridine 3.656 3.862 4.291 0.0635 Methyl alcohol 3.837 4.205 4.606 0.0769 Amyl formate 4.026 4.329 4.646 0.0620 Propioriic acid 4.078 4.417 4.787 0.0709 Amyl acetate 4.119 4.411 1 . 850 0.0731 Glacial acetic acid 4.679 5.129 5.614 0.0935 Isobutyl acetate 4.691 4.968 0.0554 Acetic anhydride 5.206 5.720 6 '.218 0.1012 Acetone 6 295 6.921 0.1252 Methyl acetate 6.494 (Just, Z. phys. Ch. 1901. 37. 354.) Absorption of CO 2 by organic substances-}- Aq at 15. P = % of the organic substance in the sol- vent. 0i 5 = Coefficient of absorption at 15. Si6 = Solubility at 15. Organic substance used P a P15 S 15 Chloral hydrate 0.996 0.992 l!656 1.012 17.7 0.885 0.935 21.8 0.860 0.908 31.6 0.803 0.848 37.0 0.790 G.834 38.3 0.781 0.825 49.8 0.760 0.802 51.1 0.769 0.812 52.6 0.764 i 0.807 57.1 0.765 i 0.808 61.1 0.780 0.824 68.8 0.797 0.842 71.0 0.812 0.857 74.6 0.848 0.895 79.4 0.903 0.953 Glycerine 1.003 1-064 1.013 26.11 0.785 0.829 27.69 0.800 845 43 72 0.639 0.675 46.59 0.620 655 62.14 0.511 0.540 73.36 0.449 0.474 77.75 0.430 0.454 87.74 0.422 0.446 90.75 0.404 0.427 96.64 0.415 0.438 99.26 0.410 0.438 (Hammel, Z. phys. Ch. 1915, 90. 123.) Solubility of carbon dioxide in solutions of aniline at 25. I. Concentration, 0.206 g. aniline in 100 c. c. of solution. P = Pressure. S = Solubility calc. according to formula given in original article. P s p s 748 808 920 0.865 0.855 0.857 1053 1159 1243 0.855 0.862 0.860 II. Concentration, 0.425 g. aniline in 100 c. c. of solution. p s p s 760 816 921 0.909 0.897 0.897 1150 1236 1380 0.897 0.902 0.908 174 CARBON SELENIDE Solubility of carbon dioxide in solutions of aniline at 25. Continued III. Concentration, 0.566 g. aniline in 100 c. c. of solution. p s P s 760 823 941 0.935 0.929 0.925 1082 1223 1341 0.923 0.924 0.930 IV. Concentration, 0.743 g. aniline in 100 c. c. of solution. p 1 s P s 760 895 983 0.953 0.941 0.940 1063 1223 1302 0.94C 0.940 0.942 (Findlay and Creighton, Chem. Soc. 1910, 97. 555.) Solubility of CO 2 in CS 2 increases approx. proportionally with the pressure. The ab- sorption is preater at lower temp, and less at higher temp, than is required by Dalton's law. (Woukoloff, C. R. 1889, 108. 674.) Absorption of C02 by sugar +Aq. Sugar +Aq Grams CO2 absorbed by 75 cc. of solution at 15.5 and 720 mm. Vio-N sugar solution V-N " i-N " " 0.1225 0.1089 0.0931 (Christoff, Z. phys. Ch. 1905, 53. 329.) Absorption of C0 2 in sugar +Aq at 20. Cone, of solution Sp. gr. Coefficient of absorption Vs mol. per 1. !/4 " " " v, 1 a (s (( 1.01518 1.03125 1.06372 1.12809 0.846 0.815 0.756 0.649 (Usher, Chem. Soc. 1910, 97. 72.) Liquid. Not miscible with H 2 O, though slightly sol. therein, or with fatty oils; mis- cible with alcohol, ether, CS 2 , and the essen- tial oils. (Thilorier, Mitchell.) Unacted upon by H 2 O; sol. in alcohol, ethers, petroleum, oil of turpentine, and CS 2 . (Mareska and Donny.) Petroleum dissolves 5 to 6 vols. liquid CO 2 (Cailletet, C. R. 75. 1271.) SI. sol. in CS 2 . (Cailletet.) Solid. When immersed in H 2 O, rapidly volatilizes and dissolves. With alcohol or ether it forms a semi-fluid mixture. (Chan- ning, Am. J. Sci. (2) 5. 186.) Only slightly sol. in anhydrous ether, but may be mixed therewith to a paste. (Thil- orier.) Sol. in methyl chloride below 65 to the point of sat. without decomp. (Villard, C. R. 1895, 120. 1413.) +6H 2 O. (Villard, C. R. 1894, 119. 369.) Carbon selenide, C 4 Se. Sol. only in hot cone. H 2 SO 4 . (v. Bartal, Ch. Z. 1906, 30. 810.) C 6 Se. Insol. in H 2 O, CS 2 , and ether. Easily sol. in hot cone. H 2 SO 4 ; sol. in cone. NaOH+Aq from which it is pptd. by HC1. (v. Bartal.) Carbon silicide CSi. (Carborundum.) Not attacked by any acids, even HF; si. attacked by caustic al- kalies or carbonates. (Acheson, C. N. 68. 179.) Not attacked by KOH+Aq. (Schiitzen- berger, C. R. 114. 1089.) Carbon mowosulphide, CS. Insol. in H 2 O, alcohol, oil of turpentine, or benzene; somewhat sol. in CS 2 or ether; sol. in warm HNOs; sol. in cone. KOH+Aq. (Sidot, C. R. 81. 32.) Readily absorbed by alcohol and aniline. (Deninger, J. pr. 1895, (2) 51. 349.) Carbon ^sulphide, CS 2 . Very si. sol. in H 2 O. 1 1. H 2 O dissolves 2-3 g. CS 2 (Ckiandi, Bull. Soc. 43. 562); 3.5-4.52 g, (Peligot, ib. 43. 563). 30 ccm. CS 2 shaken with 8690 com. H 2 O at 20-23 for 18 days decreased 11 ccm. in 9 days and 1.4 ccm. in the next 3 days by diffused light, and 0.6 ccm: in the last 5 days (no light). Part of the CS 2 was decomp. and 7.85 ccm. were dissolved, therefore H 2 O dissolves Viooo of its weight CS 2 . (Sestini, Gazz. eh. it. 1. | 473.) Solubility of CS 2 ID H 2 O. 100 pts. H 2 O dissolve 0.203 pts. CS 2 at 12-13 0.191 " " 15-16 0.168 " " 25-27 0.145 " " 30-33. (Page, C. N. 41. 195.) Solubility of CS 2 in H 2 O. a = g. ccm. solution at t. CS 2 in 1000 a t a t a t 2.04 1.99 1.94 1.87 5 10 15 1.79 1.69 1.55 1.37 20 25 30 35 1.11 0.70 0.14 40 45 49 (Chancel and Parmentier, C. R. 100. 773.) 100 g. H 2 O dissolve at t: t 10 20 30 0.258 0.239 0.201 0.195 g. CS 2 . (Rex, Z. phys. Ch. 1906, 55. 365.) CARBONATES 175 Absorption of CS 2 vapor by H 2 O at t. t Coefficient of absorption 10 20 30 3.573 2.189 1.346 0.799 Calc. from data of Chancel and Parmentier, C. R. 100. 733.) (Winkler, Z. phys. Ch. 1906, 55. 352.) Vapors of C$2 are most easily absorbed by alcoholic solution of KOH. SI. absorbed by KOH+Aq, and very slowly by CuS0 4 , Pb(C 2 H 3 O0 2 +Aq, cone. H 2 SO 4 , or CaCl 2 in HCl+Aq. (Berthelot, A. ch. (3) 51. 74.) Solubility in alcohol. S = strength of alcohol in per' cent by weight; P = pts. CS 2 which dissolve in 10 ccm. alcohol at 17. s p s p 100 98.5 98.15 96.95 93.54 oo 18.20 13.20 10.00 7.00 91.37 84.12 76.02 48.40 47.90 5.00 3.00 2.00 0.20 0.00 (Tuchschmidt and Follenius, B. 4. 583.) Miscible with absolute alcohol, ether, ethe- real and fatty oils, and liquid CO 2 . Tncarbon bisulphide, C 3 S 2 . Insol. in H 2 O; easily sol. in alcohol, ether, chloroform, benzene, and CS 2 . The alcoholic and ethereal solutions decomp. on standing. (Lengyel, B. 26. 2960.) Sol. in alcohol with decomp. Sol. in CS 2 and in benzene. (Stock, B. 1912, 46. 3575.) Solid modification. Insol. in H 2 O and ordinary solvents. Sol. in KOH+Aq. (Lengyel.) Carbon sulphoselenide, CSSe. Mpt. 85 C , bpt. +84. Decomp. by light. Not attacked by H 2 O. Sol. in hot cone. HNO 3 . Decomp. by Br 2 to an oil. Sol. in alcohol with decomp. Mis- cible with CS 2 . (Stock, B. 1914, 47. 150.) Carbon sulphotelluride, CSTe. Mpt, 54. Very unstable. Miscible with CS 2 and benzene without decomp. (Stock, B. 1914, 47. 142.) Carbonatochloroplatindiamine carbon- ate chloroplatindiamine nitrate. Cl^ 3 [ Pt N 2 H 6 J 2 ( C 3 ) 2 > Cl 2 Pt(N 2 H 6 N0 3 ) 2 . Precipitate. \Cleve, J. B. 1867. 321.) Carbonatonitratoplatind'z'amine carbon- ate, ( Cgs^ [Pt(N 2 H 6 ) 2 ] 2 (C0 3 ) 2 . Sol. in boiling H 2 O. (Cleve.) Carbonatotetramine cobaltic bromide, Co(NH 3 ) 4 CO 3 Br. Much less sol. than chloride. (Jorgensen, Z. anorg. 2. 279.) - carbonate, [Co(NH 3 ) 4 CO 3 ] 2 CO 3 +3H 2 O. Very sol. in H 2 O. (Jorgensen.) - chloraurate, [Co(NH 3 ) 4 CO 3 ] 2 AuCl 4 + Somewhat sol. in H 2 O; nearly absolutely insol. in alcohol. (Jorgensen.) - chloride, Co(NH 3 ) 4 CO 3 Cl. Easily sol. in H 2 O; insol. in alcohol. (Jor- gensen.) - chloroplatinate, [Co(NH 3 ) 4 CO 3 ] 2 PtCl 6 + 2H 2 O. Nearly insol. in H 2 O and alcohol. (Jorgen- sen.) - chloroplatinite, [Co(NH 3 ) 4 CO 3 ] 2 PtCl 4 . Nearly insol. in H 2 O; wholly in alcohol. (Jorgensen.) - dithionate, [Co(NH 3 ) 4 CO 3 ] 2 S 2 O 6 . Ppt. (Jorgensen.) - iodide, Co(NH 3 ) 4 CO 3 I. Much less sol. than bromide or chloride. (Jorgensen.) - nitrate, Co(NH 3 ) 4 CO 3 NO 3 +^H 2 O. Sol. in about 15 pts. cold H 2 O; insol. in alcohol. (Jorgensen.) - sulphate, [Co(NH 3 ) 4 C0 3 ] 2 SO 4 +3H 2 O. Considerably less sol. in H 2 O than the ni- trate. (Jorgensen.) Carbonic acid, H 2 CO 3 See Carbon dioxide. Carbonates. Carbonates of Na, K, Rb, and Cs are easily sol. in H 2 O; carbonates of Li and Tl are much less sol.; other carbonates are nearly or quite insol. All carbonates are sol. to some extent in H 2 O containing CO 2 . All carbonates, ex- cept those of NH 4 , Rb, and Cs, are insol. in alcohol. Sol. in those acids which are themselves sol. in H 2 O, except HCN and H 3 BO 3 . Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 824.) 176 CARBONATE, ALUMINUM, BASIC Aluminum carbonate, basic. 5A1 2 O 3 ,6CO 2 +37H 2 O = 3A1(OH) 3 , A1 2 (CO 3 ) 3 + 14H 2 O. (Seubert, Z. anorg. 1893, 4. 67.) A1 2 O 3 , CO 2 . (Parkmann, Sill. Am. J. (2) 34. 324.) 3A1 2 O 3 , 2CO 2 +16H 2 O. (Muspratt and Danson, A. 72. 120.) 3A1 2 O 3 , 2CO 2 +9H 2 O. (Wallace, Chem. Gaz. 1868. 410.) 5A1 2 O 3 , 3CO 2 + 18H 2 O. (Bley, J. pr. 39. 11.) 2A1 2 O 3 , CO 2 +6H 2 O.=10A1(OH) 3 , A1 2 (CO 3 ) 3 +3H 2 0. Sol. in cold dil. acids. (Schlum- berger, Bull. Soc. 1895, (3) 13. 46.) +8H 2 O. (Urbain and Renoul. J. Pharm. (4)30. 340.) = 10A1(OH) 3 , A1 2 (CO 3 ) 3 +9H 2 O. (Seubert, Z. anorg. 1893. 4. 67.) 8A1 2 O 3 , 3CO 2 +40H 2 O. (Langlois, A. ch. (3) 48. 505.) All are precipitates, insol. in H 2 O, sol. in acids, and give off CO 2 at slight heat. There are no definite carbonates of alum- inum. (Cameron, J. phys. Chem. 1908, 12. 572.) Aluminum ammonium carbonate, A1 2 O 3 , CO 2 , (NH 4 ) 2 CO 3 +4H 2 0. Precipitate. (Rose, Pogg. 91. 460.) Aluminum sodium carbonate, A1 2 O 3 , CO 2 , 2Na 2 CO 3 +24H 2 O. Precipitate. Sol. in cold dil. acids. (Bley, J. pr. 39. 22.) Ammonium carbonate, (NH 4 ) 2 C0 3 +H 2 O. Sol. at 15 in its own weight H 2 O. Solution in H 2 O gives off gas at 70-75, and boils at 75-80. SI. sol. in cold dil. NH 4 OH+Aq, more sol. at ordinary temp. Insol. in cone. NH 4 OH+Aq. (Divers, Chem. Soc. (2) 8. 171, 259, and 364.) . . Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) Insol. in alcohol. Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6.257.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) 100 g. pure glycerine dissolve 20 g. (NH 4 ) 2 CO 3 at 15. (Ossendowski, Pharm. J. 1907, 79. 575.) Ammonium hydrogen carbonate, NH 4 HCO 3 . Sol. at 15 in about 8 pts. H 2 O. (Berthol- let, J. Phys. 66. 168.) Sol. at 12.8 in about 6 pts. H 2 O. (J. Davy, N. Edinb. J. 16. 245.) Solution decomp. on air or by gentle heat or by addition of the solid salt. (Berthollet.) 100 pts. H 2 O dissolve at 0, 11.9 pts.; at 10, 15.85 pts.; at 20, 21 pts.; at 30, 27 pts. NH 4 HCO 3 . (Dibbits, J. pr. (2) 10. 417.) Solubility of NH 4 HCO 3 in NH 4 Cl+Aq, sat with CO 2 , at t. t g. per 10 g. H 2 Sp. gr. of sat. NH 4 C1 NH4HCO 3 solution 29.08 11.9- 3.6 T077 15 2.99 6.06 8.51 11.68 18.30 26.93 33.25 34.35 18.64 16.29 14.22 12.69 11.68 9.33 7.73 6.64 6.42 1.064 .063 .062 .062 .065 .069 .076 .085 .085 30 39.7 27.0 9.1 (Fedotieff, Z. phys. Ch. 1904, 49. 168.) Solubility of NH 4 HCO 3 in NaHCO 3 +Aq, sat. with CO 2 at t. t g. per 100 g. H 2 O Sp. gr. of sat. solution XaHCOs NH.HCOs 15 4.82 11.90 10.94 1.072 5.92 18.64 17.06 1.064 1.090 30 7.0 27.0 23.0 (Fedotieff, Z. phys. Ch. 1904, 49. 168.) Solubility of NH 4 HCO 3 in NH 4 NO 3 -f Aq at t. t g. per 100 g. H 2 O Sp. gr. of sat. solution NH 4 NO 3 NH 4 HCO 118 11.90 4.52 1^2625 15 23.26 49.82 103.4 128.9 166.9 18.64 12.91 10.33 8.25 7.79 7.49 1.064 1.113 1.164 1.242 1 . 269 1.302 30 231.9 26.96 12.57 (Fedotieff and Koltunoff, Z. anorg. 1914, 85. 251.) Insol. in alcohol. (J. Davy.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) CARBONATE, AMMONIUM DYSPROSIUM 177 Ammonium dihydrogen carbonate, (NH 4 ) 4 H 2 (C0 3 ) 3 +H 2 0. Sp. gr. of carbonate of ammonia +Aq at 12. Continued Sol. in 5 pts. H 2 O at 15; decomp. by more H 2 O or by heat. (Divers, Chem. Soc. (2) 8. 171, 359, and 364.) Deg. Tw. Spjr. at % Carb. arnmon. Change of sp. gr. 1 O /"I SI. sol. in alcohol. for 1 C. 18 1.090 26.82 0.0007 Ammonium hydrogen carbonate carbamate, 19 1.095 28.33 0.0007 2NH 4 HC0 3 , NH 4 CONH 2 . (Salts of harts- 20 1.100 29.93 0.0007 horn.) 21 1.105 31.77 0.0007 1 pt. salt dissolves at: 22 1.110 33.45 0.0007 13 in 4 pts. H 2 O. 23 1.115 35.08 0.0007 16.7 "3.3 24 1.120 36.88 0.0007 32.2 " 2.7 " 25 1.125 38.71 0007 40.6 "2.4 " 26 ' 1 . 130 40.34 0.0007 49 " 2 " 27 . 1.135 42.20 0.0007 (J. Davy, N. Edinb. J. 16. 245.) 28 29 1.140 1.144 44.29 44.90 0.0007 0.0007 Strong alcohol dissolves out carbamate, and the carbonate remains undissolved. NH 4 HC0 3 , NH 4 C0 2 NH 2 . (Commercial carbonate of ammonia.) Sol. at 15 in 4 pts. H 2 O, at 65 in \Y 2 pts. H 2 0. (Divers.) 30 pts. salt +100 pts. H 2 O lower temp, from 15.3 to 3.2. (Rudorif, B. 2. 68.) So!, in 1.667 pts. cold, and 0.833 pt. hot H 2 O. (Four- croy.) 100 pts. H 2 O at 13 dissolve 25 pts. 17 " 30 " 37 " 37 " 41 " 40 " 49 50 " (Berzelius.) 100 pts. H 2 O at 15.5 dissolve 33 pts.; at 100, 100 pts. (lire's Diet.) 89!. in 2 pts. H 2 O at 15.5, and in less than 1 pt. boiling H 2 O; sat. solution at 15.5 contains 33.3%, and sat. boiling solution 50%. (Abl.) Sat. aqueous solution at 10 contains 15.7%. (Eller.) Sat. aqueous solution at (?) contains 6.1%. (Mus- sembroek.) Sat. solution in the cold contains 37.5%. (Fourcroy.) Does not dissolve as such in H 2 O; (NH^izCOs dis- solves out first, and NH4HCO3 later. (Scanlan.) Sp. gr. of carbonate of ammonia+Aq at 12. Deg. Tw. Sp. gr. at 12. % Carb. .minion. Change of sp. gr. for 1 C. 1 1.005 1.66 0.0002 2 1.010 3.18 0.0002 3 1.015 4.66 0.0003 4 1.020 6.04 0.0003 5 1.025 7.49 0.0003 6 . 1.030 8.93 0.0004 7 1.035 10.35 0.0004 8 1.040 11.86 0.0004 9 1.045 13.36 0.0005 10 .050 14.83 0.0005 11 .055 16.16 0.0005 12 .060 17.70 0.0005 13 .065 19.18 0.0005 14 .070 20.70 0.0005 15 .075 22.25 0.0006 16 .080 23.78 0.0006 17 1.085 25.31 0.0006 (Lunge, Chem. Ind. 1883. 2.) Sp. gr. of aqueous solution of salt with com- position 31.3% NH 3 , 56.6% CO 2 , 12.1% H 2 O. 100 pts. of solution contain 6.58 9.96 14.75 19.83 25.71 pts. salt 1.0219 1.0337 1.0497 1.0672 1.0863 sp. gr. 29.74 35.85 40.23 44.90 pts. salt. 1.0995 1.1174 1.1297 1.1414 sp. gr. (J. H. Smith, Chem. Ind. 1883. 3.) Cone, alcohol dissolves out carbamate and leaves carbonate. (Hiinefeld, J. pr. 7. 25.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) Ammonium cerous carbonate, (NH 4 ) 2 CO 3 , Ce 2 (CO 3 ) 3 +6H 2 O. Ppt. Very si. sol. in cone. (NH 4 ) 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 104.) Ammonium chromous carbonate, (NH 4 ) 2 CO 3t CrCO 3 +H 2 O. Decomp. by moist air; sol. in dil. HC1 and H 2 SO 4 . (Bauge", C. R. 1896, 122. 476.) Ammonium cobaltous carbonate, (NH 4 ) 2 CO 3 , CoCO 3 +4H 2 O. Permanent. Sol. in H 2 O. (Deville, A. ch. (3) 36. 460.) (NH 4 ) 2 O, 2CoO, 4C0 2 +9H 2 O. Quickly de- comp. on air: sol. in H 2 O. (Deville.) +12H 2 O. Sol. in H 2 O. Ammonium didymium carbonate, (NH 4 ) 2 CO S , Di 2 (C0 3 ) 3 +3H 2 0. Insol. in H 2 O. (Cleve.) Ammonium dysprosium carbonate, NH 4 Dy(C0 3 ) 3 +H 2 0. Only si. sol. in H 2 O. (Jantsch, B. 1911, 44. 1277.) 178 CARBONATE, AMMONIUM GLUCINUM Ammonium glucinum carbonate, 2(NH 4 ) 2 CO 3 , 3G1CO 3 (?). Very sol. in cold, decomp. by hot H 2 O. Nearly insol. in alcohol. (Debray.) Composition is (NH 4 ) 2 CO 3 , 2G1CO 3 , G1(OH) 2 +2H 2 O. (Humpidge, Royal Soc. Proc. 39. 1.) Ammonium lanthanum carbonate, La 2 (CO 3 ) 3 , (NH 4 ) 2 C0 3 +4H 2 0. Ppt. (Meyer, Z. anorg. 1904, 41. 102.) Ammonium magnesium carbonate, (NH 4 ) 2 Mg(C0 3 ) 2 +4H 2 0. Sol. in 71 pts. H 2 O with decomp.; more sol. in NH 4 Cl-f Aq. (Divers, Chem. Soc. 51. 196.) H 2 O containing (NH 4 ) 2 CO 3 dissolves very slightly; more sol. in H 2 O containing NH 4 C1. (Favre, A. ch. (3) 10. 473.) Ammonium magnesium hydrogen carbonate, (NH 4 ) 2 Mg 2 H 2 (CO 3 ) 4 +8H 2 O, or 12H 2 O. Decomp. on air. (Deville, A. ch. (3) 35. 454.) Ammonium neodymium carbonate, (NH 4 ) 2 CO 3 , Nd 2 (C0 3 ) 3 +4H 2 O. Ppt. SI. sol. in cone. (NH 4 ) 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 106.) Ammonium nickel carbonate, NH 4 HCO 3 , NiCO 3 -t-4H 2 O. Insol. in H 2 O. (Deville, A. ch.'(3) 35. 452.) Ammonium praseodymium carbonate, (NH 4 ) 2 C0 3 , Pr 2 (C0 3 ) 3 +4H 2 0. Ppt. Insol. in (NH 4 ) 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 105.) Ammonium samarium carbonate, (NH 4 ) 2 C0 3 , Sm 2 (CO 3 ) 3 +4H 2 O. Ppt. Ammonium scandium carbonate, (NH 4 ) 2 CO 3 , . 2Sc 2 (C0 3 ) 3 +6H 2 0. Difficultly sol. in H 2 O. Sol. in cold alkali- carbonate 4-Aq, less sol. in hot. (R. Meyer, Z. anorg. 1910, 67. 410.) Ammonium tin (stannous) carbonate, (NH 4 ) 2 CO 3 , 2SnCO 3 +3H 2 O. Decomp. by cold H 2 O. (Deville, A. ch. (3) Ammonium uranyl carbonate, 2(NH 4 ) 2 CO 3 , U0 2 CO 3 . Sol. at 15 in 20 pts. H 2 O, more abundantly in H 2 O containing (NH 4 ) 2 CO 3 . (Ebelmen.) Insol. in pure H 2 O; sol. in H 2 O containing (NH 4 ) 2 CO 3 . Solution is decomp. by boiling. (Berzelius.) Sol. in SO 2 +Aq. (Berthier, A. ch. (3) 7. 76.) 3(NH 4 ) 2 CO 3 , 2(UO 2 )CO 3 +4H 2 O. Sol. in H 2 O. (Giolitti C. C. 1905, II. 227.) Ammonium vanadyl carbonate, 3(NH 4 ) 2 O, 7VO 2 , 5CO 2 +16H 2 O. SI. sol. in H 2 O. Sol. in acids and alkalies. (Koppel, Z. anorg. 1905, 45. 350.) Ammonium yttrium carbonate, (NH 4 ) 2 GO 3 , Y 2 (C0 3 ) 3 +2H 2 0. Insol. in (NH 4 ) 2 CO 3 +Aq. (Mosander.) Ammonium zinc carbonate, basic, 3ZnO, NH 4 OH, 2CO 2 +H 2 O. Insol. in H 2 O. (Kassner, Arch. Pharm. (3) 27. 673.) Ammonium zinc carbonate, (NH 4 ) 2 CO 3 , ZnCO 3 . Insol. in H 2 O. (Deville.) Quite sol. in H 2 O; more sol. than (NH 4 ) 2 CO 3 , MgCO 3 . Tolerably permanent in the air. Slowly decomp. by cold, rapidly by hot H 2 O. Very sol. in (NH 4 ) 2 CO 3 +Aq. Not attacked by alcohol. (Favre, A. ch. (3) 10. 481.) Barium carbonate, BaCO 3 . Sol. in 4304 pts. cold, and 2304 pts. boiling H 2 O. (Fourcroy.) Sol. in 47,620 pts. H 2 O. (Bineau, A. ch. (3) 51. 290.) Sol. in 14,137 pts. H 2 O at 16-20, and 15,421 pts. at 100. (Fresenius.) Sol. in 12,027 pts. H 2 O at 15. (Kremers, Pogg. 85. 247.) Calculated from electrical conductivity of solution, 1 pt. BaCOs is sol. in 64,070 pts. H 2 O at 8.8 and 45,566 pts. at 24.2. (Hollemann, Z. phys. Ch. 12. 125.) Solubility in H 2 O at t. 14 18 23 27 32 38 g. sol. in 100 g. H 2 O 4.32 x 10- 4 4.57 x 10- 4 4.89 x 10- 4 5.22 x 10- 4 5.69 x 1C- 4 6.27 x 10- 4 (Weissenberger, Z. phys. Ch. 1914, 88. 266.) "Solubility product" =8.1 x 10-' mol. 1. (McCoy and Smith, J. Am. Chem. Soc. 1911, 33. 473.) Sol. in H 2 CO 3 +Aq. (See barium hydrogen carbonate.} Easily sol. in dil. acids. Not acted upon by cone. HNO 3 +Aq. Not decomp. by 1 pt. H 2 SO 4 +6 pts. ab- solute alcohol. Slowly decomp. by 1 pt. CARBONATE, BARIUM URANYL 179 HNO 3 +6 pts. absolute alcohol. Slowly de- comp. by 1 pt. H 2 G2O 4 +6 pts. absolute al- cohol. Not decomp. by absolute alcoholic solu- tions of racemic, tartaric, citric, or glacial acetic acids. (Babington and Phillips, 1816.) Almost completely insol. in H 2 O containing NH 4 OH and (NH 4 ) 2 CO 3 , when digested in such a solution and allowed to stand. 1 pt. BaCO 3 dissolves in 141,000 pts. of such a solu- tion. (Fresenius.) Not more sol. in NaCl+Aq than in H 2 O. (Karsten.) Sol. in cold NH 4 C1, NH 4 NO 3 , or NH 4 suc- cinate+Aq. (Vogel, J. pr. 7. 453.) 2 mols. NH 4 C1 dissolved in H 2 O dissolve 1 mol. BaCO 3 by continued boiling. (Smith, Phil. Mag. J. 9. 540.) Solubility in H 2 O increases by addition of NH 4 C1, at first strongly, then less strongly and finally strongly again. (D'Agustino and Pellegrino, Gazz. ch. it. 1908, 38 (1) 532.) Somewhat sol. in K 2 CO 3 +Aq. (Wacken- roder, A. 24. 30.) Solubility of BaCO 3 in KCl+Aq at bpt. of solution g. KC1 per 100 g. solution g. BaCOs per 1000 cc. sat. solution 0.15 0.0847 1 0.1781 3 0.2667 10 0.4274 30 0.5550 (Cantoni and Goguelia, Bull. Soc. 1905, (3) 33. 13.) Solubility of BaCO 3 in NaCl+Aq at bpt. of solution g. NaCl per 100 g. solution g. BaCOs per 1000 cc solution sat. 0.15 0.0587 1 0.0787 3 0.1056 10 0.1575 30 0.2784 (Cantoni and Goguelia, 1. c.) Solubility of BaCO 3 in 10% KCl+Aq at t. t g. BaCOs per 1000 cc. sat. solution 10 20 40 60 80 0.2175 0.2408 0.2972 0.3491 0.4049 (Cantoni and Goguelia, 1. c.) Solubility of BaCO 3 in 10% NaCl+Aq at t c t g. BaCOa per 1000 cc. sat. solution 10 20 40 60 80 0.1085 0.1126 0.1231 0.1303 0.1418 (Cantoni and Goguelia, 1. c.) Slowly sol. in cone. Na 2 SO 4 , MgSO 4 , ZnSO 4 , Ca(NO 3 ) 2 , or CaCl 2 +Aq, but insol. in ZnCl 2 -f-Aq. (Karsten.) SI. decomp. by boiling K 2 SO 4 +Aq. SI. decomp. in the cold by 1 pt. K 2 SO 4 +2 pts. Na 2 SO 4 +Aq. 'Decomp. by salts of Al, Mn, Cr, Fe, U, Bi, Cd, Cu, Hg, Pb, Sn", Sn iv , Hg 2 , Rh, Ir, Au, with pptn. of oxide of metal. (Rose, Tr.) Pptn. of BaCO 3 is hindered by. presence of alkali citrates or metaphosphates. Sol. in solutions of various salts, as in the case of calcium carbonate (see Calcium car- bonate) . The solvent power of these solutions for barium carbonate is somewhat less than for calcium carbonate. Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. B. 1909, 42. 3790) ; ethyl acetate. (Naumann, B. 1904, 37. 3602.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Min. Witherite. Barium hydrogen carbonate, BaH 2 (CO 3 ) 2 (?). 100 pts. H 2 O containing CO 2 dissolve 0.079 pt. BaCO 3 . (Bineau.) 100 pts. H 2 O containing CO 2 dissolve 0.17 pt. BaCO 3 . (Lassaigne.) 100 pts. H 2 O sat. with CO 2 under a pressure of 4-6 atmospheres dissolve 0.725 pt. BaCO 3 . Upon evaporating, BaCO 3 is deposited. (Wagner, Z. anal. 6. 167.) BaCO 3 is sol. in 833 pts. H 2 O sat. with CO 2 at 10. (Lassaigne.) BaCO 3 is sol. in 830 pts. H 2 O sat. with CO 2 at 10. (Fourcroy.) BaCO 3 is sol. in 1550 pts. H 2 O sat. with CO 2 at 10. (Bergman.) 100 cc. H 2 O sat. with CO 2 dissolve 0.73 g. BaH 2 (CO 3 ) 2 . (McCoy and Smith, J. Am. Chem. Soc. 1911, 33. 473.) Barium calcium carbonate, BaCO 3 , CaCO 3 . Min. Barytocalcite, Bromlite. Sol. in dil. acids. Barium uranyl carbonate, BaO, 2UO 3 , 2CO 2 +5H-.O. Decomp. by H 2 O. (Blinkoff. Dissert. 1900.) +8H 2 O. Decomp. by H 2 O. (Blinkoff.) 180 CARBONATE BISMUTH, BASIC Bismuth carbonate, basic, (BiO) 2 CO 3 + Insol. in H 2 O; sol. in acids. Insol. in CO 2 + Aq. (Bergman.) Completely sol. in (NH 4 ) 2 CO 3 +Aq; si. sol. in K 2 CO 3 +Aq.; insol. in Na 2 CO 3 +Aq. (Lau- gier.) Absolutely insol. in (NH 4 ) 2 CO 3 +Aq unless H 3 PO 4 or H 3 AsO 4 are present. (Berzelius.) Insol. in (NH 4 ) 2 CO 3 , K 2 CO 3 , or Na 2 CO 3 + Aq. (Rose.) Sol. in NH 4 Cl+Aq. (Wackenroder.) In- sol. in NH 4 NO 3 +Aq. (Brett.) Sol. in CaCl 2 +Aq. (Pearson.) Min. Bismuthosphaerite. 3Bi 2 O 3 , CO 2 . Min. Bismuthite. Easily sol. in acids. 4Bi 2 O 3 , 3CO 2 +4^H 2 O. Min. Bismuth spar. Easily sol. in acids. Bismuth potassium carbonate, Bi 2 OK 4 (CO 3 ) 4 +H 2 0.. Decomp. by large quantities of H 2 O. (Rey- nolds, Chem. Soc. 1898, 73. 266.) Cadmium carbonate, CdC0 3 . Insol. in H 2 O; easily sol. in acids; insol. in K 2 CO 3 , and Na 2 C0 3 +Aq; very si. sol. in (NH 4 ) 2 CO 3 +Aq. (Fresenius.) Easily sol. in NH 4 sulphate, nitrate, and succinate+Aq. (Wittstein.) Sol. in KCN+Aq; sol. in cold NH 4 Cl+Aq; less sol. in NH 4 NO 3 +Aq. (Brett, 1837.) Not prevented from pptn. by non- volatile organic substances. (Rose.) Not pptd. from solutions containing sodium citrate. (Spiller.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898,20.827.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790) ; 'ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) + 3^H 2 O. (Lefort, J. B. 1847. 346.) (Kraut, Z. anorg. 1897, 13. 14.) Cadmium carbonate hydrazine, CdCO 3 , 2N 2 H 4 . Easily sol. in cold NH 4 OH + Aq. (Franzen, Z. anorg. 1908, 60. 281.) Caesium carbonate, Cs 2 CO 3 . Very deliquescent, and sol. in H 2 O. 100 pts. absolute alcohol dissolve 11.1 pts. Cs 2 CO 3 at 19; 20.1 pts. Cs 2 CO 3 at boiling temp. (Bunsen.) Caesium hydrogen carbonate, CsHCO 3 . Not deliquescent. Sol. in H 2 O. Calcium carbonate basic, CaO, CaCO 3 +H 2 O. Hardened by H 2 O, but not dissolved. (Raoult, C. R. 92. 189.) Calcium carbonate, CaCO 3 . More sol. in cold than in hot H2O. (Gmeliii.) When recently pptd., sol. in 8834 pts. boiling, and 10,601 pts. cold EhO; much less sol. in H2O containing NH4OH and (NH^COs, 65,246 pts. of which dissolve 1 pt. CaCOs. (Fresenius (1846), A. 59. 122.) Sol. in 16,000 pts. pure H 2 O. (Brandes, 1825.) Sol. in 12,858 pts. pure H 2 O at 15. (Kremers, Pogg. Sol. in 16,000-24,000 pts. pure H 2 O. (Bucholz.) 1 1. H 2 O dissolves 34 mg. CaCO 3 . (Cheva- let, Z. anal. 8. 91; Hoffmann, Z. anal. 4. 414.) 1 1. H 2 O may contain 0.016 g. CaCO 3 . i. e., 1 pt. is sol. in 62.500 pts. H 2 O. (Bineau, A. ch. (3) 51. 290.) 1 1. H 2 O dissolves 0.02 g. CaC0 3 , i. e., 1 pt. CaCO 3 is sol. in 50.000 pts. H 2 O. (Peligot.) Solubility is much affected by CO 2 of the air. 1 1. H 2 O at 16 dissolves 13.1 mg. CaCO 3 . (Schlcsing, C. R. 74. 1552.) Calculated from electrical conductivity of CaCO 3 +Aq, 1 pt. CaCO 3 is sol. in 99,500 pts. H 2 O at 8.7, and 80,040 pts. at 23.8. (Holle- mann, Z. phys. Ch. 12. 125.) By continued boiling CaH 2 (CO 3 ) 2 , 36 mg. CaCO 3 remain in solution. (Weltzien, A. 136. 165.) Solubility in H 2 O at different pressures. Pressure in atmos. Solubility 1079 1403 1820 2109 (Engel, C. R. 101. 949.) 100 pts. H 2 O dissolve C.0005 pt. (calculated as CaO) from pptd. CaCO 3 , and 0.0027 pt. from calcspar. (Lubavin, J. russ. Soc. 24. 389.) 1 1. H 2 O dissolves 13 mg. CaCO 3 at 18. (Kohlrausch, Z. phys. Ch. 1893, 12. 241.) 1 1. CO 2 free water dissolves 17.4 mg. CaO or 31.0 mg. CaCO 3 . (Gothe, Ch. Z. 1915, 39. 305.) CaCO 3 dissolves in 9662 pts. H 2 O at 12. (Pollacci, C. C. 1896, II. 946.) 1 1. H 2 O free from CO 2 dissolves 9.6 mg. CaCO 3 . (McCoy and Smith, J. Am. Chem. Soc. 1911, 33. 473.) Found dissolved in 10,000 pts. sea water. (Davy.) Pptd. amorphous CaCO 3 dissolves in 1600 pts. sea water. Pptd. crystalline CaCO 3 dis- solves in 8000 pts. sea water. (Irvine and Young, Chem. Soc. 66. 344.) Artificial sea water sat. with CO 2 dissolves CaCO 3 corresponding to 57.27 mg. of com- bined CO 2 per litre at 15. Sea water which contains 52-55 mg. neutral combined CO 2 per litre must be sat. with CaCO 3 . (Cohen, Chem. Soc. 1900, 78 (2) 725.) For action of H 2 CO 3 +Aq, see Calcium hydrogen carbonate. CARBONATE, CALCIUM 181 Sol. in H 2 SO 4 , eyen when native. Sol. in acids generally. When treated with acids in closed vessels effervescence ceases on increase of pressure, but is renewed at once on remov- ing it. (Link, 1814.) Unacted upon by cone. HNO 3 , even when boiling, as Ca(N0 3 )2 is insol. in cone. HNO 3 . Not decomp. by mixture of 1 pt. H 2 SO<, and 6 pts. absolute alcohol, but immediately by HNO 3+ absolute alcohol. Not decomp. by absolute alcoholic solutions of oxalic, racemic, tartaric, citric, or glacial acetic acids. (Babington and Phillips, 1816.) Unacted upon by glacial HC2H 3 O 2 , even when boiling. Freshly pptd. CaCO 3 is sol. in cold NH 4 C1+ Aq ; but the solution becomes 'cloudy on ex- posure to air, a portion, however, of CaC0 3 remains dissolved, which cannot be pptd. even by boiling. If ppt. is washed and allowed to stand 24 hours, it is not as sol. in NH 4 C1 as at first, but natural CaCO 3 is not wholly insol. in NH 4 Cl+Aq; it is, however, much less sol. than MgCO 3 . (Vogel, J. pr. 7. 453.) Sol. in boiling NH 4 Cl+Aq with evolution of NH 3 . (Demarcay, 1834.) When TSlH 4 OH+Aq, incompletely sat. with CO 2 , is mixed with CaCl 2 +Aq, no ppt. occurs even during several days, if kept in a closed vessel; and only a slight ppt. if the mixture is exposed to the air, but CaCO 3 is pptd. if the solution is boiled. NH 4 OH+Aq wholly sat. with CO 2 pro- duces ppt. when mixed with OaCl 2 +Aq, but pptn. is not complete until heat is applied. Also when an excess of CaCl 2 +Aq is added to a solution of crystallized carbonate of am- monia, orly a portion of the CaCO 3 is pptd. until the solution is boiled. (Vogel, 1814.) When CaCl 2 +Aq mixed with NH 4 OH+Aq is exposed to an atmos. of pure CO 2 , no ppt. occurs for several hours, but CaCO 3 is com- pletely pptd. in several days. (Vogel.) When recently pptd., readily sol. in NH 4 C1, and NH 4 NO 3 +Aq. (Brett, 1837; Wacken- roder, A. 41. 315.) When recently pptd., readily sol. in (NH 4 ) 2 C0 3 , (NH 4 ) 2 SO 4 , NH 4 NO 3 , NH 4 C1, and NH 4 succinate+Aq. (Wittstein.) Sol. in NH 4 C 2 H 3 O 2 +Aq. (Thomson.) More sol. in NH 4 C1, or NH 4 N0 3 +Aq, or in neutral potassium, or sodium salts -j-Aq than in H 2 O. (Fresenius.) From solutions in NH 4 salts, NH 4 OH, and (NH 4 ) 2 CO 3 +Aq precipitate CaCO 3 more completely than BaCO 3 . (Fresenius.) When boiled with NH 4 Cl+Aq, CaCO 3 is dissolved, and (NH 4 ) 2 CO 3 given off. (D. Smith.) CaCl 2 +Aq prevents pptn. of CaCO 3 in the cold, as do also NH 4 C1, KC1, or NaCl+Aq, but it is pptd. when boiled, if the latter solu- tions are not too cone. K 2 SO<, KNO 3 , (NH,) 2 SO,, or Na 2 SO 4 +Aq have a similar effect. A large excess of (NH^COs+Aq when quickly added to CaCl 2 +Aq produces no ppt. in the cold. Na 2 CO 3 , or K 2 CO 3 +Aq act likewise. (Storer, Am. J. Sci. (2) 26. 41.) 1 g. CaCO 3 requires 13.98 g. NH 4 C1, 8.380 g. (NH 4 ) 2 SO 4 , or 14.438 g. NH 4 NO 3 to effect solution. (Bertrand, Monit. Sci. (3) 10. 477.) Less sol. in Na than in NH 4 salts, but more than in K salts. (Berthelot.) When NH 4 OH+Aq, partially neutralized by CO 2 , is mixed with CaO 2 H 2 +Aq, no cloudiness appears until the mixture is boiled; when more CO 2 has been added to NH 4 OH + Aq, a ppt. appears at first, which disappears and only reappears on addition of much CaO 2 H 2 +Aq; but NH 4 OH+Aq does not dissolve pptd. CaC0 3 . (Vogel.) Solubility in NH 4 salts +Aq at 25. NH 4 salt Millimols NH 4 salt per 1. Millimols CaO dis- solved per 1. NH 4 C1 1000 500 250 125 6.770 5.008 3.724 2.743 NH 4 NO 3 500 250 125 62.5 5.267 3.830 2.779 2.004 Triammonium citrate 500 250 125 62.5 66.87 39.80 22.64 14.92 (Rindell, Z. phys. Ch. 1909, 70. 454.) Solubility of CaCO 3 in NH 4 Cl+Aq at 12-18. Time, 98 days. g. per 1. of sat. solution NHC1 CaCOa 53.5 100 200 0.423 0.609 0.645 (Cantoni and Goguelia, Bull. Soc. 1905, (3) 33. 27.) Solubility of CaCO 3 in NH 4 NO 3 +Aq at 18. g. per 1. of sat. solution NHiNOs CaCOs 5 10 20 40 80 0.131 0.211 0.258 0.340 0.462 0.584 (Berju and Kosminiko, Landw. Vers. Sta. 1904, 60. 422.) 182 CARBONATE, CALCIUM CaO 2 H 2 +Aq dissolves a little CaCO; (Welter and Berthollet, 1789.) CaO 2 H 2 +Aq retains a little CaCO 3 in solu- tion at ordinary temperature, which is pptd. on boiling. (Eliot and Storer. Proc. Am. Acad. 1860. 5. 63.) CaO 2 H 2 +Aq, mixed with dil. NaOH, KOH, or NH 4 OH+Aq, gives no immediate ppt. when CO 2 is passed through it, unless boiled. Sol. in boiling MgCl 2 +Aq even when dilute. Couste".) Not decomp. when boiled with K 2 SO 4 , Na 2 SO 4 , CaS0 4 , MgSO 4 , and Na 2 B 4 O:+Aq; but partially decomp. by boiling with (NH 4 ) 2 S0 4 , K 2 S0 3 , Na 2 S0 3 , (NH 4 ) 2 SO 3 , Na 2 HPO 4 , (NH 4 ) 2 HPO 4 , K 2 HPO 3 , Na 2 HPO 3 , (NH 4 ) 2 HP0 3 , K 2 HAs0 4 , Na 3 AsO 4 , K 2 C 2 O 4 , (NH 4 ) 2 C 2 4 , NaF, and K 2 CrO 4 +Aq. With the NH 4 salts the decomposition is complete. (Dulong, A. ch. 82. 286.) Not decomp. by alkali sulphates +Aq. (Malaguti.) Precipitation of CaCO 3 is much hindered by alkali citrates or metaphosphates. Solubility in K 2 SO 4 +Aq at 25 . Sp..gr. 25/25 % K 2 S0 4 % CaCO 3 1.010 1.021 1.033 1.048 1.061 1.069 1.083 1.084 1.60 3.15 4.73 6.06 7.85 8.88 10.18 10.48 0.0104 0.0116 0.0132 0.0148 0.0168 0.0192 0.0192 0.0188 (Cameron and Robinson, J. phys. Chem. 1907, 11. 578.) The solubility of CaCO 3 in Na 2 SO 4 +Aq in equilibrium, with air steadily increases with increasing amounts of CaSO 4 in the solution up to saturation point of the CaSO 4 . In the presence of solid CaSO 4 the solubility of CaCC 3 is much decreased. (Cameron and Seidell, J. phys. Chem. 1902, 6. 56.) See under CaH 2 (CO 3 ). Solubility in Na 2 SO 4 -f Aq in contact with CO 2 free air at 25. Sp. gr. 25/25 %KC1 % CaC0 3 g. per 100 g. H 2 O Na 2 SO, CaCOs 1.000 1.024 1.046 1.072 .092 .101 .122 .133 .179 0.00 3.90 7.23 11.10 13.82 15.49 18.21 19.84 26.00 0.0013 0.0078 0.0078 0.0076 0.0072 0.0076 0.0070 0.0072 0.0060 0.97 0.0151 1.65 0.0180 4.90 0.0262 12.69 0.0313 14.55 0.0322 19.38 0.0346 23.90 0.0360 (Cameron, Bell and Robinson, J. phys. 1907, 11. 396.) Solubility in salts +Aq. Ch. (Cameron and Robinson, J. phvs. Chem. 1907, 11. 578.) Solubility in NaCl+Aq in contact with CO 2 free air at 25. g. salt added per litre mg. CaO dissolved per litre Sp. gr. 2o/25 g. per 100 g. H 2 O 0.000 17.4 NaCl CaC0 3 0. 585 g. NaCl 1.17g. 2.93g. 20.05 24.9 31.1 ' .0079 1.60 .0314 5.18 .0466 9.25 .0734 11.48 .0949 16.66 .1346 22.04 .1794 30.50 O.C079 O.C086 O.C094 0.0104 0.0106 0.0115 0.0119 0.85g. NaNO 3 1.70 4.25 24.35 27.7 34.5 0.805g. Na 2 SO 4 , 10H,O 1.61 g. 4.03g. 25.95 31.15 40.7 (Cameron, Bell and Robinson, J. phys. Ch. 1907, 11. 396.) Solubility of CaCO 3 in NaOH +Aq. 0.53g. Na 2 CO 3 1.06g. 2.65g. 8.4 7.2 4.4 Solvent 1 litre dissolves at 18 at 95-100 H 2 O (a. 0.0001 n. NaOH ca. 0.001 n. NaOH ca. 0.01 n. NaOH 12.8 mg. CaCOs 8.7 " 4.2 " 4.3 " 20.7 mg. CaCOs 9.6 " " 6.9 " " 5.7 " " 0.55g. CaCl 2 , 6H 2 O l.lOg. 2.75g. 9.0 8.4 8.4 a,e Blanc, Z. anorg. 1906, 51. 185.) The solubility of CaCO 3 in CO 2 -free water CARBONATE, CALCIUM HYDROGEN 183 is therefore increased by the addition o NaCl, NaNO 3 or Na 2 SO 4 , 10H 2 O, but de- creased by the addition of Na 2 CO 3 or CaCL 6H 2 0. (Gothe, Ch. Z. 1915, 39. 306.) Sol. in ferric chloride or nitrate +Aq with evolution of CO 2 and pptn. of Fe 2 O 6 H 6 (Fuchs 1831) ; also in chlorides or nitrates of Al, Mn Cr, or U, but not in FeCl 2 +Aq. Sol. in cold SnCl 4 +Aq with pptn. of SnO 2 Insol. in cone. Na 2 SO 4 , MgSO 4 , BaCl 2 MgCl 2 , Pb(NO 3 ) 2 , or AgNO 3 +Aq. (Kar sten.) Abundantly sol. when freshly precipitatec in CaCl 2 +Aq, and MgSO 4 +Aq. (Hunt.) Absolutely insol. at 15-19 in BaO 2 H 2 + Aq; also on boiling. 1 1. H 2 O containing 3-4 g. MgSO 4 dissolves 1-2 g. CaCO 3 , and als6 1 g. MgCO 3 . (Hunt Am. J. Sci (2) 26. 109.) 100 pts. NaCl+Aq (2.525% NaCl) dissolve 0.0037 pt. (calculated as CaO) pptd. CaCO 3 and 0.0053 pt. calcspar. (Lubavin, J. russ Soc. 24. 389.) Insol. in liquid NH 3 . (Franklin, Am. Ch J. 1898, 20. 827.) Insol. in liquid CO 2 . (Biichner, Z. phys Ch. 1906, 64. 674.) Alcohol dissolves traces of CaCO 3 . (Gris- chow.) Sol. in Na citrate +Aq. (Spiller.) Sol. in Ca sucrate-j-Aq. (Barreswill.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910,43.314.) Amorphous. Solubility in H 2 cannot be determined because of its instability. (Ken- dall, Phil. Mag. 1912, (6) 23. 972.) Min. Calcite. In contact with air free from CO 2 , 11. H 2 O dissolves at: 25 50 100 0.01433 0.01504 0.01779 g. calcite. (Kendall, Phil. Mag. 1912, (6) 23. 964.) In contact with air containing 3.7 pts. C0 2 per 10,000. the solubility of calcite in H 2 O was found 'to be 0.04608 g. per 1. at 25 and 0.02925 g. per 1. at 50. (Kendall, Phil. Mag. 1912, (6) 23. 973.) Min. Aragonite. In contact with air free from C0 2 , 1 1. H 2 O dissolves at: 25 0.01528 50 0.01617 100 0.01902 g. aragonite. (Kendall, Phil. Mag. 1912, (6) 23. 964.) +5H 2 O. Efflorescent. +6H 2 O. (Pelouze.) Calcium hydrogen carbonate, CaH 2 (CO 3 ) 2 . Known only in aqueous solution. CaCO 3 dissolves in CO 2 +Aq. CaCO 3 is sol. in 1428 pts. H 2 O sat. with CO 2 at 0, and 1136 pts. at 10. (Lassaigne, J. ch. med. 4. 312.) Bineau could dissolve, even in large quantities of H 2 O sat. with CO 2 , only */5 enough CaCOs to form 2 3 2 . Chalk dissolves in 994.5 pts. H 2 O sat. with CO 2 , while Iceland spar requires 3149 pts. (Bischof.) CaCOs is sol. in 1015 pts. H 2 O sat. with CO 2 at 21 and 748.3 mm. (Warington, Chem. Soc. 6. 296.) Solubility of CaCO 3 in CO 2 +Aq at p pressure in atmospheres. CaO+CO 2 = mg. C0 2 and CaO dissolved, corresponding to CaC0 3 =mg. CaC0 3 . P CaO +C0 2 CaC0 3 ' 0.000504 60.96 74.6 0.000808 72.11 85.0 0.00333 123 137.2 0.03187 218.4 223.1 0.0282 310.4 296.5 0.05008 408.5 360 0.1422 533 0.2538 1072 663.4 0.4167 1500 787.5 0.5533 1846 885.5 0.7297 2270 972 0.9841 2864 1086 (Schlosing, C. R. 74. 1522.) With high pressure, 1 1. H 2 O containing CO 2 lissolves at most 3 g. CaCO 3 . This maximum s reached at 5 under 4 atmospheres' pres- sure; at 10-13 under 5 atmospheres; and at 20 under 7 atmospheres. (Caro, Arch. Pharm. (3) 4. 145.) CaCO 3 is sol. in about 1000 pts. H 2 C0 3 + A.q, and solubility is considerably increased by Na 2 SO 4 or MgSO 4 . 000 pts. H 2 O sat. with CO 2 dissolve pts. Carrara marble at t, and B= height of barometer in millimetres. t B Pts. CaCOs t B Pts. CaCOj 7.5 8.5 9.5 20.5 21.5 754 752 754 741 744 1.224 1.202 1.115 0.975 0.935 22.0 26.0 26.5 27.0 28.0 746 740 743 741 737 0.920 0.875 O.$60 0.885 0.770 Or, from 7.5-9.5, 1000 pts. H 2 O sat. with CO 2 dissolve 1.181 pts. CaCO 3 ; from 20.5- 22; 0.9487 pt. CaCO 3 ; from 26-28, 0.855 pt, CaCO 3 . 1S4 CARBONATE, CALCIUM HYDROGEN Other varieties of CaCO s are dissolved as follows in 1000 pts. H f O sat. with CO S . \arunv Luneburg chalk . . Pptd. CaCOj . . . Iceland spar. . . . Calcite Traversella .... Dolomite, semi-trans- parent Dolomite, opaque, in small crystals . . Dolomite, opaque, in large crystals . . Dolomite, transparent, in large crystals Oolithic limestone . . . Dolomitic limestone . 18 IS 18 12 12 11.5 11.5 11 11 15 15.5 741) 740 735 754 754 749 755 746 749 747 740 Pts. O.s3f> 0.950 1.970 1.223 .212 0.654 0.725 .224 1.073 .252 .573 (Cossa, Z. anal. 8. 145.) Solubility of CaCOj in H*0 containing CO S at various pressures. CO- pressure in at in. Solubility (Engel, C. R. 1885, 101. 951.) 1246 1079 1403 1820 2109 1 1. H,O dissolves 0.3850 g. CaH s (CO 3 ), at 15. (Treadwell, Z. anorg. 1898, 17. 186.) 1 1. of sat. CaHj(CO s )j+Aq, obtained from pure or impure limestone, contains 1.13-1.17 f. CaCO 8 at 15. (Treadwell, Z. anorg. 1898, 7. 189.) Solubility of CaHj(CO 8 ) 2 in H 8 O containing CO, at 15. carbonic acid in gas at and 760 mm. partial pressure mm. Free car- bonic acid mg. CaH^Os)i in 100 cc. of the solution mg. Ca 8.94 67.9 157.4 187.2 46.2 6.04 45.9 86.3 175.5 43.3 5.45 41.4 52.8 159.7 39.4 2.18 16.6 48.5 154.0 38.0 1.89 14.4 34.7 149.2 36.8 1 . 72 13.1 24.3 133.1 32.9 0.79 6.0 14.5 124 9 30 8 0.41 3.1 4.7 82.1 20.3 0.25 1.9 29 59.5 14.7 0.08 0.6 40.2 9.9 38 5 9 5 3s f> 9 5 38 5 9* (Treadwell and Reuter, Z. anorg. 1898, 17 185.) 1 1. H>O sat. with carbonic acid dissolves 1.30 g. CaC0 8 at 13.2; 1 r> g. at 2,8 ^Treadwell. /. anon;. 1S9S. 17. IS*U At 30 C. in equilibrium \\ith the aii, not more than 3 per cent of the ealeium present is eomhinetl as CaCO s . At lower tempera- tures and lesser e.oneent rat ions the pereent- age of normal earbonate is even less, aiul prae- tieally all the ealeium present is eombimxl as r'a iUV ... (.Cameron aiul Briggs, ,). phys. (.'hem. 1901, 5. 549.) With pressures less than 4.5 atmosMluMTs of CO 2 no other than normal ealeium ear- bonate or a hydrate of the normal earbonate ean exist as the solid phase at 0. (.Cameron. J. phys. Chem. 191XS, 12. 560.) Solubility in H 2 O in eontaet with air, con- taining TO; with varying partial pres- sures at t. P = partial pressure of CO 8 . t-15 0.8 1.5 1.7 O.S 9.9 13.0 14.0 31.6 g. per 1. 0.193 0.193 0/J3S 0.445 0.627 0.723 o.oso l.ltfO t'Ov 0.117 0.152 o L35 3-J7 0.456 o ;>oo 0.023 1.117 0.7 1.6 4.6 7.8 16.5 30.1 35.5 K. per 1. 0.1 59 0.177 0.341 0.440 o39 0.743 0.755 0.091 0.111 0/20S 0.301 O.S03 t-40 06 1.7 2.9 3.5 7 14.9 22.2 31.7 g. per 1. CnCO, 130 0.143 0.175 O.'JJVJ 0.284 0.3S4 0.427 0.4SO OOi 0.07S O.OS5 0.1(X> 0.169 0231 . 293 0.333 0.470 Similar results at 20, 30, and 35 are also given. (Leather and Sen, Mem. Dept. Agrie. (India) Them. Ser. 1909, 1. 117: Seidell, Solubil- ities, 1919.) CAKBOXATi;, CALCIl.'M HVDJiOr ;K\ 185 Solubility of calcite in H 2 O at 25, in contact with CO 2 under varying pressures. P = approximate pressure of CO 2 in atmos- pheres. Solubility in NaCl+Aq at 25 C. and in equilibrium with air. Ca(HCOah NaCI Grama per liter Reacting wt. per liter Grams per liter Reacting wts. per litre o.ooo" 0.168 0.362 0.522 0.872 1.195 1.695 2.540 4.040 4.520 P g. per 1. sat. solution Solid phase HzCOa Ca(HCOa): 0.1046 0.1770 0.2051 0.2152 0.2252 0.2212 0.2172 0.1971 0.1569 0.1227 0.00065 0.00110 0.00128 0.00134 0.00140 0.00138 0.00135 0.00123 0.00095 0.00076 0.000 9.720 21.010 30.301 50.620 69.370 98.400 147.400 234.500 262.300 O.I 1.1 9.9 13.2 Hi :; 25.4 0..22 2.3 20.0 27.5 34 1 53.2 0.67 1.58 3.62 4.04 4.21 4.22 CaCOa it t( ti Ca(HC0 3 ) 2 n (McCoy and Smith, J. Am. Chem. Soc. 1911, 33. 468.) 1 1. H 2 dissolves 2.3374 g. CaCO, at 5 under a CO 2 pressure of 2 atmos. (Ehlert, Z. Kl.'ktrpchem. 1912, 18. 727.) Solubility data for calcite in H 2 O contain- ing CO 2 , with and without the presence of salts are given by Seyler and Lloyd (Chem. Sac, 1009, 96. 346.) A critical analysis and recalculation of re- sults of Schloesing and others is given by Johnston (J. Am. Chem. Soc. 1915, 37. 2001). CaCO 3 is not dissolved by CO 2 and H 2 O in presence of MgCO 3 . (Leather and Sen, C. A. 1915. 181.) 1 1. of 1/10-normal NaCl+Aq dissolves 0.3320 g. CaH 2 (C0 3 ) 2 at 15. (Treadwell and Router, Z. anorg. 1898, 17. 193.) Solubility of CaH 2 (CO 3 ) 2 in NaCl+Aq sat. with carbonic acid at 15, containing 5 g. NaCiperl/of NaCl+Aq. '/. carbonic ticid in j/as at and mrn. 11 v - partial ftjfo, mg. CaH z (COah in 100 cc. of cf 7(50 mrn. pressure the solution 16.95 128.8 132.5 218.4 53.9 11.47 87.2 110.1 214.3 52.9 6.07 46.1 23.5 149.2 36.8 3.16 24.0 13.5 118.3 29.2 0.50 3.8 2.7 73.9 18.2 0.41 3.4 0.3 49.0 12.1 34.9 8.6 33.7 8.3 32.9 8.1 33.2 8.2 (Treadwell and Reuter, Z. anorg. 1898, 17. 193.) (Cameron and Seidell, J. phys. Chem. 1902, 6. 51.) Solubility in various salts +Aq under a CO 2 pressure of 2 atmos. at 5. Salt g. salt per lOOOg. HzO g. CaCOa sol. in 1 1. of solvent H 2 2.3374 MgCl 2 -f-6H 2 O 6.08 50.0 86.0 350.0 700.0 1150.0 1725.0 2300 (sat.) 2.3518 3.4045 4.0826 3 . 3009 2.7357 ' 2.2054 1.7058 1.4060 NaCI 27 96 50.0 86.0 106.9 175.6 263.4 351 .'2 3.2796 3.7399 3.7828 3.6900 3.3495 2.8107 2. 1625 at 8 MgS0 4 +7H 2 105.3 (14) sat. at 14 2.1768 0.91356 Na 2 SO 4 + 10H 2 O 137. sat. 7 (14) at 14 1.4060 1.9199 (Ehlert and Hempel, Z. Elektrochem. 1912, 18. 727.) Solubility of CaCO 3 in KCl+Aq at 25 sat. with CO 2 at atmospheric pressure. % KCl % CaCOa 3.90 7.23 11.10 13.82 15.49 18.21 19.84 . 26.00 0.145 0.150 0.166 0.165 0.167 0.154 0.140 0.126 (Cameron and Robinson, J. phys. Chem. 1907, 11. 579.) 186 CARBONATE, CALCIUM COPPER URANIUM Solubility in NaCl+Aq in contact with CO at atmospheric pressure at 25. g. per 100 g. H 2 O NaCl 1.45 5.69 11.08 15.83 19.62 29.89 35.85 CaC0 3 0.150 0.160 0.174 0.172 0.159 0.123 0.103 (Cameron, Bell and Robinson, J. phys. Ch 1907, 11. 396.) Solubility in K 2 SO 4 +Aq, sat. with CO 2 atmospheric pressure and 25 temp. at % S0.3 % CaO 0.69 0.69 1.37 0.69 1.67 0.47* 2.18 0.30* 2.99 0.24* * Solid phase, CaSO 4 , K 2 SO 4 . (Cameron and Robinson.) Solubility in Na 2 SO 4 +Aq at 24 in equili- brium with air. Total Ca calc. asCa(HC03) 2 . Grams per liter Ca actually dissolved as Ca(HCO 3 ) 2 . Grams per liter Na 2 S04. Grams per liter 0.0925 0.0925 0.000 0.1488 0.1488 2.800 0.1729 0.1729 + 5.235 0.2330 0.2210 11.730 0.3240 0.3020 36.860 0.3960 0.3440 74.010 0.4580 0.3660, 116.100 0.5630 0.3940 184.200 0.5910 0.4060 213.700 0.6650 0.4300 255.900 (Cameron and Seidell, J. phys. Chem. 1902, 6. 53.) Data are also given for solubility of CaCO 3 in NaCl+Na 2 SO 4 +Aq, and CaCO 3 +CaSO 4 in NaCl+Na 2 SO 4 +Aq. (Cameron, Bell and Robinson.) Calcium copper uranium carbonate, CaCO 3 3CuCO 3 , 4U(CO 3 ) 2 +24H 2 O. Sol. in acids. Calcium lead carbonate, zCaCO 3 , */PbCO 3 . Min. Plumbocalcite. Calcium magnesium carbonate, CaCO 3 , MgC0 3 . Min. Dolomite. 1 1. H 2 O sat. with CO 2 at 18 and 750 mm. dissolves 0.31 g. dolomite. (Cossa, B. 2. 697.) Not obtained by evaporating solution, but can be crystallized from CO 2 +Aq between 100 and 200. (Hoppe-Seyler.) Dolomite is dissolved by CO 2 and H->O, but solution is prevented partially by CaCO 3 , and wholly by MgCO 3 . (Leather and Sen. C. A. 1915. 181.) Insol. in cold dil. acids. (Dolomieu, J. Phys. 39. 1.) Insol. in cold acetic acid. (Forchhammer.) Calcium potassium carbonate, CaK 2 (CO 3 ) 2 . Decomp. by H 2 O. (Reynolds, Chem. Soc. 1898, 73. 265; Butschli, C. A. 1907, 2223). 2CaCO 3 , 3K 2 CO 3 H-6H 2 O. (Butschli.) Calcium sodium carbonate, CaNa 2 (CO 3 ) 2 . Anhydrous. Decomp. by H 2 0. +2H 2 O. (Butschli, C. A. 1907. 2223.) +5H 2 O. Min. Gaylussite. Sparingly sol. in H 2 O. Calcium uranyl carbonate, CaCO 3 , UO 2 C0 3 + 20H 2 O. Min. Liebigite. Sol. in HCl-fAq. +zH 2 O. Decomp. by H 2 O. (Blinkoff, Dissert. 1900.) 2CaO, 4UO 3 , 3C0 2 +24H 2 O. Decomp. by H 2 O. (Blinkoff, Dissert. 1900.) Calcium carbonate chloride, CaC0 3 , CaClo + 6H 2 0. Sol. in H 2 O with immediate decomp. (Fritzsche, J. pr. 83. 213.) Cerous carbonate, Ce 2 (C0 3 ) 3 +5, and 9H 2 O. Insol. in H 2 O, and solution -of CO 2 in H 2 O. (Vauquelin.) Somewhat sol. in (NH 4 ) 2 CO 3 +Aq. (Jolin.) Insol. in neutral salt solutions and neutral alkali carbonates +Aq; easily sol. in SO 2 + Aq. (Berthier, A. ch. (3) 7. 77.) Ceric carbonate, Ce(CO 3 ) 2 + 3^H 2 O. Precipitate. (Hisinger, A. ch. 94. 108.) Insol. in H 2 O. Sol. in slight traces in Na 2 CO 3 +Aq; si. sol. in NaHCO 3 +Aq, and n (NH 4 ) 2 C0 3 +Aq. (Rose.) Cerous lanthanum carbonate fluoride. Min. Batncesite, Hamartite, Hydrofluocerite. Slowly decomp. by HCl-fAq, easily by H 2 SO 4 . carbonate, Ce 2 (CO 3 ) 3 , Cerous potassium K 2 CO 3 +3H 2 O. Ppt. (Jolin.) Ce 2 (CO 3 ) 3 , K 2 CO 3 + 12H 2 O. Ppt. Sol. in 30% K 2 CO 3 +Aq. (Meyer, anorg. 1904, 41. 103.) Z. CARBONATE, CUPRIC, BASIC 187 Perceric potassium carbonate, Ce 2 O 3 (CO 3 ) 3 , 4K 2 CO 3 + 12H 2 O. Crystalline. SI. sol. in H 2 O containing K 2 CO 3 ; sol. in dil. H 2 SO 4 with decomp. (Job, C. R. 1899, 128. 1098.) Cerous sodium carbonate, Ce 2 (CO 3 )3, 2Na 2 CO 3 +2H 2 O. Ppt. (Jolin.) 2Ce 2 (CO 3 ) 3 , 3Na 2 CO 3 +24H 2 Q(?). Ppt. Easily decomp. (Meyer, Z. anorg. 1904, 41. 103.) Chromous carbonate, CrCO 3 . Sol. in much H 2 O; si. sol. in KHCO 3 +Aq. (Moberg, J. pr. 44. 328; Moissan, A. ch. (5) 21. 199.) Chromic carbonate, basic, Cr 2 O 3 , 2CO 2 . Precipitate. (Parkmann, Sill. Am. J. (2) 34. 321.) Cr 2 O 3 , CO 2 +4H 2 O. Insol. in H 2 O; sol. in acids; when freshly pptd. is sol. in K 2 CO 3 , or (NH 4 ) 2 CO 3 +Aq, and still more sol. in KOH +Aq. (Meissner.) Insol. in ethyl acetate (Naumann, B. 1910, 43. 314); methyl acetate. (Naumann, B. 1909, 42. 3790.) 2Cr 2 O 3 , CO 2 +6H 2 O. Precipitate. (Lang- lois, A. ch. (3) 48. 502.) Chromous potassium carbonate, CrC0 3 , K 2 C0 3 + 1^H 2 0. Sol. in H 2 O when freshly prepared; slowly polymerizes; stable in dry air, decomp. in moist air; sol. in acids with decomp. (Bauge, C. R. 1898, 126. 1568.) Chromous sodium carbonate, CrNa 2 (CO 3 ) 2 + H 2 O. Decomp. when heated. In Aq. solution, passes into the hydrate containing 10 mols H 2 O. (Bauge, C. R. 1897, 125. 1179.) + 10 H 2 O. Very sol. in cold H 2 O; Aq. solu- tion decomp. below 100; effloresces in the air sol. in HCl+Aq and H 2 SO 4 +Aq. (Bauge, C. R. 1897, 125. 1178.) Cobaltous carbonate, basic, 5CoO, 2CO 2 -|- 4H 2 O. Insol. in H 2 O; sol. in (NH 4 ) 2 SO 4 , (NH 4 ) 2 CO 3 , NH 4 NO 3 , and NH 4 Cl+Aq. Sol. in cold NH 4 NO 3 , and NH 4 Cl+Aq (Brett, 1837.) Sol. in CO 2 +Aq, and acid alkali carbonates +Aq, from which it is pptd. on boiling Very si. sol. in cone. Na 2 CO 3 , or K 2 CO 3 +Aq largely sol. in (NH 4 ) 2 CO 3 +Aq, and partly sol inNH 4 OH+Aq. (Berzelius.) Not pptd. from solutions containing Na citrate. (Spiller.) 4CoO, CO 2 +4H 2 O. Ppt. (Beetz.) +3H 2 O. (Meigen, C. C. 1905, I. 1363.) Cobaltous carbonate, basic, 3CoO, CO 2 + 2H 2 O. (Meigen, C. C. 1905, I. 1363.) 3H 2 O. (Rose, Pogg. 84. 551.) 3CoO, 2CO 2 +4H 2 O. (Bratin, Z. anal. 6. 76.) 2CoO, CO 2 +3^H 2 O. Converted into 5CoO, 2CO 2 +4H 2 O by H 2 O. (Beetz.) Cobaltous carbonate, CoCO 3 . Anhydrous. Not attacked by cold cone. HC1, or HNO 3 +Aq. (Senarmont, A. ch. (3) 30. 129.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Min. Sphcerocobaltite. SI. attacked by cold HNO 3 , or HCl+Aq. + 2 / 3 H 2 O. Sol. in acids. (Deville, A. ch. (3) 33. 95.) +6H 2 O. (Deville.) Decomp. by H 2 O with formation of a basic carbonate. (Berzelius.) Cobaltous potassium carbonate, CoCO 3 , K 2 CO 3 +4H 2 O. Decomp. by H 2 O. (Deville, A. ch. (3) 33. 90.) Ppt. Decomp. by H 2 O. (Reynolds, Chem. Soc. 1898, 73. 264.) CoCO 3 , KHCO ? +4H 2 O. Decomp. by H 2 O. (Deville.) Cobaltous sodium carbonate, CoCO 3 , Na 2 CO 3 +4H 2 O, and 10H 2 O. Decomp. by H 2 O. (Deville, A.-ch. (3) 33. 75.) Cupric carbonate, basic. The compounds produced by pptn. of copper solutions by carbonates are unstable and possess varying solubilities in solutions of C0 2 . On treatment with solutions of CO 2 , these substances pass over into an apparently stable compound possessing a definite solu- bility in solutions of CO 2 of definite concen- tration, which solubility increases with the concentration of CO 2 . Solubility of this compound in various salts +Aq is recorded. (Free, J. Am. Chem. Soc. 1908, 30. 1374.) 8CuO, CO 2 +5H 2 O. (Deville, A. ch. (3) 33. 75.) 6CuO, CO 2 . (Field, Chem. Soc. 14. 70.) 3CuO, CO 2 +2H 2 O. (Favre, A. ch. (3) 10. 119.) 5CuO, 2CO 2 +6H 2 O. (Struve.) 2CuO, CO 2 +H 2 O. Insol. in H 2 O; easily sol. in acids, even H 2 SO 3 +Aq; si. sol. in H 2 CO 3 +Aq, 30,720 pts. of the solution con- taining 1 pt. CuO. (Jahn.) Sol. in 4690 pts. H 2 CO 3 +Aq sat. at 4-6 atmos. pressure. (Wagner.) Sol. in 3833 pts. sat. H 2 C0 3 +Aq. (Lassaigne, J. ch. med. 4. 312.) Sol. in NH 4 salts+Aq. Partially sol. in Na 2 CO 3 , or K 2 CO 3 +Aq, and more sol. in 188 CARBONATE, COPPER POTASSIUM, BASIC NaHCO 3 , or KHCO 3 +Aq; sol. in (NH 4 ) 2 CO 3 +Aq. (Favre, A. ch. (3) 10. 18.) Less sol. in (NH 4 ) 2 CO 3 +Aq than CuO in NH 4 OH+Aq. (Thomson, 1831.) Sol. in KCN+Aq. (Berzelius.) Sol. in NH 4 C1, or NH 4 NO 3 +Aq. (Brett.) Sol. in ferric salts with pptn. of Fe 2 O 6 H 6 . Insol. in liq. NH 3 . (Franklin and Kraus, Am. Ch. J. 1898, 20. 827.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910,43.314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Sol. in ethyl amine carbonate +Aq. (Wurtz.) Sol. in cane sugar +Aq. (Peschier, Repert. 1820, 6. 85.) Not pptd. from solutions containing sodium citrate. (Spiller.) Insol. in pvridine. (Schroeder, Dissert. 1901.) Min. Malachite. Sol. in acids, and NH 4 OH +Aq. +2H 2 O. (Favre.) 8CuO, 5CO 2 +7H 2 O. (Groger, Z. anorg. 1900, 24. 137.) 3CuO, 2CO 2 +H 2 O. Insol. in H 2 O. Sol. in NH 4 OH+Aq, also in hot cone. NaHCO 3 + Aq. Min. Azwite. Copper potassium carbonate, basic, 8CuO, 2K 2 CO 3 , 7CO 2 +17H 2 0. Ppt.; decomp. by H 2 O. (Groger, B. 1901, 34. 430.) Mixture. (Wood and Jones, C. A. 1907. 2667). 5CuO, 4CO 2 , K 2 CO 3 +10H 2 O. Decomp. by H 2 O. (DeviUe,.A. ch. (3) 33. 102). Cupric potassium carbonate, CuCO 3 , K 2 CO 3 . Decomp. by H 2 O. (Wood and Jones, C. A. 1907. 2667.) +H 2 O. (Wood and Jones.) +4H 2 O. Decomp. by H 2 O. (Reynolds, Chem. Soc. 1898, 73. 263.) Could not be obtained. (Wood and Jones.) 2CuCO 3 , K 2 CO 3 +4H 2 O. Decomp. by H 2 O. '(Wood and Jones.) Cupric sodium carbonate, CuCO 3 , Na 2 CO 3 . Not decomp. by cold H 2 O. (Debray, C R 49. 218.) +3H 2 O. Cupric zinc carbonate, 2CuO, 3ZnO, 2CO 2 + 3H 2 O, or 3CuO, 9ZnO, 4CO 2 +8H 2 O. Min. Aurichalcite. Easily sol. in HC1 + Aq. Cupric carbonate ammonia (cuprammonium carbonate), CuCO 3 , 2NH 3 . Decomp. by H 2 O. Insol. in alcohol and ether. Sol. in (NH 4 ) 2 CO 3 +Aq. (Favre, A. ch. (3) 10. 116.) Didymium carbonate, Di 2 (CO 3 ) 3 +H 2 O, or 6H 2 0. Insol. in H 2 O. Only traces dissolve in CO 2 +Aq. Insol. in solutions of alkali carbonates or bicarbonates-f-Aq. (Marignac, A. ch. (3) 38. 166.) Very si. sol. in cone. NH 4 Cl+Aq. (Rose.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +8H 2 O. (Cleve, Bull. Soc. (2) 43. 363.) Didymium potassium carbonate, Di 2 (CO 3 ) 3 , K 2 C0 3 +4H 2 0. Insol. in H 2 O. (Cleve, Bull. Soc. (2) 43. 363.) + 12H 2 O. (Cleve.) Didymium sodium carbonate, 2Di 2 (COsK 3Na 2 CO 3 +9H 2 O. Ppt. (Cleve.) Di 2 (CO 3 ) 3 ,2Na 2 CO 3 +8H 2 O. Ppt. (Cleve.) Dysprosium carbonate, Dy 2 (CO 3 ) 3 +4H 2 O. Insol. in H 2 O. (Jantsch, B. 1911, 44. 1277.) Erbium carbonate, Er 2 O 3 , 2C0 2 +2H 2 O. Insol. in H 2 O. (Hoglund.) Erbium sodium carbonate, Er 2 (CO 3 ) 3 , 5Na 2 CO 3 +36H 2 O. Efflorescent. Decomp. by H 2 O. Gadolinium carbonate, basic, Gd(OH)CO 3 + H 2 O. Ppt. (Benedicks, Z. anorg. 1900, 22. 417.) Glucinum carbonate, basic, 3G1O, CO 2 ; 4G1O, C0 2 ; 5G10, C0 2 +5H 2 0, etc. Not perceptibly sol. in H 2 O or H 2 CO 3 +Aq. Decomp. by boiling H 2 O. Easily sol. in acids. Sol. in NH 4 salts, and KOH, or NaOH+Aq. Sol. in alkali carbonates, especiallv (NH 4 ) 2 CO 3 +Aq. (Vauquelin.) SI. sol. in K 2 CO,+Aq. When solution in (NH 4 ) 2 CO 3 is boiled, a more basic carbonate is pptd. (Rose.) Glucinum carbonate, G1C0 3 +4H 2 O. Efflorescent. Sol. in278pts. H 2 O. (Klatzo, J. pr. 106. 242.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) No definite carbonate of glucinum exists. (Cameron, J. phys. Chem. 1908, 12. 572.) CARBONATE, LANTHANUM 189 Glucinum potassium 2K 2 CO 3 . carbonate, 3G1C0 3 , Easily sol. in H 2 O, but decomp. by boiling. (Debray.) Less easily sol. in alcohol. Indium carbonate, In 2 (CO 3 ) 3 . Ppt. Insol. in K 2 CO 3 , or Na 2 CO 3 -f-Aq. Sol. in (NH 4 ) 2 CO 3 +Aq. (Winkler, J. pr. 94. 1.) Iron (ferric) carbonate, basic. 9Fe 2 O 3 , CO 2 + 12H 2 O. (Wallace, Chem. Gaz. 1858. 410.) 3Fe 2 O 3 , CO 2 +4H 2 O, and 8H 2 O. (Barrat, C. N. 1. 110.) +6H 2 O. (Wallace.) 2Fe 2 3 , C0 2 + 1KH 2 0. (Rother, Pharm. J. Trans. (3) 4. 576.) Fe 2 O 3 , CO 2 . (Parkmann, Sill. Am. J. (2) 34. 321.) These and other similar basic salts are ppts., easily decomp. on standing into Fe 2 O 6 H 6 . Iron (ferrous) carbonate, FeCO 3 . Insol. in H 2 O. Sol. in acids, even in H 2 CO 3 +Aq. See Carbonate, ferrous hydrogen. Min. Siderite, Spathic ore. SI. attacked by dil . acids . Sol . in H 2 CO 3 + Aq under pressure . Insol. in NH 4 C1, or NH 4 NO 3 +Aq. (Brett.) +H 2 O. SI. sol. in H 2 O; easily sol. in acids: sol. inH 2 CO 3 +Aq. Sol. in NH 4 C1 + Aq . Sol. in ferric salts + Aq with evolution of CO 2 and pptn. of Fe 2 O 6 H 6 . Soluble in an aqueous solution of cane sugar. Solubility in salts+Aq free from CO 2 . Salt g. salt per 1000 g. H 2 1 1. of solvent dissolves g. FeCOa NaCl 351.2 0.35042 MgCl 2 + 6H 2 O 2300.0 4.2049 Na 2 SO 4 + 10H 2 O 137.7 sat. at +14 0.70085 0.93444 MgS0 4 + 7H 2 O 105.3 sat. at +18 1.4667 2.9334 (Ehlert, Z. Elektrochem. 1912, 18. 728.) Iron (ferrous) hydrogen carbonate, FeH 2 (C0 3 ) 2 (?). Known only in aqueous solution. By conducting CO 2 at ordinary pressure through H 2 O, in which Fe is suspended, a solu- tion containing 9.1 pts. FeCO 3 to 10,000 pts. H 2 O is obtained, (v. Hauer, J. pr. 81. 391.) 100 pts. H 2 CO 3 +Aq dissolve 0.72 pt. FeC0 3 . (Wagner.) FeCO 3 dissolves in 1381 pts. H 2 O saturated with CO 2 , under a pressure of 4-6 atmos- pheres. (Wagner, J. B. 1867. 135.) 1 1. H 2 O dissolves 6.1907 g. FeCO 3 (pure) under a CO 2 pressure of 2 atmos. (Ehlert, Z. Elektrochem. 1912, 18. 728.) Solubility in various salts+Aq in presence of CO 2 under pressure of 2 atmos. Salt With COz of 2 atmos. pressure g. salt per 1000 g. H 2 1 1. of solvent dissolves g. FeCCh H 2 6.1907 NaCl 50 106.9 175.6 263.4 351.2 MgCl 2 + 6H 2 O 86.9 700.0 1150.0 1437.5 1725.0 2300.0 5.8403 4.5553 4.4587 4.6934 5.3975 9.0524 Na 2 SO 4 + 10H 2 O 137.7 sat. at +14 7.9428 9.5780 MgS0 4 + 7H 2 O 105.3 sat. at +18 6.2423 7.3922 (Ehlert, Z. Elektrochem. 1912, 18. 728.) A bicarbonate of ferrous iron is not formed under pressures of CO 2 up to 5 atmospheres at 0. (Cameron, J. phys. Chem. 1908, 12. 571.) Iron (ferrous) magnesium carbonate, FeCO 3 , Mo-rn, Min. Pistomesite. FeCO 3 , 2MgCO 3 . Min. Mesitite. Iron (ferrous) potassium carbonate, FeK 2 (CO 3 ) 2 +4H 2 O. Ppt. Decomp. by H 2 O. (Reynolds, Chem. Soc. 1898, 73. 265.) Lanthanum carbonate, La 2 (CO 8 ) 3 -f-H 2 O, 3H 2 O, and 8H 2 O. Insol. in H 2 O. CO 2 +Aq dissolves traces. Insol. in (NH 4 ) 2 CO 3 +Aq. Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Min. Lanthanite. 190 CARBONATE, LANTHANUM POTASSIUM Lanthanum potassium carbonate, La 2 (CO s ) 3 , K 2 CO 3 + 12H 2 O. Sol. in 30% K 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 101.) Lanthanum sodium carbonate, 2La 2 (CO 3 ) 3 , 3Na 2 CO 3 +20H 2 O(?). Ppt. Easily decomp. (Meyer, Z. anorg. 1904, 41. 102.) Lead carbonate, basic, 2PbCO 3 , PbO 2 H 2 ; 5PbCO 3 , 3PbO 2 H 2 ; 3PbCO 3 , PbO 2 H 2 ; 5PbCO 3 , PbO 2 H 2 . Whit" Le~d. Insol. in H 2 O. Nearly insol. in H 2 CO 3 +Aq, even under pressure. Sol. in dil., insol. in cone. KOH+Aq. Insol. in normal, or acid alkali carbonates + Aq . (Bott- ger.) Sol. in cold dil. NH 4 Cl+Aq. (Brett.) PbCO 3 , PbO 2 H 2 . Very si. sol. in H 2 O. (Yorke.) 2PbCO 3 , PbO 2 H 2 . Solubility is less than O.OC02 millimol Pb in 1 liter H 2 O at 18. (Pleissner, C. C. 1907, II. 1056.) When not exposed to air, sol. in 32,000 pts. (NH 4 ) 2 SO 4 +Aq (0.2 g. per 1.); 26,000 pts. KNO 3 +Aq (0.2 g. per 1.); 23,000 pts. CaCl 2 +Aq (0.2 g. per 1.); 4600 pts. NH 4 NO 3 +Aq (0.2 g. per 1.); 4300 pts. H 2 O sat. with CO 2 . When exposed to air in beakers, sol. in 43,000 pts. (NH 4 ) 2 SO 4 +Aq (0.2 g. per 1.); 43,000 pts. KNO 3 +Aq (0.2 g. per 1.); 26,000 pts. CaCl 2 +Aq (0.2 g. per 1.); 26,000 pts. NH 4 NO 3 +Aq (0.2 g. per 1.); 4300 pts. H 2 O sat. with CO 2 (0.2 g. per 1.). (Muir, Chem. Soc. 31. 664.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) 3PbO,4PbCO 3 +2H 2 O. Ppt. (Stromholm, Z. anorg. 1904, 38. 446.) Lead carbonate, PbCO 3 . Sol. in 50,551 pts. H 2 O at ordinary temp. Sol. in 23,450 pts. H 2 O with little ammo- nium acetate, carbonate, and free ammonia; and in somewhat less H 2 O, containing much ammonium nitrate with carbonate and free ammonia. (Fresenius, A. 69. 124.) Calculated from electrical conductivity of PbCO 3 +Aq, 1 1. H 2 O dissolves 3 mg. PbCO 3 at 10. (Kohlrausch and Rose, Z. phys. Ch. Solubility is 0.0002 millimol. Pb in 1 liter H 2 O at 18. (Pleissner, C. C. 1907, II. 1056.) SI. sol. in H 2 O. 1.5 x 10- 3 g. are contained in 1 1. of sat. solution at 20. (Bottger, Z phys. Ch. 1903, 46. 604.) Easily sol. in acids, even HC 2 H 3 O 2 ; but not decomp. by cone. HNO 3 +Aq on account of insolubility of Pb(NO 3 ) 2 in HNO 3 +Aq. In- sol. in a mixture of 1 pt. H 2 SO 4 and 6 pts. absolute alcohol, or in an alcoholic solution of racemic or tartaric acids. Insol. in H 2 CO 3 +Aq. (Jahn, A. 28. 117.) Very si. sol. in H 2 CO 3 +Aq, but solution is prevented by traces of various salts. (Tiin- nerman.) Sol. in 7144 pts. sat. H 2 CO 3 +Aq. (Lassaigne, J. ch. med. 4. 312.) H 2 O sat. with CO 2 under 4-6 atmos. pressure dissolves only traces of Pb; 1000 pts. of solution containing 0.5 pt. PbCO 3 . (Wagner, Z. anal. 6. 167.) Solubility of PbCO 3 in H 2 CO 3 +Aq at 18. mg. per 1. C0 2 2.8 5.4 14.4 26 43.5 106 PbCO* 1.75 6 7 8.2 9.9 10.9 15.4 (Pleissner, C. C. 1907, II. 1056.) Sol. in NH 4 C 2 H 3 O 2 +Aq, and NH 4 Cl+Aq. (Weppen, 1837.) Sol. in KOH+Aq; not ab- solutely insol. at ord. temp, in an excess of K 2 CO 3 , or Na 2 CG 3 +Aq, and still more sol. at 100; but absolutely insol. in NaHC0 3 , KHCO 3 , or (NH 4 ) 2 CO 3 +Aq. (Rose.) Insol. in NH 4 OH+Aq; sol. in KOH or NaOH+Aq; decomp. by boiling Ca(NO 3 ) 2 +Aq. (Berze- lius.) SI. decomp. (Persoz), not at all decomp. (Malaguti) by alkali sulphates +Aq. Partially decomp. by boiling with K 2 SO 4 , Na 2 S0 4 , (NH 4 ) 2 S0 4 , CaSO 4 , MgSO 4 , Na 2 HPO 4 , NaNH 4 HPO 4 , K 2 SO 3 , Na 2 SO 3 , (NH 4 ) 2 SO 3 , Na 2 HPO 3 , Na 2 B 4 O 7 , K 3 As0 4 , Na 3 AsO 4 , K 2 C 2 O 4 , Na 2 C 2 O 4 , NaF, and K 2 CrO 4 +Aq. With the NH 4 salts, the decomp. is complete. (Dulong, A. ch. 82. 290.) Easily sol. in hot NH 4 Cl+Aq. (Brett; Rose.) When 1 mol. PbCO 3 is boiled with 1 mol. K 2 C 2 O 4 , 15% of the PbCO 3 is decomp.; with 1 mol. K 2 CO 3 , 93.28% is decomp. (Mala- guti.) Not decomp. by K 2 SO 4 +Aq. (Rose.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898,^20.828.) Sol. in an aqueous solution of acetates. (Mercer, 1844.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Not pptd. in presence of Na citrate. (Spiller.) Min. Cerussite. Lead sodium carbonate, 4PbCO 3 , Na 2 CO 3 . Insol. in H 2 O. (Berzelius, Pogg. 47. 199.) Lead carbonate bromide, PbCO 3 , PbBr 2 . Insol. in H 2 O. (Storer's Diet.) CARBONATE, LITHIUM 191 Lead carbonate chloride, PbCO 3 , PbCl 2 . Insol. in H 2 O. (Miller, Chem. Soc. (2) 8. 37.) Min. Phosgenite. Easily sol. in acids. Lead carbonate iodide, PbCO 3 , PbI 2 . Insol. in H 2 O. (Poggiale.) (Tschugaeff, Z. anorg. 1914, 86. 159.) Sat. solution boils at 102. (Kremers.) More sol. in CO 2 +Aq than in H 2 O. 100 pts. sat. CO 2 +Aq dissolve 5.25 pts. Li 2 CO 3 . (Troost.) See LiHCO 3 . Sol. in NH 4 salts +Aq. Solubility in salts -f-Aq at 25. C = concentration of salt solution in g.- equiv. per 1. S = solubility of Li 2 CO 3 in g.-equiv. per 1. Lead carbonate sulphate, PbCO 3 , PbSO 4 . Min. Lanarkite. Sol. in HNO 3 +Aq with residue of PbSO 4 . 3PbCO 3 , PbSO 4 . Min. LeadhilLite. As above. Lithium carbonate, Li 2 CO 3 . 100 pts. H 2 O dissolve 1 pt. Li 2 CO 3 . (Vau- quelin, A. ch. 7. 284.) 100 pts. H 2 O at 13 dissolve 0.769 pt. Li 2 CO 3 ; at 102, 0.778 pt. Li 2 CO 3 . (Kremers, Pogg. 99. 48.) 100 pts. H 2 O, cold or hot, dissolve 1.2 pts. Li 2 CO 3 . (Troost, A. ch. (3) 61. 103.) 100 pts. HoO dissolve 1.4787 pts. at 15, 0.7162 pt. at 100. (Draper, C. N. 56. 169.) 100 pts. H 2 O dissolve pts. Li 2 CO 3 at t. Salt C s KNO 3 0.25 0.50 0.75 1.00 1.50 2.00 0.3647 0.3688 0.3676 0.3656 0.3490 0.3268 KC1 0.10 0.25 0.50 0.75 1.00 1.50 2.00 0.3553 0.3590 0.3782 0.3832 0.3835 0.3731 0.3558 NaCl 0.10 0.25 0.50 0.75 1.00 1.50 2.00 0.3569 0.3691 0.3867 0.3956 0.3946 0.3901 0.3776 t Pts. LixCOi t Pts. Li 2 CO 3 1.539 75 0.866 10 1.406 100 0.728 20 1.329 102 0.796 50 1 . 181 K 2 SO 4 0.25 0.50 1.00 0.4028 0.4356 0.4860 2 0.796 pt. is dissolved at 102 in less than J4 hour, and 0.955 in 1 hour. (Beketow, J. russ. Soc. 1884. 591.) Sat. solution at 15 has sp. gr. 1.014, and contains 1 g. Li 2 CO 3 to 70 g. H 2 O, while solu- tion sat. at has sp. gr. 1.0168 and contains 1 g. Li 2 CO 3 in 64.6 g. H 2 O. By long spon- taneous evaporation at 15 a solution can be obtained of 1.0278 sp. gr. containing 1 g. Li 2 CO 3 in 45.57 g. H 2 O. (Fliickiger, Arch. Pharm. (3) 25. 549.) By boiling for an instant with H 2 O a solu- tion is obtained, which has sp. gr. 1.0074 and contains 1 g. Li 2 CO 3 to 139 g. H 2 O. (Fliicki- ger, Arch. Pharm. (3) 26. 543.) 0.1687 mol. is sol. in 1 1. H 2 O at 25. (Roth- mund, Z. phys. Ch. 1909, 69. 531.) Sat. Li 2 CO 3 +Aq contains at: 95 75 0.723 0.833% by wt. Li 2 CO 3 . Na 2 SO 4 0.50 1.00 2.00 0.4411 0.4926 0.5534 2 NH 4 C1 0.10 0.25 0.50 0.75 1.00 1.50 2.00 4.00 0.3902 0.4677 0.5659 0.6270 0.6810 0.7463 0.7739 . 0.7881 (NH 4 ) 2 S0 4 0.25 0.50 1.00 1.50 2.00 0.5059 0.7863 0.9804 1.109 1.174 2 KC10 3 0.1 0.2 0.4 0.3500 0.3570 0.3616 (Geffcken, Z. anorg. 1905, 43. 198.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) 192 CARBONATE, LITHIUM HYDROGEN Solubility in organic compds. +Aq at 25. Solubility in H 2 O at 25 =0.1687 mols. litre. Solubility in organic compds. +Aq. at 25 -Continued. Organic compd. Normality of the solution Mol. Li 2 C0 3 sol. in 1 1. Organic compd. Normality of the solution Mol. Li 2 C0 3 sol. in 1 1. Methyl alcohol 0.250 0.5 1.0 0.1604 0.1529 0.1394 Thio-urea 0.125 0.250 0.5 1.0 0.1667 0.1643 0.1600 0.1523 Ethyl alcohol 0.125 0.250 0.5 1.0 0.1614 0.1555 0.1417 0.1203 Dimethyl-pyrone 0.125 0.250 0.5 1.0 0. 1562 0-. 1460 0.1284 0.0992 Propyl alcohol 0.125 0.250 0.5 1.0 0.1604 0.1524 . 1380 0.1097 Ammonia 0.125 0.250 0.5 1.0 0.1653 0.1630 0.1577 0.1466 Tertiary amyl alcohol 0.125 0.250 0.5 1.0 0.1564 0.1442 0.1224 0.0899 Diethylamine 0.125 0.250 0.5 1.0 0.1589 0.1481 0.1283 0.0937 Acetone 0.125 0.250 0.5 1.0 0.1600 0.1515 0.1366 0.1104 Pyridine 0.125 0.250 0.5 1.0 0.1592 0.1503 0.1347 0.1091 Ether 0.125 0.250 0.5 0.1580 0.1476 0.1300 Piperidine 0.125 0.250 0.5 1.0 0.1584 0.1488 0.1320 0.1009 Formaldehyde 0.125 0.250 0.5 1.0 0.1668 0.1653 0.1606 0.1531 Urethane 0.125 0.250 0.5 1.0 0.1604 0.1525 0.1377 0.1113 Glycol 0.125 0.250 0.5 1.0 0.1660 0.1629 0.1565 0.1472 Acetamide 0.250 0.5 1.0 0.1614 0.1520 0.1358 Glycerine 0.125 0.250 0.5 1.0 0.1670 0.1647 0.1613 0.1532 Acetonitrile 0.125 0.250 0.5 1.0 0.1618 0.1556 0. 1429 0.1178 Mannitol 0.125 0.250 0.5 0.1705 0.1737 0.1778 Mercuric cyanide 0.125 0.250 0.1697 . 1704 Glucose '0.125 0.250 0.5 1.0 0.1702 0.1728 0.1752 0.1778 (Rothmund, Z. phys. Ch. 1909, 69. 531.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Lithium hydrogen carbonate, LiHCOs. 100 pts. H 2 O dissolve 5.501 pts> at 13. (Bewad, B. 17. 406 R.) Sucrose 0.125 0.250 0.5 1.0 0.1693 0.1689 0.1661 0.1557 Urea 0.125 0.250 0.5 1.0 0.1686 0.1673 0.1643 0.1605 CARBONATE, MAGNESIUM 193 Magnesium carbonate, basic, Mg 3 C 2 O 7 + 3H 2 O =3MgO, 2CO 2 +3H 2 O or 2MgC0 3 , MgO 2 H 2 +2H 2 O. (Fritzsche, Pogg. 37. 310.) Magnesia alba, 3MgCO 3 , Mg(OH) 2 + 4H 2 0, 4MgG0 3 , Mg(OH) 2 +5H 2 0, or 5MgC0 3 , 2Mg(OH) 2 +7H 2 0. Very si. sol. in H ? O. Sol. in 10,000 pts. hot or cold H 2 0. (Bineau.) Sol. in 2500 pts. cold, and 9000 pts. hot H 2 0. (Fyfe.) Sol. in H 2 Q containing CO 2 . Very easily sol. in acids. Easily sol. in dil. HCl+Aq. Easily sol. in NH 4 sulphate, nitrate, or suc- cinate+Aq, also in (NH 4 ) 2 C0 3 +Aq. (Witt- stein.) Sol. in cold Na 2 CO 3 , K 2 C0 3 , K 2 S0 4 , KC1, or KNO 3 +Aq (Longchamp); also in NH 4 Cl+Aq, separating out on heating. (Vogel, J. pr. 7. 455.) Slowly sol. in cone. BaCl 2 , CaCl 2 , or ZnSO 4 +Aq. (Karsten.) Sol. in MgSO 4 +Aq. (Dulong.) Sol. in ferric salts +Aq with evolution of C0 2 and pptn. of Fe 2 6 H 6 . (Fuchs.) Sol. in boiling Co, Ni, Zn, Mn, or Cu nitrates or chlorides +Aq. Min. Hydromagnesite, 4MgO, 3CO 2 + 4H 2 O. -j-10H 2 O. Sol. in considerable amount in H 2 C0 3 +Aq as MgH 2 (CO 3 ) 2 +Aq. (Engel, C. R. 100. 911.) Magnesium carbonate, MgCO 3 . A'i hydrous. Insol. in H 2 O. 1 1. H 2 O dis- solves 106 mg. MgC0 3 . (Chevalet, Z. anal. 8.91.) Sol. in 5071 pts. H 2 O at 15. (Krem- ers.) MgCO 3 combines with H 2 O to form MgCO 3 +3H 2 O, and +5H 2 O, which are less sol. in H 2 O than anhydrous salt. (Engel, C. R. 101. 814.) Very hydroscopic. About 20 g. are sol. in 1 1. H 2 O. (Engel, C. R. 1899, 129. 598.) 0.7156 g. are sol. in 1 1. H 2 O at 15. 0.627 g. are sol. in 1 1. H 2 O at 15 with vapour pressure of CO 2 equal to zero. 6.977 grams are sol. in 1 1. H 2 at 15 with vapour pressure CO 2 equal to 1 atmos. (Treadwell and Reuter, Z. anorg. 1898, 17. 202.) 94.4 mg. are sol. in 1 1. of CO 2 -free water. (Gothe, Ch. Z. 1915, 39. 306.) Solubility in H 2 O in equilibrium with Mg(HC0 3 ) 2 and CO 2 . Svstem: MgCO 3 , Mg(HC0 8 ) 2 and CO 2 at 30 t). Total Mg (gram- atoms per liter) Mg as MgCOs Per cent MgasMg(HCO 3 )2 Per cent 0.00100 0.00545 0.00667 50.00 51.92 53.93 50.00 48.08 46.07 Total salts in solution. Grams per liter MgCOa Mg(HC0 3 ) 2 Grams per liter Per cent Grrms per liter Per cent 0.1144 0.6174 0.7479 0.0418 0.2368 0.3012 36.5 38.2 40.3 0.0726 0.3806 0.4467 63.5 61.7 59.7 Total Mg (grams per liter) Mg as MgCOa (grams per liter) Mg as Mg(HC03)2 (grams per liter) 0.02410 0.13135 0.16087 0.01205 0.06820 0.08676 0.01205 0.06314 0.07411 Solubility in H 2 O in equilibrium with Mg(HCO 3 ) 2 and CO- 2 ~Continued. System: MgCO 3 , Mg(HCO 3 ) 2 and CO 2 at 30 C. In a solution near the saturation point and in equilibrium with atmospheric air upwards of 50 per cent of the magnesium is in the form of the normal carbonate. When the solution is brought in contact with the solid phase, the proportion of the base combined as normal carbonate falls to about 34 per cent, or lower. (Cameron and Briggs, J. phys. Chem. 1901, 5. 552-3.) For solubility in H 2 CO 3 +Aq, see Magne- sium hydrogen carbonate. Scarcely acted upon by HCl+Aq. (Senar- mont.) The solubility of MgC0 3 in NaCl+Aq when in contact with ordinary air increases with increasing concentration of NaCl up to a maximum, and then decreases. (Cam- eron and Seidell, J. phys. Chem. 1903, 7. 579.) Solubility of MgC0 8 in salts +Aq in equilib- rium with an atmosphere free from CO 2 NaCl+Aq;t = 23. Weight of liter of solution Grams NaCl per liter Grams MgCOs per liter Reacting weights NaCl per liter Reacting weights MgCOa per liter 0.00210 0.00500 0.00630 0.00699 0.00650 0.00550 0.00470 0.00350 996.92 1016.82 1041.09 1070.50 1094.53 1142.48 1170.14 1199.28 0.0 28.0 59.5 106.3 147.4 231.1 272.9 331.4 0.176 0.418 0.527 0.585 0.544 0.460 0.393 0.293 0.000 0.482 1.025 1.831 2.539 3.981 4.701 5.709 (Cameron and Seidell, J. phys. Chem. 1903, 7. 585.) 194 CARBONATE, MAGNESIUM Solubility of MgCO 3 in salts +Aq Continued Na 2 S0 4 +Aq;t=24. Solubility in salts +Aq. -Continued g. salt added per litre mg.MgCOs dissolved per litre Weight of liter of solution Grams Na 2 S0 4 per liter Grams MgCOs per liter Reacting wts. Na 2 S04 per liter Reacting wts. MgCO per liter 0.805g. Na 2 SO 4 , 10H 2 O 1.61 g. 4.03g. , " 145.05 162.05 150.75 997.52 1021.24 1047.60 1080.95 1133.85 1157.34 1206,03 1223.91 1241.99 0.00 25.12 54.76 95.68 160.80 191.90 254.60 278.50 305.10 0.216 0.586 0.828 1.020 1.230 1.280 1.338 1.338 1.388 0.000 0.178 0.388 0.678 1.140 1.360 1.804 1.973 2.162 0.00258 0.00700 0.00990 0.01219 0.01470 0.01530 0.01600 0.01600 0.01660 0.53g. Na 2 C0 3 1.06g. " 2.65g. " 98.6 53.5 15.7 0.51g. MgCl 2 , 6H 2 O 1.02g. 2.55g. 47.0 39.5 35.3 The solubility of MgCO 3 in CO 2 -free water is increased by the addition of NaCl, IS aNO or Na 2 SO 4 , 10H 2 O but decreased by the addi- tion of Na 2 CO 3 or MgCl 2 , 6H 2 0. (Gothe, Ch. Z. 1915, 39. 306.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) Min. Magnesite. Very si. attacked by warm cone. HCl+Aq. 100 pts. H 2 O dissolve 0.0027 pt., calculated as MgO. (Lubavin.) Solution in H 2 O contains 0.018 g. Mg and 0.065 g. C0 2 per 1. at 20. (Wells, J. Am. Chem. Soc. 1915, 37. 1705.) Solution in H 2 O containing 27.2 g. NaCl per 1. contains 0.028 g. Mg and 0.086 g. C0 2 per 1. at 20. (Wells, J. Am. Chem. Soc. 1915, 37. 1705.) +H 2 0. +2H 2 O. Decomp. by suspension in H 2 into basic salt. (Engel, C. R. 100. 911.) +3H 2 0. Small quantities of this salt are wholly dissolved by much H 2 O. (Bineau.) The solution contains in 100 pts. at 6.5 8 16 0.15 0.153 0.155 0.179 pts. MgCO 3 -f3H 2 0. (Norgaard, 1860.) Decomp. by boiling H 2 O into a basic insol. salt and CO 2 . 100 pts. H 2 O dissolve 0.1518 pt. at 19. (Fritzsche, Pogg. 37. 304.) Sol. in 48 pts. H 2 0, and decomp. by large amt. (Fourcroy.) 100 pts. H 2 O~ dissolve 0.1518 pt. at 19, or sol. in 658 pts. H 2 O at 19. (Beckurts, J: B. 1881. 212.) 100 pts. H 2 O dissolve 0.0812 pt., calculated as MgO. (Lubavin, J. russ. Soc. 24. 389.) Solution in H 2 O contains 0.36 g. Mg and 1.01 g. CO 2 per 1. at 20. (Wells, J. Am. Chem. Soc. 1915, 37. 1707.) Solubility in H 2 O sat. with C0 2 has been determined at 20, 25, 30, 34 and 39 and t=35.5. Weight of liter of solution Grams Na 2 S04 per liter Grams MgCOs per liter Reacting weights Na 2 S04 per liter Reacting weights MgCOs per liter 995.15 1032.89 1067.23 1094.77 1120.38 1151.70 1179.82 1196.32 1236.52 0.32 41.84 81.84 116.56 148.56 186.70 224.00 247.20 199.20 0.131 0.577 0.753 0.904 0.962 1.047 1.088 1.100 1.130 0^296 0.579 0.826 1.052 1.323 1.587 1.751 2.120 0.00156 0.00689 0.00900 0.01080 0.01149 0.01251 0.01300 0.01314 0.01350 (Cameron and Seidell.) Na 2 CO 3 -fAq;t=25. Weight of liter of solution Grams Na 2 COs per liter Grams MgCOs per liter Reacting weights Na 2 COs per liter Reacting weights MgCOs per liter 096.84 1019.89 1047.72 1082.47 1118.91 1147.66 1166.05 1189.38 0.00 23.12 50.75 86.42 127.30 160.80 181.90 213.20 0.223 0.288 0.510 0.879 1.314 1.636 1.972 2.317 0.000 0.220 0.482 0.820 1.209 1.526 1.727 2.024 0.00266 0.00344 0.00620 0.01027 0.01570 0.01955 0.02357 0.02770 (Cameron and Seidell.) Solubility in salts +Aq. g. salt added per litre mg.MgCOs dissolved per litre 0.0 94.4 0.585g. NaCl 1.17g. " 2.93g. " 128.3 134.4 120.95 0.85 g. NaN0 3 1.70g. " 4.25 g. " 122.85 138.80 137.20 CARBONATE, MAGNESIUM HYDROGEN 195 at CO 2 pressures corresponding with 0.5 to 30.3% CO 2 in the gas phase. (Leather and Sen, Chem. Spc. 1915, 108 (2) 13.) Easily sol. in acids, even when dil Not decomp. by 1 pt. H 2 SO 4 +6 pts. al- cohol, or by alcoholic solutions of glacial acetic, racemir, or tartaric acids, but is slowly decomp. by alcoholic solution of citric acid, or HN0 3 +abs. alcohol. (Butini, 1827.) 100 pts. NaCl+Aq (2.525%) dissolve 0.1250 pt., calculated as MgO. (Lubavin.) 1% Na 2 CO 3 +Aq, when mixed with 1% MgSO 4 +Aa, cause no ppt., but 1.5-2% solu- tions ppt. this salt. (Brandes, 1825.) More sol. in NH 4 Cl+Aq than CaC0 3 . Sol. in NH 4 NO 3 +Aq, but less easily than in NH 4 Cl+Aq. Solubility in KHCO 3 +Aq at t. Values are given in mol./litre. t K Mg Solid phase 15 0.0 0.0095 MgC0 3 +3H 2 O O.G992 0.0131 " . 1943 0167 " 3992 0.0211 " labile 0.2681 0.0192 MgCOs +3H 2 +MgC0 3 KHCOs +4H 2 O 0.5243 0.0097 MgC0 3 , KHCOs +4H 2 O, 0.6792 0.0074 " 0:9810 0.0028 M 25 0.0 0.0087 MgCOs+3H 2 O 0.0985 0.0115 " 0.2210 0.014P " 0.3188 0.0175 " 0.3434 0.0181 " 0.4216 0.0205 labile 0.4985 0.0207 0.3906 C.0196 MgCOs +3H 2 O +MgCOs KHC0 3 +4H 2 O 0.5893 0.0128 MgCOs, KHC0 3 -HH 2 O 0.6406 0.0117 " 0.788 0.0089 1.125 0.0061 " 35 0.0 0.0071 MgCO 3 +3H 2 O 0.1092 0.0098 " 0.2001 0.0132(?) 0.2811 0.0142 3704 0163 < 4847 0177 ! 5807 G 0198 " 5088 0184 MgCO.3 +3H 2 O +MgCO 3) KHCOs +4H 2 O 6231 0153 MgCOs, KHCOs +4H 2 O 8435 0119 The experiments were performed in such a way as to prevent, as far as possible, loss of CO 2 from the solutions. f (Auerbach, Z. Elektrochem. 1904, 10. 164.) 1 1. H 2 O, containing 6% MgSO 4 +7H 2 O and a little NaCl, dissolves 5 g. MgCO 3 . (Hunt, Sill. Am. J. (2) 42. 49.) More sol. in cold alkali borates+Aq than in hot. (Wittstein.) Sol. in Na citrate +Aq. +4H 2 O. Efflorescent. +5H 2 0. Two modifications. a. Plates. Sol. in 600 pts. H 2 at 0-7; solution gradually separates out MgCO 3 -f 2H 2 O. H 2 C0 3 +Aq sat. at 3-4 atmos. pres- sure dissolves 9% at 0-4, MgSO 4 +Aq dis- solves 4% moist salt at 3-4, and it is easily sol. in Na 2 CO 3 , or NaHCO 3 +Aq. (Norgaard.) 13. Prisms. More efflorescent than a. Sol. in 600 pts. H 2 O but not in MgSO 4 , or Na 2 CO 3 +Aq. Both forms are decomp. by boiling H 2 O. (Norgaard.) Magnesium hydrogen carbonate, MgH 2 (C0 3 ) 2 (?). Known only in solution. 1 1. H 2 CO 3 +Aq sat. at 1 atmos. pressure dissolves 23.5 g. MgCO 3 . (Bineau.) 1 1. carbonic acid water dissolves 0.115 g. magnesite at 18 and 0.75 m. pressure. (Cossa, B. 2. 697.) 1 pt. MgOO 3 dissolves in H 2 O saturated with CO 2 at 5 and a pressure of 123 456 atmospheres in 161 144 134 100.7 110 76 pts. H 2 O (Merkel, Techn. J. B. 1867. 213.) H 2 CO 3 +Aq sat. at 3-4 atmos. pressure and 0-4 dissolved 9% MgCO 3 +5H 2 O. (Norgaard.) MgCO 3 +3H 2 O is sol. in 72.4 pts. H 2 CC 3 + Aq sat. at 20 and ord. pressure; 30.5 pts. H 2 CO 3 +Aq sat. at 2 atmos. pfessure; 26.0 pts. H 2 CO 3 +Aq sat. at 3 atmos. pressure; 21.1 pts. H 2 CO 3 +Aq sat. at 4 atmos. pres- sure; 17.09 pts. H 2 CO 3 -}-Aq sat. at 5 atmos. pressure. (Beckurts, J. B. 1881. 212.) 1. H 2 O sat. with CO 2 at p pressure and t dissolves g. MgC0 3 . atmos. 1.0 2.1 3.2 4.7 5.6 6.2 7.5 9.0 19.5 19.5 19.7 19.0 19.2 19.2 19.5 18.7 Mg g COs .79 .11 .3 .5 .2 .51 .2 .59 P mm. 751 760 762 764 764 765 765 765 765 13.4 19.5 29.3 46 62 70 82 91 100 Mg g COs 28.45 25.79 21.95 15.7 10.4 8.1 4.9 2.4 0.0 (Engel and Ville, C. R. 93. 34.) The low figures of other observers are due to their using basic carbonates. By very care- ful experiments it was found that 1 1. H 2 O 196 CARBONATE, MAGNESIUM POTASSIUM sat. with CO2 at 1 atmos. pressure and t dis- solved the following amts. of MgC0 3 : t MgCO: t MgCOs t MgCOs 3.5 12 35.6 26.5 18 30 22.1 15.8 40 50 22.1 9.5 (Engel, G. R, 100. 444.) Solubility in NaCl+Aq at 23C. in equilib- rium with an atmosphere of CO 2 . g. NaCl per liter g. Mg(HCO 3 )2per liter 7.0 56.5 119.7 163.9 224.8 306.6 30.64 30.18 - 27.88 24.96 20.78 10.75 (Cameron and Seidell, ,T. phys. Chem. 1903, 1.9540 g. are sol. 1 1. H 2 O at 15. (Tread- i. ooz.; well and ' euter, Z. anorg. 1898, 17. 202.) MgH 2 (CO 3 ) 2 is not stable except in the presence of free C0 2 . Solubility in Na 2 S0 4 +Aq at 23 C. in equilib- rium with an atmosphere of CO 2 . At 15 and 760 mm., a solution having the partial pressure of CO 2=0, contains Strength of Na2SO4+Aq g. MgCHCOs)? in 100 ccm. 1.9540 g. MgH 2 (C0 3 ) 2 and 0.7156 g. MgCO 3 0.0 1.463 per liter. (Treadwell and Ii euter, Z. anorg. 12% 1.916 1898,17.204.) saturated 1 . 612 (Cameron ard Seidell.) Solubility of MeH^COs)? in H 2 O containing carbonic acid, at 15. . Magnesium potassium carbonate, MgK 2 (C0 3 ) 2 +4H 2 0. a Quickly decomp. by cold H 2 O. (Deville, el H g| a u A. ch. (3) 33. 87.) -X o3 i M 8 0*3 ^ '"5 M Ppt. Decomp. by H 2 O. (Reynolds, Chem. I -si s tc a> 0"o.2 Soc. 1898, 73, 264.) 111 ~ S J S".2 H gJ2 M MgKH(CO 3 ) 2 +4H 2 0. Insol. in H 2 O, but fP S S ** tab So .0 K S decomp. thereby into an insol. basic Mg car- $$ c g MC g2 bonate, and MgH 2 (CO 3 ) 2 and KHCO 3 , which S"* dissolve. (Berzelius.) 18.86 5.47 4.45 143.3 41.6 33.8 119.0 86.6 223.5 1210.5 1210.5 1210.5 .... 201.6 201.6 201.6 Magnesium rubidium hydrogen carbonate, MgRbH(C0 3 ) 2 +4H 2 0. 1.54 11.7 1076.6 77^3 201^6 Decomp. in the air. (Erdmann, A. 1897, 1.35 10-3 762.9 76.5 149.2 294. 75.) 1.0V 8.2 595 2 80 7 122 4 0.62 4.7 366.3 7o!i 86^5 Magnesium sodium carbonate, MgCO 3 , 0.60 4.6 341.7 75.8 78.8 Na 2 CO 8 . 0.33 2.5 . . . 263.2 74.8 65.5 Quickly decomp. with H 2 O. (Deville, A, 0.21 1.6 222.9 77.1 59.4 ch. (3)33.89.) 0.14 1.1 216.9 71.0 56.6 +15H 2 0. (Norgaard.) 0.03 0.3 . . . 203.6 71 1 54 5 . . . 203.3 68.5 53.6 Magnesium sodium carbonate 'sodium chlo- ... 196.0 70.2 52.9 ride, MgCO 3 , Na 2 C0 3 , NaCl. 203.6 62.5 52.0 Decomp. by H 2 O. (de Schulten. C. R. 195.4 61.6 51.1 1896, 122. 1427.) . . . 195.4 64.1 51.8 (Treadwell and R euter, Z. anorg. 1898, 17. 200.) No bicarbonate of magnesium is formed under pressures of CO 2 up to five atmos- pheres at 0. (Cameron, J . phys. Chem. 1908 12. 570.) A critical analysis and recalculation of results of Engel and others is given fa Johnston (J. Am. Chem. Soc. 1915 37 Permanent. Practically insol. in H 2 0. Sol. in H 2 CO 3 +Aq and in acids generally. 1 1. H 2 O dissolves 0. 065 g. at 25. (Ageno and Valla, Att. Accad. Line. 1911, 20, II. 706.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Min. Rhodochrosite. + 1 A, or 1H 2 O. Insol. in H 2 O. Sol. in acids. Sol. in H 2 CO 3 +Aq. 1 pt. MnCO 5 requires 2000 pts. H 2 CO z +Aq for solution. CARBONATE, POTASSIUM 197 (Lassaigne.) Sol. in 7680 pts. H 2 O, and 3840 pts. H 2 O containing CO 2 . (Jahn.) When freshly precipitated is sol. in NH 4 salts +Aq. (Wittstein.) Not more sol. in H 2 contain- ing Na 2 CO 3 or K 2 CO 3 than in pure H 2 O. (Ebelmen.) Insol. in NH 4 C1, or NH 4 N0 3 + Aq. (Brett.) Sol. in ferric salts +Aq, with evolution of CO 2 and pptn. of Fe 2 O 6 H 6 . (Fuchs.) Not pptd. in presence of Na citrate. (Spiller.) Manganous potassium carbonate, MnK 2 (CO 3 ) 2 +4H 2 O. Ppt. Decomp. by H 2 O alone. SI. sol. in Mn(C 2 H 3 O 2 ) 2 +Aq or K 2 CO 3 + Aq. (Reynolds, Chem. Soc. 1898, 73. 264.) Manganous carbonate hydroxylamine, 4MnC0 3 , 3NH 3 0+2H 2 0. Ppt. Sol. in acids. (Goldschmidt Syngros, Z. anorg. 5. 138.) and Mercurous carbonate, Hg 2 CO 3 . Ppt. Decornp. by hot H 2 O. Sol. in hot or warm NH 4 Cl+Aq, but less easily than mer- curic carbonate; less sol. in NH 4 NO 3 +Aq. (Brett, 1837.) SI. sol. in K 2 CO 3 +Aq; partially sol. with decomp. in NH 4 OH-f-Aq. (Wittstein.) Mercuric carbonate, basic, 4HgO, CO 2 . Can be washed with cold H 2 without de- comp. (Millon, A. ch. (3) 19. 368.) 3HgO, CO 2 . Insol. in cold H 2 O. Sol. in CC 2 -}-Aq; si. sol. in K 2 CO 3 +Aq. Easily sol. in NH 4 Cl+Aq. (Berzelius.) Neodymium potassium carbonate, Nd 2 (C0 3 ) 3 , K 2 C0 3 +12H 2 O. Ppt. Sol. in 30% K 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 105.) Neodymium sodium carbonate, 2Nd 2 (CO 3 ) 3 , 3Na 2 C0 3 +22H 2 O(?). Ppt. Easily decomp. SI. sol. in cone. Na 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 106.) Nickel carbonate, basic, 3NiO, CO 2 +5H 2 O. Min. Zaratile. Easily sol. in HCl+Aq. Pptd. nickel carbonate is a basic salt of varying composition. Insol. in H 2 or H 2 C0 3 +Ao. Sol. in acids. Sol. in (NH 4 ) 2 CO 3 +Aq; very si. sol. in Na 2 CO 3 -fAq; sol. in warm NH 4 Cl+Aq, andKCN+Aq. (Rose.) Not pptd. in presence of Na citrate. (Spil- ler.) Nickel carbonate, NiCO 3 . 1 1. H,O dissolves 0.0925 g at 25%. (Ageno and Valla, Att. Accad. Line. 1911, 20, II. 706.) Not attacked by cold cone. HC1, or HNO, +Aq. (Senarmont, A. ch. (3) 30. 138.) +6H 2 O. Sol. in acids. (Deville, A. ch. (3) 35. 446.) See also Carbonate, nickel, basic. Nickel potassium carbonate, NiCO 3 , K 2 CO 3 -f- 4H 2 0. Ppt. (Deville, A. ch. (3) 33. 96.) NiC0 3 ,KHC0 3 +4H 2 0. Decomp. by H 2 O, but may be washed by KHCO 3 +Aq without decomp. (Rose, Pogg. 84. 566.) Nickel sodium carbonate, NiC0 3 , Na 2 CO 8 + 10H 2 O. Ppt. (Deville.) Nickel carbonate hydroxylamine, 2Ni(OH) 2 , 4NiC0 3 , 5NH 2 OH+7H 2 O. Ppt. (Goldschmidt and Syngros, Z. anorg. 1894, 5. 143.) 2Ni(OH) 2 , 4NiCO 3 , 6NH 2 OH+6H 2 O. Ppt. (Goldschmidt and Syngros.) Palladious carbonate, PdCO 3 , 9PdO + 10H 2 O. Insol. in H 2 O; partly sol. in NH 4 OH+Aq; si. sol. in Na 2 CO 3 +Aq; sol. in acids. (Kane, 1842.) Potassium carbonate, K 2 CO 3 . Deliquescent. Very sol. in H 2 O with evolu- tion of heat. Sol. in 1.05 pts. H 2 O at 3; 0.962 pt. at 6; 0.900 pt. at 12.6; 0.747 pt. at 26; and 0.490 pt. at 70. (Osann.) Sol. in 0.92 pt. H 2 O. (M. R. and P.) Sol. in 0.922 pt. H 2 O at 15. (Gerlach.) Sol. in 1 pt. H 2 O. (Abl.) 100 pts. H 2 O at 15.5 dissolve 100 pts. K 2 CO 3 . (lire's Diet.) Solubility in 100 pt?. H 2 O at t. t Pts. K 2 C0 3 t 40 50 60 70 Pts. K 2 C0 3 t Pts. K 2 C0 3 10 20 30 83.12 88.72 94.06 100.09 106.20 112.90 119.24 127.10 80 90 100 135 134.25 143 18 153.66 205.11 (Poggiale, A. ch. (3) 8. 468.) CARBONATE, POTASSIUM Solubility in 100 pts. H 2 at t. Sp. gr. of K 2 CO 3 +Aq at 15 Continued. t 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 Pts. K 2 C0 3 t Pts. K 2 C0 3 t Pts. K 2 C0 3 % K 2 C0 3 Sp. gr. % K 2 C0 3 Sp. gr. 23.496 24.475 25.454 26.432 27.412 28.391 29 . 360 30.349 31.328 32.807 1.2836 1 . 2980 1 3078 1.3177 1 . 3277 1.3378 1 . 3480 1 . 3585 1 . 3692 1.3803 33.286 34 . 265 35 . 244 36 . 223 37 . 202 38.181 39.160 40.139 40 . 504 1.8915 1 . 4030 .4147 . 4265 .4384 .4504 . 4620 .4750 .4812 89.4 94 97 100 102 104 105 106 107 108 109 109 109 110 110 110 111 111 111 111 112 112 112 112 112 113 113 113 113 114 114 114 114 115 115 115 115 116 116 116 117 117 117 118 118 119 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 87 88 89 90 119 120 120 121 121 122 122 123 124 124 125 125 126 127 127 128 128 129 130 130 131 132 132 133 133 134 135 135 136 137 137 138 139 139 140 141 141 142 143 144 144 145 146 147 147 91 92 93 94 95 96 97 98 99 100 101 102 103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 119 120 121 122 123 124 125 126 127 128 129 130 131 132 133 134 135 148 149 150 151 151 152 153 154 155 156 157 158 159 160 161 162 163 164 166 167 168 169 171 172 173 175 176 178 179 181 182 184 185 187 188 190 191 193 195 196 198 200 201 203 205 Sp.gr (Tiinnerman.) . and boiling-point of K 2 COs+Aq. K 2 C0 3 Sp. gr. B.-pt. KzCOa Sp. gr. B.-pt. 4.7 9.0 13.2 16.8 20.5 24.0 27.3 30.5 33.6 36.2 39.0 41.7 1.06 1.11 1.15 1.19 1.22 1.25 1.28 1.31 1.34 1.38 1.41 1.44 100.56 100.56 101.11 101.11 101.66 102.22 102.78 103,33 104.44 105.56 107.22 108 . 33 43.3 45.8 48.8 52.1 56.0 60.4 65.5 71.8 79.2 88.4 100.0 1.46 1.50 1/54 1.58 1.63 1.70 1.80 1.95 2.15 2.40 2.60 109.44 111.11 112.78 114.44 116.11 117.78 119.44 122 22 125 . 5 K 2 CO 3 .12H 2 41.0 6.3 77.6 11.8 37.7 7.0 68.3 12.6 31.0 10.5 53.0 17.9 29.8 11.3 50.5 19.1 25.2 14.1 41.4 23.2 22.4 16.6 36.8 27.3 19.8 18.7 32.1 30.3 19.1 19.7 31.2 32.1 15.1 23.2 24.5 37.6 Na 2 CO 3 , K 2 CO 3 .12H 2 O 14.5 22.8 23.1 36.4 +Na 2 CO 3 .10H 2 O Na 2 CO 3 10H 2 O 10.8 22.7 16.2 34.0 10.7 22.4 16.0 33.5 4.7 21.9 6.4 29.8 22.71 29.37 (Osaka, J. Tok. Chem. Soc. 1911, 32. 870.) Solubility of K 2 CO 3 +Na 2 CO 3 in H 2 O at 24.2. In 1000 ccm. H 2 O Na 2 CO 3 K 2 COs 28.35 354.2 369.7 363.0 330.8 273.8 187.2 130.0 137 9 112.3 95.2 25.5 150.03 226.6 243.5 282.7 344.9 483.9 921 5 982 6 1074.0 1085.1 1108.6 1125.7 Solid phase Na 2 CO 3 Na 2 CO 3 , K 2 CO 3 .6H 2 O Na 2 C0 3 , K 2 C0 3 .6H 2 + Na 2 CO 3 d K 2 C0 3 (Kremann and Zitek, M. 1909, 30. 317.) Solubility of K 2 CO 3 +Na 2 CO 3 in H 2 O at 10 C In 1000 ccm. H 2 O Na 2 C0 3 K 2 C0 3 119.8 176.4 108. 61.19 354.1 500.1 0052.9 1084.0 Solid phase Na 2 C0 3 Na 2 CO 3 , K 2 CO 3 K 2 CO S (Kremann and Zitek, M. 1909, 30. 324.) Solubility of K 2 CO 3 +KNO 8 in H 2 O at 25.2 C 1 1. of the solution contains Mol. K 2 C0 3 Mol. KNOa 0.00 0.59 1.35 2.10 2.70 3.58 3.217 2.62 1.97 1.46 1.14 0.79 (Touren, C. R. 1900, 131. 259.) Solubility of K 2 CO 3 +KNO 3 in H 2 O at 10. In 1000 ccm. H 2 O Solid phrase , KNOa K 2 C0 3 208.9 26.62 1076 !o 1084.0 KNO 3 KN0 3 , K 2 C0 8 K 2 C0 3 (Kremann and Zitek, M. 1909, 30. 325.) CARBONATE, POTASSIUM 201 Solubility of K 2 CO 3 +KNO 3 in H 2 O at 24.2 In 1000 ccm. H 2 O KNOa 376.85 285.00 161.67 141.80 73.04 38.78 31.11 K 2 C0 3 130.3 348.4 371.9 688.1 878.3 1112.2 Solid phase KNO ? KN0 3 , K 2 C0 3 (Kremann and Zitek, M. 1909, 30. 316.) Solubility of K 2 CO 3 +KC1 in H 2 O at 30. KoCOs ft Solid phase 53.27 52.22 51.66 1.03 1.07 K 2 C0 3 .l^H 2 b+KCl KC1 1.64 26*22 28.01 KC1 u * Author gives intermediary data, (de Waal, Dissert. 1910.) Solubility of K 2 CO 3 +KQH in H 2 O at 20. % KOH % K 2 C0 3 Solid phase 55.75 55.14 53.77 * 2.05 2.50 53*27 KOH.2H 2 O KOH.2H 2 O+K 2 CO 3 .13/6H 2 O K 2 C0 3 .1^H 2 * Author gives intermediary data, (de Waal, Dissert. 1910.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20, 828.) Sol. in 9 pts. alcohol of 17 B. Insol. in absolute alcohol. Not decomp. by 1 pt. H 2 SO 4 +6 pts. ab- solute alcohol. Not decomp. by 1 pt. HNO 3 + 6 pts. absolute alcohol. Not decomp. by an alcoholic solution of HC1, oxalic, racemic, tar- taric, or glacial acetic acids, but is decomp. by alcoholic solution of citric acid. Solubility in methyl alcohol. Composition of liquids in equilibrium with solid K 2 CO 3 att. t -30 -20 -20 +17 35 Upper layer Lower layer 8 M K C te o k? Q a ss $ g o Q W * 21.7 13.8 12.4 7.6 7.4 6.2 5.0 42.2 52.1 36.1 34.1 44.2 46.3 46.6 48.3 8.2 6.7 6.6 5.7 4.3 47.6 47 46.8 46 44.7 66.3 26.1 69.6 72. P 24.2 22.1 (de Bruyn, Z. phys. Ch. 1900, 32. 63 and ff.) Solubility in ethyl alcohol. Composition of liquids in equilibrium with solid K 2 CO 3 at t. t Upper layer Lower layer 8 &s w c B d SS g t K 6 tf? o 5$ -18 +17 35 50 75 0.03 0.04 0.06 0.07 0.09 0.12 90.3 91.9 91.5 90.9 91.8 91.4 9.7 8.1 8.4 9 8.1 8.5 51.2 51.3 52.1 53 4 55.3 57.9 0.2 0.2 0.2 0.2 0.2 2.0 48.6 48.5 47.7 46.4 44.5 40.9 (de Bruyn.) Solubility in ethyl alcohol +Aq at 25. When K 2 CO 3 is dissolved in ethyl alcohol + Aq two layers are formed, the compositions of which are as follows: Upper layer ale 81.25 71.67 56.98 53.92 50.21 43.93 37.64 28.43 H 2 O K 2 CO 3 18.61 27.91 41.55 44.13 47.24 52.04 56.45 61.57 0.14 0.42 1.47 2.05 2.55 3.92 5.90 10.00 Lower layer % % 70 alcohol H 2 K 2 C0.3 0.82 1.79 4.02 4.88 5.54 7.71 10.54 15.73 42 61 73 87 06 56 40 38 43.76 36.60 30.25 28.25 27.41 24.74 22.06 17.90 (Cuno, W. Ann. 1909, (4) 28. 664.) Solubility of K 2 CO 3 in alcohol +Aq at 30 C 53.27 53.09 0.13 0.04 Alcohol 0.1 90.49 99.92 46.73 46.81 9.38 0.04 Solid phase K 2 C0 3 .1^H 2 K 2 C0 3 K 2 CO,+K 2 CO 3 . * Solution separates into two layers, (de Waal, Dissert. Leiden, 1910.) A full discussion ot the solubility of K 2 CO S in methyl, ethyl, propyl, isopropyl, and allyl alcohols is given by Frankforter and Frary (J. phys. Ch. 1913, 17. 402), and Frankforter and Temple (J. Am. Chem. Soc. 1915, 37. 2697). 202 CARBONATE, POTASSIUM HYDROGEN K 2 CO 3 will "salt out" acetone from aqueous solution. The table shows the composi- tion of the solutions at the points at which inhomogeneous solutions of K 2 CO 3 , acetone and H 2 O just become homoge- neous at 20. 100 g. of the solution con- tain: K 2 C0 3 H*b g. acetone K 2 C0 3 H g ; g. acetone 18.84 73.22 7.94 2.43 55.36 42.21 13.32 71.38 15.30 22.29 72.81 4.90 11.83 70.34 17.83 17.86 73.12 9.02 10.13 69.03 20.84 15.81 72.53 11.66 8.24 67.31 24.45 14.39 71.89 13.72 7.22 65.99 26.79 10.29 69.46 20.25 6.04 64.39 29.57 1.91 54.05 44.04 28.87 69.08 2 05 1.76 52.86 45.38 23.94 71.98 4 08 1.60 51.60 46.80 21.52 72.75 5.33 1.29 49.57 49.14 19.60 73.10 7.70 1.08 47.86 51.06 6.46 65.34 28.20 0.94 46.73 52.33 5.91 64.65 29.44 0.75 44.72 54.53 5.60 63.93 30.47 0.66 43.31 56.03 5.04 62.80 32.16 0.60 42.49 56.91 4.50 61.48 34.02 0.54 41.73 57.73 3.80 59.79 36.41 0.50 40.69 58.81 3.18 57.95 38.87 0.46 40.48 60.06 2.73 56.50 40.77 (Frankforter and Cohen, J. Am. Chem. Soc. 1914, 36. 1121.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 34. 314.) . Sol. in phenol. Sol. in 13.5 pts. glycerine of 1.225 sp. gr. (Vogel,N.Repert. 16.557.) 100 g. sat. K 2 CO 3 + sugar +Aq contains 22.44 g. K 2 CO 3 and 56 g. sugar at 31.25 (Kohler, Z. Ver. Zuckerind. 1897, 47. 447.) Very deliquescent. (Pohl.) Deliquescent only in very moist air. (Stadeler.) Sol. in H 2 O with evolution of heat. (Pohl.) Sol. at 17.6 with absorption of heat, at 32 with evolution of heat, and at 25 with neither absorption nor evolution of heat. (Berthelot, C. R. 78. 1722.) Sat. solution of K 2 C0 3 +1^H 2 O in H 2 O contains 53.27 g. anhydrous K 2 CO 3 in 100 g. solution at 30. (de Waal, Dissert. 1910.) +2H 2 O. Salt usually given as containing 1^H 2 O contains 2H 2 0. (Gerlach, Z. anal. 26. 460.) Sat. solution of K 2 CO 3 +2H 2 O contains 112 g. anhydrous K 2 COi in 100 g. H 2 O at 25. (Osaka, J. Tok. Ch. Soc. 1911, 32/870.) -f 4H 2 O. Not deliquescent in closed vessels. (Gerlach, I. c.) Potassium hydrogen carbonate, KHCO 3 . Not deliquescent. Sol. in 3.5 pts. H 2 O at 15. (Redwood.) Sol. in 4 pts. H 2 O at moderate temperatures. (Bergmann.) Sol. in 0.8333 pt. boiling H 2 O (Pelletier) ; in 4 pts. cold, and 1.2 pts. boiling H 2 O (M. R. and P.'s Pharm.). Sol. in 4 pts. H 2 O at 18.75. (Abl.) 100 pts. H 2 O at 15.5 dissolve 30 pts. and at 100, 83 pts. (Ure's Diet.) 100 pts. H 2 O at 10-11.2 dissolve 26.1 pts. KHCOs, and the sp. gr. of solution is 1.1536. (Anthon, Dingl. 161. 216.) 100 pts. H 2 O dissolve at 10 20 30 19.61 23.23 26.91 30.57 pts. KHCO,, 40 50 60 70 34.15 37.92 41.35 45.24 pts. KHCO 3 . (Poggiale, A. ch. (3) 8. 468.) 100 pts. H 2 O dissolve pts. KHCO 3 at t. t Pts. KHCOs t Pts. KHCOs 20 22.4 33.2 40 60 45.2 46.4 (Dibbits, J. pr. (2) 10. 417.) Sp. gr. of KHCO 3 +Aq at 15 containing 5% KHCO 3 = 1.0328; containing 10% KHCO 3 = 1.0674. (Kohlrausch, Z. anal. 28. 472.) Sol. in 12CO pts. boiling alcohol. (Berthol- let.) Insol. in alcohol. (Dumas.) 100 pts. H 2 O dissolve 19.3 pts. KHCO 3 and 8.3 pts. NaHC0 3 if the sat. solution of latter is sat. with former; and 26.1 pts. KHCO 3 and 6.0 pts. NaHCO 3 , if the sat. solution of the former is sat. with the latter, all at 10. (Mulder, J. B. 1866. 67.) Insol. in sat. K 2 CO 3 +Aq. (Engel, C. R. 102. 365.) Solubility of KHCO 3 +KNO 3 in H 2 O in an atmosphere of CO 2 . 1 litre of the solution contains at 14.5 at 25.2 Mol. KHCOs Mol. KNC) 3 Mol. KHCOt Mol. KNOs 0.00 2.33 0.00 3.28 0.39 2.17 0.89 2.84 0.76 2.03 1.33 2.65 1.16 1.92 1.91 2.45 1.55 1.81 This case is complicated by the fact that KN0 3 is more sol. in H 2 O sat. with CO 2 than in pure H 2 O. (Touren, C. R. 1900, 131. 261.) Insol. in benzonitrile (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); "ethyl acetate (Naumann, B. 1Q10, 43. 314.) Potassium praseodymium carbonate, K 2 CO 3 , Pr 2 (CO 3 ) 3 -}-12H 2 O. Ppt. Sol. in 30% K 2 CO 3 +Aq. (Meyer, Z. anorg. 1904, 41. 104.) CARBONATE, SODIUM 203 Potassium samarium carbonate, K 2 CO 3 , Sm 2 (CO 8 ) 3 + 12H 2 O. (Cleve.) Potassium silver carbonate, KAgCO 3 . Decomp. by H 2 O. (de Schulten, C. R. 105. 811.) Ppt. Decomp. by H 2 O. (Reynolds, Chem. Soc. 1898, 73. 265.) Potassium sodium carbonate, KNaCO 3 + 6H 2 O. Slightly efflorescent. Sol. in 0.75 pt. H 2 O at 12.5; in 0.54 pt. H 2 O at 15. Sat. solution at 15 has sp. gr. = 1.366. (Stolba, J. pr. 94. 406.) Decomp. by recrystallizing from H 2 O, but crystallizes undecomposed from sat. K 2 CO 3 + Aq. Sol. in H 2 O. (Osaka, C. A. 1911. 2601.) See K 2 CO 3 +Na 2 CO 3 under Na 2 CO 3 . +3H 2 O. (Kremann and Zitek, M. 1909. 30. 317.) Does not exist. (Osaka.) K 2 CO 3 , 2Na 2 CO 3 + 18H 2 O. SI. efflorescent. Very sol. in H 2 O. (Marignac.) Potassium stannous carbonate, K 2 CO 3 , 2SnCO 3 +2H 2 O. Decomp. by H 2 O. (DeviUe.) Potassium uranyl carbonate, 2K 2 CO : , (UO 2 )CO 3 . Sol. without decomp. in 13.5 pts. H 2 O at 15, and in somewhat less warm H 2 O. Sol. in boiling H 2 O with decomp. More sol. in K 2 CO 3 , or KHCOc+Aq than in H 2 O. (Rose.) Insol. in alcohol. (Ebelmen, A. ch. (3) 5. 189.) Potassium zinc carbonate, 4K 2 O, 6ZnO, 11CO 2 +8H 2 O. Can be washed with cold H 2 O without decomp. (Deville, A. ch. (3) 33. 99.) Praseodymium carbonate, Pr 2 (COc) 3 +8H 2 O. Sol. in H 2 O. (von Schule, Z. anorg. 1898, 18. 362.) Praseodymium sodium carbonate, 2Pr 2 (CO 3 ) 3 , 3Na 2 CO 3 +22H 2 O(?). Ppt. Easily decomp. (Meyer, Z. anorg. 1904, 41. 105.) Radium carbonate. Less sol. in H 2 O than corresponding Ba comp. (Curie, Dissert. 1903.) Rubidium carbonate, Rb 2 CO 3 . Very deliquescent, and sol. in H?O. 100 pts. absolute alcohol dissolve 0.74 pt. Rb 2 CO 3 . (Bunsen.) Rubidium hydrogen carbonate, RbHCO 3 . Not deliquescent. Easily sol. in H 2 O. (Bunsen.) Samarium carbonate, Sm 2 (CO 2 ) 3 +3H 2 O. Insol. in H 2 O. (Cleve, Bull. Soc. (2) 43. 168.) Samarium sodium carbonate, Sm 2 (CO 3 ) 3 , Na 2 CO 3 +16H 2 O. Ppt. (Cleve.) Scandium carbonate, Sc 2 (CO 3 ) 3 + 12H 2 O. (Crookes, Roy. Soc. Proc. 1908, 80, A. 518.) Scandium sodium carbonate, Sc 2 (C0 3 ) 8 , 4Na 2 CO 3 +6H 2 O. Difficultly sol. in H 2 O. Sol. in cold, less sol. in hot alkali carbonates +Aq. (R. Meyer, Z. anorg. 1910, 67. 410.) Silver carbonate, Ag 2 CO 3 . Somewhat sol. in H 2 O. Sol. in 31,978 pts. H 2 O at 15. (Kremers, Pogg. 85. 248.) 1 g. Ag 2 C0 3 dissolves in 2 1. boiling H 2 O. (Joulin, A. ch. (4) 30. 260.) Solubility in H 2 O at 25 = 1.16 x 10- 1 mol.ll. (Spencer and Le Pla, Z. anorg. 1910, 65. 14.) 1 1. H 2 O at 25 dissolves 1.2 x 10- 4 gram atoms of silver. (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) Insol. in H 2 CO 3 +Aq. (Bergman.) Sol. in 961 pts. H 2 CO 3 +Aq. (Lassaigne.) 1 1. sat. H 2 CO 3 +Aq dissolves 846 g. Ag 2 CO 3 at 15. (Johnson, C. N. 54. 75.) Sol. in (NH 4 ) 2 CO 3 +Aq or NH 4 OH+Aq; si. sol. in K 2 CO 3 +Aq. (Wittstein.) Easily sol. in Na 2 S 2 O 3 +Aq. (Herschel, 1819.) Sol. in hot NH 4 Cl+Aq, and si. sol. in NH 4 NO 3 + Aq. (Brett, 1837.) Not pptd. in presence of Na citrate. (Spiller.) Decomp. by HC1+ Aq, and chlorides+Aq. Somewhat sol. in cone. NaNO 3 +Aq. (de Coninck, Belg. Acad. Bull. 1909, 333.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Silver carbonate ammonia. Easily sol. in H 2 O. Sol. in NH 4 OH+Aq, from which it is precipitated by absolute al- cohol. (Berzelius.) Ag 2 CO 3 , 4NH 3 . Ppt. Insol. in alcohol. (Keen, C. N. 31. 231.) Sodium carbonate, Na 2 CO 3 . Anhydrous. Sol. in H 2 O with evolution of heat. Sol in 5.967 pts. HzO at 15. (Fresenius.) 100 pts. H 2 O at 14.6 dissolve 7.74 pts. Na^CCs, or 20.64 pis. NasCOs lOHzO is sol. in rather loss than 1 pt. boiling HzO (Thomson, 1831.) Sol. in 2 pts. H 2 O. (Bergman. > Sol in 2 pts. H 2 at 18.75. (A hi.) 204 CARBONATE, SODIUM Solubility in 100 pts. H 2 O at t. t Pts. Na 2 C0 3 Pts. NazCOs + 10H 2 O t Pts. NazCOs Pts. NajCOs + 10H 2 10 20 7.08 16.66 30 83 21.52 61.98 123.12 25 30 104.6 35.90 35.90 48.50 171.33 241.57 420.68 (Poggiale, A. ch. (3) 8. 468.) Possesses four different degrees of solubil- ity, according to different states of molecular constitution and degrees ot hydration. (Lowel. A. ch. (3) 44. 330.) Little more sol. at 34-38 than at 104, but maximum of solubility is probably at 15. (Lowel.) Solubility of , Na 2 CO 3 +10H 2 O, Na 2 CO 3 +7H 2 O (a), and Na 2 C0 3 +7H 2 O (6) in H 2 O. t Sat. solution of NazCO.rflOHaO contains Sat. solution of NazCO 3 +7H 2 O (6) contains Sat. solution of Na 2 COs+7H 2 (a) contains Pts. NazCOs in lOOpts. H 2 Pts. Na 2 CO 3 + 10H 2 O in lOOpls. HzO Pts. NazCOa in 100 pts. H 2 O Pts. Na 2 CO 3 + 7H 2 (6) in 100 pts. H 2 O Pts. Na 2 C0 3 + 10H 2 O in 100 pts. H 2 O Pts. Na 2 COa in 100 pts. HzO Pis. Na 2 COs + 7H 2 O (a) in lOOpls. HzO Pts. Na 2 COs + 10H 2 O in 100 pts. H 2 O 10 15 20 25 30 38 104 6.97 12.06 16.20 21.71 28.50 37.24 51.67 45.47 21.33 40.94 63.20 92.82 149.13 273.64 1142.17 539.63 20.39 26.33 29.58 38.55 38.07 43.45 58.93 83.94 100.00 122.25 152.36 196.93 84.28 128.57 160.51 210.58 290.91 447.93 31.93 37.85 41.55 45.79 112.94 150.77 179.90 220.20 188.37 286.13 381.29 556.71 (Lowel, A. ch. (3) 33. 382.) 100 pts. H 2 O at 14 dissolve 60.4 pts. Na 2 CO 3 + 10H 2 O; at 36, 833 pts.; at 104, 445 pts. Solubility increases to 36, then diminishes. (Payen, A. ch. (3) 43. 233.) There are apparently two maxima of solu- bility; the one occurring at 15, or even lower, as warm solutions cool; the other at 34-38, when cold solutions are warmed. (Payen. A. ch. (3) 44. 330.) Solubility in ICO pts. H 2 O at t. Pts. Pts. Pts. t Na 2 COs t NazCOs t NazC0 3 7.1 22 23.8 43 46.2 1 7.5 23 25.1 44 46.2 2 7.8 24 26.5 45 46.2 3 8.4 25 28.0 46 46.2 4 8.9 26 29.7 47 46.2 5 9.5 27 31.6 48 46.2 6 10.0 28 33.6 49 46.2 7 10.6 29 35.8 50 46.2 8 11.2 30 38.1 51 46.2 9 11.9 31 41.4 52 46.2 10 12.6 32 46.2 53 46.2 11 13.3 32.5 59.0 54 46.2 12 14.0 33 46.2 55 46.2 13 14.8 34 46.2 56 46.2 14 15.6 35 46.2 57 46.2 15 16.5 36 46.2 58 46.2 16 17-. 4 37 46.2 59 46.2 17 18.3 38 46.2 60 46.2 18 19.3 39 46.2 61 46.2 19 20.3 40 46.2 62 46.2 20 21.4 41 46.2 63 46.2 21 22.6 42 46.2 64 46.2 Solubility in 100 pts. H 2 O at t Continued t Pts. Na 2 C0 3 t Pts. NazCOs t Pts. Na 2 CO 3 65 46.2 79 46.2 93 45.6 66 46.2 80 46.1 94 45.6 67 r 46.2 81 46.1 95 45.6 68 46.2 82 46.1 96 45.6 69 46.2 83 46.0 97 45.5 70 46.2 84 46.0 98 45.5 71 46.2 85 45.9 99 45.5 72 46.2 86 45.9 100 45.4 73 46.2 87 45.8 101 45.4 74 46.2 88 45.8 102 45.3 75 46.2 89 45.8 103 45.3 76 46 2 90 45.7- 104 45.2 77 46.2 91 45.7 105 45.1 78 46.2 92 45.7 ... (Mulder, Scheik. Verhandel. 1864. 129.) Liable to form supersaturated solutions. Supersat. Na 2 CO 3 +Aq (2 pts. Na 2 CO 3 , 10H 2 O: 1 pt. H 2 0) may be kept in a flask closed with cotton wool. (Schroder.) When supersat. Na 2 CO 3 +Aq is exposed to low temperatures; the 10H 2 salt crystallizes out; but under other circumstances two other salts are formed, each containing 7H 2 O; one is four times as sol. at 10 as the 10H 2 O salt, and the other twice as sol. See above. (Lowel, A. ch. (3) 33. 337.) See also Na 2 CO 3 +H 2 O, 7H 2 O, and 10H 2 O. CARBONATE, SODIUM 205 Sp. gr. of Na 2 CO 3 +Aq at 15. Sp. gr. of Na 2 CO 3 +Aq at 17.5 C . % Na 2 CO 3 Sp. gr. % Na 2 CO 3 Sp. gr. Na 2 C0 3 Na 2 C0 3 +10H 2 C Sp. gr. Na 2 CO 3 +10H 2 C > Sp. gr. 0.372 0.744 1.116 1.488 1.850 2.232 2.504 2.976 3.348 3.720 4.090 4.464 4.836 5 . 208 5.580 5 . 972 6.324 6.396 6.768 7 . 440 1 . 0040 1.0081 1.0121 1.0163 1 . 0204 f.0245 1.0286 1 . 0327 1.0368 1.0410 1.0452 1 . 0494 1.0537 1 . 0576 1.0625 1 . 0669 1.0713 1 . 0757 1.0802 1 . 0847 7.812 8 . 184 8.556 8.928 9.300 9.672 10.044 10.416 10.788 11.160 11.532 11.904 12.276 12.648 13.020 13.392 13.764 14.136 14 . 508 14 . 880 1.0892 1.0937 1.0982 1 . 1028 1 . 1074 1.1120 1.1167 1.1214 1.1261 1 . 1308 1 . 1356 1 . 1404 1 . 1452 1.1500 1-.1549 1 . 1598 1 . 1648 1 . 1698 1.1748 1.1816 1 2 3 4 5 6 7 8 2.70 5.40 8.10 10.18 13.50 16.20 18.90 21.60 .010 .020 .031 .041 .052 .063 .073 1.084 9 10 11 12 13 14 15 24.30 27.00 29.70 32.40 35.10 37.80 40.50 1.095 1.105 1.116 1.127 1.137 1.148 1.157 (Hager.) Sp. gr. of Na 2 CO 3 +Aq increases or di- minishes by a change of temperature of 1 by the following amounts (Tiinnerman.) Sp. gr. of Na 2 C0 3 +Aq at 15. Corr. % Na 2 C0 3 0.0004 0.00033 0.00026 13-15 8-12 3-7 % Sp. gr. if % is Na 2 C0 3 Sp. gr. if % is Na 2 CO 3 +10H 2 O (Hager, Comm. 1883.) Sp. gr. of cone. Na 2 CO 3 +Aq at 30. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 1.0105 .0210 .0315 .0420 .0525 .0631 .0737 .0843 .0950 .1057 .1165 .1274 .1384 .1495 1.004 1.008 1.012 1.016 1.020 1.023 1.027 ' .031 .035 .039 .043 .047 .050 .054 .058 .062 .066 .070 .074 .078 .082 1.086 1.090 1.094 1.099 1.103 1.106 1.110 1.114 1.119 1.123 1.126 1.130 1.135 1.139 1.143 1.147 1.150 Sp. gr. NauCOc Na 2 C0 3 in 1 1. Sp. gr. 1.220 1.210 1.200 .190 .180 .170 .160 .150 .140 Na 2 COs NafcO.3 in 1 1. 1.310 1.300 1.290 1.280 1.270 1.260 1.250 1.240 1.230 28.13 27.30 26.46 25.62 24.78 23.93 23.08 22.21 21.33 368.5 354.9 341.3 327.9 314.7 301.5 288.5 275.4 262.3 20.47 19.61 18.76 17.90 17.04 16.18 15.32 14.47 13.62 249.7 237.3 225.1 214.0 201.1 18913 177.7 166.4 155.3 (Lunge, Chem. Ind. 1882. 320.) Sp. gr. of Na 2 CO 3 +Aq at 23. ii Na 2 COs Sp. gr. 3 NajCOa Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 0.370 0.741 1.112 1.482 1.853 2.223 2.594 2.965 3.335 3.706 4.076 4.447 4.817 5.188 5.558 1.0038 1.0076 1.0114 1.0153 1.0192 1.0231 1.0271 1.0309 1.0348 1.0388 1.0428 1.0468 1.0508 1.0548 1.0588 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 5.929 6.299 6.670 7.04-1 7.412 7.782 8.153 8.523 8.894 9.264 9.635 10.005 10.376 10.746 11.118 .0628 .0668 .0708 .0748 .0789 .0836 .0871 .0912 .0953 1.0994 1.1035 1.1076 1.1117 1.1158 1.1200 CGftrlao.h. Z. anal. 8. 279 .) 206 CARBONATE, SODIUM Sp. gr. of NA 2 CO 3 +Aq at 23^-Continued. 31 32 33 34 35 36 37 38 39 40 Na 2 C0 3 11.488 11.859 12.230 12.60C 12.971 13.341 13.712 14.082 14.530 14.824 Sp. gr. 1.1242 1.1284 1 . 1326 1.1368 1.1410 1.1452 1 . 1494 1 . 1536 1.1578 1.1620 03O S? 41 42 43 44 45 46 47 48 49 50 NazCOa 15.195 15.556 15.936 16.307 16.677 17.048 17.418 17.789 18.159 18.530 Sp. gr. 1.1662 1704 1746 1.1788 1830 1873 1916 1959 2002 2045 (Schiff, A. 113. 186.) Sp. gr. of Na 2 CO 3 +Aq at 23.3. o = number of grms. X Yz mol. wt., dissolved in 1000 grms. H 2 0; 6 = sp. gr. if a = Na 2 CO 3 , 10H 2 O (Y 2 mol. wt. = 143); c=sp. gr. if o = Na 2 CO 3 (% mol. wt.=53). 1.048 1.086 1.117 1.142 1.052 1.100 1.145 1.187 1.163 1.182 1.198 1.226 (Favre and Valson, C. R. 79. 968). Sp. gr. of Na 2 CO 3 +Aq at 18. % N 7 a 2 CO3 Sp.gr. % NazCOs Sp. gr. 5 10 1.0511 1.1044 15 1.1590 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of Na 2 CO 3 +Aq g.-equivalents Na 2 C0 3 per 1. t Sp. gr. t/t. 0.002524 16.004 1.0001418 0.005041 16.026 .0002844 0.01006 16.049 .000568 0.02501 16.028 .001413 0.04954 16.050 .002789 0.10188 16.030 .005699 0.24646 16.041 .013598 0.002628 16.051 .0001473 0.003948 16.088 .0002216 0.009182 16.081 .0005181 0.01830 16.089 1.001033 0.10842 16.042 1.006048 0.21570 16.055 1.011910 0.4297 15.14 1.02346 2.5015 16.05 1.12533 (Kohlrausch, W. Ann. 1894, 53. 26.) Sp. gr. of Na 2 CO 3 +Aq at t. H 2 O at 4 60 C 80 C % Na 2 C0 3 28.74 25.20 22.25 18.23 14.06 28.59 18.26 Sp. gr. 2971 2546 2191 1746 1 . 1277 1.2807 1.1607 (Wegscheider, M. 1905, 26. 690.) Sp. gr. of dil Na 2 CO 3 +Aq at 20.004. Conc.=g. equiv. Na 2 CO 3 per 1. at 20.004 and 730 mm. Sp. gr. compared, with H 2 O at 20.004 = !. Cone. Sp. gr. o.ooco 1.000,000,0 0.0001 1.000,005,6 0.0002 1.000,011,2 0.0004 1.000,022,5 0.0005 1.000,C28,1 0.0010 1.000,056,3 0.0020 1.000,112,7 0.0040 1.000,225,8 0.0050 1.000,282,4 0.0100 1.000,564,8 (Lamb and Lee, J. Am. Chem. Soc, 1913, 35. 1685.) Na 2 CO 3 +Aq containing 5% Na 2 CO 3 boils at 100.5; 10% Na 2 CO 3 , at 101.1: 15% Na 2 CO 3 , at 101.8. (Gerlach.) Sat. solution boils at 104.4 (Griffiths, 1825); 106 (Kremers); 104. (Payen.) Sat. solution forms a crust at 104.1, and contains 42.2 pts. Na 2 CO 3 to 100 pts. H 2 O; highest temperature observed, 105. (Ger- lach, Z. anal. 26. 427.) B.-pt. of Na 2 CO 3 +Aq containing pts. Na 2 CO 3 to 100 pts. H 2 O. G = according to Ger- lach (Z. anal. 26. 458); L = according to Legrand (A. ch. (2) 59. 426). B.-pt. 100.5 101.0 101.5 102.0 102.5 103.0 5.2 10.4 15.6 20.8 26.0 31.1 7.5 14.4 20.8 26.7 32.0 36.8 B.-pt. 103.5 104.0 104.5 104.63 105.0 36.2 41.2 46.2 51.2 Less sol. in dil. NH 4 OH+Aq than in H 2 O. (Fresenius.) See also under Ammonia. Solubility of Na 2 CO 3 +NH 4 Cl. See under Ammonium Chloride. Solubility of Na 2 CO 3 +K 2 CO 3 . See under Carbonate, potassium. CARBONATE, SODIUM 207 The reciprocal solubility of sodium car- bonate and sodium hydrogen carbonate in H 2 O has been determined, (de Paepe, C. A. 1911, 2603, and 1912, 2723.) Solubility of Na 2 CO 3 +NaHCO 3 in H 2 O at 25. Solubility of Na 2 CO 3 +NaBr in H 2 O at 30. % Na 2 CO3 % NaBr Solid phase 27.98 27.54 26.72 26.23 23.40 22.68 19.86 19.57 18.11 8.45 6.90 3.04 2.99 2.60 2.41 4.06 6.26 11.00 12.22 16.88 16.95 19.32 33.39 36.13 44.75 45.31 45.68 49.40 Na 2 CO 3 .10H 2 O Na 2 C0 3 . 1 OH 2 +Na 2 CO 3 .7H 2 O Na 2 CO 3 .7H 2 O Na 2 C0 3 .7H 2 O +Na 2 CO 3 .H 2 O Na 2 CO 3 .H 2 NaBr.2H2O+Na 2 CO 3 .H 2 O NaBr.2H 2 O g. per 100 g. H2O Solid phase NaHCOs Na 2 CO 3 2.1 4.2 5.7 7.3 9.0 10.1 28.3 27.3 26.5 19.2 12.4 6.2 1.0 Na 2 CO 3 .10H 2 O Na 2 C0 3 .10H 2 O+NaHCO 3 NaHCO 3 a (i K (de Paepe, Bull. Soc. Chim. Belg. 1911, 25. 174.) Solubility of Na 2 CO 3 +NaHCO 3 in H 2 O at 25. g. per 1. XaHC0 3 Na 2 C0 3 98.7 50.8 27.6 0.0 0.0 216.6 276.3 276.4 Solid phase >.* NaHCOa NaHC0 3 +Na 2 CO 3 ,NaHCO 3 .2H 2 Na 2 CO 3 ,NaHC03.2H 2 O +NaCO. 10H 2 O Na 2 CO 3 .10H 2 O (McCoy and Test, J. Am. Chem. Soc. 1911 33. 474.) Equilibrium between Na 2 CO 3 , NaHCO and CO 2 . hydrogen. See under Carbonate, sodium Solubility of NaNO 3 in Na 2 CO 3 +Aq at 10 In 1000 ccm. H 2 O NaNOa 805.0 704.8 Na 2 C0 3 87.5 119.8 Solid phase NaNO 3 NaN0 3 , Na 2 CO 3 Na 2 CO 3 (Kremann, M. 1909, 30. 325.) Solubility of NaNO 3 in Na 2 CO 3 +Aq at 24.2' In 1000 ccm. H 2 O NaNO 3 913.58 844.50 627.75 544.3 459.6 Na 2 C0 3 59.61 217.85 246.30 263.30 28.55 Solid phase NaN0 3 K NaNO 3 +Na 2 CO 3 .7H 2 O Na 2 CO 3 .7H 2 O Na 2 CO 3 .10H 2 O Na 2 CO 3 .10H 2 O (Kremann.) (Cocheret, Dissert. 1911.) Solubility in NaCl+Aq. 100 pts. H 2 O dis- solve pts. NaCl and pts. Na 2 CO + 10H 2 O, when that salt is in excess at 15. Pts. NaCl 0.00 4.03 8.02 12.02 16.05 19.82 Pts. Na 2 CO 3 +10H 2 61.42 53.86 48.00 43.78 40.96 39.46 Pts. NaCl 23.70 27.93 31.65 35.46 sat. 37.27 Pts. Na 2 C0 3 +10H 2 O 39.06 39. 73 41.44 43.77 45.32 Solubility of anhydrous Na 2 CO 3 in 100 pts. NaCl+Aq containing % NaCl at 15. % NaCl 1 2 3 4 5 6 7 8 9 10 11 Pts. Na 2 C0 3 16.408 15.717 15.060 14.438 13.851 13.299 12.783 12.305 11.864 11.461 11.097 10.773 % NaCl 12 13 14 15 16 17 18 19 20 21 22 Pts. Na 2 CO 3 10.488 10.244 10.041 9.880 9.762 9.686 9.655 9.667 9.725 9.828 9.997 (Reich, W. A. B. 99, 2b. 433.) Solubility of Na 2 CO 3 -f NaCl in H 2 O at 30. Na 2 CO; 27.98 27.48 27.12 26.82 25.59 24.26 % NaCl 0.9 3.33 4.15 5.17 5.93 Solid phase Na 2 CO 3 .10H 2 Na 2 C0 3 . 10H 2 +Na 2 C0 3 .7H 2 O Na 2 C03.7H 2 208 CARBONATE, SODIUM Solubility of Na 2 CO 3 +NaCl in H 2 O at 30 Continued. Solubility of Na 2 CO 3 in alcohol +H 2 O at 30. %Na 2 CO 3 % alcohol Solid phase Na 2 CO 3 NaCl Solid phase 27.4 26.61 2.64 (26.14* 3.411* 1.38 44.81] 0.62 52.99 0.61 53.26 0.53 55.70 0.51 56.56 0.47 62.61 0.40 63.20 0.15 72.80 0.11 73.06 0.07 78.19 0.07 82.26 0.06 86.76 0.06 90.95 0.04 93.09 0.03 95.06 95.65 ... 98.46 Na 2 COs.lOH 2 O Na 2 CO 3 .10H 2 O +Na 2 C.O 3 .7H 2 O Na 2 C0 3 .7H 2 Na 2 CO 3 .7H 2 O +Na 2 CO 3 .H 2 O Na 2 COs.H 2 O Na 2 C0 3 .H 2 +Na 2 C0 3 Na 2 CO 3 22.75 20.72 18.00 14.81 9.71 5.05 10.24 11.49 14.12 16.26 18.76 21.94 26.47 Na 2 CO.7H 2 O +Na 2 C0 3 .H 2 O Na 2 COs.H 2 NaCl+Na 2 COs.H 2 O NaCl (Cocheret, Dissert. 1911.) Solubility of Na 2 C0 3 +NaI in H 2 O at 30. * a 2 CO 3 /al. Solid phase 27.4 26.5 25.5 25.2 24.4 24.3 23.0 20.8 20.0 18.7 15.3 13.1 10.4 6.4 4.2 3.1 2.7 1.5 0.9 0.6 0.3 0.0 2.4 4.7 5.2 8.6 9.5 11.2 14.0 15.7 18.4 25.4 29.1 33.3 40.4 46.0 49.5 51.0 54.6 57.6 61.2 65.6 65.5 Na 2 CO 3 .10H 2 O +Na 2 CO 3 .7H 2 O Na 2 C0 3 .7H 2 Na 2 .CO 3 .7H 2 O-i Na 2 CO 3 .H 2 O Na;CO 3 .H 2 O NaI.2H 2 +Na 2 C0 3 .H:0 NaI.2H>0 * Conjugated liquid phases. (Cocheret, Dissert. 1911.) See also under Na 2 CO 8 +H 2 O, +7H 2 O and +10H 2 O. Not decomp. by 1 pt. H 2 SO 4 +6 pts. ab- solute alcohol. Not decomp. by alcoholic solutions of race- mi^, tartaric, or glacial acetic acids; slowly decomp. by HNO 3 +absolute alcohol. Solubility of Na 2 CO 3 +NaBr, NaCl and Nal in alcohol. Numerical data given by Cocheret (Dissert. 1911), reported in Tables annuelles international es des Constants, etc. for 1911. Solubility of Na 2 CO 3 in propyl alcohol at 20. Alcohol, wt. per cent g. Na 2 COs per 100 g. solution (Cocheret, Dissert. 1911.) Insol. in liquid C0 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Insol. in liquid NH 8 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. (Fresenius.) SI. sol. in absolute alcohol; apparently insol. in an alcoholic solution of soap. (Duffy, Chem. Soc. 6. 305.) Solubility of Na 2 CO 3 in ethyl alcohol at 20. 28 38 44 46 48 50 54 62 4.4 2.7 1.7 1.5 13 1.2 0.9 0.4 (Linebarger, A. Ch. J. 1892, 14. 380.) A full discussion of the solubility of Na 2 C0 3 in propyl, and allyl alcohol is given by Frank- forter and Temple (J. Am. Ch. Soc. 1915, 37. 2697). Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3602.) ' Alcohol, wt. per cent g. Na-COs per 100 g. solution 44 46 48 - 50 54 1.7 1.13 0.9 0.84 0.80 (Linebarger, A. Ch. J. 1892, 14. 380.) CARBONATE, SODIUM 209 Solubility in mixtures of pyridine and H 2 O from 65 to +200. Solubility curves are given. (Limbosch, Chem. Soc. 1909, 96 (2), 472.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) 100 g. glycerine (sp. gr. = 1.262) dissolve 98.3 g. Na 2 CO 3 at 15-16. (Ossendowski, Pharm. J. 1907, 79. 575.) 100 g. sat. solution in glycol contain 3.28- 3.4 g. Na 2 CO 3 . (de Coninck, Bull. Soc. Belg. 1907, 21. 141.) 100 g. sat. Na 2 CO 3 +sugar-|-Aq contain 6.89 g. Na 2 CO 3 +64.73 g. sugar at 31.25. (Kohler, Z. Ver. Zuckerind. 1897, 47. 447.) +H 2 O. Takes up H 2 O from the air. Less sol. in H 2 O at 104 than at 38; at 15-20, 100 pts. H 2 O dissolve 52.4 pts. of this salt, cal- culated as Na 2 CO 3 . Insol. in alcohol. (Lowel.) Solubility in 100 pts. H 2 O at t. Corrected t. (Hydrogen scale) Pts. anhydrous salt 29.86 50.53 29.89 50.75 31.80 50.31 35.17 49.63 35.37 49.67 35.66 49.37 35.86 49.44 36.45 49.36 36.90 49.29 .37.91 49.11 38.92 49.09 40.94 48.51 40.93 48.52 43.94 47.98 (Wells and McAdam, J. Am. Chem. Soc. 1907, 29. 726.) Solubility in alcohol +Aq. Composition of the alcohol and water layers in contact with the solid phase Na 2 CO 3 +H 2 O. t Alcohol layer Water layer % alcohol % salt % water % alcohol % salt % water 68 49 40 36 35 55.8 61.0 61.0 62.0 62.9 0.9 0.4 0.4 0.3 0.3 43.3 38.6 38.6 37.7 36.8 2.3 1.2 1.2 1.1 1.0 28.8 31.5 31.9 32.1 32.4 68.9 67.3 66.9 66.8 66.6 (Ketner, Z. phys. Ch. 1902, 39. 651.) +3H 2 O. (Schickendantz, A. 156. 359.) +5H 2 O. (Persoz, Pogg. 32. 303.) Not efflorescent. Sol. in H 2 O. +6H 2 O. (Mitscherlich, Pogg. 8. 441.) +7H 2 O. Efflorescent. Two salts, 7H 2 O (6) ( = + 8H 2 O of Thomson), and 7H 2 O (a). See also under Na 2 CO 3 . Solubility in 100 pts. H 2 O at t. Corrected t. (Hydrogen scale) 30.35 31.82 32.86 34.37 34.76 35.15 35.17 35.62 Pts. anhydrous salt 43.50 45.16 46.28 48.22 48.98 49.23 49.34 50.08 (Wells and McAdam, J. Am. Chem. Soc. 1907, 29. 726.) Composition of the solutions which can be in equilibrium with Na 2 CO 3 +7H 2 O/3 at different temperatures. 32.1 32.5 33.3 33.9 34.5 % Na 2 C03 31.8 32.1 32.7 33.0 33.9 (Ketner, Z. phys. Ch. 1902, 39. 646.) Composition of the alcohol and water layers in contact with the solid phase, Na 2 CO3-f- 7H 2 O/8, at different temperatures. t Alcohol layer Water Jayer % alcohol % salt % water %al- cobol % salt % water 33.2 32.3 31.9 31.45 31.2 58.1 56.1 54.8 53.5 52.4 0.5 0.6 0.7 0.7 0.8 42.4 43.3 44.5 45.8 46.8 1.4 1.5 1.7 31.0 30.2 29.8 29.3 29.3 67.6 68.3 68.5 (Ketner.) Composition of the two liquid layers which at different temperatures can be in metastabile equilibrium with Na 2 CO 3 + 7H 2 0]8. t Alcohol layer Water layer % alcohol salt % water % 1- cohol % salt % water 28.9 .26.6 23.0 46.9 39.1 24.5 1.3 1.3 6.7 51.8 59.6 68.8 2.3 3.3 7.0 26.3 25.4 20.2 71.4 71.3 72.8 (Ketner.) +10H 2 O. Efflorescent. Sol. in 1.05 pts. H 2 O at 23, and sat. solution has sp. gr. 1.1995. (Schiff, A. 109. 326.) Melts in crystal H 2 O at 34. (Tilden, Chem. Soc. 46. 409.) See above under Na 2 CO 3 for further data. 210 CARBONATE, SODIUM HYDROGEN Solubility in 100 pts. H 2 O at t. Composition of the alcohol liquids which can be in equilibrium with Na 2 CO 3 +10H 2 O and Na 2 CO 3 +7H 2 Oj8 at different tem- peratures. Corrected t. (Hydrogen scale) Pts. anhydrous salt 27.84 29.33 29.85 30.35 31.45 31.66 31.72 32.06 34.20 37.40 38.89 40.12 43.25 43.95 44.21 45.64 t % alcohol % salt % water 29 26 21 62.3 67.8 73.3 C.3 0.1 C.06 37.4 32.1 26.6 (Ketner.) See also under Na 2 CO 3 . +15H 2 0. (Jacquelain, A. 80. 241.) /TIT 11 _ J TV*- A J - T A - fVL* . C( 1 f\f\>-r 29. 726.) Sat. solution at 25 contains 29.37 g. anhyd. Na 2 CO 3 in 100 g. H 2 O. (Osaka, J. Tok. Ch. Soc. 1911, 32. 870.) Sat. solution at 25 contains 28.3 g. anhyd. Na 2 CO 3 in 100 g. H 2 O. (de Paepe, Bull. Soc. Chim. Belg. 1911, 25. 174.) Sat. solution at 30 contains 27.4-27 98 g. anhyd. Na 2 CO 3 in 100 g. of the solution. (Cocheret, Dissert. 1911.) Sat. solution at 25 contains 27.64 g. anhyd. Na 2 CO 3 in 100 cc. of the solution. (McCoy and Test, J. Am. Chem. Soc. 1911, 33. 474.) Solubility in alcohol. Composition of the alcohol and water layers in contact with the solid phase, Na 2 CO 3 + 10H 2 O, at different temperatures. Alcohol layer Water layer t t 7 7 % al- % 7 alcohol salt water cohol salt water 30.6 47.8 1.2 51.0 2.3 27.8 69.9 29.7 40.0 2.1 57.9 2.9 25.5 71.6 29.0 32.7 3.8 63.5 4.3 22.7 73.0 28.2 23.5 7.3 69.2 7.9 18.6 73.5 (Ketner, Z. phys. Ch. 1902, 39. 651.) Solubility in alcohol +Aq. Liquids which can be in equilibrium with Na 2 C0 3 +10H 2 Oat21. % alcohol % salt % water 18.5 81.5 6.2 12.7 81.1 15.3 6.9 77 8 26.1 3.2 70 7 39.2 1.2 59 6 58.2 0.2 41.6 67.1 0.1 32.8 73.3 0.06 26.64 (Ketner.) Sodium hydrogen carbonate, NaHCO 3 . 100 pts. cold H 2 O dissolve 7.7 pts. NaHCOs. (Rose, Schw. J. 6. 52.) 100 pts. H 2 O at 11.25 dissolve 8.27 pts. NaHCOs to form solution of 1.0613 sp. gr. (Anthon, Dingl. 161. 216.) 100 pts. HoO dissolve at 10 20 30 8.95 10.04 11.15 12.24 pts. NaHCO 3 , 40 50 60 70 13.35 14.45 15.57 16.69 pts. NaHCO 3 . (Poggiale, A. ch. (3) 8. 468.) 100 pts. H 2 O dissolve its. NaHCO 3 at t. t Pts. NaHCOs t Pts. NaHCOs t Pts. NaHCOs 6.90 21 9.75 42 13.05 1 7.00 22 9.90 43 13.20 2 7.10 23 10.05 44 13.40 3 7.20 24 10.20 45 13.55 4 7.35 25 10.35 46 13.75 5 7.45 26 10.50 47 13.90 6 7.60 27 10.65 48 14.10 7 7.70 28 10.80 49 14.30 8 7.85 29 10.95 50 14.45 9 8.00 30 11.10 51 14.65 10 8.15 31 11.25 52 14.85 11 8.25 32 11.40 53 15.00 12 8.40 33 11.55 54 15.20 13 8.55 34 11.70 55 15.40 14 8.70 35 11.90 56 15.60 15 8.85 36 12.05 57 15.80 16 9.00 37 12.20 58- 16.00 17 9.15 38 12.35 59 16.20 18 9.30 39 12.50 60 16.40 19 9.40 40 12.70 20 9.60 41 12.90 (Dibbits, J. pr. (2) 10. 417.) Experiments with solutions of sodium hy- drogen carbonate show that they gradually decompose after a time. (Treadwell, Z. anorg. 1898, 17. 204.) The source of error of many solubility de- terminations of this substance is due to loss of CO 2 . Solutions exposed to the air lose CO 2 . (McCoy, Am. Ch. J. 1903, 29. 438.) 1 1. sat. solution at 25 contains 98.4 g. NaHCO 3 . (McCoy and Test, J. Am. Chem. Soc. 1911, 33. 474.) CARBONATE, SODIUM HYDROGEN 211 NaHCOs+Aq sat. at 16 has sp. gr.= 1/lftQfM f^tnlhn ^ Temperature, 75 C. .UOyUrt. [fWOUJnj Nearly insol. in sat. Nad, or Na 2 SO 4 +Aq. (Balmain, B. 5. 121.) Gram atoms Na Amount solution used for titration Amount Na combined as NazCOs Amount Na combined as NaHCOs Equilibrium between Na 2 CO 3 and NaHC0 3 in H 2 O and in contact with the air. System: Na 2 CO 3 , NaHCO 3 , and CO 2 . Temperature, 25 C. per liter cc. Per cent Per cent 0.003 50 25 25 25.7 74.3 Amount Amount Amount Na 0.019 20 34.8 65.2 Gram solution used Na combined combined as on atoms Na per liter for titration cc. as Na2COs Per cent NaHCOs Per cent 0.036 i\J 10 55.7 44.3 10 0.0044 50 8.7 91.3 0.270 5 79.5 20.5 50 5 0.0143 20 20.0 80.0 0.702 1 85.0 15.0 20 1 0.0562 10 37.3 62.7 6.56 1 84.8 15.2 10 1 0.2248 1C 59.3 40.7 0.8847 10 2 64.0 36.0 System: Na 2 CO 3 and NaHCO 3 at 25 C. 2 Total salts Na 2 COs NaHCOs dissolved Temperature, 37 C. grams Weight Grams Weight J er cent Q ra mg Per cent Amount Amount Amount 0.3555 0.0203 5.71 03352 94.29 Gram atoms Na per liter solution used for titration Na combined as NwCOi Per cent Na combined as NaHCOs Per cent 1.1053 4.0443 0.1505 1.1041 13.62 0.9548 86.38 27.30 2.9402 72.70 ' 14.6558 7 0212 47.91 7.6o Ufi 52 09 0.0019 50 10.5 89.5 56^3982 29.8223 52.88 26.5759 47.12 O.C071 50 20 20 21.1 78.9 (Cameron and Briggs, J. phys. Chem. 1901, 6. 540.) 0.0276 1C 10 41.3 58 7 100 g. a cohol of 0.941 sp. gr. dissolve 1.2 g. .030 1C 64.5 35.5 NaHCO 3 at 15.5. 0.421 10 2 81.9 18.1 100 g. glycerol dissolve 8 g. NaHCO 3 at 15.5. (Ossendowski, Pharm. J. 1907, 79. 2 575.) 0.815 2 86.5 13.5 Insol. in acetone. (Naumann, B. 1904, 37. 9 4329.) 1.795 2 + 2 83.4 16.6 Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Temperature, 50 C. Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Amount Amount Amount Gram atoms Na per liter solution used for tit ration cc. Na combined as Na 2 COs Per cent, Na combined as NaHCOs Per cent Sodium rWhydrogen bicarbonate, Na 4 H 2 (C0 ) 3 +3H 2 0. 0.0017 50 22.2 77.8 More sol. than NaHCO 3 , less sol. tnan Na 2 CO 3 in H 2 O. (Rose, Pogg. 34. 160.) 0.0071 25 20 20 32.9 67.1 100 pts. H 2 O dissolve, calculatec 3C0 2 I as 2Na 2 0, 0.0266 10 50.7 49.3 at 12.63 pts. at 60 29.68 pts. 20 10 15.50 " 70 32.55 " 0.1014 10 70.0 30.0 20 18.30 " 80 35.8 " 10 30 21.15 " 90 38.63 " 0.4066 10 81.0 19.0 40 23.95 " 100 41.59 " 2 50 26.78 0.8068 2 2 86.8 13.2 (Poggiale, A. ch. (3) 8. 468.) 1.7486 2.1 87.1 12.9 Min. Trona, Urao. See Na 3 H(CO a )-f 2 2H 2 0. 212 CARBONATE, SODIUM HYDROGEN Tnsodium hydrogen carbonate, Na 3 H(CO 3 )2 +2H 2 0. Sol. in H 2 O. True formula of "Trona" and "Urao." (Zepharovich, Zeit. Kryst. 13. 135; de Mon- desir, C. R. 104. 1505.) Sodium thorium carbonate, 3Na 2 CO 3 , Th(CO 3 ) 2 +12H 2 O. Decomp. by H 2 O. (Cleve.) Sodium uranyl carbonate, 2Na 2 CO 3 , (U0 2 )C0 3 . Slowly sol. in H 2 O. Solution sat. at 15 has sp. gr. = 1.161. (Anthon, Dingl. 166. 207.) Sodium yttrium carbonate, Na 2 CO 3 , Y 2 (CO 3 ) 3 +4H 2 0. Ppt. Not decomp. by cold H 2 O. (Cleve.) Sodium zinc carbonate, 3Na 2 O, 8ZnO, 11CO 2 +8H 2 O = 3Na 2 C0 3 , 8ZnCO 3 +8H 2 O. SI. decomp. by pure H 2 O. (Wohler.) Less easily decomp. by H 2 O than most double carbonates. (Deville, A. ch. (3) 33. 101.) Na 2 O, 3ZnO, 4CO 2 +3H 2 O. (Kraut, Z. anorg. 1897, 13. 13.) Sodium carbonate sulphite, Na 2 C0 3 , 2Na 2 SO 3 +21H 2 0. Sol. in hot H 2 O, si. sol. in cold H 2 O. (John- son, J. Soc. Chem. Ind. 1895, 14. 271.) Strontium carbonate, SrCO 3 . Sol. in 18,045 pts. H 2 O at ordinary temp. (Fresenius.) Sol. hi 12,522 pts. H 2 at 15. (Kremers, Pogg. 85. 247.) Sol. in 33,000 pts. H 2 O. (Bineau, C. R. 41. 511.) Less sol. in H 2 O than SrSO 4 . (Dulong.) Sol. in 1536 pts. boiling H 2 O. (Hope, Edinb. Trans. 4. 5.) Calculated from electrical conductivity of SrCO 3 +Aq, SrCO 3 is sol. in 121,760 pts. H 2 O at 8.8 and 91,468 pts. at 24.3 (Holle- mann, Z. phys. Ch. 12. 130). 1 1. H 2 O dissolves 11 mg. SrC0 3 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) "Solubility product " = 15. 67 X 10- 10 mol. litre. (McCoy and Smith, J. Am. Chem. Soc. 1911, 33. 473.) Sol. in 833 pts. H 2 CO 3 +Aq at 10. (Gmelin.) Sol. in 56,545 pts. H 2 O containing NH 4 OH and (NH 4 ) 2 CO 3 . Quite sol. in NH 4 Cl+Aq or NH 4 N0 3 -f-Aq, but reprecipitated on addition of NH 4 OH and (NH. 4 ) 2 CO 3 +Aq. (Fresenius.) Partially decomp. by boiling with aqueous solutions of K 2 SO 4 , Na 2 SO 4 , CaSO 4 (NH 4 ) 2 S0 4 , MgS0 4 , Na 2 HP0 4 , (NH 4 ) 2 HP0 4 K 2 S0 3 , Na 2 S0 3 , (NH 4 ) 2 S0 3 , Na 2 B 4 O 7 , Na 2 AsO 2 , K 2 AsO 2 , K 2 C 2 O 4 , Na 2 C 2 O 4 , NaF, and K 2 CrO 4 . Decomp. is complete with the NH 4 salts. (Dulong, A. ch. 82. 286.) SI. decomp. by Na 2 SO 4 , or K 2 SO 4 +Aq. (Persoz.) Easily sol. in NH 4 chloride, nitrate, or succinate+Aq, but less so than BaCO 3 . (Fresenius.) Sol. in ferric salts +Aq, with pptn. of Fe 2 OeH 6 . Sol. in Na citrate +Aq. (Spiller.) Not decomp. by a mixture of 1 pt. H 2 SO 4 and 6 pts. absolute alcohol, or by al- coholic solutions of tartaric, racemic, citric, or glacial acetic acids; immediately decomp. by HNO 3 +absolute alcohol, or H 2 C 2 O 4 + . alcohol. Solubility of SrCO 3 in NH 4 Cl+Aq. abi % NH 4 C1 % SrCOs 5.35 10 20 0.179 0.259 . 0.358 (Cantoni and Goguelia, Bull. Soc. 1905, (3) 33. 13.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3602.) Insol. in acetone. (Naumann, B. 1904. 37, 4329.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Min. Strontianite. Strontium hydrogen carbonate. SrC0 3 is sol. in 850 pts. of a sat. solution of CO 2 in H 2 O. Strontium uranyl carbonate, SrO, 2UO 3 , 2CO 2 +16H 2 O. As Ba comp. (Blinkoff, Dissert. 1900.) Terbium carbonate. Ppt. Insol. in excess (NH 4 ) 2 CO 3 +Aq. (Potratz, C. N. 1905, 92. 3.) Thallous carbonate, T1 2 CO 3 . 100 pts. H 2 O dissolve pts. T1 2 CO 3 (C = ac- cording to Crookes; L = according to Lamy) at 15.5 18 62 100 100.8 4.2 5.23 12.85 27.2 22.4 pts. T1 2 CO 3 . C L L C L Insol. in absolute alcohol (L), and ether (C). Insol. in acetone and pyridine. (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Thallous carbonate, acid, T1 2 O, 2CO 2 . Rather easily sol. in cold H 2 O. (Carstan- jen.) CARBONATE, ZIRCONIUM 213 T1HCO 3 . (Giorgis, Gazz. ch. it. 1894, 24. 474-479.) Thallous carbonate platinocyanide, T1 2 CO 8 , Tl 2 Pt(CN) 4 . SI. sol. in hot, insol. in cold H 2 O. (Fris- well, Chem. Soc. (2) 9. 461.) Thorium carbonate, basic, 2ThO 2 , C0 2 -f 3H 2 0. Insol. in CO 2 +Aq, but sol. in excess of alkali carbonates +Aq, if cone. Tin (stannous) carbonate, 2SnO, CO 2 . Easily decomp. on air; insol. in H 2 O or H 2 CO 3 +Aq. (Devnie, A. ch. (3) 35. 448.) Uranyl carbonate, basic, 5(U0 2 )(OH) 2 , 3(UO 2 )CO 3 +6H 2 O. Ppt. (Seubert and Elten, Z. anorg. 1893, 4. 80.) Ytterbium carbonate, basic, Yb(OH)C0 8 + H 2 0. Ppt. (Cleve, Z. anorg. 1902, 32. 146.) Ytterbium carbonate, Yb 2 (CO 8 ) 3 +4H 2 O. Ppt. (Cleve, Z. anorg. 1902, 32. 146.) ' Yttrium carbonate, Y 2 (CO 3 ) 3 +3H 2 O. Insol. in H 2 O; very si. sol. in H 2 CO 3 +Aq. Sol. in SO 2 +Aq and all mineral acids. Sol. in NH 4 salts, and alkali carbonates +Aq to some extent. More sol. in (NH 4 ) 2 CO 3 -f Aq than in K 2 CO 3 +Aq. (Berlin.) More sol. in (NH 4 ) 2 CO 3 +Aq than cerium, but 5 or 6 times less sol. than glucinum carbonate. (Vauquelin.) Sol. in large excess of KHCO 3 + Aq. (Rose.) Slowly sol. in NH 4 salts +Aq. (Berzelius.) Zinc carbonates, basic, 8ZnO, CO 2 +2H 2 O; 5ZnO, 2CO 2 +3, or 7H 2 O; 3ZnO, CO 2 + H 2 O; HZnO, 4CO 2 + 14H 2 O; 14ZnO, 5CO 2 +9H 2 O; 2ZnO, CO 2 +H 2 O; 8ZnO, 3CO 2 +5H 2 O, etc. All ppts. formed from Zn salts and carbo- nates +Aq. Sol. in 2000-3000 pts. cold H 2 O, separates out on heating and does not redis- solve on cooling. (Schindler.) Sol. in 20,895 pts. H 2 O at 15. (Kremers, Pogg. 85. 248.) Sol. in 44,600 pts. H 2 O at ord. temp. (Fre- senius.) Sol. in 1428 pts. sat. H 2 CO 3 +Aq. (Las- saigne.) Sol. in 189 pts. H 2 CO 3 +Aq sat. at 4-6 atmos. (Wagner, Z. anal. 6. 107.) Easily sol. in KOH, NaOH, NH 4 OH, (NH 4 ) 2 CO 3 + Aq, and in acids. Somewhat sol. in alkali bicarbonates and NH 4 salts +Aq. (Frese- nius.) Sol. in hot (Fuchs), also cold (Brett, 1837) NH 4 Cl+Aq; less sol. in NH 4 NO 3 +Aq. (Brett.) Sol. in all NH 4 salts +Aq excepting (NH 4 ) 2 S +Aq. (Terreil, Bull. Soc. (2) 9. 441.) Insol. in Na 2 CO 3 , or K 2 CO 3 +Aq. Sol. in ferric salts -fAq with pptn. of Fe 2 O 6 H 6 . (Fuchs, 1831.) The carbonates described by Boussingault, Wackenroder, Rose, and probably all salts between ZnO, CO 2 and 5ZnO, 2CO 2 are mix- tures. (Kraut, Z. anorg. 1897, 13. 1-15.) 3ZnO, CO 2 +2H 2 O. Min. Zinc bloom, Hy- drozincite. ZnCO 3 , 3ZnO 2 H 2 . Min. AuricalcUe. Zinc carbonate, ZnCO 3 . 1 1. H 2 O at 15 dissolves 0.01 g.; 1 1. H 2 O dissolves 1.64 x 10- 4 mols., or 0.206 g. ZnCO 3 at 25. (Ageno and Valla, Att. ace. Line. 1911, 20, II. 706.) 1 1. 5.85% NaCl+Aq dissolves 0.0586 g; 11. 7.45% KCl+Aq dissolves 0.0477 g. ZnCO,. (Essen, Gm.-K. 4, 1. 680.) Sol. in acids, KOH+Aq, and NH 4 salts -f Q Sol. inH 2 CO 3 -fAq. Solubility hi various salts -fAq. Solvent 10% NaNO 3 +Aq sat. NaN0 3 +Aq 5% NaCl+Aq 10% NaCl+Aq sat. NaCl+Aq 10% Na 2 SO 4 +Aq sat. Na 2 SO 4 +Aq g. ZnCOs sol in 1 1. of the solvent 0.058981 0.149000 0.021730 0.046564 0.130380 0.009313 0.015521 (Ehlert, Z. Elektrochem. 1912, 18. 728.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Min. Calamine, Smithsonite. Calamine is sol. in NH 4 OH+Aq only in the presence of NH 4 salts. (Brandhorst, Zeit. angew. Ch. 1904, 17. 513.) + ^H 2 O. (Mikusch, Z. anorg. 1908, 56. 366.) +H 2 O. (Belar, Zeit. Kryst. 1890, 17. 126.) Zinc carbonate ammonia, ZnCO 3 , NH 3 . Slowly decomp. by H 2 O, but not on the ah*, or by boiling with alcohol. (Favre, A. ch. (3) 10. 474.) Zinc carbonate hydroxylamine, ZnCO 3 , 2NH 3 O. Insol. in H 2 O. Decomp. by acids. (Gold- schmidt and Syngros, Z. anorg. 5. 129.) Zirconium carbonate, 3ZrO 2 , CO 2 +6H 2 O. Decomp. by hot H 2 O, all CO 2 being given off. (Hermann.) Sol. in alkali carbonates +Aq. 214 CARBONIC ACID Percarbonic acid. See Percarbonic acid. Carbonic anhydride, CO 2 . See Carbon dioxide. Carbonophosphoric acid. Potassium carbonophosphate, (K 2 HP0 4 ) 2 , 2C0 2 , 2KHC0 3 . Known only in solution. (Barille, C. R. 1903, 137. 566.) Carbonyl bromide, COBr 2 . Decomp. by H,O. (Besson, C. R. 1895, 120. 192.) Carbonyl platinous bromide, CO, PtBr 2 . Sol. in H 2 O with almost instant decomp. Sol. in absolute alcohol. (Pullinger, Chem. Soc. 59. 603.) Quite easily sol. in hot C 6 H 6 , insol. in ligroine, and can be crystallized from CC1 4 . Very easily sol. in HBr+Aq. (MyHus and Forster, B. 24. 2432.) Carbonyl bromochloride, COClBr. Decomp. by H 2 0. (Besson.) Carbonyl chloride, COC1 2 . Phosgene. Cold H 2 O dissolves 1-2 vols. COC1 2 gas with slow decomposition. Alcohol decomp. immediately. Immediately absorbed by KOH, or NH 4 OH+Aq. Very sol in gla- cial HC 2 H 3 O 2 , benzene, and most liquid hy- drocarbons. (Berthelot, Bull Soc. (2) 13. 14.) Sol. in SC1. 1 vol. AsCl 3 absorbs 10 vols. COC1 2 . ZH'carbonyl cuprous chloride, Cu 2 Cl 2 , 2CO + 4H 2 0. Decomp. by air. (Jones, Am. Ch. J. 1899, 22. 305.) Carbonyl platinous chloride, 2COC1 2 , PtCl 2 . SI. deliquescent. Easily sol. in H 2 O with- out decomp.; si. sol. in alcohol. Almost insol. in CC1 4 . (Pullinger, Chem. Soc. 69. 600.) .owocarbonyl platinous chloride, CO, PtCl 2 . Decomp. by H 2 O and alcohol; sol. in hot CC1 4 . (Schiitzenberger, A. ch. (4) 15. 100.) Sol. in cone. HCl-j-Aq. (Mylius and For- ster.) Zh'carbonyl platinous chloride, 2CO, PtCl 2 . Decomp. by H 2 O and alcohol. Sol. in CC1 4 . (Schiitzenberger.) Decomp. by cone. HCl+Aq into CO and CO, PtCl 2 . (Mylius and Forster.) Sesquicarbonyl platinous chloride, 3CO, 2PtCl 2 . Decomp. by H 2 O or alcohol. Much more sol. in CC1 4 than 2CO, PtCl 2 . Carbonyl platinous iodide, CO, PtI 2 . Not hygroscopic. Insol. in, but slowly de- comp. by, H 2 O. Easily sol. in benzene or ether, also in alcohol, which decomp. on warm- ing; sol. in HI+Aq. (Mylius and Forster.) Carbonyl platinous sulphide, CO, PtS. Easily decomp. Insol. in ordinary solvents. (Mylius and Forster.) Carbonyl sulphide, COS. H 2 absorbs 1 vol. COS. Absorption of COS by H 2 O at t. 10 20 30 Coefficient of absorption 1.333 0.835 0.561 0.403 (Winkler, Z. phys. Ch. 1906, 55. 351.) 1 ccm. H 2 O at 13.5 and 756 mm. pres. dissolves 0.8 ccm. COS. (Hempel, Zeit. angew. ch. 1901, 14. 867.) 1 ccm. of a hydrochloric acid solution of Cu 2 Cl 2 absorbs about 0.2 ccm. COS. (Hem- pel.) Carbonyl ferrocyanhydric acid. H 3 Fe(CO)(CN) 5 . Very sol. in H 2 O; decomp. on heating. (Muller, A. ch. (6) 17. 94.) Cobalt carbonyl ferrocyanide. SI. sol. in H 2 O; very sol. in dil. HN0 3 +Aq. (M.) ^ Cupric carbonyl ferrocyanide, Cu 3 [Fe(CO)(CN) 5 ] 2 . Insol. in H 2 O, H 2 SO 4 , or dil. HNO 3 -f Aq. (M.) Iron (ferric) carbonyl ferrocyanide, FeFeCO(CN) 5 . Insol. in H 2 0. Sol. in H 2 C 2 O 4 +Aq. Insol. in acetic, lactic, succinic, tartaric, and citric acids +Aq, but easily sol. in the neutral salts of those acids. Insol. in KC1, or KNO 3 +Aq, but sensibly sol. in Na 2 HPO 4 +Aq. Insol even on warming in very dil. H 2 SO 4 , or H 3 PO 4 . -fAq. (Muller.) Potassium carbonyl ferrccyanide, K 3 Fe(CO)(CN) 6 +3^H 2 O. 100 pts. H 2 O dissolve 148 pts. at 16. (Muller, C. R. 104. 992.) CEROUS HYDROXIDE 215 Silver carbonyl f errocyanide, Ag 3 Fe(CO)(CN) 5 . Insol. in H 2 O; si. sol. in dil. H 2 S0 4; HC1, or HN0 3 +Aq; scarcely attacked by cone. HC 2 H 3 2 +Aq. (Muller.) Sodium carbonyl ferrocyanide, Na 3 Fe(CO)(CN) 5 +6H 2 O. Sol. inH 2 O. (Muller.) Uranyl carbonyl ferrocyanide, (UO 2 ) 3 [FeCO(CN) 6 ] 2 +5H 2 O. SI. sol. in H 2 O, but more easily if H 2 O is acidified with HC 2 H 3 O 2 . Cericotungstic acid. Ammonium cericotungstate, 2(NH 4 ) 2 0, Ce 2 O 3 , 16WO 8 +2H 2 O. Insol. in H 2 O, but decomp. by boiling therewith. (Smith, J. Am. Chem. Sec. 1904. 26. 1481.) Cerium, Ce. Decomp. pure H 2 O very slowly at ordinary temp. Not attacked by cold cone. H2SO4 or red fuming HNO 3 . Sol. in dil. H 2 SO 4 +Aq, HNO 3 +Aq, and cone, or dil. HCl+Aq. (Hillebrand and Norton, Pogg. 155. 633.) Cerous bromide, CeBr 3 . Anhydrous. As the chloride. (Robinson, Proc. Roy. Soc. 37. 150.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +zH 2 O. Very deliquescent. (Jolin.) Cerium gold bromide, CeBr 3 , AuBr 3 +8H 2 O. See Bromaurate, cerium. Cerium carbide, CeC 2 . Decomp. by fused alkali nitrates, chlorates, hydroxides and carbonates; and by cone. H 2 SO 4 on heating. Insol. in cone. HNO 3 ; decomp. by H 2 O and dil. acids. (Moissan, C. R. 1896, 122. 359.) CeC 3 . Not attacked by hot cone, acids. (Delafontaine, J. B. 1865. 176.) Cerous chloride, CeCl 3 . Anhydrous. Deliquescent. Sol. in H 2 O with hissing and evolution of heat; sol. in alcohol. Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Difficultly scl. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) +7H 2 O. Insol. in NH 4 OH-f Aq. (Den- nis, Z. anorg. 1894, 7. 260.) +73/H 2 O. Deliquescent. (Berzelius.) Decomp. by boiling with H 2 O. Sol. in 1 pt. H 2 O at ord. temp, and 3-4 pts. alcohol. (Dumas.) Ceric chloride. Known only in solution, which decom- poses by slight heat. (Berzelius.) Cerous mercuric chloride. Not deliquescent, (v. Bonsdorff.) CeCl 3 , 4HgCl 2 +10H 2 O. Permanent; eas- ily sol. in H 2 O. (Jolin, Bull. Soc. (2) 21. 533.) Cerium stannic chloride. See Chlorostannate, cerium. Cerous chloride zinc iodide. Sol. in H 2 and alcohol. (Holzmann, J. pr_ 84. 76.) Cerous fluoride, CeF 3 . Insol. ppt. Ceric fluoride, CeF 4 . Insoluble precipitate. (Berzelius.) +H 2 O Insol. in H 2 O. (Brauner, B. 14. 1944.) Ceric cobaltous 'fluoride, 2CeF 4 , CoF 2 +7H 2 O. Ppt. Easily decomp. by H 2 O. (Rimbach v A. 1909, 368. 107.) Ceric cupric fluoride, 2CeF 4 , CuF 2 -f 7H 2 O. Ppt. Decomp. by H 2 O. (Rimbach, L c.) Ceric nickel fluoride, 2CeF 4 , NiF 2 -f 7H 2 O. Ppt. Decomp. by H 2 O. (Rimbach, 7. c.) Ceric potassium fluoride, 2CeF 4 , 3KF+2H 2 O. Icsol. in H 2 O. (Brauner, B. 14. 1944; 15. 109.) Could not be obtained pure. (Rimbach, /. c.) Ceric zinc fluoride, 2CeF 4 , ZnF 2 +7H 2 O. Ppt. Decomp. by H 2 0. (Rimbach, L c.) Ceroceric fluoride, 2CeF 8 , CeF 4 . Min. Fluocerite. Cerium hydride, CeH 2 . Decomp. by acids. (Winkler, B. 24. 873.) CeH 8 . Decomp. in moiet air; decomp. by hot or cold H 2 O; sol. in acids with evolution of H 2 0. Decomp. by alkalis. (Muthmann, A. 1902, 326. 266.) Cerous hydroxide, Ce 2 O s , zH 2 O. Easily sol. in acids. Insol. in excess of alkali hydroxides +Aq. Sol. in (NH 4 ) 2 CO 4 + Aq. 100 ccm. of a solution in glycerine +Aq containing about 60% by vol. of glycerine contain 7.9 g. Ce 2 O a . (Muller, Z. anorg. 1905, 43. 322.) Exists in two modifications: one insol. in 216 CERIC HYDROXIDE cold HCl+Aq; the other sol. in cold HC1+ Aq. (Brauner, C. N. 1895, 71. 283.) Ceric hydroxide, 2CeO 2 , 3H 2 0. Sol. in HNO 8 or H 2 SO 4 ; also in HCl+Aq, forming cerous chloride and free chlorine. Insol. in hydrofluoric, acetic, or formic acids + Aq. Somewhat sol. in dil. HNO 8 , or HC1+ Aq. (Ordway,Am.J.Sci.(2)26.205.) Insol. in NH 4 OH, KOH, and NaOH+Aq. SI. sol. in alkali carbonates +Aq. (Dumas.) SI. sol. in (NH 4 ) 2 CO 3 +Aq. (Ordway.) 100 com. of a solution in glycerine +Aq containing about 60% by vol. of glycerine contain 0.08 g. CeO 2 . (Mttller, Z. anorg. 1905, 43. 232.) Cerous iodide, Gels. Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) +9H 2 0. Very deliquescent and sol. in H 2 O. (Lange, J. pr. 82. 134.) Sol. in alcohol. Cerium nitride, CeN. Decomp. by H 2 O and alkali. Sol. in min- eral acids with formation of cerous and am- monium salts. (Muthmann, A. 1902, 325. 272.) Cerous oxide, Ce 2 O 3 . When ignited, insol. in HCl+Aq; when long digested with H 2 SO 4 , is sol. in HCl+Aq with addition of alcohol. Ceric oxide, CeO 2 . When ignited, is only dissolved in traces, even on heating, by HC1 or HNO 3 +Aq. Sol. in cone. H 2 SO 4 when warmed. Sol. in the cold in a solution of Kl in HCl+Aq (Bunsen), in & mixture of HC1 and FeCl 2 +Aq, or any re- ducing substance. Cerium peroxide, Ce 4 O 9 . Insol. in boiling cone, acids. Sol. in H 2 SO 4 by long digestion. (Popp, A. 131. 361.) Probably does not exist. (Rammelsberg, Pogg. 108. 40.) Ce 2 O 5 . (Hermann, J. pr. 30. 184.) Probably does not exist. (Rammelsberg.) CeO 8 +xH 2 O. Sol. in HCl+Aq. (Popp, A. 131. 361); (Lecoq de Boisbaudran, C. R. 100. 605.) Ce0 2 +H 2 O 2 , according to Cleve (Bull. Soc. (2) 43. 57.) Cerium oxycarbide, CeC 2 , 2Ce0 2 . Stable in the air. Slowly attacked by cold HjO. With hot H 2 and with acids, it gives unsat. hydrocarbons. (Sterba, C. R. 1902, 134. 1058.) Cerium oxychloride, CeOCl. Slightly attacked by hot cone. HCl+Aq. Slowly sol. in cone. HNO 3 +Aq. (Wohler.) Easily sol. in dil. acids. (Didier, C. R. 101. 882.) Cerium oxychloride tungsten fn'oxide, CeOCl, WO 3 . (Didier, C. R. 102. 823.) Cerium selenide. Insol. in H 2 O; difficultly sol. in acids. (Berzelius.) Cerium silicide, CeSi 2 . Insol. in H 2 O, by which it is acted upon only very slowly. H 2 . in HC1 and HF+Aq with evolution of Not attacked by alkalis +Aq or NH 4 OH+ Aq. Insol. in organic solvents. (Sterba, C. R. 1902, 136. 170.) Cerium silicide, Ce 2 Si 8 . Insol. in acids. (Ullik, W. A. B. 52, 2. 115.) Cerium bisulphide, Ce 2 S 4 . Not decomp. by cold H 2 O. Slowly sol. in cold dil. H 2 SO 4 , HC1 and acetic acid. Rapidly sol. in warm dil. H 2 S0 4 , HC1 and acetic acid with decomp. (Biltz, B. 1908, 41. 3342.) Cerium sesgmsulphide, Ce 2 S 3 . Insol. in, and not decomp. by, H 2 O, but easily decomp. by the weakest acids. (Mo- sander); (Didier, C. R. 100. 1461.) Afonochloramine, NH 2 C1. Easily sol. in H 2 O. (Raschig. Ch. Z. 1907, 31. 926.) Chlorteframine comps. See Chlorotetramine comps. Metachlorantimonic acid, HSbCl 6 + Hydroscopic. Sol. in H 2 O with decomp.; sol. in alcohol, acetone, and acetic acid. (Weinland, Z. anorg. 1905, 44. 43.) Metachlorantimonic acid ammonia, HSbCle, 2NH 3 . Sol. in H 2 O and in alcohol. (Weinland and Schmid, Z. anorg. 1905, 44. 59.) Aluminum wefachlorantimonate, Al(SbCle) +15H 2 0. Hydroscopic. Sol. in dil. HCl+Aq. (Weinland, B. 1903, 36. 254.) CHLORAURATE, CERIUM 217 Ammonium raetachlorantimonate, NH 4 SbCl 6 +H 2 0. Hydroscopic. Sol. in H 2 O. Solution decomp. slowly when cold, rapidly on warming. Sol. in dil. HC1. (Weinland, B. 1903, 36. 251.) Cadmium wetachlorantimonate ammonia, Cd(SbCl 6 ) 2 , 7NH 3 . Ppt. (Weinland and Schmid, Z. anorg. 1905, 44. 56.) Calcium raetachlorantimonate, Ca(SbCl 6 )2+ 9F 2 0. Hydroscopic. Sol. in dil. HCl+Aq. (Weinland, B. 1903, 36. 253.) Chromium raetachlorantimonate, Cr(SbCl 6 )3 +13H 2 O. Hydroscopic.' Sol. in dil. HCl+Aq. (Weinland.) Chromium ort/iochlorantimonate, CrSbCl 8 + 10H 2 O. Hydroscopic. Sol. in dil. HCl+Aq. (Weinland.) Cupric wetachlorantimonate ammonia, Cu(SbCl 6 ) 2 , 5NH 3 . (Weinland and Schmid, Z. anorg. 1905, 44. 55.) Glucinum we/achloraDtimonate, Gl(SbCl fi ) 2 + 10H 2 O. Very hydroscopic. Sol. in dil. HC1. (Weinland, B. 1903, 36. 252.) Iron (ferric) or^ochlorantimonate, FeSbCls +8H 2 O. Hydroscopic. Can easily be cryst. from dil. HCl+Aq. (Weinland.) Lithium metochlorantimonate, LiSbCl6+ 4H 2 0. Very hydroscopic. Sol. in dil. HCl+Aa. (Weinland, I. c.) Magnesium pi/rochlorantimonate, MgSbCly +9H 2 0. Hydroscopic. Sol. in dil. HCl+Aq. (Weinland.) Nickel metachlorantimonate ammonia, Ni(SbCl 6 ) 2 , 6NH 3 . Sol. in H 2 O. (Weinland and Schmid, Z. anorg. 1905, 44. 57.) Potassium wetachlorantimonate, KSbCl 6 + H 2 O. Hydroscopic. Sol. in H 2 O. Solution decomp. slowly when cold, rapidly when warmed. Sol. in dil. HCl+Aq. (Weinland, B. 1903, 36. 250.) Rubidium metachlorantimonate, RbSbCl 6 . Hydroscopic. Sol. in dil. HCl+Aq. (Weinland.) Silver raetachlorantimonate ammonia. AgSbCle, 2NH 3 . Decomp. by H 2 0. (Weinland and Schmid.) Zinc melachlorantimonate ammonia, Zn(SbCl 6 ) 2 , 4NH 3 . (Weinland and Schmid.) Chlorarsenious acid. See Arsenyl chloride. Chlorauric acid, HAuCl 4 +4H 2 O. Sol. in H 2 O, alcohol, and ether. Sol. in POC1 3 . (Walden, Z. anorg. 1900, 25. 212.) Difficultly sol. in PC1 3 . (Walden.) Cryst. with 3H 2 O as stated by Weber and Schcttlander and not with 4H 2 O as stated by Thomsen. (Schmidt, C. C. 1906, II. 855.) Chloraurates. All chloraurates are easily sol. in H 2 and in alcohol, (v. Bonsdorff, 1829.) Ammonium chloraurate, NH 4 AuCl 4 +H 2 O. Very easily sol. in H 2 0. +2H 2 O. Very easily sol. in H 2 0. Barium chloraurate, Ba(Auri 4 ) 2 +zH 2 O. Deliquescent in moist air. Sol. in H 2 O and alcohol, (v. Bonsdorff, Pogg. 17. 261.) Cadmium chloraurate. Not deliquescent. Sol. in H 2 O and alcohol. (v. Bonsdorff.) Caesium chloraurate, CsAuCU. 100 pts. aqueous sat. solution contain at: 10 20 30 40 50 0.5 0.8 1.7 3.2 5.4 pts. anhydrous salt, 60 70 80 90 100 8.2 12.0 16.3 21.7 27.5 pts. anhydrous salt. (Rosenbladt, B. 19. 2538.) + ^H 2 O. (Wells and Wheeler, Am. J. (3) 44. 157.) Calcium chloraurate, Ca(AuCl 4 ) 2 +6H 2 0. Deliquescent. Sol. in H 2 and alcohol, (v. Bonsdorff.) Cerium chloraurate, CeCl 3 , AuCl 3 +10H 2 O. Extremely deliquescent. Easily sol. in H 2 O and absolute alcohol. (Holzmann, C. C. 1863. 206.) +13H 2 O. (John, Bull. Soc. (2) 21. 534.) 218 CHLORAURATE, COBALT Cobalt chloraurate, Co(AuCl 4 ) 2 +8H 2 O. Sol. in H 2 O and alcohol. (Topsoe.) Didymium chloraurate, DiCl 3 , AuCJ 3 -flOH 2 O. Very deliquescent. (Cleve, Bull. Soc. (2) 43. 361.) 2DiCl,, 3AuCl 3 +20H 2 C. (Cleve.) Gadolinium chloraurate, GdCl 3 , AuCl 3 + 10H 2 O. Sol. in H 2 C. (Benedicks, Z. anorg. 1900, 22. 404.) Lanthanum chloraurate, LaCl 3 , AuCl 3 +5H 2 O. Deliquescent in moist air. Sol. in H 2 O. (Cleve, B. 8. 128.) Lithium chloraurate, LiAuCl 4 . 100 pts. aqueous solution contain at: 10 20 30 40 53.1 57.7 62.5 67.3 pts. anhydrous salt, 50 C 60' 70 80 C 72.0 76.4 81.0 85.7 pts. anhydrous salt. (Rosenbladt.) +2H 2 O. (Antony and Lucchesi, Gazz. ch. it. 1890, 20. 601.) +4H 2 0. Not stable. Sol. in H 2 O and alcohol. (Fasbender, C. C. 1894, 1. 409.) Magnesium chloraurate, Mg(AuCl 4 ) 2 +8H 2 0. Somewhat deliquescent. Sol. in H 2 O and alcohol. (Topsoe.) +12H 2 0. Manganese chloraurate, Mn(AuCl 4 ) 2 -f 8H 2 0. Deliquescent. Sol. in H 2 and alcohol. (Topsoe.) +12H 2 O. Nickel chloraurate, Ni(AuCl 4 ) 2 +8H 2 O. Deliquescent. Sol. in H 2 O and alcohol. (Topsoe.) Potassium cbloraurate, KAuCl 4 . Anhydrous. Very stable. (Lainer, W. A. B. 99, 2b. 247.) ICO pts. solution in H 2 O contain at: 10 20 30 27.7 38.2 48.7 pts. anhydrous salt, 40 50 60 59.2 70.0 80.2 pts. anhydrous salt. (Rosenbladt, B. 19. 2538.) Sol. in H 2 O and alcohol; insol. in ether. (Fasbender, C. C. 1894, I. 409.) 1 pt. is sol. in 4 pts. 98% alcohol. (Fas- bender, C. C. 1894, II. 609.) +2H 2 O. Efflorescent. Praseodymium chloraurate, PrCl 3 , AuCl 3 + 10H 2 O. Very sol. in H 2 O; sol. in cone. HC1. (von Schule.. Z. anorg. 1898, 18. 354 ) Rubidium chloraurate, RbAuCl 4 . 100 pts. sat. RbAuCl 4 +Aq contain at: 10 20 30 40 50 4.6 9.0 13.4 17.7 22.2 pts. anhydrous salt, 60 70 80 90 100 26.6 31.0 35.3 39.7 44.2 pts. anhydrous salt. (Rosenbladt.) 1 pt. sol. in 54 pts. 98% alcohol. Insol. in ether. (Fasbender, C. C. 1894, II. 609.) Samarium chloraurate, SmCl 3 , AuCl 3 + 10H 2 0. Deliquescent. Easily sol. in H 2 0. (Cleve, Bull. Soc. (2) 43. 165.) Scandium chloraurate, 3ScCl 3 , 2AuCl 3 + 21H 2 O. Very deliquescent. (Crookes, Phil. Trans. 1910, 210. A, 365.) Silver chloraurate, AgAuCl 4 . Decomp. in the air. Decomp. by H 2 O, HC1 and NH 3 . (Herr- mann, B. 1894, 27. 597.) Sodium chloraurate, NaAuCl 4 +2H 2 O. Easily sol. in H 2 O and absolute alcohol. 100 pts. aqueous solution contain at: 10 20 30 58.2 60.2 64.0 pts. anhydrous salt, 40 50 60 69.4 77.5 90.0 pts. anhydrous salt. (Rosenbladt.) Easily sol. in NaCl+Aq. Easily sol. in H 2 O, alcohol and ether. (Fas- bender, C. C. 1894, I. 409.) Strontium chloraurate. Sol. in H 2 O. (v. Bonsdorff.) Thallium chloraurate. (Carstanjen.) Ytterbium chloraurate, YbCl 3 , AuCl 3 +9H 2 O. Ppt. (Cleve, Z. anorg. 1902, 32. 138.) Yttrium chloraurate, YtCl 3 , 2AuCl 3 + 16H 2 O. Very sol. in H 2 O. (Cleve.) Zinc chloraurate, Zn(AuCl 4 ) 2 +8H 2 O. Sol. in H 2 O. (Topsoe.) +12H 2 O. Sol. in H 2 O and alcohol, (v. Bonsdorff.) CHLORHYDRIC ACID 219 Chlorauricyanhydric acid. Barium chlorauricyanide, Ba[Au(CN) 2 Cl 2 ] 2 + 8H2O. Very sol. in H 2 O or alcohol. (Lindbom, Lund Univ. Arsk. 12. No. 6.) Potassium chlorauricyanide, KAu(CN) 2 Cl 2 + H 2 O. Very sol. in H 2 O or alcohol. Strontium chlorauricyanide, Sr[Au(CN) 2 Cl 2 ] 2 -f-8H 2 O. Sol. in H 2 O. Zinc chlorauricyanide, Zn[Au(CN) 2 Cl 2 ] 2 + 7H 2 O. Very sol. in H 2 0. Chlorhydric acid, HC1. Liquid. Miscible with liquid CO 2 , and H 2 S. Gas. Absorbed by H 2 O with production of much heat. H 2 O absorbs 400-500 vols. at ord. temp, and pressure or a little less than 1 pt. by weight. (Dalton.) 1 vol. H 2 O absorbs 480 vols. at 0; sp. gr. of sat solu- tion is 1.2109. (Davy.) 1 vol. H 2 O absorbs 417 822 vols. at 20, the vol. in- creasing to 1.4138 vols.; 1 vol. of HCl+Aq then con- tains 311 vols. HC1, has sp. gr. 1.1958. and contains 40.39% HC1 by weight. (Thomson, 1831.) 1 vol. H 2 O absorbs 464 vols. and sat. solution has 1.21 sp. gr. and contains 42.4% HC1 by weight. (Wittstein.) H 2 O sat. at contains 480 times its vol. of HC1. and sp. gr. =1.2109: sat. at ord. temp., contains 38.3% of its weight in HC1, and sp. gr. =1.192. (Berzelius.) 1 vol. H 2 O absorbs V vols. HC1 at t and 760 mm. pressure, and the liquid foimed has the given sp. gr., and contains the given per cent HC1. t V Sp. gr. %HC1 o 4 8 12 14 18 18.25 23 525.2 494.7 480.3 471.3 462.4 451.2 450.7 435.0 1 . 2257 .2265 .2185 .2148 .2074 .2064 1 . 2056 1 . 2014 45.148 44.361 43.828 43.277 42.829 42 . 344 42 . 283 41.536 (Deicke, Pogg. 119. 156,) At 760 mm. pressure 1 g. H 2 O absorbs g. HCl at t. t g. HCl t g HCl t g. HCl 0.825 22 0.710 44 0.618 2 0.814 24 0.700 46 0.611 4 0.804 26 0.691 48 0.603 6 0.793 28 0.682 50 0.596 8 0.783 30 0.673 52 0.589 10 0.772 32 0.665 54 0.582 12 0.762 34 0.657 56 575 14 0.752 36 0.649 58 0.568 16 0.742 38 0.641 60 0.561 18 0.731 40 0.633 20 0.721 42 0.626 (Roscoe and Dittmar.) Cone. HCl+Aq loses HCl, and dil. HC1+ Aq loses H 2 O on warming, until an acid of constant composition is formed, containing 20.18% HCl, with a sp. gr. of 1.101 at 15, which can be distilled unchanged at 110. (Bineau, A. ch. (3) 7. 257.) The above is true if barometer is at 760 mm., but the composition changes with the pressure as follows Mm. Hg % HCl Mm. Hg. %HC1 Mm. Hg %HC1 50 23.2 800 20.2 1700 18.8 100 22.9 900 19.9 1800 18.7 200 22.3 1000 19.7 1900 18.6 300 21.8 1100 19.5 2000 18.5 400 21.4 1200 19.4 2100 18.4 500 21.1 1300 19.3 2200 18.3 600 20.7 1400 19.1 2300 18.2 700 20.4 1500 19.0 2400 18.1 760 20.24 1600 18.9 2500 18.0 (Roscoe and Dittmar.) Cone. HCl+Aq gradually gives off HCl on the air until it has a sp. gr. 1.128 at 15, and contains 25.2% HCl. (Bineau, I. c.) According to Roscoe and Dittmar, this de- pends on the temperature. If a current of ah* is passed through HCl+Aq, acid or water is given off according as the acid is strong or weak, until an acid of constant composition for a given temperature is formed, as follows Temp. % HCl Temp. % HCl Temp. % HCl 25.0 35 23. 9 70 22.6 5 24.9 40 23. 8 75 22.3 10 24.7 45 23.6 80 22.0 15 24.6 50 23.4 85 21.7 20 24.4 55 23. 2 90 21.4 25 24.3 60 23. 95 21.1 30 24.1 65 22. 8 100 20.7 From the above it is seen that the acid which distils unchanged at a given pressure, that is, boils at a certain constant tempera- ture, is identical with the acid which under- goes no change in composition by a current of dry air at the same temperature, and under the ordinary pressure, thus Mm. Hg B.-pt. % HCl Temp, of air current %HCI 100 61-62 22.8 62 22.9 200 76-77 22.1 77 22.2 300 84-85 21.7 85 21.7 380 91 21.3 91 21.4 490 97 20.9 < )8 21.1 620 103 20.6 fRosnop n.nrl Ditfmnr ^ 220 CHLORHYDRIC ACID Solubility of HCl in H 2 O at under different degrees of pressure. P = partial pressure in mm. Hg, i. e., total pressure minus the tension of aqueous vapour at the given temp.; G = grammes of HCl dissolved in 1 g. H 2 O at the pressure P and temp. Sp. gr. of HCl-fAq. Sp. gr. %HC1 Sp. gr. %HC1 Sp gr. %HC1 1.203 1.179 1.162 1.149 1.139 40 . 66 37.00 33.95 31.35 29.13 1 . 1285 1.1197 1.1127 1 . 1060 1 . 1008 27.21 25 . 52 24.03 22.70 21.51. 1 . 0960 1 . 0902 1.0860 1 . 0820 1 . 0780 20.44 19.47 18.59 17.79 17.05 P G P G (Thomson, in his System, 2. 189.) Sp. gr. of HCl +Aq. 60 70 80 90 100 110 120 130 140 150 175 200 225 250 275 300 a. 613 0.628 0.640 0.649 0.657 0.664 0.670 0.676 0.681 0.686 0.697 0.707 0.716 0.724 0.732 0.738 350 400 450 500 550 600 650 700 750 800 900 1000 1100 1200 1300 0.751 0.763 0.772 0.782 0.791 0.800 0.808 0.817 0.824 0.831 0.844 a. 856 0.869 0.882 0.895 Sp. gr. %HC1 Sp. gr. %HC1 1.21 1.20 1.19 .18 .17 .16 .15 .14 .13 .12 .11 42.43 40.80 38 . 38 36.36 34.34 32.32 30 . 30 28.28 26.26 24.24 20.30 1.10 1.09 1.08 1.07 1.06 1.05 1.04 1.03 1.02 1.01 20.20 18.18 16.16 14 . 14 12.12 10.10 8.08 6.06 4.04 2.02 (Edm. Davy.) Sp. gr. of HCl +Aq. Sp. gr. % HCl B.-pt. Sp. gr. % HCl B.-pt. (Roscoe and Dittmar, A. 112. 334.) 1 vol. H 2 O dissolves 560 vols. HCl at 12 " " 500 " " " " 440 " " +20 (Berthelot, C. R. 76. 779.) 1 vol. H 2 O absorbs 480 vols. HCl at 15 to form a solution containing 42.85% HCl with a sp. gr. of 1.215. (Hager.) Solubility of HCl at low temperatures, and 760 mm. pressure. 1.199 1.181 1.166 1 . 154 1.144 1.136 1.127 1.121 34.01 31.09 28.29 26.57 24.84 23.25 21.06 20.74 49 65 76 87 100 103 105 109 .094 .075 .064 .047 .035 .018 1.009 16 13 11 8 6 3 1 .08 .16 .16 .62 .92 .52 .86 111 109 ]07 105 104 102 101 (Kirwan and Dalton.) Sp.gr. of HCl +Aq at 15. % HCl Sp. gr. % HCl Sp. gr. "t Pts. HCl in 1 pt. H 2 O t Pts. HCl in 1 pt. H 2 O 2.22 3.80 6.26 11.02 15.20 18.67 20.9] 23.72 25.96 .0103 .0189 .0310 .0557 .0751 1 . 0942 1.1048 1.1196 1 . 1308 ?9 . 72 31.50 34.24 36.63 38.67 40.51 41.72 43.09 1.1504 1 . 1588 1 . 1730 1 . 1844 1 . 1938 1.2021 1 . 2074 1.2124 - 5 -10 -15 -17 0.842 0.864 0.898 0.933 0.949 -18 -19 -20 -21 -24 0.957 0.965 0.974 0.983 1.012 (Roozeboom, R. t. c. 1884, 3. 79.) Solubility in H 2 O at t. (Kolb, C. R. 74. 337.) Sp. gr. of HCl +Aq at 15. t %HC1 Sp. gr. % HCl Sp. gr. % HCl Sp. gr. %HC1 50 45 40 35 30 20 15 10 5 - 5 -10 -50 -20 61.65 61.76 62.27 62.90 63.21 64.19 64.70 65.18 65.48 65.85 66.44 66.71 67.29 67.65 1 . 2000 1 . 1982 1 . 1964 1 . 1946 1 . 1928 1.1910 1 . 1893 1.1875 1 . 1859 1 . 1846 1 . 1822 1 . 1802 1 . 1782 1 . 1762 1.1741 1.1721 1 . 1701 1.1681 1.1661 1J641 40 40 39 39 39 38 38 37 37 37 36 36 35 35 34 34 33 33 33 777 369 961 554 146 738 330 923 516 108 700 292 884 476 068 660 252 845 437 029 .1620 . 1599 . 1578 .1557 . 1536 . 1515 .1494 .1473 . 1452 .1431 .1410 . 1389 .1369 .1349 .1328 . 1308 .1287 .1267 .1247 .1226 32.621 32.213 31 . 805 31.398 30 . 990 30 . 582 30.174 29 . 767 29.359 28.951 28.544 28.136 27.728 27.321 26.913 26.505 26 . 098 25 . 690 25 . 282 24.874 1 . 1206 1.1185 1.1164 1.1143 1.1123 1.1102 1 . 1082 1.1061 1.1041 1.1020 1 . 1000 1 . 0980 1 . 0960 1.0939 1.0919 1.0899 1.0879 1 . 0859 1.0838 1.0818 24 . 466 24 . 058 23 . 650 23 . 242 22 . 834 22.426 22.019 21 611 21.203 20.796 20.288 19.980 19 . 572 19.165 18.757 18.349 17.941 17.534 17.126 16.718 (Rupert, J. Am. Chem. Soc. 1909, 31. 860.) CHLORHYDRIC ACID 221 Sp. gr. of HCl+Aq at 15 Continued. Sp. gr. of HCl+Aq at 15. Sp. gr. % HCl Sp. gr. %HC1 Sp. er %HC1 HCl Sp. gr. HCl Sp. gr. ric. Sp " gr ' 1.0798 16.310 1.0778 15.902 1.0758 15.494 1.0738 15.087 1.0718 14.679 1.0697 14.271 1.0677 13.363 1.0657 13.456 1.0637 13.409 1.0617 12.641 1 . 0597 12 . 233 1.0577 11.825 1.0557 11.418 1.0537 11.010 1.0517 1 . 0497 .0477 .0457 .0437 .0417 .0397 .0377 .0357 .0337 .0318 1.0298 1 . 0279 10.602 10.194 9.768 9.379 8.971 8 . 563 8 . 1 5 7.747 7.340 6.932 6.524 6.116 5.709 1 . 0259 1 . 0239 1 . 0220 1 . 0200 1.0180 1.0160 1.0140 1.0120 1.0100 1 . 0080 1 . 0060 1 . 0040 1.0020 5.301 4.893 4.486 4 . 078 3.670 3.262 2.854 2.447 2.039 1.631 1.224 . 816 0.408 5 10 15 1.0244 1 . 0488 1.0733 20 25 30 1 0982 1.1234 1 . 1488 35 1 1739 40 1.1969 41 1.2013 (Hager, Adjumenta varia, Leipzig, 1876.) Sp. gr. of HCl+Aq at 15 (H 2 O at 15= 1). % HCl Sp. gr. %HC1 Sp. gr. (Ure, Hand? Sp. gr. of HCl+Aq. according to Ure; cording to Kremei /6i terbuc h.) . gr. at 15.55 gr. at 15 ac- U-sp K=sp s. 44. 43. 41. 41. 39. 37. 345 1.21479 136 1.21076 901 1.20430 212 1.20204 831 1.19703 596 1.18687 34.464 1.17138 25.260 1.12479 19.688 1.09675 14.788 1.07255 6.382 1.03150 %HC1 u K %HC1 u K 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 1.005 010 015 .020 .025 .030 .034 .039 .044 .048 .053 .059 .064 .069 .074 .079 1.084 1.089 1.094 1 098 1.104 .005 010 .015 020 .025 .030 1.034 1.039 1.044 1.048 1.053 1.059 1 065 1.070 1.075 1.080 1.085 1 090 1.095 1.100 1.105 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 1 109 1 114 1 119 1 124 1 128 1 133 1 138 1 143 1 147 1 153 1 157 1 163 1 169 1 174 1 179 1 183 1 188 1 193 1 197 1 203 1.111 1.116 1.121 1.126 1.131 1.136 1.141 1.146 1.151 1.157 1.163 1.169 1.179 (Pickering, B. 26. 277.) Most accurate table. Sp. gr. of HCl+Aq at 15 (H 2 O at 4= 1). Sp. gr. % HCl Kg. HCl in 1 . Sp. gr. % HCl Kg.HCl in 11. 1.000 1.0C5 1.010 1.015 1.020 1.025 1.030 1.035 1.040 1.045 1.050 1.055 1.060 1.065 1.070 1.075 1.080 1.085 1.090 1.095 1.100 0.16 1.15 2.14 3.12 4.13 5.15 6.15 7.15 8.16 9.16 10.17 11.18 12.19 13.19 14.17 15.16 16.15 17.13 18.11 19.06 20.01 0.016 0.012 0.022 0.032 0.042 0.053 0.064 0.074 0.085 0.096 0.107 0.118 0.129 0.141 0.152 0.163 0.174 0.186 0.197 0.209 0.220 1.105 1.110 1.115 1.120 1.125 1.130 1.135 1.140 1.145 1.15C 1.155 1.160 1.165 1.170 1.175 1.180 1.185 1.190 1.195 1.2CO 20.97 21.92 22 . 86 23.82 24.78 25.75 26.70 27.66 28.61 29.57 30.55 31.52 32.49 33.46 34.42 35.39 36.31 37.23 38.16 39.11 0.232 0.243 0.255 0.267 0.278 0.291 0.303 0.315 0.322 0.340 0.353 0.366 0.379 0.392 0.404 0.418 0.430 0.443 0.456 0.469 (Calculated by Gerlach, Z. anal. 8. 292.) Sp. gr. of HCl+Aq at 15 (H 2 O at = 1). HCl Sp. gr. , *; Sh Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 0.9992 1.00503 1.01005 1.01508 1.02010 1.02513 .03016 .03518 .04021 .04524 .05026 . 05529 .06031 1.06534 1.07037 15 1.07539 16 1.08042 17 1.08545 18 1.09047 19 1.09550 20 1.10052 21 1 . 10555 22 1.11058 23 1.11560 24 1.12063 25 1.12566 26 1 . 13068 27 1.13571 28 1 . 14074 29 1 . 14516 30 31 32 33 34 35 36 37 38 39 40 41 42 43 1 . 15079 1 . 15581 1 . 16084 1 . 16587 1 . 17089 1 . 17592 1 . 18095 1 . 18597 1.191 1.196 1.200 1.204 1.208 1.212 (Lunge and Marchlewski, Z. angew. Ch. 1891. 133.) Sp. gr. of HCl+Aq at room temp. %HC1 Sp. gr. 8.14 16.125 23.045 1.0370 1.0843 1.1138 (Kolb, recalculated by Gerlach, Z. anal. 27. 316.) (Wagner, W. Ann. 1883, 18. 264.) 222 CHLORHYDRIC ACID Relation of sp. gr. of HCl+Aq at t to sp. gr. at 19.5 = 1.0. t 8.9 % HC1 sp.gr. =1.0401 16 6 % HC1 sp. gr. =1.0704 25.5% HC1 sp. gr. =1.101 35.8% HCI sp. gr. =1.133 46.6 % HCI sp. gr. =1.1608 19.5 40 60 80 IOC 0.99557 1.00000 1.00707 1.01588 1.02639 1.03855 0.99379 .00000 .00781 .01665 .02676 .03801 0.99221 l.OOOCO 1.C0877 1.01794 1.02791 1.03867 0.99079 1.00000 1.00990 '1.01969 1.C2986 1.04059 0.98982 1.00000 1.01063 1.02180 (Kremers, Fogg. 108. 115.) Sp. gr. of HCl+Aq. Sp.gr. of HCl + Aq at 20. G. equivalents HCI per liter. t Sp. gr. t/t Normality of HCl+Aq. % HCI. Sp. gr. 0.005036 0.01006 6. 02008 0.04990 0.09885 0.19641 0.29247 0.48278 0.4994 4.994 17.111 17.125 17.148 17.138 17.133 17.162 17.147 17.140 17.28 17.35 . 0000943 .0001892 .0003775 .000935 .001843 .003633 .005382 .008811 1.00908 1.08390 8.42 5.784 3.77 2.031 1.588 1.138 0.523 27.10 19.30 12.94 7.17 5.65 4.05 1.90 .1336 .0936 .0618 .0334 .0261 1.0187 1.0076 (Forchheimer, Z. phys. Ch. 1900, 34. 28.) Sp. gr. at 20 of HCl+Aq containing M g. mols. HCI per liter. M 0.025 0.05 0.075 0.10 Sp.gr. 1.00034 1.00101 1.00135 1.00180 (Kohlrausch, W. Ann. 1894, 53. 28.) Sp. gr. of a normal solution of HCl+Aq at 18/4= 1.0165. CLoomis W Ann ISQft v*V** \-**ns\jmta* TT . -tiiAiJ., J.O7v/j Sp. gr. of HCl+Aq at 19.5, when p =per cent strength of solution; d= observed density; w = volume cone, in grams M Sp. gr. 0.25 1 .00425 0.50 1.00849 0.75 1.01264 1.0 1.01749 P er cc - ^ = M 1.5 2.0 Sp.gr. 1.02542 1.03414 (Jones and Pearce, Am. Ch. J. 1907, 38. 730.) p- d. W 36.0 .1818 0.4255 29.97 .1511 0.3450 24.35 .1207 0.2729 18.55 .0910 2024 12 22 .0587 0.1294 9.148 1 0433 0.0954 6.559 1.0305 0.0676 3.540 1.0159 0360 5.345 1.356 1.0246 1.0G51 0.0548 0.0136 (Barnes, J. Phys. Chem. 1898, 2. 546.) Sp. gr. of HCl+Aq at 18/4. g. HCI in 100 g. of solution Sp. gr. 0-12149 O.C60757 0.040609 0.030328 0.99928 0.99900 0.9988V 99881 (Jahn, Z. phys. Ch. 1900, 33. 567.) HCI is not absorbed by cone. H 2 SO 4 +Aq / but in large amounts by anhydrous H 2 SO 4 (Aime.) Absorption of HCI by H 2 SO 4 +Aq. Temp. = 17. g. per 1. g. per 100 g. Sp. gr. HCI H 2 S0 4 HCI H 2 SO4 1.211 517.8 42.7 1.220 487.3 '22^7 39.9 Y.86 1.220 478.8 58.0 39.2 4.75 1.235 455.3 99.3 36.9 8.04 1.260 418.0 161.7 33.2 12.8 1.305 371.4 273.2 28.5 20.9 1.355 306.6 417.7 22.6 30.8 1.430 215.3 638.2 15.0 44.6 1.545 96.7 917.6 6.26 59.4 1.580 51.3 1033.5 3.25 65.4 1.660 10.3 1224.0 0.62 73.7 1.735 1.89 1344.9 0.11 77.5 1.815 1.24 1615.3 0.068 89.0 CHLORHYDRIC ACID 223 Absorption of HC1 by H 2 SO 4 +Aq Cont. Temp. = 40. gr. .185 .195 .210 .255 .255 ,340 ,400 ,520 575 1.650 1.725 1.755 1.770 ff. per 1. 421.4 416.4 392.1 346.3 325.4 247.4 161.6 50.9 18.5 2.9 1.4 0.57 0.52 HS04 42.2 70.0 107.7 211.2 236.3 383.7 619.4 929.3 1046.0 1207.6 1370.5 1428.4 1478.4 g. per 100 g HC1 35.6 34.8 32.4 27.6 25.9 18.5 11.5 3.35 1.17 0.17 0.081 0.032 0.029 H 2 S0 4 3.5 5.8 8.9( 16.8 18.8 28.6 44.2 61 .'1 66.4 73.2 79.4 81.4 83.5 Temp. =70. gr. 145 150 160 180 225 230 315 1.380 510 560 700 745 1.745 HCl 374.1 357.3 353.8 341.3 277.7 274.3 173.7 96.5 23 6 8.4 0.86 0.62 0.57 H 2 S0 4 18.4 38.9 55.7 93.6 231.9 246.4 476.7 661.8 946.1 1055.0 1371.3 1448.2 1455.2 g. per 100 g. HCl 32.7 31.1 30.5 28.9 22.8 22.3 13.2 6.99. 1.56 0.54 0.05 0.035 0.032 H 2 S0 4 1.61 3.38 4.80 7.93 18.9 20.0 36.2 48.0 62.7 67.6 80 ..7 83.0 83.4 (Coppadoro, Gazz. ch. it. 1910, 39. II, 626.) 100 pts. alcohol of 36 B absorb 68 pts. HCl at 12.5. (Boullay.) Alcohol of 0.836 sp. gr. dissolves 327 vols. HCl at 17.5 and 758 mm. pressure, and the solution has sp. gr.= 1.005. (Pierre, A. ch. (3) 31. 135.) Solubility of HCl in methyl alcohol (absolute) att. t % HCl t % HCl -10.3 54.6 18 46.9 51.3 31.7 43 (de Bruyn, R. t. c. 11. 112.) Solubility of HCl in ethyl alcohol (absolute) at t. t % HCl t %HC1 6.5 11.5 45.4 44.2 42.7 19.2 23.5 32.0 41 40.2 38.1 (de Bruyn, l.c .) Solubility of HCl in ether at t and 760 mm. pressure. t %HC1 t % HCl 9.2 37.51 15 27.62 5 37.0 20 24.9 35.6 25 22.18 + 5 33.1 30 19.47 10 30.35 (Schuncke, Z. phys. Ch. 1894, 14. 336.) Sol. in glacial HC 2 H 3 O 2 , ether, hexane, benzene, xylene, etc. Oil of turpentine absorbs 50% HCl (Thenard.) Oil of turpentine absorbs 163 vols. HCl at 22 and 724 mm.; isoterebenthene absorbs 34% at 24 and 724 mm.; metaterebenthene absorbs 17.7% at 24 and 724 mm. (Berthe- lot.) Oil of lavender absorbs 68.7 vols at 24 (Thfnard.) Oil of lavender absorbs 210 vols. without being saturated; oil of rosemary absorbs 218 vols. at 22; sol. in 0.4 vol. petroleum. (Saussure.) Absorbed by caprylic alcohol. (Bouis.) Fuming HCl-fAq is sol. in glycerine and miscible with cone. HC 2 HO 2 . Solubility of HCl in phenol -f-Aq at 12. Comp. of H2O layer HCl 3.1 6.6 8.0 10.7 % phenol 7.45 6.6 5.3 5.1 4.8 Ccmp. of phenol layer % HCl 0.09 0.2 0.36 0.52 % phenol 72 7g 80.3 82.6 84.5 Composition of solution in contact with solid phenol. H 2 O 11.22 14.98 84.5 80.38 72.43 60.25 HCl C.52 10.7 15.64 24.37 36.25 % phenol 88.78 84.5 4.8 3.98 3.2 3.5 Schreinemakers, Z. phys. Ch. 1912, 79. 553.) +H 2 O. F.-pt.- 15.35. Very sol. in H 2 O but only slightly sol. in HCl. (Rupert, J. Am. Chem. Soc. 1909, 31. 66.) +2H 2 O. M.-pt.~17.4 c . +3H 2 O. M.-pt.-24.8. (Pickering, B. 893, 26. 280.) The composition of the hydrates formed y HCl at different dilutions is calculated 224 CHLORHYDRIC CYANHYDRIC ACID from determinations of the lowering of the Solubility of Ba(ClO 3 ) 2 in H 2 O. f.-pt. produced by HC1, and of the conduc- tivity and sp. gr. of HCl+Aq. (Jones, Am. t g. Ba(ClO 3 )2 in Sp. gr. Ch. J. 1905, 34. 323.) 100 g. H 2 O Chlorhydric cyanhydric acid, 3HC1, 2HCN. 25.5 1.195 Decomp. by H 2 O or alcohol; sol. in HC2H 3 O 2 . Insol. in ether, chloroform, or 20 40 39.3 55.9 1.274 1.355 acetic ether. (Claisen, B. 16. 309.) 60 74.1 1 . 433 HC1, HCN. Sol. in H 2 O, absolute alcohol, 80 92.1 1.508 HC 2 H 3 O 2 , and CHC1 3 , with decomp.; de- comp. is especially rapid in H 2 O. (Gautier, 100 105.6* 113.2 120. 1.580 1.600 A. ch. (4) 17. 130.) * Rnt. nf sfl.f. anl lit/inn Chloric acid, HC1O 3 . Known only in aqueous solution, which can be concentrated in vacuo to a sp. gr. of 1.282 at 14.2, and then contains 40.10% HC1O 3 , corresponding to HC1O 3 +7H 2 O; if left longer in vacuo over H 2 SO 4 an acid corresponding to HC1O 3 +4KH 2 O is obtained. Aqueous solu- tion of HCir 3 decomp. at 40. (Kammerer, Pogg. 138. 390.) Chlorates. All chlorates except mercurous chlorate are sol. in H 2 O; most of them are deliquescent; many are sol. in alcohol. Aluminum chlorate, A1(C10 3 ) 3 +6H 2 O. Very hygroscopic. (Dobroserdow, G. C. 1904, II. 177.) +9H 2 O. Very sol. in cold but much less than in hot H 2 O. (Dobroserdow.) Ammonium chlorate, NH 4 C1O 3 . Easily sol. in H 2 O; less sol. in alcohol. Much less sol. in H 2 O at than NaC10 3 . (Storer.) Very si. sol. in absolute alcohol. (Wachter, J. pr. 30. 321.) Barium chlorate, Ba(ClO 3 ) 2 -hH 2 O. Sol. in 4 pts. cold, and less hot H 2 0. (Chevenix.) 100 pts. H 2 O dissolve at: 20 40 60 80 1CO 22.8 37.Q 52.1 77.5 98.0 126.4 pts. Fa(ClO 3 ) 2 . 100 grams sat. Ba(ClO 3 ) 2 +Aq at t con- tain grams anhydrous Ba(ClO 3 ) 2 . t Grams Ba(C10 3 )2 t Grams Ba(ClO 2 )a Eutectic point. -2.749 0.004 +10 20 25 30 40 15.28 16.90 21.^3 25.26 27.53 29.43 33.16 50 60 70 80 90 99.1 "104.6 36.69 40.05 43.04 45.90 48.70 51.17 52.67 * 104.6 is bpt. at 740 mm. pressure= 105.0 at 760 mm. pressure. (Anschutz, Z. phys. Ch. 1906, 56. 238.) (Carlson, Dissert. 1910.) Only slight traces dissolve in absolute alcohol. (Wachter, J. pr. 30. 334.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethylacet ate (Naumann, B. 1910, 43. 314.) Bismuth chlorate. Known only in solution, which decomp. on evaporation. Cadmium chlorate, Cd(ClO 8 ) 2 +2H 2 O. Very deliquescent; sol. in H 2 O and alcohol. Melts in crystal H 2 O at 80. (Wachter, J. pr. 30.321.) ' Solubility in H 2 O. Sat. solution contains at: -20 72.18 49 80.08 -15 72.53 74.95 + 18 76.36 65 82.95% Cd(ClO 3 ) 2 . Sp. gr. of solution containing 76.36% Cd(ClO 3 ) 2 at 18 =2.284. (Meusser, B. 1902, 35. 1422.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Cadmium chlorate ammonia, Cd(ClO 3 ) 2 , 6NH 3 . Ppt. (Ephraim, B. 1915, 48. 49.) Caesium chlorate, CsClO 3 . 100 g. H 2 O dissolve at: 8 19.8 30 42.2 2.46 3.50 6.28 9.53 14.94 50 77 99 19.40 41.65 76.5 g. CsClO 3 . (Calzolari, Ace. Sc. med. di Ferrara, 1911, 85. 150.) Calcium chlorate, Ca(ClO 3 ) 2 -f 2H 2 O. Deliquescent; very sol. in H 2 O and alcohol. (Wachter, J. pr. 30. 323.) CHLORATE, MAGNESIUM 225 Melts in its water of crystallization at over 100. Sp. gr. of solution sat. at 18 = 1.729, con- taining 64% Ca(ClO 8 ) 2 . (Mylius B. 1897, 30. 1718.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Chromic chlorate. Easily sol. in H 2 O. (Prudhomme, C. C. 1890, 1. 668.) Cobaltous chlorate, Co(ClO 3 ) 2 +2H 2 O. (Meusser, B. 1902, 35. 1418.) +4H 2 O. Solubility in H 2 O. Sat. solution contains at: 18 21 35 47 61 64.19 64.39 67.09 69.66 76.12% Co(GlO 3 ) 2 . Sp. gr. of solution containing 64.19% Go(ClO 3 ) 2 at 18 = 1.861. (Meusser, B. 1902, 35. 1418.) +6H 2 O. Very deliquescent. Sol. in H 2 O and alcohol. Melts in crystal H 2 O at 50. (Wachter, J. pr. 30. 321.) Solubility in H 2 O. Sat. solution contains at: -21 -19 +10.5 53.30 53.61 57.45 61.83% Co(ClO 3 ) 2 . (Meusser, B. 1902, 35. 1418.) Cupric chlorate, basic, Cu(ClO 3 ) 2 , 3Cu(OH) 2 . Insol. in H 2 O. Very sol. in dil. acids. Sol. in warm cone. Cu(ClO 3 ) 2 +Aq, the solubility increasing with the cone, and temp. (Bour- geois, Bull. Soc. 1898, (3) 19. 950.) Cupric chlorate, Cu(ClO 3 ) 2 +4H 2 0. Solubility in H 2 O. Sat. solution contains at: -31 -21 54.59 57.12 +0.8 18 45 58.51 62.17 66.17 59.6 71 69.42 76.9% Cu(ClO 3 ) 2 . Sp. gr. of the solution containing 62.17% Cu(C10 8 ) 2 at 18 = 1.695. (Meusser, B. 1902, 35. 1420.) +6H 2 O. Very deliquescent. Easily sol. in H 2 O and alcohol. Melts in its crystal H 2 O at 65. (Wachter, J. pr. 30. 321.) Sp. gr. of Cu(ClO 3 ) 2 +Aq at 15. %Cu(C10 3 ) 2 2.106 4.778 6.945 Sp. gr. 1.01620 1.03857 1.05714 Cu(ClO 3 ) 2 10.016 14.387 p. gr. 1.0844 1.12531 (Traube, Gm.-K. 6. 1, 921.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Cupric chlorate ammonia, Cu(ClO 3 ) 2 , 4NH 3 . Ppt. Not hydroscopic. Insol. in alcohol. Cu(ClO 3 ) 2 ,6NH 3 . Not hydroscopic. (Eph- raim, B. 1915, 48. 46.) Erbium chlorate, Er(ClO 3 ) 3 +8H 2 O. Deliquescent. Sol. in H 2 O and alcohol. Glucinum chlorate. Known only in aqueous solution, which de- composes on evaporation. Ferrous chlorate. Known only in solution. Ferric chlorate, Fe(ClO 3 ) 3 . Sol. in H 2 O. Basic salt. Insol. in H 2 O. Lanthanum chlorate, La(ClO 3 ) 3 . Deliquescent. (Cleve.) Lead chlorate, Pb(ClO 3 ) 2 +H 2 O. Deliquescent; easily sol. in H 2 O and alcohol. (Wachter, J. pr. 30. 321.) Sp. gr. of solution sat. at 18 = 1.947 and contains 60.2% Pb(ClO 3 ) 2 . (Mylius, B. 1897, 30. 1718.) ICO g. H 2 O dissolve 440 g. Pb(ClO 8 ) 2 at 18; sp. gr. of sat. solution = 1.63. (Carlson, Dissert. 1910.) Lithium chlorate, LiClO 3 +^H 2 O. Very deliquescent and sol. in H 2 O. Very easily sol. in alcohol. Melts at 50 in its crystal water. (Wachter, J. pr. 30. 321.) LiClO 3 +Aq sat. at 18 contains 75.8% LiClO 3 . Sp. gr. = 1.815. (Mylius, B. 1897, 30. 1718.) 483 g. LiClOs dissolve in 100 g. H 2 O at 15; sp. gr. of solution = 1.82. (Carlson, Dissert. 1910.) Contains 3H 2 O, and is not deliquescent. (Lagorip, Zeit. f. Kryst. 16. 80.) Salt is anhydrous. (Retgers, Z. phys. Ch. 5. 449.) Magnesium chlorate, Mg(ClO 3 ) 2 . 128.1 g. Mg(ClO 3 ) dissolve in 100 g. H 2 O at 19; sp. gr. of solution = 1.59. (Carlson, Dissert. 1910.) Sp. gr. of solution containing 56.5% Mg(C10 3 ) 2 at 18 = 1.564. (Meusser, I.e.) Sp. gr. of solution sat. at 18 = 1.594, con- taining 56.3% Mg(ClO 3 ) 2 . (Mylius, B. 1897, 30. 1718.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) +2H 2 O. Solubility in H 2 O. Sat. solution contains at: 39.5 61 68 93 65.37 69.46 70.69 73.71% Mg(ClO 3 ) 2 . (Meusser, B. 1902, 36. 1416.) 226 CHLORATE, MANGANOUS +4H 2 O. Solubility in H 2 0. Sat. solution contains at: 42 65.5 63.82 69.12% Mg(ClO 3 ) 2 . (Meusser, I.e.) +6H 2 O. Very deliquescent and sol. in H 2 O. Very easily sol. in alcohol. Melts at 40 in its crystal water. (Wachter, J. pr. 30. 325.) Solubility in H 2 O. Sat. solution contains at: -18 +18 29 35 51.64 53.27 56.50 60.23 63.65% Mg(C10 8 ) 2 . (Meusser) Manganous chlorate, Mn(C10 3 ) 2 . Known only in solution which decomposes on evaporation. (Wachter.) Mercurous chlorate, Hg 2 (ClO 3 )2. o. Easily sol. in alcohol and H 2 0. (Wach- ter, J. pr. 30. 321.) /8. Insol. in H 2 0; easily sol. in HC 2 H 3 O 2 + Aq. (Wachter.) Decomp. by boiling H 2 O. Mercuric chlorate, 2HgO, C1 2 O 6 +H 2 O. Deliquescent. Decomp. by H 2 O into oxide and an acid salt. (Wachter.) Sol. in 4 pts. cold H 2 O. (Chevenix, 1802.) Nickel chlorate, Ni(ClO 3 ) 2 +4H 2 O. Solubility in H 2 O. Sat. solution contains at: 48.5 55 65 79.5 67.60 68.78 69.05 75.50% Ni(ClO,) 2 . (Meusser, B. 1902, 35. 1419.) +6H 2 O. Deliquescent. Easily sol. in H 2 O and alcohol. Melts in crystal H 2 O at 80. "(Wachter, J. pr. 30. 321.) Solubility in H 2 O. Sat. solution contains at: ' ; /.; -18 -8 +18 40 49.55 51.52 52.66 56.74 64.47% Ni(ClO 3 ) 2 . Sp. gr. of solution containing 56.74% Ni(C10 3 ) 2 atl8 Goes over into 4H 2 O salt at 39. (Meusser.) 156 g. Ni(ClO 3 ) 2 dissolve in 100 g. H 2 O at 16; sp. gr. of solution = 1.76. (Carlson, Dis- 1910. t ... 28 3 5 4.0 2.3 14.4 47 65 18.3 29.1 Pts. KClOs . . 9.5 1 (Gerardin.) ' 100 pts. H 2 O dissolve pts. KClOs -at t. t Pts. KC1O 3 t Pts. KClOs 12.05 18.96 35.40 60 . 24 ' 13.32 15.37 24.43 3.33 5.60 6.03 8.41 35.0 49.08 74.89 104 . 78 (Gay-Lussac, A. ch. 11. 314.) 100 pts. H 2 O dissolve pts. KC1O 3 at t. t Pts. KClOs t Pts. KClOs 100 3.3 56.5 130 180 88.5 190 sert. .) JNickel chlorate ammonia, Ni(ClO 3 ) 2 , 6NH 3 . Ppt. (Ephraim, B. 1915, 48. 47.) Potassium chlorate, KC1O 3 . Sol. in H 2 O with absorption of heat. Sol. in about 16 pts. cold, and in much less hot H 2 O (Chevenix, 1802.) Sol. in 30.03 pts. H 2 O at 0; 17.85 pts. at 13.3; and n 1.66 pts. .at 104.78. , (M. R. and P, .) Sol. in 16 pts. H 2 O at 18.75. (Abl.) 100 pts. HsO at 15.5 dissolve 6.2 pts.; at 100, 40 pts. (Ure's Diet.) 100 pts. H 2 O dissolve pts. KClOs at t- (Tilden and Shenstone, Roy. Soc. Proc. 35. 345.) 100 pts. H 2 O dissolve pts. KC1O 3 at t. t Pts. KClOs t Pts. KClOs 120 136 73.7 98.9 160 190 148 183 (Tilden and Shenstone, Phil. Trans. 1884. 23.) Coefficient of solubility is 3.2+0.109t+ 0.0043t2 between and 35. (Blarez, C. R. 112. 1213.) Sat. KClO 3 +Aq contains % KC10 3 at t. t % KClOs t % KClOs -0.5 2.6 92 31.2 -0.3 2.4 106 37.2 +4.5 3.5 130 47.0 4.5 2.9 171 , 59.8 11 4.7 180 62.1 19 6.1 190 63.1 29 8.9 200 64.2 36 9.9 207 66.0 42 11.4 300 87.0 56 15.1 330 96.7 58 16.6 ' Cfitard, A. ch. 1894, (7) 2. 528.) CHLORATE, MANGANOUS 227 Solubility in H 2 O. Temp. % KC10 3 in a sat. sol. Pts. sol. in 100 pts. H 2 O Pts. H 2 O to 1 pt. KClOs 3 06 3.14 31.8 5 3.67 3.82 26.2 10 4.27 4.45 22.5 15 5.11 5.35 18.5 20 6.76 7.22 13.6 25 7.56 8.17 12.2 30 8.46 9.26 10.8 35 10.29 11.47 8.7 40 11.75 13.31 7.5 45 13.16 14.97 6.6 50 15.18 17.95 5.6 55 16 85 20.27 4.9 60 18.97 23.42 4.2 65 20.32 25.50 3.9 70 22.55 29.16 3.4 75 24.82 32.99 30 80 26.97 36.93 2.6 85 29.25 41.35 2.4 90 31.36 46.11 2.1 95 33.76 . 51.39 1.9 100 35.83 55.54 1.8 (Pawlewski, B. 1899, 32. 1041.) 1 1. KClO 3 +Aq at 25 contains 675 milli- mols. KC10 3 . (Calvert, Z. phys. Ch. 1901, 38. 541.) 100 g. H 2 O dissolve at: 20 40 60 3.3 7.4 13.8 24.0 g. KC1O 3 Sp. gr. 1.021 1.045 1.073 1.115 80 100 104 * 37.7 56.5 59.9g.KC10 3 , Sp.gr. 1.165 1.219 1.230 * Bpt. of sat. solution. (Carlson, Dissert. 1910.) 100 g. H 2 O dissolve at: 8 19.8 30 99 4.48 7.15 10.27 57.3 g. KC1O 3 . (Calzolari, Ace. Sc. med. di Ferrara, 1911, 85. 150.) Sat. KClO 3 +Aq contains at: 53 68 81 86(?) 17.37 23.25 23.53 30.46% KC1O 3 . (Tschugaeff, Z. anorg. 1914, 86. 161.) Sp. gr. of KClO 3 +Aq, according to Kremer's experiments (Pogg. 96. 62), and Gerlach's calculations. (Z. anal. 8. 290.) % KClOs Sp. gr. % KClOs Sp. gr. 1 1.007 6 1.039 : 2 1.014 7 1.045 3 1.020 8 1.052 4 1.026 9 1.059 5 1.033 10 1.066 Sp. gr. of KC10 3 +Aq at 20 containing 1 mol. KC1O 3 to 100 mols. H 2 O = 1.04122. (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of KClOs+Aq at 15 containing 5% KC1O 3 = 1.0316. (Kohlrausch, W. Ann. 1879. 1.) B.-pt. of KClOa+Aq containing pts. KC1O 3 .;.'>: to 100 pts. H 2 O. Pts. KClOs B.-pt, Pts. KClOa B.-pt. 6.5 13.2 20.2 27.8 35.8 100.5 101.0 101.5 102.0 102.5 44.6 53.4 62.2 69.2 103.0 103.5 104.0 104.4 (Gerlach, Z. anal. 26. 450.) Saturated solution boils at 105. (Kremers.) Saturated solution boils at 104.2, and con- tains 61.5 pts. KC1O 3 to 100 pts. H 2 O. (Legrand.) Saturated solution boils at 103.3, and con- tains 66.6 pts. KC10 3 to 100 pts. H 2 O. (Grif- fiths.) Saturated solution boils at 104.4. (Ger- lach, Z. anal. 26. 427.) Sol. in pure HNO 3 without decomp., but decomp. at once by HNO 3 containing NO 2 . (Millon, A. ch. (3) 6. 92.) Sol. in sat. NH 4 Cl+Aq without causing pptn. 1 mol. ( = 129 pts.) KC1O 3 dissolves in 2493 vols. H 2 O; in 2208 vols. H 2 O when 1 mol. ( = 59 pts.) NaCl is added; in 2060 vols. H 2 O with 2 mols. ( = 118 pts.) NaCl; and in 1910 vols. H 2 O with 4 mols. (=236 pts.) NaCl. (Gladstone, Chem. Soc. 16. 302.) KC1O 3 is sol. in about 29.50 pts. H 2 O. 35.50 pts. NH 4 OH+Aq cone. . 39.00 pts. dil. NH 4 OH+Aq (1 vol. cone.: 3 vols. H 2 O). 30.50 pts. HNOa+Aq (1 vol. cone. HNO 3 : 5 vols. H 2 O). 33.0 pts. HCl+Aq (1 vol. cone. HC1: 4 vols. H 2 0). 48.00 pts. HC 2 H 3 O 2 +Aq (1 vol. commer- cial HC 2 H 3 O 2 :1 vol. H 2 0). 31.50 pts. NH 4 Cl+Aq (1 pt. NH 4 C1:10 pts. H 2 O). 18.00 pts. NH 4 NO 3 +Aq (1 pt. NH 4 NO 3 :10 pts. H 2 O). 34.00 pts. NH 4 C 2 H 3 2 +Aq (dil. NH 4 OH + Aq+dil. HC 2 H 8 2 +Aq). 32.50 pts. NaC 2 H 3 O 2 -f-Aq (commercial HC 2 H 3 O 2 +Na 2 CO 3 , diluted with 4 vols. H 2 O). 31.50 pts. Cu(CjH|Oi)+Aq. (See Stolba, Z. anal. 2. 390.) 33.50 pts. cane-sugar (1 pt. cane-sugar : 10 pts. H 2 O). 36.50 pts. grape-sugar (1 pt. grape-sugar: 10 pts. H 2 O). (Pearson, Zeit. Chem. 1869. 662.) Addition of K salts to sat. KClO 3 -f-Aq ppts. KC1O 3 in such a way, that the sum of the 228 CHLORATE, MANGANOUS KC10 3 remaining in solution and the K in the salt added, is a constant, which constant is equal to the solubility of KC1O 3 , so that the following formula represents the coefficiency of solubility of KC1O 3 after addition of a K salt, 3.2+0.109t+0.0043t 2 -K of salt added. (Blarez, C. R. 112. 1213.) Solubility of KC1O 3 +T1C1O 3 . Solubility in KOH+Aq at 25 o KOH +Aq Millimols KClOs per litre of the solulion Vs-normal ^-normal 624 573 (Calvert, Z. phys. Ch. 1901, 38. 541.) Solubility in H 2 O 2 at 25. 100 g. H 2 O dissolve g. salts t g. TIClOs g. KClOs Concentration of H 2 C>2 millimols per litre Millimols KClOa per litre of the solution 15 50 100 2.8 10 12.67 57.3 3.3 1.5 16.2 48.2 1260 1310 730 737 (Calvert, I.e.) Solubility in l / normal KOH+Aq iD presence of H2O2 at 25. (Rabe, Z. anorg. 1902, 31. 156.) Solubility of KC1O 3 in KNO 3 +Aq. t g. per 1. Concentration of EbOz millimols per litre Millimois KClOs per lit.re of the solution KNO 3 KC10 3 15 276 954 1073 578 584 616 673 19.85 0.00 69.88 12.65 64.86 25.29 60.33 101.19 45.85 202.38 40.20 (Calvert, I.e.) Moderately sol. in liquid NH 3 . (Franklin. Am. Ch. J. 1898, 20. 828.) Neither dissolved nor attacked by liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) Sol. in 120 pts. alcohol of 83% at 16. (Wittstein.) Sol. in 120 pts. alcohol of 77.1%. (Pohl, W. A. B. 6. 595.) Insol. in absolute alcohol. (Gerardin.) Solubility of KC1O 3 in dil. alcohol. D = sp. gr. of alcohol; S = solubility in 100 pts. alcohol at t. 23.87 0.00 79.09 50.59 63.14 (Arrhenius, Z. phys. Ch. 1893, 11. 397.) Solubility in KCl+Aq at 20 C. G. KCl in 1 litre G. KC10 3 in 1 litre Sp. gr. 10 20 30 40 50 60 70 80 90 100 110 120 130 140 150 160 170 180 190 200 210 220 230 240 250 71.1 58 49 43 39.5 36.5 34 32 30 28 27 25.5 24.5 23.5 22.5 21.5 21.0 20.5 20.0 20.0 20 20 20 20 20 20 1.050 .050 .050 .050 .054 .058 .064 .070 .075 .081 .086 .091 .098 1.103 1.108 1.113 1.119 1.124 1.130 1.135 1.140 1.145 1.150 1.156 1.161 1.168 D =0.9904 D =0.9848 D =0.9793 t s 49 63 75 9.1 10.2 13.6 16.2 t 14 26 39 47 55 65 66 s 4.7 7.1 9.3 12.8 16.1 22.3 22.5 t g 13 21 25 30 35 44 50 14 26 38 46 51 63 65 3.2 5.4 7.9 10.8 12.2 17.5 19.0 D =0.9726 D =0.9573 D =0.9390 t s t s t s 13 20 33 43 56 59 2.2 3.3 5.8 7.2 11.4 12.9 13 20 29 36 55 60 63 1.9 2.7 3 6 4.3 7.9 9.7 10.5 14.5 28 40 50 62 67 1.1 2.2 3.4 4.3 6.6 7.6 (Winteler, Z. Elektrochem. 1900, 7. 361.) CHLORATE, SODIUM 229 Solubility of KCIO 3 in dil. alcohol -Continued. Potassium silver chlorate, KC1O 3 , AgClO 3 . D =0.9111 D = =0.8967 D =0.8429 (Pfaundler, W. A. B. 46, 2. 266.) t s t S t s Rubidium chlorate, RbClO 3 . 13 25 32 52 0.74 1.08 1.78 3.35 12 31 43 58 6.46 25 1.28 34 1.95 56 3.10 64 0.09 0.12 0.24 0.32 100 pts. H 2 O dissolve 2.8 pts. at 4.7; 3.9 pts. at 13; 4.9 pts. at 18.2; 5.1 pts. at 19. (Reissig, A. 127. 33.) 100 g. H 2 O dissolve 3.1 RbClO 8 at 15; sp. gr. of solution = 1.07. (Carlson, Dissert. (Gerardin, A. ch. (4) 6. 148.) 1910.) 100 g. H 2 O dissolve at: Solubility of KC1O 3 in alcohol +Aq. 8 19.8 30 wt. % alcohol g. KC1O 3 per 100 g. solution 2.138 3.07 5.36 8.00 g. RbClO 8 , t=30 t=40 42.2 50 76 99 12.48 15.98 34.12 62.8 g. RbClO 3 . 5 9.23 7.72 12.23 10.48 (Calzolari, Ace. Sc. med. di Ferrara, 1911, 86. 10 6.44 8.84 ; 2 n 4.51 6.4C V 30 3.21 4^67 Scandium chlorate. 40 2.35 3.41 (Crookes, Roy. Soc. Proc. 1908, 80. A, 518.) 50 1.64 2.41 60 1.01 4.41 Silver chlorate, AgClO 3 . 70 80 90 0.54 0.24 G.06 0.78 0.34 0.12 Sol. in 10-12 pts. cold H 2 O (Vauquelin); in 8-10 pts. cold, and 2 pts. hot H 2 O (Chev- enix); in 5 pts. cold H 2 O (Wachter). SI. sol. in alcohol (Chevenix); easily sol. in alcohol (Wachter). (Taylor, J. phys. Ch. 1897, 1. 301.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Very si. sol. in acetone. (Krug and M'El- roy, J. Anal. Ch. 6. 184.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Solubility of KC10 3 in acetone +Aq. wt. % acetone g. KClOs per 100 g. solution t =30 t =40 ' 9.23 12.23 5 8.32 11.10 9.09 7.63 10.28 20 6.09 8.27 30 4.93 6.69 40 3.90 5.36 50 2.90 4.03 60 2.03 2.86 70 1.24 1.68 80 0.57 0.79 90 0.18 0.24 (Taylor, J. phys. Ch. 1897, 1. 301.) Insol. in methyl acetate. (Naumann, B 1909, 42. 3790); ethyl acetate. (Naumann B. 1904, 37. 3601.) Solubility in glycol = 0.9% at ord. temp (de Coninck, Belg. Acad. Bull. 1905. 359 ) 100 g. glycerol (sp. gr. 1.256) dissolve 3.54 g KC1O 3 at 15-16. (Ossendowski, Pharm. J 1907, 79. 575.) Silver chlorate ammonia, AgClO 3 , 2NH 3 . Easily sol. in H 2 O or alcohol. (Wachter, 1843.) Sodium chlorate, NaC10 3 . Deliquescent. Sol. in 3 pts. cold and less hot H 2 O. (Wachter; Chevenix.) Sol. in 3 pts. H 2 at 18.75. (Abl.) 100 pts. H 2 O dissolve 35.5 pts. NaClOs. (Ure's Diet.) 100 pts. H 2 O dissolve at: 20 40 60 81.9 99 123.5 147.1 pts. NaC10 3 , 80 100 120 175.6 232.6 333.3 pts. NaClO 3 . (Kremers, Pogg. 97. 4.) 100 pts. H 2 O dissolve 89.3 pts. NaClO 3 at 12 C . (Schlosing.) ICO g. H 2 O dissolve at: -15 20 40 72 79 101 126 pts. NaClO 3 , Sp.gr. 1.380 1.389 1.430 1.472 60 80 100 122* 155 189 230 286 pts. NaClO 3 . Sp.gr. 1.514 1.559 1.604 1.654 * Bpt. of sat. solution. (Carlson, Dissert. 1910.) 230 CHLORATE, SODIUM 100 g. NaC10 3 +Aq contain at: 4.78 19.85 30.05 35.10 44.72 45.47 48.91 51.22 52.36 54.50 g. NaClO 3 . (Le Blanc and Schmandt, Z. phys. Ch. 1911, 77. 614.) Sp. gr. of NaClO 3 +Aq, containing: 10 15 20 25 30 25% NaClO 3 . 1.070 1.108 1.147 1.190 1.235 1.282 (Gerlach, Z. anal. 8. 290.) Sp. gr. of NaClOs+Aq at 20 containing 1 mol. NaClO 3 in 100 mols. H 2 O = 1.03844. (Nicol, Phil. Mag. (5) 16. 122.) NaClO 3 +Aq containing 7.23% NaClO, has sp. gr. 20 /20 = 1.0496. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) Sat. solution boils at 132, and temp, can be raised to 135 by supersaturation. (Krem- ers, Pogg. 97. 4.; Easily sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) NaClOa+NaCl. 100 pts. H 2 O dissolve 50.75 pts. NaClO 3 + 24.4 pts. NaCl at 12; ICO pts. H 2 O dissolve 249.6 pts.NaC10 3 +11.5 pts. NaCl at 122, and when cooled to 12 contain 68.6 pts. NaClO 3 +11.5 pts. NaCl. (Schlosing, C. R. 73. 1272.) Solubility in NaCl+Aq at 20 C. G. NaCl in 1 litre G. NaClOs in 1 litre Sp. gr. 5 668 1.426 10 661 1.424 15 653 1 423 20 645 1.421 25 638 1.419 30 630 1.418 35 622 1.417 40 615 1.415 45 607 1.414 50 599 1.412 55 590 1.411 60 582 1.409 65 574 1.408 70 566 1.406 75 559 1.405 80 551 1.404 85 544 .402 90 537 .401 95 529 .399 100 522 .398 105 514 .396 110 507 .394 115 499 .392 120 491 .391 125 484 .389 130 476 .387 135 467 .385 140 459 .383 145 451 .381 Solubility in NaCl+Aq at 20 C. Continued G. NaCl in 1 litre G. NaClOs in 1 litre Sp. gr. 150 442 1.379 155 432 1.377 16C 423 1.374 165 414 1.372 170 403 1.369 175 393 1.365 180 382 1.362 185 371 1.359 190 360 1.355 195 349 1.350 200 338 1.345 205 326 1.340 210 315 1.335 215 302 1.330 220 287 1.324 225 271 1.319 230 257 1.313 235 243 1.307 240 228 1.301 245 211 1.295 250 197 1.289 255 ' 184 1.283 26C 170 1.276 265 150 1.270 270 135 1.263 275 120 1.256 280 105 1.249 285 91 1.241 290 78 1.235 295 67 1.226 300 55 1.217 (Winteler, Z. Elektrochem. 1900, 7. 361.) Very sol. in liquid NH 3 . (Franklin, Am* Ch. J. 1898, 20. 829.) Sol. in 34 pts. alcohol of 83% at 16 and in less hot alcohol. (Wittstein.) Somewhat more easily sol. in alcohol than NaCl. (Berzelius.) Solubility of NaClO 3 in alcohol. (g. NaClO 3 per 1. of solution.) t Alcohol 90 % 75% 50 % 20 40 60 70 16.1 22.9 29.0 110.8 133.5 155.8 161.3 311.3 321.8 326.8 (Carlson, Dissert. 1910.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) 100 g. glycerol dissolve 20 g. NaClO 3 at 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) CHLORINE 231 Strontium chlorate, Sr(ClO 3 ) 2 +5H 2 O. Very deliquescent, and sol. in H 2 0. (Top- soe, W. A. B. 66, 2. 29.) Sp. gr. of solution sat. at 18 containing 63.3% Sr (C1O 3 ) 2 = 1.839. (Mylius, B. 1897, 30. 1718.) Easily sol. in H 2 O, less in alcohol, but more sol. in alcohol than SrCl 2 . (Souchav, A. 102. 381.) Insol. in absolute alcohol. (Wachter.) Thallous chlorate, T1C1O 3 . Sol. in H 2 O, but decomp. by heating. 100 pts. H 2 O dissolve at: 20 50 80 100 2.80 3.92 12.67 36.65 57.31 pts. T1C1O 3 . (Muir, Chem. Soc. 29. 857.) 1 1. TIClOg+Aq sat. at 10 contains 25.637 g. T1C10 3 . (Roozeboom, Z. phys. Ch. 8. 532.) 1 1. H 2 O dissolves 0.134 equivalents TICK) 3 at 20; or 38.51 g. in 1 1. of the solu- tion (mean of 10 experiments). (Noyes and Farrell, J. Am. Chem. Soc. 1911, 33. 1657.) Solubility in Tl 2 SO 4 +Aq at 20. G. equiv. per 1. Solid phase TIClOs T1 2 S0 4 0.1058 0.1366 T1C1O 3 +T1 2 SO 4 (Noyes and Farrell, I.e.) Thallic chlorate, T1(C10 3 ) 3 +4H 2 O. Very deliquescent; sol. in H 2 O. Decomp. slowly in the air. (Gewecke, Z. anorg. 1912, 76. 273.) Ytterbium chlorate. Sol. inH 2 O. (Popp, A. 131. 179.) Yttrium chlorate, Y(C1O 3 ) 3 +8H 2 O. Deliquescent. Easily sol. in alcohol. SI. sol. in ether. (Cleve.) Zinc chlorate, Zn(ClO 3 ) 2 +4H 2 O. Solubility in H 2 O. Sat. solution contains at: +18 66.52 30 67.66 of 40 69.06 55 C 75.44% Zn(ClO 3 ) 2 . solution containing 66.52% Sp. gr. Zn(ClO 3 ) 2 at 18 = 1.916. (Meusser, B. 1902, 35. 1417.) More sol. in H 2 O than chlorates of Mg, Co, Ni or Cu; less sol. than chlorate of Cd; more sol. than Zn(N0 3 ) 2 . (Meusser, I.e.) +6H 2 O. Very deliquescent. Easily sol. iD H 2 O and alcohol. Melts in crystal H 2 O at 60. (Vauquelin, A. ch. 95. 113.) Solubility in H 2 O. Sat. solution contains at: -18 55.62 59.19 8 15 60.20 67.32% Zn(ClO 3 ) 2 . (Meusser, I.e.) Sp. gr. of solution sat. at 18 containing 65% Zn(ClO 3 ) 2 = 1.914. (Mylius, B. 1897, 30. 1718.) Zinc chlorate ammonia, Zr(ClO 3 ) 2 , 4NH 3 . Zn(ClO 3 ) 2 , 6NH 3 . Ppt. (Ephraim, B. 1915, 48. 48.) Perchloric acid See Perchloric acid. Chlorides. Most chlorides are sol. in H 2 O; a few, how- ever, are insol. or nearly so therein, the chief of which are AgCl, Hg ? Cl 2 , Cu 2 Cl 2 , PtCl 2 , and AuCl. Several chlorides are decomp. into insol. basic salts or hydroxides, either by the addition of H 2 O, as in the case of BiCl 3 and SbCl 3 , or on evaporating the aqueous solution, as A1C1 3 , ZnCl 2 , MgCl 2 , etc. Some chlorides are sol. in alcohol or ether. See under each element. Chlorine, C1 2 . The maximum solubility of Cl in H 2 O is at 1C (Schonfeld); at 8-10 (Gay-Lussac) ; at 9-10 (Pelouze). Solubility decreases from 9-0; at 100 the solubility =0. (Gay-Lussac.) Cl 2 +Aq sat, at 6 has sp. gr. = 1.003. (Ber- thelot.) 1 vol. H 2 O at t absorbs vols. Cl reduced to and 760 mm. pressure. t Vols. Cl t Vols. Cl 10 2.5852 26 1.9099 11 2.5413 27 1.8695 12 2.4977 28 .8295 13 2.4543 29 .7895 14 2.4111 30 .7499 15 2.3681 31 .7104 16 2.3253 32 .6712 17 2.2828 33 .6322 18 2.2405 34 .5934 19 2.1984 35 1.5550 20 2.1565 36 1,5166 21 2 1148 37 1.4785 22 2.0734 38 1.4406 23 2.0322 39 1.4029 24 1.9912 40 1.3655 25 1.9504 (Schonfeld, A. 93. 26 .) 232 CHLORINE Ivol . H 2 O absorbs vols. Cl at t (not corrected). Solubility of C1 2 in H 2 O. pi = Vol. of Cl (reduced to and 760 mm.) absorbed by 1 vol. H 2 O under a total pressure of 760 mm. q=g. C1 2 absorbed by 100 g. H 2 O under a total pressure of 760 mm. Vols. Cl t Vols. Cl t Vols. Cl t c 1. 1. 2. 2. 43 52 08 17 3 6.5 7 3 3 2 1 .04 .00 37 .61 8 10 17 35 1.19 0.71 0.15 50 70 100 t P l q t l q 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 3.095 2.996 2.900 2.808 2.720 2.635 2.553 2.474 2.399 2.328 2.260 2.200 2.143 2.087 2.035 0.980 948 918 889 861 835 809 784 760 738 716 698 680 662 646 25 26 27 28 29 30 35 40 45 50 60 70 80 90 100 .985 .937 .891 .848 .808 .769 .575 .414 1.300 1.204 1.006 0.848 0.672 0.380 0.000 0.630 615 600 587 574 562 501 451 415 386 324 274 219 125 000 (Gay-Lussac, A. ch. (3) 7. 124.) 1 vol. H2O at 8 absorbs 3.04 vols. Cl, which is the maximum of solubility. At 50, 1.09 vols. are absorbed ; and at 0, 1.5 vols. (Pelouze and Fremy.) 1 vol. EbO at t dissolves vols. Cl (not corrected) . t Vols. Cl t Vols. Cl t Vols. Cl 9 10 1.75-1.80 2.70-2.75 2.70-2.75 12 14 30 2 . 50-2 . 60 2.45-2.50 2 . 00-2 . 10 40 50 70 1 . 55-1 . 60 1.15-1.20 0.60-0.65 (Pelouze, A. ch. (3) 7. 188.) 1 vol. H 2 O absorbs vols. Cl at t. t Vols. Cl t Vols. Cl t Vols. Cl 5 8 1.5 -1.6 2.05-2.1 2.5 -2.6 9 10 12 2.65-2.70 2.9 -3.0 2.65-2.75 14 16 30 2.6 -2.65 2.35-2.4 1.8 -1.85 (Riegel and Walz, Berz. J. B. 1846. 72.) Solubility in H 2 O : a = coefficient of solubility. t a t a t a 6.9 8.4 9.3 2.2931 2.5469 2.7135 10.1 11.2 13.7 2.8741 2.7267 2.5079 21.7 32.1 36.7 2.0422 1.5766 1.3802 (Goodwin, B. 16. 3040.) Goodwin also gives tables for solubility of Cl in HC1 and various chlorides, but they do not show eviden ce of accurate work. ( A.M .C . ) Cl 2 +Aq contains at 760 mm. pressure: 1.44% Cl at 1.07% " " 6 0.95% " " 9 0.87% " " 12 (Roozeboom, R. t. c. 1884, 3. 29.) See also C1 2 +8H 2 O. (Winkler, Landolt and Bornstein, Tab. 4th Ed. 1912, 597.) 1 1. HCl+Aq (38% HC1) dissolves 17.3 g. Cl; 1 1. HCl+Aq (33% HC1) dissolves 11 g. Cl; 1 1. HCl+Aq (3% HC1) dissolves 6.5 g. Cl. (Berthelot, C. R. 91. 191.) Solubility of C1 2 in HCl+Aq at 20-21 C 759-761 mm. pressure. and g. HC1 per 1. g. C1 2 per 1. Coefficient of absorption Solubility 7.23 2.1157 2.2799 3.134 5.30 1.5496 .6698 6.248 4.94 .4483 .5607 9.402 4.76 .3942 .5013 12.540 4.85 .4200 .5292 15.670 5.10 .4933 .6092 31.340 5.81 .6736 .8033 62.680 6.38 .8682 2.0131 94.020 7.19 2.1044 2.2677 125.360 7.76 2.2711 2.4473 156.700 8.58 2.5095 2.7043 188.040 9.23 2.7020 2.9117 219.380 9.93 2.9243 3.1312 250.720 10.68 3.1272 3.3677 282.060 11.87 3.3278 3.5859 313.401 12.03 3.5492 3.8224 (Mellor, Chem. Soc. 1901, 75. 227.) Solubility of Cl in NaCl+Aq. a = coefficient of solubility. NaCl = 9.97%. t a t a 7.9 11.9 15.4 1.8115 1.5879 1.3684 18.8 22.6 1.2785 1.0081 CHLORINE OXIDE 233 Solubility of Cl in NaCl+Aq. Continued NaCl = 16.01%. Coefficient of solubility of C1 2 in organic liquids at 15. Substance Coefficient of Solubility t a t a Carbon tetrachloride 51 . 7 Acetic anhydride 39 . 6 Acetic acid (99.84%) 36 . 7 " (90vol. %) 25.3 (75vol. %) 16.43 (65vol. %) 13.43 6 11.6 16.4 1.5866 1.2227 1.0121 21 26 .4 .9 0.8732 0.7017 NaCl = l9.66%. (Jones, Chem. Soc. 1911, 99. 392.) +8H 2 O. Critical temp, of decomposition in open vessel = 9.6; in closed vessel = 28.7. Solubility in H 2 O. % C1 2 = % of C1 2 in Cl 2 +Aq sat. at t and 760 mm. in presence of C1 2 +8H 2 O. t a t a 9.2 9.3 14.8 1.6978 1.2145 1 . 2068 0.9740 15.4 20.4 21.9 0.9511 0.7758 0.7385 t % CU t %CU (Kumpf, W. Ann. Beibl. 6. 276.) Solubility of Cl in sat. NaCl-f-Aq at t and 760 mm. pressure. 0.505 12.5 3 0.64 20 6 0.709 28.5 9 0.900 1.10 1.82 3.50 (Roozeboom, R. t. c. 1884, 3. 57.) Chlorine wojjoxide, C1 2 O. Sol. in H 2 O. At 0, H 2 O absorbs at least 200 times its volume of C1 2 O gas. Chlorine dioxide, C1 2 O 3 . Decomp. on air at 57 with explosion. H 2 O absorbs 5-6 vols. C1 2 3 . (Millon, A. ch. (3) 7. 298.) H 2 O absorbs at 8.5 and 753 mm. press. 8.591 vols. C1 2 O 3 . (Brandan.) 100 g. H 2 O dissolve at: f < Coefficient of absorp- ion at and 760 mm. Solubility at and 760 mm. 14.5 29.0 60.0 82.0 0.3607 0.3125 0.1332 O.G586 0.3898 0.3458 0.1625 0.0763 (Kohn and O'Brien, J. Soc 17. 1100. . Chem. Ind. 1898, Sat. KCl+Aq absorbs V* less Cl at 15 than pure H 2 O. (Dettmer, A. 38. 35.) 1 1. of a solution of CaCl 2 (1 pt. in 15 pts. H 2 O) dissolves 2.45 g. Cl at 12. 1 1. of a solution of MgCl 2 (1 pt. in 15 pts. H 2 O) dissolves 2.33 g. Cl at 12. 1 1. of a solution of MnCl 2 (1 pt. in 15 pts. H 2 O) dissolves 2.00 g. Cl at 12 C . SI. sol. in KOH+Aq. (Fremy.) Somewhat sol. in liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) CC1 4 absorbs 10% of C1 2 at 13. (Perkins, Chem. Soc. 1894, 65. 20.) 1 mol. CrOCl 2 dissolves at 0, 0.70 atom Cl; at- 14, 1.24 atoms; at- 21, 2.31 atoms; and at- 24, 3.00 atoms Cl. (Roozeboom, R. t. c. 4. 379.) Sulphuryl chloiide absorbs 71 vols. Cl or 0.136 pt. Cl by weight at 0. (Schulze, J. pr. (2) 27. 168.) Insol. in benzene. (Moride.) SI. sol. in chloral and iodal. (Dumas.) Sol. in perchlorethylene. (Faraday.) Sol. in a very large quantity of ether with decomp. 8.5 and 752.9 mm. press. 4.7655 g. C1 2 O 3 . 14 " 756.3 " " 5.0117 21 " 754 " " 5.4447 93 " 760 " " 5.6508 (Brandan, A. 161. 340.) Does not exist, and above data are for mix- ture of C1O 2 and Cl. (Garzarolli-Thurnlakh, A. 209. 184.) Chlorine tefroxide, C1O 2 . H 2 O at 4 absorbs about 20 vols. C1O 2 with formation of HC1O 2 and HC1O 3 . H 2 SO 4 at- 18 absorbs about 20 vols. C1O 2 . (Millon, A. ch. (3) 7. 285.) Solubility of C1O 2 in H 2 O. t g. C1O 2 per 1. 1 10.7 14.0 >108.6 116.7 >107.9 ray, Z. phys. Ch. 1906, 54. 569.) 234 CHLORINE OXIDE +8H 2 O (=fclH 2 O). Lithium chloriridate, Li 2 IrCl 6 . Solubility in H 2 O. Somewhat deliquescent; very sol. in H 2 O. (Antony, Gazz. ch. it. 23, 1. 190.) t g. C1O 2 per 1. t g. C1O 2 per 1. Potassium chloriridate, K 2 IrCl 6 . 0.79* 1 26.98 27.59 29 48 10 15.3 18 2 60.06 60.06 107 9 SI. sol. in cold H 2 O; sol. in 15 pts. boiling H 2 O; less sol. in H 2 O containing HC1; insol. in alcohol or sat. KC1, and CaCl 2 +Aq. 5.7 42.10 Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Entertic. (Bray.) Chlorine oxide, Cl 6 Oi 7 . Very easily decomp. (Millon, A. 46. 281.) Probably a mixture of C1O 2 and O. Chlorine Aep/oxide, C1 2 7 . Explosive; decomp. by H 2 O; sol. in well cooled benzene with si. decomp. (Michael, Am. Ch. J. 1909, 23. 447.) Chlorirididiamine chloride, C1 j NH 3 NH 3 C1. ul2lr NH 3 NH 3 Cl SI. sol. in cold, easily in hot H 2 O. (Skobli- koff, A. 84. 275.) nitrate, Cl 2 Ir(N 2 H 6 NO 3 ) 2 . Sol. in H 2 O. - sulphate, Cl 2 Ir(N 2 H 6 )SO 4 . SI. sol. in cold, much more easily in hot H 2 O. Chloriridic acid. Chloriridates. Most of the chloriridates are very difficultlv sol. in H 2 O, but a little more sol. than the corresponding chloroplatinates. Insol. or nearly so in alcohol, but not so difficultly sol. as the chloroplatinates. (Rose.) Ammonium chloriridate, (NH 4 ) 2 IrCl 6 . Sol. in 20 pts. cold H 2 O (Vauquelin); si. sol. in cold, much more in hot H 2 O (Glaus) ; sol. in HCl+Aq (Soblewsky); insol. in cold NH 4 Cl+Aq (Glaus); insol. in alcohol (Ber- zelius). 100 pts. H 2 O dissolve at: 14.4 26.8 39.4 0.699 0.905 1.226 pts. (NH 4 ) 2 IrCl 6 , 52.2 61.2 69.3 1.608 2.130 2.824 pts. (NH 4 ) 2 IrCl c . (Rimbach and Korten, Z. anorg. 1907, 52. 407.) Caesium chloriridate, Cs 2 IrCl 6 . Only si. sol. in H^O. (Delepine, C. R. 1908, 146. 1268.) Rubidium chloriridate, Rb 2 lrCl 6 . Very si. sol. in H 2 O. (Rimbach, Z. anorg. 1907, 52. 408.) Sodium chloriridate, Na 2 IrCl G +6H 2 O. Easily sol. in H 2 O; sol. in alcohol of 0.837 sp. gr. Thallium chloriridate, Tl 2 IrCl 6 . Decomp. by hot HC1 forming Tl 3 IrCl 6 . (Delepine, C. R. 1909, 149. 1073.) Chloriridium pentamine comps. See Iridope^amine chloro comps. Chloriridosulphuious acid. Potassium chloriridosulphite. K 4 Ir 2 Cl 2 (SO 3 ) 4 , 4KC1+12H 2 C Insol. in cold, decomp. by hot H 2 O. K 4 lr 2 Cl 2 (S0 3 ) 4 , 2K 2 SO 3 . Decomp. by H 2 O. Cl 2 Ir 2 (S0 3 ) 2 , 8KC1+4H 2 O. Sol. in H 2 O; insol. in alcohol. (Glaus, J. pr. 42. 354.) Chloriridous acid. Ammonium chloriridite, (NH 4 ) 3 IrCl 6 . Decomp. by H 2 O. (Delepine, C. R. 1908, 146. 1268.) + 1KH 2 O. Sol. inH 2 O. (Glaus.) IrCl 5 (H 2 O) (NH 4 ) 2 . (Delepine.) Caesium chloriridite, IrCl 5 (H 2 O)Cs 2 . (Delepine.) Lithium chloriridite, Li 3 IrCl 6 +12H 2 O. Deliquescent; sol. in H 2 O and alcohol. (Delepine, C. R. 1914, 158. 1277.) Lithium sodium chloriridite, Li 2 NaIrCl 6 + 12H 2 O. Stable in aq. solution in the presence of excess of lithium salt. (Delepine, C. R. 1914, 158. 1278.) LiNa 2 IrCl 6 +12H 2 O. Stable in aq. solu- tion in the presence of excess of sodium salt. (Delepine, C. R. 1914, 158. 1278.) Potassium chloriridite, K 3 IrCl 6 . Decomp. by H 2 0. (Delepine.) +3H 2 O. Easily sol. in H 2 O; insol. in al- cohol; insol. in sat. KCl+Aq. (Berzelius.) IrCl 5 (H 2 O)K 2 . (Delepine.) CHLOROCOLUMBIUM CHLORIDE 235 Rubidium chloriridite, IrCl 5 (H 2 O)Rb 2 . (Delepine.) Silver chloriridite, Ag 3 IrCl 6 . Insol. in H 2 or acids; si. sol. in NH 4 OH + Aq. Ppt. (Delepine, Bull. Soc. 1910, (4), 7. 55.) Sodium chloriridite, Na 3 IrCl 6 + 12H 2 O. Efflorescent; sol. in ^ pt. H 2 0. Insol. in alcohol. Melts in crystal H 2 O at 50. Thallium chloriridite, Tl 3 IrCl 6 . Sol. in hot HC1; pptd. on cooling. (Dele- pine, C. R. 1909, 149. 1073.) Chlorofeframine chromium comps. See Chlorotetramine chromium comps. Chloro-azoimide, N 3 C1. SI. sol. in H 2 0. (Raschig, B. 1908, 41. 4194.) Chlorobromo comps: See Bromochloro comps. Chlorocarbonic acid. See Carbonyl chloride. Chlorochromic acid. Known only in its salts. CrO 2 Cl 2 . See Chromyl chloride. Ammonium chlorochromate, NH 4 CrO 3 Cl = Cr 2 ONH 4 . More sol. in H 2 O than the K salt. (Peligot, A. ch. 52. 283.) Barium chlorochromate chloride, Ba(Cr0 3 Cl) 2 , BaCl 2 . Deliquescent. Very sol. in H 2 O. (Prator- ius, A. 201. 1.) +H 2 O. Not deliquescent. Calcium chlorochromate, Ca(OrO 3 Cl) 2 . Deliquescent. (Peligot.) +5H 2 O. Very deliquescent. (Pratorius.) Chromous chlorochromate. See Tn'chromyl chloride. Cobalt chlorochromate, Co(CrO 3 Cl) 2 +9H 2 O. Deliquescent; melts at 40 in crystal H 2 O. (Pratorius.) Lithium chlorochromate, LiCrO 3 Cl. Sol. in H 2 O acidified with HC1 without decomp. (Lowenthal, Z. anorg. 1894, 6. 357.) Magnesium chlorochromate, Mg(CrO 3 Cl) 2 . Deliquescent. (Peligot.) -f 9H 2 O. Less deliquescent than the other chlorochromates. (Pratorius, A. 201. 1.) Very hydroscopic; sol. in H 2 O acidified with HC1 without decomp. (Lowenthal, Z. anorg. 1894, 6. 359.) Nickel chlorochromate, Ni(CrO 3 Cl) 2 -f9H 2 O. Deliquescent; melts in its crystal H 2 O at 4&-48 . (Pratorius.) Potassium chlorochromate, KCrO 3 Cl = CrO 2 (Cl)OK. Sol. in H 2 O with decomp. Cryst. from H 2 O containing HC1 without decomp. (Peligot.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Sodium chlorochromate, NaCrO 3 Cl. Deliquescent. (Peligot.) +2H 2 O. Deliquescent. (Pratorius.) Strontium chlorochromate, Sr(CrO 3 Cl) 2 + 4H 2 O. Deliquescent; melts in crystal H 2 O at 72. (Pratorius.) Thallous chlorochromate, TlCrO 3 Cl. Decomp. by H 2 0. (Lachaud and Lepierre, C. R. 103. 198.) Zinc chlorochromate, Zn(CrO 3 Cl) 2 +9H 2 O. Deliquescent; melts at 37.5 in crystal H 2 O. (Pratorius.) Very hydroscopic; very sol. in H 2 O and acids. (Lowenthal, Z. anorg. 1894, 6. 360.) ZHchloro chromium bromide, [Cr(H 2 O) 4 Cl 2 ]Br. Very deliquescent. Sol. in fuming HBr, in a mixture of equal volumes ether and fum- ing HBr, in alcohol and in acetone. (Bjerrum, B. 1907, 40. 2919.) Chlorochromotetrammonium comps. See Chlcrotetramine chromium comps. Chlorocolumbium bromide, (Cb 8 Cli 2 )Br 2 -h 7H 2 0. Sol. in a small quantity of cold H 2 O. (Harned, J. Am. Chem. Soc. 1913, 36. 1083.) Chlorocolumbium chloride, (Cb 6 Cli 2 )Cl 2 + 7H 2 O. Insol. in cold, sol. in boiling H 2 O. Not easily decomp. by boiling with NH 4 OH. Cone. HN0 3 decomp. a boiling solution of this comp. Completely sol. in cone, alkalies. (Harned, J. Am. Chem. Soc. 1913, 36. 1080.) 236 CHLOROCOLUMBIUM HYDROXIDE Chlorocolumbium hydroxide, (Cb 6 Cli 2 ) (OH) 2 +8H 2 O. Insol. in H 2 O. Sol. in acids and alkalies. (Earned, J. Am. Chem. Soc. 1913, 35. 1082.) Chloroctamine cobaltic carbonate, Cl 4 Co 2 (NH 3 ) 8 CO 3 +2H 2 O. Very sol. in H 2 O. (Vortmann and Bias- berg, B. 22. 2651.) Cl 2 Co 2 (NH 3 ) 8 (CO 3 ) 2 +H 2 O. (Vortmann and Blasberg.) Chloroferrous acid. Calcium chloroferrite, CaO, CaCl 2 , Fe 2 O 3 . Insol. in H 2 O. (le Chatelier, C. R. 99. 276.) Di'chlorofulminoplatinum, Pt 4 N 4 Cl 2 12 H 22 (?). Insol. in H 2 O. (v. Meyer, J. pr. (2) 18. 305.) Y'n'chlorofulininoplatinum, Pt 4 N 4 Cl 3 (OH)0 12 H 24 (?). Insol. in H 2 O; sol. in HCl+Aq. (v. Meyer.) T^racUorofulminoplatinum, Pt 4 N 4 Cl 4 12 H 24 (?) Insol. in H 2 O. (v. Meyer.) Chlorohydroxylonitritoplatin6e?m'di- amine nitrite, (OH)ClNO 2 Pt(NH 3 ) 2 NO 2 . Easily sol. in hot H 2 0. (Cleve.) Chlorohydroxyloplatindi'amine bromide, SI. sol. in H 2 O. - carbonate, Insol. in H 2 O. (Cleve.) - chloride, O 81. sol. in HjO. (Cleve.) Nearly insol. in H 2 0. Ppt. (Cleve.) nitrate (Raewsky's nitrate), SI. sol. in cold, more easily in hot H 2 O. (Gerhardt.) Chlorohyposulphuric acid, S 2 O 3 C1 4 . fee Sulphur oxy^rachloride. Chloromanganic acid. Se3 Manganic hydrogen chloride. Chloromercurosulphrous acid. Ammonium chloromercurosulphite, NH 4 SO 3 HgCl. Sol. in H 2 O. (Earth, Z. phys. Ch. 9. 205.) Barium chloromercurosulphite, Ba(SO 3 HgCl) 2 . Insol. in H 2 O. (Barth.) Potassium chloromercurosulphite, KSO 8 HgCl. Sol.inH 2 0. (Barth.) Sodium chloromercurosulphite, NaSO 3 HgCl +H 2 0. Very sol. in H 2 0. (Barth.) Chloromolybdenum bromide, Cl 4 Mo 3 Br 2 +3H 2 O. Insol. in H 2 O and dil. acids; sol. in alcohol. +6H 2 O. At first easily sol. in H 2 O, but a precipitate soon forms. Can be crystallized from dil. HBr+Aq. Sol. in alcohol and ether. (Blomstrand.) bromide, Chloromolybdenum potassium Cl 4 Mo 3 Br 2 , 2KBr+2H 2 O. Decomp. by H 2 O. Can be cryst. from HBr -fAq. (Blomstrand.) Chloromolybdenum chloride, Cl 4 Mo 3 Cl 2 = molybdenum ^'chloride, MoCl 2 . Insol. in H 2 O; easily sol. in HCl+Aq or H 2 SO 4 +Aq; si. sol. in HN0 3 ; sol. in NH 4 OH +Aq, NaOH+Aq, or KOH-fAq, with sep- aration of precipitate on boiling; sol. in alcohol and ether. (Blomstrand, J. pr. 77. 96.) Very sol. in cone. HC1. (Rosenheim and Kohn, Z. anorg. 1910, 66. 2.) +3H 2 O. Insol. in H 2 O. +4iH 2 O. Insol. in H 2 O. (Liechti and Kempe, A. 170. 351.) +6H 2 O. Sol. in H 2 0, alcohol, or ether. (Blomstrand.) Chloromolybdenum hydrogen chloride, Mo 3 Cl 6 , HC1+4H 2 0. Sol. in H 2 O, but ppt. forms after a few minutes. (Rosenheim and Kohn, Z. anorg. 1910, 66. 5.) Chloromolybdenum potassium chloride, Cl 4 Mo 3 Cl 2 , 2KC1+2H 2 O. Decomp. by pure H 2 O; can be recrystal- lized from HCl+Aq. (Blomstrand, J. pr. 77. 108.) CHLORONITRITE, IRIDIUM POTASSIUM 237 Chloromolybdenum hydroxide, Cl 4 Mo 3 (OH 2 ) +2H 2 0. Insol. in H 2 O or alcohol. Easily sol. in strong acids if fresh, and washed only with cold H 2 O. If washed with warm H 2 0, it is less sol. in acids. If precipitated hot, is insol. in acids, even H 2 SO 4 or fuming HNO 3 . (Blom- strand, J. pr. 77. 100.) +8H 2 O. Chloromolybdenum iodide, Cl 4 Mo 3 I 2 +3H 2 O. Precipitate. +6H 2 O. Sol. in H 2 O and alcohol. Chloromolybdenum potassium iodide, Cl 4 Mo 3 I 2 , 2KI+2H 2 O. Decomp. by H 2 O. Recryst. from HI+Aq. (Blomstrand.) OTT Chloromolybdenum oxybromide, Cl 4 Mo 3 g r +2H 2 O. Insol. in alcohol. (Blomstrand, J. pr. 77. 116.) Chlcromolybdic acid, MoOCl 3 (OH)+7H 2 O. Very hydroscopic. (Weinland, B. 1904, 37. 572.) Di'ammonium tefrachloromolybdate, MoCl 4 (ONH 4 ) 2 +2H 2 0. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies and ammonia. (Wein- land, Z. anorg. 1905, 44. 83.) Caesium chloro/ranolybdate, acid, Mo 6 O u Cl 14 (Cs 2 0)+22H 2 0. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies, and ammonia. (Wein- land, I.e.} Monoc&siwa. Jn'chloromolybdate, MoOCl 3 (OCs)+H 2 0. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies and ammonia. (Wein- land.) ZH'csesium fc^rachloromolybdate, MoCl 4 (OCs) 2 . Hydroscopic. Sol. in H 2 O with decomp. Sol. in dilute acids, alkalies, and ammonia. (Weinland, Z. anorg. 1905, 44. 83.) Morcopotassium Zn'chloromolybdate, MoOCl 3 (OK)+H 2 O. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies, and ammonia. (Wein- land.) Dipotassium tefrachloromolybdate, IVLC1 4 (OK) 2 +2H 2 O. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies, and ammonia. (Wein- land.) Potassium hydrogen jchloro/rimolybdate, Mo 6 u ri 14 , K 2 O+6H 2 O. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies, and ammonia. (Wein- land.) Afoworubidium fnchloromolybdate, MoOCl 3 (ORb)+H 2 0. Hydroscopic. Decomp. by H 2 O. Sol. in dilute acids, alkalies, .and ammonia. (Wein- land.) Dirubidium tefrachloromolybdate, MoCl 4 (ORb) 2 . Hydroscopic. Decomp. by H 2 0. Sol. in dilute acid, alkalies, and ammonia. (Wein- land.) Chloronitratoplatinamine nitrite, Easily sol. in H 2 O. Chloronitratoplatindx'amine nitrate, Decomp. by H 2 O with formation of ^Pt[(NH 3 ) 2 N0 3 )] 2 . - sulphate, i C^ Pt(N2 H 6 ) 2 S0 4 +H 2 0. SI. sol. in cold, more easily in hot H 2 O. Chloronitritotetramine cobaltic chloride, Cl(N0 2 )Co(NH 3 ) 4 Cl. Not very sol. in cold H 2 0. (Jorgensen, Z. anorg. 5. 195.) Chloromtritoplatinse/mdmmine chloride, Cl 2 (N0 2 )Pt(NH 3 ) 2 Cl. 100 pts. solution in H 2 sat. at 18 contain 1.8 pts. salt; sat. at 100, 6 pts. Insol. in abs. alcohol or ether. Not decomp. by cone. HNO 3 , HC1, or H 2 C 2 O 4 +Aq, and by H 2 SO 4 only at a high heat. Formula given was PtNeHiaCleO*. (Pey- , J. B. 1865. 421.) rone, nitrite, Cl 2 (N0 2 )Pt(NH 3 ) 2 N0 2 . Sol. in H 2 O. (Blomstrand.) Chlorophosphatoplatincfaamine phos- ClPt(N 2 H 6 ) 2 phate, \ / +2H 2 O. PO 4 Nearly insol. in cold, and only very si. sol. inhotH 2 O. (Raewsky.) Chloronitrous acid. Indium potassium chloronitrite, Ir 2 Cl2(NO 2 ) 4 , 6KC1, Ppt.; decomp. by boiling H 2 O. Sol. in cold H 2 O. (Leidi^, C. R. 1902, 134. 1583.) 238 CHLOROPALLADIC ACID Ir 3 K J2 Cl 16 (NO 2 ) 8 +4H 2 0. Ppt. (Quen- nessen, C. R. 1905, 141. 258.) Chloropalladic acid. Chloropalladates. The chloropalladates are generally very sol. in H 2 O, and sol. in alcohol, (v. Bonsdorff, Pogg. 17. 264.) Ammonium chloropalladate, (NH 4 ) 2 PdCl 6 . SI. sol. in H 2 0. (Berzelius.) Barium chloropalladate. Sol. in H 2 O and alcohol, (v. Bonsdorff.) Cadmium chloropalladate. As above. Caesium chloropalladate, Cs 2 PdCl 6 . Nearly insol. in cold H 2 O. Decomp. by boiling with H 2 O or by hot cone. H 2 SO 4 . (Gutbier, B. 1905, 38. 2386.) Calcium chloropalladate. Deliquescent; sol. in H 2 O and alcohol, (v. Bonsdorff, 1829.) Glucinum chloropalladate, GlPdCl 6 -f8H 2 O. Very hydroscopic, and sol. in H 2 O. Magnesium chloropalladate, MgPdCl 6 + 6H 2 O. Deliquescent; sol. in H 2 O. Nickel chloropalladate, NiPdCl 6 +6H 2 O. Extremely deliquescent. Potassium chloropalladate, K 2 PdCl 6 . SI. sol. in cold H 2 O. Decomp. by long boil- ing with H 2 O. SI. sol. in dil. HCl+Aq with- out decomp. Insol. in NH 4 C1, KC1, or NaCl H-Aq. Insol. in alcohol. (Berzelius.) Rubidium chloropalladate, Rb 2 PdCl 6 . Insol. in cold H 2 O. Decomp. by boiling with H 2 O or by hot cone. H 2 SO 4 . (Gutbier, B. 1905, 38. 2387.) Zinc chloropalladate, ZnPdCl 6 +6H 2 O. Very deliquescent, (v. Bonsdorff.) Chloropalladous acid Aluminum chloropalladite, Al 2 Pd 2 Cli + 20H 2 O. Deliquescent. Sol. in H 2 O, alcohol, or ether. (Welkow, B. 7. 804.) Ammonium chloropalladite, (NH 4 ) 2 PdCl 4 + H 2 O. Easily sol. in H 2 O. Insol. in alcohol. Sol inNH 4 Cl+Aq. (Glaus.) Easily sol. in H 2 O. (Gutbier, B. 1905, 38. 2386.) Barium chloropalladite. Easily sol. in H 2 O or alcohol. Cadmium chloropalladite. Not deliquescent. Caesium chloropalladite, Cs 2 PdCl 4 . Can be cryst. from hot H 2 O. (Gutbier, B: 1905, 38. 2386.) Calcium chloropalladite. Deliquescent. Sol. in H 2 O or alcohol. Glucinum chloropalladite, GlPdCl 4 +6H 2 O. Very hygroscopic; or ether. (Welkow.) Very hygroscopic; very sol. in H 2 O, alcohol, . (We Magnesium chloropalladite. Deliquescent. Easily sol. in H 2 O. (v. Bonsdorff.) Manganese chloropalladite. Sol. in H 2 and alcohol. Nickel chloropalladite. Sol. in H 2 O. Potassium chloropalladite, K 2 PdCL. Much more sol. in hot than cold H 2 O. (Joannis, C. R. 96. 295.) Sol. in NH 4 OH+ Aq. (Berzelius.) Sol. in cold sat. KCl+Aq. (Gibbs, Sill. Am. J. (2) 31. 70.) Insol. in al- cohol. (Wollaston.) Somewhat sol. in al- cohol of 0.84 sp. gr., but insol. in absolute al- cohol; decomp. on boiling (Berzelius.) Rubidium chloropalladite, Rb 2 PdCl 4 . Can be cryst. from hot H 2 O. (Gutbier, B. 1905, 38. 2387.) Sodium chloropalladite. Deliquescent. Sol. in H 2 O and alcohol. Zinc chloropalladite. Very deliquescent. Sol. in H 2 O and alcohol. (v. Bonsdorff.) Chlorophosphoarsenioiridic acid, 2IrCl 3 . 3H 3 P0 3 , 3H 3 P0 4 , 5H 3 As0 4 (?). Very sol. in H 2 0. (GeisenheimerJ Lead chlorophosphoarsenioiridate, 4IrCl 3 , 3Pb 2 H 2 (P0 3 ) 2 , 3Pb,(P0 4 )*, 5Pb 2 H 2 (AsO 4 ) 2 . Insol. in H 2 O. Chlorophosphoiridic acid, 2IrCl 3 , 3H 3 PO 4 , 3H 3 PO 3 . Very sol. in H 2 O. Insol. in alcohol. (Geisenheimer, A. ch. (6) 23. 254.) 2IrCl 3j 3H 3 PO 4 . Sol. in H 2 O and alcohol. CHLOROPLATINATE, AMMONIUM 239 Ammonium chlorophosphoiridate, 2IrCl 3 , 3(NH 4 ) 3 P0 4 , 3(NH 4 ) 2 HP0 3 . Very deliquescent. Very sol. in H 2 0. (Geisenheimer.) Lead chlorophosphoiridate, 4IrCl 3 , 3Pb 3 (P0 4 ) 2 , 3PbH 2 (P0 3 ) 2 . Insol. in H 2 O or acetic acid; very sol. in dil. HNOs+Aq. (Geisenheimer.) Silver chlorophosphoiridate, 2IrCl 3 , 3AgH 2 PO 4 , 3AgH 2 PO 3 . Insol. in H 2 O. Sol. in HNO 3 +Aq, and NH 4 OH+Aq. (Geisenheimer.) Chlorophosphoplatinic acid. See Chloroplatinophosphoric acid. Chlorophosphoric acid. Thorium chlorophosphate, 3ThO 2 ,ThCl 4 , 2P 2 6 . Insol. in H 2 O and acids; decomp. by boil- ing with H 2 SO 4 and fusing with alkali car- bonates. (Golani, C. R. 1909, 149. 208.) Chloroplatinamine chloride, C^Pt^^j 1 Sol. in about 700 pts. H 2 O at 0, and 33-34 pts. at 100. Not attacked by boiling cone. HNO 3 or H 2 SO 4 . Sol. in boiling KOH+Aq with decomp. Sol. in NH 4 OH+Aq. (Cleve, Sv. V. A. H. 10, 9. 30.) nitrite, Cl 2 Pt(NH 3 NO 2 ) 2 . SI. sol. in cold, easily in hot H 2 O. nitrite silver nitrite, Cl 2 Pt(NH 3 N0 2 ) 2 , AgN0 2 . Easily sol. in hot, si. sol. in cold H 2 O. (Cleve.) nitritochloride, Sol. in H 2 O. (Cleve.) CMoroplatinefa'amine bromide, Cl 2 Pt(N 2 H 6 Br) 2 . SI. sol. in hot H 2 O. (Cleve.) - chloride (Gros'. chloride), Cl 2 Pt(N 2 H 6 Cl) 2 . Nearly insol. in cold, and only si. sol. in hot H 2 O. Sol. in hot cone. KOH+Aq, with de- comp. (Grimm.) Sol. in cold KOH+Aq without decomp. Nearly insol. in NH 4 OH+Aq. (Buckton.) + y n H 2 O. (Raewsky.) chloroplatinate, NCl 2 Pt( 2 H 6 Cl) 2 , PtCl 4 . Easily sol. in hot H 2 O. - chloroplatinite, Cl 2 Pt(N 2 H 6 Cl) 2 , PtCl 2 . SI. sol. in H 2 0. (Cleve.) . Chloroplatintfiamine chromate, Cl 2 Pt(N 2 H 6 ) 2 CrO 4 . Nearly insol. in H 2 O. (Cleve.) bichromate, Cl 2 PtfN 2 H 6 ) 2 Cr 2 O7. SI. sol. in cold, more sol. in hot H 2 O. (Cleve.) - nitrate (Gros' nitrate),Cl 2 Pt(N 2 H 6 NO 8 ) 2 . Much more easily sol. in hot than in cold H 2 O. Sol. in hot KOH+Aq with decomp. Nearly insol. in cone. HNO 3 +Aq. - nitritochloride, Ppt. (Jorgensen.) - phosphate. See Chlorophosphatoplatin^'amine phos- phate. - sulphate, Cl 2 Pt(N 2 H 6 ) 2 SO 4 . SI. sol. in both cold or hot H 2 O. (Cleve.) +rcH 2 Q. SI. sol. in cold, easily in hot H 2 O. (Grimm.) -- sulphocyanide, Cl 2 Pt(N;>H 6 ) 2 (CNS) 2 +H 2 0. Ppt. (Cleve.) Chloroplatinwonodi'amine chloride, ri p, (NH 3 ) 2 C1 Cl2Pfc NH 3 Cl. Quite easily sol. in H 2 O. (Cleve.) Chloroplatinsewidz'amine carbonate chlo- ride, 2Pt(NH 3 ) 2 Cl 2 , Pt 2 (NH 3 ) 4 Cl 2 (C0 3 ). SI. sol. in H 2 O; insol. in alcohol and ether. Decomp. by cold HC1 +Aq . (Schon, Z. anorg. 1897, 13. 37.) Chloroplatinsewiefo'amine chloride, Cl 3 Pt(NH 3 ) 2 Cl. Sol. in 300 pts. H 2 O at 0, and 65 pts. at 100. Not decomp. by cone. H 2 SO 4 . Sol. in KOH+Aq without decomp. (Cleve.) Chloroplatinic acid, H 2 PtCl 6 +6H 2 O. Dehquescent. Sol. in H 2 0, alcohol, or ether. +4H 2 O. Deliquescent. (Pigeon, C. R. 112. 1218.) PtCl 4 , HC1+2H 2 O. (Pigeon.) Aluminum chloroplatinate, A1C1 3 , PtCl 4 + 15H 2 O. Very sol. in H 2 O and alcohol. (Welkow, B. 7. 304.) Insol. in ether. Ammonium chloroplatinate, (NH 4 ) 2 PtCl 6 . SI. sol. in cold, more easily in hot H 2 O. (Fresenius.) 100 ptSi H 2 O dissolve 0.666 pt. at ord. temp, and 12.5 pts. at 100. (Crookes, C. N. 9.37.) . 240 CHLOROPLATINATE, BARIUM Insol. in cold HCl+Aq. Separates out on cooling from solution in hot HC1, HNO 3 , or H 2 S0 4 . (Fischer.) Very si. sol. in cold, easily in hot NH 4 OH + Aq. (Fresenius.) Cone. NH 4 Cl+Aq ppts. it almost com- pletely from aqueous solution. (Bottger-.) Sol. in NH 4 succinate+Aq. (Dopping.) Less sol. in H 2 PtCl 6 +Aq than in H 2 O. (Rogojski, A. ch. (3) 41. 452.) Sol. in SnCl 2 +Aq. (Fischer.) Very sol. with decomp. in KCNS+Aq. (Glaus.) At 15-20, sol. in 26,535 pts. 97.5% alcohol, in 1476 pts. 76% alcohol, and in 665 pts. 55% alcohol. If free HC1 is present, it is sol. in 672 pts. 76% alcohol. (Fresenius, A. 69. 118.) Insol. in absolute alcohol or ether. Barium chloroplatinate, BaPtCl 6 +6H 2 O. Permanent; sol. in H 2 O; decomp. by alcohol, (v. Bonsdorff, Pogg. 17. 250.) Barium rwonochloroplatinate, PtCl(OH) 5 Ba+ H 2 0. Insol. in H 2 O and in org. solvents. (Bel- lucci, C. C. 1903, 1. 131.) Barium pe/itachloroplatinate, OH.PtCl 5 Ba-f- H 2 0. (Miolati, Chem. Soc. 1900, 78. (2) 732.) Cadmium chloroplatinate, CdPtCl 6 +6H 2 O. Deliquescent, and easily sol. in H 2 O. (v. Bonsdorff.) Caesium chloroplatinate, Cs 2 PtCl 6 . 100 pts. H 2 dissolve at: 10 20 30 0.024 0.050 0.079 0.110 pts. Cs 2 PtCl 6 , 40 C 50 60 70 0.142 0.177 0.213 0.251 pts. Cs 2 PtCl 6 , 80 90 100 0.291 0.332 0.377 pts. Cs 2 PtCl 6 . (Bunsen, Pogg. 113. 337.) Sol. in 1308 pts. H 2 O at 15, and 261 pts. at 100. (Crookes, C. N. 9. 205.) Calcium chloroplatinate, CaPtCl 6 +8H 2 O. Deliquescent; easily sol. in H 2 O. (v. Bons- dorff.) Calcium wonochloroplatinate, PtCl(OH) 6 Ca +H 2 0. Insol. in H 2 O and in org. solvents. (Bel- lucci, C. C. 1903, I. 131.) Cerium chloroplatinate, CeCl 3 , PtCl 4 +13H 2 O. Deliquescent; very sol. in H 2 O or alcohol; insol. in ether. (Marignac.) 4CeCl s , 3PtCl 4 +8H 2 O. Deliquescent; easily sol. in H 2 O or alcohol; insol. in ether. (Holzmann, J. pr. 84. 80.) Chromium chloroplatinate, CrCl 3 , PtCl 4 + Deliquescent. (Nilson, B. 9. 1056.) +10H 2 O. Very sol. in H 2 O and alcohoL Nearly insol. in acetone. (Higley, J. Am. Chem. Soc. 1904, 26.617.) Cobalt chloroplatinate, CoPtCl 6 +6H 2 0. Very deliquescent. (Jorgensen.) Copper chloroplatinate, CuPtCl 6 +6H 2 O. Deliquescent in moist air. (v. Bonsdorff.} Didymium chloroplatinate, DiCl 3 , PtCl 4 + 13H 2 O. Less deliquescent than the cerium salt. (Marignac.) +10^H 2 0. Deliquescent. (Cleve, Bull. Soc. (2) 43. 361.) Erbium chloroplatinate, ErCl 3 , PtCl 4 + 11H 2 O. Very deliquescent. (Cleve.) Gadolinium chloroplatinate, GdCl 3 , PtCl 4 + 10H 2 0. Ppt. (Benedicko, Z. anorg. 1900, 22. 204.) Glucinum chloroplatinate, GlPtCl 6 +8H 2 0. Deliquescent in moist air. Very sol. in H 2 O, moderately in alcohol. Insol. in ether. (Welkow, B. 6. 1288.) Indium chloroplatinate, 2InCl 3 , 5PtCl 4 + 36H 2 O. Deliquescent. (Nilson.) Iron (ferrous) chloroplatinate, FePtCl6+ 6H 2 O. Deliquescent. (Topsoe.) Iron (ferric) chloroplatinate, FeCl 3 , PtCl 4 -f Deliquescent. (Nilson.) Lanthanum chloroplatinate, LaCl s , PtCl 4 + 13H 2 O. Deliquescent; extremely sol. in H 2 O. (Cleve.) Lead chloroplatinate, PbPtCl 6 +3H 2 O. Easily sol. in H 2 O and alcohol (Topsoe), with decomp. (Birnbaum, Zeit. Oh. 1867. 520.) Lead wo/iochloroplatinate, [PtCl(OH) 6 ]Pb, Pb(OH) 2 . Ppt. (Bellucci, Chem. Soc. 1902, 82, II. 155.) Lead pentachloroplatinate, basic, PtCl 6 (OH)Pb, Pb(OH) 2 . (Miolati, Chem. Soc. 1900, 78. (2) 732.) Lithium chloroplatinate, Li 2 PtCl 6 -|-6H 2 O. Extremely deliquescent (Jorgensen) ; efflor- escent. Easily sol. in H 2 O, alcohol, or ether- alcohol; insol. in ether. (Scheibler.) Lithium perctachloroplatinate, OH.PtCl 6 Li 2 . Very hydroscopic. (Miolati, Chem. Soc. 1900, 78 (2) 732.) CHLOROPLATINAXE, POTASSIUM 241 Magnesium chloroplatinate, MgPtCl 6 +6H 2 O. Sol. in H 2 O and abs. alcohol. +12H 2 O. Sol. in H 2 O. Manganese chloroplatinate, MnPtCl 6 +6H 2 O. Not deliquescent; sol. in H 2 O. +12H 2 O. SI. efflorescent. Nickel chloroplatinate, NiPtCl 6 +6H 2 O. Sol. in H 2 0. Potassium chloroplatinate, K 2 PtCl 6 . 100 pts. H 2 dissolve at: 10 20 30 40 50 0.74 0.90 1.12 1.41 1.76 2.17 pts. K 2 PtCl 6 , 60 70 80 90 100 2.64 3.19 3.79 4.45 5.18 pts. K 2 PtCl 6 . (Bunsen, Pogg. 113. 337.) Sol. in KOH+Aq. Insol. in cold or hot alkali carbonates or bicarbonates+Aq. (Rose. Easily sol. in warm Na 2 S 2 O 3 + Aq. (Himly.) Sol. in NH 4 Cl+Aq. (Brett.) Sol. in NH 4 succinate+Aq. (Dopping.) At 15-20, sol. in 12,083 pts. absolute al- cohol, in 3775 pts. 76% absolute alcohol, and in 1053 pts. 55% absolute alcohol. (Fresen- ius.) Sol. in 1835 pts. 76% alcohol containing HC1 at 15-20. (Fresenius.) Nearly absolutely insol. in alcohol con- taining ether. Sol. in 42,600 pts. absolute alcohol. (Precht, Z. anal. 18. 509.) 1 1. methyl alcohol dissolves 0.072 g. at 20. (Peligot, Monit. Sci. 1892, (4) 6. I, 873.) Solubility in methyl alcohol +Aq at 20. 100 pts. H 2 O dissolve 0.926 pt. at 15 , and 5.26 pts. at 100. (Crookes, C. N. 9. 205.) 100 g. H 2 O dissolve at: 2 16 25 35 48 0.4812 0.6718 0.8641 1.132 1.745g.K 2 PtCl 6 , 59 68 78 92 2.396 2.913 3.589 4.484 g. K 2 PtCl 6 . (Archibald, J. Am. Chem. Soc. 1908, 30. 752.) Not attacked by cold cone. H 2 SO 4 . (Las- saigne.) SI. sol. in cold, more easily in hot dil. acids. Less sol. in KCl+Aq than in H 2 O, and nearly insol. in sat. KCl+Aq. (Schrotter, W. A. B. 50, 2. 268.) Solubility in KCl+Aq at 20. % alcohol by wt. G. KoPtCle in 100 g. of solution 5 10 20 30 40 50 60 70 80 90 100 0.7742 0.5350 0.4120 0.2642 0.1831 0.1165 0.0625 0.0325 0.0182 0.0124 0.0038 0.0027 (Archibald, J. Am. Chem. Soc. 1908, 30. 755.) Solubility in ethyl alcohol +Aq at 20. G. mol. KC1 per 1. of KC1 +Aq. G. K 2 PtCl6 in 100 g. of solution. % alcohol by wt. G. KzPtCle in 100 g. of solution 0.00 0.20 0.25 0.50 1.00 2.00 3.00 4.00 sat. 0.7742 0.0236 0.0207 0.0109 0.0046 0.0045 0.0043 0.0042 0.0034 5 10 20 30 40 50 60 70 80 90 100 0.7742 0.4910 0.3720 0.2180 0.1340 0.0760 0.0491 0.0265 0.0128 0.0085 0,0025 0.0009 (Archibald, J. Am. Chem. Soc. 1908, 30. 757.) Solubility in NaCl+Aq at 16. G. mol. NaCl per litre of NaCl+Aq. G. K 2 PtCl 6 in 100 g. of solution (Archibald, J. Am. Chem. Soc. 1908, 30. 755.) Solubility in isobutyl alcohol +Aq at 20. 0.00 0.05 0.10 0.25 0.50 0.75 1.00 2.00 0.672 0.700 0.729 0.758 0.775 0.791 0.805 0.834 % alcohol g. KzPtClein 100 g. of solution 8.20 sat. 0.7742 0.6250 0.3180 (Archibald, J. Am. Chem. Soc. 1908, 30. 757.) (Archibald, J. Am. Chem. Soc. 1908, 30. 755.) 242 CHLOROPLATINATE, POTASSIUM Potassium pen/achloro/^roplatinate, K 2 (PtCl 5 OH). Easily sol. in H 2 O. (Ruff, B. 1913. 46. 925.) Praseodymium chloroplatinate, PrCl 3 , PtCl 4 +12H 2 O. Very sol. in H 2 O. Sol. in cone. HC1. (von Scheele, Z. anorg. 1898, 18. 353.) Rubidium chloroplatinate, Rb 2 PtCl 6 . 100 pts. H 2 O dissolve at: 10 20 0.184 0.154 0.141 pts. Rb 2 PtCl 6 , 30 40 50 0.145 0.166 0.203 pts. Rb 2 PtCl 6; 60 0.253 90 0.521 70 0.329 100 0.634 80 0.417 pts. Rb ? PtCl, pts. Rb 2 PtCl 6 . (Bunsen, Pogg. 113. 337.) Sol. in 740 pts. H 2 O at 15, and 157 pts. at 100. (Crookes, C. N. 9. 205.) Insol. in alcohol. Samarium chloroplatinate, SmCl 3 , PtCl 4 + Deliquescent. Very sol. in H 2 O. (Cleve, Bull. Soc. (2) 43. 165.) Silver chloroplatinate, Ag 2 PtCl 6 . Ppt. Gradually decomp. by H 2 O into AgCl and PtCl 4 . (Jorgensen, J. pr. (2) 16. 345.) Ag 2 PtCl 4 (OH) 2 . Ppt. Silver mo/iochloroplatinate, [PtCl(OH) 5 ]Ag 2 . Ppt. (Bellucci, Chem. Soc. 1902, 82. (2) 155.) Silver pewtochloroplatinate, (OH)PtCl 5 Ag 2 . Ppt.; stable in boiling H 2 O. (Miolati Chem. Soc. 1900, 78 (2). 732.) Silver chloroplatinate ammonia, Ag 2 PtCl 6 2NH 3 . Insol. in H 2 O. (Birnbaum.) Sodium chloroplatinate, Na 2 PtCl 6 +6H 2 O. Easily sol. in H 2 O. Sat. solution at 15 contains 39.77 g. Na 2 PtCl 6 and has sp. gr of 1.368. Sol. in NaCl+Aq. More sol. in absolute alcohol than in 95% alcohol. Sat solution in abs. alcohol contains 11.90%; 95 <7 alcohol, 6.34%. Mixture of equal parts o alcohol and ether dissolve 2.43%. Insol. in ether. (Precht, Z. anal. 18. 502.) Sodium per^achloroplatinate, (OH)PtCl 5 Na ; Exists only in solution. (Miolati, I.e.} Strontium chloroplatinate, SrPtCl s -f 8H 2 O. Very sol. in H 2 O. trontium raowochloroplatinate, PtCl(OH) 8 Sr +H 2 0. Insol. in H 2 O and org. solvents. (Bellucci, . C. 1903, I. 131.) Thallium chloroplatinate, Tl 2 PtCl 6 . Very si. sol. in H 2 O. Sol. in 15,585 pts. H 2 O at 15, and 1948 pts. at 100. (Crookes.) Thallium woochloroplatinate, [PtCl(OH) 6 ]T1 . Ppt. (Bellucci, Chem. Soc. 1902, 82. (2). 55.) Thallium pewtochloroplatinate, (OH)PtCl 5 Tl 2 . (Miolati, Chem. Soc. 1900, 78 (2). 732.) Thorium chloroplatinate, ThCl 4 , PtCl 4 -f 12H 2 O. Very deliquescent. (Cleve, Bull. Soc. (2). 21. 118.) Tin (stannic) chloroplatinate, SnCl 4 , PtCl 4 + 12H 2 O. (Nilson, B. 9. 1142.) ytterbium chloroplatinate, 2YbCl 3 , PtCl 4 + 22H 2 O, and +35H 2 O. Ppt. (Cleve, Z. anorg. 1902, 32. 137.) Vanadyl chloroplatinate, (VO)PtCl 4 + Sol. in H 2 O; cryst. from PtCl 4 +Aq. ^Brauner, M. 3. 58.) Yttrium chloroplatinate, 4YC1 3 , 5PtCl 4 + 52H 2 0. Very deliquescent. (Cleve.) 2YC1 3 , 3PtCl 4 +30H 2 O. (Nilson, B. 9. 1059.) 2YC1 3 , PtCl 4 +21H 2 O. (Nilson.) Zinc chloroplatinate, ZnPtCl 6 +6H 2 O. Deliquescent; sol. in H 2 O and alcohol. Zinc tefrachloroplatinate, ZnPt(OH) 2 Cl 4 + 5H 2 O. Extremely sol. in H 2 O and alcohol. (Mio- lati, Z. anorg. 1900, 22. 458.) Zirconyl chloroplatinate, (ZrO)PtCl 6 +12H 2 O. (Nilson.) Chloroplatinoanhydropf/rophosphoric acid, ClPtP 2 6 H 4 = ClPt ' > O \PO(OH) 2 . Not deliquescent. Sol. in H 2 O. (Schiitzen- berger, Bull. Soc. (2) 18. 154.) Chloroplatinocyanhydric acid, H 2 Pt(CN) 4 Cl 2 . See Perchloroplatinocyanhydric acid. CHLOROPLATINITE, MAGNESIUM 243 Potassium chloroplatinocyanide, 5K 2 Pt(CN) 4 , K 2 Pt(CN) 4 Cl 2 +21H 2 O. Sol. in H 2 O; insol. in alcohol. Silver chloroplatinocyanide, Ag 2 (PtCl 2 (CN) 4 ) 2 . Ppt. (Miolati, C. C. 1901, I. 500.) Chloroplatinophosphoric acid, Cl 2 PtP(OH) 3 . Very deliquescent, and sol. in H 2 O. (Schiitzenberger, Bull. Soc. (2) 17. 493.) Lead chloroplatinophosphate, Pb 3 (Cl 2 PtPO 3 ) 2 +8H 2 0. Ppt. Pb 3 (Cl 2 PtP0 3 )2, 2PbO+4H 2 0. Ppt. (Schiitzenberger, Bull. Soc. (2) 17. 494.) Silver chloroplatinophosphate, Ag 2 HPO 3 , PtCl 2 . Ppt. (Schutzenberger, Bull. Soc. (2) 17. 494.) ChloroplatinofHphosphoric acid, PtCl 2 , P 2 (OH) 6 . Very deliquescent, and easily sol. in H 2 O. (Schutzenberger, Bull. Soc. (2) 18. 153.) Chloroplatino/wrophosphoric acid. ^P(OH), ClPt'^O \P(OH) 3 . Less deliquescent than chloroplatinoGfa'phos- phoric acid. Chloroplatinous acid, H 2 PtCl 4 . Known only in solution. Aluminum chloroplatinite, AlPtCl 5 +10HH 2 O. Very deliquescent; sol. in H 2 O. (Nilson, J. pr. (2) 15. 260.) Ammonium chloroplatinite, (NH 4 ) 2 PtCl 4 . SI. sol. in cold, easily in hot H 2 O. Insol. in alcohol. (Peyrone, A. 55. 206.) Barium chloroplatinite, BaPtCl 4 +3H 2 O. Not deliquescent; sol. in H 2 O. Very si. sol. in 93% alcohol. Cadmium chloroplatinite ammonia. CdPtCl 4 , 4NH 3 . Insol. in H 2 O or NH 4 OH+Aq. Sol. in HCl+Aq. (Thomsen, B. 2. 668.) Caesium chloroplatinite, Cs 2 PtCl 4 . SI. sol. in cold, easily in hot H 2 O. 100 pts. H 2 O dissolve 3.4 pts. salt at 20 " " 6.73 " " 40 " " 8.68 " " 60 " " 10.92 " " 80 " 12.10 " " (Godeffroy, A. 181. 176.) 100. Cs 2 PtCl 5 . Ppt. Very sensitive to sun- light. Decomp. by H 2 O into the higher and lower chlorides. (Wohler, B. 1909, 42. 4104.) Calcium chloroplatinite, CaPtCl 4 +8H 2 O. Deliquescent; sol. in H 2 O. Cerium chloroplatinite, CeCl 3 , 2PtCl 2 + Deliquescent; easily sol. in H 2 O. (Nilson, B. 9. 1847.) Chromium chloroplatinite, Cr 2 Pt 3 Cli 2 + 18H 2 O. Deliquescent. Cobalt chloroplatinite, CoPtCl 4 +6H 2 O. SI. deliquescent in moist, efflorescent in dry air. Copper chloroplatinite, CuPtCl 4 +6H 2 O. Extremely deliquescent. (Topsoe.) Copper chloroplatinite ammonia (cupram- monium chloroplatinite), Cu(NH 3 ) 4 PtCl 4 . Insol. in H 2 O or NH 4 OH+Aq; easily sol. in H 2 SO 4 +Aq. (Millon and Commaille, C. R. 57. 822.) Didymium chloroplatinite, DiCl 3 , 2PtCl 2 -f- 10H 2 O. Deliquescent; very sol. in H 2 O. (Nilson.) 2DiCl 3 , 3PtCl 2 + 18H 2 O. As above. (Nil- son.) Erbium chloroplatinite, ErPtCl 5 +13^H 2 O. Deliquescent. Er 2 Pt 3 Cli 2 +24H 2 O. Deliquescent in moist air. Glucinum chloroplatinite, GlPtCl 4 +5H 2 O. Deliquescent in moist air. Sol. in H 2 O in all proportions. Iron (ferrous) chloroplatinite, FePtCl 4 -f 7H 2 O. Deliquescent. Rather si. sol. in cold, very sol. in hot H 2 O. (Nilson.) Lanthanum chloroplatinite, La 2 Pt 3 Cli 2 +18, and 27H 2 O. Deliquescent. Lead chloroplatinite, PbPtCl 4 . Insol. in cold H 2 O. Lithium chloroplatinite, Li 2 PtCl 4 +6H 2 O. Sol. in H 2 O. Magnesium chloroplatinite, MgPtCl 4 +6H 2 O. Not very deliquescent; very sol. in H 2 O. 244 CHLOROPLATINITE, MANGANESE Manganese chloroplatinite, MnPtCl 4 +6H 2 O. As the Mg salt. Mercurous chloroplatinite. Ppt. Nickel chloroplatinite, NiPtCl 4 +6H 2 O. As the Co salt. Potassium chloroplatinite, K 2 PtCl 4 . Moderately sol. in H 2 O; insol. in alcohol. Rubidium chloroplatinite, Rb 2 PtCl 4 . SI. sol. in colfl; easily in hot H 2 O. Silver chloroplatinite, Ag 2 PtCl 4 . Insol. in H 2 O. NH 4 OH+Aq dissolves out AgCl. (Lang.) AgCl, PtCl 2 (?). As above. (Commaille, Bull. Soc. (2) 6. 262.) Silver chloroplatinite ammonia, Ag 2 PtCl 4 , 4NH 3 . (Thomsen.) Sodium chloroplatinite, Na 2 PtCl 4 -f 4H 2 O. Deliquescent; very sol. in H 2 O. Strontium chloroplatinite, SrPtCl 4 +6H 2 O. Deliquescent. Very sol. in H 2 O. Thallium chloroplatinite, Tl 2 PtCl 4 . Very si. sol. even in boiling H 2 O. Thorium chloroplatinite, Th 2 Pt 3 Cli 4 -f-24H 2 O. Very deliquescent. Yttrium chloroplatinite, Y 2 Pt 3 Cli 2 +24H 2 O. Deliquescent. Zinc chloroplatinite, ZnPtCl 4 +6H 2 O. SI. sol. in cold, more easily in hot H 2 O; insol. in alcohol. Zinc chloroplatinite ammonia, ZnPtCl 4 , SI. sol. in H 2 O; easily sol. in HCl+Aq. Insol. in alcohol. (Thomsen, J. B. 1868. 278.) Zirconyl chloroplatinite, (ZrQ)PtCl 4 +8H 2 O. (Nilson.) Tnchloroplatinous acid, H 2 Pt(OH)Cl 3 . Sol. in H 2 O. (Miolati, Z. anorg. 1902. 33. 265.) +H 2 O. (Nilson, J. pr. (2) 15. 260.) Lead fnchloroplatinite, PbPt(OH)Cl 3 . Ppt. (Miolati.) Silver fn'chloroplatinite, Ag 2 Pt(OH)Cl 3 . Ppt. (Miolati.) Chloroplatosulphurous acid. Ammonium chloroplatosulphite, acid, NH 4 PtClSO 3 , H 2 SO 3 +4H 2 O. Sol. in H 2 0. (Birnbaum, A. 152. 149.) Ammonium chloroplatosulphite chloride sul- phite, NH 4 PtClS0 3 , (NH 4 ) 2 S0 3 , NH 4 C1. Very deliquescent. (Birnbaum.) Ammonium chloroplatosulphite sulphite, NH 4 ClPtS0 3 , (NH 4 ) 2 S0 3 +3H 2 0. Sol. in H 2 O. (Birnbaum.) Barium chloroplatosulphite chloride am- monium chloride, Ba(ClPtSO 3 ) 2 , Ba(PtClSO 3 )Cl, 6NH 4 C1+3H 2 O. Sol. in H 2 O. (Birnbaum.) Potassium chloroplatosulphite ammonium chloride, KPtClSO 3 , 2NH 4 C1. Very deliquescent. (Birnbaum, A. 152. 142.) e chloride, Potassium chloroplatosulphit KPtClSO 3 , 2KC1. Deliquescent; sol. in H 2 O. (Birnbaum, A. 152. 145.) Potassium chloroplatosulphite ammonium potassium sulphite, KPtClSO 3 , (NH 4 )KSO 3 +3H 2 O. Very deliquescent. (Birnbaum, A. 159. 120.) Sodium chloroplatosulphite ammonium chlo- ride, NaPtClSO 3 , 2NH 4 C1. Very deliquescent. (Birnbaum, A. 159. 117.) Chloroplumbic acid, H 2 PbCl 6 . Decomp. in solution on standing. (Gut- bier, J. pr. 1914, (2) 90. 497.) Ammonium chloroplumbate, (NH 4 ) 2 PbCl 6 . Ppt. Difficultly sol. in a small amount of H 2 O. Solution decomp. slowly when cold, more rapidly when warmed. Decomp. by a large amount of H 2 O. Sol. without decomp. in 20% HC1. Decomp. by dil. acids and alkalis. (Elbs, Z. Elektrochem. 1903, 9. 778.) Difficultly sol. in small amount of H 2 and solution decomp. slowly in the cold, more rapidly when warmed. Decomp. by a large amount of H 2 O. (Gutbier, J. pr. 1914, (2) 90. 498.) Sol. in cold HNO 3 without decomp. (Fried- rich, M. 1893, 14. 511.) Insol. in cone. NH 4 Cl+Aq. (Nikoljukin, B. 18. 370 R.) 5NH 4 C1, 2PbCl 4 . Not hygroscopic. De- comp. by H 2 O with pptn. of PbO 2 . Sol. in HCl+Aq and in cold HNO 3 +Aq without CHLOROPURPUREOCOBALTIC CHLORIDE 245 decomp. (Classen and Zahorski, Z. anorg. 4. 100.) Composition is 2NH 4 C1, PbCl 4 . (Fried- rich, W. A. B. 102, 2b. 527.) Caesium chloroplumbate, Cs 2 PbCl 6 . Nearly absolutely insol. in cone. CsCl+Aq in presence of Cl. (Wells, Z. anorg. 4. 335.) 1 com. cone. HCl+Aq containing PbCl 4 dis- solves 0.000049 g. Cs 2 PbCl 6 . (Wells, Z. anorg. 4. 341.) Reacts with H 2 as the corresponding am- monium salt. (Gutbier, J. pr. 1914, (2) 90. 500.) Potassium chloroplumbate, K 2 PbCl 6 . Decomp. by H 2 0; sol. in KCl+Aq. (Wells, Z. anorg. 4. 335.) Readily decomp. in the air. (Gutbier, J. pr. 1914,, (2) 90. 499.) Rubidium chloroplumbate, Rb 2 PbCl 6 . Decomp. by H 2 0; si. sol. in cone. RbCl + Aq. (Wells, Z. anorg. 4. 335.) 1 ccm. cone. HCl+Aq. containing PbCl 4 dissolves 0.003 g. Rb 2 PbCl s . (Wells, Z. unorg. 4 341.) Reacts with H 2 O as the corresponding am- monium salt. (Gutbier, J. pr. 1914, (2) 90. 499.) Decomp. by cone. H 2 SO 4 . Insol. in 96% alcohol. (Erdmann, A. 1896, 294. 76.) Chloropurpureochromium bromide, CrCl(NH 3 ) 5 Br 2 . Somewhat more easily sol. in H 2 O than the chloride. (Jorgensen, J. pr. (2) 20. 105.) chloride, CrCl(NH 8 ) 6 Cl 2 . Difficultly sol. in cold, and decomp. by hot H 2 0. 1 pt. dissolves in 154 pts. H 2 at 16. Insol. in cone. HCl+Aq. More sol. in dil. H 2 SO 4 +Aq than in H 2 O. Sol. in NH 4 OH + Aq without decomp. (Jorgensen, J. pr. (2) 20. 105.) mercuric chloride, CrCl(NH 3 )6Cl 2 , . 3HgCl 2 . Very difficultly sol. in H 2 O. (Jorgensen.) chloroplatinate, CrCl(NH 3 )5(PtCl 6 ). Extremely difficultly sol. in H 2 O. (Jorgen- sen.) chromate, CrCl(NH 3 ) 6 (CrO 4 ). SI. sol. in H 2 O; si. more sol. than chloro- purpureocobalt chromate. (Jorgensen.) dithionate, CrCl(NH 3 )5(S 2 O 6 ). Very si. sol. in cold, but much more easily in hot H 2 O. (Jorgensen.) Chloropurpureochromium f errocyanide. [CrCl(NH 3 ) 6 ] 2 Fe(CN) 6 +4H 2 0. Very difficultly sol. in cold H 2 O. (Jorgen- sen.) - fluosilicate, CrCl(NH 8 ) 6 (SiF 6 ). Very difficultly sol. in H 2 O. Insol. in H 2 SiF 6 +Aq. (Jorgensen, J. pr. (2) 20. 105.) mercuric iodide, CrCl(NH 3 )5l 2 , 2HgI 2 . Decomp. bv H 2 0: sol. in alcohol and warm KCN+Aq. " CrCl(NH 3 ) 5 I 2 , HgI 2 . Very difficultly sol. in cold H 2 O; easily sol. in KCN+Aq. (Jor- gensen, I.e.) nitrate, CrCl(NH 3 ) 6 (N0 3 ) 2 . Sol. in 71 pts. H 2 O at 17.5. Insol. in HNOs+Aq. (Jorgensen.) oxalate, CrCl(NH 3 ) 5 C 2 O 4 . Very si. sol. in cold H 2 0. (Jorgensen, I.e.) ~ sulphate, CrCl(NH 3 ) 5 SO 4 +2H 2 O. Sol. in H 2 O; precipitated by alcohol. (Jor- gensen.) sulphate, acid,[CrCl(NH 3 ) 5 ] 4 S0 4 (HS0 4 )6. Quite sol. in H 2 O. (Jorgensen, J. pr. (2) 20. 185.) pe^asulphide, CrCl(NH 3 ) 6 S 5 . Very si. sol. in cold, easily sol. in warm H 2 O. Decomp. by dil. HCl+Aq. Insol. in alcohol. (Jorgensen.) Chloropurpureocobaltic bromide, CoCKNH 3 ) 6 Br 2 . Properties resemble the chloride very closely. Sol. in 214 pts. H 2 O at 14.3 (Jor- gensen, J. pr. (2) 18. 205.) mercuric bromide, 4CoCl(NH 3 ) 5 Br 2 , 9HgBr 2 . Ppt. (J.) bromoplatinate, CoCl(NH 3 ) 6 Br 2 , PtBr 4 . Very si. sol. in H 2 O. (J.) carbonate, CoCl(NH 3 ) 5 CO 3 +4^H 2 O. Efflorescent; very easily sol. in H 2 O. (J.) chloride, CoCl(NH 3 ) 5 Cl 2 . Very si. sol. in cold, more easily in hot H 2 0. Sol. in 244 pts. H 2 O at 15.5. (Claudet, Phil. Mag. J. (4) 2. 253.) In 287 pts. H 2 O at 10.2 and 255 pts. at 11.5. (Rose, Pogg. 20. 152.) 100 pts. H 2 O dissolve 0.232 pt. CoCl 3 , 5NH,, at 0, and 1.031 pts. at 46.6. (Kurnakoff, J. Russ. Soc. 24. 629.) SI. decomp. by cold, completely by boiling H 2 O: decomp. prevented by a little HC1. Pptd. from aqueous solution by alcohol, HC1, 246 CHLOROPURPUREOCOBALTIC ANTIMONY CHLORIDE or sat. KC1 or NaCl+Aq; not decomp. by boiling HCl+Aq. (Claudet, I.e.] IN early insol. in cold, but sol. in hot H 2 O, to which a few drops of HC1 have been added. Less sol. in dil. HCl+Aq than luteocobaltic chlor- ide. (Rogojski, A. ch. (3) 41. 447.) Insol. in alcohol. (Gibbs and Genth.) Chloropurpureocobaltic antimony chloride, 2CoCl(NH 3 ) 5 Cl 2 , SbCl 3 . Ppt. Decomp. by H 2 O. (Gibbs.) bismuth chloride. Insol. in cone. HC1. Easilv decomp. by H 2 0. (Gibbs.) mercuric chloride, CoCl(NH 3 ) 5 Cl 2 , 3HgCl 2 . Insol. in cold, less sol. in hot H 2 O than Chloropurpureocobaltic chloride. Insol. in cold fuming HCl+Aq; si. sol. in hot HC1+ Aq, separating on cooling; si. sol. in hot aqua regia; moderately sol. in hot HNO 3 +Aq; partly sol. in cold cone. H 2 SO 4 , wholly on warming. Easily sol. in warm H 2 C 2 O 4 +Aq. Insol. in HgCl 2 +Aq. Moderately sol. in NH 4 OH+Aq or (NH 4 ) 2 CO 3 +Aq. (Carstanjen.) CoCl(NH 3 ) 5 Cl 2 , 2HgCl 2 . SI. sol. in cold, but much more easily in hot H 2 O.. (Gibbs, Proc. Am. Acad. 10. 33.) - chlcropalladite, CoCl(NH 3 ) 5 Cl 2 , PdCl 2 . SI. sol. in cold, moderately sol. in hot H 2 O. (Carstanjen.) - chloroplatinate, CoCl(NH 3 ) 5 Cl 2 , PtCl 4 . Nearly insol. in cold. Very si. sol. in hot H 2 O. (Gibbs and Genth, Sill. Am. J. (2) 23. 319.) - chromate, CoCl(NH 3 ) 5 CrO 4 . Very si. sol. in H 2 O. (J.) - dichromate, CoCl(NH 3 ) 5 Cr 2 7 . Much more easily sol. in H 2 O than the neutral salt. (J.) dithionate, CoCl(NH 3 ) 5 S 2 O 6 . Very si. sol. in cold, more easily in hot H,0. (J.) manganic fluoride. Ppt. SI. sol. in dil. HF+Aq. (Christen- sen, J. pr. (2) 35. 161.) fluosilicate, CoCl(NH 3 ) 5 SiF 6 . Very si. sol. in HF+Aq. - iodide, CoCl(NH 3 ) 6 I 2 . Much more sol. in H 2 O than bromide or chloride. Sol. in 54.5 pts. H 2 O at 15.6, and 50 pts. at 19.3. (J.) Chloropurpureocobaltic mercuric iodide, CoCl(NH s ) 5 I 2 , 2HgI 2 . SI. sol. in H 2 O. (J.) CoCl(NH 3 ) 5 l 2 , HgI 2 . Verv si. sol. in cold H 2 0. (J.) nitrate, CoCl(NH 3 ) 5 (NO 3 ) 2 . Sol. in 80 pts. H 2 O at 15. Rather easily sol. in hot H 2 O. (Jorgensen, J. pr. (2) 18. 209.) oxalate, CoCl(NH 3 ) 5 C 2 O 4 . SI. sol. in H 2 O. (J.) - p^/rophosphate, CoCl(NH 3 ) 5 (H 2 P 2 O 7 ). SI. and very slowly sol. in cold, much more easily in warm H 2 O. (J.) [CoCl(NH 3 ) 5 ] 2 P 2 7 +zH 2 0. Quite easily sol. in H 2 O. cfo'phosphopentamolybdate, [CoCl(NH 3 ) 5 ] 2 (5MoO 3 , 2HPO 4 ). Ppt. Nearly insol. in pure H 2 O; more sol. in dil. H 2 SO 4 +Aq without decomp. (J.) [CoCl(NH 3 ) 5 ] 2 (5MoO 3 , 2NH 4 PO 4 ). Ppt. As above. sulphate, CoCl(NH 3 ) 6 SO 4 . Anhydrous. Slowly sol. in 128-131.9 pts. H 2 O at 16. +2H 2 O. Sol. in 133.4 pts. H 2 O at 17.3. Rather easily sol. in hot H 2 O, and much more rapidly than the anhydrous salt. (J.) [CoCl(NH 3 ) 5 ] 4 SO 4 (SO 4 H) 6 . Decomp. by H 2 O into neutral sulphate. Sol. in H 2 SO 4 . tartrate, CoCl(NH 3 ) 5 (C 4 H 5 O 6 ) 2 + Moderately sol. in H 2 O; insol. in alcohol. - thiosulphate, CoCl(NH 3 ) 5 S 2 O 3 . Nearly insol. in cold H 2 O; very si. sol. in boiling H 2 O with partial decomp. (J.) Chloropurpureoiridium comps. See Iridopentamine comps. Chloropurpureorhodium carbonate, ClRh(NH 3 ) 5 CO 3 +H 2 O. Easily sol. in H 2 O. (Jorgensen.) - chloride, ClRh(NH 3 ) 5 Cl 2 . Sol. in 179 pts. H 2 O at 17, and more easily in hot H 2 O. Sol. in cone. H 2 SO 4 or boiling NaOH+Aq without decomp. Very si. sol. in cold dil. HCl+Aq (1 : 1). SI. sol. in hot HC1 +Aq. Insol. in alcohol. (Jorgensen, J. pr. (2) 27. 433; 34. 394.) - - rhodium chloride, 3ClRh(NH 3 ) 5 Cl 2 , 2RhCl 3 . Ppt. (Jorgensen, Z. anorg. 5. 75.) CHLORORUTHENATE, RUBIDIUM 247 Chloropurpureorhodium chloroplatinate, ClRh(NH 3 ) 5 PtCl6. Insol. in cold H 2 O. (J.) fluosilicate, ClRh(NH 3 )5SiF 6 . Very si. sol. in cold H 2 O. Sol. in NaOH + Aq as roseo salt. (J.) -hydroxide, ClRh(NH 3 ) 5 (OH) 2 . Known only in solution. (J.) nitrate, ClRh(NH 3 )5(NO 3 ) 2 . SI. sol. in cold H 2 O, but more easily than the chloride. Sol. in boiling NaOH+Aq as roseo salt. (J). sulphate, ClRh(NH 3 ) 5 SO 4 +2H 2 O. SI. sol. in cold, more easily in hot H 2 O. (J.) 4ClRh(NH 3 ) 5 SO 4 , 3H 2 SO 4 . SI. sol. in cold, more easily in hot H 2 O. (J.) Chlororhodous acid. Ammonium chlororhodite, (NH 4 ) 2 RhCl 5 + B 2 0. (Gutbier, B. 1908, 41. 213.) Sol. in HoO; insol. in alcohol. (Wollaston.) Not obtainable. (Leidie, A. ch. (6) 17. 275.) (NH 4 ) 3 RhCl 6 +lKH 2 O. Sol. in H 2 O, but less easily than Na salt; insol. in alcohol. Sol. in dil. NH 4 Cl+Aq. (Glaus, J. B. 1865. 423.) (Gutbier, 1. c.) Ammonium chlororhodite nitrate, (NH 4 ) 3 Rh 2 Cl 6 , 2NH 4 NO 3 . Very sol. in H 2 O. Decomp. by boiling with H 2 O. SI. sol. in HNO 3 +Aq. (Leidie, C. R. 107.234.) Barium chlororhodite, Ba 3 (RhCl 6 ) 2 . Resembles the Na salt. (Bunsen, A. 146. 276.) Caesium chlororhodite, Cs 2 RhCl 5 +H 2 O. Difficulty sol. in H 2 O. (Gutbier, B. 1908, 41. 214.) Lead chlororhodite, Pb 3 (RhCl 6 ) 2 . Ppt. Insol. in H 2 O. (Glaus.) Not obtain- able. (Leidie.) Mercurous chlororhodite, Hg 3 RhGle. Ppt. Insol. in H 2 O. (Glaus.) Not obtain- able. (Leidie.) Potassium chlororhodite, K 2 RhCl 5 +H 2 O. Not efflorescent. SI. sol. in H 2 O. SI. sol. in KC1 Aq. (Gibbs.) Insol. or si. sol. in alcohol. (Berzelius.) Salt is anhydrous. (Leidie.) Contains IHoO. (Seubert and Kobbe, B. 23. 2556.) Can be cryst. from H 2 O containing a little HC1. (Gutbier, B. 1908, 41. 212. K 3 RhCl 6 +3H 2 0. Efflorescent. SI. sol. in H 2 O. Aqueous solution decomp. to above on standing. (Glaus.) Not obtainable. (Leidie".) Also obtained by Seubert and Kobbe. (B. 23. 2556.) . (Leidie, C. R. 111. 106.) Rubidium chlororhodite, Rb 2 RhCl 6 +H 2 O. Difficulty sol. in H 2 O. (Gutbier, B. 1908, 41, 214. Silver chlororhodite, Ag 3 RhCl 6 . Ppt. Insol. in H 2 0. (Glaus.) Not obtainable. (Leidie.) Sodium chlororhodite, Na6Rh,Cl 12 + 18H 2 O. Na 3 RhCl 3 +9H 2 0. Efflorescent. Sol. in 1.5 p*ts. H 2 O. Melts in crystal H 2 O at 50. Insol. in alcohol. (Glaus.) +12H 2 O. (Gutbier, B. 1908, 41. 213.) Chlororuthenic acid. Ammonium chlororuthenate, (NH 4 ) 2 RuCI 6 . Easily sol. in H 2 O. (Glaus.) Formula is (NH 4 ) 2 Ru(NO)Cl 5 . (Joly, C. R, 107. 994.) Sol. in H 2 O with decomp. Sol. in HC1. (Howe, J. Am. Chem. Soc. 1904, 26. 549.) Ammonium agwochlororuthenate, (NH 4 ) 2 Ru(H 2 O)Cl 5 . Ppt. (Howe, J. Am. Chem. Soc. 1904, 26. 548.) Cassium chlororuthenate, Cs 2 RuCle. SI. sol. in H 2 O. Sol. in hot dil. HCl+Aq. (Howe, J. Am. Chem. Soc. 1901, 23. 784.) Potassium chlororuthenate, K 2 RuCl 6 . Very sol. in H 2 O. Very si. sol. in cone. NH 4 Cl+Aq. Insol. in 70% alcohol. (Glaus.) Formula is K 2 Ru(NO)Cl 5 . (Joly.j Very si. sol. in cold H 2 O. Insol. in pres- ence of KC1. Partially decomp. in hot aqueous solution. (Antony, Gazz. ch. it. 1899, 29. (2), 82.) Easily sol. in H 2 O with rapid decomp. Sol. in HC1. (Howe, J. Am. Chem. Soc. 1904, 26. 548.) Potassium ag-wochlororuthenate, K 2 Ru(OH 2 )Gl 6 . Sol. in H 2 O. (Howe, J. Am. Chem. Soc. 1904, 26. 547.) Rubidium chlororuthenate, Rb 2 RuCl. SI. sol. in H 2 O; sol. in hot dil. HCl+Aq. (Howe, J. Am. Chem. Soc. 1901, 23. 784.) 248 CHLORORUTHENIOUS ACID Chlororuthenious acid. Ammonium chlororuthenite, (NH 4 ) 4 Ru 2 Clio. SI. sol. in H 2 O. Insol. in NH 4 Cl+Aq or alcohol. (Glaus, J. pr. 80. 282.) Caesium chlororuthenite, Cs 2 RuCl 5 +H 2 0. SI. sol. in H 2 O; sol. in HCl+Aq. (Howe, J. Am. Chem. Soc. 1901, 23. 785.) Potassium cblororuthenite, K 4 Ru 2 Cli9. Moderately sol. in cold, more easily in hot H 2 O. Decomp. easily by heating. Insol. in ng. % cone. NH 4 Cl-f Aq. Insol. in 80% alcohol. Rubidium chlororuthenite, Rb 2 RuCl6+H 2 0. SI. sol. in H 2 O; sol. in HCl+Aq. (Howe, J. Am. Chem. Soc. 1901, 23. 786.) Sodium chlororuthenite, Na 4 Ru 2 Clio. Deliquescent* Sol. in H 2 O or alcohol. Tn'chlorosilicomercaptane. See Silicon chlcrohydrosulphide. Chlorosmic acid. Ammonium chlorosmate, (NH 4 ) 2 OsCl 6 . SI. sol. in H 2 0. Insol. in alcohol and H 2 O containing HC1. Potassium chlorosmate, K 2 OsCl 6 . Properties as the NH 4 salt. Potassium amino chlorosmate, (NH 2 )OsCl 3 ,2KCl. Ppt. (Brizard, A. ch. 1900, (7) 21. 375.) Potassium amino, chlorosmate hydrogen Chloride, (NH 2 )CsGl 3 ,2KCl,HCl. Ppt. (Brizard, A. ch. 1900, (7) 21. 378.) Silver chlorosmate, Ag 2 OsCl 6 . Irspl. in H 2 O or HNO 3 -j-Aq. (Claus and Jacoby.) Silver chlorosmate ammonia, Ag 2 OsCl 6 , 2NH 8 . Sol. in much H 2 O. SI. sol. in KOH+Aq. Easily sol. in KCN+Aq. (C.andJ.) Sodium chlorosmate, Na 2 OsCl 6 +2H 2 0. Easily sol. in H 2 O or alcohol. Chlorosmious acid. Ammonium chlorosmite, (NH 4 ) 4 Os 2 Cl 10 +3H 2 O. Easily sol. in H 2 O and alcohol; insol. in ether. (Claus and Jacoby, J. pr. 90. 65.) Potassium chlorosmite, K 6 Os 2 Cl 12 +6H 2 O. Very easily sol. in H 2 O or alcohol. Insol. in ether. (C. and J.) Chlorosmisulphurous acid. Potassium hydrogen chlorosmisulphite, OsCl 4 (SO 3 ) 4 K 6 H 2 . Ppt. (Rosenheim, Z. anorg. 190Q, 24. 422.) Sodium chlorosmisulphite, OsCl 2 (SO 3 ) 4 Na 6 +10H 2 O. Ppt, 420.) (Rosenheim, Z. anorg. 1900, 24. Chloropi/roselenious acid. Ammonium chloropz/roselenite, NH 4 C1, 2SeO 2 +2H 2 O. Sol. in H 2 O. (Muthmann and Schafer, B. 26. 1008.) Potassium chloropyroselenite, KC1, 2SeO 2 + H 2 O. AsNH 4 salt. (M.andS.) Rubidium chlorop^/roselenite, RbCl, 2SeO 2 +2H 2 O. As NH 4 salt. (M. and S.) Chlorostannic acid, SnO(OH)Cl. (Mallet, Chem. Soc. 35. 524.) H 2 SnCl 6 +6H 2 O. Extremely deliquescent; sol. in H 2 O. (Seubert, B. 20. 793.) Ammonium chlorostannate, (NH 4 ) 2 SnCl 6 (pink salt). Sol. in 3 pts. H 2 O at 14.5. Solution de- comp. on boiling when dilute, but not when cone. (Bolley.) Barium chlorostannate, BaSnCle+5H 2 O. Sol. in H 2 O. (Lewy, A. ch. (3) 16. 308.) Caesium chlorostannate, Cs 2 SnCle. Nearly insol. in cone. HCl+Aq. (Sharp- ies, Sill. Am. J. (2) 47. 178.) Calcium chlorostannate, CaSnCl 6 +5H 2 O. Very deliquescent. (Lewy, A. ch. (3) 16. 308.) Cerium chlorostannate, CeSnCl 7 +9H 2 O. Deliquescent. Sol. in H 2 O. (Cleve, Bull . Soc. (2) 31. 197.) Cobalt chlorostannate, CoSnCl 6 +6H 2 O. Sol. in H 2 O. (Jorgensen.) Didymium chlorostannate, DiCl 3 , SnCl 4 + 10^H 2 0. Sol. in H 2 O. (Cleve.) Glucinum chlorostannate, GlSnCl 6 +8H 2 O. Deliquescent. Sol. in H 2 O. (Atterberg, Sv. V. A. Handl. 12. No. 4. 14.) CHLOROTELLURATE, RUBIDIUM 249 Lanthanum chlorostannate, 4LaCl 3 , 5SnCl 4 + 45H 2 O. Deliquescent. Sol. in H 2 O. (Cleve.) Lithium chlorostannate, Li 2 SnCl 6 +8H 2 O. Sol. in little H 2 O without decomp., but decomp. by dilution. (Chassevant, A. ch. (6) 30. 42.) Magnesium chlorostannate, MgSnCl 6 +6H 2 O. Very deliquescent. (Lewy.) Manganous chlorostannate, MnSnCl 6 +6H 2 O. Deliquescent in moist, efflorescent in dry air. (Jorgensen.) Nickel chlorostannate, NiSnCl 6 +6H 2 O. Sol. in H 2 O. (Jorgensen.) Potassium chlorostannate, K 2 SnCl 6 . Sol. in H 2 O. Sodium chlorostannate, Na 2 SnCl 6 +6H 2 O. Easily sol. in H 2 O. (Topsoe, Gm. K. Handb. 6te aufl. III. 149.) Strontium chlorostannate, SrSnCl 6 +8H 2 0. SI. deliquescent, and easily sol. in H 2 O. (Topsoe.) Yttrium chlorostannate, YC1 3 , SnCl 4 +8H 2 0. Sol. in H 2 O. (Cleve, Bull. Soc. (2) 31.197.) Zinc chlorostannate, ZnSnCl 6 +6H 2 O. (Biron, C. C. 1904, II. 410.) Chlorosulphobismuthous acid. Cuprous chlorosulphobismuthite, 2Cu 2 S, Bi 2 S 3 , 2BiSCl. Stable in air and insol. in H 2 O at ord. temp. Decomp. by boiling H 2 0. Decomp. by mineral acids with evolution of H 2 S. (Ducatte, C. R. 1902, 134. 1212.) Lead chlorosulphobismuthite, PbS, Bi 2 S 3 , 2BiSCl. Stable in the air. Insol. in H 2 O; decomp. by boiling H 2 O; sol. in dil. acids with de- comp. and evolution of H 2 S. (Ducatte.) Chlorosulphonic acid, HC1S0 3 . See Sulphuryl hydroxyl chloride. Chloropi/rosulphonic acid. Ammonium chlorop^/rosulphonate, C1S 2 O 6 NH 4 . Fumes in the air. Decomp. by H 2 O and alcohol. (Traube, B. 1913, 46. 2519.) Sodium chloropi/rosulphonate, ClS 2 O 6 Na. Fumes in the air. Decomp. by H 2 O and alcohol. (Traube.) Chlorosulphuric acid, HS0 8 C1. See Sulphuryl hydroxyl chloride. SO 2 C1 2 . See Sulphuryl chloride. Aluminum chlorosulphate, A1(SO 4 )C1+6H 2 O. Very sol. in H 2 O. Nearly insol. in abs. alcohol. (Recoura, Bull. Soc. 1902, (3) 27. 1155.) Chromium chlorosulphate, CrClSO 4 +5H 2 O. Green. (Weinland, Z. anorg. 1905, 48. 253.) (Recoura, C. R. 1902, 135. 164.) Violet. (Weinland, Z. anorg. 1905, 48. 254.) Very sol. in H 2 O. Insol. in a mixture of alcohol and acetone. (Recoura, C. R. 1902, 135. 164.) +8H 2 O. Two isomeric modifications: (a) Green needles. Easily sol. in H 2 O. (Weinland, Z. anorg: 1906, 48. 251.) (b) Violet plates. Easily sol. in H 2 O. (Weinland.) Chlorosulphurous acid. Ammonium palladious tfnchlorosulphite, (NH 4 ) 3 PdCl 3 S0 3 +H 2 O. Easily sol. in H 2 0. (Rosenheim, Z. anorg. 1900, 23. 30. Chlorotelluric acid. Ammonium chlorotellurate, (NH 4 ) 2 TeCl 6 . Sol. without decomp. in a small amt. of H 2 O, but decomp. by much H 2 O or alcohol. Caesium chlorotellurate, Cs 2 TeCl 6 . Decomp. by H 2 O. Sol. in dil. HCl+Aq. 100 pts. HCl+Aq (sp. gr. 1.2) dissolve 0.05 pt. at 22. 100 pts. HCl+Aq (sp. gr. 1.05) dissolve 0.78 pt. at 22. Insol. in alcohol. (Wheeler, Sill. Am. J. 145. 267.) Potassium chlorotellurate, K 2 TeCl 6 . Deliquescent; decomp. by H 2 O and abso- lute alcohol. (Berzelius.) The most sol. in H 2 O of the chloro- or bromo-tellurates. Easily sol. in dil. HC1 + Aq; cone. HCl+Aq ppts. KC1. (Wheeler, Sill. Am. J. 145. 267.) Rubidium chlorotellurate, Rb 2 TeCl 6 . Decomp. by H 2 O. Much more sol. in dil. HCl+Aq than Cs 2 TeTl 6 . 100 pts. HCl+Aq (sp. gr. 1.2) dissolve 0.34 pt. at 22. 100 pts. HCl+Aq (sp. gr. 1.05) dissolve, 13.99 pts. at 22. SI. sol. in alcohol. (Wheeler.) 250 CHLOROTETRAMINE CHROMIUM BROMIDE Chlorotetramine chromium bromide, ClCr(NH 3 )4(OH 2 )Br 2 . Very easily sol. in H 2 O. (Cleve, 1861, (Jorgensen, j". pr. (2) 42. 210.) chloride, ClCr(NH 3 ) 4 (OH 2 )Cl 2 . Sol. in H 2 O, but decomp. by boiling. Sol. in HCl+Aq, and this solution may be boiled without decomp. (Cleve.) Sol. in 15.7 pts. H 2 O at 15. (Jorgensen, J. pr. 42. 208.) chromate, ClCr(NH 3 ) 4 (OH 2 )CrO 4 . Precipitate. (Cleve.) fluosilicate, ClCr(NH 3 ) 4 (OH 2 )SiF 6 . SI. sol. in H 2 O. (Jorgensen, J. pr. (2) 42. 218.) - hydroxide, ClCr(NH 3 ) 4 (OH) 2 . Known only in solution. (Cleve.) iodide, ClCr(NH 3 ) 4 (OH 2 )I 2 . Easily sol. in H 2 O. (Cleve.) - nitrate, ClCr(NH 3 ) 4 (OH 2 )(NO 3 ) 2 . Very easily sol. in H 2 O. (Cleve); (Jorgen- sen, J. pr. (2) 42. 209.) - sulphate, ClCr(NH 3 ) 4 (OH 2 )SO 4 . Very difficulty sol. in cold, more easily in hotH 2 O. (Cleve.) Chlorotetramine cobaltic bromide, ClCo(NH 3 ) 4 (OH 2 )Br 2 . More sol. in H 2 O than chloride. Nearly insol. in HBr+Aq/l:l). (Jorgensen, J. pr. (2) 42. 215.) - chloride, ClCo(NH 3 ) 4 (OH 2 )Cl 2 . Sol. in about 40 pts. H 2 O, and is identical with octamine cobaltic purpureochloride of Vortmann. (Jorgensen, J. pr. (2) 42. 211.) chloroplatinate, ClCo(NH 3 ) 4 (OH,)PtCl 6 +2H 2 0. SI. sol. in H 2 O. (Jorgensen.) - chromate, ClCo(NH 3 ) 4 (OH 2 )CrO 4 . Easily sol. in cold H 2 O. (Jorgensen, J. pr. .(2)42.216.) - fluosilicate, ClCo(NH 3 ) 4 (OH 2 )SiF 6 . SI. sol. in H 2 O. Nearly insol. in H 2 SiF 6 + Aq. (Jorgensen, J. pr. (2) 42. 219.) - sulphate, ClCo(NH 3 ) 4 (OH 2 )SO 4 . Sol. in H 2 O. (Jorgensen, J. pr. (2) 42. 214.) Chlorotitanic acid, TiCl 4 ,2HCl = H 2 TiCl 6 . Known only in solution. (Kowalewsky, Z. anorg. 1900, 25. 192.) Chlorous acid, HC10 2 . Known only in aqueous solution. 100 g. H 2 O at 8.5 and 753 mm. pressure dissolve 4.7 g. C1 2 O 3 . Hydrate with 50.07-67.43% H 2 O, perhaps HC1O 2 +H 2 O, separates out at 0. (Brandan, A. 151. 340.) Pure HC1O 2 is not known even in solution. (Garzarolli-Thurnlakh, A. 209. 184.) Chlorites. All chlorites are 'easily sol. in H 2 O and alcohol, with gradual decomp. Ammonium chlorite. Known only in aqueous solution, which decomposes on evaporation or long standing. Barium chlorite, Ba(ClO 2 ) 2 . Deliquescent; easily sol. in H 2 O. Solu- tion decomp. on evaporation. Easily sol. in alcohol. (Millon, A. ch. (3) 7. 298.) Lead chlorite, Pb(ClO 2 ) 2 . Nearly insol. in cold H 2 O, and only si. sol. in hot H 2 O. Sol. in KOH+Aq. (Garzarolli and Hayn, A. 209. 203.) Lead chlorite chloride, 6Pb(ClO,) 2 ,4PbCl 2 , PbO. Rather difficulty sol. in H 2 O. (Schiel, A. 109. 317.) Potassium chlorite, KC1O 2 . Very deliquescent and sol. in H 2 O. Sol. in alcohol of 38. (Millon, A. ch. (3) 7. 323.) Sol. in HClO 2 +Aq. Silver chlorite, AgClC 2 . Sol. in hot, less in cold H 2 O. Easily de- comp. bv heating above '100 C . Decomp. by weakest acids. (Millon, A. ch. (3) 7. 329.) Sodium chlorite, NaClO 2 . Very deliquescent, and sol. in H 2 O. Strontium chlorite, Sr(ClO 2 ) 2 . Deliquescent and sol. in H 2 O. Decomp. by slow evaporation. (Millon, A. ch. (3) 7. 327.) Chloroxyfulminoplatinum, Pt 4 N 4 Cl(OH)O 12 H 22 . Insol. in H 2 O ; sol. in HCl+Aq. (v. Meyer, J. pr. (2) 18. 305.) Chloruranic acid, HUO 3 C1+2H 2 O. Sol. in H 2 O; si. sol. in alcohol. (Mylius, B. 1901, 34. 2776.) Chromacichloride, CrO 2 Cl 2 . See Chromyl chloride. )hromatoiodic acid. See Chromoiodic acid. CHROMATE, AMMONIUM CHROMYL 251 Chromic acid, H 2 CrO 4 . Very sol. in H 2 O. (Moissan, C. R. 98. 1851.) Does not exist except in solution. (Field, Chem. Soc. 61. 405.) The composition of the hydrates formed by H 2 CrO 4 at different dilutions is calculated from determinations of the lowering of the fr-pt. produced by H 2 CrO 4 and of the con- ductivity and sp. gr. of H 2 CrO 4 +Aq. (Jones, Am. Ch. J. 1905, 34. 333.) See also Chromium ^noxide. Chromates. Chromates of the alkali metals and of Ca, Mg, and Sr are sol. in H 2 C; the others are generally insol. or si. sol. in H 2 O, but sol. in HNOs+Aq. Aluminum chromate, basic, A1 2 O 3 , CrO 3 + 7H 2 0. Easily sol. in NH 4 OH+Aq, alum, or acetic acid+Aq. Insol. in NH 4 Cl+Aq. (Farrie, Chem. Soc. 4. 300.) Insol. as such as H 2 O, but easily decomp. into H 2 CrO 4 and a basic insol. comp. Sol. in alkaline solutions and acids. Decomp. by many salts. (Eliot and Storer, Proc. Am. Acad. 5. 214.) Aluminum sodium chromate silicate, 4Al 2 O 3 ,5Na 2 O,CrO 3 ,7SiO 2 . (Weyberg, C. B. Miner, 1904. 727.) Ammonium chromate, basic, 5(NH 4 ) 2 O, 4Ci0 3 (?). Easily sol. in cold H 2 O. (Pohl, W. A. B. 6. 592.) Ammonium chromate, (NH 4 ) 2 CrO 4 . Very sol. in H 2 O; pptd. from aqueous solu- tion by alcohol. (Malaguti and Sarzeau.) 100 g. H 2 O dissolve 40.46 g. at 30. (Schreinemakers, Chem. Weekbl. 1905, 1. 395.) Sol. in H 2 O without decomp. ( Schreine- makers, C. C. 1905, II. 1067.) Sp. gr. of (NH 4 ) 2 CrO 4 +Aq at t/4. t 13 13.7 19.6 % (NH 4 ) 2 CrO 4 10.52 19.75 28.04 Sp. gr. 1.0633 1.1197 1.1727 (Slotte, W. Ann. 1881, 14. 18.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) Difficulty sol. in acetone. (Naumann, B. 1904, 37. 4328.) Ammonium ^chromate, (NH 4 ) 2 Cr 2 O 7 . Less sol. in H 2 O than (NH 4 ) 2 CrO 4 . (Moser.) . 100 g. H 2 O dissolve 47.17g at 30. (Schreinemakers, Chem. Weekbl. 1905, 1. 395.) Sp. gr. of (NH 4 ) 2 Cr 2 O 7 +Aq at t/4. t 12 10.5 12 % (NH 4 ) 2 Cr 2 O 7 6.85 13.00 19.93 Sp. gr. 1.0393 1.0782 1.1258 (Slotte, W. Ann. 1881, 14. 18.) Sol. in alcohol. (Ranitzer, Zeit. angew ch. 1913, 26. 456.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) Ammonium Jn'chromate, (NH 4 ) 2 Cr 3 Oi . Not deliquescent, but very sol. in H 2 O. (Siewert.) Decomp. by H 2 O into chromic acid and dichromate. (Jager and Kriiss, B. 22. 2036.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Ammonium te/rachromate, (NH 4 ) 2 Cr 4 Oi 3 . Deliquescent. Decomp. bv H 2 O. (Jager and Kriiss, B. 22. 2037.) Ammonium hexachromate. (NH 4 ) 2 Cr B Oi 9 + 10H 2 O (?) Very efflorescent. (Rammelsberg, Pogg. 94. 516.) Ammonium barium chromate, BaCrO 4 ,(NH 4 ) 2 CrO 4 . Ppt. Decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 414.) Ammonium cadmium chromate, (NH 4 ) 2 O, 4CdO, 4CrO 3 +3H 2 O. Ppt. Decomp. by boiling II 2 O. (Groger, M. 1904, 25. 533. Ammonium cadmium chromate ammonia, (NH 4 ) 2 CrO 4 ,CdCrO 4 , ^NH 3 + 1 ^H 2 O . Decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 418.) (NH 4 ) 2 Cd(CrO 4 ) 2 , 2NH S . Insol. in cold, decomp. by hot H 2 O. Sol. in dil. acids or in NH 4 OH+Aq. (Briggs, Chem. Soc. 1903, 83. 395.) Ammonium chromous chromate (?), (NH 4 ) 2 Cr0 4 ,CrCrO 4 = (NH 4 ) 2 Cr(CrO 4 ) 2 . Difficultly sol. in H 2 O. Insol. in alcohol, ether, chloroform, or glacial acetic acid. Easily sol. in cone, acids, from which it is separated on dilution. Decomp. by NaOH-|- Aq. (Heintze, J. pr. (2) 4. 220.) * Ammonium chromyl chromate, i3(NH 4 ) 2 O, 2CrO 2 ,3CrO 3 . Nearly insol. in H 2 O. (Pascal, C. R. 1909, 148. 1465.) 252 CHROMATE, AMMONIUM COBALTOUS Ammonium cobaltous chromate. (NH 4 ) 2 Co(CrO 4 ) 2 +6H 2 O. Ppt. Easily decomp. (Briggs, Z. anorg. 1907, 66. 247.) (NH 4 ) 2 O, 4CoO, 4CrO 3 +3H 2 O. Insol. in H 2 O. Sol. in cold dil. H 2 SO 4 . (Groger, Z. anorg. 1906, 49. 202.) Ammonium cobaltous bichromate, CoCr 2 7 ,(NH 4 ) 2 Cr 2 O 7 +2H 2 O. SI. hydroscopic; sol. in H 2 O, insol. in al- cohol. (Kruss, Z. anorg. 1895, 8. 454.) Ammonium cobaltous chromate ammonia, 3CoCrO4,(NH 4 ) 2 CrO 4 , 2NH 3 +3H 2 O. Ppt.; decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 422.) Ammonium cupric bichromate, 2CrCr 2 7 ,3(NH 4 ) 2 Cr 2 7 +6H 2 0. Sol. in H 2 O. (Kruss, Z. anorg. 1895, 8. 455.) Ammonium cupric chromate ammonia, (NH 4 ) 2 CrO 4 ,CuCrO 4 ,2NH 3 . Decomp. by H 2 O. (Groger, Z. anorg. 1908, 68. 420.) Insol. in cold, decomp. by hot H 2 O. Sol. in dil. acids or in NH 4 OH+Aq. (Briggs, Chem. Soc. 1903, 83. 394.) Ammonium iron (ferric) chromate, (NH 4 ) 2 CrO 4 ,Fe 2 (CrO 4 ) 3 +4H 2 O. More easily decomp. by H 2 O than K 2 CrO 4 , Fe 2 (CrO 4 ) 3 +4H 2 O. (Hensgen, B. 12. 1300.) 6CrO 3 , 5Fe 2 O 3 , 6(NH 4 ) 2 O, and 4CrO 8 , Fe 2 O 3 ,(NH 4 ) 2 O+4H 2 O. Ppts. (Lepierre, C. R. 1894, 119. 1217.) Ammonium lithium chromate, NH 4 LiCrO 4 -f 2H 2 0. Not deliquescent. (Rammelsberg.) Ammonium lead chromate. (NH 4 ) 2 CrO 4 , PbCr0 4 . Ppt. Decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 424.) Ammonium magnesium chromate, (NH 4 ) 2 Cr0 4 , MgCr0 4 +6H 2 0. Much more sol. in H a O than the correspond- ing sulphate, (v. Hauer.) Sol. in H 2 O. (Groger, Z. anorg. 1908, 58. 416.) Ammonium manganous chromate, (NH 4 ) 2 CrO 4 , 2MnCrO 4 . Sol. in H 2 O. (Hensgen, R. t. c. 3. 433.) Ammonium nickel chromate, (NH 4 ) 2 CrO 4 , NiCrO 4 +6H 2 O. Sol. in H 2 O. (Groger, Z. anorg. 1906, 51. 353.) Can be cryst. from H 2 O under 40. (Briggs, Chem. Soc. 1903, 83. 392.) Ammonium nickel chromate ammonia, (NH 4 ) 2 CrO 4 ,NiCrO 4 ,NH 3 +H 2 O. Decomp. by H 2 O. (Groger, Z. anorg. 1906, 51. 354.) (NH 4 ) 2 Ni(CrO 4 ) 2 , 2NH 3 . Insol. in cold H 2 O. Decomp. by hot H 2 O. Sol. in dil. acids or in NH 4 OH+Aq. .(Briggs, Chem. Soc. 1903, 83. 393.) +6H 2 O. (Briggs, Proc. Chem. Soc. 1902, 18. 254.) Ammonium potassium chromate, NH 4 KCr0 4 . Sol. in H 2 O. (E. Kopp, C. N. 11. 16.) +H 2 O. (Etard, C. R. 85. 443.) 2(NH 4 ) 2 CrO 4 , 3K 2 CrO 4 . Very sol. in H 2 O. (Zehenter, M. 1897, 18. 51.) Ammonium silver chromate, (NH 4 ) 2 CrO 4 , 3Ag 2 CrO4. Decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 423.) Ammonium sodium chromate, NH 4 NaCrO 4 + 2H 2 O. Very sol. in H 2 O. (Zehenter, M. 1897, 18. 54.) ' Ammonium strontium chromate, (NH 4 ) 2 CrO 4 , SrCrO 4 . Ppt. Decomp. by H 2 O. (Groger, Z. anorg. 1P08, 58. 415.) Ammonium uranyl chromate, (NH 4 ) 2 CrO 4 , 2(UO 2 )CrO 4 +6H 2 O. Decomp. by boiling with H 2 O. Sol. in acidulated H 2 O. (Formanek, A. 257, 106.) +3H 2 O. (Formanek.) Ammonium zinc chromate, (NH 4 ) 2 O, 2ZnO, 2Cr0 3 +H 2 O. Decomp. by hot H 2 O. (Groger, M. 1904, 25. 520.) Ammonium zinc chromate ammonia, (NH 4 ) 2 Zn(Cr0 4 ) 2 , 2NH 3 . Insol. in cold, decomp. by hot H 2 O. Sol. in dil. acids or in NH 4 OH+Aq. (Briggs,, Chem. Soc. 1903, 83. 394.) 4ZnCrO 4 , 2(NH 4 ) 2 CrO 4 , 3NH 3 +3H 2 O. Ppt. Decomp. by H 2 O. (Groger, Z. .anorg. 1908, 58. 416.) Ammonium bichromate chloride mercuric chloride, (NH 4 ) 2 Cr 2 O 7 ,2NH 4 Cl,4HgCl 2 + 2H 2 O. Ppt. Sol. in cold, more sol. in warm H 2 0. (Stromholm, Z. anorg. 1912, 76. 280.) Ammonium bichromate chloride mercuric cyanide, (NH 4 ) 2 Cr 2 O 7 , 4NH 4 C1, 6Hg(CN) 2 +4H 2 0. (Stromholm, Z. anorg. 1913, 80. 157.) CHROMATE, BISMUTH, BASIC 253 Ammonium chromate chromyl fluoride, (NH 4 ) 2 CrO 4 , CrO 2 F 2 . Sol. in H 2 O. (Varenne, C. R. 91. 989.) Ammonium chromate iodate. See Chromoiodate, ammonium. Ammonium cfa'chromate mercuric chloride. (NH 4 ) 2 Cr 2 7 , HgCl 2 . Cannot be recryst, from H 2 O or HgCl 2 +Aq, but from (NH 4 ) 2 Cr 2 O 7 +Aq. (Jager and Kriiss, B. 22. 2044.) +H 2 O. (Richmond and Abel, Chem. Soc. Q. J. 3. 199.) Cannot be made to crystallize with H 2 O. (Jager and Kriiss.) 3(NH 4 ) 2 Cr 2 O 7 , HgCl 2 . Decomp. by H 2 O. (J. and K.) 4(NH 4 ) 2 Cr 2 O 7 , HgCl 2 . Decomp. by H 2 O. (J. and K.) (NH 4 ) 2 Cr 2 O 7 , 3HgCl 2 . (J. and K.) ' (NH 4 ) 2 Cr 2 O 7 , 4HgCl 2 . (J. and K.) Ammonium chromate phosphate. See Phosphochromate, ammonium. Ammonium chromate tellurate. See Chromotellurate, ammonium. Barium chromate, BaCrO 4 . Extremely si. sol. in HaO. Calculated from electrical conductivity of BaCrO 4 +Aq, 1 1. H 2 O dissolves 3.8 *mg. BaCrO 4 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) When not ignited, BaCrO 4 is sol. in 86,957 pts. H 2 0; 22,988 pts. NH 4 Cl+Aq (0.5% NH 4 C1); 3670 pts. HC 2 H 3 O 2 +Aq (5% HC 2 H 3 O 2 ); 1986 pts. HC 2 H 3 2 +Aq (10% HC 2 H 3 O 2 ); 1813 pts. H 2 CrO 4 +Aq(10% CrUa). When ignited, 160,000 pts. H 2 O are necessary for solution. (Schweitzer, by Fre- senius, Z. anal. 29. 414.) Sol. in 23,000 pts. boiling H 2 O. (Mescher- zerski, Z. anal. 21. 399.) 3.5 mg. BaCr0 4 are dissolved in 1 1. of sat. solution at 18 r . (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Easily sol. in HNO 3 ,HC1, or chromic acid + Aq, from which it is precipitated by NH 4 OH, or by dilution with H 2 O. (Bahr.) Insol. in K 2 Cr 2 O 7 +Aq. (Schweitzer.) Sol. in 4P.381 pts. NH 4 C 2 H 3 O 2 +Aq (0.75 % salt) at 15; in 23,355 pts. NH 4 C 2 H 3 O 2 +Aq (1.5% salt) at 15; in 45,162 pts. NH 4 N0 3 +Aq (0.5% salt) at 15. (Fresenius, Z. anal. 29. 418.) Easily sol. in alkali tartrates, or citrates + Aq. (Fleischer, J. pr. (2) 6. 326.) C.22X10- 4 g. equiv. BaCrO 4 are dissolved in 1 1. of 45% alcohol at ord. temp. (Guerini, Dissert, 1912.) Insol. in acetic acid and in M 2 Cr 2 O 7 +Aq. Partly sol. in a mixture of the two, except in presence of MC 2 H 3 O 2 . (Caron and Raquet, Bull. Sor. 1906, (3) 36. 1064.) Not completely insol. in acetic acid. (Bau- bigny, Bull. Soc. 1907, (4) 1. 58.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Barium ^chromate, BaCr 2 O 7 +2H 2 O. Decomp. by H 2 O with separation of BaCrO 4 . Sol. in H 2 CrO 4 +Aq. (Bahr, J. B. 1853. 358.) Sol. in cold H 2 O with formation of BaCrO 4 and CrO 3 . Insol. in glacial acetic acid. (Mayer, B. 1903, 36. 1742.) Barium calcium chromate, BaCa(CrO 4 ) 2 . (Bourgeois Bull. Soc. Min. 1879, 2. 124.) Barium potassium chromate, BaK 2 (CrO 4 ) 2 . Decomp. by H 2 O. (Groger, Z. anorg. 1907, 54. 186.) Decomp. by H 2 O. Stable in K 2 CrO 4 -fAq, containing: 2.181 pts. K 2 CrO 4 per 100 pts. H 2 O at 11.5 3.395 " " " " " " " 27 5 5.120 " " " " " " " 50.0 7.119 " " " " " " " 76.0 9.036 " " " " " " "100.0* (Barre, C. R. 1914, 158. 497.) Barium potassium fn'chromate, Ba 2 K 2 (Cr 3 Oio)3+3H 2 O. Extremely deliquescent. (Bahr.) Bismuth chromates, basic. These comps. are insol. in H 2 O even in presence of H 2 Cr0 4 ; sol. in HC1 or HNOj-f- Aq. (Lowe, J. pr. 67. 288.; 100 pts. H 2 O dissolve 0.00008 pt. "bis- muth chromate"; 100 pts. acetic acid dis- solve 0.00021 pt. "bismuth chromate"; 100 pts. HNO 3 +Aq (sp. gr. = 1.038) dissolve 0.00024 pt. "bismuth chromate"; 100 pts. KOH+Aq (sp. gr. = 1.33) dissolve 0.00016 pt. "bismuth chromate." (Pearson, Phil. Mag. (4) 11. 206.) Not insol. in dil. HNO+Aq unless K 2 CrO 4 is present. Less sol. in hot NaOH+Aq than PbCrO 4 . (Storer.) "Bismuth chromate" is insol. in acetone. (Naumann, B. 1904, 37. 4329.) 3Bi 2 O 3 , 2CrO 3 =2(BiO) 2 CrO 4 , Bi 2 O 3 . Insol. in H 2 O; sol. in HNO 3 +Aq. Bi 2 O 3 , CrO 3 = (BiO) 2 CrO 4 . Insol. in H 2 O; easily sol. in dil. HCl+Aq, less in dil. HNO or H 2 SO 4 +Aq. (Muir.) Bi 2 O 3 , 2CrO 3 = (BiO) 2 Cr 2 O 7 . Insol. in H 2 0. +H 2 0. 5Bi 2 O 3 , HCrO 3 +6H 2 O. . (Muir, Chem. Soc. 31. 24.) 254 CHROMATE, BISMUTH, ACID 3Bi 2 O 3 , 7CrO 3 . Insol. in H 2 O; easily sol. in mineral acids, especially HCl+Aq. Partly sol. inKOH+Aq. Bismuth chromate, acid, Bi 2 O 3 , 4CrO 3 +H 2 O. Insol. in hot or cold H 2 O. Sol. in dil. HC1 or HNOs+Aq. (Muir, Chem. Soc. 30. 17.) Bismuth potassium chromate, Bi 2 (CrO4) 3 , K 2 CrO 4 . Insol. in H 2 O. Decomp. with hot H 2 O. Bi 2 O 3 , K 2 O, 6CrO 3 +H 2 O. (Preis and Ray- mann, J. B. 1880. 336.) Bromomolybdenum chromate. (Atterberg.) Cadmium chromate, basic, 2CdO, CrO 3 + H 2 O. Very si. sol. in H 2 O; very slowly sol. in NH 4 OH+Aq with combination. (Malaguti and Sarzeau, A. ch. (3) 9. 431.) Composition as above. (Freese, B. 2. 478.) Cadmium chromate, CdCrO 4 . Insol. in H 2 O; sol. in acids; decomp. by heating with H 2 O. (Schulz, Z. anorg. 1895, 10. 153.) Sol. in hot cone. CdSO 4 +Aq. (Briggs, Z. anorg. 1907, 56. 253.) +2H 2 O. Decomp. by boiling H 2 O. (Schulz, Z. anorg. 1895, 10. 153.) Cadmium t/ichromate, CdO,2CrO 3 +H 2 O. Easily sol. in H 2 O without decomp; hydroscopic. (Schulz, Z. anorg. 1895, 10. 152.) Easily sol. in H 2 O but decomp. on evapo- ration. (Groger, Z. anorg. 1910, 66. 11.) Cadmium /richromate, CdCr 3 Oi 9 +H 2 O. Deliquescent. (Groger, Z. anorg. 1910, 66. 12.) Cadmium chromate ammonia. CdCrO 4 , 4NH 3 +3H 2 O. Efflorescent. Decomp, by H 2 O. Sol. in NH 4 OH+Aq; insol. in alcohol and ether. (Malaguti and Sarzeau.) Cadmium potassium chromate, CdKo(CrO 4 ) 2 +2H 2 0. Ppt. Decomp. by H 2 O. (Groger, Z. anorg. 1907, 64. 189.) 3CdO, K 2 0, 3CrO 3 +3H 2 O. p pt . (Preis and Raymann, Sitzungsb. bohms. Gesell. 1880.) 4CdO, K 2 O, 4CrO 3 +3H 2 O. Ppt, Slowly decomp. by H 2 O. (Groger, M. 1904, 26. 533.') Cadmium potassium Bichromate, CdCr 2 7 ,K 2 Cr 2 7 +2H 2 0. Sol. in H 2 O; jsl. hydroscopic. (Kriiss, Z. anorg. 1895, 8. 454.) Cadmium Bichromate mercuric cyanide, CdCr 2 O 7 , 2Hg(CN) 2 +7H 2 O. Sol. in H 2 O without decomp. (Kriiss, Z. anorg. 1895, 8. 460.) Caesium chromate, Cs 2 CrO 4 . (Chabrie, C. R. 1901, 132. 680.) Aq. solution sat. at 30 contains 47%. (Schreinemakers, C. C. 1909, I. 11.) Caesium bichromate, Cs 2 Cr 2 O 7 . (Chabrie, C. R. 1901, 132. 680.) Much more sol. in hot H 2 O, than in cold. (Fraprie, Am. J. Sci. 1906, (4) 21. 309.) Aq. solution sat. at 30 contains 5.2. (Schreinemakers, C. C. 1909, 1. 11.) Caesium bichromate, Cs 2 Cr 3 Oi . Decomp. by H 2 O. (Schreinemakers, Chem. Weekbl. 1908, 6. 811.) Sol. in H 2 O. (Fraprie, Am. J. Sci. 1906, (4) 21. 315.) Caesium ^rachromate, Cs 2 Cr 4 Oi 3 . Sol. in H 2 O with decomp. (Schreine- makers, Chem. Weekbl. 1908, 6. 811.) Caesium cobaltous chromate, CsoCo(CrO 4 ) 2 +6H 2 O. (Briggs, Z. anorg. 1907, 66. 248.) Caesium magnesium chromate, Cs 2 Mg(CrO 4 )i>+6H 2 O. (Briggs, Chem. Soc. 1904, 85, 680.) Caesium nickel chromate, Cs 2 Ni(CrO 4 ) 2 +6H 2 0. Sol. in cold H 2 O without much change, but decomp. by warm H 2 O. (Briggs, Chem. Soc. 1904, 86. 679.) Calcium chromate basic, Ca 2 CrO 5 +3H 2 O. Sol. in 230 pts. H 2 O without decomp. (Mylius and Wrochem, Gm. K. 3. I, 1385.) Calcium chromate, CaCrO 4 . Anhydrous. Very si. sol. in H 2 O. (Sie- wert, J. B. 1862. 148.) Aq. solution, sat. at 18 contains 2.3% CaCrO 4 ; sp. gr. = 1.023. (Mylius and Wrochem, B. 1900, 33. 3688.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) + ^iH 2 O. Aq. solution sat. at 18 con- tains 4.4% CaCrO 4 ; sp. gr. = 1.044. (Mylius and Wrochem, B. 1900, 33. 3688.) +H 2 O. Solubility in H 2 O at t. t c 8 13 18 25 % CaCrO 4 11.5 10.8 10.3 9.6 9.1 t 40 60 75 90 100 % CaCrO 4 7.8 5.7 4.6 3.6 3.1 (Mylius and Wrochem, Gm.-K. 3. I, 1386.) CHROMATE, CHROMOUS POTASSIUM 255 Sp. gr. of solution containing 9.6% by wt. CaCrO 4 at 18 = 1.096. (Mylius and Wrochom, B. 1900, 33, 3688.) +2H 2 O. Sol. in 241.3 pts. H 2 O at 14. (Siewert.) Sol. in 34 pts. H 2 O. (Schwarz, Dingl. 198. 159.) Solubility of two modifications in H 2 O at t. a modification. t 20 30 45 % CaCrO 4 14.75 14.22 13.89 12.53 /3 modification. QC 18 19.5 30 40 % CaCrO 4 9.8 1C 10.3 1G.4 10.4 10.4 (Mylius and Wrochem. Gm.-K. 3. I, 1387.) a modification. Sp. gr. of the solution con- taining 14.3% by wt. CaCrO 4 at 18 = 1.149. (Mylius and Wrochem, B. 1900, 33. 3688.) p modification. Sp. gr. of the solution con- taining 10.3% by wt. CaCrO 4 at 18 = 1.105. (Mylius and Wrochem, B. 1900, 33. 3688.) Easily sol. in H 2 O containing CrO 3 . Insol. in absolute alcohol. 50 cc. of alcohol (29%) dissolve 0.608 g. CaCrO 4 ; 50 cc. of alcohol (53%) dissolve 0.44 g. CaCrO 4 . (Fresenius, Z. anal. 30. 672.) Sol. in acids and in dilute alcohol. (Caron and Raquet, Bull. Soc. 1906, (3) 35. 1064.) Calcium Bichromate, CaCr 2 O 7 +3H 2 O. Very deliquescent. (Bahr, J. pr. 60. 60.) In sat. solution at 18, 61% CaCr 2 O 7 is present. (Mylius and Wrochem, Gm.-K. 3. I, 1387.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Calcium potassium chromate, CaCrO 4 , K 2 Cr0 4 (Barre, C. R. 1914, 158. 495.) +H 2 O. Easily sol. in H 2 O. (Duncan.) Insol. in H 2 O when ignited. +2H 2 O. Easily sol. in H 2 O, even after ignition. Insol. in alcohol. (Duncan, J. B. 1850. 313.) Formed below 45. (Barre, C. R. 1914, 158. 495.) Sol. in cold H->O. SI. sol. in sat. K 2 CrO 4 + Aq. (Groger, Z. anorg. 1907, 54. 187.) Two modifications. Solubility of a modi- fication is somewhat less than that of the P modification. (Wyrouboff, Bull. Soc. Miri. 1891, 14. 255.) Solubility of two modifications in H 2 O at t. t 15 Solubility of a 23.06 25.06 a p 23.01 24.45 (Rakowski, C. C. 1909, I. 133.) 4CaCrO 4 , K 2 CrO 4 . 5CaCrO 4 , K 2 CrO 4 . Sol. in much H 2 O. (Bahr.) Calcium chromate potassium sulphate, CaCrO 4 , K 2 SO 4 +H 2 O. Decomp. by H 2 O. (Hannay, Chem. Soc. 32. 399.) CaCrO 4 , K 2 SO 4 , K 2 CrO 4 . As above. (H.) Cerous chromate. Insol. in H 2 O. Calcium strontium chromate, CaSr(CrO 4 ) 2 . (Bourgeois, Bull. Soc. Min. 1879, 2. 123.) Ceric bichromate, CeO 2 , 2CrO 3 +2H 2 O. Insol. in H 2 O; sol. in acids; decomp. com- pletely by boiling H 2 O. (Bricout, C. R. 1894, 118. 145.) Chromic chromate, CrO 2 = Cr 2 O 3 , CrO 3 . Insol. as such in H 2 O, but decomp. thereby into CrO-j and Cr 2 O 3 ; decomp. by alkaline and many saline solutions. Easily sol. in dil. acids if recently pptd, but with difficulty if dried at a high temp. (Eliot and Storer, Proc. Am. Acad. 5. 207.) Cr 5 O 12 = Cr 2 O 3 , 3CrO 3 . Sol. in HCl+Aq. Very slowly sol. in HNO 3 +Aq. Slowly de- comp. by H 2 SO 4 or NH 4 OH+Aq. Easily de- comp. by KOH+Aq. Does not exist. (Eliot and Storer, I.e.) Cr 8 O ]5 = 3Cr 2 O 3 , 2CrO 3 . Easily sol. in HC1 or HNOs+Aq: difficulty sol. in acetic acid. Easily sol. in KOH+ Aq. (Traube, A. 66. 108.) Existence doubtful. O 5 O 9 =2Cr 2 O 3 , CrO 3 . Insol. in all acids, even aqua regia; slowly attacked by a boiling cone, solution of alkali hydroxides. (Geuther and Merz, A. 118. 62.) Cr 3 O 5 , according to Wohler. Chromic cupric chromate, CuCr 4 O 9 , Cr 2 O 3 + 12H 2 O. Insol. in H 2 O and H 2 SO 4 . Sol. in HC1 and HNO 3 . (Rosenfeld, B. 1879, 12. 957.) 6CuO, Cr 2 O 3 , CrO 3 +9H 2 O. Insol. in H 2 O. Sol. in acids. (Rosenfeld, B. 1879, 12. 958.) Chromic potassium chromate, Cr 2 H 2 (CrO 4 ) 2 , K 2 CrO 4 (?). Insol. in H 2 O, alcohol, or acetic acid. Not attacked by cold HNO 3 +Aq; si. oxidized when hot. Insol. in cold, easily sol. in hot H 2 SO 4 . SI. sol. in SO 2 +Aq. Sol. in cone. HCl-fAq. (Tommasi, Bull. Soc. (2) 17. 396.) Chromous potassium chromate, K 2 CrO 4 (Cr0 2 ) 2 = K 2 Cr(CrO 4 ) 2 (?). Sat. cold solution in H 2 O contains 9% of the salt. Insol. in alcohol and ether. (Heintze, J. pr. (2) 4. 212.) 256 CHROMATE, COBALTOUS, BASIC Cobaltous chromate, basic, 3CoO, CrO 3 + Ppt. Decomp. by H 2 O. (Malaguti and Sarzeau, A. ch. (3) 9. 431.) True formula is 2CoO, CrO 3 +2H 2 O. (Freese, Pogg. 140. 252.) 4CoO, 3CrO 3 +2H 2 O. Decomp. by H 2 O. (Groger, Z. anorg. 1906, 49. 203.) Cobaltous chromate, CoCrO 4 . Much more sol. in H 2 O than NiCrO 4 . Easily sol. in hot dil. HNO 3 +Aq. (Briggs, Z. anorg. 1909, 63. 327.) +2H 2 O. Ppt. (Briggs, Z. anorg. 1909, 63. 328.) Cobaltous ^chromate, CoCr 2 O 7 +H 2 O. Deliquescent. Very sol. in H 2 O. (Briggs. Z. anorg. 1907, 66. 247.) Cobaltous potassium chromate, basic. K 2 O, 4CoO, 4CrO 3 +3H 2 O. Sol. in cold dil. H 2 SQ 4 +Aq. (Groger, Z. anorg. 1906, 49. 199.) Cobaltous potassium chromate, K 2 Co(CrO 4 ) 2 +2H 2 0. Decomp. by H 2 O. (Groger, Z. anorg. 1906, 49. 200.) Cupric chromate, basic, 3CuO, CrO 3 + 2H 2 O. Insol. in H 2 0. Easily sol. in dil. HNO 3 -f Aq and in NH 4 OH+Aq. Decomp. by KOH +Aq. (Malaguti and fearzeau, A. ch. (3) 9. 434.) 7CuO, 2CrO 3 +5H 2 O. Ppt. (Rosenfeld, B. 13. 1469.) 7CuO, CrO 3 +5H 2 0. Ppt. (R.) Cobaltous cfo'chromate mercuric cyanide, CoCr 2 O 7 , 2Hg(CN) 2 +7H 2 O. Very stable. Sol. in H 2 O. (Kriiss, Z. anorg. 1895, 8. 458.) Cupric chromate, CuCrO 4 Insol. in H 2 O; very sol. in chromic acid and in other acids; decomp. by boiling with H 2 O. (Schulz, Z. anorg. 1895, 10. 152.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Cupric di'chromate, basic, CuCr 2 O 7 , 2CuO. (Stanley, C. N. 64. 194.) Cupric ^'chromate, CuCr 2 O 7 +2H 2 O. Deliquescent. Very easily sol. in H 2 O, NH 4 OH+Aq, and alcohol. (Droge, A. 101. 39.) Aqueous solution is decomp. by boiling. (Malaguti and Sarzeau, A. ch. (3) 9. 456.) Very hygroscopic. Very sol. in H 2 O with- out decomp. (Schulz, Z. anorg. 1895, 10. 150.) Cupric tefrachromate, CuCr 4 Oi 3 +2H 2 O. Deliquescent. Decomp. when its solution in H 2 O is concentrated. (Groger, Z. anorg. 1910, 66. 15.) Cupric lead chromate, 2(PbCrO 4 , PbO), (2CuCrO 4 , CuO). Min. Vauquelinite. Sol. in acids. Cupric potassium chromate, basic, KCu 2 (OH)(CrO 4 ) 2 +H 2 O. Ppt. (Groger, M. 1903, 24. 485.) 3CuO, K 2 O, 3CrO 3 +2H 2 O. Nearly insol. in H 2 O. Sol. in NH 4 OH or (NH 4 ) 2 C0 3 +Aq. (Knop, A. 70. 52.) Does not exist. (Rosenfeld, B. 13. 1472.) 4CuO, K 2 O, 4Cr0 3 +H 2 O. Decomp. by boiling H 2 O. (Gerhardt.) +3H 2 O. Decomp. by boiling H 2 O. (Gro- ger, Dissert. 1880.) Cupric potassium chromate ammonia, K 2 Cu(CrO 4 ) 2 , 2NH 3 . Very sol. in dil. NH 3 -f-Aq. ; decomp. by H 2 0. (Briggs, Chem. Soc. 1904, 85. 672.) Cupric chromate ammonia, CuCrO 4 , 4NH 3 . Decomp. by H 2 O. Sol. in dil. NH 4 OH + Aq. (Parravano and Pasta, Gazz. ch. it. 1907, 37. (2), 255.) 4CuCrO 4 , 3NH 3 +5H 2 O. Sol. in HC1 and NH 4 OH+Aq.; insol. in organic solvents; easily sol. in AgNO 3 +Aq. (Schuyten, C. C. 1900, I. 399.) 2CuCrO 4 , 7NH 3 +H 2 O. Decomp. by H 2 O. Very sol. in dil. NH 4 OH+Aq. (Briggs, Chem. Soc. 1904, 85. 673.) 3CuO, 2CrO 3 , 10NH 3 +2H 2 O. Decomp, by H 2 O; si. sol. or insol. in alcohol, ether, or NH 4 OH+Aq. (Malaguti and Sarzeau.) Decomp. by hot H 2 O; insol. in alcohol. (Bottger.) Cupric d^chromate ammonia, CuCr 2 O 7 , 4NH 3 +2H 2 0. Decomp. by H 2 O. Sol. in dil. NH 4 OH + Aq. (Parravano and Pasta, Gazz. ch. it. 1907, 37. (2) 255.) Cupric cfo'chromate mercuric cyanide, CuCr 2 O 7 , Hg(CN) 2 +5H 2 O. Not hygroscopic. Sol. in H 2 O. (Kriiss, Z. anorg. 1895, 8. 461.) Didymium chromate, Di 2 (CrO 4 ) 3 . SI. sol. in H 2 O, easily in dil. acids. (Fre- richs and Smith, A. 191. 353.) +7H 2 0. (Cleve.) Didymium potassium chromate, Di 2 (CrO 4 ) 3 , K 2 CrO 4 . Precipitate. Decomp. by H 2 O. (Cleve.) CHROMATE, LEAD 257 Dysprosium chromate, Dy 2 (CrO 4 ) 3 +10H 2 O. Very si. sol. in H 2 O. 1.0002 pt. is sol. in 100 pts. H 2 O at 25. (Jantsch, B. 1911, 44. 1276.) Glucinum chromate, basic, GlCrO 4 , 13G1O + 23H 2 O. Ppt. Insol. in H 2 O. (Creuzberg, Dingl. 163. 449.) GlCrO 4 , 6G1(OH 2 ). Ppt. Insol. in H 2 0. (Glassmann, B. 1907, 40. 2603.) Glucinum chromate, GlCrO 4 +H 2 O. Decomp. by H 2 O with separation of the basic chromate. (Glassmann, B. 1907, 40. 2603.) Gold (auric) chromate, Au 2 (CrO 4 ) 3 ,CrO 3 . Ppt. (Orloff, Ch. Z. 1907, 31. 1182.) Indium chromate. Ppt. (Meyer.) Indium bichromate. Very sol. in H 2 O. Known only in solution. Iron (ferric) chromate, basic. Decomp. by H 2 0. (Maus.) Fe 2 O 3 , CrO 3 . Insol. in H 2 O, but decomp. thereby, or by saline solutions; easily sol. in acids. Sol. in H 2 CrO 4 +Aq. (Eliot and Storer, Proc. Am. Acad. 6. 216.) Iron (ferric) bichromate. Sol. in H 2 O and alcohol. (Maus, Pogg. 9. 132.) Iron (ferric) potassium chromate, basic, 2CrO 3 , 6Fe 2 O 3 , 3K 2 O. 4CrO 3 , 3Fe 2 O 3 , 4K 2 O. 10CrO 3 , 6Fe 2 O 3 , 7K 2 O. HCrOa, 3Fe 2 O 3 , 4K 2 O+9H 2 O. 9CrO 3 , 2Fe 2 O 3 , 6K 2 O+6H 2 O. 9CrO 3 , 2Fe 2 O 3 , 6K 2 + 10H 2 O. lOCrO,, 3Fe 2 O 3 , 6K 2 O+5H 2 O. 7CrO 3 , 2Fe 2 O 3 , 2K 2 O+7H 2 O. 4CrO 3 , Fe 2 O 3 , K 2 O+4H 2 O. 6Cr0 3 , 2Fe 2 O 3 , 3K 2 O. 16CrO 3 , 4Fe 2 O 3 , 5K 2 O+8H 2 O. Above compounds are ppts., insol. in H 2 O, alcohol and ether. (Lepierre, C. R. 1894, 119, 1215-18.) Iron (ferric) potassium chromate, Fe 2 (Cr0 4 ) 3 , K 2 CrO 4 +4H 2 O. Decomp. by much H 2 O, cone. HC1, or NH 4 OH+Aq. Not decomp. by alcohol. (Hensgen, B. 12. 130C.) Iron (ferric) sodium chromate, basic, 5CrO 3 , 7Fe 2 O 3 , 4Na 2 O. Ppt. (Lepierre, C. R. 1894, 119, 1217.) Lanthanum chromate, La 2 (CrO 4 ) 3 . SI. sol. in cold, more easily in hot H 2 O; easily sol. in acids. (Frerichs and Smith, A. 191. 355.) +8H 2 O. Ppt. (Cleve.) Lanthanum potassium chromate. (Cleve.) Lead chromate, basic, 2PbO, CrO 3 (chrome red). Insol. in H 2 O; acetic acid dissolves out % the PbO. Sol. in KOH+Aq. (Badams, Pogg. 3. 221.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) 3PbO. CrO 3 . (Hermann, Pogg. 28. 162.; +H 2 O. Ppt. (Strdmholm, Z. anorg. 1904, 38. 443.) Min. Melanochroile, Phcenicocroite. Sol. in acids. PbO, PbCrO 4 . Ppt. (S.) Lead chromate, PbCrO 4 . Insol. in H 2 O. Pptd. from Pb(NO,) 2 in presence of 70,000 pts. H 2 O. (Harting.) Calculated from electrical conductivity of PbCrO 4 +Aq, 1 1. H 2 O dissolves 0.2 mg, PbCrO 4 at 18. (Kohlrausch and Rose, Z, phys. Ch. 12. 241.) 1 1. H 2 O dissolves 1.2 X KH g. PbCrO 4 at 25. (Hevesy, Z. anorg. 1913, 82. 328.) Sol. in dil. H 2 SO 4 +Aq (Storer); si. sol. in dil. HNO 3 +Aq. Sol. in 560 pts. HNO 3 +Aq of 1.12 sp. gr.; in 150 pts. HNO 3 +Aq of 1.225 sp. gr.; in 130 pts. HNOs+Aq of 1.265 sp. gr.; in 80 pts. HNO 3 +Aq of 1.395 sp. gr. (Storeys Diet.) Solubility of PbCrO 4 in HNO 3 +Aq. at 18. (Millimols. per 1.) 0.1N 0.2N 0.3N 0.4N 0.506 0.844 1.13 . 1.44 (Beck and Stegmuller, Z.c.) Easily decomp. by hot HCl+Aq. (Frese- inus.) Solubility of PbCrO 4 in HCl+Aq. (Millimols. per 1.) t 0.1N 0.2N 0.3N 0.4N 0.5N 0.6N 18 25 37 0.186 0.239 0.357 0.393 0.485 0.744 0.654 0.839 1.31 1.07 1.32 2.10 1.56 4.06 3.28 2.25 2.95 4.69 (Beck and Stegmuller, Arb. K. Gesund. Amt. 1910, 34. 446.) Insol. in HC 2 H 8 O 2 +Aq. Easily sol. in KOH, or NaOH+Aq. 1 1. KOH+Aq (YZ normal) dissolves 11.9 g. PbCrO 4 at 15 ;16.2 g. at 60; 26.1 g. at 80; 258 CHROMATE, LEAD 38.5 g. at 102. (Lachaud and Lepierre, Bull. Soc. (3) 6. 230.) Insol. in NH 4 Cl+Aq. (Brett, 1837.) Sol. in K 2 Cr 2 O 7 +Aq; almost completely insol. in NH 4 C 2 H 3 2 , or NH 4 NO 3 +Aq. Not pptd. in presence of Na citrate. (Spil- Insol. in liquid NH 3 . (Franklin, Am. Ch. 'J. 1898, 20. 828.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Min. Crocoite. Sol. in hot HCl+Aq; diffi- cultly sol. in HNO 3 +Aq; sol. in KOH+Aq. Lead bichromate, PbCr 2 O7. Decomp. by H 2 O. +2H 2 O. As above. (Preis and Raymann, B. 13. 340.) Lead lithium chromate, PbCrO 4 , Li 2 CrO 4 . (Lachaud and Lepierre, C. R. 110. 1035.) Lead potassium chromate, PbCrO 4 , K 2 Cr0 4 . Insol. in hot or cold H 2 O or in alcohol. Dil. acids dissolve out K 2 CrO 4 . (Lachaud and Lepierre, C. R. 110. 1035.) Decomp. by H 2 O. Stable in contact with solutions containing: 8.950 pts. K 2 CrO 4 per 100 pts. H 2 O at 10 8.077 " " " " " " ' 27.5 7*.629 " 7.150 " 6.145 " 4.940 (Barre, C. R. 1914, 168. 497.) 37.5 50.0 76.0 100.0 Lead sodium chromate, PbCrO 4 , NaCrO 4 . Sol. in H 2 O(?). (Lachaud and Lepierre.) PbCrO 4 , 2PbO, Na 2 CrO 4 . (L. and L.) Lithium chromate, Li 2 CrO 4 . 100 cc. of solution sat. at 18 contain 85 g. anhydrous salt. (Kohlrausch, B. A. B. 1897. 90.) 99.94 pts. are sol. in 100 pts. H 2 O at 30. ^Schreinemakers, C. C. 1905. II, 1486.) +2H 2 O. Very easily sol. in H 2 O. (Ram- ;melsberg, Pogg. 128. 323.) 100 g. H 2 O dissolve 111 g. salt at 20. (Von Weimarn, C. C. 1911. II, 1300.) Sp. gr. of solution sat. at 18 = 1.574, and contains 52.6% LiCrO 4 . (Mylius and Wro- chem, B. 1897, 30. 1718.) Lithium bichromate, Li 2 Cr 2 O 7 . 130.4 pts. are sol. in 100 pts. H 2 O at 30. (Schreinemakers, C. C. 1905. II, 1486.) +2H 2 O. Deliquescent. Sol. in H 2 0. (Rammelsberg.) Lithium potassium chromate, K 2 CrO 4 , , Li 2 Cr0 4 +^H 2 O. Hydroscopic. (Zehenter, M. 1897, 18. 54.) Magnesium chromate, MgCrO 4 . Sol. in H 2 S0 4 , and HC1; insol. in HNO 3 . (Dufau, C. R. 1896, 123. 888.) Sp. gr. of MgCrO 4 -f-Aq sat. at b/4. t 13.6 14.5 13.6 &MgCrO 4 12.31 21.86 27.71 p. gr. 1.0886 1.1641 1.2170 (Slotte, W. Ann. 1881, 14. 19.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) +7H 2 O. Easily sol. in H 2 O. (Vauquelin.) 100 cm. of solution sat. at 18 contain 60 g. MgCrO 4 . (Kohlrausch, B. A. B. 1897. 90.) Sp. gr. of solution sat. at 18 =1.422, and contains 42% MgCrO 4 . (Mylius and Wro- chem, B. 1897, 30. 1718.) +5H 2 O. Very sol. in H 2 O. (Wyrouboff, Bull. Soc. Min. 12. 60.) Magnesium bichromate, Mg 2 Cr 2 O 7 . SoL in H 2 O. SI. sol. in alcohol. (Reinitzer, Zeit. angew. 1913, 26. 456.) Magnesium potassium chromate, MgCrO 4 , K 2 CrO 4 +2H 2 O. 100 pts. H 2 O dissolve 28.2 pts. at 20; 34.3 pts. at 60. (Schweitzer.) Sol. in H 2 O. SI. sol. in sat. K 2 CrO 4 +Aq. (Groger, Z. anorg. 1907, 54. 188.) Insol. in alcohol. +6H 2 O. Efflorescent. (Briggs, Chem. Soc. 1904, 85. 679. Magnesium rubidium chromate, MgRb 2 (CrO 4 ) 2 +6H 2 O. (Briggs, Chem. Soc. 1904, 85. 679.) (Barker, Chem. Soc. 1911, 99. 1327.) Magnesium sodium chromate. (Stanley, C. N. 54. 194.) Manganous chromate, 2MnO, CrO 3 +H 2 O. Ppt. Sol. in dil. H 2 SO 4 , or HNO 3 +Aq. (Warrington and Reinsch, Schw. J. 3. 378.) Manganous potassium chromate, MnCrO 4 , K 2 CrO 4 +2H 2 O. Decomp. by H 2 0. Sol. in dil. H 2 SO 4 . (Groger, Z. anorg. 1905, 44. 459.) 2MnCrO 4 , K 2 CrO 4 +4H 2 O. Sol. in H 2 O. (Hensgen, R. t. c. 3. 433.) Mercurous chromate, basic, 4Hg 2 O, 3CrO 3 . Very si. sol. in cold, more in boiling H 2 O. SI. sol. in HNO 3 +Aq. Decomp. by HC1+ Aq. SI. sol. in NH 4 Cl+Aq or NH 4 NO 3 +Aq. (Brett.) Does not exist. (Richter, B. 15. 1489.) 3Hg 2 O, CrO 3 . Sol. in HNO 3 +Aq. (Rich- ter.) CHROMATE AMMONIA, NICKEL 259 3Hg 2 O, 2CrO s . Ppt. (Fichter, Z. anorg. 1912, 76. 350.) Mercurous chromate, Hg 2 CrO 4 . Very si. sol. in cold, more readily in hot H 2 O. SI. sol. in dil. HNO 3 +Aq; sol. in cone. HNO 3 ; sol. in KCN+Aq; insol. in Hg 2 (NO 3 ) 2 +Aq. (Rose, Pogg. 53. 124.) Less sol. in K 2 CrO 4 +Aq. than in H 2 O. (Fichter, Z. anorg. 1912, 76. 349.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Mercuric chromate, basic, 2HgO, CrO 3 . Sol. in HC1, and in HNO 3 +Aq. (Geuther.) 3HgO, CrO 3 . SI. sol. in H 2 O. (Millon.) The only true compound. All others are mixtures of HgO or HgCrO 4 with this com- pound. (Cox, Z. anorg. 1904, 40. 155.) 4HgO, CrO 3 . SI. sol. in H 2 O. (Millon, A. ch. (3) 18. 365.) 7HgO, 2CrO 3 . Easily sol. in warm HNO 3 , when freshly precipitated. Easily sol. in HCl+Aq. (Geuther, A. 106. 247.) " Does not exist. (Freese, B. 2. 477.) 5HgO, CrO 3 . Easily sol. in HCl+Aq. Very si. sol. in HNO 3 +Aq. Decomp. by H 2 O into 6HgO, CrO 3 . Insol. in H 2 O. (Jager and Kriiss, B. 22. 2049.) Mercuric chromate, HgCrO 4 . Decomp. by H 2 O and acids into basic salt. (Geuther.) Sol. in acids. Sol. in warm NH 4 C1, or NH 4 NO 3 +Aq. Sol. in Hg(NO 3 ) 2 , orHgCl 2 + Aq. Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Mercuric bichromate, HgCr 2 O 7 . Ppt. (Gawalowski, C. C. 1906. II, 1307.) Mercurous potassium chromate, Hg 2 K 2 (Cr0 4 ) 2 . Ppt.: decomp. by H 2 O. (Groger, Z. anorg. 1907,54.191.) Mercuric chromate, basic, ammonia, 12HgO, 3CrO 3 , 2NH 3 +3H 2 O. (Groger, Z. anorg. 1908, 58. 420.) Mercuric chromate ammonia, HgCrO 4 , 2NH 3 +H 2 O. (Groger, Z. anorg. 1908, 58. 419.) Mercuric chromate sulphide, 2HgCrO 4 , HgS. Not attacked by weak acids. (Palm, C. C. 1863. 121.) Nickel chromate, basic, 4NiO, CrO 3 +6H 2 O. Insol. in H 2 0; easily sol. in NH 4 OH+Aq. (Malaguti and Sarzeau, A. ch. (3) 9. 451.) 3NiO, CrO 3 +6H 2 O. Insol. in H 2 O: sol. in NH 4 OH+Aq. (Freese, J. B. 1869. 271.) 2NiO, CrO 3 +6H 2 O. As above. (Schmidt, A. 156. 19.) 5NiO, 2CrO 3 + 12H 2 O. As above. (Schmidt.) Nickel chromate, NiCrO 4 . Not attacked by boiling H 2 O. Nearly insol. in hot dil. HNO 3 . Slowly sol. in cone. HNO 3 and aqua regia. Somewhat sol. in NH 3 -fAq. (Briggs, Z. anorg, 1909, 63. 326.) Nickel ^chromate, 2NiCr 2 O 7 +3H 2 O. Slowly sol. in cold, rapidly sol. in hot H 2 O. Deliquescent. (Briggs, Z. anorg. 1907, 56. 246.) Nickel potassium chromate, NiCrO 4 , K 2 CrO 4 +2H 2 O. (Groger, Z. anorg. 1906. (Briggs, Chem. Decomp. by H 2 O. 51. 353.) +6H 2 O. Efflorescent. Soc. 1904, 85. 678.) Nickel rubidium chromate, NiRb(CrO 4 ) 2 + 6H 2 O. SI. efflorescent at ord. temp. (Briggs, Chem. Soc. 1904, 85. 678.) Nickel chromate ammonia, NiCrO 4 , 6NH 3 + 4H 2 O. Decomp. by H 2 O. Quite easily sol. in NH 4 OH+Aq of 0.96 sp. gr. (Schmidt.) In- sol. in alcohol or ether. Potassium chromate, K 2 CrO 4 , K 2 Cr 2 O 7 , etc. System: K 2 O, CrO 3 , H 2 O at 100 g. of the sat. solu- tion contain Solid phase g. K 2 O g. Cr3 3 31.18 26.06 0'54 K 2 Cr0 4 19.31 4.27 (4 17.73 5.50 (1 17.06 11.77 K 17.18 11.91 u 17.62 18.71 (I 17.63 18.72 tt 17.61 18.91 K 2 Cr0 4 +K 2 Cr 2 O 7 17.79 19.10 17.80 19.10 n 10.90 11.93 K 2 Cr 2 O 7 8.07 8.93 > 1.87 3.13 i 1.41 3.00 ( 1.42 3.01 t 0.97 3.94 1 0.78 22.38 i 1.02 38.83 i 1.26 40.10 1.36 40.41 i 1.22 41.70 (i 260 CHROMATE, POTASSIUM System: K 2 O, CrO 3 , H 2 at Continued System: K 2 O, CrO 3 , H 2 O at 30 100 g of the sat. solu- 100 g. of the sat. solu- tion contain Solid phase tion contain Solid phase g. KsO g. CrOs _ *K.(\ o PrOo g. J\2O g. i^/rv/3 46.8 26.89 6i94 KOH, 2H 2 O K 2 CrO 4 1.28 41.75 K 2 Cr 2 7 1.40 42.10 tt 22.25 3.06 t( 1.23 42.11 ft 19.52 6.99 it 1.33 42.16 ft 18.65 13.72 (i 1.31 42.28 tt 18.60 17.00 (4 1.38 42.48 tt 18.70 17.03 tt 1.40 42.68 if 19.12 20.30 11 1.47 42.93 K 2 Cr 2 7 +K 2 Cr 3 10 19.35 21.00 K 2 Cr0 4 +K 2 Cr 2 7 1.47 42.95 u 15.04 16.85 K 2 Cr 2 7 1.47 43.09 ft 14.77 16.51 1.25 44.52 K 2 Cr 3 O 10 12.28 14.57 N 1.27 44.95 ft 11.20 13.11 t( 1.18 45.84 t( 4.98 10.48 tl 1.17 46.84 tt 3.07 19.34 (( 1.36 47.22 K 2 Cr s O 10 +K 2 Cr 4 13 2.42 28.21 (I 1.36 47.31 ( 2.35 33.77 11 1.40 47.67 1 2.30 36.78 (( 1.24 48.23 K 2 Cr 4 13 2.30 40.41 (( 1.35 51.66 t 2.50 44.50 K 2 Cr 2 7 +K 2 Cr 3 Oio 1.10 53.81 2.25 49.95 K 2 Cr 3 0,o+K 2 Cr 4 Oi3 1.08 55.63 t 1.35 53.39 K 2 Cr 4 18 1.16 56.93 t 0.69 62.81 K 2 Cr 4 13 +Cr0 8 0.96 57.63 t . 62.52 Cr0 3 1 16 59.46 i 0.91 59.87 (Koppel and Blumenthal, Z. anorg. 1907, 53. 0.81 60.16 ft 235.) 0.70 61.76 K 2 Cr40 18 +Cr0 3 0.62 61.77 ft 0.57 61.78 n System: K 2 O, CrO 3 , H 2 O at 60 67 61.86 61.51 61.52 CrO 3 4, Na 2 CrO 4 . Sol. in H 2 O. (v. Hauer, J. pr. 83. 359.) 64.2 pts. are sol. in 100 pts. H 2 O at 14. (Zehenter, M. 1897, 18. 49.) Potassium strontium chromate, K 2 Sr(Cr0 4 ) 2 . Ppt. Decomp. by H 2 O. (Groger, Z. anorg. 1907, 54. 187.) Decomp. by H 2 O. Stable in contact with solutions containing: at 11.5, 2.914 pts. K 2 CrO 4 per 100 pts. H 2 O. at 27.5, 4.123 " at 50, 5.942 " " " " " " at 76, 7.920 " at 100, 9.784 " " " " " " (Barre, C. R, 1914, 158. 496.) Potassium thallium chromate, K 2 CrO 4 , Tl 2 CrO 4 . (Lachaud and Lepierre, Bull. Soc. (3) 6. 232 ) +2H 2 O. Rapidly hydrolyzed by H 2 O un- less a large excess of the CrO 4 ion is present. Readily sol. in dil. mineral acids. Difficulty sol. in K 2 Cr 2 O 7 +Aq. (Hawley, J. Am. Chem. Soc. 1907, 29. 304.). Potassium uranyl chromate, K 2 CrC>4, 2(UO 2 )CrO 4 +6H 2 O. Decomp. by boiling with H 2 O. Sol. in acidified H 2 O. (Formanek, A. 257. 103.) K 2 CrO 4 , (UO 2 )CrO 4 +H 2 O; 2K 2 CrO 4 , 3(U0 2 )Cr6 +7H 2 0: 3K 2 CrO 4 , 4(UO 2 )Cr0 4 +7H 2 0; and K 2 CrO 4 , 3(U0 2 )CiO 4 +14H 2 O. Precipitates. (Wiesner, C. C. 1882. 777.) Potassium ytterbium chromate, basic, 2KYb(Cr0 4 ) 2 +Yb(OH) 3 +15^H 2 0. Ppt. (Cleve, Z. anorg. 1902, 32. 151.) 264 CHROMATE, POTASSIUM YTTRIUM Potassium yttrium chromate, K 2 CrO 4 , Y 2 (Cr0 4 ) 3 +*H 2 0. Ppt. (Cleve.) Potassium zinc chromate, basic, K 2 O, 5ZnO, 4CrO 3 +6H 2 O, or K 2 O, 4ZnO, 3CrO 3 +3H 2 O. Slightly sol. in cold, decomp. by hot H 2 O. (Wohler.) ' K 2 O, 4ZnO, 3CrO 3 +3H 2 O. Insol. in cold, decomp. by hot H 2 O. (Groger, M. 1904, 26. 520.) Potassium zinc chromate, K 2 Zn(CrO 4 ) 2 -f 2H 2 0. Ppt. Decomp. by H 2 0. (Groger, Z. anorg. 1907, 54. 189.) Potassium bichromate chloride mercuric chloride, K 2 Cr 2 O 7 ,2KCl,4HgCl 2 +2H 2 O. Solution in H 2 sat. at 20.5 contains 6.78% salt. Salt is much more sol. in hot H 2 O. (Stromholm, Z. anorg. 1912, 76. 278.) Potassium chromate iodate. See Chromoiodate, potassium. Potassium chromate magnesium sulphate, K 2 CrO 4 , MgSO 4 +9H 2 O. Sol. in H 2 O. (Etard, C. R. 85. 443.) Potassium chromate 'mercuric chloride, K 2 CrO 4 , 2HgCl 2 . Easily sol. in H 2 O. Sol. in dil. HCl+Aq. (Darby.) Potassium Bichromate mercuric chloride, K 2 Cr 2 O 7 , HgCl 2 . Ether or absolute alcohol dissolves out HgCl 2 . (Millon, A. ch. (3) 18. 388.) Can be crystallized from H 2 O. (Jager and Kruss, B. 22. 2046.) Potassium chromate mercuric cyanide, 2K 2 Cr0 4 , 3Hg(CN) 2 . Easily sol. in H 2 O. +H 2 O. (Dexter.) Formula is K 2 OrO 4 , 2Hg(CN) 2 . (Clarke and Sterne, Am. Ch. J. 3. 352.) Potassium dichromate mercuric cyanide, K 2 Cr 2 7 , Hg(CN) 2 +2H 2 0. Sol. in H 2 O. (Wyrouboff, J. B. 1880. 309.) Potassium chromate phosphate. See Phosphochromate, potassium. Potassium chromate sulphate, K 2 CrO 4 , 6K 2 SO,. Easily sol. in H 2 O. (Boutron-Chalard.) Potassium chromate tellurate. See Chromotellurate, potassium. Rubidium chromate, Rb 2 CrO 4 . Sol. in H 2 O. (Piccard, J. pr. 86. 455.) Solubility in H 2 O at t. t % Rb 2 Cr0 4 . 7 36.65 38.27 10.3 40.22 20 42.42 30 44.11 40 46.13 50 47.44 60.4 48.90 (Schreinemakers and Filippo, Chem. Weekbl. 1906, 3. 157.) Rubidium bichromate, Rb 2 Cr 2 O 7 . Sol. in H 2 O. (Grandeau, A. ch. (3) 67 227.) Very si. sol. in H 2 O; 5% at 10, 8% at 26, 35% at 60. (Wyrouboff, Bull. Soc. Min. 1881, 4. 129.) 100 pts. H 2 O dissolve 10.46 pts. Rb 2 Cr 2 O 7 at 30. The solution contains 9.47% salt. (Schreinemakers and Filippo, Chem. Weekbl. 1906, 3. 157.) Two forms of crystals. Figures denote pts. salt per 100 pts. H 2 O. t 14 26 43 Monoclinic form 4.45 8.00 16.52 Triclinic form 4.40 7.91 16.57 (Wyrouboff, Bull. Soc. 1908, (4) 3. 7.) Solubility of monoclinic and triclinic forms. Pts. of salt in Pts. of salt in 100 pts. H 2 O 100 pts. H 2 O Temp Temp Mono- Tri- Mono- Tri- clinic clinic clinic clinic 18 5.42 4.96 40 13.22 12.90 24 6.94 6.55 50 18.94 18.77 30 9.08 8.70 60 28.1 27.3 (Stortenbeker, C. C. 1907, II. 1588.) Rubidium bichromate chloride mercuric chloride, Rb 2 Cr 2 O 7 , 2RbCl. 4HgCl 2 + 2H 2 O. Sol. in H 2 O. Solution sat. at 20.5 contains 5.35% salt. (Stromholm, Z. anorg. 1912, 75. 284.) Silver (argentous) chromate, Ag 4 CrO 4 . Sol. in dil. acids. (Wohler and Rauten- berg.) Existence very doubtful. Silver chromate, Ag 2 CrO 4 . Absolutely insol. in H 2 O. Sol. in acids, ammonia, and alkali chromates+Aq. (War- ington, A. 27. 12.) Appreciably sol. in cold, and still more in hotH 2 O. (Meineke, A. 261. 341.) 100 ccm. H 2 O dissolve 0.064 grain Ag 2 Cr0 4 at 100; 100 ccm. H 2 O containing 50 grains CHROMATE, SODIUM, BASIC of the following salts dissolve the given amts. of A g2 CrO 4 at 100: NaNO 3 , 0.064 grain; KNOs, 0.192 grain; NH 4 NO 3 , 0.320 grain; Mg(NO 8 ) 2 , 0.256 grain. (Carpenter, J. S. C. I. 5. 286.) According to electrical conductivity of Ag 2 CrO 4 +Aq, 1 1. H 2 O dissolves 28 mg. Ag 2 CrO 4 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) 1 1. H 2 O dissolves 25 mg. Ag 2 CrO 4 at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 25 mg. are contained in 1 1. of sat. solution at 18. Solubility increases unusually rapidly with temp. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Sol. in 26,378 pts. cold H 2 O and 9116 pts. HoO at 100. (Koninck and Nihoul, Zeit. angew. Ch. 1891, 5. 295.) 1 1. H 2 O dissolves 1.2X10- 4 gram, atoms of silver at 25. (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) 1 1. H 2 O dissolves 0.029 g. Ag 2 CrO 4 at 25. (Schafer, Z. anorg. 1905, 45. 310.) 1 1. H 2 O dissolves 0.0256 g. Ag 2 Cr0 4 at 18; 0.0341 g. at 27; 0.0534 g. at 50. (Whitby Z. anorg. 1910, 67. 108.) Sol. in hot NH 4 OH+Aq of sp. gr. 0.94 (15.63% NH 3 ); si. sol. in cold NH 4 OH-f Aq of sp. gr. 0.91 (24.99% NH 3 ). (Margosches, Z. anorg. 1904, 41. 73.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) , 1 1. 65% alcohol dissolves 0.0129 g. Ag 2 CrO 4 at ord. temp. (Guerini, Dissert. 1912.) Insol. in H 2 O containing acetic acid in presence of large excess of AgNOj. (Gooch and Weed, Am. J. Sci. 1908, (4) 26. 85.) Practically insol. in glacial acetic acid but somewhat sol. in dil. acetic acid. It be- haves in a similar manner toward propionic, lactic and other organic acids. The red modi- fication is more sol. than the greenish-black. (Margosches, Z. anorg. 1906, 51. 233.) Silver dzchromate, Ag 2 Cr 2 O 7 . SI. sol. in H 2 O. Easily sol. in HNO 8 , or NH 4 OH+Aq. (Warington.) Decomp. by boiling with H 2 O into CrO 3 and Ag 2 Cr0 4 . (Jager and Kriiss, B. 22. 2050.) Decomp. by cold H 2 O. (Autenrieth, B. 1902, 35. 2061.) 1 pt. is sol. in 12,000 pts. H 2 O at 15. (Mayer, B. 1903, 36. 1741.) Solubility in H 2 O at 25 = 7.3X10- 3 atoms Ag per 1. Decomp. by HNO 3 +Aq (less than 0.06 N) with separation of Ag 2 CrO 4 . (Sherrill and Russ, J. Am. Chem. Soc. 1907, 29. 1674.) Solubility of Ag 2 CrO 7 in HNO 3 +Aq at 25. Solubility of Ag 2 CrO 4 inNH 4 OH+Aqat25. Mols. HNOs per 1. Milliat. per 1. Solid Phase Mols. NH 4 OH per 1. Mols. X 103 Ag 2 CrO 4 per 1. Cr Ag 0.01 2.004 32.20 5.390 Ag 2 CrO 4 + 0.02 4.169 Ag 2 CrO 7 0.04 8.595 0.01 25.06 6.131 " 0.08 17.58 0.02 20.21 7.148 n 0.04 13.59 9.529 " (Sherrill and Russ. J . Am. Chem. Soc. 1907, 0.06 11.10 11.10 Ag 2 Cr 2 O 7 29. 1662.) 0.08 11.10 11.10 " SI. sol. in very cone. K 2 CiO 4 +Aq. Prac- 0.08+0.1AgNO 3 6.624 tically insol. in AgNO 3 +Aq. (Margosches.) (Sherrill and Russ, J. Am . Chem. Soc. 1907, Solubility of Ag 2 CrO 4 in HNO 3 +Aq at 25' 29. 1664 ) Mols. Milliat. per 1. Silver uranyl chromate, 2Ag 2 CrO 4 , UO 2 CrO 4 . HNOs per 1. Cr Ag Solid Phase Ppt. (Formanek, A. 257. 110.) 0.01 0.015 0.02 3.157 3.730 4.177 6.315 8^356 Ag 2 CrO 4 Silver chromate ammonia, Ag 2 CrO 4 , 4JNJ1 3 . Decomp. by H 2 O. Sol. in warm cone. NH 4 OH+Aq. (Mitscherlich, Pogg. 12. 141.) 0.025 OfkO 4.567 Silver bichromate mercuric cyanide, . Uo 0.04 5.803 11.62 Ag 2 Cr 2 7 , Hg(CN) 2 . 05 6 380 Sol. in cold H 2 O; very sol. in hot H 2 O 0.06 6.833 without decomp. (Kriiss, Z. anorg. 1895, 8. 0.07 7.333 456.) o!os 7^477 7.260 14.85 15.45 4-Ag 2 Cr 2 O 7 Ag 2 Cr 2 O 7 , 2Hg(CN) 2 . Scarcely sol. in cold, more readily in hot H 2 O. Sol. in hot HNO 3 + 0.10 5.647 19.01 Aq, separating on cooling. (Darby, Chem. 0.13 4.293 23.89 11 Soc. 1. 24.) 0.14 3.948 25.63 " Sodium chromate, basic, Na 4 CrO 6 -f-13H 2 0. (Sherrill and Russ. J . Am. Chem. Soc. 1907, Sol. without decomp. in H 2 O. 29. 1663.) Sat. solution at 30 contains 41.3% 266 CHROMATE, SODIUM Na 4 CrO 5 . (Schreinemakers, 1906, 55. 93.) Deliquescent. Solubility in H 2 O at t. t ' % Na 4 CrO 5 33.87 t 27.7 % Na 4 Cr0 5 40.09 Z. phys 10 35.58 35 44.09 Ch. 20.5 38.05 37 45.13 +6H 2 O. Solubility in H 2 O at t. t 17.7 19.2 21.2 % Na 2 Cr04 Mols. H 2 O to 1 mol. anhy- drous salt Mols. anhy- drous salt to 100 mols. H 2 O 43.65 44.12 44.64 11.60 11.40 11.16 8.62 8.77 8.96 (Mylius and Funk, Gm.-K. 3. I, 1379.) Na 4 CrO 5 +Aq sat. at 18 contains 37.50% Na 4 CrO 5 , and has sp. gr. = 1.446. (Mylius and Funk, B. 1900, 33. 3688.) Sodium chromate, Na 2 CrO 4 . 100 ccm. of solution sat. at 18 contain 54 g. Na 2 CrO 4 . (Kohlrausch, B. A. B. 1897. 90.) Solubility in H 2 O at t. t % Na 2 CrO4 70 80 100 55.15 55.53 55.74 (Mylius and Funk, Gm.-K. 3. I, 1379.) Na 2 CrO 4 +Aq sat. at 18 contains 40.10% Na 2 CrO 4 , and has sp. gr. = 1.432. (Mylius and Funk, B. 1900, 33. 3686.) See also +4, 6, and 10H 2 O. Sp. gr. of Na 2 CrO 4 +Aq at t/4. t 17.4 17.1 % Na 2 CrO 4 5.76 10.62 Sp. gr. 1.0576 1.1125 (Slotte, W. Ann. 1881, 14. 18.) 20.7 14.81 1.1644 +4H 2 O. Sat. solution at 30 contains 46.62% Na 2 CrO 4 . (Schreinemakers, Z. phys. Ch. 1906, 55. 93.) Solubility in H 2 O at t. t %Na 2 CrO4 t 49.5 54.5 59.5 65 %Na 2 CrO4 25.6 31.5 36 40 45 46.08 47.05 47.98 48.97 50.20 50.93 52.28 53.39 55.23 (Mylius and Funk, Gm.-K. 3. I, 1379.) Solubility in H 2 O at t. t % Na 2 Cr0 4 Mols. H 2 to 1 mol anhy- drous salt Mols. anhy- drous salt to 100 mols. H 2 28.9 29.7 31.2 46,47 46.54 47.08 10.37 10.34 10.12 9.64 9.67 9.88 (Salkowski, B. 1901, 34. 1948.) (Salkowski, B. 1901, 34. 1948.) + 10H 2 O. Deliquescent. (Kopp, A. 42. 99.) Easily sol. in H 2 O. Melts in crystal H 2 O at 23. (Berthelot.) Sp. gr. of solution sat. at 18 = 1.409, and contains 38.1 % Na 2 CrO 4 . (Mylius and Funk, B. 1897, 30. 1718.) Solubility in H 2 O at t. t %Na 2 CrO 4 10 18.5 19.5 21 24.04 33.41 41.65 44.78 47.40 (Mylius and Funk, Gm.-K. 3. I, 1379.) Sp. gr. of solution at 18 containing 40.1% Na 2 CrO 4 = 1.432. (Mylius, B. 1900, 33. 3688.) SI. sol. in alcohol. (Moser.) 100 g. absolute methyl alcohol dissolve 0.345 g. Na 2 CrO 4 at 25. ^(de Bruyn, Z. phys. Ch. 10. 783). Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Sodium efo'chromate, Na 2 Cr 2 O 7 . More sol. in H 2 O than Na 2 CrO 4 . Solubility in H 2 O at t. 93' 98 C NazCnOz 81.19 81.25 (Mylius and Funk, Gm.-K. 3. I, 1380.) Sp. gr. of aqueous solution containing 1 5 10 15 20 25% Na 2 Cr 2 O 7 , 1.007 1.035 1.071 1.105 1.141 1.171 30 35 40 45 50 % Na 2 Cr 2 O 7 . 1.208 1.245 1.280 1.313 1.343 (Stanley, C. N. 54. 194.) Sp. gr. of sat. solution containing 63.92% Na 2 r 2 O 7 at 18 = 1.745. (Mylius and Funk, B. 1900, 33. 3688.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) CHROMATE, THALLOUS 267 Sol. in acetone. (Naumann, B. 1904, 37 4328.) +2H 2 O. Deliquescent. 100 pts. H 2 O dissolve at 15 30 80 100 139 107.2 109.2 116.6 142.8 162.8 209.7 pts. salt (Stanley, C. N. 64. 194.) Solubility in H 2 O at t 17 34. 52 72 81 % Na 2 Cr 2 O 7 61.98 63.82 67.36 71.76 76.90 79.80 (Mylius and Funk, Gm.-K. 3. I, 1380.) 100 g. H 2 O at 30 dissolve 197.6 g. Na 2 Cr 2 O : or sat. solution at 30 contains 66.4%, Na 2 Cr 2 O 7 . (Schreinemakers, Z. phys. Ch 1906, 65. 97.) 100 ccm. of a solution of sodium dichro- mate in alcohol contain 5.133 g. Na 2 Cr 2 O 7 2H 2 O at 19.4. The solution decomp. rapidly. (Reinitzer, Zeit. angew. Ch. 1913, 26. 456.) The composition of the hydrates formed by Na 2 Cr 2 O 7 at different dilutions is calculated from determinations of the lowering of the fr.= pt. produced by Na 2 Cr 2 O 7 and of the conductivity and sp. gr. of Na 2 Cr 2 O 7 +Aq. (Jones, Am. ch. J. 1905, 34. 317.) Sodium ^nchromate, NaCr 3 Oi . Deliquescent. Very sol. in H 2 O. (Stanley, C. N. 54. 194.) -fH 2 O. Sat. solution at 30 contains 80% Na 2 Cr 3 O 10 . (Schreinemakers, Z. phys. Ch. 1906, 55. 94.) Solubility in H 2 O at t. t ' 15 55 99 %Na 2 Cr.,O 10 80.03 80.44 82.68 85.78 (Mylius and Funk, Gm.-K. 3. I, 1380.) Sp. gr. of sat. solution containing 80.6% Na 2 Cr 3 O 10 at 18 =2.059. (Mylius and Funk, B. 1900, 33. 3688.) Sodium tetrachr ornate, Na 2 Cr 4 Oi 3 +4H 2 0. Solubility in H 2 O at t. t ' 16 22 %Na 2 Cr 4 13 72.19 74.19 76.01 (Mylius and Funk, Gm.-K. 3. 1, 1380.) Deliquescent. Sat. solution at 18 contains 74.6% Na 2 Cr 4 O 13 and has sp. gr. = 1.926. (Mylius and Funk, B. 1900, 33. 3688.) Sodium uranyl chromate, Na 2 CrO 4 , 2(UO 2 )CrO 4 +10H 2 O. Easily sol. in H 2 O. (Formanek, A. 257. 108.) 100 pts. of the solution in H 2 O contain 52.52 pts. of the anhydrous salt at 20. (Rim- bach, B. 1904, 37. 482.) Sodium chromate silicate, Na 2 O, Cr 2 3 , 2SiO 2 +14H 2 O. Not decomp. by HCl-fAq. (Singer, Dis- sert. 1910.) 2Na 2 O, 3Cr 2 O 3 , 6SiO 2 . Not decomp. by boiling cone, acids -except HF. (Weyberg, C. B. Miner, 1908. 519.) 5Na 2 O, 2Cr 2 O 3 , HSiO 2 . (Weyberg.) 3Na 2 O, 2Cr 2 O 3 , 9.5SiO 2 . (Weyberg.) Strontium chromate, SrCrO 4 . Somewhat sol. in H 2 O. Sol. in 840 pts. H 2 O (Meschezerski, Z. anal. 21. 399); sol. in 831.8 pts. H 2 O at 15. (Fresenius, Z. anal. 29. 419.) 100 cc. H 2 O dissolve 0.4651% at 10; 1% at 20; 2.417% at 50; 3% at 100.- (Rei- chard, Ch. Z. 1903, 27. 877.) Easily sol. in HC1, HNO 3 , or H 2 CrO 4 +Aq. Sol. in 512 pts. 0.5% NH 4 Cl-fAq at 15. Sol. in 63.7 pts. 1% HC 2 H 3 O 2 +Aq at 15. Sol. in 348.8 pt.s. solution containing 0.75% NH 4 C 2 H 3 O 2 , 4 drops HC 2 H 3 O 2 , and 6 drops (NH 4 ) 2 Cr0 4 +Aq. (Fresenius.) 100 ccm. NH 4 Cl+Aq sat. at bpt. dissolve 1 g. SrCrO 4 . (Dumesnil, A. ch. 1900, (7) 20. 125.) 50 ccm. alcohol (29%) dissolve 0.0066 g. SrCrO 4 . 50 ccm. alcohol (53%) dissolve 0.001 g. SrCrO 4 . (Fresenius, Z. anal. 30. 672.) Strontium cfo'chromate, SrCr 2 O 7 . Easily sol. in H 2 O. Strontium fn'chromate, SrCr 3 Oi +3H 2 O. Very deliquescent, and sol. in H 2 O. (Preis and Raymann, B. 13. 340.) Strontium chromate mercuric hydrogen chloride, SrCrO 4 , 2HgCl 2 , HC1. According to Stromholm is SrCl 2 , SrCr 2 7 , 4HgCl 2 +H 2 O. Recryst. from H 2 O. (Imbert and Belugon, Bull. Soc., 1897, (3) 17. 471.) 2SrCrO 4 , 6HgCl 2 , HC1. (Imbert and Belu- gon.) Thallous chromate, TlCrO 4 . 100 pts. H 2 O dissolve 0.03 pt. at 60. Rupp and Zimmer, Z. anorg. 1902, 33. 157.) Ppt. Insol. in cold moderately cone. HC 2 H 3 O 2 +Aq, or in very dil. HNO 3 + Aq, and very si. sol. on boiling therewith. Dil. S"H 4 OH, and Na 2 CO 3 -f Aq have the same action. Attacked by very dil. HCl+Aq. >ol. in hot cone. HCl+Aq. Decomp. by dil. HoSO 4 +Aq. (Carstanjen.) 268 CHROMATE, THALLOUS 1 1. KOH+Aq (112 g. per 1.) dissolves about 3.5 g. Tl 2 CrO 4 on boiling, which separates out on cooling. Boiling cone. KOH+Aq (31% KOH) dis- solves 18 g. Tl 2 CrO 4 per litre. (Lepierre and Lachaud, C. R. 113. 196.) Thallous bichromate, Tl 2 Cr 2 O 7 . Insol. in H 2 O, etc. Has the same proper- ties as Tl 2 CrO 4 . Thallous bichromate, Tl 2 Cr 3 Oi . Sol. in 2814 pts. H 2 O at 15, and 438.7 pts. at 100. (Crookes.) Thallic chromate. Ppt. Thorium chromate, basic, Th(OH) 2 CrO 4 . Ppt.; unstable in solution. (Palmer, Am, Ch. J. 1895, 17. 278.) Thorium chromate, Th(CrO 4 ) 2 +H 2 O. Ppt. Sol. in HC1 and NH 4 Cl+Aq. 1 pt. is sol. in 284 pts. H 2 O at 22. (Palmer, Am. Ch. J. 1895, 17. 375 and 278.) +3H 2 O. Ppt. (Haber, M. 1897, 18. 689.) +8H 2 O. Insol. in H 2 O. (Chydenius, Pogg. 119. 54.) Tin (stannous) chromate. Ppt. Sol. in dil. acids. (Berzelius.) Tin (stannic) chromate. Ppt. (Leykauf, J. pr. 19. 127.) Uranyl chromate, basic, UO 3 , 2(UO 2 )CrO 4 +8H 2 0. Ppt. (Orloff, Ch. Z. 1907, 31. 375.) UO 3 , (UO 2 )CrO.,+6H 2 O. (Orloff.) Uranyl chromate, (UO 2 )CrO 4 +3H 2 O. 1 pt. is sol. in 13.3 pts. H 2 O at 15; slowly sol. in alcohol to give a solution which is de- comp. on boiling. (Orloff, Ch. Z. 1907, 31. 375.) + 11H 2 0. Very sol. in H 2 O. (Formanek, A. 257. 108.) Yttrium chromate. Deliquescent. Easily sol. in H 2 O. (Ber- lin.) Zinc chromate, basic, 4ZnO, Cr0 3 +3H 2 O. (GrSger, Z. anorg. 1911, 70. 135.) -f 5H 2 O. Insol. in H 2 O; sol. in hot H 2 Cr0 4 +Aq; slowly sol. in NH 4 OH+Aq. (Ma- laguti and Sarzeau, A. ch. (3) 9. 431.) 3ZnO, CrO 3 +2H 2 O. (Groger.) 2ZnO, CrO 3 +H 2 O. (Briggs, Z. anorg. 1907, 66. 254.) +1^H 2 O. Ppt. Insol. in H 2 O. Sol. in hot H 2 CrO 4 +Aq. (Prussen and Phil- lipona, A. 149. 92.) + 2H 2 O. Ppt. Not wholly insol. in H 2 O. (Prussen and Phillipona.) 3ZnO, 2CrO 3 +H 2 O. (Groger.) Zinc chromate, ZnCrO 4 . Insol. in H 2 O; very sol. in acids; decoinp. by boiling with H 2 O. (Schulze, Z. anorg. 1895, 10. 154.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +H 2 O. (Groger, Z. anorg. 1911, 70. 135.) Zinc dichromate, ZnCr 2 O 7 +3H 2 O. Hygroscopic. Very sol. in H 2 O and si. decomp. by boiling. (Schulze, Z. anorg. 1895, 10. 153.) Zinc ^'chromate, ZnCr 3 Oio+3H 2 0. Deliquescent; very sol. in H 2 O. (Groger, Z. anorg. 1910, 66. 10.) Zinc chromate ammonia, ZnCrO 4 , NH 3 + H 2 0. Decomp. by H 2 O. (Groger, Z. anorg. 1908, 58. 417.) ZnCrO 4 , 4NH 3 +5H 2 O. Decomp. by H 2 O. Sol. in NH 4 OH+Aq. Insol. in alcohol and ether. (Malaguti and Sarzeau, A. ch. (3) 9. 431.) +3H 2 O. Efflorescent. Decomp. by H 2 O. Easily sol. in dil. acids and NH 4 OH+Aq. (Bieler, A. 151. 223.) 2ZnO, 3CrO 3 , 10NH 3 +10H 2 O. Ppt. (Malaguti and Sarzeau.) Zinc bichromate mercuric cyanide, ZnCr 2 O 7 , 2Hg(CN) 2 +7H 2 0. Very sol. in H 2 0. Stable in aqueous solu- tion at 100. (Kruss, Z. anorg. 1895, 8. 460.) Perchromic acid See Perchromic acid. Chromicomolybdic acid, Cr 2 O 3 , 12MoO 3 +28H 2 0. Slowly sol. in H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29. 708.) Ammonium chromicomolybdate, 3(NH 4 ) 2 O, Cr 2 O 3 , 12MoO 3 +20H 2 O. Sol. in H 2 O. (Struve, J. pr. 61. 457; Hall, J. Am. Chem. Soc. 1907, 29. 695.) +26H 2 O. (Marckwald, Dissert, 1895.) Ammonium barium chromicomolybdate, (NH 4 ) 2 O, 22BaO, Cr 2 O 3 , 12MoO 3 + 20H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29. 707.) CHROMIUM 269 Barium chromicomolybdate, 4BaO, Cr 2 O 3 , 12Mo0 3 +15H 2 O; 4BaO, Cr 2 O 3 , 12Mo0 3 + 18H 2 O; 5BaO, Cr 2 O 3 , 12MoO 3 + 16H 2 O. Ppts. (Hall, J. Am. Chem. Soc. 1907, 29. 705.) Lead chromicomolybdate, 4PbO, Cr 2 O 3 , 12MoO 3 +22H 2 O, and +24H 2 O. Ppts. (Hall, J. Am. Chem. Soc. 1907, 29. 706.) Mercurous chromicomolybdate, 8Hg 2 O, Cr 2 O 3 , 12MoO 3 +16H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 707.) Potassium chromicomolybdate, K 2 O, Cr 2 O 3 , 3MoO s . Sol. in HCl+Aq with evolution of Cl. (Bradbury, Z. anorg. 1894, 7. 46.) 3K 2 O, Cr 2 O 3 , 12MoO 3 +20HoO. Sol. in 38.51 pts. H 2 O at 17. (Striive; Hall.) +24H 2 O. (Hall.) 4K 2 O, Cr 2 O 3 , 12MoO 3 +15H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29. 709.) 7K 2 O, 2Cr 2 O 3 , 24MoO 3 +32H 2 O. (Hall.) Silver chromicomolybdate, 5Ag 2 O, Cr 2 O 3 12MoO 3 -H7H 2 O. Ppt. (Hall.) Sodium chromicomolybdate, 3Na 2 O, Cr 2 O 3 , 12MoO 3 +21H 2 O. Efflorescent. Easily sol. in H 2 O. (Strtive. Chromic sulphuric acid. See Sulphochromic acid. Chromicyanhydric acid, H 3 Cr(CN) 6 (?). Insol. in H 2 O. (Kaiser, A. Suppl. 3. 163. Ammonium chromicyanide, (NH 4 ) 3 Cr(CN) 6 Easily sol. in H 2 O. (Kaiser. A. Suppl. 3 163.) Cupric chromicyanide, Cu 3 [Cr(CN) 6 ]2. Ppt. Insol. in dil. or cone, acids, except o heating. Insol. in NH 4 OH, or KOH+Aq (Kaiser.) Lead chromicyanide, basic, 3Pb(CN) 2 , 2Cr(CN) 3 , Pb(OH) 2 . Ppt. Sol. in HNO 3 , NaOH+Aq, or P salts +Aq. (Kaiser.) Potassium chromicyanide, K 3 Cr(CN) 6 . Very sol. in H 2 O. 100 pts. cold H 2 O dissolve 30.9 pts. sal Insol. in absolute alcohol, but somewha sol. in dil. alcohol. Sol. in cone. H 2 SO 4 without decomp. Kaiser, A. Suppl. 3. 170.) ilver chromicyanide, Ag 3 Cr(CN) 6 Insol. in all solvents, excepting KCN+Aq. Kaiser.) Sol. in large excess of HCl+Aq. SI. sol. n cold, easily sol. in hot cone. HNO 3 . Very ol. in cone. H 2 SO 4 . Insol. in hot or cold cetic acid. (Cruser, Dissert. 1896.) Chromisulphocyanhydric acid. H 3 Cr(SCN) 6 . Known only in aqueous solution. Ammonium chromisulphocyamde, (NH 4 ) 3 Cr(SCN) 6 +4H 2 O. Easily sol. in H 2 O. (Rossler, A. 141. 185.) Barium chromisulphocyanide, Ba 3 [Cr(SCN) 6 ]2 +16H 2 O. Deliquescent, and sol. in H 2 O. (R.) Lead chromisulphocyamde, Pb 3 [Cr(SCN) 6 ] 2 , 4PbO 2 H 2 +8H 2 O. Insol. in H 2 O, but decomp. thereby into Pb 2 [Cr(SCN) 5 ] 2 , 4PbO 2 H 2 +5H 2 O. Insol. nH 2 0. Potassium chromisulphocyanide, K 6 Cr(SCN) 6 +4H 2 0. ' Sol. in 0.72 pt. H 2 O, and 0.94 pt. alcohol. Silver chromisulphocyanide, Ag 6 Cr(SCN). Insol. in H 2 O or cone. HNOs+Aq. Insol. in NH 4 OH+Aq. Sol. in KCN+Aq. Sodium chromisulphocyanide, Na 6 Cr(SCN) 6 +7H 2 O. Deliquescent; sol. in H 2 O. Chromium, Two modifications (o) Not attacked by H 2 O. Easily sol. in cold HCl+Aq. SI. sol. in dil. H 2 SO 4 +Aq. (Deville.) Easily sol. in a hot mixture of 1 pt H 2 SO 4 and 20 pts. H 2 O. (Regnault, A. ch. 62. 357.) Easily sol. in warm cone. H 2 SO 4 . (Gmelin.) Very slowly sol. in hot HNO 3 +Aq. (Vauquelin.) Insol. in dil. or cone. HNO 3 +Aq. (Deville.) Very slowly (Richter), not at all (Berzelius) sol. in hot aqua regia. Easily sol. in HF+Aq. (jS) Insol. in all acids, even aqua regia (Fremy); probably contains Si. Pure Cr is sol. in cone. H 2 SO 4 , HC1 and dil. HNO 3 ; sol. in HgCl 2 +Aq. Insol. in fuming HNOj and aqua regia. (Moissan, C. R. 1894. 119, 187.) Cr prepared by aluminothermic method is sol. in haloid acids to form chromic and chromous salts, even in absence of air. (Doring, J. pr. 1902, (2) 66. 65; 1906, (2) 73. 393.) Aluminothermic Cr is active in contact 270 CHROMIUM AMMONIA COMPOUNDS with HC1, HBr, HI, HF, H 2 SO 4 , H 2 C 2 4 , i. e., sol. in cold cone, or warm dil. acids. Is inactive in contact with cone. HN0 3 , H 2 Cr 2 O 4 , HC1O 3 , HC1O 4 , H 3 PO 4 , KOH, citric, formic, acetic and tartaric acids. Cause attributed to a different electric state. (Hittorff, Z. phys. Ch. 1898, 25. 729.) Chromium ammonia compounds. See Bromotetramine chromium compounds, BrCr(NH 3 ) 4 X 2 . Bromopurpureochromium compounds, BrCr(NH 3 ) 5 X 2 . Chlorotetramine chromium compounds, ClCr(NH 3 ) 4 X 2 . Chloropurpureochromium compounds, ClCr(NH 3 ) 5 X 2 . Diamine chromium sulphocyanides, Cr(-NH 3 ) 2 (SCN) 4 M. Erythrochromium compounds, (HO)Cr 2 (NH 3 ) 10 X 2 . lodopurpureochromium compounds, ICr(NH 3 )5X 2 . lodotetramine chromium compounds, ICr(NH 3 ) 4 X 2 . Luteochromium compounds, Cr(NH 3 ) 6 X 3 . Rhodochromium compounds, (HO)Cr 2 (NH 3 ) 10 X 5 . Rhodosc chromium compounds, (HO) 3 Cr 2 (NH 3 )6X 3 . Roseochromium compounds, Cr(NH 3 ) s (OH 2 )X 4 . Xanthochromium compounds, (H0 2 )Cr(NH 3 ) 5 X 2 . Chromium arsenide, CrAs. Insol. in mineral acids. (Dieckmann, Z. anorg. 1914, 86. 294.) Cr 2 As 3 . Insol. in mineral acids. (Dieck- mann.) Chromium azoimide, CrN 3 . Pptd. by addition of alcohol and ether. Insol. in H 2 O. (Curtius, J. pr. 1900, (2) 61. 410.) Chromium boride, CrB. Insol. in HC1, dil. H 2 SO 4 , HF, HF+HNO 3 . SI. sol. in HNO 3 and in aqua regia. (Wede- kind, B. 1907, 40. 299.) Sol. in cold dil. or cone. HC1, HF, and H 2 SO 4 . (Jassonneix, C. R. 1906, 143. 1151.) Cr 3 B 2 . Sol. in cone, or dil. HF, HC1, H 2 SO 4 ; insol. in HNO 3 or alkalis +Aq. (Jas- sonneix.) Chromous bromide, CrBr 2 Sol. in H 2 O. Not deliquescent in dry ah 1 . (Moissan, C. R. 92. 1051.) Chromic bromide, CrBr 3 . Anhydrous. Insol. in H 2 O, but dissolves at once in presence of the least trace of CrBr 2 . (Bauck, A. 111. 382.) +6H 2 O. Deliquescent. Very sol. in H 2 O. H 2 O dissolves more than 2 pts. crystals at ord. temp. Very sol. in alcohol. Insol. in ether. (Recoura, C. R. 110. 1029.) Blue modification. Insol. in alcohol. (Recoura, C. R. 110. 1193.) Very hygroscopic. Easily sol. in alcohol and acetone. Insol. in ether. (Werner, A. 1902, 322. 343.) +8H 2 O. Sol.inH 2 O. (Varenne, C. R. 93. 727.) Chromium molybdenyl bromide, CrMo 3 O 4 Br 4 . Apparently wholly insol. in dil. acids. Sol. in hot cone. HCl+Aq with decomp. Insol. in M 2 Cr0 4 +Aq. (Atterberg.) -f-2H 2 O. Apparently wholly insol. in dil. acids. Sol. in hot cone. HCl+Aq with decomp. Insol. in M 2 CrO 4 +Aq. (Atterberg.) Chromic rubidium bromide, CrBr 3 , 2RbBr +H 2 0. Sol. in H 2 O with decomp. (Werner, A. 1902,322.345.) Chromic bromide ammonia. See Bromotetramine chromium bromide. Chromous bromide hydrazine, CrBr 2 , 2N 2 H 4 . Insol. in H 2 O. Sol. in acids. Insol. in alcohol, ether and similar solvents. (Traube, B. 1913,46. 1507.) Chromium carbide, Cr 4 C. (Moissan, C. R. 1894, 119. 187.) Cr 3 C 2 . Does not decomp. H 2 O at ordinary temp, or at 100; insol. in cone. HC1, HNO 3 and aqua regia; sol. in dil. HC1 (slowly) ; insol. in fused KOH; sol. in fused KNO 3 . (Moissan, Bull. Soc. 1894, (3) 117. 1016.) Chromium iron carbide, 3Fe 3 C, 2Cr 3 C 2 . Decomp. by H 2 O; sol. in gaseous hy- dracids; insol. in HNO 3 and aqua regia. (Wil- liams, C. R. 1898, 127. 484.) Chromium tungsten carbide, CW 2 , 3Cr 3 C 2 . Not attacked by acids. Slowly attacked by fused KOH or alkali carbonates. Rapidly decomp. by fused alkali nitrates or KC1O 3 . (Moissan, C. R. 1903, 137. 294.) Chromous chloride, CrCl 2 . Deliquescent. Very sol. in H 2 O with evolu- tion of much heat. (Moberg, J. pr. 29. 175.) CHROMIC CHLORIDE 271 Practically insol. in ether. Moderately sol. in absolute alcohol, methyl alcohol, and acetaldehyde. (Rohland, Z. anorg. 1899, 21. 39.) +l^HoO. (Moissan, A. ch. (5) 26. 40.) +2H 2 O. (Knight and Rich, Chem. Soc. 1911, 99. 89.) +3H 2 O. (Knight and Rich.) Chromous hydrogen chloride, 3CrCl 2 , 2HC1+ 13H 2 O. Decomp. by H 2 O. (Recoura, C. R. 100. 1227.) SI. sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Chromic chloride, CrCl 3 . Anhydrous. Peach-blossom-colored modi- fication. Insol. in pure H 2 O (Peligot), but by long continued boiling of the finely divided salt with H 2 O, traces are dissolved with decomp. Not decomp. by boiling eonc. H 2 SO 4 , or other acids, even aqua regia. Easily sol. with evolution of heat in H 2 O containing only V^ooo pt. CrCl 2 . (Peligot, J. pr. 36. 150). Also sol. in presence of traces of SnCl 2 (5 mg. SnCl 2 cause 1 g. CrCl 3 to dis- solve), FeCl 2 , Cu 2 Cl 2 , Na 2 S 2 O 3 , and other reducing substances; chlorides without re- ducing properties have no effect. (Pelouze, A. ch. (3) 14. 251). TiCl 3 and SO 2 have similar solvent action. (Ebelmen. A. ch. (3) 20. 390); also Zn+dil. acids. (Moberg.) Insol. in dil. alkalies +Aq; very slowly decomp. by boiling cone, alkalies or alkali carbonates +Aq. (Fellenberg, Pogg. 50. 76.) Difficulty sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Insol. in acetone. (Eidmann, C. C. 1899. II, 1014.) Practically insol. in absolute ethyl alcohol, methyl alcohol, acetaldehyde and ether. (Rohland, Z. anorg. 189'9, 21. 39.) Yellow. SI. sol. in benzonitrile. (Nau- mann, B. 1914, 47. 1369.) Violet modification. Very sol. in H 2 O to form a green solution. (Moberg, J. pr. 44. 325.) The violet mod. is almost insol. in H 2 O but if V2o,ooo pt. chromous chloride is present, it is readilv sol. (Rohland, . anorg. 1899, 21. 39.) +4H 2 O. SI. deliquescent. Very sol. in H 2 O, alcohol, and ethyl acetate. (Godeffroy, Bull. Soc. (2) 43. 229.) -f 6H 2 O. Deliquescent. Sol. in H 2 O, but probably decomp. to CrOCl 2 . Practically insol. in ether. Moderately sol. in absolute ethyl alcohol, methyl alcohol and acetaldehyde. (Rohland, Z. anorg. 1899, 21. 39.) " Monochlorochromic chloride" is sol. in ether and fuming HC1(1:1). (Bjerrum, B. 1906, 39. 1599.) Time Total Solu- bility in % Composition of the sat. solution % violet salt % green salt ^hr. 58.36 8.30 91.70 ^hr. 12.57 87.43 4hrs. 63.27 24.80 75.20 1 day 68.50 37.64 62.36 2 days 40.90 59.10 3 " 68.95 42.78 57.22 11 " 42.84 57.16 13 " 42.39 57! 61 19 " 68.58 42.62 57.38 Green modification. Solubility in H 2 O at 25. 25 g. green CrCl 3 +6H 2 O and 10 g. H 2 O. (Olie, Z. anorg. 1906, 51. 55.) Solubility of green CrCl 3 +6H 2 O in H 2 O at 32. 10 g. CrCl 3 +6H 2 O and 4 g. H 2 O. Time Total solubility in % Composition of the dissolved substance Solid phase % violet salt % green salt r 45' 2 h 5' 48 h *lldys. 63.69 66.24 69.53 69.33 70.81 12.87 21.43 34.53 45.27 45.27 87.13 78.57 65.47 54.73 54.73 Almost all dis- solved * First 8 days at 35. (Olie, Z. anorg. 1907, 63. 276.) Solubility of green CrCl 8 +6H 2 O in H 2 O at 35. 10 g. CrCl 3 +6H 2 O and 3.3 g. H 2 O. Composition of the Time Total solubil- ity in % dissolved substance % violet salt % green salt 8' 65.85 16.47 83.53 38' 66.74 25 02 74.98 l h 66.21 25.45 74.55 2 h 10' 68.90 31.47 68.53 4 h 70.79 36.28 63.72 23 h 71.34 42.95 57.05 72 h 70.79 42.88 57.12 (Olie, I. c.) If a solution saturated with the green hexa- hydrate below 32 is cooled, the decahydrate separates out; if the solution is saturated above 32, both the decahydrate and hexa- hydrate separate out on cooling. (Olie, I. c.) 272 CHROMIC GLUCINUM CHLORIDE Violet modification. Solubility in H 2 O at 25. 25 g. violet CrCl 3 +6H 2 O and 10 ccm. of a 35% solution of green CrCl 3 +6H 2 O. Composition of the Composition of- Total Solu- sat. solution the dissolved Time Total % violet salt Time solubil'y Solid pha^e in % IVe hr. 65.. 49 84.05 15.95 salt % green salt 5 " 29 " 84.47 78 16 15.53 21 84 7' 61.35 8.71 91.29 CrCl,+10H 2 O 2dys. 4 " 70.47 73.19 68 71 26.81 31 29 20' I h 55' 62.46 65.04 9.90 25.05 90.10 74.95 Cl n 5 " 5 dys, 6 hrs. 6dys. 8 " 76.38 73 26 60.66 60.36 65.10 65 80 39.34 39.64 34.90 34 20 4 h 30' 24 h 28 h 29 h 67.41 69.44 67 .'59 32.90 42.93 31.78 33.65 67.10 57.07 68.22 66.36 CrCl 3 +6H 2 O . all dissolved CrCl 3 +10H 2 O CrCl 8 +6H 2 O 10 " 58 08 41 92 48 h 69.42 42.17 57.83 ti 12 " 71.14 41.40 58.60 72 h 68.69 43.80 56.20 u Green modification. Solubility of green CrCl 3 +10H 2 O in H 2 O at 29. 14.2 g. CrCl 3 +10H 2 O and 2.5 g. H 2 O. (Olie, Z. anorg. 1906, 51. 57.) Solubility in H 2 O at 25. 25 g. violet CrCl 3 +6H 2 O and 10 g. H 2 O. Composition of the Time Total Solu- sat. solution bility in % % violet salt % green salt Ve hr. 61.99 98.47 1.53 4/2 hrs. 96.70 3.30 Idy. 63 .'88 91.54 8.46 2 ' . . . 83.37 16.63 4 ' 70.68 69.11 30.89 5 ' 62.20 37.80 7 ' 72!il 62.72 37.28 8 ' . 54.63 45.37 12 " 46.39 53.61 13 " 47.66 52.34 26 " 70^62 48.55 51.45 (Olie, I. c.) Green modification. 100 pts. H 2 O dissolve 130 pts. salt at 15. Sol. in al- cohol. (Recoura, C. R. 102. 518.) Grayish-blue modification. Very sol. in H 2 O. (Recoura, C. R. 102. 548.) flOHjO. Very deliquescent; melts in crystal H 2 O at 6-7. Very sol. in H 2 O, alcohol, and ethyl acetate. (Godeffroy.) Easily sol. in H 2 O; can be recryst. from H 2 O. Sol. in alcohol and ether. (Werner. B. 1906, 39. 1827.) (Olie, Z. anorg. 1907, 53. 275.) The composition of the hydrates formed byCrCl 3 at different dilutions is calculated from determinations of the lowering of the fr. pt. produced by CrCl 3 and of the con- ductivity and sp. gr. of CrCl 3 +Aq. (Jones, Am. Ch. J. 1905, 34. 310.) Chromic glucinum chloride, CrCl 3 , G1C1 2 +H 2 0. Sol. in H 2 O with decomp. (Neumann, A. 244. 329.) Chromic lithium chloride, CrCl 3 , 2LiCl+ Very hygroscopic. Sol. in ice water but solution soon decomp. Easily sol. in alcohol. (Werner, B. 1901, 34. 1603.) [Cr(OH 2 )Cl 5 ]Li 2 +4H 2 0. Very hygroscopic. Sol. in ice cold H 2 O and in alcohol. (Werner, B. 1901, 34. 1604.) Chromic magnesium chloride, CrCl 3 , MgCl 2 +H 2 O. Decomp. by H 2 O. (Neumann.) Chromic phosphoric chloride, CrClj, PC1 5 . Decomp. by H 2 O. (Cronander.) Chromium platinum chloride. See chloroplatinate, chromium. Chromic potassium chloride, CrCl 3 , KCL Decomp. by H 2 O. CrCl 3 , 2KC1+H 2 O. (Neumann, A. 244. CrCls, 3KC1. Easily sol. in H 2 O with de- comp. (Fremy, A. ch. (3) 12. 361.) CHROMIC HYDROXIDE 273 Chromic rubidium chloride, CrCl 3 , 2RbCl+ H 2 O. Decomp. by H 2 O. (Neumann, A. 244. 329.) Slowly sol. in cold, rapidly sol. in hot H 2 O with decomp. (Werner, B. 1901, 34. 1603.) CrCl 3 , 3RbCl+8H 2 O. Unstable. Decomp. by alcohol. (Werner, B. 1906, 39. 1830.) Chromic sodium chloride, CrCl 3 , NaCl. Sol. in H 2 O. (Berzelius.) OC1 3 , 3NaCl. Sol. in H 2 O. (Berzelius.) Chromic thallium chloride, CrCl 3 , 3T1C1. Sol. with decomp. in H 2 O. (Neumann, A. 244. 329.) Chromic chloride ammonia. See Chlorotetramine chromium chloride. Chromous chloride hydrazine, CrCl 2 . 2N 2 H 4 . Insol. in H 2 O. Sol. in acids. Insol. in alcohol, ether and similar solvents. (Traube, B. 1913, 46. 1506. Chromic chloride ferric oxide. Fe 2 O 3 is easily sol. in dil., difficultly sol. in cone. CrCls+Aq. (Bechamp. A, ch. (3) 57. 311.) Chromous fluoride, CrF 2 . SI. sol. in H 2 O, hot H 2 SO 4 or dil. HN0 3 . Sol. in boiling HC1. Insol. in alcohol. (Poulenc, C. R. 1893, 116. 254.) Chromic fluoride, CrF 3 . Perfectly sol. in H 2 O. (Berzelius.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) +3H 2 0. Insol. in H 2 O. (Werner and Costachescu, B. 1908, 41. 4243.) +3^H 8 O. Sol. in H 2 O. (Poulenc, C. R. 1893, 116. 255.) +6H 2 O. SI. sol. in H 2 O. (Werner and Costachescu, B. 1908, 41. 4242.) +9H 2 O. Violet modification. Very si. sol. in H 2 O. Insol. in alcohol. Sol. in HC1, and KOH+Aq. (Fabris, Gazz. ch. it. 20. 582.) Chromium Aezafluoride, CrF 6 . Decomp. by H 2 O with evolution of heat. (Berzelius.) Correct composition is CrO 2 F 2 . (Oliveri, Gazz. ch. it. 16. 218.) Chromic cobaltous fluoride, CrF 3 , CoF 2 + 7H 2 O. Easily sol. in H 2 O. (Petersen, J. pr. (2) 40. 60.) Chromic cupric fluoride, CrCuF 6 +5H 2 O. Can be cryst. from HF+Aq. (Higley, J. Am. Chem. Soc. 1904, 26. 630.) Chromic nickel fluoride, CrF 3 , NiF 2 +7H 2 O. Somewhat more sol. in H 2 O than CrF 8 , CoF 2 +7H 2 O. (Petersen, J. pr. (2) 40. 61.) Chromic potassium fluoride, CrF 3 , 3KF. Nearly insol. in H 2 O. (Christensen, J. pr. (2) 36. 161.) CrF 3 , 2KF+H 2 O. Nearly insol. in H 2 O. Sol. in cone. HCl+Aq. (Christensen.) Chromic sodium fluoride, CrF 3 , 2NaF+H 2 O. (Wagner, B. 19. 896.) Chromic thallous fluoride, 2CrF 3 , 3T1F. Sol. in hot H 2 O, less sol. in cold. SI. sol. in HF. (Ephraim, Z. anorg. 1909, 61. 242.) Chromic zinc fluoride, CrF 3 , ZnF 2 +7H 2 O. Can be cryst. from HF+Aq. (Higley, J. Am. Chem. Soc. 1904, 26. 630.) Colloidal solution is perfectly clear. (Biltz, B. 1902, 36. 4433.) Chromous hydroxide, CrO 2 H 2 . Decomp. by H 2 O, especially if hot. (Pc- ligot, A. ch. (3) 12. 539.) Slowly sol. in cold cone, acids, even aqua regia; almost insol. in dil. acids. (Moberg, J. pr.43. 119.) Chromic hydroxide, Cr 2 O 3 , zH 2 O, probablv Cr 2 6 H 6 . Insol. in H 2 0. Easily sol. in acids. Easily sol. in cold KOH, or NaOH+Aq; much less sol. in cold NH 4 OH+Aq; the presence of NH 4 C1 has no influence upon solubility in NH 4 OH+Aq. (Fresenius.) Insol. in NH 4 OH+Aq if it has been thoroughly washed. Insol. in KCN+Aq, but si. sol. in KCN + HCN+Aq. (Rodgers, 1834.) Gradually sol. in dil. FeCl 3 +Aq; after three months, 2 mols. Cr 2 O 6 H 6 are dissolved by 1 mol. FeCl 3 without pptn. of Fe 2 6 H G . (Be- champ, A. ch. (3) 67. 296.) Alsl sol. in CrCl 3 +Aq; in four months. \ 1 A mols. Cr 2 O 6 H 6 are dissolved by 1 mol. CrCl 3 . (Bechamp.) Sol. in Cr(NO 3 ) 3 +Aq, and clear solution formed as long as 3 mols. HNO 8 are present for 8 mols. Cr 2 O 3 . (Ordway, Sill. Am. J. (2) 27. 197.) Chromic hydroxide, pptd. by alkalies is easily sol. in excess of the reagent; after being dried in a vacuum, however, it is insol. in alkalies. (Herz, Z. anorg. 1901, 28. 344.) Freshly pptd. it is sol. in aq. alkali, but it is readily changed into a modification which is insol. (Herz, Z. anorg. 1902, 31. 352.) The solubility of chromic hydroxide in an 274 CHROMOCHROMIC HYDROXIDE aqueous solution of red chromic chloride is not directly proportional to the concentration of the latter a basic chloride is probably formed. (Fischer, Z. anorg. 1904, 40. 43.) Not pptd. in presence of Na citrate. (Spil- ler.) Insol. in amylamine+Aq; not pptd. in presence of alkali tartrates, sugar, etc. Cr 2 O6H 6 +4H 2 O. Difficultly sol. in acids. Cr 2 O 6 H6-i-H 2 O. Extremely hygroscopic. Exists. in a soluble modification, obtained by dialysis; solution can be diluted with pure H 2 O, but gelatinizes with traces of salts. (Graham, Roy. Soc. Trans. 1861. 183.) Cr 2 O 2 (OH) 2 . Insol. in boiling dil. HC1 + Cr 2 O(OH) 4 (Guignet's green). Scarcely sol. in boiling HCl+Aq. (Salvetat, C. R. 48. 295.) Guignet gave formula as 2Cr 2 3 +3H 2 O. Chromochromic hydroxide, Cr 3 O 4 , H 2 O(?). Slightly attacked by acids. (Peligot, A. ch. (3) 12. 539.) Chromous iodide, CrI 2 . Easily sol. in H 2 O. (Moissan, A. ch. (5) 25. 401.) Chromic iodide, CrI 3 (?). Insol. in cold, sol. in hot H 2 O, but no sepa- ration occurs on cooling. (Berlin.) -f9H 2 O. Hygroscopic. Sol. in alcohol and acetone. Insol. in CHC1 3 . (Higley, J. Am. Chem. Soc. 1904, 26. 628.) Chromous iodide hydrazine, CrI 2 , 2N 2 H 4 (Traube, B. 1913, 46. 1507.) Chromium nitride, ON. Insol. in dil. acids and alkalies, cone HNO 3 , HC1, or HF+Aq, even on heating Slowly sol. in hot aqua regia or cold H 2 SO 4 Sol. in cold solutions of alkali hypochlorites (Ufer, A. 112. 281.) Insol. in HC1, HNO 3 and aqua regia (Feree, Bull. Soc. 1901, (3) 26. 618.) Unacted upon by acids at ordinary temper- atures. (Smite, Chem. Soc. 1897, 72. (2) 33.) Cr 3 N 2 . Slowly attacked by cone. HNO C and by HNO 8 +HC1. All other reagents are without action. (Henderson and Galletly, J Soc. Chem. Ind. 1908, 27. 387.) CrN 3 . See Chromium azoimide. Chromous oxide, CrO. Insol. in HNO 3 and dil. H 2 SO 4 +Aq. Sol. in HC1. (Feree, Bull. Soc. 1901, (3 25. 619.) Chromic oxide, Cr 2 O 3 . When ignited is nearly insol. in acids, but tissolves in H 2 SO 4 by long boiling. Insol. n liquid HC1. (Gore.) Insol. in acetone. (Fidmann, C. C. 1899. I, 1014.) Solubility in (calcium sucrate+sugar)4- Aq. 1 1. solution containing 418.6 g. sugar and 34.3 g. CaO dissolves 1.07 g. Cr 2 O 3 ; 1 1. solu- ;ion containing 296.5 g. sugar and 24.2 g. CaO dissolves 0.56 g. Cr 2 O 3 ; 1 1. solution contain- ing 174.4 g. sugar and 14.1 g. CaO dissolves 0.20 g. Cr 2 O 3 . (Bodenbender, J. B. 1865. 600.) See also Chromic hydroxide. +H 2 O. The compound to which Bunsen gave the formula Cr 5 O 6 . Insol. in acids, but easily attacked by HNO 3 . (Feree, Bull. Soc. 1901, (3) 25. 620.) Chromochromic oxide, Cr 3 O 4 = CrO, Cr 2 O 3 . Known only in form of hydroxide, which see. +3H 2 O. Stable in dry air. Decomp. in moist air. (Bauge, C. R. 1898, 127. 552.) Cr 4 O 6 , or Cr 6 O 6 (?). Insol. in acids or in aqua regia. (Bunsen, Pogg. 91. 622.) Not obtainable. (Geuther, A . 118. 66.) Formula is Cr 2 O 3 +H 2 O. (Feree.) Chromium ^noxide, CrO 3 . Deliquescent, and very sol. in H 2 O, to form solution of H 2 Cr0 4 or H 2 Cr 2 7 . Solubility in H 2 O at t. t 15 50 99 %CrO 3 62.08 62.38 64.55 67.39 (Mylius and Funk, Gm. K. 3. 1, 1332.) Sat. CrO 3 +Aq contains at: 61.54 20 62.52 60 65.12% CrO 3 . (Koppel and Blumenthal, Z. anorg. 1907, 53. 228.) The system CrO 3 H 2 O has been studied at temp, from 0to 74. In the limits of concentration investigated, from 71.2% CrO 3 , no hydrate of CrO 3 cryst. from the aq. solution. (Kremann, M. 1911, 32. 622.) Sat. CrO 3 +Aq contains at: 82 66 100 67.4 115 68.4% Cr0 3 . (Kremann, M. 1911, 32. 620.) CHROMIUM OXIDE POTASSIUM CYANIDE 275 Solubility in H 2 O at . B.-pt. of CrO 3 +Aq at ord. pressure. t % by \vt. CrOs Solid phase. B.-pt. G. CrOs in 100 g. of the solution. -0.9 3.6 Ice 102 10.81 -1.9 7.8 it 104 24.08 -3.7 11.5 it 107 36.47 -4.8 14.1 tf 110.5 45.15 10.95 24.9 u 116 54.56 -11.7 25.2 a 120 61.54 -18.75 33.5 it 127 71 . 24 sat. solution OK OK OQ O if 1 -i>) . Ad -43.5 49^1 (Koppel and Blumenthal, Z. anorg. 1907, 53. -60 53.3 u 254.) 20 61.7 CrOo 62.24 '- ~~ o Sol. in H 2 SO 4 ; the solubility is least when +24.8 62.88 H the acid contains 66% H 2 SO 4 (Schrotter); 40 63.50 u 84.5% H 2 SO 4 (Bolley). 65 64.83 Verv sol. in H 2 SO 4 of 1.85 sp. gr. SI. sol. 90 68.5 u in cold KHSO 4 +Aq. (Fritzsche.) 122 70.7 If The statement that CrO 3 is insol. in acids 193-196 100 tt is incorrect. 2.85 g. (ignited) are sol. in HNO 3 to the extent of 2.58 g. 0.81 g. (ignited) are (Buchner and Prins, Z. phys. Ch. 1912, 81. 114.) sol. in HNO 3 to the extent of 0.77 g. (Jovit- schitsch, M. 1909, 30. 48.) Practically insol. in POC1 3 . (Walden, Z. anorg. 1910, 68. 312.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. Sp. gr. of CrO 3 +Aq at t. J. 1898, 20. 827.) Sol. in alcohol with decomp. t Sp. gr. % CrOs Sol. in anhydrous ether. Sol in QiCGtio 3/nlivciri.cl.G fFrv J A.m 16.0 1.0606 8 .25 Cheni. Soc. 1911, 33. 702.) ' 18.0 1.0679 8 .79 Sol. in acetone. (Naumann, B. 1904, 4328.) 14.5 1.0694 8 .79 Sol. in benzonitrile. (Naumann, B. 1914, 19.5 1.0957 12 .34 47, 1369.) 19.0 1 . 1569 19 .33 Sol. in methyl acetate. (Naumann, B. 20.9 1 . 20269 31 .83 1909, 42. 3790.) 20.1 1.20264 31 .83 Difficultly sol. in ethyl acetate. (Nau- 12.0 1.20714 31 .83 mann, B. 1910, 43. 314.) 35.0 1 20940 32 .59 18.6 1.21914 32 .59 Chromium oxide, Cr 5 O 9 =2Cr 2 O 3 , CrO 3 . 15 2 1.22106 32 .59 /~i s\ Of*** (~\ Of^W^ 9.7 22.0 19.2 22.0 1.22384 1.3441 1.3448 1.34416 1.7028 32 37 37 37 62 .59 .77 .82 .82 .23 V-/1 8^15 Ovyl 2^-'3j A\^'L\J^ CrO 2 = Cr 2 3 , CrO 3 . Cr 6 Oi 2 =Cr 2 3 , 3CrO 3 . Cr 6 O 15 = Cr 2 O 3 , 4CrO 3 . See Chromate, chromium. (Zettnow, Pogg. 143. 474.) Sp. gr. of CrO 8 +Aq (H 2 CrO 4 +Aq). M = according to Mendelejeff at 15 : Z = ac- cording to Zettnow, calculated by Ger- lach(Z. anal. 27. 300). % CrOs M Z % CrOs M Z 5 .036 1.037 35 1.324 1.312 10 .076 1.076 40 1.383 1.373 15 : .119 1.118 45 1.445 1.440 20 .166 1.162 50 1.510 1.512 25 .215 1.208 55 1.579 1.587 30 .268 1.258 60 1.656 More sol. in ether than in H 2 O. Ether solution is somewhat more stable than aque- ous solution. (Aschoff, J. pr. 81. 401.) Formula is CrO 3 , H 2 O 2 . (Moissan, C. R. 97. 96.) Chromium peroxide ammonia, CrO 4 , 3NH 3 . Sol. in H 2 O with partial decomp. SI. sol. in NH 4 OH+Aq. Sol. with decomp. in 20% acetic acid. (Hofmann, B. 1905, 38. 3060.) Chromium tetfroxide potassium cyanide, CrO 4 , 3KCN. Sol. in H 2 O. Insol. in other ordinary solvents. (Wiedo, B. 1899, 32, 381.) 276 CHROMIC OXYCHLORIDE Chromic oxy chloride. From Cr 2 O 3 . Sol. in H 2 O as long as 1 mol. CrCl 3 is present for 2 l / 2 mols. Cr 2 6 H 6 . (Ord- way, Sill. Am. J. (2) 27. 197.) Cr 2 3 , 2CrCl 3 . Sol. in H 2 O. (Kletzinsky, Zeit. Ch. 1866. 277.) Cr 2 O 3 , CrCl 3 = CrOCl. Anhydrous. Only partly sol. in H 2 O. +3H 2 O. Very deliquescent, and sol. in H 2 O. (Peligot.) Cr 2 O 3 , 4CrCl 3 +6H 2 =Cr 2 OCl 4 +2H 2 O. (Peligot, J. pr. 37. 38.) +9H 2 O=Cr 2 OCl 4 +3H 2 O. Sol. in H 2 O (Moberg); =Cr 2 (OH) 2 Cl 4 +2H 2 0. (Schiff, A. 124. 157.) Cr 2 O 3 , 7CrCl 3 = Cr 3 OCl 7 . Very sol. in H 2 O with decomp. (Besson and Fo'urnier, C. R. 1909, 148. 1194.) Cr 2 O 3 , 8CrCl 3 +24H 2 O. Sol. in H 2 O (Mo- berg) ; = Cr 2 (OH)Cl 6 +4H 2 O. (Schiff, I. c.) (CrO 2 ) 3 Cl 2 . (Pascal, C. R. 1909, 148. 1464.) Cr 6 O 9 Cl 4 . Insol. in H 2 O. (Pascal, C. R. 1909, 148. 1464.) From CrO 3 . See Chromyl chloride. Chromic oxychloride potassium chloride. CrOCl 3 , 2KC1. Decomp. in the air. Sol. in cone. HC1 without decomp. (Wein- land, B. 1906, 39. 4043.) Chromic oxychloride ruhidium chloride. CrOCl 3 , 2RbCl. Decomp. in the air. Sol. in cone. HC1 without decomp. (Wein- land, B. 1906, 39. 4045.) Chromium oxyfluoride, Cr0 2 F 2 . See Chromyl fluoride. Chromium phosphide, CrP. Insol. in acids, but a trace dissolves in aqua regia. Insol. in HF-f Aq. (Berzelius.) Not attacked by acids or by aqua regia. (Granger, C. N. 1898, 77. 228.) Insol. in all acids except a mixture of HNO 3 and HF. (Maronneau, C. R. 1900, 130. 658.) Insol. in mineral acids. (Dieckmann, Z. anorg. 1914, 86. 295.) Insol. in aqua regia. (Granger, C. R. 1897, 124, 191.) Cr 2 P 3 . Insol. in mineral acids. (Dieck- mann, Z. anorg. 1914, 86. 295.) Chromous selenide, CrSe. (Moissan, C. R. 90. 817.) Chromic selenide, Cr 2 Se 3 . Insol. in H,O. (Moissan, C. R. 90. 817.) Chromic potassium selenide, K 2 Cr 2 Se 4 . Insol. in HC1. Easily sol. in cone. HNO 3 . (Milbauer, Z. anorg. 1904, 42. 451.) Chromium silicide, Cr 2 Si. Sol. in fused KNO 3 ; insol. in cold HC1 and aqua regia. Insol. in HF+Aq. (Moissan, C. R. 1895, 121. 625.) CrSi 2 . Sol. in HF. Insol. in HC1 and aqua regia. (Chalmot, Am. Ch. J. 1897, 19. 69.) Cr 3 Si 2 . Insol. in dil. HC1; sol. in warm cone. HC1 and in HF; insol. in HNO 3 and H 2 SO 4 . (Lebeau, C. R. 1903, 136. 1330.) Cr 3 Si. Sol. in HF; insol. in other acids; sol. in fused KOH and fused alkali nitrates and carbonates. (Zettel, C. R. 1898, 126. 834.) Chromous sulphide, CrS. Insol. in H 2 O or K 2 S+Aq. (Peligot.) Easily sol. in acids. (Moissan. C. R. 90. 817.) Sol. in cold cone, acids. Sol. in molten alkalies. (Mourlot, C. R. 1895, 121. 944.) Min. Daubrelite. Chromic sulphide, Cr 2 S 3 . Insol. in H 2 O or alkali sulphides + Aq. SI. attacked by HCl+Aq. (W. Muller, Pogg. 127. 404.) HNO 3 +Aq decomposes or not according to method of preparation. Easily decomp. by aqua regia. Insol. in caustic alkalies +Aq. Insol. in K 2 S+Aq. (Berzelius.) Chromochromic sulphide, Cr 3 S 4 , =CrS, Cr 2 S 3 . Insol. in H 2 O, HC1, or dil. H 2 SO 4 +Aq. Easily sol. in HNO 3 +Aq. (Groger, W. A. B. 81. (2) 531.) Chromic zinc sulphide, Cr 2 ZnS 4 . (Groger, W. A. B. 1880, 81. 534.) Chromicyanhydric acid. Cadmium chromicyanide, Cd 3 [Cr(CN)e] 2 . Readily sol. in an excess of KCN and in NH 4 OH+Aq. Decomp. by cone. HC1, HNO 3 or H 2 SO 4 . Slowly decomp. by cold, rapidly by hot dil. HC1, HNO 3 , or H 2 SO 4 . Quickly dissolved by aqua regia. Decomp. by boiling with Na 2 O 2 , by NaOH+Aq and by Na 2 CO 3 +Aq. Slowly decomp. by boiling acetic acid. (Cruser and Miller, J. Am. Chem. Soc. 1906, 28. 1136.) Cobaltous chromicyanide, Co 3 [Cr(CN) 6 ] 2 . Sol. in cold, readily sol. in hot cone. HC1 or H 2 SO 4 . SI. sol/ even in boiling cone. CHROMOSULPHURIC ACID 277 HN0 3 . Slowly sol. in cold dil. H 2 SO 4 , HC1 or HNO 3 . Readily sol. in boiling dil. HC1 or H 2 SO 4 . Decomp. but not entirely dissolved by aqua regia. Readily sol. in an excess of KCN. Decomp. by NH 4 OH, NaOH or Na 2 CO 3 +Aq. Decomp. by boiling with Na 2 O 2 . Insol. in cold or boiling acetic acid. (Cruser and Miller.) Cuprous chromicyanide, Cu 3 Cr(CN) 6 . Sol. in KCN, cold cone, or boiling dil. HNO 3 +Aq. Slowly sol. in cold cone. H 2 SO 4 , still more slowly sol. in dil. H 2 SO 4 but rapidly sol. in hot dil. and cone. H 2 SO 4 . Readily decomp. by aqua regia. Decomp. by dil. or cone. HC1, slowly going into solution in the cold, but quickly on boiling. (Cruser and Miller.) Cupric chromicyanide, Cu 3 [Cr(CN) 6 ] 2 . Slowly sol. in cold dil. HC1, HNO 3 or H 2 SO 4 : on boiling the first two readily dissolve it, but the H 2 SO 4 dissolves it only slowly. Sol. in aqua regia or cold cone. H 2 SO 4 . Readily sol. in cold or hot cone. HC1. Decomp. by cold, dissolved by boiling HNO 3 . Decomp. by boiling Na 2 O 2 + Aq . Decomp . by NH 4 OH, NaOH or Na 2 CO 3 +Aq. Readily sol. in an excess of KCN+Aq. Insol. in cold acetic acid. (Cruser and Miller.) Nickel chromicyanide, Ni 3 [Cr(CN) 6 ]2. Slowly sol. in cold, readily sol. in hot dil. HC1, HN0 3 or H 2 SO 4 . Slowly sol. in cold, readily sol. in hot cone. H 2 SO 4 , HC1 or HNO 3 . Slowly decomp. by cold, rapidly by boiling aqua regia. Readily sol. in excess of KCN. Sol. in NH 4 OH+Aq. Decomp. by NaOH, Na 2 CO 3 +Aq or Na 2 O 2 +Aq. Insol. in cold, si. sol. in boiling acetic acid. (Cruser and Miller.) Potassium tballous chromicyanide, K 2 TlCr(CN) 6 . (Fischer and Benzian, Ch. Z. 1902, 26. 50.) Thallous chromicyanide, Tl 3 Cr(CN) 6 . Easily sol. in H 2 O. (Fischer and Benzian, Ch. Z. 1902, 26. 50.) Zinc chromicyanide, Zn 3 [Cr(CN) 6 ]2. Insol. in H 2 O. Sol. in excess of NH 4 OH, NaOH and KCN+Aq. Decomp. by Na 2 C0 3 +Aq. Sol. in cold dil. HC1. Slowly sol. in dil. H 2 SO 4 and in dil. HNO 3 . By boiling with dil. acids a clear solution is quickly obtained. (Cruser, Dissert. 1906.) Chromisulphocyanhydric acid. Caesium chromisulphocyanide, Cs 3 Cr(SCN) 6 +2H 2 O. Less sol. in H 2 O than K salt. Dissert. 1907.) (Osann, Lithium chromisulphocyanide, Li 3 Cr(SCN) 6 +H 2 O. Extremely deliquescent. (Osann.) Rubidium cbromisulphocyanide, Rb 3 Cr(SCN) 6 +4H 2 O. Appreciably less sol. in H 2 O and alcohol than the K salt. (Osann.) Chromocyandric acid, H 4 Cr(CN) 6 . Decomp. rapidly on air. Sol. in H 2 O (Moissan, A. ch. (6) 4. 144.) Potassium chromocyanide, K 4 Cr(CN) 6 . Very sol. in H 2 O; 100 pts. H 2 O dissolve 32.33 pts. at 20. Much more sol. in hot H 2 O. Insol. in alcohol, ether, benzene, or chloroform. (Moissan, A. ch. (6) 4. 136.) Above salt was K 3 Cr(CN) 6 . (Christensen.) +3H 2 0. (Christensen, J. pr. (2) 31. 166.) Chromoiodic acid, CrO 3 , HIO 3 +2H 2 O. Deliquescent. (Berg, C. R. 104. 1514.) Ammonium chromoiodate, CrO 3 , NH 4 IO 3 + H 2 O. Moderately sol. in H 2 O. (Berg.) Lithium chromoiodate, CrO 3 , LiIO 3 +H 2 O. Very sol. in H 2 O. (Berg.) Magnesium chromoiodate. Sol. inH 2 O. (Berg.) Potassium chromoiodate, CrO 3 , KIO 8 . Sol. in H 2 O. (Berg.) +H 2 O = KCrIH 2 O 7 . SI. decomp. by H 2 O. (Blomstrand, J. pr. (2) 40. 331.) Silver chromoiodate, CrO 3 , AgI0 3 . SI. attacked by cold, rapidly decomp. by hot H 2 O. (Berg, C. R. 111. 42.) Sodium chromoiodate, CrO 3 , NaIO 3 +H 2 O. Very sol. in H 2 O. (Berg.) Chromosulphocyanhydric acid. Sodium chromosulphocyanide, Na 3 Cr(SCN) 6 +10, or 11H 2 O. Unstable. Decomp. by H 2 O. (Koppel, Z. anorg. 1905, 45. 360.) Chromosulphuric acid, H 2 Cr 2 (SO 4 ) 4 . S.ol. in H 2 O in all proportions, but solution is easily decomp. on standing or boiling. (Recoura, Bull. Soc. (3) 9. 586.) H 4 Cr 2 (SO 4 )5. As above. H 6 Cr 2 (SO 4 ) 6 . As above. 278 CHROMOSULPHATE, AMMONIUM Ammonium chromosulphate, (NH 4 ) 2 Cr 2 (S0 4 ) 4 +5H 2 0. Sol. in H 2 O after a few minutes. (Recoura.) Chromium potassium chromosulphate, [Cr 2 (S0 4 ) 3 Ci<)4]K 2 ,[Cr 2 (S0 4 ) 3 (Cr0 4 ) 2 ]K4, and [Cr 2 (SO 4 ) 3 (CrO4)3]K 6 . Sol. in H 2 O. (Recoura, Bull. Soc. 1897, (3) 17. 934.) Potassium chromosulphate, K 2 Cr 2 (SO 4 )4+ 4H 2 O. Sol. in H 2 O in a few minutes. (Recoura, Bull. Soc. (3) 9. 590.) Sodium chromosulphate. Na 2 Cr 2 (SO 4 ) 4 + 10H 2 O. As K salt. (Recoura.) Chromotelluric acid. Ammonium chromotellurate, 2(NH 4 ) 2 0, 4CrO 3 , TeO 3 . Sol. in H 2 O. (Berg, C. R. 1911, 162. 1588.) Potassium chromotellurate, 2K 2 O, 4Cr0 3 , TeO 3 . SI. sol. in cold H 2 O without decomp. Sol. in boiling H 2 O. (Berg, Bull. Soc. 1911, (4) 9. 583.) Chromous acid, H 2 Cr 2 O 4 =Cr 2 O 3 , H 2 O. Chromic hydroxide shows slightly acid prop- erties, and salts corresponding to the above acid are known. Aluminum ferrous magnesium chromite (chrome iron ore), (Fe, Mg)O, (Cr 2 , A1 2 )0 3 . Insol. in H 2 O or acids, even a mixture of H 2 SO 4 and HF. (Ebelmen.) Barium chromite, BaCr 2 0<. Insol. in H 2 O. (Gerber, Bull. Soc. (2) 27. 436.) Barium ^rachromite, BaO, 4Cr 2 O 3 . Undecomp. by steam at red heat; insol. in HC1, H 2 SO 4 , HNO 3 ; sol. in fused KOH + KN0 3 ; decomp. in the air. (Dufau, C. R. 1896, 122. 1126.) . Cadmium chrcmite, CdCr 2 O 4 . Not attacked by acids. (Viard, C. R. 109. 142.) Calcium chromite, CaCr 2 O 4 . Insol. in H 2 O. (Gerber, Bull. Soc. (2) 27. 436.) Insol. in HC1, HF, HNO 3 , H 2 SO 4 ; sol. in gaseous HC1 and HF at red heat: sol. in fused KOH, KNO 3 , KC1O 3 , K 2 CO 3 . (Dufau, C. R. 1895, 121. 690.) 2CaO, Cr 2 O 3 . Insol. in H 2 O, KOH, or NH 4 OH+Aq; slowly decomp. by H 2 CO 3 , or M 2 CO 3 -|-Aq; insol. in sugar solution. (Pelouze, A. ch. (3) 33. 9.) 4CaO, Cr 2 O 3 . Attacked by H 2 O. (Mois- san, C. R. 1894, 119. 188.) Cobaltous chromite, CoCr 2 O 4 . (Elliot, Dissert, Gottingen, 1862.) Cuprous chromite, Gu 2 O, Gr 2 O 3 . Insol. in HNO 3 +Aq(sp. gr. 1.4). (Wohler, Z. phys. Ch. 1908, 62. 445.) Cupric chromite basic, 5CuO, 4Cr 2 O 3 . (Wohler, Z. phys. Ch. 1908, 62. 445.) Cupric chromite, CuCr 2 O 4 . Not attacked by HNO 3 +Aq. (Persoz, A. ch. (3) 25. 283.) Not attacked by cone. HC1. Insol. in dil. acids. (Wohler, Z. phys. Ch. 1908, 62. 446.) CuO, 3Cr 2 3 . (Rosenfeld, B. 1879, 12. 958.) Glucinum chromite, GlCr 2 O 4 . Insol. in H 2 O. (Mallard, C. R. 105. 1260.) Iron (ferrous) chromite (chrome iron ore). See Chromite, aluminum ferrous magne- sium. Iron (ferroferric) chromite, FeO, Fe 2 3 , Cr 2 O 3 . Not attacked by HCl+Aq. (Ebelmen.) Iron (ferrous) magnesium chromite. Insol. in HCl+Aq. Scarcely attacked by H 2 S0 4 . Lead chromite, PbCr 2 O 4 . Ppt. Insol. in KOH+Aq. (Chancel, C. R. 43. 927.) Lithium chromite, Li 2 Cr 2 O 4 . Very si. sol. in acids. (Weyberg, C. C. 1906, II. 1659.) Magnesium chromite, MgO, 2Cr 2 O 3 . Insol. in H 2 O. (Nichols, Sill. Am. J. (2) 47. 16.) MgCr 2 Os. Insol. in acids or alkalies, ex- cept boiling H 2 SO 4 . (Schweitzer, J. pr. 39. 259.) Could not be obtained. (Viard, Bull. Soc. (3) 5. 934.) Easily attacked by boiling H 2 SO 4 +Aq. Less easily by HC1 or HF+Aq not at- cked by boilii 1896, 123. 886.) ly fa- tacked by boiling HNO 3 . (Dufau, C. R. 2MgO, Cr 2 O 3 . Insol. in H 2 O or acids. (Nichols.) 5MgO, 4Cr 2 O 3 . Insol. in acids. (Viard, C. R. 112. 1003.) 3MgO,2Cr 2 O 3 . As above. (V.) COBALT, AMMONIA COMPOUNDS 279 Manganese chromite, MnCr 2 O 4 . Entirely insol. in acids. (Ebelmen, A. ch. (3) 33. 44.) Zinc chromite, ZnCr 2 O 4 . Insol. in acids and alkalies, ("faard, C. R. 109. 142.) + zH 2 O. (Chancel, C. R. 43. 927.) 3ZnO, 2Cr 2 O 3 . As above. (Viard, C. R. 112. 1003.) 6ZnO, 5Cr 2 3 . As above. (V.) 8ZnO, 3Cr 2 O 3 . (Groger, M. 1904, 25, 520.) Chromovanadic acid. Ammonium chromovanadate, 2(NH 4 ) 2 O, 2Cr0 3 , V 2 5 +7H 2 0. Sol. in H 2 0. (Ditte, C. R. 102. 1105.) Chromyl amide, CrO 2 (NH 2 ) 2 . Sol. in H 2 O. (Ohly, C. N. 1899, 80. 134.) Chromyl sw&chloride, (CrO 2 ) 5 Cl 6 . Deliquescent, sol. in H 2 O with decomp., insol. in dry ether. (Pascal, C. R. 1909, 148, 1463.) Chromyl chloride (chlorochromic acid) CrO 2 Cl 2 . Decomp. by H 2 O with evolution of much heat. Sol. in glacial acetic acid without de- composition. Sol. in CC1 4 , C 6 H 6 , (mol. wt. det.). (Oddo, Gazz. ch. it. 1899, 29. (2) 318; Chem. Soc. 1900, 78. (2) 75.) Tnchromyl chloride, Cr 3 O 6 Cl 2 . Deliquescent. Sol. in H 2 O with gradual decomposition. Sol. in cone. HCl+Aq. (Thorpe, Chem. Soc. (2) 8. 31.) Scarcely sol. in CS 2 . Sol. in alcohol and ether. (Rawson, C. N. 1889. 59. 185.) Chromyl chic rides. From Cr 2 O 3 . See Chromium oxy chlorides. Chromyl chloride nitrogen fe/roxide, Cr 6 Cl 6 7 , 2N0 2 . Sol. in H 2 O with decomp. (Thomas, C. R. 1899, 129. 828.) Chromyl fluoride, CrO 2 F 2 . Decomp. by H 2 O with evolution of heat. (Oliveri, Gazz. ch. it. 16. 218.) Clay. See Silicate, aluminum, A1 2 O 3 , SiO 2 -f- 2H 2 0. Cobalt, Co. Not attacked by H 2 O. Sol. in dil. HC1, or H 2 SO 4 . or HNO 8 +Aq. Cone, hot H 2 SO 4 , and HNO 3 decomp. with evolution of SO 2 or NO gas. Exists also in passive state. See Iron. (Nickles, J. pr. 61. 186.) Sol. in cone. KOH-j-Aq when in finely divided state. (Winkler, J. pr. 91. 211.) Sol. in NH 4 OH+Aq in presence of air. (Hodgkinson and Bellairs, C. N. 1895, 71. 73.) Cobalt ammonia compounds. See Anhydrooxycobaltamine compounds, [Co(NH 3 ) 5 ] 2 [g| OH) ]x 4 . Bromotetramine cobaltic compounds, BrCo(NH 3 ) 4 X 2 . Bromopurpureocobaltic compounds, BrCo(NH 3 ) 5 X 2 . Carbonatotetramine cobaltic compounds,. (C0 3 )Co(NH 3 ) 4 X. Chlorotetramine cobaltic compounds, ClCo(NH 3 )4X 2 Chloropurpureocobaltic compounds, ClCo(NH 3 ) 5 X 2 Croceocobaltic compounds, Co(NH 3 ) 4 (N0 2 ) 2 X. Decamine cobaltic sulphite, Co 2 (NH 3 ) 10 (S0 3 ) 3 . Diamine cobaltic nitrites, Co(NH 3 ) 2 (NO 2 ) 4 M. Dichrocobaltic compounds, Co(NH 3 )sX 8 . Flavocobaltic compounds, (NO 2 ) 2 Co(NH 3 ) 4 X. Fuscocobaltic compounds, (OH)Co(NH 3 ) 4 X 2 . lodotetramine cobaltic compounds, ICO(NH 3 )4X 2 . Luteocobaltic compounds, Co(NH 3 )6X 8 . Melanocobaltic compounds, [Co(NH 3 ) 3 Cl 2 ] 2 , NH 2 C1. Nitratotetramine cobaltic compounds, (N0 3 )Co(NH 3 ) 4 X 2 . Nitratopurpureocobaltic compounds, (NO) 3 Co(NH 3 ) 6 X 2 . Nitritocobaltic compounds, (N0 2 )Co(NF 3 ) 6 X 2 . Octamine cobaltic compounds, Co 2 (NH 3 ) 8 X,. (=Tetramine cobaltic compounds, Co(NH 8 )y HNO 8 . Not attacked by dil. but decomp. by cone. H 2 SO 4 . Rapidly attacked by aqua regia. (Moissan, A. ch. 1896, (7) 9. 272.) CoB 2 . (Jassonneix, C. R. 1907, 146. 241.) Cobaltous bromide, CoBr 2 . Deliquescent. Sol. in H 2 O, alcohol, and ether. Sat. CoBr 2 +Aq contains at: 59 75 97 66.7 66.8 68.1% CoBr 2 . 2.818 2.805 2.880 2.805 2 '243 2.258 2.138 5.235 5.430 5.312 5.390 0.525 0.516 0.391 0.336 0^562 662 0.667 (Bodlander, 1. c.) Sol. in cone. HCl+Aq; insol. in dil. HNO 3 , or H 2 SO 4 +Aq. Not attacked by cold cone. H 2 SO 4 , and only si. on warming. (Rosen- feld, B. 12. 954.) Sol. in NH 4 OH+Aq; sol. in hot NaCl, KC1, FeCl 3 , ZnCl 2 , MnCl 2 , etc. +Aq. 1 mol. Na 2 S 2 O 3 in aqueous solution dis- solves 1 mol. Cu 2 Cl 2 . (Winklrr, J. pr. 88. 428.) Sol. inKI, I 2 , KCN, or(NH 4 ) 2 SO 4 + Aq. (Renault, C. R. 59. 558.) Solubility in HCl+Aq at 17. Cu 2 Cl 2 YO 28.1 20.7 6.0 6.2 10% is sol. in H 2 O at 18. (Mylius, Z. anorg. 1911, 70. 210.) 80 pts. acetone +20 pts. H 2 O 23.1 21.8 5.3 5.6 Cupric lithium chloride, CuCl 2 , LiCl + 80 pts. acetone +20 pts. methyl alcohol 10 pts. methyl alcohol +90 pts. 23.1 24.0 12.0 11.6 Decomp. on air. Decomp. by dissolving in H 2 . Sol . in cone . LiCl + Aq without decomp . Decomp. by alcohol. (Chassevant, A. ch. (6) 30. 33.) ethyl alcohol (98) 24.2 25.0 5.4 5.1 +2H 2 0'. (Meyerhoffer, W. A. B. 100, 2b. 621.) 20 pts. methyl alcohol +80 pts. ord. ether 24.1 15.1 Cupric mercuric chloride. 80 pts. abs. alcohol +20 pts. ord. 22.4 24.1 15.7 8.8 Easily sol. in H 2 0. (v. Bonsdorff.) ether Cupric mercuric potassium chloride, CuCl 2 , " 25.0 8.5 3HgCl 2 , 6KC1+2H 2 O. Comm. methyl alcohol 85 pts. pyridine+15 pts. H 2 O 23.9 23.0 24.4 5.4 5.6 63.4 Deliquescent in moist air. Sol. 'in boiling H 2 O without decomp., and recrystallises if cooled slowly. Insol. in absolute alcohol. 60 pts. pyridine+40 pts. H 2 O 23.6 27.3 63.7 26.7 (v. Bonsdorff, Pogg. 33. 81.) 75 pts. a picoline +25 pts. H 2 O 70 pts. a picoline +30 pts. H 2 O 28.0 26.1 25.1 26.1 26.2 51.6 52.3 47.3 Cuprous nitrosyl chloride, Cu 2 Cl 2 , 2NOC1. Very deliquescent and sol. in H 2 O with im- mediate decomp. (Sudborough, Chem. Soc. 59. 658.) (de Coninck, C. R. 1900, 131. 59.) Solubility in organic solvents. Sol. in propyl alcohol, hot glycol, hot glycerine, hot paraldehyde, hot crys. acetic acid, pure acetone, 30% methylamine+Aq, pure pyridine, pure a-picoline, acetonitrile; si. sol. in isobutyl and amyl alcohols, crystal- lizable formic acid, ethyl acetate; insol. in cold glycol, cold glycerine, cold paraldehyde, benzaldehyde, cold crystallizable acetic acid, ord. ether, abs. ether, hot and cold CS 2 , cold aniline, cold orthotoluidine, methylene chlor- ide, ethyl iodide, propyl iodide, ethylene bromide, benzene, toluene, xylene, ligroin, nitrobenzene, cold piperidine and essence of terebenthine. (de Coninck, C. R. 1900, 131. 59.) +5H 2 0. Aq. sol. at 35 contains 2.921 Mol. % CuCl 2 . 15 " 1.11 (Schreinemakers, C. C. 1911, II. 349.) Cuprous hydrogen chloride, CuCl,HCl. Sol. in H 2 O. (Neumann, M. 1894, 15. 493.) Cupric hydrogen chloride, CuCl 2 , HC1+3H 2 O Decomp. by H 2 O. Sol. in HCl+Aq below .(Engel, C. R. 106. 273.) Cuprous potassium chloride, Cu 2 Cl 2 , 4KC1. Sol. in H 2 O. (Mitscherlich, A. ch. 73. 384.) For solubility data, see Cu 2 Cl 2 +KCl under cuprous chloride. Cupric potassium chloride. CuCl 2 ,KCl. (Meyerhoffer, Z. phys. Ch. 3. 336.) Sol. in H 2 O; only si. sol. in cone. HCl+Aq. (Groger, Z. anorg. 1899, 19. 330.) CuCl 2 , 2KC1+2H 2 O. Sol. in H 2 O and alcohol. (Berzelius, Pogg. 13. 458.) The composition of the hydrates formed by this salt at different dilutions is calculated from determinations of the lowering of the fr. pt. produced by the salt and of the con- ductivity and sp. gr. of its aqueous solutions. (Jones, Am. Ch. J. 1905, 34. 322.) For solubility data, see CuCl 2 +KCl under cupric chloride. Cupric rubidium chloride, CuCl 2 , 2RbCl. Easily sol. in H 2 O and HCl+Aq. (Godef- froy, B. 8. 9.) +2H 2 O. Sol. in H 2 O. (Wyrouboff, J. B. 1887. 538.) Cuprous sodium chloride. Very sol. in H 2 O. 302 CUPRIC SODIUM CHLORIDE Cupric sodium chloride. Easily sol. in cone. NaCl-f-Aq. Sol. in alcohol of 0.837 sp. gr. No double salt exists. (Schreinemakers and de Baat, Z. phys. Ch. 1909, 66. 586.) Cupric thallic chloride, CuCl 2 , 2T1C1 3 . Sol. in H 2 O. (Willm, A. ch. (4) 6. 55.) +6H 2 O. Can be cryst. from H 2 O. (Gewecke, A. 1909, 366. 225.) Cuprous chloride ammonia, Cu 2 Cl 2 , NH 3 . (Lloyd, J. phys. Chem. 1908, 12. 399.) Cu 2 Cl 2 , 2NH 3 . Decomp. by H 2 O or acids, not by alcohol. (Ritthausen, J. pr. 59. 369.) Cu 2 Cl 2 , 3NH 3 . (Lloyd, J. phys. Chem. 1908, 12. 399.) Cu 2 Cl 2 , 6NH 3 . (Lloyd, J. phys. Chem. 1908, 12. 399.) Cupric chloride ammonia, CuCl 2 , 2NH 3 . Decomp. by H 2 O. (Kane, A. ch. 72. 273.) CuCl 2 ,4NH 8 . Sol.inH 2 O. (Bouzat,C.R. 1902, 135. 294.) +H 2 O (Cuprammonium chloride). Sol. in H 2 O and hot NH 4 OH+Aq. +2H 2 O. Sol. in small amt. of H 2 O. Cu(OH) 2 is pptd. by dilution. (Bouzat, A. ch. 1903, (7) 29. 350.) CuCl 2 , 5NH 3 . (Bouzat, A. ch. 1903, (7) 29. 350.) + 1^H 2 O. Sol. in H 2 0. On dilution Cu(OH) 2 is pptd. Sol. in NH 4 OH+Aq; solubility decreases as NH 3 concentration increases. (Bouzat, A. ch. 1903, (7) 29. 350.) CuCl 2 , 6NH 3 . Completely sol. in H 2 O. (Rose, Pogg. 20. 55.) Sol. in H 2 O but decomp. by great dilution with pptn. of Cu(OH) 2 . Insol. in liquid NH 3 . (Bouzat. A. cb. 1903, (7) 29. 350.) Cuprocupric chloride ammonia, Cu 2 Cl 2 , CuCl 2 , Decomp. by H 2 O or alcohol. Abundantly sol. in NH 4 Cl+Aq, but with partial decom- position. (Ritthausen.) Cupric chloride ammonia platinous chloride, CuCl 2 , 4NH 3 , PtCls. See Platodiamine cupric chloride. Cuprous chloride carbon monoxide, Cu 2 Cl 2 , 2CO+4H 2 O. Very sol. in HC1 (sp. gr. 1.19) with evolu- tion of CO. Sol. in NH 4 OH-f Aq. (Man- chot and Friend, A. 1908, 359. 110.) 2Cu 2 Cl 2 , CO+2H 2 O. Insol. in H 2 O. (Ber- thelot, A. ch. 1856, (3) 46. 488.) 4Cu 2 Cl 2 ,3CO+7H 2 O. Insol. in H 2 0, but decomp. therewith very quickly. Sol. in Cu 2 Cl 2 +HCl. Cupric chloride hydrazine, CuCl 2 , 2N 2 H 4 . Easily decomp. (Hofmann and Marburg, A. 1899, 305. 222.) Cuprous chloride mercuric sulphide, Cu 2 Cl 2) 2HgS. Insol. in H 2 O; sol. in cone, hot HCl+Aq; not decomp. by boiling dil. H 2 SO 4 +Aq, but decomp. by cone. H 2 SO 4 . (Heumann, B. 7. 1390.) Cuprous fluoride, Cu 2 F 2 . Insol. in H 2 or HF. Sol. in cone. HCl-f Aq, from which it is precipitated by H 2 O. Insol. in alcohol. (Berzelius, Pogg. 1. 28.) Decomp. by H 2 O into sol. CuF 2 . Sol. in boiling HCl+Aq and in HNO 3 +Aq. Only si. attacked by warm H 2 SO 4 . (Poulenc, C. R. 116. 1447.) Cupric fluoride, CuF 2 . Easily takes up H 2 O to form CuF 2 +2H 2 O. Sol. in HC1, HNO 3 , or HF+Aq. (Poulenc, C. R. 116. 1448.) Solubility at 25 in HF-f Aq. Normality of HF +Aq. g. atoms Cu in 1000 c. c. of solution 0.12 0.28 0.57 1.08 2.28 0.0307 0.1164 0.2494 0.388 0.463 Solubility is decreased by presence of KF. (Jaeger, Z. anorg. 1901, 27. 29.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) +2H 2 O. SI. sol. in cold, decomp. by hot H 2 O. (Berzelius.) Cupric hydrogen fluoride, CuF 2 , 5HF+5H 2 O. Deliquescent. Easily sol. in H 2 O and dil. acids. Sol. in NH 4 OH+Aq with decomp. (Bb'hm, Z. anorg. 1905, 43, 329.) Cupric potassium fluoride, CuF 2 , 2KF. Easily sol. in H 2 0. CuF 2 , KF. Very si. sol. in H 2 O; si. sol. in dil. acids. (Helmholt, Z. anorg. 3. 115.) Cupric rubidium fluoride, CuF 2 , RbF. As the K salt. (Helmholt.) Cupric silicon fluoride. See Fluosilicate, cupric. CUPRIC HYDROXIDE 303 Copper stannic fluoride. See Fluostannate, copper. Copper tantalum fluoride. See Fluotantalate, copper. Copper titanium fluoride. See Fluotitanate, copper. Copper tungstyl fluoride. See Fluoxytungstate, copper. Copper zirconium fluoride. See Fluozirconate, copper. Cupric fluoride ammonia, CuF 2 , 4NH 3 + 5H2O. Decomp. rapidly in the air. Easily sol. in H 2 O. Decomp. by boiling with H 2 with evolu- tion of NH 3 . Easily sol. in dil. acids. (Bohm. Z. anorg. 1905, 43. 333.) SolubiUty in NH 4 OH+Aq at 25. NHs nc nr>. g. Cu per 1. equiv. CuOzHz perl. 2.63 2.00 1.32 3.05 2.12 1.08 0.096 0.067 0.034 2.540 1.965 1.280 0.973 0.870 0.540 0.391 6.26 6.28 4.13 3.36 3.08 2.36 2.04 0.197 0.166 0.129 0.106 0.097 0.074 0.064 3.176 2.070 1.272 0.451 0.320 8.06 5.72 4.75 2.54 2.13 0.253 0.180 0.149 0.080 0.067 The non-agreement of the results is due to the presence of different modifications of CuO 2 H 2 . Cuprous hydride, CuH. Insol. inH 2 0. Sol. in HCl+Aq. (Wurtz, C. R. 18. 102.) Sol. in warm cone. HC1 with decomp. (Bartlett, Am. Ch. J. 1895, 17. 187.) Cupric hydride, CuH 2 . Sol. in HC1 with decomp. (Bartlett, Am. Ch. J. 1895, 17. 187.) Copper hydrosulphide, 7CuS, H 2 S. (Linder and Picton, Chem. Soc. 1892, 61. 120.) 9CuS, H 2 S. (Linder and Picton.) 22CuS, H 2 S. (Linder and Picton.) Cuprous hydroxide, Cu 2 O, zH 2 O. Sol. in acids as cupric salt. Insol. in NaOH, or KOH+Aq. Sol. in NH 4 OH, and (NH 4 ) 2 CO 3 +Aq; sol. in Na 2 S 2 O 3 +Aq. Cuprocupric hydroxide, CuOH, 3Cu(OH) 2 +3H 2 O. Sol. in acids. (Francke, Dissert. 1907.) Cupric hydroxide, 3CuO, H 2 O. Insol. in H 2 O or dil. alkalies. Easily sol. in warm NH 4 Cl+Aq. (Rose.) Much more difficultly sol. than Cu0 2 H 2 in KOH+Aq. (Chodnew, J. pr. 28. 220.) True composition is 6CuO, H 2 O. See also Cupric oxide. CuO 2 H 2 . Insol. in H 2 O, but decomp. into 6CuO, H 2 O by being boiled therewith. Extremely easily sol. in acids. Sol. in NH 4 OH, and NH 4 salts + Aq. .(Bonsdorff, Z. anorg. 1904, 41. 182.) Solubility in NH 4 OH+Aq at 18. NHs mols per 1. Cu g. atoms per 1. 0.20 0.00054 0.50 0.0033 1.0 * 0.0109 1.5 0.0204 2.0 0.0314 2.5 0.0442 3.0 0.0548 4.0 0.0784 5.0 0. 1041 6.0 0.1254 8.0 0.1599 9.96 0.1787 (Dawson, Z. phys. Ch. 1909, 69. 111.) Sol. in cold NaOH, or KOH+Aq (Proust); but CuO is pptd. on boiling (Berthollet) : is not pptd. (Chodnew, J. pr. 28. 220.) Insol. in NaOH or KOH+Aq unless they contain organic matter (Berzelius). This is contradicted by Volcker (A. 59. 34). Entirely sol. in cone. KOH+Aq, but solu- tion is decomp. by heating. (Tremy, A. ch. (3) 12. 510.) Sol. in NaOH+Aq (70% NaOH). (Low, Z. anal. 9. 463.) The solubility in NaOH of CuO 2 H 2 , pre- pared either from CuSO 4 or Cu(NO 3 ) 2 , de- creases with decrease in concentration of the 3e. The solubility of CuO 2 H 2 in NaOH is only very slightly affected by the addition of sodium or potassium carbonate. (Fischer, Z. anorg. 1904, 40. 41.) 304 CUPRIC HYDROXIDE Solubility of crystalline CuO 2 H 2 in ammoni- acal Ba(OH) 2 and NaOH solutions at Solubility of crystalline Cu0 2 H 2 in ammoni- acal salt solutions at 18 Continued 18. Cone, of dis- Cu concentra- Solvent contains per litre solved Cu. g. Solvent contains per litre tion g. atoms atoms per 1. per 1. 3 mol. NH 3 +0.10 mol. (NH 4 ) 2 SO 4 " +0.20 0.1740 1 mol. NH 3 +0 mol. Ba(OH) 2 0.01090 +0.0025 0.00907 +0.40 ^044- +0.005 0.00801 4 mol. NHs+0.00 mol. (NH 4 ) 2 SO 4 \J . UU^ETc 0.0784 " +0.01 " 0.00633 +0.01 OQ22 +0.02 0.00526 " +0.025 \j . \* Cu 2 I 2 Not pptd. in presence of aromatic oyxacids or phenols of the ortho series. Thus in pres- 0^678 756 i . . ' -- 2.557 3 204 ence of salicylic acid, pyrocatechin, gallic acid, pyrogallic acid, etc., NaOH+Aq does not ppt. CuO 2 H 2 from Cu solutions, but (K844 0.898 0.964 3^954 4.436 pptn. is not prevented by benzoic acid, re- 1 032 5.685 sorcin, hydroquinone, etc. (Weith, B. 9. 1.090 6^282 342.) Sol. in solutions of alkali salts of "spal- tungsprodukte" of albumen. (Kalle and 1.112 1.232 i f)40 6.530 7.653 fi 44Q Cu 2 I +I 2 Co, Pat. 1901.) X . V_TVJ 808 U . rirt7 ^ iQ4 2 Sol. in starch emulsion which has become \J . Oi/O 0.748 iJ . Uty^t 4.711 thin liquid in an alternating magnetic field. 0.606 3 856 (Rosenthal, C. C. 1908, 1. 593.) CuO, 2H 2 O. (Rubenovitch, C. R. 1899, 0^448 0.300 2 '949 2.069 129. 336.) 159 1 230 CuO, 3H 2 O. CKosmann, Z. anorg. 1893, 3. 373.) 0^925* J . -OU 5.461 US66 Cu 2 I 2 +I 2 2CuO, 3H 2 O. (Cross, Gm K. 5. 1, 753.) ' . ouu 4CuO, H 2 O. Insol. in NH 4 OH+Aq. * at 0. ** at 40. (Mailhe, A. ch. 1902, (7) 27. 393.) (Fedotieff, Z. anorg. 1911, 69. 26.) Cupric hydroxide ammonia, Cu0 2 H 2 , 4NHs. Present in ammoniacal solution of CuO 2 H 2 . (Dawson, Z. phys. Ch. 1909, 69. 110.) Cuprous imide, Cu 2 NH. Decomp. at 160 forming Cu 3 N. Readily hydrolysed by H 2 O. Sol. in liquid NH 3 solutions of NH 4 N0 8 . (Franklin, J. Am. Chem. Soc. 1912, 34. 1502.) Cuprous iodide, Cu 2 I 2 . Insol. in H 2 O, or dil. acids. Calculated from electrical conductivity of Cu 2 I 2 +Aq, 1 1. H 2 O dissolves about 8 mg. Cu 2 I 2 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) Sol. in cone. H 2 SO 4 . (Vitali, Gm. K. 6. 1, 947.) Sol. with difficulty in cone. HCl+Aq. Decomp. by cone. HNO 3 , or H 2 SO 4 . Insol. in NaCl, KNO 3 , Na 2 SO 3 , KBr, or NH 4 C1+ Aq. Sol.inNH 4 OH,Na 2 S 2 3 ,KCN,orKI + Aq. (Renault, C. R. 59. 558.) Appreciably sol. in N/10 HC1. Practically insol. in N/10 H 2 SO 4 . (Moser, Z. anal. 1904, 43. 604.) Results of experiments on solubility of Cu 2 l2 in I 2 +Aq in presence of acids and salts are given by Bray and MacKay. Cu 2 I 2 was found to be si.. sol. in H 2 O but a considerable amt. dissolves in presence of I 2 , owing to formation of Culo and Culs- (J. Am. Chem. Soc. 1910, 32. 1207.) Solubility in NH 4 Br+Aq at 20. NEUBr+Aq. g. Cu2lz in 1 1. of the solution 2-N 3-N 4-N 1.9068 3.6540 6.0588 (Kohn and Klein, Z. anorg. 1912, 77. 254.) Sol. in FeCl 3 +Aq. (Fleischer, C. N. 1869, 19. 206.) Solubility in KBr+Aq at t. t KBr+Aq. g. Cuzl2 in 1 I. of the solution 19.5 24.0 19.5 23.0 22.0 22.0 2-N 2-N 3-N 3-N 4-N 4-N 1.4666 1.5576 3.4094 3.5949 7.1263 6.9768 The solutions undergo change in the course of a few days, iodine being set free; the sol- ubility of the cuprous iodide is not markedly affected thereby. (Kohn, Z. anorg. 1909, 63. 337.) 1 1. of a 0.2N solution of KI dissolves 0.000157 g. mol. Cu 2 I 2 . (Bodlander, Z. anorg. 1902, 31. 475.) Very sol. in liquid NH 8 . (Franklin, Am. Ch. J. 1898, 20. 827.) 306 CUPRIC IODIDE Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Practically insol. in methvlene iodide. (Retgers, Z. anorg. 1893, 3. 347.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in acetone (Naumann, B. 1904, 37. 4329); (Eidmann, C. C. 1899, II, 1014.) 100 g. acetonitrile dissolve 3.52 g. Cu 2 I 2 at 18. (Naumann and Schier, B. 1914, 47. 249.) Mm. Marshite. (Gin K. 5. 1, 945.) Cupric iodide, CuI 2 , Exists only in very dil. aqueous solution. (Traube, B. 17. 1064.) Copper periodide, CuI 4 . Sol. in H 2 O. (Walker and Dover, Chem. Soc. 1905, 87. 1588.) Copper ammonium iodide ammonia. See Cupriammonium iodide ammonia. Cuprous mercuric iodide, Cu 2 l 2 , HgI 2 . KI+Aq dissolves out BTgI 2 . Cuprous mercuric iodide ammonia, CuI 2 , 2HgI 2 , 4NH 3 . Decomp. by H 2 or acids. Sol. in a mix- ture of acetic acid and alcohol. CuI 2 , HgI 2 , 4NH 3 . As above. (Jorgensen, J. pr. (2) 2. 347.) Cupric nitrogen iodide, CuI 2 , N 2 H 4 I 2 . Decomp. by H 2 O; or NH 4 OH+Aq. (Guy- ard, C. R. 97. 526.) Cupric thallic iodide ammonia, CuI 2 , 2T1I 3 , 4NH 8 . Decomp. slowly by H 2 O. Sol.inNH 4 OH+ Aq with decomp. Sol. in alcohol. Cuprous iodide ammonia, Cu 2 I 2 , NH 8 . Ppt. (Anderline, Gazz. ch. it. 1912, 42. I, 321.) +4H 2 O. Insol. in H 2 O. Very sol. in NH 4 OH+Aq. (Silberrad, Chem. Soc. 1905, 87. 67.) Cu 2 I 2 , 3NH 3 . (Lloyd, J. phys. Chem. 1908,12.399.) Cu 2 I 2 , 4NH 3 . (Levol, J. Pharm. 4. 32S.) +H 2 O. (Saglier, C. R. 104. 1440.) Cu 2 I 2 , 6NH 8 . (Lloyd.) Cupric iodide ammonia, CuI 2 , 4NH 3 +H 2 O. Decomp. by H 2 O. Sol.in NH 4 OH+Aq without decomp. Not attacked by cold alcohol or ether. (Berthemont, J.. Pharm. 15. 445.) (Pozzi-Escot, C. R, 1900, 130. 90.) CuI 2 , 6NH 3 . Sol. in liquid NH 3 . (Horn, Am. Ch. J. 1908, 39. 205.) 3CuI 2 , 10NH 3 . Decomp. by H 2 O. (Rich- ards, Am. Ch. J. 1895, 17. 302.) Sol. in liq. NH 3 . (Horn, Am. Ch. J. 1908, 39. 204.) Cupriammonium iodide ammonia, 3Cu(NH 3 ) 2 I 2 , 4NH 3 . Decomp. by air and by H 2 O. (Richards, Am. Ch. J. 1895, 17. 302. Copper periodide ammonia, 2CuI, I 4 , 5NH 3 +H a O. Because of its insolubility it cannot be recryst from any solvent. (Silberrad, Chem. Soc. 1905, 87. 66.) Copper tetraiodide, ammonia, CuI 4 , 4NH 3 . (Jorgensen, J. pr. (2) 2. 353.) Copper Aezaiodide ammonia, Cule, 4NH 3 . Not decomp. in H 2 O in closed vessels. (Jorgensen.) Copper mercuric iodide ammonia, CuHg 3 I 6 , 5NH 3 . CuHgI 3 , 2NH 3 . Ppt. Decomp. by H 2 O and by alcohol. CuHg 2 I 6 , 3NH 3 . Ppt. Decomp. by long washing with H 2 O. CuHg 2 I 5 , 4NH 3 . Ppt. Decomp. by H 2 O. SI. attacked by abs. alcohol. CuI 2 , HgI 2 , 4NH 3 . Ppt. (Anderline, Gazz. ch. it. 1912, 42, (1) 321; C. C. 1912, II. 95.) Copper nitride, Cu 6 N 2 . Decomp. by dil. or cone, acids. Easily decomp. by H 2 O when finely pow- dered. (Rossel, C. R. 1895, 121. 942.) Copper sw&oxide, Not attacked by H 2 O. Decomp. by dil. H 2 Sq 4 +Aq into Cu and CuSO 4 ; dil. HCl+Aq has similar action. Not attacked by NH 4 OH +Aq or NH 4 OH+(NH 4 ) 2 CO 8 +Aq. (Rose, Pogg. 120. 1.) Cu 3 O. Not attacked by dil. or cone. min. acids, even aqua regia. Slowly sol. in HF-f- Aq. (Bailey and Hopkins, Chem. Soc. 1890, 67. 272.) Is a solution of oxide in Cu. (Jordis, Zeit. angew. Ch. 1908, 21. 51.) Cuprous oxide, Cu 2 O. Insol. in H 2 Q. Decomp. by H 2 SO 4 +Aq, H 3 PO 4 +Aq, or cold very dil. HNO 3 +Aq into a cupric salt and Cu. Converted by HC1+ Aq into cuprous chloride. CUPRIC OXIDE 307 Solubility of Cu 2 O in NH 4 OH+Aq at 25. Solubility of CuO in HF+Aq at 25. Cone, of total Cu Cone, of total NH 3 Time G. CuO in 10 ccm. of the solution G. in 1000 g. of solution G. mol. in 1000 g. of solution G. in 1000 g. of solution G. mol. in 1000 g. of solution 0.25N-H* Ikhrs. 25k ;; 17Q 1 A " 0.0431 0.0619 0.0812 0.0823 0.0907 Preparation I 0.3593 0.5024 0.6869 0.6964 1.0144 1.0462 1.0557 1.2243 1.3229 1.4882 1.5105 1.6313 1.6981 0.00566 0.00791 0.01080 0.01095 0.01597 0.01645 0.01660 0.01924 0.02081 0.02340 0.02375 0.02565 0.02670 3.91 12.07 13.77 16.15 27.03 32.64 36.89 45.73 68.68 74.12 81.26 98.52 122.40 0.23 0.71 0.81 0.95 1.59 1.92 2.17 2.69 4.04 4.36 4.78 5.56 7.20 N-HF (a) 52 2 " 201^ " 226^ " 0.3018 0.2797 0.2747 0.2339 0.2353 N-HF (b) 4k " 44k " 117% ;; 0.3220 0.2930 0.2431 0.2219 2.02N-HF 5 * 1' 156^1 " 0.3646 0.4533 0.3583 0.3311 Preparation II (Deussen, Z. anorg. 1905, 44. 421.) Solubility of CuO in HF at 25. Cu = g-atoms Cu in 1 1. of the solution. 0.4229 0.6678 0.9890 1.0494 1.3528 1.5047 1.5963 1.6555 0.00665 0.01050 0.01555 0.01650 0.02127 0.02366 0.02510 0.02603 7.82 8.16 22.61 28.39 54.15 72.08 78.20 102.05 0.46 0.48 1.33 1.67 3.19 4.24 4.60 6.00 HF normality Cu 0.12 0.0307 0.28 0.1164 0.57 0.2494 1.08 0.388 2.28 0.463 (Donnan and Thomas, Chem. Soc. 1911, 99. 1791.) Sol. in boiling NH 4 Cl+Aq. (Rose.) SI. sol. in excess of KOH + Aq . (Chodnew.) Sol. in cone. MgCl 2 , and FeCl 2 -fAq. (Hunt, C. R. 69. 1357.) SI. attacked by liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Min. Cuprite. Sol. in HC1, HN0 3 , and NH 4 OH+Aq. Cupric oxide, CuO. Insol. in F 2 O. Easily sol. in acids. Sol. in H 2 SO 3 +Aq. Insol. in NH 4 OH+Aq, but dissolves on addition of a few drops of acid or (NH 4 ) 2 CO 3 +Aq. Insol. in dil., but sol. in warm cone. NaOH, and KOH+Aq. (Low, Z. anal. 9. 463.) CuO prepared at a low temp, is easily sol. in dil. acids, but when ignited is slowly sol. in boiling cone, acids, but moderately rapidly in a cold mixture of NHJ+HC1. (Joannis, C. R. 1886, 102. 1161.) Solubility in N-HNO 3 . 1 1. of the solution contains 0.4802 g. atoms Cu at 25. (Jaeger, Z. anorg. 1901, 27, 33.) (Jaeger, Z. anorg. 1901, 27. 29.) Solubility of CuO in HF+KF at 25. Cu = g-atoms Cu in 1 1. of the solution. HF normality Cu 0.12 0.28 0.57 1. 11(1. 08) 2.17(2.28) 0.0356 0.06437 0.1442 0.2451 0.2517 (Jaeger, 1. c.) SI. sol. in large excess of KOH+Aq. (de Coninck, C. C. 1904, II, 65.) Slowly sol. in boiling NH 4 Cl+Aq, and less easily in NH 4 NO 3 +Aq. (Rose.) Sol. in boiling H 2 O solutions of A1 2 , Gl, U, Cr 2 , Fe 2 , or Bi nitrates and chlorides, Hg(NO 3 ) ? , Hg 2 (NO 3 ) 2 , SbCl 3 , SnCl 2 , and SnCl 4 , with pptn. of oxides of the bases of those salts. Unacted upon by boiling H 2 O solutions of Mn, Mg. Ni, Co, Zn, Ce, or 308 CUPROCUPRIC OXIDE Fe nitrates or chlorides, AgNO 3 , Pb(N0 3 ) 2 , Cd(NO 3 ) 2 , and HgCl 2 . (Persoz.) Pure CuO is very si. sol. in NH 4 OH+Aq but the solution is greatly increased by the addition of NH 4 salts. (Muthmann, C. C. 1904. II, 410.) Sol. in hot (NH 4 ) 2 SO 4 or (NH 4 ) 2 S0 3 +Aq. (Jumau, Electrochem. Ind. 1908, 6. 258.) 15% dissolves in (NH 4 )oCO 3 +Aq in '24 hrs. (Schnabel, Z. B. H. Sal. 1880, 28. 282.) SI. attacked by liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Solubility in N-acetic acid. 1 1. of the solu- tion contains 0.1677 g-atoms Cu at 25. (Jaeger, Z. anorg. 1902, 27. 33.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) SI. sol. in benzamide. (Dessaignes, A. ch. 1852, (3), 34. 146.) Insol. in piperidine. (Cahours, G. R. 1852, 34. 481.) ' Sol. in acid amines as asparagin. (Piria, A. ch. 1848, (3), 22. 160.) Sol. in amines alone or mixed with NH 3 . (Lance, Dissert. 1906.) Slowly sol. in Ca or any other alkali su- crate+Aq, but not in cane sugar +Aq. (Hunton.) Solubility in (calcium su crate + sugar) +Aq. 1 1. solution containing 418.6 g. sugar and 34.3 g. Cap dissolves 10.26 g. CuO. 1 1. solution containing 296.5 g. sugar and 24.2 g. CaO dissolves 5.68 g. CuO. 1 1. solution containing 174.4 g. sugar and 14.1 g. CaO dissolves 3.47 g. CuO. (Boden- bender, J. B. 1865. 600.) Polypeptides in aqueous solution dissolve CuO by short boiling. (Fischer, B. 1906, 39. 576.) + V 6 H 2 O=6CuO+H 2 O. Insol. in dil., but sol. in cone. KOH or NaOH -fAq. Sol. in volatile oils. See also Cupric hydroxide. Min. Melaconite. Sol. in HC1, or HNO 3 + Aq. Cuprocupric oxide, Cu 5 O 3 =2Cu 2 O, CuO. (Favre and Maumene".) Cu 3 O 2 +H 2 O = Cu 2 O, CuO+H 2 O. When freshly pptd., sol. in HCl+Aq, but insol. after drying. (Siewert, J. B. 1866. 257.) Cu 4 O 3 = Cu 2 O, 2CuO. (Siewert.) All oxides of Cu except Cu 4 O, Cu 2 O, CuO, and CuO 2 are mixtures. (Osborne, Sill. Am. J. (3) 32. 33; Debray, C. R. 99. 583.) Copper dioxide, CuO 2 +H 2 O. Insol. in H 2 O. Decomp. by acids with for- mation of cupric salt and H 2 O 2 . (Weltzien, A. 140. 207.) Cuprous oxide ammonia (cuprosammonium oxide). Known only in solution. (Wagner, C. C. 1863. 239.) Cupric oxide ammonia (cuprammonium hy- droxide), 3CuO, 4NH 3 +6H 2 O. Insol. in H 2 O. (Kane, A. ch. 72. 283.) CuO, 4NF 8 +4H 2 O. Very deliquescent. Decomp. in the air and by H 2 O. (Malaguti and Sarzeau, A. ch. (3) 9. 438.) Cuprous oxybromide, Cu 2 Br 2 , CuO+H 2 O. (Spring and Lucion, Bull. Ac. Bele;. (3) 24. 21.) Cupric oxybromide, CuBr 2 , 3CuO+3H 2 O. Insol. in H 2 O. Easily sol. in dil. acids or NH 4 OH+Aq. (Brun, C. R. 109. 66.) Insol. in H 2 O but decomp. by continued boiling. Sol. in cone, acetic acid, si. sol. in cone. CuBr 2 -fAq. Insol. in dil. KBr+Aq. (Richards, Proc. Am. Acad. 1890, 25. 215.) Cupric oxybromide ammonia, 2CuO, CuBr 2 , 2NH 3 +3H 2 O. (Kohlschiitter and Pudschies, B. 1904, 37. 1159.) Cuprous oxychloride, Cu 2 Cl 2 , CuO+3H 2 0. (Spring and Lucion, Bull. Ac. Belg. (3) 24. 21.) Cupric oxychloride, CuO, CuCl 2 +H 2 0. Decomp. by H 2 O. (Rousseau, C. R. 1890, 110. 1263.) 2CuO, CuCl 2 . Insol. in H 2 0. Sol. in HC1 4-Aq, from which it is reprecipitated by dilution with H 2 O. +H 2 O. (Kane, A. ch. 72. 277.) +4H 2 O. (Gladstone, Chem. Soc. 8. 211.) 3CuO, CuCl 2 +2H 2 O. (Miller and Ken- rick, Trans. Roy. Soc. Can. 1901, (2) 8, III. 35.) -j-3H 2 O. (Dupont and Jansen, Bull. Soc. 1893, (3), 9. 193.) +33^H 2 O. Insol. in cold H 2 O, si. decomp. by boiling. (Reindel, J. pr. 106. 378.) Insol. in boiling H 2 O. (Habermann, W. A. B. 90. 2. 268.) +4H 2 0. Sol. in alkaline solution of KNa tartrate. (Groger, Z. anorg. 1902, 31. 327.) (Brunswick green}. Insol. in H 2 O. Easily sol. in acids. Min. Atacamite. Sol. in acids, and NH 4 OH +Aq. Sol. in cold sat. citric acid+Aq. (Bolton, B. 1880, 13. 732.) 4CuO, CuCl 2 +6H 2 O. (Kane, Gm. K. 5. 1, 919.) +8H 2 O. Min. Tallingite. (Church, Gm. K. 5. 1, 919.) 5Cu(OH)o, Cu,Cl 2 Cl(OH). Insol. in H 2 O. Decomp. by hot H 2 O. (Kuhling, B. 1901, 34. 2852.) 7CuO, 2CuCl 2 +9H 2 O. (Reindel.) 6CuO,CuCl 2 +9H 2 O. Insol. in H 2 O. Sol. in acetic acid. (Neumann, Repert, 37. 304.) 8CuO, CuCl 2 + 12H 2 O. Min. Footeite. (Konig, Zeit. Kryst. 1891, 19. 601.) CUPROUS SILICIDE 309 Cupric zinc oxychloride, ZnO, 2ZnCl 2 , 5CuO +6H 2 O. (Andre, C. R. 1888, 106. 855.) Cupric oxychloride ammonia, 2CuO, CuCl 2 , 2NH 3 +3H 2 0. (Deherain, Gm. K. 6. 1, 932.) Cupric oxyfluoride, CuO, CuF 2 +H 2 O. InsDl. in H 2 O. (Berzelius.) (Balbiano, Gazz. ch. it. 14. 74.) ' Cupric oxyfluoride ammonia (cuprammonium oxyfluoride), Cu(OH)F, 2NH 3 . (Balbiano, Gazz. ch. it. 14. 74.) 3CuO, CuI 2 +zH 2 O. (Tschiriwinski, Gm. K, 5. 1, 1584.) Cuprous oxyiodide, Cu 2 I 2> CuO +H 2 O. (Spring and Lucion, Bull. Ac. Belg. (3) Cupric oxyiodide, 2CuI 2 , CuO+4H 2 O, Easily decomp. by H 2 O. (Carnegie, Watts ' Diet. II, 257.) Copper oxysulphide, 2Cu 2 S, CuO. Insol. in H 2 O. (Maumene, A. ch. (3) 18. 311. 5CuS, CuO. Ppt. (Pelouze.) 2CuS, CuO. Insol. in H 2 O. CuS, CuO. Insol. in H 2 O. Above comps. do not exist. (Pickering, Chem. Soc. 33. 136.) Copper phosphide, Cu 6 P 2 . Easily sol. in HNO 3 or aqua regia; insol. in HCl+Aq. (Rose, Pogg. 6. 209.) Sol. in HNO 3 and Br 2 +Aq. Decomp. by hot cone. H 2 SO 4 . (Rubenovitch. C. R. 1899. 128. 1399.) Cu 2 P. Sol. in HNO 3 -f-Aq. (Granger, A. ch. 1898, (7), 14. 64.) Crystallized. Completely sol. in hot HN0 3 , aqua regia and HF+HNO 3 . Slowly sol. in hot HC1 or H 2 SO 4 . Not attacked by hot or cold HF or acetic acid. (Maronneau, C. R. 1899, 128. 939.) Cu 3 P 2 . Easily sol. in HNO 3 . Sol. in hot cone. H 2 SO 4 . Sol. in cone. HCl+Aq before the phosphide has been heated. (Rose. Pogg. 4. 110.) Cu 2 P 2 . Easily sol. in HNO 3 , or HCl+Aq. Sol. in NH 4 OH+Aq. (Granger, Bull. Soc. (3) 9. 661.) CuP 2 . Decomp. by HNO 3 ; not readily sol. in HC1. Easily attacked by C1 2 or Br 4 + Aq. (Granger, C. R. 1895, 120. 924.) Cu 6 P 2 . (Granger, C. N. 1898, 77. 229.) Very sol. in HNO 3 and Br 2 +Aq. Decomp. by hot cone. H 2 S0 4 . (Rubenovitch, C. R. 1899, 129. 338.) Cupric zinc phosphide, 10Cu 6 P 2 , Zn 8 P 2 (?). (Hvoslef, A. 100. 99.) Copper phosphoselenide, CuSe, P 2 Se. Insol. in H 2 O or HCl+Aq; sol. in HNO 3 + Aq. Insol. in cold alkalies, but decomp. slowly when heated therewith. (Hahn, J. pr. 93. 436.) 2CuSe, P 2 Se 3 . Attacked only by fuming HN0 3 . (Hahn.) 2CuSe, P 2 Se 6 . Sol. only in HN0 3 +Aq. (Hahn.) Copper phosphosulphide, 2Cu 2 S, P 2 S. Cu 2 S, P 2 S. (Berzelius.) 2Cu,,S, P 2 S 3 . (Berzelius.) CuS, P 2 S. Insol. in H 2 O and dil. HC1 +Aq. Sol. in cone. HCl+Aq, from which it is precipitated by H 2 O. (Berzelius, A. 46. 252.) 8CuS, P 2 S 5 . (Berzelius.) Cu 4 PS 3 . Sol. in cone. HNO 3 and in aqua regia. Insol. in HC1. Not attacked by hot H 2 SO 4 or cone. NaOH+Aq. (Ferrand, A ch. 1899, (7), 17. 407.) Cuprous selenide, Cu 2 Se. Ppt. Sol. in HC1 and in H 2 SO 4 . Decomp. by HNO 3 . Sol. in NH 4 OH+Aq. (Fonzes-Diacon, C. R. 1900, 131. 1207.) Sol. in KCN+Aq. (Heyn and Bauer, Metall. 1903, 3. 84.) Min. Berzelianite. Cupric selenide, CuSe. (Little, A. 112. 211.) Ppt. Sol. in HC1 and in H 2 SO 4 . Decomp. by HNO 3 . (Fonzes-Diacon, C. R. 1900, 131. Cuprocupric selenide, Cu 3 Se 2 . Min. Umangite. Sol. in HNO 3 . (Klock- mann, Zeit. Kryst. 1891. 19, 270.) Cuprous lead selenide, 3Cu 2 Se, PbSe. Min. Zorgite. Sol. in cold cone. HN0 3 + Aq with separation of Se. Cupric lead selenide, CuSe, PbSe. Sol. in cold cone. HNO 3 with separation of Se. (Karsten.) CuSe, 2PbSe. As above. CuSe, 4PbSe. As above. Cuprous silver selenide, Cu 2 Se, Ag 2 Se. Min. Eucainite. Sol. in hot HN0 3 with decomp. (Berzelius.) Cuprous silicide, Cu 4 Si. Sol. in warm dil. or cone. HNO 3 . Only si. sol. in HC1, H 2 S0 4 and HF. Sol. in a mixture of HNO 3 and HF. Not attacked by solutions of alkalies. (Vi;ouroux. C. R. 1906 142. 88.) 310 CUPROUS SULPHIDE Cu 2 Si 3 . Sol. in aqua regia and fused sodium potassium carbonate, (de Chalmot, Am. Ch. J. 1896, 18, 95.) Cu 2 Si. Decomp. by water and moist air, and by acids and fused alkali. (Vigouroux, C. R. 1896, 122. 319.) Cuprous sulphide, Cu 2 S. More sol. in H 2 O than Ag 2 S, but much less than PbS. (Bodlander, Z. phys. Ch. 1898. 27, 64.) 1 1. H 2 dissolves 3.1+1CH 5 moles Cu 2 S at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Very slowly decomp. by dil. H 2 SO 4 in presence of oxygen. (Thompson, Electro- chem, Ind. 1904. 2, 225.) Decomp. by cone. H 2 SO 4 . (Pickering, C. N 1878, 37, 37:) Cold HNO 3 +Aq dissolves out Cu and leaves CuS; hot HNQ 2 dissolves with separa- tion of S. SI. sol. in boiling cone. HC1 + Aq. Insol. in (NH 4 ) 2 S+Aq. 5N-HC1 dissolves Cu 2 S very slightly (0.0038 g. Cu in 7^ hrs.) but it is more sol. in presence of Cl, when 0.672 g. are dis- solved in 7^2 hours. (Egii, Z. anorg. 1902, 30. 46.) Sol. with exclusion of air in NH 4 OH+Aq. (Malzac, Pat. 1904.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Min. Chalcocite. Completely sol. in warm HNO 3 with separation of S. Cupric sulphide, CuS. Almost absolutely insol. in H 2 O; sol. in 950,000 pts. H 2 0. When exposed to the air, dissolves in H 2 O as CuSO 4 . Easily sol. in boiling HNO 3 with separation of S. Diffi- cultly sol. in hot cone. HCl+Aq. Insol. in dil. H 2 SO 4 +Aq-(l:6). (Hoffmann, A. 115. 286. Pptd. by H 2 S or (NH 4 ) 2 S+Aq in presence of 100,000 pts. H 2 O (Pfaff), 200,000 pts. H 2 O (Lassaigne), 15,000 pts. H 2 O and 7500 pts. HC1, but with 40,000 pts. H 2 O and 20,000 pts. HC1 no colour is visible (Reinsch). 1 1. H 2 O dissolves 3.51 + 1(H moles CuS at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Insol. in H 2 SO 3 +Aq. (Guerout, C. R. 1872, 75. 1276.) Decomp. by cone. H 2 SO 4 . (Kliche, J. B. 1890, 593.) Sol.in(NH 4 ) 2 CO 3 +Aq. (Berzelius.) Sol. in alkali bicarbonates +Aq. Insol. in NH 4 NO 3 . or NH 4 Cl+Aq. (Brett.) Insol. in acidified cone, alkali chlorides + Aq. (Cushmann, Am. Ch. J. 1895, 17, 382.) Sol. in FeCl 3 +Aq with separation of S. (Cumenge and Wimmer, Dingl. 1883, 250. 123.) Decomp. by boiling CuCl 2 +Aq in presence of HC1 or NaCl. (Raschig, Gm K. 5. 1, 819.) Sol. in Fe 2 (SO 4 ) 3 +Aq in presence of large excess of air. (Thompson, Electrochem. Ind. 1904, 2, 228.) Insol. in KOH, or K 2 S+Aq, especially if boiling; appreciably sol. in colourless and even more readily in hot yellow (NH 4 ) 2 S+Aq. SI. sol. in Na 2 S+Aq, more easily in NaSH-f- Aq. (Becker, Sill. Am. J. (3) 33. 199.) 100 cc. sat. Na 2 S+Aq-(sp. gr. = 1.225) dissolve 0.0032 g. CuS. (Holland, Ann. Chim. Anal. 1897," 2. 243.) Sol. in K polysulphides (3-64%). (Prost, Bull. Soc. Belg. Chim. 1897. 103.) Appreciably sol. in alkali polysulphides + Aq. (Rossing, Z. anal. 1902, 41, 1.) Sol. in considerable quantity in alkali sulph- arsenates, sulphantimonates, and sulpho- stannates+Aq. Therefore when a mixed ppt. of CuS and As 2 S 3 , Sb 2 S 3 , or SnS is treated with K 2 S, a portion of the CuS is dissolved. (Wohler, A. 34. 236.) Sol. in alkali sulphovandates, or sulpho- tungstates+Aq. (Storch, B. 16. 2015.) Sol. in alkali sulphomolybdates + Aq. (Debray, C. R. 96. 1616.) Insof. in K thiocarbonate + Aq. (Rosen- bladt, Z. anal. 26. 15.) Sol. inKCN+Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790) ; ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Insol. in Na xanthogenate. (Ragg, Ch. Z. 1908, 32. 677.) Solubility of CuS in sugar +Aq at t. g. CuS per 1. of solution. t 10% sugar 30% sugar 50% sugar 17.5 45 75 0.5672 0.3659 1 . 1345 0.8632 0.7220 1.2033 0.9076 1 . 0589 1.2809 (Stolle, Z. Ver. Zuckerind. 1900, 50. 331.) Min. Covellite. Colloidal. Aqueous solution is stable when it contains 5 g. CuS in a litre; when it contains 4 or 5 times that amount it is decomposed in an hour. Solutions of salts of the following concen- tration cause a precipitate in the above solu- tion. Salts of univalent elements Salts of univalent elements K 3 Fe(CN) 6 1 K 4 Fe(CN) 6 1 Na 2 S 2 3 1 Na 2 CO 3 1 Na 2 HP0 4 1 Na 2 SO 4 1 K 2 Cr 2 7 . 1 KI 1 KBr KClOa 62 127 157 200 252 333 2083 80 133 166 CUPROUS SODIUM SULPHIDE 311 Salts of univalent elements Continued. NaC a H,O 2 1 : 221 (NH 4 ) 2 C 2 O 4 1 : 255 Cupric iron (ferric) sulphide, CuS, Fe 2 S 8 . Min. Cubanite. NaCl . 1 : 400 NaHCO 3 1 : 2500 Copper iron potassium sulphide, K 2 FeCuS4. K 2 S0 4 . 1 : 117 SI. attacked by cold dil. HCl+Aq. De- K 2 CrOi NaC 7 H 5 2 1 :133 1 : 166 comp. by warming. (Schneider, Pogg. 138. 318.) K 2 S 2 O 6 $* 1 :222 KC1 . . 1 : 333 Copper iron sodium sulphide, Na 2 FeCu 3 S 4 . KNO 3 . . 1 : 500 Salts of bivalent metals SI. attacked by cold dil., easily decomp, by hot HCl+Aq. (Schneider, Pogg. 138. 318.) BaS 2 O 6 . 1 : 2242 Cd(N0 3 ) 2 MgSO 4 ' . 1 : 3483 . 1 : 6830 Cuprous lead sulphide, 9Cu 2 S, 2PbS. Ba(N0 3 ) 2 . 1 : 2677 3Cu 2 S, 2PbS. BaCl 2 . . 1 : 3921 2Cu 2 S, 2PbS. Min. Cuproplumbite. Pb(C10 3 ) 2 . 1 : 6988 CdSO 4 . MnSO 4 si- . 1 : 3442 . I : 5518 Copper phosphorus sulphide. See Copper phosphosulphide. Salts of trivalent metals Ammonia alum . Chrome alum ' . A1 2 (S0 4 ) 3 . 7 . Vij . 1 : 31,896 . 1 : 58,889 . 1 : 90,909 Cupric platinum sulphide. See Sulphoplatinate, cupric. Acids SUCCITIIC 1-100 Cuprous potassium sulphide, 4Cu 2 S, K 2 S. Oxalic . J. AvA/ . 1 : 162 (Ditte, C. R. 98. 1429.) HC1 . 1 : 733 H 2 S0 4 . Citric . . . . 1 : 208 . 1 :20 Cuprocupric potassium sulphide, 3Cu 2 S, 2CuS, K 2 S. Acetic . . Not at all Not decomp. by very dil. HCl+Aq, but Tartaric . . easily by cone. HCl+Aq on warming. (Spring and de Boeck, Bull . Soc. (2) 58. 165.) (Schneider, Pogg. 138. 311.) Copper poZ^/sulphide, Cu 2 S 3 . Amorphous. Ppt. Decomp. by boiling alcohol. (Rossing, Z. anorg. 1900, 25. 413.) Cu 4 S 6 . Amorphous. Ppt. can be boiled with H 2 O without decomposition. (Rossing, Z. anorg. 1900, 25. 4, 11.) Cu 2 S 6 . Ppt.; insol. in alkali sulphides; decomp. by cone. HN0 3 . (Bodroux, C. R. 1900, 130. 1398.) Could not be obtained. (Rossing, Z. anorg. 1900, 25. 414.) Cu 2 S,. Ppt. Decomp. by H 2 O. Sol. in alkali and barium po]ysulphides+Aq. Decomp. by colorless alkali sulphides +Aq. (Rossing, Z. anorg. 1900, 25. 407.) Cuprous iron (ferric) sulphide, Cu 2 S, Fe 2 S 3 . Decomp. by cone. HCl+Aq. Sol. in boiling HNO 3 +Aq of 1.2 sp. gr. (Schneider, J. pr. (2) 38. 569.) Min. Chalcopyrite. Insol. in HCl+Aq. When heated in a sealed tube with H 2 S+Aq. a portion of it dissolves with difficulty and subsequent deposition of S. (Senarmont, A. ch. (3) 32. 168.) Cuprocupric iron (ferric) sulphide, Cu 2 S, CuS, FeS. Min. Bornite. Sol. in HCl+Aq with a residue of S. Copper potassium pofysulphide, KCuS 4 . SI. sol. in cold H 2 O. Decomp. by hot H 2 O. Decomp. by cone, and dil. HC1, H 2 SO 4 and HNO 8 . SI. sol. in alcohol. (Biltz and Herms, B. 1907, 40. 977.) 2CuS 3 , K 2 S. Decomp. by H 2 O, NH 4 OH, or NH 4 SH+Aq. (Priwoznik, B. 5. 1291.) K 2 Cu 8 Sio. Easily sol. in H 2 O. 1 g. is sol. in less than 5 com. H 2 O. Rapidly decomp. by dil. acids, slowly by cone, acids. SI. sol. in alcohol. (Biltz and Herms, B. 1907, 40. 983.) Cupric rubidium poZi/sulphide, RbCuS 4 . As K salt. (Biltz and Herms, B. 1907, 40. 978.) Rb 2 Cu 8 Sio. Easily sol. in H 2 0. Decomp. acids. SI. sol. in alcohol. (Biltz and Herms, B. 1907, 40. 985.) Cuprous silver sulphide, Cu 2 S, Ag 2 S. Min. Stromeyerite. Sol. in HNO 8 +Aq with separation of S. Cu 2 S, 3Ag 2 S. Min. Jalpaite. As above. Cuprous sodium sulphide, Na 2 S, Cu 2 S. (Bodlander. Z. Elektrochem. 1905, 11. 181.) Na 2 S, 2Cu 2 S. (Bodlander, Z. Elektrochem. L905, 11. 181.) 312 CUPROCUPRIC SODIUM SULPHIDE Cuprocu Na sodium sulphide, Cu 2 S, CuS, Scarcely decomp. by cold dil. HCl-fAq; cone. HCl+Aq decomp. easily on warming, without, however, dissolving all the Cu 2 S. Completely decomp. by warm HNO 3 +Aq. (Schneider, Pogg. 138. 315.) Copper zinc sulphide, CuS, 3ZnS. Copper sulphophosphide. See Copper phosphosulphide. Cupric telluride, CuTe. Cu 2 Te. Insol. in H 2 O. (Parkmann, Sill. Am. J. (2) 3. 335.) Cu 2 Te. (Brauner, M. 1889. 423.) Croceocobaltic bromide. Co(NH 8 ) 4 (N0 2 ) 2 Br. Very si. sol. in cold, easily in hot H 2 O. (Gibbs, Proc. Am. Acad. 10. 1.) chloraurate, 2Co(NH 8 ) 4 (N0 2 ) 2 Cl, AuCl 3 . Difficultly sol. in H 2 O. chloride, Co(NH 8 ) 4 (NO 2 ) 2 Cl. Very si. sol. in cold easily in hot H 2 O, but more sol. than the sulphate. (Gibbs.) chloroplatinate, 2Co(NH 3 )4(NO 2 ) 2 Cl, PtCl 4 . Can be recrystallised without decomp. with difficulty. (Gibbs and Genth, Sill. Am. J. (2) 24. 91.) chromate,[ Co(NH,) 4 (NO 2 ) 2 ] 2 CrO 4 . SI. sol. in H,O. (Gibbs.) bichromate, [Co(NH 8 ) 4 (NO 2 ) 2 ] 2 Cr 2 O 7 81. sol. in H 2 0. (Gibbs.) periodide, Co(NH 8 ) 4 (NO 2 ) 2 I, I 2 . Difficultly sol. in cold H 2 O and alcohol. Decomp. by hot H 2 0. (Gibbs.) nitrate, Co(NH 8 ) 4 (N0 2 ) 2 NO 8 . SI. sol. in cold, easily sol. in hot H 2 O or dil. .acids. Much more sol. than the sulphate. +4H 2 0. SI. sol. in H 2 O; insol. in alcohol. (Loebe Dissert, 1902,) Cadmium cyanide, Cd(CN) 2 . SI. sol. in H 2 O. 100 pts. H 2 O dissolve 1.7 pts. Cd(CN) 2 at 15. (Joannis.) Easily sol. in acids; sol. in KCN+Aq. Sol. in warm NH 4 OH+Aq, but insol. in (NH 4 ) 2 CO 3 +Aq. (Wittstein.) Insol. in benzonitrile. (Naumann, B 1914, 47. 1370.) Cadmium calcium cyanide, Cd(CN) 2 , 4Ca(CN) 2 +20H 2 O. Sol. in H 2 O and in alcohol. (Loebe, Dis- sert, 1902.) Cadmium chromic cyanide. See Chromicyanide, cadmium. Cadmium cobaltic cyanide. See Cobalticyanide, cadmium. Cadmium cuprous cyanide, 2Cd(CN) 2 , Cu 2 (CN) 2 . Permanent. Insol. in H 2 O. SI. sol. in cold, easily in warm HCl+Aq without de- comp., except by long boiling. Insol. in NH 4 OH, or NH 4 salts+Aq. (Schiiler.) Cadmium cupric cyanide, Cd(CN) 2 , Cu(CN) 2 . Very unstable. Cadmium gold (aurous) cyanide, Cd(CN) 2 , 2AuCN. Nearly insol. in cold H 2 O. SI. sol. in boil- ing H 2 O. Insol. in alcohol. (Lindbom.) Cadmium mercuric cyanide, 2Cd(CN) 2 , 3Hg(CN) 2 . Permanent. Readily sol. in cold H 2 O. (Schiiler.) Cadmium mercuric cyanide mercuric iodide, Cd(CN) 2 , Hg(CN) 2 , HgI 2 +8H 2 0. Very sol. in H 2 O. (Varet, Bull. Soc. (3) 6.8.) +7H 2 O. Sol. mH 2 OandinNH 4 OH+Aq. (Varet, C. R. 1890, 111, 679.) Cadmium mercuric cyanide mercuric iodide, Cd(CN) 2 , Hg(CN) 2 , HgI 2 +8H 2 0. Very sol. in H 2 O. (Varet, Bull. Soc. (3) 6. 8.) " -f7H 2 O. Sol. inH 2 OandinNH 4 OH+Aq. (Varet, C. R. 1890, 111. 679.) Cadmium mercuric cyanide mercuric iodide ammonia, Cd(CN) 2 , Hg(CN) 2 , Hgl, 4NH 8 . Very easily decomp. (Varet, Bull. Soc. (3) 6. 22.) Cadmium molybdenum cyanide. See Molybdocyanide, cadmium. Cadmium potassium cyanide, Cd(CN) 2 , 2KCN. Sol. in 3 pts. cold, and 1 pt. boiling H 2 O. Insol. in absolute alcohol. (Rammelsberg.) Cadmium sodium cyanide, Na 2 Cd 2 (CN) 6 +3H 2 O. Sol. in H 2 and in alcohol. (Loebe, Dis- sert, 1902.) Cadmium strontium cyanide, Cd(CN) 2 , 2Sr(CN) 2 +3H 2 0. Sol. in H 2 O and in alcohol. (Loebe. Dis- sert. 1902.) Cadmium tungsten cyanide, Cd 2 W(CN) 8 + 8H 2 O. Nearly insol. in H 2 O. SI. sol. in dil. HC1. Sol. in cone. NH 4 OH + Aq. Insol. in organic solvents. (Olsson, Z. anorg. 1914, 88. 68.) Cadmium cyanide c&hydrazine, Cd(CN) 2 , (N 2 H 4 ) 2 . Easily sol. in dil. acids. (Franzen. Z. anorg. 1911, 70. 152.) Caesium cuprous cyanide, CsCN, CuCN + H 2 separates CuCN. (Grossmann, Z. anorg. 1905, 43. 98.) 2CsCN, CuCN+H 2 O. Sol. in H 2 O. (Grossmann, Z. anorg. 1905, 43. 98.) 2CsCN, SCuCN. Insol. in, and not de- comp. by H 2 O. (Grossmann, Z. anorg. 1905, 43. 98.) Caesium tungsten cyanide. See Tungstocyanide, caesium. lalcium cyanide, Ca(CN) 2 . Sol. in H 2 O, but the solution is very un- stable. (Schulz.) Ca(CN) 2 , 3CaO+15H 2 O. Decomp. by H 2 O. (Joannis, A. ch. (5) 26. 496.) Jalcium cuprous cyanide, Ca(CN) 2 , CuCN + 4H 2 O. Easily decomp. by H 2 O. (Grossmann, Z. anorg. 1905, 43. 106.) Ca(CN) 2 , 3CuCN+8H 2 O. Immediately CYANIDE AMMONIA, CUPRIC MOLYBDENUM 315 decomp. by H 2 O. (Grossmann, Z. anorg. 1905, 43. 99.) Calcium gold (aurous) cyanide, Ca(CN) 2 , 2AuCN+3H 2 O. Easily sol. in hot or cold H 2 O or in alcohol. (Lindbom.) Calcium manganous cyanide, Ca(CN) 2 , 2Mn(CN) 2 . Ppt. (Descamps.) See also Manganocyanide, calcium. Calcium mercuric cyanide, Ca(CN) 2 , 2Hg(CN) 2 +8H 2 0. Very deliquescent. (Grossmann, B. 1904, 37. 4143.) 2Ca(CN) 2 , 3Hg(CN) 2 +6H 2 O. Very sol. in H 2 O. (Grossmann, B. 1904, 37. 4143.) Calcium mercuric cyanide iodide, Ca(CN) 2 , HgI 2 , Hg(CN) 2 +7H 2 0. (Varet, C. R. 1895, 121. 499.) Calcium nickel cyanide, Ca(CN) 2 , Ni(CN) 2 + zH 2 O. Sol. in H 2 O. Calcium. tungsten cyanide. See Tungstocyanide, calcium. Calcium zinc cyanide, (Ca(CN) 2 , Zn(CN) 2 + Sol. in H 2 and in alcohol. (Loebe, Dis- sert. 1902.) Cerous cyanide (?). Ppt. Very easily decomp. (Behringer, A, 42. 139.) Chromic cyanide, with MCN. See Chromicyanide, M. Chromous potassium cyanide. See Chromocyanide, potassium. Cobaltous cyanide, Co(CN) 2 +H 2 O. Insol. in H 2 O. Easily sol. in NH 4 OH+Aq and KCN+Aq; also in (NH 4 ) 2 C0 3 , or NH succinate+Aq; insol. in NH 4 NO 3 , or NH 4 C +Aq. (Wittstein.) Cobaltous cyanide with 4MCN. See Cobaltocyanide, M. Cobaltic cyanide with 3MCN. See Cobaltocyanide, M. Cobalt gold (aurous) cyanide, Co(CN) 2 2AuCN. Insol. in H 2 O or cold HCl+Aq. Cobalt hydrazine cyanide, (N 2 H 4 ) 4 Co(CN) 6 . Deliquescent. (Franzen, Z. anorg. 1911, 70. 155.) Cobaltous cyanide ammonia, Co(CN) 2 , 2NH 3 . ' Unstable. (Peters, B. 1908, 41. 3178.) Cuprous cyanide, Cu 2 (CN) 2 . Insol. in H 2 O and dil. acids. Sol. in NH 4 OH, (NH 4 ) 2 SO 4 , or NH 4 succinate-f Aq, and in hot NH 4 C1, or NH 4 NO 3 +Aq. Sol. hi cone. HCl+Aq. Sol. in KCN+Aq. Easily sol. in cone. NH 4 SCN or KSCN + Aq SI. sol. in NaSCN+Aq, (Grossmann, Z. anorg. 1903, 37. 408.) SI. sol. in liquid NH 2 . (Franklin, Am. Ch. J. 1898, 20. 827.) Very si. sol. hi pyridine. (Schroeder, Dissert. 1902.) Mol. weight determined hi pyridine. Werner, Z. anorg. 1897, 15. 20.) Cupric cyanide, Cu(CN) 2 . Easily decomp. Insol. in H 2 O. Sol. in pyridine. (Schroeder, Dissert. 1901.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Cuprocupric cyanide, Cu(CN) 2 , Cu 2 (CN) 2 + 5H 2 O. Insol. in H 2 O, but decomp. by boiling. Sol. in cold cone. HCl+Aq. Sol. in NH 4 OH+Aq. (NH 4 ) 2 CO 3 +Aq, and in hot NH 4 salts +Aq. Easily sol. in KCN+Aq. +H 2 O. Ppt. (Dufau.) +Cu(CN) 2 , 2Cu 2 (CN) 2 +H 2 0. Ppt. Cuprous hydrazine cyanide, Cu 2 (CN) 2 , N 2 H S CN. Insol. hi alcohol and H 2 O. (Ferratini, C.C. 1912, 1. 1281.) Cupric iridium cyanide. See Iridicyanide, cupric. Cuprous lithium cyanide, Cu 2 (CN) 2 , LiCN + H 2 0. Gradually decomp. by H 2 O. (Grossmann, Z. anorg. 1905, 43. 97.) Cuprous magnesium cyanide, Cu 2 (CN) 2 , Mg(CN) 2 + llH 2 0. Decomp. by H 2 O. (Grossmann, Z. anorg. 1905, 43. 103.) Cuprous mercuric cyanide bromide, Cu(CN) 2 , 2Hg(CN) 2l HgBr 2 . Sol. in H 8 O. (Varet, C. R. 1890, 110. 148.) Cupric molybdenum cyanide ammonia. See Molybdocyanide ammonia, cupric. 316 CYANIDE, CUPROUS POTASSIUM Cuprous potassium cyanide, Cu(CN) 2 , 2KCN. SI. sol. in H 2 O, with partial decomp. De- comp. by acids, but not by alkalies. Decomp. by boiling H 2 O. Sol. in NH 4 OH +Aq. (Fleurent, C. R. 1893, 116. 191.) Sol. without decomp. in cone. KSCN. (Grossmann, Z. anorg. 1903, 37. 407.) Sol. without decomp. in KCN+Aq. (Tread well and Girsewald, Z. anorg. 1904, 38. 94.) Cu 2 (CN) 2 , KCN+HoO. Almost insol. in cold H 2 O. 100 cc. H 2 O dissolve 0.0594 g. at 15. Decomp. by much hot H 2 O with sep- aration of Ciio(CN) 2 . Sol. in KCN+Aq or in NH 4 OH+Aq. (Treadwell and Girsewald, Z. anorg. 1904, 38. 93.) 3Cu 2 (CN) 2 , 4KCN. Sol. in H 2 O. Cu 2 (CN) 2 , 6KCN. Sol. in H 2 O. Cuprous potassium cyanide ammonia. Cu 2 (CN) 2 , KCN, NH 3 . (Treadwell and Girsewald, Z. anorg. 1904, 39. 88.) Cuprous potassium cyanide potassium sul- phocyanide, Cu 2 (CN) 2 , 4KCN, 2KSCN, H 2 O. Easily sol. in cold H 2 O. (Itzig, B. 1902, 36. 108.) Cupric potassium cyanide, Cu(CN) 2 , 2KCN. Sol. in 3 /4 pt. H 2 O at 15 and Vs pt. at 100. (Buignet, J. Pharm. 1859, (3), 35. 168.) Cuprocupric potassium cyanide. Cu 2 (CN) 2 , Cu(CN) 2 , 2KCN. (Straus, Z. anorg. 1895, 9. 15.) Cuprous rubidium cyanide, Cu 2 (CN) 2 , 2RbCN. SI. sol. in H 2 0. Pure H 2 separates CuCN. (Grossmann, Z. anorg. 1905, 43. 100.) 3Cu 2 (CN) 2 , 4RbCN. SI. sol. in H 2 O. Pure H 2 separates CuCN. (Grossmann, Z. anorg. 1905, 43. 98.) Cuprous silver cyanide, Cu 2 (CN) 2 , 2AgCN. Ppt. Cu 2 (CN) 2 , 6AgCN. Sol. in excess of Cu 2 (CN) 2 , KCN+Aq. (Rammelsberg.) Cuprous sodium cyanide, Cu 2 (CN) 2 , 2NaCN. CTraube, Z. anorg. 1894, 8. 21.) +4H 2 O. Docomp. by H 2 O. Sol. in excess of NaCN+Aq. (Grossmann, Z. anorg. 1905, 43. 96.) Cu 2 (CN) 2 , NaCN+2H 2 O. Decomp. by H 2 Q. ( Grossmann, Z. anorg. 1905, 43. 96.) Cu 2 (CN) 2 , 4NaCN+6H 2 O. Very sol. in H 2 O without decomp. (Grossmann/Z. anorg. 1905, 43. 96.) Cu 2 (CN) 2 , 6NaCN+6H 2 O. Very sol. in H 2 O without decomp. (Grossmann, Z. anorg. 1905, 43. 96.) Cuprous strontium cyanide, Cu 2 (CN) 2 , Sr(CN) 2 +8H 2 O, H 2 O separates Cu 2 (CN) 2 . (Grossmann, Z. anorg. 1905, 43. 103.) Cuprous cyanide ammonia, Cu 2 (CN) 2 , 2NH 3 . Nearly insol. in cold H 2 O. Easily sol. in NH 4 OH+Aq in absence of oxygen. Insol. in alcohol and ether. Decomp. by hot H 2 O and acids. (Treadwell and Girsewald, Z. anorg. 1904, 39. 87.) Cuprocupric cyanide ammonia, Cu 2 (CN) 2 , Cu(CN) 2 , 2NH 3 . (Malmberg, Arch. Pharm. 1898, 236. 256.) +H 2 O. SI. sol. in cold, decomp. by boiling H 2 O. Sol. in NH 4 OH+Aq. (Dufau/A. 88. 278.) Cu(CN) 2 , Cu 2 (CN) 2 3NH 3 . (Mills, Z. Ch. 1867. 545.) SI. decomp. by boiling H 2 0. Sol. in NH 4 OH+Aq and can be recryst. therefrom. Insol. in alcohol and ether. Decomp. by alkalies and acids. (Treadwell and Girse- wald, Z. anorg. 1904, 39. 96.) Cu(CN) 2 , Cu 2 (CN) 2 , 4NH 3 . Insol. in cold, decomp. by hot H 2 O. Sol. in NH 4 OH, or (NH 4 ) 2 CO 3 +Aq. (Treadwell and Girse- wald, Z. anorg. 1904, 39. 92.) 2Cu 2 (CN) 2 , Cu(CN) 2 , 2NF 3 . Insol. in H 2 O, alcohol and ether. Sol. in NH 4 OH + Aq. Decomp. by boiling acids and alkalies. (Treadwell and Girsewald, Z. anorg. 1904, 39. 92.) +H 2 O. (Monthier, J. Pharm. 11. 257.) Cu(CN) 2 , 2Cu 2 (CN) 2 , 4NH 3 . (Hillen- kamp, A. 97. 218.) Cu(CN) 2 , 2Cu 2 (CN) 2 , 6NH 3 . (Schiff and Becchi, A. 134. 33.) 2Cu(CN) 2 , Cu 2 (CN) 2 , 2NH 3 +3H 2 O. (Fleurent, C. R, 114. 1060.) 2Cu(CN) 2 , Cu 2 (CN) 2 , 4NH 3 +H 2 O. Cor- rect formula for Cu(CN) 2 , Cu 2 (CN) 2 , 4NH 8 . (Bouveault, Bull. Soc. (3)4. 641.) Cuprous cyanide ammonium sulphocyanide, Cu 2 (CN) 2 , 3NH 4 SCN. Decomp. by H 2 O. (Grossmann, Z. anore. 1903, 37. 409. Cupric cyanide hydrazine, Cu(CN) 2 (N 2 H 4 ). Insol. in H 2 O and cold dil. acids. Sol. in warm dil. acids. (Franzen, Z. anorg. 1911,70. 154.) Cuprous cyanide mercuric iodide, Cu 2 (CN) 2 , HgI 2 . Sol. in H 2 O. (Varet, Bull. Soc. (3) 4. 484.) CYANIDE, MANGANOUS STRONTIUM 317 Cuprous cyanide potassium sulphocyanide, Cu 2 (CN) 2 , 3KSCN. Decomp. by H 2 O. (Grossmann, Z. anorg. 1903, 37. 409.) Gold (aurous) cyanide, AuCN. Insol. in H 2 O, alcohol, or ether. Not at- tacked by dil., or cone, acids, even boiling aqua regia. Sol. in NH 4 OH+Aq, also in soluble cy- anides +Aq. Slowly decomp. by boiling KOH+Aq, also by (NH 4 ) 2 S+Aq. Sol. in K 4 Fe(CN) 6 +Aq. (Bentel, Z. anorg. 1912, 78. 152.) Gold (auric) cyanide with MCN. See Auricyanide, M. Gold (auroauric) mercuric cyanide auric mercuric chloride, 4AuCN, Au(CN) 3 , 5Hg(CN) 2 , 7AuCl 3 , 5HgCl 2 . (Schmidt, Ch. Z. 1896, 20. 633.) Gold (aurous) potassium cyanide, AuCN, KCN. Sol. in 7 pts. cold, and less than 0.5 pt. boil- ing H 2 O. SI. sol. in cold, and somewhat more sol. in boiling alcohol. Insol. in ether. (Himly, A. 42. 160.) Decomp. by warm acids, even tartaric, and acetic acids. Gold (aurous) sodium cyanide, AuCN, NaCN. SI. sol. in cold, more easily in hot H 2 0. SI. sol. in alcohol. (Lindbom.) Gold (aurous) strontium cyanide, 2AuCN, Sr(CN) 2 +3H 2 0. As the Na salt. Gold (aurous) zinc cyanide, 2AuCN, Zn(CN) 2 . Nearly insol. in hot or cold H 2 O. Insol. in cold HCl+Aq. Gold (auric) cyanide auric mercuric chloride, Au(CN) 3 , AuCl 3 , 2HgCl 2 . (Schmidt, Ch. Z. 1896, 20. 633.) Gold (auroauric) cyanide aurous mercuric chloride, 12AuCN, 3Au(CN) 3 , 4AuCl, 2HgCl 2 . (Schmidt, Ch. Z. 1896, 20. 633.) Gold (auroauric) cyanide mercuric chloride. ISAuCN, 2Au(CN) 3 , 5HgCl 2 . (Schmidt, Ch. Z. 1896, 20. 633.) Iridium cyanide, Ir(CN) 3 . Insol. in H 2 O. Sol. in HCN +Aq. Iridium cyanide with MCN. See Iridicyanide, M Lanthanum cyanide, La(CN) 3 , Ppt. (Frerichs and Smith, B. 11. 910, 1151.) Lead cyanide, Pb(CN) 2 . SI. sol. in cold, more in hot H 2 O. Sol. in HNOs+Aq, and KCN+Aq. Partially sol. in NH 4 OH+Aq, and NH 4 salts+Aq. Not pptd. in presence of Na citrate. Above compound is 2PbO, Pb(CN) 2 + H 2 O. (Joannis, A. ch. (5) 26. 204.) 2PbO, Pb(CN) 2 +H 2 6. Insol. in H 2 O. Lead tungsten cyanide. See Tungstocyanide, lead. Lead zinc cyanide, Pb(CN) 2 , 2Zn(CN) 2 . Ppt. (Rammelsberg.) Lead cyanide chloride, 2Pb(CN) 2 , PbCl 2 . Insol. in H 2 O. (Grissom and Thorp, Am. Ch. J. 10. 229.) Lithium mercuric cyanide mercuric iodide, 2Li(CN) 2 , Hg(CN) 2 , HgI 2 +7H 2 0. Deliquescent; s.ol. in H 2 O. (Varet, C. R. 111. 526.) Magnesium cyanide, Mg(CN) 2 . Known only in aqueous solution which de- composes on evaporation. (Schulz.) Magnesium mercuric cyanide, 2Mg(CN) 2 , 3Hg(CN) 2 +5H 2 0. (Grossmann, B. 1904, 37. 4143.) Magnesium mercuric cyanide mercuric bromide, Mg(CN) 2 , Hg(CN) 2 , HgBr 2 + 8H 2 O. Very sol. in H 2 O. (Varet, Bull. Soc. (3) 7. 170.) Magnesium mercuric cyanide mercuric iodide, Mg(CN) 2 , Hg(CN) 2 , Hgl + 8H 2 O. Sol. in H 2 O. (Varet, Bull. Soc. (3) 7. 170.) Magnesium platinum cyanide. See Platinocyanide, magnesium. Magnesium tungsten cyanide. See Tungstocyanide, magnesium. Manganous and manganic cyanides. See Manganocyanhydric, and Mangani- cyanhydric acids. Manganous strontium cyanide, 2Mn(CN) 2 . Sr(CN) 2 . Ppt. (Descamps.) See also Manganocyanide, strontium. 318 CYANIDE, MANGANOUS TUNGSTEN Manganous tungsten cyanide. See Tungstocyanide, manganous. Manganic cyanide, with MCN. See Manganicyanide, M. Manganous cyanide with MCN. See Manganocyanide, M. Mercuric cyanide, basic, Hg(CN) 2 , HgO. SI. sol. in cold, moderately sol. in hot H 2 O. Sol. with decomp. in KOH, KCN, or KC1 + Aq. (Johnston.) Decomp. by H 2 O over 80. (Holdermann, Arch. Pharm. 1906, 244. 135.) Cold H 2 O dissolves about 1%, boiling H 2 O about 5%. (Borelli, Gazz. ch. it. 1908, 38. (1;, 361.) 1.1% dissolves in H 2 O at ord. temp. (Richard, J. Chim. Phys. (6) 18. 555.) At 1/100 mol. dissolve in 1 1. H 2 O. At 25 1/32 " " " " " At 90 1/10 " " " " " (Borelli, Gazz. ch. it. 1908, 38. (1), 361.) 1000 cc. cold H 2 O dissolve 1.35g. (Holder- mann, Arch. Pharm. 1906, 244. 135.) Less sol. in cold H 2 O than Hg(CN) 2 . (Pieverling, J. B. 1899, 783.) Somewhat sol. in dil. alcohol. Practically insol. in alcohol, ether, C 6 H 6 and all organic solvents. (Borelli, Gazz. ch. it. 1908, 38, (1), 361.) Sol. in 110 pt. alcohol of 90 Be. (Richard, J. Chim. Phys. (6), 18. 555.) 3Hg(CN) 2 , HgO. (Joannis, A. ch. (5) 26. 469.) Moderately sol. in H 2 O. (Barthe, J. Pharm. 1896, (6), 3. 186.) Very sol. in hot, less sol. in cold H 2 Q. (Holdermann, Arch. Pharm. 1904, 242. 32!) Easily sol. in HC1. (Joannis, A. ch. 1882, (5) 26. 511.) Hg(CN) 2 , 3HgO. More sol. in H 2 O than Hg(CN) 2 , HgO. Mercuric cyanide, Hg(CN) 2 . Moderately sol. in H 2 O. 100 pts. Hg(CN) 2 +Aq sat. at 101.1 con- tain 35 pts. Hg(CN) 2 , or 100 pts. H 2 O dis- solve 53.85 pts. Hg(CN) 2 at 101.1. (Grif- fiths.) Sol. in 8 pts. H 2 O at 15. (Abl.) Sol. in 11 pts. cold, and 2.5 pts. boiling H 2 O. (Wittstein.) 8 g. are sol. in 100 g. H 2 O at -0.45. (Guthrie, Phil. Mag. 1878, (5) 6. 40.) 100 g. H 2 O dissolve 9.3 g. at 13.5. (Timo- feiev, Dissert. 1894.) 100 cc. sat. solution contain 9.3 g. at 20. (Konowalow, J. russ. Soc. 1898, (4) 30. 367.) Solubility in H 2 at 25 = 0.44 mol. 1 (Sherrill, Z". phys. Ch. 1903, 43. 735.) 1 1. H 2 dissolves 0.3956 mol. (Hofmann and Wagner, Z. Elektrochem. 1909, 15. 444.) 100 g. H 2 O dissolve 12.5 g. at 15. (Marsh and Struthers, Chem. Soc. 1905, 87. 1879.) 100 g. H 2 O dissolve 11.27 g. at 25. Sp. gr. solution = 1.08 13. (Herz and Anders, Z. anorg. 1907, 52. 164.) Hg(CN) 2 +Aq containing 7.23% Hg(CN) 2 has sp.gr. 20/20 = 1.0572. Hg(CN) 2 +Aq containing 9.07% Hg(CN) 2 hassp. gr. 20/20 = 1.0743. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 282.) Sp. gr. at 16/4 of Hg(CN) 2 +Aq contain- ing 7.8921% Hg(CN) 2 = 1.06376; containing 5.4037% = 1.04246; containing 7.5009% = 1.06049. (Schonrock, Z. phys. Ch. 1893, 11. 770.) Not decomp. by acids except hot cone. H 2 S0 4 . Sol. without decomp. in HNO 3 +Aq. (Ber- zelius.) 1 1. NH 4 OH+Aq (5.2% NH 3 ) dissolves 204.3 g. at about 25. (Konowalow.) Solubility in bases. 1 1. H 2 O containing 0.3286 mols. KOH dis- solves 0.5179 mols. Hg(CN) 2 . 1 1. H 2 containing 0.2350 mols. NaOH dissolves 0.4840 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.4775 mols. NaOH dissolves 0.5977 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.9475 mols. NaOH dis- solves 0.79603 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.970 mols. LiOH dis- solves 0.6543 mols. Hg(CN) 2 . 1 J. H 2 O containing 0.480 mols. LiOH dis- solves 0.5500 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.243 mols. LiOH dis- solves 0.4840 mols. Hg(CN) 2 . (Hofmann and Wagner, Z. Elektrochem. 1909, 15. 444.) Solubility in KCN+Aq at 25. Concentration of KCN Mols. per litre Solubility of Hg(CN) 2 Mols. per litre 0.0493 0.0985 0.1970 0.4855 0.5350 0.627. (Sherrill, Z. phys. Ch. 1903, 43. 719.) Solubility in Na 2 CO 3 +Aq. 1 1. H 2 O containing 0.4923 mols. Na 2 CO 3 dissolves 0.4956 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.2443 mols. Na 2 CO 3 dissolves 0.4464 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.1250 mols. Na 2 CO 3 dissolves 0.4147 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.0000 mols. Na 2 CO 3 dissolves 0.3952 mols. Hg(CN) 2 . (Hofmann and Wagner, Z. Elektrochem, 1909, 15. 444.) CYANIDE, MERCURIC 319 Solubility in KNO 3 +Aq at 25. 1 1. H 2 O containing 0.9574 mols. KNO 3 dissolves 0.5383 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.4614 mols. KN0 3 dissolves 0.4619 mols. Hg(CN) 2 . 1 1. H 2 O containing 0.0000 mols. KNO 3 dis- solves 0.3956 mols. Hg(CN) 2 . (Hofmann and Wagner, Z. Elektrochem. 1909 15. 444.) Insol. in liquid CO 2 . (Buchner, Z. phys Ch. 1906, 54. 674.) Very easily sol. in liquid NH 3 . (Franklin Am. Ch. J. 1898, 20. 829.) Solubility of Hg(CN) 2 in ethyl alcohol at t Solubility of Hg(CN) 2 in ethyl alcohol +Aq at 25. P = g. alcohol in 100 g. alcohol +Aq. Hg(CN) 2 = millimols Hg(CN) 2 in 10 cc. of the solution. p Hg(CN) 2 Sp. gr. 20.18 40.69 70.01 100 4.34 3.47 3.58 3.80 3.25 1.0813 1.0339 1.0006 0.9419 0.8552 (Herz and Anders, . c.) Solubility of Hg(CN) 2 in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the solvent. Hg(CN) 2 =g. Hg(CN) 2 in 10 ccm. of the solution. S 25/4=Sp. gr. of the sat. solution. t % HgCl 2 10 20 30 40 8.3 8.8 9.25 9.8 10.3 (Timofeiev, Solubility of Hg(CN) HeCCN^ ff Hff( Dissert. 1894.) 2 in methyl alcohol at t. CN) 2 in 100 g. of the ution. p Hg(CN) 2 S 25/4 sol 4.37 10.4 41.02 80.69 84.77 91.25 100 0.819 0.902 1.01 1.67 2.82 2.96 3.09 3.43 0.8552 0.8618 0.8707 0.9267 1.024 1.034 1.052 1.076 t Hg(CN) 2 0.0 14.7 23.4 27.4 31.7 38.1 44.5 26.10 29.17 32.01 31.77 32.53 33.29 34.05 (Herz and Kuhn, Z. anorg. 1908, 58. 166.) (Dukelski, Z. anorg. 1907, 53. 337.) 100 pts. methyl alcohol dissolve 44.2 pts. Hg(CN) 2 at 19!5; 100 pts. ethyl alcohol dissolve 2.09 pts. at 19.5. (de Bruyn, Z. phys. Ch. 1892, 10. 784.) Sol. in 2.5 pts. methyl alcohol at 14; in 20 pts. ethyl alcohol at 15. (Marsh, Chem. Soc. 1905, 87. 1878.) Solubility of Hg(CN) 2 in methyl alcohol + Aq at 25. P = g. alcohol in 100 g. alcohol+Aq. Hg(CN) 2 = millimols. Hg(CN) 2 in 10 cc. of the solution. 100 g. propyl alcohol dissolve 3.79 g. Hg(CN) 2 at 13.5. (Timofeiev, Dissert. 1894.) Solubility in mixtures of propyl and methyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. Hg(CN) 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. P Hg(CN) 2 Sp. gr. p G S 25/4 10.60 30.77 37.21 47.06 64.00 78.05 100 4.34 4.37 4.94 5.40 6.49 8.13 9.75 13.60 1.0813 1.0642 1.0484 1.0430 1.0426 1.0441 1 . 0484 1.0762 11.11 23.8 65.2 91.8 93.97 96.6 100 3.43 2.952 2.448 1.048 0.504 0.423 0.398 0.344 1.0760 1.0327 0.9891 0.8800 0.8376 0.8335 0.8322 0.8283 (Herz and Anders, Z. anorg. 1907, 62. 165.) (Herz and Kuhn, Z. anorg. 1908, 60.158.) 320 CYANIDE AMMONIA, MERCURIC NICKEL Solubility in mixtures of propyl and ethyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. Hg(CN) 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. 100 g. acetonitrile dissolve 9.58 g. Hg(CN) 2 at 18. (Naumann and Schier, B. 1914, 47. 249.) Solubility in benzonitrile at 18 = 1.093 g. in 100 g. (Naumann, B. 1914, 47. 1370.) SI. sol. in ethyl amine. (Shinn, J. phys. Chem. 1907, 11. 538.) Very sol. in liquid methyl amine. (Gibbs, J. Am. Chem. Soc. 1906, 28. 1419.) Sol. in paratoluidine. (Werner, Z. anorg. 1897, 15. 7.) Mol. weight determined in pyridine and benzonitrile. ''Werner, Z. anorg. 1897, 15. 20 and 32.) 100 g. pyridine dissolve 64.8 g. Hg(CN) 2 at 18. (Schroeder, Z. anorg. 1905, 44. 6.) Solubility in pyridine. P G S 25/4 8.1 17.85 56.6 88.6 91.2 95.2 100 0.819 0.790 0.730 0.521 0.387 0.384 0.364 0.344 0.8552 0.8549 0.8527 ' 0.8386 0.8311 0.8306 0.8293 0.8283 (Herz and Kuhn, 1. c.) Sp. gr. at 16/4 of Hg(CN) 2 +alcohol, containing 8.2206 %Hg(CN) 2 = 0.85273; con- taining 5.8652 % = 0.8348 + . Sp. gr. of 16/4 of Hg(CN) 2 + pyridine containing 29.6018% Hg(CN) 2 = 1.28155; containing 23.2275% = 1.20198. (Schonrock, Z. phys. Ch. 1893, 11. 771.) 1 1. ether dissolves 0.01 mol. at 25. (Sher- rill, Z. phys. Ch. 1903, 43. 735.).) Easily sol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 84.) 100 g. glycerol dissolve 27 g. Hg(CN) 2 at 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) Nearly insol. in C 6 H 6 . (Sherrill, Z. phys. Ch. 1903, 43. 735.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) 100 g. boiling methyl acetate dissolve 3.2 g. (Steiner, Dissert, 1906.) Solubility of Hg(CN) 2 in ethyl acetate +Aq at 25. P = g. ethyl acetate in 100 g. ethyl acetate +Aq. Hg(CN) 2 =rnillimols Hg(GN) 2 in 10 cc. of the solution. Mols. per 100Hg(CN) 2 Temp, of Solidification Mols. per 100Hg(CN) 2 Temp, of Solidification 7.1 8.7 10.1 10.4 11.3 12.9 13.8 15.8 15.9 17.3 18.4 19.3 20.6 22.3 9 11 12.3 12.2 13 13.5 14.5 16.5 20.5 22.5 28.5 32 38 42 22.9 23.7 25.3 26.0 26.6 27.5 27.7 29.0 32.0 33.8 34.4 38.3 45 46 53 54.5 56.6 68 70 86 111 122.5 125 141 (Staronka, Anz. Ak. Wiss. Krakau, 1910. 372.) Solubility in quinoline. Mols. per 100Hg(CN) 2 Temp of Solidification Mols. per 100Hg(CN) 2 Temp, of Solidification 4.2 6.0 8.2 9.2 45 54 89(61) 99(61) 13.2 17.4 22.5 27.1 137 161 180 192 p Hg(CN) 2 Sp. gr. 4.39 96.76 100 4.34 4.295 1.056 0.714 1.0810 1.0797 1.9374 0.09097 (Staronka, 1. c.) Solubility in aniline. Mols. per 100Hg(CN) 2 Temp, of Solidification Mols. per 100Hg(CN) 2 Temp, of Solidification (Herz and Anders, Z. anorg. 1907, 52. 165.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Solubility in organic solvents at 18-20. 100 g. tetrachlormethane dissolve 0.001 g. Hg(CN) 2 . 100 g. bromoform dissolve 0.005 g. Hg(CN) 2 . 100 g. ethyl bromide dissolve 0.013 g. Hg(CN) 2 100 g. ethylene dibromide dissolve 0.001 g. Hg(CN) 2 . (Sulc, Z. anorg. 1900, 25. 401.) 3.7 4.9 5.7 7.7 9.2 26'(?) 30. 5(?) 35 (?) 38. 5(?) 14.2 18.2 19.7 23.4 77 (?) 83. 5(?) 84 (?) 88. 5(?) (Staronka, 1. c.) Mercuric nickel cyanide ammonia, 2Hg(CN) 2 , 4Ni(CN) 2 , 5NH 3 + 2H 2 O. (Papiermeister, Dissert. 1898.) 5Hg(CN) 2 , 18Ni(CN) 2 , 8NH 3 + 15H 2 O. (Papiermeister, Dissert. 1898.) CYANIDE, MERCURIC ZINC BROMIDE AMMONIA 321 Mercuric potassium cyanide, Hg(CN) 2 , 2KCN. Sol. in 4.4 pts. cold H 2 O; si. sol. in alcohol; decomp. by acids. 100 g. H 2 O dissolve 22.7 g. (Fronmuller, B. 1878, 11. 92.) Abundantly sol. in liquid NH 3 . (Frank- lin, Z. phys. Ch. 1909, 69. 295.) Mercuric silver cyanide, basic, Hg(CN) 2 , HgO, 7AgCN. Ppt. (Bloxam, B. 16. 2669.) Mercuric silver cyanide mercuric sulphate, Hg(CN) 2 , 2AgCN, HgS0 4 +H 2 0. Mercuric sodium cyanide, Hg(CN) 2 , NaCN Sol. in H 2 O. (Grossmann, B. 1904, 37. 4141.) Mercuric strontium cyanide, Hg(CN) 2 Sr(CN) 2 +5H 2 O. Very hygroscopic. Sol. in H 2 O. (Gross- mann, B. 1904, 37. 4142.) Mercuric strontium cyanide iodide, Sr(CN) 2 HgI 2 , Hg(CN) 2 +7H 2 0. (Varet, C. R. 1895, 121. 499.) Mercuric thallium cyanide, Hg(CN) 2 ,2TlCN. Easily sol. in H 2 O. 100 pts. H 2 O dissolve 7.9 pts. at 1, and 10.3 pts. at 10. (Fron- muller, B. 11. 92.) Mercuric zinc cyanide, 4Zn(CN) 2 , Hg(CN) 2 . Insol. in H 2 O. (Dunstan, Chem. Soc. 6. 666.) Mercuric zinc cyanide mercuric bromide ammonia, Hg(CN) 2 , Zn(CN) 2 , HgBr 2 , 4NH 3 . Decomp. by H 2 O. SI. sol. in cold NH 4 OH +Aq. (Varet, C. R. 1889, 109. 810.) Mercuric cyanide ammonia, Hg(CN) 2 , NH 3 . Very sol. in H 2 O, NH 4 OH + Aq, and alcohol. (Varet, C. R. 1889, 109. 903.) SI. sol. in H 2 O. (Schmidt, B. 1894, 27. 232.) 8Hg(CX) 2 , 2NH 3 -f-KH 2 0. Easily de- camp. (Varet, Bull. Soc. (3) 6. 221.) Mercuric cyanide bromide, Hg(CN) 2 , HgBr 2 . Very si. sol. even in boiling H 2 0. (Prussia, Gazz. ch. it. 1898, 28, (2), 114.) Mercuric cyanide barium bromide, 2Hg(CN) 2 BaBr 2 +6H 2 O. Easily sol. especially in hot H 2 O and al- cohol. (Varet, C. R. 1895, 121. 398.) Mercuric cyanide cadmium bromide, Hg(CN) 2 , CdBr 2 +3H 2 O. Sol. in H 2 O and NH 4 OH+Aq. (Varet, Bull. Soc. (3) 5. 8.) 2Hg(CN) 2 , CdBr 2 +4.5 H 2 O. Sol. in H 2 O and in NH 4 OH+Aq. (Varet, C. R. 1890, 111. 680.) Mercuric cyanide cadmium bromide ammonia 2Hg(CN) 2 , CdBr 2 , 4NH 3 +2H 2 O. Decomp. by H 2 O. SI. sol. in NH 4 OH+Aq. (Varet, C. R. 1891, 112. 535.) Mercuric cyanide calcium bromide, 2Hg(CN) 2 , CaBr 2 +5H 2 O. Sol. in 1 pt. cold, and 0.25 pt. boiling H 2 O; also in 2 pts. cold, and 1 pt. boiling 90% alcohol. (Custer.) +7H 2 0. (Varet, C. R. 1895, 121. 399.) Mercuric cyanide cupric bromide ammonia, 2Hg(CN) 2 , CuBr 2 , 4NH 3 . Decomp. by H 2 O; si. sol. in NH 4 OH+Aq. (Varet, Bull. Soc. (3) 6. 221.) Mercuric cyanide lithium bromide, 2Hg(CN) 2 2LiBr+7H 2 0. Deliquescent. (Varet, C. R. 111. 526.) Mercuric cyanide magnesium bromide. See Magnesium mercuric cyanide mercuric bromide. Hg(CN) 2 , 2KBr. Very sol. in H 2 O. (Harth, Z. anorg. 1897, 14. 351.) Mercuric cyanide potassium bromide, Hg(CN) 2 , KBr+2H* 2 O. " Sol. in 13.34 pts. H 2 O at 18, and less than 1 pt. boiling ipts. H 2 O. (Brett.) Sol. without decomp. in hot dil. H 2 SO 4 , HNO 3 , or HCl+Aq. (Brett.) Contains 1^H 2 O. (Berthelot, A. ch. (5) 29. 226.) Mercuric cyanide sodium bromide, Hg(CN) 2 , Sol. in H 2 O and alcohol. Mercuric cyanide strontium bromide, 2Hg(CN) 2 , SrBr 2 +6H 2 O. Sol. in H 2 O and in alcohol. (Varet, C. R. 1895, 121. 399.) Mercuric cyanide zinc bromide, HgBr Hg(CN) 2 , Zn(CN) 2 +8H 2 0. Sol. in H 2 O and NH 4 OH+Aq. (Varet, Bull. Soc. (3) 5. 8.) Mercuric cyanide zinc bromide ammonia, HgBr 2 , Hg(CN) 2 , Zn(CN),, 4NH 3 . As the corresponding chloride. (Varet.)i 322 CYANIDE CHLORIDE, MERCURIC Mercuric cyanide chloride, Hg(CN) 2 , HgCl 2 . Sol. in H 2 O. Decomp. by alcohol, which dissolves out HgCl 2 . Mercuric cyanide ammonium chloride, Hg(CN) 2 , NH 4 C1. Sol. in H 2 O and alcohol. (Poggiale.) Hg(CN) 2> 4NH 4 C1. Mercuric cyanide barium chloride, 2Hg(CN) 2 , BaCl 2 +4H 2 O. Efflorescent. Easily sol. in H 2 O and alcohol +6H 2 O. (Dexter.) Mercuric cyanide barium chloride ammonia, 2Hg(CN) 2 , BaCl 2 , 4NH 3 . Decomp. by H 2 6. SI. sol. in NH 4 OH+Aq. Varet, Bull.^Soo. (3) 6. 221.) Mercuric cyanide cadmium chloride, Hg(CN) 2 , CdCl 2 +2H 2 O. Sol. in H 2 O and NH 4 OH-f Aq. (Varet, Bull. Soc. (3) 6. 8.) Mercuric cyanide calcium chloride, 2Hg(CN) 2 , CaCl 2 +6H 2 0. Efflorescent. Very sol. in H 2 O. (Varet, C. R. 1895, 121. 349.) Mercuric cyanide cerium chloride, 3Hg(CN) 2 , CeCl 3 +8H 2 0. Very sol. in H 2 O. (Ahlen, Bull. Soc. (2) 27. 365.) Mercuric cyanide cobaltous chloride, Hg(CN) 2 , 2CoCl 2 +4H 2 O. Sol. inH 2 O. (Poggiale.) 2Hg(CN) 2 , CoCl 2 +7H 2 O. (Dexter.) Mercuric cyanide cupric chloride, Hg(CN) 2 , CuCl 2 -f-6H 2 0. Efflorescent. Sol. in H 2 O and in NH 4 OH+Aq. (Varet. C. R. 1888, 107. 1002.) 2Hg(CN) 2 , CuCl 2 +6H 2 O. Efflorescent. Very sol. in H 2 O and in NH 4 OH+Aq. (Varet, C. R. 1888, 107. 1002.) Mercuric cyanide cupric chloride ammonia, 2Hg(CN) 2 , CuCl 2 , 4NH 3 . Decomp. by H 2 O. SI. sol. in cold NH 4 OH +Aq. (Varet, Bull. Soc. (3) 6. 221.) Mercuric cyanide didymium chloride, 3Hg(CN) 2 , DiCl 3 +8H 2 O. Very sol. in H 2 O. (Ahlen.) Mercuric cyanide erbium chloride, 3Hg(CN) 2 , ErCl 3 +8H 2 O. Easily sol. in H 2 0. (Ahle"n.) Mercuric cyanide hydrazine chloride, Hg(CN) 2 , N 2 H 4 , HC1. Very sol. in H 2 O. Nearly insol. in alcohol and ether. (Fer- ratini, Gazz. ch. it. 1912, 42. (1), 154.) Mercuric cyanide ferric chloride, 2Hg(CN) 2 , FeCl 3 +3^H 2 0. (Dexter.) Mercuric cyanide lanthanum chloride, 3Hg(CN) 2 , LaCl 3 +8H 2 O. Very sol. in H 2 O. (Ahlen.) Mercuric cyanide magnesium chloride, 2Hg(CN) 2 , MgCl 2 +2H 2 O. Easily sol. in H 2 O and dil. alcohol. (Pog- giale.) Mercuric cyanide manganous chloride, Hg(CN) 2 , MnCl 2 +3H 2 O. Efflorescent. Very sol. in H 2 O. (Poggiale.) Mercuric cyanide nickel chloride, Hg(CN) 2 , NiCl 2 +6H 2 0. Deliquescent. Sol. in H 2 O. (Poggiale.) 2Hg(CN) 2 , NiCl 2 +7H 2 O. (Dexter.) Mercuric cyanide chloride nickel chloride oxychloride, 1 !Hg(CN) 2 , 8HgC] 2 , 2NiCl 2 , 8Ni(OH)Cl+76H 2 O. (Papiermeister, Dissert. 1898.) Mercuric cyanide potassium chloride, Hg(CN) 2 , KC1+H 2 0. Sol. in 6.75 pts. H 2 O at 18. (Brett.) Sol. in alcohol. Mercuric cyanide sodium chloride, Hg(CN) 2 , NaCl. Easily sol. especially in hot H 2 O; insol. in alcohol. (Poggiale.) Mercuric cyanide strontium chloride, 2Hg(CN) 2 , SrCl 2 +6H 2 O. Easily sol. in H 2 O and dil. alcohol. (Varet, C. R. 1895, 121. 349.) Mercuric cyanide yttrium chloride, 3Hg(CN) 2 YC1 3 -|-8H 2 O. Easily sol. in H 2 O. (Ahlen, Bull. Soc. (2) 27. 365.) Mercuric cyanide zinc chloride, 2Hg(CN) 2 , ZnCl 2 +6H 2 0. Efflorescent. Sol. in H 2 O. (Kane.) HgCl 2 , Hg(CN) 2 , Zn(CN) 2 +7H 2 O. Ef- florescent. Very sol. in H 2 O. (Varet. Bull. Soc. (3) 5. 8.) Mercuric cyanide zinc chloride ammonia, HgCl 2 , Hg(CN) 2 , ZnCl 2 , 4NH 3 . Decomp. by H 2 O. Sol. in NH 4 OH-f Aq. (Varet, Bull. Soc. (3) 6. 221.) Hg(CN) 2 , Zn(CN) 2 , HgCl 2 , 6NH 3 . (Varet, C. R. 106. 1080.) CYANIDE ZINC NITRATE, MERCURIC 323 Mercuric cyanide potassium chromate. See Chromate mercuric cyanide, potassium. Mercuric cyanide potassium ferrocyanide, 3Hg(CN) 2 , K 4 Fe(CN) 8 +4H 2 O. Readily sol. in H 2 O. Mercuric cyanide hydrazine, Hg(CN) 2 , N 2 H 4 . Very sol. in H 2 O with partial decomp. (Hofmann and Marburg, A. 1899, 305. 215.) Hg(CN)*, N 2 H 4 . Ppt. (Franzen, Z. anorg. 1911, 70. 154.) Mercuric cyanide potassium hydroxide, Hg(CN) 2 , KOH. (Hofmann and Wagner, B. 1908, 41. 321.) +1HH 2 O. (Hofmann and Wagner, B. 1908, 41. 1630.) 2Hg(CN) 2 , KOH-f-H 2 O. Very sol. in H 2 O. (Hofmann and Wagner, B. 1908, 41. 320.) Mercuric cyanide sodium hydroxide, Hg(CN) 2 .NaOH + l^H 2 O or H 2 O. (Hofmann and Wagner, B. 1908, 41. 1631.) Mercuric cyanide barium iodide, 2Hg(CN) 2 , BaI 2 +4H 2 O. Slowly deliquescent. Sol. in 16.5 pts. cold, and 0.4 pt. boiling H 2 O. Sol. in 22.5 pts. cold, and 1.6 pts. hot 90% alcohol. Solution is decomp. on boiling. (Custer.) Mercuric cyanide cadmium iodide, Hg(CN) 2 , Cd(CN) 2 ,HgI 2 +8H 2 0. See Cadmium mercuric cyanide mercuric iodide. Mercuric cyanide caesium iodide, Hg(CN) 2 , Csl. Recryst. from H 2 O without decomp. Decomp. by acids. (Mathewson and Wells, Am. Ch. J. 1903, 30. 433.) Mercuric cyanide calcium iodide, 2Hg(CN) 2 , CaI 2 +6H 2 O. SI. efflorescent. More sol. in H 2 O than corresponding Sr. comp. (Custer.) Mercuric cyanide lithium iodide, Hg(CN) 2 , 2Li(CN) 2 , HgI 2 +7H 2 O. See Cyanide, lithium mercuric mercuric iodide. Mercuric cyanide magnesium iodide, Hg(CN) 2 , Mg(CN) 2 , HgI 2 +8H 2 O. See Cyanide, magnesium mercuric mercuric iodide. Mercuric cyanide potassium iodide. Hg(CN) 2 KI. Sol. in 16 pts. cold, and less hot H 2 O. Sol in 96 pts. cold alcohol of 34 Baume. (Cail- lot.) SI. sol. in ether. Decomp. by acids. 3Hg(CN) 2 , 2KI-f-3^H 2 O. (Berthelot.) Mercuric cyanide sodium iodide, Hg(CN) 2 , NaI+2H 2 O. Sol. in 4}/ pts. H 2 O at 18, and / 7 pt. Doiling H 2 O. Sol. in 2 pts. boiling, and 6^ pts. cold 90% alcohol. (Custer.) Mercuric cyanide strontium iodide, 2Hg(CN) 2 , SrI 2 +6H 2 O. Sol. in 7 pts. H 2 O at 18, and 1 A pt. at b.-pt. Sol. in 4 pts. 90% alcohol at 18, and Y 2 pt. at b.-pt. (Custer.) Mercuric cyanide zinc iodide, 2Hg(CN) 2 , ZnI 2 +6H 2 O. Efflorescent; sol. in H 2 O. Mercuric cyanide iodide potassium cyanide, HgI 2 , Hg(CN) 2 , 2KCN. Easily decomp. by dil. acids. (Rupp. Apoth. Ztg., 23. 374.) Mercuric cyanide cadmium nitrate, 2Hg(CN) 2 , Cd(NO 3 ) 2 +7H 2 O. Decomp. by H 2 O, not by alcohol. (Ny- lander, J. B. 1859 271.) Mercuric cyanide cobalt nitrate, 2Hg(CN) 2 , Co(NO 3 ) 2 +7H 2 O. Decomp. by H 2 O, not by alcohol. (Ny- lander.) Mercuric cyanide copper nitrate, Hg(CN) 2 , Cu(NO 3 ) 2 +5H 2 O. Decomp. by H 2 O, not by alcohol. (Ny- lander.) Mercuric cyanide ferrous nitrate, 2Hg(CN) 2 , Fe(NO 3 ) 2 +7H 2 O. Decomp. by H^O, net by alcohcl. (Ny- lander.) Mercuric cyanide manganous nitrate, Hg(CN) 3 , Mn(NO 3 ) 2 +5H,O. Decomp. by H 2 O, not by alcohol. (Ny- lander.) 2Hg(CN) 2 , Mn(NO 3 ) 2 +7H 2 O. As above. Mercuric cyanide nickel nitrate, 2Hg(CN) 2 , Ni(NO 3 ) 2 +7H 2 O. Decomp. by H 2 O, not by alcohol. (Ny- lander.) Mercuric cyanide silver nitrate, 2Hg(CN) 2 , AgNO 3 +2H 2 O. SI. sol. in cold, more readily in hot H 2 0. Sol. with decomp. in HNO 8 +Aq. As sol. in alcohol as in H 2 O. Mercuric cyanide zinc nitrate, 2Hg(CN) 2 , Zn(NO 3 ) 2 +7H 2 O. Sol. in H 2 O with decomp. Not decomp. by alcohol. (Nylander, J. B. 1859. 271.) 324 CYANIDE, MERCURIC NITRATE SILVER CYANIDE, BASIC Mercuric cyanide nitrate silver cyanide, basic, Hg(NO 3 )CN, lOAgCN, Hg(OH)NO 3 . (Schmidt, Z. anorg. 1895, 9. 431.) Mercuric cyanide potassium selenocyanide, Hg(CN) 2 , KSeCN. SI. sol. in cold, much more easily sol. in hot H 2 O or alcohol. Traces dissove in ether. (Cameron and Davy, C. N. 44. 63.) Mercuric cyanide nickel sulphate, Hg(CN) 2 , NiSO 4 +9H 2 O. (Papiermeister, Dissert. 1898.) Mercuric cyanide ammonium sulphocyanide, Hg(CN) 2 , NH 4 SCN. Easily sol. in hot H 2 O. (Cleve, Bull. Soc. (2) 23. 71.) Mercuric cyanide barium sulphocyanide, 2Hg(CN) 2 , Ba(SCN) 2 -f-4H 2 O. Permanent. Sol. in hot H 2 O. (Cleve.) Mercuric cyanide cadmium sulphocyanide, 2Hg(CN) 2 , Cd(SCN) 2 +4H 2 0. Permanent. Sol. in hot H 2 O. (Cleve.) Mercuric cyanide calcium sulphocyanide, 2Hg(CN) 2 , Ca(SCN) 2 +8H 2 O. Sol. in H 2 O. (Cleve.) Mercuric cyanide cerium sulphocyanide, 3Hg(CN) 2 , Ce(SCN) 3 + 12H 2 O. Easily sol. in hot H 2 O. (John.) Mercuric cyanide didymium sulphocyanide, 3Hg(CN) 2 , Di(SCN) 3 +6H 2 O. SI. sol. in cold, easily in hot H 2 O. (Cleve.) Mercuric cyanide erbium sulphocyanide, 3Hg(CN) 2 , 2Er(SCN) 3 + 12H 2 O. SI. sol. in cold, easily in hot H 2 O. (Cleve.) Mercuric cyanide lanthanum sulphocyanide, 3Hg(CN) 2 , La(SCN) 3 + 12H 2 O. Very sol. in H 2 O. (Cleve.) Mercuric cyanide magnesium sulphocyanide, 2Hg(CN) 2 , Mg(SCN) 2 +4H 2 0. ' Permanent. Easily sol. in hot H 2 O. (Cleve.) Mercuric cyanide potassium sulphocyanide, . Hg(CN) 2 , KSCN. Permanent. Easily sol. in hot H 2 O. (Cleve.) +2H 2 O. (Philip, Z. Ch. 1867. 552.) Mercuric cyanide rubidium sulphocyanide, Hg(CN) 2 Rb(SCN). Sol. in hot H 2 O without decomp. (Gross- mann, B. 1904, 37. 1259.) Mercuric cyanide samarium sulphocyanide, 3Hg(CN) 2 , Sm(SCN) 2 + 12H 2 O. Easily sol. in H 2 O. (Cleve.) Mercuric cyanide sodium sulphocyanide, Hg(CN) 2 , NaSCN+2H 2 O. Efflorescent. Sol. in H 2 6. (Cleve, Bull. Soc. (2) 23. 71.) Mercuric cyanide strontium sulphocyanide, 2Hg(CN) 2 , Sr(SCN) 2 +4H 2 O. Efflorescent. (Cleve.) Mercuric cyanide yttrium sulphocyanide, 3Hg(CN) 2 , Y(SCN) 3 + 12H 2 O. . SI. sol. in warm, much less in cold H 2 O. (Cleve.) Mercuric cyanide zinc sulphocyanide, 2Hg(CN) 2 , Zn(SCN) 2 +4H 2 O. SI. sol. in H 2 O. (Cleve.) Mercuric cyanide zinc sulphocyanide am- monia, 2Hg(CN) 2 , Zn(SCN) 2 , 3NH 3 . Not efflorescent. Decomp. by H 2 O. Mercuric cyanide potassium thiosulphate, Hg(CN) 2 , K 2 S 2 3 .. Permanent. Sol. in H 2 O. (Kessler.) +H 2 O. (Fock and Klliss, B. 24. 1355.) Molybdenum hydroxyl potassium cyanide, K 3 Mo(OH) 2 (CN) 5 . (Rosenheim and Koss, Z. anorg. 1906, 49. 155.) K 5 Mo(OH) 2 (CN) 8 . Very sol. in H 2 O. (Rosenheim and Koss.) Molybdenum cyanide with MCN. See Molybdocyanide M. Molybdenyl potassium cyanide, MoO 2 (CN) 2 , 2KCN. Very sol. in H 2 O. Aqueous solution is stable in presence of alkalies. Insol. in alcohol. (Pechard, C. R. 1894, 118. 805.) Mo0 2 (CN) 2 , 3KCN. Sol. in H 2 O. Insol. in alcohol. (Hofmann, Z. anorg. 1896, 12. 287.) +H 2 O. Sol. in H 2 O. Insol. in alcohol. (Hofmann.) +4H 2 O. Sol. in H 2 O. Insol. in alcohol. (Hofmann.) Nickel cyanide, Ni(CN) 2 +zH 2 O. Insol. in H^O. 1 ? Insoh in cone. HC1, H 2 SO 4 , or HNOs+Aq, but decomp. by heating there- with. Sol. in NH 4 OH, warm (NH 4 ) 2 SO 4 , or NH 4 succinate+Aq; also in KCN+Aq SI. sol. in NH 4 C1, or NH 4 NO 3 +Aq. (Witt- stein.) Insol. in methyl acetate. (Naumann B 1909, 42. 3790.) CYANIDE, POTASSIUM VANADIUM 325 +3H 2 0, and +5^H 2 O. (Papiermeister, Dissert. 1898.) +4H 2 O. (Hofmann and Hochtlen, B. 1903, 36. 1149.) Nickel potassium cyanide, Ni(CN) 2 , 2KCN +H 2 0. Sol. in H 2 O. Decomp. by acids with residue of insol. Ni(CN) 2 . + 3^H 2 O. (Rammelsberg.) Nickel sodium cyanide, Ni(CN) 2 , 2NaCN + 3H 2 0. Sol. in H 2 0: decomp. by acids with residue of Ni(CN) 2 . Nickel strontium cyanide, Ni(CN) 2 , Sr(CN) 2 +zH 2 O. Sol. in H 2 O. (Handl, J. B. 1859. 273.) Nickel cyanide ammonia, Ni(CN) 2 , NH 3 + Scarcely attacked by H 2 O or dil. acids. Sol. in cone. H 2 SO 4 . Sol. in (NH 4 ) 2 CO 3 + Aq, cone. NH 4 OH+Aq. (NH 4 ) 2 C 2 O 4 +Aq, (NH 4 ) 2 S+Aq, and KCN+Aq. Decomp. by boiling with NaOH or KOH. (Bernoulli and Grether, Ch. Z. 1901, 25. 436.) Nickel cyanide ^nhydrazine, Ni(CN) 2 , (N 2 H 4 ) 3 . Ppt. (Franzen, Z. anorg. 1911, 70. 155.) Osmium cyanide, Os(CN) 2 (?). Insol. in H 2 O; not attacked by acids. See also Osmocyanhydric acid. Osmium potassium cyanide. See Osmocyanide, potassium. Palladous cyanide, Pd(CN) 2 . Insol. in H 2 O. Insol. in dil. acids. Sol. in KCN or NH 4 OH+Aq, also in cone. HCN +Aq. Platinous cyanide, Pt(CN) 2 . Insol. in H 2 O, alkalies, or acids. Sol. in KCN+Aq. When freshly pptd., sol. in NH 4 OH+Aq. Platinous cyanide with MCN. See Platinocyanide, M. Potassium cyanide, KCN. Deliquescent. Very sol. in H 2 Q. 100 pts. KCN+Aq, sat. at b.-pt. 103.3, contain 55 pts. KCN, i. e. 100 pts. H 2 O dis- solve 122.2 pts. KCN at 103.3. (Griffiths.) KCN+Aq containing 3.25% KCN has sp. gr. = 1.0154; 6.5% KCN, 1.0316. (Kohl- rausch, W. Ann. 1879. 1.) KCN+Aq containing 9.64% KCN has sp. gr. 20/20 = 1.0514. KCN+Aq containing 14.42% KCN has sp. gr. 20/20 = 1.0768. (Le Blanc and Roh- land, Z. phy. ch. 1896, 19. 278. Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Almost insol. in absolute alcohol. Sol. in 80 pts. 95% alcohol when boiling, and easily sol. in 35% alcohol. (Geiger, A. 1. 50.) 100 pts. absolute methyl alcohol dissolve 4.91 pts. at 19.5; 100 pts. absolute ethyl alcohol dissolve 0.87 pt. at 19.5. (de Bruyn, Z. phys. Ch. 10. 783.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790) ; ethyl acetate. (Naumann, B. 1904, 37. 3601.) 100 g. glycerol dissolve 32 g. KCN at 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) Sol. in CS 2 when pure. (Loughlin, J. B. 1875. 234.) Wholly insol. in CS 2 . (Moldenhauer, Z. anal. 16. 199.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Potassium chromium Mroxide pentacyanide, K 5 [(Cr0 4 ) 2 (CN) 6 ]+5H 2 0. Very hygroscopic. Sol. in H 2 O. (Riesenfeld, B. 1908, 41. 3548.) Potassium -chromium tetroxide cfo'cyanide ammonia, K 2 [CrO 4 (CN) 2 NH 3 ]+5H 2 O. Hygroscopic in the ah 1 . Easily sol. in H 2 O and in NH 4 OH+Aq. (Riesenfeld, B. 1908, 41. 3545.) Potassium rhodium cyanide. See Rhodocyanide, potassium. Potassium ruthenium cyanide. See Ruthenocyanide, potassium. Potassium silver cyanide, KCN, AgCN. . Sol. in 4.7 pts. H 2 O at 15, 4 pts. at 20, and in much less at higher temp. Sol. in 25 pts. 85% alcohol. (Baup, A. ch. (3) 53. 464.) Potassium silver sodium cyanide, 2KCN, NaCN, 3AgCN. Sol. in 4.4 pts. H 2 O at 15, and 22 pts. 85% alcohol at 17. (Baup.) Potassium tungsten cyanide. See Tungstocyanide, potassium. Potassium uranyl cyanide, (UO,)(CN)t, 2KCN. Ppt. Sol. in H 2 O. SI. sol. in presence of large excess of KCN. (Aloy, A. ch. 1901, (7) 24. 417.) Potassium vanadium cyanide, K 3 V(CN) fi . Readily sol. in H 2 O; decomp. slowly in neu- tral aq. solution, rapidly in acid aq. solution; 326 CYANIDE, POTASSIUM ZINC insol. in alcohol. (Locke, Am. Ch. J. 1898, 20. 601.) K 4 V(CN) 3 +3H 2 O. Sol. in H 2 O. Insol. in alcohol and ether. (Petersen, Z. anorg. 1904, 38. 345.) Potassium zinc cyanide, 2KCN, Zn(CN) 2 . 100 pts. H 2 O dissolve 11 pts. at 20. (Sharwood, Eng. Min. J. 1904, 77. 845.) Potassium cyanide molybdenum dioxide, 4KCN, MoO 2 +5H 2 O. Sol. in H 2 O. Insol. in alcohol. (Hof- mann, Z. anorg. 1896, 12. 287.) +6H 2 O. " Potassium dioxotetracyan- omolybdate." Very sol. in H 2 O. (Winkler, Dissert. 1909.) +8H 2 O. (Rosenheim, Kohn and Gar- funkel, Z. anorg. 1910, 65. 174.) + 10H 2 O. Decomp. by cone. HC1, HNO 3 and H 2 S0 4 . Not acted upon by cold dil. acids, (v. der Heide and Hofmann, Z. anorg. 1896, 12. 285.) 5KCN, MoO 2 +8H 2 O. Sol. in H 2 O. Insol. in alcohol. (Kalischer, Dissert. 1902.) Potassium cyanide molybdenum cfaoxide hydroxylamine, 4KCN, MoO 2 , NH 2 OH +H 2 0. Sol. in H 2 O. Decomp. by dil. acids, (v. der Heide and Hofmann, Z. anorg. 1896, 12. 282.) Potassium cyanide molybdenum sulphide, 6KCN, Mo 2 S 3 +5H 2 O. Easily sol. in H 2 O. Decomp. by dil. aeids. (Hofmann, Z. anorg. 1896, 12. 289.) Very sol. in H 2 O. Slowly decomp. in the cold bv dil. mineral acids, (v. der Heide and Hofmann, Z. anorg. 1896, 12. 289.) Potassium cyanide molybdenum sulpho- cyanide, 2KCN, MoS 2 (CN) 2 . (Pechard, C. R. 1894, 118, 806.) 5KCN, Mo 3 S 4 (CN) 3 +7H 2 0. Sol. in H 2 O. Stable toward dil. acids and alkalies. (Hof- mann, Z. anorg. 1896, 12. 289.) Potassium cyanide molybdenum sulphoxy- cyanide, 4KCN, Mo 2 SO(CN) 2 +4H 2 O. Sol. in H 2 O. Stable toward dil. acids. (Hofmann, Z. anorg. 1896, 12. 289.) Potassium cyanide nitrite, KCN, KNO 2 Sol. in H 2 O; decomp. slowly by H 2 O / explosive. (Hofmann, Z. anorg. 1895, 10. 260- 261.) Potassium cyanide sulphur dioxide, KCN S0 2 +H 2 0. Much more sol. in hot than cold H 2 O (fitard, C. R. 88. 649.) KCN, HCN, 2SO 2 +3H 2 O. Very si. sol. in cold H 2 O; decomp. by hot H 2 O. (Etard.) Rubidium tungsten cyanide. See Tungstocyanide, rubidium. Rhodium cyanide, Rh(CN) 3 . Ppt. Not decomp. by acids. Sol. in KCN+Aq. .(Martius, A. 117. 361.) Rhodium cyanide with 3KCN. See Rhodicyanide, potassium. Ruthenium cyanide with 4MCN. See Ruthenocyanide, M. Silver cyanide, AgCN. $1. sol. in H 2 O. 2.2 + 10- 4 g. sol. in 1 liter of H 2 O at 19.96. (Bottger, Z. phys. ch. 1903, 46. 603.) 1 1. solution "in H 2 O contains 0.000043 g. AgCN at 17.5. (Ab.egg and Cox, Z. phys. Ch. 1903,46. 11.) Solubility in H 2 O at 25=2.22 + KH mol. per 1. (Lucas, Z. anorg. 1904, 41. 198.) Insol. in dil. acids. Decomp. by cone, acids. Not sol. to any extent in HCN+ Aq. Freshly pptd. AgCN is not dissolved by cold dil. HNO 3 , but is attacked by very dil. HNO 3 on boiling. From dry AgCN is dis- solved 5% by boiling 1 hour with 1% HNO 3 +Aq. Cone. HNO 3 dissolves more. (Brunck, B. 1901, 34. 1605.) Sol. in NH 4 OH+Aq. Sol. in boiling KC1, NaCl, CaCl 2 , BaCl 2 , or MgCl 2 +Aq, but very slowly sol. therein at ord. temp. Sol. in Na 2 S 2 3 ,K 4 Fe(CN) 6 , (NH 4 ) 2 CO 3 , (NH 4 ) 2 SO 4 , NH 4 NO 3 , and NH 4 succinate-f Aq, and in large amt. of hot NH 4 Cl+Aq. (Wittstein.) Sol. in KCN, NaCN, Ba(CN) 2 , Ca(CN) 2 , or Sr(CN) 2 +Aq. Insol. in KOH, or NaOH +Aq. Sol. in cone, boiling AgNO 3 +Aq. (Wohler.) Sol. in 431.7 pts. 5% NH 4 OH+Aq (sp. gr. 0.998) at 12; in 184.5 pts. 10% NH 4 OH+ Aq (sp. gr. 0.96) at 18. (Longi, Gazz, ch. it. 13. 87.) SI. sol. in Na citrate +Aq. Sol. in Hg(NO 3 ) 2 +Aq. 1 1. of a 3-N solution of AgN0 3 dissolves 1.216 g. AgCN at 25. (Hellwig, Z. anorg. 1900, 26. 177.) Very sol. in (NH 4 ) 2 S 2 O 3 +Aq. (Rosen- heim and Steinhauser, Z. anorg. 1900, 25. 105.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) SI. sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Abundantly sol. in quinoline at 60. (Varet, C. R. 1893, 116. 60.) SI. sol. in ethyl amine. (Shinn, J. phys. Chem. 1907, 11. 538.) Insol. in methyl acetate. (Bezold, Dissert. 1906; Naumann, B. 1909, 42. 3790); ethyl CYANOGEN 327 acetate. (Hamers, Dissert. 1906; Naumann B. 1910, 43. 314.) Silver hydrogen cyanide, AgCN, HCN. (Euler, B. 1903, 36. 1859.) Silver sodium cyanide, AgCN, NaCN. Sol. in 5 pts. H 2 O at 20 and in much less hot H 2 O. Sol. in 24 pts. 85% alcohol at 20. (Baup, A. ch. (3) 63. -468.) Silver thallous cyanide, AgCN, T1CN. Easily sol. in H 2 0. 100 pts. H 2 O dissolve 4.7 pts. at 0, and 7.4 pts. at 16. (Fron- muller, B. 11. 92.) Silver tungsten cyanide. See Tungstocyanide, silver. Silver cyanide ammonia, AgCN, NH 3 . Efflorescent. Decomp. on air. Very sol. in ammonia at -10. (Joannis, C. R. 1894, 118. 1151.) Silver cyanide hydrazine, AgCN, N 2 H 4 . Decomp. in the air. Decomp. by H 2 O. (Franzen, Z. anorg. 1911, 70. 153.) Silver cyanide nitrate, 2AgCN, AgNO 3 . Decomp. by H 2 0. Sodium cyanide, NaCN. Sol. in H 2 and 75% alcohol. + >iH 2 O, and 2H 2 0. Very sol. in H 2 O; si. sol. in alcohol. (Joannis, A. ch. (5) 26. 484.) Sodium tungsten cyanide. See Tungstocyanide, sodium. Sodium zinc cyanide, NaCN, Zn(CN) 2 + Much more sol. in H 2 O than the correspond- ing K Zn salt. (Rammelsberg.) +8H 2 O. (Loebe, Dissert. 1902.) Sodium cyanide molybdenum dioxide, 4NaCN, MoO 2 +6H 2 O. (Winkler, Dissert. 1909.) +14H 2 O. Sol. in H 2 O. (Rosenheim, Garfunkel and Kohn, Z. anorg. 1910, 65. 174.) Sodium cyanide molybdenum dioxide hy- droxylamine, 4NaCN, MoO 2 , NH 2 OH +H 2 0. As K comp. (Winkler, Dissert. 1909.) Strontium cyanide, Sr(CN) 2 +4H 2 O. Very unstable; very deliquescent, and sol. in H 2 O. (Joannis, A. ch. (5) 26. 496.) Strontium tungsten cyanide. See Tungstocyanide, strontium. Strontium zinc cyanide, 2Sr(CN) 2 , 3Zn(CN) 2 +H 2 O. Sol. in H 2 O and alcohol. (Loebe, Dissert. 1902.) Thallous cyanide, T1CN. 100 pts. H 2 O dissolve 16.8 pts. at 28.5. (Fronmuller, B. 6. 1178.) Thallothallic cyanide, T1 2 (CN) 4 = T1CN, T1(CN) 3 . Easily sol. in H 2 O. 100 pts. H 2 O dissolve 27.3 pts. at 30, 15.3 pts. at 12, 9.7 pts. at 0. (Fronmuller, B. 11. 92.) Thallous tungsten cyanide. See Tungstocyanide, thallous. Thallous zinc cyanide, 2T1CN, Zn(CN) 2 . Easily sol. in H 2 O. 100 pts. H 2 dissolve 8.7 pts. at 0; 15.2 pts. at 14; and 29.6 pts. at 31. (Fronmuller, B. 11. 92.) Tungsten cyanide with MCN. See Tungstocyanide, M. Zinc cyanide, Zn(CN) 2 . Insol. in H 2 O and alcohol. Sol. in alkalies. Easily sol. in KCN+Aq. Sol. in hot NH 4 salts +Aq. (Wittstein.) Easily sol. in (NH 4 ) 2 CO 3 +Aq. (Gore.) Sol. in KOH+Aq. Solution is stable when less than 1 mol. Zn(CN) 2 to 2 mols. KOH is present. When proportion is 1:1, ZnO 2 H 2 soon separates. Sol. in dil. KCN+Aq. (Sharwood, J. Am. Chem. Soc. 1903, 26. 587.) SI. sol. in cone. Zn salts +Aq. 1 1. cone. Zn(C 2 H 3 O 2 ) 2 +Aq dissolves 4 g., and 1 1. cone. ZnSO 4 +Aq dissolves 2 g. Zn(CN) 2 . Insol. in HCN-f Aq. Easily sol. in dil. acids. (Joannis.) Very sol. in liquid NH 3 . (Franklin, Am. h. J. 1898, 20. 830.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Zinc cyanide ammonia, Zn(CN) 2 , 2NH 3 . Decomp. on air. (Varet, C. R. 105. 1070.) +H 2 O. Decomp. on air. Decomp. by H 2 O. Sol. in NH 4 OH+Aq. (Varet.) Zinc cyanide cfo'hydrazine, Zn(CN) 2 , 2N 2 H 4 . Decomp. by H 2 O. (Franzen, Z. anorg 1911, 70. 153.) Cyanogen, CN. H 2 O absorbs 4*/ vols. CN gas at 20. Alco- 10! absorbs 23 vols., and ether 5 vols. at the same temperature. (Gay-Lussac.) The solution gradually decomposes, but this is prevented by traces of acids. 328 CYCLOTRIBORENE 0.221 mol. litre are dissolved in H 2 O at 0. (Naumann, Z. Electrochem. 1910, 16. 177.) Oil of turpentine absorbs 5 vols. (Gay- Lussac.) Absorbed by many essential oils. Very sol. in CuCl 2 -f Aq. Absorbed with decomp. by NH 4 OH+Aq and other alkaline liquids. k Absorbed by aniline. (Jacquemain, C. R. 100. 1006.) Cyclotriborene, B 3 H 3 . Insol. in H 2 O. (Ramsay and Hatfield, Proc. Chem. Soc. 1901, 17. 152.) Decamine cob al tic sulphite, Co 2 (NH 3 ) 10 (S0 3 ) 3 +3H 2 0. Sol. in H 2 O. (Vortmann and Magdeburg, B. 22. 2636.) Decamine cobaltisulphurous acid. Cobaltic decamine cobaltisulphite, Co 2 (NH 3 ) 10 (S0 3 ) 6 Co 2 +8H 2 0. Ppt. (Vortmann and Magdeburg, B. 22. 2635.) Sodium decamine cohaltisulphite, Co 2 (NH 3 ) 10 (S0 3 Na) 6 -}-2H 2 0. Sol. in H 2 O. (Vortmann and Magdeburg, B. 22. 2635.) Diamide, N 2 H 4 . See Hydrazine. Diamine chromium sulphocyanhydric acid, Cr(NH 3 ) 12 (SCN) 3 , HSCN+H 2 O. Sol. in H 2 O. (Nordenskiold, Z. anorg. 1. 130.) Diamine chromium cfo'aquo sulphocyanide. Cr(NH 3 ) 2 (SCN) 3 +2H 2 0. Sol. in H 2 O, from which it is pptd. by con. HCl+Aq. (Nordenskiold, Z. anorg. 1. 137.) Ammonium diamine chromium sulphocy- anide, Cr(NH 3 ) 2 (SCN) 3 , NH 4 SCN. (Reinecke' s salt.) Quite easily sol. in H 2 O, less in alcohol, and insol. in benzene. Slowly decomp. by boiling H 2 O or dil. acids. (Nor- denskiold, Z. anorg. 1. 130.) . +H 2 O. Insol. in absolute ether. (Christen- sen, J. pr. (2) 45. 218.) Ammonium diamine chromium sulphocyanide iodide, Cr(NH 3 ) 2 (SCN) 3 , NH 4 SCN, I. Barium , [Cr(NH 3 ) 2 (SCN) 3 ] 2 , Ba(SCN) 2 . Sol. in H 2 O and alcohol. (N.) Cadmium diamine chromium sulphocyanide, Cd(SCN) 2 , [Cr(NH 3 ) 2 (SCN) 3 ] 2 +H 2 O. Nearly insol. in cold, si. sol. in hot H 2 O. SI. sol. in boiling alcohol. (Christensen, J. pr. (2) 45. 371.) Cupric [Cr(NH 3 ) 2 (SCN)< Cu(SCN) 2 , Insol. in H 2 O or dil. acids. (Reinecke, A. 126. 116.) Ferric Fe(SCN) 3 . (N.) Luteocobaltic , Co(NH 3 ) 6 (SCN) 3 [Cr(NH 3 ) 2 (SCN) 3 ] 3 . As good as insol. in cold H 2 O. SI. sol. in hot H 2 O and alcohol. (Christensen, J. pr. (2) 45. 370.) Mercuric , [Cr(NH 3 ) 2 (SCN) 3 ] 2 , Hg(SCN) 2 . Insol. in H 2 O. (N.) Insol. in H 2 O and dil. acids. (Reinecke.) Potassium = , Cr(NH 3 ) 2 (SCN) 3 , KSCN. Properties as the NH 4 salt. (N.) Cr(NH 3 ) 2 (SCN) 3 , KSCN, I. As the NH 4 salt. (N.) Sodium , NaSCN, Cr(NH 3 ) 2 (SCN) 3 . Sol. in H 2 O, alcohol, and ether. (Reinecke.) Diamine cobaltic nitrite ammonium nitrite, CO(NH 3 ) 2 (NO 2 ) 3 , NH 4 N0 2 . Sol. inH 2 O. (Erdmann.) nitrite lead nitrite, 2Co(NH 3 ) 2 (NO 2 ) 3 , Pb(NO 2 ) 2 . Sol. in hot H 2 O with partial decomp. nitrite mercurous nitrite, 2Co(NH 3 ) 2 (N0 2 ) 3 , Hg 2 (N0 2 ) 2 . Ppt. Not sol. in hot H 2 O without decomp. nitrite potassium nitrite, Co(NH 3 ) 2 (NO 2 ) 3 , KNO 2 . Sol. in H 2 O. (Erdmann, J. pr. 97. 385.) nitrite silver nitrite, Co(NH 3 ) 2 (N0 2 ) 3 , AgN0 2 . Ppt. Crystallises out of hot H 2 O. (Erd- mann.) nitrite thallium nitrite, Co(NH 3 ) 2 (NO 2 ) 3 , T1NO 2 . Crystallises out of hot H 2 O without de- comp. DIDYMIUM OXIDE 329 Dichrocobaltic carbonate, Co(NH 3 ) 3 (OH)C0 3 + l^H 2 0. Sol. in H 2 O. (Vortmann, B. 15. 1901.) Dichrocobaltic chloride, Co(NH 3 ) 3 Cl 3 +H 2 O. Quite sol. in cold H 2 O, dil. acids, cone. H 2 SO 4 ,or dil. alcohol. From solution in cone. H 2 SO 4 , the salt is precipitated by much HCl+Aq. Composi- tion is Co(NH 3 ) 3 (OH 2 )Cl 3 . (Jorgensen, Z. anorg. 5. 189.) nitrate, Co(NH 3 ) 3 (NO 3 ) 3 +4H 2 O. Deliquescent. Sol. in H 2 0. More sol. in dil. HNO 3 +Aq than praseocobaltic nitrate. (Vortmann, B. 15. 1897.) Anhydrous. Insol. in H 2 O as such, but converted into above salt thereby. (Jorgen- sen, Z. anorg. 5. 186.) nitrite, Co(NH 3 ) 3 (NO 2 ) 3 . Difficultly sol. in cold, but rather easily sol. in hot H 2 O. sulphate, [Co(NH 3 ) 3 l 2 (SO 4 ) 3 +6H 2 O. Easily sol. in H 2 O. (Vortmann, B. 15. 1900.) sulphite, [Co(NH 3 ) 3 ] 2 (SO 3 ) 3 +H 2 O. Nearly insol. in cold, slowly decomp. by hot H 2 O. Decomp. by acids or KOH+Aq. Insol. in cold, sol. in warm NH 4 OH+Aq. (Kunzel, J. pr. (1) 72. 209.) According to Geuther (A. 128. 157), is a double salt [Co(NH 3 ) 3 ] 2 (S0 3 ) 3 , Co 2 (S0 3 ) 3 +2H 2 0. Didymium, Di. Slowly decomp. by H 2 O. Insol. in cold cone. H 2 SO 4 . Sol. in dil. acids. Compound of two elements, neodymium and praseodymium, (v. Welsbach. W. A. B. 92. 317.) Didymium bromide, DiBr 3 +6H 2 O. Very deliquescent, and sol. in H 2 O. (Cleve.) Didymium nickel bromide, 2DiBr 3 , 3NiBr 2 + 18H 2 O. Deliquescent. Very sol. in H 2 O. (Frerichs and Smith, A. 191. 342.) Didymium zinc bromide, DiBr 3 . 3ZnBr 2 + 12H 2 O. Extremely deliquescent. (Cleve, Bull. Soc. (3) 43. 361.) 2DiBr 3 , 3ZnBr 2 +36H 2 O. (F. and S.) Didymium chloride, DiCl 3 . Anhydrous. Deliquescent. Sol. in H 2 O and alcohol. (Marignac.) +6H 2 O. Deliquescent. Easily sol. in H 2 O and alcohol. (Marignac.) Didymium mercuric chloride, 2DiCl 3 , 9HgCl 2 +24H 2 0. More sol. in H 2 O than the corresponding La salt. (Marignac.) DiCl 3 , 4HgCl 2 +HH 2 O. Not deliquescent. Easily sol. in H 2 O. Didymium stannic chloride. See Chlorostannate, didymium. Didymium fluoride, Precipitate. (Cleve.) Didymium hydrogen fluoride, 2DiF 3 , 3HF. Precipitate. (Smith.) Does not exist. (Cleve.) Didymium potassium fluoride, DiF 3 , KF + H 2 O. Sol. in H 2 O. (Brauner, B. 15. 114.) +V 3 H 2 O. As above. (B.) 2DiF 3 , 3KF+H 2 O. As above. (B.) Didymium hydroxide, Di 2 O 6 H 6 . Insol. in KOH, or NaOH+Aq, but is si. sol. in NH 4 Cl+Aq. (Rose.) See also Di 2 O 3 . Didymium pent hydroxide, DiO 4 H 3 = Di 2 5 , 3H 2 O. Precipitate. (Brauner, B. 15. 113.) Didymium zinc iodide, 2DiI 3 , 3ZnI 2 +24H 2 O. Very deliquescent. (Frerichs and Smith.) Didymium oxide, Di 2 O 3 . With H 2 O slowly forms Di 2 O 6 H 6 . Sol. in cone., or dil. mineral acids (Marig- nac), and in acetic acid (Hermann). Sol. in ammonium salts +Aq. Slightly more slowly sol. in cone. NH 4 NO 3 +Aq than La 2 O 3 . (Damour and Deville.) A solution of NH 4 NO 3 in H 2 O that can dissolve 2.9 mols. La 2 O 3 dissolves 1 mol. Di 2 O 3 . (Brauner, B. 15. 114.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Didymium peroxide, Di 4 9 . Sol. in acids with decomp. (Frerichs, B. 7. 799.) Not obtained by Cleve. (B. 11. 910.) The contradictory statements concerning the composition of Di peroxide are owing to the fact that praseodidymium is the only one of the constituents of Di which easily forms a peroxide, (v. Welsbach.) Didymium peroxide, Di 2 6 . Sol. in dil. HNO 3 , or H 2 SO 4 +Aq in the cold without evolution of gas, but gas is evolved if treated with cone, acids. Insol. in HF+Aq. SI. sol. in cold NH 4 NO 3 +Aq. = Di 4 O 9 . (Cleve.) 330 DIDYMIUM OXYBROMIDE Didymium oxybromide, DiOBr. (Frerichs and Smith.) Didymium oxychloride, DiOCl. Anhydrous. Insol. in H 2 O. (Smith.) +3H 2 O. Sol. in cold dil. HNO 3 +Aq. (Marignac.) SI. sol. in HCl+Aq. (Her- mann.) Didymium oxysulphide, Di 2 O 2 S. Insol. in H 2 O. Sol. in HCl+Aq without residue. (Marignac.) Didymium sulphide, Di 2 S 3 . Insol. in H 2 O. Decomp. by dil. acids. (Marignac, A. ch. (3) 38. 159.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Disulphuric acid, H 2 S 2 O 7 . See Disulphuric acid. Dithionic acid (Hyposulphuric acid), H 2 S 2 O 6 . Known only in aqueous solution, which is stable only when dil. Can be evaporated in vacuo until sp. gr. = 1.347, but decomp. upon further evaporation. (Welter and Gay- Lussac, A. ch. 10. 312.) Dithionates. All dithionates are sol. in H 2 O. Aluminum dithionate, A1 2 (S 2 O 6 ) 3 +18H 2 O. Extremely deliquescent. Easily sol. in H 2 or absolute alcohol. (Kliiss, A. 246. 218.) Aluminum ammonium dithionate. A1 2 (S 2 6 ) 3 , (NH 4 ) 2 S 2 6 +27H 2 0. SI. deliquescent. Sol. in H 2 O. (Kliiss, A. 246. 303.) Ammonium dithionate, (NH 4 ) 2 S 2 O 6 . Very sol. in H 2 O. Sol. in 0.79 pt. H 2 O at 16, with reduction of temp.- Not decomp. on boiling. Insol. in absolute alcohol. (Heeren, Pogg. 7. 172.) Contains }/H 2 0. Sol. in 0.56 pt. H 2 O at 19. (Kliiss, A. 246. 194.) Ammonium cadmium dithionate, 2(NH 4 ) 2 S 2 O 6 , CdS 2 O 6 +4^H 2 O. Sol. in H 2 O. (Kliiss, A. 246. 298.) Ammonium cobalt dithionate, 9(NH 4 ) 2 S 2 O fi , 2CoS 2 6 + 16^H 2 0. Sol. in H 2 O. (Kliiss.) Ammonium cupric dithionate, (NH 4 ) 2 S 2 O 6 , 2CuS 2 O 6 +8H 2 O. Sol. in H 2 O. Ammonium ferrous dithionate, 3(NH 4 ) 2 S 2 O 6 , Fe 2 S 2 O 6 +6H 2 O. Sol. iii H 2 0. (Kliiss, A. 246. 300.) 9(NH 4 ) 2 S 2 O 6 , 2Fe 2 S 2 O 6 + 16^H 2 0. Sol. in H 2 0. (Kliiss.) Ammonium manganous dithionate, 9(NH 4 ) 2 S 2 O 6 , 2MnS 2 O 6 . Sol. in H 2 O. (Kliiss, A. 246. 301.) Ammonium nickel dithionate, 9(NH 4 ) 2 S 2 O 6 , 2NiS 2 O 6 + 16^H 2 O. Sol.inH 2 O. (Kliiss.) Ammonium zinc dithionate, 5(NH 4 ) 2 S 2 6 , ZnS 2 O 6 +9H 2 O. Easily sol. in H 2 O. (Kliiss, A. 246. 296.) 9(NH 4 ) 2 S 2 O C , 2ZnS 2 O 6 +16MH 2 O. Easily sol. in H 2 O. (Kliiss.) Ammonium dithionate chloride, (NH 4 ) 2 S 2 O 6 , NH 4 C1. Sol. in H 2 O. (Fock and Kliiss, B. 24. 3017.) Barium dithionate, BaS 2 O 6 +2H 2 O. Not efflorescent. Sol. in 7.17 pts. H 2 O at 8, 4.04 pts. at 18, and 1.1 pts. H 2 O at 100. Insol. in alcohol. (Gay-Lussac, Heeren.) Sol. in 0.994 pt. H 2 O at 102, the boiling- point of the sat. solution. (Baker, Bull. Soc. (2) 44. 166.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +4H 2 O. Very efflorescent. (Heeren.) Barium magnesium dithionate, BaMg(S 2 O 6 )2 +4H 2 O. Sol. in H 2 O. (Schiff, A. 118. 97.) Barium rubidium dithionate, BaRb 4 (S 2 O 6 )3 +H 2 0. Sol. in H 2 O. Solubility is diminished by presence of excess of Rb 2 SO 4 , but increased by BaS 2 O 6 . (Bodlander, Chem. Ztg. 14. 1140.) Barium sodium dithionate, BaNa 4 (S 2 O 6 )3 + 4H 2 O. Sol. in H 2 O . Decomp. by recrystallisation. (Kraut, A. 118. 95.) +6H 2 O. (Schiff.) Barium dithionate chloride, BaS 2 O 6 , BaCl 2 + 4H 2 O. (Fock and Kliiss, B. 23. 3001.) Bismuth dithionate, basic, Bi 2 O 3 , S 2 O 5 + +5H 2 O. Efflorescent. Insol. in H 2 O, but decomp. thereby into the following salt. Easily sol. in dil. acids, especially HCl+Aq. (Kluss, A. 246. 183.) 4Bi 2 O 3 , 3S 2 O 6 +5H 2 O. Insol. in H 2 O. Sol. in dil. acids. (Kliiss.) DITHIONATE, MANGANOUS 331 Cadmium dithionate. Deliquescent in moist air; very sol. in H 2 O. (Heeren, Pogg. 7. 183.) Cadmium dithionate ammonia, CdS 2 O e , Decomp. by alcohol; sol. in NH 4 OH+Aq, but decomp. on heating. (Rammelsberg, Pogg. 68. 298.) Caesium dithionate, Cs 2 S 2 O 6 . Easily sol. in H 2 O. (Chabrie, C. R. 1901, 133. 297.) Calcium dithionate, CaS 2 O e +4H 2 O. Sol. in 2.46 pts. H 2 O at 19; 0.8 pt. at 100. Insol. in alcohol. (Heeren, Pogg. 7. 178.) Insol. in acetone. (Naumann. B. 1904. 37. 4329.) Cerous dithionate, Ce 2 (S 2 O 6 ) 3 +24H 2 O. Very sol. in H 2 O. (Jolin.) +3, and5H 2 O. (Wyrouboff.) Chromic dithionate, Cr 2 (S 2 O 6 ) 3 +18H 2 O. Sol. in H 2 O and alcohol. (Kltiss, A. 246. 189.) 3O 2 O 3 , 4S 2 6 +24H 2 O. Easily sol. in H 2 O or alcohol. Insol. in ether. (Kliiss.) Cobaltous dithionate, CoS 2 O 6 +6H 2 O. Not deliquescent. Very sol. in H 2 O. (Heeren.) +8H 2 O. Sol. in 0.49 pt. H 2 O at 19. Sol. in absolute alcohol. (Kliiss, A. 246. 203.) Cupric dithionate basic, 4CuO, S 2 O 6 +4H 2 O. Very sl^ sol. in H 2 O. (Heeren, Pogg. 7. 18.) Insol. in H 2 O; easily sol. in dil. acids. (Kliiss, A. 246. 208.) +3H 2 O. Insol. in H 2 and NaC 2 H 3 O 2 + Aq; sol. in traces in cone. CuS 2 O f +Aq. Easily sol. in dil. acids, even HC 2 H 3 O 2 , or H 2 S 2 O 6 +Aq. (Kliiss.) Cupric dithionate, CuS 2 O 6 +4H 2 O. Not efflorescent. Very sol. in H 2 O. Insol. in alcohol. (Heeren.) H-5H 2 O. (Efflorescent. Sol. in 0.64 pt. H 2 Oatl8.5. (Kliiss, A. 246. 204.) Cupric dithionate ammonia, CuS 2 O 6 , 4NH 3 . Difficultly sol. in cold H 2 O, moderately sol. in H 2 O at 40. Decomp. by much H 2 O or by heating the solution above 60. Decomp. by HCl+Aq. (Heeren.) Can be recryst. from NH 4 OH+Aq. Sol. in liquid NH 3 . (Horn, Am. Ch. J. 1908, 39. 213.) CuS 2 O 6 , 9NH 3 . Decomp. at ord. temp, in the air. Insol. in liquid NH 3 . (Horn, Am. Ch. J. 1908, 39. 213.) Didymium dithionate, Di 2 (S 2 O 6 ) 3 +24H 2 O. Extremely sol. in H 2 O. (Cleve.) Erbium dithionate, Er 2 (S 2 O 6 ) 3 + 18H 2 O. Very sol. in H 2 O or alcohol; insol. in ether. (Hoglund.) Glucinum dithonate, basic, 5G1O, 2S 2 O 6 + 14H 2 0. Easily sol. in H 2 O and absolute alcohol. (Kliiss, A. 246. 196.) Iron (ferrous) dithionate, FeS 2 O 6 +5H 2 0. Very sol. in H 2 O. Insol. in alcohol. De- comp. in aqueous solution into FeSO 4 by boiling. (Heeren, Pogg. 7. 181.) +7H 2 O. Sol. in 0.59 pt. H 2 O at 18.5. (Kliiss, A. 246. 198.) Iron (ferric) dithionate, basic, 8Fe 2 O 3 , S 2 O 6 + 20H 2 O. Insol. in H 2 or alcohol. Very si. sol. in H 2 S 2 O 6 +Aq; easily sol. in HCl+Aq. (Heeren.) Contains 14H 2 O. (Kliiss, A. 246. 200.) 3Fe 2 O 3 , S 2 8 +8H 2 O. Insol. in H 2 O. Easily sol. in acids. (Kliiss, A. 246. 201.) Lanthanum dithionate, La 2 (S 2 O 6 ) 8 +16H 2 O, and 24H 2 O. Sol. in H 2 O. (Cleve.) Lead dithionate, basic, 2PbO, S 2 O 6 +2H 2 O. Very difficultly sol. in H 2 0. (Heeren, Pogg. 7. 171.) lOPbO, S 2 O 6 +2H 2 O. SI. sol. in H 2 O. (Heeren.) Lead dithionate, PbS 2 O 6 +4H 2 O. Easily sol. in H 2 O. (Heern.) Sol. in 0.869 pt. H 2 O at 20.5. (Baker, C. N. 36. 203.) Lead strontium dithionate, (Pb,Sr)S 2 O 6 + 4H 2 0. (Rammelsberg.) Lithium dithionate, Li 2 S 2 O 6 +2H 2 O. SI. deliquescent, and easily sol. Insol. in alcohol. (Rammelsberg.) Magnesium dithionate, MgS 2 O 6 +6H 2 0. Sol. in 0.85 pt. H 2 O at 13. Solution can be boiled without decomp. (Heeren, Pogg. 7. 179.) Sol. in 0.692 pt. H 2 O at 17. (Baker, C. N. 36. 203.) Manganous dithionate, MnS 2 O 6 +3H 2 O. Sol. in H 2 O. (Kraut, A. 118. 98.) +6H 2 O. Efflorescent. Sol.inH 2 O. (Mar- gnac, J. B. 1855. 380.) 332 DITHIONATE, MERCUROUS Mercurous dithionate, Hg 2 S 2 O 6 . SI. sol. in cold, decomp. by hot H 2 0. (Rammelsberg.) Mercuric dithionate, basic, 5HgO, 2S 2 O 5 . SI. sol. in cold, decomp. by hot H 2 O. Easily sol. in HNO 3 +Aq. (Rammelsberg, Pogg. 59. 472.) Mercuric dithionate, HgS 2 O 6 +6H 2 O. Decomp. by H 2 O or on standing. (Kluss, A. 246. 216.) Nickel dithionate, NiS 2 O 6 +6H 2 O. Sol. inH 2 O. (Topsoe.) Sol. in 0.897 pt. H 2 O at 12. (Baker, C. N. 36. 203.) Nickel dithionate ammonia, NiS 2 O 6 , 6NH 3 . Can be recryst. from warm NH 4 OH+Aq. Decomp. by H 2 Q. (Rammelsberg, Pogg. 58. 295.) Nickel dithionate hydrazine, NiS 2 , 3N 2 H 4 . Unstable. Sol. in NH 4 OH+Aq. (Franzen, Z. anorg. 1908, 60. 267.) Potassium dithionate, K 2 S 2 O 6 . Not deliquescent. Sol. in 16.5 pts. H 2 O at 16, and 1.58 pts. at 100. Insol. in alcohol. (Heeren.) Sol. in 2.65 pts. H 2 O at 16. (Dumas.) Sol. in 16.5 pts. H 2 O at 16; in 1.58 pts. boiling H 2 O. Insol. in alcohol. (Heeren, Pogg. 1826, 7. 72.) Praseodymium dithionate, Pr 2 (S 2 Oc) 3 + 12H 2 O. Deliquescent; very sol. in H 2 O. (von Schule, Z. anorg. 1898, 18. 361.) Rubidium dithionate, Rb 2 S 2 O 6 . Sol. in H 2 0. (Topsoe and Christiansen:) Ruthenium dithionate, RuS 2 O 6 . Ppt. from aq. sol. by alcohol. (Antony, Gazz. ch. it. 1898, 28. 139-142.) Silver dithionate, Ag 2 S 2 O 6 +2H 2 O. Sol. in 2 pts. H 2 O at 16. Sol. in NH 4 OH + Aq. (Heeren, Pogg. 7. 191.) Silver sodium dithionate, AgS 2 O 6 , Na 2 S 2 O 6 +4H 2 0. Sol. in H 2 O. (Kraut, A. 118. 96.) Silver dithionate ammonia, Ag 2 S 2 O 6 , 4NH 3 . Sol. in H 2 O without decomp. (Rammels- berg, Pogg. 58. 298.) Sodium dithionate, Na 2 S 2 O 6 +2H 2 O. 89!. in 2.1 pts. H 2 O at 16, and in 1.1 pts. boiling H 2 O. Insol. in alcohol. Fuming HCl+Aq precipitates the salt from aqueous solution. (Heeren, Pogg. 7. 76.) +6H 2 O. (Kraut, A. 117. 97.) Strontium dithionate, SrS 2 O 6 +4H 2 O. Sol. in 4.5 pts. H 2 O at 16, 1.5 pts. boiling H 2 O. Insol. in alcohol. (Heeren, Pogg. 7. 177.) Thallous dithionate, T1 2 S 2 O 6 . Very easily sol. in H 2 O. (Werther.) Thallous dithionate sulphate, 3T1 2 S 2 O 6 , T1 2 S0 4 . Sol. in H 2 O. (Wyrouboff, Ann. Phys. Beibl. 8. 802.) Thorium dithionate, Th(S 2 O 6 ) 2 +4H 2 O (?). Very unstable. (Kluss, A. 246. 188.) Tin (stannous) dithionate, SnS 2 Oe. Known only in solution. 8SnO, S 2 O 5 +9H 2 O. Insol. in H 2 O. Sol. in dil. acids, even dithionic acid+Aq. (Kluss, A. 246. 186.) Uranous dithionate, 6UO 2 , S 2 O 5 + 10H 2 O. Insol. in H 2 O; sol. in warm HCl+Aq. (Kluss, A. 246. 191.) 7UO 2 , S 2 O 5 +8H 2 O. As above. 8UO 2 , S 2 O 6 +21H 2 O. As above. Zh'vanadyl- dithionate, (VO 2 ) 2 S 2 O 6 .* Sol. in H 2 O. (Bevan, C. N. 38. 294.) Yttrium dithionate, Y 2 (S 2 O 6 )3 + 1SH 2 O. Not deliquescent. Easily sol. in H 2 O, but difficultly sol. in alcohol. Insol. in ether. (Cleve, Bull. Soc. (2) 21. 344.) Zinc dithionate, ZnS 2 O 6 +6H 2 O. Very sol. in H 2 O; decomp. on boiling. (Heeren, Pogg. 7. 183.) Zinc dithionate ammonia, ZnS 2 O e , 4NH 3 . Decomp. with H 2 O; sol. in warm, less sol. in cold NH 4 OH+Aq. (Rammelsberg, Pogg. 58. 297.) +H 2 O. Ppt. (Ephraim, B. 1915, 48. 640.) Dysprosium, Dy. (Lecoq de Boisbaudran, C. R. 102. 1005.) Dysprosium chloride, DyCl 3 +6H 2 O. Deliquescent, sol. in H 2 O. (Urbain, C. R . 1908, 146. 129.) FERRATE, SODIUM 333 Europium. Europium chloride, EuCl 2 . Sol. in H 2 O. Stable in very dil. aqueous solution, but decomp. when the solution is concentrated at 100. (Urbain, C. R. 1911, 163. 1157.) Erbium, Er. Decomposes H 2 O. (Hoglund.) The so-called element "erbium'' can be further decomp. into simple substances. (Kriiss, Z. anorg. 3. 353.) Erbium bromide, ErBr 3 +9H 2 O. Very deliquescent. Erbium chloride, ErCl 3 +6H 2 O. Deliquescent. Sol. in H 2 O and alcohol. (Hoglund.) Erbium mercuric chloride, ErCl 3 , 5HgCl 2 + Deliquescent. (Cleve.) Erbium fluoride, ErF 3 . Insol. in H 2 O. Very si. sol. in HF+Aq. (Hoglund, Bull. Soc. (2) 18. 193.) Erbium hydroxide, Er 2 O(OH) 4 . Insol. in KOH, or NaOH+Aq. Easily sol. in acids. Decomp. ammonium salts by boiling therewith. Erbium iodide, ErI 3 . Very deliquescent. Very sol. in H 2 and alcohol. Insol. in ether. (Hoglund.) Erbium oxide, Er 2 O 3 . Difficultly but completely sol. in warm HNO a , H 2 SO 4 , or HCl+Aq. Decomp. NH 4 salts by boiling therewith. Erbium peroxide, Er 2 O 5 . Precipitate. (Cleve, Bull. Soc. (2) 43. 53.) Erbium sulphide. Decomp. in moist air and with acids. Erythrochromium bromide, HOCr 2 (NH 3 ) 10 Br 5 +H 2 O. Very easily sol. in H 2 O. Insol. in HBr + Aq. Sol. in NH 4 OH+Aq. (Jorgensen, J. pr. (2) 25. 398.) - bromide, basic, HOCr 2 (NH 3 )io(OH)Br 4 +H 2 0. Very sol. in H 2 O. (Jorgensen.) - chloroiodide, HOCr 2 (NH 3 ) 1 oClI 4 +H 2 O. Sol. in H 2 O and in alcohol. (Jorgensen.) Erythrochromium chloroplatinate, [HOCr 2 fNH 3 ) 10 ] 2 (PtCl 6 ) 6 + 10H 2 0. Nearly insol. in H 2 O. (Jorgensen.) dithionate, basic, HOCr 2 (NH 3 ) 10 (S 2 Oe) 2 (OH)+2H 2 O. Insol. in H 2 O. Easily sol. in very dil. HNO 3 , HBr, HCl+Aq. Sol. in cone. NH 4 C1 +Aq. (Jorgensen.) -nitrate, HOCr 2 (NH 3 ) 10 (NO 3 ) 5 +H 2 O. Easily sol. in H 2 O. Insol. in dil. HNO 3 + Aq. Sol. in cone. HNO 3 with decomp. Very sol. in dil. NH 4 OH+Aq. Insol. in alcohol. (Jorgensen.) nitrate r basic, HOCr 2 (NH 3 ) 10 (NO 3 ) 4 OH +3^H 2 0. Sol. in cold H 2 O. (Jorgensen.) - sulphate, [HOCr 2 (NH 3 ) 10 ] 2 (SO 4 ) 5 . Nearly insol. in H 2 O. (Jorgensen.) Tdraferriammonium, Fe 2 N. See Iron nitride. Ferric acid. Barium ferrate, BaFeO 4 +H 2 O. Ppt. Can be boiled for some time with H 2 O without decomp. Decomp. by mineral acids. Sol. in dil. acetic acid. (Fremy, A. ch. (3) 12. 373.) Insol. in H 2 O; not readily acted upon by acids when dry. (Rosen, J. Am. Chem. Soc. 1895, 17. 766.) Ppt. Easily decomp. by acids. (Moeser, Arch. Pharm. 1895, 233. 526.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Calcium ferrate, CaF 2 O 4 . Sol. in H 2 O. (Resell, J. Am. Chem. Soc. 1895, 17. 760-69.) Potassium ferrate, K 2 FeO 4 . Very deliquescent. Easily sol. in cold H 2 O with evolution of much heat. Decomp. by standing or warming. Decomp. by acids or alkalies. (Fremy, A. ch. (3) 12. 369.) Sol. in H 2 O; insol. in alcohol. (Moeser, Arch. Pharm. 1895, 233. 524.) Quickly decomp. by potassium tartrate or racemate, sugar, or albumen without separa- tion of Fe 2 O 6 H 6 , by alcohol with separation of Fe 2 O 6 H 6 . Potassium oxalate, acetate, formate, and benzoate, also citrate decomp. much more slowly. Insol. in cone. KOH + Aq. (Wackenroder, A. 33. 41.) Sodium ferrate, Na 2 FeO 4 . Sol. in H 2 O and in cone. NaOH+Aq. (Fremy, 1. c.) 334 FERRATE, STRONTIUM Strontium ferrate, SrFeO 4 . SI. sol. in H 2 O by which it is decomp. Decomp. by acids. Sol. in aqueous solutions of Na aud K salts with partial decomp. Insol. in sat. SrBr 2 +Aq., alcohol and ether. (Eidmann, B. 1903, 36, 2290.) Ferricomolybdic acid. Ammonium ferricomolybdate, 3(NH 4 )aO, Fe 2 O 3 , 12MoO 3 + 19H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 697.) Ferricyanhydric acid, H 3 Fe(CN) 3 , (or H e Fe 2 (CN) 12 ). Easily sol. in H 2 or alcohol. Solution decomposes slowly by standing, more rapidly by heating. Insol. in ether. Ferricyanides. The alkali, and alkaline-earth ferricyanides are sol. in H 2 O; the others are insol. The ferricyanides of metals, the oxides of which are sol. in NH 4 OH, or KOH+Aq, are them- selves sol. in those reagents. Ammonium ferricyanide, (NH 4 ) 3 Fe(CN) 6 + 3H 2 0. Permanent. Readily sol. in H 2 O (and alcohol?). Ammonium ferrous ferricyanide, NH 4 FeFe(CN) 6 + 1 HH 2 O. Sol. in H 2 O and not pptd. by alcohol from aqueous solution. More stable than the cor- responding K salt. Ammonium lead ferricyanide, NH 4 PbFe(CN) 6 +3H 2 O. Ammonium potassium ferricyanide, (NH 4 ) 2 KFe(CN) 6 . Sol. in H 2 O. (Schaller, Bull. Soc. (2) 1. 275.) Barium ferricyanide, Ba 3 [Fe(CN) 6 ] 2 + 20H 2 O. Easily sol. in H 2 O; insol. in alcohol. (Schuler, W. A. B. 77. 692.) Barium potassium ferricyanide, BaKFe(CN) 6 +3H 2 O. Permanent. Easily sol. in H 2 O, less in alcohol. Barium ferricyanide bromide, Ba 3 [Fe(CN) 6 ]2, 2BaBr 2 +20H 2 O. Easily sol. in H 2 O. Boiling alcohol does not dissolve out BaBr 2 . (Rammelsberg, J. pr. (2) 39. 463.) Bismuth ferricyanide, Bi 3 [Fe(CN") 6 ]5. Insol. in H 2 O, but decomp. by boiling therewith. (Muir, Chem. Soc. 32. 40.) Cadmium ferricyanide ammonia, Cd 3 [Fe(CN) 6 ] 2 , 6NH 3 +3H 2 0. Effloresces to form Cd 3 [Fe(CN)] 2 , 4NH 3 +2H 2 0. Insol. in H 2 O. (WyroubofT, A. he. (5) 10. 413.) Calcium ferricyanide, Ca 3 [Fe(CN) 6 ] 2 +10, or 12H 2 0. Deliquescent. Sol. in H 2 O and dil. alcohol. Calcium potassium ferricyanide, CaKFe(CN) 5 . Sol. in H 2 O. Cerous ferricyanide, CeFe(CN) 6 +4H 2 O. Sol. in H 2 O; easily decomp. (Jolin.) Chromic ferricyanide (?). Ppt. Cobaltous ferricyanide, Co 3 [Fe(CN) 6 ] 2 . Insol. in H 2 O and HCl+Aq. Sol. in NH 4 OH+Aq. Cobaltous ferricyanide ammonia, Co 3 [Fe(CN) 6 ] 2 , 4NH 3 +6H 2 0. Cobaltic ferricyanide ammonia. See Luteo,- purpureo,- etc. cobaltic fern- cyanide. Cuprous ferricyanide, (Cu 2 ) 3 [Fe(CN) 6 ] 2 . Sol. in NH 4 OH+Aq; insol. in NH 4 salts-f- Aq. (Wittstein.) Cupric ferricyanide, Cu 3 [Fe(CN) 6 ] 2 . Insol. in H 2 O or NH 4 salts +Aq. Sol. in NH 4 OH, and (NH 4 ) 2 CO 3 +Aq. (Wittstein.) Insol. in HCl+Aq. Iron (ferrous) ferricyanide, Fe 3 [Fe(CN) e ] 2 + zH 2 O. (TurnbuWs blue.) Properties as ferric ferrocyanide (Prussian blue), with which it is perhaps identical. (Gintl, Z. anal. 21. 110.) Iron (ferrosoferric) ferricyanide, Fe 13 (CN) 36 =Fe I 4 I Fe I I[Fe(CN) 6 ] 6 . (Prussian green.) Insol. in H 2 O or cone. HCl+Aq, but slowly decomp. by boiling therewith. Fe 3 (CN) 8 +4H 2 p = Fe I JFe II 2 I [Fe(CN)f] 4 + 12H 2 O. Properties as above. (Reynolds, Chem. Soc. 64. 767.) Iron (ferrous) potassium ferricyanide, KFe 2 (CN) 6 =KFeFe(CN) 6 +4, or 3H 2 O. (Soluble Prussian blue.) Sol. in H 2 O, but insol. in salts+Aq or alcohol. FERRICYANIDE, POTASSIUM 335 Salt of the same composition, called "Wil- liamson's blue," is insol. in H 2 O. Lead ferricyanide, basic, Pb 3 [Fe(CN) 6 ] 2 , 3Pb0 2 H 2 + llH 2 0. (Schuler.) Lead ferricyanide, Pb 3 [Fe(CN) 6 ] 2 +16H 2 O. SI. sol. in H 2 O; more sol. in hot, than cold H 2 O, but decomp. on boiling. (Gmelin.) +4H 2 O. Easily sol. in H 2 O; si. sol. in alcohol. (Schuler, W. A. B. 77. 692.) Lead potassium ferricyanide, PbKFe(CN)e +3H 2 O. Sol. in 4.75 pts. H 2 O at 16, and the solu- tion decomp. on standing. (Schuler.) + 1^H 2 O. Efflorescent. Much more sol. in H 2 O than the Pb salt. Insol. in alcohol. (Wyrouboff.) Lead ferricyanide nitrate, Pb 3 [Fe(CN) B ] 2 , Pb(NO 3 ) 2 +12H 2 O. Sol. in 13.31 pts. H 2 O at 16. (Schuler.) +11H 2 O. (Joannis, A. ch. (5) 26. 528.) Magnesium ferricyanide, Mg 3 [Fe(CN) 6 ]2. Sol. in H 2 0. Magnesium potassium ferricyanide, MgKFe(CN) 6 . (Reindel, J. pr. 103. 166.) Manganous ferricyanide, Mn 3 [Fe(CN) 6 ] 2 . Insol. in H 2 O, acids, NH 4 OH, or NH 4 salts +Aq. Mercurous ferricyanide, Hg 3 Fe(CN) 6 . Ppt. (Fernekes, J. Am. Chem. Soc. 1906, 28. 604.) Mercuric femcyanide, Hg 3 [Fe(CN) 6 ] 2 . Very sol. in H 2 O. Solution quickly decomp. (Fernekes, J. Am. Chem. Soc. 1906, 28. 603.) Nickel ferricyanide ammonia, Ni 3 [Fe(CN) 6 ] 2 , 4NH 3 +H 2 O. Sol. in NH 4 OH+Aq. (Reynoso, A. ch.(3) 30. 254.) Nickel ferricyanide, Ni 3 [Fe(CN) 6 ] 2 (?). Ppt. Insol. in HCl+Aq. Potassium ferricyanide, K 3 Fe(CN) 6 , (or K 6 Fe 2 (CN) 12 ). Permanent. Easily sol. in H 2 O. '100 pts. H 2 O dissolve pts. K 3 Fe(CN) 6 at t. t Pts. salt t Pts. salt t Pts. salt 4.4 10 33.0 36.6 15.6 37.8 40.8 58.8 100 104.4 77.5 82.6 (Wallace, Chem. Soc. 7. 80.) 100 pts. H 2 O at 13 dissolve 38 pts., and the solution has sp. gr. = 1.1630. (Schiff, A. 113. 350.) 1 1. sat. solution in H 2 O at 25 contains 385.5 g. K 3 Fe(CN) 6 . (Grube, Z. Electrochem. 1914, 20. 342.) Sp. gr. of K 3 Fe(CN) 6 +Aq at 13. % salt Sp. gr. % salt Sp. gr. S St Sp. gr. 1 1.0051 11 1 . 0595 21 1 . 1202 2 .0103 12 1.0653 22 1 . 1266 3 .0155 13 1.0712 23 1.1331 4 .0208 14 1.0771 24 1.1396 5 .0261 15 1.0831 25 1.1462 6 .0315 16 1 . 0891 26 1.1529 7 .0370 17 1.0952 27 1.1596 8 .0426 18 1.1014 28 1 . 1664 9 1.0482 19 1.1076 29 1 . 1732 10 1.0538 20 1.1039 30 1.1802 (Schiff.) Sp. gr. of K 3 Fe(CN) 6 +Aq at 25. Concentration of K 3 Fe(CN) 6 +Aq. Sp. gr. 1 normal Vr- ;; Vs " 1 . 0574 1 . 0289 1.0143 1.0092 (Wagner, Z. phys. Ch. 1890, 5. 37.) Sat, K 3 Fe(CN) 6 +Aq boils at 104.4. (Wallace.) 1 1. sat. solution at 25 of K 8 Fe(CN) 6 + K 4 Fe(CN) 6 contains 338.1 g. K 3 Fe(CN) 6 and 79.02 g. K 4 Fe(CN) 6 . (Grube.) Solubility of K 3 Fe(CN) 6 +K 4 Fe(CN) 6 in KOH+Aq at 25. KOH Normality g. per 1. K 3 Fe(CN) 6 K 4 Fe(CN) 6 0.4687 0.9628 1.949 309 275.3 200.8 66.64 55.19 35.95 (Grube.) Solubility in KOH+Aq at 25. KOH Normality 0.4687 0.9628 1.949 g. K 3 Fe(CN) 6 per 1. 342.7 302.3 215.1 (Grube, Z. Electrochem, 1914, 20. 342.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) 336 FERRICYANIDE, POTASSIUM SODIUM Insol. in absolute alcohol, and only si. sol. in dil. alcohol. Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Insol. in methyl acetate ( Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43, 314.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Potassium sodium ferricyanide, KNa 2 Fe(CN) 6 . Sol. in H 2 O. K 2 NaFe(CN) 6 . Sol. in H 2 O. K 3 Na 3 [Fe(CN) 6 ] 2 . Sol. in H 2 O. +3H 2 O. Potassium ferricyanide iodide, K 3 Fe(CN) 3 , KI. Very unstable. Silver ferricyanide, Ag 3 Fe(CN) 6 . 1 1. H 2 O dissolves 0.00066 g. Ag 3 Fe(CN) 6 at 20. (Whitby, Z. anorg. 1910, 67. 108.) Sol. in NH 4 OH, and hot (NH 4 ) 2 CO 3 +Aq, but insol. in NH 4 salts +Aq. Insol. in Hg(NO 3 ) 2 +Aq. (Wackenroder, A. 41. 317.) Silver ferricyanide ammonia, 2Ag 3 Fe(CN) 6 , Insol. in H 2 O. Sol. in NH 4 OH+Aq. (Gintl.) 2Ag 3 Fe(CN) 6 , 5NH 3 . (Carlo, Gazz. ch. it. 1910, 40. (2) 477.) Sodium ferricyanide, Na 3 Fe(CN) 6 +H 2 O. Deliquescent. Sol. in 5.3 pts. cold, and 1.5 pts. boiling H 2 O. Insol. in alcohol, but not pptd. thereby from aqueous solution. (Bette.) Ferrinitrososulphydric acid. See Ferrofteptanitrososulphydric acid. Ferrocyanhydric acid, H 4 Fe(CN)6. Sol. in H 2 O and alcohol. 100 pts. H 2 O dissolve 15 pts. acid at 14. (Joannis, A. ch. (5) 26. 514.) Insol. in ether, and much less sol. in ether- alcohol than in alcohol. Insol. in cone. HCl+Aq. Ferrocyanides. The ferrocyanides of the alkali and alka- line-earth metals are sol. in H 2 O; the others are insol., but sol. in alkalies +Aq in case the base is sol. therein. Aluminum ferrocyanide, Al 4 [Fe(CN) s ] 3 + 17H 2 O. SI. sol. in H 2 0. SI. sol. in HCl+Aq with partial decomp. (Wyrouboff, A. ch. (5) 8. 446.) Ammonium ferrocyanide, (NH 4 ) 4 Fe(CN) 6 + 3H 2 0. Very sol. in H 2 O; insol. in alcohol. +H 2 O. (Berzelius.) Ammonium cadmium ferrocyanide ammonia, (NH 4 ) 2 Cd 3 [Fe(CN) 6 ] 2 , 2NH 3 +H 2 O. Sol. in H 2 O. (Wyrouboff, A. ch. (5) 10. 413.) Ammonium calcium ferrocyanide, (NH 4 ) 2 CaFe(CN) 6 . SI. sol. in H 2 O. (Kunheim and Zimmer- man, Dingl. 252. 47'8.) 100 g. sat. solution in H 2 O contain 0.258 g. at 16. (Brown, J. phys. Ch. 1898, 2. 51.) Ammonium cuprous ferro cyanide, (NH 4 ) 2 Cu 2 Fe(CN) 6 . Insol. in H 2 O and alcohol. Decomp. in the air. (Messner, Z. anorg. 1895, 8. 382.) Ammonium cu ionium cupric ferrocyanide, (NH 4 ) 2 CuFe(CN) 6 . Ppt. +xH 2 O. Very unstable. Insol. in H 2 O; decomp. by boiling H 2 O. (Messner, Z. anorg. 1895, 8. 384.) Ammonium lithium ferrocyanide, (NH 4 ) 2 Li 2 Fe(CN) 6 +3H 2 O. Sol. in H 2 O. (Wyrouboff, A. ch. (4) 21. 270.) Ammonium magnesium ferrocyanide. (NH 4 ) 2 MgFe(CN) 6 . 1 1. sat. solution at 17 contains 2.48 g. (NH 4 ) 2 MgFe(CN). (Robinson, Chem. Soc. 1909, 95. 1353.) Ammonium manganous ferrocyanide, (NH 4 ) 2 MnFe(CN) 6 . Ppt. (Blum, Z. anal. 30. 284.) Ammonium potassium ferrocyanide, NH 4 K 3 Fe(CN) 6 +3H 2 0. Easily sol. in cold, more easily in hot H 2 O. Insol. in alcohol. (NH 4 ) 2 K 2 Fe(CN) G +3H 2 O. Sol. in H 2 O. Ammonium potassium ferrocyanide ammo- nium chloride, (NH 4 ) 3 KFe(CN) 6 , 2NH 4 C1. Sol. in H 2 O. (Etard, J. pr. (2) 31. 430.) Ammonium ferrocyanide bromide, (NH 4 ) 4 Fe(CN) 6 , 2NH 4 Br. Permanent. Very sol. in H 2 O. Ammonium ferrocyanide chloride, (NH 4 ) 4 Fe(CN) 6 , 2NH 4 C1+3H 2 0. Permanent. Very sol. in H 2 O, but less so than NH 4 C1. (Bunsen.) FERROCYANIDE, CUPROUS 337 Antimony ferrocyanide, 25H 2 O. Ppt. (Atterberg.) Sb 4 [Fe(CN) 6 ] 3 + Barium ferrocyanide, Ba 2 Fe(CN) 6 +6H 2 O. Permanent. SI. sol. in H 2 O. Sol. in 584 pts. cold, and 116 pts. boiling H 2 O (Duflos, 1832); sol. in 1800 pts. cold H 2 O (Porrett, 1814); sol. in 1920 pts. cold, and about 100 pts. boiling H 2 O (Thomson); sol. in 2000 pts. cold, and 100 pts. boiling H 2 O. (Ure'sDict.) Sol. in 1000 pts. H 2 O at 15, and 100 pts. at 75. (Wyrouboff, A. ch. (4) 16. 292.) Sol. in HNO 3 , HC1, or cone. H 2 SO 4 +Aq. Barium cupric ferrocyanide, BaCuFe(CN) 6 . Insol. in H 2 O. (Messner, Z. anorg. 1895, 8. 389.) Barium potassium ferrocyanide, BaK 2 Fe(CN) 6 +3H 2 O. Sol. in 38 pts. cold, and 9.5 pts. boiling H 2 O (Duflos, 1832); in 36.4 pts. H 2 at 14, and 11.9 pts. at b.-pt. (Mosander.) Not more sol. in NH 4 Cl+Aq than in H 2 O. Sol. in dil., insol. in cone. HCl+Aq. (Rose.) +5H 2 O. Sol. in 300 pts. H 2 O at ord. temp. (Wyrouboff.) Bismuth ferrocyanide, 5H 2 0(?). SI. sol. in pure H 2 O. Bi 4 [Fe(CN) 6 ] 5 . Ppt. 31. 657.) Bi 2 Fe(CN) 6 + (Wyrouboff.) (Muir, Chem. Soc. Bismuth potassium ferrocyanide, BiKFe(CN) 6 +7H 2 O, or 4H 2 O. Ppt. Cadmium potassium ferrocyanide, CdK 2 Fe(CN) 6 +H 2 O. Insol. in H 2 0. Formula given by Wyrouboff is Cd 5 K 6 lFe(CN) 6 ] 4 + 1 1H 2 (?) . Calcium ferrocyanide, Ca 2 Fe(CN) 6 +12H 2 O. Very sol. in H 2 O. Sol. in 0.66 pt. H 2 at 90 and not pptd. by cooling, and is ap- parently less sol. in warm than cold H 2 O. (Wyrouboff, A. ch. (4) 16. 280.) Calcium cuprous ferrocyanide, CaCu 2 Fe(CN) 6 . (Messner, Z. anorg. 1894, 8. 387.) Calcium cupric ferrocyanide, CaCuFe(CN) 6 . Insol. in H 2 O. (Messner, Z. anorg. 1895 8. 388.) Calcium potassium ferrocyanide, CaKjFe(CN).; SI. sol. in H 2 O. (Kunheim and Zimmer- man, Dingl. 262. 478.) +3H 2 O. Sol. in 795 pts. H 2 O at 15, and 145 pts. at b-pt., with decomp. in the latter case. Sol. in dil., insol. in cone. HCl+Aq. Sol. in HNO 3 of 1.2 sp. gr. (Mosander.) Insol. in NH 4 Cl+Aq. Calcium sodium ferrocyanide, CaNa6[Fe(CN) 6 ] 2 . Sol. in H 2 O. Calcium strontium ferrocyanide, CaSrFe(CN) 6 + 10H 2 O. Efflorescent. Sol. in about 3 pts. H 2 0. (Wyrouboff, A. ch. (4) 21. 278.) Cerium ferrocyanide, Ce 4 [Fe(CN) 6 ]s+ 30H 2 0. Ppt. (Wyrouboff.) Cerium potassium ferrocyanide, CeKFe(CN) 6 +3H 2 0. Ppt. (John.) +4H 2 O. (Wyrouboff.) Chromic ferrocyanide, 20H 2 O. Ppt. Cr 2 [Fe(CN) 6 ] 3 + Cobaltous ferrocyanide, Co 2 Fe(CN) 6 + 7H 2 0. Wholly insol. in H 2 O. Sol. in H 2 SO 4 with decomp. Insol. in HCl+Aq. SI. sol. in NH 4 OH+Aq. Sol. in (NH 4 ) 2 CO 3 +Aq. Insol. in NH 4 Cl+Aq. Sol. inKCN+Aq. Cobaltous ferrocyanide ammonia, Co 2 Fe(CN) 6 , 8NH 3 + 10H 2 O. Ppt. Decomp. on standing. (Curda, Z. Ch. 1869. 369.) Co 2 Fe(CN) 6 , 12NH 3 +9H 2 O. As above. (Curda.) Cobaltous potassium ferrocyanide, CoK 2 Fe(CN) 6 . Ppt. (Wyrouboff.) Co 5 K 5 [Fe(CN) 6 ] 4 (?). Ppt. Insol. onlyrin presence of an excess of K 4 Fe(CN) 6 . (Wy- rouboff.) Columbium potassium ferrocyanide, Cb 16 K[Fe(CN) 6 ] 2 +67H 2 O (?). Sol. inH 2 O. (Wyrouboff.) Cb 12 K 2 Fe(CN) 6 + 39H 2 O (?). Sol. in H 2 0. (W,.) (CbO) 5 K 9 [Fe(CN) 6 ] 6 +10H 2 0(?). Ppt. (At- terberg.) Cuprous ferrocyanide, Cu 4 Fe(CN) 6 . Insol. in H 2 O; sol. in NH 4 OH+Aq; insol. in NH 4 Cl+Aq. 338 FERROCYANIDE, CUPRIC, BASIC Cupric ferrocyanide, basic, CuFe(OH) 4 (CN) 4 . Ppt. (Bong, Bull. Soc. 23. 231.) Cupric ferrocyanide, Cu 2 Fe(CN) 6 +7H 2 O. Insol. in H 2 O or acids. - Insol. in NH 4 salts +Aq. Sol. in NH 4 OH+Aq. Sol. in (NH 4 ) 2 C 2 O 4 +Aq and in KCN+Aq. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) + 10H 2 O. Sol. in excess of K 4 Fe(CN) 6 + Aq, especially if hot. (Wyrouboff.) Cupric ferrocyanide ammonia (cupram- monium ferrocyanide), Cu 2 Fe(CN) 6 , 4NH 3 +H 2 O. Insol. in H 2 O or alcohol. Sol. in NH 4 OH + Aq. (Bunsen.) Cu 2 Fe(CN) 6 , 8NH 3 +H 2 0. Cuprous magnesium ferrocyanide, Cu 2 MgFe(CN) 6 . Very unstable. Decomp. in air. Insol. in H 2 O. (Messner, Z. anorg. 1895, 8. 385.) Cupric magnesium ferrocyanide, CuMgFe(CN) 6 . Insol. in H 2 O. Decomp. by boiling H 2 O. Very unstable. (Messner, Z. anorg. 1895, 8. 387.) Cuprous potassium ferrocyanide, Cu 2 K 2 Fe(CN) 6 . Insol. in H 2 O. Decomp. by boiling H 2 O. Decomp. by acids. Insol. in alcohol. (Mess- ner, Z. anorg. 1895, 8. 378.) +l>HtO. Insol. in H 2 O, alcohol, or ether. Decomp. by acids. Sol. in KCN+Aq. K 3 Cu 2 Fe(CN) 6 +4H 2 O. +5H 2 O. (Wonfor.) +6H 2 O. (Wyrouboff.) Cupric potassium ferrocyanide, K 2 CuFe(CN) 6 +H 2 0. Insol. in cold, si. decomp. by boiling H 2 O. K 2 Cu,[Fe(CN) 6 ] 2 + 12H 2 O. Ppt. Cuprous sodium ferrocyanide, Cu 2 Na 2 Fe(CN) 6 . Decomp. by boiling H 2 O; insol. in alcohol; insol. in H 2 O; decomp. by acids. (Messner, Z. anorg. 1895, 8. 373.) Cupric sodium ferrocyanide, CuNa 2 Fe(CN) 6 . Insol. in cold H 2 O. Decomp. by boiling H 2 O. (Moissan, Z. anorg. 1895, 8. 376.) Cupric strontium ferrocyanide, CuSrFe(CN) 6 . Insol. in H 2 O. (Messner, Z. anorg. 1895, 8. 389.) Didymium potassium ferrocyanide,. DiKFe(CN) 6 +4H 2 O. Ppt. (Cleve.) +2H 2 O. (Wyrouboff.) Erbium potassium ferrocyanide, ErKFe(CN) 6 +zH 2 O. (Hoglund.) Gallium ferrocyanide. Sol. in boiling HCl+Aq. (de Boisbaudran, C. R. 99.526.) Glucinum ferrocyanide, Gl 2 Fe(CN) 6 , 4G10 2 H 2 +7H 2 (?). Sol. in H 2 O. (Atterberg.) Iron (ferric) ferrocyanide, Fe7(CN)j 8 = Fe 4 [Fe(CN) 6 ] 3 +zH 2 0. (Prussian blue.) Insol. in H 2 O, alcohol, ether, or oils. Decomp. slowly by boiling H 2 O. Insol. in dil. mineral acids. Sol. in cone. HCl+Aq, and cone. H 2 SO 4 without de- comp. Sol. in H 2 C 2 4 or NH 4 tartrate+Aq. Insol. in NH 4 OH+Aq. Decomp. by NaOH, or KOH+Aq. Not pptd. in presence of tar- trates or citrates. Iron (ferrous) potassium ferrocyanide, FeK 2 Fe(CN) 6 . Insol. in H 2 O. Decomp. on air. Iron (ferric) potassium ferrocyanide, FeKFe(CN) 6 . Is probably ferrous potassium ferricyanide, which see. Iron (ferric) ferrocyanide ammonia, Fe 4 [Fe(CN) 6 ] 3 , 6NH 3 +9H 2 O. Insol. in NH 4 tartrate+Aq. Lanthanum potassium ferrocyanide, LaKFe(CN) 6 +4H 2 O. Ppt. Lead ferrocyanide, Pb 2 Fe(CN) 6 +3H 2 O. Insol. in H 2 O, acids, or NH 4 OH+Aq. (Wyrouboff, A. ch. (5) 8. 480.) SI. sol. in cone. H 2 SO 4 , from which it is pptd. by H 2 O. (Berzelius.) Sol. in hot NH 4 C1, or NH 4 succinate+Aq; insol. in other NH 4 salts +Aq. (Wittstein.) Insol. in NH 4 Cl+Aq. (Brett.) Not pptd. in presence of Na citrate. (Spiller.) Lithium ferrocyanide, Li 4 Fe(CN) 6 +9H 2 O. Deliquescent. Very sol. in H 2 O. Lithium potassium ferrocyanide, Li 2 K 2 Fe(CN) 6 +3H 2 O. Very sol. in H 2 O. Sol. in 1.5 pts. H 2 O at ord. temp. (Wyrouboff, A. ch. (4) 21. 274.) FERROCYANIDE, POTASSIUM 339 Magnesium ferrocyanide, Mg 2 Fe(CN) 6 + 6H 2 O. Sol. in 3 pts. cold H 2 O. (Bette, A 22 148.) Magnesium potassium ferrocyanide. MgK,Fe(CN).. Sol. in 1575 pts. H 2 O at 15, and 238 pts. at 100. Solution is decomp. by boiling (Storer's Diet.) 1 1. sat. solution at 17 contains 1.95 g MgK 2 Fe(CN) 6 . (Robinson, Chem. Soc 1909, 75. 1353.) Manganous ferrocyanide, Mn 2 Fe(CN) 6 + 7H 2 O. Insol. in H 2 0. Sol. in HCl+Aq. Insol in NH 4 C1, or NH 4 NO 3 +Aq. Manganic ferrocyanide, Mn 2 Fe 3 (CN)i 2 . Insol. in H 2 O. Easily decomp. in the air Sol. in HC1. (Straus, Z. anorg. 1895, 9. 8.) Manganous potassium ferrocyanide, MnK 2 Fe(CN) 6 . Ppt. (Berzelius.) 5Mn 2 Fe(CN>, 4K 4 Fe(CN) 6 +4H 2 O(?). Ppt. Sol. in dil. HCl+Aq. (Wyrouboff.) Mercuric potassium ferrocyanide. K 2 HgFe(CN) 6 . Insol. in H 2 O. Appreciably sol. in K 4 Fe(CN) 6 +Aq. (Fernekes, J. Am. Chem. Soc. 1906, 28. 87.) Molybdenum ferrocyanide, Mo 4 Fe(CN) 6 + 20H 2 O(?). . Very sol. in NH 4 OH+Aq. (Wyrouboff.) Mo 2 Fe(CN) 6 +8H 2 O (?). (W.) + 14H 2 O (?). Very sol. in H 2 O; insol .in alcohol. (W.) Molybdenum potassium ferrocyanide. K 4 Mo 8 [Fe(CN) 6 ] 2 +40H 2 (?). (Wyrouboff.) K 2 (Mo0 2 ) 3 [Fe(CN) 6j2 , 2MoO 3 +20H 2 O (?). (Atterberg.) K 6 Mo 2 [Fe(CN) 6 ] 2 , 2MoO 3 + 12H 2 O (?). (Atterberg.) Nickel ferrocyanide, Ni 2 Fe(CN) 6 +llH 2 O, or 14H 2 O. Ppt. Insol. in H 2 O or HCl+Aq. Sol. in NH 4 OH+Aq; insol. in NH 4 salts +Aq. Sol. in KCN+Aq. Nickel ferrocyanide ammonia, Ni 2 Fe(CN) 6 , 4NH 3 +H 2 O. Completely insol. in H 2 O and not attacked thereby; sol. in NH 4 OH+Aq to form Ni 2 Fe(CN) 6 , 10NH 3 +4H 2 O. Decomp. by hot H 2 O. (Reynoso, A. ch. (3) 30. 252.) Ni 2 Fe(CN) 6 , 2NH 3 +4, and 9H 2 O. Hygro- scopic. Easily decomp. (Gintl, J. B. 1868. Ni 2 Fe(CN) 6 , 8NH 3 +4H 2 O. Sol. in NH 4 OH+Aq. (G.) Ni 2 Fe(CN) 6 , 12NH 3 +9H 2 0. Sol. in NH 4 OH+Aq, but less so than the above compounds. (G.) Nickel potassium ferrocyanide, NiK 2 Fe(CN) 6 +3H 2 O. Ppt. (Wyrouboff.) Osmium ferrocyanide, Os 2 Fe(CN) 6 . Ppt. (Martius, A. 117. 368.) Potassium ferrocyanide, K 4 Fe(CN) 6 . Permanent. Easily sol. in cold, and more easily in hot H 2 O. Sol. in 4.23 pts. H 2 O at 15, or 100 pts."H 2 O dissolve 23.6 pts. salt at 15. (Schiff, A. 113. 350.) 100 pts. H 2 dissolve 27.8 pts. at 12.2; 65.8 pts. at 37.7; 87.6 pts. at 65.5: and 90.6 pts. at 96.3. (Thomson.) Sol. in 4 pts. cold, and 2 pts. boiling H 2 O. (Wittstein.) 100 pts. H 2 dissolve 29.2 pts. salt at 15, and solution has sp. gr. = 1.1441. (Michel and Kraft, A. ch. (3) 41. 478.) Solubility of K 4 Fe(CN) 6 in H 2 O at t. 2 +7 14 30 56 10.8 '15.4 17.9 23.0 31.7% 60 75 89 98 157 34.0 39.1 41.9 42.6 46.8% (Etard, A. ch. 1894, (7) 2. 546.) K 4 Fe(CN) 6 +Aq sat. at 8 has sp. gr.= 1.13. (Anthon.) Sp. gr. of K 4 Fe(CN) 6 +Aq at 15. OB |1 1"! g Sp. gr. o 11 ^ Sp. gr. "O^- 11 S Sp. gr. i 2 3 4 5 6 7 1.0058 1.0116 1.0175 1.0234 1.0295 1 . 0356 1.0417 8 9 10 11 12 13 14 1.0479 1.0542 1 . 0605 1.0669 1.0734 1.0800 1.0866 15 16 17 18 19 20 1.0932 1.0999 1.1067 1.1136 1 . 1205 1 . 1275 (Schiff, A. 113. 199.) Sp. gr. of K 4 Fe(CN),+Aq at 25. Concentration of K 4 Fe(CN)6+Aq. Sp. gr. 1 normal ] A " 'A " Vs " Vl6 " 1.0617 1.0300 1.0150 1.0074 1.0037 (Wagner, Z. phys. Ch. 1890, 6. 37.) 340 FERROCYANIDE, POTASSIUM SAMARIUM Solubility in KOH+Aq at 25. KOH Normality g. K 4 Fe(CN)6+3H 2 Operl. 0.09984 0.2496 0.4963 0.7036 0.9415 1.395 1.883 308.5 283.5 247.1 217.4 184.8 132.1 86.12 (Grube, Z. Electrochem, 1914, 20. 342.) K 4 Fe(CN) 6 +NaCl+Aq sat. at 20 con- tains 26.6 g. NaCl and 17.8 g. K 4 Fe(CN) 6 per 100 g. H 2 O; sat, at 93 it contains 27.4 g. NaCl and 35.9 g. K 4 Fe(CN) 6 per 100 g. H 2 O. (Cohroy, J. Soc. Chem. Ind. 1898, 17. 105.) K 4 Fe(CN) 6 +KCl+Aq sat. at 21 con- tains 27.2 g. KC1 and 4.2 g. K 4 Fe(CN) 6 per 100 g. H 2 O; sat. at 99 it contains 39.6 g. KC1 and 17.0 g. K 4 Fe(CN) 6 per 100 g. H 2 O. (Conroy.) K 4 Fe(CN) 6 +Na 2 CO 3 +Aq. sat. at 22 contains 29.9 g. Na 2 CO 3 and 26.7 g. K 4 Fe(CN) 6 per 100 g. H 2 0; sat. at 97 it con- tains 42.0 g. Na 2 CO 3 and 27.5 g. K 4 Fe(CN) 6 per 100 g. H 2 O. (Conroy.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol even when dilute. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) +3H 2 O. 1 1. sat. salution in H 2 O contains 319.4 g. K 4 Fe(CN) 6 +3H 2 O. (Grube, Elec- trochem, Z. 1914, 20. 342.) Two modifications with different solubil- ities. 25.0 g. of a modification are contained in 100 g. of salution at 20. 24.6 g. of modification are contained in 100 g. of solution at 20. (Briggs, Chem. Soc. 1911, 99. 1024.) 32.0 g. K 4 Fe(CN) 6 (anhydrous) are dis- solved in 100 g. H 2 O at 25. (Wagner, Z. phys. Ch. 1910, 71. 428.) Potassium samarium ferrocyanide, KSmFe(CN) 6 +5H 2 O. Precipitate. (Cleve.) Potassium sodium ferrocyanide, KNa 3 Fe(CN) 6 +12H 2 O. Sol. in H 2 O. K 2 Na 2 Fe(CN) 6 +8H 2 O. Easily sol. in H 2 O. K 3 NaFe(CN) 6 +3H 2 O. Permanent. Eas- ily sol. in H 2 O; insol. in alcohol. Potassium sodium ferrocyanide nitrate, K 2 Na 2 Fe(CN) 6 , 4KNO 3 . Sol. inH 2 O. (Martius.) Potassium strontium ferrocyanide, K 2 SrFe(CN) 6 +3H 2 0. Easily decomp. Sol. in H 2 O;'sl. sol. in alcohol. (Wyrouboff, A. ch. (4) 21. 276..) Potassium stannic ferrocyanide, KSn 3 [Fe(CN) 6 ] 3 +68H 2 O (?) Ppt. (Wyrouboff.) K 4 Sn 10 [Fe(CN) 6 ] u +230H 2 ( berg.) (Atter- Potassium titanium ferrocyanide, K 3 Ti 3 [Fe(CN) 6 ] 2 + llH 2 (?). Ppt. Sol. in K 4 Fe(CN) 6 +Aq. (Wyrou- boff.) K 4 Fe(CN) 6 , HTi 2 Fe(CN) 6 +43H 2 O (?). Ppt. (Wyrouboff.) K 2 (TiO) 3 [Fe(CN) 6 j 2 +23H 2 O (?). Ppt. (Atterberg.) K 2 (TiO)n[Fe(CN) 6 ] 6 + HOH 2 (?). Ppt. (Atterberg.) Potassium tungsten ferrocyanide, KW 2 Fe(CN) 6 +7H 2 O (?). Sol. in H 2 O. (Wyrouboff.) K 2 W 5 Fe(CN) 6 +2bH 2 O (?). Sol. in H 2 O. (W.) Potassium uranium ferrocyanide, K 2 U 3 [Fe(CN) 6 ] 2 +6H 2 r?). Ppt. (Wyrouboff.) K 2 (U0 2 ) 3 [Fe(CN) 6 ] 2 +6H 2 O. Ppt. (Atter- berg.) - * K 6 (U0 2 ) 5 [Fe(CN) 6 ] 4 +12H 2 0. Sol. in f _H 2 O. (Atterberg.) Potassium vanadium ferrocyanide, K 18 V[Fe(CN) 6 ] 6 +39H 2 O (?). Ppt. SI. sol. in H,O. (Wyrouboff.) K 6 (VO) 5 [Fe(CN) 6 ] 4 +60H 2 O(?). Ppt. (At- terberg.) Potassium ytterbium ferrocyanide, KYbFe(CN) 6 +3H 2 0. Ppt. Sol. in excess K 4 Fe(CN) 6 +Aq. (Cleve, Z. anorg. 1902, 32. 140.) Potassium yttrium ferrocyanide, KYFe(CN) e +2H 2 O. Ppt. (Wyrouboff, A. ch. (5) 8. 444.) Potassium zinc ferrocyanide, K 4 Zn 6 [Fe(CN) e ] 4 + 12H 2 O. Absolutely insol. in H 2 O. (Wyrouboff, A. ch. (5) 8. 485.) Potassium ferrocyanide carbonyl, K 8 Fe(CN) 6 (CO) +3^H 2 O. See Carbonyl ferrocyanide, potassium. Rubidium ferrocyanide, Rb 4 Fe(CN) 6 +2H 2 O. Sol. in less than 1 pt. H 2 O at ord. temp, with great absorption of heat. (Wyrouboff. A. ch. (4) 16. 307. FERRONITROSULPHIDE, POTASSIUM 341 Silver ferrocyanide, Ag 4 Fe(CN) 6 +H 2 O. Insol. in HoO or dil. acids. Insol. in NH 4 OH, or NH 4 salts + Aq. Sol. in KCN + Aq. Decomp. by warm NH 4 OH+A-. (Weith, Z. Ch. (2) 5. 381.) Silver ferrocyanide ammonia, Ag 4 Fe(CN) 6 , 2NH 3 +H 2 0. (Wyrouboff.) + 6H 2 O. (Gintl.) Sodium ferrocyanide, Na 4 Fe(CN) 6 +12H 2 O. Efflorescent. Less sol. in H 2 O than K 4 Fe(CN) 6 . Sol. in 4.5 pts. H 2 O at 12. (John.) 100 pts. H 2 O at 15.5 dissolve 22 pts. (Ure's Diet.) 100 pts. H 2 O dissolve at: 18 20 42 53 16.7 17.875 30.2 37.1 pts. Na 4 FeCN 6 , 58 60 77 80 41.7 42.5 54.8 59.2 pts. Na 4 FeCN 6 , 96 98 98.5 62.1 61.6 * 6. 30 pts. Na 4 FeCN 6 . (Conroy, J. Soc. Chem. Ind. 1898; 17. 104.) + 10H 2 O. 100 pts. H 2 O dissolve at: 18 20 42 29.45 31.85 58.5 pts. Na 4 Fe(CN) 6 + 10H 2 O, 53 58 60 75.9 88.4 90. 2 pts. Na 4 Fe(CN) 6 + 10H 2 O, 77 80 96 129.5 146.0157.0 pts. Na 4 Fe(CN) 6 + 10H 2 0, 98 98.5 156.5 161 .0 pts. Na 4 Fe(CN) 6 + 10H 2 O. (Conroy.) Strontium ferrocyanide, Sr 2 Fe(CN) 6 +15H 2 O. Efflorescent. Sol. in 2 pts. cold, and less than 1 pt. boiling H 2 O. (Bette.) Excessively sol. in H 2 O. (Wyrouboff, A. ch. (4) 16. 280.) +8H 2 O. (Wyrouboff.) Thallous ferrocyanide, Tl 4 Fe(CN) 6 +2H 2 O. 100 pts. H 2 O dissolve 0.37 pt. at 18, and 3.93 pts. at 101. (Lamy.) Sol. in KCN+Aq. (Kuhlmann.) Thorium ferrocyanide, ThFe(CN) 6 +4H 2 O. Ppt. (Cleve, Bull. Soc. (2) 24. 355.) Tin (stannous) ferrocyanide, Sn 2 Fe(CN) 6 + 4H 2 O. Insol. in H 2 O or acids; si. sol. in NH 4 OH + Aq. (Wyrouboff.) Tin (stannic) ferrocyanide, Sn 5 [Fe(CN) 6 ] 2 + 18^H 2 O (?). (Wyrouboff.) Titanium ferrocyanide, Ti 7 [Fe(CN) 6 ] 2 (?). Ppt. (Wyrouboff.) Uranium ferrocyanide, UFe(CN) 6 + 10H 2 O. Ppt. (Wyrouboff.) Vanadyl ferrocyanide, (VO) 2 Fe(CN) 6 + 11H 2 O. Ppt. (Atterberg.) Yttrium ferrocyanide, Y 4 [Fe(CN) 6 ] 3 . Easily sol. in H 2 O; insol. in alcohol. (Popp, A. 131. 179.) Zinc ferrocyanide, Zn 2 Fe(CN) 6 +3H 2 O. Insol. in H 2 O or acids. Insol. in HCl+Aq. (Lea, Sill. Am. J. (2) 31. 191.) Sol. in NH 4 OH, or NH 4 salts+Aq. (Witt- stein.) Insol. in NH 4 C1, or NH 4 NO+Aq. (Brett.) SI. sol. in boiling K 4 Fe(CN) 6 , or K 3 Fe(CN) 6 +Aq. (Gore.) Na 4 Fe(CN) 6 +NaCl+Aq sat. at 21 con- tains 29.0 g. NaCl and 5.8 g. Na 4 Fe(CN) 6 per 100 g. H 2 O; sat, at 90 it contains 24.7 g. NaCl and 21.3 g. Na 4 Fe(CN) 6 per 100 g. H 2 O. (Conroy, J. Soc. Chem. Ind. 1898, 17. 105.) Na 4 Fe(CN) 6 +Na 2 CO 3 +Aq sat. at 22 contains 22.6 g. Na 2 CO 3 and 6.5 g. Na 4 Fe(CN) 6 per 100 g. H 2 O; sat. at 95 it contains 29.8 g. Na 2 CO 3 and 36.8 g. Na 4 Fe(CN) 6 per 100 g. H 2 O. (Conroy.) Very si. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Insol. in alcohol. +4H 2 O. Absolutely insol. in H 2 O. (Wyrouboff, A. ch. (5) 8. 485.) +8H 2 O. (Weith, A. 147. 329.) + 10H 2 O. (Pebal, A. 233. 165.) Ferro^ranitrososulphydric acid, H 2 S 2 (NO) 4 Fe 2 . Insol. in H 2 O; si. sol. in alcohol; more easily in ether; very sol. in CS 2 or CHC1 3 . Not obtained in a pure state. (Pawel, B. 16. 2600.) Ethyl ferro^ranitrososulphide, (C 2 H 5 )S 2 (NO) 4 Fe 2 . Insol. in H 2 O, difficultly sol. in alcohol, more easily in ether, and very easily in CS 2 , CHC1,, C 2 H 5 I, or C 6 H 6 . (Pawel, B. 16. 2609.) Ferrous , FeS 2 (NO) 4 Fe 2 . More difficultly sol. in H 2 O and alcohol than the hepta salt. Sol. in ether. Potassium , K 2 S 2 (NO) 4 Fe 2 +4H 2 O. Sol. in H 2 O. Easily sol. in alcohol; insol. in ether. (Pawel, B. 16. 2600.) True composition of " nitrosulphide of 342 FERRONITROSOSULPHIDE, SODIUM iron and potassium" of Roussin. (A. ch. (3) 52. 297.) (Pawel, B. 13. 1949.) Sodium ferroteZranitrososulphide, Na 2 S 2 (NO) 4 Fe2+8H 2 O. Sol. in H 2 O; easily sol. in alcohol; insol. in ether. (Pawel.) True composition of "nitrosulphide of iron and sodium" of Roussin. (Pawel.) Thallium , Tl 2 S 2 (NO) 4 Fe 2 . Insol. in H 2 O, alcohol, or ether. (Pawel.) Ferro/iep/anitrososulphydric acid. HS 3 (NO) 7 Fe 4 . Insol. in H 2 O, alcohol, and ether. Easily sol. in CS 2 or CHC1 3 . (Pawel, B. 15. 2604.) May be called Ferrinitrososulphydric acid. Ammonium ferroAeptonitrososulphide, NH 4 S 3 (NO) 7 Fe 4 +H 2 O. Less easily sol. in H 2 than the K com- pound. (Pawel, B. 15. 2600.) "Binitrosulphide of iron" of Roussin. Sol. in about 2 pts. boiling H 2 O; very si. sol. in cold H 2 O. Very sol. in alcohols, methyl, ethyl, or amyl, and in HC 2 H 3 O 2 . Miscible with ether. Insol. in CS 2 or CHC1 3 . Decomp. by cone. HC1, HNO 3 , or H 2 SO 4 . Not attacked by H 2 C 2 O 4 , or H 2 C 4 H 4 O 6 + Aq. Insol. in NH 4 OH, and KOH+Aq. (Rous- sin, A. ch. (3) 52. 286.) Sol. in H 2 O. Insol. in alcohol. (Hofmann, Z. anorg. 1895, 9. 299.) Barium . Easily sol. in H 2 O. (Pawel.) Caesium , Fe 4 (NO) 7 S 3 Cs+H 2 O. Insol. in H 2 O. Difficultly sol. in alcohol and ether. (Pawel.) Sparingly sol. in H 2 O. (Hofmann, Z. anorg. 1895, 9. 298.) Calcium . Easily sol. in H 2 O. (Pawel.) Ferrous , Fe[S 3 (NO) 7 Fe 4 ] 2 +8H 2 O. More easily so], in H 2 O than Na salt. (Pawel.) Lead . Difficultly sol. in H 2 O. (Pawel.) Magnesium . Easily sol. in H 2 O. (Pawel.) Potassium , KS 3 (NO) 7 Fe 4 . Sol. in H 2 O, alcohol, and very sol. in ether with slight decomp. (Pawel, B. 15. 2600.) Rubidium feiroheptamtroso sulphide, RbS 3 (NO) 7 Fe 4 . Less soluble in H 2 O than the NH 4 salt. (Pawel.) +H 2 O. Ppt. (Hofmann, Z. anorg. 1895, 9.298.) Sodium , NaS 3 (NO) 7 Fe 4 +2H 2 O. More sol. in H 2 than the potassium salt. (Pawel.) Thallium , T1S 3 (NO) 7 Fe 4 +H 2 O. Very difficultly sol. in H 2 0. More easily sol. in alcohol. (Pawel.) (Hofmann, Z. anorg. 1895, 9. 297.) Ferrodinitrosothiosulphonic acid. Ammonium ferrodmitrosothiosulphonate, Fe(NO) 2 S 2 3 NH 4 +H 2 0. Can be cryst. from warm H 2 O without de- comp. (Hofmann, Z. anorg. 1895, 8. 321.) Caesium , Fe(NO) 2 S 2 O 3 Cs. Sparingly sol. in H 2 O. (Hofmann.) Potassium , Fe(NO) 2 S 2 O 3 K+H 2 O. SI. sol. in H 2 O without decomp. atT80. Sol. in 50% alcohol. Sol. in H 2 SO 4 without decomp. (Hof- mann) . Rubidium , Fe(NO) 2 S 2 O 3 Rb+H 2 0. Less sol. in H 2 O than the corresponding Na salt. (Hofmann.) Sodium , Fe(NO) 2 S 2 O 3 Na+2H 2 O. Closely resembles K salt, but is more sol. in H 2 O and alcohol. (Hofmann.) Ferrotungstic acid. Sol. in H 2 O. (Laurent, C. R. 31. 693.) Ammonium manganous ferrotungstate. 12(NH 4 ) 2 0, 6MnO, 2Fe 2 3 , 3H 2 O, 45W0 3 +81H 2 0. Sol. in H 2 O. (Laurent.) Barium ferrotungstate, 21BaO, 2Fe 2 O 3 , 45W0 3 +27H 2 0. Sol. in H 2 O. (Laurent.) Potassium ferrotungstate, 9K 2 O, 2Fe 2 O 3 , 12H 2 0, 45W0 3 +54H 2 0. Sol. in H 2 O. (Laurent.) 18K 2 O, 2Fe 2 3 , 3H 2 O, 45W0 3 +54H 2 O. (Laurent.) Ferrous acid. Barium ferrite, BaO, Fe 2 O 3 . Ppt. (List, B. 11. 1512.) FLUOBORIDE, CALCIUM 343 Calcium ferrite, 4CaQ, Fe 2 O 3 . Insol. in H 2 O, or sugar+H 2 O. Decomp. by the weakest acids, but not by boiling KOH+Aq. (Pelouze, A. ch. (3) 33. 5.) CaO, Fe 2 3 . (List.) 3CaO, Fe 2 O ? . Much less readily attacked by H 2 O and acids than the silicates. (Hilpert, B. 1909, 42. 4581.) 3CaO, 2Fe 2 O 3 . As above. (Hilpert, B. 1909, 42. 4581.) Calcium ferrite chloride, CaO, Fe 2 O 3 , CaCl 2 . Not decomp. by H 2 0. (Chatelier, C. R. 99. 276.) . Cupric ferrite, CuO, Fe 2 O 3 . Ppt. (List.) +5H 2 O. (List.) arge Fe 2 O 3 (?). Easily decomp. by HCl+Aq. Not com- pletely sol. in dil. HNO 3 +Aq. Easily sol. in cone. HN0 3 . Decomp. by acetic acid. (Rose, Pogg. 10. 323.) Magnesium ferrite, MgO, Fe 2 O 3 . Insol. in H 2 O. Not attacked by boiling cone. HNO 3 . (Deville. C. R. 52. 1264.) Min. Magnesioferrite. Difficultly sol. in HCl+Aq. (Rammelsberg, Pogg. 107. 451.) +4H 2 O. Ppt. (List, B. 11. 1512.) 6MgO, Fe 2 O 3 +9H 2 O. Ppt. +15H 2 O. Min. Pyroaurite. i Manganous ferrite, MnO, Fe 2 O 3 . .ir \ Ppt. (List.) Nickel ferrite, NiO, Fe 2 O 3 . Ppt. (List.) Potassium ferrite, 3K 2 O, 4Fe 2 O 3 . Decomp. by H 2 O, KOH+Aq, NaOH+Aq, etc., but only slowly by NH 4 Cl+Aq. (Salm- Horstmar, J. pr. 55. 349.) K 2 Fe 2 O 4 . Decomp. by H 2 O. (Rousseau and Bernheim, C. R. 107. 240.) Silver (argentous) ferrite, Ag 4 O, Fe 2 O 3 (?). Decomp. by dil. HNO 3 +Aq. (Rose, Pogg. 10. 323.) Sodium ferrite, Na 2 O, Fe 2 O 3 . Na 2 O is dissolved out by H 2 O. Easily sol. in dil. HCl+Aq. Not easily decomp. by NH 4 Cl+Aq. (Salm-Horstmar.) Zinc ferrite, ZnO, Fe 2 O 3 . Sol. in boiling cone. HCl+Aq. (Ebel- men, A. ch. (3)33.47.) Min. Franklinite. Flavocobaltic compounds. See also Xanthocobaltic compounds. Flavocobaltic chloraurate, (NO 2 ) 2 Co(NH 3 ) 4 AuCl 4 . More easily sol. than the chloroplatinate. Not wholly insol. in absolute alcohol. (Jb'r- gensen, Z. anorg. 6. 159.) chloroplatinate, [(NO 2 ) 2 Co(NH 3 ) 4 ] 2 PtCl 6 As the chloroplatinite. (Jorgensen.) chloroplatinite, [(NO 2 ) 2 Co(NH 3 ) 4 ] 2 PtCl 4 . Somewhat sol. in H 2 O, and not insol. in 50% alcohol. (Jorgensen.) chromate, [(N0 2 ) 2 Co(NH 3 ) 4 ]2Cr 2 07. Ppt. (Jorgensen.) nitrate, Co(NO 2 ) 2 (NH 3 ) 4 NO 3 . Sol. in about 33 pts. cold H 2 O; insol. in HNO 3 . (Jorgensen.) Co(NO 2 ) 2 (NH 3 ) 4 NO 3 , HNO 3 . Decomp. by H 2 O or alcohol. (Jorgensen.) cobaltic nitrite, 3(NO 2 ) 2 Co(NH 3 ) 4 , Co 2 (N0 2 ) 6 +2H 2 0. SI. sol. in H 2 O. (Jorgensen, Z. anorg. 5. 179.) diamine cobaltic nitrite, (N0 2 ) 2 Co(NH 3 ) 4 , (N0 2 ) 2 (NH 3 ) 2 Co(N0 2 ) 2 . Very si. sol. in H 2 O. (Jorgensen.) sulphate, [(N0 2 ) 2 Co(NH 3 ) 4 ] 2 S0 4 . SI. sol. in H 2 O, more easily in HC 2 H 8 2 + Aq. (Jorgensen.) Fluoborhydric acid, HBF 4 . Decomp. by H 2 O very rapidly. (Landolph, C. R. 86. 603.) Aluminum fluoboride, 2A1F 3 , 3BF 8 . Sol. in H 2 O only when acidulated; sol. in acids. (Berzelius.) Ammonium fluoboride, NH 4 BF 4 . Easily sol. in H 2 O. Sol. in 4 pts. H 2 O at 16, and 1.02-1.05 pts. boiling H 2 O. (Stolba, Chem. techn. Cent. Anz. 7. 459.) SI. sol. in alcohol. Barium fluoboride, Ba(BF 4 ) 2 +2H 2 O. Deliquescent; easily sol. in H 2 0; decomp. by alcohol. (Berzelius.) Caesium fluoboride, CsBF 4 . 100 pts. H 2 O dissolve 0.92 pt. CsBF 4 at 20, and 0.04 pt. at 100. (Godeffroy, B. 9. 1367.) 0.02 pts. are sol. in 100 pts. H 2 O at 20. (Erdmann, Arch. Pharm. 1894, 232. 21.) Calcium fluoboride, Ca(BF 4 ) 2 . Decomp. by H 2 O, with formation of a sol. acid salt and an insol. basic salt. (Berzelius.) 344 FLUOBORIDE, CUPBIC Cupric fluoboride, Cu(BF 4 ) 2 . Deliquescent, and very sol. in H 2 O. (Ber- zelius.) Lead fluoboride, Pb(BF 4 ) 2 . Sol. in H 2 O. Decomp. by boiling with H 2 O or alcohol into an acid soluble, and a basic insoluble salt. (Berzelius.) Lithium fluoboride, LiBF 4 . Hygroscopic. Easily sol. in H 2 O. (Ber- zelius.) Magnesium fluoboride. Easily sol. in H 2 O. (Berzelius.) Potassium fluoboride, KBF 4 . Sol. in 223 pts. H 2 O at 20. (Stolba.) Sol. in 70.4 pts. cold H 2 O. (Berzelius.) Sol. in 15.94 pts. H 2 O at 100. (Stolba.) 1.43 pts. are sol. in 100 pts. H 2 O at 20. (Erdmann, Arch. Pharm. 1894, 232. 21.) Not more sol. in NH 4 OH+Aq than in H 2 O; sol', in hot KOH, NaOH, or M 2 CO 3 +Aq. (Berzelius.) More sol. in NH 4 Cl+Aq. (Rose, Pogg. 80. 276.) Insol. in 20% KC 2 H 3 O 2 +Aq. (Stromeyer.) Insol. in cold, si. sol. in boiling alcohol. Rubidium fluoboride, RbBF 4 . 100 pts. H 2 O dissolve 0.55 pt. at 20, and 1.0 pt. at 100. (Godeffroy, B. 9. 1337.) 0.55 pts. are sol. in 100 pts. H 2 O at 20. (Erdmann, Arch. Pharm. 1894, 232. 21.) Sodium fluoboride, NaBF 4 . Easily sol. in H 2 0. Very si. sol. in alcohol. (Berzelius.) Yttrium fluoboride. Sol. in H 2 O with excess of acid. (Berze- lius.) Zinc fluoboride, Zn(BF 4 ) 2 . Deliquescent. Sol. in H 2 0. (Berzelius.) Fluoboric acid, HBF 4 . See Fluoborhydric acid. H 4 B 2 O 7 , 3HF and H 4 B 2 O 9 , 2HF (?). Fume on air, and are decomp. with H 2 O. (Lan- dolph, B. 12. 1583.) HBO 2 , 3HF. Decomp. by H 2 O. (Ber- zelius, Pogg. 69. 644.) Is either a mixture, or a solution of HB0 2 in HF, and is decomp. by distillation, and the salts are decomp. by recrystallisation. (Bas- arow, C. R. 78. 1698.) Potassium fluoborate, K 2 B 2 3 F 2 (?). SI. deliquescent. Scarcely sol. in boiling alcohol. (Schiff, A. Suppl. 6. 175.) See Boron fn'oxide potassium fluoride, B 2 3 , 2KF. Fluochromic acid. Ammonium fluochromate, NH 4 CrO 3 F. Sol. in H 2 0. (Varenne, C. R. 91. 989.) Potassium fluochromate, KCrO 3 F. Efflorescent. Sol. in H 2 O, with gradual decomp. (Streng, A. 129. 225.) Fluocolumbic acid. See also Fluoxycolumbic acid. Ammonium fluocolumbate fluoxycolumbate, (NH 4 ) 2 CbF 3 , 2CbOF 3 , NH 4 F. Cadmium fluocolumbate, Cd 5 H 5 Cb 3 F 30 + 28H 2 0. Insol. in, and decomp. by H 2 O. (Streng.) Cobalt fluocolumbate, Co 5 H 5 Cb 3 F 33 +28H 2 O. Insol. in, and decomp. by H 2 O. (Streng.) Copper fluocolumbate, Cu 2 HCbFi +9H 2 O. Insol. in, and decomp. by H 2 O. Ferrous fluocolumbate, Fe 3 H 4 Cb 2 F 20 +19H 2 O. As above. Manganous fluocolumbate, Mn 5 H 5 Cb 3 F 3 o+ 28H 2 O. Mercuric fluocolumbate, Hg 3 CbFn+8H 2 O. As above. Nickel fluocolumbate, Ni 3 H 4 Cb 2 F 20 +19H 2 O. As above. Potassium fluocolumbate, K 2 CbF 7 . Decomp. by solution in H 2 O. (Marignac A. ch. (4) 8. 34.) Rubidium fluocolumbate, Rb 2 CbF 7 . Sol. in H 2 O and HF+Aq. Insol. in al- cohol. (Pennington, J. Am. Chem. Soc. 1896, 18. 58.) Zinc fluocolumbate, Zn 5 H 5 Cb3F 3 o+28H 2 0. Insol. in cold H 2 O; decomp. by hot H 8 0. (Santesson, Bull. Soc. (2) 24. 52.) Fluodithionic acid. Caesium wonofluodithionate, S 2 O 5 (OH)FCs 2 +H 2 O. Easily sol. in H 2 O with decomp. Sol. in HF; very unstable. (Weinland, Z. anorg. 1899, 21. 66.) Potassium difluodithionate, S 2 O 5 F 2 K 2 +3H 2 O. Easily sol. in H 2 O with decomp. Sol. in HF; very unstable. (Weinland.) FLUOPERBORATE, POTASSIUM 345 Rubidium cfcfluodithionate, S 2 O 5 F 2 Rb 2 + 3H 2 0. Easily sol. in H 2 O with decomp. Sol. in HF; very unstable. (Weinland.) Fluogermanic acid, H 2 GeF 6 . Known only in solution. (Winkler, J. pr. (2) 36. 177.) Potassium fluogermanate, K 2 GeF 6 . Sol. in 173.98 pts. H 2 O at 18. (Winkler.) Sol. in 184.61 pts. H 2 at 18. (Kriiss and Nilson, B. 20. 1696.) Sol. in 34.07 pts. H 2 O at 100. (Winkler.) Sol. in 38.76 pts. H 2 O at 100. (Kriiss and Nilson.) Insol. in alcohol. IH'fluoiodic acid. Ammonium cfa'fluoiodate, NH 4 IO 2 F 2 . Like K salt. Sol. in 40% HF+Aq. (Weinland, Z. anorg. 1899, 20. 30.) Sol. in H 2 O. Easily decomp. (Weinland, B. 1897,30.868.) Caesium cftfluoiodate, CsIO 2 F 2 . (Weinland, Z. anorg. 1899, 20. 36.) Caesium hydrogen c&fluoiodate. CsI0 2 F 2 , HI0 2 F 2 +2H 2 0. Efflorescent. Sol. in H 2 O with decomp. (Weinland, Z. anorg. 1899, 22. 257.) Potassium dzfluoiodate, KI0 2 F 2 . Sol. in H 2 0. Decomp. in moist air. (Weinland, B. 1897, 30. 867. Decomp. in air. Sol. in H 2 O with decomp. Sol. without decomp. in 40% HF+Aq. (Weinland, Z. anorg. 1899, 20. 31. Rubidium cftfluoiodate, RbIO 2 F 2 . Resembles K salt. Sol. in (Weinland, Z. anorg. 1899, 20. 35.) Rubidium hydrogen cfc'fluoiodate, RbIO 2 F 2 ,HIO 2 F 2 +2H 2 O. Sol. in 40-60% HF+Aq. (Weinland, Z. anorg. 1899, 22. 260.) Sodium (ftfluoiodate, NaIO 2 F 2 . Decomp. by H 2 O. (Weinland, B. 1897, 30. 868.) Sol. in HF. (Weinland, Z. anorg. 1899, 20. 37.) Fluomanganic acid, H 2 MnF 6 . Decomp. by H 2 O. Sol. in alcohol and ether in absence of H 2 O. (Nickles, C. R. 66. 107.) Ammonium fluomanganate, (NH 4 ) 2 MnF 6 . More sol. than the K salt. (Nickles, C. R. 65. 107.) True composition is (NH 4 ) 4 Mn 2 Fi = 4NH 4 F, Mn 2 F 6 . (Christensen, J. pr. (2) 34. 41.) Cobalt fluomanganate, 2CoF 2 , Mn 2 F 6 + 8H 2 O. Sol. in H 2 O. (Christensen.) Nickel fluomanganate, 2NiF 2 , Mn 2 F 6 + 8H 2 O. Sol. in H 2 O. (Christensen.) Potassium fluomanganate, K 2 MnF 6 . Difficultly sol. in H 2 O. Decomp. bv much H 2 O. (Nickles, C. R. 65. 107.) Composition is K 4 Mn 2 F 10 = 4KF, Mn 2 F 6 . Also with 2H 2 O. (Christensen, J. pr. (2) 34. 41.) Decomp. by H 2 O. Sol. in HC1, H 2 SO 4 and HNO 3 with decomp. Can be recryst. from 40% HF+Aq. Insol. in acetic acid. (Wein- land and Lauenstein, Z. anorg. 1899, 20. 41.) Rubidium fluomanganate, Rb 2 MnF 6 +2H 2 O. As the K salt. (Weinland and Lauenstein. Z. anorg. 1899, 20. 44.) Silver fluomanganate, Ag 2 Mn 2 F 8 +14H 2 O. (Christensen, J. pr. (2) 34. 41.) Sodium fluomanganate, 4NaF, Mn 2 F 6 . Decomp. by much H 2 O. (Christensen.) Zinc fluomanganate, 2ZnF 2 , Mn 2 F 6 +8H 2 O. Sol. in H 2 O. (Christensen.) Fluomolybdic acid. See Fluoxyhypomolybdic, and Fluoxymolyb- dic acids. Fluopalladous acid. Potassium fluopalladite, SI. sol. in H 2 O. Sodium fluopalladite. SI. sol. in H 2 O. (Berzelius.) Fluoperboric acid. Ammonium fluoperborate, NH 4 OOB(F)OOB(F)OONH 4 . Ppt. Insol in ether. (Petrenko, C. C. 1902, I. 1191.) Potassium fluoperborate, K 4 B 4 F 4 On+H 2 O. Dry salt is rather stable. Easily sol. in H 2 O. Aqueous solution decomp. rapidly when warmed; at ordinary 346 FLUOPERURANIC ACID temp, the decomp. proceeds slowly. Insol. in alcohol. (Melikoff, B. 1899, 32. 3350. KOOB(F)OOB(F)OK + 13^H 2 O. Ppt. Insol. in ether. (Petrenko, C. C. 1902, I. 1191; J. Russ, phys. chem. Soc. 34. 37.) Fluopemranic acid. Potassium fluoperuranate, K 4 U 4 F fi Oi 5 + 4H 2 0=3U0 4 KF, U0 3 F 2 , KF+4H 2 0. Ppt. (Lordkipanidse, C. C. 1900, II. 525. Sodium fluoperuranate, U0 4 NaF+5H 2 O. Ppt. (Lordkipanidse, C. C. 1900, II. 525.) Fluophosphamide, PF 3 (NH 2 ) 2 . Sol. in H 2 O. (Poulenc, A. ch. (6) 24. 566.) Fluophosphoric acid. Monoc&sium wowofluophosphate, P(OH) 3 (OCs)F. Like the K salt. (Weinland, Z. anorg. 1899, 21. 48.) Mowopotassium wonofluophosphate, P(OH) 3 (OK)F. Sol. in 40% HF+Aq; decomp. in the air. (Weinland, Z. anorg. 1899, 21. 44.) Potassium wowofluophosphate, KHF.PO 3 +H 2 O. Decomp. by H 2 O; unstable. (Weinland, B. 1898, 31. 124-125.) Moworubidium wonofluophosphate, P(OH) 3 (ORb)F. Sol. in 40% HF+Aq. (Weinland, Z. anorg. 1899, 21. 47.) Rubidium raonofluophosphate, RbHFPO 3 +H 2 O. Decomp. by H 2 O. (Weinland, B. 1898, 31. 124.) Fluoplatinic acid. Ammonium fluoplatinate. Secomp. by H 2 O to a sol. acid, and an insol. basic salt. Insol. in alcohol. (Berzelius.) Potassium fluoplatinate. Deliquescent. Insol. in alcohol. Decomp. by H 2 O. (Berzelius.) Sodium fluoplatinate. Decomp. by H 2 O. (Berzelius.) Fluor- and Fluoro-. See Fluo-. Fluorhydric (Hydrofluoric) acid, HF or H 2 F 2 . Attracts H 2 O from air with great avidity. Very sol. in H 2 O with evolution of much heat. Sat. solution has sp. gr. 1.25. (H. Davy.) On boiling the aqueous solution an acid of constant composition is obtained, which boils at 120, has sp. gr. 1.15, and contains 35.37% HF (Bineau, A. ch. (3) 7. 257.) The residual acid after boiling contains 36 to 38% HF, and by standing over CaO gives off HF until an acid containing 32.5 to 32.7% HF is formed. Weaker acids increase their strength to 32.2 to 32.4% HF, while an acid containing 32.5% HF remains unchanged. (Roscoe, A. 116. 218.) Does not attack gutta-percha. Sol. in H 2 S0 4 . Sp. gr. of HF+Aq at 15. Sp. gr. % HF Sp. gr. %HF Sp. gr. % HF 1.01 2.90 1.10 29.00 1.19 55.10 1.02 5.80 1.11 31.90 1.20 58.00 1.03 8.70 1.12 34.80 1.21 60.90 1.04 11.60 1.13 37.70 1.22 63.80 1.05 14.50 1.14 40.60 1.23 66.70 1.06 17.40 1.15 43.50 1.24 69.60 1.07 20.30 1.16 46.40 1.25 72.50 1.08 23.20 1.17 49.30 1.09 26.10 1.18 52.20 (Hart, J. Anal. Ch. 3. 372.) Sp. gr. of HF+Aq at ord. temp. Deg. Baum6 Sp. gr. % HF 1 1.0069 2.32 2 1.0139 4.04 3 1.0211 5.76 4 1 . 0283 7.48 5 1 . 0356 9.20 6 1 . 0431 10.92 7 1 . 0508 12.48 8 1 . 0583 14.04 9 1.0661 15.59 10 1.074 17.15 11 1.082 18.86 12 .0901 21.64 13 .0983 24.42 14 .1067 27.20 15 .1152 29.98 16 .1239 32.78 17 .1326 35.15 18 .1415 37.53 19 .1506 39.91 20 .1598 42.29 21 .1691 44.67 22 .1786 47.04 23 .1883 49.42 24 .1981 51 . 57 25 .2080 53.72 26 .2182 55.87 27 .2285 58.02 FLUOSELENATE, RUBIDIUM 347 Sp. gr. of HF+Aq at ord. temp. Continued. Aq. solution of sp. gr. 1.138 at 18 contains 43.2% HF and has a constant bpt. of 111 Deg. Baum6 Sp. gr. % HF at 750 mm. (Deussen, Z. anorg. 1906, 49. 28 29 30 31 1.2390 1.2497 1 . 2605 1.2716 60.17 62.32 64.47 66.61 297.) The strongest acid that can be obtained by distillation contains 48.17% HF and boils at 125-125.5. (Gore.) 32 1 . 2828 68.76 33 1.2943 70.91 Fluorides. 34 35 36 37 38 1.3059 1.3177 1.3298 1 . 3421 1.3546 73.06 75.21 77.36 79.51 81.66 The alkali fluorides, also AgF and SnF 2 , are sol. in H 2 O; the fluorides of Fe, Sr, and Cd are si. sol.; the others are insol. in H 2 O. Most fluorides are sol. in acids, especially HF i \ n 39 40 1.3674 1 . 3804 83.81 85.96 +Aq. Insol. in liquid NHs. (Franklin, Am. Ch. T 18Q8 20 892 ") 41 1 . 3937 88.10 tl . J.Ot7Oj *iw '^i-j.J See under each element. 42 1 . 4072 90.24 43 1.4211 92.39 44 1 . 4350 94.54 Fluorine, F 2 . 45 1 . 4493 96.69 J Decomposes H 2 O and all organic solvent (Eckelt, Ch. Z. 1898, 22. 225.) with great violence. (Moissan, C. R. 103. 202 and 256.) Sp. gr. of HF+Aq at 0. Liquified at 185 to a yellowish liquid which does not dissolve glass nor ignite cooled % HF Sp. gr. % HF Sp. gr. Si, B, C, S, P, or Fe. (Moissan, C. R. 1897, 0.484 1.005 71.73 1.262 124. 1202-1204.) 1.504 1.009 72.21 1.260 2.48 1.012 78.05 1.260 Fluomolybdic acid. 4.80 1.017 84.27 1.235 7.75 15.85 1.035 .065 87.72 88.11 1.212 1.210 Ammonium fluomolybdate, (NH 4 )MoF 4 + 24.47 .097 88.82 1.207 l 2 vy. 28 48 110 89 02 1 202 Somewhat more sol. in H 2 O thau the K salt. 29.83 .120 89.15 1.200 Hydrolysed by H 2 O. (Rosenheim, Z. anorg. 34.23 38.50 .130 1.145 89.82 90.20 1.190 1.185 1905, 46. 321.) (NH 4 ) 3 Mo 2 F 9 +2H 2 O. (Rosenheim.) 41.00 1.155 90.64 .175 41.15 41.92 47.52 1.155 1.157 1.182 91.04 92.09 92.81 .165 .152 .135 Potassium fluomolybdate, KMoF 4 +H 2 O. Nearly insol. in H 2 O. (Rosenheim.) 48.49 1.187 92.91 .130 50.97 55.09 1.200 1.217 94.26 95.84 1.095 1.065 Fluoselenic acid. 55.39 1.220 97.50 1.035 57.66 1.230 98.22 1.022 Ammonium monofluoselenate, 61.66 1.245 100.05 1.0005 Se0 3 (OH)F(NH 4 ) 2 . 65.19 1.255 Not hygroscopic. Easily sol. H 2 O with decomp. Sol. in HF. (Weinland, Z. anorg. 1899, 21. (Hill, Roy. Soc. Proc. 1909, 83. A. 144.) Sp. gr. of HF+Aq at 18. 58.) % HF Sp. gr. rnpotassium difluocftselenate, Se 2 O 7 F 2 K 3 H + 484 1.003 H 2 O. 1 504 005 Decomp. in the ajr; sol. in H 2 O with de- 2^48 ^009 comp.; sol. in HF. (Weinland.) 4.80 .017 7.75 15.85 .028 .058 Tn'rubidium cfofluocftselenate, Se 2 O 7 F 2 Rb 3 H 24.4' r .087 i"Xi 2 L/. 29 '. 83 103 Decomp. in the air; sol. in H 2 O with de- comp.; sol. in HF. (Weinland, Z. anorg. (Hill.) 1899, 21. 57.) 348 FLUOSILICIC ACID Fluosilicic acid, H 2 SiF 6 . Sp. gr. of H 2 SiF 6 +Aq at 17.5 (H 2 O at 17.5 = 1.000). 1 pt. BaSiF 6 dissolves in 306 pts. sat. NH 4 Cl+Aq at 22; in 361 pts. 15% solution of NF 4 C1; in 563 pts. sat. boiling NaCl+Aq; in 349 pts. 10% solution of NaCl at boiling temp.; in 2185 pts. 10% solution of NaCl at 20; in 1140 pts. 5% solution of NaCl at 20. (Stolba.) Nearly absolutely insol. in alcohol. (Fre- senius.) Solubility in a mixture of H 2 O, alcohol (96%). HCl+Aq (20%), H 2 SiF 6 +Aq (3.7%). 1 pt. BaSiFc is sol. in pts. of solutions of given composition. % H 2 SiF 6 Sp. gr. % H 2 SiF 6 Sp. gr. 2 4 6 8 10 12 14 16 18 1.0161 1.0324 1.0491 1 . 0661 1 . 0834 1.1011 1.1190 1.1373 1.1559 20 22 24 26 28 30 32 34 1.1748 1.1941 .2136 .2335 .2537 .2742 .2951 .3162 H 2 Alcohol HCl+Aq H 2 SiF 6 +Aq BaSiFe (Stolba, J. pr. 90. 193.) +2H 2 O. Very deliquescent, and sol. in H 2 O. (Kessler, C. R. 90. 1285.) Solution decomp. into HF and SiF 4 on evaporation, when it becomes concentrated. Fluosilicates. Most of the fluosilicates are sol. in H 2 0, but the alkali salts (especially K) and the Ba salt are only si. sol. in H 2 O. 50 74.1 70.8 77.95 73.0 97.09 75.0 50 25 25 20 25 25 0.9 4.2 0.9 0.9 1.25 1.15 1.1 1.66 37,219 5,263 2,860 39,061 70,679 3,247 16,914 (Fresenius, Z. anal. 29. 143.) Aluminum fluosilicate, Al 2 (SiF 6 ) 3 . Easily sol. in H2O. After evaporating to dryness, the residue is slowly but completely sol. in H 2 O. (Deyille, A. ch. (3) 61. 327.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) Aluminum fluosilicate silicate, Al 2 SiFi , 5AI 2 Si0 5 . Min. Topaz. Insol, in acids. Ammonium fluosilicate, (NH 4 ) 2 SiF 6 . Sol. in 5.38 pts. H 2 O at 17.5 to form a solu- tion of 1.0961 sp. gr.; sol. in 1.8 pts. hot H 2 0; sol. in 45.5 pts. alcohol of 31%. (Stolba, C. C. 1877. 418.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) 3NH 4 F, SiF 4 = (NH 4 ) 2 SiI 6 , NH 4 F. Sol. in H 2 O. (Marignac, Ann. Min. (5) 15. 221.) Barium fluosilicate, BaSiF 6 . Sol. in 3802 pts. cold H 2 O. (Fresenius, A. 59. 120.) Sol. in 3731 pts. H 2 O at 17.5; in 3315 pts. at 21; in 1175 pts. at 100. (Stolba, J. pr. 96. 22.) Sol. in 640-733 pts. H 2 containing a little HC1. (Fresenius.) 488 pts. HCl+Aq containing 4.25% HC1 dissolve 1 pt. at 22. (Stolba.) More sol. in HNO 3 +Aq than in H 2 O. (Fresenius.) 272 pts. HNO 3 +Aq, containing 8% N 2 O 5 , dissolve 1 pt. at 22. (Stolba.) 1 pt. BaSiF 6 dissolves in 428 pts. sat. NH 4 Cl+Aq; in 589 pts. sat. NH 4 Cl+Aq + 2 vols. H 2 O. (Mallet, Sill. Am. J. (2) 28. 48.) Cadmium fluosilicate, CdSiF 6 +6H 2 O. Extremely sol. in H 2 O. Easily sol. in 50% alcohol. (Engelskirchen, Dissert. 1903.) Caesium fluosilicate, Cs 2 SiF 6 . Sol. in 166 pts. H 2 O at 17, and much less h2t H 2 O. Insol. in alcohol. (Preis, J. pr. 103. 410.) Calcium fluosilicate, CaSiF 6 +2H 2 0. SI. sol. in, and partly decomp. by H 2 O. Sol. in HF and HCl+Aq. Sol. in fluosilicic acid without decomp. Easily sol. in 60% alcohol. (Fleischer.) Cerium fluosilicate. Very difficulty sol. in H 2 O, acetic, or fluo- silicic acids. Insol. in alcohol. (Stolba, C. C. 1874. 130.) Chromium fluosilicate. Deliquescent. (Berzelius.) Efflorescent. Sol. in H 2 0. (Berlin.) Cobaltous fluosilicate, CoSiF 6 +6H 2 O. Easily sol. in H 2 0. (Berzelius.) Cuprous fluosilicate, Cu 2 SiF 6 . Insol. in H 2 O. (Berzelius, Pogg. 1. 199.) Cupric fluosilicate, CuSiF 6 +6H 2 O. Deliquescent in moist, efflorescent in dry air. Sol. in 0.428 pt. H 2 O at 17. Sp. gr. of solution sat. at 17 = 1.6241. Sol. in 17.5 pts. alcohol of 62 vol. % at 20; in 150 pts. of 85% at 20; in 617 pts. of 92% at 20. (Stolba, J. pr. 102. 7.) FLUOSILICATE, POTASSIUM 349 Insol. in methyl acetate. (Naumann, B, 1909, 42. 3790.) Contains 1 A H 2 O. (Stolba.) +5^H 2 O. (Knop and Wolf.) Cupric fluosilicate phosphate, CuSiF 6 , Cu 3 (P0 4 ) 2 . Insol. in H 2 O, but easily sol. in dil. HC1 + Aq. (Thorpe and Rodger, Chem. Soc. 65. 320.) Glucinum fluosilicate. Known only in solution. Iron (ferrous) fluosilicate, FeSiF 6 +6H 2 0. Easily sol. in H 2 O. (Berzelius.) Iron (ferric) fluosilicate, Fe 2 (SiF 6 ) 3 . Sol. in H 2 O. (Berzelius.) Lead fluosilicate, PbSiF 6 +2H 2 O. Deliquescent. Easily sol. in H 2 O. Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +4H 2 O. (Marignac.) Lithium fluosilicate, Li 2 SiF 6 +2H 2 O. 100 pts. H 2 O at 17 dissolve 73 pts. crystal- line salt. (Marignac.) 100 pts. cold H 2 O dissolve 52.6 pts. crystals. Sol. in dil. alcohol. (Stolba, J. pr. 91. 456.) 100 pts. alcohol of 46 vol. % dissolve about 4 pts., and 100 pts. alcohol of 79 vol. % dis- solve about 0.4 pt. crystals. (Stolba, Z. anal. 3. 311.) Insol. in ether or benzene. Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1904,37.3601.)" Magnesium fluosilicate, MgSiF 6 +6H 2 O. Efflorescent. Sol. in 1534 pts. cold H 2 O, forming a solution of 1.235 sp. gr. at 17.5. Separates out SiO 2 on warming, which nearly all redissolves on cooling. (Stolba, C. C. 1877. 578.) Magnesium fluosilicate silicate, Mg 5 Si 2 Fi 8 , .TMg 5 Si 2 9 . Min. Humite; Chondrodite. Gelatinises with HC1, or H 2 SO 4 +Aq. Manganous fluosilicate, MnSiF 6 +6H 2 O. Sol. in H 2 O. (Marignac, J. pr. 83. 202.) 100 pts. dissolve in 71.4 pts. H 2 O at 17.5, and sp. gr. of solution = 1.44825. Much more sol. in hot H 2 O, and less sol. in alcohol, the stronger the alcohol. (Stolba, C. C. 1883. 292.) Mercurous fluosilicate, Hg 2 SiF 6 . SI. sol. in H 2 O without decomp. (Lemaire, C. C. 1897, I. 1046.) +2H 2 0. SI. sol. in H 2 O. More easily sol. in acidified H 2 O, but precipitated by HC1 + Aq. (Berzelius.) Mercuric fluosilicate, basic, HgSiF 6 , HgO + 3H 2 O. Decomp. by H 2 O, but sol. in weakest acids- (Berzelius, Pogg. 1. 200.) Mercuric fluosilicate, HgSiF 6 +6H 2 O. Deliquescent, and easily sol. in H 2 0. (Finkener, Pogg. 111. 246.) Nickel fluosilicate, NiSiF 6 +6H 2 O. Easily sol. in H 2 O. (Marignac, Ann. Min. (5) 16. 262.) Potassium fluosilicate, K 2 SiF 6 . Sol. in 833.1 pts. H 2 O at 17.5, and 104.8 pts. at 100. (Stolba, J. pr. 103. 396.) Sol. in 3800 pts. cold, and more easily sol. in hot H 2 O. (Fresenius.) More sol. in HCl+Aq than in H 2 O. Sol. in 337 pts. HCl+Aq of 26.5% at 14; in 307 pts. of 25.7% at 15; in 340 pts. of 14.1 % at 14; in 303 pts. of 13.6% at 15; in 327 pts. of 9.6% at 14; in 313 pts. of 9.2% at 15; in 376 pts. of 2.7% at 14; in 319 pts. of 2.4% at 15; in 409 pts. of 1.8% at 14. (Stolba, 1. c.) Sol. in 428 pts. sat., and 589 pts. dil. NH 4 Cl+Aq. (Mallet.) Much less sol. in K 2 SO 4 , KNO 3 , or KC1+ Aq, but more sol. in NH 4 Cl+Aq than in H 2 O. (Stolba.) Sol. in 24,066 pts. K 2 SO 4 +Aq containing 9.92% K 2 SO 4 at 17; in 17,858 p!s. containing 6% at 18; in 19,530 pts. containing 5% at 17; in 10,721 pts. containing 1% at 17. Sol. in 125,000 pts. KNO 3 +Aq containing 18.4% KNO 3 at 15; in 43,478 pts. containing 8.7% at 15; in 1735 pts. containing 8.8% at 100; in 35,814 pts. containing 4.3% at 15; in 10,203 pts. containing 1.00% at 15. Sol. in 40,070 pts. KCl+Aq containing 25% KC1 at 17; in 38,352 pts. containing 18.4% at 17; in 41,254 pts. containing 13.4% at 14; in 24,032 pts. containing 6.7% at 12; in 1200 pts. containing 0.65% at 17; in 1095 pts. containing 0.45% at 18. Sol. in 358 pts. NH 4 Cl+Aq containing 26.3 %NH 4 C1 at 17; in 306 pts. containing 15% at 15; in 339 pts. containing 10% at 15; in 436 pts. containing 5% at 15. (Stolba, J. pr. 103. 306.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Insol. in liquid NH 3 . (Gore, Am. ch. J. 1898, 20. 829.) Completely pptd. from aqueous solution by an equal vol. of alcohol. 350 FLUOSILICATE, RUBIDIUM SI. sol. in benzbnitrile. 1914, 47. 1369.) Insol. in methyl acetate. 1909, 42. 3790.) (Naumann, B. (Naumann, B. Rubidium fluosilicate, Rb 2 SiF 6 . Sol. in 625 pts. H 2 O at 20, and 73.05-74.5 pts. at 100. More sol. in acidified water. Insol. in alcohol. (Stolba, J. pr. 101. 1.) Insol. in H 2 O. (Eggeling, Z. anorg. 1905, 46. 175.) Less sol. in H 2 O than K 2 SiF 6 . (Gossner, Zeit. Kryst. 1904, 38. 149.) Silver fluosilicate, Ag 2 SiF 6 +4H 2 O. Deliquescent. Easily sol. in H 2 O. (Marig- nac, Ann. Min. (5) 15. 221.) Sodium fluosilicate, Na 2 SiF 6 . Much more sol. in H 2 O than K 2 SiF 6 , es- pecially in hot H 2 O. Addition of acid does not increase solubility. (Berzelius.) Sol. in 153.3 pts. H 2 O at 17.5, and 40.66 pts. at 100. Easily forms supersaturated solutions. (Stolba, Z. anal. 11. 199.) Much less sol. in NaCl+Aq than in H 2 O. (Stolba, J. pr. 1865 (1) 96. 26.) Precipitated completely from aqueous solu- tion by alcohol. (Rose.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Strontium fluosilicate, SrSiF 6 +2H 2 O. Sol. in cold H 2 O, but decomp. somewhat on heating. Sol. in 31.06 pts. H 2 O. (Fresenius.) Easily sol. in acidified H 2 O without de- comp. Sol. in alcohol. Solubility in a mixture of H 2 O, alcohol (96%), HCl+Aq (20%), H 2 SiF 6 +Aq (3.7%). 1 pt. SrSiF is sol. in pts. of solutions of given composition. H 2 Alcohol HCl+Aq H 2 SiF 6 +Aq SrSiFa 50 50 15.29 74.1 25 82.93 70.8 25 4.2 50.9 77.95 20 0.9 1.15 55.0 73 25 0.9 1.1 82.97 75 25 147.4 95.24 2.04 2.72 7.3 (Fresenius, Z. anal. 29. 143.) Thallous fluosilicate, Tl 2 SiF 6 -f-2H 2 O. Very easily sol. in H 2 O. (Kuhlmann.) Thorium fluosilicate, Th(OH) 2 SiF 6 (?). (Cleve.) Tin (stannic) fluosilicate, SnF 4 , SiF 4 . Very easily sol. in H 2 O. (Berzelius.) Uranyl fluosilicate. Very si. sol. in acids. (Berzelius.) Sol. in alcohol. (Stolba, Z. anal. 3. 71.) Vanadium fluosilicate. Deliquescent. Sol. in H 2 O. (Guyard, Bull. Soc. (2) 25. 352.) Yttrium fluosilicate. Insol. in pure, sol. in acidified H 2 O. (Berzelius.) Zinc fluosilicate, ZnSiF 6 +6H 2 O. Very easily sol. in H 2 O. (Berzelius.) Zirconium fluosilicate. Sol. in H 2 O. Solution clouds up on boiling. (Berzelius.) Fluostannic acid. Ammonium fluostannate, (NH 4 ) 2 SnF 6 . Sol. in H 2 O. (Marignac, Ann. Min. (5) 15. 224.) 4NH 4 F,SnF 4 . Sol. in H 2 O. (Marignac.) Barium fluostannate, BaSnF 6 . Slowly sol. in H 2 O. +3H 2 O. Sol. in 18 pts. H 2 O at 18. (Marignac, Ann. Min. (5) 15. 246.) Decomp. by warming with H 2 SO 4 with evolution of HF. (Emich, M. 1904, 25. 1912.) Calcium .fluostannate, CaSnF 6 +2H 2 O. Sol. in H 2 O. (Marignac, Ann. Min. (5) 15. 250.) Cadmium fluostannate, CdSnF 6 +6H 2 O. Sol. in H 2 O. (Marignac.) Cobaltous fluostannate, CoSnF 6 +6H 2 O. (Gossner, Zeit. Kryst. 1907, 42. 482.) Cupric fluostannate, CuSnF 6 +4H 2 O. Not deliquescent. (Marignac, Ann. Min. (5) 15. 291.) Lithium fluostannate, Li 2 SnF 6 -f-2H 2 O. Sol. in H 2 O. (Marignac, Ann. Min. (5) 15. 242.) Magnesium fluostannate, MgSnF 6 +6H 2 O. Not deliquescent. Sol. in H 2 O. (Marig- nac, Ann. Min. (5) 15. 256.) Manganous fluostannate, MnSnF 6 +6H 2 0. Slowly efflorescent. (Marignac.) Nickel fluostannate, NiSnF 6 +6H 2 O. Sol. in H 2 O. (Marignac. Ann. Min. (5) 15. 262..) FLUOTELLURATE, AMMONIUM 351 Potassium fluostannate, K 2 SnF 6 +H 2 O. Two modifications (a) Thin plates. Sol. in 2.3 pts. H 2 O at 100, and in 15-16 pts. at 18. (Marignac.) (b) Octahedra. Sol. in 3 pts. HoO at 100, and 27 pts. at 18. (Marignac.) Sol. in hot H 2 O. Can be cryst. from hot H 2 O. With cone. H 2 SO 4 , HF is evolved. (Emich, M. 1904, 25. 911.) Potassium hydrogen fluostannate, 3KF, HF, SnF 4 . Sol. in H 2 O. (Marignac.) Silver fluostannate, Ag 2 SnF 6 +4H 2 O. SI. deliquescent. Easily sol. in H 2 O. (Marignac.) Sodium fluostannate, Na 4 SnF 6 . Sol. in 18-19 pts. H 2 O at 20. (Marignac.) Strontium fluostannate, SrSnF 6 +2H 2 O. Sol. in 5.5 pts. H 2 O at 18. (Marignac.) Zinc fluostannate, ZnSnF 6 +6H 2 O. Sol. in H 2 O. (Marignac.) Fluosulphonic acid, HSO 3 F. See Sulphuryl hydroxyl fluoride. Ammonium fluosulphonate, FSO 3 NH 4 . Easily sol. in H 2 O from which it can be cryst. Sol. in ethyl alcohol, more sol. in methyl alcohol. Can be cryst. from abs. alcohol. (Traube, B. 1913, 461 2528.) Sodium fluosulphonate, FSO 3 Na. Hydroscopic. Sol. in alcohol and acetone. (Traube.) Fluosulphuric acid. Tn'caesium c^fluocfo'sulphate, S 2 O 7 F 2 Cs 3 H+ H 2 O. As the K salt. (Weinland, Z. anorg. 1899, 21. 53.) Tn'potassium c&fluoeftsulphate, S 2 7 F 2 K 3 H+H 2 0. Sol. in HF; quite stable in air; sol. in H 2 O with decomp. (Weinland, Z. anorg. 1899, Tn'rubidium difluodisulphate, S 2 O 7 R 2 Tb 3 H +H 2 O. Sol. in HF. (Weinland, Z. anorg. 1899, 21. 53.) Fluotantalic acid. Ammonium fluotantalate, (NH 4 ) 2 TaF 7 . Very sol. in H 2 O. (Marignac, A. ch. (4) 9. - 272.) (NH 4 ) 3 TaF 8 . (Balke, J. Am. Chem. Soc. 1905, 27. 1151.) Caesium fluotantalate, CsTaF 6 . Can be recryst. from HF+Aq. (Balke.) Cs 2 TaF 7 . Can not be recryst. from H 2 O as it tends to go into CsF, TaF 6 . (Balke, J. Am. Chem. Soc. 1905, 27. 1151.) ISCsF, TaF 5 . SI. sol. in H 2 O. (Penning- ton, J. Am. Chem. Soc. 1896, 18. 59.) Calcium fluotantalate. Difficulty sol. in H 2 O (Berzelius.) Cupric fluotantalate, CuTaF 7 +4H 2 O. Deliquescent. Easily sol. in H 2 O. (Marig- nac, A. ch. (4) 9. 294. Lead fluotantalate. Difficulty sol. in H 2 O. (Berzelius.) Lithium fluotantalate, LiF, TaF 8 +2H 2 O. Can be recryst. from cone. HF. (Balke, J. Am. Chem. Soc. 1905, 27. 1143.) Potassium fluotantalate, K 2 TaF 7 . SI. sol. in cold, much more easily in hot H 2 O. Decomposes, with formation of a white precipitate on boiling. (Berzelius.) Much more sol. in HF+Aq. 1 pt. of the salt is sol. in 200 pts. H 2 O containing a trace of HF, and in 150-160 pts. of H 2 O containing a little more HF. (Marignac. A. ch. (4) 9. 267.) Potassium hydrogen fluotantalate, KF, HF, TaF 6 (?). Sol. in H 2 O. (Berzelius.) Rubidium fluotantalate, Rb 2 TaF 7 . Sol. in HF+Aq. (Pennington, J. Am. Ch. Soc. 1896, 18. 58.) 3RbF, 2TaF 5 . (Balke, J. Am. Chem. Soc. 1905, 27. 1151.) Sodium fluotantalate, 3NaF, TaF 5 , Easily sol. in H 2 O. Na 2 TaF 7 +H 2 O. Sol.inH 2 O. (Marignac.) Thallous fluotantalate, Tl 2 TaF 7 . Sol. in HzO. On boiling the aqueous solu- tion tantalic acid separates. Decomp. by cone. H 2 SO 4 . Difficultly sol. in cold, easily sol. in hot HF. (Ephraim. B. 1909, 42. 4461.) Zinc fluotantalate, ZnTaF 7 +7H 2 O. Very deliquescent. Sol. in H 2 O. (Marig- nac, A. ch. (4) 9. 249.) Fluotelluric acid. Ammonium fluotellurate, NH 4 TeF 5 +H 2 O. Decomp. by H 2 O. (Hogbom, Bull. Soc. (2) 35. 60.) 352 FLUOTELLURATE, BARIUM Barium fluotellurate, Ba(TeF 5 ) 2 +H 2 O. As above. Potassium fluotellurate, KTeF 5 . As above. TeO 3 F 2 K 2 +3H 2 O. Stable in dry air; only si. sol. in H 2 O with decomp.; sol. in HF. (Weinland, Z. anorg. 1899, 21. 61.) Rubidium ^fluotellurate, Te0 3 F 2 Rb 2 +3H 2 O. SI, sol. in H 2 O with decomp. , Sol. in HF. (Weinland, Z. anorg. 1899, 21. 62.) Fluotitanic acid. Known only in solution as titanium hydro- gen fluoride. Ammonium fluotitanate, (NH 4 ) 2 TiF 6 . Sol. in H 2 O. (Marignac.) 3NH 4 F, TiF 4 . Sol. in H 2 O. (Marignac.) Ammonium fluosegtutitanate, 6NH 4 F, Ti 2 F' 6 . Easily sol. in H 2 O. SI. sol. in NH 4 F+Aq. (Petersen, J. pr. (2) 40. 54.) Insol. in NH 4 F+Aq. (Piccini, C. R. 97. 1064.) 4NH 4 F, Ti 2 F 6 . Properties as the cor- responding K salt. (Piccini, B. 18. 257 R.) Barium fluotitanate, BaTiF 6 . Very si. sol. in H 2 O. More easily sol. in dil. HNO 3 or HC1. (Engelskirchen, Dissert. 1903.) + y 2 B. 2 O. (Emich,M.1904,25.907.) Cadmium fluotitanate, CdTiF 6 +6H 2 O. Extremely sol. in H 2 O. Easily sol. in 50% alcohol. (Engelskirchen, Dissert. 1903.) Caesium fluotitanate, Cs 2 TiF 6 . More sol. in hot than cold H 2 O and much more sol. than the Rb comp. (Engels- kirchen, Dissert. 1903.) 4CsF, TiF 4 . More sol. in H 2 O than Csi5TaF 2 o and is not decomp. by pure H 2 O. (Pennington, J. Am. Chem. Soc. 1896, 18. 60.) Calcium fluotitanate, CaTiF 6 +3H 2 O. Decomp. by pure H 2 O. Sol. without de- comp. in acidified H 2 O. (Berzelius.) Separates a precipitate with cold H 2 O, which dissolves on heating. (Marignac, Ann. Min. (5) 15. 250.) Cupric fluotitanate, CuTiF 6 +4H 2 O. Sol. in pure H 2 O with partial decomp.; easily and completely sol. in acidified H 2 O. (Berzelius.) Cupric fluotitanate ammonium fluoride, CuTiF 6 , NH 4 F+4H 2 O. Efflorescent. Easily sol. in H 2 O. (Marig- nac, Ann. Min. (5) 15. 267.) Cupric fluotitanate potassium fluoride, CuTiF 6 , KF+4H 2 O. As the above salt. (Marignac.) Ferrous fluotitanate, FeTiF 6 +6H 2 O. Sol. in H 2 O. (Weber, Pogg. 120. 287.) Ferric fluotitanate. Decomp. by H 2 O. (Berzelius.) Lead fluotitanate. Easily sol. in H 2 O. (Berzelius.) Lithium fluotitanate, Li 2 TiF 6 +2H 2 O. Very sol. in H 2 O. (Engelskirchen. Dissert, 1903.) Magnesium fluotitanate, MgTiF 6 +6H 2 O. Easily sol. in cold H 2 O. (Marignac, Ann. Min. (5) 15. 257.) Nickel fluotitanate, NiTiF 6 +6H 2 O. Easily sol. in H 2 O. (Weber, Pogg. 120. 282.) Potassium fluotitanate, K 2 TiF 6 . Difficultly sol. in cold, much more easily in hot H 2 O. 100 pts. H 2 O dissolve at: 3 6 10 14 20 0.556 0.667 0.775 0.909 1.042 1.28 pts. K 2 TiF 6 . (Marignac, A. ch. (4) 8. 65.) Sol. in 78.6 pts. H 2 O at 21. Sol. in acids. (Piccini, Gazz. ch. it, 1886, 16. 104.) Sol. in 78 pts. H 2 O at 20; 9.4 pts. at 100. By addition of small amount of HF, the solubility, is increased. (Weiss and Kaiser, Z. anorg. 1910, 65. 354.) Sol. in HF. (Marchetti, Z. anorg. 1895, 10. 66.) +H 2 O. Much less sol. in H 2 O in presence of KBr or KI. (Hall, J. Am. Chem. Soc. 1904, 26. 1246.) Sol. in H 2 O or HF with decomp. (Mar- chetti, Z. anorg. 1895, 10. 66.) Potassium fluoses^wztitanate, 4KF, Ti 2 F 6 . Scarcely sol. in H 2 O; sol. in dil. acids. (Piccini, B. 18. 257 R.) Rubidium fluotitanate, Rb 2 TiF 6 . Very si. sol. in cold, somewhat more sol. in hot H 2 O. (Engelskirchen, Dissert. 1903.) Silver fluotitanate. Very deliquescent. (Marignac.) Sodium fluotitanate, Na 2 TiF 6 . Much more sol. in H 2 O than the corre- sponding potassium salt. (Marignac, Ann. Min. (5) 15. 238.) FLUOXHYPOMOLYBDATE, CUPRIC 353 Sodium hydrogen fluotitanate, Na 2 TiF 6 , NaHF 2 . Sol.inH 2 O. (Marignac.) Strontium fluotitanate, SrTiF 6 +2H 2 O. Sol. in cold H 2 O. Solution clouds up on heating. (Marignac.) Zinc fluotitanate, ZnTiF 6 +6H 2 O. Sol. in H 2 O. (Marignac, A. ch. (3) 60. 304.) Fluovanadic acid. Ammonium fluovanadate, 3NH 4 F, VF 3 . Moderately sol. in H 2 O. More easily sol. in dil. acids. Nearly insol. in alcohol or MF +Aq. (Petersen, J. pr. (2) 40. 52.) 2NH 4 F, VF 3 +H 2 O. Easily sol. in H 2 O. SI. sol. in alcohol. (Petersen.) NH 4 F, VF 3 +2H 2 O. As above. (Peter- son.) Cadmium fluovanadate, CdF 2 , VF,+7H 2 O. Very si. sol. in H 2 O. (Piccini and Giorgis, Gazz. ch. it. 22, 1. 89.) Cobalt fluovanadate, CoF 2 , VF 3 -f2H 2 0. Sol. in H 2 O without decomp. (Petersen, I c.) Nickel fluovanadate, NiF 2 , VF 3 +2H 2 O. As the Co salt. (Petersen.) Potassium fluovanadate, 2KF, VF 3 +H 2 O. SI. sol. in H 2 O; easily sol. in acids. Insol. in KF+Aq. (Petersen, J. pr. (2) 40. 51.) Potassium fluovanadate fluoxyvanadate, 4KF, VF 3 , VOF 3 . Easily sol. in H 2 O, and still more easily in HF+Aq. SI. sol.- in KF+Aq. (Petersen, J. pr. (2) 40. 274.) Sodium fluovanadate, 5NaF, 2VF 3 +H 2 0. As the potassium salt. (Petersen.) Thallous fluovanadate, T1F, VF 3 +2H 2 O. Easily sol. in H 2 O. Sol. with decomp. in cone. H 2 SO 4 , dil. HNO 3 or cold dil. HC1. Insol. in NaOH+Aq. (Ephraim, B. 1909, 42. 4460.) 2T1F, VF 3 +H 2 O. Easily sol. in H 2 0. Sol. in cone. H 2 S0 4 , dil. HNO 3 , or cold dil. HC1 with decomp. Insol. in cold or hot NaOH+Aq. (Ephraim, B. 1909, 42. 4461.) Zinc fluovanadate, ZnF 2 , VF,+7H 2 O. SI. sol. in cold H 2 O. Decomp. on heating. (Piccini and Giorgis.) Fluoxycolumbic acid. Ammonium fluoxycolumbate, 3NH 4 F, CbOF,. Cubic salt. Sol. in H 2 O. (Marignac, A. ch. (4) 8. 38.) 2NH 4 F, CbOF 3 . Lamellar salt. Much more sol. in H 2 O than 2KF, CbOF 3 . (M.) 5NH 4 F, 3CbOF 3 +H 2 0. Hexagonal salt. (M.) NH 4 F, CbOF 3 . Rectangular salt. (M.) Ammonium fluoxycolumbate columbiuxn flu- oride, 3N1 (Marignac.) >xyc oride, 3NH 4 F, CbOF 3 , CbF 6 . Cupric fluoxycolumbate, CuF 2 , CbOF 3 + 4H 2 O. SI. deliquescent. Sol. in H 2 O. (Marignac, A. ch. (4) 8. 42.) Potassium fluoxycolumbate, 2KF, CbOF 8 + H 2 O. Sol. in 12.5-13 pts. H 2 O afc 17-21. Much more sol. in hot H 2 O, or H 2 O containing HF. (Marignac.) 3KF, CbOF 3 . Decomp. by H 2 O into above salt. (M.) 5KF, 3CbOF 8 +H 2 0. Sol. in H 2 0. (M.) 4KF, 3CbOF 3 + H 2 O. Sol. in H 2 O. (M.) 3KF, 2Cb 2 O fi +5H 2 O. SI. sol. in H 2 O. (Petersen, J. pr. (2) 40. 287.) KF, Cb 2 O 6 +3H 2 O. SI. sol. in H 2 O. (Pe- tersen.) 2KF, 3CbO 2 F. Insol. in H 2 O. Sol. in HF. (Kriiss and Nilson, B. 20. 1689.) See also Fluoxypercolumbate, potassium. Potassium hydrogen fluoxycolumbate, 3KF, HF, CbOFs. Sol. in H 2 O. (Marignac.) Sodium fluoxycolumbate, 2NaF, CbOF,-f 2H 2 0. Sol. in H 2 0. NaF, CbOF 3 +H 2 O. (Marignac.) Zinc fluoxycolumbate, ZnF 2 , CbOF 3 +6H 2 O. Sol. in H 2 0. (Marignac, A. ch. (4) 8. 41.) Fluoxyhypomolybdic acid. Ammonium fluoxyhypomolybdate, MoOF, 2NH 4 F. Decomp. by H 2 O. (Mauro, Gazz. ch. it. 19. 179.) 3MoOF 3 , 5NH 4 F+H 2 0. Decomp. by H 2 O. (Mauro.) Cupric fluoxyhypomolybdate, CuF 2 , MoOF t + 4H 2 0. Deliquescent. Sol. hi H 2 O. (Mauro, Real. Ac. Line. 1892, 1. 194.) 354 FLUOXYHYPOMOLYBDATE, POTASSIUM Potassium fluoxyhypomolybdate, MoOF 3 2KF+H 2 0. Sol. in H 2 O with decomp. Sol. in HF or HC1 +Aq. (Mauro and Pana- bianco, Gazz. ch. it. 12. 80.) 3MoOF 3 , 5KF+H 2 O. Sol. in H 2 O with decomp. (Mauro, Gazz. ch. it. 19. 179.) Thallous fluoxyhypomolybdate, 2T1F, MoOF 3 . (Mauro, B. 1894, 27R. 109.) Zinc fluoxyhypomolybdate. ZnF 2 , MoOF 3 + 6H 2 0. Rapidly deliquescent. Sol. in H 2 O. (Mauro, Real. Ac. Line. 1892. 1. 194.) Fluoxyhypovanadic acid. See Fluoxyvanadic acid. Fluoxymanganic acid. Ammonium fluoxymanganate, (NH 4 ) 2 MnOF 4 . Precipitate. (Nickles.) Potassium fluoxymanganate, K 2 MnOF 4 . Precipitate. (Nickles, C. R. 65. 107.) /Sesgm'fluoxymanganic acid. Potassium sesgwifluoxymanganate, K 4 Mn 2 OF 8 = 4KF, Mn 2 OF 4 . Precipitate. (Nickles.) Fluoxymolybdic acid. See also Fluoxyhypomolybdic, and fluoxy- permolybdic acids. Ammonium fluoxymolybdate, NH 4 F, MoO 2 F 2 . Sol. in H 2 O. (Mauro, Gazz. ch. it. 20. 109.) +H 2 O. ' More sol. in H 2 O than 2NH 4 F, MoO 2 F 2 . (Delafontaine, N. Arch. Sci. ph. nat. 30. 250.) Correct formula is 3NH 4 F, MoO 2 F 2 . (Mauro, Gazz. ch. it. 18. 120.) 2NH 4 F, MoO 2 F 2 . Much more sol. than 2KF, MoO 2 F 2 . (Delafontaine.) 3NH 4 F, MoO 2 F 2 . Sol. in H 2 O. (Mauro.) 5NH4F 3MoO 2 F 2 +H 2 O. Sol. in H 2 O. (Mauro, Gazz. ch. it. 20. 109.) Ammonium fluoxymolybdate molybdate, Mo0 2 F 2 , 4NH 4 F, (NH 4 ) 2 MoO 4 . Sol. in H 2 O, but with decomp. (Mauro, Gazz. ch. it. 18. 120.) Cadmium fluoxymolybdate, CdF 2 , Mo0 2 F 2 -f 6H 2 O. SI. efflorescent. (Delafontaine, J. B. 1867. 236.) Cobaltous fluoxymolybdate, CoF 2 , MoO 2 F 2 + 6H 2 O. Sol. in H 2 O. (Delafontaine, J. B. 1867. 236.) Cupric fluoxymolybdate, CuF 2 , MoO 2 F 2 + 4H 2 O. Deliquescent. (Mauro, Real. Ac. Line. 1892, 1. 194. Nickel fluoxymolybdate, NiF 2 , Mo0 2 F 2 + 6H 2 0. Sol. in H 2 O. (Delafontaine, J. B. 1867. 236.) Potassium fluoxymolybdate, 2KF, MoO 2 F 2 + H 2 O. Easily sol. in boiling H 2 O. Sol. in H 2 O with decomp. Sol. in HF. (Marchetti, Z. anorg. 1895, 10. 68.) KF, MoO 2 F 2 +H 2 O. Gradually efflores- cent. (Delafontaine.) Rubidium fluoxymolybdate, 2RbF, 2Mo0 2 F 2 +2H 2 0. Sol. in cold, more sol. in hot H 2 O. (Dela- fontaine.) Sodium fluoxymolybdate, NaF, MoO 2 F 2 + ^H 2 0. Sol. in H 2 0. (Delafontaine.) Thallous fluoxymolybdate, 2T1F, MoO 2 F 2 -h H 2 O. Sol. in hot H 2 O. (Delafontaine.) Zinc fluoxymolybdate, ZnF 2 , MoO 2 F 2 +6H 2 0. Sol. in H 2 0. (Delafontaine.) Fluoxypercolumbic acid. Potassium fluoxypercolumbate, 2KF, CbO 2 F 2 +H 2 O. (Piccini, Z. anorg. 2. 21.) Sol. in H 2 O with decomp. Sol. in HF. (Marchetti, Z. anorg. 1895, 10. 67.) Fluoxypermolybdic acid. Ammonium fluoxypermolybdate, MoO 3 F 2 , 3NH 4 F. Sol. in H 2 O. '(Piccini, Z. anorg. 1. 51.) Caesium fluoxypermolybdate, Mo0 3 F 2 , 2CsF +H 2 O. (Piccini.) Potassium fluoxypermolybdate, MoO 3 F 2 , 2KF+H 2 0. Not very sol. in H 2 O; more sol. in HF-f- A.q without decomp. (Piccini.) FLUOXYTUNGSTATE, ZINC 355 Rubidium fluoxypermolybdate, MoO 3 F 2 , 2RbF+H 2 O. Somewhat more sol. in H 2 O than K salt. Easily sol. in HF+Aq. (Piccini.) Fluoxypertantalic acid. Potassium fluoxypertantalate, 2KF, TaO 2 F 3 +H 2 0. Sol. in H 2 O. (Piccini, Z. anorg. 2. 21.) Fluoxypertitanic acid, TiO 2 F 2 , HF. Known only in solution. (Piccini, B. 18. 255 R.) Ammonium fluoxypertitanate, TiO 2 F 2 , 2NH 4 F. Very unstable. (Piccini, Gazz. ch. it. 17. 479.) TiO 2 F 2 , 3NH 4 F. Sol. in H 2 O. Sol. in H 2 O 2 . (Piccini, Z. anorg. 1895, 10 439.) 2Ti0 2 F 2 , 3NH 4 F. Sol. in H 2 O. (Piccini, B. 18. 698 R.) Barium fluoxypertitanate, TiO 2 F 2 , BaF 2 . Precipitate. Easily sol. in acids. (Piccini, B. 18. 698 R.) 2TiO 2 F 2 , 3BaF 2 . Insol. in H 2 O; sol. in dil. acids. (Piccini, Gazz. ch. it. 17. 479.) Potassium fluoxypertitanate, TiO 2 F 2 , 2KF. Sol. in H 2 O. (Piccini, B. 21. 1391.) Sol. in H 2 O 2 . (Piccini, Z. anorg. 1895, 10. 438.) Fluoxypertungstic acid. Potassium fluoxypertungstate, 2KF, WO 3 F-f- H 2 O. (Piccini, Z. anorg. 2. 11.) Fluoxytantalic acid. See also Fluoxypertantalic acid. Ammonium fluoxytantalate,'3NH 4 F, TaOF 2 . Easily sol. in H 2 O. The solution clouds up by standing or on warming. (Joly, C. R. 81. 1266.) Fluoxytitanic acid. See also Fluoxypertitanic acid. Barium fluoxytitanate, TiOF 2 , BaF 2 . Insol. in H 2 0; sol. in dil. acids. (Piccini, Gazz. ch. it. 17. 479.) Fluoxytungstic acid. Ammonium fluoxytungstate, 2NH 4 F, WO 2 F 2 . Very sol. in H 2 O. (Marignac, A. ch. (3) 69. 65.) NH 4 F, WO 2 F 2 +H 2 O. Decomp. by H 2 O. Crystallises unchanged from H 2 O containing HF. (Marignac.) Ammonium fluoxytungstate tungstate, 4NH 4 F, WO 2 F 2 , (NH 4 ) 2 WO 4 . Incompletely sol. in H 2 O. Residue dis- solves in NH 4 OH+Aq. (Marignac.) Cadmium fluoxytungstate. Very sol. in H 2 O. (Marignac.) Cupric fluoxytungstate, CuF 2 , WO 2 F 2 +4H 2 O. Very sol. in H 2 O. (Marignac, C. R. 56. 888. Cupric fluoxytungstate ammonium fluoride, CuF 2 , WO 2 F 2 , NH 4 F+4H 2 O. Sol. in H 2 0. (Marignac.) Manganese fluoxytungstate. Very sol. in H 2 O. (Marignac.) Nickel fluoxytungstate, NiF 2 , WO 2 F 2 + 10H 2 0. Deliquescent. Very sol. in H 2 O. (Marig- nac.) Potassium fluoxytungstate, KF, W0 2 F 2 + H 2 : Can be recrystallised without decomp. only from H 2 O containing HF. (Marignac, A. ch. (3) 69. 70.) 2KF, WO 2 F 2 +H 2 0. Difficultly sol. in cold, more easily in hot H 2 O. (Berzelius.) Sol. in 17 pts. H 2 O at 15. (Marignac.) Can be recrystallised without decomp. from H 2 O, or H 2 O containing HF. (Marig- nac.) Sol. in H 2 O with decomp. Sol. in HF. (Marchetti, Z. anorg. 1895, 10. 71.) ' See also Fluoxypertungstate, potassium. Silver fluoxytungstate. Very easily sol. in H 2 O. (Marignac.) Sodium fluoxytungstate, 2NaF, WO 2 F 2 . More sol. in H 2 O than the corresponding K compound. (Berzelius.) Thallous fluoxytungstate, T1F, W0 2 F 2 . Insol. in H 2 O. Decomp. by H 2 O. (Ephraim and Heymann, B. 1909, 42. 4463.) 2T1F, WO 2 F 2 . Insol. in H 2 O'but decomp. thereby. (Ephraim and Heymann, B. 1909, 42. 4462.) 3T1F, 2WO 2 F 2 . Insol. in H 2 O. Decomp. by acids. (Ephraim and Heymann, B. 1909, 42. 4462.) Zinc fluoxytungstate, ZnF 2 , WO 2 F 2 +10H 2 O. Very sol. in H 2 O. (Marignac.) 356 FLUOXYURANIC ACID Fluoxyuranic acid. Ammonium fluoxyuranate, 3NH 4 F, UO 2 F 2 . Easily sol. in H 2 O, less in HF. Insol. in alcohol. (Bolton.) 100 g. solution sat. at 27 contain 10.11 g. salt. 100 g. solution sat. at 81.3 contain 20.71 g. salt. (Burger, Dissert. 1904.) Barium fluoxyuranate, 3BaF 2 , 2U0 2 F 2 + 2H 2 O. Traces dissolve in hot H 2 O. Easily sol. in dil. acids. (Bolton.) Potassium fluoxyuranate, 3KF, ITO 2 F 2 . Sol. in 8 pts. H 2 at 21. Insol. in alcohol and ether. (Bolton, J. pr. 99. 269.) Does not exist. (Smithells, Chem. Soc. 43. 125.) 4KF, UO 2 F 2 . Insol. in H 2 O. Easily sol. in dil. acids. (Ditte, C. R. 91. 115.) 5KF, 2UO 2 F 2 . (Baker, Chem. Soc. 35. 760.) 3KF, 2UO 2 F 2 +2H 2 O. (Baker.) Sodium fluoxyuranate, NaF, U0 2 F 2 . +2H 2 O. Not efflorescent. +4H 2 0. Insol. in H 2 O and dil. acids. SI. sol. in cone. HCl+Aq. Sol. in cone. H 2 SO 4 . (Bolton, J. B. 1866. 212.) 4NaF, U0 2 F ? . (Ditte.) Does not exist. (Smithells, Chem. Soc. 43. 125.) Fluoxyvanadic acid. Ammonium fluoxyvanadate, 12NH 4 F, V 2 O 6 , 2VOF 3 . Easily sol. in H 2 0, and not attacked by cold cone. H 2 SO 4 . (Baker, Chem. Soc. 33, 388.) Formula is 3NH 4 F, VO 2 F. (Petersen, J pr. (2) 40. 289.) 3NH 4 F, VO 2 F. Sol. in H 2 0. (Petersen U.) Much less sol. in H 2 in presence of NH 4 F (Piccini and Giorgis, Gazz. ch. it. 27. 1. 65.). +H 2 O. (Piccini and Giorgis, Gazz. ch. it 1892, 22. 55.) 3NH 4 F, VOF 2 . "Hypoyanadate." Quite sol. in H 2 O. Very si. sol. in MF+Aq. Less sol. in alcohol than in H 2 O. (Petersen, J pr. (2) 40. 195.) 2NH 4 F, VOF 2 . Sol. in H 2 O. (Petersen.; +H 2 0. (Piccini and Giorgis.) 7NH 4 F, 4VOF 2 +5H 2 O. Very sol. in H 2 O (Petersen.) 3NH 4 F, 2VO 2 F. Sol. in H 2 O without de- comp. Sol. in cone. HF+Aq. (Piccini anc Giorgis, Gazz. ch. it. 24. 1. 68.) 3NH 4 F, 2VOF 3 +H 2 O. Sol. in H 2 O with decomp. V 2 O 5 , 2NH 4 F. (Ditte, C. R. 106. 270.) V 2 O 6 , 8NH 4 F+4H 2 O. As above. V 2 6 , 4NH 4 F+4H 2 0. As above. Sol. in H 2 0. Ammonium hydrogen flucfo'oxyvanadate, 7NH 4 F, HF, 4VO 2 F. Very sol. hi H 2 O. (Petersen, J. pr. (2) 40. 284.) . Ammonium hydrogen fnfluoxyvanadate, 3HF, 9NH 4 F, 5VOF 3 . Easily sol. in H 2 O. SI. sol. in MF+Aq. Petersen, J. pr. (2) 40. 280.) 3NH 4 F, 3HF, 2VOF 3 . Sol. in H 2 O. (Baker, Chem. Soc. 33. 388.) Identical with 3HF, 9NH 4 F, 5VOF 3 . Petersen.) Barium fluoxyvanadate, BaF 2 , VO 2 F. Ppt. (Ephraim, Z. anorg. 1903, 35. 79.) Cadmium fluoxyvanadate, CdF 2 , VOF 2 + 7H 2 O. Hypovanadate." As the Co salt. (Pic- cini and Giorgis.) Cobalt fluoxyvanadate, CoF 2 , VOF 2 +7H 2 O. " Hypovanadate." Sol. in H 2 O. (Piccini and Giorgis.) Nickel fluoxyvanadate, NiF 2 , VOF 2 +7H 2 O. "Hypovanadate." As the Co salt. (Piccini and Giorgis.) Potassium fluoxyvanadate, 7KF, 3VOF 2 . Very si. sol. in H 2 O and MF+Aq. Easily sol. in dil. acids. (Petersen, J. pr. (2) 40. 199.) 2KF, VOF 2 . As above. (Petersen.) 2KF, 2V 2 O 5 +8H 2 O. Sol. in H 2 O and H 2 SO 4 . (Ditte, C. R. 105. 1067.) 2KF, 3V 2 O 6 +5H 2 O. As above. 2KF, 4V 2 O 6 +8H 2 O. As above. 4KF, V 2 O 5 . Less sol. than 4KF, 3V 2 5 . +2H 2 O, and +3H 2 O. Sol. in H 2 O. 4KF, 3V 2 O 6 +4H 2 O, and +6H 2 O. Less sol. than 2KF, 3V 2 O 6 +5H 2 O. 8KF, V 2 O 5 +2H 2 O, and +3H 2 O. Sol. in H 2 O. Potassium fn'fluoxyvanadate, 2KF, VOF 3 . Ppt. (Petersen, J. pr. (2) 40. 272.) 6KF ; V 2 6 , 2VOF 3 +2H 2 O. Sol. in H 2 0. Insol. in cold cone. H 2 SO 4 . (Baker, Chem. Soc. 33. 300.) Formula is 3KF, 2V0 2 F. (Piccini and Giorgis.) See also Fluovanadate fluoxyvanadate, potassium. Potassium flucftoxyvanadate, 2KF, VO 2 F. Easily sol. in H 2 O. (Petersen, J. pr. (2) 40. 278.) FULMINATING PLATINUM 357 3KF, VO 2 F. As above. (Petersen.) 3KF, 2VO 2 F. Sol. in H 2 O; scarcely at- tacked by H 2 SO 4 . (Piccini and Giorgis.) Potassium hydrogen fluoxyvanadate, 3KF, HF,2VOF 3 . Sol. in H 2 0. (Petersen.) Sodium fluoxyvanadate, 8NaF, 3VOF 2 -f 2H 2 0. Sol. in HoO. (Petersen, J. pr. (2) 40. 200.) 3NaF, V0 2 F, VOF 3 (?). Very easily de- comp. (Piccini and Giorgis.) 2NaF, 2V 2 O 6 -hlOH 2 O. Sol. in H 2 O. (Ditte, C. R. 106. 270.) 4NaF, V 2 O 6 . As above. 4NaF, 3V 2 O 6 +18H 2 O. As above. 6NaF, V 2 O 6 +5H 2 O. As above. 8NaF, V 2 6 -f 3H 2 O. (As above. Thallous fluoxyvanadate, 2T1F, VOF 2 . Somewhat sol. in cold H 2 O without decomp. Sol. in boiling H 2 O with exception of a black residue, which is easily sol. in dil. H 2 SO 4 . (Ephraim, B. 1909, 42. 4460.) 3T1F,2VO 2 F. Insol.inH 2 O. Sol. in H 2 containing H 2 SO4. (Ephraim and Hey- mann, B. 1909, 42. 4459.) Zinc fluoxyvanadate, ZnF 2 , ZnO, 2VOF 8 + 14H 2 O. Decomp. on air; sol. in H 2 O. (Baker, Chem. Soc. 33. 388.) True composition is represented by the for- mula ZnF 2 , VO 2 F+7H 2 O. (Petersen.) ZnF 2 , VO 2 F+7H 2 O. Very sol. in H 2 O. (Piccini and Giorgis.) ZnF 2 , VOF 2 +7H 2 O. "Hypovanadate." Sol. in cold H 2 O, but decomp. by boiling; sol. in dil. HF+Aq. (Piccini and Giorgis.) Fluozirconic acid. Ammonium fluozirconate, (NH 4 ) 2 ZrF 6 . Sol. in H 2 O. 3NH 4 F, ZrF 4 . Sol. in H 2 O. (Marignac.) Cadmium fluozirconate, 2CdF 2 , ZrF 4 +6H 2 O. Sol. in H 2 O; can be recrystalised therefrom. (Marignac, A. ch. (3) 60. 257.) CdZrF 6 +6H 2 O. Sol. in H 2 O. (Marignac.) Caesium fluozirconate, CsF, ZrF 4 +H 2 O. Sol. in H 2 O without decomp. (Wells, Z. anorg. 1895, 10. 434.) 2CsF, ZrF 4 . Sol. in H 2 without decomp. (Wells, Z. anorg. 1895, 10, 434.) 2CsF, 3ZrF 4 +2H 2 O. Only si. sol. in H 2 0. (Wells, Z. anorg. 1895, 10. 434.) Cupric fluozirconate, 2CuF 2 , ZrF 4 -f-12H 2 O. Easily sol. in cold H 2 O. (Marignac, A. ch. (3) 60. 296.) 3CuF 2 , 2ZrF 4 + 16H 2 O. Sol. in H 2 O. (Marignac.) Lithium fluozirconate, 2LiF, ZrF 4 . Ppt. (Wells, Am. J. Sci. 1897, (4) 3. 4LiF, ZrF 4 + 3^H 2 O. Sol. in H 2 O with decomp. (Wells, Am. J. Sci. 1897, (4) 3. 469.) Magnesium fluozirconate, MgZrF 6 +5H 2 0. Sol. in H 2 O. (Marignac.) Manganous fluozirconate, MnZrF 6 +5H 2 O. Sol. in H 2 O. (Marignac, J. pr. 83. 202.) Nickel fluozirconate, 2NiF 2 , ZrF 4 +12H 2 0. Sol. in H 2 O. (Marignac, A. ch. (3) 60. 291.) NiZrF 6 +6H 2 O. Sol. in H 2 O. (Marig- nac.) Nickel potassium fluozirconate, K 2 ZrF 6 , NiZrF 6 +8H 2 O. Sol. inH 2 0. (Marignac.) Potassium fluozirconate, KF, ZrF 4 +H 2 0. Much more sol. in hot, than cold H 2 O. (Marignac.) 2KF, ZrF 4 = K 2 ZrF 6 . 100 pts. H 2 dis- solve at 2, 0.781 pt.; at 15, 1.41 pts.; at 19. 1.69 pts.; at 100, 25.0 pts. K 2 ZrF 6 . (Marig- nac.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) 3KF, ZrF 4 . Sodium fluozirconate, 5NaF, ZrF 4 . 100 pts. H 2 dissolve 0.387 pt. at 18, and 1.67 pts. at 100. (Marignac.) 2NaF, ZrF 4 . (Wells, Am. J. Sci. 1897, (4) 3. 469.) 5NaF, 2ZrF 4 . Sol. in H 2 O with decomp. (Wells.) Tellurium fluozirconate, TeF, ZrF 4 . Sol. in H 2 O without decomp. (Wells, Am. J. Sci. 1897, (4) 3. 470.) +H 2 O. Sol. in H 2 O without decomp. (Wells.) 3TeF, ZrF 4 . Sol. in H 2 O without decomp. (Wells.) 5TeF, 3ZrF 4 . Sol. in H 2 O without decomp. (Wells.) Zinc fluozirconate, ZnZrF 6 +6H 2 0. Sol. inH 2 O. (Marignac.) 2ZnF 2 , ZrF 4 +12H 2 O. Sol. in H 2 O. (Mar- ignac, A. ch. (3) 60. 257.) Fulminating gold. See Auroamidoimide. Fulminating platinum. See Fulminoplatinum. 358 FULMINATING SILVER Fulminating silver. See Silver nitride. Fulminoplatinum compounds. See Dichlorofulminoplatinum. TVicUorofulmmoplatinum. Te^achlorofulminoplatinum. Chloroxyfulminoplatinum. Fuscocobaltic chloride, Co(NH 3 )4(OH)Cl 2 +H 2 0. Sol. in H 2 O, from which it is precipitated by NH 4 Cl+Aq; decomp. by boiling H 2 O; pptd. from aqueous solution by alcohol. (Fremy, C. R. 32. 501.) nitrate, Co(NH 3 ) 4 (OH)(NO 3 ) 2 +H 2 O. Sol. in H 2 O. Properties as the chloride. (Fremy.) sulphate, Co(NH 3 ) 4 (OH)SO 4 +l^H 2 O. Sol. in H 2 O. Insol. in NH 4 OH+Aq. (Fremy, C.R. 32. 501.) Insol. in H 2 O. Sol. in cone. HCl+Aq, or H 2 SO 4 , from which it is precipitated by H 2 O. (Vortmann, N. 6. 412.) Fusible white precipitate. See Mercuricfo'ammonium chloride. Gadolinium, Gd. (Marignac, C. R. 102. 92.) Gadolinium bromide, GdBr 3 +6H 2 O. Sol. in HBr. (Benedicks, Z. anorg. 1900, 22. 403.) Gadolinium chloride, GdCl 3 +6H 2 O. Somewhat deliquescent. Sol. in H 2 O. (Benedicks.) Gadolinium platinum chloride. See Chloroplatinate, gadolinium. Gadolinium fluoride, GdF 3 . Insol. in H 2 O ; si. sol. in hot HF. (Popovici, B. 1908, 41. 635.) Gadolinium hydroxide, Gd(OH) 8 . Ppt. (Benedicks, Z. anorg. 1900, 22. 402.) Gadolinium oxide, Gd 2 O 3 . Sol. in acids, (de Boisbaudran, C. R. 111. 394.) Somewhat hydroscopic; easily sol. in acids. (Benedicks.) Gallium, Ga. Not decomp. by H 2 O; easily sol. in cold HC1 +Aq. Slowly sol. in warm dil. HNO 3 + Aq. Not attacked by cone. HNO 3 free from N 2 O 3 below 40-50, and only slowly in presence of N 2 O 3 . (Dupre, C. R. 86. 720.) Easily sol. in cold or warm KOH+Aq. (de Boisbaudran, A. ch. (5) 10. 100.) Gallium bromide, GaBr 3 . Deliquescent, and sol. in H 2 O. Gallium bichloride, GaCl 2 . Deliquescent, and decomp. by H 2 0. (Nil- son and Petersen, C. R. 107. 527.) Gallium chloride, GaCl 3 . Deliquescent, and very sol. in little H 2 O. Decomp. by much H 2 O, with formation of basic salt, which is slowly sol. in dil. HC1 +Aq. Gallium hydroxide. Sol. in acids; sol. in KOH or NaOH+Aq, less easily in NH 4 OH+Aq, even in presence of ammonium salts. Gallium iodide, GaI 3 . Deliquescent, and sol. in H 2 O. (de Bois- baudran and Jungfleisch, C. R. 86. 578.) Gallium sw&oxide, GaO (?). Sol. in HNO 3 +Aq. (Dupre.) Sol. in dil. H 2 SO 4 +Aq. Gallium oxide, Ga 2 O 3 . Sol. in acids. Germanium, Ge. Insol. in HCl+Aq. Easily sol. in aqua regia. Decomp. by HNO 3 +Aq to oxide. Cone. H 2 SO 4 decomp. to sulphate. Insol. in boiling KOH+Aq. (Winkler, J. pr. (2) 34. 177; 36. 177.) Germanium te^rabromide, GeBr 4 . Decomp. by H 3 O. (Winkler.) Germanium bichloride, GeCl 2 . Decompl by H 2 O. (Winkler.) Germanium t eti ochloride, GeCl 4 . Sinks in H 2 O, and is gradually decomp. thereby. (Winkler, J. pr. 34. 177.) Insol. in and not attacked by hot cone. H 2 S0 4 . (Friedrich, W. A. B. 102, 2b. 540.) Germanium chloroform, GeHCl 3 . Decomp. by H 2 O. Sol. in HCl+Aq. (Winkler.) Germanium teti afluoride, GeF 4 . Deliquescent, and sol. in H 2 O. +3H 2 O. Deliquescent. Melts in its crystal H 2 O when warmed. (Winkler.) GLASS 359 Germanium potassium fluoride. See Fluogermanate, potassium. Germanium hydride, GeH 4 . SI. sol. in hot HC1. Sol. in NaOCl+Aq. (Voegelen, Z. anorg. 1902, 30. 327.) Germanium te^raiodide, Gel4. Deliquescent, and sol. in H 2 O with decomp. (Winkler.) Germanium wowoxide, GeO. Not appreciably sol. in dil. H 2 SO 4 +Aq. Easily sol. in HCl+Aq. Insol. in alkalies. (Winkler, J. pr. (2) 34. 177.) Somewhat sol. in H 2 O ; insol. in H 2 SO 4 -f Aq, even when hot and cone, (van Bemmelen, R. t. c. 6. 205.) Germanium dioxide, GeO 2 . Not very difficultly sol. in H 2 O. Sol. in 247.1 pts. H 2 O at 20; in 93.3 pts. at 100. (Winkler.) Easily sol. in alkali carbonates or hydrates +Aq; si. sol. in acids. Germanium oxychloride, GeOCl 2 . Insol. in H 2 O: sol. in acids. (Winkler, J. pr. (2) 36. 177.) Germanium mowosulphide, GeS. Sol. in 402.9 pts. H 2 O. Sol. in cone, hot HCl+Aq. Sol. in KOH+Aq. Sol. in (NH 4 ) 2 S+Aq when precipitated. Insol. in (NH 4 ) 2 S+Aq if crystalline. Also exists in a colloidal state. (Winkler.) Germanium ^'sulphide, GeS 2 . Sol. in 221.9 pts. H 2 O. Easily sol. in. KOH+Aq, or NH 4 OH+Aq. Insol. in acids. Exists also in a colloidal state. (Winkler.) Glass. Numerous and extensive researches have been made on the action of H 2 O and various solutions on glass. The older work has a cer- tain historical interest, but only a brief state- ment of some of the more important results can be given here. For a very thorough resume of the work before the year 1861, Storer's Dictionary, p. 555, should be con- sulted. All glass is more or less attacked by H 2 O, the more easily the greater the amount of alkali present, the finer it is powdered, and the higher the temperature. Glass, as that of a flask, is decomposed to a consider- able exlent by several days' boiling with H 2 O, a portion of the fixed alkali being dissolved, but when powdered glass is rubbed with distilled H2O in a mortar, the H 2 O remains pure and exhibits no alkalinity. (Scheele.) Glass of alembics is partially dissolved by long boil- ing with H 2 O. (Lavoiser.) H 2 O extracts potash or soda from glass together with Powdered lead glass gives up appreciable amounts of )O to weakly acidified H 2 O. (Pelouze.) a portion of the silica, the decomposition taking place the more easily in proportion as the glass is richer in alkalies, more minutely divided, or the temperature of the water higher. (Bischof, Kastn. Arch. 1. 443.) Powdered crown glass and some varieties of window glass render cold H 2 O alkaline when in contact there- with. (Dumas.) 100 pts. finely divided flint glass lose 7 pts. potash when boiled one week with H 2 O. (Griffiths, Q. J. Sci. 20. 258.) Retorts of ordinary or flint glass are partially dis- solved by H 2 O when it is evaporated therein. (Chev- reul, 1811.) Finely powdered plate-glass (Faraday, Pogg. 18. 569), and Thuringian potash glass (Ludwig, Arch. Pharm. 91. 47) redden moistened turmeric paper. The alkaline reaction disappears by continued wash- ing, but reappears when the glass is freshly rubbed. (Griffiths.) Cold HzO takes up SiO 2 as well as alkali from glass powder. (Fuchs.) PbO When powdered white glass, containing 12.4% Na2O, 15.5% CaO, and 72.1% SiO 2 , is treated repeatedly with HjO, more than 3% of the glass is dissolved, and the undissolved part gives up 1.5% CaO to HCl+Aq with effervescence. A glass containing more alkali, i. e. 16.3% Na 2 O, 6.4% CaO, 77.3% SiO 2 , lost with the same treatment 18.2%, and the residue gave up 2% CaO to HCl+Aq. (Pelouze, C. R. 43. 117.) In the above case the fineness of the glass has an influence as well as its composition. When the same sample of glass was boiled 1 hour with HsO, amounts were dissolved in the proportion 1 : 4 : 28, according as the glass was in form of a coarse, fine, or very fine powder. Glass of the composition of the above samples, as given by Pelouze, lost 10 and 32% respectively. If powdered glass is boiled with H 2 O and CO 2 con- ducted into the solution, it is absorbed; if boiled with K 2 SO4. Na 2 SO 4 is dissolved. (Pelouze.) Glass tubes are converted into a white crystalline mass by heating with H 2 O several months to 75-150; lead glass and Bohemian glass most easily, English crown glass least. A little H 2 O attacks glass more than much H 2 O. The action of H 2 O is greatly increased by finely pulverising the glass. H 2 O dissolved 10% of a glass containing 12% Na 2 0, 15.5% CaO, and 72.5% SiO 2 , and 32% of another glass containing 16.3% Na 2 O, 6.4% CaO, and 77.3% SiO 2 . (Vogel, B. A. Munchen, 1867. 437.) Action of H 2 O on a glass containing 74% Si0 2 , 8.6% CaO, 14% Na 2 O 0.6% K 2 O, with traces of A1 2 O 3 , Fe 2 O 3 , MnO, and MgO. By boiling with H 2 a decrease of 3.9 mg. was observed for the first hour, which soon became constant at 2.2 mg. per hour. The action was then proportional to the time, and also to the surface in contact with the liquid, but independent of the amount of liquid evaporating. The action decreases rapidly with the tem- perature, so that at 90-100 only ^ as much ass is dissolved as by boiling H 2 O . (Emmer- ag, A. 150. 257.) When steam condenses in tubes of Na glass, they are so strongly attacked that the H 2 O has an alkaline reaction, but tubes of hard or Bohemian K glass are not so strongly at- tacked. (Tollens, B. 9. 1540.) The effect of H 2 O is so great as to impart a distinctly alkaline reaction to water condens- ing in a tube of ordinary"glass. By condensing water in long tubes of various kinds of glass the following results were obtained. 360 GLASS I. Easily fusible Thuringian glass. Sur- face exposed = 324 sq. cm. After 2 hours, 62.0 mg. KOH were dis- solved. After 3 hours more, 36.0 mg. KOH were dis- solved. After 3 hours more, 33.2 mg. KOH were dis- solved. After 3 hours more, 20.8 mg. KOH were dis- solved. After 3 hours more, 20.8 mg. KOH were dis- solved. Or, in 14 hours, 172.8 mg. KOH were dis- solved. II. Less easily fusible Thuringian glass. Surface exposed = 499 sq. cm. After 3 hours, 19.2 mg. KOH were dis- solved. After 3 hours more, 15.2 mg. KOH were dis- solved. After 3 hours more, 12.4 mg. KOH were dis- solved. After 3 hours more, 11.2 mg. KOH were dis- solved. Or, after 12 hours, 58.0 mg. KOH were dis- solved. III. Combustion tubing of very difficultly fusible Bohemian glass. Surface exposed 1130 sq. cm. After 3 hours 4.16 mg. KOH were dis- solved. After 3 hours more 4.16 mg. KOH were dis- solved. After 3 hours more 4.16 mg. KOH were dis- solved. After 3 hours more 4.16 mg. KOH were dis- solved. Or, after 12 hours, 16.64 mg. KOH were dis- solved. . IV. Easily fusible Bohemian glass. Sur- face exposed = 1394 sq. cm. After 3 hours, 7.88 mg. KOH were dis- solved. After 3 hours more, 8.56 mg. KOH were dis- solved. After 3 hours more, 1.97 mg. KOH were dis- solved. Or, after 9 hours, 24.32 mg. KOH were dis solved. (Kreusler and Henzold, B. 17. 34 V From the above the following table has been calculated. 50 ccm. H 2 O dissolves from a surface o 1000 sq. m. in 1 hour: 96.0 mg. from easily fusible Thuringian glass. 12.8 mg. from less fusible Thuringian glass 1.2 mg. from combustion tube of Bohemian glass. 2.0 mg. from harder tube of Bohemian glass. (Kreusler and Henzold, B. 17. 34.) 100 ccm. H 2 O dissolves so much glass from flask every 2 seconds, when in contact there- with that 0.1 ccm. y% normal oxalic acid i neutralised thereby. (Bohlig, Z. anal. 23 518.) Action of H 2 O on various kinds of Na glass, g. of finely powdered glass was boiled 10-15 minutes in a silver dish with 100 ccm. H 2 O, nd the per cent of Na 2 O (or K 2 O) in the olution was determined. %Na 2 (K 2 0) )rthoclase feldspar . . . . . 0.17 lass of a Bohemian combustion tube . 0.56 flask (German manuf.) . 0.69 " champagne bottle . . 1.7 STatrolite . . . \ .1.32 lass of a wine bottle (Hungarian) . 2 . 22 lass which was attacked by H 2 O under pressure . . .3.7 l,ead glass Grlass that broke easily . . .4.8 Glass tubing that became rough when fused . . V. .6.1 lass tubing that became opaque by fusing i>.-,' . . .14.35 Solid water glass . . . .26.97 (Wartha, Z. anal. 24. 220.) The relative ease by which various kinds of glass are attacked by H 2 O is shown by the Allowing table. The glass was powdered and leated on a water bath with exclusion of atmospheric CO 2 . Potassium water glass ;i^J 291 Sodium water glass . .-:., 196 Yellow glass rich in alkali . 34 Thuringian glass . . 19 Ditto from Tittel and Co*. 8 Window glass . Lead glass from Jena 6 Bohemian glass from Kavalier 2 . 4 Lead crystal glass . . 1.4 Thermometer glass, 16IV, from Jena. ... 1.0 Zinc glass, 362, from Jena . 0.8 Lead glass, 434,. from Jena . 6 Lead glass, 483, from Jena 0.2 Heaviest lead silicate, from Jena . (Mylius, C. C. 1888. 1313.) Solubility of various kinds of glass in H 2 O. The amounts dissolved from various kinds of glass by heating 5 hours with H 2 O were as follows. Yellow glass rich in alkali (13% K 2 O, 15% Na 2 O) . . 249 mg. Poor Thuringian glass (6.6% K 2 O, 16.5% Na 2 O) . . . 91.4 " Glass from Tittel and Co. (7.1% K 2 O, 14.3% Na 2 O) . . 30.4 " Bottle glass from Schilling (4.2% K 2 O, 11.9% Na 2 O) . . 13.0 " Bohemian glass from Kavalier (13.3% K 2 O, 11.4% Na 2 O) . 10.1 " Rhenish window glass (13.5% Na 2 0) . . . 8.4 " Lead crystal glass from Ehren- feld(12.1%K 2 O) . . 8.5 " Green bottle glass (1.3% K 2 O, 9.5 % Na 2 0) . . . .6.5 " GLASS 361 Solubility of various kinds of glass in H 2 O Continued. Thermometer glass 16III from Jena (14.0% Na 2 O, 7% ZnO) 6.4 mg Lead glass, No. 483, from Jena (47%PbO,7.3%K 2 0). . 3.3 " Lead silicate . . . 0.6 " (Mylius and Forster, B. 22. 1100.) By calculation from the electrical conduct- ivity of the solutions formed, various data were obtained by Kohlrausch (B. 24. 3565), which showed that different varieties of glass were attacked in very different degree by cold H2O, and, moreover, the amount dis- solved was proportionately much greater during the first few minutes of treatment with H 2 O than afterwards, and, furthermore, the rate of decrease was much faster for good glass than poor. Increase of temperature increased the rate of solubility to a very great degree, the increase for 1 C. being about 17%. In 7 hours at 80 half as much was dissolved as in 6 months at 18. Ex- tensive tables are given. (Kohlrausch, B. 24. 3651.) See also Kohlrausch (W. Ann. 44. 577). A very extensive research on the action of H 2 O on glass, with a historical review of the work previously done on the subject, has been published by Mylius and Forster. (Z. anal. 31. 241 .) The general results may be summed up as follows: 1. The solution of glass in H 2 is caused by a decomposition, by which free alkali is formed. 2. The silicic acid of the glass is brought into solution by a secondary reaction of the free alkali in the solution. 3. The constituents of the solution change according to the conditions of the diges- tion. 4. The amount of alkali going into solution from a given surface under certain conditions is a measure for the resistance of a glass under those conditions. 5. The rate of attack of glass surfaces by cold H 2 O decreases rapidly with the length of time of digestion, and finally approaches a constant value. 6. The solubility increases very rapidly with increase of temperature. 7. The ratio of the solubility of several kinds of glass is dependent on the tempera- ture. 8. From glasses which show the same ease of attack unequal amounts of substance may be dissolved. 9. The solubility of a glass is influenced by the condition of the surface from "weather- ing" by prolonged exposure to the GO 2 and H 2 O of the air. 10. The poorer a glass is the less will its solubility decrease by prolonged treatment with H 2 O. 11. A good glass is essentially less easily attacked after having been previously treated withH 2 O. 12. After treatment with H 2 O, glass sur- faces have the property of fixing alkali from the solutions formed, and giving it up again by a subsequent treatment with H 2 O. 13. Potassium glass is much more sol. than sodium glass (contrary to previous re- searches), but the difference decreases as the glass becomes richer in CaO. 14. In glass flasks which are to be only slightly attacked by cold or hot H 2 O, the CaO, alkalies, and SiO 2 must stand in a fixed rela- tion to each other. 15. Of the more common varieties of glass, lead flint glass is least sol. in H 2 O, but its surface is corroded, and it is easily decomp. by acids. (Mylius and Forster, Z. anal. 31. 241.) Bottle glass containing much AlzOs is easily attacked by acids. From powdered flint glass, boiling HC1 +Aq extracts K, but no Pb. (Griffiths.) Bottles of flint glass with (NH^COs+Aq became so fragile that on shaking pieces of glass were detached. (Griffiths.) All glass is decomp. by HF. Cone. H 3 PO4 also attacks all glass. Glass containing small amounts of SiO2 are attacked by H 2 SO 4 ; poorer glass by boiling HC1, HNOs, and aqua regia. (Berzelius.) Cone. HNOs does not act on flint glass at 145-150. (Sorby, C. R. 50. 990.) Glass of ordinary chemical apparatus gives up traces of metals to HC1 and HNO 3 + Aq, but hard Bohemian glass consisting of 75% SiO 2 , 15%K 2 O, 10% CaO, resists the action of warm cone, acids; also an easily fusible Na K glass with 77 % SiO 2 , 7.7% K 2 O, 5% Na 2 O, 10.3% CaO, is not easily attacked. (Stas.) KOH, and NaOH+Aq dissolve SiO 2 from glass the more easily the hotter and the more cone, the solutions are. (Miiller.) NH 4 OH, and (NH 4 ) 2 CO 3 +Aq attack many kinds of glass, especially flint glass. CaO 2 H 2 attacks a;lass appreciably at 45 and lower; still more strongly on boiling. (Lamy, A. ch. (5) 14. 155.) The action of various solvents on the glass mentioned on page 359 in Emmerling's ex- periments is as follows: The action of HCl+Aq containing 0.2 to 3% HC1 is practically null, but is increased either by dilution or concentration. A very small quantity (0.02%) HC1 added to H 2 O almost wholly prevents its action on glass. With HCl+Aq (11% HC1) a decrease of 4.2 mg. was noticed in the first hour, and only 3-4 mg. afterwards. The same is the case for 3NO 3 +Aq in still greater degree, 0.008% HNO 3 sufficing to nearly counteract the solvent action of H 2 0. H 2 SO 4 -f Aq has about double the solvent effect possessed by H 2 O. Oxalic and acetic acids both diminish the solvent action of H 2 O. The addition of even traces (0.04%) of 362 GLASS Na 2 CO 3 increases the solvent action, and this is further rapidly increased by an increase in the amount of Na 2 CO 3 . Na 2 CO 3 +Aq con- taining 1% Na 2 CO 3 dissolves about 10 times as much as pure H 2 O, i. e. about 35 mg. per hour. The above is also the case with KOH+Aq, but in even greater degree. KOH+Aq con- taining 0.025% KOH dissolved three times as much as pure H 2 0. (NH 4 ) 2 CO 3 +Aq has about the same action as H 2 O. With NH 4 OH+Aq (9% NH 3 ) 7 mg. de- crease for the first hour, and 3 mg. afterwards was noticed. The concentration of the NH 4 OH+Aq was apparently without effect. The addition of NH 4 C1 decreases the solv- ent action of H 2 O proportionately to the amount added, but with new flasks large amounts are dissolved. With NH 4 Cl+Aq (7%NH 4 C1) 4.2 mg. were dissolved in the first hour, and the amount dissolved gradually decreased to null after 24 hours on account of the liberation of HC1 by the decomp. of NH 4 C1. NaCl, KC1, KNO 3 , and Na 2 SO 4 show a similar behaviour to that of NH 4 C1. Na 2 HPO 4 +Aq containing 0.4% Na 2 HPO 4 has six times the solvent action of pure H 2 0. but the action is not increased by further concentration. In general, those salts the acids of which form insol. Ca salts, as Na 2 CO 3 , Na 2 SO 4 , Na ? HPO 4 , (NH 4 ) 2 C 2 O 4 , increase the solvent action of H 2 O, and this effect is greater the more concentrated the solution. KC1, KN0 3 , NH 4 C1, and CaCl 2 decrease the effect, and the stronger the solution the less is the action. All Na glass with approximately the above composition has the same power of resistance against H 2 O; Bohemian K glass shows a greater resistance, especially against acids. (Emmerling, A. 160. 257.) Action of various reagents on hard Bohemian glass. 100 ccm. substance dissolved mg. glass in 6 days at 100. H 2 O . . .10.0 H 2 S+Aq '' > . 8.7 Dil. (NH 4 ) 2 S+Aq. . 52.5 Cone. (NH 4 ) 2 S+Aq. 47.2 Conc.NH 4 OH+Aq . 42.5 Dil.NH 4 OH+Aq. . 7.7 NH 4 SH+Aq. .51.2 (Cowper, Chem. Soc. 41. 254.) Action of various solutions on glass of different composition. (The figures denote decrease in weight in mg. of a 100 ccm. flask.) Time 1 2 3 4 5 6 7 8 9 10 H 2 . H 2 S0 4 +Aq (25% H 2 S0 4 ) . HCl+Aq (12% HC1) NH 4 OH+Aq (10% NH 3 ) . Na 2 HPO 4 +Aq (12% Na 2 HPO 4 ) Na 2 CO 8 +Aq (2% Na 2 C0 3 ) 5 hrs. 3 3 3 3 3 62 '85 283 31 43 ie>6 29 35 27 62 81 130 17 8 4 11 64 124 13 7 2 8 40 50 9 6 1 7 35 45 7 5 1 7 34 42 7 5 1 6 30 42 5 5 5 15 26 4 3 5 12 25 Composition of above varieties of glass. i 2 3 4 5 6 7 8 9 10 Si0 2 . . A1 2 3 . CaO . K 2 O . Na 2 O . 76.22 4^27 19] 51 74.09 0.40 5.85 7.32 12.34 76.39 0.50 5.50 4.94 12.67 68.56 1.85 7.60 2.24 19.75 74.48 0.50 7.15 6.64 11.23 74.69 0.45 7.85 8.64 8.37 66.75 1.31 13.37 05.50 3.07 74.12 0.50 8.55 4.86 11.97 77.07 0.30 8.10 3.75 10.78 74.40 0.70 8.85 4.40 11.65 It is seen that glass which resists the attack of H 2 O also resists acids and alkalies, and that the relative resistance of all varieties to any of the solutions is the same. Therefore the action of H 2 O may be accepted as a criterion for judging of the resistance of a glass to all solvents. Glass No. 10, in which the molecu- lar ratio of SiO 2 :CaO:K 2 O(Na 2 O) is 8: 1:1.5, is recommended as best suited for chemical uses. (Weber and Sauer, B. 25. 70.) Mylius and Forster (B. 25. 97) recommend a glass in which the molecular ratio of SiO 2 : CaO: K 2 O (Na 2 O) is 7.2: 1: 1.1 as the best suited for chemical apparatus. In an exhaustive research on the action of aqueous solutions on glass, which cannot be given in full on account of its great length, the following conclusions are reached: 1. Solutions of caustic alkalies act on glass much more strongly than H 2 O, dissolving all the constituents ot the glass that is, the glass as such. Very dilute solutions form an ex- ception. 2. Ot the caustic alkalies, NaOH+Aq has the strongest action, then come KOH, NH 4 OH, and BaO 2 H 2 +Aq in the order named. 3. Increase in temperature increases the GLUCINUM STANNIC CHLORIDE 363 strength of the attack of alkalies very con- siderably. 4. At high temperatures, the ease with which glass is attacked increases at first rapidly with the concentration of the alkali, but afterwards more slowly. 5. At ordinary temperatures very concen- trated alkali solutions have less action on glass than dil. solutions. 6. Solutions of pure alkalies, if not too cone., act less on glass than when contamin- ated with small amounts of SiO 2 . 7. Alkali carbonates +Aq attack glass much more than H 2 O, even when they are very dilute. The action corresponds less to that of the caustic alkalies than to that of other salts. With equivalent concentration, Na 2 CO 3 -f Aq has a stonger action than K 2 CO 3 +Aq. 8. The action of salt solutions on glass is a compound one, depending both on the con- centration and the kind of salt dissolved, and is made up of the action of the H 2 O and the salt in solution. 9. Each kind of attack is differently in- fluenced by the composition of the glass. 10. Solutions of those salts, the acids of which form insol. Ca salts, have a stronger action than H 2 O, and the action increases with the concentration. 11. Solutions of those salts, the acids of which form sol. Ca salts, have less action than H 2 0, and the action decreases with the concentration. (Forster, B. 25. 2494.) Data on this subject published since the first edition of this work have not been con- sidered. Glucinic acid. Potassium glucinate, K 2 G1O 2 . Very deliquescent. Sol. in H 2 O and acids. (Kriiss and Moraht, B. 23. 733.) Glucinum (Beryllium), Gl. Not attacked by hot or cold H 2 O. Sol. in cold dil. HNOs+Aq. (Wohler, Pogg. 13. 577.) Sol. only in boiling cone. HNO 3 +Aq. (Debray, A. ch. (3) 44. 5.) Sol. in dil. HCl+Aq. dil. and cone. H 2 S0 4 + Aq, and KOH+Aq, but insol. in NH 4 OH+ Aq. (Wohler, Debray.) Sol. in hot HC1, hot cone. HNO 3 , and hot cone. H 2 SO 4 . (Lebeau, A. ch. 1899, (7), 16. 474.) Glucinium azoimide, G1N 3 . Decomp. by hot H 2 O. (Curtius, J. pr. 1898, (2), 58. 292.) Glucinum borocarbide, 3G1 2 C, B 6 C. Insol. in H 2 O. Easily sol. in mineral acids especially HN0 3 . (Lebeau, A. ch. 1899, (7) 16.481.) C 4 B 6 G1 6 . Stable in air. Easily sol. in mineral acids, cone, and dil. (Lebeau, C. R. 1898, 126. 1349.) Glucinum bromide, GlBr 2 . Sol. in H 2 O with evolution of much heat. (Wohler.) Sol. in abs. alcohol. (Lebeau, A. ch. 1899, (7) 16. 484.) Glucinum carbide, G1 2 C. Decomp. by H 2 O. Slowly attacked by cold or hot cone. HC1 and HNO 3 . Gradu- ally but completely sol. in dil. acids. (Le- beau, A. ch. 1899, (7), 16. 476.) G1C 2 . Not easily decomp. by strong acids. Easily sol. with decomp. in dil acids. (Lebeau, C. R. 1895, 121. 497.) Glucinum chloride, G1C1 2 . Anhydrous. Fumes and deliquesces in air. Sol. in H 2 O with hissing and evolution of much heat. Easily sol. in alcohol. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Sol. in alcohol and ether. SI. sol. in C 6 H 6 , CHCls, C1 4 and CS 2 . (Lebeau, A. ch. 1899, (7) 16. 493.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +4H 2 O. Very hydroscopic. Easily sol. in H 2 O and in alcohol. (Mie- leitner, Z. anorg. 1913, 80. 73.) Glucinum chloride ammonia, G1C1 2 , 4NH S . (Mieleitner, Z. anorg. 1913, 80. 73.) Glucinum chloride iodine trichloride, 2IC1 3 , G1C1 2 +8H 2 0. Hygroscopic. (Weinland, Z. anorg. 1902, 30. 140.) Glucinum ferric chloride, G1C1 2 , FeCl 3 +H 2 O. Decomp. by H 2 O. (Neumann, A. 244. 329.) Glucinum mercuric chloride, G1C1 2 , 3HgCl 2 + 6H 2 O. Sol. in H 2 0. (Atterberg, B. 6. 1288.) Glucinum thallic chloride, 3G1C1 2 , 2T1C1 3 . Cryst. from HC1 solution. (Neumann, A. 244. 348.) Glucinum stannic chloride. See Chlorostannate, glucinum. 364 GLUCINUM FLUORIDE, BASIC Glucinum fluoride, basic, 2G1O, 5G1F 2 . Solubility of freshly pptd. G1O 2 H 2 in NaOH + Sol. in H 2 O. (Lebeau, A. ch. 1899, (7) 16. A O A \ Aq at room temperature. 484.) millimols Na per 1. G. G1O dissolved in 1 1. Glucinum fluoride, G1F 2 . 649 3.6 Deliquescent. Sol. in H 2 O. Insol. in anhydrous HF. Sol. in alcohol. (Lebeau, C. R. 1898, 126. 1421.) 540 540 483 ooo 2.92 2.53 1.69 1f\ A Sol. in H 2 O in all proportions. Somewhat sol. in abs. alcohol. Easily sol. in 90% al- 080 388 qon .64 1.53 1AJC cohol, also in a mixture of alcohol and ether. OoO qnrj .40 1C) A Insol. in anhydrous HF. (Lebeau, A. ch. oyu . 4*1 1899, (7) 16. 484.) In the first two cases the values were ob- Glucinum potassium fluoride, G1F 2 , KF. SI. sol. in H 2 O. (Awdejew.) Much more sol. in hot than cold H 2 O. (Berzelius.) G1F 2 , 2KF. Sol. in about 50 pts. H 2 O at 20, and 19 pts. boiling H 2 O. (Marignac.) Glucinum sodium fluoride, G1F 2 , 2NaF. Sol. in 34 pts. H 2 O at 100, and 68 pts. at 18. (Marignac.) Glucinum hydroxide, G1O 2 H 2 . Easily sol. in acids. Sol. in H 2 SO 3 +Aq. Sol. in CO 2 +Aq; 100 com. sat. CO 2 +Aq dissolve 0.0185 g. G1O. (Sestini, Gazz. ch. it. 20. 313.) Also sol. in KOH, NaOH, NH 4 OH, or (NH 4 ) 2 CO 3 +Aq, especially when freshly pre- cipitated; also in Na 2 CO 3 , or K 2 CO 3 +Aq. (Debray.) Insol. hi NH 4 OH+Aq containing NH 4 C1+ Aq. Very si. sol. in Li 2 CO 3 +Aq. (Gmelin.) Sol. in H 2 SO 4 +Aq. (Berthier.) Sol. in BaO 2 H 2 +Aa, from which it is pptd. by NH 4 salts, but not by boiling. Sol. in boiling NH 4 Cl+Aq when freshly pptd. Sol. in NH 4 F+Aq. (Helmholt, Z. anorg. 3. 130.) Solubility of G1O 2 H 2 in NaOH+Aq. G. Na in 20 com. 0.3358 0.6717 0.8725 1.7346 G. Gl. in 20 ccm. 0.0358 0.0882 0.1175 0.2847 (Rubenbauer, Z. anorg. 1902, 30. 334.) When glucinum hydroxide is treated with alkali, more dissolves at first than corresponds with the true equilibrium under the prevail- ing conditions, for such solutions spontane- ously deposit more or less glucinum hydrox- ide according to the concentration. (Ruben- bauer.) tained by adding to GlCl 2 +Aq at 0, ice cold NH 4 OH and treating the ppt. with NaOH+ Aq. In the remaining cases by dissolving basic G1CO 3 in HC1 and pouring into NaOH + Aq. (Haber, Z. anorg. 1904, 38. 386.) Solubility of G1O 2 H 2 , which is one week old' in NaOH+Aq at t. NaOH 1-N 2-N 1-N 2-N 2-N 20-23 20-23 20-23 50-53 50-53 50-53 100 100 100 G. G1O in 1 1. 0.060 0.170 0.570 0.080 0.230 0.900 0.080 0.290 1.020 (Haber.) Solubility of G1O 2 H 2 in NaOH+Aq at 25 C G. mols. Na 0.268 0.318 0.446 0.526 0.563 0.801 0.854 Gl. 0.0330 0.0492 0.0841 0.089 0.101 0.143 0.202 (Wood, Chem. Soc. 1910, 97. 884.) Insol. in NH 4 OH+Aq and in alkyl amines. (Renz, B. 1903, 36. 2753.) Sol. in GlSO 4 +Aq. (Parsons, J. phys. Chem. 1907, 11. 658.) A form insol. in acids and alkalies can be obtained by sufficiently long heating in boil- ing H 2 O, Na 2 CO 3 +Aq, NH 4 OH+Aq, or solutions of NaOH or KOH so dil. that the GIO 2 H 2 is either insol. or very si. sol. therein, (van Oordt, C. C. 1906, 1. 108.) 100 ccm. of glycerine+Aq containing about 60% by vol. of glycerine dissolve 0.1 g. G1O. (Muller, Z. anorg. 1905, 43. 322.) Contains VsHaO (Schaffgotsch) ; 4 /sH 2 O (At- terberg). GLUCINUM SELENIDE 365 Solubility of G1O 2 H 2 , which has been boiled with alkali, in various solvents. Alkali used Time Solvent Solubility 10-N NaOH NaOH NaOH 23/Shrs. Long time 2hrs. 0.106-X XaOH 0.39-X XaOH 0.97-X XaOH 2.0-X XaOH 2.0-X XaOH 10-X K 2 CO 2 Dil. HC1 Hot cone. HC1 Dil. acetic acid 1 mol. G1O 2 H 2 331 mole XaOH 1 mol. G1O 2 H 2 183 mole XaOH 1 mol. G1O 2 H 2 91.8 mole XaOH 1 mol. G1O 2 H 2 49 mole XaOH 1 mol. G1O 2 H 2 49 mole XaOH Insol. SI. sol. Slowly sol. Almost insol. KOH TiU flocculent ppt. appeared 1-X KOH 1-X XaOH Warm dil. HC1 Insol. it Sol. i^-N Xa 2 C0 3 f Jf-X Xa,CO, for \ then Vio-N Na 2 CO 3 [ for 3hrs. 3 hrs. and 4hrs. 1-X XaOH Dil. HC1 1-X XaOH Dil. HC1 Easily sol. SI. sol. Slowly sol. i^-X K 2 CO 3 10-X K 2 CO 3 6 hrs. Short time 10-X K,CO 3 1-X XaOH Cold 10-X K 2 CO 3 Insol. Easily sol. Very slowly sol. XH 4 OH 5 hrs. 24-X XaOH Very si. sol. (Haber.) Glucinum iodide, G1I 2 . Sol. in H 2 with evolution of much heat. (Wohler.) Decomp. in moist air and by H 2 O. Sol. in abs. alcohol. Insol. in most neutral organic solvents, as benzene, toluene, etc. (Lebeau, C. R. 1898, 126. 1273.) Insol. in CeH 6 , CvH s and oil of turpentine. Easily sol. in CS 2 . Sol. in anhydrous alcohols without evolution of heat. (Lebeau, A. ch. 1899, (7) 16. 490.) Glucinum iodide ammonia, 2G1I 2 , 3XH 3 . Ppt. (Lebeau, A. ch. 1899, (7) 16. 492.) Glucinum oxide, G1O. Crystalline. Insol. in acids except cone. H 2 SO 4 . (Ebelmen, C. R. 32. 710.) Amorphous. Absolutely insol. in H 2 O. The higher the temp, to which the substance has been heated the more insol. is it in acids. Insol. in XH 4 OH+Aq or (XH 4 ) 2 CO 8 +Aq. Insol. in cone. XH 4 Cl+Aq, or KOH, and XaOH+Aq. (Rose.) When obtained by ignition of G1SO 4 , it is very slowly but completely sol. in HC1, and H 2 SO 4 +Aq. (Rose.) Insol. in hydracids. Sol. in cone. H 2 S0 4 . (Lebeau, C. R. 1896, 123. 819.) Insol. in liquid XH 3 . (Gore, Am. ch. J. 1898, 20. 828.) Glucinum peroxide basic, 2G1O 2 , 3G1O. +8KH 2 O. (Komarovski, Chem. 1913, 104 (2) 707.) Soc. Glucinum oxybromides. Sol. in H 2 O if three or less equivalents of base are present to one of acid; insol. if more of the base is present. (Ordway, Am. J. Sci. (2) 26. 207.) Glucinum oxychloride, G1 2 OC1 3 = G1O, GlClj. Insol. in H 2 O. 3G1C1 2 , 2G1O+2H 2 O (?). Sol. in H 2 O. GlCl 2 ! r 3G10+3H 2 (?). Sol. in H 2 O,.biit solution soon becomes cloudy and deposits a fine ppt. By boiling the solution it is decomp. into above salt, and G1C1 2 , 12G1O 2 H 2 + 10H 2 O, which is insol. hi H 2 O; decomp. into G1O 2 H 2 by washing. Sol. in acids. (Atter- berg.) Glucinum oxyfluoride, 5G1F 2 , 2G1O. Readily sol. in H 2 O. (Lebeau, C. R. 1898,. 126. 1419.) Glucinum phosphide. Decomp. by H 2 O. (Wohler.) Glucinum selenide. SI. sol. in H 2 O. (Berzelius.) 366 GLUCINUM SULPHIDE Glucinum sulphide. Slowly sol. without decomp. in H 2 O, but easily decomp. by acids. (Wohler.) Gold, Au. Gold which has been pptd. from AuCl 3 + Aq by FeS0 4 is si. sol. in HC1. (Awerkiew, Z. anorg. 1909, 61. 10.) Not attacked by H 2 O. Insol. in HNO 3 or HCl+Aq. Easily sol. in aqua regia or any mixture evolving Cl or Br. Sol. in selenic acid, or antimonic acid+Aq; less easily in arsenic acid+Aq. Sol. in mixtures of HC1 and nitrates, or HNO 3 and chlorides; also in (NaCl+KNO 3 +K 2 Al 2 (SO 4 ) 4 )+Aq (?). Insol in H 2 SO 4 , except in presence of KMnO 4 , HNO 3 , or HIO 3 . Sol. in a solution of I in ether in direct sunlight. Sol. in solutions of ferric, and cupric salts. Sol. in HCl+Aq containing H 2 CrO 4 , H 2 MnO 4 , H 2 SeO 4 , H 3 AsO 4 , or FeCl 3 . (Wurtz). Attacked by fuming HC1 (sp. gr. 1.178) at ord. temp, in direct light, especially in the presence of a trace of MnCl 2 , but not attacked in the dark even in the presence of this salt. (Berthelot, C. R. 1904, 138. 1298.) 100 com. hot cone. HC1 dissolve 0.008 g. yellow Au powder in 4 hours. (Hanriot and Raoult, C. R. 1912, 166. 1086.) Upon boiling 25 and 50 cc. HCl+Aq (sp. gr. 1.178), dil. to 125 cc. with 250 mg. sheet Au x /s in. square, 0.009 in. thick, weighing 250 mg. for several hours, there was no loss of weight of Au. (McCaughey, J. Am. Chem. Soc. 1909, 31. 1263.) From 5 g. finely divided ordinary yellow gold; 100 cc. HNO 3 of 22 B. dissolve 0.002 g. 100 00. HNO 3 of 32 B. dissolve 0.0119 g. in 2 hrs. 100 cc. HNO 8 of 36 B. dissolve 0.028 g. in 2 hrs. 100 cc. HNO 3 monohydrate dissolve 0.076 g. in 2 hrs. (Hanriot and Raoult, C. R. 1912, 166. 1085.) From 5 g. brown gold: 100 ccm. HNO 8 of 22 Baume dissolve 0.006 g. in 2 hrs. 100 ccm. HNO 3 of 32 Baume dissolve 0.039 g. in 2 hrs. 100 ccm. HNO 3 of 36 Baume dissolve 0.078 g. in 2 hrs. 100 ccm. HNO 3 monohydrate dissolve 1.540 g. in 2 hrs. (Hanriot and Raoult.) SI. sol. in boiling HNO 3 (sp. gr. = 1.42). The solution deposits Au by standing several days. (Dewey, J. Am. Chem. Soc. 1910, 32. 320.) Best composition of aqua regia for dissolv- ing Au is 200 cc. HC1 (sp. gr. 1.1946) 45 cc. HNO 3 (sp. gr. 1.4) and 245 cc. H 2 0. 1 pt. Au is sol. in 4.3 pts. of such a mixture. (Priwoznik, C. C. 1910, II. 1743.) Sol. in 1 pt. HNO 3 +4 pts. HC1 as repre- senting the most economical mixture. (Pri- woznik, Chem. Soc. 1911, 100. (2), 484.) Easily sol. in nitrosulphonic acid from sul- phuric acid manufacture, when mixed with equal parts cone. HCl+Aq. (Borntrager, Rep. anal. Ch. 1887. 741.) Sol. in hot cone. H 2 SO 4 in the presence of MnO 2 , Mn 2 O 3 , Mn 3 O 4 , PbO 2 , Pb 2 3 , Pb 3 O 4 , CrO 3 , CrO 4 and Ni 2 3 . Solution also takes place slowly in the cold. Sol. in hot H 2 SO 4 + KMnO 4 . Slowly sol. in cold, more rapidly in hot H 2 SO 4 +HN0 3 . (Lenher, J. Am. Chem. Soc. 1904, 26. 550.) Sol. in a hot solution of crystalline telluric acid in H 2 SO 4 or H 3 PO 4 . Sol. in hot H 3 PO 4 in the presence of MnO 2 , Mn 2 O 3 , Mn 3 O 4 , the higher oxides of lead, CrO 3 , chromium tetroxide and nickelic oxide. Solution takes place more slowly in the cold. Sol. in hot H 3 PO 4 in the presence of KMn0 4 . Slowly sol. in a cold, more rapidly sol. in a hot mixture of H 3 PO 4 and HN0 3 . Sol. in hot arsenic acid in the presence of MnO 2 , Mn 2 O 3 and Mn 3 O 4 . (Lenher, J. Am. Chem. Soc. 1904, 26. 550.) Gold leaf is not attacked by cold cone. H 2 SeO 4 , when completely free from halogens, but is dissolved by cone. H 2 SeO 4 at 300. (Lenher, J. Am. Chem. Soc. 1902, 24. 354.) Solubility of thin sheet Au in HC1 solution of iron alum. Mg. Au dissolved Time, hours lg. Fe 1 g. Fe 2g. Fe 2g. Fe 25 cc. HC1 50 cc. HC1 25 cc. HC 50 cc. HC1 Temp. 38-43. 16 1.00 1.30 1.08 1.47 22 1.12 1.55 1.20 1.81 40 1.52 2.15 1.82 2.75 46 1.71 2.34 2.02 2.95 64 1.96 3.10 2.60 3.79 72 2. 12 3.30 2.83 4.05 89 2^32 3.65 3.22 4.65 100 2.40 3.76 3.38 4.81 113 2.45 3.95 3.51 5.12 124 2.60 4.09 3.63 5.39 161 2.78 4.36 3.95 5.96 185 2.90 4.49 4.11 6.22 Temp. 98-100. 1 1.13 0.78 1.15 1.27 2 1.99 1.74 2.56 2.86 4 3.46 3.31 4.55 5.06 16 10.09 11.37 13.15 15.56 20 12.20 13.72 15.59 19.41 24 14.37 16.49 17.96 23.29 36 17.38 23.27 22.07 31.73 42 18.79 26.30 24.62 35.29 54 20.94 31.39 29.49 42.11 59^ 21.64 33.12 30.64 44.43 GOLD 367 The solution contained the given amounts of Fe as iron alum, the sp. gr. of the HC1 was 1.178, and the solutions diluted to 125 cc. (McCaughey, J. Am. Chem. Soc. 1909, 31. 1263.) The solvent action of ferric salt occurs even in presence of a ferrous salt, but de- creases with increase of concentration of ferrous salt. (McCaughey.) Solubility of thin sheet Au in HC1 solution of CuCl 2 . Solubility of Au which has been pptd. from AuCl 3 -|-Aq by various precipitants in HCl+formaldehyde. HCHO (40%) ccm. HCl (1.19) ccm. Au dis- solved g- Au used was pptd. from AuCls+Aq. by 150 100 125 100 150 250 500 100 100 100 150 250 150 100 100 100 150 100 25 200 150 250 500 500 200 200 300 125 75 200 200 100 0.0007 0.0006 0.0008 0.0009 0.0003 0.0002 0.0008 0.0004 0.0006 0.001 0.0013 0.0008 0.0006 0.0005 FeS0 4 a, (C sugar oxalic acid n FeS0 4 oxalic acid a sugar ti FeS0 4 it ECHO (( Time, hours Mg. Au dissolved 1 g. Cu 25cc.HCl 1 g. Cu 50 cc. HC1 2g. Cu 25 cc. HC1 2g. Cu 50 cc. HC1 Temp. 38-43. 19 25 43 493^ 66^ 78 91 102 139 163 0.03 0.09 0.10 0.12 0.11 0.14 0.14 0.16 0.18 0.23 0.26 0.36 0.54 0.61 0.76 0.87 0.92 1.02 1.34 1.60 0.05 0.05 0.14 0.15 0.17 0.22 0.24 0.27 0.32 0.39 0.39 0.54 0.94 1.07 1.40 1.58 1.75 1.90 2.45 2.84 180 360 360 209 540 720 720 400 0.001 0.0019 0.0013 FeS0 4 sugar FeSO 4 In the last four cases the solubility was determined at the ordinary temp.; in the first sixteen the gold was boiled with the mixture of HCl and HCHO. (Awerkiew, Z. anorg. 1909, 61. 3.) Solubility of Au in boiling HC1+ paraformaldehyde. Temp. 98-100. 1 4 16 20 26 38 43 48 60 0.15 0.55 1.34 1.63 2.17 3.13 3.61 4,07 4.82 0.34 1.23 5.00 6.5? 9.13 13.98 16.54 19.26 26.37 0.17 0.55 2.12 2.78 3.59 5.07 5.77 6.26 7.47 0.46 1.35 8.80 11.86 15.70 23.14 26.62 30.80 39.09 (CH 2 0) 3 g- HCl (1.19) g. Dissolved Au g. Au used was pptd. from AuCls+Aq. by 5 5 25 20 20 20 20 20 20 40 20 20 10 10 60 25 25 125 400 400 400 400 400 400 400 300 300 200 200 120 0.0005 0.0004 0.006 0.0024 0.0034 0.003 0.0065 0.0044 0.0005 0.001 0.0024 0.003 0.0008 0.0006 0.0015 FeSO 4 oxalic' acid sugar CHOH CH 3 OH u sugar formic acid it CH 3 OH FeS0 4 14 CH 8 OH oxalic acid FeS0 4 Conditions the same as above for HC1+ iron alum. (McCaughey.) Finely powdered gold is sol. in cone HC1 in the presence of alcohol, etc. 0.0302 g. Au. is sol. in 100 cc. HCl +100 cc. CH 3 OH. 0.0230 g. Au. is sol. in 100 cc. HC1+100 cc. CHC1 3 . 0.0066 g. Au. is sol. in 100 cc. HC1+100 cc. C 2 H 5 OH. 0.0190 g. Au. is sol. in 100 cc. HC1+100 cc. C 5 H n OH. 0.0125 g. Au. is sol. in 100 cc. HCl-f-50 cc. CC1 3 CH(OH) 2 . (Awerkiew.) (Awerkiew, C. C. 1908, II. 1566.) 368 GOLD Solubility of Au in boiling HCl-f methyl alcohol. Solubility of Au in boiling HCl+phenol. CeHsOH g- HCl (1.19) g. Dissolved Au g. Au used was pptd. from AuCb +Aq. by CHsOH (99%) ccm. HCl (1.19) ccm. Dissolved Au g. Au used was pptd. from AuCh+Aq. by 10+25 10 20 25 25 50 25 25 100 40 50 100 150 200 250 250 0.001 0.0004 0.0003 0.0005 0.0005 0.0005 0.0012 C 6 H 6 OH oxalic acid u FeSO 4 HCOH u FeS0 4 1C 100 150 150 25 50 50 50 50 50 100 500 1000 50 100 100 75 90 75 80 100 100 50 100 150 150 25 50 50 50 50 50 100 500 1000 100 200 300 25 30 25 20 50 50 200 0.0302 0.0043 0.028 0.001 0.0002 0.0005 0.0002 0.0015 0.002 0.0009 0.0128 0.0281 0.0084 0.0006 0.005 0.005 0.0014 0.0005 0.0018 0.0008 0.001 FeSO 4 oxalic acid sugar CH 4 OH oxalic acid CH 3 OH oxalic acid FeSO 4 u oxalic acid FeS0 4 it (i (i (i HCOH <( u tt FeSO 4 CH 3 OH it (Awerkiew.) Solubility of Au in boiling HCl + chloroform. CHCh g. HCl (1.19) g. Dissolved Aug. Au used was pptd. from AuCU+Aq. by 50 100 100 150 200 250 300 100 100 100 50 400 250 300 0.0009 0.023 0.0017 .0.0012 0.0024 0.002 0.0106 FeS0 4 a (i p NH 2- Correct formula for p?/r0phosphonamic acid of Gladstone. (Mente, A. 248. 241.) Imidocfo'phosphoric acid, HO PO < I 1 > PO OH. Correct name for p?/rophosphaniic acid. (Mente, A. 248. 251.) Barium imidodiphosphate, Ba/O > po SI. sol. in H 2 O. (Mente, A. 248. 243.) Barium imidocfo'phosphate, basic, /O. po / > N Ba N X POH3s 2H 2 O. Ppt. (Mente.) 396 IMIDOPHOSPHATE, FERRIC Ferric imidocftphosphate. SI. sol. in cone, acids. (Mente, A. 248. 241.) Silver imidod? phosphate, Ag 3 H 2 P 2 NO6. Insol. in H 2 O. (Stokes, Am. Ch. J. 1896, 18. 660.) Ag 4 HP 2 NO 6 . Ppt. (Stokes.) Dumidodiphosphoric acid, HO PO < Ng > po OH. Correct name for p?/rophosphocfaamic acid. (Mente, A. 248. 241.) Barium cfoimidocfophosphate, SI. sol. in dil. acids. (Mente, A. 248. 244.) Sodium (Mmidocftphosphate, basic, /ONa \ONa. SI. sol. in H 2 O. (Mente, A. 248. 245.) ZH'imidoJn'phosphoric acid. Silver dumido^nphosphate, Ag3H 4 P 3 N 2 O8. Insol. in H 2 O. Very sol. in NH 4 OH-fAq. Rather si. sol. in dil. HNO 3 . (Stokes, Am Ch. J. 1896, 18. 657.) Ag 5 H 2 P 3 N 2 O 8 . Insol. in H 2 O. Very sol. in NH 4 OH+Aq. Decomp. by HNO 3 . (Stokes.) Tnsodiumdumido^nphosphate, P 3 N 2 8 H 4 Na 3 . Sol. in H 2 O. Insol. in alcohol. (Stokes.) Tn'imidotetfraphosphoric acid. Silver 2nimidotemphosphate. Ag 4 H 5 P 4 N 3 O ]0 . Ppt. (Stokes, Am. Ch. J. 1898, 20. 755.) Sodium inimidofefraphosphate, P 4 N 3 10 H 5 Na 4 . Easily sol. in H 2 O; insol. in sodium acetate solution and dil. alcohol. (Stokes, Am. Ch. J. 1898, 20. 754.) Imidosulphamide, NH 2 .SO 2 .NH.SO 2 .NH 2 . "Sulphamide" of Traube. Very sol. in H 2 O with decomp. appreci- ably sol. in cold, easily sol. in hot methyl and ethyl alcohol. Insol. in C 6 H 6 , and CHC1 3 . SI. sol. in ether, cold and hot acetic ether and glacial acetic acid. Moderately stable toward alkalies. (Hantzsch and Stuer, B. 1905, 38. 1022.) Ammonium imidosulphamide, NH 4 S 2 O 4 N 3 H 4 . (Hantzch and Stuer.) Imidosulphonic acid, Ammondisulphonic acid of Glaus. Known only in aqueous solution. (Divers and Haga, Chem. Soc. 61. 943.) Very unstable. (Berglund, B. 9. 252.) Ammonium imidosulphonate, basic, (NH 4 )N(S0 3 NH 4 ) 2 Sol. in 9 pts. of H 2 O. Solution is stable. Insol. in alcohol. SI. sol. in warm cone. H 2 SO 4 without de- comp. (Rose, Pogg. 1834, 32. 81.) Much less sol. than the neutral salt. (Berg- lund, B. 9. 255.) = "Parasulphatammon." +H 2 O. Gradually efflorescent. Sol. in H 2 O with subsequent decomp. (Divers and Ammonium imidosulphonate, HN(SO 3 NH 4 ) 2 . Sol. in H 2 O. (Raschig, A. 241. 161.) Ammonium barium imidosulphonate, NH 4 BaN(SO 3 ) 2 (?). Very si. sol. in H 2 O. (Divers and Haga.) (NH 4 ) 2 Ba 5 N 4 (S0 8 ) 8 +8H 2 O. (D. and H.) Ammonium calcium imidosulphonate. (Divers, Chem. Soc. 1892, 61. 968.) Ammonium sodium imidosulphonate, NH 4 Na 5 N 2 (SO 3 ) 4 +7H 2 O, and 2^H 2 O. Very si. sol. in NH 4 OH+Aq. (Divers and Haga.) Ammonium sodium imidosulphonate nitrate, HN(S0 3 NH 4 ) 2 , NaN0 3 . Very sol. in H 2 O. (Divers and Haga.) Barium imidosulphonate, Ba[N(SO 3 ) 2 Ba] 2 + 5H 2 O. SI. sol. in H 2 O. (Berglund, B. 9. 255.) Sol. in dil. HNO 3 +Aq without decomp. (Divers and Haga.) HN(SO 3 ) 2 Ba+H 2 O. Moderately sol. in H 2 O. (D. and H.) Barium mercury imidosulphonate, N 2 Hg(S0 3 ) 4 Ba 2 . Almost insol. in cold H 2 O. (Divers and Haga, Chem. Soc. 1892, 61. 977.) Barium sodium imidosulphonate, Ba 1 iNa 8 N 10 (SO 3 ) 2 o + 13H 2 O. Sparingly sol. in H 2 O. Readily sol. in HNO 3 or HC1. (Divers, Chem. Soc. 1892, 61. 967.) IMIDOSULPHOPHOSPHATE, AMMONIUM HYDROGEN 397 Calcium imidosulphonate, Ca[N(SO 3 ) 2 Ca] 2 + 6H 2 0. SI. sol. in H 2 O. (Berglund.) Calcium mercury imidosulphonate, N 2 Hg[(S0 3 ) 2 Ca] 2 . Very sol. in H 2 O. (Divers and Haga, Chem. Soc. 1896, 69. 1629.) Calcium mercury imidosulphonate chloride, (NS,0Ca),Hg,Cl+12H,0. Decomp. by H 2 O. (Divers and Haga, Chem. Soc. 1896, 69. 1629.) Calcium sodium imidosulphonate, NaN(SO 3 ) 2 Ca+3H 2 O. SI. sol. in cold H 2 0. (Divers and Haga, Chem. Soc. 61. 968.) Lead imidosulphonate, (PbOHSO 3 ) 2 NPbOH. Ppt. (Berglund.) Insol. in H 2 O. (Divers and Haga.) (PbOH) 3 N(SO 3 ) 2 , PbO. Insol. in H 2 O; easily sol. in dil. HNO 3 +Aq. (D. and H.) Mercurous imidosulphonate, basic, [Hg 2 N(S0 3 ) 2 Hg 2 ] 2 O+6H 2 O. Much more sol. in dil. HNO 3 than mer- curic salt. Sol. in cold cone. KI+Aq, leaving half Hg as metal. (Divers and Haga, Chem. Soc. 1896, 69. 1631.) Mercuric imidosulphonate, basic, NH(S0 3 , HgO) 2 Hg. Easily decomp. (Divers and Haga.) Mercuromercuric imidosulphonate, [HgnN(SOa)HgI],0+3H,0. (Divers and Haga.) [HgnN(S0 3 ) 2 Hg' 2 ] 2 0, [Hg' 2 N(S0 3 ) 2 H g2 , HgnN(SO 3 ) 2 Hg I 2 ]O+6H 2 O. (Divers and Haga.) Mercury sodium imidosulphonate, basic, Hg 2 ON(SO 3 ) 2 Na+2H 2 O. Slightly efflorescent. Decomp. by long washing with H 2 O. Much more readily sol. in HC1 than 'in HNO 3 or H 2 SO 4 and is wholly decomp. thereby. (Divers and Haga, Chem. Soc. 1892, 61. 983.) Mercury sodium imidosulphonate, HgN 2 (SO 3 Na) 4 +6H 2 O. Sparingly sol. in cold H 2 O. Readily sol in HNO 3 and in HC1. Decomp. by HC1 immediately, but not by HN0 3 . (Divers and Haga, Chem. Soc. 1892, 61. 981.) Potassium imidosulphonate, basic, KN(S0 3 K) 2 +H 2 0. Sol. in H 2 O. (Raschig, A. 241. 161.) Less sol. than neutral salt. (Berglund.) Potassium imidosulphonate, HN(SO 3 K) 2 . Sol. in H 2 O. (Raschig, A. 241. 161.) = Potassium ammoncfosulphonate of Glaus. Difficultly sol. in cold H 2 O, sol. in 64 pts. H 2 O at 23. (Fremy.) Gradually decomp. by boiling. (Glaus.) SI. sol. in H 2 O. (Berglund, B. 9. 255.) Potassium mercury imidosulphonate, N 2 Hg(SO 3 K) 4 +4H 2 O. See Mercurimidosulphonic acid. Silver imidosulphonate, AgN(SO 3 Ag) 2 . SI. sol. in H 2 O. (Berglund.) Silver sodium imidosulphonate, NaN(S0 3 Ag) 2 . SI. sol. in H 2 O. (Divers and Haga.) AgNa 2 N(S0 3 ) 2 . SI. sol. in H 2 O, but more sol. than the two preceding salts. (D. and H.) Sodium imidosulphonate, HN(SO 3 Na) 2 + 2H 2 O. Not efflorescent. Very sol. in H 2 O. (Diver and Haga.) NaN(SO 3 Na) 2 +12H 2 O, Efflorescent. SI. sol. in cold H 2 O, but very sol. in hot H 2 O. Sol. in 5.4 pts. H 2 at 27.5. (Divers and Haga.) Sodium strontium imidosulphonate, SrNaNS 2 O 6 +3H 2 O. SI. sol. in H 2 O. (Divers, Chem. Soc. 1896, 69. 1625.) Strontium imidosulphonate, Sr[N(S0 3 ) 2 Sr] 2 +6H 2 0. SI. sol. in H 2 O. (Berglund.) +12H 2 O. Somewhat sol. in hot H 2 O. (Divers, Chem. Soc. 1896, 69. 1623.) Imido2nsulpho0r/w>phosphoric acid, NH:P(SH) 3 . Insol. in CS 2 and readily decomp. by H 2 O. (Stock, B. 1906, 39. 1991.) Ammonium imido/nsulphoo? ^ophosphate, NHP(SNH 4 ) 3 . Very hydroscopic. Loses NH 3 in the air. Somewhat sol. in liquid NH 3 . Decomp. by any other solvent in which it is sol. (Stock, B. 1906, 39. 1983.) Diammonium hydrogen imido^nsulphoor^o- phosphate, SHP(SNH 4 ) 2 NH. (Stock, B. 1906, 39. 1983.) Ammonium ^'hydrogen SNH 4 P(SH) 2 NH. (Stock.) 398 IMIDOSULPHOPHOSPHATE, SODIUM HYDROGEN Di sodium hydrogen imido^nsulphcor^ophos- phate, SHP(SNa) 2 NH. Very easily sol. in H 2 O. Decomp. by H 2 O. Somewhat sol. in methyl and ethyl alcohol. (Stock.) Z)iimidopentasulphop2/rophosphoric acid, P 2 S 5 N 2 H 6 . Not known in pure state. (Stock, B. 1906, 39. 1967.) Ammonium diimidopentasvlphopyrophos- phate, S[P(SNH 4 ) 2 NH] 2 . Very hydroscopic. Sol. in cold H 2 O with decomp. (Stock, B. 1906, 39. 1978.) Inidosulphurous acid. Ammonium imidosulphite, HN(SO 2 NH 4 ) 2 . Somewhat deliquescent. Very unstable. Easily sol. in H 2 O with decomp; into thiosulphate and amidosul- phate. Insol. in alcohol. (Divers and Ogawa, Chem. Soc. 1901, 79. 1100.) Ammonium barium imidosulphite, Ba(SO 2 NHSO 2 NH 4 ) 2 . Sol. in H 2 O. (Divers, Chem. Soc. 1901, 79. 1102.) Potassium imidosulphite, NH(S0 2 K) 2 . (Divers and Owaga, Proc. Chem. Soc. 1900, 16. 113.) Very sol. in H 2 0. (Divers, Chem. Soc. 1901, 79. 1101.) Imidosulphuryl amide, S 2 O 4 N 3 H5 = S0 2 < S0 2 < NH 2 NH NH 2 . Sol. in NH 4 OH-f-Aq. Decomp. by cone. HC1. Insol. in alcohol sat. with NH 3 . (Mente, A. 248. 265.) Indie acid. Magnesium indate, MgIn 2 O 4 +3H 2 O. Ppt. Insol. in H 2 O. Sol. in HCl+Aq. (Renz, B. 1901, 34. 2764.) Indium, In. Does not decomp. hot H 2 O. Sol. in dil. HC1, and H 2 SO 4 +Aq. Decomp. by cone. H 2 SO 4 . Easily sol. in HNO 3 +Aq. Insol. in acetic acid. Insol. in KOH-j-Aq. (Winkler, J. pr. 102. 273.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Yz com. oleic acid dissolves 0.0039 g. In in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Indium monobromide, InBr. Decomp. by hot H 2 O. Easily sol. in acids. Easily sol. in cold cone. HC1. (Thiel, Z. anorg. 1904, 40. 328.) Indium ^bromide, InBr 2 . Decomp. by hot H 2 O. Easily sol. in acids. (Thiel, Z. anorg. 1904, 40. 329.) Indium fhbromide, InBr 3 . Deliquescent. Very sol. in H 2 O. Indium monochlciide, InCl. Deliquescent. Decomp. by H 2 O into InCl 3 . and In. (Nilson and Pettersson, Chem. Soc. 43. 820.) Indium ^chloride, InCl 2 . Deliquescent in moist air; decomp. by F 2 O into InCl 3 and In. (Nilson and Pettersson, Chem. Soc. 43. 818.) Indium frzchloride, InCl 3 . Very deliquescent; sol. in H 2 O with hissing and great evolution of heat. Indium lithium chloride. Extremely deliquescent. Sol. in H 2 O. (Meyer, A. 150. 144.) Indium potassium chloride, 3KC1, InCl 3 + 1^H 2 0. Easily sol. in H 2 O. (Meyer.) Indium Znfluoride, InF 3 +3H 2 O. Sol. in H 2 O; readily decomp. (Thiel, B. 1904, 37. 175.) 1 1. H 2 O dissolves 86.4 g. at 25. Decomp. on boiling. (Thiel, Z. anorg. 1904, 40. 331.) +9H 2 O. SI. sol. in cold H 2 O. Sol. in HC1 and in HNO 3 . Insol. in alcohol and ether. (Chabrie, C. R. 1905, 140. 90.) Indium hydrosulphide. Decomp. by acids. (Meyer.) Indium hydroxide, In 2 O 6 H e . Sol. in acids; also in KOH, or NaOH+Aq but the solution clouds up on standing or boiling, with separation of In 2 O 6 H 6 . Insol. in NH 4 OH, or NH 4 Cl+Aq. SI. sol. in NH 4 OH+Aq. (Renz, B. 1904, 37. 2110.) SI. sol. in alkylamines but completely ppt. by addition of the hydrochloride of the base. (Renz, B. 1903, 36. 2754.) Indium rrconoiodide, Inl. Slowly decomp. in moist air. Not attacked by boiling H 2 O. Sol. in dil. HNO 3 in presence of AgNO 3 . Very slowly sol. in cold, more rapidly sol. in IODAURICYANIDE, BARIUM 399 hot acids with evolution of H 2 . Very sol. in sulphurous acid. Insol. in alcohol, ether and chloroform. (Thiel, Z. anorg. 1910, 66. 302.) Indium ohiodide, InI 2 . (Thiel, Z. anorg. 1910, 66. 302.) Indium tfniodide, InI 3 . Deliquescent. (Meyer.) Sol.inCHCls. Decomp. byxylene. (Thiel, Z. anorg. 1904, 40. 330.) Indium nitride, InN. Decomp. by heat. (Franz Fischer,' B. 1910, 43. 1469.) Indium monoxide, InO. Gradually sol. in HCl+Aq. (Winkler, J. pr. 94. 1.) Indium sesquioxide, Slowly sol. in cold, easily in hot acids. Four modifications: (1) Yellow. Amorphous. Sol. in acids. Its hydroxide is insol. in ammonia and NH 4 C1. (2) White. Amorphous. Insol. in acids. (3) White. Amorphous. Sol. in acids. Its hydroxide is sol. in ammonia, but pptd. by NH 4 C1. (4) Crystallized. Crystalline modification is insol. in acids. (Renz, B. 1904, 37. 2112.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Indium oxide, In 7 O 9 = 3InO, 2In 2 3 (?). (Winkler.) In 4 O 5 = 2InO, In 2 O 3 (?). (Winkler.) Indium oxy bromide (?). Not decomp. by hot acids or alkalies. (Meyer, A. 150. 137.) Indium oxychloride, InOCl. Very si. sol. in H 2 O. (Thiel, B. 1904, 37. 176.) Very si. sol. in cold or hot dil. acids. Quickly sol. in hot cone, acids. (Thiel, Z. anorg. 1904, 40. 327.) Indium Znselenide, In 2 Se 3 . Sol. in strong acids with evolution of H 2 Se. (Thiel, Z. anorg. 1910, 66. 315.) Diindium sulphide, In 2 S. Sol. in acids. (Thiel, Z. anorg. 1904, 40. 326.) Indium monosulphide, InS. Easily sol. in HC1 with evolution of H 2 S. Sol. in HNO 3 with evolution of oxides of nitrogen. (Thiel, Z. anorg. 1910, 66. 314.) Indium sesgiasulphide, In 2 S 3 . Partially sol. in (NH 4 ) 2 S+Aq. Indium potassium sulphide, In 2 S 3 , K 2 S. Insol. in H 2 O; decomp. by weak acids with separation of In 2 S 3 ; sol. in cone, acids. (Schneider, J. pr. (2) 9. 209.) Indium silver sulphide, In 2 S 3 , Ag 2 S. Insol. in H 2 O. (Schneider, I. c.) Indium sodium sulphide, In 2 S 3 , Na 2 S-f-2H 2 0. Insol. in H 2 O. (Schneider, I. c.) Indium wonotelluride, InTe. Sol. in HNO 3 ; insol. in HCl+Aq. (Thiel, Z. anorg. 1910, 66. 318.) Infusible white precipitate. ZXiodamine, NHI 2 . Decomp. by H 2 O. lodammonium iodide, NIH 3 I. Decomp. by H 2 O, caustic alkalies, and acids. Sol. in KI+Aq, alcohol, ether. CS 2 , CHC1 3 . (Guthrie, Chem. Soc. (2) 1. 239.) lodauric acid, HAuI 4 (?). Not known with certainty. Ammonium iodaurate. Deliquescent. Decomp. by H 2 O. (John- ston, Phil. Mag. (3) 9. 266.) Barium iodaurate. Sol. in BaI 2 +Aq. Caesium iodaurate, CsAuI 4 . (Gupta, J.Am. Chem. Soc. 1914, 36. 748.) Ferrous iodaurate. Sol. inH 2 O. (Johnston.) Potassium iodaurate, KAuI 4 . Decomp. by H 2 O. Sol. in KI, and HI-fA. (Johnston.) Sodium iodaurate. Very deliquescent. (Johnston.) lodauricyanhydric acid, HAu(CN) 2 I 2 . Known only in its salts. Barium iodauricyanide, Ba[Au(CN) 2 I 2 ] 2 + 10H 2 O. SI. sol. in cold, easily in hot H 2 O. Easily sol. in alcohol. (Lindbom, Lund. Univ. Arsk. 12. No. 6.) 400 IODAURICYANIDE, CALCIUM Calcium iodauricyanide, Ca[Au(CN) 2 I 2 ] 2 + 10H 2 O. Not stable. (L.) Cobalt iodauricyanide, Co[Au(CN) 2 I 2 ] 2 + 10H 2 O. Most insol. of all iodauricyanid.es, and only si. sol. in warm H 2 O. Easily sol. in alcohol. Potassium iodauricyanide, KAu(CN) 2 I 2 + H 2 O. SI. sol. in cold, easily sol. in warm H 2 O and alcohol. (L.) Strontium iodauricyanide, Sr[Au(CN) 2 I 2 ] 2 + 10H 2 O. SI. sol. in cold, more easily in hot H 2 O. lodhydric Acid, HI. Very easily and quickly absorbed by H 2 O, with evolution of much heat. Solution is decomp. on exposure to the air. 1 vol. H 2 absorbs 450 vols. HI at 10. (Thomson.) I vol. H 2 O absorbs 425 vols. HI at 10. (Berthelot, C. R. 76. 679.) Weak or strong solutions when boiled in an atmosphere of H leave a residue of constant composition, which distils unchanged at 126 (de Luynes), at 127 (Roscoe, Chem. Soc. 13. 146; Naumann; Topsoe), at 128 (Bineau, A. ch. (3) 7. 266); and has a sp. gr. of 1.67 (Nau- mann), of 1.70 (Bineau, de Luynes), of 1.708 (Topsoe); and contains 56.26 % HI (Bineau), 57.0% HI (Roscoe), 57.75% HI (Topsoe.) By conducting dry H gas through the aqueous solution of HI, a constant residue is Solution in H 2 O sat. at has sp. gr. = 1 . 99 (de Luynes, A. ch. (4) 2. 385); 2.0 (Vigier). Sp.gr. of HI +Aq. Sp. gr. % HI Temp. 1.017 2.286 13.5 1.0524 7.019 13.5 1.077 10.15 13.5 1.095- 12.21 13 1.102 13.09 13.5 .126 15.73 13.5 .164 19.97 13.5 . .191 22.63 13.8 .225 25.86 13.8 .2535 28.41 13.5 1.274 30.20 13.5 1.309 33.07 13 1.347 36.07 13 1.382 38.68 13 1.413 40.45 13 1.451 43.39 13 1.4865 45.71 13 1.528 48.22 13 1.542 49.13 13.5 .5727- 50.75 13 .603 52.43 12.5 .630 53.93 14 .674 56.15 13.7 .696 57.28 13 .703 57.42 12.5 .706 57.64 13.7 .708 57.74 12 (Topsoe, B. 3. 403.) Sp. gr. of HI+Aqat 15. ODcamea, containing ou.o-uu./ ~/ JO.JL 11 temp, is 15-19, and 58.2-58.5% HI if temp, is %HI Sp. gr. %HI Sp. gr. %HI Sp. gr. 100. (Roscoe.) 1 1.008 21 1.175 41 1.414 Solubility of HI, in H 2 O at t. 2 3 1.015 1.022 22 23 1.185 1.195 42 43 1.429 1.444 t % HI Solid Phase 4 1.029 24. 1.205 44 1.459 5 1.037 25 1.216 45 .475 -10 20.3 Ice 6 1.045 26 1.227 46 .491 -20 29 3 7 1.053 27 1.238 47 .508 30 35 1 8 1.061 28 1.249 48 .525 -40 39 9 1.069 29 1.260 49 .543 50 42 10 1.077 30 1.271 50 .561 -60 44.4 11 1.085 31 1.283 51 .579 -70 46.2 12 1.093 32 1.295 52 .597 -80 -60 47.9 52.6 Ice+HI, 4H 2 O HI, 4H 2 O 13 14 1.102 1.110 33 34 1.307 1.320 53 54 .615 .634 -40 59 15 1.118 35 1.333 55 .654 35.5 64 16 1.127 36 1.346 56 .674 -40 65 5 17 1.137 a7 1.359 57 .694 -49 48 66.3 70.3 HI,4H 2 O+HI, 3H 2 O HI, 3H 2 O 18 19 1.146 1.155 38 39 1.372 1.386 58 .713 -56 73.5 HI,3H 2 O+HI,2H 2 O 20 1.165 40 1.400 -52 74 HI, 2H 2 O (Topsoe, calculated by Gerlach, Z. anal. 27. (Pickering, B. 1893, 26. 2307.) 316.) IODATE, AMMONIUM 401 Sp. gr. of HI+Aqatl5. Sp. gr. of HIO 3 -f Aq a t 15. %HI Sp. gr. %HI Sp. gr. %HI Sp. gr. %I^ Sp. gr. % I 2 5 Sp. gr. 5 1.045 25 1.239 45 1.533 1 1.0053 35 .4428 10 15 1.091 1.138 30 35 1.296 1.361 50 52 1.650 1.700 5 10 1.0263 1.0525 40 45 .5371 .6315 20 1.187 40 1.438 15 20 1.1223 1.2093 50 55 .7356 .8689 25 1.2773 60 .9954 Only a " moderate degree of accuracy " is 30 1.3484 6$ 2.1269 claimed for this table. 253.) Mpt. 43 +2H 2 O. 26. 2308.) +3H 2 O. +4H 2 O. (Pickering, B. 1893, Mpt. 48. (Pickering.) Mpt. 36.5. (Pickering.) lodic acid, HIO 3 . Very sol. in H 2 O and alcohol. 100 g. H 2 O dissolve 286.1 g. HIO 3 at 13.5. Sp. gr. of HIO 3 +Aq. =2.4256. 100 g. H 2 O dissolve 293 g. HIO 3 at 18. Sp. gr. of HIOa+Aq. =2.4711. (Groschuff, Z. anorg. 1905, 47. 337.) Solubility of HIO 3 in H 2 O at t. Solid phase t G. HI0 3 in 100 g. of the solution G. I 2 O 5 in 100 g. of the solution ice 0.30 1.78 1.69 u 0.67 4.35 4.13 tt 1.01 7.17 6.81 u 1.90 17.66 16.75 u 2.38 27.65 26.22 4.72 54.19 51.42 u 6.32 60.72 57.61 (( 12.25 71.04 67.40 (I 13.5 72.2 68.5 u 15 73.8 70.0 ' it 19 76.2 72.3 ice+HIO 3 14 72.8 69.1 HIO 3 74.1 70.3 11 + 16 75.6 71.7 <( 40 77.7 73.7 u 60 80.0 75.9 u 80 82.5 78.3 H 85 83.0 78.7 U 101 85.2 80.8 HI0 3 +HI 3 8 110 86.5 82.1 HI 3 8 125 87.2 82.7 u 140 88.3 83.8 u 160 90.5 85.9 (Groschuff, Z. anorg. 1905, 47. 343.) Sat. solution has sp. gr. 2.842 at 12.5, and boils at 104. (Ditte, B. 6. 1533.) Sat. solu- tion has sp. gr. 2.1629 (1.874 pts. I 2 O 5 in 1 pt. H 2 O) at 13, and boils at 100. (Kammerer, Pogg. 138. 400.) (Kammerer.) According to Thomsen (B. 7. 71) solutions of HIO 3 have sp. gr. HIO 3 + 10H 2 O = 1.6609. HIO 3 + 20H 2 O = 1.3660. HIO 3 + 40H 2 O = 1.1945. HIO 3 + 80H 2 O = 1.1004. HIO 3 + 160H 2 O = 1.0512. HIO 3 +320H 2 O = 1.0258. H 2 SO 4 at nearly boiling temp, dissolves Vi its weight of iodic acid. (Millon.) Solubility in HNO 3 containing 27.73% HNO 3 . 100 g. of the sat. solution contain at: 20 40 60 18 21 27 38 g. HIO 3 . Solubility in HNO 3 containing 40.88% HNO 3 . 100 g. of the sat. solution contain at: 20 40 60 9 10 14 18 g. HIO 3 . (Groschuff, Z. anorg. 1905, 47. 344.) Less sol. in HNO 3 than H 2 O; nearly insol. in anhydrous HNO 3 . (Groschuff, Z. anorg. 1905, 47. 347.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Unattacked and undissolved by liquid NOj. (Frankland, Chem. Soc. 1901, 79. 1362.) Insol. in absolute alcohol. Alcohol of 35 B. dissolves half its weight in HIO 3 . (Kam- merer.) (Grosschuff, Z. anorg. 1905, HIO 3 , I 2 O 6 . 47. 343.) lodates. The alkali iodates are sol. in H 2 O, the others are si. sol. or insol. therein. Aluminum iodate, A1(IO 3 ) 3 (?). Deliquescent. (Berzelius.) Ammonium iodate, NH 4 IO 3 . SI. sol. in H 2 O. Sol. in 38.5 pts. H 2 O at 15, 6.9 pts .at 100. (Rammelsberg, Pogg. 44. 555.) 402 IODATE, AMMONIUM Solubility of NH 4 IO 3 in HIO 8 +Aq at 30. % HI0 3 % NHJOa in the in the Solid phase solution solution 4.20 NH 4 IO 3 2.54 3.89 * 4.52 3.83 . NH 4 IO 3 +NH 4 IO 3 , 2HIO 3 4.51 3.86 4.56 3.75 4.73 3.53- NHJO 2H10 3 6.57 1.94 8.45 1.09 9.12 0.89 24.00 0.62 36.01 0.41 44.43 0.39 58.12 0.37 76.35 0.31 NHJ0 3 , 2HI0 3 +HI0 3 76.70 HI0 3 (Meerburg, Z. anorg. 1905, 45. 341.) , +H 2 O. (Ditte, A. ch. (6) 21. 146.) Ammonium cfoiodate, NH 4 H(IO 3 ) 2 . SI. sol. in cold H 2 O. (Ditte, A. ch. (6) 21. 145.) Ammonium /niodate, NH 4 H 2 (IO 3 ) 3 . Sol. in H 2 O. (Blomstrand, J. pr. (2) 42. 335.) See also solubility in H1O 3 , under Am- monium iodate. (Meerburg.) Ammonium cobalt iodate. Decomp. by H 2 O. Insol. in alcohol. (Rammelsberg.) Ammonium manganic iodate, Mn(IO 3 ) 4 , 2NH 4 I0 3 . Ppt. Insol. in H 2 O. Insol. in HIO 3 . (Berg, "C. R. 1899, 128. 675.) Ammonium oxydimercuriammonium iodate. See Oxyd^mercuriammonium ammonium iodate. Ammonium tellurium iodate. See lodotellurate, ammonium. Ammonium iodate selenate. See lodoselenate, ammonium. Barium iodate, Ba(IO 3 ) 2 . Anhydrous salt is sol. in 1746 pts. H 2 O at 15, and 600 pts. H 2 O at 100 (Rammelsberg, Pogg. 44. 577); in 3018 pts. H 2 O at 13.5, and 681 pts. H 2 O at 100. (Kremers, Pogg. 84. 27.) Solubility of Ba(IO,) 2 in H 2 p, 100 g. sat. Ba(IO 3 ) 2 +Aq at t contain g. anhydrous Ba(I0 3 ) 2 . 03 ^. to f ' 03 " t is t 1 t 2 O 08 O c3 O c3 w n Eutectic point 0.046 0.002 0.008 30 0.031 70 0.093 + 10 0.014 40 0.041 80 0.115 20 0.022 50 0.056 90 0.141 25 0.028 60 0.074 *99 . 2 0.197 *Bpt. at 735 mm. pressure = about 100 at 760 mm. pressure. (Anschiitz, Z. phys. Ch. 1906, 56. 241.) 1 1. sat. aq. solution contains 0.284 g. Ba(IO 3 ) 2 at room temp. (Hill and Zink, J. Am. Chem. Soc. 1909, 31. 44.) 1 1. H 2 O dissolves 0.3845 g. Ba(IO 3 ) 2 at 25. (Harkins and Winninghof, J. Am. Chem. Soc. 1911, 33. 1828.) Easily sol. in cold HCl+Aq; difficultly sol. in warm HNO 3 +Aq. (Rammelsberg.) Insol. in H 2 SO 4 . (Ditte.) 100 cc. NH 4 OH+Aq (sp. gr.=0.90) dis- solve 0.0199 g. Ba(IO 3 ) 2 . (Hill and Zink.) Solubility in salts +Aq at 25. C = concentration of salt in salt solution expressed in equivalents per 1. S=solubility of Ba(IO 3 ) 2 in salts+Aq ex- pressed in equivalents per 1. Salt c s Ba(N0 3 ) 2 0.001 0.002 0.005 . 0.020 0.050 0.100 0.200 0.001362 0.001212 0.0009753 0.0006744 0.0006131 0.0005659 0.0005580 KNO 3 0.002 0.010 0.050 0.200 0.001624 0.001820 0.002640 0.003190 KIO 3 0.00010608 0.0005304 0.0010608 0.001510 0.001242 0.0009418 (Harkins and Winninghof, J. Am. Chem. Soc. 1911, 33. 1829.) Insol. in alcohol. 100 cc. 95% alcohol dissolve 0.0011 g. Ba(IO 3 ) 2 at room temp. (Hill and Zink.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014.) +H 2 O. Sol. in 3333 pts. H 2 O at 18, and 625 pts. H 2 O at 100. (Gay-Lussac, A. ch. 91. 5.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) IODATE, COBALTOUS 403 Barium manganic iodate, Mn(IO 3 ) 4 , Ba(IO 3 ) 2 . Insol. in H 2 O. Insol. in HIO 3 . (Berg, C. R. 1899, 675.) 128. Bismuth iodate, basic. Insol. in H 2 O. Very difficultly sol. in HNO 3 +Aq. (Rammelsberg, Pogg. 44. 568.) ; Bi(IO 3 ) 3 +l^H 2 O. Insol. in H 2 O. Cadmium iodate, Cd(IO 3 ) 2 . Very si. sol. in H 2 O. Easily sol. in HNO 3 , or NH 4 OH+Aq. Sol. in Cd(C 2 H 3 O 2 ) 2 + Aq. (Rammelsberg, Pogg. 44. 566.) +H 2 O. SI. sol. in H 2 O. Very sol. in dil. HNOg+Aq. (Ditte, A. ch.- (6) 21. 145.) Cadmium iodate ammonia, Cd(IO 3 ) 2 , 2NH 3 . Insol.inH 2 O;sol.inNH 4 OH+Aq. (Ditte.) A. ch. (6) 21. 145.) Cd(IO 3 ) 2 ,2NH 3 +H2O. As above. (Ditte. Caesium iodate, CsIO 3 . 100 pts. H 2 O dissolve 2.6 pts. CsIO 3 at 24. Insol. in alcohol. (Wheeler, Sill. Am. J. 144. 123.) 2CsIO 3 , 1 2 O 5 . 100 pts. H 2 O dissolve 2.5 pts. at 21. Not decomp. by hot H 2 O. (Wheeler.) 2CsIO 3 , I 2 O 5 , 2HIO 3 . SI. sol. in cold H 2 0. and decomp. thereby into 2CsIO 3 , I 2 Os. (Wheeler.) Caesium iodate chloride, CsCl, HIO 3 . Decomp. by H 2 O into 2CsIO 3 , I 2 O 5 . (Wheeler.) Caesium hydrogen iodate periodate, HCsIO 3 , IO 4 +2H 2 O. , Ppt. Sol. in dil. HNO 3 . (Wells, Am. Ch. J. 1901, 26. 280.) Calcium iodate, Ca(IO 3 ) 2 . 100 pts. dissolve 0.22 pt. at 18, and 0.986 pt. at 100. (Gay-Lussac.) Sol, in cone. HCl+Aq. (Filhol.) Much more sol. in HNO 3 +Aq than in H 2 O. (Rammelsberg.) Insol. in H 2 SO 4 . (Ditte.) Scarcely sol. in sat. KIO 3 +Aq. (Sonstadt, C. N. 29. 209.) +H 2 O. Sat. solution contains at: 21 0.37 35 0.48 40 0.52 45 0.54%Ca(I0 3 ) 2 , 50 0.59 60 0.65 80 0.79 100 0.94%Ca(I0 3 ) 2 . (Mylius and Funk, B. 1897, 30. 1724.) -f6H 2 O. Efflorescent. Sol. in 253 pts. H 2 O at 15, and 75 pts. at 100. (Rammelsberg.) Sat. solution contains at: 10 18 30 0.1 0.17 0.25 0.42% Ca(IO 3 ) 2 , 40 50 54 60 0.61 0.89 0.14 1.36%Ca(IO 3 ) 2 . (Mylius and Funk, B. 1897, 30. 1724.) Much more sol. in HNO 3 +Aq. Pptd. by alcohol from Ca(IO 3 ) 2 +Aq. Insol. in H 2 SO 4 . (Ditte.) Pptd. by alcohol from aqueous solution. (Henry.) Cerous iodate, Ce(IO 3 ) 3 +2H 2 O. SI. sol. in cold, easily sol. in hot H 2 O and in acids. (Holzmann, J. pr. 76. 321.) Solubility in H 2 O. 100 cc. of the sat. solution contain 0.1456 g. at 25. (Rimbach, Z. phys. Ch. 1909, 67. 199;) Calc. from electrical conductivity of Ce(IO 3 ) 3 +Aq., 100 cc. of the sat. solution contain 0.1636 g. Ce(I0 3 ) 3 at 25. (Rim- bach, Z. phys. Ch. 1909, 67. 199.) Ceric iodate, Ce(IO 3 ) 4 . Slightly hydrolyzed by H 2 O. 0.34 g. is sol. in' 100 cc. hot cone. HNO 3 . (Barbieri, Chem. Soc. 1907, 92. (2) 467.) Cobaltous iodate, Co(IO 3 ) 2 . Anhydrous. Sol. in warm dil. H 3 PO 4 , or H 2 SO 4 +Aq. (Ditte, A. ch, (6) 21. 14.) Solubility in H 2 O Form Temp. CO(I03)2 Mots, of water free salt to 100 mols H 2 O Co(I0 3 ) 2 +4H 2 0.54 0.028 tt 18 0.83 0.038 d' 30 1.03 0.046 K 50 1.46 0.065 it 60 1.86 0.084 t( 65 2.17 0.098 C.o(I0 3 ) 2 +2H 2 0, 0.32. 0.014 ct 18 0.45 0.020 (i 30 0.52 0.023 i ' f .- << 50 0.67 0.030 11 KHIO 3 , KHSO 4 . More sol. in H 2 O than .00 7.09 .32 1.0 ' u KHIO 3 . (Serullas.) 8.04 3.47 0.85 3.57 KIO 3 HIO 3 +KIO 3 , 2HIO 3 KIO 3 , 2HIO 3 (labile) Potassium iodate tungstate. 4.80 2.90 u See Tungstoiodate, potassium. 6.45 1.35 " 9.35 0.64 KI0 3 , 2HIO 3 Rubidium iodate, RbIO 3 . 12.04 17.50 31.20. 0.44 0.30 0.52 a n 100 pts. HsO dissolve 2.1 pts. RbIO 3 at 23. Easily sol. in cold HCl+Aq. (Wheeler Sill. Am. J. 144. 123.) 53.64 0.68 11 62.52 76.40 0.72 0.80 KI0 3 , 2HIO 3 +HI0 3 Rubidium hydrogen iodate, RbH(IO 3 ) 2 . 76.70 HIO 3 SI. sol. in cold, more readily in hot H 2 O, RbIO 3 separating on coolins Insol in alco- (Meerburg, Z. anorg. 1905, 46. 330.) hoi. (Wheeler.) - '. RbH 2 (IO 3 ) 3 . As above. (Wheeler.) Rubidium iodate chloride, RbIO 3 , HC1, or HI0 3 , RbCl. Decomp. by cold H 2 O. (Wheeler.) 3RbCl, 2HIO 3 . Sol. in H 2 O, from which RbIO 3 separates. (Wheeler.) Rubidium iodate selenate. See lodoselenate, rubidium. Samarium iodate, Sm(IO 3 ) 3 -f;6H 2 O. Precipitate. (Cleve.) IODATE IODIDE, SODIUM 407 Scandium iodate, Sc(IO 3 ) 3 + 10, 13, 15, and 18H 2 0. Nearly insol. in H 2 O. (Crookes, Phil. Trans. 1910, 210. A, 361.) (Hill and Simmons, Z. phys. Ch. 1909, 67. 602.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Insol. in methyl acetate. (Bezold, Dis- sert. 1906; Naumann, B. 1909, 42. 3790); ethyl acetate. (Hamers, Dissert. 1906; Naumann, B. 1910, 43. 314.) Silver iodate ammonia, 2AgIO 3 , 3NH 3 + Very sol. in cold H 2 O. (Ditte, A. ch. (6) 21. 145.) AgIO 3 , 2NH 3 . SI. sol. in cone. NH 4 OH+Aq. (Rosen- heim, A. 1899, 308. 52.) Sodium iodate, NaIO 3 . ICO pts. H 2 O dissolve 7.25 pts. NaIO 3 at 14.5. (Gay-Lussac.) 100 pts. H 2 O dissolve 2.52 pts. at 0; 9.07 pts. at 20; 14.39 pts. at 60; 27.7 pts. at 80; 33.9 pts. at 100. (Krem- ers, Pogg. 97. 5.) Sat. solution boils at 102 (Kremers), 105 (Ditte). Sol. in warm H 2 SO 4 +Aq diluted with Y* vol. H 2 O. Crystallizes out on standing over H 2 S0 4 . (Ditte.) Silver iodate, AgIO 3 . 189XlO~ 4 moles or 5.36X10~ 2 g. AgIO 3 Solubility of NaIO 3 in HIO 3 +Aq at 30. are sol. in 1 liter H 2 O at 25. (Noyes and % HI0 3 % NalOs Kohr, Z. phys. Ch. 1903, 42. 338.) SI. sol. in H 2 O. 4.35X10- 2 g. are dissolved in the solution in the solution Solid phase in 1 liter of sat. solution at 20. (Bbttger, Z. o 9 . 36 NaIO 3 +l/^H 2 O phys. Ch. 1903, 46. 603.) 1.98 9.52 1 1. H 2 O dissolves 40 mg. AgIO 3 at 18. 4! 86 10.22 t (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 5^86 11.04 i 1 1. H 2 O dissolves 0.0275 g. AgIO 3 at 9.43; 7.40 11.60 ' ll U'l 0.039 g. at 184; 0.0539 g. at 26.6. Solu- 9*73 14.73 [labile bility increases rapidly with temp. (Kohl- 6^76 11.18 NaIO 3 +l^H 2 O + rausch, Z. phvs. Ch. 1908, 64. 168.) 1 1. H 2 O dissolves 0.039 g. AgIO 3 at 20. 6.66 11.28 Na 2 O, 2I 2 6 (Whitby, Z. anorg. 1910, 67. 108.) Not completely insol. in H 2 O. (Rose.) Sol. 7^80 9.15 10^30 9.00 Na 2 O, 2I 2 O 6 u in NH 4 OH+Aq; sol. in HNO 3 +Aq. (Na- 9.93 8.71 n quet, J. B. 1860. 201.) Sol. in cone. KI+Aq. 11 20 7 54 a (Ladenburg, A. 135. 1.) Sol. in 27,700 pts. H 2 O at 25; in 42.4 pts. 11.89 11.75 7.21 7.18 Na 2 0, 2I 2 O 5 -f NaIO 3 , 2HIO 8 5% NH 4 OH+Aq at 25; in 2.1 pts. 10% 14.62 5.65 NalO 2HlOs NH 4 OH+Aq at 25; in 1044.3 pts. 35% 23.23 3.69 a HNO 3 +Aq (sp. gr. 1.21) at 25. (Longi, 32.68 2.91 (i Gazz. ch. it. 13. 87.) 40. 9l 2.64 tt 46 62 2 67 (i Solubility in HNO 3 +Aq at 25. 55.48 2.12 tt Normality HNOs G. AglOs dissolved per 1. 65.47 76.19 1.83 1.42 NaIO 3 , 2HIO 3 +HIO 3 0.000 0.0503 76.70 HI0 3 0,125 0.250 0.0864 0.1075 (Meerburg, Z. anorg. 1905, 45. 334.) 0.500 1.00 0.1414 0.2067 Insol. in alcohol. Sol. in dil. HC 2 H 8 O 2 + 2.00 400 0.3319 q- Insol. in methyl acetate. (Naumann, B. . uu IK O^ K 1909,42.3790.) 8.00 .5875 +13^H 2 O. See Meerburg above. Sodium duodate, Na 2 O, 2I 2 O 6 . See Meerburg under NaIO 3 . Sodium Zniodate, NaIO 3 , Very sol. in H 2 O. (Blomstrand, J. pr. (2) 42. 337.) See also Meerburg under NaIO 3 . Sodium iodate bromide, NaIO 3 , 2NaBr+ 9H 2 0. Sol. in H 2 O. (Rammelsberg.) Sodium iodate chloride, NaIO 8 , NaCl+4H 2 O, and 2NaIO 3 , 3NaCl+18H 2 O. Cold H 2 O dissolves out NaCl. . Sodium iodate iodide, NaIO 3 , Nal. Hot H 2 O or alcohol dissolves out Nal. +8H 2 O. + 10H 2 O. 2NaIO 3 , 3NaI+20H 2 O. (Penny, A. 37. 202.) 408 IODATE, STRONTIUM Stable in a solution of Nal+NaOH+Aq. (Eakle, C. C. 1896, II. 650.) Strontium iodate, Sr(IO 3 ) 2 . Anhydrous. Insol. in H 2 SO 4 (Ditte); easily sol. in cold HCl+Aq. (Rammelsberg. Pogg. 44. 575.) +H 2 O. Difficultly sol. in H 2 O. +6H 2 O. Sol. in 416 pts. H 2 O at 15, and 138 pts. at 100 (Gay-Lussac); 342 pts. at 15, and 110 pts. at 100. Difficultly sol. in warm HNO 3 +Aq. (Rammelsberg, Pogg. 44. 575.) Thallous iodate, T1IO 3 . Difficultly sol. in warm H 2 O. (Oettinger.) Insol. in H 2 O; difficultly sol. in HNO 3 +Aq. (Rammelsberg.) SI. sol. in H 2 O. 0.58 X10- 1 g. are dissolved in 1 liter of sat. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) 2.12X10- 3 mols. =0.667 g. are sol. in 1 1. H 2 O at 25. (Spencer, Z. phys. Ch. 1912, 80. 707.) Sol. in a little NH 4 OH+Aq, also in boiling HNO 3 , H 2 SO 4 , or. HC1 + Aq. Insol. in alcohol. (Oettinger.) + i^H 2 O. Very si. sol. in H 2 O or dil. boil- ing acids. (Ditte, A. ch. (6) 21. 145.) Thallic iodate, basic, T1(OH)(IO 3 ) 2 +H 2 O = T1 2 O 3 , 2I 2 O 6 +3H 2 O. Insol. in H 2 O; sol. in cold HCl+Aq, and warm dil. H 2 SO 4 +Aq. (Ditte, A. ch. (6) 21. 145.) Thallic iodate, T1(IO,),+1^ H 2 O. Insol. in H 2 O; si. sol. in HNO 3 +Aq. Decomp. by alkalies. (Rammelsberg.) +12H 2 O. Difficultly sol. in H 2 O. Easily sol. in dil. acids. (Gewecke, Z. anorg. 1912, 76, 275.) Thorium iodate, Th(IO 3 ) 4 . Precipitate. (Cleve.) Tin (stannous) iodate. Ppt. Sol. in SnCl 2 +Aq; insol. in NaIO 3 + Aq. Tin (stannic) iodate. Ppt. Uranous iodate. Precipitate. Very unstable. (Rammels- berg.) Uranyl iodate, UO 2 (IO 3 ) 2 . Sol. or insol. in HNO 3 and H 3 PO 4 +Aq, according to method of preparation. (Ditte.) +H 2 O. Sl.sol.inHNO 3 +Aq. (Rammels- berg.) Ytterbium iodate, Yb(IO 3 ) 3 +6H 2 O. Ppt. (Cleve, Z. anorg. 1902, 32. 136.) Yttrium iodate, Y(IO 3 ) 3 +3H 2 O. Sol. in 190 pts. H 2 O. (Berlin.) Zinc iodate, Zn(IO 3 ) 2 . Anhydrous. (Ditte, A. ch. (6) 21. 145.) +2H 2 O. Sol. in 114 pts. cold, and 76 pts. hot H 2 O. (Rammelsberg, Pogg. 43. 665.) Sol. in HNO 3 , and NH 4 OH+Aq. Exists also in a very sol. modification. (Mylius and Funk, B. 1897, 30. 1723.) Zinc iodate ammonia, 3ZndO 3 ) 2 , 8NH 3 . Decomp. by H 2 O; sol. in NH 4 OH+Aq, from which it is pptd. by alcohol. (Rammels- berg, Pogg. 44. 563.) Zn(IO 3 ) 2 , 2NH 3 . Insol. in H 2 O. (Ditte, A. ch. (6) 21. 145.) Zn(IO 3 ) 2 , 3NH 3 +H 2 O. Insol. in H 2 O. (Ditte.) Zn(IO 3 ) 2 , 4NH 3 . (Ditte, A. ch. 1890, (6) 21. 1Q4.) (Ephraim, B. 1915, 48. 53.) Periodic acid. See Periodic acid. Iodides. The iodides are in general easily sol. in H 2 O; exceptions are HgI 2 , PbI 2 , Agl, Cu 2 I 2 , and BiI 3 , also the iodides of the Pt metals, all of which are insol. SnI 4 , SbI 3 , and T1I 3 are decomp. by H 2 O. Many iodides are more sol. in solutions of salts than in H 2 O, and several are sol. in alcohol or ether. See under each element. Iodine, I 2 . Sol. in 5524 pts. H 2 O at 0-12. (Wittstein, J. B. 1857. 123.) Sol. in 7000 pts. H 2 O. (Gay-Lussac.) Sol. in 3800 pts. H 2 O at 15. (Basse.) Sol. in 500 pts. H 2 O. (Jacquelain.) Sol. in 7196.4 pts. B 2 O at 18.75. (Abl.) Pure H 2 O dissolves 0.01519173 g. I per litre, or I is sol. in 6582 pts. H 2 O at 6.3. (Dossius and Weith, Zeit. Ch. 12. 378.) Sol. in about 4500 pts. H 2 O. (Hager, Comm. 1883.) Sol. in 7000 pts. H 2 O. (Cap and Garot, J. Pharm. (3) 26. 80.) 1 1. H 2 O at 25 dissolves 0.3387 g. I 2 . (Jakowkin, Z. phys. Ch. 1895, 18. 590.) 1 1. H 2 O dissolves 1.342 millimols of iodine at 25. (Noyes, Z. phys. Ch. 1898, 27. 359.) When iodine is shaken with H 2 O at 15, 1 pt. dissolves in 3750 pts. H 2 O; when iodine and H 2 O are heated together and then cooled to 15, 1 pt. iodine dissolves in 3500 pts. H 2 O. At 30*, 1 pt. is sol. in 2200 pts. H 2 O. (Dietz, Chem. Soc. 1899, 76, (2) 150.) 1 1. H 2 O dissolves 0.279 grams I 2 at 25. (McLauchlan, Z. phys. Ch. 1903, 44. 617.) IODINE 409 Solubility of I 2 in H 2 O at t. Solubility hi HgCl 2 +Aq at 25. t g. I 2 per 1. H 2 10 ccm. of the solution contain: 18 0.2765 25 0.3395 35. 0.4661 45 0.6474 55 0.9222 millimols 1 2 millimols Hg 0.0134 0.1294 0.9444 0.1460 1.2442 0.1806 1.9542 0.2543 3.3460 (Hartley, Chem. Soc. 1908, 93. 744.) Solubility of I 2 in H 2 O at t. (Herz and Paul, Z. anorg. 1914, 85. 214.) Sol. in solutions of soluble iodides. 100 pts. KI+200 pts. H 2 O dissolve 153 pts. I; from this solution H 2 O precipitates % the dissolved I. 100 pts. KI+400 pts. H 2 O dissolve quickly 76.5 pts. I. If more water is present, the solution takes place more slowly. (Baup.) CS 2 extracts the I from the above solutions. Solubility of I in KI+Aq at 7-7.3. t g. per 1. milliat. per 1. 0.1649 1.30 20 0.2941 2.30 40 0.5684 4.56 (Fedotieff, Z. anorg. 1910, 69. 30.) 1.32 millimol I 2 are sol. in 1 1. H 2 O. (Bray' J. Am. Chem. Soc., 1910, 32. 938.) Calculated from electrical conductivity of sat. I 2 +Aq. 1 1. H 2 O dissolves 0.0006383 mols. I 2 at 0. (Jones, J. Am. Chem. Soc. 1915, 37. 256.) Cone. H 2 S0 4 , HC1, HNO 3 , H 3 PO 4 , HC 2 H 3 O 2 , tartaric, or citric acids +Aq dis- solve I, but give it up to CS 2 on shaking therewith. (Tessier, Z. anal. 11. 313.) Sol. in 150 pts. H 2 SO 4 on warming, but crystallizes out in part on cooling. (Kraus.) Much more sol. in HBr+Aq than in pure H 2 O; HBr+Aq of sp. gr. 1.486 dissolves 3-4%. (Bineau.) SI. sol. in HCl+Aq. Easily sol. in even dil. HI+Aq. 1 1. 0.001 N-HCl+Aq sat. with I 2 contains 0.338 g. I 2 . (Bray and Mackay, J. Am. Chem. Soc. 1910, 32. 1919.) % KI in KI +Aq Pts I dissolved Sp. gr. of solution 1.802 3.159 4.628 5.935 7.201 8.663 10.036 11.034 11.893 12.643 1.173 2.303 3.643 4.778 6.037 7.368 8.877 9.949 11.182 12.060 1.0234 1.0433 1.0668 1.0881 1.1112 1.1382 1.1637 1.1893 1.2110 1.2293 1 1. 0.1 N HNO 3 +Aq sat. with I 2 contains 0.340 g. I 2 . (Sammet, Z. phys. Ch. 1905, 53. 644.) 1 1. 0.1 N-H 2 SO 4 +Aq sat. with I 2 contains 0.341 g. I 2 . (Sammet.) Sol. in H 2 SO 3 +Aq with decomp. 1 1. 0.9 N. H 3 BO 3 dissolves 0.300 g. I 2 at 25. (McLauchlan, Z. phys. Ch. 1903, 44. 617.) 100 cc. of a 10% solution of BaBr 2 dis- solve 0.231 g. I 2 at 13.5. (Meyer, Z. anorg. 1902, 30. 114.) 100 cc. of a 10% solution of BaCl 2 dissolve 0.067g. I 2 at 18.5. (Meyer.) 100 cc. of a 10% solution of BaI 2 dissolve 6.541 g. I 2 at 13.5. (Meyer.) 100 cc. of a 10% solution of CaBr 2 dis- solve 0.274 g. I 2 at 13.5. (Meyer.) 100 cc. of a 10% solution of CaCl 2 dissolve 0.078 g. I 2 at 18.5 (Meyer.) 100 cc. of a 10% solution of CaI 2 dissolve 8.062 g. I 2 at 13.5. (Meyer.) Easily sol. in boiling dil. HgCl 2 +Aq. (Selmi.) (Dossius and Weith, Zeit. Ch. (2) 6. 379.) Solubility of I 2 in KI+Aq at room tempera- ture, 14.5-15.1. % KI %I I/KI 1.80 3.16 4.63 5.93 7.20 8.66 10.04 11.03 11.89 12.64 1.17 2.30 3.64 4.78 6.04 7.37 8.88 9.95 11.18 12.06 0.651 0.729 0.786 0.805 0.839 0.851 0.884 0.902 0.940 0.954 (Weith and Dossius, Z. phys. Ch. 1898, 26. 150.) 410 IODINE S.olubility of I 2 in KI+Aq at 15 Solubility in KI+Aq at 25. % KI ccm. 1/10-n. iodine in 5cmm. of the solution I/KI Sp. gr. Analysis of liquid phase Analysis of solid phase together with adhering mother liquor 10 8 6 4 2 1 35.0 27.1 19.7 12.7 6.25 3.04* 35.0 . 33.9 32.8 31.8 31.2 30.4 % KI %i '% KI | % I (a) 1.733 1.888 2.066 2.216 2.539 2.560 2.665 3.232 3.246 (b) 1.349 1.516 1 . 769 1.910 2.403 2.904 3.082 (c) In\ 3.316 [n equilib 60.39 54.415 49.045 44.82 38.065 37.655 35.805 29.71 27.92 In equili 16.025 19.705 22.88 23,55 24.78 24.995 25.18 '-ariant po 26.05 25.96 26.04 25.92 rium with 0.0 11.63 23.085 31.01 44.56 45.55 49.61 62.81 66.45 Drium wit 18.49 26.16 36.06 40.515 53 . 605 63 . 125 66.04 int. Exc( 68.06 68.01 68.16 68.13 excess o 84.92 85.94 80.46 78.56 77.32 39.99 38.78 i excess 3.04 4.48 3.70 6.49 8.62 4.82 4.00 iss of KI 16.14 11.32 f KI. 0.0 4.05 6.32 10.84 15.23 16.73 56.10 56.27 of I. 85.43 83.87 89.33 83.62 83.81 92.41 94.39 and I. 83.77 86.56 * Obtained with 1/100-normal iodine. (Brunei, Z. phys. Ch. 1898, 26. 151.) Solubility of I 2 in KI+Aq at 25. Millimols KI per liter Millimols dissolved iodine per liter 106.3 53.15 26.57 13.29 6.643 3.322 1.661 0.8304 55.28 28.03 14.68 8.003 4.667 3.052 2.235 1.814 (Noyes and Seidenstricker, Z. phys. Ch. 1898, 27. 359.) Solubility in KI+Aq at 25, (Parsons and Whittemore, J. Am. Chem. 1911, 33. 1934.) Solubility in KI+Aq at 0. KI mol./l. I G. atoms/1. 1.91 2.85 4.51 5.36 5.55 3.29 5.45 11.52 17.12 17.16 (Abegg, Z. anorg. 1906, 50. 427.) Solubility of I 2 in KI+Aq at 25, Millimol KI per 1. Millimol 1 2 dissolved 100 51.35 50 25.77 20 11.13 10 6.185 5 3.728 2 2.266 1 1.788 (Bray and MacKay, J. Am. Chem. Soc. 1910, 32. 919.) KI+Aq KI+Aq. sat. with I 2 Wt. norm. Sp. gr. 0/4 G. I 2 in 1 g. of solution Sp. gr. 0/4 0.09871 (1.0123) 0.01199 (1.0219) 0.09861 1.01231 0.01199 1.02187 0.04969 (1.0061) 0.006094 (1.0109) 0.04966 1.00610 0.006083 1.01089 0.01992 1.00236 0.002535 1.00429 0.01983 (1.0024) 0.0025325 (1.0044) 0.00998 (1.0011) 0.0013532 (1.0020) 0.00992 (1.001.1) 0.0013585 (1.0020) 0.004999 (1.0005) 0.0007609 (1.0010) 0.004991 (1.0005) 0.0007577 (1.0011) 0.002000 (1.0001) 0.0004137 (1.0004) 0.002000 (1.0001) 0.0004015 (1.0004) 0.000999 (0.9999) 0.0002839 (1.0002) 0.000992 (1.0000) 0.00028125 (1.0002) Values in parentheses are found by inter- polation. (Jones and Hartman, J. Am. Ghem. Soc. 1915, 37. 247.) 1 mol. KI in alcohol dissolves 2 atoms I, and the solution does not give up I to CS 2 . (Jorgensen, J. pr. (2) 2. 347.) IODINE 411 Solubility in KI+60% alcohol at 25. Solubility in KI+40% alcohol at Continued. 25. Sp. gr. Analysis of liquid phase Analysis of solid phase together with adhering mother liquor Sp. gr. Analysis of liquid phase Analysis of solid phase together with adhering mother liquor % KI %i % I % KI % KI % I %KI %i (a) 1.148 1.191 1.285 1.368 1.427 1.533 1.776 2.250 2.507 2.845 (b 1.134 1.530 1.721 1.90 2.11 2.22 2.80 2.99 (c)Ii 3.162 In equilit 30.93 29.87 28.39 28.00 27.60 27.00 25.90 24.90 24.40 22.49 21.50 ) In equil 0.0 7.36 10.60 12.44 13.74 15.20 17.72 19.30 ivariant p 20.11 20.03 20.05 19.98 20.08 20.06 20.05 >rium wit 0.0 4.51 12.48 18.60 21.80 28.00 40.52 52.42 58.93 65.75 68.95 ibrium wi 23.04 43.05 49.38 55.33 59.26 62.66 69.10 71.90 oint. Ex 72.51 72.46 72.54 72.44 72.51 72.44 72.48 ti excess 89.13 86.60 87.30 85.75 84.39 81.05 76.21 73.20 71.66 70.04 th excess: 0.0 1.40 2.50 3.72 4.41 5.80 7.15 7.45 cess KI 2l! 84 7^40 20.61 33^46 KI. 0.0 0.71 2.27 3.21 4.25 6.05 10.30 16.73 21.04 24.15 26.42 a. i 88.76 88.21 87.10 86.60 85.20 85.49 88.96 and I. 74.64" KI+I 89!gi'l 74.09 KI+I 33.19KI (t 0.962 1.292 1.581 2'.000 2.173 1.749 2.902 (c)I 3.246 In equilibrium w 0.0 2.97 8.45 28.70 12.56 40.63 15.20 49.95 16.02 52.95 17.18 57.38 19.20 66.89 20.12 69.10 nvariant point. EJ 22.50 70.79 22.43 70.88 ith excess 0.0 1.85 3.41 4.98 5.60 6.61 8.45 7.08 ccess KI i 19.48 69.37 I. 84.51 84.02 83.81 82.96 83.60 85.16 88.81 mdl. 76.24 26.14 (Parsons and Corliss, J. Am. Chem. Soc. 1910. 32. 1372.) See also under KI. . - Sol. in KI +nitrobenzene. (Dawson, Chem. Soc. 1902, 81. 529.) .Solubility in KIO 3 +Aq is the same as in H 2 O. (Lami, C. A. 1909. 1622.) Solubility of I 2 in KBr+Aq at 25. G. KBr per 1. G. atoms Iz per 1. 60.6 106.9 175.9 229.8 281.9 330.6 377.1 411.0 461.7 509.8 548.0 567.9 sat. 0.0176 0.0278 0.0415 0.0532 0.0628 0.0717 0.0797 0.0864 0.0948 0.1006 0.1062 0.1094 (Parsons and Corliss, J. Am. Chem. Soc. 1910, 32. 1370.) Solubility in KI+40% alcohol at 25. Sp. gr. Analysis of liquid phase Analysis of solid phase together with adhering mother liquor. (Bell and Buckley, J. Am. Chem. Soc. 1912, 34. 13.) Solubility in NaBr+Aq at 25. % KI % I % KI %l. G. NaBr per 1. G. atoms It per 1. (a] 1.339 1.377 1.455 1.532 1.605 1.655 1.847 2.024 2.169 2.558 2.784 In equili 42.10 40.83 38.94 37.41 36.25 35.38 33.26 31.71 30.59 28.56 26.95 24.52 23.04 Drium wi 0.0 3.76 10.09 15.71 20.52 24.44 33.62 39.99 44.76 55.30 60.27 65.93 69.93 ,h excess 89.21 88.80 88.19 87.04 86.08 83.61 82 ..06 80.80 75.90 74.77 72.98 72.45 KI. 0.0 0.70 1.90 3.02 4.21 5.11 8.41 10.76 12.35 18.63 20.86 23.61 25.04 96.4 187.7 271.8 357.4 422.4 499.1 569.9 632.0 679.7 750.5 756.1 sat. 0.0266 0.0425 0.0538 0.0598 0.0638 0.0648 0.0644 0.0622 0.0595 0.0551 0.0550 (Bell and Buckley, J. Am. 34. 13.) Chem. Soc. 1912, 412 IODINE 100 cc. of a 10% solution of SrBr 2 dissolve 0.270 g. I 2 at 13.50. (Meyer, Z. anorg. 1902, 30. 114.) 100 cc. of a 10% solution of SrCl 2 dissolve 0.066g. I 2 at 18.5. (Meyer.) 100 cc. of a 10% solution of SrI 2 dissolve 6.616g. I 2 at 13.5. (Meyer.) Solubility in salts +Aq at 25. Salt +Aq Grams la sol. in 1 liter Salt +Aq Grams I 2 sol. in 1 liter i^-N.Na 2 SO 4 ^-N.K 2 S0 4 i^-N.(NH 4 ) 2 S0 4 N.NaNO 3 N.KNO 3 N.NH 4 NO 3 0.160 0.238 0.246 0.257 0.266 0.375 N.NaCl N.KC1 N.NH 4 C1 N.NaBr N.KBr N.NH 4 Br 0.575 0.658 0.735 3.29 3.801 4.003 (McLauchlan, Z. phys. Ch. 1903, 44. 617.) 1.14 g. are sol. in 100 ccm. liquid H 2 S. (An- tony, Gazz. ch. it. 1905, 35, (1) 206.) Sol. in liquid NH 3 . (Franklin, Am. ch. J. 1898, 20. 822.) SI. sol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Sol. in liquid SO 2 (Sestini), and SO 2 (Weber). 100 pts. AsCl 3 dissolve 8.42 pts. I at 0; 11.88 pts. I at 15; 36.89 pts. I at 96. (Sloan, C. N. 46. 194.) Sol. in liquid SO 2 , AsCl 3 , SO 2 C1 2 , and acetaldehyde. (Walden, Z. phys. Ch. 1903, 43. 407.) Very sol. in liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) Sol. in 10-12 pts. alcohol. (Wittstein.) Sol. in wood-spirit. (Playfair.) Abundantly sol. in amyl (Pelletan), and hexyl alcohol (Bouis). Iodine is sol. in 20 pts. alcohol, 110 pts. oil, 7000 pts. H 2 O, 100 pts. glycerine. (Cap and Garot, J. Pharm. (3) 26. 80.) Solubility of I 2 in C 2 H 5 OH+Aq at room temperature (14.5 15.1). Volumes of C 2 H 5 OH in 100 volumes of C 2 H 5 OH +H 2 Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 61.7 90 29.4 80 16.6 70 9.2 60 4.45 50 3.4 40 1.0 30 0.4 20 0.25 10 0.2 0.0 (Bruner, Z. phys. Ch. 1898, 26. 150.) Solubility of I 2 in C 3 H 7 OH+Aq at room temperature (14.5 15.1). Volumes of C 3 H 7 OH in 100 volumes of C 3 H ; OH , +H 2 Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 58.8 90 36.0 80 23.6 70 16.1 60 10.7 ,50 6.4 40 3.7 30 1.56 20 0.42 . 10 0.19 .... (Bruner, Z. phys. Ch. 1898, 26. 150.) Solubility in ethyl alcohol +Aq at 25. Molecules of C 2 H 5 OH in 100 molecules C 2 H 5 OH +H 2 O Molecule's of H 2 O in 100 molecules C 2 H 6 OH +H 2 O Normality of the iodine solution 0.0 100 0.0022 0.03 99. 7(?) 0.0024 0.06 99. 4(?) 0.0024 1.12 98.88 0.0023 1.83 98.27(?) 0.0025 9.40 90.60 0.0059 13.48 86.52 0.0111 23.80 76.20 0.0617 50.80 49.20 0.4326 100 1.590 (McLauchlan, Z. phys. Ch. 1903, 44. 627.) Solubility in acetic acid+Aq at 25. Molecules of CEbCOOH in 100 molecules CHsCOOH +H 2 O Molecules of H 2 O in 100 molecules CHsCOOH +H 2 O Normality of the iodine solution 0.0 6.98 16.40 31.90 55.70 100 100 93.02 83.60 68.10 44.30 0.0022 0.0049 0.0112 0.0331 0.0882 0.205 (McLauchlan, Z. phys. Ch. 1903, 44. 627.) Very sol. in ether, chloroform, and bromo- form. Solubility in ether. 100 g. of the sat. solution contain at: 83 90 108 15.39 14.58 15. 09 g. I 2 . (Arctowski, Z. anorg. 1896, 11. 276.) About as sol. in all fatty oils as in CHC1 3 , etc. (Gruel, Arch. Pharm. 223. 431.) IODINE 413 Sol. in 56.6 pts. chloroform at 10. (Dun- can, Pharm. J. Trans. 51. 544.) Solubility in CHC1 3 . 100 g. of the sat. solution contain at: 49 55.5 60 69.5 73.5 0.188 0.144 0.129 0.089 O.OSOg. I 2 . (Arctowski, Z. anorg. 1896, 11. 276.) Very sol. in methvlene iodide. (Retgers, Z. anorg. 3. 343.) Solubility of I 2 in C 6 H 6 +CHC1 3 at room temperature (14.5 15.1). Solubility of I 2 in. CS 2 +CC1 4 at room temperature (14.5 15.1). Volumes of CS2 in 100 volumes of CS 2 +CCU Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 90 80 70 60 50 40 30 20 10 69.1 56.9 48.6 40.7 33.9 26.9 21.8 17.7 13.25 10.2 8.1 Volumes of C 6 H 6 in 100 volumes of CeHe+CHCU Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 90 80 70 60 50 40 30 20 10 41.05 38.8 34.6 30.5 27.4 24.4 21.0 % % - 19.2 * 17.8 16.0 14.3 (Bruner.) Solubility of I 2 in C 2 H 5 OH+CHC1 3 at room temperature (14.5 15.1). Volumes of CiHsOH in 100 volumes of C 2 H 5 OH + CHCh Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 90 80 70 60 50 40 30 20 10 61.7 37.1 34.2 30.7 27.9 26.1 24.6 22.7 19.9 17.1 14.25 (Bruner, Z. phys. Ch. 1898, 26. 147.) Solubility of I 2 in CS 2 +CHC1 3 at room temperature (14.5 15.1). Volumes of CS2 in 100 volumes of CS 2 +CHCU Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 90 80 70 60 50 40 30 20 10 69.4 62.7 55.9 47.9 42.0 35.8 30.4 25.3 20.8 17.0 14.3 (Bruner.) Solubility of I 2 in C 3 H 7 OH+CHC1 3 at room temperature (14.5 15.1). Volumes of CsHrOH in 100 volumes of CzR-.OH +CHC1 3 Ccm. of 1/10-normal iodine in 5 cc. of the solution (Bruner.) Solubility of I 2 in C 6 H 6 +CC1 4 at room temperature (14.5 15.1). 100 90 80 70 60 50 40 30 20 10 58.8 51.9 44.2 35.4 31.8 30.8 27.9 25.3 21.8 17.8 14.25 Volumes of C 6 H 6 in 100 volumes of CePU+CCU Ccm. of 1/10-normal iodine in 5 cc. of the solution 100 90 80 70 60 50 40 30 20 10 41.05 37.2 33.6 29.6 26.1 22.4 19.25 16.1 13.4 10.75 8.1 (Bruner.) Sol. in acetone. (Naumann, B. 1904, 37. 4328); (Eidmanri, C. C. 1999, II. 1014.) Sol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) Sol. in allyl mustard oil, phenyl mustard (Bruner.) 414 IODINE oil, phenyl isocyanate, pyridine, and alcohol. (Mathews, J. phys. Chem. 1905, 9. 649.) Solubility of I 2 in glycerine +Aq at 25. G = g. glycerine in 100 g. glycerine +Aq. I2 = g. la in 100 cc. of the solution. G I 2 Sp. gr. 0.0304 0.9979 7.15 0.0342 1.0198 20.44 0.0482 1.0471 31.55 0.0621 1.0750 40.95 0.0875 1.0995 48.7 0.135 1 . 1207 69.2 0.278 1 . 1765 100 1.223 1.2646 (Herz and Knoch, Z. anorg. 1905, 45. 269.) 1 1. N-NH 4 C 2 H 3 O 2 +Aq dissolves 0.440 g. I 2 at 25. 1 1. 0.7 N-(NH 4 ) 2 C 2 O4+Aq dissolves 0.980 g. I 2 at 25. (McLauchlan, Z. phys. Ch. 1903, 44. 617.) Very sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) 1 1. CC1 4 dissolves 30.33 g. I 2 at 25. (Jakowkin, Z. phys. Ch. 1895, 18. 590.) Solubility in CS 2 . 100 g. of the sat. solution contain at: 80 87 92.5 94 0.509 0.440 0.391 0.378g. (Arctowski, Z. anorg. 1896, 11. 274.) When an aqueous solution of I is shaken with CS 2 , 400 pts. go into solution in CS 2 for 1 pt. remaining in H 2 O. (Berthelot and Jung- fleisch, C. R. 69. 338.) Abundantly sol. in methane. (Villard, A. ch. 1897, (7) 10. 387.) Easily sol. in hot, less in cold naphtha. (Pelletier and Walker.) Sol. in about 8 pts. hot petroleum from Amiano. (de Saussure.) SI. sol. in cold, more readily in hot ben- zene. (Mansfield.) Easily sol. in benzene. (Moride, A. ch. (3) 39. 452.) Solubility in benzene. 100 g. of the sat. solution contain at: 4.7 6.6 10.5 13.7 16.3 8.08 8.63 9.60 10.44 11.23g. 1 2 . (Arctowski, Z. anorg. 1896, 11. 276.) 1 1. benzene sat. with iodine at 25 contains 139 g- iodine. Abegg, Z. anorg. 1906, 50. 409.) 1 1. nitrobenzene dissolves 50.62 g. I 2 at 16-17. (Dawson and Gawler, Chem. Soc. 1902, 81. 524.) oomDinty in i^s 2 at i . Solubility of I 2 in nitrobenzene + iodides at t Grams iodine in 100 g. of sat. room temp. solution G. per 1. 0.32 Salt 100 - 95 0.37 Salt 12 90 0.41 KI 12.35 112.7 85 0.46 45.56 295.7 80 0.51 115.8 698.2 75 0.55 155.2 943.6 25 3.47 Nal 13.55 57.7 125 393 20 4.14 109.1 738 15 4.82 228. 1251 10 5.52 Rbl 85.4 421 5 6.58 a 217.5 1060 7.89 Lil 84.1 642 ,-f 5 10 15 20 25 30 36 40 42 9.21 10.51 12.35 14.62 16.92 19.26 22.67 25.22 26.75 Csl NH 4 I a SrI 2 BaI 2 Aniline hydriodide Dimethyl aniline hydriodide 48.2 223. 69.5 94.3 106.5 42.2 158.5 164 160 213 858 482 669 599 237 809 721 626 (Arctowski, Z. anorg. 1894, 6. 404.) Tetramethylammonium iodide 49.3 266 1 1. CS 2 dissolves 230 g. I 2 at 25. 1 1 r.TTRr. rlifianliroa 1 Q fifi o- ! a <- 9* tt 51.4 280 (Dawson and Goodson, Chem. Soc. 1904, 85. 796.) Sol in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 51. 236.) . Easily sol. in oil of turpentine, but an explo- sion soon occurs. (Walker.) Sol. in oil of mandarin. (Luca.) IODINE 415 Sol. in oil of arnica root. (Zeller.) Very sol. in CS 2 , lignone, furfurol, glycerine, aldehyde, chloral, warm retinole, toluene, sali- cylic acid, methyl nitrate, methyl salicylate, mercaptan, amyl carbamate, ethyl sulp hyd- rate, allyl iodide, ethyl disulphocarbonate, carbon chloride, SC1 2 , IC1 3 , H 2 S 5 , chloro- chromic acid, amyl valerianate, valerianic acid, warm butyric acid, creosote, aniline, quinoline, methylsalicylic acid. Quickly sol. in oil of dill, peppermint, sassafras, and tansy. Slowly sol. in oil of cloves, cinnamon, cajeput, and rue. Other essential oils decompose it. (Various authorities.) Sol. in potassium croconate + Aq. (Gmelin.) Sol. in potassium antimony tartrate+Aq. 176 pts. H 2 O-f6 pts. potassium antimony tartrate dissolve 2.75 pts. I; 378 pts. H 2 6 +6 pts. potassium antimony tartrate dissolve 4.12 pts. I. More sol. in tannic acid than in H 2 O. 1 pt. I is sol. in 450 pts. H 2 O with 3.3 pts. tannic acid at 12; 1 pt. I is sol. in 240 pts. H 2 O with 0.015 pt. tannic acid at about 30. (Roller, Zeit. Ch. 1866. 380.) 200 g. H 2 O containing 0.3-g. tannic acid dissolve 1.0 g. I. (Hager, Comm. 1883.) Sol. in considerable quantity, especially on warming, in resorcin, orcin, or phloroglu- cin-f-Aq, without coloration or formation of HI-j-Aq. These solutions withdraw 1 from CS 2 solution, and do not give it up on boiling, but on evaporation in vacuo the I is sublimed in a pure state. (Hlasiwetz, Z. anal. 6. 447.) Partition coefficient for iodine between CS 2 arid Aq at 25C. A = concentration of the water layer. C = concentration of the carbon bisulphide layer. A C h=C/A 0.2913 0.1934 0.1276 0.0818 0.0516 25.61 16.54 10.88 6.966 4.412 87.91 85.51 85.30 85.13 85.77 (Jakowkin, Z. phys. Ch. 1895, 18. 586-588.) G. alcohol in 100 cc. of mixture C aq. alcohol ccs 2 * 10 30.5 26.7 22.9 19.1 16.3 11.4 7.6 1.29 0.76 0.49 0.34 0.28 0.23 0.20 A C h=C/A 0.2571 167.6 651.8 0.2195 140.2 638.7 0.1947 122.0 626.4 0.1743 108.3 620.0 0.1605 98.27 612.2 0.1229 73.23 595.8 0.1104 65.81 596.0 0.0939 55.29 590.5 0.0518 30.36 586.2 Partition coefficient for iodine between CHBrj and Aq at 25C. A = concentration of the water layer. C = concentration of the CHBr 3 layer. Partition coefficient for iodine between CC1 4 and Aq at 25C. A = concentration of the water layer. C = concentration of the CC1 4 layer. (Osaka, Chem. Soc. 1905, 88. (2) 811.) Division of iodine between CS 2 and Na 2 SO 4 +Aqat25. A = concentration of I in H 2 O layer. C = concentration of I in CS 2 layer. Na 2 SOi +Aq A C 1-N 1 / 2 -N Vr-N Va-N 0.1518 0.1809 0.2022 0.2138 142.4 141.7 143.6 142.4 Division of iodine between CS 2 and NaNOs +Aq. NaNOs +Aq A C 1-N Vr-N' Vr-N 0.1923 0.2090 0.2164 142.4 143.7 143.5 (Jakowkin, Z. phys. Ch. 1896, 20. 25.) Partition between CHC1 3 and glycerine. C=millimols iodine in 10 g. CHC1 3 layer. W = millimols iodine in 10 g. glycerine layer. A C g=C/A C w c/w 0.2736 0.1752 0.1084 0.0757 144.36 85.11 49.93 32.65 527.6 485.7 460.5 431.7 0.564 0.919 0.151 0.244 0.397 0.500 2.31 2.32 2.30 0.0517 22.19 429.3 (Herz, Z. Elektrochem. 1910, 16. 870.) 416 IODINE BROMIDE Partition of I 2 between CHC1 3 and other solvents. C =millimols iodine in 10 ccm. of the CHC1 3 layer. W = millimols iodine in 10 ccm. of the other layer. Distribution of I 2 between glycerine and CC1 4 att. MI = concentration of I 2 in CC1 4 layer ex- pressed in g.-mol. per 1. M 2 = concentration of I 2 in glycerine layer expressed in g.-mol. per 1, Other Solvent C w c/w t Mi Mi Water 0.338 1.546 2.318 3.207 3.439 0.0025 0.0120 0.0184 0.0242 0.0259 134.6 129.0 126.3 132.8 132.8 25 0.002230 0.0024113 0.0048227 0.010452 0.038973 0.04598 0.05820 0.0014386 0.0014595 0.0027014 0.005581 0.019959 0.023948 0.030097 75% by vol. H 2 O + 25% by vol. glycerine 1.217 1.893 2.434 3.219 0.0183 0.0290 0.0367 0.0483 66.32 65.33 66.31 66.65 40 0.00227 0.00239 0.00461 0.01092 0.02540 0.04091 0.06074 0.00127 0.00138 0.00272 0.00482 0.01116 0.01749 0.02701 50% by vol. H 2 O + 50% by vol. glycerine 1.217 1.835 2.376 3.294 0.0405 0.0609 0.0782 0.1020 30.0 30.1 30.4 32.2 25% by vol. H 2 O + 75% by vol. glycerine 1.188 1.806 2.656 2.859 3.400 0.116 0.173 0.249 0.265 0.312 10.25 10.45 10.66 10.80 10.93 50 0.00257 0.00500 0.01363 0.02549 0.04167 0.06309 0.00118 0.00225 0.00596 0.01050 0.01693 0.02502 (Herz, Z. Elektrochem. 1910, 16. 870.) Distribution of I 2 between benzene and glycerine at t. MI = concentration of I 2 in benzene layer expressed in g.-mol. per 1. M 2 = concentration of I 2 in glycerine layer expressed in g.-mol. per 1. (Landau, Z. phys. Ch. 1910, 73. 203.) Distribution of I 2 between ether and ethylene glycol at t. MI = concentration of I 2 in ether layer, expressed in g.-mol. per 1. M 2 = concentration of I 2 in C 2 H 6 O 2 layer, expressed in g.-mol. per 1. t Mi Ms 25 0.00757 0.01610 0.02719 0.04024 0.06255 0.07923 0.10243 0.12201 0.13342 0.16734 0.001604 0.002664 0.004115 0.005794 O.OOS34 0.01033 0.01324 0.01559 0.01668 0.02081 t Mi M 2 0.00843 0.03082 0.06551 0.08105 0.12528 0.31511 0.00571 0.01713 0.03736 0.04605 0.07148 0.17524 40 0.008545 0.01544 0.04432 0.095004 0.13271 0.18508 0.00181 0.002593 0.006242 0.012013 0.01632 0.02193 25 0.00870 0.01677 0.02710 0.03046 0.06385 0.11951 0.30820 0.00571 0.01001 0.01586 0.01713 0.03594 0.06725 0.17524 50 0.00865 0.01523 0.02683 0.04413 0.0620 0.07832 0.10153 0.12166 0.13199 0.18438 0.00184 0.00253 0.00390 0.00576 0.00744 0.00942 0.01214 0.0145 0.01560 0.02122 (Landau, Z. phys. Ch. 1910, 73. 205.) Iodine mowobromide, IBr. Slowly sol. in H 2 O with slight decomp. Sol. in CHC1 3 , CS 2 , ether, and alcohol. +5H 2 O. (Lowig, Pogg. 14. 485.) Does not exist. (Bornemann, A. 189. 183.) (Landau, Z. phys. Ch. 1910, 73. 202.) IODINE SULPHIDE 417 Iodine pew/abromide, IBr 5 (?). Sol. iri H 2 O with separation of iodine. (Lowig, Pogg. 14. 485.) Iodine wonochloride, IC1. Decomp. by H 2 O; sol. without decomp. in alcohol, ether, and HCl+Aq. Sol. in CS 2 . Iodine hydrogen chloride, IC1, HC1. Unstable. Sol. in ether. (Schiitzenberger, C. R. 84. 389.) Iodine ^nchloride, IC1 3 . Deliquescent. With H 2 O, a part is dissolved without decpmp., and the rest is decomp. The aqueous solution contains more un- changed Ids, the more cone, it is. (Serullas.) Precipitated from aqueous solution by H 2 SO 4 . Sol. in HCl+Aq. Sol. in warm cone. H 2 SO 4 without decomp. Sol. in alcohol, and ben- zene. Decomp. by small amount of CS 2 . (Christomanos, B. 10. 434.) Ether does not remove it from aqueous solution. (Serullas.) Iodine lithium chloride, IC1 3 , LiCl+4H 2 O. See Lithium chloroiodide. Iodine trichloride magnesium chloride, 2IC1 3 , MgCl 2 +5H 2 O. Very deliquescent and easily decomposed. (Filhol, J. Pharm. 25. 442.) +8H 2 O. Hydroscopic. (Weinland, Z. anorg. 1902, 30. 141.) Iodine ^'chloride manganous chloride, 2IC1 3 , MnCl 2 +8H 2 O. Hydroscopic. (Weinland, Z. anorg. 1902, 30. 139.). Iodine bichloride nickel chloride, 2IC1 3 , MC1 2 +8H 2 O. Hydroscopic. CC1 4 dissolves out IC1 3 . (Weinland, Z. anorg. 1902, 30. 138.) Iodine raonochloride phosphorus pentathloT- ide, IC1, PC1 5 . Very deliquescent; decomp. by H 2 O. Iodine potassium chloride, IC1 3 , KC1. Sol. in H 2 O with decomp. Ether dissolves out IC1 3 . (Filhol, J. Pharm. 25. 433, 506.) See Potassium chloroiodide. Iodine sodium chloride, IC1 3 , NaCl+2H 2 O. See Sodium chloroiodide. Iodine trichloride strontium chloride, 2IC1 3 , SrCl 2 +8H 2 O. Hydroscopic. (Weinland, Z. anorg. 1902. 30. 142.) Iodine trichloride sulphur te^rachloride, IC1 3 , SC1 4 . Very deliquescent in air; decomp. by H 2 O. Decomp. with formation of clear solution by dil. HNO 3 +Aq. (Weber, Pogg. 128. 459.) SC1 2 , 2IC1 3 . (Jaillard, J. B. 1860. 95.) Correct formula is as above. (Weber, I. c.) 2IC1,, SC1 4 . Sol. in S0 2 C1 2 , SOC1,, POC1 3 , warm SC1 2 , petroleum ether, ligroin, CHCls, CC1 4 , CS 2 and abs. ether. (Ruff, B. 1904, 37. 4519.) Iodine trichloride zinc chloride, 2IC1 3 , ZnCl 2 + 8H 2 O. Unstable. Hydroscopic. (Weinland, Z. ahorg. 1902, 30. 140.) Iodine perctafluoride, IF 5 . Fumes in air; decomp. with H 2 O. (Gore. C. N. 24. 291.) Decomp. by H 2 into iodic acid and HF. Decomp. by solutions of the alkalies. (Mois- san, C. R. 1902, 135. 564.) Iodine ^n'oxide, I 2 O 3 . Decomp. by H 2 O. (Ogier, C. R. 85. 957; 86. 722.) Probably a mixture. Iodine tafroxide, I 2 O 4 (?). Insol. in cold, decomp. by hot H 2 O; insol. in alcohol. Decomp. by HNO 3 +Aq. Sol. in H 2 SO 4 . (Millon, J. pr. 34. 319, 337.) Iodine pentoxide, I 2 O 5 . Very sol. in H 2 O, and in dil. alcohol. Insol. in absolute alcohol, ether, CS 2 , chloro- form, and hydrocarbons. Forms hydrates, iodic acid HIO 3 , and 3I 2 O5, H 2 O; insol. in ordinary alcohol. For sp. gr. of aqueous solution, see iodic acid. Iodine oxides, IioO 19 , I 3 Oi 3 . The compounds, IioOig (Millon, J. pr. 34. 336), and I 3 O 13 (Kammerer, J. pr. 83. 81), are probably mixtures. Millon's oxides are impure I 2 O 4 . (Kap- peler, B. 1911, 44. 3496.) Iodine sulphur oxide, 5I 2 O 5 , SO 3 . Decomp. by H 2 O. (Kammerer.) I 2 O S , 3SO 3 . Decomp. by H 2 O; si. sol. in hot SO 4 . (Weber, B. 20. 86.) = (IO) 2 (SO 4 ) 3 . lodyl sulphate (?). Iodine oxyfluoride, IOF 3 +5H 2 O. Fumes in the air. (Weinland, Z. anorg. 1908, 60. 163.) Iodine sulphide, S 2 I 2 . Sol. in CS 2 . (Linebarger, Am. Ch. J. 1895. 17. 57.) 418 IODINE SULPHOXIDE Iodine sulphoxide, I 2 SO 8 (?). Decomp. by H 2 O. (Schultz-Sellack.) I 2 (SO 3 ) 2 (?). Decomp. by H 2 O. (Weber, J. pr. (2) 26. 224.) Is(SO 8 )(?). As above. (Weber.) See also lodosulphuric anhydride. lodiridic acid. Ammonium iodiridate, (NH 4 ) 2 IrI 6 . Very easily sol. in cold H 2 O, decomp. on warming. Insol. in alcohol. (Oppler, J. B. 1857. 263.) Potassium iodiridate, K 2 IrI 6 . Very easily sol. in H 2 O. Insol. in alcohol. Sodium iodiridate, Na 2 IrI 6 . Insol. in cold. si. sol. in hot H 2 O. Easily sol. in acids. (Oppler.) lodiridous acid. Ammonium iodiridite, (NH 4 )6lr 2 Ii 2 +H 2 O. Very sol. in H 2 0, but decomp. on warming. (Oppler.) Potassium iodiridite, K 6 Ir 2 Ii 2 . Insol. in H 2 O, or alcohol. Slowly sol. in acids; easily in warm alkalies +Aq. Silver iodiridite, Ag 6 Ir 2 Ii 2 . Ppt. lodochloroplatiml/amine chloride, ( ? 1 Pt(N 2 H 6 Cl) 2 . 81. sol. in H 2 O. lodochromic acid. Potassium iodochromate, KCr0 3 I. Decomp. by boiling H 2 O. (Guyot, C. R. 73. 46.) . See also Chromoiodic acid. lodomolybdic acid. See Molybdoiodic acid. lodonitratoplatinraonodiamine bromide, I pf (NH 3 ) 2 Br m NO 3 rt NH 3 Br u;> Very si. sol. in H 2 O. (Cleve.) lodonitritoplatin^'amine nitrate, I(N0 2 )Pt(N 2 H 6 ) 2 (N0 3 ) 2 . Quite easily sol. in hot H 2 O. (Cleve.) lodopalladous acid. Potassium iodopalladite. Deliquescent. (Lassaigne.) lodophosphoric acid. See Phosphoiodic acid. lodoplatinamine iodide, I 2 Pt(NH 3 I) 2 . Sol. in H 2 O, especially easily if boiling. (Cleve.) lodoplatin^amine iodide, I 2 Pt(N 2 IU)2. Sol. in H 2 0, especially when hot. (Cleve.) mercuric iodide, I 2 Pt(N 2 H 6 I) 2 , 2HgI 2 . Extremely difficultly sol. in cold H 2 O; partly decomp. by boiling. (Jorgensen, Gm. K. 3. 1214.) nitrate, I 2 Pt(N 2 H 6 NO 3 ) 2 . More sol. in hot than cold H 2 Q. sulphate, I 2 Pt(N 2 H 6 ) 2 SO 4 . Very si. sol. in H 2 O. (Jorgensen. J. pr. (2) 15. 429.) lodoplatinsew^amine iodide, I 3 Pt(NH 3 ) 2 I(?). 81. sol. in H 2 O. (Jorgensen, J. pr. (2) 16. 345.) periodide, I 3 Pt(NH 3 ) 2 I, I 2 . Moderately si. sol. in H 2 O. (Cleve.) lododi'platinamine iodide, I 2 Pt 2 (N 2 H6) 2 I 4 . Insol. in H 2 O. lododiplatincfo'amine anhydroiodide, I 2 Pt 2 (N 2 H 6 ) 4 OI 2 . Insol. in NH 4 OH+Aq. anhydronitrate, I 2 Pt 2 (N 2 H 6 ) 4 O(NO 3 ) 2 . Easily sol. in warm H 2 SO 3 +Aq. (Cleve.) iodide, I 2 Pt 2 (N 2 H 6 ) 4 I 4 . Ppt. nitrate, I 2 Pt 2 (N 2 H 6 ) 4 (NO 3 ) 4 +4H 2 O. 81. sol. in cold, moderately sol. in hot H 2 O. (Cleve.) phosphate, I 2 Pt 2 (N 2 H 6 ) 4 [O 3 P(OH)] 2 . Nearly insol. in H 2 O. sulphate, I 2 Pt 2 (N 2 H 6 ) 4 (S0 4 ) 2 . Nearly insol. in H 2 O. platoeframine sulphate, I 2 Pt 2 (N 2 H 6 ) 4 SO 4 , Pt(NH 3 ) 2 S0 4 . Very si. sol. in H 2 O. (Carlgren Sv. V. A. F. 47. 306.) lodoplatinic acid, H 2 PtIe+9H 2 O. Deliquescent. Easily sol. in H 2 O, with de- comp. into PtI 4 and HI on standing or warni- ng. (Topsoe.) IODOSELENATE, POTASSIUM 419 Ammonium iodoplatinate, (NH 4 ) 2 Ptl6. Easily sol. in H 2 O. (Topsoe.) NHJ, PtI 4 . SI. sol. in H 2 O; insol. in alcohol. (Lassaigne, A. ch. (2) 51. 128.) Barium iodoplatinate, BaPtle. Deliquescent, but less so than Na 2 PtI 6 which it otherwise resembles. (Lassaigne.) Calcium iodoplatinate, CaPtI 6 + 12H 2 O. Not so deliquescent as Na salt. Cobalt iodoplatinate, CoPtI 6 +9H 2 O. Very deliquescent. Lead tefraiodoplatinate, [PtI 4 (OH) 2 ]Pb, Pb(OH) 2 . Ppt. (Belluci, C. C. 1902, I. 625.) Magnesium iodoplatinate, MgPtIe+9H 2 O. Sol. in H 2 O. Manganese iodoplatinate, MnPtI 6 +9H 2 O. Very deliquescent. Mercuric ^raiodoplatinate, [PtI 4 (OH) 2 ]Hg. Ppt. (Belluci, C. C. 1902, I. 625.) Nickel iodoplatinate, NiPtI 6 +9H 2 O. Very deliquescent. Potassium iodoplatinate, K 2 PtI 6 . Easily sol. in H 2 O. Insol. in alcohol. Not attacked by cold cone. H 2 SO 4 . * Silver tefraiodoplatinate, Pt[I 4 (OH) 2 ]Ag 2 . Ppt. (Belluci, C. C. 1902, I. 625.) Sodium iodoplatinate, Na 2 PtI 6 +6H 2 O. Not deliquescent, but easily sol. in H 2 O iqi] .ol. and alcohol. (Vauquelin.) Deliquescent. (Lassaigne.) Thallium te(miodoplatinate, [PtI 4 (OH) 2 ]Tl 2 . Ppt. (Belluci, C. C. 1902, I. 625.) Zinc iodoplatinate, ZnPtI 6 +9H 2 O. Easily sol. in H 2 O. lodoplatinocyanhydric acid, H 2 Pt(CN) 4 l2. See Periodoplatinocyanhydric acid. Silver iodoplatinocyanide, Ag 2 (PtI 2 (CN 4 ) 2 . Ppt. (Miolati, Gazz. ch. it. 1900, 30. 588.) Strontium iodoplatinocyanide platinocyanide, SrPt(CN) 4 I 2 , 10SrPt(CN) 4 +zH 2 O. (Hoist.) lodopurpureochroiaium chloride, ICr(NH 3 )5Cl 2 . Quite sol. in H 2 O. (Jorgensen, J. pr. (2) 25. 83.) chloroplatinate, ICr(NH 3 ) 5 PtCl. Precipitate. (Jorgensen, I. c.) iodide, ICr(NH 3 ) 6 I 2 . Difficultly sol. in H 2 O. Insol. in HI, or KI+Aq; insol. in alcohol. (Jorgensen, 1. c.) nitrate, ICr(NH 3 )5(NO 3 ) 2 . Much less sol. in H 2 O than the chloride. (Jorgensen, 1. c.) lodopurpureocobaltic iodide, CoI(NH 3 ) 6 I 2 . (Claudet.) Does not exist. (Jorgensen, J. pr. (2) 26. 94.) lodopurpureorhodium chloride, IRh(NH 3 ) 5 Cl 2 . Relatively easily sol. in H 2 O; insol. in HC1 +Aq and alcohol. Insol. in KI+Aq. (Jor- gensen, J. pr. (2) 27. 433.) fluosilicate, IRh(NH 3 ) 5 SiF 6 . Nearly insol. in cold H 2 O. iodoplatinate, IRh(NH 3 ) 5 PtI 6 . Ppt. iodide, IRh(NH 3 ) 5 I 2 . Very si. sol. in cold H 2 O; more sol. in hot H 2 O; insol. in dil. HI-f-Aq, and alcohol. (Jorgensen, J. pr. (2) 27. 433.) nitrate, IRh(NH 3 ) 5 (NO 3 ) 2 . SI. sol. in H 2 O, more easily sol. in hot H 2 O; insol. in dil. HNO 3 +Aq, and alcohol. sulphate, IRh(NH 3 ) 5 SO 4 , and -f 3H 2 O. SI. sol. in even hot H 2 O. (Jorgensen.) lodoselenic acid. Ammonium iodoselenate, 2(NH 4 ) 2 O, I 2 O 5 2SeO 3 +H 2 O. Decomp. by H 2 O. (Weinland, B. 1903, 36. 1400.) 2(NH 4 ) 2 O, 3I 2 O 5 , 2SeO 3 +5H 2 O. Sol. in H 2 O with decomp.(?). (Weinland.) Potassium iodoselenate, 2K 2 O, I 2 O 5 , 2SeO 3 + H 2 O. Decomp. by H 2 O. (Weinland.) 2K 2 O, 3I 2 O 5 , 2SeO 3 +5H 2 O. Sol. in H 2 O with decomp.(?) (Weinland.) 420 IODOSELENATE, RUBIDIUM Rubidium iodoselenate, 2Rb 2 O, 3I 2 O 5 , 2Se0 3 +5H 2 0. Sol. inH 2 O. (Weinland.) lodostannous acid. Data concerning solubility of SnI 2 in HI + Aq indicate formation of this compound. (Young, J. Am. Chem. Soc. 1897, 19. 853.) lodosulphobismuthous acid. Cuprous iodosulphobismuthite, 2Cu 2 S, Bi 2 S 3 , 2BiSI. Decpmp. by H 2 O at ord. temp. Decomp. by mineral acids with evolution of H 2 S. (Ducatte, C. R. 1902, 134. 1213.) Lead iodosulphobismuthite, PbS, Bi 2 S 3 , 2BiSI. Insol. in H 2 O. Partially decomp. by boil- ing H 2 O. Decomp. by dil. mineral acids with evolution of H 2 S. (Ducatte.) * Io do sulphuric acid. Ammonium iodosulphate, (NH 4 ) 2 SO 3 I 2 (?). Very sol. in H 2 O. (Zinno, N. Rep. Pharm. 20. 449.) Mercuric iodosulphate, Hg 2 (SO 4 )I 2 . See Mercuric sulphate iodide. Potassium iodosulphate, K 2 SO 3 I 2 (?). Sol. in 7.14 pts. H 2 O at 15. (Zinno, N. Rep. Pharm. 20. 449.) Sodium iodosulphate, Na 2 SO 3 I a +10H 2 O. Sol. in 3.64 pts. H 2 at 15 and in dil. alcohol. (Zinno, N. Rep. Pharm. 20. 449.) Does not exist. (Michaelis and Koethe, B. 6. 999.) lodosulphuric anhydride, ISO 3 . Decomp. very violently by H 2 O. (Weber, J. pr. (2) 25. 224.) Diiodosulphuric anhydride, I 2 SO 3 . Decomp. with H 2 O, but not so violently as ISO 3 . (Weber, J. pr. (2) 25. 224.) lodo^n'sulphuric anhydride, I(SO 3 ) 3 . Decomp. by H 2 O. (Weber, J. pr. (2) 25. 224.) lodotelluric acid. Ammonium iodotellurate, (NH 4 ) 2 O, I 2 O fi 2TeO 3 +6H 2 O. Sol. in H 2 O. (Weinland, Z. anorg. 1901 28. 52.) (NH 4 ) 2 O, I 2 O 5 , 2TeO 3 +8H 2 O. Sol. in H 2 O. (Weinland, B. 1900, 33. 1017.) Caesium iodotellurate, Cs 2 TeI 4 . Insol. in Csl, or HI+Aq. Decomp. slowly by cold, rapidly by hot H 2 O. (Wheeler, Sill. Am. J. 145. 267.) Potassium iodotellurate, K 2 TeI 6 +2H 2 O. SI. efflorescent. Somewhat sol. in KI+Aq, and dil. HI+Aq. (Wheeler.) K 2 O, I 2 O 5 , TeO 3 +3H 2 O. Sol. in H 2 O. Partially decomp. on recryst. from H 2 O. (Weinland, Z. anorg. 1901, 28. 53.) K 2 O, I 2 O 5 , 2TeO 3 +6H 2 O. Sol. in H 2 O without decomp. (Weinland.) Rubidium iodotellurate, Rb 2 TeI 6 . SI. sol. in HI, or Rbl+Aq. Decomp. by H 2 O. Somewhat sol. in alco q. hol. (Wheeler.) Rb 2 O, I 2 O 5 , 2TeO 3 +6H 2 O. Sol. in H 2 O. (Weinland.) lodotetramine chromium iodide, ICr(NH 3 ) 4 I 2 +H 2 0. Sol. in H 2 O. Pptd. by alcohol. (Cleve.) lodotetramine cobaltic sulphate, ICo(NH 3 ) 4 SO 4 . (Vortmann and Blasberg, B. 22. 2652.) lodotungstic acid. See Tungstoiodic acid. lodous acid, I 2 O 3 . See Iodine ^noxide. lodovanadic acid, I 2 O 5 , V 2 O 5 +5H 2 O. Very easily sol. in H 2 O. 2V 2 O 5 , 3I 2 O 5 +18H 2 O. (Ditte, C. R. 102. 757.) Ammonium iodovanadate, 3(NH 4 ) 2 O, 2V 2 O 5 , 5I 2 O 6 +20H 2 O. Sol. in H 2 O. (Ditte, C. R. 102. 1019.) Irididiamine compounds, Cl 2 Ir(NH 3 ) 4 X 2 . See Chloriridfamine compounds'. Iridic acid. Potassium iridate (?). Sol. in H 2 O and HCl-f Aq. Iridicyanhydric acid, H 3 Ir(CN) 6 . Easily sol. in H 2 O, still more easily in al- cohol, less in ether. (Martius, A. 117. 369.) Barium iridicyanide, Ba 3 fIr(CN) 6 ] 2 +18H 2 O. Efflorescent. Easily sol. in hot or cold H 2 O. Nearly insol. in alcohol. Not decomp. by acids. IRIDIUM PHOSPHORUS SULPHUR CHLORIDE 421 Cupric iridicyanide ammonia, Cu 3 Ir9(CN)i 2 , 6NH 3 +4H 2 O. Ppt. Decomp. in air. (Rimbach, Z. anorg. 1907, 62. 413.) Potassium iridicyanide, K 3 Ir(CN) 6 . Easily sol. in H 2 O. Silver iridicyanide ammonia, Ag 3 Ir(CN) 6 , 2NH 3 +3H 2 O. Ppt. Decomp. in the light. (Rimbach, Z. anorg. 1907, 52. 414.) Indium, Ir. Insol. in all acids, including aqua regia, except when in finely divided state, as "iridium black," when it is sol. in aqua regia. (Glaus, J. pr. 42. 251.) Iridium ammonia compounds. See Chloriridicfo'amine comps., ClIr(NH 3 ) 2 X. Irido^namine Iridopeft/amine Iridoaquope /famine Iridosoamine Iridosocfo'amine Ir(NH 3 ) 3 X 3 . Ir(NH 3 ) 5 X 3 . Ir(NH 3 ) 4 X 2 . Ir(NH 3 ) 5 (OH 2 )X 3 . Ir(NH 3 ) 2 X 2 . ' Ir(NH 3 ) 4 X 2 . Iridium fribromide, IrBr 3 +4H 2 O. Easily sol. in H 2 O. Insol. in alcohol or ether. (Birnbaum.) Iridium tefrabromide, IrBr 4 , or H 2 IrBr 6 . Deliquescent. Sol. in H 2 O and alcohol. (Birnbaum.) See Bromiridic acid. Iridium hydrogen sesquibromide, 3HBr, IrBr 3 +H 2 O =H 3 IrBr 6 +3H 2 O. See Bromiridous acid. Iridium sesquibromide with MBr. See Bromiridite, M. Iridium te^rabromide with MBr. See Bromiridate, M. Iridium phosphorous bromide, IrBr 3 , 3PBr 3 . Partially decomp. by H 2 O into a sol., and insol. modification. Sol. in PBr 3 . (Geisen- heimer.) IrBr 3 , 2PBr 3 . Not easily attacked by H 2 O. IrBr 4 , 2PC1 3 . See Iridium phosphorus chlorobromide. Iridium carbide, IrC 4 (?). (Berzelius.) Stable toward H 2 O, acids, and alcohol. (Strecker, B. 1909, 42. 1773.) Iridium wowochloride, IrCl. Insol. in acids and bases. (Wohler, B. 1913, 46. 1584.) Iridium ^chloride, IrCl 2 . Insol. in acids and bases. (Wohler, B. 1913, 46. 1585.) Iridium bichloride, IrCl 3 . Insol. in acids or alkalies. (Glaus, C. C. 1861. 690.) Insol. in H 2 O, acids and alkalies, (Leidie, C. R. 1899, 129. 1251.) +4H 2 O. Sol. inH 2 O. (Claus.) Iridium tefrachloride, IrCl 4 , or H 2 IrCl 6 (?). Deliquescent, and easily sol. in H 2 O. Iridium ^'chloride with MCI. See Chloriridite, M. Iridium tetmcbloride with MCI. See Chloriridate, M. Iridium chloride with potassium chloride and sulphite. See Chloriridosulphite, potassium. Iridium phosphorus chloride, IrP 2 Cl 9 . Insol. in cold H 2 O. SI. decomp. by hot H 2 O. (Geisenheimer, A. ch. (6) 23. 254.) IrP 2 Clio. Very sol. in chloroform. (G.) IrP 3 Cl 12 . Easily sol. in PC1 3 , or CHC1 3 , also in CS 2 with gradual decomp. SI. sol. in cold H 2 O. Decomp. by boiling into IrCl 3 , 3H 3 PO 4 . SI. sol. in benzene, ligroin and CC1 4 . (Strecker, B, 1909, 42. 1772.) +H 2 O. Insol. in PC1 3 at 100. Very slowly sol. in boiling H 2 O. (Geisenheimer, A. ch. (6) 23. 266.) IrP 3 Cl 15 . Decomp. by H 2 O into 2IrCl 3 , 3H 3 PO 3 , 3H 3 PO 4 . Violently decomp. by alcohol. SI. sol. in cold, more in hot POC1 3 , without decomp. Very sol. in PC1 3 with decomp. into IrP 3 Cli 2 ; similarly in PBr 3 . Sol. in AsCl 3 with combination. Sol. in CS 2 with decomp. Sol. in SC1 2 with combination. Easily sol. in cold C G H 6 with decomp. Insol. in CC1 4 . Sol. in CHC1 3 with decomp. (Gei- senheimer, A. ch. (6) 23. 254.) Iridium phosphorus arsenic chloride, 2IrP 3 Cl 15 , 5AsCl 3 . Sol. in H 2 O with decomp. into correspond- ing acid. (Geisenheimer, C. R. 110. 1336.) IrCl 3 , 2PC1 3 , 2AsCl 3 . Very sol. in H 2 O with decomp. Sol. in AsCl 3 ; insol. in CC1 4 . ( Geisenheimer . ) Iridium phosphorus sulphur chloride, IrCl 3 , 2PC1 3 , 2SC1 2 . Very sol. in si. amt. H 2 O, with decomp. into an acid analogous to chlorophosphoiridic acid. Sol. in SC1 2 . (Geisenheimer.) 422 IRIDIUM PHOSPHORUS CHLOROBROMIDE Iridium phosphorus chlorobromide, IrBr 4 , 2PC1 3 . (Geisenheimer, C. R. 111. 40.) Iridium ^hydroxide, IrO 2 , 2H 2 O = IrO 4 H 4 . Insol. in dil. HNO 3 , or H 2 SO 4 +Aq. Slowly but completely sol. in HCl-j-Aq. Sol. in KOH, and NaOH+Aq. (Glaus, J. pr. 39. 104.) Iridium sesqmhy dioxide, Ir 2 O 6 H 6 . Not attacked by acids, except slightly by cone. HCl+Aq. (Glaus, C. C. 1861. 690.) Iridium friiodide, IrI 3 . Very si. sol. in cold, somewhat more in hot H 2 O. Insol. in alcohol. (Oppler. J. B. 1857. 263.) Iridium tetraiodide, IrI 4 . Insol. in H 2 O or acids. (Lassaigne.) Sol. in solutions of iodides. (Oppler.) Iridium Zn'iodide with MI. See lodiridite, M. Iridium tetraiodide with ML See lodiridate, M. Iridium dioxide, IrO 2 . Very si. sol. in acids. Freshly pptd. Sol. in cone. H 2 SO 4 , hot 2-N H 2 SO 4 , HNO 3 , HC1. Insol. in 2-N KOH and si. sol. in hot 1-N KOH. Dried in a dessicator. Sol. in HC1. Insol. in H 2 SO 4 , HNO 3 and KOH. Dried at 100. Sol. in hot cone. HC1. Insol. in H 2 SO 4 , HNO 3 and KOH. (Wohler, Z. anorg. 1908, 67. 334.) See also Iridium dihy dioxide. Iridium trioxide, IrO 3 . Unstable. (Wohler, Z. anorg. 1908, 67. 340.) Iridium sesquioxide t Ir 2 O 3 . Insol. in acids. Sol. in cone. H 2 SO 4 , and hot cone. HC1. Forms colloidal solution with dil. HC1. Cone. HNO 3 converts it into the dioxide. Insol. in KOH+Aq. (Wohler, Z. anorg. 1908, 57. 339.) Iridium oxybromide, Ir 3 Br 8 O 2 =2IrBr 4 , IrO 2 . Not decomp. by H 2 O. (Geisenheimer, A. ch. (6) 23. 286.) Iridium phosphide, Ir 2 P. (Clarke and Joslin, Am. Ch. J. 6. 231.) Iridium sesgwselenide, Ir 2 Se 3 . Insol. in HNO 3 ; slowly sol. in hot aqua regia. (Chabrie" and Bouchonnet, C. R. 1903, 137. 1060.) Iridium raonosulphide, IrS. Inso!. in HNO 3 -f-Aq, and very si. sol. if at all in aqua regia. (Berzelius.) Sol. in K 2 S, and KSH+Aq. +zH 2 O. SI. sol. in H 2 O; sol. in cold HNO 3 +Aq. Insol. in NH 4 Cl+Aq or dil. acids. More sol. in K 2 S+Aq than PtS 2 . (Berzelius.) Iridium ^sulphide, IrS 2 . Not attacked by H 2 O, but decomp. when exposed moist in air. Not Attacked by sat. HCl+Aq or by cone. HNO 3 +Aq, but is oxidised by fuming HNO 3 +Aq, and aqua regia. Insol. in NH 4 sulphides, or polysul- phides+Aq. Slowly sol. in alkali polysul- phides-f Aq. (Antony, Gazz. ch. it. 23, 1. 190.) Iridium sesgm'sulphide, Ir 2 S 3 . SI. sol. in H 2 O. Sol. in HNO 3 , or K 2 S+Aq. IridoJnamine chloride, Ir(NH 3 ) 3 Cl 3 . SI. sol. in H 2 O. Not attacked by boiling H 2 SO 4 . (Palmaer, B. 22. 15.) Irido^raamine chloride, Ir(NH 3 ) 4 Cl 3 . Very sol. in H 2 O. (Palmaer, B. 22. 15.) chlorosulphate,[Ir(NH 3 ) 4 Cl 2 ]S0 4 + 4H 2 O. (Palmaer.) Iiidopentamme bromide, Ir(NH 3 )6Br 3 . Sol. in 352 pts. H 2 O at 12.5. (Palmaer, B. 23. 3817.) bromochloride, Ir(NH 3 ) 5 ClBr 2 . Sol.inH 2 O. (Palmaer, B. 24. 2090.) bromonitrite, Ir(NH 3 ) 6 Br(NO 2 ) 2 . Sol. in 17.9 pts. H 2 O at 18. (Palmaer.) bromosulphate, Ir(NH 3 ) 5 BrSO 4 +H 2 O. Sol. in H 2 O. (Palmaer.) carbonate, [Ir(NH 3 ) 5 ] 2 (C0 3 ) 3 +3H 2 O. Sol. in H 2 O. (Glaus, J. pr. 63. 99.) ^chloride, Ir(NH 3 ) 6 Cl 3 . Sol. in 153.1 pts. H 2 O at 15.1, (Palmaer, B, 23. 3810.) Sol. in hot H 2 O containing HC1. (Glaus, J. pr. 69. 30.) chlorobromide, Ir(NH 3 ) 5 ClBr 2 . Sol. in 213.6 pts. H 2 O at 15. (Palmaer.) chloroiodide, Ir(NH 3 ) 6 ClI 2 . Sol. in 104.5 pts. H 2 O at 15. (Palmaer.) chlorooxalate, Ir(NH 3 ) 5 ClC 2 O 4 . SI. sol. in H 2 O. (Palmaer.) IRON 423 Iridopentamine chloronitrate, Ir(NH 3 )6Cl3N0 3 )2. Sol. in 51.54 pts. H 2 O at 15.4. (Palmaer.) chloronitrite, Ir(NH 3 ) 5 Cl(N0 2 ) 2 . Easily sol. in H 2 O. (Palmera.) chloroplatinate, Ir(NH 3 ) 5 Cl 3 , PtCl 4 . Very si. sol. in H 2 O. (Palmear.) chlorosulphate, Ir(NH 3 ) 5 ClSO 4 +2H 2 O. Sol. in 134.5 pts. H 2 O at 15. (Palmaer.) hydroxide, Ir(NH 3 ) 5 (OH) 3 . Known only in solution, which decomp. on evaporation. (Glaus.) nitrate, Ir(NH 3 ) 5 (NO 3 ) 3 . Moderately sol. in H 2 O. (Glaus.) Sol. in 349 pts. H 2 O at 16. (Palmaer.) sulphate, [Ir(NH 3 ) 6 ]2(SO 4 ) 3 . Sol. in H 2 O. (Glaus.) Iridoaquopentfamine bromide, Ir(NH 3 ) 5 (OH 2 )Br 3 . Sol. in 4 pts. H 2 O. Pptd. from aqueous solution by HBr+Aq. (Palmaer, B. 24. 2090.) chloride, Ir(NH 3 ) 6 (OH 2 )Cl 3 . Sol. in 1.2 to 1.5 pts. H 2 O at ord. temp. Pptd. by HCl+Aq from aqueous solution. (Palmaer, B. 24. 2090.) nitrate, Ir(NH 3 ) 5 (OH 2 )(NO 3 ) 3 . Sol. in about 10 pts. H 2 O at 17. Pptd. from aqueous solution by HNO 3 +Aq. (Pal- maer.) Iridonitrous acid, H 6 Ir 2 (NO 2 )i2. Easily sol. in H 2 O. (Gibbs, B. 4. 281.) Ammonium iridonitrite, (NH4)eIr 2 (NO 2 )i2. Almost insol. in cold H 2 O; decomp. by hot H 2 O with evolution of N 2 . Decomp. by hot cone. H 2 SO 4 or HC1. Insol. in sat. NH 4 C1+ Aq. (Leidie, C. R. 1902, 134. 1583.) Barium iridonitrite iridochloride, Ba 3 Ir 2 (NO 3 ) 12 , Ba 3 Ir 2 Cli 2 . Sol. in H 2 O. (Lang.) Mercuric iridonitrite, Hg 3 Ir 2 (NO 2 )i 2 . Insol. in H 2 O. (Gibbs, B. 4. 280.) Potassium iridonitrite, K 6 Ir 2 (NO 2 )i 2 . SI. sol. in cold, more sol. in boiling H 2 O. Decomp. by hot HC1 or H 2 SO 4 . Insol. in KCl+Aq. (Leidie, Bull. Soc. 1902, (3) 27. 937.) +2H 2 O. Moderately sol. in H 2 O. Potassium iridonitrite iridochloride, K 6 Ir 2 (N0 2 ) 12 , K 6 Ir 2 Cl 12 . Sol. in H 2 O. Silver iridonitrite, Ag 6 Ir 2 (NO 2 )i 2 . Difficultly sol. in cold, more easily in hot H 2 0. Sodium iridonitrite, Na6lr 2 (NO 2 )i 2 +2H 2 O. SI. sol. in H 2 O. Sol. in cold H 2 O. Decomp. by hot cone. H 2 SO 4 or HC1. (LeidiS, C. R. 1902, 134. 1583.) Sodium iridonitrite iridochloride, Na 4 Ir 2 Cl 2 (N0 2 ) 8 +2H 2 O. SI. sol. in H 2 O. (Gibbs.) Na6lr 2 (NO 2 )i 2 , NaJraCle. Insol. in cold, si. sol. in hot H 2 0. (Lang.) Iridosamine chloride, Ir(NH 3 ) 2 Cl 2 . Nearly insol. in H 2 O. (Skoblikoff, A. 84. 275.) sulphate, Ir(NH 3 ) 2 SO 4 . Easily sol. in H 2 O. (Skoblikoff.) Iridosodiamine chloride, Ir(N 2 H6) 2 Cl 2 . Insol. in cold, decomp. by hot H 2 O. (Skob- likoff.) - nitrate, Ir(N 2 H 6 NO 3 ) 2 . Easily sol. in H 2 O. . sulphate, Ir(N 2 H 6 ) 2 SO 4 . SI. sol. in cold, easily in boiling H 2 O. SI., sol. in alcohol. Irido sulphuric acid. Potassium iridosulphate, K 6 Ir 2 (SO 4 ) 6 . Sol. in H 2 O. (de Boisbaudran, C. R. 96. 1406.) Iridosulphurous acid. Ammonium iridosulphite, (NH 4 ) 6 Ir 2 (SO 8 )6+ 6H 2 O. Slightly sol. in H 2 O. (Birnbaum, A. 136. 179.) Potassium iridosulphite, K 6 Ir 2 (SO 3 ) 6 +6H 2 O. Slightly sol. in H 2 O. Sodium iridosulphite, Na6lr 2 (SO 3 )6+8H 2 O. Scarcely sol. in H 2 O. Iron, Fe. Permanent in dry air; oxidises only slowly in moist air, but rapidly when in contact with air and H 2 O simultaneously. Fe does not rust in contact with air and 424 IRON H 2 O containing alkalies even in very small amounts. (Payen, A. ch. 50. 305.) Not attacked at ord. temp, by H 2 O free from air. More easily oxidised by NH 4 salts -j-Aq than by H 2 O when exposed to air simultaneously. (Persoz, A. ch. (3) 24. 506.) Iron is slowly attacked by distilled H 2 O in presence of air. 100 ccm. distilled water re- moved 29 mg. from 11.8 sq. cm. iron in one week, while air free from CO 2 was passed through the solution. In presence of CO 2 , 54 mg. were removed. (Wagner, Dingl. 221. 260.) CO 2 acts as a catalyst for the solution of Fe by H 2 O. (Whitney, J. Am. Chem. Soc. 1903, 25. 394.) Iron is most easily oxidised when it is ex- posed to air, and H 2 O is deposited on it at the same time in liquid form. 100 1. sea water dissolve 27.37 g. from 1 sq. metre Fe; 29.16 g. from 1 sq. metre steel; 1.12 g. from 1 sq. metre galvanised Fe. (Cal- vert and Johnson, C. N. 11). 171.) Readily sol. in HC1, dil. H 2 SO 4 +Aq, and most other acids. Action of H 2 SO 4 +Aq (1:12) is very much accelerated by a few drops of PtCl 4 +Aq; the addition of As 2 O 3 arrests the action com- pletely. Tartar emetic and HgCl 2 diminish the action, but do not arrest it. CuSO 4 -|-Aq strongly accelerates the action, and Ag 2 SO 4 + Aq also to a less extent. In the case of HCl+Aq, the addition of small amts. of metallic salts also influences the action. Weak HC 2 H 3 O 2 +Aq has but little action, and the addition of PtCl 4 in- creases it; As 2 O 3 stops it; other solutions have no effect. With racemic and tartaric acids the phenomena are the same. With oxalic acid, PtCl 4 prevents the action. Saline solutions and even distilled H 2 O, when mixed with PtCl 4 , have slight solvent action. (Millon, C. R. 21. 45.) Above phenomena are due to galvanic ac- tion from metal deposited on the iron. (Barreswill, C. R. 21. 292.) H 2 SO 4 has only si. action on cast-iron at ord. temp, with exclusion of air. Weak acids have a strong action at higher temperatures. Charcoal pig-iron, and case-hardened cast- iron are much less attacked by weak acids at b.-pt. than other sorts of Fe. Scotch pig-iron is most strongly attacked. 99.8% H 2 SO 4 has very si. action on iron at ord. temp, when air is excluded. (Lunge, Dingl. 261. 131.) Resistance against dil. H 2 SO 4 +Aq is greatly increased by increase in amt. of C if chemically combined, less so by P or Si. (Ledebur, Dingl. 223. 326.) Passive Iron. When Fe is treated with pure cone. HNO 3 +Aq of 1.512-1.419 sp. gr., it soon becomes coated with a bluish or black coating, apparently FeO, and when thus covered Fe is not attacked by HNO 3 +Aq of any strength at ord. temp, or at the temp, of a freezing mixture; but action occurs on heating. Nor is Fe attacked at ord. temp, by acid of 1.401 sp. gr. or even somewhat weaker acid, though action begins at once on heating. Very dil. HNO 3 +Aq attacks Fe at ord. temp, with formation of NH 4 NO 3 and Fe(NO 3 ) 2 . The action of HNO 3 +_Aq is influenced by PtCl 4 . If acid containing 4.5 equivalents of H 2 O is diluted with 2-3 vols. H 2 O, and then poured on Fe turnings, they dissolve at once with evolution of nitrous fumes and formation of ferric salt, but if to the acid one drop of PtCl 4 be added, only H gas is evolved, and NH 4 NO 3 and Fe(NO 3 ) 2 are formed. (Millon, C. R. 21. 47.) The more H 2 O the acid contains the lower will be the temp, at which the Fe remains passive. Shaking the wire hastens the pas- sivity. Contact with Pt, Au, or C does not prevent it. Fe wire becomes passive by re- maining 10 min. in HNO 3 vapour. (Renard, C. R. 79. 159.) Iron may be made passive by HC1O 3 , HBrO 3 , HIO 3 , H 2 CrO 4 , in the same way as by HNO 3 . Iron may also be made passive by moderate ignition. Passivity occurs with HNO 3 +Aq of 1.38 sp. gr. after a short time at 31; but if temp, is 32, passivity does not occur. Colourless HNO 3 +Aq of 1.42 sp. gr. pro- duces passivity at 55 but not at 56. Red fuming HNO 3 +Aq of 1.42 sp. gr. produces passivity at 82 but not at 83. (Ordway, Sill. Am. J. (2) 40. 316.) The passivity of Fe is destroyed when it is placed in a magnetic field at a much lower temperature than when in normal condition. (Nichols and Franklin, Sill. Am. J. (3) 34. 419.) Passivity depends on a coating of NO which hinders the action of the acid. All operations which remove this layer terminate the pas- sivity, as shaking, rubbing, placing in a vacuum, etc. (Varenne, C. R. 89. 783.) When Fe is plunged in HNO 3 +Aq of 1.42 sp. gr. there is a sudden evolution of gas which ceases after 3 to 20 seconds, and the surface becomes bright. The same phenomena take place with a more dilute acid, if of not less than 1.32 sp. gr. In the latter case, there is an immediate evolution of gas, which sud- denly ceases and the metal becomes bright, but soon the acid begins to act again at a single point, and the action gradually spreads over the whole surface; this, however, soon ceases again, and we have an "intermittent passivity." If a part of a piece of iron is immersed in strong acid, the whole of it is made passive. This is explained by the NO spreading over the whole surface by capillarity. The passivity ceases when the Fe is placed in dil. acid, after a longer or shorter time, IRON BORIDE 425 according to the dilution of the acid, when the acid has sp. gr. = 1.30, after 11 days (( (f (( I OO ti K (( L26 " 32 hours it it (i j 16 (i 12 it Iron may also be made passive by long standing in NO gas under pressure. ( Varenne, C. R. 90. 998.) Fe is made passive by a coating of Fe 3 O 4 , not by NO. (Schonbein, Pogg. 39. 342.) (Beetz, Pogg. 67. 286.) (Ramann, B. 14. 1430.) Passivity may also be caused by NH 4 NO 3 +Aq, ammoniacal AgNO 3 -fAq, Fe(NO 3 ) 3 , Fe(N0 3 ) 2 , A1(N0 3 ) 3 , Co(NO 3 ) 2 , Ni(NO 3 ) 2 , etc.+Aq instead of HNO 3 +Aq. (Ramann. B. 14. 1933.) Hardly attacked by either dil. or cone, acids when they are under high pressure. (Cailletet C. R. 68. 395.) Iron is dissolved by HNO 3 +Aq, even when very cone., but no gas is evolved and the pro- cess is very slow. HNO 3 +Aq of the following sp. gr. dissolves the given amts. from strips of pure Fe. Sp. gr. of acid Diminution of weight in 24 hours 1.28 1.34 1.38 1.48 1.53 0.82% 0.75 0.29 0.34 5.80 (Gautier and Charpy, C. R. 113. 1451.) Insol. in liquid chlorine below 90. (Lange, Zeit. angew. Ch. 1900, 13. 686.) Insol. in liquid NH 3 . (Gore, Am. ch. J. 1898, 20. 828.) Not attacked by alkalies. Sol. in NaOH+Aq (34%) when air is blown through the liquid. (Zirnite, Ch. Ztg. 12. 355.) NaOH+Aq attacks iron and steel. (Vena- tor, Dingl. 261. 133.) NaOH -f- Aq has slight action on Fe between 15 and 100. (Lunge, Dingl. 261. 131.) Presence of alkalies prevent rusting en- tirely, and fats and oils greatly hinder it. (Wagner.) Sol. in alkali hydrogen carbonates +Aq. (Berzelius.) Sat. NaCl+Aq has si. but perceptible ac- tion on Fe. NH 4 Cl+Aq has stronger action than NaCl+Aq. (Lunge.) 100 ccm. H 2 O containing 0.5 g. NaCl or KC1 removed 42 mg. from 11.8 sq. cm. iron in one week, while air free from CO 2 was passed through the solution, and 72 mg. in presence of CO 2 . 100 ccm. H 2 O containing 1 g. NH 4 C1 re- moved 45 mg., and 76 mg. respectively under the above conditions. 100 ccm. H 2 O containing 0.8 g. MgCl 2 re- moved 49 mg., and 65 mg. respectively under the above conditions. Not attacked by 100 ccm. H 2 O containing 1 g. Na 2 CO 3 , or by CaO 2 H 2 +Aq. (Wagner, Dingl. 221. 260.) Action of KClO 3 +Aq. KClO 3 +Aq (6.3% KC1O 3 ) oxidised 11.21 g. cast iron and 20.1 g. pure iron from a surface of 1 sq. metre in 7 hours; KClO 3 +Aq (25% KC1O 3 ) oxidised 24.59 g. cast, and 44.90 g. pure Fe under above conditions; Ca(ClO 3 ) 2 , CaCl 2 +Aq (20 Baume) obtained by passing Cl through CaO 2 H 2 +Aq oxidised 85 g. cast, and 95 g. pure Fe under the above conditions. (Lunge and Deggeler, J. Soc. Chem. Ind. 4. 32.) Easily sol. in organic acids. Comparative action of oils on Fe. Amount Fe dissolved Neatsfoot oil 0.0875 grains Colza " 0.0800 Sperm 0.0460 Lard 0.0250 Olive 0.0062 Linseed " 0.0050 Seal 0.0050 Castor " 0.0048 Paraffine " 0.0045 Almond " 0.0040 "Lubricating" oil 0.0018 (Watson, C. N. 42. 190.) l/ p.c.m nlpin a.niH Hissolvps 0097 e\ FP in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Fe dissolves in albumen solution to the extent of 1 to 2 per cent. (Buchner, Arch. Pharm. (3) 20. 417.) Attacked by sugar +Aq at 115-120, also by inverted sugar or malt extract, not by glycerine or mannite+Aq. (Klein and Berg, C. R. 102. 1170.) Iron arsenide, FeAs 2 . Min. Lollingite. Sol. in HNO 3 +Aq with separation of As 2 O 3 . Fe 3 As4. Min. Leucopyrite. Iron arsenide sulphide, FeAs 2 , FeS 2 . Min. Arsenopyrite. Sol. in HNO 3 +Aq with separation of S and As 2 O 3 ; wholly sol. in aqua regia; not attacked by HCl+Aq. Iron boride, Fe 2 B. Decomp. by H 2 O. Sol. in hot dil. HC1 or H 2 SO 4 and in hot cone. HC1 or H 2 SO 4 . Sol. in hot dil., or cold cone. HNO 3 . (Jassonneix, C. R. 1907, 146. 122.) FeB. Sol. in molten alkali carbonates; not sol. in dil. or cone. H 2 SO 4 in the cold; sol. in boiling H 2 SO 4 and in HNO 3 . (Moissan, Bull. Soc. 1895, (3) 13. 958.) Stable in dry air. Decomp. by aqua regia, 426 IRON BROMIDE but not readily sol. in cone. H 2 SO 4 and HC1. (Moissan, C. R. 1895, 120. 176.) FeB 2 . Decomp. by H 2 O. Sol. in HNO 3 and in hot cone. HC1. (Jassonneix, C. R. 1907, 145. 122.) Iron (ferrous) bromide, FeBr 2 . Sol. in H 2 O. Decomp. by heating on air. Sat. FeBr 2 +Aq contains at: 21 7 +10 21 47.0 48.3 52.3 53.7%FeBr 2 , 37 50 65 95 56.0 58.0 59.4 63.3%FeBr 2 . (Etard, A. eh. 1894, (7) 2. 541.) +4H 2 O. Very sol. in H 2 O; pptd. from cooled aq. solution. (Volkmann, C. C. 1894, II. 611.) +6H 2 O. Sol. in H 2 O. (Lowig.) +9H 2 O. (Volkmann.) Ferric bromide, FeBr 3 . Deliquescent. Sol. in H 2 O, alcohol, and ether. (Lowig.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) +6H 2 O. Sol. in alcohol and ether. (Bol- schakoff, C. C. 1898, II. 660.) Ferrous mercuric bromide. Deliquescent, (v. Bonsdorff.) Ferric rubidium bromide, Rb 2 FeBr 6 +H 2 O. Sol. in H 2 O. (Walden, Z. anorg. 1894, 7. 332.) Ferrous stannic bromide. See Bromostannate, ferrous. Ferrous bromide nitric oxide, 3FeBr 2 , 2NO. Sol.inH 2 O. Not isolated. (Thomas, C. R. 1896, 123. 944.) Ferric bromochloride, FeCl 2 Br. Very deliquescent, and sol. in H 2 O, alcohol, and ether. Notably sol. in chloroform, ben- zene, and toluene. Insol. in CS 2 . (Lenor- mand, C. R. 116. 820.) Iron carbide, Fe 8 C. (Gurlt, J. B. 1856, 781.) Mixture of Fe and FeC 4 . (Tunner, Polyt. Centralbl. 1861. 1227.) Fe 4 C. (Karsten, J. pr. 40. 229.) Fe 3 C. Sol. in hot cone. HC1; oxidized slowly by moist air. (Campbell, Am. Ch. J. 1896, 18. 840-841.) Fe 2 C 2 . (Rammelsberg, C. C. 1847. 60.) Iron molybdenum carbide, Fe 3 C, Mo 2 C. Sol. in hydracids; insol. in HNO 3 . (Wil- liams, C. R. 1898, 127. 484.) Iron tungsten carbide, 2Fe 3 C, 3W 2 C. Insol. in H 2 O and hydracids; sol. in HNO 3 and H 2 SO 4 . (Williams, C. R. 1898, 127. 411.) Iron carbonyl, Fe(CO) 5 . Slowly decomp. on air. Not attacked by dil. H 2 SO 4 , HNO 3 , or HCl+Aq. Cone. HNO 3 , Cl 2 +Aq, or Br 2 +Aq decomp. easily. Sol. in alcoholic solution of KOH or NaOH with sub- sequent decomp. Sol. in alcohol, ether, benzene, mineral oils, etc. (Mond and Lan- ger, Chem. Soc. 59. 1090.) Fe 2 (CO) 7 . Decomp. on air. Not attacked by H 2 SO 4 or HCl+Aq. Sol. in alcoholic potash. Very much less sol. in organic sol- vents than Fe(CO) 5 . (Mond and Langer.) Ferrous chloride, FeCl 2 . Deliquescent. Easily sol. in H 2 O with evolution of heat, or in alcohol. Insol. in ether. (Jahn.) Sol. in 2 pts. H 2 O at 18.75. (Abl.) Sol. in 1 pt. strong alcohol. (Wenzel.) Sp. gr. of FeCl 2 =Aq at 15.5. Sp. gr. % FeCh % FeCh, 4H 2 1.05 5.40 8.45 1.06 6.43 10.09 1.07 7.47 11.69 .08 8.48 13.29 .09 9.49 14.86 .10 10.47 16.41 .11 il.45 17.86 .12 12.42 19.46 .13 13.37 20.96 .14 14.31 22.41 .15 15 24 23.87 .16 16.15 25.31 .17 17.05 26.73 .18 17.94 28.13 .19 18.83 29.51 .20 19.68 30.85 .21 20.50 32.14 .22 21.39 33.53 .23 22.24 34.84 .24 23.05 36.11 .25 23.86 37.38 .26 24.68 38.67 .27 25.44 39.87 .28 26.19 41.04 .29 26.98 42.29 .30 27.75 43.49 .31 28.49 44.65 .32 29.23 45.81 .33 29.96 46.94 1.34 30.68 48.08 1.35 31.39 49.18 1.36 32.10 50.30 1.37 32.79 51.39 1.38 33.47 52.46 1.39 34.14 53.50 1.40 34.80 54.55 1.41 35.46 55.57 1.42 36.09 56.56 1.43 36.73 57.55 1.44 37.33 58.51 (Dunn, J. So< 3. Chem. Ind. 1 902, 21. 390.) IRON CHLORIDE 427 Insol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Sol. in acetone; insol. in methylal. (Eid- mann, C. C. 1899, II. 1014.) Sol. in acetone. (Naumaim, B. 1904, 37. 4328.) SI. sol. in methyl acetate. (Naumann, B. 1909,42.3790.) Sol. .in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Yellow modification is sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Mol. weight determined in pyridine. (Wer- ner, Z. anorg. 1897, 16. 21.) +2H 2 O. (Jonas.) +4H 2 O. Deliquescent. Easily sol. in alcohol. Sol. in 0.68 pt. cold H 2 O. (Reimann, Mag. Pharm. 17. 215.) Sat. aq. solution contains at: 16 18 25 28 43 40.5 40.9 41.0 42.5 44.4%FeCl 2 , 50 53 72 89 96 118 45.0 45.9 49.2 51.3 51.0 51.7%FeCl 2 . (fitard, A. ch. 1894, (7) 2. 537.) 100 g. FeCl 2 , 4H 2 O+Aq contain 17.54 g. Fe at 22.8; 18.59 g, at 43.2. (Boecke, . N. Jahrb. Min. 1911, I, 61.) More sol. in water containing NO than in pure H 2 O. (Gay, Bull. Soc. (2) 44. 175.) Sol. in hot HCl+Aq. (Sabatier, Bull. Soc. 1895, (3) 13. 599.) [Sabatier could not obtain FeCl 2 +6H 2 O of Lescceur.] Ferroferric chloride, Fe 3 Cl 8 +18H 2 O. Deliquescent. (Lefort, J. Pharm. (4) 10. 85.) Ferric chloride, Fe 2 Cl 6 or FeCl 3 . Very deliquescent, and sol. in H 2 O with evolution of great heat. 100 mols. H 2 O dissolve mols. anhydrous Fe 2 Cl 6 at t. t Mols. FezCle t Mols. FeaCle 66 70 75 29.20 29.42 28.92 80 100 29.20 29.75 (Roozeboom, Z. phys. Ch. 10. 477.) See also hydrated salts below. Solution in H 2 O is decomp. into colloidal Fe 2 O 3 , zH 2 O and HC1, upon heating if cone., and on simple standing if dil. Krecke (J. pr. (2) 3. 286) gives the following table. % Fe 2 Cl 6 in solution Temp, at which Graham's colloidal hydrate is formed Temp, at which Saint Gilles' colloidal hy- drate is formed Temp, at which oxychlorides are formed Temp, at which FeaOs is formed 32 100-130 100 + 140 16 100-120 Fe 2 Cl 6 re- . . . " 120 8 100-110 formed on " 110 4 90-100 cooling. 90 2 87 87 1 83 i(XM30 . . . 0.5 75 Fe 2 Cl 6 not a .... . . . 0.25 64 reformed it ... 0.125 54 on cooling. " . . . 0.0625 36 " Sp. gr. of Fe 2 Cl 6 +Aq. % Fe 2 Cl 6 Sp. gr. at 4.8 Sp. gr. at 9.7 Sp. gr. at 14.6 Sp. gr. at 19.7 49.61 1.5609 1 . 5575 1.5540 1 . 5497 41.00 1.4413 1.4387 1.4361 1.4335 36.95 1.3847 1 . 3824 1.3800 33.25 1^3381 1.3359 1.3339 1.3317 24.60 1.2351 1.2334 1.2318 1.2298 22.54 1.2140 1.2129 1.2107 1.2090 16.79 1 . 1534 1 . 1521 1 . 1507 1.1491 10.45 1.0939 1.0930 1.0918 1.0901 4.65 1.0382 2.70 1.0221 (Schult, from Gerlach, Z. anal. 27. 278.) Sp. gr. of Fe 2 Cl 6 +Aq increases or diminishes between 8 and 24 for a decrease or in- crease of temp, of 1 by the following amts. % Fe 2 Cl6 Corr. % FesCle Corr. 50-60 45-49 40-44 0.0008 0.0007 0.0006 30-39 20-29 10-19 0.0005 0.0004 0.0003 (Hager, 1. c.) 428 IRON CHLORIDE Sp.gr. of Fe 2 Cl 6 +Aq at 17.5. ' Solubility of Fe 2 Cl 6 in HCl+Aq. ji -2? _s Sat. solution contains CD Sp. gr. \^sl Sp. gr. k\ ^ Sp. gr. per 100 mols. H 2 O fe LXJ ^ t Solid phase mols. HC1 mols. Fed 3 1 1.0073 1f\t AC* 21 1 . 1644 41 1.3746 3 .0146 1.0219 22 23 . 1746 .1848 42 43 1 . 3870 1.3994 30 12.70 4 1.0292 24 .1950 44 1.4118 " 5.92 16.07 5 1.0365 25 .2052 45 1.4242 tt 20.90 6 1 . 0439 26 .2155 46 1.4367 25 10.90 7 1.0513 27 .2258 47 1.4492 tt 2.33 23.72 8 1.0587 28 .2365 48 1.4617 ti 24.50 9 1.0661 29 .2464 49 .4742 20 10.20 10 1.0734 30 .2568 50 .4867 " 5.60 23.60 11 1.0814 31 1.2673 51 .5010 u 25.70 12 1.0894 32 1.2778 52 .5153 10 9.10 13 1.0974 33 1.2883 53 .5296 u 8.75 8.00 14 .1054 34 1.2988 54 .5439 it 16.70 16.65 15 .1134 35 1.3093 55 1.5582 " 13.80 23.35 16 .1215 36 1.3199 56 1 . 5729 8.25 17 .1297 37 1 . 3305 57 1 . 5876 tt 7.52 6.51 18 .1378 38 1.3411 58 1.6023 It 13.37 6.33 18 19 .1378 . 1458 38 39 1.3411 1.3517 58 59 1.6023 1.6170 11 It 16.80 18.45 8.70 10.23 Fe 2 Cl 6 +12H 2 O 20 1542 40 1.3622 60 1.6317 It 20.40 15.40 11 20 10 16 00 (Franz, J. pr. (2) 5. 283.) It 19.95 17.70 Sp. gr. of Fe 2 Cl 6 +Aq at 17.5. It It 19.00 18.05 22.75 23.40 O. Can be crystallised from HCl+Aq. (Wohler, A. 144. 250.) Ferrous chloride ammonia, 3FeCl 2 , 2NH 3 . Decomp. by H 2 O. (Rogstadius, J. pr. 86. 310.) FeCl 2 ,6NH 3 . Loses 4NH 3 at 100. (Miller, Am. Ch. J. 1895, 17. 577.) FeCl 2 , 2NH 3 . Decomp. in the air (Miller). Ferric chloride ammonia, FeCl 3 , NH 3 . Slowly deliquescent. Sol. in H 2 O with evolution of heat. (Rose, Pogg, 24. 302.) FeCl 3 , 6NH 3 . Not deliquescent; not sol. in H 2 O; sol. in HC1 with decomp. (Miller, Am. Ch. J. 1895, 17. 577.) Loses NH 3 to give FeCl 3 , 5NH 3 , and FeCl 3 , 4NH 3 . Ferric chloride cyanhydric acid, FeCl 3 , 2HCN. Deliquescent. (Klein, A. 74. 85.) Ferrous chloride nitric oxide, FeCl 2 , NO. Sol. in H 2 O without evolution of gas. (Thomas, C. R. 1895, 121. 204.) +2H 2 O. Sol. in cold H 2 O without decomp. (Thomas, C. R. 1895, 120. 448.) 2FeCl 2 , NO. Very hydroscopic. (Thomas, C. R. 1895, 121. 129.) 10FeCl 2 , NO. Very hygroscopic. (Thomas C. R. 1895, 121. 128.) Ferric chloride nitric oxide, Fe 2 Cl 6 , NO. Very hygroscopic. Loses NO when ex- posed to the air. 2Fe 2 Cl 6 , NO. Very hygroscopic. In con- tact with H 2 O gives off NO. (Thomas, C. R. 1895, 120. 447.) Iron (ferrous) fluoride, FeF 2 . SI. sol. in H 2 O; insol. in alcohol and ether. Partly sol. in hot HCl+Aq; slowly sol. in cold, easily in hot HNO 3 ; decomp. by H 2 SO 4 . (Poulenc, C. R. 115. 941.) +8H 2 O. Difficultly sol. in H 2 O; more easily if it contains HF. (Berzelius.) Ferroferric fluoride, FeF 3 , FeF 2 -f 7H 2 O. Sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 268.) Ferric fluoride, FeF 3 . SI. sol. in H 2 O; insol. in alcohol or ether. SI. attacked by HNO 3 , HC1, or H 2 SO 4 +Aq. (Poulenc, C. R. 115. 941.) +4^H^O. More sol. in hot than cold H 2 O. Insol. in alcohol. (Scheurer-Kestner, A. ch. (3) 68. 472.) Ferric nickel fluoride, FeF 3 , NiF 2 +7H 2 O. SI. sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 268.) Ferrous potassium fluoride, FeF 2 , KF+2H 2 O. (Wagner, B. 19. 896.) FeF 2 ,2KF. SI. sol. in H 2 O. (Berzelius.) Ferric potassium fluoride, FeF 3 , 2KF. Somewhat sol. in H 2 O, especially if hot. (Berzelius.) +H 2 O. (Christensen, J. pr. (2) 35. 164.) FeF 3 , 3KF. Properties as above. (Ber- zelius.) Ferric sodium fluoride, FeF 3 , 2NaF+3^H 2 O. Rather easily sol. in H 2 O. Solution de- comp. on heating. Very sol. in FeCl 3 +Aq. (Nickles, J. Pharm. (4) 10. 14.) FeF 3 , 3NaF. (Wagner, B. 19. 896.) Ferric thallous fluoride, 2FeF 3 , 3T1F. Sol. in hot H 2 O, less sol. in cold. SI. sol. in HF. (Ephraim, Z. anorg. 1909, 61. 239.) Ferrous titanium fluoride. See Fluotitanate, ferrous. Ferric zinc fluoride, FeF 3 , ZnF 2 +7H 2 O. SI. sol. in dil. HF+Aq. (Weinland, Z. anorg. 1899, 22. 269.) Ferrous hydroxide, FeO 2 H 2 . Sol. in 150,000 pts. H 2 O. (Bineau, C. R. 41. 509.) Insol. in KOH, or NaOH+Aq. Sol. in NH 4 salts +Aq. SI. sol. in NaC 2 H 3 O 2 +Aq. (Mercer.) Not pptd. in presence of Na citrate. Insol. in boiling cane sugar +Aq, but si. sol. when KOH has been added. Not pptd. in presence of much H 2 C 4 H 4 O 6 . (Rose.) IRON HYDROXIDES 433 Solubility in glycerine -j-Aq containing about 60% by vol. of glycerine. 100 ccm. of the solution contain 1.0 g. FeO (Muller, Z. anorg. 1905, 43. 322.) Iron (ferric) hydroxides, Fe 2 O 3 , rcH 2 O. Many indefinite compounds of Fe 2 O 3 and H 2 O are known, and uncertainty exists as to their composition. According to van Bemmelen (R. t. c. 7. 106) there are probably no true definite compounds of Fe 2 O 3 and H 2 O. According to Tommasi (B. 12. 1924, 2334), there are two series of Fe hydroxides, a, red hydroxides, and /3, yellow hydroxides. a Hydroxides. Fe 2 O 6 H 6 (unstable), Fe 2 O 3 , 2H 2 O (loses H 2 O at 50), and Fe 2 O 3 , H 2 O (loses H 2 at 92). Sol. in dil. acids and in Fe 2 Cl 6 +Aq, and pptd. from the latter solution by Na 2 SO 4 , or H 2 S0 4 +Aq. j3 Hydroxides. Fe 2 O 6 H 6 (stable below 70), Fe 2 O 3 , 2H 2 O (loses H 2 O at 105), Fe 2 O 3 , H 2 O (loses H 2 O at 150). SI. sol. in acids, and insol. in Fe 2 Cl 6 +Aq. (Tommasi.) The following more or less uncertain data are given. 2Fe 2 O 3 , H 2 O. Sol. in HCl+Aq. Very si. sol. in HNO 3 +Aq. (Davies, Chem. Soc. (2) 4. 69.) Min. Turgite. Fe 2 O 3 ,*H 2 O. Insol. in cold acids, difficultly sol. in warm HC1 and H 2 SO 4 +Aq, and especi- ally in warm HNO 3 +Aq. (Schiff, A. 114. 199.) Min. Gothite. 2Fe 2 O 3 , 3H 2 O. SI. sol. in tartaric, citric, or acetic acids, but easily sol. in HCl+Aq. (Wittstein.) Scarcely attacked by cone. HNO 3 , or HC1+ Aq. Sol. in acetic acid or dil. HNO 3 , or HC1 + Aq, from which solution it is pptd. by trace of alkali salts. (St. Gilles.) Min. L-imonite. 3Fe 2 O 3 , 5H 2 O. (Muck.) Fe 2 O 3 , 2H 2 O. Easily sol. in HCl+Aq. Min. Xanthosiderite. Fe 2 O 3 , 3H 2 O. SI. sol. in acetic acid of 1.03 sp. gr., but easily sol. if of 1.076 sp. gr. Sol. in mineral acids. (Limberger, J. B. 1863. 70.) Pptd. Fe 2 O 3 , xH 2 O=Fe 2 O 6 H 6 (?). Insol. in H 2 O, or in solutions of the alkalies or NH 4 salts. When recently pptd. is easily sol. in acids. (Fresenius.) SI. sol. in NH 4 OH, and NH 4 salts +Aq. (Odling.) Apparently insol. in NH 4 C1, or (NH 4 ) 2 CO 3 +Aq. (Brett, 1837.) SI. sol. in cone., but insol. in dil. KOH+Aq. (Chodnew, J. pr. 28. 221.) SI. sol. in very cone. KOH+Aq free from CO 2 . (Volcker, A. 69. 34.) Not at all sol. in pure cone. KOH+Aq, solubility noticed by previous observers being caused by the presence of silicic acid. (Sand- rock.) SI. sol. in cone, alkali carbonates +Aq. When freshly pptd., it is not acted upon by cone. K 2 CO 3 +Aq. (Grotthaus.) Readily sol. in cone. (NH 4 ) 2 CO 3 +Aq, but pptd. by addition of H 2 O. Sol. in excess of (NH 4 ) 2 CO 3 +Aq when pptd. by that reagent. (Wohler.) Sol. in solutions of the alkali bicarbonates. (Berzelius.) Sol. in aqueous solutions of water-glass. (Ordway.) Immediately dissolved by H 2 SO 3 +Aq. Sol. in NH 4 F+Aq. (Helmholt, Z. anorg. Sol. in cone. Al 2 (SO 4 ) 3 +Aq. (Schneider, B. 23. 1352:) SI. sol. in a solution of MgCO 3 (?). (Bis- chof). Insol. in ethylamine, or amylamine+Aq. (Wurtz, A. ch. (3) 30. 472.) Sol. in boiling solution of Bi(NO 3 ) 3 , with pptn. of Bi 2 O 3 . (Persoz.) Sol. in Cr 2 Cl 6 +Aq; after 3 months 15 mols. Fe 2 O 6 H 6 were dissolved by 1 mol. Cr 2 Cl 6 . (Bechamp, A. ch. (3) 57. 296.) Insol. in fumaric acid, even when freshly pptd. When recently pptd., it is easily sol. in KHC 4 H 4 O 6 +Aq, but after drying it is dif- ficultly sol. therein. When moist easily sol. in H 2 C 4 H 4 O 6 +Aq, but after drying is scarcely sol. therein when cold, and only si. sol. when hot. (Werther.) Easily sol. in acetic, citric, and other acids. (Wittstein.) Solubility in glycerine +Aq containing about 60% by vol. of glycerine. 100 ccm. of the solution contain 0.8 g. Fe 2 O 3 . (Muller, Z. anorg. 1905, 43. 322.) Easily sol. in aqueous solution of su crates of Ca, Ba, Sr, K, Na. (Hunton, 1837.) Unacted upon by cane sugar +Aq. (Glad- stone*) SI. sol. in cane sugar +Aq, from which it is pptd. by (NH 4 ) 2 S+Aq, but not by NH 4 OH, or K 4 FeC 6 N 6 +Aq. (Peschier.) Solubility of Fe 2 O 6 H 6 in sugar solutions. 1 1. of sugar solution of given strength dis- solves mg. of Fe2OeH 6 . Mg. Fe 2 O6H 6 % Sugar at 17.4 at 45 at 75 10 3.4 3.4 6.1 30 2.3 2.7 3.8 50 2.3 1.9 3.4 fStolle, Z. Ver. Zuckerind. 1900, 60. 340.) Not pptd. from solutions by alkalies or alkali carbonates in presence of many organic substances, as tartaric acid, sugar, etc. \ Not pptd. by NH 4 OH from solutions con- taining Na 4 P 2 O 7 . (Rose, Pogg. 76. 19.) Not pptd. by NH 4 OH in presence of Na citrate. (Spiller.) 434 IRON HYDROXIDE Soluble, (a) By dialysis. Solutions con- taining 1% can be concentrated somewhat whereupon they gelatinise. They also gela- tinise by cold, or addition of traces of H 2 SO 4 , alkalies, alkali carbonates or sulphates, or neutral salts, not, however, by HC1, HN0 3 alcohol, or sugar. (Graham, A. 121. 46.) When a dil. solution of a solid organic acid or an alkali, or salt is added to a dialysed solution of Fe 2 O 6 H 6 , a coagulum sol. in H 2 O is formed, but if the solutions are cone, the separating coagulum is no longer sol. in HoO (Athenstadt, C. C. 1871. 822.) (6) Pean St. Gilles' hydroxide, or meta-iron hydroxide. Sol. in H 2 O. Pptd. from solution by traces of H 2 SO 4 , HC1, HNO 3 +Aq, and alkalies; the ppt. is insol. in cold acids, but sol. in pure H 2 O. (Pean St. Gilles, A. ch. (3) 46. 47.) See also table by Krecke in the article on ferric chloride. Iron (Ferroferric) hydroxide, Fe 3 O 4 , H 2 O (?). Sol. in acids. Fe 3 O 4 , 4H 2 O. (Lefort.) Ferrous iodide, FeI 2 . Very deliquescent. Sol. in H 2 O. Solution decomp. on evaporating. ' 4-4H 2 O. Very deliquescent; si. sol. in H 2 O; sol. in ether. (Jackson, Am. Ch. J. 1900, 24. 19.) -f-5H 2 O. Deliquescent. Sol. in alcohol. Sol. in sugar +Aq, and solution is much -more stable than aqueous solution. Easily sol. in glycerine. Insol. in methylene iodide. (Retgers, Z. anorg. 3. 343.) +6H 2 O, and +9H 2 O. Very sol. ; pptd. from cooled aq. solution. (Volkmann, C. C. 1894, II. 611.) Ferric iodide, FeI 3 . Has not been isolated. Solution of I in FeI 2 +Aq in the molecular ratio of I : FeI 2 probably contains FeI 3 . Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Ferrous mercuric iodide, FeI 2 , 2HgI 2 +6H 2 O. As the corresponding Mg salt. (Duboin, C. R. 1907, 145. 714.) Ferrous iodide ammonia, FeI 2 , 6NH 3 . Decomp. by H 2 O. (Jackson, Am. Ch. J. 1900, 24. 27.) Ferrous mercuric iodide. Very deliquescent. Decomp. by H 2 O; sol. in HC 2 H 3 O 2 or alcohol. Iron molybdenide, FeMo 2 . Attacked by HCl+Aq with difficultly Sol. in hot cone. H 2 SO 4 . (Steinacker.) Iron nitride. Easily decomp. by H 2 O when finely pow- dered. (Rossel, C. R. 1895, 121. 942.) Fe 2 N. Easily sol. in HNO 3 , HC1, or H 2 SO 4 +Aq. Very slowly decomp. by H 2 O. (Stahl- schmidt, Pogg. 125. 37.) . Sol. in HC1 with decomp.; decomp. by steam and by H 2 S at 200. (Fowler, C. N. 1894, 68. 152.) FesNa. Probably the same as the above compound. (Rogstadius, J. pr. 86. 307.) Iron nitrososulphantimonate, Fe 4 S(NO) 6 Sb 2 S 5 . (Low, C. C. 1865. 948.) Does not exist, but was impure sodium fer- rofefranitrososulphide. (Pawel, B. 15. 2600.) Iron nitrososulphides. See Ferrofefranitrososulphydric acid and Ferro/ieptanitrososulphide, ammonium. Fe 3 S 5 H 2 (NO) 4 . (Roussin, C. R. 46. 224.) Fe 3 S 3 (NO) 4 +2H 2 O. (Porczinsky, A. 125. 302.) Fe 6 S 5 (NO) 19 +4H 2 O. (Rosenberg, B. 3. 312.) The compound to which the above formula were given was impure, according to Pawel (B. 12. 1407 and 1949; 15. 2600), and contained more or less Na or NH 4 . Pawel considers the substance as NH 4 salt of ferroAeptanitroso- sulphydric acid, which see. Fe 3 S 2 N 5 O 6 + 13^H 2 O. Sol. in H 2 O, alcohol, ether, CHC1 3 , acetone and ethyl acetate. Insol. in benzene and light petroleum. (Marie, C. R. 1896, 122. 138.) Iron sodium nitrososulphide, 3Na 2 S, Fe 2 S 3 , 2NO. (Roussin.) Na 8 Fe8S9(NO) 18 . (Rosenberg.) Correct formula is Na 2 S 2 (NO) 4 Fe 2 , sodium ferrotetfranitrososulphide. Iron nitrososulphocarbonate, Fe 4 S(NO) 6 CS 2 + 3H 2 O. (Low, C..C. 1865. 948.) Correct formula is NaS 3 (NO) 7 Fe 4 +2H 2 O, sodium ferro/ieptanitrososulphide. (Pawel, B. 15. 2600.) Ferrous oxide, FeO. Insol. in H 2 O. Sol. in acids. Easily sol. in HC1, and HNO 3 +Aq; nearly insol. in H 2 SO 4 . even when heated. (Tissan- dier, C. R. 74. 531.) Ferric oxide, Fe 2 O 3 . Attacked by acids with difficulty, the more so the higher it has been heated. HCl+Aq is the best solvent, in which it is more quickly sol. by long digestion at a gentle heat than ' boiling. (Fresenius.) Most easily sol. in 16 pts. of a mixture of 8 pts. H 2 SO 4 and 3 pts. H 2 O. (Mitscherlich, J. pr. 81. 110.) IRON OXIDE 435 Solubility of Fe 2 O 3 in HF+Aq at 25. Absolutely insol. in Br 2 +Aq. (Balard.) Insol. in hot NH 4 Cl+Aq. (Rose.) Insol. in KOH+Aq. (Chodnew, J. pr. 28. 222.) Slowly sol. in an aq. solution of calcium hydrogen carbonate. The velocity of the reaction may be much increased by the addi- tion of small amounts of alkali sulphate or CaSO 4 . (Rohland, Z. anal. 1909, 48. 629.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Solubility in (calcium sucrate+ sugar) +Aq. 1 1. solution containing 418.6 g. sugar and 34.3 g. CaO dissolves 6.26 g. Fe 2 O 3 ; 296.5 g. sugar and 24.2 g. CaO dissolves 4.71 g. Fe 2 O 3 ; 174.4 g. sugar and 14.1 g. CaO dissolves 3.08 g. Fe 2 O 3 . (Bodenbender, J. B. 1865. 600.) Solubility of Fe 2 O 3 in sugar solutions. 1 1. of sugar solution of given strength dis- solves mg. Fe 2 O 3 . Time G. Fe 2 O 3 in 10 ccm. of the solution N-HF 4^ hrs. 21fc " 45^ " 0.1581 0.2235 0.2279 0.5N-HF 2H " 8M " 23^ " 56^ " 0.0579 0.0884 0.1045 0.1162 0.25N-HF 2M " 8^ " 24% " 142^ " 0.0180 0.0345 0.0475 0.0534 equal amts. N-HF+N-HC1 2M " 8^ " 23M " 96 264 0.1011 0.1611 0.1976 0.2223 0.2297 mg. Fe 2 O 3 (Deussen, Z. anorg. 1905, 44. 414.) ' Solubility of Fe 2 O 3 in HCl+Aq at 25. at 17.5 at 45 10 1.4 30 1.4 50 0.8 2.0 i.i Time G. ~FezOs in 10 ccm. of the solution (Stolle, Z. Ver. Zuckerind, 1900, 60. 340.) Calcined. Solubility of calcined Fe 2 O 3 in acids at 25. N-HC1 4% hrs. 213^ " 45^ " 0.0409 0.1230 0.2125 0.5N-HC1 2% " 8^ " 23^ " 5Q 1 A " 0.0126 0.0188 0.0382 0.0672 Acid Time g. Fe 2 Os in 10 ccm. of the solution N-HF 4^ hrs. 43^ " 129K " 0.0889 0.2035 0.2194 0.25N-HC1 2X " &A " 24% " U2 1 A " 0.0040 0.0054 0.0120 0.0306 N-HC1 4^ " 43^ " 1393/S " 0.0224 0.1000 0.1910 equal vol. N-HCl+N-NaF 2% " m " 23% " ' 72^ " 215 0.0444 0.0640 0.0743 0.0757 0.0766 (Deussen, Z. anorg. 1905, 44. 413.) See also Ferric hydroxide. Min. Hematite. Rather easily sol. in HC1 +Aq, but not readily sol. in other acids. Metairon oxide. See Ferric hydroxides. Ferroferric oxide, 6FeO, Fe 2 O 3 . FeO, Fe 2 O 3 = Fe 3 O 4 . With insufficient HC1 +Aq for complete solution, FeO is dissolved and Fe 2 O 3 left. (Berzelius.) Insol. in HNO 3 +Aq at the ordinary tem- perature. (Millon.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) (Deussen, 1. c.) Solubility of Fe 2 O 3 in N-oxalic acid at 25. rr,- G. Fe 2 Os in 10 ccm. of ' Time the solution 1% hrs. 0.0310 6% 0.0790 22 " 0.1960 94 " 0.2326 (Deussen.) 436 IRON OXIDE ZINC OXIDE Solubility of Fe 2 O 4 in sugar solutions. 1 1. of sugar solution of given strength dissolves mg. Fe?O 4 . mg. FeaCU c/ Suear at 17.5 at 45 at 75 10 10.3 10.3 12.4 30 12.4 10.3 12.4 50 14.5 10.3 14.5 (Stolle, Z. Ver. Zuckerind. 1900, 50. 340.) Min. Magnetite. Insol. in HNO 3 , but sol. in hot HCl+Aq. Iron sesquioxide zinc oxide, Fe 2 O 3 , ZnO. See Ferrite, zinc. Ferric oxybromide. Basic ferric bromides containing three equivalents, or less, of base to one of acid may be obtained dissolved in H 2 O. (Ordway, Am. J. Sci. (2) 26. 202.) The most basic soluble compound obtained by three months' digestion of Fe 2 OeH6 with Fe 2 Br 6 +Aq, is Fe 2 Br 6 , 14Fe 2 O 3 . (Bechamp.) Ferric oxychlorides. (a) Soluble. Fe 2 O 6 H 6 dissolves in Fe ? Cl 6 + Aq. By digesting until the acid reaction of the chloride has disappeared a solution of Fe 2 Cl 6 , 2Fe 2 O 3 is obtained. (Pettenkofer, Repert. (2) 41. 289.) By digesting for several days in the cold, Fe 2 Cl 6 ,5Fe 2 O 3 is obtained, and still more basic compounds by further addition of Fe 2 O 6 H 6 . When the solution contains Fe 2 Cl 6 , 12Fe 2 O 3 it gelatinises, but still dissolves completely in H 2 O. The most basic soluble compound is Fe 2 Cl 6 , 20Fe 2 O 3 . (Bechamp, A. ch. (3) 57. 296.) If the digestion is carried on several weeks, a solution containing Fe 2 Cle, 23Fe 2 O 3 is ob- tained; this can be boiled and diluted with- out pptn., but Fe 2 O 6 H 6 is precipitated by the addition of very many salts. (Ordway, Sill. Am. J. (2) 26. 197.) Solutions containing 10 or less molecules Fe 2 O 3 to 1 mol. Fe 2 Cl 6 can be dried without the oxychloride becoming insoluble. (Ord- way.) The above solutions do not become cloudy by boiling or diluting. (Phillips.) A very dil. solution of Fe 2 Cl 6 , 10Fe 2 O 3 re- mains clear after protracted boiling, and may be boiled without decomp. even when Fe 2 Cl 6 , 20Fe 2 O 3 is present. (Be" champ.) HNO 3 , and HCl+Aq form precipitates in the above solutions, which are sol. on addition of more H 2 O. H 2 SO 4 +Aq forms a precipi- tate insol. in H 2 O. (Be"champ.) Fe 2 Cl 6 , 9Fe 2 O 3 is easily sol. in H 2 O, weak alcohol, and glycerine; but solutions are pptd. by small amts. of H 2 SO 4 , M 2 SO 4 , citric or tartaric acids, or a few drops of HC1, or HNOa+Aq. (Jeannel, C. R. 46. 799.) Solutions containing 5 mpls. Fe 2 O 3 to 1 mol. Fe 2 Cl 6 are completely precipitated by K 2 SO 4 , Na 2 S0 4 , MgS0 4 , KN0 3 , NaNO 3 , Zn(NO 3 ) 2 , KC1, NaCl, NH 4 C1, CaCl 2 , MgCl 2 , ZnCl 2 , KBr, or KSCN. (Bechamp.) Ba(NO 3 ) 2 does not precipitate solutions of less than 18-20 Fe 2 O 3 to 1 Fe 2 Cl 6 . Pb(NO 3 ) 2 or Pb(C 2 H 3 O 2 ) 2 do not precipi- tate solutions containing the compound Fe 2 Cle, 12Fe 2 O 3 , but a mixture of the two salts causes complete precipitation. Solution has-been obtained containing 116 Fe 2 O 3 to 1 FeCl 6 , probably owing to a forma- tion of soluble colloidal Fe 2 O 3 . (Magnier de la Source, C. R. 90. 1352.) Solubility determinations in the system Fe 2 O 3 , HC1 and H 2 O, show that at 25 no definite basic chloride is formed, but that the stable solid phase is one of a series of solid solutions containing Fe 2 O 3 , HC1 and H 2 O. (Cameron, J. phys. Chem. 1907, 11. 694.) (/3) Insoluble. Fe 2 Cl 6 , 6Fe 2 O 3 +9H 2 O. (1) By exposing FeCl 2 +Aq to air. Insol. in H 2 O ; si. sol. in HCl+Aq. (Wittstein.) (2) From FeCl 2 +Aq and HNO 3 . Insol. in H 2 O, and si. sol. in HCl+Aq. (Bechamp.) 2Fe 2 Cl 6 , 25Fe 2 O 3 +41H 2 O. Insol. in H 2 O. (Bechamp.) Fe 2 Cl 6 , 2Fe 2 O 3 +3H 2 O. Decomp. by H 2 O with residue of Fe 2 O 3 ; si. sol. in dil. acids. (Rousseau, C. R. 110. 1032.) Fe 2 Cl 6 , 3Fe 2 O 3 . As above. (Rousseau, C. R. 113. 542.) Ferric oxyfluoride, 3Fe 2 O 3 , 2FeF 3 +4H 2 O. Ppt. (Scheurer-Kestner.) Ferric oxy sulphide, Fe 2 O 3 , 3Fe 2 S 3 . (Rammelsberg.) Iron phosphide, FeP. Very slowly (Freese), not (Hvoslef, A. 100. 99) sol. in hot HCl+Aq. Still more insol. in dil. H 2 SO 4 +Aq. (Freese.) Slowly sol. in HNO 3 +Aq, and easily sol. in aqua regia. (Struve.) Insol. in ammonum citrate +Aq; si. sol. in HC1. (Dennis, J. Am. Chem. Soc. 1894, 16. 483.) Fe 2 P. Slowly but completely sol. in HC1, or dil. H 2 SO 4 +Aq. Sol. in hot cone. H 2 SO 4 , in HNO 3 , and in aqua regia. (Freese, Pogg. 132. 225.) Insol. in all acids except in a mixture of HNO 3 and HF. (Maronneau, C. R. 1900, 130. 657.) Fe 3 P 4 . Very slowly sol. in hot cone. HC1 + Aq. 0.1 g. dissolves by 4 days' heating with HCl+Aq; 0.3 g. dissolves in hot cone. H 2 SO 4 inl l /2 hours; 0.4 g. in 2 hours in HNO 3 +Aq. Quite easily sol. in aqua regia on warming. (Freese.) Fe 2 P 3 . Insol. in HC1, HNO 3 and aqua regia. Sol. in potassium hypobromite solu- IRON SULPHIDE 437 tion. (Granger, Bull. Soc. 1896, (3) 15. 1086.) Fe4P 3 . Very slowly sol. in boiling HCl-f- Aq. Easily sol. in HNO 3 or aqua regia. (Struve, J. B. 1860. 77.) Mixture. (Freese, Pogg. 132. 225.) Almost insol. in aqua regia. Sol. in fused alkali. (Granger.) Fe 3 P. Nearly insol. in dil. acids; rapidly sol. in HNO 3 or aqua regia; decomp. by cone. HC1, or KOH+Aq. (Schneider, J. B. 1886. 2026.) Of the nine iron phosphides described the constitution has been established for only two, Fe 3 P and Fe 2 P. Fe 3 P. Sol. in cone. HC1. Fe 2 P. Sol. in hot aqua regia. Insol. in other acids. (Le Chatelier, C. R. 1909, 149. 709.) Iron selenide, Fe 2 Se. Not attacked by HNO 3 or acetic acid. SI. attacked by cone. HC1. Readily attacked by aqua regia. Sol. in HF. (Vigouroux, C, R. 1905, 141. 829.) FeSe+zH 2 O. Sol. in HC1, HNO 3 , or HC 2 H 3 O 2 +Aq. Insol. in alkalies, or (NH 4 ) 2 S +Aq. (Reeb, J. Pharm. (4) 9. 173.) Fe 2 Se 3 . Sol. in dil. HC1, or HNO 8 +Aq with evolution of H 2 Se. Sol. in cone. HNO 3 +Aq. (Little, A. 112. 211.) Fe 3 Se4. Decomp. by fuming HNO 3 . (Fonzes-Diacon, C. R. 1900, 130. 1711). FerSeg. Decomp. by fuming HNO 3 . (Fonzes-Diacon, C. R. 1900, 130. 1711.) FeSe 2 . Insol. in cone. HC1; decomp. by fuming HNO 3 . (Fonzes-Diacon, C. R. 1900, 130. 1711.) Iron silicide, Fe 4 Si. Difficultly sol. in HCl+Aq; easily sol. even in dil. HF+Aq. (Hahn, A. 129. 57.) Fe 2 Si. Not easily sol. in cone. HC1 and HNO 3 but readily sol. in HF. (Moissan, C. R. 1895, 121. 623.) FeioSi 9 . Sol. in hot HCl+Aq only when most finely powdered. (Hahn.) FeSi 2 . Not attacked by cone. HF or H 2 SO 4 . (Hahn.) Sol. in cold HF. (de Chalmot, Am. Ch. J. 1897, 19. 123.) Existence questioned by Jouve, (Bull. Soc. 1901, 25. 290-293). Fe 3 Si 2 . Sol. in HF and in fused KNO 3 and KNaCO 3 . (de Chalmot, J. Am. Chem. Soc. 1895, 17. 924.) Iron seraisulphide, Fe 2 S. Sol. in dil. acids with decomposition. (Arf- vedson, Pogg. 1. 72.) Ferrous sulphide, FeS. Decomp. by dil. acids, with evolution of H 2 S and without separation of S, except with HNO 3 +Aq. +zH 2 O. SI. sol. in H 2 O, especially if hot. (Berzelius.) 1 1. H 2 O dissolves 70.1 x 1Q- 6 moles FeS at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Very violently decomp., even by dil. acids. Sol. in H 2 S0 3 +Aq. Insol. in H 9 S, or (NH 4 ) 2 S +Aq. SI. sol. in Na 2 S, or K 2 S+Aq. Sol. in Na 2 S or K 2 S +Aq. (de Koninck, Z. angew. Ch. 1891. 204.) Insol. in NH 4 NO 3 , or NH 4 Cl+Aq. (Brett.) Not completely pptd. in presence of Na cit- rate. (Spiller.) Contrary to assertion of Persoz, it can be nearly completely pptd. in presence of Na 4 P 2 O 7 by (NH 4 ) 2 S+Aq. (Rose, Pogg. 76. 18.) Sol. in alkali sulpho-molybdates, -tung- states, -vanadates, -arsenates, -antimonates, and -stannates. (Storch, B. 16. 2015.) Sol. in KCN+Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Solubility of FeS in sugar solutions. 1 1. sugar of given strength dissolves mg. FeS. mg. FeS 7 Sugar at 17.5 at 45 at 75 10 3.8 3.8 5.3 30 7.1 9.1 7.2 50 9.9 19.8 9.1 (Stolle, Z. Ver. Zuckerind. 1900, 50. 300.) Colloidal. A very dilute solution has been obtained which coagulated very readily. (Winssinger, Bull. Soc. (2) 49. 452.) Ferric sulphide, Fe 2 S 3 . Decomp. by dil. HC1, or H 2 SO 4 +Aq with evolution of H 2 S, leaving a residue of FeS 2 . + 13/H 2 O. 89!. in NH 4 OH+Aq, also in alcoholic ammonia. SI. sol. in (NH 4 ) 2 S+very dil. Na 2 S 2 O 3 +Aq. (Phipson, C. N. 30. 139.) Iron bisulphide, FeS 2 . Insol. in dil. HC1, or H 2 SO 3 + Aq. Decomp. by HNO 3 or aqua regia with separation of S. Insol. in a 10% solution of alkali sulphide. Min. Pyrite, Marcasile. Sol. in a mixture of Na 2 S and NaOH+Aq, Na 2 S+Aq, or mix- ture of Na 2 S and NaSH+Aq; insol. in cold NaSH+Aq. Marcasite is more easily sol. in above than pyrite. (Becker, Sill. Am. J. (3) 33. 199.) Ferroferric sulphide, Fe 8 S 9 or Fe 7 S 8 . Min. Pyrrhotile. Sol. in dil. acids with a residue of S. Extremely slowly sol. in a 10% solution of alkali sulphides. (Terreil, C. R. 69. 1360). 438 IRON NICKEL SULPHIDE lion (ferrous) nickel sulphide, 2FeS, NiS. Min. Pentlandite. Ferrous phosphorus sulphide, FeS, P 2 S. (Berzelius.) 2FeS, P 2 S 3 . Slowly decomp. by H 2 O. In- sol. in boiling HCl+Aq; decomp. by aqua regia. (Berzelius, A. 46. 256.) Iron potassium sulphide (potassium sulpho- ferrite), K 2 Fe 2 mae (po 4 = K 2 S, ] Fe 2 S 3 . Insol. in cold or hot H 2 O. Violently at- tacked by dil. acids. Not decomp. by boiling with alkalies, alkali carbonates, or sulphides + Aq. Decomp. by KCN, or Na 2 S 2 O 3 +Aq. (Preis, J. pr. 107. 16.) K 2 S, 2FeS. (Schneider, Pogg. 136. 460.) Iron silver sulphide (silver sulphoferrite), Ag 2 S, Fe 2 S 3 . Not attacked by dil. HCl+Aq; decomp. by cone. HCl+Aq. (Schneider.) 2Ag 2 S, FeS,. (Schneider, Pogg. 138. 305.) Ag 2 S, 3FeS, FeS 2 . Min. Sternbergite. De- comp. by aqua regia. Iron sodium sulphide (sodium sulphoferrite), Na 2 Fe 2 S 4 +4H 2 O. Insol. in H->O. Decomp. by very dil. acids. (Schneider, Pogg. 138. 302.) Iron sulphophosphide, Fe 2 PS 3 . Attacked by acids at 100. Decomp. by boiling NaOH+Aq. (Ferrand, A. ch. 1899, (7) 17. 410.) Ferrous telluride, FeTe. Insol. in H 2 O; sol. in acids. (Fabre, C. R.' 105. 277.) Kermes. See Antimony Znsulphide. " Knallplatin " compounds. See Fulminoplatinum compounds. Krypton, Kr. Absorption by H 2 O at t. t Coefficient of absorption det. by two series of experiments 10 20 30 40 50 0.1249 0.0965 0.0788 0.0762 0.0740 0.0823 0.1166 0.0877 0.0670 0.0597 0.0561 0.0610 (Antropoff, Roy. Soc. Proc. 1910, 83. A. 480.) Lanthanic acid. Barium wetolanthanate, Ba(H 9 La 5 Oi5) 2 . (Baskerville, J. Am. Chem. Soc. 1904, 26. 79.) Lithium metalanthanate, LiH 9 La 5 Oi5+2H 2 O. (Baskerville.) Potassium wetalanthanate, KH 9 La5O 15 + 15H 2 O. Decomp. by H 2 O. (Baskerville.) Sodium metalanthanate, NaH 9 La 5 Oi 5 + 4H 2 O. Almost insol. in H 2 O, but decomp. by it. (Baskerville.) Dtsodium te^ralanthanate*, Na 2 La 4 O 7 . Insol. in H 2 O. (Baskerville.) Lanthanicotungstic acid. Ammonium lanthanicotungstate, 2(NH 4 ) 2 O, La 2 O 3 , 16WO 3 + 16H 2 O. Ppt. Insol. in H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1904, 26. 1481.) Barium lanthanicotungstate, 5BaO, La 2 O 3 , 16WO 3 +16H 2 O. Ppt. (E. F. Smith.) Silver lanthanicotungstate, 5Ag 2 O, La 2 O 3) 16WO 3 +4H 2 O. Very insol. in H 2 O. (E. F. Smith.) Lanthanum, La. Slowly dtecomp. cold, rapidly hot H 2 O. Not attacked by cold cone. H 2 SO 4 , but energet- ically by cold cone. HNO 3 +Aq. Sol. in dil. acids. (Hillebrand and Nortdn, Pogg. 166. 633.) Lanthanum bromide, LaBr 3 +7H 2 O. Easily sol. in H 2 O. Not very sol. in ab- solute alcohol. Insol. in ether. (Cleve. Sv. V. A. H. Bih. 2. No. 7.) Lanthanum nickel bromide, 2LaBr 3 , 3NiBr 2 + 18H 2 0. Deliquescent. (Frerichs and Smith, A. 191 Jeliqu .355. Lanthanum zinc bromide, 2LaBr 3 , 3ZnBr 2 + 36H 2 0. Very deliquescent. (F. and S.) Lanthanum carbide, LaC 2 . I Decomp. by H 2 O and dil. acids. (Petters- son, B. 1895, 28. 2422.) Sol. in cone. H 2 SO 4 and dil. acids; insol. in cone. HNO 3 . LEAD 439 Sol. in fused oxidizing agents; decomp. , H 2 O at ordinary temps. (Moissan, C. R 1896, 123. 149.) Lanthanum chloride, LaCl 3 . Anhydrous. Deliquescent. (Hermann.) Insol. in acetone. (Naumann, B. 1904, 37 329.) +73^H 2 O. Not deliquescent. (Zschiesche.^ Easily sol. in alcohol. (Hermann.) Lanthanum mercuric chloride, 2LaCl 3 , HgCl + 8 / 3 H 2 O. Not deliquescent. Very sol. in H 2 O (Marignac, Ann. Min. (5) 15. 272.) Lanthanum stannic chloride. See Chlorostannate, lanthanum. Lanthanum fluoride, LaFH H 2 O. Precipitate. SI. sol. in HCl+Aq. (Cleve.) Lanthanum hydrogen fluoride, 2LaF 3 , 3HF. Precipitate. (Frerichs and Smith, A. 191 355.) Does not exist. (Cleve, B. 11. 910.) Lanthanum hydride, La 2 H 3 . Decomp. by dil. acids. (Dinkier, B. 24. 1966.) LaH 3 . Decomp. by H 2 O. Sol. in acids with evolution of H 2 . Decomp. by alkalis. (Muthmann, A. 1902, 325. 266.) Lanthanum hydroxide, La 2 O 6 H 6 . Insol. in H 2 O; easily sol. in acids; insol. in KOH, or NaOH+Aq. Sol. in citric acid. (Baskerville, J. Am. Chem. Soc: 1904, 26. 49.) Lanthanum zinc iodide, 2LaI 3 , 3ZnI 2 +27H 2 O. Very sol. in H 2 O. (Frerichs and Smith, A. 191. 358.) Lanthanum nitride, LaN. Decomp. by H 2 O with evolution of NH 3 . Sol. in mineral acids. Decomp. by alkali. (Muthmann, A. 1902, 325. 275.) Lanthanum oxide, La 2 O 3 . Easily sol., even when ignited, in mineral, and acetic acids. (Hermann.) Sol. in boiling cone. NH 4 Cl+Aq. (Mos- ander.) Sol. in cold cone. NH 4 NO 3 +Aq. (Damour and Deville.) Insol. in (NH 4 ) 2 CO 3 +Aq. (Mosander.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Lanthanum peroxide, La 4 O . Sol. in HC1, H 2 SO 4 , HNO 3 , and HC 2 H 8 O 2 + Aq with decomp. (Cleve, Bull. Soc. (2) 43. 359.) La 2 O 5 +zH 2 O. Unstable. Sol. in dil. H 2 SO 4 +Aq with decomp. (Melikoff, Z. anorg. 1899, 21. 71.) Lanthanum oxybromide, LaOBr. Ppt. (Frerichs and Smith.) Lanthanum oxychloride, 3La 2 O 3 , 2LaCl 3 . Insol. in H 2 O. Difficultly and slowly sol. in HC1, or HNO 3 +Aq. (Hermann.) LaOCl. Boiling H 2 O dissolves only traces. (Frerichs and Smith.) Lanthanum sulphide, La 2 S 3 . Decomp. by H 2 O and acids. (Didier.) Lanthanum ^sulphide, LaS 2 . Decomp. 'by heat. (Biltz, Z. anorg. 1911. 71. 435.) Lead, Pb. Lead, in contact with fhO and air free from CCh, gives a solution of PbO which turns litmus blue and turmeric red, and is turned brown with EhS. H2p which has been boiled does not dissolve Pb if there is no access of air. When shaken up with air it dissolves 0.01 to 0.008% PbO in 2 hours. Pure spring water, containing 1% grains salts in 2 pounds II2O and no CO2, when conducted though a lead pipe 150 feet long, dissolves so much lead that it turns brown with H 2 S. (Yorke, Phil. Mag. J. 5. 82.) CO2 or small amts. of salts prevent the solution of Pb. 1 vol. HzO with % vol. CC>2 dissolves only a trace of Pb. Spring PhO, containing in 10 pounds 1.21 grains NaCl and CaCb, and 6.4 grains CaCOs dissolved in CO2, does not dissolve lead. (Yorke.) If the amt. of salts in solution equals g^ the amt. of EhO, and especially if they are carbonates, very slight amts. of Pb are dissolved. (Christison, Phil. Mag. J. 21. 158.) CaCOs dissolved in CO2 water decreases the solu- bility of Pb more than any other salt. Distilled EbO, quietly standing in a closed flask with lead and air free from COz, deposits white flocks of PbO 2 H 2 , and dissolves 7 j,Jjj ff pt. PbO. The solution has an alkaline reaction, (v. Bonsdorff , Pogg, 41. 305.) Water of 3 hardness does not take up enough Pb to become injurious. (Clarke, J. B. 1856. 608.) Soluble carbonates increase the solubility of Pb in H 2 O (Nevins, C. C. 1851. 608); especially (NH^COs. (Bottger.) Presence of H 2 SO 4 decreases the solubility of Pb. (Horsford, Chem. Gaz. 1849. 247.) H2O containing K2SOi takes up only a trace of Pb. (Wetzlar, Schw. J. 54. 324.) Presence of sulphates diminishes (Christison), does not diminish (Graham, Miller, and Hoffmann), the action of H 2 O on Pb. CaSO4 protects Pb, but it is attacked by much MgSO4. (Nevins.) NaCl +Aq dissolves only a trace of Pb. aflW pt- of a chloride in H2O is not sufficient to pre- vent the solubility 9f Pb in H 2 O. (Christison.) Presence of chlorides increases the solubility. (Gra- ham, Miller, and Hoffmann; Nevins.) H2O containing KNOs does not corrode Pb. Nitrates hinder the action of H2O. (v. Bonsdorff.) Nitrates increase the action of H2O. (Graham, Miller, and Hoffman.) Nitrates have no influence. (Kersting.) 10 Ibs. of H 2 O dissolved the following amts. 'rom Pb pipes in 24 hours: if distilled H 2 O-f- 1% Na 2 C0 3 , 0.38 grain Pb; if Duna water, 0.19 grain Pb; if canal water, 0.15 grain Pb; if distilled H 2 O + 1% NH 4 NO 3 , 0.15 grain Pb: if hard well water, 0.04 grain Pb; if distilled H 2 O+1% KNO 3 , 0.01 grain Pb. (Kersting, Dingl. 169. 183.) 200 1. Manchester drinking water dissolved 2.094 g. from 1 sq. metre Pb in 8 weeks; 9 1. well water dissolved 1.477 g. from 1 sq. metre D b in 8 weeks; 11 1. distilled H 2 O containing 440 LEAD are dissolved 110.003 g. from 1 sq. metre Pb in 8 weeks; distilled H 2 O free from air dis- solved 1.829 g. from 1 sq. metre Pb in 8 weeks; sea water dissolved 0.038 g. from 1 sq. metre Pb in 8 weeks. (Calvert and Johnson, C. N. 16. 171.) A lead pipe taken up in Paris, which had been exposed to action of ordinary H 2 O for 200 years, was found perfectly smooth and uncorroded. (Belgrand, C. R. 77. 1055.) Pb is attacked by all waters, hard or soft; even highly calcareous water dissolves some lead. (Mayengon and Bergeret, C. R. 78. 484.) Pure distilled H 2 O does not act T>n Pb, but extremely small quantities of NH 3 , HNO 3 , etc. cause an action; but for this action on Pb the presence of air and CO 2 is also required. (Stallman, Dingl. 180. 366.) 100 ccm. distilled H 2 O dissolved 3 mg. from 11.8 sq. cm. lead in one week when air with- out CO 2 was passed through the solution. 8 mg. were dissolved when the air contained CO 2 . (Wagner, Dingl. 221. 260.) Action of dil. salt solutions on lead. In 500 ccm. of the solutions containing salt, bright sheets of lead of 5600 sq. metres' surface were so suspended that the liquid reached all parts of the metal without hindrance, and the amts. dissolved determined after 24, 48, and 72 hours of action. Salt g. salt in 100 ccm. mg. Pb dissolved without CCh with CO 2 KC1 0.5 21 12 NaCl 0.5 21 12 NH 4 C1 1.0 12 5 MgCl 2 0.83 20 35 K 2 S0 4 1.0 KNO 3 1.0 14 20 Na 2 CO 3 1.0 NaOH 0.923 430 CaO 2 H 2 Saturated 137 Salt Grammes salt per litre Dissolved Pb in mg. per litre after 24 48 72 hrs. NH 4 NO 3 0.020 13.0 25 a 0.040 15.0 32 u 0.080 15.0 KN0 3 + 0.020 NaN0 3 0.050 2.0 2.0 KN0 3 + 0.040 Na 2 S0 4 0.212 0.8 1.0 KNO 3 + 0.045 K 2 CO 3 0.308 0.3 > KNO 3 + 0.070 K 2 S0 4 0.504 0.5 CaSO 4 0.252 '6'.4 0.8 0.408 0.4 i!6 K 2 C0 3 0.310 .... . 6'.2 0.516 .... _ 0.2 CaCl 2 0.250 '6'.5 6!s 0.5 0.510 0.3 0.4 Na 2 SO 4 0.200 0.8 it 0.400 0.5 f NH 4 N0 3 + 0.020 CaCl 2 060 1.8 NH 4 NO 3 + 0.020 K 2 C0 8 + 0.100 0.4 Na 2 SO 4 0.200 'Na 2 S0 4 + 0.200 K 2 CO 3 + 040 0.1 CaCl 2 0.100 Vater from L. Katrine 1.0 1.0 1.5 distilled water . 2.0" 2.0 3.0 (Muir, C. N. 26. 294.) Action of salt solutions on 11.8 sq. cm. Pb in one week while air either with or without O 2 was passed through the solution. Solubility of Pb in salt solutions. 100 ccm. solutions containing the given amts. salts dissolve Pb in mg. : (Wagner, Dingl. 221. 260.) Solubility of Pb in salt solutions. 25 sq. cm. were acted upon by a solution containing 0.2 g. salt in a litre for 21 days. Three series of experiments were carried on. I. In corked flasks. II. In beakers covered with porous paper; diameter of mouth of beaker = 11.5 cm. III. In basins covered with porous paper; diameter of mouth of basin = 14.5 cm. IV. In corked flasks with constant current of air. V. In beakers half filled and covered with porous paper, the lead being suspended so that equal amts. of surface were above and beneath the liquid. The amts. in mgs. of Pb dissolved were as follows : Salt used I- n. ill. IV. 1.5 3.5 5.0 0.6 2.0 v. 3^5 2.5 0.3 NH 4 NO 3 KN0 3 . CaCl 2 . (NH 4 ) 2 S0 4 . K 2 CO 3 . Dist. H 2 O 1.8 1.6 3.0 0.7 0.3 1.5 4.0 0.5 2.8 1.3 0.3 0.8 16.0 6.0 5.5 16.0 0.7 4.2 (Muir, Chem. Soc. 36. 660.) H 2 O sat. with CO 2 dissolves 0.012 g. Pb to a litre in 3 days. (Marais, C. R. 77. 1529.) Action of H 2 charged with CO 2 under 760 mm. pressure on Pb. 3 mg. of Pb were dis- solved per litre in 24 hours, and the amt. was not increased by further action. The addition of 100 mg. K 2 CO 3 +20 mg. NH 4 NO 3 to a litre prevented all action. Action of H 2 O charged with CO 2 under 6 atmos. pressure on Pb. 14.8 mg. were dissolved per 1. in 24 hours, and 24 mg. per 1. in 48 hours. Action of various salt solutions added to above solution of CO 2 were as follows: LEAD 441 mg. salt per 1. mg. Pb dissolved niter 24 hrs. after 48 hrs. K 2 C0 3 . . . K 2 C0 3 . . . CaCl 2 . . . NH 4 NO 8 . . NH 4 NO 3 . . Distilled H 2 . 80 160 160 16 40 13.2 32^6 5.0 10.0 14.8 32.0 6.0 44.0 35.Q 24.0 (Muir, C. N. 33. 125.) The corrosion of Pb by ordinary distilled H 2 O depends upon the presence of CO 2 and O. If the dissolved CO 2 is double the amt. of the dissolved O, the action is most energetic. When CO 2 is wholly absent and O present, the action is very slight, and when the H 2 O contains 1% or more vol. % CO 2 with normal amt. of oxygen, there is no visible corrosion. Pure distilled H 2 O containing neither O nor CO 2 has no action on Pb. In the above cases the greater part of the Pb remains in the form of a white ppt. or crust on the Pb, but in the case where O and C0 2 are both present in the ratio of 1 : 2, very small amts. of Pb go into solution in a few days; the amt., how- ever, diminishes on standing. As the amt. of CO 2 increases, the amt. of Pb dissolved in the H 2 O also increases. NH 4 OH alone does not protect Pb from corrosion, but when in combination with CO 2 the action is much diminished. CaO 2 H 2 , and NaOH+Aq attack Pb much more actively in absence of CO 2 and presence of air. In absence of dissolved O neither CaO 2 H 2 nor NaOH attacks Pb. Na 2 CO 3 +Aq in absence of CO 2 attacks Pb slightly, but NaHCO 3 +Aq has not the slight- est action. CaH 2 (CO 3 ) 2 +Aq also has not the slightest action on Pb, and the presence of CaCO 3 and CO 2 wholly prevents H 2 O attacking Pb. CaSO 4 +Aq in presence of air forms a crust on Pb, but no Pb is found in solution, but if air is excluded there is no visible action. Pres- ence of CO 2 causes a strong corrosive action. H 2 O containing CaSO 4 and CaH 2 (CO 3 ) 2 does not attack Pb. The above reactions are not in the least altered by the presence of moderate amts. of nitrates, chlorides, or ammonium, or organic compounds; but ammonium salts in excess have a strong solvent action on Pb. (Muller, J. pr. (2) 36. 317.) See also an extended report of the action of H 2 O on Pb made to the Water Committee of Huddersfield, England, in 1886, by Messrs. Crookes, Odling, and Tidy. Very extended researches are published by Cornelley and Frew (Jour. Soc. Chem. Ind. 7. 15), of which only the general conclusions can be given here. The action of slaked lime, limestone, sand calcium silicate, mortar, etc., was tested. The results were as follows: 1 . In nearly all cases the corrosion is greater with free exposure to the air than when air is excluded. The difference is especially great in those cases where the greatest action on the lead takes place. Aluminum hydroxide and blue clay form exceptions, and exert a greater corrosive action when air is excluded. In the case of CaCO 3 , old mortar, CaSiO 3 , or a mix- ture of CaCO 3 and CaO 2 H 2 , the exclusion or presence of air makes no appreciable differ- ence. KNO 3 + Aq shows a peculiar behaviour. In the presence of air it acts nearly as much on the Pb as pure H 2 O, but when air is excluded it exerts nearly as much retarding action as CaSi0 3 . 2. In the presence of air the action of H 2 O on Pb is considerably increased by the pres- ence of NH 4 NO 3 or CaO 2 H 4 ; with exclusion of air, by CaSO 4 , also by a mixture of CaO 2 H 2 and sand. All the other investigated sub- stances, even KNO 3 , hinder the action of H 2 O on Pb either with or without exclusion of air. 3. CaO 2 H 2 -j-Aq exerts in all cases a much greater corrosive action than pure H 2 O, and although this action is diminished by sand yet fresh mortar very quickly destroys lead pipes when in contact therewith. Old mortar, on the other hand, and also CaSiO 3 and CaCO 3 , have a protective action. 4. The fact is very important that sand, CaCO 3 , old mortar, CaSiO 3 , and a mixture of sand and CaCO 3 afford considerable protec- tion to lead against H 2 O. A mixture of lime- stone and sandstone has more effect than the two substances separately. 5. CaSiO 3 totally prevents the corrosive action of KNO 3 and NH 4 NO 3 , so that the lead is not attacked by solutions of those salts any more than by H 2 O containing CaSiO 3 alone. Sand, and a mixture of sand and CaC0 3 have a similar effect, but not to such a degree. 6. The protective influence of CaCO 3 does not appear to depend on the presence of CO 2 and the formation of CaH 2 (COs) 2 . 7. MgCO 3 prevents the corrosion of Pb as much as CaSiO 3 . (Carnelley and Frew, Jour. Soc. Chem. Ind. 7. 15.) Pb in contact with Zn or Fe is protected thereby from the solvent action of H 2 O, and in fact the action is nearly null. Sn, on the other hand, increases the action. This is of importance in regard to the use of tin-coated lead pipes. The presence of Ca salts does not influence the action of the H 2 O on Pb, hard or soft H 2 O provided it contains CO 2 having a strong corrosive action. Removal of air from H 2 O diminishes the solvent action. Simple nitra- tion will remove all Pb from H 2 O if suit- able filters are used. (Flogel, J. B. 1888. 2645.) 442 LEAD Pure distilled H 2 O has strong corrosive action on Pb, which is very much weakened by addition of a solution of CaCO 3 in carbonic acid water, but the presence of sulphates in- crease the action. Pb is not appreciably at- tacked by H2O in presence of chlorides alone, but very strongly when CaSO 4 is also present. H 2 O containing CO 2 also corrodes Pb. The conclusion was drawn that the absence of ac- tion of H 2 O on Pb in lead pipes is due to the presence of traces of CaH 2 (CO 3 ) 2 . (Barbaglia and Gucci, C. C. 1888. 934.) Solubility in H 2 O containing various solids in solution. Water used 1 2 3 4 Water alone, unfiltered 8.19 12.98 8.19 4.09 Water alone, filtered 3.00 4.09 2.07 2.32 Water containing . 049 g. NaCl per 1., unfiltered 1.36 2.73 0.68 4.04 " " filtered 0.68 1.50 0.67 1.36 Water containing 0.49 g. Na 2 SO 4 per 1., unfiltered 3.41 6.83 2.05 1.84 " " filtered 2.05 3.41 1.64 1.77 CaHCO 3 +Aq containing 0.04 g. CaO as carbonate per 1. CaHCO 3 +Aq with NaCl 2.45 2.05 3.14 3.41 2.63 2.35 5.70 3.40 CaHCO 3 +Aq with Na 2 SO 4 2.18 3.32 2.05 3.16 CaSO 4 +Aq containing 0.095 g. CaO as sulphate per 1. CaS0 4 +Aq with NaCl 6.83 5.46 6.83 6.57 3.41 3.51 1.35 1.50 CaSO 4 +Aq with Na 2 S0 4 4.78 5.87 3.69 1.77 Pts. of lead per 100,000 Column 1 gives the numbers for distilled water free from air; column 2 for distilled water aerated by agitation with air; column 3 for water continuously aerated by passing 1 litre of air through it per hour; column 4 for distilled water through which 1 litre of air and 400 cc. of CO 2 were passed per hour throughout the experiment. (Antony and Benelli, Gazz. ch. it. 1896, 26, (2) 97 and 352.) Almost insol. in cold HCl+Aq, and only si. attacked when boiling. Completely sol. in HNO 3 +Aq if not too cone., but presence of H 2 SO 4 or HC1 diminishes the solvent power to a great extent. (Rose.) Granulated Pb is si. sol. in cone. HCl+Aq; addition of PtCl 4 makes the action very ener- getic. Dil. HCl+Aq may also be used with PtCl 4 . (Millon, C. R. 21. 49.) HCl+Aq of 1.2 sp. gr., with Pb, gives off H at ord. temp., more abundantly when Jieated. Evolution of H is hastened by plac- ing Cu in contact with the Pb. (Stolba, J. pr. 94. 113.) Quickly decomp. by hot HCl+Aq, slowly by cold. (Sharpies, C. N. 60. 126.) Scarcely acted upon by boiling cone. HC1+ Aq. Sol. in aqua regia. HNO 3 +Aq is the best solvent, but Pb is as good as insol. in a mixture of HNO 3 and H 2 SO 4 . (Berzelius.) Not acted upon by very cone. HNO 3 +Aq. Pb is only si. attacked by HNO 3 +Aq of any strength below 15. Above 15 it is most rapidly attacked by a rather weak acid. (Montemartini, Gazz. ch. it. 22. 397.) Action of H 2 SO 4 on Pb. H 2 SO 4 of 1.842 sp. gr. dissolves 201 g. from 1 sq. metre pure lead at ordinary temp, (time?),' and H 2 SO 4 of 1.705 sp. gr. dissolves only 59 g. Slight impurities in the lead lessen this solubility. (Calvert and Johnson, Chem. Soc. (2) 1. 66.) Strongly attacked by 99.8% H 2 SO 4 at ord. temp, with exclusion of air. (Lunge, Dingl. 261. 131.) When 0.2 g. pure Pb was heated with 50 ccm. H 2 SO 4 of 66 B. there was no appreciable action below 175. At 230-250 all the Pb was suddenly converted into PbSO 4 , which dissolved. (Bauer, B. 8. 210.) Lead is slowly attacked by pure cold cone. H 2 SO 4 +Aq (99.78% H 2 SO 4 ). Lead vessels which held the H 2 SO 4 were gradually de- stroyed by long standing. (Napier and Tat- lock, C. N. 42. 314.) H 2 SO 4 +Aq (20%) does not evolve H under the same circumstances. (Stolba.) Sol. in HC 2 H 3 O 2 +Aq when in contact with the air. Strong NH 4 OH+Aq does not dissolve litharge; but lead immersed in NH 4 OH+Aq 3 days gives an ammonia solution containing 0.0139% lead. (Endemann, Am. Ch. J. 1897, 19. 892.) Somewhat sol. in NaCl+Aq. (Reichelt, Dingl. 172. 155.) NaCl+Aq attacks Pb at high temp. (Lunge, I c.) Action of KC1O 3 . KClO 3 +Aq (6.3% KC1O 3 ) oxidised 64.31 g. Pb from 1 sq. metre surface by boiling 7 hours; KClO 3 +Aq (25% KC1O 3 ) oxidised 151.12 g. under same condi- tions; and Ca(ClO 3 ) 2 , CaCl 2 +Aq (20 Baume) LEAD BROMIDE 443 tions; and Ca(ClO 3 ) 2 , CaCl 2 +Aq (20 Baume), obtained by passing C1 2 through CaO 2 H 2 -f-Aq, oxidised 437.70 g. (Lunge and Deggeler, Jour. Soc. Chem. Ind. 4. 31.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Sol. in a solution of K in liquid NH 3 . (Kraus, J. Am. Chem. Soc. 1907, 29. 1562.) YH 2 O. (Gottig, B. 20. 2912.) Lithium imide, Li 2 NH. Decomp. at high temp. Insol. in toluene, benzene, ether and ethyl acetate. Decomp. CIIC1 3 . (Ruff, B. 1911, 44. 506.) Lithium iodide, Lil. Deliquescent. Solubility in 100 pts. H 2 O at: 19 40 59 75 80 99 120 151 164 179 200 263 435 476 588 pts. Lil. Sp. gr. of Lil+Aq at 19.5 containing: 5 10 15 20 25 30% Lil, 1.038 1.079 1.124 1.172 1.224 1.280 35 40 45 50 55 60% Lil. 1.344 1.414 1.489 1.575 1.670 1.777 (Kremers, Pogg. 104. 133; 111. 60: Ger- lach, Z. anal. 8. 295.) Sp. gr. of Lil+Aq at 18 containing: 5 10 15 20 25% Lil. 1.0361 1.0756 1.1180 1.1643 1.2138 (Kohlrausch, W. Ann. 1879. 1.) Temp, of maximum g.-mol. Lil dissolved density of Lil+Aq. in 1000 g. H 2 O. 2.516 0.1795 0.039 0.4666 (de Coppet, C. R. 1900, 131. 178.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) 100 g. methyl alcohol dissolve 343.4 g. Lil at 25. 100 g. ethyl alcohol dissolve 250.8 g. Lil at 25. 100 g. propyl alcohol dissolve 47.52 g. Lil at 25. 100 g. isoamvl alcohol dissolve 112.50 g. Lil at 25. In the case of propyl alcohol the solid phase at 25 is Lil, 4C 3 H 8 O. (Turner and Bissett, Chem. Soc. 1913, 103. 1909.) Solubility in organic solvents at t. C=pts. by wt. of Lil in 100 ccm. of the sat. solution. L=no. of liters which at the saturation temp, hold in solution 1 mol. Lil. Solvent ' t C L Furfurol Nitromethane tt 25 25 45.86 2.519 1.219 0.292 5.32 10.98 (Walden, Z. phys. Ch. 1906, 66. 718.) Solubility in glycol at 15.3 = 28%. (de Coninck, Belg. Acad. Bull. 1906, 359.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Difficultly sol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) +H 2 O. Mpt. below 200. (Bogorodsky, . C. 1897, II. 175.) +2H 2 O. Mpt. 86-88. (Bogorodsky.) +3H 2 O. Mpt. 75. (Bogorodsky.) Sol. in absolute alcohol without decomp. (Thirsoff, Chem. Soc. 1894, 66. (2) 234.) The composition of the hydrates formed by Lil at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by Lil and of the conductivity and sp. gr. of Lil+Aq. (Jones, Am. Ch. J. 1905, 34. 301.) Lithium mercuric iodide, 2LiI, HgI 2 +6H 2 O. Very deliquescent. Decomp. by H 2 O. Very sol. without decomp. in alcohols, glycer- ine, acetone, fuming formic acid, acetic acid, ethyl acetate, ethyl oxalate, etc. Less sol. in nitrobenzene. Insol. in benzene and methyl iodide. (Duboin, C. R. 1905, 141. 1017.) +8H 2 O. Decomp. by H 2 O. Very sol. in alcohols, glycerine, acetone^ fuming formic acid, acetic acid, ethyl acetate, etc. without decomp. SI. sol. in nitrobenzene. Insol. in benzene and methyl iodide. (Duboin, 1. c.) +9H 2 O. Hydroscopic. Sol. in alcohol and acetone without decomp. (Dobroserdoff, C. C. 1901, 1. 664.) Lithium nitride, Li 3 N. Sol. in H 2 O with decomp. (Ouvrard, C. R. 114. 120.) Very hydroscopic. (Dafert, M. 1910, 31. 987.) Lithium oxide, Li 2 O. Slowly sol. in H 2 O to form LiOH. See Lithium hydroxide. Lithium peroxide, Li 2 O 2 . (de Forcrand, C. R. 1900, 130. 1467.) Lithium hydrogen peroxide, Li 2 O 2 , H 2 O 2 + 3H 2 O. Sol. in H 2 O. Insol. in alcohol, (de For- crand, C. R. 1900, 130. 1466.) Lithium selenide, Li 2 Se. Sol. in H 2 O. (Fabre, C. R. 103. 269.) +9H 2 O. Sol. inH 2 O. (Fabre.) Lithium silicide, Li 6 Si 2 . Decomp. by H 2 O and by dil. acids. De- comp. by aqueous solutions of alkalies with evolution of H 2 . (Moissan, C. R. 1902, 134. 1083.) 460 LITHIUM SULPHIDE Lithium ?w(wosulphide, Li 2 S. More sol. in H 2 O or alcohol than LiOH. Luteochromium bromide, Cr(NH 3 ) 6 Br 3 . Less sol. in H 2 O than the chloride. (Jor- gensen, J. pr. (2) 30. 1.) bromoplatinate, [Cr(NH 3 ) 6 ] 2 (PtBr 6 ) 3 4H 2 O. SI. sol. in H 2 O. Insol. in alcohol. (Jorgen- sen.) chloride, Cr(NH 3 ) 6 Cl 3 +H 2 O. Efflorescent, and very sol. in H 2 O. (Jorgen- chloroplatinate. (a) [Cr(NH 3 ) 6 ] 2 (PtCl 6 ) 3 +6H 2 O. Nearly completely insol. in H 2 O. (Jorgensen.) (6) Cr(NH 3 ) 6 Cl(PtCl 6 )+2^H 2 O. Decomp. by H 2 O into above; insol. in alcohol. (Jor- gensen.) (c) [Cr(NH 3 ) 6 i 2 Cl 4 (PtCl 6 )+2H 2 0. De- comp. by H 2 O into (a). (Jorgensen.) mercuric chloride, Cr(NH 3 ) 6 Cl 3 , HgCl 2 . Decomp. by H 2 O; si. sol. in dil. HCl+Aq; insol. in alcohol. Cr(NH 3 ) 6 Cl 3 , 3HgCl 2 +2H 2 O. Decomp. by dil. HCl+Aq into above salt. (Jorgen- sen.) chromicyanide, Cr(NH 3 ) 6 Cr(CN) 6 . Precipitate. cobalticyanide, Cr(NH 3 ) 6 Co(CN) 6 . Nearly insol. in H 2 O or in cone. HCl+Aq. (Jorgensen.) ferrocyanide, Cr(NH 3 ) 6 Fe(CN) 6 . Very si. sol. in cold H 2 O or dil. acids. (Jorgensen.) iodide, Cr(NH 3 ) 6 I 3 . SI. sol. in H 2 O. (Jorgensen, 1. c.) iodosulphate, Cr(NH 3 ) 6 So 4 I. Sol. in H 2 O; nearly insol. in dil. NH 4 OH + Aq or alcohol. (Jorgensen.) - nitrate, Cr(NH 3 ) 6 (NO 3 ) 3 . Sol. in 35-40 pts. H 2 O. Insol. in cold dil. HNO 3 +Aq or alcohol. Can be crystallised out of H 2 O containing a little HNO 3 . (Jor- gensen, J. pr. (2) 30. 1.) nitrate chloroplatinate, Cr(NH 3 )6(NO 3 )PtCl 6 +H 2 O. Insol. in H 2 O. Sol. in dil. H 2 SO 4 +Aq. (Jorgensen.) nitratosulphate, Cr(NH 3 ) 6 (NO 3 )SO 4 . Sol. in H 2 O; insol. in alcohol. (Jorgensen.) Luteochromium oxalate, [Cr(NH 3 ) 6 ] 2 (C 2 O 4 ) 3 + 4H 2 O. Nearly insol. in cold H 2 O. (Jorgensen.) or^ophosphate, Cr(NH 3 ) 6 PO 4 +4H 2 O. SI. sol. in H 2 O; easily sol. in dil. acids. (Jorgensen.) sodium pyrophosphate, Cr(NH 3 ) 6 (NaP 2 7 ) + Nearly insol. in cold H 2 O; wholly insol. in dil. NH 4 OH+Aq. (Jorgensen.) sulphate, [Cr(NH 3 ) 6 ] 2 (SO 4 ) 3 +5H 2 O. Quite sol. in H 2 O; insol. in alcohol. (Jor- gensen.) sulphate chloroplatinate, [Cr(NH 3 ) 6 (SO 4 )] 2 PtCl 6 . Nearly insol. in H 2 O. (Jorgensen.) Luteocobalt examine chromium sulpho- cyanide. See Diamine chromium luteocobalt sulpho- cyanide. Luteocobaltic bromide, Co(NH 3 ) 6 Br 3 . Sol. in H 2 0. Precipitated from saturated H 2 O solution by dil. HBr+Aq. (Jorgensen. J. pr. (2) 35. 417.) bromopermanganate, Co(NH 3 ) 6 Br 2 (MnO 4 ). Easily sol. in H 2 O. (Klobb, A. ch. (6) 12. 5.) bromoplatinate, Co(NH 3 ) 6 Br 3 , PtBr 4 + H 2 O. SI. sol. in H 2 O; can be recrystallised from hot H 2 O containing HBr. (Jorgensen.) - bromosulphate, Co(NH 3 ) 6 Br(SO 4 ). Nearly insol. in H 2 O. Very si. sol. in dil. NH 4 OH+Aq. (Jorgensen.) - carbonate, [Co(NH 3 ) 6 ] 2 (CO 3 ) 3 +7H 2 O. Efflorescent; easily sol. in H 2 O. [Co(NH 3 ) 6 ] 2 (C0 3 ) 3 , H 2 C0 3 +5H 2 0. Less sol. in H 2 O than the neutral salt. (Gibbs and Genth.) chloride, Co(NH 3 ) 6 Cl 3 . Sol. in 17.09 pts. H 2 O at 1(X5 ; 16.81 pts'. at 11.4; 16.48 pts. at 12; and more easily in hot H 2 O. (F. Rose.) 100 pts. H 2 O dissolve 4.26 pts. at 0, and 12.74 pts. at 46.6. (Kurnakoff, J. russ. Soc. 24. 629.) Not appreciably sol. in cone. HCl+Aq. (Jorgensen.) Insol. in alcohol or solutions of the alkali ihlorides. (Gibbs and Genth.) Insol. in NH 4 OH+Aq. LUTEOCOBALTIC CHROMATE 461 Aqueous solution is pptd. by alcohol, min- eral acids, or alkali chlorides. Luteocobaltic mercuric chloride, Co(NH 3 ) 6 Cl 3 , Sol. in hot H 2 O. (Krok, 1870.) By recrystallizing from hot H 2 containing HC1 is converted into Co(NH 3 ) 6 Cl 3 , 3HgCl 2 +H 2 O. Very si. sol. in cold H 2 O. (Jorgensen.) Co(NH 3 ) 6 Cl 3 , 2HgCl 2 + ^H 2 O. Sol. in hot H 2 O, from which it crystallizes on cooling. Insol. in cold cone. HCl+Aq, and is pptd. from H 2 O solution by HC1 or alcohol. (Car- stanjen.) Does not exist. (Jorgensen.) +3H 2 O. More easily sol. in cold H 2 O and other solvents than the preceding comp. (Carstanjen, Berlin, 1861.) Does not exist. (Jorgensen.) - stannous chloride, 2Co(NH 3 ) 6 Cl 3 , 3SnCl 2 + 10H 2 O. +8H 2 O. - chloraurate, Co(NH 3 ) 6 Cl 3 , AuCl 3 . Very si. sol. in cold, more easily in hot H 2 O containing HC1. (Gibbs and Genth, Sill. Am. J. (2) 23. 330.) - chloriodate, [Co(NH 3 )6Cl 2 ] 2 I 4 O 11 +H 2 O. - chloriridite, Co(NH 3 ) 6 , IrCl 6 . Insol. in boiling H 2 O or dil. HCl+Aq. (Gibbs.) - chloriridate, 2Co(NH 3 ) 6 Cl 3 , 3IrCl 4 . Insol. in H 2 O. (Gibbs.) - chlorochromate, Co(NH 3 ) 6 CrO 4 Cl+ 3H 2 O. Sol. in H 2 O. (Klobb, Bull. Soc. 1901, (3) 26. 1027.) - chlorofluoride, Co(NH 3 ) 6 Cl 2 F. (Bohm, Z. anorg. 1905, 43. 339.) chloropalladite, 2Co(NH 3 ) 6 Cl 3 , 3PdCl 2 . Easily sol. in dil. HCl+Aq. (Gibbs, Sill. Am. J. (2) 37. 58.) - chloroperchlorate, Co(NH 3 ) 6 Cl(ClO 4 ) 2 . (Millosevich, Gazz. ch. it. 1901, 31. (2) 285.) - chloropermanganate, Co(NH 3 ) 6 Cl 2 (MnO 4 ). Can be recrystallized from H 2 O. (Klobb, C. R. 103. 384.) - chloropermanganate ammonium chlor- ide, Co(NH 3 ) 6 Cl 2 (MnO 4 ), NH 4 C1. Easily sol. in H 2 O. (Klobb.) Luteocobaltic chloropermanganate potassium chloride, Co(NH 3 ) 6 Cl 2 (MnO 4 ), KC1. Very easily sol. in H 2 O, with decomp. into constituents; sol. in KCl+Aq. (Klobb.) chloropermanganate sodium chloride, Co(NH 3 ) 6 Cl 2 (MnO 4 ), NaCl. Very sol. in H 2 0. (Klobb.) chloroplatinate, 2Co(NH 3 ) 6 Cl 3 , 3PtCl 4 + 6H 2 O. Can be recrystallized from much hot H 2 O. (Gibbs and Genth.) +21H 2 O. (Gibbs and Genth.) Co(NH 3 ) 6 Cl 3 , PtCl 4 +^H 2 O. Very si. sol. in cold, decomp. by hot H 2 O into 2Cp(NH 3 ) 6 Cl 3 , PtCl 4 +2H 2 O. By recrys- tallizing from hot H 2 O containing HC1 this salt is converted into the above salt. (Jor- gensen.) chlororhodite. Nearly insol. in boiling H 2 O or dil. acids. Sol. in cone. HCl+Aq. (Gibbs, Sill. Am. J. (2) 37. 57.) chlororuthenate, 2Co(NH 3 ) 6 Cl 3 , 3RuCl 4 . Sol. in dil. acids. (Gibbs.) chloroselenate, Co(NH 8 ) 6 ClSeO 4 +3H 2 O. Decomp. by H 2 O. (Klobb, Bull. Soc. 1901, (3) 25. 1029.) chlorosulphate, Co(NH 3 ) 6 Cl(SO 4 ). Sol. in H 2 O. +3H 2 O. Only si. sol. in cold H 2 O. (Klobb, Bull. Soc. 1901, (3) 26. 1025.) ammonium chlorosulphate, [Co(NH 3 ) 6 ] 4 Cl 2 (S0 4 ) 5 , 3(NH 4 ) 2 S0 4 + . 6H 2 O. Decomp. by H 2 O. (Klobb, Bull. Soc. 1901, (3) 26. 1027.) chlorosulphate chloroplatinate, 2Co(NH 3 ) 6 Cl(SO 4 ), PtCl 4 . Very si. sol. in cold pure H 2 O. .Can be re- crystallized out of H 2 O containing HC1. (Krok.) chlorosulphate mercuric chloride, Co(NH 3 ) 6 Cl(S0 4 ), HgCl 2 . Scarcely sol. in pure H 2 O, but can be crys- tallized from warm acidified H 2 O. (Krok.) chlorosulphite, Co(NH 3 ) 6 (SO 8 )Cl+ 3H 2 O. Sol. in H 2 O. (Vortmann and Magdeburg, B. 22. 2637.) chromate, [Co(NH 3 ) 6 ] 2 (CrO 4 ) 3 +5H 2 O. Ppt. Sol. in hot H 2 O. [Co(NH 3 ) 6 ] 2 (Cr 2 0) 3 +5H 2 0. sol. in hot H 2 O. Moderately 462 LUTEOCOBALTIC CHROMICYANIDE Luteoccbaltic chromicyanide. Co(NH 3 ) 6 Cr(CN) 6 . Ppt. (Braun.) cobalticyanide, Co(NH 3 ) 6 Co(CN) 6 . Ppt. dithionate, basic, 4[Co(NH 3 ) 6 (S 2 6 )(OH)], Co 2 (S 2 6 ) 2 0. Sol. in H 2 O and dil. alcohol. ferricyanide, Co(NH 3 ) 6 Fe(CN) 6 + 3^H 2 0. Insol. in H 2 O. (Braun.) - fluoride, Co(NH 3 ) 6 F 3 . SI. sol. in cold H 2 O. Nearly insol. in acids. (Bohm, Z. anorg. 1905, 43. 340.) hydrogen fluoride, Co(NH 3 ) 6 H 3 F 6 . SI. sol. hi H 2 O. Decomp. by hot H 2 O. (Miolati and Rossi, Real. Ac. Line. 1896, (5) 5. II, 185.) hydrogen boron fluoride, Co(NH 3 ) 6 F 3 , 3BF 3 , HF. Cryst. from H 2 O acidified with HF. Mio- lati and Rossi.) molybdenyl fluoride, Co(NH 3 ) 6 F 3 , 2 MoO 2 F 2 . Cryst. from H 2 O containing HF. (Miolati and Rossi.) silicon fluoride, Co(NH 3 ) 6 F 3 , 2SiF 4 . Rossi.) (Miolati and titanium hydrogen fluoride, 2Co(NH 3 ) 6 F 3 , 3TiF 4 , 2HF. and Rossi.) (Miolati tungstyl fluoride, Co(NH 3 ) 6 F 3 , 2WO 2 F 2 . (Miolati and Rossi. ) uranyl fluoride. Co(NH 3 ) 6 F 3 , UO 2 F 2 . Can be cryst. from H 2 O containing HF. (Miolati and Rossi.) vanadyl fluoride, 2Co(NH 3 ) 6 F 3 , 5V0 2 F, 7HF. Ppt. (Miolati and Rossi.) fluoride nitrate, Co(NH 3 ) 6 F(N0 3 ) 2 . {Bohm, Z. anorg. 1905, 43. 336.) - hydroxide, Co(NH 3 ) 6 (OH) 3 . Known only in aqueous solution. Luteocobaltic mercuric hydroxychloride, CoN 6 H 14 (HgCl) 3 (HgOH)Cl 3 . Ppt. Easily decomp. (Vortmann and Morgulis, B. 22. 2644.) CoN 6 H 14 (HgOH) 4 Cl 3 . Ppt. (V. and M.) CoN 6 Hi 6 (HgOH) 2 Cl 3 . Ppt. (V. and M.) iodide, Co(NH 3 ) 6 I 3 . Insol. in cold, but moderately sol. in hot H 2 0. According to Jorgensen, contains HNO 3 and has the formula Co 2 (NH 3 ) 12 I 4 (NO 3 ) 2 . iodosulphate, Co(NH 3 ) 6 I(SO 4 ). Can be recrystallized from hot H 2 O. SI. sol. in warm/ nearly insol. in cold H 2 O. (Krok, B. 4. 711.) mercuriodide, Co 2 Ni 2 H 33 (HgI) 3 I 6 . Ppt. (Vortmann and Borsbach.) CoN 6 H 16 (HgI) 2 I 3 . Ppt. (V. and B.) mercuriodide, basic, CoN 6 H 16 (HgOH) 2 I 2 (OH). Insol. in H 2 O. SI. sol. in H 2 O. (Vort- mann and Borsbach, B. 23. 2804.) nitrate, Co(NH 3 ) 6 (NO 3 ) 3 . Sol. in H 2 O. Can be recrystallised from boiling H 2 0. Sol. in about 60 pts. H 2 O. Insol. in cone. HNO 3 +Aq. (Jorgensen, J. pr. (2), 35. 417.) Almost insol. in acids. (Rogoiski, A. ch. (3), 41. 454.) Insol. in NH 4 OH, HC1, and HNO 3 +Aq; decomp. by H 2 SO 4 +Aq. (Gibbs and Genth.) Co(NH 3 ) 6 (NO 3 ) 3 , HNO 3 . Decomp. by H 2 O or dil. alcohol. (Jorgensen, J. pr. (2), 44. 63.) nitrate chloroplatinate, Co(NH 3 ) 6 (NO 3 )Ch, PtCl 4 +H 2 O. Not decomp. by H 2 O. (Jorgensen.) nitratosulphate, Co(NH 3 ) 6 (NO 3 )(SO 4 ). Sol. in H 2 O. (Jorgensen.) nitrite cobaltic nitrite, Co 2 (NH 3 ) 12 (NO 2 ) 6 , Co 2 (NO 2 ) 6 = Co(NH,),(NOOeCo. Nearly insol. in H 2 O. (Jorgensen.) Much less sol. in H 2 O than the correspond- ing roseo salt. (Gibbs.) diamine cobaltic nitrite, Co(NH 3 ) 6 [Co(NH 3 ) 2 (N0 2 ) 4 ] 3 . Ppt. (Gibbs.) = Co(NH 3 ) 6 ](N0 2 ) 2 (NH 3 ) 2 Co(N0 2 ) 2 ] 3 . Nearly insol. in cold, si. sol. in boiling H 2 O. (Jorgensen, Z. anorg. 6. 179.). - oxalate, [Co(NH 3 ) 6 ] 2 (C 2 O 4 ) 3 +4H 2 0. Insol. in hot or cold H 2 O. Easily sol. in H 2 C 2 O 4 +Aq. LUTEOCOBALTIC SULPHATE BROMAURATE 463 Luteocobaltic oxalate chloraurate, 2Co(NH 3 ) 6 (C 2 O 4 )Cl, AuCl 3 +4H 2 O. Easily sol. in hot H 2 O. (Gibbs.) - perchlorate, Co(NH 3 )6(ClO 4 )3. (Millosevich, Gazz. ch. it. 1901, 31, (2) 285.) permanganate, [Co(NH 3 ) 6 ] 2 (MnO 4 ) 3 . Nearly insol. in H 2 O. 100 pts. H 2 O at dissolve only 0.072 pt. salt. Moderately sol. in hot H 2 O. (Klobb, A. ch, (6) 12. 5.) persulphate sulphate, [Co(NH 3 ) 6 ] 2 S 2 8 (S0 4 ) 2 . Much less sol. in H 2 than the sulphate. Sol. in 641 pts. H 2 O at 18.8 and in 632 pts. at 20. Not easily sol. even in boiling H 2 O. (Jorgensen, Z. anorg. 1898, 17. 459.) or^ophosphate, Co(NH 3 ) 6 (PO 4 ) + 4H 2 O. SI. sol. in cold H 2 O. Easily sol. in dil. acids. (Jorgensen.) [Co(NH 3 ) 6 ] 3 (P0 4 )(P0 4 H) 3 +5KH 2 (?). Ppt. (Braun.) [Co(NH 3 ) 6 ] 2 (PO 4 H) 3 +4H 2 O. Ppt. Easily sol. in very dil. HCl+Aq. (Jorgensen.) raetaphosphate. Ppt. p?/rophosphate, [Co(NH 3 ) 6 ] 2 P 4 O 13 + 6H 2 O. (Gibbs, Am. Acad. Proc. 11. 29); or Co 2 (NH 3 )i 2 P 4 O 13 (ONa) 2 (Vortmann, B, 11. 2181); or Co(NH 3 )6(P 2 O 7 Na)+ll^H 2 O. (Jorgensen, J. pr. (2) 35. 438.) Very nearly insol. in H 2 O. With H 2 O at 80 it is decomp. into [Co(NH 3 ) 6 ]4(P 2 O ) 3 +20H 2 O. Less easily sol. than the preceding salt. p*/rophosphate, acid, Co(NH 3 ) 6 (P 2 O 7 H). Wholly insol. in H 2 O. Somewhat sol. in dil. HC 2 H 3 O 2 +Aq. Easily sol. in HCl+Aq (Jorgensen.) sodium ps/rophosphate, Co(NH 3 ) 6 (P 2 O 7 Na) +11^H 2 O. Ppt. Not wholly insol. in cold H 2 O. Decomp. by hot H 2 O. Less sol. in NH 4 OH + Aq than in H 2 O. (Jorgensen.) [Co(NH 3 ) 6 ] 4 (P 2 O 7 ) 3 , 2Co(NH 3 ) 6 (NaP 2 O 7 ) +39 H 2 0. As above. (Jorgensen.) selenate, [Co(NH 6 )] 2 (SeO 4 ) 3 +5H 2 O. Very sol. in H 2 O. (Klobb, Bull. Soc. 1901, (3) 26. 1028.) hydrogen selenate, [Co(NH 3 ) 6 ]H(SeO 4 ) 2 +2^H 2 O. Not decomp. by H 2 O. .(Klobb.) Luteocobaltic ammonium selenate, [Co(NH 3 ) 6 ] 2 (Se0 4 ) 3 , (NH 4 ) 2 Se0 4 + 4H 2 O. Very sol. in H 2 O. [Co(NH 6 ] 2 (SeO 4 ) 3 , (NH 4 ) 2 SeO 4 +8H 2 O. Very sol. in H 2 O. (Klobb.) sulphocyanide, Co(NH 3 ) 6 (SCN) 3 . Decomp. by hot H 2 O. (Miolati, Z. anorg. 1900, 23. 241.) mercuric sulphocyanide, Co(NH 3 ) 6 (SCN) 3 , 2Hg(SCN) 2 . Decomp. by H 2 O. Cryst. from dil. NH 4 SCN+Aq. (Miolati.) platinum sulphocyanide, [Pt(SCN) 4 ] 3 [Co(NH 3 ) 6 (SCN 3 )] 2 . Decomp. by hot H 2 O. (Miolati.) silver sulphocyanide, Co(NH 3 ) 6 (SCN) 3 , 2AgSCN. Decomp. by hot H 2 O. (Miolati.) sulphate, [Co(NH 3 ) 6 ] 2 (SO 4 ) 3 +5H 2 O. SI. sol. in cold, more easily in hot H 2 O. +6H 2 O. (Krok,B.4.711.) hydrogen sulphate, . Co(NH 3 ) 6 H(S0 4 ) 2 . Decomp. by alcohol to sulphate, gensen, Z. anorg. 1898, 17. 458.) (Jor- 4[(Co6NH 3 ) 2 (SO 4 ) 3 ], 5H 2 SO 4 +10H 2 O. Very sol. in H 2 O with decomp. into the normal sulphate. When pulverized it seems to dissociate slowly in contact with abs. alcohol. (Klobb, Bull, Soc. 1901, (3) 25. 1025.) ammonium sulphate, [Co 6 (NH 3 ) 6 ] 2 (S0 4 ) 3 , (NH 4 ) 2 S0 4 +8H 2 0. Sol. in H 2 with decomp. (Klobb.) cerium sulphate, [Co(NH 3 ) 6 ] 2 (SO 4 ) 3 , Ce 2 (S0 4 ) 3 +l^H 2 0. Very si. sol. in cold, and practically insol. in boiling H 2 O. Sol. in acids. (Gibbs, Am. Ch. J. 15. 560.) [Co(NH 3 ) 6 ] 2 (S0 4 ) 3 , 3Ce(S0 4 ) 2 +H 2 0. As above. (Wing, Sill. Am. J. (2) 49. 363.) lanthanum sulphate, [Co(NH 3 )6] 2 (SO 4 )j, La,(S0 4 ),+H,0. SI. sol. in H 2 O. (Wing.) thallic sulphate, [Co(NH 3 ) 6 ] 2 (SO 4 ) 3 , T1 2 O(SO 4 ) 2 +5H 2 O. Decomp. by cold H 2 O. (Gibbs.) sulphate bromaurate, Co(NH 3 ) 6 (S0 4 )(AuBr 4 ). Very si. sol. in H 2 O with apparent decomp. Insol. in alcohol. (Jorgensen.) 464 LUTEOCOBALTIC SULPHATE CHLORAURATE Luteocobaltic sulphate chloraurate. Co(NH 3 ) 6 (SO 4 )AuCl4. SI. sol. in H 2 O. (Jorgensen.) cobaltic sulphite, [Co(NH 3 ) 6 ] 2 (SO 3 ) 3 , Co 2 (SO 3 ) 3 +H 2 O = dichrocobaltic sul- phite, [Co(NH 3 ) 3 ] 2 (SO 3 ) 3 +2H 2 O, which see. [Co(NH 3 ) 6 ] 2 (S0 3 ) 3 , 2Co,(SO,),+15H,0 = diamine cobaltic sulphite, [Co(NH 3 ) 2 ] 2 (SO 3 ) 2 +5H 2 O, which see. Luteorhodium bromide, Rh(NH 3 ) 6 Br 3 . Less sol. in H 2 O than the chloride. (Jor- gensen, J. pr. (2) 44. 51.) chloride, Rh(NH 3 ) 6 Cl 3 . Sol. in 7 to 8 pts. H 2 O at 8. (J.) +H 2 O. Extremely efflorescent. (J.) rhodium chloride, Rh(NH 3 ) 6 Cl 3 , RhCl 3 . Sol. in H 2 O. (Jorgensen, Z. anorg. 5. 174.) chloroplatinate, 2Rh(NH 3 ) 6 Cl 3 , 3PtCl 4 + 6H 2 0. Insol.inH 2 O. Sol.in warmHCl+Aq. (J,) Rh(NH*)gCl, PtCl 4 +^H 2 O. Decomp. by H 2 into chloride and above salt. ( J.) nitrate, Rh(NH 3 ) 6 (NO 3 ) 3 . Sol. in 48 to 49 pts. H 2 O at ord. temp. HNO 3 +Aq diluted with 5 vols. H 2 O ppts. the salt completely from aqueous solution. (Jorgensen, J. pr. (2) 44. 51.) Rh(NH 3 ) 6 (NO 3 ) 3 , HNO,. Decomp. by H 2 O or dil. alcohol. (Jorgensen, J. pr. (2), 44. 63.) or^ophosphate, Rh(NH 3 ) 6 P0 4 +4H 2 O. SI. sol. in cold H 2 O. (J.) sodium p?/rophosphate, [Rh(NH 3 ) 6 ] 2 (P 2 7 ) 3 Na 2 +23H 2 0. Nearly wholly insol. in H 2 O. Wholly insol. inNH 4 OH+Aq. (J.) sulphate, [Rh(NH 3 ) 6 ] 2 (SO 4 ) 3 +5H 2 O. Sol. in 43 pts. H 2 O at 20. (J.) Magnesium, Mg. Does not decomp. H 2 O at ord. temp.j but decomp. slowly at 100. H 2 O containing acids dissolves Mg easily. Sol. in cold dil. HC 2 H 3 O 2 +Aq. Difficultly sol. in cold H 2 SO 4 +Aq. (Bunsen.) Cold nitrosulphuric acid does not attack. (Bunsen.) Cold NH 4 OH+Aq, KOH+Aq, or NaOH+Aq do not attack. (Maak, Phippson.) Sol. in NH 4 C1 or (NH 4 ) 2 CO 3 -f Aq. (Wohler.) Very rapidly sol. in K 2 S 2 O 8 +Aq and (NH 4 ) 2 S 2 O 8 +Aq with violent evolution of gas. (Levi, Gazz. ch. it. 1908, 38. (1), 583.) Attacked by aqueous solution of KCL NH 4 C1, NaCl, LiCl, CuCl 2 , CdCl 2 , CoCl 2 , PbCl 2 , HgCl 2 , FeCl 3 , CrCl,, PtCl 4 , AuCl 3 , CuSO 4 , ZnSO 4 , FeSO 4 and MnSO 4 . SI. attacked by hot 30% CaCl 2 +Aq, not by 30% MgCl 2 +Aq, BaCl 2 +Aq and SrCl 2 + Aq. (Tommasi, Bull. Soc. 1899, (3), 21. 886.) Not attacked by NH 4 F+Aq, very slowly by solutions of BaCl 2 , CaCl 2 , KC1, K 3 Fe(CN) 6 , NaNO 8 , Na 2 S 2 O 3 and Na 2 HPO 4 . Solutions of NaC 2 H 3 O 2 , Na 2 B 4 O,, alum and chrome alum attack vigorously. Solutions of (NH 4 ) 2 C0 3 , NH 4 C1, (NH 4 ) 2 C 2 4 , (NH 4 ) 2 S and Na 2 CO 3 attack even more vigorously. (Mouraour, C. R. 1900, 130. 140.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Insol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Somewhat sol. in liquid NH 3 , if a clean metallic surface is in contact with the pure solvent. (Kraus, J. Am. Chem. Soc, 1907, 29. 1561.) ^ccm. oleic acid dissolves 0.0104 g. Mg in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Magnesium arsenide, Mg 3 As 2 . Decomp. on air. (Parkinson, Chem. Soc. 5. 127.) Magnesium azoimide, Mg(N 3 ) 2 . Decomp. by hot H 2 O. (Curtius, J. pr. 1898, (2) 58. 292.) Magnesium boride, Mg 9 B 2 . Sol. in HCl+Aq. (Winkler, B. 23. 774.) Magnesium bromide, MgBr 2 . Deliquescent. Very sol. in H 2 O with evolu- tion of heat. Sat. MgBr 2 -f-Aq contains at: 18 +1-7 48 62 97 52 58 60.9 62.5 65.8% MgBr 2 . (fitard, A. ch. 1894, (7), 2. 541.) See also MgBr 2 +6H 2 O. Sp. gr. of MgBr 2 +Aq at 19.5 containing: 5 10 15 20 25 % MgBr 2 , 1.043 1.087 1.137 1.191 1.247 30 35 40 45 50 % MgBr 2 . 1.31 1.377 1.451 1.535 1.625 (Kremers, Pogg. 108. 118, calculated by Gerlach, Z. anal. 8. 285.) MgBr 2 +Aq is si. decomp. by evaporation. MAGNESIUM BROMIDE 465 Solubility of MgBr 2 in alcohols. MgBr 2 forms with methyl alcohol a com- plex, MgBr 2 , 6CH 3 OH. Solubility of MgBr 2 , 6CH 3 OH in CH 8 OH at t Solubility of MgBr 2 , 6(iso)C 4 H 9 OH in C 4 H 9 OH at t. t % by weight of MgBr 2 , 6isoC 4 HOH t VKSff* 6isoC 4 H 9 OH 10 20 30 40 50 55.8 60.5 65.2 69.8 74.3 78.5 60 65 71 75 77 80 mpt. 82.4 84.2 88.0 ' 92.0 94.6 100 t % by weight of MgBr 2 , 6CH 3 OH t % by weight of MgBr 2 , 6CH 3 OH 20 40 60 80 100 110 120 42.6 44.6 46.7 48.9 51.4 55.5 58.0 60.7 130 140 150 160 170 180 185 190 mpt. 63.6 66.8 70.2 74.0 78.5 84.5 88.0 100 (Menschutkin.) MgBr 2 forms with isoamylalcohol a com- plex, MgBr 2 , 6(iso)C5H n OH. Solubility of MgBr 2 , 6(iso)C 6 HnOH in C 6 H n OH at t. (Menschutkin, Z. anorg. 1907, 62. 11.) MgBr 2 forms with ethyl alcohol a complex, MgBr 2 , 6C 2 H 5 OH. Solubility of MgBr 2 , 6C 2 H 6 OH in C 2 H 6 OH at t. t % by weight of MgBr 2 , GisoCsHnHO t % by weight of MgBr 2 , GisoCsHnOH 10 20 30 35 70.2 75.6 80.2 84.5 86.7 38 40 42 44 46 mpt 88.7 90.0 92.0 94.2 100 t % by weight of MgBr 2 , 6C 2 H 5 OH t % by weight of MgBr 2 , 6C 2 H 6 OH (Menschutkin.) Solubility in ether at t. t % MgBr 2 % MgBr 2 , 2C 4 HioO 10 20 30 40 50 60 70 75 17.2 24.9 32.7 40.3 47.8 55.1 62.2 68.8 71.4 80 85 90 95 100 103 106 108. 5 mpt. 73.8 76.2 78.7 82.3 86.7 90.0 94.4 100 8 + 10 14 16 18 20 22 mpt. 0.6 0.8 1.27 1.64 1.93 2.3 2.7 3.22 1.08 1.44 2.3 2.95 3.48 4.14 4.86 5.80 (Menschutkin.) MgBr 2 forms with propyl alcohol a com- plex, MgBr 2 , 6C 3 H 7 OH. Solubility of MgBr 2 , 6C 8 H 7 OH in C 3 H 7 OH att. Solubility of MgBr 2 , 2C 4 Hi O in ether at t. 'Lower solution"=the melted MgBr 2 , 2C 4 Hi O which does not mix with the ether above. t ' % by weight of MgBr 2 , 6C 3 H 7 OH t % by weight of MgBr 2 , 6C 3 H 7 OH 10 20 30 40 77.9 81.5 85.1 89.5 92.0 43 46 48 50 52 mpt. 93.0 94.3 95.8 97.8 100 (Menschutkin.) MgBr 2 forms with isobutylalcohol a com- plex, MgBr 2 , 6(iso)C 4 H 9 OH. t Composition of lower solution Composition of the upper layer % MgBr 2 lc' % MgBr, % MgBr 2 , 2C 4 H 10 10 42.0 75.7 1.8 3.2 41.0 73.9 2.3 4.1 +10 40.1 72.2 2.8 5.0 20 39.3 70.8 3.3 5.9 30 38.7 69.8 3.8 6.8 40 38.2 68.8 4.3 7.7 50 37.8 68.0 4.7 8.5 60 37.6 67.7 5.1 9.2 70 37.6 67.7 5.4 9.7 80 37.8 68.0 5.6 10.0 90 38'. 1 68.6 5.7 10.2 (Menschutkin.) 466 MAGNESIUM BROMIDE Solubility of MgBr 2 in formic acid. MgBr 2 forms with formic acid a complex, MgBr 2 , 6HCOOH. Solubility of MgBr 2 , 6HCOOH in HCOOH att. Solubility of MgBr 2 in acetone. MgBr 2 forms with acetone a complex. MgBr 2 , 3CH 3 COCH 3 . Solubility of MgBr 2 , 3CH 3 COCH 3 in CH 3 COCH 3 at t. t % by wt. MgBr 2 , 6HCOOH t % by wt. MgBr 2 , 3CH 3 COCH 3 20 40 60 70 80 86 88 mpt. 49.8 57.5 65.1 73.1 78.1 86.0 95.0 100 30 60 70 72 73 74 75 76 80 84 88 92 mpt. 0.2 0.8 1.45 2.0 3.7 5.5 14.0 50.0 71.6 83.3 89.8 95.2 100 (Menschutkin, Z. anorg. 1907, 64. 90.) Solubility of MgBr 2 in acetic acid. MgBr 2 forms with acetic acid a complex. MO-HT... ftnTT-nnnw Solubility of MgBr 2 , 6CH 3 COOH in CH 3 COOH at t. Solubility of MgBr 2 in acetamide. MgBr 2 forms with acetanide a complex, MgBr 2 , 6CH 3 CONH 2 . Solubility of MgBr 2 , 6CH 3 CONH 2 in CH 3 CONH 2 at t. t % by wt. MgBr 2 , GCHsCOOH 17 30 50 60 70 80 85 90 100 105 110 112 mpt. 0.3 1.5 4.5 7.9 16.2 38.5 49.5 57.7 71.8 80.0 89.5 100.0 t % H%^' 50.5 70 90 110 130 150 '-' 160 165 169 mpt. 56.0 57.8 60.5 65.0 71.5 80.0 85.5 90.0 100.0 (Menschutkin.) Solubility of MgBr 2 in acetic anhydride. MgBr 2 forms with acetic anhydride a com- plex, MgBr 2 , 6(CH 3 CO) 2 O. Solubility of MgBr 2 , 6(CH 3 CO) 2 O in (CH 3 CO) 2 O at t. (Menschutkin, Z. anorg. 1909, 61. 106.) Solubility of MgBr 2 in acetanilide. MgBr 2 forms with acetanilide a complex, MgBr 2 , 6CH 3 CONHC 6 H 5 . Solubility of MgBr 2 , 6CH 3 CONHC 6 H 5 in CH 3 CONHC 6 H 5 at t. t % by wt. MgBr 2 , 6(CH 3 CO) 2 t % by wt. MgBr 2 , 6CH 3 CONHC 6 H 5 26.4 107.5 9.0 30 30.0 140 19.3 60 37.7 170 29.6 90 44.5 185 39.0 120 57.8 195 49.0 130 69.8 200 59.5 135 85.0 205 73.2 136-137 mpt. 100 . 209 mpt. 100.0 (Menschutkin, Z. anorg. 1909, 61. 112.) (Menschutkin, Z. anorg. 1909, 61. 109.) MAGNESIUM BROMIDE 467 Solubility of MgBr 2 in aniline. MgBr 2 forms with aniline three complexes: MgBr 2 , 6C 6 H 5 NH 2 ; MgBr 2 , 4C 6 H 5 NH 2 : MgBr 2 , 2C 6 H 5 NH 2 . Solubility of these complexes in aniline. Solubility of MgBr 2 in methylal. MgBr 2 forms with methylal a complex, MgBr 2 , 2CH 2 (OCH 3 ) 2 . Solubility of MgBr 2 , 2CH 2 (OCH 3 ) 2 in CH 2 (OCH 3 ) 2 at t. Solubility of MgBr 2 , 6C 6 H 6 NH 2 in C 6 H 5 NH 2 . t % by wt. MgBr 2 , 2CH 2 (OCH 3 ) 2 t % by weight of MgBr 2 , 6C 6 H 5 NH2 20 40 60 80 100 106 106 108 110 112 mpt. 0.3 0.45 0.6 0.75 0.9 1.1 86.2 90.8 95.4 100 10 30 50 70 90 100 103.5 3.2 3.9 5.1 7.5 12.8 18.5 27.5 Solubility of MgBr 2 , 4C e H 5 NH 2 in C 6 H 5 NH 2 . (Menschutkin, Z. anorg. 1907, 53. 32.) Solubility of MgBr 2 in dimethylcarbinol. MgBr 2 forms with dimethylcarbinol a complex, MgBr 2 , 4(CH 3 ) 2 CHOH. Solubility of MgBr 2 , 4(CH 3 ) 2 CHOH in (CH 3 ) 2 CHOH at t. t % by weight of MgBr 2 , 4CH 5 NH 2 103 120 140 160 180 200 220 230 237 24.0 24.3 24.9 26.0 28.3 33.5 45.0 55.0 76.3 t % by weight of MgBr 2 , 4(CH 3 ) 2 CHOH % by weight t of MgBr 2 , 4(CH 3 ) 2 CHOH 20 40 60 80 100 40.0 42.2 45.0 48.5 53.3 59.0 110 62.5 120 67.3 130 74.0 136 83.6 138 90.00 139 mpt. 100 Solubility of MgBr 2 , 2C6H5NH2 in C 6 H 5 NH 2 t % by weight of MgBrj, 2C 6 H 5 NH 2 237 250 260 270 76.3 77.3 78.1 79.0 ( M enschutkin . ) Solubility of MgBr 2 in trimethylcarbinol. MerBr* forms with trimethvlcarbinol a (Menschutkin, Z. anorg. 1907, 62. 159.) complex, MgBr 2 , 4(CH 3 ) 3 COH. Solubility of MgBr 2 in benzaldehyde. MgBr 2 forms with benzaldehyde a com- plex, MgBr 2 , 3C 6 H 5 CHO. Solubility of MgBr 2 , 3C 6 H 5 CHO in C 6 H 5 CHO at t. Solubility of MgBr 2 , 4(CH 3 ) 3 COH in (CH 3 ) 3 COH at t. t % by wt. MgBtt, 3C 6 H 5 CHO t % by wt. MgBr 2 , SCeHsCHO 0.7 140 17.8 30 1.3 145 37.5 60 1.9 146 65.0 80 2.5 148 84.5 100 3.4 153 93.2 120 6.0 159 mpt. 100 130 9.5 (Menschutkin, Z. anorg. 1907, 63. 26.) t % by weight of MgBr,, 4(CH 3 )3COH t % by weight of MgBr 2 , 4(CH 3 ) 3 COH 24.4 25 35 45 55 60 0.06 1.0 9.5 19.1 32.2 40.5 65 70 75 77.5 79 80 mpt. 50.5 62.5 77.0 85.0 91.5 100 Menschutkin.) Solubility of MgBr 2 in phenylhydrazine. MgBr 2 forms with CeHsNHNH^ a complex. MgBr 2 , 6C 6 H 6 NHNH 2 . 468 MAGNESIUM MANGANOUS BEOMIDE Solubility of MgBr 2 , 6C 6 H 5 NHNH 2 in C 6 H 5 NHNH 2 at t. MgBr 2 , 6NH 2 COOC 2 H 5 decomposes at 90.5-91 forming MgBr 2 , 4NH 2 COOC 2 H 5 . Solubility of MgBr 2 , 4NH 2 COOC 2 H 5 in NH 2 COOC 2 H 6 at t. t % by wt. of MgBr 2 , 6C 6 H 5 NHNH 2 20 40 60 80 99 100 140 180 200 3.0 7.0 16.4 33.0 54.8 54.8 60.8 68.4 73.4 t % by wt. MgBr 2 , 4NH 2 COOC 2 H 5 91 100 110 115 120 123 mpt. 69.4 73.8 80.0 84.1 90.0 100.0 (Menschutkin, Z. anorg. 1907, 52. 162.) Solubility of MgBr 2 in urea. MgBr 2 forms with urea a complex, MgBr 2 , 6CO(NH 2 ) 2 . Solubility of MgBr 2 , 6CO(NH 2 ) 2 in urea at t' (Menschutkin.) +6H 2 O. Solubility of MgBr 2 +6H 2 O in H 2 O at t. t % by weight of MgBr 2 + 6H 2 O t % by weight of MgBr 2 + 6H 2 t ^NlS? 1 * 20 40 60 80 100 76.0 78.1 80.2 82.3 84.4 86.6 120 140 150 160 164 mpt. 89.0 92.0 94.9 98.0 100 108.5 115 120 125 127 130 24.2 29.8 35.0 41.6 45.5 60.0 (Menschutkin, Z. anorg. 1907, 52. 153.) (Menschutkin, Z. anorg. 1909, 61. 116.) MgBr 2 , 6CO(NH 2 ) 2 decomposes at 130 giving MgBr 2 , 4CO(NH 2 ) 2 . Solubility of MgBr 2 , 4CO(NH 2 ) 2 in urea at t. t - % by wt. MgBr 2 , 4CO(NH 2 ) 2 130 145 160 165 170 171 58.0 60.7 67.2 71.4 83.7 96.0 (Menschutkin, Z. anorg. 1909, 61. 116.) Solubility of MgBr 2 in urethane. MgBr 2 forms with urethane a complex, MgBr 2 , 6NH 2 COOC 2 H 6 . Solubility of MgBr 2 , 6NH 2 COOC 2 H 5 in NH 2 COOC 2 H 5 at t. 35 50 70 80 85 90 *91.5 by wt. MgBr 2 , 2 COOC 2 H 5 43.3 45.6 51.3 56.2 59.8 66.5 75.5 * Mpt. of MgBr 2 , 6NH 2 COOC 2 H 5 . (Menschutkin, Z. anorg. 1909, 61. Sp. gr. of solution sat. at 18 = 1.655, and contains 50.8% MgBr 2 . (Mylius and Funk, B. 1897, 30. 1718.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. in alcohol. Sol. in acetone. (Nau- mann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) + 10H 2 O. Sol. in H 2 O. (Panfiloff, Chem. Soc. 26. 234.) Magnesium manganous bromide, MgBr 2 , 2MnBr 2 + 12H 2 O. Deliquescent. (Saunders, Am. Ch. J. 14. 150.) Magnesium mercuric bromide, MgBr 2 , HgBr 2 MgBr 2 , 2HgBr 2 . Not deliquescent. Magnesium molybdenyl bromide, MgBr 2 , MoOBr 3 +7H 2 O. ' (Weinland and Knoll, Z. anorg. 1905, 44. 112.) Magnesium potassium bromide, MgBr 2 , 2KBr+6H 2 O. Easily sol. in H 2 O, from which KBr crys- tallises at 75 to 87. Alcohol dissolves out MgBr 2 . (Lowig, Repert. 29. 261.) MAGNESIUM CHLORIDE 469 Formula is MgBr 2 , KBr+6H 2 0. De- Sp. gr. of MgCl 2 -t-Aq at 15. liquescent. (Lerch, J. pr. (2) 28. 338.) Magnesium stannic bromide. -? o o See Bromostannate, magnesium. M Sp. gr. j Sp. gr. 1 Sp. gr. Magnesium chloride, MgCl 2 . &5 5 55 Deliquescent. Very sol. in H 2 O with 1 1.0084 13 1.1130 2-5 1.2274 evolution of heat. The solution decomposes 2 1.0169 14 1 . 1220 26 1.2378 on evaporation losing HC1, when less than 6 3 1.0253 15 1.1311 27 1.2482 mols. H 2 O are present to 1 mol. MgCl 2 . 4 1.0338 16 1 . 1404 28 1.2586 (Casaseca, C. R. 37. 350.) 5 1.0422 17 1.1498 29 1.2690 Anhydrous. Sol. in 1.857 pts. H 2 O at 15. 6 .0510 18 .1592 30 1.2794 (Gerlach.) 7 .0597 19 .1686 31 1.2903 Sol. in 1 pt. cold H 2 0. (Fourcroy.) Sat. MgCl 2 +Aq at 12.5 contains 64.8% MgCl 2 . 8 9 .0684 .0772 20 21 .1780 .1879 32 33 1.3012 1.3121 (Hassenfratz.) 100 pts. H 2 O at 15.5 dissolve 200 pts. MgCU. (Ure's Diet.) 10 11 .0859 .0949 22 23 .1977 .2076 34 35 1.3230 1.3340 12 1040 24 .2175 100 pts. H 2 O dissolve 52.2 pts. MgCl 2 at and sp. gr. of sat. solution = 1.36 19 at 15. rr\ i u rr ! o 001 \ 1000 mols. H 2 6 dissolve 108 mols. MgCl 2 at 25C. (Lbwenherz, Z. phys. Ch. 1894, 13. 479.) Sp. gr. of MgCl 2 +Aq at 18. 100 mols. MgCl 2 +Aq contain at t: t 67.5 68.5 68.7 79.5 79.95 Mol.MgCl 2 11.58 11.92 11.71 12.28 12.39 t 116.67 152.6 181-2 186 Mol. MgCl 2 16.2 18.24 23.8 24.1-24.4 (Vant Hoff and Meyerhoffer, B. A. B. 1897, 73.) Solubility of MgCl 2 in H 2 O at t. | Sp. gr. 1 S Sp. gr. o g Sp. gr. 5 1.0416 10 1.0859 20 30 1.1764 1.2779 34 1.3210 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of MgCl 2 +Aq at 0. S=pts. salt in 100 pts. of solution; Si = mols. salt in 100 mols. solution. t MgCl 2 Solid phase 10 20 30 33.6 20 11.4 16. 19.4 20.6 26.7 30.5 31.6 34.3 34.6 34.9 35.3 35.6 36.5 37.9 39.8 42.2 46.1 49.1 55.8 56.1 Ice K Ice+MgCl 2 , 12H 2 MgCl 2 , 12H 2 O tt MgCl 2 , 12H 2 + MgCl 2 , 8H 2 O MgCl 2 , 8H 2 0+MgCl 2 , 6H 2 O MgCl 2 , 6H 2 O n MgCl 2 , 6H 2 0+MgCl 2 , 4H 2 MgCl 2 , 4H 2 O MgCl 2 , 4H 2 0+MgCl 2 , 2H 2 MgCl 2 , 2H 2 16.4 1ft Q s Si Sp. gr. 3.4 10 20 22 40 60 80 100 116.7 152.6 181.5 186 29.2056 20.9293 15.7989 11.3249 6.2008 7. 4. 3. 2. 1. 230 762 423 355 233 1.2788 1.1927 1.1427 1.1007 1.0545 (Charpy, A. ch. (6) 29. 23.) Sp. gr. of MgCl 2 +Aq at 19.5. Pts. MgCl 2 in 100 pts. Sp. gr. H 2 Pts. MgClz in 100 pts. Sp. gr. H 2 10.7 1.0826 22.0 1.1592 35.3 1.2388 51.5 1.3235 (Landolt-Bornstein, Tab. 5th Ed. 1912. 480.) See also MgCl 2 +6H 2 O. (Kremers, Pogg. 104. 155.) 470 MAGNESIUM CHLORIDE Sp. gr. of MgCl 2 +Aq at 14. Sp. gr. ofMgC! 2 +Aq. go Sp. gr. | Sp. gr. 1 Sp. gr. V* MgCl 2 g. in 1000 g. of solution Sp. gr. 16/16 0.4400 0.8801 1.7780 3.4533 7.4691 14.7187 29.6307 . 1 1 1 1 1 1 1 1 .000000 .000372 .000741 .001458 .002888 .006219 .012235 .024647 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 0.9993 .0033 .0073 .0113 .0154 .0194 .0234 .0274 .0314 .0355 .0395 1.0435 1.0476 1.0517 1.0558 1.0599 1.0641 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 1.0682 1.0724 1.0765 1.0807 1.0849 1.0891 1.0933 1.0976 1.1018 1.1061 1.1103 1.1146 1.1189 1 . 1232 1 . 1275 1.1319 1.1363 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 1.1407 1.1451 1.1495 1.1540 .1584 .1628 .1673 .1718 .1763 .1809 .1855 1.1901 1.1948 1.1995 1.2042 (Dijken, Z. phys. Ch. 1897, 24. 108.) Sp. gr. of MgCl 2 at 20.1. p=per cent strength of solution; d = ob- served duesity; w = volume cone, in grams per cc. ( Joo =w -) P d w 28.83 25.59 20.31 15.79 10.185 8.058 5.919 3.913 ' 3.903 * 1.743 1.2569 1.2241 1.1735 1 . 1324 1.0833 1.0650 1.0473 1.0304 1.0240 1.0126 0.36237 0.31327 0.23842 0.17877 0.11033 0.08583 0.06198 0.04022 0.03210 0.01765 (Oudemans, Z. anal. 7. 420.) Sp. gr. of MgCl 2 +Aq at 24. I Sp. gr. 1 Sp. gr. 1 Sp. gr. (Barnes, J. Phys. Chem. 1898, 2. 546.) Sp. gr. of MgCl 2 +Aq at t. 2 4 6 8 10 12 14 16 18 20 22 24 26 28 1.0069 1.0138 1.0207 1.0276 1.0345 1.0415 1.0485 1.0556 1.0627 1.0698 1.0770 1.0842 1.0915 1.0988 30 32 34 36 38 40 42 44 46 48 50 52 54 56 1.1062 1.1137 1.1212 1.1288 1 . 1364 1 . 1441 1.1519 1.1598 1.1677 1.1756 1 . 1836 1.1918 1.2000 1.2083 58 60 62 64 66 68 70 72 74 76 78 80 1.2167 1.2252 .2338 .2425 .2513 .2602 .2692 .2783 .2875 .2968 .3063 .3159 t Concentration of MgCh+Aq Sp. gr, 23 24 1 pt. MgCl 2 in 8.1874 pts. H 2 O 1 pt. " " 102.1 " " 1.0906 1.0065 (Hittorf, Z. phys. Ch. 1902, 39. 628.) Sp. gr. of MgCl 2 at 0. G. MgCl 2 in 100 ccm. of solution 6.7158 9.9506 Sp. gr. 1.0591 1.0845 G. MgCl 2 in 100 ccm. of sol. 13.8111 20.004 Sp. gr. 1.1106 1.1605 (Bremer, C. C. 1902, I. 293.) (Gerlach, Z. anal. 8. 283. Calculated from Schiff.) Sp. gr. of MgCl 2 +Aq at 25. Concentration of MnCh+Aq. Sp. gr. 1-normal Vr- " V- " Vr- " 1.1375 1.0188 1.0091 1.0043 (Wagner, Z. phys. Ch. 1890, 6. 38.) Sp. gr. of MgCl 2 +Aq at 20 containing M g. mols. MgCl 2 per 1. M 0.00493 0.007327 0.01 0.03104 Sp. gr. 1.000344 1.000524 1.000842 1.002756 M 0.05108 0.07171 0.10 0.25 Sp. gr. 1.004224 1.006036 1.008505 1.020966 M 0.50 0.75 0.9415 Sp. gr. 1.038496 1.056905 1.069617 (Jones and Pearce, Am. Ch. J. 1907, 38. 699.) MAGNESIUM MERCURIC CHLORIDE 471 MgCl 2 +Aq containing 10% MgCl 2 boils at 101.6; containing 20% MgCl 2 boils at 106.2; containing 30% MgCl 2 boils at 115.6. (Ger- lach.) Sat. MgCl 2 +Aq forms a crust at 122.5, and contains 52.9 pts. MgCl 2 to 100 pts. H 2 O. (Gerlach, Z. anal. 26. 426.) B.-pt. of MgCl 2 +Aq. P=pts. MgCl 2 to 100 pts. H 2 0. B.-pt. p B.-pt. p B.-pt. P 101 4.9 111 34.6 121 50.8 102 9.2 112 36.6 122 52.2 103 13.2 113 38.4 123 53.6 104 16.7 114 40.2 124 55.0 105 19.9 115 41.8 125 56.4 106 22.5 116 43.4 126 57.7 107 25.0 117 44.9 127 59.0 108 27.5 118 46.4 128 60.3 109 29.9 119 47.9 129 61.6 110 32.3 120 49.4 130 62.9 Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +2H 2 O. Very deliquescent. (Ditte, A. ch. 1881, (5) 22. 560.) +4H 2 O. (van't Hoff and Meyerhoffer.) +6H 2 O. Deliquescent. Sol. in 0.6 pt. (Gerlach, Z. anal. 26. 440.) B.-pt. of MgCl 2 +Aq containing % MgCl 2 . % MgCl 2 B.-pt. % MgCl 2 B.-pt. 4.6 8.4 101 102 11.6 14.3 103 104 (Skinner, Chem. Soc. 61. 341.) Sol. in KCl+Aq at 50. (Uhlig, C. C. 1913, II. 749.) Sol. in 7 pts. alcohol at 15. (Bergmann.) ' 5 ' moderate heat. (.B) 100 pts. alcohol of given sp. gr. dissolve pts. MgCl 2 : Sp. gr. Pts. MgCh Sp.gr. Pts. MgCh 0.900 0.848 21.25 23.75 0.834 0.817 36.25 50.00 cold, and 0.273 pt. hot H 2 O. (Casaseca, I. c.) Solubility in H 2 O at t. t 1000 mols H 2 O dissolve mols MgCl 2 100 g. H 2 O dis- solve g. MgCh 3.5 25.0 50.0 99.6 104.5 110.6 52.65 55.26* 58.66 (Biltz and Marcus, Z. anorg. 1911, 71. 169.) Solubility in KCl+NH 4 Cl+Aq at 25 has been studied. (Biltz and Marcus. Z. anorg. 1911, 71. 178.) When the solid phases are MgSO 4 +6H 2 O and MgCl 2 +6H 2 O, 1000 mols. H 2 O dissolve 104 mols. MgCl 2 and 14 mols. MgSO 4 at 25. (Lowenherz, Z. phys. Ch. 1894, 13. 480.) Solubility of MgCl 2 +6H 2 O in (NH 4 )MgCl 8 + 6H 2 O+Aq at t. t Per 1000 mols H 2 O Mols NH 4 C1 Mols MgCh 3.5 25.0 50.0 0.5 0.5 0.8 99.5 103.8 111.2 (Biltz and Marcus, Z. anorg. 1911, 71. 170.) (Kirwan.) MgCl 2 +6H 2 O is sol. in 5 pts. alcohol of 0.90 sp. gr. and in 2 pts. alcohol of 0.817 sp. gr. Sol. in 0.1828 pt. strong alcohol at 82.5. (Wenzel.) B.-pt. of an alcoholic solution of MgCl 2 . % MgCl 2 B.-pt. 5.56 8.53 9.62 13.84 78. 43 +0.73 " +1.34 " +1.77 " +3.54 (Skinner, Chem. Soc. 61. 341.) Even more sol. in acetic ether than CaCl 2 . (Cann, C. R. 102. 363.) Sol. in boiling amyl alcohol. (Riggs, Sill. Am. J. 144. 103.) SI. sol. in anhydrous pyridine. Sol. in 97%, 95% and 93% pyridine+Aq. (Kahlen- berg, J. Am. Chem. Soc. 1908, 30. 1107.) Solubility data of MgCl 2 +KCl+MgKCl, are given by van't Hoff and Meyerhoffer. (Z. phys. Ch. 1899, 30. 64.) +8H 2 O. Pptd. from an aqueous solution which contains about 10 mols. H 2 O to 1 mol. MgCl 2 . + 12H 2 O. Pptd. from an aq . solution which contains 1 mol. MgCl 2 in about 12.06 mols. of H 2 O. (Bogorodsky, C. C. 1899, 1. 246.) Magnesium manganous chloride, MgCl 2) 2MnCl 2 +12H 2 O. Deliquescent. Very sol. in H 2 O and al- cohol. (Saunders, Am. Ch. J. 14. 148.) 2MgCl 2 ,MnCl 2 +12H 2 O. Ppt. Deliquesces in the air. (Gossner, C. C. 1904, 1. 707.) Magnesium mercuric chloride, MgCl 2 , +6H 2 O. Very deliquescent. More sol. than the fol- lowing salt. (v. Bonsdorff, Pogg. 17. 133.) MgCl 2 , 3HgCl 2 +5H 2 O. Sol. in H 2 O with- 472 MAGNESIUM PHOSPHORYL CHLORIDE out decomp. Easily sol. in alcohol, (v. Bonsdorff.) Magnesium phosphoryl chloride. MgCl 2 , POC1 8 . Deliquescent. Sol. in H 2 O with evolution of heat and decomposition. Very si. sol. in warm POC1 3 . (Casselmann, A. 98. 223.) Magnesium potassium chloride. MgCl 2 , 2KC1+6H 2 0. Deliquescent, forming a solution of MgCl 2 , while KC1 remains undissolved. 100 pts. H 2 O dissolve 64.5 pts. at 18.75. 20 pts. salt dis- solved in 80 pts. H 2 O lower the temp. 1.75. (Bischof.) Alcohol dissolves out MgCl 2 . De- comp. into the two salts by solution in H 2 O. (Marcet.) A sat. solution in contact with solid KC1 and KC1, MgCl 2 , H 2 O at 50 contains 79.5 mol. MgCl 2 and 14.9 mol. KC1 per 1000 mol. H 2 O. A sat. solution in contact with solid MgCl 2 , 6H 2 O and KC1, MgCl 2 , H 2 O at 50 contains 111.9 mol. MgCl 2 and 1.2 mol. KC1 per 1000 mol. H 2 O. (Uhlig, Chem. Soc. 1913, 104. (2) 775; C. B. Miner. 1913, 417.) Min. Carnallite. Magnesium rubidium chloride, MgCl 2 , RbCl +6H 2 0. Not decomp. by a small quantity of H 2 0. (Feit and Kubierscky, Ch. Ztg. 16. 335.) Magnesium sodium chloride, MgCl 2 , NaCl+ 2H 2 0. Sol. in H 2 O. (Poggiale.) Magnesium thallic chloride, 2T1C1 3 , MgCl 2 + 6H 2 O. Hydroscopic. Can be cryst. from H 2 O. (Gewecke, A. 1909, 366. 224.) Magnesium stannic chloride. See Chlorostannate, magnesium. Magnesium vanadium chloride, MgCl 2 , VC1 3 +H 2 0. Difficultly sol. in H 2 O and alcohol. (Stab- ler, B. 1904, 37. 4412.) Magnesium zinc chloride, MgCl 2 , ZnCl 2 + 6H 2 O. Deliquescent; sol. in H 2 O. (Warner, C. N. 27. 271.) Magnesium chloride ammonia, MgCl 2 , 4NH 3 . Easily decomp. (Clark, A. 78. 369.) Magnesium chloride hydroxylamine, MgCl 2 , 2NH 2 OH+2H 2 O. 100 g. of solution in H 2 O contain 44.4% at 20. (Antonow, J. Russ. Phys. Chem. Soc. 1905, 37. 478.) Magnesium fluoride, MgF 2 . 1 1. H 2 O dissolves 76 mg. MgF 2 at 18. (Kohlrausch, Z. phys. Ch. 1904, 60. 356.) 87 mg. are dissolved in 1 1. of sat. solution at 18. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Scarcely sol. in acids. (Gay-Lussac and Thenard.) Insol. in excess of HF. When precipitated, is sol. in aqueous solution of ammonium and magnesium salts. Sol. in dil. HNO 3 +Aq, from which it is precipitated by alcohol. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Min. Sellaile. Magnesium potassium fluoride, MgF 2 , KF. Decomp. by H 2 SO 4 . (Duboin, C. R. 1895, 120. 679.) MgF 2 , 2KF. Decomp. by H 2 SO 4 . (Du- boin.) Magnesium sodium fluoride, MgF 2 , NaF. Insol. in H 2 0. (Geuther, J. B. 1865. 173.) Magnesium stannic fluoride. See Fluostannate, magnesium. Magnesium titanium fluoride. See Fluotitanate, magnesium. Magnesium zirconium fluoride. See Fluozirconate, magnesium. Magnesium hydrosulphide, MgS 2 H 2 . Known only in aqueous solution, which decomposes on warming. Solution contain- ing 16% MgS 2 H 2 has sp. gr. 1.118 at 12. (Divers and Shimidzu, Chem. Soc. 46. 699.) Magnesium hydroxide, MgO 2 H 2 . MgO is sol. in 55,368 pts. EbO at ordinary temp., and also at 100. (Fresenius, A. 59. 117.) MgO is sol. in 5142 pts. H 2 O at 15.5 (Fyfe) ; in 5800 pts. at 15.8 (Henry, J. Pharm. 13. 2) ; in 7900 pts. (Kir- wan) ; in 16,000 pts. (Dalton); in 100,000-200,000 pts. cold H 2 O (Bineau); in 36,000 pts. boiling HaO (Fyfe, Ed. Phil. J. 5. 305.) Calculated from electrical conductivity of MgO 2 H 2 +Aq, 1 1. H 2 O dissolves 9 mg. MgO 2 H 2 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) Calculated from electrical conductivity, 1 1. H 2 O dissolves 00.076 g. MgO 2 H 2 at 18. (Dupre* and Brutus, Z. angew. Ch. 1903, 16. 55.) Presence of CaO 2 H 2 or CaSO 4 does not de- crease the solubility. (Henry.) Presence of the salts of the alkali metals, especially am- monium salts, increase the solubility. Insol. in cone. Na 2 SO 4 , NaNO 3 , NaCl, or KNO 3 + Aq. (Karsten.) Sol. in NH 4 OH+Aq, but insol. in KOH+Aq. (Odling.) Easily sol. in acids. Sol. in an aqueous solution of sugar. Boiling alcohol dissolves traces. MAGNESIUM IODIDE 473 Solubility of MgO 2 H 2 in NH 4 Cl+Aq at 29. ai ISI 0.7 0.466 0.35 I 0.23 [0.17 1121 0.09835 0.1108 0.09835 0.1108 0.1108 Normality of MgOsH, NH 4 C1 0.156 0.108 0.089 . 0638 0.049 0.388 0.250 0.172 0.106 0.0771 G. per 1. MgO*H 8 NH 4 C1 4.55 3.15 2.60 1.86 1.43 20.86 13.39 9.21 5.67 4.13 (Herz and Muhs, Z. anorg. 1909, 38. 140.) Solubility of MgO 2 H 2 in NH 4 NO 3 +Aq at 29. Cone of NH 4 NOs +Aq (Nor- mal) Acid re- quired for liber- ated NH 3 in 25cc. (Normal) Normality of G. per 1. MgO 2 H 2 NH 4 NO 3 MgOjHj NH 4 N0 3 0.35 0.175 0.1108 0.1108 0.0833 0.0495 0.1834 0.076 2.43 1.45 14.69 6.09 (Herz and Muhs.) ^"Completely insol. in 16% NaCl+Aq in presence of 0.8 g. NaOH. (Maigret, Bull. Soc. (3) 33. 631.) Solubility of MgO 2 H 2 in NaCl+NaOH+Aq. G. NaCl per 1. G. MgO per 1. of solution with added 0.8 g. NaOH per 1. 4.0 g. NaOH per 1. 125 140 160 0.07 0.045 None 0.03 None (Maigret.) Freshly pptd. Mg(OH) 2 is sol. in Th(NO 3 ) 4 +Aq forming a colloidal solution. (Halla, Z. anorg. 1912, 79. 262.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II, 1014.) See also Magnesium oxide. Min. Brucite. Sol. in cold citric acid+Aq. (Bolton, C. N. 37. 14.) 2MgO, 3H 2 0. (Bender, B. 3. 932.) Magnesium iodide, MgI 2 . Very deliquescent. Solubility in H 2 O. See MgI 2 +6, and 8H 2 O. Sp. gr. of MgI 2 +Aq at 19.5 containing: '5 10 15 20 25 30%MgI 2 , 1.043 1.088 1.139 1.194 1.254 1.32 35 40 45 50 55 60% MgI 2 . 1.395 1.474 1.568 1.668 1.78 [1.915 (Kremers, Pogg. 111. 62, calculated by Gerlach, Z. anal. 8. 285.) MgI 2 +Aq decomp. slightly on evaporation. Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. in alcohol, ether, and wood-spirit. Solubility of MgI 2 in alcohols. MgI 2 forms with methyl alcohol a complex, MgI 2 , 6CH 3 OH. Solubility of MgI 2 , 6CH 3 OH in CH 3 OH at t. 20 40 60 80 100 % by weight of MgI 2 , CH 3 OH 49.6 52.6 55.3 58.0 60.6 63.3 120 140 160 180 200 j by weight of gls, 6CH 3 OH 66.2 69.5 73.2 77.1 81.5 (Menschutkin, Z. anorg. 1907, 52. 15.) MgI 2 forms with ethyl alcohol a complex, MgI 2 , 6C 2 H 5 OH. Solubility of MgI 2 , 6C 2 H 5 OH in C 2 H 5 OH at t. t % by weight of MgI 2 , 6C 2 H 5 OH t % by weight of MgI 2 , 6 C 2 H 5 OH 20 40 60 80 100 110 21.9 33.2 44.4 55.3 65.5 74.7 78.8 120 130 135 140 143 145 146.5 mpt. 82'. 7 87.2 90.0 93.3 96.0 98.0 100 (Menschutkin.) MgI 2 forms with dimethylcarbinol a com- plex, MgI 2 , 6(CH 3 ) 2 CHOH. Solubility of MgI 2 , 6(CH 3 ) 2 CHOH in (CH 3 ) 2 CHOH at t. t % by weight of MgI 2 , 6(CH S ) 2 CHOH t % by weight of MgI 2 , 6(CH 3 ) 2 CHOH 10 30 50 70 90 57.1 60.0 63.3 67.0 71.2 110 120 130 136 138 mpt. 76.2 79.4 84.8 91.7 100 (Menschutkin.) Solubility of MgI 2 in ether at t. t % MgI 2 % Mgls, 2C 4 HioO 5.4 11.8 15.6 18.1 20.4 22.2 1.45 2.43 3.46 5.4 7.55 11.28 2.2 3.7 5.3 8.3 11.6 17.3 (Menschutkin, Z. anorg. 1906, 49. 41.) 474 MAGNESIUM IODIDE t % MgI 2 % MgI 2 , 2C 4 HioO Solubility of MgI 2 in acetone. MgI 2 forms with acetone a complex, MgI 2l 6CH 3 COCH 3 . Solubility of MgI 2 , 6CH 3 COCH 3 in CH 3 COCH 3 at t. in lower layer 14.8 17.6 20 28.4 33 35 35.5 35.5 35.8 35.5 35.7 35.3 54.4 54.4 54.8 54.4 54.7 54.1 t % by wt. MgI 2) 6CH 3 COCH 3 30 50 60 70 80 85 90 95 100 105 106. 5 mpt. 4.9 6.7 8.3 10.2 15.2 28.6 40.0 59.2 80.0 92.5 98.5 100 in upper layer 18.6 23.2 24.4 32.4 13.57 14.4 14.6 15.82 20.8 22.1 22.4 24.2 in solution when two layers mix 37.3 38.5 38.5 38.5 38 19.4 22.45 26.07 29.8 32.8 29.3 34.4 39.9 45.7 50.3 (Menschutkin, Z. anorg. 1907, 53. 30.) Solubility of MgI 2 in acetal. MgI 2 forms with acetal a complex, MgI 2t 2CH 3 CH(OC 2 H 5 ) 2 . Solubility of MgI 2 , 2CH 3 CH(OC 2 H 6 ) 2 in CH 3 CH(OC 2 H 5 ) 2 at t. (Menschutkin.) Solubility of MgI 2 in acetic acid. MgI 2 forms with acetic acid a complex, MgI 2 , 6CH 3 COOH. Solubility of MgI 2 , 6CH 3 COOH in CH 3 COOH at t. t % by wt. MgI 2 , 2CH 3 CH(OC 2 H 5 ) 2 20 60 77 77 79 81 83 86 mpt. 0.15 0.45 .. 0.6 92.0 93.7 95.5 97.3 100 t % by wt. MgI 2 , GCHsCOOH 20 40 60 70 75 80 85 95 105 115 125 135 140 142 mpt. 0.6 2.0 5.0 9.5 13.0 18.5 27.1 42.0 54.5 65.0 73.8 85.0 94.0 100.0 (Menschutkin, Z. anorg. 1907, 53. 33.) Solubility of MgI 2 in acetamide. MgI 2 forms with acetamide a complex, MgI 2 , 6CH 3 CONH 2 . Solubility of MgI 2 , 6CH 3 CONH 2 in CH 3 CONH 2 a_t t. t % ^c& 12 ' 49 80 110 130 150 160 170 175 177 mpt. 56.5 63.4 70.5 76.0 82.1 85.5 90.8 96.2 100.0 (Menschutkin, Z. anorg. 1907, 54. 93.) (Menschutkin, Z. anorg. 1909, 61. 108.) MAGNESIUM IODIDE 475 Solubility of MgI 2 in acetonitrile. MgI 2 forms with acetonitrile a complex, MgI 2 , 6CH 3 CN. Solubility of MgI 2 , 6CH 3 CN in CH 3 CN att. Solubility of MgI 2 in methyl acetate. MgI 2 forms with ethyl acetate a complex, MgI 2 , 6CH 3 COOC 2 H 5 . Solubility of MgI 2 , 6CH 3 COOC 2 H 5 in CH 3 COOC 2 H 5 at t. t % by wt. MgI 2 , 6CH 3 CN t % by wt.MgI 2 , 6CH 3 COOC 2 H 5 30 50 70 80 89 37.2 ! 49.8 58.2 , . 67.9 76.5 91.3 20 40 50 55 60 65 70 75 78 . 5 mpt. 3.2 4.8 8.6 13.7 21.5 38.0 63.5 90.5 97.7 100.0 (Menschutkin, Z. anorg. 1909, 61. 110.) Solubility of MgI 2 in benzaldehyde. MgI 2 forms with benzaldehyde a complex, MgI 2 , 6C 6 H 5 CHO. ( M enschutkin . ) Solubility of MgI 2 , 6C 6 H 6 CHO in C 6 H 6 CHO att. (Menschutkin, Z. anorg. 1907, 53. 28.) Solubility of MgI 2 in methyl acetate. MgI 2 forms with methyl acetate a complex, MgI 2 , 6CH 3 COOCH 3 . Solubility of MgI 2 in ethyl formate. MgI 2 forms with ethyl formate a complex, MgI 2 , 6HCOOC 2 H 5 . t % by wt. MgI 2 , GCeHsCHO Solubility of MgI 2 , 6HCOOC 2 H 5 in HCOOC 2 H 5 at t. 3.2 20 40 3.8 5.3 t % by wt. MgI 2 , 6HCOOC 2 H 5 60 7.7 o I K 1 80 100 110 11.0 18.5 26.5 10 20 on 17.4 20.5 120 40.0 40 Q1 C 125 53.0 50 44 130 74.5 60 fiS 133 136 86.0 94.2 70.5 mpt. 100 139 mpt. 100 (Menschutkin.) Solubility of MgI 2 in isoamylacetate. MgI 2 forms with isoamylacetate a complex, MgI 2 , 6CH 3 COO(iso)C5Hn. Solubility of MgI 2 , 6CH 3 COO(iso)C 5 H u in CH 3 COO(iso)C 6 H u at t Solubility ol Mgi 2 , 6U1 3 (JUUCJ1 3 in CH 3 COOCH 3 at t. t % by wt. MgL>, 6CH 3 COO(iso)C 5 Hn t GCHsCOOCHs' 20 40 45 50 55 57.5 60 mpt. 7.7 11.5 20.9 25.5 33.2 47.8 63.0 100.0 30 60 90 100 103 103 110 120 121 mpt. 0.4 0.55 0.75 0.9 1.8 2.4 74.2 81.7 98.0 100.0 (Menschutkin.) Solubility of MgI 2 in isobutyl acetate. MgI 2 forms with isobutylacetate a com- plex, MgI 2 , 6CH 3 COOC 4 H 9 . (Menschutkin, Z. anorg. 1909, 61. 101.) 476 MAGNESIUM MERCURIC IODIDE Solubility of MgI 2 , 6CH 3 COO(iso)C 4 H 9 in CH 3 COO(iso)C 4 H 9 . +8H 2 O. Sp. gr. of solution of MgI 2 +8H 2 O sat. at 18 containing 59.7% MgI 2 = 1.909. (Mylius, B. 1897, 30. 1718.) Solubility of MgI 2 +8H 2 O in H 2 O at t. t % by wt. MgI 2 , 6CH 3 COO(iso)C4H 9 20 40 50 60 70 75 80 85 87.5mpt. 10.5 13.6 17.6 20.4 24.9 33.7 40.5 52.0 89.0 100.0 t % by weight of MgI 2 +8HzO 20 40 43.5 76.0 81.0 88.0 90.8 (Menschutkin.) +10H 2 0. Sol. in H 2 0. (Pdnfiloff, C. C. 1894, II. 610.) ( M enschutkin . ) Solubility of MgI 2 in propyl acetate. MgI 2 forms with propyl acetate a complex, MgI 2 , 6CH 3 COOC 3 H 7 . Solubility of MgI 2 , 6CH 3 COOC 3 H 7 in CH 3 COOC 3 H 7 at t. t % by wt. MgI 2 , 6CH 3 COOC 3 H7 4.1 20 5.4 30 6.5 35 7.8 40 19.0 45 46.0 50 72.5 55 88.2 60 96.0 65 mpt. 100.0 (Menschutkin.) Solubility of MgI 2 in urethane. MgI 2 forms with urethane a complex, MgI 2 , 6NH 2 COOC 2 H 6 . Solubility of MgI 2 , 6NH 2 COOC 2 H 5 in NH 2 COOC 2 H 5 at t. t % by wt. MgI 2 , 6NH 2 COOC 2 H 5 32 50 70 80 84 87 mpt. 51.8 59.4 70.7 78.8 85.0 100.0 (Menschutkin.) +6H 2 O. Solubility of MgI 2 +6H 2 O in H 2 O at t. t % by weight of , MgI 2 +6H 2 % by weight of MgI 2 +6H 2 43 80 120 89.8 160 90.3 200 90.9 215 91.7 93.4 94.3 (Menschutkin, Z. anorg. 1907, 52. 156.) Known only in solution. +9H 2 O. Very deliquescent. (Duboin, C. R. 1906, 142. 1338.) Very sol. in ethyl, methyl, propyl, butyl, isobutyl, amyl, isopropyl* and allyl alcohols, ethyl, amyl, propyl and isobutyl acetates, ethyl cyanide and acetone. Sol. in benzyl alcohol. Decomp. by glycerine. SI. sol. in ethyl benzoate, amyl benzoate, nitrobenzene. Decomp. by ethyl oxalate. Insol. in toluene, benzene, ethyl iodide, CHC1 3 , CC1 4 , ethylene bromide, monochlor and monobrombenzene. (Duboin, A. ch. 1909, (8) 16. 276.) MgI 2 , 2HgI 2 . -Decomp. by H 2 O into HgI 2 and above compound, which remains in solu- tion. (Boullay.) +7H 2 O. Sat. solution in H 2 O at 17.8 has the composition MgI 2 , 1.29 HgI 2 , 11.06 H 2 O. (Duboin, C. R. 1906, 142. 1338.) Magnesium potassium iodide, MgI 2 , KI + 6H 2 O. Deliquescent. (Lerch, J. pr. (2) 28. 338.) Very hygroscopic, (de Schulten, Bull. Soc. 1900 (3) 23. 158.) Magnesium iodide ammonia, MgI 2 , 6NH 3 . Practically insol. in liquid NH 3 . (Franklin, J. Am. Chem. Soc. 1913, 35. 1459.) Magnesium nitride, Mg 3 N 2 . Decomp. by moist air or H 2 O. Sol. in dil. or cone. HCl+Aq, or HNO 3 +Aq. Sol. in warm H 2 SO 4 . Insol. in alcohol, ethyl iodide, or phosphorus oxychloride. (Briegleb and Geuther, A. 123. 236.) Decomp. by H 2 O. (Smits, R. t. c. 1894, 12. 198.) Easily decomp. H 2 O when finely powdered. (Rossel, C. R. 1895, 121. 942.) Magnesium sw&oxide (?). Decomp. H 2 O. Sol. in dil. acids. (Beetz, Pogg. 127. 45.) Magnesium oxide, MgO. Sol. in 50,000-100,000 pts. H 2 O (Bineau, C. R. 41. 510) ; in 55,368 pts. cold or hot H 2 O (Fresenius, A. 59. 123) ; in 100,000-200,000 pts. H 2 O (Bunsen) ; in 16,000 pts. H 2 O at ord. temp. (Dalton) ; in 7900 pts. H 2 O at ord. temp. (Kirwan) ; in 5760 pts. H 2 O at 15.5, and 36,000 pts. at 100 (Fyfe). MAGNESIUM OXYSULPHIDE 477 Calc. from electrical conductivity of MgO +Aq. 1 pt. MgO is sol. in 172,000 pts. H 2 O at 18. (Dupre", Zeit. angew. Ch. 1903, 16. 55.) "Heavy" MgO is more sol. in H 2 O than "light" MgO. The temp, of preparation affects the rate of solution, the rate being diminished as the temp, of preparation is increased. (Anderson, Chem. Soc. 1905, 87. 265.) Easily sol. in acids, even in H 2 SO 3 +Aq. Solubility in P 2 O 5 +Aq at 25. Composition of the solution * Solid phase G. MgO perl. G. P205 perl. 0.207 0.486 0.280 0.732 0.553 1.917 1.438 4.85 2.23 7.35 1^006 4.73 16.84 1.017 11.19 38.59 1.042 17.33 61.21 1.069 26.09 37.40 75.5 93.09 130.7 281.8 1.109 1.144 1.285 MgHP0 4 , 3H 2 109.5 439.0 122.6 498.4 1.470 129.9 546.5 140.0 584.0 146.8 623.3 l!595 147.3 625.9 150.3 645.8 155.5 680.7 87.1 77.1 779.6 809.6 l'.626 1.644 MgH 4 (P0 4 ) 2 , 70.6 835.1 1.654 . x 2 (Cameron, J. phys. Chem. 1907, 11. 364.) Sol. in NH 4 salts, NaCl, or KCl+Aq. (Fresenius.) Solubility in MgCl 2 +Aq at 25. % MgCU % MgO as Mg(OH) 2 2.36 0.00008 4.47 0.00028 6.79 0.00048 9.02 0.00080 13.14 0.00115 15.15 0.00195 17.53 . 0.00240 18.52 0.00250 22.04 0.00245 23.78 0.00235 25.13 0.00230 26.88 0.00250 28.34 0.00230 29.80 0.00240 30.04 0.00250 34.22 0.0030 (Robinson, J. phys. Chem. 1909, 13. 676.) More sol. in K 2 SO 4 , and Na 2 SO 4 +Aq than in H 2 O. (Warrington.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. in methyl alcohol to form a colloidal solution containing 1.6% MgO. (Neuberg and Rewald. (Biochem. Z. 1908, 9. 547.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3602.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Solubility in (calcium sucrate+ sugar) + Aq. 1 1. solution containing 418.6 g. sugar and 34.3 g. CaO dissolves 0.30 g. MgO; contain- ing 296.5 g. sugar and 24.2 g. CaO dissolves 0.24 g. MgO; containing 174.4 g. sugar and 14.1 g. CaO dissolves 0.22 g. MgO. (Boden- bender, J. B. 1865. 600.) See also Magnesium hydroxide. Min. Periclasite. Magnesium peroxide, MgO 2 . Sol. in 14,550 pts. H 2 O at 20. (Foregger and Philipp, J. Soc. Chem. Ind. 1906, 26. 298.) 5MgO,2MgO 2 +3H 2 O. 3MgO, 2MgO 2 +3H 2 O. 2MgO,2MgO 2 +3H 2 O. 4MgO,2MgO 2 +3H 2 O. Above salts are decomp. by H 2 O. (Carrasco, Gazz. ch. it. 1909, 39, (1) 47.) Magnesium oxybromide, MgBr 2 , 3MgO -f 12H 2 0. Decomp. in the air and also by H 2 O, al- cohol and most reagents. (Tassilly, C. R. 1897, 126. 607.) Magnesium oxychloride, Mg 2 OCl 2 + 16H 2 O. Easily decomp. by H 2 O and alcohol. (Andre, A. ch. (6) 3. 80.) +6H 2 O. (Andre.) 2MgO, HC1, 5H 2 O or 3MgO, MgCl,+ 10H 2 O. Solubility determinations show that this salt is the solid phase in equilibrium at 25 with solutions of MgCl 2 and MgO con- taining from 10-15% MgCl 2 . (Robinson, J. phys. Chem. 1909, 13. 677.) Mg 6 O 5 Cl 2 +6, 8, 14, or 17H 2 O. Decomp. by H 2 O, which dissolves out MgCl 2 . (Ben- der, B. 3. 932.) Mg n O 10 Cl 2 +14, or 18H 2 O. (Krause, A. 166. 38.) Mg,oO 9 Cl 2 + 24H 2 O = 9MgO, MgCl 2 + 24H 2 O. H 2 O removes all MgCl 2 by long di- gesting. (Bender, A. 159. 341.) + 10, and 15H 2 O. (Bender.) Magnesium oxysulphide, Mg 2 OS. (Reichel, J. pr. (2) 12. 55.) 478 MAGNESIUM PHOSPHIDE Magnesium phosphide, Mg 3 P 2 . Decomp. by H 2 O, dil. HCl+Aq, or HNO 3 +Aq. (Parkinson, Chem. Soc. 5. (2) 125 and 309.) Insol. in moderately dil. cold HCl+Aq, or boiling dil. H 2 SO 4 +Aq. Difficultly and slowly sol. in aqua regia. (Blunt, Chem. Soc. 3. (2) 106.) Decomp. by H 2 O, HC1, cone. H,SO 4 and by HXO 3 . (Gautier, C. R. 1899, 128. 1169.) Magnesium silicide, MgsSi 3 . Slowly decomp. by warm H 2 O. Slowly decomp. by cold, rapidly by hot NH 4 Cl+Aq. Decomp. by cold dil. HCl+Aq. (Geuther, J. pr. 95. 425.) MgsSi. Decomp. by HCl+Aq with residue of Si. (Wohler, A. 107. 113.) Slowly decomp. by H 2 O at ord. temp. Violently decomp. by HC1. (Lebeau and Bossuet, C. R. 1908, 146. 284.) Magnesium sulphide, MgS. Decomp. by H 2 O. (Rachel, J. pr. (2) 12. 55.) SI. sol. in H 2 O with rapid decomp. (Fremy.) Sol. in acids with decomp. Anhydrous. Crustattine. Only very si. sol. in cold H 2 O. Sol. in HNO 8 and HjSO 4 at ord. temp. Sol. in PCls and in chromyl chlor- ide. (Mourlot, C. R. 1898, 127. 182.) Magnesium poZysulphide, MgSj. Known only in solution. (Rachel.) Magnus' green salt. See Platcxftamine chloroplatmite. Manganese, Mn. Decomposes H 2 O even in the cold, more rapidly when hot. (Regnault.) Decomposes cold water violently. (Bun- sen.) Sol. in all dil. acids. Slowly sol. in cold HjjSO,. (John.) Insol. in cold, but rapidly sol. in hot H 2 SO 4 . Very easily sol. in dil. HzSO 4 , or HCl+Aq, HNO 3 , or HC 2 H 3 O 2 +Aq. (Brunner.) Pure manganese is unaltered in dry air, even when finely powdered. Slowly attacked by cold, quickly by hot H 2 O. Very si. at- tacked by cold H 2 SO 4 , rapidly on warming; rapidly attacked by cold dil. H 2 SO 4 +Aq; violently by cone. HNO 3 +Aq; and rapidly by dil. HN0 3 , HC1, HC 2 H 3 O 2 +Aq, and also NaOH+Aq. Sol. in NH 4 Cl+Aq. (Pre- linger, W. A. B. 102, 2b. 359.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) ^2 ccm. oleic acid dissolves 0.0276 g. Mn in 6 days. (Gates, J. phys. Chem. 1911, 15. 14o.) Manganese antimomde, MnSb. Sol. in hot aqua regia. (Wedekind, B. 1907, 40. 1266.) Manganese azoimide, basic, Mn(OH)N 3 . Only si. sol. in H 2 O with decomp. (Cur- tius, J. pr. 1898, (2) 58. 293.) Manganese bismuthide, MnBi. Very sensitive towards acids with the exception of cone. HC1. (Wedekind, B. 1911, 44. 2665.) Manganese boride, MnB. Attacked by cold H 2 O and by acids. ( Jas- soneix, C. R. 1904, 139. 1210.) Easily attacked by HC1, H 2 SO 4 and HF with evolution of BH 3 . (Wedekind, B. 1905, 38. 1231.) MnB 2 . Sol. in acids, with evolution of H 2 . (Troost and Hautefeuille, A. ch. (5) 9. 65.) Slowly decomp. by H 2 O. Sol. in dil. HC1 and other dil. acids with evolution of BH 3 . (Wedekind, B. 1905, 38. 1229.) Manganous bromide, MnBr 2 . Anhydrous. Very deliquescent. Sat. MnBr 2 +Aq contains at: 21 +7 11 18 38 52 52.1 56.5 57.0 59.1 62.7 64.2% MnBr 2 , 64 76 89 97 105 68.2 70.1 69.7 69.2 70.2% MnBr 2 . (fitard, A. ch. 1894, (7) 2. 541.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) +H,O. (Lescoeur, A. ch. 1894, (7) 2. 104.) +4H 2 O. More deliquescent than MnCl 2 . Melts in crystal water when heated. (Berthe- mot.) +6H 2 0. (Kuznetzoff, C. C. 1897, II. 329.) Manganous mercuric bromide. Deliquescent. Manganous palladium bromide. See Bromopalladite, manganous. Manganous stannic bromide. See Bromostannate, manganous. Manganese carbide, MnC. (Brown, J. pr. 17. 492.) MnC 2 . Mn 3 C. (Troost and Hautefeuille, A. ch. (5) 9. 60.) Decomp. by H 2 O and by dil. acids. (Mois- san, C. R. 1896, 122. 422.) Manganous chloride, MnClz. Anhydrous. Deliquescent. MAXGAXOUS CHLORIDE 479 100 pts. H 2 O at t dissolve pts. MnCl 2 : Pts. MnCl 2 Pts. MnCU Sp. gr. of MnCl 2 +Aq at room temp. MnCl 2 Sp. gr. 10 31.25 62.5 62.16 85.72 122.22 87.5 106.25 122.22 123.81 or, sat. MnCl 2 +Aq at t contains: 8.007 15.650 30.330 40.132 1.0960 1.1963 1.3372 1.4530 t % MnClz t % MnCU 10 31.25 62.5 38.33 46.15 55.0 87.5 106.25 55.0 55.32 (Wagner, W. Ann. 1883, 18. 273.) Sp. gr. of MnCl 2 +Aq at t' (Brandes, Pogg. 22. 263.) See also below under +2H 2 O, and +4H 2 O. Sp. gr. of MnCl 2 +Aq at 15. a=sp. gr. if % is MnCl 2 ; b=sp. gr. if % is MnCl 2 + 4H 2 0. t % MnCli Sp. gr. 14.5 14.5 14.0 14.5 14.0 14.6 5.0 11.99 14.98 19.92 23.10 28.51 1.0457 1.1076 1.1379 1.1891 1.2246 1.2888 5 10 15 20 25 30 35 1.045 .091 .138 .189 .245 .306 1.372 1.0285 1.057 1.086 1.116 1.147 1.180 1.214 40 45 50 55 60 65 70 1.443 1.514 1.250 .290 .331 .375 .419 .463 .508 (Long, W. Ann. 1880, 11. 38.-) Sp. gr. of MnCl 2 +Aq at 25. Concentration of MnClz +Aq 1-normal Vr- " V<- " Vr- " Sp. gr. 1.0513 1.0259 1.0125 1.0063 (Gerlach, Z. anal. 28. 476.) (Wagner, Z. phys. Ch. 1890, 5. 38.) Solubility of MnCl 2 +KCl in HO at t. t % MnCl. %KC1 Solid phase 6 40.23 35.94 9^41 23.06 MnCl 2 , 4H 2 O MnCl 2 , 4H 2 0+MnCl 2 , KC1, 2H S O+KC1 KC1 28.4 44.46 43.28 38.65 8^66 13.79 26.91 MnCl 2 , 4H 2 O MnClj, 4H 2 O+MnCl 2 , KC1, 2H,O MnCl 2 , 4H,0+MnCl 2 , 2KC1, 2H 2 O+KC1 KC1 52.8 50.14 6.01 MnCl 2 , 4H 2 O+MnCl 2 , 2H 2 O+MnCl 2 , KC1, 2H 2 O 62.6 51.86 49.95 44.05 36.85 6".67 12.49 18.77 31.57 MnCl 2 , 2H 2 MnCl 2 , 2H 2 0+MnCl 2 , KC1, 2H 2 O MnCl 2 , KC1, 2H 2 0+MnCl 2 , 2KC1, 2H 2 O MnCl 2 , 2KC1, 2H 2 O+MnCl 2 , 4KC1 KC1 (Suss, Z. Kryst. Min. 1912, 51. 262.) Insol. in liquid XH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Solutions of MnCl 2 in 75% alcohol saturated at t contain: t % MnCU t % MnCli 10 25 23.1 36.1 43.75 87.5 (B.-pt.) 37.5 32.2 480 MANGANESE CHLORIDE Solutions of MnCl 2 in rated at t absolute alcohol satu- contain: Sat. aq. solution contains at: 22 5 +7 17 19 34.7 37.8 40.4 41.2 42.3% MnCl 2 35 55 57 80 100 140 44.4 48.2 50.0 51.0 53.7 54.7% MnCl 2 . (fitard, A. ch. 1894, (7) 2. 537.) Solubility in H 2 O at t. t % MnCl 2 t % MnCl 2 11.25 37.5 33.3 33.3 76.25 (B.-pt.) 36.2 (Brandes, I. c.) MnCl 2 crystallises from above solutions on standing. When 15-20 vols. ether are added to 1 vol. absolute alcohol sat. with MnCl 2 , MnCl 2 is completely pptd. (Dobereiner.) Insol. in oil of turpentine. Sol. in urethane. (Castoro, Z. anorg. 1899, 20. 61.) SI. sol. in .benzonitrile. (Naumann, B. t Pts. MnCh per 100 pts. H 2 O Sp. gr. of sat. solution 25 30 40 50 *57.65 77.18 80.71 88.59 98.15 105.40 1.4991 1.5049 1.5348 1.5744 1.6097 1914, 47. 1369.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910. 43. 314.) +H 2 O. Solubility in HCl+Aq decreases with increasing amt. of HC1. It is greater when hot than cold, but is not inconsiderable even when HC1 is cone. 1 1. cone. HCl+Aq sat. at 12 dissolves 190 g. MnCl 2 from MnCl 2 +H 2 O. (Ditte, C. R. 1881, 92. 243.) + 5 /3H 2 O. MnCl 2 +4H 2 O effloresces to MnCla+VsHaO in a dry atmosphere and under low pressure and not to MnCl 2 + 2H 2 O. (Sabatier, Bull. Soc. 1894, (3) 11. 547.) +2H 2 0. Solubility in H 2 O at t. 60 70 80 Pts. MnCl 2 per 100 pts. H 2 O 108.6 110.6 112.7 Sp. gr. of sat. solution 1.6108 1.6134 (Dawson and Williams, Z. phys. Ch. 1899, 31. 63.) Sat. aqueous solution of MnCl 2 +2H 2 O. Contains 51.86% MnCl 2 at 62.6. (Suss. Z. Krist. 1912, 61. 262.) +4H 2 O. Deliquescent. 100 pts. H 2 at t dissolve: t Pts. MnCh +4H 2 O t Pts. MnCh +4H 2 8 31.25 62.5 151 265 641 87.5 106.25 641 656 (Brandes, I. c.) Sol. in 0.8 pt. H 2 O at 18.75. (Abl.) Pptd. from solution in 9.17 mols. (Kuznetzoff, C. C. 1899, I. 246.) H 2 O *Temp. of transition into MnCl 2 +2H 2 O. (Dawson and Williams, Z. phys. Ch. 1899, 31. 63.) Sat. aqueous solution of MnCl 2 +4H 2 O contains 40.23% MnCl 2 at 6; 44.6% MnCl 2 at 28.4. (Sites, Z. Krist. 1912, 51. 262.) 100 pts. 75% alcohol dissolve at t: 10 25 Pts. MnCh +4H 2 53 132 43.75 87.5 Pts. MnCl 2 +4H 2 O 144 100. (Brandes, I. c.) Insol. in absolute ether, which also does not abstract crystal H 2 O. Insol. in boiling oil of turpentine. (Brandes. Sol. in cone. HNO 3 +Aq. +5H 2 O. (Muller-Erzbach, B. 1889, 22. 3181.) +6H 2 O. Pptd. from solution in 11.7 mols. H 2 O at 21. (Kuznetzoff, C. C. 1899, I. 246.) Manganese ^nchloride, MnCl 3 . Immediately decomp. by H 2 O; sol. in abs. ether and in abs. alcohol. (Holmes, J. Am. Chem. Soc. 1907, 29. 1285.) Manganese teZrachloride, MnCl 4 . Has not been isolated. Sol. in H 2 O, alcohol, or ether. (Nickles, J. B. 1866. 225.) Composition is Mn 2 Cl 6 . (Christensen, J. pr. (2) 34. 41.) Manganese hydrogen tetraddoride (chloro- manganic acid), MnCl 4 , 2HC1. Sol. in ether; decomp. by H 2 O. (Franke, (2) 36. 31.) Manganese Tieptachloride, MnCl 7 (?). Decomp. by H->O. (Dumas, Berz. J. B. 7. 112.) MANGANIC SODIUM FLUORIDE 481 Has the formula MnO 3 Cl (?). (Aschoff, J. pr. 81. 29.) Manganous mercuric chloride, MnCl 2 , HgCl 2 +4H 2 0. Deliquescent in moist air. Easily sol. in H 2 O. (v. Bonsdorff.) MnCl 2 , 2HgCl 2 . (Varet, C. R. 1896, 123, 422.) Manganous potassium chloride, MnCl 2 , KC1 +2H 2 O. Deliquescent. Very sol. in H 2 O, but is decomp. thereby. (Remsen and Saunders, Am. Ch. J. 14. 129.) MnCl 2 , 2KC1+2H 2 O. (Suss, Z. Kryst. 1912, 51. 262.) Manganic potassium chloride, MnCl s , 2KC1+ H 2 O. Decomp. by H 2 O. Sol. in HC1 apparently without decomp. (Rice, Chem. 73. 261.) >c. 1898, MnCl 4 , 2KC1. Very easily decomp. (Meyer and Best, Z. anorg. 1899, 22. 186.) nC! 4 , MnCl 3 , 5KC1. Easily decomp. (Meyer and Best, Z. anorg. 1899, 22. 185.) Manganous rubidium chloride, MnCl 2 , 2RbCl. (Godeffroy.) +3H 2 O. Easily sol. in H 2 O. Insol. in alcohol; cone. HCl+ppt. anhydrous salt from aqueous solution. (Godeffroy, Arch. Pharm. (3) 12. 40.) Contains only 2H 2 O. (Saunders, Am. Ch. J. 14. 139.) Manganous thallic chloride, MnCl 2 , 2T1C1 3 + 6H 2 O. Can be cryst. from H 2 O. (Gewecke, A. 1909, 366. 224.) Manganous stannic chloride. See Chlorostannate, manganous. Manganous chloride hydrazine, MnCl 2 , 2N 2 H 4 . Ppt. (Franzen, Z. anorg. 1908, 60. 285.) Manganous chloride hydroxylamine. MnCl 2 , 2NH 2 OH. Very stable: insol. in alcohol. (Feldt, B. 1894, 27. 405.) Manganous fluoride, MnF 2 . Only sol. in H 2 O containing HF. (Ber- zelius.) Insol. in H 2 O; decomp. by boiling with H 2 O; si. sol. in liquid NH 3 ; easily sol. in cold or hot cone. HNO 3 and HC1; slowly sol in dil. HC1; decomp. by fused K 2 CO 8 , KOH, KNO 3 , and KC1O 3 ; insol. in alcohol and ether. Slowly sol. in acetic acid. (Moissan, C. R. 1900, 130. 1160.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Manganese Znfluoride, MnF 3 . Completely sol. in a little H 2 O, but decomp. by dilution or boiling. (Berzelius.) -H>H 2 O. Efflorescent. (Christensen, J. pr. (2) 35. 57.) Sol. in H 2 SO 4 , HC1, HNO 3 ; decomp. by H 2 0; insol. in most organic solvents. (Mois- san, C. R. 1900, 130. 626.) Manganomanganic fluoride, Mn 3 F8+10H 2 O. Sol. in a little H 2 O, but decomp. by dilu- tion. (Nickles, C. R. 67. 448.) Manganese tefrafluoride, MnF 4 . Not isolated. Sol. in absolute alcohol or ether; decomp. by H 2 O. (Nickles, C. R. 65. 107.) Probably does not exist. (Christensen, J. pr. (2) 35. 161.) Manganese Aeptafluoride, MnF 7 (?). Sol. in H 2 O with decomp. (Wohler.) Manganese sesquiftuoride with MF. See also Fluomanganate, M. Manganic nickel fluoride, 2NiF 2 , Mn 2 F 6 + 8H 2 O. (Christensen, J. pr. (2) 34. 41.) Manganic potassium fluoride, Mn 2 F 6 , 4KF+ 2H 2 0. Decomp. by H 2 O. Sol. in cone. HCl+Aq, dil. HNO 3 +Aq, cone. H 2 SO 4 +Aq, H 3 PO 4 + Aq, H 2 C 2 O 4 +Aq, H 2 C 4 H 4 O 6 + Aq, and dil. HF+Aq. (Christensen, J. pr. (2) 35. 72.) MnF 4 , 2KF. Difficultly sol. in H 2 O. De- comp. by much H 2 O. (Nickles, C. R. 65. 107.) True composition is Mn 2 F 6 , 4KF, also with 2H 2 O. (Christensen, J. pr. (2) 34. 41.) MnF 4 , 4KF. (Nickles.) See also Fluomanganate, potassium. Manganic rubidium fluoride. See Fluomanganate, rubidium. Manganic silver fluoride, 2AgF, Mn 2 F 6 + 14H 2 O. Sol. in HF+Aq. (Christensen, J. pr. (2) Manganic sodium fluoride, Mn 2 F 6 , 4NaF. Decomp. by much H 2 O. Not as sol. in HF +Aq as the K salt. (Christensen, J. pr. (2) 35. 161.) 482 MANGANOMANGANIC THALLOUS FLUORIDE Manganomanganic thallous fluoride, 5T1F, 2MnF 3 , MnF 2 . Decomp. by H 2 O. SI. sol. in dil., easily sol. in cone. HF. Sol. in cone. HC1, dil. HNO 3 , and cold or hot cone. H 2 SO 4 . Sol. in warm H 2 O 2 containing H 2 S0 4 . Sol. in dil. tartaric and oxalic acids. (Ephraim, B. 1909, 42. 4458.) Manganous stannic fluoride. See Fluostannate, manganous. Manganic zinc fluoride, 2ZnF 2 , Mn 2 F 6 +8H 2 O See Fluomanganate, zinc. Manganous zirconium fluoride. See Fluozirconate, manganous. Manganous fluoride ammonia, 3MnF 2 , 2NH 3 . (Moissan, C. R. 1900, 130. 1161.) Manganous hydroxide, MnO 2 H 2 . 2.15 x 10- 5 g.-mol. are sol/, in 1 1. H 2 O at 18. (Sackur, Z. Elektrochem, 1909, 15. 846.) Solubility in H 2 O =0.6 x 10~ 4 g. mol. (Herz, Z. anorg. 1899, 22. 284.) 1 1. H 2 O dissolves 2 x 10~ 4 mol. MnO 2 H 2 . (Tamm, Z. phys. Ch. 1910, 74. 500.) Very si. sol. in H 2 O or alkalies. (Fresen- ius.) Easily sol. in acids. Insol. in NaOH, orKOH+Aq. Sol. in NH 4 salts +Aq. Insol. in NH 4 OH+Aq. Sol. in NaOH+Aq in presence of glycerine. (Donath, Dingl. 229. Not pptd. by NH 4 OH+Aq in presence of H 2 C 4 H 4 O e ; by KOH+Aq in presence of cane sugar; by KOH+Aq in presence of Na citrate. Solubility of MnO 2 H 2 in organic Na salts + Aq. (0.5 normal.) Na tartrate, 0.0068 mol. per 1. Na malate, 0.0042 " " " Na citrate, 0.0126 " " " (Tamm, Z. phys. Ch. 1910, 74. 496.) Min. Pyrochroite. Manganomanganic hydroxide, Mn 3 O 4 , #H 2 O. Not attacked by boiling NH 4 Cl+Aq. Be- haves towards acids as Mn 2 O 3 . Manganic hydroxide, Mn 2 O 3 , H 2 O. Insol. in hot or cold dil. H 2 SO 4 +Aq. Sol. in cone. H 2 SO 4 at somewhat over 100. ; in HXQ* aad Hd-f-Aq. Xot KOHHrAq. Drccnp. by KO, X Aq. (ffiMiiMniA,FqBB-4aLl&Lj> -A: soL by 2HCL Conceit ftwmpiMftioii of mereim snide chloride. fTBaksfra, Gazz. eh. it M, *S?L. Decamp, by B^O. XHsiCL HCL Decomp. by HdO. Ba- --, . : fflOL SoLinHdO. (Ray,Froe. by HaO, ndflj by KOH+Aq. A. eh. 1911 r (8) tt. 212L) Fpt. SoL in HBr. f Biy, Ftoe. Soe. 1902, 1BL ofwhathasbeenealled Bm- Inaol.VeoH'SttHnp. by hot H4) (M3^ n, A. eh. (3) 18. 413.) SoL in GOO pta. HjO. (Wittrtein.) SoL in 719.98 pts. H^OatlS.75". (AbL) InsoL in aleohoL SoL in acids, even in HCJBdOx+Aq, abo in XH^XO^ (X^)j^O^, and Aq. (Pekmze and Fremy.) Oto*t) m SI soL in alkali ehlorides+Aq, which par- tially decamp. Miahle, A. eh. (3) 6. 180.) Decomp. by KOH-f Aq. SoL in KI, or NaAO,+Aq, with evolution of XH^ (Ba- lesbn.) When freshly prepared is soL in o XH/JH-rAq. (Saha and Choudhuri, 1910, 67. 359.) in excess of . (Hofmann and Marburg, A. 1899, 905. 212.) SL soL in HXO,. (Bay, Z. anorg. 1902, 33.209.) ammonium nitrate, NHgjNOj, +H,0. Correct formula for mercuriammonium nitrate, XHjHgXOj-h^iHjO. (Pesci, Gaxx. ch. it. 20. 485.) XHg 2 XO,, 2NH4NO,+2HsO. Correct for- 490 MERCURIAMMONIUM NITRITE mula for oxy^'mercuriammonium ammonium nitrate, (NHg 2 OH 2 )NO 3 , 2NH 4 NO 3 +H 2 O. (Pesci.) NHg 2 N0 3 , 3NH 4 N0 3 . Decomp. by cold H 2 O; sol. in NH 4 OH+Aq. (Pesci.) 3NHg 2 NO 3 , NH 4 NO 3 +2H 2 O. Correct for- mula for mercuriammonium oxyrftmercuriam- monium nitrate, NH 2 HgNO 3 , (NHg 2 OH 2 )NO 8 +H 2 O. (Pesci.) Di'mercuriammonium nitrite, NHg 2 NO 2 . Readily sol. in warm HC1 or HBr. (Ray, Chem. Soc. 1902, 81. 648.) + 3/H 2 O. Ppt. SoLinHCl. (Ray, Proc. Chem. Soc. 1902, 18. 85.) +H 2 O. (Hofmann and Marburg, A. 1899, 305.214.) oxide, (NHg 2 ) 2 0. Slowly decomp. by H 2 O. Sol. in HC1, or HNO 3 +Aq. Decomp. by hot KOH, or KC1 +Aq. (Weyl, Pogg. 121. 601.) Sol. in KCN+Aq by heating 4-5 hours at 130. Not completely sol. in HC1 owing to formation of Hg 2 Cl 2 . (Gaudechon, C. R. 1907, 144. 1419.) phosphate, (NHg 2 ) 2 PO 4 , 2NHg 2 OH + 10H 2 0. (Rammelsberg, J. pr. (2) 38. 567.) Sec Oxycfo'mercuriammonium phosphate. ammonium salicylate, 2NHg 2 C 6 H 4 OHCO 2 , 5NH 4 C 6 H 4 OHCO 2 . Decomp. by H 2 O. Sol. in NH 4 C 2 H 3 O 2 , HC1, or KI+Aq. (Balestra.) selenate, (NHg) 2 SeO 4 +2H 2 O. Ppt. Insol. in H 2 O; sol. in NH 4 OH+Aq. (Cameron and Davy, C. N. 44. 63.) sulphate, (NHg 2 ) 2 SO 4 +2H 2 O. Insol. in H 2 O. Easily sol. in HCl+Aq. (Rammelsberg, J. pr. (2) 38. 565.) Sol. (Kane), insol. (Hirzel) in HNO 3 +Aq. Sol. in KI, or Na 2 S 2 O 3 +Aq with evolution of NH 3 . (Balestra.) +H 2 O. Insol. in H 2 O; sol. in HC1. (Ray, Chem. Soc. 1905, 87. 9.) ammonium sulphate, (NHg 2 ) 2 SO 4 , 3(NH 4 ) 2 SO 4 +4H 2 O. Correct formula for mercuriffo'ammonium sulphate, 2NH 3 , HgO, SO 3 +H 2 O. (Pesci, Gazz. ch. it. 20. 485.) 5(NHg 2 ) 2 SO 4 , 14(NH 4 ) 2 SO 4 +16H 2 O. (Pesci.) 7(NHg 2 ) 2 S0 4 , (NH 4 ) 2 S0 4 + 12H 2 0. Cor- rect formula for mercuriammonium oxycfo'mer- curiammonium sulphate, (NHg 2 H 2 ) 2 SO 4 , 3(NHg 2 OH 2 ) 2 SO 4 . (Pesci.) Dimercuriannnonium tartrate, (NHg 2 ) 2 C 4 H 4 6 +2^H 2 0. Insol. in H 2 O. Sol. in HC1, KI, Na 2 S 2 O 3 , NH 4 C 2 H 3 O 2 , or (NH 4 ) 2 C 4 H 4 O 6 +Aq. (Bal- estra, Gazz. ch. it. 22, 2. 563.) ammonium tartrate, 2(NHg 2 ) 2 C 4 H 4 O 6 , (NH 4 ) 2 C 4 H 4 6 +H 2 0. As above. (B.) Tnmercuriammonium sulphate, (NHg 2 )(NHgH 2 )S0 4 +2H 2 0. Decomp. by H 2 O. (Millon.) Does not exist. (Pesci, Gazz. ch. it. 20. 485.) Dimercuriarsonium mercuric chloride, AsHg 3 Cl 3 =AsHg 2 Cl, HgCl 2 . Decomp. by H 2 O. Decomp. by warm HNOs+Aq. (Rose, Pogg. 51. 423.) Mercurimidosulphonic acid, (H0 3 S) 4 N 2 Hg. Very unstable. (Berglund, B. 9. 256.) Barium mercurimidosulphonate, Ba 2 (S0 3 ) 4 N 2 Hg+5H 2 0. (Berglund, B. 9. 256.) Cadmium , Cd 2 HgN 2 (SO 3 ) 4 +12H 2 O. Unstable; si. sol. in H 2 O. (Berglund, Bull. Soc. (2) 25. 452.) Cobalt , Co 2 HgN 2 (SO 3 ) 4 +15H 2 O. Sol. inH 2 O. (B.) Copper , Cu 2 HgN 2 (SO 3 ) 4 + 15H 2 O. Very sol. in H 2 O. (B.) Magnesium , Mg 2 HgN 2 (SO 3 ) 4 +15H 2 O. Very sol. in H 2 O. (B.) Manganous , Mn 2 HgN 2 (SO 3 ) 4 +10B[ 2 O. Unstable. (B.) Mercuric , (Hg 2 O) 2 HgN 2 (SO 3 ) 4 . Nearly insol. in H 2 O. (B.) Nickel (B.) -, Ni 2 HgN 2 (S0 3 ) 4 + 15H 2 0. Potassium , (KO 3 S) 4 N 2 Hg+4H 2 O. Precipitate. (Raschig, A. 241. 161.) -, (AgS0 3 ) 2 (KS0 3 ) 2 HgN. Potassium silver +3H 2 O. SI. sol. in H 2 O. (Berglund.) Sodium , (NaSO 3 ) 4 HgN 2 +5H 2 O. More sol. in H 2 O than K salt. (Berglund.) Strontium , Sr 2 (SO 3 ) 4 HgN 2 +15H 2 O. More sol. than Ba salt. (B.) MERCURY 491 Zinc mercurimidosulphonate, Zn 2 (SO 3 ) 4 HgN 2 + 15H 2 O. Very sol. in H 2 O. (B.) imercuriphosphonium mercuric bro- mide, 2PHg 2 Br, HgBr 2 . (Lemoult, C. R. 1907, 146. 1176.) Zh'mercuriphosphonium mercuric chloride, HgCl 2 , PHg 2 Cl. (Lemoult, C. R. 1907, 145. 1176.) +1^H 2 O. Decomp. by hot, slowly by cold H 2 O into Hg, HC1, and H 3 PO 3 . Decomp. by acids or alkalies. (Rose, Pogg. 40. 75.) Dmiercuriphosphonium mercuric iodide, HgI 2 , PHg,I. Slowly decomp. by cold or warm H 2 O, quickly by MOH+Aq . Not attacked by HC1 or H 2 SO 4 +Aq. Rapidly attacked by HNO 3 and aqua regia. (Lemoult, C. R. 1904, 139. 479.) Zh'mercuriphosphonium mercuric nitrate, P 2 Hg 3 , 6HgO, 3N 2 6 = 2[PHg 2 N0 3 , Hg(NO,U 3HgO. (Rose, Pogg. 40. 75.) Dimercuriphosphonium mercuric sulphate, P 2 Hg 3 , 6HgO, 4S0 3 +4H 2 = (PHg 2 ) 2 SO 4 , 3HgS0 4 , 2HgO+4H 2 0. Sol. in aqua regia. (Rose, Pogg. 40. 75.) Mercuric acid. Calcium mercurate (?). (Berthollet, A. ch. 1. 61.) Potassium mercurate, K 2 O, 2HgO. Gradually decomp. by H 2 O; less rapidly by absolute alcohol. (St. Meunier, C. R. 60. 557.) Sodium mercurate, Na 2 O, HgO. (Bettekoff, Bull. Soc. (2) 34. 328.) Mercuroammonium chloride, Hg(NH 3 )Cl. (Rose, Pogg. 20. 158.) Mixture of Hg, HgNH 2 Cl, and NH 4 C1. (Barfoed, J. pr. (2) 39. 201.) nitrate, (NHg 2 H a )NO 3 , "Hahnemann's soluble mercury." Sol. in hot HC1, and HC 2 H 3 O 2 +Aq. De- comp. by NH 4 OH+Aq, or NH 4 salts +Aq. Probably mixture of mercurous salts and Hg. Mercurodiammonium chloride, Hg 2 (NH 3 ) 2 Cl 2 . Easily decomp. (Rose, Pogg. 20. 158.) Mixture of Hg, NH 2 HgCl, and NH 4 C1. (Barfoed, J. pr. (2) 39. 201.) Mercurod; 'ammonium fluoride, Hg 2 (NH 3 ) 2 F 2 (?). Decomp-. by H 2 O. (Finkener, Pogg. 110. 147.) Mercurosulphonic acid. Mercurosulphonates, Hg(SO 3 M) 2 . Correct composition for the double sul- phites, HgSO 3 , M 2 SO 3 . (Divers and Shimid- zu, Chem. Soc. 49. 583; Earth, Z. phys. Ch. 9. 195.) Mercuroxy-comps. See Oxymercur- comps. Mercury, Hg. Not attacked by'H 2 O. Not attacked by boiling cone. HC1 or dil. H 2 SO 4 +Aq. Easily sol. in dil. or cone. HNO 3 +Aq: also in HBr orHI+Aq. Not attacked by pure HNO 3 unless heated, but readily attacked by cold dil. HNO 3 +Aq containing NO. (Millon.) Anhydrous H 2 SO 4 attacks Hg gradually at ord. temp. (Berthelot, C. R. 1897, 126. 749.) H 2 S0 4 attacks only when hot and cone. (Ditte, A. ch. 1890, (6) 19. 68.) Cone. H 2 SO 4 does not attack dry or moist Hg either with or without air. (Pitman, J. Am. Chem. Soc. 1898, 20. 100.) H 2 SO 4 attacks Hg at 20 if it contains 99.7%; does not attack if it contains only 95.6%. (Baskerville, J. Am. Chem. Soc. 1898, 20. 515.) Insol. in H 2 SO 3 +Aq alone or in presence of HC1 or dil. H 2 SO 4 . (Berthelot, A. ch. 1898, (7) 14. 198.) Not attacked by HF+Aq at any temp. (Gay-Lussac.) HI dissolves Hg rapidly at ord. temp. (Norris and Cottrell, Am. Ch. J. 1896, 18. 99.) More rapidly attacked by HBr+Aq than by HCl+Aq. Rapidly acted upon by HI in absence of O. (Bailey, Chem. Soc. 1888, 53. 760.) Not attacked by pure HCl+Aq, but in presence of O, Hg 2 OCl 2 +H 2 O is formed. Action is apparently less in sunlight than in the dark. (Bailey, Chem. Soc. 1888, 53. 759.) Small amts. of ferric salts hinder action of HNOs on Hg, but it is hastened bv pres- ence of Mn(NO 3 ) 2 or NaNO^. (Ray/Chem. Soc. 1911, 99. 1015.) HNO 3 under 33% does not attack Hg if metal and acid are kept in motion and HNO 2 is absent. (Veley, B. 1895, 28. 928.) Rapidly sol. in HC1O. (Balard, Dissert. 1834.) Alkali chlorides +Aq in presence of air decomp. Hg; action is not increased by heat. Miahle.) Insol. in alkali chlorides +Aq in neutral or 492 MERCUROUS ACETYLIDE alkaline solution. (Bhaduri, Z. anorg. 1897. 13. 407.) Very sol. in cone, solution of I in KI+Aq. (Varet, Bull. Soc. 1897, (3) 17. 451.) Slowly sol. in KC1 or KI+Aq in presence of air. (Palmaer, Z. phys. Ch. 1907, 59. 136.) Slowly sol. in Na 2 S+Aq in presence of air. (Palmaer, Z. phys. Ch. 1907, 59. 137.) Hg is appreciably sol. in the sulpho salts of Mo, W, V, As, Sb and Sn. (Storch, B. 1883, 16. 2015.) Persulphates in alkali or neutral solution attack Hg. (NH)&Oi in NH 4 OH solution has strongest action. This dissolves Hg by repeated shaking at high temp. (Tarugi, Gazz. ch. it. 1903, 33, (1) 127.) Insol. in KCN+Aq.' (Elmer, J. pr. 1888, (2)37.442.) Slowly sol. in KCN+Aq in presence of air. (Palmaer, Z. phys. Ch. 1907, 59. 136.) Sol. in considerable quantity in 6% KCN + Aq. (Goyder, C. N. 1894, 69. 268.) Most sol. in K 4 Fe(CN) 6 +Aq when KOH is present. (Smith, J. Am. Chem. Soc. 1905, 27. 544.) Hg dissolves in Br 2 in the presence of KBr si. faster than in I 2 but in CuBr 2 much more slowly. (Van Name and Edgar, Am. J. Sci. 1910, (4) 29. 255.) Not attacked by PC1 3 even at 350. (Moissan, A. ch. 1885 (6) 6. 457.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) % ccm. oleic acid dissolves 0.0075 g. Hg in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Mercurous acetylide, Hg 2 C 2 +H 2 O. (Burkard and Travers, Chem. Soc. 1902 81. 1271.) Mercuric acetylide, basic, 2HgO, 3HgC 2 + 2H 2 0. (Burkard and Travers, Chem. Soc. 1902 81. 1272.) Mercuric acetylide, HgC 2 . Very sol. in HC1 with evolution of H 2 C 2 (Keiser, Am. Ch. J. 1893, 15. 535.) + VsH 2 O. Insol. in H 2 O, alcohol and ether Sol. in NH 4 acetate +Aq, and in KCN+Aq SI. attacked by cold HC1, easily by hot Easily sol. in HNO 3 . Dil. H 2 SO 4 attacks slowly; cone, causes explosion. (Plimpton and Travers, Chem. Soc. 1894, 65. 267.) Mercuric acetylide chloride, HgC 2 , HgCl 5 Not acted upon by dil. HC1. Decomp. bj fuming HNO 3 or aqua regia. Insol. in al cohol and ether. (Keiser, Am. Ch. J. 1893 15. 538.) Mercuric acetylide mercuromercuric chloride HgC 2 , HgCl, HgCl 2 +H 2 0. Insol. in all ordinary solvents. (Biltz an Mumm, B. 1904, 37. 4420.) Mercurous amidofluoride, HgNH 2 F. Insol. in H 2 O, HNO 3 and H 2 SO 4 . Sol. in il. HC1. Probably cfo'mercuriammonium ammonium luoride, NHg 2 F, NH 4 F. (Bohm, Z. anorg. 904,43.327.) Mercury ammonium comps. Mercuroammonium comps., NH 3 HgR. Dimercuroammonium comps., NH 2 Hg 2 R. Mercurous chloramide, Hg(NH 2 )Cl. Dimercuriammonium comps., NHgR. Mercuric chlor-, brom-, etc., amide, Hg(NH 2 )R. MercurWiammonium comps., Hg(NH 3 ) 2 R. Mercuriammonium comps., HgNH 2 R. Diinercuricframmonium comps., Hg 2 N 2 H 4 R. TVimercuriammonium comps., N 2 H 2 Hg 3 R. Oxy^Tmercuriammonium. comps., NH 2 Hg 2 O)R. Mercurous arsinchloride, AsHgCl. Decomp. by H 2 O. (Capitaine, J. Pharm. 25. 559.) Mercurous arsinchloride chloride, AsHg 2 Cl 2 = 2AsHgCl, Hg 2 Cl 2 (?). Decomp. by H 2 O. (Capitaine.) Mercurous azoimide, HgN 3 . Wholly insol. in H 2 O. (Curtius, B. 24. 3324.) 1 1. H 2 O dissolves 0.25 g. (Wohler and Krupko, B. 1913, 46. 2050.) Mercuric azoimide, HgN 6 . Sol. in H 2 O especially when hot. (Ber- thelot and Vieille, Bull. Soc. 1894, (3) 11. 747.) Moderately sol. in H 2 O. (Wohler and Krupko, B. 1913, 46. 2050.) Mercuric bromamide, Hg(NH 2 )Br. Insol. in H 2 O and alcohol. SI. sol. in NH 4 OH+Aq. (Mitscherlich, J. pr. 19. 455.) Correct composition is dimercuriammon- ium ammonium bromide, Hg 2 NBr, NH 4 Br, which see. (Pesci, Gazz. ch. it. 19. 511.) Mercurous bromide, Hg 2 Br 2 . Solubility in H 2 O=9.1XlO- 7 g. equiv. per 1. (Bodlander, Z. phys. Ch. 1898, 27. 61.) Solubility in H 2 O=7XlO^ mols. per liter at 25. (Sherrill, Z. phys. Ch. 193, 430. 735.) MERCURIC BROMIDE 493 Solubility of HgBr 2 in KBr+Aq at 25. Mols. per liter Solubility in H 2 O at 25 = 1.4 X 10~ 7 equiva- lents per 1. (Thompson, J. Am. Chem. Soc. 1906, 28. 762.) Insol. in H 2 O and dil. acids. Decomp. by HCl+Aq. Sol. in hot cone. H 2 SO 4 with evolution of SO 2 . SI. sol. in hot HNO 3 +Aq of 1.42 sp. gr. (Stromann, B. 20. 2818.) Decomp. into Hg and HgBr 2 by boiling with NH 4 Br, or NH 4 Cl+Aq; also by am- monium carbonate or succinate, but not by ammonium sulphate or nitrate. (Witt- stein.) Sol. in Hg(NO 3 ) 2 +Aq. (Wackenroder, A. 41. 317.) Partially decomp. by alkali chlorides +Aq ; when out of contact of air this decomp. is slight and HgBr 2 is formed, while in the air HgCl 2 is the resulting product. Much more rapidly decomp. in hot than cold solutions. (Miahle, A. ch. (3) 5. 177.) A solution of HgBr in 0.1 N KBr contains about 1 mg. Hg ions in 1300 1. Insol. in alcohol. Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790) ; ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4329); (Eidmann, C. C. 1899, II. 1014.) Mercuric bromide, HgBr 2 . Sol. in 250 pts. H2O at ordinary temp., and 25 pts. boiling HoO. (Wittstein.) Sol. in 240 pts. H 2 O at 18.75. (Abl.) Sol. in 94 pts. H 2 O at 9, and in 4-5 pts. at 100. (Lassaigne, J. chim. med. 12. 177.) Solubility in g-equivalents per litre = 2X10- 2 . (Bodlander, Z. phys. Ch. 1898, 27. 61.) 1 1. H 2 O dissolves about 4 g. at ord. temp. (Morse, Z. phys. Ch. 1902, 41. 731.) 1 1. H 2 O dissolves 0.017 mol. at 25. (Jan- der, Dissert, 1902.) Solubility in H 2 O at 25 = 0.017 mol. liter. (Sherrill, Z. phys. Ch. 1903, 43. 735.) Solubility at ord. temp. =0.8%; at bpt. 8-9%. (Larine, J. Pharm. 1904, (6) 20. 450.) Solubility in cold H 2 O=4%, but solution prepared by heating contains more Hg on account of decomp. into HBr and oxybrom- ide. (Vicario, C. C. 1907, II. 1224.) 1 1. H 2 O dissolves about 5-6 g. at ord. temp. (Gaudechon, A. ch. 1911, (8) 22. 212.) 1 1. aqueous solution at 25 contains 0.017 mol. (Herz and Paul, Z. anorg. 1913, 83. 431.) Decomp. by warm HNO 3 , or H 2 SO 4 +Aq. Sol. in warm H 2 SO 4 . (Ditte, A. ch. (5) 17. 124.) 1 mol. is sol. in 1 mol. warm HI+Aq. in 1 mol. cold cone. HC1 and in y% mol. hot cone. HC1. . (Lowig.) KBr 0. 0.05 0.10 0.5 0.866 2 3 4 HgBr 2 0.017 0.055 0.088 0.0359 0.611 1.407 2.096 2.339 (Sherrill, Z. phys. Ch. 1903, 43. 705.) Solubility in various salts+Aq at 25. Salt NaBr KBr CaBr 2 SrBr, BaBr 2 In 10 ccm. of the solution Millimols Hg Br 2 Millimols salt 0.17 0.78 2.85 5.40 12.76 15.50 23.06 0.17 0.98 4.72 13.60 19.30 0.17 1.17 6.76 13.58 27.66 36.66 0.17 1.04 4.71 9.02 17.70 22.38 0.17 3.70 5.40 7.59 14.78 1.18 5.96 11.42 24.48 29.97 52.46 2.09 7.70 23.80 34.70 0.72 6.45 18.92 24.79 37.54 0.62 3.28 6.68 14.01 18.72 2.74 3.96 5.79 10.96 (Herz and Paul, Z. anorg. 1913, 82. 434.) Solubility in 0.1 -N Hg(NO 3 ) 2 +Aq is about 20 g. per liter. (Morse, Z. phys. Ch. 1902, 41. 731.) Sol. in KBr or NaBr+Aq. (Jander, Dissert. 1902.) Solubility in 10 cc. Br 2 +Aq at 25. MillimolBr 2 0.753 1.797 2.231 " Hg 0.1844 0.1947 0.2120 (Herz and Paul, Z. anorg. 1914, 86. 215.) 494 MERCURIC BROMIDE Sat. solution in liquid SO 2 contains about 1.5% HgBr 2 at 159.4. (Niggli, Z. anorg. 1912, 75. 182.) Moderately sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 27.) 1 ccm. of sat. solution in abs. alcohol at ord. temp, contains 0.0958 g. HgBr 2 ; at bpt. contains 0.1262 g. (Hamper, Ch. Z. 1887, 11. 905.) Solubility of HgBr 2 in alcohols +Aq at t. Alcohol t G. HgBr 2 per 100 g. alcohol Methyl alcohol 10 19 22 39 65 97 41.15 40.5 66.3 60.9 71.3 90.8 139.1 Ethyl alcohol 10 19 39 65 89 25.2 26.3 29.7 31.9 44.5 66.9 Propyl alcohol 10 19 39 65 86.5 14.6 15.6 15.5 20.8 31.3 42.7 Isobutyl alcohol 10 23 39 65 4.61 5.63 6.65 9.58 15.80 (Timofeiew, Dissert. 1894.) Much more sol. than HgI 2 in alcohol. 100 g. of solution sat. at contain 13.33- 13.05 g. HgBr 2 ; 16.53 g. at 25; 22.63 g. at 50. (Reinders, Z. phys. Ch. 1900, 32. 522.) Solubility of HgBr 2 in methyl alcohol +Aq at 25. P = g. alcohol in 100 g. alcohol +Aq. HgBr 2 = millimols. HgBr 2 in 10 cc. of the solution. p HgBr 2 Sp. gr. 1.0022 0.9857 0.9588 0.9508 P HgBr 2 Sp. gr. 10.60 30.77 37.21 0.167 0.201 0.358 0.422 47.06 -64.00 78.05 100 0.700 1.90 4.07 13.96 0.9401 0.9386 0.9744 1.2275 Solubility of HgBr 2 in ethyl alcohol +Aq at 25. P = g. alcohol in 100 g." alcohol +Aq. HgBr 2 = millimols. HgBr 2 in 10 cc. of the solution. p HgBr 2 Sp. gr. 20.18 40.69 70.01 100 0.167 0.187 0.440 1.829 6.337 1.0022 0.9717 0.9435 0.9214 0.9873 (Herz and Anders.) Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. HgBr 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. p G S 25/4 11.11 23.8 65:2 91.8 93.75 96.6 , 100 5.02 4.728 4.153 2.530 1.635 1.586 1.466 1.873 1.227 1 . 1954 1 . 1524 1.0257 0.9437 0.9368 0.9275 0.9213 (Herz and Kuhn, Z. anorg. 1908, 60. 158.) Solubility in mixtures of ethyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. HgBr 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. P G S 25/4 8.1 17.85 56.6 88.6 91.2 95.2 100 2.28 2.225 2.106 1.763 1.476 1.464 1.406 1.378 0.9873 0.9802 0.9740 0.9487 0.9269 0.9239 0.9227 0.9213 (Herz and Kuhn, Z. anorg. 1908,. 60. 161.) Solubility of HgBr 2 in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the mixtures. HgBr 2 =g. HgBr 2 in 10 ccm. of the solution. S25 4 = sp. gr. of the sat. solution. (Herz and Anders, Z. anorg. 1907, 52. 165.) P HgBr 2 S 25/4 2.28 0.9873 4.37 2.31 0.9932 10.4 2.54 1.009 41.02 3.33 1.080 80.69 4.57 1.185 84.77 4.68 1.193 91.25 4.86 1.211 100 5.02 1.227 (Herz and Kuhn, Z. anorg. 1908, 58. 163.) MERCURIC SODIUM BROMIDE 495 Cold sat. solution in anhydrous ether con- tains 0.00567 g. in 1 cc.; hot solution contains 0.032 g. (Hampe, Ch. Z. 1887, 11. 905.) Solubility in organic solvents at 18-20. 100 g. chloroform dissolve 0.126 g. HgBr 2 . 100 g. tetrachlormethane dissolve 0.003 g. HgBr 2 . 100 g. bromoform dissolve 0.679 g. HgBr 2 . 100 g. ethyl bromide dissolve 2.310 g. HgBr 2 . 100 g. ethylene dibromide dissolve 2.340 g. HgBr 2 . (Sulc, Z. anorg. 1900, 25. 401.) Solubility in CS 2 at t. t 100 pts. sat. solution contain pts. HgBr 2 10 0.049 5 0.068 0.087 + 5 0.105 10 0.122 15 0.140 20 0.187 25 0.232 30 0.274 Mols. HgBr 2 per 100 s Mols. HgBr 2 per 100 s Mols. HgBr 2 per 100 S 4.9 10. 12.5 14.9 19.7 23.4 9 43.5 57 68 89 106 ,25.4 33.9 39.5 41.9 43.9 46.2 115.5 117 108 113 118 121 49.6 54.9 58.8 64.0 123 124 134 133 (Staronka, Anz. Ak. Wiss. Krakau, 1910, 372.) Solubility of HgBr 2 in quinoline. (Arctowski, Z. anorg. 1894, 6. 267.) 100 g. boiling methyl acetate (bpt. 56.2- 56.7) dissolves 24 g. HgBr 2 . (Schroeder and Steiner, J. pr. 1909, (2) 79. 49.) 1 g. HgBr 2 is sol. in 4.56 g. methyl acetate at 18. Sp. gr. 18/4 of sat. solution = 1.09. (Naumann, B. 1909, 42. 3795.) 100 g. anhydrous ethyl acetate or sat. with H 2 O at 18 dissolve 130.5-135 g. HgBr 2 . (Hamers, Dissert. 1906.) Solubility of HgBr 2 in ethyl acetate -f-Aq at 25. P = g. ethyl acetate in 100 g. ethyl acetate +Aq. HgBr 2 = millimols HgBr 2 in 10 cc. of the solution. p HgBr 2 Sp. gr. 4.39 96.76 100 0.167 0.159 7.42 3.93 1.0022 1.0018 1.1159 1.0113 (Herz and Anders, Z. anorg. 1907, 62. 172.) 1 pt. HgBr 2 sol. in 7.66 pts. ethyl acetate at 18. (Naumann, B. 1910, 43. 315.) Easily sol. in acetone. (Oppenheim, B. 2. 572.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Acetone dissolves much more HgBr 2 than HgI 2 . 100 g. sat. solution at 25 con- tain 34.58 g. HgBr 2 . (Reinders, Z. phys. Ch. 1900, 32. 514.) Solubility in diethyl oxalate is much greater than that of HgI 2 and is equal to 12% at 100. (Reinders, Z. phys. Ch. 1900, 32. 507.) Solubility in benzene = 0.0194 mol. per 1. at 25. (Sherrill, Z. phys. Ch. 1903, 43. 735.) Sol. in allyl mustard oil. (Mathews, J. phys. Chem. 1905, 9. 647.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Solubility in aniline. S = temp. of solidification. S = temp. of solidification. Mols. HgBr 2 per 100 4.4 8.9 14.3 17.6 S 88 111 127 134 (Staronka, Anz. Wiss. Krakau, 1910. 372.) Mol. weight determined in ethyl sulphide. (Werner, Z. anorg. 1897, 15. 30.) +4H 2 O. (Thomsen.) , Mercuric perbromide, HgBr 4 . (Herz and Paul, Z. anorg. 1914, 85. 216.) Mercuric hydrogen bromide (Bromomercuric acid), HgBr 2 , HBr = HHgBr 3 . Decomp. by H 2 O. (Neumann, M. 10. 236.) Mercuric nickel bromide, basic, HgBr 2 , NiBr 2 , 6NiO+20H 2 O. (Mailhe, A. ch. 1902, (7) 27. 369.) Mercuric platinum bromide. See Bromoplatinate, mercuric. Mercuric potassium bromide, HgBr 2 , KBr. Sol. in H 2 O, but decomp. by a large amount, with separation of one half of the HgBr 2 . (v. Bonsdorff, Pogg. 19. 339.) 2HgBr 2 , KBr+2H 2 O. Permanent. Sol. in H 2 O and alcohol, (v. Bonsdorff.) Mercuric sodium bromide, HgBr 2 , NaBr. Deliquescent, (v. Bonsdorff.) (Varet, C. R. 1890, 111, 527.) 496 MERCURIC SODIUM BROMIDE HgBr 2 , 2NaBr. Very sol. in H 2 O. (Vicario, J. Pharm. 1907, (6) 26.. 145.) 2HgBr 2 , NaBr+3H 2 O. Sol. in H 2 O and alcohol. (Berthemot.) Mercuric strontium bromide, HgBr 2 , SrBr 2 . Sol. in all proportions of H 2 O. (Lowig, Mag. Pharm. 33. 7.) 2HgBr 2 , SrBr 2 . Decomp. by H 2 O into HgBr 2 and HgBr 2 , SrBr 2 . (Lowig.) Mercuric zinc bromide. Deliquescent in moist air. (v. Bonsdorff.) Mercuric zinc bromide cyanide ammonia. See Cyanide zinc bromide ammonia, mer- curic. Mercuric bromide ammonia, HgBr 2 , 2NH 3 . Decomp. by boiling H 2 O. Sol. in min. acids and acetic acid. (Naumann, B. 1910, 43. 316.) Mercuric bromide cadmium oxide, HgBr 2 , CdO+H 2 O. (Mailhe, A. ch. 1902, (7) 27. 371.) Mercuric bromide cupric oxide, HgBr 2 , CuO+3H 2 O. (Mailhe, Bull. Soc. 1901, (3) 25. 791.) Mercuric bromide hydrazine, HgBr 2 , N 2 H 4 . (Hofmann and Marburg, A. 1899, 305. 215.) Mercuric bromide potassium chloride, HgBr 2 , 2KC1. Decomp. by H 2 O. (Harth, Z. anorg. 1897, 14. 345.) Mercuric bromide zinc oxide, HgBr 2 , ZnO + 8H 2 O. (Mailhe, C. R. 1901, 132, 1274.) Mercuric bromoiodide, HgBrl. Sol. in alcohol and ether. Can be recrystal- lised from ether without decomp. (Oppen- heim, B. 2. 571.) Mercurous chloramide, Hg 2 (NH 2 )Cl. Insol. in boiling H 2 O or NH 4 OH+Aq. (Kane, A. ch. (2) 72. 215.) Mixture of Hg and HgNH 2 Cl. (Barfoed, J. pr. (2), 39. 201.) Mercuric chloramide, Hg(NH 2 )Cl. Composition is dimercuriammonium am- monium chloride, Hg 2 NCl, NH 4 C1, which see. Mercuric chloramide oxymercuriammonium chloride, 4Hg(NH 2 )Cl, (NHg 2 OH 2 )Cl. (Millon.) Correct composition is cfomercuriammonium ammonium chloride, NHg 2 Cl, NH 4 C1, which see. (Balestra, Gazz. ch. it. 21. (2) 294.) Hg(NH 2 )Cl, (NHg 2 OH 2 )Cl. (Millon.) . True composition is rfomercuriammonium mercuric chloride, 2Hg 2 NCl, HgCl 2 +H 2 O; or fKmercuriammonium hydrogen chloride, NHg 2 Cl, HC1. (Balestra.) Mercuric chloramide chloride, Hg(NH 2 )Cl, HgCl 2 . Properties as mercuric chloramide. De- comp. by cold HCl+Aq. (Millon.) True composition is dmiercuriammonium hydrogen chloride, NHg 2 Cl, 2HC1. (Ba- lestra, Gazz. ch. it. 21. (2) 294.) Mercuric chloramide chromate, 2Hg(NH 2 )Cl, HgCrO 4 . Decomp. by hot H 2 O. Easily sol. in HNO 3 or HCl+Aq. (Jager and Krtiss, B. 22. 2048.) Mercurous chloride, Hg 2 Cl 2 . Ahnost absolutely insol. in cold, but gradu- ally si. decomp., by boiling H 2 O. Calculated from electrical conductivity of Hg 2 Cl 2 +Aq, 1 1 H 2 O dissolves 3.1 mg. Hg 2 Cl 2 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) 1 1. H 2 dissolves 2 mg. Hg 2 Cl 2 at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 1 1. H 2 O dissolves 1.4 mg. at 0.5; 21 mg. at 18; 2.8 mg. at 24.6; 7 mg. at 43. (Kohl- rausch, Z. phys. Ch. 1908, 64. 150.) When finely divided, is 10% more sol. than when coarsely crystalline. (Sauer, Z. phys. Ch. 1904, 47. 184.) Solubility in H 2 O = 0.8 X 10- 6 g. mol. (Ley, Z. Elektrochem. 1904, 10. 301.) SI. sol. with decomp. in boiling H 2 O free from air, 20 ccm. H 2 O affording 0.002 g. HgCl 2 after boiling 1 hour with Hg 2 Cl 2 . (Miahle, A. ch. (3) 5. 176.) Hg 2 (NO 3 ) 2 + Aq containing 1 pt. Hg 2 (NO 3 ) 2 to 250,000 pts. H 2 O give ppt. of Hg 2 Cl 2 with HCl+Aq. Sol. with decomp. in cone. HCl+Aq, hot HNO 3 +Aq, aqua regia, or Cl 2 +Aq. (Fre- senius.) Insol. in cold dil. acids, but slowly sol. on heating. The solubility of Hg 2 Cl 2 in HCl+Aq in- creases slowly with time, and finally reaches a point where it increases very rapidly, which takes place sooner the more dil. the acid. Presence of Hg 2 (NO 3 ) 2 +Aq helps the solu- bility. (Why not oxidation to HgCl 2 ?) (Varenne, C. R. 92. 1161.) MERCURIC CHLORIDE 497 Solubility of Hg 2 Cl 2 in HCl+Aq at 25. Solid phase = Hg 2 Cl 2 +0.1 g. Hg. G. per 1. Sp. gr. of solutions HC1 HgzCh 31.69 0.034 36.46 0.048 95.43 0.207 l!042 158.4 0.399 1.069 209.2 0.548 1.091 267.3 0.654 1.114 278.7 0.675 1.119 317.3 0.670 1.132 364.6 0.673 1.153 (Richards and Archibald, Z. phys. Ch. 1902. 40. 385.) Cold cone. H 2 SO4 does not dissolve or decomp. Boiling H 2 SO 4 dissolves with evo- lution of SO 2 . (Vogel.) Solubility of Hg 2 Cl 2 in chlorides +Aq at 25. Solid phase =Hg 2 Cl 2 +0.1 g. Hg. Salt G. pe r liter Sp. gr. of NaCl Hg 2 Cl 2 solutions NaCl 5.85 58.50 119. 148.25 222.3 292.5 0.0041 0.041 0.129 0.194 0.380 0.643 i!6io 1.078 1.093 1.142 1.188 BaCl 2 104.15 156.22 208.30 312.54 0.044 0.088 0.107 0.231 1.088 1.134 1.174 1.263 CaCl 2 39.96 55.5 111 138.75 195.36 257.52 324.67 432.9 499.5 0.022 0.033 0.081 0.118 0.231 0.322 0.430 0.518 0.510 !664 .105 .151 .205 .243 .315 1.358 (Richards and Archibald, Z. phys. Ch. 1902, 40. 385.) Sol. in cold HCN+Aq with separation of Hg. Sol. in alkali chlorides+Aq. NH 4 Cl+Aq dissolves out HgCl 2 at ord. temp., much more at 40-50. Dil. NH 4 Cl+Aq decomposes more slowly than cone. Access of air hastens reaction. (Miahle.) When heated several hours to 40-50, 100 pts. NH 4 Cl+833 pts. H 2 O form 0.75 pt. HgCl 2 from 25 pts. Hg 2 Cl 2 ; 100 pts. NaCl+ 833 pts. H 2 O form 0.33 pt. HgCl 2 from 25 pts. Hg 2 Cl 2 ; 100 pts. KC1+833 pts. H 2 O form 0.25 pt. HgCl 2 from 25 pts. HgCl 2 ; 100 pts. BaCl 2 +833 pts. H 2 O form 0.33 pt. HgCl 2 from 25 pts. Hg 2 Cl 2 . (Miahle, J. Pharm. 26. 108.) Other chlorides act as NH 4 C1, only less vigorously. (Pettenkofer.) By boiling 1 pt. Hg 2 Cl 2 10 times with a solution of 1 pt. NaCl each time, the Hg 2 Cl 2 is finally completely decomp. (Henne.) Boiling BaCl 2 +Aq or CaCl 2 +Aq dissolve traces. K 2 SO 4 +Aq, KNO 3 +Aq, or KHC 4 H 4 O 6 +Aq do not dissolve. (Petten- kofer.) Sol. in (NH 4 ) 2 SO 4 +Aq. Insol. in NH 4 nitrate, or succinate+Aq. (Wittstein.) Sol. in hot Hg 2 (NO 3 ) 2 +Aq, and still more in hot Hg(NO 8 ) 2 +Aq; on cooling it crystal- lises out completely. 25 g. Hg 2 Cl 2 dissolve in 1.5 1. H 2 O containing 50 g. Hg(NO 3 ) 2 . (De- bray, C. R. 70. 995.) Sol. in PtCl 2 +Aq. Decomp. by NH 4 OH+Aq. Decomp. by KOH, or NaOH+Aq. Sol. in Na 2 S 2 O 3 +Aq. (Faktor, C. C. 1905, I. 1524.) Very si. sol. in NH 4 succinate. (Witt- stein.) Insol. in SbCl 3 . (Klemensiewicz, C. C. 1908, II. 1850.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol or ether. More sol. in H 2 O containing pepsin and an acid than in H 2 O, and is not converted thereby into HgCl 2 . (Torsellini, Ann. Chim. Ch. farm. (4) 4. 105.) Small amts. are. sol. with decomp. in al- cohol, ether and CHC1 3 . 1 g. CHC1 3 dis- solves 0.0046 g. Hg 2 Cl 2 . (Maclagan, Arch. Pharm. 1884, 222, 788.) Formic acid (95%) dissolves at 16.5, 0.02%; at 18, 0.0003%. (Aschan, Ch. Z. 1913, 37. 1117.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Hamers, Dissert. 1906; Naumann, B. 1904, 37. 3602.) Somewhat sol. in hydroxylamine hydro- chloride. (Adams, Am. Ch. J. 1902, 28. 1216.) Insol. in benzonitrile. (Naumann, B/. 1914, 47. 1370.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Solubility in organic solvents at 18-20. 100 g. chloroform dissolve traces of HgCl. 100 g. bromoform dissolve 0.055 g. HgCl. 100 g. ethyl bromide dissolve traces of HgCl. 100 g. ethylene dibromide dissolve traces of HgCl. (Sulc. Z. anorg. 1900, 25. 401.) Mercuric chloride, HgCl 2 . Permanent. Sol. in 18.5 pts. H 2 O at 13.8, and 2-3 pts. at 100. (J. Davy, 1822.) Sol. in 3 pts. boiling H 2 O. (Wenzel.) Sol. in 18.23 pts. IPO at 10, and 3 pts. at 100. (M. R. and P.) Sol. in 18.46 pts. at 18.75. (Abl.) Sol. in 16 pts. cold, and 3 pts. warm HjO. (Dumas.) 498 MERCURIC CHLORIDE 100 pts. H 2 O dissolve pts. HgCl 2 at t: t Pts. HgCh t Pts. HgCU t Pts. HgCb 10 20 30 5.73 6.57 7.39 8.43 40 50 60 70 9.62 11.34 13.86 17.29 80 90 100 24.30 37.05 53.96 (Poggiale, A. ch. (3) 8. 468.) Solubility of HgCl 2 in H 2 O. t % HgCl 2 t % HgCl 2 + 1 3.9 80 23.6 4.5 4.8 87 28.2 4.5 4.8 100 39.3 7.5 5.1 121 59.7 13.8 5.2 127 69.7 25.1 7.1 140 77.0 29.5 7.6 150 78.4 38.0 9.9 159 80.2 49 11.3 160 81.7 61 15.1 165 81.8 (Etard, A. ch. 1894, (7) 2. 557.) 71.17 g. HgCl 2 are sol. in 1 1. H 2 O at 25. (Morse, Z. phys. Ch. 1902, 41. 726.) Solubility at 25 = 0.267 mol. in 1 1. H 2 O. (Jander, Z. Elektrochem. 1903, 8. 688.) Solubility in H 2 O at 25 = 0.263 mol. liter. (Sherrill, Z. phys. Ch. 1903, 43. 735.) Sat. HgCl 2 +Aq at 25 contains 6.9% HgCl 2 . (Foote, Am. Ch. J. 1906, 35. 238.) HgCl 2 +Aq contains 3.95 g. HgCl 2 in 100 g. of solution at 0; 7.67 g. at 30. (Schreine- makers, Ch. Weekbl. 1910, 7. 202.) HgCl 2 +Aq sat. at (?) contains 6.8% HgCl 2 . (Abe, J. Tok. Chem. Soc. 1912, 33. 1087.) HgCl 2 +Aq sat. at 35 contains 8.51% HgCl 2 . (Schreinemakers and Thonus, Ver. K. Akad. Wet. Amsterdam, 1912, 21. 333.) 1 1. aqueous solution sat. at 25 contains 0.265 mol. HgCl 2 . (Herz and Paul, Z. anorg. 1913, 82. 431.) H 2 O dissolves 7.39% at 20. (Aschan, Ch. Z. 1913, 37. 1117.) HgCU+Aq sat. at 8 has 1.041 sp. gr. (Anthon, Sp. gr. of HgCl 2 +Aq at 20. % HgCU Sp. gr. % HgCl 2 Sp. gr. 1 2 3 1.0072 1.0148 1.0236 4 5 1.0323 1.0411 (Schroder, calculated by Gerlach, Z. anal. 27. 306.) Sp. gr. of HgCl 2 +Aq at 15. % HgCl 2 Sp. gr. % HgCU Sp. gr. 8 9 10 1.071 1.0815 1.095 11 12 13 1 . 1035 1.115 1.127 (Mendeleieff, calculated by Gerlach, Z. anal. 27. 306.) Sp.gr. of HgCl 2 +Aq. HgCl 2 Sp. gr. at at lb at 20 at 30 4.72 3.57 2.42 1.22 1.04070 1.03050 1.02035 1.01008 1.04033 1.03022 1.02018 1.00990 1.03856 1.02885 1.01856 1.00835 1.03566 1.02577 1.01585 1.00575 (Schroder, B. 19. 161 R.) Sp. gr. of HgCl 2 +Aq at room temp, con- taining: 0.226 3.55% HgCl 2 . 1.0233 1.0328 (Wagner, W. Ann. 1883, 18. 266.) Sp. gr. of HgCl 2 +Aq at 25. Concentration of HgCU +Aq. Sp. gr. 1 /4-normal l/ 8 _ 1.0275 1.0138 (Wagner, Z. phys. Ch. 1890, 6. 39.) Sp. gr. at 16/4 of HgCl 2 +Aq containing 4.5256% HgCl 2 = 1.03806. Sp. gr. at 16/4 of HgCl 2 +Aq containing 4.2224% HgCl 2 = 1.03491. (Schonrock, Z. phys. Ch. 1893, 11. 768.) HgCl 2 +Aq containing 6.04% HgCl 2 has sp. gr. 20/20 = 1.0523. HgCl 2 +Aq containing 6.08% HgCl 2 has sp.gr. 20 /20 = 1.0526. (Le Blanc and Rohland, Z. phys. ch. 1896, 19. 282.) Sat. HgCU+Aq boils at 101.1. (Griffiths.) B.-pt. of HgCl 2 +Aq % HgCU B.-pt. % HgCU B.-pt. 4.8 9.0 100.10 100.16 11.04 15.2 100.20 100.275 (Skinner, Chem. Soc. 61. 340.) Solubility in HCl+Aq is greater than in H 2 O. (Dumas.) Sol. in 0.5 pt. HCl+Aq of 1.158 sp. gr. at 23.3, form- ing a solution of 2.412 sp. gr. (Davy, 1822.) MERCURIC CHLORIDE 499 Solubility of HgCl 2 in HCl+Aq. Solubility of HgCl 2 in NH 4 Cl+Aq Pts. HCl in 100 pts. H 2 9 Pts. HgCl 2 dissolved by 100 pts. liquid Pts. HCl in 100 pts. H 2 Pts. HgCl 2 dissolved by 100 pts. liquid at 30. Continued. Composition of liquid phase Solid phase 0.0 5 6.8 A(\ C 21.6 Q1 A 127.4 mQ HgCl 2 NH!CI % H 2 10.1 73.7 50.0 148.0 55.55 15.94 28.51 HgCl 2> NH 4 C1, H 2 13.8 87.8 68.0 154.0 55.85 15.35 28.80 " en 71 M99 on ryr ii (Ditte, A. ch. (5) 22. 551.) 57.04 14.10 28.86 HgCl 2 , NH4C1, Hv-0 + 56.98 14.14 28.88 3HgCl 2> 2NH4C1, H 2 Solubility in HCl + Aq at 0. ^y^ = ^mols. 56.83 56.26 13.90 13.04 29.27 30.70 SHgCh, 2NH4C1, H 2 O HgCl 2 (in mgs.) in 10 ccm. solution; HCl = mols. HCl ditto; H 2 O=grms. H 2 O present 56.43 56.70 57.05 11.88 11.05 9.92 31.69 32.23 33.02 58 55 9 23 32 22 " HgCh HCl. Sp. gr. H 2 O 58.65 9.20 32.15 / SHgClj, 2NH4C1, H 2 O + { 9HgCl 2 , 2NH 4 C1 * 51.83 8.76 39.41 9HgCl 2 , 2NH4C1. 9.7 19.8 35.5 55.6 68.9 72.37 85.5 88.65 4.3 9.9 17.8 26.9 32.25 34.25 41.5 48.1 1.117 1.238 1.427 1.665 1.811 1.874 2.023 2.066 9.704 9.340 9.816 8.135 7.714 7.679 7.131 6.893 46.00 39.02 35.60 35.10 32.90 29.65 40.12 21.00 7.52 6.28 5.26 5.18 5.06 3.62 5.13 2.29 46.48 54.70 59.14 59.72 62.04 66.73 54.75 76.71 9HgCl 2) 2NH4Cl+HgCl 2 HgCh 95.675 70. 875 . 2.198 6.431 7.67 92.33 (Engel, A. ch. (6) 17. 362.) Not decomp. by H 2 SO 4 or HNO 3 +Aq. Sol. in 630 pts. H 2 SC>4, and in more than 500 pts. hot HNOs+Aq of 1.41 sp. gr. without decomp. (J. Davy.) Sol. in H 2 SO 4 , HNO 3 , HIO 3 , or H 2 CrO 4 without decomp. (Millon, A. ch. (3) 18. 373.) Very si. sol. in HNO 3 , but not decomp. thereby. (Wurtz.) Solubility of HgCl 2 in NH 4 Cl+Aq at 30. Composition of liquid phase Solid phase % HgCl 2 N&Jl %H 2 29.5 70.5 NH 4 C1 15.68 27.56 56.76 11 22.80 26.91 50.29 " 31.96 26.16 41.88 " 42.45 25.05 32.50 ** 50.05 24.79 25.16 (NH4Cl+HgCl 2 , 2NH4C1, 1 H 2 50.60 24.31 25.09 HgCh, 2NHiCl, H 2 53.08 22.77 24.15 55.97 21.42 22.61 . 58.91 20.06 21.03 HgCh, 2NH 4 C1, H 2 O + 58.89 19.98 21.13 HgCh, NH 4 C1, H 2 56.83 18.86 24.61 HgCh, NH4C1, H 2 56.38 18.50 25.12 " 55.83 17.70 26.47 55.70 17.13 27.17 . 55.58 16.82 27.60 - 1 pt. sat. NaCl+Aq dissolves 1.29 pts. HgCl 2 at 14. (Voit, A. 104. 354.) Sat. NaCl +Aq (20 grains H 2 O +7 grains NaCl) dis- solves 32 grains HgCh at 15.5, and 3 grains more on warming. Sp. gr. of solution =2.14. (Davy, 1822.) Sat. KCl+Aq (21 grains H 2 O+7 grains KC1) dis- solves 8 grains HgCl 2 on being gently heated. (Davy.) Sat. BaCl 2 +Aq (20 grains H 2 O +8.7 grains BaClz + 2H 2 O) dissolves 16 grains HgCl 2 at 15.5, and 4 grains more on heating. Sp. gr. of solution =1.9. (Davy.) MgCl 2 +Aq (31 grains HCl+Aq of 1.58 sp ; gr. neutralised with MgO) dissolves 40 grains HgCl 2 , and 25 grains more on gently heating. Sp. gr. of solution = 2.83. (Davy.) Sol. in sat. KC1, NaCl+Aq, and in MnCl 2 , ZnCl 2 , CoCl 2 , FeCl 2 , NiCl 2 , and CuCl 2 +Aq. (v. Bonadorff, Pogg. 17. 123.) The solubility in H 2 O is greatly increased by the addition of cupric chloride. 8.5% HgCl 2 is sol. in pure H 2 O and 52.8% HgCl 2 is sol. in 18.06% CuCl 2 +Aq. (Schreine- makers, C. C. 1913, I. 1858.) 500 MERCURIC CHLORIDE Solubility of HgCl 2 +KCl at 25% Composition Composition of of solution undissolved residue % KC1 26.46 26.24 26.23 26.33 26.33 23.74 22.36 21.39 20.32 20.26 17.85 9.26 7.80 6.84 6.66 6.52 6.64 6.27 5.77 4.68 4.66 4.69 HgCh 15.04 15.02 15.02 14.92 18.91 21.39 23.88 27.62 27.38 25.34 18.95 19.56 22 81 24.32 25.13 25.16 25.11 24.73 24.75 25.17 24.82 6.90 100 34.61 34.77 34.05 21.89 21.02 20.76 20.75 20.54 12.09 11.87 % HgCb 3.63 26.15 52.01 61.04 61.66 62.02 61.84 65.24 73.98 75.10 73.36 73.06 74.54 73.99 76.46 80.60 83.20 83.18 84.46 93.58 98.50 100 3.73 3.21 3.35 3.01 5.62 6.18 4.71 5.47 4.71 4.95 Solid phase KC1 KC1+2KC1, HgCh, H 2 2KC1, HgCh H 2 2KC1, HgCl 2 H 2 O+KC1, HgCh,H 2 KC1, HgCl 2 , H 2 KC1, HgCl 2 , HiO+KCl, 2HgCh, ( 2H 2 O KC1, 2HgCl 2 , 2H 2 O KC1, 2HgCl 2 , 2H 2 O+HgCh HgCh (Foote and Levy, Am. Ch. J. 1906, 35. 239.) Solubility of |HgCl 2 +KCl at 20. G. per 100 g. H 2 O 1.12 2.39 4.05 4.84 5.60 6.71 7.39 7.46 8.95 15 17.57 20.35 26.31 30.32 34.12 34.18 34.34 34.54 37.72 41.13 39.66 37.87 35.32 HgCh 7.39 11.63 15.72 22.17 25.16 25.13 25.66 26.41 24.70- 19.93 22.87 26.12 29 34.83 39.10 42.82 39.34 35.16 30.63 24.30 19.33 15.76 10.28 2.1 Solid phase HgCl 2 HgCl 2 +2HgCl 2 , KC1 2HgCl 2 , KC1 a 2HgCl 2 , KCl+HgCl 2 , KC1 /HgCl 2 , KC1 HgCl 2 , KCl+HgCl 2 , 2KC HgCl 2 , 2KC1 HgCl 2 , 2KC1+KC1 KC1 u (Tichomiroff, J. russ. Phys. Chem. Soc. 1907 39. 731.) Solubility of HgCl 2 +RbCl in H 2 0. Solu- )ility data are given showing double salts ormed at 25. (Foote and Levy, 1. c.) Solubility in NaCl+Aq. 100 pts. NaCl+Aq containing given % .NaCl dissolve g. HgCl 2 . % NaCl 26 25 10 5 1 0.5 g. HgCh at 15 128 120 58 30 14 10 g. HgCh at 65 152 142 68 36 18 13 g. HgCh at 100 208 196 110 64 48 44 Homeyer and Ritsert, Pharm. Ztg. 33. 738.) Solubility of HgCl 2 +NaCl at 25%. Composition of solution 26.5 18.66 18.71 18.64 18.87 14.97 14.03 13.25 13.17 12.97 13.14 13.15 % HgCh 51.35 51.32 51.42 51.26 57.74 59.69 62.16 62.59 62.50 62.48 62.55 Composition of undissolved residue 100 16.38 16.36 16.16 15.96 % HgCh 16.39 21.98 65.45 71.25 74.18 74.21 74.70 74.76 78.20 88.64 90.83 9.44 9.43 9.14 9.28 Solid ph NaCl NaCl+NaCl, HgCh, 2H 2 NaCl, HgCh, 2H 2 NaCl, HgCh, 2H 2 O+HgCh (Foote and Levy, Am. Ch. J. 1906, 36. 239.) 105.0 g. HgCl 2 are sol. in 1 1. of 0.1-N Hg(NO 3 ) 2 +Aq at 25. (Morse, Z. phys. Ch. 1902, 4 . 726.) Solubility in MCl+Aq at 25. Salt LiCl NaCl In 10 ccm. of the solution Millimols HgCh 2.65 3.51 6.66 10.21 16.78 22.14 28.96 30.62 2.65 3.72 5.08 7.48 11.92 20.22 27.54 34.34 Millimols salt 4.14 8.35 12.71 17.38 22.65 30.91 35.27 2.12 4.16 6.71 11.53 19.41 27.83 31.62 MERCURIC CHLORIDE 501 Solubility in MCl+Aq at 25. Continued. 16.2 mols. methyl, 12.4 mols. ethyl, and 18 mols. propyl alcohol at 20; in 6.8 mols. methyl, 10.6 mols. ethyl, and 14.6 mols. propyl alcohol at 38.2. (Timofejew, C. R, 112. 1224.) 100 pts. absolute methyl alcohol dissolve 66.9 pts. HgCl 2 at 25; 100 pts. absolute ethyl alcohol dissolve 49.5 pts. HgCl 2 at 25. (de Bruyn, Z. phys. Ch. 10. 783.) At 15, 1 pt. by weight is sol. in: 13.53 pts. H 2 O. 1.5 " methyl alcohol of sp. gr. 0.7990 2.5 " ethyl " " " " 0.8100 6.3 " propyl " " " " 0.8160 (Rohland, Z. anorg. 1899, 18. 328.) 100 g. HgCl 2 +CH 3 OH contain 1.2 g. HgCl 2 at the critical temp. (Centnerszwer, Z. phys. Ch. 1910, 72. 437.) Solubility of HgCl 2 in methyl alcohol +Aq at 25. P = g. alcohol in 100 g. alcohol -f-Aq. HgCl 2 = millimols HgCl 2 in 10 cc. of the solution. Salt In 10 com. of the solution Millimols HgCh Millimols salt KC1 2.65 3.55 3.81 8.36 . 1.74 2.21 6.83 MgCl 2 2.65 3.74 7.19 11.31 18.64 25.69 32.06 1.68 4.15 5.70 9.97 13.20 17.28 CaCl 2 2.65 3.64 7.66 11.08 18.11 26.45 33.04 1.90 4.02 6.56 9.64 14.29 17.23 SrCl 2 2.65 3.15 5.63 8.29 13.42 17.76 22.93 1.64 3.11 5.19 7.24 10.46 13.86 p HgCl 2 Sp. gr. 10.60 30.77 37.21 47.06 64.00 78.05 100 2.67 2.92 4.18 4.96 7.27 14.19 21.11 17.95 1.0565 1.0441 1.0420 .0507 .0809 .2015 .3314 .2160 BaCl 2 2.65 6.97 11.67 16.20 26.45 53.48 3.85 5.72 7.76 13.36 30.30 /"ET/vprr n-nrl A-n/^ofo *?. a-nrwer 1 QflT KO 1AK \ (Herz and Paul, Z. anorg. 1913, 82. 433.) Solubility in H 2 O is increased by presence of I 2 . (Herz and Paul, Z. anorg. 1914, 85. 214.) Solubility in H 2 O is increased by presence of hydroxylamine hydrochloride. (Adams, Am. Ch. J. 1902, 28. 213.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 64. 674.) Abundantly sol. in H 2 PtCl 4 +Aq. (Nilson, B. 1876, 9. 1146.) 100 cc. 90% ethyl alcohol dissolve 27.5 g. HgCl 2 at 15.5. Sp. gr. 15 of sat. solution = 1.065. (Greenish and Smith, Pharm. J. 1903, 71. 881.) 100 g. 99.2% ethyl alcohol dissolve 33.4 g. HgCl 2 at 25. (Osaka.) Solubility of HgCl 2 in ethyl alcohol +Aq at 25. P = g. alcohol in 100 g. alcohol +Aq. HgCl 2 = millimols HgCl 2 in 10 cc. of the solution. Sol. in 2.5 pts. cold alcohol (Richter) ; 3 pts. (Karl) ; 2.5 pts. alcohol of 0.833 sp. gr. at ordinary temp., and 1.167 pts. on boiling (Berzelius) ; 2 pts. alcohol of p HgCh Sp. gr. 0.816 sp. gr. at 15.5 (sp. gr. of solution =1.08) (J. Davy, Phil. Trans. 1822. 358). 2.67 1.0565 At 10, sol. in 2.57 pts. alcohol of 39 (Cartier), in 20 18 2 49 1 0214 2.9 pts. alcohol of 38; in 3.6 pts. alcohol of 35; in 4.2 pts. alcohol of 30; in 9.3 pts. alcohol of 22; in 14.6 pts. alcohol of 14. (N. E. Henry.) 40^69 70.01 3^94 8.70 i!oiso 1.0616 100 13.61 1 . 1067 Sol. in 25 mols. methyl 13.1 mols. ethyl and 20.3 mols. propyl alcohol at 8.5; in (Herz and Anders, Z. anorg. 1907, 62. 170.) 502 MERCURIC CHLORIDE Solubility of HgCl 2 in ethyl alcohol +Aq at 25. % C 2 H 6 OH % HgCl 2 % C 2 H 5 OH % HgCh 6.80 45.84 15.36 5.08 6.65 49.86 18.18 14.49 6.41 53.61 21.40 21 6.55 57.26 24.51 26.25 7.31 60.55 27.67 31.53 8.51 63.95 29.86 36.85 10.32 67.39 32.40 41.36 12.69 (Abe, J. Tok. Chem. Soc. 1912, 33. 1087.) Solubility in alcohol is increased by presence of hydroxylamine hydrochloride. (Adams, Am. Ch. J. 1902, 28. 213.) Solubility of HgCl 2 in a mixture of methyl and ethyl alcohol at 25. P = % methyl alcohol in the mixture. HgCl 2 = g. HgCl 2 in 10 ccm. of the solution. S=sp. gr. of the sat. solution. C 4.37 10.4 41.02 80.69 84.77 91.25 100 HgCl 2 3.686 3.943 4.261 5.837 6.167 5.782 5.385 4.862 S 25/4 c 107 130 157 294 1.321 288 254 216 (Herz and Kuhn, Z. anorg. 1908, 58. 161.) Solubility in mixtures of methyl and propy alcohol at 25. P=%pro 1 alcohol in the solvent. 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. P G S 25/4 4.862 1.2160 - 11,11 5,03^ 1.2278 23.8 5.714 1.2848 65.2 4.228 1.1568 91.8 2.509 1.0090 93.75 2.323 1.0029 96.6 2.152 0.9851 100 2.003 0.9720 (Herz and Kuhn, Z. anorg. 1908, 60. 157.) olubility in mixtures of propyl and ethyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. HgCl 2 in 10 ccm. of the solution. S = Sp. gr, of the sat. solution. 8.1 17.85 56.6 88.6 91.2 95.2 100 3.686 3.667 3.406 2.711 166 160 087 2.003 S 25/4 1.1070 1.0988 1.0857 1.0272 0.9854 0.9824 0.9772 0.9720 (Herz and Kuhn, Z. anorg. 1908, 60. 160.) Sp. gr. of HgCl 2 +alcohol. % HgClz 5.44 6.52 Sp. gr. 25/20 0.7948 0.8346 0.8431 (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 283.) Sp. gr. of alcoholic solution of HgCl 2 . HgCb 0.00 1.22 2.38 4.42 8.56 12.43 15.91 19.32 22.46 Sp. gr. at 0.83135 0.8397 0.8484 0.8635 0.8966 0.9306 0.9629 0.9951 1.0285 at 10 0.82286 0.8312 0.8399 0.8549 0.8877 0.9213 0.9523 0.9852 1.0184 at 20 0.81435 0.8228 0.8314 0.8463 0.8789 0.9119 0.9425 0.9753 1.0083 at 30 0.80594 0.8141 0.8227 0.8375 0.8689 0.9024 0.9329 0.9652 0.9982 (Schroder, B. 19. 161 R.) Sp. gr. at 16/4 of HgCl 2 +ethyl alcohol containing 23.5489% HgCl 2 = 0.99885; con- taining 11. 8801% =0.88572. (Schonrock, Z. phys. Ch. 1893, 11. 768.) Sp. gr. at 16/4 of HgCl 2 +amyl alcohol containing 10.9948% HgCl 2 = 0.89550. ' (Schonrock, Z. phys. Ch. 1893, 11. 769.) Sol. in 4 pts. ether (Karls); in 4.1 pts. (Henry); in 2.86 pts. ether of 0.745 sp. gr. (sp. gr. of solution = 1.08); the solvent power is not increased by elevating the temp., and b.-pt. of ether is not raised. (J. Davy.) Ether extracts HgCl 2 from HgCl 2 +Aq. (Orfila); very slightly if HgCl 2 +Aq is dil. (Lassaigne.) Very si. sol. in pure ether. (Polis, B. 20. 6.35 pts. are sol. in 100 pts. ether at 0. 6.44 " " " " 100 " " " 18. 6.38 " " " -" 100 " " " 35.5. (Laszczynski, B. 18.94, 27. 2286.) MERCURIC CHLORIDE 503 Sol. in 7J4-8 pts. ether. (Madsen, Ch. Z. Repert. 1897, 21. 169.) Solubility in 100 cc. ether at 17 = 4.1-4.12 g. (Stromholm, J. pr. 1902, (2), 66. 450.) The solubility of HgCl 2 in H 2 O is only si. affected by the presence of ether. An aqueous solution sat. with ether and HgCl 2 contains about 10% less HgCl 2 than a pure sat. aqueous solution. Partition coefficient for = 4.9 at 0; 3.02 at 14.6; 2.80 at 16.8. "(Stromholm, Z. phys. Ch. 1903, 44. 70.) 126.80 pts. HgCl 2 are sol. in 100 pts. acetone at 18. (Lasczynski, B. 1894, 27. 2287.) 1 g. HgCl 2 is sol. in 0.70 g. acetone at 18-. gr. of sat. solution 18/4 = 1.956.) (Naumann, B. 1904, 37. 4334.) Sat. solution in acetone contains 57.74 g. HgCl 2 in 100 g. solution at 25. (Foote and Haigh, J. Am. Chem. Soc. 1911, 33. 461.) Sp. gr. at 26.7/4 of HgCl 2 +acetone con- taining 36.25% HgCl 2 - 1.1585. (Schonrock, Z. phys. Ch. 1893, 11. 769. Sp. gr. of HgCl 2 + acetone. Solubility of HgCl 2 in ether+Aq at 25. % Ether % H 2 O % HgCl 2 87.86 1.2 5.2 5.4 5.4 5.22 93.6 90.5 91.8 93.1 6.92 5.2 4.3 2.8 1.5 % HgCl 2 Sp. gr. 20/20 10.94 21.05 0.8003 0.8847 0.9799 (Abe, J. Tok. Chem. So,c. 1912, 33. 1087.) (Le Blanc and Rohland, Z. phys. Ch. 1896. 19. 283.) 100 g. methyl acetate dissolve 46 g. at bpt. (56.5). (Schroeder and Steiner, J. pr. 1909, (2) 79. 49.) 1 g. HgCl 2 is sol. in 2.35 g. methyl acetate at 25. at 18. Sp. gr. 18/4 of the sat. solution = 1.251. (Naumann, B. 1909, 42. 3793.) Solubility in ethyl acetate. % Alcohol % IigCl 2 ' % Alcohol. % HgCh 67.57 58.59 51.02 44.79 38.69 32.84 32.43 32.50 37.39 37.96 38.24 37.75 27.16 22.48 15.20 8.97 36.29 34.08 28.55 20.67 5.49 Pts. sol. in 100 pts. ethyl acetate. Pts. HgCl 2 t , 28.92 29.03 30.71 31.87 32.77 35.98 13 35 48 60 83 (Abe.) 4 pts. ether dissolve 1 pt. HgCl 2 , but 4 pts. ether +1.33 pts. camphor dissolve 1.33 pts. HgCl 2 ; 4 pts. ether +4 pts. camphor dis- solve 2 pts. HgCl 2 ; 4 pts. ether +8 pts. cam- phor dissolve 4 pts. HgCl 2 ; 4 pts. ether +16 pts. camphor dissolve 8 pts. HgCl 2 . (Karls, Pogg, 10. 608.) 3 pts. alcohol dissolve 1 pt. HgCl 2 , but 3 pts. alcohol +1 pt. camphor dissolve 2 pts. HgCl 2 ; 3 pts. alcohol +3 pts. camphor dis- solve 3 pts. HgCl 2 ; 3 pts. alcohol+6 pts. camphor dissolve 6 pts. HgCl 2 . (Karls, I. c.) Solution can be obtained containing 25 pts. camphor, 16 pts. HgCl 2 , and only 4 pts. alcohol. Sp. gr. of solution = 1.326. (Simon, Pogg. 37. 553.) 100 pts. acetone dissolve 60 pts. HgCl 2 at 25. (Krug and M'Elroy, J. Anal. Appl. Ch. 184.) 9836 pts. HgCl 2 are sol. in 100 pts. acetone atO. 110.95 pts. HgCl 2 are sol. in 100 pts. acetone at 10. (Laszczynski, B. 1894, 27. 2286.) Solubility in ethyl acetate- 1 : 3.466 at 18. (Alexander, Dissert. 1899.) Solubility of HgCl 2 in ethyl acetate. Temp. 13 30 40.5 50.2 Mol. HgCl 2 in 100 mols. C 4 H 8 O 2 15.4 15.9 16.0 16.1 16.3 (Linebarger, Am. Ch. J. 1894, 16. 214.) 1 g. HgCl 2 is sol. in 3.5 g. ethyl acetate at 18. Sp. gr. of sat. solution 18/4 = 1.110. (Naumann, B. 1904, 37. 3602.) 504 MERCURIC CHLORIDE Solubility of HgCl 2 in ethyl acetate and Sat. solution acetone at t. Solvent t contains % HgCl 2 t Molecules HgCU sol. in 100 mol- ecules of ethyl Molecules HgClz sol. in 100 mol- ecules of acetone Solid present in acetone Ethyl alcohol 60 55 43 40 3.0 7.8 8.8 9.8 acetate 30 14.3 15 9.10 14.5 HgCl 2 , CH 3 COCH 3 23 21 18.6 1Q 1 9.25 14.3 ' 20 J-t7 . X 21.9 +10 10 .... 18.7 23.5 HgCl, 17 11 22.1 24.7 17 .... 23.2 , g 27 25 9.15 22.8 u 5 29^7 (Aten, Z. phys. Ch. 1906, 54. 121.) . + 3 29.0 30.0 7 30.9 Solubility of HgCl 2 in ethyl c\ pro acetate +Aq at 10 14 31.3 31.3 &V . 19 32.0 P = g. ethyl acetate in 100 g. ethyl acetate 31 34.2 +Aq. 43 36.4 HgCl 2 =millimols . HgCl 2 in 10 cc. of the 51 38.9 solution. 62 42.1 63 42 5 P HgCU Sp. gr. 68 44^7 A CT O 2.67 1.0565 80 45.2 48.0 4 .39 2.72 1.0581 92 51.0 96.76 15.34 1.2371 93 51.4 100 9.75 1.1126 100. 1 -1 K 53.6 ftfk A (Herz and Anders, Z. anorg. 1907, 52. 172.) 110 127 OU.O 65.3 138 67.8 1 pt. is sol. in 2.05 pts. ethyl acetate at 18 or 100 g. ethyl acetate dissolve 48.7 g. HgCl 2 . (Naumann, B. 1910, 43. 315.) N-propyl alcohol 32 22 14 14.7 15.4 15.6 16.4 Easily sol. in glycerine; sol. in 14 pts. glycerine. (Fairley, Monit. Scient. (3) 9. +16 41 16.5 18.2 23.8 685.) 53 27 9 100 g. glycerine dissolve 80 g. HgCl 2 at 25. (Moles and Maquina, Ann. Soc. Eshan. fis 62 67 29^4 32.7 quin. 1914, 12. 383.) 78 36.4 100 43.8 Solubility in organic solvents 127 52.7 Allyl alcohol -21 9O fi Solvent t Sat. solution 1 +J\J . \J 29.6 contains 1 9J HgCb -[- O oo . 22 48.7 Methyl alcohol 34 7.6 Acetone 23 51.4 20 11.5 18 52.9 15 12.8 15 56.6 2 18.7 10 56.7 + 4 23.2 8 58.4 12 27.6 4 59.1 36 53.1 1 60.1 51 61.0 + 6 61.9 62 63.6 12 61.4 64 63.7 15 61.8 74 64.3 27 62.0 100 68.7 36 61.9 127 75.2 54 62.1 MERCURIC CHLORIDE 505 Solubility in organic solvents. Continued. Solubility in organic solvents. -Continued. Solvent t Sat. solution contains % HgCU Solvent t Sat. solution contains % HgCh N-butyl alcohol 21 6 + 9 21 59 82 12.4 13.0 14.3 15.9 25.8 33.1 Acetic acid +21 22 33 43 50 61 87 95 95 115 116 127 145 182 207 2.7 3.0 5.0 6.0 6.7 8.0 11.0 12.0 12.5 16.0 17.0 20.0 26.3 44.8 55.2 Isobutyl alcohol 11 6 +11 63 98 127 145 155 5.5 6.2 6.7 7.5 19.3 32.1 42.0 47.2 50.4 Amyl alcohol 13 8.6 8.9 14.0 29.8 35.1 +26 50 90 106 Formic acid 21 50 90 2.0 3.2 7.3 Very si. sol. in propionic and isobutyric acids. (Etaid, A. ch. 1894, (7) 2. 557 et seq.) Solubility of HgCl 2 in organic solvents at t. Ether 47 40 35 30 19 +13 83 100 115 5.6 5.8 6.1 5.9 5.6 5.8 5.8 8.4 8.7 9.0 Solvent t % HgCI 2 Ethyl formate 20 3 +24 +46 29.6 29.2 30.0 31.0 CHC1 3 20.5 +44.2 0.01 0.12 C 6 H 6 +6.5 18.0 34.1 54.1 69.0 0.26 0.53 0.64 1.02 1.39 Ethyl acetate 50 20 14 6 + 7 19 45 66 100 131 150 180 39.6 40.5 40.2 40.0 39.5 39.9 40.2 41.6 44.0 47.8 50.1 57.0 59.3 C 2 H 4 C1 2 12.5 20.8 25.3 30.2 33.0 45.9 1.33 1.55 1.68 1.73 1.92 2.05 2.42 Methyl acetate 20 +24 55 42.0 40.3 41.5 CH 3 COOC 2 H5 6.5 26.1 38.5 45.3 22.8 22.7 22.8 23.5 26.4 Amyl acetate +22 48 18.3 18.5 Ethyl butyrate +20 55 71 12.6 13.5 15.1 Dukelski, Z. anorg. 1907, 63. 329. 506 MERCURIC CHLORIDE Solubility of HgCl 2 in mixed organic solvents at t. Solubility of HgCl 2 in mixed organic solvents at t Continued. Solvent t % HgCl 2 Solvent t HgCh C 6 H 6 +C 2 H 5 OH 2.5 0.0 6.0 20.5 20.65 24.5 34.5 54.4 54.5 15.20 15.40 16.38 18.40 18.50 19.33 21.34 24.84 24.42 C 2 H 4 C1 2 +CH 3 OH 0.0 12.5 20.8 25.3 30.2 33,0 37.4 45.9 13.33 21.30 29.23 34.78 36.87 37.01 37.95 39.36 CH 3 COOC 2 H 6 +C 6 H 6 0.0 6.5 '25.7 27.6 35.5 45.3 9.62 9.62 9.78 9.78 10.81 13.69 C6H 6 +2C 6 H 5 OH 5.2 +9.1 20.9 24.4 36.5 53.7 74.0 19.45 20.13 21.65 23.57 24.19 26.53 31.27 38.74 CH 3 COOC 2 H 6 +CHC1 3 0.0 26.1 36.1 46.0 48.5 3.34 4.07 4.78 5.38 5.10 CHC1 3 +C 2 H 6 OH 20.5 12.0 0.0 +8.0 23.0 38.5 44.2 45.6 3.82 4.43 4.89 5.37 7.12 8.51 9.51 9.98 2CH 3 COOC 2 H 6 +CC1 4 0.0 10.3 25.7 27.6 38.5 45.3 9.24 9.05 9.32 9.50 9.89 11.70 CHC1 3 +2C 2 H 6 OH 20.5 0.0 +8.0 23.0 38.5 44.2 6.60 7.69 8.96 10.66 12.50 14.40 (Dukelski, Z. anorg. 1907, 63. 335.) Solubility in organic solvents at 18/20. 100 g. chloroform dissolve 0.106 g. HgCl 2 . 100 g. tetrachlormethane dissolve 0.002 g. HgCl 2 . 100 g. bromoform dissolve 0.486 g. HgCl 2 . 100 g. ethyl bromide dissolve 2.010 g. HgCl 2 . 100 g. ethvlene dibromide dissolve 1.530 g. HgCl 2 . (Silk Z. anorg. 1900, 25. 401.) Solubility of HgCl 2 in various organic solvents at 25. G. =g. HgCl 2 dissolved in 1 mol. of solvent. CHC1 3 +CH 3 OH 12.0 0.0 +8.0 23.0 24.9 30.6 38.5 1.73 3.51 5.63 10.15 10.71 11.40 12.02 CHC1 3 +2CH 3 OH 12.0 0.0 +8.0 23.0 24.9 30.6 38.5 3.33 6.73 8.21 16.56 18.45 19.70 20.83 Solvent G. HgCl 2 Ethylene chloride 1 . 216 Tetrachlorethane 0.146 Chloroform 0.120 Dichlorethylene , 0.110 Pentachlorethylene . 039 Trichlorethylene . 036 Perchlorethylene . 012 Carbon tetrachloride Trace CC1 4 +2CH 3 OH 0.0 7.7 24.9 30.6 35.5 36.1 48.5 '5.20 6.69 14.06 19.40 20.50 21.80 21.90 (Hofman, et al., B. 1910, 43. 188.) Very si. sol. in nitromethane at ord. temp. Very sol. on warming. (Bruner, B. 1903, 36. 3298.) MERCURIC HYDROGEN CHLORIDE 07 Solubility in CS 2 at t. Solubility of HgCl2 in pyridine. Continued. t = point of fusion. Solid Phase = HgCl 2 , C 8 H 5 N. . t 100 pts. sat. solution contain pts. HgCh 10 5 + 5 10 15 20 25 30 0.010 0.014 0.018 0.022 0.026 0.032 0.042 0.053 0.063 t HgCl 2 t % HgCl 2 t H?C1 74.7 83.5 86.5 87.3 48.38 50.53 52.37 52.02 90.61 75.0 99.5 99.5 100.5 53.50 56.45 56.07 57.01 57.84 104.1 104.2 104.7 107. 60.09 60.72 58.97 63.06 Solid Phase = 3HgCl 2 , C 6 H 5 N. (Arctowski, Z. anorg. 1894, 6. 267.) 0.030 g. is dissolved in 100 g. sat. solution in CS 2 at 8. (Arctowski, Z. anorg, 1894, 6. 256.) Formic acid (95%) dissolves 2.1% at 19. (Aschan, Ch. Z. 1913, 37. 1117.) Sol. in molten urethane. (Castoro, Z. anorg. 1899, 20. 61.) Sol. in ethyl sulphocyanate. (Kahlenberg, Z. phys. Ch. 1903, 46. 66.) t A, t HgCl 2 t H&l, 94.7 95.2 106.4 109.8 60.72 60.77 61.93 62.58 113.6 114.0 115.7 118.2 63.06 63.18 63.37 64.09 124.2 129.4 145.5 65.00 65.63 69.66 (McBride, Z. phys. Ch. 1910, 14. 196.) Solubility in pyridine. S = temp. of solidification. Solubility of HgCl 2 in benzene. 100 pts. C 6 H 6 dissolve at: 15 41 55 84 0.54 0.62 0.85 1.80 pts. HgCl 2 . (Laszcynski, B. 1894, 27. 2287.) Solubility in C 6 H 6 = 0.0197 mol./l. at 25. (Sherrill, Z. phys. Ch. 1903, 43. 735.) Sol. in C 6 H 6 , toluene, xylene, and other aro- matic hydrocarbons. Insol. or only si. sol. in petroleum ether, hexane, decane and CS 2 . (Gulewitsch, B. 1904, 37. 1563.) Sol. in p-toluidine. (Werner.) Sol. in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 51. 236.) Solubility of HgCl 2 in pyridine. = point of fusion. Solid Phase = HgCl 2 , 2C 5 H 6 N. t % HgCl 2 t % HgCl 2 t A, 32.8 2.76 40.90 29.29 78.0 49.72 21.9 7.86 5C.10 34.94 78.7 50.37 + 0.02 13.14 60.03 40.36 80.2 51.52 12.58 17.34 7C.15 46.44 82.5 52.40 18.78 19.78 70.8 45.77 89.0 56.45 23.60 21.59 74.6 48.00 90.8 57.01 27.23 22.65 75.2 48.38 94.1 60.09 31.05 24.46 76.4 49.15 Mols. per 100 s Mols. per 100 . s Mols. per 100 s 5.8 19 27.0 87 38.5 130 5.9 18.5 28.6 (98) 41.0 137 10.2 39.5 30.3 91.5 43.2 142 14.1 52 31.2 92 44.0 143.5 21.4 74.5 33.1 108 47.5 159 25.0 83 35.1 115.5 52.8 173 (Staronka, Anz. Ak. Wiss. Krakau, 1910. 372.) Sp. gr. at 16/4 of HgCl 2 +pyridine contain- ing 17.53% HgCl 2 = 1.1523; containing 6.57% HgCl 2 = 1.0388. (Schonrock, Z. phys. Ch 1893, 11. 768.) Mol. weight determined in benzonitrile, methyl- and ethyl-sulphide. (Werner, Z. anorg. 1897, 15. 31. 26 and 30.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Easily sol. in oil of turpentine and other essential oils; si. sol. in cold benzene, but much more on heating, crystallising on cool- ing. (Franchimont, B. 16. 387.) Easily sol. in boiling creosote. Insol. in olive oil. Insol. in oils and fats but sol. when first dissolved in alcohol, free ether or anhydrous ketones. (Glock, Ch. Z. Repert. 36. 315.) Extracted from HgCl 2 +Aq by volatile oils. Mercuric hydrogen chloride (Chloromercuric acid), HgCl 2 , HCl = HHgCl 3 . Decomp. by H 2 O, (Boullay, A. ch. 34. 24o.) Easily decomposed. (Neumann, M. 10. 236.) 508 MERCURIC HYDRAZINE CHLORIDE HgCJ 2 , 2HC1+7H 2 O. Decomp. by H 2 O. (Ditte, A. ch. (5) 22. 551.) 3HgCl 2 , 4HC1+14H 2 0. As above. 2HgCl 2 , HC1+6H 2 O. As above. 4HgCl 2 , 2HC1+9H 2 O. As above. 3HgCl 2 , HCl-f 5H 2 O. As above. Mercuric hydrazine chloride, HgCl 2 , 2(N 2 H 4 , HC1). Very sol. in H 2 O. More sol. in hot alcohol than in cold; decomp. by HNO 3 . (Curtius, J, pr. 1894, (2) 50. 332.) Mercuric nickel chloride, basic, HgCl 2 , 6NiO, NiCl 2 +20H 2 O, and HgCl 2 , 7NiO, NiCl 2 . (Mailhe, A. ch. 1902, (7) 27. 369.) Mercuric nickel chloride. Deliquescent, (v. Bonsdorff.) Mercuric nitrosyl chloride, HgCl 2 , NOC1. Sol. in H 2 O without effervescence. (Sud- borough, Chem. Soc. 59. 659.) Mercuric phosphoric chloride, 3HgCl 2 , 2PC1 5 . Decomp. and dissolved by H 2 O. (Baudri- mont, A. ch. (4) 2. 45.) Mercuric potassium chloride, 2HgCl 2 , KC1+ 2H 2 O. Very easily sol. in warm H 2 O. A clear solution at 18 is filled with crystals at 15. SI. sol. in alcohol, (v. Bonsdorff, Pogg. 17. 122.) HgCl 2 , KC1+H 2 O. Easily sol. in H 2 O; si. sol. in alcohol, (v. Bonsdorff, Pogg. 19. 336.) HgCl 2 , 2KC1+H 2 O. As above. Solubility determinations show that the double salts formed by mercuric and potas- sium chlorides at 25 are: 2KC1, HgCl 2 +H 2 0. KC1, HgCl 2 +H 2 O. Can be recryst. with- out decomp. KC1, 2HgCl 2 +2H 2 O. Gives HgCl 2 on recryst. from H 2 O. (Foote and Levy, Am. Ch. J. 1906, 35. 237.) Mercurous rhodium chloride. See Chlororhodite, mercurous. Mercuric rubidium chloride, HgCl 2 , RbCl. Sol. in H 2 O. HgCl 2 , 2RbCl. Sol. in H 2 O and HCl+Aq. (Godeffroy, Arch. Pharm. (3) 12. 47.) +2H 2 O. Sol. inH 2 O. (Godeffroy.) 2HgCl 2 , RbCl. Sol. in H 2 O. (Godeffroy.) Solubility determinations show that at 25 there exist five double mercuric rubidium chlorides with the following formulas: RbCl, 5HgCl 2 . Gives HgCl 2 on recryst. from H 2 O. 3RbCl,4HgCl 2 +H 2 O. Gives RbCl, 5HgCl 2 on recryst from H 2 O. RbCl, HgCl 2 +H 2 O. Gives 3RbCl, 4HgCl 2 on recryst. from H 2 O. 3RbCl, 2HgCl 2 +2H 2 O. Gives 3RbCl, 4HgCl 2 on recryst. from H 2 O. 2RbCl, HgCl 2 +H 2 O. Gives 3RbCl, 4HgCl 2 on recryst from H 2 O. (Foote and Levy, Am. Ch. J. 1906, 35. 241.) Mercurous silver chloride, HgCl, AgCl. (Jones, J. Soc. Chem. Ind. 1893, 12. 983.) 2HgCl, AgCl. Min. Bardosite. (Jones, J. Soc. Chem. Ind. 1893, 12. 983.) 3HgCl, AgCl. (Jones, Chem. Soc. 1910, 97. 338.) Mercuric sodium chloride, HgCl 2 , NaCl. Sp. gr. at 16/4 of aqueous solution con- taining 14.937% salt = 1.13310; containing 11.0736% = 1.09528. (Schonroek, Z. phys. Ch. 1893, 11. 782.) +H 2 O. (Linebarger, Am. Ch. J. 1893, 16. 344.) +1^H 2 0. Sol. in 0.33 pt. H 2 O at 15. (Schindler, Repert. 36. 240.) Extremely easily sol. in alcohol. (Voit.) Sol. in 275 pts. ether. Ether dissolves the undecomposed salt out of H 2 O solution. (Lassaigne, A. ch. 64. 104.) HgCl 2 , 2NaCl. Deliquescent. Very sol. in H 2 O. (Voit, A. 104. 354.) 2HgCl 2 , NaCl. Decomp. by H 2 O in dil. solution. Sol. in acetone and acetic ether. (Linebarger, Am. Ch. J. 1893, 15. 344.) Solubility determinations show that the only double salt formed by mercuric and sodium chlorides between 10.3 and 25 is NaCl, HgCl 2 +2H 2 O. Can be recryst. from H 2 O. (Foote and Levy, Am. Ch. J. 1906, 35. 237.) Mercuric strontium chloride, basic, SrCl 2 , HgO+6H 2 0. Decomp. by H 2 O. (Andre, C. R. 104. 431.) Mercuric strontium chloride, 2HgCl 2 , SrCl 2 + 2H 2 O. Easily sol. in H 2 O. (v. Bonsdorff.) 3HgCl 2 , SrCl 2 +5-6H 2 O. Very sol. in H 2 O. (Swan, Am. Ch. J. 1898, 20. 632.) Mercurous sulphur chloride. See Mercurous sulphochloride. Mercuric thallous chloride, HgCl 2 , T1C1. Easily sol. in H 2 O. (Jorgensen, J. pr. (2) 6. 83.) Mercurous stannous chloride, Hg 2 Cl 2 , SnCl 2 . Decomp. by H 2 O. (Capitaine. J. Pharm. 25. 549.) Mercuric yttrium chloride, 3HgCl 2 , YC1 3 + 9H 2 O. Deliquescent. Verv sol. in H 2 O. (Popp, A. 131. 179.) MERCUROUS IODIDE 509 Mercuric zinc chloride, HgCl 2 , ZnCl 2 . Very sol. in H 2 O. (Harth, Z. anorg. 1897, 14. 323.) 2HgCl 2 , ZnCl 2 . (Varet, C. R. 1896, 123. 422.) Mercuric zinc chloride ammonia, HgCl 2 , 4ZnCl 2 , 10NH 3 +2H 2 O. Insol. in boiling H 2 O, but decomp. thereby. (Andre, C. R. 112. 995.) HgCl 2 , 2ZnCl 2 , 6NH 3 + ^H 2 O. As above. (Andre.) Mercuric chloride ammonia, HgCl 2 , 12NH 3 . SI. sol. in ammonia. (Franklin, Am. Ch. J. 1900, 23. 300.) Mercuric chloride cadmium oxide, HgCl 2 , CdO+H 2 O. (Mailhe, A. ch. 1902, (7) 27. 371.) Mercuric chloride cobaltous oxide, HgCl 2 , (Mailhe, C. R. 1901, 132. 1274.) Mercuric chloride cupric oxide, HgCl 2 , 3CuO +H 2 0. (Mailhe, Bull. Soc. 1901, (3) 25. 791.) Mercuric chloride hydrazine, HgCl 2 , N 2 H 4 . Very unstable. Decomp. by H 2 O. Pptd. from alcohol solution by H 2 O; very sol. in min. acids with decomp. Easily sol. in HC1 or HNO 8 . Decomp. by alkalies. Somewhat sol. in acetic acid. (Hof- mann, B. 1897, 30. 2020.) Mercuric chloride hydroxylamine, HgCl 2 , 2NH 2 OH. Completely sol. in methyl and ethyl al- cohol; insol. in ether: decomp. by H 2 O and NaOH+Aq. Sol. in NH 2 OH,HCl+Aq. (Adams, Am. Ch. J. 1902, 28. 210.) Mercuric chloride lead oxide, HgCl 2 , 2PbO + 2H 2 0. (Mailhe, A. ch. 1902, (7) 27. 372.) Mercuric chloride strontium chromate, 2HgCl 2 , HC1, SrCrO 4 . Sol. in H 2 O without decomp. (Imbert, Bull. Soc. 1897, (3) 17. 471.) Mercuric chloroiodide, 2HgCl 2 , HgI 2 . Sol. in H 2 O. (Liebig.) HgCl 2 , HgI 2 . SI. sol. in hot H 2 O with partial decomp. More easily sol. in alcohol. (Kohler, B. 12. 1187.) Mercurous fluoride, Hg 2 F 2 . Decomp. by H 2 O with separation of Hg 2 O. Mercuric fluoride, HgF 2 +2H 2 O. Decomp. by cold H 2 O, with separation of HgO. Sol. in dil. HNO 3 +Aq, and HF+Aq. (Finkener, Pogg. 110. 628.) Mercurous hydrogen fluoride, Hg 2 F 2 , 4HF + 4H 2 0. Deliquescent. Easily sol. in H 2 O. Sol. in dil. acids and dil. HF. (Bohm, Z. anorg. 1905, 43. 327.) Mercurous silicon fluoride. See Fluosilicate, mercurous. Mercurous fluoride ammonia, Hg 2 F 2 , 2NH 3 . Stable on air. (Finkener, Pogg. 110. 142.) Mercurous hydroxide, HgOH. Nearly insol. in cold, sol. in hot H 2 O. Sol. in NaOH+Aq. (Bhaduri, Z. anorg. 1897, 13. 410.) Mercurous iodamide, Hg 2 (NH 2 )I. (Rammelsberg, Pogg. 48. 184.) Is a mixture of Hg and Hg(NH 2 )l. (Bar- foed.) Mercurous iodide, Hg 2 I 2 . Sol. in over 2375 pts. H 2 O. (Saladin,.J. chim. med. 7. 530.) Solubility in H 2 O = 2.6x 10 8 g.-equiv. per liter (calculated). (Bodlander, Z. phys. Ch. 1898, 27. 58.) Solubility in H 2 O = 3 x 10 - 10 mols. per litre at 25. (Sherrill, Z. phys. Ch. 1903, 43. 735.) Sol. in Hg(NO 3 ) 2 +Aq. (Stromann, B. 20. 2815.) Sol. in KI+Aq. Easily sol. in Hg 2 (NO 3 ) 2 + Aq. SI. sol. in NH 4 OH+Aq. Sol. in hot NH 4 Cl+Aq, but less than HgI 2 . Less sol. in NH 4 NO 3 than in NH 4 Cl+Aq. (Brett.) Partially sol. with separation of Hg and formation of HgI 2 , in cold KI+Aq, hot Nal, CaI 2 , SrI 2 , BaI 2 , MgI 2 , ZnI 2 , and NH 4 I+Aq; in warm NaCl, KC1 and NH 4 Cl+Aq, and slowly in hot HCl+Aq. (Boullay, A. ch. (2) 34. 358.) Decomp. by alkali chlorides +Aq. (Miahle, A. ch. (3) 6. 177.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Not wholly insol. in alcohol, ether, or chlor- oform. (Maclagan, Rep. anal. Ch. 1884. 378.) Decomp. by boiling alcohol: 1000 g. boiling alcohol decomp. about 3.15 g. Hg 2 I 2 . (Fran- gois, C. R. 1896, 121. 890.) Boiling alcohol decomp. Hg 2 I 2 to Hg and HgI 2 which dissolves until 0.220 g. HgI 2 are contained in 100 g. alcohol. (Frangois, C. R. 1896, 121. 889.) Insol. in cold ether. (Frangois, J. Pharm. 1897, (6), 6. 445.) Insol. in methylene iodide. (Retgers, Z. anorg. 3. 345.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Phenol at 180 decomp. it into Hg and HgI 2 until a state of equilibrium is reached with 510 MERCURIC IODIDE 2.75 g. HgI 2 to 100 g. phenol, above which point Hgl is si. sol. (0.05 g. in 100 g.) in phenol-HgI 2 mixture. Decomp. by cold aniline more rapidly than by hot. Equil- ibrium is reached when 26.35 g. HgI 2 are present to 100 g. aniline at bpt. of aniline. Aniline containing more than 26 g. HgI 2 to 100 g. dissolves Hgl in considerable quan- tity. (Francois, C. C. 1896, I, 470.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) SI. sol. in allyl mustard oil. (Mathews, J. phys. Chem. 1905, 9. 647.) Mercuric iodide, HgI 2 . Sol. in 150 (?) pts. H 2 O. (Wiirtz.) 1 1. H 2 O at 17.5 dissolves 0.0403 g. HgI 2 . (Bourgpin, A. ch. (6) 3. 429.) Sol. in about 6500 pts. H 2 O. (Hager.) According to calculation from electrical conductivity of HgI 2 +Aq, HgI 2 is much less sol., 1 1. H 2 O dissolving only 0.5 mg. HgI 2 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) 1 1. H 2 O dissolves 0.054 g. HgI 2 at 22. (Rohland, Z. anorg. 1898, 15. 412.) 1 1. H 2 O at 25 dissolves about 0.06 g. (Morse, Z. phys. Ch. 1902, 41. 731.) 1 1. H 2 O at 18 dissolves 4x10^ mol. (Abegg, Z. Elektrochem. 1903, 9. 553.) Solubility in H 2 O at 25 = 0.00013 mol. liter. (Sherrill,.Z. phys. Ch. 1903, 43. 735.) 1 1. H 2 O dissolves 0.4 mg. HgI 2 at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 1 1. H 2 O at 18 dissolves 0.2 to 0.4 mg. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) The yellow modification is always deposited from solution even in the presence of an ex- cess of the red form. (Gernez, C. R. 1903, 136. 1323.) Sol. in many acids, especially in HC1, and HI+Aq. Insol. in HC 2 H 3 2 +Aq. (Berthe- mot.) Scarcely sol. in dil. HNO 3 +Aq. Not attacked by cold H 2 SO 4 , decomp. by hot. (Ditte, A. ch. 1879, (5) 17. 124.) Sat. solution in H 2 SO 3 +Aq contains at critical temp. (158.2), 0.7% HgI 2 . (Niggli, Z. anorg. 1912, 75. 182.) Sol. in hot (NH 4 ) 2 CO 3 , (NH 4 ) 2 SO 4 , cold NH 4 C1, NH 4 NO 3 , or ammonium succinate+ Aq. (Wittstein.) Sol. in HgCl 2 , Hg(N0 3 ) 2 , or Hg(C 2 H 3 O 2 ) 2 + Aq. Easily sol. in Na 2 S 2 O 3 +Aq. Easily sol. in soluble iodides +Aq. More sol. in hot than in cold Nal or KI+Aq. When cone., 1 mol. KI in hot solution dissolves 3 mols. HgI 2 , but a portion separates on cooling: BaI 2 , SrI 2 , MgI 2 , and CaI 2 act in the same way. Easily sol. in cold, more sol. in hot ZnI 2 +Aq, 2 mols. HgI 2 beipg dissolved to 1 mol. ZnI 2 . In NHJ +Aq, 3 mols. HgI 2 are dissolved to 2 mols. NHJ. Abundantly sol. in hot KC1, NaCl, NH 4 Cl+Aq, but separates out on cooling, and the trace remaining may be pptd. by H 2 O, 2 g. KC1 in solution dissolves 1.166 g. HgI 2 . Sol. in HgCl 2 +Aq, and very easily sol. in alcoholic solution of HgCl 2 . (Boullay, A. ch. (2) 34. 346.) Solubility in MI+Aq at 25. Salt In 10 ccm. of the solution Millimols HgI 2 Millimols salt Nal 4.12 6.22 9.45 7.94 13.85 22.25 KI 1.27 1.80 5.10 7.00 12.24 3.03 3.90 10.34 15.54 25.19 CaI 2 0.50 2.61 4.40 4.58 17.06 0.53 2.52 4.68 4.84 17.99 SrI 2 2.12 3.20 5.82 6.94 2.54 3.55 5.39 6.08 BaI 2 0.59 7.42 8.98 14.62 0.99 7.48 9.78 15.08 (Herz and Paul, Z. anorg. 1913, 82. 434.) Solubility of HgI 2 +KI in H 2 0. Temp =20. %KI % Hgl 2 Solid phase 50.9 44.4 39 37.4 37.8 35.1 35.5 26.7 26.6 23.7 14.9 19.3 32.4 48 53.6 52.6 52.2 51.2 50.3 49.4 . 40.2 22.5 KI KI+KHgI 3 KHgI 3 1C KHgI 3 , H 2 O KHgI 3 +HgI 2 HgI 2 u Temp. =30 60.6 40 39.6 40 40.2 39.3 33.7 33 31.4 29.1 53 52.7 52.2 51.2 50.3 49.8 52 51.7 52.2 KI KI-fKHgI 3 KHgI 3 KHgI 3 , H 2 (Dunningham, Chem. Soc. 1914, 105. 368.) MERCURIC IODIDE 511 Very sol. in KSCN+Aq. (Philipp, Pogg. 1867, 131. 93.) Sol. in 1.09 pts. cryst. Na 2 S 2 O 3 +Aq. (Eder and Uhn, M. 1882,' 3. 197.) Very sol. in hot CaCl 2 +Aq, less sol. in BaCl 2 , KC1 and NaCl+Aq. (Lea, Z. anorg. 1896, 12. 341.) Solubility in normal Hg(NO 3 ) 2 +Aq = 48.0 g. per litre. (Morse, Z. phys. Ch. 1902, 41. 731.) Extremely sol. in cold cone. NH 4 Br+Aq. (Grossmann, B. 1903, 36. 1602.) Sol. in alkali sulphites +Aq. (Barth, Z. phys. Ch. 1892, 9. 215.) Sol. in Ca(OCl) 2 +Aq; sol. in KOH+Aq. (Melsens, A. ch. (3) 26. 222.) Sol. in liquid SO 2 . (Walden and Cent- nerszwer, C. C. 1992, I. 344.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Sol. in SOC1 2 , S 2 C1 2 , SO 2 C1 2 , warm AsCl 3 , PBr 3 , warm POC1 3 . (Walden, Z. anorg. 1900, 25. 212.) Easily sol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Insol. in liquid CO 2 . (Buchner, Z. phys. Ch. 1906, 64. 674.) More sol. in alcohol than in H 2 O. 1 1. H 2 O containing 10% of 90% alcohol dis- solves 0.08 g. HgI 2 . 1 1. of alcohol of 80 B. dissolves 2.851 g. HgI 2 , 1 1. absolute alcohol dissolves 11.86 g. HgI 2 . (Bourgoin, A. ch. (6) 3. 429.) Sol. in 130 pts. cold, and 15 pts. hot 90% alcohol. (Hager.) 100 pts. absolute methyl alcohol dissolve 3.16 pts. at 19.5; 100 pts. absolute ethyl alcohol dissolve 2.09 pts. at 19.5. (de Bruyn, Z. phys. Ch. 10. 783.) 0.00842 pt. is sol. in 1 pt. alcohol at 15. (Gautier and Charpy, C. R. 1890, 111. 647.) 100 g. methyl alcohol dissolve 3.7 g. HgI 2 at 19; ethyl alcohol, 1.86 g.; propyl alcohol, 1.25 g.; isobutyl alcohol, at 22.5, 0.51 g. (Timofeiew, Dissert. 1894.) At 15-20, 100 g. methyl alcohol dissolve 3.24 g. HgI 2 ; ethyl alcohol, 1.42 g.; propyl alcohol, 0.826 g. (Rohland, Z. anorg. 1898, 16. 412.) Solubility of HgI 2 in ethyl alcohol+Aq at 25. A = g. alcohol in 100 g. alcohol+Aq. HgI 2 =millimols. HgI 2 in 100 cc. of the solution. A HgI 2 Sp. gr. 100 95.82 92.44 86.74 78.75 67.63 3.86 2.56 1.92 1.38 0.935 0.45 0.80325 0.80950 0.81536 0.82996 0.84654 0.87214 f p HgI 2 Sp. gr. 70.01 100 0.061 0.386 0.8636 0.8032 (Herz and Knoch, Z. anorg. 1905, 45. 266.) Solubility of HgI 2 in methyl alcohol+Aq at 25 . P = g. alcohol in 100 g. alcohol+Aq. HgI 2 = millimols. HgI 2 in 10 cc. of the solution. p HgI 2 Sp. gr. 47.06 64.00 78.05 100 0.0013 0.0098 0.0347 0.0981 0.571 o!9is7 0.8834 0.8519 0.8155 (Herz and Anders, Z. anorg. 1907, 62. 165.) Solubility of HgI 2 in ethyl alcohol+Aq at 25. P = g. alcohol in 100 g. alcohol+Aq. HgI 2 = miUimols. HgI 2 in 10 cc. of the solu- tion. (Herz and Anders, Z. anorg. 1907, 52. 170.) At 15, 1 pt. by weight is sol. in: 24813 pts. H 2 O. 30.8 pts. methyl alcohol of sp. gr. at 0.7990. 70.3 " ethyl " " " "' "0.8100. 121.0 " propyl " " " " "0.8160. (Rohland, Z. anorg. 1899, 18. 328.) Solubility of HgI 2 in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the mixtures. HgI 2 = g. HgI 2 in 10 com. of the solution. S 25/4 = Sp. gr. of the sat. solution. P HgI 2 S 25/4 0.180 0.8038 4.37 0.193 0.8039 10.4 0.208 0.8046 41.02 0.232 0.8077 80.69 0.289 0.8131 84.77 . 0.296 0.8140 91.25 0.298 0.8146 100 0.316 0.8156 (Herz and Kuhn, Z. anorg. 1908, 58. 164.) 512 MERCURIC IODIDE Solubility in mixtures of methyl and propyl alcohol at 25 Solubility in organic solvents at t. P = % propyl alcohol in the solvent. G = g. HgI 2 in 10 ccm. of the solution. Solvent t 100 g. of the solvent dissolve g. HgI 2 Q Qri rrr+ .rvf fKj-v n,n f j-k1n 4 i.n.-n. r^Vi 1 nvnf /~wm A1 p G S 25/4 v^moroiorm Tetrachlormethane Ol 75 . 163 0.094 0.316 0.8156 Ethylene dichloride Isobutyl chloride 85.5 69 1.200 0.328 23.8 0.304 0.8155 Ethyl bromide 38 0.773 91.8 0.169 0.8101 Methyl alcohol 66 6.512 93.75 96.6 100 0.167 0.153 0.142 0.8110 0.8108 0.8116 Ethyl alcohol Isopropyl alcohol Isobutyl alcohol 78 81 ca. 100 4.325 2.266 2.433 (Herz and Kuhn, Z. anorg. 1908, 60. 158.) Methyl formate Ethyl formate 36-38 52-55 1.166 2.150 Solubility in mixtures of propyl and ethyl alcohol at 25 Methyl acetate Ether 56-59 35 2.500 0.470 P= % propyl alcohol in the solvent. G=g. HgI 2 in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. Acetone Acetal Chloral Epichlorhydrin 56 ca. 100 96 ca. 100 3.249 2.000 p G S 25/4 Hexane 67 0.072 Benzene 80 825 0.180 0.8038 Ethyl acetate 74-78 4.200 . 1 17.85 . 173 0.165 0.8036(?) 0.8043 (Sulc, Z. anorg. 1900, 26. 402.) 56 6 155 8075 91.2 95 2 0.152 144 0.8099 8108 Solubility in organic solvents at 18-20. 100 g. chloroform dissolve 0.040 g. HgI 2 . 100 0.142 0.8116 100 g. tetrachlormethane dissolve 0.006 g. (Herz and Kuhn, Z. anorg. 1908, 60. 161.) Solubility in 100 pts. amyl alcohol equals: 0.66 pts. at 13. 3.66 " " 71. 5.30 " " 100. 9.57 " " 133.5. (Laszcynski, B. 1894, 27. 2287.) Sp. gr. at 16/4 of HgI 2 +alcohol contain- ing 1.8358% Hglo = 0.80718; containing 1.7119% =0.80597. (Schonrock, Z. phys. Ch. 1893, 11. 770.) . Somewhat sol. in ether. Sol. in 77 pts. ether. (Saladin.) Sol. in 60 pts. ether. (Hager.) Sol. in cold ether. (Francois, J. Pharm. 1897, (6) 6. 445.) Very si. sol. in anhydrous ether. (Hampe.) 0.62 pt. is sol. in 100 pts. ether at 0. 0.97 pt. is sol. in 100 pts. ether at 36. (Laszcynski, B. 1894, 27. 2286.) Solubility in ether = 0.3% at ord. temp. (Marsh, Chem. Soc. 1910, 97. 2299.) Nearly insol. in ether. (Dunningham, Chem. Soc. 1914, 105. 368.) Data are given on the system HgI 2 +KI + ether. (Dunningham.) Solubility at 23 in chloroform = 0.071%; in ether = 0.551%; in acetone = 2. 005%: in ethyl alcohol =2%; in methyl alcohol =. 3.975%; in benzene = 0.247%. (Beckmann and Stock, Z. phys. Ch. 1895, 17. 130.) 100 g. bromoform dissolve 0.486 g. HgI 2 . 100 g. ethyl bromide dissolve 0.643 g. HgI 2 . 100 g. ethyl iodide dissolve 2.041 g. HgI 2 . 100 g. ethylene dibromide dissolve 0.748 g. HgI 2 . (Sulc, Z. anorg. 1900, 25. 401.) 1 pt. ethylene bromide dissolves 0.00553 pts. HgI 2 at 15. (Gautier and Charpy, C. R. 1890, 111. 647.) 100 pts. methylene iodide CH 2 I 2 dissolve 2.5 pts. HgI 2 at 15, 16.6 pts. at 100, and 58 pts. at 180. (Retgers, Z. anorg. 3. 252.) 1 1. sat. solution in CC1 4 at 15 contains 0.170 g. HgI 2 . (Dawson, Chem. Soc. 1909, 95. 874.) Sol. in 340 pts. glycerine. (Fairley, Monit. Scient. (3) 9. 685.) 100 pts. acetone dissolve 2.09 pts. HgI 2 at 25. (Krug and M'Elroy, J. Anal. Ch. 6. 84.) Sol. in acetone and in methylal. (Eidmann, C. C. 1899, II, 1014.) Solubility in 100 pts. acetone equals: 2. 83 pts. HgI 2 at 1. 3.36 " " " 18. 4.73 " " " 40. 6.07 " " " 58. (Laszczynski, B. 1894, 27. 2287.) 100 g. methyl acetate solution, sat. at 18, contain 1.10 g. HgI 2 . (Bezold, Dissert. 1906.) MERCURIC IODIDE 513 100 g. boiling methyl acetate slowly dis- solve 2.3 g. Hgl2. (Schroeder and Steiner, J. pr. 1909, (2) 79. 49.) Solubility in ethyl acetate at t e Pts. sol. in 100 pts. ethyl acetate t 1.49 2 1.56 + 17.5 1.64 21 2.53 40 3.19 55 4.31 76 (Laszczynski, B. 1894, 27. 2286.) 100 g. ethyl acetate anhydrous, or sat. with H 2 O at 18, dissolve at 18, 14.70 g. Hgl2. Solubility increases somewhat with temp. (Hamers, Dissert. 1906.) Solubility of HgI 2 in ethyl acetate +Aq at 25. P = g. ethyl acetate in 100 g. ethyl acetate +Aq. HgI 2 = millimols. HgI 2 in 10 cc. of the solution. p HgI 2 Sp. gr. 4.39 96.76 100 0.0028 0.412 0.241 0.9973 0.9063 0.9011 (Herz and Anders, Z. anorg. 1907, 52. 172. 1 pt. is sol. in 68.03 pts. ethyl acetate at 18. (Naumann, B. 1910, 43. 316.) Solubility in diethyl oxalate is 12.5% at bpt. and 2.5% at 100. (Reinders, Z. phys. Ch. 1900, 32. 507.) Solubility in CS 2 at t. Solubility in CS 2 . 100 g. of the sat. solution contain at: 86.5 93 116 0.024 0.023 0.017 g. HgI 2 . (Arctowski, Z. anorg. 1896, 11. 274.) 0.0028 pt. is sol. in 1 pt. CS 2 at 15. (Gau- tier and Charpy, C. R. 1890, 111. 647.) 1 1. sat. solution in CS 2 at 15 contains 3.127 g. HgI 2 . (Dawson, Chem. Soc. 1909, 95. 874.) Very sol. in liquid methylamine. (Gibbs, J. Am. Chem. Soc. 1906, 28. 1419.) Abundantly sol. in methylamine. (Fitz- gerald, J. phys. Chem. 1912, 16. 633.) Somewhat sol. in allyl mustard oil. (Math- ews, J. phys. Chem. 1905, 9. 647.) Sol.inSb(CH 3 ) 4 I+Aq. Very si. sol. in Na citrate +Aq. (Spiller.) 1 pt. C 6 H 6 dissolves 0.00217 pts. HgI 2 at 15. (Gautier and Charpy, C. R. 1890, 111. 647.) Solubility in 100 pts. benzene equals: 0.22 pts. at 15. 0.88 " " 60. 0.95 " " 65. 1.24 " "84. (Laszczynski, B. 1894, 27. 2284.) 1 1. C 6 H 6 dissolves 0.00493 mol. HgI 2 at 25. (Sherrill, Z. phys. Ch. 1903, 43. 735.) 100 g. boiling phenol dissolve 10 g. HgI 2 . (Francois, C. R. 1895, 121. 769.) SI. sol. in phenol with 20% H 2 O. Not very sol. in acetic acid at 119, in amyl acetate at 133, in amyl bromide at 119. Rather sol. in diethyl oxalate at 186, in ethylene brom- ide at 131, in amyl alcohol at 137, in amyl iodide at 150, in CHBr 3 at 151, in iodo- benzol at 190, in oil of turpentine at 160. Very sol. in benzaldehyde at 179, in methyl- ene iodide at 182. (Reinders, Z. phys. Ch. 1900, 32. 506.) 1000 pts. oil of bitter almonds dissolve 4 pts. HgI 2 at ord. temp.; 1000 pts. olive oil, 4 pts.; 1000 pts. poppy oil, 10 pts.; 1000 pts. nut oil, 15 pts.; 1000 pts. castor oil, 20 pts.; 1000 pts. lard oil, 4. 5 pts.; 1000 pts. vaseline, 2.5 pts.; 1000 pts. benzene, 4 pts. Sol. in phenol. (Mehn, Pharm. J. 3. 327; B. 19. 8 t 100 pts. sat. solution contain pts. Hgl2 R.) Solubility in aniline. S = Temp. of solidification. 10 0.107 0.141 0.173 0.207 0.239 0.271 0.320 0.382 0.445 + 5 10 15 20 25 30 Mols. per 100 s Mols. per 100 s Mols. per 100 s 5.9 8.2 10.3 14.9 16.6 12 22.5 29 41.5 45 19.9 25.8 29.3 31.7 32.4 48.5 53.5 105 122 (55) 33.0 35.6 37.5 39.2 128 140 147 156 (Arctowski, Z. anorg. 1894, 6. 267.) (Staronka, Anz. Ak. Wiss. Krakau, 1910. 372.) 514 MERCURIC IODIDE Solubility of HgI 2 in aniline at t. t g. HgI 2 per 100 g. aniline Solid phase 6.5 23.35 Hgl, 2C 6 H 5 NH 2 +0.4 28.69 it 17.8 42.85 (( 21.1 47.55 K 26.9 55.47 (t 30.1 62.05 ft 36.2 75.80 11 42.9 96.49 1C 46.8* " +HgI 2 (red) 48.8 128 '.I HgI 2 (red) 63.6 163.8 (i 70. 2 184.1 (i 76.2 201.6 (i 95.9 246.7 it 108.* HgI 2 (red)+HgI 2 (yellow) 115.7 28i!s HgI 2 (yellow) 137.2 285.2 n 181.1 279 n 199.1 863.2 te * Transition point. (Pearce and Fry, J. phys. Ch. 1914, 18. 667.) Very sol. in boiling alcoholic solution of aniline. (Vohl, Dissert. 1871.) Abundantly sol. in hot benzonitrile and other aromatic nitriles. (Werner, Z. anorg. 1897, 16. 7.) Sol. in benzonitrile (0.98 g. in 100 g. at 18). 20 times more sol. by addition of 5 g. KI to 100 cc. benzonitrile. (Naumann, B. 1914, 47. 1375.) Sol. in pyridine. (Naumann, B. 1904, 37. 4609.) Solubility of HgI 2 in pyridine. S = temp. of solidification. Mols. per 100 S Mols. per 100 s Mols. per 100 s 5 10 34.6 107 51.3 93.5 9.8 42.5 38.0 103 51.6 96 15.14 66.5 43.0 97 52.7 108 19.3 83 46.7 88.5 53.2 109 26.3 102.5 48.5 89 55.4 122 29.6 107 50.6 89 57.9 135 (Staronka, Anz. Ak. Wiss. Krakau, 1910. 372.) Sp. gr. at 16/4 of HgI 2 +pyridine con- taining 10.43% HgI 2 = 1.1482; containing 7.99% = 1.1053. (Schonrock, Z. phys. Ch. 1893, 11. 770.) Solubility of HgI 2 in quinoline. temp, of solidification. Mols. per 100 s Mols. per 100 s Mols. per 100 s 4.7 9.1 13.2 23.1 26.7 100 115.5 133.5 138 145 29.8 31.4 35.4 37.7 41.6 151 153 156 160 165 43.0 46.1 48.8 49.5 54.4 165 167 170 169.5 166.5 (Staronka, Anz. Ak. Wiss. Krakau, 1910. 372.) in pyridine, (Werner, Z. Mol. weight determined methyl- and ethyl-sulphide, anorg. 1897, 15. 20.) More or less sol. at high temp, in petroleum (bpt. 160-230), bromnaphthalene, pyridine, toluidine and amyl alcohol. (Reinders, Z. phys. Ch. 1900, 32. 503.) Yellow modification. 100 g. of sat. solution in acetone at 25 con- tain 3.0 g. HgI 2 . (Reinders, Z. phys. Ch. 1900, 32. 514.) Red modification. Solubility in alcohol equals: 0.717-0.724 g. in 100 g. solution at 1.044-1.084 g. " " " 25 2.10-2.20 g. " 50. (Reinders, Z. phys. Ch. 1900, 32. 522.) 100 g. of sat. solution in acetone at 25 contain 1.95 g. HgI 2 . (Reinders, Z. phys. Ch. 1900, 32. 514.) HgI 2 is moderately sol. in abs. alcohol at its b.-pt. The solution has a decided yellow color. On cooling, yellow crystals separate out. They soon change to the red modifica- tion. Readily sol. in hot amyl alcohol. Yellow crystals separate from the solution when cooled. Readily sol. in allyl alcohol, forming a yellow solution, from which yellow crystals separate on cooling. SI. sol. in acetone, giving a yellow solution. On cooling yellow plates separate from the solution and rapidly turn red. Sol in phenol at 150 C. Solution has yel- low color and yellow crystals separate out on cooling. Readily sol. in boiling benzene. Saturated solution is yellow. The yellow iodide sep- arates out on cooling, and changes rapidly to the red. Sol. in toluene giving yellow solution, from which yellow crystals separate on cooling. They rapidly change to red. Readily sol. in naphthalene at temperatures above its transition point. Solution is yellow and on cooling yellow crystals separate out. Readily sol. in hot pseudo-cumene giving a yellow solution. On cooling gives yellow crystals. Readily sol. in ethyl iodide giving very MERCURIC SODIUM IODIDE 515 yellow solution, from which yellow crystals separate on cooling, which change to red rapidly. Only si. sol. in ethyl bromide, giving yellow solution from which yellow crystals separate on cooling, which change rather slowly to the red. Sparingly sol. in isopropyl bromide. Moderately sol. in isobutyl bromide, giving a pink solution from which yellow crystals separate on cooling, which change slowly to red. SI. sol. in ethylidene chloride. On sudden cooling at 18 the iodide crystallizes out in yellow plates, which quickly change to red. Sparingly sol. in propyl chloride, giving a pink solution, from which yellow crystals separate on cooling. Readily sol. in ethyl cyanide, giving a yellow solution. On cooling yellow crystals separate and rapidly change to red. Moderately sol. in benzene cyanide, giving a deep yellow solution. On sudden cooling the solution deposits yellow crystals, which rapidly turn red. Rapidly sol. in benzoic acid at high tem- peratures. Sparingly sol. in ethyl acetate, giving yellow solution. Sol. in ethyl propionate. Very sol. in ethyl butyrate, giving a yellow solution. On cooling the iodide crystallized from the solution. SI. sol. in ethyl isobutyrate. Readily sol. in methyl salicylate, giving a yellow solution. Sparingly sol. in phenyl salicylate, giving yellow solution. On cooling yellow crystals separate out, which gradually change to red. (Kastle, Am. Ch. J. 1899, 22. 474.) Mercuromercuric iodide. Hg 4 l6 = Hg 2 l2, 2HgI 2 . Insol. in H 2 O or alcohol. Partially sol. in KI+Aq, in hot NaCl, and NH 4 Cl+Aq, and in hot HCl+Aq, though Very slowly. (Boul- lay, A. ch. (2) 34. 345. Mercury periodide, Sol. in KI+Aq. Decomp. by cold H 2 O or alcohol. (Jorgensen, J. pr. (2) 2. 347.) Mercuric hydrogen iodide (lodomercuric acid), HI, HgI 2 =HHgI 3 . Crystallises from Hl-f Aq. (Boullay.) Easily decomp. (Neumann, M. 10. 236.) 3HgI 2 , 2HI+H 2 O. (Francois, Dissert. 1901.) Mercuric nickel iodide, HgI 2 , NiI 2 +6H 2 O. Sol. in alcohol, ether, and acetone; not decomp. by H 2 O. (Dobroserdoff, C. C. 1901, 11.332.) " 2HgI 2 , NiI 2 +6H 2 O. Hydroscopic; decomp. by H 2 O ; sol. in acetone and ether. (Dobroser- doff, C. C. 1901, II. 332.) Mercuric potassium iodide, HgI 2 , KI + Deliquescent (v. Bonsdorff). Permanent; decomp. by H 2 O into 2KI, HgI 2 , and HgI 2 (Boullay); sol. in alcohol, ether, and cone. HC 2 H 3 O 2 , but decomp. by other acids (Ber- thempt, J. Pharm. 14. 186). Sp. gr. of sat. solution in H 2 O =2.4 to 3.1. +H 2 O. Sol. in H 2 O with decomp. Can be cryst. from alcohol. Very si. sol. in dry ether. Very sol. in wet ether. (Marsh, Chem. Soc. 1910, 97. 2297.) HgI 2 , 2KI. Sol. in H 2 O. (Thomsen and Bloxam, Chem. Soc. 41. 379.) Sat. solution of KI-f-HgI 2 in H 2 O at 22.9 contains 8.66% K, 22.49% Hg and 52.48% I, corresponding to 0.22 mol. K, 0.11 mol. Hg and 0.45 mol. I. (Duboin, C. R. 1905, 141. 385.) Sp. gr. at 16 /4 of aqueous solution con- taining 12.2875% salt = 1.10148; containing 12.2371% = 1.1038; containing 7.9843% = 1.06491. (Schonrock, Z. phys. Ch. 1893, 11. 782.) Sol. in methyl acetate. (Bezold, Dissert. 1906.) Sol, in ethyl acetate. (Alexander, Dissert. 1899; Hamers, Dissert. 1906.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Sol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) +2H 2 O. Sol. in alcohol, ether and acetone; decomp. by H 2 O. (Pawlow, C. C. 1901, I. 363.) Solubility determinations show that KHgI 3 and KHgI 3 +H 2 O are the only double salts formed at 20-30. See HgI 2 +KI under HgI 2 . (Dunningham, Chem. Soc. 1914, 105. Mercuric rubidium iodide, HgI 2 , Rbl. Sol. in alcohol; decomp. by H 2 O. HgI 2 , 2RbI. Very easily sol. in H 2 O. (Grossmann, B. 1904, 37. 1258.) Very sol. in acetic acid and alcohol; decomp. by H 2 O. Stable in aq. solution in the pres- ence of an excess of Rbl. (Erdmann, Arch. Pharm. 1894, 232. 30.) Mercuric silver iodide, HgI 2 , 2AgI. (Wegelius and Kilpi, Z. anorg. 1909, 61. 416.) Mercuric sodium iodide, HgI 2 , Nal. Deliquescent, and decomp. by much H 2 O. (v. Bonsdorff Pogg. 17. 266.) Sol. in alconol; decomp. by H 2 O. HgI 2 , 2NaI. Deliquescent; sol. in H 2 O and alcohol. (Boullay.) Sat. solution of NaI+HgI 2 in H 2 O at 24.75 contains 4.59% Na, 25% Hg, and 58.25% I, corresponding to 0.20 mol. Na, 516 MERCURIC STRONTIUM IODIDE 0.12 mol. Hg, and 0.45 mol. I. (Duboin, C. R. 1905, 141. 385.) +4H 2 O. Extremely deliquescent. (Du- boin, C. R. 1906, 143. 314.) Mercuric strontium iodide, HgI 2 , SrI 2 (?). Sol. in H 2 O without decomp. (Boullay.) +8H 2 O. As Ca salt. (Duboin, C. R. 1906, 142. 573.) 2HgI 2 , Srl 2 (?). Decomp. by much H 2 O into sol. HgI 2 , SrI 2 and insol. HgI 2 . (Boul- lay.) Mercuric thorium iodide, 5HgI 2 , ThI 4 + 18H 2 O. Very deliquescent. Easily decomp. by H 2 O. (Duboin, A. ch. 1909, (8) 16. 282.) 5HgI 2 , 2ThI 4 +21H 2 O. (Duboin.) 2HgI 2 , ThI 4 + 12H 2 O. (Duboin.) Mercuric zinc iodide. Deliquescent. Decomp. by H 2 O. (v. Bonsdorff.) Mercuric iodide ammonia, HgI 2 , 2NH 3 . Decomp. by NH 3 giving NHg 2 I and NH 4 I. (Francois, C. R. 1900, 130. 333.) Stable only in the presence of excess of ammonia. Gives off NH 3 in the air. (Fran- cois, J. Pharm. 1897, (6) 5. 388; C. C. 1897, I. 1088.) Mercuric iodide hydrazine, HgI 2 , N 2 H 4 . Decomp. by H 2 O. (Hofmann and Mar- burg, A. 1899, 306. 215.) Mercuric iodide rubidium bromide, HgI 2 , 2RbBr. Decomp. by H 2 O. Sol. in alcohol without decomp. (Gros- mann, B. 1903, 36. 1603.) Mercuric iodide silver chloride, HgI 2 , 2AgCl. Insol. in H 2 O. (Lea, Sill. Am. J. (3) 7. 34.) Mercury iodoantimonide, Hg 3 Sb 4 2HgI 2 . Sol. in HNO 3 aqua regia and hot H 2 SO 4 ; insol. in HC1. (Granger, C. R. 1901, 132. 1116.) Mercury nitride, Hg 3 N 2 . Gradually decomp. by H 2 O. Decomp. by cone. HNO 3 , or HCl+Aq. (Hirzel, J. B. 1852.419.) Not attacked by cold, but decomp. by hot dil. H 2 S0 4 . Sol. in acids +Aq. Sol. in ammoniacal solutions of ammonium salts. Insol. in excess of KNH 3 . (Franklin, Z. anorg. 1905, 46. 18.) Sol. in ammonia solutions of ammonium salts and in aq. acid solutions. Very explosive. (Franklin, J. Am. Chem. Soc. 1905, 27i 835.) HgN 3 . See Mercurous azoimide. HgN 6 . See Mercuric azoimide. Mercurous oxide, Hg 2 O. Insol. in H 2 O. Insol. in dil. HC1 or HNO 3 +Aq. Sol. in warm cone. HC 2 H 3 O 2 +Aq. Sol. in 150,000 pts. H 2 O. (Bhaduri. Z. anorg. 1897, 13. 410.) Decomp. by H 2 O or weak bases (Rose), (NH 4 ) 2 CO 3 +Aq (Wittstein), KNO 3 +Aq (Rose), KI+Aq (Berthemot), or cone. NH 4 Cl-fAq (Pagenstecher) into HgO and Hg, or HgCl 2 , etc. SI. decomp. by alkali chlorides +Aq with formation of HgCl 2 , which dissolves. (Miahle.) SI. sol. in alkali cyanides +Aq. (Jahn.) Insol. in KOH, and NaOH+Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol and ether. Mercuric oxide, HgO. Sol. in 20,000 to 30,000 pts. H 2 O. (Bineau, C.R.41.509.) Sol. in 200,000 pts. H 2 O. (Wallace, Ch. Gaz. 1858. 345.) Ordinary coarse HgO is sol. in H 2 O to the extent of 50 mg. per 1. at 25, but when finely powdered the solubility increases to 150 mg. per 1. (Hulett, Z. phys. Ch. 1901, 37. 406.) Red modification is: Sol. in 19,500 pts. H 2 O at 25; in 2,600 pts. H 2 O at 100. (Schick, Z. phys. Ch. 1903, 42. 172.) 1 1. H 2 dissolves 50 mg. red modification of HgO at 25. (Hulett, Z. phys. Ch. 1901, 37.406.) Yellow modification is: Sol. in 19,300 pts. H 2 O at 25; in 2400 pts. at 100. (Schick, Z. phys. Ch. 1903, 42. 172.) Sol. in acids. Insol in H 3 PO 4 or H 3 AsO 4 + Aq. (Haack, A. 262. 190.) Scarcely attacked by H 2 C 2 O 4 +Aq. (Mil- Ion, A. ch. (3) 18. 352.) Solubility of HgO in HF at 25. Hg = g.-atoms Hg in 1 1. of the solution. HF normal Hg 0.12 0.24 0.57 1.11 2.17 0.01258 0.0247 0.0629 0.1168 0.2586 (Jaeger, Z. anorg. 1901, 27. 26.) MERCURIC OXYCHLORIDE 517 Solubility of HgO in HF is decreased by the addition of KF, which proves the non- existence of complex fluorides. (Jaeger.) Insol. in H 3 AsO 4 , H 3 PO 4 and in primary and secondary alkali salts of these acids. (Haack, A. 1891, 262. 190.) Sol. in hot NH 4 Cl+Aq, less in NH 4 NO 3 + Aq. (Brett.) Insol. in KOH, or NaOH+Aq. Decomp. by alkali chlorides +Aq into HgCl 2 , which dissolves* (Miahle, A. ch. (3) 5. 177.) Sol. in Fe(NO 3 ) 3 , and BifNO 3 ) 3 +Aq with pptn. of oxides. Sol. in Kl-f Aq. (Persoz.) Very sol. in acid sulphites +Aq. (Earth, Z. phys. Ch. 1892, 9. 192.) Completely sol. in cone. CaCl 2 , BaClo, MgCl 2 , and SrCl 2 +Aq. (Andre, C. R. 1887, 104. 431.) Solubility in Ag salts +Aq. 100 g. Ag 2 SO 4 in aqueous solution dissolve 13 g. HgO. Sol- ubility in AgNO 3 +Aq is 15.6 : 100; in Ag acetate+Aq is 1.137:100. (Finci, Gazz. ch. it. 1911, 41. (2) 545.) Much less sol. in KC1 and NaCl+Aq than in H 2 O. (Schoch.) Sol. in U(NO 3 ) 3 , A1(NO 3 ) 3 and Fe(NO 3 ) 3 + Aq. (Mailhe, A. ch. 1902, (7) 27. 373.) Very si. sol. in cold Hg(CN) 2 -f-Aq, abun- dantly sol. at 75 with evolution of HCN. (Barthe, J. Pharm. 1896, (6) 3. 183.) Sol. in cold or hot alcoholic NH 4 SCN in large amounts. (Fleischer, A. 1875, 179. 225.) Completely sol. in KI+Aq. (Jehn, Arch. Pharm. 1873, 201. 97.) Solubility of red or yellow modification in N/50 KCl+Aq is about 25% greater than in pure H 2 O. (Schick, Z. phys. Ch. 1903, 42. 168.) Insol. in liquid HF. 1905, 46. 2.) Insol. in liquid NH 3 1898, 20. 829.) Insol. in liquid NH 3 . J. 1898, 20. 829.) Sol. in alcoholic solution of hydroxylamine hydrobromide below 0. (Adams, Am. Ch. J. 1902, 28. 216.) Insol. in alcohol. Sol. in trichloracetic acid+Aq. (Brand, J. pr. 1913, (2) 88. 342.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) When freshly pptd., is insol. in acetone + Aq. even on warming, but easily sol. if liquid is made alkaline by NaOH. Insol. in aceto- phenone even after long warming at 100. Sol. in acetaldehyde and much H 2 O and a little NaOH. (Auld and Hantzsch, B. 1905, 38. 2680.) Sol. in formamide. (Fischer, Arch. Pharm. 1894, 232. 329.) Very sol. in ethylene diamine. For 1 mol. (Franklin, Z. anorg. (Gore, Am. Ch. J. (Franklin, Am. Ch. HgO, 7-10 mols. ethylene diamine are neces- sary. (Traube and Lowe, B. 1914, 47. 1910.) Easily sol. in benzamide. (Dessaignes, A. ch. 1852, (3) 34. 146..) When freshly pptd., is sol. in picric acid + Aq. (Varet, C. R. 1894, 119. 560.) Sol. in alkaline solution of phenol disul- phonic acid. (Lumiere and Chevrotier, C. R. 1901, 132. 145.) Sol. in nucleic acid+Aq when freshly pptd. (Schweckerath, Pat. 1899.) Sol. in gum arabic+Aq. (Peschier, J. Pharm. 1896, (6) 3. 509.) Mercuric oxybromide, HgBr 2 , HgO. (Andre, An ch. (6) 3. 123.) HgBr 2 , 2HgO. (Andre.) HgBr 2 , 3HgO. (a) Yellow. Insol. in cold, si. sol. in hot H 2 O. Easily sol. in alcohol. (Lowig.) (6) Brown. Insol. in alcohol. (Rammels- berg, Pogg. 55. 248.) HgBr 2 , 4HgO. (Andre.) Insol. in ord. solvents. Decomp. by al- kalies and acids. (Fischer and von Warten- burg, Ch. Z. 1902, 26. 894.) 2HgBr 2 , 7HgO. Readily decomp. by acids and alkalies. (Fischer and von Wartenburg.) Mercurous oxychloride, Hg 2 O, 2HgCl. Min. Egleslonite. Decomp. by hot HC1 and by HNO 3 . (Moses, Am. J. Sci, 1903, (4) 16. 253.) Mercuric oxychloride, HgO, HgCl 2 . Less sol. than HgCl 2 , but not isolated. (Thummel.) Decomp. by cold H 2 O. (Andre, A. ch. (6) 3. 118.) HgO, 2HgCl 2 . Decomp. by warm H 2 O or cold alcohol into 2HgO, HgCl 2 . (Thummel, Arch. Pharm. (3) 27. 589.) Decomp. by H 2 O. Not decomp. by al- cohol. (Arctowski, Z. anorg. 1895, 9. 178.) 2HgO, HgCl 2 . Two modifications. A. Red. Insol. in H 2 O; decomp. by alkali carbonates, or chlorides +Aq into 4HgO. HgCl 2 . Acted upon by cold alkali carbonates and alkali chlorides +Aq. (Schoch, Am. Ch. J. 1903, 29. 335.) Not decomp. by H 2 O at ord. temp. (Thum- mel.) Very si. sol. in cold, completely sol. in hot H 2 O. (Haack, A. 1891, 262. 189.) A small amt. of HNO 3 converts it into a white powder; more HNO 3 dissolves it. (Haack, A. 1891, 262. 189.) B. Black. Not decomp. by alkali chlorides, or carbonates +Aq. (Thummel.) Not affected by boiling alkali carbonates or alkali chlorides +Aq. (Schoch, Am. Ch. J. 1901, 29. 335.) Insol. in cold and hot H 2 O and alcohol. Sol. in acid. (Van Nest, Dissert. 1909.) Not changed by H 2 O. (Blaas, Miner Mitt. (2) 2. 177.) 518 MERCUROMERCURIC OXYCHLORIDE Sol. in HNO 3 or HCl+Aq. fc (Blaas.) Not changed bv alcohol. (Blaas.) + iE 2 O. (Ray, A. 1901, 316. 255.) 3HgO, HgCl 2 . Decomp. by warm H 2 O. (Thiimmel.) Not attacked by cold H 2 O. (Andre.) Ppt. (Tarugi, Gazz. ch. it. 1901, 31. 313.) Decomp. by H 2 O. Not decomp. by al- cohol. (Arctowski, Z. anorg. 1895, 9. 178.) Three modifications. a. Prisms. Decomp. by boiling H 2 O. b. Brick-red, amorphous. c. Yellow plates. (Schoch, Am. Ch. J. 1903, 29. 337.) Yellow plates. Decomp. by hot H 2 O, Na 2 CO 3 or NaOH + Aq. Sol. in KHCO 3 +Aq. Insol. in cold dil. HNO 3 . (Tarugi.) 4HgO, HgCl 2 . Decomp. by H 2 O. Not decomp. by alcohol. (Arctowski, Z. anorg. 1895, 9. 178.) Two modifications. A. Yellow plates. Easily sol. in acids. Insol. in alcohol and ether. Decomp. by KOH. (Dukelski, Z. anorg. 1906, 49. 336.) B. Brown, amorphous. Easily sol. in acids. Decomp. by KOH. Insol. in alcohol and ether. (Dukelski, Z. anorg. 1906, 49. 336.) 5HgO, HgCl 2 . (Millon.) Does not exist. (Thiimmel.) 6HgO, HgCl 2 . Does not exist. (T.) +H 2 O. Insol. in cold H 2 O. (Roucher, A. ch. (3) 27. 353.) Does not exist. (T.) 7HgO, 4HgCl 2 . (Roucher.) Does not exist. (T.) Mercuromercuric oxychloride, Hg 2 OCl. Min. Terlinguaite. Decomp. by HC1 and HNO 3 . Slowly decomp. by cold acetic acid when powdered. (Hillebrand and Schaller, J. Am. Chem. Soc. 1907, 29. 1190.) Mercuric strontium oxychloride. HgO, SrCl 2 +6H 2 O. Decomp. by H 2 O. (Andre, C. R. 104. 431.) Mercuric oxyfluoride, HgO, HgF 2 +H 2 O. Decomp. by H 2 O. Sol. in dil. HNO 3 +Aq. (Finkener.) Mercuric oxyiodide, 3HgO, HgI 2 . Decomp. by H 2 O. Sol.inHI+Aq. (Weyl, Pogg. 131. 524.) Mercuric oxyphosphide, Hg 5 P 2 O 4 . Decomp. by H 2 O. (Partheil and van Haaren, Arch. Pharm. 1900, 238. 35.) Mercuric oxyselenide, 2HgSe, HgO. Easily sol. in aqua regia. (Uelsmann, A. 116. 122.) Mercury phosphide, Hg 3 P 2 . Insol. in H 2 O, HNO 3 , or HCl+Aq. Easily sol. in aqua regia. (Granger, C. R. 115. 229.) Hg 3 P 4 . (Granger, C. N. 1898, 77. 229.) Mercury phosphochloride, P 2 Hg 3 , 3HgCl 2 + 3H 2 O. See Drniercuriphosphonium mercuric chloride. Mercury phosphosujphide, 2HgS, P 2 S. HgS, P 2 S. 2HgS, P 2 S 3 . (Berzelius.) 3HgS, P 2 S 3 . (Baudrimont, C. R, 56. 323.) 2HgS, P 2 S 5 . (Berzelius, A. 47. 256.) Mercuric selenide, HgSe. Sol. in cold aqua regia when crystalline. When precipitated shows the same properties towards solvents as mercuric sulphide. (Reeb J. Pharm. (4) 9. 173.) Min. Tilmannite. Sol. only in aqua regia. Mercuric selenochloride, 2HgSe, HgCl 2 . Insol. in boiling HC1, HN0 3 , or H 2 SO 4 + Aq. Easily sol. in aqua regia and a mixture of H 2 SO 4 and cone. HNO 3 +Aq. (Uelsmann, J. B. 1860. 92.) Mercurous sulphide, Hg 2 S. Insol. in H 2 O, dil. HNO 3 , hot NH 4 OH, or (NH 4 ) 2 S+Aq. Sol. in KOH +Aq with separa- tion of Hg. (Rose.) Does not exist; only mixtures of Hg and HgS are formed. (Barfoed, J. pr. 93. 230.) See also Baskerville, J. Am. Chem. Soc. 1903, 25. 799.) Not attacked by HNO 3 below 0, but at- tacked by dil. HNO 3 and HCl+Aq when temp, is increased. Sol. in Na 2 S or K 2 S but Hg soon ppts. (Antony and Sestini, Gazz. ch. it. 1894, 24, (1) 194.) Mercuric sulphide, HgS. Insol. in H 2 O. Pptd. as a brown coloration in presence of 20,000 pts. H 2 O, and as a green coloration in presence of 40,000 pts. H 2 O. (Lassaigne.) Much less sol. in H 2 O than Ag 2 S or Cu 2 S. (Bodlander, Z. phys. Ch. 1898, 27. 64.) 11.. H 2 O dissolves 0.05 X10- 6 mols HgS at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Sol. in cold cone., and in hot dil. HI+Aq or HBr+Aq. (Kekule, A. Suppl. 2. 101.) Very si. decomp. by hot cone. HCl+Aq. Not at- tacked by hot HNO 3 +Aq. Sol. in cold aqua regia. Not attacked by 4-N HNO 3 or 4^N HNO 3 +4-N H 2 SO 4 at ord. temp, even after many days. By action of a mixture of equal volumes of 4-N HNO 3 and cone. H 2 SO 4 , there was slight action on pptd. HgS after 14, more action after 62 days. If HgS is boiled with the 4-N acids, oxidation takes place most rapidly with 4-N HNO 3 , then the mixture 66.7% 4-N H 2 SO 4 +33.3% 4-N HNO 3 , then MERCURIC SULPHOIODIDE 519 33.3% 4-N H 2 SO 4 +66.7% 4-N HNO 3 , and lastly 4-N H 2 SO 4 alone. (Moore, J. Am. Chem. Soc. 1911, 33. 1094.) Cold cone. H 2 SO 4 does not attack red or black HgS, but they are attacked by hot acid. (Berthelot, A. ch. 1898, (7) 14. 198.) Freshly pptd. HgS is insol. in dil. KCN + Aq. (Berthelot.) Sol. in K 2 S+Aq, but readily only in pres- ence of free alkali. (Brunner, Pogg. 15. 596.) Insol. in boiling KOH+Aq. Sol. in KSH or NaSH+Aq. Very si. sol. in cold yellow (NH 4 ) 2 S+Aq. Insol. in KCN or Na 2 S 2 O 3 +Aq. (Fresenius.) Easily sol. in cone. Na 2 S or K 2 S+Aq, even in absence of KOH or NaOH. Insol. in (NH 4 ) 2 S+Aq. Sol. in CaS, BaS, or SrS+Aq. Insol. in NaSH or KSH+Aq. (de Koninck, Z. angew. Ch. 1891. 51.) Solubility in NaSH is very small in com- parison with that in Na 2 S+Aq. (Knox, Trans. Faraday. Soc. 1908, 4. 30.) Solubility in BaS is practically equal to thatinNa 2 S. (Knox.) All cryst. modifications are sol. in cone. K 2 S and in cone. Na 2 S+Aq. (Allen and Crenshaw, Am. J. Sci. 1912, (4) 34. 368.) Sol. in potassium thiocarbonate+Aq. (Rosenbladt, Z. anal. 26. 15.) Sol. in alkali sulpho-molybdates, -tung- states, -vanadates, -arsenates, -antimonates, and -stannates. (Storch, B. 16. 2015.) 1 1. BaS 2 H 2 +Aq containing 50 g. Ba dis- solves no HgS in the cold, but 50-60 g. at 40-50. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Insol. in pyridine. (Schroeder, Dissert. 1901.) Insol: in ethyl acetate. (Naumann, B. 1910, 43. 314.) Exists in a colloidal state, sol. in H 2 O. (Winnsinger, Bull. Soc. (2) 49. 452.) Min. Cinnabar. Insol. in H 2 O, alcohol, dil. acids, or alkaline solutions. Decomp. by hot dil. HNO 3 +Aq. Not decomp. by HCl+Aq, but easily by hot H 2 SO 4 or aqua regia. Easily sol. in CuCl 2 + Aq. (Karsten.) Sol. in a mixture of Na 2 S and NaOH when present in the proportion of HgS : 2Na 2 S. Sol. in pure Na 2 S-f-Aq or in mixtures of Na 2 S and NaSH+Aq. Insol. in cold NaSH + Aq, but sol. on warming with evolution of H 2 S. (Becker, Sill. Am. J. (3) 33. 199.) Insol. in acetone. (Krug and M'Elroy.) Cinnabar is easily sol. in 20% HBr+Aq. (Rising and Lenher, J. Am. Chem. Soc. 1896, 18. 96.) Sol. in S 2 C1 2 . (Smith, J. Am. Chem. Soc. 1898, 20. 291.) Mercuric platinum sulphide. See Sulphoplatinate, mercuric. Mercuric potassium sulphide, K 2 S, 2HgS. Decomp. into its constituents by H 2 O; de- comp. by HC1, and HNO 3 +Aq, and by hot KOH, and NH 4 OH+Aq. (Schneider, Pogg. 127. 488.) K 2 S, HgS+5H 2 O. Decomp. by H 2 O or alkalies. (Weber, Pogg. 97. 76.) +H 2 O. (Ditte.) +7H 2 O. Sol. in K 2 S+Aq. (Ditte, C. R. 98. 1271.) K 2 S, 5HgS+5H 2 O. Easily decomp. by H 2 O. (Ditte.) Mercuric sodium sulphide, HgS, Na 2 S+ 8H 2 O. Decomp. by H 2 O or alkalies. 5HgS, 2Na 2 S+3H 2 O. Decomp. by H 2 O. (Knox, Trans. Faraday Soc. 1908, 4. 36.) Mercuric sulphobromide, 2HgS, HgBr 2 . Insol. in H 2 O. Not attacked by boiling HNO 3 orH 2 SO 4 . (Rose.) Mercuric sulphochloride, 2HgS, HgCl 2 . Insol. in H 2 O, cold or hot, dil. or cone. HNO 3 , H 2 SO 4 , or HCl+Aq. (Rose, Pogg. 13. 59.) Decomp. by hot aqua regia. By boiling with dil. HNO 3 , H 2 SO 4 and HC1, Hg and Cl go into solution. (Hamers, Dissert. 1906.) Insol. in H 2 O and H 2 SO 4 . Partly sol. in HC1 and HNO 3 ; easily sol. in aqua regia. (Alexander, Dissert. 1899.) Sol. in aqua regia. (Deniges, Bull. Soc. 1915, (4) 17. 356.) 3HgS, HgCl 2 . Properties as the above comp. (Poleck and Goercki, B. 21. 2415.) 4HgS, HgCl 2 . As above. (P. and G.) 5HgS, HgCl 2 . As above. (P. and G.) Insol. in alkali sulphides and in fuming HNO 3 ; decomp. by NaOBr+Aq and by KOH. (Bodroux, C. R. 1900, 130. 1399.) SI. sol. in solutions of alkali sulphides unless heated. (Berzelius.) Easily sol. in alkali sulphides +Aq; slowly sol. in alkalies or alkali hydrosulphides+Aq. (Atterberg, J. B. 1873. 258.) Mercurous sulphotetra chloride, Hg 2 SCl 4 . Decomp. by H 2 O with separation of S, HgCl 2 going into solution. (Capitaine, J. Pharm. 25. 525.) Mercuric sulphofluoride, 2HgS, HgF 2 . Decomp. by boiling H 2 O. Not decomp. by hot HC1 or HNO 3 +Aq, but gives HF with hot H 2 SO 4 +Aq. (Rose, Pogg. 13. 66.) Mercury sulpho'Mmide, HgN 2 S, NH 3 . Ppt. (Ruff, B. 1904, 37. 1585.) Mercuric sulphoiodide, HgS, HgI 2 . Ppt. (Rammelsberg, Pogg. 48. 175.) 2HgS, HgI 2 . (Palm, C. C. 1863. 121.) 520 MERCURIC SULPHOIODIDE AMMONIA Insol. in min. acids with exception of aqua regia. (Hamers, Dissert. 1906.) Mercuric sulphoiodide ammonia, 2HgS, Hgli, NH 3 . (Foerster, Ch. Z. 1895, 19. 1895.) Mercuric telluride, HgTe. Min. ColoradoUe. Sol. in boiling HNO 3 + Aq with separation of H 2 TeO 3 . Metastannic acid. See Stannic acid. Molybdatoiodic acid. See Molybdoiodic acid. Molybdenum, Mo. Not attacked by HC1, HF, or dil. H 2 SO 4 + Aq. Sol. in cone. H 2 SO 4 . Very easily sol. in aqua regia. Oxidised by HNO 3 + Aq either to molybdenum oxide, which dissolves in HNO 3 , or, if HNOs is in excess, to molybdic acid, which remains undissolved. Attacked by HNO 3 +Aq containing 3-70% HNO 3 , but only slowly by 70% acid, with formation of insol. white powder; much more vigorously by 50% acid, in which case a clear solution is formed. (Montemartini, Gazz. ch. it. 22. 384.) Not attacked by alkalies -fAq. (Bucholz, Scher. J. 9. 485.) With a sp. gr. 9.01, the metal is malleable and sol. in a mixture of HF and HNO 3 ; sol. in fused KC1O 3 . (Moissan, Bull. Soc. 1895, (3) 13. 966.) Ductile Mo is moderately quickly attacked by HNO 3 , H 2 SO 4 and HC1. (Fink, Met. Chem. Eng. 1910, 8. 341.) Not immediately attacked by cold dil. HNO 3 . Not attacked by dil. and cone. H 2 SO 4 . Boiling dil. HCl+Aq does not at- tack; cone, dissolves traces by long heating. Sol. in aqua regia. (Lederer, Dissert. 1911.) Dil. HC1 dissolves 20.3% Mo at 110 in 18 hrs. More slowly sol. in HC1 (sp. gr. 1.15). Insol. in dil. H 2 SO 4 at 110. Slowly sol. in cone. H 2 SO 4 (sp. gr. 1.82) at 110, rapidly sol. at 200-250. Slowly sol. in cone. HNO 3 (sp. gr. 1.40), rapidly sol. in dil. HNO 3 (sp. gr. 1.15). Rapidly sol. in hot aqua regia. Insol. in hot or cold HF. (Ruder, J. Am. Chem. Soc. 1912, 34. 388.) Insol. in KOH+Aq. Sol. in fused KOH. (Ruder, J. A.m. Chem. Soc. 1912, 34. 389.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Molybdenum acichloride. See Molybdenyl chloride. Molybdenum amide, OH.MoO 2 .NH 2 . Very unstable. Insol. in abs. alcohol. (Fleck, Z. anorg. 1894, 7. 353.) Molybdenum amide nitride, Mo 5 Ni 9 H 4 = 4MoN 2 , Mo(NH 2 ) 2 . Not attacked by HC1, or dil. HNO 3 +Aq. (Uhrlaub.) Molybdenum amidochloride, Mo 2 (NH 2 ) 3 Cl 3 . Insol. in H 2 O and dil. acids. (Rosenheim, Z. anorg. 1905, 46. 317.) Molybdenum amidochloride ammonia, Mo 2 (NH 2 ) 3 Cl 3 , 10NH 3 . Unstable in the air. (Rosenheim, Z. anorg. 1905, 46. 319.) Molybdenum boride, Mo 3 B 4 . Moderately attacked by hot cone, acids and vigorously by hot aqua regia. (Tucker and Moody, Chem. Soc. 1902, 81. 17.) Molybdenum romide, MoBr 2 = Mo 3 Br 4 Br 2 . See Bromomolybdenum bromide. Molybdenum ^ribromide, MoBr 3 . Not decomp. by H 2 O. Boiling cone. HC1, and cold dil. HNO 3 +Aq do not attack appre- ciably. Dil. alkalies act slowly, but decomp. with separation of Mo 2 O 3 on boiling. (Blom- strand, J. pr. 82. 435.) Molybdenum ^rabromide, MoBr 4 . Rapidly deliquescent, and easily sol. in H 2 O. (Blomstrand, J. pr. 82. 433.) Molybdenum bromochloride, etc. See Bromomolybdenum chloride, etc. Molybdenum bronze. See Molybdate molybdenum oxide, sodium. Molybdenum carbide, Mo 2 C. Insol. in HNO 3 . (Moissan, Bull. Soc. 1895, (3) 13. 967.) MoC. Does not decomp. H 2 O even at 500-600. Slowly attacked by hot HC1, HF and hot cone. H 2 SO 4 . Easily decomp. by HNO 3 . Not attacked by NaOH+Aq or KOH+Aq. (Moissan and Hoffmann, C. R. 1904, 138. 1559.) Molybdenum carbonyl, Mo(CO) 6 . Quickly attacked by bromine. Sol. in ether or benzene. (Mond, Hirtz and Cowap, Chem. Soc. 1910, 97. 808.) Molybdenum ^'chloride, MoCl 2 = Mo 3 Cl 4 Cl 2 . See Chloromolybdenum chloride. MOLYBDENUM NITRIDE 521 Molybdenum trichloride, MoCl 3 . Insol. in H 2 O or boiling cone. HCl+Aq. Easily sol., especially when heated, in HNO 3 +Aq. Sol. in H 2 SO 4 . Decomp. by NH 4 OH, KOH, orNaOH+Aq. SI. sol. in alcohol. (Leichti and Kempe.) Practically insol. in alcohol and ether. (Hampe, Ch. Z. 1888, 12. 5.) Molybdenum te/rachloride, MoCl 4 . Deliquescent. Hisses with little H 2 O, but only partly sol. in more H 2 O. Only si. sol. in cone. HCl+Aq. Sol. in H 2 S0 4 or HNO 3 + Aq. Partly sol. in alcohol and ether. (Liechti and Kempe.) Molybdenum perctochloride, MoCl 5 . Very deliquescent. Sol. in H 2 O with ex- treme evolution of heat. Sol. in HC1, HNO 3 , or H 2 SO 4 +Aq. When freshly prepared, is incompletely sol. in H 2 O, but after standing is easily sol. with hissing. (Kalischer, Dissert. 1902.) Sol. in a small amt. of cone. HC1. (Harnpe, Ch. Z. 1888, 12. 5.) Sol. in absolute alcohol or ether. (Liechti and Kempe.) Sol. in CHC1 3 and in CC1 4 . Sol. with hissing in many organic solvents (ethers, alcohols, ketones, aldehydes, acids, acid esters, acid anhydrides, amines). Sol. in cinnamic alde- hyde. (Kalischer, Dissert. 1902.) Molybdenum hydroxyl chloride, Mo(OH) 2 Cl 2 . Easily sol. in H 2 O. (Debray, C. R. 46. 1101.) Molybdenum /e/rachloride phosphorus penta- chloride, MoCl 4 , PC1 5 . Sol. in H 2 O. MoCl 4 , 2PC1 5 . Sol. in H 2 O. (Cronander, Bull. Soc. (2) 19. 500.) Molybdenum phosphorus pe/^achloride, MoCl 5 , PC1 5 . Easily decomp. (Smith and Sargent, Z. anorg. 1894, 6. 385.) Molybdenum phosphoryl chloride, MoCl 5 , POC1 3 . Decomp. by H 2 O: insol. in CS 2 ; sol. in C 6 H 6 and CHC1 3 . Molybdenum in-chloride potassium chloride. Efflorescent. Decomp. with H 2 O. (Ber- zelius.) MoCl 3 , 3KC1. Very sol. in H 2 O. Nearly insol. in alcohol and ether. (Chilesotti, C. C. 1903, II. 652.) +2H 2 O. Fairly easily sol. in cold H 2 O without any apparent decomp. Decomp. in aqueous solution, slowly in the cold but rapidly on boiling. This decomp. is pre- vented by the presence of HC1. SI. sol. in cone. HC1. (Henderson, Proc. Chem. Soc. 1903, 19. 245.) Molybdenum rubidium chloride, Rb 2 MoCl 5 +H 2 0. Sol. in H 2 O. Nearly insol. in alcohol and ether. (Chilesotti, C. C. 1903, II. 652.) Molybdenum pentacbloride nitrogen sul- phide, Mods, N 4 S 4 . Decomp. in moist air. (Davis, Chem. Soc. 1906, 89, (2) 1575.) Molybdenum Aezafluoride, MoF 6 . Decomp. by a little H 2 O with separation of blue oxide. Sol. in large amount of H 2 O forming a colorless solution. Absorbed by alkalies and NH 4 OH+Aq. (Ruff, B. 1907, 40. 2930.) Molybdenum fluoride with MF. See Fluomolybdate, M. Molybdenum potassium ^n'fluoride (?). Precipitate. Sol. in HCl+Aq. Molybdenum potassium tetr a fluoride (?). SI. sol. in H 2 O. (Berzelius.) Molybdenum sesquihydroxide, Mo 2 OeH6. Difficultly sol. in acids. Insol. in KOH, NaOH, NH 4 OH, or K 2 CO 3 +Aq. Somewhat sol. in (NH 4 ) 2 CO 3 +Aq, but pptd. on boiling. (Berzelius.) Molybdenum hydroxide, Mo 3 O 8 , 5H 2 O. Easily sol. in H 2 O. Insol. in CaCl 2 , NH 4 C1, or NaCl+Aq. SI. sol. in alcohol. (Berzelius.) Molybdenum d/hydroxide, MoO 2 , zH 2 O. Slowly and not abundantly sol. in H 2 O, from which it is precipitated by NH 4 C1 and other salts. Gelatinises by standing in closed vessels or by evaporating on the air. Sol. in the ordinary acids. Insol. in KOH, or NaOH +Aq. Sol. in alkali carbonates -f Aq. Molybdenum duodide, MoI 2 . Insol. in H 2 O and alcohol. SI. attacked by cold H 2 SO 4 or HNO 3 . (Guichard, A. ch. 1901, (7)23.567.) SI. deeomp. H 2 O at ordinary temp. Slowly sol. in H 2 SO 4 and HNO 3 . (Guichard, C. R. 1896, 123. 822.) Molybdenum tetraiodide (?). Completely sol. in water. (Berzelius.) Molybdenum nitride, Mo 5 N 3 , and Mo 5 N 4 . (Uhrlaub.) See Molybdenum amide. Mo 3 N 2 . (Rosenheim, Z. anorg. 1905, 46. 317.) 522 MOLYBDENUM OXIDE Molybdenum monoxide, MoO. Known only as hydroxide. (Blomstrand, J. pr. 77. 90.) Molybdenum sesq Dioxide, Mo 2 O 3 . Insol. in acids or alkalies. See Molybdenum sesginhydroxide. Molybdenum efroxide, MoO 2 . Insol. in HC1 or HF+Aq. SI. sol. in cone. H 2 SO 4 . HNO 3 oxidises to MoO 3 . Not at- tacked by KOH+Aq. (Ullik, A. 144. 227.) SI. sol. in KHC 4 H 4 O 6 +Aq. Molybdenum /noxide, MoO 3 . Sol. in 500 pts. cold, and much less hot H 2 O. (Bucholz.) Sol. in 960 pts. hot H 2 O. (Hatchett.) Sol. in 570 pts. cold, and much less hot H 2 O. (Dumas.) Sol. in acids before ignition. Insol. in acids, but si. sol. in acid potassium tartrate+Aq after ignition. Sol. in alkalies or alkali car- bonates +Aq. Sol. in NH 4 OH+Aq. See also Molybdic acid. Min. Molybdite. Sol. in HCl+Aq. Molybdenum oxide, Mo 2 O 5 . Sol. in H 2 SO 4 and HC1; only si. sol. in H 2 SO 4 . (Klason, B. 1901, 34. 151.) +3H 2 O. SI. sol. in H 2 O (2 g. in 1 1.). Insol. in NH 4 Cl+Aq. Insol. in caustic al- kalies, somewhat sol. in NH 4 OH. Much more sol. in M 2 CO 3 +Aq and in (NH 4 ) 2 CO 3 + Aq. (Klason, B. 1901, 34. 150.) Mo 4 Oio+3H 2 O. (Smith and Oberholtzer, Z. anorg. 1893, 4. 243.) Mo 4 O n +6H 2 O. Sol. inH 2 O. (Bailhache, C. R. 1901, 133. 1212.) Mo ft O 34 +6H 2 O. Very sol. in H 2 O. (Guich- ard, C. R. 1900, 131. 419.) Mo 7 O 20 . Sol. in H 2 O. (Junius, Z. anorg. 1905, 46. 447.) Mo 20 O 41 +2lH 2 O = Mo 2 O 5 , 18MoO 2 + 21H 2 O. Easily sol. in H 2 O. Insol. in NH 4 C1 +Aq. (Klason, B. 1901, 34. 160.) Mo 26 O 7 7+24H 2 O = Mo 2 O 5 , 24MoO 3 -f 24H 2 O. (Klason, B. 1901, 34. 159.) 3Mo 2 O 3 , 2Mo 7 O 24 + 18H 2 O. Sol. in H 2 O. (B.) It is probable that the five blue oxides of molybdenum described by Klason (B. 34, 148. 158) and Bailhache are either the blue oxide Mo 5 Ou prepared by the author or mix- tures of this compd. with molybdenum tri- oxide. (Guichard, C. R. 1902, 134. 173.) Mo5O 12 . Not attacked by ammonia; easily oxidised by HNO 3 +Aq. Not attacked by HC1 or H 2 SO 4 +Aq. (Wohler, A. 110. 275.) Formula is Mo 3 O 8 , according to Wohler, but Muthmann (A. 238. 108) has shown that correct formula is Mo 6 Oj 2 . Not attacked by boiling alkalies, HC1, or dil. H 2 SO 4 +Aq. Sol. in cone. H 2 SO 4 , with subsequent decomp. Sol. in aqua regia, and Cl 2 +Aq. (Muthmann.) Mo 3 O 8 . Sol. in H 2 O. (Muthmann, A. 238. 108.) Min. Ilsemannite (?). +5H 2 O. Moderately sol. in H 2 O. (Mar- chetti, Z. anorg. 1899, 19. 393.) Mo 5 O 7 . (v. d. Pfordten, B. 16. 1925.) Molybdenum tr /oxide ammonia, MoO 3 , 3NH 3 . Unstable in air. Very sol. in H 2 O with evolution of ammonia. (Rosenheim, Z. anorg. 1906, 50. 303.) 3MoO 3 , NH 3 + i^H 2 O. True composition of commercial molybdic acid. (Klason, B. 1901, 34. 156.) NH 4 H 3 MosOi 2 . Very si. sol. in cold, easily sol. in hot H 2 O with partial decomp. (Klason, B. 1901, 34. 156.) 3MoO 3 , 3NH 3 +7H 2 O = (NH 4 ) 3 H 3 Mo 3 O ls +4H 2 O. True composition of Rammelsberg's 3(NH 4 ) 2 O, 7MoO 3 +12H 2 O. (Klason, B. 1901, 34. 155.) ' 4MoO 3 , NH 3 +6H 2 O. Very si. sol. in cold, very easily sol. in hot H 2 O. An insol. modi- fication with less H 2 O gradually cryst. out. (Mylius, B. 1903, 36. 639.) 4MoO 3 , 2NH 3 +3H 2 O. (Klason, B. 1901, 34. 156.) 6MoO 3 , 3NH 3 +5H 2 O. Very si. sol. in cold, more easily sol. in hot H 2 0, with partial decomp. (Klason, B. 1901, 34. 156.) 12MoO 3 , 3NH 3 + 12H 2 O. (Klason, B. 1901, 34. 158.) 12MoO 3 , 3NH 3 , 12H 2 O+3MoO 3 , 8H 2 O. Moderately sol. in boiling H 2 O. (Klason.) 15MoO 3 , 3NH 3 +6H 2 O. Insol. in H 2 O. (Klason.) 4MoO 3 , MoO 2 , 2NH 3 +7H 2 O. Slowly sol. in H 2 O; fairly stable, gradually decomp. by dil. acids. (Hofmann, Z. anorg. 1896, 12. 280.) Molybdenum ^n'oxide ammonia hydrogen peroxide, 18MoO 3 , 14NH 3 , 3H 2 O 2 + 18H 2 0. Sol. in H 2 O. Sp. gr. of sat. solution = 1.486 at 17.4. (Baerwald, B. 1884, 17. 1206.) Molybdenum oxybromide. See Molybdenyl bromide. Molybdenum oxychloride. See Molybdenyl chloride. Molybdenum oxyfluoride. See Molybdenyl fluoride. Molybdenum oxyfluoride with MF. See Fluoxymolybdate, M, and Fluoxyhypo- molybdate, M. Molybdenum phosphide, Mo 2 P 2 . Gradually sol. in hot HNO 3 +Aq. (Wohler and Rautenberg, A. 109. 374.) MOLYBDENYL RUBIDIUM CHLORIDE 523 Molybdenum selenide, MoSe 3 . Not obtained pure. (Uelsmann, A. 116. 125.) Molybdenum silicide. Sol. in HF; only very si. sol. in other acids. (Warren, C. N. 1898, 78. 319.) MoSi 2 . Insol. in all min. acids; sol. in a warm mixture of HF+HNO 3 . (Defacqz, C. R. 1907, 144. 1425.) Insol. in min. acids; sol. in HF+HNO 3 . Unattacked by 10-20% KOH+Aq. De- comp. by fused NaOH. (Honigschmid, M. 1907, 28. 1020.) Not attacked by boiling HNO 3 , aqua regia or HF. (Watts, Trans. Am. Electrochem. Soc. 1906, 9. 106.) Mo 2 Si s . (Vigouroux, C. R. 129. 1238.) Molybdenum ^sulphide, MoS 2 . Insol. in H 2 O. Easily sol. in aqua regia. Easily oxidised by HNO 3 . Sol. in boiling H 2 SO 4 . SI. attacked by KOH+Aq. (Ber- zelius.) Min. Molybdenite. Sol. in HNO 3 +Aq, with separation of MoO 3 ; sol. in aqua regia; very si. sol. in H 2 SO 4 . Molybdenum irisulphide, MoS 3 . Somewhat sol. in H 2 O, especially if hot, but pptd. by an acid. Difficultly sol. except when boiled with KOH+Aq. SI. sol. in solutions of alkali sulphides unless heated. (Berzelius.) Easily sol. in alkali sulphides +Aq; slowly sol. in alkalies or alkali hydrosulphides+Aq. (Atterberg, J. B. 1873. 258.) Molybdenum tefrasulphide, MoS 4 . Not decomp. by hot H 2 O or acids. SI. sol. in cold alkali sulphides +Aq, but easily by boiling. (Berzelius.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Molybdenum sesg?'sulphide, Mo 2 S 3 . Insol. in HC1 and H 2 SO 4 ; sol. in hot cone. HNO 3 and aqua regia. (Guichard, C. R. 1900, 130. 138.) Molybdenum sulphide with MS. See Sulphomolybdate, M. Molybenum sulphochloride, Mo 5 S 8 Cl9. Insol. in H 2 O and alkalies. Slowly sol. in cone. HNO 3 . (Smith and Oberholtzer, Z. anorg. 1894, 5. 67.) Molybdenyl monamide, NH 4 MoO 4 or Mo Fe 2 (MoO 4 ) 6 +20H 2 O. Sol. in H 2 O. (Struve.) See also Ferricomolybdate, ammonium. Ammonium lanthanum molybdate, (NH 4 ) 6 La 2 Mo 14 O 48 +24H 2 O. Sol. in H 2 O. (Barbieri, C. A. 1909. 293.) Ammonium lithium molybdate, NH 4 LiMoO 4 +H 2 0. (Traube, N. Jahrb. Miner. 1894, I. 194.) Ammonium magnesium molybdate, (NH 4 ) 2 (X MgO, 2MoO 3 +2H 2 O = (NH 4 ) 2 MoO 4 , MgMoO 4 +2H 2 O. Easily sol. in H 2 O. (Ullik, A. 144. 344.) Ammonium manganous molybdate, 2(NH 4 ) 2 0, MnO, 3MoO 3 +5H 2 O. Decomp. by boiling H 2 O. (Marckwald, Dissert. 1895.) (NH 4 ) 2 O, 2MnO, 6MoO 3 +16H 2 O. De- comp. by boiling H 2 O. (Marckwald. Dissert. 1895.) ' 526 MOLYBDATE, AMMONIUM MANGANIC (NH 4 ) 2 O, 3MnO, 6MoO 3 +16H 2 O. De- comp. by boiling H 2 O. (Marckwald, Dissert. 1896.) 3(NH 4 ) 2 O, 2MnO, 12MoO 3 +22H 2 O. (Marckwald, Dissert. 1895.) Ammonium manganic molybdate. See Permanganomolybdate ammonium. Ammonium mercuric molybdate. Sol. in HCl+Aq. Sol. in boiling NH 4 C1+ Aq, separating out on cooling. Sol. in hot (NH 4 ) 2 SO 3 +Aq. (Hirzel.) Ammonium molybdenum molybdate, (NH 4 ) 2 O, 2MoO 2 , 4MoO 3 -f 9H 2 O. Easily sol. in H 2 O, but the solution soon becomes cloudy. (Rammelsberg, Pogg. 127. 291.) Ammonium neodymium molybdate, (NH 4 ) 3 NdMoO 24 + 12H 2 O. Ppf. (Barbieri, C. C. 1911, I. 1043.) Ammonium nickel molybdate, (NH 4 ) 2 O, 3NiO, 9MoO 3 +25H 2 O. Very si. sol. in cold, sol. in hot H 2 O with- out decomp. (Marckwald, Dissert. 1895.) 3(NH 4 ) 2 O, 2NiO, 10MoO 3 +14H 2 O. Very si. sol. in cold, sol. in hot H 2 O without de- comp. (Marckwald, Dissert. 1895.) 5(NH 4 ) 2 O, 3NiO, 16MoO 3 + 16H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29, 702.) 6(NH 4 ) 2 O, 3NiO, 16MoO 3 +29H 2 O. Very si. sol. in cold, sol. in hot H 2 O without de- comp. (Marckwald, Dissert. 1895.) 8(NH 4 ) 2 O, 6NiO, 31MoO 3 +63H 2 O. Very si. sol. in cold, sol. in hot H 2 O without de- comp. (Marckwald, Dissert. 1895.) 3(NH 4 ) 2 O, 9NiO, 34MoO 3 +120H 2 O. Very si. sol. in cold, easily sol. in hot H 2 O without decomp. (Marckwald, Dissert. 1895.) Ammonium nickelic molybdate. See Nickelimolybdate, ammonium. Ammonium nickel hydrogen molybdate, (NH 4 ) 4 H 6 [Ni(MoO 4 ) 6 ]+5H 2 O. See Nickelomolybdate, ammonium hydro- gen. Ammonium praseodymium molybdate, (NH 4 ) 3 PrMoO 24 + 12H 2 O. Ppt. (Barbieri, C. A. 1911. 1884.) Ammonium samarium molybdate, (NH 4 ) 3 SmMoO 24 + 12H 2 O. Ppt. (Barbieri, C. A. 1911. 1884.) Ammonium sodium molybdate, 7(NH 4 ) 2 O, 2Na 2 O, 21MoO 3 + 15H 2 O (?). Easily sol. in H 2 O. (Delafontaine, J. pr. 95. 136.) 7(NH 4 ) 2 O, 3Na 2 O, 25MoO 3 +30H 2 O (?). (Delafontaine.) (NH 4 , Na) 2 O, 3MoO 3 +H 2 O. Sol. in H 2 O. (Mauro, Gazz. ch. it. 11. 214.) Ammonium thorium molybdate. See Thoromolybdate, ammonium. Ammonium titanium molybdate. See Titanomolybdate, ammonium. Ammonium vanadium molybdate. See Vanadiomolybdate, ammonium. Ammonium zinc molybdate. Sol. in H 2 O. (Berzelius.) Ammonium zirconium molybdate. See Zirconomolybdate, ammonium. Ammonium molybdate hydrogen rfzoxide, 18Mo0 3 , 7(NH 4 ) 2 0, 3H 2 2 + 11H 2 0. Sol. in H 2 O. (Barwald, B. 17. 1206.) Barium molybdate, basic, 2BaO, MoO 3 + H 2 (?). Insol. in H 2 O. Sol. in dil. HCl+Aq or HNO 3 +Aq. (Heine, J. pr. 9. 204.) Barium molybdate, BaMoO 4 . Difficultly sol. in H 2 O; sol. in dil. HC1, and HNO 3 +Aq. (Svanberg and Struve.) Sol. in 17,200 pts. H 2 O at 23. More sol. in NH 4 NO 3 +Aq than in H,O. (Smith and Bradbury, B. 24. 2930.) +3H 2 O. (Westphal, Dissert. 1895.) BaMo 3 O 19 +3H 2 0. SI. sol. in H 2 O. Ba 3 MoO 24 +9H 2 O. Appreciably sol. in H 2 O. (Jorgensen.) According to Svanberg and Struve = Ba 2 Mo 6 Oi +6H 2 O. + 12H 2 O or 5BaO, 12MoO 3 +20H 2 O. (Junius, Z. anorg. 1905, 46. 433.) +22H 2 O. Ppt. (Westphal, Dissert. 1895.) BaO, 4MoO 3 +3^H 2 O. Ppt. (Wempe. Z. anorg. 1912, 78. 320.) +12H 2 O. Ppt. (Rosenheim, Z. anorg. 1913, 79. 299.) BaMo 9 O 28 +4H 2 O. Insol. in cold or hot H 2 O or HNO 3 +Aq. Extremely slightly de- comp. by H 2 SO 4 , or H 2 SO 4 +HNO 3 , or HC1+ Aq. (Svanberg and Struve.) Barium paramolybdate, 5BaO, 12MoO 3 + 10H 2 O. Ppt. Sol. in excess of BaCl 2 +Aq. (Junius, Z. anorg. 1905, 46. 433.) Barium te^amolybdate, BaH 2 (Mo 4 Oj 3 ) 2 + 17H 2 O. Insol. in cold, apparently decomp. by hot H 2 O, a small part dissolving, and the rest forming an insol. residue. (Ullik, A. 144. 336.) MOLYBDATE, COBALTOUS SODIUM 527 +14H 2 O. Insol. in cold and hot H 2 O. (Wempe, Z. anorg. 1912, 78. 320.) BaO, 8Mo0 3 +17H 2 O. (Felix, Dissert. 1912.) Barium chromic molybdate. See Chromicomolybdate, barium. Barium cobaltic molybdate. See Cobaltimolybdate, barium. Barium manganic molybdate. See Permanganomolybdate, barium. Barium nickelic molybdate. See Nickelimolybdate, barium. Barium nickel hydrogen molybdate, Ba 2 H 6 [Ni(MoO 4 )6] + 10H 2 O. See Nickelomolybdate, barium hydrogen. Barium vanadium molybdate. See Vanadiomolybdate, barium. Barium molybdate hydrogen dioxide, 8BaO, 19MoO 3 ,2H 2 O 2 + 13H 2 O. Precipitate. (Barwald.) Bismuth molybdate, Bi 2 O 3 , 3MoO 3 . Somewhat sol. in H 2 O. Sol. in 500 pts. H 2 O and in the stronger acids. (Richter.) Bromomolybdenum molybdate. See under Bromomolybdenum comps. Cadmium molybdate, CdMoO 4 . Insol. in H 2 O; sol. in NH 4 OH+Aq, KCN+ Aq, or acids. (Smith and Bradbury, B. 24. 2390.) CdO, H 2 O, 8MoO 3 +6H 2 O. Decomp. by boiling with H 2 O. (Wempe, Z. anorg. 1912, 78. 323.) Caesium molybdate, Cs 2 O, 3MoO 3 +H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 270.) Cs 2 0, 5Mo0 3 +3H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 270.) +3J^H 2 O. Very si. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) 2Cs 2 O, 5MoO 3 +5H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 271.) 3Cs 2 O, 10MoO 3 +3H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 271.) Cs 2 O, 16MoO 3 +8H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 271.) 3Cs 2 O, 10MoO 3 +3H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 271.) Caesium teJramolybdate, Cs 2 O, 4MoO 3 . Only si. sol. in H 2 O. (Muthmann, B. 1898, 31. 1841.) +2H 2 O. SI. sol. in H 2 O. (Muthmann, B. 1898, 31. 1841.) +3H 2 O. Easily sol. in cold or hot F 2 O. (Wempe, Z. anorg. 1912, 78. 317.) +5H 2 O. Very sol. in cold and hot H 2 O. (Wempe, Dissert. 1911.) Cs 2 O, MoO 3 , Cs 2 O, 3MoO 3 +4.5H 2 O. Sol. in H 2 O. (Wempe, Z. anorg. 1912, 78. 317.) Caesium paramolybdate, 5Cs 2 O, 12MoO 3 -f 11H 2 O. Efflorescent. Easily sol. in H 2 O. (Wempe, Z. anorg. 1912, 78. 317.) Calcium molybdate, CaMoO 4 . Insol. precipitate. (Ullik.) SI. sol. in H 2 O; insol. in alcohol. (Smith and Bradbury, B. 24. 2930.) +H 2 O. (Westphal, Dissert. 1896.) +2H 2 O. (Westphal, Dissert. 1895.) +6H 2 O. Difficultly sol. in cold, easily in hot H 2 O. (Ullik, A. 144. 231.) CaMo 4 O 13 +9H 2 O. Easily sol. in cold H 2 O. CaO, 2H 2 O, 12MoO 3 +21H 2 O. Efflores- cent. SI. sol. in cold, easily sol. in hot H 2 O. (Wempe.) Calcium hydrogen teiramolybdate, CaH 2 (Mo 4 O 13 ) 2 +17H 2 O. SI. sol. in cold, easily sol. in hot H 2 O with decomp. (Ullik.) +16H 2 O. Insol. in cold, difficultly sol. in hot H 2 O. (Wempe, Z. anorg. 1912, 78. 318.) Cerium molybdate, Ce 2 (MoO 4 ) 3 . Precipitate. Insol. in H 2 O; sol. in acids. (Cossa, B. 19. 536 R.) Chromic molybdate. Insol. in H 2 O, but sol. in acids. Sol. in NH 4 molybdate +Aq. (Berzelius.) See also Chromicomolybdic acid. Chromic molybdate, with M. molybdate. See Chromicomolybdate. M. Cobaltous molybdate, CoMoO 4 . Decomp. by alkalies and strong acids. (Berzelius.) +H 2 0. SI. sol. in pure, easily sol. in acidi- fied H 2 O. (Coloriano, Bull. Soc. (2) 50. 451.) CoO, 2MoO 3 +2H 2 O. (Marckwald, Dis- sert. 1895.) 6^H 2 O. SI. sol. in H 2 O. (Marckwald.) CoMo 3 O 10 +10H 2 O. Very si. sol. in cold, but very easily sol. in hot H 2 O. (Ullik, W. A. B. 56, 2. 767.) Cobaltic potassium molybdate. See Cobaltimolybdate, potassium. Cobaltous sodium molybdate, Na 2 O, 2CoO, 6MoO 3 -{-18H 2 O. (Marckwald, Dissert. 1895.) 2Na 2 O, CoO, 7MoO 3 +20H 2 O. Sol. in cold H 2 O without decomp. Decomp. on heating. (Marckwald.) 528 MOLYBDATE AMMONIA, COBALTOUS 3Na 2 O, 2CoO, 12MoO 3 +27H 2 O. (Marck- wald.) 3Na 2 O, 3CoO, 14MoO 3 +50H 2 O. Sol. in much cold H 2 O. (Marckwald.) 4Na 2 O, 6CoO, 25MoO 3 +68H 2 O. (Marck- wald.) Cobaltous molybdate ammonia, CoMoO 4 , 2NH 3 +H 2 O. Sol. in H 2 O. (Sonnenschein, J. pr. 53. 340.) - Cupric molybdate, basic, 4CuO, 3MoO 3 + 5H 2 O. Insol. in H 2 O. (Struve, J. B. 1854. 350.) Cupric molybdate, CuMoO4. 81. sol. in.H 2 O; decomp. by acids and alkaline solutions. CuMo 3 Oi9+6^H 2 O. Easily sol. in cold H 2 0. (Ullik, A. 144. 233.) +9H 2 O. Very si. sol. in cold, and ex- traordinarily easily sol. in hot H 2 O. (Ullik.) Cupric molybdate ammonia, CuMoO 4 , 2NH 3 +H 2 O. Gives off NH 3 at ord. temp. Decomp. by H 2 O. Sol. in dil. NH 4 OH+Aq from which it can be cryst. (Briggs, Chem. Soc. 1904, 85. 674.)' CuMoO 4 , 4NH 3 . Decomp. by H 2 O. Sol. in dil. NH 4 OH+Aq. (Jorgensen, Ch. Z. Repert. 1896, 20. 225.) Didymium molybdate, Di 2 (MoO 4 ) 8 . Ppt. Insol. in H 2 O. (Cossa, B. 19. 536R.) Di 2 O 3 , 6MoO 3 + 3H 2 O (?). Precipitate. (Smith.) Glucinum molybdate, basic, 2G1O, MoO 3 + 3H 2 0. Nearly insol. in H 2 O. (Atterberg, J. B. 1873. 258.) Glucinum molybdate, GlO, s Mo0 3 +2H 2 O. Sol. in H 2 O with decomp. (Rosenheim, Z. anorg. 1897, 15. 307.) GlMoO 4 , MoO 8 +^H 2 O. Easily sol. in H 2 O. (Atterberg.) Gold (auric) molybdate (?). 81. sol. in H 2 O. Sol. in HC1, and HNO 3 + Aq. (Richter.) Hydroxylamine potassium molybdate. Mo0 4 H 2 (NH 3 0) 3 (NH 2 OK). Easily sol. in H 2 O; pptd. by alcohol. (Hof- mann, A. 1899, 309. 324.) Indium molybdate, rn 2 (MoO 4 ) 3 +2H 2 O. Ppt. Insol. in H 2 O. Easily sol. in HC1. (Renz, B. 1901, 34. 2765.) Iron (ferrous) molybdate, FeMoO 4 . Insol. in H 2 O. (Schultze, A. 126. 55.) Iron (ferric) molybdate, Fe 2 O 3 , 4MoO 3 + 7H 2 O. Nearly insol. in H 2 O. Slowly sol. in cold, easily in hot HC1, or HNO 3 +Aq. Dil. acids gradually dissolve out Fe 2 O 3 in the cold. When ignited, difficultly sol. in all solvents. (Steinacker.) Fe 2 O 3 , 5MoO 3 + 16H 2 O. Very' si. sol. in H 2 O. (Struve, J. B. 1854. 346.) 2Fe 2 O 3 , 7MoO 3 +34H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 704.) Ferric potassium molybdate, Fe 2 O 3 , 3K 2 O, 12MoO 3 +20H 2 O = 3K 2 Mo 2 O 7 , Fe 2 (Mo 2 O 7 ) 3 +20H 2 O. Sol. inH 2 O. (Struve.) Lanthanum molybdate, LaH 3 (MoO 4 ) 3 = La 2 O 3 , MoO 3 +3H 2 O. (?) Precipitate. (Smith.) Lead molybdate, PbMoO 4 . Insol. in H 2 O. Sol. in warm HNO 3 +Aq; decomp. by H 2 SO 4 ; sol. in cone. HCl+Aq, or KOH+Aq. Min. Wulfenite. As above. Lithium molybdate, Li 2 MoO 4 . Moderately sol. in cold, and only si. more sol. in hot H 2 O. (Ephraim, Z. anorg. 1909, 64. 259.) + 2 /*H 2 O. Easily sol. in H 2 O. 5Li 2 O, 5MoO 3 +2H 2 O. 46. 13 g. are present in 100 ccm. of the aqueous solution at 20, and sp. gr. of the solution = 1.44. (Wempe, Z. anorg. 1912, 78. 309.) Li 2 O, 2MoO 3 +5H 2 O. Sol. in cold, easily sol. in hot H 2 O. (Ephraim, Z. anorg. 1909, 64. 258.) Li 2 O, 3MoO 3 +H 2 O. Easily sol. in warm H 2 O. (Wempe, Dissert. 1911.) +4H 2 O. (Wempe.) +4MH 2 O. (Wempe.) +7H 2 O. Nearly insol. in cold, sol. in hot H 2 O. (Ephraim, Z. anorg. 1909, 64. 258.) 2Li 2 O, 3MoO 3 . 81. sol. in H 2 O. (Ephraim, Z. anorg. 1909, 64. 258.) Lithium paramolybdate, 3Li 2 O, 7MoO 3 -f- 12H 2 O. Sol. in H 2 O. (Rosenheim, Z. anorg. 1897, 15. 181.) +28H 2 O. Easily sol. in cold and hot H 2 O. Ephraim, Z. anorg. 1909, 64. 258.) Lithium teiramolybdate, Li 2 O, 4MoO 3 +7H 2 O. Sol. in cold H 2 O. (Ephraim, Z. anorg. 1909, 64. 258.) Li 2 O, H 2 O, 8MoO 3 +10H 2 O. Easily sol. MOLYBDATE, POTASSIUM 529 in hot H 2 O. (Wempe, Z. anorg. 1912, 78. 308.) Li 2 O, 3H 2 O, 16MoO 3 +6^H 2 O. Easily sol. in warm H 2 O. (Wempe, Z. anorg. 1912, 78. 308.) Lithium potassium molybdate, KLiMoO 4 + H 2 O. (Traube, N. Jahrb. Miner, 1894, I. 194.) Magnesium molybdate, MgMoO 4 . Min. Belonesia. Insol. in HCl+Aq. (Scacchi, Zeit. Kryst. 1888, 14. 523.) +5H 2 O. Easily sol. in cold, but still more sol. in hot H 2 O. (Delafontaine.) Sol. in 12-15 pts. cold H 2 O. (Brandes.) +7H 2 O. Easily sol. in hot or cold H 2 O. (Ullik.) MgMo 3 Oi9-j-10H 2 0. Difficultly sol. in cold, very easily in hot H 2 O. (Ullik.) Magnesium paramolybdate, Mg 3 Mo 7 O 24 + 20H 2 O. Quite sol. in cold, more easily in hot H 2 O. (Ullik.) Magnesium teframolybdate, MgO, H 2 O, 8MoO 3 + 19H 2 O. Magnesium hydrogen feramolybdate, MgH 2 (Mo 4 O 13 ) 2 +19H 2 O. Easily sol. in cold H 2 O. (Ullik, A. 144. 335.) SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) +20H 2 O. Ppt. (Wempe, Z. anorg. 1912, 78. 323.) Magnesium hydrogen octomolybdate, MgH 2 (Mo 8 O 26 ) 2 +29H 2 O. Very difficultly sol. in cold, very easily sol. in hot H 2 O. (Ullik, W. A. B. 60, 2. 314.) Magnesium potassium molybdate, MgMoO 4 , K 2 MoO 4 +2H 2 O. Slowly sol. in cold, easily in hot H 2 O. (Ullik, A. 144. 343.) Manganous molybdate, MnMoO 4 +H 2 O. Insol. in H 2 O. SI. sol. in pure, easily sol. in acidified H 2 O. Decomp. by alkalies or alkali carbonates +Aq. (Coloriano, Bull. Soc. (2) 50. 451.) +VsH 2 O. (Marckwald, Dissert. 1895.) +10H 2 O. (Marckwald.) Manganic potassium molybdate. See Permanganomolybdate, potassium. Manganic silver molybdate. See Permanganomolybdate, silver. Mercurous molybdate, Hg 2 Mo 2 O7. Decomp. by H 2 O. (Struve, J. B. 1754. 350,) Sol. in 500-600 pts. H 2 O; decomp. by HNO 3 +Aq. (Hatchett.) Molybdenum molybdate. See Molybdenum oxides, Mo 3 O7, Mo 4 Oo, etc. Neodymium molybdate, Nd 2 (MoO 4 ) 3 . Very si. sol. in H 2 O. 1 pt. is sol. in 53790 pts. H 2 O at 28. 1 " " " " 32466 " H 2 O "75. (Hitchcock, J. Am. Chem. Soc. 1895, 17. 532.) Nickel molybdate, NiMoO 4 + 2 / 3 H 2 O, - and +5H 2 O. (Marckwald, Dissert. 1895.) NiO, 3MoO 3 +18H 2 O. SI. sol. in cold; easily sol. in hot H 2 O. (Marckwald.) 5NiO, 14MoO 3 +57H 2 O. and +70H 2 O. SI. sol. in cold; easily sol. in not H 2 O. (Marck^ wald.) Nickel potasshun molybdate, 3NiO, 5K 2 O 16MoO 3 +21H 2 O. Can be cryst. from H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29. 701.) Nickelic potassium molybdate. See Nickelimolybdate, potassium. Nickel potassium hydrogen molybdate, K 4 H 6 [Ni(MoO 4 ) 6 ] +5H 2 O. See Nickelomolybdate, potassium hydro- gen. Nickel sodium molybdate, 2NiO, Na 2 O, 6MoO 3 +17H 2 O. Sol. in cold H 2 O without decomp. but de- comp. on warming. (Marckwald, Dissert. 1895.) Nickel molybdate ammonia, NiMoO 4 , 2NH 3 +H 2 0. Decomp. by H 2 O. (Sonnenschein, J. pr. 53. 341.) Potassium molybdate, K 2 MoO 4 . Deliquescent in moist air. Very sol. in H 2 O. Insol. in alcohol. (Svanberg and Struve, J. pr. 44. 265.) 184.6 grams are sol. in 100 grams H 2 O at 25. (Amadori, C. A. 1912. 2878.) Solubility of K 2 MoO 4 +K 2 SO 4 at 25. G. per 100 g. H 2 O G. per 100 g. H 2 O K 2 S0 4 K 2 MoO4 K 2 S0 4 K 2 MoO< 0.46 - 0.72 0.98 1.27 184.6 180.7 177. 127.2 107.5 1.50 2.13 3.95 8.55 12.10 99.49 45.89 17.48 4.73 (Amadori, Att. ace. Line. 1912, 21, I. 467, 667.) 530 MOLYBDATE, POTASSIUM Easily sol. in H 2 O. (Wempe, Dissert. 1911.) K 2 O, 8MoO 3 +13H 2 O. Easily sol. in warm H 2 O. (Wempe, Dissert. 1911.) K 2 O, 10MoO 3 +9H 2 O. Nearly insol. in hot and cold H 2 O. 100 g. H 2 O dissolve 0.682 g. at 100. (Felix, Dissert, 1912.) +15H 2 O. Sol. inH 2 O. (Felix.) 5K 2 O, 12MoO 3 +8H 2 O. SI. sol. in cold H 2 O. (Junius, Z. anorg. 1905, 46. 439.) Potassium inmolybdate, K 2 Mo 3 Oio. Difficultly sol. in cold, but much more easily in hot H 2 O. When ignited is absolutely insol. in H 2 O. (Svanberg and Struve.) +2H 2 O. (Junius, Z. anorg. 1905, 46. 439.) SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) " +2MH 2 O. Easily sol. in H 2 O. (Wempe, Dissert. 1911.) +3H 2 O. Very si. sol. in cold, more easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) +11H 2 O. Practically insol. in H 2 O. (Westphal, Dissert. 1895.) Potassium hydrogen teframolybdate. K 6 H 4 [H 2 (Mo 2 O 7 )6]+18H 2 O. SI. sol. in cold H 2 O. Decomp. by boiling H 2 O. (Rosenheim, Z. anorg. 1913, 79. 298.) KHMo 4 O 13 +6H 2 O. Decomp. by H 2 O. (Ullik'.) Potassium paramolybdate, K 6 Mo 7 O 24 + 4H 2 O. Decomp. even by cold H 2 O. (Delafon- taine.) Formula is KgMogOsi +6H 2 O, according to Svanberg and Struve (?). Potassium selenium molybdate. See Selenomolybdate, potassium. Potassium sodium molybdate, K 2 MoO 4 , 2Na 2 MoO 4 +14H 2 O. Very easily sol. in cold, still more easily in hot H 2 O. (Delafontaine.) Potassium vanadium molybdate. See Vanadiomolybdate, potassium. Potassium zinc molybdate. Sol. in H 2 O. (Berzelius.) Potassium molybdate hydrogen rftoxide, 6K 2 O, 16MoO 3 , 4H 2 O 2 + 13H 2 O. Sol. in H 2 O. (Barwald, C. C. 1885. 424.) Potassium molybdate sulphocyanide. KSCN, K 2 Mo 3 O 10 +4H 2 O. Decomp. by H 2 O. Sol. in dil. HCl+Aq. (Pechard, C. R. 1894, 118. 806.) Praseodymium molybdate, Pr 2 (MoO 4 ) 3 . Very si. sol. in H 2 O. 1 pt. is sol. in 65820 pts. H 2 O at 23. 1 " " " " 69800 " " " 75. (Hitchcock, J. Am. Chem. Soc. 1895, 17. 530.) Rubidium molybdate, Rb 2 O, MoO 3 . Hygroscopic. (Ephraim, Z. anorg. 1909, 64. 263.) Rb 2 O, 2MoO 3 +2H 2 O. Easily sol. in H 2 O. (Ephraim, Z. anorg. 1909, 64. 263.) Rb 6 Mo 7 O 24 +4H 2 O. Very si. sol. in cold, much more easily sol. in hot H 2 O. (Dela- fontaine, N. Arch. Sc. phys. nat. 30. 233.) (Ephraim, Z. anorg. 1909, 64. 263.) +4 2 / 3 H 2 O. (Wempe, Dissert. 1911.) 2Rb 2 O, 7MoO 3 +5H 2 O. Very si. sol. in cold, very easily sol. in hot H 2 O. (Wempe.) 5Rb 2 O, 7MoO 3 +14H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 268.) 3Rb 2 O, 8Mo0 3 +6H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 269.) 5Rb 2 O, 12MoO 3 +H 2 O. 100 cc. H 2 O dis- solve 1.941 g. at 24. (Wempe, Z. anorg. 1912, 78. 258.) Rb 2 O, 3MoO 3 . Insol. in H 2 O. (Muth- mann, B. 1898, 31. 1839.) +H 2 0. (Muthmann, B. 1898, 31. 1839.) -j-3H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) 6^H 2 O. (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 269.) 2Rb 2 O, 3MoO 3 +4H 2 O. SI. sol. in cold, easily in hot H 2 O. (Wempe, Dissert. 1911.) Rb 2 O, 4MoO 3 . Difficultly sol. in cold, easily in hot H 2 O. (Wempe, Z. anorg. 1912, 78. 312.) + ^H 2 O. Practically insol. in H 2 0. Very sol. by addition of NH 3 . (Ephraim and Herschfinkel, Z. anorg. 1909, 64. 266.) +2.5H 2 O. Insol. in H 2 O. (Ephraim, Z. anorg. 1909, 64. 263.) +4H 2 O. Sol. in cold, more easily sol. in hot H 2 O. (Wempe, Z. anorg. 1912, 78. 312.) Rb 2 O, MoO 3 , Rb 2 O, 3MoO 3 +5H 2 O. Sol. in cold or hot H 2 O. (Wempe, Z. anorg. 1912, 78. 312.) Rb 2 O, H 2 O, 8MoO 3 +3H 2 O. Difficultly sol. in cold, easily in hot H 2 O. (Wempe, Z. anorg. 1912, 78. 312.) Rb 2 O, HMoO 3 +5.5H 2 O. Ppt. (Ephraim, Z. anorg. 1909, 64. 263.) Rb 2 O, 13MoO 3 +4H 2 O. Ppt. (Ephraim.) Rb 2 O, 18MoO 3 . Ppt. (Ephraim.) Samarium molybdate, Sm 2 (MoO 4 ) 3 . Insol. in H 2 O. (Cleve.) Samarium sodium molybdate, Na 2 Sm 2 (MoO 4 ) 4 . Insol. in H 2 O. Easily sol. in warm dil. HN0 3 +Aq. (Cleve.) MOLYBDATE MOLYBDENUM OXIDE SODIUM 531 Silver (argentous) molybdate, Ag 4 O, 2MoO 3 . Sol. in HNO 3 +Aq. KOH+Aq dissolves MoO 3 and Ag 4 O separates out. Not decomp. by dil. NH 4 OH+Aq. (Wohler and Rauten- berg, A. 114. 119.) Does not exist. (Muthmann, B. 20. 983.) Silver (argentic) molybdate, Ag 2 MoO 4 . Somewhat sol. in H 2 O; less when HNO 3 is present. (Richter.) Very si. sol. in pure H 2 O; easily sol. in H 2 O acidulated with HNO 3 . (Struve and Svanberg.) Sol. in KCN or NaOH+Aq. (Smith and Bradbury.) Ag 2 O, 2MoO 3 . SI. sol. in H 2 O. Sol. in KCN+Aq. (Junius, Dissert. 1905.) 2Ag 2 O, 5MoO 3 . Somewhat sol. in H 2 O. (Svanberg and Struve, J. B. 1847-48. 412.) Ag 2 O, 4MoO 3 -f 6H 2 O. SI. sol. in H 2 O with decomp. (Wempe, Z. anorg. 1912, 78. 322.) Silver thorium molybdate. See Thoromolybdate, silver. Silver molybdate ammonia, Ag 2 MoO 4 , 4NH 3 . Sol. in H 2 O with rapid decomposition. (Widmann, Bull. Soc. (2) 20. 64.) Silver molybdate hydrogen dioxide, 13Ag 2 O, 2H 2 O 2 , 32MoO 3 . Ppt. (Barwald, B. 1,7. 1206.) Sodium molybdate, Na 2 MoO 4 . Anhydrous. Easily and completely sol. in H 2 O. +2H 2 O. Sol. inH 2 O. +10H 2 O. Efflorescent. Solubility in H 2 O at t. oe ^ 3 3 g! sl 0^2 S +a 03 gifi Solid phase t . i| w| l8S fej>> ^06 O "2 rt *f* |s Na 2 MoO 4 , 10 2 HO 30.63 25.92 3.86 u 4 33.83 22.38 4.47 11 6 35.58 20.72 4.83 u 90 38.16 18.54 5.39 Na 2 MoO 4 , 2H 2 O 10 39.28 17.70 5.65 " 15.5 39.27 17.70 5.65 M 32. 39.82 17.30 5.78 " 51.5 41.27 16.28 6.14 " 100 45.57 13.67 7.32 (Funk, B. 1900, 33. 3699.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Na 2 Mo 2 O7. After ignition, very difficultly sol. in cold, and very slowly sol. in hot H 2 O. (Svanberg and Struve.) +H 2 O. Easily sol. in H 2 O. Easily sol. in cold or hot H 2 O. (Wempe, Dissert. 1911.) -|-4H 2 O. Easily and completelv sol. in coldH 2 O. (Ullik.) +6^H 2 O. SI. sol. in cold, very easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) +7H 2 O. Difficultly sol. in cold H 2 O, but more easily than the corresponding K salt. 100 pts. H 2 O dissolve 3.878 pts. at 20 and 13.7 pts. at 100. (Ullik, A. 144. 244.) +9H 2 O. Easily sol. in cold, very easily sol. in hot H 2 0. (Wempe.) +11H 2 O. (Junius, Z. anorg. 1905, 46. 437.) 3Na 2 0, 7MoO 3 . Easily sol. in cold, very easily sol. in hot H 2 O. (Ott, Dissert. 1911.) +20H 2 O. (Westphal,* Dissert. 1895.) +22H 2 O. Efflorescent. Easily sol. in H 2 O. (Ullik, A.144. 219.) Na 2 O, 8MoO 3 + 3^H 2 O. Very sol. in cold or hot H 2 0. (Wempe, Dissert. 1911.) +4H 2 0. Insol. 'in H 2 O. (Ullik, W. A. B. 60, 2. 312.) +15H 2 O. (Rosenheim, Z. anorg. 1897, 15. 188.) Na 2 O, 10MoO 3 +6H 2 O. Very si. sol. in H 2 O. 100 g. H 2 O dissolve 0.842 g. at 100. (Felix, Dissert. 1912.) +7H 2 O. (Felix.) Nearly insol. in hot and cold H 2 O. (Rosenheim, Z. anorg. 1903, 37. 323.) +12H 2 O. Difficultly sol. in H 2 O. -f 21H 2 O. Abundantly but slowly sol. in coldH 2 0. = NaHNa 5 16 +10H 2 0. (Ullik.) 5Na 2 O, 12MoO 3 +8H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) +20H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) +36H 2 O. (Junius, Z. anorg. 1905, 46. 436.) +44H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Wempe, Dissert. 1911.) Sodium teframolybdate, Na 2 Mo 4 Oi 3 +6H 2 O. Difficultly sol. in cold, easily in hot H 2 O. (Ullik.) 100 cc. H 2 O dissolve at 21, 28.39 g. of the salt. Sp. gr. of the solution = 1.47. (Wempe, Z. anorg. 1912, 78. 306.) -f 17H 2 O. (Felix, Dissert. 1912.) Na6H 4 [H 2 (Mo 2 O 7 )6]+21H 2 O. Slowly sol. in cold, easily sol. in hot H 2 O. (Rosenheim, Z. anorg. 1913, 79. 298.) NaHMo 4 Oi 3 +8H 2 O. Very sol. in hot or cold H 2 O. (Ullik, A. 144. 333.) NaHMo 8 O 26 + 4H 2 O. Insol. in H 2 O. (Ullik.) Sodium manganous molybdate, 2Na 2 O, MnO, 6MoO 3 -H9H 2 O. (Marckwald, Dissert. 1895.) Sodium molybdate molybdenum oxide, Na 2 Mo 5 Oi5. Insol. in H 2 O. Sol. in HNO 3 and aqua regia. Insol. in HC1 and in H 2 SO 4 . Sol. in 532 MOLYBDATE, STRONTIUM alkalies. (Stavenhagen and Engels, B. 1895, 28. 2280.) Strontium molybdate, SrMoO4. SI. sol. in H 2 O. (Schultze.) Sol. in 9600 pts. H 2 O at 17. (Smith and Bradbury, B. 24. 2930.) SrO, 3MoO 3 + KH 2 O. Scarcely sol. in cold, easily in hot H 2 O. (Wempe, Dissert. 1911.) SrO, H 2 O, 8MoO 3 +6H 2 O. Scarcely sol. in cold, easily in hot H 2 O. (Wempe, Dissert. 1911.) 2SrO, 3H 2 O, 20MoO 3 +21H 2 O. Ppt. (Wempe, Z. anorg. 1912, 78. 321.) Thallous molybdate, Tl 2 MoO 4 . Insol. in H 2 O. Sol. in alkalies. Insol. in alcohol. (Oettinger, J. B. 1864, 254.) SI. sol. in hot or cold H 2 O. (Ullik, J. B. 1867, 234.) 8T1 2 O, llMoO 3 . Sol. in hot H 2 O. (Flem- ing, J. B. 1868, 250.) 3T1 2 O, 8MoO 3 . (Fleming.) Thallous teframolybdate, T1 2 O, 4MoO 3 +H 2 O. SI. sol. in H 2 O with decomp. (Wempe, Z. anorg. 1912, 78. 322.) Thallous paramolybdate, 5T1 2 O, 12MoO 3 . Insol. in H 2 O. Easily sol. in mineral acids and in alkali hydroxides and carbonates. (Junius, Z. anorg. 1905, 46. 432.) Tin (stannic) molybdate. Insol. in H 2 O. Sol. in dil. or cone. HC1+ Aq, or in KOH+Aq. Not decomp. by HNO 3 +Aq. (Berzelius.) Uranous molybdate. Precipitate. Sol. in HCl+Aq. Decomp. by KOH+Aq. U(MoO 4 ) 2 . (Lancien, C. C. 1908, I. 1763.) Uranyl molybdate, (UO 2 )MoO 4 . Insol. in H 2 O, methyl and ethyl alcohol, ether, acetic acid ? CHC1 3 , CeHe and CyHs. Sol. in mineral acids. (Lancien, C. C. 1907. I. 784.) 2UO 3 , 3MoO 3 (?). Insol. in H 2 O. Sol. in strong acids and (NH 4 ) 2 CO 3 +Aq. (Ber- zelius.) 3UO 3 , 7MoO 3 . Insol. in hot and cold H 2 O. Insol. in NaOH, KOH, and NH 4 OH+Aq. Sol. in all min. acids and decomp. by an ex- cess of H 2 O. Insol. in acetic acid. (Lancien, C. C. 1908, 1. 1763.) UO 3 , 8MoO 3 . (Lancien.) +13H 2 O. Insol. in HNO 3 . (Lancien.) Ytterbium molybdate, Yb 2 O 3 , 7MoO 3 +6H 2 O. Insol. in hot H 2 O. (Cleve, Z. anorg. 1902, 32. 152.) 2Yb 2 O 3 , MoO 3 . Ppt. (Cleve.) Yttrium molybdate. Insol. in H 2 O. Sol. in HNO 3 +Aq. (Ber- lin.) Zinc molybdate, ZnMoO 4 . Difficultly sol. in H 2 O; easily in acids. (Schultze, A. 126. 49.) +H 2 O. SI. sol. in H 2 O. Easily sol. in dil. acids. (Coloriano, Bull. Soc. (2) 50. 451.) ZnMo 3 O 19 +10H 2 O. yery difficultly sol. in cold, but extraordinarily easily sol. in hot H 2 O. (Ullik, W. A. B. 55, 2. 767.) Zinc teframolybdate, ZnMo 4 O 13 +8H 2 O. Easily sol. in cold H 2 O. (Ullik.) ZnO,H 2 O,8MoO 3 +14H 2 O. Ppt. (Wempe, Z. anorg. 1912, 78. 324.) Zinc molybdate ammonia, ZnMoO 4 , 2NH 3 + H 2 O. (Sonnenschein, J. pr. 53. 339.) Pmnolybdic acid. See Permolybdic acid. Molybdic sulphuric acid, MoO 3 , S0 3 . Deliquescent. (Schultz-Sellack, B. 4. 14.) Very deliquescent. Very sol. in H 2 0. (Muthmann, A. 1886, 238. 126.) MoO 3 , 3SO 3 +2H 2 O (?). Molybdocyanhydric acid, H 4 Mo(CN) 8 -f 6H 2 O. Easily sol. in H 2 O and abs. alcohol. Solu- tions are stable at ord. temp. (Rosenheim and Garfunkel, Z. anorg. 1910, 65. 168.) Cadmium molybdocyanide, Cd 2 Mo(CN) 8 + 8H 2 O. Insol. in H 2 O. (Rosenheim.) Cadmium molybdocyanide ammonia, Cd 2 Mo(CN) 8 , 4NH 3 +2H 2 O. (Rosenheim.) Cupric molybdocyanide ammonia, Cu 2 Mo(CN) 8 , 4NH 3 +7H 2 O. (Rosenheim.) Potassium molybdocyanide, K 4 Mo(CN) 8 + 2H 2 0. Very sol. in H 2 O. (Rosenheim.) Thallous molybdocyanide, Tl 4 Mo(CN) 8 . Very si. sol. in H 2 O. (Rosenheim.) Molybdoiodic acid, HIO 3 , H 2 MoO 4 +H 2 O. Easily sol. in H 2 O. (Blomstrand, J. pr. (2) 40. 320.) I 2 O 5 , 2MoO 3 +2H 2 O. Very sol. in H 2 O. Insol. in cold, sol. in hot HNO 3 . Sol. in al- cohol. (Chretien, A. ch. 1898, (7) 15.. 402.) MOLYBDOIODATE, ZINC 533 Ammonium molybdoiodate, NH 4 IO 3 , H 2 MoO 4 . Somewhat more sol. than K salt. (Blom- strand.) (NH 4 ) 2 O, I 2 O 5 , 2MoO 3 . Very si. sol. in cold H 2 O. More sol. in hot H 2 O. (Rosen- heim and Liebknechfc, A. 1899, 308. 50.) +H 2 O. 1 1. H 2 O dissolves 5.39 g. salt at 15; 30.94 g. at 100. More sol. in dil. HNO 3 +Aq. (Chretien, A. ch. 1898, (7) 15. 409.) 3(NH 4 ) 2 0, (1,0,, 2Mo0 3 ) 4 +6H 2 0. (Chr6- tien.) Barium molybdoiodate, BaO, 1 2 O 5 , 2MoO 3 -f 2H 2 O. 4.23 g. are sol. in 1 1. H 2 O at ord. temp. (Chretien.) Cadmium molybdoiodate, acid, 3CdO, (I 2 O 5 , 2MoO 3 ) 6 +16H 2 0. SI. sol. in H 2 O. (Chretien.) Calcium molybdoiodate, CaO, I 2 O 5 , 2MoO 3 + 6H 2 O. 1 1. H 2 O dissolves 7.8 g. of the salt at 15; 20.89 g. at 90. (Chretien.) Cobaltous molybdoiodate, CoO, I 2 O 5 , 2Mo0 3 +6H 2 O. 5.11 g. are sol. in 1 1. H 2 O at 15; 22.27 g. at 100. (Chretien.) Cobaltous molybdoiodate acid, CoO, (I 2 O 5 , 2MoO 3 ) 5 +18H 2 O. Very sol. in H 2 O. (Chretien.) Cupric molybdoiodate, CuO, I 2 O 5 , 2MoO 3 + 3H 2 O. 1 1. H 2 O dissolves 10.63 g. of the salt at 15; 25.55 g. at 100. (Chretien.) Lithium molybdoiodate, Li 2 O, I 2 O 5 , 2MoO 3 + 197.83 g. are sol. in 1 1. H 2 O at 15. Sol. in dil. HNO 3 +Ag. (Chretien.) Magnesium molybdoiodate, MgO, I 2 O 6 , 2MoO 3 +6H 2 O. 1 1. H 2 O dissolves 3.85 g. of the salt at 15; 18.2 g. at 100. (Chretien.) Manganous molybdoiodate, 3MnO, (I 2 5 , 2MoO 3 ) 4 +9H 2 O. 1 1. H 2 O dissolves 17.05 g. of the salt at 15; 55.05 g. at 100. (Chretien.) Nickel molybdoiodate, NiO, I 2 O 5 , 2MoO 3 6H 2 O. 5.43 g. are sol. in 1 1. H 2 O at 15; 21.8 g. at 100. (Chretien.) 2NiO, 2IjO 6 , 3MoO 3 +23H 2 O. Easily sol. in H 2 O. Not decomp. by acids. (Maass, Dissert. 1901.) Nickel molybdoiodate, acid, 2NiO, (I 2 O 5 , 2MoO 3 ) 5 +15H 2 O. Very sol. in H 2 O. (Chretien.) Potassium molybdoiodate, KHO 2 IO 2 MoO 3 OH, or KIO 3 , MoO 3 -f- 2H 2 0. Ppt. SI. sol. in H 2 O. (Blomstrand, J. pr. 2) 40. 320.) K 2 O, I 2 O 5 , 2Mo0 3 . Only si. sol. in cold H 2 O; sol. on long boiling. 4.48 grs. are sol. in 1 1. H 2 O at 12. (Compare Blomstrand: not identical.) (Rosenheim, A. 1899, 308. 50.) +H 2 O. SI. sol. in H 2 O. 3.45 g. are sol. in 1 1. H 2 O at 15; 28.38 g. at 100. More sol. in dil. HNO 3 +Aq. (Chretien, A. ch. 1898, (7) 16. 404.) Potassium molybdoiodate, acid. (I 2 O 5 , 2Mo0 3 ) 6 , 4K 2 O+7H 2 O. (I 2 O 5 , 2MoO 3 ) 3 , 2K 2 O + 13H 2 O. (I 2 O 5 , 2MoO 3 ) 2 , K 2 O+4H 2 O. (I 2 O 5 , 2MoO 3 ) 3 , K 2 O+7H 2 O. (I 2 O 6 , 2MoO 3 ) 4 , K 2 O+5H 2 O. (Chretien.) Silver molybdoiodate, Ag 2 O, I 2 O 5 , 2MoO 3 -h Insol. in H 2 O. 4Ag 2 O, 4I 2 O 5 , 3MoO 3 . Sol. in H 2 O con- taming HNO 3 . (Chretien.) Sodium molybdoiodate, Na 2 O, I 2 O 5 , 2MoO 3 + H 2 O. SI. sol. in H 2 O. Sol. in HNO 3 with decomp. (Chretien, C. R. 1896, 123. 178.) 1 1. H 2 O dissolves 6.97 g. of the salt at 15; 22.75 g. at 90. 1 1. HNO 3 +Aq (1 : 10) dissolves 23.78 g. of the salt at ord. temp. (Chretien, A. ch. 1898, (7) 15. 410.) +2H 2 O. Only si. sol. in cold H 2 O; sol. on long boiling. 3.35 grams are sol. in 1 1. H 2 O at 12. (Rosenheim, A. 1899, 308. 50.) Strontium molybdoiodate, SrO, I 2 O 6 , 2MoO + 3H 2 O. Very sol. in H 2 O. (Chretien, A. ch. 1898, (7) 15. 415.) Strontium molybdoiodate, acid, 3SrO, (I 2 O 6 , 2MoO 3 ) 4 +15H 2 O. 1 1. H 2 O dissolves 2.94 g. of the salt at 15; 13.64 g. at 100. (Chretien.) Uranyl molybdoiodate, 2UO 3 , 4I 2 O 6 , 3MoO 3 + 3H 2 O. (Chretien.) Zinc molybdoiodate, ZnO, I 2 O 6 , 2MoO 3 + 5H 2 O. 1 1. H 2 O dissolves 4.08 g. of the salt at 15; 16.25 g. at 100. (Chretien.) 534 MOLYBDOIODATE ACID, ZINC Zincmolybdoiodate acid, ZnO, (I 2 O 5 , 2MoO 3 ) 3 +16H 2 O. Very sol. in H 2 O. (Chretien.) . Molybdoperiodic acid. Ammonium molybdoperiodate, 5(NH 4 ) 2 O, I 2 O 7 , 12MoO 3 +12H 2 O. Sol. in H 2 O. (Blomstrand, Sv. V. A. H. Bih. 1892. No. 6.) 4(NH 4 ) 2 O, I 2 O 7 , 8MoO 3 +7H 2 O. Very si. sol. in cold H 2 O. (Blomstrand.) Ammonium sodium , 2(NH 4 ) 2 O, Na 2 O, I 2 O 7 , 2MoO 3 +10H 2 O. Very si. sol. in H 2 O. (B.) -, 9BaO, Na 2 O, 2I 2 O 7 , Barium sodium 24MoO 3 +28H 2 O.' Very si. sol. in H 2 O. (B.) Calcium , 5CaO, I 2 O 7 , 12MoO 3 +26H 2 O. Extremely sol. in H 2 O. (Blomstrand.) 4CaO, I 2 O 7 , 12MoO 3 +21H 2 O. Less sol. in H 2 O than above salt. Lithium , 5Li 2 O, I 2 O 7 , 12MoO 3 +30H 2 O. Not so efflorescent as Na salt. Sol. in H 2 O. (B.) + 18H 2 0.) (B.) -, 2MnO, 3Na 2 0, Manganous sodium I 2 O 7 , 12MoO 3 +32H 2 O. Sol.inH 2 0. (B.) Potassium , 5K 2 O, I 2 O 7 , 12MoO 3 + 12H 2 O. Not efflorescent. (Blomstrand.) Sodium , 5Na 2 O, I 2 O 7 , 12MoO 3 +34H 2 O. Efflorescent. Very sol. in H 2 O. (Blom- strand, Sv. V. A. H. Bih. 1892. No. 6. 24.) +26H 2 O. Not efflorescent. Very sol. in H 2 O. (Blomstrand.) Sodium strontium , Na 2 O, 4SrO, I 2 O 7 , 12MoO 3 +20H 2 O. Sol. inH 2 O. (B.) Molybdophosphoric acid. See Phosphomolybdic acid. Molybdosw&phosphoric acid. Sodium molybdosu&phosphate, Na 2 [P(Mo 2 O 7 ) 3 ]+8H 2 O. Ppt. (Rosenheim, Z. anorg. 1913, 84. 222.) Molybdophosphorous acid. Potassium molybdophosphite, K 2 [HP(Mo 2 O 7 ) 3 ] + 1 1H 2 O. Difficultly sol. in cold H 2 0. (Rosenheim, Z. anorg. 1913, 84. 219.) Sodium molybdophosphite, Na 2 [HP(Mo 2 O 7 ) 3 ] + llH 2 O. SI. sol. in H 2 O. (Rosenheim, Z. anorg. 1913, 84. 218.) Molybdophosphovanadic acid. See Phosphovanadiomolybdic acid. Molybdoselenious acid. Ammonium molybdoselenite, 4(NH 4 ) 2 O, 3SeO 2 , 10MoO 3 +4H 2 O. More sol. in hot than cold H 2 O; insol. in alcohol. (Pechard, A. ch. (6) 30. 403.) Ammonium potassium molybdoselenite, 2(NH 4 ) 2 O, 2K 2 O, 3SeO 2 , 10MoO 3 + 5H 2 O. Very sol. in H 2 O; insol. in alcohol. (Pech- ard.) Barium molybdoselenite, 4BaO, 3SeO 2 , 10MoO 3 +3H 2 O. SI. sol. in cold, easily in warm H 2 O. (Pechard.) Potassium molybdoselenite, 4K 2 O, 3SeO 2 , 10MoO 3 +5H 2 O. Very sol. in H 2 O; insol. in alcohol. (Pech- ard.) Sodium molybdoselenite, 4Na 2 O, 3SeO 2 , 10Mo0 3 + 15H 2 O. Very efflorescent, and sol. in H 2 0; insol. in alcohol. (Pechard.) Molybdosilicic acid. See Silicomolybdic acid. Molybdosilicovanadic acid. See Silicovanadiomolybdic acid. Molybdosulphuric acid. Appreciably sol. in H 2 O. (Hoffmann, Dissert. 1903.) Ammonium molybdosulphate, (NH 4 ) 2 O, 2MoO 3 , SO 3 +4H 2 O, and +9H 2 O. Decomp. by H 2 O. (Weinland, Z. anorg. 1907, 64. 261.) (NH 4 ) 2 O, 2MoO 3 , 3SO 3 + 10H 2 O. (Wein- land.) Ammonium molybdenyl molybdosulphate, (NH 4 ) 2 O, MoO 2 , 7MoO 3 , SO 3 +zH 2 O. 1^(NH 4 ) 2 O, MoO 2 , 7MoO 3 , SO 3 +5H 2 O. 2(NH 4 ) 2 O, MoO 2 , 7MoO 3 , SO 3 +14H 2 O. (Hoffmann, Dissert. 1903.) 3NH 3 , MoO 2 , 7MoO 3 , S9 3 +10H 2 O. Very sol. in H 2 O. Very si. sol. in NH 4 salts +Aq. Very stable toward alkali +Aq. (Pechard, C. R. 1893, 116. 1441.) NEODYMIUM HYDROXIDE 535 5NH 3 , MoO 2 , 7MoO 3 , SO 3 +8H 2 O. (Pe- chard, C. R. 1893, 116. 1441.) Potassium molybdosulphate, K 2 O, 2MoO 3 , SO 3 +2H 2 O. K 2 O, 2MoO 3 , SO 3 +6H 2 O. K 2 O, 2MoO 3 , 3SO 3 +6H 2 O. (Weinland, Z. anorg. 1907, 54. 260.) Potassium molybdenyl molybdosulphate, K 2 O, MoO 2 , 7MoO 3 , SO 3 +8H 2 O. (Hoffmann, Dissert. 1903.) Molyb do sulphurous acid. Ammonium molybdosulphite, 4(NH 4 )2O, 3SO 2 , 10MoO 3 +6H 2 O. SI. sol. in cold, more easily in hot H 2 O. Insol. in alcohol. (Pechard, "A. ch. (6) 30. 396.) 3(NH 4 ) 2 O, 8MoO 3 , 2SO 2 +5H 2 O. SI. sol. in cold, easily sol. in warm H 2 O. Easily de- comp. by H 2 O, and can be recryst. only in presence of an excess of sulphurous acid. (Rosenheim, Z.. anorg. 1894, 7. 177.) Ammonium potassium molybdosulphite, 2(NH 4 ) 2 O, 2K 2 O, 3SO 2 , 10MoO 3 +9H 2 O. SI. sol. in cold H 2 O. Decomp. on warming. (Pechard.) Barium molybdosulphite, 2BaO, 5MoO 3 , 2SO 2 -flOH 2 O. (Rosenheim, Z. anorg. 1897, 15. 185.) Caesium molybdosulphite, 2Cs?O, 5MoO 3 , 2SO 2 +6H 2 O. Unstable. As K salt. (Rosenheim.) Potassium molybdosulphite, 4K 2 O, 3SO 2 , 10Mo0 3 +10H 2 O. Very si. sol. in H 2 O, but decomp. on warm- ing. (Pechard.) 2K 2 O, 5MoO 3 , 2SO 2 +H 2 O. (Rosenheim.) Rubidium molybdosulphite, 2Rb 2 O, 5MoO 3 , 2S0 2 + ^H 2 0. As K salt. (Rosenheim.) Sodium molybdosulphite, 4Na 2 O, 3SO 2 , 10MoO 3 + 12H 2 O. Very sol. in cold H 2 O; insol. in alcohol. (Pechard.) + 16H 2 O. Very efflorescent. (Pechard.) 2Na 2 O, 5MpO 3 , 2SO 2 +8H 2 O. In dry state it gradually gives off SO 2 and soon effloresces. (Rosenheim.) Strontium molybdosulphite, 2SrO, 5MoO 3 , H 2 O. + 12 (Rosenheim.) Molybdotitanic acid. See Titanomolybdic acid. Molyb dous acid. Magnesium molybdite, Mg 2 Mo 3 O 8 =2MgO, 3MoO 2 . Not attacked by KOH, and HCl+Aq. (Muthmann, A. 238. 108.) Zinc molybdite, Zn 2 Mo 3 O 8 = 2ZnO, 3MoO 2 . Easily sol. in aqua regia. (Muthmann, A. 238. 108.) Molybdovanadates. See Vanadiomolybdates. Neodymicotungstic acid. Ammonium neodymicotungstate, 3(NH 4 ) 2 O, Nd 2 O 3 , 16WO 3 +20H 2 O. Difficultly sol. in H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1904, 26. 1480.) Barium neodymicotungstate, 6BaO, Nd 2 O 3 , 16WO 3 +17H 2 O. Insol. in H 2 O. (E. F. Smith.) Neodymium. See also under Didymium. Neodymium bromide, NdBr 3 . (Matignon, C. R. 1905, 140. 1638.) Neodymium carbide, NdC 2 . Decomp. by H 2 O; insol. in cone. HNO 3 ; decomp. by dil. HNO 3 . (Moissan, C. R. 1900, 131. 597.) Neodymium chloride, NdCl 3 . 100 g. H 2 O dissolve 98.68 g. NdCl 3 at 13; 140.4 g. at 100. Sp. gr. at 15/4 of the solution sat. at 13 = (Matignon, A. ch. 1906, (8) 8. 249.) Bp. 1.74. 44.5 g. are sol. in 100 g. abs. alcohol at 20. 1.8 g. " " " " pyridine at 15. Insol. in ether, CHC1 3 , quinoline, toluidine, etc. SI. sol. in aniline and in phenylhydra- zine. (Matignon, A. ch. 1906, (8) 8. 266.) +6H 2 O. Deliquescent. At 13, 100 pts. H 2 O dissolve 246.2 pts. of the hydrated salt. At 100, 100 pts. H 2 O dissolve 511 pts. of hydrated salt. Sat. solution at 13 has a sp. gr. 15/4 = 1.741. (Matignon, C. R. 1901, 133. 289.) Neodymium chloride ammonia, NdCl 3 . 12NH 3 . Decomposes on heating into NdCl 8 +NHj; +2NH 3 ; +4NH 8 ; +5NH 3 ; +8NH 3 ; and +11NH 8 . (Matignon, C. R. 1906, 142. 1043.) Neodymium hydroxide. Sol. in citric acid. (Baskerville, J. Am. Chem. Soc. 1904, 26. 49.) 536 NEODYMIUM HYDRIDE Solubility in glycerine -fAq containing about 60% by vol. of glycerine. 100 ccm. of the solution contain 4.5 g. neodymium oxide. (Miiller, Z. anorg. 1905, 43. 322.) Neodymium hydride, NdH 2 (?). Slowly attacked by boiling H 2 O. Sol. in acids with violent evolution of H 2 . (Muth- mann, A. 1904, 331. 58.) Neodymium iodide, NdI 3 . (Matignon, C. R. 1905, 140. 1638.) Neodymium nitride, NdN. Decomp. in moist air with evolution of NH 3 . (Muthmann, A. 1904, 331. 59.) Neodymium oxide, Nd 2 O 3 . Easily sol. in acids, (v. Welsbach, M. 6. 477.) Neodymium oxychloride, NdOCl. (Matignon, C. R. 1905, 140. 1638.) Neon, Ne. Less sol. than argon in H 2 O; sol. in liquid oxygen. (Ramsay, B. 1898, 31. 3118.) Absorption by H 2 O at t. 10 20 30 40 50 Coefficient of absorption 0.0114 0.0118 0.0147 0.0158 0.0203 0.0317 (Antropoff, Roy. Soc. Proc. 1910, 83. A, 480.) Nickel, Ni. Not attacked by H 2 O. Very slowly sol. in dilute H 3 PO 4 , H 2 SO 4 , or HCl+Aq. (Tup- puti, A. ch. 78. 133.) Very easily attacked by HNO 3 +Aq, and difficultly by hot H 2 SO 4 . When pure, is con- verted into passive condition by cone. HNO 3 . (Nickles, C. R. 38. 284.) Very si. attacked by cold acids, except HNO 3 +Aq. (Tissier, C. R. 60. 106.) Not attacked by NaOH+Aq. (Venator, Dingl. 261. 133.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Nickel amide, Ni(NH 2 ) 2 . Decomp. by H 2 O; slowly sol. in min. acids. Insol. in liquid NH 3 . (Bohart, J. phys. Chem. 1915, 19. 560.) Nickel antimonide, NiSb. Insol. in HCl+Aq; easily sol. in HNO 3 + Aq. (Christofle, 1863.) Min. Breithauptite. Insol. in acids; easily sol. in aqua regia. Ni 3 Sb 2 . (Christofle.) Nickel antimonide sulphide, NiSb 2 , NiS 2 = NiSbS. Min. Nickel glance, Ullmannite. Decomp. by HNO 3 +Aq; completely sol. in aqua regia with separation of S. Nickel arsenide, NiAs. Min. Niccolite. Sol. in cone. HNO 3 +Aq with separation of As 2 O 3 ; more easily sol. in aqua regia. NiAs 2 . Min. Chloanthite, Rammelsbergite. Sol. in HNO 3 +Aq. Ni 3 As 2 . Sol. in HNO 3 and in aqua regia. Readily attacked by fused alkali. (Granger, C. R. 1900, 130. 915.) Nickel arsenide sulphide, NiAs 2 , NiS 2 . Min. Gersdorffite. Partly sol. in HN0 3 + Aq with separation of S and As 2 O 3 ; not at- tacked by KOH+Aq. Nickel azoimide, basic, Ni(OH)N 3 Insol. in H 2 O. (Curtius, J. pr. 1898, (2) 58. 300.) Nickel azoimide, NiN 6 +H 2 O. Sol. in H 2 O; insol. in alcohol and ether. (Curtius, J. pr. 1900, (2) 61. 418.) Nickel potassium azoimide, Ni(N 3 ) 2 , KN 3 (?). Sol. in H 2 O. (Curtius, J. pr. 1898, (2) 58. 302.) Nickel boride, Ni 2 B. Attacked by HNO 3 . Slowly sol. in hot HC1. (Jassoneix, C. R. 1907, 145. 240.) NiB. Decomp. by moist air and by alkali nitrates, chlorates, hydroxides and carbon- ates; decomp. by steam at red heat. Not attacked by HC1. Easily attacked by HNO 3 and aqua regia; by H 2 S0 4 only on heating. (Moissan, C. R. 1896, 122. 425.) NiB 2 . (Jassoneix, C. R. 1907, 145. 241.) Nickel bromide, NiBr 2 . Deliquescent. Slowly sol. in H 2 O. Sat. NiBr 2 +Aq contains at: 21 6 +19 38 47.1 51.7 56.6 58.9% NiBr 2 , 58 77 98 100 140 60.5 60.3 61.0 61.0 60.7% NiBr 2 . (Etard, A. ch. 1894, (7) 2. 542.) Somewhat hygroscopic. Nearly insol. in cold H 2 O but begins to dissolve appreciably at 50, and somewhat more rapiotly at 90, but even at that temp. 1 g. requires 1-2 hours for solution. HNO 3 does not appreciably hasten solution. (Richards and Cushman, Z. anorg. 1898, 16. 169.) NICKEL CHLORIDE 537 SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 61. 236.) +3H 2 O. Deliquescent. Very sol. in H 2 0, HCl+Aq, NH 4 OH+Aq, alcohol, and ether. (Berthemot, A. ch. 44. 389.) +6H 2 O. (Bolschakoff, C. C. 1897, II. 331 and 726.) +9H 2 O. (Bolschakoff, C. C. 1897, II. 726 and 331.) Nickel stannic bromide. See Bromostannate, nickel. Nickel bromide ammonia, NiBr 2 , 6NH 6 . Sol. in little H 2 O, but decomp. by more. (Rammelsberg, Pogg. 55. 243.) Sol. in warm cone. NH 4 OH+Aq; insol. in cold. (Richards and Cushmann, Z. anorg. 1898, 16. 175.) Nickel bromide cupric oxide, NiBr 2 , 3CuO + 4H 2 O. Not decomp. by H 2 O. (Mailhe, A. ch. 1902, (7) 27. 377.) Nickel bromide hydrazine, NiBr 2 , 2N 2 H 4 . Easily sol. in dil. acids and NH 4 OH+Aq. NiBr 2 , 3N 2 H 4 . Sol. in dil. acids. (Franzen, Z. anorg. 1908, 60. 263-4.) Nickel carbonyl, Ni(CO) 4 . Insol. in H 2 O; not attacked by dil. acids or alkalies or cone. HCl+Aq. Easily sol. in cone. HNOs+Aq and in aqua regia. Sol. in alcohol, benzene, and chloroform. (Mond, Langer, and Quincke, Chem. Soc. 57. 749.) Sol. in hydrocarbons, especially oil of tur- pentine. (Berthelot, C. R. 1891, 112. 1346.) Sol. in acetone, toluene, methyl and ethy] alcohol, etc. (Lenher and Loos, J. Am. Chem Soc. 1900, 22. 114.) Nickel chloride, NiCl 2 . Anhydrous. Not immediately sol. in H 2 O but gradually dissolves on boiling or by addi- tion of HCl+Aq. Deliquesces on air, and is then easily sol. in H 2 O. Sol. in NH 4 OH+Aq. Sol. in alcohol. Sol. in hot HCl+Aq only slowly. Sp. gr. of NiCl 2 +Aq containing: 5 10 15 20 25% NiCl 2 1.0493 1.0995 1.1578 1.2245 1.3000 (B. Franz, J. pr. (2) 6. 285.) Sp. gr. of NiCl 2 +Aq containing, grms. H 2 O, g. NiCl 2 +7H 2 O at 23.1: 128 g. ( = Y 2 mol.) 256 384 512 1.057 1.107 1.149 640 768 896 1024 1.220 1.249 1.276 1.301 in 100C 1.187 Hontaining g. NiCl 2 (anhydrous) : 65 g. ( = Y 2 mol.) 130* 195 260 325 390 1.061 1.119 1.176 1.230 1.284 1.335 (Gerlach, Z. anal. 28. 468.) Sp. gr. of NiCl 2 +Aq at room temp, con- aining : 11.449 22.69 30.40% Ni.Cl 2 . 1.1093 1.2264 1.3371 (Wagner, W. Ann. 1883, 18. 269.) Sp. gr. of NiCl 2 +Aq at 25. Concentration of NiCb+Aq 1-normal Vr- " V Sp. gr. 1.0591 1.0308 1.0144 1.0067 (Wagner, Z. phys. Ch. 1890, 5. 39.) Insol. in liquid NH 3 . (Franklin, A.m. Ch. J. 1898, 20. 828.) 100 pts. absolute alcohol dissolve at room temperature 10.05 pts. NiCl 2 . (Bodtker, Z. phys. Ch. 1897, 22. 511.) Sol. in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 51. 236.) < Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Solubility in glycol = 16. 1-16.3%. (de Coninck, C. C. 1905, II. 1234.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Anhydrous NiCl 2 -is insol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) +H 2 O. (Baubigny.) 1 1. sat. HCl+Aq at 12 contains 40 g. NiCl 2 dissolved from NiCl 2 , H 2 O. (Ditte.) +2H 2 O. (Sabatier, Bull. Soc. (3) 1. 88.) +6H 2 O. Deliquescent in moist, efflores- cent in dry air; sol. in H 2 O with evolution of heat. Sol. in 1.5 to 2 pts. H 2 O. Easily sol. in alcohol. (Tupputi.) 1 1. H 2 O dissolves 600 g. NiCl 2 +6H 2 O. (Ditte, A. ch. 1879, (5) 22. 551.) Sat. aq. solution contains at: 17 16 +10 18 29.7 31.0 37.3 38.5% NiCls, 38 59 78 96 41.9 45.0 46.6 46.7% NiCl 2 . (fitard, A. ch. 1894, (7) 2. 539.) Solubility of NiCl 2 +6H 2 O = 37.53% NiCl 2 at 25. (Foote, J. Am. Chem. Soc. 1912, 34. 882.) 100 pts. absolute alcohol dissolve at room temperature 53.71 pts. NiCl 2 +6H 2 O. (Bodt- ker, Z. phys. Ch. 1897, 22. 511.) 538 NICKEL HYDROGEN CHLORIDE +7H 2 O. 100 g. absolute alcohol dissolv 2.16 g. NiCl 2 +7H 2 O at 17 and 1.4 g. at 3 (de Bruyn, R. t. c. 1892, 11. 156.) Nickel hydrogen chloride, 3NiCl 2 , 2HC1+ 1^H 2 O. (Reitzenstein, Z. anorg. 1898, 18. 270.) Nickel rubidium chloride, NiCl 2 , 2RbCl. Easily sol. in H 2 O and HCl+Aq. (Godef- froy, B. 8. 9.) Nickel thallic chloride, NiCl 2 , 2T1C1 3 +8H 2 O Deliquescent. Can be cryst. from H 2 O. (Gewecke, A. 1909, 366. 221.) Nickel tin (stannous) chloride, NiCl 2 , SnCl 2 + 6H 2 O. Sol. in H 2 O. (Jorgensen.) Nickel tin (stannic) chloride. See Chlorostannate, nickel. Nickel chloride ammonia, NiCl 2 , 2NH 3 . Sol. in H 2 O, decomp. on boiling; insol. in alcohol. NiCl 2 , 3NH 3 +3H 2 O. (Andre, C. R. 1888, 106. 937.) NiCl 2 , 6NH 3 . Sol. in cold H 2 O without decomp. Insol. in alcohol. Very si. sol. in cone. NH 4 OH+Aq. Nearly insol. in a sat. solution of NH 4 C1 in NH 4 OH+Aq. (Sorensen, Z. anorg. 1894, 5. 363.) Nickel chloride cupric. oxide, NiCl 2 , 3CuO + 4H 2 O. Not decomp. by H 2 O. (Mailhe, A. ch. 1902, (7) 27. 377.) Nickel chloride hydrazine, NiCl 2 , 2N 2 H 4 . Sol. in dil. acids and NH 3 +Aq. (Franzen, Z. anorg. 1908, 60. 262.) NiCl 2 , 3N 2 H 4 . Sol. in dil. acids. (F.) Nickel potassium fluoride, NiF 2 , KF. +H 2 O. Sol. in H 2 0. (Wagner, B. 19. 896.) NiF 2 , 2KF. SI. sol. in H 2 O. in methyl or ethyl alcohol (Poulenc, C. R. 114. 747.) Scarcely sol. , or benzene. Nickel potassium zirconium fluoride. See Fluozirconate, nickel potassium. Nickel manganic fluoride. See Fluomanganate, nickel. Nickel sodium fluoride, NiF 2 , NaF-fH 2 O. Sol. in H 2 O. (Wagner, B. 19. 896.) Nickel stannic fluoride. See Fluostannate, nickel. Nickel titanium fluoride. See Fluotitanate, nickel. Nickel tungstyl fluoride. See Fluoxytungstate, nickel. Nickel vanadium fluoride. See Fluovanadate, nickel. Nickel zirconium fluoride. See Fluozirconate, nickel. Nickel fluoride ammonia, 5NiF 2 , 6NH 3 + 8H 2 O. Insol. in cold H 2 O. Decomp. by hot H 2 O. Easily sol. in dil. acids. (Bohm. Z. anorg. 1905, 43. 334.) Nickelous hydroxide, 4NiO 2 H 2 , H 2 O. -Very si. sol. in H 2 O. Sol. in acids. Insol. in KOH or NaOH+Aq. Somewhat diffi- cultly sol. in (NH 4 ) 2 CO 3 or NH 4 OH+Aq, but easily sol. in- presence of NH 4 salts. Sol. in NH 4 salts+Aq. Sol. in KCN+Aq. (Rod- gers, 1834.) Sol. in boiling NH 4 Cl+Aq. Nickel fluoride, NiF 2 . Sol. in about 5000 pts. H 2 O; insol. in alcohol and ether. Not attacked by HC1, HNO 3 , or H 2 SO 4 even when hot. (Poulenc, C. R. 114. 1426.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) +2H 2 O. Decomp. by pure H 2 O. Sol. in H 2 O acidulated with HF. (Berzelius.) +3H 2 O. (Clarke, Sill. Am. J. (3) 13. 291.) Nickel hydrogen fluoride, NiF 2 , 5HF+6H 2 O. Easily sol. in H 2 O and dil. acids. Sol. in NH 4 OH+Aq with decomp, (Bohm, Z. n-nn-nrr 1 Qfl AQ QQfl "> Ni0 2 H 2 . Solubility in NH 4 OH+Aq at 25. NHs norm. G. Ni per 1. G. Ni0 2 H 2 per 1. 1 2 3 4 0.084 0.170 0.257 0.360 0.00287 0.00579 0.00875 0.01227 4.911 3.900 2.101 0.602 2.580 1.780 0.835 0.158 0.0879 0.0607 0.0284 0.0054 ;he formation of different modifications of NiO 2 H 2 . (Bonsdorff, Z. anorg. 1904, 41. 185.) NICKEL PHOSPHIDE 539 Solubility in NH 4 OH+Aq. Cone, of Ni = 0.014N in IN NH 4 OH+Aq. " " " =0.036N "2NNH 4 OH+Aq. CStarck, B. 1903, 36. 3840.) Sol. in hot NH 4 F+Aq. (von Helmolt, Z. anorg. 1893, 3. 133.) Insol. in methyl or amyl amine. (Wurtz.) Not pptd. in presence of Na citrate. (Spiller.) Not pptd. in presence of a large number of non-volatile organic substances, particularly H 2 C 4 H 4 O 6 . (Rose.) Nickelonickelic hydroxide, Ni 3 O 4 , 2H 2 O. Sol. in acids; insol. in H 2 O and alkalies. (Dudley, J. Am. Chem. Soc. 1896, 18. 901.) Nickelic hydroxide, Ni 2 O 3 , 2H 2 O (?). (Wernicke, Pogg. 141. 122.) Ni 2 O 3 , 3H 2 O (?). Sol. in acids as nickelous salts. Not attacked by boiling KOH or NaOH+Aq. Slowly sol. in HC 2 H 3 O 2 +Aq. Sol. in NH 4 OH, and NH 4 salts+Aq. (Od- ling.) Nickel iodide, NiI 2 . Deliquescent and sol. in H 2 O. (Erdmann, J. pr. 7. 254.) Sat. NiI 2 +Aq contains at: 23 6 +11 16 51.8 54.3 57.8 59.0% NiI 2 , 43 80 85 90 64.1 65.0 65.2 65.7% NiI 2 . (Etard, A. ch. 1894, (7) 2. 546.) +6H 2 O. Deliquescent. Easily sol. in H 2 O. (Erdmann.) Nickel iodide ammonia, NiI 2 , 4NH 3 . (Rammelsberg, Pogg. 48. 119.) NiI 2 , 6NH 3 . Decomp. by H 2 O. Sol. in warm oil. NH 4 OH+Aq. Very si. sol. in cone. NH 4 OH+Aq. (Erdmann.) Nickel iodide hydrazine, NiI 2 (N 2 H 4 ) 2 . Insol. in H 2 O. Sol. in acids. (Franzen, Z. anorg. 1911, 70. 150.) Nickel sutoxide, Ni 3 O 2 +H 2 O. Insol. in H 2 O; sol. in HC1 and H 2 SO 4 and HNO 3 ; also in KCN+Aq. (Moore, C. N. 1895, 71. 81.) Nickelous oxide, NiO. Insol. in H 2 O. Sol. in cone, acids, except when crystalline, when it is scarcely attacked by acids. (Ebelmen, C. R. 33. 256.) Very si. sol. in boiling NH 4 Cl+Aq. (De- margay.) Very slowly sol. in NH 4 OH+Aq. Insol. in KOH, and NaOH+Aq. Sol. in min. acids, especially HCl+Aq, when warmed; insol. in HC 2 H 3 O 2 , NH 4 C1, and NH 4 SCN+Aq. Insol. in cone. NaOH+ Aq. (Zimmerman, A. 232. 324.) 1 1. solution containing 418.6 g. sugar and 34.3 g. CaO dissolves 0.29 g. NiO. (Boden- bender, J. B. 1866. 600.) Min. Bunsenite. Nickelonickelic oxide, Ni 3 4 . Sol. in acids. (Baubigny, C. R. 87. 1082.) +2H 2 O. Insol. in H 2 O, and in alkalies+ Aq. Sol. in acids. (Dudley, J. Am. Chem. Soc. 1896, 18. 901.) 6NiO, Ni 2 O 3 +H 2 O. (Schonbein, J. pr. 93. 35.) Nickelic oxide, Ni 2 O 3 . Sol. in HNO 3 , H 2 SO 4 , or HCl+Aq with decomp., also in NH 4 OH and (NH 4 ) 2 CO 3 + Aq. (Winkelblech, A. 13. 259.) Nickel peroxide, Ni 3 O 6 (?). (Bayley, C. N. 39. 81.) Correct composition is Ni 2 O 3 . (Carnot, C. R. 108. 610.) Ni 4 O 7 (?). (Wicke, Zeit. Ch. 1865. 303.) NiO 4 . (Hollard, C. R. 1903, 136. 230.) Nickel oxychloride. SI. sol. in H 2 O. (Berzelius.) NiCl 2 , 8NiO+13H 2 O. (Raoult, C. R. 69. Nickel oxyiodide, NiI 2 , 9NiO + 15H 2 O. Insol. in H 2 O. Sol. in HNO 3 +Aq or acetic acid. Insol. in NH 4 OH+Ac*. Alcohol dis- solves out NiI 2 . (Erdmann.) Nickel oxyselenide. Ahnost insol. in boiling HC1; decomp. by HNO 3 . (Fonzes-Diacon, C. R. 1900, 131. 557.) Nickel phosphide, Ni 2 P. Sol. in HNO 3 +Aq and aqua regia; insol. in HCl+Aq. (Struve, J. pr. 79. 321.) Sol. in aqua regia and in HNO 3 ; sol. in fused alkali. (Granger, Bull. Soc. 1896, (3) 15. 1089.) Easily sol. in HN0 3 . (Granger, C. N. 1898, 77. 229.) When prepared by heating phosphorus, copper and nickel in electric furnace, is insol. in all acids except a mixture of HNO 8 and HF. (Maronneau, C. R. 1900, 130. 657.) NiP 2 . Sol. in HNO 3 ; decomp. by fused NaOH. (Jolibois, C. R. 1910, 150. 107.) NiP 3 . Sol. in HNO 3 ; decomp. by fused NaOH. (J.) Ni 2 P 3 . Insol. in HNO 3 , HC1 and aqua regia; stable in the air even when heated (Granger, Bull. Soc. 1896, (3) 15. 1086.) Ni 3 P 2 . Not attacked by HC1. Easily at- tacked by HNO 3 . (Rose, Pogg. 1832^ 24. 232.) 540 NICKEL PHOSPHOSULPHIDE N 5 P2. Sol. in HNO 3 , aqua regia and in fused alkali. (Granger, C. R. 1896, 123. 177. Nickel phosphosulphide, Ni 3 PS 3 . Decomp. by hot H 2 O or by aqua regia SI. attacked by HNO 3 . (Ferrand, A. ch 1899, (7) 17. 417.) Nickel semiselenide, Ni 2 Se. Almost insol. in boiling HC1; decomp. by HNO 3 . (Fonzes-Diacon, C. R. 1900, 131. 557.) Nickel selenide, NiSe. Insol. in H 2 O, dil. or cone. HCl+Aq slowly sol. in HNO 3 +Aq; easily in aqua regia (Little, A. 112. 211.) Almost insol. in boiling HC1; decomp. by HNO 3 . (Fonzes-Diacon, C. R. 1900, 131. 557.) NiSe 2 . (Fonzes-Diacon.) Ni 3 le 4 3 j Almosfc inso1 - in boiling HC1; decomp. by HNO 3 . (Fonzes-Diacon.) Nickel siHcide, Ni 2 Si. Sol. in HF and aqua regia; insol. in cold H 2 O; decomp. by steam at red heat; sol. in fused alkali carbonates. (Vigouroux, C. R. 1895, 121. 687.) Nickel semzsulphide, Ni 2 S. Sol. in HNp 3 +Aq, with residue of S. Difficultly sol. in cone. HCl+Aq; insol. in dil. HCl+Aq. (Arfvedson, Pogg. 1. 65; Gautier, C. R. 108. 1111.) Does not exist. (Bornemann, C. A. 1908. 1686.) Nickel raonosulphide, NiS. Anhydrous. Insol. in H 2 O, HC1, or H 2 SO 4 +Aq. Sol. in HNO 3 +Aq or aqua regia. Min. Millerite. +rcH 2 O. Insol. in H 2 O, but decomp. by H 2 O in contact with the air (Clermont and Guiot, C. R. 84. 714), or by boiling with H 2 O. (Geitner, A. 139. 354.) When pptd. with (NH 4 ) 2 S, is somewhat sol. in H 2 0. 1 1. H 2 O dissolves 39.87 X 10 6 moles NiS at 18. (Weigel, Z. phys. Ch. 1907, 68. 294.) Very si. sol. in dil. HCl+Aq, and still less in HC 2 H 3 O 2 +Aq. (Fresenius.) More sol. in HNO 3 +Aq, and easily in aqua regia. Somewhat sol. in NH 4 OH+Aq or solutions of alkali sulphides. Insol. in NH 4 SH+Aq. (Fresenius.) Sol. at moment of formation in Na 2 S but not in (NH 4 ) 2 S+Aq. (Villiers, C. R. 1894, 119. 1264.) Sol. while yet moist in H 2 SO 3 +Aq. (Ber- thier.) When recently pptd., sol. in KCN+Aq. (Haidlen.) Pptd. in presence of non- volatile organic substances as tartaric acid, etc. (Rose.) Sol. in potassium thiocarbonate+Aq. (Rosenbladt, Z. anal. 26. 15.) Exists in a colloidal form in a very dil. solution. (Winnsinger, Bull. Soc. (2) 49. 452.) a modification: Very sol. in 2N-HCl+Aq sat. with H 2 S. j8 modification: 0.033 g. is sol. in 1 1. 2N-HCl+Aq sat. with H 2 S; very sol. in 2N-HCl+Aq. 7 modification: Insol. in 2N-HCl+Aq sat. with H 2 S. 0.013 g. is sol. in 2N-HCl+Aq. (Thiel, C. C. 1914, I. 19.) Nickel sulphide, Ni 3 S 2 , (Bornemann, C. A. 1908. 1686.) Ni 3 S 4 . (Bornemann.) Ni 6 S 6 . (Bornemann.) Ni 4 S 5 . Min. Polydymite. Insol. in HC1+ Aq. Sol. in HNO 3 +Aq with separation of S. Ni 5 S 7 . Min. Beyrichite. Sol. in HCl+Aq. Nickel bisulphide, NiS 2 . (Fellenberg, Pogg. 50. 75.) Does not exist. (Bellucci, C. A. 1909. 293.) Nickel potassium sulphide, 3NiS, K 2 S. Insol. in H 2 O. (Schneider, J. pr. (2) 9. EsNiiiSio. Not attacked by hot (NH 4 ) 2 S; slowly attacked by HC1 or cold aqua regia; quickly by hot aqua regia. HF and H 2 SQ 4 dissolve only on heating. Insol. in organic acids, alkalies and 12% HC1, also in KCN, AgNO 3 or CuSO 4 +Aq. (Milbauer, Z. anorg. 1904, 42. 447.) Nickel telluride, Ni 2 Te 3 . Min. Melonite. Sol. in HN0 3 +Aq. NiTe. (Fabre, C. R. 105. 277.) Nickelicotungstic acid. Ammonium nickelicotungstate, 2(NH 4 ) 2 O, .2Ni 2 O 3 , 8WO 3 +14H 2 O. (Rogers and Smith, J. Am. Chem. Soc. 1904, 26. 1476.) 3(NH 4 ) 2 0, Ni 2 3 , 16W0 3 +22H 2 0. Very si. sol. in H 2 O. (Rogers and Smith.) Barium nickelicotungstate, 19BaO, Ni 2 O 3 , 16W0 3 . Ppt. Very insol. in H 2 O. (E. F. Smith.) STickelimolybdic acid. Barium nickelimolybdate, 3BaO, NiO 2 , 9MoO 3 + 12H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 02.) NITRATOPURPUREOCOBALTIC BROMIDE 541 Potassium nickelimolybdate, 3K 2 O, NiO 2 , 9MoO 3 +63^H 2 O. Very insol. even in hot H 2 O. (Hall.) Nickelomolybdic acid. Ammonium hydrogen nickelomolybdate, (NH 4 )4H 6 [Ni(MoO 4 ) 6 ] +5H 2 O. SI. sol. in H 2 O, easily in dil. acids. (Bar- bieri, C. A. 1915. 897.) Barium hydrogen nickelomolybdate, Ba 2 H 6 [Ni(MoO 4 ) 6 ] + 10H 2 O. Ppt. (Barbieri.) Potassium hydrogen nickelomolybdate. K 4 H 6 [Ni(Mo0 4 ) 6 ]+5H 2 0. SI. sol. in H 2 O, easily in acids. (Barbieri.) Silver hydrogen nickelomolybdate, Ag 4 H 6 [Ni(Mo0 4 ) 6 ]+3H 2 0. Insol. in H 2 O; sol. in NH 4 OH, or HNO 3 + Aq. (Barbieri.) Nickelonickelous acid. Potassium nickelonickelite, K 2 Ni 2 O 4 or K 2 O, NiO, NiO 2 . '(Hofmann and Hiendlmaier, B. 1906, 39. 3186.) Sodium nickelonickelite, Na 2 Ni 3 O 6 = Na 2 O, NiO, 2NiO 2 . (Bellucci and Rubegni, C. C. 1907, 1. 794.) Nickelous acid. Barium eftnickelite, BaO, 2NiO 2 . Unstable; decomp. by cold H 2 O; slowly and very rapidly by hot H 2 O. (Dufau, C. R. 1896, 123. 496.) Niobium, Nb. For niobium and its compounds, see colum- bium, Cb, and the corresponding compounds. Nitramide, NH 2 NO 2 . Decomp. by cone. H 2 S0 4 . Easily sol. in H 2 O, alcohol, 'ether and acetone. Less sol. in benzol. Almost insol. in ligroin. (Thiele and Lachman, A. 1895, 288. 297.) Sol. in ether, insol. in petroleum ether. Very unstable; decomp. by hot H 2 O. (Thiele and Lachman, B. 1894, 27. 1909.) Nitratochloroplatinamine comps. See Chloronitratoplatinamine comps. Nitratocobalt octamine comps. See Nitratooctamine cobaltic comps. Nitratooctamine cobaltic carbonate, (N0 3 ) 2 Co 2 (NH 3 ) 8 (C0 3 ) 2 +H 2 0. Less sol. than other octamine carbonates. (Vortmann and Blasberg, B. 22. 2650.) chloride, (NO 3 ) 2 Co 2 (NH 3 ) 8 Cl 4 +4H 2 O. (Vortmann and Blasberg, B. 22. 2652.) iodide, (NO 3 ) 2 Co 2 (NH 3 ) 8 I 4 +2H 2 O. (Vortmann and Blasberg.) nitrate. See Octamine cobaltic nitrate. sulphate, (N0 3 ) 2 Co 2 (NH 3 ) 8 (S0 4 ) 2 + 2H 2 0. +4H 2 O. (Vortmann and Blasberg, B. 22. 2652.) Nitratoplatinarnine nitrate, (N0 3 ) 2 Pt(NH 3 N0 3 ) 2 . SI. sol. in cold, more easily in hot H 2 O; easily sol. in dil. HNO 3 +Aq. (Cleve.) nitrite, (NO,),Pt(NH,NO,),. Easily sol. in H 2 O. (Cleve.) Nitratoplatindiamine chloride, (NO 3 ) 2 Pt(N 2 H 6 Cl) 2 +H 2 O. Moderately sol. in cold, very easily in hot H 2 O. chloroplatinate, (NO 3 ) 2 Pt(N 2 H 6 Cl) 2 , PtCl 4 +2H 2 O. Ppt. chromate, (NO 3 ) 2 Pt(N 2 H 6 ) 2 CrO 4 . Nearly insol. in H 2 O. (Cleve.) ^chromate, (NO 3 ) 2 Pt(N 2 H 6 ) 2 Cr 2 O 7 . SI. sol. in H 2 O. nitrate, (NO 3 ) 2 Pt(N 2 H 6 NO 3 ) 2 . Sol. in H 2 O. Insol. in HNO 3 +Aq. phosphate, NO 3 Pt(N 2 H 6 ) 2 +H 2 O. \ / P0 4 Very si. sol. in H 2 O. (Cleve.) Nitratodi'platindiamin e nitrate, (N0 3 ) 2 Pt 2 (N 2 H 6 ) 4 (N0 3 ) 4 . Sol. in H 2 O with decomp. Nitratopurpureocobaltic bromide, Co(NO 3 )(NH 3 ) 6 Br 2 . Resembles the chloride in its properties. (Jorgensen, J. pr. (2) 23. 227.) 542 NITRATOPURPUREOCOBALTIC CARBONATE Nitralopurpureocobaltic carbonate, Co(N0 3 )(NH 3 )5(C0 3 )+H 2 0. Less sol. in H 2 O than other purpureocar- bonates. (Vortmann and Blasberg, B. 22. 2648.) chloride, Co(NO 3 )(NH 3 ) 5 Cl 2 . SI. sol. in cold H 2 O, but more than nitrate; more easily sol. in hot H 2 O, but is converted into roseo salt. Insol. in HCl+Aq or alcohol. (Jorgensen, J. pr. (2) 23. 227.) mercuric chloride, Co(NO 3 )(NH 3 ) 5 Cl 2 , HgCl 2 . Not wholly insol. in H 2 O. (Jorgensen.) chloroplatinate, Co(NO 3 )(NH 3 ) 5 Cl 2 , PtCl 4 . Ppt. Nearly insol. in cold H 2 O. (Jorgen- sen.) chromate, Co(NO 3 )(NH 3 ) 5 CrO 4 . Nearly insol. in H 2 O. (Jorgensen.) bichromate. SI. sol. in H 2 O, but more easily than the neutral salt. (Jorgensen.) dithionate, Co(NO 3 )(NH 3 ) 5 S 2 O 6 . Very si. sol. in cold, more easily in hot H 2 O. (Jorgensen.) nitrate, Co(NO 3 )(NH 3 ) 5 (NO 3 ) 2 . Sol. in 273 pts. H 2 O at 16. Much more sol. in hot H 2 O containing HNO 3 . (Jorgensen, J. pr. (2) 23. 227.) cobaltic nitrite, 3Co(NO 3 )(NH 3 ) 5 , 2Co(NO 2 ) 6 +2H 2 O. Very si. sol. in H 2 O. (Jorgensen, Z. anorg. 5. 176.) diamine cobaltic nitrite, Co(NO 3 )(NH 3 ) 6 (N0 2 ) 4 Co(NH 3 ) 2 . Ppt. (Jorgensen.) oxalate, Co(NO 8 )(NH 3 ) 5 C 2 O 4 . Ppt. sulphate, Co(NO 3 )(NH 3 ) 5 SO 4 +H 2 O. Rather difficultly sol. in cold H 2 O. (Jor- gensen.) Nitratopurpureorhodium chloride, (NO 3 )Rh(NH 3 ) 5 Cl 2 . SI. sol. in cold H 2 O, but more easily than the nitrate. (Jorgensen, J. pr. (2) 34. 394.) - dithionate, (NO 3 )Rh(NH 3 ) 5 S 2 O 6 +H 2 O. Nearly insol. in cold H 2 O. (Jorgensen.) Nitratopurpureorhodium nitrate, (NO 3 )Rh(NH 3 ) 5 (NO 3 ) 2 . Very si. sol. in cold H 2 O. Insol. in alcohol. (Jorgensen.) Nitric acid, HNO 3 . Miscible with H 2 O. When HNO 3 +Aq is distilled at 760 mm. pressure, an acid contain- ing 68% HNO 3 is formed, which boils at 120.5 under 735 mm. pressure. By distilling at 150 mm. pressure the acid contains 67.6% HNO ? ; at 70 mm. (b.-pt. 65-70) the acid contains 66.7% HN0 3 . The percentage of HNO 3 in the liquid obtained by passing dry air into HNO 3 +Aq containing 64-68% HNO 3 varies with the temp.; the higher the temp, the greater the percentage of HNO 3 . (Roscoe, Chem. Soc. 13. 150.) HNOs-trAq of 1 .51 sp. gr. contains 67% N 2 O 6 . 142 " " 54 1.35 " " 44.4 1.315 " " 38.6 (Dalton.) HNOs+Aq of 1 .52 sp. gr. contains 88.82% N 2 O 5 . 1.522 " " 86.17% " 1.4 " " 44 (Mitscherlich.) HNOs+Aq of 1.298 sp. gr. contains 36.75% N 2 O S . (Kirwan.) HNOs+Aq of 1.298 sp. gr. contains 48%. (Davy.) HNOs+Aq of 1.298 sp. gr. contains 32-33%. (Ber- thollet.) For Ure's table of sp. gr. of HNO 3 +Aq, see Watt's Diet.. 1st ed. Sp. gr. of HNO 3 +Aq at and 15. % HN0 3 & . Sp. gr. at Sp. gr. at 15 100.00 85.71 1.559 1.530 99.84 85.57 1.559 1.530 99.72 85.47 1.558 1.530 99.52 85.30 1.557 1.529 97.89 83.90 1.551 1.523 97.00 83.14 1.548 1.520 96.00 82.28 1.544 1.516 95.27 81.66 .542 1.514 94.00 80.57 .537 1.509 93.01 79.72 .533 1.506 92.00 78.85 .529 1.503 91.00 78.00 .526 1.499 90.00 77.15 .522 1.495 89.56 76.77 .521 1.494 88.00 75.43 1.514 1.488 87.45 74.95 1.513 1.486 86.17 73.86 1.507 1.482 85.00 72.86 1.503 1.478 84.00 72.00 1.499 .474 83.00 71.14 1.495 .470 82.00 70.28 1.492 .467 80.96 69.39 1.488 .463 80.00 68.77 1.484 .460 79.00 67.71 1.481 .456 77.66 66.56 1.476 .451 76.00 65.14 1.469 .445 75.00 64.28 1.465 .442 74.01 63.44 1.462 .438 NITRIC ACID 543 Sp. gr. of HNO 3 , etc. Continued. Sp. gr. of HNO 3 +Aq at 15. a = %;b = sp. nloa NTb 5 Sp. gr. at Sp. gr. at 15 gr. if % is N 2 O 5 ; c-sp. gr. if % is HNO 3 . a b C a b c 73.00 72.39 71.24 69.96 69.20 68.00 67.00 66.00 65.07 64.00 63.59 62.00 61.21 60.00 59.59 58.88 58.00 57.00 56.10 55.00 54.00 53.81 53.00 52.33 50.99 49.97 49.00 48.00 47.18 46.64 45.00 62.57 62.05 61.06 60.00 59.31 58.29 . 57.43 . 56.57 55.77 54.84 54.50 53.14 52.46 51.43 51.08 50.47 49.71 48.86 48.08 47.14 46.29 46.12 45.40 44.85 43.70 42.83 42.00 41.14 40.44 39.97 38.57 1.457 1.455 1.450 1.444 1.441 1.435 ,1.430 1.425 1.420 1.415 1 . 413 1.404 1.400 1.393 1.391 1.387 1.382 1.376 1.371 1.365 .359 .358 .353 .349 .341 .334 .328 .321 .315 .312 .300 1.435 1.432 1.429 1.423 1.419 .414 .410 .405 .400 .395 .393 .386 .381 .374 1.372 1.368 1.363 1.358 1.353 1.346 1.341 1.339 1.335 1.331 1.323 1.317 .312 .307 .398 .295 .284 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 1.007 1.014 1.021 1.027 1.034 1.040 1.047 1.053 1.061 1.069 1.076 1.083 1.091 1.098 1.104 1.112 .120 .126 .134 .141 .149 .156 .165 .172 .180 .187 .195 .202 .211 .218 .225 1.006 1.012 1.018 1.024 1.029 1.035 1.040 1.045 I'.OSl 1.057 1.064 1.070 1.077 1.083 .089 .095 .100 .106 .112 .120 .126 .132 .138 .145 .151 .159 .166 .172 1.179 1.185 1.192 5t 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 1.372 1.378 1.385 1.390 1.396 1.401 1.407 1.413 1.418 1.423 1.427 1.432 1.436 1.440 1.445 1.449 1.452 1.457 1.461 1.466 .470 .474 .478 .482 .486 1.490 1.494 1.499 1.503 1.507 1.511 1.323 1.329 1.335 1.341 1.346 1.356 1.358 1.363 1.369 1.374 1.380 1.386 1.390 1.395 1.400 1.405 1.410 1.414 1.419 1.422 1.427 1.430 1.435 1.439 1.442 1.445 1.449 1.452 1.456 1.460 1.463 43.53 37.31 .291 .274 32 1 . 232 1.198 82 1.515 1.467 42.00 36.00 .280 .264 33 1.240 1.204 83 1.519 1.470 41.00 35.14 .274 .257 34 1.248 1.210 84 1.523 1.474 40.00 39.00 37.95 34.28 33.43 32.53 .267 1.260 1.253 .251 .244 .237 35 36 37 1.255 1.264 1.271 1.218 1.225 1.230 85 86 87 1.527 1.530 1.478 1.481 1.484 36.00 30.86 1.240 1.225 38 1.280 1.236 88 1.488 35.00 29.99 1.234 1.218 39 .286 1.244 89 1.491 33.86 29.02 1.226 1.211 40 .295 1.251 90 1.495 32.00 27.43 1.214 1.198 41 .304 1.257 91 1.499 31.00 26.57 1.207 1.192 42 312 1 264 92 1.503 30.00 25.71 1.200 1.185 43 .318 1.270 93 1.506 29.00 24.85 :1.194 1.179 44 .325 1.276 94 1.509 28.00 24.00 1.187 .172 45 1.332 1.284 95 1.512 27.00 23.14 1.180 .166 46 1.340 1.290 96 1.516 25.71 22.04 .171 .157 47 1.346 1.298 97 1.520 23.00 19.71 .153 .138 48 1.352 1.304 98 1.523 20.00 17.14 .132 .120 49 1.360 1.312 99 1.526 17.47 14.97 .115 1.105 50 1.366 1.316 100 1.530 15.00 12.85 .099 1.089 13.00 11.14 1.085 1.077 (Kolb, calculated by Gerlach, Z. anal. 8. 292. 11.41 7.72 9.77 6.62 1.075 1.050 1.067 1.045 Sp. gr. of HNO 3 +Aq at 17.5. 4.00 3.42 1.026 1.022 2.00 1.71 1.013 1.010 N^>5 Sp. gr. Njfos Sp. gr. Nabs * Sp. gr. 0.00 o on i nru~i OQOQ \J . \J\J . t/iy t7 1 o (Kolb, A. ch. (4) 10. 140.) 6 1.'038 10 1.'068 lo 14 1.'096 7 1.045 11 1.075 15 1.104 8 1.053 12 1.082 16 1.111 541 NITRIC ACID Sp. gr. of HNO 3 , etc. Continued. Most accurate table. %N 2 6 So. gr. % N 2 5 Sp. gr. %N 2 C>5 Sp. gr. Sp. gr. of HNO 3 +Aq at 15; H 2 O at 4 = 1. 17 18 1.118 1.125 40 41 1.294 1.301 63 64 1.434 1.438 Sp. gr. % N 2 5 % HN0 3 Kg. HNO 3 in 1 1. 1Q 1 . 132 '4.9 1 OAC (C IAAf) I t 7 20 l!l40 TTA 43 . OUo 1.315 DO 66 . i fi 1.447 .000 0.08 0.10 0.001 21 1.147 44 1.323 ! 67 1.451 .005 0.85 1.00 0.010 22 1.115 45 1.330 68 1.456 .010 1.62 1.90 0.019 23 1.163 46 1 . 338 69 1.460 .015 2.39 2.80 0.028 24 1.170 47 1.345 70 1.465 .020 3.17 3.70 0.038 25 1.178 48 1.352 71 1.469 .025 3.94 4.60 0.047 26 1.186 49 1.35$ 72 1.472 .030 4.71 5.50 0.057 27 1.194 50 1.364 73 1.476 .035 5.47 6.38 0.066 28 1.201 51 1.371 74 1.480 .040 6.22 7.26 0.075 29 1.209 52 1.377 75 1.484 .045 6.97 8.13 0.085 30 1.217 53 1.383 76 1.488 .050 7.71 8.99 0.094 31 1.221 54 1.389 77 1.492 .055 8.43 9.84 0.104 32 1.232 55 1.394 78 1.496 .060 9.15 10.68 0.113 33 1.239 56 1.400 79 1.500 .065 9.87 11.51 0.123 34 1.247 57 1.406 80 1.504 .070 10.57 12.33 0.132 35 1.255 58 1.412 81 1.508 .075 11.27 13.15 0.141 36 1.263 59 1.416 82 1.512 .080 11.96 13.95 0.151 37 1.271 60 1.421 83 1.516 1.085 12.64 14.74 0.160 38 1.279 61 1.426 84 1.519 1.090 13.31 15.53 0.169 39 1.287 62 1.430 85 1.523 1.095 13.99 16.32 0.179 1.100 14 67 17.11 188 (Hager, Comm. 1883.) l!l05 15^34 17! 89 0^198 Sp. gr. HNO 3 +Aq at 17.5. 1.110 ' 16.00 18.67 0.207 %N 2 O 5 Sp. gr. % N 2 O 6 Sp. gr. % N 2 6 Sp. gr. .115 .120 16.67 17.34 19.45 20.23 0.217 0.227 10 15 20 30 1.068 1.104 1.140 1.217 40 50 60 1.293 1.361 1.417 70 80 85 1.465 1.500 1.5.14 .125 .130 .135 .140 18.00 18.66 19.32 19.98 21.00 21.77 22.54 23.31 0.236 0.246. 0.256 0.266 ' * .145 20.64 24.08 0.276 (Hager, Adjumenta varia, Leipzig, 1876.) .150 21.29 24.84 0.286 Sp. gr. of HNO 3 +Aq at 15. .555 1 IfiO 21.94 99 fin 25.60 9fi ^fi 0.296 Oqrvc % HN0 3 Sp. gr. % HN0 3 Sp. gr. -L . JLIJU 1.165 6 . DU 23.25 \J . OO 27.12 . oUO 0.316 1 1.00581 26 1 . 15869 1.170 23.90 27.88 0.326 2 1.01136 27 1.16660 1.175 24.54 28.63 0.336 3 1.01713 28 1.17371 1.180 25.18 29.38 0.347 4 1.02286 29 1.18073 1.185 25.83 30.13 0.357 5 .02851 30 1 . 18830 1.190 26.47 30.88 0.367 6 .03439 31 1 . 19552 1.195 27.10 31.62 0.378 7 .04019 32 1.20276 1.200 27.74 32.36 0.388 8 .04592 33 .20635 1.205 28.56 33.09 0.399 9 .05234 34 .21300 1.210 28.99 33.82 0.409 10 .05746 35 .22013 1.215 29.61 34.55 0.420 11 .06330 36 .22675 1.220 30.24 35.28 0.430 12 . 06951 37 .23347 1.225 30.88 36.03 0.441 13 .07581 . 38 .23980 1.230 31.53 36.78 0.452 14 .08126 39 .24510 1.235 32.17 37.53 0.463 15 .08843 40 .25235 1.240 32.82 38.29 0.475 16 .09500 41 .25850 1.245 33.47 39.05 0.486 17 1 . 10102 42 .26475 1.250 34.13 39.82 0.498 18 1.10725 43 .27125 1.255 34.78 40.58 0.509 ' 19 1.11321 44 .28895 1.260 35.44 41.34 0.521 20 1.12024 45 .28450 1.265 36.09 42.10 0.533 21 1.12714 46 .29110 1.270 36.75 42.87 0.544 22 1 . 13349 47 .29780 1.275 37.41 43.64 0.556 23 1 . 13890 48 .30443 1.280 38.07 44.41 0.568 24 1 . 14460 49 .31101 1.285 38.73 45.18 0.581 25 1.15164 50 .31722 1.290 39.39 45.95 0.593 1.295 40.05 46.72 0.605 (Squires, Pharm. Era, Jan. 1891.) NITRATES 545 Sp. gr. of HNO 3 , etc. Continued. Sp. gr. of N-HNO 3 +Aq at 18/4 = 1.0324. W4 1 OA^ /*f\ f ff\ \ ifr, wvm. (Loomis, . Ann. 18i: >o, ou. oou.; Sp. gr. % N 2 5 % HN0 3 in 11. Sp. gr. (reduced to a vacuum) of HNO 3 from 78-100% concentration at 4/4, 14.2 /4and24.2/4 . 1.300 1 . 305 40.71 41.37 47.49 48.26 0.617 0.630 1 310 42 06 49.07 0.643 1.315 Ioon 42' 76 49^89 CA *71 0^656 O/J/JA frf TTTVT/^ Sp. gr. .620 1.325 44! 17 oU. /I 51.53 .659 0.683 % MJNUs 4/4 14.2/4 24.2/4 1.330 1.335 .340 44.89 45.62 46.35 52.37 53.22 54.07 0.697 0.710 0.725 78.22 79.14 1.47129 1.45504 1.46011 1.43964 1.44372 .345 .350 48.07 47.82 54.93 55.79 0.739 0.753 79.59 81.97 1 . 47496 1.48391 1.46680 1^45092 .355 48.57 56.66 0.768 84.90 1 . 49495 .360 .365 49.35 50.13 57.57 58.48 0.783 0.798 85.21 85.80 1.49581 i'. 47826 I. 46224 .370 50.91 59.39 0.814 87.55 i.502li 0*7 er er i &f\ f*f\ on Ooork 87.90 .48491 1 . 46891 .375 oor\ 51.69 ero co 60.30 /j -| O*T .829 OO A C 89.73 1 50898 49125 . . o8() .385 .390 .395 .400 52.52 53.35 54.20 55.07 55.97 bl.27 62.24 63.23 64.25 65.30 .846 0.862 0.879 0.896 0.914 92.34 94.04 95.62 96.64 1.51804 ' 1.51949 1 . 52192 1.52510 .49968 .50149 .50358 .50632 1.48264 1.48516 1.48677 1.48887 1.405 1.410 1.415 56.92 57.86 58.83 66.40 67.50 68.63 0.933 0.952 0.971 97.33 98.07 99.97 i.532i2 1.54212 .50911 .51298 .52236 1.49137 1.49543 1.50394 1.420 1.425 59.83 60.84 69.80 70.98- 0.991 1.011 (Veley and Manley, Chem. Soc. 1 f\~t * \ 1903, 83. 1.430 61.86 72.17 1.032 1016.) 1.435 1.440 62.91 64.01 73.39 74.68 1.053 1.075 Sp. gr. at 20 of HNO 3 +Aq containing M g. mols. HNO 3 per liter. 1.445 65.13 75.98 .098 M 0.025 0.05 0.075 0.10 .450 66.24 77.28 .121 Sp. gr. 1. 000926 1.001798 1.002653 1.003496 .455 67.38 78.60 .144 .460 68.56 79.98 .168 M 0.25 0.5 0.75 1.0 .465 69.79 81.42 .193 Sp.gr. 1. 008481 1.01686 1.02503 1.0336 .470 71.06 82.90 .219 M 2.0 .475 72.39 84.45 .246 Sp. gr. 1.0670 .480 .485 73.76 75.18 86.05 87.70 .274 .302 (Jones and Pearce, Am. Ch. J. 1907, 38. 732.) 1.490 . 1.495 76.80 78.57 89.60 91.60 .335 .369 For sp H 2 SO 4 . . gr. of HN0 3 +H 2 S0 4 , see under 1.500 80.65 94.09 .411 Partition coefficient for HNO 3 between 1.501 81.09 94.60 .420 ether and H 2 O is increased by the addition 1.502 81.50 95.08 .428 of nitrates. (Tanret, C. R. 1897. 124. 464.1 1.503 1.504 1.505 1.506 81.91 82.29 82.63 82.94 95.55 96.00 96.39 96.76 .436 .444 .451 .457 The hydrates described by Erdmann do not exist. There are only two authentic hy- drates, the mono- and the tri-hydrate. (Kiister, Ch. Z. 1904, 28. 132.) 1.507 1.508 1.509 1.510 1.511 1.512 83.26 83.58 83.87 84.09 84.28 84.46 97.13 97.50 97.84 98.10 98.32 98.53 .464 .470 .476 .481 .486 .490 The composition of the hydrates formed by HNO 3 at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by HNO 3 and of the con- ductivity and sp. gr. of HNO 3 +Aq. (Jones, Am. Ch. .1. 1905. 34. 328.1 1.513 84.63 98.73 .494 1.514 84.87 98.90 .497 )mitric acid, H 2 N 4 U = 2N 2 6 , H 2 0. 1.515 1.516 1.517 84.92 85.04 85.15 99.07 99.21 99.34 .501 .504 ;507 ; Fumes evolution 6Q4.0 ^ on air. Miscible with of much heat. (Weber H 2 O, with , J. pr. (2) 1.518 85.26 99.46 . .510 ' > I _ . 1.519 85.35 99.57 , .512 Nitrates. 1.520 85.44 99 . 67 .515 All nitrates are sol. in H 2 O except a few (Lunge and Rey, Z. f . angew. Ch. 1891. 165.) basic compounds. Most nitrates are insol. in 546 NITRATE, ALUMINUM, BASIC cone. HNOs+Aq; many are sol. in alcohol; 100 pts. H 2 O dissolve 183 pts. NH 4 NO 3 at some are sol. in glycerine. 19.5. (Mulder.) Aluminum nitrate, basic, 2A1 2 O 3 , 3N 2 O 6 + 3H 2 O. Solubility in H 2 O at t. Sol. in H 2 O. (Ordway, Sill. Am. J. (2) 26. OAO "\ t Specific gravity of the saturated Mols. of NH 4 N0 3 soluble in 100 zOo.) Basic aluminum nitrates containing 2 mols. solution mols. of water or less of A1 2 O 3 to one of N 2 O 5 may be ob- 12.2 1 . 2945 34.50 tained sol. in H 2 O, but the compounds con- 20^2 1.3116 43.30 taining more than 2 mols. A1 2 3 are insol. in 23.0 .3159 46.57 H 2 O. (Ordway, I. c.) 2A1 2 O 3 , N 2 O 6 +10H 2 O. (Ditte, C. R. 110. 25.0 27.7 .3197 .3257 48.19 51.67 782.) 28 3260 51.86 Al 6 O 14 Hio, HNO 3 . Sol. in H 2 O. (Schlum- berger, Bull. Soc. 1895, (3) 13. 59.) 3o!o 30.2 !3299 .3308 54^40 54.61 Aluminum nitrate, A1(NO 3 ) 3 +9H 2 O. Deliquescent. Very sol. in H 2 O, HNO 3 + Aq, or alcohol. (Berzelius.) Melts in its crystal H 2 O at 72.7. (Ordway. Sol. in 1 pt. strong alcohol. (Wenzel.) Difficultly sol. in acetone. (Naumann, B. 31.9 32.1 32.7 34.0 35.0 35.1 35.6 .3348 .3344 .3356 .3375 .3394 .3397 .3408 57.20 57.60 57.90 58.89 59.80 60.00 60.62 1904, 37. 4328.) Insol. in ethyl acetate. (Naumann, B. 36.0 36 6 .3412 3420 61.00 1910, 43. ai4.) 37'5 ]3432 62^90 Ammonium nitrate, NH 4 NO 3 . 38.0 .3438 63.60 Deliquescent. Sol. in 0.502 pt. H 2 O at 18. (Karsten.) Sol. in 0.54 pt. H 2 O at 10. (Harris, C. R. 24. 816.) 38.5 39.0 39.5 .3440 .3448 .3460 64.10 65.09 65.88 Much more sol. is hot than cold H2O. (Harris.) 40.0 1.3464 66.80 Sol. in 2 pts. H 2 O at 15.5 and 0.5 pt. boiling H 2 O. (Fourcroy.) Sol. in 1 pt. cold, and 0.5 pt. boiling H 2 O. (Fourcroy.) (Miiller and-Kaufmann, Z. phys. Ch. 1903 Sol. in 0.5 pt. H 2 O at 18. (Berzelius.) 42. 4 yy.; Sol. in 2 pts. H 2 O at 18. (Abl.) Decomp. by boiling H 2 O. Solubility in H 2 at t. Solubility in 100 pts. H 2 O at t. G. NH 4 NO 3 t Pts. t Pts. Pts. t per 100 g. Solid phase t NH 4 NO 3 t NH 4 NO 3 NH 4 NO 3 solution water 1 97 101 24 25 205 210 48 49 351 358 12.2 54.19 60.53 118.3 153.4 NH 4 N0 3 , rhomb. 2 105 26 216 50 365 20 2 65 80 192 4 ,, 3 4 5 6 109 113 117 121 27 28 .29 30 221 226 232 238 51 52 53 54 372 379 387 395 25.Q 30.0 32.1 68^17 70.73 71.97 2U.2 241.8 256.9 NH 4 N0 3 , rhomb. + rhomb, ft 7 8 125 130 31 32 244 250 55 56 402 410 35 40 72.64 74 82 265.8 297.0 NH 4 NO 3 , rhomb, a 9 134 33 256 57 418 50 4 rr . O^w 77.49 344.0 M 10 139 34 262 58 425 60 80^81 421 io (l 11 143 35 268 59 433 70 S3. 32 499 'o (J 12 148 36 274 60 441 80 85 25 580 o 13 14 152 157 37 38 280 286 61 62 449 457 90 100 88^08 QQ 71 740 '.0 871.0 NH 4 NOs, rhomb. (?) 15 161 39 292 63 465 i\J\J Ot/ . f 1 16 166 40 298 64 473 (SeidelPs Solubilities 1st ed. 28. Calc. from 17 170 41 304 65 481 Miiller & Kauffmann, see above, and 18 175 42 311 66 490 Schwarz. Ostwald's Lehrb., p. 425.) 19 180 43 317 67 499 20 185 44 324 68 508 100 g NH 4 NO 3 +Aq contain: 21 190 45 331 69 517 54.19 g. NH 4 NO 3 at 0. 22 195 46 337 70 526 70 10 g " " 30. 23 200 47 344 84.03 g. " 70. (Mulder, Scheik. Verhandel. 1864. 95.) (de Waal, Dissert. Leiden, 1910.) NITRATE, AMMONIUM 547 70.19 g. NH 4 NO 3 are contained in 100 g. Sp. gr. of NH 4 NO 3 +Aq. NH 4 NO 3 +Aq sat. at 30. (Schreinemakers and de Baat, Arch. neer. Sc. 1911, (2) 16. % NH 4 NO 3 ' Sp. gr. 16/ 16 415.) 60 pts. NH 4 NO 3 mixed with 100 pts. H 2 O lower the temperature from 13.6 to 13.6, that is 27.2, but if the initial temperature is it will fall only to 16.7, the freezing- point of the mixture. (Rudorff, B. 2. 68.) 0.6419 1.4101 2.7501 5.4890 11.7981 .000000 .000271 .000593 .001153 .002300 .004916 Sp. gr. of NH 4 NO 3 +Aq at 18. 23.4480 47 9500 .009758 019952 Pts. NH 4 NO 3 Pts. H 2 O Sp. gr. (Dijken. Z. phys. Ch. 1897, 24. 107.) 80 1800 1 . 0180 80 900 1.0331 Sp. gr. 20/4 of a normal solution of NH 4 NO 3 80 360 1.0743 = 1.030435; of a 0.5-normal solution 1 = .014505. (Haigh, J. Am. Chem. Soc. 1912, 34. 1151.) (Thomsen and Gerlach, Z. anal. 28. 520.) Sp. gr. of NH 4 NO 3 +Aq at 15. B.-pt. of NH 4 NO 3 -fAq containing pts. NH 4 NO 3 to 100 pts. H 2 O. G = according to Gerlach (Z. anal. 26. 445); L= accord- % NH 4 NO 3 Sp. gr. % NH 4 NO 3 Sp. gr. ing to Legrand (A. ch. (2) 59. 426.) 5 1.0201 30 1.1304 * ^ 10 1.0419 40 1.1780 G L i G L 20 1.0860 50 1.2279 pq ffl (Kohlrausch, W. Ann. 1879. 1.) 101 102 10 20 10 20.5 140 141 682 719 770.5 Sp. gr. of NH 4 NO 3 +Aq at 17.5. 103 30 31.3 142 737 840 ' 6 104 41 42 4 143 765 % NH 4 N0 3 Sp. gr. % NH 4 N0 3 Sp. gr. 105 1 f\G 52 fiO 53.8 144 1 A K. 793 915.5 1 1.0042 33 1 . 1454 106 107 OO 74 77^3 145 146 853 995.5 2 1.0085 34 1.1502 108 85 89.4 147 883 3 .0127 35 1 . 1550 109 96 101.9 148 914 1081.5 4 .0170 36 1.1598 110 108 114.9 149 945 5 .0212 37 1 . 1646 111 120 128.4 150 977 U73.5 6 .0255 38 .1694 112 132 142 4 551 1009 7 .0297 39 .1742 113 145 156.9 152 1043 1273 8 1.0340 40 .1790 114 158 172 153 1079 9 1.0382 41 .1841 115 172 188 154 1116 1383 10 1.0425 42 .1892 116 187 204.4 155 1155 11 1.0468 43 .1942 117 202 221.4 156 1196 1504" 12 1.0512 44 .1994 118 217 238 4 157 1238 13 1.0555 45 .2045 119 232 256.8 158 1281 1637 14 1.0599 46 .2096 120 248 275.3 159 1325 15 1.0642 47 .2147 121 265 160 1370 1775 16 1.0686 48 .2198 122 283 3l4 161 1417 17 1.0729 49 .2249 123 301 162 1464 1923' 18 1.0773 50 .2300 124 319 354 163 1511 19 1.0816 51 .2353 125 337 164 1558 2084' 20 1.0860 52 .2407 126 356 396 165 1606 21 1.0905 53 .2460 127 376 166 1653 22 .0950 54 .2514 128 396 440.2 167 1700 23 .0995 55 1.2567 129 417 168 1748 24 .1040 56 1.2621 130 439 487.4 169 1796 25 .1085 57 1.2674 131 461 170 1844 26 .1130 58 .2728 132 484 537.3 180 2400 oo 27 .1175 59 .2781 133 507 190 3112 28 1 . 1220 60 .2835 134 530 590 200 4099 29 1.1265 61 .2888 135 554 210 5618 30 1.1310 62 .2942 136 578 645 220 8547 31 1.1358 63 .3005 137 603 230 16950 32 1.1406 64 .3059 138 629 ere 705.5 240 00 ... (Gerlach, Z. anal. 27. 310.) 139 DOO * * * " * 548 NITRATE, AMMONIUM Ch Very sol. in HNO 3 +Aq. (Schulz, Zeit. . 1869. 531.) Solubility of NH 4 NO 3 in HNO 3 . Solution temp. % by wt. NH 4 N0 3 Solid phase +8 21.1 NH 4 NO 3 , 2HNO 3 (solu- tion in HNO 3 ) 23.0 28.7 tt 28.5 34.5 11 29.5* 38.8 (solution in NH 4 NO 3 ) 27.5 44.6 u 27.0 45.8 t( 23.5 49.4 (( 23.0 50.0 u 17.5 54.0 (( 16.5 54.3 (I 4.0 45.8 NH 4 NO 3 , HNO 3 labile (solution in HNO 3 ) 9.5 49.4 (i 11.0 51.7 u 11.5 52.7 u 12.0 54.3 u 12.0 54.7 (I 11.5 57.6 (solution in NH 4 NO 3 ) 11.5 54.0 NH 4 N0 3 (labile) 14.5 54.3 a 17.0 54.7 stable 26.0 55.9 n 27.0 56.2 (( 33.5 57.5 It 49.0 60.4 u 79.0 68.1 fl * Mpt. of NH 4 NO 3 , 2HNO 3 . (Groschuff. Z. anorg. 1904, 40. 6.) Solubility of NH 4 NO 3 in NH 4 OH+Aq. Grams of NH 4 N0 3 Grams of NH 3 Molecules ofNBUNOs in 100 molecules NH 4 N0 3 + NH 3 Temperature at which the solu- tions are in equilibrium with the solid phase 100. about 168 6^7578 61 0588 74.2 109.8 0.6439 0.0665 67.3 94.0 4.2615 0.7747 53.8 68.8 0.7746 0.1857 47.0 35.9 0.9358 0.2352 45.9 33.3 0.7600 0.2607 38.3 0.9675 0.3515 36.9 10.5 0.8308 0.3700 32.3 -30.0 0.9526 1.2457 13.9 -44.5 1.3918 4.4327 6.25 60 100 about 80 (Kuriloff, Z. phys. Ch. 1898, 26. 109.) NH 4 NO 3 +NH 4 C1. 100 pts. H 2 O dissolve 29.1 pts. NH 4 C1 and 173.8 pts. NH 4 NO 3 . (Rudorff, B. 6. 484.) Sol. in sat. NH 4 Cl+Aq with pptn. of NH 2NH 4 N0 3 30.87 20.43 (NH 4 ) 2 SO 4 , 2NH 4 NO 3 +(NH 4 ) 2 SO 4 , 15 83.9 24.03 81.21 42.81 79.34 64.6 78.06 1.375 1.386 1.392 1.401 31.61 45.99 49.12 19.50 9.53 6.00 3NH 4 N0 3 (NH 4 ) 2 SO 4 , 3NH 4 NO 3 (NH 4 ) 2 SO 4 , 3NH 4 NO 3 +NH 4 NO NH 4 NO 3 110.9 75.81 1.417 54.19 152. 75.35 1.428 155.3 75.38 1.429 Temp. =70 156.1 60.76 1.405 159 36.50 1.364 . d d 160 27.79 1.350 KO^S Solid phas6 162.3 17.63 1.330 H M 167.4 1.298 * g 30 96.12 1.401 47.81 (NH 4 ) 2 SO 4 220.8 88.31 1.450 11.10 40.81 14 232.6 1.329 70.15 6.71 (NH 4 ) 2 SO 4 + (NH 4 )SO 4 , 2NH 4 NO 3 71 .58 5.82 (NH 4 ) 2 SO 4 , 2NH 4 NO 3 (Fedotieff and Koltunoff, Z. anorg. 1914, 85. 73.48 5^14 (NH 4 ) 2 S0 4 , 2NH 4 NOs+(NH 4 ) 2 SO 4 , 251.) 3NH 4 NOs 76.01 3.96 (NH 4 ) 2 S0 4 , 3NH 4 NO 3 80.25 2.68 " 81.01 2.45 (NH 4 ) 2 SO 4 , 3NH 4 N0 3 +NH 4 N0 3 81.38 2.41 NH 4 N0 3 84.03 it (de Waal. Dissert. Leiden. 1910.) 550 NITRATE, AMMONIUM HYDROGEN Very easily sol. in liquid NH< Am. Ch. J. 1898, 20. 826.) (Franklin, 1 pt. NH 4 NO 3 dissolves in 2.29 pts. alcohol of 66.8% at 25. (Pohl, W. A. B. 6. 599.) 1 pt. NH 4 NO 3 dissolves in 1.1 pt. boiling alcohol. 100 pts. absolute methyl alcohol dissolve 17.1 pts. at 20.5. (de Bruyn, Z. phys. Ch. 10. 783.) 100 g. absolute methyl alcohol dissolve 14.6 g. NH 4 NO 3 at 14 and 16.3 g. at 18.5. (Schiff and Monsacchi, Z. phys. Ch. 1896, 21. 277.) 100 pts. absolute ethyl alcohol dissolve 3.8 pts. at 20.5: (de Bruyn, Z. phys. Ch. 10. 783.) 100 g. absolute ethyl alcohol dissolve 4.6 g. at 14. (Schiff and Monsacchi, Z. phys. Ch. 1896, 21. 277.) Solubility of NH 4 NO 3 in H 2 O is decreased by presence of ethyl alcohol but increased by presence of methyl alcohol. NH 4 NO 3 is only very si. sol. in abs. ethyl alcohol and the sol- ubility increases slowly with rise in temp.; it is more sol. in abs. methyl alcohol and the solubility increases rapidly with rise in temp. (Fleckenstein, Phys. Zeit. 1905, 6. 419.) Solubility in methyl alcohol +Aq. at 30. % by wt. H 2 O % by wt. alcohol % by wt. NH 4 NO 3 29.9 21.6 20.6 16.5 11.5 24.5 31.3 46.0 59.4 83.3 70.1 53.9 48.1 37.5 29.1 16.7 (Schreinemakers, Z. phys. Ch. 1909, 65. 556.) Solubility of NH 4 NO 3 in ethyl alcohol +Aq. at 30. Composition of sat. solution. % by wt. H 2 O % by wt. alcohol %bywt.NH 4 NO 3 29.9 70.1 26.9 18.6 54.5 23.2 39.3 37.5 18.3 58.5 23.2 11.6 76.5 11.9 5.8 86.2 8.0 96.4 3.6 (Schreinemakers, Z. 555.) Ch. 1909. 66. Solubility of NH 4 NO 3 in alcohol. t % NH 4 N0 3 % Alcohol % H 2 54.19 45.81 42.69 12.70 44.61 1.96 97.93 0.11 O 22.6 2(NH 4 ) 2 W 4 13 +4H 2 0. 16 8^3 68 22.9 Decomposes by recrystallising out of H 2 O. 17 8.5 69 23.3 (Marignac, A. ch. (3) 69. 61.) 18 8.8 70 23.6 19 9.0 71 23.9 Antimony nitrate, Sb 4 O 6 , N 2 O 5 . 21 9.2 9.5 72 73 24 3 24.9 Decomp. by cold H 2 O. (Bucholz.) 22 9.7 74 25.0 Aqueous solution sat. at 10 contains 30.4% 23 9.9 75 25.4 salt. (Eller.) 24 10.1 76 25.7 Sol. in strong, less sol. in dil. HNO 3 +Aq. 25 10.4 77 26.0 (Peligot, A. ch. (3) 20. 288.) 26 10.6 78 26.4 Insol. in acetone. (Naumann, B. 1904, 37. 27 10.8 79 26.7 4329.) 28 11.1 80 27.0 29 11.3 81 27.4 OA HA 82 27 7 Barium nitrate, Ba(NO 3 ) 2 . 31 . u 11.8 OH 83 I0f 4 28.1 Sol. in H 2 O with absorption of heat. 32 12.1 84 28.4 100 pts. H 2 O at dissolve 5.0 parts 33 12.3 85 28.8 Ba(NO 3 ) 2 . (Gay-Lussac, A. ch. 11. 313.) 34 12.6 86 29.1 100 pts. H 2 O at dissolve 5.2 parts 35 12.8 87 29.5 Ba(NO 3 ) 2 . (Mulder.) 36 13.1 88 29.8 Ba(NO 3 ) 2 +Aq sat. at 20 contains 8.57 pts. 37 13.4 89 30.2 Ba(NO 3 ) 2 to 100 pts. H 2 O, and has 1.0679 sp. 38 13.7 90 30.6 gr. (Karsten); sat. at 20 has 1.064 sp. gr., 39 14.0 91 30.9 and contains 7.94 pts. Ba(NO 3 ) 2 to 100 pts. 40 14.2 92 31.3 H 2 O. (Michel and Krafft.) 41 14.5 93 31.7 42 14.8 94 32.0 100 pts. H 2 O dissolve pts. Ba(NO 3 ) 2 at t. 43 44 15.1 15.4 95 96 32.4 32.7 Pts o PtS. 45 15.6 97 33.1 Ba(N0 3 ) 2 Ba(N0 3 ) 2 46 15.9 98 33.5 47 1ft 9 QQ qq o 5.00 52.11 17.97 rt/ 48 1O . ~i 16.5 yy 100 oo . o 34.2 14.95 8.18 73.75 25.01 49 16.8 101 34.5 17.62 8.54 86.21 29.57 50 17.1 101.9 34.8 37.87 13.67 101.65 35.18 51 17.4 40 29 17 07 T^t/.X'jj JL 1 . V/l ... ... (Moulder calculated from his own and other (Gay-Lussac, A. ch. (2) 11. 313.) experiments, Scheik. Verhandel. 1864. 50.) NITRATE, BARIUM 553 Sat. Ba(NO 3 ) 2 +Aq contains % Ba(NO 3 ) at t. 0.4 2.1 6.0 6.5 11.0 15.3 18.0 28.5 45.5 52.0 Ba(NO.) 2 4.3 4.9 5.6 5.6 6.4 7.1 7.7 9.7 12.8 14.9 60.0 73.0 92.0 110.0 132.0 134.0 150.0 152.0 171.0 215.0 % Ba(i\0 8 ). 16.1 19.4 23.4 27.4 31.8 32.5 34.9 35.4 38.3 45.8 (Etard, A. ch. 1894, (7) 2. 528.) 100 g. H 2 O dissolve 8.54 g. Ba(NO 3 ) 2 at 17. (Gmelin-Kraut, Handbuch der anorg. Chemie.) 100 g. H 2 O dissolve 7.87 g. Ba(N0 3 ) 2 at 15; 8.32 g. at 17. (Euler, Z. phys. Ch. 1904, 49. 315.) 1000 g. H 2 O dissolve 0.72 gram-equivalents Ba(NO 3 ) 2 at 21.5. (Euler, Z. phys. Ch 1904, 49. 312.) 10.30 g. anhydrous Ba(NO,) 2 are sol. in 100 g. H 2 O at 25. (Parsons and Colson, J. Am. Chem. Soc. 1910, 32. 1385.) 4.74 g. Ba(NO 3 ) 2 are contained in 100 g. Ba(NOj) 2 sat. at 0. (Coppadoro, Gazz. ch. it. 1911, 42, I. 233.) Solubility of Ba(NO 3 )-> in H 2 O =0.427 mol. 1. at 30. (Masson, Chem. Soc. 1911, 99. 1136.) Solubility of Ba(NO 3 ) 2 in H 2 O at 30 = 10.33%. (Coppadoro, Gazz. ch. it. 1913, 43. I. 240.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 9.1 21.1 35 6.25 8.46 11.39 g. Ba(NO 3 ) 2 . (Findlay, Chem. Soc. 1914, 105. 780.) Sp. gr. of Ba(NO 3 ) 2 +Aq at 19.5. Sp.gr. of Ba(NO 3 ) 2 +Aq at 17.5. m Ba(NO 8 ) 2 Sp. gr. Ba(tfOi) Sp. gr. 1 2 3 4 5 1.0085 1.0170 1.0255 1.0340 1.0425 6 7 8 Sat. sol. 1.0510 1.0600 1.0690 1.0690 (Gerlach, Z. anal. 27. 283.) Sp. gr. of Ba(NO 3 ) 2 -fAq at room temp. % Ba(NOr)i 5.25 2.98 Sp. gr. 1.0507 1.0274 (Wagner, W. Ann. 1883, 18. 264.) Sp. gr. of Ba(NO,) 2 +Aq at 25. Concentration of Ba(NOs) 2 +Aq. V 2 normal Sp. gr. 1.0518 1.0259 1 . 0130 (Wagner, Z. phys. Ch. 1890, 6. 35.) Ba(NO 3 ) 2 +Aq containing 6.08% Ba(NO 3 ) 2 has sp. gr. 20 /20 = 1.0517. Ba(NO 3 ) 2 + Aq containing 6.97% Ba(NO 3 ) 2 has sp. gr. 20/20 = 1 .0597. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 279.) Sp. gr. of Ba(NO 3 ) 2 +Aq at 20 containing M g. mols. salt per liter. M Sp. gr. 0.01 1.002031 0.025 1.005224 0.05 1.010591 M 0.075 0.10 0.15 Sp. gr. 1.015671 1.021143 1.031770 (Jones and Pearce, Am. Ch. J. 1907, 38. 708.) Ba(jfo 3 ) 2 Sp. gr. Ba(N0 3 ) 2 Sp. gr. Sp. gr. ot sat. i*a(W0 3 ) 2 +Aq at t. t g. Ba(NOi)isol. in 100 g. H 2 O Sp. gr. 1 2 3 4 5 .009 .017 .025 .034 .042 6 7 8 9 10 1.050 1.060 1.069 1.078 1.087 10 20 30 40 50 60 70 5.2 7.0 9.2 11.6 14.2 17.1 20.3 23.6 1.043 1.056 .073 .087 .104 .121 .137 .146 (Calculated by Gerlach, Z. anal. 8. 286, from Kremers, Pogg. 95. 110.) Sp. gr. of Ba(NO 3 ) 2 +Aq at 18. % B a (N0 3 ) 2 Sp. gr. Tschernaj, J. Russ. Phys. Chem. Soc. 1912, 44. 1565.) Saturated BaNO 3 +Aq contains: 36.18 pts. Ba(NO 3 ) 2 to 100 pts. H 2 O, and boils at 101.1. (Griffiths.) 4.2 8.4 1.0340 1.0712 (Kohlrausch, W. Ann. 1879. 1.) 554 NITRATE, BARIUM 35.2 pts. Ba(NO 3 ) 2 to 100 pts. H 2 O, and boils at 101.65. (Gay-Lussac.) 34.8 pts. Ba(NO 3 ) 2 to 100 pts. H 2 O, and boils at 101.9. (Mulder.) 34.8 pts. Ba(NO 3 ) 2 to 100 pts. H 2 O, and boils at 102.5. (Kremers.) Sat. Ba(NO 3 ) 2 +Aq forms a crust at 101.1; highest temp, observed was 101.5. (Gerlach, Z. anal. 26. 427.) B. pt. of Ba(NO 3 ) 2 +Aq containing pts. Ba(NO 3 ) 2 to 100 pts. H 2 O. B.-pt. Pts. Ba(NO 3 ) 2 100.5 101.0 101 . 1 12.5 26.0 27.5 (Gerlach, Z. anal. 26. 440.) Insol. in cone. HNO 3 +Aq, and much less sol. in dil. HNO 3 +Aq or HCl+Aq than in H 2 O. 13.67 pts. NH 4 Cl+Aq (1 pt. NH 4 C1+10 pts. H 2 O) at ord. temp., and 4.67 pts. at 100. 24.00 pts. NH 4 NO 3 +Aq (1 pt. NH 4 NO 3 + 10 pts. H 2 O) at ord. temp. 17.33 pts. Nri 4 C 2 H 3 O 2 +Aq (dil. NH 4 OH neutralised by dil. HC 2 H 3 O 2 ) at ord. temp., and 4.33 pts. at 100. 14.67 pts. NaC 2 H 3 O 2 +Aq (dil. HC 2 H 3 O 2 neutralised by Na 2 CO 3 and dil, with 4 vols. H 2 O) at ord. temp., and 5.33 pts. at 100. 17.33 pts. Cu(C 2 H 3 O 2 ) 2 +Aq (see Stolba, Z. anal. 2. 390) at ord. temp., and 6.00 pts. at 100. 18.67 pts. grape sugar (1 pt. grape sugar +10 pts. H 2 0) at ord. temp. (Pearson, Zeit. Ch. 1869. 662.) Sol. in sat. NH 4 Cl+Aq without pptn. at first, but finally NH 4 C1 is pptd. until a cer- tain state of equilibrium is reached. (Kar- sten.) Solubility in BaO 2 H 2 , 8H 2 O+Aq at 25. Solubility of Ba(NO 3 ) 2 in HNO 3 +Aq at 30. Sp. gr. 25/25 G. BaO as Ba(OH) 2 in 1 f\f\ re XT (~\ G. Ba(N0 3 ) 2 in 100 g. H 2 Solid phase Ba(NO 3 ) 2 1UU g. 1 2 U i 07Q7 o 10 "30 G. mol. per 1. X . \J t t7 1 1 . 1002 \J 1.55 JL\J . OLF 10.66 Sp. gr. of sat. 1.1210 3.22 11.04 HNOs Ba(NO 3 ) 2 *1 . 1448 5.02 11.48 1.0891 1.0811 l!o663 0.0000 0.1318 0.2496 0.4995 0.4270 0.3282 0.3268 0.2410 * This solution is sat. with respect to both Ba(OH) 2 , 8H 2 O and Ba(NO 3 ) 2 . (Parsons. J. Am. Chem. Soc. 1910, 32. 1385.) 1.0619 0.7494 0.1785 See also under BaO 2 H 2 . .0609 1.000 0.1353 .0633 .0668 1.247 1.493 0.1056 0.0847 Solubility in BaCl 2 +Aq at t. .0783 1.998 0.0598 Sat. solution contains .1050 2.993 0334 t 1.1341 3.986 0.0218 % BaCl 2 % Ba(N0 3 ) 2 1.1341 3.994 0.0223 1.1645 5.012 0.0147 n J 21.4 00 A 4.0 4- (Masson, Chem. Soc. 1911, 99. 1136.) +1.5 d . \J 22.6 TT . \J 4.4 2 5.0 Less sol. in dil. HC 2 H 3 O 2 +Aq than in dil. HCl+Aq. 10 21 24^7 24.5 6.1 5.6 Solubility in NH 4 Cl+Aq is the same as in 32 26.6 7.7 H 2 O. 35 26.4 7.7 Less sol. in NH 4 OH+Aq, NH 4 C 2 H 3 O 2 + Aq, or NH 4 NO 3 + Aq than in H 2 O. (Pearson, Zeit. Ch. (2) 6. 662.) 38 48 53 26.7 28.1 28.5 7.8 8.0 9.0 Ba(NO 3 ) 2 is sol. in about: 53 28.3 9.2 13.33 pts. H 2 O at ord. temp., and 4.67 pts. 66 28.0 10.0 at 100. 73 30.0 10.5 14.67 pts. NH 4 OH+Aq (cone.) at ord. 79 30.3 11.2 temp., and 5.67 pts. at 100. 90 32.1 12.5 16.50 pts. NH 4 OH+Aq (1 vol. cone. +3 155 32.5 23.1 vols. H 2 O) at ord. temp. 162 33.1 23.4 28.00 pts. HCl+Aq (1 vol. cone. HC1+4 210 32.5 31.9 vols. H 2 O) at ord. temp. 29.00 pts. HC 2 H 3 O 2 +Aq (1 vol. commer- cial HC 2 H 3 O 2 + 1 vol. H 2 O) at ord. temp. (fitard, A. ch. 1894, (7) 3. 287.) See also under BaCl 2 . NITRATE, BARIUM 555 Ba(N0 3 ) 2 +Pb(NO 3 ) 2 . Very si. sol. in sat. Pb(NO 3 ) 2 +Aq. (Kar- sten.) 100 pts. sat. Ba(NO 3 ) 2 +Pb(NO 3 ) 2 +Aq contain 33.95 pts. of the two salts at 19-20. (v. Hauer, J. pr. 98. 137.) Solubility of Ba(N0 3 ) 2 +Pb(N0 3 ) 2 at 25. J 01^ G. ] Der 1. Sp. gr. 100 pt 3. Of SOlu- Ba(N0 3 ) 2 Pb(NO)i tion contain Solid phase 102.2 .079 pts. KNOs pts. Ba(NOs) 2 54 9 17 63 088 86.5 49.80 .108 15.24 6.64 Ba(NO 3 ) 2 +2KNO 3 , Ba(NO 3 ) 2 79.7 68.10 .119 14.69 6.60 it 77.0 97.20 .140 14.79 6.62 tt 69.8 66.0 130.7 177.3 .163 .198 16.30 21.99 5.49 3.04 2KN0 3 , Ba(N0 3 ) 2 tt 57.5 25.9 247.7 334.3 .252 .294 27.66 27.81 2.01 2.09 KNO 3 +2KNO 3 , Ba(NO 3 ) 2 a 28.8 429.7 .376 27.94 1.92 (f 553.8 1.459 27.64 2.05 (t (Fock, Z. Kryst. Min. 1897, 28. 365, 397.) 100 ccm. Ba(N0 3 ) 2 +Pb(NO 3 ) 2 +Aq sat. at 17 contain 3.22 g. Ba(NO 3 ) 2 and 38.59 g. Pb(N0 3 ) 2 and solution has sp. gr. = 1.350. (Euler, Z. phys. Ch. 1904, 46. 313.) 100 pts. sat, Ba(NO 3 ) 2 +Pb(NO 3 ) 2 + Sr(NO 3 ) 2 +Aq contain 45.90 pts. of the three salts at 19-20. (v. Hauer, 1. c.) Ba(N0 3 ) 2 +Sr(N0 3 ) 2 . 100 pts. sat. Ba(NO 3 ) 2 +Sr(NO 3 ) 2 +Aq con- tain 45.96 pts. of the two salts at 19-20. (v. Hauer, I. c.) Ba(N0 3 ) 2 +KNO 3 . 100 pts. H 2 O dissolve: (Mulder) (1) KNO 3 . Ba(N0 3 ) 2 . . 29.7 28.8 5.4 8^9 34.2 (Karsten) (Kopp) (4) ' (5) (2) (3) KNO 3 Ba(N0 3 ) 2 . 13.31 6.91 29.03 1.00 5.7 33.1 3.5 36.3 20.22 30.03 38.8 39.8 1. Sat. Ba(NO 3 ) 2 +Aq sat. with KNO 3 at 18.5. 2. To sat. KNO 3 +Aq, Ba(NO 3 ) 2 +Aq was added. 3. To sat. Ba(NO 3 ) 2 +Aq, KNO 3 was added. 4. Both salts in excess +Aq at 21.5. 5. Both salts in excess -f-Aq at 23. 1 1. of the solution contains 59.1 g. Ba(NO 3 ) 2 +124.2 g. KNO 3 = 183.35 g. mixed salts at 17. Sp. gr. Ba(NO 3 ) 2 +KNO 3 +Aq = 1.120. 1 1. of the solution contains 88.7 g. Ba(NO 3 ) 2 +213.6 g. KNO 3 = 302.3 g. mixed salts at 30. Sp. gr. Ba(NO 3 ) 2 +KNO 3 +Aq = 1.191. (Euler, Z. phvs. Ch. 1904, 49. 313.) These results show that a double salt of potassium and barium nitrates is formed at 25. (Foote, Am. Ch. J. 1904, 32. 252.) Solubility of Ba(NO 3 ) 2 +KNO 3 at t. t Ba(NOs)2 % KNOs Solid phase 9.1 6.25 Ba(N0 3 ) 2 4.20 8.15 Ba(NO 3 ) 2 +2KNO 3 , Ba(N0 3 ) 2 1.98 0.98 12.02 16.80 2KNO 3 , Ba(NO 3 ) 2 2KN0 3 , Ba(N0 3 ) 2 + KNO 3 16.76 KNO 3 21.1 8.46 Ba(N0 3 ) 2 7.47 2.12 " 6.35 5.98 " 6.06 8.47 Cl 5.98 13.24 Ba(NO 3 ) 2 +2KNO 3 , Ba(N0 3 ) 2 3.35 18.24 2KNO 3 , Ba(NO 3 ) 2 2.30 21.47 tt 1.76 24.86 2KN0 3 , Ba(N0 3 ) 2 + KNO 3 24.77 KNO 3 35 11.39 Ba(N0 3 ) 2 8.18 12.99 " 8.08 17.48 H 8.42 19.75 Ba(NO 3 ) 2 +2KNO 3 , Ba(NO 3 ) 2 5.85 24. 2KN0 3 , Ba(N0 3 ) 2 5.02 26.05 1C 3.02 34.87 2KNO 3 , Ba(NO 3 ) 2 + KNO 3 1.77 34.98 KNO 3 35.01 it (Findlay, Chem. Soc. 1914, 105. 779.) 556 NITRATE, BARIUM Ba(NO.)H-NaNO. Ba(NO 3 ) ? is sol. in sat. NaNO 3 +Aq with- out separation. 100 pts. H 2 O dissolve: NaNO 3 Ba(NO,), . . . (Karsten) At 18.75 86.6 88.14 3.77 8^9 NaNO, Ba(N0 3 ) 2 . . . (Kopp) At 20.2 87.7 88.6 3.6 M Solubility of Ba(NO 3 ) 2 +NaNO 3 in H 2 O at 0. % NaNOs % Ba(NOs)* Solid phase 4.74 Ba(N0 3 ) 2 0.41 4.33 0.61 4.03 K 1.68 3.34 <( 3.54 2.50 (( 8.05 1.60 t( 12.71 1.56 u 20.24 1.53 u 2CK92 1.43 u 27.74 1.56 a 30.81 1.55 a 33.79 1.53 it 35.83 1.49 it 41.30 1.55 Ba(NO 3 ) 2 +NaNO 3 41.68 0.51 NaNO 3 42.47 u (Coppadoro, Gazz. ch. it, 1912, 42 (1) 233.) Solubility of Ba(NO 3 ) 2 +NaNO 3 in H 2 O at 30. % NaNOs Ba(NOs)2 Solid phase 10.33 Ba(N0 3 ) 2 2.33 8.58 7.09 5.28 12.07 3.89 14.41 3.54 17.87 3.20 19.06 3.07 23.55 2.81 41.22 2.27 48.22 2.11 Ba(NO 3 ) 2 +NaNO 3 48.50 1.00 NaNO 3 49.16 it (Coppadoro, Gazz. ch. it. 1013, 43, I. 240.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) 100 pts. hydrazine dissolves 81.1 pts. Ba(NO 3 ) 2 at 12.5-13. (de Bruyn, R. t. c. 1899, 18. 297.) 100 pts. anhydrous hydroxylamine dissolve 11.4 pts. Ba(NO 3 ) 2 . (de Bruyn, R. t. c. 1892, 11. 18.) Insol. in absolute alcohol. Solubility in dilute alcohol increases with the temp. (Gerardin, A. ch. (4) 5. 145.) Solubility in ethyl alcohol +Aq at 25. % C2H 5 OH in the solvent % C 2 H 5 OH in the solution % Ba(N0 3 ) 2 in the solution 9.55 10.25 9.5 7.63 18.60 17.5 6.02 25.05 23.7 5.25 40.20 38.8 3.53 58.00 57.0 1.85 78.70 78.2 0.62 90.10 89.9 0.18 99.40 99.39 0.005 (D'Ans and Siegler, Z. phys. Ch. 1913, 82. 37.) Completely insol. in boiling amyl alcohol. (Browning, Sill. Am. J. 143. 314.) Solubility in organic solvents. Solvent Methyl alcohol Ethyl alcohol Acetone Ether Paracetaldehyde % Ba(NO 3 )2in the solution at 25 0.50 0.005 0.005 very small (D'Ans and Siegler, Z. phys. Ch. 1913, 82. 44.) Solubility in phenol +Aq at 25. Concentration of the phenol Mol./ Liter 0.000 0.045 0.082 0.146 0.310 0.401 0.501 0.728 (sat.) Solubility of Ba(NOs) 2 Mol./Liter 0.3835 0.3785 0.3746 0.3664 0.3492 0.3400 0.3299 0.3098 (Rothmund and Wilsmore, Z. phys. Ch. 1902, 40. 620.5 Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3602.) Insol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) NITRATE, BISMUTH MANGANOUS 557 Barium mercurous nitrate, 2BaO, 2Hg 2 O, 3N 2 O 5 . Decomp. by H 2 O. Sol. in hot dil. HNO 3 + Aq and hot Hg 2 (NO 3 ) 2 +Aq, from which it crystallises on cooling. (Stadeler, A. 87. 129.) Barium potassium nitrate, Ba(NO 3 ) 2 , 2KNO 3 . Ppt. (Wallbridge, Am. Ch. J. 1903, 30. 154.) Solubility determinations show that the only double salt formed by barium and potassium nitrates at 25 is Ba(NO 3 ) 2 , 2KNO 3 . See Ba(NO 3 ) 2 +KN0 3 under Ba(NO 3 ) 2 . (Foote, Am. Ch. J. 1904, 32. 252.) Barium nitrate raetatungstate, 2Ba(NO 3 ) 2 . BaW 4 13 +6H 2 0. Efflorescent. Sol. in warm H 2 O. (Pe"ch- ard, A. ch. (6) 22. 198.) Bismuth nitrate, basic, Bi 2 O 3 , N 2 O 5 +2H 2 O. Sol. in a large amount of H 2 O. Sol. in HNO 3 +Aq. (Heintz.) Sol. in 135 pts. H 2 O at 90-93. (Ruge, J. B. 1862. 163.) + ^H 2 O. Sol. in much H 2 O. (Yvon, C.R. 84. 1161.) +H 2 O. (Ruge.) 2Bi 2 O 3 , N 2 O 6 . Not acted upon by H 2 O. (Ditte, C. R. 84. 1317.) +H 2 O. (Yvon.) Bi 2 O 3 , 2N 2 O 5 +H 2 O. (Ruge.) HBi 2 O 3 , 5N 2 O 5 +16H 2 O. Not decomp. by H 2 O. (Yvon.) 5Bi 2 O 3 , 4N 2 O 5 +8H 2 O. Ppt. Not attacked by H 2 O. (Schulten, Bull. Soc. 1903, (3) 29. 722.) 5Bi 2 O 3 , 5N 2 O 5 +9H 2 O. Sol. in H 2 O with decomp. (Schulten.) 6Bi 2 O 3 , 5N 2 O 5 +8H 2 O, and +9H 2 O. (Rut- ten, Z. anorg. 1902, 30. 368.) At 25 the salt Bi 12 O 13 (NO 3 )io, 9H 2 O is in equilibrium with HNO 3 +Aq from 0.03- 0.32-N; the salt BiO(NO 3 ), H 2 O is in equi- librium with HNO 3 +Aq from 0.425-0.72-N. At 50 the salt Bi 4 O 6 (NO 3 ) 2 , H 2 O is in equilibrium with HNO 3 +Aq from 0.057- 0.285-N; the salt Bi 12 Oi 3 (NO 3 )io, 9H 2 O is in equilibrium with HNO 3 +Aq from 0.285- 0.446-N. At 75 the salt Bi 4 O 6 (NO 3 ) 2 , H 2 O is in equilibrium .with HNO 3 +Aq from 0.109- 0.314-N. (Allan, Am. Ch. J. 1901, 25. 314.) Bismuth nitrate, Bi(NO 3 ) 3 . Permanent. Decomp. by little H 2 O with separation of a basic salt: This decomposition is prevented by slight excess of HNO 3 , and then the salt is completely sol. in a large amount of H 2 O. (Rose.) Sol. in dil. HNO 3 +Aq. Not decomp. by H 2 O in presence of HC 2 H 3 O 2 or ^fa pt. NH 4 NO 3 . (Lowe, J. pr. 74. 341.) Completely sol. in HNO 3 +Aq containing 83 g. HNO 3 per liter. (Ditte.) Solubility of Bi(NO 3 ) 3 in 2.3N-HNO 3 +Aq. = 2.04 g. at Bi per 1.; in 0.922N-HNO 3 +Aq. = 2.23 g. at Bi per 1. (Dubrisay, C. R. 1911. 153. 1077.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Krug and M'Elroy.) Solubility of Bi(NO 3 ) 3 in 6.67% acetone+ 2.3N-HNO 3 +Aq = 1.89 g. at Bi per 1.; in 6.67% acetone +0.922N-HNO 3 +Aq. =2.17 g. at Bi per 1.; in 13.33% acetone +0.922N- HNO 3 +Aq =2.08 g. at Bi per 1. (Dubrisay, C. R. 1911, 153. 1077.) When Bi(NO 3 ) 3 -is mixed with mannite (dulcite, sorbite) in proportion to the mol. wts. and H 2 O is added, a clear solution is ob- tained which is not pptd. by addition of much H 2 O. These solutions are more stable the greater the proportion of mannitol. (Vanino and Hunser, Z. anorg. 1901, 28. 211.) + 1^H 2 O. (Ditte.) +5H 2 O. If treated with increasing amts. of H 2 O, the amt. of Bi which dissolves de- creases, and when 1 pt. is treated with 50,000 pts. H 2 O, no Bi goes into solution. (Antony and Gigli, Gazz. ch. it. 1898, 28. 245.) 48.66 pts. are sol. in 100 pts. acetone at 0. 41.70 " " " " 100 " " " 19. (Laszczynski, B. 1894, 27. 2287.) +5^H 2 O. (Yvon, C. R. 84. 1161.) + 10H 2 O. Melts in crystal H 2 O with de- comp. at 74. (Ordway.) Bismuth caesium nitrate, Bi(NO 3 ) 3 , 2CsNO 3 . Ppt. (Wells, Am. Ch. J. 1901, 26. 277.) Bismuth cobalt nitrate, 2Bi(NO 3 ) 3 , 3Co(N0 3 ) 2 +24H 2 O. 100 cc. sat. solution in HNO 3 +Aq (sp. 'gr. 1.325) contain 54.67 g. hydrated salt. (Jantsch Z. anorg. 1912, 76. 321.) Bismuth magnesium nitrate, 2Bi(NO 3 ) 3 , 3Mg(NO 3 ) 2 +24H 2 O. Deliquescent. Effloresces in dry air. Decomp. by H 2 O. (Urbain and Lacombe, C. R. 1903, 137. 569.) 100 cc. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contain 41.69 g. hydrated salt. (Jantsch Z. anorg. 1912, 76. 321.) Bismuth manganous nitrate, 2Bi(NO 3 ) 3 , 3Mn(NO 3 ) 2 +24H 2 O. Deliquescent. Effloresces in dry air. Decomp. by H 2 O. (Urbain and Lacombe. C. R. 1903, 137. 569.) 100 cc. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contain 65.77 g. hydrated salt. (Jantsch Z. anorg. 1912, 76. 321.) 558 NITRATE, BISMUTH NICKEL Bismuth nickel nitrate, 2Bi(NO 3 ) 3 , 3Ni(NO 3 ) 2 +24H 2 O. Deliquescent. Effloresces in dry air. Decomp. by H 2 O. (Urbain and Lacombe, C. R. 1903, 37. 569.) 100 cc. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contain 46.20 g. hydrated salt at 16. (Jantsch.) Bismuth zinc nitrate, 2Bi(NO 3 ) 3 , 3Zn(NO 3 ) 2 + 24H 2 O. Deliquescent. Decomp. by H 2 O. (Ur- bain and Lacombe, C. R. 1903, 137. 569.) 100 cc. sat. solution in JENO 3 +Aq (sp. gr. 1.325) contain 57.51 g. hydrated salt at 16. (Jantsch.) Cadmium nitrate, basic, Cd(OH)NO 3 +H 2 O. Decomp. by H 2 O, or ordinary alcohol. (Klinger,B. 16.997.) 12CdO, N 2 5 +11H 2 0. SI. sol. in H 2 O; more sol. in H 2 O than basic sulphate. (Haber- mann, 5. 432.) 5 CdO, 2N 2 O 6 -f8H 2 O. Decomp. by cold H 2 O. (Rousseau and Tite, C. R. 114. 1184.) Cadmium nitrate, Cd(N0 3 ) 2 . Deliquescent, and very sol. in H 2 O. See +4, and 9H 2 O. Sp. gr. of aqueous solution containing: 5 10 15 20 25%Cd(NO 3 ) 2 , 1.0528 1.0978 1.1516 1.2134 1.2842 30 35 40 45 50%Cd(NO 3 ) 2 . 1.3566 1.4372 1.5372 1.6474 1.7608 (Franz, J. pr. (2) 5. 274.) Sp. gr. of Cd(NO 3 ) 2 +Aq at 18. %Cd(NO 3 ) 2 1 5 10 15 Sp.gr. 1.0069 1.0415 1.0869 1.136 Cd(NO 3 ) 2 20 25 30 35 . gr. 1.1903 1.25 1.3125 1.3802 Cd(NO 3 ) 2 40 45 48 p. gr. 1.459 1.543 1.5978 (Grotrian, W. Ann. 1883, 18. 193.) Sp.gr. of Cd(NO 3 ) 2 +Aq at room temp, containing: 7.81 15.71 22.36% Cd(NO 3 ) 2 . 1.0744 1.1593 1.2411 (Wagner, W. Ann. 1883, 18. 265.) Sp.gr. of Cd(N0 3 ) 2 +Aq. % Cd(NO3) 2 "t Sp. gr. at t Sp. gr. at 18 0.0492 17.57 0.99912 0.99904 21.14 0.99839 0.100 18.00 0.99945 0.249 17.34 1.0008 1.0007 20.22 1.0002 0.464 18.00 1.0025 0.952 18.00 1.0065 (Wershofen, Z. phys. Ch. 1890, 5. 493.) Sp. gr. of Cd(NO 3 ) 2 +Aq at 25. Concentration of Cd(NOs)2+Aq. 1-normal Vr- " Sp. gr. 1.0954 1.0479 1.0249 1.0119 (Wagner, Z. phys. Ch. 1890, 6. 36.) Sp. gr. of Cd(NO 3 ) 2 +Aq at 18/4. %Cd(NO 3 ) 2 54.027 43.716 30.879 Sp.gr. 1.711 1.515 1.321 %Cd(NO 3 ) 2 21.353 14.899 8.683 Sp. gr. 1.204 1.134 1.074 (de Muynck, W. Ann. 1894, 53. 561.) Cd(NO 3 ) 2 +Aq containing 7.89% Cd(NO 3 ) 2 has sp. gr. 20/20 = 1.0673. Cd(NO 3 ) 2 + Aq containing 12.14% Cd(NO 3 ) 2 has sp. gr. 20/20 = 1.1070. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 282.) Sat. Cd(NO 3 ) 2 +Aq boils at 132. Almost entirely insol. in cone. HNO 3 -fAq. (Wurtz.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Sol. in alcohol. Sol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Sol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) +4H 2 O. M.-pt. of Cd(NO 3 ) 2 -HH 2 O = 59.5. (Ordway; Tilden, Chem. Soc. 45. 409.) Solubility in H 2 O. Solubility in H 2 O at t. t % Cd(NO ? ) 2 in the solution Mols. H 2 O to 1 mol. Cd(NO 3 ) 2 18 30 40 59.5 mpt. 52.31 55.90 58.40 61.42 76.54 11.96 10.34 9.34 8.24 4.00 (Funk, B. 1899, 32. 105.) Sat. solution of Cd(NO 3 ) 2 +4H 2 O in H 2 O at contains 52.3% Cd(NO 3 ) 2 ; at 18, 55.9% Cd(NO 3 ) 2 . (Mvlius, Z. anorg. 1912, 74. 411.) Sol. in liquid NH 3 . (Johnson and Wils- more, Elektroch. Z. 1908, 14. 227.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Sol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 13 1 +1 37.37 47.33 52.73% Cd(NO 3 ) 2 . NITRATE, CALCIUM 559 Cryohydrate is formed at 16. (Funk, Z. anorg. 1899, 20. 416.) The composition of the hydrates formed by Cd(NO 3 ) 2 at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by Cd(NOs) 2 and of the con- ductivity and sp. gr. of Cd(NO 3 ) 2 +Aq. (Jones, Am. Ch. J. 1905, 34. 308.) Cadmium uranyl nitrate, Cd(NO 3 ) 2 , (UO 2 )(NO 3 ) 2 +30H 2 O. Sol. in H 2 O and acids. Insol. in alcohol and alkalies +Aq. (Lancien, C. C. 1912. 1. 208.) Cadmium nitrate ammonia. Cd(NO 3 ) 2 , 6NH 3 +H 2 0. (Andre, C. R. 104. 987.) Cadmium nitrate cupric oxide, Cd(NO 3 ) 2 , CuO+5H 2 O. Ppt. (Mailhe, C. R. 1902, 134. 235.) Cadium nitrate cupric oxide, Cd(NO 3 ) 2 , 3CuO+5H 2 O. (Mailhe, A. ch. 1902, (7) 27. 383.) Cadmium nitrate hydrazine, Cd(NO 3 ) 2 , 3N 2 H 4 . Decomp. by hot H 2 O. Sol. in warm NH 4 OH. (Franzen, Z. anorg. 1908, 60. 282.) Caesium nitrate, CsNO 3 . 100 pts. H 2 O dissolve 10.58 pts. CsNO 3 at 3.2. SI. sol. in absolute alcohol. (Bunsen.) h. Solubility of CsNO 3 in H 2 O at t. t G. CsNOs per 100 g. t G. CsNOa per 100 g. Solu- tion Water Solu- tion Water 10 20 30 40 50 8.54 12.97 18.7 25.3 32.1 39.2 9.33 14.9 23.0 33.9 47.2 64.4 60 70 80 90 100 106.2 45.6 51.7 57.3 62.0 66.3 68.8 83.8 107.0 134.0 163.0 197.0 220.3 (Berkeley, Trans. Roy. Soc. 1904, 203. A, 213.) 100 g. H 2 O dissolve 26.945 g. CsNO 3 at 25. (Haigh, J. Am. Chem. Soc. 1912, 34. 1148.) Sp. gr. 20/4 of a normal solution of CsNO 3 = 1.140905; of a 0.5 normal solution = 1.07001. (Haigh.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Solubility in glycol=8% at ord. temp, (de Coninck, Belg. Acad. Bull. 1905, 359.) Caesium hydrogen nitrate. CsNO 3 , HNO 3 . Sol. in H 2 O. (Wells, Am. Ch. J. 1901, 26. 273.) CsNO 3 , 2HNO 3 . (W.) Caesium cerium nitrate, Cs 2 Ce(NO 3 )6. Sol. in H 2 O; very si. sol. in HNO 3 . (Meyer, Z. anorg. 1901, 27. 371.) ' Sol. in HNO 3 . (Meyer, B. 1900, 33. 2137.) Caesium ferric nitrate, CsNO 3 , Fe(NO 3 ) 3 + 7H 2 O. Deliquescent. (Wells, Am. Ch. J. 1901, 26. 276.) Caesium silver nitrate, CsNO 3 , AgNO 3 . Sol. in H 2 O. (Russell and Maskelyne, Roy. Soc. Proc. 26. 357.) Caesium thorium nitrate, Cs 2 Th(NO 3 ) 6 . Decomp. by H 2 O; si. sol. in HNO 3 . (Meyer, Z. anorg. 1901, 27. 384.) Caesium uranyl nitrate, Cs(UO 2 )(NO 3 ) 3 . Decomp. by H 2 O. Sol. in cone. HNO. (Meyer, B. 1903, 36. 4057.) Decomp. by H 2 O at low temp., so that the solid phase in contact with the solution con- sists of the double salt and CsNO 3 . At 16.1 100 pts. by wt. of the solution in H 2 O con- tain 31.39 pts. UO 2 and 6.59 pts. Cs. (Rim- bach, B. 1904, 37. 477.) Calcium nitrate, basic, Ca?(NO 3 ) 2 , CaO 2 H 2 + Decomp. by H 2 O. (Werner, A. ch. (6) 27. 570.) +H 2 O. As above. (Rousseau and Tite, C. R. 114. 1184.) Calcium nitrate, Ca(NO 3 ) 2 . Deliquescent. Very sol. in H 2 O with evolu- tion of much heat. 100 pts. H 2 O at dissolve 84.2 pts. Ca(NO 3 ) 2 . (Poggiale.) 100 pts. H 2 O at dissolve 93.1 pts. Ca(NO 3 ) 2 . (Mulder.) Sol. in 0.25 pt. cold PhO with reduction of temp. Sol. in all proportions in boiling HeO. (Berzelius.) Sol. in 2 pts. cold, and 0.6667 pt. boiling HjO. (Fourcroy.) Sat. Ca(NOs)2+Aq at 12.5 contains 33.8%. (Has- senfratz, A. ch. 28. 29.) Solubility in H 2 O. 100 g. of the solution contain at: 55 80 90 100 78.16 78.20 78.37 78.43 g. Ca(NO 3 ) 2 , 125 C 147.5 78.80 151 (bpt. of sat. solution at 760 mm.) 78.57 78.80 79.00 g. Ca(NO 8 ) 2 . The anhydrous salt is the stable solid phase above 51.3. (Bassett and Taylor, Chem. Soc. 1912, 101. 580.) 560 NITRATE, CALCIUM 100 g. sat. Ca(NO 3 ) 2 +Aq contain 77.3 g Ca(NO 3 ) 2 at 25. (Taylor and Henderson. J. Am. Chem. Soc. 1915, 37. 1692.) See also +2, 3, and 4H 2 O. Sp.gr. of Ca(NO 3 ) 2 +Aq at room temp containing : 17.55 30.10 40.13 % Ca(NO 3 ) 2 . 1.1714 1.2739 1.3857 (Wagner, W. Ann. 1883; 18. 270.) Sp. gr. of Ca(NO 3 ) 2 +Aq at 17.5 Ca(NO 3 ) 2 +Aq containing 7.15% Ca(NO 3 ) 2 has sp. gr. 20/20 = 1.0554. Ca(NO 3 ) 2 +Aq containing 7.91% Ca(NO 3 ) 2 has sp. gr. 20/20 = 1.0613. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 284.) Sp. gr. of Ca(NO 3 ) 2 +Aq'at 20 containing M g. mols. of salt per liter. M 0.0125 0.025 0.05 0.125 Sp.gr. 1.001846 1.003166 1.00604 1.01523 Ca(NO 3 ) 2 Sp. gr. Ca(N0 3 ) 2 Sp. gr. M 0.25 0.5 0.75 Sp. gr. 1.03074 1.06011 1.08874 M 1.00 1.50 Sp. gr. 1.11751 1.17375 (Jones and Pearce, Am. Ch. J. 1907, 38 Saturated Ca(NO 8 ) 2 +Aq containing pts. Ca(NO 3 ) 2 to 100 pts. H 2 O boils a (Legrand); 152 (Kremers). Forms a crust at 141, and contains pts. Ca(NO 3 ) 2 to 100 pts. H 2 O; highest observed, 151. (Gerlach, Z. anal. 26. 4 B.-pt. of Ca(NO 3 ) 2 +Aq containing Ca(NO 3 ) 2 to 100 pts. H 2 O. G = a ing to Gerlach (Z. anal. 26. 447 according to Legrand (A. ch. (2) 59 . 704.) 351.2 it 151 333.5 temp. 27.) ; pts. ccord- ). j 1 5 10 15 20 25 30 1.009 1.045 1.086 1.129 1.174 1.222 1.272 35 40 45 50 55 60 1.328 1.385 1.447 1.515 '1.588 1.666 (Franz, J. pr. (2) 5; 274.) , Sp. gr. of Ca(NO 3 ) 2 +Aq at 17.5. Ca(N0 3 ) 2 Sp. gr. Catf ?0 JO 3) 2 Sp. gr. 10 20 30 1.076 1.163 1.261 40 50 ' 60 1.368 1.483 1.605 , L = .436). B.-pt G L B.-pt. G L (Gerlach, Z. anal. 27. 283.) Sp. gr. of Ca(NO 3 ) 2 +Aq at 18. 101 102 103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 119 120 121 122 123 124 125 126 10 20 30 40 50 60 70 80 89 98 106.5 114.5 122.5 130 137.5 144 150.5 157 163.5 170 176 182.5 189 195.5 202 208.5 15 25.3 34.4 42.6 50.4 57.8 64.9 71.8 78.6 85.3 91.9 98.4 104.8 111.2 117.5 123.8 130 136.1 142.1 148.1 160 !l 172 '.2 184 .'5 127 128 129 130 131 132 133 134 135 136 137 138 139 140 141 142 143 144 145 146 147 148 149 150 151 151.97 215.5 222.5 230 237.5 245 253 261.5 270 278.5 287 296 305 314.5 324 333.5 343.5 354 364.5 375 386 397.5 409 420.5 432.5 444.5 455.68 197^0 209! 5 222^2 235^1 248 .1 261.3 274 .'7 288 .'4 302-6 317.4 333^2 351 .'2 362.2 Ca(N0 3 ) 2 Sp. gr. ' Ca(N0 3 ) 2 Sp. gr. 6 12 25 .25 .5 .0 1.0487 1.1016 1.2198 37 50 .5 .0 1.3546 1.5102 (Kohlrausch, W. Ann. 1879. 1 Sp. gr. of Ca(NO 3 ) 2 +Aq at 24.65. of g.X^> mol. wt. dissolved in H 2 O; b=sp. gr. if a is Ca(NO 3 ) YZ mol. wt. = 118; c = sp. gr. Ca(NO 3 ) 2 , y% mol. wt. =82. a=no. 1000 g. 2, 4H 2 O, if a is a b c a b c 1 2 3 4 5 1.056 1.104 1.145 1.181 1.213 1.059 1.112 1.160 1.205 1.246 6 7 8 9. 10 1.243 1.270 1.294 1.316 1.336 1.286 1.323 (Favre and Valson, C. R. 79. 968.) Sp. gr. of Ca(NO 3 ) 2 +Aq at 25. Concentration of Ca(NOs) 2 +Aq. Sp. gr. Sat. Ca(NO 3 ) 2 +Aq boils at 132. (Ord- way, Sill. Am. J. (2) 27. 14.) Cone. HNO 3 precipitates Ca(NO 3 ) 2 from ts aqueous solution. (Mitscherlich, Pogg. 18. 159.) Very sol. in cone. HNO 3 . (Rawson, J. Soc. Chem. Ind. 1897, 16. 113.) 1-normal l /l " 1.0596 1.0300 1.0151 1,0076 (Wagner, Z. phys. Ch. 1890, 6. 36.) NITRATE, CALCIUM 561 Solubility in HNO 3 +Aq at 25. Solubility of Ca(NO 8 ) 2 +CaS 2 O 8 at t. 100 g. of the solution contain Solid phase t Ca(Nbs)2 m CaS 2 3 Solid phase G. Ca(NOs) 2 G. HNOs 57.98 54.82 52 96 0.00 3.33 5.87 1 9 46.02 45.68 27.92 5.46 6.81 10.46 Ca(N0 3 ) 2 , 4H 2 " CaS 2 O 8 , 6H 2 O CaS 2 O 3 , 6H 2 O 51 .'58 7.21 10.49 22.81 u 47.82 11.27 29.33 45.59 40.70 13.71 19.65 Ca(NO 3 ) 2 +4H 2 O 25 54.03 4.27 Ca(N0 3 ) 2> 4H 2 38.17 34.46 32.84 22.80 28.81 32.63 ";' 50.25 45.92 42.93 9.10 13. 13.83 "+CaS 2 O 8 , 6H 2 O CaS 2 O 3 , 6H 2 O 32.50 33.52 32.01 17.09 (( 33.44 35 63 ' 19.51 23.78 29.05 41'. 66 Ca(N0 8 ) 2 +3H 2 O 8.15 29.85 it 27.79 45.70 31.09 40.56 (Kremann and Rothmund, Z. anorg. 1914, 26.07 45.70 86. 373.) 17.41 12.25 55.48 62.05 Ca(N0 3 ) 2 +2H 2 9.34 65.69 8.52 5.06 67.20 71.12 Very easily sol. in liquid NH 8 . (Franklin, Am. Ch. J. 1898, 20. 827.) 2.53 74.77 Sol. in 0.8 pt. alcohol (Macquer); 1 pt. 1.05 0.54 78.56 80.83 Ca(NO 3 ) 2 boiling alcohol. (Bergmann.) Dry Ca(NO 3 ) 2 is sol. in 7 pts. alcohol at 0.36 0.01 (about) 85.83 90.90 15 and 1 pt. boiling alcohol. (Bergmann.) 0.00 96.86 These results show that the hydrates of Ca(NO 3 ) 2 which are stable at 25 in contact Sp. gr. of Ca(NO 8 ) 2 +alcohol. with HNO 3 +Aq are Ca(NO 3 ) 2 +4H 2 O, +3H 2 O and +2H 2 O. % Ca(NOs)2 Sp. gr. 20/20 (Bassett and Taylor, Chem. Soc. 1912, 101. 0.7949 582.) 4.96 0.8278 6.47 0.8383 Sol. in glacial HC 2 H 3 O 2 . (Persoz.) Sol. in sat. KNO 3 +Aq with elevation of temp, and pptn. of a portion of KNO 3 . (Fourcroy and Vauquelin, A. ch. 11. 135.) Solubility of Ca(NO 3 ) 2 +NaN0 8 at t. t % Ca(NOi) a % NaNOa Solid phase 9 47.51 46.08 26.67 11.76 9.51 12.56 23.32 34.26 Ca(N0 8 ) 2 , 4H 2 " +NaNO 8 NaNO 3 t( 25 54.58 53.22 52.73 52.40 37.31 26.91 14.61 7.25 10.70 12.08 11.58 19.48 24.98 36.12 Ca(NO 3 ) 2 , 4H 2 O (t " +NaNO 8 NaNO 8 u n 68.74 Methyl alcohol 65.5 Ethyl alcohol 52.0 42.7 42.45 mpt. of Ca(NO 3 ) 2 +4H 2 < 71.70 Propyl alcohol 36 . 5 Isobutyl alcohol 25 . (Bassett and Taylor, I. c.) Amyl alcohol 13.3 Acetone 58 . 5 (D'Ans and Siegler, I. c.) Solubility of a and ft modifications in H 2 at t. a modification is the stable form. Sol. in 1.87 pts. ether-alcohol (1 : 1). (Fresenius, Z. anal. 32. 191.) r c CNO } Ether ppts. Ca(NO 3 ) 2 from its alcoholic t in 100 g. of" Solid phase solution. Easily sol. in boiling amyl alcohol. /T~> " Cl'11 A T H Aft r-O \ solution (Browning, bill. Am. J. 143. 53.) Sol. in acetone. (Naumann. B. 1904. 37. 50.17 aCa(NO 3 ) 2 +4H 2 ( 4328.) 22.2 56.88 a " Insol. in benzonitrile. (Naumann, B. 1914, 25.0 57.90 a 47. 1370.) 30.0 60.16 a Insol. in methylal. (Eidmann, C. C. 1899. 30.0 61.57 ft II. 1014.) 34.0 63.66 ft 1 g. Ca(NO 3 ) 2 is sol. in 1.44 g. methyl 35.0 62.88 a ' acetate at 18. Sp. gr. 18/4 of sat. solution 38.0 64.34 a ' a it = 1.313. (Naumann, B. 1909, 42. 3795.) 38.0 66.65 ft Sol. in ethyl acetate. (Naumann, B. 1910,, 43. 314.) 39.0 1 39.6 67.93 69.50 ft ft +2H 2 O. Solubility in H 2 O. 2 39.0 75.34 ft 100 g. of the solution contain at: 40.0 66.21 a 49 51 1-42.7 69.50 a " 77.49 78.05 g. Ca(NO 3 ) 2 . 2 42.4 71.70 a " Solutions in stable equilibrium with the dihydrate can only exist between the limits of temp. 48.4 and 51.3. (Bassett and Tay- 1 mpt. of hydrate. 2 reflex pt. lor, Chem. Soc. 1912, 101. 580.) +3H 2 O. Solubility in H 2 O. 100 g. of the solution contain at: (Taylor and Henderson, 1915, 37. J. Am. Chem. So( 1692. 40 45 50 ' 51 70.37 71.45 73.79 74.73 g. Ca(NO 3 ) 2 . Mpt. of Ca(NO 3 ) 2 +3H 2 O=51.1. (Bassett and Taylor, I. c.) Sp. gr. of solution sat. at 18 = 1.548, con taining 54.8% Ca(NO 3 ) 2 . (Mylius, B. 1897 30. 1718.) +4H 2 O. Ca(NO 3 ) 2 +4H 2 O melts in its crystal H 2 O at 44. (Tilden, Chem. Soc. 45. 409.) NITRATE, CERIC ZINC 563 Solubility in ethyl alcohol +Aq at 25. Ceric magnesium nitrate, CeMg(NO 3 )6. IQTT n % C 2 H 5 OH in the solvent % C 2 H 5 OH in the solution % Ca(NO 3 ) 2 in the solution -|-orl 2 \J. Decomp. by H 2 O; sol. in HNO 3 +Aq with- out decomp. (Meyer, Z. anorg. 1901, 27. 57.5 373.) 18.3 3.5 56.1 39.2 8.1 55.2 Cerous manganous nitrate, 2Ce(NO 3 )3, 59.2 14.1 52.9 3Mn(NO 3 ) 2 +24H 2 O. 80.4 22.3 50.2 Sol. in H 2 O. (Lange, J. pr. 82. 129.) 90.4 29.4 49.0 1 1. sat. solution in HNO 3 +Aq (sp. gr. 99.4 31.1 49.7 1.325) contains 193.1 g. hydrous salt at 16. 99.4 31.2 52.0 (Jantsch.) 99.4 29.5 56.2 60.1 28.3 58.9 Ceric manganous nitrate, CeMn(NO 3 ) 6 -f- 60.1 27.8 60.0 8H 2 0. 60.1 60.1 27.3 26.5 60.7 62.3 Decomp. by H 2 O and dil. HNO 3 ; sol. in cone. HNO 3 without decomp. (Meyer, Z. (D'Ans and Siegler, Z. phys. Ch. 1913, 82. 42.) anorg. 1901, 27. 377.) Calcium nitrate hydrazine, Ca(NO 3 ) 2 , 2N 2 H 4 +H 2 0. Ppt. (Franzen, Z. anorg. 1908, 60. 288.) Calcium nitrate tungstosilicate, Ca 2 Wi 2 SiO 4 o, Ca(NO 3 ) 2 . + 13H 2 O and +15H 2 O. Decomp. by H 2 O. (Wyrouboff, Chem. Soc. 1897, 72. (2) 176.) Cerous nitrate, Ce(NO 3 ) 3 +6H 2 O. Not very deliquescent. (Jolin.) Very sol. in H 2 O; sol. in 2 pts. alcohol. (Vauquelin.) Sol. in acetone. (Eidmann, C. C. 1899. II. 1014; Naumann, B. 1904, 37. 4328.) Ceric nitrate, Ce(NO 3 ) 4 . Deliquescent. Decomp. by hot H 2 O. (Berzelius.) Sol. in alcohol. (Dumas.) Basic compounds containing 12 mols. or less CeO 2 to 1 mol. N^Os may be obtained, which are sol. in H 2 O. (Ordway.) Cerous cobaltous nitrate, 2Ce(NO 3 ) 3 , 3Co(NO 3 ) 2 +24H 2 O. Deliquescent. Easily forms supersaturated solutions. (Lange, J. pr. 82. 129.) 1 1. sat. solution in HN0 8 +Aq (sp. gr. 1.325) contains 103.3 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 321.) Ceric cobaltous nitrate, CeCo(NO 3 ) 6 -|-8H 2 O. Decomp. by H 2 O when heated; sol. in cold H 2 O; si. sol. in HNO 3 . (Meyer, Z. anorg. 1901, 27. 376.) Cerous magnesium nitrate, 2Ce(NO 3 ) 3 , 3Mg(NO 3 ) 2 +24H 2 O. Slightly deliquescent. Easily sol. in H 2 O or alcohol, and easily forms supersaturated solutions. (Holzmann, J. pr. 75. 330.) 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 63.8 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 321.) Cerous nickel nitrate, 2Ce(NO 3 ) 3 , 3Ni(NO 3 ) 2 +24H 2 O. Easily sol. in H 2 O. (Holzmann, J. pr. 76. 321.) 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 80.3 g. hydrous salt at 16. (Jantsch.) Ceric nickel nitrate, CeNi(N0 3 ) 6 +8H 2 O. Decomp. by H 2 O when heated; sol. in H 2 O in the cold; si. sol. in HNO 3 . (Meyer, Z. anorg. 1901, 27. 375.) Cerous potassium nitrate, Ce(NO 3 ) 3 , 2KN0 3 +2H 2 0. Sol. in H 2 0. (Lange, J. pr. 82. 136.) Ceric potassium nitrate, CeK 2 (NO 3 ) 6 . Sol. in H 2 with decomp. (Meyer, Z. anorg. 1901, 27. 370.) Efflorescent. (Holzmann, J. pr. 75. 324.) Ceric rubidium nitrate, CeRu 2 (NO 3 ) 6 . Very sol. in H 2 O ; si. sol. in HNO 3 . (Meyer.) Ceric sodium nitrate. Deliuescent. tion eliquescent. Decomp. by recrystalliza- .. (Holzmann.) Cerous thallous nitrate, [Ce(NO 3 ) 5 ]Tl 2 -{- 4H 2 0. Very hydroscopic. Decomp. by H 2 O. (Jantsch, Z. anorg. 1911, 69. 229.) Cerous zinc nitrate, 2Ce(NO 3 ) 3 , 3Zn(NO 3 ) 2 -f 24H 2 O. Sol. in H 2 O. Easily forms supersat. solu- tions. (Lange, J. pr. 82. 129.) 1 1. sat. solution in HNO 3 +Aq (sp. gr. ] 325) contains 124.1 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 321.) Ceric zinc nitrate, ZnCe(NO 3 ) 6 +8H 2 0. Decomp. by H 2 O; sol. in HN0 3 +Aq. (Meyer, Z. anorg. 1901, 27. 374.) 564 NITRATE, CEROCERIC ZINC Ceroceric zinc nitrate (?), Ce 3 O 4 , 2ZnO, 6N 2 O 5 +18H 2 O (?). Easily sol. in H 2 O. (Holzmann, J. pr. 76. 321.) Chromic nitrate, basic, Cr 2 O(NO 3 )4. Sol.inH 2 O. (Lowel.) +12H 2 O. Sol. in H 2 O. (Ordway.) Chromic nitrate, Cr(NQ 3 ) 3 +9H 2 O. Very sol. in H 2 O and alcohol. (Lowel.) Melts in its crystal H 2 O at 36.5. Sat. Cr(NO 3 ) 3 +Aq boils at 125.6. (Ordway.) Sp. gr. of Cr(NO 3 ) 3 -f-Aq. M = concentration of solution in gram, mols. W = wt. of 25 cc. of solution. M 0.0934 0.1868 0.3736 0.5604 0.9340 W 25.4300 25.8828 26.7302 27.5524 29.3072 M 1.1208 1.3076 1.4944 1.8680 W 30.0668 30.8464 31.6327 33.3379 (Jones and Getman, Z. phys. Ch. 1904, 49. 426.) Sol. in acetone. (Naumann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) Chromic nitrate chloride, CrCl 2 (NO 3 ). Sol. in H 2 O and alcohol. (SchinyA. 124. 177.) Cr(NO 3 ) 2 Cl. (Schiff.) Chromic nitrate sulphate, Cr 2 (S0 4 )(NO 3 ) 4 . Hygroscopic. Completely sol. in H 2 O. Cr 2 (S0 4 ) 2 (N0 3 ) 2 . Sol. inH 2 0. (Schiff, A. 124. 174.) Cobaltous nitrate, basic, 6CoO, N 2 O 5 +5H 2 O. Ppt. Gradually sol. in H 2 O with deposition of CoO. (Winkelblech, A. 13. 155.) Sol. in cold HC1, and HNO 3 +Aq. De- comp. by hot KOH+Aq. 4CoO, N 2 O 6 +6H 2 O. Ppt. (Habermann, M. 6. 432.) Cobaltous nitrate, Co(NO 3 ) 2 . Deliquescent in moist air. Very sol. in H 2 0. See +3, 6, and 9H 2 O. Sp. gr. of aqueous solution at 17.5 con- taining: 5 10 15 20%Co(NO 3 ) 2 , 1.0462 1.0906 1.1378 1.1936 25 30 35 40%Co(NO 3 ) 2 . 1.2538 1.3190 1.3896 1.4662 Sp. gr. of sat. solution = 1.5382. (Franz, J. pr. (2) 6.274.) Sp. gr. of Co(NO 3 ) 2 +'Aq at room temp, containing: 8.28 15.96 24.528% Co(NO 3 ) 2 . 1.0732 1.1436 1.2288 (Wagner, W. Ann. 1883, 18. 268.) Sp. gr. of Co(NO 3 ) 2 +Aq at 25 C Concentration of Co(NCh)2+Aq. 1-normal r- " V4- Sp. gr. 1.0728 1.0369 1.0184 1.0094 (Wagner, Z. phys. Ch. 1890, 5. 37.) Sp. gr. at 20 of Co(NO 3 ) 2 +Aq containing M g. mols. Co(NO 3 ) 2 per liter. M 0.01 0.025 0.05 0.075 Sp. gr. 1.001496 1.003863 1.007579 1.011289 M 0.10 0.25 0.5 0.75 Sp. gr. 1.015084 1.03737 1.07415 1.11204 M 1.0 1.5 2.0 Sp. gr. 1.14612 1.21720 1.28576 (Jones and Pearce, Am. Ch. J. 1907, 38. 715.) Sol. in liquid NH 3 . (Guntz, Bull. Soc. 1909 (4) 6. 1009.) 100 g. sat. solution in glycol contains 80 g. Co(NO 3 ) 2 . (de Coninck, C. C. 1905, II. 883.) Sol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) +3H 2 O. Solubility in H 2 O. Sat. solution contains at: 55 62 70 84 91 mpt. 61.74 62.88 64.89 68.84 77.21% Co(NO,) 2 . (Funk, Z. anorg. 1899, 20. 408.) +6H 2 O. Melts in its crystal H 2 O at 56 (Ordway); 38 (Tilden). Solubility in H 2 O. Sat. solution contains at: 21 10 4 41.55 43.69 44.85 45.66% Co(NO 3 ) 2 , +18 C 49.73 41 56 mpt. 55.96 62.88% Co(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 408.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Easily sol. in alcohol. Sol. in 1 pt. strong alcohol at 12.5. (Wenzel.) Easily sol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Difficultly sol. in ethyl acetate. (Nau- mann, B. 1910, 43. 314.) +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 26 23.5 20.5 39.45 40.40 42.77% Co(N0 3 ) 2 . Cryohydrate is formed at 29. (Funk, Z. anorg. 1899, 20. 409.) NITRATE, CUPRIC 565 Cobaltous didymium nitrate, 3Co(NO 3 ) 2 , 2Di(NO 3 ) 3 -j-48H 2 O. Very deliquescent. (Frerichs and Smith, A. 191. 331.) Cobaltous gadolinium nitrate, 3Co(NO 3 ) 2 , 2Gd(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 3 (sp. gr. 1.325) contains 451.4 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Cobaltous lanthanum nitrate, 3Co(NO 3 ) 2 , 2La(NO 3 ) 3 +24H 2 0. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 109.2 g.. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Cobaltous neodymium nitrate, 3Co(NO 3 ) 2 , 2Na(NO 3 ) 3 +24H 2 0. 5 1.0452 10 1.0942 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 151.6 hydrous salt at 16. 20 1.2036 25 1.2644 (Jantsch.) 35 40 f^rkHflltrtnc nrac*rkflvtriiitin riifrato 3f^rf''\rO..'W 1.3974 1.4724 2Pr(N0 3 ) 3 +24H 2 O. 1 1. sat. solution in HN0 3 +Aq (sp. gr. 8H 2 O. Hydroscopic; sol. in HNO 3 +Aq. (Meyer, Z. anorg. 1901, 27. 387.) Cobaltous nitrate ammonia, Co(NO 3 ) 2 , 6NH 3 +2H 2 O. Decomp. by H 2 O with separation of basic nitrate. (Fremy.) Sol. in NH 4 OH+Aq. (Hess.) Cobaltous nitrate cupric oxide, Co(NO 3 ) 2 , 3CuO+3H 2 O. Ppt. (Mailhe, C. R. 1902, 134. 234.) Cobaltous nitrate hydrazine, Co(NO 3 ) 2 , 3N 2 H 4 . Decomp. by hot H 2 O. (Franzen, Z. anorg, 1908, 60. 274.) Cupric nitrate, basic, 2CuO, N 2 O 5 . (Ditte, A. ch. 1879, (5) 18. 339.) 4CuO, N 2 9 5 +3H 2 O. Insol. in H 2 O. Eas- ily sol. in acids. (Graham, A. 29. 13.) Insol. in H 2 O; easily sol. in acids. (Athan- asesco, Bull. Soc. 1895, (3) 11. 1113.) +3^H 2 O. Insol. in H 2 O, and decomp. by heat. (Casselman, Z. anal. 4. 24.) Cupric nitrate, Cu(NO 3 ) 2 . Deliquescent. Very easily sol. in H 2 O or alcohol; also in moderately cone. HNO 3 +Aq, but is precipitated from cone, aqueous solu- tion by HNO 3 -f Aq of 1.522 sp. gr. (Mit- scherlich, Pogg. 18. 159.) . Sat. Cu(NO 3 ) 2 +Aq contains at: 10 3 +3 38.8 41.6 44.5% Cu(NO 3 ) 2 , 8 20 32 48.5 54.1 % 61.2% Cu(N"O 3 ) 2 . (fitard, A. ch.' 1894, (7) 2. 528.) See +3, 6, and 9H 2 O. Sp. gr. of Cu(NO 3 ) 2 -hAq at 17.5 contain- ing: 15% anhydrous salt, 1.1442 30% anhydrous salt, 1.3298 45% anhydrous salt. 1.5576 (B. Franz, J. pr. (2) 5. 274.) Sp. gr. of Cu(NO 3 ) 2 -f Aq at 15. (Jantsch.) % Cu(N0 3 )2 Sp. gr. Cobaltous samarium nitrate, 3Co(NO 3 )2, 5.22 1.046 2Sm(N0 3 ) 3 +24H 2 0. 10.44 1.094 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 34.27 g. hydrous salt at 16. 15.67 20.85 1.146 1.202 (Jantsch.) 26.12 1.262 /~Wa1frtliei +Vi/~tMiirvi ni+i-a+a P'/iTl-i ( XTT^ -^ - _l_ 35.00 1.377 (Long, W. Ann. 1880, 11. 39.) Sp. gr. of Cu(NO 3 ) 2 +Aq at room temp, containing: 18.99 26.68 46.71% Cu(NO 3 ) 2 . 1.1774 1.2637 1.5363 (Wagner, W. Ann. 1883, 18. 272.) Sp. gr. of Cu(NO 3 ) 2 +Aq at 25. Concentration of Cu(NOi)+Aq Sp. gr. 1-normal Vr- " V- " Vs- " 1.0755 1.0372 1.0185 1.0092 (Wagner, Z. phys. Ch. Sp.gr. of Cu(NO 3 ) 2 +Aq % Cu(NO 3 ) 2 1 5 1890, 5. 38.) at 12.5. 10 14 Sp. gr. 1.0059 1.0320 1.0655 1.0916 %Cu(NO 3 ) 2 20 24 30 34 Sp.gr. 1.1350 1.1716 1.2320 1.2712 %Cu(N0 3 ) 2 40 44 50 56 Sp.gr. 1.3320 1.3749 1.4440 1.5205 (Hassenfratz, Muspratt, 1893, 4. 2243.) 566 NITRATE, CUPRIC, AMMONIA Sp. gr. at 20 of Cu(NO 3 ) 2 +Aq containing M g. mols. salt per liter. M 0.01 0.025 0.05 0.075 Sp. gr. 1.001504 1.004076 1.007859 1.011715 M 0.25 0.50 0.75 0.935 Sp. gr. 1.040290 1.07723 1.11469 1.14262 Sp. gr. 1.5 2.0 1.29262 M 1.22618 (Jones and Pearce, Am. Ch. J. 1917, 38. 719.) Sat. Cu(NO 3 ) 2 +Aq tfoils at about 173. (Griffiths.) Insol. in fuming HNO 3 . (Ditte, A. ch. 1879 (5) 18. 339.) Solubility of Cu(NO 3 ) 2 +Pb(NO 3 ) 2 in H 2 O at 20. In 1 1. of solution Sp. gr. Cu(NOs) 2 Pb(NO 3 ) 2 Solid phase g- g. mol. g. g. mol. 1.354 70.5 0.375 359.5 1.086 Pb(N0 3 ) 2 1.322 139.2 0.742 257.2 0.777 1.321 226.5 1.207 175.1 0.529 1.343 301.8 1.608 133.4 0.403 1.360 341.8 1.821 117.8 0.356 1.451 519.4 2.767 70.5 0.213 1.546 681.7 3.632 44.0 0.133 1.622 798.1 4.252 28.1 0.085 1.700 943.2 5.028 17.2 0.052 Pb(NOs)2 + Cu(NO 3 ) 2 .6H 2 O (Fedotieff, Z. anorg. 1911, 73. 178.) Very sol. in liquid NH 3 (Guntz, Bull. Soc. 1909, (4) 5. 1007.) Easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) +3H 2 O. Melts in crystal H 2 O at 114.5. (Ordway; Tilden, Chem. Soc. 45. 409.) Solubility in H 2 O. Sat. solution contains at: 25 30 40 50 60.01 60.44 61.51 62.62% Cu(NO 3 ) 2 , 60 70 80 114.5 Mpt. 64.17 65.79 67.51 77.59% Cu(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 413.) 100 pts. HNO 3 dissolve 2 pts. at 13, con- siderably more on heating. (Ditte, A. ch. 1879, (5) 18. 339.) Sol. in 1 pt. strong alcohol at 12.5. (Wen- zel.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +6H 2 O. Efflorescent. Melts in crystal H 2 Oat38. (Ordway.) Solubility in H 2 O. Sat. solution contains at: 21 10 +10 39.52 42.08 45.00 48.79% Cu(NO 3 ) 2 , 18 20 26.4 mpt. 53.86 55.58 63.39% Cu(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 413.) Sat. solution of Cu(NO 3 ) 2 +6H 2 O in H 2 O at 20 contains 5.04 g. mol. per 1. Sp. gr. of sat. solution = 1.688. (Fedotieff, Z. anorg. 1911, 73. 78.) Sat. solution of Cu(NO 3 ) 2 +6H 2 O m{H 2 contains 45.0 g. Cu(NO 3 ) 2 in 100 g. solution at 0; 53.9 g. at 18. (Mylius, Z. anorg. 1912, 74.411.) +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 23 21 20 36.08 37.38 40.92% Cu(NO 3 ) 2 . Cryohydrate is formed at 24. (Funk, Z. anorg. 1899, 20. 414. Cupric nitrate ammonia (Cuprammonium nitrate), Cu(NO 3 ) 2 , 4NH 3 . Easily sol. in H 2 O, from which it can be recrystallized. Sol. in alcohol. (Berzelius.) Sol. in 1 pt. liquid NH 3 . (Horn, Am. Ch. J. 1908, 39. 216.) Cu(NO 3 ) 2 , 5NH 3 . (Horn, Am. Ch. J. 1907, 37. 620.) 4Cu(NO 3 ) 2 , 23NH 3 . (Horn.) Cupric nitrate hydrazine, Cu(NO 3 ) 2 , N 2 H 4 . Decomp. by H 2 O. (Hofmann and Marburg, A. 1899, 305. 221.) Cupric nitrate mercuric oxide, Cu(NO 3 ) 2 , HgO+3H 2 O. Sol. in HC1, HNO 3 and H 2 SO 4 . (Finzi, Gazz. ch. it. 1913, 43. (2) 709.) Didymium nitrate, basic, 4Di 2 O 3 , 3N 2 O 5 + 15H 2 O. Insol. in H 2 O. (Marignac.) 2Di 2 O 3 , 3N 2 O 5 . (Becquerel, A. ch. (6) 14. 257.) Didymium nitrate, Di(NO 3 ) 3 . Anhydrous. Very sol. in H 2 O. As sol. in 96% alcohol as in H 2 O, and the solution is not precipitated by much ether. Insol. in pure ether. (Marignac, A. ch. (3) 36. 161.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Sol. in acetone. (Naumann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) +6H 2 O. Very deliquescent. (Cleve, Bull. Soc. (2) 43. 361.) NITRATE, IRON 567 Didymium nickel nitrate, 2Di(NO 3 )3, 3M(NO 3 ) 2 +36H 2 O. Very deliquescent. (Frerichs and Smith, A. 191. 355.) See Neodymium and praseodymium. Didymium zinc nitrate, 2Di(NO 3 ) 3 , 3Zn(NO 3 ) 2 +69H 2 0. Very deliquescent. (F. and S.) -See Neodymium and praseodymium. Dysprosium nitrate, Dy(NO 3 )+5H 2 O. Very sol. in H 2 O; less sol. in H 2 O+HNO 3 . Sol. in alcohol. (Urbain, C. R. 1908, 146. 129.) Erbium nitrate, basic, 2Er 2 O 3 , 3N 2 O 6 +9H 2 O. Decomp. by H 2 O. SI. sol. in HNO 3 . (Bahr and Bunsen.) 3Er 2 O 3 , 4N 2 O 5 +20H 2 O. (Cleve, BuU. Soc. (2) 21. 344.) Erbium nitrate, Er(NO 3 ) 3 +6H 2 O, Easily sol. in H 2 O, alcohol, and ether. (Hoglund.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Gadolinium nitrate, Gd(NO 3 ) 3 +6^H 2 O. Sol. in H 2 O. (Benedicks, Z. anorg. 1900, 22. 406.) +5H 2 O. Sol. inHNO 3 . (B.) Gadolinium magnesium nitrate, 2Gd(NO 3 ) 3 , 3Mg(NO 3 ) 2 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. 1.325) contains 352.3 g. hydrous salt at 1 (Jantsch, Z. anorg. 1912, 76. 303.) y , 76. gr. 6. Gadolinium nickel nitrate, 2Gd(NO 3 ) 3 , 3Ni(NO 3 ) 2 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 400.8 g. hydrous salt at 16. (Jantsch.) Gadolinium zinc nitrate, 2Gd(NO 3 ) 3 , 3Zn(NO 3 ) 2 +24H 2 O. 1 1. sat. solution in HN0 3 +Aq (sp. gr. 1.325) contains 472.7 g. hydrous salt at 16. (Jantsch.) Gallium nitrate, Ga(NO 3 ) 3 . Very deliquescent, and sol. in H 2 O. (Dupre*.) Glucinum nitrate, basic, 2G1O, N 2 O 6 + 3H 2 O (?). Sol. in H 2 O. 3G1O, N 2 O 5 . Sol. in H 2 0. (Ordway, Sill. Am. J. (2) 26. 205.) Compounds more basic than this are insol. in H 2 O. (Ordway.) Glucinum nitrate, G1(N0 3 ) 2 +3H 2 O. Very deliquescent. (Joy, Sill. Am. J. (2) 36. 90.) Easily sol. in H 2 O and alcohol. (Vauquelin.) Melts in its crystal H 2 O at 29.4. (Ord- way.) Sat. Gl(NO 3 ) 2 +Aq boils at 140.5. (Ord- way.) Gold (auric) nitrate, basic, Au 2 O 3 , N 2 O 6 -J- 2 / 5 H 2 O, or Auryl nitrate, (AuO)NO 3 + (Schottlander, A. 217. 364.) 2Au 2 O 3 , N 2 O 5 +2H 2 O = Au 4 O 5 (NO 3 ) 2 -f- 2H 2 O. Slowly sol. in HNO 3 +Aq at 100. (Schottlander, A. 217. 356.) Gold (auric) nitrate, Au(NO 3 ) 3 +zH 2 O. Decomp. by H 2 O. Sol. in acetone. (Han- riot and Raoult, C. R. 1912, 155. 1086.) Gold (auric) hydrogen nitrate, Au(NO 3 ) 3r HNO 3 +3H 2 O. Decomp. by H 2 O. Sol. in HNO 3 +Aq. (Schottlander, A. 217. 356.) Gold (auric) potassium nitrate, KAu(NO 3 ) 4 . Easily sol. in H 2 O. HK 2 Au(NO 3 ) 6 . Decomp. immediately by H 2 0. 2KAu(NO 3 ) 4 , K 2 HAu(NO 3 ) 6 . (Schott- lander, J. B. 1884. 453.) Gold (auric) rubidium nitrate, RbAu(NO 3 )4. Easily sol. in H 2 O. HRb 2 Au(NO 3 ) 6 . As above. (Schott- lander.) Gold (auric) thallium nitrate, TlAu(NO 3 ) 4 . Easily sol. in H 2 O. 6Au 2 O 3 , 2T1 2 O 3 , 3N 2 5 -fl5H 2 O. Ppt. (Schottlander.) Indium nitrate, In(NO 3 ) 3 +4^H 2 O. Very deliquescent. Easily sol. in H 2 O and absolute alcohol. (Winkler.) Iron (ferrous) nitrate, Fe(NO 8 ) 2 +6H 2 O. 100 pts. of crystals dissolve in 50 pts. H 2 O at 0, sp. gr. of solution = 1.44; 40.8 pts. H 2 O at 15, sp. gr. of solution = 1.48; 33.3 pts. H 2 O at 25, sp. gr. of solution = 1.50. (Ordway, Sill. Am. J. (2) 40. 325.) Sat. solution contains at: 9 +18 24 60.5 Mpt. 39.68 41.53 45.14 46.51 62.50% Fe(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 406.) Sat. solution of Fe(NO 3 ) 2 +6H 2 O in H 2 O contains 41.5% Fe(NO 3 ) 2 at 0; 45.1% at 18. (Mylius, Z. anorg. 1912, 74. 411.) 568 NITRATE, IRON, BASIC +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 27 21.5 19 15.5 35.66 36.10 36.56 37.17% Fe(NO 3 ) 2 . Cryohydrate is formed at 28. (Funk, Z. anorg. 1899, 20. 407.) Fe(NO 3 ) 2 -|-Aq decomposes on heating; less rapidly when dil., more readily in presence of excess of acid. (Ordway.) Iron (ferric) nitrate, basic, 36Fe 2 O 3 , N 2 O 5 + 48H 2 O (?). Easily sol. in H 2 O. SI. sol. in dil. HN0 3 -f Aq; very si. sol. in alcohol. (Hausmann, A. 89. 111.) 8Fe 2 O 3 , N 2 O 5 +12H 2 O. SI. sol. in H 2 O; very si. sol. in cold or warm dil. HNO 3 + Aq; more easily sol. in hot HCl+Aq. (Haus- mann.) -f-#H 2 O. Sol. in H 2 O; completely pptd. from aqueous solution by NaCl, NH 4 C1, KI, KC1O 3 , Na 2 SO 4 , CaSO 4 , ZnSO 4 , CuSO 4 , KNO 3 NaNO 3 , Ba(C 2 H 3 O 2 ) 2 , or Zn(C 2 H 3 O 2 ) 2 +Aq. More slowly pptd. by NH 4 NO 3 , Mg(NO 3 ) 2 , Ba(NO 8 ) 2 , or Pb(NO 3 ) 2 +Aq. Not pptd. by alcohol, Pb(C 2 H 3 O 2 ) 2 , Cu(C 2 H 3 O 2 ) 2 , Hg(CN) 2 , AgNO 3 , or As 2 O 3 +Aq. (Ordway, Sill. Am. J. (2) 9. 30.) 4Fe 2 O 3 , N 2 O 5 +1^H 2 O. Easily sol. in H 2 O; si. sol. in dil. HNO 3 -f Aq, and in al- cohol. (Hausmann.) +3H 2 0. Insol. in H 2 O or HNO 3 +Aq; sol. in HCl+Aq. (Scheurer-Kestner, C. R. 87. 927.) +9H 2 O. Not deliquescent; easily sol. in H 2 O. (Ordway.) 3Fe 2 O 3 , N 2 O 5 +2H 2 O. Insol. in H 2 O. (Scheurer-Kestner.) 2Fe 2 O 3 , N 2 O 6 +H 2 O. Decomp. by H 2 O. (Scheurer-Kestner. ) +8H 2 O. (S.-K.) Fe 2 O 3 , N 2 O 6 . Decomp. by H 2 O. (S.-K.) Fe 2 O 3 , 2N 2 O 5 . Sol. in H 2 O or alcohol in all proportions. Insol. in HNO 3 +Aq. N 2 O 6 with 1, 2, 3, 4, 5, 6, and 8Fe 2 O 3 forms compounds, sol. in H 2 O. (Ordway.) Solubility determinations show that there are no definite basic nitrates of iron formed from solutions at 25, and that the solid phase under these conditions is a solid solution of Fe 2 O 3 , HNO 3 and H 2 O. The normal salt, Fe 2 O 3 , 3N 2 O 5 , 18H 2 O is stable in solutions containing about 30-45% N 2 O 8 . In higher concentrations of nitric acid it appears to be metastable and a new salt, Fe 2 O 3 , 4N 2 O 5 , 18(?)H 2 O is the stable form. (Cameron, J. phys. Chem. 1909, 13. 252.) Iron (ferric) nitrate, Fe(NO 3 ) 3 . +H 2 O. (Scheurer-Kestner, A. ch. (3) 65. 113.) +6H 2 O. Deliquescent, and sol. in any amount of H 2 O. (Schonbein, Pogg. 39. 141.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) +9H 2 O. Deliquescent. Sol. in H 2 O and alcohol. SI. sol. in HNO 3 +Aq. 2 pts. salt with 1 pt. H 2 O lower the temperature 18.5. (Scheurer-Kestner.) Sp. gr. of solution at 17.5 containing: 5 10 15 20 25% Fe(NO 3 ) 3 , 1.0398 1.0770 1.1182 1.1612 1.2110 30 35 40 45 50% Fe(NO 3 ) 3 , 1.2622 1.3164 1.3746 1.4338 1.4972 55 60 65% Fe(NO 3 ) 3 . 1.5722 1.6572 1.7532 (Franz, J. pr. (2) 5. 274.) Nearly insol. in cone. HNO 3 +Aq at temp, below 15.5. Easily sol. in alcohol. Melts in crystal H 2 O at 47.2. (Ordway.) Sat. Fe(NO 3 ) 3 -hAq boils at 125. (Ord- way.) Lanthanum nitrate, La(NO 3 ) 3 +6H 2 0. Very deliquescent; easily sol. in H 2 O and alcohol. (Mosander.) Melts in its crystal H 2 O at 40; boils at 124.5. (Ordway.) La(NO 3 ) 3 +Aq sat. at 25% contains 60.17% La(NO 3 ) 3 , or 100 g. H 2 O dissolve 151.1 g. La(NO 3 ) 3 at 25. (James and Whittemore, J. Am. Chem. Soc. 1912, 34. 1169.) Sol. in acetone. (Naumann, B. 1904, 37. 4328; Eidmann, C. C. 1899, II. 1014.) Lanthanum magnesium nitrate, 2La(N0 3 ) 3 , 3Mg(NO 3 ) 2 +24H 2 O. Deliquescent in moist air. (Holzmann, J. pr. 75. 350.) 1 1. sat. solution in HN0 3 +Aq (sp. gr. 1.325) contains 63.8 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 321.) Lanthanum manganous nitrate, 2La(NO 3 ) 3 , 3Mn(NO 3 ) 2 +24H 2 O. Sol. in H 2 O. (Damour and Deville.) 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 193.1 g. hydrous salt at 16. (Jantsch.) Lanthanum nickel nitrate, 2La(NO 3 ) 3 , 3Ni(NO 3 ) 2 +36H 2 O. Very sol. in H 2 O. (Frerichs and Smith, A. 191. 355.) +24H 2 O. 1 1. sat. S9lution in HN0 3 + Aq (sp. gr. 1.325) contains 80.3 g. hydrous salt at 16. (Jantsch.) Lanthanum rubidium hydrogen nitrate, [La(NO 3 ) 4 ]Rb, HNO 3 +6H 2 O. Sol. in H 2 O and HNO 3 . (Jantsch, Z. anorg. 1911, 69. 225.) Lanthanum thallous nitrate, [La(NO 3 ) 5 ]Tl 2 4- 4H 2 0. Hydroscopic. (Jantsch, Z. anorg. 1911, 69. 228.) NITRATE, LEAD 569 Lanthanum zinc nitrate, 2La(NO 3 ) 3 , Solubility in 100 pts. H 2 O at t. 3Zn(NO 3 ) 2 +24H 2 O. * Very sol. in H 2 O. (Damour and Deville, J. B. 1858. 135.) t Pts. Pb(N0 3 ) 2 t Pts. Pb(NO) 2 t Pts. Pb(NO 3 ) 2 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 124.1 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 321.) +69H 2 O. (Frerichs and Smith, A. 191. or*- \ 1 2 3 36.5 37.4 38.3 39.1 36 37 38 39 65.9 66.7 67.6 68.5 72 73 74 75 99.7 100.7 101.7 102.6 o5o.) 4 39.8 40 69.4 76 103.6 5 40.5 41 70.3 77 104.6 Lead nitrate, basic, 2PbO, N 2 O 5 +H 2 O = Pb(OH)NO 3 . 6 7 8 41.2 42.0 42.8 42 43 44 71.2 72.1 73.0 78 79 80 105.6 106.6 107.6 Sol. in 5.15 pts. H 2 O at 19.2. (Pohl, W. A. B. 6. 597.) Very si. sol. in cold, much more inhotH 2 O. (Berzelius.) Sol. inPb(C 2 H 3 O 2 ) 2 9 10 11 43.6 44.4 45.2 45 46 47 74.0 74.9 75.9 81 82 83 108.6 109.6 110.6 +Aq. .(Guignet, C. R. 56. 358.) Insol. in H 2 O; sol. in acids. (Athanesco, 12 13 46.0 46.8 48 49 76.8 77.7 84 85 111.5 112.5 Bull. Soc. 1895, (3) 13. 178.) 14 47.5 50 78 7 86 113.5 +2H 2 O. (Andre, C. R. 100. 639.) 15 48.3 51 79.6 87 114.5 3PbO, N 2 O 6 +13^H 2 O. SI. sol. in pure H 2 O. 16 49.1 52 80.5 88 115.4 Insol. in H 2 O containing HC1. (Berzelius.) 17 49.9 53 81.5 89 116.4 +3H 2 O. Sol. in 119.2 pts. cold, and 10.5 18 50.7 54 82.4 90 117.4 pts. boiling H 2 O. Sol. in Pb(C 2 H 3 O 2 ) 2 +Aq, 19 51.5 55 83.3 91 118 4 but si. sol. in KNO 3 +Aq. (Vogel, jr. A. 94. 20 52.3 56 84.3 92 119.4 97.) 21 53.1 57 85.2 93 120.3 = lOPbO, 3N 2 O 5 -f 5H 2 O. (Wakemann and 22 53.9 58 86.1 94 121.3 Wells, Am. Ch. J. 9. 299.) 23 54.7 59 87.1 95 122 3 +4H 2 O. (Andre, C. R. 100. 639.) 6PbO, N 2 O 5 -hH 2 O. Nearly insol. in H 2 O. 24 25 55.6 56.4 60 61 88.0 89.0 96 97 123.2 124.2 (Lowe, J. pr. 98. 385.) lOPbO, 3N 2 O 5 +4H 2 O. Less sol. in H 2 O 26 27 57.3 58.1 62 63 90.0 90.9 98 99 125.2 126 1 than Pb(NO 3 )OH, and not decomp. by boiling 28 59.0 64 91.9 100 127.0 H 2 O. (Wakemann and Wells, Am. Ch. J. 9. 29 59.8 65 92.8 101 128.0 299.) 30 60.7 66 93.8 102 128.9 31 61.6 67 94.8 103 129.9 32 62.4 68 95.7 104 130 9 Lead nitrate, Pb(NO 3 ) 2 . 33 63.3 69 96.7 104.7 131.5 Sol. in H 2 O with absorption of much heat. 34 64.1 70 97.7 (Rose.) 35 65.0 71 98.7 1 pt. Pb(NO 3 ) 2 dissolves in 7Y 2 pts. cold H 2 O. (Mitscherlich.) 1 pt. Pb(NO 3 )2 dissolves in 1.989 pts. H 2 O at 17.5 and forms a liquid of 1.3978 sp. gr. (Karsten.) 1 pt. Pb(NO 3 ) 2 dissolves in 1.707 pts. H 2 O at 22.3; in 1.585 pts. H 2 O at 24.7. (Kopp.) Sol. in 1.87 pts. H 2 O at 17.5. (Schiff, A. 109. 326.) 100 pts. Pb(NO$)2+Aq sat. at 102.2 contain 52.5 pts. Pb(NO 3 ) 2 , or 100 pt. H 2 O dissolve 110.526 pts. Pb(NO 3 ) 2 at 102.2. (Griffiths.) Sol. in 7.5 pts. cold H 2 O and much less hot H 2 O. (Wittstein.) 100 Dts. boiling H 2 O dissolve 13 pts. Pb(NOs) 2 . (Ure's Diet.) 100 pts. Pb(NO 3 ) 2 +Aq sat. at 19-20 con- tain 35.80 pts. salt. (v. Hauer, W. A. B. 53, 2. 221.) 1 pt. dissolves: at 10 25 45 65 85 100 in 2.58 2.07 1.65 1.25 0.99 0.83 0.72 pts. H 2 O. (Kremers, Pogg. 92. 497.) 1 1. Pb(NO 3 ) 2 +Aq sat. at 15 contains 461.49 g. Pb(NO 3 ) 2 and 928.58 g. H 2 O, and has sp. gr. 1.39. (Michel and Krafft, A. ch. (3) 41. 471.) (Mulder, Scheik. Verhandel. 1864. 66.) 100 g. H 2 O dissolve 52.76 g. Pb(NO 3 ) 2 at 17. (Euler, Z. phys. Ch. 1904, 49. 315.) Solubility of Pb(NO 3 ) 2 in H 2 O at 20 = 1.52 g. mol. per 1. Sp. gr. of sat. solution = 1.419. (Fedotieff, Z. anorg. 1911, 73. 178.) Sat. Pb(NO 3 ) 2 +Aq at contains 26.7% Pb(NO 3 ) 2 ; at 18, 29.1% Pb(NO 3 ) 2 . (Mylius, Z. anorg. 1912, 74. 411.) Sp. gr. of Pb(NO 3 ) 2 +Aq at 19.5. % PbCNOsh Sp.gr. Pb(NOi)i Sp. gr. 5 10 15 20 1.045 1.093 1.144 1.203 25 30 35 1.266 1.334 1.414 (Kremers, calculated by Gerlach, Z anal 8 286.) 570 NITRATE, LEAD Sp. gr. of Pb(NO 3 ) 2 +Aq at 17.5. Pb(NO 3 ) 2 Sp. gr. % Pb(N0 3 ) 2 Sp. gr. 5 10 15 20 1.044 1.092 1.144 1.200 25 30 35 sat. sol. 1.263 1.333 1.409 1.433 (Gerlach, Z. anal. 27. 283.) Sp. gr. of Pb(NO 3 ) 2 +Aq sat. at 8 C (Anthon.) 1.372, Sp. gr. of Pb(NO 3 ) 2 +Aq at 17.5. Pb(NO 3 ) 2 Sp. gr. Pb(NOs) 2 Sp. gr. 1 1.0080 20 1.1902 2 1.0163 21 .2016 3 1.0247 22 .2132 4 1.0331 23 .2251 5 1.0416 24 .2372 6 1.0502 25 .2495 7 1.0591 26 .2620 8 1.0682 27 1.2747 9 1.0775 28 1.2876 10 1.0869 29- 1.3907 11 1.0963 30 1.3140 12 1 . 1059 31 1.3276 13 1.1157 32 1.3416 14 1 . 1257 33 1.3558 15 1 . 1359 34 1.3702 16 1 . 1463 35 1.3848 17 1 . 1569 36 1.3996 18 1.1677 37 1.4146 19 1.1788 (Schiff, calculated by Gerlach, Z. anal. 8. 286.) Sp. gr. of Pb(NO 3 ) 2 +Aq at t. t % Pb(N0 3 ) 2 Sp. gr. 14 5 1.0451 14 10 1.0939 14.5 15 1 . 1468 14.3 20 1.2045 15 25 1.2678 15 32.28 1.3716 (Long, W. Ann. 1880, 11. 40.) Sp. gr. of Pb(NO 3 ) 2 +Aq at room temp, containing: 17.93 32.22% Pb(NO 8 ) 2 . 1.1786 1.3619 (Wagner, W. Ann. 1883, 18. 267.) Sp. gr. of Pb(NO 3 ) 2 +Aq at 25. Concentration of Pb(NO 3 ) 2 +Aq Sp. gr. 1-normal Vr- " Vc- " Vs- " 1.1380 1.0699 1.0351 1.0175 (Wagner, Z. phys. Ch. 1890, 6. 36.) Pb(NO 3 ) 2 +Aq containing 15.93% Pb(NO 3 ) 2 has sp. gr. 20/20 = 1.1558. Pb(NO 3 ) 2 +Aq containing 30.57% Pb(NO 3 ) 2 has sp. gr. 20/20 = 1.3436. Pb(NO 3 ) 2 +Aq containing 30.69% Pb(NO 3 ) 2 has sp. gr. 20/20 = 1.3465. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 279.) Sat. Pb(NO 3 ) 2 +Aq boils at 103.5. (Krem- ers.) Sat. Pb(NO 3 ) 2 +Aq boils at 102.2, and contains 140 pts. Pb(NO 3 ) 2 to 100 pts. H 2 O. (Griffiths.) Sat. Pb(NO 3 ) 2 +Aq boils at 103.5. (Ger- lach, Z. anal. 26. 427.) B.-pt. of Pb(NO 3 ) 2 +Aq containing pts. Pb(NO 3 ) 2 to 100 pts. H 2 O, according to Gerlach (Z. anal. 26. 449). B.-pt. Pts. Pb(NO 3 ) 2 B.-pt. Pts. Pb(NOs)2 100.5 101 101.5 102 11 26 44 65 102.5 103 103.5 87 111 137 Insol. in cone. HNO 3 +Aq. Solubility of Pb(NO 3 ) 2 +Ba(NO 3 ) 2 , See under Ba(NO 3 ) 2 . Solubility of Pb(NO 3 ) 2 +Cu(NO 3 ) 2 . See under Cu(NO 3 ) 2 . Sol. in sat. KNO 3 +Aq without pptn., 100 pts. H 2 at 18.75 dissolving 114 pts. mixed salt, viz. 84.1 pts. Pb(NO 3 ) 2 and 29.9 pts. KNO 3 . (Karsten.) 100 pts. H 2 O dissolve 119.6 pts. Pb(NO 3 ) 2 and 67.1 pts. KNO 3 at 21.2. (Riidorff, B. 6. 484.) 100 g. H 2 O dissolve 95.39 g. Pb(NO 3 ) 2 and 61.05 g. KNO 3 at 20. (Le Blanc and Noyes. Z. phys. Ch. 1890, 6. 386.) Sol. in sat. NaNO 3 +Aq without pptn., 100 pts. H 2 O at 18.75 dissolving 121.9 pts. mixed salt, viz. 87.8 pts. Pb(NO 3 ) 2 and 34.1 pts. NaNO 3 . (Karsten.) Solubility of Pb(N0 8 ) 2 +NaNO 8 . Solid phase = Pb(NO 3 ) 2 . t of saturation % NaNOs % Pb(N0 3 ) 2 32 34.42 19.69 35.5 34.15 20.33 39.5 33.71 21.35 44. 33.35 22.19 49.1 32.94 23.15 55 32.60 23.93 58 32.47 24.24 62 32.33 24.57 65 32.14 24.89 NITRATE, NITRITE, LEAD, BASIC 571 Solubility of Pb(NO 3 ) 2 +XaNO 3 Continued. Solubility of Pb(NO 3 ) 2 in pyridine at t. Solid phas e = NaNO 3 t G.Pb(NOs)2 per 100 g. CoH 6 N Solid phase t of saturation % NaNOs % Pb(NO 3 ) 2 21 26.5 31 38.8 41 44.25 51 58 64 40 42 43 44 45 46 47 49 49 .97 .04 .18 .63 .11 .03 .28 .03 .92 13.62 13.38 12.88 12.78 12.94 12.45 12.50 11.76 11.56 19.4 14.5 10 5.4 8.7 14.72 19.97 24.75 30.03 34.97 40.03 45. 49.97 51 tr. pt. 59.52 70 80 89.93 94.94 96 tr. pt 99.89 104.90 109.90 2.93 2.14 1.90 3.54 3.93 5.39 6.13 6.78 8.56 10.98 13.20 16.94 22.03 29.37 36] 70 47.29 61.60 90.21 128.06 143] 36 152 163.80 Pb(NO 3 ) 2 , ( 4C5H 6 N u t( tt t( it (t 1C 11 (( It (I {( "+Pb(N0 3 ) 2 , 3C 5 H 6 N Pb(NO 3 ) 2 , 3C 6 H 5 N ft d 1C {( "+Pb(N0 3 ) 2 , 2C 6 H 5 N Pb(NO 3 ) 2 , 2C 5 H 5 N it u (Isaac, Chem. Soc. 1908, 93. 398.) Also sol. in KNO 3 +NaNO 3 +Aq. 100 pts. sat. Pb(NO 3 ) 2 +Sr(N0 3 ) 2 +Aq contain 45.98 pts. of the two salts at 19.20. (v. Hauer, J. pr. 98. 137.) Solubility of Pb(N0 3 ) 2 +Sr(NO 3 ) 2 at 25. G. per 100 cc. Mol. per cent in solid phase Pb(NO 3 ) 2 Sr(N0 3 ) 2 Pb(NOs)2 Sr(NO 3 ) 2 46.31 50.47 53.92 45.34 44.48 25.23 19.13 4.56 8.14 17.81 18.74 35.03 37.54 71.04 100. 99.05 98.11 97.02 96.06 83.84 32.88 0.95 1.89 2.98 3.94 16.16 67.12 100. (Walton and Judd, J. Am. Chem. Soc. 1911, 33. 1036.) Lead mercurous nitrate, 2PbO, 2Hg 2 O, 3N 2 O 5 . Decomp. by H 2 O. Sol. in warm dil. HNO 3 , or Hg 2 (NO 3 ) 2 +Aq without decomp. (Stad- eler, A. 87. 129.) Lead silver nitrate, Pb(NO 3 ) 2 , 2AgNO 3 . Sol. in H 2 O. (Sturenberg, Pogg. 74. 115.) (Fock, Z. Kryst. Min. 1897, 28. 365.) Very easily sol. in liquid NH 3 . (Franklin Am. Ch. J. 1898, 20. 828.) 100 pts. alcohol of 0.9282 sp. gr. dissolve: at 4 8 22 40 50 4.96 5.82 8.77 12.8 14.9 pts. Pb(NO 3 ) 2 (Gerardin, A. ch. (4), 5. 129.) 100 pts. absolute methyl alcohol dissolv< 1.37 pts. at 20.5. 100 pts. absolute ethyl alcohol dissolve 0.04 pt. at 20.5. (de Bruyn. Z. phys. Ch. 10 783.) Very si. sol. in acetone. (Krug and M'El- roy, J. Anal. Ch. 6. 184.) Insol. in cold, si. sol. in hot CS 2 . (Arctow- ski, Z. anorg. 1894, 6. 257.) Insol. in benzonitrile. (Naumann, B. 1914 47. 1370.) Insol. in methyl acetate. (Naumann, B 1909, 42. 3790); ethyl acetate. (Naumann B. 1910, 43. 314.) Mol. weight determined in pyridine. (Wer- ner, Z. anorg. 1897, 16. 21.) Lead silver nitrate iodide, Pb(NO 3 ) 2 , 8AgNO 3 , 4AgI. Decomp. by H 2 O. (Sturenberg.) Pb(NO 3 ) 2 , 2AgNO 3 , 2AgI. Decomp. by H 2 O. (Sturenberg.) Lead nitrate nitrite, basic, 4PbO, N 2 O 5 , N 2 O 3 +2H 2 O=Pb(OH)NO 8 , Pb(OH)NO 2 . SI. sol. in cold, easily in hot H 2 O. Sol. in 80 pts. H 2 O at 23 (Chevreuil); 85 pts. at ord. temp. (Bromeis, A. 72. 38); 10.6 pts. at 100 (Chevreuil). +2H 2 0. Solubility in acetic acid. Normality of acid g. PbO per 100 cc. sat. solution Normality of acid g. PbO per 100 cc. sat. solution 0.05 0.10 0.601 1.323 2.185 0.25 0.50 0.75 5.450 9.690 15.874 (Chilesotti, Att. Acad. Line. 1908, (5) 17, II. 475.) 572 NITRATE, LEAD, PHOSPHATE Formula is 3Pb(OH)NO 3 , 5Pb(OH)NO 2 + H 2 O. (v. Lorenz, W. A. B. 84, 2. 1133.) +3H 2 O. (v. Lorenz.) 4PbO, N 2 O 5 , 3N 2 O 3 +4H 2 O. Sol. in H 2 (Bromeis.) 6PbO, N 2 O 6 , 2N 2 O 3 +3 2 /3H 2 O=Pb(OH)NO 3 2Pb(OH)NO 2 + 2 / 3 H 2 O. ( v . Lorenz.) 6PbO, 2N 2 O 6 , N 2 O 3 + 3 2 / 3 H 2 O = 2Pb(OH)NO 3 , Pb(OH)NO 2 +V 3 H 2 O. (v Lorenz.) 7PbO, N 2 O 3 , N 2 O 5 +3H 2 O. Less sol. in H 2 O than 4PbO, N 2 O 5 , N 2 O 3 +2H 2 O; sol. in cold cone. HNO 3 +Aq. (Peligot, A. 39. 338.) 8PbO, N 2 O 5 , 3N 2 O 3 +4 2 / 3 H 2 O=Pb(OH)NO 3 3Pb(OH)NO 2 + V 3 H 2 O. (v. Lorenz.) lOPbO, N 2 5 , 4N 2 3 +5H 2 = Pb(OH)N0 3 4Pb(OH)NO 2 . (v. Lorenz.) 12PbO,N 2 O 6 ,5N 2 O 3 +6H 2 O = Pb(OH)NO 3 , 5Pb(OH)NO 2 . (v. Lorenz.) 10PbO,5N 2 O 6 ,2N 2 O 3 +4H 2 0=Pb(OH)N0 3 , 2Pb(OH)NO 2 , 2PbO + 3^H 2 O. (v. Lorenz.) 14PbO, N 2 O 6 , 3N 2 O 3 +6H 2 O=Pb(OH)NO 3 , 3Pb(OH)NO 2 , 3PbO+H 2 O. (Bromeis.) 14PbO, 3N 2 O 5 , N 2 O 3 +6H 2 O = 3Pb(OH)NO 3 , Pb(OH)NO 2 , 3PbO+H 2 O. (Bromeis.) 16PbO, 2N 2 O 5 , 3N 2 O 3 +6H 2 O = 4Pb(OH)N0 3 , 6Pb(OH)N0 2 , 5PbO, Pb(OH) 2 (v. Lorenz.) 16PbO, 3N 2 O 5 , 5N 2 O 3 +10H 2 O = 3TPb(OH)NO 3 , 5Pb(OH)NO 2 +H 2 O. (v. Lorenz.) 26PbO, 6N 2 O 5 , 7N 2 3 -}-21H 2 O = 6Pb(OH)NO 3 , 7Pb(OH)NO 2 +4H 2 O. (v. Lorenz.) Lead nitrate phosphate, Pb(NO 3 ) 2 , Pb 3 (PO 4 ) 2 +2H 2 0. Completely insol. in cold H 2 O. Decomp. by boiling H 2 O into its constituents. Sol. in a little cone. HNO 3 +Aq without decomp. (Gerhardt, A. 72. 83.) Lead nitrate phosphite, Pb(NO 3 ) 2 , PbHPO 3 . Decomp. by H 2 O. Sol. in Pb(NO 3 ) 2 +Aq. Pb(NO 3 ) 2 +Aq (33.3 g. per litre) dissolves 1 g. salt at 15. If less than 31 g. per litre of Pb(NO 3 ) 2 are present the salt is decomp. (Amat, A. ch. (6) 24. 317.) Lead nitrate potassium nitrite. Pb(NO 3 ) 2 , 2KN0 2 +H 2 0. Difficultly sol. in H 2 O. (Lang, J. B. 1862. 102.) 3PbO, 3K 2 0, 4N 2 3 , 2N 2 O 5 +3H 2 O. Sol. in H 2 O. (Hayes, Sill. Am. J. (2) 31. 226.) Lithium nitrate, LiNO 3 . Very deliquescent, and sol. in H 2 O. 100 pts. H 2 O dissolve: at 20 40 70 100 110 48.3 75.7 169.4 196.1 227.3 256.4 pts. LiNO 3 . (Kremers, Pogg. 99. 47.) Forms supersaturated solutions with ease, which crystallize when temp, is lowered to + 1. (Kremers, Pogg. 92. 520.) Sat. solution boils at over 200. (Kremers, Pogg. 99. 43.) 1 pt. LiNO 3 dissolves in 200 pts. HNO 3 . (Schultz, Zeit. Ch. (2) 5. 531.-) 100 pts. of the sat. solution contain at: 64.2 70.9 64.9 66.1 pts. anhydrous salt. (Donnan and Burt, Chem. Soc. 1903, 83. 339.) See +^H 2 O, and 3H 2 0. Sp. gr. of LiNO 3 -f-Aq at 19.5 containing pts. LiN0 3 in 100 pts. H 2 O: 12.7 1.069 54.8 1.245 14.2 1.077 57.5 1.255 26.4 1.134 77.4 1.315 41.8 pts. LiNO 3 , 1.197 79.4 pts. LiNO 3 . 1.319 (Kremers, Pogg. 114. 45.) Sp. gr. of LiN0 3 +Aq. g. LiNOs in 1000 g. of solution Sp. gr. 16/16 4.8526 10.9128 17.9016 1.000000 1.002469 1 . 0055495 1.009113 (Dijken, Z. phys. Ch. 1897, 24. 109.) Sp. gr. 20/4 of a normal solution of LiNO 3 = 1.03803; of a 0.5-normal solution = 1.01830. (Haigh, J. Am. Chem. Soc. 1912, 34. 1151.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. in strong alcohol. Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Solubility in acetone = 0.343 g. mol. per 1. at 18. (Roshdestwensky and McBride, Chem. Soc. 1911, 99. 2140.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Difficultly sol. in ethyl acetate. (Nau- mann, B. 1910, 43. 314.) + ^H 2 O. Solubility in H 2 O. 100 pts. of the sat. solution contain at : 43.6 50.5 55.0 60.0 60.8 61.3 63.0 63.6 pts. anhydrous salt. 61.1 is the temp, at which LiNO 3 goes over into LiNO 3 . (Donnan and Burt, '"'hem. Soc. 1903, 83. 339.) NITRATE, MAGNESIUM 573 +3H 2 0. Solubility in H 2 O. 100 pts. of the sat. solution contain pts. anhydrous salt at t. Sp. gr. of Mg(NO 3 ) 2 +Aq at 21. % Mg(N03)2 +oH2O Sp. gr. % Mg(N0 3 )2 Sp. gr. 2 4 6 8 10 12 14 16 18 20 22 24 26 .0078 .0158 .0239 .0321 .0405 .0490 .0577 .0663 .0752 .0843 1.0934 1 . 1026 1.1120 28 30 32 34 36 38 40 42 44 46 48 50 1.1216 1.1312 1.1410 1.1508 1.1608 1.1709 1.1811 1.1914 1.2019 1.2124 1.2231 1.2340 t Pts. anhydrous salt 0.10 10.50 12.10 13.75 19.05 22.10 27.55 29.47 29.78 29.87 29.86 29.64 29.55 34.8 37.9 38.2 39.3 40.4 42.9 47.3 53.67 55.09 56.42 56.68 57.48 58.03 (Schiff, calculated by Gerlach, Z. anal. 8. 286.) Sp. gr. of Mg(NO 3 ) 2 +Aq at 18. Mpt. of LiNO 3 +3H 2 O is 29.88. (Donnan and Burt, Chem. Soc. 1903, 83. 337.) IMTarrmAciiiifft vti+^/t+n Vinl \ I . .- AT I \ % Mg(NOa)s Sp. gr. % Mg(N0 3 )2 Sp. gr. 5 10 1.0378 1.0763 15 17 1.1181 1.1372 AA W^AAWOA W.J..1.A .LUtA ClL\s} ILT.OXV/y iTj. ^3 X 1 ^^ O* Insol. in H 2 O and alcohol. Sol. in acids. (Chodnew, A. 71. 241.) +5H 2 O. Decomp. by H 2 O. (Didier, C. R. 1896, 122. 936.) Magnesium nitrate, Mg(N0 3 ) 2 . Anhydrous. Deliquescent. Sol in 1 pt. H 2 O at 15.6. Sol. in 4 pts. abs. alcohol at 15.6, and 2 pts. at boiling temp. More sol. in alcohol of 0.817 sp. gr. than,in that of 0.900. (Kirwan.) Sol. in 0.3458 pt. strong alcohol at 82.5. (Wenzel.) Sol. in 10 pts. strong alcohol at 15. (Bergmann.) Sol. in 9 pts. stiong alcohol on heating. (Bergmann.) Solubility in H 2 O in .presence of the an- hydrous salt. Sat. solution contains at: 89 63.14 77.5 65.67. 67' 67.55% Mg(N0 3 ) 2 . (Funk, Z. anorg. 1899, 20. 396.) See +6, and 9H 2 O. Sp. gr. of Mg(NO 3 ) 2 +Aq at 14. % Mg(NOs) 6H 2 Sp. gr. % Mg(N0 3 ) 2 , 6H 2 Sp. gr. 1 5 10 15 20 25 1.0034 1.0202 1.0418 1.0639 1.0869 1.1103 30 35 40 45 49 1.1347 1.1649 1 . 1909 1.2176 1.2397 (Oudemans, Z. anal. 7. 419.) (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of Mg(NO 3 ) 2 -f Aq a t room temp, containing: 18.62 34.19 39.77% Mg(N0 3 )o. 1.1025 1.2000 1.4298 (Wagner, W. Ann. 1883, 18. 273.) Sp. gr. of Mg(NO 8 ) 2 +Aq at 25. Concentration of Mg(N0 3 ) 2 +Aq Sp. gr. 1-normal Vr- " l /- " Ys- " 1 1 1 1 .0512 .0259 .0130 .0066 (Wagner, Z. phys. Ch. 1890, 5. 38.) Sp. gr. of solution sat. at 18 = 1.384, con- taining 43.1% Mg(NO 3 ) 2 . (Mylius, B. 1897, 30. 1718.) Sp. gr. of Mg(NO 3 ) 2 +Aq. M Mg(NOs) 2 g. in 1000 g. of solution Sp. gr. 16/16 1.000000 0.8099 1.000660 1.5621 .001253 3.3398 . 002539 7.4410 . 005523 15.161 .011151 29.356 .021580 58.353 .043329 81.025 .060773 (Dijken, Z. phys. ( Uh. 1897, 24. 107.) 574 NITRATE, MAGNESIUM NEODYMIUM Sp. gr. of Mg(NO 3 ) 2 +Aq at 20. 1. p = per cent strength of solution; d = ob- served density; w = volume concentration in grams per cc. p d w 35.02 1.3110 0.46695 31.15 1.2655 0.39420 25.03 1.2057 0.30172 19.55 .1551 0.22585 13.43 . 1028 0.14815 10.09 .0753 0.10850 6.650' .0480 0.06968 4.672 .0330 0.04826 4.001 .0276 0.04112 1.372 .0085 0.01383 (Barnes, J. phys. Chem. 1898, 2. 545.) Sp. gr. of Mg(NO 3 ) 2 +Aq at 20 containing M g. mols. of salt per liter. M 0.02 0.05 0.10 0.15 Sp. gr. 1.00224 1.005626 1.011118 1.016557 M 0.20 0.50 1.00 1.274 Sp. gr. 1.022026 1.054804 1.107865 1.136615 (Jones and Pearce, Am. Ch. J. 1907, 38. 707.) ' Less sol. in Ca(NO 3 ) 2 +Aq than in H 2 O. (Dijonval.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) +2H 2 O. Mpt. 127. (Wasiljew, C. C. 1909, II. 1966.) +4H 2 O. Mpt. 45.5. (W.) -f 6H 2 O. Deliquescent. Sol. in H 2 O and alcohol. Sol. in 0.5 pt. cold H 2 O, and 9 pts. cold alcohol of 0.84 sp. gr.; very si. sol. in abs. alcohol. (Graham.) Melts in its crystal H 2 O at 90, and the re- sulting liquid boils at 143.4. (Ordway, Sill. Am. J. (2) 27. 14.) Solubility in H 2 O. Sat. solution contains at: 18 4.5 18 38.03 39.50 39.96 42.33% Mg(NO 3 ) 2 , 40 80 90 (mpt.). 45.87 53.69 57.81% Mg(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 395.) +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 23 20.5 18 35.44 36.19 38.03% Mg(NO 3 ) 2 . Cryohydrate is formed at 29. (Funk, Z. anorg. 1899, 20. 398.) Magnesium neodymium nitrate, 3Mg(NO 3 ) 2 , 2Nd(N0 3 ) 3 +24H 2 0. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 97.7 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Magnesium praseodymium nitrate, 3Mg(NO 3 ) 2 , 2Pr(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 7.70 g. hydrous salt at 16. (Jantsch.) Magnesium samarium nitrate, 3Mg(NO 3 ) 2 . Sm(NO 3 ) 3 -f-24H 2 O. (Demargay, C. R. 1900, 130. 1187.) 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 24.55 g. hydrous salt at 16. (Jantsch.) Magnesium thorium nitrate, MgTh(NO 3 ) 6 -f- H 2 O. Hydroscopic; sol. in HNO 3 . (Meyer, Z. anorg. 1901, 27. 385.) Magnesium nitrate ammonia, Mg(NO 3 )2, 6NH 3 . SI. sol. in liquid NH 3 . (Franklin, J. Am. Chem. Soc. 1913, 35. 1459.) Manganous nitrate, basic, 2MnO, N 2 O 5 -h 3H 2 0. Sol. in H 2 O. (Gorgeu.) Manganous nitrate, Mn(NO 3 ) 2 . Deliquescent. Easily sol. in H 2 O and alcohol. See +3, and 6H 2 O. Sp. gr. of Mn(NO 3 ) 2 +Aq at 8. % Mn(NOs)2 +6H 2 O Sp. gr. % Mn(N0 3 ) 2 +6H 2 O Sp. gr. 5 1.0253 45 1.2705 10 1.0517 50 1.3074 15 1.0792 55 1.3459 20 1 . 1078 60 1.3861 25 1.1137 65 1.4281 30 1 . 1688 70 1.4721 35 1.2012 71 1.4811 40 1.2352 (Oudemans, Z. anal. 7. 421.) Sp. gr. of aqueous solutions containing: 10 20 30 % Mn(NO 3 ) 2 +6H 2 0, 6.237 12.474 18.711% Mn(NO 3 ) 2 , 1.052 1.107 1.165 40 50 60 % Mn(NO 3 ) 2 +6H 2 O, 24.948 31.185 37.422% Mn(NO 3 ) 2 , 1.230 1.302 1.381 70 80 % Mn(NO 3 ) 2 -f-6H 2 O. 43.659 49.896% Mn(NO 3 ) 2 . 1.466 1.558 (Gerlach, Z. anal. 28. 477.) Sp. gr. of Mn(NO 3 ) 2 +Aq at room temp, containing: 18.309 29.602 49.309% Mn(NO 3 ) 2 . 1.1482 1.3227 1.5056 (Wagner, W. Ann. 1883, 18. 271.) NITRATE, MERCURIC 575 Sp. gr. of Mn(NO 3 ) 2 +Aq at 25. Concentration of Mn(NOs)2+Aq 1-normal Sp. gr. 1.0690 1.0349 1.0174 1.0093 (Wagner, Z. phys. Ch. 1890, 5. 39.) Sol. in liquid NH 3 . (Guntz, Bull. Soc 1909, (4) 6. 1006.) Very sol. in liquid NH 3 . (Franklin, Am Ch. J. 1898,20.828.) +H 2 O. Deliquescent. (Guntz, Bull. Soc 1909 (4) 5. 1005.) +3H 2 O. From solution in HNO 3 . (Schultz- Sellack, Zeit. Ch. 1870. 646.) Solubility in H 2 O. Sat. solution contains at: 27 29 30 34 35.5 mpt. 65.66 66.99 67.38 71.31 76.82% Mn(NO 3 ) 2 . (Funk, Z. anorg. 1899, 20. 403.) +6H 2 O. Melts in its crystal H 2 O at 25.8 and boils at 129.4. (Ordway.) Solubility in H 2 O. Sat. solution contains at: 29 26 21 16 5 42.29 43.15 44.30 45.52 48.88% Mn(NO 3 ) 2 , +11 18 25.8 mpt. 50.49 54.50 57.33 62.37% Mn(NO,) 2 . Cryohydrate is formed at 36. (Funk, Z. anorg. 1899, 20. 403.) Manganous neodymium nitrate, 3Mn(NO 3 ) 2 , 2Nd(N0 3 ) 3 +24H 2 0. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 296 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Manganous praseodymium nitrate, 3Mn(NO 3 ) 2 , 2Pr(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 23.4 g. hydrous salt at 16. (Jantsch.) Manganous samarium nitrate, 3Mn(NO 3 ) 2 , 2Sm(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 50.04 g. hydrous salt at 16. (Jantsch.) Manganous thorium nitrate, MnTh(NO 3 ) 6 -f- 8H 2 O. Ppt. (Meyer, Z. anorg. 1901, 27. 388.) Manganous nitrate cupric oxide, Mn(NO 3 ) 2 , 3CuO+3H 2 O. Ppt. (Mailhe, C. R. 1902, 134. 234.) Manganous nitrate hydrazine, Mn(NO 3 ) 2 , 2N 2 H 4 . Not decomp. by H 2 O. (Franzen, Z. anorg. 1908, 60. 286.) Mercurous nitrate, basic, 2Hg 2 O, N 2 Os+ H 2 O. Ppt. Decomp. by boiling with H 2 O. (Marignac, A. ch. (3) 27. 332.) Slowly sol. in cold, rapidly in hot HCl+Aq: insol. in NH 4 C1, and NH 4 NO 3 +Aq. + 10H 2 O. Slowly sol. in normal HNO 3 . (Reuss, Dissert. 1886.) 4Hg 2 O, 3N 2 O 6 +H 2 O. Sol. in a small quan- tity of H 2 O; decomp. by a large amt. of H 2 O or by warm H 2 O. (Rose, Pogg. 83. 154.) Is 3HgO, 2N 2 O 5 +H 2 O according to Ger- hardt. +5H 2 O. (Reuss, Dissert. 1886.) 5Hg 2 O, 3N 2 O 5 +2H 2 O. (Marignac.) Is 2Hg 2 O, N 2 O 5 +H 2 O. (Lefort, A. 56. 247.) Sol. in boiling, less sol. in cold H 2 O. (Marig- nac, L c.) +4H 2 O, and +6H 2 O. (Reuss, Dissert. 1886.) 8Hg 2 O, 5N 2 O 5 +5H 2 O, and +11H 2 O. (Reuss.) HHg 2 O, 6N 2 O 5 +25H 2 O. (Reuss.) 16Hg 2 O, 9N 2 O 6 + 19H 2 O, +23H 2 O, and +31H 2 O. (Reuss.) 3Hg 2 O,N 2 O 5 +2H 2 O. (Cox, Z. anorg. 1904, 40. 177.) Mercurous nitrate, HgNO 3 . Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Fairly sol. in boiling CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in methylamine. (Franklin, " J. Am. Chem. Soc. 1906, 28. 1419.) +H 2 O. Completely sol. in a little warm H 2 O, but decomp. by more H 2 O. Completely sol. as acid salt in H 2 O containing HNO 3 . (Marignac, A. ch. (3) 27. 332.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +1V4H 2 0, +1V.HA +W 2 H 2 0, etc. (Reuss, Dissert. 1896.) Mercuric nitrate, basic, 6HgO, N 2 O 5 (?). Insol. in hot H 2 O. (Kane.) 3HgO, N 2 O 5 +H 2 O. Decomp. to oxide by washing with cold H 2 O. Sol. in dil. HNO 3 + Aq. (Millon, A. ch. (3) 18. 361.) 2HgO, N 2 O 5 +H 2 O. SI. deliquescent. De- comp. by H 2 O; sol. in dil. HNO 3 +Aq. Millon.) +2H 2 O. Decomp. by cold H 2 O. Deli- quescent. Sol. in H 2 O containing HNO 3 . (Marignac.) +3H 2 O. (Ditte, J. B. 1854. 366.) Mercuric nitrate, Hg(NO 3 ) 2 . Very sol. in liquid NH 3 . (Franklin, Am. h. J. 1898, 20. 829.) 576 NITRATE, MERCUROMERCURIC Neither dissolved nor attacked by liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Difficultly sol. in ethyl acetate. (Naumann, B. 1910, 43^. 314.) Sol. in methylal. (Eidmann, C. C. 1899. II, 1014.) + MH 2 O. Deliquescent. Very sol. in a little H 2 O. H 2 O precipitates basic salt from cone. Hg(NO 3 ) 2 +Aq. Insol. in alcohol. Decomp. by ether. (Millon.) +H 2 O. Extraordinarily sol. in H 2 O. (Cox, Z. anorg. 1904, 40. 159.) +8H 2 O. Melts at 6 in crystal H 2 O. (Ditte.) Mercuromercuric nitrate, Hg 2 O, 2HgO, N 2 O 5 . Boiling H 2 O gradually dissolves out Hg 2 (NO 3 ) 2 , and leaves residue of HgO and Hg. ' (Brooks, Pogg. 66. 63.) 2Hg 2 O, HgO, N 2 O 6 +H 2 O. (Ray, Chem. Soc. 1905, 87. 175.) Hg 2 0, 2HgO, N 2 5 +H 2 0. (Ray.) Mercurous hydrogen nitrate, 4HgNO 3 , HNO 3 +8H 2 O. (Reuss, Dissert. 1886.) 5HgNO 3 , 3HNO 3 +26H 2 O. (Reuss.) Mercuric silver nitrate, Hg(NO 3 ) 2 , 2AgNO 3 . Easily sol. in H 2 O without decomp. (Ber- zelius.)* Mercurous strontium nitrate, 2SrO, 2Hg 2 O, 3N 2 5 . Decomp. by H 2 O. Much more sol. in H 2 O than the corresponding Ba compound. Readily sol. in warm dil. HNO 3 +Aq or Hg 2 (NO 3 ) 2 +Aq without decomposition. (Stadeler, A. 87. 131.) Mercurous thallous nitrate, HgNO 3 , T1NO 3 . Miscible with H 2 O. (Retgers, N. Jahrb. Miner, 1896. II, 183.) Mercuric nitrate bromide, Hg(NO 3 ) 2 , HgBr 2 . (Morse, Z. phys. Ch. 1902, 41. 733.) Mercuric nitrate cadmium oxide, Hg(NO 3 ) 2 , CdO+2H 2 O. Ppt. (Mailhe, Bull. Soc. 1901, (3) 26. 788.) +3H 2 O. Decomp. by H 2 O. (Mailhe.) Mercuric nitrate cobaltous oxide, Hg(NO 3 ) 2 , CoO+3H 2 O. Ppt, ' (Mailhe, C. R. 1901, 132. 1275.) +4H 2 O. Decomp. by H 2 O. (Mailhe, A. ch. 1902, (7) 27. 369.) Mercuric nitrate cupric oxide, Hg(N0 3 ) 2 , CuO+2H 2 O, and +4H 2 O. (Mailhe, Bull. Soc. 1901, (3) 25. 791.) +5H 2 O. Decomp. by H 2 O. (Mailhe, A. ch. 1902, (7) 27. 365.) ' Mercuric nitrate cyanide, Hg(NO 3 ) 2 , Hg(CN) 2 . Very sol. in H 2 O. Very sol. in methyl al- cohol and solution is not decomp. at bpt. Ethyl alcohol apparently decomp. it. (Prus- sia, Gazz. ch. it. 1898, 28. (2) 115.) Mercurous nitrate hydrazine, 2HgNO 3 , N 2 H4. Decomp. by H 2 O. Stable in dil. HNO 3 + Aq solution. (Hofmann and Marburg, A. 1899, 305. 215.) Ppt.; very unstable. (Hofmann, B. 1897, 30.2021.) Hg(NO 3 ) 2 , N 2 H 4 . Sol. in dil. HC1 and HNO 3 . (Hofmann and Marburg, A. 1899, 305. 215.) Ppt.; sol. in acids; decomp. by alkali. (Hofmann, B. 1897, 30. 2021.) Mercuric nitrate iodide, Hg(NO 3 ) 2 , 2HgI 2 . Decomp. by long boiling with H 2 O. (Rie- gel, Jahrb. Pharm. 11. 396.) 2Hg(NO 3 ) 2 , 3HgI 2 . Easily decomp. by H 2 O ; less easily by alcohol or ether. (Riegel.) Hg(NO 3 ) 2 , HgI 2 . Decomp. very quickly by HNO 3 +Aq or alcohol of 0.814 sp. gr. (Souville, J. Pharm. 26. 474.) Mercuric nitrate manganous oxide, Hg(NO 3 ) 2 , MnO+2H 2 O. Decomp. by H 2 O. (Mailhe, Bull. Soc. 1901, (3) 26. 790.) +3H 2 O. (Mailhe.) +4H 2 O. (Mailhe, A. ch. 1902, (7) 27. 370.) Mercuric nitrate nickel oxide, Hg(NO 3 ) 2 , NiO +2H 2 O. (Mailhe, Bull. Soc. 1901, (3) 25. 788.) +4H 2 O. Decomp. by H 2 O. (Mailhe, A. ch. 1902, (7) 27. 369.) Mercurous nitrate phosphate, HgNO 3 , Hg 3 P0 4 +H 2 0. Insol. in H ? O, but decomp. by boiling there- with. Insol. in H 3 PO 4 +Aq or alcohol. Com- pletely sol. in hot NH 4 Cl-hAq. Decomp. by cold KOH+Aq, and warm K 2 CO 3 +Aq. (Wittstein.) 2HgNO 3 , Hg,O, 5Hg 3 PO 4 +H 2 O. (Haack, A. 262. 192.) Mercuric nitrate silver bromide, Hg(NO 3 ) 2 , AgBr. (Morse, Z. phys. Ch. 1902, 41. 733.) NITRATE, NICKEL 577 Mercuric nitrate silver cyanide, basic, Hg(OH)NO 3 , AgCN+2H 2 O. ' (Schmidt, Z. anorg. 1895, 9. 431.) Hg(OH)NO 3 , . 5Ag 2 O, 20AgCN+7H 2 O. (Schmidt.) ^VTercuric nitrate silver iodide, Hg(N0 3 ) 2 , Decomp. by H 2 O. (Preuss, A. 29. 328.) Mercuric nitrate sulphide, Hg(NO 3 ) 2 , 2HgS. Very si. sol. in hot H 2 O. Insol. in HNO 3 + Aq. Decomp. by hot H 2 SO 4 or aqua regia, also by hot HCl+Aq. (Barfoed, J. pr. 93. 230.) Sol. in aqua regia. (Deniges, Bull. Soc. 1915, (4) 17. 355.) 2Hg(N0 3 ) 2 JftgO, 6HgS+12H 2 0. Insol. in H 2 O, and IW"O 3 +Aq of 1.2 sp. gr. (Gramp, J. pr. (2) 14. 299.) Mercuric nitrate zinc oxide, Hg(NO 3 ) 2 , ZnO-f H 2 0. Ppt. Decomp. by H 2 O. (Mailhe, C. R. 1901, 132. 1274.) Molybdenum nitrate, Mo 2 O 3 , N 2 O 6 (?). Sol. in dil. HNO 3 +Aq. (Berzelius.) MoO 2 , 2N 2 O 5 (?). Sol. in dil. HNO 3 +Aq. (Berzelius.) Neodymium nickel nitrate, 2Nd(N0 8 ) 3 , 3Ni(NO 3 ) 2 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 116.6 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Neodymium rubidium nitrate, [Nd(NO 3 ) 5 ]Rb 2 +4H 2 O. Hydroscopic. (Jantsch, Z. anorg. 1911, 69. 230.) Neodymium zinc nitrate, 2Nd(NO 3 ) 3 , 3Zn(NO 3 ) 2 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 177 g. hydrous salt at 16. (Jantsch.) Nickel nitrate, basic. Insol. in H 2 O. (Proust.) 8NiO, 2N 2 O 6 +5H 2 O. Insol. in cold or hot H 2 O. (Habermann, M. 5. 432.) 5NiO, N 2 O 5 +4H 2 O. Not decomp. by boil- ing H 2 O. (Rousseau and Tite, C. R. 114. 1184.) Nickel nitrate, Ni(NO 3 ) 2 . Solubility in H 2 O. See +3, 6, and 9H 2 O. Sp. gr. of aqueous solution at 17.5 contain- ing: 5 10 15 20 %Ni(NO 3 ) 2 , 1.0463 1.0903 1.1375 1.1935 25 30 35 40 % Ni(NO 8 ) 2 . 1.2534 1.3193 1.3896 1.4667 (Franz, J. pr. (2) 6. 295.) 91.5 g .( = 1.073 Sp. gr. of Ni(NO,;_ . Ni(NO 3 ) 2 (anhydrous) in 1000 g. H 2 O at 24.4: ' ol.) 183 274.5 369 460.5 549 1.141 1.205 1.266 1.324 1.378 (Gerlach, Z. anal. 28. 468.) Sp. gr. of Ni(NO 3 ) 2 +Aq at room temp, containing: 16.493 30.006 40.953% Ni(NO 8 ) 2 . 1.1363 1.2776 1.3879 (Wagner, W. Ann. 1883, 18. 269.) Sp. gr. of Ni(N0 3 ) 2 +Aq at 25. Concentration of Ni(NO 3 )2+Aq Sp. gr. 1-normal Vr- " 1 U- " Vs- " 1.0755 1.0381 1.0192 1.0096 (Wagner, Z. phys. Ch. 1890, 5. 39.) Sp. gr. at 20 of Ni(NO 3 ) 2 +Aq containing M g. mols. of salt per liter. M 0.01 0.025 0.05 0.075 Sp. gr. 1.001521 1.003882 1.007792 1.011541 M 0.1 0.25 0.5 0.75 Sp. gr. 1.015307 1.03837 1.07611 1.11310 M 1.0 1.5 2.0 Sp. gr. 1.14562 1.22134 1.29459 (Jones and Pearce, Am. Ch. J. 1907, 38. 720.) Sol. in liquid NH 3 . (Guntz, Bull. Soc. 1909. (4) 6. 1008.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Solubility in glycol = 7.5%. (de Coninck, C. C. 1905, II. 1234.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) +3H 2 O. Solubility in H 2 O. Sat. solution contains at: 58 60 64 70 61.61 61.99 62.76 63.95% Ni(NO 3 ) 2 , 90 95 mpt. 70.16 77.12% Ni(N0 3 ) 2 . (Funk, Z. anorg. 1899, 20. 411.) +6H 2 O. Not deliquescent in dry ah*. Sol. in 2 pts. cold H 2 O and in alcohol. (Tupputi.) Mpt. of Ni(NO 3 ) 2 +6H 2 O=56.7. (Ord- way; Tilden. Chem. Soc. 46. 409.) Sat. solution boils at 136.7. (Ordway.) Solubility in H 2 O. Sat. solution contains at: 21 12.5 10 6 39.94 41.59 42.11 43.00% Ni(NO 8 ) 2 , +20 41 56.7 mpt. 44.32 49.06 55.22 62.76% Ni(N0 3 ) 2 . (Funk, Z. anorg. 1899, 20. 410.) 578 NITRATE, NICKEL PRASEODYMIUM Sat. solution of Ni(NO 3 ) 2 +6H 2 O contains 44.3% Ni(N0 8 ) 2 at 0, and 48.7% Ni(NO 3 ) at 18. (Mylius, Z. anorg. 1912, 74. 411.) Sp. gr. of Ni(NO 3 ) 2 +Aq containing in 1000 g. H 2 O at 24.4, g. Ni(NO 3 ) 2 +6H 2 O. 145.5 g. ( = H mol.) 291 436.5 582 1.069 1.128 1.179 1.224 727.5 873 1018.5 1164 1.264 1.299 1.329 1.357 (Gerlach, Z. anal. 28. 468.) Sol. in NH 4 OH+Aq. Insol. in absolute alcohol. SI. sol. in acetone. (Krug and M'Elroy.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) +9H 2 O. Solubility in H 2 O. Sat. solution contains at: 23 21 10.5 39.02 39.48 44.13% Ni(N0 3 ) 2 . Cryohydrate is formed at 27. (Funk, Z. anorg. 1899, 20. 411.) Nickel praseodymium nitrate, 3Ni(NO 3 ) 2 , 2Pr(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 3 +Aq (sp. gr. 1.325) contains 9.28 g. hydrous salt at 16. (Jantsch, Z. anorg. 1912, 76. 303.) Nickel samarium nitrate, 3Ni(NO 3 ) 2 , 2Sm(NO 3 ) 3 +24H 2 O. 1 1. sat. solution in HNO 8 +Aq (sp. gr. 1.325) contains 29.11 g. hydrous salt at 16. (Jantsch.) Nickel thorium nitrate, NiTh(N0 3 ) 6 +8H 2 O. Sol. in HN0 3 +Aq. (Meyer, Z. anorg. 1901, 27. 387.) Nickel uranyl nitrate, 10Ni(NO 3 ) 2 , 3(U0 2 )(N0 3 ) 2 . Sol. in H 2 O and acids; insol. in aq. alkali. (Lancien, C. C. 1912, 1. 208.) Nickel nitrate ammonia, Ni(NO 3 ) 2 , 4NH 3 + 2H 2 0. Efflorescent. Easily sol. in cold H 2 O; decomp. by boiling. Insol. in alcohol. (Erdmann, J. pr. 97. 395; Ephraim, B. 1913, 46. 3106.) . (Andre, C. R. 106. 936.) Nickel nitrate chloride ammonia, 6Ni(NO 3 ) 2 , NiCl 2 , 30NH 3 +16H 2 O. Sol. in H 2 with decomp. (Schwarz, W. A. B. 1850. 272.) Nickel nitrate cupric oxide, Ni(NO 3 ) 2 , 3CuO-f 3H 2 0. Ppt. (Maihle, C. R. 1902, 134. 234.) Nickel nitrate hydrazine, Ni(NO 3 ) 2 , 3N 2 H 4 . Insol. in H 2 O. Decomp. by hot H 2 O. Easily sol. in dil. acids. (Franzen. Z. anorg. 1908, 60. 267.) Palladium nitrate, basic, Pd(NO 3 ) 2 , 3PdO +4H 2 0. Ppt. Insol. in H 2 O. (Kane.) Palladium nitrate, Pd(NO 3 ) 2 +zH 2 O. Very deliquescent, and sol. in H 2 O. De- comp. by much H 2 O or alcohol. (Kane.) Decomp. by cold or hot H 2 O. (Rose, A. 83. 143.) Platinic nitrate, Pt(NO 3 ) 4 (?). Known only in solution, which is decomp. on evaporating. (Berzelius.) Pt(NO 3 ) 2 , 3PtO 2 +5H 2 O. Insol. in H 2 0. (Prost, Bull. Soc. (2) 46. 156.) Platinum nitrate sulphocarbamide. Pt(NO 3 ) 2 , 4CS(NH 2 ) 2 . Very sol. in H 2 O. Unstable. (Kurnokow, J. pr. 1894, (2) 50. 490.) Potassium nitrate, KNO 3 . Not deliquescent, but, according to Mulder, 100 pts. KNO 3 under a bell jar with H 2 O take up 339 pts. H 2 O in 22 days, and small amounts finally deliquesce completely. Sol. in H 2 O with absorption of heat. 16 pts. KNO 3 + 100 pts. H 2 O at 13.2 lower the temperature 10.2. If the initial temp, is 23 it falls to 12.8, if it does not fall below 2.7, which is the freezing-point of the mixture. (Riidorff, Pogg. 136. 276.) KNOa+Aq sat. at 18.1 has 1.1601 sp. gr. and con- tains 22.72% KNOa, or 100 pts. H 2 O at 18.1 dissolve 29.45 pts. KNOa. (Karsten, 1840.) Sol. in 3.745 pts. H 2 O at 15. (Gerlach.) Sol. in 3 pts. HzO at 21 (Schiff, A. 109. 326), and solution has 1.1683 sp. gr. Sol. in 3 pts. cold, and 0.5 pt. boiling H2O. (Four- croy.) KNOs+Aq sat. at 18 has sp. gr. 1.151, and contains 21.63% KNOa, or 100 pts. H 2 O dissolve 27.60 pts. KNOa at 18. (Longchamp.) Sol. in 4 pts. H 2 O at 16, and 0.25 pt. at b.-pt. (Rif- fault.) 100 pts. H 2 O at 114.5 dissolve 284.61 pts. (Griffiths.) Sol. in 7 pts. cold, and 1 pt. boiling H 2 O. (Berg- mann.) Sol. in 6.15 pts. cold H 2 O at 18.75. (Abl.) 100 pts. H 2 O at 15.5 dissolve 26.6 pts.; at 100, 100 pts. (Ure's Dictionary.) KNOa+Aq sat. at 10 contains 33.3%. (Eller.) KNOa+Aq sat. in the cold contains 25%. (Four- croy.) KNOa+Aq sat. at 12.5 contains 24.8%. (Hassen- fratz.) Solubility of KNO 3 in 100 pts. H 2 O at t. t Pts. KNOa t Pts. KNO 5 11.67 17.91 24.94 13.2 16.7 22.2 29.3 38.4 45.10 54.72 65.45 79.72 97.66 74.7 97.1 125.5 169.2 236.4 (Gay-Lussac, A. ch. 11. 314.) NITRATE, POTASSIUM 579 Solubility of KNO 3 in 100 pts. H 2 O at t. t Pts. KNOs 16.0 29 44.2 26.7 43.5 71.4 (Nordenskjold, Pogg. 136. 312.) 100 pts. H 2 O dissolve at: 10 18 27 41 53 21.2 27.9 40.1 66.3 93.3 pts. KNO 3 . (Gerardin, A. ch. (4) 6. 150.) 100 pts. KNO 3 +Aq sat. at 14 contain 16.34 pts. KNO 3 ; at 15, 18.81 pts. KNO 3 . (v. Hauer, J. pr. 98. 177.) 100 pts. H 2 O dissolve at: 4 16.3 68.3 16 27.2 132.1 pts. KNO 3 . (Andreae, J. pr. (2) 29. 456.) Solubility in 100 pts. H 2 O at t. t Pts KNOs t Pts. KNOs t Pts. KNOs 13.3 39 62 78 165 1 13.8 40 64 79 168 2 14.6 41 66 80 172 3 15.5 42 68 81 175 4 16.4 43 70 82 179 5 17.1 44 72 83 182 6 17.8 45 74 84 185 7 18.5 46 76 85 189 8 19.3 47 78 86 192 9 20.2 48 81 87 196 10 21.1 49 83 88 199 11 22.0 50 86 89 203 12 23.0 51 88 90 206 13 24.0 52 91 91 210 14 25.0 53 93 92 214 15 26.0 54 96 93 218 16 27.0 55 98 94 222 17 28.1 56 101 95 226 18 29.1 57 103 96 230 19 30.2 58 106 97 234 20 31.2 59 108 98 238 21 32.3 60 111 99 243 22 33.5 61 113 100 247 23 34.7 62 116 101 252 24 36.0 63 119 102 256 25 37.3 64 121 103 261 26 38.6 65 124 104 266 27 40.0 66 127 105 272 28 41.4 67 130 106 278 29 42.9 68 133 107 284 30 44.5 69 136 108 289 31 46.0 70 139 109 295 32 48 71 142 110 301 33 50 72 146 111 307 34 52 73 149 112 313 35 54 74 152 113 319 36 56 75 155 114 326 37 58 76 159 114.1 327.4 38 60 77 162 (Mulder, Scheik. Verhandel. 1864. 89.) 100 pts. H 2 O dissolve 493 pts. KNO 3 at 125. (Tilden and Shenstone, Phil. Trans. 1884. 23.) Rhombohedral KNO 3 is more easily soluble than the prismatic, and easily forms super- saturated solutions. (Frankenheim.) Sat. KNO 3 +Aq contains at: 139 158 160 175 180 79.8 83.7 83.9 84.0 84.2% KNO 3 . 190 215 225 258 283 86.0 89.0 90.4 91.6 96.5% KNO 3 . (fitard, A. ch. 1894, (7) 2. 526.) Solubility in 100 pts. H 2 at t. t G. KN0 3 0.40 13.43 14.90 25.78 30.80 47.52 44.75 74.50 60.05 111.18 76 156.61 91.65 210.20 114* 311.64 Sp. gr.t/4 e 1.0817 1 . 1389 1.2218 1.3043 1.3903 1.4700 1.5394 1.6269 * B.-pt. of sat. solution. (Berkeley, Phil. Trans. 1904, 203, A, 189.) 100 g. H 2 O dissolve 37.79 g. KNO 3 at 25. 100 g. H 2 O dissolve 3.08 g. equiv. KNO 3 at 20; 3.27 at 21.5. (Euler, Z. phys. Ch. 1904, 49. 312.) 1 1. H 2 O dissolves 384.48 g. KNO 3 at 25. (Armstrong and Eyre, Proc. Roy. Soc. 1910, A, 84. 123.) 1 1. sat. KNOs+Aq contains 2.8 g. mols. KNO 3 . (Rosenheim and Weinheber, Z. anorg. 1911, 69. 263.) 100 g. H 2 O dissolve 38.485 g. KNO 3 at 25. (Haigh, J. Am. Chem. Soc. 1912, 34. 1148.) Sat. KNO 3 +Aq contains at: 50 58 62 68 46.39 51.55 53.64 57.04% KNO 3 . (Tschugaeff, Z. anorg. 1914, 86. 160.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 9.1 21.1 35 16.76 24.77 35.01 g. KNO 3 . (Findlay, Chem. Soc. 1914, 105. 780.) Sp. gr. of solution sat. at 15 = 1.134. (Michel and Krafft.) Sp. gr. of solution sat. at 16 = 1.138. (Stolba, J. pr. 97. 503.) Sp. gr. of solution sat. at 18 = 1.1601, and contains 29.45% KNO 3 . (Karsten.) Sp. gr. of KNO 3 +Aq at 19.5. % KNOs Sp. gr. % KNOs . Sp. gr. 4.871 9.618 14.044 1.0307 1.0618 1.0920 17.965 21.488 1.1198 1.1457 (Kremers, Pogg. 95. 120.) 580 NITRATE, POTASSIUM Sp. gr. of KNO 3 +Aq at 21. Sp. gr. of KNO 3 +Aq at 25. % KNOs Sp. gr. % KNOs Sp. gr. Concentration of KNOs+Aq. Sp. gr. ^ 1 2 3 4 5 6 7 8 9 10 11 12 1.0058 1.0118 1.0178 .0239 .0300 .0363 .0425 .0490 .0555 .0621 .0686 1.0752 13 14 15 16 17 18 19 20 21 22 23 24 1 1 1 1 1 1 1 1 1 1 1 1 .0819 .0887 .0956 .1026 .1097 .1169 .1242 .1316 .1390 .1464 .1538 .1613 1-normal I/*- ;; 1.0605 1.0305 1.0161 1.0075 (Wagner, Sp. gr. ( p = per cent served density percc -(l55 =1 Z. phys. Ch. 18 )f KNO 3 +Aqa strength of sc 90, 5. 37.) t 20.1. Jution; d=ob- ;onc. in grams (Schiff, A. 110. 75.) Sp. gr. of KNO 3 +Aq at 15. % KNOs Sp. gr. % KNOs Sp. gr. P d w 1 2 3 4 5 6 7 8 9 10 11 .00641 .01283 .01924 .02566 .03207 .03870 .04534 .05197 .05861 .06524 .07215 12 13 14 15 16 17 18 19 20 21 1. 1. 1. 1. 1. 1. 1. 1. 1. 1. 07905 08596 09286 09977 10701 11426 12150 12875 13599 14361 25.54 21.95 17.88 13.93 8.706 5.393 4.389 2.848 2.030 0.741 1 . 1783 1.1510 1.1200 1.0913 1.0553 1.0331 1.0264 1.0165 1.0113 1.0030 0.30095 0.25270 0.20033 0.15203 0.09186 0.05571 0.04506 0.02895 0.02053 0.00743 (Gerlach, Z. anal. 8. 286.) Sp. gr. of KNO 3 +Aq at 17.5. (Barnes, J. Phys. Chem. 1898, 2. 544.) Sp. gr. 20/4 of a normal solution of KN0 3 = 1.05954; of a 0.5 normal solution = 1.029325. (Haigh, J. Am. Chem. Soc. 1912, 34. 1151.) Sp. gr. of sat. KNO 3 +Aq at t. KN^bs S P-^' KNOs Sp. gr. K ^ 0j Sp. gr. 1 . 1.006 8 2 .012 9 3 .019 10 4 .025 11 5 .032 12 6 .038 13 7 .045 14 1.051 15 1.058 16 1.065 17 1.072 18 1.078 19 1.085 20 1.092 1.099 1.106 1.113 1.120 1.127 1.134 t G. KNOs sol. in 100 g. H 2 Sp. gr. G 10 20 30 40 50 60 70 13.27 20.89 31.59 45.85 63.90 85.51 109.00 138.00 .084 .120 .161 .212 .282 .339 .403 1.446 (Hager, Comm. 1883.) Sp. gr. of KNO 3 +Aq at 18. % KNOs Sp. gr. ^ % KNOs Sp. gr. 5 10 15 1.0305 1 . 0632 1.097 20 22 1.133 1.148 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of KNO 3 +Aq at 20, containing mols. KNO 3 in 100 mols. H 2 O. (Tschernaj, J. Russ. Phys. Chem. Soc. 1912, 44. 1565.) The saturated solution boils at 114.1 (Mul- der); 114.5 (Griffiths); 115.9 (Legrand, Ger- ardin); 117 (Magnus); 118 (Kremers); 126 (Le Page). The saturated solution forms a crust at 111, and boils at 115; highest temp, ob- served, 115.3. (Gerlach, Z. anal. 26. 426.) Mols. KNOs Sp. gr. Mols. KNOs Sp. gr. 0.5 1 2 1.01730 1.03373 1.06524 4 5 1 1 . 12264 . 14888 (Nicol, Phil. Mag. (5) 16. 122.) NITRATE, POTASSIUM 581 B.-pt of KNO+Aq containing pts. KNO 3 to 100 pts. H 2 O. G = according to Gerlach (Z. anal. 26. 444); L = according to Legrand (A. ch. (2) 62. 426). B.-pt. G L B.-pt. G L 100.5 7.5 107 120.5 119.0 101 15.2 i2.'2 108 141.5 140.6 101.5 23 109 164 163.0 102 31 26\4 110 188.5 185.9 102.5 39 111 215 209.2 103 47.5 42^2 112 243 233.0 103.5 56 113 274 257.6 104 64.5 5oth salts in seated with treated with simultaneou ve 31.44 pts. pts. NaCl at excess. KNO 3 . NaCl. sly treated KNO 3 , 139 15.6, and Page and (Touren, C. R. 1900, 130. 909.) r. = 1.33. NITRATE, POTASSIUM 585 Solubility in NaCl+Aq at t. without pptn., but K 2 SO 4 is afterwards pptd. Sat. solution contains (Karsten.) t % KNOs % NaCl % total salt 22 1Q F: 7.3 7 Q 22.5 OQ * 29.8 Qn a 100 pts. i 2 u dissolve: 15.5 / . \) 8.7 22' 1 O(J. O 31.8 Mulder Karsten Kopp Mulder 7 10.1 22.5 32.6 18.75 18.75 ' 20o 40 emf atronortVi rvf anln+irm r\ nVioamrorl UTOUO1VJ y " V WilA-LAO^ \s\J\j* AXi ^,J. tl'J.J.J.0 ^SlsJ. W. /Pd \ Zinc nitrate ammonia, Zn(N0 3 ) 2 , 4NH 3 . (ioo =w -) Ppt. (Ephraim, B. 1915, 48. 638.) \ / + 2 / 3 H 2 0. p d w Deliquescent. Sol. in H 2 O. (Andre, C. R. 100. 639.) 47.28 1.5504 0.73310 13ZnO, 3N 2 O 6 , 2NH 3 + 18H 2 O. 41.32 1.4579 0.60240 Insol. in cold, decomp. by warm H 2 0. 30.86 1.3136 0.40535 (Andre, C. R. 1885, 100. 640.) 29.21 1.2933 0.37780 19.65 14.39 11.36 7.091 1.1830 1 . 1284 1.0988 1.0597 0.23246 0.16232 0.12478 0.07515 Zinc nitrate cupric oxide, Zn(NO 3 ) 2 , 3CuO+3H 2 O. (Mailhe, A. ch. 1902, (7) 27. 169.) 5.923 1.0491 0.06213 1.574 1.0118 0.01593 Zinc nitrate hydrazine, Zn(NO 8 ) 2 , 3N 2 H 4 . 1.210 1.0087 0.01221 Decomp. by hot H 2 O. (Barnes, J. Phys. Chem. 1898, 2. 545.) Sol. in NH 4 OH. (Franzen, Z. anorg. 1908, 60. 279.) Zirconium nitrate, basic, 3ZrO 2 , 2N 2 O 6 . Insol. in H 2 O. ZrO 2 , N 2 O 5 . Easily sol. in H 2 O and alcohol. +H 2 O. As above. Zirconium nitrate, Zr(NO 3 ) 4 +5H 2 O (?). Deliquescent, and sol. in H 2 O. Nitric oxide, NO. See Nitrogen dioxide. 604 NITRILOBROMOSMIC ACID Nitrilobromosmic acid. Ammonium nitri [OsNBr 5 ](NH 4 ) 2 +H 2 0. Very sol. in H 2 O. Decomp. in dil. aq. solution. Stable in HBr+Aq. Insol. in organic solvents. (Werner, B. 1906, 39. 501.) Caesium hydrogen nitrilopefttabromosmate, [OsNBr 5 ] 2 Cs 3 H. SI. sol. in H 2 O. (Werner.) Potassium nitrilotefrabromosmate. [OsNBr 4 ]K+2H 2 O. Very sol. in H 2 O. Decomp. in aq. solution. Stable in HBr+Aq. Insol. in organic sol- vents. (Werner.) Rubidium nitrilope^tobromosmate. [OsNBr 5 ]Rb 2 . Sol. in H 2 O. Decomp. in dil. aq. solution after a short time. (Werner.) Nitrilochlorosmic acid. Ammonium mtrilopen^ochlorosmate. (OsNCl 6 )(NH 4 ) 2 . Sol. in H 2 O; insol. in cone. HCl+Aq. (Werner, B. 1901, 34. 2702.) Cassium nitriloper^ochlorosmate. (OsNCl 6 )Cs 2 . Sol. in H 2 O. (Werner.) Potassium nitrilopenZachlorosmate. (OsNCl 6 )K 2 . Sol. in H 2 O; pptd. by HC1; insol. in organic solvents. (Werner.) Rubidium nitrilope^achlorosmate. (OsNCl 6 )Rb 2 . Sol. in H 2 O; decomp. in dil. neutral solu- tion. (Werner.) Nitrilofrimetaphosphoric acid. H 2 NP 3 O 7 = PO .OH PO < OH. Known only in solution. (Mente, A. 248. 260.) Aluminum nitriloZnwetaphosphate. Insol. in H 2 O, cone. HC1, or HNO 3 +Aq. Slowly sol. in boiling cone. H 2 SO 4 . Sol. in warm NaOH+Aq or Na 2 CO 3 +Aq without decomp. Insol. in NH 4 OH+Aq. (Mente.) Barium - , BaNP 3 O 7 . Insol. in dil. or cone, acids. Decomp. by boiling NaOH or Na 2 CO 3 +Aq. Insol. in NH 4 OH+Aq. (Mente.) Cadmium nitrilofriwetaphosphate. Easily sol. in NH 4 OH+Aq, or boiling (NH 4 ) 2 CO 3 , or NaOH+Aq. (Mente.) Calcium , CaNP 3 O 7 +H 2 O. Sol. in cone. HCl+Aq by long boiling, and more easily in fuming HNO 3 +Aq. Insol. in NH 4 OH or NaOH+Aq. (Mente.) Chromium . Slowly sol. in dil. acids. Easily sol. in ammonia. Sol. in cold NaOH +Aq. (Mente.) Cobalt , CoNP 3 O 7 +H 2 O. Insol. in H 2 O. SI. sol. in dil. acids. Easily sol. in NH 4 OH+Aq. Decomp. by NaOH or Na 2 CO 3 +Aq. (Mente.) Copper -. Sol. in NH 4 OH+Aq. Decomp. by NaOH +Aq. (Mente.) Ferric , Fe 2 (NP 3 O 7 ) 3 . Insol. in cone, acids. Easily sol. in NH 4 OH +Aq or (NH 4 ) 2 CO 3 +Aq. Decomp. by NaOH or Na 2 CO 3 +Aq. (Mente.) Lead . Insol. in dil. acids. Sol. in fuming HNO 3 . Insol. in NH 4 OH+Aq. Sol. in NaOH+Aq. (Mente.) Magnesium , MgNP 3 O 7 +H 2 O. Slowly sol. in HCl+Aq. Sol. in H 2 SO 4 or fuming HNO 3 with addition of Br 2 . Insol. inNH 4 OHor(NH 4 ) 2 CO 3 +Aq. (Mente.) Manganous , MnNP 3 7 +H 2 O. Insol. in dil. acids. Very si. sol. in NaOH+ Aq. Insol. in Na 2 CO 3 or (NH 4 ) 2 CO 3 +Aq. Easily sol. in NH 4 OH+Aq. (Mente.) Mercurous , Hg 2 NP 3 O 7 . Insol. in dil. acids, NH 4 OH, NaOH, or (NH 4 ) 2 CO 3 +Aq. Easily sol. in fuming HN0 3 . (Mente.) Nickel -, NiNP 3 O 7 +H 2 O. Insol. in dil. acids, NH 4 OH, or (NH 4 ) 2 CO 3 +Aq. (Mente.) Zinc , ZnNP 3 O 7 +2H 2 O. Easily sol. in NH 4 OH, NaOH, or (NH 4 ) 2 C0 3 +Aq. (Mente.) Nitrilosulphonic acid, N(SO 3 H) 3 . Not known in free state. (Raschig, A. 241. 161.) Potassium nitrilosulphonate, N(SO 3 K) 3 + 2H 2 O. Soluble in H 2 O. (Raschig, A. 241. 161.) Is identical with "potassium ammoninsul- phonate" of Claus. NITROGEN 605 Insol. in cold H 2 O (Glaus); sol. in 50 pts. H 2 O at 23 (Fremy); in H 2 O at scarcely 40 without change. Decomp. by boiling. (Glaus.) Potassium sodium nitrilosulphonate, N(SO,K),(SO,Na). Nearly insol. in cold H 2 O. (Raschig, A. 241. 161.) Sodium nitrilosulphonate, N(SO 3 Na) 3 . Not isolated on account of its extreme solubility in H 2 O. (Raschig, A. 241. 161.) Nitrilocto'sulphophosphoric acid, NP(SH) 2 . Decomp. by H 2 O. (Stock, B. 1906, 39. 2001.) Ammonium mtrilocfasulphophosphate, NP(SNH 4 ) 2 . Easily sol. in H 2 O. Not decomp. by boiling with alkali. Decomp. by acid. (Stock.) Easily sol. in liquid NH 3 . (Stock, B. 1903, 36. 315.) Ammomum hydrogen nitrilotfisulphophos- phate, SHP(SNH 4 )N. Not decomp. by boiling with alkali. De- comp. by acids. (Stock, B. 1906, 39. 1999.) Barium nitrilodisulphophosphate, BaNPS 2 + H 2 0. Sol. in H 2 O with decomp. Decomp. by hot H 2 O. Not decomp. by warming with alkali. Decomp. by acid. (Stock.) Lead nitrilocfa'sulphophosphate, NPS 2 Pb. Sol. in liquid NH 3 . Solution decomp. rapidly with separation of PbS. (Stock.) Sodium nitriloc&sulphophosphate, NPSNa 2 . Not decomp. by boiling with alkali. De- comp. by acid. (Stock.) Nitrilosulphuric acid. Ammonium nitrilosulphate, N(SO 3 NH 4 ) 3 + 2H 2 O. Rather si. sol. in H 2 O, but much more sol. than K salt. (Divers and Haga, Chem. Soc. 1901, 79. 1094.) Sodium nitrilosulphate, N(SO 3 Na) 3 +5H 2 O. Very sol. in H 2 O. (Divers and Haga, Chem. Soc. 1901, 79. 1097.) Nitrilosulphurous acid. Ammomum nitrilosulphite, NH(SO 2 NH 4 ) 2 . Somewhat deliquescent. Very sol. in H 2 O. Slowly decomp. in solution. Decomp. by boiling with HC1. (Divers, Proc. Chem. Soc. 1901, 17. 163.) Nitritocobaltic chloride. Sol. in 200 pts. cold H' 2 O. anorg. 6. 172.) (Jorgensen, Z. Nitritoplatincfo'amine nitrate, (N0 2 ) 2 Pt(N 2 H 6 N0 3 ) 2 . Sol. in cold H 2 O with decomp.; violently decomp. on warming. (Hadow, Chem. Soc. (2) 4. 345.) Nitritopurpureocobaltic comps. See Xanthocobaltic comps. Nitritopurpureorhodium comps. See Xanthorhodium comps. Nitrocarbamic acid. Potassium mtrocarbamate, NO 2 .NK. COOK. Decomp. by H 2 O. (Thiele, B. 1894, 27. 1909.) Nitro cobalt, Co 2 NO 2 . Decomp. by H 2 O. (Sabatier and Sender- ens, C. R. 115. 236.) Nitro copper, CuNO 2 . Violently decomp. by H 2 O. (Sabatier and Senderens, C. R. 116. 756.) Nitroferricyanhydric acid. See Nitroprussic acid. Nitrogen, N 2 . Nearly insol. in all known solvents. 1 vol. recently boiled HzO absorbs 0.0147 vol. N at 15.5. (Henry, 1803.) 1 vol. recently boiled H 2 O absorbs 0.025 vol. N. (Dalton.) 1 vol. recently boiled H2O absorbs 0.0156 vol. N at ord. temp. (Dalton.) 1 vol. H 2 O at t and 760 mm. absorbs V vols. N gas reduced to and 760 mm. t v t V t V 0.02035 7 0.01713 14 0.01500 1 0.01981 8 0.01675 15 0.01478 2 0.01932 9 0.01640 16 0.01458 3 0.01884 10 0.01607 17 0.01441 4 0.01838 11 0.01577 18 0.01426 5 0.01794 12 0.01549 19 0.01413 6 0.01752 13 0.01523 20 0.01403 (Bunsen.) Coefficient of absorption = 0.020346- 0.00053887t +0.00001 1156t 2 . (Bunsen.) 606 NITROGEN 1 1. H 2 O absorbs ccm. N from atmospheric air at 760 mm. pressure and t. 5 10 ccm. N 19.29 17.09 15.36 15 20 25 ccm. N 13.95 12.80 11.81 (Dittmar, Challenger Exped. Report, vol. i.) 5 10 ccm. N 19.14 16.93 15.14 15 20 25 ccm. N 13.73 12.63 11.80 (Hamberg, 1885.) Absorption of N by H 2 O at t and 760 mm )8 = coefficient of absorption. t ft t ft t ft 0.02388 18 0.01696 36 0.01252 1 2337 19 1667 37 1233 2 2288 20 1639 38 1215 3 2241 21 1611 39 1198 4 2196 22 1584 40 1182 5 2153 23 1557 41 1166 6 2111 24 1530 42 1151 7 2070 25 1504 43 1137 8 2031 26 1478 44 1124 9 1993 27 1453 45 1111 10 1956 28 1428 46 1099 11 1920 29 1404 47 1088 12 1885 30 1380 48 1078 13 1851 31 1357 49 1069 14 1818 32 1334 50 1061 15 1786 33 1312 60 1000 16 1755 34 1291 100 1000 17 1725 35 1271 (Bohr and Bock, W. Ann. 44. 318.) Absorption of N by H 2 O at t and 760 mm ft = coefficient of absorption; fti = " Solu- bility" (see under Oxygen). t ft ft 0.02348 0.02334 1 2291 2276 2 2236 2220 3 2182 2166 4 2130 2113 5 2081 2063 6 2032 2013 7 1986 "1966 8 1941 1920 9 1898 1877 10 1857 1834 11 1819 1795 12 1782 1758 13 1747 1722 14 1714 1687 Absorption of N by H 2 O at t. Continued. ^ ft ft 15 0.1682 0.1654 16 1651 1622 17 1622 1591 18 1594 1562 19 1567 1534 20 1542 1507 21 1519 1482 22 1496 1457 23 1473 1433 24 1452 1410 25 1432 1387 26 1411 1365 27 1392 1344 28 1374 1323 29 1356 1303 30 1340 1284 31 1321 1263 32 1304 1243 33 1287 1224 34 1270 1204 35 1254 1185 36 1239 1167 37 1224 1149 38 1210 1131 39 1196 1114 40 1183 1097 41 1171 1082 42 1160 1067 43 1149 1052 44 1139 1037 45 1129 1023 46 1120 1009 47 1111 0995 48 1102 0982 49 1094 0968 50 1087 0955 52 1072 0929 54 1058 0902 56 1045 0876 58 1033 0849 60 1022 0822 62 1011 0794 64 1001 0765 66 0992 0736 68 0983 0707 70 0976 0676 72 0970 0645 74 0965 0614 76 0961 0581 78 0959 0546 80 0957 0510 82 0956 0472 84 0955 0432 86 0954 0388 88 0953 0343 90 0952 0294 92 0951 0242 94 0950 0187 96 0949 0128 98 0948 0086 100 0947 0000 (Winkler, B. 24. 3606.) NITROGEN 607 Coefficient of absorption for H 2 O =0 01432 at 25; 0.01621 at 20; 0.01789 at 15: 0.02003 at 10; 0.02173 at 5. (Braun, Z phys. Ch. 1900, 33. 730.) Solubility in H 2 O at various pressures. V= volume of the absorbing liquid. P = Hg-pressure in metres. X = coefficient of solubility. Absorption of N 2 by distilled H 2 O at t. a = ccm. of N 2 absorbed by 1 1. of H 2 O at t and 760 mm. t a t a t a 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 23.00 22.50 22.02 21.55 21.09 20.64 20.20 19.77 19.35 18.94 18.54 18.16 17.80 17.46 17.14 16.84 16.56 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 16.29 16.03 15.78 15.54 15.29 15.06 14.84 14.63 14.43 14.23 14.04 13.87 13.71 13.55 13.39 13.23 13.08 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 12.93 12.79 12.65 12.52 12.39 12.27 12.15 12.04 11.92 11.80 11.68 11.57 11.46 11.35 11.24 11.13 11.02 V t p X 33. 134 com. 19.4 0.8910 1.0453 1.2488 1.4764 1.8111 2.3961 2.9074 3.3411 4.1382 4.5958 5.1103 5.8349 6.2767 7.1059 7.5815 8.1074 0.01617 0.01616 0.01611 0.01608 0.01602 0.01597 0.01585 0.01579 0.01561 0.01554 0.01546 0.01528 0.01515 0.01499 0.01487 0.01473 (Fox, Trans. Faraday Soc. 1909, 5. 73.) Solubility in H 2 O at 25 = 0. 1561 . (Drucker and Moles, Z. phys. Ch. 1910, 75. 418.) Solubility of N 2 in H 2 O at 25 =0.0231. (Calculated according to special formula, for which see original article.) (Findlay and Creighton, Chem. Soc. 1911, 99. 1315.) Coefficient of absorption for H 2 O= 0.01689 at 15; 0.01670 at 16.2; 0.01622 at 17.2. (Muller, Z. phys. Ch. 1912, 81. 493.) 1 1. sea water (sp. gr. 1.027) absorbs com. N from atmosphere at t and 760 mm. pressure 32.152ccm. 24.9 0.8977 1.0129 1.1887 1.5573 1 . 9846 2.5171 2.8781 3.2956 4.0947 4.5581 5.0529 5.5935 6.1956 7.0333 7.5596 ? 4 . 1846 0.01498 0.01493 0.01491 0.01487 0.01482 0.01478 0.01463 0.01455 0.01440 0.01434 0.01426 0.01413 0.01408 0.01382 0.01377 0.01369 t According to Tornoe According to Dittmar According to Hamberg 5 10 15 20 25 14.40 13.25 12.10 10.95 15.60 13.86 12.47 11.34 10.41 9.62 14.85 13.32 12.06 11.04 10.25 9.62 (Cassuto, Phys. Zeit. 1904, 6. 236.) Coefficient of absorption for H 2 O =0.01565 at 20.18. (Hiifner, Z. phys. Ch. 1907, 57. 615.) No. of ccm. of N 2 (containing 1.185% argon) absorbed by a 1. of sea- water from a free dry atmosphere of 760 mm. pressure at given temperatures. Cl per 1000 0* 4 17.02 16.27 15.51 14.75 14.00 13.24 8 12 16 20 24 28 4 8 12 16 20 18.64 17.77 16.90 16.03 15.18 14.31 15.63 14.98 14.32 13.66 13. on 12.34 14.45 13.88 13.30 12.72 12.15 11.57 13.45 12.94 12.44 11.93 11.73 10.92 12.59 12.15 11.70 11.25 10.81 10.36 11.86 11.46 11.07 10.67 10.27 9.87 11.25 10.89 10.52 10.16 9.80 9.44 (Fox, Trans. Faraday Soc. 1909, 5. 77.) NITROGEN Absorption of N 2 by H 2 SO 4 +Aq at t. 1 vol. alcohol at t and 760 mm. dissolves V a = coefficient of absorption. vols. N gas reduced to and 760 mm. t V t V Normality of the acid t a o 0.12634 13 0. 12192 20.9 0.0156 1 Q! 12593 14 0^12166 4.9 20.9 0.0091 2 0.12553 15 0.12142 8.9 20.9 0.0072 3 0.12514 16 0.12119 10.7 21.2 0.0066 4 0.12476 17 0.12097 20.3 21.1 0.0049 5 0.12440 18 0.12076 24.8 21.5 0.0048 6 0.12405 19 0.12056 29.6 20.8 0.0051 7 0.12371 20 0.12030 34.3 20.9 0.0100 8 0.12338 21 0.12021 35.8 21.1 0.0129 9 0.12306 22 0.12005 10 12276 23 0. 11990 (Bohr, Z. phys. Ch. 1910, 71. 49.) 11 12 o! 12247 0.12219 24 o! 11976 Absorption of N 2 by BaCl 2 +Aq. at = coefficient of absorption at t. (Bunsen's Gasometry.) 1 vol. alcohol absorbs 0.126338-0.000418t+ 0.0000060t 2 vols. N gas. (Carius, A. 94. 136.) Per cent of BaCh in a25 a20 al5 alO a5 Solubility in alcohol at 25. the solution Vol. H 2 Vol. % alcohol Solubility 13.830 0.00783 0.00923 0.01036 0.01166 0.01270 11.927 0.00855 0.00976 0.01139 0.01249 0.01368 100 0.01634 6.903 6.738 3.870 0.01044 0.01036 0.01137 0.01184 0.01182 0.01323 0.01317 0.01340 0.01480 0.01474 0.01494 0.01660 0.01598 0.01628 0.01802 80 67 20 33 0.01536 0.01719 3.325 0.01190 0.01346 0.01502 0.01681 0.01826 100 0.1432 (Braun, Z. phys. Ch. 1900, 33. 733.) Absorption of N 2 by NaCl+Aq. ot = coefficient of absorption at t. (Just, Z. phys. Ch. 1901, 37. 361.) 1 vol. ether absorbs 0.15 vol. N (Dobereiner) ; 1 vol. caoutchine absorbs 5 vols. N in 5 weeks (Himly). Solubility of N 2 in ether = 0.2580 at 0; 0.2561 at 10. (Christoff, Z. phys. Ch. 1912, 79. 459.) Per cent of NaCl in the solution a25 a20 al5 alO ao Solubility in organic solvents Solvent Solubility at 25 C. Solu- bility at20C. ds dt 11.732 10.945 8.135 8.033 6.595 6.400 4.196 3.880 2.120 2.100 0.686 0.671 0.00470 0.00565 0.00749 0.00729 0.00802 . 00826 0.00990 0.01005 0.01131 0.01133 0.01295 0.01304 0.00657 0.00703 0.00872 0.00871 0.00972 . 00975 0.01151 0.01168 0.01311 0.01314 0.01477 0.01484 0.00810 0.00824 0.01014 0.00995 0.01120 0.01134 0.01294 0.01316 0.01469 0.01467 0.01640 0.01642 0.00930 0.00912 0.01131 0.01121 0.01252 0.01259 0.01451 0.01475 0.01638 0.01656 0.01833 0.01845 0.01016 0.01052 0.01266 0.01248 0.01380 0.01375 0.01579 0.01615 0.01795 0.01805 0.01994 0.02000 Glycerine Water Aniline Carbon bisulphide Nitrobenzene Benzene Glacial acetic acid Xylene Amyl alcohol Toluene Chloroform Methyl alcohol Ethyl alcohol (99.8%) Acetone Amyl acetate Ethyl acetate Isobutyl aceate Not measurable 0.01634 0.03074 0.05860 0.06255 0.1159 0.1190 0.1217 0.1225 0.1235 0.1348 0.1415 0.1432 0.1460 0.1542 0.1727 0.1734 . 01705 0.02992 . 05290 0.06082 0.114 0.1172 0.1185 0.1208 0:1186 0.1282 0.1348 0.1400 0.1383 0.1512 0.1678 0.1701 0.000142 +0.000164 +0.00114 +0.000346 +0.0009 +0.00036 +0 . 00062 +0.00034 +0 . 00098 +0.00132 +0 . 00134 +0.00064 +0.00154 +0.0006 +0 . 00098 +0.00066 (Braun, I c.) At 191.5 liquid oxygen dissolves 458 t.iTYiAH ifs vrl rvr RC\ 7 rvr r>onf rf i+a ixroinrlit nf gaseous nitrogen. (Erdmann, B. 1904, 37. 1191.) At 18 and 760 mm. 100 vols. H 2 O or alcohol of 0.84 sp. gr. absorb 4.2 vols. N gas. (de Saussure, 1814.) (Just, Z. phys. Ch. 1901, 37. 361.) Coefficient of absorption for petroleum = 0.117 at 20; 0.135, at 10. (Gniewasz and Walfisz, Z. phys. Ch. 1. 70.) NITROGEN 609 Absorption of N2 by propionic acid+Aq. at = coefficient of absorption at t. Absorption of N 2 by organic substances +Aq at 15. P = % of the organic substance in the sol- vent. /315 = coefficient of absorption at 15. S15 = Solubility at 15, Per cent of propionic acid in the solution <*25 a20 al5 alO a 5 11.220 11.023 9.537 9.155 6.066 5.891 4.081 3.816 0.01301 0.01295 0.01336 0.01329 0.01335 0.01338 0.01365 0.01371 0.01463 0.01447 0.01471 0.01469 0.01476 0.01480 0.01541 0.01547 0.01593 0.01585 0.01634 0.01630 0.01637 0.01648 0.01688 0.01674 0.01779 0.01800 0.01823 0.01845 0.01855 0.01872 0.01919 0.01915 0.01951 0.01977 0.02040 0.02026 0.02077 0.02089 0.02095 0.02087 Organic substance used p M| S15 Chloralhydrate 6.9 14.0 15.0 23.6 26.1 37.6 48.9 49.3 61.3 70.9 71.2 78.3 79.1 0.01725 0.01675 0.01706 0.0164 0.0154 0.0152 0.0134 0.0141 0.0123 0.0115 0.0118 0.0114 0.0131 0.0130 0.0152 0.0156 O.oi796 O.oi73 0.0162 0.0160 0.0141 0.0149 0.0130 0.0121 0.0124 0.0120 0.0138 0.0137 0.0160 0.0165 (Braun, Z. phys. Ch. 1900, 33. 732.) Solubility of N2 in isobutyric acid+Aq at t. P = Corrected pressure at end of experi- ment in mm. Hg at 0. S = Solubility of N 2 . Solvent t P 8 Pure isobutyric acid 25.05 262.6 388.3 566.1 662.4 783.5 832.2 0.1609(?) 0.1640 0.1647 0.1656 0.1656 0.1656 Glycerine 15.7 15.7 29.9 46.6 57.6 67.1 72.8 74.7 77.0 85.1 87.3 88.5 99.25 0.01707 0.01708 0.01425 0.01376 0.01087 0.00840 0.00698 0.00635 0.00552 0.00597 0.00527 0.00482 0.00492 0.00536 0.00524 37.5% solution of isobutyric acid+Aq Vapor pressure = 21.6 mm. 23.02 246 492 563 836 867 2 2 6 3 3 0.0393 0.0393 0.0393 0.0400 0.0401 it Vapor pressure = 30.6 mm. 29.02 231 468.4 480.7 536 656 720 0.0373 0.0384 0.0383 0.0385 0.0384 0.0386 (Drucker and Moles, Z. phys. Ch. 1910, 76. 434.) Absorption of N 2 by chloralhydrate+Aq. t = temp. of the solution. P = % chloralhydrate in the solution. /3t = coefficient of absorption at t. 01 5 = coefficient of absorption at 15. (Hammel, Z. phys. Ch. 1915, 90. 121.) Absorption of N 2 by glycerine +Aq. t = temp. of the solution. P = % glycerine in the solution. /3t = coefficient of absorption at t: 015 = coefficient of absorption at 15. t P /3t /3i5 15.6 15.4 16.4 16.9 17.0 15.3 14.8 15.8 28.2 37.25 47.0 56.52 71.5 78.8 0.01574 0.01418 0.01288 0.01260 0.01230 0.01415 0.01447 0.01580 0.01422 0.01300 0.01275 0.01245 0.01420 0.01495 (Miiller, Z. phys. Ch. 1912, 81. 499.) t p &> 015 16.1 25.0 0.01240 0.01266 15.6 42.2 0.00966 0.00976 14.7 51.5 0.00759 0.00759 14.9 58.0 0.00703 0.00703 15.9 80.25 0.00520 0.00530 16.2 90.0 0.00570 0.00583 18.0 95.0 0.00578 0.00716 (Miiller, Z. phys. Ch. 1912, 81. 496.) 610 NITROGEN BROMOPHOSPHIDE Solubility of N 2 in glycerine +Aq at 25. G= % by wt. of glycerine in the solvent. S= solubility of N 2 . P = corrected pressure at end of experiment in mm. Hg at 0. G p s 16 598.4 0.0103 a 915.5 0.0103 29.7 556.5 0.0067 a 846.5 0.0068 48.9 617.7 0.0052 n 859.8 0.0051 74.5 588.5 0:0025 84.1 637.3 0.0024 tt 757.0 0.0024 (Drucker and Moles, Z. phys. Ch. 1910, 76. 418.) Absorption of N 2 by sucrose +Aq. t=temp. of the solution. P = % sucrose in the solution. /3t = coefficient of absorption at t. /315 = coefficient of absorption at 15. t p /3t 015 16.2 17.2 0.01670 0.01622 0.01700 0.01688 16.8 16.9 17 17.8 18 17.7 11.38 20.00 29.93 30.12 47.89 48.57 0.01432 0.01233 0.01025 0.01033 0.00742 0.00658 0.01480 0.01280 0.01053 0.01090 O.OQ785 0.00700 (Miiller, Z. phys. Ch. 1912, 81. 493.) Absorption of N 2 by organic substances +Aq att. V = absorbed volume reduced to and 760 mm. a = coefficient of absorption. Solution Vol. of solution com. t V com. a N-dextrose 409.94 20.18 4.55 0.01215 ^N-dextrose 409.94 20.21 5.14 0.01380 ^N-dextrose 409.94 20.2 5.51 0.01480 N-levulose 409.94 20.25 4.27 0.01221 N-arabinose 409.94 20.21 4.40 0.01203 jN-erythritol 409.94 20.25 4.87 0.01321 :N-alanine 409.94 20.19 4.445 0.01213 N-glycocoll 409.94 20.16 4.47 0.01212 N-urea 409.94 20.18 5.37 0.01477 N acetamide 409.94 20.22 5.385 0.01475 (Hiifner, Z. phys. Ch. 1907, 67. 618-621.) .Nitrogen bromide, NBr 3 . Decomp. under H 2 O. Nitrogen bromophosphide, PBr 2 N. Insol. in H 2 O. Sol. in ether, less sol. in CS 2 or CHC1 3 . (Besson, C. R. 114. 1479.) Nitrogen bromosulphide. See Nitrogen sulphobromide. Nitrogen chloride, NC1 3 . Very unstable. Explodes when heated to 93 or by contact with other substances. Insol. in H 2 O, but is decomp. thereby (in 24 hours by cold H 2 O). Sol. in CS 2 , PC1 3 , and S 2 C1 2 . (H. Davy, Phil. Trans. 1813, 1. 242.) Sol. in C 6 H 6 , CS 2 , CHC1 6 , CC1 4 . (Hentschel B. 1897, 30. 1434.) Nitrogen chlorophosphide, N 3 P 3 C1 6 . Insol. in H 2 O, but slowly decomp. thereby. Insol. in hot H 2 SO 4 , HC1, or HNO 3 +Aq. Decomp. by hot fuming HNO 3 . Sol. in al- cohol; very sol. in ether, but these solutions gradually decompose. Sol.' in CS 2 , CHC1 3 , C 6 H 6 , and oil of turpentine. Sol. in POC1 3 . (Gladstone, Chem. Soc. 3. 138.) Nitrogen chlorosulphide. See Nitrogen sulphochloride. Nitrogen fluoride. Very explosive. (Warren, C. N. 56. 289.) Nitrogen worioiodamine, NH 2 I. Very rapidly decomp. by H 2 O into N 2 H 3 I 3 . (Raschig, A. 230. 212.) Nitrogen diiodamine, NHI 2 . Properties as triioddiamiue. Nitrogen Zniodcftamine, NH 3 , NI 3 . Decomp. by H 2 O. (Raschig, A. 230. 212.) Insol. in absolute alcohol. Sol. with de- comp. in HCl+Aq. (Bunsen.) Nitrogen iodide, N 3 I. See Tn'azoiodide. Nitrogen iodide, NI 3 . Insol. in H 2 O, but slowly decomp. thereby. Sol. in HCl+Aq. Sol. in KCN+Aq. (Mil- Ion, J. pr. 17. 1.) Sol. in Na 2 S 2 3 +Aq. (Guyard, C. R. 97. 526.) Sol. in KSCN+Aq. (Raschig, A. 230. 212.) Nitrogen iodide ammonia, NI 3 , 3NH 3 ; NI a , 2NH 3 ; and NI 3 , NH 3 . (Hugot, C. R. 1900, 130. 507.) NI 3 , 12NH 3 . Ppt.; insol. in ether. (Ruff, B. 1900, 33. 3028.) NITROGEN OXIDE 611 Nitrogen monoxide, N 2 O. (a.) Liquid. Miscible with alcohol or ether. (b.) Gas. 1 vol. H2O absorbs 0.78-0.86 vol. N2O at ordinary temp. (Henry) ; 0.80 vol. at ordinary temp. (Dalton) ; 0.76 vol. at ordinary temp, (de Saussure) ; 0.708 vol. at 18 (Pleisch); 0.54 vol. (Davy). 1 vol. H 2 O at t and 760 mm. absorbs V vols. N 2 O, reduced to and 760 mm. t v t V .3052 13 0.8304 1 .2605 14 0.8034 2 .2172 15 0.7778 3 . 1752 16 0.7535 4 .1346 17 0.7306 5 .0954 18 0.7090 6 .0575 19 0.6888 7 .0210 20 0.6700 8 0.9858 21 0.6525 9 0.9520 22 0.6364 10 0.9196 23 0.6216 11 0.8885 24 0.6082 12 0.8588 (Bunsen's Gasometry.) 1 vol. H 2 absorbs 1.30521-0.0453620t + 0.00068430t 2 vols. N 2 O at t and 760 mm. (Bunsen.) Coefficient of absorption by H 2 O= 0.01883 at 15. (Steiner, Z. phys. Ch. 1895, 18. 14.) Coefficient of absorption by H->O= 0.600 at 23.5; 0.773 at 15.5; 0.951 at 8.1. (Gor- don, Z. phys. Ch. 1895, 18. 4.) Absorption of N 2 O by H 2 O at t. t Coefficient of absorption 25 20 15 10 5 0.5752 0.6654 0.7896 0.9479 1.1403 (Roth, Z. phys. Ch. 1897, 24. 123.) Solubility in H 2 O at 25 =0.5942; at 20 = 0.6756; at 15 =0.7784; at 10 = 0.9101; at 5 = 1.067. (For formula for "solubility," see under oxygen.) (Geffcken, Z. phys. Ch. 1904, 49. 278.) Solubility of N 2 O in H 2 O =0.592 at 25 and 758-1362 mm. pressure. (Findlay and Creighton, Chem. Soc. 1910, 97. 538.) 100 vols. H 2 SO 4 (sp. gr. = 1.84) absorb 75.7 vols. N 2 O; 100 vols. H 2 SO 4 +Aq (sp. gr.= 1.80) absorb 66.0 vols. N 2 O; 100 vols. H 2 SO 4 +Aq (sp. gr. = 1.705) absorb 39.1 vols. N 2 O; 100 vols. H 2 S0 4 +Aq (sp. gr. = 1.45) absorb 41.6 vols. N 2 O; 100 vols. H 2 SO 4 +Aq (sp. gr. = 1.25) absorb 33.0 vols. N 2 O. CaCl 2 +Aq, and NaCl+Aq absorb con- siderable amounts of N 2 O. (Lunge, B. 14. 2188.) Absorption by acids +Aq. M = content in gram-equivalents per liter. S = solubility (see under Oxygen). Absorption of N 2 O by HNO 3 +Aq. M S25 S 15 0.610 0.614 1.253 1.254 2.405 2.435 0.5969 0.5980 0.6045 0.6061 0.6156 0.6149 0.7770 0.7766 0.7767 0.7767 0.7735 0.7737 (Geffcken, Z. phys. Ch. 1904, 49. 278.) Absorption of N 2 O by HCl-fAq. M S25 S 15 0.549 0.550 1.089 1.093 2.300 2.340 0.5775 0.5759 0.5670 0.5657 0.5546 0.5564 0.7550 0.7528 0.7360 0.7347 0.7103 0.7122 Absorptic (Geffcken.) D,, _,f TSJ n Kir ^2kO 4 n oi IN 2 u oy 2 i~Aq. M S25 S 15 0.523 0.526 1.050 1.054 2.042 2.047 2.971 2.963 3.897 3.973 0.5648 0.5657 0.5426 0.5419 0.5083 0.5087 0.4819 0.4820 0.4569 0.4577 0.7328 0.7340 0.6997 0.6984 0.6440 0.6428 0.6024 0.6030 0.5648 0.5640 (Geffcken.) Absorption of N 2 O by H 3 P0 4 +Aq at t. t 5 10 15 20 25 % of HsPCU 3.38% 4.72% 8.84% 9.89% 13.35% 1.057 1.0365 0.9883 0.8827 0.8665 0.8296 0.7388 0.7258 0.6977 0.6253 0.6147 0.5926 0.5427 0.5329 0.5143 0.9635 0.9171 0.8101 0.7711 0.6826 0.6505 0.5810 0.5555 0.5054 0.4860 (Roth, Z. phys. Ch. 1897, 24. 134.) 100 vols. cone. FeSO 4 +Aq absorb 19.5 vols. N 2 O. Solubility of N 2 O in a solution containing 47.7 g. -Fe(OH) 3 per litre at 25 =0.5799; 47.9 g. Fe(OH) 8 per litre at 25 = 0.5787. (Geffcken, Z. phys. Ch. 1904, 49. 299.) 612 NITROGEN OXIDE 100 vols. KOH+A 18.7 vols. N 2 O; 100 v pyrogallol absorb 18 NaOH+Aq (sp. gr.= sorb 23.1 vols. N 2 O; 1 with pyrogallol absor Absorption of IS M = content in grai S = solubility (see u q (sp. ols. K( 1 volj gr. = 1.12) absorb 3H+Aq sat. with 3. N 2 O; 100 vols. (7% NaOH) ab- 3. NaOH+Aqsat. vols. N 2 O. KOH+Aq. valents per litre. >xygen). Absorption of N 2 O by salts +Aq at 15. M= number of molecules of salt per litre, a = coefficient of absorption. -1.1) 00 vols b28.0 f 2 0by n-eqii] nder c Salt M a KC1 3.554 2.909 1.755 1.051 0.526 0.0892 0.1012 0.1279 0.1489 0.1667 M S 25 S 15 KNO 3 2.430 1.820 1.541 0.879 0.482 0.1180 0.1311 0.1391 0.1559 0.1683 0.541 0.542 1.074 1.082 0.5087 0.6591 0.5093 0.6595 0.4252 0.5427 0.4221 0.5392 K 2 CO 8 4.352 2.939 2.156 1.376 0.690 0.341 0.209 0.0160 0.0285 0.0462 0.0761 0.1183 0.1501 0.1628 (Geffcken, Z. phys. Ch. 1904, 49. 278.) Coefficient of solubility of N 2 O in salts +Aq at t. Salt Concentration of salt Coeff. of absorption at G. per 100 g. solu- tion G. mol. per 1. 5 10 15 20 NaCl 4.815 2.801 2.049 0.825 0.0595 0.0925 0.1130 0.1548 CaCl 2 5.79 9.86 13.99 0.547 0.964 1.416 0.819 0.608 0.510 0.697 0.586 0.441 0.591 0.509 0.380 0.500 0.435 0.328 NaNO 2 5.711 3.980 2.656 1.413 0.679 0.0578 0.0810 0.1052 0.1370 0.1603 LiCl 1.35 3.85 1 4.8 0.319 0.928 2.883 0.986 0.878 0.606 0.831 0.743 0.512 0.700 0.629 0.437 0.599 0.536 0.382 Na 2 CO 3 1.218 0.819 0.438 0.207 0.0839 0.1082 0.1385 0.1639 Li 2 SO 4 2.37 5.46 8.56 0.219 0.521 0.836 0.934 0.795 0.646 0.792 0.665 0.555 0.670 0.557 0.477 0.569 0.474 0.415 MgS0 4 5.90 7.66 10.78 0.521 0.687 0.997 0.766 0.708 0.569 0.664 0.586 0.491 0.561 0.486 0.417 0.471 0.414 0.346 Na 2 S0 4 1.364 0.638 0.335 0.0775 0.1254 0.1519 KC1 4.90 7.64 14.58 22.08 0.676 1.037 2.187 3.414 0.879 0.799 0.654 0.544 0.751 0.693 0.574 0.459 0.643 0.591 0.500 0.390 0.555 0.494 0.430 0.339 LiCl 3.734 1.800 0.835 0.0990 0.1370 0.1619 MgS0 4 2.501 1.631 0.936 0.433 0.0499 0.0797 0.1159 0.1501 K 2 S0 4 2.62 4,78 0.154 0.285 0.986 0.918 0.831 0.763 0.701 0.637 0.605 0.542 NaCl 6.20 8.88 12.78 1.107 1.614 2.391 0.800 0.713 0.634 0.682 0.603 0.532 0.585 0.510 0.449 0.509 0.434 0.386 ZnSO 4 2.180 1.277 0.899 0.397 0.0605 0.0961 0.1175 0.1525 Na 2 S0 4 5.76 8.53 12.44 0.427 0.646 0.974 0.808 0.692 0.559 0.677 0.574 0.486 0.584 0.482 0.417 0.495 0.416 0.354 CaCl 2 2.962 2.556 1.827 1.122 0.578 0.321 0.0519 0.0619 0.0839 0.1138 0.1450 0.1619 SrCl 2 3.31 5.73 13.24 0.215 0.380 0.939 0.928 0.848 0.644 0.788 0.709 0.547 0.671 0.610 0.463 0.578 0.556 0.390 (Gordon, Z. phys. Ch. 1895, 18. 5.) (Steiner, Z. phys. Ch. 1895, 18. 14-5.) NITROGEN OXIDE 613 Coefficient of absorption of N 2 O by NaCl-f- Aq at t. Absorption of N 2 O by salts +Aq. Continued. t Per cent of NaCl Salt M S25 S 15 0.990 1.808 3.886 5.865 KBr 0.546 0.550 0.937 0.959 0.5306 0.5318 0.4908 0.4899 0.6877 0.6892 0.6352 0.6334 5 10 15 20 25 1.0609 1.0032 0.8812 0.8383 0.7339 0.7026 0.6191 0.5962 t).5363 0.5190 0.9131 0.7699 0.6495 0.5520 0.4775 0.8428 0.7090 0.5976 0.5088 0.442,4 RbCl 0.439 0.444 0.977 0.993 0.558 0.559 1.070 1.102 0.5399 0.5386 0.4873 0.4846 0.5218 0.5217 0.4673 0.4639 0.7050 0.7053 0.6306 0.6276 0.6782 0.6787 0.6046 0.6020 (Roth, Z. phys. Ch. 1897, 24. 139.) Absorption of N 2 O by salts +Aq at 20. C = concentration of the solution in terms of normal, a = coefficient of absorption. Absorption of N 2 O by KNO 3 +Aq at 20. (Geffck Solubilit 39.6 g. As 2 ' As 2 S 3 per h 1 vol. alco vols. N 2 C 3n, Z. phys. y of N 2 O ii 3 3 per litre Ch. 1904, 49. 278.) i a solution containing at 25 = 0.5819; 42.4 g. 0.5833. (Geffcken.) id 760 mm. absorbs V d to and 760 mm. P C a 1.063 2.720 5.389 10.577 0.1061 0.2764 0.5630 1 . 1683 6270 6173 .6002 .5713 .5196 10! at t ai > gas reduce t V t v 1 2 3 4 5 6 7 8 9 10 11 12 4.1780 4.1088 4.0409 3.9741 3.9085 3.8442 3.7811 3.7192 3.6585 3.5990 3.5408 3.4838 3.4279 13 14 15 16 17 18 19 20 21 22 23 24 3.3734 3.3200 3.2678 3.2169 3.1672 3.1187 3.0714 3.0253 2.9805 2.9368 2.8944 2.8532 Absorption of N 2 O by NaNO 3 +Aq at 20. P C a 1. 2 5. 8. 124 531 077 701 0.1336 0.3052 0.6286 1 . 1200 .6270 .6089 .5876 .5465 .4926 (Knopp, Z. phys. Ch. 1904, 48. 107.) Absorption of N 2 O by salts+Aq. M = content in gram-equivalents per litre. S = solubility. Salt M S25 S 15 NH 4 C1 0.598 0.600 1.158 1.166 0.5532 0.5504 0.5223 0.5200 0.7203 0.7185 0.6800 0.6775 KI 0.550 0.557 0.886 0.913 0.514 0.545 0.5367 0.5344 0.5025 0.5012 0.5428 0.5406 0.6950 0.6916 0.6466 0.6442 0.7074 0.7036 LiCl 0.558 0.561 1.057 1.059 0.5276 0.5278 0.4760 0.4773 0.6884 0.6877 0.6163 0.6146 (Bunsen's Gasometry.) Coefficient of absorption = 4. 17805- 0.0698160t+0.0006090t 2 . (Carius.) At 18 and 760 mm., 100 vols. H 2 O absorb 76 vols. N2O; 100 vols. alcohol of 0.840 sp. gr. absorb 153 vols.; 100 vols. rectified naphtha of 0.784 sp. gr. absorb 254 vols.; 100 vols. oil of lavender of 0.880 sp. gr. absorb 275 vols.; 100 vols. olive oil of 0.915 so. gr. absorb 150 vols.; 100 vols. sat. KCl+Aq (23% KC1) of 1.212 sp. gr. absorb 29 vols. (de Saussure, 1814.) 1 vol. oil of turpentine absorbs 2.5-2.7 vols. N2O. (de Saussure.) Absorption of N 2 O by glycerine +Aq at t. t % by weight of glycerine 3.460% 6.726% 12.120% 16.244% 25 20 15 10 5 0.5558 0.6468 0.7672 0.9172 1.0967 0.5415 0.6303 0.7454 0.8871 1.0552 0.5268 0.6050 0.7098 0.8411 0.9990 0.5083 0.5851 0.6857 0.8102 0.9586 (Roth, Z. phys. Ch. 1897, 24. 128.) 614 NITROGEN OXIDE Absorption of N 2 O by urea+Aq at t. Absorption of N 2 O by oxalic acid+Aq at t. t % by weight of urea t Coeff. of abs. in H 2 C 2 O4 +Aq of given % strength 3.312% 4.974% 6.366% 7.296% 9.966% 8.122% 3.699% 25 20 15 10 5 0.5686 0.6533 0.7708 0.9209 1.1040 0.5669 0.6558 0.7732 0.9201 1.0964 0.5588 0.6539 0.7605 0.9086 1.0880 0.7502 0.6553 0.7722 0.9208 1 . 1012 Q.5689 0.6508 0.7614 0.9007 1.0685 25 20 15 10 5 0.5786 0,6694 0.7940 0.9526 1.1450 0.5643 0.6538 0.7745 0.9264 1 . 1094 (Roth, Z. phys. Ch. 1897, 24. 124.) Absorption of N 2 O by sugar +Aq at 15. Number of molecules of Ci 2 H 22 On per litre Coefficient of absorption 1.699 0.993 0.520 0.0892 0.1284 0.1561 (Steiner, Z. phys. Ch. 1895, 18. 15.) Absorption of N 2 O by organic substances + Aq. C = concentration of the solution in terms of normal. a = coefficient of absorption. Absorption of N 2 O by chloral hydrate +Aq at 20. P C a 2.947 6.848 13.48 16.15 19.60 24.02 0^184 0.445 0.942 1.165 1.474 1.911 0.6270 0.6182 0.6128 0.5960 0.5891 0.5793 0.5675 (Knopp, Z. phys. Ch. 1904, 48. 106.) Absorption of N 2 O by propionic acid+Aq at 20. P C a 1.492 5.702 13.680 15.011 25.589 0'.2045 0.816 2.140 2.385 4.645 0.6270 0.6323 0.6369 0.6504 0.6534 0.7219 (Knopp, Z. phys. Ch. 1904, 48. 107.) (Roth, Z. phys. Ch. 1897, 24. 130.) Coefficient of absorption for petroleum = 2.11 at 20; 2.49 at 10. (Gniewasz and Walfisz, Z. phys. Ch. 1. 70.) The solubility of N 2 O in various colloidal solutions has been determined by Findlay and Creighton (Chem. Soc. 1910, 97. 538), for which see original article. Nitrogen dioxide, NO. 1 vol. H 2 O absorbs 0.1 vol. NO gas at ordinary temp. (Davy) ; 1 vol. absorbs 0.05 vol. (Henry) ; 1 vol. absorbs 1/27 vol. (Dalton.) Absorption of NO by H 2 O at 760 mm. pressure. = Coefficient of absorption. ./3' = " Solubility." t ft 0' t ]8 ? 0.07381 0.07337 55 0.03040 0.02570 5 6461 6406 60 2954 2375 10 5709 5640 65 2877 2169 15 5147 5061 70 2810 1947 20 4706 4599 75 2751 1706 25 4323 4189 80 2700 1439 30 4004 3838 85 2665 1146 35 3734 3529 90 2648 0817 40 3507 3254 95 2638 0439 45 3311 3000 100 2628 0000 50 3152 2771 (Winkler, B. 1901, 34. 1414.) 205.69 cc. H 2 O absorb 9.6798 cc. NO at 20 and 760 mm. (Hiifner, Z. phys. Ch. 1907, 59. 420.) Sol. in cone. HNO 3 +Aq. 100 vols. HNO 3 +Aq of 1.3 sp. gr. agitated with NO gas take up 20 vols. NO. If acid is twice as strong or one^half as strong, the quantity NO is proportional to the amount of HNO 3 . Very dil. HNO 3 +Aq absorbs scarcely more NO than pure H 2 O. (Dalton.) 100 pts. HNOs+Aq of 1.4 sp. gr. absorb 90 pts. NO (Dalton); sol. in Br2, and very si. sol. in cone. H 2 SO.j. (Berthelot.) 1 ccm. cone. H 2 SO 4 of 1.84 sp. gr. absorbs 0.035 ccm. NO; of 1.50 sp. gr., 0.017 ccm. NO. (Lunge, B. 18. 1391.) NITROGEN OXIDE 615 Absorption of NO by H 2 SO 4 +Aq at 18 and 760 mm. Absorption of NO by FeSO 4 +Aq at t. Continued. a = Coefficient of solubility. 205.69 cc. of FeSO 4 +Aq contain 0.0296 g. Fe. Coefficient of absorption = 0.06505. H 2 S0 4 a H 2 SC 4 a t Pressure mm. NO absorbed ccm. 98% not constant 90% 0.0193 80% 0.0117 70% 60% 50% 0.0113 0.0118 0.0120 20.05 20.05 20.04 20.00 20.15 20.14 677.5 655.3 639.1 620.2 600.5 581.2 14.30 14.07 13.81 13.39 13.20 12.92 (Tower, Z. anorg. 1906, 50. 387.) Very sol. in aqueous solutions of ferrous salts, especially the sulphate. (Priestley.) 1 vol. FeSO 4 +Aq of 1.081 sp. gr., contain- ing 1 grain FeSO 4 to 6 grains H 2 O, absorbs 6 vols. NO. (Dalton.) Absorption by ferrous salts +Aq is propor- tional to the amount of Fe present, irrespec- tive of the acid or concentration of the solu- tion. Between and 10, about 2 mols. NO are absorbed for each atom of Fe; between 10 and 15, 1 mol. NO for 2 atoms of Fe; and at 25, only 1 mol. NO for 2 1 A to 3 atoms of Fe. The amount of NO absorbed also varies with the pressure. The sp. gr. of the ferrous salt solution is greater after the ab- sorption of NO than before. The solutions are decomp. by heat, and at 100 all NO is given off. (Gay, A. ch. (6) 5. 145.) Absorption of NO by FeSO 4 +Aq at 25. A = vol. H 2 O (in litres) containing 1 mol. FeSO 4 . V = vol. NO (in litres) absorbed. 205.69 cc. of FeSO 4 +Aq contain 0.0409 g. Fe. Coefficient of absorption = 0.06684. t Pressure mm. NO absorbed ccm. 20.04 20.02 20.00 20.00 20.10 667.6 650.6 613.1 594.6 577.1 16.79 16.65 15.71 15.41 15.32 205.69 cc. of FeSO 4 +Aq contain 0.0513 g. Fe. Coefficient of absorption =0.07981. t Pressure mm. NO absorbed ccm. 20.10 20.10 20.08 20.10 20.10 20.10 644.8 623.8 606.4 589.7 571.1 553.1 18.82 18.47 18.02 17.56 17.19 16.95 205.69 cc. of FeSO 4 +Aq contain 0.0663 g. Fe. Coefficient of absorption =0.08059. A V A V 1.2 1. 1.8 2. 2.4 2. 4.82 4. 47 01 55 40 7.2 12,0 18.6 36.0 5.52 6.46 8.01 10.40 t Pressure mm. NO absorbed ccm. 20.10 20.10 20.10 20.08 20.04 20.00 697.3 678.9 660.4 638.2 620.7 602.5 21.91 21.60 21.18 20.71 20.28 19.87 (Kohlschutter, B. Absorption of NO bj 205.69 cc. FeSO 4 +Aq Coefficient of absorpti 1907, 40 r FeSO 4 + [ contain ( on-0.06C 877.) Aq at t. ).0221 g. Fe. 167 at 20.09. 205.69 cc. of FeSO 4 +Aq contain 0.099 g. Fe. Coefficient of absorption =0.1 1661. t Pressure mm. NO absorbed ccm. t Pressure mm. VO absorbed ccm. 20.10 20.15 20.20 20.00 19.85 19.85 649.9 631.1 618.4 603.3 588.6 574.2 34.26 33.82 33.26 . 32.76 32.34 31.95 20.1 20.1 20.1 20.2 20.05 20.0 704 683 668 651 632 613 9 5 6 9 9 7 14.42 14.10 13.80 13.58 13.15 12.98 (Htifner, Z. phys. Ch. 1907, 69. 419.) 616 NITROGEN OXIDE Absorption of NO by NiSO 4 +Aq at t. 205.69 cc. NiSO 4 +Aq contain 0.0506 g. Ni. Coefficient of absorption = 0.08311. Absorption of NO I A = vol. H 2 O (in lii FeCl 2 . V vol NO (in litr< >y FeCl 2 +Aq at 22. bres) containing 1 mol. js) absorbed. t Pressure mm. NO absorbed ccm. A v 20.2 20.2 20.2 20.15 20.14 654.7 629.8 609.5 591.7 573.4 23.00 22.54 22.03 21.65 21.18 2.5' 5.18 10.35 20.7 51.8 3.30 4.83 6.56 8.32 11.89 (Hufner, I. c.) Absorption of NO by CoSO 4 +Aq at t. 205.69 cc. CoSO 4 +Aq contain 0.0598 g. Co. Coefficient of absorption = 0.09146. (Kohlschutter, B. 1907, 40. 878.) Absorption by HCl+FeCl 2 +Aq. 10.37 1. 30% HC1 containing 1 mol. FeCl 2 in solution absorb 15.64 1. NO. 10.37 1. 10% HC1 containing 1 mol. FeCl 2 in solution absorb 6.17 1. NO. (Kohlschutter, I. c.) Absorption by salts -f-Fed 2 +Aq. 10.37 1. sat. NaCl+Aq containing 1 mol. FeCl 2 in solution absorb 6.549 1. NO. 10.37 1. sat. NH 4 Cl+Aq containing 1 mol. FeCl 2 in solution absorb 6.549 1. NO. (Kohlschutter, I. c.) Solubility of NO in Fe(NO 3 ) 2 +Aq at 23. A = vol. H 2 O (in litres) containing 1 mol. Fe(N0 3 ) 2 . V = vol. NO (in litres) absorbed. f Pressure mm. NO absorbed 20.15 678.3 23.47 20.16 653.5 23.01 20.20 636.6 22.55 20.30 615.9 21.99 20.40 600.0 21.56 (Hufner, I. c.) Absorption of NO by MnCl 2 .4H 2 O+Aq at t. 205.69 cc. MnCl 2 .4H 2 O-hAq contain 0.0697 g. Mn. Coefficient of absorption = 0.061 11. A V 3.25 6.50 13.00 26.00 2.77 4.16 5.54 6.61 t Pressure mm. NO ^ rbed 20.0 711.96 14.25 20.05 686.5 13.99 20.2 657.4 13.49 20.3 638.9 13.05 20.45 621.0 12.81 (Kohlschutter, I. c.) Absorption of NO by CuCl 2 +Aq. A=vol. H 2 O (in litres) containing 1 mol. CuCl 2 . V = vol. NO (in litres) absorbed. (Hufner, I. c.) Coefficient of absorption for FeSO 4 -fAq of concentration used by Hufner (Z. phys. Ch. 1907, 69. 417) =0.180 at 20. Hiifner's re- sults are incorrect because he assumed that the absorption-coefficient of NO always had the same value, whereas it does not. NO is reduced by FeSO 4 +Aq. (Usher, Z. phys. Ch. 1908, 62. 624.) Coefficient of absorption for CoSO 4 4-Aq sat. at 20 = 0.0288. (Usher, Z. phys. Ch. 1908, 62. 624.) Coefficient of absorption for NiSO 4 +Aq of the concentration used by Hufner (c/. Z. phys. Ch. 1907, 59. 422) =0.048 at 20. Coefficient of absorption for NiSO 4 +Aq sat. at 20 =0.0245. (Usher, I. c.) Coefficient of absorption for MnCl 2 +Aq. sat. at 20 00082 (Usher Z phys Ch A v 0.231 0.277 0.371 0.120 0.098 0.052 (Kohlschutter, I. c.) Absorption of NO by CuCl 2 +conc. HC1. A = vol. cone. HC1 (in litres) containing 1 mol. CuCl 2 . V = vol. NO (in litres) absorbed. A V A v 0.389 0.410 0.840 1.230 2.462 0.801 0.933 2.838 3.426 3.989 7.499 12.500 18.750 28.650 3.931 3.606 3.153 1.976 1908, 62. 624.) (Kohlschutter, I. c.) NITROGEN OXIDE 617 Absorption of NO by CuCl 2 + acetic acid. A = vol. acetic acid (in litres) containing 1 mol. CuCl 2 . V = vol. NO (in litres) absorbed. A V A V 252 504 1269 51.77 39.67 81.60 0.37 0.62 0.925 0.515 0.120 0.000 (Kohlschtitter, I. c.) Absorption of NO by CuCl 2 +98% formic acid. A = vol. 98% formic acid (in litres) contain- ing 1 mol. CuCl 2 . V =vol. JNU (in litres) absorbed. A V 27.9 56.0 140.0 280.0 1400.0 12.76 13.17 14.34 18.68 27.29 (Kohlschtitter, I. c.) Absorption of NO by CuCl 2 + acetone. A=vol. acetone (in litres) containing 1 mol. CuCl 2 . V = vol. NO (in litres) absorbed. A v A v 4.667 29.16 58.33 14.04 24.01 24.60 291.60 583.20 1166.40 40.99 67.22 81.96 (Kohlschtitter, I. c.) Absorption of NO by CuCl 2 -f methyl alcohol. A = vol. methyl alcohol (in litres) contain- ing 1 mol. CuClj. V = vol. NO (in litres) absorbed. A v A v 1.60 8.22 3.30 5.60 20.50 82.25 6.15 4.90 (Kohlschtitter, I. c.) Absorption of NO by CuCl 2 +ethyl alcohol. A = vol. ethyl alcohol (in litres) containing 1 mol. CuCl 2 . V=vol. NO (in litres) absorbed. A V A v 1.50 3.84 12.80 8.70 12.38 15.43 38.41 76.83 192.10 18.15 18.05 15.92 (Kohlschtitter, I. c.) Absorption of NO by CuBr 2 +Aq. A = vol. H 2 O (in litres) containing 1 mol. CuBr 2 . V = vol. NO (in litres) absorbed. (Kohlschtitter, L c.) Absorption of NO by CuBr 2 + ethyl alcohol. A=vol. alcohol (in litres) containing 1 mol. CuBr 2 . V=vol. NO (in litres) absorbed. A 2.625 5.25 13.12 43.74 V A v 16.02 19.26 20.51 21.13 131.20 262.50 656.10 22.23 23.46 30.46 (Kohlschtitter, I. c.) Sol. in stannous and chromous salts+Aq. (Peligot.) Not absorbed by Fe 2 (S0 4 ) 3 +Aq. (Dalton.) 1 vol. absolute alcohol absorbs 0.31606- 0.003487t+0.000049t 2 vols. NO between and 25. (Bunsen.) 1 vol. alcohol at t and 760 mm. absorbs V vols. NO gas reduced to and 760 mm. t V "t v 0.31606 13 0.27901 1 0.31262 14 0.27685 2 0.30928 15 0.27478 3 0.30604 16 0.27281 4 0.30290 17 0.27094 5 0.29985 18 0.26917 6 0.29690 19 0.26750 7 0.29405 20 0.26592 8 0.29130 21 0.26444 9 0.28865 22 0.26306 10 0.28609 23 0.26178 11 0.28363 24 0.26060 12 0.28127 (Bunsen's Gasometry.) Abundantly absorbed by CS 2 . (Friedburg, C. N. 48. 97.) Nitrogen irioxide, N 2 O 3 . Sol. in H 2 O at 0. If large amt. of H 2 O is present, the solution is quite stable at ordi- nary temp. (Fremy, C. R. 79. 61.) Sol. inHNOa+Aq. Sol. in cone. H 2 SO 4 to form HNOSO 4 . Sol. in ether. 618 NITROGEN OXIDE STANNIC CHLORIDE Nitrogen trioxide stannic chloride, N 2 O 3 , SnCl 4 . Decomp. by H 2 O. (Weber, Pogg. 118. 471.) Nitrogen letroxide, N0 2 or N 2 O 4 . Sol. in H 2 O at with decomp. Miscible with very cone. HNO 3 . Absorbed abundantly by CS 2 , CHC1 3 , and C 6 H 5 C1. (Friedburg, C. N. 47. 52.) Sol. in C 6 H 5 NO 2 . SI. sol. in H 2 S+Aq. Sol. in H 2 SO 4 or cone. HNO 3 +Aq. H 3 PO 4 absorbs some liquid NO 2 . (Frank- land, Chem. Soc. 1901, 79. 1362.) Nitrogen pentoxide, N 2 O 6 . Very deliquescent. Combines with H 2 O to form HNO 3 with evolution of heat. Nitrogen hexoxide, NO 3 . Decomposes upon air or with H 2 O. (Haute- feuille and Chappins, C. R. 92. 80, 134; 94. 1111, 1306.) Nitrogen oxybromide. See Nitrosyl and Nitroxyl bromide. Nitrogen oxychloride. See Nitrosyl and Nitroxyl chloride. Nitrogen oxyfluoride. See Nitrosyl fluoride and Nitroxyl fluoride. Nitrogen phosphochloride, P 3 N 3 C1 6 . See Nitrogen chlorophosphide. Nitrogen selenide, NSe. Very explosive. Insol. in H 2 O. Sol. in HNOs+Aq, and NaClO+Aq. (Espenschied, A. 113. 101.) Insol. in H 2 O, ether, absolute alcohol; very si. sol. in CS 2 , C 6 H 6 , and glacial acetic acid. Decomp. by HC1 or KOH+Aq. (Verneuil, Bull. Soc. (2) 38. 548.) Nitrogen sulphide, N 4 S 4 . Insol. in H 2 O. Decomp. by hot H 2 O. SI. sol. in alcohol, ether, wood alcohol, oil of turpentine. Easily sol. in CS 2 . Slowly de- comp. by HCl+Aq or KOH+Aq, rapidly by HNOa+Aq. 15 g. dissolve in 1 kilo, of CS 2 . (Fordos and Gelis, C. R. 31. 702.) Sol. in CHC1 3 . (Demargay, C. R. 91. 854.) Sol. in warm glacial acetic acid with de- comp. on boiling. (Ruff and Geisel, B. 1904, 37. 1591.) Nitrogen pentasulphide, N 2 S 6 . Sol. in ether and most organic solvents; insol. in H 2 O; fairly stable in ethereal solu- tion, but decomp. by light. (Muthmann, Z. anorg. 1897, 13. 206.) Nitrogen sulphobromide, N 3 S 4 Br. Decomp. by boiling H 2 O and by dil. alkalies, also by boiling with alcohol. (Muthmann, B. 1897, 30. 630.) N 4 S 4 Br 4 . Decomp. by moist air. (Clever, B. 1896, 29. 340-341.) N 4 S 4 Br 6 . Decomp. by moist air. Very unstable. (Clever.) N 4 S 6 Br 2 . Insol. most solvents; unstable. (Clever.) Nitrogen sulphochloride, N 4 S 4 C1 4 . Unstable on air. Sol. in warm CHC1 3 ; crystallizes out on cooling. (Demargay, C. R. 91. 854, 1066.) Demarcay calls this comp. thiazyl chloride. Sol. in hot dry benzene, and in CC1 4 ; decomp. by moist air. (Andreocci, Z. anorg. 1897, 14. 249.) N 4 S 6 C1 2 . Partly sol. in H 2 O. (Demarcay, C. R. 92. 726.) Demargay calls this compound dithiotetra- thiazyl ^'chloride. N 2 S 3 C1 2 = N 2 S 2 , SC1 2 . Decomp. on air. (Fordos and Gelis.) pemarcay (C. R. 92. 726) calls this comp. thiodithiazyl ^chloride. N 2 S 4 C1 2 . Sol. in H 2 O with subsequent de- comp. More sol. than S in CS 2 . (Soubeiran, A. ch. 67. 71.) Is a mixture of S 2 C1 2 and N 4 S 4 . (Fordos and Gelis, C. R. 31. 702.) N 3 S 3 C1. SI. sol. in warm, insol. in cold CHC1 3 . (Demarcay, C. R. 92. 726.) " Thio/nazyl chloride." (Demargay.) N 3 S 4 C1. Sol. in H 2 0. Insol. in most solvents. SI. sol. in CHC1 3 . Easily sol. in thionyl chloride. (Demargay, C. R. 91. 854, 1066.) Demargay calls the compound ihiotri- thiazyl chloride = (NS) 3 = S Cl. N 4 S 5 C1 2 =2N 2 S 2 , SC1 2 . Decomp. on air. (Michaelis.) N 6 S 7 C1 2 = 3N 2 S 2 , SC1 2 . Not decomp. on air. Decomp. by H 2 O containing ammonia. Nitrogen sulphoiodide, N 3 S 4 I. Readily decomp. by H 2 O. and Seitter, B. 1897, 30. 627.) (Muthmann Nitrohydroxylaminic acid, H 2 N 2 O 3 . Known only in solution. (Angeli, Gazz. ch. it. 1897, 27 (2) 357.) Barium nitrohydroxylaminate, BaN 2 O 3 +H 2 O. Ppt. More stable in the air than the sodium salt. Not decomp. by prolonged boiling with H 2 O. (Angeli, Gazz. ch. it. 1896, 26. 17-25.) Cadmium nitrohydroxylaminate, CdN 2 O 3 + H 2 O. As Ba salt. (Angelico and Fanara, Gazz. ch. it. 1901, 31. (2) 21.) NITROSOBROMORUTHENATE AMMONIA, SILVER 619 Calcium nitrohydroxylaminate, GaNjOs+ ^H 2 0. (Angeli, Gazz. ch. it. 1900, 30. (1) 593.) Calcium nitrohydroxylaminate, CaN 2 O 3 + (Angelico and Fanara, Gazz. ch. it. 1901, 31. (2) 15.) Lead nitrohydroxylaminate, PbN 2 3 . (Angeli, Gazz. ch. it. 1900, 30. (1) 593.) Potassium nitrohydroxylaminate, K 2 N 2 O 3 . Like Na salt. More hygroscopic. (Angeli, Gazz. ch. it. 1897, 27. (2) 357.) Sol. in H 2 O. (Angeli, Gazz. ch. it. 1900, 30. (1) 593.) Silver nitrohydroxylaminate, Ag 2 N 2 O 3 . Ppt. (Angeli, C. C. 1901, I. 1192.) Sodium nitrohydroxylaminate, Na 2 N 2 Os. Very sol. in H 2 O. Pptd. by alcohol. Aqueous solution is readily decomp. by boil- ing. (Angeli, Gazz. ch. it. 1896, 26. (2) 17.) Strontium nitrohydroxvlaminate, SrN 2 3 + H 2 0. (Angeli, Gazz. ch. it. 1900, 30. (1) 593.) + 1J^H 2 O. (Angelico and Fanara, Gazz. ch. it. 1901, 31. (2) 15.) Nitroiodic acid, I 2 O 4 (NO) 2 See Nitrosoiodic acid. Nitronitrous acid. Platinum potassium nitronitrite, K 2 Pt(NO 2 ) 4 . N 2 4 . Decomp. by heat. (Miolati, C. C. 1896, II. 1088.) Nitroplatinous acid. See Platonitrous acid. Nitroprussic acid, H 2 FeC6N 6 O+H 2 O = H 2 Fe(CN) 5 NO+H 2 O. Deliquescent. Easily sol. in H 2 O, alcohol, or ether. (Playfair, A. 74. 317.) Nitroprussides. The alkali and alkali-earth nitroprussides are sol. in H 2 O, and the solutions are not pptd. by alcohol. The others are mostly insol. in H 2 O. Ammonium nitroprusside, onum ntroprusse, (NH 4 ) 2 Fe(CN) 5 (NO). Deliquescent. Very sol. in H 2 O; not pptd- therefrom by alcohol. (Playfair.) Barium nitroprusside, BaFe(CN) 5 NO + 4H 2 O. Very sol. in H 2 O. +6H 2 O. Cadmium nitroprusside, CdFe(CN) 5 NO. Insol. in H 2 O. Sol. in HCl+Aq. Insol. in dil. or cone. HNO 3 +Aq even when boiling. Not attacked by NH 4 OH or KOH+Aq. (Norton, Am. Ch. J. 10. 222.) Calcium nitroprusside, CaFe(CN) 5 NO + 4H 2 0. Very sol. in H 2 O. (Playfair.) Cobalt nitroprusside, CoFe(CN) 5 NO. Ppt. (Norton, Am. Ch. J. 10. 222.) +4H 2 O. Copper nitroprusside, CuFe(CN) 6 NO+2H 2 O. Insol. in H 2 O or alcohol. Ferrous nitroprusside, FeFe(CN) 5 NO + *H,0(?). Insol. in H 2 O. Mercurous nitroprusside, Hg 2 Fe(CN) 6 NO. Insol. in H 2 O. Unstable. (Norton, Am. Ch. J. 10. 222.) Nickel nitroprusside, NiFe(CN) 6 NO. As the Co salt. (Norton.) Potassium nitroprusside, K 2 Fe(CN) 6 NO + 2H 2 0. SI. deliquescent. Sol. in 1 pt. H 2 O at 16. K 2 Fe(CN) 5 NO, 2KOH. Very sol. in H 2 O. Silver nitroprusside, Ag 2 Fe(CN) 6 NO. Insol. in H 2 O, alcohol, or HISO 3 +Aq. Sol. in NH 4 OH+Aq. Sodium nitroprusside, Na 2 Fe(CN) 5 NO + 2H 2 O. Sol. in 2% pts. H 2 O at 16, and in less hot H 2 O. Zinc nitroprusside, ZnFe(CN) 6 NO. Very si. sol. in cold, more in hot H 2 O. Nitrosisulphonic acid. Cupric nitrosisulphonate, NO^gQ^Cu. Decomp. by H 2 O. (Raschig, B. 1907, 40. 4583.) Nitrosobromoruthenic acid. Silver nitrosobromoruthenate ammonia, Ag 2 Ru(NO)Br 5 , NH 3 . Decomp. by H 2 O. SI. sol. in NH 4 OH+ Aq. Very sol. in Na 2 S 2 O 3 +Aq. (Brizard, Bull. Soc. 1895, (3) 13. 1093.) 620 NITROSOBROM03MIC ACID Nitrosobromosmic acid. Potassium nitrosobromosmate, K 2 Os(NO)Br 5 . Stable in aqueous solution. (Wintrebert, A. ch. 1903, (7) 28. 132.) Nitrosochloroplatinic acid. Potassium nitrosochloroplatinate, KsPtClf(NO). Sol. in H 2 O. (Vezes, C. R. 110. 757.) Nitrpsochlororuthenic acid. Ammonium nitrosochlororuthenate. (NH 4 ) 2 Ru(NO)Cl5. Sol. in H 2 O. (Joly, C. R. 107. 991.) 5 pts. are sol. in 100 pts. H 2 O at 25. 22 60. (Howe, J. Am. Chem. Soc. 1894, 16. 390.) Caesium nitrosochlororuthenate. Cs 2 Ru(NO)Cl 5 . 0.20 pt. is sol. in 100 pts. H 2 O at 25. 0.56 " " " " " " " " 100 (Howe.) +2H 2 O. Very sol. in H 2 O. 105.8 pts. are sol. in 100 pts. H 2 O. (Howe.) Potassium nitrosochlororuthenate. K 2 Ru(NO)Cl 5 . Sol. inH 2 O. (Joly.) 12 pts. are sol. in 100 pts. H 2 O at 25. 80 " " " " " " " " 60. (Howe.) Rubidium nitrosochlororuthenate. Rb 2 Ru(NO)Cl 5 . Sol. in boiling H 2 O without decomp. 0.57 pt. is sol. in 100 pts. H 2 O at 25. 2.13 " " " " " " " " 60. (Howe.) Silver nitrosochlororuthenate ammonia, Ag 2 Ru(NO)Cl 5 , NH 3 . Decomp. by H 2 0. SI. sol. in NH 4 OH+Aq. Very sol. in Na 2 S 2 O 3 +Aq. (Brizard, Bull. Soc. 1895, (3) 13. 1092.) Nitrosoiodic acid, I 2 O 4 (NO) 2 (?) Decomp. with H 2 O, alcohol, ether, or acetic ether. Slowly sol. in H 2 SO 4 . (Kammerer, J. pr. 83. 65. Nitrososulphonic acid. Potassium dinitrososulphonate, N 2 O.OK. SO 3 K. Sol. in H 2 O. Very unstable. (Hantzsch, B. 1894, 27. 3268.) Potassium nitrosoc&sulphonate, ON(SO 3 K) 2 . Sol. in H 2 O. Very explosive. (Hantzsch, B. 1895, 28. 996 and 2744.) Potassium nitroso^n'sulphonate, ON(SO 3 K) 3 +H 2 O. Sol. in H 2 O. (Hantzsch, B. 1895, 28. 2750.) Sodium nitrosofrisulphonate, NO 2 (SO 3 ) 3 Na. Decomp. by H 2 O. (Traube, B. 1913, 46. 2521.) Nitrososulphuric acid, H 2 N 2 S0 5 =H 2 S0 3 (NO) 2 . Not known in free state. Ammonium (fa'nitrososulphate, (NH 4 ) 2 (NO) 2 S0 3 . Sol. in H 2 O. Insol. in hot alcohol. (Pe- louze, A. 15. 240.) Barium , Ba(NO) 2 SO 3 . Sol. in H 2 O. (Divers and Haga, Chem. Soc. 47. 364.) Barium potassium , BaK 2 (SN 2 O5) 2 . Sol. in much H 2 O to form a clear liquid, but the solution gradually deposits BaSO 4 . (Hantzsch, B. 1894, 27. 3271.) Cupric nitrosodteulphate, Cu(NO)(SO 3 ) 2 . (Sabatier, Bull. Soc. 1897, (3) 17. 787.) Lead cfo'nitrososulphate. Insol. in H 2 O. (Divers and Haga, Chem. Soc. 47. 364.) Potassium , K 2 (NO) 2 SO 3 . Decomp. by H 2 O at ordinary temp. Insol. in alcohol. (Pelouze, A. ch. 60. 160.) Sol. in about 8 pts. H 2 O at 14.5. Less sol. in presence of KOH. (Divers and Haga, Chem. Soc. 1895, 67. 455.) Sodium , Na 2 (NO) 2 SO 3 . More sol. than K salt. (Pelouze.) SI. sol. in H 2 O; very unstable moist or dry; decomp. by H 2 O. (Divers, C. N. 1895, 72. 266.) Nitrososulphurbus acid. Ruthenium sodium nitrososulphite, O[Ru(SO 3 ) 2 (NO)Na 2 ] +2H 2 O. SI. sol. in cold H 2 O. (Miolati, Gazz. ch. it. 1900, 30. 511.) Nitrosulphide of iron. See Ferrofeiranitrososulphonic acid. Z^nitrosulphide of iron. Roussin's comp. is ammonium ferrohepta- nitrososulphonate, which see. NITRITE, AMMONIUM 621 Nitrosulphonic acid, HNSO fi .HO 'NO 2 S0 2 . (Lead chamber crystals.') Rapidly sol. in H 2 O with decomp. When brought into large amount of H 2 O, no gas is evolved. (Fremy, C. R. 70. 61.) Sol. in H 2 SO 4 without decomp. Sol. in cold H 2 SO 4 +Aq of sp. gr. 1.7-1.55. (Weber, J. pr. 100. 37.) SI. sol. in H 2 S0 4 +Aq of 1.6 sp. gr. (Dana.) More difficultly sol. in dil. than cone. H 2 SO 4 +Aq. (Muller.) Potassium nitrosulphonate, KOSO 2 NO 2 (?). Decomp. by H 2 O. (Schultz-Sellack, B. 4. 113.) Nitrosulphonic anhydride (?), N 2 O 3 , 2SO 3 = S 2 6 (N0 2 ) 2 . Rapidly sol. in H 2 O with decomp. Abund- antly soh in cold H 2 SO 4 . (Rose, Pogg. 47. 605.) Insol. in cold, slowly sol. in warm H 2 SO 4 . (Prevostaye, A. ch. 73. 362.) Nitrosulphonic chloride, NO 4 SC1 = NO 2 SO 2 C1 (?). Decomp. by H 2 O. Sol. in fuming H 2 SO 4 without decomp. Decomp. by cone. H 2 SO 4 . (Weber, Pogg. 123. 333.) Dmitrosulphuric acid. See ZH'nitrososulphuric acid. Nitrosyl bromide, NOBr. Decomp. with cold H 2 O. (Landolt, A. 116. 177.) Nitrosyl fnbromide, NOBr 3 . Decomp. by H 2 O or cold alcohol. Miscible with ether. (Landolt, A. 116. 177.) Mixture of NOBr and Br 2 . (Frohlich, A. 224. 270.) Nitrosyl platinic bromide, 2NOBr, PtBr 4 . Deliquescent. Decomp. by H 2 O. (Top- see, J. B. 1868. 274.) Nitrosyl chloride, NOC1. Decomp. by H 2 O. Absorbed by fuming H 2 S0 4 without decomp. Nitrosyl boron chloride, NOC1, BC1 3 . See Boron nitrosyl chloride. Nitrosyl platinic chloride, 2NOC1, PtCl 4 . Very deliquescent, and sol. in H 2 O with evolution of NO. (Rogers and Boye, Phil. Mag. J. 17. 397.) Nitrosyl thallium chloride, 2NOC1, T1C1, T1C1 3 . Very deliquescent, and sol. in H 2 O with decomp. (Sudborough, Chem. Soc. 59. 657.) Nitrosyl stannic chloride, 2NOC1, SnCl 4 . Decomp. by H 2 O, chloroform, or benzene, not by carbon disulphide. (Jorgensen.) Nitrosyl titanium chloride, 2NOC1, TiCl 4 . Decomp. by H 2 O. (Weber, Pogg. 118. ,476.) Nitrosyl zinc chloride, NOC1, ZnCl 2 . Very deliquescent, and sol. in H 2 O with evolution of NO. (Sudborough, Chem. Soc. 69. 656.) Nitrosyl chloride sulphur Jnoxide, NOC1, SO 3 . Decomp. by H 2 O. Sol. in cone. H 2 SO 4 with evolution of HC1. (Weber, Pogg. 123. 233.) Nitrosyl fluoride, NOF. Sol. in H 2 O. Solution decomp. on standing with formation of NO and HNO 3 . (Ruff and Stauber, Z. anorg. 1905, 47. 190.) Nitrosyl sulphate, acid, H(NO)SO 4 . See Nitrosulphonic acid. Nitrosyl sulphate, anhydro, (NO) 2 S 2 O 7 . See Nitrosulphonic anhydride. Nitrosyl selenic acid, SeO 2 (ONO) 2 . Decomp. by H 2 O. (Lenher and Mathews, J. Am. Chem. Soc. 1906, 28. 516.) Nitrosyl sulphuric acid, H(NO)SO 4 See Nitrosulphonic acid. Nitrous acid, HNO 2 . Known only in aqueous solution. See Nitrogen Znoxide. Nitrites. Normal nitrites, except AgNO 2 , are sol. in H 2 O and alcohol; but, as a rule, they are less sol. than the corresponding nitrates. Ammonium nitrite, NH 4 N0 2 . Very deliquescent, and sol. in H 2 O. H 2 O solution decomp. at 50. (Berzelius.) Very dil. solution can be evaporated on water bath without decomp. (Bohlig, A. 126. 25.) Solution containing Vioo,ooo pt. NH 4 NO 2 can be evaporated to % its vol. without decomp. Solution containing Vsoo pt. gives a distillate containing 8.6% of NH 4 NO 2 , while residue contains 82% of original quantity, 9.4% being lost. (Schoyen.) Very deliquescent, sol. in H 2 O; slowly but easily sol. in alcohol; insol. in ether. (Soren- sen, Z. anorg. 1894, 7. 38.) 622 NITRITE, AMMONIUM BARIUM CUPRIC Ammonium barium cupric nitrite, (NH 4 ) 2 BaCu(NO 2 )6. Ppt.; decomp. readily. (Przibylla, anorg. 1897, 15. 424.) Z. Ammonium bismuth silver nitrite, (NH 4 ) 2 BiAg(N0 2 ) 6 . Moderately sol. in H 2 O. Rapidly hydro- lyzed by H 2 O. (Ball and Abram, Chem. Soc. 1913, 103. 2120.) Ammonium bismuth sodium nitrite, 2NH 4 NO 2 , Bi(NO 2 ) 3 , NaNO 2 . Easily decomp. (Ball, Chem. Soc. 1905, 87. 761.) Ammonium cadmium nitrite ammonia, basic, 2NH 4 N0 2 , Cd(N0 2 ) 2 , Cd(OH) 2 , 2NH 3 . Decomp. by H 2 O. (Morin, C. R. 100. 1497.) Ammonium calcium cupric nitrite, (NH 4 ) 2 CaCu(NO 2 ) 6 . Ppt.; decomp. easily. Sol. in H 2 O. SI. sol. in alcohol. (Przibylla, Z. anorg. 1897, 15. 423.) Ammonium cobaltic nitrite, 3(NH 4 ) 2 O, Co 2 O 3 , 6N 2 3 +1^H 2 0. SI. sol. in H 2 O, decomp. in aq. solution on heating. (Rosenheim, Z. anorg. 1898, 17. 45.) +3H 2 0. Somewhat sol. in cold H 2 O; decomp. by boiling. Decomp. by cone. H 2 SO 4 , not by acetic or dil. mineral acids. (Erdmann, J. pr. 97. 405.) Ammonium cupric lead nitrite, CuPb(NH 4 ) 2 (NO 2 ) 6 . Stable at ordinary temp.; sol. in HNO 3 with decomp. 2.575 pts. are sol. in 100 pts. H 2 O at 20, or 2.51 %' salt in sat. solution at 20. (Przibylla, Z. anorg. 1897, 15. 420.) Ammonium cupric strontium nitrite, nonium cupric stron (NH 4 ) 2 CuSr(N0 2 ) 6 . Ppt.; sol. in H 2 O with decomp. (Przibylla, I. c.) Ammonium iridium nitrite. See Iridonitrite, ammonium. Ammonium lead nickel nitrite, (NH 4 ) 2 PbM(N0 2 ) 6 (?). Ppt. (Przibylla, Z. anorg. 1897, 15. 433.) Ammonium osmium nitrite. See Osminitrite, ammonium. Ammonium osmyl oxynitrite. See Osmyloxynitrite, ammonium. Ammonium platinum nitrite. See Platonitrite, ammonium. Ammonium rhodium nitrite. See Rhodonitrite, ammonium. Ammonium ruthenium hydrogen nitrite, Ru 2 H 2 (NO 2 ) 4 , 3NH 4 NO 2 +3H 2 O. See Rutheninitrite, ammonium hydrogen. Barium nitrite, Ba(NO 2 ) 2 +H 2 O. Permanent. Very sol. in H 2 O. Solubility in H 2 O at t. t G. in 100cc.Ba(NO 2 ) 2 Sp. gr. 20 25 30 35 58 63 71 82 97 1.40 1.45 1.50 1.52 1.61 (Vogel, Z. anorg. 1903, 35. 389. 100 pts. H 2 O dissolve at: 10 20 30 63.5 69.5 79.5 93 pts,. Ba(N0 2 ) 2 +H 2 O, 40 50 60 70 113 136 170 202 pts. Ba(NO 2 ) 2 +H 2 O, 90 100 110 331 461 765pts.Ba(NO 2 ) 2 +H 2 O. 80 254 The sat. solution at 17 contains 40% Ba(NO 2 ) 2 , and has sp. gr. 17/0 = 1.4897. (Oswald, A. ch. 1914, (9) 1. 62.) 100 g. H 2 O at 13.5 dissolve 64 g. Ba(N0 2 ) 2 +10.2 g. AgNO 2 with excess of AgN0 2 , and 75.6 g. Ba(NO 2 ) 2 +9.5 g. AgNO 2 , with ex- cess of AgNO 2 . (Oswald.) Sol. in 64 pts. 94% alcohol; nearly insol. in absolute alcohol. (Lang, Pogg. 118. 285.) Solubility in alcohol +Aq at t. t Solvent 100 ccm. of the sat. solution contain g. Ba(NO 2 ) 2 +H 2 O 19.5 10% alcohol 49.30 21.0 20% " 29.30 20.5 30% " 18.41 20.5 40% " 13.33 20.5 50% " 9.11 20.0 60% " 4.84 19.0 70% " 2.66 19.5 80% " 0.98 20.0 90% " 0.00 20.0 absolute alcohol 0.00 (Vogel, Z. anorg. 1903, 35. 390.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) NITRITE, CADMIUM POTASSIUM 623 Barium caesium nitrite, CsBa 2 (NO 2 )5. Sol. in H 2 O. (Jamieson, Am. Ch. J. 1907, 38. 616.) Cs 2 Ba(NO 2 ) 4 +H 2 O. Very sol. in H 2 O. (Jamieson, Am. Ch. J. 1907, 38. 616.) Barium caesium silver nitrite, Cs 3 AgBa(NO 2 ) 6 +2H 2 O. Decomp. by cold H 2 O. (Jamieson, Am. Ch. J. 1907, 38. 616.) Barium cobaltic nitrite, 2BaO, Co 2 O 3 , 4N 2 O 3 + 10H 2 O. Sol. in moderately warm H 2 without de- comp. but not recryst. therefrom. (Rosen- heim, Z. anorg. 1898, 17. 51-54.) 3BaO, Co 2 O 3 , 6N 2 O 3 +H 2 O. Ppt.; very un- stable. Nearly insol. in H 2 O. (Rosenheim, Z. anorg. 1898, 17. 47.) Barium cobaltous potassium nitrite, Ba(NO 2 ) 2 , Co(NO 2 ) 2 , 2KNO 2 . Decomp. by H 2 O. (Erdmann, J. pr. 97. 385.) Barium cupric nitrite, Ba[Cu(OH)(N0 2 ) 2 ] 2 . Ppt. Insol. in H 2 O. Decomp. by H 2 O. Insol. in alcohol, but slowly decomp. by it. (Kurtenacker, Z. anorg. 1913, 82. 208.) Barium cupric potassium nitrite, BaCuK 2 (NO 2 ) 6 . Stable when dry, easily decomp. when moist; sol. in H 2 O with decomp. 45.86 pts. are sol. in 100 pts. H 2 O at 20, or 31.45% salt is contained in sat. solution at 20. (Przibylla, Z. anorg. 1897, 15. 424.) Barium cupric thallium nitrite, BaCuTl 2 (NO 2 ) 6 . SI. sol. in H 2 O. (Przibylla, Z. anorg. 1898, 18. 461.) Barium iridium nitrite. See Iridonitrite, barium. Barium mercuric nitrite, 2Ba(NO 2 ) 2 , 3Hg(N0 2 ) 2 +5H 2 0. Very sol. in H 2 O and easily decomp. (Ray, Chem. Soc. 1910, 97. 327.) Barium nickel nitrite, 2Ba(NO 2 ) 2 , Ni(N0 2 ) 2 . Somewhat more easily sol. in H 2 O than nickel potassium nitrite. (Lang.) Barium nickel potassium nitrite, Ba(NO 2 ) 2 , Ni(NO 2 ) 2 , 2KNO 2 . SI. sol. in cold, easily in hot H 2 O without apparent decomp. (Lang.) Barium nickel thallium nitrite, NiBaTl 2 (NO 2 ) 6 Ppt. (Przibylla, Z. anorg. 1898, 18. 462.) Barium osmium nitrite. See Osminitrite, barium. Barium osmyl oxynitrite. See Osmyloxynitrite, barium. Barium potassium nitrite, Ba(NO 2 ) 2 , 2KNO 2 +H 2 0. Easily sol. in H 2 O; insol. in alcohol. (Lang, Pogg, 118. 293.) Barium rhodium nitrite, 3Ba(NO 2 ) 2 , Rh 2 (N0 2 ) 6 . See Rhodonitrite, barium. Barium silver nitrite, Ba(NO 2 ) 2 , 2AgNO 2 + H 2 O. Resembles the potassium salt. (Fischer.) Less stable than the Na salt. (Oswald.) Bismuth nitrite, basic, (BiO)NO 2 Sol. in HC1. (Vanino, J. pr. 1906, (2) 74. 150.) Bismuth caesium silver nitrite, Cs 2 BiAg(NO 2 ) 6 . Very si. sol. in H 2 O. Slowly decomp. by H 2 O. (Ball and Abram, Chem. Soc. 1913, 103. 2122.) Bismuth potassium nitrite, Bi(NO 2 ) 3 , 3KNO 2 +H 2 0. Decomp. by H 2 O. (Ball, Chem. Soc. 1905, 87. 762.) Bismuth potassium silver nitrite, K 2 BiAg(NO 2 ) 6 . Less sol. in H 2 O than NH 4 salt. (Ball and Abram, Chem. Soc. 1913, 103. 2121.) Bismuth rubidium silver nitrite, Rb 2 BiAg(NO 2 ) 6 . SI. sol. in H 2 O with slow hydrolysis. (Ball and Abram.) Bismuth silver thallous nitrite, BiAgTl 2 (NO 2 ) 6 . Insol. in H 2 O, but decomp. thereby. (Ball and Abram.) Cadmium nitrite, basic, 2CdO, N 2 O 3 . Insol. in H 2 O. (Hampe, A. 126. 335.) Cadmium nitrite, Cd(NO 2 ) 2 +H 2 O. Deliquescent. Sol. in H 2 O. (Lang, J. B. 1862. 99.) Cadmium potassium nitrite, Cd(NO 2 ) 2 , KNO 2 . Easily sol. in H 2 O. Very difficultly sol. in absolute alcohol, and only si. sol. in 90% alcohol. (Hampe, A. 125. 334.) Cd(N0 2 ) 2 , 2KN0 2 . Easily sol. in H 2 O. Insol. in alcohol. (Lang, J. B. 1862. 99.) Cd(NO 2 ) 2 , 4KNO 2 . More sol. in H 2 O than the above salt. (Lang.) 624 NITRITE, OESIUM Caesium nitrite, CsNO 2 . Very hydroscopic. Very sol. in H 2 O (Ball/Chem. Soc. 1913, 103. 2130.) Caesium calcium nitrite, Cs 2 Ca(NO 2 )4+H 2 O Ppt. (Jamieson, Am. Ch. J. 1907, 38. 617.; Caesium cobaltic nitrite, Cs 3 Co(NO 2 ) 6 -|-H 2 O. Sol. in 20,100 pts. H 2 O at 17. (Rosen- bladt, B. 19. 2531.) Caesium lead nitrite, CsPb(NO 2 ) 8 +H 2 O. Sol. in cold H 2 O without decomp. When solution is heated, some basic lead salt sep- arates. (Jamieson, Am. Ch. J. 1907, 38. 618.) Caesium lead silver nitrite, Cs 3 AgPb(NO 2 ) 6 + 2H 2 0. Ppt. (Jamieson.) Caesium silver nitrite, CsAg(NO 2 ) 2 . Decomp. by H 2 O. (Jamieson.) Caesium silver strontium nitrite, Cs 3 AgSr(NO 2 ) 6 +2H 2 O. Partially decomp. by H 2 O. (Jamieson.) Caesium strontium nitrite, CsSr(NO 2 ) 3 +H 2 O. Ppt. Sol. in H 2 O. (Jamieson.) Calcium nitrite, Ca(NO 2 ) 2 +H 2 O. Very deliquescent. Insol. in dil. alcohol. (Fischer, Pogg. 74. 115.) 100 ccm. of the sat. solution contain 111.6 g. Ca(NO 2 ) 2 +H 2 O at 20.5. (Vogel, Z. anorg. 1903, 35. 395.) Solubility in H 2 O at t. t %Ca(NO 2 )2 Solid phase 38.3 Ca(N0 2 ) 2 , 4H 2 18.5 43 u 42 51.8 it 44 54 53.5 55.2 " +Ca(N0 2 ) 2 , H 2 Ca(NO 2 ) 2 , H 2 O 64 58.4 70 60.3 " 73 61.5 it 91 71.2 (t (Oswald, A. ch. 1914, (9) 1. 32.) Sat. solution of Ca(NO 2 ) 2 +AgN0 2 con- tains 92.4 g. Ca(NO 2 ) 2 and 11.2 g. AgNO 2 per 100 g. H ? O at 14. (Oswald.) Solubility in alcohol. 100 ccm. of sat. solution in 90% alcohol contain 39.0 g. Ca(NO 2 ) 2 +H 2 O at 20. 100 ccm. of sat. solution in absolute alcohol contain 1.1 g. Ca(N0 2 ) 2 +H 2 O at 20. (Vogel.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) +4H 2 O. The sat. solution at 16 contains 42.3% Ca(NO 2 ) 2 and has sp. gr. at 16/0 = 1.4205. (Oswald, A. ch. 1914, (9) 1. 66.) Calcium cobaltous potassium nitrite, Ca(NO 2 ) 2 , Co(NO 2 ) 2 , 2KNO 2 . Decomp. by H 2 O. (Erdmann.) Calcium cupric potassium nitrite, CaCuK 2 (NO 2 ) 6 . Ppt., insoL in alcohol; sol. in H 2 O with, decomp. 14.97 pts. are sol. in 100 pts. H 2 at 20, or 13.02 per cent of salt is contained in sat. solution. (Przibylla, Z. anorg. 1897, 15. 422.) Calcium mercuric nitrite, Ca(NO 2 ) 2 ,Hg(N0 2 ) 2 +5H 2 0. Very sol. in H 2 O. (Ray, Chem. Soc. 1910, 97. 327.) Calcium nickel potassium nitrite, Ca(NO 2 ) 2 , Ni(N0 2 ) 2 , 2KN0 2 . Very si. sol. in cold, easily in hot H 2 O. Insol. in alcohol. SI. sol. in dil. HC 2 H 3 O 2 -J- Aq. (Erdmann.) Calcium osmium nitrite. See Osminitrite, calcium. Calcium potassium nitrite, CaK(NO 2 ) 3 + 3H 2 O. Sol. in H 2 O. (Topspe, W. A. B. 73, 2. 112.) Deliquescent. (Lang.) Cobaltous nitrite. Known only in solution. Cobaltic lead nitrite, 3PbO, Co 2 O 3 . 6N 2 O 3 -h 12H 2 0. Insol. in H 2 O. (Rosenheim, Z. anorg. 1898, 17. 48.) Cobaltic lead potassium nitrite, 3K 2 0, 3PbO, 2Co 2 O 3 , 10N 2 O 3 -f-4H 2 O. Sol. by boiling in much H 2 O. Sol. in hot acids with evolution of N 2 O 3 . (Stromeyer, A. 96. 228.) Cobaltous potassium nitrite, 2Co(NO 2 ) 2 , 2KN0 2 +H 2 0. Ppt. (Sadtler.) Co(N0 2 ) 2 , 2KN0 2 +H 2 0. Ppt. (Sadtler.) 3Co(NO 2 ) 2 , 6KNO 2 +H 2 O. Insol. in cold, >ol. in hot H 2 O. SI. sol. in KC 2 H 3 O 2 +Aq. 'Erdmann, J. pr. 97. 397.) Insol. in ethyl acetate. (Naumann, B. .904, 37. 3602.) Cobaltic potassium nitrite (cobalt yellow), Co 2 (NO 2 ) 6 , 6KNO 2 +3H 2 O. Very si. sol. in cold H 2 O. Insol. in alcohol md ether. Sol. in traces in CS 2 . (St. Evre, NITRITE, IRON LEAD THALLOUS 625 C. R, 36. 552.) Insol. in boiling cone. K 2 SO 4 , KC1, KNO 3 , or KC 2 H 3 O 2 +Aq. Sol. in 1120 pts. H 2 O at 17. (Rosenbladt, B. 1886, 19. 2535.) Decomp. when heated in aq. solution. (Rosenheim, Z. anorg. 1898, 17. 42.) More sol. in NH 4 C1 or NaCl+Aq than in H 2 O. (Stromeyer.) SI. decomp. by KOH+Aq, except when very cone.; easily decomp. by NaOH or Ba(OH) 2 +Aq. Very si. sol. in KC 2 H 3 O 2 +Aq, or KNO 2 +Aq. (Fresenius.) Sol. in HCl+Aq. Sol. in HC 2 H 3 O 2 , or H 2 C 2 4 +Aq. (Stro- meyer.) Small quantity of HC 2 H 3 O 2 +Aq does not dissolve. (Fresenius.) Cobaltic potassium silver nitrite, KCoAg 2 (NO 2 ) 6 , and K 2 CoAg(NO 2 ) 6 . Very si. sol. in H 2 O. Less sol. than Na comp. (Burgess and Karum, J. Am. Chem. Soc. 1912, 34. 653.) Cobaltous potassium strontium nitrite, Co(NO 2 ) 2 , 2KNO 2 , Sr(NO 2 ) 2 . Decomp. by H 2 O. (Erdmann, J. pr. 97. 385.) Cobaltic rubidium nitrite, Rb 3 Co(NO 2 ) 6 + H 2 O. Sol. in 19,800 pts. H 2 O. (Rosenbladt, B. 19. 2531.) Cobaltic silver nitrite, CoAg 8 (NOa). Fairly sol. in H 2 O. (Cunningham and Perkin, Chem. Soc. 1909, 95. 1568.) 2Ag 2 O, Co 2 O 3 , 3N 2 O 3 +3H 2 O. SI. sol. in H 2 O; decomp. by boiling H 2 O. (Rosenheim, Z. anorg. 1898, 17. 56.) Cobaltic silver hydroxynitrite, Co 2 Ag 3 (OH) 3 (N0 2 ) 6 . SI. sol. in H 2 O. (Suzuki, Chem. Soc. 1910, 97. 729.) Cobaltic silver nitrite ammonia, Co 2 O 3 , Ag 2 O, 4N 2 O 3 , 4NH 3 . See Cobalt ammonium comps. Cobaltic sodium nitrite, 2Na 2 O, Co 2 O 3 , 4N 2 O 3 . Sol. in H 2 O and alcohol. (Rosenheim, Z. anorg. 1898, 17. 50.) * +H 2 O. Ppt. (Sadtler, Sill. Am. J. (2) 49. 196). 3Na 2 O, Co 2 O 3 , 6N 2 O 3 +zH 2 O. Sol. in H 2 O; decomp. on heating; insol. in alcohol. (Rosen- heim, Z. anorg. 1898, 17. 43.) Cobaltic strontium nitrite, 2SrO, Co 2 O 3 , 4N 2 O 3 + 11H.O. Ppt. (Rosenheim, Z. anorg. 1898, 17. 54.) Cobaltic thallium nitrite, Co 2 (NO 2 ) 6 , 6T1NO 2 . Sol. in 23,810 pts. H 2 O at 17. (Rosen- bladt, B. 19. 2531.) Cobaltic zinc nitrite, 2ZnO, Co 2 O 3 , 3N 2 O S + 11H 2 O. Sol. in dil. acetic acid. (Rosenheim, Z. anorg. 1898, 17. 56.) Cobalt nitrite nitrate, 2CoO, Co 2 O 3 , 3N 2 O 3 , Co(NO 3 ) 2 +14H 2 O. Ppt. (Rosenheim, Z. anorg. 1898, 17. 58.) Cupric nitrite, basic, 2CuO, N 2 O 3 . (Hampe, A. 125. 345.) Cu(NO 2 ) 2 , 3Cu(OH) 2 . Very si. sol. in H 2 O or alcohol. Easily sol. in dil. acids or am- monia, (van der Meulen, B. 12. 758.) Cupric nitrite. Known only in solution. Cupric lead potassium nitrite, CuPbK 2 (NO 2 ) 6 . (van Lessen, R. t. c. 10. 13.) 3.056 pts. are sol. in 100 pts. H 2 O at 20, or 2.51% salt is contained in sat. solution at 20 p. 429. (Przibylla, Z. anorg. 1897, 15. 429.) Cupric potassium strontium nitrite, CuSrK 2 (NO 2 ) 6 . Sol. in H 2 O with decomp. 10.82 pts. are sol. in 100 pts. H 2 O at 20, or 9.77 per cent salt is contained in sat. solution at 20. (Przibylla, Z. anorg. 1897, 15. 425.) Cupric rubidium nitrite, Rb 3 Cu(NO 2 ) 5 . Easily sol. in H 2 O. Sol. in alcohol. (Kur- tenacker, Z. anorg. 1913, 82. 206.) Cupric nitrite ammonia, Cu(NO 2 ) 2 , 2NH 3 + 2H 2 O. Sol. in little H 2 O with absorption of much heat. Decomp. by much H 2 O. (Peligot, C. R. 53. 209.) 3CuO, N 2 O 3 , 2NH 3 +H 2 O. As above. (Peligot.) Iridium hydrogen nitrite, Ir 2 H 6 (NO 2 )i 2 . See Iridonitrous acid. Iridium nitrite with MNO 2 . See Iridonitrite, M. Iron (ferrous) lead potassium nitrite, FePbK 2 (NO 2 ) 6 . Ppt.; insol. in cold H 2 O; stable at ordinary temp. (Przibylla, Z. anorg. 1897, 15. 439.) Iron (ferrous) lead thallous nitrite, FePbTl 2 (NO 2 ) 6 . Ppt. (Przibylla, Z. anorg. 1898, 18. 463.) 626 NITRITE, LEAD, BASIC Lead nitrite, basic, 4PbO, N 2 O 3 +H 2 O = Pb(OH)NO 2 , PbO. Sol. in 143 pts. H 2 O at 23, and 33 pts. at 100. (Chevreul.) Sol. in 1250 pts. cold H 2 O, and 34.5 pts. at 100. (Peligot.) Sol. in cold HNO 3 or HC 2 H 3 O 2 +Aq. Composition is 3PbO, N 2 O 3 +H 2 O. (Meiss- ner, J. B. 1876. 194.) Composition is as above, (v. Lorenz, W. A. B. 84, 2. 1133.) 3PbO, N 2 O 3 = Pb(NO 2 ) 2 , 2PbO. Sol. in H 2 O. (Bromeis, A. 72. 38; v. Lorenz.) 2PbO, N 2 O 3 +H 2 O. SI. sol. in H 2 O. (Bromeis.) +3H 2 O. (Meissner.) 4PbO, 3N 2 O 3 -f-2H 2 O. Sol.inH 2 O. (Meiss- ner, J. B. 1876. 195.) Lead nitrite, Pb(NO 2 ) 2 +H 2 O. Easily sol. in H 2 O. (Peligot, A. ch. 77. 87.) Lead nickel potassium nitrite, Pb(NO 2 ) 2 , KNO 2 , Ni(NO 2 ) 2 . Insol. in H 2 O. (Baubigny, A. ch. (6) 17. 111.) Ppt. (Przibylla, Z. anorg. 1897, 15. 432.) Lead nickel thallous nitrite, NiPbTl 2 (NO 2 ) 6 . Ppt. (Przibylla, Z. anorg. 1898, 18. 462.) Lead potassium nitrite, 4Pb(NO 2 ) 2 , 6KNO 2 + 3H 2 O. Easily sol. in H 2 O and in absolute alcohol. (Hampe, A. 125. 334.) Pb(NO 2 ) 2 , 2KNO 2 +H 2 O. Easily sol. in H 2 O. Insol. in alcohol. (Lang, J. B. 1862. 102.) Lead potassium silver nitrite, K 3 AgPb(NO 2 ) 6 +2H 2 0. Ppt. (Jamieson, Am. Ch. J. 1907, 38. 619.) Lead nitrite nitrate. See Nitrate nitrite, lead. Lithium nitrite, LiNO 2 + 3^H 2 O. Deliquescent. Easily sol. in alcohol and H 2 O. (Vogel, Z. anorg. 1903, 35. 403.) Sat. solution of LiNO 2 +^H 2 O in H 2 O contains at: 65 81.5 91 96 92.5 63.8 68.7 72.4 91.8 94.3% LiNO 2 . (Oswald.) +H 2 O. Very sol. in H 2 O, readily forming supersat. solutions. Very sol. in abs. alcohol. (Ball, Chem. Soc. 1913, 103. 2133.) 100 pts. H 2 O dissolve at: 10 20 125 156 189 pts. LiNO 2 +H 2 O. 30 242 40 316 50 459 pts. LiNO 2 +H 2 O. LiNO 2 , H 2 O+Aq sat. at 19 contains 48.9% LiNO 2 and has sp. gr. = 1.3186. (Oswald, A. ch. 1914, (9) 1. 61.) 100 g. H 2 O dissolve 78.5 g. LiNO 2 +10.5 g. AgNO 2 at 14. (Oswald.) Lithium mercuric nitrite, LiNO 2 , Hg(NO 2 ) 2 + H 2 O. (Ray, Chem. Soc. 1907, 91. 2033.) 4LiNO 2 , Hg(NO 2 ) 2 +4H 2 O. Extremely deliquescent. (Ray.) Magnesium nitrite, Mg(NO 2 ) 2 -f2H 2 O. Deliquescent, and sol. in H 2 O. Solution decomp. by boiling. Easily sol. in absolute alcohol. (Hampe, A. 125. 334.) Insol. in absolute alcohol. (Fischer.) +3H 2 Q. Sol. in H 2 O and absolute alcohol. Very deliquescent. (Vogel, Z. anorg. 1903, 35. 397.) Magnesium osmium nitrite. See Osminitrite, magnesium. Magnesium potassium nitrite. Deliquescent, and easily sol. in H 2 O. Insol. in alcohol. (Lang.) Magnesium silver nitrite. Sol. in H 2 O with decomp. (Spiegel, Ch. Z. 1895, 19. 1423.) Manganous nitrite. Deliquescent, and sol. in H 2 O. (Mitscher- lich.) Not obtained in a solid state, as the solution decomp. on evaporation. (Lang, Pogg. 118. 290.) Mercurous nitrite, Hg 2 (NO 2 ) 2 . Sol. in H 2 O with partial decomp. to Hg and Hg(NO 2 ) 2 . (Ray, A. 1901, 316. 252.) Sol. in cold cone. HNO 3 . Very slowly sol. in cold dil. HNO 3 . (Ray, Chem. Soc. 1897, 71. 339.) Decomp. by boiling H 2 O and by cold dil. H 2 SO 4 . (Ray, Z. anorg. 1896, 12. 366.) +H 2 O. Slowly decomp. by H 2 O. (Ray, Chem. Soc. 1897, 71. 340.) Mercuric nitrite, basic, Hg(NO 2 ) 2 , 2HgO + H 2 O. Ppt. (Lang.) 12HgO, 5N 2 O 3 +24H 2 O. (Ray, Chem. Soc. 1897, 71. 341.) Mercuric nitrite, Hg(NO 2 ) 2 . Deliquescent. Partly sol. in boiling H 2 O, but the greater part is decomp. into HgO + HNO 2 . (Ray, Proc. Chem. Soc. 1904, 20. 57.) Mercuromercuric nitrite, basic, a. 9Hg 2 O, 4HgO, 5N 2 O 3 +8H 2 O. /3. Hg 2 O, 2HgO, N 2 O 3 +2H 2 O. (Ray, Chem. Soc. 1897, 71. 341.) NITRITE POTASSIUM 627 Mercuric potassium nitrite, Hg(NO 2 ) 2 Easily sol. in H 2 O. Insol. in alcohol (Lang, 1860.) KHg(NO 2 ) 3 . Obtained from K 3 Hg(NO 2 ) 6 H 2 0+Aq containing a small excess of KNO 2 Decomp. by H 2 O. (Rosenheim, Z. anorg 1901, 28. 173.) K 3 Hg(NO 2 ) 5 +H 2 O. Sol. in H 2 O. For mula of Lang is incorrect. (Rosenheim, Z anorg. 1901,28. 172.) Mercuric sodium nitrite, Na 2 Hg(NO 2 )4. Very hydroscopic. Decomp. by hot H 2 O (Rosenheim, Z. anorg. 1901, 28. 173.) +2H 2 O. Deliquescent. (Ray, Chem. Soc 1907, 91. 2032.) 2Hg(NO 2 ) 2 , 3NaNO 2 . Decomp. by H 2 O (Ray, Chem. Soc. 1907, 91. 2032.) Mercuric strontium nitrite, 3Hg(NO 2 ) 2 , 2Sr(N0 2 ) 2 +5H 2 0. Very sol. in H 2 O. (Ray, Chem. Soc. 1910 97. 327.) Mercuric nitrite hydrazine, Hg(NO 2 ) 2 , N 2 H 4 . Ppt. Decomp. by H 2 O. (Hofmann and Marburg, A. 1899, 305. 215.) Nickel nitrite, basic, 2NiO, N 2 O 3 . Ppt. (Hampe, A. 125. 343.) Nickel nitrite, Ni(NO 2 ) 2 . Sol. in H 2 O and alcohol. (Lang, J. B. 1862. 100.) Nickel potassium nitrite, Ni(NO 2 ) 2 , 4KNO 2 . Moderately sol. in H 2 O. (Fischer, Pogg. 74. 115.) Extremely sol. in H 2 O. (Hampe, A. 125. 346.) Insol. in absolute alcohol. Nickel potassium strontium nitrite, Ni(NO 2 ) 2 , 2KNO 2 , Sr(NO 2 ) 2 . SI. sol. in cold, easily sol. in hot H 2 O. Nickel nitrite ammonia, Ni(NO 2 ) 2 , 4NH 3 . Sol. in cold H 2 O. Decomp. on standing or by heating. Insol. in alcohol. Can be re- crystallized by dissolving in NH 4 OH+Aq, and adding much absolute alcohol. (Erd- mann, J. pr. 97. 395.) Ni(NO 2 ) 2 , 5NH 3 . Decomp. in the air giving Ni(NO 2 ) 2 , 4NH 3 . (Ephraim, B. 1913, 46. 3110.) Osmium nitrite, Os(NO 2 ) 3 . Ppt. (Wintrebert, C. R. 1905, 140. 587.) Osmium nitrite with MNO 2 . See Osminitrite, M. ! Osmyl nitrite with MNO 2 . See Osmylnitrite, M. Osmyl oxynitrite with MNO 2 . See Osmyloxynitrite, M. Osmyl nitrite ammonia, Os0 2 (NO 2 ) 2 , 4NH 3 . (Wintrebert, A. ch. 1903, (7) 28. 56.) Palladious nitrite with MNO 2 . See Palladonitrite, M. Platinous hydrogen nitrite, H 2 Pt(NO 2 ) 4 . See Platonitrous acid. Platinous nitrite with MNO 2 . See Platonitrite, M. Potassium nitrite, KNO 2 . Deliquescent. Sol. in H 2 O. Pure KNO 2 is not deliquescent. (Oswald, A. ch. 1914, (9) 1. 32.) Sol. in about l / 3 its wt. of H 2 O. (Divers, Chem. Soc. 1899, 75. 86.) 100 pts. H 2 O dissolve at: 10 20 30 40 281 291 302 313 325 pts. KNO 2 , 50 60 70 80 90 337.5 351 365 380 395 pts. KNO 2 , 100 110 120 130 413 432 451 473 pts. KNO 2 . Bpt. of sat. KNO 2 -fAq is 132 at 758.5 mm. pressure. (Oswald, A. ch. 1914, (9) 1. 58.) Sp. gr. of KNO 2 +Aq at 17.5 containing: 10 20 30 40% KN"O,. 1.049 1.126 1.208 40% KN0 2 , 1.295 50 1.377 60 70 1.491 1.599 (Oswald.) 74.5% KN"0 2 . 1.646 100 g. H 2 O at 13.5 dissolve 18 g. KNO 2 + 2.36 g. AgNO 2 ; at 25, 23.1 g. KNO 2 +5.3 g. A.gN0 2 with excess of AgNO 2 . 100 g. H 2 O at 13.5 dissolve 276 g. KNO 2 + 26.3 g. AgNO 2 ; at 25, 279 g. KNO 2 +39.3 g. A.gNO 2 with excess of KNO 2 . (Oswald.) See also under AgNO 2 . Very sol. in liquid NH 3 . (Franklin, Am. h. J. 1898, 20. 829.) Deliquesces in 90% alcohol; insol. in cold 94% alcohol. More sol. in H 2 O than KNO 3 , ut less sol. in alcohol. (Fischer.) Ppt. from its cone. aq. solution by the addition of methyl alcohol. Addition of sthyl alcohol to a cone. aq. solution of KNO 2 auses separation into two layers, of which he lower aq. solution contains 71.9% KNO 2 rhile the upper alcoholic layer contains 6.9% NO 2 . (Donath, Ch. Z. 1911, 35. 773.) Very si. sol. in acetone. (Krug and M'El- oy, J. Anal. Ch. 6. 184.) 628 NITRITE, POTASSIUM RHODIUM Insol. in acetone. (Eidmann, C. C. 1899, niOIA- "Maiiman-n "R 1 C\C\A V7 AQ9Q ^ Solubility in H 2 O at t. . iui-1, i\aumann, >. lyiM, of. lozy.; Insol. in methyl acetate. (Naumann, B. t % AgNO2 1909, 42. 3790); ethvl acejtate. (Naumann, B. 1904, 37. 3602.) 1 0.1589 15 0.2752 OT 412^ Potassium rhodium nitrite, 6KNO 2 , 3 s ) fiOlfi Rh 2 (N0 2 ) 6 . 51 1 . 0240 See Rhodonitrite, potassium. 60 1.3625 Potassium ruthenium nitrite. See Ruthenonitrite, potassium. Potassium silver nitrite, KNO 2 , AgNO 2 + Completely sol. in a little H 2 O, but decomp. by more H 2 '6. Sol. in KNO 2 +Aq without decomp. Insol. in alcohol. (Lang.) Potassium strontium nitrite, 2KNO 2 , Sr(N0 2 ) 2 . Sol. in H 2 O: insol. in alcohol. (Lang, Poge. 118. 293.) Potassium zinc nitrite, 2KNO 2 , Zn(NO 2 ) 2 + H 2 O. Deliquescent. Easily sol. in H 2 O. (Lang,. J. B. 1862. 101.) K 3 Zn(NO 2 ) 6 +3H 2 O. Very hydroscopic. Decomp. by H 2 O. (Rosenheim, Z. anorg. 1901, 28. 174.) Rhodium nitrite with MNO 2 . See Rhodonitrite, M. Rubidium nitrite, RbNO 2 . Deliquescent; very sol. in H 2 O; si. sol. in hot alcohol, almost insol. in acetone. (Ball, Chem. Soc. 1913, 103. 2131.) Ruthenium nitrite with MNO 2 . See Ruthenonitrite, M. Silver nitrite, AgNO 2 . Sol. in 120 pts. cold H 2 O (Mitscherlich), in 300 pts. (Fischer), and more abundantly in hot H 2 O. 1 1. H 2 O dissolves 3.1823 g. or 0.02067 g. mols. at 18. (Naumann and Riicker, B. 1905, 38. 2294.) 1 litre H 2 O dissolves at 8 14 16 18 25 33 0.0113 mol. AgNO 2 0.0159 0.0189 0.0203 0.0216 0.0260 (Pick and Abegg, Z. anorg. 1906, 61. 3.) 1 1. H 2 O dissolves 3.609 g. AgNO 2 at 21. (Oswald, A. ch. 1914, (9) 1. 33.) (Creighton and Ward, J. Am. Chem. Soc 1915, 37. 2335.) Solubility in AgNO 3 +Aq at 18. Mols. AgNOs per 1. of the solution Mols. AgNO2 dissolved per 1. 0. 0.0026 0.0052 0.0103 0.0207 0.0413 0.0827 0.0207 0.0198 0.0190 0.0169 0.0144 0.0117 0.0096 (Abegg and Pick, B. 1905, 38. 2573.) 1 1. 0.2-N NaNO 3 +Aq dissolves 4.956 g AgNO 2 at 25. (Ley and Schaefer, B. 1906 39. 1263.) 1 1. sat. KNO 2 +Aq dissolves 26% AgNO at 13.5. (Oswald, A. ch. 1914, (9) 1. 33.) Solubility in salts +Aq at 25. Salt AgN0 3 KNO 2 Cone, of the salt mols. per 1. 0.00258 0.00588 0.01177 0.02355 0.04710 0.00258 0.00588 0.01177 0.02355 0.04710 G.AgNOsinlOOg, of solution 0.4135 0.3991 0.3735 0.3432 0.2943 0.2498 0.3974 0.3820 0.3560 0.3119 0.2765 (Creighton and Ward, J. Am. Chem. Soc 1915, 37. 2336.) See also under KNO 2 . AgNO 2 +NaNO 2 . 1 1. 0.02 N-NaNO 2 +Aq dissolves 3.185 g, AgNO 2 at 25, 0.2-N NaNO 2 , 3.016 g. AgNO 2 . (Ley and Schaefer, B. 1906, 39. 1263.) 100 g. H 2 O sat. with AgNO 2 and Sr(N0 2 ) 2 contain 10.9 g. AgNO 2 and 78.3 g. Sr(N0 2 ) 2 at 14. (Oswald.) NITRITE, SODIUM 629 Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B, 1904, 37. 4328.) 100 pts. acetonitrile dissolve 23 pts. at ord. temp. ; 40 pts. at 81.6. (Scholl and Steinkopf, B. 1906, 39. 4393.) SI. sol. in methyl acetate. (Bezold, Dis- sert. 1906.) Insol. in ethyl acetate. (Hamers, Dissert. 1906; Naumann, B. 1910, 43. 314.) Silver sodium nitrite, AgNO 2 , NaNO 2 . Completely sol. in a little H 2 O, but decomp. by more H 2 O. (Fischer.) + ^H 2 O. (Oswald, A. ch. 1914, (9) 1. 75.) Silver nitrite ammonia, AgNO 2 , NH 3 . SI. sol. in H 2 O; less sol. in alcohol; nearly insol. in ether. (Reychler, B. 16. 2425.) AgNO 2 , 2NH 3 . (Reychler.) AgNO 2 , 3NH 3 . Deliquescent. Sol.inH 2 O. (Reychler.) Sodium nitrite, NaNO 2 . Not deliquescent. Very sol. in H 2 O. More sol. in H 2 O than NaNO 3 , but less in alcohol. 6 pts. H 2 O dissolve 5 pts. NaNO 2 at 15. (Divers, Chem. Soc. 1899, 76. 86.) 100 g. H 2 O dissolve 83.25 g. NaNO 2 at 15. (Niementowski and Roszkowski, J. phys. Ch. 1897, 22. 146.) 100 pts. H 2 O dissolve at : 10 20 30 40 73 78 84 91.5 98.5 pts. NaNO 2 , 50 60 70 80 107 116 125.5 136 pts. NaNO 2 , 90 100 110 120 147 160.5 178 198.5 pts. NaN0 2 . B-pt. of sat. NaNO 2 +Aq = 128 at 761.5 mm. pressure. Sat. solution at 20 has a sp. gr. = 1.3585. (Oswald, A. ch. 1914, (9) 1. 59.) Solubility in NaNO 3 +Aq at t. Solubility in NaNO 3 +Aq at t. Continued. t 100 pts. H 2 O dissolve NaN0 2 NaNOs 21 84.75 81.1 79.7 73.8 73.1 64.2 46.8 21.6 9.6 23.5 50.8 54.5* 56.7 62.8 74.7 89.3 52 108.8 107.9 104.3 101.8 99.5 98.0 97.8 65.2 44.2 27.2 14.7 6.7 20.6 34.5 43.2 62.6* 82.0 88.0 92.9 101.4 109 118 65 120.7 111.5 108.5 107.8 78.3 49.5 28.4 14.7 34.8 62.8 90.6* 96 104.1 113.4 121 A 131 81 137.1 125.7 122.7 122.6 79.1 50.0 27.2 38.8 69.8 101.0* 111.5 121.0 131.7 150 92 149.7 141.2 134.6 132.3 60.2 30.3 23.6 57.6 107.8* 130.6 145.0 163.5 100 pts. H 2 O dissolve t 103 166 153.3 148.8 142.4 100.0 60.1 33.2 58.8 116.0* 126.8 142.9 181.2 NaNOa NaNOs 73 .0 68.5 19 67.1 36.3 64.9 41.7* 50.3 46.8 30.2 55.4 74.2 * Both salts in solid phase. (Oswald, A. ch. 1914, (9) 1. 71.) 630 NITRITE, STRONTIUM Solubility in H 2 O is decreased by presence of Na 2 SO 4 . 100 pts. H 2 O dissolve 11.8 pts. Na 2 SO 4 +53.9 pts. NaNO 2 . (Oswald.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Neither dissolved nor attacked by liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) Sol. in warm 90% alcohol. (Hampe, A. 125. 336.) 100 pts. absolute methyl alcohol dissolve 4.43 pts. at 19.5; 100 pts. absolute ethyl alcohol dissolve 0.31 pt. at 19.5. (de Bruyn, Z. phys. Ch. 10. 783.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Strontium nitrite, Sr(NO 2 ) 2 . Very sol. in H 2 O, and very si. sol. in boiling alcohol. (Lang, Pogg. 118. 287.) Easily sol. in 90% alcohol. (Hampe, A. 125. 340.) +H 2 O. Hydroscopic. 100 ccm. of the sat. solution contain 62.83 g. Sr(NO 2 ) 2 +H 2 O at 19.5. (Vogel, 2,. anorg. 1903, 35. 393.) 100 pts. H 2 O dissolve at: 10 20 30 58.9 67.6 75.5 84 pts. Sr(NO 2 ) 2 +H 2 O, 40 50 60 70 94 105 116 130 pts. Sr(NO 2 ) 2 +H 2 O, 80 90 100 145 162 182 pts. Sr(NO 2 ) 2 +H 2 O. Bpt. of sat. solution is 112.5 at 763 mm pressure. The sat. solution at 19 contains 39.3% Sr(NO 2 ) 2 and has sp. gr. at 19/0 C 1.4461. (Oswald, A. ch. 1914, (9) 1. 64.) Solubility in alcohol. 100 ccm. of the solu- tion in 90% alcohol contain 0.42 g. Sr(NO 2 ) 2 +H 2 O at 20. 100 ccm. of the solution in absolute alcohol contain 0.04 g. Sr(NO 2 ) H 2 O at 20. (Vogel, Z. anorg. 1903, 35. 393.) Thallous nitrite, T1NO 2 . Sol. in H 2 O. Ppt. from solution in H 2 by absolute alcohol. (Togel, Z. anorg. 1903 35. 404.) Very sol. in H 2 O; insol. in alcohol. (Ball Chem. Soc. 1913, 103. 2131.) Zinc nitrite, basic, 2ZnO, N 2 O 3 . (Hampe, A. 125. 334.) Zinc nitrite, Zn(NO 2 ) 2 +3H 2 O. Deliquescent. Sol. in H 2 O and alcohol (Lang, J. B. 1862. 99.) Nitrous oxide, N 2 O. See Nitrogen monoxide. Nitroxyl bromide, NO 2 Br. Decomp. spontaneously or with H 2 O. Hasenbach, J. pr. (2) 4. 1.) Does not exist. (Frohlich, A. 224. 270.) Nitroxyl chloride, NO 2 C1. . Decomp. by H 2 O without evolution of gas. Probably does not exist. (Geuther, A. 245. 98.) Nitroxyl fluoride, NO 2 F. Absorbed by H 2 O with formation of HNO 3 and HF. Decomp. by H 2 O, alcohol, and ether. (Moissan and Lebeau, C. R. 1905, 140. 1624.) Nitroxypyrosulphuric acid, (HO)S 2 5 (N0 3 ), H 2 0. Very deliquescent. Sol. in H 2 O with de- comp. (Weber, Pogg. 142. 602.) Nitryl chloride, NO 2 C1. See Nitroxyl chloride* Octamine cobaltic compounds. The formulae of the following octamine cobaltic compounds should be reduced one- half, and they should be classed with the tetramine cobaltic compounds. (Jorgenseii, Z. anorg. 2. 279.) Octamine cobaltic carbonate, Co 2 (NH 3 ) 8 (CO 3 ) 6 +3H 2 O. Easily sol. in H 2 O. (Vortmann and Bias- berg, B. 22. 2654.) See Carbonatotetramine carbonate. Co 2 (NH 3 ) 8 O 3 (CO 3 ) 4 +3H 2 O. Rather diffi- cultly sol. in H 2 O. chloride (?)., Co 2 (NH 3 ) 8 (OH) 2 C1 4 4- 2H 2 O. Ppt. Co 2 (NH 3 ) 8 (OH) 2 Cl 4 , 2HgCl 2 . Co 2 (NH 3 ) 8 (OH) 2 Cl 4 , PtCl 4 +H 2 O. (Vort- mann and Blasberg, B. 22. 2654.) - mercuric chloride, Co 2 (NH 3 ) 8 Cl 6 3HgCl 2 +H 2 O. Co 2 (NH 3 ) 8 Cl 6 , HgCl 2 . Difficultly sol. ir cold H 2 O, decomp. on warming. (Vortmann.] chlorosulphite, Co 2 (NH 3 ) 8 (SO 3 ) 2 Cl ! +4H 2 0. Sol. in H 2 O. (Vortmann and Magdeburg, B. 22. 2635.) chromate, Co 2 (NH 3 ) 8 (CrO 4 ) 3 (H 2 O) 2 +2H 2 O. Sol. in H 2 O or acetic acid. +8H 2 O. Sol. in warm H 2 O or acetic acid Co 2 (NH 3 ) 8 (CrO 4 ) 2 Cr 2 q 7 (H 2 O) 2 +H 2 p. Eas : ily sol. in H 2 O, from which it is precipitatec by dil. HNO 3 +Aq. (Vortmann, B. 15. 5895.] OSMIAMIC ACID 631 Octamine cobaltic nitrate, Co 2 (NH3)8(NO 3 ) 6 +2H 2 0. Sol. in H 2 O; precipitated by cone. HNO 3 + Aq. (Vortmann.) nitratocarbonate, Co 2 (NH 3 ) 8 (N0 3 ) 2 (C0 3 ) 2 +H 2 0. Less sol. than other octamine carbonates, (Vortmann and Blasberg, B. 22. 2650.) See Carbonatotetramine cobaltic nitrate. purpureochloride, Co 2 (NH 3 ) 8 Cl 6 (H 2 0) 2 . Easily sol. in H 2 O; partly precipitated from ~>y cone. HC1 mann, B. 10. 1451.) aqueous solution by cone. HCl+Aq. (Vort- = Chlorotetramine cobaltic chloride, ClCo(NH 3 ) 4 (OH 2 )Cl 2 , wich see. (Jorgen- sen, J. pr. (2) 42. 211.) purpureomercuric chloride, Co 2 (NH 3 ) 8 Cl 6 (H 2 O) 2 , 6HgCl 2 . SI. sol. in cold, easily in hot H 2 O. (Vort- mann.) = Chlorotetramine cobaltic mercuric chlo- ride. (Jorgensen, J. pr. (2) 42. 211.) purpureomercuric hydroxychloride, Co 2 N 8 H 16 (HgCl)4(HgOH) 4 Cl 6 . Ppt. (Vortmann and Morgulis, B. 22. 2647.) Co 2 N 8 H 16 (HgOH) 8 Cl 6 . (V. and M.) Co 2 N 8 H 16 (HgOH) 8 Cl 4 (OH) 2 . (V. and M.) purpureomercuriodide, basic, Co 2 N 8 H 18 (HgOH) 6 I 6 . (Vortmann and Borsbach, B. 23. 2805.) purpureochloroplatinate . Very si. sol. in H 2 O. (Vortmann.) = Chlorotetramine cobaltic chloroplatinate, ClCo(NH 3 ) 4 (OH 2 )PtCl 6 +2H 2 O. (Jorgensen, J. pr. (2) 42. 215.) roseochloride, Co 2 (NH 3 ) 8 Cl 6 (H 2 O) 2 +2H 2 O, or 4H 2 O. Sol. in H 2 O. (Vortmann, B. 15. 1891.) See Roseotetramine cobaltic chloride. roseomercuric chloride, Co 2 (NH 3 ) 8 Cl 6 (H 2 0) 2 , 6HgCl 2 +3H 2 0. Ppt. (Vortmann.) roseomercuric hydroxychloride, Co 2 N 8 H ]6 (HgCl) 6 (HgOH) 2 Cl 6 . (Vortmann and Morgulis, B. 22. 2647.) Co 2 N 8 H 16 (HgOH) 8 Cl 6 . (V. and M.) Co 2 N 8 H 16 (HgOH) 8 Cl 4 (OH) 2 . (V. and M.) roseomercuric iodide, Co 2 N 8 H 2 ,(HgI) 3 I 6 . Ppt. Sol. in HC1 or HNO 3 . (Vortmann and Borsbach, B. 23. 2806.) Co 2 N 8 H 20 (HgI) 4 I 6 . Ppt. (V. and B.) Co 2 N 8 H 20 (H g I) 4 l4(OH) 2 . Ppt. (V.andB.) Octamine cobaltic sulphate, Co 2 (NH 3 ) 8 (OH) 2 (S0 4 ) 2 +3H 2 0. (?). Insol. in H 2 O or dil. H 2 SO 4 +Aq. Sol. in moderately cone. HCl+Aq. (Vortmann and Blasberg, B. 22. 2653.) Co 2 (NH 3 ) 8 (SO 4 ) 3 +6H 2 O. Sol. in H 2 O. (Vortmann.) +4H 2 O. Easily sol. in H 2 O. See Roseotetramine cobaltic sulphate. sulphatocarbonate, Co 2 (NH 3 ) 8 SO 4 (CO 3 ) 2 .+3H 2 O. Sol. in H 2 O. (Vortmann, B. 10. 1458.) See Carbonatotetramine cobaltic sulphate. Co 2 (NH 3 ) 8 (SO 4 ) 2 CO 3 +4H 2 O. Sol. in H 2 O. (Vortmann and Blasberg, B. 22. 2650.) ammonium sulphite, Co 2 (NH 3 ) 8 (SO 3 NH 4 ) 6 +10H 2 O. See Octamine cobaltisulphite, ammonium. Octamine cobaltisulphurous acid. Ammonium octamine cobaltisulphite, Co 2 (NH 3 ) 8 (SO 3 NH 4 ) 6 + 10H 2 O. Sol. in H 2 O. (Vortmann and Magdeburg, B. 22. 2632.) Co 2 (NH 3 ) 8 (S0 3 ) 2 (S0 3 NH 4 ) 2 +4H 2 0. Ammonium barium , Co 2 (NH 3 ) 8 (S0 3 ) 6 Ba 2 (NH 4 ) 2 +7H 2 0. Ppt. (V. and M.) Barium 7H 2 O, Ppt. (V. andM.) , Co 2 (NH 3 ) 8 (S0 3 ) 6 Ba 3 + Cobaltic Co 2 (NH 3 ) 8 (SO 3 ) 6 Co 2 +36H 2 O, and 24H 2 0. Luteocobaltic , Co 2 (NH 3 ) 8 (S0 3 ) 6 (NH 3 ) 12 Co 2 +8H 2 0. Ppt. (V. and M.) Octamine iridium chloride, Ir 2 (NH 3 ) 8 Cl 6 . Very, sol. in H 2 O. (Palmaer, B. 22. 16.) Octamine iridium chlorosulphate, Ir 2 (NH 3 ) 8 Cl 4 S0 4 +4H 2 0. (Palmaer.) Osmiamic acid, H 2 N 2 Os 2 O 6 , or H 2 N 2 Os 2 6 (?). Known only in aqueous solution, which is unstable. 632 OSMIAMATE, AMMONIUM Ammonium osmiamate. Easily sol. in H 2 O or alcohol. (Fritzsche and Struve, J. pr. 41. 97.) Barium osmiamate, BaN 2 Os 2 O 5 . Moderately sol. in H 2 O. Lead osmiamate. Ppt. Sol. in acids without decomp. Lead osmiamate chloride. Ppt. Mercurous osmiamate. Ppt. Mercuric osmiamate. Ppt. Potassium osmiamate, K 2 N2Os 2 O5, or K 2 N 2 Os 2 O 6 . 81. sol. in cold, much more easily in hot H 2 O. 81. sol. in alcohol. Insol. in ether. Silver osmiamate, Ag 2 N 2 Os 2 O 6 . Extremely si. sol. in H 2 O or cold HNO 3 + Aq. Sol. in NH 4 OH+Aq. Sodium osmiamate. Easily sol. in H 2 O or alcohol. Zinc osmiamate, ZnN 2 Os 2 O 5 . Decomp. by H 2 O. Nearly insol. in NH 4 OH +Aq. Osmic acid, H 2 OsO 4 . Stable in H 2 O containing alcohol. Sol. in HNO 3 or HCl+Aq. Not attacked by H 2 SO 4 -f Aq. (Moraht and Wischin, Z. anorg. 3. 153.) 100 g. H 2 dissolve 5,88 g. H 2 Os0 4 at 15. (Squire and Cains, Pharm. J. 1905, 74. 720.) Attacked by liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Barium osmate, BaOsO 4 +H 2 O. Insol. in H 2 O. (Glaus, Pogg. 65. 205.) Calcium osmate, CaOsO 4 . Insol. in H 2 O. (Fremy, J. pr. 33. 411.) Lead osmate. Insol. in H 2 O. (Fremy.) Potassium osmate, K 2 OsO 4 +2H 2 O. SI. sol. in cold, much more sol. in hot H 2 O, but is decomp. thereby. 81. sol. in KNO 2 + Aq. Insol. in dil. or cone, alcohol and ether. Fremy, A. ch. (3) 12. 516.) Insol. in cone, saline solutions. (Gibbs, Am. J. Sci. (2) 31. 70.) Sodium osmate, Na 2 OsO 4 . Sol. in H 2 O; insol. in alcohol and ether. (Fremy, /. c.) Perosmic acid. See Perosmic acid. Osminitrous acid. Ammonium osminitrite, (NH 4 ) 2 Os(NO 2 ) 5 + 2H 2 O. Sol. in H 2 O. Decomp. when solution is warmed. (Wintrebert, C. R. 1905, 140. 586.) Barium osminitrite, BaOs(NO 2 ) 5 . +H 2 O; +4H 2 O. (Wintrebert.) Calcium osminitrite, CaOs(NO 2 ) 5 +4H 2 O. (Wintrebert.) Magnesium osminitrite, MgOs(NO 2 ) 5 + 4H 2 O. (Wintrebert.) Potassium osminitrite, K 2 Os(NO 2 ) 5 . Very hygroscopic. Very sol. in H 2 O. Decomp. by HC1, HBr and HI. (Wintrebert, A. ch. 1903, (7) 28. 135.) Silver osminitrite, Ag 2 Os(NO 2 ) 5 +2H 2 O. 81. sol. in H 2 O with partial decomp. (Win- trebert, C. R. 1905, 140. 586.) Sodium osminitrite, Na 2 Os(NO 2 ) 6 -f-2H 2 O. Sol. in H 2 O. (Wintrebert.) Strontium osminitrite, SrOs(NO 2 ) 5 +2H 2 O. (Wintrebert.) Zinc osminitrite, ZnOs(NO 2 ) 5 +3^H 2 O. (Wintrebert.) Osmyloxynitrous acid. Ammonium osmyloxynitrite, (NH 4 ) 2 OsO 3 (NO 2 ) 2 . Decomp. by boiling cone. HC1 and by KOH +Aq. (Wintrebert, A. ch. 1903, (7) 28. 107.) Barium osmyloxynitrite, BaOsO 3 (NO 2 ) 2 + 4H 2 O. (Wintrebert.) Potassium osmyloxynitrite, K 2 OsO 3 (NO 2 ) 2 + 3H 2 0. 81. sol. in cold H 2 O. Aqueous solution de- comp. slowly. Sol. with decomp. in dil. KOH +Aq. (Wintrebert.) Silver osmyloxynitrite, Ag 2 OsO 3 (NO 2 ) 2 +H 2 O. (Wintrebert.) OSMIUM OXIDE 633 Strontium osmyloxynitrite, SrOsO 3 (NO 2 ) 2 + 3H 2 O. (Wintrebert.) Osmylnitrous acid. Potassium osmylnitrite, K 2 OsO 2 (NO 2 ) 4 . Decomp. by H 2 O and by excess of KOH+ Aq. (Weinland, A. ch. 19C3, (7) 28. 54.) Osmisulphurous acid. Potassium osmisulphite, [Os(H 2 O)(SO 3 ) 5 ]K 6 +4H 2 0. Ppt. (Rosenheim, Z. anorg. 1899, 21. 144.) Potassium hydrogen osmisulphite, [Os 2 (H 2 O)(SO 3 ) n ]K u H 3 +5H 2 O. Sol . in H 2 O without decomp . ( Rosenheim . ) [Os(SO 3 ) 6 ]K 6 H 2 +2H 2 O. Sol. in H 2 O with- out decomp. (Rosenheim.) Sodium osmisulphite, [Os(SO 3 ) 6 ]Na 8 +8H 2 O. Only si. sol. in H 2 O. [Os(H 2 O)(SO 3 ) 5 ]Na6+4H 2 O. Ppt. [OsO(SO 8 ) 4 ]Na-r-3H 2 O. Ppt. (Rosen- heim.) Osmium, Os. When finely divided and not ignited to a very high temperature, Os is sol. in HNO 3 + Aq or aqua regia. When ignited it is not at- tacked by any acid. Insol. in liquid NH 3 . (Gore, Am. ch. J. 1898, 20.. 828) Osmium ammonium comps. See Oxyosmiumamine comps., OsO(NH 3 ) 2 X. Oxyosmiumcfa'amine comps., OsO 2 (NH 3 )4X 2 . Osmium bromide with MBr. See Bromosmate, M. Osmium ^chloride, OsCl 2 . Deliquescent. Sol. in little, but decomp. by more H 2 O, with pptn. of Os. Sol. in cone, alkali chlorides +Aq with combination and partial decomp. (Berzelius.) Sol. in alcohol and ether. Insol. in H 2 O. Insol. in HC1 and H 2 SO 4 SI. sol. in HNO 3 and aqua regia. Slowly sol in strong alkali. Insol. in liquid C1 2 . Insol in alcohol and formaldehyde. (Ruff, Z. anorg 1910, 65. 455.) Osmium trichloride, OsCl 3 . Hydroscopic. Sol. in cone. H 2 SO4, HC1 anc cone. HNO 3 . Sol. in alkali and in NH 4 OH Insol. in liquid C1 2 . Easily sol. in alcohol SI. sol. in ether. (Ruff, Z. anorg. 1910, 65 453.) +3H 2 O. Sol. in H 2 O. (Moraht and Wis- chin, Z. anorg. 3. 153.) Osmium tefrachloride, OsCl 4 . Sol. in a little II 2 O, but decomp. by further addition of that solvent. Sol. in cone. HC1+ Aq. Osmium trichloride with MCI. See Chlorosmite, M. Osmium tetracbloride with MCI. See Chlorosmate, M. Osmium sodium chloride, Na 2 OsCl 6 +2H 2 O. Very sol. in H 2 O and in alcohol. (Rosen- heim, Z. anorg. 1899, 21. 133.) Osmium tefrafluoride, OsF*. Sol. in H 2 O. (Ruff, B. 1913, 46. 948.) Osmium fterrafluoride, OsF 6 . Decomp. by H 2 O and cone. H 2 SO 4 . Sol. in NaOH+Aq. (Ruff, B. 1913, 46. 945.) Osmium octofluoride, OsF 8 . Sol. in H 2 O, but is somewhat hydrolyzed. Sol. in cone. H 2 SO 4 with decomp. Sol. in NaOH+Aq. (Ruff, B. 1913, 46. 944.) Osmium worcohydroxide, OsO, zH 2 O. Insol. in H 2 O. SI. sol. in KOH+Aq. Slowly but completely sol. in acids. (Ber- zelius.) Osmium dihydroxide, OsO 2 , H 2 O. Sol. in HCl+Aq while still moist. Insol. in H 2 SO 4 or HNO 3 +Aq. +2H 2 O. Sol. in HC1, HNO 3 , or H 2 SO 4 + Aq while still moist. (Glaus and Jacoby.) Osmium sesgwihydroxide, Os 2 OeH6. Sol. in acids, and partly sol. in KOH+Aq. (Glaus and Jacoby.) Osmium iodide, Osl4. Extremely deliquescent. Sol. in H 2 O of alcohol, but solution is unstable. (Moraht and Wischin, Z. anorg. 3. 153.) Osmium potassium nitrosochloride, K 2 Os(NO)Cl 5 . Stable in aqueous solution. Only si. at- tacked by hot HNO 3 . (Wintrebert, A. ch. 1903, (7) 28. 132.) Osmium monoxide, OsO. Insol. in H 2 O or acids. (Glaus and Jacoby.) Osmium dioxide, OsO 2 . Insol. in H 2 O or acids. Osmium sesgiuoxide, Os 2 O 3 . Insol. in acids. (Glaus and Jacoby.) 634 OSMIUM OXIDE Osmium ^noxide, " Osmic acid," OsO 3 . See Osmic acid. Osmium tetroxide, " Perosmic acid," OsO 4 . Slowly but abundantly sol. in H 2 O. Sol. in alcohol and ether with gradual decomposition. Sol. in NH 4 OH+Aq, the solution undergoing decomposition on heating. Osmium oxide ammonia, OsO 2 , 2NH 3 +H 2 O. See Oxyosmiumamine hydroxide. Osmium oxysulphide, Os 3 S 7 O 5 +2H 2 O. Unstable. OsSO 3 +l^H 2 O. Insol. in H 2 O. (v. Meyer, J. pr. (2) 16. 77.) Os 2 O 2 S 2 +H 2 O. Decomp. and dissolved by HNO 3 , HC1, or H 2 SO 4 +Aq. (Moraht and Wischin, Z. anorg. 3. 153.) Osmium sulphide, Os 2 S 3 (?). (Berzelius.) Min. Laurite. Insol. in all acids, even in aqua regia. Osmium cfa'sulphide, OsS 2 . SI. sol. in H 2 O; not more sol. in alkali hydrates or carbonates +Aq. Insol. in al- kalies after drying. (Fremy, A. ch. (3) 12. 521.) Osmium tefrasulphide, OsS 4 +^H 2 O. Insol. in alkali sulphides, carbonates, or hydroxides +Aq. Sol. in cold dil. H,NO 3 + Aq. (Glaus.) Osmocyanhydric acid, H 4 Os(CN) 6 . Easily sol. in H 2 O and alcohol. Insol. in ether. (Martius, A. 117. 361.) Barium osmocyanide, Ba 2 Os(CN) 6 +6H 2 O. Easily sol. in H 2 O and dil. alcohol. (M.) Barium potassium osmocyanide, BaK 2 Os(CN) 6 +3H 2 O. Efflorescent. SI. sol. in cold, easily in hot H 2 O. Ferric osmocyanide, Fe 4 [Os(CN) 6 ] 3 +zH 2 O. Insol. in H 2 O. Potassium osmocyanide, K 4 Os(CN) 6 +3H 2 O. Moderately sol. in boiling, less in cold H 2 O. Insol. in alcohol and ether. Osmosyl ammonium comps. See Oxyosmium amine comps. Osmyl pottasium bromide, K 2 OsO2Br 4 + 2H 2 0. Same properties as the chloride. (Wintre- bert, A, ch. 1903, (7) 28. 94.) Osmyl potassium chloride, K 2 OsO 2 Cl 4 . Very sol. in H 2 O. Solution is stable only in the presence of a small amt. of HC1. De- :Comp. by hot cone. HC1. +2H 2 O. As the anhydrous salt. (Wintre- bert, A. ch. 1903, (7) 28. 86.) Osmyl c&tetramine comps. See Oxyosmium famine comps. Oxamidosulphonic acid. See Hydroxylamine wonosulphonic acid. Oximidosulphomc acid. See Hydroxylamine efosulphonic acid. Oxyamidosulphonic acid. See Hydroxylamine sulphonic acid. Oxyammonium salts. See Hydroxylamine salts. Oxycobaltamines, acid comps. (Maquenne, C. R, 96. 344.) Are anhydrooxycobaltamine comps., which see. (Vortmann, M. ch. 6. 404.) Oxycobaltamine chloride, Co 2 (NH 3 ) 10 ( gg ) Cl 4 . (Vortmann, M, ch. 6. 404.) Co 2 (NH 3 ) 10 O 2 Cl 4 , HC1+3H 2 O. Is anhy drooxycobaltamine chloride, which see. chloronitrate hydrochloride, Co 2 (NH 3 ) 10 (OH)(O.OH)(NO 3 ) 2 Cl 2 , 4HC1+3H 2 O. Is anhydrooxycobaltamine chloronitrate, which see. chlorosulphate, , 4HC1. Easily decomp. - iodide, Co 2 (NH 3 ) 10 ( (OH)) 14 - SI. sol. in H 2 O. Decomp. by much H 2 O. (Vortmann.) - nitrate, Co 2 (NH 3 ) 10 (OH)(O.OH)(NO 3 ) 4 +H 2 0. Decomp. by H 2 O. Co 2 (NH 3 ) 10 (OH)(O.OH)(N0 3 ) 4 , HNO 3 + 2H 2 O. Decomp. by H 2 O. nitratosulphate, Co 2 (NH 3 ) ]0 (OH)(O.OH)(SO 4 )(NO 3 ) 2 , 4HNO 3 . Decomp. at once by H 2 O. OXYGEN 635 Oxycobaltamine sulphate, Absorption of O by HaO. Continued Co 2 (NH 3 ) 10 O2(SO 4 ) 2 , H 2 SO 4 +H 2 O. t g 0i Very si. sol. in H 2 O with decomp.; more easily sol. in acidified H 2 O. Sol. in acids. (Maquenne, C. R. 96/344.) 14 15 16 0.3486 3415 3347 0.3431 3358 3288 CoatNHsho/Q^Q^) (SO 4 ) 2 +3H 2 O. 17 3283 3220 \ / 18 3?20 3155 Co 2 (NH 3 ) 10 ( ^ I) )(HS0 4 ) 4 . Decomp. 19 20 3161 3102 3093 3031 violently by H 2 O. 21 3044 2970 22 2988 2911 Oxygen, O 2 . 23 2934 2853 100 vols. H2O absorb 4.6 vols. O gas at ord. temp. 24 2881 2797 (Otto-Graham.) Sol. in 27 pts. H 2 O at ord. temp. (Pelouze and Fremy.) 25 26 2831 2783 2743 2691 100 vols. H 2 O dissolve 0.925 vol. O. (Gay-Lussac.) 27 2736 2641 1 vol. H 2 O at t and 760 mm. absorbs V vols. O gas, reduced to and 760 mm. 28 29 30 2691 2649 2608 2592 2545 2500 t V t V t V 31 2572 2459 32 (} c\f-r 0.04114 7 0.03465 14 0.03034 O^faf 33 2503 2380 1 0.04007 8 0.03389 15 0.02989 34 2471 2342 2 0.03907 9 0.03317 16 0.02949 35 2440 2306 3 0.03810 10 0.03250 17 0.02914 36 2410 2270 4 0.03717 11 0.03189 18 0.02884 37 2382 2236 5 0.03628 12 0.03133 19 0.02858 38 2355 2203 6 0.03544 13 0.03082 20 0.02838 39 2330 2171 40 41 2306 2280 2140 2107 (Bunsen's Gasometry.) Coefficient of absorption of O by H 2 O = 42 2256 2075 0.041 15-0.0010899t +0.000022563t 2 . (Bun- 43 2232 2043 sen and Pauli, A. 93. 21.) 44 2209 2012 Coefficient of absorption of O in H 2 O at 45 2187 1981 6.4 = 0.041408; at 12.6 = 0.036011. (Timofe- 46 2166 1952 jew, Z. phys. Ch. 6. 148.) 47 2145 1922 Absorption of O by H 2 O. Pi = " solubility," i. e., the amount of gas (reduced to and 760 mm.) which is absorbed by 1 vol. of the liquid when the barometer indicates 760 mm. pressure; j8 = coefficient of ab- sorption, i. e., amount absorbed by the liquid when the pressure of the gas itself without the tension of the liquid amounts 48 49 50 52 54 56 58 60 62 2126 2108 2090 2057 2026 1998 1971 1946 1921 1894 1865 1837 1782 1728 1674 1619 1565 1508 to 760 mm.; /3i=j8 760 ~ f . when f=va- 64 1897 1450 760 66 1874 1392 por tension of solvent at t. 68 pyf\ 1853 1332 70 1833 1270 t ft ft 72 *J A 1815 1208 0.04890 0.04860 74 76 1799 1785 1144 1078 1 4759 4728 78 1772 1010 2 4633 4601 80 1761 0939 3 4512 4479 82 1752 0865 4 4397 4362 84 1743 0788 5 4286 4250 86 1736 0707 6 4181 4142 88 1729 0622 7 4080 4040 90 1723 0532 8 3983 3941 92 1717 0437 9 3891 3847 94 1712 0337 10 3802 3756 96 1708 0231 11 3718 3670 98 1704 0119 12 3637 3587 100 7001 0000 13 3560 3507 (Winkler, B. 24. 3609.) OXYGEN Absorption of O by H 2 O at t and 760 mm. /3 = coefficient of absorption. ? ft t t |8 0.04961 23 0.03006 46 0.02163 1 4838 24 2956 47 2139 2 4720 25 2904 48 2115 3 4606 26 2855 49 2092 4 4496 27 2808 50 2070 5 4389 28 2762 51 2049 6 4236 29 2718 52 2029 7 4186 30 2676 53 2009 8 4089 31 2635 54 1990 9 3994 32 2596 55 1972 10 3903 33 2558 56 1955 11 3816 34 2521 57 1938 12 3732 35 2486 58 1922 13 3651 36 2452 59 1907 14 3573 37 2419 60 1893 15 3497 38 23 87 65 1832 16 3425 39 2356 70 1787 17 3357 40 2326 75 1752 18 3292 4J 2297 80 1726 19 3230 42 2269 85 1707 20 3171 43 2241 90 1693 2] 3114 44 2214 95 1684 22 3059 45 2188 100 1679 (Bohr and Bock, W. Ann. (2) 44. 318.) Coefficient of absorption of O by H 2 O be- tween and 30 = 0.04890 0.0013413t + 0.0000283t 2 0.00000029534t 3 . (Winkler, I. c.) Solubility in H 2 O at 25 =0.03080; at 15 = 0.03630. (Geffcken, Z. phys. Ch. 1904, 49. 269.) Absorption of O 2 by distilled- H 2 O at t. a = ccm. of O 2 absorbed by 1 1. of H 2 O at t and 760 mm. t a t a t a 49.24 17 33.21 34 25.19 1 47.94 18 32.58 35 24.85 2 46.65 19 32.01 36 24.52 3 45.45 20 31.44 37 24.20 4 44.31 21 30.91 38 23.89 5 43.21 22 30.38 39 23.59 6 42.15 23 29.86 40 23.30 7 41.15 24 29.38 41 23.02 8 40.19 25 28.90 42 22.75 9 39.28 26 28.42 43 22.49 10 38.37 27 27.94 44 22.24 11 37.51 28 27.51 45 22.00 12 36.75 29 27.08 46 21.77 13 35.98 30 26.65 47 21.55 14 35.26 31 26.27 48 21.34 15 34.55 32 25.90 49 21.14 16 33.88 33 25.54 50 20.95 (Fox, Trans. Faraday Soc. 1909, 5. 74.) Solubility in H 2 O at various pressures. V = volume of the absorbing liquid. P = Hg-pressure in metres. X = coefficient of solubility. V t P X 33.320 ccm. 23 0.9595 0.02937 1.0941 0.02939 1.2883 0.02938 1.4976 0.02935 1.7638 0.02939 2.0838 0.02931 2.5011 0.02928 3.0402 0.02909 3.8675 0.02886 4.2504 0.02872 4.6301 0.02855 5.1360 0.02832 5.6973 0.02818 6.1857 0.02797 6.7343 0.02772 7.3051 0.02741 7.7138 0.02729 8.1406 0.02708 32.003 ccm. 25.9 0.8611 0.02848 0.9808 0.02849 1.0833 0.02846 1.2039 0.02842 1.4112 0.02845 1.6602 0.02847 2.3854 0.02831 2.6482 0.02826 2.8995 0.02816 3.2883 0.02803 3.9133 0.02798 4.2720 0.02785 4.6905 0.02776 5.0559 0.02762 5.6141 0.02740 6.0120 0.02734 6.5687 0.02719 7.1056 0.02687 7.4729 0.02676 8.1889 0.02645 (Cassuto, Phys. Zeit. 1904, 5. 236.) Solubility of O in H 2 O at 25 = 0.0294. (Findlay and Creighton, Bioch. J. 1911, 5. 294.) Coefficient of absorption for H 2 O= 0.03398 at 15; 0.03375 at 15.3; 0.03330 at 16.2. (Miiller, Z. phys. Ch. -1912, 81. 494.) OXYGEN 637 Solubility in H 2 O at t. 1 760 = solubility of atmospheric O 2 in H 2 O at 760 mm. and t. 1 2 3 4 5 6 7 8 9 10 11 12 1760 10.26 9.99 9.73 9.48 9.25 9.02 8.80 8.59 8.39 8.20 8.02 7.84 7.67 13 14 15 16 17 18 19 20 21 22 23 24 25 1760 51 36 21 07 93 6.80 6.67 6.55 6.43 6.32 6.21 6.10 6.00 (Carlson, Zeit. angew. Ch. 1913, 26. 714.) Solubility of atmospheric O 2 in mixtures of distilled H 2 O with sea water diminishes regu- larly with the proportion of sea water present. (Clowes, J. Soc. Chem. Ind. 1904, 23. 359.) No. of ccm. of O 2 absorbed by 1 1. of sea water from a free dry atmosphere of 760 mm. pressure. Cl per 1000 G 4 8 12 16 20 .299 10 9.83 9.36 8. 8. 7.97 908 437 8 8.407 26 8.858.04 8.457.687 04 64 7.23 7.33 6.97 6.62 12 .68 7. .04 6. 6.43 11 366 746 10 7 .80 .52 .24 5.96 5.69 20 075 576.145.75 5.53 5.31 5.91 67 6.33 5.'825.445. 5.565.204 5.31 28 .86 4.954.62 (Fox, Trans. Faraday Soc. 1909, 5. 77.) For O absorbed from the air, see also air, atmospheric, p. 1. Absorption of O 2 by acids +Aq. M = content in gram-equivalents per litre. S = solubility. HNO,+Aq. M S25 S 15 0.492 0.494 1.00 1.008 1.88 1.901 0.03021 0.03016 0.02954 0.02963 0.02853 0.03478 0.03490 0.03354 0.03365 0.03175 0.03166 Absorption of O 2 by acids+Aq. Continued. HCl+Aq. M S25 S 15 0.578 0.579 1.170 1.176 1.736 1.982 0.02963 0.02960 0.02817 0.02833 0.02733 0.02674 0.03431 0.03410 0.03217 0.03109 0.03069 0.02988 H 2 S0 4 +Aq. 0.489 0.527 0.977 1.017 1.896 1.829 2.947 3.512 4.951 5.293 S 25 0.02887 0.02875 0.02757 0.02745 0.02545 0.02577 0.02285 0.02198 0.01918 S 15 0.03366 0.03375 0.03210 0.03217 0.02886 0.02930 0.02584 0.02399 0.02174 0.02067 (Geffcken, Z. phys. Ch. 1904, 49. 269.) Absorption of O 2 by H 2 SO 4 +Aq at t. a = coefficient of absorption. Normality of the acid 4.9 8.9 10.7 20.3 24.8 29.6 34.3 35.8 20.9 20.9 20.9 21.2 21.1 21.5 20.8 20.9 21.2 0.0310 0.0195 0.0155 0.0143 0.0119 0.0103 0.0117 0.0201 0.0275 (Bohr, Z. phys. Ch. 1910, 71. 49.) Absorption of O 2 by NaOH-fAq. M = content in gram-equivalents per litre. S = solubility. M 825 S 15 0.559 0.601 1.033 1.059 2.077 2.089 0.02434 0.02424 0.02020 0.01991 0.01295 0.01272 0.02777 0.02784 0.02291 0.02262 0.01479 0.01456 638 OXYGEN Absorption of O 2 by KOH+Aq. M S 25 S 15 0.577 0.579 1.157 1 . 170 0.02447 0.02435 0.01920 0.01914 0.02791 0.02791 0.02191 0.02181 (Geffcken, Z. phys. Ch. 1904, 49. 270.) NaCl+Aq with a chlorine content of 1,930 per 100,000 dissolved 82.9% of the amount of O 2 dissolved by distilled H 2 O alone. (Clowes, J. Soc. Chem. Ind. 1904, 23. 359.) Absorption of O 2 by salts +Aq. M = content in gram-equivalents per litre. S = solubility. Absorption of O= by K2 ^ 4 +Aq. M S25 S 15 0.499 0.506 0.968 0.970 0.025^8 0.02530 0.02096 0.02944 0.02922 0.02395 0.02377 Absorption of O 2 by NaCl+Aq. M S25 S 15 0.530 0.535 1.02C 1.034 1.880 1.890 1.921 0.02598 0.02604 0.02226 0.02202 0.01663 0.01654 0.03045 0.03052 1 0.02601 0.02557 0.01898 0.01904 0.01869 (Geffcken, Z. phys. Ch. 1904, 49. 270.) Solubility of O 2 in NaCl+Aq. Data indicate cc. O 2 dissolved per 1. 760 mm. and 0. at t NaCl +Aq 1 g. mol. per 1. NaCl +Aq 2 g. mol. per I. NaCl +Aq sat. at 20 5 10 15 20 25 30 6.50 5.80 5.25 4.77 4.39 4.06 3.76 3.14 2.84 2.59 2.41 2.25 2.13 2.01 1.27 1.22 1.17 1.12 1.07 1.02 0.97 (Winkler, Z. anorg. 1911, 24. 342.) Solubility of O 2 in KCN+Aq at 20 9 . % KCN 1 10 20 30 50 Coeff. of abs. 0.029 0.018 0.013 0.008 0.003 (McLaurin, J. S. C. I. 1893, 63. 737.) 1 vol. alcohol absorbs 0.28397 vol. O at all temperatures between and 24. (Bunsen.) Absorption by alcohol (99.7%) at t. = coefficient of absorption; Pi = solubility. (See p. 635.) t ft ft 0.23370 0.22978 1 0.23296 0.22878 2 0.23222 0.22777 3 0.23149 0.22675 4 0.23077 0.22572 5 0.23005 ' 0.22469 6 0.22934 0.22365 7 0.22863 0.22260 8 0.22793 0.22155 9 0.22724 0.22047 10 0.22656 0.21937 11 0.22588 0.21827 12 0.22521 0.21715 13 0.22455 0.21601 14 0.22389 0.21484 15 0.22324 0.21365 16 0.22259 0.21245 17 0.22195 0.21122 18 0.22132 0.20994 19 0.22069 0.20862 20 0.22007 0.20733 21 0.21946 0.20600 22 0.21886 0.20459 23 0.21826 0.20317 24 0.21767 0.20172 (Timofejew, Z. phys. Ch. 6. 151.) Solubility of O 2 in alcohol at 20 and 760 mm. Wt. % alcohol Vol.% abs. O 2 wt. % alcohol Vol. % abs. 2 0.0 9.09 16.67 23.08 28.57 2.98 2.78 2.63 2.52 2.49 33.33 50.0 66.67 80.0 2.67 3.50 4.95 5.66 (Lubarsch, W. Ann. 1889, (2) 37. 525.) Solubility of O 2 in methyl alcohol at t. t l. - t 1. 5 10 15 20 0.31864 0.30506 0.29005 0.27361 0.25574 25 30 40 50 0.23642 0.21569 0.16990 0.11840 (Levi, Gazz. ch. it. 1901, 31. II, 513.) Solubility of O 2 in ether at = 0.4235; at 10 =0.4215. (Christoff, Z. phys. Ch. 1912, 79. 459.) OXYMERCURIAMMONIUM CARBONATE 639 Solubility of O 2 in acetone at t. Absorption of O 2 by glucose +Aq. t = temp. of the solution. P = % glucose in the solution. t = coefficient of absorption at t. 20 = coefficient of absorption at 20. t l. t 1. 5 10 15 20 0.2997 0.2835 0.2667 0.2493 0.2313 25 30 40 50 0.2127 0.1935 0.1533 0.1057 t p /3t 20 21.2 21.5 19.9 20.5 21.7 10.84 20.7 33.8 51.9 58.84 0.02650 0.02202 0.01814 0.01378 0.01221 0.02690 0.02250 0.01815 0.01390 0.01250 (Levi, Gazz. ch. it. 1901, 31. II, 513.) Absorption of O 2 by chloralhydrate+Aq. t = temp. of the solution. P = % chloralhydrate in the solution. /3 t = coefficient of absorption at t. /3 15 = coefficient of absorption at 15. /3 20 = coefficient of absorption at 20. (Muller.) Absorption of O 2 by sucrose +Aq. t=temp. of the solution. P = % sucrose in the solution. j9 t = coefficient of absorption at t. 15 = coefficient of absorption at 15 C t P ftt ft 15 t P ftt ft 15 18.3 16.9 15.4 22.9 28.0 36.6 0.02759 0.02690 0.02590 0.02940 0.02800 0.02560 15.3 16.2 0.03375 0.03330 0.03400 0.03397 16.6 12.8 16.2 15.9 17.2 16.9 38.6 51.3 58.44 70.0 80.85 80.9 0.02402 0.02439 0.02350 0.02659 0.03200 0.03140 0.02477 0.02339 0.02407 0.02710 0.03300 0.03250 16.0 15.6 16.6 15.6 16.2 17.2 12.1 24.38 28.44 42.96 49.25 50.0 0.02911 0.02367 0.02113 0.01582 0.01348 0.01302 0.02969 0.02396 0.02181 0.01600 0.01380 0.01359 ft 20 (Muller.) 20.0 21.0 21.0 20.4 21.8 21.0 22.2 16.9 32.0 52.9 61.08 65.5 71.4 78.0 0.02795 0.02443 0.02375 0.02390 0.02500 0.02680 0.03090 0.02795 0.02495 0.02325 0.02410 0.02580 0.02730 0.03280 Abundantly absorbed by oil of turpentine. Oil of turpentine absorbs its own vol. O when exposed two weeks to the air, but does not give it off on boiling. (Brandes.) Absorbed by other oils, but this is decom- position rather than absorption, as the oils are oxidized. (See Storer's Diet.) (Muller, Z. phys. Ch. 1912, 81. 499.) 100 vols. arterial O. (Magnus.) blood dissolve 10-13 vols. Coefficient of absorption for petroleum = 0.202 at 20: 0.229 at 10. (Gniewasz and Absorption of O 2 by glycerine +Aq. Walfisz, Z. phvs. Ch. 1. 70.) t = temp. of the solution. P = % glycerine in the solution. ft t = coefficient of absorption at t. ft 15 = coefficient of absorption at 15. The author examined the solubility of O 2 and N 2 at low temp, in alcohols, ethers, ace- tone, CHC1 3 , petroleum, benzene and various inorganic liquids; at low temp, the solubility of the N 2 increases at the same rate as that of i'L /~\ //~il J s~*i T? i onn 1 9 1 /MO \ t P ftt ft 15 , 12.2 12.5 20.5 25.0 0.02904 0.02654 0.02742 0.02521 Oxyrfimercuriaminonium bromate, (NHg 2 OH 2 )BrO 3 . 14.6 37.3 0.02038 0.02022 (Rammelsberg, Pogg. 56. 82.) 13.5 45.0 0.01800 0.01744 12.4 52.0 0.01623 0.01570 - carbonate, (NHg 2 OH 2 ) 2 CO 3 + ^H 2 O. 12.1 13.3 71.5 88.5 0.01010 0.00906 0.00950 0.00886 Insol. in H 2 O. Decomp. by HCl+Aq only when cone. Not decomp. by boiling KOH + Aq. Decomp. by KI or K 2 S+Aq. (Hirzel.) (Muller.) +H 2 As above. (Hirzel.) 640 OXYMERCURIAMMONIUM CHLORIDE Oxycfomercuriammonium chloride, (NHg 2 OH 2 )Cl. Is dzmercuriammonium chloride, NHg 2 Cl + H 2 O, which see. oxy^nmercuriammonium chloride, (NHg,OH,)Cl, (NHg 3 2 H 2 )Cl (?). Insol. in H 2 O. Easily sol. in dil. HCl+Aq. More difficultly sol. in very dil. H 2 SO 4 or HNO 3 +Aq. .Insol. in cone. H 2 SO 4 . Sol. in boiling NH 4 Cl+Aq, or (NH 4 ) 2 SO 4 +Aq. De- comp. by KOH+Aq. (Schmieder.) chromate, (NHg 2 OH 2 ) 2 CrO 4 . Not decomp. by KOH+Aq. (Hirzel, J. B. 1852. 421.) mercuric chromate, (NHg 2 OH 2 ) 2 CrO 4 , 4HgO, 3CrO 3 . Decomp. by HNO 3 without going into solu- tion. Easily sol. in HC1. (Hirzel.) Composition is (NHg 2 OH 2 ) 2 O, 2Cr() 3 , 3[(NH 4 ) 2 0, 2Cr 2 3 ] = (NHg 2 OH 2 ) 2 Cr 2 O 7 , 3(NH 4 ) 2 Cr 2 O 7 . (Hensgen, R. t. c. 5. 187.) Probably (NHg 2 )oCr 2 O 7 , 3(NH 4 ) 2 Cr 2 O 7 + 2H 2 0. fluoride, acid, (NHg 2 OH 2 )F, HF. (Finkener, Pogg. 110. 632.) Probably NHg 2 F, HF+H 2 O. hydroxide, (NHgoOH 2 )OH = NHg 2 OH + H 2 O. (Millon's base.) SI. sol. in H 2 O, especially if warm. Sol. in 13,000 pts. H 2 O at 17, and 1700 pts. at 80. Insol. in alcohol or ether. (Gerresheim, A. 195. 373.) +H 2 O. Insol. in H 2 O or alcohol. Sol. in traces in NH 4 OH+Aq. Not decomp. by cold KOH+Aq; si. decomp. if hot. (Millon.) ammonium iodate, (NHg 2 OH 2 )IO 3 , 2NHJO 3 . Insol. in H 2 O. (Millon, A. ch. (3) 18. 410.) - iodide, (NHg 2 OH 2 )I. Sol. in warm HCl+Aq. Not decomp. by boiling KOH+Aq. Sol. in warm KI+Aq. (Rammelsberg, Pogg. 48. 170.) Correct formula is NHg 2 I+H 2 O. (Ram- melsberg.) nitrate, (NHg 2 OH 2 )NO 3 . Insol. in H 2 O; not decomp. by boiling KOH+Aq. Sol. in cold HCl+Aq, from which it is precipitated by H 2 O. SI. sol. without decomp. in HNO 3 or H 2 SO 4 +Aq Easily sol. in NH 4 OH+Aq. (Soubeiran.) Is dimercuriammonium nitrate, NHg 2 NO 3 . (Pesci, Gazz. ch. it. 20. 485.) ammonium nitrate, NHg 2 OH 2 )NO 3 , 2NH 4 NO 3 +H 2 O. Decomp. by H 2 O. Kane, A. ch. 72. 242.) Is dimercufiammonium ammonium nitrate NHg 2 NO 3 , 2NH 4 NO 3 +2H 2 O. (Pesci.) Oxycfo'mercuriammonium oxide, (NHg,OH,),0. Insol. in H 2 O or alcohol; not attacked by boiling cone. KOH + Aq. Sol. in hot NH 4 NO 3 + Aq, NH 4 C1 + Aq, (NH 4 ) 2 SO 4 + Aq, NH 4 C 2 H 3 O 2 +Aq, (NH 4 ) 2 C 2 O 4 +Aq. (Mil- Ion, A. ch. (3) 18. 397.) mercuric phosphate, Hg(NHg 2 OH 2 )PO 4 . Insol. in H 2 O. Slowly sol. in hot HNO 3 + Aq; not decomp. by boiling with KOH+Aq, but by KI or K 2 S+Aq. Sol. in HCl+Aq or much hot (NH 4 ) 2 HPO 4 +Aq. (Hirzel.) mercuric sulphite, (NHg 2 OH 2 ) 2 SO 3 . HgS0 3 . Insol. in H 2 O. Sol. in much (NH 4 ) 2 SO 3 + Aq. Sol. in HCl+Aq with decomposition. Insol. in boiling KOH+Aq. (Hirzel.) - sulphate, (NHg 2 OH 2 ) 2 SO 4 . Sol. in traces in H 2 O. Easily sol. in HC1 or HNO 3 +Aq. (Kane.) Insol. in HNO 3 +Aq. (Hirzel.) Slowly sol. in boiling cone. H 2 SO 4 . (Hir- zel.) Insol. in cone., easily sol. in dil. H 2 SO 4 + Aq. (Schmieder, J. pr. 76. 147.) Moderately sol. in much (NH 4 ) 2 SO 4 or boil- ing NH 4 Cl+Aq. Not decomp. by boiling KOH+Aq. (Hirzel.) Easily decomp. by boiling with dil. KOH + Aq. (Schmieder.) Does not. exist. (Pesci.) 2NH 3 , 2HgO, SO 3 . See Di'mercuriammonium sulphate. Oxytfn'mercuriammonium chloride, (NH g3 2 H 2 )Cl (?). Insol. in H 2 O. - nitrate, (NHg 3 O 2 H 2 )NO 3 . Sol. in cold HCl+Aq, from which it is pre- cipitated by NH 4 OH+Aq. Sol. in NH 4 OH + Aq without decomp. Not decomo. by H 2 SO 4 or warm KOH+Aq. (Pagenstecher.) Does not exist. (Pesci, Gazz. ch. it. 20. 485.) Oxyfrimercuridi'ammonium sulphate, 2NH 3 , 3HgO, SO 3 . See Tnmercuriammomum sulphate. Oxyfrimercurioxydimercuriammonium sulphate, Completely sol. in NH 4 Cl+Aq, or (NH 4 ) 2 SO 4 +'Aq. Sol. in dil. or cone. HC1 + Aq, and very dil. H 2 SO 4 +Aq. Insol. in HNO 3 +Aq or cone. H 2 SO 4 . (Schmieder.) Does not exist. (Pesci.) OZONE 641 Oxyfeframercuriammonium mercuric nitrate (?), 2(NHg 4 O 2 )NO 3 , HgNO 3 (?) Completely insol. in HNO 3 +Aq. Sol. in warm HCl+Aq. Slowly decomp. by boilin KOH-f-Aq. Graduallv sol. in hot cone NH 4 NO 3 +Aq. (Hirzel.) Does not exist. (Pesci, Gazz. ch. it. 485.) Oxynitrosulphonic anhydride, a ~ ^NO 2 /9 N Sol. in H 2 O with decomp. (Weber, Pogg 123. 339.) Oxyosmiumamine hydroxide (Osmo- sylcfa'amine hydroxide), OsO(NH 3 OH) 2 . Insol. in H 2 O. SI. sol. in acids. Sol. in KOH+Aq. When moist, sol. in NH 4 OH + Aq. Oxyosmiumdi'amine chloride (OsmylteJr- amine chloride), OsO 2 (N 2 H 6 Cl) 2 . SI. sol. in cold, more easily in hot H 2 O Insol. in NH 4 Cl+Aq. (Gibbs, Am. Ch. J 3. 233.) chloroplatinate, OsO 2 (N 2 H 6 Cl) 2 , PtCl 4 . SI. sol. in H 2 O. (Gibbs.) hydroxide, OsO 2 (N 2 H 6 OH) 2 . Known only in solution. nitrate, OsO 2 (N 2 H 6 NO 3 ) 2 . sulphate, OsO 2 (N 2 H 6 ) 2 SO 4 +H 2 O. (Gibbs, Am. Ch. J. 3. 233.) Oxyphosphuretted hydrogen (?), P 4 H(OH). P 4 O of Leverrier, and Goldschmidt has this formula according to Franke (J. pr. (2) 35. 341). Decomp. slowly by H 2 O or alkalies. Forms potassium salt, P 4 H(OK), sol. in H 2 O. - hydroiodide, P 4 H(OH), HI. Decomp. at 80. /Se6 1.010 1.015 1.020 1.90 2.77 3.61 1.240 1.245 1.250 33.85 34.40 34.95 1.470 1.475 1.480 54.89 55.18 55.56 U\J&y JL . J.jUO.y 1.025 4.43 1.255 35.49 1.485 55.95 1.030 5.25 1.260 36 03 1.490 56.32 Barium percarbonate, BaCO 4 . 1.035 6.07 1.265 36.56 1.495 56.69 Insol. in H 2 O. (Merck, C. C. 1906, II. 1.040 6.88 1.270 37.08 .500 57.06 1743.) 1.045 9.68 1.275 37.60 .505 57.44 Decomp. slowly in the air. Not rapidly 1.050 8.48 1.280 38.10 .510 57.81 decomp. by H 2 O. Rapidly decomp. by acids. 1.055 9.28 1.285 38.60 .515 58.17 ( Wolff enstein, B. 1908, 41. 280.) 1.060 10.06 1.290 39.10 .520 58.54 1.065 10.83 1.295 39.60 .525 58.91 Potassium percarbonate, K 2 CO 4 . Sol. in H 2 O with decomp. SI. sol. in al- cohol, (v. Hansen, Z. Elektrochem. 1897, 3. 1.070 1.075 1.080 1.085 11.58 12.33 13.08 13.83 1.300 1.305 1.310 1.315 40.10 40.59 41.08 41.56 .530 .535 .540 .545 59.28 59.66 60.04 60.41 448 ) K 2 C 2 O 6 . Sol. in H 2 O at with only slight decomp. but is decomp. at ord. temp. SI. sol. in alcohol. (Treadwell, Ch. Z. 1901, 26. inns "i 1.090 1.095 1.100 1.105 14.56 15.28 16.00 16.72 1.320 .325 .330 .335 42.03 42.49 42.97 43.43 .550 .555 .560 .565 60.78 61.15 61.52 61.89 \J\JO.) 1.110 17.45 .340 43.89 .570 62.26 1 115 18 16 345 44 35 .575 62.63 Rubidium percarbonate, Rb 2 CO 4 , 2H 2 O 2 + 1.120 18.88 .350 44.81 .580 63.00 H 2 O. .125 19.57 .355 45.26 .585 63.37 Hydroscopic; decomp. by H 2 O; pptd. by .130 20.26 .360 45.71 .590 63.74 alcohol. .135 20.95 .365 46.16 .595 64.12 Rb 2 CO 4 , H 2 O 2 +2H 2 O. Hydroscopic; de- .140 21.64 .370 46.61 .600 64.50 comp. by H 2 O; pptd. by alcohol. .145 22.32 .375 47.05 .605 64.88 Rb 2 CO 4 +2^H 2 O. Hydroscopic; decomp. .150 22.99 .380 47.49 .610 65.26 by H 2 O; pptd. bv alcohol. (Peltner, B. 1909, .155 23.65 1.385 47.93 .615 65.63 42. 1782.) .160 24.30 1.390 48.37 .620 66.01 Rb 2 C 2 O 6 . Very deliquescent. (Constam 1.165 24.94 1.395 48.80 .625 66.39 and Hansen, Z. Elektrochem. 1897, 3. 144.) 1.170 25.57 1.400 49.23 .630 66.76 1.175 26.20 1.405 49.68 1.635 67.13 Sodium percarbonate, Na 2 CO 4 +l}/H 2 O. Sol. in H 2 O with gradual decomp. (Tana- tar, B. 1899, 32. 1544.) 1.180 1.185 1.190 1.195 26.82 27.44 28.05 28.66 1.410 1.415 1.420 1.425 50.10 50.51 50.91 51.31 1.640 1.645 1.650 1.655 67.51 67.89 68.26 68.64 1.200 29.26 1.430 51.71 1.660 69.02 Sodium hydrogen percarbonate, 4Na 2 CO 4 , 1.205 29.86 .435 52.11 1.655 69.40 H 2 CO 3 . .210 30.45 .440 52.51 1.670 69.77 Ppt. (Merck, Chem. Soc. 1908, 94. (2) .215 31.04 .445 52.91 1.675 70.15 180.) .220 31.61 .450 53.31 .225 32.18 .455 53.71 Perchloric acid, HC1O 4 . .230 32.74 .460 54.11 Combines with H 2 O with a hissing sound and evolution of much heat. (Emster, Z. anorg. 1907, 62. 278.) PERCHLORATES Sp. gr. of HCK) t -f Aq. % HCK> Sp* gr. at 15 4 ; -V " mt304= 50 4 11.14 35.63 55.63 69 SI 1.0670 1.2569 1.4807 1 6708 1.2451 1.4637 1.0507 1.2292 1.4421 1 62S4 (Emster, Z. anorg. 1907, 62. 279.) Sp. gr. of HdO 4 -rAq. and boOs at 200* (Serollas): has -1.72-1.S2 sp. gr. and bofls at 200 Xativelle, J. pr. 26. Sol. in alcohol with decamp.; often explo- sive. +2MHiO. (v. Wyck.) . +3H,O. (T. Wyek.) (v.Wyek.) -7 E> 1 . 767': 1.7817 1 .7386 .6471 2901 1.1778 y-- IHH .7259 .7531 .7690 .7756 .7619 .7023 .6110 .5007 377- 1574 20 1.7716 1.7858 1.S100 .7425 Hi am 2927 1.1SOO .7312 .7475 .7751 .7912 .7m 7S40 .7237 6311 SIM 1 1715 Sr H by wt. CtOti* tfe 100 62 n 07 75.59 H ^2 n AX 50.51 39.73 27.07 AU perchkratCB are soL in HA KC1O*, 3\^1\_)^. J^TWI C^, 5\_ l\_/4 9QQftCWuftfc ^fimCPftty* They are all deliquescent, and sol in alcohol, excepting XH^CK)^ KClOt, Pb(CK))^ * Hg, CK.- (SerulLis, A. ch. (2) 46, 296.) Ahnn chl< te, Al Very deliquescent. (Weinland, Z. 1913, 84. 370.) sodiom ALN a dO^)^ SL hygroscopic. (Wcadand, Z. anorg. 1913, 84. 370. SoL in acetoaa. (NaMMon, B. 19Oi ? 37. OHL (T. Wyk, Z, of HC9O 4 +Aq. at mm 45. 4- 72.4 li v 65.2 61.2 56.65 3S.90 24 23 0.0 _:_;; 7: 4 4-0 :: 6.06 0.9 00 NH 7 181.2 162 3 1^0 132.4 114.8 106. S : :: (T. Wyfc. Z. anoKg. 1905, 48. 35.) Bpt. of BCX>4+Aq. at 18 mm. pn -. : - " H ' . . .- "T 5-- 100 -1 > .-: 1 >4 S 79.S 70.5 : : :- : :-i - -:. r 70 9(2 107 Permanent. SoL in 5 pts. HjO; aoLmafaohoL MJtorbrrtirii, Fog. 300.) of XH-> ~ l :-: -- -, 591.15 1 MB n us .193 .21ft .221 (Grin, S-.: 1911. 262.) (T. Wyk, Z. Mi I. 36 (Borne, A. 1H. O dboive 1&5 *^.*m 100 g. sat, solution in H/) contain 1.735 7^5?) g. XHdCK) a* l^T. (Tim and MMI Chan. Soc. 1915^ MT. 36L) InaoL in cone. HCK)+A< ::: r PERCHLORATE, HYDRAZINE 649 +3II 2 O. Solubility of Ba(ClO 4 ) 2 +3H 2 O in H 2 at t. Cobaltous perchlorate, Co(ClO 4 ),+9H 2 0. Solubility in H 2 O at t. t G.perlOOg.HjO Sp. gr. t G. anhydrous salt in 100 com. Sp. gr. of sat. solution at t/4 20 40 00 80 100 120 140 t r^ i t 1 206 9ft 308 432 497 .%! 645 758 1.782 1.912 2,009 2.070 2.114 2.155 2.195 2.230 30.7 21.3 + 7.5 18 26 45 83.14 90.57 100.13 101.92 103.80 113.45 115.10 1.5639 1.5658 1.5670 1.5811 1.5878 Bismuth perchlorate, (BiO)ClO 4 . Insol. in IL.O. Easily sol. in HC1 or HNO 3 +Aq, less c.'isilv in ir 2 SO 4 +Aq. (Muir, C. N. 33. 15.) Cadmium perchlorate, Cd(ClO 4 ) 2 . Very l-li(|iicscciil,. Sol. in H 2 () and al- cohol.' (Sri-alias, A. cli. 46. 305.) I III..O. (Salvadori, C. C. 1912, II. 414.) +(>K 2 0. (S.) Cadmium perchlorate ammonia, Cd(CK)4) 2 , Cd(ClO 4 ) 2 , 4NH 8 . (Salvadori, C. C. 1912, II. 114.) Caesium perchlorate, CsClO 4 . \ n-y si. sol. in H 2 O. (Rotgers, Z. phys. Ch. 8. 17.') Solubility in H,O. 100 g. H 2 O dissolve at: 8.5 14 33.7 42 50 O.'.M 1.19 2.99 4.09 5.47 g. CsClO 4 , 60 70 84 99 7.30 9.79 16.51 28.57 g. CsC10 4 . (Calzoliiri, Ace. Se. Med. Ferrara, 1911, 85. 150.) Solubility in H 2 O at t. t G. per 100 g. H 2 O Sp. gr. 5 25 80 0.97 2.05 17.05 1.007 1.010 1.084 (Carlson, Festsk. Stockholm, 1911. 262.) Calcium perchlorate, Ca(ClO 4 ) 2 . Very deliquescent. Very sol. in H 2 O and alcohol. (Scnillos, A. ch. 46. 304.) Cerous perchlorate, Ce(C10 4 ) 8 +8H 2 O. Very deliquescent. (Jolin.) Chromic perchlorate, Cr(ClO 4 ) 3 +6H 2 O. Very hygroscopic. (Weinland, Z. anorg. 1913,84. 371.) +91 U ). ( '.-in be crvst. from H 2 O. (Wein- land.) (Golblum and Terlikowsky, Bull. Soc. 1912, (4) 11. 146.) +6H 2 O. (Salvadori, Gazz. ch. it. 1912, 42. (1) 458.) Cobalt perchlorate ammonia, Co(ClO 4 ) 2 6NH 8 . Co(ClO 4 ) 2 , 5NH 8 . Co(ClO 4 ) 2 , 4NH 3 , and +2H 2 O. Co(ClO 4 ) 2 , 3NH 3 , and +3H 2 O. Co(ClO 4 ) 2 , 3NH 3 +2H 2 O. (Salvadori, Gazz. ch. it. 1912, 42. (1) 458.) Cupric perchlorate, basic, Cu(ClO 4 ) 2 , Cu(OH) 2 . Ppt. (Salvadori, C. C. 1912, II. 414.) Cupric perchlorate, Cu(ClO 4 ) 2 . Deliquescent. Sol. in H 2 O and alcohol. (Serullas, A. ch. 46. 306.) +4H 2 O. (Salvadori, C. C. 1912, II. 414.) Cupric perchlorate ammonia, Cu(ClO 4 ) 2 , 4NH 8 +2H 2 O. Not deliquescent. Sol. in NH 4 OH+Aq. (Roscoe, A. 121. 346.) Cu(ClO 4 ) 2 , NH 8 +H 2 O. Cu(ClO 4 ) 2 , 2CuO+2H 2 O, NH 3 . Cu(ClO 4 ) 2 , 2CuO+2H 2 O, 2NH 3 . Cu(ClO 4 ) 2 , Cu(OH) 2 +2H 2 O, 6NH 3 . Cu(C10 4 )i, Cu(OH) 2 +2H 2 0, 4NH 3 . (Salvadori, C. C. 1912, II. 414.) Didymium perchlorate, Di(ClO 4 ) 3 +9H 2 O. Very deliquescent. Very sol. in H 2 O and alcohol. (Cleve.) Erbium perchlorate, Er(ClO 4 ) 3 +8H 2 O. Very deliquescent. Glucinum perchlorate, G1(C1O 4 ) 2 +4H 2 O. Very deliquescent, and sol. in H 2 O. (Atter- berg.) Hydrazine perchlorate, (N 2 H 4 )(HC1O 4 ) 2 + 3H 2 O. 1 1. of sat. solution in H 2 O contains 417.2 g. at 18, sp. gr. = 1.264; 669 g. at 35, sp. gr. = 1.391. (Carlson, Festsk. Stockholm, 1911. 262.) 650 PERCHLORATE, INDIUM Indium perchlorate, In(ClO 4 ) 3 +8H 2 O. Deliquescent. H 2 O solution decomp. at 40 with separation of basic salt. Sol. in H 2 O and easily forms sat. solutions. Sol. in abs. alcohol, but much less sol. in ether. (Mathers, J. Am. Chem. Soc. 1908, 30. 212.) Iodine perchlorate, I(C1O 4 ) 3 +2H 2 O. Decomp. by H 2 O. Indifferent toward or- ganic solvents. (Fichter, Z. anorg. 1915, 91. 135.) Iron (ferrous) perchlorate, Fe(C10 4 )2. Tolerably permanent; sol. in H 2 O. (Serul- las, A. ch. 46. 335.) Iron (ferric) perchlorate, Fe(ClO 4 ) 3 . Sol. inH 2 O. (Serullas.) Iron (ferric) sodium perchlorate, [Fe(ClO 4 ) 4 ]Na+6H 2 O. Hydroscopic. Can be cryst. from H 2 O. (Weinland, Z. anorg. 1913, 84. 366.) Lanthanum perchlorate, La(ClO 4 ) 3 +9H 2 O. Extremely deliquescent. Sol. in H 2 O and absolute alcohol. (Cleve.) Lead perchlorate, basic, 2PbO, C1 2 O 7 + per H 2 O. Decomp. by H 2 O into an insol. more basic salt, and sol. Pb(ClO 4 ) 2 . (Marignac.) Lead perchlorate, Pb(ClO 4 ) 2 +3H 2 O. Permanent; extremely easily sol. in H 2 O. (Roscoe, A. 121. 356.) Sol. in about 1 pt. H 2 O. (Serullas.) Lithium perchlorate, LiClO 4 . Deliquescent. Sol. in H 2 O and alcohol. (Serullas.) +3H 2 O. (Wyrouboff, Zeit. Kryst. 10. 626.) Magnesium perchlorate, Mg(C10 4 ) 2 . Deliquescent, and sol. in H 2 O and alcohol. (Serullas.) +6H 2 O. (Weinland, Z. anorg. 1913, 84. 372.) H 2 O. Decomp. by alcohol. (Chikashige", Chem. Soc. 1895, 67. 1016.) +6H 2 O. Very deliquescent. (Roscoe, A. 121. 356.) Permanent. (Serullas.) Mercuric perchlorate, basic, HgO, 2Hg(C10 4 ) 2 . Anhydrous. Ppt. Insol. in either HC1 or HNO 3 . Decomp. and dissolved by a mixture of the two. (Chikashige", Chem. Soc. 1905, 87. 824.) + 12H 2 O. Very sol. in H 2 O. (Chikashige".) 2HgO, Hg(C10 4 ) 2 . a-salt. Decomp. by H 2 O. Sol. in acids. (Chikashige", Chem. Soc. 1895, 67. 1015.) /3-salt. Insol. in H 2 O; insol. in HC1 or HNO 3 . (Chikashige", Chem. Soc. 1905, 87. 825.) Mercuric perchlorate, Hg(ClO 4 ) 2 . Very deliquescent. Sol. in H 2 0; si. sol. with decomp. in alcohol. (Serullas, A. ch. 34. 243.) +6H 2 O. Very hygroscopic. Very sol. in H 2 O. Slowly decomp. by H 2 O, more easily by alcohol. (Chikashige", Chem. Soc. 1895, 67. 1014.) Mercuric perchlorate bromide, HgC10 4 Br. Decomp. by H 2 O. (Borelli, Gazz. ch. it. 1908, 38. (2) 421.) Mercuric perchlorate cyanide, Hg(ClO 4 ) 2 , Hg(CN) 2 . Very sol. in H 2 O. Sol. in alcohol. (Borelli.) Mercuric perchlorate iodide, Hg(C10 4 )I. Deliquescent. Decomp. by H 2 O. Sol. in much alcohol. Decomp. by HNO 8 . Com- pletely sol. in KI or KCN-f-Aq. (Borelli.) Mercuric perchlorate sulphocyanide, Hg(C10 4 ) 2 , Hg(SCN) 2 . Insol. in H 2 O and cone, acids. Sol. in aqua regia. (Borelli.) +6H 2 0. (Salvadori, C. C. 1912, II. 414.) Nickel perchlorate, Ni(ClO 4 ) 2 . Deliquescent; easily sol. in alcohol and H 2 O. (Groth, Pogg. 133. 226.) Manganous perchlorate, Mn(ClO 4 ) 2 . ouiu.uiiiu.y 111 j.j. 2 v_/ ai> u . Very deliquescent. Sol. in H 2 O and al- cohol. (Serullas, A. ch. 46. 335.) t G. anhydrous salt in 100 ccm. Sp. gr. of the sat. solution +6H 2 O. Sol. in 0.342 pts.H 2 O. (Salvadori, C. C. 1912, II. 414.) 30.7 21.3 89.98 92.48 Manganous perchlorate ammonia, Mn(ClO 4 ) 2 , 5NH 3 +H 2 O. +7.5 18 104.55 106.76 110.05 1.5726 1.5755 1 . 5760 Sol. in HC1; insol. in HNO 3 . (Salvadori, 26 112.15 1.5841 C. C. 1912, II. 414.) 45 118.60 1 . 5936 Mercurous perchlorate, (HgClO 4 ) 2 +4H 2 O. (Golblum and Terlikowsky, Bull. Soc. 1912, Very sol. in H 2 O. Gradually decomp. by (4) 11. 147.) PERCHLORATE, POTASSIUM 651 -f 5H 2 O. (Golblum and Terlikowsky.) +6H 2 O. (Salvador!, C. C. 1912, II. 414.) +9H 2 O. (Golblum and Terlikowsky.) Nickel perchlorate, 6NH 3 . Ppt. (Salvadori.) ammonia, Ni(ClO 4 ) 2 Nitrosyl perchlorate, NO.O.C1O 8 +H 2 O. Ppt.; si. hydroscopic; decomp. by H 2 O (Hofmann, B. 1909, 42. 2032.) Platinum perchlorate, Pt 6 ClO 9 +15H 2 O. Insol. in H 2 O. (Prost, Bull. Soc. (2) 46 156.) Potassium perchlorate, KC1O 4 . Sol. in 57.9 pts. H 2 O at 21.3 (Longuinine, A. 121 123) ; in 65 pts. H 2 O at 15 (Serullas, A. ch. (2) 46. 297) ; in 88 pts. H 2 O at 10; in 55 pts. H 2 O at 100 (Hutstein, J. B. 1851. 331.) Solubility in H 2 O. 1 pt. KC1O 4 dissolves in 142.9 pts. H 2 O at 6, and solution has sp. gr. = 1.0005; in 52.5 pts. H 2 O at 25, and solution has sp. gr. = 1.0123; in 15.5 pts. H 2 O at 50, and solution has sp. gr, = 1.0181; in 5.04 pts. H 2 O at 100, and solution has sp. gr. = 1.0660. (Muir, C. N. 33. 15.) 1 1. H 2 O dissolves 78.07 millimols. KC1O 4 at 10; 120.4 millimols. at 20; 179.9 milli- mols. at 30. (Noyes and Sammet, Z. phys. Ch. 1903, 43. 538.) 1 1. H 2 O dissolves 0.1475 mol. KC1O 4 at 25. (Rothmund, Z. phys. Ch. 1909, 69. 539.) Solubility in H 2 O at t. 10 15 20.5 G. KC1O 4 in 100 g. H 2 0.70 1.14 1.54 1.90 50 70 99 G. KC1O 4 in 100 g. H 2 O 6.45 12.3 22.2 (Calzolari, Ace. Sci. Med. Ferrara, 1911, 85. 150.) t G.perlOOg.H 2 O Sp. gr. 0.79 1.007 20 1.80 1.011 40 4.81 1.022 60 8.71 1.033 80 14.78 1.053 100 20.98 1.067 (Carlson, Festsk. Stockholm, 1911. 262.) 1 1. H 2 O dissolves 0.1481 equivalents KC1O 4 at 25. (Noyes and Boggs, J. Am. Chem. Soc. 1911, 33. 1652.) 100 cc. of sat. solution of KC1O 4 in H 2 O con- tains 2.085 g. KC1O 4 at 25.2. (Thin and Gum- ming, Chem. Soc. 1915, 107. 361.) KC1O 4 is sol. in 22.C pts. H 2 O at ord. temp., and 4.00 pts. at 100; in 29.6 pts. NH 4 OH + Aq (cone.) at ord. temp.; in 30.4 pts. NH 4 OH +Aq (1 vol. cone. +3 vols. H 2 O) at ord. temp.; in 22.4 pts. HNO 3 -j-Aq (1 vol. conc.+ 5 vols. H 2 O) at ord. temp., and 5.00 pts. at 100; in 30.4 pts. HCl+Aq. (1 vol. conc.+ 4 vols. H 2 O) at ord. temp.; 45.2 pts. HC 2 H 3 2 +Aq (1 vol. commercial acid-j-1 vol. H 2 O) at ord. temp.; in 24.4 pts. NH 4 C 2 H 3 O 2 +Aq. (dil. HC 2 H 3 O 2 +dil. NH 4 OH+Aq) at ord. temp., and 6.00 pts. at 100; in 25.6 pts. NH 4 Cl+Aq (1 pt. NH 4 C1+ 10 pts. H 2 O) at ord. temp., and 6.00 pts. at 100; in 16.0 pts. NH 4 NO 3 +Aq (1 pt. NH 4 NO 3 +10 pts. H 2 O) at ord. temp., and 4.00 pts. at 100; in 25.6 pts. NaC 2 H 3 O 2 +Aq (cone. HC 2 H 3 O 2 + Na 2 CO 3 +4 vols. H 2 O) at ord. temp., and 7.00 pts. at 100; in 29.2 pts. Cu(C 2 H 3 O 2 ) 2 + Aq (Stolba, Z. anal. 2. 390) at ord. temp., and 7.00 pts. at 100; in 27.2 pts. cane sugar (1 pt.+lO pts. H 2 O) at ord. temp.; in 36.8 pts. grape sugar (1 pt. + lO pts. H 2 O) at ord. temp. (Approximate.) (Pearson, Zeit. Chem. 1869. 662.) Solubility of KC1O 4 in HC10 4 at 25.2. Normality of HC1O< 0.01 0.10 1.00 1.999 1.485 0.527 (Thin and Gumming, Chem. Soc. 1915. 107. 361.) Solubility in KCl+Aq at 25. Concentration of KC1 Equivalents per litre 0.04973 0.09933 Solubility of KCJ04 Equivalents per litre 0.1282 0.1123 (Noves and Boggs, J. Am. Chem. Soc. 1911, 33. 1652.) Solubility in K 2 SO 4 +Aq at 25. Concentration of K 2 SC>4 Equivalents per litre 0.04970 0.09922 Solubility of KC1O 4 Equivalents per litre 0.1315 0.1181 (Noyes and Boggs.) Very si. sol. in abs. alcohol, and insol. if alcohol contains trace of an acetate. (Ros- coe ) Insol. in alcohol of 0.835 sp. gr. (Schlos- ing, C. R. 73. 1269.) Sol in 6400 pts. 97.2% alcohol; in 5000 pts. 95.8% alcohol; in 2500-3000 pts. 90% alcohol; in 25,000 pts. alcohol-ether (2 pts. 1 pt. ether). Practically insol. 652 PERCHLORATE, POTASSIUM RUBIDIUM in an alcoholic solution of HC1O 4 . (Wenze' Z. angew. Ch. 1891. 691.) Solubility of KC1O 4 in ethyl alcohol +Aq at 25.2. Solubility in H 2 O at t. t G. in 100 g. H 2 Sp. gr. 1.10 20 1.56 - 40 3.26 60 6.27 80 11.04 100 15.75 1.007 1.010 1.017 1.028 1.050 1.070 Vol. % alcohol soLin^O^aicoho, 51.2 93.5 98.8 0.754 0.051 0.019 (Carlson, Festsk. Stockholm, 1911. 262.) Scandium perchlorate. (Crookes, Roy. Soc. Proc. 1908, 80. A, 518.) Silver perchlorate, AgClO 4 . Deliquescent. Sol. in H 2 O and alcohol. (Serullas, A. ch. 46. 307.) Sodium perchlorate, NaClO 4 . Deliquescent, and very sol. in H 2 O and alcohol. (Serullas.) Not deliquescent. (Potilitzin, J. russ. Soc. 1889, 1. 258.) Solubility in H 2 O at t. (Thin and Gumming, Chem. Soc. 1915, 107. 361.) Solubility in organic compds.+Aq. at 25. Solvent Mol. KC1O 4 sol. in 1 litre 0.5-N methyl alcohol ethyl alcohol propyl alcohol tert. amyl alcohol acetone ether glycol glycerine urea ammonia diethylamine pyridine urethane formamide acetamide acetic acid phenol l methylal methyl acetate 0.1402 0.1356 0.1343 0.1279 0.1451 0.1336 0.1416 0.1404 0.1510 0.1474 0.1342 0.1410 0.1400 0.1539 0.1447 0.1462 0.1362 0.1400 0.1429 f0 G. in 1 1. of solution Sp. gr. 15 1076 50 1234 143 1414 1.666 1.731 1.789 (Carlson, Festsk. Stockholm, 1911. 262.) +H 2 O. Not deliquescent. (Potilitzin.) Strontium perchlorate, Sr(ClO 4 ) 2 . Very deliquescent. Sol. in H 2 O and al- cohol. (Serullas, A. ch. 46. 304.) (Rothmund, Z. phys. Ch. 1909, 69. 539.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Potassium rubidium perchlorate, KRb 2 (ClO 4 )s. 15.5 g. are contained in 1 1. solution sat. at 20; sp. gr. = 1.013. (Carlson.) Rubidium perchlorate, RbClO 4 . Sol. in 92.1 pts. H 2 O at 21.3. (Longuinine, A. 121. 123.) 1 pt. sol. in 92.1 pts. H 2 O at 21 as com- pared with 1 pt. KC1O 4 sol. in 57.9 pts. H 2 O at 21. (Erdmahn, Arch. Pharm. 1894, 232. Terbium perchlorate. Very sol. in H 2 O and in alcohol. (Potratz, C. N. 1905,92.3.) Thallous perchlorate, T1C1O 4 . 1 pt. salt dissolves in 10 pts. H 2 O at 15, and 0.6 pt. at 100. (Roscoe, Chem. Soc. (2) 4. 504.) Solubility in H 2 O at t. .6/0.; Solubility in H 2 O at t. t G. per 100 g. H 3 Sp. gr. t G. RbC10 4 in 100 g. H 2 t G. RbClO 4 in 100 g. H 2 10 30 50 70 80 6.00 8.04 19.72 39.62 65.32 81.49 1.060 1.075 1.146 1.251 1.430 1.520 8 19.8 30 2.46 3.50 6.28 9.53 42.2 50 77 99 14.94 19.40 41.65 76.5 (Carlson, Festsk. Stockholm, 1911. 262.) SI. sol. in alcohol. (Roscoe.) (Calzolari, Ace. Sci. Med. Ferrara, 1911, 85. 150.) PERCOLUMBATE, OESIUM 653 Thallic perchlorate, T1(C1O 4 ) 3 +6H 2 O. Very hydroscopic, sol. in H 2 O. Decomp. in moist air. (Gewecke, Z. anorg. 1912, 76. 274.) Uranyl perchlorate, (UO 2 )(C1O 4 )2+4H 2 O. (Salvadori, Ch. Z. 1912, 36. 513.) +6H 2 O. (Salvadori.) Yttrium perchlorate, Y(C1O 4 ) 3 +8H 2 O. Very deliquescent. Sol. in H 2 O and alcohol. (Cleve.) Zinc perchlorate, Zn(ClO 4 ) 2 . Deliquescent. Sol. in H 2 O and alcohol. (Serullas, A. ch. 46. 302.) +4H 2 O, and 6H 2 O. (Salvadori, C. C. 1912, II. 414.) Zinc perchlorate, ammonia, Zn(ClO 4 ) 2 , 4NH 3 . Ppt. (Salvadori, C. C. 1912, II. 414.) Zn(ClO 4 ) 2 , 6NH 3 . (Ephraim, B. 1915, 48. 643.) Perchromic acid. Sol. in ethyl acetate and valerate; in amyl chloride, formate, acetate, butyrate, and valerate. (All give blue solutions.) Insol. in CS 2 , C 6 H 6 , CHC1 3 , CC1 4 , C 6 H 5 NH 2 , C 6 H 5 NO 2 and toluene. (Grosvenor, J. Am. Chem. Soc. 1895, 17. 41-43.) H 3 CrO 8 +2H 2 O. Decomp. above 30. (Riesenfeld, B. 1914, 47. 552.) Ammonium perchromate, (NH 4 ) 3 CrO 8 . Very unstable. SI. sol. in cold H 2 O. De- comp. by cone. H 2 SO 4 . Insol. in pure al- cohol and pure ether. Decomp. by boiling alcohol containing more than 50% H 2 O. (Wohlers, B. 1905, 38. 1888.) CrO 4 , 3NH 3 . Sol. in 10% NH 4 OH+Aq; sol. in H 2 O with decomp., insol. in other solvents. (Wiede, B. 1897, 30. 2181.) NH 4 CrO 6 , H 2 O 2 . Decomp. in the air. Sol. in ice cold H 2 O, decomp. when warmed. Insol. in alcohol, ether, ligroin and CHC1 3 . (Wiede, B. 1898, 31. 518.) Ammonium hydrogen perchromate, Cr0 2 (O.O.NH 4 )(O.OH). Sol. in H 2 O with decomp. Difficultly sol. in cold abs. alcohol. (Hofmann, B. 1904, 37. 3406.) Barium perchromate, BaCr 2 O 8 . (Byers and Reid, Am. Ch. J. 1904, 32. 513.) Calcium perchromate, CaCr 2 O 8 . Very sol. in H 2 O. (Mylius, B. 1900, 33. 3689; Byers and Reid, Am. Ch. J. 1904, 32. 513.) Lithium perchromate, Li 2 Cr 2 O 8 . (Byers and Reid, Am. Ch. J. 1904, 32. 511.) Magnesium perchromate, MgCr 2 O 8 . (Byers and Reid.) Potassium perchromate, K 3 CrO 8 . SI. sol. in cold H 2 O. Decomp. by cone. H 2 SO 4 . Insol. in pure alcohol and pure ether. Decomp. by boiling alcohol contain- ing more than 50% H 2 O. ( Wohlers, B. 1905, 38. 1888.) +xH 2 O. Sol. in H 2 O at without de- comp. (Riesenfeld and Kutsch, B. 1908, 41. 3948.) K 2 Cr 2 O 8 . Sol. in H 2 O. Decomp. in the air. (Byers and Reid, Am. Ch. J. 1904, 32. 505.) KCrO 6 , H 2 O 2 or KH 2 CrO 7 . Sol. in ice cold H 2 O, decomp. when warmed; explosive. (Wiede, B. 1898, 31. 520.) Sodium perchromate, Na 3 CrO s . SI. sol. in cold H 2 O. Decomp. by cone. H 2 SO 4 . Insol. in pure alcohol and pure ether. Decomp. by boiling with ale. containing more than 50% H 2 O. (Wohlers, B. 1905, 38. 1888.) Na fi Cf 2 O 16 +28H 2 O. Efflorescent. SI. sol. in cold, easily in hot H 2 O, with decomp. Not decomp. by NaOH +Aq. (Haussermann, J. pr. (2) 48. 70.) Na 2 Cr 2 O 8 . (Byers and Reid, Am. Ch. J. 1904, 32. 511.) Perchloroplatinocyanhydric acid, H 2 Pt(CN) 4 Cl 2 +4H 2 O. Very sol. in H 2 O and alcohol. Ammonium perchloroplatinocyanide, (NH 4 ) 2 Pt(CN) 4 Cl 2 +2H 2 O. Sol. in H 2 O. Barium , BaPt(CN) 4 Cl 2 +5H 2 O. Very sol. in H 2 O. Calcium , CaPt(CN) 4 Cl 2 . Sol. in H 2 0. Magnesium Sol. in H 2 O. -, MgPt(CN) 4 Cl 2 +zH 2 0. Manganous , MnPt(CN) 4 Cl 2 +5H 2 O. Sol. in H 2 O and alcohol. Potassium , K 2 Pt(CN) 4 Cl 2 +2H 2 O. Very efflorescent, and sol. in H 2 and alcohol. Percolumbic acid, HCbO 4 +nH 2 O. Insol. in H 2 O. Sol. with decomp. in warm H 2 SO 4 . (Melikoff, Z. anorg. 1899, 20. 341.) Caesium percolumbate, Cs 3 CbO 8 . Ppt. (E. F. Smith, J. Am. Chem. Soc. 1908, 30. 1658.) 654 PERCOLUMBATE, CAESIUM MAGNESIUM Caesium magnesium percolumbate, MgCsCbO 8 +8H 2 O. Sol. in H 2 O without decomp. (E. F. Smith.) Calcium potassium percolumbate, CaKCbO 8 +4H 2 O. Difficultly sol. in H 2 O. (E. F. Smith.) Calcium sodium percolumbate,CaNaCbO 8 + 4H 2 0. Difficultly sol. in H 2 O. (E. F. Smith.) Magnesium potassium percolumbate, MgKCbO 8 +7H 2 O. Sol. in H 2 O without decomp. (E. F. Smith.) Magnesium rubidium percolumbate, MgRbCbO 8 +7^H 2 O. Sol. in H 2 O without decomp. (E. F. Smith.) Magnesium sodium percolumbate, MgNaCbO 8 +8H 2 O. Sol. in H 2 O without decomp. (E. F. Smith.) Potassium percolumbate, K 3 CbO 8 . Sol. in H 2 O. Ppt. from aq. solution by alcohol. (E. F. Smith.) K 4 Cb 2 On+3H 2 O. Sol. with decomp. in H 2 O. Ppt. by alcohol. Sol. in KOH+H 2 O 2 +Aq. (Melikoff, Z. anorg. 1899, 20. 342.) Rubidium percolumbate, Rb 3 Cb0 8 . Sol. in H 2 O. ' Insol. in alcohol. (E. F. Smith.) Sodium percolumbate, Na 3 CbO 8 . Sol. "in H 2 O. Insol. in alcohol. (E. F. Smith.) Perf erricyanhydric acid. Potassium perferricyanide, K 2 Fe(CN) 6 + H 2 (?). Very hygroscopic, and sol. in H 2 0. Nearly insol. in absolute alcohol. Decomp. by hot H 2 O. (Skraup, A. 189. 368.) Periodic acid, H B IO 6 . Deliquescent in moist air; very sol. in H 2 O. (Bengieser, A. 17. 254.) Rather easily sol. in alcohol and Aether. (Bengieser.) Rather easily sol. in alcohol, less in ether. (Langtoch.) SI. sol. in alcohol, still less in ether. (Lang- lois, J. pr. 66. 36.) Sp. gr. of H 5 IO 6 +Aq. H 5 IO 6 + 20H 2 O = 1.4008. H 5 IO 6 + 40H 2 = 1.2165. H 5 IO 6 + 80H 2 O = 1.1121. H 5 IO 6 + 160H 2 O = 1.0570. H 6 IO 6 +320H 2 O = 1.0288. (Thomsen, B. 7. 71.) Periodates. Most periodates are insol. or si. sol. in H 2 O; all are insol. or very si. sol. in alcohol, but they all dissolve in dil. HNO 3 +Aq. (Ben- gieser.) Aluminum wetoperiodate, A1(IO 4 ) 3 +3H 2 O. Stable in solution containing HNO 3 . (Eakle, C. C. 1896. II, 649.) Ammonium metoperiodate, NH 4 IO 4 . SI. sol. in HoO. Cryst. with 3H 2 O (Ihre, B. 3. 316), 2H 2 O (Langlois, A. ch. (3) 34. 257). Stable in solution containing free ammonia. (Eakle, Zeit. Kryst. 1896, 26. 258-88.) 100 pts. H 2 O dissolve 2.7 pts. NHJO 4 at 16; sp. gr. of sat. solution at 16/4 = 1.0178. (Barker, Chem. Soc. 1908, 93. 17.) Ammonium dzmesoperiodate, (NH 4 ) 4 I 2 Og + 3H 2 O. Sol. in H 2 O. (Rammelsberg, Pogg. 134. 379.) Stable in solution containing free ammonia. Two modifications. (Eakle, Zeit. Kryst. 1896, 26. 558-88; C. C. 1896. II, 649.) Ammonium lithium dimesoperiodate, (NH 4 ) 2 Li 2 I 2 9 +7H 2 0. Sol. in H 2 O. (Ihre.) Ammonium magnesium mesoperiodate, NH 4 MgIO 5 +3H 2 O. Precipitate. (Rammelsberg, Pogg. 134. 510.) Barium metoperiodate, Ba(IO 4 ) 2 . Known only in solution. Barium dmesoperiodate, Ba 2 I 2 O 9 . SI. sol. in H 2 O; easily sol. in dil. HNO 3 + Aq. (Rammelsberg, Pogg. 134. 391.) Cryst. also with 3H 2 O, 5H 2 O, and 7H 2 O. Barium mesoperiodate, Bas(IO 5 ) 2 +6H 2 O. (Ihre.) Barium or^operiodate, Ba 5 (IO 6 ) 2 . Insol. in H 2 O. Sol. in HNO 3 +Aq. (Ram- melsberg.) Barium dimesodiperiodate, Ba 5 I 4 Oi 9 +5H 2 O. Precipitate. Sol. in dil. HNO 3 +Aq. (Rammelsberg, Pogg. 134. 395.) Barium periodate tungstate. See Tungstoperiodate, barium. Caesium metoperiodate, CsIO 4 . SI, sol. in cold H 2 O; readily sol. in hot H 2 O. (Wells, Am. Ch. J. 1901, 26. 279.) 2.15 pts. are sol. in 100 pts. H 2 O at 15. Sp. gr. of the sat. aq. solution at 15/4 = 1.0166. (Barker, Chem. Soc. 1908, 93. 17.) PERIODATE, MAGNESIUM 655 Caesium periodate hydrogen fluoride, 2CsIO 4 , 3HF+H 2 O. Sol. in 40-60% HF+Aq. Decomp. by H 2 O. Efflorescent. (Wemland, Z. anorg. 1899, 22. 263.) Cadmium raetaperiodate, Cd(IO 4 )2. Ppt. (Rammelsberg, Pogg. 134. 516.) Cadmium cforaesoperiodate, Cd 2 I 2 O9+9H 2 O. Insol. in H 2 O. (Rammelsberg.) Cadmium raesoperiodate, Cd 3 (IO 5 ) 2 +5H 2 O. Ppt. CdHIO 5 . (Kimmins, Chem. Soc. 66. 151.) Cadmium t&periodate, Cd 4 l 2 On+3H 2 O. Insol. in H 2 O. (Rammelsberg.) Cadmium periodate, Insol. in H 2 O. (Rammelsberg.) Calcium wetaperiodate, Ca(IO 4 ) 2 . Sol. in H 5 IO 6 +Aq and acids. (Rammels- berg, Pogg. 134. 405.) Calcium dmesoperiodate, Ca 2 I 2 O 9 +7H 2 O, and 9H 2 O. SI. sol. in H 2 O. (Rammelsberg.) +3H 2 O. (Langlois.) Calcium orthoperiodsite, Ca 5 (IO 6 )2. Insol. in H 2 O. Sol. in HNO 3 +Aq. (Ram- melsberg, Pogg. 44. 577.) Cobaltous periodate, 7CoO, 2I 2 O 7 -|-18H 2 O. Attacked by HC1, and sol. on warming. Slowly but completely sol. in NHO 3 . (Lautsch, J. pr. 100. 89.) Could not be obtained by Rammelsberg. Cupric cforaesoperiodate, Cu 2 I 2 O 9 +6H 2 O. Decomp. by H 2 O without dissolving. (Rammelsberg.) Cupric ort/ioperiodate, Cu 2 HIO 6 . Very sol. in HNO 3 +Aq. (Kimmins, Chem. Soc. 55. 150.) Cupric cfo'periodate, Cu 4 I 2 On+H 2 O. Insol. in H 2 O; sol. in dil. HNO 3 +Aq. (Rammelsberg.) +7H 2 O. (R.) Cupric periodate, 5CuO, I 2 O 6 +5H 2 O. Wholly insol. in H 2 O. (Rammelsberg, B. 1.73.) Didymium peroidate, Di 2 O 2 (IO 4 )2. Precipitate. DiIO 5 +4H 2 O. Ppt. (Cleve, Bull. Soc. (2) 43. 362.) Erbium periodate. Sol. inH 2 O. (Hoglund.) Glucinum periodate, G1 3 (IO5)2+11H 2 O. Decomp. by H 2 O without dissolving. Eas- ily sol. in HNO 3 +Aq. +13H 2 O. Nearly insol. in H 2 O. (Atter- berg, B. 7. 474.) Iron (ferrous) orZ/ioperiodate, Fe 6 (IO 6 ) 2 . (Kimmins, Chem. Soc. 55. 150.) FeH 3 IO 6 . (Kimmins.) Iron (ferric) periodate, 2Fe 2 O 3 , I 2 O 7 +21H 2 O. Ppt. (Rammelsberg.) Iron (ferric) dmesoperiodate, FeHI 2 O 9 . Insol. in dil. HNO 3 +Aq. (Kimmins, Chem. Soc. 55. 149.) Iron (ferric) wetaperiodate, Fe(IO 4 ) 3 . (Kimmins.) Lanthanum periodate, La(IO 4 ) 3 +2H 2 O. Precipitate. (Cleve.) Lead wetaperiodate, Pb(IO 4 ) 2 . Sol. in HNO 3 +Aq. (Kimmins.) Lead or^operiodate, Pb 3 H 4 (IO 6 ) 2 . Sol. in HN0 3 +Aq. (Kimmins, Chem. Soc. 55. 149.) Lead mesoperiodate, Pb 3 (IO 6 ) 2 +2H 2 O. Insol. in H 2 O or excess of periodic acid+ Aq. Decomp. by dil. H 2 SO 4 +Aq. (Ben- gieser, A. 17. 254.) Lithium wetoperiodate, LiIO 4 . Difficultly sol. in H 2 O. (Rammelsberg, B. 1. 132.) Somewhat deliquescent. +H 2 O; sol. in H 2 O. (Barker, Chem. Soc. 1911, 99. 1326.) Lithium dmesoperiodate, Li 4 I 2 O 9 +3H 2 O. Very si. sol. in H 2 O. (Rammelsberg, Pogg. 134. 387.) Lithium ortftoperiodate, Li 5 IO 6 . H 2 O dissolves out a slight amount of Lil. Easily sol. in HNO 3 +Aq. (Rammelsberg, Pogg. 137. 313.) Magnesium wetoperiodate, Mg(IO 4 ) 2 -f 10H 2 O. Easily sol. in H 2 O. (Rammelsberg.) Magnesium diperiodate, Mg 4 I 2 Ou+6H 2 O, or 9H 2 O. SI. efflorescent. Insol. in H 2 O. (Rammels- berg.) 656 PERIODATE, MAGNESIUM Magnesium cftmesoperiodate, Mg 2 I 2 O 9 + 3H 2 O. (Rammelsberg, Pogg. 134. 499.) + 15H 2 O. Insol. in H 2 O. Sol. in periodic acid-f-Aq. (Langlois.) Manganic periodate. See Manganiperiodic acid. Mercurous cfoperiodate, 5Hg 2 O, I 2 O 7 , or 4Hg 2 O, I 2 O 7 = Hg 8 I 2 O n . Insol. in H 2 O. Easily sol. in HNO 3 +Aq and in HCl+Aq. (Lautsch, J. pr. 100. 86.) Mercuric or^operiodate, Hg 6 (IO 6 )2. Insol. in H 2 O. Easily sol. in HC1. SI. sol. in HNO 3 . (Lautsch.) Mercuric potassium periodate, lOHgO, 5K 2 O, 6I 2 7 . Insol. in H 2 O. Difficultly sol. in warm HNOs without decomp. (Rammelsberg, Pogg. 134. 526.) Nickel c&mesoperiodate, Ni 2 I 2 O 9 . (Kimmins, Chem. Soc. 56. 151.) Nickel mesoperiodate, Ni 3 (IO 5 ) 2 . (Kimmins.) Nickel periodate, 7NiO, 4I 2 O 7 +63H 2 O. Insol. in H 2 O. Easily sol. in H 5 IO e +Aq. (Rammelsberg, Pogg. 134. 514.) Potassium metaperiodate, KIO 4 . SI. sol. in H 2 O. Sol. in 290 pts. cold H 2 O. (Rammelsberg, Pogg. 134. 320.) Almost insol. in KOH+Aq. 0.66 pt. is sol. in 100 pts. H 2 O at 13. Sp. gr. of the sat. sol. at 13/4 = 1.0051. (Barker, Chem. Soc. 1908, 93. 16.) Insol. in methyl acetate. (Naumann, B. 1909,42.3790.) Potassium mesoperiodate, K 3 IO 6 +4H 2 O. Deliquescent. Easily sol. in H 2 0. (Ihre.) Potassium c&mesoperiodate, K 4 I 2 O 9 +9H 2 O. Sol. in 9.7 pts. cold H 2 O. (Rammelsberg, Pogg. 134. 320.) Sol. in KOH+Aq. +3H 2 O. Potassium hydrogen dimesoperiodate, K 3 HI 2 O 9 . Less sol. in H 2 O than KIO 4 . (Kimmins, Chem. Soc. 51. 356.) Potassium manganic periodate. See Manganiperiodate, potassium. Potassium zinc periodate, K 2 O, 4ZnO, 2I 2 O 7 +4H 2 0. Ppt. (Rammelsberg, Pogg. 134. 368.) Potassium periodate tungstate. See Tungstoperiodate, potassium. Rubidium periodate, RbIO 4 . 0.65 pt. is sol. in 100 pts. H 2 O at 13. Sp. gr. of the sat. aq. solution- at 13/4 = 1.0052. (Barker, Chem. Soc. 1908, 93. 16.) Samarium periodate, Sm(IOj+4H 2 O. Precipitate. (Cleve.) Silver metaperiodate, AgIO 4 . Decomp. by cold H 2 O into Ag 4 I 2 O 9 +3H 2 O, and by warm H 2 O into Ag 4 I 2 O 9 -}-H 2 O. (Am- mermiiller and Magnus, Pogg. 28. 516.) +H 2 O. Insol. ppt. (Kimmins.) Silver mesoperiodate, Ag 3 IO 5 . (Fernlunds, J. pr. 100. 99.) Ag 2 HIO 5 . Insol. ppt. (Kimmins, Chem. Soc. 51. 358.) Ppt. by dil. HNO 3 ; sol. in HNO 3 . (Rosen- heim, A. 1899, 308. 57.) Silver cfomesoperiodate, Ag 4 I 2 O 9 +H 2 O, or 3H 2 O. Insol. ppt. (Kimmins.) Decomp. by boiling H 2 O into Ag 6 IO 6 . (Rammelsberg.) Silver ori/ioperiodate, Ag 5 IO 6 . Sol. inHNO 3 orNH 4 OH-fAq. (Rammels- berg, Pogg. 134. 386.) Sol. in excess NH 4 OH+Aq; pptd. by HNO 3 . (Rosenheim, A. 1899, 308. 56.) Ag 3 H 2 IOe. Insol. ppt. (Kimmins, Chem. Soc. 51. 358.) Ag 2 H 3 IO 6 . As above. (Kimmins.) Sol. in dil. HNO 3 . (Rosenheim, A. 1899, 308. 53.) Silver eftperiodate, Ag 8 I 2 On. SI. sol. in HNO 3 +Aq; insol. in NH 4 OH+ Aq. (Lautsch, J. pr. 100. 75.) Silver cfo'wesocfo'periodate, Agi I 4 Oi 9 . HNO 3 +Aq dissolves out Ag 2 O. Insol. in NH 4 OH+Aq. (Lautsch.) Sodium metoperiodate, NaIO 4 . Easily sol. in H 2 O. +2H 2 O. (Langlois.) +3H 2 O. Efflorescent; sol. in 12 pts. H 2 O at ord. temp. (Rammelsberg, J. pr. 103. 278.) Sodium ^mesoperiodate, Na 4 I 2 O 9 +3H 2 O. Scarcely sol. in cold, si. sol. in hot H 2 O. (Magnus and Ammermiiller, Pogg. 28. 514.) Very sol. in dil. HNOs+Aq. (Langlois.) Sol. in HC 2 H 3 O 2 +Aq with decomp. (Bengieser, A. 17. 254.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790,) +4H 2 0. PERMANGANATE, CUPRIC 657 Sodium raesoperiodate, Na 3 IO 6 + 5 /4H 2 O. Sol. in H 2 O. (Ihre.) -f H 2 O = Na 3 H 3 IO 6 . Less sol. in H 2 O than Na 4 I 2 O 9 + 3H 2 O( = Na 2 H 3 IO 6 ). (Kimmins, Chem. Soc. 61. 357.) Sodium orf/ioperiodate, Na 5 IO 6 . Na 2 H 3 IO c . Correct composition for Na 4 I 2 O 9 +3H 2 O. (Kimmins.) Na 3 H 2 IOe. Correct composition for Na 3 IOs +H 2 O. (Kimmins.) Strontium metaperiodate, Sr(IO 4 ) 2 +6H 2 O. Sol. in H 2 O. Strontium cfowesoperiodate, Sr 2 I 2 Og. Decomp. by H 2 O. +3H 2 O. Strontium raesoperiodate, Sr 3 (IO 5 ) 2 . Precipitate. Strontium or^/ioperiodate, (Rammelsberg, Pogg. 44. 577.) Thallic periodate, 3T1 2 O 3 , I 2 O 7 +30H 2 O. Insol. in H 2 O. Decomp. by alkalies. (Rammelsberg, B. 3. 361.) Thorium periodate. Precipitate. Sol. in HNO 3 +Aq. Uranous periodate. Precipitate, which quickly decomposes. Ytterbium periodate, YbIO 5 +2H 2 O. Hydroscopic. (Cleve, Z. anorg. 1902, 32. 136.) Yttrium periodate, Y 2 (IO 6 )2+8H 2 O. Very slightly sol. (Cleve.) 3Y 2 O 3 , 2I 2 O 7 +6H 2 O. Precipitate. (Cleve.) Zinc dimesoperiodate, Zn 2 I 2 O 9 +6H 2 O. (Rammelsberg, Pogg. 134. 513.) Zinc periodate, 3ZnO, 2I 2 O 7 +7H 2 O. (Langlois.) Zinc ^'periodate, Zn 4 I 2 On+H 2 O. Easily sol. in H 2 O, si. acid with HNO 3 . (Langlois, A. ch. (3) 34. 257.) Zinc dimesodiperiodaie, (Rammelsberg.) (?). Zinc periodate, 9ZnO, 2I 2 O 7 + 12H 2 O. (Rammelsberg.) Periodoplatinocyanhydric acid. Barium periodoplatinocyanide, BaPt(CN)j2 +rcH 2 O. Easily sol. in H 2 O or alcohol. (Hoist, Bull. Soc. (2) 22. 347.) Potassium periodoplatinocyanide, K 2 Pt(CN)J 2 . Permanent. Easily sol. in H 2 O or alcohol. Permanganic acid, HMnC>4. Known only in solution, which decomposes by evaporation or warming. Permanganates. All permanganates are sol. in H 2 O, except- ing AgMnO 4 , which is si. sol. Ammonium permanganate, NH 4 Mn0 4 . Sol. in 12.6 pts. H 2 O at 15. (Aschoff.) Sol. in H 2 O with decomp. (Christensen, Z. anorg. 1900, 24. 206.) Barium permanganate, Ba(MnO 4 ) 2 . Sol. in H 2 O. Cadmium permanganate, Cd(MnO 4 ) 2 +8H 2 O. Stable. (Klobb, Bull. Soc. 1894, (3) 11 607.) Cadmium permanganate 'ammonia, Cd(MnO 4 ) 2 , 4NH 3 . Sol. in HoO with decomp. (Klobb, Bull. Soc. (3) 3. 510.) Caesium permanganate, CsMnO 4 . SI. sol. in cold, somewhat more easily sol. in hot H 2 O. (Muthmann, B. 1893, 26. 1018.) Solubility in H 2 O. 100 ccm. of the sat. solution contain at: 1 19 59 0.097 0.23 1.25 g. CsMnO 4 . (Patterson, J. Am. Chem. Soc. 1906, 28. 1735.) Calcium permanganate, Ca(MnO 4 ) 2 +5H 2 O. Deliquescent. Cupric permanganate. Deliquescent. 658 PERMANGANATE AMMONIA, CUPRIC Cupric permanganate ammonia, Cu(MnO 4 ) 2 , Sol. in H 2 O with slow decomp. (Klobb, Solubility in H 2 O at t. p = pts. KMnO 4 sol. in 100 pts. H 2 O at t. Bull. Soc. (3) 3. 509.) t P t p t p t P Didymium permanganate, Di(MnO 4 ) 3 + 1 2.76 2.90 19 20 6.26 6.48 38- 39 11.74 12.12 57 58 20.29 20.83 21H 2 O. 2 3.06 21 6.70 40 12.51 59 21.39 SI. sol. in H 2 O. (Frerichs and Smith, A. 3 3.22 22 6.94 41 12.91 60 21.96 191. 331.) 4 3.38 23 7.18 42 13.31 61 22.55 Has not been prepared. (Cleve, B. 11. 912.) 5 3.54 24 7.42 43 13.72 62 23.15 6 3.70 25 7.68 44 14.14 63 23.76 Lanthanum permanganate, La(MnO 4 ) 3 + 7 8 3.86 4.04 26 27 7.94 8.20 45 46 14.56 15.00 64 65 24.38 25.01 Ppt. (Frerichs and Smith, A. 191. 331.) Has not been prepared. (Cleve, B. 11. 910.) 9 10 11 4.22 4.40 4.58 28 29 30 8.48 8.77 9.07 47 48 49 15.44 15.88 16.32 66 67 68 25.67 26.34 27.03 12 4.78 31 9.37 50 16.77 69 27.84 Lead permanganate. Sol. in HNO 3 +Aq. (Forchhammer.) 13 14 15 4.98 5.18 5.38 32 33 34 9.69 10.01 10.34 51 52 53 17.23 17.71 18.21 70 71 72 28.56 29.30 30.05 16 5.60 35 10.68 54 18.71 73 30.81 Lithium permanganate, LiMnO 4 +3H 2 O. Sol. in 1.4 pts. H 2 O at 16. (Aschoff.) 17 18 5.82 6.04 36 37 11.02 11.38 55 56 19.23 19.75 74 74.5 31.57 31.95 Magnesium permanganate, Mg(MnO 4 ) 2 . Insol. in CHC1 3 , CC1 4 , C 6 H 6 , toluene, nitro- benzene, ligroin, ether and CS 2 . Sol. in methyl alcohol, acetone, pyridine, and readily sol. in glacial acetic acid. Only pyridine and glacial acetic acid are sufficiently stable to- ward the salt to be of any practical use for oxidation purposes. (Michael and Garner, Am. Ch. J. 1906, 35. 268.) +6H 2 O. Easily deliquescent. Nickel permanganate ammonia. Ni(MnO 4 ) 2 , 4NH 3 . Sol. in H 2 O with decomp. (Klobb, Bull. Soc. (3) 3. 509.) Potassium permanganate, KMnO 4 . (Worden, J. Soc. Chem. Ind. 1907, 26. 453.) Solubility in H 2 O. 100 com. of the sat. solution contain at: 15 15.3 30 2.84 5.22 5.30 8.69 g. KMnO 4 . Sp. gr. of sat. solution at 15 = 1.035. (Patterson, J. Am. Chem. Soc. 1906, 28. 1735.) 1 1. sat. KMnO 4 +Aq contains at: 10 20 30 40 0.176 0.278 0.411 0.573 0.792 mol. KMnO 4 , 53 63 70 75 1.154 1.429 1.812 2.047 mol. KMnO 4 . (Sackur, Z. Elektrochem. 1912, 18. 723.) Solubility of KMnO 4 in H 2 O at t. DQI. in ID pts. 1 2 U at 15 . (Mitscnerlicn.j Solubility in 100 pts. H 2 O at t. Grams KMnCU sol. in 100 grams H2O t 0.58 1.01 2.02 2.91 4.22 5.20 7.53 11.61 16.75 -0.18 t Pts. KMnO 4 0.27 0.48 0.58 +10 + 15 +25 +40 +50 9.8 19.8 24.8 29.8 34.8 40.0 45.0 50.0 55.0 65.0 2.83 4.31 . 6.34 7.59 9.03 10.67 12.56 14.58 16.89 19.33 25.03 (Voerman, C. C, 1906, I. 125.) Sol. in cone. H 2 SO 4 . Deliquesces in liquid HC1, but does not dissolve. (Gore.) Slowly sol. in H 3 PO 4 +Aq. (Chevillot and Edwards.) (Baxter, J. Am. Chem. Soc. 1906, 28. 1343.) PERMANGANATE AMMONIA, SILVER 659 Solubility in KOH+Aq at t expressed in mol. per 1. of the sat. solution. t H 2 l-n KOH 2-n KOH 4-n KOH 6-n KOH 8-n KOH 10-n KOH 0.176 0.050 0.031 0.027 0.023 0.017 0.012 10 0.278 0.112 0.068 0.048 0.042 0.028 0.016 20 0.411 0.179 0.119 0.079 19 0.074 0.032 0.029 30 0.573 32 0.316 32 0.213 32 0.149 0.114 32 0.062 0.040 40 0.792 0.439 0.306 0.211 0.161 0.084 0.052 50 53 1.154 50 0.638 0.462 0.304 0.219 0.111 63 1.429 61 0.904 60 0.639 0.427 0.291 61 G.143 0'071 70 1.812 1.172 0.869 0.572 0.390 0.188 0.082 75 2.047 0.651 0.089 80 1.513 ivioo 0^500 0*231 84 1.655 1.352 83 0^803 85 0.572 90 0.649 0^297 (Sackur, Z. Elektrochem. 1912, 18. 723.) Solubility in salts +Aq. at t. Solubility in ace bone+Aq. at 13. 100 ccm. acetone +Aq. s KMnO 4 in 100 ccm. Solvent t Mol. KMnO 4 in 1 1. of sat. solution A ccm. acetone in 1 /6KMnO 4 =millimol of the solution. ^K.CO, 25 40 0.1462 0.4375 0.7380 A 1/5 KMnO 4 2 10 20 30 40 50 60 70 80 90 100 148.5 162.2 177.3 208.2 257.4 289.7 316.8 328.0 312.5 227.0 67.6 l-n 5-92.' 25 40 0.0629 0.2589 0.5007 2-n 5*22.' 2 40 0.0446 0.3519 ^K.00. ' 25 0.0270 0.0930 (Herz and Knoch, Z. anorg. 1904, 41. 317.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Difficultly sol. in methyl acetate, (Nau- mann, B. 1909, 42. 3795.) Sol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Rubidium permanganate, RbMnO 4 . Solubility in H 2 O lies between K and Cs salts. (Muthmann, B. 1893, 26. 1018.) Solubility in H 2 O. 100 ccm. of the sat. solution contain at: 2 19 60 0.46 1.06 4.68 g. RbMnO 4 . (Patterson, J. Am. Chem. Soc. 1906, 28. 1735.) fl^K.CO. 2 0.0156 0.1-nKCl 25 40 0.1395 0.4315 0.7380 0.5-nKCl 25 40 0.0760 0.3060 0.5840 1-nKCl 25 40 0.0532 0.220 0.444 2-nKCl 25 40 0.0379 0.1432 0.288 (Sackur, Z. Elektrochem. 1912, 18. 723.) Very sol. in liquid NH 3 . (Moissan, A. ch. 1895 (7) 6. 428; Franklin, Am. Ch. J. 1898, 20. 829.) Decomp. immediately by alcohol. Sol. in acetone. (Eidmann, C-. C. 1899. II, 1014; Naumann, B. 1904, 37. 4328.) Sol. in 109 pts. cold H 2 O and much less hot H->O. Decomp. by boiling. (Mitscherlich, >ogg. 25. 301.) Silver permanganate ammonia. SI. sol. in cold, more easily in hot H 2 O. Klobb, C. R. 103. 384.) 660 PERMANGANATE, SODIUM Sodium permanganate, NaMnO 4 +3H 2 O. Deliquescent. Extremely sol. in H 2 O. Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Strontium permanganate, Sr(MnO 4 ) 2 +4H 2 O. Deliquescent. Sol. in H 2 O. (Fromherz.) Thallous permanganate, TlMnO 4 . Sol. in H 2 O with decomp. (R. Meyer, Z. anorg. 1899, 22. 188.) Zinc permanganate, Zn(MnO 4 ) 2 +6H 2 O. Deliquescent. Very sol. in H 2 O. (Marten- son, J. B. 1873. 274.)^ Zinz permanganate ammonia, Zn(MnO 4 ) 2 , 4NH 3 . Sol. in H 2 O with decomp. (Klobb, Bull. Soc. (3) 3. 509.)' Permanganomolybdic acid, MnO 2 , 12MoO 3 +10H 2 O. Sol. in H 2 O. Decomp. by alkalis. Sol. in alcohol. (Pochard, C. R. 1897, 125. 31.) Ammonium permanganomolybdate, 2(NH 4 ) 2 O, MnO 2 , 7MoO 3 +5H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 73.) 3(NH 4 ) 2 O, MnO 2 , 9MoO 3 +6H 2 O. (Fried- heim and Allemann, Mit. d. Nat. Ges. Bern. 1904. 23.) +7H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 70.) 4(NH 4 ) 2 O, MnO 2 , HMoO 3 +7H 2 O. (Fried- heim and Samelson.) 3(NH 4 ) 2 O, MnO 2 , 12Mo0 3 +5H 2 O. SI. sol. in cold H 2 O. Decomp. by alkalis. Insol. in alcohol. (Pochard, C. R. 1897, 125. 30.) Ammonium manganous permanganomolyb- date, 3[(NH 4 ) 2 , Mn]O, MnO 2 , 9MoO 3 + 6H 2 O and +7H 2 O. (Friedheim and Allemann, Mitt. d. Nat. Ges. Bern. 1904. 23.) 3](NH 4 ) 2 , Mn]O, MnO 2 , 10MoO 3 +10H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 94.) 4[(NH 4 ) 2 , Mn]O, MnO 2 , 10MoO 3 +6H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 75.) 4[(NH 4 ) 2 , Mn]O, MnO 2 , HMoO 3 +8H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 72.) Ammonium manganous potassium perman- ganomolybdate, 2(NH 4 ) 2 O, MnO, K 2 0, MnO 2 , 10MoO 3 +5H 2 O. Very si. sol. in cold, easily sol. in H 2 O at 70-80. (Rosenheim, Z. anorg. 1898, 16. 79.) 3[(NH 4 ) 2 , K 2 , Mn]O, MnO 2 , 9MpO 3 -f 7H 2 O. (Friedheim and Allemann, Mitt. d. Nat. Ges. Bern. 1904. 23.) 4[(NH 4 ) 2 , K 2 , Mn]O, MnO 2 , 10MoO 3 -f 5H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 97.) 3[(NH 4 ) 2 , K 2 , Mn]O, MnO 2 , 10MoO 3 -f 6H 2 O, and + 10H 2 O. (Friedheim and Samel- son, Z. anorg. 1900, 24. 92.) Ammonium potassium permanganomolyb- date, 3[(NH 4 ) 2 , K 2 ]O, MnO 2 , 8MoO 3 + 4H 2 O. (Friedheim and Samelson.) Barium permanganomolybdate, 3BaO, MnO 2 , 9MoO 3 + 12H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 700.) Manganous potassium permanganomolyb- date, 2K 2 O, MnO, MnO 2 , 9MoO 3 + 8H 2 0. True formula for 5K 2 O, Mn 2 O 3 , 16MoO 3 + 12H 2 O of Struve. (Friedheim and Samelson, Z. anorg. 1900, 24. 86.) 3[K 2 ,Mn]O, MnO 2 , 9MoO 3 +6H 2 O. (Fried- heim and Allemann, Mitt. d. Nat. Ges. Bern. 1904. 23.) 2.6 K 2 O, 0.4 MnO, MnO 2 , 9MoO 3 +7H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 700.) 4[K 2 , Mn]O, MnO 2 , HMoO 3 +7H 2 0. (Friedheim and Samelson, Z. anorg. 1900, 24. 80.) Manganous potassium sodium permangano- molybdate, 3[K 2 , Na 2 , MnjO, MnO 2 , 8MnO 3 +4H 2 O. (Friedheim and Allemann, Mitt. d. Nat. Ges. Bern. 1904. 48.) Manganous sodium permanganomolybdate, 3[Na 2 , MnjO, MnO 2 , 9MoO 3 + 15H 2 O. (Friedheim and Allemann.) Potassium permanganomolybdate, 3K 2 O, MnO 2 , 8MoO 3 +3H 2 O. Much less sol. in H 2 O than NH 4 comp. (Friedheim and Samelson, Z. anorg. 1900, 24. 78.) -|-5H 2 O. Nearly insol. in cold or hot H 2 0. (Rosenheim and Itzig, Z. anorg. 1898, 16. 81.) 3K 2 O, MnO 2 , 9MoO 3 +5H 2 O. (Friedheim and Samelson, Z. anorg. 1900, 24. 81.) +6H 2 O. (Hall, J. Am. Chem. Soc. 1907, 29. 700.) 3K 2 O, MnO 2 , 12MoO 3 +4H 2 O. Nearly insol. in cold H 2 O. Decomp. by alkalis. Insol. in alcohol. (Pochard, C. R. 1897, 125. 31.) Silver permanganomolybdate, 3Ag 2 O, MnO 2 , 9MoO 3 +6H 2 O. Ppt. (Hall, J. Am. Chem. Soc. 1907, 29. 700.) PEROXYNITRATE, SILVER 661 Sodium permanganomolybdate, 3Na 2 O, MnO 2 , 12MoO 3 + 13H 2 O. Efflorescent. Very sol. in H 2 O. Decomp. hv alkalies. Insol. in alcohol. (Pechard, C. R. 125. 31.) Permanganotungstic acid. Ammonium manganous permanganotung- state, 4(NH 4 ) 2 O, MnO, MnO 2 , 12WO 3 + 23H 2 O. Readily sol. in H 2 O. Can be cryst. there- from. (Rogers and Smith, J. Am. Chem. Soc. 1904, 26. 1475.) Sodium permanganotungstate, 3Na 2 O, MnO 2 , 5WO 3 + 18H 2 O. Rather easily sol. in hot H 2 O. Solution decomp. on long boiling with separation of manganese peroxide. (Just, B. 1903, 36. 3621.) Permolybdic acid, Mo 2 O 7 , 5H 2 O = HMoO 4 +2H 2 O. Verv sol. in H 2 O, and not decomp. by boil- . ing. (Pechard, A. ch. (6) 28. 550.) H 2 MoO 5 + lKH 2 O. "Ozo-molybdic acid." Only very si. sol. in H 2 O after being dried in the air. 801. in fairly cone. H 2 SO 4 . (Muth- mann, B. 1898, 31. 1838.) H 2 Mo 2 O 7 , H 2 O 2 . SI. sol. in cold, more eas- ily sol. in hot H 2 O, but does not separate on cooling. Sol. in dil. acids, also in H 3 PO 4 . (Cammerer, Ch. Z. 1891, 15. 957.) Ammonium permolybdate, NH 4 MoO 4 + 2H 2 O. Very sol. in H 2 O; si. sol. in alcohol, but alcohol extracts it from H 2 O, forming a very cone, supersat. solution, which is pptd. by a crystal of NH 4 MoO 4 , and only a si. amount remains in solution. (Pochard.) 3(NH 4 ) 2 O, 5MoO 3 , 2MoO 4 +6H 2 O. (Muth- mann, B. 1898, 31. 1837.) 3(NH 4 ) 2 O, 7MoO 4 +12H 2 O. Ppt. (Muth- mann, Z. anorg. 1898, 17. 76.) 3(NH 4 ) 2 0, 5MoO 4 +6H 2 O. Ppt. (Muth- mann.) Ammonium nickel permolybdate ammonia (NH 4 ) 2 Ni(MoO 4 ) 2 ,2NH 3 . Decomp. by H 2 O. Sol. in dil. NH 4 OH. (Briggs, Chem. Soc. 1904, 85. 674.) Barium permolybdate, Ba(MoO 4 ) 2 +2H 2 O. (Pechard, A. ch. 1893, (6) 28. 537.) 8BaO, 19MoO 3 , 2H 2 O 2 + 13H 2 O. (Baer- wald, Dissert. 1885.) Caesium permolybdate, Cs 2 O, 4MoO 4 +6H 2 O. Sol. hot HoO. (Muthmann, B. 1898, 31. 1841.) 3Cs 2 O, 7MoO 3 , 3MoO 4 +4H 2 O. Ppt. (Muthmann.) Copper permolybdate, Cu(MoO 4 ) 2 +H 2 O. Insol. in H 2 O; easily sol. in acids. Sol. in NH 4 OH+Aq with decomp. (Pechard.) Magnesium permolybdate, Mg(MoO 4 ) 2 + 10H 2 O. Very sol. in H 2 O; si. sol. in alcohol. (Pech- ard.) Mercurous permolybdate. Insol. in H 2 O or NH 4 NO 3 + Aq. (Pechard.) Potassium permolybdate, KMoO 4 +2H 2 O. SI. sol. in cold, more in hot H 2 O. SI. sol! in alcohol. (Pechard.) K 2 O,2MoO 3 , MoO 4 +3H 2 O. Ppt, (Muth- mann, Z. anorg. 1898, 17. 77.) K 2 O 2 , MoO 4 , H 2 O 2 . Decomp. by H 2 O. (MelikofT and Pissarjewsky, B. 1898, 31. 2449.) K 2 MoO 5 +3H 2 O. Nearly insol. in cold, easily sol. in hot H 2 O. (Mazzuchelli and Zangrilli, Gazz. ch. it. 1910, 40. (2) 56.) Rubidium permolybdates. ' ' Rubid ium ozo-molybdate. ' ' 3Rb 2 O, 10MoO 4 +14H 2 O. Ppt. Rb 2 O, 2MoO 3 , MoO 4 +3H 2 O. May be re- cryst. from H 2 O 2 -f-Aq. 3Rb 2 O, 5MoO 3 , 2MoO 4 +6H 2 O. Ppt. Rb 2 O, 3MoO 3 , MoO 4 +4H 2 O. Ppt. (Muth- mann, B. 1898, 31. 1839-41.) Silver permolybdate, AgMoO 4 . . (Pechard.) Sodium permolybdate, NaMoO 4 +3H 2 O. Very sol. in H 2 O; insol. in alcohol, but behaves similarly to K salt. (Pechard.) Thallous permolybdate. Insol. in H 2 O. (Pochard, A. ch. 1893, (6) 28. 559.) Pemitric acid, NO 3 . See Nitrogen hexoxide. Silver pernitrate, basic, 3Ag 2 O 2 , AgNO 5 . Decomp. H 2 O. (Mulder, R. t. c. 1898, 17. 142.) Perosmic acid. Potassium perosmate (?). Sol. in H 2 O, but very easily decomp. Peroxynitric acid. Silver peroxynitrate. Analysis of the black compound formed, under certain circumstances, in a silver volt- ameter when an aqueous solution of AgNO 3 662 PEROXYLAMINE SULPHONIC ACID is electrolyzed, points to the composition 3Ag 2 O, 5O, AgNO 3 , perhaps 2Ag,O 4 , AgNO 8 or 3Ag 2 O 2 , AgNO 5 . (Mulder, Chem. Soc. 1896, 70. (2) 561.) Peroxylaminesulphonic acid. Potassium peroxylaminesulphonate, N 2 O 2 (SO 3 K) 4 . Very unstable in H 2 O. Very si. sol. in cold H 2 O. 'More stable in.N/10 KOH+Aq. 100 pts. N/10 KOH+Aq dissolve 0.62 pt. of the salt at 3; 6.6 pts. at 29. (Haga, Chem. Soc. 1904, 86. 86.) Perstannic acid, H 2 Sn 2 O 7 . Known in colloidal state, sol. in H 2 O. (Spring, Bull. Soc. (2) 51. 180.) Potassium perstannate, KSnO 4 +2H 2 O. Sol. in H 2 O. Insol. in alcohol. (Tanatar, B. 1905, 38. 1185.) Sodium perstannate, NaSnO 4 +2H 2 0. Difficultly sol. in H 2 O with decomp. (Tanatar.) Persulphuric See Sulphur heptoxide. H 2 S 2 8 . Sp. gr. of H 2 S 2 8 +Aq. Ammonium lead persulphate, (NH 4 ) 2 Pb(S0 4 ) 3 . Decomp. by H 2 O. Almost insol. in cold H 2 S0 4 of sp. gr. = 1.7. SI. sol. in H 2 SO 4 (sp. gr. = 1.7) at 50. Sol. in fuming H ? SO 4 and in cold cone. HC1. Sol. in acetic acid, in Na acetate +Aq acidified with acetic acid and in excess of cold 20%NaOH+Aq. (Elbs, Z. Elektrochem. 1900, 7. 346.) Ammonium mercurous persulphate am- monia, (NH 4 )HgS 2 O 8 , 2NH 3 . Decomp. by H 2 O. Insol. in dil. or cone., hot or cold H 2 SO 4 or HNO 3 . Sol. in HC1. (Tarugi, Gazz. ch. it. 1903, 33. (1) 131.) Barium persulphate, BaS 2 O 8 +4H 2 O. Very sol. in H 2 O. 100 pts. H 2 O at dis- solve 39.1 pts. BaS 2 O 8 , or 52.2 pts. BaS 2 O 8 + 4H 2 O. Sol. in absolute alcohol with pptn. of BaS 2 O 8 +H 2 O. Insol. in alcohol. (Marshall.) Cadmium persulphate ammonia, CdS 2 O 8 , 6NH 3 . Sol. in H 2 O. (Barbieri, Z. anorg. 1911. 71. 350.) Caesium persulphate, Cs 2 S 2 O 8 . Sol. in H 2 O. 8.71-8.98 pts. are sol. in 100 pts. H 2 O at 23. (E. F. Smith, J. Am. Chem. Soc. 1899, 21. 935.) Calcium persulphate. Very sol. in H 2 O. (Marshall, J. Soc. Chem. Ind. 1897, 16. 396.) Copper persulphate ammonia, CuS 2 O 8 , 4NH 8 . Sol. in H 2 O. (Barbieri, Z. anorg. 1911, 71. 351.) Lead persulphate, PbS 2 O 8 . Decomp. by H 2 O. SI. sol. in H 2 SO 4 , and in pyrosulphuric acid. Sol. in cold cone. HC1. Insol. or sol. with decomp. in all ord. solvents. (Elbs, Z. Elektrochem. 1900, 7. 345.) Sp. gr. 14/14 % H 2 S 2 8 g. HzSzOs per 1. Solubility of Pb(SO 4 ) 2 in H 2 SO 4 +Aq. at 22. 1.042 7.2 75 v= moles of H 2 SO 4 per mole of H 2 O; 1.096 15.4 169 c=millimols Pb(SO 4 ) 2 in 1 1. 11 K.A OQ \ 979 . 1O' 1.246 35'2 &% & 438 V C V C (Elbs and. Schonherr, Z. Elektrochem. 1896, 0.304 0.00 0.558 37.2 2. 245.) 0.348 1.8 0.699 40.5 0.387 3.0 0.917 23.3 Ammonium persulphate, (NH 4 ) 2 S 2 O 8 . Very sol. in H 2 O. 100 pts. H 2 O at dis- solve 58.2 pts. (NH 4 ) 2 S 2 O 8 . (Marshall, Chem. Soc. 59. 771.) 0.407 0.435 0.477 0.515 3.9 5.3 14.4 23.3 1.11 1.54 2.08 2.13 23.7 49.6 83.5 88.2 Solubilitv in H 2 O equals 58% at 8. (Moreau, C. C. 1901, II. 56.) (Dolezalek and Finckli, Z. anorg. 1906, 51. 321.) 100 pts. H 2 O dissolve 65 pts. at ord. temp. (Elbs, J. pr. 1893, (2) 48. 185.) +3H 2 O. Deliquescent. Very sol. in H 2 0. (Marshall.) Lead potassium persulphate, K 2 Pb(SO 4 ) 3 . Decomp. by H 2 O. Almost insol. in cold H 2 SO 4 of sp. gr. = 1.7. SI. sol. in H 2 S0 4 (sp gr. = 1.7) at 50. Sol. in fuming H 2 SO 4 , cole cone. HC1, excess of cold 20% NaOH+Aq acetic acid, and in Na acetate +Aq acidifiec with acetic acid. (Elbs, Z. Elektrochem 1900, 7. 346.) PERTUNGSTATE, LITHIUM 663 Nickel persulphate ammonia, NiS 2 O 8 , 6NH Unstable in the air. Sol. in H 2 O with de- comp. (Barbieri, Z. anorg. 1911, 71. 351.) Potassium persulphate, 100 pts. H 2 O at dissolve 1.77 pts. K 2 S 2 O; more sol. in hot H 2 O with very si. decomp Less sol. in H 2 O than any other persulphate (Marshall.) Rubidium persulphate, Rb 2 S 2 O 8 . Sol. in H 2 O. 3.32-3.49 pts. are sol. in 10( pts. H 2 O at 22.5. (E. F. Smith, J. Am Chem. Soc. 1899, 21. 934.) Silver persulphate, basic, 5Ag 2 O 2 , 2Ag 2 SO 7 . Decomp. by H 2 O and acids. (Mulder, C. C 1899. I, 16.) Sodium persulphate, Na 2 S 2 O 8 . Very sol. in H 2 O. (Lowenherz.) Strontium persulphate. Very sol. in H 2 O. (Marshall, J. Soc. Chem Ind. 1897, 16. 396.) Thallium persulphate, T1 2 S 2 O 8 . Very sol. in H 2 O. (Smith, J. Am. Chem Soc. 1898, 21. 936.) Zinc persulphate ammonia, ZnS 2 O 8 , 4NH 3 . Sol. in H 2 O. (Barbieri, Z. anorg. 1911, 71 350.) . Persulphomolybdic acid. See Persulphomolybdic acid. Pertantalic acid, HTaO 4 -f-nH 2 O. Ppt. (Melikoff, Z. anorg. 1899, 20. 345.) Caesium pertantalate, Cs 3 TaO 8 . Ppt. (E. F. Smith, J. Am. Chem. Soc. 1908, 30. 1667.) Calcium potassium pertantalate. CaKTaO 8 + 43^H 2 0. Insol. in cold H 2 O; decomp. by hot H 2 O. (Melikoff, Z. anorg. 1899, 20. 3470 Calcium sodium pertantalate, CaNaTaO 8 + Difficultly sol. in H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1908, 30. 1668.) Magnesium potassium pertantalate, MgKTaO 8 +7H 2 O. Somewhat sol. in H 2 O. (E. F. Smith.) Magnesium rubidium pertantalate, MgRbTa0 8 +9H 2 O. Somewhat sol. in H 2 O. (E. F. Smith.) Magnesium sodium pertantalate, MgNaTaOs +8H 2 0. Somewhat sol. in H 2 O. (E. F. Smith.) Potassium pertantalate, Sol. in H 2 O with decomp.; sol. in KOH+ H 2 O 2 +Aq; pptd. by alcohol. (Melikoff, Z. anorg. 1899, 20. 346.) Rubidium pertantalate, Rb 3 TaO 8 . Somewhat sol. in H 2 O. (E. F. Smith.) Sodium pertantalate, Na 3 TaO 8 +H 2 O. Pptd. by alcohol. SI. sol. in H 2 O, decomp. on heating with H 2 O. (Melikoff, Z. anorg. 1899, 20. 348.) NaTaO 4 +NaOTaO 4 +13H 2 O. Sol. in H 2 O 2 +Aq; pptd. by alcohol. (Melikoff, Z. anorg. 1899, 20. 349.) Pertitanic acid. Ammonium pertitanate, (NH 4 ) 2 O 2 , TiO 3 -f H 2 2 . Fairly stable; decomp. rapidly in aq. solu- tion. (Melikoff, B. 1898, 31. 955.) Barium pertitanate, BaO 2 , TiO 3 +5H 2 O. SI. sol. in H 2 O. (Melikoff and Pissarjew- sky, Z. anorg. 1898, 18. 59.) Potassium pertitanate, K 2 O 2 , TiO 3 , K 2 O 4 + 10H 2 O. Stable at zero; deliquesces and decomp. at ordinary temp. (Melikoff, B. 1898, 31. 680.) Sodium pertitanate, Na 2 O 2 , TiO 3 +3H 2 O. Sol. in H 2 O. Pptd. in alcohol. (Melikoff, B. 1898, 31. 955.) 4Na 2 O 2 , Ti 2 O 7 +10H 2 O. Decomp. by H 2 0. [Melikoff.) Pertungstic acid. Barium pertungstate, BaO, 2WO 3 , O+6H 2 O. Insol. in H 2 O. Decomp. by acids. (Kell- ner, Dissert. 1909.) Caesium pertungstate, 3Cs 2 O, 12WO 3 , 2O + 12H 2 O. SI. sol. in cold, easily sol. in warm H 2 O. Kellner.) 5Cs 2 O, 12WO 3 , 24O + 11H 2 O. SI. sol. in H 2 O. (Kellner.) Calcium pertungstate, 3CaO, 6WO 3 , 8O + 8H 2 O. Sol. inH 2 O. (Kellner.) ,ithium pertungstate, Li 2 O, 2WO 3 , 2O-f- 6H 2 0. SI. sol. in H 2 O. (Kellner.) 3Li 2 O, 4WO 3 , O+9H 2 O. Sol. in H 2 0. KeUner.) 664 PERTUNGSTATE, MAGNESIUM Magnesium pertungstate, 2MgO, 4WO 3 , 6O + 9H 2 O. Easily sol. in H 2 O. (Kellner.) Potassium pertungstate, K 2 O 4 , WO 4 +H 2 O. Sol. in H 2 O with decomp.; explodes in the air at 80. (Melikoff, B. 1898, 31. 634.) K 2 O, 2WO 3 , 4O+4H 2 0. Sol. in H 2 O from which it is ppt. by alcohol and ether. (Kell- ner.) 7K 2 O, 10WO 3 , 5O+22H 2 O. Very si. sol. inH 2 0. (Kellner.) Rubidium pertungstate, 2Rb 2 O, 4WO 3 , O + 3H 2 O. Sol. in H 2 O with slow decomp. (Kellner.) 5Rb 2 O, 12W( H 2 O. (Kellner.) 5Rb 2 O, 12WO 3 , 3O + 12H 2 O. Insol. in nap. .0. Sodium pertungstate, NaWO 4 +H 2 O. Very sol. in H 2 O. (Pechard, C. R. 112. 1060.) +2H 2 O. Sol. in H 2 O but easily decomp. (Kellner.) Na 2 W 2 O 9 -f-6H 2 O. Sol. in H 2 O and can be cryst. therefrom. (Pissarjewsky, Z. anorg. 1900, 24. 113.) Na 2 2 , W0 4 +H 2 2 , (Na 2 2 )W0 4 +7H 2 0. Decomp. in the air. Sol. in H 2 O with decomp. (Melikoff, B. 1898, 31. 633.) Na 2 Q 2 , WO 4 , H 2 O 2 . Very unstable. De- comp. in the air and by H 2 O. (Melikoff.) Strontium pertungstate, SrO, 2WO 3 , O + 6H 2 0. (Kellner.) Peruranic acid, UO 6 , zH 2 O (?). Known only in its salts. Ammonium peruranate, (NH 4 ) 2 O 2 , (UO 4 ) 2 + 8H 2 O. Sol. in H 2 0; decomp. by acids and by A1(OH) 3 in aq. solution. (Melikoff, B. 1897, 30. 2904.) Ammonium uranyl peruranate, (NH 4 ) 2 (UO 2 )UO 8 +8H 2 O (?). Easily sol. in H 2 O. (Fairley, Chein. Soc. (2) 31. 134.) Barium peruranate, BaUO 5 . As K salt, (de Coninck, C. C. 1909, I. 1970.) (Ba0 2 ) 2 UO 4 +8H 2 0. Decomp. by H 2 S0 4 and H 2 C0 8 . (Melikoff, B. 1897, 30. 2905.) BaO 2 (UO 4 ) 2 +9H 2 O. Ppt. (Melikoff.) Calcium peruranate, CaUO 5 . As K salt, (de Coninck.) Calcium peruranate, (CaO 2 ) 2 UO 4 +10H 2 O. Ppt. (Melikoff, B. 1897, 30. 2906.) Copper peruranate, (CuO 2 ) 2 UO 4 . Ppt. (Melikoff.) Lead peruranate, (PbO) 2 UO 4 , PbO, UO 3 . Ppt. (Melikoff.) Lithium peruranate, (Li 2 O 2 )(UO 4 ) 2 +8H 2 O. Sol. in H 2 O; decomp. by acids and by A1(OH) 3 in aq. solution; very unstable. (Melikoff.) Nickel peruranate, (NiO) 2 UO 4 . Ppt. (Melikoff.) Potassium peruranate,. K 4 UO 8 + 10H 2 O (?). Unstable. (Fairley.) K 2 UO 6 . (de Coninck, C. R. 1909, 148. 1769.) +3H 2 O. Decomp. by H 2 O, HC1 and dil. HNO 3 . (Aloy, Bull. Soc. 1903, (3) 29. 293.) Silver peruranate, Ag 2 U 2 On (?). (Guyard, Bull. Soc. (2) 1. 95.) Does not exist. (Alibegoff, A. 233. 117.) Sodium peruranate, Na 4 UO 8 +SH 2 O. Sol. in H 2 O. SI. sol. in alcohol. (Fairley.) Na 2 UO 5 . As K salt, (de Coninck, C. C. 1909, I. 1970.) +5H 2 O. Decomp. by H 2 O and HC1. (Aloy, Bull. Soc. 1903. (3) 29. 293.) (Na 2 O 2 ) 2 UO 4 -f-8H 2 0. Sol. in H 2 O; de- comp. by dil. HC1, H 2 S0 4 , and by Al(OH) t in aq. solution. (Melikoff, B. 1897, 30. 2903.) Sodium uranyl peruranate, Na 2 (UO 2 )UO 8 + 6H 2 O (?). Sol. inH 2 O. (Fairley.) Pervanadic acid, HVO 4 (?). Sol. in H 2 O. (Pissarjewsky, C. C. 1902, II. 565.) Ammonium pervanadate, NH 4 VO 4 . Sol. in H 2 O 2 +Aq; insol. in alcohol. (Scheuer Z. anorg. 1898, 16. 294.) (NH 4 ) 3 VO 6 +2^H 2 O. Sol. in H 2 O; insol. in alcohol. (Melikoff, B. 1909, 42. 2292.) (NH 4 ) 4 V 2 On. Sol. in H 2 O 2 -f-Aq; ppt. from aq. solution by alcohol. (Melikoff, Z. anorg. 1899, 19. 406.) Barium pervanadate, Ba(VO 4 ) 2 . SI. sol. in H 2 2 +Aq free from H 2 SO 4 ; insol. in alcohol. (Scheuer, Z. anorg. 1898, 16. 288.) Cadmium pervanadate, Cd(VO 4 ) 2 . SI. sol. in H 2 O 2 +Aq; insol. in alcohol. (Scheuer.) Calcium pervanadate, Ca(VO 4 ) 2 . Sol. in H 2 O 2 +Aq; insol. in alcohol. (Scheuer.) PHOSPHIMATE, BARIUM 665 Lead pervanadate, Pb(VO 4 ) 2 . SI. sol. in H 2 O 2 +Aq free from H 2 SO 4 ; insol. in alcohol. (Scheuer.) Lithium pervanadate, LiVO 4 . Sol. in H 2 O 2 +Aq; insol. in alcohol. (Scheuer.) Potassium pervanadate, KVO 4 . Sol. in H 2 O 2 +Aq acidified with H 2 SO 4 ; insol. in alcohol. (Scheuer.) K 8 VO 8 +2^H 2 O. Sol. in H 2 O; insol. in alcohol. (Melikoff, B. 1909, 42. 2293.) 3K 2 2 V0 4 , 2KV0 4 +2H 2 O. 0.855 g. is sol. in 100 g. H 2 O at 19; si. sol. in KOH+ Aq; very stable in the air. (Melikoff and Pissarjewsky, Z. anorg. 1899, 19. 408.) K 4 V 2 O 12 +2H 2 O. (Melikoff and Pissar- jewsky, Z. anorg. 1899, 19. 411.) K 4 V 2 Oi 3 +3^H 2 O. Moderately sol. in H 2 with slow decomp. (Melikoff and Pissar- jewsky, Z. anorg. 1899, 19. 410.) Silver pervanadate, AgVO 4 . SI. sol. in H 2 O 2 +Aq free from H 2 S0 4 ; sol. in alcohol. (Scheuer.) Sodium pervanadate, NaVO 4 . Sol. in H 2 O-^ acidified with H 2 SO 4 ; insol. in alcohol. (Scheuer.) Strontium pervanadate, Sr(VO 4 ) 2 . SI. sol. in H 2 O 2 +Aq free from H 2 SO 4 ; insol. in alcohol. (Scheuer.) Philippium, Ph (?). (Delafontaine, C. R. 87. 559.) Consists of terbium and yttrium. (Roscoe, B. 15. 1274.) Phosgene, CoCl 2 . See Carbonyl chloride. Phosphame, PN 2 H (?). Insol. in H 2 O. Insol. in dil. HNO 3 +Aq; gradually decomp. by cone. HNO 3 . (Rose, Pogg. 24. 308.) Insol. in cone. HNO 3 . (Pauli, A. 123. 236.) Sol. in H 2 SO 4 with decomp. (Rose.) Insol. in dil., but decomp. by cone. KOH or NaOH+Aq. Insol. in alcohol or ether. Formula is perhaps P 3 N 3 H 4 . (Sal/mann, B. 6. 494.) Phosphamic acid, PO<; \OH. (Schiff.) Does not exist, but was impure pyrophos- phodiamic acid. (Gladstone.) Also Mente (A. 248. 245). Pi/rophosphamic acid, P 2 NH 3 O 6 = P 2 O 3 (OH) 3 NH 2 . Deliquescent in moist air; easily sol. in H 2 O or alcohol; si. sol. in ether. (Gladstone, "hem. Soc. 3. 152.) Correct composition is imidocfo'phosphoric acid, P 2 NH 4 O 6 = HO- ' (Mente, A. 248. 232.) Barium pyrophosphamate, Ba 3 (P 2 NH 2 O 6 )2. Sol. in HC1 or HNO 3 +Aq, not in HC 2 H 3 O 2 , Aq. (Gladstone and Holmes, Chem. Soc. (2) 2. 233.) Cupric , C Ppt. Decomp. by cold KOH+Aq. stone, Chem. Soc. 3. 135.) (Glad- Ferric , Fe 2 (P 2 NH 2 O 6 ) 2 +2H 2 O. Insol. in dil. acids. Sol. in cone. H 2 SO 4 , and decomp. by warming. Easily sol. in NH 4 OH+Aq. Decomp. by KOH+Aq. (Gladstone, Chem. Soc. 3. 142.) Lead , Pb 3 (P 2 NH 2 O 6 ) 2 -f 4H 2 O. Insol. in NH 4 OH+Aq. Potassium -, K 3 P 2 NH 2 O 6 . Deliquescent. Sol. in H 2 O. Insol. .in alcohol. (Gladstone, A. 76. 85.) Silver - Ppt. -, Ag 3 P 2 NH 2 O 6 +5H 2 O. Zinc , Zn 3 (P 2 NH 2 O 6 ) 2 . (Gladstone and Holmes, Chem. Soc. (2) 2. 225.) Phosphamide, PON. See Phosphoryl nitride. PN 2 H 3 O. See Phosphoryl imidoamide. jPnphosphamide, PON 2 H 6 . See Phosphoryl iriamide. Tnwetaphosphimic acid, PsNsI^. Sol. in H 2 O; aq. solution does not coagulate albumen. (Stokes, Am. Ch. J. 1895, 17. 275.) Ammonium fn'wetaphosphimate, (NH 4 ) 3 P 3 N 3 6 H 3 . Sol. in H 2 O, insol. in alcohol; unstable. (Stokes, Am. Ch. J. 1896, 18. 643.) Barium Jriwetaphosphimate, Ba 3 (P3N 3 O 6 H 3 )2 +4H 2 0. +6H 2 O. SI. sol. in H 2 O. Easily sol. in NH 4 Cl+Aq and in NaCl+Aq. (Stokes.) 666 PHOSPHIMATE, BAREUM SODIUM Barium sodium inwetaphosphimate, P 3 N 3 O 6 H 3 NaBa + 1 Jjli . Almost insol. in H 2 O; easily sol. in NH 4 C1+ Aq and in NaCl+Aq. (Stokes.) Magnesium Znwetaphosphimate, (P 3 N 3 6 H 3 ) 2 Mg3 (?). Sol. in H 2 O; insol. in alcohol; aq. solution decomp. on boiling. (Stokes.) Potassium ^nwetaphosphimate, K 3 P 3 N 3 O 6 H 3 . Sol. in H 2 O; insol. in alcohol. (Stokes.) Silver in'metophosphimate, Ag 3 P 3 N 3 O 6 H 3 . Ppt.; sol. in NH 4 OH+Aq; insol. in H 2 O; si. sol. in HNO 3 + Aq. (Stokes.) a Sodium Zn'wetaphosphimate, P 3 N 3 O 6 H 3 Na 3 +4H 2 0. 18.3 pts. are sol. in 100 pts. H 8 O at 20; very sol. in hot H 2 O; decomp. by alkali on long boiling. (Stokes.) /3 Sodium ^nwetaphosphimate, P 3 N 3 O 6 H 3 Na 3 +H 2 0. Sol. in H 2 O; insol. in alcohol. (Stokes.) TeJrawetaphosphimic acid, P 4 N 4 8 H 8 +2H 2 0. Very si. sol. in H 2 O; decomposes the sol. salts of HC1, H 2 SO 4 and HNO 3 . (Stokes, Am. Ch. J. 1895, 17. 290.) 100 pts. H 2 O at 20 dissolve 0.64 pt. crystal- lized acid. Somewhat more sol. in boiling H 2 O. (Stokes.) 100 pts. 10% HNO 3 +Aq at 20 dissolve 0.26 pt. of crystallized acid. (Stokes.) Not decomp. by boiling alkalies +Aq. (Stokes, Am. Ch. J. 1896, 18. 785.) Insol. in alcohol. (Stokes, Am. Ch. J. 1896, 18. 784.) Ammonium terametaphosphimate, P 4 N 4 8 H 6 (NH 4 ) 2 . Only si. sol. in boiling H 2 O; sol. in excess ofhot5%HNO 3 . (Stokes.) P 4 N 4 O 8 H 4 (NH 4 ) 4 +4H 2 O. Readily sol. in H 2 O; si. sol. in NH 4 OH+Aq. (Stokes.) Barium tefraraetaphosphimate, P 4 N 4 O 8 H 4 Ba 2 +2H 2 0. Ppt.; insol. in H 2 O. (Stokes.) Potassium ^rametaphosphimate, P 4 N 4 O 8 H 6 K 2 . SI. sol. in boiling H 2 O; sol. in cold dil. KOH +Aq. (Stokes.) P 4 N 4 Q 8 H 4 K 4 (?). Very sol. in H 2 O. (Stokes.) Silver ^rametaphosphimate, P 4 N 4 O 8 H 4 Ag 4 . Ppt.; insol. in H 2 O; si. sol. in HNO 8 +Aq. (Stokes.) P 4 N 4 O 8 Ag 8 . Ppt.; sol. in NH 4 NO 3 +Aq. (Stokes.) Sodium ^rawetaphosphimate, P 4 N 4 O 8 H 4 Na 4 wetap ?) H 2 SI. sol. in cold H 2 O. Easily sol. in hot H 2 O. Ppt. from aqueous solution by excess of al- kali. (Stokes.) Penfometaphosphimic acid, PO ro / NH - pa ( OH ) NH - PO ( H )\NH u - ( - u1 \NH.PO.(OH)NH.PO(OH)/ JN = HioPsNsOio. Sol. in H 2 O; pptd. by alcohol. (Stokes, Am. Ch. J. 1898, 20. 748.) Magnesium pentametaphosphimatej (P 5 N 5 10 Hg) 2 Mg, Ppt. (Stokes.) P 5 N 6 OioH 6 Mg 2 +5H 2 O. Ppt., insol. in al- cohol; almost insol. in H 2 O; si. sol. in cone. acetic acid. (Stokes.) Silver pentaraetaphosphimate, P 5 NsOioH 6 Ag5. Ppt., sol. in cold KOH+Aq with decomp. (Stokes.) Sodium pewtametaphosphimate, P 5 N5O 10 H 5 Na5+2H 2 O. Sol. in H 2 O; insol. in alcohol. (Stokes.) P 5 N5O 10 H 6 Na 4 +2H 2 O. Sol. in 80% acetic acid; pptd. by alcohol. (Stokes.) Hexametaphosphiirdc acid. Silver Aezaraetaphosphimate, PeNeO^HeAge. Ppt.; decomp. by cold KOH+Aq. (Stokes, Am. Ch. J. 1898, 20. 757.) Sodium hexametaphosphimaLte, PeNe 1 +2H 2 O. Sol. in H 2 O; pptd. by alcohol. (Stokes.) Phosphine. See Hydrogen phosphide. PT/rophosphodiamic acid, P 2 N 2 H 6 S = P 2 3 (OH) 2 (NH 2 ) 2 . Deliquescent. Easily sol. in H 2 O, alcohol, or ether. Sol. in cold cone. H 2 SO 4 without decomp. (Gladstone, Chem. Soc. 3. 353.) Correct composition is cftimidodiphosphoric acid, P 2 N 2 H 4 4 +H 2 =HO PO = (NH) 2 = PO OH. (Mente.) Aluminum pyrophosphodiaitLate. Precipitate. Sol. in NH 4 OH+Aq. Insol. in acids. (Gladstone, A. 76. 82.) Ammonium , Psty^jj^' Very deliquescent in moist air. Sol. in H 2 O. ery equescen (Schiff, A. 103. 168.) PHOSPBOARSENIOVANADICOVAN ADIOTUN GSTATE, AMMONIUM 667 Barium p^/rophosphocftamate, BaP 2 O 6 (NH 2 ) 2 . Precipitate. SI. sol. in H 2 O. Sol. in NH 4 OH+Aq. (Gladstone.) Calcium , CaP 2 O 5 (NH 2 ) 2 . Insol. in NH 4 OH+Aq. Sol. in NH 4 C1+ Aq and acids. (Gladstone and Holmes.) Lead . Ppt. Decomp. by H 2 O. Magnesium . Ppt. (Gladstone and Holmes.) Silver , Ag 2 P 2 O 5 (NH 2 ) 2 . SI. sol. in H 2 O. Sol. inHNO 3 +Aq. (Glad- stone and Holmes.) Strontium . Sol. in acids and NH 4 Cl+Aq. Insol. in NH 4 OH+Aq. (Gladstone and Holmes, Chem. Soc. (2) 4. 295.) Zinc , ZnP 2 O 6 (NH 2 ) 2 . Ppt. (Gladstone and Holmes.) Pyrophosphotriamic acid, P 2 N 3 H 7 O 4 = OH Decomp. by boiling H 2 O or HC1. Sol. in cone. H 2 SO 4 upon heating. (Gladstone and Holmes.) Correct formula is. HO PO< NH 2 =diimidod^phosphoworiamic acid. (Mente, A. 248. 241.) Ammonium pyrophosphotriamate, p o ) 4 F2 3 (NH 2 ) 3 . Insol. in H 2 O. (Gladstone and Holmes.) Barium , BaP 2 N 3 H 5 O 4 . BaH 2 (P 2 N 3 H 5 O 4 ) 2 . Decomp. by HCl+Aq. (Gladstone, Chem. Soc. 4. 6.) Cobaltous --- , CoP 2 N 3 H 5 O 4 . Slowly decomp. by dil. H 2 SO 4 +Aq, not by HCl+Aq. (Gladstone and Holmes, Chem. Soc. (2) 4. 1.) Cupric - , CuP 2 N 3 H 5 O 4 . Insol. in H 2 O or NH 4 OH + Aq. (Gladstone and Holmes, Chem. Soc. (2) 4. 1.) Ferrous -- , FeH 6 (P 2 N 3 H 3 O 4 ) 2 . ' Insol. in dil. acids. (Gladstone, Chem. Soc. (2) 4. 1.) Lead -- , H 2 Pb 3 (P 2 N 3 H 3 O 4 ) 2 . Ppt. (Gladstone and Holmes, Chem. Soc. (2) 4. 1.) H 4 Pb 2 (T 2 N 3 H 3 O 4 ) 2 . Ppt. (G. and H.) H 6 Pb(P 2 N 3 H 3 O 4 ) 2 . (G. and H.) Mercuric pyrophosphotriamate, Hg 2 P 2 N 3 H 3 4 . Insol. in H 2 O or dil. HC1 or HNO 3 +Aq. (Gladstone and Holmes, Chem. Soc. (2) 4. 1.) Platinum , Pt 2 P 2 N 3 H 3 O 4 . Decomp. by H 2 O when freshly pptd. (G. and H.) Potassium , KP,N 3 H 6 O 4 . Almost insol. in H 2 O. (Gladstone, Chem. Soc. 4. 10.) Silver , Ag 3 P 2 N 3 H 4 O 4 . Ppt. SI. attacked by HC 2 H 3 O 2 ; decomp. by HNO 3 or NH 4 OH+Aq into AgH 2 P 2 N 3 H 4 O 4 . Insol. in H 2 O. Decomp. by HC1. (Gladstone, Chem. Soc. (2) 4. 1.) Zinc . Insol. in H 2 O. (Gladstone and Holmes.) JWraphosphocframic acid, P 4 N 2 H 8 Oii = P 4 7 (OH), (NH 2 ) 2 . Known only as NH 4 salt. Ammonium tetraphosphodiamate, 4 H(NH 4 ) 3 ^ Very deliquescent, and sol. in H 2 O. (Glad- stone.) Ammonium ^hydrogen te^raphosphocfo'amate, :etraphosph( 4 H 2 (NH 4 ) 2 Insol. in cold, easily sol. in hot H 2 O and dil. acids. (Gladstone.) Tetraphosphotetramic acid, Sol. in H 2 O. Insol. in alcohol. (Gladstone.) Ammonium tetraphosphot etramate, p (0 2 HNH 4 ) P4 7 (NH 2 ) 4 . Sel. in H 2 O, and precipitated from solution by alcohol. (Gladstone.) Silver -- , Ag 6 P 4 N 4 H 4 O 9 . Ppt. Ag 2 H 4 P 4 N 4 H 4 9 . Ppt. Ammonium phosphoarseniovanadico- vanadiotungstate. See Arseniophosphovanadicovanadiotung- state, ammonium. 668 PHOSPHOAZOTIC ACID Tetraphosphopentsizotic acid, Ins pi. in H 2 O. Decomp. gradually by boil- ing with H/). (Gladstone.) Ammoniotetraphosiphopentazotic acid (?), Decomp. by H 2 O. (Gladstone.) Cupric tetraphosphopentazot&te, (Gladstone, Chem. Soc. (2) 6. 261.) Lead^ . (Gladstone, Chem. Soc. (2) 6. 261.) Potassium , KOP 4 N 5 H 8 6 . Insol. in HoO. (Gladstone, Chem. Soc. (2) 6. 268.) Phosphoboric acid, H 3 BO 3 , H 3 PO 4 = BPO 4 +3H 2 O. Not decomp. by boiling H 2 O or cone, acids. Sol. in boiling solution of caustic alkalies. (Vogel, N. Repert. Pharm. 18. 611.) Phosphochloroplatinous acid, P(OH) 3 , PtCl 2 . See Chloroplatinophosphoric acid. Phosphochromic acid. Ammonium phosphochromate, 3(NH 4 ) 2 O, P 2 O 5 , 8CrO 3 +H 2 O. Sol. in H 2 O with decomp. (Friedheim, Z. anorg. 1894, 6. 284.) Potassium phosphochromate, 2K 2 O, P 2 O 5 , 4CrO 3 +H 2 O. Sol. in H 2 O but cannot be cryst. therefrom without decomp. Can be cryst. without de- comp. from H 2 O containing phosphoric acid. (Friedheim.) 3K 2 O, P 2 O 6 , 8CrO 3 . Sol. in H 2 O but cannot be cryst. therefrom without decomp. (Blondel, C. R. 1894, 118. 194.) Phosphohypophosphotungstic acid. Potassium sodium phosphohypophosphotung- state, 9K 2 O, Na 2 O, 4P 2 O 5 , 2PO 2 H 3 , 26WO 3 +23H 2 O. Precipitate. Easily sol. in hot H 2 O. (Gibbs, Am. Ch. J. 7. 313.) Tetraphosphotetrimidic acid, Known only in its salts. (Gladstone.) Silver ^raphosphoterimidate. Ppt. (Gladstone.) Phosphoiodic acid, P 2 O 5 , 18I 2 O 5 +4H 2 O. Decomp. by H 2 O. (Chretien, A. ch. 1898, (7) 15. 389.) Ammonium phosphoiodate, 4(NH 4 ) 2 O, P 2 O 5 , 18I 2 O 5 + 12H 2 O. Sol. in H 2 O. SI. sol. in cone. H 3 PO 4 +Aq. (Chretien.) Lithium phosphoiodate, 3Li 2 O, P 2 O 5 , 18I 2 O 5 + 11H 2 O. Sol. in H 2 O. SI. sol. in cone. H 3 PO 4 +Aq. (Chretien.) Potassium phosphoiodate, 4K 2 O, P 2 O 5 , 18I 2 O 5 +5H 2 O. Decomp. by a small amt. of H 2 O; sol. in a large amt. SI. sol. in cone. H 3 PO 4 +Aq. (Chretien.) Sodium phosphoiodate, 6Na 2 O, P 2 O 5 , 18I 2 O 5 +5H 2 0. Sol. in H 2 O. SI. sol. in cone. H 3 PO 4 +Aq. (Chretien.) Phosphoiridic acid. See Chlorophosphoiridic acid. Phospholuteotungstic acid, H 5 PW 8 O 29 . See under Phosphotungstic acid. Phosphomolybdic acid, P 2 O 6 , 18MoO 3 11 Phospholuteomolybdic acid." Deliquescent. Sol. in H 2 O in all propor- tions. (Kehrmann, Z. anorg. 1894, 7. 418.) 3H 2 O, P 2 O 5 , 20MoO 3 +21H 2 O. Very sol. in H 2 O. Sol. in ether. By evaporation of H 2 O solution crystals with 44H 2 O, or from a strong solution in cone. HNO 3 +Aq, with 19H 2 O, are obtained; also crystals with 38, and 48H 2 O are known. (Debrav, C. R. 66. 704.) According to Rammelsberg (B. 10. 1776) formula is 3H 2 O, P 2 O 5 , 22MoO 3 . According to Gibbs (Am. Ch. J. 3. 317) formula is 3H 2 O, P 2 O 5 , 24MoO 3 +59H 2 O. Finkener (B. 11. 1638) gives the formula as 3H 2 O, P 2 O 5 , 24MoO 3 +58H 2 O, also with 29H 2 0. P 2 O 5 , 20MoO 3 +52H 2 O. Sol. in dry ether with evolution of heat, and subsequent separ- ation into two layers, the upper consisting of pure ether, and lower of a solution of acid in ether. Sp. gr. of lower layer, when sat. at 13, is 1.3. On warming lower layer, ether separates out and forms an upper layer. This redissolves on cooling and shaking. The lower layer is insol. in H 2 O and miscible with al- cohol. PHOSPHOMOLYBDATE, AMMONIUM CADMIUM 669 100 pts. ether thus dissolve 80.6 pts. acid at 0; 84.7 pts. at 8.1; 96.7 pts. at 19.3; 103.9 pts. at 27.4; 107.9 pts. at 32.9. (Par- mentier, C. R. 104. 688.) P 2 O 5 , 22MoO 3 +57H 2 O, and +58H 2 O. (Pohl, Dissert. 1906.) P 2 O 5 , 23MoO 3 +61H 2 0. (Pohl.) P 2 O 5 , 24MoO 3 +61H 2 O. (Miolati, C. C. 1903, 11. 789.) +64H 2 O. (Pohl.) Diphosphope/itomolybdic acid, H 6 P 2 Mo 5 O 23 = 3H 2 O, P 2 O 5 , 5MoO 3 . Not known in free state. Ammonium phosphomolybdate, (NH 4 ) 2 O, P 2 O 5 , 2MoO 8 +2H 2 O. (Meschorier, Dissert. 1894.) 2(NH 4 ) 2 O, P 2 O 6 , 4MoO 3 +5H 2 O. (Fried- heim, Z. anorg. 1894, 6. 33.) +6H 2 O. (Perlberger, Dissert. 1904.) (NH 4 ) 3 PO 4 , HMo0 3 +6H 2 O. Formula is (NH 4 ) 3 PO 4 , 10MpO 3 + l^H 2 O, according to the older authorities. Scarcely sol. in H 2 O or aqueous acid solu- tions. Easily sol. in ammonia, and alkalies + Aq. (Svanberg and Struve, J. pr. 44. 291.) It is almost completely insol. in a mixture of CNH 4 ) 2 MoO 4 +Aq, and dil. HNO 3 +Aq. Absolutely insol. in a dil. nitric acid solution of ammonium nitrate. (Richters, Z. anal. 10. 471.) Solubility is increased even in presence of ammonium molybdate and free HNO 3 by HC1, ammonium, and other chlorides, tar- taric acid, or large quantities of ammonium oxalate or citrate. Not precipitated in pres- ence of excess of H 3 PO 4 . (Fresenius, Z. anal. 3. 446.) Sol. in 10,000 pts. H 2 O at 16; in 6600 pts. H 2 O containing 1 vol. % HNO 3 ; in 550 pts. HCl+Aq of 1.12 sp. gr.; in 620 pts. alcohol of 0.80 sp. gr.; in 190 pts. HNO 3 +Aq (sp. gr. - 1.2) at 50; in 5 pts. cone. H 2 SO 4 at 100; in 3 pts. NH 4 OH+Aq of 0.95 sp. gr. (Eggertz, J. pr. 79. 496.) Sol. in 21,186 pts. H 2 O, 38,117 pts. dil. alcohol, and 13,513 pts. strong alcohol. (Hehner, Analyst, 1879. 23.) According to Sonnenschein, the solubility is increased by much H 2 O or alcohol, alkaline hydroxides, carbonates, ortho-, pyro-, and metaphosphates; sodium borate, hyposul- phate, thiosulphate, acetate, arsenate, and arsenite; potassium sodium tartrate, ammo- nium oxalate, orthophosphoric acid, and sul- phuric acid. It is not increased by ammo- nium molybdate or sulphate, potassium sul- phate, acid tartrate, acid oxalate, nitrate, or chlorate, iodide, chloride, or bromide; sodium bromide or nitrate; nitric, hydrochloric, boric, tartaric, oxalic, and dilute sulphuric acids. (Sonnenschein, J. pr. 63. 342.) Sol. in hot H 2 O. Sol. in cold caustic alkalies, alkali carbonates, and phosphates, NH 4 C1, and (NH 4 ) 2 C 2 O 4 +Aq; si. sol. in (NH 4 ) 2 SO 4 , KNO 3 , and KCl+Aq; very si. sol. in NH 4 NO 3 +Aq. Sol. in K 2 SO 4 , Na 2 SO 4 , NaCl, MgCl 2 , H 2 SO 4 , HC1, and cone, or dil. HNO 3 +Aq. Presence of (]\H 4 ) 2 MoO 4 totally changes the effect of acid liquids; insol. in dil. HNO 3 or H 2 SO 4 +Aq containing (NH 4 ) 2 MoO 4 , but somewhat sol. in HCl+Aq, even in presence of that salt. Tartaric acid and similar organic substances totally prevent the precipitation of this salt. (Eggertz in Fresenius' Quant, anal.) 5(NH 4 ) 2 O, 48MoO 3 , 2P 2 O 6 + 17H 2 O = 3(NH 4 ) 2 O, 24MoO 3 , P 2 O 5 +2(NH 4 ) 2 O, H 2 O, 24MoO 3 , P 2 O 5 +16H 2 O. Formula of above salt according to Gibbs. 3(NH 4 ) 2 O, 22MoO 3 , PoO 5 +9H 2 O, or 12H 2 0. 8(NH 4 ) 2 O, H 2 O, 60MoO 3 , 3P 2 O 5 +11H 2 O. SI. sol. in H 2 O. 3(NH 4 ) 2 O, 16MoO 3 , P 2 Oft+14H 2 O. Insol. in cold, sol. with decomp. in hot H 2 O. Sol. in NH 4 OH+Aq. (Gibbs, Am. Ch. J. 3. 317.) 5(NH 4 )oO, P 2 O 5 , 16MoO 3 . (Meschoirer, Dissert, 1894.) 3(NH 4 ) 2 O, P 2 O 5 , 18MoO 3 +14H 2 O. Sol. in H 2 O. The aqueous solution is stable at ordinary temp, for several days, but when warmed ordinary ammonium phosphomolyb- date separates. (Kehrmann, Z. anorg. 1894, 7. 414.) 3(NH 4 ) 2 O, P 2 O 5 , 28MoO 3 +8H 2 O. 100 g. H 2 O dissolve 0.0238 g. at 15. 1 pt. is sol. at 15 in 4206 pts. H 2 O; 7300 pts. 5% NH 4 N0 8 + Aq; 4930 pts. 1% HNO 3 +Aq. (de Lucchi, Rass. Min. 1910, 32. 21.) 9(NH 4 ) 2 O, 2P 2 O 5 , 28MoO 3 +8H 2 O. (Mes- choirer, Dissert. 1894.) Ammonium eftphosphopentamolybdate, 2(NH 4 ) 3 PO 4 , 5MoO 3 +7H,O = 3(NH 4 ) 2 O, 5MoO 3 , P 2 O 5 +7H 2 O. Easily sol. in hot, less in cold H 2 O. (Zenk- ner, J. pr. 58. 256.) 5(NH 4 ) 2 O, H 2 O. 10MoO 3 , 2P 2 O 5 +6H 2 O = 3(NH 4 ) 2 O, 5MoO 3 , P 2 O 5 +2(NH 4 ) 2 O, H 2 O, 5MoO 3 , P 2 O 5 +6H 2 O. Sol. in H,O. (Gibbs, Am. Ch. J. 1895, 17. 87.) +8H,O. (Perlberger.) + 18H 2 O. (Mazzuchelli and Zangrilli, Gazz. ch. it. 1910, 40. (2) 55.) 5(NH 4 ) 2 O, P 2 6 , 10MoO 8 +13H 2 O, and +14H 2 O. (Perlberger, Dissert. 1904.) Ammonium barium phosphomolybdate, 3(NH 4 ) 2 O, 30BaO, P 2 O 5 , 30MoO 3 . Insol. precipitate. (Seligsohn, J. pr. 67. 478.) Ammonium cadmium phosphomolybdate, 5(NH 4 ) 2 O, CdO, P 2 O 5 , 6MoO 3 +8H 2 O. (Perlberger, Dissert, 1904.) 3(NH 4 ) 2 , 2CdO, 2P 2 O 6 , 9MoO 3 -f 141H 2 O. (Perlberger.) 670 PHOSPHOMOLYBDATE, AMMONIUM COBALTOUS Ammonium cobaltous phosphomolybdate, (NH 4 ) 2 O, 2CoO, P 2 O 8 , 5MoO 3 + 10H 2 O. Decomp. by cold H 2 O. Sol. in acids and hot H 2 O. (Arnfeld, Dissert, 1898.) 4(NH 4 ) 2 6, CoO, 2P 2 O 5 , 10MoO 3 + 12H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Arn- feld.) , Ammonium manganous phosphomolybdate, (NH 4 ) 2 O, 2MnO, P 2 O 5 , 5MoO 3 +20H 2 O. Decomp. by H 2 O, but dissolves clear on heating. (Arnfeld.) 4(NH 4 ) 2 O, MnO, 2P 2 O 5 , 10MoO 3 + 13H 2 O. (Arnfeld.) 5(NH 4 ) 2 O, IGMnO, 2P 2 O 5 , 20MoO 3 + 10H 2 O. Very si. sol. in H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 87.) Ammonium nickel phosphomolybdate, (NH 4 ) 2 O, 2NiO, P 2 O 5 , 5MoO 3 + 10H 2 O. Decomp. by cold, but sol. in hot H 2 O. (Arnfeld.) (NH 4 ) 2 O, NiO, 2P 2 O 5 , 10MoO 8 + 12H 2 O. Very sol. in H 2 O. ' (Arnfeld.) Ammonium potassium phosphomolybdate, 6(NH 4 ) 2 O, 15K 2 O, 2P 2 O 5 , 60MoO 3 + 12H 2 0. Sol. in H 2 O. Insol. in alcohol. (Seligsohn, J. pr. 67. 477.) Ammonium sodium phosphomolybdate, 6(NH 4 ),O, 15Na 2 O, 2P 2 O 5 , 60MoO 3 + 18H 2 O. Sol. in much boiling H 2 O. Insol. in alcohol. (Seligsohn, J. pr. 67. 474.) Barium phosphomolybdate, 3BaO, P 2 O 5 , 24MoO 3 +zH 2 O. Moderately sol. in cold, very easily sol. in hot H 2 O. Decomp. in aqueous solution at ordinary temp, on standing. (Kehrmann, Z. anorg. 1894, 7. 414.) Cgssium phosphomolybdate, 3Cs 2 O,^P 2 O 5 , 6MoO 3 -H8H 2 O. Ppt. (Ephraim, Z. anorg. 1910, 65. 240.) 2Cs 2 O, P 2 O 5 , 14MoO 3 +3H 2 O. Difficultly sol. in H 2 O. (Ephraim.) 3Cs 2 O, P 2 6 5 , 21MoO 3 +4H 2 O (?). (Ephraim.) Calcium potassium phosphomolybdate, 2CaO, 3K 2 O, 2P 2 O 5 , 10MoO 3 +22H 2 O. (Friedheim, Z. anorg. 1893, 4. 293.) Cobaltous phosphomolybdate, 2CoO, P 2 O 5 , 4MoO 3 +zH 2 O. (Arnfeld, Dissert. 1898.) 3CoO, P 2 O 5 , 5MoO 3 + 16MH 2 O, and + 17K H 2 O. Extremely sol. in H 2 O. (Arnfeld.) 3CoO, P 2 O 5 , 18MoO 3 +38H 2 O. Sol. in H 2 O. (Arnfeld.) 3CoO, P 2 O 6 , 24MoO 3 -|-58H 2 O, and+60H 2 O. Sol. in HoO. (Arnfeld.) Cobaltous potassium phosphomolybdate, K 2 O, 2CoO, P 2 O 5 , 5MoO 3 +15H 2 O. (Arnfeld.) 4K 2 O, CoO, 2P 2 O 5 , 10MoO 3 + 12H 2 O. SI. sol. in cold, easily sol. in hot H 2 0. (Arnfeld.) Croceocobaltic phosphomolybdate, 24MoO 3 , P 2 5 , [Co(NH 3 ) 4 (N0 2 ) 2 ] 2 0, 2H 2 + 21H 2 O. SI. sol. in cold, easily in hot H 2 O. (Gibbs, Am. Ch. J. 3. 317.) Gold phosphomolybdate ammonia, 12Au 2 O 3 , 7P 2 O , 3MoO 3 , 24NH 3 +21H 2 O. Insol. in H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 172.) Gold sodium phosphomolybdate ammonia, 5Au 2 O 3 , Na 2 O, P 2 O 5 , HMoO 3 , 15NH 3 + 10H 2 O. Sol. in dil. HC1. Almost insol. in NH 4 OH + Aq. (Gibbs.) Lead phosphomolybdate, 23PbMo0 4 , P 2 O 5 , 2PbPO 4 +7H 2 O. Sol. in 500,000 pts. H 2 O. Insol. in NH 4 OH +Aq. Easily sol. in KOH, ISlaOH, or HNO 3 4-Aq; somewhat less sol. in HC 2 H 3 O 2 -fAq. (Beuf, Bull. Soc. (3) 3. 852.) Lithium phosphomolybdate, 12Li 2 O, 4P 2 O 5 , 5MoO 3 + 18H 2 O. Partially sol. in H 2 O. (Ephraim, Z. anorg. 1909, 64. 233.) 3Li 2 O, P 2 O 5 , 5MoO 3 + 16H 2 O. Ppt. (Ephraim, Z. anorg. 1910, 65. 233-6.) 3Li 2 O, P 2 O 5 , 5MoO 3 + 17H 2 O. Ppt. (E.) 5Li 2 O, 2P 2 O 5 , 8MoO 3 +28H 2 O. Easily sol. in H 2 O. (E.) 3Li 2 O, P 2 O 5 , 12MoO 3 + 18H 2 O. Ppt. (E.) 3Li 2 O, P 2 O 5 , 18MoO 3 +27H 2 O. Sol. in H 2 O. (E.) Manganous phosphomolybdate, 3MnO, P 2 O 5 , 5MoO 3 +20H 2 O. Very sol. in H 2 O. SI. sol. in alcohol. (Arn- feld.) 3MnO, P 2 O 5 , 18MoO 3 +38H 2 O. Sol. in H 2 O. (Arnfeld.) 3MnO, P 2 O 5 , 24MoO 3 +58H 2 O, and +60 H 2 O. Easily sol. in H 2 O. (Arnfeld.) Manganous potassium phosphomolybdate, 2MnO, 3K 2 O, 2P 2 O 5 , 10MoO 3 +30H 2 O. Sol. in hot H 2 O. (Arnfeld.) Manganous sodium phosphomolybdate, 7MnO, 9Na 2 O, 2P 2 O 5 , 22MoO 3 +57H 2 O. Nearly insol. in cold H 2 O. Sol. in boiling H 2 O but decomp. thereby. (Gibbs, Am. Ch. J. 1895, 17. 85.) Nickel phosphomolybdate, 2NiO, P-..O 5 , 4MoO 3 +zH 2 O. Ppt. (Arnfeld.) 3NiO, P 2 O 5 , 5MoO 3 +20H 2 O. Decomp. by H 2 O. '(Arnfeld.) PHOSPHONITRYLATE, SILVEB 671 3NiO, P 2 O 5 , 18MoO 3 -t-34H 2 O. Sol. in H,O. (Arnfeld.) 3NiO, P 2 O 5 , 24MoO 3 +58H 2 O, and+60H 2 O. Efflorescent. Sol. in H 2 O. (Arnfeld.) Nickel potassium phosphomolybdate, K 2 O. 2NiO, P 2 O 5 , 5MoO 3 + 13H 2 O. Decomp. by cold H 2 O, but goes into solu- tion by boiling. (Arnfeld.) 4K 2 O, NiO, 2P 2 O 5 , 10MoO 3 + 12H 2 O. Sol. in H 2 O. (Arnfeld.) Potassium phosphomolybdate, K 3 PO 4 , HMoO 3 + l^H 2 O =3K 2 O, P 2 O 5 , 22MoO 3 +3H 2 O. Insol. in H 2 O. Easily sol. in alkalies. (Svanberg and Struve.) 100 g. H 2 O dissolve 0.007 g. at 30; 100 g. 10% HNOa+Aq dissolve 0.204 g. at 30. (Donk, Bull. 90, Bur. of Chem., U. S. Dept. of Agric. 1905.) According to older authorities the formula is K 3 PO 4 , 10MoO 3 + l^H 2 O. -f6H 2 O. (Rammelsberg.) 2K 2 O, H 2 O, 24MoO 3 , P 2 O 5 +3H,O. SI. sol. in cold H 2 O. 5K 2 O, H 2 O, 44MoO 3 , 2P 2 O 5 +21H,O. (Gibbs, Am. Ch. J. 3. 317.) 3K 2 O, P 2 O 6 , 18MoO 3 +llH 2 O, and +15H 2 O (EUas.) + 14H 2 O. SI. sol. in cold, very easily sol. in hot H 2 O. Can be cryst. from hot H 2 O. (Kehrmann, Z. anorg. 1894, 7. 416.) 3K 2 O, P 2 O 5 , 17MoO 3 + 12H 2 O. Moder- ately sol. in H 2 O. (Elias, Dissert. 1906.) 5K 2 O, P 2 O 6 , 17MoO 3 +zH 2 O. Aqueous solution decomp. rapidly in the cold. (Kehr- mann, Z. anorg. 1894, 7. 423.) 4K 2 O, 2H 2 O, 9MoO 3 , P 2 O 5 + 18H 2 O. (Zenkner.) 5K 2 O, H,O, 10MoO 3 , P 2 O 5 + 19H 2 O. Eas- ily sol. in H 2 O. (Rammelsberg, B. 10. 1776.) 6K 2 O, 15MoO 3 , P 2 O 5 . Insol. in H 2 O. Sol. inKOH+Aq. (Rammelsberg.) K 2 O, P 2 O 5 , 2MoO 3 + 13H 2 6. Very sol. in H 2 O. (Friedheim, Z. anorg. 4. 287.) 2K 2 O, P 2 O 5 , 4MoO 3 +8H 2 O. Sol. in H 2 O. (Friedheim.) Potassium diphosphopentamolybdate, 3K 2 O, P 2 O 5 , 5MoO 3 +7H 2 O. Sol. in H 2 O; precipitated by HNO 3 or HC1 +Aq. (Zenkner, J. pr. 68. 261.) 2K 2 O, P 2 O 5 , 5MoO 3 +6H 2 O. (Friedheim.) Potassium cfo'phosphopentamolybdate nitrate, 2K 3 PO 4 , 5MoO 3 , 6KNO 3 +9H 2 O. (Debray, C. R. 66. 706.) Rubidium phosphomolybdates: 7Rb 2 O, P 2 O 5 , 22MoO 3 +12H 2 O; 3Rb 2 O, P 2 5 , 20MoO 3 + 12H 2 O; 6RboO, ; P 2 O 5 , 18MoO 3 + 10H.O; 5Rb 2 O, 2P 2 O 6 , 9MoO 3 + 13H 2 O; 7Rb 2 O, 3P 2 O 5 , 10Mo0 8 + 15H 2 O. (Ephraim, Z. anorg. 1910, 65. 237-9.) Silver phosphomolybdate, 7Ag 2 O, P 2 O 5 , 20MoO 3 +24H 2 O. Ppt. Sol. in dil. HNO 3 +Aq, forming 2Ag 2 O, P 2 O 5 , 20MoO 3 +7H 2 O. SI. sol. in H 2 O. (Rammelsberg.) Formula of first salt is 7Ag 2 O, 22MoO 3 , P 2 O 5 + 14H 2 O. Sol. in hot H 2 O, but solution is quickly decomp. (Gibbs, Am. Ch. J. 3. 317.) 7Ag 2 O, P 2 O 5 , 24MoO 3 . Ppt. (Miolati, J. pr. 1908 (2) 77. 451.) Silver cftphosphopentamolybdate, Ag 6 Mo 5 P 2 O 23 +7H 2 O. Easily sol. in H 2 O. (Debray, C. R, 66. 705.) Sodium phosphomolybdate. Sol. in H 2 O and HNO 3 +Aq. (Sonnen- schein, A. 104. 45.) Na 2 O, 5HoO, P 2 O 6 , 18MoO 3 +xH 2 O. 2Na 2 O, 4H 2 O, P 2 O 5 , 18MoO 3 +xH 2 O. 3Na 2 O, P 2 O 5 , 18MoO 3 +26H 2 O. (Fried- heim.) 3Na 2 O, P 2 O 5 , 24MoO 3 +42H 2 O. (Rosen- heim and Pinsker, Z. anorg. 1911, 70. 79.) Sodium diphosphopentomolybdate, 3Na 2 O, P 2 O 5 , 5MoO 3 +14H 2 O. Easily sol. in H 2 O. (Debray.) Sodium auramine phosphomolybdate, Na 2 O, 5Au 2 O 3 , 2P 2 O 5 , HMoO,, 15NH 3 . Sol. in hot H 2 O. Very sol. in hot HC1. (Gibbs, Am. Ch. J. 1895, 17.171.) Metaphosphomolybdic acid. Ammonium mono wetaphosphomolyb date, 3(NH 4 ) 2 O, 4NH 4 PO 3 , 10MoO 3 +9H 2 O. Very sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 392.) Barium Aezcmetaphosphomolybdate, BaO, Ba 3 (PO 3 ) 6 , 14MoO 3 +55H 2 O. Sol. inH 2 O. (Gibbs.) PwrophosphonitryUc acid, P,HNO 4 = OH P,O ; N. Not known in free state. Ammonium pyrophosphonitrylate, ONH 4 2 3 N. Insol. but gradually decomp. by H 2 O. (Gladstone.) Potassium , KP 2 NO 4 . Insol. in H 2 O. (Gladstone.) Silver , AgP 2 NO 4 . Ppt. 672 PHOSPHONITRILIC CHLORAMIDE TYiphosphonitrilic chloramide, P 3 N 3 C1 4 (NH2)2. Sol. in H 2 O without decomp.; sol. in ether, alcohol; si. sol. in benzene. (Stokes, Am. Ch. J. 1895, 17. 287.) TViphosphonitrilic tefrachlorhydrin, P 3 N 3 C1 4 O 2 H 2 . Sol. in ether, alcohol, and H 2 O; insol. in benzene and CS 2 . (Stokes, Am. Ch. J. 1895, 17. 286.) Tn'phosphonitrilic chloride, P 3 N 3 C1 6 . Sol. in glacial acetic acid and H 2 SO 4 . 100 pts. ether dissolve 46.5 pts. at 20. (Liebig.) Insol. in light petroleum; sol. in benzene. (Stokes, Am. Ch. J. 1897, 19. 783.) TWraphosphonitrilic chloride, P 4 N 4 C1 8 . Sol. in alcohol, ether, benzene, H 2 SO 4 . SI. sol. in H2O with decomp. 100 pts. ether dis- solve 12.3 pts. at 20. (Stokes, Am. Ch. J. 1895, 17. 281.) Pentaphosphonitrilic chloride, (PNC1 2 ) 5 = P 5 N 5 C1 10 . Sol. 'in benzene, light petroleum, acetic acid, ether, CS 2 ; insol. in H 2 O. (Stokes, Am. Ch. J. 1897, 19. 790.) flerraphosphonitrilic chloride, (PNC1 2 ) 6 = P 6 N 6 C1 12 . Sol. in benzene, light petroleum, ether, CS 2 ; insol. in H 2 O. (Stokes.) JF/eptaphosphonitrilic P 7 N 7 C1 14 . chloride, (PNC1 2 ) 7 = Sol. in benzene, light petroleum, ether, CS 2 ; insol. in H 2 O; sol. in alcohol with decomp. (Stokes.) Pofo/phosphonitrilic chloride, (PNCl 2 )a;. Depolymerizes on distillation; insol. in benzene and light petroleum and all neutral solvents; sol. in H 2 O with decomp. (Stokes.) Phosphonitrilochloramide, P 2 N 2 C1 3 (NH 2 ) . Slowly sol. in H 2 O with decomp. Insol. in ether and CSo. SI. sol. in boiling CC1 4 . (Besson and Rosset, C. R. 1908, 146. 1149.) Phosphonium bromide, PH 4 Br. Decomp. violently by H 2 O. Phosphonium chloride, PH 4 C1. (Ogier, Bull. Soc. (2) 32. 483.) Phosphonium titanium chloride, 2PH 4 C1, 3TiCl 4 . Decomp. by H 2 O, HC1, or alkalies +Aq. R ose.) Phosphonium iodide, PH 4 I. Decomp. by H 2 O, alkalies, alcohol, etc. (Rose, Pogg. 46. 636.) Decomp. by PC1 3 . (Wilde, B. 16. 217.) Phosphonium sulphate (?). . Deliquescent; very unstable. (Besson, C. R. 109. 644.) Phosphoramide, P(NH 2 ) 3 . Insol. in NH 4 Br, 3NH 3 ; sol. in NHJ, 3NH 3 . (Hugot, C. R. 1905, 141. 1235.) Phosphortn'amide, PON 3 H 6 . See Phosphoryl in'amide. Phosphoric acid, anhydrous, P 2 Os. See Phosphorus pentoxide. Afetaphosphoric acid, HPO 3 . Sol. in H 2 O. Not isolated. (Fleitmann, Pogg. 78. 362.) Deliquescent. Sol. in H 2 O, but aqueous solution decomp. into H 3 PO 4 , slowly in the cold, but more rapidly on heating. Cone, solutions decomp. more rapidly than when dil. (Giran, A. ch. 1903, (7) 3(f. 203.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) ZH'raetaphosphoric acid, H 2 P 2 O 6 . Not isolated. (Fleitmann.) Tnmetaphosphonc acid, H 3 P 3 O 9 . Sol. in H 2 O; the solution is permanent in the cold, but on evaporation it is quickly de- comp. to H 3 PO 4 . Tetrametaphosphonc acid, H 4 P 4 Oi 2 . Not isolated. Hexametaphosphoric acid, H 6 P 6 Oi 8 . (Glacial phosphoric acid.) Deliquescent; easily sol. in H 2 O with evolu- tion of heat and conversion into H 3 PO 4 . Not easily sol. in presence of slight impurities. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Or#w>phosphoric acid, H 3 PO 4 . Very sol. in H 2 O. 100 pts. of the solution contain at: 26.23 27.02 29.42 29.77 95.9 95.98 96.15 96.11 pts. H 3 PO 4 , 37.65 39.35 42.30 (mpt.) 97.8 98.48 100 pts. H 3 PO 4 . (Smith and Menzies, J. Am. Chem. Soc. 1909, 31. 1186.) See also 10H 3 PO 4 +H 2 O, and 2H 3 P0 4 + H 2 O. Sp. gr. of H 3 PO 4 +Aq containing: 10 20 30 40 50 %P 2 O 5 . 1.1 1.23 1.39 -1.6 1.85 (Dalton.) PHOSPHORIC ACID 673 Sp. gr. of H 3 PO 4 +Aq. Sp.gr. of H 3 PO 4 + Aq at 17 . 5. Sp.gr. % P=0 5 Sp. gr. % P 2 6 Sp. gr. % P 2 5 & Sp. gr. % P 2 6 Sp. gr. A Sp. gr. 1.508 1.492 1.476 1.464 1.453 .442 .434 .426 .418 .401 1.392 1.384 1.376 1.369 1.356 1.347 1.339 49.60 48.41 47.10 45.63 45.38 44.13 43.95 43.28 42.61 41.60 40.86 40.12 39.66 39.21 38.00 37.37 36.74 .328 .315 .302 .293 .285 .276 .268 .257 1.247 1.236 1.226 1.211 1.197 1.185 1.173 1.162 1.153 36.15 1.144 34.82 1.136 33.49 1.124 32.71 1.113 31.94 1.109 31.03 1.095 30.13 1.081 29.16 1.073 28.24 1.066 27.30 1.056 26.36 1.047 24.79 1.031 23.23 1.022 22.07 1.014 20.91 1.006 19.73 18.81 17.89 16.95 15.64 14.33 13.25 12.18 10.44 9.53 8.62 7.39 6.17 4.15 3.03 1.91 0.79 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 1.007 1.014 1.021 1.028 1.036 1.044 1.053 1.061 1.070 1.078 1.086 1.095 1.103 1.112 1.120 1.129 1.139 1.148 1.158 1.168 1.178 1.188 1.198 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 1.208 1.219 1.229 1.240 1.250 1.261 1.272 1.282 1.293 1.304 1.315 1.326 .338 .350 .362 .374 .386 .398 1.410 1.423 1.436 1.448 1.462 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 1.476 1,491 1.505 1.521 1.536 1.551 1.566 1.581 1.597 1.613 1.629 1.645 1.661 1.677 1.693 1.709 1.725 1.741 1.758 1.775 1.792 1.809 (Watts, C. N. 12. 160.) Specific gravity of H 3 PO 4 +Aq containing: 6 12 18 %H 3 P0 4 , 1.0333 1.0388 1.1065 24 36 54 %H 3 PO 4 . 1.1463 1.2338 1.3840 (Schiff, A. 113. 183.) Sp. gr. of H 3 PO 4 +Aq at 15. a= sp. gr. if % is P 2 O 5 ; b=sp. gr. if % is H 3 PO 4 . (Hager, Adjumenta varia, Leipzig, 1876.) Table for correction to be added or subtracted for 1 change in temperature. % 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 a b % a b % P 2 O 6 Corr. % P 2 O 5 Corr. 1:009 1.017 1.025 1.032 1.039 1.047 1.055 1.063 1.071 1.080 1.089 1.098 1.106 1.115 1.124 1.133 1.142 .151 .161 .171 .182 .192 1.202 1.212 1.223 1.233 1.244 1.254 1.265 1.277 1.0054 1.0109 1.0164 1.0220 1.0276 1.0333 1.0390 1.0449 1.0508 1.0567 1.0627 1.0688 1.0749 1.0811 1.0874 1.0937 1.1001 1.1065 .1130 .1196 .1262 .1329 .1397 1.1465 1.1534 1 . 1604 1 . 1674 1.1745 1.1817 1.1889 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 1.288 1.299 1.310 1.321 1.333 1.345 1.357 1.369 1.381 1.393 1.407 1.420 1.432 1.445 1.1962 1.2036 1.2111 1.2186 1.2262 1.2338 1.2415 1.2493 1.2572 1.2651 1.2731 1.2812 1.2894 1.2976 1.3059 1.3143 1.3227 1.3313 1.3399 1.3486 1.3573 1.3661 1.3750 1.3840 1.3931 1.4022 1.4114 1.4207 1.4301 1.4395 10-14 0.00035 15-25 0.0004 26-35 0.00052 36-45 0.00068 46-55 0.00082 56-68 0.001 (Hager.) Sp. gr. of H 3 PO 4 +Aq. G.-equivalents HsPO 4 per litre t Sp. gr. t/t 0.002572 0.005142 0.01025 0.02042 0.03056 0.04065 j.,-507 0.10046 0.19951 0.29716 0.49057 0.5070 5.0700 17.714 17.706 17.685 17.683 17.687 17.704 17.663 17.696 17.749 17.701 17.719 17.58 17.84 1.001552 1.0003051 1.000595 1.001158 1.001708 1.002252 1.002790 1.005412 1.010560 1.015584 1.025469 1.02627 1.25162 (Kohlrausch, W. Ann. 1894, 63. 29.) Miscible with cone. HC 2 H 3 O 2 +Aq. Sol. in 30 pts. warm creosote. 1 cc. of a sat. solution of ether in H 2 O dis- solves 0.0886 grams H 3 PO 4 . (Schiff, calculated by Gerlach, Z. anal. 8. 292.) 674 PHOSPHORIC ACID 1 cc. of a sat. solution of H 2 O in ether dis- solves 0.000033 grams H 3 PO 4 . Solutions of H 3 PO 4 in H 2 O containing less than 0.434 grams.acid per 1 cc. lose an insig- nificant amount of acid to ether when agi- tated therewith. (Berthelot, C. R. 1896, 123. 345.) The composition of the hydrates formed by H 3 PO 4 at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by H 3 PO 4 and of the conductivity and sp. gr. of H 3 PO 4 +Aq. (Jones, Am. Ch. J. 1905, 34. 331.) 10H 3 PO 4 +H 2 O. Solubility in H 2 O. 100 pts. of the solution contain at: 24.11 24.38 24.40 94.78 94.80 94.84 pts. H 3 P0 4 , 24.81 25.41 25.85 94.95 95.26 95.54 pts. H 3 PO 4 . (Smith and Menzies, J. Am. Chem. Soc. 1909, 31. 1186.) 2H 3 PO 4 +H 2 O. Solubility in H 2 O. 100 pts. of the solution contain at: 16.3 0.5 14.95 24.03 27.0 76.7 78.7 81.7 85.7 87.7 pts. H 3 P0 4 , 28.5 C 92.5 29.15 29.35 (mpt.) 90.5 91.6 pts. H 3 P0 4 , 27.0 25.41 93.4 94.1 pts. H 3 PO 4 . Retroflex part of curve. (Smith and Menzies, J. Am. Chem. Soc. 1909, 31. 1186.) Pwrophosphoric acid (Diphosphoric acid), H 4 P 2 7 . Very sol. in H 2 O. The solution may be kept without change, but on heating it is converted into H 3 PO 4 . The acid in solution gradually changes to H 3 PO 4 ; the conversion being more rapid with more concentrated solutions. (Montemartini and Egidi, Gazz. ch. it. 1902, 32. (1) 381.) Phosphoric acid, H 8 P 2 O 9 (?). Sol. in H 2 O. (Joly, C. R. 100. 447.) Phosphates. The phosphates of NH 4 , K, Na, Li, Cs, and Rb are sol. in H 2 O, with the exception of certain metaphosphates; the other phosphates excepting neutral Tl salts, are nearly insol. in H 2 0, excepting when an excess of H 3 PO 4 is present. The latter are all sol. in HNO 3 +Aq. (a) Metaphosphates. Monometaphosphates. Only alkali mono- metaphosphates are known, and they are all insol. in H 2 0. 1 Dimetaphosphates. Alkali dimetaphos- phates and some doublt salts containing an alkali as one of the bases are sol. in H 2 O, the rest are si. sol. or insol. in H 2 O. Tn'metaphosphates. All salts are sol. in H 2 0. Teirametaphosphates. The alkali salts are sol. in H 2 O, the others are insol. #e:rametaphosphates. The alkali salts are sol., the others insol., in H 2 O, but are mostly sol. in Na hexametaphosphate+Aq. (6) Orthophosphates. K, Na, Li, Cs, and Rb orthophosphates are sol. in H 2 O. All the others are insol. in H 2 O, but sol. in excess of H 3 PO 4 , and HNO 3 +Aq; less easily sol. in HC 2 H 3 O 2 +Aq. Pb, Al, and Fe 2 phosphates are insol. in HC 2 H 3 O 2 +Aq. SI. sol. in NH 4 salts +Aq, especially NH 4 Cl+Aq, from which solution they are pptd. by NH 4 OH+Aq. Orthophosphates insol. in H 2 O are also insol. in an excess of alkali orthophosphates +Aq. All orthophosphates are insol., or very si. sol. in alcohol. (c) Pyrophosphates. Alkali pyrophos- phates are sol. in H 2 O; the others are insol. in H 2 O, but are mostly sol. in an excess of Na pyrophosphate + Aq . Aluminum metophosphate, A1 2 (PO 3 ) 6 . Insol. in H 2 O and cone, acids. (Maddrell, A. 61. 59.) Aluminum or^ophosphate, basic. 3A1 2 3 . P 2 5 + 18H 2 0. Min. Evansite. 4A1 2 O 3 , 3P 2 O 5 + 18H 2 O. Ppt. Insol. in H 2 O. (Rammelsberg.) 2A1 2 3 , P 2 5 . +3H 2 O. Min. Angelite. +5H 2 O. Min. Kalaite (Turquoise). Sol. in HCl+Aq. +6H 2 O. Decomp. by H 2 O. (Hautefeuille, J. pr. (2) 37. 111.) Min. Peganite. More or less sol. in HC1, and HNO 3 +Aq. +8H 2 O. Ppt. (Munroe, A. 159. 278.) Min. Fischerite. SI. attacked -by HC1 or HNO 3 +Aq; sol. in H 2 SO 4 +Aq. 3A1 2 O 3 , 2P 2 O 5 +8H 2 O, or 12H 2 O. Sol. in acids, even after ignition. (Millot, C. R. 82. 89.) +10H 2 O. Min. Caeruleolactite. Sol. in acids. + 12H 2 O. Min. Wavellite. Aluminum or^ophosphate, A1 2 (PO 4 ) 2 . Crystalline. Not attacked by cone. HC1 or HNO 3 +Aq, difficultly by hot cone. H 2 SO 4 . (de Schulten, C. R. 98. 1583.) Ignited A1 2 (PO 4 ) 2 is si. decomp. by H 2 O, so that solubility determinations are variable. For an extended discussion, see original paper. (Cameron and Hurst, 1904, 26. 898.) PHOSPHATE, AMMONIUM 675 +4H 2 O. Easily sol. in mineral acids, inso in acetic and other organic acids. Easil sol. in KOH+Aq, but is reprecipitated fr NH 4 Cl+Aq. Sol. in NH 4 OH+Aq. Sol. ii a large amount of alum+Aq (Rose), in aluminum acetate and other aluminum salt +Aq (Fleischer, Z. anal. 6. 28). More so than ferric phosphate in ammonium oxalat< or citrate +Aq. (Millot.) Acid I\H 4 citrate +Aq dissolves 3% of the P 2 O 5 ; neutral NH 4 citrate +Aq dissolves 6.6 of the P 2 O 5 ; ammoniacal NH 4 citrate + A. dissolves completely in 25 min. (Erlenmeyer B. 14. 1869.) Sol. in NH 4 OH+Aq, especially in presence of alkali phosphates, (de Koninck, Z. anal 23. 90.) Not pptd. in presence of alkali tartrates o: citrates, sugar, glycerine, etc. Insol. in ethyl acetate. (Naumann, B 1910, 43. 314.) Min. Variscite. Very quickly sol. in warm cone. HCl+Aq. +5H 2 O. Min. Zepharovitchite. +8H 2 O. Min. Gibbsite. Aluminum or^/iophosphate. acid, 2A1 2 O 3 , 3P 2 5 + 16H 2 0. Insol. in acids after being ignited. (Millot Bull. Soc. (2) 22. 244.) +4H 2 O, and 6H 2 O. Insol. in H 2 O or alco- hol. (Hautefeuille and Margottet, J. pr. (2) A1 2 O 3 ', 2P 2 O 5 +8H 2 q. Insol. in acids or aqua regia after being ignited. (Millot.) 2A1 2 O 3 , 5P 2 O 5 -{-14H 2 O. Decomp. by cold H 2 O into 4A1 2 O 3 , 7P 2 O 5 +9H 2 O. Decomp. by hot H 2 O. (Erlenmeyer, A. 194. 200.) A1 2 O 3 , 3P 2 O 5 +3H 2 O=A1 2 (H 2 PO 4 ) 6 . Deli- quescent; completely sol. in a little cold H 2 O, and cone, solution can be boiled without decomp., but dil. solution (1 : 20) separates A1 2 (PO 4 ) 2 on boiling, which redissolves on cooling, the more quickly the more dilute the original solution. (Erlenmeyer, A. 194. 198.) Aluminum pyrophosph&te, A1 4 (T 2 O 7 ) 3 + 10H 2 O. Precipitate. Sol. in mineral acids, and Na 4 P 2 O 7 +Aq; insol. in acetic acid. Sol. in KOH+Aq; sol. in NH 4 OH+Aq, but when dissolved in HCl+Aq is reprecipitated by NH 4 OH+Aq, and is not redissolved in an excess thereof. (Schwarzenberg, A. 65. 147.) Sol. in alum+Aq. (Rose, Pogg. 76. 19.) Aluminum pz/roraetaphosphate, A1 2 O 3 , 2P 2 O 5 . (Hautefeuille and Margottet, C. R. 96. 849.) Aluminum ammonium dihydrogen orthophos- phate, NH 4 H 2 PO 4 , A1PO 4 . Partially decomp. by H 2 O. Sol. in acids and alkalies. Nearly insol. in 50% acetic acid. (Cohen, J. Am. Chem. Soc. 1907, 29. 720.) Aluminum calcium phosphate, A1 2 O 3 , 3CaO, P 2 5 +3H 2 0. Min. Tavistockite. 2A1 2 O 3 , 6CaO, 3P 2 O 5 +3H 2 O. Min. Kirro- lite. Aluminum calcium phosphate sulphate, 3A1 2 O 3 , SO 3 , Ca 3 (PO 4 ) 2 +6H 2 O. Min. Svanbergite. Scarcely attacked by HCl+Aq, and only si. by H 2 SO 4 +Aq. Aluminum ferrous magnesium phosphate. (Mg, Fe),Al 2 P 2 10 +4H 2 0. Min. Childrenite. Slowly sol. in HCl+Aq. Min. Eosphorite. Sol. in HNO 3 or HC1 + Aq. (Mg, Fe)Al 2 P 2 O 9 +H 2 O. Min. Lazulite. Only si. attacked by acids, when not pre- viously ignited. Aluminum lithium phosphate, A1->(PO 4 ) 2 , 4Li 3 PO 4 +30H 2 O. Precipitate. (Berzelius.) Insol. in H 2 O; easily sol. in acids. Aluminum magnesium phosphate. Min. Lazulite. See Phosphate, aluminum ferrous mag- nesium. Aluminum potassium phosphate, A1 2 O 3 , K 2 O, 2P 2 5 . Insol. in acids. (Ouvrard, A. ch. (6) 16. 289.) 2A1 2 O 3 , 2K 2 O, 3P 2 O 5 . (Ouvrard.) Aluminum silver raetophosphate, 2A1 2 O 8 , Ag 2 0, 4P 2 5 . (Hautefeuille and Margottet, C. R. 96. 849, 1142.) Aluminum sodium pT/rophosphate, Al 2 Na 2 (P 2 O 7 )2. Insol. in H 2 O and acids. (Wallroth.) Nearly insol. in acids. (Ouvrard. A. ch. 6) 16. 338.) 2A1 2 O 3 , 3Na 2 O, 3P 2 O 6 . Sol. in HNO 3 +Aq. Ouvrard.) A1 4 (P 2 O 7 ) 3 , 2Na 4 P 2 O 7 +30HoO. Very difficultly sol. in H 2 O. (Pahl, Bull. Soc, (2) 22. 122.) iluminum phosphate lithium fluoride, 2A1 2 (PO 4 ) 2 , 3LiF. Min. Amblygonite. SI. attacked by HC1+ ^.q, more easily by H 2 SO 4 +Aq. Ammonium wetophosphate, NH 4 PO 3 . Insol. in H 2 O. (Fleitmann, Pogg. 78. 345.) Ammonium dimetaphosphsde, (NH 4 )2(PO 8 ) 2 . Sol. in 1.15 pts. cold or hot H 2 O. (Fleit- mann, Pogg. 78. 245.) More sol. in dil. Icohol than Na or K salt. 676 PHOSPHATE, AMMONIUM Sol. in 0.9 pts. H 2 O; easily sol. in acids pecially by boiling (Glatzel, Dissert. 1880.) . . . . especially by boiling with cone. H 2 SO4. (Gla Ammonium trimetaphosphate, (NH 4 ) 3 P 3 O9. Very sol. in H 2 O. (Lindbom, Acta Lund. 1873. 15.) Ammonium tetrametaphosphate, (NH 4 ) 4 P 4 12 . Sol. in H 2 O. (Warschauer, Z. anorg. 1903, 36. 177.) +4H 2 O. Much more sol. in H 2 O than the K or Na salt. 1 pt. is sol. in 8 pts. H 2 O. (Glatzel, Dissert. 1880.) Ammonium pentametaphosphate, (NH 4 ) 5 P 5 15 . Sol. in H 2 O. (Tammann, J. pr. 1892, (2) 46. 455.) Ammonium dekametaphosphate, (NH 4 ) 10 P 10 3 o. Very si. sol. in H 2 O; 100 g. H 2 O dissolved 1.20-1.54 g. in 2 months. Easily sol. in hot H 2 O with decomp. (Tammann, J. pr. 1892, (2) 45. 448.) + 12H 2 O. (Tammann, J. pr. 1892, (2) 45. 100 g. H 2 O dissolve 131 g. at 15; sp. gr. of sat. solution = 1.343. (Greenish and Smith, Pharm. J. 1901, 66. 774.) Solubility in H 3 PO 4 +Aq at 25. In 1000 g. of the solution, mols. NH 4 P0 4 6.42 3.23 6.46 3.74 6.56 4.01 6.78 4.34 7.26 4.83 7.16 4.82 (D'Ans and Schreiner, Z. phys. Ch. 1910, 75. 105.) Insol. in acetone. (Eidmann, C. C. 1899. II, 1014; Naumann, B. 1904, 37. 4329.) Ammomum ^hydrogen NH 4 H 2 PO 4 . Does not effloresce. Less easily sol. in H 2 O than (NH 4 ) 2 HPO 4 . (Mitscherlich, A. ch. 19. 385.) Sol. in 5 pts. cold, and less hot H 2 O. Solubility in H 8 PO 4 +Aq at 25. 100.; Ammomum or^ophosphate, (NH 4 ) 3 PO 4 + 3H 2 O. Difficultly sol. in H 2 O. Less sol. in H 2 O than (NH 4 ) 2 HPO 4 . (Ber- zelius.) Insol. in alkalies +Aq. (Berzelius.) SI. sol. in H 2 O. Decomp. in the air. (Schottlander, Z. anorg. 1894, 7. 344.) Solubility in H 8 PO 4 +Aq at 25. In 1000 g. of the solution, mols. NH 4 P0 4 6.72 5.62 4.62 2.72 2.50 2.58 2.76 3.06 3.10 4.54 3.88 3.36 . 2.59 2.54 4.29 6.21 7.70 7.86 In 1000 g. of the solution, mols. (D'Ans and Schreiner, Z. phys. Ch. 1910, 75. 106.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Ammonium o?-///ophosphate, acid. Decomp. into NH 4 H 2 PO 4 at 77-78. (Parravano and Mieli, Gazz. ch. it. 1908, 38, II. 536.) NH 4 PO4 7.42 5.02 2.95 3.04 3.32 4.78 0.084 0.20 0.46 1.02 1.32 2.32 ("TV Ann and Sn.hrpinpr 7 nhvs C!h 1Q10 75. 105.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) +5H 2 O. (Sestini, Gazz. ch. it. 9. 298.) Ammonium hydrogen or^ophosphate, (NH 4 ) 2 HP0 4 . Easily sol. in H 2 O. Effloresces to form NH 4 H 2 PO 4 . (Schiff, A. 112. 88.) Sol. in 4 pts. cold, and less hot H 2 O. Solu- tion loses NH 3 by boiling. Insol. in alcohol. Ammonium p?/r0phosphate, (NH 4 ) 4 P 2 O 7 . Easily sol. in H 2 O. Alcohol precipitates it from the aqueous solution. (Schwarzenberg, A. 65. 141.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Ammonium hydrogen p?/rophosphate (NH 4 ) 2 H 2 P 2 7 . Very sol. in H 2 O. Insol. in alcohol. (Schwarzenberg, A. 65. 141.) PHOSPHATE, AMMONIUM MAGNESIUM 677 Ammonium barium trimetaphospha.te, (NH 4 )BaP 3 O 9 +H 2 O. Easily sol. in H 2 O. (Lindbom.) Ammonium cadmium cfo'raetaphosphate, (NH 4 ) 2 O, CdO, 2P 2 O 5 +3H 2 O = (NH 4 ) 2 Cd(P 2 O G ) 2 . Efflorescent. (Fleitmann, Pogg. 78. 347.) Ammonium cadmium orZ/iophosphate, NH 4 CdPO 4 +li/4H 2 O. Easily sol. in NH 4 OH+Aq and acids. (Drewson, Gm. K. Handb. 6te Aufi. III. 74.) Ammonium calcium dimetaphosphaie, (NH 4 ) 2 Ca(P 2 O 6 ) 2 -f2H 2 O. Very si. sol. in H 2 O. Not decomp. by acids. (Fleitmann, Pogg. 78. 344.) Ammonium calcium phosphate, !SH 4 CaPO 4 + Ppt. (Herzfeld and Feuerlein, Z. anal. 20. 191.) -j-7H 2 O. Not completely decomp. by cold H 2 O in y\ hour; rapidly by hot H 2 O. (Lasne, Bull. Soc. 1902, (3) 17. 131.) Ammonium chromium or^ophosphate, basic, 5(NH 4 )H 2 PO 4 , 2CrPO 4 , 4Cr(OH) 3 . (Cohen, J. Am. Chem. Soc. 1907, 29. 1196.) (NH 4 ) 2 HPO 4 , 2CrPO 4 +3H 2 O. Ppt. (Cohen.) Ammonium chromic pyro phosphate, NH 4 fCrP 2 7 )+6H 2 0. SI. sol. in cold H 2 O. Decomp. by boiling H 2 O. (Rosenheim, B. 1915, 48. 586.) Ammonium cobaltous wefaphosphate. Extremely sol. in H 2 O and in NH 4 OH+Aq. (Persoz, J. pr. 3. 215.) Ammonium cobaltous or^Aophosphate, NH 4 CoPO 4 +H,O. Not decomp. by boiling H 2 O. (Debray, J. Pharm. (3) 46. 121.) + 12H 2 O. Ppt. (Chancel, 1862.) Co(NH 4 ) 2 H 2 (PO 4 ) 2 +4H 2 O. Insol. in H 2 O. (Debray.) Ammonium copper cfo' (NH 4 ) 2 P 2 6 , CuP 2 O c +2H 2 O. Very si. sol. in H 2 O; insol. in alcohol. (Fleitmann, Pogg. 78. 345.) +4H 2 O. Efflorescent. Very si. sol. in H 2 O; insol. in alcohol. (F.) Sol. in 50 pts. H 2 O. Slowly attacked by acids. Only boiling H 2 SO 4 attacks easily. (Glatzel, Dissert. 1880.) Ammonium glucinum orZ/iophosphate, NH 4 G1PO 4 . Insol. in cold, si. sol. in hot H 2 O. (Rossler, Z. anal. 17. 148.) Ammonium glucinum sodium orZ/iophosphate, (NH 4 ) 2 GlNa 2 (PO 4 ) 2 +7H 2 O. (Scheffer, A. 109. 146.) Ammonium iron (ferrous) ort/iophosphate, NH 4 FePO 4 +H 2 O. Insol. even in boiling H 2 O. When still moist, easily sol. in dil. acids, but sparingly and slowly sol. after drying, even in cone, acids. Decomp. by NH 4 OH, KOH, and NaOH+Aq. Insol. in alcohol. (Otto, J. pr. 2. 409.) (NH 4 ) 2 FeH 2 (PO 4 ) 2 +4H 2 O. (Debray.) Ammonium iron (ferric) hydrogen orthophos- phate, basic, 2(NH 4 ) 2 HPO 4 , 3FePO 4 , 3Fe(OH) 3 . Ppt. Insol. in 95% alcohol. (Cohen, J. Am. Chem. Soc. 1907, 29. 719.) Ammonium iron (ferric) hydrogen orthophos- phate, NH 4 H 2 Fe(PO 4 ) 2 . Ppt. Same properties as Na salt. (Wein- land, Z. anorg. 1913, 84. 356.) Partially hydrolyzed by H 2 O. Readily sol. in HC1, HNO 3 , H 2 S0 4 and H 3 PO 4 . Partially hydrolyzed by cold NH 4 OH+Aq. Sol. in excess of hot NH 4 OH+Aq. Completely hydrolyzed by caustic alkalies. Practically insol. in 50% acetic acid. (Cohen, J. Am. Chem. Soc. 1907, 29. 718.) Ammonium lead cfo'raeZaphosphate, (NH 4 ) 2 Pb(P 2 6 ) 2 . Very difficultly sol. in H 2 O and acids. (Fleitmann, Pogg. 78. 343.) Ammonium lithium metophosphate, Li 2 O, 2(NH 4 ) 2 O, 3P 2 O 5 +8H 2 O. Not appreciably sol. in cold H 2 O but rapidly and abundantly sol. in H 2 O at 70. (Tammann, J. pr. 1892, (2) 45. 442. ) Ammonium lithium phosphate, (NH 4 ) 2 LiPO 4 . SI. sol. in H 2 O. (Berzelius.) Ammonium magnesium wetaphosphate, (NH 4 ) 2 0, 2MgO, 2P 2 5 +9H 2 (?). Sol. with difficulty in H 2 O or acids when heated. Easily sol. in H 2 O before heating. (Wach, Schw. J. 59. 29.) Precipitated from aqueous solution by alcohol. Ammonium magnesium cfo'w-etaphosphate, (NH 4 ) 2 Mg(P 2 6 ) 2 +6H 2 0. Efflorescent. (Fleitmann, Pogg. 78. 346.) Ammonium magnesium phosphate, NH 4 MgPO 4 , and +6H 2 O. 1 1. H 2 O. dissolves 66 mg. anhj^drous NH 4 MgPO 4 at 15. (Fresenius, A. 55. 109.) 1 1. H 2 O dissolves 74.1 mg. anhydrous NH 4 MgPO 4 at 20.5-22.5. (Ebermayer.) 678 PHOSPHATE, AMMONIUM MAGNESIUM HYDROGEN 1 1. H 2 O dissolves 106 mg. anhydrous NH 4 MgPO 4 . (Liebig.) Insol. in H 2 O, but when boiled with H 2 O it loses NH 3 and H 2 O. (Struve, Z. anal. 1898, 37. 485.) Solubility of NH 4 MgPO 4 +6H 2 O in H 2 O at t. t G. salt in 100 g. H 2 O 20 40 50 60 70 80 0.0231 0.0516 0.0359 0.0303 0.0401 0.0163 0.0195 (Wenger, Dissert. Geneva, 1911.) Aqueous solution is precipitated by NH 4 OH, but not by Na 2 HPO 4 +Aq. (Fre- senius.) Sol. in 44,600 pts. H 2 O containing am- monia. More sol. in H 2 O containing NH 4 C1, and is sol. in 7548 pts. of a solution containing 1 pt. NH 4 C1 to 5 pts. H 2 O and ammonia, and in 15,627 pts. of a solution containing 1 pt. of NH 4 C1 to 7 pts. H 2 O and ammonia. (Fre- senius.) According to Kremers (J. pr. 65. 190), a solution of 3 pts. H 2 O to 1 pt. NH 4 OH+Aq of 0.96 sp. gr. is best suited for washing the precipitated NH 4 MgPO 4 . According to Ebermayer (J. pr. 60. 41), 1 pt. anhydrous salt is sol. in 13,497 pts. H 2 O at 23; in 31,098 pts. NH 4 OH+Aq (4 pts. H 2 O: 1 pt. NH 4 OH+Aq of 0.961 sp. gr.) at 21.25; in 36,764 pts. NH 4 OH+Aq (3 pts. H 2 O: 1 pt. NH 4 OH+Aq) at 20.6; in 43,089 pts. NH 4 OH+Aq (1 pt, H 2 O: 1 pt. NH 4 OH + Aq) at 22.5; in 45,206 pts. NH 4 OH+Aq (1 pt. H 2 O: 2 pts. NH 4 OH+Aq) at 22.5; in 52,412 pts. NH 4 OH+Aq (1 pt. H 2 O: 3 pts. NH 4 OH+Aq) at 22.5; in 60,883 pts. pure NH 4 OH+Aq (sp. gr. 0.961) at 22.5. Almost absolutely insol. in H 2 O containing K vol. NH 4 OH+Aq (sp. gr. 0.96) and NH 4 C1, i.e., much more insol. than given by Fresenius. (Kubel, Z. anal. 8. 125.) According to Kissel (Z. anal. 8. 173), 1 1. NH 4 OH+Aq (3 pts. H 2 O: 1 pt. NH 4 OH+Aq of 0.96 sp. gr.) dissolves 4.98 mg. in 24 hours, while 13.9 mg. are dissolved if 18 g. NH 4 C1 to a litre of H 2 O are also present. (NH 4 ) 2 SO 4 +Aq containing 2.2 g. per litre dissolves 71.7 mg.; 3.0 g., 113 mg.; 10 g., 147 mg.; NaCl+Aq containing 2 g. NaCl per 1. dissolves 123.4 mg.; NaNO 3 -j-Aq containing 3 g. NaNO 3 per 1. dissolves 93.1 mg. (Liebig, A. 106. 196.) Completely insol. in water containing am- monium phosphate or ammonium sodium phosphate. (Berzelius.) 800 com. H 2 O, sat. with CO 2 , dissolve 1.425 g. (Liebig.) Easily sol. in H 2 SO 3 +Aq, acetic and other acids, also in boiling solution of ammonium citrate. (Millot, Bull. Soc. (2) 18. 20.) When in presence of Fe or Al salts it is sol. to a considerable extent in H 2 C 4 H 4 06+Aq. 6 g. NH 4 C1 in 100 ccm. H 2 O containing 10 ccm. 6.34% NH 4 OH+Aq dissolve pptd. salt = 0.0029 g. Mg 2 P 2 O 7 . 1 g. (NH 4 ) 2 C 2 O 4 in 100 ccm. H 2 O, and NH 4 OH+Aq dissolve = 0.0061 g. Mg 2 P 2 O 7 . 2 g. citric acid in excess of NH 4 OH+Aq dissolve = 0.0147 g. Mg 2 P 2 O 7 . Solubility prevented by excess of magnesia mixture. (Lindo, C. N. 48. 217.) Solubility of NH 4 MgPO 4 +6H 2 O in salts+Aq at t. (G. salt dissolved in 100 g. solvent.) t 5% NH 4 N0 3 +Aq. 5% NH 4 Cl+Aq. 1 pt. NH 4 OH (D =0.96) +4 pts. EhO 0.1100 0.0597 0.0087 20 0.0463 0.1055 0.0098 30 0.0546 0.1133 40 0.0645 0.0713 0.6135 50 0.0723 0.0931 0.0153 60 0.0846 0.1728 0.0174 70 0.0834 0.1239 0.0178 80 0.1009 0.1913 0.0145 t 4% NH 4 OH+Aq and 5%NH 4 Cl+Aq. 4% NH 4 OH +Aq and 10% NH 4 Cl+Aq. 20 60 0.0165 0.0274 0.0541 0.0731 (Wenger, Dissert. Geneva, 1911.) About 3 times as sol. in a(C 2 H 3 2 ) 2 +Aq as in NaC 2 H 3 O 2 +Aq, but solubility is pre- vented by excess of MgCl 2 . (Ville, Bull. Soc. (2) 18. 316. SI. sol. in ammonium citrate +Aq contain- ing 400 g. ammonium citrate in a litre. Solubility = 0.457% at ord. temp, and 0.58% at 50. (Bolis, Ch. Z. 1903, 27. 1151.) Min. Struvite. +HoO. Insol. in H 2 O or citric acid+Aq. (Millot and Maquenne, Bull. Soc. (2) 23. 238.) Ammonium magnesium hydrogen orthophos- phate, (NH 4 ) 2 MgH 2 (P0 4 ) 2 +3H 2 (?). (Graham.) Ammonium magnesium phosphate, 5MgO, (NH 4 ) 2 O, 2P 2 O 5 +24H 2 O. (Gawalovsky, C. C, 1885. 721.) Ammonium magnesium sodium pyrophos- phate, fNH 4 ) 3 Mg 6 Na(P 2 7 ) 4 . Insol in H 2 O and not decomp. thereby. (Berthelot and Andre", A. ch. 1897, (7) 11. 186.) PHOSPHATE, AMMONIUM SODIUM 679 Ammonium manganous c^wetaphosphate, (NH 4 ) 2 Mn(PO 8 ) 4 +4H 2 O. Relatively easily attacked by acids. (Glat- zel, Dissert! 1880.) +6H 2 0. Efflorescent. (Fleitmann, Pogg. 78. 346.) Ammonium manganous or^ophosphate, NH 4 MnPO 4 +H 2 O. Sol. in 32,092 pts. cold, and 20,122 pts. boiling H 2 O, and in 17,755 pts. NH 4 Cl+Aq (1.4% NH 4 C1). (Fresenius.) +7H 2 O. Insol. in H 2 O below 70; at 70 100 g. H 2 O dissolve 0.0052 g. salt; at 80, 0.0067. (Wenger, Dissert. Geneva, 1911.) Easily sol. in dil. acids. Decomp. by KOH+Aq, but not by NH 4 OH+Aq or K 2 CO 3 +Aq. Insol. in NH 4 OH or NH 4 salts +Aq. (Gibbs.) Solubility in salts +Aq at t. (G. in 100 g. solvent.) t 5% NH 4 NO +Aq. 5% NH4Cl+Aq. 1 pt. NH 4 OH D =0.96 +4 pts. H 2 O. 0.0206 0.0020 0.0116 20 0.0200 0.0255 0.0122 30 0.0226 0.0345 40 0.0209 0.0386 0.0118 50 0.0226 0.0355 0.0132 60 0.0270 0.0384 0.0193 70 0.0281 0.0414 0.0191 80 0.0326 0.0451 0.0197 (Wenger, L c.) Insol. in alcohol. Insol. in acetone. (Naumann. B. 1904, 37. 4329.) Ammonium manganic pyrophosphate. NH 4 MnP 2 O 7 +3H 2 O. Decomp. bv cold H 2 O with separation of Mn 2 O 3 . (Rosenheim, B. 1915, 48. 584.) Ammonium manganous sodium pyrophos- phate, NH 4 NaMnP 2 O 7 +3H 2 O. Insol. in H 2 O or alcohol. Easily sol. in very dil. acids. (Otto, J. pr. 2. 418.) formula is Na 4 (NH 4 ) 4 Mn 2 (P 2 O 7 ) 3 + 12H 2 O, according to Berzelius. Ammonium mercuric metaphosphate. Sol. in H 2 O, or at least in NH 4 OH+Aq. (Persoz, J. pr. 3. 216.) Ammonium nickel metaphosphate. Insol. in H 2 O. Sol. in NH 4 OH+Aq, from which it is repptd. on evaporation of the NH 3 . (Persoz, J. pr. 3. 215.) Ammonium nickel dimetaphosphate, (NH 4 ) 2 NiP 4 12 +4H 2 0. Sol. in 12.5 pts. H 2 O. (Glatzel, Dissert. 1880.) Ammonium nickel or^ophosphate, NH 4 NiPO 4 +2H 2 O. Ppt. (Debray, C. R. 69. 40.) +6H 2 O. Decomp. by boiling H 2 O. (De- bray.) Ammonium potassium dimetaphosphate, (NH 4 )ioK<(P,0,)7. More sol. in H 2 O than following salt. (Fleitmann, Pogg. 78. 341.) NH 4 K 3 P 4 O 12 +2H 2 O. Difficultly sol. in H 2 O. (Fleitmann.) Ammonium potassium pz/rophosphate, Deliquescent. Sol. in H 2 O. Decomp. on boiling. (Schwarzenberg.) Ammonium sodium dimeiaphosphatej NH 4 NaP 2 O 6 +H 2 O. More sol. in H 2 O than Na 2 P 2 O 6 , but less than (NH 4 ) 2 P a Oe. Less sol. in alcohol than in H 2 O. (Fleitmann, Pogg. 78. 340.) Ammonium sodium ori/iophosphate, (NH 4 ) 2 NaPO 4 +4H 2 O. Decomp. by H 2 O. Cryst. from NH 4 OH + Aq of 0.96 sp. gr. From H 2 O solution, NaNH 4 HPO 4 +4H,O separates out. (Uels- mann, Arch. Pharm. (2) 99. 138.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +5H 2 O. NH 4 Na 2 PO 4 +12H 2 O. (Herzfeld, Z. anal. 20. 191.) (NH 4 ) 5 Na(PO 4 ) 2 +6H 2 O. Sol. in H 2 O with decomp. Cryst. from hot cone. NH 4 OH+Aq. (Uelsmann, Arch. Pharm. (2) 99. 138.) Ammonium sodium hydrogen phosphate (Mi- crocosmic salt), NH 4 NaHPO 4 +4H 2 O. Efflorescent. Easily sol. in H 2 O. Sol. in 6 pts. cold, and 1 pt. boiling H 2 O. Insol. in alcohol. Aqueous' solution gives off NH 3 , especially if hot. Insol. in acetone. (Eidmami, C. C. 1899, II. 1014.) Min. Stercorite. +5H 2 O. (Uelsmann.) The composition of the hydrates formed by this salt at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by the salt and of the con- ductivity and sp. gr. of its aqueous solutions. (Jones, Am. Ch. J. 1905, 34. 319.) (NH 4 ) 3 Na 3 H 6 (PO 4 ) 4 +3H 2 O. Decomp. by H 2 0. (Filjiol and Sendereng, C. R. 93. 388.) Ammonium sodium p^/rophosphate, (NH 4 ) 2 Na 2 P 2 O 7 +5H 2 O. Easily sol. in H 2 O. Aqueous solution de- comp. fcy boiling. (Schwarzenberg, A. 65. 142.) +6H 2 O. (Rammelsberg.) 680 PHOSPHATE, AMMONIUM SODIUM GLUCINUM Ammonium sodium glucinum or/Aophosphate, (NH 4 ) 2 Na 2 Gl(PO 4 ) 2 +7H 2 O. Precipitate. (Scheffer.) Ammonium thallous orZAophosphate, (NH 4 ) 3 P0 4 , (NH 4 ) 2 T1P0 4 , or H 2 NH 4 P0 4 , HT1 2 PO 4 . Sol. in H 2 O. (Lamy; Rammelsberg.) Ammonium uranyl phosphate, NH 4 (U0 2 )P0 4 +o;H 2 0. Insol. in H 2 O and HC 2 H 3 O 2 +Aq. Sol. in mineral acids, from which it is precipitated by NH 4 C 2 H 3 O 2 +Aq, in which it is insol'. (Knop.) +3H 2 O. Insol. in H 2 O and acetic acid. Sol. in all mineral acids, oxalic acid and M 2 CO 3 +Aq. (Lienau, Dissert. 1898.) Ammonium vanadium phosphate. See Phosphovanadate, ammonium. Ammonium zinc e&wetaphosphate, (NH 4 ) 2 Zn(P 2 6 ) 2 +6H 2 0. Efflorescent. (Fleitmann, Pogg. 78. 347.) +4H 2 O. Sol. in 70 pts. H 2 O. Decomp. by H 2 SO 4 . (Glatzel, Dissert. 1880.) Ammonium zinc or^ophosphate, basic, 3NH 3 , 2ZnO, P 2 O 5 +8H 2 O. (Rother, A. 1867, 143. 356.) 4(NH 4 ) A 6ZnO, 3P 2 O 5 +4H 2 O. (Schweik- ert, A. 1868, 146. 57.) Ammonium zinc or/ftophosphate, NH 4 ZnPO 4 +H 2 0. Insol. in H 2 O. Sol. in acids, and caustic alkalies. (Bette, A. 15. 129.) Ammonium zinc hydrogen phosphate, NH 4 H 2 PO 4 , ZnHPO 4 +H 2 O. Insol. in H 2 O. (Debray.) 4(NH 4 ) 2 O, 6ZnO, 3P 2 O 5 . (Schweikert, A. 146. 57.) 3(NH 4 ) 2 O, 4ZnO, 2P 2 O 5 + 13H 2 O. (Rother, A. 143. 356.) Ammonium phosphate selenate. See Selenophosphate, ammonium. Barium /riphosphate, 5BaO, 3P 2 O 6 . Insol. in H 2 O; insol. in acids after heating to a high temp. (Schwarz, Z. anorg. 1895, 9. 264.) Barium raetophosphate, Ba(PO 3 ) 2 . Insol. in H>O or dil. acids. (Maddrell, A. 61. 61.) Not decomp. by boiling with acids or alkali carbonates +Aq. (Fleitmann, Pogg. 78. 352.) Barium cfo'wetophosphate, BaP 2 O 6 +2H 2 O. More difficultly sol. in H 2 O than Ba 3 (P 3 O 9 ) 2 . Slightly attacked by boiling cone. HCl+Aq or HNO 3 +Aq. Easily decomp. by H 2 SO 4 . (Fleitmann, Pogg. 78. 254.) Barium Zrmetaphosphate, Ba 3 (P 3 O 9 ) 2 +2H 2 O. Somewhat sol. in H 2 O. (Fleitmann, A. 65. 313.) +6H 2 O. Easily sol. in HCl+Aq. (Lind- bom.) 1 1. H 2 O dissolves 2.589 g. at ord. temp. (Wiesler, Z. anorg. 1901, 28. "198.) Barium hexametaphosph&te, Ba 3 P 6 O, 8 (?). Sol. in H 2 O only after boiling several hours. Nearly insol. in H 2 O. (Liidert, Z. anorg. 6. 15.) Insol. in NH 4 Cl+Aq. (Wackenroder.) Sol. in Na 6 P 6 O 18 +Aq. Sol. in HNO,+Aq. After ignition it is nearly insol. in HNO 3 +Aq. Barium ort/iophosphate, Ba 3 (PO 4 ) 2 . Precipitate. Very si. sol. or insol. in H 2 O. (Graham, Pogg. 32. 49.) Sol. in HCl+Aq. Decomp. by SO 2 +Aq. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Barium hydrogen phosphate, BaHPO 4 . Sol. in 10,000 pts. H 2 O. (Malaguti, A. ch. (3) 61. 346.) Sol. in 20,570 pts. H 2 O at 20. (Bischof, 1833.) Not completely soluble in water containing CO 2 , but BaCl 2 causes no ppt. in Na 2 HPO 4 + Aq containing 7.16 g. or less Na 2 HPO 4 in a litre after it has been saturated with CO 2 . (Setschenow, C. C. 1876. 97.) Easily sol. in H 3 PO 4 +Aq, and dil. HC1+ Aq. HNO 3 + Aq of 1 .275 sp. gr. if not diluted has scarcely any solvent action, but more dis- solves on dilution until a maximum is reached, when 10 vols. of H 2 O have been added. (Bischof, Schw. J. 67. 39.) Sol. in 367-403 pts. acetic acid (1.032 sp. gr.) at 22.5. (Bischof, I. c.) Easily sol. in H 2 O containing NH 4 C1, NH 4 NO 3 , or NH 4 succinate, from which solu- tions it is completely pptd. by NH 4 OH+Aq. (Rose.) Insol. in Na 2 HPO 4 or BaCl 2 +Aq. (Rose, Pogg. 76. 23.) More sol. in BaCl 2 or NaCl+Aq than in H 2 O, 1 pt. BaHPO 4 being sol. in 4362 pts. H 2 O containing 1.2% NaCl and 0.8% BaCl 2 . (Ludwig, Arch. Pharm. (2) 56. 265.) Sol. in Na citrate +Aq. (Spiller.) Barium tefrahydrogen phosphate, BaH 4 (PO 4 ) 2 . Sol. in H 2 O. (Mitscherlich, 1821.) Decomp. by much H 2 O into BaHPO 4 . Sol. in phosphoric, and certain other acids. (Berzelius, A. ch. 2. 153.) Barium pi/rophosphate, Ba 2 P 2 O 7 +zH 2 O. Somewhat sol. in H 2 O, in much H 4 P 2 O 7 + Aq, also in HCl+Aq or HNO 3 +Aq. Insol. in HC 2 H 3 O 2 + Aq or Na 4 P 2 O 7 + Aq. (Schwar- zenberg.) Insol. in NH 4 Cl+Aq. (Wackenroder.) PHOSPHATE, BORON 681 Barium hydrogen pyrophosphate, Ba 2 P 2 O 7 +3H 2 O. Ppt. (Knorre and Oppelt, B. 21. 773.) Barium teraphosphate, Ba 3 P 4 Oi3. Insol. in H 2 O or acids when strongly heated. (Fleitmann and Henneberg, A. 65. 331.) Barium manganic pyrophosphate, Ba(MnP 2 O 7 ) 2 +5H 2 O. Almost insol. in H 2 O. (Rosenheim, B. 1915, 48. 585.) Barium potassium fn'mefaphosphate, BaKP 3 O 9 +H 2 O. Much less sol. in H 2 O than NH 4 BaP 3 O 9 or NaBaP 3 O 9 . (Lindbom.) Sol. in HCl+Aq after ignition. Barium potassium or^ophosphate, BaKPO4. Insol. in H 2 O. (Ouvrard, A. ch. (6) 16. 297.) + 10H 2 O. (de Schulten, C. R. 96. 706.) Barium sodium diwefaphosphate, BaNa.(P 2 O 6 ) 2 +4H 2 O. (Glatzel, Dissert. 1880.) Barium sodium n'weaphosphate, BaNaP 3 O 9 +4H 2 0. More easily sol. in 1I 2 O than Ba 3 (P 3 O 9 ) 2 . Sol. in acids, unless ignited. (Fleitmann and Henneberg, A. 65. 314.) Efflorescent. Sol. in HCl+Aq after igni- tion only by long boiling. When fused it is easily sol. in HCl+Aq. (Lindbom, Acta Lund. 1873. 21.) Barium sodium orZ/iophosphate, BaNaPO 4 + 10H 2 O. (de Schulten, C. R. 96. 706.) Not attacked by cold, but decomp. by hot H 2 O. (Villiers, C. R. 104. 1103.) SI. sol. in H 2 O. (Quartaroli, C. A. 1911. 2375.) Barium sodium pi/rophosphate, Ba 4 Na 4 (P 2 O 7 ) s . Sol. in hot HC1 and HNO 3 . (Tammann, J. pr. 1892, (2) 45. 469.) 6Ba 2 P 2 O 7 , Na 4 P 2 O 7 +6H 2 O. Completely insol. in Na 4 P 2 O 7 +Aq, but not insol. in H 2 O or NH 4 OH+Aq. Easily sol. in HNO 8 or HC1 +Aq. Insol. in alcohol. (Baer, Pogg. 75. 164.) Barium uranous metaphosphate, UO 2 , BaO, P 2 5 . (Colani, A. ch. 1907, (8) 12. 142.) Barium uranyl ori/iophosphate, Ba(UO 2 ) 2 (PO 4 ) 2 +8H 2 O. Min. Uranocirrite. Barium phosphate chloride, 3Ba 3 (PO 4 ) 2 , BaCl 2 . Min. Barytapatite. (Deville and Caron, A. ch. (3) 67. 451.) 4BaH 4 (PO 4 ) 2 , BaCl 2 . (Erlenmeyer, J. B. 1857. 145.) ISBaO, 6P 2 O 5 , BaCl 2 +6H 2 O (?). Sol. in 18,000 pts. cold H 2 O. Much more sol. in H 2 O containing BaCl 2 , NH 4 C1, and NH 4 OH. (Ludwig, Arch. Pharm. (2) 56. 271.) Bismuth ortftophosphate, basic, 2BiPO 4 , 3Bi 2 O 8 . Insol. in H 2 O. Sol. in HCl+Aq. (Cavazzi, Gazz. ch. it. 14. 289.) Bismuth or/ftophosphate, BiPO 4 . Insol. in H 2 O or HNO 3 +Aq. SI. sol. in NH 4 salts+Aq. (Chancel, C. R. 50. 416.) Not decomp. by H 2 O. Other phosphates of Bi are decomp*. by H 2 O. (Montmartini, C. C. 1900, II. 1256.) Not hydrolyzed by hot H 2 O; si. sol. in BiCl s +Aq; decomp. by boiling alkali. (Caven, J. Soc. Chem. Ind. 1897, 16. 30.) More sol. in HCl+Aq than in HNO 3 +Aq. (Rose.) Sol. in UO 2 (NO 3 ) 2 +Aq. (M'Curdy, Am. J. Sci. (2) 31. 282.) Insol. in MNO 3 +Aq. Insol. in Bi salts+Aq. (Rose, Pogg. 76. 26.) Sol. in NH 4 Cl+Aq, but insol. in NH 4 NO 3 + Aq. (Brett, 1837.) + 1^H 2 O. (Kiihn.) +3H 2 O. Ppt. Decomp. by H 2 S or KOH +Aq. (Vanino, J. pr. 1906, (2) 74. 151.) Bismuth p^/rophosphate, basic, 2BiO s , P2O 5 . Insol. in H 2 O and HC 2 H 3 O 2 +Aq; sol. in hot HC1 and HNO.+Aq. Insol. in Na 4 P 2 O 7 +Aq, and NH 4 citrate +Aq. (Passerini, Cim. 9. 84.) Bismuth pi/rophosphate, Bi 4 (P 2 O 7 ) 3 / Insol. in H-O or HNO 3 +Aq. (Chancel, C. R. 50. 416.) Decomp. by H 2 O. (Wallroth, Bull. Soc. (2) 39. 316.) Sol. in Na 4 P 2 O 7 +Aq. (Stromeyer.) Bismuth sodium pyrophosphate, NaBiP 2 O 7 +3H 2 O. Insol. in H 2 O. (Rosenheim, B. 1915, 48. 588. Boron phosphate, BPO 4 . Insol. in II 2 O. Not attacked by boiling alkalies. (Meyer, B. 22. 2919.) 682 PHOSPHATE, BROMOMOLYBDENUM Bromomolybdenum phosphate. See under Bromomolybdenum comps. Cadmium ^'phosphate, Cd 5 (P 3 Oio) 2 . Insol. in H 2 O and acids. (Gliihmann, Dissert, 1899.) Cadmium te^mphosphate, 6CdO, 4P->O 6 + 1SH 2 O. Insol. in acids. (Gliihmann.) Cadmium metaphosphate. Very sol. in NH 4 OH+Aq. (Persoz, A. ch. 56.334.) Cadmium dimetaphosphate, Cd(PO 3 )^+2H 2 O. Sol. in 32 pts. H 2 O. Scarcely attacked by acids, especially cone. H 2 SO 4 . (Glatzel, Dissert. 1880.) Cadmium te^rawefaphosphate. Insol. in H 2 O. Easily decomp. by Na 2 S + Aq. (Fleitmann, Poggf 73. 358.) Cd 2 (PO 3 ) 4 +10H 2 Or Not so very difficultly attacked by acids but insol. after ignition. (Glatzel, Dissert. 1880.) Cadmium or^ophosphate, Cd s (PO 4 )2. Ppt. Insol. in H 2 O. Sol. in Cd salts +Aq. (Stromeyer.) Easily sol. in NH 4 sulphate, chloride, nitrate, or succinate+Aq. (Wittstein, Repert. 57. 32.) H 2 Cd 5 (PO 4 ) 4 +4H 2 O. Sol. in dil. H 3 PO 4 + Aq. (de Schulten, Bull. Soc. (3) 1. 473.) Cadmium ZeZrahydrogen phosphate, CdH 4 (PO 4 ) 2 +2H 2 O. Decomp. by great excess of H 2 O. (de Schulten.) Cadmium p?/r-0phosphate, Cd 2 P 2 O 7 +2H 2 O. Insol. in H 2 O. Sol. in NH 4 OH, Na 4 P 2 O 7 + Aq, or acids. Insol. in KOH+Aq. Sol. in SO 2 +Aq. (Schwarzenberg, A. 65. 183.) Cadmium hydrogen or^ophosphate hydra- zine ti nydroge , CdHPO 4 , 2N 2 H 4 . Decomp. by light. (Franzen, Z. anorg. 1908, 60. 283.) Cadmium potassium te/rawetaphosphate, CdK 3 (PO 3 ) 4 +3H 2 O. Sol. in 135 pts. H 2 O. Difficultly decomp. by acids. (Glatzel, Dissert. 1880.) Cadmium potassium or^iophosphate. CdKP0 4 . Insol. in H 2 O; sol. in dil. HCl+Aq. (Ouv- rard, A. ch. (6) 16. 321.) Cadmium potassium p?/rophosphate, CdK 2 P 2 O 7 . Insol. in H 2 O; sol. in dil. HCl+Aq. (Ouv- rard.) 5Cd 2 P 2 O 7 , 4K 4 P 2 O 7 +30H 2 O. Much more easily sol. in H 2 O than the CdNa salt. (Pahl, Sv. V. A. F. 30, 7. 39.) Cadmium sodium ^riphosphate, Na 3 CdP 3 Oio + 12H 2 O. Sol. in acids even after ignition. (Gliih- mann, Dissert. 1899.) Cadmium sodium /n'metaphosphate, Na 4 Cd(PO 3 ) 6 +4H 2 O. SI. sol. in H 2 O. Insol. in alcohol. (Wiesler, Z. anorg. 1901, 28. 204.) Cadmium sodium tetrametaphosphate, Na 2 Cd(PO 3 ) 4 +3H 2 O. Completely insol. in H 2 O. (Glatzel, Dis- sert. 1880.) Cadmium sodium or/^ophosphate, CdNa 4 (PO 4 ) 2 . Insol. in H 2 O; very sol. in dil. acids. CdNaPO 4 . As above. (Ouvrard.) Cadmium sodium pyro phosphate, CdNa 2 P 2 O 7 . Sol. in dil. acids, even acetic acid. (Wall- roth.) +4H 2 0. Insol. in H 2 O. (Pahl, Sv. V. A. F. 30, 7. 39.) Cadmium phosphate bromide, 3Cd 3 (PO 4 ) 2 , CdBr 2 . Sol. in cold very dil. HN0 3 +Aq. (de Schulten, Bull. Soc, (3) 1. 472.) Cadmium phosphate chloride, 3Cd 3 (PO 4 ) 2 , CdCl 2 . Sol. in dil. HNO 3 + Aq. (de Schulten.) Caesium raetaphosphate, CsPO 3 . Sol. in H 2 O. (von Berg, B. 1901, 34. 4185.) Caesium orZftophosphate, Cs 3 PO 4 +5H 2 O. Deliquescent ; very sol . in H 2 O . (von Berg.) Caesium hydrogen or^/iophosphate, Cs 2 HPO4 +H 2 O. Very sol. in H 2 O. (von Berg.) Ccesium rf^hydrogen or^ophosphate, CsH 2 PO 4 . Sol. in H 2 O; insol. in alcohol, (von Berg.) Cesium pyrophosphate, Cs 4 P 2 O 7 . Very sol. in H 2 O; very hydroscopic. (von Berg.) PHOSPHATES, CALCIUM 683 Calcium /riphosphate, 5CaO, 3P 2 O 5 . Insol. in H 2 O. (Schwarz, Z. anora. 1895, 9. 264.) Calcium monometaphosphate t Ca(PO 3 ) 2 . Insol. in H 2 O and dil. acids. (Maddrell, A. 61. 61.) Not decomp. by digestion with alkali car- bonates +Aq. (Fleitmann.) Calcium dimetaphosphate, Ca 2 (P 2 O 6 ) 2 + 4H 2 O. Insol. in H 2 O. Decomp. by warm H 2 SO 4 , but not appreciably by cone. HC1 or HNO 3 + Aq. (Fleitmann, Pogg. 78. 255.) Calcium hexametaph.ospha.te (?). Insol. in H 2 O. Sol. in Na 6 P 6 Oi 8 +Aq and in HCl+Aq. (Rose, Pogg. 76. 3.) Ca 3 P 6 Oi8. Nearly insol. in H 2 O; sol. in dil. acids. (Liidert, Z. anorg. 5. 15.) Calcium or/Aophosphate, basic, 3Ca 3 (PO 4 % + CaO 2 H 2 . (Warington, J. B. 1873. 253.) 4CaO, P 2 O 5 . (Hilgenstock.) Calcium or^Aophosphates, Solubility of CaO in P 2 O 5 +Aq at 25. g. CaO per 1. of solution g. PsOsperl. of solution Solid phase 7 61 19.96 6.51 16.52 5.01 12.82 CaHP0 4 3.42 8.16 2.42 5.75 1.58 3.66 0.544 1.516 0.400 1.108 0.291 0.773 Solid phases are 0.232 0.662 evidently solid 0.145 0.381 solutions 0.062 0.109 0.049 0.088 0.034 0.015 Ca 3 (PO 4 ) 2 0.587 0.013 \ Solid phase is prob- 0.789 0.012 j ably a solid solution (Cameron and Seidell, J. Am. Chem. Soc. 1905, 27. 1513.) Solubility of CaO in P 2 O 5 +Aq at 50.7. Solubility of CaO in P 2 O 5 +Aq at 25. 100 g. of the solution contain Solid phase g. CaO per 1. of solution g. P 2 O 5 per 1. of solution Solid phase g. P 2 6 g. CaO > 62.01 0.336 CaH4P2O 8 +CaH4P 2 O8, H 2 O 1.71 4.69 58.08 0.635 CaH4P 2 O s , H 2 7.48 22.39 54.67 0.939 >< 8.10 23.37 50.25 1.428 II 11.57 36.14 46 15 2.100 < 12.88 41.24 41.92 2.974 .< 18.77 59.35 37.33 3.898 19.25 63.03 33 18 4.880 II 23.31 75.95 CaHPO 4 , 2H 2 O 29.61 5.725 CaH 4 P 2 8 , H 2 +CaHPOi 23.69 79.10 15.48 3.507 CaHPO 4 32.41 109.8 9.465 2.328 35.90 129.8 6.157 1.563 39.81 139.6 2.946 0.852 40.89 142.7 2.281 0.692 <> 43.82 154.6 0.1521 0.0588 49.76 191.0 0.1527 0.0596 CaHPO4, 2H 2 O 55.52 216.5 0.1331 0.0514 Ca3P 2 S) H 2 0. 59.40 234.6 0.0942 0.0351 70.31 279.7 0.0309 0.0106 72.30 fiQ ^ 351.9 OfM 1 0.00068 0.00071 " V)i7 . OO 65.46 63.53 OD1 . 380.3 395.1 (Bassett, Z. anorg. 1908, 69. 15.) 59.98 419.7 CaH 4 (PO 4 ) 2 , H 2 O 59.25 424.6 57.74 428.0 53.59 451.7 48.78 475.3 44.52 505.8 41.86 528.9 39.89 538.3 (Cameron and Seidell, J. Am. Chem. Soc. 1905, 27. 1508.) 684 PHOSPHATE, CALCIUM Solubility of CaO in P 2 O 5 +Aq at 40. 100 g. of the solution contain Solid phase g. P 2 5 g. CaO 45.42 1.768 CaH 4 P 2 O 8 , H 2 O 41.33 2.588 u 36.79 3.584 u 32.46 4.505 (c 28.27 5.501 " 21.67 4.813 CaHP0 4 17.78 4.100 " 16.35 3.810 K 9.905 2.536 n 6.979 1.847 <( 4.397 1.267 ce 1.819 0.576 (i 0.423 0.156 u 0.294 0.110 (( 0.158 0.0592 a 0.146 0.0519 u 0.128 0.0508 Ca 3 P 2 8 , H 2 O 0.0262 0.0098 u trace 0.0709 Ca 4 P 2 O 9 , 4H 2 O u 0.0814 it ti 0.0829 se 0.0840 ee (Bassett, Z. anorg. 1908, 59. 18.) Solubility of CaO in P 2 O 5 -fAq at 25. 100 g. the solution contain Solid phase g. PsOs g. CaO 36.11 3.088 CaH 4 P 2 O 8 , H 2 O 31.97 4.128 28.34 4.908 ii 27.99 4.930 it 25.45 5.489 11 22.90 5.523 CaHPO 4 17.55 4.499 " 15.34 4.027 9.10 2.638 u 6.049 1.878 a 3.613 1.181 (t 2.387 0.826 a 0.417 0.165 CaHPO 4 +CaHPO 4 , 2H 2 O 0.178 0.0696 (( 0.0332 0.0126 u 0.0948 0.0352 Probably Ca 3 P 2 Os, H 2 O 0.0571 0.0211 a 0.0525 0.0175 M 0.0468 0.0186 11 trace 0.1131 Ca 4 P 2 9 ,4H 2 0+Ca(OH) 2 0.118 Ca(OH) 2 (Bassett, Z. anorg. 1908, 59. 20.) Calcium or^ophosphate, Ca 3 (PO 4 ) 2 . Decomp. by long boiling with H 2 O into basic salt, 3Ca 3 (PO 4 ) 2 , CaO 2 H 2 . This de- comp. begins with cold H 2 O, so that the solu bility at 6-8 varies from 9.9 to 28.6 mg. in a litre^ (Warington, Chem. Soc. (2) 11. 983.) 1 1. cold H 2 O dissolves in 7 days 31 mg. gnited, and 79 mg. freshly precipitated Ca 3 (PO 4 ) 2 . (Volcker, J. B. 1862. 131.) 100,000 pts. H 2 O dissolve 2.36 pts. gelatin- ous Ca phosphate; 2.56 pts. ignited Ca phos- )hate; 3.00 pts. Ca phosphate from bone dust. Maly and Donath, J. pr. (2) 7. 416.) Solubility of bones in various solvents is given bv Maly and Donath, I. c. 0.009" g. Ca 3 (PO 4 ) 2 is sol. in 1 1. H 2 O. 0.153 " " " " " " sat. with CO 2 . (Joffre, Bull. Soc. 1898, (3) 19.372.) Determinations of solubility in H 2 O as stated in the literature vary because Ca 3 (PO 4 ) 2 s apparently a solid solution of CaHPO 4 and UaO. When placed in contact with H 2 O more PO 4 ions dissolve than Ca ions, the resulting solution is acid and solid phase icher in Ca than before addition of H 2 O. For material of the approximate composition, a 3 (PO 4 ) 2 , the amt. dissolved by CO 2 free H 2 O at ord. temp, is 0.01-0.10 g. per 1. depending on conditions of experiment. H 2 O sat with 2 dissolves 0.15-0.30 g. per 1. (Cameron and Hurst, J. Am. Chem. Soc. 1904, 26. 903.) The decomposition of Ca 3 (PO 4 ) 2 in H 2 O is increased by presence of CaSO 4 ; decreased by presence of CaCO 3 or of CaSO 4 and CO 2 . CO 2 increases the amount of PO 4 dissolved in the solution of water alone and the sat. CaSO 4 solutions, but has no other effect than to in- crease the amount of Ca in the solutions in contact with CaCO 3 . (Cameron and Seidell, J. Am. Chem. Soc, 1904, 26. 1458.) Sol. in CO 2 +Aq. 1 1. H 2 O containing 1 vol. CO 2 dissolves in 12 hours at 10 0.75 g. precipitated Ca 3 (PO 4 ) 2 ; 0.166 g. Ca 3 (PO 4 ) 2 from bone ash; 0.300 g. Ca 3 (PO 4 ) 2 from bones which had been buried 20 years. (Lassaigne, J. ch. me"d. (3) 3. 11.) 1 1. H 2 O containing 0.8 vol. CO 2 dissolves 0.61 g. Ca 3 (PO 4 ) 2 . (Liebig, A. 106. 196.) H 2 O sat. with CO 2 at 5-10 and 760 mm. pressure dissolves 0.527-0.60 g. Ca 3 (PO 4 ) 2 , or, if containing 1% NH 4 C1, 0.739 g. Ca 3 (PO 4 ) 2 . (Warington, Chem. Soc. (2) 9. 80.) Solubility varies according to form of Ca 3 (PO 4 ) 2 / In apatite, 1 pt. Ca 3 (PO 4 ) 2 dissolves in 222.222 pts. H 2 O sat. with CO 2 ; in raw bones, in* 5698 pts.; in bone ash, in 8029 pts.; in So. Carolina phosphate, in 6983 pts.; in phos- phatic guano from Orchilla Id., in 8009 pts. (Williams, C. N. 24. 306.) A1 2 O 6 H 6 and Fe 2 O 6 H 6 prevent the solubility of Ca 3 (PO 4 ) 2 in H 2 O containing CO 2 . (War- ington, I. c.} 1 1. H 2 O dissolves 0.22848 g. Ca 3 (PO 4 ) 2 . under a CO 2 -pressure of 2 atmos. at 14. (Ehlert, Z. Elektrochem. 1912, 18. 728.) Sol. in S0 2 +Aq, forming a liquid of 1.3 sp. gr. at 9 from freshly precipitated Ca 3 (PO 4 ) 2 , and of 1.188 sp. gr. from bone ash. Sol. in H 2 S+Aq. 1 1. H 2 O sat. with H 2 S PHOSPHATE, CALCIUM 685 dissolves 190-240 mg. Ca 3 (PO 4 ) 2 . (Bechamp, A. ch. (4) 16. 241.) Easily sol. in HNO 3 or HCl+Aq. 100 pts. very dil. HCl+Aq dissolve 198-225 pts. Ca 3 (PO 4 ) 2 . (Crum, A. 63. 294.) 100 pts. HC1 of 1.153 sp. gr. (containing 31% HC1) dissolve at 17 when diluted with: 0147 pts. H 2 O, 25.3 45.0 62.3 64.7 pts. Ca 3 (PO 4 )2, 10 13 16 19 pts. H 2 O. 68.0 71.9 69.5 69.7 pts. Ca 3 (PO 4 ) 2 . (Bischof, Schw. J. 67. 39.) Decomp. by H 2 SO 4 . Completely decomp. to CaSO 4 and H 3 PO 4 by a mixture of H 2 SO 4 and alcohol. Solubility in HNO 3 +Aq. 1 pt. of Ca 3 (PO 4 ) 2 dissolves at 16.25-17.5 in pts. HNOs+Aq which contain pts. H 2 O to 1 pt. HNO 3 (sp. gr. = 1 .23). Dry Ca 3 (POO (boiled) con- taining 10% NH 4 C1 at 17; 1788 pts. H 2 O sat. with CO 2 and containing 10% NH 4 C1 at 10 and 751 mm. pressure; 1351 pts. H 2 O sat. with CO 2 and containing 1% NH 4 C1 at 12 and 745 mm. pressure; 42,313 pts. H 2 O sat. with CO 2 and containing CaCO 3 at 21 and 756.3 mm. pressure; 18,551 pts. HoO sat. with CO 2 and containing CaCO 3 and 1% NH 4 C1 at 16 and 746.1 mm. pressure. (Warington, Chem. Soc. (2) 4. 296.) Aqueous solutions of the following NH 4 salts dissolve the given amts. of Ca 3 (PO 4 ) 2 , calculated for 100 pts. of the corresponding acid: NH 4 C1, 0.655 pt.; NH 4 NO 3 , 0.306 pt.; Pts. HNOs+Aq Pts. H 2 Pts. HNOs+Aq Pts. H 2 O (,iNn 4 ; 2 i5U 4 , i.uou pts.; i\n 4 ^ 2 jn 3 vj 2 , u.zoo pt.; NH 4 tartrate, 4.56 pts.; NH 4 citrate, 7.015 pts.; NH 4 malate, 1.125 pts. Ca 3 (PO 4 ) 2 . (Ter- reil, Bull. Soc. (2) 35. 578.) Solubility in various salts +Aq under a CO 2 pressure of 2 atmospheres, at 14. 2.72 4.23 10.25 15.45 20.34 20.82 0.827 3.309 5.791 8.273 10 30.64 26.48 32.14 36.06 127.81 10.754 13 13.236 15.718 40 Salt G. salt per 100 g. H 2 O G. Cas(PO 4 ) 2 sol. in 1 1. of the solvent. (Bischof, 1833.) More sol. in acetic, lactic, malic, and tar- taric acids than in HC1 or HNO 3 +Aq. (Crum.) Solubility in H 3 PO 4 -f Aq. H 2 0.22848 NaCl 50 cone. 1.3208 0.64089 G. HsPO 4 HaPO n 100 cc. of 4+Aq G. Ca 3 (PO 4 ) 2 dissolved by 100 cc. of solvent MgCl 2 +6H 2 O 86.9 cone. 1.2873 2.8923 5 10 15 20 25 30 3.85 7.28 9.45 12.50 13.79 15.10 KMgCl 3 +6H 2 O 79.2 cone. 1.5771 1.1536 K 2 S0 4 ,MgS0 4 , MgCl 2 +6H 2 O 70.95 cone. 1.7777 2.4911 NaN0 3 72.7 cone. 1.5827 0.8638 (Causse, C. K. 1892, 114. 414.) Very small quantities of the salts of the alkali metals increase the solubility in H 2 O. (Lassaigne, J. chim. med. (3) 3. 11.) 1 litre cold HoO with 2 g. NaCl dissolves 45.7 mg. Ca 3 (PO 4 ) 2 ; with 3 g. NaNO 3 , 33 mg. Ca 3 (P0 4 ) 2 . (Liebig.) 1 litre H 2 O containing 8.75% NaCl dissolves 317.5 mg. Ca(PO 4 ) 2 . (Lassaigne.) NH 4 salts have even more effect, especiallv NH 4 Cl+Aq, which dissolves Ca 3 (PO 4 ) 2 in the cold; also ammonium nitrate and suc- cinate. (Wittstein.) (NH 4 ) 2 SO 4 +Aq dissolves Ca 3 (PO 4 ) 2 as easily as CaSO 4 . (Liebig, A. 61. 128.) 1 litre H 2 O containing 2 g. NaCl dissolves at 7-12.3 45.7 mg. Ca 3 (PO 4 ) 2 ; 3 g. NaNO 3 at 17.3, 33 rng. Ca 3 (PO 4 ) 2 ; 2.2 g. (NH 4 ) 2 SO 4 , 76.7 mg. Ca 3 (PO 4 ) 2 . (Liebig, A. 106. 185.) K 2 S0 4 74.5 cone. 4.9041 4.7649 (NH 4 ) 2 S0 4 56.5 cone. 2.4131 5.8849 Na 2 SO 4 +10H 2 O 137.7 cone. 2.4911 3.2267 MgSO 4 +7H 2 O 105.3 cone. 1.9728 3.6001 NH 4 C1 45.74 cone. 1.3710 1.2929 (Ehlert and Hempel, Z. Elektrochem. 1912, 18. 728.) 686 PHOSPHATE, CALCIUM Ca 3 fPO 4 ) 2 is sol. in K 2 C 2 O 4 +Aq. 100 ccm. K 2 C 2 O 4 +Aq (iy 2 % K 2 C 2 O 4 ) dissolves 57.1% of the P 2 O 5 from phosphorite, 71 % from guano by boiling 25 min. At ord. temp, bone meal gives up 50-80% of its P 2 O 5 to K 2 C 2 O 4 +Aq in 36 hours. (Liebig, Landw. J. B. 1881. 603.) Sol. in Ca suorate+Aq. (Bobierre, C. R. 32. 859.) More sol. in H 2 O containing starch, glue, or other animal substances than in pure H 2 O. (Vauquelin, Pogg. 85. 126.) Sol. in H 2 O containing organic matter, therefore when bones decay under H 2 O, Ca 3 (PO 4 )o is dissolved in considerable quan- tity. (Hayes, Edin. Phil. J. 5. 378.) Sol. in sodium citrate +Aq. (Spiller.) Solubility in NH 4 citrates +Aq. Ammonium citrate solution of 1.09 sp. gr. at 30-35 dissolves precipitated Ca 3 (PO 4 ) 2 completely, but not phosphorite. (Frese- nius.) Dried on the oir, with 2V&H 2 O. Sol. in 40 min. in diammonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq (sp. gr. = 1.09) dissolves 55.3% of the P,O 5 ; citric acid +Aq (H%) dissolves 83.8% of the P 2 O 5 . (Erlenmeyer, B. 14. 1253.) Dried at 50, with 1 7 /8H 2 O. Sol. in 45 min. in diammonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq dissolves 52.3% of the P 2 O 5 . (Erlenmeyer.) Ignited. Diammonium citrate+Aq (sp. gr. 1.09) dissolves 93% of the P 2 O 5 ; triammonium citrate+Aq (sp. gr. 1.09) dissolves 32% of the P 2 O 5 ; citric acid (M%) dissolves 53.4% of the P 2 O 8 . (Erlenmeyer.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in alcohol and ether. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Min. Apatite. 0.002 g. is sol. in 1 1. H 2 O. 0.014 " " " " 1 1. H 2 O sat. with CO 2 . (Joffre, Bull. Soc. 1898, (3) 19. 374.) +H 2 O. Solubility in H 2 O, in H 2 O sat. with CO 2 , and in H 2 O containing CO 2 +CaH 2 (CO 3 ) 2 . Temp. 16-20. ooiveut P 2 O 5 mg. CaO mg. (1) Boiled distilled H 2 O. 0.74 (2) 1200 cc. distilled H 2 O+50 cc. H 2 O sat. with CO 2 . 6.9 (3) 1000 cc. " " +250 cc. " " tt tt 48.5 (4) 1250 cc. H 2 O sat. with CO 2 . 91.9 Solutions of CO 2 +CaH 2 (CO 3 ) 2 . 1 1. (filtered) contains: Calcium carbonate 13 mg. (5) j Bicarbonate j gf acid 166 ' 73 ' 0.38 100.0 Free carbonic acid 9 ' Calcium carbonate 13 ' (6) Bicarbonate { gf acid 277 ' 122 " 1.1 162.3 Free carbonic acid 49 " Calcium carbonate 13 " (7) Bicarbonate ^ v^aroonate 376 " 165 " 0.80 218.8 Free carbonic acid 105 " Calcium carbonate 13 " (8) Bicarbonate { g^^cacid 475 " 209 " 1.77 273.3 Free carbonic acid 206 " Calcium carbonate 13 " (9) -DlCcWDOIlSlt/G "{ /~*\ i i 545 " 240 " 1.30 312.7 Free carbonic acid 301 " In 1 1. of the filtrate (Schloesing, C. R. 1900, 131. 151.) PHOSPHATE, CALCIUM HYDROGEN 687 Calcium hydrogen phosphate. CaHPO 4 , and +2H 2 0. Insol. or nearly so in H 2 O. Gradually decomp. by cold, more quickly by hot H 2 O. 1000 pts. H 2 O dissolve 0.135-0.152 pt. CaHPO 4 +2H 2 O. Solution clouds up on boil- ing. (Birnbaum.) 1000 pts. H 2 O dissolve 0.28 pt., and if sat. with CO 2 , 0.66 pt. CaHPO 4 +2H 2 O. (Dusart and Pelouze.) When this salt dissolves in H 2 O, decomp. takes place and a very considerable time is necessary to establish equilibrium. (Rindell, C. R. 1902, 134. 112.) Much less decomp. by H 2 O than Ca 3 (PO 4 ) 2 or CaH 4 (PO 4 ) 2 , and the decomposition of this salt in water depends only slightly upon the relative amounts of solid and solvent which are present. The decomposition is in- creased by the addition of CO 2 . The presence of CaSO 4 or of CaCO 3 decreased the amount of phosphoric acid which dissolved. See original paper. (Cameron and Seidell, J. Am. Chem. Soc, 1904, 26. 1460.) When the ratio of P 2 O 5 : CaO is above 1.0 or below 1.27, H 2 O dissolves 0.4CK).54 g. CaO and 1.11-1.52 g. P 2 O 5 (see original paper). (Cameron and Bell, J. Am. Chem. Soc. 1905, 27. 1512.) Solubility in H 3 PO 4 +Aq. G. H 3 PO 4 in 100 cc. H3PO 4 +Aq G. CaHPO 4 dissolved by 100 cc. of solvent 5 4.30 10 7.15 15 9.30 20 11.86 25 13.40 30 15.10 (Causse, C. R. 1892, 114. 415.) 1 1. H 2 O containing 2.2 g. (NH 4 ) 2 SO 4 , 2 g. NaCl, or 3 g. NaNO 3 dissolves 79.2, 66.3, or 78.9 mg. CaP 2 O 7 , which is present in form of CaHPO 4 . (Liebig, A. 106. 185.) Slowly but completely sol. in boiling NH 4 Cl+Aq. (Kraut, Arch. Pharm. (2) 111. 102.) Easily sol. in H 2 SO 3 +Aq. (Gerland, J. pr. (2) 4. 123.) Very sol. in HC1 or HNO 3 +Aq. Less sol. in HC 2 H 3 O 2 . (Berzelius.) More sol. in dil. than cone. HC 2 H 3 O 2 +Aq, but 60 pts. HC 2 H 3 O 2 (1 mol.) dissolve at most 23.1 pts. P 2 O 5 (1 mol. = 142 pts.) from this compound. Aqueous solution of sodium acetate dissolves more easily than H 2 O, and becomes turbid on boiling. (Birnbaum.) Completely sol. in K 2 C 2 O 4 +Aq. (Liebig, Landw. J. B. 1881. 603.) 1 1. of sat. solution in N/200 acid K tartrate +Aq at 25 contains 0.235 g. CaHPO 4 . Insol. in alcohol. Sol. in many organic substances, as starch or gelatine +Aq. Insol. in acetone. (Eidmann, C. C. 1899, II. 1014.) + V 3 H 2 O. (Vorbringer, Z. anal. 9. 457.) +H 2 O. (Gerlach, J. pr. (2) 4. 104.) +2H 2 O. Min. Brushite. +3H 2 O. Min. Metabrushite. + 5H 2 O. (Dusart, C. R. 66. 327.) Calcium tetrahydrogen or^Aophosphate, CaH 4 (P0 4 ) 2 +H 2 0. Very deliquescent. Crystals take up 97.7 pts. H 2 O in 16 days, and 226 pts. H 2 O in 28 days from air saturated with moisture. (Birnbaum, Zeit. Ch. (2) 7. 131.) Not hygroscopic when pure. (Stocklasa, B. 23. 626 R.) Completely sol. in 100 pts. H 2 O, but de- comp. by 10-40 pts. H 2 O with separation of CaHPO 4 , which slowly dissolves. (Erlen- meyer, J. B. 1873. 254.) Later (B. 9. 1839) Erlenmeyer says CaH 4 (PO 4 ) 2 +H 2 O is sol. in 700 pts. H 2 O and decomp. into CaHPO 4 by a less amount of H 2 O. Wattenberg (Z. anal. 19. 243) says that the decomposition by small amts. of H 2 O down to 144 pts. H 2 O to 1 pt. salt is inappre- ciable. Completely sol. in 200 pts. H 2 O if pure, and in less H 2 O in presence of H 3 PO 4 . (Stocklasa.) Sol. in 25 pts. H 2 O at 15. Solution begins to decompose when warmed to 50. (Otto, C. C. 1887. 1563.) Greatly decomp. by H 2 O and the resulting solution is to be regarded as a solution of the decomposition products rather 'than of the substance itself. The presence of an excess of CaSO 4 does not materially affect the amount of phosphoric acid entering the solu- tion. (Cameron, J. Am. Chem. Soc. 1904, 26. 1462.) Violently decomp. by H 2 O in cone, solu- tion; only si. decomp. when dissolved in 200 pts. H 2 O. (Stocklasa, Z. anorg. 1892, 1. 310.) Solubility of CaH 4 P 2 O 8 in H 3 PO 4 +Aq at pressure of 745 mm. at high temp. ft PP 100 g. of the solution contain Solid phase G. P 2 5 G. CaO 115 132 169 43.60 53.43 63.95 5.623 4.327 4.489 CaH 4 P 2 8 , H 2 O+CaHPO 4 CaH 4 P 2 O 8 +CaH 4 P 2 O 8 , H 2 O CaH^Os (Bassett, Z. anorg. 1908, 69. 26.) Glacial HC 2 H 3 O 2 ppts. it completely from aqueous solution even in presence of HNO 3 . (Persoz.) Decomp. by 50 pts. absolute alcohol at b.- pt. in 1 hour; by 30 pts. in 2 hours. Sol. in absolute ether. (Erlenmeyer, I.e.) 688 PHOSPHATE, CALCIUM Calcium p?/rophosphate, Ca 2 P 2 O 7 +4H 2 O. Somewhat sol. in H 2 O; completely sol. in mineral acids; less sol. in acetic acid, and in- sol. in Na 4 P 2 O 7 +Aq. (Schwarzenberg, A. 65. 145.) Less sol. in warm than in cold acetic acid. (Baer, Pogg. 75. 155.) Insol. in NH 4 Cl+Aq. (Wackenroder, A. 41. 316.) Insol. in CaCl 2 +Aq. Min. Pyrophosphorite. Calcium hydrogen pz/rophosphate, CaH 2 P 2 O 7 +2H 2 O. Sol. in H 2 O. (Pahl, B. 7. 478.) 2CaH 2 P 2 O 7 , Ca ? P 2 O 7 +6H 2 O. Decomp. by boiling with H 2 O into CaIi 2 P 2 O 7 , Ca 2 P 2 O 7 +3H 2 O. Insol. in hot H 2 O. (Knorre and Oppelt, B. 21. 771.) Tefracalcium hydrogen phosphate, Ca 4 H(P0 4 ) 3 +H 2 0. Ppt. Insol. in H 2 O, but decomp. by boiling therewith. Sol. in acids. (Warington, Chem. Soc. (2) 4. 296.) +2H 2 O. Calcium tefraphosphate, Ca 3 P 4 O 13 . Insol. in acids when ignited. (Fleitmann and Henneberg, A. 65. 331.) Calcium lithium phosphate, CaLiPO 4 . Insol. in H; 2 O. (Rose, Pogg. 77. 298.) Calcium potassium cfo'raefaphosphate, CaK 2 (P 2 O 6 ) 2 +4H 2 O. As BaK comp. (Glatzel, Dissert. 1880.) Calcium potassium or/ftophosphate, CaKPO 4 . Insol. in H 2 O. (Rose, Pogg. 77. 291.) Easily sol. in acids. (Ouvrard, A. ch. (6) 16. 308.) Calcium potassium p^/rophosphate, CaK 2 P 2 O 7 . Insol. in H 2 O; easily sol. in dil. acids. (Ouvrard, C. R. 106. 1599.) Calcium sodium dimetaphosphate, CaNa 2 (P 2 O 6 ) 2 +4H 2 O. As BaNa comp. (Glatzel.) Calcium sodium Znwetaphosphate, CaNaP 3 O 9 +3H 2 O. SI. sol. in H 2 O. (Fleitmann, A. 65. 315.) Easily sol. in H 2 O. Difficultly sol. in HCI+ Aq when heated to redness. Easily sol. in boiling HCl+Aq after being fused. (Lind- bom.) Calcium sodium or^/iophosphate, CaNaPO 4 . Insol. in H 2 O. (Rose, Pogg. 77. 292.) Easily sol. in dil. acids. (Ouvrard, A. ch. (6) 16. 308.) 3CaO, 3Na 2 O, 2P 2 O 5 . Sol. in dil. acids. (Ouvrard, C. R. 1888, 106. 1599.) Calcium sodium p?/rophosphate, CaNa 2 P 2 O 7 +4H 2 O. Insol. in Na 4 P 2 O 7 +Aq. Easily sol. in IICl+Aq, HNO 3 +Aq, and also in HC 2 H 3 O 2 +Aq. (Baer, Pogg. 75. 159.) Ca 10 Nai 6 (P 2 O 7 ) 9 . Sol. in acids. (Wallroth, Bull. Soc. (2) 39. 316.) 3CaO, 3Na 2 O, 2P 2 O 5 . Easily sol. in acids. (Ouvrard, A. ch. (6) 16. 307.) Calcium thorium raetaphosphate, ThO 2 . CaO, P 2 5 . (Colani, C. R, 1909, 149. 209.) Calcium uranous raetaphosphate, UO 2 , CaO, P 2 5 . Insol. in acids. (Colani, A. ch. 1907, (8) 12. 140.) Calcium uranyl phosphate, Ca(UO 2 )H 2 (PO 4 ) 2 +2, 3, or 4H 2 O. Sol. in HNO 3 +Aq. (Debray.) Ca(UO 2 )o(PO 4 ) 2 +8H 2 O. Min. Uranite. Sol. in HNO 3 +Aq. 3CaO, 5UO 3 , 2P 2 6 +16H 2 O. (Blinkoff, Dissert. 1900.) Calcium phosphate chloride, Ca 3 (PO 4 ) 2 , CaCl 2 . (Deville and Caron, A. ch. (3) 67. 458.) 3Ca 3 (P0 4 ) 2 , CaCl 2 . Chlor apatite. Insol. in H 2 0. (Daubree, Ann. Min. (4) 19. 684.) 7CaH 4 (PO 4 ) 2 , CaCl 2 +14H 2 O. Sol in HCl+Aq. 4CaH 4 (PO 4 ) 2 , CaCl.+SHsO. CaH 4 (PO 4 )o, CaCl 2 +2H 2 O. Partly sol. in H 2 O with decomp. Also with 8H 2 O. (Erlen- meyer, J. B. 1857. 145.) Calcium phosphate chloride fluoride, 3Ca 3 (PO 4 ) 2 , CaClF. Min. Apatite. Boiling H 2 O dissolves out CaCl 2 ; dil. mineral acids dissolve easily, acetic acid with more difficulty. Easily soluble in molten NaCl, crystallizing on cooling. (Forch- hammer.) Calcium phosphate silicate, Ca 3 (PO 4 ) 2 , Ca 2 SiO 4 . Insol. in H 2 O; decomp. by HCl+Aq. (Carnot and Richard, C. R. 97. 316.) 4Ca 3 (PO 4 ) 2 , Ca 3 SiO 5 . (Bucking and Linck, C. C. 1887. 562.) 4Ca 3 (PO 4 ) 2 , 3Ca 3 SiO 5 . (B. and L.) Ca(PO 3 ) 2 , CaSiO 3 . (Stead and Ridsdate, Chem. Soc. 51. 601.) Calcium dihydrogen phosphate sulphite, CaH 2 (PO 4 ) 2 , CaSO 3 +H 2 O. Not decomp. by cold, slowly by boiling H 2 O. Slightly sol. in NH 4 OH+Aq. Sol. in mineral acids. Insol. in cold, slowly sol. in boiling acetic acid. More sol. in a solution of oxalic acid. (Gerland, C. N. 20. 268.) PHOSPHATE, COBALTOUS 689 Cerous metaphosphate, Ce(PO 3 ) 3 . (Rammelsberg.) Ce 2 O 3 , 5P 2 O&. Insol. in H 2 O or acids. (Johnsson, B. 22. 976.) Cerous or^ophosphate, CePO 4 . Insol. in H 2 O. Easily sol. in acids. (Grandeau, A. ch. (6) 8. 193.) Insol. in acids. (Hartley, Proc. Roy. Soc. 41. 202.) +2H 2 O. Insol. in H 2 O. Sol. in acids. (Jolin.) Insol. in H 3 PO 4 +Aq; si. sol. in HC1 or HNO 3 +Aq. (Hisinger.) Insol. in HNO 3 +Aq. (Boussingault, A. ch. (5) 6. 178.) Min. Cryptolite. Completely decomp. by H. 2 SO 4 when finely powdered. Insol. in dil. HNOa+Aq. Ceric or^ophosphate, 4CeO 2 , 6P 2 O 5 +26H 2 O. Ppt. (Hartley, Proc. Roy. Soc. 41. 202.) Cerous p?/rophosphate, Ce 2 H 2 (P 2 O 7 ) 6 +6H 2 O. Sol. in cerous nitrate +Aq. Ce 4 (P 2 O 7 ) 3 + 12H 2 O. Sol. in excess of sodium pyrophosphate+Aq. Easily sol. in HC1. (Rosenheim, B. 1915, 48. 592.) Cerous lanthanum thorium phosphate, (Ce, La, Th) 2 (PO 4 ) 2 . Min. Monazite. Sol. in HCl+Aq with white residue. Cerous potassium orZ/iophosphate, 2Ce 2 O 3 , . 3K,O, 3P 2 O 5 = 2CePO 4 , K 3 PO 4 . Insol. in H 2 O; sol. in acids. (Ouvrard, C. R. 107. 37.) Cerous sodium or^ophosphate, Ce 2 O 3 , 3Na 2 O, 2P 2 O 5 = CeP0 4 , Na 3 PO 4 . Insol. in H 2 O. (Ouvrard, C. R. 107. 37.) Cerous sodium pyrophosphate, CeNaP 2 O7. Insol. in acetic, and cold dil. mineral acids. Sol. in warm acids. (Wallroth.) Chromous phosphate, Cr 3 (PO 4 ) 2 . Insol. in H 2 O. Easily sol. in citric, tartaric and acetic acids. SI. sol. in H 2 CO 3 +Aq. (Moissan, A. ch. 1882, (5) 25. 415.) +H 2 O. Precipitate. Easily sol. in acids. (Moberg; Moissan, A. ch. (5) 21. 199.) Chromic wetaphosphate, Cr 2 (PO 3 ) 6 . Insol. in H 2 O or cone, acids. (Maddrell, A. 61. 53.) Chromic ort'/iophosphate, CrPO 4 . Hydrolyzed by hot H 2 O. Somewhat sol. in NH 4 OH+Aq and in Cr 2 (SO 4 ) 3 +Aq. (Caven, J. Soc. Chem. Ind. 1897/16. 29.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Chromic phosphate, Cr 2 (PO 4 ) 2 + 12H 2 O. Violet modification. Precipitate. (Ram- melsberg, Pogg. 68. 383.) -f-6H 2 O. Green modification. Very si. sol. in ~HoO and still less in NH 4 NO 3 or NH 4 C 2 H 3 6 2 +Aq. (Carnot, C. R. 94. 1313.) Insol. in acetic, but easily sol. in mineral acids. Easily sol. in cold KOH or NaQH + Aq, from which it is separated on boiling. (Bowling and Plunkett, Chem. Gaz. 1868. 220.) Chromic hydrogen phosphate, Cr 2 H 6 (PO 4 ) 4 + 16H 2 O. Sol. in H 2 O. (Haushofer.) Chromic p?/rophosphate, Cr 4 (P 2 O 7 ) 3 . Anhydrous. Insol. in H 2 O or acids. (Ouv- rard, A. ch. (6) 16. 344.) +7H 2 O. Precipitate. Sol. in strong mineral acids, SO 2 +Aq, KOH+Aq, and Na. 4 P 2 O 7 +Aq. (Schwarzenberg, A. 65. 149.) Insol. in Na 4 P 2 O 7 +Aq. (Stromeyer.) Chromic potassium phosphate, Cr 2 O 3 , K 2 O, 2P 2 O 6 . Insol. in H 2 O and in acids. (Ouvrard, A. ch. (6) 16. 289.) Chromic potassium p^/rophosphate, K(CrP 2 O 7 )+5H 2 O. SI. sol. in cold H 2 O. Decomp. by boiling H 2 O. (Rosenheim, B. 1915, 48. 586.) Cr 2 K 2 H 4 (P 2 O 7 ) 3 . Insol. in H 2 O, acids, or alkalies. SI. decomp. by boiling cone. H 2 SO 4 . (Schjerning, J. pr. (2) 45. 515.) Chromic silver phosphate, 2Cr 2 O 3 , 2Ag 2 O, 5P 2 O 5 . (Hautefeuille and Margottet, C. R. 96. 1142.) Chromic sodium or^ophosphate, Na 2 HPO 4 , 2CrPO 4 +5H 2 O. Decomp. by H 2 O. (Cohen, J. Am. Chem. Soc. 1907, 29. 1197.) Chromic sodium p/rophosphate, Cr 2 Na 2 (P 2 O 7 ) 2 . Insol. in acids. (Wallroth, Bull. Soc. (2) 39. 316.) + 10H 2 O, and 16H 2 O. SI. sol. in cold H 2 O. Decomp. by boiling H 2 O. (Rosenheim, B. 1915, 48. 586.) Cobaltous raorcoraetaphosphate, Co(PO 3 ) 2 (?). Insol. in H 2 O and dil. acids. Sol. in cone. HCl+Aq. (Maddrell, A. 58. 61.) 690 PHOSPHATE, COBALTOUS Cobaltous dimetaphosphate, Co2(P 2 O 6 )2. Insol. in cold cone. H 2 SO 4 ; si. sol. on warming, but sol. in H 2 O after treating with H 2 SO 4 . Sol. in cone. NH 4 OH+Aq. Scarcely attacked by boiling Na 2 S+Aq. (Fleitmann.) Cobaltous hexametaphosphate (?). Ppt. Sol. in sodium hexametaphosphate + Aq. (Rose, Pogg. 76. 4.) Cobaltous orthophosphate i Co 3 (PO 4 ) 2 + zH 2 O. Sol. in H 3 PO 4 +Aq or NH 4 OH+Aq; si. sol. in NH 4 C1 or NH 4 NO 3 +Aq. (Salvetat, C. R. 48. 295.) Sol. in Co salts +Aq. +2H 2 O. (Debray, A. ch. (3) 61. 438.) +8H 2 O. (Reynoso, C. R. 34. 795.) Cobaltous hydrogen orthophosphate. Ppt. (Debray.) +2^H 2 O. Ppt. Insol. in H 2 O. Sol. in H 3 PO 4 +Aq. (Bodeker, A. 94. 357.) Cobaltous telrahydrogen. orthophosphate, CoH 4 (P0 4 ) 2 Sol. in H 2 O. (Reynoso.) Cobaltous pyrophosphate. . Ppt. Sol. in Na 4 P 2 O 7 +Aq. (Stromeyer.) Sol. in NH 4 OH+Aq. (Schwarzenberg.) Cobaltous pyrometaphosphate, 3CoO, 2P 2 O 5 . (Braun.) 6CoO, 5P 2 O 5 . (Braun.) Cobaltous potassium phosphate, CoKPO 4 . Insol. in H 2 O; easily sol. in dil. acids. (Ouvrard, C. R. 106. 1729.) 3CoO, 3K 2 O, 2P 2 O 5 . As above. Cobaltous sodium ^'phosphate, NaCo 2 P 3 Oi . (Schwarz, Z. anorg. 1895, 9. 260.) Na 3 CoP 3 Oio+12H 2 O. Very sol. in H 2 O; decomp. in aq. solution. Sol. in acids. (Schwarz, Z. anorg. 1895, 9. 258.) . Cobaltous sodium raetaphosphate. Co 3 Na 2 (P0 3 )8. Insol. in H 2 O or acids, even cone. H 2 SO 4 . (Watts' Diet.) Cobaltous sodium worwwietaphosphate, 6Co(PO 3 ) 2 , 2NaPO 3 . Insol. in H 2 O and dil. acids. Sol. in cone. H 2 SO 4 . (Maddrell, A. 61. 57.) Cobaltous sodium Jnraetophosphate. CoNa. 1 (PO 3 ) 3 +8H 2 O. Sol. in H 2 O. (Fleitmann and Henneberg, A. 65. 315.) Cobaltous sodium orthophosphate, CoNaPO 4 . Insol. in H 2 O. (Ouvrard, C. R. 106. 1729.) Co 3 (PO 4 ) 2 , 2Na 2 HPO 4 +8H 2 O. (Debray, J. Pharm. (3) 46. 119.) Cobaltous sodium pyrophosphate, Co 10 Nai6(P 2 O 7 )9. Insol. in H 2 O. Sol. in acids. (Wallroth.) +zHoO. Sol. in H 2 O. (Stromeyer.) Cobaltous zinc phosphate, Co 3 (PO 4 ) 2 , 3Zn 3 (PO 4 ) 2 + 12H 2 O. Ppt. Sol. in acids. (Gentele.) CoZn 2 (PO 4 ) 2 +6H 2 O. Insol. in H 2 O. Columbium phosphate (?) Insol. in H 2 O. (Blomstrand.) Cupric diraetaphosphate, Cu 2 (P 2 O 6 ) 2 . Insol. in H 2 O. Sol. in cone. H 2 SO 4 . (Mad- drell, A. 61. 62.) Insol. in most cone, acids and in alkalies, except hot NH 4 OH+Aq or cone. H9SO 4 , in which it is moderately sol. Not decomp. by H 2 S, but by (NH 4 ) 2 S+Aq, less easily by Na 2 S, and K 2 S-j-Aq. (Fleit- mann, Pogg. 78. 242.) +8H 2 O. Completely insol. in H 2 O. (Fleit- mann.) Cupric /lezametophosphate (?). Sol. in Na 8 P 6 O 18 +Aq or CuCl 2 +Aq. (Rose, Pogg. 76. 5.) Cu 3 P 6 O l8 . Easily sol. in H 2 O or acids, especially when freshly pptd. (Liidert, Z. anorg. 5. 15.) Cupric orthophosphate. basic, 6CuO. P 2 O 5 + 3H 2 0. Min. Phosphocalcite. 5CuO, P 2 O 5 +2H 2 O. Min. Dihydrite. +3H 2 O. Min. Ehlite. Easily sol. in NH 4 OH+Aq, and HNO 3 +Aq. 4 CuO, P 2 O 5 +H 2 O. Slowly sol. in NH 4 OH or (NH 4 ) 2 CO 3 +Aq; insol. in" cold Na 2 S 2 O 3 + Aq. (Steinschneider, C. C. 1891, II. 51.) SI. sol. in CuCl 2 +Aq and CaSp 4 +Aq Decomp. by boiling H 2 O and boiling Aq potash. (Caven, J. Soc, Chem. Ind. 1897, 16. 29.) Min. Inbethenite. Sol. in acids and NH 4 OH+Aq. +2H.O. Min. Pseudolibethenite. Sol. in acids and NH 4 OH+Aq. +3H 2 O. Min. Tagilite. Sol. in acids and NH 4 OH+Aq. Cupric ^nphosphate, 5CuO, 3P 2 O 5 + 13H 2 O. Sol. in H 2 O. Sol. in HNO 3 . (Schwarz, Z. anorg. 1895, 9. 262.) Cupric dimetaphosphate t CuP 2 O 6 +4H 2 O. Sol. in 78 pts. H 2 O. Easily decomp. by hot cone. H 2 SO 4 . (Glatzel, Dissert. 1880.) PHOSPHATE, CUPRIC URANYL 691 Cupric /n'wetaphosphate, C Very si. sol. in H 2 O (0.04 g. in 1 1. at 20) (Tammann, J. pr. 1S92, (2) 45. 425.) Cupric tetrametaphosphsite, Cii2P4Oi2. Insol. in H 2 O and in HC1. SI. sol. in boiling HNO 3 . Very sol. in boiling cone. H 2 SO 4 (Glatzel.) -f8H 2 O. Nearly insol. in H 2 O. Slowly attacked by acids except cone. H 2 SO 4 (Glatzel.) Cupric ortfiophosphate, Cu 3 (PO 4 ) 2 +3H 2 O. Insol. in H 2 O; easily sol. in acids, even H 3 PO 4 , HC 2 H 3 O 2 , or H 2 SO 3 +Aq. Sol. in NH 4 OH+Aq. SI. sol. in NH 4 salts +Aq. SI. sol. in Cu salts +Aq. (Rose, Pogg. 76. 25.) Sol. in cold Na 2 S 2 O 3 +Aq. (Steinschnei- der, C. C. 1891, II, 51.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 827.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Cupric hydrogen phosphate, CuHPO 4 + Insol. in H 2 O; sol. in H 3 PO 4 +Aq, and HC 2 H 3 O 2 +Aq. Insol. in NH 4 C1, and NH 4 NO 3 +Aq. (Brett, Phil. Mag. (3) 10. 98.) Cupric p?/rophosphate, basic. Cu 2 P 2 O 7 , 2CuO, H 2 O+3H 2 O. Insol. in H 2 O. (Pahl, J. B. 1873. 229.) Cupric pj/rophosphate, Cu 2 P 2 O 7 . Anhydrous. Insol. in H 2 O, and very si. sol. in cone, acids. (Fleitmann, Pogg 78. 244.) As insol. as Cu metaphosphate, but de- comp. by H 2 S. (Rose, Pogg. 76. 14.) +2H 2 O. Sol. in mineral acids, and NH 4 OH +Aq; also in Na 4 F 2 O 7 +Aq. (Sehwarzen- berg, A. 66. 156.) Sol. in cold H 2 SO 3 -j-Aq without decomp., crystallizing out on boiling. Decomp. by boiling KOH+Aq. Sol. in large excess of CuSO 4 +Aq. +2^H 2 O. (Pahl, Sv. V. A. F. 30, 7. 40.) -f5H 2 O. Very si. sol. in H 2 O. Sol. in dil. acids. (Wiesler, Z. anorg. 1901, 28. 202.) Cupric iron (ferric) pz/rophosphate, Cu 3 Fe 2 (P 2 O 7 ) 3 + 12H 2 O. Ppt. (Pascal, C. R. 1908, 146. 2.33.) Cupric potassium phosphate, 4CuO, K 2 O, 3P 2 O.5. Insol. in H 2 O. COuvrard, C. R. 111. 177.) CuKPO 4 . As above. Cupric potassium teft*ametaphosphate, K 2 CuP 4 O 12 +4H 2 O. Sol. in 58 pts. H 2 O. Easily attacked by acids'. (Glatzel, Dissert. 1880.) Cupric potassium pyrophosphate, CuK 2 P 2 O 7 . Extremely easily sol. in H 2 O. (Persoz, A. ch. (3) 20. 315.) Cu 2 P 2 O 7 , 3K 4 P 2 O 7 +4H 2 O. Insol. in H 2 O. (Pahl, Sv. V. A. F. 30, 7. 44.) Cupric sodium phosphate, Cu 3 Na 6 (PO 4 ) 4 . Insol. in HC 2 H 3 O 2 +Aq. Sol. in cone. acids. (Wallroth, Bull. Soc. (2) 39. 316.) Cupric sodium inphosphate, CuXa 3 P 3 Oio+12H 2 O. SI. sol. in H 2 O; very unstable. Easily sol. in acids. (Stange, Z. anorg. 1896, 12. 458.) Cupric sodium tetrametaphosphate, CuNa 2 P 4 Oi 2 . As insol. in H 2 O as Cu dimetaphosphate. Difficultly decomp. by digestion with Na 2 S-f Aq. (Fleitmann, Pogg. 78. 355.) +4H 2 O. Sol. in 45 pts. H 2 O. (Glatzel, Dissert. 1880.) Cupric sodium or^Aophosphate, 3Cu 3 (PO 4 ) 2 , NaH 2 PO 4 . Decomp. by H 2 O to 4CuO, P 2 O 5 . (Stein- schneider, C. C. 1891, II. 52.) 2Cu 3 (PO 4 ) 2 , Na 2 HPO 4 . Decomp. by H 2 O into 3Cu 3 (PO 4 ) 2 , Na 2 HPO 4 . Decomp. by H 2 O. (S.) Cu 3 (PO 4 ) 2 , NaH 2 PO 4 . Decomp. by H 2 O. (S.) 6Cu 3 (PO 4 ) 2 , 2Na 3 PO 4 . Decomp. by H 2 O. Cupric sodium p^/rophosphate, CuNa 2 P 2 O 7 . Insol. in H 2 O. (Fleitmann and Henne- berg, A. 65. 387.) + 2 / 3 H 2 O. (F. and H.) Much more sol. than the next salt. (Pahl.) +6H 2 O. (Persoz, A. ch. (3) 20. 315.) Cu 2 P 2 O 7 , CuNa a P 2 O 7 +3^H 2 O. Very ef- florescent; insol. in H 2 O. (F. and H.) + 10^H 2 O. (Pahl, Sv. V. A. F. 30, 7. 42. CuNa 2 P 2 O 7 , Na 4 P 2 O 7 . Sol. in H 2 O. (-F. and H.) +2H 2 O. (F. amd H.) + 12, and 16H 2 O. Very efflorescent, and sol. in H 2 O. (Pahl.) Cu 3 Na 2 P 4 Oi 4 +10H 2 O. Insol. in H 2 O; sol. in HC1 and HNO 3 even after heating. (Stange, Z. anorg. 1896, 12. 456.) Cupric uranyl phosphate, (UO 2 ) 2 Cu(PO 4 ) 2 + 8H 2 O. Insol. in H 2 O; easily sol. in acids. (De- Dray.) Min. Chalcolite. Sol. in HNO 3 +Aq. 692 PHOSPHATE, CUPRIC, AMMONIA Cupric orthophosphate ammonia, Cu 3 (PO 4 ) 2 , 4NH 3 . SI. sol. in H 2 O. Easily sol. in H 2 O contain- ing NH 4 OH. (Schiff, A. 123. 41.) 2CuO, 3P 2 O 5 , 20NH 3 +21H 2 O. Easily sol. in cold H 2 O, with subsequent decomp. (Metzner, A. 149. 66.) 2CuO, P 2 O 5 , 6NH 3 . (Maumene\) Cupric p/rophosphate ammonia, SCuO, 3P 2 O 5 , 4NH 3 +4H 2 O. SI. sol. in H 2 O. (Schwarzenberg, A. 66. 133.) Cu 2 P 2 O 7 , 4NH 3 +H 2 O. SI. sol. in H 2 O. (Schiff, A. 123. 1.) Didymium raetaphosphate, Di(PO 3 ) 3 . Precipitate. (Smith.) Di 2 O 3 , 5P 2 O 5 . Insol. in H 2 O. (Cleve.) Didymium phosphate, 2Di 2 O 3 , 3P 2 O 5 . Insol. in H 2 O. (Ouvrard, C. R. 107. 37.) Didymium or^ophosphate, DiPO 4 . Insol. in H 2 O. Very si. sol. in dil., easily sol. in cone, acids. (Marignac.) Insol. in H 2 O. (Wallroth, Bull. Soc. (2) 39. 316.) +H 2 O. (Frerichs and Smith, A. 191. 355.) Didymium ^nhydrogen phosphate, Di 2 H 3 (P0 4 ) 3 . Precipitate. (Frerichs and Smith.) Existence is doubtful. (Cleve,B. 12. 910.) Didymium hexahydrogen phosphate, DiH 3 (PO 4 ) 2 +H 2 O. Precipitate. (Hermann.) Didymium pyrophosphate, Di 4 (P 2 O 7 ) 3 -f 6H 2 O. Precipitate. (Cleve.) Didymium hydrogen pz/rophosphate, Di 2 H 6 (P 2 O 7 ) 3 . Precipitate. Sol. in disodium pyrophos- phate+Aq. (Frerichs and Smith, A. 191. 355.) Does not exist. (Cleve.) Didymium potassium phosphate, 2Di 2 O 3 , 3K 2 O, 3P 2 O 6 = 2DiPO 4 , K 3 PO 4 . Insol. in H 2 O. (Ouvrard, C. R. 107. 37.) Didymium sodium ortAophosphate, Di 2 O 3 , 3Na 2 O, 2P 2 O 8 = DiPO 4 , Na 3 PO 4 . Insol. in H 2 O. (Ouvrard.) Didymium sodium p?/rophosphate, Di 2 O 3 , Na 2 O, 2P 2 O 5 = DiNaP 2 O 7 . Insol. in H 2 O. (Ouvrard, C. R. 107. 37.) Dysprosium orf/iophosphate, DyPO 4 +5H 2 O. Nearly insol. in H 2 O. Easily sol. in dil. acids or acetic acid. (Jantsch, B. 1911, 44. 1276.) Erbium phosphate, ErPO 4 +H 2 O. Precipitate. Erbium p?/rophosphate, ErHP 2 O 7 +3KH 2 O. Scarcely sol. in boiling H 2 O. Slowly sol. in acids. Erbium sodium p?/r0phosphate, ErNaP 2 O 7 . Precipitate. ^Wallroth.) Glucinum metophosphate, G1(PO 3 ) 2 . Insol. in H 2 O ana acids. (Bleyer, Z. anorg. 1912, 79. 274. Glucinum or^ophosphate, basic. 2G1 3 P 2 O 8 , G1O + 13H 2 O. Ppt. (Bleyer, Z. anorg. 1912, 79. 268.) Glucinum ort/iophosphate, G1 3 (PO 4 ) 2 +6H 2 O. Precipitate. Insol. in H 2 O. Sol. in acids. (Atterberg, Sv. V. A. Handl. 12, 6. 33.) 1 1. 2% HC 2 H 3 O 2 +Aq dissolves 0.55 g. of the anhydrous salt; 1 1. 10% HC 2 H 3 O 2 +Aq dissolves 1.725 g. (Sestini, Gazz. ch. it. 20. 313.) +7H 2 O. (Atterberg.) Glucinum hydrogen or^ophosphate, G1HPO 4 +3H 2 0. G1H 4 (PO 4 ) 2 hydroscopic. (Bleyer, Z. anorg. 1912, 79. 266.) Precipitated by alcohol. (Atterberg.) Glucinum phosphate, 5G1O, 2P 2 O 5 +8H 2 O. Ppt. Sol. in H 2 O with decomp. (Scheffer.) 3G1O, P 2 O 5 , 3H 2 O+H 2 O. (Sestini, Ga/z. ch. it. 20. 313.) Glucinum p?/rophosphate, G1 2 P 2 7 +5H 2 O. Precipitate. (Scheffer.) Sol. in Na 4 P 2 O 7 +Aq. (Stromeyer.) Glucinum potassium phosphate, G1KPO 4 . Insol. in H 2 O. (Ouvrard, C. R. 110. 1333.) Glucinum sodium phosphate, GlNaPO 4 . SI. sol. in cold, easily sol. in hot acids. (Wallroth.) Insol. in acetic acid. Min. Beryllonite. G1O, 2Na 2 O, P 2 O 5 . Insol. in H 2 O. (Ouv- rard, C. R. 110. 1333.) Gold (Auric) sodium pT/rophosphate (?), Au 4 (P 2 O 7 ) 3 , 2Na 4 P 2 O 7 4-H 2 O. Sol.inH 2 O. (Persoz.) PHOSPHATE, IRON 693 Gold sodium pyrophosphate, ammonia, 14Au 2 O s , 6P 2 O S , 3Na 2 O, 14NH 3 +24H 2 O. Insol. in H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 172.) Iron (ferrous) inmetophosphate, Fe(P 3 O 9 ) 3 + 12H 2 O. Rather si. sr>l. in cold, more easily in hot H 2 O. After ignition sol. in HCl+Aq only after long boiling. (Liridbom, Acta Lund. 1873. 17.) Ferrous hexametaphosphate, Fe 3 P 6 Oi 8 . When freshly pptd. is sol. in H 2 O, and very sol. in least traces of acids, or Na 6 P 6 Oi 8 +Aq. (Liidert, Z. anorg. 5. 15.) Ferrous phosphate, basic, 7FeO, 2P 2 O 5 + 9H 2 O. Min. Ludlamite. Sol. in dil. H 2 SO4 or HCl+Aq. Decomp. by boiling KOH or NaOH+Aq. Ferrous orZAophosphate, Fe 3 (PO 4 ) 2 . Insol. in H 2 O; sol. in acids. Sol. in 1000 pts. H 2 O containing more than 1 vol. CO 2 . (Pierre.) Sol. in an excess of ferrous salts +Aq. Sol. in 560 pts. H 2 O containing V 56 o pt. HC 2 H 3 O 2 . Sol. in 1666 pts. H 2 O containing 150 pts. NH 4 CoH 3 O 2 . (Pierre, A. ch. (3) 36. 78.) Sol. in NH 4 salts +Aq. Sol. in NH 4 OH+Aq. Not pptd. in pres- ence of Na citrate. Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +H 2 O. (Debray, A. ch. (3) 61. 437.) +8H 2 O. Min. Vivianite. Easily sol. in HC1 or HNOs+Aq. Boiling KOH+Aq dis- solves out phosphoric acid. Sol. in cold citric acid+Aq. (Bolton, C. N. 37. 14.) Insol. in H 2 O. Sol. in acids. (Evans, C. C. 1897, I. 580.) Ferrous hydrogen or^ophosphate, FeHPO 4 + H 2 O. Ppt. (Debray, A. ch. (3) 61. 437.) Is impure Fe 3 (PO 4 ) 2 . (Erlenmeyer and Heinrichs, A. 194. 176.) Ferrous tetrahydrogen or^Aophosphate, FeH 4 (P0 4 ) 2 +H 2 0. Easily sol. in H 2 O. Not changed by al- cohol. (Erlenmever and Heinrichs, A. 194. 176.) Ferrous p^/rophosphate. Ppt. Sol. in an excess of Na 4 P 2 O 7 or FeSO 4 +Aq. (Schwarzenberg, A. 65. 153.) Ferric 7wetophosphate, Fe 3 (PO 3 ) 6 or Fe(PO 3 ) 3 . Insol. in H 2 O or dil. acids. Sol. in cone. H 2 SO 4 . (Maddrell, Phil. Mag. (3) 30. 322.) Iron (ferric) orthophosphate, basic, 2Fe 2 O 3 , P 2 O 5 +zH 2 O. Insol. in NH 4 citrate, sol. in NH 4 tartrate +Aq. (Wittstein.) +3H-X). Min. Krauri'.e. Easily sol. in HCl+A~q. +4H 2 O. Ppt. (Millot, C. R. 82. 89.) +5H 2 O. Min. Dufrenite. + 12H 2 O. Min. Cacoxene. Sol. in HC1 + Aq. + 18, or 24H 2 O. Min. Delvauxite. 5Fe 2 O 3 , 3P,O d + 14H 2 O. Min. Beraunile. Sol. in HCl+Aq. 3Fe 2 O 3 , 2P 2 O 5 +8H 2 O. Min. Eleonorite. Sol. in HCl+Aq. Ferric ortfiophosphate, Fe 2 (PO 4 ) 2 +:rH 2 O, or 2Fe 2 O 3 , 3P 2 5 +zH 2 O. +4, or 8H 2 O. (Pptd. ferric phosphate.) Insol. in H 2 O. Sol. in 1500 pts. boiling H 2 O. (Bergmann, 1815.) Sol. in pure H 2 O when all traces of soluble salts are absent. (Frese- nius.) Very si. sol. in, but decomp. by H 2 O. (LachowiczJ W. A. B. 101, 2b. 374.) For an extended discussion of solubility in and de- composition by H 2 O and effect of salts see Cameron and Hurst, (J. Am. Chem. Soc. 1904, 26. 888.) Easily sol. in dil. mineral acids, excepting H 3 PO 4 +Aq. Insol. in cold HC 2 H 3 O 2 +Aq. (Wittstein.) 100 ccm. cold H 2 O containing 10% HC 2 H 3 O 2 dissolve 0.007 g. salt. (Ses- tini, Gazz. ch. it. 5. 252.) When freshly pptd. easily sol. in H 2 SO 3 +Aq, or (NH 4 ) 2 SO 3 +Aq. (Berthier.) Easily sol. in tartaric or citric acid+Aq, also in NH 4 salts of those acids, and Na citrate+Aq. (Heydenreich, C. N. 4. 158.) See below. Sol. in 12,500 pts. H 2 O sat. with CO 2 . (Pierre, A. ch. (3) 36. 78.) Insol. in NH 4 salts +Aq. (Wittstein.) Sol. in NH 4 OH+Aq in presence of Na 2 HPO 4 ; insol. in hot Na 2 HPO 4 +Aq; sol. in (NH 4 ) 2 CO 8 +Aq (Berzelius). NH 4 OH, KOH, or NaOH+Aq dissolve out H 3 PO 4 . Sol. in ferric salts +Aq, even ferric acetate, but insol. in ferrous acetate+Aq. Partially sol. in large amt. of Na 2 CO 3 +Aq. Not pptd. in presence of Na citrate. (Spiller.) Arth (Bull. Soc. (3) 2. 324) obtained a modification of Fe 2 (PO 4 ) 2 , insol. in HNO 3 + Aq, but sol. in hot cone. HCl+Aq. +4H 2 O. Min. Strengite. Easily sol. in HCl+Aq; insol. in HNO 3 +Aq. +5H 2 O. Only si. sol. in H 2 O. Slowly sol. in HNO 3 , easily sol. in HC1. (Weinland, Z anorg. 1913, 84. 361.) Diammonium citrate +Aq dissolves 4.8% of the P 2 O 5 ; triammonium citrate, 5.8% P 2 O 6 ; and with an excess of NH 4 OH, 21.2% P 2 O 6 is dissolved. (Erlenmej^er, B. 14. 1253.) +9H 2 O. Dissolves in 35 min. in diam- mpnium citrate +Aq (sp. gr. 1.09); in 55 mm. in triammonium citrate +Aq (sp. gr. Q ( 1 A% citric acid) dis- solves 17.5% of the P 2 O 5 . (Erlenmeyer, I. c.} 1.09); citric acid +Aq ( l /i% citric acic 694 PHOSPHATE, IRON, ACID Iron (ferric) phosphate, acid, 8Fe 2 O 3 , 9P 2 O 5 +3H 2 O. Insol. in H 2 O. (Riimpler, Z. anal. 12. 151.) 6Fe 2 O 3 , 7P 2 O 5 +3H 2 O. 4Fe 2 O 3 , 5P 2 O 5 +3H 2 O. 2Fe 2 O 3 , 3P 2 O 5 +8H 2 O. Ppt. Decomp. by H 2 O finally into Fe 2 (PO 4 ) 2 . (Erlenmeyer and Heinrich, A. 194. 176.) 8Fe 2 O 3 , 11P 2 O 5 +9H 2 O. As above. (E. and H.) 4Fe 2 O 3 , 7P 2 O 5 +9H 2 O. As above. (E. and H.) Fe 2 O 3 , 2P 2 O 5 +8H 2 O. Insol. in H 2 O or HC 2 H 3 O 2 +Aq; sol. in NH 4 citrate, alkali hydrates, or carbonates +Aq. (Winkler.) Slowly decomp. by H 2 O. (E. and H.) + 10H 2 O. (Waine, C. N. 36. 132.) 2Fe 2 O 3 , 5P 2 O 5 + 17H 2 O. Fe 2 O 3 , 3P 2 O 5 +6H 2 O = FeH (PO 4 ) 3 . Deli- quescent. Insol. in H 2 O, but decomp. into Fe 2 (PO 4 ) 2 . (E. andH.) +4H 2 O. (Hautefeuille and Margottet, C. R. 106. 135.) Ferric pz/rophosphate, Fe 4 (P 2 O 7 ) 3 . Two modifications. (a) Sol. in acids, Na 4 P 2 O 7 +Aq, FeCl 3 +Aq, NH 4 OH+Aq, and in (NH 4 ) 2 CO 3 +Aq. Insol. in acetic, sulphurous acid, or NH 4 C1 +Aq. Sol. in NH 4 citrate+Aq. (Schwarzen- berg, A. 65. 153.) (6) Insol. in dil. acids, Na 4 P 2 O 7 +Aq, FeCl 3 +Aq. Sol. in IsH 4 OH+Aq. (Gladstone, Chem. Soc. (2) 6. 435.) Solubility of Fe 4 (P 2 O 7 ) 3 in NH 4 OH+Aq at 0. 100 g. sat. solution contain 100 g. sat. solution contain G. NH 3 G. Fe4(P 2 07)3 G. NHs G.Fe4(P 2 O7) 3 0.884 1.59 3.71 4.72 5.93 7.91 5.606 9.75 14.85 15.94 13.92 14.61 5.92 8.26 10.55 15.96 18.83 14.71 13.89 7.40 2.52 0.445 (Pascal, A. ch. 1909, (8) 16. 374.) Insol. in acetone. (Krug and M'Elroy, J. Anal. Appl. Ch. 6. 184.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.). Ferroferric or^/iophosphate, 2Fe 3 (PO 4 ) 2 , 3(Fe*O 3 , 2P 2 O 5 ) + 16H 2 O. Ppt. Sol. in HCl+Aq. (Rammelsberg.) 4Fe 2 O 3 , 6FeO, 5P 2 O 5 +40H 2 O. Sol. in' 40 min. in diammonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq (sp. gr. = 1.09) dissolves 55.7% of the P 2 O 6 . (Erlen- meyer, B. 14. 1253.) Ferrous lithium phosphate, Li 3 PO 4 , Fe 3 (PO 4 ) 2 . Min. Triphylline. Easily sol. in acids; not wholly decomp. by KOH+Aq. Iron (ferrous) manganous phosphate, Fe 3 (PO 4 ) 2 , Mn 3 (PO 4 ) 2 . Min. Triplite. Easily sol. in HCl+Aq. 5(Mn,Fe)O, 2P 2 O 5 +5H 2 O. Min. Hur- eaulite. Sol. in acids. Ferric manganous sodium phosphate, FePO 4 , (Na 2 ,Mn) 3 PO 4 +}^H 2 O. Min. (?). Ferrous manganous phosphate chloride, 3(Mn,Fe) 3 (PO 4 ) 2 , MnCl 2 . (Deville and Caron.) Ferrous manganous phosphate fluoride, (Mn,Fe) s (PO 4 ) 2 , (Mn,Fe)F 2 . Min. Triplite, Zwielesite. Sol. in HCl+Aq. 3(Mn,Fe) 3 (PO 4 ) 2 , MnF 2 . (Deville and Caron, C. R, 47. 985.) Ferric potassium phosphate, 2Fe 2 O 3 , 3K 2 O, 3P 2 5 . Not attacked by boiling H 2 O. (Ouvrard, A. ch. (6) 16. 289.) Fe 2 O 3 , K 2 O, 2P 2 O 5 . Insol. in H 2 O; very si. attacked by acids. (Ouvrard.) Ferric silver wetophosphate, 2Fe 2 O 3 , 2Ag 2 0, 5P 2 O 5 . (Hautefeuille and Margottet, C. R. 96. 1142.) Ferric silver p?/rophosphate, Fe 2 Ag 6 (P 2 O 7 ) 3 + 4H 2 O. Ppt. (Pascal, C. R. 1908, 146. 232.) Ferric sodium phosphate, 2P"e 2 O 3 , 3Na 2 O, 3P 2 5 . Decomp. by H 2 O. (Ouvrard.) Ferrous sodium /n'phosphate, FeNa 3 P 3 Oio+ Stable dry; sol. in HNO 3 : decomp. in con- tact with H,O. (Stange, Z. anorg. 1896, 12. 451.) Ferric sodium hydrogen Fe(PO 4 ) 2 H 2 Na+H 2 O. or^ophosphate, Difficultly sol. in H 2 O. Slowly decomp. by boiling with H 2 O. Sol. in dil. HC1 and dil. HNO 3 . Decomp. by alkalies and alkali car- bonates. (Weinland, Z. anorg. 1913, 84. 354.) Fe(PO 4 ) 3 H 5 Na+H 2 O. Difficultly sol. in H 2 O. Decomp. by boiling with H 2 O. Sol. in dil. HC1 and in dih HNO 3 . Decomp. by al- kalies and alkali carbonates. (Weinland, Z. anorg. 1913, 84. 358.) Ferric sodium p?/rophosphate, Fe 4 (P 2 O 7 ) 3 , 2Na 4 P 2 7 +7H 2 Slowly but completely sol. in H 2 O. Pptd. by alcohol. (Milck, J. B. 1865. 263.) Very sol. in H 2 O. (Fleitmann and Henne- berg.) PHOSPHATE, LEAD SODIUM 695 +5, and 6H 2 O. Easily sol. in H 2 O, espe- cially if warm. (Pahl, J. B. 1873. 229.) FeNaP 2 O 7 . Insol. in H 2 O, dil. HC1, or HNOa+Aq; si. sol. in cone. HCl+Aq; de- comp. by cone, hot H 2 SO 4 without solution. (Jorgensen, J. pr. (2) 16. 342.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Na6Fe 2 (P 2 O 7 ) 3 +9H 2 O. Decomp. by H 2 O. (Rosenheim, B. 1915, 48. 586.) Fe 4 (P 2 O 7 ) 3 , 5Na 4 P 2 O 7 +7H 2 O. (Pahl, J. B. 1873. 229.) Iron (ferric) phosphate sulphate, 3Fe 2 (PO 4 ) 2 , 2Fe 2 (SO 4 ) 3 , 2Fe 2 O 6 H 6 . Min. Diaochite. Lanthanum raetaphosphate, La 2 (PO 3 )6. Precipitate. (Frerichs and Smith.) La 2 O 3 , 5P 2 O 5 . Insol. in H 2 O, dil., or cone. acids. (Johnsson, B. 22. 976.) Lanthanum or/iophosphate, LaPO 4 . Precipitate. (Hermann.) Insol. in H 2 O and acids. (Ouvrard, C. R. 107. 37.) Lanthanum hydrogen phosphate, La 2 H 3 (P0 4 ) 3 . Precipitate. (Frerichs, B. 7. 799.) Existence is doubtful. (Cleve, B. 11. 910.) Lanthanum phosphate, acid, La 2 O 3 , 2P 2 O 5 . Precipitate. (Hermann.) Lanthanum p?/rophosphate, LaHP 2 O 7 +3H 2 O. (Cleve.) La 2 H 6 (P 2 O 7 ) 3 . Precipitate. (Frerichs and Smith.) Does not exist. (Cleve.) Lanthanum potassium or//iophosphate, 2La 2 O 3 , 3K 2 O, 3P 2 O 5 = 2LaPO 4 , K 3 PO 4 . Insol. in H 2 O. (Ouvrard, C. R. 107. 37.) Lanthanum sodium ort/iophosphate, La 2 O 3 , 3Na 2 O, 2P 2 O 5 . Insol. in H^O. (Ouvrard.) Lanthanum sodium p?/rophosphate, LaNaP 2 O 7 . Insol. in acetic, and dil. cold mineral acids. Sol. in warm dil. acids. fWallroth.) Lead dirae/aphosphate, Ppt. Almost insol. in H 2 O. Sol. in HNO 3 +Aq. (Fleitmann, Pogg. 78. 253.) Lead inwetophosphate, Pb 3 (P 3 O 9 ) 2 +3H 2 O. Nearly insol. in H 2 O. Less sol. in H 2 O than the corresponding Ag salt. (Fleitmann and Henneberg, A. 66. 304.) Most insol. of the tfnmetaphosphates. (Lindbom, Acta Lund. 1873. 12.) Anhydrous salt is insol. in H 2 O; easily sol. in HNO 3 +Aq. (Lindbom.) Lead fe^rametophosphate, Insol. in H 2 O. More easily decomp. by acids than the other insol. metaphosphates. Easily decomp. by alkali hydrosulphides+Aq in the cold. (Fleitmann, Pogg. 78. 353.) Lead hexametaphosphate, PbsPeOis. Nearly insol. in H 2 O; sol. in acids. (Lii- dert, Z. anorg. 5. 15.) Lead or/ftophosphate, basic, 4PbO, P 2 O 5 . (Gerhardt, A. 72. 85.) Lead or/Aophosphate, Pb 3 (PO 4 ) 2 . Insol. in H 2 O; sol. in HNO 3 +Aq. Insol. in HC 2 H 3 O 2 +Aq. SI. sol. in H 2 O. 1.35 X10- 4 g. is contained in 1 litre of sat. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 604.) Not hvdrolyzed by boiling H 2 O. Sol. in boiling KOH+Aq; insol. in NH 4 OH+Aq. Insol. in Pb(NO 3 ) 2 +Aq. (Caven, J. Soc. Chem. Ind. 1897, 16. 30.) Sol. in 782.9 pts. HC 2 H 3 O 2 +Aq containing 38.94 pts. pure HC 2 H 3 O 2 . (Bertrand, Monit. Scient. (3) 10. 477.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Lead hydrogen phosphate, PbHPO 4 . Insol. in H 2 O. Decomp. by H 2 SO 4 , or HC1 +Aq. Sol. in HNO 5 , or in KOH or NaOH+ Aq. Insol. in HC 2 H 3 O 2 +Aq. Sol. in cold NH 4 Cl+Aq (Brett), from which it can be completely precipitated by a great excess of NH 4 OH+Aq. More sol. in NH 4 C 2 H 3 O 2 +Aq at 18.8-25 than in pure H 2 O. (Wappen.) Sol. in sat. NaCl+Aq, but less than PbSO 4 . (Becquerel, C. R. 20. 1524.) Insol. in Pb salts +Aq. Not pptd. in presence of Na citrate (Spiller.) Lead pyrophosphate, Pb 2 P 2 O 7 +H 2 O. Insol. in H 2 O. Sol. in HNO 3 , or KOH+Aq. Insol. in NH 4 OH+Aq, HC 2 H 3 O 2 , or SO 2 + Aq. (Schwarzenberg, A. 65. 133.) Sol. in Na 4 P 2 O 7 +Aq. (Stromeyer.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Lead potassium phosphate, PbKPO 4 . Decomp. by hot H 2 O. (Ouvrard, C. R. 110. 1333.) Lead sodium phosphate, PbNaPO 4 . Very sol. in dil. acids. (Ouvrard, C. R. 110. 1333.) lOPbO, 8Na 2 O, 9P 2 O 5 . (Ouvrard.) 696 PHOSPHATE, LEAD SODIUM Lead sodium pyrophosphate, PbNa 2 P2O 7 . Insol. in hot H 2 O. (Gerhardt, A. ch. (3) 22. 506.) Lead Znphosphate sodium pyrophosphate, Pb 5 INa 4 P 8 O 27 + 10H 2 O. Sol. in HNO 3 after melting. (Stange, Z. anorg. 1896, 12. 459.) Lead phosphate chloride, 2PbHPO 4 , PbCl 2 . Insol. in boiling H 2 O; sol. in dil. HNO 3 + Aq. (Gerhardt, A. ch. (3) 22. 505.) 2Pb 3 (PO 4 ) 2 , PbCl 2 . Ppt. (Heintz, Pogg. 73. 119.) 3Pb 3 (PO 4 ) 2 , PbCl 2 . Min. Pyromorphite. Sol. in HNO 3 , and KOH+Aq. SI. sol. in cold citric acid+Aq. (Bolton, C. N. 37. 14.) +H 2 O. Insol. in H 2 O. Sol. in dil. HNO 3 +Aq. (Heintz.) Lithium metophosphate, LiPO 3 . Insol. in boiling H 2 O. Scarcely sol. in acetic acid. Easily sol. in mineral acids. (Merling, Z. anal. 1879, 18. 565.) Lithium te^raraetaphosphate, Li 4 P 4 Oi 2 + 4H 2 0. Very sol. in H 2 O. (Warschauer, Z. anorg. 1903, 36. 180.) Lithium or^ophosphate, Li 3 PO 4 . Very slightly sol. in H 2 O. Sol. in 2539 pts. pure H 2 O and 3920 pts. ammoniacal H 2 O; much more readily in H 2 O containing NH 4 salts. Easily sol. in HC1+ Aq or HNO 3 +Aq. (Mayer, A. 98. 193.) Easily sol. in carbonic acid water. (Troost.) Sol. in dil. acids or acetic acid, (de Schulten, Bull. Soc. (3) 1. 479.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) rH 2 O. Lithium hydrogen phosphate, Li 2 HPO 4 . Nearly insol. in H 2 O. (Gmelin.) Sol. in 833 pts."H 2 O at 12. (Rammelsberg.) Li 5 H(PO 4 ) 2 +H 2 O. Sol. in 200 pts. H 2 O. (Rammelsberg.) Lithium dihydrogen phosphate, LiH 2 PO 4 . Deliquescent, and very sol. in H 2 O. (Ram- melsberg.) Heptaliihium cfthydrogen phosphate, Li 7 H 2 (P0 4 ) 3 . + 1H 2 O, or 2H 2 O. Sol. in H 2 O. (Ram- melsberg.) Lithium pentahydrogen phosphate, LiH 5 (PO 4 ) 2 +H 2 O. Deliquescent, and sol. in H 2 O. ,ithium p?/rophosphate, Li 4 P 2 O 7 +2H 2 O. (Rammelsberg, B. A. B. 1883. 21.) Lithium manganous phosphate, Li 3 PO 4 , Mn 3 (PO 4 ) 2 . Min. Lithiophilite. Lithium potassium wetaphosphate, Li 2 O, 2K 2 O, 3P 2 O 5 +4H 2 O. As NH 4 comp. (Tammann, J. pr. 1892, (2) 46. 443.) Lithium potassium pz/rophosphate, Li 3 KP 2 O 7 . (Kraut, A. 1876, 182. 170.) Lithium sodium phosphate, 3Li 2 O, Na 2 O, P 2 5 . Insol. in H 2 O. Sol. in dil. acids. (Ouvrard, C. R. 110. 1333.) 2Li 2 O, Na 2 O, 2P 2 O 5 . As above (Ouvrard.) Lithium sodium pyrophosphate, Li 2 O, Na 2 O, P 2 O . 5Li 2 0, Na 2 O, 3P 2 O 5 . 4Li 2 O, 6Na 2 O, 5P 2 O 5 . (Kraut, "A. 1876, 182. 168.) Magnesium metaphosphate, Mg(PO 3 ) 2 . Insol. in H 2 O or dil. acids, but sol. in H 2 SO 4 +Aq. (Maddrell, A. 61. 62.) Not decomp. by very long digestion with alkali carbonates, or orthophosphates +Aq. (Fleitmann.) Magnesium dimetaphosphate, Mg 2 (P 2 Oe) 2 + 9H 2 0. Insol. in H 2 O; decomp. by acids. (Fleit- mann, Pogg. 78. 259.) Magnesium trimetaph.ospha.te, Mg 3 (P 3 O 9 ) 2 . SI. sol. in cold H 2 O, more easily in hot H 2 O. When ignited, insol. in boiling HCl+Aq. (Lindbom.) Cryst. with 12, or 15H 2 O. Magnesium tetrametaphosphate, Mg 2 P 4 O i2 . Insol. in H 2 O, somewhat sol. in HCl+Aq. More easily sol. in HNO 3 +Aq, especially easily sol. in cone. H 2 SO 4 . (Glatzel, Dissert. 1880.) + 10H 2 O. Sol. in 70 pts. H 2 O. (Glatzel.) Magnesium or^ophosphate, Mg a (PO 4 ) 2 , and +5, or 7H 2 O. 1 litre H 2 O dissolves 0.1 g. ignited Mg 3 (PO 4 ) 2 in 7 days, but 0.205 g. if freshly precipitated. (Volcker, J. B. 1862. 131.) 1 1. H 2 O with 2 g. NaCl dissolves 75.8 mg.; 1 1. H 2 O with 3 g. NaNO 3 dissolves 61.9 mg. Mg 3 (PO 4 ) 2 . (Liebig, A. 106. 185.) Easily sol. in acids, except in acetic acid. (Schaffner, A. 60. 145.) Easily sol. in H 2 O in presence of alkali salts. PHOSPHATE, MAGNESIUM, CHLORIDE 697 +6}^H 2 O. Sol. in 30 min. in diamrnonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq (sp. gr. = 1.09) dissolves 37.5% of the P 2 O 5 . (Erlenmeyer, B. 14. 1253.) +20H 2 O. Sol. in 10 min. in diammonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq (sp. gr. = 1.09) dissolves 23.2% of the P 2 O 5 ; sol. in 15 min. in Y% citric acid +Aq. (Erlenmeyer, I. c.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Magnesium hydrogen phosphate. MgHPO 4 + 7H 2 0. Sol. in 322 pts. cold H 2 O in several days. If heated to 40 becomes milky, and separates a precipitate out at 100 of same salt, so that solution at 100 contains only 1 pt. salt in 498 pts. H 2 O. Much more sol. in H 2 O containing traces of acids, even dil. oxalic or acetic acids. (Graham, Phil. Mag. Ann. 2. 20.) Easily sol. in H 2 SO 8 +Aq. (Gerland, J. pr. (2) 4. 127.) Sol. in aqueous solution of Mg salts, but insol. in Na 2 HPO 4 +Aq. (Rose.) Sol. in sodium citrate+Aq. (Spiller.) When freshly precipitated it is sol. in hot NH 4 Cl+Aq, and NH 4 OH+Aq does not completely reprecipi- tate it; less sol. in INH 4 NO 3 +Aq. (Brett, Phil. Mag. (3) 10. 96.) Insol. in alcohol. (Berzelius.) For solubility in H 3 PO 4 , see under MgO. + 3^H 2 O. (Debray.) +H 2 O. Easily sol. in dil. acids, (de Schulten, C. R, 100. 263.) +3H 2 O. SI. sol. in H 2 O, easily in acids. (Stoklasa, Z. anorg. 3. 67.) +4^H 2 O. (Bergmann.) +6H 2 O. (Debray.) Magnesium tetrahydrogen phosphate, MgH 4 (P0 4 ) 2 . Not hygroscopic. Sol. in 5 pts. H 2 O with- out decomp. (Stoklasa, Z. anorg. 3. 67.) +2H 2 O. Not hygroscopic. Sol. in H 2 O without decomp. (Stoklasa, Z. anorg. 1. 307.) Decomp. by alcohol into MgHPO 4 +3H 2 O Magnesium pyrophospnate, Mg 2 P 2 O 7 . Nearly insol. in H 2 O; readily sol. in HC] or IINO 3 +Aq. (Fresenius.) +3H 2 O. SI. sol. in H 2 O, easily in HC1 or HNO 3 +Aq; sol. in H 2 SO 3 +Aq, and Na 4 P 2 O 7 +Aq. (Schwarzenberg.) Sol. in MgSO 4 +Aq, and (NH 4 ) 2 CO 3 +Aq Magnesium te/raphosphate, Mg 3 P 4 Oi 3 . Insol. in H 2 O. (Fleitmann and Henneberg A. 65. 331.) Magnesium potassium dimefaphosphate, K 2 Mg 2 (P 2 6 ) 3 . Very sol. in dil. acids. (Ouvrard, C. R 1888, 106. 1729.) +4H 2 O. Sol. in 10.2 pts. H 2 O. (Glatzel.; Magnesium potassium or^ophosphate. MgKP0 4 . SI. sol. in H 2 O. Decomp. by H 2 O. Easily ol. in acids. +6H 2 O. 2MgO, K 2 O, 3P 2 O 5 . Insol. in H 2 O; sol. in dil. HCl+Aq. (Ouvrard, C. R. 106. 1729.) Mg 2 HK(PO 4 ) 2 + 15H 2 0. (Haushofer.) Magnesium rubidium or^ophosphate, RbMgPO 4 +6H 2 O. Easily sol. in warm dil. HCl+Aq. Not decomp. by boiling H 2 O. (Erdmann, A. 1897, 294. 73.) Magnesium sodium ^nphosphate, MgNa 3 P 3 Oio+13H 2 O. Decomp. in the air. (Stange, Z. anorg. 1896, 12. 454.) Magnesium sodium metophosphate, 3MgO, Na 2 O, 4P 2 O 5 . Insol. in H 2 O or H 3 PO 4 +Aq. Scarcely sol. in HCl+Aq, or aqua regia. Not decomp. by (NH 4 ) 2 CO 3 +Aq. Sol. in cone. H 2 SO 4 . (Maddrell, A. 61. 53.) Magnesium sodium dwietaphosphate, MgNa 2 (P 2 O 6 ) 2 +4H 2 O. Sol. in 25 pts. H 2 O. (Glatzel, Dissert. 1880.) Magnesium sodium /n'metophosphate, MgNa 4 (P 3 O 9 ) 2 +5H 2 O. SI. sol. in H 2 O. After ignition is insol. in H,O. (Lindbom.) Magnesium sodium phosphate, lOMgO, 8Na 2 O, 9P 2 O 5 . Insol. in H 2 O; easily sol. in dil. acids. (Ouvrard, C. R. 106. 1729.) Magnesium sodium ori/iophosphate, MgNaPO 4 . Insol. in H 2 O. (Rose.) +9H 2 O. (Schoeoker -and Violet, A. 140. 232.) MgO, 2Na 2 O, P 2 O 5 . Insol. in H 2 O. (Ouvrard.) 3MgO, 3Na 2 O, 2P 2 O 5 . Insol. in H 2 O. (Ouvrard.) Magnesium sodium p?/rophosphate, basic (?). "Precipitate; si. sol. in H 2 O. Easily in HC1+ Aq, HNO 3 +Aq, and Na 4 P 2 O 7 +Aq. (Baer, Pogg. 75. 168.) Sol. in (NH 4 ) 2 CO 3 +Aq, and in MgSO 4 + Aq. Insol. in alcohol. Magnesium phosphate chloride, Mg 3 (PO 4 ) 2 , MgCl 2 . (Deville and Caron, A. ch. (3) 67. 455.) 698 PHOSPHATE, MAGNESIUM, NITROGEN OXIDE Magnesium pyrophosph&te nitrogen dioxide Mg,P,0 7 , H 2 0, N0 2 . Scarcely sol. in water. (Luck, Z. anal. 13, 255.) Magnesium phosphate fluoride, Mg 3 (PO 4 )2) MgF 2 . Min. Wagnerite. Slowly sol. in hot HNO 3 , and H 2 SO 4 . Magnesium phosphate calcium fluoride, 2Mg 3 (P0 4 ) 2 , CaF 2 . Min. Kjerulfite. Manganous dimetaphosphate, Mn 2 (P 2 O 6 ) 2 . Anhydrous. Insol. in H 2 O and dil. acids. (Fleitmann.) Sol. in cone. H 2 SO 4 . (Mad- drell.) Scarcely attacked by warm Na 2 S + Aq, and not much more by (NH 4 ) 2 S+Aq. Decomp. by Na 2 CO 3 +Aq. -f-8H 2 O. Insol. in H 2 O and dil. acids. (Fleitmann, Pogg. 78. 257.) Manganous trimeiaphosphate, Mn 3 (P 3 O 9 ) 2 + 11H 2 O. Difficultly sol. in cold or warm H 2 O. More easily sol. in cold, very easily in warm HC1 + Aq. When ignited, is insol. in acids, even aqua regia. (Lindbom.) Manganous hexametaphosphate. Sol. in sodium hexametaphosphate +Aq. (Rose, Pogg. 76. 4.) Mn 3 P 6 Oi 8 . Nearly insol. in H 2 O; easily sol. in acids. (Liidert, Z. anorg. 5. 15.) Manganic raetaphosphate, Mn(PO 3 ) 3 . Insol. in H 2 O or acids; decomp. by alkalies. (Schjerning, J. pr. (2) 45. 515.) Insol. in II 2 O; sol. in HC1; decomp. by alkalies +Aq. (Barbier, C. R. 1902, 135. 1055.) +H 2 O. Insol. in H 2 O or acids, except HCl+Aq. SI. decomp. by boiling with H 2 SO 4 . (Hermann, Pogg. 74. 303.) Manganous tetrametaphosphate, Mn 2 (PO 3 ) 4 . Not attacked by acids. (Glatzel, Dissert. 1880.) + 10H 2 O. Sol. only in boiling cone. H 2 S0 4 . (Glatzel.) Manganous (Mawetaphosphate, 5MnO, 5P 2 O 5 +12H 2 O. Ppt. (Tammann, J. pr. 1892, (2) 45. 450.) Manganous ort/iophosphate, Mn 3 (PO 4 ) 2 . +H 2 O. (Debray.) +3H 2 O. Sol. in 20 min. in diamonium citrate + Aq (sp. gr. = 1 ,09) ; triammonium citrate+Aq (sp. gr. = 1.09) dissolves 30.2% of the P 2 O 5 . (Erlenmeyer, B. 14. 1253.) 2 O. Efflorescent. (Erlen- meyer and Heinrich, A. 190. 208.) +7H 2 O. Very si. sol. in H 2 O. (Berzelius.) Easily sol. in mineral acids; sol. in HC 2 H 3 O 2 +Aq. Easily sol. in SO 2 +Aq. (Gerland, J. pr. (2) 4. 97.) Somewhat sol. in boiling (NH 4 ) 2 CO 3 +Aq, but deposited on cooling. (Berzelius.) Partly sol. in cold NH 4 C1, or NH 4 NO 3 +Aq. (Brett.) Sol. in cold or hot solutions of ammonium sulphate or succinate. (Wittstein.) SI. sol. in Mn salts +Aq. (Rose, Pogg. 76. 25.) Insol. in alcohol. Sol. in 10 min. in diarnmonium citrate+Aq (sp. gr. = 1.09); triammonium citrate+Aq (sp. gr. = 1.09) dissolves 53% of the P 2 O 5 . (Erlenmeyer, B. 14. 1253.) Manganous c&hydrogen orthophosphate, MnHPO 4 +3H 2 O. SI. sol. in H 2 O. Solution decomp. at 100. (Debray.) Slowly decomp. by cold H 2 O into Mn 3 (PO 4 ) 2 . (Erlenmeyer and Heinrich, A. 190. 203.) Easily sol. in H 2 SO 3 + A.q. (Gerland.) SI. sol. in HC 2 H 3 O 2 , easily in cone, mineral acids. (Heintz.) Sol. in* (NH 4 )oCO 3 +Aq, from which it is repptd. on boiling. Decomp. by boiling KOH+Aq. Insol. in alcohol. Mn 3 (PO 4 ), 2MnHPO 4 +4H 2 O. (de Schul- ten, C. C. 1905, 1. 188.) Manganous te^rahydrogen phosphate, MnH 4 (PO 4 ) 2 +2H 2 O. Deliquescent. Easily sol. in H 2 O, with decomp. to MnHPO 4 . (Erlenmeyer and Heinrich, A. 190. 208.) Not decomp. by H 2 O. (Otto, C. C. 1887. 1563.) H 2 O decomp. it into MnHPO 4 and H 3 PO 4 containing some dissolved salt. The less H 2 O used, the more MnHPO 4 separates. The acid nitrate separates MnHPO 4 on boiling. A.t the decomp. increases in proportion to the amt. of salt, but 1 g. of the salt is un- changed in 100 g. H 2 O. With less than 20 g. of salt to 100 g. H 2 O the decomp. is analogous to that of CaH 4 (PO 4 ) 2 , but with larger amts. of salt it is the opposite, becoming less with ncreasing amts. of the salt. (Viard, C. R. 1899, 129. 412.) Alcohol dissolves out H 3 PO 4 . (Heintz.) Pentomanganous c&hydrogen phosphate, Mn 6 H 2 (PO 4 ) 4 +4H 2 O. Not decomp. by boiling H 2 O. (Erlen- meyer and Heinrich, A. 190. 208.) Manganic or/Aophosphate, basic, Mn 2 P 3 O 8 + H 2 O. SI. sol. in H 2 O. PHOSPHATE, MERCUROUS 699 Manganic orf/iophosphate, MnPO 4 +H 2 O. Sol. in acids. (Christensen, J. pr. (2) 28. 1.) Manganous p?/rophosphate, Mn 2 P 2 O 7 . Anhydrous. (Lewis, Sill. Am. J. (3) 14. 281.) +H 2 O. H-3H 2 O. Insol. in H 2 O. Insol. in MnSO 4 + Aq, but sol. in Na 4 P 2 O 7 +Aq. (Rose.) Difficultly sol. in Na 4 P 2 O 7 +Aq, but easily sol. in K 4 P 2 O 7 +Aq. (Pahl.) Decomp. by KOH+Aq. Sol. in H 2 SO 3 +Aq. (Schwar- zenberg.) Insol. in acetone. (Naumann, 13. 1-04, 37. 4329.) Manganous hydrogen p^ophosphate, MnH 2 P 2 O 7 +4H 2 O. Sol. inII 2 O. (Pahl.) pyrophosphate, ; O 21 + 14H,O. Manganic Mn 4 P Sol. in H 2 SO 4 , and H 3 PO 4 . (Auger, C. R. 1901, 133. 95.) MnHP 2 O 7 . Insol. in H 2 O; very si. at- tacked by dil. HCl+Aq, easily by cone. Sol. in cone. H 2 SO 4 . (Sehjerning, J. pr. (2) 46. 515.) Manganous potassium cfo'metaphosphate. K 2 Mn(PO 3 ) 4 +6H !J O. Sol. in 95 pts. H 2 O. When ignited is not attacked by acids. (Glatzel, Dissert. 1880.) Manganous potassium ort/zophosphate, Insol. in H 2 O; easily sol. in dil. acids. (Ouvrard.) Manganic potassium pyrophosphate, MnKP 2 O 7 . +5H 2 O. SI. sol. in cold H,O. +3H 2 O. SI. sol. in cold H 2 O. (Rosen- heim, B. 1915, 48. 584.) Manganous potassium phosphate, MnK 2 P 2 O 7 Insol. in H 2 O; sol. in dil. acids. (Ouvrard C. R. 106. 1729.) +8H 2 O. SI. sol. in H 2 O. (Pahl.) Mri,P 2 O 7 , 2K 4 P 2 O 7 + 10H 2 O. sol. in H 2 O. (Pahl.) Difficultly Manganic potassium p?/r0phosph.ate, MnKP 2 O 7 . Insol. in H 2 O. Decomp. by acids ami bases. (Schjerning.) iganic silver pyrop AgMnP 2 O 7 +3H 2 O. Almost insol. in H 2 O. (Rosenheim, B 1915, 48. 585.) Manganous sodium ^phosphate, MnNa 3 P 3 O 10 +12H 2 O. SI. sol. in H 2 O; the melt obtained by heating the salt is readily sol. in H 2 SO 4 . (Stange, Z. anorg. 1896, 12. 455.) Manganous sodium dimetaphosphate, MnNa 2 (PO 3 )i+6H 2 O. Easily sol. in boiling H 2 SO 4 , but not at- tacked by acids after boiling. (Glatzel, Dissert. 1880.) Manganous sodium ^nmetaphosphate, Sol. in H 2 O. (Fleitmann and Henneberg.) MnNa(PO 3 ) 3 . Insol. in H 2 O, dil. acids, or alkalies. (Schjerning, J. pr. (2) 45. 515.) Manganous sodium ocforaetaphosphate, Mn 3 Na 2 (PO 3 ) 8 Insol. in acids except cone. H 2 SO 4 . (Tam- mann, J. pr. 1892, (2) 45. 469.) +5H 2 O. Almost insol. in cold H 2 O. Decomp. by boiling H 2 O with separation of Mn 2 O 3 . (Rosenheim, B. 1915, 48. 584.) Manganous sodium or^ophosphate. MnNaPO 4 . Insol. in H 2 O. (Ouvrard, C. R. 106. 1729.) MnO, 2Na 2 O, P 2 O 5 . As above. Manganous sodium pz/rophosphate, MnNa 2 P 2 O 7 . Insol. in H 2 O; easily sol. in dil. acids. (Wallroth.) +43^H 2 O. Very si. sol. in H 2 O. (Pahl.) 3Mn 2 P 2 O 7 , 2Na 4 P 2 O 7 +24H 2 O. Very si. sol.inH 2 O. (Pahl.) Manganic sodium p?/rophosphate, MnNaP 2 O 7 +H 2 O. (Christensen, J. pr. (2) 28. 1.) Manganic dipyrophosphate ammonia, Mn 2 P 4 O 14 , 2NH 3 . Insol. in H 2 O. Decomp. by HC1 and by alkalies. (Bar- bier, C. R. 1902, 135. 1109.y Manganous phosphate chloride, Mn 3 (PO 4 ) 2 , MnCl 2 . Insol. in H 2 O. (Deville and Caron, A. ch. (3) 67. 459. 3Mn 3 (PO 4 ) 2 , MnCl 2 . Insol. in H 2 O. (De- ville and Caron.) Mercurous /iexawetaphosphate (?). Ppt. Sol. in sodium hexametaphosphate +Aq. (Rose.) Hg 6 P 6 O ]8 . Insol. in H 2 O; very si. sol. in acids. (Liidert, Z. anorg. 5. 15.) Moderately sol. in H 2 O when freshly pptd. More sol. in acids than the mercurous salt. (Liidert.) 700 PHOSPHATE, MERCUROUS Mercurous on'/iophosphate, (Hc, 3 ) 2 (PO 4 ) 2 . Ppt. Decomp. by boiling with H 2 O. (Ger- hardt.) Sol. in HNOs+Aq. Sol. in Hg 2 (NO 3 ) 2 + Aq. Insol. in H 3 PO 4 +Aq. Mercuric ortfiophosphate, Hg 3 (PO 4 ) 2 . Insol. in H 2 O. SI. sol. in hot H 2 O, crystal- lizing out on cooling. (Haack, A. 262. 185. Slowly sol. in cold dil., quickly in hot dil. or cold cone. HCl + Aq. Less easily sol. in HNO 3 +Aq. Sol. in H 3 PO 4 +Aq.~ (Berze- lius.) InsDl. in H 3 PO 4 +Aq. (Haack.) De- comp. by NaCl+Aq into insol. HgCl 2 , 3HgO, but sol. in NaCl+Aq, containing HNO 3 . (Haack.) Sol. in 6 pts. NH 4 C1 in aqueous solution by heating. (Tromrnsdorff.) Sol. in (NH 4 ) 2 CO 3 , (NH 4 ) 2 SO 4 , or NH 4 NO 3 +Aq. (Wittstein.) Insol. in alcohol. Mercuromercuric ort/iophosphate, 7Hg 2 O, 14HgO, 2P 2 O 5 +20H 2 O. (Brooks, Pogg. 66. 63.) Mercurous p?/rophosphate, Hg 4 P 2 O 7 +H 2 O. Sol. in Na 4 P 2 O 7 +Aq, when recently pptd. Insol. in Na 4 P 2 O 7 +Aq, when heated to 100. Sol. in HNO 3 +Aq. Decomp. by HCl+Aq. (Schwarzenberg, A. 65. 133.) Mercuric ?/r0phosphate, Hg 2 P 2 O 7 . Sol. in acids; insol. in Na 4 P 2 O 7 +Aq, after being heated to 100. Sol. in NaCl+Aq; quickly decomp. bv NaOH+Aq, and Na 2 HPO 4 +Aq. Sol. in 6 pts. NH 4 Cl+Aq. (Trommsdorff.) Sol. in NH 4 NO 3 ,(NH 4 )SO 4 , and (NH 4 ) 2 CO 3 +Aq; also in KI+Aq. Mercurous silver ort/iophosphate, AgHg 2 PO 4 . Sol. in HNO 3 . (Jacobsen, Bull. Soc. 1909, (4) 6. 949.) Molybdenum phosphate, Mo 2 (PO 4 ) 2 (?). Insol. in H 2 O. Sol. in MoCl 2 +Aq. Molybdenum sodium p^/rophosphate, Na(MoP 2 O 7 ) + 12H 2 0. Ppt, (Rosenheim, B. 1915, 48. 589.) Nickel dimetaphosphsLte, NiP 2 O 3 . Insol in H 2 O or dil. acids. Sol. in cone. H 2 SO 4 . Not decomp. by boiling alkali car- bonates or sulphides + Aq. (Maddrell, A. 61. 58. +4H 2 O. Sol. in cold acids. (Glatzel, Dissert. 1880.) Nickel Zdraraetaphosphate, Ni 2 P 4 O 12 . Insol. in HC1. Sol. in cone. HNO 3 and especially sol. in H 2 SO 4 on boiling. (Glatzel.) Nickel telrametaphosphate, Ni 2 P 4 Oi 2 + 12H 2 O. Easily sol. in acids. (Glatzel.) Nickel ortfiophosphate, Ni 3 (PO 4 ) 2 +7H 2 O. Insol. in H 2 O. Sol. in acids. (Rammesl- berg, Pogg. 68. 383.) Sol. in Ni salts +Aq. (Rose, Pogg. 76. 25.) Insol. in NaoHPO 4 +Aq. (Tupputi, 1811.) Very si. sol. in hot (NH 4 ) 2 HPO 4 +Aq. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethylacetate. (Naumann, B. 1910, 43. 314.) Nickel pyrophosphate, Ni 2 P 2 O 7 +6H 2 O. Insol. in H 2 O; sol. in mineral acids, Na 4 P 2 O 7 +Aq, and NH 4 OH+Aq. Not pptd. from Ni 2 P 2 O 7 + Aq by alcohol. (Schwarzenberg, A. 65. 158.) Nickel potassium cfometaphosphate, NiK 2 P 4 O 12 +6H 2 O. Sol. in 130 pts. H 2 O. (Glatzel.) Nickel potassium or^ophosphate, NiKPO 4 . Insol. in H 2 O; sol. in dil. acids. (Ouvrard, R. 106. 1729.) 3NiO, 3K 2 O, 2P 2 O 6 . As above. Nickel sodium ^nphosphate, Na 3 NiP3O 19 + 12H 2 O. Very sol. in H 2 O; decomp. in Aq solution. (Schwarz, Z. anorg. 1895, 9. 261.) Nickel sodium meta phosphate, 3Ni(PO 3 ) 2 , NaPO 3 . Insol. in H 2 O and dil. acids. Sol. in cone. H 2 SO 4 . (Maddrell, A. 61. 56.) NiNa 4 (PO 3 ) 3 +8H 2 O. Easily sol. in H 2 O. (Lindbom.) Nickel sodium cfe'raetaphosphate, NiNa 2 P 4 Oi 2 +6H 2 O. SI. sol. in H 2 O. Moderately sol. in acids. (Glatzel, Dissert. 1880.) Nickel sodium ^nmetaphosphate. Ni 2 Na 2 (P 3 9 ) 2 +9H 2 0. 1 1. H 2 O dissolves 60.6 g. at 20. (Tam- mann, J. pr. 1892, (2) 45. 426.) Na 3 NiP 3 Oio4-12H 2 p. Insol. and not de- comp. by H 2 O. Sol. in acids. (Schwarz, Z. anorg. 1895, 9. 261.) Nickel sodium octoraetaphosphate, Na 2 Ni 3 (PO 3 ) 8 . (Tammann, J. pr. 1892, (2) 45. 469.) Nickel sodium or^ophosphate, NiNaPO 4 + 7H 2 0. Ppt. (Debray, C. R. 59. 40.) NiO, 2Na 2 O, P 2 O 5 . Insol. in H 2 O. Easily sol. in dil. acids. (Ouvrard.) PHOSPHATE, POTASSIUM HYDROGEN 701 Nickel sodium pi/rophosphate, Ni 10 Na ]fi (P 2 O 7 )9. Insol. in H 2 O. Moderately sol. in acids. (Wallroth.) Osmium phosphate (?). SI. sol. in H 2 O; sol. in HNO 8 +Aq. (Ber- zelius.) Palladium or^Aophosphate (?). Ppt, Phosphorus phosphate, 4P 4 O, 3P 2 O 5 (?). Decomp. spontaneously. Sol. in H 2 O and alcohol when fresh; insol. in ether, (le Verrier, A. 27. 167; Reinitzer, B. 14. 1884.) Platinum phosphate, PtP 2 O 7 . Insol. in H 2 O, acids and alkalies. Decomp. by fusing with potassium carbonate. (Bar- nett, C. N. 1895, 71. 256.) Potassium raoraowetaphosphate, KPO 3 . Nearly insol. in H 2 O;*s3l. in weak acids, even in acetic acid. (Maddrell, A. 61. 62.) Insol. in H 2 O and weak acids. (Fleitmann, Pogg. 78. 250.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Potassium eftmetaphosphate, K 2 P 2 Oe+H 2 O. Sol. in 1.2 pts. cold H 2 O, but not more in hot H 2 O. (Fleitmann, Pogg. 78. 250.) Potassium trimetaphospha.te, K 3 P 3 O 9 . Very sol. in cold H 2 O before it is fused. (Lindbom, Acta Lund. 1873. 14.) Potassium or^ophosphate, K 3 PO4. Not deliquescent. Very sol. in H 2 O. (Graham, Pogg. 32. 47.) Very si. sol. in cold, easily in hot H 2 O. (Darracq.) Solubility in H 3 PO 4 +Aq at 25. In 1000 g. of the solution, me K P04 9.14 8.84 8.42 7.52 6.90 6.88 3.13 3.22 3.44 3.78 4.15 4.12 (D'Ans and Schreiner, Z. phys. Ch. 1910, 76. 103.) Insol. in alcohol. Potassium hydrogen or^ophosphate, 2K 2 HP0 4 , KH 2 PO 4 +H 2 O. Very unstable; very sol. in H 2 O with de- comp. Identical with the substance de- In 1000 g. of the solution, mols. K P04 6.80 4.08 6.80 4.05 6.76 3.96 6.50 3.81 6.16 3.61 5.24 3.25 4.42 2.94 scribed as dipotassium phosphate by Ber- zelius. (Staudenmaier, Z. anorg. 1894, 6. 389.) 3K 2 HPO 4 , KH,PO 4 +2H 2 O. Very unstable; very sol. in H 2 O with decomp. (Stauden- maier.) Potassium hydrogen or^ophosphate, K 2 HPO 4 . Deliquescent. Very sol. in H 2 O and alcohol. Solubility in H 3 PO 4 +Aq at 25. (D'Ans and Schreiner, Z. phys. Ch. 1910, 76. 103.) Potassium cfahydrogen phosphate, KH 2 PO 4 . Deliquescent. Easily sol. in H 2 O. (Vau- quelin, A. ch. 74. 96.) 1 1. sat. aq. solution at 7 contains 249.9 g. KH 2 PO 4 . (Muthmann and Kuntze, Z. Kryst. Min. 1894, 23. 308.) Solubility in H 3 PO 4 +Aq at 25. In 1000 g. of the solution, mols. K P0 4 2.90 2.36 1.70 1.71 1.60 1.67 1.48 1.46 1.78 3.15 2.18 4.65 2.54 6.32 2.66 6.76 2.98 8.03 3.32 8.80 (D'Ans and Schreiner, Z. phys. Ch. 1910, 75. 103.) Sp. gr. of KH 2 PO 4 +Aq at 18 containing: 5 10 15%KH,PO 4 . 1.0341 1.0691 1.1092 (Kohlrausch, W. Ann. 1879. 1.) Sol. in 20% KC 2 H 3 O 2 +Aq. (Strom ever.) For solubility in H 2 O, see K 2 HPO 4 , H 8 PO 4 . Insol. in alcohol.* 702 PHOSPHATE, POTASSIUM, ACID Potassium orthophosphate. acid. KH 2 PO 4 , H 3 P0 4 . Solubility in H 2 O at t. t % KH 2 P04,H3P04 Solid phase 0.6 3.337 Ice - 2.5 12.13 a - 6.7 29.43 K - 9.2 36.98 a -13 44 Ice+KH 2 PO 4 0(?) 45.8 KH 2 P0 4 +10.9 50.3 t( 65.2 68.44 (i 78 72.43 n 87.5 77.6 (i 105.5 85.9 K 120 92.1 "+KH 2 P0 4 , H 3 P0 4 135 96.1 KH 2 PO 4 , H 3 PO 4 139 100 (i (Parravano and Mieli, Gazz. ch. it. 38. II, 536.) Solubility in anhydrous H 3 PO 4 at t. t % KH 2 P04, H 3 PO4 38.5 84 110 126.5 18.17 58.42 77.53 92.26 (Parravano and Mieli.) Potassium pyrophosphate, K 4 P 2 O 7 +3H 2 O. Very deliquescent, and sol. in H 2 O. Precipitated from aqueous solution by al- cohol. (Schwarzenberg, A. 65. 136.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Potassium hydrogen pyrophosphate, K 2 H 2 P 2 O 7 . Very deliquescent, and sol. in H 2 O. Insol. in alcohol. (Schwarzenberg.) Potassium silver raetaphosphate, K 2 As; 4 (P0 3 ) 6 +H 2 0. (Tamrnann, J. pr. 1892, (2) 45. 417.) Potassium sodium cfawetophosphate, KNaP 2 O 6 +H 2 O. Sol. in 24 pts. H 2 O. (Fleitmann, Pogg. 78. 339.) Potassium sodium phosphate. KNaHPO 4 + 7H 2 0. Not efflorescent. Sol. in H 2 O. Tnpotassium ^nsodium hexahydrogen phos- phate, H 6 Na 3 K 3 (PO 4 ) 4 -f 22H 2 O. Sol. in H 2 O. (Filhol and Senderens, O. R 93. 388.) Potassium sodium pyrophosphate, K 2 Na 2 P 2 O 7 + 12H 2 O. Sol. in H 2 O. (Schwarzenberg, A. 65. 140.) Potassium strontium cftraetaphosphate, K 2 Sr(P 2 O 6 ) 2 +4H 2 O. As the KBa comp. (Glatzel, Dissert. 1880.) Potassium strontium hexametaphosphate, K 2 Sr 2 P 6 O 18 . (Tammanri, J. pr. 1892, (2) 45. 435.) Potassium strontium or^ophosphate, KSrPO 4 . Insol. in H 2 O; sol. in dil. acids. (Grandeau, A. ch. (6) 8. 193.) Potassium strontium pyrophosphate, K 2 SrP 2 O 7 . Insol. in H 2 O; sol. in dil. acids. (Ouvrard, C. R. 106. 1599.) Potassium thorium phosphate, K 2 O, 4ThO 2 , 3P 2 5 . Insol. in HC1, HNO 3 , or aqua regia. (Troost and Ouvrard, C, R. 102. 1422.) K 2 O, ThO 2 , P 2 O 5 . Insol. in H 2 O; sol. in HNOs+Aq. (Troost and Ouvrard.) 6K 2 O, 3ThO 2 , 4P 2 O 5 . Sol. in acids. (Troost and Ouvrard.) Potassium tin (stannic) phosphate, K 2 0, 4SnO 2 , 3P 2 O 6 . (Ouvrard, C. R. 111. 177.) K 2 O, 2SnO 2 , P 2 O 5 . (Ouvrard.) Potassium titanium phosphate, K 2 O, 4TiO 2 , 3P 2 6 . (Ouvrard. C. R. 111. 177.) K 2 O, 2TiO,>, P 2 O 5 . (Ouvrard.) Potassium uranous phosphate, 4UO 2 , K 2 O, 3P 2 5 . Practically insol. in cone. HNO 3 and HC1, even when the acids are boiling. Attacked- by HF-f HNO 3 . (Colani, A. ch. 1907, (8) 12. 133.) Potassium uranous wetaphosphate, U0 2 , K 2 O, P 2 O 5 . Easily sol. in HNO 3 . Sol. in cone. HC1. (Colani.) Potassium uranous pyrophosphate, SUOz, 6K 2 O, 4P 2 O 5 . Sol. in acids. (Colani.) Potassium uranyl phosphate, K 2 O, UO 3 , P2O 5 . (Ouvrard, C. R. 110. 1333.) 2K 2 O, UO 8 , P 2 O 5 . (Ouvrard.) K 2 O, 2UO 3 , P 2 O 5 . (Ouvrard.) PHOSPHATE, SILVER 703 Potassium uranyl or^ophosphate. K(UO 2 )PO 4 -f3H 2 O. As NH 4 comp. (Lienau, Dissert. 1898.) Potassium vanadium phosphate. See Phosphovanadate, potassium. Potassium yttrium phosphate, 3K 2 O, Y 2 O 3 2P 2 O 5 . K 2 O, Y 2 O 3 , 2P 2 O 5 . 3K 2 O, 5Y 2 O 3 , 6P 2 O 5 . (Duboin, C. R. 107 622.) Potassium zinc te/rawetaphosphate, K,Zn(PO 3 ) 4 +6H 2 O. Sol. in 70 pts. H 2 O. (Glatzel, Dissert 1880.) Potassium zinc phosphate, KZnPO 4 . Insol. in H 2 O. Sol. in dil. acids. (Ouvrard C. R. 106. 1729.) K 2 ZnP 2 O 7 . As above. Potassium zirconium phosphate, K 2 O, 4ZrO 2 3P 2 O 5 . Insol. in acids or aqua regia. (Troost anc Ouvrard, C. R. 102. 1422.) K 2 O, ZrO,, P 2 O 5 . Insol. in H 2 O, HNO 3 HC1, or aqua regia. Sol. in hot cone. H 2 SO 4 (Troost and Ouvrard.) Potassium phosphate selenate. See Selenophosphate, potassium. Potassium hydrogen phosphate sulphate, Decomp. by H 2 O and alcohol. (Jacque- lain.) Rhodium phosphate, basic, 4Rh 2 O 3 , 3P 2 O 5 -f 32H 2 O. Insol. in H 2 O or acids. (Glaus.) Rh 2 O 3 , P 2 5 +6H 2 O = RhPO 4 +3H 2 O Sol in H 2 O. (Glaus.) Rubidium metophosphate, RbPO 3 . Sol. in H 2 O. (von Berg, B. 1901, 34. 4183.) Rubidium or^ophosphate, Rb 3 PO 4 -j-4H 2 O. Hydroscopic; sol. in H 2 O; pptd. by alcohol, (von Berg, B. 1901, 34. 4183.) Rubidium hydrogen or^ophosphate, Rb 2 HP0 4 +H 2 0. Sol. in H 2 O; insol. in cone. NH 4 OH+Aq- insol. in alcohol, (von Berg.) Rubidium dihydrogen or/Aophosphate, RbHvPO 4 . Very sol. in H 2 O; pptd. by alcohol, (von Berg.) Rubidium pyrophosphate, Rb 4 P 2 O 7 . Hydroscopic; sol. in H 2 O. (von Berg.) Samarium anhydrometaphosphate, Sm 2 O 8 , 5P 2 O 6 . Insol. in H 2 O or HNO 3 +Aq. (Cleve.) Samarium or^ophosphate, SmPO 4 . Scarcely attacked by boiling HNO 3 +Aq. (Cleve.) +2H 2 0. Samarium pz/rophosphate, SmHP 2 O 7 + 13^H2O. (Cleve.) Silicon phosphate. See Silicophosphoric acid. Silver metophosphate, Ag 2 O, 2P 2 O 5 +H 2 O. (Kroll, Z. anorg. 1912, 76. 408.) Silver cftmetaphosphate, Ag 2 P 2 O c . Very si. sol. in H 2 O. (Fleitmann, Pogg. 78. 253.) Sol. in cold aniline metaphosphate-f-Aq. (Nicholson.) Very si. sol. in H 2 O. (Warschauer, Dis- sert. 1903.) +H 2 O. Very sol. in H 2 O. (Langheld, B. 1912, 45. 3760.) Silver Znraetaphosphate, Ag 3 P 3 O 9 . Sol. in 60 pts. cold H 2 O. Can be crystal- lized from cone. HNO 3 +Aq. (Fleitmann and Henneberg.) +H 2 O. (Lindbom.) Silver hexametaphosphate, AgePeOis. Insol. in H 2 O. Sol. in HNO 3 or NH 4 OH + Aq, and in a large excess of sodium hexa- metaphosphate+Aq. (Rose.) Easily decomp. by Na 2 S+Aq. Decomp. gradually by hot H ? O into When freshly pptd., easily sol. in H 2 O. Casily sol. in dil. acids. (Liidert, Z. anorg. 5. 15.) Silver ort/iophosphate, Ag 3 PO 4 . Very si. sol, in H 2 O. 1 1. H 2 O dissolves 6.5 X10- 3 g. Ag 3 PO 4 at 19.46. (Bottger, Z. phys. Gh. 1903, 46. 603.) Sol. in H 3 PO 4 , HNO 3 , or HC 2 H 3 O 2 +Aq, in \H 4 OH or (NH 4 ) 2 CO 3 +Aq. Less easily in ammonium nitrate or succinate, and incom- letely in (NH 4 ) 2 SO 4 +Aq. (Lassaigne, J. Pharm. (3) 16. 289.) Insol. in Na 2 HPO 4 +Aq. (Stromeyer.) Not pptd. in presence of Na citrate. Spiller.) If 1 mol. Ag 3 PO 4 is boiled with 1 mol. \ T a 2 CO 3 , 44% of it is decomp. (Malaguti.) Readily sol. in soluble hyposulphites +Aq ith decomp. (Herschel.) Insol. in Ag salts -j-Aq. (Rose.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 898, 20. 829.) 704 PHOSPHATE, SILVER HYDROGEN Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); "ethyl acetate. (Naumann, B. 1910, 43. 314.) Silver hydrogen or^ophosphate, Ag 2 HPO 4 . Decomp. by H 2 O or alcohol into H 3 PO 4 and Ag a PO 4 . (Joly, C. R. 103. 1071.) Sol. in H 3 PO 4 +Aq; insol. in ether. (Schwarzenberg, A. 65. 162.) Silver pi/rophosphate, Ag 4 P 2 O 7 . Insol. in hot or cold H 2 O. Sol. in cold HNO 3 +Aq without decomp. Decomp. by hot HNO 3 or H 2 SO 4 into orthophosphate. Decomp. by HCl+Aq into AgCl and H 3 PO 4 . Insol. in HC 2 H 3 O 2 +Aq. Sol. in NH 4 OH + Aq without decomp. (Stromeyer, Schw. J. 58. 126.) Insol. in Na 4 P 2 O 7 +Aq. Very si. sol. in AgNO 3 +Aq. (Schwarzenberg, A. 65. 161.) Not completely insol. in Na 4 P 2 O 7 +Aq. (Rose.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Silver hydrogen pt/rophosphate, Ag 2 H 2 P 2 O 7 . Decomp. by H 2 O into Ag 4 P 2 O 7 . (Hurtzig and Geuther, A. 111. 160.) Decomp. by cold H 2 O. (Cavalier, C. R. 1904, 139. 285.) Silver hydrogen pT/rophosphate metaphos- phate, 2Ag 2 HP 2 O 7 , HPO 3 . Decomp. by H 2 O. Easily sol. in HNO 3 + Aq. (BLandG.) Silver ZeJraphosphate, 6Ag 2 O, 4P 2 O 5 = Ag 6 P 4 O 13 . Insol. in, but gradually decomp. by boiling H 2 O. (Berzelius.) Sol. in large excess of the corresponding Na salt+Aq. Silver de/caphosphate, Agi 2 Pi O 3 i. Easily sol. in sodium dekaphosphate+Aq. (Fleitmann and Henneberg, A. 65. 330.) Silver ^raphosphate, Ag 2 O, 3P 2 O 5 . (Kroll, Z. anorg. 1912, 76. 407.) Silver sodium dwetaphosphate, AgNaP 2 O 6 . Sol. in H 2 O. (Fleitmann and Henneberg, Pogg. 65. 310.) Silver sodium pyrophosph&te, 6Ag 4 P 2 O 7 , Na 4 P 2 O 7 +4H 2 O. Not completely sol. in Na 4 P 2 O 7 +Aq. Easily sol. in HNO 3 +Aq. (Baer, Pogg. 75. 152.) Easily sol. in H 2 O. (Stromeyer.) Ag 3 NaP 2 O 7 + KH 2 O. p p t. (Stange, Z anorg. 1896, 12. 460.) Silver uranyl phosphate, 2Ag 2 O, 6UO 3 , 3P 2 O +30H 2 O. (Blinkoff, Dissert. 1900.) Silver phosphate ammonia, Ag 3 PO 4 , 4NH 3 . (Widmann, B. 17. 2284.) Sodium /n'phosphate, Na 5 P 3 Oi . Very sol. in H 2 O; decomp. easily in aa. solution at 100. (Schwarz, Z. anorg. 1895, 9. 253.) Sodium monoraetaphosphate, NaPO 3 . Insol. in H 2 O. Sol. in dil. and cone, acids. (Maddrell, A. 61. 63.) Insol. in acids. (Graham.) Gradually deoomp. by alkalies. Sodium diwetophosphate, Na 2 P 2 O 6 +2H 2 O. Deliquescent. Sol. in 7.2 pts. of cold or hot H 2 O. Very sol. in cone. HCl+Aq. Sol. in NaOH+Aq. Insol. in strong, verv si. sol. in dilute alcohol. (Fleitmann, Pogg. 78. 246.) Sodium inwetaphosphate, Na 3 P 3 O 9 +6H 2 O. Sol. in 4.5 pts. cold H 2 O. Insol. in strong, very si. sol. in dil. alcohol. (Fleitmann and Henneberg, A. 65. 307.) Decomp. by boiling H 2 O. (Lindbom.) Sodium te/rawetophosphate, Na 4 P 4 O J2 . Sol. in H 2 O; cryst. with about 4H 2 O. Less sol. in alcohol than in H 2 O. (Fleitmann, Pogg. 78. 854.) Sodium heximetaphosphate, Na 6 P 6 Ois. Deliquescent. Very sol. in H 2 O. Insol. in alcohol. (Graham, Pogg. 32. 56.) Sodium or//iophosphate, Na 3 PO 4 + 12H 2 O. Not deliquescent in dry air. 100 pts. H 2 O dissolve 19.6 pts. crystals at 15.5. (Graham.) 100 pts. H 2 O dissolve 28.3 pts. Na 3 PO 4 + 12H 2 O at 15. (Schiff.) Solubility in H 3 PO 4 +Aq at 25. In 1000 g. of the solution, mols. Na PO4 4.28 3.24 2.24 2.73 0.040 0.183 0.752 1.08 (D'Ans and Schreiner, Z. phys. Ch. 1910, 75. 101.) Sp. gr. of Na 3 PO 4 +Aq at 15. = %Na 3 P0 4 +12H 2 0. % Sp. gr. % Sp. gr. % Sp. gr. 1 2 3 4 5 6 7 8 .0043 .0086 .0130 .0174 .0218 .0263 .0308 .0353 9 10 11 12 13 14 15 16 1.0399 1.0455 1.0492 1.0539 1.0586 1.0633 1.0681 1 . 0729 17 18 19 20 21 22 23 24 1.0778 1.0827 1.0876 1.0925 1.0975 1.1025 1.1076 1.1127 (Schiff, calculated by Gerlach, Z. anal. 8. 280.) PHOSPHATE, SODIUM 705 InsoL in CS 2 . (Arctowski, Z. anorg. 1894 6O\7 \ Solubility in H 2 at t. AOl .) Insol. in methyl acetate. (Naumann, B t G. Na 2 HPO4 in 100 g. H 2 O 1909. 42. 3790.) +10H 2 O. (Rammelsberg.) 10.26 3.55 Could not be obtained. (Hall, J. pr. 94 237) 25.15 40.29 12.02 54.88 +7H 2 O. (Hall.) Melts in crystal water at 76.6. (Graham. 60.23 99.77 83.00 102.15 Sodium hydrogen phosphate, Na 2 HPO 4 . Three breaks in the curve: at 36.45, transi- Sol. in H 2 O with evolution of heat. 100 pts. H 2 O dissolve at t. tion from dodecahydrate to heptahydrate; .at 48, transition from heptahydrate to the dihydrate; at 95.2, transition from dihydrate to the monohvdrate. (Shiomi, C. C. 1909, to Pts. 4.0 PtS. ,o Pts. N a2 HP.O4 . t Na2HPO 4 NazHPO II. 106.) 10 on 1.55 4.10 1 1 no 40 50 ftfl 30.88 80 43.31 90 K pr OO 1 nn 81.29 95.02 i no on Solubility of Na 2 HPO 4 in H 2 O at t. 4U 30 1 .l.Uo 19.95 ou 70 oo.^y iuu 68.72 106.2 lUo.^U 114.43 t G. Na 2 HP04 in 100 g. H 2 O Solid phase (Poggiale, J. Pharm. (3) 44. 273.) 100 pts. H 2 O at 13 dissolve 3.4 pts. NaaHPO 0.43 1.42 Ice (Ferein, Ph. Viertelj. 7. 244); at 15, 5.9 pts. (Neese) at 16, 6.3 pts. (Mulder); at 16, 8.4 pts. (Miiller, J -0.24 OPak 0.70 M pr. 95. 52) ; at 20, 6.8 p ts. (Neese, Russ. Z. Pharm. 1 .5* 101); at 25, 12.5 pts. (ibid.). +0.05 1.67 Na 2 HPO 4 +12H 2 O Solubility in 100 pts. H 2 O at t. 20.0 25 7.66 12 u Pts. ,o Pts. Pts. 32! o J-^f . \J 25.7 (i t Na 2 HPO t Na 2 HPO t Na 2 HPO 4 34.0 33.8 ii 1 2.5 2.6 35 36 39.3 43.6 69 70 94.8 95.0 35.2* 39.2 AK. 51.8 fi7 ^ Na 2 HPO 4 +7H 2 O t( 2 2.6 37 49.5 71 95.1 T:O . \J 4.C Q* U i . O 3 4 2.7 2.7 38 39 55.5 60.6 72 73 95.2 95.4 rrO . O 50.0 fiO 80.2 Na 2 HPO 4 +2H 2 O 5 2.8 40 63.9 74 95.6 v/v/ U 80 Q9 Q tt 6 3.0 41 66.2 75 95.8 Oly . \J on O--I . t/ oo 4 (i 7 3.2 42 68.6 76 96.0 t/U \J of;* *->& . Tt 10T te 8 9 10 3.4 3.6 3.9 43 44 45 70.8 72.9 74.8 77 78 79 96.1 96.3 96.5 J7t_| 96.2 105.0 ion J.U.1 \J 104.6 102.3 QQ 9 Na 2 HP0 4 11 n 11 4.2 46 76.5 80 96.6 \.i\j yif . i 12 13 14 15 4.5 4.9 5.3 5.8 47 48 49 50 78.2 79.7 81.2 82.5 81 82 83 84 96.8 96.9 97.0 97.1 (Menzies and Humphery, Int. Cong. App. Chem. 1912, 2. 177.) * Transition points. 16 17 6.3 6.9 51 52 83.7 84.8 85 86 97.2 97.4 Solubility in H 2 O at t. 18 7.6 53 85.8 87 97.5 100 g. H 2 O 19 8.4 54 86.7 88 97.6 t dissolve g. Solid phase 20 9.3 55 87.7 89 97.7 Na-sHPO 21 22 10.3 1.1.4 56 57 88.6 89.4 90 91 97.8 97.9 25 2.51 10 47 Na 2 HP0 4 , 12H 2 (t 23 24 12.6 14.0 58 59 90.2 90.9 92 93 98.0 98.1 35.4* 40 3 l TC / 46.11 K.A QfJ Na 2 HP0 4 , 7H 2 n 25 26 15.4 16.9 60 61 91.6 92.2 94 95 98.2 98.4 ^t\J O 48.35* KQ 7 UTC . iH 2 O. Sol. in H 2 O. (Filhol and Senderens, C. R. 93. 388.) 60 70 80 a. 21.83 25.62 30.04 b. 44.07 52.11 63.40 (Poggiale.) 90 100 35.11 40.26 77.47 93.11 Sol. in H 2 feO 4 . (Walden, Z. anorg. 1902, 29. 384.) 708 PHOSPHATE, SODIUM HYDROGEN Crystallizes unchanged from NH 4 Cl+Aq (Winkler), or cone. NH 4 OH+Aq.(Uelsmann.) Decomp. into orthophosphate by heating with H 2 SO 4 , HC1, HC 2 H 3 O 2 , or H 3 PO 4 +Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Sodium hydrogen pyi ophosphate, Na 2 H 2 P 2 O 7 . Decomp. by H 2 O. Sol. in H 2 O containing HC 2 H 3 O 2 without decomp. (Bayer, J. pr. 106. 501.) SI. sol. in alcohol. Much more sol. in HoO than NaH 2 PO 4 . +6H 2 O. (Rammelsberg, B. A. B. 1883. 21.) 100 g. sat. solution contain 14.95 g. Na 2 H 2 P 2 O 7 at 18. (Giran, A. ch. 1902, (7) 30. 249.) NaH 3 P 2 O 7 . Very hydroscopic. (Salzer, Arch.-Pharm. 1894, 232.* 369.) 100 g. sat. solution contain 62.7 g. at 18. (Giran, A. ch. 1902, (7) 30. 249.) Na 3 HP 2 O 7 +H 2 O. Sol. in 3 pts. H 2 O. (Salzer, Arch. Pharm. 1894, 232. 366.) +6H 2 O. 100 g. sat. solution contain 28.17 g. Na 3 HP 2 O 7 at 18. (Giran.) Sodium te^raphosphate, NaeP 4 O] 3 . Slowly sol. in 2 pts. cold H 2 O. Easily decomp. + 18H 2 O. (Uelsmann.) Sodium hydrogen fe/raphosphate, Na 4 H 2 P 4 13 . Sol. in H 2 O. Sodium de/caphosphate, Nai 2 PioO 3 i. Sol. in H 2 O. (Fleitmann and Henneberg, A. 65. 333.) Sodium strontium diraetaphosphate, Na 2 Sr(P 2 O 6 ) 2 +4H 2 O. As the NaBa comp. (Glatzel, Dissert. 1880.) Sodium strontium ^nraetaphosphate, NaSrP 3 O 9 +3H 2 O. Easily sol. in H 2 O and acids, (Fleitmann, A. 65. 315.) Sodium strontium or^ophosphate, NaSrPO 4 +H 2 0. Scarcely sol. in H 2 O; sol. in acids. +9H 2 O. (Joly, C. R. 104. 905.) Sodium strontium p^/rophosphate (?). SI. sol. in H 2 O. Insol. in Na 4 P 2 O 7 +Aq. (Baer, Pogg. 75. 166.) Easily sol. in HCl+Aq, or HNO 8 +Aq. Sol. in NH 4 OH+Aq. Sodium thallium p^/rophosphate, Na6[Tl(P 2 O7)2]+6H 2 O=Na(TlPoO 7 ), Na 4 P 2 O 7 +6H 2 O. Decomp. by H 2 O. (Rosenheim, B. 1915, 48. 588.) Sodium thorium ort/iophosphate, NaTh,(P0 4 )*. Insol. in acids. (Wallroth, Bull. Soc. (2) 39. 316.) Sodium thorium phosphate, Na 2 O, 4ThO 2 , 3P 2 O 6 . Insol. in HNO 3 , HC1, or aqua regia. (Troost and Ouvrard, C. R. 105. 30.) 5Na 2 O, 2ThO 2 , 3P 2 O 5 . Sol. in HNO,+Aq. (T. and O.) Na 2 O, ThO 2 , P 2 O 5 . (T. and O.) Sodium thorium p?/rophosphate, Na 4 P 2 O 7 , ThP 2 O 7 +2H 2 O.' (Cleve.) Sodium tin (stannic) phosphate, NaSn 2 (P0 4 ) 8 . (Ouvrard, C. R. 111. 177.) Na 2 Sn(PO 4 ) 2 . (Wunder, J. pr. (2) 4. 339.) 6Na 2 O, 3SnO 2 , 4P 2 O 5 . (Ouvrard.) Sodium titanium phosphate, NaTi 2 (PO 4 ) 3 . Insol. in acids. (Rose, J. B. 1867. 9.) 6Na 2 O, TiO 2 , 4P 2 O 5 . (Ouvrard, C. R. 111. 177.) Sodium uranium phosphate, UO 2 ,Na 2 O, P 2 O 5 . Easily attacked bv acids. (Colani, A. ch. 1907, (8) 12. 137.) Sodium uranium metophosphate, 4UO 2 , Na 2 O, 3P 2 & . Insol. in boiling HNO 3 . (Colani.) Sodium uranium pyrophosph&te, 3UO 2 , 6Na 2 O, 4P 2 O 6 . Sol. in acids. (Colani.) Sodium uranyl phosphate, Na 2 O, UO 3 , P 2 O 5 . (Ouvrard, C. R. 110. 1333.) 2Na 2 O, UO 3 , P 2 O 5 . (Ouvrard.) Na 2 O, 5UO 3 , 2P 2 O 5 +3H 2 O. Insol. in H 2 O; decomp. by acetic acid. (Werther, A. 68. 312.) Sodium uran3'l p^/rophosphate. Very sol. in H 2 O. (Persoz, A. ch. (3) 20. 322.) Sodium ytterbium p?/rophosphate, NaYbP 2 7 . Easily sol. in the strong acids. (Wallroth.) Sodium yttrium p?/rophosphate, NaYP 2 7 . Sol. in H 2 O. (Stromeyer.) Insol. in H 2 O. Easilv sol. in strong acids. (Wallroth.) PHOSPHATE, STRONTIUM THORIUM 709 Sodium zinc /nphosphate, Na 2 O, 4ZnO, 3P 2 O 5 + 19H 2 O. Sol. in H 2 O. (Schwarz, Z. anorg. 1895, 9. 266.) Sodium zinc tfn'raetaphosphate, Na 2 O, 2ZnO, 3P 2 5 . Ppt. Sol. in H 2 O. (Fleitmann and Henne- berg, A. 65. 304.) Sodium zinc tetrametaphospha.te, Na 2 Zn(PO 3 ) 4 +6H 2 O. As K comp. (Glatzel, Dissert. 1880.) Sodium zinc ocfowetaphosphate, Na 2 Zn 3 (PO 3 )8 Insol. in acids. Sol. in cone. H 2 SO 4 . (Tammann, J. pr. 1892, (2) 45. 420.) Sodium zinc orthophosphate, NaZnP0 4 . Difficultly sol. in H 2 O or acetic acid. Easily sol. in dil. mineral acids. (Scheffer, A. 145. 53.) 2Na 2 O, ZnO, P 2 O 5 . Insol. in H 2 O; sol. in dil. acids. (Ouvrard, C. R. 106. 1796.) Sodium zinc /M/rophosphate, Na 2 ZnP 2 O 7 . Insol. in H 2 O; sol. in dil. acids. (Wall- roth.) 3Na 4 P 2 O 7 , Zn 2 P 2 O 7 +24H 2 O. Very efflores- cent. (Pahl.) Na 4 P 2 O 7 , Zn 2 P 2 O 7 +2H 3, 3y 2 , and 8H 2 O. Insol. in H 2 O; sol. in Na 4 P 2 O 7 +Aq. (Pahl, Sv. V. A. F. 30, 7. 35.) 4Na 4 P 2 O 7 , 5Zn 2 P 2 O 7 +20H 2 O. Insol. in H 2 O. (Pahl.) Na 4 P 2 O 7 , 4Zn 2 P 2 O 7 + 12H 2 O. SI. sol. in H 2 O. (Pahl.) Sodium zirconium phosphate, Na 2 O, 4ZrO 2 , 3P 2 O 5 = NaZr 2 (PO 4 ) 3 . Insol. in acids or aqua regia. (Troost and Ouvrard, C. R. 105. 30.) 6Na 2 O, 3ZrO 2 , 4P 2 O 5 . Sol. in acids. (T. and 0.) 4Na 2 O, ZrO 2 , 2P 2 O 6 . Sol. in acids. (T. and O.) Sodium phosphate fluoride, Na 3 PO 4 , NaF + 12H 2 O. 100 pts. H 2 O dissolve, at 25, 12 pts. salt and form solution of 1.0329 sp. gr.; at 70, 57.5 pts. salt and form solution of 1.1091 sp. gr. (Briegleb, A. 97. 95.) 2Na 3 PO 4 , NaF+19H 2 O, and 22 H 2 O. Sol. in H 2 O. (Baumgarten, J. B. 1865. 219.) Sodium phosphate stannate, 4Na 3 PO 4 , Na 2 SnO 3 +4SH 2 O. (Prandtl, B. 1907,. 40. 2132.) Sodium phosphate titanate, NazO, TiO 3 , P 2 O 5 +3H 2 O. Hygroscopic. (Mazzuchelli and Pantan- elli, C. C. 1909, II. 420.) Sodium phosphate vanadate. See Phosphovanadate, sodium. Strontium wonoraetaphosphate, Sr(PO 3 ) 2 . Insol. in H 2 O and acids. Not decomp. by alkali carbonates +Aq. (Maddrell, A. 61. 61.) Strontium hexametaphosph&te. Nearly insol. in H 2 O; easily sol. in acids. (Ludert, Z. anorg. 5. 15.) Strontium or^ophosphate, basic, Sr(OH) 2 , Sr 3 (PO 4 ) 2 . (Woyczynski, Z. anorg. 1894, 6. 311.) Strontium or/Aophosphate, Sr 3 (PO 4 ) 2 . Insol. in H 2 O. Sol. in HCl+Aq. (Erlen- meyer, J. B. 1857. 145.) Strontium hydrogen phosphate, SrHPO 4 . Insol. in H 2 O. Sol. in H 3 PO 4 , HC1, or HNO 3 -|-Aq. (Vauquelin.) Easily sol. in cold ammonium nitrate, chloride, or suc- cinate+Aq, but is partly precipitated by a little NH 4 OH+Aq. (Brett.) Sol. in boiling NH 4 Cl+Aq. (Fuchs, 1834.) Sol. in Na citrate +Aq. (Spiller.) Partly decomp. by boiling Na 2 CO 3 , and K 2 CO 3 +Aq. (Dulong.) SrH 4 (PO 4 ) 2 +2H 2 O. Decomp. by treating with H 2 O, leaving 4.29%SrHPO 4 . (Barthe.) Strontium phosphate, acid, H->O, 2SrO, 3P 2 O 5 +zH 2 O. Entirely sol. in H 2 O. (Barthe, C. R. 114. 1267.) Strontium p^/rophosphate, Sr 2 P 2 O 7 -fH 2 O. Somewhat sol. in H 2 O. Easily sol. in HC1 or HNO 3 +Aq. Insol. in HC 2 H 3 O 2 or Na 4 P 2 O 7 -|-Aq. (Schwarzenberg, A. 65. 144.) +2}/6H,O. (Knorre and Oppelt, B. 21. 773.) Strontium hydrogen pyrophosphsite, SrH 2 P 2 O 7 , 2Sr,P 2 O 7 +6H 2 O. Ppt. (Knorre and Oppelt, B. 21. 772.) SrH 2 P 2 O 7 , 3Sr 2 P 2 O 7 +H 2 O, and +2H 2 O. (Knorre and Oppelt.) Sr 9 H 2 (P 2 O 7 ) 6 +8H 2 O, and +12H 2 O. Ppt. (Pahl, Gm. - K. 2, 2. 172.) Sr 19 H 2 (PoO 7 ) 10 +5H 2 O, +18H 2 O and +20H 2 O. Insol. in Sr(NO 3 ) 2 +Aq or Na 4 P 2 O 7 +Aq. (Pahl, Gm.-K. 2, 2. 171.) Strontium thorium phosphate, Th 2 O. SrO, P 2 O 5 . (Colani, C. R. 1909, 149. 209.) 710 PHOSPHATE, STRONTIUM URANIUM Strontium uranium raetaphosphate, UO 2 , SrO, P 2 O 5 . (Colani, A. ch. 1907, (8) 12. 141.) Strontium uranyl phosphate, SrO, 4UO 3 , 2P 2 O 5 +21H 2 O. (Blinkoff, Dissert. 1900.) 2SrO, 5UO 3 , 2P 2 O 6 +24H 2 O. As Ba comp. (Blinkoff.) Strontium phosphate chloride, 3Sr 3 (PO 4 ) 2 , Strontium apatite. Insol. in H 2 O. (De- ville and Caron.) Tellurium phosphate (?). Insol. in H 2 O. (Berzelius.) Thallous wetaphosphate, T1PO 3 . Two modifications: a. Difficultly sol. in H 2 O. j8. Extremely easily sol. in H 2 O. (Lamy.) Thallous ort/bphosphate, T1 3 PO 4 . 1 pt. is sol. in 201.2 pts. H 2 O at 15, and 149 pts. boiling H 2 O; sol. in HNO 3 +Aq. (Crookes.) SI. sol. in HC 2 H 3 O 2 +Aq. Very easily sol. in solutions of NH 4 salts. (Car- stanjen.) Insol. in alcohol. (Lamy.) Thallous hydrogen phosphate, T1 2 HPO 4 . Anhydrous. Much less sol. in H 2 O than the hydrous salt, but easily sol. in a solution of the hydrous salt. (Lamy.) + ^H 2 O. Easily sol. in H 2 O. Insol. in alcohol. (Lamy.) Composition is HT1 2 PO 4 , 2H,T1PO 4 . (Rammelsberg, W. Ann. 16. 694.) Thallous cfthydrogen phosphate, T1H 2 PO 4 . Verv easily sol. in H 2 O. Insol. in alcohol. (Rammelsberg, B. 3. 278.) Tnthallous tfnhydrogen phosphate, T1 2 HPO 4 . 2T1H 2 PO 4 . True composition of T1 2 HPO 4 of Lamy. (Rammelsberg.) Thallous pyrophosphate, T1 4 P 2 O 7 . Sol. in 2.5 pts. H 2 O with slight decomposi- tion. (Lamy.) +2H 2 O. More sol. in H 2 O than the above salt, with partial decomp. (Lamy.) Thallous hydrogen pyrophosphate, H 2 T1 2 P 2 O 7 +H 2 O. Very sol. in H 2 O. (Lamy.) Thallic phosphate, basic, 2T1 2 O 3 , P 2 O 6 + 5H 2 O. Insol. in H 2 O. ThaUic phosphate, basic, T1 8 P 9 O 27 + 13H 2 O. (Rammelsberg, W. Ann. 16. 694.) T1, ; P 4 19 +12H 2 0. (R.) Thallic phosphate, T1PO 4 +2H 2 O. Completely insol. in H 2 O. Sol. in cone. HNO 8 , and dil. HCl+Aq. (Willm.) Thorium metophosphate, Th(PO 3 ) 4 . Insol. in H 2 O. (Troost, C. R. 101. 210.) Thorium wetaphosphate, ThO 2 , 2P 2 O 5 . Insol. in acids. (Johnsson, B. 22. 976.) Thorium ort/wphosphate, Th 3 (PO 4 ) 4 +4H 2 O. Insol. in H 2 O and phosphoric acid (Ber- zelius); also acetic acid. (Cleve.) Sol. in HC1, and HNO 3 +Aq. (Cleve.) Thorium hydrogen phosphate, ThH 2 (PO 4 )o-f H 2 0. Precipitate. Thorium pi/rophosphate, ThP 2 O 7 +2H 2 O. Precipitate. Insol. in H 2 O. Sol. in great excess of pyrophosphoric acid or sodium pyro- phosphate+Aq. (Cleve.) Thorium phosphate bromide. See Bromophosphate, thorium. Thorium phosphate chlroide. See Chlorophosphate, thorium. Tin (stannous) phosphate, 5SnO, 4P 2 O 5 + 4H 2 O. Insol. in H 2 O. (Lenssen, A. 114. 113.) Sn 3 (PO,f) 2 . Insol. in HO. Sol. in mineral acids. (Kiihn.) Insol. in NH 4 C1 or NH 4 NO 3 +Aq. Sol. in KOH+Aq. Tin (stannic) phosphate, 2SnO 2 , P 2 O c -f 10H 2 0. Insol. in H 2 O or HNO 3 + Aq. (Reynoso, J. pr. 54. 261.) Anhydrous. Insol. in acids. (Hautefeuille and Margottet, C. R. 102. 1017.) Tin (stannic) phosphate, SnP 2 O 7 . Insol. in acids. (Hautefeuille and Margot- tet, C. R. 102. 1017.) Tin (stannous) phosphate chloride, 3SnO, P 2 5 , SnCla+HW). Not decomp. by hot H 2 O. (Lenssen, A. 114. 113.) Titanium phosphate, Ti 2 PA> = 2TiO 2 , P 2 O 6 . Insol. in acids. (Hautefeuille and Margot- tet, C. R. 102. 1017.) (Ouvrard, C. R. 111. 177.) +3H 2 O. Ppt. Insol. in H 2 O. (Merz.) PHOSPHATE, YTTRIUM 711 TiO a , P 2 O 6 . (Knop.) Is NaTi 2 (PO 4 ) 3 . (Wunder, J. B. 1871. 324.) H 8 TiP0 7 . Sol. in HC1, HNO 8 , H 2 S0 4 . SI. sol. in H 3 PO 4 . Sol. in KOH, NH 4 OH, (NH 4 ) 2 CO 3 and (NH 4 ) 2 HP0 4 +Aq. Very si. sol. in acetic acid. (Faber, Z. anal. 1907, 46. 288.) Uranous wetaphosphate, U(PO 3 ) 4 . Insol. in HNO 3 , HC1, or H 2 SO 4 , even when hot and cone. (Colani, A. ch. 1907, (8) 12. 105.) Uranic raetophosphate, U 2 (PO 3 )c. Insol. in H 2 O and acids. (Plautefeuille and Margottet, C. R. 96. 849.) Uranous or^ophosphate, U 3 (PO 4 ) 4 . More easily attacked by acids than the pyro and meta phosphates, especially by HNO 3 . (Colani, A. ch. 1907, (8) 12. 123.) Uranous hydrogen ortAophosphate, tJHPO 4 + H 2 O. Insol. in H 2 O. Insol. in dil., si. sol. in cone. HCl+Aq. Decomp. by KOH+Aq, not by NH 4 OH+Aq. (Rammelsberg, Pogg. 59. 1.) Uranous p?/r0phosphate, UP 2 O 7 . Insol. in H 2 O. SI. sol. in min. acids. (Colani.) Uranous phosphate, 2U0 2 , P 2 O 5 . Easily attacked by boiling HNO 3 . (Colani.) UO 2 , P 2 O 6 +5H 2 O. Insol. in H 2 S0 4 and in HCl+Aq of medium concentration. Sol. in very cone. HCl+Aq. (Aloy, Dissert. 1901.) Uranyl wetaphosphate, UO 2 (PO 3 ) 2 . (Rammelsberg, B. A. B. 1872. 447.) UO 3 , 2P 2 O 5 . Insol. in acids. (Johnsson, B. 22. 976.) Uranyl or^ophosphate, UO 2 HPO 4 +1^H 2 O. Insol. in H 2 O. +3HoO. +4H 2 "0. +4VH 2 O. Insol. in H,O. Sol. in 67,000 pts. HC 2 H 3 O 2 +Aq, 50,000 pts. NH 4 C 2 H 3 O 2 + Aq, and 300,000 pts. of a mixture of the above two solutions. Sol. in K 2 CO 3 or Na 2 CO 3 + Aq. (Kitschin, C. N. 27. 199.) Uranyl cfthydrogen phosphate, UO 2 H 4 (PO 4 ) 2 +3H 2 0. Decomp. by H 2 O. Sol. in H 3 PO 4 +Aq. (Werther,J.pr.43.322.) Uranyl p^/rophosphate, (UO 2 ) 2 P 2 O 7 +5H 2 O. Efflorescent. Insol. in H 2 O. Sol. in HNOs+Aq, and Na 4 P 2 O 7 +Aq. Insol. in Na 2 HPO 4 +Aq. Insol. in alcohol or ether. (Girard, C. R. 34. 22.) +4H 2 O. (Casteing, Bull. Soc. (2) 34. 20.) Uranyl tetraphosphate (?), UO 2 P 4 On. (Johnsson, B. 22. 978.) Uranous ortftophosphate chloride, U 3 (PO 4 ) 4 , UC1 4 . SI. sol. in HCl+Aq. Sol. in HNO 3 and HNOs+HCl. (Colani, A. ch. 1907, (8) 12. 127.) Uranous hydrogen or^ophosphate chloride, U(HPO 4 ) 2 , UC1 4 . Very si. sol. in H 2 O. (Aloy, Dissert. 1901.) Vanadium phosphate, (VO 2 )H 2 PO 4 +4^H 2 O. Sol. in H 2 O. See Phosphovanadic acid. Vanadium pi/rophosphate, V 4 (P 2 O 7 ) 3 +30H 2 O. Insol. in H 2 O. (Rosenheim, B. 1915, 48. 590.) Divanadyl phosphate. Very deliquescent, and sol. in H 2 O. Insol. in alcohol. (Berzelius.) Ytterbium wetophosphate, Yb(PO 3 ) 3 . Insol. in H,O. (Cleve, Z. anorg. 1902, 32. 149.) Ytterbium ortfiophosphate, YbPO 4 +43/H 2 O. Ppt. (Cleve.) Ytterbium phosphate, Yb 2 O 3 , 2P 2 O 5 +5H 2 O. Sol. in H 2 O. (Cleve.) Yttrium wetophosphate, Y(PO 3 ) 3 . Insol. in H 2 O or acids. (Cleve.) Yttrium ortftophosphate, YPO 4 . Anhydrous. Insol. in H 2 O or acids after ignition. Min. Xenotime. Insol. in cone, acids. SI. sol. in much cone. HCl+Aq, but easity sol. therein when first heated with a little HC1+ Aq. (Wartha, A. 139. 237.) Yttrium hydrogen or^ophosphate, Y 2 (HPO 4 ) 3 . Decomp. by boiling with H 2 O into insol. YPO 4 and sol. acid salt. Yttrium p?/rophosphate, YHP 2 O 7 +3KH 2 O. Difficultly sol. in acids. Decomp. by H 2 SO 4 . Sol. in Na 4 P 2 O 7 +Aq. (Cleve.) 2Y 2 O 3 , 3P 2 O ft . Insol. in acids. (Johnsson, B. 22. 976.) 712 PHOSPHATE, ZINC Zinc raetaphosphate. Sol. in H 2 O. (Berzelius.) Zinc cftwetaphosphate, ZnP 2 O 6 . Sol. only in boiling H 2 SO 4 . (Fleitmann, Pogg. 78. 350.) Not decomp. by boiling Na 2 S or (NH 4 ) 2 S + Aq. +4H 2 O. Insol. in H 2 O, but decomp. by boiling therewith. (Fleitmann, Pogg. 78. 25S.) Sol. in 4 pts. H 2 O. Cone. H 2 SO 4 decomp. it easily; other acids act slightly. (Glatzel, Dissert. 1880.) Difficultly decomp. by boiling acids. Zinc Znmetaphosphate, Zn 3 (PO 3 ) 6 -h 9H 2 O. 1 1. H 2 O dissolves 0.1 g. at 20 C . (Tam- mann, J. pr. 1892, (2) 45. 426.) Zinc tetrametaphosphate, Zn 2 (PO 3 ) 4 + 10H 2 O. Sol. in 55 pts. H 2 O. Decomp. by acids only on boiling. (Glatzel, Dissert. 1880.) Somewhat sol. in HNO 3 +Aq. Sol. in boiling H 2 SO 4 . (Glatzel.) Zinc or^ophosphate, Zn 3 (PO 4 ) 2 +4H 2 O. Insol. in H 2 O. Easily sol. in acids, NH 4 OH, (NH 4 ) 2 CO 3 , (NH 4 ) 2 SO 4 , or NH 4 NO 3 +Aq. (Heintz, A. 143. 356.) Sol. in NH 4 Cl+Aq. (Fuchs.) Easily sol. in Zn salts +Aq. (Rose.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Min. Hopeite. +6H 2 O. (Reynoso.) Zinc hydrogen phosphate, ZnHPO 4 +H 2 O. Insol. in H 2 O; sol. in H 3 PO 4 +Aq. (Gra- ham.) Zinc tetrohydrogen phosphate, ZnH 4 (PO 4 ) 2 + 2H 2 O. Nearly insol. in HO, but decomp. thereby into H S PO 4 and lOZnO, 4P 2 O 5 + 10H 2 O. (Demel, B. 12. 1171.) Zinc phosphate, lOZnO, 4P 2 O 5 + 10H 2 O. Insol. in H 2 O. (Demel, B. 12. 1171.) Zinc pyrophosphate, Zn 2 P 2 O 7 + 3 /2H 2 O. Ppt. Sol. in H 2 SO 3 +Aq. Sol. in acids, KOH+Aq, NH 4 OH+Aq. (Schwarzenberg, A. 65. 151.) Sol. in Na 4 P 2 O 7 +Aq (Gladstone), and in ZnSO 4 +Aq. (Rose.) Insol. in acetic acid. (Knorre, Z. anorg. 1900, 24. 389.) +5H 2 O. Insol. in H 2 O. (Pahl, J. B. 1873. 229.) Zinc hydrogen pyrophosphate. Sol. in H 2 O. (Pahl, Sv. V. A. F. 30, 7. 45.) Zinc raetaphosphate ammonia. Ppt. (Bette.) Zinc or^ophosphate ammonia, 2ZnO, P 2 O 5 , 3NH 3 +8H 2 O. (Rother, A. 143. 356.) 6ZnO, 3P 2 O 6 , 8NH 3 +4H 2 O. (Schweikert, A. 145. 517.) Zinc pyroohosphate ammonia, 3Zn 2 P 2 O 7 , 4NH 3 +9H 2 O. Ppt. Insol. in H 2 O. (Bette.) Zirconium oriAophosphate, 5ZrO 2 , 4P 2 O 5 + 8H 2 O. Somewhat sol. in acids. (Hermann, J. pr. 97. 321.) Insol. in acids. (Paykull, Bull. Soc. (2) 20. 65.) 2ZrO 2 , P 2 O 5 . Not attacked by acids. (Hautefeuille and Margottet, C. R. 102. 1017.) Zirconiuni pyrophosphate, Zr(PO 3 ) 2 . (Knop, A. 159. 36.) Phosphoricovanadicotungstic acid. Ammonium phosphoricovanadicotungstate, 14(NH 4 ) 2 O, 2P->O 3 , 7V 2 O 3 , 31WO 3 + 78H 2 O. Sol. in H 2 O. Insol. in alcohol, ether, CS 2 and benzene. (Rogers, J. Am. Chem. Soc. 1903, 25. 305.) Phosphorimidamide, PN 2 H 3 . (Joannis, C. R. 1904, 139. 365.) Phosphorimide, P 2 (NH) 3 . Very sol. in ammoniacal solution of NHJ. (Hug6t, C. R. 1905, 141. 1236.) Phosphornitryl, PON. See Phosphoryl nitride. Phosphorosomolybdic acid, P 2 O 3 , 24MoO 3 +63H 2 O. (Rosenheim and Pinsker, Z. anorg. 1911, 70. 77.) Ammonium phosphorosomolybdate, 2(NH 4 ) 2 O, 2H 3 PO 3 , 12Mo Insol. in cold, slightly sol. in hot H 2 O. (Gibbs, Am. Ch. J. 5. 361.) Phosphorosophosphomolybdic acid. Ammonium phosphorosophosphomolybdate, 9(NH 4 ) 2 O, 2H 3 PO 3 , 3P 2 O 5 , 72MoO 3 + 38H 2 O. Nearly insol. in H 2 O. (Gibbs.) PHOSPHITE, COBALTOUS 713 Phosphorosophosphotungstic acid. Potassium phosphorosophosphotungstate, 5K 2 O, 2H 3 PO 3 , P 2 O ft , 24WO 3 + 13H 2 O. Sol. in much boiling H 2 O. (Gibbs, Am. Ch. J. 7. 313.) Phosphorosotungstic acid. Ammonium phosphorosotungstate, 6(NH 4 ) 2 O, 4HPO 8 , 22WO 3 +25H 2 O. SI. sol. in cold H 2 0. Potassium , 5K 2 O, 16H 3 PO 3 , 32WO 3 + 46H 2 0. SI. sol, in hot H 2 O. Sodium , 2Na 2 O, 8H 3 PO 3 , 22WO 3 + 35H 2 O. Nearly insol. in cold, si. sol. in hot H 2 O. (Gibbs, Am. Ch. J. 7. 313.) Phosphorous anhydride, P 2 O 3 . See Phosphorus ^n'oxide. Phosphorous acid, H 3 PO 3 . Deliquescent. Very sol. in H 2 O. Phosphites. The neutral alkali phosphites are sol. in H 2 O; most of the others are si. sol. in H 2 O, but sol. in H 3 PO 3 +Aq; all are insol. in alcohol. Aluminum phosphite, basic. A1 2 (HPO 3 )3. A1 2 (OH) 6 . Ppt. (Griitzner, Arch. Pharm. 1897, 235. 698. j Aluminum phosphite. Precipitate. . (Rose, Pogg. 9. 39.) SI. sol. in H 2 O. Ammonium phosphite, (NH 4 ) 2 HPO 3 +H 2 O. Very deliquescent, and sol. in H 2 O. (Rose, Pogg. 9. 28.) Sol. in 2 pts. cold, and less hot H 2 O. Insol. in alcohol. (Berzelius.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Ammonium hydrogen phosphite, (NH 4 H)HPO 3 . Very deliquescent, and sol. in H 2 O. 1 pt. H 2 O dissolves 1.71 pts. salt at 0; 1.9 pts. at 14.5; and 2.60 pts. at 31. (Amat, C. R. 105. 809.) Ammonium hydroxylamine phosphite, NH 4 (NH 3 OH)HPO 3 . Sol. in H 2 O and abs. alcohol. (Hofmann, Z. anorg. 1898, 16. 466.) Ammonium magnesium phosphite, (NH 4 ) 2 M g3 (PH0 3 ) 4 + 16H 2 0. Slightly sol. in H 2 O. (Rammelsberg, Pogg. 131. 367.) Antimonyl phosphite, (SbO)H 2 PO 3 . Very sol. in H 2 O containing HG1. (Griitz- ner, Arch. Pharm. 1897, 235. 694.) Barium phosphite, BaHPO 3 . 100 pts. H 2 O dissolve 0.25 pt. (lire.) Very slightly sol. in H 2 O, and decomp. by boiling H 2 O. (Dulong.) Easily sol. in H 2 O containing NH 4 C1. (Wackenroder, A. 41. 315.) Sol. in H 3 PO 3 + Aq or HC1 + Aq. (Railton.) Barium hydrogen phosphite, Ba 2 H 2 (HPO 3 ) 3 + 8PI 2 O. Easily sol. in H 2 O, but decomp. by boiling therewith. Insol. in alcohol. (Rammelsberg, Pogg. 132. 496.) Barium dihydrogen phosphite, BaH 2 (HPO 3 ) 2 Easily sol. in H 2 O. (Rose, Pogg. 9. 215.) +H 2 O. Sol. in H 2 O; decomp. by boiling H 2 O into a neutral insol., and an acid sol. salt. (Wurtz, A. 58. 66.) +2H 2 O. Easily sol. in H 2 O. (Rammels- berg, Pogg. 132. 496.) Insol. in alcohol. (Wurtz.) Bismuth phosphite, 2Bi 2 O 3 , 3P 2 O 3 . Insol. in H 2 O. Bi 2 (HPO 3 ) 3 +3H 2 O. Ppt. (Griitzner, Arch. Pharm. 1897, 235. 696.) Decomp. by H 2 S. Not decomp. by KOH +Aq. (Vanino, J. pr. 1906, (2) 74. 151.) Cadmium phosphite, CdHPO 3 +3H 2 O. Ppt. (Rose, Pogg. 9. 41.) Calcium phosphite, CaHPO 3 + 3 / 2 H 2 O. SI. sol. in H 2 O; the aqueous solution is de- comp. by boiling. +H 2 O. Sol. in NH 4 Cl+Aq. (Wacken- roder, A. 41. 315.) Insol. in alcohol. Calcium hydrogen phosphite, CaH 2 (HPO 3 ) 2 + H 2 O. Sol. in H 2 O. Aqueous solution is decomp. by alcohol. (Wurtz, A. ch. (3) 7. 212.) Chromic phosphite. Precipitate. Almost insol. in H 2 O. (Rose, Pogg. 9. 40.) Cobaltous phosphite, CoPHO 3 +2H 2 O. Ppt. SI. sol. in H 2 O. (Rose.) 714 PHOSPHITE, CUPRIC Cupric phosphite, CuHPO 3 +2H 2 O. Ppt. Insol. in H 2 O. (Wurtz, A. ch. (3) 16. 213.) Didymium phosphite, Di 2 (HPO 3 )3. Precipitate. (Frerichs and Smith, A. 191. 331.) Glucinum phosphite. Precipitate. Insol. in H 2 O. (Rose, Pogg. 9. 39.) Iron (ferrous) phosphite, FeHPO 3 +a;H 2 O. Ppt. Nearly insol. in H 2 O. (Rose, Pogg. 9. 35.) Iron (ferric) phosphite, basic, Fe 2 (HPO 3 ) 3 , Fe 2 (OH) 6 . (Griitzner, Arch. Pharm. 1897, 235. 697.) Fe 4 (HPO 3 ) 6 , Fe(OH) 3 +5H 2 O. Hydro- scopic. (Berger, C. R. 1904, 138. 1500.) Iron (ferric) phosphite, Fe 2 (HPO 3 )2+9H 2 O. Ppt. Sol. in iron alum+Aq. (Rose.) Lanthanum phosphite, La 2 (HPO 3 ) 3 . Precipitate. (Smith.) Lead phosphite, basic, 4PbO, P 2 O 3 +2H 2 O. . Ppt. (Rose, Pogg. 9. 222.) 3PbO, F 2 O,+H S 6. Insol. in H 2 O. Sol. in warm dil. H 3 PO 3 -|-Aq, from which it is pptd. by NH 4 OH+Aq. (Wurtz, A. ch. (3) 16. 214.) Lead phosphite, PbHPO 3 , Insol. in H 2 O. Very si. sol. in a solution of phosphorous acid; easily sol. in cold HNO 3 +Aq. (Wurtz.) Lead hydrogen phosphite, PbH 4 (PO 3 ) 2 ' Decomp. by H 2 O. (Amat, C. R. 110. 901.) Lead pyrophosphite, PbH 2 P 2 O 5 . Gradually decomp. by H 2 O into H 3 PO 3 and PbHPO 3 . (Amat, C. R. 110. 903.) Lithium hydrogen phosphite, LiH 2 PO 3 . Very sol. in H 2 O. (Amat, A. ch. (6) 24. 309.) Lithium p^/rophosphite, Li 2 H.,P 2 O 5 . Very sol. in H,O. (Amat. A. oh. 1891, (6) 24. 352.) Magnesium phosphite, MgHPO 3 +3H 2 O. SI. sol. in H 2 O. (Rose, Pogg. 9. 28.) Sol. in 400 pts. H 2 O. (Berzelius.) +4H,0. Magnesium pyrophosphite, Mg(H 2 PO 3 ) 2 . Very sol. in H 2 O. (Amat. A. ch. 1891, (6) 24. 313.) Manganous phosphite, Difficultly sol. in H 2 O, easily in MnCl 2 or MnSO 4 +Aq.- (Rose, Pogg. 9. 33.) Nickel phosphite, NiHPO 3 +3MH 2 O. Ppt. SI. sol. in H 2 O. Potassium phosphite, K 2 HPO 3 . Very deliquescent. Very sol. in H 2 O. Insol. 'in alcohol. (Dulong'.) Potassium hydrogen phosphite, (KH)HPO 3 . 1 pt. H 2 O dissolves about 1.72 pts. salt at 20. (Arnat. C. R. 106. 1351.) K 2 HPO 3 , 2H 3 PO 3 . Very sol. in H 2 O. (Wurtz, A. 58. 63.) Sol. in 3 pts. cold, and in less hot H 2 O. (Fourcroy and Vauquelin.) Potassium pyrophosphite, K 2 H.,P 2 O5. Very sol. in H 2 O. (Amat. A, ch. (6) 24. 351.) Sodium phosphite, basic, Na 2 HPO 3 , NaOH (?). Not obtained in pure state (Zimmerman, B. 7. 290);=Na 8 PO (Wislicenus.) Does not exist. (Amat.) Sodium phosphite, Na 2 HPO 3 +5H,O. Deliquescent, and very sol. in H 2 0. In- sol. in alcohol. Correct formula for Na 3 PO 3 of Rose and Dulong. Sodium hydrogen phosphite. (NaH)HPO 3 -f 0.56 pt. salt dissolves in 1 pt. H 2 O at 0; 0.66 pt. at 10; 1.93 pts. at 42. (Amat, C. R. 106. 1351 j Na 2 H 4 (HPO 3 ) 3 +H 2 O. Deliquescent in moist air. Sol. in 2 pts. cold, and about the same amt. hot H 2 O. SI. sol. in spirit. (Four- croy and Vauquelin.) Sodium pyrophosphite, Na 2 H 2 P 2 O5. Very sol. in H 2 O with gradual decomp. into Na 2 HPO 3 . (Amat.) Strontium phosphite, SrHPOa + l Difficultly sol. in H 2 O. Aqueous solution decomp. on heating into a sol. acid salt and an insol. basic salt. Strontium hydrogen phosphite, SrH 4 (PO 3 ) 2 . Very sol. in H 2 O. (Amat, A. ch. (6) 24. 312.) Thallous hydrogen phosphite, T1H 2 PO 3 . Very sol. in H 2 O. (Amat, A. ch. (6) 24. 310.) Thallous pyrophosphite, T1 2 H 2 P 2 O 5 . Deliquescent. Very sol. in H 2 O. (Amat.) PHOSPHORUS 715 Tin (stannous) phosphite, SnHPO 3 . Ppt. Sol. in HCl+Aq. (Rose, Pogg. 9 45.) Tin (stannic) phosphite, 2SnO 2 , P 2 O 3 . Ppt. (Rose, Pogg. 9. 47.) Titanium phosphite (?) Precipitate. (Rose, Pogg. 9. 47.) Uranyl phosphite, (UO 2 ) 3 H 2 (HPO 3 ) 4 + 12H 2 O Precipitate. (Rammelsberg. Pogg. 132, 500.) Zinc phosphite, ZnHPO 3 . Sol. in H 2 O. (Rammelsberg, Pogg. 132. 481.) +2;HjH 2 O. More easily sol. in cold than warm H 2 O. (Rammelsberg.) Zinc phosphite, acid, Zn 2 H 3 P 3 O 8 . Sol. in H 2 O. +2H 2 O. Sol. in HoQ. (Rammelsberg, Pogg. 132. 498.) Zn 3 H 5 P 5 O 13 . Sol. in H 2 O. +3H 2 O. Sol. in H 2 O. (Rammelsberg.) Zn 2 H 9 P 5 O J4 . Sol. in H 2 O. -fH 2 O. Sol. in H 2 O. (Rammelsberg.) Zirconium phosphite, Zr(PO 3 )->+H 2 O. Ppt. Nearly insol. in dil. mineral acids. (Hauser, Z. anorg. 1913, 84. 92.) Phosphorous anhydride, P 2 O 3 . See Phosphorus ^noxide. Phosphorus, P. (a) Ordinary white phosphorus. Insol. in H 2 O, but slowly decomp. thereby (G. K.); very si. sol. in H 2 O. (Berzelius and others.) A pure aqueous solution containing 0.1 g. P in 500 cc. H 2 O can be obtained by dissolv- ing 0.1 g. P in CS 2 mixed with ether and hot alcohol; this solution is poured into 500 cc. boiling H 2 O free from air, and the boiling continued with stirring until the alcohol, ether and CS 2 are boiled off. (Bokorny, Ch Ztg 1896, 20. 1022.) 100 g. H 2 O sat. with P contains 0.0003 g P. (Stich, C. C. 1903, 1. 1291.) Sol. with decomp. in hot cone. HNO 3 +Aq. Decomp. by boiling caustic alkalies +Aq Easily sol. in SC1 2 , especially if hot. (Woh- ler.) Sol. in sulphur phosphides. Largely sol. in PC1 3 . Easily sol. in PC1 6 . Sol. in PBr 3 . Sol. in PSC1 3 , easily on warm- ing, separating on cooling. (Serullas, A ch. 1829, 42. 25.) Sol. in liquid SO 2 . (Sestini, Bull Soc 1868, (2) 10. 226.) Sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. in S 2 C1 2 without foaming. (Nicolardot, C. R. 1908, 147. 1304.) Sol. in PS 4 C1 5 . (Gladstone, A. 1850, 74. 91.) Sol. in 320 pts. cold alcohol of 0.799 sp. gr., and in 240 pts. of the same when warm. Pptd. from alcoholic solution by H 2 O. (Biich- ner.) One grain P dissolves in 1 ounce abs. alco- hol. (Schacht.) Sol. in 20 pts. absolute ether at 20 and 240 pts: ordinary ether at 20. (Bucholz.) Sol. in 80 pts. absolute ether at 15.5, and 240 pts. ordinary ether at 15.5. (Brug- natelli, A. ch. 24. 73.) Solubility of P 4 in 100 g. ether at t. t G. phosphorus Sp. gr. 0.4335 5 0.62 8 0.79 ' 10 0.85 15 0.9 at 13 0.7257 18 1.005 20 1.04 at 190.7i87 23 1.121 25 1.39 0.7283 28 1.601 30 1.75 33 1.8 35 1 . 9984 (Christomanos, Z. anorg. 1905, 46. 136.) Solubility of P 4 in 100 g. benzene at t. t G. phosphorus Sp. gr. 1.513 5 1.99 8 2.31 10 2.4 15 2.7 at 13 0.8959 18 3.1 20 3.21 at 19 0.8912 23 3.3995 at 22 0.8875 25 3.7 0.8861 28 4.35 . . . 30 4.601 . . 33 5.0 . . 35 5.17 . . . 40 5.75 45 6.105 50 6.8 55 7.315 . . . 60 7.9 . . . 65 8.4 . . 70 8.898 . . . 75 9.4 81 10.027 (Christomanos.) 716 PHOSPHORUS Sol. to about 1% in acetic acid. (Vulpius, Arch. Pharm. 1878, 213. 38.) 100 g. 96% acetic acid dissolve 0.105% P. (Stich, Pharm. Ztg. 1903, 48. 343.) Sol. in 0.05 pt. CS 2 (Bottger); 0.125 pt. (Trommsdorf.) Alcohol ppts. P from CS 2 solution. 1 pt. CS 2 dissolves 17-18 pts. P. (Vogel, J. B. 1868. 149.) Solubility in CS 2 at t, (g. per 100 g. of solution.) t G.P 4 t G,P 4 -10 -7.5 -5 -3.5 -3.2 31.40 35.85 41.95 66,14 71 . 72 -2.5 0.0 +5.0 +10.0 75.00 81.27 86.30 89.80 (Cohen and Inouye, Z. phys. Ch. 1910, 72. 418.) Very sol. in methylene iodide. (Retgers, Z. anorg. 3. 343.) Strong vinegar dissolves P. (Beudet.) Sol. in considerable amount in stearic acid. (Vulpius, Arch. Pharm. (3) 13. 38.) Sol. in ethyl chloride, benzoyl chloride, stannic chloride, and in liquid cyanogen. SI. sol. in ethyl nitrite, and wood-spirit. SI. sol. in acetone, with gradual decomposi- tion. Insol. in nicotine, and coniine. SI. sol. in cold, more sol. in hot benzene. (Mansfield.) Sol. in 14 pts. hot, and less in cold petro- leum from Amianp. (Saussure.) SI. sol. in "liquid paraffine." (Crismer, B. 17. 649.) SI. sol. in warm essential oils, as oil of tur- pentine, and in the fatty oils. Sol. in hot oil of copaiba, separating out on cooling. Sol. in hot oil of caraway, and mandarin oil. (Luca.) SI. sol. in cold, more sol. in hot caoutchin, depositing on cooling. Readily sol. in warm, less in cold styrene. Sol. in aniline, and quinoline. (Hofmann.) SI. sol. in cold creosote. Somewhat sol. in fusel oil. Easily sol. in valerianic acid, and amyl valerate. Sol. in hexyl alcohol, ethylene chloride, allyl sulphocyanide, mercury methyl, chloro- form, bromoform, warm chloral, acetic ether, aldehyde, hot cacodyl sulphide, and in cacodyl oxide. 100 g. oil of almonds sat. with P contain 1.25 g. (Stich, C. C. 1903, I. 1291.) 100 g. oleic acid sat. with P contain 1.06 g. (Stich.) 100 g. paraffine sat. with P contain 1. g. (Stich.) (b) Amorphous phosphorus. Insol. in H 2 O. Insol. in NH 4 OH+Aq. (Fliickiger.) Sol. in boiling KOH+Aq. The statement of Burgess and Chapman, (Chem. Soc. 79. 1235) that red P is sol. in aqueous alcoholic alkali is incorrect. Both ordinary crystalline and amorphous red P are insol. in aqueous alcoholic alkali. (Michaelis, A. 1902, 325. 367.) Insol. in liquid NH 3 . (Hugot, A. ch. 1900 (7) 21, 31); (Franklin, Am. Ch. J. 1898, 20. 828.) Bright red variety is sol. in liquid NH 3 at ord. temp, leaving a black residue. (Stoch, Bottcher and Lenger, B. 1909, 42. 2854.) Red. Amorphous. Sol. in S 2 C1 2 with foaming. (Nicolardot, C. R. 1908, 147. 1304.) Solubility of amorphous bright red P4 in PBr 3 is diminished by long heating as follows: 172 185 Initial concentration . 555 . 476 Final concentration . 374 . 397 Length of expt. in hours 34 24 198 218 0.592 0.476 0.416 0.592 18 17 {Buck, Dissert. 1904.) Ordinary amorphous P 4 is sol. in PBr 3 . A sample prepared by heating bright red amorphous P with 94.2% P dissolved by heating in PBr 3 as follows: %P 0.106 0.121 0.178 hours 10 20 42 A finely pulverized commercial product containing 98.0% P: %P 0.92 0.116 hours 10 20 An ordinary commercial product with 98% P: %P 0.056 0.108 hours 10 42 (Buck.) 100 g. PBr 3 dissolve 0.2601 g. bright red phosphorus at 172; 0.3634 g. at 184. (Schenk, B. 1902, 35. 353.) Insol. in KOH+Aq. Cone. H 2 SO 4 does not act upon it in the cold, but dissolves easily when hot. Insol. in dil., easily sol. in cone. HNO 3 + Aq with decomposition. Much more sol. in HNO 3 +Aq than ordi- nary P. (Personne, C. R. 45. 115.) Insol. in methylene iodide. (Retgers.) Appreciably sol. in isobutyl alcohol. (Svedberg.) Insol. in CS 2 , alcohol, ether, naphtha, ligroine, PCls, etc. SI. sol. in boiling oil of turpentine and PHOSPHORUS PLATINIC CHLORIDE 717 other high-boiling liquids, with conversion into ordinary phosphorus. Insol. in oil of turpentine even at 270. (Colson, A. ch. 1908, (8) 14. 554.) (c) Crystalline. Insol. in, and not attacked by dil. HNO 3 +Aq. Sol. in CS 2 . Phosphorus ^n'bromide, PBr 3 . Decomposed by H 2 O, slowly at 8, but very rapidly at 25. (Lowig, Pogg. 14. 485.) Sol. in liquid H 2 S. (Antony and Magri, Gazz. ch. it. 1905, 35. (1) 206.) Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 27.) Sol. in ether, acetone, CHC1 3 , C 6 H 6 and CS 2 . (Christomanos, Z. anorg. 1904, 41. 287.) Phosphorus pentabromide, PBr 6 . Fumes on air, and is violently decomp. by H 2 0. Phosphorus ^nbromide ruthenium bromide, Ru 2 P 5 Bri 9 . Decomp. by boiling H 2 O. Slowly sol. in hot alcohol with decomp. Insol. in benzene, CC1 4 , ligroin and cold alcohol. (Strecker, B. 1909, 42. 1775.) Phosphorus thiophosphoryl bromide, PBr 3 , PSBr 3 . Decomp. by H 2 O into PSBr 3 . (Michaelis.) Phosphorus ^nbromide ammonia, 3PBr 3 , 5NH 3 . Slowly but completely sol. with decomp. in H 2 O. (Storer's Diet.) Phosphorus pentabromide ammonia. PBr 5 , 9NH 3 . (Besson, C. R. 111. 972.) Phosphorus wonobromo^rachloride, PBrCl 4 . Decomp. by H 2 O. (Prinvault, C. R. 74. 868.) Phosphorus e&bromo/nchloride, PCl 3 Br 2 . Very unstable. (Michaelis, B. 5. 9.) Phosphorus ^rabromo^nchloride, PCl 3 Br 4 . Decomp. with H 2 O. (Geuther.) Phosphorus heptdbromodichlonde, PCl 2 Br 7 . Very unstable. (Prinvault, C. R. 74. 868.) Phosphorus octobromo^nchloride, PCl 3 Br 8 . Very easily decomp. (Michaelis, B. 6. 9.) Phosphorus bromofluoride, PF 3 Br 2 . Decomp. violently with H 2 O. (Moissan, Bull. Soc. (2) 43. 2.) Phosphorus bromonitride. See Nitrogen bromophosphide. Phosphorus bichloride, P 2 Cl4. Decomp. by H 2 O. (Besson, C. R. 1910. 150. 103.) Phosphorus trichloride, PC1 3 Gradually decomp. by H 2 O. 0.11 g. is sol. in 100 ccm. liquid H 2 S. (An- tony, Gazz. ch. it. 1905, 35 .(1) 206.) Acted upon by liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Miscible with CS 2 , C 6 H 6 , CHC1 3 , and ether. Decomp. with alcohol. Phosphorus pentochloride, PC1 5 . Very deliquescent, and sol. in H 2 O with violent decomp. and evolution of heat. Sol. in liquid HC1. Acted upon by liquid NH 3 . Somewhat sol. without decomp. in CS 2 . (Schiff, A. 102. 118. (Franklin, Am. Ch. J. 1898, 20. 828.) Sol. without decomp. in benzoyl chloride. (Gerhardt.) Sol. in oil of turpentine with evolution of heat. Monophosphorus platinous chloride, PC1 3 . PtCl 2 . Deliquescent. Sol. in H 2 O with formation of chloroplatinophosphoric acid. Similarly decomp. by alcohol. Abundantly sol. in hot benzene, toluene, chloroform, or carbon tetra- chloride, and crystallizes on cooling. (Schtit- zenberger, Bull. Soc. (2) 17. 482.) Diphosphorus platinous chloride, 2PC1 3 , PtCl 2 . Decomp. by H 2 O with formation of chloro- platinodiphosphoric acid. Similarly decomp. by alcohol. Sol. without decomp. in PC1 3 , CC1 4 , CHC1 3 , C 6 H 6 , orC 7 H 8 . (Schiitzen- berger.) Sol. in propyl alcohol with formation of the propyl ether of platinochlorophosphor- ous acid and HC1. (Pomey, C. R. 104. 364.) Phosphorus diplatinous chloride, PC1 3 , 2PtCl 2 . Sol. in alcohol, with formation of ether (PtCl 2 ) 2 P(OC 2 H 5 ) 3 . (Cochin, C. R, 86. 1402.) Phosphorus platinic chloride, PC1 3 , (Schiitzenberger.) Phosphorus pentachloride platinic chloride, PC1 6 , PtCl 4 , or (PCl 4 ) 2 PtCl 6 . Decomp. at once by H 2 O. (Baudrimont, A. ch. (4) 2. 47.) 718 PHOSPHORUS SELENIUM CHLORIDE Phosphorus pentacbloride selenium tetra- chloride, 2PC1 5 , SeCl 4 . Sol. in H 2 O with decomp. (Baudrimont, A. ch. (4) 2. 5.) Phosphorus ^nchloride ruthenium chloride, Ru 2 P 5 Cl 19 . Slowly decomp. by boiling H2O. Sol. in benzene and CHC1 3 . SI. sol. in CC1 4 . Insol. in ligroin. (Strecker, B. 1909, 42. 1774.) Phosphorus tellurium chloride, PC1 5 , 2TeCl 4 . Very deliquescent. Sol. in H 2 O. (Metzner, A. ch. 1898, (7) 15. 203.) Phosphorus pentochloride stannic chloride, PC1 5 , SnCl 4 . Very deliquescent. Sol. in much H 2 O with evolution. of heat, forming SnCl 4 , HC1, and H 3 PO 4 , and soon separates out stannic phos- phate. (Casselmann, A. 83. 257.) Phosphorus ^nchloride titanium chloride, PC1 3 , Til 4 . (Bertrand, Bull. Soc. (2) 33. 565.) Phosphorus pentachloride titanium chloride, PC1 6 , TiCl 4 . Deliquescent. Decomp. by H 2 O and alco- hol. Sol. in ether. SI. sol. in PC1 3 . (Tiitts- chew, A. 141. 111.) Completely sol. in dil. acids. (Weber.) Phosphorus uranium perctachloride, PC1 5 , UC1 5 . Decomp. with H 2 O. Phosphorus pentacbloride zirconium chloride, PC1 5 , ZrCl 4 . Decomp. by H 2 O with pptn. of Zr phos- phate. (Paykull.) Phosphorus trichloride ammonia, PC1 3 , 5NH 3 . Insol. as such in H 2 0, but slowly decomp. by boiling H 2 O. More easily sol. with de- comp. in acids. Sol. with decomp. by boiling with KOH or NaOH + Aq. (Berzelius.) Phosphorus pentacbloride ammonia, PC1 5 . 5NH 3 . Properties as PC1 3 , 5NH 3 . (Berzelius.) PC1 B , 8NH 3 . SI. decomp. on air. (Besson, C. R. 111. 972.) Phosphorus pentachLoride tungsten ^n'oxide, 2PC1 5 , W0 3 (?). (Persoz and Bloch, C. R. 28. 389.) Phosphorus chlorobromide. See Phosphorus bromochloride. Phosphorus chlorofluoride, PC1 2 F 3 . Absorbed by H 2 O with decomp. Absorbed by alcohol or ether. (Poulenc, A. ch. (6) 24. 555.) Phosphorus chloroiodide, PC1 3 I 2 . Decomp. by moist air or H 2 O. Sol. in CS 2 . (Most, B. 13. 2029.) Phosphorus chloronitride. See Nitrogen chlorophosphide. Phosphorus ^fluoride, PF 3 . Decomp. slowly by H 2 O. (Moissan, Bull. Soc. (2) 43. 2.) Rapidly absorbed by KOH or NaOH+Aq, slowly by BaO 2 H 2 , and K 2 CO 3 +Aq. Ab- sorbed by absolute alcohol with decomp. (Moissan, C. R. 99. 655.) Phosphorus pentofluoride, PF 5 . Fumes on air. (Thorpe, A. 182. 20.) Phosphorus pentofluoride ammonia, 2PF 5 , 5NH 3 . (Moissan, C. R. 101. 1490.) Phosphorus pentofluoride nitrogen peroxide. Decomp. by H 2 O. (Tassel, C. R. 110. 1264. Phosphorus fluobromide. See Phosphorus bromofluoride. Phosphorus fluochloride. See Phosphorus chlorofluoride. Phosphorus sw&iodide, P 4 I. Sol. in dil. HNO 3 and in alkalies +Aq. (Boulouch, C. R. 1905, 141. 257.) Phosphorus cftiodide, P 2 I 4 . Decomp. by H 2 O. Sol. in CS 2 . (Coren- winder, A. ch. (3) 30. 242.) 0.09 g. is sol. in 100 ccm. liquid H 2 S. (An- tony, C. C. 1906, I. 1692.) Phosphorus ^niodide, PI 3 . Very deliquescent. Decomp. in moist air and by H 2 O. (Corenwinder, A. ch. (3) 30. 242.) Very sol. in CS 2 . Phosphorus pentaiodide, PI 5 (?). (Hampton, C. N. 42. 180.) Phosphorus iodosulphide. See Phosphorus sulphoiodide. Phosphorus nitride, P 3 N 5 . Very slightly decomp. by long boiling with H 2 O. Completely insol. in any solvent. (Stock, B. 1903, 36. 317.) PHOSPHORUS SULPHIDE 719 Phosphorus sw&oxide, P4O. Unchanged in dry, gradually oxidized in moist air. Insol. in H 2 O, alcohol, ether, and oils; not acted on by HCl+Aq; oxidized by HNO 3 or H 2 SO 4 . (Marchand, J. pr. 13. 442.) SI. sol. in H 2 O. (le Verrier, A. 27. 167.) Forms hydrate P 4 O, 2H 2 O, which gives up its H 2 O when dried. Two modifications: (a) decomp. slowly by H 2 O or alkalies, (6) not decomp. by H 2 O or alkalies. (Reinitzer and Goldschmidt, B. 13. 847.) Is oxyphosphuretted hydrogen (?), P 4 H(OH). (Franke, J. pr. (2) 35. 341.) H 3 P 5 0. Insol. in all solvents. Decomp. by H 2 O. Not attacked by non-oxidizing acids. De- comp. by dil. alkalies. (Gautier, C. R. 76. 173.) P 4 HO. Insol. in nearly all substances. Not at- tacked by dilute acids; oxidized by ordinary HNO 3 , and cone. H 2 SO 4 at 200. Attacked by very dil. alkaline solutions. Perhaps identical with phosphorus suhoxide P 4 O. (Gautier, C. R. 76. 49.) Phosphorus oxide, P 2 O. Decomp. by heating with H 2 O at 100. (Besson, C. R. 1897, 124. 764.) Phosphorus dioxide, P 4 O 6 (formerly P 2 O 3 ), Deliquescent, but very slowly dissolved by cold H 2 O to form H 3 P0 3 . Violently decomp. by hot H 2 O or alcohol. Sol. without decomp. in ether, carbon disul- phide, benzene, or chloroform. (Thorpe and Tutton, Chem. Soc. 57. 545.) Phosphorus teZroxide, P 2 O 4 . Very deliquescent. Sol. with evolution of heat in H 2 O. (Thorpe and Fulton, Chem. Soc. 49. 833.) Phosphorus pentoxide, P 2 Os. Very deliquescent. Sol. in H 2 O with great evolution of heat, forming H 3 PO 4 . Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Insol. in acetone. (Eidmann, C. C. 1899, Q. 1014); (Naumann, B. 1904, 37. 4329.) Phosphorus sulphur oxide, P 2 O 5 , 3SO 3 = (PO) 2 (SO 4 ) 3 (phosphoryl sulphate) (?). Decomp. by H 2 O. Sol. in cold, more sol. in warm SO 3 . (Weber, B. 20. 86.) Phosphorus oxy-compounds. See under Phosphoryl compounds. Phosphorus oxy sulphide. See Phosphorus sulphoxide. Phosphorus semiselenide, P 4 Se. Decomp. with H 2 O. Insol. in cold, de- comp. by boiling KOH+Aq. Insol. in, but apparently decomp. by alcohol and ether. Easily sol. in CS 2 . (Harm, J. pr. 93. 430.) Phosphorus monoselenide, P 2 Se. Stable in dry, decomp. in moist air and by H 2 O. Insol. in alcohol and ether. Decomp. by boiling KOH+Aq. CS 2 dissolves out P. (Hahn, J. pr. 93. 430.) SI. sol. in CS 2 . (Gore, Phil. Mag. (4) 30. 414.) Phosphorous sesgmselenide, P 4 Se 3 . Sol. in CCli; si. sol. in CS 2 . (Meyer, 7. anorg. 1902, 30. 258.) Phosphorus ^nselenide, P 2 Se 3 . Decomp. by boiling H 2 O and slowly in moist air. Easily sol. in cold KOH+Aq, less easily in M 2 CO 3 +Aq. Insol. in alcohol, ether, and CS 2 . (Hahn, J. pr. 93. 430.) Phosphorus pentoselenide, P 2 Se 5 . Slowly decomp. in moist air or by H 2 O, easily by KOH+Aq or alcohol. Insol. in CS 2 . Sol. in CC1 4 . (Hahn, J. pr. 93. 430.) Phosphorus selenides with M 2 Se. See M phosphoselenide, under M. Phosphorus semisulphide, P 4 S(?). 1. Liquid. Not decomp. by, and insol. in boiled H 2 O. Insol. in alcohol and ether. SI. sol. in fats and volatile oils; decomp. by alkalies. Dissolves P on warming, with separation on cooling. Sol. in CS 2 . 2. Red modification. Not attacked at first by HNO 3 +Aq (sp. gr. 1.22), but after a time is attacked with the greatest violence. Weak acids attack only when hot. (Berze- lius, A. 46. 129.) Existence is doubtful. (Schulze, B. 13. 1862; Isambert, C. R. 96. 1628.) Phosphorus monosulphide, P 2 S(?). 1. Ordinary. Same properties as phos- phorus semsulphide, 1. 2. Red modification. Unchanged by air, H 2 O, or alcohol. Decomp. by cone. KOH + Aq, not by dilute. SI. sol. in NH 4 OH+Aq. (Berzelius, A. 46. 129.) Existence is doubtful. (Schulze; Isam- bert.) Does not exist. (Helff, Z. phys. Ch. 12. 206.) Phosphorus sesgwisulphide, P 4 S 3 . Not attacked by cold, slowly by hot H 2 O. Cold KOH+Aq dissolves with decomp. 720 PHOSPHORUS SULPHIDE Oxidized by HNO 3 and aqua regia. Sol. in alcohol and ether with decomp. Sol. in CS 2 (100 pts. CS 2 dissolve 60 pts. P 4 S 3 ), PC1 3 , and PSC1 3 . and in K 2 S or Na 2 S+Aq. (Lemoine, Bull. Soc. (2) 1. 407.) Very sol. in CS 2 . (Rebs, A. 246. 367.) Decomp. by dil. and cone. KOH+Aq. 1 pt. P 4 S 3 is sol. in 9 pts. CS 2 at-20; in 3.7 pts. CS 2 at 0; in 1 pt. CS 2 at 17; in 40 pts. benzene at 17; in 9 pts. benzene at 80; in 32 pts. toluene at 17; in 6.5 pts. toluene at 111. (Stock, B. 1910, 43. 156.) Phosphorus Zn'sulphide, P 2 S 3 . Decomp. by water. (Kekule*, A. 90. 310.) Sol. in M 2 CO 3 +Aq with separation of S. Easily sol. in KOH, NaOH, NH 4 OH+Aq. (Berzelius, A. 46. 129.) Sol. in alcohol and ether. (Lemoine.) Correct formula is P 4 S 6 . (Isambert, C. R. 102. 1386.) Extremely si. sol. in CS 2 . (Rebs, A. 246. 368.) Existence doubtful. (Helff, Z. phys. Ch. 12. 210.) Phosphorus sulphide, P 4 S 7 . SI. sol. in CS 2 . (Mai, A. 265. 192.) Slowly decomp. by cold, rapidly by hot H 2 O. Sol. in cold alkalies. 1 pt. is sol. in 3500 pts. CS 2 at 17; in 20,000 pts. at 0. (Stock, B. 1910, 43. 416.) Phosphorus bisulphide, P 3 S 6 (formerly P 2 S 4 ). Almost insol. in CS 2 . (Helff.) Phosphorus pentasulphide, P 2 S 5 . Very deliquescent. Decomp. by H 2 O. Very sol. in KOH, NaOH, NH 4 OH+Aq. Sol. in M 2 CO 3 +Aq with separation of S at low temp. Decomposes alcohol, acetic acid, etc. (Kekul<, A. 106. 331.) Sol. in CS 2 . (Isambert, C. R. 102. 1386.) Not very sol. in CS 2 . (Rebs, A. 246. 367.) Mpt., 290; bpt., 513-515 at 760 mm. Decomp. by H 2 O. Easily sol. in warm NaOH+Aq. 1 pt. is sol. in 450 pts. CS 2 at room temp.; in 550 pts. at ; in 1200 pts. at 20. (Stock, B. 1910, 43. 1225.) Ordinary form. Sol. in 195 pts. boiling CS 2 . New form. Sol. in 32 pts. CS 2 . (Stock, B. 1905, 38. 2722.) Phosphorus persulphide, P 2 S i2 (?). Decomp. by H 2 O, alkalies, etc. Consist's of S, and mechanically united P. (Ramme, B. 12. 941.) Phosphorus sulphides with M 2 S. See M Phosphosulphide, under M. Phosphorus zinc sulphide, ZnP 3 S 2 . Sol. in HCl+Aq with separation of P 3 S (?). (Berzelius, A. 46. 150.) Phosphorus ^'sulphide ammonia, P 2 S 3 , 2NH 8 . Decomp. by H 2 O. (Bineau.) Phosphorus pentosulphide ammonia, P 2 S 5 , 6NH 3 . Sol. in liquid NH 3 . (Stock, B. 1903, 36. 314.) P 2 S 5 , 7NH 3 . (Stock.) Phosphorus sulphobromide. See Thiophosphoryl bromide. Phosphorus sulphochloride. See Thiophosphoryl chloride. Phosphorus sulphoiodide, P 2 S 3 I. SI. attacked by cold, rapidly by hot H 2 O; violently decomp. by fuming HNO 3 . Easily sol. in CS 2 . SI. sol. in C 6 H 6 or CHC1 3 , and still less in ether or absolute alcohol. (Ouv- rard, C. R. 115. 1301.) P 2 S 2 I 2 . Easily sol. in CS 2 . More easily than P 4 S 3 I 2 and less than PI 3 . (Ouvrard, A. ch. 1894, (7) 2. 224.) P 2 SI 4 . Easily decomp. (Ouvrard.) P 4 S 3 I 2 . Insol. in H 2 O; sol. in warm ether. SI. sol. in benzene, CHCls and glacial acetic acid; sol. in toluene and xylene. (Wolter, Ch. Ztg. 1907, 31. 640.) Easily sol. in CS 2 . SI. sol. in benzene, ether, absolute alcohol and CHC1 3 . (Ouvrard, C. R. 1892, 115. 1301.) Phosphorus sulphoxide, P 4 O 6 S 4 . Deliquescent. Easily sol. in H 2 O with de- comp. Sol. in 2 pts. CS 2 without decomp. Sol. in benzene with decomp. (Thorpe and Tutton, Chem. Soc. 59. 1019.) P 2 2 S 3 . Slowly decomp. by H 2 O. Vio- lently attacked by fuming HN0 3 . (Besson, C. R. 1897, 124. 152.) P 4 S 3 O 4 . Deliquescent; sol. in H 2 with decomp.; insol. in most solvents. (Stock, B. 1913, 46. 1382.) Phosphoryl Jn'amide, PO(NH 2 ) 3 . Insol. in boiling H 2 O, KOH+Aq, or diL acids. Decomp. by long boiling with HC1 or HNO 3 -|-Aq. More easily decomp. with aqua regia. Easily sol. in warm H 2 SO 4 or nitrosulphuric acid. (Schiff, A. 101. 300.) Does not exist. (Gladstone; Mente, A. 248. 238.) Phosphoryl bromide, POBr 3 . Not miscible with H 2 O, but gradually de- comp. in contact with it. Sol. in H 2 SO 4 , ether, oil of turpentine (Gladstone, Phil. Mag. (3) 35. 345); in CHC1 3 , CS 2 (Baudri- mont, Bull. Soc. 1861. 118). PHOSPHOTELLURATE, AMMONIUM 721 Easily sol. in AsBr 1902, 29. 374.) (Walden, Z. anorg. Sol. in CC1 4 , and in C 6 H 6 . (Oddo, Chem. Soc. 1900, 78. (2) 75.) Phosphoryl bromide sulphide. See Thiophosphoryl bromide. Phosphoryl bromochloride, POCl 2 Br. Decomp. by H 2 O. (Menschutkin, A. 139. 343.) Phosphoryl cfaibromochloride, POClBr 2 . Decomp. by H 2 O. (Geuther, Jena Zeit. 10. 130.) Phosphoryl chloride, POC1. Very hygroscopic. Sol. in H 2 O with de- comp. Insol. in most solvents. Sol. in PC1 3 . (Besson, C. R. 1897, 125. 772.) POC1 3 . Decomp. by H 2 O. Not acted on by liquid CO 2 , P, PH 3 , CS 2 , I, Br, Cl, etc. Sol. in CC1 4 , C 6 H 6 , CS 2 , CHC1 3 and ether. (Oddo, Gazz. ch. it. 1899, 29. (2) 318; Chem. Soc. 1900, 78 (2) 74.) Phosphoryl boron chloride, POC1 3 , BC1 3 . See Boron phosphoryl chloride. Phosphoryl stannous chloride, POC1 3 , SnCl 2 . Deliquescent. Decomp. by H 2 O (Cassel- mann, A. 91. 242.) Phosphoryl stannic chloride, POC1 3> SnCl 4 . Deliquescent. Decomp. by H 2 O. (Cassel- mann.) Phosphoryl titanium chloride, POC1 3 , TiCl 4 . Deliquescent, and decomp. by H 2 O. (Weber, Pogg. 132. 453.) Pyrophosphoryl chloride, P 2 O 3 C1 4 . Decomp. violently with H 2 O. (Geuther and Michaelis, B. 4. 766.) Very sol. in H 2 O with decomp.; very un- stable. (Besson, C. R. 1897, 124. 1100.) Metophosphoryl chloride, PO 2 C1. Decomp. by H 2 0. (Gustavson.) Does not exist. (Michaelis.) Phosphoryl fluoride, POF 3 . Absorbed and decomp. at once by H 2 O or alcohol. (Moissan, C. R. 102. 1245.) Phosphoryl imidoamide, PN 2 H 3 O = PO(NH)NH 2 . Insol. in H 2 O; gradually decomp. by boiling with H 2 O, more rapidly in presence of KOH. Insol. in boiling cone. HCl+Aq. Insol. in cold, decomp. by hot H 2 SO 4 . Moderately dil. H 2 SO 4 +Aq dissolves without evolution of gas. Insol. in boiling nitric or nitrosul- phuric acid. (Gerhardt, A. ch. (3) 20. 255.) Insol. in alcohol, oil of turpentine, etc. Phosphoryl iodide, P 3 I 6 O 8 (?). Sol. in H 2 O, alcohol, and ether. (Burton, Am. Ch. J. 3. 280.) PO 2 I 2 . (Burton.) Phosphoryl nitride, PON. Insol. in H 2 O, acids, or alkalies. (Glad- stone, Chem. Soc. 2. 121.) Phosphoryl chlorosulphide, P 2 O 2 SC1 4 . Slowly decomp. in contact with H 2 O. (Besson, C. R. 1897, 124. 153.) Phosphoryl thio-campounds. See Thiophosphoryl compounds. Phosphoselenic acid. See Selenophosphoric acid. Phosphoselenide, M. See under M. Phosphosilicic acid. See Silicophosphoric acid. Phosphosilicosovanadicotungstic acid. Ammonium phosphosilicosovanadicotung- state. Exact formula not known. (E. F. Smith, J. Am. Chem. Soc. 1903, 26. 1225.) Phosphosilicovanadic acid, 3SiO 2 , 2V 2 O 6 , 2P 2 O 6 +6H 2 O. Sol. in H 2 O. (Berzelius.) Phosphostannosovanadicotungstic acid. Ammonium phosphostannosovanadicotung- state. Exact formula not known. (E. F. Smith, J. Am. Chem. Soc. 1903, 26. 1226.) Phosphosulphide, M. See under M. Phosphosulphuric anhydride, P 2 O 6 , 3SO 8 . Very easily decomp. (Weber, B. 19. 3190.) Phosphotelluric acid. Ammonium phosphotellurate, 2(NH 4 ) 2 O, P 2 O 5 , TeO 3 +4H 2 O. Easily sol. in H 2 O. (Weinland, Z. anorg. 1901, 28. 61.) 4(NH 4 ) 2 O, 3P 2 O 5 , 2TeO 3 + llH 2 O. Sol. in H 2 O without decomp. (Weinland.) 722 PHOSPHOTELLURATE, POTASSIUM Potassium phosphotellurate, 1.5K 2 O, P 2 O 6 , TeO 3 . +17.5 H 2 O. Very sol. in H 2 O. +4.5 H 2 O. Ppt. (Weinland.) Rubidium phosphotellurate, 1.5Rb 2 O, P 2 O 5 , TeO 3 +4.5H 2 O. Ppt. (Weinland.) Sodium phosphotellurate, 2Na 2 O, P 2 O 5 , 2TeO 3 +9H 2 O. Difficultly sol. in cold H 2 O. (Weinland.) Phosphothorosovanadicotunstic acid. Ammonium phosphothorosovanadicotung- state. Exact formula not known. (E. F. Smith, J. Am. Chem. Soc. 1903, 25. 1226.) Solubility in H 2 O at t. t 100 ccm. H 2 O dis- solve g. of the cryst. acid Sp. gr. of the solution 22 43 92 16.206 49.718 53.64 86.75 1.1890 1.6913 1.8264 2.5813 (Soboleff, Z. anorg. 1896, 12. 31.) Solubility in ether at t. t 100 ccm. ether dissolves g. of the cryst. acid. 7. 18. 24. 8 2 2 81.196 85.327 96.017 101 . 348 Phosphotitanosovanadicotunstic acid. Ammonium phosphotitanosovanadicotung- state. Formula not known. (E. F. Smith, J. Am. Chem. Soc. 1903, 25. 1226.) Phosphotungstic acid, P 2 O 5 , 12WO 3 + 42H 2 O. Not efflorescent. Sol. in H 2 O, alcohol, and ether. (PSchartf, C. R. 110. 754.) P 2 O 5 , 16WO 3 +69H 2 O. Very efflorescent. Sol. in H 2 O, alcohol, and ether. (Pe*chard, C. R. 109. 301.) +zH 2 O = HsPWgO;* +zH 2 O (o-phospholu- teotungstic acid). Known only in aqueous solution. (Kehrmann, B. 20. 1808.) +48H 2 O =H 3 PW 8 O 28 + 16H 2 O (a-anhydro- phospholuteotungstic acid) . Sol. in its crystal H 2 O by warmth of the hand; sol. in less than Vs pt. H 2 O. (Kehrmann.) Correct composition is represented by H 3 PW 9 O 31 +9H 2 O. (Kehrmann, Z. anorg. 1. 422.) P 2 O 5 , 20WO 3 +8H 2 O. Very efflorescent. (Gibbs, B. 10. 1386.) +19H 2 O = HnPW 10 O 3 8+8H 2 O. Sol. in H 2 O. (Scheibler, B. 5. 801.) +50, and 62H 2 O. Very efflorescent. (P6chard, C. R. 109. 301.) 3H 2 O, P 2 O 5 , 21WO 3 +30H 2 O. Efflores- cent. Sol. in H 2 O in nearly every proportion. P 2 O 5 , 22WO 3 +28H 2 O=H B PW 1 iO 43 + 18H 2 O. Efflorescent. (Scheibler, B. 5. 801.) Composition is 6H 2 O, 22WO 3 , P 2 O 5 + 45H 2 O. (Gibbs.) H 3 PO 4 , 12WO 3 + 18H 2 O, or P 2 O 5 , 24WO 3 + 39H 2 O. Sol. in H 2 O, alcohol and ether. (Soboleff, Z. anorg. 1896, 12. 18.) P 2 O 5 , 24WO 3 +40H 2 O = 6H 2 O, P 2 O 5 , 24WO 3 +34H 2 O. Very efflorescent. Sol. in H 2 O. (Gibbs.) +45H 2 O. (Soboleff.) +53H 2 O=6H 2 O, P 2 O 5 , 24WO 3 +47H 2 O. Sol. inH 2 O. (Gibbs.) Sol. in ether. If an equal vol. of ether is placed above a layer of cone, aqueous solution of acid, oily drops form between the two layers, which sink to bottom, forming a third layer. The sp. gr. of the latter is 1.525. The crystallized acid dissolved in smallest amt. ether forms an oil of sp. gr. =2.083. Ethereal solution is miscible with alcohol, and also with a large quantity of H 2 O. (Drechsel, B. 20. 1452.) +61H 2 O. Sol. in H 2 O. (Gibbs, Proc. Am. Acad. 16. 116.) Aluminum ammonium phosphotungstate. See Aluminicophosphotungstate, ammo- nium. Ammonium phosphotungstate, 3(NH 4 ) 2 O, P 2 5 , 7W0 3 +Aq. SI. sol. in cold H 2 O without decomp. De- comp. by hot H 2 O. (Kehrmann, Z. anorg. 1892, 1. 438.) 2(NH 4 ) 2 O, P 2 O 6 , 12WO 3 +5H 2 O. Insol. in cold H 2 0. (Pochard, C. R. 110. 754.) 6(NH 4 ) 2 O, P 2 O 6 , 16WO 3 +10H 2 O. Easily sol. in hot H 2 O. (Pe'chard.) 5(NH 4 ) 2 O, P 2 O 5 , 16WO 3 +zH 2 O = (NH 4 ) 5 PW 8 O 2 9+zH 2 O. (Ammonium a-phos- pholuteotungstate). SI. sol. in H 2 O. (Kehr- mann.) 3(NH 4 ) 2 O, P 2 O 5 , 16WO 3 + 16H 2 O = (NH 4 ) 3 PW 8 O 28 +8H 2 O. (Ammonium a-an- hydrophospholuteotungstate) . Efflorescent. Easily sol. in H 2 O. (Kehrmann.) 5(NH 4 ) 2 O, P 2 O 5 , 17WO 3 + 16H 2 O. Very si. sol. in cold H 2 O. (Kehrmann, Z. anorg. 1894, 6. 387.) 3(NH 4 ) 2 0, P 2 6 , 18W0 3 +14H 2 0. (Phos- pholutestungstate.) (Kehrmann, Z. anorg. 1893, 4. 140.) PHOSPHOTUNGSTATE, POTASSIUM 723 3(NH 4 ) 2 O, P 2 Os, 2lWO 3 +zH 2 O. Rather si. sol. in cold, easily in hot H 2 O and alcohol Insol. in sat. NH 4 Cl+Aq. (Kehrmann and .Freinkel, B. 25. 1972.) 3(NH 4 ) 2 O, 3H 2 O, P 2 O 5 , 22WO 3 + 18H 2 O. SI. sol. in cold H 2 O. (Gibbs.) 3(NH 4 ) 2 O, 3H 2 O, P 2 O 5 , 24WOs+26H 2 O. Very si. sol. even in hot H 2 O. (Gibbs, Proc. Am. Acad. 16. 122.) Ammonium barium a-anhydrophospholuteo- tungstate r NH 4 BaPW 8 O2*+zH 2 O = (NH 4 ) 2 O, 2BaO, P 2 O 5 , 16WO 3 +zH 2 O. Sol. in H 2 O. (Kehrmann.) Barium phosphotungstate, 2BaO, P 2 O 5 , 12WO 3 + 15H 2 O. Very efflorescent. Sol. in H 2 O; insol. in alcohol. (Pechard, C. R. 110. 754.) 3BaO, P 2 O 5 , 16WO 3 +zH 2 O = Ba 3 (PW 8 O 2S ) 4-#H 2 O. (Barium a-anhydrophospholuteo- tungstate). Not efflorescent. Quite diffi- cultly sol. in H 2 O. (Kehrmann.) 2BaO,P 2 O 5 , 16WO 3 + 10H 2 O. Efflorescent. (Pochard, A. ch. (6) 22. 240.) 2BaO, 6H 2 O, P 2 O 5 , 20WO 3 +24H 2 O. Sol. in H 2 O. (GiBbs, B. 10. 1386.) 6BaO, 2H 2 O, P 2 O 5 , 20WO 3 +46H 2 O. Sol. in H 2 O. (Gibbs, Proc. Am. Acad. 16. 126.) 7BaO, P 2 O 5 , 22WO 3 +59H 2 O. Sol. in H 2 0, (Sprerger, J. pr. (2) 22. 418.) +53H 2 O. (Kehrmann, B. 24. 2335.) 4BaO, 2H 2 O, P 2 O 5 , 22WO 3 +39H 2 O. Sol. m H 2 O without decomp. (Gibbs.) BaO, P 2 O 5 , 24WO 3 +59H 2 O. Sol. in H 2 O. (Sprenger.) 2BaO, P 2 O 5 , 24WO 3 +59H 2 O. Sol. in H 2 0. (Sprenger.) 3BaO, P 2 5 , 24WO 3 +46H 2 O =3BaO, 3H 2 O, P 2 O 5 , 24WO 3 +43H 2 O. Easily sol. in hot H 2 O. (Gibbs.) 3BaO, P 2 O 5 , 24WO 3 +48H 2 O. Sol. in H 2 O. (Soboleff, Z. anorg. 1896, 12. 18.) +58H 2 O. Sol. in H 2 O. (Sprenger.) Efflorescent. SI. sol. in dil. BaCl 2 +Aq. (Kehrmann, Z. anorg. 1. 423.) Barium potassium phosphotungstate. 5BaO. 2K 2 O, P 2 O 5 , 22WO 3 +48H 2 O. Sol. in H 2 O. (Kehrmann and Freinkel, B. 25. 1968.) Barium silver phosphotungstate, 4BaO 3 A g2 O, P 2 O 6 , 22WO 3 +34H 2 O. Very si. sol. in H 2 O. (Kehrmann and Freinkel, B. 25. 1966.) Barium sodium phosphotungstate, 2BaO, Na 2 O, P 2 O 5 , 24WO 3 +46H 2 O. Sol. in H 2 O, forming cloudy liquid, which clears up. Solution in HC1 is not cloudy. (Brandhorst and Kraut, A. 249. 380.) Calcium phosphotungstate, CaO, 5H 2 O, 16WO 3 , P 2 O 5 +3H 2 O. Readily sol. in H 2 O. (Gibbs, Proc. Am. Acad. 16. 130.) 2CaO, P 2 O 6 , 12WO 3 +19H 2 O. Efflores- cent. Insol. in alcohol. (Pochard, C. R. 110. 754.) 2CaO, P 2 O, 20WO 3 +22H 2 O. Efflores- cent. (Pochard, A. ch. (6) 22. 233.) Cadmium phosphotungstate, 2CdO, P 2 O 5 , 12WO 3 + 13H 2 O. SI. efflorescent. Very sol. in H 2 O. (P6- chard, C. R. 110. 754.) Cupric phosphotungstate, 3CuO, 24WO 3 , P 2 O 5 +58H 2 O. Sol. in H 2 O. (Sprenger, J. pr. (2) 22. 418.) 2CuO, P 2 O 5 , 12WO 3 + 11H 2 O. Very efflores- cent. (Pochard, C. R. 110. 754.) 2CuO, P 2 O 5 , 20WO 3 + 13H 2 O. Efflores- cent. (Pe*chard, A. ch. (6) 22. 235.) Lead phosphotungstate, 2PbO, P 2 O 5 , 12WO 3 +6H 2 0. Insol. in cold, sol. in boiling H 2 O. (Pe*- chard, C. R. 110. 754.) 2PbO, P 2 O 5 , 20WO 3 +6H 2 O. Sol. in boiling H 2 O. (Pochard, A. ch. (6) 22. 236.) Lithium phosphotungstate, Li 2 O, P 2 O 5 , 12W0 3 +21H 2 0. Sol. in H 2 O. (Pochard, C. R. 110. 754.) Magnesium phosphotungstate, 2MgO, P 2 O 6 / 12WO 3 . SI. efflorescent. (P4chard, C. R. 110. 754.) 2MgO, P 2 O 5 , 20WO 3 + 19H 2 O. SI. efflores- cent. (Pochard, A. ch. (6) 22. 234.) Mercurous phosphotungstate. Insol. in dil. HNO 3 +Aq. (Pochard, C. R. 110. 754.) Potassium phosphotungstate, K 2 O, P 2 O 5 , 12WO 3 +9H 2 O. Insol. in cold, si. sol. in hot H 2 O. (Pochard, C. R. 110. 754.) 5K 2 O, P 2 O 5 , 16WO 3 +zH 2 O = K 5 PW 8 O 29 -f- zH 2 O. (Potassium a-phospholuteotungstate) . Very si. sol. in cold, more easily in hot H 2 O. Sol. in cold dil. HN0 3 +Aq. (Kehrmann.) 3K 2 O, P 2 O 5 , 16WO 3 + 16H 2 O=K 3 PW 8 O 2 9 +8H 2 O. (Potassium a-anhydrophospho- luteotungstate) . Efflorescent. Easily sol. in H 2 O. (Kehrmann.) 5K 2 O, P 2 O 5 , 17WO 3 +21 or 22H 2 O. SI. sol. in cold H 2 O. (Kehrmann, Z. anorg. 1894, 6. 387.) 3K 2 O, P 2 O 5 , 18WO 3 +28H 2 O. (Duparc and Pearce, Bull. Soc. Min. 1895, 18. 42.) K 2 O, 5H 2 O, P 2 O 6 , 18WO 3 + 14H 2 O, Very si. sol. in H 2 O. (Gibbs.) 6K 2 O, P 2 O 5 , 18WO 3 +30H 2 O, and 23H 2 0. 724 PHOSPHOTUNGSTATE, POTASSIUM LEAD The 23H 2 O salt is more sol. in H 2 O than the 30H 2 Osalt. (Gibbs.) 7K 2 O, H 2 O, P 2 O 6 , 20WO 3 +27H 2 O. Sol. in H 2 O. (Gibbs, B. 10. 1386.) K 2 O, P 2 O 5 , 20WO 3 +5H 2 O. Nearly insol. in H 2 O. (Pochard, A. ch. (6) 22. 231.) 8K 2 O, P 2 O 5 , 20WO 3 + 18H 2 O. SI. sol. in H 2 O. (Gibbs.) 3K 2 O, P 2 O 5 , 21WO 3 +31H 2 O. Easily sol. in cold H 2 O or alcohol. Much less sol. in very dil. HC1 + Aq or KC1 +Aq. Decomp. by boil- ing H 2 O. (Kehrmann and Freinkel, B. 25. 1971.) 2K 2 O, 4H 2 O, P 2 O 5 , 22WO 3 +2H 2 O. Very si. sol. in H 2 O. (Gibbs.) 7K 2 O, P 2 O 5 , 22WO 3 +31H 2 O. Easily sol. in cold or hot H 2 O. Insol. in alcohol. (Kehr- mann, B. 25. 1966.) 3K 2 O, 3H 2 O, P 2 O 6 , 24WO 3 +8, and 14H 2 O. Sol. in a large amount of H 2 O with partial de- comp. (Gibbs ; Proc. Am. Acad. 16. 120.) Practically insol. in H 2 O. Easily sol. in NH 4 OH, alkalies, or alkali carbonates +Aq. (Kehrmann, B. 24. 2329.) 6K 2 O, P 2 O 6 , 24WO 3 + 18H 2 O. Sol. in H 2 O. (Gibbs, Proc. Am. Acad. 15. 1.) Potassium lead a-phosphoZwteotungstate. SI. sol. in H 2 O. (Kehrmann.) Silver phosphotungstate, Ag 2 O, P 2 O S , 12WO 3 +8H 2 O. Ppt. Insol. in H 2 O. (Pochard, C. R. 110. 754.) 5Ag 2 O, P 2 O 5 , 16WO 3 +zH 2 O=Ag 5 PW 8 O 29 +zH 2 O (Silver a-phospholuteotungstate) . Ppt. (Kehrmann.) 3Ag 2 O, P 2 O 6 , 16WO 3 +16H 2 O=Ag 3 PW 8 O 28 +8H 2 O. (Silver a-anhydrophospholuteo- tungstate). Easily sol. in H 2 O. (Kehrmann.) Ag 2 O, 24WO 3 , P 2 O 5 +60H 2 O. Insol. in H 2 O. 3Ag 2 O. 24WO 3 , P 2 O 6 +58H 2 O. Insol. in H 2 O. (Sprenger, J. pr. (2) 22. 418.) Sodium phosphotungstate, 3Na 2 O, P 2 O 5 , 7WO 3 +Aq. Sol'in H 2 O. (Kehrmann, Z. anorg. 1. 437.) 5Na 2 O, 11H 2 O, 2P 2 O 5 , 12WO 3 +26H 2 O = Na 5 HnP 2 W 6 O 31 -|-13H 2 O (?). (Scheibler, B. 5. 801.) 2Na 2 O, P 2 5 , 12WO 3 + 18H 2 O. Sol. in H 2 O. Insol. in alcohol. (Pochard, C. R. 110. 754.) 5Na 2 O, 14WO 3 , 2P 2 O 5 +42H 2 O. Easily sol. in H 2 O. (Gibbs.) Na 2 O,P 2 O 5 ,20WO 3 ,2H 2 O+19H 2 0. Sol. in H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 183.) Na 2 O, P 2 O 5 , 20WO 3 +23H 2 O = Na 2 O, 7H 2 O, P 2 O 5 . 20WO 3 + 16H 2 O. Easily sol. in H 2 O. (Gibbs.) +25H 2 O. SI. efflorescent; very sol. in H 2 O; insol. in alcohol. (Pochard, A. ch. (6) 22. 227.) 2Na 2 O, P 2 O 5 , 20WO 3 + 10H 2 O. Sol. in H 2 0; insol. in alcohol. (Pe*chard.) +30H 2 O. (P.) 3Na 2 O, P 2 O 6 , 20WO 3 +32H 2 O. As above. (P.) 2Na 2 O, P 2 O 5 , 22WO 3 +9H 2 O. Very si. sol. in H 2 O. (Gibbs.) 3Na 2 O, P 2 O 5 , 24WO 3 +22H 2 O. Sol. in H 2 O. (Brandhorst and Kraut, A. 249. 379.) +30H 2 O. Sol. in H 2 O. (Soboleff, Z. anorg. 1896, 12. 18.) +42H 2 O. Solubility in H 2 O at t. t 100 ccm. H2O dissolve g. of the cryst. salt 22 93 22.04 59.65 98.184 (Soboleff, Z. anorg. 1896, 12. 31.) 2Na 2 O, 4H 2 O, 24WO 3 , P 2 O 5 +23H 2 O. Readily sol. in H 2 O. (Gibbs, Proc. Am. Acad. 16. 118.) Sp. gr. at 20 of solutions of 2Na 2 O, 4H 2 O, P 2 O 6 , 24WO 3 +23H 2 O containing: 10.22 20.94 31.13% salt, 1.085 1.190 1.3^6 42.61 52.92 64.11% salt. 1.496 1.702 2.001 or, by calculation, a = sp. gr. if % is crystal- lized salt, b = sp. gr. if % is anhydrous salt: 5 10 15 20 25% salt, a 1.040 1.084 1.131 1.181 1.237 b 1.044 1.092 1.143 1.199 1.262 30 35 40 45 50% salt, a 1.299 1.370 1.449 1.538 1.640 b 1.333 1.414 1.507 1.613 1.734 55 60 64% salt, a 1.754 1.884 1.998 b 1.872 ... (Brandhorst and Kraut, A. 249. 377.) Strontium phosphotungstate, 2SrO, P 2 O 5 , 12WO 3 + 17H 2 O. Sol. in H 2 O. Insol. in alcohol. (Pochard, C. R. 110. 754.) Thallium phosphotungstate, T1 2 O, P 2 O 6 , 12WO 3 +4H 2 O. Ppt. (Pochard, C. R. 110. 754.) Zinc phosphotungstate, 2ZnO, P 2 O 5 , 12WO 3 7H 2 O. Efflorescent. (Pochard, C. R. 110. 754.) Monometaphosphotungstic acid. Ammonium wonowetaphosphotungstate, (NH 4 ) 2 O, 2NH 4 PO 3 , 18WO 3 + 11H 2 O. SI. sol. in cold H 2 O. PHOSPHOVANADICOZIRCONOSOTUNGSTATE, AMMONIUM 725 Potassium monowetaphosphotungstate, 3K 2 O, 2KPO 3 , 24WO 3 +20H 2 O. Very si. sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 319.) Orthometaphosphotungstic acid. Potassium sodium orthometaphosphotung- state, 2K 2 O, 4Na 2 O, 6NaPO 3 , 6K 3 PO 4 , 22WO 3 +42H 2 O. SI. sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 319.) Ps/rophosphotungstic acid. Ammonium manganous sodium pyrophos- photungstate, 5(NH 4 ) 2 O, 6MnO, 2Na 2 O, 2P 2 O 5 , 28WO 3 +48H 2 O. Very sol. in cold and in hot H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 90.) Ammonium sodium pi/rophosphotungstate, 6(NH 4 ) 4 P2O 7 , 3Na 4 P 2 O 7 , 2(NH 4 ) 2 O, 22WO 3 +31H 2 O. Nearly insol. in cold H 2 O or NH 4 OH+Aq. Sol. in a large amount of hot H 2 O. Manganous sodium pyrophosphotungstate, 6Na 2 O, 3MnO, P 2 O 5 , 14WO 3 +36H 2 O. Efflorescent in dry air. Sol. in H 2 O and can be recryst. therefrom. (Gibbs.) Potassium ps/rophosphotungstate, 9K 4 P 2 O 7 , 22WO 3 +49H 2 O. Very si. sol. in cold H 2 O. 6K 4 P 2 O 7 , 3H 4 P 2 O 7 , 22WO 3 , K 2 O, H 2 O + 42H 2 O. SI. sol. in cold. Sol. in much boiling H 2 O. (Gibbs, Am. Ch. J. 7. 392.) Phosphovanadic acid, P 2 O 5 ,V 2 O5, 2H 2 O+ 9H 2 0. Sol. in H 2 O. Composition is vanadium phosphate (VO 2 )H 2 PO 4 +4^H 2 O. (Friedheim, B. 23. 1531.) This is the only "acid" which exists. (F.) P 2 O 5 , V 2 O 5 +14H 2 O. Sol. in H 2 O; can be recryst. from dil. H 3 PO 4 +Aq. (Ditte, C. R. 102. 757.) 3P 2 O 5 ,2V 2 O 6 +9H 2 O. Sol,inH 2 O. (Ditte.) P 2 O 5 , 3V 2 O 5 . (Berzelius.) 3H 2 O, 7P 2 O 5 , 6V 2 O 5 +34H 2 O. Sol. in H 2 O. Decomp. by much H 2 O into 6H 2 O, P 2 O 6 , 20V 2 O 6 +53H 2 O. Sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 209.) Ammonium phosphovanadate, (NH 4 ) 2 O, P 2 5 , V 2 5 +H 2 0. SI. sol. in cold H 2 0. (Gibbs, Am. Ch. J. 7. 209.) +3H 2 O. Composition is (VO 2 )(NH 4 )HPO 4 +H 2 O. (Friedheim.) (NH 4 ) 2 O, P 2 O 5 , 2V 2 O 5 +7H 2 O. Easily sol. in H 2 O. (Gibbs.) SI. sol. in H 2 O. (Fried- heim.) Composition is (NH 4 ) 2 O, V 2 O 5 , +2(VO 2 )H 2 PO 4 +5H 2 O. (Friedheim.) 5(NH 4 ) 2 O, 2P 2 O 5 , 3V 2 O 5 +24H 2 O. Easily sol. in H 2 O. (Ditte, C. R. 102. 1019.) Could not be obtained. (Friedheim.) 5(NH 4 ) 2 O, 4P 2 O 5 , 2V 2 O 5 +24H 2 O. As above. (Ditte.) Could not be obtained. (Friedheim.) 7(NH 4 ) 2 O, P 2 O 5 , 12V 2 O 5 +26H 2 O. Easily sol. in H 2 O. Composition is 2(NH 4 ) 2 HPO 4 + 5(NH 4 ) 2 O, 12V 2 O 6 +25H 2 O. (Friedheim.) Potassium phosphovanadate, K 2 O. P 2 O 5 , 2V 2 O 5 +7H 2 O. SI. sol. in H 2 O; decomp. thereby to 7K 2 O, 12V 2 O 5 , P 2 O 5 +26H 2 O. Composition is K 2 O, V 2 O 8 +2(VO 2 )H 2 PO 4 +5H 2 O. (Friedheim.) 3K 2 O, 4P 2 O 5 , 6V 2 O 6 +21H 2 O. SI. sol. in H 2 O. (Gibbs.) 7K 2 O, P 2 O 6 , 12V 2 O 5 +26H 2 O. Easily sol. in H 2 O. Composition is 2K 2 HPO 4 +5K 2 O, 12V 2 O 5 +25H 2 O. (Friedheim.) 2K 2 O, P 2 O 5 , V 2 O 5 . 3K 2 O, 2P 2 O 5 , 2V 2 O 5 +5H 2 O. 13K 2 O, 2P 2 O 5 , 22V 2 O 5 +58H 2 O. 15K 2 O, 2P 2 O 5 , 25V 2 O 5 +76H 2 O. (Friedheim, Z. anorg. 1894, 5. 446.) 16K 2 O, 2P 2 6 , 27V 2 O 5 +57H 2 O. 6K 2 O, P 2 O 5 , 11V 2 O 5 +33H 2 O. 7K 2 O, P 2 O 6 , 13V 2 O 6 +38H 2 O. 4K 2 O, P 2 O 5 , 3V 2 O 5 +3H 2 O. (Friedheim, Z. anorg. 1894, 6. 459-465.) Silver phosphovanadate, 2Ag 2 O, P 2 O 5 , V 2 O 5 + 5H 2 O. SI. sol. in cold or hot H 2 O. (Gibbs.) Phosphovanadicotungstic acid. Ammonium phosphovanadicotungstate, (NH 4 ) 2 O, P 2 O 5 , V 2 O 3 , WO 3 +zH 2 O. Ppt. (Smith, J. Am. Chem. Soc. 1902, 24. 577.) 15(NH 4 ) 2 0, 2P 2 5 , 6V 2 3 , 44WO 3 + 106H 2 O. Sol. in H 2 O. Insol. in alcohol, ether or benzene. (Rogers, J. Am. Chem. Soc. 1903, 25. 303.) Phosphovanadicovanadiotungsticacid. Ammonium phosphovanadicovanadiotung- state, 14(NH 4 ) 2 O, 2P 2 O 5 , 3V 2 O 3 , 7V 2 O 5 , 27WO 3 +66H 2 O. Sparingly sol. in cold H 2 O. Sol. in hot H 2 O. (Rogers, J. Am. Chem. Soc. 1903, 26. 309.) Phosphovanadicozirconosotungstic acid. Ammonium phosphovanadicozirconosotung- state. Exact formula not known. (E,. F. Smith J. Am. Chem. Soc. 1903, 25. 1226!) 726 PHOSPHOVANADICOVANADIC ACID Phosphovanadicovanadic acid. Ammonium phosphovanadicovanadate, 7(NH 4 ) 2 O, 2P 2 O 6 , VO 2 , 18V 2 O 5 +50H 2 O. Sol. in H 2 O. (Gibbs, Am. Ch. J. 7. 209.) 7(NH 4 ) 2 O, 14P 2 O 5 , 16VO 2 , 6V 2 O 5 -f-65H 2 O. Decomp. by boiling with H 2 O into 5(NH 4 ) 2 O, 10P 2 O 5 , 11VO 2 , V 2 O 6 +41H 2 O. Sol. inH 2 O. (Gibbs.) Potassium , 5K 2 O, 12P 2 O 6 , 12VO 2 , 6V 2 O 6 +40H 2 0. Decomp. by hot H 2 O into 7K 2 O, 12P 2 O 5 , 14VO 2 , 6V 2 O 5 +52H 2 O. Sol. inH 2 O. (Gibbs.) Sodium , 4Na 2 O, 5P 2 O 6 , VO 2 , 4V 2 O 6 + 37H 2 O. Insol. in H 2 O. (Gibbs.) Phosphovanadiomolybdic acid. Ammonium phosphovanadiomolybdate, 7(NH 4 ) 2 O, 2P 2 O 5 , V 2 O 5 , 48MoO 3 + 30H 2 O. SI. sol. in cold, somewhat more in hot H 2 O with partial decomp. (Gibbs, Am. Ch. J. 6. 391.) 8(NH 4 ) 2 O, P 2 O 6 , 8V 2 O 5 , 14MoO 3 +50H 2 O. Easily sol. in hot H 2 O without decomp. (Gibbs.) 5(NH 4 ) 2 O, P 2 O 6 , 2^V 2 O 6 , 2l^MoO 3 + 50H 2 O. 8(NH 4 ) 2 O, P 2 O 5 , 5V 2 O 5 , 18MoO 3 +45H 2 O. 7(NH 4 ) 2 O, P 2 O 5 , 5y 2 V z O 5 , 16^Mo0 3 + 50H 2 O. 8(NH 4 ) 2 O, P 2 O 5 , 7V 2 O 5 , 15MoO 3 +50H 2 O. All above compounds are sol. ih H 2 O. (Blum, J. Am. Chem. Soc. 1908, 30. 1859.) 6(NH 4 ) 2 O, P 2 O 6 , 7V 2 O 5 , 9MoO 3 +28H 2 O, +33H 2 O, and +37H 2 O. Can be recryst. from H 2 O. (Hinsen, Dis- sert. 1904.) 4(NH 4 ) 2 O, P 2 O 5 , 4V 2 O 5 , HMoO 3 +37H 2 O. (Jacoby, Dissert. 1900.) 6(NH 4 ) 2 O, P 2 O 5 , 7V 2 O 6 , HMoO 3 +34H 2 O and+43H 2 O. (Hinsen, Dissert. 1904.) 8(NH 4 ) 2 O, P 2 O 6 , 7V 2 O 5 , HMoO 3 +30H 2 O. (Hinsen.) 5(NH 4 ) 2 O, P 2 O 5 , 4V 2 O 6 , 12MoO 3 +39H 2 O. 1 cc. of solution in H 2 O contains 0.2624 g. of hydrous salt. Sp. gr. of solution at 18 = 1.0932. (Lahrmann, Dissfert. 1904.) 6(NH 4 ) 2 O, P 2 O 5 , 4V 2 O 5 , 12MoO 3 +24H 2 O. Nearly insol. in cold H 2 O. (Lahrmann.) 7(NH 4 ) 2 O, P 2 O 5 , 6V 2 O 5 , 12MoO 3 +33H 2 O. (Stamm, Dissert. 1906.) 6(NH 4 ) 2 O, P 2 O 5 , 4V 2 O 6 , 13MoO 3 +37H 2 O. 1 cc. of solution sat. at 18 contains 0.1543 g. hydrous salt and has sp. gr. = 1.0900. (Tog- genburg, Dissert. 1902.) 6(NH 4 ) 2 O, P 2 O 5 , 5V 2 O 5 , 13MoO 3 +29H 2 0. 1 cc. solution sat. at 18 contains 0.2533 g. hydrous salt. Sp. gr. = 1.0797. (Stamm, Dissert. 1906.) +32H 2 O. (Stamm.) +34H 2 O. Stamm.) 6(NH 4 ) 2 O, P 2 O 5 , 4V 2 O 5 , 14MoO 3 +28H 2 O. Easily sol. in H 2 O with decomp. (Toggen- burg, Dissert. 1902.) 8(NH 4 ) 2 O, P 2 O S , 4V 2 O 5 , 14MoO 3 +24H 2 O. Decomp. by cold H 2 0. (Lahrmann, Dissert. 1904.) 5(NH 4 ) 2 O, P 2 O 5 , 3V 2 O 5 , 5MoO 3 +39H 2 O. 1 cc. of solution sat. at 18 contains 0.2445 g. hydrous salt and has sp. gr. = 1.144. (Ja- coby, Dissert. 1900.) 6(NH 4 ) 2 O, P 2 O 6 , 3V 2 5 , 15 MoO 3 +41H 2 O. Extraordinarily easily sol. in H 2 0. (Ja- coby.) 7(.NH 4 ) 2 O, P 2 O 6 , 3 2 O 5 , 18MoO 3 +31H 2 O. (Schulz Dissert. 1905.) 6(NH 4 ) 2 O, P 2 O 5 , 3V 2 O 5 , 18MoO 3 +40H 2 O. (Schulz.) 8(NH 4 ) 2 O, P 2 O 5 , 5V 2 O , 73MoO 3 +26H 2 O. +33H 2 O. (Stamm, Dissert 1905.) Ammonium barium , 0.5(NH 4 ) 2 O, 5.5BaO, P 2 O 5 , 6V 2 O 5 , 8MoO 3 +38H 2 O. (Hinsen, Dissert. 1904.) 2(NH 4 )*O, 4BaO, P 2 O 5 , 7V 2 O 5 , 10 MoO 3 + 43H 2 O. SI. sol. in H 2 O. Decomp. on heating. (Toggenburg, Dissert. 1902.) (NH 4 ) 2 O, 5BaO, P 2 O 5 , 6V 2 O 5 , 12MoO 3 + 49 H 2 0. Less sol. in H 2 O than NH 4 comp. (Jacoby, Di^sert. 1900.) 2(NH 4 ) 2 0, 4BaO, P 2 O 5 , 4V 2 O 5 , 13MoO 3 + 37 H 2 O. Sol. in much hot H 2 with decomp. (Toggenburg, Dissert. 1902.) 2(NH 4 ) 2 O, 4BaO, P 2 O 5 , 5V 2 O 5 , 13MoO 3 + 46H 2 O. (Stamm, Dissert. 1905.) 3 NH 4 ) 2 O, 4BaO, P 2 O 5 , 5V 2 O 5 , 13MoO 3 + 40H 2 O. (Stamm.) 3(NH 4 ) 2 O, 3BaO, P 2 O 5 , 4V 2 O 5 , 14MoO 3 + 39H 2 O. (Stamm.) 2(NH 4 ) 2 O, 4BaO, P 2 O 5 , 3V O 5 , 17MoO 3 + 46H 2 O. (Schulz, Dissert. 1906.) Ammonium potassium , (NH 4 ) 2 O, 6K 2 O, P 2 6 , 6V 2 O 6 , 10 MoO 3 +38H 2 O. (Jacoby, Dissert. 1900.) (NH 4 ) 2 O, 6K 2 O, P 2 O 5 , 7V 2 O 6 , HMoO 3 + 25H 2 O. (Jacoby, Dissert. 190\) (NH 4 ) 2 O, 5K 2 O, P 2 O 5 , 6V 2 O 5 , 12MoO 3 + 46H 2 O. (Jacoby.) (NH 4 ) 2 6, 5K 2 O, P 2 O 5 . 5V 2 O 5 , 13MoO 3 + +25H 2 O;+29H 2 O; +30H 2 O. SI. sol. in cold, more easily in hot H 2 O. (Stamm, Dissert. 1905.) 5K 2 O, (NH 4 ) 2 O, P 2 O 5 , 4V 2 O 5 , 14Mo0 3 + 31 2 O. (Stamm.) (NH 4 ) 2 O, 4K 2 O, P 2 O 5 , 3V 2 O 5 , 15MoO 3 + 36H 2 O. (Jacoby, Dissert. 1900.) (NH 4 ) 2 O, 6K 2 O, P 2 O 5 , 3V 2 O 5 , 18MoO 3 + 43H 2 O. (Schulz. Dissert. 1906.) 5(NH.-)oO, K 2 O, P 2 O 5 , 2V 2 O 5 , 20MoO 3 + 52H 2 O. (Schulz.) Barium potassium , 2BaO, 2K 2 0, P 2 O 5 , 2V 2 6 , 18 MoO s +47H 2 O. (Schulz, Dissert. 1905.) PLATINATE, BARIUM, BASIC 727 Potassium phosphovanadiomolybdate, 7K 2 O P 2 O 5 , 7V 2 O 5 , 9MoO 3 +25H 2 O. (Hinsen, Dissert. 1904.) 5K 2 O, P 2 O 5 , 2V 2 O 5 , 20MoO 3 +53H 2 O (Schulz, Dissert. 1905.) Phosphovanadiotungstic acid. Ammonium phosphovanadiotungstate, 10(NH 4 ) 2 O, 3P 2 O 5 , V 2 O 5 , 60WO 3 60H 2 O. Nearly insol in cold, si. sol. in hot H 2 O Sol. in (NH 4 ) 2 HPO 4 +Aq, and in NH 4 OH + Aq. 5(NH 4 ) 2 O, P 2 O 5 , 3V 2 O 5 , 16WO 3 +37H 2 O Easily sol. in H 2 O. (Gibbs, Am. Ch. J. 5 391.) 13(NH 4 ) 2 O, 2P 2 O 6 , 8V 2 O 5 , 34WO 3 +86H 2 O Very sol. in cold and hot H 2 O. nsol. in alcohol, ether, CS 2 , benzene anc nitrobenzene. (Rogers, J. Am. Chem. Soc 1903, 25. 299.) Banum , ISBaO, 3P 2 O 6 , 2V 2 O , 60WO + 144H 2 O. Easily sol in hot H 2 O with decomp (Gibbs,Am.Ch.J.6.391.) Potassium 3K 2 O, P 2 O 6 , V 2 O 5 , 7WO 3 + 11H 2 O. Sol. in H 2 O. 8K 2 O, 3P 2 O 6 , 4V 2 O 5 , 18WO 3 +23H 2 O. Sol in hot H/J with decomp. into preceding salt (Gibbs, Am. Ch. J. 5. 391.) SUver , 13Ag 2 0, 2P 2 6 , 8V 2 , 33WO 8 + 41H 2 O. Somewhat sol. in H 2 O. Completely sol. in H 2 O containing a few drops HNO 3 . (Rogers, J. Am. Chem. Soc. 1903, 25. 302.) Phosphovanadiovanadicotungstic acid. Barium phosphovanadiovanadicotungstate, 18BaO, 3P 2 O 5 , VO S , VO 2 , 60WO 3 + 150H 2 O. SI. sol. in cold, easily sol. in hot H 2 O. (Gibbs, Am. Ch. J. 5. 391.) Phosphuretted hydrogen. See Hydrogen phosphide. Platibromonitrous acid. Potassium platibromonitrite, K 2 Pt(N0 2 ) 4 Br 2 . Rather si. sol. in H 2 O. (Blomstrand, J. pr. (2) 3. 214.) Sol. in about 40 pts. cold, and 20 pts. boil- ing H 2 O. Insol. in alcohol. SI. sol. in KBr or KNO 2 +Aq. (Vezes, A. ch. (6) 29. 198.) K 2 Pt(NO 2 ) 8 Br 3 . Sol. in about 5 pts. warm H 2 O with decomp. (Vezes.) K 2 Pt(NO 2 ) 2 Br 4 . Sol. in less than 5 pts. H 2 O with decomp. (Vezes.) Platichloronitrous acid. Potassium platichloronitrite, K 2 Pt(NO 2 ) 4 Cl 2 . Rather si. sol. in H 2 O. (Blomstrand J. pr. (2)3.214.) Sol. in 40 pts. cold, and 20 pts. boiling H 2 O. Insol. in alcohol SI. sol. in KC1 or KNO 2 + Aq. (Vezes, A. ch. (6)29. 183.) K 2 Pt(NO 2 ) 8 Cl 3 . Very sol. in H 2 O. (Vezes.) K 2 Pt(NO 2 )Cl*+H 2 O. Sol. in H 2 O with decomp. (Vezes.) Platiiodonitrous acid. Potassium platiiodonitrite, K 2 Pt(NO 2 ) 2 I 4 . SI. sol. in cold, more easily in hot H 2 O; de- comp. by boiling. (Veze , A. ch. (6) 29. 207.) K 2 Pt(NO 2 )I 5 . As above. (Vezes.) Platin-. See also Pla ino-, plato-, p'at-, and platos-. Platincfo'amine compounds. See Chloro-, bromo-, hydroxylo-, iodo-, ni- rato-, nitrito-, sulphate-, etc., platincfa'amine compounds. Platin^namine carbonate, Pt(NH 3 ) 6 (C0 3 ) 2 . Ppt. Sol. in NaOH+Aq. (Geddes, J. pr. (2) 26. 257.) -chloride Pt(NH 3 ) 6 Cl 4 . Sol. in hot H 2 O (Gerdes.) chloroplatinate, Pt(NH 3 ) C1 4 , PtCl 4 -{- 2H 2 O. Very si. Bol. in H 2 O. (Gerdes.) - nitrate, Pt(NH 3 ) 6 (NO 8 ) 4 . Easily sol. in H 2 O; si. sol. in HNO 3 +Aq. (Gerdes.) - sulphate, Pt(NH 3 ) 6 (S0 4 ) 2 +H 2 0. Nearly insol. in H 2 O. (Gerdes.) Mraplatinamine iodide, Pt 4 (NH 3 ) 8 I 10 . (Blomstrand, B. 16. 1469.) Ocfoplatinamine iodide, Pt 8 (NH 3 )i 6 Ii 8 . (Blomstrand.) Platinic acid. Barium platinate, basic (?), 3BaO, 2Pt0 2 . Insol. in HC 2 H 3 O 2 +Aq; easily sol. in HCl+Aq. (Rousseau.) 728 PLATINATE, BARIUM Barium platinate, BaPtO 3 . (Rousseau, C. R. 109. 144.) +H 2 O. Insol. in dil. HNO 3 +Aq; sol. in warm HCl+Aq. (Topsoe, B. 3. 464.) +4H 2 O. Very si. sol. in H 2 O, BaO 2 H 2 , or NaOH-f Aq. Easily sol. in dil. acids, except HC 2 H 3 O 2 , in which it is insol. in the cold, but decomp. on heating. (Topsoe, I. c.) Composition is 3BaPtO 3 , BaCl 2 , PtCl 2 O + 4H 2 O (?). (Johannsen, A. 156. 204.) Calcium platinate chloride (?), 2Ca 2 Pt2O 5 Cl2 +7H 2 (?). "Herschel's precipitate." Easily sol. in HCl+Aq, and in HNO 3 +Aq, if freshly pptd. (Herschel. * Very sol. in HNO 3 +Aq. (Weiss and Dobereiner, A. 14. 252.) Composition is CaPtO 3 PtCl 2 O, CaO + 7H 2 O (?). (Johannsen, A. 155. 204.) Potassium platinate. Sol. in H 2 O. (Berzelius.) K 2 O, PtO 2 +3H 2 O. V sol. in H 2 0. .ry 2 w, JTivy 2 -rojn. 2 v^. very t. (Blondel, A. ch. 1905, (8) 6. 90.) K 2 Pt(OH) 6 . Sol. in H 2 O; insol. in alcohol. (Bellucci, Z. anorg. 1905, 44. 173.) Sodium platinate, Na 2 O, 3PtO 2 +6H 2 O. Dil. acids dissolve out Na 2 O and leave PtO 2 . Sol. in HNO 3 +Aq. (Dobereiner, Pogg. 28. 180.) Na 2 0, Pt0 2 +3H 2 0. Sol. in H 2 O. (Blon- del.) Afetoplatinic acid, 5Pt0 2 , 5H 2 O. Insol, in H 2 0. (Blondel, A. oh. 1905, (8) 6. 103.) Sodium wetoplatinate, Na 2 O, 5PtO 2 +9H 2 O. Insol. in H 2 O. (Blondel.) Platinimolybdic acid, 4H 2 O, PtO 2 , 10MoO 3 , (Gibbs.) Ammonium platinimolybdate, 8Mo0 3 , 2Pt0 2 , 3(NH 4 ) 2 + 12H 2 0. 4MoO 3 , 2PtO 2 ,2(NH 4 ) 2 0+19H 2 O. Sol. in hot H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 80-82.) Potassium platinimolybdate, 60Mo0 3 , PtO 2 , 10K 2 O+40H 2 O. So . in hot H 2 O. (Gibbs.) Silver platinimolybdate. Sodium platinimolybdate, 4Na 2 O, PtO 2 10 MoO 8 -f29H 2 0. Sol. in H 2 O. (Gibbs, Sill. Am. J. (3) 14 61.) Platinitungstic acid. Ammonium platinitungstate, 4(NH 4 ) 2 O, PtO 2 , 10WO 3 +12H 2 O. Sol. in H 2 O. (Gibbs, B. 10. 1384.) Potassium platinitungstate, 4K 2 O, PtO 2 , 10WO 3 +9H 2 O. Sol. in H 2 O. (Gibbs.) Sodium platinitungstate, 4Na 2 O, PtO 2 , 10WO 8 +25H 2 O. Sol. in H 2 O. (Gibbs.) 5Na 2 O, 7WO 3 , 2PtO 2 +35H 2 O. Sol. in H 2 O. (Gibbs.) Is double salt 3Na 2 O, 7WO 3 +2Na 2 PtO 3 . Rosenheim, B. 24. 2397.) 10WO 3 , PtO 2 , 4Na 2 O+23H 2 O. 10WO 3 , PtO 2 , 6Na 2 O+28H 2 O. 20WO 3 , PtO 2 , 9Na 2 O+58H 2 O. 30WO 3 , 2PtO 2 , 15Na 2 O+89H 2 O. 30WO 3 , PtO 2 , 12Na 2 O+72H 2 O. All are sol. in boiling H 2 O. (Gibbs, Am. Ch. J. 1895, 17. 74-80.) Platino-. See also Plato . Platinochlorophosphoric acid. See Chloroplatinophosphoric acid. Platinocyanhydric acid, H 2 Pt(CN) 4 . Deliquescent. Very sol. in H 2 O, alcohol, and ether. Ammonium platinocyanide, (NH 4 ) 2 Pt(CN) 4 +3H 2 O. Very sol. in H 2 O. +2H 2 O. Sol. in 1 pt. H 2 O, and still more easily in alcohol. +H 2 0. Ammonium hydroxylamine platinocyanide, NH 4 (NH 4 O)Pt(CN) 4 +3^H 2 0. Sol. in H 2 O. (Scholz, M. Ch. 1. 900.) Ammonium magnesium platinocyanide, (NH 4 ) 2 Mg[Pt(CN) 4 ] 2 +6H 2 0. Barium platinocyanide, BaPt(CN) 4 +4H 2 O. Sol. in 33 pts. H 2 O at 16, and in much less at 100. Sol. in alcohol. Barium potassium platinocyanide, BaK 2 [Pt(CN) 4 ] 2 . Sol. in H 2 O. Barium rubidium platinocyanide, BaRb 2 [Pt(CN) 4 ] 2 . Sol.inH 2 O. PLATINOCYANIDE, PRASEODYMIUM 729 Cadmium platinocyanide, CdPt(CN) 4 . Ppt. Sol. in NH 4 OH+Aq. (Martius, A. 117. 376.) CdPt(CN) 4 , 2NH 3 +H 2 O. (M.) Calcium platinocyanide, CaPt(CN) 4 +5H 2 O. Very sol. in H 2 O. Calcium potassium platinocyanide, CaK 2 [Pt(CN) 4 ] 2 . Sol. in H 2 O. Cerium platinocyanide, Ce 2 [Pt(CN) 4 ] 3 + 18H 2 O. Sol. in H 2 O. Cobaltous platinocyanide ammonia, CoPt(CN) 4 , 2NH 3 . Insol. in H 2 O, but sol. in hot NH 4 OH+Aq. Cupric platinocyanide, CuPt(CN) 4 +sH 2 O. Ppt. Cupric platinocyanide ammonia, CuPt(CN) 4 , 2NH 3 +H 2 O. CuPt(CN) 4 , 4NH 3 . Sol. in H 2 O, alcohol, and ether. Didymium platinocyanide, Di 2 [Pt(CN) 4 ] 3 + 18H 2 O. Efflorescent in dry air. Sol. in H 2 O. (Cleve.) Dysprosium platinocyanide, Dy 2 [Pt(CN) 4 ] 3 + 21H 2 O. Easily sol. in H 2 O. (Jantsch, B. 1911, 44. 1277.) Erbium platinocyanide, Er 2 [Pt(CN 4 )] 3 + 21H 2 O. Sol. in H 2 O. (Cleve.) Gadolinium platinocyanide, 2Gd(CN),, 3Pt(CN) 2 +18H 2 O. Sol. in H 2 O; decomp. in the ah 1 . (Bene- dicks, Z. anorg. 1900, 22. 405.) Glucinum platinocyanide, GlPt(CN) 4 . (ToczynsU, Dissert. 1871.) Hydroxylamine platinocyanide, (NH 4 O) 2 Pt(CN) 4 +2H 2 O. Deliquescent. Very sol. in H 2 O. (Scholz.) Hydroxylamine lithium platinocyanide, (NH 4 O)LiPt(CN) 4 +3H 2 O. Sol. in H 2 O. Indium platinocyanide, In 2 [Pt(CN) 4 ] 3 +2H 2 O. Hydroscopic; sol. in H 2 O. (Renz, B. 1901, 34. 2765.) Lanthanum platinocyanide, La 2 [Pt(CN) 4 ] 3 + 18H 2 0. Easily sol. in H 2 O. (Cleve.) Magnesium platinocyanide, MgPt(CN) 4 + 2H 2 O. Solubility in H 2 O. 100 g. of the sat. solution contain at: 96.4 100 44 .33 43 . 96 g. MgPt(CN) 4 (Buxhoevden, Z. anorg. 1897, 15. 325.) +4H 2 0. Solubility in H 2 O. 100 g. of the sat. solution contain at: 42.2 46.3 48.7 55 40.21 39.79 40.75 40.02 g. MgPt(CN) 4 , 58.1 69 77.8 87.4 42.01 43.48 44.88 45.52 g. MgPt(CN) 4 , 93 45.04g.MgPt(CN) 4 . (Buxhoevden.) 90 45.59 +7H 2 O. Sol. in 3.4 pts. H 2 O at 16. Easily sol. in alcohol and ether. Solubility in H 2 O. 100 g. of the sat. solution contain at: 4.12 +0.5 5.5 18.0 24.9 26.33 28.07 31.23 g. MgPt(CN) 4 , 36.6 45.0 46.2 38 .36 41 . 32 41 . 96 g. MgPt(CN) 4 . (Buxhoevden.) Magnesium potassium platinocyanide, MgK 2 [Pt(CN) 4 ] 2 +7H 2 O. Sol. in H 2 O. Mercuric platinocyanide, HgPt(CN) 4 . Ppt. Mercuric platinocyanide nitrate, 5HgPt(CN) 4 Hg(NO 3 ) 2 + 10H 2 O. Ppt. Nickel platinocyanide ammonia, NiPt(CN) 4 , 2NH 3 +H 2 0. Potassium platinocyanide, K 2 Pt(CN) 4 + '3H 2 O. Extremely efflorescent. SI. sol. in cold, easily in hot H 2 O. (Willm, B. 19. 950.) Sol. in alcohol and ether. Potassium sodium platinocyanide, K 2 Pt(CN) 4 , Na 2 Pt(CN) 4 +6H 2 0. Sol. in H 2 O. (Willm, B. 19. 950.) Praseodymium platinocyanide, 2Pr(CN) 3 , 3Pt(CN) 2 . Sol. in H 2 O. (Von Scheele, Z anorg. 1898, 18. 355.) 730 PLATINOCYANIDE, SAMARIUM Samarium platinocyanide, Sm 2 [Pt(CN 4 )]3 + 18H 2 O. Sol.inH 2 O. (Cleve.) Scandivun platinocyanide, Sc 2 [Pt(CN) 4 ]3 +21H 2 0. Sol. in H 2 O and insol. in alcohol; when boiled in alcohol it is dehydrated. (Crookes, Phil. Trans. 1910, 210. A, 368.) +21H 2 O. (Orlow, Ch. Z. 1912, 36. 1407.) Silver platinocyanide, Ag 2 Pt(CN) 4 . Insol. in H 2 O. Sol. in NH 4 OH+Aq. Silver platinocyanide ammonia, Ag 2 Pt(CN) 4 , 2NH 3 . Insol. in H 2 O. Sol. in NH 4 OH+Aq. Silver platinocyanide bromide. See Bromoplatinocyanide, silver. Silver platinocyanide chloride. See Chloroplatinocyanide, silver. Silver platinocyanide iodide. See lodplatinocyanide, silver. Sodium platinocyanide, Na 2 Pt(CN) 4 +3H 2 O. Easily sol. in H 2 O. (Willm, Z. anorg. 4. 298.) Sol. in alcohol. Strontium platinocyanide, SrPt(CN) 4 +5H 2 O. Sol. in H 2 O. Thallous platinocyanide, Tl 2 Pt(CN) 4 . Nearly insol. in cold, si. sol. in hot H 2 O. (Friswell, Chem. Soc. 24. 461.) Thallous platinocyanide carbonate, 2Tl 2 Pt(CN) 4 , T1 2 C0 3 . Nearly insol. in cold H 2 O. (F.) Thorium platinocyanide, Th[Pt(CN) 4 ] 2 + 16H 2 O. Somewhat difficultly sol. in cold, easily in hot H 2 O. (Cleve, Sv. V. A. H. Bih. 2. No. 6.) Uranyl platinocyanide, (UO 2 )Pt(CN) 4 +a;H 2 O. Sol. in H 2 O. (Levy, Chem. Soc. 1908, 93. 1459.) Ytterbium platuiocyanide, 2Yb(CN) 3 , 3Pt(CN) 2 + 18H 2 O. Easily sol. in H 2 O. (Cleve, Z. anorg. 1902, 32. 139.) Yttrium platuiocyanide, Y 2 [Pt(CN)J 3 + 21H 2 O. Easily sol. in H 2 O. Insol. in absolute alcohol. (Cleve and Hoglund.) Zinc platinocyanide ammonia, ZnPt(CN) 4 , 2NH 3 +H 2 O. Platinonitrous acid. See Platonitrous acid. Platinoplatinicyanhydric acid, HPt(CN) 4 +zH 2 0. Sol. in H 2 O. (Levy, Chem. Soc. 1912, 101. 1093.) Platinoselenocyanhydric acid. Potassium platinoselenocyanide, K 2 Pt(SeCN) 6 . Sol. in H 2 O and alcohol. (Clarke and Dud- ley, B. 1878, 11. 1325.) Platinoselenostannic acid. See under Selenostannate, platinum. Platinososulphocyanhydric acid, H 2 Pt(SCN) 4 . Known only in aqueous solution. Potassium platinososulphocyanide, K 2 Pt(SCN) 4 . Permanent. Sol. in 2.5 pts. H 2 O at 15, and more readily at higher temp. Very sol. in warm alcohol. Silver , Ag 2 Pt(SCN) 4 . Insol. in H 2 O. Sol. in KSCN+Aq, and partly sol. in NH 4 OH+Aq. Platinosulphocyanhydric acid, H 2 Pt(SCN) 6 . Known only in aqueous, and alcoholic solu- tions. Ammonium platinosulphocyanide, (NH 4 ) 2 Pt(SCN) 6 . Sol. in H 2 O and alcohol. Barium , BaPt(SCN) 6 . Sol. in H 2 O and alcohol. Ferrous , FePt(SCN) 6 . Insol. in H 2 O or alcohol. Not attacked by dil. H 2 SO 4 , HC1, orHNO 3 +Aq. Lead , PbPt(SCN) 6 . SI. sol. in cold, decomp. by hot H 2 O. Sol. in alcohol. PbPt(SCN) 6 , PbO. Insol. in H 2 O or alco- hol. Sol. in acetic or nitric acids. Mercurous , Hg 2 Pt(SCN) 6 . Ppt. Insol. in H 2 O. PLATINUM AMMONIUM COMPOUNDS 731 Potassium platinosulphocyanide, K 2 Pt(SCN) 6 . Sol. in 12 pts. H 2 O at 60. Much more easily in boiling H 2 O, and still more easily in hot alcohol. +2EUO. (Miolati and Bellucci, Gazz. Ch. it. 1900, 30, II. 592.) Silver , Ag 2 Pt(SCN) 6 . Insol. in H 2 O or K 2 Pt(SCN) 6 +Aq. Sol. in cold NH 4 OH+Aq and in KCNS+Aq. Sodium , Na;Pt(SCN) 6 . Sol. in H 2 O and alcohol. Platinosulphostannic acid. See under Sulphostannate, platinum. Platino sulphurous acid. See Plato sulphurous acid. Platinum, Ft. Not attacked by H 2 O, H 2 SO 4 , HC1, or HNO 3 +Aq. Slowly sol. in aqua regia, or a mixture of HBr and HNO 3 , but much less easily than Au. Precipitated Pt is remarkably sol. in HCl+Aq in presence of air. (Wilm, B. 1881, 14. 636.) Pure Pt foil is attacked by fuming HC1 under influence of light, but not in the dark. (Berthelot, C. R. 1904, 138. 1297.) Dil. HCl+Aq dissolves 10-15% Pt from active Pt black. (Wohler, B. 1903, 36. 3482.) Cone. HNO 3 oxidizes Pt black; Pt sponge, less easily; sheet Pt, slightly. (Wohler, Dissert. 1901.) Pt in presence of Hg is more or less sol. in cone. HNO 3 . (Tarugi, Gazz. ch. it. 1903, 33, II. 171.) Pt vessels are attacked by evaporating HNO 3 therein. (Jaunek and Meyer, Z. anorg. 1913, 83. 71.) SI. sol. in cone. H 2 SO 4 containing small amounts cf nitrogen oxides. (Scheurer- Kestner, C. R. 86. 1082.) Pt black, pptd. by formic acid, is easily sol. in boiling H 2 SO 4 . (Deville and Stas, Paris, 1878.) Thin sheet Pt is attacked by boiling H 2 SO 4 containing K 2 SO 4 ; 1 sq. cm. loses 0.01 g. in 1 hour and velocity of the reaction is not accelerated by addition of HNO 3 . Pt black is completely dissolved under the above con- ditions in 50 hours. (Delepine, C. R. 1905, 141. 1013.) Further data on solubility of Pt in H 2 SO 4 are given by Delepine. (C. R. 1906, 142. 631.) 95% H 2 SO 4 dissolves 0.04 g. Pt from com- mercial Pt at 250-260 in 28 hours. (Con- roy, J. Soc. Chem. Ind. 1903, 22. 465.) See also Quenessen. (Bull Soc. 1906, (3) 35. 620.) 0.0038 g. is dissolved by 10 cc. of boiling H 2 SO 4 . (McCoy, Eighth Inter. Cong. App. Chem. 1912. 2.) HC1+HNO 3 , so long as they are sufficiently dil. or the temperature is so low that they cannot react on each other, have no action on Pt. Addition of Cl does not bring about re- action, but a few drops of KNO 2 or N 2 O 3 +Aq bring about an immediate reaction. (Millon.) Slowly sol. in HI+Aq. (Deville, C. R. 42. 896.) Cone. H 3 PO 4 attacks Pt when heated in presence of air, but not in its absence. (Hiitt- ner, Z. anorg. 1908, 69. 216.) Pt dissolves easily in most acids when they contain H 2 O 2 . (Fairley, B. 1875, 8. 1600.) Slowly sol. in boiling FeCl 3 +Aq. (Saint- Pierre, C. R. 64. 1077.) FeCl 3 in acid solution is without influence on Pt. (Marie, C. R. 1908, 146. 476.) Pt is completely insol. in KCN+Aq. (Rossler, Z. Chem. 1866. 175.) Pt is attacked by boiling cone. KCN +Aq. (Deville and Debray, C. R. 82. 241.) Solubility of Pt in 10% KCN+Aq is very small at ord. temp. (1.4 mg. in 8 days) but is considerably greater in boiling cone. KCN +Aq. (71.5 mg. in 5 hours). (Glaser, Z. Elektrochem. 1903, 9. 15.) Pt foil is dissolved in boiling KCN+Aq (0.030 g. for 1 cc. in 1 hour). Insol. in cold KCN+Aq. (Brochet and Petit, C. R. 1904, C. R. 138. 1255.) Sol. in RbClJ+Aq. (Erdmann, Arch. Pharm. 1894, 232. 30.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Platinum ammonium compounds. Data published since the first edition of this work have not been included in this edition. See Platosamine comps., Pt Platosem^'amine comps., p, .NH 3 .NH 3 .R Pt< R. Platowonoefo'amine comps., NH 3 .NH 3 .R Platosamine comps., NH 3 NR 3 R ine comps., Pt

f ^NHs.NH.s.R Pt< NH 3 .R. Chloroplatinwonodiamine comps., NH 3 .NH 3 .R lodonitratoplatinmonodiamine comps., ^ Pt ^NH 3 .NH 3 .R 3 )Pt< NH3R Hydroxyloplatinmono^'amine comps., P ^NH 3 .NH 3 .R 2 Pt< NHsR Bromoplatindzamine comps., Rrp , NH 3 .NH 3 .R lir2 ^ t< NH 3 .NH 3 .R. Bromocarbonatoplatind^amine comps., Bromochloroplatin^'amine comps., BrClPt(NH 3 ) 4 R 2 . Bromohydroxyloplatindzamine comps., Br(OH)Pt(NH 3 ) 4 R 2 . Bromonitratoplatindiamine comps., Br(NO 3 )Pt(NH 3 ) 4 R 2 . Bromosulphatoplatindmmine comps., Br 2 (SO4)[Pt(NH 3 ) 4 R2] 2 . Carbonatochloroplatindzamine comps., (C0 3 )Cl 2 [Pt(NH 3 ) 4 R 2 ] 2 . Carbonatonitratoplatindiamine comps. , (C0 3 )(N0 3 ) 2 lPt(NH 3 ) 4 R 2 ] 2 . Chloroplatincfoamine comps., :i 2 Pt(NH 3 ) 4 R 2 . Chlorohydroxyloplatin^amine comps., ^1(OH)(NH 3 ) 4 R 2 . Chloroiodoplatinrfiamine comps., :iIPt(NH 3 ) 4 R 2 . Chloronitratoplatindiamine comps., Cl(NO 3 )Pt(NH 3 ) 4 R 2 . Hydroxyloplatindiamine comps., (OH) 2 Pt(NH 3 ) 4 R 2 . Hydroxylonitratocfoamine comps., (OH)(N0 3 )Pt(NH 3 ) 4 R 2 . Hydroxylosulphatodiamine comps., (OH) 2 S0 4 [Pt(NH 3 ) 4 R 2 ] 2 . lodoplatin^'amine comps., I 2 Pt(NH 3 ) 4 R 2 . lodonitritoplatindiamine comps., I(N0 2 )Pt(NH 3 ) 4 R 2 . Nitratoplatindiamine comps., (N0 3 ) 2 Pt(NH 3 ) 4 R 2 . Nitritoplatincfo'amine comps., (N0 2 ) 2 Pt(NH 3 ) 4 R 2 . Sulphatoplatindiamine comps., (S0 4 )Pt(NH 3 ) 4 R 2 . lodo^'platinamine comps., T p f< .NH 3 .R I Pt< NHaR T J> t .NH 3 .R Pt< NH 3 .R. Bromo^'platindiamine comps., NH 3 .NH 3 .R NH 3 .NH 3 .R Br Pt< R L .NH 3 .NH 3 .R Br ~ Pt< NH 3 .NH 3 .R. Hydroxylodiplatindiamine comps., (OH) 2 Pt 2 (NH 3 ) 8 R 4 . lodo^platin^amine comps., I 2 Pt 2 (NH 3 ) 8 R 4 . Nitratodiplatindiamine comps., (N0 3 ) 2 Pt 2 (NH 3 ) 8 R 4 . Platinfnamine comps., P p, .NH 3 .NH 3 .NH 3 .R K2rt< NH 3 .NH 3 .NH 3 .R. 7 7 e^raplatinamine comps., Pt 4 (NH 3 ) 8 Rio. Octoplatinamine comps., Pt 8 (NH 3 )i 6 Ri 8 . Platinum antimonide, PtSb 2 . (Christofie, 1863.) Platinum arsenide, Pt 3 As 2 . (Tivoli, Gazz. ch. it. 14. 487.) PtAs 2 . Min. Sperrylite. SI. attacked by aqua regia. (Wells, Sill. Am. J. (3) 37. 67.) Platinum arsenic hydroxide (?), PtAsOH. Insol. in, and slowly decomp. by H 2 O and alcohol. Easily decomp. by HCl+Aq; not attacked by HNO 3 +Aq. Sol. in aqua regia; not attacked by cold cone. H 2 SO 4 , but de- comp. on heating. (Tivoli, Gazz. ch. it. 14. 487.) PLATINOUS CHLORIDE CARBONYL 733 Platinum potassium azoimide. Ppt. Explodes violently even in aq. solu- tion. (Curtius, J. pr. 1898, (2) 68. 304.) Platinum boride, Pt 2 B 2 . Very slowly sol. in aqua regia. (Martins, A. 109. 79.) Platinous bromide, PtBr 2 . Insol. in H 2 O. Sol. in HBr+Aq. SI. sol. in KBr+Aq. (Topsoe, J. B. 1868. 274.) Platinic bromide, PtBr 4 . Not deliquescent; sol. in H 2 O. (Meyer and Ziiblin, B. 13. 404.) SI. sol. in H 2 O. 100 g. PtBr 4 +Aq sat. at 20 contain 0.41 g. PtBr 4 . (Halberstadt, B. 17. 2962.) Easily sol. in HBr+Aq; si. sol. in HC 2 H 3 O 2 +Aq. Sol. in considerable amount in K or NH 4 oxalate+Aq. Very si. sol. in alcohol or ether, also in glycerine. (Halberstadt.) Platinic hydrogen bromide. See Bromoplatinic acid. Platinous bromide carbonyl. See Carbonyl platinous bromide. Platinic bromide with MBr. See Bromoplatinate, M. Platinum carbide, PtC 2 . Hot aqua regia dissolves out nearly all the Pt. (Zeise, J. pr. 20. 209.) Platinum carbon efo'sulphide, PtCS 2 . See Platinum sulphocarbide. Platinum monochloride, PtCl+zH 2 O. Easily sol. in HC1; mod. sol. in hot dil. H 2 S0 4 without decomp. (Sonstadt, Proc. Chem. Soc. 1898, 14. 179.) Platinous chloride, PtCl 2 . Insol. in H 2 O, cone. H 2 SO 4 , or HNO 3 . Sol. in hot HCl+Aq with exclusion of air. (Ber- zelius.) Insol. in alcohol or ether; sol. in NH 4 OH + Aq. (Raewsky, A. ch. (3) 22. 280.) Sol. in aqua regia with formation of PtCl 4 . Insol. in cold cone. KI+Aq, but sol. when heated. (Lassaigne, A. ch. (2) 51. 117.) SI. sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Insol. in acetone. (Fidmann, C. C. 1899, II. 1014.) Platinum ^'chloride, PtCl 3 . SI. sol. in cold, more sol. in hot H 2 O. Partially hydrolyzed by boiling with H 2 O. Insol. in cold cone. HC1. Sol. in hot cone. HC1 with decomp. Sol. in KI+Aq. (Wohler, B. 1909, 42. 3961.) Platinic chloride, PtCl 4 . Not deliquescent. Very sol. in H 2 O. (Pul- linger, Chem. Soc. 61. 420.) Sp. gr. of aqueous solution containing: 5 10 15 20 25 % PtCl 4 , 1.046 1.097 1.153 1.214 1.285 30 35 40 45 50 % PtCl 4 . 1.362 1.450 1.546 1.666 1.785 (Precht, Z. anal. 18. 512.) Insol. in cone. H 2 SO 4 . (Dumas.) SI. sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Sol. in alcohol and ether; sol. in anhydrous acetone. (Zeise, A. 33. 34.) Insol. in ether. (Willstatter, B. 1903, 36. 1830.) SI. sol. in methvl acetate. (Naumann, B. 1909, 42. 3790.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) +H 2 O. Sol. in H 2 O. (Gutbier and Hem- rich, Z. anorg. 1913, 81. 378.) +4H 2 0. Sol. in H 2 O. (Pigeon, C. R. 1891, 112. 792.) +5H 2 O. Not deliquescent. Sol. in H 2 O or HCl+Aq. Composition is probably H 2 PtCl 4 O+4H 2 O. (Norton, J. pr. 110. 469.) +7H 2 O. Sol. in H 2 O. (Pigeon.) +8H 2 O. (Blondel, A. Ch. 1905, (8) 6. 98.) Platinic thallium chloride, Tl 3 Pt 2 Cl8H 5 O4. Ppt.; insol. in H 2 O. (Miolati, Z. anorg. 1900, 22. 460.) Platinous hydrogen chloride. See Chloroplatinous acid. Platinic hydrogen chloride. See Chloroplatinic acid. Platinous chloride with MCI. See Chloroplatinite, M. Platinic chloride with MCI. See Chloioplatinate, M. Platinous phosphorus chloride. See Phosphorus platinous chloride. Platinic phosphorus chloride. See Phosphorus platinic chloride. Platinous chloride carbonyl. See Carbonyl platinous chloride. 734 PLATINUM CHLORIDE HYDROXYLAMINE Platinum chloride hydroxylamine, Pt(NH 2 OH) 2 Cl 2 . Ppt. Sol. in alcohol and in ether. De- comp. in aq. solution. Pt(NH 2 OH) 4 Cl 2 . Sol. in H 2 O. (Uhlen- huth, A. 1900, 311. 124.) Platinous chloride sulphocarbamide, PtCl 2 , 4CS(NH 2 ) 2 . SI. sol. in H 2 O; very sol. in hot H 2 O; decomp. si. on boiling. (Kurnakow, J. pr. 1894, (2) 50. 483.) Platinum chloroiodide, PtCl 2 I 2 . Very deliquescent. (Kammerer, A. 148. 329.) PtClI 3 . Insol: in H 2 O. SI. sol. in alcohol. Sol. in KOH+Aq, from which it is pptd. by H 2 SO 4 . (Mather, Sill. Am. J. 27. 257.) Platinum chloronitride, PtNCl. (Alexander, C. C. 1887. 1254.) Platinous cyanide with MCN. See Platinocyanide, M. Platinous fluoride, PtF 2 f?). Insol. in H 2 O. (Moissan, A. ch. (6) 24. 287.) Platinic fluoride, PtF 4 . Deliquescent. Sol. in H 2 O with immediate decomp. into PtO 4 H 4 and HF. (Moissan, C. R. 109. 807.) Platinous hydroxide, PtO 2 H 2 . Sol. in HC1, HBr, and H 2 SO 3 +Aa, but not in other oxygen acids. Decomp. by boiling KOH+Aq. (Thomsen, J. pr. (2) 16. 344.) When freshly pptd, is insol. in dil. HNO 3 and H 2 SO 4 , and in HC 2 H 3 O 2 ; sol. in cone. HNO 3 and H 2 SO 4 . Very sol. in H 2 SO 3 and HC1. After drying, is insol. in cone. HNO 3 and H 2 SO 4 . (Wohler, Z. anorg. 1904, 40. 424.) Platinic hydroxide, Pt(OH) 4 . Easily sol. in dil. acids and in NaOH+Aq. (Topsoe', J. B. 1870. 386.) Nearly insol. in acetic acid. (Dobereiner.) Insol. in all acids except cone. HC1 and aqua' regia. fWohler, Z. anorg. 1904, 40. 438.) +H 2 O. Ppt. (Prost, Bull. Soc. (2) 44. 256.) Insol. in 2N-H 2 SO 4 and dil. HNO 3 +Aq: mod. sol. in cone. HNO 3 , H 2 SO 4 , 2N-HC1 and NaOH+Aq. (Wohler.) +2H 2 O. Easily sol. in dil. acids, even acetic acid, and in NaOH+Aq. (Topsoe.) Insol. in acetic acid; si. sol. in 2N-H 2 SO 4 and HNO 3 ; easily sol. in HC1, and NaOH+ Aq. (Wohler.) Platinoplatinic hydroxide, Pt 3 O 4 , 9H 2 O. Ppt. (Prost, Bull. Soc. (2) 46. 156.) 11H 2 O. Ppt. (Prost.) Platinum hydroxylamine comps. See Plato^oxamine comps., Pt(NH 3 O) 4 R 2 . Platosoxamine comps., Pt(NH 3 O) 2 R 2 . Platosoxamine-amine comps., Pt(NH 3 O) 3 NH 3 R 2 . Platinous iodide, PtI 2 . Insol. in H 2 O, acids, or alcohol. (Lassaigne, A. ch. (2) 51. 113.) Difficultly sol. in Na 2 SO 3 +Aq. (Topsoe.) Gradually decomp. by hot HI+Aq of 1.038 sp. gr., also by hot KI+Aq, PtI 4 being dis- solved out and Pt left behind. Not attacked by cone. H 2 SO 4 , HC1, or HNO 3 +Aq, but gradually decomp. by KOH or NaOH+Aq. (Lassaigne.) Insol. in acetone. (Eidmann, C. C. 1889, II. 1014.) Platinic iodide, PtI 4 . Insol. in H 2 O. Sol. in NaOH or Na 2 CO 3 + Aq, H 2 SO 3 , or Na 2 SO 3 +Aq. Sol. in HI+Aq or alkali iodides +Aq. Sol. in alcohol, with partial decomp. Not attacked by acids. (Lassaigne, A. ch. (2) 61. 122.) Very sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) Sol. in alcohol. (Belluci, C. C. 1902, I. 625.) Platinic iodide with MI. See lodoplatinate, M. Platinum nitride chloride, PtNCl. See Platinum chloronitride. Platinous oxide, PtO. Sol. in H 2 SO 3 +Aq. Insol. in other acids. (Dobereiner, Pogg. 28. 183.) Sol. in cone. H 2 SO 4 ; easily in cone. HC1+ Aq. (Storer's Diet.) Very si. sol. in HCl+Aq. SI. sol. in aqua regia. (Wohler, B. 1903, 36. 3482.) Platinic oxide, PtO 2 . Insol. in acids, even aqua regia. (Wohler, Dissert, 1901.) Platinum noxide, PtO 3 Unattacked by dil. H 2 SO 4 , HNO 3 or acetic acid Sol. with decomp. in dil. and cone. HC1, cone. H 2 SO 4 or cone. HNO 3 . (Wohler, B. 1909, 42. 3329.) Platinum sesgwioxide, Pt 2 O 3 +zH 2 O. Insol. in dil. sol. in cone. H 2 SO 4 . SI. sol. in hot dil. HNO 3 . Sol. in HC1. Sol. in cone. alkali hydroxides +Aq. (Wohler, B. 1909, 42. 3964.) PLATINUM TELLURIDE 735 +2H 2 0. Insol. in HNO 3 and H 2 SO 4 . Insol. in alkalies +Aq, also cold dil. HCl+Aq. Sol. in aqua regia. (Dudley, Am. Ch. J. 1902, 28. 66.) +5H 2 O. (Delepine, Bull. Soc. 1910, (4) 7. 103.) Platinoplatinic oxide, Pt 3 O 4 . Not attacked by long boiling with HC1, HNO 3 , or aqua regia. (Jorgensen, J. pr. (2) 16. 344.) Does not exist. (Wohler, Z. anorg. 1904, 40. 450.) Platinum oxychloride, 3PtO, PtCl 2 (?). Sol. in HC1, and in KOH+Aq. (Kane, Phil. Trans. 1842. 298.) PtCl 2 (OH) 2 = H 2 PtCl 2 O 2 . (Jorgensen, J. pr. (2) 16. 345.) 5Pt0 2 , 2HC1+9H 2 O. Insol. in cold H 2 O; decomp. on boiling. Slowly sol. in HC1. (Blondel, A. ch, 1905, (8) 6. 100.) Platinum oxysulphide, PtOS. See Platinum sulphydroxide. Platinum phosphide, PtP 2 . Insol. in HCl+Aq. Sol. in aqua regia. (Schrotter, W. A. B. 1849. 303.) PtP 2 H 2 . Insol. in H 2 O, and HCl+Aq. (Cavazzi, Gazz. ch. it. 13. 324.) PtP. Insol. in aqua regia. (Clark and Joslin.) Pt 2 P. Sol. in aqua regia. (Clark and Joslin.) Pt 3 P 5 . Partially sol. in aqua regia. (Clark and Joslin, C. N 48. 385.) Attacked very slowly by aqua regia. Rapidly sol. in molten alkalies. (Granger, C. N. 1898, 77. 229.) Completely sol. in aqua regia if the action sufficiently prolonged, though with difficulty. (Granger, C. R. 1893, 123. 1285.) Platinum cftselenide, PtSe 2 . As PtS 2 . (Minozz;, Chem. Soc. 1909, 96. (2) 899.) Platinum friselenide, PtSe 3 . SI. attacked by hot cone. HNO 3 ; not at- tacked by cold cone. HCl+Aq; slowly sol. in aqua regia and Cl 2 +Aq; insol. in CS 2 . Platinum silicide, Pt 2 Si. Sol. in hot aqua regia. (Vigouroux, C. R. 1896, 123. 117.) Pt 3 Si 2 . (Co^on, C. R. 94. 27.) Pt 4 Si 3 . Slowly decomp. by aqua regia. (Guyard, Bull. Soc. (2) 25. 511.) PtSi. Insol. in HNO,, H 2 SO 4 , HF, and HC1. Completely sol. in aqua regia. (Lebeau and Novitzky, C. R. 1907, 145. 241.) Platinum sulphydroxide, PtOS+H 2 O = PtS(OH) 2 . Decomp. easily into Pt 2 S 2 3 H 2 =^| O gg = PtOS + ^H 2 0. H 2 cannot be removed without decomposing the compound, (v. Meyer, J. pr. (2) 15. 1.) Platinous sulphide, PtS. Not attacked by boiling acids, aqua regia, or KOH+Aq. (BSttger, J. pr. 2. 274.) Sol. in large excess of (NH 4 ) 2 S+Aq. Platinoplatinic sulphide, Pt 2 S 3 . Not attacked by HC1 or HNO 3 +Aq, and only slowly by aqua regia. (Schneider, Pogg. 138.607.) Platinic sulphide, PtS 2 . Anhydrous. Aqua regia attacks si., other acids not at all. (Davy.) Hydrated Insol. in HCl+Aq; si. sol. in boiling HNO 3 +Aq. Sol. n aqua regia. (Fresenius.) Sol. in alkali sulphides, hydrates and carbonates +Aq. (Berzelius.) Very si. sol. in (NH 4 ) 2 S+Aq. (Claus.) Insol. in NH 4 C1, or NH 4 NO 3 +Aq. 1 pt. PtCl 4 in 100 pts. H O+25 pts. HC1 is not pptd. by H 2 S. (Reinsch.) Difficultly sol. in alkali sulphydroxides+ Aq, but more easily in presence of SnS, Sb 2 S 3 , As 2 S 3 , or SnS 2 . (Ribau, C. R. 86. 283.) Platinum sulphide, Pt 6 S 6 , or T^raplatinum sulphoplatinate, 4PtS, PtS 2 . Decomp. on moist air, but not attacked by acids. (Schneider, J. pr. (2) 7. 214.) Platinum sulphides with M 2 S. See Sulphoplatinate, M. Platinum sulphocarbide, PtC 2 S 2 . Not attacked by hot HC1, HN0 3 +Aq, slightly by aqua regia. (Schiitzenberger, C. R. 111. 391.) Platinum teUuride, PtTe. Decomp. by fused oxidizing agents; slowly sol. in cone. HNO 3 . (Roessler, Z. anorg. 1897, 15. 407.) Platinum ditelluride, PtTe 2 . Insol. in boiling cone. KOH+Aq; slowly sol. in boiling cone. HNO 3 ; decomp. oy fused oxidizing agents. (Roessler.) Plato-. See also Plathio-. 736 PLATOAMIDOSULPHONIC ACID Platoamidosulphonic acid. Potassium platoamidosulphonate, K 2 Pt(NH 2 S0 3 ) 4 +2H 2 0. Very si. sol. in cold H 2 O; sol. in 10 pts. boiling H 2 O. (Ramberg and St. Kahlen- berg, B. 1912, 46. 1514.) Sodium , Na 2 (Pt(NH 2 S0 3 ) 4 +4H 2 O. Very sol. in H 2 6. (Ramberg and St. Kahlenberg.) Platocframine bromide, Pt[(NH 3 ) 2 Br] 2 + 3H 2 O. Easily sol. in H 2 O. (Cleve.) carbonate, Pt(N 2 H 6 ) 2 CO 3 +H 2 O. Sol. in H 2 O. (Peyrone, A. 61. 14.) Pt(N 2 H 6 Cp 3 H) 2 . SI. sol. in, but decomp. by boiling with H 2 O into sesgm'carbonate. More sol. than preceding salt. (Reiset, C. R. 11. 711.) chloride, Pt[(NH 3 ) 2 Cl] 2 +H 2 0. "Reiset's first chloride." Sol. in 4 pts. H 2 O at 16.5, and in less hot H 2 O. Insol. in alcohol or ether. (Reiset, A. ch. (3) 11. 419.) As sol. in NH 4 Cl+Aq as in H 2 O; insol. in absolute alcohol; si. sol. in dil. alcohol; very sol. in dil. HCl+Aq. (Peyrone, A. ch. (3) 12. 19o.) cuprous chloride, Pt(NH 3 ) 4 Cl 2 , Cu 2 Cl 2 . Sol. in H 2 O, and pptd. from H 2 O solution by alcohol. (Buckton.) cupric chloride, Pt(NH 3 ) 4 Cl 2 , CuCl 2 . SI. sol. in cold, decomp. by hot H 2 O into Pt(NH 3 ) 4 Cl 2 , Cu 2 Cl 2 . (Buckton, Chem. Soc. 6. 218.) Nearly insol. in H 2 O; easily sol. in warm HCl+Aq; insol. in alcohol. (Millon and Commaille, C. R. 67. 822.) Millon and Commaille's salt is Cu(NH 3 ) 4 Cl 2 , PtCl 2 , cuprammonium chloro- platinite. lead chloride, Pt(NH 3 ) 4 Cl 2 , PbCl 2 . Sol. in hot, much less in cold H 2 O. Insol. in HCl+Aq or alcohol. (Buckton, Chem. Soc. 6. 213.) mercuric chloride, Pt(NH 3 ) 4 Cl 2 , HgCl 2 . Easily sol. in hot H 2 O, much less in cold. Insol. in HCl+Aq. (Buckton.) zinc chloride, Pt(NH 3 ) 4 Cl 2 , ZnCl 2 . Easily sol. in hot H 2 O. Insol. in alcohol. (Buckton.) Plato^amine chloroplatinate, Pt(NH 3 ) 4 Cl 2 , PtCl 4 . Ppt. Inso]. in H 2 O. (Cossa, Gazz. ch. it. 17. 1.) chloroplatinite, Pt(NH 3 ) 4 Cl 2 , PtCl 2 . (Magnus' green salt.) Insol. in, and not de- comp. by H 2 O, HCl+Aq, or alcohol. (Mag- nus.) Slowly sol. in boiling NH 4 OH+Aq and in cone. NH 4 salts +Aq. (Reiset, A. ch. (3) 11. 427.) Almost as sol. in (NH 4 ) 2 CO 3 +Aq as in NH 4 OH+Aq. Sol. in hot PtCl 4 +Aq. (Rei- set.) Not decomp. by boiling KOH, dil. HC1, or H 2 SO 4 +Aq, but easily by HNO 3 +Aq. (Gros, A. 27. 245.) chromate, Pt(NH 3 ) 4 CrO 4 . Scarcely sol. in H 2 O. (Cleve.) bichromate, Pt(NH 3 ) 4 Cr 2 O 7 . SI. sol. in H 2 O. Insol. in alcohol. Sol. in KOH+Aq. (Buckton, Chem. Soc. 6. 213.) platinous cyanide, Pt(NH 3 ) 4 (CN) 2 , Pt(CN) 2 . SI. sol. in cold, easily in boiling H 2 O; sol. in KOH, HC1, and dil. H 2 SO,+Aq without decomp., but cone. H 2 SO 4 decomposes. potassium ferrocyanide, Pt(NH 3 ) 4 K 2 [Fe(CN) 6 ] 2 +3H 2 0. hydroxide, Pt[(NH 3 ) 2 OH] 2 . " Reiset's first base." Easily sol. in H 2 O. SI. sol. in alcohol. ' iodide, Pt[(NH 3 ) 2 I 2 ]. SI. sol. in cold, more easily in hot H 2 O, but slowly decomp. on boiling. (Reiset.) nitrate, Pt[(NH 3 ) 2 NO 3 ] 2 . Sol. in about 10 pts. boiling H 2 O. Insol. or but si. sol. in alcohol. (Peyrone, A. ch. (3) 12. 203.) nitrate sulphate, [Pt(NH 3 ) 4 NO 3 ] 2 SO 4 , Pt(NH 3 ) 4 S0 4 . Very easily sol. in H 2 O. (Carlgren, Sv. V. A. F. 47. 310.) nitrite, Pt[(NH 3 ) 2 NO 2 ] 2 +2H 2 O. Efflorescent. Very sol. in hot or cold H 2 O. Insol. in 90% alcohol. (Lang.) platinous nitrite, Pt[(NH 3 ) 2 NO 2 ] 2 , Pt(N0 2 ) 2 . Scarcely sol. in cold, somewhat more easily in hot H 2 O. Not attacked by cold dil. acids. More sol. in NH 4 OH+Aq than in H 2 O. (Lang.) PLATOAMINE SULPHATE 737 Plataftamine phosphate, Pt(N 2 H 6 ) 2 HPO 4 +H 2 0. Rather difficultly sol. in cold, and very easily in hot H 2 O. (Cleve.) ammonium phosphate, Pt[(N 2 H 6 )PO 4 (NH 4 )2]2, 4NH 4 H 2 PO 4 + H 2 O. Very easily sol. in H 2 O with decomp. into Pt(N 2 H 6 H 2 PO 4 ) 2 , 2NH 4 H 2 PO 4 +9H 2 O. Much more sol. in H 2 O than the preceding, comp. (Cleve.) sulphate, Pt(NH 3 ) 4 SO 4 . Sol. in 32 pts. H 2 O at 16.5; more easily when heated . ( Reiset . ) Sol. in 50-60 pts. boiling H 2 O; less in cold ing (Clc H 2 O; insol. in alcohol. (Cleve.) sulphate, acid, Pt[(NH 3 ) 2 SO 4 H] 2 +H 2 O. Decomp. by H 2 O or alcohol into neutral salt. 3Pt(NH 3 ) 4 SO 4 , H 2 SO 4 +H 2 O. Sol. in H 2 O. (Cleve.) sulphite, Pt(NH 3 ) 4 SO 3 . Nearly insol. in cold H 2 O. (Birnbaum, A. 152. 143.) Pt[(NH 3 ) 2 S0 3 H] 2 +2H 2 0. HCl+Aq. (Cleve.) Ppt. Sol. in platinous sulphite, 3Pt(NH 3 ) 4 SO 3 , PtSO 3 +2H 2 O. Scarcely sol. in cold H 2 O; sol. in 190 pts. H 2 O at 100. Easily sol. in warm HCl+Aq with decomp. (Peyrone.) +4H 2 O. (Carlgren, Sv. V. A. F. 47. 308.) 2Pt(NH 3 ) 4 SO 3 , PtSO 3 , H 2 SO 3 Insol. in cold H 2 O or alcohol. Scarcely sol. in hot H 2 O. (Peyrone.) sulphocyanide, Pt(NH 3 ) 4 (CNS) 2 +H 2 O. Very sol. in H 2 O. Solution is decomp. on boiling. (Cleve, Sv. V. A. H. 10, 9. 7.) platinous sulphocyanide, Pt(NH 3 ) 4 (CNS) 2 , Pt(CNS) 2 . Insol. in H 2 O and alcohol; sol. in dil. HC1+ Aq. (Buckton, Chem. Soc. 13. 122.) Platowumodiamine chloride, Pt Easily sol. in H 2 O. (Cleve.) Pla.tomonodiam.ine chloroplatinite 2P (NH 3 ) 2 C1 ptri 2Pt ' PtUz ' NH,Cl Moderately sol. in cold, but more easily in hotH 2 O. (Cleve.) nitrate, Easily sol. in H 2 O. (Cleve.) PUtoroonoeKamine sulphate, Easily sol. in cold, but much more in hot H 2 O. Platosemiaiamine bromide, Sol. in H 2 O. Easily sol. in NH 4 OH+Aq. (Cleve.) - chloride, Pt' NO ' Moderately sol. in H 2 O. (Cleve.) - nitrite, Very si. sol. in cold, more easily in hot H 2 O. oxalate, Pt(NH 3 ) 2 C 2 O 4 . (Cleve.) +2H 2 O. (Cleve.) - sulphate, Pt< (NH 3 ) 2>ga Very si. sol. even in hot H 2 O. (Cleve.) 738 PLATOAMINE SULPHOCYANIDE Platosemirfiamine sulphocyanide, Pt(SCN)(NH 3 ) 2 SCN. Easily sol. in warm H 2 O, but solution soon decomposes. PlatosewiVfa'amine sulphurous acid. Ammonium platoseraicftamine sulphite, Pt< (NH 3 ) 2 S0 3 (NH 4 ) rNH N SO Ft< S0 3 (NH 4 ) ' (NH 4 ) 2 b0 3 . Very sol. in H 2 O. (Cleve.) Barium , Pt(SO 3 )[(NH 3 ) 2 SO 3 ]Ba, BaSO 3 . Ppt. (Cleve.) Silver . Pt(S0 3 Ag)[(NH 3 ) 2 S0 3 Ag], Ag 2 S0 3 . Ppt. (Cleve.) Diplatocfo'amine chloride, Pt 2 (NH 3 ) 4 Cl 2 . Insol. in H 2 O. hydroxide, Pt 2 (NH 3 ) 4 (OH) 2 +H 2 O. Insol. in H 2 O. nitrate, Pt 2 (NH 3 ) 4 (NO 3 ) 2 . Insol. in H 2 O. (Cleve.) sulphate, Pt 2 (NH 3 ) 4 SO 4 . Insol. in H 2 O. (Cleve.) Platobromonitrous acid. Potassium platobromonitrite, K 2 Pt(NO 2 ) 3 Br +2H 2 0. Sol. in about 3 pts. cold, and 2 pts. boiling H 2 O. (Vezes, A. ch. (6) 29. 194.) K 2 Pt(NO 2 ) 2 Br 2 -fH 2 O. Sol. in 1 pt. cold, and still less hot H 2 O. Insol. in alcohol. Platochloronitrous acid. Potassium chloronitrite, K 2 Pt(NO 2 )sCl + 2H 2 O. Sol. in about 3 pts. cold, and 2 pts. boiling H 2 O. (Vezes, A. ch. (6) 29. 178.) K 2 Pt(NO 2 ) 2 Cl 2 . Sol. in about 3 pts. cold, and 2 pts. boiling H 2 O. (Vezes.) Platochlorosulphurous acid. See Chloroplatosulphurous acid. Platoiodonitrous acid, H 2 Pt(NO 2 ) 2 I 2 . Known only in solution. (Nilson, J. pr. (2) 21. 172.) Aluminum platoiodonitrite, Al 2 [Pt(NO 2 ) 2 I 2 ] 3 +27H 2 0. Easily sol. in H 2 O. (Nilson.) Ammonium, (NH 4 ) 2 Pt(NO 2 ) 2 I 2 +2H 2 O. Sol. in H 2 O; decomp. on heating. Barium platoiodonitrite, BaPt(NO 2 ) 2 Io 4H 2 O. Very sol. in H2O. Cadmium - , CdPt(NO 2 ) 2 I 2 +2H 2 O. Easily sol. in H 2 O. Caesium - , Cs 2 Pt(NO 2 ) 2 I 2 +2H 2 O. Easily sol. in H 2 O. Calcium, CaPt(NO 2 ) 2 I 2 +6H 2 O. Very easily sol. in H 2 O. Cerium - , Ce 2 [Pt(NO 2 ) 2 I 2 ] 3 + 18H 2 O. Easily sol. in H 2 O. Cobalt, CoPt(NO 2 ) 2 I 2 +8H 2 O. Sol. in H 2 O. Didymium , Di 2 [Pt(NO 2 ) 2 I 2 ] 3 +24H 2 O. Sol. in H 2 O. Erbium - , Er 2 [Pt(NO 2 ) 2 I 2 Sol. in H 2 O. H 2 O. Ferrous , FePt(NO 2 ) 2 I 2 +8H 2 O. Sol.inH 2 O. Ferric - , Fe 2 [Pt(NO 2 ) 2 I 2 ] 3 +6H 2 O. Sol. in H 2 O. Lanthanum - , La 2 [Pt(NO 2 ) 2 I 2 ] 3 +24H 2 O. Sol. in H 2 O. Lead , basic, PbPt(NO 2 ) 2 I 2 , Pb(OH) 2 . Insol. in H 2 O. Lithium - -, Li 2 Pt(NO 2 ) 2 I 2 +6H 2 O. Very sol. in H 2 O. Magnesium -, MgPt(NO 2 ) 2 I 2 +8H 2 O. Sol. in H 2 O. Manganese - , MnPt(NO 2 ) 2 I 2 +8H 2 O. Sol. in H 2 O. Mercurous Hg 2 0+9H 2 6, Insol. in H 2 O. basic, 2Hg 2 Pt(NO 2 ) 2 I 2 , Nickel , NiPt(NO ? ) 2 I 2 +8H 2 O. Sol.inH 2 O. Potassium, K 2 Pt(NO 2 ) 2 I 2 +2H 2 O. Sol. hi H 2 O in all proportions. Very sol. hi alcohol. Rubidium, Rb 2 Pt(NO 2 ) 2 I 2 +2H 2 O. i Sol. inH 2 O. PLATONITRITE, POTASSIUM 739 Silver platoiodonitrite, Ag 2 Pt(NO 2 ) 2 l2. Insol. in H 2 O. Sodium - , Na 2 Pt(NO 2 ) 2 I 2 +4H 2 O. Very sal. in H 2 O. Strontium - , SrPt(NO 2 ) 2 I 2 +8H 2 O. Sol. in H 2 O. Thallium -- -, Tl 2 Pt(NO 2 ) 2 I 2 . Insol. in H 2 O. Yttrium , Y 2 [Pt(NO 2 ) 2 I 2 ] 3 +27H 2 O. Sol. in H 2 O. Zinc -- -, ZnPt(N0 2 ) 2 I 2 +8H 2 O. Sol. in H 2 O. Tn'platoocfonitrosylic acid, H 4 Pt 3 O(NO 2 ) 8 . (Nilson, J. pr. (2) 16. 241.) Potassium ^nplatooctonitrosylate. See under Platonitrite, potassium. Platonitrous acid, H 2 Pt(NO 2 ) 4 . Sol. in H 2 O or alcohol. (Lang. J. pr. 83. 419.) Is called " Platotefranitrosylic acid" by Nilson. Aluminum platonitrite, Al 2 [Pt(NO 2 ) 4 ] 3 + 14H 2 O. Sol. in H 2 O. Al 2 (OH) 2 [Pt(NO 2 ) 2 ] 4 O 2 + 10H 2 O. SI. sol. in cold, easily in hot H 2 O and alcohol. (Nil- son, B. 9. 1727.) Ammonium platonitrite, (NH 4 ) 2 Pt(NO 2 ) 4 + 2H 2 0. Moderately sol. in cold H 2 0. (Nilson, B. 9. 1724.) Barium platonitrite, BaPt(NO 2 ) 4 +3H 2 O. SI. sol. in cold, very sol. in hot H 2 O. (Lang.) Cadmium platonitrite, CdPt(N0 2 ) 4 +3H 2 O. Easily sol. in H 2 O. (Nilson.) Caesium platonitrite, Cs 2 Pt(NO 2 )4. Resembles K salt. Calcium platonitrite, CaPt(NO 2 ) 4 +5H 2 O. Very sol. in H 2 O. (Nilson.) Cerium platonitrite, Ce 2 [Pt(NO 2 )4] 3 Sol. inH 2 O. (Nilson.) Chiomium diplatonitrite, r 2 (OH) 2 [Pt(NO 2 ) 2 ] 4 O 2 +24H 2 O. " Sol. inH 2 O. (Nilson.) Cobalt platonitrite, CoPt(NO 2 ) 4 +8H 2 O. Easily sol. in H 2 O. (Nilson.) Copper platonitrite, CuPt(NO 2 ) 4 +3H 2 O. Sol. in H 2 O. (Nilson.) 3CuPt(NO 2 ) 4 , CuO + 18H 2 O. Decomp. by H 2 O. (Nilson.) Didymium platonitrite, Di 2 [Pt(NO 2 ) 4 ] 3 -f- 18H 2 0. Deliquescent; sol. in H 2 O. Erbium platonitrite, Er 2 [Pt(NO 2 ) 4 ] 3 +9, and 21H 2 0. Deliquescent: sol. in H 2 O. Glucinum diplatonitrite, Gl r Pt(NO 2 ) 2 ] 2 O-h 9H 2 O. SI. sol. in cold H 2 O. Indium ^platonitrite, In(OH) 2 [Pt(NO 2 ) 2 ] 4 O 2 + 10H 2 O. SI. sol. in H 2 O. Fenic ^'platonitrite, Fe 2 [Pt(NO 2 ) 2 ] 6 O 3 + 30H 2 O. SI. sol. in cold, easily in hot H 2 O. Lanthanum platonitrite, La 2 [Pt(NO 2 ) 4 ] 3 + 18H 2 O. Deliquescent; sol. in H 2 O. Lead platonitrite, PbPt(NO 2 ) 4 +3H 2 O. SI. sol. in H 2 O. (Nilson.) Lithium platonitrite, Li 2 Pt(NO 2 ) 4 +3H 2 O. SI. deliquescent; easily sol. in H 2 O. Magnesium platonitrite, MgPt(NO 2 ) 4 +5H 2 O. Easily sol. in H 2 O. Manganese platonitrite, MnPt(NO 2 ) 4 + 8H 2 O. Sol. in H 2 O. Mercurous platonitrite, Hg 2 Pt(NO 2 ) 4 , Hg 2 O ? Nearly insol. in H 2 O. (Lang, J. pr. 83. 415.) +H 2 6. Nearly insol. in H 2 O. (Nilson.) Nickel platonitrite, NiPt(NO 2 ) 4 +8H 2 O. Easily sol. in H 2 O. (Nilson.) Potassium platonitrite, K 2 Pt(NO 2 ) 4 . Sol. in 27 pts. H 2 O at 15; more easily sol. in warm H 2 O. (Lang, J. pr. 83. 415.) +2H 2 O. Efflorescent. (Lang.) K 2 H 4 Pt 3 O(NO 2 ) 6 +3H 2 O. Very si. sol. in cold (0.01 mol. in 1 1. at 16), but very easily in hot H 2 O. (Vezes, A. ch. (6) 29. 162.) K 4 Pt 3 O(NO 2 ) 8 +2H 2 O. SI. sol. in warm H 2 O. (Nilson.) 740 PLATONITRITE, POTASSIUM, BROMIDE Potassium platonitrite bromide. See Platibromonitrite and platobromoni- trite, potassium. Potassium platonitrite chloride. See Plati- and platochloronitrite, potassium. Potassium plat nitrite hydrogen chloride. K 2 Pt(N0 2 ) 4 , HC1. Sol. in H 2 O. (Miolati, Att. Line. Rend. 1896, (5) 6, II. 358.) Potassium platonitrite iodide. See Plati- and platoiodonitrite, potassium. Potassium platonitrite nitrogen dioxide, K,PtrNOi) 4> 2NO 2 . Violently decomp. by H 2 0. (Miolati, Atti Line. Rend. 1896, (5) 6, II, 356.) Rubidium platonitrite, Rb 2 (Pt)(NO 2 ) 4 , and +2H 2 0. Very slowly sol. in cold, more easily in warm H 2 O. (Nilson.) Silver platonitrite, Ag 2 Pt(NO 2 ) 4 . Very si. sol. in cold, easily in hot H 2 O. Silver ^platonitrite, Ag 2 Pt 2 (NO 2 ) 4 O. Insol. in H 2 O. (Nilson.) Sodium platonitrite, Na 2 Pt(N0 2 ) 4 . Easily sol. in H 2 O. Strontium platonitrite, SrPt(NO 2 ) 4 +3H 2 O. Somewhat si. sol. in cold H 2 O, but easily sol. in warm H 2 O. Thallium platonitrite, Tl 2 Pt(NO 2 ) 4 . Very si. sol. in H 2 O. (Nilson.) Yttrium platonitrite, Y 2 [Pt(NO 2 )J 3 +9, or 21H 2 0. Sol. in H 2 O. Zinc platonitrite, ZnPt(NO 2 ) 4 +8H 2 O. Sol. in H 2 0. Plato d /examine chloride, Pt(NH 3 O.NH 3 OCl) 2 . Easily sol. in H 2 O. (Alexander, A. 246. 239.) chloroplatinite, Pt(NH 3 O.NH 3 OCl) 2 , PtCl 2 . Sol. in warm HCl+Aq. Insol. in cold H 2 O or alcohol; very si. sol. in hot H 2 O. (Alex- ander.) hydroxide, Pt(NH 3 O.NH 3 O) 2 (OH) 2 . Insol. in B 2 O or alcohol. Easily sol. in HC1 or HNO 3 +Aq. Difficultly sol. in hot dil. H 2 SO 4 +Aq. (Alexander.) Platodioxamine oxalate, Pt(NH 3 O.NH 3 O) 2 C 2 O 4 . Insol. in cold H 2 O, alcohol, or organic acids. (Alexander.). phosphate, Pt 3 (NH 3 O.NH 3 O) 12 (PO 4 ) 2 -f 3H 2 O. Ppt. (Alexander.) sulphate, Pt(NH 3 O.NH 3 O)SO 4 +H 2 O. SI. sol. in H 2 O. (Alexander,) Platosamine bromide, Pt(NH 3 Br) 2 . SI. sol. even in hot H 2 O. (Cleve.) - chloride, Pt(NH 3 Cl) 2 . " Reiset's second chloride." Sol. in 1 40 pts. H 2 O at 100. (Peyrone, A. 61. ISO.) Sol. in 130 pts. H 2 O at 100, and 4472 pts. atO. (Cleve.) Easily sol. in NH 4 OH+Aq, HNO 3 , or aqua regia, with decomp. Sol. in KClSl -j-Aqfwith evolution of NH 3 . (Cleve.) ammonium chloride, Pt(NH 3 Cl) 2 , 2NH 4 C1. SI. sol. in cold, easily in hot H 2 O; insol. in alcohol; sol. in NH 4 OH or (NH 4 ) 2 CO 3 +Aq. (Grimm, A. 99. 75.) * Platosamine chlorosulphurous acid, p,NH 3 Cl rt NH 3 SO 3 H. Easily sol. in H 2 O without decomp. (Cleve.) Ammonium platosamine chlorosulphite, Pt(NH 3 Cl)NH 3 SO 3 NH 4 +H 2 O. Sol. in H 2 O. (Peyrone, A. 61. 180.) Platosamine cyanide, Pt(NH 3 CN) 2 . Quite easily sol. in H 2 O or NH 4 OH+Aq. (Buckton.) hydroxide, Pt(NH 3 OH) 2 . "Reiset's second base." Very sol. in H 2 O. (Odling, B. 3. 685.) iodide, Pt(NH 3 I) 2 . Very si. sol. in H 2 O. Sol. in cold NH 4 OH+ Aq to form platodiamine iodide. (Cleve.) nitrate, Pt(NH 3 NO 3 ) 2 . Moderately sol. in hot H 2 O. Sol. in NH 4 OH+Aq with combination. (Reiset, A. ch. (3) 11. 26.) nitrite, Pt(NH 3 NO 2 ) 2 . Very si. sol. in cold, easily in hot H 2 O. Insol. in alcohol. (Lang.) PLATOSULPHITE, POTASSIUM 741 Platosamine platinous nitrite, Pt(NH 3 NO 2 ) Pt(N0 2 ) 2 . Slowly and si. sol. in cold, more easily sol. in hot H 2 O. Extremely si. sol. even in cone, acids; more sol. in NH 4 OH+Aq than in H 2 O. (Lang.) oxide, Pt(NH 3 ) 2 O. Insol. in H 2 O or NH 4 OH+Aq. (Reiset.) oxalate, Pt(NH 3 ) 2 H 2 (C 2 O 4 ) 2 +2H 2 O. Ppt. (Cleve.) sulphate, Pt(NH 3 ) 2 SO 4 +H 2 O. SI. sol. in cold, more easily in hot H 2 O. sulphite, Pt(NH 3 ) 2 SO 3 +H 2 O. Easily sol. in H 2 O. (Cleve.) sulphocyanide, Pt(NH 3 SCN) 2 . Insol. in H 2 O; can be cryst. from alcohol; not attacked by HC1 or H 2 SO 4 +Aq. (Buck- ton.) Very sol. in hot H 2 O. (Cleve.) silver sulphocyanide, Pt(NH 3 ) 2 Ag 4 (SCN) 6 . (Cleve.) Platosamine sulphurous acid, Pt(NH 3 S0 3 H) 2 . Exists only in its salts. See Platosamine sulphite. Ammonium platosamine sulphite, Pt(NH 3 SO 3 NH 4 ) 2 . Sol. in H 2 O. Insol. in alcohol. Barium platosamine sulphite, Pt(NH 3 ) 2 (S0 3 ) 2 Ba+3H 2 0. Ppt. (Cleve.) Cobalt 6H 2 0. Pt(NH 3 ) 2 (S0 3 ) 2 CO + Very si. sol. in H 2 O. Sol. in HCl+Aq. Copper - 5H 2 O. , Pt(NH 3 ) 2 (SO 3 ) 2 Cu + Very si. sol. in H 2 O; sol. in HCl+Aq. , Pt(NH 3 ) 2 (S0 3 ) 2 Pb+H 2 0. Lead- Ppt. Manganese +4H 2 0. Ppt. SI. sol. in H 2 O. , Pt(NH ) 2 (SO 3 ) ? Mn Nickel -, Pt(NH 3 ) 2 (S0 3 ) 2 Ni+7H 2 0. SI. sol. in H 2 O. Sodium platosamine sulphite, Pt(NH 3 SO 3 Na) 2 +5^H 2 O. Sol. in H 2 O. 100 com. sat. solution at 20 contains 5.52 g. cryst. salt. (Haberland and Hanekop, A. 246. 235.) Silver Ppt. -, Pt(NH 3 S0 3 Ag) 2 +H 2 0. Uranyl -- , Pt(NH 3 ) 2 (SO 3 ) 2 UO 2 +H 2 O. Ppt. Zinc -- , Pt(NH 8 ) 2 (SO 3 ) 2 Zn+6H 2 O. Ppt. Very si. sol. in H 2 O. (Cleve.) Platososermamine potassium chloride, PtQ 11 ' 01 , KC1+H 2 0. Very sol. in H 2 O; insol. in alcohol. (Cossa, B. 23. 2507.) Platosoxamine chloride, Pt Sol. in H 2 O. Much less sol. in H 2 O than platoeftoxamine chloride. (Alexander, A. 246. 239.) Platosoxamine amine chloride, Easily sol. in H 2 O. Insol. in alcohol and cone. HCl+Aq. (Alexander, A. 246. 239.) - chloroplatinite, Ppt. Platosulphurous acid. Ammonium platosulphite, (NH 4 ) 6 Pt(SO 3 ) 4 + 3H 2 O. Sol. in H 2 O. (Birnbaum, A. 139. 170.) (NH 4 ) 2 Pt(SO 3 ) 2 +H 2 O. Sol.inH 2 O. (Lie- big, Pogg. 17. 108.) Ammonium platosulphite chloride, (NH 4 ) 2 Pt(S0 3 ) 2 , 2NH 4 C1. Sol. in H 2 O. (Birnbaum.) PtClSO 3 H, 2NH 4 C1. Deliquescent; sol. in H 2 O. (Birnbaum, A. 162. 143.) See also Chloroplatosulphite, ammonium. Potassium platosulphite, K 6 Pt(SO 3 ) 4 +4H 2 O. SI. sol. in cold, easily in hot H 2 O. Much more sol. than the Na salt. (Birnbaum, A. 139. 168.) +3H 2 O. (Lang, J. pr. 83. 415.) 6K 2 O, 2PtO, 10SO 2 . SI. sol. in H 2 O. Glaus, J. B. 1847-48. 453.) Does not exist. (Lang.) K 2 Pt(SO 3 ) 2 . Sol. in H 2 O. 742 PLATOSULPHITE, SILVER Silver platosulpbite, Ag 6 Pt(SO 3 ) 4 . Ppt. Very sol. in cold NH 4 OH+Aq. (Lang. J, pr. 83. 415.) Sodium platosulphite, Na 6 Pt(SO 3 ) 4 . Very si. sol. in cold, somewhat more easily in hot H 2 O. Not decomp. by boiling KOH or NaOH+Aq. Gradually sol. in (NH 4 ) 2 S or K 2 S+Aq. Insol. in NaCl+Aq or alcohol. (Litton and Schnedermann, A, 42. 316.) +7H 2 O. Na 2 Pt(SO 3 H) 4 . Moderately sol. in H 2 0. (Litton and Schnedermann.) Platothiosulphuric acid. Sodium platothiosulphate, Na 6 Pt(S 2 O 3 ) 4 + 10H 2 O. Very sol. in H 2 O (Schottlander, A. 140. 200.) PtS 2 O 3 , 4Na 2 S 2 O 3 + 10H 2 O. PtS 2 O 3 , 6Na 2 S 2 O 3 + 19H 2 O. 2Pt 2 S 2 O 3 , 7Na 2 S 2 O 3 + 18H 2 O. (Jochum, C. C. 1885. 642.) Plumbic acid. Barium plumbate, Ba 2 PbO 4 . Insol. in H 2 O. Sol. in HCl+Aq with evolution of Cl. Sol. in acids in presence of a reducing substance. (Kassner, Arch. Pharm. 228. 109.) Calcium plumbate. Insol. in H 2 O. HNO 3 +Aq dissolves out CaO. (Crum, A. 65. 218.) Ca 2 PbO 4 . Properties as Ba 2 PbO 4 . (Kass- ner, Arch. Pharm. 228. 109.) +4H 2 O. Easily decomp. by HNO 3 . (Kassner, Arch. Pharm. 1894, 232. 378.) Calcium hydrogen plumbate, H 2 CaPb 2 O 6 . Fairly stable; slowly sol. in HNO 3 in the cold. (Kassner.) Calcium lead or//ioplumbate, CaPbPbO 4 . Insol. in H 2 O. Sol. in HC1. HNO 3 , acetic and other acids cause a separation of PbO 2 . (Kassner, Arch. Pharm. 1903, 241. 147.) Copper raetaplumbate, CuPbO 3 . Decomp. by acids. Insol. in NH 4 OH+Aq. Acetic acid dissolves Cu. (Hoehnel, Arch. Pharm. 1896, 234. 399.) Lead raetaplumbate, PbPbO 3 . Identical with lead sesquioxide. (Hoehnel, Arch. Pharm. 1896, 234. 399.) Manganese metoplumbate. Decomp. by acids. (Hoehnel, Arch. Pharm. 1896, 234. 399.) Potassium plumbate, K 2 PbO 3 +3H 2 O. Very deliquescent. Decomp. by pure H 2 O into PbO 2 and KOH. Sol. in KOH + Aq with- out decomp. (Fremy, J. Pharm. (3) 3. 32.) Silver metoplumbate, Ag 2 PbO 3 . Ppt. (Griitzner, Arch. Pharm. 1895, 233. 518.) Sodium plumbate. Sol. in H 2 O with decomposition. SI. sol. in alkalies +Aq. (Fremy, A. ch. (3) 12. 490.) Sodium metaplumbate, Na 2 PbO 3 +4H 2 O. Decomp. by H 2 O; insol. in alcohol. (Hoeh- nel, Arch. Pharm. 1894, 232. 224.) Strontium plumbate, Sr 2 PbO 4 . Properties as Ba 2 PbO 4 . (Kassner, Arch. Pharm. 228. 109.) Zinc wetoplumbate, ZnPbO 3 +2H 2 O. Decomp. by dil. acids; insol. in H 2 O. (Hoehnel, Arch. Pharm. 1896, 234. 398.) Plumb ous acid. Calcium plumbite. SI. sol. in H 2 O. (Karsten, Scher. J. 5. 575.) Potassium plumbite, PbO, zK 2 O. Known only in solution. Silver plumbite, Ag 2 PbO 2 . Insol, in H 2 0, NH 4 OH+Aq and KOH+ Aq; sol. in HNX) 3 and acetic acid; and in cone. H 2 SO 4 , HI, and HF. (Bullnheimer, B. 1898, 31. 1288.) +2H 2 O. Insol. in H 2 O. Decomp. on air. (Kratwig, B. 15. 264.) Sodium plumbite. Known only in solution. Potassium, K 2 . Violently decomposes H 2 O or alcohol. Insol. in hydrocarbons. Sol. with violent action in acids. Solubility in fused KOH at t. t G. K sol. in 100 g. fused KOH 480 600 650 700 7.8-8.9 3 -4 2 -2.7 0.5-1.3 (Hevesy, Z. Elektmchem. 1909, 15. 534.) Sol. in liquid NH 3 . (Seely, C. N. 23. 169); (Franklin, Am. Ch. J. 1898, 20. 829.) 1 gram atom of K dissolves in 4.74 mol. POTASSIUM ARSENIDE, AMMONIA 743 liquid NH 3 at 0; in 4.79 mol. at 50; in 4.82 mol. at 100. (Ruff, B. 1906, 39. 839.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Slowly sol in ethylene diamine. Insol. in ethyl amine and in secondary and tertiary amines. (Kraus, J. Am. Chem. Soc. 1907, 29. 1561.) Potassium acetylide, K 2 C 2 . (Moissan, C. R. 1898, 127. 917.) Potassium acetylide acetylene, K 2 C 2 , C 2 H 2 . (Moissan, C. R. 1898, 127. 915.) Potassium amalgams. Hg 4 K, Hg 5 K, HgK, Hg 10 K, Hg 12 K and Hg ]8 K. (Guntz, C. R. 1900, 131. 183.) Hgi 4 K. Stable up to 0. Can be cryst. from Hg without decomp. below 0. Hg 12 K. Stable from to 71 or 73. Can be cryst. from Hg without decomp. at any temp, between these limits. Hg 10 K. Stable from 71 or 73-75. Can be cryst. from Hg without decomp. at any temp, between these limits. (Kerp, Z. anorg. 1900, 25. 68.) Potassium amide, KH 2 N. Decomp. by water or alcohol. Insol. in hydrocarbons. Potassium ammonickelate, Ni 2 N 3 K 5 , 6NH 3 . Decomp. by H 2 O. SI. sol. in liquid NH 3 . (Bohart, J. phys. Chem. 1915, 19. 559.) Potassium ammonoargentate, AgNHK, NH 3 or AgNH 2 , KNH 2 . Ppt., decomp. in the air. Decomp. by H 2 O or by liquid NH 3 solutions of acids. (Frank- lin, J. Am. Chem. Soc. 1915, 37. 855.) Potassium ammonobarate, BaNK, 2NH 3 . Hydrolyzed by H 2 O. Insol. in liquid NH 3 . Decomp. and dissolved in a solution of NH 4 NO 3 in liquid NH 3 . (Franklin, J. Am. Chem. Soc. 1915, 37. 2297.) Potassium ammonocadmiate, Cd(NHK) 2 , 2NH 3 . Ppt. (Franklin, Am. Ch. J. 1912, 47. 310.) Cd(NHK) 2 , 2NH 3 . Decomp. by H 2 O. Insol. in liquid NH 3 . (Bohart, J. phys. Chem. 1915, 19. 542.) Potassium ammonocalciate, CaNK, 2NH 3 . Hydrolyzed by H 2 O. Readily sol. in a solution of NH 4 NO 3 in liquid NH 3 . (Frank- lin, J. Am. Chem. Soc. 1915, 37. 2300.) Potassium ammonocuprite, CuNK 2 , 3NH 3 . Very sol. in liquid NH 3 . CuNK 2 , 2NH 3 . CuNK 2 , NH 3 . (Franklin, J. Am. Chem. Soc. 1912, 34. 1503.) CuNK 2 , 2>iNH 3 , Ppt. (Franklin, Am. Ch. J. 1912, 47. 311.) Potassium ammonomagnesate, Mg(NHK) 2 . 2NH 3 . SI. sol. in liquid NH 3 . Rapidly hydrolyzed by H 2 O. (Franklin, J. Am. Chem. Soc. 1913, 35. 1463.) Potassium ammonoplumbite, PbNK, Completely hydrolyzed by action of water vapor. Violently decomp. by H 2 O or dil. acids. Sol. in liquid NH 3 . (Franklin, J. phys. Chem. 1911, 15. 519.) Potassium ammonostannate, Sn(NK) 2 , 4NH 8 . Decomp. by H 2 O. Readily sol. in HC1+ Aq. SI. sol. in liquid NH 3 . Readily sol. in a solution of NH 4 I in liquid NH 3 . (Fitzgerald, J. Am. Chem. Soc. 1907, 29. 1696.) Potassium ammonostrontiate, SrNK, 2NH 3 . Hydrolyzed vigorously by H 2 O. Sol. in solutions of NH 4 NO 3 in liquid NH 3 . Insol. in liquid NH 3 . (Franklin, J. Am. Chem. Soc. 1915, 37. 2299.) Potassium ammonotballate, T1NK 2 , 4NH 3 . Sensitive to action of air or moisture. Vio- lently decomp. by H 2 O or dil. acids. Mod- erately sol. in liquid NH 3 at 20, more sol. at higher temp, and much less sol. at lower temp. Decomp. by liquid NH 3 solutions of acids. (Franklin, J. phys. Chem. 1912, 16. 689.) Potassium ammonotitanate, (N) TiNHK. Vigorously hydrolyzed by H 2 O. Insol. in liquid NH 3 solutions of either potassium amide or NH 4 Br. (Franklin, J. Am. Chem. Soc. 1912, 34. 1500.) Potassium ammonozincate, Zn(NHK) 2 , 2NH 8 . Decomp. by water. SI. sol. in liquid NH 8 . (Fitzgerald, J. Am. Chem. Soc. 1907, 29. 663.) Decomp. by H 2 O. Sol. in dilute acids. SI. sol, in liquid NH 8 . Sol. in solutions of ammonium salts in liquid NH. (Franklin, Z. anorg. 1907, 55. 195.) Potassium arsenide, K 3 As. (Hugot, C. R. 1899, 129. 604.) K 2 As 4 . (Hugot.) Potassium arsenide, ammonia, AsK 3 , NH 8 . Nearly insol. in liquid NH 3 . (Hugot.) K 2 As 4 , NH 3 . (Hugot.) 744 POTASSIUM AZOIMIDE Potassium azoimide, K Stable in aq. solutioi 46.5 pts. are sol. in at. i. 100 pts. H 2 O at 10.5. 100 " H 2 O " 15.5. 100 " H 2 O " 17. 100 " abs. alcohol at (Curtius, J. pr. 1898, Br. L 100 pts. H 2 O at t. 41.5+0.1378t from 30 to 120. (fifcard. C. R. 98. 1432.) Solubility of KBr in 100 g. H 2 O at t. 48.9 " " " " 49.6 " " " " 0.1375 " " " " 16. Insol. in pure ether. (2) 68. 280.) Potassium bromide, K Solubility of KBr ic t G. KBr. t G. KBr. 10.5 10 3.5 -5 -8 UK 62.1 60.7 55.5 52.6 50.1 47.5 45.3 -11 -10.5 -10 - 8.5 - 8 - 6.5 44.9 41.8 39.7 35.7 31.2 25.0 t Pts. KBr t Pts. KBr (Meusser, Z. anorg. 1905, 44. 80.) 68.74 g. KBr are sol. in 100 g. H 2 O at 25. (Amadori and Pampanini, Rend. Ac. Line. 1911, V, 20. 473.) Sp. gr. of KBr+Aq at 19. 20 40 53.48 64.52 74.63 60 80 100 85.35 93.46 102.0 (Kremers, Pogg. 97. 151.) Solubility of KBr in 100 pts. H 2 O at t. t Pts. KBr t Pts. KBr %KBr Sp. gr. %KBr Sp. gr. 13.4 6.2 +3.4 5.2 12.65 13.0 13.3 18.3 26.05 30.0 37.9 46.17 49.57 53.32 55.60 56.63 61.03 61.17 61.45 64.11 68.31 70.35 74.46 43.15 45.45 50.5 54.8 60.15 66.75 71.45 74.85 86.5 97.9 110.0 77.0 77.73 80.33 82.78 85.37 88.22 90.69 92.25 97.28 102.9 110.3 5 10 15 20 25 1.037 1.075 1.116 1.159 1.207 30 35 40 45 1.256 1.309 1.366 1.432 (Gerlach, Z. anal. 8. 285.) Sp. gr. of KBr+Aq at 15 containing: 5 10 20 30 36% KBr. 1.0357 1.074 1.1583 1.2553 1.3198 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr of KBr+Aq at t. Solubility is represented by a straight line of the formula 54.43 +0.5128t. (Coppet, A. ch. (5) 30. 416.) 100 pts. KBr+Aq sat. at 15-16 contain 39.06 pts. KBr. (v. Hauer, J. pr. 98. 137.) Solubility of KBr in 100 pts. H 2 O at high temp. G. KBr dis- solved in 100 g H 2 O G. KBr in 100 g. of the t solution Sp. gr. 4.166 11.111 25.000 42.867 4 10 20 30 14.5 15.7 16.5 16.0 ] . 0291 1 . 0753 1.1625 1.2580 t Pts. KBr 140 181 120.9 145.6 (de Lannoy, Z. phys. Ch. 1895, 18. 460.) (Tilden and Shenstone, Phil. Trans. 1884. 23.) Sat. solution boils at 112. (Kremers.) Sat. KBr+Aq contains at: 12 10 +3 32 39 31.0 31.5 35.7 41.6 47.7% KBr, 55 77 140 173 220 45.5 48.7 54.1 58.5 61.6% KBr. (fitard, A. ch. 1894, (7) 2. 539.) If solubility S = pts. KBr in ICO pts. solu- tion, S = 34.5+0.2420t from to 40, S = gr. 20/20 = 1.0521. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) Sp. gr. of KBr+Aq at 20.5. Normality of KBr+Aq. G. KBr inlOO g. of solution Sp. gr. t/4 4.29 3.01 2.00 1.00 37.97 28.83 20.49 11.03 1.3449 1.2407 1.1629 1.0815 (Oppenheimer, Z. phys. Ch. 1898, 27. 452.) POTASSIUM BROMIDE 745 Solubility of KBr+NH 4 Br at 25. Solubility of KBr+KCl in H 2 O at t. % KBr % NH 4 Br Sp. gr t Sat. solution contains 55.81 55.42 53.65 51.68 44.12 34.73 26.23 26.03 23.22 22.23 17.99 0.0 0. 0. 2. 5. 15. 26. 34. 38. 41. 43. 48. 57. 64 46 13 29 22 76 14 78 25 08 73 1.3756 1.3745 1.3733 1.3721 1.3711 1.3715 1.3753 1.3753 1.3766 1.3777 1.3766 1.3763 % KC1 % KBr % total salt -14 -13.7 -13.5 -7 +5.2 +6 10 21 26 30 32 39 47 52 55 71 73 102 152 160 168 225 10.7 l6! 7 ii!3 11.0 10.8 11.2 ii!6 ii!6 11.0 11.9 12.0 11.8 12.8 13.2 12.5 li!7 18.8 19^8 22^6 23.7 25.5 26\6 30"8 31.2 29.9 31.7 32.9 35.8 40.6 42.3 45^6 29.5 29.4 29.5 30.5 34.4 33.9 34.7 35.3 36.7 39.4 38.5 39.8 41.8 42.2 41.8 43.7 44.7 48.6 53.8 54.8 55.0 59.7 (Fock, Z. Kryst. Min. 1897, 28. 357.) Solubility in KNO 3 +Aq. 1 litre of the solution contains at 14.5 at 25.2 Mol. KN0 3 Mol. KBr Mol. KNO 3 Mol. KBr 0.0 0.362 0.706 1.235 4.332 4.156 4.093 3.939 0.0 0.131 0.527 0.721 1.090 1.170 1.504 4.761 4.72 4.61 4.54 4.475 4.44 4.375 (fitard, A. eh. 1894, (7) 3. 281.) Solubility of KBr+KCl in H 2 O at 25. G. per 100 g. H 2 O. KBr KCl 68.47 62.26 58.50 52.45 45.42 38.70 26.62 12.94 0.0 0.0 5.43 8.46 12.48 17.17 21.23 25.88 31.02 36.12 (Touren, C. R. 1900, 130. 911.) See also under KNO 3 . 100 pts. KBr+KCl+Aq sat. at 15-16 con- tain 37.55 pts. of the two salts; 10.0 pts. KBr+KI+Aq sat. at 15-16 contain 57.96 pts. of the two salts; 100 pts. KBr+KCl + KI+Aq sat. at 15-16 contain 57.88 pts. of the three salts, (v. Hauer, J. pr. 98. 137. (Amadori and Pampanini, Att. Ace. Line. 1911, 20, II. 475.) Solubility in KCl+Aq at 25.2. ooaiDUity 01 j\.Br-r-iY 32.66 34.32 25.7 29.25 38.0 41.45 46.15 48.8 55.1 60.55 36.10 37.31 39.71 40.67 42.34 42.86 44.51 45.90 64.95 71.65 74.25 80.75 86.6 91.4 47.17 48.76 49.27 51.24 52.53 53.49 +3.9 9.4 11.4 14. & 19.0 t g- KCl t g. KCl + 18.5 11.5 10 7.5 2.5 -1 33.3 31.2 30.8 29.8 28.4 27.5 27.2 -4.5 -9 -8.5 -8 7'i 25.9 23.9 21.5 20.0 17.5 15.7 14.3 (Coppet, A. ch. (5) 30. 414.) Solubility is reoresented bv a straight line. -6 -5.5 (Coppet.) 100 pts. H 2 O dissolve 29.33 pts. KCl at 4, 45.5 pts. at 60. (Andreae, J. pr. (2) 29. 456.) 100 pts. H 2 O dissolve at: 100 130 180 29.2 56.5 66 78 pts. KCl. (Tilden and Shenstone, Lond, R. Soc. Proc. 35. 345.) Solubility of KCl in 100 pts. H 2 O at high temp. t Pts. KCl t Pts. KCl t Pts. KCl 125 133 59.6 69.3 147 175 70.8 75.2 180 77.5 (Tilden and Shenstone, Phil. Trans. 1884. 23.) (Meusser, Z. anorg. 1905, 44. 80.) Sat. KCl+Aq at 25 contains 26.46% KCl. (Foote, Am. Ch. J. 1906, 35. 238.) 28.01 g. KCl are contained in 100 g. solu- tion sat. at 30. (de Waal, Dissert. 1910.) 36.12 g. KCl are sol. in 100 g. H 2 O at 25. (Amadori and Pampanini, Rend. Ace. Line. 1911, V. 20. 473.) 4.272 g. mol. are contained in 1 1. solution sat. at 25. (Herz. Z. anorg. 1911, 73. 274.) Solubility of KBr at 6 = 23.06%; 28.4 = 26.91%; 62.6 = 31.57. (Sites, Z. Krist. 1912, 61. 262.) Solubility at 22 = 25.68%. (Bronstedt, Z. phys. Ch. 1912, 80. 208.) 100 mol. H 2 O dissolve at: 19.3 29.7 40.1 54.5 8.2 8.99 9.75 10.39 mol. KCl. (Sudhaus, Miner. Jahrb. Beil.-Bd. 1914, 37. 18.) 750 POTASSIUM CHLORIDE KCl+Aq sat. at 16 has sp. gr. = 1.077. (Stolba, J. pr. 97. 503.) Sp. gr. of KCl+Aq at 17.5. A Sp. gr. o/ KCl Sp. gr. KCl Sp. gr. i 2 3 4 5 6 7 . 8 1.0062 1.0125 1.0189 1.0254 1.0319 1.0385 1.0451 1.0518 9 10 11 12 13 14 15 16 1.0586 .0655 .0725 .0795 .0866 .0937 .1008 .1080 17 18 19 20 21 22 23 24 .1152 . 1225 .1298 .1372 .1446 .1521 .1596 .1673 (Schiff, A. 110. 76.) Sp. gr. of KCl+Aq at 19. 5. % KCl Sp. gr. % KCl Sp. gr. 5.98 11.27 16.27 1.0382 21.31 1.0733 25.133 1 . 1075 1.1436 1 . 1720 (Kremers, Pogg. 95/119. Sp. gr. of KCl+Aq at 15 o I Sp. gr. K%1 Sp. gr. at KCl Sp. gr. 1 2 3 4 5 6 7 8 9 1.00650 1.01300 1.01950 1.02600 1.03250 1.03916 1.04582 1.05248 1.05914 10 11 12 13 14 15 16 17 18 1.06580 1.07271 1.07962 1.08654 1.09345 1 . 10036 1 . 10750 1.11465 1.12179 19 20 21 22 23 24 24.9* 1.12894 1.13608 ,14348 . 15088 . 15828 . 16568 .17234 Sp. gr. of KCl+Aq at 0. S= pts. salt in 100 pts. of solution; Si = mols. salt in 100 mols. solution. s Si Sp. gr. 20.7840 17.7214 14.4707 11.0757 7.5440 4.4968 5.954 4.940 3.922 2.918 1.931 1.123 1.1489 1 . 1258 1.1018 1.0769 1.0521 1.0308 (Charpy, A. ch. (6) 29. 23.) Sp. gr. of KCl+Aq at 25. Concentration of KCl+Aq Sp. gr. 1-normal Vr- " V 4 - " Vs- " :* 1.0466 1 . 0235 1.0117 1 . 0059 (Wagner, Z. phys. Ch. 1890, 5. 36.) KCl+Aq containing 5.05% KCl has sp. gr. 20/20 = 1.0327. KCl+Aq containing 20.55% KCl has sp. gr. 20/20 = 1.1393. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 272.) Sp. gr. of KCl+Aq. g. KCl in 1000 g. of solution Sp. gr. 16/16 0.7140 1.5042 3.0724 8.3165 1.000000 1.000464 1 . 000975 1.001991 1.005391 * Mother liquor. (Gerlach, Z. anal. 8. 281.) Sp. gr. of KCl+Aq at 20, containing mols. KCl to 100 mols. H 2 O. (Dijken, Z. phys. Ch. 1897, 24. 109.) Sp. gr. of KCl+Aq at 20.1, when p=per cent strength of solution; d= observed density, and w= volume cone, in g. per Mols. KCl Sp. gr. Mols. KCl Sp. gr. 0.5 1.0 2.0 1.01310 1.02568 1.04959 4.0 5.0 1.09415 1.11445 (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of KCl+Aq at 18. A IvUl Sp. gr. A .Kd Spigr. % JvUl Sp. gr. 5 10 1.0308 1.0638 15 20 1.0978 1.1335 25 1.1408 (Kohlrausch, W. Ann. 1879. 1.) cc - (m)= w p d w 36.43 1.853 0.43171 31.12 .1554 0.35954 24.79 .1215 0.27887 18.06 .0866 0.19610 13.17 ,QB1Z 8.412 .0386 ~~ o! 08736 6.610 .0297 0.06806 4.419 1.0193 0.4505 3.456 1.0148 0.03507 1.197 1.0040 0.01202 . (Barnes, J. phys. Ch. 1898, 2. 544.) POTASSIUM CHLORIDE 751 Sp. gr. of KCl+Aq at t. KCl+Aq containing 10% KCl boils at 101.1; containing 20%, at 103.4. (Gerlach.) Sat. KCl+Aq containing 52.7 pts. KCl to 100 pts. H 2 O forms a crust at 107.7; highest temp, observed, 108.5. (Gerlach, Z. anal. 26. 426.) B.-pt. of KCl+Aq containing pts. KCl to 100 pts. H 2 O. G= according to Gerlach (Z. anal. 26. 438); L= according to Legrand (A. ch. (2) 59. 426). t Normality of KCl+Aq. g. KCl in 100 g. of solution Sp. gr. t/4 20.5 it it <( 3.74 2.65 1.87 0.93 23.93 17.66 12.82 6.64 1.1617 1.1166 1.0829 1.0424 (Oppenheimer, Z. phys. Ch. 1898, 27. 450.) Sp. gr. of KCl+Aq at 18/4. B.-pt. G L B.-pt. G L 100.5 101.0 101.5 102 102.5 103 103.5 104 104.5 4.9 9.2 13.1 16.7 20.1 23.4 26.7 29.9 33.1 4.7 9.0 13.2 17.1 20.9 24.5 28.0 31.4 34.6 105 105.5 106 106.5 107 107.5 108 108.3 108.5 36.2 39.3 42.4 45.5 48.4 51.5 54.5 57.'4 37.8 41.0 44.2 47.4 50.5 53.7 56.9 59.4 g. KCl in 100 g. of solution Sp. gr. 0.24963 0.12459 0.08342 0.062343 1.0003 0.9995 0.99929 0.99912 (Jahn, Z. phys. Ch. 1900, 33. 559.) KCl+Aq containing 1 pt. KCl in 58.923 pts. H 2 O at 17 has sp. gr. = ] .0096. (Hittorf, Z. phys. Ch. 1902, 39. 628.) Sp. gr. 20/4 of a normal solution of KCl = 1.04443. (Haigh, J. Am. Chem. Soc. 1912, 34. 1151.) Precipitated from aqueous solution by HC1 +Aq. Much less sol. in very dil. HCl+Aq than in H 2 O. (Fresenius.) Nearly insol. in cone. HCl+Aq. 100 cc. sat. HCl+Aq dissolve 1.9 g. KCl at 17. (Ditte, A. ch. 1881, (5) 24. 226.) Sp. gr. of sat. KCl+Aq at t. G. per 100 cc. of solution t g. KCl 100 g. sol. in H 2 Sp. gr. HC1 KCl 10 10 20 30 40 50 60 70 24.98 28.50 31.23 34.11 37.28 40.12 42.86 45.48 48.30 1.139 1.156 1.168 1.177 1.183 1.190 1.195 1.199 1.203 0.0 1.42 2.41 2.59 4.05 8.39 12.40 14.95 23.88 54.20 25.73 22.69 20.84 20.51 17.71 11.93 7.46 5.60 1.49 1.52 (Tschernaj, J. Russ. phys. Chem. Soc. 1912, 44. 1565.) Sp. gr. of dil. KCl+Aq at 20.004. Conc.= g. equiv. KCl per 1. at 20.004. Sp. gr. compared with H 2 O at 20. 004= 1. (Engel, A. ch. 1888, (6) 33. 377.) Solubility of KCl in HCl+Aq. t Concentra- tion of HC1 g. mol. per 1000 g. H 2 O Wt. KCl per 1000 g. H 2 Mol. solubility Cone. Sp. gr. u ft ti Q \ 283.55 267.25 250.00 214.25 3,81 3.59 3.36 2.88 0.0000 0.0001 0.0002 0.0005 -0.0010 0.0026 0.0050 0.0100 1.000,000,0 1.000,004,8 1.000,009,7 1.000,024,2 1.000,048,5 1.000,097,1 1.000,242,6 1.000,483,6 25 n ti it 1 A Y* l 359.25 341.55 324.30 289.60 4.82 4.59 4.35 3.89 (Lamb and Lee, J. Am. Chem. Soc., 1913, 36. 1687.) (Armstrong and Eyre, Proc. R. Soc. 1910 (A) 84. 127.) 752 POTASSIUM CHLORIDE 100 g. sat. HCl+Aq dissolve 1.9 g. KG at 20. (Stoltzenberg, B. 1912, 46. 2248.) Solubility in HCl+Aq at 25. Millimols HC1 in 10 ccm. Millimols KC1 in 10 ccm. 5.66 10.20 15.90 20.94 32.52 42.72 37.49 33.79 28.68 24.74 17.39 Solubility of KC1 in MgCl 2 +Aq of given per- centage composition. 10 20 30 40 50 60 70 80 90 100 30% 1.9% 2.6 3.4 4.2 5.0 5.8 6.5 7.3 8.1 8.9 21.2% 5.3% 6.5 7.6 8.8 10.0 11.2 12.4 13.6 14.7 15.9 15% 9.9% 11.3 12.7 14.2 15.6 17.0 18.3 19.5 20.8 22.1 14.3% 15.9 17.5 19.0 20.5 21.9 23.2 24.5 25.8 27.1 (Herz, Z. anorg. 1912, 73. 275.) Solubility of KC1 in HBr+Aq at 25. Millimols HBr in 10 ccm. Millimols KC1 in 10 ccm 6.61 34.15 42.72 37.80 19.57 (Herz, Z. anorg. 1912, 73. 275.) Sol. in sat. NH 4 Cl+Aq with pptn. of NH 4 C1. When action has ceased, the solu- tion at 18.75 contains 31.6% of the mixed salt: or 100 pts. H 2 O dissolve 46.1 pts. of the mixed salt, viz, 16.27 pts. KC1 and 29.83 pts. NH 4 C1. (Karsten.) Solubility of KC1 in NH 4 Cl+Aq at 25. Dissolved in 1000 mols H 2 O. Mols KC1 Mols NH 4 C1 74.2 23.8 67.9 32.5 61.4 52.2 55.5 65.9 50.2 74.4 43.0 96.3 37.6 110.0 37.0 107.5 37.5 109.4 22.6 118.2 (Biltz, Z. anorg. 1911, 71. 174.) See also NH 4 C1. Sol. in sat. BaCl 2 +Aq with pptn. of BaCl 2 until a state of equilibrium is reached, when 100 pts. H 2 O at 16.8 dissolve 45.9 pts. mixed salts, viz. 18.2 pts. BaCl 2 and 27.7 pts. KCl. See also BaCl 2 . (Precht and Wittgen, B. 14. 1667.) Solubility of KCl+NaCl in 20% MgCl 2 +Aq. 10 20 30 40 50 %KC1 4.2 5.1 6.0 6.9 7.9 5.7 5.8 5.9 6.0 6.1 60 70 80 90 100 % KCl 8.9 9.9 10.9 11.9 13.0 6.3 6.4 6.6 6.7 6.9 (P. and W.) Sol. in sat. KNO 3 +Aq with pptn. of KNO 3 . 1 litre of the solution contains at 14.5 C Mol. KC1 Mol. KNOj 3.865 3.S10 3.782 3.710 3.667 3.629 3.597 3.582 0.0 0.204 0.318 0.615 0.818 0.910 1.176 1.220 at 25.2 Mol. KC1 Mol. KN0 8 18 11 07 93 85 81 3.70 0.0 0.136 0.318 0.902 1.212 1.397 1.805 (Touren, C. R. 1900, 130. 909.) Solubility of KC1 in KNO 3 +Aq. 25 Concentra- tion of KNO 3 in g. mol. per 1000 g. H 2 o I Wt. KCl in 1000 g. H 2 O 283.55 284.25 283.60 287.60 364.15 355.00 361.65 358.80 355.20 Mol. solubility 3.81 3.81 3.81 3.86 4.89 4.90 4.86 4.81 4.77 Armstrong and Eyre, Proc. R. Soc. 1910 [A], 84. 127.) See also KNO 3 . POTASSIUM CHLORIDE 753 Sol. in sat. NaNO 3 -f Aq without causing pptn. (See NaNO 3 .) Sol. in sat. Ba(NO 3 ) 2 +Aq without causing pptn. Solubility in KBr+Aq at 25.2. Solubility of KC1 in KOH+Aq at 0. G. per 100 cc. solution KC1 KOH 1 litre of the solution contains 26.83 23.44 21.39 17.39 13.89 10.91 8.64 6.78 4.74 0.0 1.33 2.64 5.56 8.46 11.23 13.83 16.43 19.72 Mol. KBr Mol. KC1 0.0 0.49 0.85 1.31 1.78 2.25 2.69 4.18 3.85 3.58 3.19 2.91 2.58 2.33 (Engel, Bull. Soc. 1891, (3) 6. 16.) (Touren, C. R. 1900, 130. 1252.) See also KBr. 100 pts. H 2 O dissolve 133.2 pts. KI and 10.4 pts. KC1 at 21.5, no matter how pre- pared. (Rtidorff, B. 6. 484.) 100 pts. KCl+Aq sat. at 15-16 contain 25.26-25.37 pts. KC1. 100 pts. KCl+Ki + Aq sat. at 15-16 contain 57.80 pts. of the two salts. KC1 is pptd. by KI. (v. Hauer. J. pr. 98. 137.) Solubility in KI+Aq at t. t Sat. solution contains %KC1 % KI % total salt 4.8 50.8 56.6 8 5.1 51.1 56.2 18 57.9 30 4^2 54^6 58.8 41 4.7 55.0 59.7 49 5.7 56.0 61.7 60 62.5 75 4.4 59^5 63.9 82 5.0 59.6 64.6 96 . 66.2 102 . . . 66.8 140 63^3 155 '7.'6 64.8 7214 182 8.7 65.4 74.1 190 8.6 66.0 74.6 245 10.0 66.5 76.$ (fitard, A. ch. 1894, (7) 3. 281.) Solubility of KCl+KI in H 2 at 25. G. per 100 g. H 2 O KC1 KI KCl KI 4.06 7.63 11.36 11.74 15.10 149.26 144.03 137.79 132.60 133.90 105.91 19.64 23.75 29.56 31.38 33.68 36.12 68.22 43.89 23.83 14.83 7.00 0.00 (Amadori and Pampanini, Att. Ace. Line. 1911, 20, II. 475.) Solubility in KOH+Aq at 20, G. KOH in 1 litre G. KC1 in 1 litre Sp. gr. Degrees Baum6 10 293 .185 22.5 20 285 .185 22.5 30 276 .190 23.0 40 265 .192 23.0 50 255 .195 23.5 60 245 .200 24.0 70 236 .200 24.0 80 226 .205 24.5 90 219 1.205 24.5 100 211 1.210 25.0 110 205 1.210 25.0 120 199 1.215 25.5 130 192 1.215 25.5 140 185 1.220 26.0 150 178 1.225 26.5 160 171 1.225 26.5 170 165 1.230 27.0 180 159 1.235 27.5 190 153 1.240 28.0 200 148 1.245 28.5 210 142 1.250 29.0 220 137 1.255 29.5 230 133 1.260 30.0 240 128 1.265 30.5 250 124 1.270 30.8 260 120 1.275 31.3 270 115 1.280 31.7 280 112 1.285 32.0 290 108 1.290 32.5 300 104 1.295 33.0 310 ioo 1.300 33.5 320 96 1.305 34.0 330 93 1.310 34.2 340 89 1.315 34.6 350 85 1.320 35.0 360 81 1.325 35.5 370 78 1.330 36.0 380 74 1.335 36.3 390 71 1.340 36.7 400 68 1.345 37.1 410 64 1.350 37.5 754 POTASSIUM CHLORIDE Solubility in KOH+Aq at 20. -Continued. Solubility of KCl+NaCl in H 2 O at t. 100 pts. H 2 O dissolve pts. KCl and pts. NaCl. G. KOH in 1 litre G. KCl in 1 litre Sp. gr. Degrees Baum6 Pts. KCl Pts. NaCl Pts. KCl Pts. NaCl 420 430 440 450 460 470 61 58 55 53 50 47 :355 .360 .365 .370 .375 .380 38.0 38.5 38.9 39.2 39.5 40.0 TO 12.5 20 14.7 30 17.2 40 19.5 50 22.0 29.7 29.2 28.7 28.2 27.7 60 24.6 70 27.3 80 30.0 90 32.9 100 34.7 27.2 26.8 26.4 26.1 25.8 480 490 44 42 .385 .390 40.2 40.6 (Precht and Wittgen, B. 14. 1667.) 500 510 520 530 40 38 35 33 .397 .405 .410 .415 41.0 41.5 42.0 42.3 100 pts. H 2 O dissolve 13.99 pts. KC1+30.54 pts. NaCl = 44.53 pts. mixed salts at 20. (Nicol, Phil. Mag. (5) 31. 385.) 540 31 .420 42.6 550 KftfV 29 97 .425 1 4.^0 43.0 /iq K Solubility of KCl in NaCl+Aq at 20. 570 25 1.435 43.7 G. per 100 g. H 2 O 580 24 1.440 44.0 NaCl KCl 590 23 1 445 44 3 600 22 1.450 44.6 0.0 34.52 610 21 1.455 45.0 6.5 29.37 620 20 1.460 45.5 13.0 4.71 630 18 1.465 45.9 19.5 0.42 640 17 470 46 2 650 16 .475 46.5 (Nicol, Phil. Mag. 1891, 31. 369 .) 660 15 .480 46.8 670 680 15 15 .485 .490 47.0 47.5 Solubility of KCl+NaCl at t. 690 15 .495 47.9 G. per 100 g. H 2 O 7OO 14. KAA AQ 9 710 14 .505 48.5 KCl NaCl 720 730 13 13 .510 .515 48.8 49.1 25 15.8 14 .5 740 13 .520 49.5 1C 29.0 31 .3 750 13 .525 49.7 80 30.0 25 .2 760 12 .530 50.0 n 26.4 34 .0 770 780 12 12 .535 .540 50.3 50.6 (Soch, J. phys. Ch. 1898, 2. 46. ) 790 11 .545 51 800 11 .550 51.3 Solubility of KCl+NaCl at ? 810 820 10 10 .560 .565 51.5 51.8 G. salts in 100 g. H 2 O 830 9 1.570 52.2 NaCl KCl Solid phase 840 1 .7^ co a 850 9 1.580 53.0 9.89 28.34 KCl 1 R ^P 22 75 " (Winteler, Z. Elektrochem, 1900, 7. 360.) 29.88 31.57 16.28 KCl+NaCl 10.91 NaCl 33.17 5.65 KCl+NaCl. 100 pts. KCl+NaCl+Aq sat. at 13-16 contain 30.18 pts. of the two salts, (v. Hauer.) 100 pts. H 2 O dissolve 13.92 pts. KCl and 30.65 pts. NaCl at 15.6, and solution has sp. gr. = 1.233. (Page and Keightley.) 100 pts. H 2 O dissolve 10.11 pts. KCl, 32.15 Ets. NaCl, and 4.69 pts. K 2 SO 4 , and solution as sp. gr. = 1.250. (P. and K.) 100 pts. H 2 O dissolve 29.9 pts. NaCl and 15,7 -pts.-KCl at 18.8. (Riidorff.)- (Uyeda, Mem. Col. Sc. Kioto, 1910, 2. 245.) 100 g, H 2 O sat. .with NaCl dissolve 0.216 gram-equivalent KCl at 25. * 100 g H 2 O sat. with K 2 SO 4 dissolve 0.466 gram-equivalent KCl at 25. (Euler, Z. phys. Ch. 1904, 49. 315.) Solubility in NaCl+Aq at 20, 30, 40 and 91. Tables given in the original show that each salt diminishes the solubility of the other. (Leather, Chem. Soc. 1915, 108. (2) 13.) POTASSIUM CHLORIDE 755 Solubility of KCl+NaCl in HCl+Aq at 25. %HC1 %NaCl %KC1 8.61 17.16 20.65 32.78 19.95 10.65 3.56 2.03 0.18 10.90 7.58 3.80 2.86 1.27 (Hicks, J. Am. Chem. Soc. 1915, 37. 846.) See also under NaCl. KCl+SrCl 2 . 100 pts. H 2 O dissolve 11.2 pts. KC1 and 48.6 pts. SrCl 2 at 14.5. (v. Hauer.) If SrCl 2 +Aq. sat. at 14.5 is sat. with KC1 at same temp., 100 pts. H 2 O dissolve: KC1 . . . SrCl 2 . . . 33.2 11.2 48.6 50!7 59.8 (Mulder, Scheik. Verhandel. 1864.) KC1+(NH 4 ) 2 SO 4 . Sat. solution of KC1 + (NH 4 ) 2 SO 4 at b.-pt. when cooled to 14 has different composition from sat. solution of (NH 4 )C1 and K 2 SO 4 , and its composition is changed by warming it with either KC1 or (NH 4 ) 2 SO 4 . (Riidorff.) KC1+K 2 SO 4 . 100 pts. H 2 O contain the following amounts salt at 18.75: (1) sat. with KC1 alone; (2) sat. first with KC1 then with K 2 SO,; (3) sat. with K 2 SO 4 and KC1 together; (4) sat. first with K 2 SO 4 then with KC1; (5) sat. with K 2 SO 4 alone. KC1 . K 2 S0 4 . i 2 3 4 5 34.5 32.96 1.79 33.12 1.75 33.12 1.83 iols (Karsten.) 100 pts. H 2 O sat. with both K 2 S0 4 and KC1 contain the following amounts. KC1 K 2 S0 4 . . . At 14.8 33.5 28.2. 2.0 1613 KC1 K 2 S0 4 . . . At 15.8 33.6 27.9 2.3 16!4 KC1 K 2 S0 4 . . . At 16.1 33.6 27.1 3.3 16! 4 (Kopp, A. 34. 264.) Sat. K 2 SO 4 +Aq dissolves KC1 only with pptn. of K 2 SO 4 , but sat. KCl+Aq dissolves some K 2 SO 4 without any separation. (Kar- sten.) Solubility of KC1+K 2 SO 4 : 100 pts. H 2 O dissolve at t. t Pts. KC1 Pts. K 2 S0 4 t Pts. KC1 Pts. K 2 S0 4 10 20 30 40 50 30.9 33.4 36.1 38.7 41.3 1.32 1.43 1.57 1.68 1.82 60 70 80 90 100 43.8 46.5 49.2 52.0 54.5 1.94 2.06 2.21 2.38 2.53 (Precht and Wittgen.) 100 g. H 2 O dissolve 34.76 g. KC1+2.93 g. K 2 SO 4 at 25. (Van't Hoff and Meyerhoffer, Z. phys. Ch. 1898, 27. 75.) Sol. in 20% KC 2 H 3 O 2 +Aq. (Stromeyer.) Quickly attacked by liquid NO 2 in the presence of traces of moisture, with evolution of C1 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Easily sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) 100 g. hydrazine dissolves 8.5 pts. KC1 at 12.5-13. (de Bruyn, R. t. c. 1899, 18. 297.) 100 g. anhyd. hydroxylamine dissolve 12.3 g. KC1 at 17-18. (de Bruyn, Z. phys. Ch. 1892, 10. 782.) 100 pts. alcohol of 0.900 sp. gr. dissolve 4.62 pts.; 0.872, 1.66 pts.; 0.834, 0.38 pt.; 0.817, 0.00 pt. KC1. (Kirwan.) Sol. in 48 pts. boliing alcohol. (Wenzel.) Insol. in absolute alcohol containing LiCl. (Mits- cherlich.) 15, 100 pts. alcohol of p percenta ae (S = sp. gr.) dissolve pts. K< At volume follows: 10 0.984 KC1 19.8 20 0.972 14.7 30 0.958 10.7 KC1 50 0.918 5.0 60 0.896 2.8 ;e by 1 as 40 0.940 7.7 80 0.848 0.45 (Schiff, A. 118. 365.) 100 pts. of a mixture of 40% alcohol with 60% H 2 O dissolve 9.2' pts. KC1 at 15. (Schiff.) Insol. in absolute alcohol or in 96% alcohol at 15 or below. At 20, 100 pts. of the latter dissolve 0.04 pt.; at 25, 0.06 pt.; at 30, 0.20 pt. KC1. Dilute alcohol dissolves less KC1 than the contained H 2 O would dissolve by itself. 756 POTASSIUM CHLORIDE Solubility in dil. alcohol. D = sp. gr. of alco- hol; S = solubility in 100 pts. alcohol at t. Solubility of KCl in ethyl alcohol at 0. Concentration of alcohol Mol. g. alcohol per 1000 g.H 2 Solubility in 1000 g. H 2 Molecular solubility D =0.9904 D =0.9848 D =0.9793 D =0.9726 t S t s t S t s 0^25 0.50 1.00 3.00 285.15 277.95 271.10 265.50 208.80 3.80 3.73 3.64 3.45 2.81 4 22 25 34 52 23.2 24.8 29.4 30.2 32.8 37.5 4 20 27 30 37 60 20.9 25.5 26.6 27.5 29.0 35.2 4 21 28 43 16.4 20.3 22.0 25.6 3 5 16 20 25 34 12.2 12.7 15.4 16.1 17.3 19.0 (Armstrong and Eyre, Proc. Rov. Soc. 1910. (A) 84. 127.) Solubility of KCl in ethyl alcohol +Aq at 25. D =0.9573 D =0.9390 D =0.8967 D =0.8244 t S t/ s t s t S 10 11 17 30 40 60 8.8 9.0 10.3 12.5 13.9 16.7 2 7 16 30 38 57 4.2 5.1 6.4 8.5 9.6 11.3 12 31 47 65 2.87 4.35 4.88 5.65 4 15 20 25 32 0.00 0.00 0.04 0.06 0.20 wt. % alcohol G. KCl per 100 cc. sat. solution wt. % ' alcohol G. KCl per 100 cc. sat. solution (Gerardin, A. ch. (4) 6. 140.) Solubility of KC1 in dil.' alcohol at 14.5 10 20 30 40 50 31.18 23.93 17.89 13.27 9.40 6.26 60 70 80 90 100 4.18 2.27 0.93 0.31 0.08 Sp. gr. 100 ccm. contain CMcIntosh, J. phys. Ch. 1903, 7. 350.) 100 pts. absolute methyl alcohol dissolve 0.5 pt. at 18.5; 100 pts. absolute ethyl al- cohol dissolve 0.034 pt. at 18.5. (de Bruyn, Z. phys. Ch. 10. 783.) 100 pts. 40% wood alcohol dissolve 9.2 pts. KCl. (Schiff.) Solubility of KCl in methyl alcohol+Aq at 25. Alcohol Water KCl 1.1720 1.1542 1.1365 1.1075 1.1085 1.0545 1.0455 0.9695 0.9315 0.8448 2^79 4.98 10.56 15.57 20.66 24.25 40.42 48.73 68.63 88.10 85.78 84.00 79.63 75.24 70.52 67.05 50.18 40.60 15.55 29.10 26.85 24.67 20.56 17.24 14.27 13.25 6.35 3.82 0.30 (Bodlander, Z. phys. Ch. 7. 316.) Solubility of KCl in ethyl alcohol. (G. KCl per 100 g. alcohol+Aq.) P = % by wt. of alcohol in alcohol+Aq. S =Sp. gr. alcohol+Aq sat. with KCl. L = millimols KCl in 100 ccm. of the solu- tion. wt. % alcohol at 30 at 40 wt. % alcohol at 30 at 40 38.9 41.8 43.1 11.1 13.1 5.28 33.9 35.9 55.9 6.8 8.2 9.43 30.2 33.3 65.9 3.6 4.1 16.9 24.9 27.6 78.1 1.3 1.6 25.1 19.2 21.8 86.2 0.4 0.5 34.1 15.6 17.2 (Bathrick, J. phys. Ch. 1896, 1. 160.) p S 25/4 L 10.6 30.8 47.1 64.0 78.1 98.9 100 1.1782 1.125 1.033 0.9679 0.9064 0.8607 0.8242 0.7937 417.4 329 183 102 46.1 20.6 9.9 5.7 (Herz and Anders, Z. anorg. 1907, 56. 273.) POTASSIUM CHLORIDE 757 Solubility of KC1 in methyl alcohol. 500 mg. KC1 treated with 10 g. of above Concentra- mixture yield only 0.3 mg. to the liquid. (Lawren.ce Smith, Am. J. Sci. 16. 56.) t tion of alcohol. Mol. g. Solubility 1 in 1000 g. wo Molecular solubility Insol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184; Eidmann, C. C. 1899, II. alcohol per 1000 g. H 2 O JX2Vj 1014.) ii 6!25 283.55 280.00 3.81 3.76 Solubility of KC1 in acetone+Aq at t. ii 0.50 276.35 3.71 100 g. of the solution contain ii 1.00 267.85 3.60 % a 3.00 238.10 3.18 t acetone G. H 2 O G. acetone G.KCl 25 364.15 4.89 30 72.73 0.00 27.27 a 0.25 361.90 4.86 5 71.15 3.74 25.11 SI 0.50 357.10 4.79 9.09 69.62 6.96 23.42 11 1.00 348.70 4.67 20 64.88 16.22 18.90 II 3.00 324.15 4.35 30 59.49 25.45 15.06 4-O rQ 17 QK CO Uqi (Armstrong and Eyre, Proc. Roy. Soc. 1910 (A) 84. 127.) TtU 50 60 OO . -L * 45.98 37.97 OO . O^ 45.98 56.91 . OJ- 8.04 5.12 70 29.22 68.18 2.60 At room temp. 1 pt. by weight is sol. in: 200 pts. methyl alcohol, D 15 0.7990. 750 " ethyl " D 15 0.8035. 80 90 100 19.82 9.98 0.00 79.43 89.88 100.00 0.76 0.13 0.00 Insol. in propyl alcohol. (Rohland, Z. anorg. 1899, 18. 325.) 100 g. methyl alcohol dissolve 0.53 g. KC1 at 25. 40 5 9.09 71.31 69.62 67.88 0.00 3.67 6.79 28.69 26.72 25.33 100 g. ethyl alcohol dissolve 0.022 g. KC1 at 25. 15 20 65.15 62.97 11.51 15.75 32.34 21.28 100 g. propvl alcohol dissolve 0.004 g. KC1 at 25. 80 85 19.81 14.94 79.34 84.66 0.58 0.40 100 g. isoamyl alcohol dissolve 0.0008 g. KC1 at 25. 90 95 10.00 4.97 89.84 94.96 0.16 0.07 (Turner and Bissett, Chem. Soo. 1913, 103. 100 0.00 100.00 0.00 1909.) Sinnck +Viof* ia Vin-f f\r\c* li^nirl YtV*aoa V*vt*/\ Insol. in propyl alcohol. (Schlamp, Z. phys. Ch. 1894, 14. 276.) Solubility of KC1 in propyl alcohol. t Concentra- tion of alcohol. Mol. g. per 1000 g. H 2 O Solubility in 1000 g. H 2 Molecular solubility (1 0^25 0.50 1.00 283.55 274.10 265.45 248.0 3.81 3.68 3.56 3.33 25 it u it 0^25 0.50 1.00 365.10 355.40 347.70 331.50 4.90 4.77 4.67 4.45 (Armstrong and Eyre, Proc. Roy. Soc. 1910, (A) 84. 127.) Insol. in fusel-oil. (Gooch, Am. Ch. J. 9. 53.) Very si. sol. in mixture of equal pts. ab- solute alcohol and ether. (Berzelius.) these figures represent the solubility of KC1 in acetone+Aq at 30 and 40. (Snell, J. phys. Chem. 1898, 2. 484.) The addition of KC1 to mixtures of acetone and H 2 O will cause a division into two layers. The following table gives the temp, at which sat. solutions of KC1 in acetone+Aq of varying concentra- tions separate into two layers and also the compositions of the sat. solutions of KC1 in acetone+Aq. % acetone Temp, of division 100 g. of solution contain G.H 2 G. acetone G.KCl 26 46.5 30 40.0 59.36 25.44 15.20 40 34.2 53.21 35.47 11.32 50 32.6 45.97 45.97 8.06 60 33.3 37.86 56.80 5.34 70 35.5 29.09 68.25 2.66 75 39.0 80 45.6 19.80 79.20 1.00 (Snell.) 758 POTASSIUM CHLORIDE The following table gives the compositions of the solutions of KCl in acetone +Aq at the points at which the solution just divides into two layers. Temp. = 40. 100 g. of the solution contain Solubility in acetone +Aq at 20. A=ccm. acetone in 100 ccm. acetone+Aq. KCl=millimols KC1 in 100 cem. of the solution. G. H 2 G. acetone G. KCl 56.68 28.63 14.68 53.05 35.67 11.29 50.34 39.82 9.83 47.60 43.83 8.58 44.35 48.36 7.29 42.68 50.75 6.57 38.53 56.26 5.21 36.59 58.84 4.57 32.37 64.18 3.45 30.62 66.43 2.95 28.12 69.45 2.44 A KCl 410.5 10 351.7 20 286.6 30 223.7 40 166.5 50 115.4 60 71.2 . $ 70 38.5 80 12.9 90 2.0 100 (Herz and Knoch, Z. anorg. 1904, 41. 317.) (Snell.) Solubility of KCl in glycerine +Aq at 25. G=g. glycerine in 100 g. glycerine+Aq. The addition of KCl to aqueous acetone causes the separation of the liquid into two layers. The following table gives the composition of these layers at 40. KCl = millimols KCl in 100 cc. tion. of the solu- G KCl Sp. gr. 13.28 25.98 45.36 54.23 83.84 100 424.5 383.4 339.3 271.4 238.5 149.0 110.6 1.1800 1.1848 1.1935 1.2106 1.2189 1.2590 1.2860 Upper layer contains per 100 g. of solution G. H 2 O G. acetone G. KCl 55.20 54.27 53.27 51.69 51.23 50.34 49.08 48.02 47.62 46.49 45.65 45.64 58.99 31.82 36.69 35.44 37.76 48.50 39.88 41.67 43.18 43.73 45.34 46.52 46.57 25.24 12.99 12.03 11.29 10.55 10.27 9.77 9.26 8.79 8.64 8.17 7.83 7.79 15.77 (Herz and Knoch, Z. anorg. 1905, 45. 267.) Insol. in CS 2 . (Baeyer; Arctowski, Z. anorg. 1894, 6. 257.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethy 1 acetate. (Naumann, B. 1910, 43. 314.) Solubility of KCl in organic compounds +Aq i at 25. Lower layer contains per 100 g. of solution G. HH 2 O. Sol. in alcohol. Potassium hydroxide, KOH. Very deliquescent, and sol. in H 2 O with evolution of much heat. 100 pts. KOH, ex- posed over H 2 O at 16-20 take up 460 pts. H 2 O in 56 days. (Mulder.) 1 pt. KOH dissolves in 0.5 pt. cold H 2 O (Lowitz) ; in 0.47 pt. cold H 2 O (Bineau, C. R. 41. 509) ; in 1 pt. H 2 0. (Abl.) Solubility of KOH in H 2 O at t. t G. KOH per 100 g. Solid phase H 2 O solution 22 3.7 3.6 Ice 20.7 22.5 18.4 " 65.2 44.5 30.8 " 36.2 36.2 26.6 KOH.4H 2 O 32.7 77.94 43.8 " 33 80 44.4 KOH.4H 2 O+KOH. 2H 2 O 23.2 85 45.9 KOH.2H 2 O 97 49.2 " 10 103 50.7 " 15 107 51.7 " 20 112 52.8 " 30 126 55.76 " 32.5 135 57.44 KOH.2H 2 0+KOH. H 2 O 50 140 58.33 KOH.H 2 O 100 178 64.03 " 125 213 68.06 " 143 311.7 75.73 (Pickering, Chem. Soc. 1893, 63. 908.) 100 pts. KOH are sol. in 93.4 pts. H 2 O at 15 or 100 pts. H 2 O dissolve 107 pts. KOH at 15". Sp. gr. = 1.5355 at 15. 762 POTASSIUM HYDROXIDE All higher values found in solubility tables are incorrect. (Ferchland, Z. anorg. 1902 30. 133.) 100 g. sat. aq. solution at 15 contain 50.48 g. KOH. (de Forcrand, C. R. 1909, 149. 719.) Sat. KOH+Aq boils at 157.7 (Griffiths) 340. (Gerlach). B.-pt. of KOH+Aq containing pts. KOH tc 100 pts. H 2 O. B.-pt. 105 C 110 115 120 125 130 135 140 145 150 155 160 165 170 175 180 185 190 195 200 205 210 Pts. KOH 20.5 34.5 46.25 57.5 67.5 76.8 85.0 92.5 99.8 106.5 114.05 121.7 129.35 137.0 144.8 152.6 160.4 168.2 176.5 185.0 193.5 202.0 B.-pt. 215 220 225 230 235 240 245 250 255 260 265 270 275 280 285 290 295 300 310 320 33C 340 Pts. KOH 210.5 219.8 230.0 240.9 251.9 263.1 274.4 285.7 298.5 312.5 328.0 343.5 359.0 375.0 391.0 408.2 425.5 444.4 484.0 526.3 571.5 623.6 (Gerlach, Z. anal. 26. 464.) Sp. gr. and b-pt. of KOH-f-Aq according to Dalton. % K 2 Sp. gr. B.-pt. %K 2 p Sp. gr. B.-pt. 4.7 1.06 100.56 36.8 1.44 123.89 9.5 .11 101 . 11 39.6 1.47 i 129.44 13.0 .15 101.66 42.9 1.52 135.56 16.2 .19 103.33 46.7 1.60 143.33 19.5 .23 104.44 51.2 1.68 ; 160 . 00 23.4 .28 106.66 56.8 1.78 , 188 . 22 26.3 .33 109.44 63.6 1.88 : 215.56 29.4 .36 112.22 72.4 2.00 315.56 32.4 .39 115.56 84.0 2.2 i red heat 34.4 .42 118.89 100 2.4. Sp. gr. of KOH +Aq at 15. %K 2 Sp. gr. % K ? Sp. gr. % K 2 d> Sp. gr. 0.568 1.0050 10.750 1 . 1059 20.935 .2268 1.697 1.0153 11.882 1.1182 21.500 .2342 2.829 1.0560 13.013 1 . 13Q8 22 . 632 .2493 3.961 1.0369 14.145 1 . 1437 23 . 764 .2648 5 . 002 1.0478 15.277 1.1568 24 . 895 .2805 6.224 1 . 0589 16.408 1 . 1702 26.027 .2966 7.355 1.0703 17.540 1 . 1839 27.158 1.3131 8.487 1.0819 18.671 1 . 1979 28 . 290 1 . 3300 9.619 1.0938 19 . 803 1.2122 (Zimmerman, N. J. Pharm. 18, 2. 5. Sp. gr. of KOH + Aq. %K 2 Sp. gr. % K 2 Sp. gr. % K ? Sp. gr. 2.44 1.02 23.14 1.22 37.97 1.42 4.77 1.04 24.77 1.24 40.17 1.44 7.02 1.06 26.34 1.26 42.31 1.46 9.20 1.08 27.86 1.28 44.40 1.48 11.28 1.10 29.34 1.30 46.45 1.50 13.30 1.12 30.74 1.32 48.46 1.52 15.38 1.14 32.14 1.34 50.09 1.54 17.40 1.16 33.46 1.36 51.58 1.56 19.34 1.18 34.74 1.38 53.06 1.58 21.25 1.20 35.99 1.40 (Richter.) Sp. gr. of KOH +Aq at 15. a = K 2 O;b = sp. gr. if % is % i 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 .010 .020 .030 .039 .048 .058 .068 .078 .089 .099 .110 .121 .132 .143 .154 .166 .178 .190 .202 .215 230 242 256 270 285 300 312 326 340 1.355 .009 .017 .025 .033 .041 .049 .058 .065 .074 .083 .092 .110 .111 .119 .128 .137 .146 1.155 1.166 1.177 1.188 1.198 1.209 1.220 1.230 1.241 1.252 1.264 1.278 1.288 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 1.370 1.385 1.403 1.418 1.431 445 460 475 490 504 522 539 564 570 584 600 615 630 645 660 676 690 705 1.720 1.733 1.746 1.762 1.780 1.795 1.810 (Calculated by Gerlach, Z. anal. 8. 279, after Zimmermann, N. J. Pharm. 18, 2. 5, ana Schiff, A. 107. 300.) Sp.gr. of KOH+Aq at 15. %KOH 4.2 8.4 12.6 16.8 Sp. gr. 1.0382 1.0776 1.1177 1 . 1588 % KOH 21.0 25.2 29.4 Sp. gr. 1.2008 1.2439 1.2880 (Kohlrausch, W. Ann. 1879. 1.) POTASSIUM HYDROXIDE 763 Sp.gr. of KOH+Aqat 15. Sp. gr. of KOH+Aq. % KOH 6.87 Sp. gr. 20/20 1.0601 (Le Blanc and Rohland, 19. 272 KOH4-Aa containing 12.10 1.1025 Z. phys. Ch. eoual nts. of 1896, KOH % KOH Sp. gr. % KOH Sp. gr. 10 20 30 40 1.077 1.175 1.288 1.411 50 60 70 1.539 1.667 1.790 (Gerlach, Z. anal. 27. 275, calculated from Schiff, A. 107. 300.) Sp. gr. of K 2 O+Aq at 15. %K 2 Sp. gr. %K 2 Sp. gr. 5 10 15 20 25 1.054 1.111 1 . 171 1.231 1.294 30 35 40 45 1.358 1.428 1.500 1.576 (Hager, Adjumenta varia, Leipsic, 1876.) Sp. gr. of KOH+Aq at 20 containing 2 mols. KOH to 100 mols. H 2 O = 1.05325. (Nicol, Phil. Mag. (5) 16. 122.) Sp.gr. of KOH+Aqat 15. KH Sp.gr. KOH Sp. gr. % KOH Sp. gr. 52 1 . 53822 34 1.33313 16 1 . 14925 51 1.52622 33 1.32236 15 1 . 13955 50 1.51430 32 1.31166 14 1.12991 49 .50245 31 .30102 13 1.12031 48 .49067 30 .29046 12 1.11076 47 .47896 29 .27997 11 1.10127 46 .46733 28 . 26954 10 1.09183 45 .45577 27 . 25918 9 1.08240 44 .44429 26 1 . 24888 8 1.07302 43 .43289 25 1.23866 7 1.06371 42 .42150 24 1.22849 6 1.05443 41 .41025 23 1.21838 5 1.04517 40 .39906 22 1.20834 4 1.03593 39 .38793 21 1.19837 3 1.02671 38 . 37686 20 1 . 18839 2 1.01752 37 . 36586 19 1.17855 1 1.00834 36 1.35485 18 1 . 16875 0.99918 35 1.34396 17 1 . 15898 (Pickering, Phil. Mag. 1894, (5) 37. 375.) Sp. gr. of N solution at 18/4 = 1.0481. (Loomis, W. Ann. 1896, 60. 550.) and H 2 O freeze^ at 54. (Guyton-Morveau, Gm.-K. 2, 1. 18.) KOH is completely miscible with NaOH and with RbOH in both the liquid and the solid states. (Hevesy, Z. phys. Ch. 1910, 73. 667.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Abundantly sol. in strong alcohol or wood- spirit. See below under KOH+2H 2 O. Readily sol. in glycerine. Sol. in not less than 25 pts. of ether. (Boullay .) Sol. in much more than 25 pts. of ether. (Connell.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904,37.3601.) Insol. in acetone. Readily sol. in fusel oil. Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014:) Sol. in aqueous solution of mannite. (Favre, A. ch. (3) 11. 76.) The composition of the hydrates formed by KOH at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by KOH and of the conductivity and sp. gr. of KOH+Aq. (Jones, Am. Ch. J. 1905, 34. 337.) +H 2 0. +2H 2 O. Very deliquescent, and sol. in H 2 O with absorption of much heat. 100 g. sat. solution in H 2 O at 30 contain 55.75 g. anhyd. KOH. (de Waal, Dissert. 1910.) Solubility of KOH+2H 2 O in alcohol+Aq'at 30. % KOH % alcohol % HzO 55.75 44.25 54.81 0.43 44.76 rf * 31 'O 57/50 1150 28.99 65.07 5.94 27.67 69.92 2.41 27.20 73.01 negative 26.25 81.98 |t< *Separates into two layers. (de Waal, Dissert, 1910.) +4H 2 0. 764 POTASSIUM HYDROGEN TITANIUM IMIDE Potassium hydrogen titanium diimide, TS ( TV TT MSI K" Solubility of KI in 100 pts., etc. Continued. 111 IN -tLjIN-tY. Decomp. by H 2 O and alcohol. Insol. in t Pts. KI t Pts. KI t Pts. KI all ord. indifferent organic solvents. (Ruff, 57 174 78 191 99 208 B. 1912, 46. 1371.) 58 175 79 192 100 209 59 175 80 192 101 210 60 176 81 193 102 211 Potassium iodide, KI. 61 177 82 194 103 212 Deliquescent only in very moist air. Very sol. in H 2 O with absorption of heat. The temp, of H 2 O can be lowered 24 by dissolving KI. (Baup.) 140 pts. KI dissolved in 100 pts. H 2 O at 10.8 lower the temp. 22.5. (Rtidorff, Pogg. 136. 276.) 62 63 64 65 66 67 68 178 179 180 180 181 182 183 83 84 85 86 87 88 89 195 196 197 197 198 199 200 104 105 106 107 108 109 110 213 213 214 215 216 217 218 100 pts. H 2 O dissolve 126.6 pts. KI at (Kremers); 127.8 pts. KI at (Mulder); 127.9 pts. KI at 0. (Gerardin.) By boiling, 100 pts. H 2 O dissolve 221 pts. KI at 120 (Baup); 222.2 pts. KI at 120 (Gay-Lussac); 222.6 pts. KI at 118.4 (Mul- der); 223.58 pts. KI at 117 (Legrand); 223.6 pts. KI at 117. (Gerardin.) Between these temps, the solubility in- 69 70 71 72 73 74 75 76 77 184 184 185 186 187 188 188 189 190 90 91 92 93 94 95 96 97 98 201 202 202 203 204 205 206 207 208 111 112 113 114 115 116 117 219 220 220 221 222 223 223.6 creases proportional to temp. (Mulder, calculated from his own and other Sr.1 in O 73/i r>t TT.O ot 1 9 Z \r> O 7flQ r>t TToO at. observations, Scheik. Verhandel. 1864. 63.) 16; in 0.7 pt. H 2 O at 18; in 0.45 pt. H 2 O at 120. (Graham-Otto.) 100 pts. KI+Aq sat. at 15-16 contain 58.07 pts. KI. (v. Hauer, J. pr. 98, 137.) 100 pts! H 2 O at *12.5 dissolve 136 pts.; at 16, 141 OU1UULU.UJ UJ. -LVJ. Ill 1\J\J JJUO. xx 2 vy ai/ u . pts. KI. (Baup.) 100 pts. H 2 O at 18 dissolve 143 pts. KI; at 120, 271 pts. (Gay-Lussac.) t Pts. KI t Pts. KI t Pts. KI Sol. in 0.79 pt. H 2 O at 0; in 0.70 pt. H 2 at 20; in 0.63 pt. H 2 O at 48; in 0.57 pt. H 2 O at 60; in 0.53 pt. H 2 O at 80; in 0.51 pt. H 2 O at 100. (Kremers, Pogg. 97. 15.) -22.65 -22.35 -16.8 107.2 106.6 111.1 21.05 25.6 29.1 143.3 146.6 149.6 71.1 74.75 81.6 183.5 185.6 192.0 -11.35 116.3 37.3 156.7 86.35 194.6 Sol. in 0.71 pt. H 2 O at 15. CEder, Dingl. 991 8Q ^ -5.9 120.4 126.1 42.3 45.75 160.3 163.6 93.5 100.7 200.3 205.6 AtfX* Ot7.J +3.25 130.1 51.8 167.6 110.2 216.1 9.55 134.0 55.05 169.1 113.7 218.8 * 12.75 137.1 60.55 173.4 Solubility of KI in 100 pts. H 2 O at t. 12.9 137.9 65.0 178.3 t Pts. KI t Pts. KI t Pts. KI (Coppet, A. ch. (5) 30. 417.) 127.9 19 143.4 38 159 1 128.7 20 144.2 39 160 2 129.6 21 145.1 40 160 Solubility is represented by a straight line 3 130.4 22 145.9 41 161 of the formula 126.23 +0.8088t. (Coppet.) 4 131.2 23 146.7 42 162 5 132.1 24 147.5 43 163 6 7 132.9 133.7 25 26 148.3 149.1 44 45 164 164 Solubility of KI in 100 pts. H 2 O at high temp. 8 134.5 27 149.9 46 165 t Pts. KI t Pts. KI 9 135.3 28 150.7 47 166 10 136.1 29 151.5 48 167 124 233.9 144 264.6 11 137.0 30 152.3 49 168 133 249.3 175 310.4 12 137.8 31 153 50 168 13 138.6 32 154 51 169 (Tilden and Shenstone, Phil. Trans . 1884. 23.) 14 139.4 33 155 52 170 15 140.2 34 156 53 171 16 17 18 141.0 141.8 142.6 35 36 37 156 157 158 54 55 56 172 172 173 If solubility S =pts. KI in 100 pts. solution, S = 55.8+0.122t from to 165. (fitard, C. R. 98. 1432.) POTASSIUM IODIDE 765 Sat. KI+Aq contains % KI at t. Sp. gr. of KI+Aq at 21. ft 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 Sp. gr. % KI Sp. gr. '& Sp. gr. t % KI t %KI -21 -21 -21 -19 -15 -9 +21 44 72 50.7 51.0 51.2 52.2 53.2 54.5 56.9 59.3 60.8 64.3 78 96 150 151 175 176 190 193 213 64.8 66.9 70.6 70.9 71.6 72.7 73.8 74.5 75.7 1.0075 1.0151 1.0227 1.0305 1.0384 1.0464 1.0545 1.0627 1.0710 1.0793 1.0877 1.0962 1.1048 1.1136 1 . 1226 1.1318 1.1412 1.1508 1 . 1605 1 . 1705 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 .1807 .1911 .2016 .2122 .2229 1.2336 1.2445 1.2556 1.2699 1.2784 1.2899 1.3017 1.3138 1.3262 .3389 .3519 .3653 .3791 .3933 1.4079 41 42 43 44 45 46 47 . 48 49 50 51 52 53 54 55 56 57 58 59 60 .4224 .4371 .4520 .4671 .4825 .4982 .5142 .5305 .5471 .5640 .5810 .5984 .6162 .6343 .6528 .6717 .6911 .7109 .7311 .7517 (fitard, A. ch. 1894, (7) 2, 542.) Solubility of KI in 100 g. H 2 O at t. t g.KI t g.KI. -1 5 122.2 119.8 117.4 115.1 75.8 -11.5 9 5 64.7 51.5 42.6 34.4 25.7 -4 -10 -14 -7 -6 -5 (Schiff, A. 110. 75.) Sp. gr. cf KI+Aq. S = according to Schiff (A. 108. 340) at 21; K = according to Kremers (Pogg. 96. 62), interpolated bv Gerlach (Z. anal. 8. 285.) (Meusser, Z! anorg. 1905, 44. 80.) 102.70 pts. by weight are contained in 100 cc. KI+Aq sat. at 25, or 59.54 pts. in 100 g. of solution; sp. gr. = 1.7254. 94.05 pts. by weight are contained in ICO cc. KI+Aq sat. at 0, or 56.34 pts. in 100 g. of solution; sp. gr. = 1.6699. (Walden, Z. phys. Ch. 1906, 55. 715.) Solubility of KI in H 2 O at low temperatures. 5 10 S 1.038 1.079 K 1.038 1.078 35 40 S 15 20 1.123 1.171 . 1.120 1.166 1 45 50 1 .483 25 .. ] 218 ] 55 30% KI, ..279 ..271 60% KI. K 1.331 1.396 1.469 1.546 1.636 ] Sp. gr. of KI+Aq at 18. .734 g Sp. gr. & Sp. gr. | Sp. gr. t %KI Solid phase t % KI Solid phase 5 1.0363 10 1.0762 20 1 . 1679 30 40 50 1.273 1.3966 1.545 55 1.630 -12.5 IK 38 41.2 44.6 48 51.2 51.9 Ice +KI -22 20 52.1 52.6 53.5 54.5 55.4 56.4 KI u It (( ({ (I -17.5 -20 -22.5 -15 -10 - 5 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of KI+Aq at 18. 23.2 %KI Sp. gr. (Kremann and Kershbaum, Z. anorg. 1907, 56. 218.) 1.044 5.0 1.0062 1 . 0363 149.26 g. KI dissolve in 100 g. H 2 O at 25. (Amadori and Pampanini, Rend. Ace. Line. 1911, V, 20. 473.) 60.39 g. in 100 g. KI+Aq sat. at 25. (Parsons and Whittemore, J. Am. Chem. Soc. 1911, 33. 1934.) 56.1 g. in 100 g. KI+Aq set. at 0; 60.35 g. in 100 g. KI+Aq sat. at 30. (Van Dam and Donk, Chem. Weekbl. 1911, 8. 848.) (Giotrian, W. Ann. 1883, 18. 191.) Sp. gr. at 16/4 of KI+Aq containing 32.4875% KI = 1.30238. (Schonrock, Z. phys. Ch. 1893, 11. 781.) KI+Aq containing 9.35% KI has sp. gr. 20/20 = 1.0726. KI+Aq containing 11.35% KI has sp. gr. 20/20 = 1.0892. '(Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) 766 POTASSIUM IODIDE B.-pt. of KI+Aq containing pts. KI to 100 pts. H 2 O. Sol. in liquid SO 2 . (Walden, B. 1899, 32. 2864.) Solubility in SO 2 decreases with rise of temp. (Walden, Z. phys. Ch. 1903, 42. 456.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Hydrazine dissolves 135.7 pts. KI at 12.5- 13. (de Bruyn, R. t. c. 1899, 18. 297.) 100 pts. alcohol of 0.85 sp. gr. dissolve 18 pts. KI at 12.5. 100 pts. absolute alcohol dissolve 2.5 pts. B.-pt. Pts. KI B.-pt. Pts. KI B.-pt. Pts. KI 101 102 103 104 105 106 107 15 30 45 60 74 87 99.5 108 109 110 111 112 113 114 111.5 123 134 145 155 165 175 115 116 117 118 118.5 185 195 205 215 220 (Gerlach, Z. anal. 26. 439.) Sat. KI+Aq boils at H9. (Kremers.) Sat. KI+Aq forms a crust at 117.5, and contains 210 pts. KI to 100 pts. H 2 O; highest temp, observed, 118.5. (Gerlach, Z. anal. 26. 426.) 100 pts. alcohol of D sp. gr. at dissolve at 18 D 0.9904 0.9851 0.9726 0.9665 0.9528 130.5 119.4 100.1 89.9 76.9 pts. KI, D 0.9390 0.9088 0.8464 0.8322 66.4 48.2 11.4 6.2 pts. KI. Solubility of KI in I 2 +Aq at 25. KI mol./l. I g. -atoms/1. 6.15 6.23 6.40 6.36 6.33 6.24 0.00 3.64 11.11 13.16 13.2 17.03 (Abegg, Z. anorg. 1906, 60. 428. Solubility of KI+I 2 in H 2 O at 25. a %l Solid phase | %l Solid phase 29.45 28.91 26.84 27.18 27.14 64.34 63.88 66.54 67.14 66.60 KI+KI 3 if KI 3 +KI 7 it tt 25.88 25.57 27.86 27.27 26.95 25.71 68.79 69.01 66.56 66.91 67.17 67.91 KI 7 +I 2 a KI 3 a KI 7 tt (Foote and Chalker, Am. Ch. J. 1908, 39. 564.) See also under Iodine. KI+Aq sat. at 14.5 containing 139.8 pts. KI to 100 pts. H 2 O dissolves 1.0 pt. K 2 S0 4 with separation of 2.2 pts. KI, so that solution contains 137.6 pts. KI and 1.0 pt. K 2 SO 4 to 100 pts. H 2 O. (Mulder, Rotterdam, 1864.) 100 pts. H 2 O dissolve 86.3 pts. KI and 2.1 pts. Na 2 SO 4 at 14.5. (Mulder, J. B. 1866. 67.) Sol. in AsCl 3 , SnCl 4 and POC1 3 . (Walden, Z. anorg. 19CO, 25. 21 4.) Attacked by dry liquid KO 2 with liberation of I 2 . (Frankland, Chem. Soc. 1901, 79. 1361 . That is, aqueous alcohol dissolves approxi- mately the same amount of KI that the water present in the alcohol would dissolve, and it is therefore probable that KI is insol. in strictly absolute alcohol. (Gerardin.) Solubility in 100 pts. alcohol of 0.9496 sp. gr. at: 8 13 25 46 55 62 67.4 69.2 75.1 84.7 87.5 90.2 pts. KI. (Gerardin, A. ch. (4) 5. 155.) Sol. in 68.3 pts. absolute alcohol (Eder, Dingl. 221. 89); in 370 pts. ether (sp. gr. 0.729), (Eder, I.e.); in 120 pts. alcohol-ether (1 : 1), (Eder, I. c.) Sol. in 10-12 pts. 90% alcohol, and 40 pts. absolute alcohol. (Hager, Comm. 1883.) 100 pts. absolute methyl alcohol dissolve 16.5 pts. at 20.5; 100 pts. absolute ethyl alcohol dissolve 1.75 pts. at 20.5. (de Bruyn, Z. phys. Ch. 10. 783.) Solubility of KI in methyl alcohol +Aq at 25 c p = % by wt. of alcohol in alcohol +Aq. S =Sp. gr. of alcohol+Aq sat. with KI. L = millimols KI in tion. 100 ccm. of the solu- P S 25/4 L 1.7213 620 10.6 1.634 555 30.8 1.460 431 47.1 1.325 335 64.0 1.185 243 78.1 1.066 169 98.9 0.9700 113 100 0.9018 .80 (Herz and Anders, Z. anorg. 1907, 55. 274.) POTASSIUM IODIDE 767 Solubility of KI in CH 3 OH. G = g. KI in 100 g. of the solution, ti =temp. of complete solution. t 2 = temp, at which salt begins to separate out. Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G =g. KI in 10 ccm. of the solution. S =Sp. gr. of the sat. solution. G ti t2 P G S 25/4 8.64 12.95 14.2 14.6 14.97 19.2 26.8 28.9 "6 20 25 85 115 144 266 262 256 242 229 11.11 23.8 65.2 91.8 93.75 100 1.316 1.096 0.854 0.262 0.060 0.058 0.043 0.9018 0.8823 0.8629 0.8187 0.8045 0.8041 0.8041 29.6 188 196 33.0 (Herz and Kuhn.) (Centnerszwer, Z, phys. Ch. 1910, 72. 432.) Solubility of KI in methyl alcohol at t. Solubility in mixtures of propyl and ethyl alcohol at 25. t g. KI in 100 g. alcohol t g. Klin 100 g. alcohol y/o propyl alconoi in tne solvent. G = g. KI in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. 15 30 50 80 100 120 140 160 14.50 16.20 18.9 22.5 25.0 27.2 29.2 30.6 180 200 220 240 245 247 250 252.5* 30.7 29.1 27.5 24.8 22.6 21.0 13.8 7.6 p G S 25/4 8.1 17.85 56.6 88.6 91.2 95.2 100 0.155 0.146 0.137 0.075 0.052 0.049 0.044 0.043 0.8015 0.7983 0.7991 0.7988 0.8022 0.8027 0.8029 0.8041 *Critical temp, of solution. (Tyrer, Chem. Soc. 1910. 97. 626.) At room temp. 1 pt. KI by weight is sol. in 6 pts. methyl alcohol D 15 0.7990. 16 " ethyl " D 15 0.8322. 219 " propyl " D 15 0.8160. (Rohland, Z. anorg. 1898, 18. 325.) Solubility in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the solvent. G =g. KI in 10 ccm. of the solution. S =Sp. gr. of the sat. solution at 25. P G S 25/4 0.00 0.155 0.8015 4.37 0.191 0.8041 10.40 0.225 0.8071 41.02 0.494 0.8295 80.69 1.013 0.8794 84.77 1.072 0.8795 91.25 1.184 0.8908 100.00 1.316 0.9018 (Herz and Kuhn.) 100 g. methyl alcohol dissolve 18.04 g. KI at 25. 100 g. ethyl alcohol dissolve 2.16 g. KI at 25. 100 g. propyl alcohol dissolve 0.43 g. KI at 25. 100 g. isoamyl alcohol dissolve 0.09 g. KI at 25. (Turner and Bissett, Chem. Soc. 1913, 103. 1909.) 0.455 g. is sol. in 100 g. propyl alcohol. Schlamp, Z. phys. Ch. 1894, 14. 276.) Alcoholic solution can be mixed with ^ vol. ether without pptn. 100 g. 95% formic acid dissolve 38.2 g. KI at 18.5. (Aschan, Chem. Ztg. 1913, 37. .113.) (Herz and Kuhn, Z. anorg. 1908, 60. 155.) 768 POTASSIUM IODIDE Solubility in organic solvents at t. C = pts. by wt. of KI in 100 ccm. of the sat. solution. L = no. of litres which at the saturation temp, hold in solution 1 mol. KI. S = sp. gr. of the solution at t, referred to H 2 O at t. p = pts. by wt. of KI in 100 g. of the solu- tion. Solvent t c L S p Water 25 102.70 0.162 1.7254 59.54 94.05 0.177 1 . 6699 56.32 Methyl alcohol 25 13.48 1.231 . 9003 14.97 ( * 25 14.26 " 11.61 1.430 0.8964 12^95 Ethyl alcohol 25 1.520 10.92 . 7908 1 . 922 1.197 13.87 0.8085 1.479 Glycol 25 45.85 . 362 ) 1 . 3888 33.01 " 25 47.23 0.351) " 43.28 0.383 1 . 3954 31^03 Acetonitrile 25 1.551 10.70 25 1.590 10.44 0.7936 2^003 ' 1.852 9.00 0.8198 2.259 Propiomtrile 25 0.316 52 . 53 ) 0.7821 0.404 1 25 0.355 46.76V ) ' 0.344 48 . 26 ) V 0.8005 0^429 0.412 40.29 } Benzonitrile 25 0.051 325.5 1 . 0076 0^050 Nitromethane 25 0.349 47.56 1 . 1367 0.307 25 0.289 57.44 " 0.366 45.36 1 . 1627 0^315 " 0.314 52.87 Nitrobenzene 25 0.0019 87.40 Acetone 25 1.038 16.0 0.7968 l'302 1.732 9.58 . 8227 2.105 Furfurol 25 5.93 2.80 1.2014 4.94 " 15.10 1.10 Benzaldehyde 25 0.343 48.4 1 . 0446 0^328 Salicy laldehy d e 25 0.549 30.24 1 . 1373 0.483 " 1.257 13.21 1.1501 1.093 Anisaldehyde 25 0.720 23.06 1.1180 0.644 " 1.520 10.92 1 . 1223 1.355 Ethyl acetate Methyl cyan- 25 0.0013 12.80 acetate 25 2.459 6.75 1 . 1358 2.165 3.256 5.10 1.1521 2.827 Ethyl cyan- acetate 25 0.888 18.7 1 . 0579 0.839 25 1.090 15.23 1.0678 1.021 (Walden, Z. phys. Ch. 1906, 65. 715.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3789.) Sol. in ethyl acetate. (Casaseca, C. R. 30. 821.) Insol. in ethyl acetate. (Naumann, B 1910, 43. 314.) Insol. in ethylamine. (Shinn, J. phys Chem. 1907, 11. 538.) 100 pts. acetone dissolve 2.930 pts. KI at 25. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Sol. in acetone, insol. in methylal. (Eid- mann, C. C. 1899. II. 1014.) 3.08 pts. sol. in 100 pts. acetone at 2.5. 2.38 " "' " 100 " " " +22. 1.21 " " " 100 " " " 56. 0.26 " " " 100 0.11 " " " 100 (Laszczynski, B. 1894, 27. 2287.) " pyridine " 10. " " " 119. Freely sol. in glycerine. Insol. in acetic acid. (Berthemot.) Sol. in 3 pts. glycerine; insol. in olive oil. and Garot.) 100 g. glycerol dissolve 40 g. KI at 15.5. Ossendowski, Phann. J. 1907, 79. 575.) Potassium riiodide, KI 3 . Very deliquescent; very sol. in H 2 O and alcohol. (Johnson, Chem. Soc. 1877, 1. 249.) Solution of I in K I contains this salt (see KI). Decomp. by heat or shaking with CS 2 , ther, chloroform. Sol. in alcohol, from which CS 2 does not remove I. (Jorgensen, J. pr. (2) 2. 247.) Potassium periodide. Solubility determinations show that the compds. KI 3 and KI 7 are the only periodides of potassium which form solids at 25. See under KI+I. (Foote and Chafer, Am. Ch. J. 1908, 39. 566.) K1 7 . See above. Potassium mercuric iodide ammonia, K 2 HgI 4 , 2NH 3 . (Peters,' Z. anorp. 1912, 77. 188.) Potassium silver iodide, KI, Agl. Sol. in KI+Aq. Sol. in hot alcohol. (Boullay, A..ch. 34. 377.) 2KI, Agl, Sol. in KI+Aq. Decomp. by H 2 O (Boullay.) Hygroscopic. (Hellwig, Z. anorg. 1900, 25. 180.) SKI, Agl. Decomp. by H 2 O. (Ditte, C. R. 93, 415.) KI, 2 Agl. Sol. in methylethylketone. (Marsh, Chem. Soc. 1913, 103. 783.) Potassium silver polyiodide, AgK 3 I 12 , 3KI + 5H 2 O. Very deliquescent. (Johnson, Chem. Soc. 33. 183.) Potassium tellurium iodide. See lodotellurate, potassium. Potassium thallic iodide, KI, T1I 3 . Decomp. by H 2 O. Can be crystallized from alcohol. (Willm.) SKI, 2T1I 3 +3H 2 O. Partially decomp. by H 2 O. (Rammelsberg.) Potassium (tin) stannous) iodide, KI, SnI 2 + When treated with a small quantity of H 2 O, KI dissolves out; but when more H 2 O is added, the substance is completely dissolved. More sol. in warm than cold alcohol. (Boul- lay.) POTASSIUM SULPHIDE 769 Potassium zinc iodide, KI, ZnI 2 . Very deliquescent. (Rammelsberg, Pogg 43. 665.) K 2 ZnI 4 +2H 2 O. Hydroscopic. (Ephraim Z. anorg. 1910, 67. 382.) Potassium iodide sulphur dioxide, KI, SO 2 (Pochard, C. R. 1900, 130. 1188.) KI, 4SO 2 . (Walden, Z. phys. Ch. 1903 42. 439.) KI, 14SO 2 . fWalden.) Potassium nitride, K 2 N. Decomp. violently by H 2 O. (H. Davy. Potassium ruthenium efoTiydronitrosobromide Ru 2 H 2 NOBr 3 , 2HBr, 3KBr. Ppt. (Brizard, A. ch. 1900, (7) 21. 362.) Potassium ruthenium nitrosochloride, Ru 2 H 2 NOCl 3 , 3KC1, 2HC1. SI. sol. in H 2 O. (Brizard, C. R. 1899, 129 216.) Potassium sw&oxide. Decomposes H 2 O. Does not exist. (Lupton, Chem. Soc. 1876, 2. 565.) Potassium oxide, K 2 O. Very sol. in H 2 O with much heat. See Potassium hydroxide. Potassium dioxide, K 2 O 2 . Deliquescent. Sol. in H 2 O. Wf t Forms compound K 2 O 2 , 2H 2 O 2 . (Schone. A. 193. 241.) Potassium peroxide, K 2 O 4 . Deliquescent. Very sol. with decomp. in H 2 0. Potassium silicon oxyfluoride, SiF 2 (OK) 2 and SiO(F)OK. (Schiff and Becjii, A. Suppl. 4. 33.) Potassium tantalum oxyfluoride, K 4 Ta 4 O 6 F 14 . Insol. in boiling water. Easily sol. in HF + Aq. (Marignac, A. ch. (4) 9. 268.) Potassium phosphide, KP 3 . Decomp. by H 2 O. (Joannis, C. C. 1894, II. 834.) KP 5 . Easily decomp. by H 2 O. (Hugot, C. R. 1895, 121. 208.) Potassium hydrogen phosphide, PH 2 K. Decomp. by H 2 O. (Joannis, C. R. 1894, 119. 558.) Potassium phosphoselenide, KSeP = K 2 Se, P 2 Se. Sol. in cold H 2 O with rapid decomp. Sol. in alcohol with slight decomp. (Hahn, J. pr 93. 430.) Potassium phospho^nselenide, 2K 2 Se, P 2 Se 3 . Deliquescent. Decomp. violently with H 2 O. Sol. in alcohol or ether, or in a mixture of the two, with slight decomp., but decomp. gradu- ally on the air. (Hahn, J. pr. 93. 430.) Potassium phosphopentoselenide, K 4 P 2 Se7 = 2K 2 Se, P 2 Se 5 . Deliquescent; immediately decomp. by H 2 O, alcohol, or ether. (Hahn.) Potassium phosphosulphide, 4K 2 S 2 , P 2 S 3 . Deliquescent. Sol. in H 2 O with decomp. Potassium selenide, K 2 Se. Sol. in H 2 O with subsequent decomp. on the air. Insol. in liquid NH 3 ; sol. in air free H 2 O to a colorless liquid. (Hugot, C. R. 1899, 129. 299.) +2H 2 O. Sol. in H 2 O with decomp. (Clever, Z. anorg. 1895, 10. 143.) +9, 14, or 19H 2 O. (Fabre, C. R. 102. olo.) Potassium te^raselenide, K 2 Se 4 . Easily sol. in H 2 O. Decomp. on standing. Sol. in liquid NH 3 . (Hugot, C. R. 1899, 129. 299.) Potassium wonosulphide, K 2 S. Deliquescent. Sol. in H 2 O and alcohol. H 2 O solution decomp. on air. Sol. in 10 pts. glycerine. (Cap and Garot, J. Pharm. (3) 26. 81.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Insol. in methyl acetate. (Naumann. B 1909, 42. 3790.) +5H 2 O. (Schone, Pogg. 131. 380.) All potassium sulphides are sol. in glycerine; nsol. in ether and ethyl acetate. Potassium ^'sulphide, K 2 S 2 . Sol. in H 2 O and alcohol, with gradual de- omp. Potassium Zn'sulphide, K 2 S 3 . Sol. in H 2 O and alcohol, with gradual de- onip. on the air. Potassium tefrasulphide, K 2 S 4 . Sol. in H 2 O and alcohol. +2H 2 O. Sol. in H 2 O. SI. sol. in alcohol. +8H 2 O. Sol. in H 2 O. Alcohol takes out r ater. (Schone.) Vrtassium pentasulpbide, K 2 S 6 . Sol. in H 2 O and alcohol. 770 POTASSIUM PALLADIUM SULPHIDE Potassium palladium sulphide. See Sulphopalladate, potassium. Potassium platinum sulphide. See Sulphoplatinate, potassium. Potassium silver sulphide, 4Agr 2 S, K 2 S+2H 2 O. Decomp. by H 2 O. (Ditte, C. R. 1895, 120. 91.) Potassium rhodium sulphide, 3K 2 S, Rh 2 S 3 . Decomp. by H 2 O. (Leidie\) Potassium tellurium sulphide. See Sulphotellurate, potassium. Potassium thallium sulphide, K 2 S, T1 2 S 3 . Not decomposed by H 2 O, or hot NH 4 OH, or KOH+Aq. Decomp. by HC1 or moderately cone. H 2 S0 4 +Aq. Hot HNO 3 +Aq decomp. with separation of S. (Schneider, J. pr. 110. 168.) Potassium tin (stannic) sulphide. See Sulphostannate, potassium. Potassium zinc sulphide, K 2 S, 3ZnS. Not attacked by H 2 O, but easily decomp. by the most dil. acids. (Schneider, J. pr. (2) 8. 29.) Potassium telluride, K 2 Te. Sol. in H 2 O. (Demargay, Bull. Soc. (2) 40. 99.) Sol. in H 2 O and liquid NH 3 . (Hugot, C. R. 1899, 129. 388.) Praseocobaltic chloride, Co(NH 3 ) 4 Cl 3 +H 2 0. Easily sol. in H 2 O. Dil. HCl-i-Aq dissolves traces; cone. HC1+ Aq dissolves more. Sol. in NH 4 OH+Aq with decomp. Sol. in cone. H 2 SO 4 without de- comp. SI. sol. in dil. H 2 SO 4 +Aq. (Rose.) mercuric chloride, Co(NH 3 ) 4 Cl 3 , HgCl 2 . SI. sol. in cold H 2 O; insol. in HgCl 2 +Aq. .(Vortmann, B. 15. 1892.) chloride bichromate, [CoCl 2 (NH 3 ) 4 ] 2 Cr 2 O 7 +H 2 O. Scarcely sol. in cold, 'easily sol. in warm W>. (Vortmann, B. 15. 1897.) ;Praseocobaltic chloride nitrate, CoCl 2 (NH 3 ) 4 N0 3 +H 2 0. Much less sol. in H 2 O than the chloride. 'Precipitated from aqueous solution by dil. IHNOa+Aq. (Vortmann, B. 15. 1896.) Praseodymicotungstic acid. Ammonium praseodymicotungstate, 2(NH 4 ) 2 O, Pr 2 O 3 , 16WO 3 + 16H 2 O. Very si. sol. in H 2 O. Decomp. by acids and alkalies. (E. F. Smith, J. Am. Chem. Soc. 1904, 26. 1478.) Barium praseodymicotungstate, 4BaO, Pr 2 3 , 16WO 3 +7H 2 O. Ppt. Insol. in H 2 O. 6BaO, Pr 2 O 3 , 16WO 3 +9H 2 O. Ppt. (E. F. Smith.) Silver praseodymicotungstate, 4Ag 2 O, Pr 2 O 3 , 16WO 3 +8H 2 O. Insol. in H 2 O. (E. F. Smith.) Praseodymium, Pr. Praseodymium bromide, PrBr 3 +6H 2 O. Very sol. in H 2 O; sol. in HBr. (von Schule, Z. anorg. 1898, 18. 353.) Praseodymium carbide, PrC 2 . Decomp. by H 2 O; insol. in cone. HNO 3 , decomp. by dil. HNO 3 . (Moissan, C. R. 1900, 131. 597.) Praseodymium chloride, PrCl 3 . Very sol. in H 2 O. Insol. in PC1 3 or SnCl 4 . Sol. in alcohol. Insol. in ether and most or- ganic solvents. (Matignon, C. R. 1902, 134. 427.) 2.14 g. PrCl 3 dissolve in 100 g. pyridine at 15. (Matignon, Int. Cong. App. Cbem. 1909, 2. 53.) +H 2 0. +3H 2 O. +7H 2 O. 100 g. H 2 O dissolve 334.2 g. PrCl 3 +7H 2 O or 103.9 g. of the anhydrous salt at 13. The aqueous solution sat. at 14 has a sp. gr. 16716 = 1.687. At 100, the solubilitv in H 2 O is unlimited. (Matignon, A. ch. 1906, (8) 8. 388.) Sol. in cone. HC1. (von Schule, Z. anorg. 1898, 18. 352.) 100 pts. of a solution of the salt in HCl+Aq contain at 13, 41.05 pts. of anhydrous salt and 7.25 pts. HC1. Sp. gr. of this solution at 16 = 1.574. (Matignon, A. ch. 1906, (8) 8. 388.) Praseodymium hydride, PrH 3 (?). (Muthmann, A. 1904, 331. 59.) Praseodymium hydroxide. Sol. in citric acid. (Baskerville, J. Am. Chem. Soc. 1904, 26. 49.) Praseodymium nitride, PrN. Decomp. in moist air with evolution of NH 3 . (Muthmann, A. 1904, 331. 59.) RADIUM EMANATION 771 Praseodymium oxide, Pr 2 O 3 . Easily sol. in H 2 O. (v. Welsbach, M. 6. 477.) Decomp. by heating in the air. (Scheele, Z. anorg. 1898, 17. 322.) Praseodymium raonoperoxide, Pr(OH) 2 .H 2 O. (Melikoff, Chem. Soc. 1902, 82. (2) 140.) Praseodymium s?;pm>xide, Pr(OH) 2 (OOH). Ppt. (Melikoff, C. C. 1902, I. 172.) Praseodymium trisuperoxide, Pr(OOH) 3 . Ppt. (Melikoff.) Praseodymium peroxide, Pr 4 O 7 . Sol. in acids with evolution of O. (v. Welsbach.) Praseodymium oxy sulphide, Pr 2 SO 2 . (Biltz, Z. anorg. 1911, 71. 436.) Praseodymium ^'sulphide, PrS 2 . Decomp. by heat. (Biltz, Z. anorg. 1911, 71. 437.) Purpureocobaltic salts. For other purpureocobaltic salts, see Chloropurpureocobaltic salts. Bromopurpureocobaltic salts. Nitratopurpureocobaltic salts. Suiphatopurpureocobaltic salts. Purpureocobaltic cobalticyanide, Co(NH 3 ) 5 Co(CN) 6 + l^H 2 O. Insol. in H 2 O. ferricyanide, Co(NH 3 ) 5 Fe(CN) 6 . Insol. in cold H 2 O. Probably belongs to roseo series. mercuric hydroxycbloride, CoN5H u (H g Cl) 3 (HgOH)Cl 3 . Ppt. (Vortmann and Morgulis, B. 22. 2645.) CoN 5 H n (HgOH) 4 Cl 3 . Ppt. (V. and M.) mercuriodide, basic, Co^ 5 H n (HgI 2 ) 2 (HgOH) 3 I 3 . Ppt. SI. sol. in acids. Sol. in KI+Aq. (Vortmann and Borsbach, B. 23. 2804.) ^ molybdate, Co 2 O 3 (NH 3 ) 10 , 7MoO 3 + 3H 2 O (?). Insol. in H 2 O or dil. HC 2 H 3 O 2 +Aq. (Car- not, C. R. 109. 109.) sulphate. See Suiphatopurpureocobaltic salts. tungstate, Co(NH 3 ) 6 O(WO 4 ). Scarcely sol. in cold or hot H 2 O. (Gibbs.) Co 2 O 3 (NH 3 ) 10 , 10WO 3 +9H 2 O (?). Insol. in H 2 O, or dil. HC 2 H 3 O 2 +Aq, or NH 4 OH + Aq. (Carnot, C. R. 109. 147.) Purpureocobaltic vanadate, Co 2 O 3 (NH 3 )io, 5V 2 O 5 +9H 2 O (?). Ppt. Insol. in H 2 O. (Carnot, C. R. 109. 147.) Purpureocobaltic octamine salts. See Octamine cobaltic purpureo salts. Pyrosulphuric acid, H 2 S 2 O 7 . See Disulphuric acid. Radium, Ra. Radium A. More sol than Radium B and C in all solvents; sol. even in organic solvents, espe- cially CS 2 . (Ramstedt, Le Radium, 1913, 10. 159.) Radium B. More quickly sol. than Radium C in H 2 O and acids; less quickly sol. in alkaline solu- tions; very si. sol. in organic solvents. (Ram- stedt, Le Radium, 1913, 10. 159.) Radium C. Sol. in common acids, less so in alkaline solutions and in H 2 O, only very si. sol. in organic solvents. (Ramstedt, Le Radium, 1913, 10. 159; Chem. Soc. 1913, 104. (2) 659.) Radium bromide. Less sol. in H 2 O than corresponding Ba comp. (Curie, Dissert. 1903.) Radium chloride. Less sol. in H 2 O than corresponding Ba coniD. (Curie, Dissert. 1903.) Radium emanation. Coefficient of absorption for H 2 O =0.245 at 3; 0.23 at 20; 0.17 at 40; 0.135 at 60; 0.12 at 70; 0.12 at 80. (Hofmann, Phys. Zeit. 1905, 6. 339.) Solubility in H 2 O at t. Coefficient of solubility = cone, of the emanation in the liquid: cone, of the emana- tion in the gas. t Coefficient of solubility 0.506 4.3 0.424 . 5.7 0.398 10.0 0.340 14.0 0.303 17.6 0.280 20.0 0.245 26.8 0.206 31.6 0.193 39.1 0.160 Coefficient of solubility in sea-water of sp. gr. at 14 = 1.022 is 0.255. (Boyle, Phil. Mag. 1911, (6) 22. 850.) 772 RHODICYANHYDRIC ACID Solubility in H 2 O. Temp. 0.5 17.5 Sol. 0.526 0.283 35 0.183 41 0.161 Temp. Sol. 60 74 79 82 0.127 0.112 0.111 0.111 (Kofler, M. 1913, 34. 389.) 51 0.138 91 0.108 Coefficient of solubility of radium emana- tion at 14 in various solvents. Ethyl alcohol Amyl alcohol Toluene Sea water Mercury 7.34 9.31 13.7 0,255 (Boyle, Phil. Mag. 1911, (6) 22. 851.) Coefficient of solubility emanation of radium in various solvents at t. Solvents t=18 t=o t = 18 Ethyl acetate 7.35 9.41 13.6 Acetone 6.30 7.99 10.8 Absolute alcohol 6.17 8.28 11.4 Aniline 3.80 4.43 Benzene 12.82 16.54 at 3 Chloroform 15.08 20.5 28^5 Cylclohexane 18. 04 at 80 Water 0.285 6!52 Ether 15.08 20.09 29! i Glycerine 0.21 Hexane 16.56 23^4 35^2 Paraffine oil 9.2 12.6 Carbon- bisulphide 23.14 33.4 50.3 Toluene 13.24 18.4 27 Xylene 12.75 (Ramstedt, Le Radium, 1911, 8. 255.) Solubility in various oils, etc., at t. Rape oil Poppy seed oil Oil of turpentine t -3 10 20 100 200 Solubility 51.2 35.3 26.1 6.2 3.3 t Solubility t Solubility -5 16 40 65 90 50.5 30.2 19.1 12.4 8.4 -21 18 50 6.5 42.5 23.1 16.6 7.5 4.08 Solubility in 10% dammar resin in oil of turpentine = 16 . 7 at 18. Solubility in 5% colophony in amyl alcohol = 11. 2 at 20 C . Solubility in amyl alcohol = 10.6 at 18. Solubility in 20% colophony in amyl alcohol = 11.1 at 20. (Curie, Thesis. 1910.) Coefficient of absorption for petroleum = 22.70 at -21. 12.87 at +3. 9.55 at 20. 8.13 at 40. 7.01 at 60. (Hofmann, Phys. Zeit. 1905, 6. 339.) Rhodicyanhydric acid, H 3 Rh(CN) 6 . Not known in the free state. Potassium rhodicyanide, K 3 Rh(CN) 6 . Sol. in H 2 O. Easily decomp. by acids. Very sol. in H 2 O. (Leidi<, C. R. 1900, 130. 89.) Rhodium, Rh. Insol. in all acids, including aqua regia. Rhodium "sponge" is sol. in HNO 3 +Aq, and somewhat in HCl+Aq when exposed to Rhodium ammonia compounds. See Bromopurpureorhodium comps., BrRh(NH 3 ) 6 X 2 . Chloropurpureorhodium comps., ClRh(NH 3 )5X 2 . lodopurpureorhodium comps., ERh(NH.)X* Luteorhodium comps., Rh(NH 3 ) 6 X 3 . Nitratopurpureorhodium comps., (NO 3 )Rh(NH 3 ) 5 X 2 . Roseoihodium comps., Rh(NH 3 ) 5 (OH 2 )X 3 . Xanthorhodium comps., ^ NO 2 )Rh(NH 3 ) 5 X 2 . Rhodium ^bromide, RhBr 3 +2H 2 0. Very sol. in H 2 O. (Goloubkine, Chem. Soc. 1911, 100. (2) 45.) Rhodium rubidium bromide. See Bromorhodite, rubidium. Rhodium sodium bromide. See Bromorhodite, sodium. Rhodium ^chloride, RhCl 2 (?). Insol. in H 2 O, HC1, or HNO 3 +Aq. Not attacked by boiling KOH or K 2 CO 3 +Aq. (Fellenberg.) Decomp. by boiling KOH + Aq. (Berzelius.) Does not exist. (Leidie", C. R. 106. 1076. Rhodium ^n'chloride, RhCl 3 . Insol. in acids, even aqua regia. When boiled for a long time with KOH+Aq, it be- comes si. sol. in HCl+Aq. Insol. in H 2 O and acids; sol. in alkalies+Aq. (Leidie*, C. R. 18P9, 129. 1251.) +4H 2 O. Very si. deliquescent. Easily sol. in H 2 O, HCl+Aq, or alcohol. Insol. in ether. Decomp. by H 2 SO 4 only when boiling. (Glaus, J. pr. 80. 282.) RHOlfoCHROMIUM SULPHATE 773 No definite amount of crystal H 2 O. (Leidie" A. ch. (6) 17. 271.) Rhodium chloride with MCI.. See Cblororhodite, M. Rhodium dzhydroxide, RhO 2 , 2H 2 O, or Rhodium rhodate, Rh 2 O 3 , RhO 3 +6H 2 O. Sol. in HCl+Aq. Rhodium sesgiuhydroxide, Rh 2 O 6 H 6 . Only si. sol. in cone. HCl+Aq. (Glaus.) +2H 2 O. Easily sol. in HC1, H 2 SO 4 , H 2 SO 3 , HNO 3 , or HSCN+Aq; also when moist, in HC 2 H 3 O 2 + Aq. Sol. in cone. KOH + Aq ; very si. sol. in H 3 BO 3 , H 3 PO 4 , H 2 C 4 H 4 O 6 , and HCN +Aq. Sol. in acid alkali oxalates+Aq. (Leidie", C. R. 107. 234.) Rhodium Zniodide, RhI 3 . Ppt. (Goloubkine, Chem. Soc. 1911, 100. (2) 45.) Rhodium monoxide, RhO. Not attacked by acids. (Deville and De- bray, A. ch. (3) 61. 83.) Rhodium ses^wioxide, Rh 2 Os. Insol. in H 2 O, boiling KOH+Aq, or any acid, even aqua regia. (Glaus.) Rhodium dioxide, RhO 2 . Insol. in all acids or alkalies. Rhodium ^noxide, RhO 3 . "Rhodic acid." Known only in solution of " Potassium rhodate," which is very easily decomp. (Glaus.) Rhodium oxybromide, Rh(OH) 2 Br+2H 2 O. Sol. in H 2 O. (Goloubkine, Chem. Soc. 1911, 100. (2) 45.) Rhodium raonosulphide, RhS. Insol. in aqua regia. Rhodium sesgiwsulphide, Rh 2 S 3 . Sol. in alkali sulphides +Aq. (Debray, C. R. 97. 1332.) Insol. in alkali sulphides +Aq. Not at- tacked by HNO 3 , aqua regia, or Br 2 +Aq. (Leidie, Bull. Soc. (2) 50. 664.) Rhodium sodium sulphide, 3Na 2 S, Rh 2 S 3 . Decomp. by H 2 O. (Leidie".) Rhodium sesgiusulphydroxide, Rh 2 S 6 H 6 . Easily sol. in aqua regia or Br 2 +Aq. Insol. in alkali sulphides +Aq or acids. (Leidie", Bull. Soc. (2) 60. 664.) Rhodochromium bromide, HOCr 2 (NH 3 ) 10 Br 5 +H 2 O. Rather difficultly sol. in H 2 O. Decomp. by boiling or standing. Sol. in NH 4 OH+Aq or NaOH+Aq. Insol. in dil. HBr+Aq, KBr+Aq, or alcohol. (Jorgensen, J. pr. (2) 26.321.) bromide, basic, HOCr 2 (NH3) 10 (OH)Br4 +H 2 0. SI. sol. in H 2 O. Sol. in NH 4 OH or NaOH + Aq. Insol. in alcohol. (Jorgensen.) bromoplatinate, HOCr 2 (NH 3 ) 10 Br 3 PtBr6, HOCr 2 (NH 3 ) 10 Br 3 (PtBr 6 ) 2 +4H 2 O. Ppt. (Jorgensen.) chloraurate, HOCr 2 (NH 3 ) 10 Cl 3 (AuCl 4 ) 2 +2H 2 O. Difficultly sol. but not insol. in H 2 O. (Jor- gensen). chloride, HOCr 2 (NH 3 )ioCl 6 +H 2 O. Sol. in about 40 pts. of cold H 2 O. Insol. in cold dil. HCl+Aq, NH 4 Cl+Aq, or alcohol. Sol. in NH 4 OH+Aa. C Jorgensen, J. pr. (2) 25. 321.) chloroiodide, basic, HOCr 2 (NH 3 ) 10 (OH)C1 2 I 2 . SI. sol. in cold H 2 O; insol. in alcohol. (Jorgensen.) chloroplatinate, HOCr 2 (NH 3 )ioCl 3 PtCl 6 , HOCr 2 (NH ? ) 10 Cl(PtCl 6 ) 2 +4H 2 O. Precipitate. (Jorgensen.) dithionate, [HOCro(NH 3 ) 10 ] 2 (S 2 O 6 )5 + 2H 2 O. Nearly insol. in H 2 O. * dithionate, basic, HOCr 2 (NH 3 ) 10 OH(S 2 O 6 ) 2 +H 2 O. Insol. in H 2 O, cold NH 4 OH+Aq, or NaOH+Aq. iodide, HOCr 2 (NH 3 ) 10 I 8 +H 2 O. Very difficultly sol. in H 2 O. Insol. in very dil. HI+Aq or alcohol. SI. sol. in NH 4 OH or KOH+Aq. (Jorgensen.) - nitrate, HOCr 2 (NH 3 ):o(NO 3 ) & . Rather difficultly sol. in H 2 O, from which it is precipitated by a few drops of HNO 3 + Aq. Sol. in hot dil. NH 4 OH+Aq. nitrate chloroplatinate, HOCr 2 (M H 8 ) io(NO 3 ) (PtCl 6 ) 2 +4H 2 O. Precipitate. (Jorgensen.) Rhodochromium sulphate, [HOCr 2 (NH 3 ) 10 ] 2 (SO 4 ) 5 +2H 2 O. Very si. sol. in cold H 2 O. Easily sol. in cold dil. H 2 SO 4 +Aq. 774 RHODONITROUS ACID Almost insol. in a mixture of 3 vols. H 2 O, 1 vol. alcohol, and l / 3 vol. dil. H 2 SO 4 +Aq. (Jorgensen.) Rhodonitrous acid. Ammonium rhodonittite, (NH 4 ) 6 Rh 2 (NO 2 )i 2 . Nearly insol. in cold, si. sol. in hot H 2 O. Insol. in cone. JNH 4 C1 or NH 4 C 2 H3O 2 +Aq. Insol. in alcohol. (Leidie", C. R. 111. 108.) Barium rhodonitrite, Ba 3 Rh 2 (NO 2 )i 2 . SI. sol. in cold, more easily in hot H 2 O. (Lamy.) + 12H 2 O. Sol. in 50 pts. H 2 O at 16, and 6.5 pts. at 100. (Leidie*, C. R. 111. 108.) Potassium rhodonitrite, K 6 Rh 2 (NO 2 ) ]2 . Nearly insol. in cold, very si. sol. in boiling H 2 O. Completely insol. in KNO 2 +Aq, and in KCl+Aq (30% KC1), or KC 2 H 3 O 2 +Aq (50%KC 2 H 3 O 2 ). Insol. in alcohol. (Leidie*, C. R. 111. 106.) Sodium rhodonitrite, Na6Rh 2 (NO 2 ) 12 . Sol. in 2^2 pts. H 2 O at 17, and 1 pt. at 100. Insol. in alcohol. Decomp. by HC1+ Aq. (Leidie", C. R, 111. 107.) Rhodosochromium bromide. Sol. in H 2 O; insol. in dil. HBr+Aq (I : 1). (Jorgensen, J. pr. (2) 46. 260.) chloraurate, Cr 2 (NH 3 ) 6 (HO) 3 Cl3, 2AuCl 3 +2H 2 O. Not insol. in cold H 2 O. (Jorgensen.) chloride, Cr 2 (NH 3 ) 6 (HO) 3 Cl 3 +2H 2 O. Sol. in 10.6 pts. H 2 O at 18; decomp. by boiling. Pptd. by ^ to 1 vol. dil. HCl+Aq. Sol. in cold dil. NH 4 OH+Aq. (Jorgensen, J. pr. (2) 46. 260.) chloroplatinate, 2Cr 2 (NH 3 ) 6 (OH) 3 Cl 3 , 3PtCl 4 +6H 2 O. Insol. in H 2 O. (Jorgensen.) Cr 2 (NH 3 ) 6 (OH) 3 Cl 3 , 2PtCl 4 +2H 2 O. Insol. in 95% alcohol. (Jorgensen.) chromate, [Cr 2 (NH 3 ) 6 (OH) 3 ] 2 (CrO 4 ) 3 + 7H 2 O. (Jorgensen.) Very si. sol. in H 2 O. (Jorgensen.) iodide, Cr 2 (NH 3 ) 6 (OH) 3 I 3 +2H 2 O. Sol. in H 2 O. Insol. in dil. HI+Aq. (Jor- gensen.) nitrate, Cr 2 (NH 3 ) 6 (OH) 3 (NO 3 ) 3 +H 2 O. Much less sol. in cold H 2 O than the chloride. Insol. in dil. HNO 3 +Aq. (Jorgensen.) oxalate, [Cr 2 (NH 3 ) 6 (OH) 3 ] 2 (C 2 4 )(HC 2 4 ) 4 + 2H 2 O. Sol. in cold H 2 O, but not very easily. (Jor- gensen.) Rhodosochromium sulphate, [Cr 2 (NH 3 )6(OH) 3 ] 2 (SO 4 ) 3 +5H 2 O. Very si. sol. in cold H 2 O. Easily sol. in dil. NH 4 Cl+Aq. (Jorgensen.) [Cr 2 (NH 3 ) 6 (OH) 3 ]SCL, HSO 4 +1^H 2 O. De- comp. by H 2 O into H 2 SO 4 and above com- pound. (Jorgensen.) ulphide, [Cr 2 (NH 3 ) 6 (OH) 3 ] 2 S n + Ppt. Insol. in H 2 O. (Jorgensen.) Rhodosulphuric acid. Potassium rhodosulphate, K 6 Rh 2 (SO 4 ) 6 . Two modifications: (a) Slowly sol. in cold, easily in hot H 2 O. (b) Insol. in H 2 O. Does not exist. (Leidie*, C. R. 107. 234.) Sodium rhodosulphate. Insol. in H 2 O, HC1, HNO 3 , or aqua regia. (Claus.) Does not exist. (Leidie".) Na 2 Rh 2 (SO 4 ) 4 . Insol. in H 2 O. (Seubert and Kobbe*, B. 23. 2560.) Rhodosulphurous acid. Potassium rhodosulphite, KeRh 2 (SO 3 ) 5 + 6H 2 0. Nearly insol. in H 2 O. Slowly sol. in acids. Not decomp. by boiling KOH+Aq. (Claus.) Sodium rhodosulphite, Na 6 Rh 2 (SO 3 ) 5 +4^H 2 O = 3Na 2 SO 3 , 2RhSO 3 . Insol. in cold, very si. sol. in hot H 2 O. Easily sol. in HNO 3 +Aq. (Seubert and Kobbe", B. 23. 2558.) Roseochromium bromide, Cr(NH 3 ) 5 Br 3 +H 2 0. Easily sol. in H 2 O. Insol. in HBr+Aq. (Christensen, J. pr. (2) 23. 26.) bromochromate, Cr(NH 3 ) 5 Br(CrO 4 ). Somewhat sol. in H 2 O, but decomp. on standing. (Jorgensen, J. pr. (2) 25. 398.) bromoplatinate, Cr(NH 3 ) 5 Br(PtBr 6 ) + 2H 2 O. Precipitate. Difficultly sol. in H 2 0. (Chris- tensen, I. c.) chloride, Cr(NH 3 ) 5 Cl 3 +H 2 0. Easily sol. in H 2 O with subsequent decomp. Insol. in alcohol. (Christensen, J. pr. (2) 23. 26.) mercuric chloride, Cr(NH 3 ) 5 Cl 3 , 3HgCU +2H 2 O. SI. sol. in H 2 O. Sol. in dil. HCl+Aq with decomposition. (Christensen, I. c.} ROSEOCOBALTIC MERCURIODIDE 775 Roseochromium dithionate, basic, Cr(NH 3 ) 6 (OH) 2 S 2 O 6 +H 2 O. Easily sol. in very dil. HCl+Aq. (Jorgen- sen, J. pr. (2) 25. 398.) iodide, Cr(NH 3 ) 5 l3. Easily sol. in H 2 O; decomp. by boiling. (Christensen, I. c.) nitrate, Cr(NH 3 ) 6 (NO 3 ) 3 +H 2 O. Rather easily sol. in H 2 O. (Christensen, I. c.) Cr(NH 3 ) 5 (NO 3 ) 3 (OH 2 ) 2 , HNO 3 . Decomp. by H 2 O or alcohol. (Jorgensen, J. pr. (2) 44. sulphate, [Cr(NH 3 ) 5 ]2(SO 4 ) 3 +5H 2 O. Easily sol. in H 2 O. Precipitated by alcohol. (Christensen, I. c.) sulphate bromoplatinate, [Cr(NH 3 ) 5 (S0 4 )] 2 PtBr 6 . Difficultly sol, in H 2 O. (Christensen, I. c.) sulphate chloroplatinate, [Cr(NH 3 ) 5 (S0 4 )j 2 PtCl 6 . Difficultly sol. in H 2 O. (Christensen, I. c.) Roseocobaltic bromide, Co(NH 3 ) 5 (OH 2 )Br 3 . Sol. in H 2 O; insol. in HBr+Aq. (Jorgen- sen, J. pr. (2) 31. 49.) 3 bromoplatinate, Co(NH 3 ) 6 (OH 2 )Br3, PtBr 4 +H 2 O. Somewhat sol. in H 2 O or dil. alcohol. Insol in strong alcohol. (Jorgensen.) 2Co(NH 3 ) 5 (OH 2 )Br 3 , 3PtBr 4 +4H 2 O. Ppt. (Jorgensen.) bromosulphate, Co(NH 3 ) 5 (OH 2 )Br(SO 4 ). Sol. inH 2 O. (Krok.) bromosulphate bromaurate, Co(NH 3 ) 5 (OH 2 )(S0 4 )Br, AuBr 3 . carbonate. Very sol. in H 2 O. chloraurate, Co(NH 3 ) 6 (OH 2 )Cl 3 , AuCl 3 . Moderately sol. in cold H 2 O. chloride, Co(NH 3 )5(OH 2 )Cl 3 . Sol. in 4.8 pts. H 2 O at 10.1, but decomp. on heating. 100 pts. H 2 O dissolve 16.12 pts. at 0, and 24.87 pts. at 16.19. (Kurnakoff, J. russ Soc 24. 269.) SI. sol. in 1000 pts. fuming HCl+Aq, more easily in 20% HCl+Aq. (Rose.) Roseocobaltic mercuric chloride, Co(NH 8 ) 6 (OH 2 )Cl3, 3HgCl 2 +H 2 O. More easily sol. in solvents than the anhydrous purpureo salt. (Carstanien.) Co(NH 3 ) 5 (OH 2 )Cl 3 , HgCl 2 . Sol. in HC1+ Aq with decomp. into above salt. (Jorgensen.) chloroplatinate, Co(NH 3 ) 5 (OH 2 )Cl 3 , PtCl 4 +^H 2 0. Decomp. by H 2 O. (Jorgensen.) 2Co(NH)(OHi)Cl,, PtCl 4 +2H 2 0. De- comp. by H 2 O. 2Co(NH 3 ) 5 (OH 2 )Cl 3 , 3PtCl 4 +6H 2 O. Not difficultly sol. in warm H 2 O. (Gibbs.) Co(NH 3 ) 5 Cl 3 , PtCl 4 +H 2 O. (Gibbs.) chlorosulphate, Co(NH 3 )5Cl(SO 4 ). Easily sol. in H 2 O. chlorosulphate mercuric chloride, Co(NH 3 ) 5 Cl(SO 4 ), HgCl 2 +3H 2 O. Sol. in hot H 2 O, and can be recrystallized without decomp. (Krok.) cfa'chromate, [Co(NH 3 ) 5 ] 2 (Cr 2 7 ) 3 +5H 2 0. Can be recrystallized out of weak acetic acid. cobalticyanide,Co(NH 3 )6(OH 2 )Co(CN)6. Nearly absolutely insol. in cold H 2 O. (Jor- gensen.) +H 2 O. (Gibbs and Gentele.) dithionate, Co(NH 3 ) 5 (S 2 O 6 )(OH). Decomp. by H 2 O. (Rammelsberg, Pogg. 58. 296.) Co(NH 3 ) 5 (OH 2 XS 2 6 )+2H 2 0. Ppt. (Jdr- gensen.) hydroxide, Co(NH 2 ) 5 (OH) 3 . Known only in aqueous solution. - mercuric hydroxychloride, CoN 5 H 12 (HgOH) 3 Cl 3 . Ppt. Sol. in dil. acids. (Vortmann and Morgulis, B. 22. 2646.) CoN 6 H 12 (HgOH) 3 Cl 2 (OH). Ppt. Sol. in dil. acids. (Vortmann and Morgulis.) iodide, Co(NH 3 ) 5 (OH 2 )I 3 . Less sol. in H 2 O than bromide. Insol. in HI+Aq. (Jorgensen.) iodosulphate, Co(NH 3 ) 6 (OH 2 )I(SO 4 ). Easily sol. in H 2 O. (Krok.) meicuriodide, [CoN 5 Hi 3 ] 2 (HgI) 3 I 6 . Ppt. (Vortmann and Borsbach, B. 23. 2805.) CoN 6 H 13 (HgI) 2 I 3 . Ppt. (Vortmann and Borsbach.) CoN 6 H 13 (HgI) 2 I 2 (OH). Ppt. 776 ROSEOCOBALTIC NITRATE Roseocobaltic nitrate, Co(NH 3 ) 5 (OH 2 )(N0 3 ) 3 . Three modifications: a. Sol. in 20 pts. H 2 O at 15. (Jorgensen.) /3. Known only in solution. Insol. in cold HNO 3 +Aq. (Gibbs.) 7. Easily sol. in hot H 2 O. (Gibbs.) (Pur- pureo salt ?) Co(NH ? ) 5 (OH 2 )(NO 3 ) 3 , HNO 3 . Decomp. by H 2 O or alcohol. (Jorgensen, J. pr. (2) 44. 63.) nitrate chloroplatinate, Co(NH 3 ) 6 (OH 2 )(NO 3 )Cl 2 , PtCl 4 +H 2 O. Ppt. (Jorgensen.) niti atosulphate, Co(NH 3 ) 5 (OH 2 )(N0 3 )(S0 4 ). SI. sol. in cold, easily in hot H 2 O. oxalate, [Co(NH 3 ) 5 (OH 2 )] 2 (C 2 O 4 ) 3 + 2H 2 O. Nearly insol. in H 2 O. [Co(NH 3 ) 6 ] 2 (C 2 4 ) 3 , 4H 2 C 2 4 . oxalochloroplatinate, [Co(NH 3 ) 5 J 2 C 2 4 Cl 2 , PtCl 4 . Sol. in hot H 2 O. oxalosulphate, [Co(NH 3 ) 6 ] 2 (SO 4 ) 2 C 2 O 4 , H 2 C 2 4 +2H 2 0. Sol. in hot H 2 O. [Co(NH 3 ) 6 ] 2 (SO 4 ) 2 (C 2 O 4 )(OH) 2 +6H 2 O. SI. sol. in H 2 O. orthophosphate, Co(NH 3 ) 5 (OH 2 )(PO 4 H)(OH)+xH 2 O. Nearly insol. in H 2 O. [Co(NH 3 ) 5 (OH 2 )] 2 (Pq 4 H) 3 +4H 2 O. Very si. sol. in cold H 2 O; easily in H 2 O containing HC1. (Jorgensen.) p?/rophosphate, [Co(NH 3 ) 6 (OH,)] 4 (P 2 7 ) 3 .+ 12H 2 0. Insol. in H 2 O. (Jorgensen.) Co(NH 3 ) 6 (OH 2 )(P 2 O 7 ]Na) + 12H 2 O. Nearly insol. in cold, easily sol. in hot H 2 O containing NH 4 OH. (Jorgensen, J. pr. (2) 23. 252.) sulphate, [Co(NH 3 ) 5 (OH 2 )] 2 (SO 4 ) 3 + 3H 2 O. Three modifications: a. SI. sol. in cold H 2 O. Sol. in 58 pts. at 27 (Gibbs); 83.5 pts. at 20.2, and 94.6 pts at 17.2 (Jorgensen); more easily sol. in hot H 2 O, and still more easily in NH 4 OH+Aq. /3. Sol. in 1-2 pts. H 2 O. (Gibbs.) 7. Less sol. than luteosulphate. (Jorgen- sen.) +2H 2 O. Easily sol. in H 2 O. (Vortmann.) Roseocobaltic sulphate, acid, [Co(NH 3 } 6 ] 2 (SO 4 ) r , 2H 2 SO 4 +3H 2 O. (Fremy), or 4[CoCNH)}(SO,},, 9H 2 SO 4 + 11H 2 O (Jorgensen). More easily sol. in H 2 O than neutral sul- phate, into which it is converted by recrystal- lization. Sol. in about 13 pts. H 2 O. (Jorgen- sen.) cerium sulphate, [Co(NH 3 ) 5 (OH 2 )] 2 (S0 4 ) 3 , Ce 2 (S0 4 ) 3 + SI. sol. in cold, practically insol. in boiling H 2 O. Sol. in acids. (Gibbs, Am. Ch. J. 15! 560.) [Co(NH 3 ) 5 (OH 2 )] 2 (S0 4 ) 3 , Ce(S0 4 ) 2 + . As above. (Gibbs.) sulphate chlorauiate. Ppt. Three modifications: a. Co(NH 3 ) 5 (OH 2 )(SO 4 )Cl, AuCl 3 . ( Jorgensen.) /3. CWNH,) 6 (SOi); AuCl 3 +2H 2 O. SI. sol. in cold H 2 O. (Gibbs.) 7. As above. Can be recrystallized from hot H 2 O. sulphate chloioplatinate, 2Co(NH 3 ) 6 (OH 2 )(SO 4 )Cl 2 , PtCl 4 . Three modifications, all difficultly sol. in hot or cold H 2 O. CJorgensen.) sulphite, [Co(NH 3 ) 6 (OH 2 )J 2 (SO 3 ) 3 +H 2 O. SI. sol. in cold, decomp. by hot H 2 O. (Gibbs.) cobaltic sulphite, [Co(NH 3 ) 5 ] 2 (SO 3 ) 3 , Co 2 (SO 3 ) 3 +9H 2 O. Insol. in cold, decomp. by hot H 2 O. (Kiin- zel.) Roseocobaltic octamine compounds. See Roseotetramine cobaltic compounds. Roseoiridium compounds. See Iridoaquopentamine compounds. Roseorhodium bromide, Rh(NH 3 ) 5 (OH 2 )Br 3 . Sol. in cold H 2 O. (Jorgensen, J. pr. (2) 34. 394.) Roseorhodium cobalticyanide, Rh(NH 3 ) 5 (OH 2 )Co(CN) 6 . Scarcely sol. in H 2 O. iodosulphate, Rh(NH 3 ) 6 (OH 2 )I(SO 4 ). Very si. sol. in H 2 O; easily sol. in NH 4 OH + Aq. (Jorgensen.) nitrate, Rh(NH 3 ) 5 (OH 2 )(NO 3 ) 3 . Moderately sol. in cold H 2 O. (Jorgensen.) Rh(NH 3 ) 6 (OH 2 )(NO 3 ) 3 , HNO 3 . Decomp. RUBIDIUM BROMIDE 777 by H 2 O or alcohol. (Jorgensen, J. pr. (2) 44. 63.) Roseorhodium nitrate chloroplatinate, [Rhf NH 3 ) 5 ( OH 2 ) (NO,)] 2 PtCl 6 +2H 2 O . Ppt. (Jorgensen.) or/ftophosphate, [Rh(NH 3 ) 6 (OH 2 )] 2 (HP0 4 ) 3 +4H 2 0. Very si. sol. in H 2 O. sodium p7/rophosphate, [Rh(NH 3 ) 5 (OH 2 )] 2 NaP 2 O 7 +23H 2 O. Ppt. Very si. sol. in cold H 2 O. Easily sol. in very dil. acids. sulphate, lRh(NH 3 ) 5 (OH 2 ) 2 ](SO 4 )3+3H 2 O. Very si. sol. in cold, much more in hot H 2 O. sulphate chloroplatinate, Rh(NH 3 ) 5 (OH 2 )(SO 4 )PtCl 6 . Ppt. Nearly insol. in H 2 O or alcohol. Roseotetramine cobaltic bromide, Co(NH 3 ) 4 (OH 2 ) 2 Br 3 . Sol. in H 2 O; insol. in HBr+Aq. Nearly in- sol. in alcohol. (Jorgensen, Z. anorg. 2. 295.) chloride, Co(NH 3 ) 4 (OH 2 ) 2 Cl 3 . Easily sol. in H 2 O; insol. in cone. HCl+Aq; sol. in sat. HgCl 2 +Aq. (Jorgensen.) cobalticyanide, Co(NH 3 ) 4 (OH 2 ) 2 Co(CN) 6 . (Jorgensen.) oxalate sulphate, [Co(NH 3 ) 4 (OH 2 ) 2 MS0 4 ) 2 C 2 4 . Ppt. ( Jorgensen.) -- p2/rop [Co(NH 3 ) 4 (OH 2 ) J 4 (P 2 7 ) , +6H 2 0. Nearly insol. in H 2 O, but easily sol. in very dil. acids +Aq. (Jorgensen.) --- sulphate, [Co(NH 3 ) 4 (OH 2 ) 2 ] 2 (S0 4 ) 3 +3H 2 0. Sol. in about 35 pts. H 2 O, and more easily by addition of dil. HC1 or H 2 SO 4 +Aq. (Jor- gensen.) --- sulphate bromaurate. [Co(NH 3 ) 4 (OH 2 ) 2 ] 2 (S0 4 ) 2 AuBr 4 . SI. sol. in cold H 2 O; insol. in alcohol. (Jorgensen.) sulphate chloroplatinate, [Co(NH 3 ) 4 (OH 2 ) 2 ] 2 (SO 4 ) 2 PtCl 6 . As the bromaurate. (Jorgensen.) Rubidium, Rb 2 . Decomp. H 2 O with violence. Insol. in hydrocarbons. Sol. in liquid NH 3 . (Seely, C. N. 23. 169); (Franklin, Am. Ch. J. 1898, 20. 829). Rubidium acetylide acetylene RbC 2 , C 2 H 2 . Very hygroscopic. Insol. in CC1 4 and in ether. (Moissan, C. R. 1903, 136. 1220.) Rubidium amalgam, RbHgi 2 . Stable in contact with Hg below 0. Above the composition of the amalgam varies. Can be cryst. from Hg without de- comp. below 0. (Kerp, Z. anorg. 1900, 26. 68.) Rubidium amide, RbNH 2 . Very deliquescent. Violently decomp. by H 2 O; less violently acted on by alcohol. (Titherley, Chem. Soc. 1897, 71. 470.) Rubidium ammonia, RbNH 3 . Decomp. by H 2 O. Very sol. in liquid NH 3 . (Moissan, C. R. 1903, 136. 1178.) Rubidium azoimide, RbN 3 . SI. hydroscopic. Stable in aq. solution. 107. 1 pts. are sol. in 100 pts. H 2 O at 16. 114.1 " " " " 100 " H 2 O " 17. 0.182 " " " "100 " abs. alcohol at 16. Insol. in pure ether. (Curtius, J. pr. 1898, (2) 68. 281.) Rubidium bromide, RbBr. 100 pts. H 2 O dissolve 98 pts. at 5; 104.8* pts. at 16. (Reissig, A. 127. 33.) Solubility in H 2 O. 100 pts. of the solution contain at: 0.5 5.0 16.0 47.26 49.50 51 . 17 pts. RbBr, 39.7 57.5 113.5 56 .87 60 . 39 67 . 24 pts. RbBr. (Rimbach, B. 1905, 38. 1557.) Sp. gr. of RbBr containing g. equiv. RbBr per 1. G. equiv. RbBr Sp.gr. 6/6 Sp. gr. 18,' 18 Sp. gr. 30/30 0.508 1.020 2.031 4.072 1.06448 1.12931 1.25622 1.50574 1.06389 1.12799 1.25366 1.50107 1.06326 1.12626 1.25187 1.49870 (Clausen, W. Ann. 1914, (4) 44. 1070.) 778 RUBIDIUM BROMIDE RbBr+Aq. containing 6.60% RbBr has sp.gr. 20/20 = 1.0525. RbBr+Aq. containing 14.36% RbBr has sp. gr. 20/20 = 1.1226. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 279.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) Insol. in methyl acetate. (Naumann, B. 1909,42.3790.) Rubidium ^n'bromide, RbBr 3 . Very sol. in H 2 O; decomp. by alcohol and ether. (Wells and Wheeler, Sill. Am. J. 143. 475.) Rubidium ruthenium bromide. See Bromoiuthenate and bromoruthenite, rubidium. Rubidium seleDium bromide. See Bromoselenate, rubidium. Rubidium tellurium bromide. See Biomotellurate, rubidium. Rubidium thallic bromide, RbBr, TlBr 3 +H 2 O. Recryst. from H 2 O unchanged. (Pratt, Am. J. Sci. 1895, (3) 49. 403.) 3RbBr, TlBr,+H 2 O. Very sol. in H 2 O. (Pratt.) Rubidium stannic bromide. See Bromostannate, rubidium . Rubidium bromochloiide, RbBr 2 Cl. Easily decomp., even by H 2 O. (Wells and Wheeler.) RbBrCl 2 . Sol. in H 2 O; decomp. by alcohol and ether. (Wells and Wheeler.) Rubidium bromochloroiodide, RbBrClI. Sol. in H 2 O and alcohol. Decomp. by ether. (Wells and Wheeler.) Rubidium bromoiodide, RbBr 2 I. Very sol. in H 2 O. Sat. solution contains about 44% RbBr 2 I, and sp. gr. = 3.84. (Wells and Wheeler.) Rubidium carbide, Rb 2 C 2 . Decomp. violently by H 2 O. (Moissan, C. R. 1903,136. 1221.) Rubidium chloride, RbCl. 100 pts. H 2 O dissolve 76.38 pts. at 1; 82.89 pts. at 7. (Bunsen.) Solubility in H 2 O at t. 100 pts. of the solution contain pts. RbCl. t Pts. RbCl 0.4 15.5 57.3 114.9 43.61 46.56 53.71 59.48 (Rimbach, B. 1902, 36. 1304.) Solubility of RbCl in H 2 O at t. t G. RbCl per 100 g. t G, RbCl per 100 g. H 2 6 Solution H 2 Solution 10 20 30 40 50 77.0 84.4 91.1 97.6 103.5 109.3 43.5 45.8 47.7 49.4 50.9 52.2 60 70 80 90 100 112.9 115.5 121.4 127.2 133.1 138.9 146.6 53.6 54.8 56.0 57.1 58.9 59.5 (Berkeley, Phil. Trans. Roy. Soc. 1904, 203, A. 189.) Sat. RbCl+Aq at 25 contains 48.57% RbCl. (Foote, Am. Ch. J. 1906, 35. 242.) Sp. gr. of RbCl+Aq containing in 100 pts. H 2 0: 13 .14 25 . 88 33 . 13 pts. RbCl. 1.1066 1.2156 1.2675 sp.gr. (Tammann, W. Ann. 24. 1885.) A normal solution of RbCl has sp. gr. at 25 = 1.0610. (Wagner, Z. phys. Ch. 1890, 5. 39.) RbCl+Aq containing 6.64% RbCl has sp. gr. 20/2C = 1.0502. RbCl+Aq containing 10.59% RbCl has sp gr 20720 = 1.0815. (Xe Blanc and Roh- land, Z. phys. Ch. 1896, 19. 278.) Sp. gr. 20/4 of a normal solution of RbCl = 1.085405. (Haigh, J. Am. Chem. Soc. 1912, 34. 1151.) Sp. gr. of RbCl+Aq sat. at t. t Sp. gr. t Sp. gr. 0.55 18.7 31.5 44.7 1.4409 1.4865 1.5118 1.5348 60.25 75.15 89.35 114* 1.5558 1.5746 1.5905 1.6148 * Boiling point. (Berkeley.) Sp. gr. of RbCl containing g. equiv. RbCl perl. G. equiv. RbCl Sp. gr. 6/6 Sp. gr. 18/18 Sp. gr. 30/30 0.5123 1.001 2.073 3.984 1.06410 1.08916 1.18200 1.34334 1.04538 1.08810 1.17959 1.33967 1.04503 1.08749 1.17828 1.33757 (Clausen, W. Ann. 1914, (4) 44. 1069J RUBIDIUM URANYL FLUORIDE 779 Very si. sol. in liquid NH 3 . (Franklin, Am. Ch. Jf 1898, 20. 829.) Solubility in alcohols at 25. 100 g. methyl alcohol dissolve 1.41 g. 100 g. ethyl alcohol dissolve 0.078 g. 100 g. propyl alcohol dissolve 0.015 g. 100 g. isoamyl alcohol dissolve 0.0025 g. (Turner and Bissett, Chem. Soc. 1913, 103. 1909.) Insol. in anhydrous pyridine and in 97% pyridine+Aq. Very si. sol. in 95% pyridine +Aq; si. sol. in 93% pvridine+Aq. (Kah- lenberg, J. Am. Chem. Soc. 1908, 30. 1107.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790);acetone; (Naumann, B. 1904, 37. 4329); (Eidmann, C. C. 1899, II. 1014). Rubidium ruthenium ^chloride. See Chlororuthenite, rubidium. Rubidium ruthenium tetrachloride. See Chlororuthenate, rubidium. Rubidium oxyruthenium chloride, Rb 2 RuO 2 Cl 4 . Ppt.; decomp. by H 2 O; sol. in cold HC1. (Howe, J. Am. Chem. Soc. 1901, 23. 779.) Rubidium tellurium chloride. See Chlorotellurate, rubidium. Rubidium thallic chloride, 2RbCl, T1C1 3 + H 2 O. Can be recryst. from H 2 O without change (Pratt, Am. J. Sci. 1895, (3) 49. 399.) 3RbCl, T1C1 8 . Crystallizes from HC1 solu- tion. (Neumann, A. 244. 348.) +H 2 O. Very sol. in cold H 2 O. (Pratt Am. J. Sci. 1895, (3) 49. 398.) +2H 2 O. Efflorescent in dry air. Sol. in 7.5 pts. H 2 O at 18, and 1.6 pts. at 100. (Godeffroy, Zeitschr. d. allgem. osterr. Apothekerv. 1880. No. 9.) Rubidium stannic chloride. See Chlorostannate, rubidium. Rubidium titanium chloride, 2RbCl, TiCl 3 Sol. in H 2 O. (Stabler, B. 1904, 37. 4408.) Rubidium tungsten chloride, Rb 3 W 2 Cl 9 . SI. sol. in cold, more sol. in hot H 2 O. Sol. in very dil. NaOH+Aq. Nearly insol. in most organic solvents. (Olsson, B. 1913, 46. 574.) Rubidium uranous chloride, Rb 2 UCl 6 . As K salt. (Aloy, Bull. Soc. 1899, (3) 21. 264.) Rubidium uranyl chloride, 2RbCl, (UO 2 )C1 2 +2H 2 O. Solubility in H 2 O. 100 pts. of the solution contain at: 24.8 80.3 57 . 8 65 . 73 pts. UO 2 C1 2 , 2RbCl. (Rimbach, B. 1904, 37. 467.) Rubidium vanadium chloride, Rb 2 VCl 5 +H 2 0. SI. sol. in H 2 O and alcohol. Decomp. by H 2 O on standing so that it dissolves. (Stabler, B. 1904, 37. 4411.) Rubidium zinc chloride, 2RbCl, ZnCl 2 . Easily sol. in H 2 O and HCl+Aq. (Godef- froy, B. 8. 9.) Rubidium chloride selenium dioxide, RbCl, 2SeO 2 +2H 2 O. Sol. in H 2 O. (Muthmann, B. 1893, 26. 1013.) Rubidium chloroiodide, RbCl 2 I. Properties are similar to those of RbBrClI. (Wells.) RbCl^. Sol. in alcohol, not attacked by ether. (Wells and Wheeler, Sill. Am. J. 144. 42.) Sol. in POC1 3 . (Walden, Z. anorg. 1900, 25. 212.) Nearlv insol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Very stable; si. sol. in H 2 O at 0; only very si. sol. in BCJl. (Erdmann, Arch. Pharm. 1894, 232. 32.) (C. C. 1894, I. 670.) Rubidium fluoride, RbF. Very sol. in H 2 O. (Eggeling, Z. anorg. 1905, 46. 174.) 100 g. H 2 O dissolve 130.6 g. RbF at 18. (de Forcrand, C. R. 1911, 152. 1210.) Sol. in dil. HF. (Pennington, J. Am. Chem. Soc. 1896, 18. 57.) Insol. in liquid NH 3 . (Core, Am. Ch. J. 1898, 20. 829.) Rubidium hydrogen fluoride, RbF, HF. Very deliquescent. Insol. in alcohol and ether. (Chabrie*, C. R. 1905, 140. 91.) Very hygroscopic. Sol. in H 2 O. (Eggeling, Z. anorg. 1905, 46. 175.) RbF, 2HF. Very si. sol. in H 2 O. (Egge- ling, Z. anorg. 1905, 46. 176.) Rubidium silicon fluoride. See Fluosilicate, rubidium. Rubidium tantalum fluoride. See Fluotantalate, rubidium. Rubidium uranyl fluoride, 4RbF, UO 2 F 2 + 6H 2 O. (Ditte, C. R. 91. 115.) 780 RUBIDIUM HYDRIDE Rubidium hydride, RbH. Decomp. by H 2 O with evolution of H 2 . (Moissan, C. R. 1903, 136. 589.) Rubidium hydroxide, RbOH. Deliquescent, and very sol. in H 2 O. Sol. in alcohol. (Bunsen.) Sat. RbOH+Aq contains 64.17% RbOH at 15. (de Forcrand, C. R. 1909, 149. 1344.) Rubidium iodide, Rbl. 100 pts. H 2 O dissolve 137.5 pts. at 6.9; 152 pts. at 17.4. (Reissig, A. 127. 33.) Sat. Rbl+Aq. at 25 contains 61.93% Rbl. (Foote and Chalker, Am. Ch. J. 1908, 39. 567.) Sp. gr. of Rbl+Aa containing: 5% 10% cold hot sat. sat. Sp.gr. 1.0353 1.0755 1.726 1.9629. (Erdmann, Arch. Pharm. 1894, 232. 25.) Sp. gr. of Rbl+Aq containing g. equiv. Rbl per I, G. equiv. Rbl Sp. gr. 6/6 Sp. gr. 18/18 Sp. gr. 30/30 0.510 1.025 2.025 4.015 1.08347 1.16751 1.33012 1.64781 1.08268 1 . 16569 1.32637 1.64144 1.08226 1 . 16433 1.32531 1.63780 (Clausen, W. Ann. 1914, (4) 44. 1070.) Nearly insol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Sol. in AsCl 3 . (Walden, Z. anorg. 1900, 26. 214); liquid SO 2 . (Walden, Z. anorg. 1902, 30. 161); S 2 C1 2 . (Walden, Z. anorg. 1900, 25. 217): SO 2 C1 2 . (Walden); POC1 3 . (Walden.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Solubility in organic solvents at t. C = pts. by wt.of Rbl in 100 ccm. of the sat. solution. L = no. of litres which at the saturation temp, hold in solution 1 mol. Rbl. Solvent t C L Furfurol 25 4.93 4.31 Acetonitrile 25 1.350 15.73 ii 1.478 14.36 Propionitrile 25 0.305 69.61 " 0.274 77.48 Nitro methane 25 0.518 41.00 a 0.567 37.44 Acetone 25 0.674 31.5 I 0.960 22.1 (Walden, Z. phys. Ch. 1906, 55. 718.) Rubidium raodide, RbI 3 . Very sol. in H 2 O. Sol. in about V pt. H 2 O at 20; sol. in alcohol. Decomp. by ether. (Wells and Wheller, Sill. Am. J. 143. 475.) Solubility determinations show that RbI 3 is the only polyiodide of rubidium formed at 25. Rbl 7 and RbI 9 , mentioned by Abegg and Hamburger, (Z. anorg. 50, 403) could not be obtained. (Foote and Chalker, Am. Ch. J. 1908, 39. 567.) Rubidium silver iodide, 2RbI, Agl. Easily decomp. by H 2 O. (Wells and Wheeler, Sill. Am. J. 144. 155.) Rbl, AgI + V2H 2 O. (Marsh, Chem. Soc. 1913, 103. 783.) Rbl, 2AgI. Not deliquescent. Very sol. in acetone. (Marsh, Chem. Soc. 1913, 103. 783.) Rubidium tellurium iodide. See lodotellurate, rubidium. Rubidium thallic iodide, Rbl, T1I 3 +2H 2 O. Decomp. by H 2 O. (Pratt, Am. J. Sci. 1895, (3) 49. 403.) Rubidium nitride, Decomp. by heat. (Franz Fischer, B. 1910, 43. 1468.) See also Rubidium azoimide. Rubidium dioxide, Rb0 2 . Decomp. by H 2 O. (Erdmann, A. 1897, 294. 68.) Rubidium sulphide, Rb 2 S+4H 2 O. Deliquescent; very sol. in H 2 O. Z. anorg. 1906, 48. 299.) (Biltz, Rubidium bisulphide, Rb 2 S 2 . Anhydrous. Sol. in H 2 O. Very hydroscopic. (Biltz, Z. anorg. 1906, 50. 72.) " +H 2 O. From Rb 2 S 2 +Aq. Hydroscopic. (Biltz.) Rubidium bisulphide, Rb 2 S 3 . Anhydrous. Sol. in H 2 O. Hydroscopic. (Biltz, Z. anorg. 1906, 50. 75.) +H 2 O. From Rb 2 S 3 +Aq. (Biltz.) Rubidium tefrasulphide Rb 2 S 4 +2H 2 O. Sol. in H 2 O. (Biltz, Z. anorg. 1906, 48. 304.) Rubidium pewtosulphide, Rb 2 Ss. Deliquescent. Decomp. by H 2 O. Very easily sol. in 70% alcohol. Insol. in ether, ethyl sulphide or CHC1 3 . (Biltz, B. 1905, 38. 127.) RUTHENIUM NITROSOOXIDE 781 Rubidium hydrogen sulphide, RbHS. Deliquescent, very sol. in H 2 O. (Biltz, Z. anorg. 1906, 48. 300.) Rubidium copper tefrasulpbide, RbCuS 4 . Decomp. very slowly in the air. SI. sol. in H 2 O. Very slowly decomp. by cold cone., more rapidly by hot cone., and still more rapidly by dil. HC1, H 2 SO 4 and HNO 3 . SI. sol. in alcohol. (Biltz, B. 1907, 40. 978.) Ruthenic acid. Barium ruthenate, BaRuO 4 +H 2 O. Ppt. (Debray and Joly, C. R. 106. 1494.) Calcium ruthenate, CaRuO 4 .* Ppt. Magnesium ruthenate, MgRuO 4 . Ppt. Potassium ruthenate, K 2 RuO 4 +H 2 O. Very sol. in H 2 O. Perruthenic acid. Potassium perruthenate, KRuO 4 . SI. sol. in HoO. (Debray and Joly, C. R. 106. 1494.) Sodium perruthenate, NaRuO 4 +H 2 O. SI. sol. in H 2 O. Ruthenium, Ru. Not attacked by acids, except aqua regia, which dissolves it only very slightly. (Glaus, Pogg. 65. 218.) Ruthenium ammonium comps. See Ruthenoefo'amine comps, etc. Ruthenium ^n'bromide, RuBr 3 . Sol. in H2O. Solution decomposes slowly on standing, but rapidly on heating. (Gut- bier, Z. anorg. 1905, 46. 178.) Ruthenium ^nbromide, ammonia, 2RuBr 3 , 7NH 3 . Sol. in H 2 O and ammonia with slight warm- ing. Insol. in alcohol. (Gutbier, Z. anorg. 1905, 45. 182.) Ruthenium cfo'chloride, RuCl 2 . Insol. in acids, even in aqua regia. SI. attacked by acids. Traces are dissolved by boiling with cone. KOH+Aq. 4-#H 2 O. Known only in aqueous solution. (Glaus, A. 59. 238.) Ruthenium ^n'chloride, RuCl?. Deliquescent. Sol. in H 2 O and alcohol, but solution is decomp. by heating into Ru 2 O 3 and HC1. (Glaus.) Pure RuCl 3 is insol. in cold H 2 O, mineral, or organic acids. Slowly decomp. by boiling H 2 O. Insol. in CC1 4 , CS 2 , CHC1 3 /PC1 3 , or ether. Slowly sol. in hot absolute alcohol, but decomp. into Ru(OH)Cl 2 by 95% alco- hol. (Joly, C. R. 114. 292.) Hydroscopic. Sol. in H 2 O; decomp. at 50. Sol. in alcohol. (Gutbier, Z. anorg. 1905, 45. 174.) See also Ruthenium nitrosochloride. Ruthenium ^rachloride, RuCl 4 . Sol. in H 2 O and alcohol. (Glaus.) Ruthenium trichloride with MCI. See Chlororuthenite, M. Ruthenium te^rachloride with MCI. See Chlororuthenate, M. Ruthenium sesgznhydroxide, Ru 2 O 6 H 6 . Sol. in acids; insol. in alkalies. Less sol. in NH 4 OH+Aq than any other oxide of the Pt metals. (Glaus.) Ruthenium ^'hydroxide, RuO 4 H 4 +3H 2 O. Sol. in acids and alkalies. (Glaus, A. 59. 237.) Contains NO. Joly, C. R. 107. 994.) Ruthenium ^n'odide, RuI 3 . Ppt. (Glaus.) Insol. in H 2 O, KI+Aq, and aldohol. (Gutbier, Z. anorg. 1905, 45. 181.) Ruthenium Iniodide ammonia, 2RuI 3 , 7NH 3 . Sol. in H 2 O and ammonia with slight warm- ing. Insol. in alcohol. (Gutbier, Z. anoig. 1905, 45. 182.) Ruthenium nitrosochloride, RuCl 3 (NO) + H 2 O, and 5H 2 O. Slowly sol. in cold, easily in hot H 2 O. (Joly, C. R. 108. 855.) Ruthenium efthydronitrosochloride, NO.Ru 2 H 2 Cl 3 , 2HC1. Sol. in H 2 O. (Brizard, A. ch. 1900, (7) 21. 353.) Ruthenium silver nitrosochloride, NO.Ru 2 H 2 Cl 3 , 2HC1, 3AgCl. Ppt. (Brizard, A. ch. 1900, (7) 21, 357.) Ruthenium nitrososesom'oxide, Ru 2 O 3 (NO) 2 +2H 2 0. Ppt. (Joly, C. R. 108. 854.) 782 RUTHENIUM HYDRONITROSOHYDROXIDE Ruthenium cfthydronitrosohy dioxide, NO.Ru 2 H 2 (OH) 3 +2H 2 O. SI. sol. in cold H 2 O with decomp. (Briz- ard, A. ch. 190C, (7) 21. 349.) Ruthenium cfohydronitrosooxychloride, NO.Ru 2 H 2 Cl 2 OH+2H 2 O. Ppt. (Brizard, A. ch. 1900, (7) 21. 349.) Ruthenium monoxide, RuO. Insol. in acids. (Glaus, A. 59. 236.) Ruthenium sesgm'oxide, Ru 2 O 3 . Insol. in acids. Mixture of Ru and RuO 2 . (Debray and Joly, C. R. 106. 1494.) See Ruthenium nitrososesgwioxide. Ruthenium dioxide, RuO 2 . Insol. in acids. (Debray and Joly.) Ruthenium ^noxide, RuO 3 . "Ruthenic acid." Known only in its salts. Ruthenium te/roxide, RuO 4 . Rather difficultly and slowly sol. in H 2 O. (Glaus.) Decomp. in aqueous solution into Ru 2 O 5 + 2H 2 O. (Debray and Joly.) Ruthenium pentoxide, Ru 2 O 6 . (Debray and Joly, C. R. 106. 1494.) +2H 2 O. Ppt. (Debray and Joly.) Ruthenium heptoxide, Ru 2 O 7 . "Pemithenic acid." Known only in its salts: Ruthenium oxide, Ru 4 O s . (Debray and Joly.) Ruthenium oxychloride, Ru(OH)Cl 2 . Very sol. in H 2 O, but decomp. by an excess. (Joly, C. R. 114. 293.) Ruthenium silicide, RuSi. Insol. in boiling acids; slowly attacked by a mixture of fused KHSO 4 and KNO 3 . (Moissan, C. R. 1903, 137. 231.) Ruthenium bisulphide, RuS 3 . Ppt. (Antony, Gazz. ch. it. 1900, 30. 539.) Ruthenomonamine hydroxide, Ru(OH) 2 (NH 3 ) 2 +4H 2 O. See Ruthenosamine hydroxide. Ruthenocfo'amine carbonate, Ru(N 2 H 6 ) 2 CO 3 +5H 2 O. Easily sol. in H 2 O. Insol. in alcohol. (Glaus.) Ruthenoc&amine chloride, Ru(N 2 H 6 Cl) 2 +3H 2 O. Not very sol. in cold, easily sol. in hot H 2 O. Insol. in alcohol. See Ruthenonitrosocfo'amine comps. mercuric chloride, Ru(N 2 H 6 Cl) 2 , HgCl 2 . Nearly insol. in cold, sol. in hot H 2 O. (Gibbs, Sill. Am. J. (2) 34, 350.) chloroplatinate, Ru(N 2 H 6 Cl) 2 , PtCl 4 . SI. sol. in H 2 O. (Glaus.) hydroxide, Ru(N 2 H 6 OH) 2 . Known only in aqueous solution. nitrate, Ru(N 2 H 6 NO 3 ) 2 +2H 2 O. Somewhat difficultly sol. in cold, easily in hot H 2 O. Insol. in alcohol. sulphate, Ru(N 2 H 6 ) 2 SO 4 +4H 2 O. Moderately sol. in H 2 0. Insol. in alcohol. (Glaus.) Ruthenocyanhydric acid, H 4 Ru(CN) 6 . Easily sol. in H 2 O and alcohol. Less sol. in ether. (Glaus, J. B. 1866. 444.) Potassium ruthenocyanide, K 4 Ru(CN) 6 + 3H 2 O. SI. efflorescent. Very sol. in H 2 0; si. sol. in dil. alcohol. (Glaus.) Ruthenonitrosocfa'amine bromide, Ru(NO)(NH 3 ) 4 Br 3 . SI. sol. in H 2 O. (Joly, C. R. 111. 969.) Ru(NO)OH(NH 3 ) 4 Br 2 . Less sol. than cor- responding chloride. (Joly, C. R. 108. 300.) chloride, Ru(NO)(NH 3 ) 4 Cl 3 . SI. sol. in H 2 O. (Joly, C. R. 111. 969.) Ru(NO)OH(NH 3 ) 4 Cl 2 . Sol. in H 2 O. (Joly, C. R. 108. 1300.) Ru(NO)(NH 3 ) 4 Cl 3 +2H 2 O = Ru(NO)(OH)(NH 3 ) 4 Cl 2 , HC1+H 2 O (?). Very sol. in H 2 O. (Joly, C. R. 111. 969.) chloroplatinate, Ru(NO)OH(NH 3 ) 4 PtCl 6 . Scarcely sol. in boiling H 2 O. (Joly, C. R. 108. 1300.) Ru(NO)(NH 3 ) 4 Cl 3 , PtCl 4 . Ppt. (Joly, C. R. 111. 969.) iodide, Ru(NO)(NH 3 ) 4 I 3 . SI. sol. in H 2 O. (Joly, C. R. 111. 969.) Ru(NO)OH(NH 3 ) 4 I 2 . Less sol. than the corresponding bromide. (Joly, C. R. 108. 1300.) nitrate, Ru(NO)(NH 3 ) 4 (NO 3 ) 3 . . More sol. in H 2 O than Ru(NO)(OH)(NH,) 4 (NO 8 ) 2 . (Joly, C. R. 111. 969.) SCANDIUM HYDROXIDE 783 Ru(NO)OH(NH 3 ) 4 (NO 3 ) 2 . SI. sol. in cold H 2 O; insol. in cone. HNO 3 +Aq. (Joly, C. R. 108.1300.) Ruthenonitrosocfaamine sulphate, [Ru(NO)(NH 3 )4]2(SO 4 ) 3 + 10H 2 O. SI. sol. in H 2 O. (Joly, C. R. 111. 969.) [Ru(NO)(NH 3 ) 4 ]4(SO 4 )6, H 2 SO 4 +H 2 O. De- comp. by cold H 2 O. (Joly.) Ru(NO)(OH) 4 (NH 3 ) 4 SO 4 +H 2 O. Most sol. in H 2 O of this class of salts. (Joly, C. R. 108. 1300.) Ruthenonitrous acid. Ammonium ruthenonitrite, RuH 2 (NO 2 ) 4 , 3NH 4 NO 2 +2H 2 O. Easily sol. in H 2 O; practically insol. in KCl+Aq. (Brizard, A. ch. 1900, (7) 21. 368.) Potassium ruthenonitrite, K 6 Ru 2 (NO 2 ) 12 = 6KN0 2 , Ru 2 (NO 2 ) 3 . Easily sol. in H 2 O, alcohol, or ether. (Gibbs, Sill. Am. J. (2), 34. 344.) SI. sol. in H 2 O. Easily sol. in KNO 2 +Aq. (Glaus.) K 4 Ru 2 (NO 2 )io = Ru 2 O 2 (N 2 O 3 ) 3 , 4KNO 2 . Very sol. in H 2 O. (Joly and Vezes, C. R. 109. 667!) K 8 Ru 2 (NO 2 ) 14 = Ru 2 O 2 (N 2 O 3 ) 2 ,8KNO 2 . SI. sol. in H 2 O. Sol. in cold dil. acids. (Joly and Vezes.) Ru 2 H 2 (NO 2 ) 4 , 3KNO 2 +4H 2 O. Very sol. in H 2 O. Aqueous solution decomp. si. on long boiling. Almost insol. in cone. KCl-j- Aq. (Brizard, C. R. 1899, 129. 216.) SUver ruthenonitrite, NO.Ru 2 H 2 (NO 2 ) 4 , 3AgNO 2 +2H 2 O. Ppt. (Brizard, A. ch. 1900, (7) 21. 368.) Sodium ruthenonitrite, Ru 2 (N0 2 ) 6 , 4NaNO 2 + 4H 2 O. Very sol. in H 2 O without decomp. (Joly, C. R. 1894, 118. 469.) Ruthenosamine hydroxide, Ru(NH 3 OH) 2 +4H 2 O (?). Very deliquescent, and sol. in H 2 O. (Glaus.) Samarium, Sm. The element has not been isolated. Samarium bromide, SmBr 3 +6H 2 O.. Very deliquescent. (Cleve.) Samarium carbide, SmC 2 . Decomp. by water and acids. (Moissan, C. R. 1900, 131. 925.) Samarium bichloride, SmCl 2 . Decomp. by H 2 O with liberation of H 2 and formation of samarium oxide and samarium oxy chloride. Insol. in CS 2 , CHC1 3 , benzene, abs. alcohol, pyridine and toluene. (Matig- non, C. R. 1906, 142. 85.) Samarium ^nchloride, SmCl 3 . The anhydrous salt is very hydroscopic and easily sol. in H 2 O. (Matignon, C. R. 1902, 134. 1309.) Very sol. in H 2 O. Very sol. in abs. alcohol. 6.38 g. are sol. in 100 grams pyridine at ord. temp.; insol. in quinoline. (Matignon, A. ch. 1906, (8) 8. 406.) +3H 2 O. Deliquescent. Samarium chloride ammonia, SmCl 3 +NH 3 ; +2NH 3 ; +3NH 3 ; +4NH 3 ; +5NH 3 ; +8NH 3 ; +9.5NH 3 ; +11.5NH 3 . (Matignon, C. R. 1905, 140. 143.) Samarium fluoride, Precipitate. Insol. in H 2 O and dil. acids. (Cleve.) Samarium iodide, SmI 3 . (Matignon, A. ch. 1906, (8) 8. 413.) Samarium hydroxide, Sm 2 (OH) 6 . Insol. in alkalies; easily sol. in acids, and decomposes ammonium salts. (Cleve, C. N. 61. 145.) Samarium oxide, Sm 2 O 3 . Easily sol. in acids. (Cleve, C. N. 51. 145.) Samarium peroxide, Sm 4 O 9 . Precipitate. (Cleve.) Samarium oxy chloride, SmOCl. (Matignon, A. ch. 1906, (8) 8. 412.) Samarium sulphide, Sm 2 S 3 . (Matignon, A. ch. 1906, (8) 8. 415.) Scandium, Sc. Element has not been isolated. Scandium bromide, Sc 2 Br 6 +3H 2 O, and +12H 2 0. (Crookes, Roy. Soc. Proc. 1908, 80. A, 518.) Scandium chloride, Sc 2 Cl6, +3H 2 O, and + 12H 2 O. (Crookes, Roy. Soc. Proc. 1908, 80. A, 518.) Scandium hydroxide. Easily sol. in cone. HNO 3 or HCl+Aq. (Crookes, Roy. Soc. Proc. 1908, 80. A, 518.) 784 SCANDIUM OXIDE Scandium oxide, Sc 2 O 3- Sp. gr. of H 2 SeO 4 +Aq at 20 compared with Easily sol. by boiling with cone. HNO 3 or H 2 O at 4. HCl+Aq. Wts. corrected to vacuum. Scandium Decomp sulphide, Sc 2 S 3 . . by H 2 O and by acids with evolu- Sp. gr. % H 2 Se04 Sp. gr. 07 II H 2 Se0 4 I] Sp " gr ' % H 2 SeO 4 tion of H 2 S. (Wirth, Z. anorg. 1914, 87. 5.) 1.000 1.295 32.64 1.590 54.62 Selenantimonic acid. 1.005 0^9 1.300 33.08 1.595 54.92 Sodium selenantimonate, Na 3 SbSe 4 +9H 2 O. 1.010 1.015 1.56 2.12 1.305 1.310 33.50 33.92 1.600 1.605 55.28 55.62 Sol. in 2 pts. cold H 2 O. Insol. in alcohol. 1.020 2.92 .315 34.36 1.610 55.96 (Hofacker, A. 107. 6.) 1.025 3.62 .320 34.82 1.615 56.30 SI. sol. in H 2 O; unstable. (Pouget, A. ch. 1.030 4.16 .325 35.26 1.620 56.60 1899, (7) 18. 562.) 1.035 4.70 .330 35.72 1.625 56.88 Selenantimonous acid. 1.040 1.045 5.32 6.08 .335 .340 36.10 36.43 1.630 1.635 57.20 57.48 Potassium or//ioselenantimonite. K 3 SbSe 3 . 1.050 6.66 .345 36.88 1.640 57.70 Ppt. Decomp. by 1 8QQ (7} 18 560 ) H 2 O. (Pouget, A. ch. 1.055 1.060 7.34 7.92 .350 1.355 37.34 37.80 1.645 1.650 58.04 58.47 -LOt/i/j V'/ AO *J\J\J*J 1.065 8.56 1.360 38.24 1.655 58.86 Potassium paraselenantimonite, K 2 Sb 4 Se 7 + 1.070 9.20 1.365 38.66 1.660 59.24 3H 2 O. 1.075 9.82 1.370 39.10 1.665 59.56 SI. sol. in H 2 O; unstable. (Pouget, A. ch. 1.080 10.44 1.375 39.50 1.670 59.74 1899, (7) 18. 560.) 1.085 11.02 1.380 39.98 1.675 59.94 Sodium ort/ioselenantimonite, Na 3 SbSe 3 + 1.090 1.095 11.62 12.20 1.385 .390 40.06 40.66 1.680 1.685 60.18 60.36 9H 2 O. 1.100 12.88 .395 41.10 1.690 60.58 Very sol. in H 2 O. Aqueous solution on 1.105 13.58 .400 41.56 1.695 60.80 standing deposits red crystals of sodium selen- 1.110 14.14 .405 41.98 1.700 61.06 antimonate, Na 3 SbSe 4 +9H 2 O. (Pouget, A. 1.115 14.66 .410 42.36 1.705 61.36 ch. 1899, (7) 18. 562.) 1.120 15.20 .415 42.78 1.710 .61.64 Sodium paraselenantimonite, Na 2 Sb 4 Se7. 1.125 15.74 .420 43.16 .715 61.90 (Pouget, A. ch. 1899, (7) 18. 561.) .130 .135 16.32 16.86 .425 .430 43.56 43.94 .720 .725 62.24 62.48 Selenic acid, H 2 SeO 4 . .140 17.38 .435 44.32 .730 62.76 Very sol in H 2 O with evolution of heat. .145 17.90 .440 44.52 .735 63.06 If aqueous solution is evaporated at temp. .150 18.44 .445 45.00 .740 63.32 of 165, acid has 2.524 sp. gr.; at temp, of .155 18.92 .450 45.32 .745 63.60 267, acid has 2.60 sp gr.; at temp, of 285, 1.160 19.48 .455 45.68 .750 63.86 acid has 2 .625 sp. gr. Decomp. to H 2 SeO 3 1.165 20.02 .460 46.04 .755 64.04 at higher temp. (Mitscherlich, Pogg. 9. 623.) 1.170 20.58 .465 46.36 .760 64.24 By evaporation at 265, acid of 2.609 sp. 1.175 21.08 .470 46.70 1.765 64.42 gr. containing 95% H 2 SeO 4 is obtained. If 1.180 21.60 .475 47.01 1.770 64.62 brought at same temp . in vacuo over H 2 SO 4 , 1.185 22.22 .480 47.32 1.775 64.84 acid of 2.627 sp. gr.'with 97.5% H 2 SeO 4 is 1.190 22.66 1.485 47.66 1.780 65.06 obtained . (Fabian, A Suppl. 1. 243.) 1.195 23.18 1.490 47.98 1.785 65.28 Sp.gr. of H 2 Se0 4 +Aq. 1.200 1.205 23.70 24.26 1.495 1.500 48.28 48.54 1.790 1.795 65.48 65.66 % H2Se04 Sp. gr. % H 2 SeO4 Sp. gr. 1.210 24.84 1.505 48.92 1.800 65.90 1.215 25.30 1.510 49.30 1.805 66.12 99.73 2.6083 90.0 2.3848 1.220 25.84 1.515 49.68 1.810 66.36 99.50 2.6051 89.0 2.3568 1.225 26.30 1.520 50.02 1.815 66.64 99.00 2.6975 88.0 2.3291 1.230 26.84 1.525 50.34 1.820 66.90 98.5 2.5863 87.0 2.3061 1.235 27.28 1.530 50.68 1.825 67.16 98.0 2.5767 86.0 2.2795 1.240 27.70 1.535 51.04 1.830 67.46 97.5 2.5695 85.0 2.5558 1.245 28.18 1.540 51.38 1.835 67.72 97.0 2.5601 84.0 2.2258 1.250 28.58 1.545 51.66 1.840 68.02 96.0 2.5388 83.0 2.1946 1.255 29.06 1.550 51.98 1.845 68.30 95.0 2.5163 82.0 2.1757 1.260 29.44 1.555 52.28 1.850 68.50 94.0 2.4925 81.0 2.1479 .265 29.82 1.560 52.56 1.855 68.70 93.0 2.4596 80.0 2.1216 .270 30.26 1.565 52.88 1.860 68.92 92.0 2.4322 79.0 2.0922 .275 30.76 1.570 53.28 1.865 69.12 91.0 2.4081 73.50 1.9675 .280 31.26 1.575 53.56 1.870 69.34 .285 1.290 31.74 32.18 1.580 1.585 53.94 54.30 1.875 1.880 69.56 69.72 (Cameron and Macallan, Lond. R 46. 13.) Soc. Proc. SELENATE, AMMONIUM CADMIUM 785 Sp. gr. of H 2 SeO 4 +Aq Concluded. Selenates. All the neutral and. acid salts of H 2 SeO 4 arc Sp. gr. % H 2 SeO4 Sp. gr. % H 2 Se04 Sp. gr. % H 2 SeO4 sol. in H 2 O, except BaSeO 4 , SrSeO 4 , CaSeO 4 , and PbSeO4, which are nearly or quite insol. inH 2 O orHNOs+Aq. 1.885 69.94 2.125 80.25 2.365 89.14 1.890 1.895 70.14 70.38 2.130 2.135 80.42 80.68 2.370 2.375 89.30 89.48 Aluminum selenate, Al 2 (SeO 4 ) 3 . 1.900 70.64 2.140 80.74 2.380 89.60 . Resembles in every way aluminum sul- 1.905 70.78 2.145 80.96 2.385 89.72 phate. (Berzelius.) 1.910 71.00 2.150 81.14 2.390 89.84 1.915 71.21 2.155 81.36 2.395 89.96 Aluminum ammonium selenate, 1.920 71.38 2.160 81.60 2.400 90.10 Al 2 (NH 4 ) 2 (SeO 4 ) 4 +24H 2 O. 1.925 1.930 1.935 71.68 72.00 72.38 2.165 2.170 2.175 81.80 82.02 82.22 2.405 2.410 2.415 90.20 90.30 90.46 More sol. in H 2 O than the corresponding sulphate. (Wohlwill, A. 114. 191.) 1.940 1.945 72.66 72.88 2.180 2.185 82.44 82.64 2.420 2.425 90.74 91.00 Aluminum caesium selenate, Al 2 Cs 2 (SeO 4 ) 4 + 1.950 73.12 2.190 82.78 2.430 91.24 24H 2 O. 1.955 73.34 2.195 82.96 2.435 91.46 (Peterson, B. 9. 1563.) 1.960 73.54 2.200 83.10 2.440 91.70 Much more sol. in H 2 O than the corre- 1.965 73.74 2.205 83.24 2.445 92.00 sponding sulphate. (Fabre, C. R. 105. 114.) 1.970 73.98 2.210 83.44 2.450 92.28 1.975 1.980 74.22 74.44 2.215 2.220 83.62 83.78 2.455 2.460 92.56 92.85 Aluminum potassium seJenate, Al 2 K 2 (SeO 4 ) 4 +24H 2 O. 1.985 1.990 74.66 74.86 2.225 2.230 83.96 84.14 2.465 2.470 93.02 93 . 20 More sol. in H 2 O than common alum. 1.995 75.08 2.235 84.30 2.475 93.36 (Weber, Pogg. 108. 615.) 2.000 75.28 2.240 84.48 2.480 93.68 2.005 75.46 2.245 84.60 2.485 94.02 Aluminum rubidium selenate, Al 2 Rb 2 (SeO 4 ) 4 2.010 75.66 2.250 84.82 2.490 94.32 +24H 2 O. 2.015 75.88 2.255 85.02 2.495 94.48 (Peterson, B. 9. 1563.) 2.020 76.06 2.260 85.26 2.500 94.64 Much more sol. in H 2 O than the corre- 2.025 2.030 76.14 76.48 2.265 2.270 85.44 85.60 2.505 2.510 94.80 94.96 sponding sulphate. (Fabre, C. R. 105. 114.) 2.035 2.040 76.68 76.84 2.275 2.280 85.78 85.96 2.515 2.520 95.32 95.58 Aluminum sodium selenate, Al 2 Na 2 (SeO 4 ) 4 + 94.TT O 2.045 2.050 77.08 77.36 2.285 2.290 86.16 86.38 2.525 2.530 95.86 96.10 5, 12SeO 2 + 12H 2 O. (Prandtl and Lustig.) 3K 2 O, 5V 2 O 5 , 16SeO 2 +40H 2 O. (Prandtl and Lustig.) 4K 2 O, 6V 2 O 5 , 21SeO 2 +37H 2 O. (Prandtl and Lustig.) 5K 2 O, 10V 2 O 5 , 26SeO 2 +43H 2 O. (Prandtl and Lustig.) Sodium selenovanadate, 4Na 2 O, 6V 2 O 5 , 5SeO 2 +20H 2 O. Very sol. in H 2 O. Solution decomp. grad- ually. (Prandtl and Lustig.) 2Na 2 O, 7V 2 O 6 , 10SeO 2 + 13H 2 O. (Prandtl and Lustig.) 2Na 2 O, 7V 2 O 6 , 12SeO 2 +45H 2 O, and +90H 2 O. (Prandtl and Lustig.) Selenoxyarsenic acid. Ammonium selenoxyarsenate, 2(NH 4 ) 2 O, 2SeO 3 , As 2 O 6 +3H 2 O. Sol. in H 2 O with decomp. (Weinland, B. 1903, 36. 1403.) Barium sodium selenoxyarsenate, BaNaAsO 3 Se+9H 2 O. Ppt. (Weinland, Z. anorg. 1897, 14. 56.) Potassium selenoxyarsenate, 2K 2 O, 2SeO 3 , As 2 O 5 +3H 2 O. Sol. in H 2 O with decomp. (Weinland and Barttlingck, B. 1903, 36. 1403.) 7K 2 O,10Seq 3 ,2As 2 O 5 + llH 2 O. Very sol. in H 2 O. (Weinland and Barttlingck.) 3K 2 O, As 2 Se 5 -f 10H 2 O. Easily decomp. by SILICIC ACID 801 moisture. Very sol. in H 2 O. (Clever, Z anorg. 1895, 10. 126.) Rubidium selenoxyarsenate, 2Rb 2 O, 2SeO 3 As 2 O 5 +3H 2 O. Sol. in H 2 O with decomp. (Weinland and Barttlingck.) Sodium selenoxyarsenate, Na 3 AsSeO 3 . Fairly stable in air and in aq. solution. (Weinland, B. 1896, 29. 1010.) Na 3 AsSeO 3 + 12H 2 O. Stable in the air when pure; sol. in H 2 O with decomp. (Wein- land, Z. anorg. 1897, 14. 50.) N a3 AsSeO 3 + 12H 2 O. Very sol. in H 2 O; very unstable. (Szarvasy, B. 1895, 28. 2657.) 3Na 2 O, 3Na 2 Se, As 2 O 6 +50H 2 O. Easily sol. in H 2 O. Solution may be boiled for a long time without decomp. (Clever, Z. anorg. 1895, 10. 136.) Selenoxyphosphoric acid. Ammonium /nselenmowoxyphosphate, (NH 4 ) 3 PSe 3 O + 10H 2 O. Ppt. (Ephraim, B. 1910, 43. 280.) Ammonium hydrogen /melenraonoxyphos- phate, (NH 4 ) 5 H(PSe 3 O) 2 +18H 2 O. Ppt. (Ephraim.) Barium hydrogen efo'selen^'oxyphosphate, BaHPSe 2 O 2 + 14H 2 O. Decomp. in moist air. (Ephraim.) Potassium selenoxyphosphate, K 3 PSe 2 . 5 Oi. 6 +H 2 0. Decomp. by HNO 3 . Insol. in alcohol and ether. (Ephraim.) Sodium raowoselen^n'oxyphosphate, Na 3 PSeO 3 +20H 2 O. Decomp. by H 2 O. (Ephraim.) Sodium friselenwowoxyphosphate, Na 3 PSe 3 O + 10H 2 0. Sol, in H 2 O. Decomp. in aq. solution. Easily sol. in cone. NaOH+Aq. (Muth- mann, Z. anorg. 1897, 13. 199.) Selenyl bromide, SeOBr 2 (?). (Schneider, Pogg. 129. 450.) Selenyl bromide sulphur inoxide, SeOBr 2 , SO 3 . (Prandtl, Z. anorg. 1909, 62. 242.) Selenyl chloride, SeO 2 Cl 2 . Easily decomp. by H 2 O. (Weber, Pogg. 118. 615.) Selenyl sulphur chloride. See Sulphoselenyl chloride. Selenyl stannic chloride, 2SeOCl, SnCl 4 . Extremely deliquescent. Completely sol. in H 2 O. (Weber, B. A. B. 1866. 154.) Selenyl titanium chloride, 2SeOCl 2 , TiCl 4 . Decomp. by H 2 O with separation of an insol. residue. Decomp. by NH 4 OH+Aq. (Weber, B. A. B. 1865. 154.) Sesquiauramine. See Sesquiaurainine. Sesquihydraurylamine, (HOAu) 3 N, NH 8 . See esgmhydraurylamine. Silicic acid, SiO 2 , zH 2 O. See also Silicon dioxide. Silicic acid is sol. in 1000 pts. pure H 2 O. (Kirwan.) When pptd. from alkali silicates +Aq by CO 2 , 0.021 pt. SiO 2 remains dissolved in 100 pts. H 2 O. (Struckmann, A. 94. 341.) When pptd. as above, 100 pts. H 2 O dissolve 0.09 pt. SiO 2 in 3 days; 100 pts. H 2 CO 3 +Aq dissolve 0.078 pt. SiO 2 in 3 days. But if heated much more dissolves, the jelly itself becoming liquid, such jelly containing 2.49 pts. SiO 2 to 100 pts. H 2 O. This solution is not pptd. by considerable quantities of al- cohol, but cone. (NH 4 ) 2 CO 3 , NaCl, or CaCl 2 + Aq, etc., cause gelatinization. (Maschke, J. pr. 68. 234.) Solubility in H 2 O depends on the amt. of H 2 O, in presence of which the silicic acid is set free by dil. acids, CO 2 , or alkali salts+ Aq. If H 2 O is present in sufficient quantity to retain the silicic acid, much more will remain in solution than can be dissolved by digesting the gelatinous acid with H 2 O after- wards. 1 pt. SiO 2 can thus be held in solution by 500 pts. H 2 O. Presence of NH 4 OH, (NH 4 ) 2 CO 3 , or NH 4 C1 (in solutions of which SiO 2 is remarkably insol.) diminishes the power of H 2 O to retain SiO 2 in solution. SiO 2 is always more sol. in dil. than cone. NH 4 OH +Aq. (Liebig, A. 94. 373.) Silicic acid from the coagulation of the col- loidal form (see p. 802) is sol. in about 5000 pts. H 2 O when formed from a 1% solution, and 10,000 pts. when formed from a 5% solu- tion, but is insol. after being dried. (Graham, A. 121. 36.) Silicic acid is more sol. in dil. acids than in H 2 O, because, when acid is added in excess to moderately dil. K 2 SiO 3 +Aq, the solution remains clear, but if only enough acid is added to neutralize the base present, silicic acid will gradually separate out. If acid is added to cone. K 2 SiO 3 +Aq, silicic acid sep- arates out insol. in excess of acid, but if 20-30 pts. H 2 O are present to 1 pt. K 2 SiO 3 , and an excess of acid added at once, the silicic acid will remain in solution. This result is obtained with HC1, HNO 3 , H 2 SO 4 , or 802 SILICIC ACID HC 2 H 3 O 2 + Aq . These solutions may dissolve a neutral salt until saturated and no silicic acid will separate out. Therefore it is the acid that holds the SiO 2 in solution, and not the H 2 O. (C. J. B. Karsten, (1826) Pogg. 6. 353.) Even CO 2 has the power of holding SiO 2 in solution. (Karsten, I. c.) Solubility in acids of silicic acid of Struck- mann (see above): 100 pts. dil. HCl+Aq of 1.088 sp. gr. dissolve 0.0172 g. SiO 2 in 11 days; 100 pts. H 2 O sat. with CO 2 dissolve 0.0136 g. SiO 2 in 7 days. Silicic acid obtained by passing SiF 4 into H 2 O is sol. while still moist in 11,000 pts. cold, and 5500 pts. boiling HCl+Aq of 1.115 sp. gr. (Fuchs, A. 82. 119.) Silicic acid at the moment of separation (as in dissolving cast-iron, steel, etc.) is abun- dantly sol. in aqua regia (3 pts. HCl+Aq of sp. gr. 1.13 and 1 pt. HNO 3 +Aq of sp. gr. 1.33). (Wittstein, Z. anal. 7. 433.) The aq. solution obtained by the hydroly- sis of ethyl silicate is more stable in acids + Aq or alkali than in pure H 2 O. (Jordis, Z. anorg. 1903, 35. 16.) NH 4 OH+Aq dissolves considerable freshly precipitated silicic acid, (NH 4 ) 2 CO 3 only a very little. (Karsten, Pogg. 6. 357.) Dry or ignited SiO 2 is sol. in NH 4 OH + Aq. 100 pts. NH 4 OH+Aq containing 10% NHs dissolve: 0.714 pt. SiO 2 from gelatinous silicic acid; 0.303 pt. from artificially dried silicic acid; 0.377 pt. from amorphous SiO 2 ; 0.017 pt. from quartz. (Pribram, Z. anal. 6. 119.) NH 4 OH+Aq dissolves 0.382 pt. SiO 2 from dry silicic acid: 0.357 pt. from ignited SiO 2 ; 0.00827 pt. from quartz. (Souchay, Z. anal. 11. 182.) Silicic acid precipitated from alkali silicates +Aq with CO 2 is sol. as follows: 100 pts. pure H 2 O dissolve 0.021 pt. SiO 2 ; 100 pts (NH 4 ) 2 CO 3 +Aq containing 5% (NH 4 ) 2 CO 3 0.020 pt.; 100 pts. containing 1%(NH 4 ) 2 CO 3 ; 0.062 pt.; 100 pts. NH 4 OH+Aq containing 19.2% NH 3 , 0.071 pt.; 100 pts. containing 1.6%, 0.0986 pt. (Struckmann, A. 94. 341.) 100 pts. NH 4 OH+Aq (10% NH 3 ) dissolve of: crystallised SiO 2 , 0.017 pt.; amorphous SiO 2 , ignited, 0.38 pt.; amorphous 3SiO 2 , 4H 2 O, 0.21 pt.; amorphous silicic acid in form of jelly, 0.71 pt. Upon evaporation no ppt is formed, even when 80 mols. SiO 2 are presenl to 1 mol. NH 3 . (Wittstein, J. B. 1866. 192.' Sol. in KOH or NaOH+Aq, especially i: warm. (Dumas.) Sol. in K 2 SiO 3 or Na 2 SiO 3 +Aq. (Fuchs.) Easily sol. in boiling Na 2 C0 3 +Aq, separat ing as a jelly on cooling. (Pfaff.) NH 4 C1 or other NH 4 salts ppt. SiO 2 from solution in Na 2 CO 3 +Aq. 100 pts. T1 2 O in H 2 O dissolve 4.17 pts : amorphous SiO 2 in 24 hours' boiling. (Flem lining, Jena. Zeit. 4. 36.) Sol. in butyl amine. (Wurtz, A. ch. (3) 42. 166.) Not more sol. in H 2 O containing sugar than n pure H 2 O. (Petzholdt, J. pr. 60. 368.) Soluble silicic acid. Colloidal form by dialysis. Solutions con- ;aining 4.9% SiO 2 may be evaporated until they contain 14 % SiO 2 . The SiO 2 is separated rom its solution thus made in many ways (1) By standing. This happens the more easily the more cone, the solution is, and is mstened by heat. A 10-12% solution gelatin- zes at ordinary temp, in a few hours, and mmediately upon heating. A. 5-6% solution may be kept 5-6 days, a 2% solution, 2-3 months, and a 1% solution may be kept 2 or more years without gelatinizing. (2) When the solution is evaporated to dry- ness in vacuo at 15 a transparent glass is left which is insol. in H 2 O. (3) The coagulation of colloidal silicic acid is accelerated by powdered graphite and other indifferent bodies, and it is brought about in a few minutes by a solution of 'the alkali car- bonates, even when only Vio,ooo pt. of the carbonate is present. (Graham, A. 121. 36.) (4) Coagulation is also brought about by passing CO 2 through the solution. (Liebig.) CO 2 does not cause coagulation. (Maschke.) Coagulation is not caused by H 2 SO 4 , HC1, HNO 3 , HC 2 H 3 O 2 , H 2 C 4 H 4 O 6 , or NH 4 OH + Aq, or by neutral or acid salts+Aq. (Gra- ham.) NaCl and Na 2 SO 4 +Aq coagulate the solu- tion. (Maschke.) Alcohol, sugar, glycerine, or caramel do not coagulate. Soluble A1 2 O 6 H 6 , Fe 2 O 6 H 6 , albumen, and casein precipitate soluble SiO 2 . (Graham, A. 121. 36.) The jelly from colloidal SiO 2 is very sol. in slightly alkaline H 2 O. 1 pt. NaOH in 10,000 pts. H 2 O dissolves in an hour at 100 an amt. of the jelly corresponding to 200 pts. SiO 2 . (Graham.) Other colloidal forms. Various solutions of silicic acid may be obtained as follows: The jelly formed when SiF 4 is passed through H 2 O dissolves in a large amt. of H 2 O, and SiO 2 separates out on evaporation. This is still sol. in H 2 O, but is made insol. by evap- oration with HC1 or H 2 SO 4 . (Berzelius.) When SiF 4 is absorbed by crystallized H 3 BO 3 , and the HF and H 3 BO 3 removed by a large excess of NH 4 OH+Aq, a silicic acid is obtained which is very sol. in H 2 O. The solution is not decomp. by boiling, but on evaporation an insol. powder remains. (Ber- zelius, A. ch. 14. 366.) When K 2 SiO 3 +Aq is precipitated by CuCl 2 , the precipitate washed and dissolved in HC1+ Aq, the solution treated with H 2 S filtered and boiled, a solution of silicic acid is obtained SILICATE, ALUMINUM CALCIUM 803 which gelatinizes with KOH or NH 4 OH+Aq. (Doveri, A. ch. (3) 21. 40.) When Na 2 SiO 3 -|-Aq containing at most 3% SiO 2 is saturated with HCl+Aq of 1.10 sp. gr., and Na 2 SiO 3 added until the solution is slightly opalescent and carefully warmed to 30, a gelatinous mass is obtained which will dissolve in H 2 O by 12-16 hours' boiling if treated before being exposed to the air. The solution is slightly opalescent. The solution can be evaporated by heat until it contains 6% SiO 2 . In a vacuum or over H 2 SO 4 , solu- tions containing 10% may be obtained. The electric current, freezing, alcohol, or H 2 SO 4 precipitate or coagulate the solution. (Kuhn, J. pr. 59. 1.) SiS 2 with H 2 O gives off H 2 S, and forms a solution of SiO 2 which, after dilution, can be kept for months. But when boiled or evapo- rated, or when a sol. silicate is added, it becomes gelatinous. It leaves an insol. residue when evaporated to dryness. (Fremy, A. ch. (3) 38. 314.) Various forms of silicic acid have been de- scribed as definite compounds of SiO 2 with varying amounts of H 2 O, but it is doubtful if any true definite compounds exist, as the per- centage of H 2 O varies with the moisture of the air to which it is exposed. (See Ebelmen, A. ch. (3) 16. 129; Doveri, A. ch. (3) 21. 40; Fuchs, A. 82. 19; Merz, J. pr. 99. 177; van Bemmelen, B. 11. 2232, etc.) Silicates. The silicates are insol. in H 2 O with the ex- ception of the alkali salts, and these are sol. only when the ratio of the base to the acid is above a certain limit. Aluminum silicate, 2A1 2 O 3 , SiO 2 + 10H 2 O. Min. Collyrite. Sol. in acids, with forma- tion of SiO 2 , zH 2 O. Becomes transparent in H 2 O and is decomp. 4A1 2 O 3 , 3SiO 2 . Min. DiUnite. A1 2 O 3 , SiO 2 . Min. Andalusite, Chiastolite, Sillimanniie, Disthene or Cyanite. Insol. in acids. +5-7 H 2 O. Min. Allophane. Completely sol. in dil. acids; decomp. by cone, acids with separation of SiO 2 , o;H 2 O. 2A1 2 O 3 , 3SiO 2 +4H 2 O. Min. Pholeri'.e. In- sol. in HNO 3 +Aq. +6H 2 O. Min. Glagerite. A1 2 O 3 , 2Si0 2 +2H 2 O. Min. Kaolin, Clay. Insol. in dil. HC1 or HNO 3 +Aq; moderately dil. H 2 SO 4 +Aq, when heated to evaporation, extracts A1 2 O 3 and some SiO 2 , ana leaves the rest of the SiO 2 , sol. in boiling Na 2 CO 3 +Aq. All the A1 2 O 3 is dissolved by heating with 5-6 pts. H 2 SO< + lpt.H 2 O until H 4 SO 4 evaporates, and then treating with H 2 O. Quickly attacked by H 2 SiF 6 +Aq. Decomp. by boiling KOH+Aq, with resi- due of SiO 2 . (Rammelsberg.) KOH+Aq extracts ^ of the SiO 2 (Malar guti); is converted thereby into double sili- cates of K and Al, which are sol. in HCl+Aq. (Lemberg.) Solubility in KOH and HC1 increased if first heated to a low glow. (Glinka, C. C. 1899, II. 1063.) Colloidal day. (Schlosing, C. R. 79. 473.) +4H 2 O. Halloysite. Decomp. by acids. 4A1 2 O 3 , 9SiO 2 + 12H 2 O. Min. Porcelain clay from Passau. A1 2 O 3 , 3SiO 2 +3H 2 O. Min. Razoumoff- sklne. A1 2 O 3 , 4SiO 2 +7H 2 O. Min. Montmoril- lonite. Not decomp. by HCl+Aq, but by hot H 2 SO 4 . +H 2 O. Min. Pyrophyllite. Not decomp. by H 2 S0 4 . +3H 2 O. Min. Anauxite. 2A1 2 O 3 , 9SiO 2 +6H 2 O. Min. Cimolite. "Aluminum silicafe" is insol. in acetone. (Naumann, B. 1904, 37. 4328); ethyl acetate. (Naumann, B. 1910, 43. 314.) Aluminum barium silicate, A1 2 O 3 , BaO, 2SiO 2 +H 2 (?). Min. Edingtonite. Decomp. by HCl+Aq with separation of SiO 2 , zH 2 O. 5A1 2 O 3 , 4BaO, 10SiO 2 . (Fremy and Feil, C. R. 85. 1033.) 2A1 2 O 3 , 4BaO, 7Si0 2 . Min. Barylite. Very si. decomp. by alkali carbonates +Aq. (Blom- strand.) Aluminum barium potassium silicate, A1 2 O 3 , (Ba, K 2 )O, 5SiO 2 +2H 2 O. Min. Harmot'ome. When finely powdered, difficultly decomp. by HCl+Aq with separa- tion of pulverulent SiO 2 , zH 2 O. A1 2 O 3 , (Ba,K 2 )O. 4SiO 2 . Min. Hagalophane. Scarcely attacked oy acids. Aluminum caesium silicate, H 2 Cs 2 Al 2 Si 5 O 16 (?) Min. Pollucite. Very si. decomp. by HC1+ Aq. Aluminum calcium silicate, A1 2 O 3 , CaO, 2SiO 2 . Min. Anorthite. Completely decomp. by HCl+Aq with separation of pulverulent SiO 2 , zH 2 O. Min. Barsowite. Instantaneously decomp. by HCl+Aq, with separation of gelatinous SiO 2 , xH 2 O. +4H 2 O. Min. Gismondite. Gelatinizes with HCl+Aq. A1 2 O 3 , CaO, 3SiO 2 +3H 2 O. Min. Scolezite. Easily sol. in HCl+Aq, without formation of gelatinous SiO 2 . Sol. in H 2 C 2 O 4 +Aq with pptn. of CaC 2 O 4 . Decomp. by, and sol. to a certain extent in H 2 CO 3 +Aq, and decomp. also even by pure H 2 O. (Rogers, Am. J. Sci. (2) 5. 408.) +5H 2 O. Min. Levyn. Decomp. by acids without gelatinizing. A1 2 O 3 , CaO, 4SiO 2 +3H 2 O. Min. Capor- cianite. Leonhardite. Efflorescent. Easily 804 SILICATE, ALUMINUM CALCIUM FERRIC sol. in acids, with pptn. of gelatinous SiO 2 , A1 2 O 3 , CaO, 4SiO 2 +4H 2 O. Min. Laumon- tite. Easily gelatinizes with HC1 or HNO 3 + Aq, but is not affected by H 2 SO4 unless hot. A1 2 O 3 , CaO, 6SiO 2 +5H 2 O. Min. Epistil- bite. Gelatinizes with cone. HCl+Aq. (Gold- schmidt, Z. anal. 17. 267.) Scarcely decomp. by boiling cone. HC1+ Aq. (Jannasch and Tenne, Miner. Jahrb. 1880, 1. 43.) +6H 2 O. Stilbite. Heulandite. Slowly but completely gelatinized by HCl+Aq. A1 2 O 3 , 2CaO, 3SiO 2 +H 2 O. Min. Prehnite. Imperfectly decomp. by acids before ignition, but easily afterwards. A1 2 O 3 , 3CaO, 3SiO 2 . Lime alumina garnet. Grossularite. Partially decomp. by acids before ignition, but easily afterwards. 2A1 2 O 3 , CaO, 2SiO 2 +H 2 O. Margarite. Not attacked by acids. 3A1 2 O 3 , 4CaO, 6SiO 2 +H 2 O. Zoisite. Par- tially decomp. by HCl+Aq. 4A1 2 O 3 , 6CaO, 9SiO 2 . Min. Meionite. Completely sol. in HCl+Aq. Aluminum calcium ferric silicate, 2A1 2 O 3 , 4CaO, Fe 2 O 3 , 6SiO 2 +H 2 O. Min. Epidote. Only si. attacked by HC1+ Aq before ignition. Aluminum calcium ferric magnesium silicate, H u (Ca, Mg) 40 (Al 2 , Fe 2 ) 10 Si 3 5O 14 7. Min. Vesuvianite, Idiocrase. Only partially decomp. by HCl+Aq before ignition. Aluminum calcium iron, etc., silicate borate, H 2 R I 6 1 (A1 2 , B 2 ) 3 Si 8 O 32 . Min. Axinite. Not attacked by HCl+Aq before ignition. Aluminum calcium magnesium silicate, 4H 4 Ca 2 Mg 8 Si 6 O 2 4, 5H 2 CaMgAl 6 O 12 = 15A1 2 O 3 , 13CaO, 37MgO, 24SiO 2 + 13H 2 0. Min. Clintonite. Completely decomp. by HCl+Aq without gelatinization. 3H 4 Ca 2 Mg 8 Si 6 24 , 4H 2 CaMgAl 6 O ]2 . Min. Brandisite. Not attacked by HCl+Aq. Slowly decomp. by boiling cone. H 2 SO 4 . 5H 4 Ca 2 Mg 8 Si 6 O 24 , 8H 2 CaMgAl6O 12 . Min. Xanthophyllite. Very si. decomp. by hot HCl+Aq. 3(Ca, Mg)O, A1 2 O 3 , 2SiO 2 . Min. Gehlenite. Easily decomp. by acids. Aluminum calcium potassium silicate, (H, K) 2 CaAl 2 Si 5 O 15 +6H 2 O. Min. Chabosite. Decomp. by HCl+Aq. (K 2 , Ca)Al 2 Si 3 O 10 +4H 2 O. Min. Zeagonite. Completely sol: in HCl+Aq. Aluminum calcium sodium silicate, 3A1 2 O 3 , 8CaO, Na 2 O, 9SiO 2 . Min. -Sarcolite Decomp. by acids. 2A1 2 O 3 , 12(Ca,Na 2 )O, 9SiO 2 (?). Min. Mellilite. Gelatinized by acids. Na 2 CaAl 4 Si 2 Oi 2 (?). Min. Margarite. Na 2 CaAl 4 Sii O 28 . Min. Faiijasite. De- comp. by HCl+Aq. (Na 2 , 'Ca)Al 2 Si 4 O 12 . Min. Gmelinite. De- comp. by HCl+Aq. (Ca, Na 2 )Al 2 Si 6 Oi9+6H 2 O. Min. Foresite. Difficultly decomp. by HCl+Aq. (Ca, Na 2 )Al 2 Si 2 O 8 +2>H 2 O. Min. Thom- sonite. Gelatinizes with HCl+Aq. zNa 2 Al 2 Si 6 O 16 , ?/CaAl 2 Si 2 O 8 . Min. Oligo- clase, Labradorite. SI. decomp. by acids, more easily the larger the amt. of Ca present. Aluminum calcium sodium silicate sulphate, 2(Na 2 , Ca)Al 2 (SiO 4 ) 2 , (Na 2 , Ca)SO 4 . Min. Hauyn. Gelatinizes with HCl+Aq. Aluminum glucinum silicate, A1 2 O 3 , 3G1O, 6Si0 2 . Min. Beryl. Emerald. Not decomp. by acids, excepting partially by H 2 SO 4 after be- ing ignited. A1 2 O 3 , 2G1O, 2SiO 2 +H 2 O. Min. Euclase. Not attacked by acids. Aluminum ferrous silicate, Al 2 Fe(SO 4 ) 3 . Min. Garnet. SI. decomp. by HCl+Aq. H 2 FeAl 2 SiO 7 . Min. Chloritoid. Not at- tacked by HCl+Aq. Completely decomp. by H 2 S0 4 . A1 2 O 3 , 3FeO, 3SiO 2 +3H 2 O. Min. Voiglite. Aluminum iron lithium potassium silicate, K 3 Li 3 Fe 4 Al 12 Si 20 O 6 5. Min. Zinnwaldite. SI. decomp. by acids. Aluminum ferrous magnesium silicate, % 6A1 2 O 3 , 3(Mg, Fe)O, 6SiO 2 +H 2 O. Min. Siaurolite. Not attacked by acids. Aluminum ferric magnesium silicate, 2(A1 2 , Fe 2 )O 3 , 2MgO, 5SiO 2 . Min. Cordierite. SI. attacked by acids. +rcH 2 O. Min. Esmarkite, Chlorophyllite. Aluminum ferrous manganous silicate, A1 2 O 3 , FeO, 2MnO, 3SiO 2 . Min. Partschinite. Aluminum ferrous sodium, etc., silicate borate, ) (B 2 ).Si 4 O 20 + R 1 ?(Al 2 ) 2 (B 2 )Si 4 O 2 o, etc. Min. Tourmaline. Not decomp. by HC1+ Aq; very si. decomp. by H 2 SO 4 . Aluminum lithium silicate, A1 2 O 3 , Li 2 O, 5Si0 2 . Not attacked by acids. (Hautefeuille, C. R. 90. 541.) A1 2 O 3 , Li 2 O, 6SiO 2 . A1 2 O 3 , Li 2 O, 4SiO 2 . [Min. Spodumene. Not attacked by acids. SILICATE, OESIUM 805 4A1 2 O 3 , 3Li 2 O, 30SiO 2 . Min. Petalite. .Not attacked by acids. Aluminum lithium potassium silicate, (Li, K) 10 Al 10 Sii 6 O 5 2. Min. Lepidolite. SI. decomp. by acids. Aluminum magnesium silicate, 5A1 2 O 3 , 4MgO, 2SiO 2 . Min. Sapphirine. Aluminum magnesium potassium silicate, zH 4 K 2 Al 6 Si 6 O 24 , 2/Mg 12 Si 6 O 21 . Min. Lepidomelane. Easily decomp. by HC1 or HNO 3 +Aq, with residue of a skeleton of SiO 2 . 3A1 2 O 3 , 12MgO, 2K 2 O, 12SiO 2 +H 2 O. Min. Anomite. 7A1 2 O 3 , 35MgO, 7K 2 O, 36SiO 2 . Min. Phlogopite. Aluminum manganous silicate, 2A1 2 O 3 , 6MnO, 6SiO 2 . Not decomp. by very dil. HCl+Aq. (Gor- geu, C. R. 97. 1303.) Aluminum potassium silicate, A1 2 O 3 , K 2 O, SiO 2 . Very slowly decomp. by cold H 2 O; 12% is dissolved by hot H 2 O. Sol. in alkali hydrox- ides+Aq, but insol. in carbonates +Aq. K 2 O, A1 2 O 3 , 2SiO 2 . Insol. in cold H 2 O, but 6% dissolves on boiling. Sol. in dil. acids. Insol. in alkali hydroxides or carbonates +Aq. (Gorgeu, A. ch. (6) 10. 45.) K 2 O, A1 2 O 3 , 3SiO 2 +3H 2 O. Easily sol. in HNO 3 +Aq. (Deville, A. ch. (3) 61. 313.) K 2 O, A1 2 O 3 , 4SiO 2 . Min. Leucite. De- comp. by HCl+Aq with separation of pul- verulent SiO 2 . +4H 2 O. Ppt. (Deville, C. R. 64. 324.) H 4 K 2 Al 6 Si 6 O 24 . Min. Muscovite, "Mica." Not attacked by HC1 or H 2 SO 4 +Aq. K 2 Al 4 Si 5 O 17 +3H 2 O. Min. Finite. Partly decomp. by HCl+Aq. K 2 Al 2 Si 6 Oi6. Min. Orthoclase. Feldspar. Scarcely attacked by acids. Slowly sol. in H 2 SO 4 or HCl+Aq when finely powdered. (Rogers.) Aluminum potassium sodium silicate, K 2 Al 2 (SiO 3 ) 4 , 5Na 2 Al 2 (SiO 4 ) 2 (?). Min. Nepheline. Decomp. by HCl+Aq. Aluminum silver silicate, Al 2 Ag 4 Si 2 O 9 . Insol. in NH 4 OH+Aq. (Silber, B. 14. 941.) Al 6 Ag 2 Na 4 Si 6 O 4 . As above. (Silber.) Aluminum sodium silicate, A1 2 O 3 , Na 2 O, SiO 2 . Insol. in cold H 2 O, but 38-40% dissolves in hot H 2 O. (Gorgeu.) A1 2 O 3 , Na 2 O, 2SiO 2 . Insol. in cold H 2 O; boiling H 2 O dissolves 1-2%. Sol. in HC1 or HNO 3 diluted with 10-20 vols. H 2 O. Insol. in alkali hydroxides or carbonates +Aq. (Gorgeu, A. ch. (6) 10. 145.) Not attacked by H 2 O. (Silber, B. 14. 941.) +3H 2 O. Easily sol. in HCl+Aq. (v. Ammon.) A1 2 O 8 , Na 2 O, 3SiO 2 +3H 2 O. Decomp. by acids. (Deville, A. ch. (3) 61. 326.) A1 2 O 3 , Na 2 O, 4SiO 2 +3H 2 O. Easily sol. in HCl+Aq. (v. Ammon.) 2A1 2 O 3 , 3Na 2 O, 3SiO 2 . Insol. in cold H 2 O, but 27-30% dissolves on boiling. (Gorgeu.) H 4 Na 2 Al 6 Si6O 24 . Min. Bafagonite. De- comp. by cone. H 2 SO 4 . Na 2 Al 2 Si 4 O 12 +2H 2 O. Min. Anaclite. Readily decomp. by HCl+Aq. Na 2 Al 2 Si 3 Oio+2H 2 O. Min. Natrolite. Sol. in H 2 O with separation of SiO 2 . Also sol. in H 2 C 2 O 4 +Aq. Na ? Al 2 SiOi6. Min. Albite. Not attacked by acids. Aluminum sodium silicate chloride, 3Na 2 Al 2 (SiO 4 ) 2 , 2NaCl. Min. Sodalite. Easily decomp. by HC1, and HNOs+Aq. Aluminum sodium silicate sulphate, 3Na 2 Al 1 (SiO 4 ) 2 , Na 2 SO 4 . Min. Nosean. Easily decomp. by HC1 + Aq. Aluminum sodium silicate sulphide. See Ultramarine. Barium silicate, BaSiO 3 . Somewhat sol. in boiling H 2 O. Completely sol. in dil. HCl+Aq. (v. Ammon.) +6H 2 O, or 7H 2 O. Boiling H 2 O decom- poses, and dissolves about }/% the weight of this substance, (le Chatelier, C. R. 92. 931.) 2BaO, SiO 2 . Decomp. by H 2 O into BaSiO 3 +6H 2 O. (Laudrin.) Bismuth silicate, 2Bi 2 O 3 , 3SiO 2 . Min. Eulytite. Decomp. by HCl+Aq. Bismuth ferric silicate, Bi 2 Fe 4 Si 4 Oi 7 . Min. Bismuthoferrite. Boron calcium silicate. See Borate silicate, calcium, and Silicate borate, calcium. Cadmium silicate, CdSi0 3 +l^H 2 O. Sol. in HCl+Aq with deposition of pul- verulent SiO 2 , zH 2 O. (Rousseau and Tite, C. R. 114. 1262.) Caesium silicate, Cs 2 SiO 3 . (Kahlenberg, J. phys. Chem. 1898, 2. 82.) 806 SILICATE, CALCIUM Calcium silicate, CaSiO 3 . Slowly sol. in H 2 O; sol. in HCl+Aq. Sol. in about 100,000 pts. H 2 O. (Gorgeu. A. ch. 1885, (6) 4. 550.) 100 cc. sat. aq. solution of air dried cal- cium silicate contains 0.0046 g. CaO = 0.0095 g. CaSiO 3 at 17. (Weisberg, Bull. Soc. 1896, (3) 15. 1097.) 100 cc. sat. solution of air dried calcium silicate in 10% sugar solution at 17 contains 0.0065 g. CaO = 0.0135 g. CaSiO 3 ; 20% sugar solution, 0.0076 g. CaO = 0.0175 g. CaSiO,. After boiling and filtering hot, 10% sugar solution contains 0.0094 g. CaO = 0.0195 g. CaSiO 3 ; 20% sugar solution, 0.0120 g. CaO = 0.0249 g. CaSiO 3 . (Weisberg.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate: (Naumann, B. 1910, 43. 314.) 4CaO, 3SiO 2 . (Laudrin.) 5CaO, 3SiO 2 +5H 2 O. When freshly pre- cipitated is somewhat sol. in H 2 O and easily decomp. by HCl+Aq. (v. Ammon.) CaO, 3SiO 2 +2H 2 O. (Hjeldt, J. pr. 94. 129.) 2CaO, 9SiO 2 +3H 2 O. Ppt. CaSiO 3 . Min. Wollastonite. Gelatinizes with HCl+Aq. CaSi 2 O 5 +2H 2 O. Min. Okenite. Easily de- comp. by cold HCl+Aq when powdered. Calcium glucinum silicate sodium fluoride, (Ca, Gl)i5Sii 4 O 4 3, 6NaF. Min. Leucophane. 7(Ca, Gl) 3 Si 2 O 7 , 6NaF. Min. Melinophane. Calcium ferrous silicate, CaSiO 3 , FeSiO 3 . Min. Hederibergite, Pyroxene. SI. decomp. by acids. Calcium ferric silicate, Ca 3 Fe 2 (SiO 4 )s. Min. Garnet. SI. decomp. by HCl+Aq. 2CaSiO 3 , 11 Fe 2 (SiO 3 ) 3 . Min. Szaboite. SI. attacked by HCl+Aq, and still less by H 2 SO 4 +Aq. Calcium ferroferric silicate, 2CaO, 4FeO, Fe 2 O 3 , 4SiO 2 +H 2 O = H 2 Ca 2 Fe 4 Fe 2 Si 4 O 18 . Min. Lievrite, Ilvaite. Easily gelatinizes with HCl+Aq. Calcium ferrous magnesium silicate, (Ca, Fe, Mg)SiO 3 . Min. Amphibole, Hornblende, Asbestos, Actinolite, Tremolite. Only si. attacked by acids. Calcium ferroferric sodium silicate, CaSiO 3 , FeSiO 3 , Fe 2 (SiO 3 ) 3 , Na 2 SiO 3 . Min. Aegirite. Calcium magnesium silicate, CaO, MgO, 4SiO 2 . (Mutschler, A. 176. 86.) Ca 2 SiO 4 , Mg 2 SiO 4 . Min. Monticellite. Completely sol. in dil. HCl+Aq. (Oa,Mg)SiO 3 . Min. Diopside, Pyroxene. Very si. attacked by 'acids. Calcium manganous silicate, CaSiO 3 , 2MnSiO 3 . Min. Bustamite. Calcium potassium silicate. See under Glass. Calcium sodium silicate, (Ca, Na 2 , H 2 )SiO 8 . Min. Pectolite. Decomp. by HCl+Aq. See under glass. Calcium sodium silicate zirconate, Na 4 Ca(Si,Zr) 9 O 2 i +9H 2 O. Min. Wohlente. Decomp. by HCl+Aq. Calcium uranyl silicate, 3CaO, 5UO 3 , 6SiO 2 + 18H 2 O. Min. Uranophane. Gelatinizes with acids. CaO, 3UO 3 , 3SiO 2 +9H 2 O. Min. Uranotile. Calcium silicate chloride, 2CaO, SiO 2 , CaCl 2 . Insol. in H 2 O or alcohol. Sol. in HCl+Aq. (le Chatelier, C. R. 97. 1510.) Calcium silicate fluoride, 2CaO, 3SiO 2 , 6CaF 2 . (Deville, C. R. 62. 110.) Calcium silicate potassium fluoride, 4H 2 CaSi 2 O 6 , KF+4H 2 O. Min. Apophyllite.. Decomp. by HCl+Aq. Calcium silicate stannate. See Silicostannate, calcium. Calcium silicate titanate, CaO, SiO 2 , TiO 2 . (Hautefeuille, A. ch. (4) 4. 154.) Min. Titanite. Incompletely decomp. by HCl+Aq, wholly by H 2 SO 4 +Aq. Cerous silicate, Ce 2 (SiO 3 ) 3 . More or less attacked by HC1, HNO 3 , or H 2 SO 4 +Aq, according to the concentration. (Didier, C. R. 101. 882.) Cerium didymium lanthanum silicate, 2(Ce,La,Di) 2 O 3 , 3SiO 2 . Min. Cerite. Gelatinizes with HCl+Aq. Cerium glucinum yttrium silicate, (Y,Ce,Gl) 2 SiO 5 . Min. Gadolinite. Easily gelatinized by HCl+Aq. Cerous silicate chloride, 2Ce 2 O 3 , 3SiO 2 , 4CeCl 3 = Ce 4 (SiO 4 ) 3 , 4CeCl 3 . Insol. in H 2 O, but slowly decomp. thereby. (Didier, C. R. 101. 882.) SILICATE, MAGNESIUM, FLUOSILICATE 807 Cobaltous silicate, Co 2 SiO 4 . Gelatinizes with HCl+Aq. (Bourgeois, C. R. 108. 1077.) Cupric silicate, CuH 2 SiO 4 . Min. Dioptase. Sol. in HC1, HNO 3 , or NH 4 OH+Aq with separation of SiO 2 . Not attacked by KOH+Aq. CuSiO 3 +2H 2 O. Min. Chrysocolla. De- comp. by HCl+Aq. +3H 2 O. Min. Asperolite. Easily de- comp. by HCl+Aq. "Cupric silicate" is insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Cupric silicate ammonia, CuSi 2 O 5 , 2NH 3 . Ppt. (Schiff, A. 123. 38.) Glucinum silicate, Gl 2 Si0 4 . Min. Phenacite. Not attacked by acids. Glucinum ferrous manganous silicate ferrous manganous sulphide, 3(G1, Fe, Mn) 2 SiO 4 , (Mn, Fe)S. Min. Helvine. Decomp. by HCl+Aq. Iron (ferrous) silicate, Fe 2 SiO 4 . Min. Fayalite. Gelatinizes with HC1+ FeSiO 3 . Min. Grunerite. +6H 2 O. Min. Chlorophite. 4FeO, SiO 2 . (Zobel, Dingl. 154. 111.) Iron (ferric) silicate, Fe 2 Si 3 O 9 +5H 2 O. Min. Nontronite. Gelatinizes with hot acids. 4Fe 2 O 3 , 9SiO 2 + 18H 2 O. Min. Hisingerite. 2Fe 2 O 3 , 9SiO 2 +2H 2 O. Min. Anthosider- ite. Iron (ferroferric) magnesium silicate, (Fe, Mg) 3 Fe 2 Si 2 10 +4H 2 0. Min. Cronstadtite. Gelatinizes with acids. Iron (ferroferric) sodium silicate, 5Na 2 SiO 3 , 2FeSiO 3 , 4Fe 2 (SiO 3 ) 3 . Min. Aknite. SI. decomp. by acids. Iron (ferrous) magnesium silicate, Fe 2 SiO 4 , Mg 2 SiO 4 . Min. Olivene, Chrysolite, Peridote. Gelat- inizes with HC1 or H 2 SO 4 +Aq. (Fe, Mg)SiO 3 + 3 /2H 2 O. Min. Picrophyllite. + i^H 2 O. Min. Monradite. (Fe,Mg)SiO 3 . Min. Bronzite, Hypersthene. Not attacked by acids. zMgSiOs, 2/FeSiO 3 . Min. Anthophyllite. Not attacked by acids. Iron (ferrous) manganous silicate, Fe 2 SiO 4 , Mn 2 SiO 4 . Min. Knebelite. Gelatinizes with HC1+ Aq. Iron (ferrous) manganous silicate chloride, 7(Fe,Mn)SiO 3 , (Fe,Mn)Cl 2 +5H 2 O. Min. Pyrosmalite. Completely decomp. by cone. HNO 3 +Aq. Iron (ferric) potassium silicate, Fe(SiOs)3, K 2 SiO 3 . (Hautefeuille and Perrey, C. R. 107. 1150.) Iron (ferric) sodium silicate, Na 2 Fe 2 Si 4 Ou. Min. Crokydolite. Not attacked by acids. Lead silicate. Insol. in acetone. (Naumann, B. 1904, 37. 4329); methyl acetate. (Naumann, B. 1909, 42. 3790.) See under Glass. Lithium 'silicate, Li 2 Si 5 On. Li 4 SiO 4 . Li 2 SiO 3 . More stable towards H 2 O than the other alkali metasilicates. (Rieke and Endell, C. C. 1911, I. 7.) Decomp. by boiling H 2 O and acids. (Frie- del, C. C. 1901, II. 89.) Scarcely attacked by cold H 2 O. (Friedel, Bull. Soc. Min. 1901, 24. 141.) Insol. in ethyl acetate. (Naumann, B. 1904, 37. 3601); methyl acetate. (Naumann, B. 1909, 42. 3790.) Magnesium silicate, Mg 3 Si 2 O 7 +2H 2 O. Min. Serpentine. Decomp. by HCl+Aq, more easily by H 2 SO 4 . Min. Chrysotile. Mg 4 Si 3 Oio+6H 2 O. Min. Gymnite, Soap- stone. Decomp. by H 2 SO 4 . MgSiO 3 . Not completely decomp. by HCl+Aq. + J^H 2 O. Min. Aphrodite. Decomp. by hot acids. + 3/H 2 O. Min. Picrosmine. -flVsHaO. Sol. in dil. acids, (v. Ammon.) Min. Forsterite. 3MgO, 4SiO 2 +H 2 O or 4MgO, 5SiO 2 + ^H 2 O. Min. Talc or Steatite. Not at- tacked by HC1 or H 2 SO 4 +Aq. Mg 5 Si 6 O 17 +4H 2 O. Min. Spadaite. De- comp. by cone. HCl+Aq. Mg 2 Si 3 O 8 +4H 2 O. Min. Meerschaum. Decomp. by HCl+Aq. "Magnesium silicate," is insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Magnesium potassium silicate, MgO, K 2 O, 3SiO 2 . Easily sol. in acids with decomp. (Du- boin, C. R. 1895, 120. 681.) Magnesium silicate fluosilicate, Mg 5 Si 2 O 9 , M g5 Si 2 F 18 . Min. Humite, Chondrodite. Gelatinizes with HC1 or H 2 SO 4 +Aq. SILICATE, MANGANOUS Manganous silicate, Mn 2 SiO 4 . Min. Tephroite. Decomp. by HCl+Aq with formation of a stiff jelly. MnSiO 3 . Min. Rhodonite, Hermannite. Not attacked by HCl+Aq. Mn 4 Si 3 Oio+2H 2 O. Min. Friedelite. Easily gelatinized by HCl+Aq. "Manganous silicate" is insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Manganous zinc silicate, (Mn,Zn) 2 SiO 4 . Min. Troostite. Manganous silicate chloride, MnSiO 3 , MnO. MnCl 2 . Decomp. by H 2 O. (Gorgeu.) Nickel silicate, Ni 2 Si0 4 . Easily decomp. by acids. (Bourgeois, C. R. 108. 1077.) Potassium silicate, K 2 SiO 3 . Completely sol. in H 2 O. (Ordway, Sill. Am. J. (2) 33. 34.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) K 2 Si 2 O 5 . Sol.inH 2 O. Conc.K 2 Si 24 O 5 +Aq contains 28% of the salt, and has sp. gr. 1.25. (Fuchs.) Hydroscopic. Decomp. at once by H 2 O. (Morey, J. Am. Chem. Soc. 1914, 36. 222.) K 2 Si 8 O 17 . Partially sol. in H 2 O as K 2 SiO 3 . K 2 Si 24 O 49 + 16H 2 O. Insol. in H 2 O. (Forch- hammer.) The K silicates are pptd. from their aqueous solution by alcohol with partial decomp., but less readily than Na silicates. More sol. in H 2 O than the corresponding Na salts. (Ordway, Sill. Am. J. (2) 32. 155.) Solution can be obtained which is perfectly clear when 4^SiO 2 are present to 1K 2 O, if there are no impurities present. (Ordway.) The K silicates resemble the Na salts, which see for further data. Potassium hydrogen silicate, KHSi 2 O 6 . Not readily affected by H 2 O, even by treat- ment at 100 for several hours. Decomp. by heating with dil. HC1. (Morey, J. Am. Chem. Soc. 1914, 36. 222.) Potassium zinc silicate. Sol. in KOH+Aq. (Schindler.) K 2 O, 6ZnO, 4Si0 2 . Sol. in HCl+Aq. (Du- boin, C. R. 1905, 141. 255.) 8K 2 O, 9ZnO, 17SiO 2 . Sol. in HCl+Aq. (Duboin.) Potassium zirconium silicate, K 2 O, ZrO 2 , 2Si0 2 . Decomp. by HCl+Aq. (Melliss.) Rubidium silicate, Rb 2 SiO 3 . (Kahlenberg, J. phys. Chem. 1898, 2. 82.) Silver silicate, Ag 2 SiO 3 . Decomp. by all acids; sol. in NH 4 OH+Aq. (Hawkins, Sill. Am. J. 139. 311.) Sodium silicate, Na 2 SiO 3 . Rapidly decomp. by H 2 O. (Morey, J. Am. Chem. Soc. 1914, 36. 224.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +5, 6, and 8H 2 O. Easily sol. in H 2 O. +9H 2 O. Solubility in 3^-N NaOH + Aq. 100 ccm. of the solution contain 25.56 g. Na 2 Si0 3 +9H 2 Oat 17.5. Sp. gr. of the solution = 1.1 29. (Vester- berg, C. C. 1913. 777.) 100 ccm. of a sat. solution of sodium sili- cate in Y 2 -N. NaCl+Aq. contain 3.83 g. Na 2 SiO 3 +9H 2 O at 17.5. Sp. gr. of solution = 1.15. 100 ccm. of a sat. solution of sodium silicate in sat. NaCl+Aq contain 20.64 g. Na 2 SiO 3 +9H 2 O at 17.5. (Vesterberg.) Na 2 Si 2 O 6 . Sol. in H 2 O. Slowly decomp. by cold H 2 O. (Morey J. Am. Chem. Soc. 1914, 36. 223.) Na 4 Si 6 12 . Na 2 Si 3 O 7 . Na 2 Si 4 O 9 . Slowly sol. in H 2 O. + 12H 2 O. Above compounds are all more or less indefinite. Water glass. zNa 2 O, ?/SiO 2 +zH 2 O. Sol. in H 2 O, but solution is decomposed by all weak acids, even CO 2 . Fused water glass is but little acted on by cold H 2 O, but when pure, easily dissolves in H 2 O by long boiling. (Ordway, Am. J. Sci. (2) 32. 337.) When the SiO 2 is present in greater propor- tion than in Na 2 O, 3SiO 2 , it is very difficult to dissolve in H 2 O. Na silicate is less easily sol. in H 2 O than the corresponding K compound. Solubility of water glass in H 2 O is much impaired by earthy impurities, so that traces have great effect in preventing the solubility. NH 4 salts decomp. water glass solutions. A solution containing l /$% Na 2 SiO 3 is scarcely . precipitated by NH 4 C1, but easily by NH 4 NO 3 . (Fluckinger.) Precipitated by NH 4 OH+Aq as Na 2 SiO 3 . Many sodium and potassium salts, espe- cially the chlorides and acetates, form precipi- tates in solutions of water glass; these pre- cipitates are larger the more concentrated the solution is, and the greater amount of SiO 2 it contains. Heating hastens the pre- cipitation by chlorides, nitrates, and sul- phates, but delays that by acetates. KOH + Aq does not precipitate. Cold sat. Na 2 SO 4 +Aq does not precipitate even on heating, but 1 pt. anyhydrous Na 2 SO 4 dissolved in 2 pts. H 2 O precipitates a hot solution of Na 2 SiO 3 . SILICATE, ZINC 809 NaNO? dissolved in 1 pt. H 2 O precipitate Na 2 SiO 3 +Aq of 1.392 sp. gr.; NaNO 3 in 2 pts. H 2 O when mixed with a solution of Na 2 SiO 3 , as above, if the two are present in equal vols., causes no ppt. in the cold, but solidifies when warmed to 54, and redis- solves on cooling rapidly, but if 2 vols. NaNO 3 +Aq are present to 1 vol. Na 2 SiO 3 +Aq, the precipitate dees not disappear on cooling. If 1 pt. NH 4 OH+Aq (0.921 sp. gr.) is added to 10 pts. Na 2 SiO 3 +Aq, no ppt. forms, but by increasing the amt. of NH 4 OH+Aq to 2 pts., the greater pt. of the Na2SiO 3 is pptd., but redissolves on heating to 90, separ- ating again on cooling. When 1 pt. NH 4 OH +Aq is added to 6-8 pts. Na 2 SiO 3 +Aq and heated to 30, a clear liquid is formed which separates into two layers at ordinary temp. The most sol. K, Na, Li, and NH 4 salts separate SiO 2 from cone. Na 2 SiO2+Aq. Most of these salts lose this power by dilu- tion, but the NH 4 salts and KSON keep this power until the solution is very dil. This is especially the case with NH 4 C1 and NH 4 NO 3 . Bromine, chlorine, propyl amine, crecsote, phenole dissolved in glycerine, chloral hy- drate, dil. albumen solution, and glue solu- tion ppt. SiO 2 from Na 2 SiO 3 +Aq; but sugar, dextrine, glycerine, urea, si. alkaline solution of urea nitrate, coniine, nicotine, saponine, convolvuline, jalappine, and colophonium dissolved in KOH+Aq do not ppt. SiO 2 . (Fluckinger, Arch. Pharm. (2) 144. 97.) Alcohol ppts. water glass as such from its aqueous solution, even when this is very dil., but there is some decomposition, the alcohol tending to hold in solution a portion of a silicate more alkaline than that previously dissolved in H 2 O, while the ppt. formed con- tains more SiO 2 than the original silicate. Many neutral K or Na salts ppt. water glass as such when added to aqueous solutions. Like alcohol, these solutions exert a decom- posing action, the ppt. being always more siliceous than the original silicate. Na sili- cate yields a larger deposit than K silicate; when a silicate of one base is pptd. by a salt of the other, both bases enter into the com- position of the ppt, and the relative propor- tion of Na and K is very nearly the same as in the average of the liquids mixed. Different salts have very unequal pptg. power, the acetates and chlorides being parti- cularly efficient. Heat increases the pptg. power of the chlorides, sulphates, and ni- trates, and diminishes that of the acetates. The alkali acetates are somewhat more efficient than the chlorides, but NaC 2 H 3 O 2 gives only a slight ppt. with Na 2 O, 2^SiO 2 , even after some time. NaNO 8 has but little effect on the more alkaline silicates. Na 2 SO 4 has still less power than NaNO 3 . Na 2 CO 3 has no pptg. power, and Na 3 AsO 4 or Na 3 PO 4 have very little effect. MHSO 4 , MHCO 3 , M 2 HPO 4 , M 2 HAs0 4 ppt. SiO 2 . NH 4 salts also have that effect. Pptd. water glass, as mentioned above, is much more sol. in H 2 O than ordinary water glass, and dissolves in H 2 O without decomp. For numerous further details, see articles by Ordway in Sill. Am. J. Sci. vols. 32 and 33; also Storer's Diet. Sp. gr. of water glass solution containing 14-15% SiO 2 , 13-14% Na 2 O, and 70-72% H 2 O is 1.30-1.35. (Hager, Comm. 1883.) Sp. gr. of sat. Na 2 SiO 3 +Aq freshly pre- pared at 18 is 1,2600, and 1 litre contains 4.5 gramme-equivalents ^2Na 2 SiO 3 . Sp. gr. of sat. solution of Na 2 O, 3.4SiO 2 is 1.366, and 1 litre contains 3.7 gramme- equivalents H(Na 2 O, 3.4SiO 2 ). (Kohl- rausch, Z. phys. Ch. 12. 773.) Sodium zirconium silicate, Na 2 O, ZrO 2 , SiO 2 . Decomp. by hot H 2 O or HCl+Aq. (Gibbs, Pogg. 71. 559.) Na 2 O, 8ZrO 2 , SiO 2 + llH 2 O. Decomp. by H 2 SO 4 . (Melliss.) Strontium silicate, SrSiO 3 . (Stein, Z. anorg. 1907, 55. 164.) +H 2 O. Sol. in H 2 O. (Jordis and Kanter, Z. anorg. 1903, 35. 90.) Sr 2 SiO 4 . (Stein, Z. anorg. 1907, 55. 167.) 3SrO, SiO 2 . SI. sol.' in H 2 O. Sol. in acids. (Vauquelin.) Thallous silicate, 3T1 2 O, 10SiO 2 . 100 pts. of a solution of T1 2 O dissolve 4.17 pts. SiO 2 by 24 hours' boiling. Sol. in H 2 O. (Flemming, J. B. 1868. 251.) Thorium silicate, ThO 2 , SiO 2 . Insol. in acids. Attacked by KHSO 4 . (Troost and Ouvrard, C. R. 105. 255.) + 13/H 2 O. Min. Thorite. Decomp. by HCl+Aq. ThO 2 , 2SiO 2 . Insol. in acids or KHSO 4 . (T. and O.) Yttrium silicate, Y 2 O 3 , SiO 2 . Attacked by HC1, HNO 3 , or H 2 SO 4 +Aq. (Duboin, C. R. 107. 99.) Zinc silicate, ZnSiO 3 . (Stein, Z. anorg. 1907, 55. 165.) Zn 2 SiO^. Min. Willemite. Gelatinizes with HCl+Aq; sol. in KOH+Aq. Decomp. by cold sat. citric acid+Aq. (Bolton, C. N. 1881, 43. 34.) +H 2 O. Min. Calamine. Sol. in HCl+Aq with separation of gelatinous SiO 2 , o:H 2 O. Sol. in HC 2 H 3 O 2 +Aq, and KOH+Aq. Insol. in NH 4 OH + (NH 4 ) 2 CO 3 +Aq. (Brandhorst, Zeit. angew. Ch. 1904, 17. 513.) ZnO, 3SiO 2 . (Borntrager, Ch. Z. 1893, 8. 186.) 810 SILICATE, ZIRCONIUM Zirconium silicate, SiO 2 , ZrO 2 . Min. 7ircon. Insol. in acids, except H 2 SO 4 , in which it is very slowly and si. sol. 3SiO 2 , 2ZrO 2 Min. Auerbachite. " Silicium oxide," Si 3 H 2 O 5 . (Geuther, J. pr. 95. 430.) This substance is identical with silicoformic anhydride ac- cording to Otto-Graham's Handb. anorgan. Chem. 7te Aufl. 2. 953. Siliciuretted hydrogen. See Silicon hydride. Silicobromoform, HSiBr 3 . Fumes on air; decomp. by H 2 O. Silicochloroform, HSiCl 3 . Decomp. by H 2 O and alcohol. Completely miscible with CS 2 , CC1 4 , CHC1 3 , C 6 H f , SiCl 4 , SnCl 4 , TiCl 4 , and AsCl 3 . (Ruff, B. 1905, 38. 2230.) Silicoethane. See Silicon hydride. Silicofluoroform, SiHF 3 . Decomp. by H 2 O. Decomp. by NaOH and abs. alcohol with evolution of hydrogen. Decomp. by abs. ether. Sol. in toluene. (Ruff, B. 1905, 38. 63.) Silicoformic anhydride, H 2 Si 2 O 3 = (HSiO) 2 O. Somewhat sol. in H 2 O. Acids, even cone. HNO 3 +Aq, have no action, except HF, which dissolves it easily with evolution of hydrogen. Solutions of alkali hydrates, ammonium hy- drate, and alkali carbonates +Aq also dis- solve with evolution of hydrogen. (Ruff and Wohler, A. 104. 101.) Silicoiodoform, HSiI 3 . Decomp. by H 2 O. Sol. in CS 2 . (Friedel, A. 149. 96.) Miscible with C 6 H 6 and CS 2 . (Ruff, B. 1908, 41. 3739.) Silicomethane, SiH 4 . See Silicon hydride. Silicomethyl chloride, SiH 3 Cl. Decomp. by H 2 O and by alkalies. (Besson and Fournier, C. R. 1909, 148. 556.) Silicomethylene chloride, SiH 2 Cl 2 . Decomp. by H 2 O and by alkalies. (Besson and Fournier, C. R. 1909, 148. 556.) Silicomolybdic acid, SiO 2 , 12MoO 3 + 26H 2 O. Very easily sol. in H 2 O and dil. acids. (Parmentier, C. R. 94. 213.) Forms a solution with a little ether, which separates into two layers by addition of H 2 O or more ether. (Parmentier, C. R. 104. 686.) (Copaux, Bull. Soc. Min. 1906, 29. 79.) +32H 2 O. Decomp. by alkali. (Asch, Z. anorg. 1901, 28. 293.) +33H 2 O. (Copaux, Bull. Soc. Min. 1906, 29. 79.) Aluminum silicomolybdate, 2A1 2 O 3 , 3(SiO 2 , 12MoO 3 )+93H 2 O. (Copaux, A. ch. 1906, (8) 7. 118.) Aluminum sodium silicomolybdate, 4(Na 2 O, A1 2 O 3 , 2SiO 2 ), Na 2 MoO 4 +7H 2 O. Sol. in HCl+Aq. (Thugutt, Z. anorg. 1892, 2. 87.) Ammonium silicomolybdate. Sol. in H 2 O. (Parmentier, C. R. 94. 213.) Barium silicomolybdate, 2BaO, SiO 2 , 12MoO 3 + 16H 2 O. (Copaux, A. ch. 1906, (8) 7. 118.) +22H 2 O. Sol. in 4 pts. H 2 O. (Copaux, Bull. Soc. Min. 1906, 29. 80.) +24H 2 O. Efflorescent. Very sol. in H 2 O. (Asch, Z. anorg. 1901, 28. 282.) +29H 2 O. Efflorescent. (Copaux, A. ch. 1906, (8) 7. 118.) Cadmium silicomolybdate, 2CdO, SiO 2 , 12MoO 3 +22H 2 O. Very unusually sol. in H 2 O. (Copaux, A. ch. 1906, (8) 7. 140.) Caesium silicomolybdate. SI. sol. in H 2 O; insol. in silicomolybdic acid+Aq. Calcium silicomolybdate, 2CaO, SiO 2 , 12MoO 3 +24H 2 O. Efflorescent. Very sol. in H 2 O. (Asch, Z. anorg. 1901, 28. 282.) +26H 2 O. (Copaux, A. ch. 1906, (8) 7. 118.) +31H 2 O. (Copaux.) Chromium silicomolybdate, 2Cr 2 O 3 , 3(SiO 2 , 12MoO 3 )+93H 2 O. (Copaux.) Cupric silicomolybdate, 2CuO, SiO 2 , 12MoO 3 +31H 2 O. ' Very sol. in H 2 O. (Copaux.) Lithium silicomolybdate, 2Li 2 O, SiO 2 , 12MoO 3 +29H 2 O. Very sol. in H 2 O. (Copaux.) Magnesium silicomolybdate, 2MgO, SiO 2 , 12MoO 3 +30H 2 O. (Asch, Z. anorg. 1901, 28. 282.) +31H 2 O. Very efflorescent and sol. in H 2 O. (Copaux.) SILICON BROMOSULPHIDE 811 Potassium silicomolybdate, 2K 2 O, Si0 2 , 12MoO 3 + 16H 2 O. Efflorescent. Very sol. in H 2 O. (Asch, Z anorg. 1901, 28. 282.) 1.5'K 2 O, SiO 2 , 12MoO 3 + 14H 2 O. (Asch.) Sol. in H 2 O with decomp. (Copaux.) Potassium silver silicomolybdate, K 2 O 3Ag 2 O, 2(Si0 2 , 12MoO 3 ) + 14H 2 O; +22H 2 O; +30H 2 O. Sol. in H 2 O with decomp. Sol. unchangec in dil. mother liquor. (Copaux, Bull. Soc Min. 1907, 30. 293.) Rubidium silicomolybdate. SI. sol. in H 2 O. Silver silicomolybdate, l.oAgjO, SiO 2 , 12MoO 3 + llH 2 O. Sol. in cold H 2 O. (Asch.) 2Ag 2 O, SiO 2 , 12MoO 3 + 12H 2 O. Decomp. by boiling H 2 O. Sol. in NH 4 OH+Aq. 4Ag 2 O, SiO 2 , 12MoO 3 + 15H 2 O. (Asch.) Sodium siHcomolybdate, 2Na 2 O, SiO 2 , 12MoO 3 + 14H 2 O. (Copaux.) 2Na 2 O, SiO 2 , 12MoO 3 +21H 2 O. Very sol. in H 2 O. Efflorescent. (Asch.) +22H 2 O. (Copaux.) 1.5Na 2 O, SiO 2 , 12MoO 3 + 17H 2 O. (Asch.) 3Na 2 O, 2(SiO 2 , 12MoO 3 ) + 17H 2 O. (Co- paux.) Strontium silicomolybdate, 2SrO, SiO 2 , 12MoO 3 +26H 2 O. (Copaux.) Zinc siHcomolybdate, 2ZnO, SiO 2 , 12MoO 3 + 31H 2 O. Extremely sol. in H 2 O. (Copaux.) Silicon, Si. Amorphous. Insol. in H 2 O. Sol. before igniting in cold HF. Insol. in other mineral acids and aqua regia. Sol. in cone. KOH+Aq. When amorphous Si is ignited, it becomes insol. in HF and KOH+Aq. Amorphous Si is sol. in aqua regia and in a mixture of HNO 3 and HF. (Vigouroux- Moissan, C. R. 1895, 120. 367.) Insol. in liquid CO 2 . (Buchner, Z. phys. Ch. 1906, 64. 674.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Graphitic. Sol. in HNO 3 +HF. (Ber- zelius, A. 49. 247.) Crystalline. Insol. in all acids, except a mixture of HF and HNO 3 . Sol. in moderately cone. KOH+Aq even when cold. (Deville.) Although it has been generally understood that crystallized Si is not attacked by HF, it is now found that this applies only to HF + Aq. Gaseous HF readily attacks cryst. Si. (Newth, C. N. 1896, 72. 287.) Si cryst. from Ag is incompletely sol. in HF. According to the temp, to which the Ag Si mixture has been heated, the following percentages of Si are dissolved in HF: 970, 58.02%; 1150, 27.66%; 1250, 19%; 1470, 16%. (Moissan and Siemens, C. R. 1904, 138. 657, 1300.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Silicon amide, Si(NH 2 ) 4 . Unstable; decomp. by H 2 O and partially decomp. by HNO 3 ; sol. in most organic sol- vents. (Lengfeld, Am. Ch. J.-1899, 21. 531.) Decomp. by H 2 O; insol. in liquid NH 3 . (Vigouroux, C. R. 1903, 136. 1670.) Silicon 2nT>oride, SiB 3 . Slowly attacked by HNO 3 . Decomp. by hot cone. H 2 SO 4 or fused KOH. (Moissan, C. R. 1900, 131. 142.) Silicon Aezaboride, SiB 6 . Readily attacked by HNO 3 . Slowly de- comp. by hot cone. H 2 SO 4 . Not attacked by fused KOH. (Moissan, C. R. 1900, 131. 142.) Silicon fnbromide, Si 2 Br 6 . Decomp. by KOH+Aq. (Friedel and Ladenburg, A. 203. 253.) HSiBr 3 . See Silicobromoform. Silicon fefrabromide, SiBr 4 . Rapidly decomp. by H 2 O; decomp, in sev- eral days by H 2 SO 4 . (Friedel and Ladenburg. A. 147. 362.) Silicon bromide, Si 3 Br 8 . (Besson, C. R. 1910, 151. 1056.) Si 4 Brio. (Besson.) Disilicon hydrogen pentobrcmide, HSi 2 Br 5 or Si 2 Br 5 (?). Decomp. by H 2 O. (Mahn, Zeit. Chem. (2) . 279.) Silicon teirabromide ammonia, SiBr 4 , 6NH 3 . Decomp. by H 2 O. (Lay, Dissert. 1910.) SiBr 4 , 7NH 3 . Decomp. by H 2 O. (Besson, . R. 110. 240.) Silicon bromoiodide, SiIBr 3 . Decomp. by H 2 O. Sol. in CS 2 . (Friedel, B. 2. 60.) SiBr 2 I 2 . As above. (F.) SiBrls. As above. (F.) ilicon bromosulphide, SiSBr 2 . Decomp. in moist air. Violently decomp. >y H 2 O. Sol. in CS 2 and other organic sol- ents. (Blix, B. 1903, 36. 4218.) 812 SILICON CARBIDE Silicon carbide, SiC. Very stable; insol. in H 2 SO 4 and HNO 3 ; sol. in fused KOH at red heat. (Moissan, Bull. Soc. 1894, (3) 11. 997.) Cryst. modification. Insol. in acids; sol. in fussd alkalies. (Moissan, C. R. 1893, 117. 427.) Insol. in all acids; sol. in molten alkalies. (Muhlhaeuser, Z. anorg. 1894, 5. 116.) See Silundum. Silicon sw&chloride, SiCl 2 (?). Decomp. by H 2 O. (Troost and Haute- feuille, A. ch. (5) 7. 463.) Silicon inchloride, Si 2 C 6 . Decomp. by H 2 O and alkalies. (Troost and Hautefeuille, A. ch. (5) 7. 459.) SiHCl 3 . See Silicochloroform. Silicon teZrachloride, SiCl 4 . Decomp. by H 2 O and alcohol. Silicon ociochloride, Si 3 Cls. "Perchlorsilicopropane." Decomp. by H 2 O. (Gattermann, B. 1894, 27. 1947.) Silicon chloride, Si 4 Clio. (Besson, C. R. 1909, 149. 36.) SisCla. "Perchlorsilicobutane." Decomp. by H 2 O. Fumes in the air. (Besson.) Si 6 Cli 4 . "Perchlorsilicohexane." Decomp. by H 2 0. (Besson, C. R. 1909, 148. 841.) Silicon Znchloride ammonia, Si 2 Cl 6 , 5NH 3 . Slowly decomp. by H 2 O. (Besson, C. R. 110. 516.) Silicon tefrachloride ammonia, SiCl 4 , 6NH 3 . Decomp. by H 2 O. (Persoz, A. ch. 44. 319.) Silicon tefrachloride hydrazine, SiCl 4 , 4N 2 H 4 . Extremely hygroscopic and quickly de- comp. by H 2 O. (Lay, Dissert. 1910.) Silicon chlorobromide, SiCl 3 Br. Decomp. by H 2 O. (Friedel and Laden- burg, A. 145. 187.) SiCl 2 Br 2 . As above. (Friedel and Laden- burg.) SiBraCl. Decomp. by H 2 O. (Reynolds, Chem. Soc. 61. 590.) Silicon chlorobromide ammonia, 2SiCl 3 Br, 11NH 3 . Decomp. by H 2 O. (Besson, C. R. 112. 788.) SiCl 2 Br 2 , 5NH 3 . As above. (B.) 2SiClBr 3 , 11NH 3 . As above. (B.) Silicon chlorohydrosulphide, SiCl 3 SH. Decomp. by H 2 O or alcohol. (Pierre, A. ch. (3) 24. 286.) Silicon chloroiodide, SiCl 3 I. Decomp. by H 2 O. (Besson, C. R. 112. 611.) SiCl 2 I 2 . As above. (B.) SiClIs. As above. (B.) Silver chloroiodide ammonia, 2SiCl 3 I, 11NH 3 . (Besson.) SiCl 2 I 2 , 5NH 8 . Silicon chloronitride, Si5N 6 Cl 2 . (Schiitzenberger, C. R. 92. 1508.) Silicon chloiosulphide, Si 2 Cl 2 S 2 . Decomp. violently by H 2 O. Sol. in CC1<. (Besson, C. R. 113. 1040.) SiSCl 2 . Violently decomp. by H 2 O; sol. in CS 2 . (Blix, B. 1903, 36. 4223.) Silicon difluoride, SiF 2 (?). Decomp. by H 2 O or NH 4 OH +Aq. (Troost and Hautefeuille, A. ch. (5) 7. 464.) Silicon tefrafluoride, SiF 4 . Abundantly absorbed by H 2 O with decomp. 100 pts. H 2 O absorb 140.6 pts. SiF 4 in 24 hours (Berzelius); 124.1 pts. SiF 4 in 24 hours (Davy). Absorbed abundantly by HNO 3 +Aq. (Kuhlmann, A. 39. 319.) Absorbed abundantly by alcohol, without separation of silicic acid, if the alcohol con- tains less than 8% of water. Sol. in cone. HF+Aq. Absorbed by ether. SI. sol. in naptha, and oil of turpentine. Silicon hydrogen fluoride, H 2 SiF 6 . See Fluosilicic acid. Silicon fluoride with MF. See Fluosilicate, M. Silicon fluoride ammonia, SiF 4 , 2NH 3 . Decomp. by H 2 O. (Davy.) Silicon hydride, SiH 4 . Insol. in H 2 O. Decomp. by KOH+Aq. Not changed by NH 4 OH+Aq, H 2 SO 4 +Aq, or HCl+Aq. Si 2 H 2 . " Silicoacetylene." Sol. in 20% NaOH+Aq. with evolution of H. (Bradlev, C. N. 1900, 82. 149.) Si 2 H 6 . "Silicoethane." (Lebeau, C. R. 1909, 148. 44.) SI. sol. in H 2 O. Best solvent is ethyl orthosilicate. (Moissan, Bull. Soc. 1903, (2) 29. 443.) Silicon nitrogen hydride, SiHN. Decomp. by H 2 O and NaOH. (Ruff, B. 1905, 38. 2241.) SILICON OXIDE 813 Silicon hydroxide, SiO 2 , #H 2 O. See Silicic acid. Si 2 H 2 O 4 . See Silicooxalic acid. Si 2 H 2 O 3 . See Silicoformic anhydride. Si 4 H 4 O 3 . See Silicone. Silicon imide, (Si(NH) 2 . Decomp. by H 2 O. (Vigouroux, C. R. 1903, 136. 1671.) SiliconeMmide, Si(NH),. Decomp. by H 2 O with evolution of much heat. (Blix, B. 1903, 36. 4224.) Silicon imide hydrochloride, Si(NH 2 ) 2 , 2HC1. Rather stable in air. (Blix, B. 1903, 36. 4225.) Silicon cfoiodide, SiI 2 . Insol. in CS 2 , CHC1 3 , C 6 H 6 , and SiCl 4 . (Friedel and Ladenburg, A. 203. 247.) Silicon tfniodide, Si 2 I 6 . Decomp. with H 2 O even at 0. 100 pts. CS 2 dissolve 19 pts. Si 2 I 6 at 19; 26 pts. Si 2 I 6 at 27. (Friedel and Ladenburg, Bull. Soc. (2) 12. 92.) HSiI 3 . See Silicoiodoform. Silicon teZraiodide, SiI 4 . Decomp. by H 2 O. Acts on alcohol and ether. 1 pt. CS 2 dissolves 2.2 pts. SiI 4 at 27 (Friedel, A. 149. 96.) Silicon nitride, SiN. Partially decomp. by boiling with cone H 2 SO 4 . Not attacked by dil. acids with the excep- tion of HF. Decomp. by HF. Partially decomp. by boiling with alkalies + Aq. (Weiss, Z. anorg. 1910, 65. 89.) Si 2 N 3 . Partially decomp. by boiling with cone. H 2 SO 4 . Not attacked by dil. acids with the ex ception of HF. Decomp. by HF. Partially decomp. by boiling with alkalies + Aq. (Weiss, Z. anorg. 1910, 65. 89.) Si 3 N 4 . Not attacked by H 2 O. Partially decomp. by boiling with co H 2 SO 4 . Not attacked by dil. acids with the excep tion of HF. Decomp. by HF. Partially decomp. by boiling with alkalies + Aq. (Weiss, Z. anorg. 1910, 65. 89.) Silicon nitrimide, Si 2 N 3 H. "Silicam." Sol. in HF, and rapidly in KOH+Ao (Schutzenberger, C. R. 92. 1508.) Decomp. by cold, more rapidly by hot H 2 C and much more rapidly by alkalies. Sol. ir HF+Aq. Not attacked by HNO 3 . Decomp by cone. H 2 SO 4 . (Lay, Dissert. 1910.) Not decomposed by H 2 O. Sol. in hot alkalies+Aq with decomp. Blix, B. 1903, 36. 4227.) ilicon sw&oxide, Si 3 O 2 . (Honigschmid, M. 1909, 30. 509.) silicon monoxide, SiO. Much less easily sol. in HF+Aq but more asily sol. in alkalies+Aq than SiO 2 . (Potter, :. C. 1907, II. 1952.) Silicon dioxide, SiO 2 . See also Silicic acid. (a) Crystalline. Mm. Quartz, Tridymite. Insol. in H 2 O, and acids, except HF. SI. sol. in boiling K 2 CO 3 +Aq, and KOH + i; see below. Insol. in cold KOH+Aq; extremely slowly sol. in boiling KOH+Aq. (Fuchs.) Sol. in HF with formation of SiF, and H 2 O. Insol. in sugar +Aq, contrary to assertion of Verdeil and Rissler. (Petzholdt, J. pr. 60. 368.) (b) Amorphous. Min. Opal, etc. Insol. in H 2 O, and acids except HF. 100 pts. H 2 O containing CO 2 dissolve 0.078 pt. amorphous SiO 2 (Maschke); 0.0136 pt. (Struckmann). 100 pts. cold HCl+Aq of 1.088 sp. gr. dis- solve 0.017 pt. SiO 2 . (Struckmann.) 100 pts. HCl+Aq of 1.115 sp. gr. dissolve in the cold 0.009 pt. SiO 2 , and 0.018 pt. on boiling. 100 pts. NH 4 OH+Aq (containing 10% NH 8 ) dissolve 0.017 pt. quartz and 0.38 pt. ignited SiO 2 . (Pribram, Z. anal. 6. 119.) Sol. in boiling K 2 CO 3 or Na 2 CO 3 +Aq, separating out on cooling as a gelatinous mass. (Pfaff, Schw. J. 29. 383.) The differ- ent forms of SiO 2 have different degrees of solubilitv in K 2 CO 3 +Aq. Unignited amor- phous SiO 2 from SiF 4 dissolves most readily, then come opal, ignited amorphous SiO 2 , fused SiO 2 , and tridymite; quartz powder is the most difficultly soluble. (Rose.) A similar behaviour is shown to KOH+Aq. Opal is much more sol. in KOH+Aq than quartz, and hyalite is the least sol. of the varieties of opal. (Fuchs.) Opal is easily sol. in KOH+Aq, even after ignition. (Schaffgotsch, Pogg. 68. 147.) Rammelsberg (Pogg. 112. 177) made the following experiments on the solubilitv of SiO 2 in KOH + Aq. The KOH + Aq used~con- tained 1 pt. KOH to 3 pts. H 2 O. 1 pt. of the powdered mineral was boiled half an hour in a silver dish with such an amount of the KOH+Aq that 20 pts. KOH were present. 7.75% of milky white quartz was dissolved by repeating the above process three times. 12.8-15% of gray hornstone was dissolved by twice boiling; 2.43% of moderately finely powdered agate of 2.661 sp. gr. was dissolved by once boiling; 9.7% of unignited hyalite remained undissolved after thrice boiling; 814 SILICON THORIUM OXIDE 21% of ignited hyalite remained undissolved after thrice boiling; 7.21% of semi-opal of 2.101 sp. gr. remained undissolved after thrice boiling; 18.5-19.2% of impure semi- opal of 2.101 sp. gr. remained undissolved after thrice boiling; 79.9% of chalcedony of 2.624 sp. gr. remained undissolved after thrice boiling; 6.12% of chalcedony of 2.567 sp. gr. remained undissolved after fourth boiling; 14.4% chrysophrase of 2.623 sp. gr. remained undissolved after once boiling; 49.41% of chrysophrase of 2.635 sp. gr. re- mained undissolved after thrice boiling; 6.62% of flint of 2.603 sp. gr. remained un- dissolved after twice boiling; 38.1% of fire- opal of 2.625 sp. gr. remained undissolved after fourth boiling; 26.6% of fire-opal of 2.625 sp. gr. remained undissolved after fifth boiling. Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1908, 54. 674.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) The solubility of crystals of quartz on different faces in HF has been determined by Lebrun. (Belg. Acad. Bull. 1913, 953.) Silicon thorium oxide. See Silicate, thorium. Silicon zirconium oxide. .See Silicate, zirconium. Silicon oxychloride, Si 2 OCl6. Decomp. by H 2 and alcohol. Miscible with CS 2 , SiCl 4 , CC1 4 , CHC1 3 , or ether. (Friedel and Ladenburg, A. 147. 355.) Si 4 3 Cl 10 ; Si 4 4 Cl 8 ; Si 8 O 1(J Cl 12 ; (Si, Si 4 O7Cl 2 . Sol. in above oxy chlorides. (Troost and Hautefeuille, Bull. Soc. (2) 36. 360.) OH Silicon oxyfluorhydrin, Si 2 O 3F (Landolt, A. Suppl. 4. 27.) Silicon selenide, SiSe 2 . Decomp. by H 2 O or KOH + Aq. (Sabatier, C. R. 113. 132.) Silicon sulphide, SiS 2 . Sol. in H 2 O with decomp. Acts on alcohol or ether in the cold. (Fremy, A. ch. (3) 38. 314.) SiS. Decomp. by H 2 O; easily sol. in dil. alkalies. (Schiitzenberger, Bull. Soc. (2) 38. 56.) Silicon sulphocfa'amide, SiS(NH 2 ) 2 . Slowly decomp. in the air. Insol. in cold liquid NH 3 . (Blix, B. 1903, 36. 4219.) Silicon sulphobromide. See Silicon bromosulphide. Silicon sulphochloride. See Silicon chlorosulphide. Silicon sulphourea, SiS(NH 2 ) 2 . Slowly decomp. in air. Decomp. by H 2 O. Insol. in cold liquid NH 3 . (Blix, B. 1903, 36. 4219.) Silicone, Si 4 H 4 3 . Insol. in H 2 O, but gives off hydrogen when warmed therewith. Not attacked by chlorine or nitric or sulphuric acids even on heating, but is gradually sol. in HF. Decomp. by alkalies, even by the most dil. NH 4 OH+Aq, with greatest violence and evolution of heat and hydrogen gas. Insol. in alcohol, SiCl 4 , PC1 3 , or CS 2 . (Wohler, A. 127. 257.) H 3 Si 3 O 2 . Decomp. by H 2 O and by dil. acids. Violently decomp. by fuming HNO 3 . Not attacked by cone. H 2 SO 4 . Very slowly decomp. by cone. HC1, rapidly by alkali es-j- Aq and by pyridine. (Honigschmid, M. 1909, 30. 509.) Insol. in H 2 O, alcohol. SiCl 4 , PC1 3 , and CS 2 . Not attacked by acids except HF. (Donath and Liesner, C. C. 1909, II. 1707.). H 12 Sii O 8 . Scarcely attacked by acids, but easily decomp. by hot H 2 O, NaOH+Aq etc. but not by NH 4 OH+Aq. (Kolb, Z. anorg. 1909, 64, 353.) H 10 Si 10 8 . (Kolb.) H 8 Si 8 O 13 . AsH 12 Si 10 O 8 . (Kolb.) Silicowesoxalic acid, Si(OH) 2 (SiO.OH) 2 . Insol. in cold H 2 O, decamp, by hot H 2 O. (Gattermann, B. 1899, 32. 1116.) Silicooxalic acid, Si2H 2 O4-Si 2 O 2 (OH) 2 . Decomp. by bases with evolution of hydro- gen. Takes up HNO 3 to form compound, but not HC1 or H 2 SO 4 . (Troost and Haute- feuille, A. ch. (5) 7. 463.) Silicophosphoric acid, SiO 2 , P2O 6 . Slowly decomp. by H 2 O. Unchanged by alcohol. Exists also in two modifications which are not attacked by H 2 O. (Haute- feuille and Margottet, C. R. 99. 789.) SiO 2 , 2P 2 O 5 +4H 2 O. Decomp. by moist air. Sol. in H 2 O at 0, but decomp. by warm- ing to ordinary temp. (Hautefeuille and Margottet, C. R. 104. 56.) Calcium silicophosphate. See Phosphate silicate, calcium. Silicostannic acid. Calcium silicostannate, Ca(Si,Sn)O 3 . Not attacked by acids, KHSO 4 , or alkalies +Aq. (Bourgeois, Bull. Soc. (2) 47. 297.) SILICOTUNGSTATE, CADMIUM HYDROGEN 815 Silicodea'tungstic acid, 3H 2 O=4H 2 O, SiO 2 , 10WO 3 +3H 2 O. Sometimes sol. in H 2 O, but usually sep- arates out gelatinous silica. (Marignac, A. ch. (4) 3. 55.) See also S&icoduodecitungstic acid. Ammonium silicodea'tungstate, (NH4) 8 W 10 SiO 36 +8H 2 O. Sol. in 4.5 pts. H 2 O at 18. Very sol. in hot H 2 O. (Marignac, A. ch. (4) 3. 59.) (NH 4 ) 6 H 2 W 10 SiO 36 +9H 2 O. (Marignac.) Ammonium potassium , (NH 4 ) 3 K4HSiW 10 O 36 + 15H 2 O. (Marignac.) Barium , Ba4SiW 10 O 3 6+22H 2 O. Precipitate. Insol. in H 2 O. (Marignac.) Potassium , K 8 SiWioO 36 + 17H 2 O. Sol. in H 2 O. (Marignac.) K 4 H 4 SiW 10 O 36 +8H 2 O. Sol. in H 2 O. (Marignac.) Potassium silicotungstate (?), K 8 SiWuO 39 + 14H 2 O. K 4 H 4 SiW n O 39 + 10H 2 O. (Marignac.) Silver , Ag 8 W 19 SiO 36 +3H 2 O. Not appreciably sol. in cold H 2 O. (Marig- nac, A. ch. (4) 3. 65.) Silicotungstic acid or Stticoduodeci- tungstic acid, H 8 SiWi 2 O 4 2. (H 4 SiWi O 4 o, according to Copaux. (Bull. Soc. 1908, (4) 3. 101.) +20H 2 O. Sol. in H 2 O; very sol. in alcohol; behaves with ether as the acid with 22H 2 O (Marignac, A. ch. (4) 3. 10.) +22H 2 O. Solubility as acid with 29H 2 O. 100 pts. deliquesce with 13 pts. ether. To this mixture 20-25 pts. of ether can be added, but a further quantity no longer mixes with, but floats above the mixture. Ethereal solu- tion is miscible with H 2 O. Ether is taken up by a saturated aqueous solution with evolu- tion of heat, until the volume has become doubled; more ether floats on the mixture. By warming the latter a liquid separates out which forms a layer between the two original layers. Alcoholic solution of the acid mixes with an equal vol. of ether, but on adding more ether a cone, ethereal solution separates as a syrupy layer. (Marignac, A. ch. (4) 3. 3. 10.) +29H 2 O. Efflorescent. Sol. in H 2 O. Sat- urated solution at 18 contains 1 pt. crystal- lized acid to 0.104 pt. H 2 O, and has 2.843 sp. gr. Melts in crystal H 2 O. Easily sol. in absolute alcohol and anhydrous ether. +*H 2 O. (Drechsel, B. 1887, 20. 1452.) Aluminum silicotungstate, Al 4 Hi 2 (SiWi 2 O 42 ) 3 +75H 2 O. Not deliquescent; very sol. in H 2 O. (Marignac). Al 4 (SiW 12 4 o) 3 +60H 2 0. (Wyrouboff. Chem. Soc. 1897, 72, (2) 174.) +87H 2 O. (Wyrouboff.) 4-93H 2 O. Very efflorescent. (Wyrouboff.) Aluminum ammonium , Al 4 (NH 4 ) 18 (SiW 12 43 ) 3 +75H 2 0. Sol. in H 2 O. (Marignac.) Ammonium -, basic, (NH 4 ) 4 SiWi 2 O 40 4NH 4 OH + 14H 2 O. (Wyrouboff, Chem. Soc. 1897, 72. (2) 174.) Ammonium , (NH 4 ) 8 SiW :2 O 42 + 16H 2 O. Very sol. in hot H 2 O. (Marignac, A. ch. (4) 3. 17.) (NH 4 ) 4 H 4 SiW 12 O 42 +6H 2 O. Less soluble in H 2 O than the preceding salt. (Marignac.) (NH 4 ) 4 SiW 12 40 +8H 2 0. (Wyrouboff, Chem. Soc. 1897, 72. (2) 174.) Barium , Ba 2 H 4 SiW 12 O< 2 + 14H 2 O. Sol. in H 2 O. +22H 2 O. Gradually efflorescent. (Marig- nac.) Sol. in cold H 2 0, 1 : 0.7 pts. (Copaux, Bull. Soc. Min. 1906, 29. 80.) Sol. in 4 pts. cold H 2 O. (Wyrouboff, Bull. Soc. Min. 1896, 19. 278.) Ba 4 SiWi 2 O 42 +27H 2 O. Nearly insol. in cold, si. sol. in hot H 2 O. (Marignac.) Ba 2 SiWi 2 O 40 + 16H 2 O. (Wyrouboff.) Barium potassium , Ba 2 K 2 SiWi 2 O 40 -f- 17H 2 O. (Wyrouboff, Chem. Soc. 1897, 72. (2) 176.) Barium sodium -, Na<.Ba 3 SiWi 2 O.- 2 -f- 28H 2 O. H 2 O gradually dissolves out sodium silico- tungstate. Cadmium , Cd 2 SiW 12 O 40 +23H 2 O, and +27H 2 O. (Wyrouboff.) 4CdO, 3(SiO 2 , 12WO 3 )+4H 2 O. (Wyrou- boff.) Caesium , Cs 8 SiWi 2 O 42 . 100 pts. H 2 O dissolve only 0.005 pt. at 20; 0.52 pt. at 100. Completely insol. in alcohol, and HCl+Aq. Somewhat sol. in dil. NH 4 OH+Aq. (Godef- froy, B. 9. 1363.) Cadmium hydrogen , 2Cd 2 SiWi 2 O 40 , H 4 SiW 12 O, +42H 2 O. (Wyrouboff.) 816 SILICOTUNGSTATE, CALCIUM Calcium silicotungstate, Ca 2 H 4 SiWi 2 O 42 20H 2 O. Not deliquescent. Extremely easily sol in H 2 O. (Marignac.) Ca 2 SiW 12 O 40 + 18, 24 and 27H 2 O. (Wyrou- boff.) Calcium silicotungstate nitrate, Ca 2 SiWi 2 O 40 Ca(NO 3 ) 2 + 15H 2 O. (Wyrouboff.) Cerous , Ce 2 SiW 12 O 4 o+27H 2 O. (Wyrouboff.) Ce 2 SiW 12 O 4 o, CeH 2 SiWi 2 O, -|-34H 2 O. (Wyrouboff.) Chromium - , Cr 4 (SiWi 2 O 40 ) 3 +60, 87 and 93H 2 O. (Wyrouboff.) Cupric -- , Cu 2 SiW 12 O 40 +18, 27 and 29H 2 O. Very efflorescent. (Wyrouboff.) Didymium - , Di 2 SiW 12 O 40 +26 and 27H 2 O. (Wyrouboff.) Di 2 SiW 12 0, ;0 , DiH 2 SiW 12 40 +34H 2 0. (Wyrouboff.) Gallium , Ga 4 (SiW 12 O 40 ) 3 +60, 87, and 93H 2 O. (Wyrouboff.) Glucinum - -, Gl 4 (SiW 12 d 40 ) 3 +45, 87 and 93H 2 O. (Wyrouboff.) Indium - , In 2 O 3 , H 2 O, 2(SiO 2 , 12WO 3 ) + 40H 2 O. (Wyrouboff.) 2In 2 O 3) 3(SiO 2 , 12WO 3 )+63 and 93H 2 O. (Wyrouboff.) Iron (ferric) - , Fe 4 (SiW ]2 O 40 ) 3 +60 and 93H 2 0. (Wyrouboff.) Lanthanum , La 2 SiWi 2 O 40 +27H 2 O. Efflorescent. (Wyrouboff.) La 2 SiWi 2 O. .LaH 2 SiW 12 O 40 +34H 2 O. (Wyrouboff.) Lead - , basic, Pb 2 SiW 12 O 40 , 2PbO+20H 2 O. SI. sol. in H 2 O. (Wyrouboff.) Lead - , Pb 2 SiWi 2 O 40 +21 H 2 O. Sol. in H 2 O. (Wyrouboff.) Lithium , Li 2 O, SiO 2 , 12WO 3 + 14 and 24H 2 0. (Wyrouboff.) Magnesium , Mg 2 H 4 SiWi 2 O 42 Stable on the air. (Marignac.) Mercurous silicotungstate, basic, H g4 SiW 12 O 40 , 2Hg 2 O+5H 2 O. Insol. inH 2 O. Insol. in dil. HNO 3 . Slowly sol. in cone. warm. HNO 3 . (Wyrouboff.) Mercurous - , Hg 8 SiWi 2 O 42 . Insol. in H 2 O. Scarcely sol. in dil. HNO 3 + Aq. (Marignac, A. ch. (4) 3. 43.) Mercuric - , Hg 2 SiW 12 O 40 + 15H 2 O. Very sol. in H 2 O. Solution decomp. on boiling. (Wyrouboff.) Potassium - , basic, K 4 SiW 12 O 40 , 4KOH + 12H 2 O. 1 pt. is sol. in 10 pts. H 2 O at 18. (Wyrou- boff.) Potassium - , K 8 SiWi 2 O 4 Sol. in 10 pts. H 2 O at 18, and less than 3 pts. at 100. (Marignac.) +20H 2 O. Much less sol. in cold than hot H 2 O. Extremely sol. in hot H 2 O. More sol. than above comp. (Marignac.) K 4 ELSiW 12 O 42 +7H 2 O. Solubility as pre- ceding salt. K 4 H 4 SiW 12 O 42 + 16H 2 O. Sol. in 3 pts. H 2 O at 20. K 6 H: 9 (SiWi 2 O., 2 ) 2 +25H 2 O. Decomp. by dissolving in H 2 O. (Marignac.) K 4 SiW 12 O 0+6 and 15H 2 O. (Wyrouboff.) K 4 SiW 12 O 40 , K 2 H 2 SiW ]2 O 40 -f29H 2 O. (Wyrouboff.) Rubidium - , Rb 8 SiW 12 O 42 . Sol. in 145-150 pts. H 2 O at 20 and in 19-20 pts. at 100. Insol. in alcohol; difficultly sol. n acidified, but extremely easily in ammonia- cal H 2 O. (Godeffroy, B. 9. 1363.) Rb 2 H 2 SiW 12 O 40 +5H 2 O. (Wyrouboff.) Rb 4 SiW 12 O 40 , Rb 2 H 2 SiWi O 40 +22H 2 O. Wyrouboff.) Silver - , Ag 4 H 4 SiW 12 O 42 +7H 2 O. Very si. sol. in H 2 O; sol. in dil. HNO 3 + Aq. (Marignac.) SI. sol. in H 2 O. (Wyrouboff.) Sodium - , basic, Na 4 SiW 12 O 40 , 4NaOH + 5H 2 O. (Wyrouboff.) Sodium - , Na 8 SiW 12 O 42 +7H 2 O. The saturated solution at 19 contains 0.21 pt. H 2 O to 1 pt. of the salt dried at 100, and las sp. gr. = 3.05. (Marignac.) Na 4 H 4 SiWi 2 O 42 + llH 2 O. Stable on air. + 18H 2 O. Efflorescent. (Marignac.) Na 2 H 6 SiWi 2 O 42 + 14H 2 O. Decomp. by dis- solving in H 2 O. (Marignac.) Na 4 SiW 12 O 40 +14, 16 and 20H 2 O. (Wyrou- >off.) SILVER 817 Sodium silicotungstate nitrate, 3Na 4 H 4 SiW 12 Q4 2 , 4NaNO 3 +39H 2 O. Slightly deliquescent. (Marignac.) Strontium - , Sr 2 SiW 12 CU+16, 17, 23 and 27H 2 O. (Wyrouboff.) Thallium -- , Tl 2 H 2 SiW 12 O 40 +9H 2 O. (Wyrouboff.) Thorium , basic. Insol. in H 2 O. (Wyrouboff.) Thorium - , Th 2 SiWi 2 O 40 +27H 2 O. Very sol. in H 2 O. (Wyrouboff.) Th 2 SiW 12 O 40 , 2H 4 SiW 10 O 40 +45H 2 O. (Wyrouboff.) Uranium - . Thirteen salts are described by Wyrouboff. Uranyl - . Seven salts are described by Wyrouboff. Zinc -- , Zn 2 SiWi 2 O 40 +18, 27 and 29H 2 O. (Wyrouboff.) Silicovanadiomolybdic acid. Ammonium silicovanadiomolybdate, 3(NH 4 ) 2 O, SiO 2 , V 2 O 5 , 9MoO 3 +20H 2 O. Sp. gr. of sat. solution containing 0.32016 g. salt in 1 ccm. at 18 = 1.21322. (Friedheim, B. 1900, 33. 1624.) 3(NH 4 ) 2 O, SiO 2 , V 2 O 6 , 10MoO 3 +21H 2 O. Sp. gr. of sat. solution containing 0.35026 g. of salt in 1 ccm. at 18 = 1.25275. (Fried- heim.) 3(NH 4 ) 2 O, V 2 O 5 , SiO 2 , HMoO 3 +27H 2 O. Sp. gr. of sat. solution containing 0.38086 g. salt in 1 ccm. at 18 = 1.29266. (Triedheim.) 3(NH 4 ) 2 O, V 2 O 5 , SiO 2 , 15MoO 3 +24H 2 O. Sp. gr. of sat. solution containing 0.48997 g. salt in 1 ccm. at 18 = 1.43761. (Friedheim.) Ammonium potassium (NH 4 ) 2 O, 2K 2 O, SiO 2 , V 2 O 5 , 9MoO 8 +20H 2 O. Sp. gr. of sat. solution containing 0.24021 g. salt in 1 ccm. at 18 = 1.17031. (Fried- heim.) , 2K 2 0, Si0 2 , V 2 5 , 10MoO,+ 21H 2 O. Sp. gr. of sat. solution contain- ing 0.25914 g. salt in 1 ccm. at 18 = 1.19184. ( Friedheim.) (NH 4 ) 2 O, 2K 2 O, SiO 2 , V 2 O 5 , HMoOH- 12H 2 O. Sp. gr. of sat. solution contain- ing 0.27914 g. salt in 1 ccm. at 18 = 1.21378. ' (Friedheim.) Ammonium zinc , 4(NH 4 ) 2 O, 2ZnO, 2SiO 2 , 3V 2 O 6 , 18MoO 3 + 15H 2 O. SI. sol. in H 2 (X (Blum, Dissert. 1904.) Silicovanadiotungstic acid. Ammonium silicovanadiotungstate, 3(NH 4 ) 2 O, SiO 2 , V 2 O 5 , 9WO 3 +24H 2 O. Can be cryst. from H 2 O. (Friedheim, B. 1902, 36. 3244.) (NH 4 ) 6 SiV 2 W 10 O 4 o+21H2O. 1 cc. of sat. solution in H 2 O at 17.5 contains 0.6652 g. of the hydrated salt. Sp. gr. of this solution = 1.4505. Decomp. by cone, acid and alkali. (Friedheim.) Ammonium barium potassium , (NH 4 ) 2 K 2 BaSiV 2 W 10 O 40 +25H 2 O. SI. sol. in H 2 O. Decomp. by cone, acids and alkalies. (Friedheim.) Ammonium potassium (NH,)K 5 SiV 2 W 10 O 40 +23H 2 O. 1 ccm. of sat. solution at 17.5 contains 0.5072 g. of the salt. Sp. gr. of the solution at 20 = 1.3462. Can be cryst from H 2 O. Decomp. by cone, acids and alkalies. (Fried- heim.) Barium , Ba 3 SiV 2 W 10 O 40 -|-28H 2 O. 1 ccm. of the sat. solution in H 2 O at 17.5 contains 0.0384 g. of the salt. Sp. gr. of the solution = 1.0307. Decomp. by cone, acids and alkalies. (Friedheim, B. 1902, 35. 3245.) 6BaO, 2SiO 2 , 3V 2 O 6 , 18WO 3 +50H 2 O. SI. sol. in H 2 O. (Friedheim.) 7BaO, 2SiO 2 , 3V 2 O 6 , 18WO 3 +83H 2 O. SI. sol. in H 2 O. (Friedheim.) Potassium , K6SiV 2 WioO 4 o+22H 2 O. Sol. in H 2 O. Can be cryst. from H 2 O without decomp. Decomp. by cone, acids and alkalies. (Friedheim.) 6K 2 O, 2SiO 2 , 3V 2 O 5 , 18WO 3 +31H 2 O. Sol. in H 2 O. (Friedheim.) 7K 2 O, 2SiO 2 , 3V 2 O 5 , 18WO 3 -|-42H 2 O. Sol. in H 2 O. (Friedheim.) Sodium , Na6SiV 2 WioO 4 o+29H 2 O. Very sol. in H 2 O. Decomp. by cone acids and alkalies. (Friedheim.) Silundum, Si x C y . Not attacked by hot Cl or cone, acids. (Amberg, Z. Elektrochem. 1909, 15. 725.) Silver, Ag. Not attacked by H 2 O. Absolutely insol. in HC1 or HC 2 H 3 O 2 +Aq. (Lea, Sill. Am. J. 144. 444.) Easily sol. in HNO 3 +Aq on warm- ing, if not too cone. Only a minute trace is dissolved in an hour by cold dil. HN0 3 +Aq (1 pt. HNO 3 +Aq of sp. gr. 1.40 : 10 pts. H 2 O). (Lea.) Sol. in hot cone. H 2 SO 4 with evolution of SO 2 . SI. sol. in dil. H 2 SO 4 -j-Aq (1 . 4), but with more dil. H 2 SO 4 +Aq the different forms of Ag behave differently. (Lea.) Sol. in HI-fAq at ordinary temperature. 818 SILVER ACETYLIDE Sol. in KI+Aq with access of air. Sol. in hot KCN+Aq. (Christomanos, Z. anal. 7. 301.) Sol. in chromic, iodic, chloric and bromic acids. Dil. H 2 SO<- alone is incapable of dis- solving finely divided Ag, and the seeming solvent action is due to the oxygen of the air, oxygen dissolved in the acid, or derived from some external source. (Hendrixson, J. Am. Chem. Soc. 1903, 25.637.) Boiling H 2 SO4 dissolves pure Ag only when concentration equals 60 B. More dil. acid dissolves only the impure metal. (Pannani, Gazz. ch. it. 1909, 39. (2) 234.) Slowly decomp. into AgCl by alkali chlor- ides +Aq; also by CuCl 2 , etc.+Aq. Somewhat sol. in NH 4 OH+Aq in presence of O. (Lea, Sill. Am. J. 144. 444.) Sol. in KMnO 4 +dil. H 2 SO 4 +Aq. (Fried- heim, B. 20. 2554.) Sol. in Fe 2 (SO 4 ) 3 +Aq, especially on heat- ing, but completely insol. in FeSO 4 +Aq. (Vogel.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Allotropic forms (a). Very sol. in H 2 O. Solution is pptd. by saline solutions or almost any neutral substance. Alkali sulphates, nitrates, and citrates ppt. it in a sol. form, while MgSO 4 , CuSO 4 , FeSO,, NiSO 4 , K 2 Cr 2 O 7 , K 4 Fe(CN) 6 , Ba(NO 3 ) 2 , and even AgNO 3 +Aq ppt. it in an insol. form, which, however, may be made sol. again by treatment with many substances, as Na 2 B 4 O 7 , K 2 SO 4 , or Na 2 SO 4 + Aq. NaNO 2 +Aq ppts. the Ag from its solu- tion in a perfectly insol. form. (j8). The ppt. from aqueous solution by salts is sol. in NH 4 OH+Aa. (Lea, Sill. Am. J. 137. 476.) Many other allotropic forms exist. (Lea.) Pure colloidal silver is also sol. in alcohol. Schneider, B. 25. 1164.) Entirely sol. in H 2 O, even when dry. (Schneider, Z. anorg. 1894, 7. 339.) Silver acetylide, Ag 2 C 2 . . Sol. in KCN+Aq with evolution of C 2 H 2 . Decomp. by HCl+Aq. (Arth, C. R. 1897, 124. 1535.) Silver amide, AgNH 2 . Ppt.; sol. in ammonium salts+Aq and in excess of potassium amide. Sol. in liquid NH 3 . Insol. in Ag salts+Aq. (Franklin, J. Am. Chem. Soc. 1905, 27. 833.) Sol. in excess of KNH 2 . (Franklin, Z anorg. 1905, 46. 16.) Silver antimonide, Ag 2 Sb or Ag 4 Sb. Min. Discrasite. Sol. in HNO 3 +Aq Ag 3 Sb. Insol. in HCl+Aq; decomp. bj HNO 3 +Aq. (Christofle.) Silver azoimide, AgN 3 . Insol. in hot or cold H 2 O or dil. acids; sol in cone, mineral acids. Sol. in NH 4 OH+Aq (Curtius, B. 23. 3023.) Silver bromide, AgBr. Insol. in H 2 O, or H 2 O acidulated with HNO 3 , H 2 SO 4 , or HC 2 H 3 O 2 between and 33. If flbcculent or pulverulent, it is sensibly sol. therein above 33, but if granular only above 50, and then very slightly. (Stas, A. ch. (5) 3. 289.) Ag can be detected as AgBr n 10,000,000 pts. H 2 O. (Stas.) Calculated from the electrical conductivity of AgBr+Aq, AgBr is sol. in 1,971,658 pts. H 2 O at 20.2, and 775,400 pts. at 38. (Holle- man, Z. phys. Ch. 12. 133.) By same method Kohlrausch and Rose cal- culate that 1 1. H 2 O dissolves 0.4 mg. AgBr at 18. (Z. phys. Ch. 12. 240.) Solubility in H 2 O = 0. 109 mg. per 1. (Prud- homme, J/chim. Phys. 9. 519.) Solubility in H 2 O = 6.6 X 10~ 7 at 25. (Good- win, Z. phys. Ch. 1894, 13. 645.) Solubility of AgBr in H 2 O at 25 equals 8.1 X10- 7 g. mols. per 1. (Thiel, Z. anorg. 1900. 24. 57.) Aq. solution sat. at 21.1 contains 0.57 X 10~ 6 gr. equiv. per litre. (Kohlrausch, C. C. 1901, II. 1299.) 1 1. H 2 O dissolves 0.000137 g. AgBr at 25. (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) 0.84 X 10 4 g. are dissolved per liter of sat. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) 1 l.H 2 O dissolves 0.107 mg. AgBr at 21. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 3.7 mg. AgBr are contained in 1 liter of sat. solution at 100. (Bottger, Z. phys. Ch. 1906, 56. 93.) 1 mg. in 1 1. of sat. solution at 21. (Kohl- rausch, Z. phys. Ch. 1908, 64. 168.) Solubility in H 2 O=8.8XH)- 7 g. mol. per litre at 25. (A. E. Hill, J. Am. Chem. Soc. 1908, 30. 74.) Boiling H 2 O dissolves 0.000003502 of its weight of AgBr. HNO 3 +Aq (1% HNO 3 ) dissolves 0.00000543 of its weight of AgBr at 100 with si. decomposition. The solution is pptd. by AgNO 3 +Aq or HBr (or MBr) + Aq, but not completely. I pt. of AgBr m solution requires 3 pts. of Br as MBr (or HBr), or of Ag as AgNO 3 in order to be wholly precipitated. (Stas.) Not attacked by boiling HNO 3 +Aq; si. sol. in cone. HBr or HCl+Aq (Lowig). Boiling cone. H 2 SO 4 decomposes it (Balard), hardly acts on it (Dumas), dissolves a small quantity, which is repptd. by H 2 O (Berze- Very si. sol. in dil., easily in cone. NH 4 OH +Aq. 100 pts. NH 4 OH+Aq (0.986 sp. gr.) dissolve 0.51 pt. AgBr (dried at 100) at 80, and about double that amount of freshly pptd. AgBr. (Pohl, W. A. B. 41. 2670 1 g. freshly pptd. AgBr is sol. in 250 ccm. 10% NH 4 OH+Aq, but insol. in an ammoma- cal solution of AgCl. (Seiner, Pharm. J. T e; S AgBr dissolves in 8779.4 g. 5% NH 4 OH +Aq (sp. gr.= 0.998) at 12, and in 288.5 g. SILVER BROMIDE 819 10% NH 4 OH+Aq (sp. gr.=0.96) at 12. (Longi, Gazz. ch. it. 13. 87.) Solubility of AgBr in NH 4 OH+Aq at 15. G. mols. per 1. NH 3 AgBr Sp. gr. 15.5 1.085 2.365 3.410 4.590 5.725 0.0011 0.0031 0.0050 0.0074 0.0101 0.9932 0.9853 0.9793 0.9720 0.9655 (Bodlander, Z. phys. Ch. 1892, 9. 734.) Solubility in NH 4 OH+Aq at 0. 10 ccm. of the solution contain g. NH 3 and mg. Ag Br. g. NH 3 Mg. AgBr g. NH 3 Mg. AgBr 0.307 8.0 2.627 106.7 0.488 9.6 3.126 156.8 0.669 17.2 3.389 198.7 0.829 21.2 3.652 266.9 1.151 34.9 3.722 288.8 1.532 55.7 3.770 293.0 1.809 72.2 3.926 289.2 ' 1.953 74.1 3.995 285.0 (Jarry, A. ch. 1899, (7) 17. 364.) Solubility of AgBr in NH 4 OH+Aq at 25. G. mols. per 1. NH 3 AgBr NH 3 AgBr 0.1932 0.3849 0.7573 0.00060 0.00120 0.00223 1.965 3.024 5.244 0.00692 0.01163 0.02443 (Bodlander and Fittif, 1902, Z. phys. Ch. 39. 597.) Solubility in NH 4 OH+Aq at 25. g. at. Ag per 1. Mols. NH 3 per 1. 0.00170 0.00159 0.000941 0.00107 0.000391 0.000386 0.000276 0.000264 0.450 0.497 0.268 0.273 0.115 0.118 0.0764 0.0777 (Whitney and Melcher, J. Am. Chem. Soc. 1903, 25. 79.) Sol. in hot NH 4 Cl+Aq. Very si. sol. in NH 4 carbonate, sulphate, or succinate+Aq, and still less in nitrate. (Wittstein.) Not very easily sol. in Na 2 S 2 O 3 +Aq when sus- pended in much H 2 O, and is separated out again by KBr+Aq. (Field, C. N. 3. 17.) Sol. in KCN+Aq. SI. sol. in cone. KC1, KBr, NaCl, NaBr, NH 4 C1, or NH 4 Br+Aq; but insol. when dilute. Traces only dissolve in alkali nitrates +Aq. (Fresenius, C^uant. Anal.) Abundantly sol. in Hg(NO 3 ) 2 +Aq. 100 ccm. H 2 O containing 10 ccm. normal Hg(NO 3 ) 2 +Aq dissolve 0.0383 g. AgBr. (Stas.) Solubility of AgBr in Hg(NO 3 ) 2 +Aq at 25. G. mols. per 1. Hg(NO 3 )2 HNOs AgBr Hg(N0 3 ) 2 HNO 3 AgBr 1 0.10 0.05 0.03660 0.00873 0.00639 0.025 0.0125 0.0100 0.00459 0.00329 0.00306 HNO 3 was present in all cases, and it was found that there was no difference in solubil- ity of AgBr with concentrations between 0.1N and 2N HNO 3 . Cryst. and amorphous AgBr showed the same solubility. (Morse, Z. phys. Ch. 1902, 45. 708.) Difficultly sol. in hot cone. AgNO 3 +Aq. (Risse, A. 111. 39.) 100 ccm. of a 3-N solution of AgNO 3 dis- solve 0.04 g. AgBr at 25. Much less sol., in AgNO 3 +Aq than Agl. (Hellwig, Z, anorg. 1900, 25. 176.) Solubility in AgNO 3 +Aq. Volumetric measurements AgNOa N/10 KBr ccm. Opal- escent at G. AgBr retained per 100 g. AgNOs c 0.65 22 0.129 0.72 35 0.144 10 g. made up to 0.8 44 0.159 32 g. per 100 g. < 0.9 62 0.178 of solution 1.0 67 0.188 1.1 77 0.207 t 1.2 79 0.226 6.0 37 1.13 8.0 53 1.50 10.0 67 1.88 10 g. made up to 11.25 72 2.12 70 g. per 100 g. - 12.0 74 2.26 of solution 12.75 79 2.40 13.5 82 2.54 15.5 85.5 2.92 17.5 90 3.29 Gravimetric measurements at 14.5 G. AgNOa ccm. H 2 O Strength of AgNOs % G. AgBr re- tained per 100 g. AgNOs 7.326 8.290 7.255 7.35 9.32 7.65 4.84 3.95 44 52 60 65 0.144 0.185 0.283 0.365 (Lowry, Roy. Soc. Proc. 1914, 91. A, 65.) 820 SILVER BROMIDE 100 g. KBr in cone. KBr+Aq dissolve 3019 mg. AgBr at 15; 95 g. NaCl + 10 g. KBr dis- solve only 75 mg. AgBr at 15. (Schierholz, W. A. B. 101, 2b. 4.) Solubility in KBr+Aq at 25. Solubility in salts +Aq. Solvent Cone. Grams AgBr sol. in 100 grams solvent Sodium thiosulphate 25 Mol. KBr in 1 litre G. AgBr in 1 litre 4.864 4.44 4.18 3.68 2.81 2.76 26.44 17.95 13.50 7.50 2.34 2.20 (Hellwig, Z. anorg. 1900, 26. 183.) Sol. in cone. KBr or NaBr+Aq (Lowig), but less than Agl in KI+Aq (Field). 100 g. NaCl in cone. NaCl+Aq dissolve 474 mg. AgBr at 15; 100 g. NaCl in 21% NaCl+Aq dissolve 188 mgr. AgBr at 15. (Schierholz, W. A. B. 101, 2b. 4.) Solubility of AgBr in Na 2 SO 3 +Aq at 25. G. formula weights per 1. (Valenta, M. 1894, 16. 250.) Solubility of AgBr in salts +Aq at (?). (G. AgBr sol. in 1 1. of 1% solution of salts.) NaSCN 2.06 Sos Ag Sos Ag 0.232 0.0025 0.406 0.0023 0.448 0.00,23 0.466 0.0053 0.474 0.0055 0.675 0.0084 (Luther and Leubner, Z. anorg. 1912, 74. 393.) Solubility of AgBr in Na 2 SO 3 at (?). (g. salts per 1. of solution.) NH 4 SCN (NH 4 ) 2 C0 3 Na 2 SO 4 0.03 0.004 0.055 Na 2 S0 3 AgBr Na 2 SO 3 AgBr 83.75 70.75 38.2 17.65 9.47 4.85 0.790 0.570 0.265 0.116 0.0526 0.0329 2.08 1.13 0.59 0.3 0.17 0.08 0.0159 0.0086 0.0045 0.0039 0.0022 0.00075 (Mees and Piper, Photog, J. 1912, 36. 234.) Solubility in Na 2 S 2 O 3 +Aq at 35. g. Na 2 S2Os in 1 liter 100 200 300 500 g. AgBr corresponding to each g. 0.376 0.390 0.397 0.427 (Richards and Faber, Am. Ch. J. 1899, 21. 169.) (NH 4 ) 2 S 2 O 3 +Aq. dissolves AgBr more rapidly than does Na 2 S 2 O 3 +Aq. (Lumie"re and Seyewitz, C. C. 1908, II. 1138.) (Mees and Piper, Photog. J., 1912, 36. 234.) In a solution of NaC 2 H 3 O 2 +Aq, containing 10 ccm. of sat. NaC 2 H 3 O 2 +Aq at 15 and 20 ccm. normal HC 2 H 3 O 2 +Aq mixed with 970 ccm. H 2 O, about double the amt. of floc- culent AgBr is dissolved in the cold that is dissolved by boiling H 2 O from granular AgBr. This solution required 3 pts. of Ag or Br to ppt. the AgBr in solution. Pulverulent or granular AgBr are wholly insol. in dil. or cone, acetates +Aq. (Stas.) Sol. in Hg(C 2 H 3 O 2 ) 2 +Aq. 100 ccm. H 2 O containing 10% of normal Hg(C 2 H 3 O 2 ) 2 +Aq dissolves 0.0122 g. AgBr at 20. (Schierholz.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Solubility in 10 cc. methylamine+Aq of different concentrations at 11.5. g. NH 2 CH 3 4.844 4.311 3.562 3.258 mg. AgBr 289 127 73 55 g. NH 2 CH 3 1.797 1.513 1.317 1.101 mg. AgBr 28 16 12 7 (Jarry, A. ch. 1899, (7) 17. 378.) SILVER CHLORIDE 821 Solubility in methylamine+Aq at 25. G. mol. per 1. CHNH 2 AgBr 0.02 0.04 0.074 0.0947 0.1950 0.00026 0.00034 0.000395 0.00041 0.00045 (Wuth, B. 1902, 36. 2416.) Solubility of AgBr in methylamine+Aq at 25. G. mol. per 1. CH 3 NH 2 1.017 0.508 0.203 AgBr CHsNJ 0.0025 0.0013 0.00049 o.io; 0.051 AgBr 0.00026 0.00012 (Bodlander and Eberlein, B. 1903, 36. 3948.) Solubility in ethylamine+Aq at 25. G. mol. per 1. C 2 H 5 NH 2 AgBr 0.01272 0.03942 0.05512 0.05572 0.10300 0.0000867 0.000137 0.000193 0.000258 0.000711 (Wuth, B. 1902, 35. 2416.) At 25, 1 1. ethylamine+Aq containing 0.483 g. mol. CANHa dissolves 0.00231 g. mol. AgBr; 0.200 g. mol. C 2 H 5 NH 2 , 0.0097 g. mol. AgBr. (Bodlander and Eberlein, B. 1903, 36. 3948.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in acetone. (Eidmann, C. C. 1899, II, 1014); (Naumann, B. 1904, 37. 4329.) Sol. in alcoholic thiourea. (Reynolds, Chem. Soc. 1892, 61. 251.) Insol. in methyl acetate. (Bezold, Dissert. 1906); (Naumann, B. 1909, 42. 3790.) ethyl acetate. (Hamers, Dissert. 1906); (Naumann B. 1910, 43. 314.) 1.49 g. AgBr is dissolved in 1 1. of 1% thio- carbamide+Aq. (Mees and Piper, Photog. J. 1912, 36. 239.) Insol. in warm pyridine. Mol. wt. determined in piperidine. (Wer- ner, Z. anorg. 1897, 15. 16.) Min. Bromyrite, Bromite. Silver bromide ammonia, AgBr, NH 3 . (Joannis and Crozier, C. R. 894, 118. 1150.) AgBr, 1^NH 3 . (Jarry, A. ch. 1899, (7) 17. 356.) 2 AgBr, 3NH 3 , (Joannis and Crozier.) AgBr, 3NH 3 . Decomp. by H 2 O. SI. sol. in liquid NH 3 . (Jarry.) AgBr, 5NH 3 . (Jarry, C, R. 1898, 126. 1141.) Silver carbide, Ag 4 C. (Gay-Lussac.) . Ag 2 C(?). Sol. in HNOg+Aq with residue ofC. (Liebig, A. 38. 129.) Ag 2 C 2 . Sol. in HNO 3 +Aq with residue of C. (Regnault, A. 19. 153.) Silver swfrchloride, Ag 4 Cl 3 . NH 4 OH+Aq dissolves the greater part, the residue (20%) being sol. in HNO 3 +Aq. KCN dissolves the greater part; H 2 SO 4 dis- solves about 2%; acetic acid and KOH are without action. (Bibra, J. pr. 1875, (2) 12. 52.) Argentous chloride, Ag 2 Cl. Obtained in a pure state by Guntz (C. R. 112. 861). Dil. HNO 3 +Aq does not attack but warm cone. HNO 3 +Aq decomp. Easily sol. in KCN+Aq. (Guntz, C. R. 112. 1212.) The following data are for a more or less impure Ag 2 Cl. Boiling cone. HCl+Aq, NaCl+Aq, or NH 4 OH+Aq dissolve out AgCl, and leave Ag. (Scheele, Wetzlar, Bulk, Wohler.) According to Berthollet, wholly sol. in NH 4 OH +Aq. Sol. for the most part in NH^OH-f-Aq, and the resi- due is sol. in HNOs+Aq ( =Ag +AgCl). (v. Bibra, B. 7. 741.) . Silver chloride, AgCl. Nearly insol. in H 2 O. When AgCl is left in contact for some hours with pure H 2 O at 20-22, and especially at 75, traces go into solution; more Cl is dissolved than Ag. When 1 pt. Ag is pptd. as AgCl in presence of 1 million pts. H 2 O a slight bluish milkiness is observed; but in order to have a distinct ppt. 4 pts. Ag should be present. Dil. HNO 3 +Aq does not increase the solu- bility of AgCl, but AgCl is not absolutely insol. in stronger HNO 3 +Aq. (Mulder.) I pt. AgNO 3 , when mixed with HCl+Aq in presence of 120.000 (Pfaff), 240,000 (Hart- ing), pts. H 2 O, causes an opalescence. 1 pt. Ag gives a slight turbidity with HC1 + Aq in presence of 200,000 pts. H 2 O, a scarcely opalescent cloudiness with 400,000 pts. H 2 O, and the same after the lapse of 15 minutes in presence of 800,000 pts. H 2 O. (Lassaigne.) I pt. Ag can be detected as AgCl in 1 mil- lion parts H 2 O at ordinary temp., but not in 2 million parts. In NaNO 3 +Aq containing 0.79 pt. NaNO 3 in 200,000 pts. H 2 O, 1 pt. Ag can be detected as AgCl. This dissolves at 75, and is visible again on cooling. If the same liquid contains 1574 pts. NaNOj, the AgCl remains in solution after cooling. 822 SILVER CHLORIDE In 100 ccm. H 2 O containing 0.787 g. NaNO 3 , 13 drops of NaCl and silver solution, each drop of which contains 0.05 mg. Ag, cause a precipitate at 5, 20 drops at 15-17, 60 drops at 45-55. AgCl is somewhat less sol. in HNO 3 +Aq than in NaNO 3 +Aq when the amount of H 2 O remains the same. Therefore, if HC1 is used instead of NaCl, about l li less AgCl remains in solution. In 100,000 pts. of H 2 O, which contain HNO 3 and an amount of HCl corresponding to the amount of Ag salt, 1.596 pts. AgCl dissolve at 25. The solution is precipitated by either AgNO 3 or HC1. (Mulder, Silber "Probir- methode, Leipzig, 1869. 62.) (For further older data, see Storer's Dic- tionary.) White flaky AgCl is appreciably sol. in hot H 2 O, 1000 ccm. boiling H 2 O dissolving about 2 mg. AgCl. Far less sol. in H 2 O containing AgNO 3 , being practically insol. in H 2 O con- taining 0.1 g.- AgNO 3 in a litre. Solubility is also diminished one-half by addition of HC1. (Cooke, Sill. Am. J. (3) 21. 220.) Solubility in H 2 O rapidly diminishes as the temp, falls. (Cooke, I. c.) Not completely insol. in H 2 O. According to Stas (C. R. 73. 998) there are four modifica- tions: (1) gelatinous; (2) cheesy-flocculent; (3) pulverulent; (4) granular, crystalline, or fused. (4) is almost absolutely insol. in H 2 O at the ordinary temp., but the solubility in- creases with the temp., and is considerable at 100; (2), which is formed by the pre- cipitation of a cold dilute Ag solution, has the greatest solubility in pure H 2 O; and it changes its solubility by standing, or if made pulverulent by shaking with H 2 O; (3) is also sol. in H 2 O; the solution of (2) or (3) in pure H 2 O, or H 2 O acidified with HNO 3 , is precipi- tated by AgNO 3 or NaCl+Aq. In order to ppt. 1 pt. AgCl in above solu- tion 3 pts. of Cl as chloride or Ag as nitrate are necessary; the pptn. is then complete. Solubility of granular variety in boiling H 2 O is proportionately large, and pptn. is brought about by 3 pts. Cl or Ag as above, but the pptn. in this case is not complete. The salts formed simultaneously with the AgCl have no influence on the solubility of the AgCl. Presence of HNO 3 does not increase the solubility of (2), but has that effect on (3) in proportion to the amt. of HNO 3 pre- sent. (Stas, C. R. 73. 998.) Further determination by Stas are as follows: Between and 30 granular AgCl is insol. in pure H 2 O, or H 2 O acidulated with HNO 3 . Between and 30 the flocculent and pul- verulent forms of AgCl dissolve without alteration in pure H 2 U, in acidulated H 2 O, in alkali acetates +Aq, and in Hg(C 2 H 3 O 2 ) 2 +Aq containing an alkali acetate. Their degree of solubility is a function of the state of the chloride, of the temp., and of the nature and quantity of the solvent within these limits of temp. (0-30). These solvents, if they contain either Ag in the state of an Ag salt, or Cl as chloride or HCl in an amount three times that which they can dissolve as AgCl, exercise no solvent action on any of the modifications of AgCl. And reciprocally sat. AgCl+Aq is pptd. instantly by a decinormal solution of AgNO 3 or MCI. (or HCl). The AgCl is wholly pptd. when the quantity of the Ag or Cl thus added is equal to three times the quantity of the Ag or Cl dissolved as AgCl. Between 50 and 100, however, decinormal solutions of Ag or chlorides, which cause instant ppts. in solutions sat. with any of the modifications of AgCl, do not eliminate all the dissolved AgCl. At 100, they only ppt. 60% of the amt. dissolved. (Stas, A. ch. (5) 3. 323.) Calculated from electrical conductivity of AgCl +Aq, AgCl is sol. in 715,800 pts. H 2 O at 13.8, and 384,100 pts. at 26.5. (Holle- man, Z. phys. Ch. 12. 132.) Calculated in the same way, 1. 1. H 2 O dissolves 0.76 mg. at 2; 0.97 mg. at 10; 1.52 mg. at 18; 2.24 mg. at 26; 3.03 mg. at 34; 4.05 mg. at 42. (Kohlrausch and Rose, Z. phys. Ch. 12. 242.) Solubility in H 2 O = 1.25X10- 5 mol./l. at 25. (Goodwin, Z. phys. Ch. 1894, 13. 645.) Solubility of AgCl in H 2 O at 25 is 1.41X 10- 5 fin normality). (Thiel, Z. anorg. 1900, 24. 57.) 2.16 X 10 - 5 moles are sol. in 1 liter H 2 O at 25. (Noyes and Kohr, Z. phys. Ch. 1903, 42. 341.) 1.53X10~ 3 g. per liter are dissolved in sat. aq. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) 1 1. H 2 O dissolves 1.6 mg. AgCl at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 21.8 milligrams are dissolved in 1 liter of sat. solution at 100. (Eottger, Z. phys. Ch. 1906, 66. 93.) 1.34 mg. are contained in 1 1. of sat. solu- tion at 18. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) 1 1. sat. solution at t contains mg. AgCl. t mg. AgCl t mg. AgCl 1.55 4.68 9.97 0.56 0.66 0.89 17.51 25.86 . 34.12 . 1.31 1.935 2.74 (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Solubility in H 2 O = 1.6X10- 5 g.-mol. per litre at 25. (A. E. Hill, J. Am. Chem. Soc. 1908, 30. 74.) 1 1. H 2 O dissolves 0.00154 g. AgCl at 21; 0.0217 g. at 100. (Whitby, Z. anorg. 1910, 67. 108.) SILVER CHLORIDE 823 Calculated from electrical conductivity o: AgCl-f-Aq, l 1. H 2 O dissolves: 0.0105 milli-equivalents AgCl at 18. 0.0365 " " " " 50. 0.147 " " " 100. (Melcher, J. Am. Chem. Soc. 1910, 32. 55.; 1 1. H 2 O dissolves 1.02X10- 5 g. equiv. at 18; 1.429 X 10~ 5 g. equiv. at 25. (van Rossen C. C. 1912, I. 1539.) The most probable average value for solu- bility of AgCl in H 2 O is 1.04XH)- 5 g. equiv per 1. at 18, and 1.43X10- 5 g. equiv. per 1 at 25. (van Rossen, C. C. 1912, II. 1807.) 1.20X10- 6 g. AgCl are sol. in 1 1. H 2 O at 18. (Glowczynski, C. A. 1916, 741.) More sol. in H 2 O than AgSCN. (Normand, Chem. Soc. 1912, 101. 1853.) Sol. in cone. HCl+Aq, and also when not very cone.; thus the solution of 1 pt. AgNO 3 + Aq in 15,000 pts. H 2 O is clouded by a little HCl+Aq, but clears up by the addition of more. (Reinsch, J. pr. 13. 133.) 1 pt. AgCl dissolves in 200 pts. cone. HC1+ Aq and in 600 pts. HCl+Aq diluted with pts. H 2 O. (Pierre, J. Pharm. (3) 1?. 237.) Somewhat sol. in hot alcohol, to which HCJ has been added, but is precipitated on cooling (Erdmann, J. pr. 19. 341.) 100 pts. sat. HCl+Aq (sp. gr. 1.165) dis- solve 0.2980 pt. AgCl, or AgCl is sol. in 336 pts. HCl+Aq at ord. temp.; 100 pts. HC1 + Aq Csp. gr. 1.165) at b.-pt. dissolve 0.56 g. AgCl, or AgCl is sol. in 178 pts. HCl+Aq. Solubility of AgCl in dil. HCl+Aq. 100 ccm. HCl+Aq (sp. gr. 1.165), to which the given amt. H 2 O has been added, dissolve g. AgCl. ccm. HCl ccm. H 2 Agfcl Pts. HCl which dis- solve 1 pt. AgCl 100 100 100 100 10 20 30 50 0.056 0.018 0.0089 0.0035 1,785 5,555 11,235 18,571 (Vogel, N. Rep. Pharm. 23. 335.) If HCl is added to a solution in which Vi.ooo.ooo pt. Ag is suspended, the milkiness dis- appears. Solubility in HCl+Aq increases with the temp., the AgCl separating out on cooling. (Mulder.) The amounts of AgCl which dissolve in HCl+Aq are directly proportional to the volumes of acid (of fixed concentration) used. (Barlow, J. Am. Chem. Soc. 1906, 28. 1448.) 11. 1 % HCl dissolves 0.0002 g. AgCl at 21. 1 1. 5% HCl dissolves 0.0033 g. AgCl at 21. 1 1. 10% HCl dissolves 0.0555 g. AgCl at 21. (Whitby, Z. anorg. 1910, 67. 108.) Solubility in HCl+Aq at 25. HCl g.-equivalents per 1. 0.649 1.300 1.911 2.149 2.569 2.975 3.576 4.182 4.735 5.508 Ag x 10-3 g.-equivalents per 1. 0.032 0.126 0.266 0.374 0.610 0.814 1.358 2.147 3.168 4.126 (Forbes, J. Am. Chem. Soc. 1911, 33. 1941.) Solubility in 20% HCl +Aq. HCl N/10 AgN0 3 ccm. Opalescent at t G. AgCl to 100 g. anhy- drous HCl 20 g. of 1.0 20% acid 1.1 0.0 0.39 2.0 29.5 0.72 3.0 51.5 1.076 3.75 70.0 1.346 4.25 82.0 1.525 4.75 90.0 1.74 5.80 107.0 2.08 (Lowry, Roy, Soc. Proc. 1914, 91. A. 62.) SI. sol. in cone. HBr+Aq. (Lowig.) Insol. in HNO 3 +Aq. (Wackenroder.) Entirely unacted upon by HNO 3 of 1.43 sp. gr. (Wurtz, Am. J. Sci. (2) 25. 382.) Solubility in dil. HNO 3 +Aq is the same as solubility in H 2 O, i. e. l / 2,000,000 pt. of Ag can- not be detected in H 2 O with or without HNO 3 , but Vi.ooo.ooo pt. can be detected in both cases. (Mulder.) 1 pt. Ag in the form of AgCl dissolves at 25 in 83,000 pts. H 2 O containing free HNO 3 and 0.33 pt. of HCl. (Mulder.) 100,000 pts. cone. HNO 3 +Aq dissolve about 2 pts. AgCl, and solubility is not sen- sibly affected by lower nitrogen oxides. (Thorpe, Chem. Soc. (2) 10. 453.) Solubility of AgCl in HNO 3 +Aq at 25. G. per liter HNOs AgCl HNOs AgCl 0.0315 0.063 0.630 0.001647 0.001705 0.00176 18.9 94.5 0.00225 0.0245 (Glowczynski, Kolloidchem. Beih. 1914. 6. 147.) 824 SILVER CHLORIDE Insol. in cold cone. H 2 SO 4 , but on boiling Solubility in NH 4 OH+Aq at 25. is in part decomp. and in part dissolved, and does not separate on cooling. g. at. Ag Mols. NHs g. at. Ag Mols. NH 3 AgCl is not more sol. in dil. H 2 SO 4 +Aq per . per 1. perl. per 1. .1 j*i crxrn i A ^ man in 011. j.j..i.>ivy 3 -p- ri --i' Unacted upon by cold H 2 SO 3 +Aq, and but 0.151 2.042 0.0140 0.253 slightly decomp. on heating. (Vogel.) 0.149 2.017 0.0140 0.253 Abundantly sol. in H 2 PtCl 4 +Aq without 0.149 2.013 0.0140 0.252 decomp. (Birnbaum, Z. Ch. 1867. 520.) 0.147 1.991 0.0139 0.252 Insol. in cold dil. caustic alkalies +Aq but 0.0616 0.961 0.00621 0.118 decomp. by hot cone. solutions. (Gregorv.) 0.0583 0.916 0.00621 0.118 Decomp. by K 2 C0 3 +Aq. 0.0584 0.909 0.00619 0.118 SI. sol. in cold K 2 CO 3 +A"q. 0.0572 0.903 0.00625 0.118 Easily sol . even in dil. NH 4 OH+Aq. 0.0569 0.896 0.00304 0.0590 1 pt. AgCl dissolves in 1288 pts. NH 4 OH + 0.0555 0.873 0.00297 0.0589 Aq of 0.89 sp. gr. (Wallace and Lamont, 0.0541 0.863 0.00300 0.0585 Chem. Gaz. 1893. 137 ) 0.0514 0.818 0.05149 0.0288 100 pts. NH 4 OH+Aq of 0.986 sp. gr. dis- 0.0249 0.428 0.00143 0.0287 solve at 80 1.492 pts AgCl, drie d at 100. 0.0240 0.416 0.00142 0.0285 (Pohl, W. A . B. 41. 627.) 0.0235 0.411 0.00141 0.0282 1 1. NH 4 C VFr_l_A nt O QAQ er> o-r rHaanlvAQ 0.0227 0.397 51.6 g. Ag as freshly precipitated AgCl, and 47.6 g. when diluted with 1 1. H 2 O. 1 1. NH 4 OH+Aq of 0.924 sp. gr. dissolves 58 g. Ag as freshly precipitated AgCl; 1 1. NH 4 OH+Aq of 0.899 sp. gr. dissolves 49.6 (Whitney and Melcher, J. Am. Chem. Soc. 1903, 26. 78.) g.; 0.5 1. NH 4 OH+Aq (of 0.049 sp. gr.) + 0.5 1. saturated NaCl+Aq dissolves 20.8 g.; 0.5 1. NH 4 OH+Aq (of 0.949 sp. gr.)+0. 5 1. Solubility of AgCl in NH 4 OH+Aq at 25. saturated KCl+Aq dissolves 20.4 g.; 0.5 1. Ag = g. at. Ag in 1000 g. H 2 O. NH 4 OH+Aq (of 0.949 sp. gr.)+0.5 1. satu- NH 3 = g. mol. NH 3 in 1000 g. H 2 O. rated NH 4 Cl+Aq dissolves 22.4 g. Ag as Cone. = Molecular concentration of free freshly pptd. AgCl. (Millon and Commaille, NH 3 . C. R.' 66. 309.) 1 g. AgCl dissolves in 428.64 g. 5% Ag NH 3 Cone. Solid phase NH,iOH4-A rt (an nrr f QQS^ of 19 1 g. AgCl JA A-L4\JH l^-**-M V'-M"'* &* v>vt -' v -'/ *-* v -* dissolves in 12.76 g. 10% NH 4 OH + Aq(sp. gr. 0.023 0.437 0.391 AgCl 0.96) at 18. (Longi, Gazz. ch. it. 13. 87.) 0.025 0.428 0.378 f 1 g. freshly pptd. AgCl is sol. in 17 ccm. 10% NH 4 OH+Aq. Solubility is diminished 0.1197 0.1308 1.700 1.688 1.461 1.426 < by presence of AgBr (Senier, Pharm. J. 0.372 3.782 3.038 Trans. (3) 14. 1.) 0.378 3.945 3.181 1 0.574 5.10 3.95 ' 0.609 5.33 4.11 ' Solubility in NH 4 OH+Aq at 0. 0.633 0.745 5.545 6.26 4.279 4.77] AgCl+2AgCl, 3NH 3 G. per 100 g. solution. 0.754 6.27 4.76 1 ' 0.757 6.25 4.74 f 1 NH 3 AgCl NHs AgCl 0.760 0.775 6.25 6.52 4.73 1 4.97 2AgCl, 3NH 3 1.45 0.49 28.16 5.69 0.848 8.28 6.58 1.94 1.36 29.80 7.09 0.968 11.19 9.25 ' 5.60 3.44 30.19 7.25 0.980 11.78 9.82 ' 6.24 4.00 32.43 5.87 0.978 12.23 10.27 11.77 4.68 34.56 4.77 0.965 12.26 10.33 ' 16.36 5.18 37.48 3.90 1.03 12.68 10.62 ' 1.09 12.96 10.78 ' 1 049 14.34 12.24 ( (Jarry, A. ch. 1899, (7) 17. 342.) 1^039 14.47 12.39 ' Solubility in NH 4 OH-f-Aq increases with the temp. (Jarry.) (Straub, Z. phys. Ch. 1911, 77. 332.) Easily (Brett), difficultly (Wittstein), sol in NH 4 Cl+Aq, but not in other NH 4 salts. SILVER CHLORIDE 825 Solubility in NH 4 Cl+Aq at 15. NH 4 C1 10.0 14.29 17.70 19.23 21.98 25.31 28.45 Sat. % AgCl 0.0050 0.0143 0.0354 0.0577 0.110 0.228 0.340* 0.177 *24.5. (Schierholz, W. A. B., 1890, 101. 2b. 8.) Solubility in NH 4 Cl+Aq (26.31%) at t % AgCl 15 40 60 80 90 100 110 0.276 0.329 0.421 0.592 0.711 0.856 1.053 (Schierholz.) At 25, 1 1. NH 4 Cl+Aq containing 0.00053 g. NH 4 C1 dissolves 0.001604 g. AgCl; 0.00530 g. NH 4 C1, 0.002379 g. AgCl. (Glowczynski, Kolloidchem. Bern. 1914, 6. 147.) See also Forbes, page 826. 1 1. KClO 3 +Aq dissolves 1.8 mg. (Guye, J. Chim. Phys. 10. 145.) SI. sol. in cone. KCl+Aq, NaCl+Aq, and certain other chlorides. NaCl, KC1, NH 4 C1, CaCl 2 , ZnCl 2 +Aq, etc., dissolve appreciable quantities of AgCl, es- pecially if hot and concentrated, but it sep- arates out for the most part on cooling, Sol. in solutions of all the metallic chlorides which are sol. in H 2 O, thus NaCl, KC1, CaCl 2 , SrCl 2 , and BaCl 2 +Aq all dissolve AgCl, espe- cially if hot. MgCl 2 , NH 4 C1, and HgCl 2 (least) also dissolve AgCl. (Mulder.) Sol. in cone. CaCl 2 +Aq. (Wetzlar.) Sol. in roseocobaltic chloride +Aq. (Gibbs and Genth.) Insol. in SnCl 4 , HgCl 2 , CuCl 2 , ZnCl 2 , CdCl NiCl 2 , or CoCl 2 +Aq. (Vogel.) Solubility of AgCl in sat. solutions of chlorides Experiments by Hahn give different results Tom those of Vogel as follows: Solubility in various salts +Aq. Salt % salt Sat. at t % AgCl KC1. NaCl . . NH 4 C1 . . . CaCl 2 . . . MgCl 2 . . BaCl 2 . . . FeCl 2 . . . FeCl 3 . . . MnCl 2 . . . ZnCl 2 . . . CuCl 2 . . . PbCl 2 . . . 24.95 25.96 28.45 41.26 36.35 27.32 19.6 24.5 ." . 24 '.5 24^5 t( 0.0776 0.1053 0.3397 0.5713 0.5313 0.0570 0.1686 0.0058 0.1996 0.0134 0.0532 0.0000 (Hahn, Wyandotte Silver Smelting Works, 1877.) 1 1. 4-N KCl+Aq dissolves 0.915 g. KC1 at 25. (Hellwig, Z. anorg. 1900, 25. 166.) Solubility in KCl+Aq at t. t G. equiv. per 1. AgXlO-a KC1 1.0 25.0 35.0 1.734 2.415 2.786 3.325 3.083 2.955 (Forbes, J. Am. Chem. Soc. 1911, 33. 1937.) Solubility in KCl+Aq at 25. G. per liter. KCl AgCl KCl AgCl 0.00236 0.00471 0.00184 0.00218 0.01491 0.02984 0.00305 0.00321 (Glowczynski, Kolloidchem. Beih. 1914, 6. 147.) Solubility in*CaQ 2 +Aq. at ordinary temperatures. Salt 100 pts. sat. solution dissolve pts. AgCl Pts. solution required to dis- solve 1 pt. AgCl BaCl 2 0.0143 6,993 SrCl 2 . . . 0.0884 1,185 CaCl 2 . . . 0.0930 1,075 NaCl . . . 0.0950 1,050 KCl ... 0.0475 2,122 NH 4 C1 . . . 0.1575 634 MgCl 2 . . 0.1710 584 HC1 ... 0.2980 336 (Vogel, N. Rep. Pharm. 23. 335.) t G. equiv. per 1. AgXlO" CaCP 2 1.0 25.0 35.0 0.964 1.514 1.806 3.512 3.320 3.221 (Forbes, 1. c.) Sat. CuCl 2 +Aq at dissolves 2.835 g. AgCl per 1; at 100, 8.147 g. Solubility in sat. MgCl 2 +Aq is still greater. (Hahn, Eng. Min. J. 65. 434.) 826 SILVER CHLORIDE More sol. in HgCl 2 +Aq than in H 2 O. Solubility in salts +Aq at 25. (Finzi, Gazz. ch. it. 1902, 32. (2) 324.) At 15, 100 g. NaCl in 280 ccm. H 2 O dis- solve 485 mg. AgCl; 100 g. KC1 in 300 ccm. C = concentration of the salt in salt solution in g.-equivalents per litre. H 2 O dissolve 334 mg 100 g NH 4 C1 in 280 ccm. H 2 O dissolve 1051 mg. Salt c AgX 10-3 The solubility decreases with dilution g.-equivalents per 1. rapidly at first until about an equal vol. of H 2 O has been added, and then much more slowly to a minimum quantity, when the dilution is 1 : 10 for NaCl and KC1, and 1 : 20 for NH 4 C1. 100 g. NaCl in 280 ccm. H 2 O dissolve 2170 mg. AgCl at 109; 100 g. NH 4 C1 in 280 ccm. H 2 O dissolve 4000 mg. AgCl at 110; 100 g. NaCl in 620 ccm. H 2 O (14% solution) dissolve 15 mg. AgCl at 15, and 774 mg. at 104. (Schierholz, W. A. B. 101, 2b. 4.) The solubility of AgjCl in NaCl+Aq de- creases with diminishing concentration of NaCl+Aq. (Barlow, J. Am. Chem. Soc. NaCl 0.933 1.190 1.433 1.617 1.871 2.094 2.272 2.449 2.658 2.841 3.000 3.270 3.471 3 747 0.086 0.130 0.184 0.245 0.348 0.446 0.570 0.684 0.851 1.040 1.194 1.583 1.897 4 462 1906, 28. 1448.) 3.977 2.879 4.170 3.335 . Solubility in NaCl+Aq. 4.363 4.535 3.810 4.298 Gravimetric measurements, 15 5.039 6.039 Strength of salt solution G. AgCl retained per 100 g. NaCl CaCl 2 1.748 2.201 0.289 0.501 2 15% NaCl 20% NaCl 28% NaCl 0.063 0.134 0.279 2.741 3.264 3.737 4.033 0.900 1.463 2.182 2.802 4.538 4.175 Volumetric measurements 5.005 5.823 NaCl N/10 AgNO 3 ccm. Opal- escent att G. AgC retained per 100 g. vr n /-ii NH 4 C1 0.513 0.926 0.042 0.113 1.141 0.172 20 g. of 15% solution 0.25 0.4 28 40 0.119 0.191 1.574 2.143 0.365 0.842 0.7 64 0.335 2.566 1.425 1.0 1.25 1.7 78 89 102.5 0.478 0.598 0.812 2.918 3.162 3.510 2. 160 2.795 4.029 4. -363 9.353 20 g. of 20% solution 0.43 0.65 17.0 26.0 0.156 0.234 4.902 5.503 14.92 24.04 0.82 37.0 0.295 5.764 30.17 1.2 1.6 2.12 2.52 51.5 67.0 79.5 88.5 0.430 0.524 0.765 0.910 SrCl 2 0.550 0.989 1.359 0.033 0.092 0.173 2 3.08 97.0 1.10 1.572 0.236 v 3.52 105.0 1.27 1 .698 1.818 0.284 0.348 20 g. of 28% solution 2.25 2.75 3.5 4.5 36.5 45.0 56.0 69.0 0.675 0.704 0.896 1.153 2.140 2.476 2.992 3.494 0.510 0.747 1.252 2.018 5.5 84.0 1.411 4. 152 3 . 594 6.5 7.75 94.0 107.5 1.664 1.958 5.216 5.775 8. 174 12.04 (Lowry, Roy, Soc. Proc. 1914, 91. A, 61.) SILVER CHLORIDE 827 Solubility in salts +Aq. at 25 Continued. presence of NaC 2 H 3 O 2 or NH 4 OH+Ao. AgCl is pptd. from above solution by NaC 2 H 3 O 2 + Aq. (Mulder.) Sol. in Hg(NO 3 ) 2 +Aq (Wackenroder, A. 41. 317); in considerable amount (Liebig, A. 81. 128); and is precipitated by HC1, NH 4 C1, NaCl, KC 2 H 3 O 2 (Debray, C. R. 70. 849); in- completely precipitated by AgNO 3 and not by HNO 3 (Wackenroder). Solubility of AgCl in Hg(NO 3 ) 2 +Aq at 25. (G. mols. per 1.) Salt C AgXlO-3 g.-equivalents per 1. KC1 1.111 1.425 1.713 2.022 2.396 2.628 2.850 3.081 3.424 3.843 0.141 0.235 0.391 0.616 1.050 1.390 1.845 2.435 3.602 5.725 BaCl 2 1.248 1.610 2.676 3.260 0.186 0.339 1.274 2.366 Hg(N0 3 ) 2 HNOs AgCl Hg(N0 3 ) 2 HNOs AgCl 2 0.0100 0.0125 0.025 0.00432 0.00499 0.00690 0.050 0.100 1.000 0.00914 0.01395 0.04810 (Forbes. J. Am. Chem. Soc. 1911. 33. 1940). Sol. in NaNO 3 , KNO 3 ,Ca(NO 3 ) 2 ,Mg(NO 3 ) 2 , and NH 4 NO 3 -}-Aq; si. sol. at ord. temp., but solubility is much increased by heat. Solubility in NaNO 3 +Aq at 15-20. ccm. H 2 O 1 g- NaNOs mg. AgCl dissolved 100 200 300 100 to to o o 787 787 361 787 1 1 3 2 33 .93 99 53 Solubility increases with ascending temp . Temp. ccm. H 2 O g . NaNOs mg. AgCl dissolved 5 15-17 18 30 45-55 100 100 100 100 100 O OO O O .787 .787 .787 .787 .787 0.86 1.33 1.46 2.33 3.99 (Mulder.) At 25, 100,000 pts. H 2 O containing a little free HNO 3 and 0.787 g. NaNO 3 dissolve 2.128 mg. AgCl. By adding 2 g. more NaNO 3 to above solution, 2.5269 mg. (Vs more) AgCl are dissolved. (Mulder.) Solubility in H 2 O is not appreciably in- fluenced by Vio N to N-KNO 3 or NH 4 NO 3 - Aq. (van Rossen, C. C. 1912, II. 1807.) In presence of NaNO 3 and excess of HC1, 1 1. H 2 O dissolves 0.03 mg. AgCl. (Richards and Wells.) Hg(NO 3 ) 2 +Aq dissolves considerable quan- tities of AgCl, but the other nitrates do not (Mulder.) Much more sol. in hot than in cold Hg(NO 3 ) 2 +Aq, and much more sol. therein than in NH 4 NO 3 +Aq. NaCl ppts. AgCl from this solution; much less sol. therein in HNO 3 was present in all cases, and it was found that there was no difference in solubil- ity of AgCl with concentrations between 0.1N and 2N HNO 3 . (Morse, Z. phys. Ch. 1902, 46. 708.) Not sol. to appreciable extent in Cu(NO 3 ) 2 , Fe 2 (NO 3 ) 6 , Mn(NO 3 ) 2 , Co(NO 3 ) 2 , Zn(NO 3 ) 2 , or Ni(NO 3 ) 2 +Aq; insol. or exceedingly si. sol. in Pb(NO 3 ) 2 H-Aq. (Mulder.) Imperfectly sol. in AgNO 3 +Aq. (Wacken- roder;) Cone. AgNO 3 +Aq dissolves AgCl per- ceptibly. Less sol. in AgNO 3 +Aq than AgBr. (Risse, A. 111. 39.) Solubility in 0.02N AgNO 3 +Aq = 0.15X 10 - 7 g. mols. per 1. (Bottger.) 100 ccm. of 3-N solution of AgNO 3 dis- solve 0.08 g. AgCl at 25. More dil. solutions dissolve very slight amounts of AgCl. (Hell- wig, Z. anorg. 1900, 25. 177.) Solubility in 2-N AgNO 3 +Aq at ord. temp. = 0.03 X10- 3 g. equiv. AgCl. (Forbes, J. Am. Chem. Soc. 1912, 33. 1946.) Solubility in AgNO 3 +Aq at t. (Det. by volumetric method.) AgN0 3 :H 2 0=2:l G. AgN0 3 n/10 NaCl t g. AgCl re- tained per 100 ccm. g. AgNO" 6 2 57 0.478 7 2 45 0.410 8 2 40 0.359 9 2 35 0.319 11 2 30 0.261 7 1 26 0.205 10 1 22 0.143 10 4 65 0.572 10 5 86 0.715 828 SILVER CHLORIDE Solubility in AgNO 3 +Aq at t. Continued. heim and Steinhauser, Z. anprg. 1900, 25. 103.) Solubility in Na thiosulphate +Aq at 16. AgNO 3 :H 2 O=l i 5 6 7 8 9 5.5 6.5 12 1 1 1 1 1 0.5 0.5 0.5 94 84 75 66 58 48 40 23 0.286 0.239 0.205 0. 179 0.159 0.130 0.110 0.060 g. dissolved AgCl g Na-S-Hj *Hn in 100 cc. water experimental calculated 2.08 0.29 4.16 0.64 6.24 0.88 8.35 1.26 16.70 2.54 20.83 3.28 0.80 1.60 2.40 3.21 6.42 7.99 AgN0 3 :H 2 0=l :2 6 7 8 10 12 8 12 0.5 0.5 0.5 0.5 0.5 0.25 0.25 104 92 85 73 61 45 28 0.120 0.103 0.090 0.072 0.060 0.045 0.030 (Abney, Z. phys. Ch. 1895, 18. 65.) A solution of Na 2 S 2 O 3 +Aq containing 200 g. Na 2 S2O 3 per liter, dissolves 0.454 g. AgCl per g. of Na 2 S 2 O 3 at 35. (Richards and Faber, Am. Ch. J. 1899, 2J. 170.) Solubility in salts +Aq. (Lowry, Roy, Soc. Proc. 1914, 91. A, 58.) Solubility in AgNO 3 +Aq at 20. (Det. by gravimetric method.) Solvent % Cone. Grams AgCl sol. in 100 grams solvent g. AgNOs g. H 2 O g. AgCl retained per 100 g. AgNOs Sodium thiosulphate Ammonium thiosulphate Sodium sulphite Ammonium sulphite carbonate Ammonia + Aq Magnesium chloride Potassium cyanide Ammonium sulphocyanide Potassium ' Calcium Barium Aluminum Thiocarbamide - Thiosinamine 1 ' 5 10 20 1 5 10 10 20 10 10 3 15 50 5 5 10 15 10 10 10 10 10 1 5 10 0.40 2.00 4.10 6.10 0.57 1.32 3.92> 0.44' 0.95 Trace 0.05 1.40 7.58 0.50 2.75, 0.08 0.54 2.88, o.ir 0.15 0.20 2.02 0.83 0.40 1.90 3.90 20 25 20 ,25 220 220 220 220 220 110 165 220 330 440 0.1372 0.1009 0.0722 0.0402 0.0294 (Lowry, Roy. Soc. Proc. 1914, 91. A, 56.) Insol. in Na 2 SO 4 +Aq. Solubility of AgCl in Na 2 SO 3 +Aq at 25. G. formula weights per 1. 8Oi Ag SOs Ag 0.080 0.106 0.220 0.234 0.478* 0.011 0.017 0.033 0.036 0.057* 0.483* 0.470 0.652 0.890 0.937 0.059* 0.070 0.103 0.140 0.142 * In presence of 0.05 Cl. (Luther and Leubner, Z. anorg. 1912, 74. 393.) Easily sol. in Na 2 S 2 O 3 or KCN+Aq. When freshly pptd., very sol. in solutions of soluble thiosulphates, and especially in cone Na 2 S 2 O 3 +Aq, which dissolves AgCl almost as readily as H 2 O dissolves sugar. K 2 S 2 O 3 + Aq, even when very dil., also dissolves AgCl; also SrS 2 O 3 -f Aq. (Herschel, 1819.) Sol. in KAsO 2 +Aq. (Reynoso.) Cold NaHSO 3 +Aq dissolves a consider- able amount of AgCl. (Rosenheim and Stein- hauser, Z. anorg. 1900, 25. 78.) Sol. in cold sat. (NH 4 ) 2 S 2 O 3 +Aq. (Rosen- (Valenta, M. 1894, 15. 250.) Solubility in salts +Aq. 31.71 cc. of a solution of. sodium thiosul- phate containing 31.869 g. Na 2 S 2 O 3 per liter (i. e. 5 g. of the hydrate in 100 cc. of the solu- tion) dissolve 0.6124 g. AgCl. 21.88 cc. of a solution of ammonium thio- sulphate containing 50 g. (NH 4 ) 2 S 2 O 3 per liter dissolve 0.7024 g. AgCl. 27.34 cc. of a solution of potassium cyanide containing 49.511 g. KCN per liter dissolve SILVER CHLORIDE 1.4926 g. AgCl. (Cohn, Z. phys\ Ch. 1895, 18. 63.) Solubility of AgCl in sodium thiosulphate and potassium cyanide solutions may be de- termined without reference to experimental date. (Cohn.) SI. sol. in liquid NH 3 . (Franklin. Am. Ch. J. 1898, 20. 829.) Insol. in moderately dil. Pb(C 2 H 3 O 2 ) 2 +Aa. 10 ccm. normal Hg(C 2 H 3 O 2 ) 2 +Aq contain- ing 0.1 g. Hg dissolve 0.01892 g. AgCl at 15. (Stas.) 100 ccm. of a solution of a mixture of Na and Hg acetates dissolve 0.00175 g. AgCl. (Stas, A. ch. (5) 3. 145.) Only si. sol. in liquid NH 3 . Solubility curve for AgCl, AgCl, 3NH 3 , AgCl, 5NH 3 . (Jarry, A. ch. 1899, 17. 342.) Insol. in alcoholic ammonia. (Bodlander, Z. phys. Ch. 1892, 9. 731.) Nearly insol. in ether. (Mylius and Hiitt- ner, B. 1911, 44. 1316.) Perceptibly sol. on warming with solution of tartaric acid, but nearly the whole is de- posited on cooling. Insol. in acetone.. (Naumann, B. 1904, 37. 4329); insol. in acetone and in methylal. (Eidmann, C. C. 1899, II. 1014.) Insol. in methyl acetate. (Bezold, Dissert. 1906; Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Hamers, Dissert. 1906; Naumann,B. 1910, 43. 314.) Sol. in methylamine+Aq. (Wurtz, A. ch. C 2 H 5 NH 2 AgCl 0.01272 0.03942 0.05512 0.06572 0.10300 0.000114 0.000156 0.000235 0.000312 0.000824 t CsHiNHi Ag 18 0.094 0.00458 25 0.093 0.00474 25 0.094 0.00478 18 0.236 0.0132 25 0.234 0.0136 18 0.462 0.0251 At 25, 1 1. methylamine+Aq, containing 1.017 g. mols. CH 3 NH 2 , dissolves 0.0387 g. mol. AgCl; 0.508 g. mol. CH 3 NH 2 , 0.0178 g. mol. AgCl. (Bodlander and Eberlein, B. 1903, 36. 3948.) Solubility in ethyamine+Aq at 25. G. mols. per 1. (Wuth, B. 1902, 36. 2416.) Solubility in ethylamine+Aq at t. G. mols. per 1. (Euler, B. 1903, 36. 2880.) (3) 30. 453.) Solubility of AgCl in methylamine at 11.5. At 25, 1 1. ethylamine+Aq, containing 0.483 g. mol. C 2 H 6 NH 2 , dissolves 0.0314 g. mols. AgCl; 0.200 g. mol. C 2 H 6 NH 2 , 0.0115 g, mol. AgCl; 0.100 g. mol. C 2 H 5 NH 2 , 0.0062 g. mol. AgCl. (Bodlander and Eberlein.) Sol. in amylamine+Aq, but less than in NH 4 OH+Aq. Sol. in caprylamine+Aq. Easily sol. on warming in ethylene diamine +Aq. (Kurnakow, Z. anorg. 1898, 17. 220.) Easily sol. in alcoholic solution of thiaceta- mide. (Kurnakow, J. pr. 1895, (2) 61. 251.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Solubility in pyridine at t. % CHsNH 2 % AgCl % CH 3 NH 2 % AgCl 1.78 4.44 5.51 7.66 0.16 0.62 0.83 1.32 13.70 3.29 18.69 5.43 36.69 9.93 (Jarry, A. ch. 1899, (7) 17. 342.) Solubility in methylamine+Aq at 25. G. mols. per 1. CH 3 NH 2 AgCl 0.0200 0.0400 0.0740 0.0947 0.1950 0.000300 0.000370 0.000424 0.000447 0.000481 t g. AgCl sol. in 100 g. pyridine , Solid phase -52 -49 -35 -30 -25 oo 0.70 0.77 0.99 1.36 1.80 2.20 2175 3.71 3.85 4.35 5.05 5.60 AgCl, 2C 5 H 6 N AgCl, C 5 H 5 N (Wuth, B. 1902, 35. 2416.) Solubility in methylamine+Aq at t. G. mols. perl. t CH 3 NH 2 Ag transition point -20 -18 -10 - 5 - 1 18 25 25 0.93 0.93 . 0.93 0.0315 0.0338 0.0335 (Euler, B. 1903, 2 6. 2880.) 830 SILVER CHLORIDE AMMONIA Solubility in pyridine at t. Continued. Solubility of AgF in H 2 O at t. Gr-kor 1 HO o- TT O g AgCl sol t . in 100 g. Solid phase t AgF Solid phase pyridine -14.2 +18.5 18.65 60 165 169.5 Ice+AgF, 4H 2 O AgF, 4H 2 " +AgF, 2H 2 transition point 10 5^35 Q 17 ' 20 30 1.91 1.20 20 24 OK 172 178 17Q ^ .AgF, a 2H 2 40 0.80 28.5 215 ft 50 60 70 80 0.53 0.403 0.32 0.25 AgCl 32 39.5 108 193 222 205 AgF,2H 2 O+AgF AgF 90 0.22 (Guntz, A. ch. 1914, (9) 2. 101.) 100 18 110 0.12 Sp. gr. AgF+Aq at 18. (Kahlenberg, J. phys. Chem. 1909, 13. 423.) % AgF Sp. gr. Easily sol. in warm piperidine. (Varet, C. R. 1892, 115. 335.) Mol. wt. determined in piperidine. (Wer- ner, Z. anorg. 1897, 15. 16.) Quinoline dissolves traces of AgCl. (Varet, 7.20 29.60 4Q.20 56.40 66.20 1.07 1.38 1.82 2. OP 2.62 As sol. in coniine+Aq as in NH 4 OH+Aq. (Blyth, Chem. Soc. 1. 350.) Sol. in sinamine, and thiosinamine+Aq. Min. Cerargyrite. Silver chloride ammonia, AgCl, 2NH 3 . Decomp. by H 2 O. (Terreil, A. Phys. Beibl. 7. 149.) 2AgCl, 3NH 3 . Decomp. on air and in H 2 O to AgCl. Sol. in cone. NH 4 OH+Aq, from which it can be crystallised. (Rose.) Insol. in alcohol. (Bodlander, Z. phys. Ch. 9. 730.) AgCl, 3NH 3 . More easily decomp. than 2AgCl, 3NH 3 . SI. sol. in liquid NH 3 . (Jarry, A. ch. 1899, (7) 17. 343.) AgCl, 5NH 3 . SI. sol. in liquid NH 3 . (Jarry, A. ch. 1899, (7) 17. 336.) Silver chlorobromoiodides. (Rodwell, Proc. Roy. Soc. 25. 292.) Silver s?/6fluoride (argentous fluoride), Ag 2 F. Decomp. by H 2 O into Ag and AgF. (Guntz, C. R. 110. 1337.) Decomp. by H 2 O. Insol. in abs. alcohol, ether, acetone and xylene. (Wohler and Rodewald, Z. anorg. 1909, 61. 63.) Decomp. by H 2 O until the solution con- tains 64.5% AgF, independent of temp. (Guntz, C. R. 1913, 157. 981.) Silver fluoride, AgF. Extremely deliquescent. (Gore.) Sol. in 0.55 pt. H 2 O at 15.5 with evolution of heat. Sp. gr. of sat. solution at 15.5 = 2.61. (Gore.) (Guntz, A. ch. 1914, (9) 2. 104.) Data on solubility of AgF in HF+Aq are given by Guntz (I. c.). SI. sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) +H 2 O. Deliquescent. Sol. in H 2 O. (Guntz, A. ch. 1914, (9) 2. 101.) +2H 2 O. Deliquescent. Sol. in H 2 O. (Guntz.) +4H 2 O. Not deliquescent. Sol. in H 2 O. (Guntz.) + 5 /a H 2 O. Unstable in the presence of crystals of AgF+2H 2 O. (Guntz, A. ch. 1914, (9) 2. 101.) Silver hydrogen fluoride, AgF, HF. (Guntz.) AgF. 3HF. Very unstable. Sol. in HF. (Guntz, Bull. Soc. 1895, (3) 13. 114.) Silver stannic fluoride. See Fluostannate, silver. Silver tungstyl fluoride. See Fluoxtungstate, silver. Silver, fulminating. See Silver nitride. Silver hydride, AgH. Not decomp. by H 2 O. (Bartlett, Am. Ch. J. 1896, 19. 52.) Argentous hydroxide, Ag 4 O 2 H 2 . Sol. in H 2 O. Known only in solution. (Weltzein, A. 142. 105.) Silver hydroxide, AgOH. Decomp. into Ag 2 O and H 2 O above -40. See Silver oxide. SILVER IODIDE 831 Argentous iodide, Ag 2 I. (Guntz, C. R. 112. 861.) Silver imidosulphamide, AgN(SO 2 NH 2 ) 2 + Decomp. slowly in the air. Somewhat sol. in hot, more sol. in boiling H 2 O, from which it cryst. unchanged on cooling. In aqueous solution is stable toward alkali. Decomp. by acids. Difficultly sol. in dry pyridine; easily sol. in pyridine +Aq. (Hantzsch, B. 1905, 38. 1035.) '(SO 2 ) 3 N 6 H 6 Ag 3 +5^H 2 O. Nearly insol. in hot H 2 O. (Ephraim and Michel, B. 1909, 42. 3845.) (SO 2 ) 4 N 7 H 8 Ag 5 +4H 2 O. (Ephraim and Michel.) (SO 2 ) 4 N 5 HAg 6 + l^, 11, and 28 H 2 O. Easily sol. in HNO 3 and NH 4 OH+Aq. SI. sol. in pyridine. Very sol. in pyridine con- taining pyridine nitrate and can^be recryst. therefrom. (Ephraim and Michel.) (SO 2 ) 4 N 6 Ag 7 +8H 2 O. (Ephraim and Michel.) Silver iodide, Agl. Insol. in H 2 O. Calculated from electrical conductivity of Agl+Aq, Agl is sol. in 1,074,040 pts. H 2 O at 28.4, and 420, 260 pts. at 40. (Holleman, Z. phys. Ch. 12. 130.) 1 1. H 2 O dissolves 0.1 mg. Agl at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) Solubility in H 2 O = 1 X 1Q- 8 N. (Rolla.) Solubility in H 2 O = 0.97 X 1Q- 8 g. mols. per 1. at 25. (Goodwin, Z. phys. Ch. 1894, 13. 645.) Solubility of Agl in H 2 O at 25 is 1.05 X10- 8 (in normality) . (Thiel, Z. anorg. 1900, 24. 57.) A sat. aq. solution at 20.8 contains 0.0020 X10- 6 g. equiv. perl. (Kohlrausch, C. C. 1901, II. 1299.) 1 1. H 2 O dissolves 0.0035 mg. Agl at 21. (Kohlrausch, Z. phys. Ch. 1904, 50. 356 ) 11. H 2 O dissolves 0.00253 mg. Agl at 60 (Sammet, Z. phys. Ch. 1905, 53. 644.) Solubility in H 2 O = 1.23X10-8 g.-mol per litre at 25. (A. E. Hill, J. Am. Chem Soc. 1908, 30. 74.) 0.003 mg. are contained in 1 1. of sat. solu- tion at 21. (Kohlrausch, Z. phys. Ch. 1908, Insol. in dil. HNO 3 +Aq or H 3 PO 4 +Aq. Decomp. by hot. cone. HNO 3 +Aq or H 2 SO 4 . Easily sol. in cone. HI+Aq. 1 pt. Agl dissolves in 2510 pts. NH 4 OH + Aq of 0.96 sp. gr. (Martini, Schw. J. 66. 154) ; in 243 pts. of 0.89 sp. gr. (Wallace and La- mont, Ch. Gaz. 1859. 137). 1 g. Agl dissolves in 26,300 g. 10% NH 4 OH+Aq (sp. gr.=0.96) at 12. Insol. in 5% NH 4 OH+Aq. (Longi, Gazz. ch. it. 13. 87.) Coefficient of solubility in NH 4 OH+Aq (density, 0.926) is found lower than previ- ously obtained and of the order of Veoooo at 16. (Baubigny, Bull. Soc. 1908, (4) 3. 772 ) According to Field, insol. in cold cone. KC1 or NaCl+Aq, and only in traces on boiling, and separates out on cooling. 100 g. NaCl in cone. NaCl+Aq dissolve 0.95 mg. Agl at 15; 100 g. NH 4 C1 in cone. NH 4 Cl+Aq dissolve 2.9 mg. Agl at 15; 95 g. NaCl + 10 g. KBr in cone, solution dissolve 1.2 mg. Agl at 15; IOC g. KBr+225 g. H 2 O dissolve 430 mg. Agl at 15; 100 g. KBr in cone. KBr+Aq dissolve 525 mg. Agl at 15; 100 g. KI+69 g. H 2 O dissolve 89.8 g. Agl at 15; 100 g. KI+92 g. H 2 O dissolve 54.0 g. Agl at 15; 100 g. KI+366 g. H 2 O dissolve 7.25 g. Agl at 15. (Schierholz, W. A. B. 101, 2b. 4.) Sol. in cone. KI+Aq, from which it is pre- cipitated by H 2 O. (Field, C. N. 3. 17.) KI gives a ppt. with AgNO 3 in presence of 30,000 pts. H 2 O. (Harting.) Solubility in KI+Aq at 15. %KI % Agl %KI % Agl 59.16 53.13 33.3 7.33 57.15 40 25.0 2.75 50.0 25.0 21.74 1.576 40.0 13.0 20 0.80 (Schierholz, W. A. B. 1890, 101. 2b. 10.) Solubility in KI+Aq at 25. ' Mol. KI per 1. g. Agl perl. 1.937 46. 42 1.6304 24. 01 1.482 15. 46 1.406 12. 55 1.018 3. 47 1.008- 3. 32 0.734 1. 032 0.586 0. 512 0.335 ' 0. 0853 Hellwig, Z. anorg. 1900, 25. 180.) Solubility in KI+Aq. t=50 % Agl %KI Solid phase 2.5 24.8 Agl 16.0 33.8 ' 28.0 36.7 ' 39.0 38.1 ( 51.8 36.2 ' 53.5 36.5 1 53.5 36.6 Agl+. \gl, KI 53.5 37.1 Ag] ,KI 53.4 37.6 KI+AgI, KI 50.4 40.2 KI 45.0 43.2 a 38.0 47.1 n 22.8 55.5 a 10.7 59.1 a 832 SILVER IODIDE t=30 % Agl % KI Solid phase 0.1 10.2 Agl 10.0 31.4 29.4 37.6 a 42.8 38.8 i( . 49.7 49.6 38.6 39.5 Agl + Agl, 2KI Agl, 2KI 47.7 40.9 a 46.3 41.4 (t 44.1 43.2 Agl, 2KI+KI 42.8 43.9 KI 35.8 46.9 K 16.0 55.5 (( 60.35 it t=0 % A I % KI Solid phase 0.2 9.8 Agl 1.5 20.5 6.5 26.1 " 26.6 34.6 ! " 28.1 36". 4 I n 38.0 37.9 41.3 42.0 Agl + Agl, KI Agl, KI 37.6 42.7 u 37.9 44.0 Agl, KI+KI 31.3 46.6 KI 21.7 50.5 u 18.0 51.2 ii 9.0 53.0 11 56.1 << 27.5 48.7 Agl, 2KI+KI 21.0 50.3 Agl, 2KI (Van Dam and Donk, Chem. Weekbl. 1911, 8. 848.) Very sol. in KI 3 +Aq. (Muth, Dissert. 1895.) Very sol. in H 2 O in presence'of Nal. (Kur- nakow, Ch. Z. 1900, 24. 60.) Solubility in Al -f Aq at 15. Traces are dissolved by alkali nitrates +Aq. Easily sol. in hot KOH +Aq, from which it is aptd. by H 2 O or alcohol. Not decomp; by boiling KOH+Aq. (Vogel> N. Rep. Pharm. 20. 129.) 100 pts. of AgNO 3 +Aq sat. at 11 dissolve 2,3 pts. Agl in the cold, and 12.3 pts. on boil- ing. (Schnauss.) Solubility of Agl in AgNO 3 +Aq at 25. Mol. AgNOs in 1 1. g. Agl in 1 1. Solid phase 0.20 0.0680 \ 0.25 0.080 0.30 0.090 0.35 0.125 0.40 0.167 0.45 0.224 Agl 0.50 0.299 0.55 0.400 0.60 .0.528 0.65 0.672 0.70 0.850 1.215 3.08 1 1.63 6.26 Ag 2 IN0 3 2.04 10.90 J 2.54 16.1 3.115 22.7 3.75 4.055 33.2 40.0 .A g3 I(N0 3 )2 4.69 53.2 5.90 85.0 /'HWIl^r;- *7 r,.rr 1 OHO QK 171 ^ Composition of the sat. solution in mols. per 1000 mols. H 2 O Solid phase Mols. Mols. Na 2 I 2 AIi 35.63 8.14 Agl 40.54 10.94 a 61.55 25.15 " 80.55 38.19 tl 94.25 47.79 t( 107.52 117.96 57.52 51.70 Agl+AgI, Nal, 3^H 2 Agl, Nal, 3^H 2 O 134.40 46.82 u 135.83 46.36 AgI,NaI,3^H 2 O+NaI 133.81 43.03 Nal 129.02 34.85 122.56 22.82 117.11 11.93 u 111.52 lt (Krym, J. Russ. Phys. Chem. Soc. 1909, 41. 382.) Solubility of Agl in 25% AgNO 3 +Aq reaches a maximum at about 60 and at the point of maximum solubility the quantity dissolved amounts to about 5 g. Agl per 100 g. AgN0 3 . (Lowry, Roy. Soc. Proc. 1914, 91, A, 66.) Sol. in hot Hg(NO 3 ) 2 +Aq, from which it crystallizes on cooling. Solubility of Agl in Hg(N0 3 ) 2 +Aq at 25. Mols. Hg(N0 3 ) 2 perl. g. Agl perl. Mols. Hg(NOs) 8 per 1. g. Agl per 1. 0.010 0.0125 0.025 0.800 0.841 1.118 0.050 0.100 1.000 1.737 2.730 25.160 Solubility is not affected by presence of 0.1to2NHNO 3 . (Morse, Z. phys. Ch. 1902, 41. 708.) Sol. inKCN+Aq. SI. sol. in Na 2 S 2 O 3 +Aq when suspended in much H 2 O, but separates again on addition of KI+Aq. (Field.) Insol. in Na 2 S 2 O 3 +Aq. fFogh, C. R. 1890, 110. 711.) SILVER OXIDE 833 Solubility in salts+Aq. 2AgI, NH 3 . (Rammelsberg, Pogg. 48. 17O "> Solvent % Cone. grams Agl sol. in 100 grams solvent 1 i \j.) Composition is Agl, NH 3 . (Longi, Gazz. ch. it. 13. 86.) Sol. in liquid NH 3 . (Jarry, A. ch. 1899, (7) Sodium thiosulphate 1 0.03 17. 371.) " " " 5 0.15 Agl, 2NH 3 . (Terreil, C. R. 98. 1279.) " " " 10 0.30 20 " " " 15 0.40 Silver nitride, Ag 3 N. Sodium sulphite Ammonium sulphite Potassium cyanide 20 10 20 10 5 0.60 0.01 0.02 Traces 8.23 25 Berthollet's "knallsilber." Very explosive. Insol. in H 2 O. Sol. in KCN+Aq. Slowly sol. in NH 4 OH+Aq. (Raschig, A. 233. 93.) (Angeli, Chem. Soc. 1894, 66. (2) 93.) " Ammonium sulphocyanide 5 i n 0.02' One on Argentous oxide, Ag 4 O. . 1U 1 * .u 010 &\j Insol. in H 2 O. Decomp. by acids into Potassium ' J.O 10 . JLO argentic oxide and silver. Insol. in NH 4 OH + Calcium ' -LU 10 0.03 Aq or HC 2 H 3 O 2 . (v. der Pfordten, B. 20. Barium ' 10 009 1458.) Aluminum ' -LU 10 . V / w 0.02 Contains H, and is a hydroxide Ag 4 ,H 2 O. Thiocarbamide 10 7Q 25 (v. der Pfordten, B. 21. 2288.) Thiosinamine AVF 1 \J 4. t7 008 The above substance is a mixture, accord- -L 5 \J . Uv/O 0.05 ing to Friedheim (B. 20. 2557.) 10 0.09 Silver oxide, Ag 2 O. (Valenta, M. 1894, 15. 250.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829; Jarry, A. ch. 1899, (7) 17. 370.) Easily sol. in liquid NH 3 . (Ruff and Geisel, B. 1905, 38. 2662.) Insol. in acetone. (Eidmann, C. C. 1899, II, 1014); (Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Bezold, Dis- sert. 1906); (Naumann, B. 1909, 42. 3790.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Much less sol. in hot alcoholic thiourea than AgCl and AgBr. (Reynolds, Chem. Soc. 1892, 61. 253.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Slowly sol. in piperidine at 100. (Varet, C. R. 1892, 115.336.) 0.10 pts. is sol. in 100 pts. pyrioline at 10. 8.60 pts. are sol. in 100 pts. pyridine at 121. (Laszczynski, B. 1894, 27. 2288.) Mol. wt. determined in piperidine. (Wer- ner, Z. anorg. 1897, 15. 16.) Min. lodyrite. Silver hydrogen iodide, 3AgI, HI+7H 2 O. . (Berthelot, C. R. 91. 1024.) Silver sodium iodide, 2AgI, Nal. Very sol. in acetone. (Marsh, Chem. Soc. 1913, 103. 784.) Agl, NaI+3^H 2 O. (Krym, J. Russ. Phys. Chem. Soc. 1909, 41. 382.) See Agl+Nal under Agl. Silver iodide ammonia, Agl, NH 3 . Sol. in liquid NH 3 . (Jarry, A. ch. 1899, 7) 17. 371.) Somewhat sol. in H 2 O. (Bucholz.) Sol. in 3000 pts. H 2 O. (Bineau, C. R. 41. 509) ; sol. in 96 pts. H 2 O. (Abl.) Sol. in 15,360 pts. H 2 O. (Levi, Gazz. ch. it. 1901, 31. (1) 1.) Solubility in H 2 O at 25 = 2.16X10- 4 mols. AgOH per litre. (Noyes, J. Am. Chem. Soc. 1902, 24. 1147.) 1 liter sat. aqueous solution at 19.96 con- tains 2.14X10- 2 g.; at 24.94 contains 2.5 X 10 2 g. Ag 2 O. (Bottger, Z. phys. Ch. 1903, 1 1. H 2 O at 25 dissolves 1.8X10- 4 gram- atoms of silver. Determined from its solu- bility in NH 3 . (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) 1 1. H 2 O dissolves C.0215 g. Ag 2 O at 20. (Whitby, Z. anorg. ]910, 67. 108.) The solubility of Ag 2 O in H 2 O varies with the method of preparation. Solubility of Ag 2 O (prepared by action of NaOH, freshly prepared by the solution of Na in H 2 O, on a dil. solution of.AgNO 3 ) = 2.16X10- 4 g-mol. in 1 1. H 2 O at 25; 2.97 X 10- 4 g.-mol. at 50. Solubility of Ag 2 O (prepared by action of aqueous barium hydroxide on AgNO 8 ) = 2.23 X10- 4 g.-mol. in 1 1. H 2 O at 25; 3. 09X1<> 4 g.-mol. in 1 1. H 2 O at 50. Solubility of Ag 2 O (prepared by action of cone. NaOH+Aq on moist, freshly pptd. AgCl)=2.32X10- 4 g.-mol. in 1 1. H 2 O at 25; 3.55 X10- 4 g.-mol. at 50. Solubility of Ag 2 O (prepared by action of cone. NaOH+Aq. on moist, freshly pptd. Ag 2 CO 3 )=2.95X10- 4 g.-mol. in 1 1. H 2 O at 25; 3.89 X10- 4 g.-mol. at 50. (Rebiere, Bull. Soc. 1915, (4) 7. 311.) Sol. in acids. NH 4 OH, and (NH 4 ) 2 CO 3 -t Aq. Decomp. by alkali chlorides, bromides,, 834 SILVER OXIDE and iodides +Aq. Sol. in alkali cyanides, and thiosulphates+Aq. SI. sol. in nitrates +Aq; insol. in sulphates +Aq. When freshly pptd., sol. in NH 4 SCN+Aq. SI. sol. in NH 4 NO 3 +Aq. Abundantly sol. in Ba(NO 3 ) 2 +Aq without pptn. of Ba0 2 H 2 . Sol. in boiling Mn(NO 3 ) 2 , Ni(NO 3 ) 2 , Co(NO 3 ) 2 , Cu(NO 3 ) 2 , and Ce 2 (NO 3 ) 6 +Aq with pptn. of oxides. (Persoz.) Insol. in KOH, and NaOH+Aq. SI. sol. in BaO 2 H 2 +Aq. (Berzelius (?). SolubiHty in NH 4 OH+Aq at 25. G. at. Ag per 1. Mol. NH 3 per 1. 0.0654 0.214 0.0658 0.220 0.134 0.458 0.140 0.469 0.205 0.671 0.205 0.684 0.225 0.720 0.224 0.733 0.251 0.811 0.248 0.827 0.242 0.830 0.257 0.876 0.278 0.899 0.276 0.915 0.299 0.999 0.343 1.147 0.454 1.498 0.470 1.522 (Whitney and Melcher, J. Am. Chem. Soc. 1903, 25. 78.) Insol. in liquid NH 3 . (Franklin, Am. ch. J. 1898, 20. 829.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014); (Naumann, B. 1904, 37. 4329.) Insol. in ethyl acetate. (Hamers, Dissert. 1906; Naumann, B. 1910, 43. 314.) SI. sol. in amylamine+Aq, easily in methylamine+Aq fWurtz, A. ch. 30. 453); also in ethylamine,,and thiosinamine+Aq. Solubility in methylamine+Aq. at 18. G. mols. per 1. CH 3 NH 2 Ag 0.1 0.5 1.0 0.0221 0.118 0.228 (Euler, B. 1903, 36. 2879.) Solubility in ethylamine+Aq at 18. G. mols. per 1. C 2 H 6 NH 2 Ag 0.1 0.5 (interpolated) 1.0 " 0.561 0.927 0.0322 0.160 0.314 0.180 0.291 (Euler.) Silver peroxide, Ag 2 O 2 . Sol. in cone. H 2 SO 4 (Rose), and in pure HNO 3 +Aq without decomp. Sol. in NH 4 OH +Aq. (Schonbein, J. pr. 41. 321.) Sol. in HNO 3 and H 2 SO 4 with decomp. Mulder, R. t. c. 1898, 17. 151.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Silver oxide ammonia. See Silver nitride. Silver oxybromide, Ag 7 OBr 7 . Insol. in H 2 O. Insol. in HNO 3 . Sol. in lot ammonia and in NaOCl + Aq. f Seyewetz, ~. R. 1912, 154. 357.) Silver oxyfluoride, AgF, AgOH. Decomp. by H 2 O with separation of Ag 2 O. (Pfaundler.) Silver pei oxyfluoride, 2Ag 3 O 4 , AgF. (Tanatar, Z. anorg. 1901, 28. 335.) 4Ag 3 O 4 , 3AgF. (Tanatar, Z. anorg. 1901, 28. 335.) Silver oxyiodide, Ag 2 O, Agsly. (Seyewitz, Bull. Soc. 1894, (3) 11. 452.) Silver phosphide, AgP 2 . Sol. in HNO 3 . Attacked by aqua regia. (Granger, C. R. 1897, 124. 897.) Ag 4 P 6 . Insol. in HCl+Aq; easily sol. in HNOa+Aq. (Schrotter, J. B. 1849. 247.) Ag 2 P 5 . (Hackspill, C. R. 1913, 157. 720.) Ag 3 P (?). (Fresenius and Neubauer, Z. anal. 1. 340.) Silver phosphoselenide, Ag 2 Se, P 2 Se. Insol. in H 2 O or HCl+Aq. Sol.inHNO 3 + Aq. Insol. in cold, decomp. by hot alkalies + Aq; (Hahn, J. pr. 93. 436.) 2Ag 2 Se, P 2 Se 3 . Insol. in H 2 O, HC1, or HNO 3 +Aq; slowly sol. in red fuming HNO 3 . (Hahn, J. pr. 93. 440.) 2Ag 2 Se, P 2 Se 5 . Sol. only in fuming HNO 3 . (Hahn.) Silver phosphosulphide, 2Ag 2 S, P 2 S. Ag 2 S, P 2 S. (Berzelius, A. 46. 254.) 2Ag 2 S, P 2 S 3 . Easily sol. in HNO 3 +Aq without separation of P. (Berzelius.) Ag 4 P 2 S 7 . (Berzelius.) Ag 4 PS 3 . Easily attacked by hot cone. HC1. SI. decomp. Insol. in hot HNO 3 . De- comp. by aqua regia. (Ferrand. A. ch. 1899. (7) 17. 413.) Silver selenide, Ag 2 Se. Sol. in boiling HNO 3 +Aq as Ag 2 SeO 3 , which separates out by dilution with H 2 O. (Berzelius.) Insol. in Hg 2 (NO 3 ) 2 +Aq. (Wackenroder, A. 41. 327.) SODIUM ACETYLIDE ACETYLENE 835 Min. Naumannite. Insol. in dil., but sol. in cone. HNO 3 +Aq. Silver sulphamide (silver thionyl amide). SO 2 (NHAg) 2 . Insol. in pyridine. (Hantzch and Holl, B. 1901, 34. 3436.) +H 2 O. (Ephraim and Gurevitsch, B. 1910, 43. 146.) Argentous sulphide, Ag 4 S. Easily sol. in warm dil. HNO 3 +Aq, and in cone. H 2 SO 4 without separation of S. Sol. in cone. KCN+Aq. '(v. der Pfordten, B. 20. 1458; Guntz, C. R. 112. 861.) Silver sulphide, Ag 2 S. Less sol. in H 2 O than Agl. (Lucas, Z. anorg. 1904, 41. 210.) 1 1. H 2 O dissolves about 4X10 n g. at. Ag as Ag 2 S at 18. (Bernfeld, Z. phys. Ch. 1898. 26. 72.) 1 1. H 2 O dissolves 0.8X10 6 g. mols. at 16-18. (Biltz, Z. phys. Ch. 1907, 58. 291.) 1 1. H 2 O dissolves 0.552 X 10 6 g. mols. Ag 2 S at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) Sol. in cone. HNO 3 +Aq with separation of S. Sol. in hot cone. HCl+Aq. Not de- comp. by CuCl 2 +Aq, but by CuCl 2 +NaCl +Aq. Insol. in NH 4 OH+Aq. Insol. in H 2 SO 3 +Aq, or in Hg(NO 3 ) 2 +Aq. Insol. in H 2 O, dil. acids, alkalies, and alkali sulphides +Aq. (Fresenius.) Sol. in HCN+Aq. (Hahn, C. C. 1870. 240.) Pptd. Ag 2 S is very sol. in HNO 3 containing more than 5% HNO 3 . (Gruener, J. Am. Chem. Soc. 1910, 32. 1032.) Only very si. sol. in AgNO 3 +Aq, even at 100. (Lowry, Roy. Soc. Proc. 1914, 91, A. 70.) Sol. in KCN+Aq. (Hahn, C. C. 1870. 240.) Difficultly sol. in KCN+Aq; less difficultly if Ag 2 S is pptd. from a very dil. solution. Amt. of KCN present also has influence on the solubility. Ag 2 S dissolved in cone. KCN +Aq separates out on dilution. (Be"champ, J. pr. 60. 64.) Insol. in NH 4 C1 or NH 4 NO 3 +Aq. (Brett.) Min. Argentite. Acanthite. Sol. in cone. HNO 3 -f Aq with separation of S. Sol. in citric acid+Aq with addition of KNO 3 . (Bolton, C. N. 37. 48.) Silver bisulphide, Ag 2 S 2 . Sol. in H 2 O with decomp.; also sol. with decomp. in HC1, HNO 3 . CS 2 does not dissolve out S. (Hantzsch, Z. anorg. 1898, 19. 105.) Silver sodium sulphide, 3Ag 2 S, Na 2 S+2H 2 O. Sol. in cone. Na 2 S+Aq with decomp.; sol. in H 2 O with decomp. (Ditte, C. R. 1895, 120. 93.) Silver zinc sulphide, Ag 2 S, 3ZnS. (Schneider, J. pr. (2) 8. 29.) Silver sulphimide* (silver thionyl imide), S0 2 NAg. Very si. sol. in cold, more sol. in hot H 2 O. Very sol. in dil. HNO 3 . (Traube, B. 1892, 25. 2474.) Silver sulphophosphide. See Silver phosphosulphide. Silver telluride, Ag 2 Te. Min. Hessite. Sol. in warm HNO 3 -f Aq. Sodammonium, Na 2 (NH 3 ) 2 . 100 g. liq. NH 3 dissolve 60.5 g. at -23; 56.4 g. at 0; 56 g. at +5; 55 g. at 9. (Joannis A. ch. 1906, (8) 7. 41.) Sodium, Na 2 . Violently decomposes H 2 O, alcohol, etc. Insol. in hydrocarbons. Easily sol. in acids with violent action. Solubility in fused NaOH. G. sol. in 100 g. fused NaOH at temp. t G. per 100 g. NaOH 480 25.3 600 10.1 610 9.9 670 9.5 760 7.9 800 6.9 (Hevesy, Z. Elektrochem. 1909, 15. 531.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) 1 gram atom dissolves: at +22 in 6.14 mol. liquid NH 3 . 30 50 70 105 C 5.87 5.52 5.39 5.20 4.98 (Ruff, B. 1906, 39. 839.) % ccm. oleic acid dissolves 0.0449 g. Na in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Insol. in ethylamine and in secondary and tertiary amines. (Kraus, J. Am. Chem. Soc. 1907, 29. 1561.) Sodium acetylide acetylene, Na 2 C 2 , C 2 H 2 . Very deliquescent. Decomp. by H 2 O and by absolute alcohol. Insol. in ether, ligroin, etc. (Moissan, C. R. 1898, 127. 915.) 836 SODIUM AMALGAM Sodium amalgam. NaHg 6 . Stable in contact with the liquid amalgam from 0-40.5. Can be cryst. from Hg without decomp. at ^,ny temp, between these limits. NaHg 5 . Stable in contact with the liquid amalgam from 40.5-150. Can be cryst. from Hg without decomp. at any temp, be- tween these limits. (Kerp, Z. anorg. 1900, 26. 68.) 2H 2 O, of which the solubility in 100 pts. H 2 O was found to be as follows: t Pts. NaBr t Pts: NaBr t Pts. NaBr 21 20 15 10 5 71.1 71.4 73.1 75.1 77.1 79.5 +5 10 15 20 25 82.0 84.5 87.3 90.3 93.8 30 35 40 45 50 97.3 101.3 105.8 110.6 116.0 Sodium amide, NaNH 2 . Decomp. by H 2 O and alcohol. Sodium amidochloride, Na 2 NH 2 Cl. Sol. in H 2 O with decomp. fJoannis, C. R. 112. 392.) Sodium arsenide, Na 3 As. Decomp. H 2 O. (Lebeau, C. R. 1900, 130. 504.) Sodium arsenide ammonia, Na 3 As, NH 3 . Easily sol. in liquid NH 3 . (Lebeau, C. R. 1900, 130. 502.) SI. sol. in liquid NH 3 . (Hugot, C. R. 1898, 127. 554.) Sodium azoimide, NaN 3 . Not hygroscopic. Sol. in H 2 O. Insol. in alcohol and ether. (Curtius, B. 24. 3344.) 40.16 pts. are sol. in 100 pts. H 2 O at 10. 40.7 " " " " 100 " H 2 O " ]5.2. 41.7 " " "" " 100 " H 2 O " 17.0. 0.3153 pt. is sol. in 100 pts. abs. alcohol at 16. Insol. in pure ether. (Curtius, J. pr. 1898, (2) 58. 279. Sodium bromide, NaBr, and +2H 2 O. Not deliquescent. Solubility in H 2 O dif- fers according as NaBr or NaBr+2H 2 O is used. The following data for anhydrous (Coppet, A. ch. (5) 30. 420.) If solubility S = pts. NaBr in 100 pts. solu- tion, S=40.0+0.1746tfrom -20 to +40; S = 52.3+0.0125t from 50 to 150. (Etard, C. R. 98. 1432.) 100 pts. H 2 O dissolve: at 0, 77.5 pts. NaBr; at 20, 88.4 pts.; at 40, 104.2 pts.; at 60, 111.1 pts.; at 80, 112.4 pts.; at 100, 114.9 pts. (Kremers.) Sat. solution boils at 121. (Kremers, Pogg. 97. 14.) Sat. NaBr+Aq contains at: 22 10 +140 163 40.1 42.5 56.5 57.5% NaBr, 180 180 210 212 230 59.5 59.0 60.9 61.0 62.0% NaBr. (Etard, A. ch. 1894, (7) 2. 539.) 100 g. sat. NaBr+Aq at 16.4 contain 47 g. NaBr. (Greenish, Pharm. J. 1900, 66. 190.) Solubility of NaBr+2H 2 O in H 2 O at 30 = 65.5% anhydrous NaBr. (Cocheret, Dissert. 1911.) Sp. gr. of NaBr+Aq at 19.5 containing: 5 10 15 20 25 % NaBr, 1.040 1.080 1.125 1.174 1.226 30 35 40 45 1.281 1.334 1.410 1.483 1.565 (Gerlach, Z. anal. 8. 285.) NaBr were found. Pts. NaBr dissolved by 100 pts. H 2 O at t. NaBr+Aq containing 17.15% NaBr has sp. gr. 20720 = 1.1473. NaBr+Aq containing 22.72% NaBr has sp.gr. 20720 = 1.2060. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) Sp. gr. of NaBr+Aq at 20.5. t Pts. NaBr t Pts. NaBr t Pts. NaBr 44.1 51.5 55.1 60.3 64.5 115.6 116.2 116.8 117.0 117.3 74.5 80.5 86.0 90.5 118.4 118.6 118.8 119.7 97.2 100.3 110.6 114.3 119.9 120.6 122.7 124.0 Normality of NaBr+Aq g. NaBr in 100 g. of solution Sp. gr. 20.5/4 4.33 3.00 1.99 0.98 33.57 25.10 17.77 9.41 1.3284 1.2284 1 . 1526 1.0750 Solubility is of the formula Below 50 tf represe S 110 'nted by a straight line .34+0.10751. isually crystallizes with le salt i (Oppenheimer, Z. phys. Ch. 1898, 27. 452.) SODIUM BROMIDE 837 Sp. gr. at 20 of NaBr+Aq containing Solubility in ethyl alcohol at 30. M g. mols. NaBr per liter. M 0.01 0.025 0.05 0.075 Sp. gr. 1.000732 1.002177 1.004074 1.005972 wt. % Solid phase Alcohol NaBr M 0.10 0.25 6.50 0.75 59.4 NaBr,2H 2 O Sp. gr. 1.00788 1.01964 1.03908 1.05811 11.79 42.90 31.78 32.12 M 1.0 1.5 2.0 Sp. gr. 1.07632 1.11963 1.15240 43.22 54.59 65.51 26.79 20.83 16.08 (Jones and Pearce, Am. Ch. J. 1907, 38. 728.) 72.36 13.41 76.92 12.03 NaBr, 2H 2 O+NaBr Sol. in H 2 SO 4 . (Walden, Z. anorg. 1902, 87.35 7.44 NaBr 29. 384.) 1 i\f\ -~ ~ AT^TD,. 1 A ^^4- <-*4- 1C 1O ^/-.v\4-ri^ 97.08 3.01 46.05 pts. NaBr; 100 pts. NaBr+NaCl+Aq sat. at. 18-19 contain 46.59 pts. of the two salts; 100 pts. NaBr+Nal+Aq sat. at 18-19 contain 63.15 pts. of the two salts; 100 pts. NaBr+NaCl+Nal+Aq sat. at 18-19 con- tain 63.20 pts. of the three salts, (v. Hauer, J. pr. 98. 137.) Solubility of NaBr in NaOH+Aq at 17. (Ditte, C. R. 1897, 124. 30.) Easily sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) Very si. sol. in alcohol. NaBr4-2H 2 O is sol. in 1.10 pts. H 2 O at 15; in 159 pts. absolute alcohol at 15; in 1200 pts. absolute ether at 15. (Eder, Dingl. 221. 89.) NaBr+2H 2 O is sol. in 2.25 pts. 60% alco- hol, and 7 pts. 90% alcohol. NaBr is sol. in 3 pts. 60% alcohol, and 10 pts. 90% alcohol. (Hager.) 100 pts. absolute methyl alcohol dissolve 17.35 pts. at 19.5. (de Bruyn, Z. phys. Ch. 10. 783.) 100 g. NaBr+CHgOH contain 0.9 g. NaBr at the critical temp. (Centnerszwer, Z. phys. Ch. 1910, 72. 437.) At room temp., 1 pt. NaBr by weight is sol. in: 4.6 pts. methyl alcohol D 18 0.7990. 14.0 " ethyl " D 15 0.8100. 49.7 " propyl D 15 0.8160. (Rohland, Z. anorg. 1898, 18. 325.) (Cocheret, Dissert. 1911.) Solubility in mixtures of methyl and ethyl alcohol at 25. P = % methyl alcohol in the solvent. G = g. NaBr in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. (G. per 100 g. H 2 U.) P G S 25/4 NaOH NaBr NaOH NaBr 0.00 4.37 10.40 41.02 80.69 84.77 91.25 100.00 0.293 0.365 0.404 0.724 1.251 1.286 1.432 1.440 0.8189 0.8265 0.8273 0.8593 0.9079 0.9104 0.9235 0.9238 0.0 3.26 9.24 13.43 17.17 19.12 91.38 79.86 68.85 64.90 63.06 62.51 22.35 24.74 28.43 36.61 46.96 54.52 59.60 55.03 48.00 38.41 29.37 24.76 (Herz and Kuhn, Z. anorg. 1908, 60. 155.) Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. NaBr in 10 ccm. of the solution. S=Sp. gr. of the sat. solution. p G S 25/4 1.440 0.9238 11.11 1.243 0.9048 23.8 1.053 0.8887 65.2 0.442 0.8390 91.8 0.147 0.8153 93.75 0.126 0.8144 100 0.074 0.8093 (Herz and Kuhn, Z. anorg. 1908, 60. 156.) 838 SODIUM STANNIC BROMIDE Solubility in ] P = % proDv nixtures of propyl and ethyl alcohol at 25. 1 alcohol in the solvent, in 10 ccm. of the solution. F the sat solution. 100 pts. H 2 O at t dissolve pts. NaCl. t Pts. NaCl Authority G = g. NaBr S = Sp. gr. o 13.89 16.90 59.93 109 . 73 More than at 13.89 35.81 35-. 88 37.14 40.38 Gay-Lussac, A. ch. (2) 11. 310. P G S 25/4 8.1 17.85 56.6 88.6 91.2 95.2 100 0.293 0.249 0.247 0.190 0.111 0.083 0.082 0.074 0.8189 0.8147 0.8145 0.8107 0.8116 0.8083 0.8090 0.8093 12 100 35.91 39.92 Fehling, A. 77. 382. 18.75 37.731 Bischof. 10-15 35.42 Bergmann. 106 + 42.86 Griffiths, 1825. 20 35.9 Schiff, A. 109. 326. (Herz and Kuhn, Z. anorg. 1908, 60. 159.) 2.05 g. are sol. in 100 g. propyl alcohol. (Schlamp, Z. phys. Ch. 1894, 14. 276.) SI. sol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) 100 g. 95% formic acid dissolve 22.3 g. NaBr at 18.5. (Aschan, Ch. Ztg. 1913, 37. Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314); benzonitrile. (Naumann, B. 1914, 47. 1370.) The composition of the hydrates formed by NaBr at different dilutions is calculated from determinations of the lowering of the fr- pt. produced by NaBr and of the conductivity and sp. gr. of NaBr+Aq. (Jones, Am. Ch. J. 1905, 34. 303.) All temps. 37 Fuchs and Reichenbach 1826. 25 35.7 Kopp, A. 34. 262.' 18.75 36.53 C. J. B. Karsten, 1840. 1 18.75 100 36.121 36 . 724 ' 41.076 G. Karsten. 1.25 Boiling 36.119 39.324 linger, J. pr. 8. 285. 18.75 100 35.40 36.95 Karsten (?), cited by linger, I.e. 15.56 100 34.2-35.42 36.16 lire's Diet. 15 35.837 Michel and Krafft. 1 pt. NaCl is sol. in 2.789 pts. H 2 O at 15 (Gerlach) ; in 3 pts. H 2 O at 18.75 (Abl) ; in 2.8235 pts. H 2 O at ord. temp. (Bergmann); in 2.7647 pts. boiling H 2 O (Berg- Sodium stannic bromide. See Bromostannate, sodium. Sodium uranous bromide, Na 2 UBr 6 . As K salt. (Aloy, Bull. Soc. 1899, (3) 21. 264.) Sodium zinc bromide, NaBr, ZnBr 2 +H 2 O. Hygroscopic. (Ephraim, Z. anorg. 1908, 2NaBr, ZnBr 2 +5H 2 O. Hygroscopic. (Ephraim.) Sodium carbide, Na 2 C 2 . Insol. in all neutral solvents; decomp. on heating and by H 2 O. (Matignon, C. R. 1897, 125. 1034.) Sodium carbonyl, Na 2 C 2 O 2 . Decomp. by H 2 O with explosion. (Joannis, C. R. 116. 1518.) Sodium sw&chloride, Na 4 Cl 2 . Decomp. by H 2 O into NaCl and NaOH + Aq. (Kreutz, B. 1897, 30: 403.) Sodium chloride, NaCl. Sol. in H 2 O. tClllp. \DULglLlCiLlLlJ , 111 ^.(LTX* pta. U^lllUg A-L'/W V mann); in 2.857 pts. hot or cold H 2 O (Fourcroy). Not deposited from boiling aqueous solution unless the vessel containing it is open to the air. (linger, I. c.) Solubility in 100 pts. H 2 O at t. t Pts. NaCl t Pts. NaCl 1.5 13.75 33.6 35.8 70 108.5 38.1 39.4 (Nordenskjold, Pogg. 136. 315.) Solubility in 100 pts. H 2 O at t. t Pts. NaCl t Pts. NaCl 13.89 16.90 35.8 35.9 59 . 93 109.73 37.1 40.4 (Gay-Lussac, A. ch. 11. 296.) Solubility of NaCl at various pressures. The figures represent pts. NaCl in 100 pts. sat. NaCl+Aq at t and A pressure in atmospheres. A 9 12 26.35 15 20 25 30 26.47 26.53 1 20 40 26.25 26.35 26.44 26.32 26.38 26.30 26.39 26.40 26 . 35 26.37 26.37 26.47 (Muller, Pogg. 117. 386.) SODIUM CHLORIDE 839 100 pts. H 2 O -dissolve at t. Solubility of NaCl in 100 pts. H 2 O at t. Continued. t Pts. NaCl t Pts. NaCl -15 i n 32.73 33.49 34.22 35.52 35.63 35.74 35.87 36.13 40 50 60 70 80 90 100 109.7 36.64 36.98 37.25 37.88 38.22 38.87 39.61 40.35 t 90 91 92 93 94 95 96 Pts. NaCl t Pts. NaCl t Pts. NaCl - 5 5 9 14 25 39.1 39.1 39.2 39.3 39.3 39.4 39.4 97 98 99 100 101 102 103 39.5 39.6 39.7 39.8 39.8 39.9 40.0 104 105 106 107 108 109 109.7 40.0 40.1 40.1 40.2 40.3 40.3 40.4 CPoffffiale. A. oh. (M 8. 649.) 100 pts. H 2 O dissolve at: 9 12 15 35 .59 35 . 72 35 .77 35 . 68 pts. NaCl, 20 25 30 35 .77 35 . 81 36 . 00 pts. NaCl. (Muller, Pogg. 122. 337.) 100 pts. H 2 O dissolve 35.76-36.26 pts. NaCl at 15.6, and the sp. gr. of sat. solution = 1.204. (Page and Keightley, Chem. Soc. (2) 10. 566.) 100 pts. NaCl+Aq sat. at 18-19 contain 26.47 pts. NaCl. (v. Hauer, J. pr. 98. 137.) Solubility of NaCl in 100 pts. H 2 O at t. t Pts. NaCl t Pts. NaCl t Pts. NaCl 35.7 30 36.3 60 37.3 1 35.7 31 36.3 61 37.3 2 35.7 32 36.3 62 37.4 3 35.7 33 36.4 63 37.4 4 35.7 34 36.4 64 37.5 5 35.7 35 36.4 65 37.5 6 35.7 36 36.5 66 37.6 7 35.7 37 36.5 67 37.7 8 35.7 38 36.5 68 37.7 9 35.7 39 36.6 69 37.8 10 35.8 40 36.6 70 37.9 11 35.8 41 36.6 71 37.9 12 35.8 42 36.7 72 38.0 13 35.8 43 36.7 73 38.0 14 35.8 44 36.8 74 38.1 15 35.9 45 36.8 75 38.2 16 35.9 46 36.8 76 38.2 17 35.9 47 36.9 77 38.2 18 35.9 48 36.9 78 38.2 19 36.0 49 36.9 79 38.3 20 36.0 50 37.0 80 38.4 21 36.0 51 37.0 81 38.4 22 36.0 52 37.0 82 38.5 23 36.1 53 37.1 83 38.6 24 36.1 54 37.1 84 38.6 25 36.1 55 37.1 85 38.7 26 36.1 56 37.2 86 38.7 27 36.2 57 37.2 87 38.8 28 36.2 58 37.2 88 38.9 29 36.2 59 37.3 89 39.0 (Calculated by Mulder from his own and other observations, Scheik. Verhandel. 1864. 37.) Solubility in 100 pts. H 2 O at: 0-4 20 40 60 80 35.630 35.825 36.32 37.06 38.00 (Andreae, J. pr. (2) 29. 456.) Solubility in 100 pts. H 2 O from most care- ful experiments. 20 35.571 35.853 (Raupenstrauch, M. Ch. 6. 563.) 60 37.091 80 38.046 Solubility of NaCl in 100 pts. H 2 O at t. t Pts. NaCl t Pts. NaCl -14.0 32.5 44.75 36.64 -13.8 32.15 52.5 37.04 - 6.25 34.22 55.0 36.99 - 5.95 34.15 59.75 37.31 35.7 71.3 37.96 3.6 35.79 74.45 37.96 5.3 35.8 82.05 38.41 14.45 35.94 86.7 38.47 20.85 35:63 93.65 38.90 25.45 35.90 101.7 40.76 38.55 36.52 Solubility above 20 is represented by the formula S = 34.359+0.0527t. (Coppet, A. ch. (5) 30. 426.) Solubility of NaCl in 100 pts. H 2 O at high temp. t Pts. NaCl t Pts. NaCl 118 140 39.8 42.1 160 180 43.6 44.9 (Tilden and Shenstone, Phil. Trans. 1884. 23.) 840 SODIUM CHLORIDE Sat. NaCl+Aq contains % NaCl at t. Solubility of NaCl in H 2 O at 24.5 at vary- ing pressures. S=g, NaCl in 100 -g. solvent. P= pressure in atmospheres. t % NaCl t % NaCl -21 -21 -18 17 23.7 23.4 23.5 23.3 25.5 25.8 26.7 26.8 77 90 115 135 140 150 180 215 28.0 28 2 29^1 28.9 28.8 29.6 30.2 31.6 P s 100 g. of solution contains g. NaCl - 7 +15 55 1 250 500 1000 1500 35.90 36.25 36.55 37.02 37.36 26.42 26.61 26.77 27.02 27.20 100 g. H 2 O dissolve 0.616 gram-equiva- lent NaCl at 25. (Van't Hoff and Meyer- hoffer, Z. phys. Ch. 1904, 49. 3150 Solubility of NaCl in H 2 O at t. Most careful experiments. ,. g. NaCl g. NaCl t per 100 Sp. gr. t per 100 Sp. gr. g. H 2 O g. H 2 0.35 35.75 1.2090 61.70 37.28 1.1823 15.20 35.84 1.2020 75.65 37.82 1.1764 30.05 36.20 1.1956 90.50 38.53 1.1701 45.40 36.60 1.1891 107 39.65 1.1631 (Berkeley, Phil. Trans. Roy. Soc. 1904, 203. A. 189.) Sat. NaCl+Aq. at 25 contains 26.5% NaCl. (Foote, Am. Ch. J. 1906, 36. 239.) 100 g. H 2 O dissolve 35.80 g. NaCl at 25. (Cameron, Bell and Robinson, J. phys. Ch. 1907, 11. 396.) 100 g. NaCl+Aq. sat. at 15 contains 26.3 g. NaCl; at 30, 26.47 g. (Schreine- makers, Arch. nee>. Sc. 1910, (2) 15. 81.) 5.456 g. mol. are contained in 1 1. NaCl + Aq sat. at 25. (Herz, Z. anorg. 1911, 73. 274.) 5.40 g. mol. are contained in 1 1. NaCl+Aq sat. at 30. (Masson, Chem. Soc. 1911, 99. 1136.) 26.47 g. NaCl are contained in 100 g. NaCl+Aq. sat. at 30. (Cocheret, Dissert. 1911.) 35.79 g. NaCl are sol. in 100 g. H 2 O at room temp. (Frankforter, J. Am. Chem. Soc. 1914, 36. 1106.) 100 mol. H 2 O dissolve at: 19.3 29.7 40.1 54.5 11.04 11.06 11.15 11. 35 mol. NaCl. (Sudhaus, Miner. Jahrb. Beil. Bd. 1914, 37. 18.) (Cohen, Inouye and Euwen, Z. phys. Ch. 1910, 75. 257.) Sp. gr. of NaCl+Aq containing 15% NaCl is 1.109 at 15 (Francoeur); 1.116 at 15 (Soubeiran); 1.1107 at 15 (Coulier); 1.111 at 15 (Baudin, C. R. 68. 932). Sp. gr. of NaCl+Aq saturated at 15 is 1.20715 (Michel and Krafft) ; at 17.5 is 1.2046 (Karsten) ; at 8 is 1.205 (Anthon). . gr. of NaCl+Aq. % NaCl Sp. gr. % NaCl Sp. gr. % NaCl Sp. gr. 5 1.037 15 1.112 25 1.192 10 1.074 20 1.154 26.43 1.204 (Dahlmann, J. B. 7. 321.) Sp. gr. of NaCl+Aq at 20. , % NaCl Sp. gr. % NaCl Sp. gr. 1 1.0066 15 1.1090 2 1.0133 16 1.1168 3 1.0201 17 1 . 1247 4 1.0270 18 1.1327 5 1.0340 19 1.1408 6 1.0411 20 1 . 1490 7 1.0483 21 1.1572 8 1.0556 22 1.1655 9 1.0630 23 1.1738 10 1.0705 24 1.1822 11 1.0781 25 1.1906 12 1.0857 26 1.1990 13 1.0934 27 1.2075 14 1.1012 t (Schiff, A. 110. 76.) Sp. gr. of NaCl+Aq at 19.5. % NaCl Sp. gr. % NaCl Sp. gr. 6.402 12.265 17.533 1.0460 1.0895 1.1303 22.631 26.530 1.1712 1.2036 (Kremers, Pogg. 95. 120.) SODIUM CHLORIDE 841 Sp. gr. of NaCl+Aq at 15. Sp. gr. of NaCl+Aq at 20. x = mols. NaCl to 100 mols. H 2 O. % NaCl Sp. gr. % NaCl Sp.gr. x Sp gr. x Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 .00725 .01450 .02174 .02899 .03624 .04366 1.05108 1.05851 1.06593 1.07335 1.08097 1.08859 1.09622 1 . 10384 15 16 17 18 19 20 21 22 23 24 25 26 26.395 1.11146 1.11938 1 . 12730 1 . 13523 1.14315 1.15107 1.15931 1 . 16755 1 . 17580 1 . 18404 1 . 19228 1.20098 1.20433 0.5 1.01145 4.0 1.08408 1.0 1.02255 5.0 1.10276 2.0 1.01393 (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of NaCl+Aq at 0. S = weight of salt in 100 g. of solution of the given sp. gr.; Si = No. mols. of salt contained in 100 mols. of the solution. S Si Sp. gr. (Gerlach, Z. anal. 8. 279.) Sp. gr. of NaCl+Aq at 18. 23.0821 19.1932 14.3415 9.4120 5.1536 8.627 6.769 4.898 3.097 1.644 1.1821 1 . 1502 1.1111 1.0722 1.0394 (Charpy, A. ch. (6) 29. 23.) Sp. gr. of NaCl+Aq. % NaCl Sp. gr. % NaCl Sp. gr. 5 10 15 20 1.0345 1.0707 1 . 1087 1 . 1477 25 26 26.4 1.1898 1 . 1982 1.2014 G. -equivalents NaCl per liter t Sp. gr. t/t (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of NaCl+Aq at 20, containing n mols. H 2 O to 1 mol. NaCl. 0.005028 0.01005 0.02005 0.04983 0.09873 0.19388 0.28999 0.47574 18.549 18.550 18.538 18.509 18.525 18.542 18.559 18.558 1.0002119 1.0004258 .000848 .002101 .004143 .008093 .012053 .019627 n Sp. gr. n Sp. gr. 12.5 25 50 1.15292 ' 1.08207 1.04227 100 200 1.02069 1.00965 0.49860 4.9860 18.06 17.85 1.02054 1.18783 0.00259 0.005178 0.010318 0.12580 0.25019 14.07 14.076 14.097 14.097 14.076 1.0001108 1.0002210 1.0004401 1.005315 1.010505 (Marignac, J. B. 1870. 110.) Sp. gr. of NaCl+Aq at 0. NaCl = g. NaCl to 100 g. H 2 O; d=sp. gr. at 0; d T = maximum sp. g> .; T =temp. of maximum. (Kohlrausch, W. Ann. 1894, 53. 26.) Sp. gr. of NaCl+Aq at 18/18. G. NaCl d dT T 1.00000 0.5 1.003925 1 1.007634 2 1.015366 3 1.023530 4 1.030669 6 1.045975 1.000130 1.003988 1.007666 1.015367 1.023583 1.030890 1.046952 + 4 + 3 + 1.77 0.58 3.24 5.63 11.07 g. -equivalents of NaCl in 1 liter of solution Sp. gr. 0.005 1.0002104 0.010 1.0004206 0.020 1.0008476 0.050 1.002109 0.100 1.004205 (Rosetti, A. ch. (4) 17. 382.) (Tammann, Z. phys. Ch. 1895, 16. 93.) 842 SODIUM CHLORIDE Sp. gr. of NaCl+Aq sat. 18.0, when cent strength of solution; d = ( density; and w= volume cone, in grams 'pd per cc. ' P d 25.37 .1928 21.25 .1592 17.35 .1277 13.25 .0958 9.34 .0665 4.810 1.0332 2.991 1.0202 2.593 1.0173 1.746 1.0111 0.30263 0.24637 0.19503 0.14518 0.09960 0.04969 0.03052 0.2638 0.01765 (Barnes. J. Phys. Chem. 1898, 2. 544.) Sp. gr. of NaCl+Aq at 20.5. Normality of NaCl +Aq G. NaCl in 100 g. of solution Sp. gr. 20.5/4 3.97 2.96 2.01 0.97 20.22 15.56 10.90 5.49 1.1489 1.1124 1.0775 1.0373 (Oppenheimer. Z. phys. Ch. 1898, 27. 451.) Sp. gr. of NaCl+Aq at 15. Per cent NaCl Sp. gr. 5 10 15 20 25 Sat. at 15 1.00000 1.03624 1.07335 1.11146 1 . 15107 1 . 19228 1.20433 (H. C. Hahn, J. Am. Chem. Soc. 1898, 20. 622.) Sp. gr. of NaCl+Aq at 18/4. g. NaCl in 100 g. of solution Sp. gr. 0.19560 0.097952 0.065410 0.048977 1.0001 0.9994 0.99918 0.99905 (Jahn, Z. phys. Ch. 1900, 33. 572.) Sp. gr. 20/4 of a normal solution of NaCl = 1.03866. (Haigh, J. Am. Chem Soc 1912, 34. 1151.) Sp. gr. of sat. NaCl+Aq at t. t g. NaCl sol. in 100 g. H 2 O Sp. gr. 10 32.90 1.200 35.63 1.210 10 35.69 1.205 20 35.82 1.202 30 36.03 1.198 40 36.32 1.193 50 36.67 1.189 60 37.06 1.184 70 37.51 1.178 (Tschernaj, J. Russ. Phys. Chem. Soc. 1912, 44. 1565.) Sp. gr. of dil. NaCl+Aq at 20.004. Cone. =g. equiv. NaCl per 1. at 20.004. Sp. gr. compared with H 2 O at 20. 004 = 1. Cone. Sp. gr. 0.0000 0.0001 0.0002 0.0005 0.0010 0.0020 0.0040 0.0050 0.0100 1.000,000,0 1.000,004,2 1.000,008,5 1.000,021,3 1.000,042,7 1.000,085,1 1.000,169,6 1.000,211,7 1.000,423,3 (Lamb and Lee, J. Am. Chem. Soc. 1913, 35. 1686.) The saturated solution boils at 109. (Kremers.) NaCl+Aq containing 42.9 pts. NaCl to 100 pts. H 2 O boils at 106.8 (Griffiths); contain- ing 41.2 pts. NaCl to 100 pts. H 2 O boils at 108.2 (Legrand); containing 40.38 pts. NaCl to 100 pts. H 2 O boils at 109.73 (Gay- Lussac); containing 38.7 pts. NaCl to 100 pts. H 2 O forms a crust at 108.3; highest point ob- served, 108.8 (Gerlach, Z. anal. 26. 426.) Boiling-point of NaCl-f-Aq. % NaCl B.-pt. according to Bischof G. Karsten 5 10 15 20 25 29.4 101.50 103.03 104.63 106.26 107.93 107.9-108.99 101 . 10 102.38 103.83 105.46 107.27 % NaCl B.-pt. according to Legrand Gerlach 5 10 15 20 25 100.80 101.75 103.00 104.60 106.60 100.9 101.9 103.3 105.3 107.6 SODIUM CHLORIDE 843 B.-pt. of NaCl+Aq containing pts. NaCl to 100 pts. H 2 O. G = according to Gerlach (Z. anal. 26. 438; L = according to Le- grand (A. ch. (2) 69. 431). Solubility in HCl+Aq at 10-10.5. g. per 100 cc. G. per 100 cc. HC1 NaCl HC1 NaCl B.-pt. G L B.-pt. G L 0.0 9.84 12.76 15.68 20.78 35.77 33.76 33.19 32.71 31.77 26.06 94.77 102.1 120.6 30.89 20.01 19.04 16.03 100.5 101 101.5 102 102.5 103 103.5 104 104.5 105 3.4 6.6 9.6 12.4 14.9 17.2 19.4 21.5 23.5 25.5 4.4 7.7 10.8 13.4 15.9 18.3 20.7 23.1 25.5 27.7 105.5 106 106.5 107 107.5 108 108.4 108.5 108.8 27.5 29.5 31.5 33.5 35.5 37.5 39^5 40.7 29.8 31.8 33.9 35.8 37.7 39.7 41.2 (Enklaar, R. t. c. 1901, 20. 183.) Solubility in HCl+Aq at 30. Composition of the solution B.-pt. of NaCl+Aq containing g. NaCl in 100 g. H 2 0. g. NaCl 7.6 11.0 14.9 16.1 18.8 B.-pt. 102.2 103 104.2 104.8 106.1 g. NaCl 22.3 24.0 26.0 28.7 B.-pt. 107.1 107.7108.7 109.5 (Richmond, Analyst, 1893, 18. 142.) % by wt. HC1 % by wt. NaCl 6 12 17 35 .93 .50 .35 .60 26. 16. 9. 4. 0. 47 16 35 52 11 (Schreinemakers, Z. phys. Ch. 1909, 68. 85.) If NaCl is dissolved in 15 pts. H 2 O, . heat is absorbed if the temp, is 15, but much less if temp, is 86; at 100 there is neither ab- sorption nor evolution of heat. (Berthelofc, C. R. 78. 1722.) 36 pts. NaCl mixed with 100 pts. H 2 O at 12.6 lower the temp. 2.5. (Riidorff, B. 2. 68.) 33 pts. NaCl with 100 pts. snow at 1 give a temp, of 21.3. (Riidorff, Pogg. 122. 337.) The freezing-point of NaCl+Aq is lowered 0.60 for every gram ftaCl up to 10 g. When more cone, the freezing-point sinks pro- portional to NaCl, 2H 2 O, 0.342 for every gram of that salt. (Riidorff, Pogg. 113. 163.) Insol. in cone. HCl+Aq. Solubility of NaCl in HC1 + Aq at 0. NaCl = mols. NaCl (in milligrams) dissolved in 10 ccm. of liquid; HCl = mols. HCl (in milligrams) dissolved in 10 ccm. of liquid. NaCl HCl Sum of mols. Sp. gr. 53.5 1 54.5 .2045 52.2 1.85 54.05 .2025 48.5 5.1 53.6 .196 44.0 9.275 53.275 .185 37.95 15.05 53.00 .1725 23.5 30.75 54.95 .141 6.1 56.35 62.45 1.1159 (Engel, Bull. Soc. (2) 46. 654.) Solubility in HCl+Aq. Cone. = concentration of HCl. g. mol. per 1,000 g. H 2 O. NaCl = wt. NaCl dissolved in 1,000 g. H 2 O. t Cone. NaCl Molecular solubility 0.25 0.50 l.CO 357.75 341.70 324.45 291.20 6.13 5.85 5.56 4.99 25 0.25 0.50 1.00 360.80 344.50 329.05 298.10 6.18 5.90 5.64 5.10 (Armstrong and Eyre, Proc. R. Soc. 1910, (A) 84. 127.) Solubility in HCl+Aq at 30. (Jr. mols. per 1. HCl NaCl Sp. gr. 30 HCl NaCl Sp. gr. 30 0.0 0.4575 0.969 1.786 2.412 5.400 4.932 4.386 3.589 2.412 1.2018 1 . 1906 1.1801 1.1633 1.1512 3.052 4.152 5.950 7.205 2.463 1.628 0.630 0.268 1.1427 1.1289 1.1188 1.1258 (Masson, Chem. Soc. 1911, 99. 1132.) 844 SODIUM CHLORIDE Solubility in HCl-f-Aq at 25. Solubility in NaOH+Aq at 0. NaCl = mols. NaCl (in milligrams) in 10 ccm. solution; Na 2 O=mols. Na 2 O (in milligrams) in 10 ccm. solution. Millimols HC1 in 10 ccm. Millimols NaCl in 10 ccm. e'o7 10.32 15.90 21.17 32.83 54.56 48.50 44.67 37.82 32.97 23.43 NaCl Na 2 Na 2 + NaCl Sp. gr. 54.7 49.375 47.212 42.375 39.55 24.95 19.3 9.408 4.8 6.725 10.406 14.78 30.5 37.875 53.25 54.7 54.175 53.937 52.781 54.33 55.45 57.175 62.66 1.207 1.221 1.225 1.236 1.249 1.295 1.314 1.362 (Herz, Z. anorg. 1912, 73.^274.) Moderately dil. H 2 SO 4 or HNO 3 +Aq pre- cipitate NaCl from NaCl-f-Aq. (Karsten.) Sol. in H 2 SO 4 . (Walden, Z. anorg. 1902, 29. 384.) Solubility of NaCl in NH 4 OH+Aq at 30. (G. in 1 1. sat. solution.) (Engel, C. R. 112. 1130.) Solubility in NaOH+Aq at 20. G. NaOH in 1 liter G. NaCl in 1 liter Sp. gr. deg. Baume 10 20 30 40 50 60 70 80 90 100 110 120 130 140 150 160 170 180 190 200 210 220 230 240 250 260 270 280 290 300 310 320 330 340 350 360 370 380 390 400 410 420 430 308 308 306 302 297 286 277 269 261 253 244 236 229 221 213 205 197 189 181 173 165 159 152 146 139 134 129 124 118 112 107 101 96 90 85 80 76 71 66 61 56 52 48 1.200 1.210 1.215 1.225 1.230 1.235 1.240 1.245 1.250 1.250 1.252 1.252 1.260 1.265 1.270 1.275 1.275 1.280 1.285 1.290 1.295 1.295 1.300 1.303 1.305 1.310 1.315 1.320 1.325 1.330 1.333 1.335 1.340 1.345 1.350 1.355 1.360 1.365 1.370 1.375 1.380 1.385 1.390 23.5 24.0 25.5 26.4 26.9 27.4 27.9 28.4 28.8 28.8 29.0 29.0 29.7 30.2 30.6 31.1 31.1 31.5 32.0 32.4 32.8 32.8 33.3 33.5 33.7 34.2 34.6 35.0 35.4 35.8 36.0 36.2 36.6 37.0 37.4 37.8 38.2 38.6 39.0 39.4 40.0 40.2 40.6 Sp. gr. NH 3 NaCl ISp. gr. NH 3 NaCl 1.17352 1 . 1656 4 1.160 4 1 . 1494 6 !9.535 -0.655 7.26 0.78 293.38 292.5 289.7 286.5 1.140872.07 1.139572.715 1.130181.855 1.205 97.49 283.38 283.06 277.49 270.57 (Hempel and Tedesco, Z. anorg. 1911, 24. 2467.) Solubility of NaCl in NH 4 Cl+Aq at t. t G. per 100 g. H 2 O Sp. gr. NH 4 C1 NaCl 146. 1 356.3 286.4 M85 15 57. 118. 186. 198. 3 9 4 8 357.6 326.4 300 271.6 266.8 1 1 1 1 1 !200 .191 .183 .176 .175 30 255. 4 360.3 249 1*168 45 322. 1 365 233.9 . . . (Fedotieff, Z. phys. Ch. 1904, 49. See also under NH 4 C1. 168.) SODIUM CHLORIDE 845 Solubility in NaOH+Aq at 20. Continued. G. NaOH in 1 liter G. NaCl in 1 liter Sp. gr. deg. Baum6 440 45 1.395 41.0 450 42 .400 41.5 460 39 .405 41.9 470 37 .410 42.0 480 34 .415 42.3 490 32 .420 42.6 500 30 .425 43.0 510 28 .430 43.5 520 27 1.435 43.7 530 27 1.440 44.0 540 26 1.445 44.3 550 26 1.450 44.6 560 25 1.450 44.6 570 24 1.455 45.0 580 23 1.460 45.5 590 23 1.465 45.9 600 22 1.470 46.2 610 21 1.475 46.5 620 20 1.480 46.8 630 19 1.485 47.0 640 18 1.490 47.5 (Winteler, Z. Elektrochem, 1900, 7. 360.) Solubility in Na 2 O+Aq at 30. Composition of the solution % by wt. Na'O % by wt. NaCl Solid phase 26.47 NaCl 4.47 21.49 t 12.22 13.62 i 24.48 4.36 f 29.31 2.40 i 37.85 1.12 1 41.42 0.97 NaCl+NaOH, H 2 O 42 NaOH, H 2 O (Schreinemakers, Z. phys. Ch. 1909, 68. 85.) The presence of other salts increases the solubility of NaCl in H 2 O. Sol. in sat. NH 4 Cl+Aq with pptn. of NH 4 C1. When the reaction is complete, the solution has sp. gr. 1.1788, and contains 32.62% mixed salts; or 100 pts. H 2 O dissolve 48.42 pts. mixed salts, viz., 26.36 pts. NaCl and 22.08 pts. NH 4 C1. (Karsten.) (See under NH 4 C1.) Sol. in sat. BaCl 2 +Aq with pptn. of BaCl 2 until a state of equilibrium is reached, when 100 pts. H 2 O at 17 dissolve 38.6 pts. of mixed salts, of which 4.1 pts. are BaCl 2 . (Karsten.) (See under BaCl 2 .) Insol. in sat. CaCl 2 +Aq. (Vauquelin, Ann. de Chim. 13. 95.) Much more sol. in hot than in cold H 2 O containing MgCl 2 or CaCl 2 ; but NaCl is pptd. from sat. NaCl+Aq when that solution is mixed with MgCl 2 or CaCl 2 + Aq. (Fuchs and G. Reichenbach, 1826.) (See under MgCl 2 .) Less sol. in cone. CaCl 2 +Aq than in H 2 O. (Hermann.) Solubility of NaCl+CaCl 2 in H 2 O at 25. G. per 100 g. H 2 O. NaCl 1.846 1.637 1.799 7.77 10.70 18.85 32.48 35.80 CaCh 84 78.49 58.48 53.47 36.80 30.08 19.53 3.92 Sp. gr. 25/25 4441 3651 3463 2831 2653 2367 2080 1.2030 Solid phase CaCl 2 , 6H 2 O " +NaCl NaCl (Cameron, Bell and Robinson, J. phys. Chem. 1907, 11. 396.) Solubility of NaCl in NaHCO 3 sat. with CO 2 at t. u 15 ^( ... 30 45 G. per 1000 g. H 2 O NaHC0 3 6.0 7.7 0.0 10.0 0.0 13.9 0.0 0.23 NaCl 356.3 350.1 357.6 354.6 360.3 358.1 356.0 361.5 (Fedotieff, Z. phys. Ch.ll904, 49. 170.) Sol. in sat. KClO 3 +Aq; the solution can then dissolve more KC1O 3 . (Margueritte. C. R. 38. 305.) In solution containing Na, K, Cl and NO 3 ions, the solubility relations between the four salts NaCl, KC1, NaNO 3 and KNO 3 have been studied. (Uyeda, Z. anorg. 1911, 71. 2.) Sol. in sat. NH 4 NO 3 +Aq, without causing pptn. (Karsten.) Sol. in sat. NH 4 NO 3 +Aq, from which solu- tion it is not pptd. by salts which would cause its pptn. in aqueous solution. (Margueritte, C. R. 38. 307.) Sol. in sat. Ba(NO 3 ) 2 +Aq without causing pptn. Insol. in Ca(NO 3 ) 2 +Aq. Sol. in Mg(NO 3 ) 2 +Aq with pptn. of small portion of Mg(NO 3 ) 2 . Sol. in sat. KNO 3 +Aq, the mixed solution having the power to dissolve more KNO 3 , and the solubility of the KNO 3 apparently in- creasing in the same ratio as the amount of NaCl present. (Fourcroy and Vauquelin, Ann. de Chim. 11. 130.) Sol. in sat. KNO 3 +Aq; the solution thus 846 SODIUM CHLORIDE obtained at 18.13 contains 40.34% of the mixed salts, or 100 pts. H 2 O dissolve 67.72 pts. of the mixed salts, viz., 38.25 pts. NaCl and 29 . 45 pts. KNO 3 . (Karsten.) Solubility of NaCl in KNO 3 +Aq at 25. KNO 3 = g. KNO 3 in 100 cc. of solution. NaCl=g. mol. per 1. KNO 3 NaCl KN0 3 NaCl 4 8 5.44 5.52 5.45 12 16 20 5.28 5.21 5.15 (Ritzel, Z. Krist. 1911, 49. 152.) (See also under KNO 3 .) Solubility of NaCl in NaNO 3 +Aq at 15.5. g. per 100 cc. sat. s olution Sp. gr. NaNOa NaCl H 2 .2025 31.78 88.47 .2305 7.53 27.89 87.63 .2580 13.24 26.31 86.25 .2810 21.58 23.98 82.66 .3090 28.18 22.30 80.42 .3345 33.80 20.40 79.25 .3465 37.88* 19.40* 77.37 .3465 37.64* 19.67* 77.34 *Solutions sat. with both salts. (Bodlander, Z. phys. Ch. 1891, 1. 361.) Sol. in sat. NaNO 3 +Aq with pptn. of NaN0 3 . Solubility of NaCl in NaNO 3 +Aq. Cone. = concentration of NaNO 3 in g. mol. per 1,000 g. H 2 O. NaCl = g. NaCl dissolved in 1,000 g. H 2 O. t Cone. NaCl Molecular solubility 0.25 0.50 1 359.65 355.90 351.20 342.15 6.16 6.09 6.02 5.86 25 0.25 0.50 1 2 362.95 356.65 352.30 343.65 325.50 6.20 6.11 6.03 5.88 5.58 (Armstrong and Eyre, Proc. R. Soc. 1910, A. 84. 127.) (See also under NaNO 3 .) Sol. in sat. KCl+Aq with elevation of temp. (Vauquelin.) 100 g. H 2 O sat. with KCl dissolve 0.494 gram-equivalent NaCl at 25. (Fuler, Z. phys. Ch. 1904, 49. 315.) Solubility in KCl+Aq at t. t Sat. solution contains % NaCl % KCl -20 21.3 5.7 -10 21.3 6.7 21.3 7.7 +10 21.3 8.6 20 21.3 9.6 30 21.3 10.6 40 21.3 11.5 50 21.3 12.5 60 21.3 13.5 70 21.3 14.4 80 20.7 15.8 90 19.9 17.8 100 18.8 19.8 110 17.2 22.4 120 16.5 24.1 130 16.4 25.1 140 16.4 26.1 150 16.4 27.1 160 16.4 28.0 170 16.4 29.0 180 16.4 30.0 (Etard. A. ch. 1894, (7) 3. 277.) (See under KC1.) 100 pts. NaCl+Nal+Aq sat at 18-19 contain 62.33 pts. of the two salts, (v. Hauer.) Sol. in sat. Al 2 (SO 4 ) 3 +Aq with no pptn. (Vauquelin.) Sol. in sat. (NH 4 ) 2 SO 4 +Aq with pptn. of considerable amt. of (NH 4 ) 2 SO 4 +Aq. (Vau- quelin.) Sol. in sat. CuSO 4 +Aq. 100 pts. H 2 O dissolve 36.71 pts. NaCl and 7.19 pts. K 2 SO 4 at 15, and solution has sp. gr. 1.24. (Page and Keightey.) NaCl is sol. in K 2 SO 4 +Aq, and vice versa, without separation of a salt. 100 pts. H 2 O dissolve 7.03 pts. K 2 SO 4 and 37.60 pts. NaCl, when warmed and cooled to 14. (Rudorff.) Solubility of NaCl and K 2 SO 4 in H 2 O at t. 100 3ts. H 2 O contain pts. NaCl, K 2 SO 4 , and KC1. t Pts. NaCl Pts. K 2 S0 4 Pts. KCl 10 33.43 8.10 3.18 20 34.01 8.90 3.06 30 34.56 9.56 2.95 40 35.16 10.38 2.81 50 35.77 11.07 2.84 60 36.40 11.93 2.72 70 36.64 12.82 3.20 80 36.04 12.26 5.06 90 35.86 12.42 6.98 100 35.63 12.56 8.79 (Precht and Wittgen, B. 15. 1666.) SODIUM CHLORIDE 847 Sol. in cold sat. NaSO 4 +Aq at first without pptn., afterwards Na 2 SO 4 separates out. (Karsten.) Solubility in Na 2 S0 4 +Aq containing 7.45 g. Na 2 SO 4 in 100 g. of the solution. 14.80 17.90 24.85 25.60 27.75 32.18 34.28 g. NaCl in 100 g. of the solution 23.30 23.33 23.45 23.485 23.525 23.55 23.68 (Marie and Marquis, C. R. 1903, 136. 684.) See also under Na2SO 4 . Sol. in sat. ZnSO 4 +Aq with separation of Na 2 SO 4 , ZnSO 4 . (Karsten.) Insol. in liquid CO 2 . (Buchner, Z. phys. Ch. 1906, 54. 674.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) 12.2 pts. NaCl are sol. in 1 pt. hydrazine at 12.5-13. (de Bruyn, R. t. c. 1899, 18. 297.) 100 g. hydroxylamine dissolve 14.7 g. NaCl at 17.5. (de Bruyn, Z. phys. Ch. 1892, 10. 782.) 100 g. 95% formic acid dissolve 5.8 g. at 19.7. (Aschan, Ch. Ztg. 1913, 37. 1117.) Solubility in alcohol. 100 pts. alcohol of 0.900 sp. gr. dissolve 5.8 pts. NaCl; of 0.872 sp. gr. dissolve 3.67 pts. NaCl; of 0.834 sp. gr. dissolve 0.5 pt. NaCl. (Kirwan.) 100 pts. alcohol containing given % by weight of absolute alcohol dissolve pts. NaCl at 25. % alcohol Pts. NaCl % alcohol Pts. NaCl % alcohol Pts. NaCl 0.0 8.4 16.7 25.1 35.70 30.49 24.84 19.30 33.4 41.8 50.2 58.5 16.08 13.28 11.28 7.96 66.9 75.2 83.6 5.95 3.75 1.59 (Kopp, A. 40. 206.) 100 pts. alcohol of 75% by weight dissolve at: 14 15.2 38 71.5 0.661 0.700 0.736 1.033 pts. NaCl. 100 pts. alcohol of 95.5% by weight dissolve at: 15 77.2 0.174 0.171 pts. NaCl. (Wagner, A. 64. 293.) 100 pts. alcohol containing % alcohol by weight dissolve pts. NaCl at 15, or 100 pts. solution contain % NaCl. 10 20 30 40 % alcohol, 28.53 22.55 17.51 13.25 pts. NaCl, 22.2 18.4 14.9 11.7 % NaCl, 50 60 80 % alcohol, 9.77 5.93 1.22 pts. NaCl, 8.9 5.6 1.2 %NaCl. (Schiff, A. 118. 365.) Solubility of NaCl in alcohol increases with the temperature. 100 pts. (by weight) of alcohol of 0.9282 sp. gr. (50.5% by weight) dissolve at: 4 10 13 23 32 10.9 11.1 11.43 11.9 12.3 pts. NaCl, 33 12.5 44 ( 13.1 51' 13.8 60 __._ 14.1 pts. NaCl. (Gerardin, A. ch. (4) 5. 146.) Solubility in alcohol at 13. Sp. gr. 100 com. contain in g. Alcohol Water Salt 1.2030 88.70 31.60 1.1348 11.81 78.41 23.26 1.1144 15.99 74.64 20.81 1.0970 19.39 71.45 18.86 1.0698 24.95 65.80 16.23 1.0295 32.33 57.96 12.66 0.9880 40.33 49.34 9.13 0.9445 49.28 38.54 5.93 0.9075 57.91 29.37 3.47 0.8700 63.86 21.62 1.52 0.8400 72.26 11.24 0.50 (Bodlander, Z. phys. Ch. 7. 317.) Solubility in ethyl alcohol +Aq at 30. wt. % g. NaCl per 100 g. wt. % g. NaCl per 100 g. alcohol solution H 2 alcohol solution H 2 O 26.50 36.05 50 9.34 20.60 5 24.59 34.29 60 6.36 16.96 10 22.56 32.57 70 3.36 12.75 20 19.05 29.40 80 1.56 7.95 30 15.67 26.53 90 0.43 4.30 40 12.45 23.70 (Taylor, J. phys. Ch. 1897, 1. 723.) Solubility in ethyl alcohol +Aq at 40. wt. % alcohol g. NaCl per 100 g. wt. % alcohol g. NaCl +100 g. solution H 2 solution H 2 O 5 10 20 30 40 26.68 24.79 22.90 19.46 16.02 12.75 36.38 34.69 33.00 30.20 27.25 24.37 50 60 70 80 90 9.67 6.65 3.87 1.69 0.50 21.42 17.82 13.10 8.68 5.10 (Taylor, I. c.) 848 SODIUM CHLORIDE Solubility of NaCl in ethyl alcohol +Aq a 28. C&E 3.8 7.7 16.1 25.3 35.0 % H 2 73.53 71.6 69.7 64.6 58.9 52.5 NaCl 26.47 24.6 22.6 19.3 15.8 12.5 C 2 H 6 OH 45.35 56.2 67.4 78.8 89.6 % H 2 45.35 37.5 28.9 19.7 10 % NaCl 9.3 6.3 3.7 1.5 0.4 (Fontein, Z. phys. Ch. 1904, 73. 212.) Solubility of NaCl in ethyl alcohol +Aq at 25 Cone. = concentration of alcohol in g. mol per 1,000 g. H 2 O. NaCl = g. in 1,000 g.H 2 O. Cone. 0.25 0.50 1 3 NaCl 359.65 355.15 349.65 337.80 301 . 60 Molecular solubility 6.16 6.08 5.98 5.79 5.16 (Armstrong and Eyre, Proc. R. Soc. 1910, (A) 84. 127.) 100 pts. absolute methyl alcohol dissolve 1.41 pts. at 18.5; 100 pts. absolute ethyl alcohol dissolve 0.085 pt. at 18.5. (de Bruyn, Z. phys. Ch. 10. 782.) 100 pts. wood-spirit of 40% (by weight) dissolve 13.0 pts. NaCl. (Schiff, A. 118. 365.) 100 g. NaCl+CH 3 OH contain 0.1 g. NaCl at the critical temp. (Centnerszwer, Z. phys. Ch. 1910, 72. 437.) Solubility of NaCl in methyl alcohol -f-Aq. at 25. Cone. = concentration of alcohol in g. mol. per 1,000 g. H 2 O. NaCl = g. in 1,000 g. H 2 O. t Cone. NaCl Molecular solubility 0.25 0.50 1 357.75 355.20 353.10 347.45 6.13 6.08 6.05 5.95 25 0.25 0.50 1 3 362.95 359.40 357.60 353.20 336.25 6.20 6.14 6.11 6.04 5.75 (Armstrong and Eyre, Proc. R. Soc. 1910, (A) 84. 127.) Traces dissolve in propyl alcohol. (Schlamp Z. phys. Ch. 1894, 14. 276.) Solubility of NaCl in propyl alcohol +Aq. at 25. Cone. = concentration of alcohol in g. mol. per 1,000 g. H 2 O. NaCl = g. NaCl in 1,000 g. H 2 O. 25 Cone. 0.25 0.50 0.25 0.50 NaCl 357.75 351.20 345.55 362.95 355.75 350.20 Molecu lar solubility 6.13 6.01 5.91 6.20 6.10 6.00 (Armstrong and Eyre, Proc. R. Soc. 1910, A. 84. 127.) Solubility of NaCl in propyl alcohol +Aq at 23-25. NaCl 0.55 2.23 3.55 3.90 5.27 8.04 10.49 12.20 /o C 3 H 7 OH 87.7 51.57 18.99 14.78 12.77 9.49 7.79 6.57 11.75 46.20 77.46 81.32 81.96 82.47 81.72 81.23 NaCl 14.38 15.42 16.38 18.08 20.12 22.35 24.50 24.90 CsHyOH 5.39 5.11 4.47 3.83 3.27 2.64 2.13 2.3 & 80.23 79.47 79.14 78.09 76.61 75.01 75.37 72.80 Frankforter and Frary, J. phys. Ch. 1913, 17. 402.) 100 g. sat. solution of NaCl in 99.6% propy alcohol contain 0.04 g. NaCl at 25. (Frank- "orter and Frary.) Insol. in fusel oil. (Gooch, Am. Ch. J. 9. 53.) Solubility of NaCl in amyl alcohol +Aq. Liquid phases conjugated at 28. Upper layer Lower layer NaCl amyl alcohol H 2 NaCl amyl alcohol H 2 O 0.05 it a a 95.45 94.1 92.9 91.6 90.2 4.5 5.9 7.1 8.4 9.8 26.36 19 12.7 6.2 0.22 0.4 0.8 1.5 2.3 73.42 80.4 86.5 92.3 97.7 (Fontein, Z. phys. Ch. 1910, 73. 226.) At room temp. 1 pt. by weight is sol. in: 75 pts. methyl alcohol D 15 0.7990. 566 " ethyl " D 15 0.8100. 3000 " propyl " D 15 0.8160. (Rohland, Z. anorg. 1898, 18. 325.) 100 g. methyl alcohol dissolve 1.31 g. NaCl t 25. SODIUM CHLORIDE 849 100 4- OK g. ethyl alcohol dissolve 0.065 g. NaCl Solubility in acetone -f-Aq at 20. at Jo . 100 g. propyl alcohol dissolve 0.012 g. NaCl % NaCl %H 2 % acetone at 25 100 NaCl g. isoamyl alcohol dissolve 0.002 g. at 25. 25.9 24.19 73.06 71.18 1.04 4.03 25.06 72.00 2.94 (Turner and Bissett, Chem. Soc. 1913, 103. 20.85 66.78 12.37 1909.) 20.17 66.01 13.82 18.32 63.16 18.52 Solubility of NaCl in ethyl + amyl alcohol at 20.44 66.19 13.37 28. 17.89 62.21 19.90 32 13 92 85.76 Upper layer Lower layer o!l9 10.82 88.99 0.15 9.62 90.23 NaCl % amyl alcohol % ethyl alcohol N?C1 %amyl alcohol % ethyl alcohol 0.12 8.94 90.94 0.05 95.45 26.35 0.22 (Frankforter and Cohen, J. Am. Chem. Soc. 0.10 86.6 9.5 25.30 0.25 1.9 1914, 36. 1127.) 0.25 75.4 19.1 24.02 0.3 9.5 0.58 59.9 30.9 22.64 0.4 6.9 Solubility in glycol at 14.8 = 31.7%. (de 1.23 47.0 38.7 21.19 0.5 10.3 Coninck, Belg. Acad. Bull. 1905. 275.) 2.81 31.6 44.8 19.26 1.3 15.2 Sol. in glycerine. (Pelouze.) 6.56 17.7 41.5 15.81 3.69 22.1 Critical solution: amyl alcohol, 10%; ethyl alcohol, 32.5%; NaCl, 11%; H 2 O, Solubility of NaCl in glycerine +Aq at 25. G = g. glycerine in 100 g. glycerine +Aq. NaCl = millimols NaCl in 100 cc. of the 46.5%. solution. (1* ontein, Z. phys. Ch. 1910, 73. 244.) G NaCl Sp.gr. Ether ppts. NaCl from NaCl-f-Aq. 545.6 1 . 1960 CGmelin.) Very si. sol. in a mixture of equal pts. of absolute alcohol and ether. (Berzelius.) 500 mg. NaCl treated with above mixture yielded only 0.5 mg. to the liquid. (Lawrence Smith, Am* J. Sci. (2) 16. 57.) 13.28 25.98 45.36 54.23 83.84 100 501.1 448.4 370.2 333.9 220.8 167. 1 1.2048 1.2133 1.2283 1.2381 1.2696 1 2964 100 pts. of a mixture of 1 pt. 96% alcohol J-V/VJ and 1 pt. 98% ether dissolve 0.11 pt (Mayer, A. 98. 205.) NaCl. (Herz and Knoch, Z. anorg. 1905, 46. 267.) Insol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184; Eidmann, C. C. 1899, II. 1 A1 A \ Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) 1014.) Insol. in methyl acetate. (Naumann, B. Solubility in acetone +Aq at 20. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3602.) A = ccm. acetone in 100 ccm. of the solvent. NaCl = millimols NaCl in 100 ccm. of the solution. Solubility of NaCl in solutions of HgCl 2 in ethyl acetate. A NaCl 100 mo Is. ethyl acetate dissolve 537.9 Mols. HgCl 2 Mols. NaCl Mols. HgCh Mols. NaCl 10 4-fi4. fi 20 394.8 40.0 20.0 18.0 5,1 , 30 330.1 38.1 19.6 16.4 4.3 32] lower layer 308 . 5 36.0 19.2 14.1 3.8 to > 2 phases 34.9 18.5 13.2 2.9 87 J upper layer 7 . 7 34.8 18.3 12.4 2.3 88 7.3 32.1 13.8 12.0' 1.6 89 5.6 28.0 9.1 12.2 1.3 90 4.3 22.8 7.0 12.9 0.8 100 22.9 7.0 (Herz and Knoch, Z. anorg. 1904, 41. 318.) (Linebarger, Am. Ch. J. 1894, 16. 215.) 850 SODIUM STANNIC CHLORIDE Solubility of NaCl in urea+Aq at 25. Sodium stannic chloride, 2NaCl, See Chlorostannate, sodium. Sodium thallic chloride, 3NaCl, 12H 2 O. Very sol. in H 2 O. (Pratt, Am 1895, (3) 49. 404.) SnCl 4 + T1C1 3 + J. Sci. % urea % NaCl % urea % NaCl 5 9.6 13 31.80 30.63 29.05 28.46 18 23 28 27.65 27.24 26.56 (Ritzel, Z. Kryst. Min. 1911, 49. 152.) Solubility of NaCl in urea+Aq at (?). g = g. urea in 100 cc. of solution, sol. = increase of solubility of NaCl in g. per 100 cc. of the solution. g. sol. g. sol. 5 10 15 20 25 0.044 0.124 0.234 0.372 0.529 30 35 40 45 50 0.709 0.910 1.134 1.370 1.602 (Fastert, N. Jahrb. Min. Beil. Bd. 1912, 23. 286.) Solubility of NaCl in formamide+Aq at 25. % HCONH 2 % NaCl %HCONH 2 % NaCl 2.3 5.3 8 31.80 30.98 30.86 30.40 11 15 18.8 29.11 28.52 27.76 (Ritzel, Z. Kryst. Min. 1911, 49. 152.) Insol. in anhydrous and in 97% pyridine. Very si. sol. in 95% pyridine+Aa. SI. sol. in 93% pyridine+Aq. (Kahlenberg, J. Am. Chem. Soc. 1908, 30. 1107.) Insol. in oil of turpentine. (T. S. Hunt, Am. J. Sci. (2) 19. 417.) 100 g. H 2 O dissolve 236.3 g. sugar +42.3 g. NaCl at 31.25, or 100 g. sat. aq. solution (Armstrong and Eyre, Proc. R. Soc. 1910, (A) 84. 127.) Min. Halite. +2H 2 O. Efflorescent below '0; si. deli- quescent at temps, above 0. (Fuchs, 1826.) The solubility in H 2 O at 12.25 corre- sponds to 32.9 pts. of NaCl per 100 pts. H 2 O (Matignon, C. R. 1909, 148. 551.) Sodium uranium chloride, 2NaCl, UC1 4 . Non volatile and not hydroscopic. (Mois- san, C. R. 1896, 122. 1089.) Sol. in H 2 O. (Colani, A. ch. 1907, (8) 12. 59.) Sodium uranyl chloride, Na 2 (UO 2 )Cl 4 . As K salt. (Aloy, Bull. Soc. 1899, (3) 21. 264.) Sodium zinc chloride, 2NaCl, ZnCl 2 +3H 2 O. Deliquescent. Easily sol. in H 2 O. (Schind- ler, Mag. Pharm. 36. 48.) Sodium zirconium chloride, 2NaCl, ZrCl 4 . (Paykull.) Sodium chloroiodide, NaCl 4 I+2H 2 O. Easily decomp. by alcohol or ether. (Wells and Wheeler, Sill. Am. J. 143. 42.) Sodium fluoride, NaF. Very si. sol. in cold, and not more abund- antly in boiling H 2 O. (Rose.) 100 pts. H 2 O dissolve 4.78 pts. at 16. (Ber- zelius.) 100 pts. H 2 O dissolve 4 pts. at 15. (Fremy, A. ch. (3) 47. 32.) Sp. gr. of aqueous solutions containing in lOOpts. H 2 O: 1.1081 2.2162 3.3243 pts. NaF. 1.0110 1.0221 1.0333 Sat. solution has sp. gr. 1.0486. (Gerlach, Z. anal. 27. 277.) (Kohler, Z. Ver. Zuckerind, 1897, 47. 447.) Solubility of NaCl in glucose +Aq at 25. Cone. = concentration of glucose +Aq in g. mol. per 1,000 g. H 2 O. Sol. = Solubility in 1,000 g. H 2 O. taming 4.3% NaF. (Mylius and Funk, B. 1897, 30. 1718.) Solubility of NaF in HF+Aq at 21. g. per 1000 g. H 2 O g. per 1000 g. H 2 O Cone. Sol. Molecular solubility HF NaF HF NaF 0.0 10.0 45.8 56.5 41.7 41.4 22.5 22.7 83.8 129.7 596.4 777.4 22.9 23.8 48.8 81.7 0.25 0.50 1.0 361.40 364.15 364.30 369.90 6.18 6.22 6.23 6.32 m;+f P. T? TSQfi 123. 1282.) Easily sol. in liquid HF. (Franklin, Z. anorg. 1905, 46. 2.) SI. sol. in cone. KC 2 H 3 O 2 +Aq. (Strom- eyer.) Almost insol. in alcohol. (Berzelms, Pogg 1. 13.) Insol. in methyl acetate. (Naumann, B 1909, 42. 3790.) SODIUM HYDROXIDE 851 Sodium hydrogen fluoride, NaHF 2 . Rather difficultly sol. in cold, more easily in hot H 2 O. (Berzelius, Pogg. 1. 13.) Sodium tantalum fluoride. See Fluotantalate, sodium. Sodium tin (stannous) fluoride, 2NaF, 3SnF 2 . Sol. in H 2 O. (Wagner, B. 19. 896.) Sodium tin (stannic) fluoride. See Fluostannate, sodium. Sodium tantalum fluoride. See Fluotantalate, sodium. Sodium tellurium fluoride, NaF, TeF 4 . Decomp. by H 2 0. (Berzelius.) Sodium titanium fluoride. See Fluotitanate, sodium. Sodium tungstyl fluoride. See Fluoxytungstate, sodium. Sodium uranium fluoride, NaF, UF 4 (?). Somewhat soluble in H 2 O. (Bolton.) Sodium uranyl fluoride. See Fluoxyuranate, sodium. Sodium vanadium sesgiufluoride. See Fluovanadate, sodium. Sodium zinc fluoride, NaF, ZnF 2 . Sol. in H 2 O. (R. Wagner.) Sodium zirconium fluoride, 5NaF, 2ZrF 4 . See Fluozirconate, sodium. Sodium fluoride vanadium pentoxide. See Fluoxyvanadate, sodium. Sodium hydrazide, NH 2 , NHNa. Decomp. by H 2 O with explosive violence. Decomp. by alcohol. (Schlenk, B. 1915, 48. 670.) Sodium hydride, NaH. Decomp. by H 2 O and by acids. Sol. in fused Na or Na amalgam. Insol. in liquid NH 3 . Insol. in CS 2 , CC1 4 , C 6 H 6 and terebenthene. (Moissan, C. R. 1902, 134. 73.) Na 2 H 4 . Decomp. violently by H 2 O. Sodium hydrosulphide, NaSH. Deliquescent. Sol. in H 2 O and alcohol. +3H 2 O. Difficultly sol. in H 2 O. (Damoi- seau, C. C. 1885. 36.) Sodium hydroxide, NaOH. Very deliquescent. 100 pts. NaOH under a bell jar with H 2 O at 1&-20 absorb 552 pts. in 56 days. (Mulder.) Very sol. in H 2 O with evolution of much heat. Sol. in 0.47 pt. H 2 O. (Bineau, C. R. 41. 509.) Solubility of NaOH in H 2 O. t g. per 100 g. Solid phase Solu- tion H 2 O 7.8 8.0 8.7 Ice 20 16.0 19.1 " 28 19.0 23.5 Ice+NaOH.7H 2 24 22.2 28.5 NaOH.7H 2 O+NaOH.5H 2 17.7 24.5 32.5 NaOH.5H 2 O +NaOH.4H 2 O 29.6 42.0 NaOH.4H 2 O + 5 32.2 47.5 NaOH.4H 2 O +NaOH.3^H 2 O 10 34.0 51.5 NaOH.3J^H 2 O 15.5 38.9 63.53 " f. pt. 5 45.5 83.5 NaOH.3^H 2 O +NaOH.2H 2 O 12 50.7 103.0 NaOH.2H 2 +NaOH.H 2 O 20 52.2 109 NaOH.H 2 30 54.3 119 " 40 56.3 129 * 50 59.2 145 " 60 63.5 174 " 64.3 69.0 222.3 f. pt. 61.8 74.2 288 NaOH.H 2 O+NaOH 80 75.8 313 NaOH (?) 110 78.5 365 14 192 83.9 521 (Pickering, Chem. Soc. 1893, 63. 890; Mylius and Funk, W. A. B. 1900. 3. 450. Calc. by Seidell, Solubilities, 2d Edition, p. 653.) 100 g. sat. NaOH+Aq at 15 contain 46.36 g. NaOH. (de Forcrand, C. R. 149. 1344.) Sp. gr. and b-pt of NaOH -fAq. % Na 2 Sp. gr. B.-pt. &> SP. gr. B.-pt. 4.7 9.0 13.0 16.0 19.0 23.0 26.0 29.0 1.06 .12 .18 .23 .29 .32 .36 .40 100.56 101.11 102 . 78 104 . 44 106.66 108 . 89 112.78 116.66 31.0 34.0 36.8 41.2 46.6 53.8 63.6 77.8 1.44 1.47 1.50 1.56 1.63 1.72 1.85 2.00 120.00 123.89 129.44 137.78 148 . 89 204.44 315.56 red heat. (Dalton.) Sp. gr. of NaOH +Aq at 15. % Na 2 Sp. gr. % Na-20 Sp. gr. % Na 2 O Sp. gr. 0.302 1.0040 10.879 .1630 21 . 154 1.3053 0.601 1.0081 11.484 .1734 21.758 1.3125 1.209 1.0163 12 . 088 .1841 21.894 1.3143 1.813 1 . 0246 12.692 .1948 22.363 1.3198 2.418 1 . 0330 13.297 .2058 22 . 967 1 . 3273 3.022 1.0414 13.901 .2178 23.572 1 . 3349 3.626 1 . 0500 14 . 506 .2280 24 . 176 1.3426 4.231 1.0587 15.110 .2392 24 . 780 1.3505 4.835 1 . 0675 15.714 .2453 25 . 385 1 . 3586 5.440 1 . 0764 16.319 .2515 25.989 1.3668 6.044 1 . 0855 16.923 .2578 26 . 594 1.3751 6.648 1 . 0948 17.528 .2642 27 . 200 1 . 3836 7.253 1 . 1042 18.132 .2708 27 . 802 1.3923 7.857 1.1137 18.730 1 . 2775 28.407 1.4011 8.462 1 . 1233 19.341 1.2843 29.011 1.4101 9.066 1 . 1330 19.954 1.2912 29.616 1.4193 9.670 1 . 1428 20.550 1.2982 30.220 1.4285 10.275 1 . 1528 (Tunnerman, N. J. Pharm. 18. 2.) 852 SODIUM HYDROXIDE Sp. gr. of NaOH +Aq. Sp. gr. of NaOH+Aq at 15 Continued. % Na 2 O Sp. gr. % Na 2 C Sp. gr. % Na 2 O Sp. gr. % NaOH Sp. gr. % NaOH Sp. gr. 2.07 1 . 02 14 . 73 1.16 28 16 30 4.02 1.04 16.73 1.18 29.96 .32 7.66 1.0868 24.81 1.2748 5.89 1.06 18.71 1.20 31.67 .34 8.0 1 . 0909 25.3 1 2800 7.69 9 43 1.08 20.66 1 . 10 22 . 58 1.22 1 24 32.40 .35 33 08 36 8.34 1.0951 25.8 1.2857 11.10 1.12 24.47 1.26 34^41 '.38 8.68 1.0992 26.31 1.2905 12.81 1.14 1 26.33 1.28 9.0 1.1030 26.83 1.2973 9.42 1 . 1077 27.31 1 . 3032 (Richtor.) 9.74 1.1120 27.8 1.3091 Sp. gr. of NaOH+Aq at 15. 10.0 10 ^ 1.1158 1 1 1Q"i 28.31 28 83 1.3151 % Sp. gr. ^ Sp. gr. if % is NaOH % Sp. gr. if % is NfloO Sp. gr. NaOH -LU . J 10.97 11.42 -L . J. JLi/O 1.1250 1 . 1294 29^38 30.0 l!3272 1.3339 11.84 1 . 1339 30 57 1 3395 1 1 .015 1.012 32 1 .450 1.351 12.24 1.1383 31.22 1.3458 2 1 .020 1.023 33 1 .462 1.363 12 '.64 1 . 1423 31.85 1.3521 3 1 .043 1.035 34 1 .475 1.374 13.0 .1474 32.47 1.3585 4 1 .058 1.046 35 1 .488 1.384 13.55 .1520 33.0 1.3642 5 1 .074 1.059 36 1 .500 1.395 13.86 .1566 33.69 1.3714 6 1 .089 1.070 37 1 .515 1.405 14.5 .1631 34.38 1.3780 7 1 104 .081 38 1 .530 1.415 14.75 .1662 35.0 1.3858 8 1 119 .092 39 1 .543 1.426 15.0 .1697 35.65 1.3913 9 1 132 .103 40 1 .558 1.437 15.5 .1755 36.25 1.3981 10 1 145 .115 41 1 .570 1.447 15.91 .1803 36.86 1.4049 11 1 160 .126 42 1 .583 1.456 16.38 .1852 37.47 1.4118 12 1 175 .137 43 1 .597 1.468 16.77 .1901 38.13 1.4187 13 1 190 .148 44 .610 1.478 17.22 .1950 38.8' 1.4267 14 1 203 .159 45 .623 1.488 17.67 .2000 39.39 .4328 15 1 219 .170 46 .637 1.499 17.12 .2050 40.0 .4410 16 1 233 .181 47 .650 .508 18.58 .2101 40.75 .4472 17 1 245 .192 48 .663 .519 19.0 .2148 41.41 .4545 18 1 258 .202 49 .678 .529 19.58 .2202 42.12 .4619 19 1 270 .213 50 .690 .540 20.0 .2250 42.83 .4694 20 1 285 .225 51 .705 .550 20.59 .2308 43.66 .4769 21 1 300 .236 52 .719 .560 21.0 .2361 44.38 .4845 22 1 315 .247 53 .730 .570 21.42 .2414 45.27 .4922 23 1 329 .258 54 .745 .580 22.0 .2462 46.15 .5000 24 1 341 .269 55 .760 .591 22.64 .2522 46.87 1.5079 25 1 355 .279 56 .770 .601 23.15 .2576 47.60 1.5158 26 1 369 1.290 57 .785 .611 23.67 .2632 48. ai 1.5238 27 oo 1 381 oricr 1.300 1O 1 f\ 58 Kf\ .800 01 er .622 OO 24.24 .2687 49.02 1.531 28 29 1 1 395 410 .310 1.321 59 60 .815 .830 .633 .643 Hager, Comm. 1883.) 30 31 1.422 1.438 1.332 1.343 70 1.748 The sp. gr. increases or diminishes for each degree as follows: (Gerlach, Z. anal. 8. 279, calculated from % NaOH Corr. Schiff, A. 107. 300 j 40-50 0.00045 Sp. gr. of NaOH+Aq at 15. 30-39 0.0004 % NaOH Sp. gr. % NaOH Sp. gr. 20-29 10-19 . 0003 0.0002 0.61 0.9 1.0070 1.0105 4.0 4.32 1.0435 1.0473 Hager, Comm. 1883.) 1.0 1 2 1.0107 4.64 1.0511 Sp. gr. of NaOH+Aq at 15. i!e l!oi77 5^29 .0588 % NaOH Sp. gr. % NaOH Sp. gr. 2.0 2.36 1.0213 1.0249 5.58 5.87 .0627 .0667 2.5 1.0280 20 1.2262 2.71 1.0286 6.21 .0706 5 1.0568 25 1 . 2823 3.0 1.0318 6.55 .0746 10 1.1131 30 1 . 3374 3.35 1.0360 6.76 .0787 15 1 . 1790 3.67 1 . 0397 7.31 .0827 (Kohlrausch, W. Ann. 1879.) SODIUM HYDROXIDE 853 Sp. gr of NaOH+Aq at 20 containing 2 mols. NaOH to 100 mols. H 2 O = 1.04712. (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of NaOH-f-Aq at 15. % Na 2 O Sp. gr. % Na 2 O Sp. gr. 5 1.069 25 1.353 10 1.139 30 1.426 15 1.210 35 1.500 20 1.281 (Hager, Adjumenta Varia, Leipsic, 1876.) Sp. gr. of NaOH+Aq at 15. &s Sp. gr. asS Sp. gr. 4 Sp. gr. 0.999180 17 1.188707 34 1.373453 1 .010611 18 1.199783 35 1.383815 2 .021920 19 1.210861 36 1.394092 3 .033109 20 1.221933 37 1.404279 4 .044317 21 1.233062 38 1.414363 5 .055463 22 1.244119 39 1.424353 6 .066602 23 1.255134 40 1.434299 7 .077733 24 1.266092 41 1.444161 8 .088856 25 1.277063 42 1.453929 9 .099969 26 1 . 287990 43 1.463623 10 .111069 27 1.298877 44 1.473249 11 . 122165 28 1.309708 45 1.482850 12 . 133250 29 1.320496 46 1.492406 13 . 144353 30 1.331213 47 1.501927 14 . 155450 31 1.341879 48 1.511412 15 1.166538 32 1.352472 49 1.520868 16 1.177619 33 1.362991 50 1.530282 (Pickering, Phil. Mag. 1894, (5) 37. 373.) Sp. gr. of a N solution of NaOH+Aq at 18/18 = 1.0418. (Loomis, W. Ann. 1896, 60. 550.) Sp. gr. of NaOH+Aq. %NaOH 8.73 3.67 3.82 Sp. gr. 20/20 1.0968 1.0416 1.0464 (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 272.) Sp. gr. of NaOH+Aq at t. H 2 O at 4 = 1. The solutions contained a small amount of Na 2 CO 3 . 60 % NaOH 22.57 20.04 17.04 14.16 10.92 % Na 2 C0 3 0.61 0.48 0.35 0.38 0.36 Sp. gr. .2312 .2026 .1692 .1374 .1020 Sat. NaOH+Aq boils at 215.5. (Grif- fiths.) Sat. NaOH+Aq boils at 310. (Gerlach, Z. anal. 26. 427.) NaOH+Aq of 1.500 sp. gr. contains 36.8% NaOH and boils at 130. B.-pt. of NaOH+Aq containing pts. NaOH to 100 pts. H 2 O. B.-pt. Pts. NaOH B.-pt. Pts. NaOH 105 17 ' 210 425.5 110 30 215 475.5 115 41 220 526.3 120 51 225 583.3- 125 60.1 230 645.2 130 70.1 235 714.3 135 81.1 240 800 140 93.5 245 888.8 145 106.5 250 1000 150 120.4 255 1142.8 155 134.5 260 1333.3 160 150.8 265 1534 165 168.8 270 1739.1 170 187 275 2000 175 208.3 280 2353 180 230 285 2857 185 254.5 290 3571.4 190 281.7 300 4651 . 1 195 312.3 305 6451.6 200 345 310 10526.3 205 380.9 314 22222.2 (Gerlach, Z. anal. 26. 463.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Sp. gr. of Na 2 CO 3 +NaOH+Aq at 11.5. H 2 Oat4 = l. % Na 2 COs % NaOH Sp. gr. 3.845 3.171 2.204 1.642 0.2686 14.10 13.63 12.51 10.17 16.64 1.196 1.182 1.164 1.136 1.186 (Wegscheider and Walter, M. 1905, 26. 693.) Sp. gr. of Na 2 CO 3 +NaOH+Aq at t. H 2 O at4 = l. 60 C % Na 2 CO 3 15.38 13.79 12.10 9.965 9.47 7.69 % NaOH 10.63 9.52 8.29 6.86 6.70 5.22 Sp. gr. 1.2621 .2302 .1952 .1594 .1521 .1158 80 22.81 14.01 0.55 0.42 .2207 .1232 80 C 15.26 9.48 11.14 6.93 .2510 . 1417 (Wegscheider and Walter, M. 1905, 26. 691.) (Wegscheider and Walter, M. 1905, 26. 692.) 854 SODIUM HYDROXIDE Solubility of NaOH+Na 3 SbS 4 at 30. Solubility of NaI+2H 2 O in 100 pts. at t. % NaOH % NasSbS4 Solid phase Pts. ' Pts. Pts. Nal Nal Nal 9.9 27.1 13. Na 3 SbS 4 , 9H 2 O - it - 17 149.4 15 173.7 45 215.6 24.8 5.9 (t -15 150.3 20 178.7 50 227.8 32.9 10.5 u - 5 155.4 25 184.2 55 241.2 42.6 16.4 (( 158.7 30 190.3 60 256.8 47.2 49.5 17.7 9.1 " +NaOH, H 2 O NaOH, H 2 O 5 10 163.6 168.6 35 40 197.0 205.1 65 278.4 54.3 (Coppet, A. ch. (5) 60. 424.) (Donk, Chem. Weekbl. 1908, 6. 529, 629, 767.) Easily sol. in alcohol or wood spirit; sol. in fusel-oil. Sol. in an aqueous solution of mannite. (Favre, A. ch. (3) 11. 76.) Easily sol. in glycerine. Sol. to a certain extent in ether. Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate (Naumann, B. 1904, 37. 3602); benzonitrile. (Naumann, B. 1914, 47. 1370.) +H 2 O. 100 g. solution in H 2 O sat. at 25 contain 42 g. Na 2 O. (Schreinemakers, Arch. Ne'er. Sc. 1910, (2) 16. 81.) Mpt. 64.3. (See above.) +lVsH 2 O. (Cripps, Pharm. J. Trans. (3) 14. 833.) +2H 2 O. See above. +3Y2H 2 O. Deliquescent. Sol. in H 2 O with absorption of much heat. Melts at 6 (Hermes.) Mpt. 15.5. (See above.) +4, 5 and 7H 2 O. (See above.) The composition of the hydrates formed by NaOH at different dilutions is calculated from determinations of the lowering of the fr.-pt. produced by NaOH and of the con- ductivity and sp. gr. of NaOH+Aq. (Jones Am. Ch. J. 1905, 34. 336.) Sodium perhydroxide, NaO 2 H. "Natryl hydroxide." Decomp. by H 2 O. Sol. in cold alcoholic acetic acid. (Tafel, B. 1894, 27. 2300.) Sodium iodide, Nal, and +2H 2 O. Solubility of Nal and of NaI+2H 2 O in H 2 O differ. Below 65, NaI+2H 2 O usually separates out, and above that temp. Nal separates. Solubility of Nal in 100 pts. H 2 C at t. t Pts. Nal t Pts. Nal t Pts. Nal 71.3 74.1 81.6 86.4 294.4 295.3 296.8 298.3 92.4 97.1 101.7 110.7 300.2 300.3 302.5 306.2 124.7 132.5 138.1 317.5 317.3 319:2 Solubility is represented by a straight line of the formula S = 264. 19+0.3978t. If solubility S = pts. Nal in 100 pts, solu- ion, S = 61.3+0.1712t from to 80; S = 75+0.0258t from 80 to 160. (Etard, C. R. 98. 1432.) NaI+2H 2 O is sol. in 0.55 pt. H 2 at 15. Eder, Dingl. 221. 89.) 100 pts. Nal+Aq at 18-19 contain 62.98 pts. Nal. (v. Hauer, J. pr. 98. 137.) 100 pts. H 2 O dissolve at: 20 40 158.7 178.6 208.4 60 256.4 pts. Nal, 80 100 120 140 303 312.5 322.5 333.3 pts. Nal. (Kremers, Pogg. 97. 14.) Transition pt. for NaI+2H 2 9 to Nal is 64.3, and sat. solution containing 74.4% Nal. (Panfilofif, J. Russ. Phys. Chem.* Soc. 1893, 25. 162.) 100 g. H 2 O dissolve 172.4 g. Nal at 15, and sp. gr. of sat. solution = 1.8937. (Greenish, Pharm. J. 1900, 65. 190.) 100 g. solution of NaI+2H 2 O sat. at 30 contains 65.5 g. anhyd. Nal. (Cocheret, Dissert. 1910.) Sp. gr. of Nal+Aq at 19.5 containing: 5 10 15 20 25 30 % Nal, 1.040 1.082 1.128 1.179 1.234 1.294 35 40 45 50 55 60 % Nal. 1.360 1.432 1.510 1.60 1.70 1.81 (Gerlach, Z. anal. 8. 285.) Sat. solution boils at 141. Sol. in liquid SO 2 . (Walden, B. 1899, 32. 2864); POC1 3 . (Walden, Z. anorg. 1900, 25- 212.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Sol. in 12.0 pts. absolute alcohol; in 360 pts. ether. (Eder, Dingl. 221. 89.) Sol. in 3 pts. 90% alcohol. (Hager.) 100 pts. absolute methyl alcohol dissolve 77.7 pts. Nal at 22.5; ethyl alcohol, 43.1 pts. (de Bruyn, Z. phys. Ch. 10. 783.) Very sol. in abs. methyl alcohol and is not pptd. therefrom on the addition of a large volume of abs. ether, while wet ether produces immediate separation. (Loeb, J. Am. Chem. Soc. 1905, 27. 1020.) SODIUM IODIDE 855 Solubility of Nal in ethyl alcohol, (g. Nal in 100 g. alcohol.) Solubility in methyl alcohol + ethyl alcohol at 25. P = % methyl alcohol in the solvent. G = g. Nal in 10 ccm. of the solution. S = Sp. gr. of the sat. solution at 25. t Nal t Nal 10 30 50 80 100 120 160 180 43.77 44.25 44.50 45.0 45.1 45.2 45.0 44.3 200 220 230 240 250 255 260 261.5* 42.3 38.5 36.2 32.7 26.2 21.0 10.8 8.6 p G S 25/4 0.00 4.37 10.40 41.02 80.69 84.77 91.25 100.00 3.515 3.768 3.971 4.598 5.744 5.892 6.110 6.322 1.0806 1.1029 1.1123 1.1742 1.2741 1.2886 1.3056 1.3250 ""Critical temp, of solution. (Tyrer, Chem. Soc. 1910, 97. 626.) (Herz and Kuhn, Z. anorg. 1908, 60. 154.) 100 g. sat. solution of Nal in ethyl alcohol at 30 contains 30.9 g. (Cocheret, Dissert, 1910.) Solubility in mixtures of methyl and propyl alcohol at 25. P = % propyl alcohol in the solvent. G = g. Nal in 10 ccm. of the solution. S=Sp. gr. of the sat. solution. Solubility in ethyl alcohol +Aq at 30. P G S 25/4 6OOO % Nal % alcohol Solid phase 11.11 .322 5.845 .3250 .2853 65.52 Nal, 2H 2 O ( ( 23.8 65.2 5.464 4.071 .2528 .138 64 3.40 ff 91.8 2.914 .0420 54.2 r* A 18.5 1 Q Q (i 93.75 2.649 .0178 54 lo.o oo er fi 100.00 2.411 0.9968 48.8 28.5 42.35 38.5 41.7 53.2 K it (Herz and Kuhn, Z. anorg. 1908, 60. 156.) 37.91 37.49 35.65 54.7 55.37 59.24 (i Nal, 2H 2 0+NaI Nal Solubility in mixtures of propyl and ethy alcohol at 25. 33.24 61.78 a P = % propyl alcohol in the solvent. 30.90 68.70 (l G = g. Nal in 10 ccm. of the solution. S = Sp. gr. of the sat. solution. (Cocheret, Dissert. 1911.) P G S 25/4 3.515 1.0806 At room temp. 1 pt. by weight is sol in: 8.1- 17.85 3.460 3.405 1.0732 1.0720 1.2 pts. methyl alcohol D 15 0.7990. 56.6 2.841 1.0276 1.7 " ethyl " D 15 0.8100. 88.6 2.613 1.0130 3.8 " propyl " D 15 0.8160. 91.2 2.588 1.0104 (Rohland, Z. anorg. 1898, 18. 325.) 95.2 100 2.474 2.411 1.0020 0.9968 100 g. methyl alcohol dissolve 90.35 g. Nal at 25. 100 g. ethyl alcohol dissolve 46.02 g. Nal at 25. 100 g. propyl alcohol dissolve 28.22 g. Nal at 25. 100 g. isoamyl alcohol dissolve 16.30 g. Nal at 25. (Turner and Bissett, Chem. Soc. 1913, 103. 1909.) (Herz and Kuhn, Z. anorg. 1908, 60. 159.) Sol. in normal propyl alcohol. (Loeb, J. Am. Chem. Soc. 1905, 27. 1020.) 28.74 g. are sol. in 100 g. propyl alcohol. (Schlamp, Z. phys. Ch. 1894, 14. 276.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Sol. in ethyl acetate. (Casaseca, C. R. 30. 821.) Insol. in ethyl acetate. (Naumann, B. 1910,43.314.) 856 SODIUM TIN IODIDE SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Solubility in organic solvents at t. C=pts. by wt. of Nal in 100 ccm. of the sat. solution. L=no. of liters which at the saturation temp, hold in solution 1 mol. Nal. Solvent t C L Furfurol 25 25.10 0.597 Acetonitrile it 25 18.43 22.09 0.813 0.679 Propionitrile (t 25 6.230 9.091 2.406 1.649 Nitromethane (( 25 0.478 0.339 31.36 44.27 (Walden, Z. phys. Ch. 1906, 65. 718.) Very sol. in acetone. (Walden.) +5H 2 O. Transition point of NaI+5H 2 O to NaI+2H 2 O is -13.5, and sat. solution contains 60.2% Nal. (Panfiloff, J. Russ. Phys. Chem. Soc. 1893, 25. 162.) Sodium tin (stannous) iodide, Nal, SnI 2 . Very sol. in H 2 O. When treated with little H 2 O, Nal is dissolved out, but a larger amt. of H 2 O dissolves it completely. (Boullay, A. ch. (2) 34. 375.) Sodium zinc iodide, 2NaI, ZnI 2 +3H 2 O. Deliquescent. NaZnI 3 +2H 2 O. Very hydroscopic. (Ephraim, Z. anorg. 1910, 67. 383.) Sodium nitride, Decomp. by heat. (Franz Fisher, B. 1910, 43. 1468.) Sodium sw&oxide, Na 3 O. Decomp. by H 2 O. (de Forcrand, C. R. 1898, 127. 365.) Sodium oxide, Na 2 O. Very deliquescent, and sol. in H 2 O with evolution of heat. See Sodium hydroxide. Sodium peroxide, Na 2 O 2 . Deliquescent, and very sol. in H 2 O with partial decomp. Solution decomp. on boiling. Cryst. with 2H 2 O, and 8H 2 O. (Fairley, Chem. Soc. 1877. 125.) Forms hydrate Na 2 O 2 (OH) 4 +4H 2 O. Easily sol. in H 2 O or dil. acids without decomp. (Schone, A. 193. 241.) Sodium peroxide carbonate, Na 2 CO 4 . Easily decomp. (Woffenstein, B. 1908. 41. 285.) Sodium peroxide decarbonate, Na 2 C 2 O 6 . Easily decomp. (Woffenstein, B. 1908, 41. 287.) Sodium Znoxide, NaO 3 . Sol. in H 2 O forming a solution of Na 2 O 2 . (Joannis, C. R. 1893, 116. 1371.) Sodium fnoxide carbonate, Na 2 CO fi . (Woffenstein, B. 1908, 41. 296.) Sodium trioxide bicarbonate, NaHCO 4 . Two isomeric modifications. (Woffen- stein, B. 1908, 41. 390.) Sodium dioxide hydrate, NaO.OH. See Sodium perhydroxide. Isomeric with Tafel's sodyl hydroxide. OrNa.OH. (B. 27, 2297.) Insol. in alcohol. Very unstable. (Woffenstein, B. 1908, 41. 290.) Sodium phosphide, NaP 5 . Easily decomp. by H 2 O. (Hugot, C. R. 1895, 121. 208.) Sodium hydrogen phosphide, NaH 2 P. Decomp. by H 2 0. (Joannis, C. R. 1894, 119. 558.) Na 3 H 3 P 2 . Decomp. by acids and H 2 O. (Hugot, C. R.,1898, 126. 1721.) Sodium selenide, Na 2 Se. Very deliquescent. Decomp. by H 2 O. (Uelsmann, A. 116. 127.) Insol. in liquid NH 3 ; sol. in air free H 2 O to a colorless liquid. (Hugot, C. R. 1899, 129. 299.) Cryst. with 16H 2 O, 9H 2 O, and 9 /2H 2 O. (Fabre, C. R. 102. 613.) + 10H 2 O. Very sol. in H 2 O; very unstable in the air. (Clever, Z. anorg. 1895, 10. 145.) Sodium diselenide, Na 2 Se 2 . (Jackson, B. 7. 1277.) Sodium tfnselenide, Na 2 Se 3 . Sol. in H 2 O. (Mathewson, J. Am. Chem. Soc. 1907, 29. 873.) Sodium Aeoxiselemde, Na 2 Se. Sol. in H 2 O. (Mathewson, J. Am. Chem. Soc. 1907, 29. 873.) Sodium raonosulphide, Na 2 S. Sol. in H 2 O. Much less sol. in alcohol than in H 2 O. Insol. in ether. (Roussin.) STANNIC ACID 857 +5H 2 0. Tr. pt. from Na 2 S+5^H 2 O, 94. The sat. solution contains: 28.48% anhydrous salt at 50 29.27 29.92 31.38 33.95 37.20 55 60 70 80 90 Labile from 48.9-91.5; stabile from 91.5- 6. (Parravano and Fornaini, C. C. 1908, I. 5.) +6H 2 O. Less efflorescent than with 9H 2 O. Sol. in H 2 O and alcohol. The sat. solution contains: 26 . 7 % anhydrous salt at 50 28.1 " " "60 30.22 " " "70 32.95 " " "80 36.42 " " "90 Tr. pt. to Na 2 S+5MH 2 O, 91.5. (Parravano and Fornaini.) +9H 2 O. Efflorescent. Much less sol. in alcohol than H 2 O. When dissolved in H 2 O, temp, sinks from +22 to 6.1. (Finger, Pogg. 128. 635.) The sat. solution contains: 9.34% anhydrous Na 2 S at 10 13.36 ' ' " +10 14.36 ' ' ' 15 15.30 ' ' ' 18 16.2 ' ' ' 22 17.73 ' ' ' 28 19.09 ' ' ' 32 20.98 ' ' ' 37 24.19 ' ' ' 45 Tr. pt. to Na 2 S+5^H 2 O, 48.9. (Parravano and Fornaini.) Sodium cfo'sulphide, Na 2 S 2 . Sol. in H 2 O and alcohol. +5H 2 O. Not efflorescent. Sodium bisulphide, Na 2 S 3 . Sol. in H 2 O with decomp. Cryst. with 3H 2 O from an alcoholic solu- tion. (BSttger, A. 223. 355.) Sodium tefrasulphide, Na 2 S 4 +6H 2 O. Very deliquescent, and sol. in H 2 O. Diffi- cultly sol. in absolute alcohol. Insol. in ether. (Schone.) +8H 2 O. Efflorescent. (Bottger.) Sodium pentasulphide, Na 2 S 5 +6H 2 O. Sol. in H 2 O. (Schone.) Sol. in alcohol. +8H ? O. (Bottger.) Solution is easily decomp. by warming. (Jones, Chem. Soc. 37. 461.) Sodium tellurium sulphide. See Sulphotellurate, sodium. Sodium stannic sulphide. See Sulphostannate, sodium. Sodium yttrium sulphide, Na 2 S, Y 2 S 3 . Decomp. by dil. acids, even by HC 2 H 3 O 2 + Aq. (Duboin, C. R. 107. 243.) Sodium zinc sulphide, Na 2 S, 3ZnS. Not so stable as the corresponding K salt. (Schneider, J. pr. (2) 8. 29.) Sodium sulphoselenide, Na 2 SSe 2 +5H 2 O. Hydroscopic, and decomp. in the air. (Mes- singer, B. 1897, 30. 806.) Sodium telluride, Na 2 Te. Sol. in H 2 O. (Demarcay, Bull. Soc. (2) 40. 99.) Sodium fritelluride, Na 2 Te 3 . Sol. in H 2 O. Sol. in liquid NH 3 . (Hugot, C. C. 1899, II. 580.) Stannic acid, H 2 SnO 3 . Insol. in H 2 O. Sol. in HC1, and H 2 SO 4 + Aq, even when dil. (Fremy.) Easily sol. in acids, from which solution it may be pptd. by dilution or boiling. While moist it is sol. in HNO 3 +Aq, but gradually separates on stand- ing, and coagulates at once when heated to 50. If NH 4 NO 3 be added to the solution, it remains clear at ord. temp. (Berzelius.) Easily sol. in HNO 3 +Aq, when previously treated with NH 4 OH+Aq. (The'nard.) Easily sol. in KOH+Aq, but addition of large excess ppts. K 2 SnO 3 , insol. in KOH + Aq. Easily sol. in NaOH+Aq, and not pptd. by an excess of that reagent. (Barfoed, J. B. 1867. 267.) SI. sol. in NH 4 OH+Aq or (NH 4 ) 2 CO 3 +Aq. Completely sol. in K 2 CO 3 +Aq, but not in Na 2 CO 3 +Aq. Insol. in alkali hydrogen carbonates or NH 4 Cl+Aq. Sol. in alkali sulphides +Aq. (Berzelius.) Sol. in triethyltoluenyl ammonium hy- drate +Aq. Not pptd. by NH 4 OH+Aq in presence of Na citrate +Aq. SnO 2 , 2H 2 O. (Weber, Pogg. 122. 358.) " a-Orthostannic acid." Easily sol. in HCl+Aq. (Neumann, M. 12. 515.) H 10 Sn50 15 (?) Metastannic acid. Insol. in H 2 O, HNO 3 , or H 2 SO 4 +Aq. Insol. in HCl+Aq, but converted thereby into metastannic chloride, which dissolves after excess of HC1 has been removed. (Fresenius.) Insol. in HCl+Aq of sp. gr. 1.1. (Barfoed.) Sol. in large amount 858 STANNIC ACID of cone. HCl+Aq. (Allen, Chem. Soc. (2) 10. 274.) In contact with HCl+Aq, metastannic acid is converted into stannic acid. (Bar- foed.) Insol. in HNO 3 +Aq even after treatment with NH 4 OH+Aq. Insol. in NH 4 OH+Aq. Sol in KOH or NaOH+Aq with formation of metastannates, which are insol. in dil. NaOH+Aq, but sol. in H 2 O or KOH+Aq, therefore KOH+Aq dissolves metastannic acid, while NaOH+Aq does not, but if the clear solution in KOH+Aq is treated with a large excess of that reagent, a further pptn. occurs. (Barfoed, J. pr. 101. 368.) Insol. in K 2 CO 3 +Aq (Rose); alkali car- bonates +Aq. (Fremy.) Insol. in NH 4 Cl+Aq even after long boil- ing. Sol. in Fe(NO 3 ) 3 +Aq containing HNO 3 . (Lepez and Storch, W. A. B. 98, 2b. 270.) Also in Cr(NO 3 ) 3 +Aq, but not in Ce(NO 3 ) 3 , Al(NOg),, Co(NO 3 ) 2 +Aq, etc. (L. and S.) A colloidal metastannic acid sol. in H 2 O can be obtained. (Lepez and Storch.) According to Weber (Pogg. 122. 358), stannic and metastannic acids are only differ- ent hydrates of same oxide,, and it is not a case of allotropic modification. Colloidal. H 2 SnO 3 in colloidal state can be obtained in aqueous solution containing 5.164 g. SnO 2 in a litre. This solution is coagulated by HNO 3 +Aq only when in great excess; easily by dil. H 2 SO 4 +Aq, but not by cone. HCl+Aq. NH 4 OH+Aq in large excess causes coagulation; also NH 4 C1, NaOH, NaCl, Na 2 S0 4 , etc. (Schneider, Z. anorg. 6. 83.) Pamstannic acid, H 2 Sn 5 On+3H 2 O. (Engel, C. R. 1897, 126. 711.) ' Stannates. Stannates of alkali metals are sol. in H 2 O; others are insol. All metastannates, except- ing Na, K, and NH 4 salts, are insol. in H 2 O. (Fremy, A. ch. (3) 12. 474.) Ammonium stannate, (NH 4 ) 2 O, 2SnO 2 . Sol. in H 2 O. Insol. in dil. NH 4 OH+Aq. (Berzelius.) +zH 2 O. (Moberg, 1838.) Ammonium cupric stannate, (NH 4 ) 2 O, CuSnO 3 +2H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte, C. R. 96. 701.) Barium stannate, BaSnO 3 +6H 2 O. Ppt. Sol. in HCl+Aq. (Moberg.) Ba 2 SnO 4 +10H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte, C. R. 95. 641.) Calcium stannate, CaSnO 3 +4H 2 O. Ppt. (Moberg.) +5H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte, C. R. 96. 701.) 2CaO, SnO 2 . (Zulkowski, Chem. Ind. 1901, 24. 422.) Cobaltous stannate, CoSnO 3 +6H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte.) Cupric stannate, CuSnO 3 +3H 2 O. (Moberg.) +4H 2 O. Insol. in H 2 O. (Ditte.) Cuprous stannous stannate, Cu 2 O, 3SnO, SnO 2 +5H 2 O. Slowly decomp. by dil. acids, and NH 4 OH + Aq; completely decomp. by cone, acids. (Lenssen, J. pr. 79. 90.) Gold (aurous) stannate. See Gold purple. Lead stannate, RbSn(OH) 6 . Ppt. (Bellucci, Chem. Soc. 1905, 88. (2) 40.) Lithium stannate teatungstate, 2Li 2 O, SnO 2 , 6WO 3 = Li 2 SnO 3 , Li 2 W 6 O 19 . Insol. in H 2 O. (Knorre, J. pr. (2) 27. 49.) Magnesium stannate. Ppt. (Moberg.) Manganous stannate. Ppt. (Moberg.) Mercurous stannate, Hg 2 SnO 3 +5H 2 O. Ppt. Mercuric stannate, HgSnO 3 +6H 2 O. Ppt. (Moberg, J. pr. 28. 231.) Nickel stannate, NiSnO 3 +5H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte, C. R. 96. 701.) Platinous sodium stannous stannate, 2PtO, Na 2 O, SnO, SnO 2 (?). (Schneider, Pogg. 136. 105.) Platinous stannous stannate, PtO, 2SnO, SnO 2 . Decomp. by cone, alkalies. (Schneider,) Pogg. 136. 105.) Potassium stannate, K 2 SnO 3 +3H 2 O. 100 pts. H 2 O dissolve 106.6 pts. at 10, solution has sp. gr. = 1.618; 100 pts. dissolve 110.5 pts. at 20, solution has sp. gr. = 1.627. (Ordway, Sill. Am. J. (2) 40. 173.) STRONTIUM AMIDE 859 Very si. sol. in cone. KOH+Aq. Insol. in KCl+Aq. (Fremy.) Insol. in alcohol. Pptd. from aqueous solution by the ad- dition of any soluble salt, especially those of K, Na, and NH 4 (Fremy); by NH 4 C1, but not by KC1 or NaCl (Ordway). Insol. in acetone. (Naumann, B. 1904, 37. 329.) Potassium wetastannate, K 2 O, 10SnO 2 . K 2 O, 7SnO 2 +3H 2 O. Sol. in H 2 O. Solu- tion gelatinises on heating. (Rose.) K 2 O, 6SnO 2 +5H 2 O. Sol. in H 2 O, but loses its solubility by drying. (Fremy, A. ch. (3) 12. 475.) K 2 O, 5Sn0 2 +4H 2 O. Completely sol. in H 2 O. Insol. in alcohol. (Fremy, A. ch. (3) 23. 396.) K 2 O, 3SnO 2 +3H 2 O. Deliquescent. (Fremy.) Silver stannate, Ag 2 SnO 3 . Insol. in H 2 O. Unacted upon by NH 4 OH or HCl+Aq. (Ditte.) Silver (argentous) stannous stannate (?), Ag 4 O, SnO, 3SnO 2 +3H 2 O (?). Cold dil. HNOg+Aq slowly dissolves all Ag, hot HNO 3 +Aq rapidly. Easily sol. in boiling cone. H 2 SO 4 . (Schulze, J. B. 1857. 257.) Sodium stannate, Na 2 SnO 3 +3H 2 O. More easily sol. in cold than in hot H 2 O. (Fremy.) Sol. in 2 pts. H 2 O at 20 and 100. (Mar- ignac.) 100 pts. H 2 O dissolve 67.4 pts. at 0, 61.3 pts. at 20, and solutions have sp. gr. = 1.472 and 1.438 at 15.5. (Ordway, Sill. Am. J. (2) 40. 173.) Pptd. from Na 2 SnO 3 +Aq by salts of K, Na, and NH 4 . Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +4H 2 O. (Prandtl, B. 1907, 40. 2129.) +8H 2 O. (Haeffely, J. B. 1857. 650.) +9H 2 O. (Jones, C. C. 1865. 607.) + 10H 2 O. Very efflorescent. (Scheurer- Kestner, Bull. Soc. (2) 8. 389.) Sodium raetastannate, Na 2 O, 9SnO 2 + 8H 2 O. Sol. in H 2 O. Insol. in NaOH+Aq or alcohol. (Barfoed, J. B. 1867. 267.) Na 2 O, 5SnO 2 . Very difficultly sol. in H 2 O. (Fremy, A. ch. (3) 23. 399.) Insol. in KOH+Aq. +8H 2 O. (Haeffely, Chem. Gaz. 1855. 59.) Sodium stannate vanadate, Na 2 SnO 3 , 3Na 3 VO 4 +32H 2 O. Na 2 SnO 3 , 4Na 3 VO 4 +48H 2 O. Na 2 SnO 3 . 5Na 3 VO 4 +64H 2 O. Na 2 SnO 3 , 6Na 3 VO 4 +80H 2 O. (Prandtl, B. 1907, 40. 2128.) Strontium stannate, 3SrO, 2SnO 2 + 10H 2 O. Ppt. Insol. in H 2 O. Sol. in acids. (Ditte, C. R. 96. 641.) SrSn(OH) 6 . (Belluci, Chem. Soc. 1905, 88 (2) 40.) Tin (stannous) stannate, SnO, 6Sn0 2 +5H 2 O. Insol. in H 2 O. Decomp. by HNO 3 +Aq into metastannic acid. (Schiff, A. 120. 53.) Sol. in HCl+Aq, and in KOH+Aq. Tin (stannous) wetastannate, SnO, 7SnO 2 . SnO, 6SnO 2 +9H 2 O. Sol. in KOH+Aq or in HCl+Aq. (Fremy.) +4H 2 0. (Schiff.) Zinc stannate, ZnSnO 8 +2H 2 O. Ppt. (Moberg, 1838.) 3ZnO,2SnO 2 +10H 2 O. Insol. in H 2 O. Sol. in acids. (Ditte.) Perstannic acid, H 2 Sn 2 O 7 . See Perstannic acid. Stannophosphomolybdic acid. Ammonium stannophosphomolybdate, 3(NH 4 ) 2 O, 4SnO 2 , 3P 2 O 6 , 16MoO 3 + 28H 2 O. Quite insol. even in boiling H 2 O. (Gibbs, Am. Ch. J. 7. 392.) Stannophosphotungstic acid. Ammonium stannophosphotungstate, 2(NH 4 ) 2 O, 2SnO 2 , P 2 O 6 , 22WO 3 + 15H 2 O. Precipitate. SI. sol. in boiling H 2 O. (Gibbs, Am. Ch. J. 7. 319.) Stannosulphuric acid. See Sulphate, stannic. Stibine. See Hydrogen antimonide. Strontium, Sr. Decomp. by H 2 O with violence. Dil. H 2 SO 4 , and HCl+Aq decomp. and dissolve; cold H 2 SO 4 attacks slowly. Fuming HNO 3 has scarcely any action even when boiling. (Franz, J. pr. 107. 253.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Sol. in excess of liquid NH 3 at 60 form- ing Sr(NH 3 ) 6 . (Roederer, C. R. 1905, 140. 1252.) Strontium amalgam, SrHgi 2 . Stable below 30. Above 30 the com- position of the amalgam varies. Can be cryst. from Hg at any temp, below 30. (Kerp, Z. anorg. 1900, 25. 68.) Strontium amide, Sr(NH 2 ) 2 . (Roederer, Bull. Soc. 1906, (3) 36. 715.) 860 STRONTIUM ARSENIDE Strontium arsenide, Sr 3 As 2 . Decomp. by H 2 O. (Lebeau, C. R. 1899, 129. 47.) Strontium azoimide, SrN 6 . Hydroscopic. 45.83 pts. are sol. in 100 pts. H 2 O at 16. 0.095 " " " " 100 " abs. alcohol at 16. Strontium carbide, SrC 2 . Easily decomp. by H 2 O and dil. acids. (Moissan, Bull. Soc. 1894, (3) 11. 1008.) Strontium carbonyl, Sr(CO) 2 . (Roederer, Bull. Soc. 1906, (3) 35. 725.) Strontium chloride, SrCl 2 , and +6H 2 O. Deliquescent in moist air.. Insol. in pure etner. (Uurtms, J. pr. 1898, Sol. in 1.5 pts. HzO at 15, and 0.8 pt. at boiling (2) 58. 287.) (Dumas); in 1.996 pts. H2O at 15 (Gerlach). 1 pt. anhydrous SrCh is sol. in 2.27 pts. EUO at 0; Strontium boride, SrB 6 . Sol. in fused oxidizing agents; not decomp. in 1.88 pts. at 20; in 1.54 pts. at 40; in 1.18 pts. at 60; in 1.08 pts. at 80; in 0.98 pt. at 100. (Kremers, Pogg. 103. 66.) by H 2 O; insol. in aq. acids; si. sol. in cone. H 2 SO; sol. in dil. and cone. HN0 3 . (Moissan, C. R. 1897, 125. 633.) 100 pts. H 2 O dissolve 106.2 pts. SrCl 2 -f 6H 2 O at 0, and 205.8 pts. at 40. (Tilden, Chem. Soc. 45. 409.) Strontium bromide, SrBr 2 , and +6H 2 O. 100 pts. H 2 O dissolve at: Solubility in 100 pts. H 2 O at t 20 38 59 83 110 Pts. Pts. Pts. 87.7 99 112 133 182 250 pts. SrBr 2 . t SrCl 2 t SrCl 2 t SrCh (Kremers, Pogg. 103. 65.) 44.2 41 67.4 81 92.7 Sat. SrBr 2 +Aq contains at: 1 44.5 42 68.2 82 93.1 11 1 +7 18 2 44.8 43 68.9 83 93.4 43.1 46.85 48.2 51.7% SrBr 2 , 3 45.2 44 69.7 84 93.7 - 4 45.6 45 70.4 85 94.1 20 93 97 107 51.8 68.5 68.7 69.8% SrBr 2 . 5 6 46.0 46.5 46 47 71.2 72.0 86 87 94.5 . 94.9 (fitard, A. ch. 1894, (7-) 2. 540.) 7 46.9 48 72.8 88 95.4 Sp. gr. of SrBr 2 +19.5 containing: 5 10 15 20 25 % SrBr 2 , 1.046 1.094 1.146 1.204 1.266 8 9 10 11 47 .4 47.8 48.3 48.8 49 50 51 52 73.6 74.4 75.3 76.1 89 90 91 92 95.8 96.2 96.7 97.2 30 35 40 45 50 % SrBr 2 . 12 49.4 53 77.0 93 97.9 1.332 1.41 1.492 1.59 1.694 13 49.9 54 77.9 94 98.2 (Kremers, Pogg. 99. 444; calculated by Gerlach, Z. anal. 8. 285.) 14 15 50.4 51.0 55 56 78.7 79.6 95 96 98.8 99.4 16 51.5 57 80.4 97 100 Somewhat sol. in absolute alcohol. (Lowig.) Solubility of anhydrous SrBr 2 in alcohol is practically constant between and 40, 100 com. of abs. alcohol dissolving about 64.5 g. of the anhydrous salt and forming a solu- 17 18 19 20 21 52.1 52.7 53.3 53.9 54.5 58 59 60 61 62 81^3 82.2 83.1 84.0 84.9 98 99 100 101 102 103^6 101.3 101.9 102.6 103.3 tion having a sp. gr. = 1.210 at 0. (Fonzes- 22 55.1 63 85.8 . 103 104.0 Diacon, Chem. Soc. 1895, 68 (2) 223.) Much more sol. than BaBr 2 in boiling amyl 23 24 55.7 56.3 64 65 86.6 87.5 104 105 104.7 105.4 alcohol. 25 56.9 66 88.4 106 106 1 Insol. in benzonitrile. (Naumann, B. 1914, 26 57.5 66.5 88.8 107 106^9 47. 1370.) 27 58.1 67 88.9 108 107.6 Difficultly sol. in methyl acetate. (Nau- 28 58.7 68 89.1 109 108.4 mann, B. 1909, 42. 3790.) 29 59.3 69 89.3 110 109.1 Strontium stannic bromide. 30 31 60.0 60 6 70 71 89.6 89.8 111 112 109.9 130.7 See Bromostannate, strontium. 32 6l!3 72 113 111.4 Strontium bromide ammonia, 2SrBr 2 , NH 3 . 33 61.9 73 90^3 114 112.2 Sol. in H 2 O. (Rammelsberg, Pogg. 55. 238. 34 35 62.5 63.2 74 75 90.6 90.9 115 116 113.0 113.8 Strontium bromide hydrazine, SrBr 2 , 3N 2 H 4 . 36 63.9 76 91.2 117 114.6 Very sol. in H 2 O. (Franzen, Z. anorg. 37 64.6 77 91.5 118 115.5 1908, 60. 290.) 38 65.3 78 91.8 118.8 116.4 39 66 70 Q2 1 Strontium bromofluoride, SrF 2 , SrBr 2 . 40 66^7 i \y 80 "^ . J. 92.4 Decomp. by H 2 O. (Defacqz, A. ch. 1904, (8) 1. 356.) (Mulder, Scheik. Verhandel. 1864. 118.) STRONTIUM CHLORIDE 861 100 pts. H 2 O dissolve 52.4 pts. SrCl 2 at 18. (Gerardin.) Sat. SrCl 2 +Aq contains % SrCl 2 at t. Sp. gr. of SrCl 2 +Aq at 18. %SrCl 2 Sp. gr. % SrCh Sp. gr. 5 10 15 1.0443 1.0932 1 . 1456 20 22 1.2023 1.2259 t % SrClj t % SrClz -17 -11 - 5 - 1 + 2 7 18 21.5 35 44.5 54 55 59 64 70 26.5 28.6 29.3 30.8 31.3 31.7 33.7 34.7 37.8 39.8 42.8 43.8 47.7 46.4 46.1 75 80- 92 98 104 105 118 132 144 153 175 215 222 250 46.5 47.1 47.5 49.6 50.7 50.7 52.0 52.5 54.7 55.7 60.5 64.1 65.4 67.3 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of SrCl 2 +Aq at 0. S=pts. SrCl 2 in 100 pts. solution. s Sp. gr. S Sp. gr. 31.8193 27.7170 23.2300 1.3609 1.3086 1.2515 18.2629 12.9997 6.7243 1.1915 1 . 1284 1.0637 (Charpy, A. ch. (6) 29. 24.) Sat. SrCl 2 +Aq boils at 114 (Kremers); 118.8 (Mulder); 117.45, and contains 117.5 pts. SrCl 2 to 100 pts. H 2 O (Legrand) ; forms a crust at 115.5, and contains 120.7 pts. SrCl 2 to 100 pts. H 2 O; highest temp, observed, 119. (Gerlach, Z. anal. 26. 436.) (fitard, A ch. 1894, (7) 2. 535.) SrCh+Aq sat. at 8 has sp. gr. =1.379. (Anthon, A. 24. 211.) Sp. gr. of SrCl 2 +Aq. Pts. SrCh to 100 pts. H 2 O Sp. gr. Pts. SrC! 2 to 100 pts. H 2 O Sp. gr. 9.81 20.12 30.57 1 . 0823 1.1632 1 . 2401 41.04 51.69 1.3114 1.3816 (Kremers, Pogg. 99. 444.) Sp. gr. of SrCl 2 +Aq at 15. % SrCl 2 Sp. gr. % SrCl 2 Sp. gr. 5 10 15 20 1 . 0453 1.0929 1 . 1439 1.1989 25 30 33 1.2580 1.3220 1.3633 (Gerlach, Z. anal. 8. 283.) Sp. gr. of SrCl 2 +Aq at 24.7. a = no. of molecules . . in grms. dissolved in 1,000 g. H 2 O; b = sp. gr. when a = SrC! 2 +6H 2 O, Yz mol. SrCl 2 -|-6H 2 O = 133.5 g.; c = sp. gr. when a = Srd 2 , 1 A mol. =79.5 g. a b c a b c 1 1.063 1.067 7 1.304 1.401 2 1.118 1.130 8 1.330 3 1.166 1.190 9 1.354 . 4 1.207 1.247 10 1.376 . . . 5 1.243 1.301 11 1.396 . . . 6 1.275 1.352 (Favre and Valson, C. R, 79. 968.) B.-pt. of SrCl 2 +Aq containing pts. SrCl 2 to 100 pts. H 2 0. G = according to Gerlach (Z. anal. 26. 442); L = according to Le- grand (A. ch. (2) 69. 436.) B.-pt. G L B.-pt. G L 101 11 16.7 110 71.4 68.9 102 20.5 25^.2 111 76.5 74.1 103 28.9 32.1 112 81.6 79.6 104 36.2 37.9 113 87 85.3 105 43.2 43.4 114 93.1 91.2 106 49.6 48.8 115 99.5 97.5 107 55.4 54.0 116 105.9 104.0 108 60.8 59.0 117 112.3 110.9 109 66.2 63.9 117.5 . Melts in its crystal H 2 O at 112. (Tilden, Chem. Soc. 46. 409.) Sp. gr. of SrCl 2 +Aq at 25. Concentration of SrCl 2 +Aq. Sp. gr. 1-normal Vr- " Vr- " Vr- " 1.0676 1.0336 1.0171 1.0084 (Wagner, Z. phys. Ch. 1890, 6. 40.) SrCl 2 +Aq containing 3.24% SrCl 2 has sp. gr. 20/20 = 1.0284. SrCl 2 +Aq containing 7.08% SrCl 2 has sp. gr. 20/20 = 1.0638. (Le Blanc and Rohland, Z. phys. Ch. 1896> 19. 279.) 862 STRONTIUM THALLIC CHLORIDE Sp. gr. of SrCl 2 +Aq at 20. g. mols. SrCh per 1. Sp. gr. 0.01 .0012284 0.02937 .0038396 0.03987 .0053832 0.05017 .007028 0.07077 .009560 0.10 .013205 0.25 - .034433 0.50 .068379 0.75 . 101760 1.00 . 135423 (Jones and Pearce, Am. Ch. J. 1907, 38. 697.) Cone. HCl+Aq ppts. part of the SrCl 2 from SrCl 2 +Aq. (Hope.) Solubility of SrCl 2 in HCl + Aq at 0. SrCl 2 = Y^ mols. SrCl 2 (in milligrammes) dis- solved in 10 ccm. of liquid; HCl = mols. HC1 (in milligrammes) dissolved in 10 ccm. of liquid. SrCh HCl Sum of mols. Sp. gr. 55 48.2 41.25 30.6 6.1 12.75 23.3 55.0 54.3 54.00 53.9 1.334 1 . 3045 1.2695 1.220 (Engel, Bull. Soc. (2) 45. 655.) Solubility of SrCl 2 in HCl+Aq at 0. Mg. mols. per 10 cc. solution Sp. gr. of solution G. per 100 cc. solution SrCh 2 HCl SrCl* HCl 51.6 44.8 37.85 27.2 22.0 14.0 4.25 6.1 12.75 23.3 28.38 37.25 52.75 .334 .304 .269 .220 .201 .167 .133 40.9 35.5 30.0 21.56 17.44 11.09 3.37 0.0 2.22 4.65 8.49 10.35 13.58 19.23 (Engel, A. ch. 1888, (6) 13. 376.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Sol. in 6 pts. alcohol of 0.833 sp. gr. at 15. (Vau- quelin.) Sol. in 24 pts. absolute alcohol at 15. and in 19 pts. at boiling. (Bucholz.) Sol. in 2.5 pts. of boiling alcohol. Anhydrous SrCl 2 is sol. in 111.6-116.4 pts. alcohol of 99.3% at 14.5, and in 26.2 pts. of the same alcohol at boiling. (Fresenius, A. 69. 127.) 100 pts. alcohol of given sp. gr. at dis- solve pts. SrCl 2 at 18. 0.990 0.985 0.973 0.966 0.953 sp. gr. 49.81 47.0 39.6 35.9 30.4 pts. SrCl 2 , 0.939 26.8 0.909 19.2 0.846 4.9 0.832 sp. gr. 3.2 pts. SrCl 2 . Insol. in absolute alcohol. (Gerardin, A. ch. (4) 6. 156.) 100 pts. absolute methyl alcohol dissolve 63.3 pts. SrCl 2 +6H 2 O at 6; ethyl alcohol, 3.8 pts. (de Bruyn, Z. phys. Ch. 10. 787.) SI. sol. in boiling amyl alcohol. (Browning, Sill. Am. J. 144. 459.) 100 g. 95% formic acid dissolve 23.8 g. SrCl 2 at room temp*. (Aschan, Ch. Ztg. 1913, 37. 1117.) Absolutely insol. in acetic ether. (Cann, C. R. 102. 363.) Very si. sol. in acetone. (Krug and M'Elroy.) Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) SI. sol. in anhydrous pyridine. Sol. in 97%, 95% and 93% pyridine +Aq. (Kahlen- berg, J. Am. Chem. Soc. 1908, 30. 1107.) +2H 2 O. Tr. pt. from +6H 2 O is 61.5. (Richards and Churchill, Z. phys. Ch. 1899, 28. 313.) +6H 2 O. See above. Strontium thallic chloride, SrCl 2 , 2T1C1 3 + 6H 2 O. (Gewecke, A. 1909, 366. 223.) Strontium tin (stannous) chloride, SrCl 2 , SnCl 2 +4H 2 O. Sol. in H 2 O. (Poggiale, C. R. 20. 1183.) Strontium tin (stannic) chloride. See Chlorostannate, strontium. Strontium uranium chloride, SrCl 2 , UC1 4 . Decomp. by H 2 O. (Aloy, Bull. Soc. 1899, (3) 21. 265.) Strontium zinc chloride, SrZnCl 4 +4H 2 O. Very sol. in H 2 O. (Ephraim, Z. anorg. 1910, 67. 380.) Strontium chloride ammonia, SrCl 2 , 8NH 3 . Decomp. by H 2 O. (Rose, Pogg. 20. 155.) Strontium chloride hydrazine, SrCl 2 , 2N 2 H 4 +H 2 0. Hydroscopic. (Franzen, Z. anorg. 1908, 60. 289.) Strontium chloride hydroxylamine, 2SrCl 2 , 5NH 2 OH+2H 2 O. As Ca comp. (Antonow, J. Russ. Phys. Chem. Soc. 1905, 37. 482.) Strontium hydrogen chloride hydroxylamine, 2SrCl 2 , 3HC1, 9NH 2 OH+H 2 O. (Antonow, J. Russ. Phys. Chem. Soc. 1905, 37. 482.) Strontium chlorofluoride, SrF 2 , SrCl 2 . Decomp. by H 2 O, by very dil. HCl, HNO 3 or acetic acid, by hot dil. or cone. H 2 SO 4 . STRONTIUM HYDROXIDE 863 Sol. in cone. HC1 or HNO 3 . Insol. in, and 1 1 It 1 -1 Ill Solubility in Sr(NX) 3 ) 2 +Aq at 25. not decom p. oy co id or Donmg aiconoi. Sp. gr. 25/25 G. SrO as Sr(OH) 2 in 100 g. H 2 O (Defacqz, A. ch. 1904 ,(8)1 . 355.) G. Sr(NO 3 ) 2 in 100 g. H 2 O Strontium fluoride, SrF 2 . Somewhat sol. in H 2 O. (Fr. Roder.) 1.481 0. 79.27 1] .H 2 O dissolves 113.5 mg. SrF 2 at 0.26; * 1.506 1. 76 81.06 117.3 mg. at 17.4: 119.3 mg. at 27.4. 1.490 1. 71 74.27 (Kohlrausch, Z. phys Ch. 1908, 64 168.) 1.450 1. 55 66.88 Insol in HF+Aq. (Berzelius.) 1.419 1. 51 63.71 Boiling HCl+Aq dissolves; si. attacked by 1.403 1. 47 60.37 boiling HNO 3 +Aq; decomp. by hot H 2 SO 4 . 1.381 1. 41 56.30 (Poulenc, C. R. 116. 987.) 1.359 1. 34 52.90 1.327 1. 27 46.97 Strontium stannic fluoride. l!317 1. 20 44^03 See Fluostannate, strontium. 1.291 1. 14 40.83 Strontium titanium fluoride. 1.267 1.239 1.11 1.02 37.81 32.41 See Fluotitanate, strontium. 1.217 i! 01 28^80 Strontium fluoiodide, SrF 2 . SrI 2 . 1.206 0. 96 26.58 Decomp. by cold H 2 O, more rapidly by hot H 2 O. Decomp. by dil. HC1, dil. HNO 3 , dil. H 2 SO 4 or cone. H 2 SO 4 , also by alcohol and by ether, if not absolute. (Defacqz, A. ch. 1904, /O\ 4 O PT> \ 1.178 1.148 1.126 1.108 1.079 00000 95 91 87 84 81 23.83 17.96 16.21 12.78 8.96 (8) 1 ooo.; 1.059 0. 79 6.29 Strontium hydride, SrH. 1.033 0. 78 4.45 Decomp. B. 24. 1976 oy 1 2 U or JHJi-1-Aq. . (Winkler, *Solution is sat. with respect to both sub- SrH 2 . Decomp. by 1902, 134. 100.) H 2 O. (Gautier, C. R. stances. (Parsons and Perkins, J. Am. Chem. Soc. Strontium hydroselenide. 1910, 32. 1388.) Sol. in H 2 O. Sol. in methyl alcohol At room temp. 1 Strontium hydrosulphide, SrS 2 H 2 . Sol. in H 2 O; decomp. by boiling. 1. contains 31.5 g. SrO. (Neuberg and Re- wald, Biochem. Z. 1908, 9. 540.) Insol. in acetone. (Eidmann. C. C. 1899. Strontium hydroxide, SrO 2 H 2 , and +8H 2 O. II. 1014.) Deliquescent. Sol. in an aqueous solution of cane sugar. Sol. in 50 pts. cold, and 2.4 pts. boiling H 2 O (Bu- (Hunton, Phil. Mag. (3) 11. 156.) cholz) : in 50 i 5ts. H 2 O at 15.56 Dalton) ; in 51.4 nts. H 2 O at 15.56, and 2 pts. at 100 (Hope) ; in 52 pts. H 2 O at 15, and 2.4 pts. at 100 (Berzelius) ; in 48 pts. H 2 O j. 1 O TCO / A Ul\ Solubility in H 2 O containing 10 g. sugar at t. at 18.75" (AM). 100 pts. H 2 O at 20 dissolve 1.49 pts. SrO. (Bineau, t g. SrO 2 H 2 +8H 2 O t g. SrO 2 H 2 +8H 2 O C. R. A 1 AOQ 100 pts. aqueous solution of SrO 2 H 2 contain 3 3.10 24 4.79 pts. SrO and pts. SrO 2 H 2 -f8H 2 O at t. 15 3.79 40 9 . 70 Pts. ^ Pts. Pts. Pts. (Sidersky, C. C 1886. 57.) t SrO +8H 2 O t SrO SrO 2 H 2 +8H 2 O _i_, ^TToO 083*5 mn i i a ortl ir. 1 1 TT.n o* 0.35 0.90 55 2.54 6.52 T^< 25. 3-Ll2V/ vs.vsOOO IllOx. 10 OWA, AH J. i. J-JL^V^ c^u (Rothmund, Z. phys. Ch. 1909, 69. 539.) 5 0.41 1.05 60 3.03 7.77 10 15 0.48 57 1.23 1 46 65 70 3.62 4.35 9.29 11 16 Solubility in organic compds. +Aq at 25. 20 0.68 1.74 75 5.30 13^60 Solvent Mol. SrO 2 H 2 +8H 2 O 25 0.82 2.10 80 6.56 16.83 sol. in llitre 30 1.00 2.57 85 9.00 23.09 35 40 45 50 1.22 1.48 1.78 2.13 3.13 3.80 4.57 5.46 90 95 100 12.00 15.15 18.60 30.78 38.86 47.71 water . 5-N methyl alcohol ethyl alcohol propyl alcohol 0.0835 0.0820 0.0744 0.0708 . tert. amyl alcohol 0.0630 (Scheibler, J. pharm. China. 1883, (5) 8. 540.) acetone 0.0692 Sol. in cold NH 4 Cl+Aq. (Rose.) ether 0.0645 864 STRONTIUM IODIDE Solubility in organic compds.+Aq at 25. Continued. Solvent 0.5-N glycol glycerine mannitol urea ammonia diethyl amine pyridine Mol. SrO 2 H 2 +8H 2 O sol. id 1 litre 0.0922 0.1094 0.1996 0.0820 0.0785 0.0586 0.0694 (Rothmund, Z. phys. Ch. 1909, 69. 539.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) See also Strontium oxide. Strontium iodide, SrI 2j and +6, or 7H 2 O. 100 pts. H 2 O dissolve at: 20 40 70 100 164 179 196 250 370 pts. SrI 2 . (Kremers, Pogg. 103. 65.) Sat. aq. solution contains at: 20 10 3 +7 11 18 38 60.0 60.3 62.2 63.0 63.4 63.5 64.8% SrI 2 , 52 63 77 81 97 105 120 175 66.0 68.5 70.5 74.0 79.2 79.4 80.8 85.6% SrI 2 . (Etard, A. ch. 1894, (7) 2. 543.) Sp. gr. of SrI 2 +Aq at 19.5 containing: 5 10 20 30 % SrI 2 ; 1.045 1.091 1.200 1.330 40 50 60 65 % SrI 2 . 1.491 1.695 1.955 2.150 (Kremers, Pogg. 103. 67; calculated by Gerlach, Z. anal. 8. 285.) Sat. solution in abs. ethyl alcohol contains at: 20 +4 39 82 2.6 3.1 4.3 4.7%SrI 2 . (Etard, A. ch. 1894, (7) 2. 565.) Strontium periodide, SrI 3 + 15H 2 O. (Mosnier, A. ch. 1897, (7) 12. 399.) SrI 4 . (Herz and Bulla, Z. anorg. 1911, 71. 255.) Strontium stannous iodide. Very sol. in H 2 O. (Boullay.) Strontium zinc iodide, SrZnI 4 +9H 2 O. Hydroscopic. (Ephraim, Z. anorg. 1910, 67. 385.) Strontium nitride, Sr 2 N 3 . Decomp. H 2 O violently, but not alcohol. (Maquenne, A. ch. (6) 29. 225.) , Strontium oxide, SrO. Decomp. by H 2 O to SrO 2 H 2 , which see. Sol. in 160 pts. H 2 O at 15.56 (Dalton) ; in 50 pts. at 100 (Dalton) ; in 130 pts. at 20 (Bineau) ; in 40 pts. cold, and 20 pts. hot H 2 O (Dumas). Very si. sol. in alcohol. Insol. in ether. 1 1. methyl alcohol dissolves 11.2 g. SrO. (Neuberg and Rewald, Biochem. Z. 1908, 9. 540.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Sol. in cane sugar +Aq. Solubility in H 2 O containing 10 g. sugar at t. 8 15 g. SrO 1.21 1.48 24 40 g. SrO 1.87 3.55 (Sidersky, C. C. 1886. 57.) See also Strontium hydroxide. Strontium peroxide, SrO 2 . SI. sol. in H 2 O. Easily sol. in acids and NH 4 Cl+Aq. Insol. in NH 4 OH+Aq. (Con- roy, Chem. Soc. (2) 11. 812.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Strontium oxybromide, SrBr 2 , SrO+9H 2 O. Not hydroscopic; sol. in H 2 0. (Tassilly, C. R. 1895, 120. 1339.) Strontium oxychloride, SrCl 2 , SrO+9H 2 O. Very easily decomp. by H 2 O and alcohol. (Andre*, A. ch. (6) 3. 76.) Strontium oxyiodide, 2SrI 2 , 5SrO+30H 2 O. Not hydroscopic; sol. in H 2 O. (Tassilly, C. R. 1895, 120. 1339.) Strontium oxysulphide, Sr 2 OS 4 + 12H 2 O. Decomp. by H 2 O. Insol. in alcohol, ether, and CS 2 . (Schone.) Mixture of SrS 2 O 3 and SrS 2 . (Geuther, A. 224. 178.) Strontium phosphide, Sr 3 P 2 . Crystallized. Sol. in dil. acids; insol. in cone, acids; decomp. by H 2 O. Insol. in or- ganic solvents at ord. temp. (Jaboin, C. R. 1899, 129. 764.) Strontium selenide, SrSe. SI. sol. in H 2 O. (Fabre, C. R. 102. 1469.) Strontium silicide, SrSi 2 . Decomp. by H 2 O. (Bradley, C. N. 1900, 82. 150.) SULPHANTIMONATES 865 Strontium sulphide, SrS. Sol. in H 2 O with decomp. into SrO 2 H 2 and SrS 2 H 2 . Insol. in acetone. (Eidmann, C. C. 1899 II. 1014; Naumann, B. 1904, 37. 4329.) Insol. in methyl acetate. (Naumann, B 1909, 42. 3790.) Strontium tetrasulphide, SrS 4 . Very deliquescent, and sol. in H 2 O anc alcohol. Aqueous solution decomp. on air Cryst. with 2, or 6H 2 O. (Schone, Pogg. 117, 58.) Strontium pentasulphide, SrS 5 . Known only in solution. Strontium stannic sulphide. See Sulphostannate, strontium. Sulphaluminic acid. Silver sulphaluminate, 4Ag 2 S, 5A1 2 S ? . (Cambi, Real. Ac. Line. 1912, (5) 21, II. 837.) Sulphamic acid, HOS0 2 NH 2 . See Amidosulphonic acid. Ammonium sulphamate, 2NH 3 , SO 3 . (Woronin.) Is ammonium imidosulphonate, which see. (Berglund.) Ammonium sulphamate, acid, 3NH 3 , 2SO 3 . (Woronin.) Is basic ammonium imidosulphonate, which see. (Berglund.) Barium sulphamate, basic, 2BaO, 3SO 3 , 2NH 3 Somewhat sol. in H 2 O, easily in HCl+Aq. (Jacquelain, A. ch. (3) 8. 304.) BaS 2 O 6 (NH 2 ) 2 . SI. sol. in H 2 O. Decomp. by heating with H 2 O. (Woronin, J. B. 1860. 80.) Is barium imidosulphonate. (Berglund.) Sulphamide, SO 2 (NH 2 ) 2 . Very sol. in H 2 O. (Regnault, A. ch. 69. 170; Mente, A. 248. 267.) Insol. in alcohol, ether, etc. (Traube, B. 26. 607.) Very sol. in H 2 O. SI. sol. in abs. alcohol. SI. sol. in dry ether. (Divers and Ogawa, Chem. Soc. 1902, 81. 504.) Very sol. in liquid NH 3 . (Franklin and Stafford, Am. Ch. J. 1902, 28. 95.) Sol. in alcohol; very sol. in H 2 O. (Hantzsch, B. 1901, 34. 3436.) Silver sulphamide, SO 2 (NHAg) 2 . SI. sol. in cold H 2 O. Sol. in HNO 3 , and (NH 4 ) 2 CO 3 +Aq. (Traube, B. 26. 607.) 3NH 3 , 2SO 3 . (Jacquelain.) Is basic ammonium imidosulphonate, which see. (Berglund.) Sulphamidic acid. (Fremy.) See Imidosulphom'c acid. Sulphaminoplatinous acid. Ammonium tefrasulphaminoplatinite. [Pt(SO 3 NH 2 ) 4 ](NH 4 ) 2 +6H 2 O. SI. sol. in cold H 2 O. (Ramberg, B. 1912, 46. 1512.) Potassium , [Pt(SO 3 NH 2 )4]K 2 +2H 2 O. Very si. sol. in cold H 2 O. (Ramberg.) Sodium . Easily sol. in cold K^O. (Ramberg.) Sulphammonic, and Metasulphammonic acids. (Fremy.) See Nitrilosulphonic acid. Mowosulphammonic acid. (Glaus.) See Amidosulphonic acid. ZH'sulphammonic acid. (Glaus.) See Imidosulphonic acid. Tn'sulphammonic acid. (Glaus.) See Nitrilosulphonic acid. Tetrasulphamm onic acid. (Glaus.) Does not exist. See Nitrilosulphonic acid. Sulphammonium, S(NH 3 ) 2 , 2NH 3 . Sol. in liquid NH 3 . Sol. in abs. alcohol and anhydrous ether. Moissan, C. R. 1901, 132. 517.) Sulphantimonic acid. Sulphantimonates. The alkali sulphantimorrates are sol. in I 2 O, but the solutions decomp. on the air; most of the other sulphantimonates are insol. n H 2 O; all sulphantimonates are insol. in alcohol. (Rammelsberg.) 866 SULPHANTIMONATE, AMMONIUM Ammonium sulphantimonate, (NH 4 ) 3 SbS 4 . Sol. in H ? O. Sol. in dil. acids with decomp. (Stanek, Z. anorg. 1898. 17. 122.) +4H 2 O. (Stanek.) Solubility of (NH 4 )3SbS4+4H 2 O in H 2 O at t. Iron (ferric) sulphantimonate, Fe 2 (SbS 4 ) 2 . (Rammelsberg, Pogg. 62. 234.) Lead sulphantimonate, Pb 3 (SbS 4 ) 2 . Ppt. Decomp. by KOH+Aq. (Rammels- berg, Pogg. 62. 223.) *o % * . (NH4) 3 SbS4 Solid phase Lithium sulphantimonate, Li 3 SbS 4 +8^2H 2 O. 100 g. sat. solution in H 2 O contain 50.8 g. - 1.9 9.9 Ice anhyd. Li 3 SbS 4 . - 5 20.0 8 30 2 (( Solubility in alcohol at 30. -13.5 41.6 41.6 Ice+(NH 4 ) 3 SbS 4 , 4H 2 O (NH 4 ) 3 SbS 4 , 4H 2 O ** alcohol Li 3 SbS 4 Solid phase +20 47 . 7 30 54.5 ii 50.8 LiSbS 4 , 8^H 2 O 13.3 46.3 u (Donk, Chem. Weekbl, 1908, 5. 529.) 51.9 30.7 tl 54.8 29.9 11 Solubility of (NH 4 ) 3 SbS 4 in alcohol at 10. 58.4 KO f\ 30.8 qo q T ' C*1^O Ol /TJT /^V 1 T " w' I >*J ljl3ODio 4 . O7 / 2rl 2 vJ-p-Lil3ODia 4 tt Solid phase, (NH 4 ) 3 SbS 4 +4H 2 O. Oo . O 65.26 o . o 29.31 Li s SbS 4 cr 07 07 gf 74.3 24.1 a C 2 H 6 OH (NH 4 ) 3 SbS4 C 2 H 8 OH '(NH 4 ) 3 SbS4 79.5 20.5 " 43.2 43.1 8.7 (Schreinemakers and Jacobs, Ch. Weekbl. 5.1 35.9 53.1 4.1 1910, 72. 213.) 19.1 23.1 93.3 I rvTT S^i T7" 1 * TT /~\ /T> * 1 (Donk, I. c.) +9H 2 O. Very sol. in H 2 O. (Bnnkmann, Dissert. 1891.) Antimonyl sulphantimonate, (SbO) 3 SbS 4 . Sol. in HC1. (Rammelsberg, Pogg. 1841, +10H 2 O. Solubility of Li 3 SbS 4 +10H 2 O in H 2 O at t. 62. 236.) v7 t Solid phase Barium sulphantimonate, Ba 3 (SbS 4 ) +3H 2 O. 13 L 4 Sol. in H 2 O. Insol. in alcohol. - 1.7 7.1 Ice - 3.2 12.8 (l Barium potassium sulphantimonate , - 5.1 17.5 lt KBaSbS 4 +6H 2 O. -10.8 23.2 11 Easily sol. in H 2 O. Decomp. by acids. (Glatzel, 1911, 72. 100.) Z. anorg. -15.9 -26.2 -42 28.5 35.3 40.4 45.5 a Ice+Li 3 SbS 4 , 10H 2 O Li 3 SbS 4 , 10H 2 O Bismuth sulphantimonate. +10 30 46.9 50.1 ft Ppt. 50 51.3 lt Cadmium sulphantimonate. Ppt. (Rammelsberg, Pogg. 52. 236.) Calcium sulphantimonate, Ca 3 (SbS 4 ) 2 . Partially sol. in H 2 O. Insol. in alcohol. Cobaltous sulphantimonate, Co 3 (SbS 4 ) 2 . Ppt. Decomp. by HCl+Aq. (Rammels- berg, Pogg. 62. 236.) 'Cupric sulphantimonate, Cu 3 (SbS 4 ) 2 . Ppt. (Rammelsberg, Pogg. 62. 226.) Iron (ferrous) sulphantimonate. Ppt. (Donk, Chem. Weekbl. 1908, 5. 629.) At 10, 100 g. sat. Li 3 SbS 4 +10H 2 O in 10.7 % alcohol contain 41.8 g. Li 3 SbS 4 ; 26.2% alcohol, 36.5 g. Li 3 SbS 4 . (Donk, L c.) Magnesium sulphantimonate, Mg 3 (SbO 4 ) 2 . Deliquescent. Sol. in H 2 O. Decomp. by alcohol. Mercurous sulphantimonate, (Hg 2 ) 3 (SbS 4 ) 2 . Ppt. Mercuric sulphantimonate, Hg 3 (SbS 4 ) 2 . Ppt. (Rammelsberg, Pogg. 62. 229.) SULPHANTIMONATE, SODIUM Mercuric sulphantimonate chloride, Hg 3 (SbS 4 ) 2 , 3HgCl 2 , 3HgO. Insol. in acids, except aqua regia. (Ram- melsberg.) Nickel sulphantimonate, Ni 3 (SbS 4 )2. Ppt. Decomp. by hot HCl+Aq. (Ram- melsberg, Pogg. 52. 226.) Potassium sulphantimonate, K 3 SbS 4 . Sol. in H 2 O. Solubility of K R SbS 4 in H 2 O at t. Composition of the liquid layers. Alcohol layer H 2 O layer 7 7 7 C 2 H 5 OH K 3 SbS 4 alcohol KaSbS* 85 1.1 54.7 2.2 3.4 46.9 4.2 3.8 16 27.4 31.1 67.4 49.0 45.6 12.'7 (Donk, I. c.) +4V 2 H 2 O. Deliquescent. Sol. in H 2 O; more sol. than the Na salt. +3, 5, and 6H 2 O. See Donk above. 2K 2 S, Sb 2 S 3 . Decomp. by cold H 2 O. (Ditte, C. R. 102. 168.) K 2 S, 2Sb 2 S 3 +3H 2 O. SI. sol. in H 2 O. (Ditte.) K 2 S, Sb 2 S 3 . Decomp. by H 2 O. (Ditte.) K 2 S, 2Sb 2 S 3 . (Ditte.) Silver sulphantimonate, Ag 3 SbS4. Insol. in H 2 O or acids. Decomp. by KOH +Aq. (Rammelsberg, Pogg. 52. 218.) Sodium sulphantimonate, Na 3 SbS 4 +9H 2 O. (Schlippe's salt.} Sol. in 2.9 pts. H 2 O at 15. Aqueous solution is precipitated by alcohol. (Rammelsberg.) Sol. in 3 pts. cold H 2 O. (van den Corput.) Sol. in 4 pts. cold H 2 O. (Duflos.) Sol. in 1 pt. boiling H 2 O. (Duflos.) Solubility of Na 3 SbS 4 +9H 2 O in H 2 O at t. t % K 3 SbS4 Solid phase - 1.3 - 2.6 - 4 - 7.2 -10.6 -13.5 -18.5 -28.8 -34 -10 - 4.5 +10 30 50 80 9.5 17.1 24.2 35.4 42.9 48.8 52.6 59.6 62 65.5 69.1 75.4 76.2 77.1 77.7 79.2 Ice H (I u i( 11 Ice+K 3 SbS 4 , 6H 2 O K 3 SbS 4 , 6H 2 O u K 3 SbS 4 , 5H 2 O u u K 3 SbS 4 , 3H 2 O u (Donk, Chem. Weekbl. 1908, 5. 529, 629, 767.) Solubility of K 3 SbS 4 in KOH+Aq at 25. % KsSbS4 ' % KOH Solid phase 75 68.4 56.8 50.9 37.7 19.8 11.5 9.4 00.0 3.4 11.0 16.1 25.5 40.5 46.9 49.9 56.3 K 3 SbS 4 , 5H 2 O K 3 SbS 4 , 3H 2 O u K 3 SbS 4 u K 3 SbS 4 +KOH, 2H 2 - KOH, 2H 2 O t0 NalbS, Solid phase - 0.1 0.5 - 0.65 4 - 0.9 5.7 - 1.26 7.8 1.45 9.2 - 1.75 11.2 11.3 15 19.3 30 27.1 38 32 49.6 38.9 59.6 45 ' 69.6 50.7 79.5 57.1 Ice H U tt (( u Na 3 SbS 4 , 9H 2 O tt u n << tt tt tt (Donk.) Solubility of K 3 SbS 4 in alcohoI+Aq at 10. % C 2 H 5 3H K 3 SbS4 Solid phase 94 90.5 0.8* 69^2 76.1 K 3 SbS 4 , 5H 2 O u u (Donk, Chem. Weekbl. 1908, 6. 529 , 629, 767.) * Two liquid layers are formed. SrU'HANTIMO.VVII. THIOSI I. I'll Ml, ^>I)|I \1 .* Holfd Solubility of NatSbS 4 in methyl alcohol at t. S.ll.i |,l,:, < . . - !.. II S 1 '1 o s 1 0.0 4.0 11 27 3 :u ( ; . OH.O 6H,0 r -:< H.SIKS4 in aleohol+Aq at t. s.h.1 phase, Na8b8 4 +OH 2 0. t-O* a. 7 12 7 20. .,(1 S II s s,i (i D t-30* 5 10 :i 21 s 46 76.2 14.6 (i 4 i a o 3 4.7 8 *54.1 g] 47.0 4.1 * Two layers m Composition of above layers. Alcohol layer HiO Uyrr % dflohol % NsiS4 ', :,!<. ,!,<.! % Na8bS4 54.1 10 4 33.5 4.1 10 I 14.1 8.0 14 :; 18.8 27.2 36.5 27. s 24.1 18.0 (l)onk, /. r.) . ! .1! :', 1 i:, r, 2ii I :,o :', 57 81.7 02 d 'OH H i 2 H 2 1 o :< o i o o:, o 2 2.0 IX I :<:', i S<. ,1. in I Ac,; Strontium sulphantimonate. Sol. in H 8 O; pptd. by Uranium sulphantimonate. Ppt. Zinc sulphantimonate, ZnjfSbS^j. Ppt. Sol. in hot NaSbS 4 +Ao: Zn8O 4 -f Aq. Partially sol. in KC sol. in hot HCl+Aq. (Rammelsbei 62. 2 Sulphantimonous acid. Ammonium /////nitc, \H 4 SbS a . In.M.i. n, n,o. Houget, C. R. 1808, 126. 1145.) +2H|O. Insol. in H 2 O and alcoh-.I. Decomp. in the air. (8tand<, X. anorg. is!s, 17. 110.) Ammonium or//?osulphantimonite. decomp. Sl:.l,lc only in of (NH 4 )jS. SoL in H,0. Insol. in alcohol, by which it is pptd. from aqueous solution. , A. ch. 1800, (7) 18. 536.) Ammonium mn/sulphantimonite, Sh 4 S 7 . Stable in the air. Insol. in H,0. Decomp. by acids. (Stanek, Z. anorg. 1808, 17. 120.) Stable; cryst. from hot solutions. C. R. 1808, 126. 1145.) Ammonium silver ^'/.osuJphamimonite, Decamp, by HA (Pouget, A, ch, 1899, +4V.HA JkttoL in HA (Pouget, A, eh. 1899, (7)11, ML) +8HA Decomp, in the air and by HA Son* what soL in BaS+Aq, (Pouget, C, R, 1808, i ////rvfulphantimofiite, 8Hj0, Decamp, by HA Nearly insol. in BaS+Aq, (Rouget.) Barium sulphantimonite, Pptd. from aq. solution of ortho and pyro- barium salts (rouget ) B*8bA,+lHA (Pouget, A, ch, 1899, (7)19,538,) Calcium sulpfaantimonite bane, Ca(OH)8bS,, InoL in HO, 8oL in cone, HCL (Pouget, A, ch, 1899, (7)10,544.) Calcium ^rosolphoantimonite, 8oL in HaO without decamp, (Pouget, C. B. 1898, 126. 1793,) Cobaltous Ppt, (Pouget, A, ch, 1899, (7) 1*, 554,) , CuSbS<, Cuprous 8oL in mixture of HNO* and tartaric acid with separation of 8, Insol, in NHX)H+Aq, Decomp, by hot KOH and alkali sulpUdes+Aq, (Sommer- lad. / UlOfC 180^ 18. 4.-JO., Mm, Wolfgberite. SoL in HNO,+Aq with separation of 8 and Sb*O* Cuprous ^"/o5ulphLajitLm.onite, (Somnieriad, Z, anorg, 1898, Ppt, InsoL in HjO, Decomp, by HjO. (Pouget, A, ch, 1899, (7) 18. 556J Cuprous sulphantimonite, Cu^Bb^r, Min. Guejartie. Cupric /^, 129. JO*.; +3HjO, Fpt., deeamp, by H^), (Pou- get, A, ch, 18%, (7) 18,156,) Iron (ferrous) Ppt, (Pouget, A, ch, 1899, (7) 18, 554,) Mui, HertMehu. 8t sot in Ha+Aq; easily sol. in aqua regia, Lead ^/^fulphflnthnonlte, Pb,(8bS,), Ppt, Very si. sol in HjO, Decomp, by Hi), (Pouget, A, ch, 1899, (7) 18, 553,) Min, tloulfmimte. Comletely sot in hot Ha+Aq; decamp, by SoL in boiling cone, HNO*+Aq, (Pour- net.) Pb(SbS|U Min, Zinekenite. Decomp. by hot Hd~f~Aq, 4PbS, Sb&, Min, PlagionUe. 2PbS|SbjSf. Mm, J&m6it0nU6. Decamp, by hot HOl+Aq, jrjL^I f- a %/Kn \Jl ,ManlvS*tAta 4JnDD> r5Dy5j, J*im, JvlfHWyffinUK. Min. Geokronite. Min, Kfori-Jsenite (7), or//>sulphantimooite, Very sL soL in HjO, Decomp. by HjO, (Pouget, A, ch, 1899, (7) 18. 554,) Lead silver stilpfaantimoiitte, ( Afc, Pb)^b A ,. Min, Very *>1. 71 18. WD.j (Pouget, A, ch. 1899, Ppt, (Pouget, A, ch, 1899, (7) 18. 531,) Decamp, by H^). (Pouget, A. ch, 1899, (7) 18. 551.) Ppt SL soL in HA (Pouget, A, ch 1899, (7) 18. 553.) '-/-'-osuJphantim.onite, SL soL in HA Decomp. by HA (Pou- get, A. ch. 1899, (7) 18. 553,) 870 SULPHANTIMONITE, NICKEL Nickel or^osulphantimonite, Ni 3 Sb 2 S G . Ppt. (Pouget, A. ch. 1899, (7) 18. 554.) Potassium metosulphantimonite, KSbS 2 . Insol. in cold H 2 O. Decomp. by hot H 2 O. (Pouget, A. ch. 1899, (7) 18. 513.) H-l^HaO. Sol. in H 2 O, but decomp. quickly. Sol. in H 2 O. (Stanek, Z. anorg. 1898, 17. 119.) Potassium or^osulphantimonite, K 3 SbS 3 . Very deliquescent. Very sol. in H 2 O. Decomp. by acids. (Pouget, A. ch. 1899, (7) 18. 518.) Potassium sulphantimonite, K 2 Sb 4 S 7 +3H 2 O. SI. sol. in H 2 O and not decomp. thereby. (Pouget, A. ch. 1899, (7) 18. 522.) Decomp. in the air. Sol. in K 2 S+Aq. (Stanek, Z. anorg. 1898, 17. 120.) 2K 2 S, Sb 2 S 3 . Sol. in H 2 O. (Ditte, C. R. 102. 68.) zK 2 S, ?/Sb 2 S 3 . Deliquescent. When K 2 S is in excess, sol. in H 2 O; when Sb 2 S 3 is in ex- cess, partially sol. Aqueous solution is de- comp. by all acids, even CO 2 , and by K 2 CO 3 , Na 2 CQ 3 , NaHCO 3 , KHCO 3 , NH.HCOs+Aq. Insol. in absolute alcohol. (Kohl.) Potassium hydrogen sulphantimonite, KHSb 4 S 7 . (Pouget, A. ch. 1899, (7) 18. 522.) Potassium silver or^osulphantimonite, Ag 2 KSbS 3 . Decomp. by boiling H 2 O. (Pouget, C. R. 1897, 124. 1519.) Potassium zinc or^osulphantimonite, KZnSbS 3 . Decomp. by H 2 O. (Pouget, A. ch. 1899, (7) 18. 552.) Silver or^osulphantimonite, Ag 3 SbS 3 . Ppt. SI. sol. in H 2 O. (Pouget, A. ch. 1899, (7) 18. 547.) Min. Pyrargyrite. Sol. in HNO 3 +Aq with residue of S and Sb 2 O 3 . KOH+Aq dis- solves out Sb 2 S 3 . Silver sulphantimomte. AgSbS 2 . Min. Miargyrite. 5Ag 2 S, Sb 2 S 3 . Min. Stephanite. Easily decomp. by warm HNO 3 -fAq. 12Ag 2 S, Sb 2 S 3 . Min. Polyargyrite. Silver sodium or^osulphantimonite, Ag 2 NaSbS 3 . Decomp. by H 2 O. Pouget, A. ch. 1899, (7) 18. 551.) Sodium wetosulphantimonite, NaSbS 2 . Deliquescent. Decomp. by hot H 2 O. When Na 2 S is in excess, sol. in H 2 O, but partially sol. if Sb 2 S 3 is in excess. (linger, Arch. Pharm. (2) 148. 1.) Ppt. Insol. in H 2 O. (Pouget, C. R. 1898, 126. 1145.) Sodium or^Aosulphantimonite, Na 3 SbS 3 +9H 2 O. Decomp. in solution in H 2 O. (Pouget, C. R. 1898, 126. 1144.) Sodium sulphantimonite, Na 2 Sb 4 S 7 +2H 2 O. Sol. in H 2 O. (Pouget, C. R. 1898, 126. 1145.) Na6Sb 4 S 9 . (Pouget, C. R. 1898, 126. 1144.) 4Na 2 S, 3Sb 2 S 3 +3H 2 O. Permanent; sol. in H 2 O. Insol. in alcohol and ether. (Kohl.) Strontium or^osulphantimonite, Sr 3 Sb 2 S e + 10H 2 O. Sol. in H 2 O. (Pouget, C. R. 1898, 126. 1793.) Strontium py/rosulphantimonite, Sr 2 Sb 2 S 6 +15H 2 O. Sol. in H 2 O without essential decomp. (Pouget, C. R. 1898, 126. 1793.) Zinc orZAosulphantimonite, Zn 3 Sb 2 S 6 . Ppt. (Pouget, A. ch. 1899, (7) 18. 552.) Ori/iosulpharsenic acid, H 3 AsS 4 . Ppt. Loses H 2 S by prolonged boiling with H 2 O. (Nilson, J. pr. (2) 14. 145.) See also Sulphoxyarsenic acid: Ammonium sulpharsenate, (NH 4 ) 4 As 2 S 7 . Known only in solution in H 2 O. Decomp. on boiling into NH^sSs. Sol. in alcohol. (NH 4 ) 3 AsS 4 . Sol. in H 2 O. Precipitated by alcohol. (NH 4 ) 2 S, 12As 2 S5. Ppt. Insol. in H 2 O. Ammonium magnesium sulpharsenate, (NH 4 ) 2 S, MgS, As 2 S 5 . Ammonium sodium sulpharsenate, (NH 4 ) 3 AsS 4 , Na 3 AsS.. Much more sol. in H 2 O than Na 3 AsS 4 ; si. sol. in cold, more sol. in hot alcohol. (Ber- zelius.) Barium sulpharsenate, Ba(AsS 3 ) 2 . Sol. in H 2 O and alcohol. Decomp. by evaporation. Ba 2 As 2 S 7 . Sol. in H 2 O in all proportions with decomp. Decomp. by alcohol. Ba 3 (AsS 4 ) 2 . Sol. in H 2 O. Insol. in alco- hol. BaS, 3As 2 S 5 . Ppt. Insol. in H 2 O. SULPHARSENATE, SODIUM ZINC 871 Barium potassium sulpharsenate, KBaAsS 4 +6H 2 O. Easily sol. in H 2 O. Decomp. by acids with separation of As 2 S 5 . (Glatzel, Z. anorg. 1911, 71. 209.) Barium sulpharsenate sulpharsenite, Ba 3 (AsS 4 ) 2 , Ba 2 As 2 S 5 -f4H 2 O. SI. sol. in cold, more easily in hot H 2 O. (Nilson.) Bismuth sulpharsenate, 2Bi 2 S 3 , 3As 2 S 6 . Sol. in Na 3 AsS 4 +Aq. Bi 2 S 3 , 3As 2 S 5 . As above. (Berzelius.) Cadmium sulpharsenate. Ppt. (Berzelius, Pogg. 7. 88.) Calcium sulpharsenate, Ca 2 As 2 S 7 . Sol. in H 2 O and alcohol. Ca 3 (AsS 4 ) 2 . Easily sol. in H 2 O. Insol. in alcohol. +10H 2 O. Easily sol. in H 2 O. (Nilson, J. pr. (2) 14. 169.) 5CaS, 2AsS 2 S 6 +6H 2 O. Easily sol. in H 2 O. (Nilson,, J. pr. (2) 14. 163.) Cerous sulpharsenate, Ce 2 As 2 S 7 . Ppt. Ce 3 (AsS 4 ) 2 . Ppt. Ce 4 (As 2 S 7 ) 3 . Ppt. Cobaltous sulpharsenate, Co 2 As 2 S 7 . Ppt. Sol. in excess of sodium sulpharsen- ate +Aq. Cuprous sulpharsenate, Cu 3 AsS 4 . Ppt. (Preis, A. 267. 201.) Min. Enargite. Clarite. Not wholly de- comp. by HCl+Aq. Sol. in HCl+Aq with residue of As 2 O 3 . Not attacked by KOH + Aq. Cupric sulpharsenate, Cu 2 As 2 S 7 . Ppt. Sol. in (NH 4 ) 2 S+Aq. Decomp. by NH 4 OH+Aq. (BerzeUus.) Cu 3 (AsS 4 ) 2 . Ppt. (Preis, A. 267. 201.) Glucinum sulpharsenate. SI. sol. in H 2 O. Gold sulpharsenate, AuAsS 4 . Sol. in pure H 2 O. Insol. in NasAsS 4 +Aq. 2Au 2 S 3 , 3As 2 S 5 . Sol. in H 2 O. (Berzelius.) Iron (ferrous) sulpharsenate, Fe 2 As 2 S 7 . Ppt. Sol. in Na;jAsS 4 +Aq. (Berzelius.) Iron (ferric) sulpharsenate, Fe 4 (As 2 S 7 ) 3 . Ppt. Sol. in NasAsS 4 +Aq. (Berzelius.) Lead sulpharsenate, Pb 2 As 2 S 7 . Ppt. (Berzelius.) Pb 3 (AsS 4 ) 2 . Ppt. Lithium sulpharsenate, Li 3 AsS 4 . Easily sol. in hot, less sol. in cold H 2 O. Insol. in alcohol. Li4As 2 S 7 . Comoletely sol. in H 2 O. De- comp. by alcohol. LiAsS 3 . Known only in acid solution. Magnesium sulpharsenate, Mg 2 As 2 S 7 . Sol. in all proportions of H 2 O, and in al- cohol. Mg 3 (AsS 4 ) 2 . Sol. in H 2 O. Decomp. alcohol. 3MgS, As 2 S 5 . Nearly insol. in H 2 O. 5MgS, 2As 2 S 5 -M5H 2 O. Very sol. in H 2 0. (Nilson.) Manganous sulpharsenate, Mn 2 As 2 S 7 . SI. sol. in H 2 O. Mn 3 (AsS 4 ) 2 . Permanent. SI. sol. in H 2 O. 6MnS, As 2 S 5 . SI. sol. in H 2 O. Mercurous sulpharsenate, (Hg 2 ) 2 As 2 S 7 . Ppt. Mercuric sulpharsenate, Hg 2 As 2 S 7 . Ppt. (Berzelius, Pogg. 7. 29.) Hg 3 (AsS 4 ) 2 . Ppt. (Preis, A. 257. 200.) Nickel sulpharsenate, Ni 3 (AsS 4 ) 2 . Ppt. Not decomp. by HCl+Aq. Sol. in Na 3 AsS 4 +Aq. (Berzelius.) 2MS, As 2 * 6 . As above. Potassium sulpharsenate, KAsS 3 . Known only in alcoholic solution. K 4 As 2 S 7 . Deliquescent. Sol. in H 2 0, from which alcohol ppts. K 3 AsS 4 . K 3 AsS 4 . .Deliquescent. Very sol. in H 2 O, from which it is precipitated by alcohol. +H 2 O. Very deliquescent. (ISilson, J. pr. (2) 14. 159.) Potassium sodium sulpharsenate. Sol. hi H 2 O. Silver sulpharsenate, AgsAsS 4 . Ppt. (Berzelius, Pogg. 7. 29.) Ag 2 As 2 S 7 . Ppt. Sodium sulpharsenate, NaAsS 3 . Known only in alcoholic solution. Na^sszS?. Sol. in H 2 0. Alcohol ppts. Na 3 AsS 4 from H 2 O solution. N a3 AsS 4 +7^H 2 O. Easily sol. in H 2 Q, from which it is precipitated by alcohol. +8H 2 O. Insol. in alcohol; very sol. in H 2 O. (McCay, Z. anal. 1895, 34. 726.) +9H 2 O. (Nilson, J. pr. (2) 14. 160.) Na 2 S, 12As 2 S 5 (?). Insol. in H 2 O. Sodium zinc sulpharsenate, NaZnAsS 4 + 4H 2 0. Sol. in hot H 2 O with decomp. (Preis, A. 257. 202.) 872 SULPHARSENATE, STRONTIUM Strontium sulpharsenate, Sr 3 (AsS 4 ) 2 . Easily sol. in H 2 O; insol. in alcohol. Sr 2 As 2 S 7 . Easily sol. in H 2 O, from which alcohol ppts. Sr 3 (AsS 4 ) 2 . Strontium sulpharsenate sulpharsenite, Sr 3 (AsS 4 ) 2 , Sr 2 As 2 S 5 +4H 2 O. Easily sol. in H 2 O. (Nilson, J. pr. (2) 14. 162.) Thallous sulpharsenate, Tl 3 AsS 4 . Not decomp. by H 2 O. Decomp. by dil. acids. Insol. in dil. alkali sulphides. Par- tially decomp. by boiling with a cone, solu- tion of sodium sulphide. (Hawley, J. Am. Chem. Soc. 1907, 29. 1013.) Tin (stannous) sulpharsenate.. Ppt. Tin (stannic) sulpharsenate. Ppt. Uranic sulpharsenate, 2U 2 S 3 , As 2 S 5 . Ppt. Sol. in Na 3 AsS 4 +Aq. Zinc sulpharsenate, Zn 3 (AsS 4 ) 2 . Ppt. (Berzelius.) 2ZnS, As 2 S 5 . Ppt. (Berzelius.) ZnS, As 2 S 5 . (Wohler.) ZH'sulpharsenic acid. See ZKsulphoxyarsenic acid. Sulpharseniosulphomolybdic acid. Ammonium sulpharseniosulphomolybdate, (NH 4 ) 4 As 2 S 7 (MoS 3 ) 2 +5H 2 O. ' Very unstable. Sol. in H 2 O with decomp. (Weinland, Z. anorg. 1897, 16. 49.) Barium , Ba 2 As 2 S 7 (MoS 3 ) 2 +14H 2 O. Sol. in H 2 O with decomp. (Weinland.) Potassium , KAsS 3 (MoS 3 ) +4H 2 O. (Weinland.) K4As 2 S 7 (MoS 3 ) 2 +8H 2 O. Sol. in H 2 O. Decomp. by mineral acids. Insol. in alcohol. (Weinland.) Sodium , NaAsS 3 (MoS 3 )+6H 2 O. Insol. in H 2 O. Easily sol. in dil. NaOH andNH 3 +Aq. (Weinland.) Na 4 As 2 S 7 (MoS 3 ) 2 +14H 2 O. Sol. in H 2 O. Decomp. by mineral acids. (Weinland.) Sulpharseniosulphoxymolybdic acid. Barium sulpharseniosulphoxymolybdate, . Ba 2 As 2 S 7 (Mo 2 S 3 O 3 ) + 12H 2 O. Sol. in H 2 O. (Weinland, Z. anorg. 1897, 16. 60.) Magnesium sulpharseniosulphoxymolybdate, Mg 2 As 2 S 7 (Mo 2 S 3 O 3 ) +16H 2 O. Very sol. in H 2 O. (Weinland.) Potassium , KAsS 3 (MoSO 2 )+2^H 2 O. Sol. in H 2 O with decomp. (Weinland.) K 4 As 2 S 7 (Mo 2 S 3 O 3 )+6H 2 O. Very sol. in H 2 O. Weinland.) +10H 2 O. (Weinland.) Sodium , NaAsS 3 (MoSO 2 )+5H 2 O. SI. sol. in cold, very sol. in hot H 2 O. (Wein- land.) N a4 As 2 S 7 (Mo 2 S 3 O 3 )+15H 2 O. Very sol. inH 2 O. (Weinland.) Sulpharsenious acid. Ammonium sulpharsenite, NH 4 As 3 S 5 +2H 2 O. Insol. in H 2 O. Ppt. Sol. in KOH or NH 4 OH+Aq. SI. attacked by boiling HC1+ Aq. (Nilson, J. pr. (2) 14. 42.) (NH 4 ) 4 As 2 S5 = 2(NH 4 ) 2 S, As 2 S 3 . Sol. in H 2 O, from which alcohol ppts. (NH 4 ) 3 AsS 3 . (NH 4 ) 3 AsS 3 = 3(NH 4 ) 2 S, As 2 S 3 . Decomp. on air; sol. in H 2 O. Insol. in alcohol. (NH 4 ) 5 As 3 S 10 . Sol. in H 2 O. (Nilson, J. pr. (2) 14. 160.) Barium sulpharsenite, Ba 2 As 2 S 5 . SI. sol. in H 2 O. Decomp. by ; +5H 2 O. SI. sol. in H 2 O. (Nilson, J. pr. SI. sol. in H 2 O. Decomp. by alcohol. H 2 0. (2) 14. 46.) +15H 2 O. SI. sol. in cold H 2 O. (Nilson.) Ba 3 (AsS 3 ) 2 . SI. sol. in H 2 O. Precipitated by alcohol. + 14H 2 O. SI. sol. in cold, easily in hot H 2 O. (Nilson.) Ba(AsS 2 ) 2 +2H 2 O. Insol. in H 2 O. (Nil- son, J. pr. (2) 14. 44.) BaAsi 2 Si9. Insol. in HCl+Aq. (Nilson.) Bismuth sulpharsenite, 2Bi 2 S 3 , As 2 S 3 . Ppt. Cadmium sulpharsenite. Ppt. (Berzelius, Pogg. 7. 146.) Calcium sulpharsenite, Ca 2 As 2 S 5 . Sol. in H 2 O, from which alcohol ppts. Ca 3 (AsS 3 ) 2 . Ca 3 (AsS 3 ) 2 . Sol. inH 2 O. + 15H 2 O. Precipitated by alcohol. Ca(AsS 2 ) 2 +10H 2 O. Sol. in H 2 O. (Nilson, J. pr. (2) 14. 54.) CaAs 8 S 13 +10H 2 O (?). Insol. in cold H 2 O. Decomp. by hot H 2 O. (Nilson.) CaAsi 8 S 28 + 10H 2 O (?). SI. sol. in hot H 2 O. (Nilson.) Ca 7 As 2 S 10 +25H 2 O. SI. sol. in cold or hot H 2 O. (Nilson.) Cerous sulpharsenite, Ce 2 As 2 S 6 . Ppt. SULPHARSENITE, URANIC 873 Chromic sulpharsenite, 2Cr 2 S 3 , 3As 2 S 3 . Ppt. Insol. in Na 2 S+Aq. Cobaltous sulpharsenite, 2CoS, As 2 S 3 . Ppt. Sol. in excess of sodium sulpharsen- ite+Aq. Cuprous sulpharsenite, 3Cu 2 S, 2As 2 S 3 = Cu 5 As 4 S 9 . Min. Binnile. Decomp. by hot acids and KOH+Aq. 2Cu 2 S, As 2 S 3 = Cu4As 2 S 5 . Decomp. by acids, KOH and K 2 S+Aq. (Sommerlad, Z. anorg. 1898, 18. 434.) Cupric sulpharsenite, Cu 3 AsS 3 . Insol. in H 2 or HCl+Aq. Sol. in Na 3 AsS 3 +Aq. Cu 2 As 2 S 5 . Ppt. (Berzelius.) Glucinum sulpharsenite, 2G1S, As 2 S 8 . Ppt. Sol. in acids; partly sol. in NH 4 OH +Aq. Gold sulpharsenite, 2Au 2 S 3 , 3As 2 S 3 . Ppt. (Berzelius.) Iron (ferrous) sulpharsenite. Ppt. Sol. in Na 3 AsS 3 +Aq. (Berzelius.) Iron (ferric) sulpharsenite. Ppt. Sol. in excess of a ferric salt, or Na 3 AsS 3 +Aq. (Berzelius.) Lead sulpharsenite, Pb 2 As 2 S 5 . Ppt. Min. Dufreynosite. Pb(AsS 2 ) 2 = PbS, As 2 S 3 . Min. Sartorite. Pb4As 2 S 7 . Min. Jordanite. Lithium sulpharsenites. Resemble K salts. Magnesium sulpharsenite, Mg 2 As 2 S 6 . Almost completely sol. in H 2 O. Easily sol. in alcohol. (Berzelius.) +8H 2 O. SI. sol. in H 2 O. (Nilson.) Mg(AsS 2 ) 2 +5H 2 O. Slowly sol. in both cold and hot H 2 O. (Nilson, J. pr. (2) 14. 59.) Mg 3 (AsS 3 ) 2 +9H 2 O. (Nilson.) Manganous sulpharsenite, Mn 2 As 2 S 6 . Ppt. Decomp. by HCl+Aq. Mercurous sulpharsenite, (Hg 2 ) 2 As 2 S 5 . Ppt. (Berzelius.) Mercuric sulpharsenite, Hg 2 As 2 S 5 . Ppt. Hg(AsS 2 ) 2 . Ppt. (Berzelius, Pogg. 7. 149.) Nickel sulpharsenite, Ni 3 (AsS 3 ) 2 . Ppt. (Berzelius.) Platinum sulpharsenite, Pt 2 As 2 S 5 . Ppt. Potassium sulpharsenite, K 4 As 2 S 5 . Decomp. by H 2 O or alcohol. (Berzelius.) K 3 AsS 3 . Sol. in H 2 O. Insol. in alcohol. (Berzelius.) K 2 As 4 S 7 . Sol. in H 2 O and alcohol. (Ber- zelius.) K 2 AsS 2 . Decomp. by H 2 O. (Berzelius.) +2^H 2 O. Not wholly sol. in H 2 O. (Nil- son, J. pr. (2) 14. 30.) K-As 4 S 3 +8H 2 O. (Nilson.) KAs 3 S 5 +H 2 O. Insol. in H 2 O. Slowly at- tacked by hot HCl+Aq. Sol. in KOH+Aq. (Nilson.) Silver sulpharsenite, 12Ag 2 S, As 2 S 3 . Ppt. (Sommerlad, Z. anorg. 1898, 18. 428.) 5Ag 2 S, As 2 S 3 =Ag 5 AsS 4 . (Sommerlad.) Ag 3 AsS 3 . Min. Proustite. 'Sol. in HNO 3 + Aq. KOH+Aq dissolves out Sb 2 S 3 . (Senar- mont, A. ch. (3) 32. 129; Wohler, A. 27. 159.) 2Ag 2 S, As 2 S 3 . Partially sol. in HNO 3 + Aq. (Berzelius.) AgAsS 2 . (Berzelius, Pogg. 7. 150.) Sodium sulpharsenite, Attacked by HCl+Aq with difficulty. (Nilson, J. pr. (2) 14. 37.) + 1 ^H 2 O. Forms coagulum with cold, sol. in hot H 2 O. (Nilson.) Na 2 As 4 S 7 +6H 2 O. Sol. in much H 2 O; not easily decomp. by HCl+Aq. (Nilson.) NaAs 3 S 5 +4H 2 O. Ppt. (Nilson, J. pr. (2) 14. 3.) Strontium sulpharsenite, 3SrS, As 2 S 3 + 15H 2 O. Sol. in H 2 O+Aq; insol. in alcohol. (Voigt and Gottling.) 2SrS, As 2 S 3 . Sol. in H 2 O; decomp. by alcohol. +15H 2 O. (Nilson, J. pr. (2) 14. 53.) Sr(AsS 2 ) 2 +23/6H 2 O. SI. sol. in H 2 O. (Nil- son.) Thallous sulpharsenite, TlAsS 2 . Ppt. Decomp. by KOH+Aq. (Gunning, J. B. 1868. 247.) Above compound is a mixture of As 2 S 3 and T1 2 S. (Hawley, J. Am. Chem. Soc. 1907, 29. 1012.) Min. Lorandite. (Kuenner and Loezka, C. C. 1904, II. 844.) Tin (stannous) sulpharsenite, Sn 2 As 2 S 5 . Ppt. Tin (stannic) sulpharsenite, SnAs 2 S 6 . Ppt. (Berzelius, Pogg. 7. 147.) Uranic sulpharsenite, 2U 2 S 3 , As 2 S 3 . Ppt. 874 SULPHARSENITE, ZINC Zinc sulpharsenite. Ppt. (Berzelius, Pogg. 7. 145.) Zirconium sulpharsenite, 2Zr 2 S 3 , As 2 S 3 . Ppt. Insol. in solutions of alkali sulph- arsenites. SI. sol. in Na 2 S Aq. Not de- comp. by acids. (Berzelius.) " Sulphatammon," 2NH 3 , SO 3 . (Rose.) Is ammonium imidosulphonate, which see. (Berglund.) "Parasulphatammon," 3NH 3 , 2SO 3 . (Rose.) Is basic ammonium imidosulphonate, which see. (Berglund.) Sulphatoiodic acid. Potassium sulphatoiodate, K 2 H0 3 SIO 4 or KIO,, KHS0 4 . Decomp. by H 2 O. (Blomstrand, J. pr. (2) 40. 317.) See lodate sulphate, potassium. Sulphatooctamine cobaltic carbonate (SO 4 ) 2 Co 2 (NH 3 )8CO 3 +4H 2 O. Sol. in H 2 C. (Vortmann and Blasberg, B. 22. 2650.) (SO 4 )Co 2 (NH 3 ) 8 (C0 3 ) 2 +3H 2 O. Sol. in H 2 O. (V. andB.) See Carbonatotetramine cobaltic sulphate. (Jorgensen.) Sulphatoplatinamine sulphate, S0 4 Pt(NH 3 ) 2 S0 4 +3H 2 0. Easily sol. in H 2 0. Sol. in Sulphatoplatincfo'amine sulphate, SO 4 Pt(N 2 H 6 ) 2 SO 4 +H 2 O. Insol. in H 2 O. Sulphatopurpureocobaltic bromide, Co(SO 4 )(NH 3 )5Br. Sol. in H 2 O, from which it is precipitated by cone. HBr+Aq. (Jorgensen, J. pr. (2) 26. 94.) - carbonate, [(SO 4 )Co(NH 3 ) 6 ] 2 CO 3 + 4H 2 0. Sol. in H 2 O. (Vortmann and Blasberg, B. 22. 2648.) - chloroplatinate, 2Co(SO 4 )(NH 3 ) 6 Cl, PtCl 4 +2H 2 O. SI. sol. in cold H 2 O. (Jorgensen.) - nitrate, Co(SO 4 )(NH 3 ) 6 (NO 8 ). Somewhat si. sol. in cold H 2 O. (Jorgensen.) Sulphatopurpureocobaltic sulphate. [Co(S0 4 )(NH 3 ) 5 ] 2 S0 4 +H 2 0. Very easily sol. in H 2 O. (Jorgensen, J. pr. (2) 26. 94.) Co(S0 4 )NH 3 ) 5 (HS0 4 )+2H 2 0. Sol. in about 25 pts. of cold H 2 O. Sol. in dil., insol. in cone. NH 4 OH-f-Aq. (Jorgensen.) Sulphazic acid, H 4 S 2 N 2 O 9 = SO 3 H N(OH) O N (OH)SO 3 H. Known only in its salts. (Raschig, A. 241. 161.) Potassium sulphazate, K 3 HS 2 N 2 O 9 = (S0 3 K)(OK)N-^0 N(OH) (S0 3 K). Sol. in H 2 O, but decomp. on standing. (Raschig, A. 241. 161.) Sulphazidic acid. (Fremy.) See Hydroxylamine monosulphonic acid. Sulphazilinic acid. See Oxysulphazotic acid. Afetasulphazilinic acid. See Tnsulphoxyazotic acid. Sulphazinous acid. (Fremy.) See Dihydroxylamine sulphonic acid. Sulphazotic acid, H 6 N 2 S 4 Oi 4 = (SO 3 H) 3 =NH NO = OH(SO 3 H). Known only in its salts. (Glaus, A. 158. 52 and 194). Has the formula (S0 3 H) 2 NHNH(S0 3 H) 2 . (Raschig, A. 241. 161.) Lead potassium sulphazotate. Insol. in cold, decomp. by hot H 2 O. Insol. in alcohol and ether. (Fremy, A. ch. (3) 16. 439.) Potassium sulphazotate, K 5 HN 2 S 4 Oi 4 -}-H 2 O = (SO 3 K) 2 NK <> NH(SO 3 K) 2 . Very sol. in hot, less in cold H 2 O. (Ras- ig, A. 241. 161.) Decomp. gradually by boiling. (Glaus.) Insol. in alcohol or ether. (Fremy, A. ch. (3) 16. 428.) True composition is HON(SO 3 K) 2 , KON(SO 3 K) 2 +H 2 O. Potassium hydroxyl- amine disulphonate. (Divers and Haga, Chem. Soc. 1900, 77. 432.) Forms basic salt (SO 3 K) 2 NK<^>NK(SO 3 K) 2 , which is easily sol. and decomp. by H 2 O. (Raschig.) Potassium sodium sulphazotate, K 4 NaHN 2 S 4 O 14 +2H 2 O. Quite easily sol. in H 2 O. (Raschig, A. 241. 161.) SULPHOCHROMIC ACID 875 Disulphhydroxy azotic acid, ONH(SO 2 H) 3 . Known only in its salts. (Glaus, A. 158. 52 and 194.) Correct composition is hydroxy- lamine sulphonic acid HON(SO 3 H) 2 , which see. (Raschig, A. 241. 161.) Sulphhydroxylamic acid. (Glaus.) See Hydroxylamine wonosulphonic acid. Disulphhydroxyazotic acid. (Glaus.) See Hydroxylamine disulphonic acid. Sulphides. The sulphides of the alkali metals are spl. in H 2 O; those of the alkali-earth metals are much less sol., and are decomp. upon solution into hydrosulphide and hydroxide. The other sulphides are insol. in H 2 O. For each sulphide, see under the respective element. Sulphimide,.SO 2 NH. See Imidosulphamide. TYisulphimide, (SO 2 NH) 3 . Sol. in methyl alcohol; si. sol. in ether; insol. in chloroform and benzene. (Hantzsch B. 1901, 34. 3440.) Ammonium sulphimide, SO 2 N(NH 4 ). Sol. in H 2 O; insol. in alcohol. (Traube.) Barium , (SO 2 N) 2 Ba+2H 2 O. Sol. in H 2 O. (Traube.) Potassium , SO 2 NK. Not very sol. in H 2 O. Silver , SO 2 NAg. Sol. in 500-600 pts. cold, more easily in hot H 2 O. Sol. in acids. Sodium , SO 2 NNa. Ver}' sol. in H 2 O. " Sulphitammon," NH 3 , SO 2 . See Thionamic acid. Sulphobismuthous acid. Cuprous sulphobismuthite, AuBiS 2 . Min. Emplectite. Sol. in HNO 3 +Aq. Cu 6 Bi 4 S 9 . Min. Klaprothite. Completely sol.inHCl+Aq. Cu 3 BiS 3 . Min. Wittichenite. Sol. in HC1 -f Aq and in HNO 3 +Aq. Cuprous lead sulphobismuthite, Cu 2 S, 2PbS, Bi 2 S 3 . Min. Patrinite. Sol. in HNOs+Aq with residue of S and PbSO 4 . Lead , 2PbS, Bi 2 S 3 . Min. Cosalite. 2PbS, 3Bi 2 S 3 . Min. Chiviatite. Potassium , KBiS. Decomp. by H 2 O. Sol. in HCl+Aq. (Schneider, Pogg. 1869, 136. 464.) Metasulphoboric acid, B 2 S 3 H 2 S. Decomp. by H 2 O and alcohol. 1 pt. is sol. in 5 pts. benzene 1 pt. is " " 5 " CS 2 Very si. sol. in CS 2 at -20. (Stock, B. 1901, 34. 401.) Sulphocarbonic acid. Ammonium cuprous sulphocarbonate, CS 3 CuNH 4 . This salt was formerly described as cupric sulphocarbonate ammonia, CS 3 Cu, NH 3 . (Hofmann, B. 1903, 36. 1146.) Cuprous potassium sulphocarbonate, CS 3 CuK. Nearly insol. in cold H 2 O. Somewhat sol. in hot H 2 O, NaOH and NH 4 OH+Aq. (Hofmann.) Cupric sulphocarbonate ammonia, CS 3 Cu, NH 3 . Very si. sol. in strong NH 4 OH+Aq.; insol. in cold H 2 O, si. sol. in hot H 2 O. (Hofmann, Z. anorg. 1897, 14. 295.) Is ammonium cuprous sulphocarbonate. (Hofmann, B. 1903, 36. 1146.) Cuprous sulphocarbonate potassium cyanide, CS 3 Cu 2 , 2KCN+2H 2 O. Sol. in H 2 O and dil. alkalies on warming. (Hofmann, B. 1903, 36. 1148.) Zinc sulphocarbonate ammonia, CS 3 Zn, 2NH 3 . Ppt. (Hofmann, Z. anorg. 1897, 14. 277.) Sulphochromic acid, H 2 CrO 4 , SO 3 . (?). Sol. in H 2 O. (Bolley, A. 66. 113.) (SO 3 ) 4 Cr 2 O 2 (OH) 2 . Sol. in H 2 O. All salts iven alkali salts are insol. in H 2 O. (Recoura, Bull. Soc. 1896, (3) 15. 315.) [Cr 2 O 2 (OH) 4 (SO 2 ) 4 O 3 , Cr 2 O(OH) 2 (SO 2 ) 3 (OH)>](OH) 2 . Sol. in H 2 O. (Wyrouboff, Bull. Soc. 1902, (3) 27. 721.) 876 SULPHOCHROMATE, CHROMIUM Chromium sulphochromate, Cr 2 O 2 (OH)4(SO 2 ) 4 O 2 (OH) 2 Cr 2 (OH) 6 . Ppt.; decomp. by boiling H 2 O. (Wyrou- boff, Bull. Soc. 1902, (3) 27. 720.) Sulphochromous acid. Ferrous sulphochromite, FeCr 2 S 4 . Insol. in H 2 O, and nearly so in HCl+Aq. (Groger, W. A. B. 81, 2. 531.) Manganous , MnCr 2 S 4 . Insol. in H 2 O and HCl+Aq. (Groger.) Potassium -, K 2 Cr 2 S 4 . Insol. in H 2 O and in hot HCl+Aq. Easily sol. in aqua regia . Slowly sol. in cold, rapidly sol. in hot dil. HNO 3 +Aq. (Milbauer, Z. anorg. 1904, 42. 443.) K 2 Cr 4 S 7 . Stable in the air; sol. in HNO 3 and aqua regia with decomp. (Schneider, J. pr. 1897, (3) 66. 407.) Silver , Ag 2 Cr 2 S 4 . Not attacked by HCl+Aq even on heat- ing. Decomp. by cone. HN0 3 . (Schneider, J. pr. 1897, (2) 66. 401.) Sodium , Na 2 Cr 2 S 4 . Insol. in H 2 O. SI. attacked by dil. HC1 or H 2 SO 4 +Aq. Sol. in cold cone. HNO 3 or aqua regia. Sol. in hot dil. HNO 3 +Aq. (Groger.) Sol. in acids with decomp. (Schneider, J. pr. 1897, (3) 56. 415.) Zinc , ZnCr 2 S 4 . Insol. in H 2 O: sol. in traces in boiling cone. HC1 or dil. H 2 SO 4 +Aq; sol. in HNO 3 +Aq (Groger, W. A. B. 81, 2. 531.) Sulphocyanhydric acid, HSCN. Sol. in H 2 O. Sat. HSCN+Aq hag sp. gr. = 1.022. (Por- rett, 1814.) HSCN+Aq containing 12.7% HSCN has sp. gr. 1.040 at 12.7. (Hermes Z. Ch. 1866. 417.) Sulphocyanides. Most sulphocyanides are sol. in H 2 O, bu1 Cu, Pb, Hg, and Ag sulphocyanides are insol Aluminum sulphocyanide, A1(SCN) 3 . Known only in solution. A1(SCN) 2 (OH) 4 . Known only in solution (Suida.) Aluminum potassium sulphocyanide, K 3 Al(SCN) e +4H 2 O. Very hydroscopic. Sol. in H 2 O and alcohol. (Rosenheim, Z anorg. 1901, 27. 302.) Ammonium sulphocyanide, NH 4 SCN. Deliquescent, and very sol. in H 2 O. 100 pts. H 2 O dissolve 128.1 pts. at and 162.2 pts. at 20. NH 4 SCN+Aq sat. at ord. temp, has density of 1.138 and 100 cc. contains 69.16 g. NH 4 SCN. (Klason, J. pr. 1887, (2) 36. 67.) By dissolving 90 g. NH 4 SCN in 90 g. H 2 O at 17, the temp, falls to 12. (Clowes, Z. 3h. 1866. 190.) 133 pts. NH 4 SCN+100 pts. H 2 O at 13.2 .ower the temp. 31.2. (Riidorff, B. 2. 68.) Sol. in liquid SO 2 . (Walden, B. 1899, 32. 2864.) Difficultly sol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.) Very easily sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) Easily sol. in alcohol. Easily sol. in acetone. (Krug and M'Elrpy. SI. sol. in benzonitrile. (Naumann, B: 1914, 47. 1369.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Difficultly sol. in ethyl acetate. (Nau- mann, B. 1910, 43. 314.) Ammonium bismuth sulphocyanide, (NH 4 ) 3 Bi(SCN) 3 . As*K salt. (Rosenheim and Vogelgesang Z. anorg. 1906, 48. 215.) Ammonium cadmium sulphocyanide, (NH 4 ) 2 Cd(SCN) 4 +2H 2 O. Somewhat deliquescent. , Melts in crystal H 2 O at 25. Insol. in alcohol. (Grossmann, B. 1902, 35. 2667.) Ammonium cadmium molybdenyl sulpho- cyanide, NH 4 SCN, Cd(SCN) 2 , Mo(OH)(SCN) 3 +3H 2 O. (Maas and Sand, B. 1908, 41. 1513.) Ammonium cobaltous sulphocyanide, (NH 4 ) 2 Co(SCN) 4 . Decomp. in moist air. Cannot be recryst. from H 2 O. (Treadwell, Z. anorg. 1901, 26. 109.) +4H 2 O. Sol. in H 2 O. Sol. in methyl, ethyl and amyl alcohol, in acetone and in ether + Aq. Can be recryst. from H 2 O or alcohol with- out decomp. (Rosenheim and Cohn, Z. anorg. 1901, 27. 289.) Ammonium iron (ferric) sulphocyanide, 9NH 4 SCN, Fe(SCN) 3 +4H 2 O. Deliquescent, and sol. in H 2 O. (Kriiss and Moraht, A. 260. 207.) 3NH 4 SCN, Fe(SCN) 3 . Extremely deli- quescent. Ammonium mercuric sulphocyanide, 2NH 4 SCN, Hg(SCN) 2 . Easily sol. in H 2 O. (Fleischer, A. 179. 228.) SULPHOCYANIDE, BISMUTH 877 NH 4 Hg(SCN) 3 . Insol. in cold; sol. in hot H 2 O. (Rosenheim, Z. anorg. 1901, 27. 284.) Ammonium molybdenyl sulphocyanide, 3NH 4 SCN, Mo(OH)(SCN) 3 +3H 2 O. (Sand and Maas, B. 1907, 40. 4507.) Ammonium nickel sulphocyanide, (NH 4 ) 4 Ni(SCN) 6 +4H 2 O. Sol. in H 2 O with decomp. SI. sol. in cold; easily sol. in hot alcohol. (Rosenheim, Z. anorg. 1901, 27. 292.) Ammonium silver sulphocyanide, NH 4 SCN, AgSCN. Decomp. by H 2 O. Ammonium vanadium sulphocyanide, V(SCN) 3 , 3NH 4 SCN+4H 2 O. Sol. in H 2 O; sol. in alcohol; si. sol. in ether. (Ciocci, Z. anorg. 1898, 19. 311.) Ammonium vanadyl sulphocyanide, (NH 4 ) 2 VO(SCN) 4 +5H 2 O. Sol. in H 2 O, alcohol, ether, acetone, amyl alcohol and ethyl acetate. (Koppel, Z. anorg. 1903, 36. 290.) Ammonium zinc sulphocyanide, (NH 4 ) 2 Zn(SCN) 4 +3H 2 O. Easily sol. in H 2 O and in alcohol. (Walden, Z. anorg. 1900, 23. 374.) +4H 2 O. Easily sol. in cold H 2 O, acetone, alcohols and ether. (Rosenheim and Huld- schinsky, B. 1901, 34. 3913.) Ammonium sulphocyanide mercuric bromide, NH 4 SCN, HgBr 2 . Very sol. in H 2 O. Sol. in alcohol. (Grossmann, B. 1902, 35. 2945.) 2NH 4 SCN, HgBr 2 +H 2 O. Somewhat de- liquescent. Very sol. in H 2 O. Sol. in alcohol. (Grossmann.) Arsenic sulphocyanide, As(SCN) 3 . Decomp. by H 2 O. Insol. in all ordinary solvents. (Miguel, A. ch. (5) 11. 341.) Barium sulphocyanide, Ba(SCN) 2 +2H 2 O. Deliquescent. Easily sol. in H 2 O and alcohol. Boiling solution in alcohol contains 32.8% anhydrous salt. Solution sat. at 20' contains 30%. (Tscherniak, B. 16. 349.) Cryst. with 3H 2 O. (Tscherniak, B. 25. 2627.) Barium cadmium sulphocyanide, 4Ba(SCN) 2 , Cd(SCN) 2 +10H 2 O. Deliquescent. (Grossmann. B. 1902, 36 2669.) Barium caesium cuprous sulphocyanide, Ba(SCN) 2 , 3CsSCN, 2CuSCN. Rapidly decomp. by H 2 O. (Wells, Am. Ch. J. 1902, 28. 273.) Barium caesium silver sulphocyanide, Ba(SCN) 2 , 3CsSCN, 2AgSCN. 100 pts. H 2 O dissolve 92 pts. at 19. Decomp. by much H 2 O. (Wells, Am. Ch. J. 1902, 28. 272.) Barium cobaltous sulphocyanide, BaCo(SCN) 4 +8H 2 O. 290 Ppt. (Rosenheim, Z. anorg. 1901, 27. 0.) Barium mercuric sulphocyanide. BaHg(SCN) 4 . Very sol. in H 2 O and in alcohol. (Rosen- heim, Z. anorg. 1901, 27. 286.) BaHg(SCN) 3 J 2 +2H 2 O. Ppt. Nearly in- sol. in cold; easily sol. in hot H 2 O. (Rosen- heim.) Barium potassium silver sulphocyanide, Ba(SCN) 2 , 4KSCN, 2AgSCN+H 2 O. Very sol. in a little H 2 O. Decomp. by much H 2 O. (Wells, Am. Ch. J. 1902, 28. 283.) Barium rubidium silver sulphocyanide, . BaRb 2 Ag 2 (SCN) 6 +2H 2 O. Very sol. in H 2 O. (Wells, Am. Ch. J. 1903, 30. 186.) BaRb 4 Ag 2 (SCN) 8 +H 2 0. Sol. in H 2 0. (Wells.) Barium silver sulphocyanide, Ba(SCN) 2 , 2AgSC.N +2H 2 O. Stable in the air. (Wells, Am. Ch. J. 1902, 28. 269.) Barium zinc sulphocyanide, BaZn(SCN) 4 +3H 2 O. Easily sol. in alcohol. (Walden, Z. anorg. 1900, 23. 374.) Barium sulphocyanide mercuric bromide. Ba(SCN) 2 , 2HgBr 2 +5H 2 0. Very sol. in H 2 O. (Grossmann, Z. anorg. 1903, 37. 420.) Bismuth sulphocyanide, basic, Bi(OH)(SCN) 2 +5H 2 0. (Rosenheim and Vogelgesang, Z. anorg. 1906, 48. 214.) Bi(SCN) 3 , 2Bi 2 O 3 . Insol. in H 2 O, but when recently pptd. decomp. by boiling therewith. Insol. in HSCN+Aq. (Meitzen- dorf.) Bismuth sulphocyanide, Bi(SCN) 3 . Insol. or si. sol. in H 2 O. Sol. in HNO 8 , HC1, and HSCN+Aq. (Meitzendorf, Pogg. 56. 83.) 878 SULPHOCYANIDE, BISMUTH POTASSIUM Decomp. by cold H 2 O. (Bender, B. 20 723.) + 14H 2 O. Extremely deliquescent. Decomp. by H 2 O. (Rosenheim and Vogel- gesang, Z. anorg. 1906, 48. 214.) Bismuth potassium sulphocyanide, K 3 Bi(SCN) 6 . Decomp. by H 2 O. (Rosenheim and Vogel- gesang, Z. anorg. 1906, 48. 215.) Not hydroscopic. Decomp. by H 2 O. Easily sol. in alcohol. (Vanino, Z. anorg. 1901, 28. 220.) BiCSCN),. 9KSCN. Very hydroscopic. Decomp. by H 2 O. Sol. in alcohol. (Vanino, Z. anorg. 1901, 28. 221.) Bismuth sodium sulphocyanide, Na 3 Bi(SCN) 6 . As K salt. (Rosenheim and Vogelgesang, Z. anorg. 1906, 48. 215.) Boron sulphocyanide, B(SCN) 3 . Sol. in benzene and ether. (Cocksedge, Chem. Soc. 1908, (2) 93. 217.) Cadmium sulphocyanide, Cd(SCN) 2 . SI. sol. in H 2 O. Sol. in NH 4 OH+Aq with combination. Cadmium caesium sulphocyanide, CsCd(SCN) 3 . Recryst. from H 2 O. (Wells, Am. Ch. J. 1903, 30. 148.) Cs 4 Cd(SCN) 6 +2H 2 0. Very sol. in H 2 O. Can be recryst. from cone, solution but de- comp. on dilution to CsCd(SCN) 3 . (Wells.) Cadmium caesium silver sulphocyanide, Cs 2 CdAg 2 (SCN) 6 . (Wells.) +2H 2 0. (Wells.) Cs 2 CdAg 4 (SCN) 8 +2H 2 O. (Wells.) Cs 4 Cd 3 A g ,o(SCN) 20 +6H 2 O. (Wells.) Cadmium mercuric sulphocyanide, Cd(SCN) 2 , Hg(SCN) 2 . Very sol. in hot H 2 O. (Grossmann, Z. anorg. 1903, 37. 414.) Cadmium molybdenum sulphocyanide, Cd(SCN) 2 , Mo(SCN) 4 +2H 2 O. (Maas and Sand, B. 1908, 41. 1513.) +3H 2 O. (Maas and Sand.) Cadmium molybdenyl potassium sulpho- cyanide, KSCN, 4Cd(SCN) 2 , 3Mo(OH)(SCN) 3 +18H 2 O. (Mass and Sand, B. 1908, 41. 1513.) Cadmium molybdenyl sulphocyanide am- monia, 3Cd(SCN) 2 , 2Mo(OH)(SCN) 3 , 13NH 3 . (Mass and Sand, B. 1908, 41. 1512.) +2H 2 O. (Maas and Sand.) Cadmium potassium sulphocyanide, K 2 Cd(SCN) 4 +2H 2 O. Very sol. in H 2 O. (Grossmann, B. 1902, 36. 2668.) Cadmium rubidium sulphocyanide, Rb 2 Cd(SCN) 4 +2H 2 O. Very sol. in H 2 O. (Grossmann, B. 1902, 35. 2668.) Cadmium sodium sulphocyanide, NaCd(SCN) 3 +3H 2 O. (Grossmann, B. 1902, 36. 2668.) Cadmium sulphocyanide ammonia, Cd(SCN) 2 , NH 3 . Decomp. by H 2 O. (Grossmann, B. 1902, 35. 2666.) Cd(SCN) 2 , 2NH 3 . Decomp. by pure H 2 O. (Grossmann.) Cadmium sulphocyanide ammonium bromide, Cd(SCN) 2 , NH 4 Br+H 2 O. Can be recryst. from H 2 O. Decomp. in dil. solution. (Grossmann, Z. anorg. 1903, 37. 425.) Cd(SCN) 2 , 2NH 4 Br. Easily splits off NH 4 Br. (Grossmann.) Cadmium sulphocyanide ammonium chloride, Cd(SCN) 2 , 2NH 4 C1. Can be recryst from H 2 O. Decomp. in dil. solution. (Grossmann, Z. anorg. 1903, 37. 423.) Cadmium sulphocyanide potassium bromide, Cd(SCN) 2 , KBr+H 2 O. Recryst. from H 2 O. (Grossmann, Z. anorg. 1903, 37. 425.) Cd(SCN) 2 , 2KBr. Recryst. from H 2 O. (Grossmann.) Cadmium sulphocyanide potassium chloride, Cd(SCN) 2 , 2KC1. Recryst. from H 2 O. Decomp. in dil. solu- tion. (Grossmann, Z. anorg. 1903, 37. 423.) phocyank Cd(SCN) 2 , 2KI. Recryst. from H 2 O. (Grossmann.) Caesium calcium silver sulphocyanide, 2CsSCN, Ca(SCN) 2 , 2AgSCN+2H 2 O. Recryst. from H 2 O. (Wells, Am. Ch. J. 1902, 28. 275.) SULPHOCYANIDE, COBALTOUS MERCURIC 879 Caesium chromium sulphocyanide. See Chromisulphocyanide, caesium. Caesium cobaltous sulphocyanide, Cs 2 Co(SCN)4+2H 2 O. Stable in the air. (Shinn and Wells, Am. Ch. J. 1903, 29. 476.) Caesium cobaltous silver sulphocyanide, Cs 2 CoAg 2 (SCN) 6 +2H 2 O. Slowly attacked by H 2 O; decomp. by boil- ing H 2 O. Very si. sol. in CsSCN or Co(SCN) 2 +Aq. (Shinn and Wells, Am. Ch. J. 1903, 29. 478.) Caesium cuprous sulphocyanide, CsSCN. CuSCN H 2 separates CuSCN. (Roberts, Am. Ch. J. 1902, 28. 262.) Caesium cuprous nickel sulphocyanide, 2CsSCN, Ni(SCN) 2 , 2CuSCN+2H 2 O. SI. sol. in H 2 O. (Roberts and Wells, Am. Ch. J. 1902, 28. 277.) Caesium cuprous strontium sulphocyanide, 3CsSCN, 2CuSCN, Sr(SCN) 2 . As Ba salt. (Wells, Am. Ch. J. 1902, 28. 275.) Caesium magnesium silver sulphocyanide, 2CsSCN, Mg(SCN) 2 , 2AgSCN +2H 2 O. As Ca comp. (Wells, Am. Ch. J. 1902, 28. 275.) Caesium manganous silver sulphocyanide, Cs 2 MnAg 2 (SCN) 6 +2H 2 0. Rather si. sol. in H 2 O. (Wells.) Caesium mercuric sulphocyanide, CsSCN, Hg(SCN) 2 . SI. sol. in hot H 2 O. (Bristol and Wells, Am. Ch. J. 1902, 28. 260.) Caesium mercuric sulphocyanide, 2CsSCN, Hg(SCN) 2 +H 2 0. Moderately sol. in H 2 O, especially when warm. Recryst. without decomp. (Bristol and Wells, Am. Ch. J. 1902, 28. 260.) Caesium nickel silver sulphocyanide, Cs 2 NiAg 2 (SCN) 6 +2H 2 O. Slowly decomp. by hot H 2 O. (Wells, Am. Ch. J. 1902, 28. 277.) Caesium silver sulphocyanide, CsSCN, AgSCN. Easily forms supersat. . solution. (Wells, Am. Ch. J. 1902, 28. 264.) ^ 2CsSCN, AgSCN. Stable in the air. (Wells.) 3CsSCN, AgSCN. Stable in the air. (Wells.) Caesium silver strontium sulphocyanide, 3CsSCN, 2AgSCN, Sr(SCN) 2 . As Ba comp. (Wells.) Caesium silver zinc sulphocyanide, CsZnAg(SCN) 4 +H 2 O. (Wells.) Cs 2 ZnAg(SCN) 6 . Ppt. Stable in the air. (Wells.) CsZn 2 Ag 3 (SCN) 8 . Decomp. by cold, more rapidly by hot H 2 O. (Wells.) CsZn 2 Ag 4 (SCN) 9 . Slowly decomp. by H 2 O. (Wells.) Caesium zinc sulphocyanide, Cs 2 Zn(SCN) 4 + 2H 2 O. Moderately sol. in H 2 and can be recryst. therefrom. (Wells.) Calcium sulphocyanide, Ca(SCN) 2 +3H 2 O. Deliquescent. Very sol. in H 2 O and al- cohol. Calcium silver sulphocyanide, Ca(SCN) 2 , 2AgSCN+2H 2 O. (Wells.) Calcium stannic sulphocyanide, CaSn(SCN) 6 +7H 2 O. Very sol. in H 2 O. Can be recryst. there- from. Sol. in alcohol and acetone. (Wein- land and Barnes, Z. anorg. 1909, 62. 258.) Cerous sulphocyanide, Ce(SCN) 3 +7H 2 O. Deliquescent. Sol. in H 2 O and alcohol. (Jolin, Bull. Soc. (2) 21. 534.) Chromous sulphocyanide with MSCN. See Chromosulphocyanide, M. Chromic sulphocyanide, Cr(SCN) 3 . Deliquescent, and sol. in H 2 O. Somewhat sol. in organic solvents. (Sper- ansky, C. C. 1897, I. 141. See also Chromisulphocyanhydric acid. Chromic sulphocyanide with MSCN. See Chromisulphocyanide, M. Cobaltous sulphocyanide, Co(SCN) 2 +^H 2 O. Sol. in H 2 O and alcohol; also in ether. Sol. in liquid SO 2 . (Walden, B. 1899, 32. 2864.) Sol. in acetone. (Krug and M'Elroy.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +3H 2 O. Sol. in H 2 O and in alcohol. (Rosenheim and Cohn. Z. anorg. 1901, 27. 288.) Cobaltous mercuric sulphocyanide, Co(SCN) 2 . Hg(SCN) 2 . Very si. sol. in H 2 O and dil. HCl+Aq. Easily sol. in HNO 3 +Aq. (Cleve, J. pr. 91. 227.) 880 SULPHOCYANIDE, COBALTOUS POTASSIUM Cobaltous potassium sulphocyanide, CoK 2 (SCN) 4 . Decomp. by H 2 O. (Treadwell, Z. anorg. 1901, 26. 109.) +4H 2 O. Sol. in H 2 O. Sol. in methyl, ethyl and amyl alcohol, in acetone and in ether +Aq. Can be recryst. from H 2 O or alcohol without decomp. (Rosenheim and Cohn, Z. anorg. 1901, 27. 289.) Cobaltous silver sulphocyanide, CoAg(SCN) 3 +2H 2 O. Decomp. by H 2 O. (Shinn and Wells, Am. Ch. J. 1903, 29. 476.) Ag 2 Co(SCN) 4 . Almost insol. in H 2 O and in alcohol. (Rosenheim, Z. anorg. 1901, 27. 291.) Cobaltous sodium sulphocyanide, Na 2 Co(SCN) 4 +8H 2 O. Sol. in H 2 O and in alcohol. (Rosenheim.) Cobaltous sulphocyanideammonia,Co(SCN) 2/ 2NH 3 and Co(SCiV; 2 , 6NH 3 . (Peters, B. 1908, 41. 3178.) Co(SCN) 2 , 4NH 3 . Sol. in H 2 O and alcohol. (Sand, B. 1903, 36. 1439.) Cobaltous sulphocyanide mercuric chloride. 2Co(SCN) 2 , 2HgCl 2 . (Hantzsch and Shibata. Z. anorg. 1912, 73. 320.) 2Co(SCN) 2 , 3HgCl 2 . Easily decomp. (Hantsch and Shibata.) Cuprous sulphocyanide, CuSCN. 1 1. H 2 O at 18 dissolves 0.004 mg. mols. or 0.5 mg. CuSCN. (Kohlrausch and Rose, Z. phys. Ch. 1893, 12. 241.) Insol. in dil. acids. SI. sol. in cold, easily in warm cone. HCl+Aq. Decomp. by cone. H 2 SO 4 or HNO 3 +Aq. Sol. with combination in NH 4 OH+Aq. Insol. in KSCN+Aq. Less sol. in H 2 SO 3 and H 2 SO 4 +Aq than in HNO 3 . (Kuhn, Ch. Z. 1908, 32. 1056.) Sol. in Fe 2 (SO 4 ) 3 +Aq. (Johnson, J. Soc. Chem. Ind. 1889, 8. 603.) KSCN+Aq (85-90 g. in 50 g. H 2 O) dis- solves 18 g. CuSCN. (Thurnauer, B. 1890, 23. 770.) Sol. in ether. (Skey, C. N. 1867, 16. 201.) Cupric sulphocyanide, Cu(SCN) 2 . Decomp. by H 2 O to cuprous salt. Sol. in warm HC1, H 2 SO 4 , or HNO 3 +Aq. Sol. in MSCN+Aq, but solutions decomp. by dilu- tion. Sol. in NH 4 OH+Aq. Solubility in NH 4 OH+Aq at 25 and at 40. At 25. One gram of solution contains 1000 mols. H 2 O dissolve Composition of solid Sp. gr. 25/25 salt in contact with g. NH 3 g. Cu(SCN) 2 g. H 2 Mols. NH 3 Mols. Cu(SCN) 2 solution 0.99853 0.2147 0.1522 0.6331 358.04 24.09 0.99871 0.1655 0.1124 0.7221 242.02 15.60 .00703 . .01336 0.0993 0.0639 0.0798 0.0659 0.8209 0.8702 127.76 77.51 9.74 7.59 Cu(SCN),,:4NHi .01506 0.0535 0.0622 0.8843 64.05 7.04 .01705 0.0426 0.0596 0.8978 50.21 6.65 .02132 0.0250 0.0511 0.9239 28.55 5.55 .01661 0.0198 0.0408 0.9394 22.27 4.35 Cu(SCN) 2 , 2NH 3 .00816 0.0079 0.0245 0.9676 18.61 2.54 At 40. 0.1802 0.1976 0.6222 306.28 31.83 0.1398 0.1658 0.6944 213.10 23.93 0.0758 0.0550 0.1299 0.1207 0.7943 0.8243 101.00 70.59 16.38 14.67 Cu(SCN) 2 ,^4NH 3 0.0435 0.1178 0.8388 54.82 14.07 0.0352 0.0876 0.8772 42.53 10.00 0.0257 0.0655 0.9088 30.00 7.22 0.0177 0.0418 0.9405 19.86 4.46 >[Cu(SCN) 2 , 2NH 3 0.0094 0.0281 0.9625 10.31 2.93 (Horn, Am. Ch. J. 1907, 37. 471.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Cuprocupric sulphocyanide, Cu(SCN) 2 , Cu 2 (SCN) 2 . Not attacked by hot HCl+Aq. Insol. in KSCN+Aq. SULPHOCYANIDE, LEAD, BASIC 881 Cupric mercuric sulphocyanide, CuHg(SCN) 4 . Almost inspl. in cold H 2 O and in alcohol; si. sol. in boiling H 2 O. (Rosenheim, Z. anorg. 1901, 27. 286.) Cuprous potassium sulphocyanide, CuSCN, 6KSCN. Deliquescent. Decomp. by H 2 O. (Thurn- auer, B. 1890, 23. 770.) Cuprous sulphocyanide ammonia, Cu 2 (SCN) 2 , 2NH 3 . Decomp. in the air. (Richards, Z. anorg. 1898, 17. 247.) Cu 2 (SCN) 2 , 5NH 3 . Very unstable in the air. (Richards.) Cupric sulphocyanide ammonia, Cu(SCN) 2 , 2NH 3 . Sol. in little H 2 O, but decomp. by dilution with pptn. of basic salt. Sol. in NH 4 OH+Aq. By long standing a small amount dissolves in H 2 O with separation of CuSCN. (Litter- scheid, Arch. Pharm. 1901, 239. 337.) Insol. in H 2 O. Sol. in H 2 containing a small amount of ammonia. (Horn, Am. Ch. J. 1907, 37. 477.) Cu(SCN) 2 , 4NH 3 . Very unstable in the air. Sol. in H 2 O, but decomp. by much H 2 O with pptn. of a basic salt. (Horn.) 100 pts. N/10 NH 4 OH+Aq dissolve 10.4 pts. anhydrous salt at 25. (Pudschies, Dis- sert.) Loses NH 3 in the air. Sol. in H 2 O. (Kohlschiitter, B. 1904, 37. 1156.) Decomp. in the air and by H 2 and dil. and cone, acids; sol. in cold cone. HNO 3 and NH 4 OH+Aq. Sol. in boiling cone. HC1. (Richards, Z. anorg. 1898, 17. 250.) Didymium sulphocyanide, Di(SCN) 3 +6H 2 O. Deliquescent, and sol. in H 2 O. Erbium sulphocyanide, Er(SCN) 3 +6H 2 O. Deliquescent. Sol. in H 2 O. (Hoglund.) Glucinum sulphocyanide, G1(SCN) 2 (?). Sol. in H 2 O. (Hermes, J. pr. 97. 465.) Gold (aurous) potassium sulphocyanide, AuSCN, KSCN. Easily sol. in H 2 O, less in absolute alcohol. (Cleve, J. pr. 94. 16.) Gold ocyanide (aurous) potassium sulpho ammonia, KAu(SCN) 2 , 5NH 3 . (Peters, B. 1908, 41. 3178.) Gold (auric) potassium sulphocyanide am- monia, KAu(SCN) 4 , 4NH 3 . (Peters.) Gold (aurous) silver sulphocyanide, AuSCN, AgSCN. Insol. in H 2 O. Sol. in NH 4 OH+Aq. Gold (auric) potassium sulphocyanide. Sol. in H 2 O, alcohol, and ether. (Cleve.) Gold (aurous) sulphocyanide ammonia, AuSCN, NH 3 . Very si. sol. in cold, decomp. by hot H 2 O. Iron (ferrous) sulphocyanide, Fe(SCN) 2 + 3H 2 O. Very sol. in H 2 O, alcohol, or ether. Sol. in acetone. (Krug and M'Elroy.) Iron (ferric) sulphocyanide, Fe(SCN) 3 +3H 2 O. Deliquescent. Very sol. in H 2 O, alcohol, or ether. Ether extracts the salt from Fe(SCN) 3 +Aq. Decomp. by much H 2 O if pure. Not decomp. by monobasic acids, but cone. H 2 SO 4 , and H 8 PO 4 , also oxalic, tartaric, malic, etc., acids destroy the colour. Iron (ferric )lithium sulphocyanide, Fe(SCN), 9LiSCN+4H 2 0. More deliquescent than the other ferric sulphocyanides. (Kriiss and Moraht.) Iron (ferrous) mercuric sulphocyanide, Fe(SCN) 2 , Hg(SCN) 2 +2H 2 0. Moderately sol. in hot H 2 O. (Cleve, J. pr. 91. 227.) Iron (ferric) potassium sulphocyanide, Fe(SCN) 3 , 3KSCN+zH 2 O. Extremely deliquescent, and sol. in H 2 O. (Kriiss and Moraht.) Fe(SCN) 3 , 9KSCN+4H 2 O. Hygroscopic. Sol. in H 2 O without decomp. Insol. in pure anhydrous ether, but decomp. by ether con- taining traces of H 2 O into Fe(SCN) 3 and KSCN. (Kriiss and Moraht, A. 260. 204.) Iron (ferrous) sodium sulphocyanide, Na 4 Fe(SCN) 6 +12H 2 O. Sol. in H 2 O and alcohol. (Rosenheim, Z. anorg. 1901, 27. 299.) Iron (ferric) sodium sulphocyanide, Fe(SCN)s, 9NaSCN+4H 2 0. Less deliquescent than the corresponding NH 4 or K salt. (Kriiss and Moraht.) Na 3 Fe(SCN) 6 +12H 2 O. (Rosenheim, Z. anorg. 1901, 27. 297.) Lanthanum sulphocyanide, La(SCN) 8 + 7H 2 0. Deliquescent; sol. in H 2 O. (Cleve.) Lead sulphocyanide, basic, 6PbO, Pb(SCN) 2 +2H 2 O. Ppt. Pb(SCN) 2 , PbO+H 2 O. Insol. in H 2 O. (Stromholm, Z. anorg. 1904, 38. 440.) 882 SULPHOCYANIDE, LEAD Lead sulphocyanide, Pb(SCN) 2 . Nearly insol. in cold, decomp. by boiling H 2 O. (Liebig.) SI. sol. in H 2 O. 4.5X10 - 1 g. are dissolved in 1 liter of sat. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) Lead sulphocyanide bromide, Pb(SCN) 2 , 8PbBr 2 . (Grissom and Thorp, Am. Ch. J. 10. 219.) Lead sulphocyanide chloride, PbSCNCl. SI. sol. in cold, easily sol. in hot H 2 O. (Murtry, Chem. Soc. 55. 50.) Sol. in H 2 O. (Grissom and Thorp, Am. Ch. J. 10. 229.) Lead sulphocyanide iodide, 3Pb(SCN) 2 , PbI 2 . Sol. in H 2 O. (Grissom and Thorp, Am. Ch. J. 10. 229.) Lithium sulphocyanide, LiSCN. Very deliquescent. Sol. in H 2 O and alco- hol. (Hermes, Z. Ch. 1866. 417.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Magnesium sulphocyanide, Mg(SCN) 2 + 4H 2 O. Deliquescent. Easily sol. in H 2 O and alcohol. Magnesium stannic sulphocyanide, MgSn(SCN) 6 +6H 2 O. Hygroscopic. Sol. in H 2 O, alcohol and acetone. (Weinland and Barnes, Z. anorg. 1909, 62. 258.) Manganous sulphocyanide, Mn(SCN) 2 + 3H 2 0. Deliquescent. Easily sol. in H 2 O and alcohol. Mercurous sulphocyanide, Hg 2 (SCN) 2 . Insol. in H 2 O. Sol. in hot HCl+Aq. Slowly decomp. by hot aqua regia. Sol. in hot KSCN+Aq. Mercuric sulphocyanide, basic, Hg(SCN) 2 , 3HgO. Insol. in H 2 O. Easily sol. in HCl+Aq. Insol. in H 2 SO 4 or HN0 3 +Aq. (Fleischer.) Hg(SCN) 2 , 2HgO. Insol. in H 2 O. SI. attacked by acids. (Glaus, J. pr. 15. 401.) Mercuric sulphocyanide, Hg(SCN) 2 . Very si. sol. in cold, much more easily in hot H 2 O. Easily sol. in dil. HCl+Aq. (Crookes, Chem. Soc. 4. 18.) Solubility in H 2 O= 0.00218 mol. in 1 1. (Grossmann, Z. anorg, 1904, 43. 358.) More sol. in H 2 O than in alcohol. (Peters, B. 1908, 41. 3180.) Very si. sol. in H 2 O at 25. Appreciably sol. only in boiling H 2 O. (Jander Dissert. 1902.) Sol. in Hg(NO 3 ) 2 or KSCN+Aq, also in NH 4 Cl+Aq. Sol. in many sulpho cyanides +Aq. Easily sol. in cold HC1, NH 4 C1, KC1 or BaCl 2 +Aq. (Hermes, J. pr. 1866, (1) 97. 477.) Very sol. in liquid I\H 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Mercuric hydrogen sulphocyanide, Hg(SCN) 2 , 2HSCN. . Easily decomp. (Hermes, Dissert. 1866.) Mercuric nickel sulphocyanide, Hg(SCN) 2 , Ni(SCN) 2 +2H 2 O. Moderately sol. in hot H 2 O. (Cleve, J. pr. 91. 227.) Very sol. in MSCN+Aq. (Orloff, C. C. 1906, I. 1411.) Mercuric potassium sulphocyanide, Hg(SCN) 2 , KSCN. Sol. in cold, more easily in hot H 2 O. Sol. in alcohol and ether. Very sol. in NH 4 C1 or KCl+Aq. (Glaus.) K 2 Hg(SCN) 4 . Very sol. in H 2 O; sol. in alcohol. Insol. in anhydrous ether. (Rosenheim, Z. anorg. 1901, 27. 285.) Mei curie rubidium sulphocyanide, Hg(SCN) 2 , RbSCN. Sol. in alcohol without decomp. Decomp. by H 2 O. Hg(SCN) 2 , 2RbSCN + ^H 2 O. Easily sol. in H 2 O without decomp. (Grossmann, B. 1904, 37. 1259.) Mercuric sodium sulphocyanide, Na 2 Hg(SCN) 3 . Very hydroscopic. (Rosenheim, Z. anorg. 1901, 27. 286.) Mercuric zinc sulphocyanide, Hg(SCN) 2 , Zn(SCN) 2 . Scarcely sol. in cold H 2 O. Easily sol. in HCl+Aq. (Cleve.) Mercuric sulphocyanide ammonia, 2Hg(SCN) 2 , 3NH 3 +^H 2 0. Decomp. by H 2 O and alcohol. Hg(SCN) 2 , 4NH 3 . (Peters, B. 1908, 41. 3178.) Mercuric sulphocyanide ammonium bromide, Hg(SCN) 2 , NH 4 Br. Decomp. by H 2 O. Sol. in alcohol. (Gross- mann, Z. anorg. 1903, 37. 418.) SULPHOCYANIDE, POTASSIUM 883 Mercuric sulphocyanide ammonium chloride Hg(SCN) 2 , NH 4 C1. Deocmp. by H 2 O. Sol. in warm alcoho from which it can be cryst. (Grossmann.) Mercuric sulphocyanide bromide, HgSCNBr Insol. in cold H 2 O; sol. in hot H 2 O and in alcohol. (Rosenheim, Z. anorg. 1901, 27. 282.) Mercuric sulphocyanide chloride, HgSCNCl. Insol. in cold H 2 O. Sol. in hot H 2 O and alcohol. (Rosenheim.) Mercuric sulphocyanide potassium bromide, Hg(SCN) 2 , 2KBr. Very sol. in H 2 O. (Grossmann, Z. anorg. 1903, 37. 418.) Mercuric sulphocyanide potassium chloride, Hg(SCN) 2 , KC1. Decomp. by H 2 O. Not decomp. by recryst. from warm alcohol (Grossmann.) Molybdenum sulphocyanide, Mo(SCN) 3 (?). Sol. in H 2 O and ether. (Braun, Z. anal. 6. 86.) Molybdenum potassium sulphocyanide, K 3 Mo(SCN) 6 +4H 2 O. Cryst. from boiling H 2 O and alcohol. (Chilesotti, Gazz. ch. it. 1904, 34. (2) 493.) Molybdenum sodium sulphocyanide, Na 3 Mo(SCN) 6 + 12H 2 O. (Rosenheim, B. 1909, 42. 154.) Molybdenum thallous sulphocyanide, MoTl 3 (SCN-) 6 . (Rosenheim and Garfunkel, B. 1908, 41. 2388.) Molybdenum sulphocyanide zinc amine, 2Mo(SCN) 6 , 3Zn(NH 3 ) 4 . (Rosenheim and Garfunkel, B. 1908, 41. 2390.) 2Mo(SCN) 6 (OH), Zn,(NH 8 ) n . Can be cryst. from boiling NH 4 OH+Aq. Air-dried salt probably has the composition 2Mo(SCN) 6 (OH), 3Zn(NH 3 ) 4 +2H 2 0. (Maas and Sand, B. 1908, 41. 1510.) 2Mo(SCN) 6 (OH), Zn 3 (NH 3 ) I3 . (Maas and Sand.) Nickel sulphocyanide, Ni(SCN) 2 . Sol. in H 2 O. (Grossmann, B. 1904, 37. 565.) + ^H 2 O. Sol. in H 2 O and alcohol. Insol. in acetone. (Krug and M'Elroy.) +1^H 2 O. Sol. in H 2 O. (Rosenheim and Cohn, Z. anorg. 1901, 27. 292.) Nickel potassium sulphocyanide, K 4 Ni(SCN) 6 +4H 2 0. Sol. in H 2 O with decomp. SI. sol. in cold, easily sol. in hot alcohol. (Rosenheim, Z. anorg. 1901, 27. 292.) Nickel sodium sulphocyanide, NiNa 2 (SCN) 4 +8H 2 O. Sol. in H 2 O with decomp. SI. sol. cold, readily sol. hot alcohol. (Rosenheim, Z. anorg. 1901, 27. 292.) Nickel sulphocyanide ammonia, Ni(SCN) 2 , 3NH 3 . (Peters, B. 1908, 41. 3178.) Ni(SCN),, 4NH,. Decomp. by H 2 O. Platinous sulphocyanide, Pt(SCN) 2 (?). Insol. in H 2 O. See Platinosulphocyanides, and Platmoso- sulphocyanides. Potassium sulphocyanide, KSCN. Deliquescent. Very sol. in H 2 O. 100 pts. H 2 O dissolve 177.2 pts. at 0, and 217.0 pts. at 20. 100 g. sat, KSCN+Aq contain 70.5 g. KSCN at 25. (Foote, Z. phys. Ch. 1903, 46. 81.) 150 pts. KSCN +100 pts. H 2 O at 10.8 lower the temp. 34.5. (Riidorff, B. 2. 68.) Solubility of KSCN +AgSCN at 25. % KSCN % AgSCN Solid phase 70.53 0.00 KSCN 66.55 9.32 KSCN+2KSCN, AgSCN 64.47 10.62 2KSCN, AgSCN 61.25 11.76 tt 58.34 13.55 (t 53.21 17.53 (( 50.68 20.43 2KSCN, AgSCN +KSCN, AgSCN 49.43 20.32 KSCN, AgSCN 32.51 18.34 (( 24.68 16.41 u 23.86 16.07 KSCN, AgSCN + AgSCN (Foote, Z. phys. Ch. 1903, 46. 81.) See also AgSCN. Sol. in alcohol, especially easily if boiling. Sol. in acetone. (Krug and M'Elroy.) Sol. in liquid SO 2 . (Walden, Z. anorg. 1902, 30. 160.) 100 g. acetone dissolve 20.75 g. KSCN at 22, and 20.40 g. at 58. 100 g. amyl alcohol dissolve 0.18 g. KSCN at 13; 1.34 g. at 65; 2.14 g. at 100; 3.15 g. at 133.5. 100 g. ethyl acetoate dissolve 0.44 g. KSCN at 0; 0.40 g. at 14; 0.20 g. at 79. 100 g. pyridine dissolve 6.75 g. KSCN at 0; 6.15 g. at 20; 4.97 g. at 58; 3.88 g. at 884 SULPHOCYANIDE, POTASSIUM MOLYBDENYL 97; 3.21 g. at 115. (Laszcynski, B. 1894, 27. 2285.) 100 g. acetonitrile dissolve 11.31 g. KSCN at 18. (Naumann and Schier, B. 1914, 47. 249. SI. sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Potassium molybdenyl sulphocyanide, 3KSCN, Mo(OH)(SCN) 3 +4H 2 O. Sol. in H 2 O. (Sand and Maas, B. 1908, 41. 1506.) Potassium silver sulphocyanide, KSCN, AgSCN. Decomp. by H 2 0. See Donk .under KSCN. 2KSCN, AgSCN. Stable in the air. (Wells, Am. Ch. J. 1902, 28. 265.) See Donk under KSCN. 3KSCN, AgSCN. (Wells.) Potassium stannic sulphocyanide. K 2 Sn(SCN) 6 +4H 2 0. Very sol. in H 2 O. Sol. in alcohol and acetone. (Weinland and Barnes, Z. anorg. 1909, 62. 258.) Potassium titanyl sulphocyanide, 2KSCN, TiO(SCN) 2 +H 2 O. Sol. in cold H 2 O without immediate de- comp. but slowly decomp. (Rosenheim and Cohn, Z. anorg. 1901, 28. 169.) Potassium vanadium sulphocyanide, 3KSCN, V(SCN) 3 +4H 2 O. Sol. in H 2 O. Sol. in alcohol with a green color. SI. sol. in ether. (Ciocci, Z. anorg. 1898, 19. 309.) Sol. in H 2 O with decomp.; stable in aq. solution in the presence of an excess of KSCN; sol. in alcohol. (Locke, Am. Ch. J. 1898, 20. 604.) Potassium vanadyl sulphocyanide, K 2 VO(SCN) 4 +5H 2 0. Sol. in H 2 O, alcohol, ether, amyl alcohol and ethyl acetate. (Koppel, Z. anorg. 1903, 36. 292.) Potassium zinc sulphocyanide, 2KSCN, Zn(SCN) 2 +3H 2 O. Easily sol. in alcohol. (Walden, Z. anorg. 1900, 23. 374.) Potassium sulphocyanide mercuric bromide, KSCN, HgBr 2 . Very sol. in H 2 O. Sol. in alcohol. (Grossmann, B. 1902, 36. 2945.) 2KSCN, HgBr 2 . Very sol. in H 2 O. Sol. in alcohol. (Grossman.) Potassium sulphocyanide mercuric iodide, 2KSCN, HgI 2 . Undecomp. by solution in cone, alcohol, or in KSCN+Aq. (Grossmann, Z. anorg. 1903, 37. 421.) +2H 2 O. Decomp. by H 2 O. (Philipp, Pogg, 1867, 131. 94.) Silicon sulphocyanide, Si(SCN) 4 . Decomp. by H 2 O and alcohol. Sol. in CS 2 , CHC1 3 and ligroin, (Reynolds, Proc. Chem. Soc. 1906, 22. 17.) Silver sulphocyanide, AgSCN. 1 1. H 2 O dissolves 1.08X10; 6 g. mols. AgSCN at 25. (Kuster and Thiel, Z. anorg. 1902, 33. 139.) 1 1. H 2 O. dissolves 1.25X10 6 gram-atoms of silver at 25. (Abegg and Cox, Z. phys. Ch. 1903, 46. 11.) SI. sol. in H 2 O. 1 liter of sat. solution at 19.96 contains 1.37 X 10 4 g. (Bottger, Z. phys. Ch. 1903, 46. 603.) 6.4 milligrams are dissolved in 1 liter of sat. solution at 100. (Bottger, Z. phys. Ch. 1906, 56. 93.) Solubility product of AgSCN is 0.49 and 1.16X10- 12 mols. per 1. at 18 and 25 re- spectively. (Kirschner, Z. phys. Ch. 1912, 79. 245.) Solubility in H 2 O = 1.2X10- g. mol. per liter at 25. (A. E. Hill, J. Am. Chem. Soc. 1908, 30. 74.) 1 1. H 2 O dissolves 0.00025 g. AgSCN at 21. (Whitby, Z. anorg. 1910, 67. 108.) Insol. in acids, excepting cone. H 2 SO4 or HNO 3 . Insol. in dil., sol. in cone. NH 4 OH + Aq. Sol. in KSCN+Aq. Insol. in AgNO 3 or NH 4 SCN+Aq. Sol. in Hg 2 (NO 3 ) 2 + Aq. Solubility in KSCN at 25. Mol. KSCN in 1 litre g. AgSCN in 1 litre 1.25 1.20 1.12 1.066 0.626 0.573 22.34 19.93 16.18 14.10 2.80 2.06 (Hellwig, Z. anorg. 1900, 25. 184. Solubility in N/10 KSON+Aq at 18 = 2.5 X10 4 . (Kirschner, Z. phys. Ch. 1912, 79. 247.) See also KSCN. 1 1. of a 3-N solution of AgNO 3 dissolves 0.432 g. AgSCN at 25. Nearly insol. in less dil. solution. (Hellwig, Z. anorg. 1900, 25. 179.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in ethyl acetate. (Hamers, Dissert. 1906; Naumann, B. 1910, 43. 314.) SULPHOCYANIDE, TIN 885 Silver strontium sulphocyanide, 2AgSCN, Sr(SCN) 2 +2H 2 O. Stable in the air. (Wells, Am. Ch. J. 1902, 28. 270.) Silver zinc sulphocyanide, 2AgSCN, Zn(SCN) 2 . Decomp. by hot H 2 O. (Wells.) Silver sulphocyanide ammonia, AgSCN, 2NH 3 . Decomp. by H 2 O. Samarium sulphocyanide, Sm(SCN) 3 +6H 2 O. Very deliquescent. (Cleve.) Sodium sulphocyanide, NaSCN. Very deliquescent. Very sol. in H 2 O and alcohol. Sol. in benzonitrile. (Naumann, B. 1914, 47. 1369.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3789.) Sodium stannic sulphocyanide, Na 2 Sn(SCN) 6 +6H 2 O. Very sol. in H 2 O. Sol. in alcohol and ace- tone. (Weinland and Barnes, Z. anorg. 1909, 62. 257.) Sodium vanadium sulphocyanide, 3NaSCN, V(SCN) 3 + 12H 2 O. Very hygroscopic. Sol. in H 2 O and alcohol. (Ciocci, Z. anorg. 1898, 19. 313.) Strontium sulphocyanide, Sr(SCN) 2 +3H 2 O. Very deliquescent, and sol. in H 2 O and alcohol. Strontium stannic sulphocyanide, SrSn(SCN) 6 + 12H 2 O. Sol. in H 2 O, alcohol and acetone. (Wein- land and Barnes, Z. anorg. 1909, 62. 259.) Thallium sulphocyanide, T1SCN. SI. sol. in H 2 O. 3.15 g. are contained in 1 liter of sat. solution at 20; 3.905 g. at 25; 7.269 g. at 39.75. Insol. in alcohol. (Bott- ger, Z. phys. Ch. 1903, 46. 603.) Titanyl sulphocyanide, TiO(SCN) 2 +2H 2 O. Sol. in cold H 2 O. Tin (stannous) sulphocyanide, Sn(SCN) 2 . Sol. in H 2 and alcohol. (Classen, J. pr. 96. 349.) Sol. in cold H 2 0. (Rosenheim, Z. anorg. 1901, 28. 168.) Yttrium sulphocyanide, Y(SCN) 3 +6H 2 O. Not deliquescent. Very sol. in H 2 O, al- cohol, or ether. Zinc sulphocyanide, Zn(SCN) 2 . Less sol. in H 2 O and alcohol than most other cyanides. Zinc sulphocyanide ammonia. Zn(SCN) 2 , 12NH 3 . Decomp. by H 2 O. Sol. in NH 4 OH+Aq. Sulphocyanoplatinic acid. See Platinosulphocyanhydric acid. Sulphocyanoplatinous acid. See Platinososulphocyanhydric acid. Sulphohypophosphoric acid. Aluminum sulphohypophpsphate, A1 2 (PS 3 ) 3 . Unstable in the air. Sol. in H 2 O with de- comp. (Friedel, C. R. 1894, 119. 262.) Cadmium , Cd 2 P 2 S 6 . Partially decomp. in moist air. Decomp. by H 2 O, cold HNO 3 or alkalis +Aq. (Fer- rand, A. ch. 1899, (7) 17. 423; Bull. Soc. 1895, (3) 13. 116.) Chromium , Cr 2 P 2 S 6 . Insol. in HNO 3 . Very si. attacked by aqua regia. (Ferrand.) Cupric , Cu 2 P 2 S 6 . Ppt. (Friedel, C. R. 1894, 119. 262.) Iron (ferrous) , Fe 2 P 2 S 6 . Sol. in HNO 3 and in a mixture of HNO 3 with KC1O 3 . (Friedel.) Lead , Pb 2 P 2 S 6 . Not decomp. by boiling H 2 O. (Friedel.) Mercuric , Hg 2 P 2 S 6 . Slowly decomp. by boiling H 2 O, more rapidly by KOH+Aq. (Friedel.) Nickel , Ni 2 P 2 S 6 . Not attacked by boiling H 2 O or hot or cold acids. SI. attacked by aqua regia. (Ferrand. A. ch. 1899, (7) 17. 416.) Silver , Ag 4 P 2 S 6 . Ppt. (Friedel, C. R. 1894, 119. 263.) Tin (stannous) hypophosphate , SnPS 3 . Decomp. by boiling H 2 O. Sol. in dil. KOH +Aq. (Friedel, C. R. 1894, 119. 264.) Tin (stannic) , SnP 2 S 6 . Easily decomp. by boiling H 2 O. Sol. in dil. KOH+Aq. (Friedel.) SULPHOHYPOPHOSPHATE, ZINC Zinc sulphohypophosphate, Zn 2 P 2 S 6 . Decomp. in moist air. Insol. in H 2 O. Par- tially decomp. by boiling H 2 O. Violently attacked by HNO 3 . Sol. in aqua regia. Not attacked by HC1. (Ferrand, A. ch. 1899, (7) 17. 421.) Zinc , Zn 2 P 2 S 6 . Insol. in H 2 O. Partly decomp. by boiling H 2 O. Not decomp. by HC1 or HNO 3 but by aqua regia. (Ferrand, Bull. Soc. 1895, (3) 13. 115.) Sulphomolybdic acid. Ammonium sulphcmolybdate, (NH 4 ) 2 MoS 4 . Easily sol. in H 2 O; very si. sol. in alcohol. (Berzelius, Pogg. 83. 261.) Ammonium cupric sulphomolybdate. SI. sol. in H 2 O. (Debray, C. R. 96. 1616.) Barium sulphomolybdate, BaMoS 4 . More sol. in H 2 O than BaMo 3 Si . Known only in solution. (Berzelius.) BaS, 3MoS 3 =BaMo 3 Si . SI. sol. in cold, easily sol. in hot H 2 O. Not decomp. by cone 'L cold HNO 3 +Aq, but more easily by dil. HNO 3 +Aq. (Berzelius.) Cadmium sulphomolybdate. Insol. in H 2 O. (Berzelius.) Caesium sulphomolybdate, Cs 2 S, 3MoS 4 + 7H 2 0. As Rb comp. (Herschfinkel, Dissert. 1907.) 3Cs 2 S, 5MoS 4 . (Herschfinkel.) Calcium sulphomolybdate, CaS, 3MoS 3 . Sol. in H 2 O. (Berzelius.) CaMoS 4 . More sol. in H 2 O than CaS, 3MoS 3 . Known only in solution. (Berzelius.) Cerium sulphomolybdate. Precipitate. (Berzelius.) Cobalt sulphomolybdate, CoMoS 4 . Sol. in K 2 MoS 4 +Aq. (Berzelius.) Cupric sulphomolybdate. (Debray, C. R. 96. 1616.) Ferrous sulphomolybdate, FeMoS 4 . Sol. in H 2 O. (Berzelius.) Ferric sulphomolybdate, Fe 2 (MoS 4 ) 3 . Sol. in K 2 MoS 4 +Aq. Lead sulphomolybdate. Ppt. (Berzelius.) Lithium sulphomolybdate. Not deliquescent, but very easily sol. in H 2 O. (Berzelius.) Magnesium sulphomolybdate, MgMoS 4 . Sol. in K 2 MoS 4 +Aq. (Berzelius.) Manganous sulphomolybdate, MnMoS 4 . Sol. in H 2 O. (Berzelius.) Mercurous sulphomolybdate, Hg 2 MoS< (?). Ppt. Mercuric sulphomolybdate, HgMoS 4 . Insol. in K 2 MoS 4 +Aq. Nickel sulphomolybdate, NiMoS 4 . Sol. in K 2 MoO 4 +Aq. (Berzelius.) Potassium sulphomolybdate, basic, K 6 Mo 2 S 9 . Easily sol. in H 2 O. Insol. in alcohol and ether. (Kruss, B. 16. 2050.) Potassium sulphomolybdate, K 2 MoS 4 . Sol. in H 2 O, from which it is precipitated by alcohol. (Berzelius.) Rubidium sulphomolybdate, 3Rb 2 S, 8MoS 3 + 30H 2 O. Very si. sol. in H 2 O. Sol. by addition of NH 3 . (Herschfinkel, Dissert. 1907.) 5Rb 2 S, 6MoS 2 . (Herschfinkel.) Silver sulphomolybdate, Ag 2 MoS 4 . Ppt. Sodium sulphomolybdate, Na 2 MoS 4 . Sol. in H 2 O, and not precipitated by al- cohol from aqueous solution. (Berzelius.) Strontium sulphomolybdates. Exactly analogous to the Ba salts, which see. (Berzelius.) Zinc sulphomolybdate. Ppt. Insol. in H 2 O. (Berzelius.) Mowosulphomolybdic acid.] Sodium rnonosulphomolybdate, Na 2 MoO 3 S. Rather hygroscopic. Sol. in H 2 O; forms deep blue solution with H 2 SO 4 . Sol. in HC 2 H 3 O 2 +Aq. (Kruss, A. 225. 1.) ZH'sulphomolybdic acid. Ammonium ^sulphomolybdate. (NH 4 ) 2 Mo0 2 S 2 . SI. sol. in cold, easily in hot H 2 O. Insol. in sat. NH 4 Cl+Aq and absolute alcohol. Aqueous solution is decomp. by boiling. (Bodenstab, J. pr. 78. 186.) SULPHONOSMATE, POTASSIUM 887 Potassium cfosulphomolybdate, K 2 MoO 2 S 2 . Very sol. in H 2 O and alcohol. Sol. in HC 2 H 3 O 2 +Aq. (Kriiss, B. 16. 2046.) Tn'sulphomolybdic acid. Ammonium hydrogen Zn'sulphopyromolyb- date, NH 4 HMo 2 O 4 S 3 . Precipitate. Insol. in alcohol or CS 2 (Kriiss, B. 16. 2047.) Potassium hydrogen Znsulphopyromolybdate KHMo 2 4 S 3 . Very easily sol. in H 2 O. (Kriiss, B. 16, 2048.) Sodium hydrogen 2nsulphdp?/romolybdate, NaHMo 2 O 4 S 3 . Precipitate. Much more sol. in H 2 O than the NH 4 compound. (Kriiss, B. 16. 2047.) Potassium sulphoinolybdate, K 8 Mo 4 S 9 O 7 . Sol. in H 2 O, HC 2 H 3 0% and H 2 SO 4 . (Kruss B. 17. 1771.) Pewtasulphomolybdic acid. Potassium pentasulphomolybdate, KMoS 6 . Sol. in warm H 2 O. (Hofmann, Z. anorg. 1896, 12. 62.) Persulphomolybdic acid, H 2 MoS 5 . Precipitate. Insol. in H 2 O, alcohol, ether, CS 2 , and acetic acid. Decomp. slowly by hot H 2 SO 4 . Sol. in warm KOH+Aq, and cold K 2 S+Aq. Not attacked by cold KSH+Aq, but dissolves on warming. (Kriiss, B. 17. 1773.) Ammonium persulphomolybdate, (NH 4 ) 2 MoS 5 . Very si. sol. in cold, more easily in hot JI 2 O. Insol. in NH 4 OH+Aq. (Berzelius.) Barium , BaMoS 6 . Insol. in boiling H 2 O or dil. HCl-fAq. (Berzelius.) Calcium . Difficultly sol. in H 2 O. (Berzelius.) Cerium . Precipitate. (Berzelius.) Ferrous . Insol. in Fe salts -fAq, but sol. in K 2 MoS 6 + Aq. (Berzelius.) Ferric . Ppt. Lithium persulphomolybdate. SI. sol. in cold, easily sol. in hot H 2 O. (Berzelius.) Magnesium . Insol. precipitate. (Berzelius.) Nickel . Ppt. Sol. in K 2 MoS 6 +Aq, from which it separates in 24 hours. (Berzelius.) Potassium , K 2 MoS 6 . Almost insol. in cold, more sol. in hot H 2 O. Insol. in cold KOH+Aq. (Berzelius.) Potassium hydrogen , KHMoS 6 . Sol. inH 2 O. (Kruss.) Sodium , Na 2 MoS 6 . SI. sol. in cold, easily in hot H 2 O. (Ber- zelius.) Sodium hydrogen (Kruss.) -, NaHMoS 5 . Persulphomolybdic acid, HMoS 6 . Sol. in H 2 O. (Hofmann, Z. anorg. 1896, 12. 59.) Ammonium , NH 4 MoS 6 +H 2 0. SI. sol. in H 2 O and in alcohol with decomp. (Hofmann.) Caesium , CsMoS 6 Almost insol. in H 2 O. (Hofmann.) Potassium , KMoS 6 . Sol. in H 2 O. (Hofmann,) Thallium , TlMoS 6 . Insol. in H 2 O. (Hofmann.) Sulphonosmic acid. Potassium sulphonosmate, 7K 2 0, 40s0 3 , 10 S0 2 . Sol. in H 2 O. (Rosenheim, Z. anorg. 1899, 21. 127.) +3H 2 O. Sol. in H 2 O. (Rosenheim.) +7H 2 O. Easily sol. in H 2 O; decomp. in aq. solution at 70 . (Rosenheim.) 11K 2 O, 4OsO 3 , 14SO 2 +7H 2 O. Sol. in H 2 O. Rosenheim.) Sodium sulphonosmate, 3Na 2 O, OsO 8 , 4SO 2 +5H 2 O. Easily sol. in H 2 O; decomp. in aq. solution. Rosenheim.) 888 SULPHOPALLADIC ACID Sulphopalladic acid. Potassium palladious sulphopalladate, K 2 S, Pd 2 S, PdS 2 =K 2 Pd 3 S 4 . Insol. in H 2 O. Moderately cone. HCl+Aq dissolves out K without evolution of H 2 S. (Schneider, Pogg. 141. 526.) Silver sulphopalladate, Ag 2 PdS 3 . (Schneider.) Silver palladious sulphopalladate, Ag 2 S, Pd 2 S, PdS 2 =Ag 2 Pd 3 S 4 . Extraordinarily stable. (Schneider.) Sodium sulphopalladate, Na 2 PdS 3 . Slowly sol. in H 2 O. Insol. hi alcohol. (Schneider, Pogg. 141. 520.) Sulphophosphide of M. See M phosphosulphide. Sulphophosphamic acid, 1 See Thiophosphamic acid. OH Sulphophosphodiamic acid, PS/j^jV See Thiophosphocfo'amic acid. SulphophosphoJn'amide, PS(NH 2 ) 3 . See Thiophosphoryl Znamide. Sulphophosphoric acid, H 3 PSO 3 . See Thiophosphoric acid. H 3 PS 4 . Known only in its salts. Ammonium sulphophosphate, (NH 4 ) 3 PS 4 . Stable in the air. (Ephraim, B. 1911, 44. 3408.) Antimony sulphophosphate, SbPS 4 . Insol. in H 2 O, alcohol, ether, CS 2 , HC1+ Aq, dil. H 2 SO 4 +Aq, CeHe, or HC 2 H 3 O 2 . Decomp. by boiling with cone. HNO 3 +Aq, H 2 S0 4 , aqua regia, KOH, NaOH or NH 4 OH +Aq. (Glatzel, B. 24. 3886.) Arsenic sulphophosphate, AsPS 4 . Insol. in H 2 O, alcohol. HCl+Aq, etc. De- comp. by warm HNO 3 , aqua regia, dil H 2 S0 4 ; also sol. in KOH or NH 4 OH+Aq (Glatzel, Z. anorg. 4. 186.) Barium sulphophosphate, Ba 3 (PS 4 ) 2 +xH 2 0. (Ephraim, B. 1911, 44. 3409.) Bismuth sulphophosphate, BiPS 4 . Insol. in H 2 O, alcohol, ether, CS 2 , benzene HC 2 H 3 O 2 , or dil. H 2 SO 4 +Aq. Decomp. by boiling HCl+Aq, cone. H 2 SO 4 , HNO 3 , or aqua regia; also by NaOH, KOH, or NH 4 OH +Aq. (Glatzel, Z. anorg. 4. 186.) Cadmium sulphophosphate, Cd 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, ether, benzene, CS 2 , and HC 2 H 3 O 2 . Decomp. by hot HC1+ Aq. Very si. attacked by dil. H 2 SO 4 +Aq. Slowly sol. in hot HNO 3 , rapidly in aqua regia or hot cone. H 2 SO 4 . (Glatzel, Z. anorg. 4. 186.) Cuprous sulphophosphate, Cu 3 PS 4 . Insol. in H 2 O, alcohol, etc.; also in HC1 or dil. H 2 SO 4 +Aq. Decomp. by HNO 3 , aqua regia, etc., not by KOH or NaOH+Aq. 'Glatzel.) Ferrous sulphophosphate, Fe 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, ether, etc.; insol. in BC1 or hot dil, H 2 SO 4 +Aq. Decomp. by HNO 3 , aqua regia, or cone. H 2 SO 4 . Not attacked by KOH or NH 4 OH+Aq. (Glat- zel.) Lead sulphophosphate, Pb 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, etc. Decomp. by warm HCl+Aq, cone. HNO 3 +Aq; not at- tacked by NH 4 OH+Aq; si. decomp. by KOH +Aq. (Glatzel.) Manganous sulphophosphate, Mn 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, ether, benzene, CS 2 , or HC 2 H 3 O 2 . Not attacked by HCl+Aq. Sol. in HNO 3 or aqua regia, with separation of S. Not attacked by dil. H 2 SO 4 +Aq. (Glatzel, Z. anorg. 4. 186.) Mercuric sulphophosphate, Hg 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, etc.; also in HC1, dil. HNO 3 , or H 2 SO 4 +Aq. Not attacked by cone. HNO 3 or aqua regia; easily sol. in HNO 3 +Br 2 +Aq. (Glatzel.) Nickel sulphophosphate, Ni 3 (PS 4 ) 2 . As the ferrous salt. (Glatzel.) Potassium sulphophosphate, K 3 PS 4 +H 2 O. Easily sol. in H 2 O. (Ephraim, B. 1911, 44. 3407.) Silver sulphophosphate, Ag 3 PS 4 . Insol. in H 2 O, alcohol, etc.; also in HC1, HNO 3 , or dil. H 2 SO 4 +Aq. Decomp. by cone. H 2 SO 4 , and aqua regia. (Glatzel.) Sodium sulphophosphate, Na 3 PS 4 +8H 2 O. Decomp. by H 2 O. Sol. in Na 2 S+Aq. (Glatzel, Z. anorg. 1905, 44. 65.) Thallous sulphophosphate, T1 3 PS 4 . Insol. in H 2 O, alcohol, etc. Sol. in HC1, dil. H 2 SO 4 +Aq, etc. Not attacked by NH 4 OH+Aq; si. decomp. by cone. KOH+ Aq. (Glatzel.) SULPHOPHOSPHITE, SILVER Tin (stannous) sulphophosphate, Sn 3 (PS 4 )2. Insol. in H 2 O, alcohol, etc. Insol. in dil. H 2 SO 4 or HCl+Aq. Decomp. by HNO 3 + Aq, aqua regia, NH 4 OH, or KOH+Aq. (Glatzel.) Zinc sulphophosphate, Zn 3 (PS 4 ) 2 . Insol. in H 2 O, alcohol, ether, etc. Sol. in HCl+Aq or dil. H 2 SO 4 +Aq. Easily at- tacked by KOH+Aq; si. decomp. by NH 4 OH +Aq. (Glatzel.) Sulphop?/rophosphoric acid. Aluminum sulphop?/rophosphate, A1 2 P 2 S 7 . Decomp. in moist air. Violently decomp. by H 2 O or acids. (Fer- rand, A. ch. 1899, (7) 429.) Cadmium , Cd 2 P 2 S 7 . Decomp. in moist air. Not attacked by cold acids. (Ferrand.) Chromium , Cr 2 P 2 S 7 . Decomp. in moist air. Not readily attacked by acids. (Ferrand.) Cuprous , Cu 4 P 2 S 7 . Not attacked by cold H 2 SO 4 or boiling HC1. (Ferrand.) Sol. in hot cone. HNO 3 . (Ferrand.) Sol. in alkalies, and in all acids except HC1. (Ferrand, C. R. 1896, 122. 886.) Ferrous , Fe 2 P 2 S 7 . Insol. in cold acids. SI. attacked by boiling HC1 or hot KOH + Decomp. by fused KOH. (Ferrand, A. ch. 1899, (7) 17. 410.) Lead , Pb 2 P 2 S 7 . Not attacked by cold HNO 3 . (Ferrand,) Mercurous , Hg 4 P 2 S 7 . Decomp. by moist air or hot HNO 3 . (Fer- rand.) Almost insol. in acids; decomp. by H 2 O and moist air. (Ferrand, C. R. 1896, 122. 888.) Nickel , Ni 2 P 2 S 7 . Decomp. by H 2 O and by cone. HNO 3 at 150 in a sealed tube. (Ferrand, A. ch. 1899, (7) 17. 418.) Silver , Ag 4 P 2 S 7 . Not decomp. by H 2 O. Decomp. by aqua regia. Not attacked by HNO 3 . (Ferrand.) Zinc , Zn 2 P 2 S 7 . Decomp. in moist air. Decomp. by H 2 O. Violently attacked by cold HNO 3 . (Fer- rand.) Sulphophosphorous acid, H 3 PSO 2 =SPOH(?). OH See Thiophosphorous acid. H 3 PS 3 . Known only in its salts. Aluminum sulphophosphite, A1 3 (PS 3 ) 2 . Very unstable. Decomp. in the air. (Ferrand, C. R. 1896, 122. 622.) Barium sulphophosphite, Ba 3 (PS 3 ) 2 +zH 2 O. Sol. in dil. acids. Insol. in alcohol. (Ephraim, B. 1911, 44. 3412.) Chromous sulphophosphite, Cr 3 (PS 3 ) 2 . Easily attacked by hot cone. HNO 3 or aqua regia. Decomp. by boiling NaOH+Aq. (Fer- rand, A. ch. 1899, (7) 17. 419.) Quite stable in moist air; very slowly at- tacked by acids. (Ferrand, C. R. 1896, 122. 622.) Cuprous sulphophosphite, Cu 3 PS 3 . Not attacked by H 2 O or hot cone. HC1. SI. attacked by cold fuming HNO 3 . Violently attacked by HNO 3 , aqua regia and boiling cone. H 2 SO 4 . Not attacked by boiling NaOH+Aq. (Ferrand, A. ch. 1899, (7) 17. 398.) Fairly stable; decomp. by damp air. (Fer- rand, C. R. 1896, 122. 621.) Iron (ferrous) sulphophosphite, Fe 3 (PS 3 ) 2 . Very stable and resists the action of alkalies and acids. (Ferrand, C. R. 1896, 122. 622.) Insol. in cold acids or hot NCI. Sol. in hot fuming HNO 3 . Insol. in hot 40% KOH+Aq. (Ferrand, A. ch. 1899, (7) 17. 412.) Mercuric sulphophosphite, Hg 3 (PS 3 ) 2 . Decomp. in moist air. Not attacked by cold HNO 3 . Decomp. byhotHNO 3 . (Ferrand.) Unstable in the air. Very slowly attacked by acids. (Ferrand, C. R. 1896, 122. 622.) Nickel sulphophosphite, Ni 3 (PS 3 ) 2 . Unstable in the air. Attacked slowly by HNO 3 . (Ferrand.) Silver sulphophospbite, Ag 3 PS 3 . Insol. in most reagents. (Ferrand. C. R. 1896, 122. 622.) Not decomp. by H 2 O. Not easily attacked by acids. (Ferrand, A. ch. 1899, (7) 17. 414.) 890 SULPHOPHOSPHITE, SODIUM Sodium sulphophosphite, Na 3 PS 3 +zH 2 O. Very sol. in H 2 O, probably with decomp. (Ephraim, B. 1911, 44. 3410.) Zinc sulphophosphite, Zn 3 (PS 3 ) 2 . Decomp. in moist air. SI. attacked by H 2 O. Decomp. by HNO 3 . (Ferrand, A. ch. 1899, (7) 17. 422.) Very unstable in the air, and attacked violently by acids. (Ferrand, C. R. 1896, 122.622.) ' Sulphoplatinic acid, H 2 Pt 4 S 6 . Insol. in H 2 O, but decomp. on air. (Schneider, Pogg. 138. 604.) H 4 Pt 3 S 6 . Insol. in H 2 O, but decomp. very rapidly on air. (Schneider.) Copper sulphoplatinate, 2CuS, 2PtS, PtS 2 . Insol. in H 2 O. HC1, HNO 3 , or aqua regia dissolve out part of the Cu. (Schneider, Pogg. 139. 661.) Lead sulphoplatinate, 2PbS, 2PtS, PtS 2 . Insol. in hot or cold H 2 O or HCl+Aq. HNO 3 +Aq dissolves out Pb partly; aqua regia dissolves completely with difficulty. (Schneider, Pogg. 139. 662.) Mercuric sulphoplatinate chloride, 2HgS, 2PtS, PtS 2 , 2HgCl 2 . Insol. in H 2 O; not attacked by HCl+Aq, and only partially sol. in boiling aqua regia. (Schneider.) Potassium sulphoplatinate, K 2 Pt 4 S 6 . Insol. in H 2 O. HCl+Aq dissolves out K without evolution of H 2 S. Composition its potassium platinous sul- phoplatinate, K 2 S, 3PtS, PtS 2 . (Schneider, Pogg. 138. 604.) Silver sulphoplatinate, 2Ag 2 S, 2PtS, PtS 2 . Insol. in H 2 or HCl+Aq. HNO 3 +Aq dissolves out Ag on warming. Aqua regia decomp. with formation of AgCl. (Schnei- der, Pogg. 138. 664.) Sodium sulphoplatinate, Na 4 Pt 3 S 6 = 2Na 2 S, 2PtS, PtS 2 . Decomp. by hot H 2 O, with residue of PtS 2 . (Schneider.) Na 2 Pt 3 S 6 = Na 2 S, PtS, 2PtS 2 . Insol. in H 2 O. (Schneider, J. pr. (2) 48. 418.) Thallium sulphoplatinate, 2T1 2 S, 2PtS, PtS 2 . Insol. in cold H 2 O. Dil. acids dissolve out all the thallium. (Schneider, Pogg. 138. 626.) Sulphoplatinous acid, H 2 PtS 2 . Known only in solution in H 2 O, which soon decomposes. (Schneider, J. pr. (2) 48. 424.) Sodium sulphoplatinite, Na 2 PtS 2 . Sol. in H 2 O with decomp. (Schneider, J. pr. (2) 48. 420.) H 4 Na 2 (PtS 2 ) 3 . Sol. in H 2 O, from which it is pptd. by alcohol. (Schneider.) Sulphoselenantimonous acid. See Selenosulphantimonous acid. Sulphoselenarsenic acid. See Selenosulpharsenic acid. Sulphoselenostannic acid. See Selenosulphostannic acid. Sulphoselenoxyarsenic acid. See Selenosulphoxyarsenic acid. Sulphoselenyl chloride, SSeO 3 Cl 4 . Deliquescent; decomposed by H 2 O. (Claus- nitzer, B. 11. 2007.) Afetasulphosilicic acid. Sodium metosulphosilicate, Na 2 SiS 3 . Decomp. by H 2 O. (Hempel, Z. anorg. 1900, 23. 41.) Sulphostannic acid, H 2 SnS 3 . Ppt. (Kiihn, A. 84. 110.) Does not exist. (Storch, W. A. B. 98. 2b. 236.) Ammonium sulphostannate, (NH 4 ) 2 S, 3SnS 2 +6H 2 O. Easily sol. in H 2 O, and easily decomp. (Ditte, C. R. 96. 641.) (NH 4 ) 2 SnS 3 +3H 2 O, and +7H 2 O. De- comp. by acid. (Stanek, Z. anorg. 1898, 17. 124.) Barium sulphostannate, BaSnS 3 +8H 2 O. Sol. in cold H 2 O. (Ditte, C. R. 96. 641.) Calcium sulphostannate, 2CaS, SnS 2 +14H 2 O. Sol. in H 2 O. (Ditte, C. R. 96. 641.) s sulphostannate, 4PtS, SnS 2 . Not decomp. by acids. (Schneider, J. pr. (2) 7. 214.) Platinum potassium sulphostannate, 3PtS, K 2 S, SnS 2 . Insol. in cold H 2 O. Dil. HC1 or HC 2 H 3 O 2 +Aq dissolves out all the potassium. (Sch- neider, Pogg. 136. 109.) SULPHOSTANNATE, PLATINUM SODIUM 891 Platinum sodium sulphostannate, 3PtS, Na 2 S, SnS 2 . Insol. in cold H 2 O. (Schneider, Pogg. 136. 109.) Potassium sulphostannate, K 2 SnS 3 . Sol. in H 2 O. (Kuhn, A. 84. 110.) +3H 2 O. (Ditte, C. R. 96. 641.) K 4 SnS 4 +4H 2 O. Sol. in H 2 O: pptd. by alcohol. (Weinland, Z. anorg. 1898, 17. 419.) Sodium sulphostannate, Na 2 SnS 3 +2H 2 O. SI. sol. in H 2 O. (Kuhn, A. 84. 110.) +3H 2 O. (Ditte, C. R. 95. 641.) +7H 2 O. Sol. in H 2 O. (Horing, Zeitsch. Pharm. 1851. 120.) Na 4 SnS 4 + 12H 2 O. Melts in crystal H 2 O on heating. Very sol. in H 2 O. (Kuhn.) Strontium sulphostannate, SrSnS 3 + 12H 2 O. Sol. in H 2 O. (Ditte, C. R. 95. 641.) Thallium sulphostannate, Tl 4 SnS 4 . Ppt. Practically insol. in H 2 O. (Hawley, J. Am. Chem. Soc. 1907, 29. 1011.) ZH'sulphopersulphuric acid. Sodium efosulphopersulphate, Na 2 S 4 O 8 . Sol. in H 2 O. Cryst. in cold with 2H 2 O. (Villiers, C. R. 106. 851, 1354.) Contains 4H more and is sodium tetra- thionate, NaS 4 O 6 , 2H 2 O. (Villiers, C. R. 108. 402.) Sulphotelluric acid; Mercurous sulphotellurate, 3Hg 2 S, TeS 2 . Ppt. Mercuric , 3HgS, TeS 2 . Ppt. (Berzelius.) Potassium , K 2 TeS 4 . Sol. in H 2 O. (Oppenheim, J. pr. 71. 279.) Sodium . Sol. in H 2 O. (Oppenheim.) Sulphotellurous acid. Ammonium sulphotellurite, 3(NH 4 ) 2 S, TeS 2 . Decomp. on air. Sol. in H 2 O. Barium . Very slowly sol. in H 2 O. Calcium . Somewhat sol. in H 2 O. Cerium . Insol. ppt. Cobalt sulphotellurite, Co 3 TeS 6 . Ppt. Copper , Cu 3 TeS 6 . Ppt. Ferrous . Ppt. Ferric . Ppt. Lead . Ppt. Lithium . Sol. in H 2 O. Magnesium . Sol. in H 2 Q and alcohol. Manganous . Ppt. Potassium , 3K 2 S, TeS 2 . Sol. in H 2 O. Silver , 3Ag 2 S, TeS 2 . (Berzelius.) Sodium . Sol. in H 2 O. Strontium . Sol. in H 2 O. Zinc , 3ZnS, TeS 2 . Ppt. (Berzelius.) Sulphotungstic acid. Ammonium sulphotungstate, (NH 4 ) 2 WS 4 . Very deliquescent. Easily sol. in H 2 O, and still more easily in NH 4 OH+Aq. (Corleis. A. 232. 244.) *|) More sol. in pure H 2 than in H 2 O acidified with HC1. Decomp. slowly on air. |(Ber- zelius.) Barium . Sol. in BaS+Aq. Cadmium , CdWS 4 . Ppt. (Berzelius.) Calcium . Sol. in H 2 O and alcohol. (Berzelius.) Cobalt , CoWS 4 . SI. sol. in H 2 O. 892 SULPHOTUNGSTATE, COPPER Copper sulphotungstate, CuWS 4 . Ppt. Glucinum , G1WS 4 . Sol. in H 2 O(?). Ferrous , FeWS 4 . Sol. in H 2 O. Ferric . Ppt. Lead , PbWS 4 . Ppt. (Berzelius.) Magnesium , MgWS 4 . Easily sol. in H 2 O or alcohol. Manganous , MnWS 4 . Sol. in H 2 O. (Berzelius.) Mercurous . Ppt. (Berzelius.) Mercuric -, HgWS 4 . Ppt. (Berzelius.) Nickel , NiWS 4 . Ppt. (Berzelius.) Potassium , K 2 WS 4 . Sol. in H 2 O. Alcohol precipitates from aqueous solutions, but is not entirely insol. in alcohol. (Berzelius.) Very sol. in H 2 O. (Corleis, A. 232. 264.) Potassium nitrate, K 2 WS 4 , KN0 3 . Very sol. in cold or hot H 2 O, from which it is precipitated by alcohol. (Berzelius.) Potassium tungstate, K 2 W0 2 S 2 = K 2 WS 4 , K 2 W0 4 . Easily sol. in H 2 O. Not precipitated by alcohol. (Berzelius.) Is potassium ^nsulphotungstate, K 2 WOS 3 , which see. (Corleis, A. 232. 244.) Silver , Ag 2 WS 4 . Ppt. (Berzelius.) Sodium , Na 2 WS 4 . Very sol. in H 2 O; less sol. in alcohol. (Ber- zelius.) Very deliquescent. (Corleis, A. 232. 264.) Strontium . Sol. in H 2 O, and in SrS+Aq. Stannous , SnWS 4 . Ppt. (Berzelius.) Stannic , SnWS 6 . Ppt. (Berzelius.) Zinc sulphotungstate, ZnWS 4 . Sol. in H 2 O with subsequent pptn. (Ber- zelius.) Afonosulphotungstic acid. Potassium raonosulphotungstate, K 2 WOS+H 2 O. Deliquescent in moist air. Very sol. hi H 2 0. (Corleis, A. 232. 244.) ZH'sulphotungstic acid. Ammonium ^sulphotungstate, (NH 4 ) 2 WO 2 S 2 . Sol. in H 2 O and alcohol. (Berzelius.) Decomp. easily when moist. (Corleis, A. 232. 264.) Tn'sulphotungstic acid. Potassium tfn'sulphotungstate, K 2 WOS 3 -f- H 2 O. Hygroscopic. Effloresces on dry air and easily decomposed. Easily sol. in H 2 O. (Cor- leis, A. 232. 244.) Sulphovanadic acid, V 2 O 5 , 3SO 3 +3H 2 O. See Vanadiosulphuric acid, and Sulphate, vanadium. Sulphovanadates. Alkali sulphovanadates are sol. in H 2 O. Ca, Sr, and Ba sulphovanadates are si. sol. in H 2 O, and all other sulphovanadates are insol. inH 2 O. (Berzelius.) Ammonium sulphovanadate, (NH 4 ) 3 VS 4 . Easily sol. in H 2 O. Very si. sol. in cone. NH 4 SH +Aq. Insol. in ether, CS 2 , or CHC1 3 . (Kriiss and Ohnmais, A. 263. 46.) See also Sulphoxyvanadic acid. Sodium pentasulphopyrovanadate, Na 4 V 2 O 2 S 5 . Hydroscopic; sol. in H 2 O with rapid de- comp. (Locke, Am. Ch. J. 1898, 20. 375.) Sulphoxyantimonic acid. Potassium sulphoxyantimonate, K 2 HSbO 2 S 2 +2H 2 0. Sol. in hot, less sol. in cold H 2 O. Decomp. by cold H 2 O. (Weinland and Gutmann, Z. anorg. 1898, 17. 414.) Sulphoxyarsenic acid, H 3 AsO 3 S. Known only in aqueous solution. (McCay, Am. Ch. J. 10. 459.) Ammonium monosulphoxyarsenate, (NH 4 ) 3 AsSO 3 +3H 2 O. Decomp. in the air; sol. in H 2 O, decomp. on boiling. (Weinland, B. 1896, 29. 1009.) SULPHOXYARSENATE, SODIUM STRONTIUM 893 Very sol. in H 2 O; insol. in alcohol; decomp. in aq. solution and also in the air. (Weinland, Z. anorg. 1897, 14. 53.) Decomp. in the air. (McLauchlan, B. 1901, 34. 2166.) Ammonium hydrogen monosulphoxyarsenate, (NH 4 ) 2 HAsSO 3 . Ppt. (McLauchlan, B. 1901, 34. 2168.) Barium monosulphoxyarsenate. BaHAs0 3 + 10H 2 0. (Preis, A. 257. 184.) Ba 3 (AsSO 3 )2+6H 2 O. Ppt. (Weinland, Z. anorg. 1897, 14. 54.) Barium efo'sulphoxyarsenate, Ba 3 (AsS 2 O 2 ) 2 + 4H 2 O. Ppt. (Preis, A. 257. 185.) +6H 2 O. (Weinland and Rumpf, Z. anorg. 1897, 14. 64.) Barium potassium ^n'sulphoxyarsenate, KBaAsS 3 O+7H 2 O. Ppt. (McCay, Z. anorg. 1904, 41. 469.) Barium sodium monosulphoxyarsenate, BaNaAsSO 3 +9H 2 O. Ppt. (Weinland, Z. anorg. 1897, 14. 55.) Barium sodium sulphoxyarsenate, Ba 7 Na 2 As 5 O 7 S 14 (McCay and Foster, Z. anorg. 1904, 41. 467.) Calcium ^n'sulphoxyarsenate, Ca 3 (AsS 3 O) 2 + 20H 2 O. Ppt. (McCay and Foster, Z. anorg. 1904, 41. 463.) Potassium monosulphoxyarsenate, K 3 AsSO 3 . Hydroscopic. (Weinland, B. 1896, 29. 109.) Sol. in cone. KOH+Aq, free from carbon- ate; very hydroscopic. (Weinland, Z. anorg. 1897, 14. 51.) Potassium hydrogen monosulphoxyarsenate. K 2 HAsSO 3 +2^H 2 O. Very hygroscopic. (Weinland and Rumpf, Z. anorg. 1897, 14. 59.) KH 2 AsSO 3 . Sol. in H 2 O; solution slowly decomp. on standing. (McCay, Am. Ch. j. 10. 459.) Formula given by Bouquet and Cloez (A. ch. (3) 13. 44) is K 2 H 4 As 2 S 3 O5. Potassium disulphoxyarsenate, K 3 AsS 2 O 2 + 10H 2 0. Very hydroscopic; decomp. by H 2 O. (Weinland, Z. anorg. 1897, 14. 63.) Potassium ^n'sulphoxyarsenate. K 3 AsS 3 O + 7H 2 0. Yellow oil which cryst. at 20. (McCay and Foster, Z. anorg. 1904, 41. 468.) Sodium monosulphoxyarsenate, Na 3 AsS0 3 + 12H 2 0. Easily sol. in H 2 O. (Preis, A. 257. 180.) (McLaughl,an, B. 1901, 34. 2170.) Sol. in H 2 O. (Weinland, B. 1896, 29. 1009.) SI. efflorescent. Insol. in alcohol. (McCay, Z. anorg. 1902, 29. 42.) Sol. in NaOH+Aq; decomp. by boiling with cone. NaOH. (Weinland, Z. anorg. 1897, 14. 49.) Sodium hydrogen monosulphoxyarsenate, NaH 2 AsSO 3 . Deaomp. by H 2 0; insol. in alcohol. (Wein- land, Z. anorg. 1897, 14. 58.) Na 2 HAsSO 3 +8H 2 O. Easily sol. in H 2 O. (Preis.) Sodium (^'sulphoxyarsenate, Na 3 AsS 2 O 2 + 10H 2 O. Easily sol. in H 2 O. (Preis.) Sol. in H 2 O; pptd. by alcohol. (McCay, B. 1899, 32. 2472.) Not decomp. by boiling NaOH+Aq. (Weinland, Z. anorg. 1897, 14. 62.) Insol. in alcohol. (McCay, Z. anorg. 1900. 25. 461.) +11H 2 O. (McLaughlan; B. 1901, 34. 2170.) Insol. in alcohol. (McCay, Z. anorg. 1902, 29. 46.) Sodium frisulphoxyarsenate, Na 3 AsS 3 O + 11H 2 O. Decomp. by H 2 O. (McCay and Foster, Z. anorg. 1904, 41. 454.) Sodium ^nsulphoxydiarsenate, As 2 O 2 S 3 , 3Na 2 O+24H 2 O. Easily sol. in H 2 O. (Geuther, A. 240. 208.) 2As 2 O 2 S 3 , Na 2 O+7H 2 O. Sol. in H 2 O. (Nilson, J. pr. (2) 14. 14.) Correct composition is Na 8 Asi 8 S 24 O 7 + 30H 2 O. (Preis.) Sodium sulphoxyarsenate, Na 8 Asi 8 S 24 O 7 + 30H 2 O=4Na 2 O, 6As 2 S 2 , 30H 2 O. Decomp. by H 2 O. Sol. in NH 4 OH or KOH +Aq, (Preis, A. 257. 187.) = Sodium oxyin'sulpharsenate of Nilson. Sodium perc/asulphoxytefrarsenate, Nai 2 As 4 S 5 O n +48H 2 O. Less sol. in H 2 O than other sulphoxy- arsenates. (Preis.) Sodium strontium in'sulphoxyarsenate. NaSrAsS 3 O + 10H 2 O. Unstable. (McCay and Foster. Z. anorg. 1904, 41. 462.) 894 SULPHOXYAZOTIC ACID Tn'sulphoxyazotic acid, ON(SO 3 H) 3 . Known only in its salts. (Glaus, A., 158. 52 and 194.) Has the formula (SO 3 H) 3 NN(SO 3 H) 3 . (Raschig, A. 241. 161.) Potassium ^n'sulphoxyazotate, ON(SO 3 K) 3 + H 2 = (S0 3 K) 3 N<>N(S0 3 K) 3 . Easily sol. in H 2 O without decomp., even on boiling. (Claus, A. 167. 210.) Sulphoxyphosphorous acid, H H 3 PS 2 O = OPSH(?). SH See Thiophosphorous acid. Sulphoxyvanadic acid. Ammonium p^/roAezasulphoxyvanadate. (NH 4 ) 4 V 2 S 6 0. Sol. in H 2 O. (Kriiss and Ohnmais, A. 263. 53.) Potassium w/ro/iezasulphoxyvanadate. K 4 V 2 S 6 0+3H 2 0. Melts in crystal H 2 O. (Kriiss and Ohn- mais.) K 8 V 4 Si 2 O 2 +3H 2 O. More sol. in H 2 O than preceding comp; (K. and O.) Sodium or^otfnsulphoxyvanadate. Na 3 VS 3 O +5H 2 O. Ve,ry d,eliquesce,nt, and easily sol. in H 2 O Somewhat sol. in alcohol. (Kriiss and Ohn- mais.) Sodium or^omonosulphoxyvanadate, Na 3 VS9 3 +10H 2 O. Less sol. in H 2 O than other sulphoxyvana- dates. (K. and O.) Sulphur, S. The various modifications of sulphur have been classified in many different ways, and there is a difference of opinion as to whether certain forms are true allotropic modifications or not. The data, as far as concerns the solubility, may be arranged as follows: A. Sol. in CS 2 . 1. Rhombic, octahedral, or alpha sulphur, ordinary sulphur. Easily sol. in CS 2 , etc. See below for solubility in various solvents. 2. Prismatic, monoclinic, or beta sulphur. Sol. in CS 2 , but is converted into A. 1. Pris- matic sulpnur obtained by melting brimstone is not wholly sol. in CS 2 on account of admix- ture of gamma sulphur. Monoclinic modification is more sol. than rhombic in CHC1 3 , ether and benzene. (Meyer C. C. 1903, II. 481.) . 3. Soft sulphur, milk of sulphur. 4. Amorphous sol. sulphur is also a sepa- rate modification, according to Berthollet. B. Soft sulphur, obtained by strongly heating and quickly cooling, is sol. in CS 2 , but becomes insol. therein by repeatedly dis- solving and evaporating. More easily sol. in CS 2 than A, 1. C. Insol. in CS 2 . 1. By action of strong light on S in CS 2 . 2. By heating to b.-pt., cooling suddenly, and allowing to stand until hard. Has been called gamma sulphur, but is a mixture of 2 /3 A, 4 and Vs insol. S. 3. Insol. S in flowers of sujphulr. Con- verted into A. 1 by standing 3 days with alcohol. According to Berthelot (A. ch. (3) 49. 430) there are only two varieties of S.' I. "Octa- hedral," II. "Amorphous." I. Octahedral. Sol. in CS 2 . Scarcely acted upon by KHSO 3 +Aq. Converted by oxidis- ing agents into II. II. Amorphous. Insol. in neutral solvents, viz. H 2 0, alcohol, ether, CS 2 , etc. Sol. with tolerable rapidity in KHSO 3 +Aq. By long action of Na 2 S+Aq, a portion is dissolved, and the remainder converted into I. Less easily oxidised by HNO 3 +Aq than I. Some varieties of this modification are sol. to a certain extent in alcohol and ether, and by boiling the rest of the sulphur is con- verted into I; also by long-continued con- tact with cold alcohol. Berthelot holds that the modification is changed before dissolving. Solutions of the alkalies, alkali salts, and alkali sulphides change insol. into sol. sulphur. (Berthelot.) Elastic sulphur obtained by pouring mol- ten sulphur at a temp, of over 260 into H 2 O contains 35%, or more of a modification of S which is insol. in CS 2 , hot or cold, but sol. in absolute alcohol; this modification can be converted back into ord. sulphur by heat- ing to 100. (Pelouze and Fremy.) (See C. 2.) This modification can be obtained also by action of HC1 on thiosulphates. (Fordos and Ge"lis.) The soft pasty sulphur obtained by decom- position of H 2 S by SO 2 forms an almost clear emulsion (pesudo-solution) with H 2 O, from which it is pptd. by various salts and substances which have no chemical affinity for it. 23 pts. S combine in this way with 100 pts. H 2 O. When pptd. by saline S9lu- tions, some of the S remains in solution. When solution is exposed to the light, S gradually separates out; also on boiling the same takes place. The above pseudo-solu- tion is pptd. by mineral acids, and the pptd. S may still be dissolved in fresh water, if not left in contact for some time with the acid. Also pptd. by K salts, with loss of power of forming pseudo-solutions. Pptd. by NH 4 and Na salts without losing that power. SULPHUR 895 Alkali hydrates, carbonates, or sulphides convert it into insol. S. The solution may be mixed with alcohol without change. Decomp. by long shaking with napthha or oil of turpentine. The pseudo-solution combines with CS 2 , forming an emulsion which subsequently decomposes. The S itself is only partially sol. in CS 2 . (Selmi, J. pr. 57. 49.) By treatment of amorphous "insoluble" S with CS 2 or CC1 4 , a small part goes into solu- tion, the amount being dependent on the time of contact with the temp., and nature of the solvent, but independent of the amount of the solvent. It is assumed that this is due to a partial change of the "insoluble" into soluble S. (Wigand, Z. phys. Ch. 1910, 75. 235.) "Delta" sulphur. Partly sol. in H 2 O. (Debus, Chem. Soc. 63. 18.) A colloidal form wholly sol. in H 2 O exists, which, however, decomposes very easily. (Engel, C. R. 112. 866.) Black sulphur. Insol. in alcohol, ether, CS 2 , fatty oils even at 200, cold alkali hydroxides +Aq, H 2 SO 4 , HN0 3 , or aqua regia. (Knapp, J. pr. (2) 43. 305.) Green modification. Five times more sol. than ordinary sublimed sulphur in a mixture of salicylaldehyde and benzene. (Orloff, C. C. 1902, I. 1264.) The following data relate to octahedral or ordinary sulphur (A. 1): Sol. in warm liquid H 2 S (Niemann); warm P 2 S 3 , SBr 2 , SC1 2 , Br 2 , NC1 3 , BaS+Aq (Dumas); in alcoholic solution of K 2 S 5 , but is repptd. by addition of H 2 O to sat. solu- tion. Sol. in liquid SO 2 . Sol. in aqueous solution of alkali sulphates, especially when hot. SI. sol. in boiling cone. HSCN+Aq, from which it mostly separates on cooling. Na 2 CO 3 +Aq (5.6% Na 2 CO 3 ) dissolves no S at 20; 0.06775% at 100. (Pohl, Dingl. 197. 508.) The solubility 9f S in Na 2 S+Aq between and 50 diminishes slightly with increase in temp., but increases with dilution of the solution, having its largest value in a N/16 solution of Na 2 S-f Aq when the relation of Na 2 S to dissolved S equals about 1 : 4. (Kiis- ter, Z. anorg. 1905, 43. 56.) Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913, 84. 27.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) Sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 822.) Sol. in liquid NH 3 . 1 gr. S is sol. in 3-4 ccm. liquid NH 3 . (Hugot, A. ch. 1900, (7) 21. 32.) The solubility of S in liquid NH 3 is constant from 23 to 84 and equals 39%. (Ruff, Z. angew. Ch. 1910, 23. 1830.) Solubility in liquid NH 3 . (g. S in 100 g. solution.) t S' t S 78 20.5 38.6 38. T 32.34 16.4 30 40 25.65 21.0 18.5 (Ruff and Hecht, Z. anorg. 1911, 70. 62.) SI. sol. in liquid NO 2 . (Frankland, Chem. Soc. 1901, 79. 1361.) S 2 C1 2 dissolves 66.74% S at ord. temp, to form a liquid of 1.7 sp. gr. (Rose.) Solubility of S in S 2 C1 2 varies according to the variety of sulphur used. Aten has pub- lished an extended investigation on the sub- ject, which see for details. (Z. phys. Ch. 1905- 14, 54. 86, 124; 81. 268; 83. 443; 86. 1; 88. 321.) Solubility in SnCl 4 . 100 g. SnCl 4 dissolve at: 99 101 110 110 5.8 6.2 8.7 9.1 pts. solid S, 112 112 121 9.4 9.9 17.0 pts. liquid S. (Gerardin.) Sol. in alkalies +Aq with decomp. Sol. in 1926.7 pts. absolute alcohol at 15. (Pohl, W. A. B. 6. 600.) Sol. in 20 pts. hot nearly absolute alcohol, less sol. in weaker alcohol. (Laurogais.) Sol. in 600 pts. boiling alcohol of 40 B. (Chevallier, J. ch. med. 2. 587); in 500 pts. alcohol (Meissner) ; 200 pts. alcohol (Pelouze and Fremy). 100 pts. absolute alcohol dissolve 0.42 pt. at b.-pt., and 0.12 pt. S at 16; 100 pts. ether dissolve 0.54 pt. at b.-pt., and 0.19 pt. S at 16; 100 pts. benzene dissolve 17.04 pts. at b.-pt., and 1.79 pts. S at 16; 100 pts. oil of turpentine dissolve 16.16 pts. at b.-pt., and 1.35 pts. S at 16; 100 pts. CS 2 dissolve 73.46 pts. at b.-pt., and 38. 70 pts. S at 16; 100 pts. naphtha dissolve 10.56 pts. at b.-pt., and 2.77 pts. S at 16; 100 pts. tar-oil dissolve 26.98 pts. at b.-pt., and 1.51 pts. S at 16. (Payen, C. R. 34. 456.) 100 pts. absolute methyl alcohol dissolve 0.028 pt. at 18.5; 100 pts. absolute ethyl alcohol dissolve 0.053 pt. at 18.5. (de Bruyn, Z. phys. Ch. 10. 781.) Solubility in amyl alcohol. 95 110 110 1.5 2.1 2.2 pts. solid S, 112 112 120 131 2.6 2.7 3.0 5.3 pts. liquid S. (Gerardin, A. ch. (4) 5. 134.) Quickly sol. in 12.5 pts. ether. (Favre.) 100 pts. benzene dissolve 0.965 pt. S at 26; 100 pts. benzene dissolve 4.377 pts. S at 71; 100 pts. toluene dissolve 1.479 pts. S at 23; 100 pts. ethyl ether dissolve 0.972 pt. S at 896 SULPHUR 23.5; 100 pts. chloroform dissolve 1.205 pts. S at 22; 100 pts. phenol dissolve 16.35 pts. S at 174; 100 pts. aniline dissolve 85.27 pts. S at 130. (Cossa, B. 1. 139.) Solubility in benzene at t. 77 84.5 89 116 4.84 4.46 4.29 2.99 g. S. (Arctowski, Z. anorg. 1896, 11. 274.) When 20 pts. S dissolve in 50 pts. CS t g. S in 10 g. of solution 15.17 19.29 0.1480 0.1692 (Bronsted, Z. phys. Ch. 1906, 55. 377.) A mixture of S and toluene separates into two layers, containing 33 and 92.5% S re- spectively. (Haywood, J. phys. Ch. 1897, 1. CS 2 dissolves 0.35 'pt. ordinary sulphur; some varieties of S, however, are not entirely 2.99 g. S are sol. in 100 grams CS 2 at 116. (Arctowski, C. R. 1895, 121. 124.) Solubility in CS 2 . 100 g. of the sat. solution contain at: 22 the temp, is lowered 5. (Cossa.) Sat. solution of S in CS 2 boils at 55. (Cossa.) Sp. gr. of S dissolved in CS 2 at 15. (Pts. S per 100 pts. CS 2 .) sol. in CS 2 , thus Sp. gr. Pts. S Sp. gr. Pts. S Sp. gr. Pts. S Variety of Sulphur 15 ^ ^ W. s'p o. 1.271 1.272 1.273 1.274 1.275 1.276 1.277 1.278 1.279 1.280 1.281 1.282 1.283 1.284 1.285 1.286 1.287 1.288 1.289 1.290 1.291 1.292 1.293 1.294 1.295 1.296 1.297 1.298 1.299 1.300 1.301 1.302 1.303 1.304 1.305 1.306 1.307 1.308 1.309 1.310 1.311 0.0 0.2 0.4 0.6 0.9 1.2 1.4 1.6 1.9 2.1 2.4 2.6 2.9 3.1 3.4 3.6 3.9 4.1 4.4 4.6 4.8 5.1 5.3 5.6 5.8 6.0 6.3 6.5 6.7 7.0 7.2 7.5 7.8 8.0 8.2 8.5 8.7 8.9 9.2 9.4 9.7 1.312 1.313 1.314 1.315 1.316 1.317 1.318 1.319 1.320 1.321 1.322 1.323 1.324 1.325 1.326 1.327 1.328 1.329 1.330 1.331 .332 .333 .334 .335 .336 .337 .338 .339 .340 .341 .342 .343 1.344 1.345 1.346 1.347 1.348 1.349 1.350 1.351 9.9 10.2 10.4 10.6 10.9 11.1 11.3 11.6 11.8 12.1 12.3 12.6 12.8 13.1 13.3 13.5 13.8 14.0 14.2 14.5 14.7 15.0 15.2 15.4 15.6 15.9 16.1 16.4 16.6 16.9 17.1 17.4 17.6 17.9 18.1 18.4 18.6 18.9 19.0 19.3 .352 .353 .354 .355 .356 .357 .358 .359 .360 .361 .362 .363 .364 .365 .366 .367 .368 .369 .370 .371 .372 .373 .374 .375 .376 .377 1.378 1.379 1.380 1.381 1.382 1.383 1.384 1.385 1.386 1.387 1.388 1.389 1.390 1.391 19.6 19.9 20.1 20.4 20.6 21.0 21.2 21.5 21.8 22.1 22.3 22.7 23.0 23.2 23.6 24.0 24.3 24.8 25.1 25.6 26.0 26.5 26.9 27.4 28.1 28.5 29.0 29.7 30.2 30.8 31.4 31.9 32.6 33.2 33.8 34.5 35.2 36.1 36.7 37.2 Octahedral, from Sicily Crystallised in dry way, re- cently prepared Do., prepared 8 years Do., prepared 9 years Do., prepared 15 years . Red needles, recently prepared Soft yellow, do. Do., prepared 2 years Soft red, recently prepared . Do., prepared 5 years Flowers of sulphur Do., another sample Roll brimstone, outside Do., inside 0.335 0.415 0.33 0^382 oisie 0.374 0'351 0.000 0.029 0.004 0.020 0.051 0.023 0.353 0.157 0.157 0.181 0.113 0.234 0.029 0.073 (Deville, A. ch. (3) 47. 99.) The pt. insol. in CS 2 is sol. in hot absolute alcohol, crystallising on cooling; less sol. in chloroform or ether. (Deville.) 100 pts. pure CS 2 dissolve pts. S at t. t Pts. S t Pts. S 11 16.54 22 46.05 - 6 18.75 38 94.57 23.99 48.5 146.21 + 15 37.15 55 181.34 18.5 41.65 (Cossa, B. 1. 138.) Neither ordinary stick S nor flowers of S is completely sol. in CS 2 . Pptd. S is com- pletely sol. in 5 pts. CS 2 . (Tittenger, C. C. 1894, II. 267.) (Mascagno, C. N. 43. 192.) SULPHUR 897 Sp. gr. of S dissolved in CS 2 at 15. Water a Solubility in organic solvents. 4 = 1. Sat. solution Solvent t contains % S Sp. gr. % s Sp. gr. % s Sp. gr. % CS 2 61 3.6 1.2708 1.2717 1.2727 1 . 2792 1.2802 1.2812 1.2822 0.0 0.2 0.4 1.8 2.0 2.2 2.4 1.2736 1.2745 1.2755 1.3096 1.3105 1.3115 1.3125 0.6 0.8 1.0 8.0 8.2 8.4 8.6 1.2764 1.2774 1.2783 1.3409 1.3419 1.3430 1.3440 1.2 1.4 1.6 14.2 14.4 14.6 14.8 55 19 18 17 13 11 11 4.4 10.6 10.8 11.5 12.4 13.3 13.5 1.2832 2.6 1.3135 8.8 1.3450 15.0 2 17.2 1.2842 2.8 1.3145 9.0 1.3460 15.2 + 3 19.5 1.2852 3.0 .3155 9.2 1.3471 15.4 9 23.1 1.2862 3.2 .3165 9.4 1.3481 15.6 11 23.7 1.2872 3.4 .3175 9.6 1.3491 15.8 14 25.9 1.2882 1.2892 3.6 3.8 .3185 .3195 9.8 10.0 1.3502 1.3512 16.0 16.2 17 19 27.2 28.9 1.2901 4.0 .3205 10.2 1.3522 16.4 20 28.5 1.2911 4.2 .3215 10.4 1.3532 16.6 21 29.7 1.2921 4.4 .3226 10.6 1.3543 16.8 26 33.4 1.2930 4.6 .3236 10.8 1.3553 17.0 27 34.6 1.2940 4.8 .3246 11.0 1.3563 17.2 29 37.8 1 . 2949 5.0 .3256 11.2 1.3573 17.4 30.5 39.7 1.2959 5.2 1.3266 11.4 1.3584 17.6 33 42.2 1.2969 5.4 1.3277 11.6 1.3594 17.8 40 48.7 1.2978 5.6 1.3287 11.8 1.3604 18.0 44 53.2 1 . 2988 5.8 1.3297 12.0 1.3615 18.2 46 56.2 1.2998 6.0 1.3307 12.2 1.3625 18.4 48 57.5 1.3008 6.2 1.3317 12.4 1.3635 18.6 53 60.0 1.3017 6.4 1.3328 12.6 1.3646 18.8 54 60.6 1.3027 6.6 1.3338 12.8 1.3656 19.0 65 67.9 1.3037 6.8 1.3348 13.0 1.3667 19.2 77.5 76.4 1.3047 7.0 1 . 3358 13.2 1.3677 19.4 81.0 79.4 1.3056 1 3066 7.2 7 4 1.3368 1 . 3379 13.4 13.6 1.3688 1 3698 19.6 19 8 92.0 98.0 87.8 90.1 1.3076 7.6 1.3389 13^8 L3709 2o!o Ethylene dibromide 9 1.7 1.3086 7.8 1 . 3399 14.0 22 2.4 40 4.4 (Pfeiffer, Z. anorg. 1897, 16. 200.) 50 72 6.'4 12.4 Sol. in acetone. (Eidmann, C. C. 1899, II. 1014.) . 95 108 30.2 60.0 Benzene 8 1.2 10 1.3 21 1.8 Solubility of S in acetone +Aq at 25. 30 2.'e S ==millimols. g. S in 100 cc. of the solution. 39 47 3.3 4r\ A = g. acetone in 100 g. ace tone +Aq. rtl 54 f*K . u 4.9 6Q A s Sp. gr. DO 72 .8 8.6 100 65.0 0.78540 100 123 17.5 Q1 Q 95.36 45.0 0.79114 127 OJ. . t/ 34 90.62 33.0 0.81654 150 Orr . \J 36 8 85.38 25.3 0.82958 OU . o Hexane 20 0.07 (Herz and Knoch, Z. anorg. 1905, 46. 263.) +26 0.16 0.41 +68 1.2 + 130 5.2 + 142 6.2 + 184 8.3 (Etard, A. ch. 1894, (7) 2. 571.) SULPHUR Solubility in CHC1 3 at t. t g. S in 10 g. of solution 12.25 0.0744 19.29 0.0918 (Bronsted, Z. phys. Oh. 1906, 65. 377.) Solubility of octahedral and prismatic S in organic solvents at t. Solvent t % c, pnsmatic b 7 octahedral S Benzene 18.6 25.3 2.004 2.335 1.512 1.835 Chloroform 15.5 40 1.101 1.658 2.9 0.788 1.253 2.4 Ethyl ether 25.3 0.113 0.253 0.080 a. 200 Ethyl bromide 25.3 0.852 1.676 0.611 1.307 Ethyl formate 0.028 0.019 Ethyl alcohol 25.3 0.066 0.052 (Bronsted, Z. phys. Ch. 1906, 55. 377.) Solubility in organic solvents at 25. (G. S dissolved in 1 g. mol. of solvent.) Solvent g. s Ethylene chloride Tetrachlorethane Dichlorethylene Pentachlorethane Trichlorethylene Perchlorethylene Carbon tetrachloride 0.831 2.063 1.237 2.421 2.43 2.537 1 . 354 (Hoffmann et al. 1910, B. 43. 188.) 100 g. trichlorethylene dissolve 1.19 g. S at 15. (Wester and Bruins, Pharm. Weekhl 1914, 51. 1443.) Solubility in benzyl chloride at t. t g. S per 100 g. of solution in upper layer in lower layer 0.99 17 1.78 35 2.57 46.1 3.64 63.3 6.15 78.0 9.88 99.1 19.89 109.6 90.62 114.6 87.99 118.8 37! 29 121.4 40.04 85 .'62 130.0 49.71 80.07 134.2 56.20 72.23 Above 134.2 sulphur is miscible with Benzyl chloride in all proportions; below this ;emp. tAvo layers are formed. (Bogusky, J. Russ. Phys. Chem. Soc. 1905, 37. 92-99; C. C. 1906, I. 1207.) Easily sol. in boiling acetic anhydride. (Rosenfeld, B. 13. 1475.) Sol. in considerable amount in warm cone. HC 2 H 3 O 2 +Aq, but very si. sol. if dil. (Lie- bermann, B. 10. 866.) Sol. in stearic acid+Aq. (Vulpius, Arch. Pharm. (3) 13. 38.) Acetic ether dissolves '6% S. (Favre.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Sol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) SI. sol. in benzonitrile at ord. temp., much more sol. at higher temp. (Naumann, B. 1914, 47. 1369.) Sol. in 12 pts. hot petroleum from Amiano, but nearly insol. in cold, (de Saussure.) 100 pts. nicotine at 100 dissolve 10.58 pts. S, but this separates out as the solution cools. (Kiever, C. C. 1872. 434.) Sol. in warm aniline. (Barral, A. ch. (3) 20. 352.) Easily sol. in hot, less sol. in cold aniline. (Fritzsche.) Very sol. in aniline and quinoline, especially when warm. (Hofmann.) Sol. in quinoline but reacts with the solvent with evolution of H. (Beckmann and Gabel, Z. anorg. 1906, 51. 236.) l /z ccm. oleic acid dissolves 0.0335 g. S in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Sol. in 2.6 pts. of boiling, si. sol. in cold creosote. Sol. by digestion in 2 pts. oil of turpentine. Sol. in hot oil of copaiba, crystallising on cooling. Sol. in hot oil of mandarin, crystallising on cooling. Sol. in hot oil of caraway, crystallising on cooling. Somewhat sol. in hot, less in cold wood- spirit. SI. sol. in lignone, bromoform, cold ben- zene, but easily in hot benzene. (Mansfield, Chem. Soc. 1/262.) Sol. in ethyl sulphide, and carbon chlo- ride. (Rathke, A. 152. 187.) Sol. in mercuric methyl. Sol. in 20 pts. ethyl nitrate, from which is is not pptd. by H 2 O. Sol. in naphtha, aldehyde, ipdal, bromal, chloroform, warm chloral, sinkaline+Aq, ethyl chloride, warm benzoyl chloride. 100 pts. methylene iodide dissolve 10 pts S at 10. Melted sulphur is miscible with hot methylene iodide. (Retgers, Z. anorg 3. 343.) ' S dissolves in 2000 pts. glycerine. (Caj and Garot, J. Pharm. (3) 26. 81.) Glycerine dissolves 0. 10 % S. (Kiever, C. C 1872. 434.) SULPHUR CHLORIDE AMMONIA 899 100 g. glycerine dissolve 0.14 g. at. 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) Sol. in butyl sulphydrate, and warm retin- ole. Sol. in ethyl sulphydrate. Very sol. in coniine, hexyl alcohol, warm allyl sulphocyanide, cacodyl oxide. Some- what sol. in hot styrene, separating out on cooling. Readily sol. in warm, less readily in cold toluene or resin-oil. Sol. in olive oil at 115, from which it mostly separates on cooling. Sol. in hot oil of amber, crystallising upon cooling. Sol. in 2 pts. hot, si. sol. in cold caoutchin. Insol. in yalerianic acid, amyl valerate, valeryl hydride. Linseed oil dissolves % S at t. t % s t %s . t? %s 25 0.630 95 2.587 160 9.129 60 1.852 130 4.935 (Pohl.) Solubility in olive oil (sp. gr. =0.885). 100 pts. dissolve pts. S at t. t Pts. S t Pts. S t Pts. S 15 2.3 65 20.6 110 30.3 40 5.6 100 25.0 130 43.2 (Pelouze, C. H. 68. 1179.) Solubility in 100 pts. coal-tar oil at t. Pts. S in t Oil of 0.870 Oil of 0.880 Oil of 0.882 sp. gr. sp. gr. sp. gr. --!.'':': .iG B.-pt. 80-100 B.-pt. 85 120 B.-pt. 120-200 15 2.1 2.3 2.5 30 3.0 4.0 5.3 50 5.2 6.1 8.3 80 11.8 13.7 15.2 100 15.2 18.7 23.0 110 23.0 26.2 120 27.0 32.0 130 38.7 Pts. S in Oil of 0.885 Oil of 1.010 Oil of 1.020 sp. gr. B.-pt. 150 200 sp. gr. B.-pt. 210300 sp. gr. B.-pt. 220-300 15 2.6 6.0 7.0 30 5.8 8.5 8.5 50 8.7 10.0 12.0 80 21.0 37.0 41.0 100 26.4 52.5 "54.0 110 31.0 105.0 115.0 120 38.0 00 oo 130 43.8 00 00 (Pelouze, C. R. 69. 56.) Sulphur bromide, S 2 Br 2 . Decomp. gradually with H 2 O. Dissolves S on warming, which crystallises out on cooling. Sol. in CS 2 . Decomp. by current of dry air into S and Br. (Hannay, Chem. Soc. 36. 16.) Decomp. slowly by cold H 2 O, rapidly by hot H 2 O. Decomp. by dil. KOH+Aq or NaHCO 3 +Aq. (Korndorfer, Arch. Pharm. 1904, 242. 156.) A study of the mpt. curve of a series of mixtures of sulphur and bromine gave no evidence for the existence of the compounds SBr 2 and SBr 4 . (Ruff, B. 1903, 36. 2446.) Sulphur racwochloride, S 2 C1 2 . Slowly decomp. by H 2 O. Miscible with CS 2 and C 6 H 6 . Sol. in alcohol and ether with subsequent decomposition. Sol. in oil of tur- pentine. Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Sol. in CC1 4 , and C 6 H 6 . (Oddo, Gazz. ch. it. 1899, 29. (2) 318.) Sulphur ^'chloride, SC1 2 . Decomp. slowly with H 2 O, immediately by alcohol or ether. Sulphur tefrachloride, SC1 4 . Violently decomp. by H 2 O. Decomp. at temperatures above 22. (Michaelis, A. 170. 1.) Sulphur stannic chloride, 2SC1 4 , SnCl 4 . Decomp. by H 2 O. Sol. in dil. HNO 3 +Aq. Forms a mass with fuming HNO 3 which is sol. in HNO 3 +Aq. Sol. in POC1 3 . (Cassel- mann.) Very hydroscppic. Fumes in moist air. Very easily sol. in dry abs. ether and in ben- zene. Sol. in.CHCla, SO 2 C1 2 , CS 2 , POC1 3 ligroin and petroleum ether. (Ruff, B. 1904, 37. 4517.) Sulphur titanium chloride, SC1 4 , 2TiCl 4 . Very deliquescent. Easily sol. in dil. HNOs+Aq. (Weber, Pogg. 132. 454.) SC1 4 , TiCl 4 . Sol. in SO 2 C1 2 , CHC1 3 , CS 2 and petroleum ether. (Ruff, B. 1904, 37. 4516.) Sulphur chloride ammonia, S 2 C1 2 , 4NH 3 . Insol. in H 2 O, but gradually decomp. thereby; sol. without decomp. in absolute alcohol, from which it is pptd. by H 2 O. (Mertens.) Does not exist. (Fordos and Gelis, C. R. 31. 702.) SC1 2 , 2NH 3 . Decomp. by H 2 O. Sol. in alcohol or ether. (Soubeiran, A. ch. 67. 71.) Not a true chemical compound, but a mixture. (Fordos and Gelis, C. R. 31. 702.) 900 SULPHUR CHLORIDE NITROGEN SULPHIDE SC1 2 , 4NH 3 . Decomp. by H 2 O. SI. sol. in absolute alcohol and ether (Soubeiran, A. ch. 67. 71); mixture (Fordos and Gelis). Sulphur chloride nitrogen sulphide. See Nitrogen sulphochloride. Sulphur perfluoride, SF 6 . Very si. sol. in H 2 O; si. sol. in (Moissan, C. R. 1900, 130. 868.) alcohol. Sulphur monoiodide, S 2 l2. Insol. in H 2 O. Decomp. by alcohol, which dissolves out I 2 . SI. sol. in cold caoutchin, the solution decomposing when boiled. Freely sol. in glycerine. Sol. in 60 pts. glycerine, and 82 pts. olive oil. (Cap and Garot, J. Pharm. (3) 26. 81.) Very sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Sol. in CS 2 . (Linebarger, Am. Ch. J. 1895, 17. 58.) Sulphur Aeododide, SI 6 . Decomp. on air. Alcohol or alkalies dis- solve out iodine, (vom Rath, Pogg. 110. 116.) Does not exist. (M'Leod, Rep. Brit. Assn. Advn. Sci. 1892. 690.) Sulphur stannic iodide. See Tin sulphur iodide. Sulphur sesgwioxide, S 2 O 3 . Deliquescent. Violently decomp. by H 2 at ordinary temp. Sol. in fuming H 2 SO 4 . In- sol. in SO 3 . Decomp. by alcohol or other. (Weber, Pogg. 166. 531.) Sulphur dioxide, SO 2 . Liquid. Insol. in H 2 O if brought in con- tact therewith below the b.-pt. of S0 2 . Sol. in 3 yols. CS 2 on warming, separating out on cooling. Dissolves some P, little S, and no sulphuric or phosphoric acids. Dissolves ether, chloroform, P, Br, S, I, CS 2 , colophonium, and other gums; also benzene when warmed. (Sestini, Bull. Soc. (2) 10. 226.) Miscible with liquid SO 3 , but not with H 2 S0 4 . Gas. 1 vol. H 2 O absorbs 30 vols. SO 2 gas at 18 (Davy) ; 20 vols. at ord. temp. (Dalton) ; 43.78 vols. at ord. temp, (de Saussure) ; 50 vols. at 20 and 760 mm. (Pelouze and Fremy) ; 33 vols. at ord. temp. (Thomson) . 1 pt. SO 2 (by wtight) is sol. in 0.1429 pt. H 2 O at 5, and the solution has 1.020 sp. gr. 1 pt. SO i is sol. in 0.0400 pt. H 2 O at ord. temp. (Priestley) ; in 0.0909 pt. H O at 16, and sp. gr. of the solution = 1.05 13 (Thomson). Sol. in 2 pts. HiO at 10. (Pierre, A. ch. (3) 23. 421.) 100 vols. H 2 O at 18 and 760 mm. absorb 4378 vols. SO 2 gas; 100 vols. alcohol of 0.84 sp. gr. at 760 mm. absorb 11,577 vols. (de Saussure, 1814.) Solubility of SO 2 gas in H 2 O. t = temp. ; V = vols. SO 2 reduced to and 760 mm. con- tained in 1 vol. sat. SO 2 +Aq; Vi=vols. SO 2 gas reduced to and 760 mm. dis- solved by 1 vol. H 2 O under 760 mm. pres- sure. t V Vi t V Vi 68.861 79.789 21 34.986 37.970 1 67.003 77.210 22 33.910 36.617 2 65.169 74.691 23 32.847 35.302 3 63.360 72.230 24 31.800 34.026 4 61.576 69.828 25 30.766 32.786 5 59.816 67.485 26 29.748 31.584 6 58.080 65.200 27 28.744 30.422 7 56.369 62.973 28 27.754 29.314 8 54.683 60.805 29 26.788 28.210 9 53.021 58.697 30 25.819 27.161 10 51.383 56.647 31 24.873 26.151 11 49.770 54 . 655 32 23.942 25.178 12 48.182 52.723 33 23.025 24.244 13 46.618 50.849 34 22.122 23 . 347 14 45.079 49.033 35 21.234 22.489 15 43.564 47.276 36 20.361 21.668 16 42.073 45.578 37 19.502 20.886 17 40.608 43 . 939 38 18.658 20.141 18 39.165 42.360 39 17.827 19.435 19 37 . 749 40.838 40 17.013 18.766 20 36.206 39.374 (Schonfeld, A. 96. 5.) This table may be formulated as follows: 1 vol. H 2 O absorbs 79. 789-2. 6077t+ 0.029349t 2 vols. SO 2 at temp, between and 20, or 1 vol. sat. solution contains 68.861 1.87025t+0.01225t 2 vols. SO 2 . Coefficient of absorption between 21 and 40 = 75. 182 2.1716t+0.01903t 2 vols. SO 2 or 1 vol. sat. solution between 21 and 40 contains 60.952 1.38898t+0.00726t 2 vols. SO 2 . Solubility of SO 2 in H 2 O at various temps, and 760 mm. t = temp.; G = grammes SO 2 dissolved in 1 g. H 2 O; V = vols. SO 2 dis- solved in 1 g. H 2 O. t G V t G V 8 0.168 58.7 30 0.078 27.3 10 0.154 53.9 32 0.073 25.7 12 0.142 49.6 34 0.069 24.3 14 0.130 45.6 36 0.065 22.8 16 0.121 42.2 38 0.062 21.6 18 0.112 39.3 40 0.058 20.4 20 0.104 36.4 42 0.055 19.3 22 0.098 34.2 44 0'.053 18.4 24 0.092 32.3 46 0.050 17.4 26 0.087 30.5 48 0.047 16.4 28 0.083 28.9 50 0.045 15.6 (Sims, A. 118. 340.) SULPHUR OXIDE 901 Solubility of SO 2 in H 2 O at various pressures. P = "partial pressure," i.e. the total pres- sure minus the tension of aqueous vapour at given temp.; G at P = weight SO 2 in grammes, which is dissolved in 1 g. H 2 O .at pressure P; G at 760 = calculated weight SO 2 that would be contained in 1 g. H 2 O at 760 mm. if the absorption were proportional to the pressure; V = the volume of G grammes of SO 2 at and 760 mm. P 7 GatP G at 760 VatP V at 760 30 0.010 0.263 3.634 92.06 40 0.013 0.242 4.451 84.55 50 0.015 0.223 5.129 77.95 60 0.017 0.818 6.024 76.28 70 0.020 0.213 6.868 74.55 80 0.022 0.210 7.743 73.55 90 0.025 0.208 8.598 72.62 100 0.027 0.205 9.421 71.60 120 0.032 0.201 11.09 70.20 140 0.036 0.197 12.71 69.00 160 0.041 0.195 14.34 68.15 180 0.046 0.193 15.97 67.40 200 0.050 0.191 17.59 66.83 220 0.055 0.190 19.19 66.30 240 0.059 0.188 20.79 65.84 260 0.064 0.187 22.40 65.44 280 0.069 0.186 23.99 65.10 300 0.073 0.185 25.59 64.81 350 0.085 0.184 29.55 64.16 400 0.096 0.182 33.51 63.65 450 0.107 0.181 37.44 63.25 500 0.118 0.180 41.42 62.94 550 0.130 0.179 45.31 62.60 600 0.141 0.178 49.20 62.32 650 0.152 0.178 53.10 62.09 700 0.163 0.177 56.98 61.86 750 0.174 0.176 60.88 61.69 760 0.176 0.176 61.65 61.65 800 0.185 0.176 64.74 61.50 850 0.196 0.175 68.57 61.30 900 0.207 0.175 72 .41 61.15 950 0.218 0.175 76.25 61.00 1000 0.229 0.174 80.01 60.88 1050 0.240 0.174 83.97 60.77 1100 0.251 0.174 87.80 60.65 1200 0.273 0.173 95.45 60.45 1300 0.295 0.172 103.00 60.25 20 P GatP G at 760 Vat P V at 760 40 0.007 0.143 2.637 50.09 50 0.009 0.138 3.171 48.20 60 0.011 0.135 3.718 47.10 70 0.012 0.131 4.205 45.64 80 0.013 0.127 4.663 44.30 90 0.015 0.125 5.169 43.65 100 0.016 0.124 5.692 43.25 120 0.019 0.121 6.683 42.33 140 0.022 0.119 7.690 41.75 160 0.025 0.118 8.666 41.17 180 0.028 0.117 9.652 40.75 200 0.030 0.116 10.62 40.35 220 0.033 0.115 11.59 40.03 240 0.036 0.114 12.54 39.70 260 0.038 0.112 13.45 39.30 280 0.041 0.112 14.41 39.10 300 0.044 0.111 15.34 38.87 350 0.050 0.110 17.66 38.35 400 0.059 0.109 20.56 38.10 450 0.064 0.108 22.37 37.77 500 0.071 0.107 24.67 37.50 550 0.077 0.106 26.93 37.20 600 0.083 0.105 29.14 36.90 650 0.090 0.105 31,39 36.70 700 0.096 0.105 33.62 36.50 750 0.103 0.104 35.94 36.43 760 0.104 . 0.104 36.43 36.43 800 0.110 0.104 38.32 36.40 1000 0.137 0.104 47.85 36.37 1300 0.178 0.104 62.10 36.31 1600 0.218 0.104 76.35 36.27 1900 0.259 0.104 90.53 36.21 39.8 P G at P G at 760 Vat P V at 760 200 0.016 0.062 5.675 21.57 300 0.024 0.061 8.368 21.20 400 0.031 0.060 11.03 20.95 500 0.039 0.059 13.67 20.77 600 0.047 0.059 16.29 20.64 760 0.059 0.059 20.50 20.50 800 0.062 0.059 21.58 20.50 1000 0.077 0.058 26.84 20.40 1500 0.113 0.057 39.65 20.09 2000 0.149 0.057 52.11 19.80 50 P GatP G at 760 VatP V at 760 200 0.012 0.045 4.156 15.97 400 0.024 0.015 8.275 15.72 600 0.035 0.045 12.36 15.65 760 0.045 0.045 15.62 15.62 800 0.047 0.045 16.43 15.60 1000 0.059 0.045 20.51 15.59 1500 0.088 0.044 30.73 15.57 2000 0.012 0.044 39.07 15.55 (Sims? A. 118.340.) 902 SULPHUR OXIDE 1 g. H 2 O dissolves 0.0909 g. SO 2 = 34.73 cc. (at 25) at 25 and 748 mm. pressure. (Wai- den and Centnerszwer, Z. phys. Ch. 1901, 42. 462.) Solubility of SO 2 in H 2 O at t and 760 mm. pressure. Sp. gr. of SOa+Aqat 4. & Sp. gr. % S0 2 Sp. gr. & Sp. gr. \ 2 3 4 5 6 7 1.0024 1 . 0049 1.0075 1.0102 1.0130 1.0158 1.0187 8 9 10 11 12 13 14 1.0217 1.0247 1.0278 1.0311 1.0343 1.0376 1.0410 15 16 17 18 19 20 21 1.0445 1.0480 1.0517 1.0553 1.0591 1.0629 1.0667 t G. SO2 per 1 g. H 2 t G. S0 2 per 1 g. H 2 2 4 6 0.236 0.218 0.201 0.184 7 8 10 12 0.176 0.168 0.154 0.142 (Schiff, calculated by Gerlach, Z. anal. 8. 292.) (Roozeboom, R. t. c. 1884, 3. 29.) From a gas containing 10% by vol. of SO 2 at 10 1.63% by wt. is dissolved by 1 litre of H 2 O; if the pressure is increased to 5 at- mospheres, 8.14% by wt. is dissolved. (Harpf, Chem. Zeitschr., 1905, 4. 136.) Solubility of SO 2 in H 2 O at t. C = g. SO 2 in 1 cc. of the solution. P = Pressure in mm. of Hg. t C p |xW 0.000537 0.00237 0.01227 0.03894 0.4 3.5 29.4 109.4 13.4 6.78 4.17 3.48 25 0.000534 0.00234 0.01212 0.03750 1.4 11.75 87.9 313.0 3.81 2.00 1.379 1.198 50 u (I a 0.000525 0.002276 0.01181 0.03628 4.9 30.5 204.5 696.0 1.07 0.746 0.577 0.521 (Lindner, M. 1912, 33. 645.) Sp. gr. of sat. solution at 10 20 40 1.06091 1.05472 1.02386 0.95548 (Bunsen and Schonfeld, A. 95. 2.) Sat. S0 2 +Aq has sp. gr. = 1.0040. (Ber- thollet.) Sp. gr. of sat. SO 2 +Aq at t. t Sp. gr. t Sp. gr. t Sp. gr. 1.0809 9 .0548 17 1.0358 1 1.0596 10 .0547 18 .0321 2 1.0585 11 .0528 19 .0281 3 1.0576 12 .0505 20 .0239 4 1.0569 13 .0481 21 .0195 5 1.0562 14 .0454 22 1.0147 6 1.0557 15 .0424 23 1.0099 7 1.0552 16 .0392 24 0.9991 8 1.0549 Sp. gr. of SO 2 +Aq. (Schiff, A. 107. 312.) %S0 2 Temp. Sp. gr. 0.99 2.05 2.87 4.04 . 4.99 5.89 7.01 8.08 8.68 9.80 10.75 11.65 13.09 15.5 12.5 11.0 1.0051 .0102 .0148 .0204 .0252 .0297 .0353 .0399 .0438 .0492 .0541 .0597 1.0668 (Giles and Schearer, Jour. Soc. Ch. Ind. 4. 303.) Sp. gr. of SO 2 +Aq. % S0 2 Sp. gr. & Sp. gr. s% 2 S P- gr - 1 2 3 1.0052 1.0094 1.0134 4 5 6 1.0167 1.0208 1.0242 7 1.0283 8 1.0329 9 1.0402 (Anthon.) Sp. gr. of SO 2 +Aq. s 7 6, Sp. gr. % SO 2 Sp. gr. & Sp.g, 1 2 3 4 1.0042 1.0083 1.0125 1.0167 5 ; 1.0210 1.0252 1.0295 8 1.0348 9 1.0392 10 1 . 0438 (Hager, Adjumenta varia, Leipzig, 1876. 146.) SULPHUR OXIDE 903 Sp. gr. of SO 2 +Aq at 15. Solubility of SO 2 in H 2 SO 4 of 1.84 sp. gr. s 7 6, Sp. gr. s^ Sp. gr. $,. Sp. gr. t fll a^, a CO O'o GO all d& 6 i ife t III 1 . OU 82.00 910 SULPHURIC ACID Sp. gr. of H 2 SO 4 , etc. Continued. Sp. gr. of cone. H2SO4, etc. Continued. M % /o % % H 2 S0 4 Sp. gr. % H 2 S0 4 Sp. gr. Sp. gr. SO 3 TT G(~), Sp. gr. SOa H 2 SO.j 95.61 1.8414 93.32 1.8352 .760 67.30 82.44 1.829 75.03 91.90 95.55 1.8413 93.29 1.8351 .765 67.65 82.88 .830 75.19 92.10 95.50 1.8412 93.26 1.8350 .770 68.02 83.32 .831 75.35 92.30 95.45 1.8411 93.23 1.8349 .775 68.49 83.90 .832 75.53 92.52 95.40 1.8410 93.20 1.8348 .780 68.98 84.50 .833 75.72 92.75 95.35' 1.8409 93.17 1.8347 .785 69.74 85.10 .834 75.96 93.05 95.30 1.8408 93.14 1 . 8346 .790 69.96 85.70 .835 76.27 93.43 95.25 1.8407 93.12 1.8345 .795 70.45 86.30 .836 76.57 93.80 95.21 1.8406 93.09 1.8344 .800 70.94 86.90 .837 76.90 94.20 95.16 1.8405 93.06 1.8343 .805 71.50 87.60 .838 77.23 94.60 95.12 1.8404 93.00 1.8342 .810 72.08 88.30 .839 77.55 95.00 95.08 1.8403 92.98 1.8341 .815 72.69 89.05 .840 78.04 95.60 95.04 1.8402 92.95 1.83o9 .820 73.51 90.05 .8405 78.33 95.95 95.00 1.8101 92.93 1 . 8338 .821 73.63 9.0.20 .8415 79.19 97.00 94.96 1.8400 92.90 1.8337 .822 73.80 90.40 .8410 79.76 97.70 94.92 1.8399 92.87 1.8336 .823 73.96 90.60 .8415 80.16 98.20 94.88 1.8398 92.84 1.8335 .824 74.12 90.80 .8400 80.57 98.70 94.84 1.8397 92.82 1.8334 .825 74.29 91.00 .8400 80.98 99.20 94.81 1.8396 92.79 1.8333 1.826 74.49 91.25 .8395 81.18 99.45 94.77 1.8395 92.77 1.8332 1.827 74.69 91.50 .8390 81.39' 99.70 94.73 1.8394 92.73 1.8331 1.828 74.86 91.70 .8385 81.59 99.95 94.69 r\A t* rr 1.8393 Ioono 92.71 1.8330 1O OOA (Lunge and Isler, Zeit. angew. Ch. 9. 129.) y4.oo 94.61 .8392 1.8391 92^66 . 83^9 1.8328 94.57 1.8390 92.63 1.8327 Sp. gr. of cone. [2804+ Aq at 15. 94.53 94.49 1.8389 1.8388 92.61 92.59 1.8326 1 . 8325 % H 2 SO 4 Sp. gr. % H 2 S0 4 Sp. gr. 94.46 1.8387 92.56 1.8324 Q4. 40 1 OOO! QO P\4. 1 OQOQ 100 1.8384 99.02 1.8417 CJT: . T:^J 94.38 1^8385 92^52 J. . oO^SO 1.8322 99.98 1.8385 98.98 1.8418 94.34 1.8384 92.49 1.8321 99.96 1.8386 98.94 1.8419 94.31 1.8383 92.46 1 . 8320 99.94 1.8387 98.84 1.8420 94.27 1.8382 92.44 1.8319 99.92 1.8388 98.84 1.8421 94.24 1.8381 92.41 1.8318 99.90 1.8389 98.78 1.8422 94.20 1.8380 92.39 1.8317 99.88 1.8390 98.71 1.8423 94.17 1.8379 92.37 1.8316 99.86 1.8391 98.63 .8424 94.13 1.8378 92.34 1.8315 99.84 1.8392 98.56 .8425 94.10 1.8377 92.32 1.8314 99.81 1.8393 98.48 .8426 94.07 1 . 8376 92.29 1.8313 99.78 1.8394 98.40 .8427 94.03 1.8375 92.27 1.8312 99.76 1.8395 98.32 .8428 94.00 1.8374 92.24 1.8311 99.73 1.8396 98.22 .8429 93.97 1.8373 92.22 1.8310 99.70 1.8397 98.08 .8430 93.93 1.8372 92.19 1.8309 99.67 1.8398 97.85 .8431 93.90 1.8371 92.17 1.8308 99.64 1.8399 97.50 .8432 93.87 1.8370 92.15 1.8307 99.61 .8400 97.10 .8431 93.83 .8369 92.12 1.8306 95.58 .8401 96.93 1.8430 93.80 .8368 92.10 1.8305 99.55 .8402 96.76 1.8429 93.77 .8367 92.07 1.8304 99.52 .8403 93.65 1.8428 93.74 .8366 92.05 1 . 8303 99.49 .8404 96.55 1.8427 93.71 .8365 92.02 1.8302 99.46 .8405 96.46 .8426 93.68 .8364 92.00 .8301 99.43 1.8406 96.39 .8425 93.65 .8363 91.98 .8300 99.40 1.8407 96.31 .8424 93.62 .8362 91.95 .8299 99.37 1.8408 96.24 .8423 93.59 .8361 91.93 .8298 99.33 1.8409 96.16 .8422 93.56 .8360 91.91 1.8297 99.29 1.8410 96.09 .8421 93.53 .8359 91.88 1.8296 99.25 1.8411 98.02 .8420 93.50 .8358 91.86 1.8295 99.22 1.8412 95.95 .8419 93.47 1.8357 91.84 1.8294 99.19 1.8413 95.88 .8418 93.44 1.8356 91.81 1 . 8293 99.16 1.8414 95.81 .8417 93.41 1.8355 91.78 1 . 8292 99.11 1.8415 95.74 .8416 93.38 1.8354 91.76 1 . 8291 99.06 1.8416 95.67 .8415 93.35 1.8353 91.74 1.8290 SULPHURIC ACID 911 Sp. gr. of cone. H 2 SO 4 , etc. Continued. % H 2 S0 4 Sp. gr. % H 2 SO 4 Sp. gr. 91.72 .8298 90.78 1.8244 91.70 .8288 90.76 1.8243 91.68 .8287 90.74 1.8242 91.65 .8286 90.72 1.8241 91.63 .8285 90.70 1.8240 91.61 .8284 90.68 1.8239 91.59 .8283 90.66 1.8238 91.56 1 . 8282 90.64 1.8237 91.54 1.8281 90.62 1.8236 91.52 1.8280 90.60 1.8235 91.50 1.8279 90.59 1.8234 91.47 1.8278 90.57 1.8233 91.45 1.8277 90.55 1.8232 91.43 1.8276 90.53 1.8231 91.41 1.8275 90.51 1.8230 91.39 1.8274 90.49 1.8229 91.37 1.8273 90.47 1.8228 91.35 1.8272 90.46 1.8227 91.32 1.8271 90.44 1.8226 91.30 1.8270 90.42 1.8225 91.28 1.8269 90.40 .8224 91.26 1.8268 90.38 .8223 91.24 1.8267 90.37 .8222 91.22 1.8266 90.35 .8221 91.20 1.8265 90.33 .8220 91.18 1 . 8264 90.31 .8219 91.16 1.8263 90.29 .8218 91 . 14 1.8262 90.28 .8217 91.12 .8261 90.26 .8216 91'. 10 .8260 90.24 .8215 91.08 .8259 90.23 .8214 91.06 .8258 90.20 .8213 91-04 .8257 90.18 .8212 91.02 .8256 90.17 .8211 91.00 .8255 90.15 .8210 90.98 .8254 90.13 .8209 90.96 .8253 90.11 .8208 90.94 1 . 8252 90.10 .8207 90.92 1.8251 90.08 1.8206 90.90 1.8250 90.06 1.8205 90.88 1.8249 90.04 1.8204 90.86 1.8248 90.02 1.8203 90.84 1.8247 90.01 1.8202 90.82 1.8246 89.99 1.8201 90.80 1.8245 89.97 1.8200 (Richmond [calculated from Pickering, Chein Soc. 57. 64], Jour. Soc. Ch. Ind. 9. 479.) Sp. gr. of cone. H 2 SO 4 +Aq at 15 HsS0 4 90 *90.20 91 91.48 92 *92.83 93 94 *94.84 95 *95.97 Sp. gr. 1.8185 1.8195 1.8241 1.8271 1.8294 1.8334 1.8339 1.8372 1.8387 1.8390 1.8406 96 97 *97.70 98 *98.39 *98.66 99 *99.47 100 * 100. 35 Sp. gr. 1.8406 1.8410 1.8413 1.8412 1.8406 1.8409 1.8403 1.8395 1.8384 1.8411 *Determined by experiment. (Lunge and Naef, Dingl. 248. 91.) Sp. gr. of H 2 SO 4 +Aq at room temp, con- taining : 7 . 875 15 . 503 23 . 429% H 2 SO 4 1.0651 1.1305 1.2003 (Wagner, W. Ann. 1883, 18. 265). Sp. gr. of H 2 SO 4 +Aq at 25. Concentration of HzSCh+Aq 1 normal V 2 " V4- " Sp. gr. 1.0303 1.0154 1.0074 1.0035 (Wagner, Z. phys. Ch. 1890, 5. 40.) Sp. gr. of dil. H 2 SO 4 +Aq. G. -equivalents H 2 SO 4 per liter t Sp. gr. t/t 0.005049 0.01009 0.01512 0.02014 0.03014 17.343 17.360 17.382 17.398 17.419 1 . 0002082 1.0004020 1 . 0005879 1.000769 1.001125 0.002526 0.005050 0.01006 0.02005 0.03001 0.04980 0.09864 0.146560 0.19354 0.28942 0.47466 18.039 18.040 18.040 18.040 18.039 18.040 18.048 18.070 18.080 18.052 18.055 1.0001065 1.0002084 1.0004009 1.0007668 1.0011208 1.0018096 1.003460 1.005045 1.008580 1.009686 1.015616 0.4980 4.980 17.73 17.95 1.01634 1 . 15234 0.005176 0.01035 0.01551 0.12648 0.25151 0.37672 0.50503 12.997 13.020 13.005 ' 13.031 13.011 13.007 12.998 1.0002106 1.000411 1 . 000603 1.004438 1 . 008565 1 . 012639 1.016758 (Kohlrausch, W. Ann. 1894, 53. 28.) 912 SULPHURIC ACID Sp.gr. of H 2 SO 4 +Aq. Crf TJ Of\ *?n co an no oe TT Sp. gr. of fuming H 2 SO 4 at 35. 70 -"-2> Sp.gr 3V_/ 4 /.UO UU.O OU./ / . 20/20 1.7383 1.5181 1.2719 Total Free SO 3% Sp. gr. Total SO., % Free Sp. gr. % Hoi in in A Tfi /O LJ " k Sp. gr . 20/20 1.0685 1.0317 81.63 1.8186 91.1* J 52 1.9749 (Le Blanc and Rohland, Z. phys. Ch. 1896 81.99 2 1.8270 91. 5f ) 54 1.9760 19.268.) 82.36 4 1.8360 91.91 [ 56 1.9772 Sp. gr of N-H 2 SO 4 +Aq at 18/4 = 1.0306 82.73 6 1.8425 92. 2 J 58 1.9754 (Loomis, W. Ann. 1896, 60. 550,.) 83.09 8 1.8498 92. 6 i 60 1.9738 Sp. gr. of H 2 SO 4 +Aq at 19.4, when p = percent strength of solution; d = observec density; w = volume cone, in grams pei / \ 83.46 83.82 84.20 84.56 10 12 14 16 1.8565 1.8627 1.8692 1.8756 93. OS 93. 3 93. 7 94.11 J 62 5 64 > 66 68 1.9709 1.9672 1.9636 1.9600 ft / P i 84.92 18 1.8830 94. 4 > 70 1.9564 L> c \Too~ / 85.30 20 1.8919 94. 8 72 1.9502 P d w 85.66 86.03 22 24 1 . 9020 1.9092 95.21 95.55 74 76 1 . 9442 1.9379 94.10 84.59 73.08 61.35 40.72 31.94 23.77 14.72 9.802 . 4.826 .8380 .7998 .6743 .5341 .3220 .2430 .1747 .1023 .0670 .0320 1.7295 1 . 5223 1.2235 0.9412 0.5383 0.3970 0.2792 0.1623 0.1046 0.0498 86.40 86.76 87.14 87.50 87.87 88.24 88.60 88.97 89.33 89.70 90.07 26 28 30 32 34 36 38 40 42 44 46 1.9158 1 . 9220 1 . 9280 1.9338 1 . 9405 1 . 9474 1.9534 1.9584 1.9612 1 . 9643 1 . 9672 95.95 96.32 96.69 97.05 97.42 97.78 98.16 98.53 98.90 99.26 99.63 78 80 82 84 86 88 90 92 94 96 98 1.9315 1.9251 1.9183 1.9115 1.9046 1.8980 1.8888 1.8800 1.8712 1.8605 1.8488 (Barnes, J. Phys . Chem. 1898, 2. 546. 90.44 48 1 . 9702 100.00 100 1.8370 Sp. gr. of H 2 SO 4 +Aq at 20. 90.81 50 1 . 9733 Normality of H 2 S0 4 +Aq % H 2 S0 4 Sp. gr. (Knietsch, B. 1901, 34. 4101.) 11 53 70.07 .6129 Sp. gr. of H 2 SO 4 +Aq at 15/15 in air. 9 01 59.26 .4901 Sp. gr. % H 2 SO 4 Sp. gr % H 2 S0 4 Sp. gr. % H 2 S0 4 6 95 i y . lu .3872 4 77 36^68 . .2756 1.000 0.00 1.028 4.12 1.056 8.19 3 008 25.00 .1791 1.001 0.15 1.029 4.26 1.057 8.33 1 002 9.25 .0612 1.002 0.31 1.030 4.41 1.058 8.47 (Forchheimer, Z. phys. Ch. 1900, 34. 27.) 1.003 1.004 0.46 0.60 1.031 1.032 4.56 4.70 1 . 05 1.060 8.62 8.76 Sp. gr. of cone, and fuming H 2 SO 4 at 15 and 45 1.005 0.73 .033 4.85 1.031 8.90 1.006 0.87 .034 5.00 1.052 9.04 H 2 S0 4 SO 3 % 90.% Sp. gr. at- 15 Sp. gr. at 45 1.007 1.01 .035 5.14 .063 9.18 Inno 11 c fT OQ 95.98 78.35 1.8418 . UUo 1.009 . 1O 1.30 .'037 5'44 .'065 9.'47 96.68 78.92 1.8429 1.010 1.45 .038 5.58 .066 9.61 96.99 79.18 1.8431 1.011 1.60 .039 5.73 .087 9.75 97.66 79.72 1 . 8434 ma? C. ... 1.012 1.75 .040 5.88 1.068 9.89 98.65 80.53 1.8403 1.013 1.89 .041 6.03 1.069 10.04 99.40 81.14 1.8388 mir I. ... 1.014 2.04 .042 6.17 1.070 10.18 99.76 81.44 1.8418 1.015 2.19 .043 6.32 1.071 10.31 100.00 81.63 o.'o 1.8500 '.822 1.016 2.34 1.044 6.46 1.072 10.45 83.46 10.0 1.888 .858 1.017 2.49 1.045 6.60 1.073 10.59 85.30 20.0 1.920 .887 1.018 2.64 1.046 6.75 1.074 10.73 87.14 30.0 1.957 .920 1.019 2.79 1.047 6.89 1.075 10.87 88.97 40.0 1.979 .945 1.020 2.93 1.048 7.04 1.076 11.00 90.81 50.0 2.009 . 964 max. 1.021 3.08 1.049 7.18 1.077 11.14 92.65 60.0 2.020 max. 1.950 1.022 3.23 1.050 7.32 1.078 11.28 94.48 70.0 2.018 1.942 1.023 3.38 1.051 7.47 1.079 11.42 96.32 80.0 2.008 1.890 1.024 3.53 1.052 7.61 1.080 11.56 98.16 90.0 1.990 1.864 1.025 3.67 1.053 7.76 1.081 11.69 100.00 LOO.O 1.984 1.814 1.026 3.82 1.054 7.90 1.082 11.83 097 3 Q7 f\f pr 8.04 1 083 1 1 Q7 (Knietsch, B 1901, 34. 4102.) . \jt I *-> . t/ ' SULPHURIC ACID 913 Sp. gr. of H 2 SO 4 +Aq at 15/15 in air. Continued. Sp. gr. of H 2 SO 4 +Aq at 15/15 in air Continued. Sp.gr % H 2 S0 4 Sp.gr % H 2 S0 4 Sp. gn % H 2 S0 4 Sp.gr % H 2 S0 4 Sp.gr % H 2 SO 4 Sp.gr % H 2 S0 4 1.084 12.11 1.145 20.25 1.206 27.95 1.267 35.33 1.328 42.35 1.389 48.92 .085 12.24 1.146 20.38 1.207 28.08 1.268 35.45 1.329 42.46 1.390 49.02 .086 12.38 1.147 20.51 1.208 28.20 1.269 35.57 1.330 42.57 1.391 49.13 .087 12.52 1.148 20.64 1.209 28.32 1.270 35.68 .331 42.68 1.392 49.23 .088 12.66 1.149 20.77 1.210 28.45 1.271 35.80 .332 42.79 1.393 49.34 .089 12.79 1.150 20.90 1.211 28.57 .272 35.92 .333 42.90 1.394 49.44 1.090 12.93 1.151 21.03 1.212 28.69 .273 36.04 .334 43.01 1.395 49.54 1.091 13.07 1.152 21.16 1.213 28.82 .274 36.15 .335 43.12 1.396 49.65 1.092 13.20 1.153 21.28 1.214 28.94 .275 36.27 .336 43.23 1.397 49.75 1.093 13.34 1.154 21.41 1.215 29.06 .276 36.39 .337 43.35 1.398 49.86 1.094 13.48 1.155 21.54 1.216 29.18 .277 36.51 .338 43.46 1.399 49.96 1.095 13.61 1.156 21.67 1.217 29.31 .278 36.62 .339 43.57 1.400 50.06 1.096 13.75 1.157 21.80 1.218 29.43 1.279 36.70 .340 43.68 .401 50.16 1.097 13.89 1.158 21.93 1.219 29.55 1.280 36.86 .341 43.79 .402 50.26 1.098 14.02 1.159 22.05 1.220 29.69 1.281 36.97 .342 43.90 1.403 50.37 1.099 14.16 1.160 22.18 1.221 29.80 1.282 37.09 .343 44.01 1,404 50.47 1.100 14.29 1.161 22.31 1.222 29.92 1.283 37.21 .344 44.12 1.405 50.57 1.101 14.43 1.162 22.44 1.223 30.04 1.284 37.32 .345 44.23 1.406 50.67 1.102 14.56 1.163 22.56 1.224 30.17 1.285 37.44 .346 44.34 1.407 50.77 1.103 14.70 1.164 22.69 1 225 30.29 1.286 37.56 .347 44.45 1.408 50.88 1.104 14.83 1.165 22.82 l'226 30.41 1.287 37.68 .348 44.56 1.409 50.98 1.105 14.97 1.166 22.94 1.227 30.53 1.288 37.79 .349 44.67 1.410 51.08 1.106 15.10 .167 23.07 1.228 30.65 1.289 37.91 .350 44.77 1.411 51.18 1.107 15.24 .168 23.20 1.229 30.78 .290 38.03 .351 44.88 1.412 51.28 1.108 15.37 .169 23.32 1.230 30.90 .291 38.14 1.352 44.99 1.413 51.38 1.109 15.51 .170 23.45 .231 31.02 .292 38.26 1.353 45.10 1.414 51.48 1.110 15.64 .171 23.57 .232 31.14 1.293 38.37 1.354 45.21 1.415 51.58 1.111 15.78 .172 23.71 .233 31.26 1.294 38.49 1.355 45.32 1.416 51.68 1.112 15.91 1.173 23.83 .234 31.38 1.295 38.60 1.356 45.43 1.417 51.78 1.113 16.05 1.174 23.96 .235 31.50 1.296 38.72 .357 45.53 1.418 51.89 1.114 16.18 1.175 24.08 1.236 31.62 1.297 38.83 .358 45.64 1.419 51.99 1.115 16.31 1.176 24.21 1.237 31.75 1.298 38.95 .359 45.75 1.420 52.09 1.116 16.45 1.177 24.34 1.238 31.87 1.399 39.06 .360 45.86 1.421 52.19 1.117 16.58 1.178 24.46 1.239 31.99 1.300 39.18 .361 45.97 1.422 52.29 1.118 16.71 1.179 24.59 1.240 32.11 1.301 39.29 .362 46.07 1.423 52.39 1.119 16.84 1.180 24.71 1.241 32.23 1.302 39.41 .363 46.18 1.424 52.49 1.120 16.98 1.181 24.84 1.242 32.35 1.303 39.52 .364 46.29 1.425 52.59 1.121 17.11 1.182 24.97 .243 32.47 1.304 39.64 .365 46.39 1.426 52.69 1.122 17.24 1.183 25.09 .244 32.59 1.305 39.75 .366 46.50 1.427 52.79 1.123 17.37 1.184 25.22 .245 32.71 1.306 39.86 .367 46.61 1.428 52.89 1.124 17.51 1.185 25.34 .246 32.83 1.307 39.98 .368 46.71 1.429 52.98 1.125 17.64 1.186 25.47 .247 32.95 1.308 40.09 .369 46.82 1.430 53.08 1.126 17.77 1.187 25.59 .248 33.07 1.309 40.20 .370 46.92 1.431 53.18 1.127 17.90 1.188 25.72 .249 33.19 1.310 40.32 .371 47.03 1.432 53.28 .128 18.03 1.189 25.84 .250 33.31 1.311 40.43 1.372 47.14 1.433 53.38 .129 18.16 1.190 25.97 .251 33.43 1.312 40.54 .373 47.24 1.434 53.48 .130 18.30 1.191 26.09 .252 33.55 1.313 40.66 1.374 47.35 1.435 53.58 .131 18.43 1.192 26.22 .253 33.67 1.314 40.77 1.375 47.45 1.436 53.68 .132 18.56 1 . 193 26.34 1.254 33.79 1.315 40.88 1.376 47.56 1.437 53.78 .133 18.69 1.194 26.47 1.255 33.91 1.316 40.99 1.377 47.67 1.438 53.88 .134 18.82 . 1.195 26.59 1.256 34.02 1.317 41.11 1.378 47.77 1.439 53 97 .135 18.95 1.196 26.71 1.257 34.14 1.318 41.22 1.379 47.88 1.440 54.07 - .136 19.08 1.197 26.84 1.258 34.26 1.319 41.33 1.380 47.98 1.441 54.17 .137 19.22 1.198 26.96 1 . 259 34.38 .320 41.45 1.381 48.09 1.442 54.27 1.138 19.34 1.199 27.09 1.260 34.50 .321 41.56 1.382 48.10 1.443 54.36 1.139 19.47 1.200 27.21 1.261 34.62 .322 41.67 1.383 48.30 1.444 54.46 1.140 19.60 1:201 27.33 1.262 34.74 .323 41.79 1.384 48.40 1.445 54.56 1.141 19.73 1.202 27.46 1.263 34.86 1.324 41.90 1.385 48.$) 1.446 54.65 1.142 19.86 1.203 27.58 1.264 34.98 1.325 42.01 1.386 48.61 1.447 54.75 1 . 143 19.99 1.204 27.71 1.265 35.09 1 .326 42.12 1.387 48.71 1.448 54.85 1.144 20.12 1.205 27.83 1.266 35.21 1.327 42.23 1.388 48.82 1.449 54.94 914 SULPHURIC ACID Sp. gr. of H 2 SO 4 -f-Aq at 15/15 in air Continued. Sp. gr. of H 2 SO 4 +Aq at 15/15 in air Continued. Sp. gr. % H 2 S04 Sp. gr. % H 2 S0 4 Sp. gr. % H 2 S0 4 Sp. gr. % H 2 S04 Sp. gr. % H 2 S0 4 Sp. gr. % H 2 S0 4 .450 55.04 1.511 60.78 1.572 66.23 1.633 71.48 1.694 76.65 1.755 82.01 .451 55.14 1.512 60.87 1.573 66.31 1.634 71.57 1.695 76.74 1.756 82.11 .452 55.24 1.513 60.96 1.574 66.40 1.635 71.65 1.696 76.82 1.757 82.21 .453 55.33 .514 61.05 1.575 66.49 1.636 71.74 1.697 76.91 1.758 82.31 .454 55.43 .515 61.14 1.576 66.57 1.637 71.82 1.698 76.99 1.759 82.41 .455 55.53 .516 61.24 1.577 66.66 1.638 71.91 1.699 77.08 1.760 82.51 1.456 55.62 .517 61.33 1.578 66.75 1.639 71.99 1.700 77.17 1.761 82.61 1.457 55.72 .518 61.42 1,579 66.83 1.640 72.07 1.701 77.25 1.762 82.71 1.458 55.82 .519 61.51 1.580 66.92 1.641 72.16 1.702 77.34 1.763 82.80 1.459 55.91 .520 61.60 1.581 67.01 1.642 72.25 1.703 77.42 .764 82.90 1.460 56.01 .521 61.69 1.582 67.10 1.643 72.33 1 . 704 77.51 .765 83.00 1.461 56.11 .522 61.78 1.583 67.18 1.644 72.42 1 . 705 77.60 .766 83.10 1.462 56.20 .523 61.87 1.584 67.27 1.645 72.50 1.706 77.68 .767 83.20 .463 56.30 1.524 61.98 1.585 67.36 1.646 72.59 1.707 77.77 .768 83.29 .464 56.39 1.525 62.05 1.586 67.44 .647 72.67 1.708 77.85 .769 83.39 .465 56.49 1.526 62.14 1.587 67.53 .648 72.76 1.709 77.94 .770 83.49 .466 56.59 1.527 62.23 1.588 67.62 .649 72.84 1.710 78.0,3 .771 83.59 .467 56.68 1.528 62.32 .589 67.70 .650 72,93 1.711 78.11 1.772 83.69 .468 56.78 1.529 62.41 .590 67.79 .651 73,01 1.712 78.20 1.773 83.78 1.469 56.87 1.530 62.50 .591 67.88 .652 73.10 1.713 78.28 1.774 83.88 1.470 58.97 1.531 62.59 .592 67.97 .653 73.18 1.714 78.37 1.775 83.98 1.471 57.03 1.532 62.68 1.593 68.05 .654 73.27 1.715 78.46 1.776 84.08 1.472 57.16 1.533 62.77 1.594 68.14 1.655 73.35 1.716 78.54 .777 84.18 1.473 57.25 1.534 62.86 1.595 68.23 1.656 73.43 1.717 78.63 .77$ 84.29 1.474 57.35 1.535 62.95 1.596 68.31 1.657 73.52 1.718 78.72 .779 84.39 1.475 57.44 1.536 63.04 .597 68.40 1.658 73.52 1.719 78.80 .780 84.50 1.476 57.54 1.537 63.13 .598 68.49 1.659 73.69 1.720 78.89 .781 84.60 1.477 57.63 .538 63.22 .599 68.57 1.660 73.77 1.721 78.97 .782 84.71 1.478 57.73 .539 63.31 .600 68.66 1.661 73.86 1.722 79.06 .783 84.81 1.479 57.82 .540 63.40 .601 68.74 1.662 73.94 1.723 79.15 .784 84.92 1.480 57.92 .541 63.49 .602 68.83 .663 74.02 1.724 79.23 .785 85.03 1.481 58.01 .542 63.58 .603 68.92 .664 74.11 1.725 79.32 .786 85.14 1.482 58.10 .543 63.67 .604 69.00 .665 74.19 1.726 79.41 .787 85.25 1.483 58.20 .544 63.76 .605 69.09 .666 74.27 1.727 79.49 .788 85'. 36 1.484 58.29 1.545 63.85 .606 69.17 .667 74.36 1.728 79.58 .789 85.47 1.485 58.38 .546 63.94 .607 69.26 .668 74.44 1.729 79.67 .790 85.60 1.486 58.48 1.547 64.03 .608 69.35 1.669 74.53 1.730 79.75 .791 85.72 1.487 58.57 1.548 64.12 .609 69.43 1.670 74.61 1.731 79.84 .792 85.84 1.488 58.66 1.549 64.20 .610 69.52 1.671 74.69 1.732 79.93 1.793 85.96 1.489 58.75 1.550 64.29 1.611 69.60 1.672 74.78 1.733 80.02 1.794 86.G AO 1.490 58.85 1.551 64.38 1.612 69.69 1.673 74.86 1.734 80.11 1.795 86. f 1.491 58.94 1.552 64.47 1.613 69.78 1.674 74.95 1.735 80.20 1.796 86.; 1.492 59.03 1.553 64.55 1.614 69.86 .675 75.03 1.736 80.29 1.797 86.4 .493 59.12 1.554 64.64 1.615 69.95 .676 75.12 1.737 80.38 1.798 86.5, .494 59.22 .555 64.73 1.616 70.03 .677 75.20 1.738 80.47 1.799 86. -71 .495 59.31 .556 64.82 1.617 70.12 .678 75.29 1.739 80.56 1.800 86.84 .496 59.41 .557 64.91 1.618 70.20 .679 75.37 1.740 80.65 1.801 86.97 J .497 59.50 .558 65.00 1.619 70.29 .680 75.46 1.741 80.74 1.802 87.101 .498 59.59 .559 65.08 1.620 70.38 .681 75.54 1.742 80.84 1.803 87.23 .499 59.68 .560 65.17 1.621 70.46 .682 75.63 1.743 80.92 1.804 87.36 .500 59.78 .561 65.26 1.622 70.55 .683 75.71 1.744 81.01 1.805 87.50 .501 59.87 .562 65.35 1.623 70.63 .684 75.80 1.745 81.10 1.806 87.64 .502 59.96 1.563 65:44 1.624 70.72 .685 75.88 1.746 81.19 1.807 87.78 .503 60.05 1.564 65.52 1.625 70.80 .686 75.97 1.747 81.28 1.808 87.92 1.504 60.14 1.565 65.61 1.626 70.89 .687 76.05 1.748 81.37 1.809 88.06 1,505 60.23 1.566 65.70 1.627 70.97 .688 76.14 1.749 81.46 1.810 88.20 1.506 60.33 1.567 65.79 1.628 71.06 1.689 76.22 1.750 81.55 1.811 88.34 1.507 60.42 1.568 65.88 1.629 71.14 1.690 76.31 1.751 81.64 1.812 88.49 1.508 60.51 1.569 65.96 1.630 71.23 1.691 76.39 1.752 81.73 1.813 88.64 1.509 60.60 1.570 63.05 1.631 71.31 1.692 76.48 1.753 81.82 1.814 88.79 1.510 60.69 1.571 66.14 1.632 71.40 1.693 76.56 1.754 81.92 1.815 88.95 Continued on page 917. SULPHURIC ACID 915 Sp. gr. of H 2 SO 4 +Aq at t. Sp. gr. of H 2 O at 15 = 1. ^ 4 tE 10 15 20 25 30 40 50 60 1.00074 1.00060 l.OOOOQ 0.99910 0.99794 0.99654 0.99311 0.98895 0.98418 ] 1.00833 1.00773 1.00698 1.00594 1.00465 1.00312 0.99950 0.99522 0.99034 2 1.01563 1.01466 1.01381 1.01266 1.01126 1.00963 1.00585 1.00143 0.99644 t t 1.02281 1.02153 1.02055 1.01928 1.01777 1.01607 1.01216 1.00761 1.00252 L 1.03001 1.02841 1.02728 1.02590 1.02428 1.02251 1.01848 1.01383 1.00865 t 1.03728 1.03533 1.03406 1.03258 1.03086 1.02902 1.02487 1.02013 1.01484 ( 1.04461 1.04232 1.04092 1.03934 1.03756 1.03565 1.03138 1.02653 1.02114 7 1.05199 1.04939 1.04786 1.04618 1.04434 1.04235 1.03796 1.03302 1.02752 8 1.05942 1.05652 1.05486 1.05308 1.05116 1.04910 1.04458 1.03952 1.03393 9 1.06689 1.06370 1.03192 1.06002 1.05799 1.05585 1.05119 1.04605 1.04041 10 1.07439 1.07093 1.06903 1.06702 1.06490 1.06267 1.05787 1.05264 1.04696 11 1.08194 1.07821 1.07619 1.07408 1.07186 1.06955 1.06462 1.05930 1.05357 12 1.08954 1.08555 1.08342 1.08120 1.07890 1.07650 1.07145 1.06604 1.06027 13 1.09718 1.09294 1.09071 1.08839 1.08600 1.08352 1.07834 1.07284 1.06703 14 1.10488 1.10040 1.09805 1.09564 1.09316 1.09061 1.08530 1.07971 1.07385 15 1.11261 1.10790 1.10546 1.10295 1.10039 1.09776 1.09233 1.08666 1.08075 16 1.12040 1.11547 1.11292 1.11033 1.10768 1.10498 1.09944 1.09368 1.08772 17 1.12823 1.12309 1.12045 1.11777 1.11505 1.11228 1.10661 1.10077 1.09476 18 1.13610 1.13076 1.12803 1.12526 1.12246 1.11963 1.11385 1.10792 1.10186 19 1.14402 1.13848 1.13566 1.13282 1.12995 1.12704 1.12115 1.11514 1.10902 20 1.15199 1.14625 1.14335 1.14043 1.13748 1.13451 1.12851 1.12242 1.11625 21 1.15998 1.15407 1.15109 1.14809 1.14508 1.14205 1.13594 1.12977 1.12353 22 1.16803 1.16194 1.15888 1.15581 1.15273 1.14964 1.14343 1.13718 1.13089 23 1.17611 1.16986 1.16673 1.16359 1.16045 1.15731 1.15100 1.14467 1.13832 24 1.18424 1.17784 1.17464 1.17143 1.16823 1.16503 1.15862 1.15221 1.14579 25 1.19240 1.18586 1.18260 1.17933 1.17607 1.17282 1.16631 1.15982 1.15335 26 1.20061 1.19393 1.19060 1.18728 1.18396 1.18066 1.17406 1.16749 1.16096 27 1.20885 1.20204 1.19865 1.19527 1.19190 1.18854 1.18186 1.17522 1.16862 28 1.21710 1.21019 1.20675 1.20332 1.19990 1.19650 1.18973 1.18302 1.17635 29 1.22539 1.21838 1.21489 1.21142 1.20796 1.20452 1.19767 1.19087 1.18414 30 1.23370 1.22661 1.22308 1.21957 1.21607 1.21259 1.20566 1.19879 1.19198 31 1.24204 1.23487 1.23131 1.22776 1.22423 1.22071 1.21371 1.20677 1.19989 32 1.25038 1.24316 1.23957 1.23600 1.23244 1.22887 1.22179 1.21476 1.20779 33 1.25878 1.25151 1.24789 1.24429 1.24069 1.23712 1.22999 1.22292 1.21589 34 1.26723 1.25990 1.25626 1.25263 1.24901 1.24540 1.23822 1.23109 1.22400 35 1.27571 1.26834 1.26468 1.26102 1.25738 1.25375 1.24652 1.23933 1.23219 36 1.28424 1.27683 1.27314 1.26947 1.26580 1.26214 1.25487 1.24763 1.24045 37 1.29283 1.28538 1.28167 1.27797 1.27429 1.27061 1.26329 1.25:01 1.24878 38 1.30149 1.29400 1.29027 1.28655 1.28284 1.27915 1.27179 1.26448 1.25721 39 1.31022 1.30268 1.29894 1.29520 1.29148 1,28776 1.28038 1,27304 1.26575 40 1.31901 1.31144 1.30767 1.30392 1.30018 1.29646 1.28905 1.28169 1.27440 41 1.32788 1.32027 1.31648 1.31271 1.30896 .30522 1.29779 1.29042 1.28311- 42 1.33683 1.32917 1.32537 1.32158 1.31782 .31407 1.30662 1.29924 1.29193 43 1.34587 1.33817 1.33435 1.33054 1.32676 .32300 1.31553 1.30813 1.30081 44 1.35501 1.34727 1.34342 1.33960 1.33580 .33202 1.32452 1.31710 1.30976 45 1.36425 1.35647 1.35261 1.34877 1.34496 .34116 1.33363 1.32618 1.31881 46 1.37361 1.36579 1.36191 1.35805 1.35422 .35040 1.34284 1.33365 1.32797 47 1.38308 1.37522 1.37132 1.36744 1.36359 .35975 1.35215 1.34464 1.33721 48 1.39267 1.38476 1.38084 1.37694 1.37306 .36921 1.36157 1.35401 1.34655 49 1.40238 1.39441 1.39047 1.38654 1.38264 1.37877 1.37108 1.36349 1.35600 50 1.41219 1.40418 1.40021 1.39627 1.39235 1.38845 1.38073 1.37310 1.36556 51 1.42214 1.41407 1.41007 1.40610 1.40215 1.39823 1.39047 1.38280 1.37524 52 1.43220 1.42408 1.42005 1.41605 1.41208 1.40814 1.40033 1.39262 1.38502 916 SULPHURIC ACID Sp. gr. of H 2 SO 4 +Aq. at t. Sp. gr. of H 2 O at 15 = 1 Continued 4 w 10 15 20 25 30 40 50 60 53 1.44239 1.43420 1.43014 1.42611 1.42211 1.41814 1.41028 .40254 .39490 54 1.45269 1.44443 1.44034 1.43628 1.43225 1.42825 1.42034 .41255 .40488 55 1.46311 1.45477 1.45065 1.44656 1.44250 1.43847 1.43051 .42268 .41497 56 1.47364 1.46523 1.46107 1.45695 1.45285 1.44880 1.44078 .43290 .42515 57 1.48427 1.47578 1.47159 1.46743 1.46331 1.45922 1.45115 .44322 .43542 58 1.49499 1.48643 1.48221 1.47802 1.47387 1.46975 1.46162 .45364 .44579 59 1.50583 1.49719 1.49292 1.48870 1.48452 1.48037 1.47218 .46415 .45626 60 .51676 1.50804 1.50374 1.49949 1.49527 1.49109 1.48285 .47476 .46683 61 .52778 1.51899 1.51465 1.51036 1.50611 1.50190 1.49360 .48546 .47748 62 .53889 1.53002 1.52564 1.52132 .51703 1.51278 1.50442 .49622 .48819 63 .55008 .54113 1.53672 1.53236 .52804 1.52376 1.51533 .50708 .49900 64 .56135 .55233 1.54788 1.54348 .53913 1.53481 1.52632 .51801 .50988 65 .57270 .56360 .55912 1.55469 .55030 1.54595 1.53740 .52903 .52084 66 .58414 .57496 .57044 1.56597 .56154 1.55716 1.54854 .54011 .53187 67 1.59565 .58640 .58184 1.57733 .57287 .56846 .55978 .55128 .54298 68 1.60724 .59792 .59332 1.58878 .58427 .57981 .57104 .56246 .55408 69 1.61892 .60951 .60488 1.60030 .59577 .59129 .58247 .57384 .56541 70 1.63068 .62118 .61651 1.61189 .60732 .60280 .59391 .58521 .57672 71 1.64251 1.63293 .62821 1.62355 .61894 .61437 .60540 .59663 .58806 72 1.65439 1.64473 .63997 1.63527 .63062 .62601 .61696 .60811 .59946 73 1.66633 1.65658 .65178 1.64704 .64234 .63769 .62855 .61961 .61087 74 1.67831 1.66847 1.66362 1.65883 1.65408 .64939 .64015 .63111 .62227 75 1.69030 1.68037 1.67547 1.67063 1.66584 1.66109 .65175 1.64260 .63366 76 .70228 1.69225 1.68731 1.68242 1.67757 1.67278 1.66332 1.65405 1.64498 77 .71424 1.70411 1.69911 1.69416 1.68926 1.68439 1.67481 1.66540 1.65617 78 .72615 1.71589 1.71083 1.70582 1.70085 1.69591 1.68616 1.67658 1.66717 79 .73798 .72758 1.72243 1.71735 1.71231 1.70731 1.69741 1.68767 1.67809 80 .74970 .73909 1.73386 1.72868 1.72356 1.71847 1.70842 1.69854 1.68881 81 .76120 .75038 1.74504 1.73979 1.73458 1.72942 1.71921 1.70916 1.69930 82 .77244 .76140 1.75595 1.75057 1.74524 1.73998 1.72962 1.71945 1.70950 83 .78312 .77193 1.76642 1.76097 1.75557 1.75022 1.73972 1.72943 1.71937 84 .79316 .78191 1.77636 1.77087 1.76543 1.76006 1.74943 1.73902 1.72883 85 .80250 .79123 1.78567 1.78016 1.77470 1.76929 1.75863 1.74816 1.73789 86 .81108 .79982 1.79428 1.78878 1.78331 1.77789 1.76721 1.75674 1.74642 87 .81887 .80767 1.80214 1.79666 1.79123 1.78584 1.77519 1.76473 1.75445 88 1.82589 .81476 1.80926 1.80381 1.79839 1.79302 1.78242 .77199 1.76176 89 1.83216 .82111 1.81564 1.81022 1.80484 1.79950 1.78895 .77856 1.76834 90 1.83771 .82677 1.82135 1.81597 1.81063 1.80532 .79483 .78448 1.77429 91 1.84263 .83179 1.82642 1.82109 1.81580 1.81054 .80013 .78985 1.77972 92 1.84691 .83619 1.83088 1.82561 1.82037 1.81516 .80487 .79471 1.78470 93 1.85059 .83997 1.83471 1.82950 1.82432 1.81918 .80902 1.79900 1.78914 *94 1.85363 1.84311 1.83790 1.83275 1.82763 1.82255 .81253 1.80266 1.79296 95 1.85598 1.84555 1.84040 1.83526 1.83022 1.82520 1.81528 1.80553 1.79595 96 1.85765 1.84729 1.84217 1.83709 1.83207 1.82708 1.81724 1.80758 1.79809 97 1.85854 1.84816 1.84305 1.83798 1.83297 1.82800 1.81822 1.80863 1.79924 98 1.85836 1.84789 1.84275 1.83766 1.83264 1.82767 1.81792 1.80840 1.79912 99 1.85671 1.84612 1.84093 1.83581 1.83076 1.82578 1.81604 1.80658 1.79741 100 (1.85330) (1.84255) (1.83729) (1.83213) (1.82705) (1.82205) (1.81231) (1.80288) (1.79381) Auszug aus Band 5 der wissenschaftlichen Abhandlungen der Normaleichungskommission Berlin 1904, P. 257. Springer's publication. (Domke, Z. anorg. 1905, 43. 176.) SULPHURIC ACID 917 Sp. gr. of H 2 SO 4 +Aq at 15/15 in air. Freezing- and melting-points of H 2 SO 4 +Aq. Continued from page 915. Sp. gr. at 15 F.-pt. M.-pt. Sp. gr. % H 2 SO, Sp. gr. % H 2 S0 4 Sp. gr. %H 2 S04 1.671 liq. at 20 1.816 89.11 1.828 91.30 1.840 94.57 1.691 1 710 it .817 .818 89.27 89.44 1.829 1.830 91.52 91.74 1.841 1.842 94.96 95.40 .727 -7.5 -7/5 .819 .820 .821 .822 .823 .824 89.61 89.79 89.97 90.15 90.33 90.51 1.831 1.832 1.833 1.834 1.835 1.836 91.98 92.22 92.46 92.71 92.98 93.26 1.843 1.844 1.8442 1.844 1.843 1.842 96.02 96.93 97.50 99.08 99.84 99.29 .732 .74.9 .767 .7,90 .807 .822 Q/19 .5 -0.2 + 1-6 +4.5 -9.0 liq. at 20 -8.5 +4.5 +6.5 +8.0 -6.0 1.825 90.70 1.837 93.56 1.841 98.61 1.826 1.827 90.90 91.10 1.838 1.839 93.87 94.20 1.840 18.394 98.88 100.00 (Lunge, B. 15. 2644.) (Lunge, calculated by Marshall, J. Soc. Chem. Ind. 1902, 21. 1509. (Jones and Pearce, Am. Ch. J. 1907, 38. 733.) Boiling-point of H 2 SO 4 +Aq. % H 2 S0 4 B.-pt. % H 2 S0 4 B.-pt. 5 101.0 70 170.0 10 102.0 72 174.5 15 105.5 74 180.5 20 105.0 76 189.0 25 106.5 78 199.0 30 108.0 80 207.0 35 110.0 82 . 218.5 40 114.0 84 227.0 45 118.5 .86 238.5 50 124.0 88 251.5 53 128.5 90 262.5 56 133.0 91 268.0 60 141.5 92 274.5 62.5 147.0 93 281.5 65 153.5 94 288.5 67.5 161.0 95 295.0 (Lunge, B. 11. 370.) Effect of impurities on sp. gr. of H 2 SO 4 +Aq. The figures show 'the increase in sp. gr. of H 2 S0 4 + Aq caused by adding 0.1% of an impurity to acid of different strengths. Sp. gr. at 20 of H 2 S0 4 +Aq containing M g. mols. H 2 SO 4 per liter. M. 0.01 0.025 0:05 s M p : gr - 1.000719 0.075 1.001907 0.10 1.003551 0.25 Sp. gr. 1.005152 1.00677 1.01618 M. 0.50 0.75 1.0 Sp gr. 1.03218 1.04760 1.06307 M. 1.5 2.0 Sp. gr. 1.09345 1.12316 Salt 100 % 98% 94 % 80 % 70% Na 2 S0 4 CaS0 4 A1 2 (SO 4 ) 3 Fe 2 (SO4)s PbS0 4 MgS0 4 As 2 Os HSNOe 0.0011 0.0012 insol. 0.0017 0.0011 0.00029 0.0010 0.0011 insol. 0.0014 0,0010 0.0013 0.00027 . 0007 0.0009 insol. . 0006? 0.0015 0.0012 0.0008 . 0007 0.0012? 0.0008 insol. 0.0009 0.0010 0.00023 0.0007 . 0006 0.0011 0.0007 insol. 0.0009 (Marshall, J. Soc. Chem. Ind. 1902, 21. 1508.) Sp. gr. of mixtures of H 2 SO 4 (96.5%) and HNO 3 (94%) at 18/18 in air. %HN0 3 in mixture Sp. gr. %HNO 3 in mixture Sp. gr. 0.00 .8437 22.51 .8215 0.57 1.8456 25.56 .8112 1.05 1.8476 27.29 .8053 4.67 .8586 32.53 .7863 7.17 .8618 37.03 .7700 7.37 .8620 39.49 .7601 7.75 .8619 57.78 .6879 9.10 .8605 72.89 .6227 11.33 .8557 90.76 .5408 12.71 .8520 98.19 .5080 16.52 1.8414 100.00 .5009 (Marshall, J. Soc. Chem. Ind. 1902, 21. 1508.) Miscible with alcohol, with evolution of heat and formation of ethylsulphuric acid. +H 2 O=H 4 SO 5 , also called tetrahydroxyl sulphuric acid. (Marignac, A. ch. (3) 39. 184.) Mpt. 8.35. (Pickering.) +2H 2 O=H 6 SO 6 , also called perhydroxyl sulphuric acid. Mpt. 38.9. (Biron, J. Russ. Phys. Chem. Soc. 1899, 31. 517.) +3H 2 O. (Pickering, Chem. Soc. 1890, 57. 331.) 918 SULPHURIC ACID +4H 2 O. Mpt. -75. Soc. 1890, 67. 331.) (Pickering, Chem Sp. gr. and fr. pt. of hydrates of H 2 SO 4 . Hydrate ' % H.S0 4 Sp. gr. of the liquid Fr.-pt. H 2 SO 4 (pure) 100 1.842 + 10.5 H 2 S0 4 +H 2 84.48 1.777 + 3.5 H 2 SO 4 +2H 2 O 73.08 1.650 -70.0 H 2 SO 4 +4H 2 O 57.65 1.476 -40.0 H 2 SO 4 +6H 2 O 47.57 1.376 50.0 H 2 SO 4 +8H 2 O 40.50 1.311 -65.0 H 2 SO 4 + 10H 2 O 35.25 1.268 -88.0 H 2 SO 4 + 11H 2 O 33.11 1.249 -75.0 H 2 SO 4 + 12H 2 O 31.21 1.233 55.0 H 2 SO 4 + 13H 2 O 29.52 1.219 45.0 H 2 SO 4 + 14H 2 O 28.00 1.207 -40.0 H 2 SO 4 + 15H 2 O 26.63 1.196 -34.0 H 2 SO 4 + 16H 2 O 25.39 .187 -25.6 H 2 SO 4 + 18H 2 O 23.22 .170 -19.0 H 2 SO 4 +20H 2 O 21.40 .157 -17.0 H 2 SO 4 +25H 2 O 17.88 .129 - 8.5 H 2 SO 4 +50H 2 O 9.82 .067 - 3.5 H 2 SO 4 +75H 2 O 6.77 .045 0.0 H 2 SO 4 + 100H 2 O 5.16 .032 + 2.5 H 2 SO 4 +300H 2 O 1.78 .007 + 4.5 H 2 SO 4 + 1000H 2 O 0.54 .001 + 0.5 (Pictet, C. R. 1894, 119. 645.) Sulphuric acid, anhydrous, SO 3 . See Sulphur dioxide. ZH'sulphuric (Pt/rosulphuric) acid, H 2 S 2 O 7 . Very deliquescent. Miscible with H 2 O. 501. in fuming H 2 SO 4 . Miscible in liquid 50 2 . (Schultz-Sellack.) H 2 S 2 O 7 , 2H 2 SO 4 . Fumes on air. (Jacque- lain, A. ch. (3) 30. 343.) TWrasulphuric acid, H 2 S 4 Oi 3 . Fumes on air. (Weber, Pogg. 159. 313.) Sulphates. Most sulphates are easily sol. in H 2 O; but Ag 2 SO 4 , Hg 2 SO 4 , and CaSO 4 are only si. sol., while BaSO 4 , SrSO 4 , and PbS0 4 are nearly insol. therein. All sulphates are sol. in cone. H 2 SO 4 . Basic sulphates are insol. in H 2 O. Most sulphates are insol. in alcohol. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 823.) Aluminum sulphate, basic, 2A1 2 O 3 ,SO 3 + 5H 2 O. Slowly sol. in 10 mols. HC 2 H 3 2 . (Schlumberger, Bull. Soc. 1895, (3) 13. 41.) +7H 2 O. Easily sol. in 8 mols. dil. HC1+ Aq. or in 10 mols. 10% acetic acid in 24 hours. (Schlumberger.) +10H 2 O. Insol. in H 2 O; easily sol. in cold dil. mineral acids, and HC 2 H 3 O 2 +Aq. (Crum, A. 89. 174.) Min. Felsobanyite. +15H 2 O. Min. Paraluminite. 8A1 2 O 3 , 5SO 3 +25H 2 O. Insol. in H 2 0; sol. in dil. acids. (Lowe, J. pr. 79. 428.) 5A1 2 O 3 , 3S0 3 +20H 2 O. Easily sol. in acids. (Debray, Bull. Soc. (2) 7. 9.) 3A1 2 O 3 2SO 3 +9H 2 O. Nearly insol. in cone. H 2 SO 4 . (Bayer, Dirigl. 263. 211.) +20H 2 O. Ppt. 4A1 2 O 3 , 3SO 3 +36H 2 O. Insol. in H 2 O. Easily sol. in dil. mineral acids, and hot HC 2 H 3 O 2 +Aq. (Debray, Bull. Soc. (2) 7. 1.) A1 2 O 3 , SO 3 +'6H 2 O = (A1O) 2 SO 4 + H 2 O. Insol. in H 2 O or HC 2 H 3 2 +Aq. SI. sol. in hot HC1, easily sol. in warm KOH+Aq. (Bottinger, A. 244. 225.) +9H 2 O. (Athanasesco, C. R. 103. 27.) Min. Aluminite. [Al 2 (pH) 5 ]SO 4 -t-2H 2 O. Sol. in HCl-fAq. in the cold with decomp. Very unstable. (Schlumberger, Bull. Soc. 1895, (3) 13. 60.) 3A1 2 O 3 , 4SO 3 +9H 2 O. (Athanasesco, C. R. 103.271.)' +30H 2 O. Sol. in 144 pts. cold, and 30.8 pts. boiling H 2 O. Easily sol. in HC1, and HN0 3 +Aq. (Rammelsberg, Pogg. 43. 583.) 2A1 2 O 2 , 3SO 3 . Decomp. by H 2 into 3A1 2 O 3 , SO 3 and A1 2 (SO 4 ) 3 . (Maus.) A1 2 O 3 , 2S0 3 =A1 2 O(SO 4 ) 2 . Mm. Alumaine. -f-H 2 O. Sol. in small quantity of H 2 O, but decomp. by a large quantity into (A1O) 2 SO 4 and A1 2 (SO 4 ) 3 . (Maus, Pogg. 11. 80.) +12H 2 O. Easily sol. in hot or cold H 2 O. Sat. solution contains 45% salt at 15, which crystallises unchanged on evaporating. (Mar- guerite, C. R. 90. 354.) Above basic compounds are mixtures. Pickering, C. N. 45. 121, 133, 146.) Aluminum sulphate, A1 2 (SO 4 ) 8 . 100 pts. H 2 O dissolve (a) pts. A1 2 (S0 4 ) 3 , and (6) pts. A1 2 (SO 4 ) 3 +18H 2 O at: 10 20 30 40 50 i 31.3 33.5 36.15 40.36 45.73 52.13 86.85 95.8 107.35 127.6 167.6 201.4 60 70 80 90 100 a 59.09 66.23 73.14 80.83 98.11 6 262.6 348.2 467.3 678.8 1132. (Poggiale/A. ch. (3) 8. 467.) See also +18H 2 O. Sp. gr. of Al 2 (SO 4 ) 3 +Aq. % A1 2 (SO 4 )3 Sp. gr. at 15 25 35 45 5 10 15 20 25 1.0569 1.1071 1 . 1574 1 . 2074 1.2572 1.0503 1 . 1022 1 . 1522 1 . 2004 1 . 2487 1.045 1.096 1.146 1.192 1 . 2407 1.0356 1.085 1 . 1346 1.1801 1 . 2295 (Reuss, B. 17. 2888.) SULPHATE, ALUMINUM AMMONIUM 919 Sp. gr. of Al 2 (SO 4 ) 3 +Aq at 15 containing: 10 20 30%Al 2 (SO 4 ) 3 -fl8H 2 O, 1.0535 1.1105 1.1710 40 50% A1 2 (SO 4 ) 3 +18H 2 O. 1.2355 1.3050 Sp. gr. of sat. solution = 1 . 34. (Gerlach, Z. anal. 28. 493.) Sp. gr. of Al 2 (SO 4 ) 3 +Aq. at 25. Strength of Al 2 (SO 4 ) 3 +Aq Sp. gr. 1 normal V. " V4 " Vs " 1.0550 1.0278 1.0138 1.0068 (Wagner, Z. phys. Ch. 1890, 5. 35.) 100 pts. of a mixture of 1 vol. H 2 SO 4 +2 vols. H 2 O dissolve only 6.45 pts. A1 2 (SO 4 ) 3 . (Baud, C. R. 1903, 137. 494.) A1 2 (SO 4 ) 3 is completely pptd. from Al 2 (SO 4 ) 3 +Aq by an excess of glacial HC 2 H 3 O 2 . (Persoz, A. ch. (2) 63. 444.) Solubility of A1 2 (SO 4 ) 3 +(NH 4 ) 2 A1 2 (SO 4 ) 4 . See under (NH 4 ) 2 A1 2 (SO 4 ) 4 . Solubility of A1 2 (SO 4 ) 3 +K 2 A1 2 (SO 4 ) 4 . See *Solution sat. with respect to both salts. (Wirth and Bakke, Z. anorg. 1914, 87. 48.) See also under Solubility of Al 2 (SO 4 ) 3 +Li 2 SO 4 at 30. Composition of Solid phase Solution Residue \ 4 I 4 25.1 21.93 16.10 13.63 13.24 11.73 6.75 3.44 0.00 5.34 14.89 20.76 21.71 22.08 24.34 26.12 28.0 63^70 14.72 61.24 6.92 3.77 4^02 31.17 7.22 33.54 37.06 Li 2 SO 4 , H 2 O Li 2 SO 4 . H 2 O + A1 2 (SO 4 ) 3 , 18H 2 O Li 2 S0 4 , 4H 2 O A1 2 (SO 4 ) 3 , 18H 2 O tt it (Schreinemakers and de Waal, Ch. Weekbl. 1906, 3. 539.) 100 g. of sat. solution of A1 2 (SO 4 ) 3 in glycol contain 14.4 g. A1 2 (S0 4 ) 3 . (de Coninck, Bull. Ac. Roy. Belg. 1905. 359.) Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. (Naumann, B. 1904, 37. 4328.) +6H 2 O. Very slowly sol. in cold, com- pletely sol. in hot H 2 O. +8H 2 O. (Margueritte-Delarcharbonny, C. R. 112. 229.) +10H 2 O. Deliquescent, (v. Hauer, W. A. B. 13. 449.) +16H 2 O. Sol. in cone. H 2 SO 4 . (Baud, C. R. 1903, 137. 494.) +17H 2 O. (Gawalowski, C. C. 1885. 721.) +18H 2 O. Permanent. (Berzelius.) 100 g. of the aqueous solution contain 27.82 g. A1 2 (S0 4 ) 3 at 25. (Wirth, Z. anorg. 1913, 79. 361.) Solubility of A1 2 (SO 4 ) 3 + 18H 2 O in H 2 SO 4 +Aq at 25. under K 2 A1 2 (SO 4 )4. Solubility in Fe 2 (SO 4 ) 3 +Aq at 25. H 2 SO 4 +Aq % H 2 S0 4 100 g. of the solution contain g. A1 2 (SO 4 )3 1 00 g. of the solution contain 5.23 9.90 18.70 25.50 40.70 52.25 63.70 73.64 27.82 29.21 26.21 20.44 15.40 5.07 1.216 1.243 2.915 g. A1 2 (S0 4 ) 3 g. Fe 2 (SCWi 27.82 26.01 24.21 21.64 15.22 *10.70\ 10.23J 6.064 9.819 13.02 23.28 31.911 31.90} (Wirth, Z. anorg. 1913, 79. 361.) Hydrous salt is scarcely sol. in alcohol, (Berzelius.) Min. Alunogen. -f-27H 2 0. Efflorescent. (Margueritte- Delarcharbonny, C. R. 99. 800.) Aluminum sulphate, acid, A1 2 O 3 , 4SO 8 -f 4H 2 O. Extremely slowly sol. in cold, more rapidly in hot H 2 O. (Baud, C. R. 1903, 137. 493.) A1 2 O 3 , 6SO 3 +10H 2 O. Sol. in H 2 O; solu- tion soon de,comp. into A1 2 (SO 4 ; 8 +H 2 SO 4 . (Silberberger, M. 1904, 25. 221.) Aluminum ammonium sulphate (Ammonia alum), (NH 4 ) 2 A1 2 (S0 4 ) 4 +24H 2 0. 100 pts. H 2 O dissolve 2.9 pts. anhydrous salt at 0; 207.7 pts. anhydrous salt at 110.6. (Mulder.) 100 pts. H 2 O dissolve 8.74 pts. anhydrous- salt at 17.5. (Pohl, W. A. B. 6. 597.) 920 SULPHATE, ALUMINUM AMMONIUM CHROMIUM 100 pts. H 2 O at t dissolve pts. (NH 4 ) 2 A1 2 (S0 4 ) 4 . Solubility of NH 4 alum in presence of (NH 4 ) 2 S0 4 and A1 2 (SO 4 ) 3 . Pts. Pts. 100 g. f&t. solution contains t (NH4)2A1 2 (SO 4 )4 (NH4)2A1 2 (SC>4)4 + Mixture used (NH 4 ) 2 SO4 g. Al 2 (SO4)s o 2 10 3 90 10 4.99 9.52 Sat. NH 4 alum 1.42. 3.69 20 30 7.74 10.94 15.13 22.01 at 18 . 5 20 cc. above sol- 40 50 60 70 80 14.88 20.09 26.70 35.11 45.66 30.92 44.11 66.65 90.67 134.47 ution +6 g. cryst. A1 2 (SO 4 ) 3 20 cc. above sol- ution +4g. (NH 4 ) 2 S0 4 0.45 20.81 16.09 0.29 90 100 58.68 74.53 209.31 357.48 (Riidorff, 1885, B. 18. 1160.) (Poggiale, A. ch. (3) 8. 467.) According to Locke (Am. Ch. J. 1901, 26. 174), Poggiale's tables for NH 4 and K alums are evidently transposed, and the above data are applied by Poggiale to K alum. 1 I. H 2 O dissolves 91.9 g. anhydrous, or 191.9 g. hydrated salt, or 0.387 mols. an- hydrous salt at 25. (Locke, Am. Ch. J. 1901, 26. 175.) Solubility in H 2 at t. G. (NH 4 ) 2 G. mol. G. (NH 4 ) 2 A1 2 (S0 4 )4 (NH 4 ) 2 t A1 2 (SO 4 )4 +24H 2 O A1 2 (S0 4 ) 4 per 100 g. H 2 O per 100 per 100 g.H 2 g. H 2 2.10 3.90 0.0044 5 3.50 6.91 0.0074 10 4.99 9.52 0.0105 15 6.25 12.66 0.0132 20 7.74 15.13 0.0163 25 9.19 19.19 0.0194 30 10.94 22.01 0.0231 40 14.88 30.92 0.0314 50 20.10 44.10 0.0424 60 26.70 66.65 0.0569 95 109.7 00 0.2312- (Mulder, Poggiale, Locke; Marino, Gazz. ch. it. 1905, 35. II, 351; Berkeley, Trans. Roy. Soc. 1904, 203. A, 214, calc. by Seidell,' Solubilities.) B.-pt. of sat. solution is 110.6. M.-pt. of (NH 4 ) 2 A1 2 (S0 4 )4+24H 2 = 92. (Tilden, Chem. Soc. 46. 409.) ; =95. (Locke, L c.) Sp. gr. of aqueous solution at 15 contain ing: 3% 6% 9% 1 . 0423 1 . 0141 1 . 0282 hydrous salt. - (Gerlach, Z. anal. 28. 495.) Insol. in alcohol. (Mulder.) Solubility of A1(NH 4 )(SO 4 ) 2 +12H 2 O in a mixture of 93.3 g. H 2 O and 23.33 g. glycerine = 6.15 g. (Dunlop, Pharm. J. 1910, 85. 6.) Solubility in 93.3 g. H 2 O+23.3 g. glycerine +3.9 g. phenol = 5.59 g. A1(NH 4 )(SO 4 ) 2 +12H 2 O. (Dunlop.) Min. Tschermigite. Aluminum ammonium chromium sulphate, A1 2 (S0 4 ) 3 , (NH 4 ) 2 S0 4 , Cr 2 (S0 4 ) 3 + 48H 2 O. Sol. in H 2 O; decomp. by boiling. (Vohl, A. 94. 71.) Aluminum caesium sulphate. Al 2 Cs 2 (S0 4 ) 4 -{- 24H 2 0. 100 pts. H 2 O at 17 dissolve 0.619 pt. caesium alum. (Redtenbacher, J. pr. 94. 442.) Solubility in 100 pts. H 2 O at t (calculated for salt dried at 130). t Pts. alum t Pts. alum t Pts. alum 10 17 0.19 0.29 0.38 25 35 50 0.49 0.69 1.235 65 80 2.38 5.29 (Setterberg, A. 211. 104.) Solubility in H 2 O. Pts. G. mols. t anhydrous salt anhydrous salt per litre per litre 25 4.7 0.013 30 5.89 0.0167 35 7.29 0.0207 40 9.00 0.0256 (Locke, Am. Ch. J. 1901, 26. 180.) SULPHATE, ALUMINUM MAGNESIUM 921 Solubility of Al 2 Cs 2 (SO 4 )4 in H 2 O at t. (G. Al 2 Cs 2 (SO 4 )4+24H 2 O in 100 g. solution.) Aluminum chromium sulphate, Al 2 Cr 2 (SO 4 ) 6 . Insol. in H 2 O. Al 2 Cr2(SO4)6,H 2 S04. Insol. in H 2 O. (Etard C. R. 86. 1400.) Aluminum chromium potassium sulphate, A1 2 (SO 4 ) 3 , Cr 2 (SO 4 ) 3 , 2K 2 SO 4 +48H 2 O. Sol. in H 2 O, but decomp. on boiling. (Vohl.) Aluminum copper sulphate, 2A1 2 O 3 , 9CuO, 3SO 3 +21H 2 O. Min. Cyanotrichite. (Percy, Phil. Mag. (3) 36. 103.) t % salt t % salt 15 30 45 60 0.21 0.35 0.60 1.04 1.96 75 80 90 100.4 4.12 5.21 9.50 18.60 (Berkeley, Trans. Roy. Soc. 1904, 203. A, 214.) Solubility in 100 g. H 2 O at t. o o o t 03, t oo I t CO t 0.19 26 0.50 52 1.45 78 5.15 1 0.20 27 0.51 53 .51 79 5.40 2 0.21 28 0.52 54 .58 80 5.78 3 0.22 29 0.55 55 .65 81 6.05 4 0.23 30 0.57 56 1.71 82 6.4 5 0.24 31 0.59 57 1.77 83 6.7 6 0.25 32 0.60 58 1.86 84 7.0 7 0.26 33 0.62 59 1.92 85 7.4 8 0.27 34 0.65 60 2.06 86 7.7 9 0.28 35 0.69 61 2.14 87 8.0 10 0.29 36 0.72 62 2.25 88 8.3 11 0.30 37 0.75 63 2.37 89 8.6 12 0.31 38 0.77 64 2.50 90 8.8 13 0.32 39 0.80 65 2.65 91 9.0 14 0.34 40 0.85 66 2.78 92 9.2 15 0.35 41 0.87 67 2.96 93 9.5 16 0.36 42 0.91 68 3.13 94 9.9 17 0.38 43 0.96 69 3.34 95 10.1 18 0.39 44 1.01 70 3.50 96 10.4 19 0.40 45 1.06 71 3.67 97 10.8 20 0.41 46 1.10 72 3.85 98 11.1 21 0.42 47 1.17 73 4.07 99 11.5 22 0.43 48 1.21 74 4.30 100 12.0 23 0.45 49 1.27 75 4.50 24 0.47 50 1.30 76 4.72 25 0.49 51 1.39 77 4.95 Values from 0-7 obtained by interpolation using Setterberg's values for 0(A. 1882, 211. 100). From 80-100 they were calculated by extrapolation. (Hart and Huselton, J. Am. Chem. Soc. 1914, 36. 2084.) Melts in crystal H 2 O at 106 (Tilden, Chem. Soc. 45. 409); at 120.5 (Erdmann)- at 122 (Locke.) calcium sulphate, basic, A1 2 3 , 6CaO, 3SO 3 +32H 2 0. Min. Ettringite. Mostly sol. in H 2 O; sol. inHCl+Aq. Aluminum hydroxylamine sulphate, A1 2 (SO 4 ) 3 , (NH 2 OH) 2 SO 4 +24H 2 O. Sol. in H 2 0. (Meyeringh, B. 10. 1946.) Aluminum iron (ferrous) sulphate, A1 2 (SO 4 ) 8 , FeSO 4 +24H 2 O. Sol.inH 2 O. (Klauer, A. 14. 261.) Min. Halotrichite. A1 2 (SO 4 ) 3 , 2FeSO 4 +27H 2 O. Sol. in H 2 O. (Berthier.) A1 2 O 3 , 2SO 3 , 6FeSO 4 . Easily sol. in H 2 O. (Phillips.) A1 2 (SO 4 ) 3 2FeS0 4 , H 2 SO 4 . Insol. in H 2 O. (Etard, C. R. 87. 602.) Aluminum iron (ferric) sulphate, A1 2 (SO 4 ) 3 , Fe 2 (S0 4 ) 3 . Insol. in H 2 0. (Etard, C. R. 86. 1399.) A1 2 (SO 4 ) 3 , Fe 2 (SO 4 ) 3 , H 2 SO 4 . As above (Etard.) See Al 2 (SO 4 ) 3 +Fe 2 (SO 4 ) 3 , under A1 2 (S0 4 ) 3 and Fe 2 (SO 4 ) 3 . Aluminum ferrous potassium sulphate, A1 2 (SO 4 ) 3 , 12FeSO 4 , 2K 2 SO 4 +24H 2 O. Permanent. SI. sol. in H 2 0. (Dufrenoy.) Aluminum lead sulphate, Al 2 Pb 2 (SO 4 ) 6 + 20H 2 O. Permanent; insol. in F 2 O. (G. H. Bailey J. Chem. Soc. Ind. 6. 415.) Aluminum lithium sulphate, Li 2 Al 2 (SO 4 ) 4 -4- 24H 2 O. Sol. in 24 pts. cold, and 0.87 pt. hot H 2 O. (Kralovansky, Schw. J. 54. 349.) Does not exist. (Rammelsberg, J. B. 1847- 48. 394; Arfvedson; Gmelin.) Aluminum lithium potassium sulphate (?). Sol. in H 2 O, from which it crystallises on cooling. (Joss, J. pr. 1. 142.) Aluminum magnesium sulphate, MgS0 4) A1 2 (SO 4 ) 3 +22H 2 O. Min. Pickerinqite. 2MgSO 4 , A1 2 (SO 4 ) 3 +22H 2 O. Min. Pio raluminite. 3MgSO 4 , A1 2 (S0 4 ) 3 +36H 2 O. Very sol. in H 2 O. (Klauer, A. 14. 264.) 922 SULPHATE, ALUMINUM MAGNESIUM MANGANOUS Aluminum magnesium manganous sulphate A1 2 (SO 4 ) 3 , MgSO 4 , MnSO 4 +25H 2 0. As sol. in H 2 O as K alum. (Kane.) Ver} sol. in H 2 O. (Smith, Sill. Am. J. (2) 18. 379. Min. Bosjemanite. Aluminum manganous sulphate, A1 2 (SO 4 ) 3 MnSO 4 +25H 2 O. Sol. in H 2 0. (Berzelius.) +24H 2 O. Min. Apjohnite. Aluminum manganic sulphate. 2A1 2 (SO 4 ) 3 Mn 2 (S0 4 ) 3 . Insol. in H 2 0. (Etard, C. R. 86. 1399.; Aluminum nickel sulphate, A1 2 (S0 4 ) 3 , 2NiSO 4 H 2 S0 4 . Insol. in H 2 O, but gradually decbmp thereby. (Etard, C. R. 87. 602.) Aluminum potassium sulphate, basic. 3(A1 2 3 , SO,), K 2 S0 4 +6H 2 0=K 2 S0 4 , 3A1 2 (S0 4 ,)(OH) 4 . Min. Alunite. Insol. in H 2 O. Insol. in cone. HCl+Aq. Sol. in boiling H 2 S0 4 of 1.845 sp. gr., but more easily in a mixture of 12 g. H 2 SO 4 and 1.5 g. H 2 O, and also in weaker acids, if heated to 210. (Mitscherlich, J. pr. 81. 108.) +9H 2 O. Min. Lowigite. SI. sol. in boil- ing HCl+Aq. (Mitscherlich, J. pr. 83. 455.) Nearly insol. in HC1 or cone. HNO 3 +Aq, but sol. in a mixture of 1 pt. H 2 SO 4 and 1 pt. H 2 O. (Debray, Bull. Soc. (2) 7. 9.) A1 2 O(SO 4 ) 2 , K 2 SO 4 . Sol. in H 2 O, but de- comp. by heating. With varying composition. Precipitates. Insol. in H 2 O. Very si. sol. in cold, gradually in hot acids. (Bley, J. pr. 39. 17.) Very difficultly sol. in warm cone. HCl+Aq, but easily sol. in KOH+Aq. (Naumann, B. 8. 1630.) Temp. Pts. K2Al2(S0 4 )4 Temp. Pts. K 2 A1. 2 (S0 4 )4 3.0 60 25 5 3.5 70 40 10 4.0 80 71 15 5.0 90 109 20 5.9 92.5 119.5 30 7.9 100 154 40 11.7 110 200 50 17.0 111.9 210.6 100 pts. H 2 O dissolve (a) pts. anhydrous alum, and (&) pts. crystallised at t. 10 20 30 40 50 a 2.62 4.50 6.57 9.05 12.35 15.9 65.22 9.16 13.66 19.29 27.3 36.5 60 '70 80 90 100 a 21.1 26.95 35.2 50.3 70.83 6 51.3 71.97 103.1 187.8 421.9 (Poggiale, A. ch. (3) 8. 467.) According to Locke (Am. Ch. J. 1901, 26. 174), Ppggiale's tables for NH 4 and K alums are evidently transposed, and the above date are applied by Poggiale to NH 4 alum. 100 pts. H 2 O dissolve K 2 A1 2 ';S0 4 ) 4 +24H 2 O corresponding to pts. anhydrous K 2 A1 2 (SO 4 ) 4 . (Mulder, Scheik. Verhandel. 1864. 90.) 100 pts. H 2 O at 17 dissolve 13.5 pts. K 2 A1 2 (SO 4 ) 4 +24H 2 O, or 7.36 pts. K 2 A1 2 (SO 4 ) 4 . Redtenbacher, J. pr. 94. 442.) Forms supersaturated solutions very easily. Supersat. solutions are brought to crystallisa- tion by addition of a crystal of alum or an somorphous substance, as chrome or iron alum. Other substances as NaCl, etc. have no action. (Thomson, Chem. Soc. 35. 199.) 1 1. H 2 O dissolves 72.3 g. anhydrous, or Aluminum potassium sulphate (Potash alum), KA1(SO 4 ) 2 +12H 2 O or K 2 A1 2 (SO 4 ) 4 = K 2 SO 4 , A1 2 (SO 4 ) 3 +24H 2 O. 138.4 g. hydrated salt, or 0.28 g. mol. of anhydrous salt at 25. (Locke, Am. Ch. J. 1901, 26. 175.) Sol. in H 2 O with absorption of heat. Solubility in H 2 O at t. When 100 pts. H 2 O at 10.8 are mixed with J A _~J.-. -I, J-T J - 1 J -t A O (g. alum in 1000 g. H 2 O.) 14 pts. all iin, T/ue w jiup. is 10 kvereu i.. (Rudorff, B. 2. 68.) t g. alum t g. alum Burnt alum is very slowly sol. in H 2 O. 57.0 75 1280.9 100 pts. H 2 O at t dissolve P pts. K 2 Al2(S'04)4+24H 2 O. 5 76.3 76 1412.1 t P t P 10 84.9 77 1517.9 15 103 6 78 1680 1 12.5 7.6 50.0 46.7 20 120.3 79 1775.2 21.25 25 10.4 22 62.5 75.0 230.0 920.0 25 131.3 80 1950.0 37^5 44^1 87 '.5 1566' 6 30 184.9 82 2273.5 36 204.3 84 2661.5 (Brandas, 1822.) 40 250.0 Orr 84.6 2816.0 Sol. in 18 pts. cold, and 1.6 pts. boiling H 2 O (Four- 45 290.2 85.1 ' 3166.6 croy); in 14.12 pts. cold, and 0.75 pt. boiling H 2 O (Bergmann); in 15 pts. cold, and 0.75 pt. boiling H 2 O (Dumas); in 11.7 pts. H 2 O at 18.75 (Abl). 50 55 367.8 457.7 85.3 85.6 3337.2 3372.2 100 pts. H..O dissolve 14.79 pts. alum at 15.56, and 60 585.4 86 3997.8 133.33 pts. at 100. (Ure's Diet.) K 2 Al 2 (SO 4 )4+Aq sat. at 15 contains 10.939 pts. alum in every 100 pts. H 2 O. (Michel and Krafft.) 65 70 708.4 943.8 87 88 4825.4 6639.6 K2Al2(SO4) 4 ~|~AQ S8.t. in cold contains o^yo slum (Fourcroy), 6.7% (Boerhave). (Marino, Gazz. ch. it. 1905, 35. (2) 351.) SULPHATE, ALUMINUM POTASSIUM 923 Solubility in H 2 O at t. B.-pt. of K 2 Al 2 (SO 4 ) 4 +Aq containing pts. K 2 AVSO 4 ) 4 to 100 pts. H 2 O. t (S0 4 )4 per 100 g. H 2 g. K 2 Ah per 100 g. H 2 O g. mol. K 2 A1 2 (S0 4 )4 perlOOg.H 2 B.-pt. Pts. K2A1 2 (S0 4 ) 4 B.-pt. Pts. K 2 A1 2 (S0 4 ) 4 o 3 5 65 0058 100.5 17.0 104 .0 83.9 5 3 5 6 62 0088 101.0 30.2 104 .5 90.7 10 4 7 60 0077 101.5 41.8 105 .0 97.6 15 5 9 59 0097 102.0 51.6 105 .5 103.9 20 5 9 11 40 0114 102.5 60.4 106 .0 110.5 25 7 23 14 14 0140 103.0 68.7 106 .5 116.9 30 8.39 16.58 0.0162 103.5 76.7 106 .7 120.55 40 50 11.70- 17.00 23.83 36.40 . 0227 0.0329 (Gerlach, Z. anal. 26. 435.) 60 70 80 90 24.75 40.00 71.0 109.0 57.35 110.5 321.3 2,275.0 0.0479 0.0774 0.01374 0.2110 K 2 A1 2 (S0 4 >4+A1 2 (S0 4 )3. K 2 A1 2 (SO 4 ) 4 is nearly insol. in sat. A1 2 (SO 4 ) 8 +Aq. (Crum, A. 89. 156.) 92 5 119 oo 2318 Solubility in AVSOi) 3 4-Aq Solid Pha,sp = (Mulder, Poggiale, Locke; Marino, Gazz. K alum-fAl 2 'SO 4 ) 3 . ch. it. 1905, 35. (2) 351; and Berkeley, Proc. Roy. Soc. 1904, 203. A, 214, calc. by Seidell, t g ' in lOOoV. H 2 O 2 g. K 2 S0 4 in 1000 g. H 2 O Solubilities, 1st Ed.) 234.73 23.45 20 824.25 30.85 35 911.02 35.29 M.-pt. of K 2 A1 2 (SO 4 ) 4 +24H 2 O=84.5 (Tilden, Chem. Soc. 45. 409.); =92.5 (Erd- mann); =91(Locke). 50 65 77 1,243.21 1,598.00 1,872.11 59.55 119.43 183.80 1.045 (Anthon); at 15 = 1.0488 (Michel and Krafft); at 15 = 1.0456 (Stolba). Sp. gr. of K 2 Al 2 (SO 4 ) 4 +Aq at 15 con- taming 5% K 2 A1 2 (SO 4 ) 4 = 1.0477. (Kohl- rausch, W. Ann. 1879. 1.) gr. of K2Al 2 'SO 4 ) 4 +Aq at 15. K 2 AVSO 4 ) 4 +24H 2 O in 100 pts. pts. solu- tion; b=pts. K 2 AVSO 4 ) 4 in 100 pts. solution; c = pts. K 2 AVSO 4 ) 4 for 100 pts. H 2 0. a . b c Sp. gr. 4 8 12 13 2.1792 4.3584 6.5376 7.083 2.2277 4.5570 6.9950 7.622 1.0210 1.0420 1.0641 1.0690 (Gerlach, Z. anal. 27. 280.) Saturated solution boils at 111.9, and contains 210.6 pts. K 2 A1 2 (SO 4 ) 4 +24H 2 O to lOOpts. H 2 O. (Mulder.) 100 pts. H 2 O contain 52 pts. K 2 A1 2 (S0 4 ) 4 , and boils at 104.5. (Griffiths.) Crust forms at 106.3, when the solution contains 114.2 pts. K 2 A1 2 (SO 4 ) 4 to 100 pts. H 2 O. (Gerlach, Z. anal. 26. 426.) (Marino, Gazz. ch. it. 1905, 35. (2) 351.) Solubility is decreased by presence of Na alum. (Venable, C. N. 1879, 40. 198.) Nearly completed pptd. from sat. aq. solution by addition or Fc or Cr alum. (v. Hauer, J. B. 1866. 59.) K 2 Al 2 (S0 4 ) 4 +MgS0 4 . K 2 AVSO 4 ) 4 +Aq sat. at 10, and then sat. with MgSO 4 at 9, contains for 100 pts. H 2 Alum (anhydrous) . MgSO 4 .... At 10 At 9 4.0 2.7 31.2 33.9 31 .'l (Mulder.) K 2 Al 2 (S0 4 ) 4 +k 2 S0 4 . K 2 Al 2 (SO 4 ) 4 +Aq at 10, and then sat. with K 2 SO 4 at same temp., contains for 100 pts. H 2 O Alum (anhydrous) K 2 S0 4 . . . At 10 At 9 4.0 0.86 9.16 9'7 10.20 (Mulder.) 924 SULPHATE, ALUMINUM RUBIDIUM Solubility in K 2 SO4+Aq. Solid phase = K alum+K 2 SO 4 . Aluminum rubidium sulphate. Al 2 Rb 2 (S0 4 )4 +24H 2 0. 100 pts. H 2 O dissolve 2.27 pts. at 17; very sol. in hot H 2 O. (Redtenbacher, J. pr. 94. 442.) Solubility in 100 pts. H 2 O at t (calculated for salt dried at 130). t A1 2 (SO 4 ) 3 +18H 2 O in 1000 g. H 2 O g. K 2 S0 4 in 1000 g. H 2 O t A1 2 (SO 4 ) 3 +18H 2 O in 1000 g. H 2 g. K 2 S0 4 in 1000 g. H 2 0. 0.5 5. 10 15 30 5.06 8.658 16.07 18.52 20.56 39.60 75.83 75.18 85.78 96.50 109.30 147.80 40 50 60 70 80 73.88 126.00 249.70 529.01 1,044.04 163.10 195.40 238.80 323.74 517.27 t Pts. alum t Pts. alum t Pts. alum 10 17 0.71 1.09 1.42 25 35 50 1.85, 2.67 4.98 65 80 9.63 21.60 (Marino, I. c.) K 2 Al 2 (S0 4 ) 4 +Na 2 S0 4 . K 8 Al 2 (SO 4 )4+Aq sat. at 10, and then sat. with Na 2 SO at 9, contains for 100 pts. 1 2 U t Pts. per litre G. mo Is. anhydrous salt per litre Alum (anhydrous) Na 2 SO 4 .... At 10 At 9 4.0 4.1 8.8 SA 25 30 35 40 18.1 21.9 26.6 32.2 0.059 0.072 0.087 0.106 12.9 Solubility of K 2 A1 2 (S0 4 ) 4 +T1 2 A1 2 (S0 4 ) 4 in H 2 O at 25. G. K 2 A1 2 (S0 4 )4 per 1. G. T1 2 A1 2 (S0 4 )4 per 1. Solid phase Mol. % K 2 A1 2 (S0 4 ) 4 Sp. gr. 69.90 0.00 100 1.0591 74.56 0.48 99.61 1.0601 67.90 1.72 98.48 1.0598 65.30 4.52 95.45 1.0603 64.95 9.60 91.73 1.0605 53.23 18.44 82.54 1.0609 45.32 24.60 75.12 1.0609 38.02 32.48 65.73 1.0611 34.54 35.59 61.36 1.0611 28.35 42.99 51.93 1.0623 10.94 66.12 21.34 1.0654 0.00 75.46 0.00 1 . 0674 (Foch, Z. Kryst. Min. 1897, 28. 397.) Insol. in alcohol of 0.905 sp. gr. or less (Anthon, J. pr. 14. 125.) Insol. in acetone. (Naumann, B. 1904 37. 4328.) Insol. in methyl acetate. (Naumann, B 1909, 42. 3790.) Solubility in H 2 O is increased by glycerine (Dunlop, Pharm. J, 1910, 31. 6.) Min. Kalinite. +8H 2 O. Stable in dry air. (Marino, I. c.] + 14H 2 O. Converted into ord. alum in air. (Marino.) (Setterberg, A. 211. 104) Solubility in H 2 O. (Locke, Am. Ch. J. 1901, 26. 180. Melts in crystal H 2 O at 99 (Tilden, Chem. Soc. 45. 409); at 105 (Erdmann); at 109 (Locke.) Aluminum silver sulphate, Al 2 Ag 2 (SO 4 ) 4 + 24H 2 O. Decomp. by H 2 O. (Church and North- cote, C. N. 9. 155.) Aluminum sodium sulphate, Al 2 Na 2 (SO 4 ) 4 -f 24H 2 O. Very si. efflorescent. Sol. in 2.14 pts. H 2 O at 13, or 100 pts. H 2 O dissolve 46.7 pts. soda alum. Sol. in 1 pt. boiling H 2 O. (Zellner, Schw. J. 36. 183.) 100 pts. H 2 O dissolve 110 pts. at 15.5, and form a liguid of 1.296 sp. gr. (Ure.) 100 pts. H 2 O dissolve 51 pts. soda alum at 16. (Aug6, C. R. 110. 1139.) 100 pts. H 2 O dissolve 110 pts. soda alum at 0. (Tilden, Chem. Soc. 45. 409.) 100 g. H 2 O dissolve at: 10 15 20 25 30 36 . 7 38 . 7 40 . 9 43 . 145 . 8 g. anhydrous salt. (Smith, J. Am. Chem. Soc. 1909, 31. 247.) M.-pt. of Na 2 Al 2 (SO 4 ) 4 +24H 2 O = 61. (Tilden, Chem. Soc. 45. 409.); =63. (Locke, Am. Ch. J. 1901, 26. 183.) Insol. in absolute alcohol. (Zellner.) Min. Mendozite. SULPHATE, AMMONIUM 925 Aluminum thallous sulphate, T1A1(SO 4 ) 2 . 0.177 g. mols. of anyhydrous salt are sol. in 1 1. H 2 O at 25; or 1 1. H 2 O dissolves 75 g. of the anhydrous, or 117.8 g. of the hydrated salt at 25. (Locke, Am. Ch. J. 1901, 26. 175.) Solubility in H 2 O at t. t G. A1 2 T1 2 (S0 4 )4 in 100 g. H 2 O G.A1 2 T1 2 (S0 4 ) 4 +24H 2 in 100 g. H 2 O 3.15 4.84 5 3.80 5.86 10 4.60 7.12 20 6.40 10.00 25 7.60 11.95 30 9.38 14.89 40 14.40 23.57 50 22.50 38.41 60 35.36 65.19 (Seidell, Solubilities, 1st Ed., p. 15.) 3A1 2 (SO 4 ) S , T1 2 SO 4 +96H 2 O. Sol. in H 2 O. (Lamy.) Aluminum zinc sulphate, A1 2 (SO 4 ) 3 , ZnSO 4 + 24H 2 0. Sol. inH 2 O. (Kane.) Aluminum sulphate chromium chloride, Al(OH 2 ) 6 (SO 4 ) 2 CrCl 2 (OH 2 ) 4 +2H 2 O. (Werner, B. 1906, 39. 337.) Aluminum sulphate sodium fluoride. Decomp. by H 2 O. (Weber, Dingl. 112.) 263. Ammonium sulphate, (NH 4 ) 2 SO 4 . Sol. in H 2 O with absorption of heat. 75 pts. (NH 4 ) 2 SO 4 mixed with 100 pts. H 2 O lower the temperature from 13.2 to 6.8, that is, 6.4. (Riidorff, B. 2. 68.) Sol. in 1.31 pts. H 2 O at 19. (Schiff, A 109. 326.) Sol. in 2 pts. H 2 O at 18.75. (Abl.) Sol. in 2 pts. H 2 O at 15.6, and in 1 pt. boiling H 2 O. (Fourcroy.) 100 pts. H 2 O at 62.6 dissolve 78 pts. (NH 4 )2SO 4 . (Wenzel.) 100 pts. H 2 O at 15 dissolve 66.739 pts. (NH 4 ) 2 SO 4 . (Michel and Krafft.) Sol. in 1.3 pts. cold H 2 O. (Vogel, N. Rep. Pharm. 10. 9.) Sol. in 1.37 pts. cold H 2 O at 10. (Mulder, J. B. 1866. 67.) Sol. in 1.34 pts. H 2 at 16-17. (v. Hauer, W. A. B. 53, 2. 221.) 100 pts. H 2 O dissolve at: 10 20 30 71.00 73.65 76.30 78.95 pts. (NH 4 ) 2 SO 4 , 40 50 6'0 70 81.60 84.25 86.90 89.55 pts. (NH 4 ) 2 SO 4 , r>/-vO f\nO -I O 80 92.20 90 C 94.85 97. 50 pts. (NH 4 ) 2 SO 4 . ^-ttjmaru, \*>. .EX. u7. uuu.,; Solubility in 100 pts. H 2 O at t. t J t jj 6 t 4 z 5 6 70.6 37 80.1 74 93.1 1 70.9 38 80.4 75 93.4 2 71.1 39 80.7 76 93.8 3 71.4 40 81.0 77 94.2 4 71.6 41 81.3 78 94.5 5 71.8 42 81.7 79 94.9 6 72.1 43 82.0 80 95.3 7 72.3 44 82.3 81 96.6 8 72.5 45 82.7 82 96.0 9 72.8 46 83.0 83 96.4 10 73.0 47 83.3 84 96.8 11 73.2 48 83.7 85 97.2 12 73.5 49 84.0 86 97.6 13 73.7 50 84.4 87 98.0 14 74.0 51 84.7 88 98.4 15 74.2 52 85.1 89 98.8 16 74.4 53 85.5 90 99.2 17 74.7 54 85.8 91 99.6 18 74.9 55 , 86.2 92 100.0 19 75.1 56 86.6 93 100.4 20 75.4 57 86.9 94 100.8 21 75.7 58 87.3 95 101.2 22 75.9 59 87.7 96 101.6 23 76.2 60 88.0 97 102.1 24 76.4 61 88.4 98 102.5 25 76.7 62 88.7 99 102.9 26 76.9 63 89.1 100 103.3 27 77.2 64 89.5 101 103.8 28 77.5 65 89.9 102 104.2 29 77.8 66 90.2 103 104.6 30 78.0 67 90.6 104 105.1 31 78.3 68 90.9 105 105.5 32 78.6 69 91.3 106 106.0 33 78.9 70 91.6 107 106.5 34 79.2 71 92.0 108 107.0 35 79.5 72 92.4 108.9 107.5 36 79.8 73 92.7 ... ... (Mulder, calculated from his own and other observations, Scheik. Verhandel. 1864. 60.) 100 g. (NH 4 ) 2 SQ 4 +Aq contain 41.4 g. (NH 4 ) 2 SO 4 at 0. (de Waal, Dissert. 1910); 44.27 g. at 30. (Schreinemakers, Z. phys. Ch. 71. 110); 47.81 g. at 70. (de Waal.) (NH 4 ) 2 SO 4 +Aq sat. at 15 has sp. gr. 1.248. (Michel and Krafft, A. ch. (3) 41. 471.) 926 SULPHATE, AMMONIUM Sp. gr. of (NH 4 ) 2 SO 4 +Aq at 15. Sp. gr. of (NH 4 ) 2 S0 4 +Aq. % (NH)2S04 1 Sp. gr. o s W Sp. gr. 1 g Sp. gr. H(NH 4 ) 2 f in 1000 g 3O 4 g. mol. of solution Sp. gr. 16/16 0. 1. 2. 4. 10. 20. 40. 56. 5514 1251 3114 5840 0893 0138 5236 8536 1.000000 1.000347 1.000704 1.001436 1.002823 1.006093 1.012023 1.024117 1.033690 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 .0057 .0115 .0172 .0230 .0287 .0345 .0403 .0460 .0518 .0575 .0632 .0690 1.0747 1.0805 1.0862 1.0920 1.0977 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 1.1035 1.1092 1.1149 1.1207 1.1265 1.1323 1.1381 1.1439 1 . 1496 1 . 1554 1.1612 1.1670 .1724 .1780 .1836 .1892 .1948 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 1.2004 1.2060 .2116 .2172 .2228 .2284 .2343 .2402 1.2462 1.2522 1.2583 1.2644 1.2705 1.2766 1.2828 1.2890 (Dijken, Z. phys. Ch. 1897, 24. 107.) Sp. gr. of (NH 4 ) 2 SO 4 +Aq at 20. Normality of hAq % (NH 4 ) 2 S04 Sp. gr. 3.75 2.964 1.978 0.876 0.492 40.28 32.99 23.01 10.88 6.275 1 1 1 1 1 .2289 .1858 .1319 .0626 .0352 (Schiff, calculated by Gerlach, Z. anal. 8. 280.) Sp. gr. of (NH 4 ) 2 SO 4 +Aq at 15. (Forchheimer, Z. phys. Ch. 1900, Sp. gr. of (NH 4 ) 2 SO 4 +Aq at 34. 22.) 20. Solution Sp gr. weight of 10 ccm. of the solution (NH 4 ) 2 SO4 1 Sp. gr. W Sp. gr. H fc Sp. gr. sat. 1/4 ;; v! Vs " 1.24& 1.196 1.139 1.077 1.039 12. 5062 g. 11.9034" 11.3377 " 10.7232 " 53.2 39.9 26.6 13.3 6.65 (Wiener, Z. phys. Chem. 1911, 71. 120.) B.-pt. of sat. solution: crust formed at 106.2, solution containing 88.2 pts. (NH 4 ) 2 SO 4 to 100 pts. H 2 0; highest temp, observed, 108.2. (Gerlach, Z. anal. 26. 426.) 5 10 1.0292 1.0581 20 30 1.1160 1.1730 31 1 . 1787 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of (NH 4 ) 2 SO 4 +Aq at 15. B.-pt. of (NH 4 ) 2 SO 4 +Aq containing pts. (NH 4 ) 2 SO 4 to 100 pts. H 2 O. % (NH 4 ) 2 S04 Sp. gr. W Sp. gr. 1 Sp. gr. 3 6 1.0181 1.0359 10 20 1.0600 1.1190 30 40 1.1773 1.2352 (Gerlach, Z. anal. 28. 493.) Sp. gr. of sat. solution = 1.248. (Ger- lach.) B.-pt. Pts. (NH4) 2 SO4 B. pt. Pts. (NH 4 ) 2 SO4 100.5 101.0 101.5 102.0 102.5 103.0 103.5 104.0 104.5 7.8 15.4 22.8 30.1 37.2 44.2 51.1 58.0 64.9 105.0 105.5 106.0 106.5 107.0 107.5 108.0 108.2 71.8 78.7 85.5 92.3 99.1 105.9 112.6 115.3 (Gerlach, Z. anal. 26. 431.) Sol. with decomp. in HCl+Aq. SULPHATE, AMMONIUM 927 Solubility in H 2 SO 4 +Aq at 25. 100 g. of the solution contain Mol. H2S04 0.00 0.24 0.47 0.97 1.19 1.43 1.72 2.20 .60 .71 ,82 .96 .20 3.32 3.47 3.54 3.76 4.22 5.09 Mol. (NH 4 ) 2 SC>4 2.28 3.25 3.19 3.15 3.15 3.22 3.18 3.02 2.97 3.00 3.03 3.10 3.19 3.25 3.32 3.20 2.84 2.26 1.44 Solid phase (NH 4 ) 2 S0 4 (NH 4 ) 3 H(S0 4 ) 5 (NH 4 )HSO< (D'Ans, Z. anorg. 1909, 65. 229.) Solubility in H 2 SO 4 +Aq at 30. Composition of the solution by wt. H 2 S0 4 10.63 10.70 13.18 16.67 25.82 27.33 32.32 33.12 33.84 33.96 38.51 42.12 45.80 45.77 56.55 62.43 62.46 63.12 62.57 62.83 62.56 62.67 62.59 61.63 62.23 by wt. (NH 4 ) 2 SO 43.59 43.25 44.10 42.06 41.15 41.16 44.63 45.50 45.52 45.31 35.37 30.10 24.88 24.30 16.98 20.41 24.40 24.20 27.67 29.75 30.26 31.86 33.70 36.75 36.95 u by wt. H 2 O 45.79 46.05 42.72 41.27 33.03 31.51 22.26 21.83 20.64 20.73 26.12 27.78 29.32 29.93 26.37 17.16 13.14 12.68 9.76 8.42 7.28 5.47 3.71 1.72 0.82 Solid ph (NH 4 ) 2 S0 4 (NH 4 ) 2 S0 4 + 3(NH 4 ) 2 S04, H 2 8O. 3(NH 4 ) 2 S0 4 , H 2 S0 4 (NH 4 )HS0 4 Solubility of (NH 4 ) 2 SO 4 in H 2 SO 4 +Aq at 25. (Van Dorp, Z. phys. Ch. 1910, 73. 285.) In 1000 g. of the solution Solid phase Mol. SOs Mol. (NH 4 ) 2 S04 4.29 2.17 4.57 1.83 (NH 4 )HS0 4 4.85 1.60 5.25 1.36 5.66 1.22 6.16 1.26 6.47 1.55 (NH 4 )HS0 4 6.51 1.95 6.50 2.37 6.43 2.50 (NH 4 )HS0 4 +(NH 4 )H 3 (S0 4 ) 8 7.28 1.64 7.99 1.38 (NH 4 )H 3 (S0 4 ) 2 (7.60) (1.74) (8.00) (1.42) 9.02 0.96 9.21 0.832 (NH 4 )HS 2 O 7 9.60 0.977 9.68 1.00 9.67 1.26 (NH 4 )HS 2 7 +? 10.43 0.894 (D'Ans, Z. anorg. 1913, 80. 241.) Very easily sol., even in cone. NH 4 OH-f- Aq. (Girard, Bull. Soc. (2) 43. 522.) Solubility of (NH4)2SO 4 inNH 4 OH+Aqat25 . In 1000 g.of the solution Mol. (NH 4 ) 2 S04 3.28 2.60 2.13 1.59 1.16 0.78 Mol. (NH 3 ) 2 1.02 1.95 3.44 5.35 7.13 9.47 (D'Ans and Schreiner, Z. anorg. 1910, 67. 438.) 100 pts. H 2 O dissolve 46.5 pts. (NH 4 ) 2 SO 4 and 26.8 pts. NH 4 C1 at 21.5. Solubility of (NH 4 ) 2 SO 4 in NH 4 Cl+Aq at 30. Solid phase % NtuCl 6.86 14.62 17.60 17.93 19.07 19.97 22.3 24.06 29.5 (NH 4 ) 2 SO 4 44 36.15 28.6 25.69 25.81 23.22 21.3 16.33 12.72 (NH 4 ) 2 S0 4 a (i (NH 4 ) 2 SO 4 +NH 4 C1 it NH 4 C1 Schreinemakers, Arch. Neer. Sc. 1910, (2) 16. 92.) See also under NH 4 C1. 928 SULPHATE, AMMONIUM (NH 4 ) 2 S0 4 +CuS0 4 . Solubility of (NH 4 ) 2 SO 4 +CuSO 4 in H 2 O at 16. Solution Both salts in excess 15 cc. sat. sol. +3 g. (NH 4 ) 2 SO 4 15 cc. sat. sol. +3 g. CuSO,5H 2 O 8.55 1.77 15.85 7.12 18.16 5.65 (Riidorff, B. 6. 482.) Solubility of (NH 4 ) 2 SO 4 +CuSO 4 in H 2 O at 30. 2.45 5.79 6.98 8.19 9.33 17.53 29.27 38.32 43.29 44 20.32 20.19 20.53 16.77 13.65 11.03 4.05 1.57 0.77 0.49 Solid phase CuSO4.5H 2 O CuS0 4 , 5H 2 0+CuS04, (NH 4 ) 2 SO 4 6H 2 CuS0 4 , (NH 4 ) 2 S0 4 .6H 2 CuSO 4) (NH 4 )2S04.6H 2 + (NH 4 ) 2 SO 4 (NH4) 2 SO4 (Schreinemakers, Arch. Ne'er. Sc. 1910, 15. 12.) See also under CuSO 4 . (NH 4 ) 2 S0 4 +FeS0 4 . Solubility of (NH 4 ) 2 SO 4 +FeSO 4 in H 2 O + Aq at 30. Composition of the solution % F by wt. eSO 4 24.90 25.24 25.22 25.26 23.59 17.64 13.13 7.95 5.70 1.72 0.79 0.79 by wt. 5.24 5 . 93 5.89 6 . 44 8.90 11.45 16.29 19.64 34.24 43 . 86 43.90 44.27 Solid phase FeSO 4 , 7H 2 FeSO 4 , 7H 2 O + FeSO4, (NH 4 ) 2 SO 4> 6II 2 O FeS04, (NH 4 ) 2 SO4, 6H 2 O FeSO4, (NH 4 ) 2 SO 4 , 6H 2 O + (NH 4 ) 2 S04 (Schreinemakers, Z. phys. Ch. 1910, 71. 111.) (NH 4 ) 2 S0 4 +Li 2 S0 4 . Solubility of (NH 4 ) 2 SO 4 +Li 2 SO 4 . Temp. =30. NH 4 ) 2 SO 4 44.1 40.8 39.5 30 21.6 15 12.5 8.9 Li 2 SO4 3 6.6 10 15 20 21.9 23 25.1 Solid phase (NH 4 ) 2 S0 4 (i (NH 4 ) 2 SO 4 +NH 4 LiSO 4 NH 4 LiS0 4 NH 4 LiSO 4 +Li 2 SO 4 , H 2 O Li 2 SO 4 , H 2 O Temp. =50. 45.7 1 (NH 4 ) 2 S0 4 43.05 5.86 (NH 4 ) 2 SO 4 +NH 4 LiSO 4 19.65 16.35 NH 4 LiSO 4 13.90 21.20. tt 13.97 21.23 NH 4 LiSO 4 +Li 2 SO 4 , H 2 O 11.45 21.75 Li 2 S0 4 , H 2 O 9.63 22.79 tt 8.58 23.09 tf 7.56 23.86 " 24.3 tt (Schreinemakers and Cocheret, Chem. Weekbl. 1905, 2. 771.) (NH 4 ) 2 SO 4 +MnSO 4 . Solubility of (NH 4 ) 2 SO 4 +MnS0 4 in H 2 O. G. per 100 g. sat. solution. Temp. =30. MnSO 4 (NHi) 2 SO, 39.3 38.49 33.44 22.06 9.02 2.91 1.75 1.77 3.64 4.91 9.65 20.36 37.42 42.58 43.24 43.4 Solid phase MnSO 4 , 5H 2 O MnSO 4 , 5H 2 O+MnS0 4 , (NH 4 ) 2 S0 4 , 6H 2 MnSO 4 , (NH 4 ) 2 SO 4 , 6H 2 O +(NH 4 ) 2 S0 4 fNH 4 ) 2 S0 4 Temp. =50. 36.26 MnSO 4| H 2 O 35.35 2.95 MnSO 4 , H 2 O+2MnS0 4 , (NH 4 ) 2 S0 4 30.57 5.14 2MnSO 4 , (NH 4 ) 2 SO 4 16.86 17.62 M 6.92 35.98 w 6.29 39.71 5.70 43.24 2MnSO 4 , (NH 4 ) 2 SO 4 + (NH 4 ) 2 S0 4 3.49 44.02 (NH 4 ) 2 S0 4 45.7 it (Schreinemakers, Chem. Weekbl. 1909, 6. 131.) SULPHATE, AMMONIUM 929 (NH 4 ) 2 SO 4 +K 2 SO 4 . 100 pts. (NH 4 ) 2 SO 4 +K 2 SO 4 +Aq sat. 16.17 contain 38.41 pts. of the two salts of which 5.45 pts. are K 2 SO 4 , and 32.96 pts (NH 4 ) 2 SO 4 . (v. Hauer, J. pr. 28. 137.) 100 pts. H 2 O dissolve 50.6 pts. (NH 4 ) 2 SO and 7.2 pts. K 2 SO 4 at 11. (Mulder, J. B 1866. 67.) (NH 4 ) 2 S0 4 and K 2 SO 4 replace each other in solution, so that by adding one of these salts to a seemingly saturated solution of the other, it is dissolved with pptn. of the other salt. (RUdorff, B. 6. 485.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 826.) Insol. in absolute alcohol. Sol. in 500 pts alcohol of 0.872 sp. gr., and in 62.5 pts. of 0.905. sp. gr. (Anthon, J. pr. 14. 125.) Sol. in 217.4 pts. of 66.8% alcohol (sp. gr. = 0.88) at 24.3. (Pohl, J. pr. 66. 219.) Tolerably sol. in alcohol, the sp. gr. of which is greater than 0.860. Insol. in alcohol of sp. gr. less than 0.850. Solubility in dil. alcohol. Solubility of (NH 4 ) 2 SO 4 +K 2 SO 4 at 19.1. When (NH 4 ) 2 SO 4 is dissolved in dil. alcohol, two layers are formed, the compositions of which are as follows: Solution & 6 ? ^s Sp. gr. Lower layer 100 ccm. contain in g. Both salts in excess 15 cc. sat. sol.+4g. K 2 SO 4 15 cc. sat. sol. +4 g. (NH 4 ) 2 SO 4 39.3 4.94 2.05 37.97 33.26 40.80 alcohol water salt .2240 .1775 .1661 .1655 .1735 8.'85 10.62 11.29 11.42 71.43 68.26 67.70 67.34 66.54 74.16 59.54 56.56 56.30 59.20 (Rudorff, B. 6. 482.) Solubility of (NH 4 ) 2 SO 4 +K 2 SO 4 in H 2 O at 25. Sp. gr. Upper layer 100 ccm. containing. g. K 2 S0 4 perl. g.(NH^ 2 SOi par 1. g. KaSCh p^r 1. g. (NH 4 ) 2 S04 per 1. alcohol water salt 0.9530 0.9512 0.9440 0.9098 0.8750 0.8549 0.8308 41.37 44.20 44.27 52.64 62.61 67.04 77.55 48.47 45.95 45.61 36.78 24.60 18.36 5.53 5.45 4.97 4.51 1.56 0.30 0.09 0.00 127.9 135.7 84.2 0.0 115.7 281 . 1 59.28 40.27 0.0 355.0 482.7 542.3 Results are also given for 14, 15, 16, 30, 46 and 47. (Tock. Z. Krvst. Min. 1897. 28. 365.) (NH 4 ) 2 S0 4 +Th(S0 4 ) 2 . Solubility of (NH 4 ) 2 SO 4 +Th(SO 4 ) 2 at 16< Pts. per 100 pts. H 2 O. (Bodlander, Z. phys. Ch. 7. 3, 8.) Solubility in ethyl alcohol +Aq. (NH 4 ) 2 SO< I J3 h Solid phase Upper layer Temp. g. H 2 g. alcohol g. salt 2.13 4.80 10.02 16.56 28.00 35.20 15.14 49.05 >2.88 39.74 3.361 5.269 8.947 13.330 10.359 9.821 6.592 5.750 4.583 1.653 Th(SO 4 ) 2 .9H 2 O Tt (t Th(SO 4 ) 2 , 9H 2 O+Th(SO 4 ) 2 , (NH 4 ) 2 SO 4 .4H 2 O TMSO 4 ) 2 . (NH 4 ) 2 SO 4 .4H 2 O " +Th(S0 4 ) 2 , 2(NH 4 ) 2 S0 4 . 2H 2 O Th(SO 4 ) 2 , 2(NH 4 ) 2 S0 4 .2H 2 O Th(S0 4 ) 2 , 3(NH 4 ) 2 S0 4 .3H 2 16.6 33.0 41.8 55.7 52.80 47.99 47.34 45.90 40.21 46.75 47.67 49.47 6.99 5.26 4.99 4.63 Lower layer 16.6 33.0 41.8 55.7 60.33 61.02 61.16 61.59 10.19 9.80 9.74 9.46 29.48 29.18 29.10 28.95 (Traube, Z. phys. Ch. 1887, 1. 509.) (Barre, A. ch. 1911, (8) 24. 239.) * 930 SULPHATE, AMMONIUM HYDROGEN Solubility of (NH 4 ) 2 SO 4 in alcohol at 30. Two liquid layers are formed between al- cohol concentrations of 5.8 and 62. Composition of layers. Solubility in propyl alcohol +Aq at 20. % propyl alcohol % (NH 4) 2 SO 4 20 30 40 50 60 70 6.7 4.8 3.2 2.0 1.0 0.4 Upper layer Lower layer W(;HN) % ! it 4 1 Ml (Linebarger, Am. Ch. J. 1892, 14. 380.) 100 g. 95% formic acid dissolve 25.4 g. (NH 4 ) 2 SO 4 at 16.5. (Aschan, Ch. Ztg. 1913, 37. 1117.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329). Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) 2.2 2.6 3.4 13.2 17 56.6 54.5 52.3 31.8 25 41.2 42.9 44.3 55 58 37.1 35.7 33.8 21.7 17 5.8 6.3 7.4 18.4 25 57.1 58 58.8 59.9 58 At concentration of 62% alcohol, the liquid is homogeneous and contains 1.3% (NH 4 ) 2 S0 4 . (Wibaut, Chem. Weekbl. 1909, 6. 401.) Solubility of (NH 4 ) 2 S0 4 in alcohol at 60. % (NH4) 2 SO 4 % alcohol %H 2 43.02 41.1 2.32 4.1 54.66 54.8 1.2 0.2 64^5 75.5 34~3 24.3 Between 4.1 and 64.5, two liquid layers are formed. Composition of layers. Upper layer Lower layer 6 1 "o fa J B g *i "us o o 1.2 1.6 3.8 7.4 10 64.5 60 50 40 34.4 34.3 38.4 46.2 52.6 55.6 41.1 36.8 30.8 26.6 23.6 4.1 6 9 12 15 54.8 57.2 60.2 61.4 61.4 (Schreinemakers, Z. phys. Ch. 1907, 59. 641.) Solubility in alcohol +Aq at 0. % (NH 4 ) 2 SO4 % alcohol %H 2 41.4 30.0 9.41 58.6 60.59 '6.i4 73^03 26 '83 Two layers are formed between alcohol concentrations of 9.41 and 73.03%. (de Waal, Dissert. 1910.) Ammonium hydrogen sulphate, NH 4 HSO 4 . SI. deliquescent. Sol. in 1 pt. cold H 2 0. (Link.) Very si. sol. in alcohol. (Gerhardt, A. ch. (3) 20. 255.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II, 1014.) (NH 4 ) 3 H(SO 4 ) 2 . Not deliquescent. Sol. in H 2 O. (Mitscherlich, Pogg. 39. 198.) (NH 4 ) 2 SO 4 , 3H 2 SO 4 .) D'Ans and Schreiner, Z. anorg. 1913, 80. 241.) Ammonium pz/rosulphate, (NH 4 ) 2 S 2 O 7 . Decomp. by H 2 O. (Schulze.) NH 4 HS 2 O 7 . (D'Ans and Schreiner, anorg. 1913, 80. 241.) Z. Ammonium ocfosulphate, (NH 4 ) 2 S 8 O 26 . Decomp. by H 2 O. (Weber, B. 17. 2497.) Ammonium antimony sulphate, (NH 4 ) 2 SO 4 ,Sb 2 (SO 4 ) 3 . Behaves toward H 2 O and abs. alcohol as a mixture of the components. (Metzl, Z. anorg. 1805, 48. 152.) Decomp. very slowly by H 2 O. (Gut- mann, Arch. Pharm. 1898, 236. 479.) Ammonium bismuth sulphate, NH 4 Bi(SO 4 ) 2 +4H 2 0. Easily sol. in HC1, and HNO 3 +Aq; less sol. in cone. H 2 SO 4 , and hot dil. acids. Slowly decomp. by cold HC 2 H 3 O 2 , and dil. H 2 SO 4 + Aq.. (Liiddecke, A. 140. 277.) Ammonium cadmium sulphate, (NH 4 ) 2 SO 4 . CdSO 4 +6H 2 O. Can be recrystallised from a little H 2 (v. Hauer.) 1 1. H 2 O dissolves 723 g. anhydrous sal at 25. (Locke, Am. Ch. J. 1902, 27. 459.) SULPHATE, AMMONIUM CHROMIC 931 3(NH 4 ) 2 SO 4 , CdSO 4 +10H 2 O. (Andre, C. R. 104. 987.) Ammonium calcium sulphate, (NH 4 ) 2 Ca(SO 4 ) 2 +H 2 O. Decomp. by H 2 0. (Fassbender, B. 11. 1968.) Sol. in (NH 4 ) 2 SO 4 +Aq. (Rose, Pogg. 110. 292.) pfcThis double salt is stable between and 100 in solutions containing an excess of .(NH 4 ) 2 SO 4 . It is not formed if the solution contains less than 35% (NH 4 ) 2 SO 4 . (Barre, C. R. 1909, 148. 1605.) (SO 4 ) 3 Ca 2 (NH 4 ) 2 . Decomp. by H 2 O. CD'Ans, B. 1907, 40. 192.) pkThis double salt is formed in the presence of an excess of CaSO 4 and at temp, above 80. (Barre, C. R. 1909, 148. 1605.) Ca 5 (NH 4 ) 2 (SO 4 ) 6 '+H 2 O. Decomp. by H 2 O. (D'Ans, B. 1907, 40. 192.) Ammonium calcium cupric sulphate, Ca 2 Cu(NH 4 ) 2 (SO 4 )4+2H 2 O. Very stable. (D'Ans, B. 1908, 41. 1778.) Ammonium calcium potassium sulphate, NH 4 CaK(SO 4 ) 2 +H 2 O. Decomp. by cold H 2 O. (Fassbender, B. 11. 1968.) Ammonium cerous sulphate, (NH 4 ) 2 Ce 2 (SO 4 ) 4 +8H 2 O. More sol. in cold than in hot H 2 O. (Czud- nowicz). 100 g. H 2 O dissolve at: 22.3 22.35 35.1 45.2 5.331 5.328 5. 184 4.993 g. anhydrous salt, 45 55 3 55 2 2 . 994 2 . 240 2 . 187 g. anhydrous salt, 75.4 85.2 1 . 482 1 . 184 g. anhydrous salt. (Wolff, Z. anorg. 1905, 45. 102.) 5(NH 4 ) 2 SO 4 , Ce 2 (SO 4 ) 3 . (Barre, C. R. 1910, 151. 873.) Ammonium eerie sulphate, 3(NH 4 ) 2 SO 4 , Ce(SO 4 ) 2 +4H 2 O. Slightly efflorescent. Easily sol. in H 2 O. (Mendelejeff, A. 168. 50.) 3(NH 4 ) 2 SO 4 , 2Ce(SO 4 ) 2 +3H 2 O. SI. sol. in H 2 O. (Mendelejeff.) Ammonium chromous sulphate, NH 4 Cr(SO 4 ) 2 . 0.407 g. mol. anhydrous salt is sol. in 1 1. H 2 O at 25. (Locke, Am. Ch. J. 1901, 26. 175.) +6H 2 O. 100 ccm. of sat. aqueous solution contain 55 g. of the salt at 20. Insol. in alcohol. (Laurent, C. R. 1911, 131. 112.) Ammonium chromic sulphate, (NH 4 ) 2 SO 4 , Cr 2 (S0 4 ) 3 . Not attacked by boiling H 2 O or cone. HC1 +Aq. Very slowly attacked by boiling KOH -j-Aq (sp. gr. = 1.3). Insol. in CrCl 2 +Aq or SnCl 2 +Aq. (Klobb, Bull. Soc. (3) 9. 664.) +5H 2 0. Is ammonium chromosulphate, which see. +24H 2 O. Chrome Alum. Violet modification. Efflorescent. Sol. in cold H 2 O, but solution is decomp. on heating with formation of green modification. The dil. solution of green modification is grad- ually converted into violet modification by standing. Alcohol ppts. it from aqueous solution. (Schr6tter, Pogg. 53. 526.) 100 cc. H 2 O dissolve 10.78 g. anhydrous, or 21.21 g. hydrated salt at 25. Melts in crystal H 2 O at 45. (Locke, Am. Ch. J. 1901, 26. 174.) Solubility in H a O. Saturation is very slowly reached owing to transition between violet and green modifi- cations. If time of saturation is taken , at 2 l /2 hours, 100 g. of the solution contain at: 30 40 3.77 10.6 15.5 g. (NH 4 ) 2 Cr 2 (SO 4 )4. This is assumed to be the solubility of the violet modification. In 300 hours, 15.96 g. salt are dissolved at 30, and 24.64 g. in 250 hours at 40. (Koppel, B. 1906, 39. 3741.) Calc. from electrical conductivity measure- ments, a solution containing 3.8 g. of the sulphate in 100 g. contains 48% of the green compound at 40 and- 61% at 55. With solutions of 6-7 times the above concentra- tion equilibrium is reached at 40 with 30- 40% green alum. (Koppel.) Sp. gr. of aqueous solution of violet modi- fication at 15, containing: 4 8 12% (NH 4 ) 2 Cr 2 (SO 4 ) 4 +24H 2 O. 1.020 1.0405 1.0610 Sat. solution at 15 has sp. gr. = 1.070. (Gerlach.) Green modification. Sol. in H 2 O and al- cohol. When in aqueous solution, it gradually changes to violet modification. Sp. gr. of aqueous solution of green modi- fication at 15, containing: 10 20 30% (NH 4 ) 2 Cr 2 (S0 4 ) 4 +24H 2 O, 1.044 1.091 1.142 40 50 60% (NH 4 ) 2 Cr 2 (S0 4 ) 4 +24H 2 0, 1.197 1.255 1.317 70 80 90%.(NH 4 ) 2 Cr 2 (SO 4 ) 4 +24H 2 O. 1.384 1.456 1.532 (Gerlach, Z. anal. 28. 498.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) 3(NH 4 ) 2 SO 4 , Cr 2 (SO 4 ) 3 . Only si. attacked by boiling H 2 O. Not attacked by boiling cone. (NH 4 ) 2 SO 4 +Aq. (Klobb, Bull. Soc. (3) 9. 663.) 932 SULPHATE, AMMONIUM COBALTOUS Ammonium cobaltous sulphate, (NH 4 ) 2 Co(SO4)2+6H 2 O. 100 pts. H 2 O dissolve at: 10 18 23 35 8.9 11.6 15.2 17.1 19.6 pts. anhydrous salt, 40 45 50 60 75 22.3 25 28.7 34.5 43.3 pts. anhydrous salt. (Tobler, A. 96. 193.) 100 pts. saturated solution contain at: 20 40 60 80 14.9 20.8 25.6 33 pts. anhydrous salt. (v. Hauer, J. pr. 74. 433.) Solubility of (NH 4 ) 2 Cu(SO 4 ) 2 , 6H 2 O + (NH 4 ) 2 Ni(SO 4 ) 2 , 6H 2 O in H 2 O at 13-14. Mols. per 100 mols. H 2 O. Cu salt Ni salt % Cu salt in solid phase 0.1476 0.2664 0.4165 0.4785 1.0350 0.521 0.295 0.2089 0.1449 0.1202 10.29 30.59 52.23 78.80 100 (Fock, Z. Kryst. Min. 1897, 28. 365.) 1 1. H 2 O dissolves 147.2 g. anhydrous salt at 25. Tobler's results are inaccurate. (Locke, Am. Ch. J. 1902, 27 V 459.) Pptd. from aqueous solution by alcohol. Ammonium cobaltic sulphate, (NH 4 ) 2 Co 2 (S0 4 ) 4 +24H 2 0. Sol. in H 2 O with Chem. Soc. 59. 760.) decomp. (Marshall, Ammonium cobaltous cupric sulphate, 2(NH 4 ) 2 SO 4 , CoSO 4 , CuSO 4 + 12H 2 O. Quite easily sol. in hot H 2 O, but on long boiling a basic salt is pptd. (Vohl, A. 94. 58.) Ammonium cobaltous ferrous sulphate, 2(NH 4 ) 2 SO 4 , CoSO 4 , FeSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium cobaltous magnesium sulphate, 2(NH 4 )SO 4 , CoSO 4; MgSO 4 + 12H 2 O. Sol. in H 2 O. (Vohl, A- 94. 57.) Ammonium cobaltous manganous sulphate, 2(NH 4 )SO 4; CoSO 4 , MnSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium cobaltous nickel sulphate, 2(NH 4 )SO 4 , CoSO 4 , NiSO 4 +12H 2 O. Sol. in H 2 0. (Vohl, A. 94. 57.) Ammonium cobaltous zinc sulphate, 2(NH 4 ) 2 SO 4 , CoSO 4 ,ZnSO 4 + 12H 2 O. Sol, in H 2 0. (Vohl, A. 94. 57.) Ammonium cupric sulphate, (NH 4 ) 2 SC 4 , CuSO 4 +6H 2 O. Efflorescent in warm air. Sol. in 1.5 pts. boiling H2O, and separates almost wholly on ccoling. (.Vogel, J. pr. 2. 194 Sol. in 1.55 pts. H 2 O at 18.75. (Abl.) 100 pts. H 2 O at 19 dissolve 26.6 pts., and sat. solution has sp. gr. = 1.1337. (Schiff, A. 109. 426. 100 g. sat. solution at 30 contain 30.36 g. anhydrous salt. (Schreinemakers, Arch. Ne'er. Sci. 1910, (2) 16. 92.) K salt NH 4 salt' % K salt in solid phase 1.035 0.897 0.8618 5.06 0.2269 0.6490 16.76 0.2570 0.5887 30.40 0.2946 0.5096 36.63 0.3339 0.3319 50.15 0.4560 0.1961 69.93 0.4374 100. Solubility of (NH 4 ) 2 Cu(SO 4 ) 2 , 6H 2 O + K 2 Cu(SO 4 ) 2 , 6H 2 O in H 2 O at 13-14. Mols. per 100 mols. H 2 O. (Fock.) Solubility of (NH 4 ) 2 Cu(SO 4 ) 2 , 6H 2 O + (NH 4 ) 2 Zn(SO 4 ), 6H 2 O in H 2 O at 13-14. Mols. per 100 mols. H 2 O. Cu salt Zn salt % Cu salt in solid phase 0.0422 0.0666 0.1218 0.2130 0.3216 1.035 0.8069 0.5638 0.5115 0.4924 0.4022 2.39 4.52 9.03 14.67 22.62 100. (Fock.) (NH 4 ) 2 SO 4 , 2CuSO 4 . Very sol. in H 2 O (Klobb, C. R. 115. 220.) Ammonium cupric ferrous sulphate. Sol. in H 2 O without decomposition. (Vohl, A. 94. 61.) Ammonium cupric magnesium sulphate, 2(NH 4 ) 2 SO 4 , CuSO 4 , MgSO 4 + 12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium cupric magnesium potassium sul- phate, (NH 4 ) 2 SO 4 , CuSO 4 , MgSO 4 , K 2 S0 4 +12H 2 0. Sol. inH 2 O. (Schiff.) 2(NH 4 ) 2 SO 4 , CuSO 4 , 2MgSO 4 , K 2 SO 4 + 18H 2 O. Sol. inH 2 O. (Schiff.) SULPHATE, AMMONIUM IRON 933 Ammonium cupric manganous sulphate, 2(NH 4 ) 2 SO 4 , CuSO 4 , MnSO 4 + 12 H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium cupric nickel sulphate, 2(NH 4 ) 2 SO 4 , CuSO 4 , NiSO 4 + 12H 2 O. Sol. in H 2 O. (Vohl.) Ammonium cupric potassium sulphate, NH 4 KSO 4 , CuSO 4 +6H 2 O. Sol. inH 2 O. (Schiff.) Ammonium cupric zinc sulphate, 2(NH 4 ) 2 SO 4 , CuSO 4 , ZnSO 4 +12H 2 O. Sol. inH 2 O. (Vohl.) Ammonium cupric sulphate ammonia, (NH 4 ) 2 SO 4 , CuO, 2NH 3 . Sol. in 1.5 pts. cold H 2 O, but decomp. on exposure to air or dilution. Insol. in alcohol. (Kuhn.) Ammonium didymium sulphate, (NH 4 ) 2 S0 4 , Di 2 (SO 4 ) 3 +8H 2 O. Sol. in 18 pts. H 2 O, and less easily in (NH 4 ) 2 SO 4 +Aq. (Marignac.) Moderately sol. in H 2 O. (Cleve, Bull. Soc. (2) 43. 362.) Ammonium erbium sulphate, (NH 4 ) 2 SO 4 , Er 2 (SO 4 ) 3 +8H 2 O. Sol. inH 2 O. (Cleve.) Ammonium gallium sulphate, (NH 4 ) 2 Ga 2 (SO 4 ) 4 +24H 2 O. Sol. in cold water and dilute alcohol. Cone. solution clouds up on boiling, but clears on cooling. Dil. solution separates out a basic salt, insol. in hot or cold H 2 O. (Boisbaudran.) Ammonium glucinum sulphate, (NH 4 ) 2 SO 4 , G1S0 4 +2H 2 0. Sol. in H 2 O. (Atterberg.) Ammonium indium sulphate, (NH 4 ) 2 In 2 (SO 4 ) 4 +24H 2 O. 100 pts. H 2 O dissolve 200 pts. salt at 16, and 400 pts. at 30. Insol. in alcohol. Melts in crystal H 2 O at 36. (Rossler, J. pr. (2) 7. 14.) +8H 2 O. (Rossler.) Ammonium iridium sulphate, (NH 4 ) 2 SO 4 , Ir 2 (S0 4 ) 3 +24H 2 0. Easily sol. in H 2 O. (Marino, Z. anorg. 1904, 42. 221.) Ammonium iron (ferrous) sulphate, (NH 4 ) 2 Fe(S0 4 ) 2 +6H 2 0. Much less sol. in H 2 O than FeSO 4 +7H 2 O. (Vogel, J. pr. 2. 192.) 100 pts. H 2 O dissolve at: 12 20 30 36 12.2 17.5 21.6 28.1 31.8 pts. anhydrous salt, 45 55 60 65 75 36.2 40.3 44.6 49.8 56.7 pts. anhydrous salt. (Tobler, A. 95. 193.) 100 pts. H 2 O at 16.5 dissolve 35.9 pts. hydrous salt. 1 1. H 2 O dissolves 351 pts. or 1.044 g. mol. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Sol. in H 2 O without decomp. Aq. solution at 30 contains 13.13% FeSO 4 and 11.45% (NH 4 ) 2 SO 4 . (Schreinemakers, C. C. 1910, I. 801.) Sp. gr. of (NH 4 ) 2 FeSO 4 +Aq at 19. % = %(NH 4 ) 2 FeS0 4 +6H 2 0. % Sp. gr. % Sp. gr. % Sp. gr. 1 1.006 11 .066 21 1.130 2 1.013 12 .073 22 .136 3 1.018 13 .080 23 .143 4 1.024 14 .085 24 .150 5 1.030 15 .092 25 .156 6 1.036 16 .097 26 .164 7 1.042 17 .104 27 .171 8 1.047 18 .110 28 1.179 9 1.054 19 1.116 29 1.185 10 1.060 20 1.124 30 1.193 (Schiff calculated by Gerlach, Z. anal. 8. 280.) Insol. in acetone. Ammonium ferric sulphate, basic. Extremely difficultly sol. in HCl+Aq. Not decomp. by KOH+Aq. (Berzelius.) 5(NH 4 ) 2 O, 3Fe 2 O 3 , 12SO 3 +18H 2 O or 2(NH 4 ) 2 O, Fe 2 O 3 , 4SO 3 +4H 2 O. Sol. in 2.4 pts. cold H 2 O. (Maus, Pogg. 11. 79.) Ammonium iron (ferric) sulphate, (NH 4 ) 2 SO 4 , Fe 2 (S0 4 ) 3 . Attacked slowly by cold H 2 O. (Lachaud and Lepierre.) Nearly insol. in H 2 O. (Wemland, Z. anorg. 1913, 84. 363.) +24H 2 O. Iron alum. Sol. in 3 pts. H 2 O at 15. (Forchhammer, Ann. Phil. 6. 406.) 100 cc. H 2 O dissolve 44.15 g. anhydrous, or 124.40 g. hydrated salt at 25, or 1.659 g. mols. anhydrous salt are sol. in 1 1. H 2 O at 25. (Locke, Am. Ch. J. 1901, 26. 174.) Sp. gr. of aqueous solution at 15 contain- ing: 5 10 15% (NH 4 ) 2 Fe 2 (S0 4 ) 4 +24H 2 0, 1.023 1.047 1.071 20 25 30% (NH 4 ) 2 Fe 2 (S0 4 ) 4 +24H 2 0, 1.096 1.122 1.148 35 40% (NH 4 ) 2 Fe 2 (S0 4 ) 4 +24H 2 0. 1.175 1.203 934 SULPHATE, AMMONIUM IRON 40% solution is sat. at 15. (Gerlach, Z. anal. 28. 496.) Melts in crystal H 2 O at 40. (Locke.) 3(NH 4 ) 2 SO 4 , Fe 2 (SO 4 ) ? . Insol. in cold H 2 O. (Lachaud and Lepierre.) Ammonium iron (ferroferric) sulphate, 4(NH 4 ) 2 SO 4 , FeSO 4 , Fe 2 (SO 4 ) 3 +3H 2 O. SI. sol. in .cold H 2 O; decomp. into basic salt by hot H 2 O; insol. in alcohol. (Lachaud and Lepierre, C. R. 114. 916.) Ammonium ferrous magnesium sulphate, 4(NH 4 ) 2 SO 4 , 3FeSO 4 , MgSO 4 +24H 2 O. Sol. in H 2 O. (Schiff, A. 107. 64.) 2(NH 4 ) 2 SO 4 , FeSO 4 , MgSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium ferrous manganous sulphate, 2(NH 4 ) 2 SO 4 , FeSO 4 , MnS0 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium ferrous nickel sulphate, 2(NH 4 ) 2 S0 4 , FeS0 4 , NiSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium ferrous zinc sulphate, 2(NH 4 ) 2 S0 4 , FeS0 4 , ZnSO 4 +12H 2 O. Sol. in H 2 O. (Bette, A. 14. 286.) Ammonium lanthanum sulphate, (NH 4 ) 2 SO 4 , La 2 (SO 4 ) 3 +8H 2 O. SI. sol. in H 2 O. (Marignac.) Quite sol. in H 2 O. (Cleve.) +2H 2 O. (Barre, C. R. 1910, 161. 872.) 5(NH 4 ) 2 SO 4 , 2La 2 (SO 4 ) 3 . SI. sol. in (NH 4 ) 2 SO 4 +Aq of concentrations above 60%. (Barre, A. ch. 1911, (8) 24. 246.) 5(NH 4 ) 2 SO 4 , La 2 (SO 4 ) 3 . (Barre.) Ammonium lead sulphate, (NH 4 ) 2 SO 4 , PbSO 4 . Decomp. by H 2 O into its constituents. (Wohler and Litton, A. 43. 126.) Decomp. by H 2 O. Only stable in contact with solutions containing: 13.86 pts. (NH 4 ) 2 SO 4 per 100 pts. H 2 O at 20. 19.25 pts. (NH 4 ) 2 SO 4 per 100 pts. H 2 O at 50. 24.31 pts. (NH 4 ) 2 SO 4 per 100 pts. H 2 O at 75. 29.42 pts. (NH 4 ) 2 SO 4 per 100 pts. H 2 O at 100. (Barre, C. R. 1909, 149. 294.) Ammonium lithium sulphate, NH 4 LiSO 4 . Solubility in H 2 O = 35.25% at 10, and 36.18% at 70. (Schreinemakers, C. C. 1906, I. 217.) This is the only double salt which (NH 4 ) 2 S0 4 forms with Li 2 SO 4 below 100. (Spielrein, C. R. 1913, 167. 48.) Ammonium magnesium sulphate, (NH 4 ) 2 Mg(SO 4 ) 2 +6H 2 O. 100 pts. H 2 O dissolve 15.9 pts. anhydrous double salt at 13. (Mulder.) 100 pts. H 2 O dissolve at: 10 15 20 30 9.0 14.2 15.7 17.9 19.1 pts. anhydrous salt, 45 50 55 60 75 25.6 30.0 31.9 36.1 45.3 pts. anhydrous salt. (Tobler, A. 96. 193.) More sol. in H 2 O than (NH 4 ) 2 SO 4 or MgSO 4 (Graham.) 1 1. H 2 O dissolves 199 pts. anhydrous salt at 25. Tobler's results are inaccurate. (Locke, Am. Ch. J. 1902, 27. 459.) 100 g. H 2 O dissolve at: 34 41 F. 18.22 20.72 g. (NH 4 ) 2 SO 4 , MgSO 4 , 6H 2 O. 50 59 F. 22.48 24.08 g. (NH 4 ) 2 SO 4 , MgSO 4 , 6H 2 O, 60 70 F. 24.81 28.26 g. (NH 4 ) 2 SO 4 , MgSO 4 , 6H 2 O, 81 F. 33.33 g. (NH 4 ) 2 S0 4 , MgSO 4 , 6H 2 O. (Lothian, Pharm. J. 1910, (4) 30. 546.) Lothian's results for solubility in H 2 O probably incorrect because of inaccuracy of experimental method. (Seidell, Pharm. J. 1911, (4) 33. 846.) Solubility of (NH 4 ) 2 Mg(SO 4 ) 2 in H 2 O at t. t g. anhydrous salt par 103 g. solution H 2 10.58 11.83 10 12.75 14.61 20 15.23 17.96 25 16.45 19.69 30 17.84 21.71 40 20.51 25.86 50 23.18 30.17 60 26.02 35.17 80 32.58 48.32 100 39.66 65.72 (Porlezza, Att. Ace. Line. 1914, (5) 23. II, 509.) Min. Cerbolite. Ammonium magnesium nickel sulphate, 2(NH 4 ) 2 S0 4 , MgS0 4 , NiS0 4 +12H 2 0. Sol. in H 2 0. (Vohl, A. 94. 57.) Ammonium magnesium potassium zinc sul- phate, 2(NH 4 ) 2 SO 4 , 3MgSO 4 , 3K 2 SO 4 , 2ZnSO 4 +30H 2 O. Sol. in H 2 O. (Schiff, A. 107. 64.) (NH 4 ) 2 S0 4 , 2MgS0 4 , 2K 2 S0 4 , ZnSO 4 + 18H 2 O. Sol. in H 2 O. (Schiff.) (NH 4 ) 2 S0 4 , MgS0 4 , K 2 S0 4 , ZnSO 4 +12H 2 O Sol. inH 2 O. (Schiff.) SULPHATE, AMMONIUM THALLIC 935 Ammonium magnesium zinc sulphate, 2(NH 4 ) 2 SO 4 , MgSO 4 , ZnSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium manganous sulphate, (NH 4 ) 2 SO 4 MnSO 4 +6H 2 O. Deliquescent. Easily sol. in H 2 O. (Jahn.' 1 1. H 2 O dissolves 372 g. anhydrous sal at 25. (Locke, Am. Ch. J. 1902, 27. 459.) (NH 4 ) 2 SO 4 , 2MnSO 4 . Readily decomp. ty H 2 O. (Lepierre, C. R. 1895, 120. 924.) Ammonium manganic sulphate, (NH 4 ) 2 SO 4 Mn 2 (S0 4 ) 3 . Decomp. by H 2 O. Insol. in ether, C 6 H 6 , and cone. H 2 SO 4 . Sol. in dil. H 2 SO 4 +Aq. (Le- pierre, Bull. Soc. 1895, (3) 13. 596.) +24H 2 O. Decomp. by H 2 O. (Mitscher- lich.) Ammonium manganous nickel sulphate, 2(NH 4 ) 2 S0 4 , MnS0 4 , NiSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium manganous zinc sulphate, 2(NH 4 ) 2 S0 4 , MnS0 4 , ZnSO 4 +12H 2 O. Sol. inH 2 O. (Vohl.) Ammonium mercuric sulphate, (NH 4 ) 2 SO 4 , 3HgS0 4 +2H 2 0. (Hirzel, J. B. 1860. 333.) (NH 4 ) 2 S0 4 , HgS0 4 . Difficultly sol. in H 2 O. Easily sol. in NH 4 OH+Aq. Ammonium mercurous sulphate ammonia, 3H g2 0, 2(NH 4 )HgS0 4 , 2NH 3 . Insol. in hot or cold, dil. or cone. H 2 S0 4 and HNO 3 . Sol. in HC1. (Tarugi, Gazz. ch. it. 1903, 33. (1) 131.) Ammonium nickel sulphate, (NH 4 ) 2 SO 4 , NiS0 4 +6H 2 0. Sol. in 4 pts. cold H 2 O. (Link, 1796.) 100 pts. H 2 O dissolve at: 3.5 10 16 20 30 1.8 3.2 5.8 5.9 8.3 pts. anhydrous salt, 40 50 59 68 85 11.5 14.4 16.7 18.8 28.6 pts. anhydrous salt. (Tobler, A. 95. 193.) 100 pts. sat. solution contain at 20, 9.4; at 40, 13.2; at 60, 18.6; at 80, 23.1 pts. anhydrous salt. (v. Hauer, J. pr. 74. 433.) 1 1. H 2 O dissolves 75.7 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Nearly insol. in a weak acid solution of (NH 4 ) 2 SO 4 . (Thompson, C. C. 1863. 957.) Ammonium nickel zinc sulphate, 2(NH 4 ) 2 SO 4 , NiS0 4 , ZnS0 4 +12H 2 0. Sol. in H 2 O. (Vohl, A. 94. 57.) Ammonium nickel sulphate ammonia, (NH 4 ) 2 SO 4 , NiS0 4 , 6NH 3 +3H 2 O. (Andre, C. R. 106. 936.) Ammonium platinic sulphate. 2(NH4) 2 SO4, Pt 3 (SO 4 ) 3 +25H 2 O. Sol. in H 2 O. (Prost, Bull. Soc. (2) 46. 156.) Ammonium potassium sulphate, (NH 4 ) 2 SO 4 , K 2 S0 4 +4H 2 0. Soluble in H 2 O. 100 pts. H 2 O at 16 dis- solve 13.68 pts. salt. (Thomson, 1831.) Min. Taylorite. Ammonium praseodymium sulphate, (NH 4 ) 2 S0 4 , Pr 2 (S0 4 ) 3 +8H 2 0. SI. sol. in H 2 O. (von Scheele, Z. anorg. 1898, 18. 359.) Ammonium rhodium sulphate, (NH 4 ) 2 S0 4 , Rh 2 (S0 4 ) 3 +24H 2 0. Very sol. H 2 O; melts in crystal H 2 O at 102-103. (Piccini, Z. anorg. 1901, 27. 67.) Ammonium samarium sulphate, (NH 4 ) 2 SO 4 , Sm 2 (S0 4 ) 3 +8H 2 0. SI. sol. in H 2 O. (Cleve, Bull. Soc. (2) 43. 166.) Ammonium scandium sulphate, (NH 4 ) 2 S0 4 . Sc 2 (S0 4 ) 3 . Sol. inH 2 O. (Cleve.) Sol. in H 2 O and in dil. (NH 4 ) 2 SO 4 +Aq. (R. J. Meyer, Z. anorg. 1914, 86. 279.) Ammonium sodium sulphate, NH 4 NaSO 4 -f 2H 2 Q. 100 pts. H 2 O dissolve 46.6 pts. of cryst. salt at 15, and the solution has a sp. gr. of 1.1749. Sp. gr. of aqueous solution containing: 31.8 24.44 15.9% NH 4 NaSO 4 +2H 2 O, 1.17491.1380 1.0849 12 . 72 6 . 36 % NH 4 NaSO 4 +2H 2 O. 1.0679 1.0337 (Schiff, A. 114. 68.) Ammonium strontium sulphate. Insol. in excess of (NH 4 ) 2 S0 4 +Aq. (Rose. Pogg. 110. 296.) (NH 4 ) 2 S0 4 , SrS0 4 . This double salt is only stable in contact with nearly sat. solu- tions of (NH 4 ) 2 SO 4 . (Barre, C. R. 1909, 149. 293.) Ammonium tellurium sulphate, (NH 4 )HS0 4 , 2Te0 2 , SO 3 +2H 2 O. As K salt. (Metzner, A. ch. 1898, (7) 16. 203.) Ammonium thallic sulphate, NH 4 T1(SO 4 ) 2 . (Marshall, C. C. 1902, II. 1089.) +4H 2 0. Decomp. by H 2 O. Easily sol. n dil. acids. (Fortini, Gazz. ch. it. 1905. 36. 2) 450.) SULPHATE, AMMONIUM THORIUM Ammonium thorium sulphate, 2(NH 4 ) 2 SO4, Th(S0 4 ) 2 . Easily sol. in H 2 O and sat. (NH 4 ) 2 SO 4 + Aq. (Cleve.) +2H 2 O. (Barre.) (NH 4 ) 2 SO 4 , Th(SO 4 ) 2 +4H 2 O. (Barre, A. ch. 1911, (8) 24. 240.) 3(NH 4 ) 2 SO 4 , Th(SO 4 ) 2 +3H 2 O. (B.) Ammonium titanium sulphate, (NH 4 ) 2 S0 4 , TiO, S0 4 +H 2 0. Very sol. in H 2 O with decomp. Insol. in cone. H 2 SO 4 . (Rosenheim, Z. anorg. 1901, 26. 252.) (NH 4 ) 2 O, 2TiO 2 , 2SO 3 +3H 2 O. Slowly decomp. by H 2 O. (Blondel, Bull. Soc. 1899, (3) 21. 262.) Ammonium titanium ses4, becomes turbii in y> hour. (Harting, J. pr. 22. 52.) BaCNOah+Aq containing 1 pt. BaO to 25,000 pts. H 2 O gives a distinct cloud with H 2 SO 4 or Na 2 SO4+Aq; with 50,000-100,000 pts. H 2 O a slight turbidity is produced; with 200,000-400,000 pts. H 2 O the mixture becomes turbid in a few minutes; while with 800,000 pts. H 2 O no action is visible. (Lassaigne, J Chim. Med. 8. 526.) Sol. in 800,000 pts. H 2 O (Calyert); in 400,000 pts. cold or hot H 2 O (Fresenius). Calculated from the electrical conductivity of the solution, BaS0 4 is sol. in 429,700 pts. H 2 O at 18.4, and 320,000 pts. at 37.7. (Holleman, Z. phys. Ch. 12. 131.) 1 1. H 2 O dissolves 1.72 mg. at 2; 1.97 mg. at 10; 2.29 mg. at 19.0; 2.60 mg. at 26; 2.91 mg. at 34. CKohlrausch and Rose, Z. phys. Ch. 12. 241.) Calculated from the electrical conductivity of the solution, BaSO 4 is sol. in 425,000 pts. H 2 O at 18.3. Results of Fresenius and Hintz (Z. anal. 1896, 35. 170) are incorrect. (Kiister, Z. anorg. 1896, 12. 267.) Sat. aq. solution contains 2.29 mg. BaSO 4 per liter at 25 when particles of salt are not less than 1.8/u in diameter. Sat. aq. solution contains 4.15 mg. BaSO 4 per liter at 25 when particles of salt are 0.1/i in diameter. OK = 0.0001 cm.) (Hulett, Z. phys. Ch. 1901, 37. 398-9.) In general the influence of the size of the grain on the solubility of the substance is negligible when the solubility exceeds 2%. The increase of normal solubility by using finely divided solids, amounts to 80% in the case of BaSO 4 . (Hulett, Z. phys. Ch. 1904, 47. 366.) 1 1. H 2 O dissolves 2.3 mg. BaSO 4 at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) Calculated from electrical conductivitv of BaSO 4 +Aq. 0.0190 milli-equivalents are sol. in 1 liter H 2 O at 18; 0.0212 at 25; 0.0288 at 50; 0.0334 at 100. (Melcher, J. Am. Chem. Soc. 1910, 32. 55.) Not attacked by cold HC1 or HNO 3 -f-Aq after several hours, and only in traces after several days. On boiling, traces of BaSO 4 dissolve, and the liquid after cooling can be precipitated by BaCl 2 or H 2 SO 4 +Aq, but not by H 2 O alone. (Rose, Pogg. 95. 108.) By washing BaSO 4 long enough with H 2 O containing HC1 or HNO 3 IHC 2 H 3 O 2 (Siegle)], the filtrate can be precipitated by H 2 SO 4 or BaCl 2 . (Piria, J. B. 1856. 334.) 1000 pts. 3% HCl+Aq dissolve 0.06 pt. BaSp 4 in the cold, and still more on boiling. 230 com. HCl+Aq of 1.02 sp. gr. dissolve 0.048 g. BaSO 4 from 0.679 g. BaS0 4 when boiled l / hour. 168 com. HCl-f-Aq of 1.03 sp. gr. dissolve 0.0075 g. BaSO 4 from 0.577 g. BaSO 4 when boiled 5 minutes. (Siegle, J. pr. 69. 142.) 938 SULPHATE, BARIUM Solubility of BaSO 4 in HCl+Aq. No. cc. HC1 +Aq containing equi 1 mg. liv. H Cl 2.0 1.0 0.5 0.2 Mg. BaSO4 per 1 mg. equiv. of HC1 0.133 0.089 0.056 0.017 g. per 100 cc. solution HC1 BaS0 4 0.0067 0.0089 0.0101 0.0086 (Banthisch, J. pr. 1884, 29. 54.) 100,000 pts. H 2 O dissolve 0.124 pt. BaSO 4 ; 1000 pts. HNOs+Aq of 1.167 sp. gr. dissolve 2 pts. BaSO 4 ; 1000 pts. HNO 3 +Aq of 1.032 sp. gr. dissolve 0.062 pt. BaSO 4 . (Calvert, Chem. Gaz. 1856. 55.) When 0.4 g. BaSO 4 is heated K hour with 150 ccm. HNO 3 +Aq of 1.02 sp. gr., 0.165 g. is dissolved. (Siegle, J. pr. 69. 142.) Solubility of BaSO 4 in HNO 3 +Aq. No. cc. HNOs+Aq containing 1 mg. equiv. HN0 3 2.0 1.0 0.5 0.2 Mg. BaSO 4 per 1 mg. equiv. of BaS0 4 0.140 0.107 0.085 0.048 G. per 100 cc. solution HN0 3 3.15 6.31 12.61 31.52 BaSO 4 0.0070 0.0107 0.0170 0.0241 (Banthisch, J. pr. 1884, 29. 54.) Acetic acid has less solvent power than other acids. 80 ccm. HC 2 H 3 O 2 +Aq of 1.02 sp. gr. boiled with 0.4 g. BaSO 4 K hour dis- solve 0.002 g. (Siegle, J. pr. 69. 142.) Sol. in boiling cone. H 2 SO 4 . (See BaH 2 (S0 4 ) 2 ). Sol. in fuming H 2 SO 4 . (See BaS 2 O 7 .) Sol. in 2500 pts. boiling 40% HBr+Aq; in 6000 pts. boiling 40% HI+Aq. (Haslam, C. N. 63. 87.) Sol. in considerable amount in metaphos- phoric acid+Aq. (Scheerer and Drechsel, J. pr. (2) 7. 68.) Not attacked by boiling cone. KOH+Aq if CO 2 is not present. (Rose, Pogg. 95. 104.) Very si. decomp. by standing a long time with cold cone, alkali carbonates +Aq. Decomp. by boiling Na 2 CO 3 or K 2 CO 3 + Aq, not by (NH 4 ) 2 CO 3 +Aq. (See Storer's Diet, for analytical data.) Very si. sol. in NH 4 Cl+Aq, 1 pt. dissolv- ing in 230,000 pts. sat. NH 4 Cl+Aq. 500 ccm. sat. NH 4 NO 3 +Aq with 50 ccm. sat. NH 4 Cl+Aq dissolve 2 g. BaSO 4 . 100 ccm. sat. NH 4 NO 3 +Aq with 100 ccm. sat. NH 4 Cl+Aq dissolve only 0.08 g. BaSO 4 , therefore above solubility is due to free chlorine. (Mittentzwey, J. pr. 75. 214.) BaS0 4 cannot be precipitated from solu- tions containing free C1 2 . (Erdmann, J. pr. 75. 215.) Pptn. is retarded si. by tartaric and racemic acids. (Spiller.) Na metaphosphate prevents pptn. of BaSO 4 but not ortho- or pyrophosphate. (Scheerer, J. pr. 75. 114.) Not precipitated in presence of alkali ci- trates. (Spiller.) Much less sol. in NH 4 Cl+Aq than in NH 4 NO 3 +Aq. Insol. in warm cone. Na 2 S 2 3 +Aq. (Diehl, J. pr. 79. 431.) Not appreciably sol. in H 2 O containing ammonium or sodium chloride. (Brett, Witt- stein, Wackenroder.) Not appreciably sol. in H 2 O at 250, or in H 2 O containing Na 2 S. (Senarmont.) Solubility is increased by alkali nitrates, but not appreciably by NaCl, KC10 3 , or Ba(NO 3 ) 2 . (Fresenius, Z. anal. 9. 52.) Scarcely sol. in boiling cone. (NH 4 ) 2 SO 4 +Aq. (Fresenius.) Solubility in H 2 O increased by presence of MgCl 2 (Fresenius); cerium salts (Marignac). Sol. in Fe 2 Cl 6 +Aq. (Lunge, Z. anal. 19. 141.) Solubility in various salts +Aq at 20-25. g. salt Mg. BaSO 4 dissolved per 1. in per 1. FeCh A1C1 3 MgCh' 1 58 33 30 2.5 72 43 30 5 115 60 33 10 123 9,4 33 25 150 116 50 50 160 170 50 100 170 175 50 (Fraps, Am. Ch. J. 1902, 27. 290.) Solubility in sat. solution of various salts+ Aq. Salt NaNO 3 NaCl NH 4 C1 G. BaSO 4 sol. in 1 1. of the solvent , 0.2940 0.00783 0.00827 (Ehlert, Z. Elektrochem, 1912, 18. 728.) Cone. CrCl 3 +Aq dissolves 40-120 times as much BaSO 4 as H 2 O, when boiled there- with for 5 days; cone. CrCl 3 +Aq acidified with HC1, 450 times as much in 10 days. (Kuster, Z. anorg. 1905, 43. 348.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Sol. in H 2 O 2 +Aq. (Gawalowski, C. C. 1906, II. 7.) 100 cc. 95% formic acid dissolve 0.01 g. BaSO 4 at 18.5. (Aschan, Ch. Ztg. 1913, 37. 1117.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790) ; in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Min. Barite. SULPHATE, BISMUTH POTASSIUM 939 Barium hydrogen sulphate, BaH 2 (SO 4 )2. 100 pts. H 2 SO 4 dissolve 2.22 pts. BaSO 4 (Lies-Bodart and Jacquemin, C. R. 46. 1206); 5.69 pts. BaSO 4 (Struve, Z. anal. 9. 34). Boiling H 2 SO 4 dissolves 10-12% freshly precipitated BaSO 4 without separating crys- tals on cooling. H 2 SO 4 at 100 dissolves more than boiling H 2 SO 4 , and becomes cloudy if heated to boiling. (Schultz, Pogg. 133. 146.) 1 g. BaSO 4 pptd. from BaCl 2 is sol. in 3153 g. 91% H 2 SO 4 ; from Ba(NO 3 ) 2 is sol. in 1519 g. 91% H 2 SO 4 . (Varenne and Pauleau, C. R. 93. 1016.) 100 pts. hot cone. H 2 SO 4 dissolve approx. 6 pts. BaSO 4 . (Rohland, Z. anorg. 1910, 66. 206.) 10 ccm. of sat. BaSCX-f- absolute H 2 SO 4 contain approx. 2.851 g. BaSO 4 . (Bergius, Z. phys. Ch. 1910, 72. 355.) Equilibrium in the system BaSO 4 +H 2 SO 4 + H 2 O at 25. Composition of the solution % H 2 SC)4 g. BaS0 4 per 1. Solid phase 73.83 78.04 80.54 83.10 85.78 88.08 93.17 0.030 0.135 0.285 0.800 3.215 12.200 49.665 BaSO 4 ii u it BaS0 4 , 2H 2 S0 4 .H a BaSO 4 , H 2 SO 4 2 (Volkhonski, C. C. 1910, I. 1954; C. A. 1911. 617.) Decomp. by H 2 O, alcohol, or ether. +2H 2 O. (Schultz.) BaSO 4 , 2H 2 SO 4 +H 2 O. (Volkhonski.) Barium pyrosulphate, BaS 2 O 7 . 100 pts. fuming H 2 SO 4 dissolve 15.89 pts. BaSO 4 . (Struve, Z. anal. 9. 34.) Very deliquescent. Decomp. with H 2 O with hissing. (Schultz- Sellack, B. 4. 111.) Barium calcium sulphate, 3BaSO 4 , CaSO 4 . Min. Dreelite. Barium platinic sulphate (?). Insol. in H2O or boiling HC1 or HNO 3 +Aq. Sol. in hot cone. H2SO4 or aqua regia. (E. Davy.) Barium tin (stannic) sulphate, BaSO 4 , Sn(SO 4 ) 2 +3H 2 O. Decomp. by H 2 O. Insol. in HC1. (Wein- land and Kiihl, Z. anorg. 1907, 64. 249.) Barium titanium sulphate, 2BaSO 4 , 3Ti(SO 4 ) 2 . Ppt. Decomp. byH 2 O, giving titanic acid. (Weinland, Z. anorg. 1907, 64. 255.) Barium sulphate potassium chloride, 3BaSO 4 , KC1. Ppt. (Silberberger, M. 1904, 25. 233.) Bismuth sulphate, basic, (BiO) 2 SO 4 . Insol. in H 2 O. Sol. in HNO 3 or H 2 SO 4 + Aq. +2H 2 O. (Heintz, Pogg. 63. 55.) 4Bi 2 O 3 , 3SO 3 + 15H 2 O. Insol. in H 2 O. (Leist.) (BiO)HSO 4 +H 2 O. Insol. in H 2 O. Sol. in dil. H 2 SO 4 +Aq. +2H 2 O. Decomp. by H 2 O with separation of (BiO) 2 SO 4 +2H 2 O. (Heintz.) 3Bi 2 O 3 , 2SO 3 +2H 2 O. Insol. in H 2 O. (Athanasesco, C. R. 103. 271.) 5Bi 2 Q 3 , 11SO 3 +17H 2 O. This sulphate crystallizes out from sulphuric acid of any strength between H 2 SO 4 , 6H 2 O and H 2 SO 4 , 12H 2 O. (Adie, Proc. Chem. Soc. 1899, 15. 226.) Bi 2 O 3 , 2SO 3 , 2^H 2 O is in equilibrium at 50 with 5.4-51.4% H 2 SO 4 -hAq. Bi 2 O 3 , SO 3 is in equilibrium at 50 with acid solutions weaker than 5.4% H 2 SO 4 . (Allan, Am. Ch. J. 1902, 27. 287.) Bismuth sulphate, Bi 2 (SO 4 ) 3 . Very hygroscopic. Takes up H 2 O with strong evolution of heat to form 2Bi 2 (SO 4 ) 3 + 7H 2 O, which becomes Bi 2 (SO 4 ) 3 +3H 2 O at 100. Decomp. by boiling H 2 O into Bi 2 O 3 , SO 3 +H 2 O. (Hensgen, J. B. 1886. 552.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Bismuth sulphate, acid, Bi 2 O 3 , 4SO 3 . Bi 2 O 3 , 4SO 3 is in equilibrium at 50 with 51.4-90% H 2 SO 4 +Aq. (Allan, Am. Ch. J. 1902, 27. 287.) +H 2 O. Crystallizes out from sulphuric acid at temp, above 170. (Adie, Proc. Chem. Soc. 1899, 16. 226.) +3H 2 O. Crystallizes from sulphuric acid of any strength between H 2 SO 4 , H 2 O and H 2 SO 4 , 2H 2 O. (Adie.) +7, or 9H 2 O = BiH(SO 4 ) 2 +3H 2 9. Insol. in H 2 O. Easily sol. in acids, especially HC1, and HNO 3 +Aq. (Leist, A. 160. 29.) +7H 2 O. Crystallizes out from sulphuric acid of any strength between H 2 SO 4 , 3H 2 O and H 2 SO 4 , 5H 2 O. +10H2O. Crystallizes out from sulphuric acid at temp, below 170. (Adie.) Bismuth potassium sulphate, Bi 2 (SO 4 ) 3 , 3K 2 SO 4 (?). Decomp. by H 2 O; insol. in sat. K 2 SO 4 +Aq. (Heintz.) Bi 2 (SO 4 ) 3 , 2K 2 SO 4 . BiK(SO 4 ) 2 = Bi 2 (SO 4 ) 3 , K 2 SO 4 . Insol. in cold H 2 O; decomp. by boiling. (Brigham, Am. Ch. J. 14. 170.) 940 SULPHATE, BISMUTH SODIUM Bismuth sodium sulphate, Bi 4 Na6(SO 4 )9. Sp.gr. of CdSO 4 +Aq at 18. (Ludecke, A. 140. 277.) % CdSO 4 1 5 10 15 Boron sulphate. Sp.gr. 1.0084 1.0486 1 .1026 1.1607 See Boro sulphuric acid. %CdSO 4 . 20 25 30 35 Sp.gr. 1.2245 1.295 1 .3725 1.4575 Bromomolybdenum sulphate. See under Bromomolybdenum compounds. % CdSO 4 36 Sp. gr. 1.4743 Cadmium sulphate, basic, 2CdO, SO 3 , and +H 2 0. Difficultly sol. in H 2 0. (Stromeyer.) SI. sol. in hot H 2 O. (Habermann, M. 5. 432.) 4CdO, SO 3 . (Pickering, Chem. Soc. 1907, 91. 1987.) Cadmium sulphate, CdSO 4 . Sat. CdSO 4 +Aq contains at: 10 24 30 65 35.9 37.5 41.5 42.0 49.7% CdSO 4 , 86 94 130 165 188 200 43.5 91.6 27.7 14.7 7.1 2.3% CdSO 4 . CdSO 4 easily forms supersat. solutions, (fitard, A. ch. 1894, (7) 2. 552.) Solubility in H 2 O. t Per cent CdSO 4 in sat. solution Solid phase -18 43.35 Ice -10 43.27 u 43.01 CdS0 4 , 8 /sH 2 +10 43.18 15 43.20 20 43.37 30 43.75 40 43.99 60 44.99 62 45.06 72 46.2 73.5 46.6 74.5 46.7 75 46.5 CdSO ,H 2 77 42.2 78.5 41.5 85 39.6 90 38.7 95 38.1 100 37.8 H (Mylius and Funk, B. 1897, 30. 825.) See also under CdSO 4 +2 2 / 3 H 2 O, and 7H 2 O. Sp. gr. at 0/4 of CdSO 4 -f Aq containing 14.0 g. CdS0 4 in 1000 g. H 2 O = 1.0122. Sp. gr. at 12/4 of CdSO 4 +Aq containing 14.0 g. CdSO 4 in 100 g. H 2 O = 1.0121. Sp. gr. at 1274 of CdSO 4 +Aq containing 57.2 g. CdSO 4 in 1000 g. H 2 = 1.0514. Sp. gr. at 074 of CdSO 4 +Aq containing 183.1 g. CdSO 4 in 1000 g. H 2 O = 1.1552. Sp. gr. at 1374 of CdSO 4 +Aq containing 183.1 g. CdSO 4 in 1000 g. H 2 O = 1.1529. (Fouque", Ann. Observ. 1868, 9. 172.) (Grotrian, W. Ann. 1883, 18. 193.) Sp. gr. of CdSO 4 +Aq at room temp, con- taining: 7.14 14.66 22.011% CdSO 4 . 1.0681 1.1591 1.2681 (Wagner, W. Ann. 1883, 18. 268.) Sp. gr. of CdSO 4 +Aq at 25. Concentration of CdSCh +Aq Sp. gr. 1-normal Vr- " V<~ " Vr- " 1.0973 1.0487 1.0244 1.0120 (Wagner, Z. phys. Ch. 1890, 5. 36.) Sp. gr. of CdSO 4 +Aq. % CdS0 4 t Sp. gr. at t Sp. gr. at 18 0.0289 0^0498 0.0999 0.495 0.981 17.29 23.65 18.00 18.00 18.00 18.00 0.99908 0.99776 0.99893 0.99915 0.99961 1.0034 1.0084 (Wershofen, Z. phys. Ch. 1890, 5. 494.) Sp. gr. at 16/4 of CdSO 4 +Aq containing 29.4654% CdSO 4 = 1.36289; containing 21.3671% CdSO 4 = 1.24211. (Schonrock, Z. phys. Ch. 1893, 11. 781.) Sp. gr. of CdSO 4 +Aq at 18/4. % CdSO 4 25.121 18.172 Sp. gr. 1.297 1.200 % CdS0 4 Sp. gr. (de Muynck, W. Ann. 1894, 53. 561.) 9.952 1.101 5.639 1.055 CdSO 4 +Aq containing 13.40% CdSO 4 has sp. gr. 20/20 = 1.1429. CdSO 4 +Aq contaiing 16.79% CdSO 4 has sp. gr. 20720 = 1.1847. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 282.) SULPHATE, CADMIUM OESIUM 941 Sp. gr. of CdS0 4 at 18. 2, when p'=per cent strength of solution; d = observed den- sity; w = volume cone, in grams per ioo p d w 39.86 1.5639 0.6231 31.53 1.4080 0.4439 26.85 1.3310 0.3574 24.17 1.2901 0.3118 18.35 1.2084 0.2217 13.27 1 . 1437 0.1518 9.97 1 . 1045 0.1102 7.46 1.0764 0.0803 6.12 0.0619 0.0650 2.52 0.0242 0.0259 1.45 0.0132 0.0147 0.464 0.0033 0.0046 (Barnes, J. phys. Ch. 1898, 2. 543.) Sp. gr. of CdSO 4 +Aq sat. at 25 and 1 atm. = 1.617. (Sinnige, Z. phys. Ch. 1909, 67. 518.) See also under CdSO 4 +2 2 / 3 H 2 O, and +4H 2 0. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in acetone. (Naumann, B. 1904, 37. 4329); methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate: (Naumann, B. 1910, 43. 314.) +H 2 O. See Mylius and Funk, under CdSO 4 . flVi H 2 O. (Worobieff, Bull. Soc. 1896, (3) 16. 1754.) +2 2 / 3 H 2 O. 1 pt. H 2 O dissolves 0.59 pt. anhydrous salt at 23, and not much more on heating. Sat. solution boils at 102. Pre- cipitated by alcohol, (v. Hauer.) 100 g. H 2 O dissolve g. CdSO 4 at t c 100 pts. H 2 O dissolves at: 13.7 14.98 15.0 16.0 76.06 76.09 76.14 76.18 pts. anhydrous salt, 16.96 18.0 19.0 25.0 76.26 76.32 76.39 76.81 pts. anhydrous salt. (Steinwehr, W. Ann. 1902, (4) 9. 1050.) 100 g. H 2 O dissolve 76.02 g. CdSO 4 at 25. (Stortenbecker, Z. phys. Ch. 1900, 34. 109.) Solubility of CdSO 4 +2 2 / 3 H 2 O at 25 and varying pressures. Pressure in atmospheres G. CdSO 4 in 100 g. H 2 O 1 500 . ., 500 1000 1000 76.80 77.85 78.08 78.77 78.68 Det. by another method Pressure in atmospheres G. CdS0 4 inlOO g. H 2 O 250 500 750 1000 77.53 78.02 78.60 78.96 (Cohen and Sinnige, Trans. Farad. Soc. 1910, 6. 269.) Sp. gr. at 21.6/0 of CdSO 4 +Aq contain- ing 11.47% CdSO 4 + 8 / 3 H 2 O = 1.0944. (Ka- nonnikoff, J. pr. 1885, (2) 31. 346.) 100 g. H 2 O dissolve 57.61 g. CdSO 4 + 10.63 g. FeSO 4 at 25. (Stortenbecker, Z. phys. Ch. 1900, 34. 109.) +4H 2 O. (Lescoeur, A. ch. 1895, (7) 4. 222.)' Sp. gr. at 15 of CdSO 4 +Aq containing 10 g. CdSO 4 +4H 2 O in 100 c.c of solution = 1.0790; containing 20 g. CdSO 4 +4H 2 O in 100 cc. of solution = 1.1 522. (Traube, J. pr. 1885, (2) 31. 207.) Could not be obtained. (Mvlius and Funk.) +7H 2 0. Solubility in H 2 O. t G. CdS04 t % CdS0 4 5 7 9 11.5 13 15 16 17 18 19 25 75.52 75.65 65.73 75.85 75.94 76.04 76.11 76.16 76.13 76.14 76.18 76.79 -17 -16 -12 -10 - 7 - 5 - 4.5 44.45 44.5 45.3 46.1 47.5 48.5 48.7 (Mylius and Funk, B. 1897, 30. 828.) Cadmium caesium sulphate, CdSO 4 , Cs 2 SO 4 -f 6H 2 0. Sol. in H 2 O. (Tutton, Chem. Soc. 63. 337.) 1 1. H 2 O dissolves 1399 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) (Kohnstamm and Cohen, W. Ann. 1898, 65. 352.) 942 SULPHATE, CADMIUM CALCIUM POTASSIUM Cadmium calcium potassium sulphate, Ca 2 CdK 2 (SO 4 ) 4 +2H 2 O. (D'Ans, B. 1908, 41. 1778.) Cadmium cerium sulphate, CdSO 4 , Ce 2 (SO 4 ) 3 +6H 2 O. Sol.inH 2 O. (Wyrouboff.) Cadmium hydrazine sulphate, Solubility of CdNa 2 (SO 4 ) 2 , 2H 2 O+CdSO 4 , 8 / 3 H 2 O in 100 g. H 2 O at t. t 5 10 V, go Sco 2-T3 00 73.54 73.38 72.765 See c 8.85 8 . 67. r : 9.55 t 15 20 25 |o 00 73 . 76" 73 . 81 73.71 II t SO 00 Ji- 9.. 435 9.455 10.48 30 35 40 73.915 75.01 75 . 385 ll. 10 12 32 13'75 CdH 2 (SO 4 ) 2 , 2N 2 H 4 . 1 pt. is sol. in 202.5 pts. H 2 O at 12. Not attacked by dil. acids. Easily sol. in NH 4 OH+Aq. (Curtius, J. pr. 1894, (2) 50. 331.) Cadmium magnesium sulphate, CdSO 4 , MgSO 4 +14H 2 O. Very efflorescent. Sol. in H 2 O. (Schiff, A. 104. 325.) Cadmium potassium sulphate, K 2 SO 4 , CdSO 4 Sol. in H 2 O. (v. Hauer, Pogg. 133. 176.) 100 pts. H 2 O dissolve 42.50 pts. anhydrous salt at 26; 100 pts. H 2 O dissolves 42.80 pts. anhydrous salt at 31; 100 pts. H 2 O dissolve 43.45 pts. any hydrous salt at 40; 100 pts. H 2 O dissolve 44.90 pts. anyhydrous salt at 64. (Wyrouboff, Bull. Soc. Min. 1901, 24. 68.) +2H 2 O. 100 pts. H 2 O dissolve 42.89 pts. anhydrous salt at 16; 46.82 pts. at 31; 47.40 pts. at 40. (Wyrouboff.) +4H 2 O. Efflorescent. (Wyrouboff, Bull. Soc. Min. 1891, 14. 235.) .A +6H 2 O. Very efflorescent, and easily decomp. (Schiff.) Does not exist. (Wyrouboff.) Cadmium rubidium sulphate, CdSO 4 , Rb 2 S0 4 +6H 2 O. Efflorescent. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 767 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Cadmium sodium sulphate, CdSO 4 , Na 2 SO 4 + 2H 2 O. Sol. in H 2 O. (v. Hauer.) Solubility of CdNa 2 (SO 4 ) 2 +2H 2 O in 100 g. H 2 O at t. t Grams CdSO 4 Grams Na2SO4 24 35.49 24.04 25 35.88 24.46 30 36.28 24.605 35 36.69 24.99 40 37.24 25.455 (Koppel, Z. phys. Ch. 1905, 52. 413.) Decomp. by H 2 O below 20.5. (Koppel.) Solubility of CdNa 2 (SO 4 ) 2 , 2H 2 O+Na 2 SO 4 , 10H 2 O in 100 g. H 2 O at t. t Grams CdSO 4 Grams NazSCU -14.8 72.68 8.32 66.325 11.625 5 61.78 12.97 10 55.34 14.785 12 51.615 15.95 15 46.60 17.99 19.8 36.13 22.16 20 36.25 23.52 24 27.82 29.17 25 25.59 31.08 30 14.62 44.145 (Koppel.) Solubility of CdNa 2 (SO 4 ) 2 , 2H 2 O+Na 2 SO 4 (anhydrous) in 100 g. H 2 O at t. t Grams CdSCh Grams Na 2 SC>4 35 40 13.26 16.25 47.06 46.27 (Koppel.) Cadmium sulphate ammonia, CdSO 4 , 6NH 3 . Sol. in H 2 O with separation of CdO. (Rose, Pogg. 20. 152.) CdSO 4 , 4NH 3 +4H 2 O. Decomp. by H 2 O. (Malaguti and Sarzeau, A. ch. (3) 9. 431.) +2H 2 O. Ppt. (Andre, C. R. 104. 987.) +2^H 2 O. Sol. in H 2 O with separation of basic sulphate. (Mttller, A. 149. 70.) CdSO 4 , 3NH 3 . (Isambert, C. R. 1870, 70. 457.) Cadmium sulphate cupric oxide, CdSO 4 , 3CuO+zH 2 O. (Recoura, C. R. 1901, 132.1415.) 2CdSO 4 , 3CuO+8H 2 O. (Mailhe, A. ch. 1902, (7) 27. 383.) + 12H 2 O. (Mailhe.) 6CdSO 4 , 20CuO+rcH 2 O. fRecoura, C. R. 1901, 132. 1415.) Cadmium sulphate hydrazine, CdSO 4 , 2N 2 H 4 . Easily sol. in NH 4 OH+Aq but cannot be cryst. therefrom. (Franzen, Z. anorg. 1908, 60. 282.) SULPHATE, CAESIUM IRON 943 Cadmium sulphate hydrogen chloride, 3CdSO 4 , 4HC1+4H 2 O. Very deliquescent. (Baskerville and Harris, J. Am. Chem. Soc. 1901, 23. 896.) 3CdS0 4 , 8HC1. Very deliquescent. (Bas- kerville and Harris.) Caesium sulphate, Cs 2 SO 4 . Solubility in H 2 O. Temp. G. per litre G. mols. anhydrous salt per 1. 25 30 35 40 5.7 9.6 12.06 15.3 0.015 0.025 0.032 0.0405 100 pts. H 2 O dissolve 158.7 pts. Cs 2 SO 4 at 2. 100 cc. H 2 O at 17-18 dissolve 163.5 g. Cs 2 SO 4 . (Tutton, Chem. Soc. 1894, 65. 632.) Solubility in H 2 O. G. Cs 2 S0 4 G. Cs 2 SO4 * per 100 g. io- t per 100 g. 150- Solu- tion H 2 O 3$ Solu- tion H 2 O d^ 62.6 167.1 3.42 60 66.7 199.9 3.78 10 63.4 173.1 3.49 70 67.2 205.0 3.83 20 64.1 178.7 3.56 80 67.8 210.3 3.88 30 64.8 184.1 3.62 90 68.3 214.9 3.92 40 65.5 189.9 3.68 100 68.8 220.3 3.97 5,0 66.1 194.9 3.73 108.6 69.2 224.5 4.00 (Berkeley, Trans. Roy. Soc. 1904, 203. A. 210.) Solubility in Na 2 SO 4 +Aq. Sat. solution contains 54.7% Cs 2 SO 4 + 11.45% Na 2 SO 4 at 25. (Foote, J. Am. Chem. Soc. 1911, 33. 467.) Insol. in alcohol. (Bunsen.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in acetone. (Naumann, B. 1904, 37. 4329); (Eidmann, C. C. 1899, II. 1014.) Solubility in glycol at ord. temp. = 3.0- 3.2%. (de Coninck, Belg. Acad. Bull. 1905. 359.) Caesium hydrogen sulphate, CsHSO 4 . Sol. in H 2 O. Caesium pyrosulpha.te, Cs 2 S 2 O 7 . Decomp. by H 2 O. Caesium ocfosulphate, Cs 2 S 8 O 25 . Decomp. by H 2 O. (Weber, B. 17. 2497.) Caesium calcium sulphate, Ca 2 Cs 2 (S0 4 ) 3 . Very stable, (D-'Ans, B. 1908, 41. 1776.) Caesium chromium sulphate, Cs 2 Cr 2 (SO 4 ) 4 +24H 2 0. Melts in crystal H 2 O at 116. (Locke.) (Locke, Am. Ch. J. 1901, 26. 180.) Caesium cobaltous sulphate, Cs 2 S0 4 , CoSO 4 -j- 6H 2 0. Sol. in H 2 O. (Tutton, Chem. Soc. 63. 337.) 1 1. H 2 O dissolves 418.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Caesium cobaltic sulphate, Cs 2 Co 2 (SO 4 ) 4 + 24H 2 0. Melts in crystal H 2 O at 116. (Locke, Am. Ch. J. 1901, 26. 183.) Caesium copper sulphate, Cs 2 SO 4 , CuSO 4 + 6H 2 O. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 460 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Caesium gallium sulphate, Cs 2 Ga 2 (SO 4 ) 4 + 24H 2 O. (Soret, Arch. sc. phys. nat. 1888, (3) 20. 531.) Caesium indium sulphate, Cs 2 In 2 (SO 4 ) 4 + 24H 2 O. 75.7 g. anhydrous (117.39 hydrated) salt or 0.172 g. mols of anhydrous salt are sol. in 1 1. H 2 O at 25. (Locke, Am. Ch. J. 1901, 26. 175.) 100 pts. H 2 O dissolve 3.04 pts. at 16.5. (Chabrie and Rengade, C. R. 1900, 131. 1301.) Caesium indium sulphate, Cs 2 SO 4 , Ir 2 (S0 4 ) 3 +24H 2 0. Mpt. 109-110. Very si. sol. in cold. More easily sol. in hot H 2 O. (Marino, Z. anorg. 1904, 42. 218.) Caesium iron (ferrous) sulphate. Cs 2 SO 4 . FeSO 4 +6H 2 O. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 1011 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Caesium iron (ferric) sulphate, Cs 2 Fe 2 (SO 4 ) 4 +24H 2 O. Melts in crystal H 2 O at 71. (Locke.) 944 SULPHATE, CESIUM LANTHANUM Solubility in H 2 O. Caesium thallic sulphate, CsTl(SO 4 ) 4 -f 13^H 2 O. Hygroscopic. (Locke, Am. Ch. J. 1902, 27. 283.) +3H 2 O. Very si. sol. in cold; easily sol. in hot H 2 O. Can be recryst. from H 2 SO 4 -j- Aq. The recryst. salt is at once decomp. by H 2 O or 95% alcohol. (Locke.) t G. per litre G. mols. anhydrous salt per litre 25 30 35 40 17.1 25.2 37.5 60.4 0.045 0.066 0.099 0.156 (Locke, Am. Ch. J. 1901, 26. 180.) Caesium lanthanum sulphate, Cs 2 SO 4 , La 2 (SO 4 ) 3 +2H 2 O. (Baskerville, J. Am. Chem. Soc. 1904, 26.^67.) 2Cs 2 SO 4 , 3La 2 (SO 4 ) 3 . (Baskerville.) Caesium magnesium sulphate, Cs 2 SO 4 , MgSO 4 +6H 2 O. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 533 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Caesium manganous sulphate, Cs 2 S0 4 , MnSO 4 +8H 2 O. Sol. in H 2 O. (Tutton.) Sol. in H 2 O and acids with decomp. (Pic- cini, Z. anorg. 1899, 20. 14.) 1 1. H 2 O dissolves 804 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 45. Caesium manganic sulphate, Cs 2 SO 4 , Mn 2 (SO 4 ) 3 +24H 2 O. Decomp. by H 2 O and dil. acids with sep- aration of MnO 2 . Sol. in 1 :3 H 2 SO 4 +Aq and in cone. HNO 3 . Insol. in acetic acid. Sol. in oxalic acid+Aq. (Christensen, Z. anorg. 1901, 27. 332.) Caesium neodymium sulphate, Cs 2 SO 4 , Nd 2 (SO 4 ) 3 +3H 2 O. (BaskervUle, J. Am. Chem. Soc. 1904, 26. 74.) Caesium nickel sulphate, Cs 2 SO 4 , NiSO 4 + 6H 2 0. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 255.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Caesium praseodymium sulphate, Cs 2 SO 4 , Pr 2 (S0 4 ) 3 +2H 2 0. (Baskerville, J. Am. Chem. Soc. 1904, 26. 73.) +4H 2 O. (Baskerville.) Caesium rhodium sulphate, Cs 2 SO 4 ,Rh 2 (SO 4 ) 3 +24H 2 O. SI. sol. in cold, sol. in warm H 2 O; mpt. 110-111. (Piccini, Z. anorg. 1901, 27. 64.) Caesium thorium sulphate, Cs 2 SO 4 ,Th(SO 4 ) 2 -f- 2H 2 O. SI. sol. in H 2 O. (Manuelli, Gazz. ch. it. 1903, 32. (2) 523.) Caesium titanium sulphate, Cs 2 SO 4 ,Ti 2 (SO 4 ) 3 +24H 2 O. Deliquesces in the air and is decomp. SI. sol. in cold H 2 O; decomp. by hot H 2 O. (Piccini Gazz. ch. it. 1895, 25. 542.) SI. sol. in cold H 2 O, more sol. in hot H 2 O acidified with H 2 SO 4 . Decomp. in neutral aq. solution. (Piccini, Z. anorg. 1898, 17. 356.) Caesium uranyl sulphate, Cs 2 (UO 2 )(S0 4 ) 2 + 2H 2 O. As Na salt, (de Coninck, C. C. 1905, 1. 1306.) Caesium vanadium sulphate, Cs 2 V 2 (SO 4 ) 4 + 24H 2 O. 7.71 g. anhydrous (13.1 g. hydrated) salt, or 0.0204 gr. mols. of the anhydrous salt are sol. in 1 1. H 2 O at 25. (Locke, Am. Ch. J. 1901, 26. 175.) SI. sol. in cold, easily sol. in hot H 2 O. (Pic- cini, Z. anorg. 1896, 11. 114.) 100 pts. H 2 O dissolve 0.464 pts. of the salt at 10 and sp. gr. of the solution at 4/20 = 2.033. More sol. in hot H 2 O than in cold. [Piccini, Z. anorg. 1897, 13. 446.) Caesium zinc sulphate, Cs 2 S0 4 , ZnS0 4 -f- 6H 2 O. Sol. in H 2 O. (Bunsen and Kopp, Pogg. 113. 337.) 1 1. H 2 O dissolves 386.3 g. anhydrous salt at 25. (Locke. Am. Ch. J. 1902, 27. 459.) Caesium zirconium sulphate, Zr 2 O 3 ,(CsSO 4 ) 2 +HH 2 O. Ppt. (Rosenheim, B. 1905, 38. 815.) alcium sulphate, CaSO 4 , and +2H 2 O. The older determinations of the solubility of CaSO 4 in H 2 O have little, but historical, alue, as the solutions were usually either non-saturated or supersaturated. They may )e tabulated as follows. SULPHATE, CALCIUM 945 A=pts. H2O required for dissolving 1 pt. CaSO 4 , and B for 1 pt. CaSO 4 +2H 2 O at t. t A B Authority Hot or cold 500 Fourcroy Cold 500 Bergmann Boiling 450 " All temp. 322 Lassaigne (?) 438 Anthon (?) 250-300 Dumas Hot or cold 578.5 461^5 Bucholz Cold 480 380 Giese Hot 491 388 it 15-20 492 388 Tipp 12.5 503 397 Lecoq 100 pts. H 2 O at t dissolve pts. CaSO 4 t Pts. CaS0 4 t Pts. CaSCU t Pts. CaSCU 0.205 35 0.254 70 0.244 5 0.219 40 0.252 80 0.239 12 0.233 50 0.251 90 0.231 20 0.241 60 0.248 100 0.217 30 0.249 (Poggiale, A. ch. (3) 8. 469.) Poggiale worked with supersat. solutions. (Droeze, B. 10. 330.) H 2 O dissolves CaSO 4 most abundantly at 35 (Poggiale); at 32-41 (Marignac). 1 pt. CaSO 4 +2H 2 O dissolves at: 18 24 32 38 in 415 386 378 371 368 pts. H 2 O, 53 72 375 391 or (by calculation) dissolves at: 18 24 in 525 488 479 53 72 41 in 370 99 451 pts. H 2 O, pt. anhydrous CaSO 4 86 417 41 in 468 474 495 32 470 86 528 38 466 pts. H 2 O, 99 571pts.H 2 O. The above nonsat. solutions are obtained by using a large excess of CaSO 4 +2H 2 O. The undissolved part retains its water of crystal- lisation. CaSO 4 , dehydrated at 130-140, forms a supersaturated solution with H 2 O in 10 minutes, containing 1 pt. CaSO 4 to 110 pts. H 2 O, whicn soon deposits crystals. The un- dissolved part takes up its water of crystal- lisation. Ignited CaSO 4 dissolves very slowly in H 2 O, so that in 24 hours the solution con- tains Vf 33 to Vsgs anhydrous CaSO 4 . By longer contact solution continues with formation of supersaturated solutions, which contain after 10-30 days Vs7 2 to Y2s CaSO 4 , but these be- come normal as the anhydrous CaSO 4 gradually takes up its water of crystallisation. The mineral anhydrite behaves similarly, water taking up Yes* CaSO 4 in 1 day, Vasi in 40 days, and V 45 7 in 8 months. Supersaturated solutions are also obtained by evaporation of a saturated solution. By evaporation with heat, solutions are obtained containing Ysoe CaSO 4 , and in the cold with Yif2 CaSO 4j in the solution over the separated CaSO 4 +2H 2 O. Neutralising dil. H 2 SO 4 +Aq with CaCOa gives a solution containing Yin CaSO 4 , which crystallises out partly in 24 hours, leaving Y3isCaSp 4 dissolved. Supersaturated solutions containing Yno to Yiso CaSO 4 deposit crystals rapidly; those under Ysso do not crystallise spontaneously. A solution containing l /zss shows crystals in 14 days, and contains Ysia in 1 month, Y4 in 2 months, Y446 in 3 months, in spite of repeated shaking- Boiling diminishes the supersaturation without however removing it entirely. (Mar- ignac, A. ch. (5) 1. 274.) 1- pt. CaSO 4 +2H 2 O is sol. in 443 pts. H 2 O at 13.7; in 447 pts. H 2 O at 14.2; in 421 pts. H 2 O at 20.2; in 419 pts. H 2 O at 21.2; ind in 445 pts. H 2 CO 3 +Aq sat. at 18.7. (Church, J. B. 1867. 192.) Church's solutions were not sat. (Droeze, B. 10. 330.) 1000 pts. H 2 O dissolve 2.19 pts. CaSO 4 + 2H 2 O at 16.5; 2.352 pts. CaSO 4 +2H 2 O at 22. (Cossa, Gazz. ch. it. 1873. 135.) Cossa's solutions were not saturated. (Droeze.) CaSO 4 +2 H 2 O is sol. in 415 pts. H 2 O at 0; in 412 pts. H 2 O at 5; in 407 pts. H 2 O at 10; in 398 pts. H 2 O at 15; in 371 pts. H 2 O at 20; in 365 pts. H 2 O at 25; in 361 pts. H 2 O at 30; in 359 pts. H 2 O at 35. (Droeze, B. 10. 330.) Sol. in 500 pts. H 2 at 12.5. (From Marig- nac's and his own results, de Boisbaudran, A. ch. (5) 3. 477.) CaSO 4 is sol. in 564.5 pts. H 2 O at 0.8; 506.27 pts. at 14; 472-3 pts. at 32.5-38.8; 498.73 pts. at 64; 533.92 pts. at 79.6. (Raupenstrauch, M. 6. 563.) According to Goldammer (C. C. 1888. 708) H 2 O is fully saturated with CaSO 4 by shaking the finely-powdered substance 5 minutes therewith. The following results were obtained. Fig- ures denote pts. H 2 O in which 1 pt. CaSO 4 was dissolved at t (a) from pptd. CaSO 4 "ipse fact.," (b) from pptd. CaSO 4 "gehe," (c) from "glacies mariae puly.," (d) from "glacies Mariae pulv./' containing less than 2H 2 O. t a b c t d 7.5 15 22 5 561.5 526 497.5 481 558 526 497.5 481.5 557.5 520 493 479 '20 476.5 436' 30 37.5 45 60 75 90 100 475 463 473.5 484 507.5 533.5 556 475 469 474.5 486.5 508 530 557 470 465.5 470.5 482 503 534 534.5 '40 '60 80 100 450 ' 476* 502.5 547* 946 SULPHATE, CALCIUM Burnt gypsum easily forms supersat. solu- tions containing nearly 1% CaSO." It forms supersat. solutions more readily at 0, and that tendency decreases with increase of temp., hence figures in (d) which contained burnt gypsum. (Goldammer. C. C. 1888. 708.) Calculated from electrical conductivity of CaSO 4 +Aq, 1 1. H 2 O dissolves 2.07 g. CaSO 4 at 18. (Kohlrausch and Rose, Z. phvs. Ch. 12. 241.) The anhydrous salt varies in solubility. Solubility depends (1) upon temp, and time of drying, (2) upon the relative amount of salt, (3) upon time of shaking. Possibly a and modifications. (Potilizin, C. C. 1894, II. 515.) 2.04 gr. are dissolved in 1 liter of sat. solu- tion at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) At 15 and after 5 minutes shaking, the highest degree of supersaturation which can be obtained with pure sol. calcium sulphate = 9.47 g. of the anhydrous salt or 11.976 g. CaSO 4 +2H 2 O in 1 1. of H 2 O. (Cavazzi, C. C. 1905, 1. 1694.) Solubility of CaSO 4 in 100 pts. H 2 O at high temp. t Pts. CaSO 4 t Pts. CaS0 4 t Pts. CaS0 4 140 165 0.078 0.056 175-185 240 0.027 0.018 250 0.016 (Tilden and Shenstone, Phil. Trans. 1884. 31.) Pptn. of CaSO 4 which has been started by heating solution to 140-150 continues even after solution has cooled. (Storer.) CaSO 4 is completely insol. in sea water or pure H 2 O at temperatures between 140 and 150. (Couste".) Solubility of CaSO 4 in sea water at tempera- tures over 100. t = temp. ; P = pressure in atmospheres; %=per cent CaSO 4 in sat. solution. t p % t p % 103 1 0.500 118.5 1.50 0.226 103.8 1 0.477 121.2 1.5 0.183 105.15 1 0.432 124 2 0.140 108.6 1.25 0.395 127.9 2 0.097 111 1.25 0.355 130 2.5 0.060 113.2 1.25 0.310 133.3 2.5 0.023 115.8 1.50 0.267 (Couste', Ann. Min. (5) 6. 80.) Solubility of CaSO 4 in H 2 O at various pres- sures. 100 g. sat. CaSO 4 +Aq at 1 atmos. pressure and 15 contain 0.206 g. CaSO 4 ; at 20 atmos. pressure and 15 contain 0.227 g. CaSO 4 ; at 1 atmos. pressure and 16.2 contain 0.213 g. CaSO 4 . (Moller, Pogg. 117. 386.) Soluble anhydrite: 1 1. H 2 O dissolves 22.8 milliequivalents at 100. 1 1. H 2 O dissolves 6.4 milliequivalents at 156. Anhydrite: 1 1. H 2 O dissolves 9.2 milliequivalents at 100. 1 1. H 2 O -dissolves 2.7 milliequivalents at 156. 1 1. H 2 O dissolves 0.7 milliequivalents at 218 (Melcher, J. Am. Chem. Soc. 1910, 32. 63.) See also under gypsum, p. 953. Maximum solubility is at 37.5. (Cameron, J. ohys. Chem. 1901, 5. 572.) Sp. gr. of sat. CaSO 4 +Aq at 15 = 1.0022. (Stolba, J. pr. 97. 503.) Sp. gr. of sat. CaSO 4 +Aq. at 31 = 1.0031. 1 pt. CaSO 4 is sol. in 218 pts. H 2 contain- ing C0 2 . (Beyer, Arch. Pharm. (2) 150. 193.) SI. sol. in cold HCl+Aq; completely sol. in boiling dil. HC1 or HNO 3 +Aq. (Rose, Pogg. 95. 108.) Solubility of CaSO 4 in HCl+Aq. 100 ccm. 100 ccm. t % HC1 dissolve g. t % HC1 dissolve g. of CaS0 4 of CaSO4 25 0.77 0.6405 25 6.12 1.6539 25 1.56 0.8821 101 0.77 1 . 1209 25 3.06 1.2639 102 3.06 3.1780 25 4.70 1 . 5342 103 6.12 4.6902 (Lunge, J. Hoc. Chem. Ind. 4. 31.) Solubility in HNO 3 +Aq at 25. g. HNOs par 100 cc. g. CaSO 4 per 100 cc. solution g. HN0 3 per 100 cc. g. CaSO 4 per 100 cc. solution 0.208 6 1.48 1 0.56 8 1.70 2 0.82 10 1.84 3 1.02 12 1.98 4 1.20 (Banthisch, J. pr. 1884, 29. 52.) For s6lubility in H 2 SO 4 see CaH 2 (SO 4 ) 2 . Solubility in H 3 PO 4 +Aq at 25. G. P 2 O5 per 1. G. CaSO 4 per 1. Sp. gr. 25/25 0.0 2.126 5.0 3.138 L002 10.5 3.734 1.007 21.4 4.456 1.016 46.3 5.760 1.035 105.3 7.318 1.075 145.1 7.920 1.106 204.9 8.383 1.145 312.0 7.965 1.221 395.7 6.848 1.230 494.6 5.573 1.344 (Taber, J. phys. Chem. 1906, 10. 628.) Solubility in formic acid at 25. 100 cc. of solution of acid containing 4% SULPHATE, CALCIUM 947 CaCl 2 +Aq. Solubility of CaSO 4 in CaCl 2 +Aq at t 100 ccm. 100 ccm. t % CaCl 2 dissolve g. of t % CaCh dissolve g. of CaSO4 CaS04 23 3.54 0.1225 25 16.91 0.0702 24 6.94 0.0963 101.0 3.54 0.1370 25 10.36 0.0886 102.5 10.36 0.1426 25 15.90 0.0734 103.5 16.91 0.1301 dissolve 0.24 g. CaSO 4 . (Banthisch, J. pr. 1884, 29. 52.) Solubility of CaSO 4 in chloracetic acid at 25. 100 cc. of solution of acid containing 4% dissolve 0.22 g. CaSO 4 ; 10%, 0.25 g. (Banthisch, J. pr. 1.884, 29. 52.) Solubility in H 2 O is increased by presence of NH 4 C1 (Vogel, J: pr. 1. 196), ammonium succinate (Wittstein, Repert. 57. 18), (NH 4 ) 2 S0 4 , (NH 4 ) 2 B 4 7 (Popp, A. Suppl. 8. 11); also KNO 3 (Vogel, Jun.), Na 2 SO 4 (Henry, J. Pharm. 12. 31), NaCl (Tromms- dorf, N. J. Pharm. 18, 1. 234.) Decomp. by alkali carbonates +Aq. (See Storer's Diet.) 1 g. CaSO 4 is sol. in 162 ccm. sat. KCl+Aq at 8; in 147 ccm. sat. NaCl+Aq at 8.5; in 93 ccm. sat. NH 4 Cl+Aq at 12.5; in 94 ccm. sat. KNO 3 +Aq; in 92 ccm. sat. NaNO 3 +Aq; in 320 ccm. sat. NH 4 NO 3 +Aq; in 54 ccm. 2/9 sat. NH 4 NO 3 +Aq; in about 2000 ccm. sat. K 2 SO 4 +Aq. (Droeze.) More sol. in Fe 2 Cl c , Cr 2 Cl 6 , CuCl 2 , ZnCl 2 -. Aq than in H 2 O, but not more sol. in CaCl 2 + Aq. (Gladstone.) NH 4 Cl+Aq. 1 g. CaSO 4 is sol. in 92 ccm. sat. NH 4 C1+ Aq at 13.5; in 94 ccm. l / 2 sat. NH 4 Cl+Aq at 13.5-15.5; in 200 ccm. Vs sat. NH 4 Cl+Aq at 13.5; in 183 ccm. Vs sat. NH 4 Cl+Aq at 100. (Fassbender, B. 9. 1360.) Solubility of CaS0 4 in 25% NH 4 Cl+Aq. Solubility of CaSO 4 in CaCl 2 +Aq at t. (Lunge, I. c.) Solubility of CaSO 4 in H 2 O containing various amts. of CaCl 2 at 20. 100 pts. H 2 O con- taining pts. CaCl 2 dissolve pts. CaSO 4 .' Pts. CaCl 2 Pts. CaS0 4 Pts. CaCh Pts. CaSO4 0.00 11.50 14.39 0.225 0.078 0.063 19.80 51.00 67.05 0.041 0.000 0.000 (Tilden and Shenstone.) t % CaSO 4 t % CaSO4 8 9 25 39 1.030 1.023 1.096 1.126 60 80 120 1.333 1.026 1.000 (Tilden and Shenstone, Roy. Soc. Proc. 38. 335.) t Oa6l 2 % CaS04 t % CaCh 7 CaSO4 15 21 39 72 15.00 14.70 15.00 14.90 0.063 0.068 0.091 0.100 94 138 170 195 15.16 14.70 14.82 14.70 0.110 0.071 0.031 0.022 Solubility in NH 4 Cl+Aq increases with per- centage of NH 4 C1, but if solution contains more than 60 g. NH 4 C1 per 1. more CaO dis- solves than SO 3 . With 333 g. NH 4 C1 per L, the solution contains 4.9 g. SO 3 and 4.4 g. CaO, while the SO 3 content requires only 3.4 g. CaO. (Ditte, C. R. 1898, 126. 694.) Solubility of CaSO 4 in NH 4 Cl+Aq at 25. Grams NH4C1 per liter Grams CaSCh per liter 10.8 24.4 46.7 94.5 149.7 198.6 210.0 275.0 325.0 375.3 (saturated) 3.90 5.38 7.07 8.80 10.30 10.85 10.88 10.60 9.40 7.38 (Cameron and Brown, J. phys. Chem. 9. 211.) 1905, (Tilden and Shenstone, I. c.) Solubility in CaCl 2 +Aq at 25. g. per 1. of solution g. per 1. of solution CaCb CaSO4 CaCl 2 CaSO 4 0.00 2.06 51.53 1.02 7.49 1.24 97.02 0.84 11.96 1.18 192.71 0.47 25.77 1.10 280.30 0.20 32.05 1.08 367.85 0.03 (Cameron and Seidell, J. phys. Ch. 1901, 5. 643.) 1000 pts. of 1% CaCl 2 +Aq. dissolve 1.1414 pts. CaSO 4 ; 40% CaCl 2 , 0.2130 pts. CaSO 4 . (Orloff, Chem. Soc. 1903, 84, (2) 211.) 948 SULPHATE, CALCIUM Solubility in CaO 2 H 2 +Aq at 25. Solubility of CaSO 4 in NH 4 NO 3 +Aq at 25. G. CaS0 4l perl. G. CaO perl. Solid phase G. NH4NOs per 1. G. CaSO 4 per 1. 0.0 1.166 Ca(OH) 2 10 3.18 0.391 1.141 a 25 3.93 0.666 1.150 u 55 5.80 0.955 1.215 (I 100 7.65 1.214 1.242 (I 150 8.88 1.588 1.222 Ca(OH) 2 and CaSO 4 , 2H 2 O 200 9.85 1.634 0.939 CaSO 4 , 2H 2 O 300 10.80 1.722 0.611 it 400 11.40 1.853 0.349 a 550 12.02 1.918 0.176 u 750 12.20 2.030 0.062 u 1000 11.81 2.126 0.0 (t 1200 11.10 1400 10 02 (Cameron and Bell, J. Am. Chem. Soc. 1906, OQ 1OO1 A -L^wVJ saturated J-W . \J 7.55 MgCl 2 +Aq. Sol. in 324 pts. MgCl 2 +Aq (34.1% MgCl 2 ) at 19. (Karsten.) 1 g. CaSO 4 is sol. in 146 ccm. 1/9 sat. MgCl 2 +Aq at 13.5. (Fassbender.) 1 1. VQ sat. MgCl 2 +Aq dissolves 6.83 g. CaSO 4 +2H 2 O at 13.5. (Droeze.) Solubility of CaSO 4 in MgCl 2 +Aq. t % MgCU % CaSO4 9 39 80 19.7 11.1 9.99 0.765 2.744 1.038 (Tilden and Shenstone, I. c.) Solubility in MgCl 2 +Aq at 26 C g. per 1. of solution g. per . of solution MgCh CaSO* H 2 O MgClj CaSO 4 H 2 O 0.0 8.50 19.18 46.64 2.08 4.26 5.69 7.59 997.9 996.5 994.5 989.1 121.38 206.98 337.0 441.0 8.62 6.57 2.77 1.39 972.2 949.9 908.7 878.6 (Cameron and Seidell, J. phys. Ch. 1901, 6. 645.) 1 1. sat. MgCl 2 +Aq at 25 containing 476.5 g. MgCl 2 dissolves 1 .09 g. CaSO 4 . (Cameron and Brown, J. phys. Ch. 1905, 9. 214.) NH 4 NO 3 +Aq. 1 g. CaSO 4 is sol. in 320 ccm. sat. NH 4 NO 3 +Aq at 8-9; in 54 ccm. 2 /9 sat. NH 4 NO 3 + Aq at 13.5; in 103 ccm. 2 /27 sat. NH 4 NO 3 +Aq at 13.5. (Fassbender.) (Cameron and Brown, J. phys. Chem. 1905, 9. 213.) Ca(N0 3 ) 2 +Aq. Solubility of CaSO 4 in Ca(NO 3 ) 2 +Aq at 25. Weight of 1000 cc. of solution G. Ca(NOs)2per 1. G. CaSCh per 1. 998.1 2.084 1013.8 25 1.238 1031.7 50 1.196 1067.3 100 1.134 1136.9 ' 200 0.929 1203.5 300 0.759 1265.6 400 0.569 1328.1 500 0.403 1352.0 544 0.346 (Seidell and Smith, J. phys. Chem. 1904, 8. 498.) M g (N0 8 ) 2 +Aq. Solubility of CaSO 4 in Mg(NO 3 ) 2 +Aq at 25. Weight of 1000 cc. of solution grams G. Mg(NOs)2 perl. G. CaSO4 per 1. 998.1 2.084 1020.5 25 5.772 1039.8 50 7.884 1078.6 100 9.920 1149.8 200 13.340 1219.0 300 14.000 1282.1 400 14.683 1355.3 514 15.040 (Seidell and Smith, J. phys. Chem. 1904, 8 497.) 1 1. sat. Mg(NO 3 ) 2 +Aq at 25 containing 615.1 g. Mg(NO 3 ) 2 dissolves 15.26 g. CaS0 4 (Cameron and Brown, J. phys. Ch. 1905, 9 214.) SULPHATE, CALCIUM 949 KNO 3 +Aq. 1 g. CaSO 4 is sol. in 94 com. sat. KNO 3 + Aq at 13.5; in 82 com. sat. KNO 3 +Aq at 15.5; in 68 ccm. nearly sat. KNO 3 +Aq at 20. (Fassbender.) Solubility in KNO 3 +Aq at 25. KCl+Aq. 1 g. CaSO 4 is sol. in 162 ccm. sat. KCl+Aq at 8; in 295 ccm. l / b sat. KCl+Aq at 9. Solubility in KCl+Aq at 21' Wt. of 1000 ccm. G. KNO 3 G. CaSO4 g- per 1. g. per 1. per 1. per 1 per*! KTM QQO 1 On 2OR1 1008.1 12.5 3.284 2.05 60 6.6 1015.4 25.0 4.080 10 3.6 80 7.2 1032.1 50.0 5.255 20 4.5 100 ,7.5 1052.5 100.0 6.855 40 5.8 125 Double Salt 10.Q9 A. 1 CA 7 QH7 1122 A 2ao.o 8.688 (Ditte, A. ch. 1898, (7) 14. 294. 1153.9 260.0 ( 6.278 a 12.112 a Probably due to formation of double salt Solubility in KI+Aq at 21. of calcium and potassium sulphates. CaK 2 (S0 4 ) 2 +H 2 0. G. KI per 1. G. CaSO 4 perl. G. KI perl. G. CaSO4 per 1. (Seidell and Smith, J. phys. Chem. 1908. 8. 496.) 2.05 100 5.1 NaN0 3 +Aq. 1 g. CaSO 4 is sol. in 92 ccm. sat. NaNO 3 + Aq at 8.5; in 318 ccm. Vs sat. NaNO 3 + Aq at 13.5. (Fassbender.) 100 ccm. sat. NaNO 3 +Aq dissolve 1.086 g. 10 20 40 60 80 2.8 3.2 3.9 4.5 4.85 125 150 200 250 300 5.45 5.8 5.95 6.00 Double salt. CaSO 4 +2H 2 O; 100 ccm. Vs sat. NaNO 3 + Aq dissolve 0.314 g. CaSO 4 +2H 2 O. (Droeze, (Ditte, I. c.) B. 10. 338.) Solubility in NaNO 3 +Aq at 25. Wt. of 1000 ccm. of solution grams G. NaN0 3 per I. G. CaS0 4 per 1. 998.1 2.084 1016.3 25 4.252 1034.0 50 5.500 1058.4 100 7.100 1133.6 200 8.790 1191.6 300 9.282 1363.9 600 7.886 1390.4 655 7.238 (Seidell and Smith, J. phys. Chem. 1904, 8. 495.) 1 1. sat. NaNO 3 +Aq at 25, containing [| 668.4 g. NaNO 3 , dissolves 5.52 g. CaSO 4 . | (Cameron and Brown, J. phys. Ch. 1905, 9. NaCl+Aq. Sol. in 122 pts. sat. NaCl+Aq. (Anthon.) Insol. in sat. NaCl+Aq, but more sol. in dil. NaCl+Aq than in H 2 O. Maximum solubility in NaCl+Aq is when the sp. gr. is 1.033. 1 g. CaSO 4 is sol. in 147 ccm. of sat. XaCl + Aq at 8.5; in 150 ccm. of sat. NaCl+Aq at 13.5; in 149 ccm. of Vs sat. NaCl+Aq at 13.5; in 244 ccm. of ] / 5 sat. NaCl+Aq at 13.5. (Fassbender.) 100 ccm. sat. NaCl+Aq dissolve 0.6785 g. CaSO 4 +2H 2 O at 8.5; 0.6665 g. CaSO 4 + 2H 2 O at 13.5. 100 ccm. Vs sat. NaCl+Aq dissolve 0.671 g. CaSO 4 +2H 2 O at 13.5; sat. NaCl+Aq dissolve 0.4085 g. CaSO 4 + 2H 2 O at 13.5. (Droeze.) 214.) Solubility in KBr+Aq at 21. Solubility of CaSO 4 in NaCl+Aq at t. G. KBr per 1. G. CaS0 4 perl. G. KBr perl. G. CaSO4perl. t Nabl CaS04 t % NaCl % CaSCh 10 20 40 60 80 2.05 3.1 3.6 4.5 5.2 5.9 100 125 150 200 250 6.3 6.7 7.0 7.3 Double salt. 20 44 67 85 101 19.90 19.93 19.95 19.90 20.08 0.823 0.830 0.832 0.823 0.682 130 165 169 179 225 19.92 20.04 20.05 20.10 21.00 0.392 0.250 0.244 0.229 0.178 (Tilden and Shenstone, Roy. Soc. Proc. 38. 331.) (Ditte, A. ch. 1898, (7) 14. 294.) 950 SULPHATE, CALCIUM Solubility of CaSO 4 in NaCl+Aq at t. 100 ccm. 100 ccm. t l&l dissolve g. of t A dissolve g.of CaSO4 CaSO4 21.5 3.53 0.5115 17.5 17.46 0.7369 19.5 7.35 0.6429 101.0 3.53 . 4891 21 11.12 0.7215 102.5 14.18 0.6248 18 14.18 0.7340 103 17.46 0.6299 (Lunge, J. Soc. Chem. Ind. 4. 31.) 100 pts. H 2 O containing pts. NaCl dissolve pts. CaSO 4 at 20. Pts. Pts. Pts. Pts. Pts. Pts. NaCl CaSO4 NaCl CaSO 4 NaCl CaS0 4 0.00 0.225 5.05 6.34 24.40 0.820 0.52 0.301 10.00 7.38 35.10 0.734 2.03 0.441 20.00 0.823 35.86 0.709 5.02 6.15 (Tllden and Shenstone.) Solubility in NaCl+Aq at 26. g. per 1. NaCl CaS04 0.00 9.11 143.99 148.34 2.12 6.66 7.18 7.16 wt. of 1 cc. solution 0.9998 1.0644 1.0981 1.012 g. per 1. NaCl CaS0 4 176.50 228.76 264.17 320.49 7.12 6.79 6.50 5.72 wt. of 1 cc. solution 1.1196 1 . 1488 1 . 1707 1.2034 (Cameron, J. phys. Ch. 1901, 6. 556.) Solubility in NaCl+Aq at 15. G. CaSCh per 1. 2.3 2.5 3.1 3.7 4.8 5.6 7.4 G. NaCl per 1. 0.6 1.1 5.1 10.6 31.1 51.4 139.9 Solubility in NaCl+Aq. 30 52 70 82 d I-: O E sL iL 5^ L d a d d a d d a d 0.5 2.5 0.5 2.3 0.5 2.2 0.0 2.07 10.3 3.6 1.1 2.4 10.0 3.4 1.0 2.18 30.3 5.0 5.0 2.9 29.6 4.9 5.0 2.65 47.3 6.1 10.1 3.5 48.8 5.8 10.1 3.30 73.4 6.9 29.6 5.0 132.7 7.4 29.5 4.68 126.9 7.3 48.3 5.8 195.0 7.6 48.8 5.54 192.4 7.7 75.7 6.6 74.9 6.23 131.6 7.1 128.7 7.00 195.9 7.4 195.1 7.15 (Cameron, J. phys. Ch. 1901, 6. 562.) 1 1. sat. NaCl+Aq at 25 containing 318.3 g. NaCl dissolves 5.52 g. CaSO 4 . (Cameron and Brown, J. phys. Ch. 1905, 9. 214.) Solubility in NaCl+Aq. G. NaCl per 1. of NaCl+Aq G. anhydrous CaSO4 dissolved per litre at 14 at 20 0.0 1.70 2.10 2.925 2.32 2.70 5.850 2.79 3.15 11.70 3.41 3.75 14.62 3.68 4.00 29.25 4.40 4.70 58.50 5.72 6.00 87.75 6.58 6.85 102.3 6.90 7.15 117.0 7.10 7.30 131.6 7.20 7.30 146.2 7.10 7.13 160.8 7.00 7.05 175.6 6.80 6.80 204.7 6.30 6.30 234.0 5.90 5.90 263.2 5.50 5.52 292.6 5.30 5.30 (Cameron, J. phys. Ch. 1901, 6. 559.) Solubility in NaCl+Aq at 26. (d'Anselme, Bull. Soc. 1903, (3) 29. 373.) Solubility in NaCl+Aq. NaCl in 100 g. H 2 O 0.0000 9.4307 15.2056 15.6859 18.8570 25.0478 29.3509 36.5343 CaSCh in 100 g. H 2 O G. NaCl in 100 cc. solution 0.2126 0.6886 0.7581 0.7575 0.7605 0.7439 0.7219 0.6515 0.00 2.44g. 4.77g. 9.50g. 14.22g. 23.15g. 31.30g. G. CaSO4+2H 2 0.200g. 0.635g. 0.826g. 1.056 g. 1.193g. 1.275g. 1.583g. (Cameron, J. phys. Ch. 1901, 5. 564.) (Cloez, Bull. Soc. 1903, (3) 29. 167.) SULPHATE, CALCIUM 951 Solubility in NaCl+Aq at t. When a sat. solution of NaCl is shaken with a mixture of solid NaCl and CaSO 4 + 2H 2 O, the calcium sulphate dissolved, cal- culated from the amount of CaO in solution, is always greater than that calculated from the sulphuric acid in solution. Similar results are obtained when solid calcium sulphate alone is shaken with a sat. solution of NaCl. 10 25 40 50 60 62. 65 71 75 85 In 100 g. of the solution 01 15.253 15.920 15.967 16.123 16.270 16.324 16.361 16.459 16.486 16.524 16.670 17.128 CaSO4 calc. from CaO 0.4464 0.4477 0.4609 0.4938 0.5093 0.5305 0^5435 0.5578 0.5603 0.5399 0.4086 CaSO 4 calc. from SOi 0.4334 0.4426 0.4542 0.4730 0.4832 0.5047 0.5091 0.3749 0.3631 0.3587 0.3519 0.3414 (Arth, Bull'. Soc. 1906, (3) 35. 780.) Within a temp, range from 25-80 CaSO 4 CaSO 4 forms no double salt in solutions oJ NaCl. At any concentration with respect to the latter maximum solubility occurs with 155 g. NaCl per 1. and amounts to 7.3 g. CaSO 4 at 80. (Cameron, J. phys. Chem. 1907, 11. 496.) See also under Gypsum, p. 653. Solubility of CaSO 4 in NaCl+Aq in contact with solid Ca(HCO 3 ) 2 . G. CaSO4 perl. 1.9298 2.7200 3.4460 5.1560 6.4240 5.2720 4.7860 4.4620 G. Ca(HCOs) per 1. 0.0603 0.0724 0.0885 0.1006 0.0603 0.0563 0.0482 0.0402 G. NaCl perl. 0.000 3.628 11.490 39.620 79.520 121.900 193.800 267.600 (Cameron and Seidell, J. phys. Chem. 1901, 6. 653.) (NH 4 ) 2 S0 4 +Aq. Sol. in 287 pts. (NH 4 ) 2 SO 4 +Aq (1:4). (Fresenius, Z. anal. 30. 593.) 1 g. CaSO 4 is sol. in 327 ccm. (NH 4 ) 2 SO 4 +Aq at 9; in 369 ccm. l / 7 sat. (NH 4 ) 2 SO 4 + Aq at 13.5. (Fassbender.) Solubility in sat. (NH 4 ) 2 SO 4 , or Na 2 SO 4 is the same as in H 2 O. (Droeze, B. 10. 330.) Solubility in (NH 4 ) 2 SO 4 +Aq at 25. g. per 1. solution 0.00 0.129 0.258 0.821 1.643 3.287 0.208 0.204 0.199 0.181 0.166 0.154 wt. of 100 cc. solution 99.91 99.91 99.92 99.95 99.99 100.10 6.575 13.15 26.30 84.9 169.8 339.6 0.144 0.146 0.162 0.233 0.333 0.450 wt. of 100 cc. solution 100.36 100.82 101.76 105.34 110.32 119.15 (Sullivan, J. Am. Chem. Soc. 1905, 27. 529.) Solubility in (NH 4 ) 2 SO 4 +Aq at 50. Sp. gr. (NHf) 2 S04 perl. Cal'cu perl. Solid phase 2.168 1.0026 15.65 1.609 1.0113 30.67 1.750 1.0440 91.6 2.542 1.0819 160.4 3.402 .1108 221.6 4.068 CaS0 4 +2H 2 .1385 280.6 4.690 .1653 340.6 5.084 .1972 415.6 5.336 .1964 416.5 5.354 .2043 .2187 428.4 479.4 4.632 3.524 CaSO4, (NH4) 2 SO4-t- .2437 530.8 2.152 2H 2 O .2480 558.0 1.986 .2502 564.7 1.98 1.2508 566.0 1.08 (NH 4 )2SO4 1.2510 566.7 (Bell and Taber, J. phys. Chem. 1906, 10. 120.) Solubility of CaSO 4 in (NH 4 ) 2 S0 4 +Aq at t. Excess of (NH4) 2 S04 Excess of CaSO4 6 40.5 58 78 100 0.1529 0.1569 0.1662 0.1968 0.2546 *3 55 41.82 44.55 46.07 47.51 49.45 3 31 60 75 80 84 100 0.3782 0.4070 0.5083 0.5898 0.6108 0.5725 0.4895 36.62 35.50 34.97 34.86 34.88 32.40 25.97 (Barre, C. R. 1909, 148. 1605.) The solubility of CaSO 4 in H 2 O is consider- ably increased by the presence of (NH 4 ) 2 SO 4 952 SULPHATE, CALCIUM but decreased by the presence of K 2 S0 4 . (Barre, C. R. 1909, 148. 1606.) CuSO 4 +Aq. Solubility in CuSO 4 +Aq at 25. Solubility in K 2 SO 4 +Aq at 25. g. per 1. wt. of 1 cc. of solution K 2 S04 CaSO 4 0.0 4.88 5.09 9.85 19.57 28.35 30.66 32.47* 2.08 1.60 1.56 1.45 1.49 1.55 1.57 1.58 1 1 1 1 1 .9981 .0036 .0038 .0075 .151 .0229 .0236 Sp. gr. of the solution 25/25 g. CuSp4 per 1. g. CaSO 4 perl. .002 .005 .007 .009 .016 .021 .030 .041 .051 .061 .098 .146 .192 .218 1.144 3.564 6.048 7.279 14.814 19.729 29.543 39.407 49.382 58.880 97.950 146.725 196.021 224.916 2.068 1.986 1.944 1.858 1.760 1.736 1.688 1.718 1.744 1.782 1.931 2.048 2.076 2.088 *Solid phase syngenite. (Cameron and Breazeale, J.phys. Ch. 1904, 8. 335.) Solubility in K 2 SO 4 +Aq. at 25. In 1000 g. of the solution mole K 2 SO 4 mole CaSO 4 3.223 0.223 (D'Ans, Z. anorg. 1909, 62. 151.) Solubility of CaSO 4 in K 2 SO 4 +Aq at t. Excess of K 2 SO4 Excess of CaSO4 (Bell and Taber, J. phys, Ch. 1907, 11. 637.) MgS0 4 +Aq. Insol. in sat. MgSO 4 +Aq. 1 g. CaSO 4 is sol. in 1162 ccm. Vio sat. MgSO 4 +Aq at 13.5. (Fassbender, B. 9. 1360.) ^ Sol. in 635 pts. sat. MgSO 4 +Aq at 19. (Karsten.) Absolutely insol. in sat. MgSO 4 +Aq, and t 4 ^3 M 4 GC M 0* 18 51 80 99 0.1296 0.1531 0.1754 0.1922 0.1980 2.00 2.79 4.21 5.00 5.39 0.0229 0.0271 0.0300 0.0349 0.0371 6.99 9.81 14.18 17.55 19.70 of MgSO 4 . (Droeze, B. 10. 340.) 1 1. Vio sat. MgSO 4 +Aq dissolves 0.86 g. CaSO 4 +2H 2 O. (Droeze.) Solubility in MgSO 4 +Aq at 25. g. per 1. Sp. gr. at 25/25 g. per I. Sp. gr. at 25/25 MgSO4 CaSO4 MgSO4 CaS04 0.0 2.046 1.0032 149.67 1.597 1.1377 3.20 1.620 1.0055 165.7 1.549 1.1479 6.39 1.507 1.0090 171.2 1.474 1.1537 10.64 1.471 1.0118 198.8 1.422 1.1813 21.36 1.478 1.0226 232.1 1.254 1.2095 42.68 1.558 1.0419 265.6 1.070 1.2382 64.14 1.608 1.0626 298.0 1.860 1.2624 85.67 1.617 1.0833 330.6 0.647 1.2877 128.28 1.627 1.1190 355.0 0.501 1.3023 (Barre, C. R. 1909, 148. 1606.) Ag 2 S0 4 +Aq. 1 1. of the solution contains 2.31 g. CaSO 4 +7.23 g. Ag 2 SO 4 = 9.54 g. mixed salts at 17. Sp. gr. = 1.0083. 1 1. of the solution contains 2.61 g. CaSO 4 -f- 8.11 g. Ag 2 SO 4 = 10.72 g. mixed salts at 25. Sp. gr. = 1.010. (Euler, Z. phys. Ch. 1904, 49. 313.) Na 2 S0 4 +Aq. 1 g. CaSO 4 is sol. in 398 ccm. sat. Na 2 SO 4 + Aq at 10.5. Solubility of CaSO 4 in Na 2 SO 4 +Aq at 22 (Cameron and Bell, J. phys. Ch. 1906, 10. 210.) G. CaSC>4 per 1. G. Na 2 S04 per 1. 2.084 0.000 1.583 2.771 1.433 13.820 1.408 16.360 1.569 39.310 1.841 77.320 2.185 133.00 2.414 193.800 *2.578 *222.580 *Both (JaSO 4 and Na 2 iSO 4 as solid phases in contact with the solution. (Cameron and Seidell, J. phys. Chem. 1901, 5. 650.) SULPHATE, CALCIUM 953 Solubility in Na 2 SO 4 +Aq at 25. Solubility in N/200 KHC 2 H 4 O 6 +Aq+ o /o tartanc acid U.Jooo g. Ua&u 4 per 1UU wt. of 1000 ccm. of solution grams g. Na2SO4 per 1. * g. CaSO 4 per 1. g. solution. Solubility in 10% alcoholic N/400 1001.26 1007 59 2.390 9 535 1.650 1 457 KHC 2 H 4 O 6 +5% tartaric acid = 0.1086 g. CaSO 4 in 100 g. solution. (Magnanini.) 1011.45 1020.46 14.132 24.369 1.388 1.471 Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethylacetate. (Naumann, B. 1031.48 36.979 1.563 1910, 43. 314.) 1039.12 1079.47 46.150 94.220 1.650 1.980 Solubility in sugar +Aq at t. 1096.47 115.084 2.096 G. CaSO4 dissolved in 1 1. sugar solutions 1142 66 146 612 2 234 % 1176.47 205.105 2.503 sugar 30 40 50 60 70 80 1212.00 257 . 100 .650 o 2 157 1 730 1 730 1 652 1 710 (Cameron and Breazeale, J. phys. Chem. 10 2.041 1.730 1.730 1.574 1.574 1.613 1904, 8. 340.) 20 1.808 1.652 1.419 1.380 1.419 1.263 27 1.550 1.438 1.361 1.283 1.283 0.972 1 1. sat. Na 2 SO 4 +Aq at 25 containing 254.09, Na 2 SO 4 dissolves 2.58 g. CaSO 4 .. (Cameron and Brown. J. phys. Ch. 1905, 9 214.) 35 42 49 55 1.263 1.030 1.050 0^564 0.486 1.088 0.777 0.739 0.505 1.108 0.816 0.564 0.486 0.914 0.855 0.603 0.369 0^729 0.486 0.330 and accelerated by cone, solution of sodium, potassium, ammonium and magnesium sul- phates. (Rohland, Z. Elektrodiem. 1908, 14. 422.) More than 10 times as much CaSO 4 dis- solves in sat. Na 2 S 2 O 3 + Aq as in H 2 O. (Diehl. Insol. in alcohol, of 0.905 sp. gr. or less. (Anthon, J. pr. 14. 125.) Solubility in 10% alcohol = 0.0970 g. CaSO 4 per 100 g. solution. (Magnanini, Gazz. Ch. it. 1901, 31. (2) 544.) Sol. in dil. alcoholic solutions of NH 4 NO 3 , KN0 3 , NaN0 3 , NH 4 C1, KC1, and NaCl. (Margueritte, C. R. 38. 308.) Sol. to considerable extent in NH 4 C 2 H 3 O 2 + Aq, especially if freshly pptd. More sol. in NH 4 C 2 H 3 O 2 +Aq than in NH 4 Cl+Aq. (Weppen, J. pr. 11. 182.) More sol. in NH 4 C 2 H 3 O 2 + Aq than in other NH 4 salts. (Cohn, J. pr. (2) 35. 43.) More sol. in NaC 2 H 3 O 2 +Aq or KCl+Aq than in H 2 O. (Mulder.) Solubility in N/200 potassium hydrogen tartrate +Aq = 0.2323 g. CaSO 4 per 100 g. solution. (Magnanini, Gazz. ch. it. 1901, 31. (2) 544.) 72.61 millimols. per 1. of CaSO 4 +2H 2 O are sol. at 25 in ammonium citrate +Aq (con- centration = 0.5 millimols. per 1.) 36.39 millimols per 1. of CaSO 4 -f2H 2 O are sol. at 25 in sodium citrate -{-Aq. (Con- centration = 0.25 millimols per 1. (Rindell, Z. phys. Ch. 1910, 70. 452.) 100 pts. glycerine dissolve 0.957 pt. CaSO 4 +2H 2 O, and solubility increases with the temp. (Asselin, C. R. 76. 884.) 100 g. glycerine (sp. gr. 1.256) dissolve 5.17 g. CuSO 4 at 15-16. (Ossendowski, Pharm. J. 1907. 79. 575.) Solubility in 10% alcoholic N/200 KHC 2 H 4 O 6 +Aq= 0.0866 g. CaSO 4 per 100 g. solution. (Stolle, Z. Ver. Zuckerind, 1900, 60. 331). Min. Anhydrite. +2H 2 O. Min. Gypsum. Gypsum. A sat. aq. solution of gypsum of particles not less than 2^ contains 2.085 g. CaS0 4 per litre at 25. A sat. aq. solution of gypsum of particles not smaller than 0.3/u. contains 2.476 g. CaSO 4 per liter at 25. (/x =0.0001 cm.) (Hulett and Allen, Z. phys. Ch. 1901, 37. 391 and 393.) Solubility in H 2 O at t. t g. CaSCh in 100 ccm. of the solution Density of the solution at t o' 0.17590 1.001970 10 0.19285 1.001727 18 0.20160 1.000590 25 0.20805 0.999109 30 0.23935 0.997891 35 0.20960 0.996122 40 0.20970 0.994390 45 0.20835 0.992370 55 0.20095 0.987960 65.3 0.19320 0.982560 75 0.18475 0.977724 100 0.16195 (Hulett and Allen, J. Am. Chem. Soc. 1902, 24. 674.) 1 1. H 2 O dissolves 2.13 g. CaSO 4 +2H 2 at 25. (Euler, Z. phys. Ch. 1904, 49. 314.) 2023 mg. are dissolved in 1 1. of sat. solution at 18. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) 1 1. H 2 O dissolves 2.267 g. CaSO 4 +2H 2 O at 0; 2.684 g. at 35; 2.662 g. at 50; and 2.155 g. at 100. (Cavazzi, C. C. 1905, I. 1693.) 954 SULPHATE, CALCIUM HYDROGEN 1 1. H 2 O dissolves 29.5 milliequivalents at 18; 30 at 50; 23.3 at 100. (Melcher, J Am. Chem. Soc. 1910, 32. 63.) See also under CaSO 4 . Solubility of pulverized gypsum in NaCl+Aq at 23. Grams gypsum G. NaCl per 1. G. CaSO4 per 1. 2.99 0.99 2.37 3.82 4.95 3.02 4.48 10.40 3.54 6.31 30.19 4.97 7.51 49.17 5.94 8.53 75.58 6.74 9.42 129.50 7.50 9.17 197.20 7.25 8.88 229.70 7.03 7.19 306.40 5.68 6.79 315.55 5.37 (Cameron, J. phys. Chem. 1901, 6. 559.) See also under CaSO 4 . Plaster of Paris contains according to Chatelier (C. C. 1889, 1. 203). Calcium hexahydrogen sulphate, CaH 6 (SO 4 ) 4 . Decomp. by H 2 O. (Schultz, Pogg. 133. 137.) ^ Calcium cupric potassium sulphate. Ca 2 K 2 Cu(SO 4 ) 4 -f2H 2 O. (D'Ans, B. 1908, 41. 1778.) Calcium magnesium potassium sulphate. 2CaS0 4 , MgS0 4 , K 2 SO 4 +2H 2 O. Min. Polykalite. Sol. in H 2 O with residue of CaSO 4 . 4CaSO 4 , MgSO 4 K 2 SO 4 +2H 2 0. Min. Krugite. Decomp* by H 2 O. Calcium potassium sulphate, CaK 2 (SO 4 ) 2 + H 2 O. Min. Syngenite. Sol. in 400 pts. H 2 O. (Zepharovitch.) Less sol. than K 2 SO 4 . Decomp. by heating with separation of CaSO 4 Decomp. by H 2 O until 25 g. K 2 SO 4 are dis- solved in a litre, after which there is composition. (Ditte, C. R. 84. 86.) Easily sol. in dil. acids. (Phillips.) no de- Solubility of syngenite, CaK 2 (SO 4 ) 2 +H 2 O in K 2 SO 4 +Aq at 25. Calcium hydrogen sulphate, CaH 2 (SO 4 ) 2 . 100 pts. H 2 SO 4 of 1.82 sp. gr. dissolve about 2 pts. CaSO 4 ; 100 pts. fuming H 2 SO 4 dissolve 10.17 pts. CaSO 4 (Struve, Z. anal. 9. 34); 100 pts. H 2 SO 4 dissolve 2.5 pts. CaSO 4 (Lies- Bodart and Jacquemin, C. R. 46. 1206); CaSO 4 is precipitated by H 2 O from H 2 SO 4 solution. 100 pts. boiling H 2 SO 4 dissolve 10 pts. CaSO 4 . (Schultz, Pogg. 133. 137.) Solubility : of CaSO 4 in H 2 SO 4 +Aq. Wt. of 1000 ccm. of solution grams g. K 2 S0 4 per 1. g. CaSO4 per 1. 1013.08 1015.78 1020.01 1024.54 1036.82 1058.10 1085.91 16.31 19.87 25.01 30.83 46.99 75.45 112.87 *1.495 1.529 1.537 1.565 0.810 0.451 0.330 *In first four determinations syngenite completely decomposed. (Cameron and Breazeale, J. phys. Chem. 1904, 8. 339.) This double salt is stable between and )9 in the presence of an excess of either CaSO 4 or K 2 S0 4 . In this temp, interval the double sulphate, 2CaSO 4 , K 2 SO 4 , 3H 2 O de- scribed by Ditte (C. R. 84. 867) does not exist. (Barre, C. R. 1909, 148. 1607.) Ca 2 K 2 (SO 4 ) 3 +3H 2 O. Decomp. by cold H 2 O. (Ditte, C. R. 84. 867.) 5CaS0 4 , K 2 SO 4 +H 2 O. Slowly decomp. by H 2 O. (van't Hoff and Geiger, B. A. B. 1904. 935.) Calcium potassium zinc sulphate, Ca 2 K 2 Zn(SO 4 ) 4 +2H 2 O. (D'Ans, B. 1908, 41. 1778.) wt. of 1000 ccm. of solution at 25 g. H 2 S04 per 1. g. CaSO4 per 1. at 25 35 43 999.1067 1002.493 1002.553 1005.091 1009.787 1030.151 1043.470 1075.613 1113^392 1141.755 1168.143 0.00 0.48 4.87 8.11 16.22 48.67 75.00 97.35 146.01 194.70 243.35 292.02 2.126 2.128 2.144 2.203 2.382 2.727 2.841 2.779 2.571 2.313 1.901 1.541 2^209 2.451 3^397 3^606 3.150 2.145 2.236 2.456 2.760 3.116 3.843 4.146 4!i39 3.551 2.959 2.481 (Cameron and Breazeale, J. phys. Chem. 1903, 7. 574.) 100 pts. hot cone. H 2 SO 4 dissolve approx. 10 pts. CaSO 4 . (Rohland, Z. anorg. 1910, 66. 206.) Decomp. by H 2 O. Calcium rubidium sulphate, Ca 2 Rb 2 (SO 4 ) 3 . (D'Ans, B. 1907, 40. 4913.) +3H 2 O. Decomp. by H 2 O. (Ditte, C. R. 84. 86.) CaRb 2 (SO 4 ) 2 +H 2 O. (D'Ans.) SULPHATE, CEROUS 955 Calcium sodium sulphate, CaNa 2 (SO 4 )2. Min. Glauberite. Gradually sol. in H 2 O, but crystals of CaSO 4 +2H 2 O soon separate out. (Fritzsche.) Insol. in alcohol, and cone. NaC 2 H 3 O 2 + Aq; decomp. by H 2 O. (Folkhard, C. N. 43. 6.' CaNa 4 (SO 4 ) 3 +2H 2 O. Decomp. by H 2 O. (Fritzsche.) Calcium titanium sulphate, CaS0 4 , Ti(SO 4 ) 2 . Ppt.; decomp. by H 2 O giving titanic acid. (Weinland, Z. anorg. 1907, 54. 254.) Calcium uranium sulphate. Min. Uranochalcite. Min. Medjidite. Easily sol. in dil. HC1-J- Aq. Cerous sulphate, Ce 2 (SO 4 ) 3 . Anhydrous cerous sulphate is much more sol. in H 2 O than the hydrated salt. Easily sol. in cold H^O if added thereto in small amounts. If large amount of Ce 2 (SO 4 ) 3 is treated with a little H 2 O it hardens with evolution of heat, and becomes very difficultly soluble. 100 pts. H 2 O dissolve 161 pts. Ce 2 (SO 4 ) 3 at and 17.86 pts. at 19. Ce 2 (SO 4 ) 3 +Aq sat. in cold deposits Ce 2 (SO 4 ) 3 at 75, and only 2.25 pts. remain in solution at 100. (Jolin, Bull. Soc. (2) 21. 536.) 100 pts. H 2 O dissolve 8.31 pts. Ce 2 (SO 4 ) 3 at 20; 8.08 pts. at 45; 4.95 pts. at 60; 0.504 pt. at 100. (Biihrig, J. pr. (2) 12. 240.) 60 pts. anhydrous salt dissolve quickly at 0-3 in 100 pts. H 2 O. At 15 the solution solidifies, and the mother liquor contains only 27.88% Ce 2 (SO 4 ) 3 . At 15 the maximum attainable strength is 31.62% Ce 2 (SO 4 ) 3 . (Brauner, Chem. Soc. 53. 357.) 100 pts. H 2 O dissolve 10.747 pts. Ce 2 (SO 4 ) 3 at 16; 9.648 pts. at 19; 6.949 pts. at 33. The solubility of Ce 2 (SO 4 ) 3 in H 2 O is dimin- ished by the addition of (NH 4 ) 2 SO 4 , K 2 SO 4 or Na 2 SO 4 . (Barre, C. R. 1910, 151. 872.) Sp. gr. of Ce 2 (SO 4 )3+Aq was found to be con- stant whether Ce 2 (SO 4 ) 3 or Ce 2 (SO 4 ) 3 + 8H 2 O was used. The following results were obtained at 15. Pts. Ce 2 (S0 4 )3to 100 pts. H 2 O Sp. gr. Pts. Ce 2 (SO4)sto 100 pts. H 2 O Sp. gr. 3.17 6.11 8.35 9.61 10.55 11.66 .03005 .05812 .07910 .09085 .09939 . 10987 12.66 14.56 15.64 21.19 31.62 1.11917 1 . 13665 1 . 14623 1 . 19640 1.28778 Per 100 pts. H 2 O (NH 4 ) 2 S04 Ce 2 (SO4)3 0.00 10.747 3.464 1.026 9.323 0.782 19.240 0.748 29.552 0.701 45.616 0.497 55.083 0.194 63.920 0.090 72.838 0.035 (Brauner, Chem. Soc. 53. 357.) 4.5 pts. Ce 2 (SO 4 ) 3 dissolve in 100 pts. H 2 SO 4 . (Wyrouboff, Bull, Soc. (3) 2. 745.) j Solubility in (NH 4 ) 2 SO 4 +Aq at 16. (Barre, A. ch. 1911, (8) 24. 252.) Solubility in Na 2 SO 4 +Aq at 19-20. Per 100 pts. H 2 O Na 2 S0 4 Ce 2 (S0 4 )3 0.00 9.64 0.328 0.637 0.684 0.259 1.091 0.0937 1.392 0.057 1.699 0.0303 2.640 0.012 3.589 0.0065 5.660 0.0046 7.710 0.0037 (Barre, A. ch. 1911, (8) 24. 251.) Solubility in K 2 SO 4 +Aq at 16. Per 100 pts. H 2 O K 2 SO4 Ce 2 (SO 4 ) 3 0.00 0.178 0.510 0.726 1.290 10.747 0.956 0.432 0.250 0.0419 (Barre, A. ch. 1911, (8) 24. 248.) +4H 2 O. 100 g. H 2 O dissolve at: 35 -40 50 57 8.5 6.04 3.43 2.34 g. Ce 2 (SO 4 ) 3 . 65 70 82 100.5 bpt. of sat. solution. 1.883 1.38 1.01 0.43 g. Ce 2 (SO 4 ) 3 . (Koppel, Z. anorg. 1904, 41. 399.) 956 SULPHATE, CEROCERIC +5H 2 0. 100 pts. H 2 O dissolve pts. Ce 2 (SO 4 ) 3 at t. t Pts. Ce 2 (SO 4 )3 100 80 60 50 40 0.775 1.70 3.45 5.56 8.20 (Muthmann and Rolig, Z. anorg. 1898, 16. 456.) 100 g. H 2 O dissolve at: 45 60 70 8.833 3.247 1.929 g. Ce 2 (SO 4 ) 3 . 80 90 100.5 bpt. of sat. solution. 1.207 0.8355 0.469 g. Ce 2 (SO 4 ) 3 . Muthmann and Rolig's determinations are inaccurate. (Koppel.) +8H 2 0. 100 pts. H 2 O dissolve 14.92 pts. Ce 2 (SO 4 ) 3 at 20 from Ce 2 (SO 4 ) 3 +8H 2 O 3 (John.) 100 pts. H 2 O dissolve pts. Ce 2 (SO 4 ) 3 at t. t Pts. Ce 2 (S04)3 t Pts. Ce 2 (SO4) 3 18 30 19.10 17.32 16.13 50 60 70 12.48 9.40 4.24 (Muthmann and Rolig.) 100 g. H 2 O dissolve at: 15 20.4 10.09 11.06 9.525 g. Ce 2 (SO 4 ) 3 , 30 40 50 60 7.388 5.947 4.785 4.064 g. Ce 2 (SO 4 ) 3 . Previous determinations are inaccurate. (Koppel, Z. anorg. 1904, 41. 395.) 100 g. sat. solution at 25 contain 7.60 g. anhydrous salt. (Wirth, Z. anorg. 76. 174.) Solubility in H 2 SO 4 +Aq at 25. Solid phase Ce 2 (SO 4 ) 3 +8H 2 O. Normality H 2 SO 4 In 100 g. of the liquid are dissolved g. Ce 2 O 3 g. Ce 2 (SO 4 )3 0.1 1.1 2.16 4.32 6.685 9.68 15.15 4.604 4.615 3.64 3.01 2.0 0.9115 0.4339 0.145 7.60 7.618 6.00 5.018 3.301 1.505 0.733 0.239 (Wirth, Z. anorg. 1912, 76. 191.) +9H 2 O. 100 pts. H 2 O dissolve 17.52 pts. Ce 2 (SO 4 ) 3 from Ce 2 (SO 4 ) 3 +9H 2 O. (Brauner. 100 g. H 2 O dissolve at: 15 21 30 31.2 20.98 11.87 9.725 7.353 7.185 g. Ce 2 (SO 4 ) 3 , 31.6 45 50 60 65 7.164 5.13 4.673 3.88 3.595 g. Ce 2 (SO 4 ) 3 . (Koppel.) . + 12H 2 O. 100 pts. H 2 O dissolve pts. Ce 2 (SO 4 ) 3 at t. 18 25 Pts. Ce 2 (S04)s 21.40 18.44 16.22 (Muthmann and Rolig, Z. anorg. 1898, 16. 457.) 100 g. H 2 O dissolve at: 18.8 19.2 16.56 17.52 17.70 g. Ce 2 (S0 4 ) 3 . Previous determinations are inaccurate. (Koppel.) Ceroceric sulphate, Ce 2 (SO 4 ) 3 , 2Ce(SO 4 ) 2 -f 24H 2 O. Decomp. by H 2 O. Sol. in HCl+Aq with decomp. (Mendelejeff, A. 168. 45.) Ce 2 (SO 4 ) 3 , 3Ce(SO 4 ) 2 +31H 2 O. (Jolin.) Ceric sulphate, basic, CeO 2 , SO 3 -f 2H 2 O. Very si. sol. in H 2 O. Sol. in 2500 pts. H 2 O. (Mosander.) Boiling H 2 gradually dissolves out H 2 SO 4 . (Erk.) Sol. in acids. 8CeO 2 , 7SO 3 +12H 2 O; 8CeO 2 , 7SO 3 + 15H 2 O; 6CeO 2 , 5SO 3 +5H 2 O; 4CeO 2 , 3SO 3 + 7H 2 O; and 3Ce(SO 4 ) 2 , 5Ce(OH) 4 . All are insol. ppts. Ceric sulphate, Ce(SO 4 ) 2 . Anhydrous. Very slowly sol. in. cold, more rapidly in hot H 2 O. When solution has once begun, almost unlimited quantities may be dissolved. Insol. in cone. H 2 SO 4 . (Meyer, B. 1904, 37. 144.) +4H 2 O. Sol. in H 2 O with immediate de- comp. (Rammelsberg.) Decomp. by H 2 O. (Muthmann, B. 1900, 33. 1764.) Cerous hydrogen sulphate, Ce 2 (S0 4 ) 3 , 3H 2 SO 4 . Decomp. by H 2 O. (Wyrouboff, Bull. Soc. (3) 2. 745; Brauner, Z. anorg. 1904, 38. 329.) Ceroceric hydrogen sulphate, Ce 2 H(SO 4 ) 4 + 13H 2 O. Sol. in H 2 O. Forms very supersat. solu- tions. Solubility in H 2 SO 4 decreases with increase in concentration of the acid. (Meyer, B. 1904, 37. 146.) SULPHATE, CHROMIC HYDROGEN 957 Cerous potassium sulphate, Ce 2 (SO 4 ) 3 , K 2 SO 4 +2H 2 SI. sol. in H 2 O; insol. in sat. K 2 SO 4 +Aq. (Czudnowicz, J. pr. 80. 26.) 2Ce 2 (SO 4 ) 3 , 3K 2 SO 4 . As above. (Her- mann, J. pr. 30. 188.) +8H 2 O. (Barre, A. ch. 1911, (8) 24. 249.) Ce 2 (SO 4 ) 3 , 2K 2 SO 4 +3H 2 O. As above. (Jolin.) Ce 2 (SO 4 ) 3 , 3K 2 SO 4 . Sol. in about 56 pts. H 2 O at 9-20. Easily sol. in acidified H 2 O. Nearly insol. in sat. K 2 SO 4 -f Aq. (Jolin.) Ce 2 (SO 4 ) 3 , 5K 2 SO 4 . Insol. in K 2 SO 4 +Aq. (Barre, J.c.) Ceric potassium sulphate, Ce(SO 4 ) 2 , 2K 2 SO 4 +2H 2 0. SI. sol. in H 2 O with decomp. Insol. in sat. K 2 S0 4 +Aq. Ceric silver sulphate, 10Ce(SO 4 ) 2 , 6Ag 2 SO 4 . Only si. sol. in cold H 2 O; decomp. by hot H 2 O in which it is readily sol. (Pozzi-Escot, C. R. 1913, 166. 1074.) ' Cerous sodium sulphate, Ce 2 (SO 4 ) 3 , Na 2 SO 4 + 2H 2 O. Very si. sol. in H 2 O, and still less in Na 2 SO 4 +Aq. 100 ccm. sat. Na 2 SO 4 +Aq dissolve an amount corresponding to 6.2 mg. Ce 2 O 3 . (Jolin.) SI. sol. in HCl+Aq. (Czudnowicz.) Cerous thallous sulphate, Ce 2 (S0 4 ) 3 , 3T1 2 SO 4 . Ppt. Ce 2 (S0 4 ) 3 , T1 2 S0 4 +2H 2 0. Sol. in H 2 O. (Zschiesche, J. pr. 107. 98.) +4H 2 O. Very si. sol. in cold, somewhat more in warm H 2 O. (Wyrouboff, Bull. Soc. Min. 14. 83.) Cerous tin (stannic) hydrogen sulphate. CeHSn(S0 4 ) 4 . Decomp. by H 2 O. Sol. in very dil. HC1. (Weinland, Z. anorg. 1907, 64. 251.) Chromous sulphate, CrSO 4 +7H 2 O. 100 pts. H 2 O dissolve 12.35 pts. CrSO 4 + 7H 2 O. Aqueous solution can be boiled with- out decomp. SI. sol. in alcohol. +H 2 O. (Moissan, Bull. Soc. 37. 296.) Chromic sulphate, basic, 3Cr 2 O 3 , 2SO 3 + 12H 2 O =2Cr 2 (SO 4 )(OH) 4 , Cr 2 (OH) 6 + 5H 2 O. Insol. in H 2 O. Sol. in acids. Slowly de- comp. by KOH+Aq or K 2 CO 3 +Aq. 5Cr 2 O 3 , 3SO 3 . Sol. in H 2 O. (Recoura, C. R. 112. 1439.) Cr 2 O 3 , SO 3 = Cr 2 O 2 (SO 4 ). Ppt. (Schiff, A. 124. 167.) +10H 2 O or [Cr(OH) 2 (OH 2 ) 4 ] 2 SO 4 . Nearly insol. in H 2 O. (Werner, B. 1908, 41. 3451.) 5Cr 2 O 3 , 8SO 3 (?). (Siewert, A. 126. 97.) Cr 2 O 3 , 2SO 3 = Cr 2 O(SO 4 ) 2 . Easily sol. in a little H 2 O, but a precipitate is thrown down by further addition of H 2 O, which redissolves on evaporation. 5Cr 2 O 3 , 12SO 3 (?). (Siewert.) 2Cr 2 3 , 5SO 3 +15H 2 O. Sol. in H 2 O; insol. in alcohol and acetone by which it is ppt. from aqueous solution. (Nicolardot, C. R. 1907, 146. 1338.) Chromic sulphate, Cr 2 (SO 4 ) 3 . Anhydrous. Insol. in H 2 O. HNO 3 , HC1, H 2 SO 4 , aqua regia, and NH 4 OH+Aq. De- comp. by boiling caustic alkalies, and 'slowly by alkali carbonates +Aq. (Schrotter.) Ac- cording to Traube (A. 71. 92) and Siewert (A. 126. 94), Schrotter's salt is an acid sulphate, Cr 4 (S0 4 ) 6 (OS0 2 OH) 2 = 2Cr 2 (SO 4 ) 3 , H 2 SO 4 . According to fitard (Bull. Soc. (2) 31. 200) both salts exist, and formula of above salt is Cr 2 (SO 4 ) 6 Cr 2 . Formula is 2[(Cr 2 O 3 ) 2 , (SO 3 ) 6 ], 17H 2 SO 4 (?). (Cross and Higgins, Chem. Soc. 41. 113.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann. B. 1910, 43. 314.) +6H 2 O (?). Green modification. Readily sol. in H 2 O or alcohol. Sol. in cone. H 2 SO 4 . H 2 O solution is converted into the violet mod- ification by standing 3-4 weeks. (Schrotter.) +11H 2 O (?). Extremely deliquescent; be- comes liquid in moist air in 2 minutes. Not pptd. by BaCl 2 +Aq. (Recoura, C. R. 113. 857.) +18H 2 O. Violet modification. Sol. in 0.833 pt. H 2 O at 20. When the H 2 O solution is heated to 65-70 it begins to be converted into the green modification. This conversion is also brought about by cold HNO 3 , H 2 SO 4 , PC1 3 . (fitard, C. R. 84. 1090.) Sp. gr. of aqueous solution of violet modi- fication of Cr 2 (SO 4 ) 3 containing: 5 10 20% Cr 2 (SO 4 ) 3 +18H 2 O, 1.0275 1.0560 1.1150 30 40 50%Cr 2 (SO 4 ) 3 +18H 2 O. 1.1785 1.2480 1.3250 Sp. gr. of aqueous solution of green modi- fication of Cr 2 (SO 4 ) 3 containing: 10 20 30%Cr 2 (SO 4 ) 3 +18H 2 O, 1.0510 1.1070 1.1680 40 50 60%Cr 2 (S0 4 ) 3 +18H 2 0, 1.2340 1.3055 1.3825 70 80% Cr 2 (SO 4 ) 3 +18HO 2 . 1.4650 1.5535 (Gerlach, Z. anal. 28. 494.) See also Chromosulphuric acid. Chromic hydrogen sulphate, Cr 2 (SO 4 ) 3 , H 2 SO 4 +16H 2 O. Two modifications. a. Violet. Decomp. by H 2 O. b. Green. Obtained from violet modifica- tion on heating. Sol. in H 2 0. (Weinland, Z. anorg. 1906, 49. 157.) 958 SULPHATE, CHROMIC CUPRIC +24H 2 O. Decomp. by alcohol, giving the normal sulphate. (Weinland.) Cr 2 (S0 4 ) 3 , 2H 2 SO 4 +18H 2 O. Hygroscopic. Decomp. by H 2 O. (Weinland.) 2Cr 2 (S0 4 ) 3 , H 2 S0 4 = C Correct composition of Cr 2 (SO 4 ) 3 (Traube), which see. See also Chromosulphuric acid. Chromic cupric sulphate, Cr 2 (S0 4 ) 2 , 2CuS0 4 , H 2 S0 4 . Insol. in H 2 O, but gradually decomp. there- by. (Etard, C. R. 87. 602.) * Cr 2 O 3 , CuO, 4SO 3 . Insol. in H 2 O. (Recoura, C. R. 1893, 117. 39.) Chromous hydrazine sulphate, CrSO 4 , 2N 2 H 4 , H 2 S0 4 . Only si. sol. in H 2 O. Sol. in acids. (Traube B. 1913, 46. 1507.) Chromic hydroxylamine sulphate, Cr 2 (SO 4 ) 3 , (NH 2 OH) 2 SO 4 +24H 2 O. Sol. in H 2 O. (Meyeringh.) Chromic iron (ferrous) sulphate, Cr 2 (SO 4 ) 3 , 2FeSO 4 , H 2 SO 4 +2H 2 O. As above. (Etard, I.e.) Chromic iron (ferric) sulphate, Cr 2 (S0 4 ) 3 , Fe 2 (S0 4 ) 3 . Insol. in H 2 O. (Etard, C. R. 86. 1399.) Cr 2 (S0 4 ) 3 , Fe 2 (SO 4 ) 3 , H 2 SO 4 . Insol. in H 2 0. (Etard.) Chromic lithium sulphate, Cr 2 (SO 4 ) 3 , 3Li 2 SO 4 . Resembles the corresponding K salt. (Wer- nicke.) Chromic manganous sulphate, Cr 2 (SO 4 ) 3 , 3MnSO 4 . (Etard, C. R. 86. 1402.) Chromic manganic sulphate, Cr 2 (SO 4 ) 3 , Mn 2 (S0 4 ) 3 . Insol. in H 2 O. (Etard, C. R. 86. 1399.) Cr 2 (SO 4 )3. Mn 2 (SO 4 ) 3 , 2H 2 SO 4 . SI. deli- quescent. Sol. in H 2 O with decomp. (Etard.) Chromic nickel sulphate, Cr 2 (SO 4 ) 3 , NiS0 4 , 2H 2 SO 4 +3H 2 O. Insol. in H 2 O, but gradually decomp. there- by. (Etard, C. R. 87. 602.) Chromous potassium sulphate, CrSO 4 , K 2 SO 4 +6H 2 O. Sol. in H 2 O; less sol. in alcohol. (Peligot, A. ch. (3) 12. 546.) Chromic potassium sulphate, K 2 Cr 2 (SO 4 ) 4 . Anhydrous, a. Sol. in H 2 O when not heated over 350. /8. Insol. in cold H 2 O and cold acids. When ignited is insert, in hot H 2 O and acids, except slightly in boiling cone. H 2 SO 4 . (Fischer.) +2H 2 O (?) . Insol. in cold H 2 O or dil. acids. Sol. by long boiling with H 2 O, and more quickly when HC1 is added. (Hertwig.) +4H 2 0. Is potassium chromosulphate, which see. +24H 2 O. Chrome-alum. Violet modifica- tion. Efflorescent at 29. Sol. in 6-7 pts. cold H 2 O. When the H 2 O solution is heated to 60-70 it is partially decomp. into a green modification, which is more sol. in H 2 O. The green modification on standing in H 2 solu- tion is very slowly converted back into violet modification. The green modification may also be formed by heating dry salt to 100 , at which temp, it melts in its crystal H 2 O. When all crystal H 2 O has been expelled at 300-350, it still dissolves in hot H 2 O, but when heated above 350 it becomes insol. in H 2 O. (Lowel, A. ch. (3) 44. 313.) 125.1 g. anhydrous, or 243.9 g. hydrated salt, or 0.441 g. mols. anhydrous salt are sol. in 1 -1. H 2 O at 25. (Locke, Am. Ch. J. 1901, 26. 175.) Melts in crystal H 2 O at 89. (Tilden, Chem. Soc. 45. 409.) Sp. gr. of aqueous solution of violet modi- fication at 15 containing:" 5 10 15% K 2 Cr 2 (S0 4 ) 4 +24H 2 0. 1.02725 1.05500 1.08350 Sp. gr. of sat. solution at 15 = 1.0985. Sp. gr. of aqueous solution of green modi- fication at 15 containing: 10 20 30%K 2 Cr 2 (SO 4 ) 4 +24H 2 O, 1.050 1.103 1.161 40 50 60% K 2 Cr 2 (S0 4 ) 4 +24H 2 0, 1.225 1.295 1.371 70 80 90%K 2 Cr 2 (S0 4 ) 4 +24H 2 0. 1.453 1.541 1.635 (Gerlach, Z. anal. 28. 497.) Sp. gr. of chrome-alum solutions at 15 containing: 5 10 15 20 25 %salt, 1.0174 1.0342 1.0524 1.0746 1.1004 30 35 40 45 50 % salt, 1.1274 1.1572 1.1896 1.2352 1.2894 55 60 65 70 % salt. 1.3704 1.4566 1.5462 1.6362 (Franz, J. pr. (2) 5. 298.) Insol. in alcohol. 3K 2 SO 4 , Cr 2 (SO 4 ) 3 . Insol. in H 2 O, acids, or dil alkalies. Decomp. by boiling with cone. KOH+Aq. (Wernicke, Pogg. 159. 576.) Chromic rubidium sulphate, Rb 2 Cr 2 (S0 4 ) 4 + 24H 2 O. Sol. in H 2 O. (Petersson.) SULPHATE, COBALTOUS 959 Solubility in H 2 O. Solubility in 100 pts. H 2 O at t, using CoSO 4 + 7H 2 O. rp G. anhydrous G. mols. of anhy- salt per I. drous salt per 1. t Pt8. t Pts. Pts. CoSO4 CoSO4 t CoSO4 25 25 7 079 30 31.7 0.0$6 24.6 36 43.5 72 65.0 35 41.1 0.128 1 25.0 37 44.0 73 65.6 40 59.7 0.181 2 25.5 O/j f\ 38 or* 44.6 A t O 74 *7C 66.2 nr* r> Melts in crystal H 2 O at 107. 4 26.0 26.5 o9 40 45.2 45.8 75 76 66.8 67.4 (Locke, Am. Ch. J. 1901, 26. 180.) 5 6 27.0 27.5 41 42 46.4 47.0 77 78 68.0 68.6 7 28.0 43 47.6 79 69.2 Chromic sodium sulphate, Na 2 Cr 2 (SO 4 ) 4 + 8 28.5 44 48.2 80 69.8 10H 2 O. 9 29.0 45 48.8 81 70.4 Is sodium chromosulphate, which see. +24H 2 O. More efflorescent than K or NH 4 salt. Sol. in H 2 O, and properties re- semble the corresponding K salt. Cr 2 (SO 4 ) 3 , 3Na 2 SO 4 . Resembles the corre- sponding K salt. 10 11 12 13 14 15 16 29.5 30.0 30.5 31.0 31.5 32.0 32.5 46 47 48 49 50 51 52 49.4 50.0 50.6 51.2 51.8 52.4 53.0 82 83 84 85 86 87 88 71.0 71.6 72.2 72.8 73.4 74.0 74.6 17 33.0 53 53.6 89 75.2 Chromic thallous sulphate, Tl 2 Cr 2 (SO 4 ) 4 + 18 33.5 54 54.2 90 75.9 24H 2 0. 19 34.0 55 54.8 91 76.6 0.212 mols. of anhydrous salt are sol. in 1 1. H 2 O at 25. 1 1. H 2 O dissolves 104.8 g. of anhydrous or 163.8 g. hydrated salt at 25. Melts in crystal H 2 O at 92. (Locke, Am. Ch. J. 1901, 26. 175.) 20 21 22 23 24 34.5 35.1 35.6 36.2 36.8 56 57 58 59 60 55.4 56.0 56.6 57.2 57.8 92 93 94 95 96 . 77.2 77.9 78.6 79.2 79.9 25 37.4 61 58.4 97 80.6 26 38.0 62 59.0 98 81.3 Chromic sulphate chloride, Cr 2 (SO 4 ) 2 Cl 2 + 27 38.5 63 59.6 99 81.9 2H 2 0. 28 39.1 64 60.2 100 82.6 Slightly hydroscopic. Sol. inH 2 O. (Schiff, A. 124. 176.) 29 30 39.6 40.2 65 66 60.8 61.4 101 102 83.3 83.9 [CrSO 4 , 5H 2 O]C1. Sol. in H 2 O. (Wein- land, Z. anorg. 1908, 58. 176.) 31 32 33 40.7 41.3 41.8 67 68 69 62.0 62.6 63.2 103 104 105 84.6 85.3 86.0 34 42.4 70 63.8 106 86.7 Chromyl sulphate, (CrO 2 )SO 4 . 35 42.9 71 64.4 106.4 86.9 Decomp. by H 2 O. (Pictet and Karl, Bull. Soc. 1908, (4) 3. 1114.) (Mulder, calculated from his own and Tob- Cobaltous sulphate, basic. Ppt. Insol. in H 2 O. (Berzelius.) 6CoO, SO 3 + 10H 2 O. (Athanasesco, C. R. 103. 271.) 5CoO, SO 3 +4H 2 O. Ppt. Very si. sol. in H 2 O. (Habermann, M. Ch. 5. 432.) Cobaltous sulphate, CoS0 4 . 100 pts. H 2 O dissolve at: 3 10 20 24 29 26.2 30.5 36.4 38.9 40 pts. anhydrous salt, 35 44 50 60 70 46.3 50.4 55.2 60.4 65.7 pts. anhydrous salt. (Tobler, A. 96. 193.) 100 pts. H 2 O at 11-14 dissolve 23.88 pts. anhydrous salt. (v. Hauer, J. pr. 103. 114.) ler's determinations, Scheik. Verhandel. 1864. 68.) 100 g. H 2 O dissolve 37.8 g. CoSO 4 at 25. (Wagner, Z. phys. Ch. 1910, 71. 430.) See also +7H 2 O. Sp. gr. of CoSO 4 +Aq at t. S = pts. CoSO 4 in 100 pts. solution; Si = mols. CoSO 4 in 100 mols. of solution. S Si Sp. gr. 6.8910 5.8140 4.7095 3.5792 2.4273 1.2099 0.852 0.711 0.570 0.429 0.288 0.141 .0765 .0641 .0517 .0392 .0263 1.0131 (Charpy, A. ch. (6) 29. 26.) 960 SULPHATE, COBALTOCOBALTIC Sp. gr. of CoSO 4 +Aq at room temp, con- taining i 7.239 14.156 21.167% CoSO 4 . 1.0860 1.1591 1.2398 (Wagner, W. Ann. 1883, 18. 269.) Sp. gr. of CoSO 4 +Aq at 25. t g. CoS04 t g. CoS0 4 t g. CoSO4 5 10 25.53 28.05 30.55 15 20 25 33.045 36.21 39.35 30 35 40 42.26 45.80 48.85 Concentration of CoSC>4 +Aq Sp. gr. 1-normal V 2 - " V<- " Vs- " 1.0750 1.0383 1.0193 1.0110 (Koppel, Z. phys. Ch. 1905, 52. 395.) M.-pt. of CoSO 4 +7H 2 O =96-98. (Tilden, Chem. Soc. 46. 409.) (Wagner, Z. phys. Ch. 1890, 5. 37.) 100 pts. sat. solution of CoSO 4 and CuSO 4 contain 22.70 pts. of the two salts. Solubility of CoSO 4 , 7H 2 O+Na 2 SO 4 , 10H 2 O in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 and grams Na 2 SO 4 . t grams CoSCU grams Na2SO4 5 10 21.855 23.94 25.41 10.07 13.155 16.665 (Koppel, Z. phys. Ch. 1905, 52. 396.) See also under CoNa 2 (SO 4 ) 2 +4H 2 O. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) HC 2 H 3 O 2 ppts. it completely from CoS0 4 + Aq. (Persoz.) 100 pts. absolute methyl alcohol dissolve 1.04 pts. CoSO 4 at 18. (de Bruyn, Z. phys. Ch. 10. 784.) 100 pts. absolute methyl alcohol dissolve 54.5 pts. CoSO 4 +7H 2 O at 18; 100 pts. ab- solute methyl alcohol dissolve 42.8 pts. CoSO +7H 2 O at 3; 100 pts. 93.5% methyl alcohol dissolve 13.3 pts. CoSO 4 +7H 2 O at 3;100 pts. 50% methyl alcohol dissolve 1.8 pts. CoSO 4 +7H 2 O at 3. 100 pts. absolute ethyl alcohol dissolve 2.5 pts. CoSO 4 +7H 2 O at 3. (de Bruyn, Z. phys. Ch. 10. 786.) 100 g. solution in glycol contain 2.5 g. CoSO 4 . (de Coninck, Bull. Ac. Belg. 1905. 359.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) Insol. in ethyl acetate. (Naumann, B, 1904, 37. 3602.) + H 2 O. SI. sol. in cold, and only verv slowly sol. in hot H 2 O. (Vortmann, B. 15, 1888.) +4H 2 O. (Frohde, Arch. Pharm. (2) 127. 92.) +6H 2 O. (Marignac.) +7H 2 O. Sol. in 24 pts. cold H 2 O. Insol. in alcohol. (Persoz.) Solubility of CoSO 4 +7H 2 O in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 . Cobaltocobaltic sulphate, Co 2 O 3 , 6CoO, SO 3 + 15H 2 O. Precipitate. Insol. in boiling CoSO 4 +Aq or NH 4 OH+Aq. (Gentele, J. pr. 69. 130.) Cobaltic sulphate, Co 2 (SO 4 ) 3 +18H 2 O. Sol. in H 2 O with immediate decomp. and liberation of O. Sol. in dil. H 2 SO 4 +Aq with- out immediate decomp. Sol. in cone. HNO 3 , H 2 SO 4 , or HC 2 H 3 O 2 +Aq. (Marshall, Chem. Soc. 59. 760.) Cobaltous cupric sulphate, 2CoS0 4 , CuSO 4 -f 21H 2 0. Easily sol. in H 2 O. (v. Hauer, Pogg. 125. 637.) +36H 2 O. (Liebig.) 2CoSO 4 , 2CuSO 4 , H 2 SO 4 . (Etard.) Cobaltous cupric magnesium potassium zinc sulphate, CoSO 4 , CuSO 4 , MgSO 4 , 4K 2 SO 4 , ZnSO 4 +24H 2 O (?). Sol. inHsO. (Vohl.) Cobaltous cupric potassium sulphate, CoSO 4 , CuS0 4 , 2K 2 SO 4 +12H 2 O (?). Sol. inHaO. (Vohl.) Does not exist. (Aston and Pickering, Chem. Soc. 49. 123.) Cobaltous hydrazine sulphate, CoH 2 (SO 4 ) 2 , 2N 2 H 4 . 1 pt. is sol. in 305.16 pts. H 2 O at 12. Sol. in HNO 3 with decomp. Insol. in HC1. (Curtius, J. pr. 1894, (2) 50. 331.) Cobaltous iron (ferrous) potassium sulphate, CoSO,, Fe 2 SO 4 , 2K 2 SO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) 2CoS0 4 , 2FeSO 4 , H 2 SO 4 . (Etard.) Cobaltous magnesium sulphate, 3CoSO 4 , MgS0 4 +28H 2 O. Easily sol. in H 2 O. (Winkelblech.) SULPHATE HYDRAZINE, COBALTOUS 961 Cobaltous magnesium potassium sulphate CoS0 4 , MgS0 4 , K 2 S0 4 +12H 2 0. Sol. in H 2 O. (Vohl, A. 94. 57.) Does not exist. (Aston and Pickering 'Chem. Soc. 49. 123.) Cobaltous manganous potassium sulphate CoSO 4 , MnS0 4 , 2K 2 SO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Cobaltous nickel potassium sulphate, CoS0 4 , NiS0 4 , 2K 2 S0 4 +12H 2 0. Sol. in H 2 O. (Vohl, A. 94. 57.) Does not exist. (Thomson, Rep. Brit. Assn. Adv. Sci. 1877. 209.) Cobaltous potassium sulphate, CoSO 4 , K 2 SO< +6H 2 O. Less sol. in H 2 O than CoSO 4 . 100 pts. H 2 O dissolve at: 12 15 20 25 19.1 30 32.5 39.4 45.3 pts. anhydrous salt, 30 35 40 49 51.9 55.4 64.6 81.3 pts. anhydrous salt. (Tobler, A. 96. 126.) 100 pts. saturated solution contain at: 20 40 60 80 14 19.5 24.4 31.8 pts. anhydrous salt. (v. Uauer, J. pr. 74.' 433.) 1 1. H 2 O dissolves 128.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Cobaltic potassium sulphate, K 2 Co 2 (SO 4 ) 4 + 24H 2 O. Sol. in H 2 O with decomp. (Marshall, Chem. Soc. 69. 760.) Cobaltous potassium zinc sulphate, CoS0 4 , 2K 2 S0 4 , ZnSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Cobaltous rubidium sulphate, CoSO 4 , Rb 2 SO 4 +6H 2 O. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 92.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Cobaltic rubidium sulphate, Rb 2 Co 2 (SO 4 ) 2 + 24H 2 0. Decomp. by H 2 O. Sol. in dil. HC1 and ;H 2 SO 4 . Decomp. by cone. HC1 or H 2 SO 4 . by 1,J. (Howe and O'Neal, J. Am. Chem. Soc. 1898, 20. 762.) Melts in crystal H 2 O at 47. (Locke, Am. Ch. J. 1901, 26. 183.) Cobaltous sodium sulphate, CoNa 2 (SO 4 ) 2 + 4H 2 0. Solubility of CoNa 2 (SO 4 ) 2 , 4H 2 O in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 and grams Na 2 SO 4 . t g. CoSO4 g. Na 2 S04 20 25 30 35 40 26.65 25.365 23.13 22.55 20.975 24.91 23.325 21.61 20.85 20.055 (Koppel, Z. phys. Ch. 1905, 62. 397.) Solubility of CoNa 2 (SO 4 ) 2 , 4H 2 O+CoSO 4 , 7H 2 O in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 and grams Na 2 SO 4 . 18.5 20 25 28.61 29.42 30.73 23.82 23.015 20.575 CoSO4 32.695 34.065 35.01 Na 2 SO< 18.17 15.61 13.715 (Koppel, Z. phys. Ch. 1905, 62. 397.) Solubility of CoNa 2 (SO 4 ) 2 , 4H 2 O+NaSO 4 , 10H 2 O in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 and grams Na 2 SO 4 . 18.5 20 25 30 g. CcSO4 25.50 23.18 16.07 9.20 25.65 27.26 35.18 43.74 (Koppel.) Solubility of CoNa 2 (SO 4 ), 4H 2 O+Na 2 SO 4 (anhydrous) in H 2 O at t. 100 g. H 2 O dissolve grams CoSO 4 and grams Na 2 SO 4 . 35 40 g. CoS04 7.204 7.456 g. Na 2 S04 50.79 50.095 (Koppel.) See also CoSO 4 +Na 2 S0 4 under CoSO 4 . Cobaltous zinc sulphate. Efflorescent. Decomp. on air. (Link, Crell. Ann. 1790, 1. 32.) lobaltous sulphate ammonia, CoS0 4 , 6NH. Sol. hi H 2 O with separation of ppt. (Rose, 'ogg. 20. 152.) Very easily sol. in NH 4 OH+ Decomp. by alcohol. Cobaltous sulphate hydrazine, CoSO 4 , 3NaH 4 . Insol. in H 2 O. Decomp. by boiling with I 2 O. Very sol. in dil. acids and NH 4 -fAq. Franzen, Z. anorg. 1908, 60. 272.) 962 SULPHATE HYDROXYLAMINE, COBALTOUS Cobaltous sulphate hydroxylamine. CoSO 4 , NH 2 OH+2H 2 0. Insol. in cold; sol. in hot H 2 O with decomp. (Feldt, B. 1894, 27. 403.) Columbium sulphate. Sol. in H 2 O. (Blomstrand.) Cuprous sulphate, Cu 2 SO 4 . Decomp. by H 2 O. Sol. in cone. HC1, in ammonia and si. sol. in glacial acetic acid. (Recoura, C. R. 1909, 148. 1107.) Cupric sulphate, basic, lOCuO, SO 3 . (Pickering, Chem. Soc. 1907, 91. 1984.) 8CuO, SO 3 -H2H 2 O. Ppt. (Kane, A. ch. 72. 269.) 5CuO, SO 3 +6H 2 O. Ppt. (Smith, Phil. Mag. J. 23. 196.) 4CuO, SO 3 +3H 2 O. Insol. in H 2 O. (Rou- cher, J. Pharm. (3) 37. 50.) Min. Brochantite. Sol. in acids and NH 4 OH+Aq. +3KH 2 O. Insol. in H 2 O. Easily sol. in dil. acids, even HC 2 H 3 O 2 +Aq. SI. sol. in CuSO 4 +Aq. Insol. in NaC 2 H 3 2 +Aq. (Cas- selmann, Z. anal. 4. 24.) +4H 2 O. Insol. in H 2 0. (Proust.) Sol. in (NH 4 ) 2 SO 4 +Aq, and more easily in NH 4 C1, and NH 4 NO 3 +Aq. (Lea.) 1 1. cold H 2 O dissolves 0.017 g. (Pickering, C. N. 1883, 47. 182.) +5H 2 O. Min. Langite. +16H 2 O. (Andre, C. R. 100. 1138.) 7CuO, 2SO 3 +5H 2 O. (Reindel, J. pr. 100. 1.) +6H 2 O. Wholly insol. in cold or hot H 2 O. (Habermann, M. Ch. 5. 432.) +7H 2 O. Insol. in H 2 O; easily sol. in acids. Insol. in boiling CuSO 4 +Aq. (Reindel.) 3CuO, SO 3 + 1 KH 2 O . Insol. in H 2 O ; easily sol. in acids. (Steinmann, B. 16. 1412.) +2H 2 O. Insol. in H 2 O; sol. in dil. H 2 SO 4 + Aq. (Shenstone, Chem. Soc. 47. 375.) +2^H 2 O. (Reindel, J. pr. 102. 204.) +4H 2 O. Insol. in H 2 O. (Grimbert and Barre, J. Pharm. (5) 21. 414.) 5CuO, 2SO 3 +3H 2 O. (Wibel, Dissert. 1864.) HCuO, 4SO 3 +8H 2 O. (Clowes, C. N. 1898, 78. 155.) 8CuO, 3SO 3 +10H 2 O. (Marchlewski and Sachs, Z. anorg. 1892, 1. 405.) 7CuO, 3SO 3 +12H 2 O. (fitard, C. R. 1887, 104. 1615.) 5CuO, 2S0 3 +5H 2 O. (Sabatier, Gm. K. 6. 1, 839.) 6H 2 O. Min. Arnimite. (Weisbach, J. B. 1886. 2253.) 2CuO, SO 3 . Decomp. by cold H 2 O into Cu'SO 4 and 4CuO, SO 3 . (Roucher.) Insol. in H 2 O. Decomp. by hot H 2 0. ,Sol. in dil. acids. (Pozzi-Escot, Bull. Soc. .1913 (4) 13. 816.) According to Pickering (C. N. 47. 181) only 3CuO, SO 3 +23^H 2 O and 4CuO, SO 3 +4H 2 O are true chemical compounds. There is at 25 no definite basic sulphate of copper, all the basic sulphates being solid solutions. The solutions in contact with these basic sulphates contain S0 3 and CuO in equivalent quantities and are all si. acid in reaction. (Bell, J. phys. Chem. 1908, 12. 179.) Cupric sulphate, CuSO 4 . Anhydrous. Absorbs H 2 O from the air. Combines with, and dissolves in H 2 O with great evolution of heat. +HoO. Permanent. Sol. inH 2 0. (Etard, C. R. 87. 602.) +2H 2 O (?). (Storer's Diet.) +3H 2 O. (Etard, C. R. 104. 1614.) Does not exist. (Cross, C. N. 49. 220.) See Foote, p. 965. +5H 2 O. Superficially efflorescent in dry Sol. in 2.34 pts. H 2 O at 18, and sat. solution has sp. gr. 1.2147. (Schiflf, A. 109. 326.) 100 pts. CuSO 4 +Aq sat. at b. pt., 102.2, contain 45 pts. of the dry salt, or 100 pts. H 2 O at 102.2 dissolve 81.82 pts. CuSO4. (Griffiths, Q. J. Sci. 18. 90.) Sol. in less than 4 pts. H 2 O at ord. temp., and much more sol. in boiling H 2 O. (Bergmann.) Sol. in 4 pts. cold, and 2 pts. hot H2O. (Schubarth.) 100 pts. H 2 O dissolve 33.103 pts. CuSO4+5H 2 O at 15, and solution has sp. gr. =1.1859. (Michel and Krafft, A. ch. (3) 41. 478.) CuSO4+Aq sat. at 8 has 1.17 sp. gr. (Anthon, A. 24. 210.) . 1 pt. CuSO4+5H 2 O dissolves at: 4 19 31 37.5 50 in 3.32 2.71 1.84 1.7 1.14 pts. H 2 O, 62.5 C in 1.27 104 . 0.47 pts. H 2 O. (Brandes and Gruner, 1826.) 75 1.07 87.5 0.75 100 0.55 Sol. at 17.5 in 2.412 pts. H 2 O. (Karsten.) 100 pts. H 2 CTdissolve at: 9 10 ' 20 30 31.61 36.95 42.31 48.81 pts. CuSO 4 +5H 2 O, 40 50 60 70 56.90 65.83 77.39 94.60 pts. CuSO 4 +5H 2 O, 80 90 100 118.03 156.44 203.32 pts. CuSO 4 +5H 2 O (Poggiale, A. ch. (3) 8. 463.) 100 pts. H 2 O dissolve at: 20 35 54 17 24.3 28.6 36.1 pts. anhydrous CuS0 4 (Tobler, A. 96. 193.) 100 pts. CuSO 4 +Aq sat. at 11-14 cqntai 16.23 pts. anhydrous CuSO 4 . (v. Hauer, , pr. 103. 114.) 100 pts. H 2 O dissolve 15.107 pts. CuSO 4 1 0. (Pfaff, A. 99. 224.) SULPHATE, CUPRIC 963 100 pts. H 2 O dissolve pts. CuSO 4 at t. If solubilitv S = pts. anhydrous CuSO 4 in 100 pts. solution, S = 11.6+0.2614t from -2 to 55; S = 26.5+0.3700t from 55 to 105; S=45.0.-0.0293t from 105 to 190. (Etard, C. R. 104. 1614.) Solubility decreases above 120, owing to formation of basic salt. (Tilden and Shen- stone, Phil. Trans. 1884. 23.) 100 ccm. H 2 O dissolve 14.92 g. CuSO 4 at 0. (Engel, C. B. 102. 113.) 100 ccm. H 2 O dissolve 22.28-22.30 g. CuSO 4 at 20. (Trevor, Z. phys. Ch. 7. 468.) t Pts. CuSO4 17.9 24.1 14.99 20.16 22.37 (Diacon, J. B. 1866. 61.) 100 pts. H 2 O dissolve pts. CuSO 4 at t. 100 pts. H 2 O dissolve pts. CuSO 4 at t. 4-O Pts. Pts. Pts. t CuSO4 t CuSO 4 t CuS0 4 14.15 40 28.50 80 54.53 10 17.50 50 33.31 90 64.35 20 20.53 60 39.01 100 75.22 30 24.34 70 45.74 (Patrick and Aubert, Transactions of Kansas Acad. of Sci. 1874. 19.) Solubility in 100 pts. H 2 O a-t t. J.Q Pts. Pts. Pts. t CuSO4 t CuSO4 t CuSO 4 15.5 35 27.5 70 45.7 1 16.3 36 27.9 71 46.4 2 16.6 37 28.3 72 47.2 3 16.9 38 28.7 73 47.9 4 17.2 39 29.1 74 48.7 5 17.5 40 29.5 75 49.5 6 17.8 41 29.9 76 50.3 7 18.1 42 30.3 77 51.1 8 18.4 43 30.7 78 51.9 9 18.7 44 31.1 79 52.7 10 19.1 45 31.5 80 53.5 11 19.3 46 31.9 81 54.3 12 19.6 47 32.3 82 55.1 13 19.9 48 32.7 83 55.9 14 20.2 49 33.2 84 56.8 15 20.5 50 33.6 85 57.8 16 20.8 51 34.1 86 58.7 17 21.1 52 34.5 87 59.7 18 21.4 53 35.0 88 60.7 19 21.7 54 35.5 89 61.7 20 22.0 55 36.0 90 62.7 21 22.3 56 36.6 91 63.7 22 22.6 57 37.2 92 64.8 23 23.0 58 37.8 93 65.8 24 23.3 59 38.4 94 66.9 25 23.7 60 39.0 95 68.0 26 24.0 61 39.6 96 69.1 27 24.4 62 40.2 97 70.2 28 24.7 63 40.9 98 71.3 29 25.1 64 41.5 99 72.4 30 25.5 65 42.2 100 73.5 31 25.9 66 42.9 101 74.6 32 26.3 67 43.6 102 75.7 33 26.7 68 44.3 103 76.8 34 27.1 69 45.0 104 77.95 (Mulder, Scheik. Verhandel. 1864. 79.) Sat. CuSO 4 + Aq contains % CuSO 4 at t. t % CuSO4 t % CuS04 1 12.1 88 38.8 +7 14.1 89 38.9 9 14.5 94 41.8 18 16.9 96 41.9 20 17.2 97 42.0 20 17.4 100 43.6 35 21.3 108 43.8 39 21.8 110 43.4 45 23.9 116 43.8 54 26.9 116 44.0 54 26.6 120 44.8 61 28.8 132 44.8 63 29.1 133 44.7 65 30.0 143 45.0 70 31.6 160 44.2 71.7 32.6 165 44.5 76 34.5 179 42.9 80 36.6 189 42.2 86 37.8 (Etard, A. ch. 1894, (7) 2. 554.) Solubility in H 2 O at t. t g. CuSO 4 per 100 g. H 2 O 10 15 20 25 14.15 17.68 19.25 20.78 22.29 (by interpolation) (Cohen, Z. phys. Ch. 1907, 60. 713.) 1.399 mol. are sol. in 1 1. H 2 O at 25. (Herz, Z. anorg. 1910, 67. 366.) 100 g. CuS0 4 +Aq sat. at 30 contain 20.32 anhyd. CuSO 4 . (Schreinemakers, Z. phys. Ch. 1910, 71. 110.) +7H 2 O. (Boisbaudran, C. R. 66. 1249.) +6H 2 O. (Boisbaudran, C. R. 66. 487.) 964 SULPHATE, CUPRIC Sp. gr. of CuSO 4 +Aq at CuSO 4 +5H 2 O. 18. % % Sp. gr. % Sp. gr. % Sp. gr. 1 .0063 11 1.0716 21 1 . 1427 2 .0126 12 1.0785 22 1.1501 3 .0190 13 1.0854 23 1 . 1585 4 .0254 14 .0923 24 1 . 1659 5 .0319 15 .0993 25 1.1738 6 .0384 16 .1063 26 1.1817 7 .0450 17 .1135 27 1 . 1898 8 .0516 18 .1208 28 1 . 1980 9 .0582 19 .1281 29 1.2063 10 .0649 20 .1354 30 1.2146 (Schiff, calculated by Gerlach, Z. anal. 8. 288.) Sp. gr. of CuSO 4 +Aq at 23.9. a = no. of Y 2 mols. in grms. dissolved in 1000 grms. H 2 O; b = sp. gr. if a is CuSO 4 = 5H 2 O (Y 2 mol. wt. = 125); c = sp. gr. if a is CuSO 4 (3/ 2 mol. wt.=80). a b c 1 2 3 1.076 1.142 1.200 1.080 1.154 1.225 (Favre and Valson, C. R. 79. 968.) Sp. gr. of CuSO 4 +Aq at 15. % = %CuS0 4 +5H 2 0. % Sp. gr. % Sp. gr. 5 1.0335 20 1 . 1443 10 1.0688 25 1 . 1848 15 1 . 1060 mother liquor 1.185 (Gerlach, Dingl. 181. 131.) Sp. gr. of CuSO 4 +Aq at 18 C % CuSO4 Sp. gr. % CuSO4. Sp. gr. 5 10 1.0513 1 . 1073 15 17.5 1 . 1675 1.2003 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of CuSO 4 +Aq at 0. S=pts. CuSO 4 in 100 pts. solution. s Sp. gr. S Sp. gr. 11.9315 9.8159 7.5474 1.1371 1.1108 1.0833 5.2181 2.6460 1.0578 1.0290 (Charpy, A. ch. (6) 29. 26.) >. gr. of CuSO 4 +Aq at room temp. % CuSO 4 Sp. gr. 6.79 12.57 17.49 1.055 1.1151 1.1635 (Wagner, W. Ann. 1883, 18. 265.) ' Sp. gr. of CuSO 4 +Aq at 25. Concentration of Cu SC>4 . +Aq 1-normal Vr- " Vr- " Vr- " Sp. gr. 1.0790 1.0402 1.0205 1.0103 1.0050 (Wagner, Z. phys. Ch. 1890, 6. 38.) B.-pt. CuSO 4 +Aq containing pts. CuSO 4 to 100 pts. H 2 O. B.-pt. Pts. CuSO4 B.-pt. Pts. CuSCU 100.5 21.3 103.0 69.0' 101.0 36.9 103 . 5 74.9 101.5 48.0 104.0 80.1 102.0 56.2 104.2 82.2 102.5 63.0 (Gerlach, Z. anal. 26. 434.) Sat. CuSO 4 +Aq boils at 102.2, and con- tains 81.8 pts. CuSO 4 to 100 pts. H 2 O. (Griffiths.) Crust forms at 102.3, and solution contains 60.3 pts. CuSO 4 to 100 pts. H 2 O; highest temp, observed, 104.8. (Gerlach, Z, anal. 26. 426.) Sol. in HCl+Aq, causing a^ reduction of temperature of about 17. Very si. sol. in cone. H 2 SO 4 . (Schulz.) Solubility in H 2 SO 4 +Aq at 0. G. per 100 g. H 2 O Sp. gr. H 2 SO4 CuS04 0.00 14.85 1.144 2.03 14.29 1.143 7.16 15.65 1.158 15.20 9.90 1.170 26.57 6.43 1.195 27.57 6.19 1.211 35.2 3.99 1.224 (Engel, C. R. 1887, 104. 507.) SULPHATE, CUPRIC 965 Solubility in H 2 SO 4 +Aq at 25. Solubility of CuSO 4 in CuCl 2 +Aq at 30. Solution Solid phase % CuCh % CuSO4 Solid phase Sp. gr. % CuO % S0 3 6.58 15.68 25.67 39.48 42.47 43.25 43.95 20.32 13.62 8.93 4.77 3.21 2.90 1.14 CuS0 4 , 5H 2 it ee 1C CuSO 4 , 5H 2 O+CuCl 2 , 2H 2 O CuCl 2 , 2H 2 O (C .2142 .2248 .2593 .2934 .4061 .4256 i;4249 1.4516 1.4915 1.5124 1.5408 1.5643 1.6824 1.7752 1.8118 1.8266 9.17 5.91 3.39 1.82 1.32 1.38 1.02 0^38 0.368 0.109 0.105 0.15 0.07 9.26 15.90 23.09 28.75 39.74 41.29 41.04 43.63 47.82 49.07 51.46 53.51 62.14 68.34 72 .41 74.26 CuSO4 +5H 2 O CuS04+5H 2 Oand CuSO4+3H*O CuS04+3H 2 O C.uSO4+H 2 O CuSO4 (Schreinemakers, Arch. Ne'er. Sci. 1910, (2) 15. 117.) Solubility of CuSO 4 in LiCl+Aq at 25. Solid phase, CuSO 4 , 5H 2 O. (G. mols. per 1. of solution.) LiCl CuSO4 0.73 1.40 2.83 1.399 1.257 1.176 1.067 These results show that the hydrates of CuSO 4 which are stable at 25 are CuSO 4 + 5H 2 O,+3H 2 Oand+H 2 O. (Bell and Taber, J. phys. Chem. 1908, 12. 175.) (Herz, Z. anorg. 1910, 67. 366.) Solubility in H 2 SO 4 +Aq at 25. Solubility of CuS0 4 in KCl+Aq at 25. Solid phase, CuSO 4 +5H 2 O. (G. mols. per 1. of solution.) Solution contains Solid phase % CuSO % H 2 SO4 KCl CuSOi 18.47 12.62 5.92 3.25 2.63 2.59 2.83 2.83 2.84 2.70 2.19 2.11 2.15 0.95 0.17 0.15 0.19 0.44 0.42 0.40 0.19 none 11.14 25.53 36.77 42.15 47.66 49.00 49.20 49.29 50.23 54.78 55.84 55.60 61.79 77.93 83.29 85.46 85.72 85.81 86.04 92.70 CuSO 4 +5H 2 O 1 CuSO 4 +5H 2 O and CuSO 4 +3H 2 O CuSO 4 +3H 2 O U CuS 4 O 4 +H 2 O an< CuSO 4 +H 2 O CuSO 4 +H 2 O and CuSO 4 CuSO 4 0.56 1.17 2.34 1.496 1.561 1.819 (Herz.) Solubility of CuS0 4 in NaCl+Aq at 25. Solid phase, CuS0 4 +5H 2 O. (G. mols. per 1. of solution.) NaCl CuSOi 0.36 1.32 2.53 1.399 1.404 1.426 1.507 (Herz.) These results show that the hydrates of CuSO 4 which are stable at 25 are CuSO 4 + 5H 2 O,+3H 2 O and+H 2 O. (Foote, J. Am. Chem. Soc. 1915, 37. 290.) SI. sol. in sat. NH 4 Cl+Aq, with separation of a double sulphate. Solubility of CuS0 4 in RbCl+Aq at 25, containing 1.094 g. mols. per 1. = 1.568 g. mols. (Herz.) Slowly sol. in sat. KNO 3 +Aq, with sep- aration of a double sulphate. Very slowly sol. in sat. NaNO 3 -f Aq, with separation of a double sulphate. (Karsten, Berl. Abhandl. 1840. 10.) 966 SULPHATE, CUPRIC Solubility of CuSO 4 in (NH 4 ) 2 SO 4 +Aq at O c g. per 100 cc. g. par 100 cc. so ution solution 6 6 Sp. gr. g . Sp. gr. ^-N GO ^-v 02 i fc P B o 14.79 1.144 5.59 5.13 1.081 3.61 16.09 1.190 7.51 2.95 1.071 4.63 8.38 1.108 12.31 0.94 1.082 4.90 7.26 1.099 20.65 0.80 1.116 (Engel, C. R. 1886, 102. 114.) See also under (NH 4 ) 2 SO 4 . Solubility of CuSO 4 in Li 2 SO 4 +Aq at 30 C Composition of the solution . % by wt. % by wt. feoiid phase CuSO4 Li 2 S0 4 20.32 CuSO 4 , 5H 2 O 17.50 3.54. ft 16.10 6.08 u 13.55 11.94 (C 12.14 15.72 ft 11.04 17.92 it 10.05 20.55 CuSO 4 , 5H 2 O+Li 2 SO 4 , H 2 O 10.08 20.51 ii 10.07 20.49 << 6.41 22.23 Li 2 SO 4 , H 2 O 3.39 23.59 it 25.24 u (Schreinemakers, Z. phys. Ch. 1909, 66. 692.) Sol. in CuCl 2 , (NH 4 ) 2 S0 4 , NH 4 Cl+Aq at 30. (Schreinemakers, Z. phys. Ch. 1909, 69. 565.) Sol. in (NH 4 ) 2 SO 4 , Li 2 SO 4 +Aq. at 30. (Schreinemakers, Z. phys. Ch. 1909, 66. 694.) 100 pts. sat. solution of CuSO 4 and FeSO 4 contain 17.43 pts. of the salts at 11-14. (v. Hauer, J. pr. 103. 114.) 100 pts. H 2 O dissolye 10.85 pts. CuSO 4 , 17.47 pts. MgSO 4 , and 5.78 pts. Na 2 SO 4 at 0. (Diacon.) 100 pts. H 2 O dissolve 7.169 pts. CuSO 4 , 21.319 pts. MgSO 4 , and 6.330 pts. Na 2 SO 4 at 0. (Plaff.) Slowly and si. sol. in sat. MgSO 4 +Aq. (Karsten.) Solubility of CuSO 4 in H 2 O in presence of MgSO 4 . 100 pts. H 2 O dissolve No. CuS0 4 MgS0 4 No. 5 6 7 CuS0 4 MgSO 4 1 2 3 4 2.64 4.75 9.01 26.37 25.91 25.30 23.54 12.03 13.61 14.99 15.67 8.64 In 1, 2, and 3, MgSO 4 was in excess and given amt. CuSO 4 added; in 4, both CuSO 4 and MgSO 4 were in excess; in 5, 6, and 7, CuSO 4 was in excess. (Diacon, /. c.) 100 pts. sat. solution of CuSO 4 and MgSO 4 contain 28.58 pts. of the salts at 11-14. (v. Hauer, J. pr. 103. 114.) 100 .pts . sat. solution'of CuSO 4 and MnSO 4 contain 37.90 pts. of the salts at 11-14. (v. Hauer.) Solubility of CuSO 4 +MnSO 4 in H 2 O at 25. G. per 100 g. H 2 O 20.2 19.76 13.65 11.61 MnS0 4 3.69 31.52 39.41 G. per 100 g. H 2 O CuS0 4 9.39 6.47 3.01 0.0 MnSO< 46.77 53.39 58.93 61.83 (Stortenbecker, Z. phys. Ch. 1900, 34. 112.) 100 pts. sat. solution of CuSO 4 and NiSO 4 contain 31.03 pts. of the salts at 11-14. (v. Hauer.) Solubility of CuSO 4 +NiSO 4 in H 2 O. g. per 100 g. H 2 O Mol. % CuSCh t CuS0 4 NiS0 4 Solution Solid phase 35 9.62 583.9 1.57 0.35 41.66 484.4 7.69 2.12 75.39 553.5 11.66 4.77 106.40 506.5 16.92 6.52 172.0 483.8 25.6 13.88 186.9 468.8 27.90 /18.77 \94.91 67 20.04 729.3 2.65 0.93 66.01 706.2 8.31 2.86 88.08 501.6 13.55 3.92 147.94 675.0 16.39 6.66 249.9 747.8 24.46 23.32 (Fock, Z. Kryst. Min. 1897, 28. 387.) More easily sol. in sat. K 2 SO 4 +Aq than in Na 2 SO 4 or MgSO 4 +Aq, forming a double sulphate, which separates out. (Karsten.) K 2 SO 4 and CuSO 4 mutually displace each other in saturated solutions. (Riidorff, Pogg. 148. 555.) When K 2 S0 4 and CuSO 4 , both in excess, are dissolved in H 2 0, a maximum of solubilitj of 15.61 pts. of the two salts in 100 pts. H 2 C at 25 is reached in 30 minutes, after whicl the solubility decreases. This result is ob tained either by treating excess of the tw< salts with H 2 O at 25, or cooling solution of the two salts sat. at higher temp, to 25 e The salts are in the proportion of 5.2 pts K 2 SO 4 to 10.4 pts. CuSO 4 . If present in th same proportion as in their saturated soli; tions, 5.41 pts. K 2 SO 4 to 10.13 pts. CuSC would be required. SULPHATE, CUPRIC 967 If sat. solution of one salt is added to sat. solution of the other, K 2 Cu(S0 4 ) 2 +6H 2 O separates, as it is less sol. than either simple salt, until a state of equilibrium is reached, after which there is no separation, contrary to Riidorff (see above). (Trevor, Z. phys. Ch. 7. 486.) CuSO 4 +Na 2 SO 4 . Solubility of CuSO 4 in presence of Na 2 SO 4 at 0. 100 pts. H 2 O dissolve No. 1 2 3 4 CuSO 4 Na 2 S0 4 No. CuS04 Na.804 6.01 9.81 16.67 4.53 5.34 5.73 6.48 5 6 7 15.84 15.33 14.99 3.55 1.98 In 1, 2, and 3. Na 2 SO 4 was in excess and given amt. CuS0 4 added; in 4, both CuSO 4 and Na 2 SO 4 were in excess; in 5, 6, and 7, CuSO 4 was in excess and Na 2 SO 4 added. (Diacon, J. B. 1866. 61.) 100 pts. H 2 O dissolve 8.038 pts. CuSO 4 and 6.31 pts. Na 2 SO 4 at 0. (Pfaff, A. 99. 224.) 100 pts. H 2 dissolve 20.7 pts. CuSO 4 and 15.9 pts. Na 2 SO 4 at 15. (Riidorff, B. 6. 484.) Solubility of CuSO 4 +Na 2 SO 4 . 1. Solid phase, 3 mol. CuSO 4 +l mol. Na 2 SO 4 . 2. Solid phase, 1 mol. CuSO 4 +l mol. Na 2 S0 4 . 3. Solid phase, 1 mol. CuSO 4 +3 mol. Na 2 SO 4 . (G. in 100 g. H 2 0.) t i o 3 CuSOi Na 2 S0 4 CuS0 4 Na 2 S04 CuSO 4 Na 2 S0 4 12.55 15.92 22.70 15.25 10 15 30 50 19.75 20.69 22.03 32.37 12.49 15.88- 16.36 11.75 19.70 20.75 21.00 31.45 12.50 15.90 20.14 13.41 19.69 20.70 15.28 28.76 (Massol and Maldes, C. R. 1901, 133. 287.) Solubility of CuSO 4 , 5H 2 O+Na 2 SO 4 , 10H 2 O. t % CuS0 4 % NaiSOi 12 15 13.40 14.83 15.00 6.23 9.82 (Koppel, Z. phys. Ch. 1903, 42. 8.) See also under CuNa 2 (SO 4 ) 2 +6H 2 O. CuSO 4 +ZnSO 4 . Very slowly sol. in sat. ZnSO 4 +Aq, form- ing a double salt which separates. (Karsten.) 100 pts. sat. solution of CuSO 4 and ZnSO 4 contain .32.70 pts. of the salts at 11-14. hr. Hauer.) Solubility of CuSO 4 +ZnSO 4 in H 2 O at 25 C Mols. per 100 Mols. per 100 mols. H 2 O mols. H 2 O Cu Zn Cu Zn 2.28 0.82 5.03 1.83 2.08 0.51 5.59 1.41 3.60 0.30 5.56 1.19 5.01 0.00 6.42 1.86 3.36 1.19 5.01 1.22 4.45 0.51 5.59 1.01 4.72 0.267 5.77 0.00 5.94 (Stortenbecker, Z. phys. Ch. 1897, 22. 62.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 827.) Insol. in liquid CO 2 . (Biichner, Z.- phys. Ch. 1906, 54. 674.) 100 pts. of a sat. solution in 40% alcohol contains 0.25 pt. CuSO 4 +5H 2 O; 20% alcohol, 3.1 pts.; 10% alcohol, 13.3 pts. (Schiff, A. 118. 362.) Anhydrous CuSO 4 is sol. in absolute methyl alcohol, but insol. in absolute ethyl alcohol. CuSO 4 +:rH 2 O is insol. in methyl or ethyl alcohol. (Klepl, J. pr. (2) 25. 526.) 100 "pts. absolute methyl alcohol dissolve 1.05 pts. anhydrous QuSO 4 at 18. 100 pts. absolute methyl alcohol dissolve 15.6 pts. CuSO 4 +5H 2 O at 18; 100 pts. 93.5% methyl alcohol dissolve 0.93 pt. CuSO 4 +5H 2 O at 18; 100 pts. 50% methyl alcohol dissolve 0.4 pt. CuSO 4 +5H 2 O at 18; 100 pts. absolute methyl alcohol dis- solve 13.4 pts. CuSO 4 +5H 2 O at 3. 100 pts. absolute ethyl alcohol dissolve 1.1 pts. CuSO 4 +5H 2 O at 3. (de Bruyn, Z. phys. Ch. 10. 786.) Me ethyl alcohol dissolves 11.5% CuS0 4 -f 5H 2 O at 0. (Auger, C. R. 1906, 142. 1272.) Glacial acetic acid precipitates CuSO 4 com- pletely from CuSO 4 +Aq. 100 g. 95% formic acid dissolve 0.05 g. CuS0 4 +5H 2 O at 18.5. (Aschan, Ch. Ztg. 1913, 37. 1117.) Sol. in glycerine (Pelouze), picoline (Unver- dorben). 100 g. glycerine dissolve 36.3 g. CuSO 4 -f 5H 2 O at 15-16. (Ossendowski, Pharm. J. 1907, 79. 575.) 100 g. glycerine dissolve 30.0 g. CuSO 4 at 15.5. 100 g. solution of CuSO 4 in glycol contain 7.6 g. at 14.6. (de Coninck, Bull. Ac. Belg. 1905. 257.) Anhydrous CuSO 4 is insol. in acetone. (Krug and M'Elroy, J. Anal. Ch. 6. 184.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014); methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314); benzonitrile. (Naumann, B. 1914, 47. 1370.) Min. Chalcanthite. 968 SULPHATE, CUPRIC GLUCINUM Cupric glucinum sulphate, CuSO 4 , 4GlSO 4 -f 20H 2 O. Sol. hi H 2 O. (Klatzo, J. B. 1868. 205.) Does not exist. (Marignac, A. ch. (4) 30. 45.) 9CuSO 4 , G1SO 4 +50H 2 O. As above. Does not exist. (Marignac, I. c.) Cupric hydrazine sulphate, CuH 2 (SO 4 ) 2 , 2N 2 H 4 . 1 pt. is sol. in 1148 pts. H 2 at 10. Decomp. by acids. Sol. in JSiH 4 OH+Aq with decomp. (Cur- tius, J. pr. 1894, (2) 50. 331.) Cupric iron (ferrous) sulphate, CuSO 4 , FeSO 4 . Insol. in H 2 O. (Etard, C. R. 87. 602.) +2H 2 O. (fitard.) CuSO 4 , 2FeSO 4 +21H 2 O. Sol. in H 2 O. (v. Hauer.) CuSO 4 , 3FeSO 4 +28H 2 0. 100 pts. H 2 O dis- solve 75 pts. salt at 7. (Lefort.) 4CuS0 4 , FeSO 4 +34H 2 O. 100 pts. H 2 O at 15.5 dissolve 75.91 pts. (Thomson.) Cupric iron (ferric) sulphate, CuSO 4 , Fe 2 (S0 4 ) 3 +24H 2 0. Sol. in H 2 O. (Bastick.) Cupric iron (ferrous)' potassium sulphate, CuSO 4 FeSO 4 , 2K 2 SO 4 +12H 2 O. Sol. inH 2 0. (Vohl.) Cupric lead sulphate, CuO, PbO, SO 8 +H 2 O. Min. Linarite. 3CuO, 7PbO, 5SO 3 +5H 2 O. Min. Caledon- ite. Sol. in HNO 3 +Aq. Cupric magnesium sulphate, CuSO 4 , MgSO 4 +14H 2 O. Efflorescent. Sol. in H 2 O. (Vohl, A. 94. 57.) +2H 2 O. (Arrot, 1834.) CuSO 4 ,2MgSO 4 +21H 2 O. Sol.inH 2 O. (v. Hauer, Pogg. 125. 638.) CuSO 4 , 7MgSO 4 +56H 2 O. Sol. in H 2 O. (Schiff, A. 107. 64.) Cupric magnesium manganous potassium sulphate, CuSO 4 , MgSO 4 , MnSO 4 , 3K 2 S0 4 +18H 2 0. Sol. inH 2 O. (Vohl.) Cupric magnesium potassium sulphate, CuS0 4 , MgS0 4 , 2K 2 S0 4 +6H 2 0. Sol. in H 2 O. (Vohl, A. 94. 57.) Does not exist. (Aston and Pickering, Chem. Soc. 49. 123.) Cupric magnesium potassium zinc sulphate, CuSO 4 , MgO 4 , 3K 2 SO 4 , ZnSO 4 +18H 2 O. Sol. inH 2 O. (Vohl.) Cupric manganous sulphate, 5CuS0 4 , 2MnSO 4 +35H 2 O. Sol. in H 2 O. (Schauffele, J. B. 1852. 340.) 2CuSO 4 ,3MnSO 4 +25H 2 O. As above. (S.) CuSO 4 , MnSO 4 +H 2 O. (Etard, C. R. 87. 602.) Cupric manganous potassium sulphate, CuSO 4 , MnSO 4 , 2K 2 SO 4 +12H 2 O. Sol. inH 2 O. (Vohl.) Cupric nickel sulphate, CuS0 4 , NiSO 4 +3H 2 O. (Etard, C. R. 87. 602.) CuSO 4 , 2NiSO 4 +21H 2 0. Sol. in H 2 O. (v. Hauer.) + 18H 2 O. Sol. in H 2 O. (Boisbaudran, C. R. 66. 497.) 2CuSO 4 , 2NiSO 4 , 3H 2 SO 4 . (Etard.) Cupric nickel potassium sulphate, CuSO 4 , NiSO 4 , 2K 2 SO 4 -f 12H 2 O. Sol. in H 2 O. (Vohl.) Sol. in 4 pts. H 2 O; insol. in alcohol. (Bette.) 4CuSO 4 , K 2 SO 4 +4H 2 O. Very si. sol. in H 2 O. K 2 O, 4CuO, 4SO 3 +4H 2 O. Insol. in H 2 O, but decomp. by boiling H 2 O into 3CuO, SO 3 . Cupric potassium sulphate, K 2 Cu(S0 4 ) 2 -f- 6H 2 O. 100 pts. H 2 dissolve 66.666 pts. at 102.8. (Grif- fiths.) Much more sol. in hot than cold H2O. (Pierre.) Easily sol. in EUO; by bailing, de comp. into basic salt. (Perscz, A. ch. (3) 25. 272.) 100 pts. H 2 O dissolve 11.14 pts. anhydrous salt at 25. (Trevor, Z. phys. Ch. 7. 470.) 1 1. H 2 O dissolves 116.9 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) See also CuSO 4 +K 2 SO 4 . Min. Cyanochroite. Cupric potassium zinc sulphate, CuSO 4 , 2K 2 SO 4 , ZnSO 4 +12H 2 O. Sol. in H 2 0. (Vohl.) Cupric rubidium sulphate, CuSO 4 . Rb 2 SO 4 + 6H 2 0. Sol. in H 2 O. (Tutton.) 1 1. H 2 O dissolves 102.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Cupric sodium sulphate, basic, Na 2 S0 4 , Cu(OH) 2 , 3CuSO 4 +2H 2 O. Min. Natrochalcite. SI. sol. in H 2 O; easily sol. in acids. (Pa- lache and Warren, Am. J. Sci. 1908, (4) 26. 346.) SULPHATE CARBON OXIDE, CUPROUS 969 Cupric sodium sulphate, CuSO 4 , Na 2 SO 4 + 2H 2 O. Solubility of the pure double salt CuSO 4 , Na 2 SO 4 +2H 2 O. t 100 grams solution contain CuSO 4 grams Na2SO4 grams 17.7 19.5 23 30 40.15 14.34 14.54 14.36 14.07 13.73 13.34 12.90 12.76 12.37 12.26 (Koppel. Z. phys. Ch. 1903, 42. 8.) Solubility of the mixture of CuS0 4 , Na 2 SO 4 + H 2 O and CuSO 4 . t 100 g. solution contain CuSO4 grams Na2O4 grams 17.7 19.5 23 30 40.15 14.99 15.62 16.41 17.97 20.56 13.48? 12.06 11.35 9.95 8.00 (Koppel.) Solubility of the mixture of CuSO 4 , Na 2 SO 4 + 2H 2 O and Na 2 SO 4 . t 100 g. solution contain CuSCh grams NaeSCh grams 18 13.53 13.844 19.5 11.847 15.116 20 11.339 15.697 23 8.185 18.723 25 6.284 21.198 26 5.507 22.44 28 3.746 24.963 28.3 3.661 30 2.607 28^383 30.2 2.422 32.2 1.465 32^442 33.9 1.475 32.299 35.3 1.471 32.072 37.2 1.494 31.96 (Koppel.) Solubility of CuSO 4 , Na 2 SO 4 +2H 2 O in presence of varying amounts of Na 2 SO 4 . 100 g. solution contain t CuSO4 grams Na2SO4 grams 30 5.38 22.17 30 5.41 21.92 30.1 3.69 25.37 40.15 3.97 23.90 30 1.57 32.09 (Koppel.) Copper sulphate and sodium sulphate unite to form a double salt, CuSO 4 , Na 2 SO 4 + 2H 2 O, which is stable in the presence of the solution above 16.7. In the presence of copper sulphate the solubility of Na 2 S0 4 + 10H 2 O is greater than that of the pure salt. (Koppel.) Cupric thalloiis sulphate, CuSO 4 , T1 2 SO 4 + 6H 2 0. Decomp. by recrystallising from H 2 O. (Willm, A. ch. (4) 6. 55.) 1 1. H 2 O dissolves 81 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Cupric zinc sulphate, CuSO 4 , 3ZnS0 4 +28H 2 O Efflorescent. 100 pts. H 2 O dissolve 80 pts. salt at 8. Sol. in all proportions in boiling H 2 O. (Lefort.) CuSO 4 , 2ZnSO 4 +21H 2 O. (v. Hauer, Pogg. 125. 637.) CuSO* ZnSO 4 +12H 2 O. (Boisbaudran.) 2CuSO 4 , 2ZnSO 4 , H 2 SO 4 . (fitard.) Cuprous sulphate ammonia, Cu 2 SO 4 , 4NH 3 . Sol. in NH 4 OH+Aq; decomp. by pure H 2 O. (Pochard, C. R. 1903, 136. 504.) +H 2 O. Decomp. by H 2 O. (Foerster and Blankenburg, B. 1906, 39. 4434.) Cupric sulphate ammonia, basic, CuSO 4 , 3CuO, 2NH 3 +5H 2 O. Decomp. by hot H 2 O. (Pickering, Chem. Soc. 43. 336.) Cupric sulphate ammonia (Cuprammonium sulphate), CuSO 4 , NH 3 . Decomp. by H 2 O. (Kane.) Decomp. by H 2 O giving a basic sulphate. (Bouzat, C. R. 1902, 135. 535.) CuSO 4 , 2NH 3 [CuSO 4 , 2NH 3 +3H 2 O. (Mendelejeff, B. 3. 422.)]. Decomp. by ex- cess of H 2 O into CuSO 4 , 4NH 3 +H 2 O. Sol. in 1.5 pts. H 2 O, but decomp. by much H 2 O. Insol. in alco- hol. Insol. in cone. NH 4 OH+Aq. (Andre*, C. R. 100. 1138.) Sol. in small quantity of H 2 O; decomp. in dil. solution. (Bouzat.) 100 g. H 2 O dissolve 44.56 g. anhydrous comp. at 25. (Pudschies, Dissert.) 100 g. H 2 O dissolve 18.05 g. at 21-22. (Horn and Taylor, Am. Ch. J. 1904, 32. 268.) CuSO 4 , 5NH 3 . Completely sol. in H 2 O. (Rose, Pogg. 20. 150.) Sol. in small amt. of H 2 O; decomp. in dil. solution. Insol. in liquid NH 3 . (Bouzat, C. R. 1902, 135. 535.) Cuprous sulphate carbon monoxide, Cu 2 SO 4 , 2CO+H 2 0. Very unstable. (Joannis, C. R. 1903, 136. 615.) 970 SULPHATE ZINC OXIDE, CUPRIC Cupric sulphate zinc oxide, CuSO 4 , 2ZnO + 21H 2 0. (Larsen, Ch. Z. Report. 1896, 20. 317.) 2CuSO 4 , 3ZnO+12H 2 O. (Mailhe, A. ch. 1902, (7) 27. 169.) Didymium sulphate, basic, Di 2 O 3 , SO 3 = (DiO) 2 SO 4 . Insol. in cold or boiling H 2 O. (Marignac.) Slowly sol. in hot dil. HCl+Aq. Easily sol. in cone, acids. +8H 2 O. Precipitate. (Hermann.). Composition is 2Di 2 O 3/ , 3SO 3 +3H 2 O or Di 2 (SO 4 ) 3 +Di 2 O 6 H 6 . (Frerichs and Smith.) Composition is 5Di 2 O 3 , 3SO 3 +xH 2 O. (Cleve, B. 11. 910.) Didymium sulphate, Di 2 (SO 4 ) 3 . Anhydrous. By saturating cold H 2 O and warming the solution, the following results were obtained 100 pts. H 2 O dissolve at: 12 18 25 38 50 43.1 25.8 20.6 13.0 11.0 pts. Di 2 (S0 4 ) 3 . +6H 2 O. H 2 O dissolves this salt very slowly; 100 pts. H 2 O dissolve 13 pts. Di 2 (SO 4 ) 3 in 24 hours, and 16.4 pts. in 2 days. If solution is evap. in vacuo until Di 2 (SO 4 ) 3 + 8H 2 O separates out, 34 pts. Di 2 (SO 4 ) 3 remain dissolved in 100 pts. H 2 O. +5H 2 O. (Cleve.) +8H 2 O. Solutions of this salt contain at: 19 40 50 100 11.7 8.8 6.5 1.6 pts. Di 2 (SO 4 ) 3 . (Marignac, A. ch. (3) 38. 170.) +9H 2 O. (Zschiesche, J. Pr. 107. 75.) Didymium potassium sulphate, K 2 S0 4 , . Di 2 (SO 4 ) 3 +2H 2 O. Sol. in 63 pts. H 2 O. Insol. in sat. K 2 SO 4 + Aq. (Marignac.) 3K 2 SO 4 , Di 2 (SO 4 ) 3 . Sol. in 83 pts. H 2 O at 18. Insol. in cold, si. sol. in boiling sat. K 2 SO 4 +Aq, 100 ccm. of which retain 55 mg. Di 2 O 3 in solution. (Cleve.) 4K 2 SO 4 , Di 2 (SO 4 ) 3 . (Cleve.) 9K 2 SO 4 , 2Di 2 (SO 4 ) 3 +3H 2 O. (Cleve.) Didymium sodium sulphate, Di 2 (S0 4 ) 8 , Na 2 SO 4 , and +2H 2 O. Sol. in 200 pts. H 2 O (Marignac), and still less in sat. Na 2 SO 4 -f Aq, 100 ccm. of which dissolve only 70 mg. Di 2 O 3 at ord. temp. (Cleve.) Didymium thallous sulphate, (Di 2 S0 4 ) 3 , 3T1 2 SO 4 . Ppt. Di 2 (SO 4 ) 3 , T1 2 SO 4 +2H 2 O. Sol. in H 2 O. (Zschiesche, J. pr. 107. 98.) Erbium sulphate, Er 2 (S0 4 ) s . Anhydrous. Easily and rapidly sol. in H 2 O. 100 pts. H 2 O dissolve 43 pts. anhy- drous salt at 0. N C Ci N C Ci 0.1 1.1 2.16 4.604 4.615 3.64 3.04 7.60 7.618 6.00 5.018 4.32 6.685 9.68 15.15 2.00 0.9115 0.4439 0.145 3.301 1.505 0.733 0.239 +8H 2 O. Less sol. in H 2 O than anhydrous salt. 100 pts. H 2 O dissolve 30 pts. Er 2 (SO) 4 ) 3 +8H 2 O (=23 pts. Er 2 (SO 4 ) 3 ) at about 20; at 100, 100 pts. Er 2 (SO 4 ) 3 +8H 2 O remain dissolved. Sat. solution deposits crystals when heated to 55. (Hoglund.) 100 g. of sat. solution of Er 2 (SO 4 ) 3 +8H 2 O at 25 in H 2 O contains 11.94 g. anhyd. Er 2 (SO 4 ) 3 . (Wirth, Z. anorg. 1912, 76. 174.) Solubility of Er 2 (SO 4 ) 3 +8H 2 O in H 2 SO 4 at 25. N = equiv. g. H 2 SO in 1 1. of solvent. C = g. oxide in 100 g. of solution. C 1 = g. anhyd. salt in 100 g. of solution. (Wirth, Z. anorg. 1912, 76. 174.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Erbium potassium sulphate, Er 2 (SO 4 ) 3 , 3K 2 S0 4 . Slowly sol. in H 2 O. (Hoglund.) Erbium sodium sulphate, Er 2 (S0 4 ) 3 , 5Na 2 S0 4 +7H 2 0. Sol. in H 2 O. (Cleve.) Europium sulphate, Eu 2 (SO 4 ) 3 +8H 2 O. Stable in the air. (Urbain and Lacombe, C. R. 1904, 138. 628.) Gadolinium sulphate, Gd 2 (SO 4 ) 3 +8H 2 O. Solubility in H 2 O. Temp. Pts. of Gd 2 (SO4) 3 in 100 pts. H 2 O 3.98 9.3-10.6 3.33 14.0 2.80 25.0 2.40 34.4 2.26 (Benedicks, Z. anorg. 1899, 22. 409-410.) 100 g. sat. solution of Gd(SO 4 ) 3 +8H 2 O at 25 in H 2 O contain 2.981 g. anhyd. Gd 2 (SO 4 ) 3 . (Wirth, Z. anorg. 1912, 76. 174.) SULPHATE, GLUCINUM 971 Solubility in ] N = equiv. C = g. oxide C -L * 2 SO 4 . Solid phase, Gd 2 (SO 4 ) 3 + 8H 2 0. g. H 2 SO 4 in 1 1. of solvent. 5 in 100 g. of solution, yd. Gd 2 (SO 4 ) 3 in 100 g. of solu- Solubility of G1SO 4 in H 2 SO 4 +Aq at 25. H 2 S04+Aq % H 2 S0 4 100 g. of the solution con- tain g. G1SO4 Solid phase i g. ann tion. 5.23 9.61 18.70 34.00 40.35 45.51 50.63 56.59 63.24 65.24 73.64 8.212 8.429 7.944 6.603 5.631 5.773 6.628 5.438 3.640 2.244 2.128 2.185 1 } G1SO 4 +6H 2 O G1SO 4 +4H 2 O J X c Cn N C CM 0.1 0.505 1.1 1.793 1.98 2.365 2.29 2.981 3.291 3.931 3.807 2.16 6.175 12.6 1.789 0.528 0.0521 2.974 0.8777 0.0867 (Wirth.) Sol. in sat. K 2 SO 4 +Aq. Gadolinium potassium sulphate, Gd 2 (SO 4 ) 3 , K 2 SO 4 +2H 2 O. 100 grams, sat. solution in K 2 SO 4 +Aq con- tains 0.87 0.77 grams Gd 2 O 3 . (Benedicks, Z. anorg. 1900, 22. 410.) Gallium sulphate, Ga 2 (SO 4 ) 3 . Not deliquescent, but very sol. in H 2 O. Sol. in 60% alcohol; insol. in ether. (Bois- baudran.) Aqueous solution decomp. into basic salt by boiling, which redissolves, however, on cooling. Gallium potassium sulphate, Ga 2 K 2 (S0 4 ) 4 + 24H 2 O. (Soret, Arch. sc. phys. nat. 1885, 14. 96.) Gallium rubidium sulphate, Rb 2 Ga 2 (S0 4 ) 4 +24H 2 O. (Soret, Arch. sc. phys. nat. 1885, 14. 96.) Glucinum sulphate, basic, 3G1O, SO 3 +4H 2 O. Sol. in H 2 O, but decomp. by heating or dilution. (Berzelius.) 2G10, SO 3 +3H 2 O. Sol. in H 2 0. 9G1O, SO 3 +14H 2 O (?). Precipitate. In- sol. in H 2 O. (Berzelius.) Accorolmg to Debray, this salt when care- fully washed is G1O 2 H 2 . Glucinum sulphate, G1SO 4 . Anhydrous. Nearly insol. in H 2 O, but slowly attacked by cold, rapidly by hot H 2 O, and is converted into G1S0 4 +4H 2 O before dissolving. (Par- sons, Z. anorg. 1904, 42. 253.) Sp. gr. of GlSO 4 +Aq at 25. Concentration of G1SO4 +Aq Sp. gr. 1 normal Vr- " V4 " 1/16 " 1.0451 1.0229 1.0114 1.0027 (Wagner, Z. phys. Ch. 1890, 5. 35.) (Wirth, Z. anorg. 1913, 79. 359.) See also under +2, 4, and 6H 2 O. Insol. in liquid NH 3 . (Gore, Am. Ch. J., 1898, 20. 828.) +H 2 O. (Levi-Malvano, Z. anorg. 1906, 48. 447.) +2H 2 O. Solubility in H 2 O at t. t G. G1S0 4 per 100 g. H 2 O Solution 80 91.4 105 119 84.76 97.77 118.4 149.3 45.87 49.42 54.21 59.88 (Levi-Malvano.) +4H 2 O. Very sol. in H 2 O. Sol. in its own weight of H 2 at 14, and in every proportion of boiling H 2 O. Less sol. in dil. H 2 SO 4 +Aq than in water. (Debray, A. ch. (3) 44. 25.) Solubility in H 2 O at t. g. G1SO4 per g. G1SO4 per t 100 g. t 100 g. H 2 solution H 2 O solution 30 43.78 30.45 95.4 90.63 47.55 40 46.74 31.85 107.2 115.3 53.58 68 61.95 38.27 111 128.3 56.19 85 76.30 43.28 ( Le vi-M al vano . ) SI. sol. in dilute, insol. in absolute alcohol. Can be completely pptd. from GlSO 4 +Aq by HC 2 H 3 2 . (Persoz.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) 972 SULPHATE, GLUCINUM IRON +6H 2 O. Solubility in H 2 O at t. Gold (auric) sulphate, Au 2 O 3 , 2SO 3 +H 2 O, or Auryl hydrogen sulphate, (AuO)HSO 4 . Deliquescent. Decomp. by H 2 O. Sol. in HCl+Aq; not attacked by cone. HNO 3 -{- Aq. Sol. in 6 pts. cone. H 2 SO 4 . (Schott- lander.) Gold (auric) potassium sulphate, Au 2 (SO 4 ) 8 , K 2 SO 4 . Not decomp. immediately by cold H 2 O. fS5r>Vr>tflaTirlai 'i t g. G1SO 4 per 100 g. H 2 O solution 31 50 72.2 . 77.4 52.23 60.67 74.94 81.87 34.32 37.77 42.85 45.01 (Levi-Malvano . ) 100 g. of the aqueous solution contain at 25, 8.212 g. G1SO 4 . (Wirth, Z. anorg. 1913, 79.358.) Glucinum iron (ferrous) sulphate, G1SO 4 , FeS0 4 +17^H 2 0. Sol. in H 2 O. (Klatzo, J. B. 1868. 204.) 3G1SO 4 , FeSO 4 +28H 2 O. Sol. in H 2 O. (Klatzo.) Do not exist. (Marignac, A. ch. (4) 30. 45.) Glucinum nickel sulphate, (Gl,Ni)SO 4 + 4H 2 O, or 7H 2 0. (Klatzo, J. B. 1868. 205.) Does not exist. (Atterberg, Sv. V. A. F. 1873, 4. 81.) Glucinum potassium sulphate, G1S0 4 , K 2 S0 4 +2H 2 0. SI. sol. in cold, slowly but more sol. in hot H 2 O. (Debray.) +3H 2 O. (Klatzo.) Glucinum potassium hydrogen sulphate, G1H 2 (SO 4 ) 2 , 2K 2 SO 4 +4H 2 O. Easily sol. in H 2 O. Partly decomp. by recrystallisation. (Atterberg.) Glucinum sodium sulphate, 2G1SO 4 , 3Na 2 SO 4 +18H 2 O. Sol. in H 2 O. (Atterberg.) Glucuium zinc sulphate, 2G1SO 4 , 3ZnSO 4 + 35H 2 0. Sol. in H 2 O. (Klatzp, J. B. 1868. 205.) Does not exist. (Atterberg.) Gold (auroauric) sulphate, Au 2 (SO 4 ) 2 . Decomp. by moist air, H 2 O, glacial acetic acid, or HNO 3 +Aq (1.42 sp. gr.) Insol. in cone. H 2 SO 4 . (Schottlander, A. 217. 375.) Hydrazine mercuric sulphate hydrazine, (N 2 H 5 ) 2 S0 4 , 3HgS0 4 , 2N 2 H 4 . Insol. in H 2 O. Sol. in H 2 O containing HC1. (Ferratini, Gazz. ch. it. 1912, 42. (1) 142.) Hydroxylamine uranyl sulphate, (NH 2 OH) 2 , H 2 SO 4 , 2(UO 2 )SO 4 +5H 2 0. Extremely sol. in H 2 O from which it can be cryst. (Rimbach, Dissert. 1904.) Indium sulphate, In 2 (SO 4 ) 3 . Easily sol. in H 2 0. +9H 2 O. Easily sol. in H 2 O. Indium hydrogen sulphate, InH(S0 4 )j+ 4HO. Very deliquescent. (Meyer.) Indium potassium sulphate, InK(SO 4 ) 2 + 4H 2 0. Sol. in H 2 0, but decomp. by boiling. (Rossler, J. pr. (2) 7. 14.) (InO) 3 K(SO 4 ) 2 +3H 2 O. Insol. in H 2 0. (Rossler.) Indium rubidium sulphate, In 2 (S0 4 ) 3 , Rb 2 S0 4 +24H 2 0. 44.28 pts. are sol. in 100 pts. H 2 O at 15. (Chabrie-, C. R. 1901, 132. 473.) Melts in crystal H 2 O at 42. (Locke, Am. Ch. J. 1901, 26. 183.) Indium sodium sulphate, InNa(SO 4 ) 2 +4H 2 0. Sol. in H 2 O. (Rossler,, J. pr. (2) 7. 14.) Iodine sulphate, I 2 (SO 4 ) 3 . Ppt. Decomp. by H 2 O. (Fichter, Z. anorg. 1915, 91. 140.) lodyl sulphate, (IO) 2 (SO 4 ) 8 . Possible composition of Weber's (B. 20. 86) I 2 O 6 , 3SO 3 . SULPHATE, IRON 973 Iridium sulphate. Solubility in 100 pts. H 2 O at t. Sol in H 2 O or alcohol (B6rz6lius.) Ir(SO 4 ) 2 . Sol. in H 2 6. (Rimbach, Z t Pts. t Pts. t Pts. anorg. 1907, 62. 409.) FeSO4 FeSO4 FeSO4 7.9 34 37.1 67 65.1 Iridium potassium sulphate, Ir 2 (SO4) 3 , K 2 SO 4 +24H 2 O. 1 2 3 8.7 9.5 10.4 35 36 37 38.0 38.9 39.8 68 69 70 65.0 64.9 64.8 Mpt. 102-103. 4 11.2 38 40.7 71 64.7 Easily sol. in H 2 O. (Marino, Z. anorg. 5 12.0 39 41.7 72 64.5 1904, 42. 220.) 6 12.9 40 42.6 73 64.4 Ir 2 (SO 4 ) 3 , 3K 2 S0 4 . Sol. in H 2 O or dil. 7 13.7 41 43.5 74 64.2 H 2 SO 4 +Aq; nearly insol. in sat. K 2 SO 4 + 8 14.5 42 44.4 75 64.0 Aq. (Boisbaudran, C. R. 96. 1406.) 9 15.3 43 45.3 76 63.7 10 16.2 44 46.2 77 63.4 Iridium rubidium sulphate, Ir 2 (SO 4 ) 4 Rb 2 . 11 17.0 45 47.1 78 63.1 Sol. in cold; very sol. in hot H 2 O. (Marino, Gazz. ch. it. 1903, 32, (2) 511.) Mpt. 108-109. (Marino, Z. anorg. 1904, 42. 219.) 12 13 14 15 17.9 18.7 19.5 20.4 46 47 48 49 48.1 49.0 50.0 51.0 79 80 81 82 62.7 62.3 61.9 61.5 16 21.2 50 51.9 83 61.0 Iridium thallium sulphate, Ir 2 (SO 4 ) 3 , Tl 2 SO 4 -f 17 18 22.1 23.0 51 52 52.9 53.8 84 85 60.4 59.8 24H 2 O. 19 23.8 53 54.8 86 59.2 Very sol. in H 2 O. (Marino, Z. anorg. 20 24.7 54 55.7 87 58.5 1904, 42. 222.) 21 25.6 55 56.7 88 57.7 22 26.4 56 57.7 89 57.0 Iron (ferrous) sulphate, FeSO 4 . 23 27.3 57 58.7 90 56.2 +H 2 O. 24 28.1 58 59.7 91 ' 55.3 +2H 2 O. Not more sol. in H 2 Q than gyp- sum. (Mitscherlich.) 25 26 29.0 29.9 59 60 60.7 61.7 92 93 54.3 53.3 +3H 2 O. Sol. in H 2 O. (Kane.) 27 30.8 61 62.7 94 52.2 +4H 2 O. Separates from cone. FeSO 4 +Aq at 80. 28 29 31.7 32.6 62 63 63.7 64.8 95 96 51.0 49.6 +7H 2 O. Efflorescent at 33. 30 33.5 63.5 65.4 97 48.0 31 34.4 64 65.4 98 46.3 1 pt. FeSO4+7H 2 O dissolves in 1.6 pts. cold, and 0.3 32 35.3 65 65.3 99 44.5 pt. boiling H 2 O. 1 pt. FeSO4+7H 2 O dissolves at: 33 36.2 66 65.2 100 42.6 10 15 25 33 46 60 8t 90 100 in 1.64 1.43 0.87 0.66 0.44 0.38 0.37 0.27 0.3 pts. H 2 O (Brandes and Firnhaber, Br. Arch. 7. 83.) (Mulder, Scheik. Verhandel. 1864. 141.) When boiled with insufficient H 2 O for solution a white hydrate is formed which separates out. Solubility increases up to 87.5, and then diminishes, owing to the above separation. (Brandes, Pogg. 20. 581.) Sol. in 2 pts. cold, and 1 pt. boiling H 2 O (Fourcroy) : sol. in 2 pt.s cold H 2 O at 18.75 (Abl) ; sol. in 6 pts. H 2 O at moderate heat, and 0.75 pt. at 100. (Bergmann.) 100 pts. H 2 O at 15.5 dissolve 45-50 pts. (Ure's Diet.) 100 ftis. H 2 O dissolve pts. FeSO4 at t. t Pts. FeS04 t Pts. FeS04 t Pts. FeS0 4 o 10 12 20 15.8 19.9 21.3 28.0 21 30 37 27.4 32.6 36.5 45 55 70 42.9 47.0 56.5 (Tobler, A. 95. 198.) 100 pts. FeSO 4 +Aq sat. at 11-14 contain 17.02% FeSO 4 . (v. Hauer, J. pr. 103. 114.) 100 pts. FeSO 4 +Aq. sat at 15 contain 37.2% FeSO 4 +7H 2 O; solution has sp. gr. 1.2232. (Schiff, A. 118. 362.) If solubility S=pts. anhydrous FeSO 4 in 100 pts. solution, S = 13.5+0.3788t from 2 to +65; S = 37.5 constant from 65 to 98; S = 37.5 0.6685t from 98 to 156. Practi- cally insol. at 156. (fitard, C. R. 106. 740.) Sat. FeSO 4 +Aq contains at: 1 +5 24 34 52 1O.U 60 J.O. JL 67 22. / 77 2v. 0^.070 reov/ 4 , 86 94 36.4 37.7 37.8 37.8 36.7%FeSO 4 , 102 112 130 152 34.7 28.0 17.3 2.5%FeS0 4 . (Etard, A. ch. 1894, (7) 2. 553.) 100 g. H 2 O dissolve 26.69 g. FeSO 4 at 25. (Stortenbecker, Z. phys. Ch. 1900, 34. 109.) 974 SULPHATE, IRON Solubility of FeSO 4 in H 2 O at t. 100 g. H 2 O dissolve g. FeSO 4 . Sol. in hot HCl+Aq. (Kane.) Somewhat sol. in cone. H 2 SO4. (Bussy and Lecann.) Solubility in H 2 SO 4 +Aq at 25. t G. FeSO 4 t G. FeSO4 0.00 10.00 15.25 20.13 25.02 30.03 35.07 40.05 45.18 50.21 15.65 20.51 23.86 26.56 29.60 32.93 36.87 40.20 44.32 48.60 52.00 54.03 60.01 65.00 68.02 70.04 77.00 80.41 85.02 90.13 50.20 52.07 54.95 55.59 52.31 56.08 45.90 43.58 40.46 37.27 H 2 S0 4 +Aq Normality 100 g. of the solution contain g. FeSO4 Solid phase 2.25 6.685 10.2 12.46 15.15. 19.84 22.84 19.03 13.40 10.30 7.26 4.015 0.1522 FeSO 4 +7H 2 O FeSO 4 +H 2 O J FeSO 4 +7H 2 O is stable from 1.82 to +56.6; FeSO 4 +4H 2 O from 56.6 to 64.4; FeSO 4 +H 2 O above this point. (Fraenckel, Z. anorg. 1907, 56. 228.) (Wirth, Z. anorg. 1913, 79. 364.) FeSO 4 +Aq sat. at 30 contains 24.9 g. FeSO 4 in 100 g. of solution. (Schreine- makers, Z. phys. Ch. 1912, 71. 110.) Sp. gr. of FeSO 4 +Aq at 15. % = %FeSO 4 +7H 2 O. % Sp. gr. % Sp. gr. % Sp. gr. 1 1.005 15 1.082 28 1.161 2 1.011 16 1.088 29 1.168 3 1.016 17 1.094 30 1.174 4 1.021 18 1.100 31 1.180 5 1.027 19 1.106 32 1.187 6 1:032 20 1.112 33 .193 7 1.037 21 1.118 34 .200 8 .043 22 1.125 35 .206 9 .048 23 1.131 36 .213 10 .054 24 1.137 37 .219 11 .059 25 1.143 38 .226 12 1.065 26 1.149 39 .232 13 1.071 27 1.155 40 .239 14 1.077 (Gerlach, Z. anal. 8. 287.) Sp. gr. 16.6 of sat. solution = 1.219. (Greenish and Smith, Pharm. J. 1903, 71. 881.) Sat. FeSO 4 +Aq boils at 102.2 (Griffiths), and solution contains 64% FeSO 4 . Crust forms at 102.3; highest temp, observed, 104.8. (Gerlach, Z. anal. 26. 426.) B.-pt. of FeSO 4 +Aq containing pts. FeSO 4 to 100 pts. H 2 O. B.-pt. Pts. FeSO 4 B.-pt. Pts. FeSO 4 100.5 101.0 17.7 34.4 101.5 101.6 50.4 53.2 (Gerlach, Z. anal. 26. 433.) 100 g. of the sat. solution contain 22.84 g FeSO 4 at 25. (Wirth, Z. anorg. 1913, 79 364.) More sol. in water containing NO than in pure H 2 O. (Gay, Bull. Soc. (2) 44. 175.) Completely pptd. from FeSO 4 +Aq by glacial HC 2 H 3 O 2 . (Persoz.) Solubility in (NH 4 ) 2 SO 4 +Aq. See under (NH 4 ) 2 S0 4 . ooiuiDiiiiy in .L*i 2 ow 4 -t-/iq at ou . Composition of the solution Solid phase % by wt. FeSCU ,% by wt. Li 2 S0 4 24.87 22.45 21.15 18.79 16.51 16.18 16.04 15.39 12.68 5.32 3.74 4.00 5.58 11.16 15.81 16.52 16.49 16.80 18.31 22.15 23.15 25.1 FeSO 4 , t 7H 2 C t{ u FeSO 4 , 7H 2 O+Li 2 SO 4 , H 2 O tt Li 2 SO 4 , H 2 O ft C( (( (Schreinemakers, Z. phys. Ch. 1910, 71. 110.) Solubility of FeSO 4 , H 2 O+Na 2 SO 4 , 10H 2 O 4 , in 100 g. H 2 O at t. t Grams FeSO4 Grams Na2SO4 15.5 18.08 25.05 6.13 15.97 (Koppel, Z. phys. Ch. 1905, 52. 405.) See also under FeNa 2 (SO 4 ) 2 . Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Insol. in liquid CO 2 . (Biichner, Z. phys. Ch. 1906, 54. 674.) 100 pts. sat. solution of FeSO 4 in 40% alcohol contains 0.3% FeSO 4 . (Schiff.) SULPHATE, IRON 975 Insol. in alcohol of 0.905 sp. gr. or less. (Anthon, J. pr. 14. 125.) Alcohol and H 2 SO 4 precipitate FeSO 4 from FeSO 4 +Aq, also glacial acetic acid. Anhydrous FeSO 4 is insol. in acetone. (Krug and M'Elroy, 1893.) Insol. in acetone. (Eidmann, C. C. 1899, 11. 1014.) 100 g. sat. solution in gycol contain 6.0 g. FeSO 4 at ord. temp, (de Coninck.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) Iron (ferrous) sulphate, acid, 2FeO, 3SO 3 , 2H 2 O. This salt exists in contact with solutions containing SO 3 +1.637 H 2 O to about SO 3 + 2.186 H 2 O. (Kenrick, J. phys. Chem. 1908, 12. 704.) FeO, 2SO 3 +H 2 O. This compd. exists with solutions containing SO 3 + 1.342 H 2 O to (about) SO 8 +1.595 H 2 O. (Kenrick.) FeO, 4SO 3 +3H 2 O. This compd. is stable with solutions containing from SO 3 + 1.122 H 2 O to (about) SO 3 + 1.342 H 2 O. Rapidly sol. in H 2 O with ppt. of FeSO 4 +H 2 0. (Ken- rick.) Min. Melanterite. Iron (ferric) sulphate, basic, 10Fe 2 O 3 , SO 3 + H 2 O. (Athanasesco, C. R. 103. 27.) 6Fe 2 O 3 , SO 3 +10H 2 O. Insol. in H 2 O. SI sol. in warm HCl+Aq. (Scheerer, Pogg. 45. 188.) 4Fe 2 O 3 , SO 3 +11H 2 O. (Anthon, Repert, 81. 237.) 3Fe 2 O 3 , SO 3 +4H 2 O. Insol. in H 2 O, Rather easily sol. in acids. (Scheerer, Pogg 44. 453; Meister, B. 8. 771.) 2Fe 2 O 3 , SO 3 +6H 2 O. When pptd. from cold solutions, is sol. in Fe 2 (SO 4 ) 3 +Aq, but insol. therein when pptd. from hot solutions (Maus.) Only basic sulphate which is a true chem- ical compound. (Pickering, Chem. Soc. 37 807.) Min. Glockerite. Insol. in H 2 O. Sol. in cone. H 2 SO 4 . +7H 2 O. (Meister.) +8H 2 O. (Muhlhauser.) + 15H 2 O. Min. Pissophanite. Fe 2 O 3 , SO 3 = (FeO) 2 SO 4 +3H 2 O. Insol. in H 2 O. (Soubeiran, A. ch. 44. 329.) 3Fe 2 O 3 , 4SO 3 +9H 2 O. (Athanasesco.) 2Fe 2 O 3 , 3SO 3 +8H 2 O. Insol. in H 2 O (Wittstein.) + 18H 2 O. Min. Fibroferrite. SI. sol. in cold, more easily in hot H 2 O. Fe 2 O 3 , 2SO 3 +10H 2 0. Min. Stypticite. +15H 2 O. Sol. in H 2 O; decomp. by heat or evaporation. (Muck, J. pr. 99. 103.) 2Fe 2 O 3 , 5SO 3 +13H 2 O. Min. Copiapite. Fe 4 S 6 O 2 +18H 2 O =2Fe 2 O 3 , 5SO 3 +18H 2 O a-Copiapit. This salt is in equilibrium at 25 C with solutions in which the molecular ratio Fe 2 O 3 : SO 3 lies between 1 : 2.889 and 1 : 2.614. (Wirth, Z. anorg. 1914, 87. 37.) (OH)Fe 3 (SO 4 ) 4 +13H 2 O. p-Copiapit. This salt is in equilibrium at 25 with solutions in which the molecular ratio Fe 2 O 3 :SO s lies between 1:3.472 and 1:2.889. (Wirth, Z. anorg. 1914, 87. 37.) According to Pickering (Chem. Soc. 37. 807), all basic ferric sulphates are mixtures excepting 2Fe 2 O 3 , S0 3 . Iron (ferric) sulphate, Fe 2 (SO 4 ) 3 . Anhydrous. Slowly deliquescent. Nearly insol. in H 2 O, and HCl+Aq. Insol. in cone. H 2 SO 4 . Very rapidly sol. in FeSO 4 +Aq, even when very dil. (Barreswil, C. R. 20. 1366.) Sp. gr. of Fe 2 (SO 4 ) 3 +Aq. According to F = Franz at 17.5 (J. pr. (2) 5. 280); G = Ger- lach at 15 (Z. anal. 28. 494); H = Hager at 18 (Z. anal. 27. 280). 5 10 15 20 % Fe 2 (S0 4 ) 3 , F 1.0426 1.0854 1.1324 1.1826 G ... 1.096 ... 1.205 H 1.046 1.097 1.151 1.208 25 30 35 40 % Fe 2 (SO 4 ) 3 , F 1.2426 1.3090 1.3782 1.4506 G ... 1.331 . . . 1.478 H 1.271 1.337 1.411 1.490 45 50 55 60 % Fe 2 (SO 4 ) 3 . F 1.5298 1.6148 1.7050 1.8006 G ... 1.650 ... ... Solubility in H 2 SO 4 +Aq at 25. H 2 S0 4 +Aq Normality 100 g. of the solution contain g. Fe2(SO4)s 2.25 6.685 19.84 25.02 14.58 0.05 (Wirth, Z. anorg. 1913, 79. 364.) Solubility in Al 2 (SO 4 ) 3 +Aq at 25. 100 g. of the solution contain G. Al 2 (SO4)s G. Fe 2 (SO 4 )a 44.97 2.342 42.44 5.200 38.83 6.626 35.82 8.819 34.02 10.03 32.42 *10.23) 31.90) 10.70} 31.91J *Solution sat. with respect to both salts. (Wirth and Bakke, Z. anorg. 1914, 87. 48.) See also under A1 2 (SO 4 ) 3 . Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 828.) 976 SULPHATE, IRON Completely pptd. from Fe 2 (SO 4 ) 3 +Aq by HC 2 H 3 O 2 . Sol. to large extent in alcohol. Insol. in methyl acetate. (Naumann B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1910, 43. 314.) Insol. in acetone. +zH 2 O. Very deliquescent, and sol. in H 2 O. Cone. Fe 2 (SO 4 ) 3 +Aq may be boiled without decomp., but dil. solutions are de- comp. on heating. A solution containing 1 pt. salt to 100 pts. H 2 O becomes turbid at 76; 1 pt. to 200 pts., at 56; 1 pt. to 400 pts., at 47; 1 pt. to 800 pts., at 40; 1 pt. to 1000 pts., at 38; 1 pt. to 10,000 pts., at 14. (Scheerer.) +9H 2 O. Min. Coquimbite. 81.43 pts. are sol. in 18.57 pts. H 2 O. (Wirth, Z. anorg. 1914, 87. 23.) This salt is stable at 25 only in contact with solutions in which the molecular ratio Fe 2 O 3 : SO 3 lies between 1 : 3.472 and 1 : 6.699. (Wirth, Z. anorg. 1914, 87. 35.) +10H 2 O. Slowly sol. in H 2 O. (Oudemans, R. t. c. 3. 331.) Iron (ferroferric) sulphate, 6FeSO 4 , Fe 2 (SO 4 ) 3 +60H 2 O. Sol. in all proportions in H 2 O. (Poumarede. C. R. 18. 854.) 3FeSO 4 , 2Fe 2 (SO 4 ) 3 + 12H 2 0. Decomp. by H 2 0. Easily sol. in dil. HCl+Aq. Insol. in alcohol. (Abich, 1842.) FeSO 4 , Fe 2 (SO 4 ) 3 +12H 2 O. Min. Voltaite. Difficultly sol. in H 2 O. FeO, Fe 2 O 3 , 6SO 3 +15H 2 O. Deliquescent. (Lefort, J. Pharm. (4) 10. 87.) Iron (ferrous) pi/rosulphate, FeS 2 O 7 . Deliquescent. Decomp. by H 2 O. (Bolas, Chem. Soc. (2) 12. 212.) Iron (ferric) hydrogen sulphate, Fe 2 (SO 4 ) 3 , H 2 SO 4 +8H 2 O. This salt is in equilibrium at 25 only with solutions where the molecular ratio Fe 2 3 : SO 3 is more acid than 1 : 6.699. (Wirth and Bakke, Z. anorg. 1914, 87. 34.) Sat. solution of Fe 2 (SO 4 ) 3 , H 2 SO 4 +8H 2 in abs. alcohol at 25 contains 8 jg. Fe 2 O 3 + 17.18 g. SO 3 per 100 g. sat. solution. (Wirth and Bakke.) Decomp. by H 2 O. (Recoura, C. R. 1903, 137. 118.) In contact with solutions containing 25% to 28%SO 3 at 25, the stable solid is Fe 2 O 3 , 3SO 3 -j- 10H 2 O . In contact with solutions con- taining more than 28%, the stable solid is Fe 2 O 3 , 4SO 3 + 10H 2 O. (Cameron and Robin- son, J. phys. Chem. 1907, 11. 650.) Iron (ferroferric) hydrogen sulphate, Fe 2 (S0 4 ) 3 , FeS0 4 , 2H 2 SO 4 . Insol. in H 2 O, but slowly decomp. thereby. Sol. inH 2 S0 4 . (Etard, C.R. 87. 602.) Iron ( ferrous) hydrazine sulphate, FeH 2 (SO 4 ) 2 2N 2 H 4 . 1 pt. is sol. in 325 pts. H 2 O at 12. (Curtius, J. pr. 1894, (2) 60. 331.) Iron (ferrous) magnesium sulphate. FeSO 4> MgSO 4 +4H 2 O. Sol. inH 2 O. (Schiff.) Iron (ferric) magnesium sulphate. Fc 2 (SO 4 ) 8 . MgS0 4 +24H 2 0. (Bastick.) Iron (ferrous) magnesium potassium sulphate. ^ 2K 2 S0 4 , FeSO 4 , MgS0 4 +12H 2 O. Sol. in!H 2 O. (Vohl, A. 94. 57.) Iron (ferric) manganous hydrogen sulphate, Fe 2 (SO 4 ) 3 , 2MnSO 4 , H 2 S0 4 . Insol. in cold H 2 O. (Etard.) Fe 2 (SO 4 ) 3 , 2MnS0 4 , 3H 2 SO 4 . Sol. in H 2 O. (Etard, C. R. 86. 1399.) Iron (ferric) manganic sulphate, Fe 2 (SO 4 )3, Mn 2 (S0 4 ) 3 . Insol. in cold H 2 O; decomp. by hot H 2 O and HC1 +Aq. (Etard.) Iron (ferrous) manganous potassium sulphate, FeSO 4 , MnS0 4 , 2K 2 SO 4 +12H 2 O. SoUin H 2 0. (Vohl, A. 94. 57.) Iron (ferrous) nickel sulphate, 2FeSO 4 , 2NiSO 4 , H 2 SO 4 . (Etard, C. R. 87. 602.) Iron (ferric) nickel sulphate, Fe 2 (SO 4 ) 8 , NiS0 4 , 2H 2 SO 4 . Insol. in H 2 O, but gradually decomp. thereby. (Etard, C. R. 87. 602.) Iron (ferrous) nickel potassium sulphate, FeSO 4 , NiSO 4 , 2K 2 SO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Iron (ferrous) potassium sulphate, FeSO<, K 2 S0 4 . +2H 2 O. (Marignac, Ann. Min. (5) 9. 19.) Solubility in H 2 O at t. t % FeK 2 (S04) 2 t %FeK 2 (S0 4 ) 2 0.5 17.2 40.1 60 22.79 31.98 40.86 42.63 80 90 95 42.34 42.73 41.01 (Kiister and Thiel, Z. anorg. 1899, 21. 116.) SULPHATE, IRON SODIUM 977 +4H 2 0. G=Gerlach, at 15 (Z. anal. 28. 496); F = Solubility in H 2 O at t. Franz, at 17.5 (J. pr. (2) 5. 288), containing: 5 10 15% K 2 Fe 2 (S0 4 ) 4 +24H a O, F 1.0268 1.0466 1.0672 t %FeK 2 (S0 4 )2 t % FeK 2 (SO4) 2 0.5 22.94 80 40.46 G 1.025 1.0507 1.0773 17.2 40.1 26.79 32.41 90 95 43.82 44.11 20 25 30% K 2 Fe 2 (S0 4 ) 4 +24H 2 O, F 1.0894 1.1136 1.1422 60 35.68 G 1.1050 1.1340 1J645 (Kiister and Thiel.) +6H 2 0. 100 pts. H 2 O dissolve at t: 10 14,5 16 25 19.6 24.5 29.1 30.9 36.5 pits, anhydrous salt, 35 40 55 65 70 41 45 56 59.3 64.2 pts. anhydrous salt. (Tobler, A. 96. 193.) Solubility in H 2 O at t. t %FeK 2 (SO 4 ) 2 t % FeK 2 (SO 4 ) 2 0.5 17.2 40.1 18.36 25.16 36.72 60 80 42.93 45.29 (Kiister and Thiel.) Iron (ferric) potassium sulphate, basic. 4Fe 2 3 , K 2 0, 7S0 3 +9H 2 0=4(Fe 2 8 , 2H 2 O, SO,), K 2 S0 4 +7H 2 O. Insol. in boiling H 2 O. SI. sol. in HCl+Aq, more readily in aqua regia. (Rammelsberg.) 3Fe 2 O 3 , K 2 0, 4SO 3 +6H 2 O =K(FeO) 3 (S0 4 ) 2 +3H 2 O. Min. Jarosite. Fe 2 O 3 , H 2 O, 2SO 3 , 2K 2 SO 4 +5H 2 O. Sol. in 6 pts. cold H 2 O. Solution soon decomposes. (Maus, Pogg. 11. 78.) Sol. in 12.5 pts. H 2 O at 10. (Anthon, Re- pert. 76. 361.) Formula is given as 3Fe 2 O 3 , 5K 2 O, 12SO 3 + 18H 2 O by Marignac. 3Fe 2 O 3 , 6SO 3 , 2K 2 SO 4 +22H 2 O. Sol. when moist in H 2 O. Solution soon decomposes. Insol. in alcohol. (Soubeiran, A. ch. 44. 329.) 3Fe 2 O 3 , 7SO 3 , 5K 2 SO 4 +12H 2 O, and +17H 2 O. (Scheerer, Pogg. 87. 81.) 2Fe 2 O 3 , 5SO 3 , 3K 2 SO 4 +9H 2 O. (S.) 3Fe 2 O 3 , 8SO 3 , 4K 2 SO 4 +20H 2 O and 24H 2 O. (S.) Iron (ferric) potassium sulphate, K 2 SO 4 , 2Fe 2 (S0 4 ) 3 . Insol. in H 2 O, but is gradually decomp. thereby. (Grimm and Ramdohr, A. 98. 127.) +2H 2 O. Nearly insol. in H 2 O. (Weinland, Z. anorg. 1913, 84. 364.) K 2 Fe 2 (SO 4 ) 4 +24H 2 O. Iron alum. Sol. in 5 pts. H 2 O at 12.5. (Anthon.) Aqueous solution is decomp. by heating. Insol. in alcohol. Sp. gr. of aqueous solution. According to 35 % K 2 Fe 2 (S0 4 ) 4 +24H 2 0. G 1.1967. Melts in crystal H 2 O at 28. (Locke, Am. Ch. J. 1901, 26. 183.) Fe 2 (SO 4 )s,, 3K 2 SO 4 . Insol. in H 2 O, but slowly decomp. thereby, (fitard, C. R. 84. 1089.) Iron (ferric) potassium sulphate sulphite. See Sulphite sulphate, ferric potassium. Iron (ferrous) potassium zinc sulphate, FeS0 4 , 2K 2 SO 4 , ZnSO 4r fl2H 2 O. Sol. in H 2 0. Iron (ferrous) rubidium sulphate, FeS0 4 , Rb 2 S0 4 +6H 2 0. Sol. in H 2 O. (Tutton, Chem. Soc. 63. 337.) 1 1. H 2 O dissolves 242 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Iron (ferric) rubidium sulphate, RbjFei (S0 4 ) 2 +24H 2 0. Solubility in H 2 O. Temp. G. per litre Gram mols. of anhydrous salt per litre 25 30 35 97.4 202.4 Basic salt formed 0.294 0.617 (Locke, Am. Ch. J. 1901, 26. 180.) Iron (ferrous) sodium sulphate, FeSO 4 , Na 2 SO 4 +4H 2 O. Sol. in H 2 O. (Marignac, Ann. Min. (5) 9. 25.) Solubility of FeNa 2 (SO 4 ) 2 +4H 2 O in 100 g. H 2 O at t. t Grams FeSO4 Grama Na!iSO 4 21.8 24.92 34.95 40 24.34 23.62 23.91 24.01 22.51 22.04 21.83 22.62 (Koppel, Z. phys. Ch. 1905, 62. 406.) 978 SULPHATE, IRON SODIUM, BASIC Solubility of FeNa 2 (SO 4 ) 2 .4H 2 O+FeSO 4 . 7H 2 O in 100 g. H 2 O at t. t grams FeSCU grams Na 2 SO4 t grams FeS0 4 grams Na 2 S04 18.8 23 27 26.63 28.82 30.95 20.28 18.40 16.68 31 35 40 33.99 35.66 39.98 14.41 13.85 11.92 (Koppel.) Solubility of FeNa 2 (SO 4 ) 2 .4H 2 O+Na 2 SO 4 . "10H 2 O in 100 g. H 2 O at t. t grams FeS0 4 grams Na 2 S0 4 t grams FeS0 4 grams Na 2 SO4 18.8 23 27.23 20.31 22.16 26.48 28 31 11.28 6.95 35.94 44.75 (Koppel.) Solubility of FeNa 2 (SO 4 ) 2 .4H 2 O +Na 2 SO 4 (anhydrous) in 100 g. H 2 O at t. t grams FeSO 4 grams Na 2 SO 4 46.58 46.99 35 40 6.16 6.27 (Koppel.) See also under FeSO 4 . Iron (ferric) sodium sulphate, basic, 2Na 2 O, Fe 2 O 3 , 4SO 3 +7H 2 O. Only si. sol. in H 2 O with decomp. (Skrabal, Z. anorg. 1904, 38. 319.) +8H 2 O. Min. Urusite. Insol. in H 2 O; easily sol. in HCl+Aq. . 3Na 2 O, Fe 2 O 3 , 6S0 3 +6H 2 O. Sol. in H 2 with decomp. (Skrabal.) 4Fe 2 O 3 , Na 2 O, 5SO 3 +9H 2 0. Insol. in H 2 O; difficultly sol. in HCl+Aq. (Scheerer, Pogg. 45. 190.) Iron (ferric) sodium sulphate, [Fe(SO 4 ) 3 ]Na 3 +3H 2 O. Ppt. Nearly insol. in H 2 O. (Weinland, Z. anorg. 1913, 84. 365.) Iron (ferrous) thallium sulphate, FeSO 4 , T1 2 SO 4 +6H 2 0. Easily decomp. by solution in H 2 O. (Willm, A. ch. (4) 6. 56.) Iron (ferric) thallium sulphate, Tl 2 Fe 2 (SO 4 ) 4 +24H 2 O. Not efflorescent. Very easily sol. in H 2 O. 361.5 g. anhydrous, or 646 g. hydrated salt are sol. in 1 1. H 2 O at 25, or 0.799 mol. of the anhydrous salt is sol. in 1 1. H 2 O at 25. Melts in crystal H 2 O at 37. (Locke, Am. Ch. J. 1901, 26. 175.) Iron (ferrous) zinc sulphate, FeSO 4 , ZnS0 3 + 14H 2 O. 2FeSO 4 , 2ZnSO 4 , H 2 SO 4 . (Etard, C. R. 87. 602.) Iron (ferric) zinc sulphate, Fe 2 (SO 4 ) 3 , ZnSO 4 +24H 2 0. (Bastick.) Iron (ferrous) sulphate nitric oxide, FeSO 4 , NO. The solubility of NO in FeSO 4 +Aq is diminished by the presence of H 2 S0 4 , HC1, phosphoric acid and by the presence of cer- tain salts. (Manchot, A. 1910, 372. 157.) Fe(NO)SO 4 , FeSO 4 +13H 2 O. Decomp. in the air. Sol. in water. (Manchot.) Lanthanum sulphate, basic, 2La 2 O 8 , 3SO a + 3H 2 O. Precipitate. (Frerichs and Smith.) Formula is 3La 2 O 3 , SO 3 +zH 2 O. (Cleve, B. 11. 910.) Lanthanum sulphate, La 2 (SO 4 ) 3 . Anhydrous. Much less sol. in warm than in cold H 2 O. 1 pt. is sol. in less than 6 pts. H 2 O, if added in small portions thereto at 2-3, and the temperature not allowed to rise to 13; but if heated to 30, La 2 (SO 4 ) 3 +9H 2 O separates out until the solution is solid. (Mosander.) 100 pts. H 2 O dissolve 2.208 pts. La 2 (SO 4 ) at 16.5; 2.130 pts. at 18; 1.641 pts. at 34. - See also under +9H 2 O. The solubility of La 2 (SO 4 ) 3 in H 2 O is dim- inished by the presence of (NH 4 ) 2 SO 4 , K 2 S0 4 or Na 2 SO 4 . (Barre, C. R. 1910, 151. 871.) Solubility in (NH 4 ) 2 SO 4 +Aq at 18. Pts. per 100 pts. H 2 Solid phase m g 6 S 3 0.00 4.011 8.727 18.241 27.887 36.112 47.486 53.823 65.286 73.782 2.130 0.393 0.279 0.253 0.476 0.277 0.137 0.067 0.0117 0.0033 La 2 (SO 4 ) 3 +9H 2 La 2 (S0 4 ) 3 , (NH 4 ) 2 S0 4 +2H 2 u tt if tt 2La 2 (S0 4 ) 3 , 5(NH 4 ) 2 S0 4 La 2 (S0 4 ) 3 , 5(NH 4 ) 2 S0 4 " (Barre.) Solubility in K 2 SO 4 +Aq at 16.5. Pts. per 100 pts. H 2 Solid phase La 2 (SO 4 ) 8 +9H 2 O La 2 (S0 4 ) 3 , K 2 S0 4 +2H 2 u La 2 (SO 4 ) 3 , 5K 2 SO 4 tt K2SO4 La 2 (SO4)s 0.00 0.247 0.496 0.846 1.029 1.516 2.198 0.727 0.269 0.185 0.054 0.022 (Barre.) SULPHATE, LEAD 979 Solubility in Na 2 SO 4 +Aq at 18. La 2 (SO 4 ) 3 , 4K 2 SO 4 . As above. (Cleve.) Pts. per 100 pts. 2La 2 (S0 4 ) 8 , 9K 2 SO 4 . As above. (Cleve.) H 2 O Solid phase Lanthanum rubidium sulnha.tfc Na 2 SO4 La 2 (S04)s JL/CJiitlltfUiUiiA lU.UlvilU-l.li. oU.ljJliC4.LCy La 2 (S0 4 ) 3 , Rb 2 S0 4 . 0.00 2.130 La 2 (SO 4 ) 3 +9H 2 O (Baskerville, J. Am. Chem. Soc. 1904, 26. 67.) 0.395 0.689 0.774 0.997 0.353 0.299 La 2 (SO 4 ) 3 , Na 2 SO 4 tt +2H 2 O. (Baskerville.) 3La 2 (SO 4 ) 3 , 2Rb 2 SO 4 . (Baskerville.) 1.136 0. 129 (i 2^480 0^044 Lanthanum sodium sulphate, La 2 (SO 4 ) 8 , 3.802 0.019 (( Na 2 SO 4 +2H 2 0. 5.548 0.016 ii SI. sol. in H 2 0. (Cleve.) (Barre, C. R. 1910, 161. 872.) (Barre.) Insol. in liquid NH 3 . (Gore, Am. Ch. J 1898, 20. 830.) Insol. in acetone. (Naumann, B. 1904, 37.4329.) +9H 2 O. Sol. in 42.5 pts. H 2 O, calculated as anhydrous salt, at 23, and 115 pts. H 2 at 100. (Mosander.) Solubility in H 2 O. 100 pts. H 2 Q dissolve pts. La 2 (SO 4 ) 3 at t. t Pts. La 2 (SO4) 3 ar 3.02 p 14 2.60 r 30 ' 1.90 50 1.49 75 0.94 Li 100 0.68 (Muthmann and Rolig, B. 1898, 31. 1723.) , Solubility in H 2 SO 4 +Aq at 25. C In 100 g. of the 86 Normality H 2 SO4 liquid are dissolved Solid phase PI g. oxide g. sulphate i ( at 1.43 2.483 La 2 (SO 4 ) 3 +9H 2 O 12 0.505 1.69 2.934 1.10 1.796 3.118 so Z. 2.16 1.818 3.156 3.39 1.42 2,465 4.321 1.11 1.927 \^ 6.685 0.5309 0.9217 j*j 9.68 0.2659 0.4617 i *i 12.60 0.2136 0.3709 1 o 15.15 0.177 0.3073 It (Wirth, Z. anorg. 1912, 76. 189.) Lanthanum hydrogen sulphate, La(SO 4 H) 3 . (Brauner, Z. anorg. 1904, 38. 330.) Lanthanum potassium sulphate, La 2 (SO 4 ) 3 , K 2 S0 4 +2H 2 0. La 2 (SO 4 ) 3 , 5K 2 SO 4 . (Barre, C. R. 1910, 151. 872.) La 2 (SO 4 ) 3 . 3K 2 SO 4 . SI. sol. in H 2 O. Insol. in sat. K 2 SO 4 +Aq. (Cleve.) Lead sulphate, basic, 2PbO, SO 3 . Not completely insol. in H 2 O. Decomp. by acids, even dil. HC 2 H 3 O 2 +Aq, with forma- tion of PbSO 4 . (Barfoed, 1869.) 0.050 millimole calc. as Pb is sol. in 1 1. H 2 O at 18. (Pleissner, C. C. 1907, II. 1056.) 5PbO, 3SO 3 . (Frankland, Proc. Roy. Soc. 46. 364.) Pb 3 O 4 , 2SO 3 . (Frankland.) 3PbO,PbSO 4 +H 2 O. Ppt. (Stromholm, Z. anorg. 1904, 38, 442.) Pb 4 (SO 4 )(OH) 2 . 0.106 millimole calc. as Pb is sol. in 1 liter H 2 O at 18. (Pleissner, C. C. 1907. II, 1056.) Lead sulphate, PbS0 4 . Sol. in 22,816 pts. H 2 O at 11. (Fresenius, A. 69. 125.) Sol. in 31,569 pts. H 2 O at 15. (Rodwell, C. N. 11. 50.) Sol. in 13,000 pts. H 2 O. (Kremers;, Pogg. 86. 247.) Calculated from electrical conductivity of PbSO 4 +Aq, 1 1. H 2 O dissolves 46 mg. PbSO 4 at 18. (Kohlrausch and Rose, Z. phys. Ch. 12. 241.) 4.23 XHHgr. are dissolved in 1 liter of sat. solution at 20; 4.41 X 10 2 at 25. (Bottger, . phys. Ch. 1903, 46. 604.) 1 1. H 2 O dissolves 41 mg. PbSO 4 at 18. (Kohlrausch, Z. phys. Ch. 1904, 60. 16.) o!l26 millimole Pb is sol. in 1 liter H 2 O at ;. (Pleissner. C. C. 1907, II. 1056.) 40 mo- are dissolved in 1 1. of sat. solution 18. (Kohlrausch, Z. phys. Ch. 1908, 64. '8.) 0.0824 g. PbSO 4 is sol. in 1000 cc. H 2 O at 18 and also at 100. The fact that PbSO 4 dissolves in H 2 O is ascribed to hydrolysis, and n support of this it is shown that the solubil- ty of hydrated oxide of lead, PbO, H 2 O, in dil. H 2 SO 4 is the same as the solubility of >bSO 4 in H 2 O. (Sehnal, C. R. 1909, 148. 395 ) 1 1. H 2 O dissolves 26 mg. at 18; 30 mg. it 25; 38 mg. at 37. (Beck and Stegmiiller, Arb. K. Gesund. Amt. 1910, 34. 447.) 980 SULPHATE, LEAD Solubility in H 2 O at t c (Millimols per 1.) t PbSO 4 18 25 37 0.126 0.144 0.183 (Beck and Stegmuller, Arb. K. Gesund. Amt. 1910, 34. 446.) Sol. in hot cone. HCl+Aq. (Fresenius.) Solubility of PbSO 4 in HCl+Aq. Sp. gr. of HCl+Aq % HCl in HCl+Aq Pts. HCl+Aq for 1 pt. PbSO4 1.0519 1.0800 1.1070 1.1359 1 . 1570 10.602 16.310 22.010 27.525 31.602 681.89 281 . 73 105.65 47.30 35.03 (Rodwell, Chem. Soc. 16. 59.) Solubility of PbSO 4 in HCl+Aq at t. (Millimols. per 1.) t 0.1N 0.2N 0.3N 0.4N 18 0.126 1.72 2.67 3.63 25 0.144 2.07 3.14 4.29 37 0.183 2.63 4.06 5.43 (Beck and Stegmuller, Arb. K. Gesund. Amt. 1910, 34. 446.) Above measurements in HCl+Aq show solubility directly proportional to the hydro- gen ions. (Beck and Stegmuller.) Sol. in HNO 3 +Aq, and more sol. in hot or cone, than in cold or dil. HNO 3 +Aq. Sol. in 172 pts. HNO 3 +Aq of 1.144 sp. gr. at 12.5. (Bischof.) Pptd. from HNO 3 solution by dil. H 2 SO 4 + Aq and not by H 2 O. (Bischof, 1827.) Solubility of PbSO 4 in HNO 3 +Aq. Sp. gr. of HNOa+Aq 1.079 1.123 1.250 1.420 % HNOs in HNOs+Aq 11.55 17.50 34.00 60.00 Pts. HNOs+Aq for 1 pt. PbSO4 303.10 173.75 127.48 10282.78 (Rodwell, Chem. Soc. 16. 59.) Solubility in HNO 3 at 18. (Millimols per 1.) HNOs 0.1N 0.2N 0.3N 0.4N PbS0 4 0.506 0.844 1.13 1.44 (Beck and Stegmuller.) Sol. in 36,504 pts. dil. H 2 SO 4 +Aq. (Fre- senius.) See also under solubility in alcohol. SI. sol. in cone. H 2 SO 4 , from which it is partially pptd. by H 2 O or completely by alcohol. (Fresenius.) 100 pts. cone. H 2 SO 4 dissolve 6 pts. PbSO 4 . (Schultz, Pogg. 133. 137.) Cone. H 2 SO 4 dissolves 0.005 pt. PbSO 4 . (Ure.) 100 pts. H 2 SO 4 dissolve 0.13 pt. PbSO 4 , and 100 pts. fuming H 2 SO 4 dissolve 4.19 pts. (Struve, Z. anal. 9. 31.) More sol. in commercial H 2 SO 4 than in the more cone. acid. (Hayes.) 100 pts. H 2 SO 4 +Aq of 1.841 sp. gr. dissolve 0.039 pts. PbSO 4 ; of 1.793 sp. gr. dissolve 0.011 pt. PbSO 4 ; of 1.540 sp. gr. dissolve 0.003 pt. PbSO 4 . Presence of SO 2 does not increase the solu- bility; HNO 3 increases the solubility some- what, i. e., 100 pts. H 2 SO 4 +Aq of 1.841 sp. gr. with 5 pts. HNO 3 of 1.352 sp. gr. dissolve 0.044 pt. PbSO 4 ; 100 pts. H 2 SO 4 of 1.749 sp. gr. with 5 pts. HNO 3 of 1.352 sp. gr. dissolve 0.014 pt. PbSO 4 ; 100 pts. H 2 SO 4 of 1.512 sp. gr. with 5 pts. HNO 3 of 1.352 sp. gr. dissolve only a trace. Nitrous oxides do not increase the action. (Kolb, Dingl. 209. 268.) Solubility in dil. H 2 SO 4 +Aq at 18. (G. per 1.) 0.0049 0.0098 PbS0 4 0.0382 0.0333 0.0306 H 2 S0 4 0.0245 0.0490 0.4904 PbS0 4 0.0194 0.0130 0.0052 (Pleissner, Arb. K. Gesund. Amt. 1907, 26. 384.) A trace of H 2 SO 4 has a considerable effect in reducing the solubility of PbSO 4 in H 2 0. (Sehnal, C. R. 1909, 148. 1395.) Solubility in dil. H 2 SO 4 +Aq at 20. (G. per 1.) H 2 SO 4 0.0098 0.0196 PbS04 0.082 0.051 0.025 H 2 SO 4 0.0980 0.4900 0.9800 PbS0 4 0.013 0.006 (Sehnal.) Pptd. from solution in H 2 SO 4 by HCl. (Bolley, A. 91. 113.) Not more insol. in dil. HC 2 H 3 O 2 +Aq than in H 2 O. (Bischof.) Solubility in other acids is prevented by great excess of H 2 SO 4 . (Wackenroder.) Sol. in warm NH 4 OH+Aq, separating on cooling. Completely sol. in warm K.OH or NaOH+Aq. SULPHATE, LEAD 981 Decomp. by boiling with K 2 CO 3 , Na 2 CO 3 , and (NH 4 ) 2 CO 3 +Aq. Sol. in NH 4 salts +Aq, but repptd. by H 2 SO 4 +Aq. (Fresenius, A. 69. 125.) The best solvents of the NH 4 salts are the nitrate, citrate, and tartrate; the two latter should be strongly alkaline with NH 4 OH+Aq. ( Wackenroder . ) Sol. in NH 4 Cl+Aq at 12.5-25. SI. decomp. by NaCl+Aq. (Bley.) 1 1. sat. NaCl +Aq dissolves 0.66 g. PbSO 4 . (Becquerel.) Sol. in 100 pts. cold cone. NaCl+Aq, and PbCl 2 is deposited after a few hours. (Field.) Solubility in ammonium acetate +Aq at 25. NH 4 C 2 H302 Millimol. per. 1. Solubility of PbSO4 Millimols. per 1. g. per 1. 0.0 103.5 207.1 414.1 0.134 2.10 4.55 10.10 0.041 0.636 1.38 3.06 Solubility of PbSO 4 in NaCl+Aq at 18. (Millimols per 1.) oouu pnase, jruov^f .ru-LY 2 ^ow 4 j2. Composition of the solutions NaCl PbS0 4 7 KC 2 H 3 O 2 % Pb(C 2 H 3 2 ) 2 % KC 2 H 3 2 Pb(C 2 H 3 O 2 ) 2 0.1N 0.2N 0.3N 0.4N 0.546 0.904 1.28 1.68 4.33 9.03 17.81 22.07 2.54 3.55 5.43 5.95 26.58 28.82 28.93 9.83 11.40 19.41 (Beck and Stegmiiller, Arb. K. Gesund. Amt. 1910, 34. 446.) (Fox, Chem. Soc. 1909, 95. 887.) Sol. in Fe 2 Cl 6 -t-Aq. (Fresenius, Z. anal 19. 419.) Sol. in Na 2 S 2 O 3 +Aq. (Lowe.) Sol. in (NH 4 ) 2 SO 4 +Aq. (Rose.) Solubility of PbSO 4 +PbSO 4 , K 2 SO 4 in H 2 O 22 g. in 100 cc. of solution 0.195 0.396 Mol. in 100 cc. of solution 0.0112 0.0227 Solid phase K 2 SO 4 , PbSO 4 +PbSO 4 (Bronsted, Z. phys. Ch. 1911, 77. 316.) Sol in 47 pts. NH 4 C 2 H 3 O 2 +Aq) 1.036 sp, gr.), and 969 pts. NH 4 NO 3 +Aq (1.269 sp. gr.): from the solution in NH 4 C 2 H 3 O 2 it is pptd. by H 2 SO 4 or K 2 SO 4 ; from solution in NH 4 NO 3 by K 2 SO 4 , but not by H 2 SO 4 . (Bischof.) Sol. in acetates of NH 4 , Na, K, Ca, Al, and Mg. (Mercer.) Solubility in NH 4 C 2 H 3 O 2 +Aq. Excess o PbSO 4 was boiled with solution o NH 4 C 2 H 3 O 2 +Aq of varying cone. G. NH4.C 2 H 3 2 in 100 cc. g. PbSO4 contained in 5 cc.solution Hot Cooled Cooled 24 hrs. 28 30 32 35 37 40 45 0.356 0.418 0.494 0.513 0.529 0.539 0.555 0.451 0.452 0.488 0'.224 0.242 0.238 0.263 (Dunnington and Long, Am. Ch. J. 1899, 22. 218.) Noyes and Whitcomb, J. Am. Chem. Soc. 1905, 27. 756.) Solubility in KC 2 H 3 O 2 +Aq at 25. 100 pts. H 2 containing a drop of HC 2 H 3 O 2 and 2.05 pts. NaC 2 H 3 O 2 dissolve 0.054 pt. PbSO 4 ; containing 8.2 pts. NaC 2 H 3 O 2 dis- solve 0.900 pt. PbSO 4 ; containing 41.0 pts. NaC 2 H 3 O 2 dissolve 11.200 pts. PbSO 4 . Dibbits, Z. anal. 1874, 13. 139.) Solubility in NaC 2 H 3 O 2 +Aq at 25. Composition of the solutions % Na acetate % PD acetate % 6.69 11.76 16.90 19.92 21.51 6.95 0.78 2.73 5.70 8.24 10.75 0.81 0.34 1.26 2.49 3.60 4.68 0.35 %H 2 92.19 84.25 74.91 68.24 63.10 91.90 The proportion of sulphate in solution in each case corresponded with the amount of Pb present, but was calculated to sodium sulphate, since Na 2 SO 4 +10H 2 O cryst. from the solutions on cooling. The solid phase in these solutions was PbSO 4 . (Fox, Chem. Soc. 1909, 96. 887.) Sol. in Mn(C 2 H 3 O 2 ) 2 , Zn(C 2 H 3 O 2 ) 2 , Ni(C 2 H 3 O 2 ) 2 , and Cu(C 2 H 3 O 2 ) 2 , but not in Hg(C 2 H 3 O 2 ) 2 or AgC 2 H 3 O 2 +Aq. Solubility in KC 2 H 3 O 2 +Aq is not less than that in NaC 2 H 3 O a +Aq. (Dibbits, Z. anal. 13. 137.) Insol. in Pb(C 2 H 3 O 2 ) 2 -hAq. (Smith.) Sol. in basic lead acetate +Aq, but not in neutral Pb(C 2 H 3 O 2 ) 2 +Aq. (Stammer, Z. anal. 23. 67.) 12.2 pts. Ca(C 2 H 3 O 2 ) 2 in very dil. solution dissolve 1 pt. PbSO 4 . (Stadel, Z. anal. 2. 180.) Sol. in Al(C 2 H 3 O 2 ) 3 +Aq. (Lennsen.) 982 SULPHATE, LEAD HYDROGEN Very easily and abundantly sol. in NH tartrate +Aq. (Wohler, A. 34. 235.) Even when native, easily sol. in NH 4 citrate +Aq. (Smith.) Insol. in alcohol (18%) and H 2 SO 4 when NH 4 acetate, K tartrate, or NH 4 succinate are present. Insol. in alcohol (18%) and H 2 SO or (NH 4 ) 2 SO 4 when Na acetate, Na or NH 4 oxalate are present. Sol. in NH 4 cfo'citrate anc K Zricitrate in presence of H 2 SO 4 ; in NH 4 succinate and NH 4 acetate in presence oi (NH 4 ) 2 SO 4 ; and in NH 4 citrate in presence of H 2 SO 4 or (NH 4 ) 2 SO 4 . (Storer, C. N. 21. 17. Alcohol (59%) alone, or with ethylsul- phuric acid or sugar, does not dissolve Pb by 3 months action. (Storer.) Insol. in acetone. (Naumann, B. 1904 37. 4329); methyl acetate. (Naumann B. 1909, 42. 3790); ethyl acetate. (Naumann B. 1910, 43. 314.) Min. Anglesite. Sol. in cold citric acid +Aq (Bolton, C. N. 37. 14.) Lead hydrogen sulphate, PbSO 4 , H 2 S0 4 +H 2 O, Decomp. by H 2 O. Lead p^/rosulphate, Pb S 2 O 7 . Decomp. by H 2 O.(Schultz.) Lead potassium sulphate, PbSO 4 , K 2 SO 4 . When PbSO 4 is added to potassium acetate +Aq at 25 a double salt,, PbK 2 (SO 4 ) 2 is formed. This salt is insol. in the solution which contains only potassium acetate and lead acetate. (Fox, Chem. Soc. 1909, 96. 882.) Decomp. by H 2 O. Stable only in solutions of K 2 S0 4 , containing at least 0.56% K 2 SO 4 at 7; 0.62% at 17; 1.09% at 50; 1.37% at 75: 1.69% at 100. (Barre, C. R. 1909, 149. 294.) Lead sulphate chloride, PbSO 4 , 2PbCl 2 + H 2 O. Insol. in H 2 O or NaCl+Aq. (Becquerel, C. R. 20. 1523.) Lead sulphate fluoride, PbSO 4 , 2PbF 2 . Sat. Li 2 SO 4 +Aq contains at: 20 16 15 12 18.4 22.5 22.6 24.4 % Li 2 SO 4 . -4 +15 +90 25.7 25.3 23.9 % Li 2 SO 4 . (Etard, A. ch. 1894, (7) 2. 547.) Sat. solution boils at 105. (Kremers.) Sp. gr. of Li 2 SO 4 +Aq at 19.5 containing: 6.5 7.4 12.5 15.3%Li 2 SO 4 , 1.05 1.06 1.098 1.118 22.6 24.4 1.167 1.178 (Kremers, Pogg. 114. 47.) 29.4 %Li 2 SO 4 . 1.208 Sp. gr. of Li 2 SO 4 +Aq at 15 containing 5% Li 2 SO 4 = 1.0430; 10% Li 2 SO 4 = 1.0877. (Kohlrausch, W. Ann. 1879 1.) Sp. gr. of Li 2 S0 4 +Aq at 25. Concentration of Li2SC>4 +Aq Sp. gr. 1 normal V " V4 " Vr- " 1.0453 1.0234 1.0115 1.0057 (Wagner, Z. phys. Ch. 1890, 6. 38.) Sp. gr. of Li 2 SO 4 +Aq. ^Li 2 S0 4 g. in 1000 g.l of solution (2J Sp. gr. 16/16 2.9198 16.0461 1.000000 1.002589 1.014093 (Dijken, Z. phys. Ch. 1897, 24. 109.) Sp. gr. of Li 2 SO 4 +Aq at 20. 434.) Lithium sulphate, Li 2 SO 4 . More sol. in cold than in hot H 2 O. 100 pts. H 2 O dissolve 34.6 pts. Li 2 SO4 at 18. (Witt- stein.) 100 pts. H 2 O dissolve pts. Li 2 SO 4 at t Normality of Li 2 S0 4 +Aq % Li 2 S0 4 Sp. gr. 2.60 1.96 1.708 1.320 0.747 23.48 18.53 16.41 13.01 7.71 1.2330 1 . 1650 1 . 1449 1.1133 1.0678 (Forchheimer, Z. phys. Ch. 1900, 34. 24.) Insol. in SO 3 . (Weber, B. 17. 2497.) 10 ccm. of sat. Li 2 SO 4 in absolute H 2 S0 4 contain approx. 2.719 g. Li 2 SO 4 . (Bergius, Z. phys. Ch. 1910, 72. 355.) t Pts. Li 2 SO4 t Pts. Li 2 S0 4 t Pts. Li 2 SO4 20 35.34 34.36 45 65 32.38 30.3 100 29.24 (Kremers, Pogg. 95. 468.) SULPHATE, LITHIUM THALLIC Solubility in H 2 SO 4 +Aq at 30. Solubility of Li 2 SO 4 in alcohol +Aq at 30. Composition of the solution Solid phase Li 2 SU 4 , H 2 U. % H b 2Sof' \SSo7" Solid phase G. per 100 g. sat. solution C 2 H 5 OH T ' SO 12 4 P H OH T ' SO 12 4 5 .05 22 .74 Li 2 SO 4 , H 2 O 2 5 12 .23 20 .45 25.1 47.28 3.04 15 .37 19 .11 11.75 16.16 58.59 1.22 16 .60 19 .10 21.19 11.52 69.39 0.4 32 .70 13 .37 29.40 8.17 80.74 36 A O .90 11 i r\ .90 ri-r 33.31 6.66 94.11 42 48 .98 .00 10 10 .57 .20 (Schreinemakers and van Dorp, Chem. 52 .72 11 .44 Weekbl. 1906. 3. 557.) 54 .54 12 .92 55 .08 13 .69 Li 2 SO 4 56 .30 13 .87 Insol. in methyl acetate (Naumann, B. 61 .46 17 .10 1909, 42. 3790); ethyl acetate (Naumann. 61 .82 17 .00 B. 1904, 37 . 3601) ; acetone. (Eidmann, C. C, 62 62 .14 .49 17 18 .97 .89 Li 2 SO 4 H 2 SO 4 1899, II. 1014; Naumann, B. 1904, +H 2 O. Very si. efflorescent. 37. 4329.) (Rammels- 65 .70 16 .55 berg.) 69 .40 13 .75 Aq. solution contains 25.1% Li 2 SO 4 at 30. 77 .30 11 .31 (Schreinemakers, C. C. 1910, I. 1801); 24.3 78 .23 11 .64 g. at 50. (Schreinemakers and Cocheret. 81 .20 13 .28 Chem. Weekbl. 1905, 2. 771.) 81 .70 13 .85 82 .30 15 .50 83 .43 . 15 .65 Lithium hydrogen sulphate, LiHS0 4 . (Van Dorp, Z. phys. Ch. 1910, 73. 289.) Solution in H 2 SO 4 contains 17.2% Li 2 SO 4 at 30. (Van Dorp, Z. phys. Ch. 1913, 86. 112.) Solubility of Li 2 SO 4 +Th(SO 4 ) 2 in H 2 O at' 25. Solid phase, Th(SO 4 ) 2 . G. in 100 g. H 2 O. Li 2 S0 4 Th(S04) 2 Li 2 S04 Th(S0 4 )2 0.0 2.57 4.93 6.98 9.23 1.722 4.13 6.20 7.95 9.68 11.13 13.18 16.12 20.49 16.92 11.05 12.54 14.52 16.92 18.87 (Barre, Bull. Soc. 1912, (4) 11. 647.) Easily sol. (Kastner), si. sol. (Berzelius) in alcohol. Cryst. from H 2 SO 4 . (Gmelin.) LiH 3 (SO 4 ) 2 . Cryst. from H 2 SO 4 . (Schultz, Pogg. 133. 137.) Li 2 SO 4 , 7H 2 SO 4 . (Bergius, Z. phys. Ch. 1910, 72. 355.) Lithium potassium sulphate, Li 2 SO 4 ,K 2 SO 4 . This is the only compd. of Li 2 SO 4 and K 2 SO 4 which exists below 100. (Spielrein, C. R. 1913, 157. 48.) K 4 Li 2 (SO 4 ) 3 . (Knobloch.) Has the for- mula K 2 Li 8 (SO 4 ) 5 +8H 2 O, according to Ram- melsberg. Lithium sodium sulphate, Na 3 Li(SO 4 ) 2 + 6H 2 O. Na 4 Li 2 (SO 4 ) 3 +9H 2 O. Na 2 Li 8 (SO 4 ) 5 +5H 2 O . (Rammelsberg. ) Do not exist. (Troost.) Li 2 SO 4 , Na 2 SO 4 +5.5H 2 O. Exists from 0-16. +3H 2 O. Exists from 32-100. Li 2 SO 4 , 3Na 2 SO 4 +12H 2 O. Exists from 16-24. 4Li 2 SO 4 , Na 2 SO 4 +5H 2 O. Exists from 24-32. (Spielrein, C. R. 1913, 167. 47.) Lithium thallic sulphate, LiTl(SO 4 ) 2 +3H 2 O. (Meyer and Goldschmidt, C. C. 1903, I. 495.) 984 SULPHATE, LITHIUM TITANIUM Lithium titanium sulphate, Li 2 TiO 2 (SO 4 ) 2 +7H 2 O. Less hygroscopic than K compound. (Mazzuchelli and Pontanelli, C. C. 1909, II. 420. Lithium uranyl sulphate, Li 2 SO 4 , UO 2 SO 4 + 4H 2 O. (de Coninck, Chem. Soc. 1905, 88. (2) 530. Magnesium sulphate basic, 6Mg(OH) 2 , MgSO 4 +3H 2 O. SI. sol. in cold or hot H 2 O. Sol. in HCl+Aq. (Thugutt, Z. anorg. 1892, 2. 150.) Magnesium sulphate, MgSO 4 . Anhydrous. Very slowly sol. in H 2 O; sol. in hot cone. H 2 SO 4 , less in HC1, and HNO 3 + Aq. +H 2 O. Min. Kieserite. Easily sol. in warm, but slowly dissolved by cold H 2 O. 100 g. sat. solution at 83 contain 40.2 g. MgSO 4 . (Geiger, Dissert. 1904.) +6H 2 O, and +7H 2 O. The latter exists in two modifications; (a) hexagonal, and (6) the ordinary or rhombic salt. MgSO 4 +Aq, which on cooling or keeping in closed vessels has deposited MgSO 4 +6H 2 O, always contains for 100 pts. H 2 O at: 10 20 40.75 42.23 43.87 pts. MgS0 4 . If only hexagonal MgSO 4 +7H 2 has been deposited, then the mother liquor contains for 100 pts. H 2 O at: 10 20 34 . 67 38 . 71 42 . 84 pts. MgSO 4 . Solutions prepared from rhombic MgSO 4 + 7H 2 O contain for 100 pts. H 2 O at: 10 20 26.0 30.9 35. 6 pts. MgSO 4 . (Lowel.) These results may be given in tabular form as follows: Temp. A sat. aqueous solution of MgSO4+7H 2 O (a) contains for 100 pts. H 2 O Anhydrous MgSO4 7H 2 O (a) sale 34.67 111.74 10 38.71 133.67 20 42.84 159.61 Temp. A sat aqueous solution of MgSC>4 +6H2O contains for 100 pts. HzO Anhydrous MgSCU 6H 2 salt 7H 2 salt 40.75 122.22 146.02 10 42.32 129.44 155.53 20 43.87 137 . 72 167.97 It is seen from table that at the same temp, the 6H 2 O salt is more sol. than the 7H 2 O (6) salt, and the latter is more sol. than 7H 2 O (a) salt; that the solubility of the 7H 2 O (6) salt increases rapidly from to. 20; that the 6H 2 O salt is not much more sol. at 20 than at 0, and at 20 the 7H 2 O (6) salt is nearly as sol. as the 6H 2 O salt. (Lowel, A. ch. (3) 43. 405.) 100 pts. H 2 O at t dissolve pts. MgSO4. G L = accord- ing to Gay-Lussac (A. ch. (2) 11. 311); T =accord- ing to Tobler (A. 95. 198). t G L T t G L T 10 20 25 30 40 25.8 30.5 35.0 39! 8 45.2 24.7 37.1 50 55 60 70 80 90 49.7 55.9 60.4 65.1 70.3 52^8 100 pts. H 2 O at 105.5 dissolve 135.2 pts. MgSO4. (Griffiths.) MgSO4+Aq sat. at 17.5 has sp. gr. =1.2932, and contains 55.57 % MgSO4+7H 2 O, or 100 pts. H 2 O dissolve 125.06 pts. MgSO4+7H 2 O, or 60 pts. MgSO4, at 17.5. (Karsten.) 100 pts. H 2 O at dissolve 53.8 pts., and 125 pts. at ord. temp. (Otto-Graham.) Sol. in 2 pts, cold, and 0.5 pt. boiling H 2 O. (Four- croy.) The aqueous solution contains for 100 pts. H 2 O 92.217 pts. MgSO 4 +7H 2 O at 15. (Michel and Krafft.) I pt. MgS0 4 +7H0 is sol. in 0.933 pt. H 2 O at 15 (Gerlach); in 0.92 pt. H 2 O at 23 (Schiff). 100 pts. H 2 dissolve 28.067 pts. MgSO 4 at 0. (Pfaff, A. 99. 224.) 100 pts. H 2 O dissolve pts. MgSO 4 at t. Temp. A sat. aqueous solution of MgSO4+7H 2 O (6) contains for 100 pts. H 2 O t Pts. MgS0 4 17.9 24.1 26.37 33.28 35.98 Anhydrous MgS0 4 7H 2 O (6) salt 26.0 73.31 (Diacon, J. B. 1886. 62.) 100 pts. MgSO 4 +Aq sat. at 18-20 contain 25.67-26.38 pts. MgSO 4 . (v. Hauer, J. pr. 98. 137.) 10 30.9 93.75 20 35.6 116.54 SULPHATE, MAGNESIUM 985 Solubility in 100 pts. H 2 O at t, using MgSO 4 +7H 2 O. M.-pt. of MgSO 4 +7H 2 O is 70. (Tilden, Chem. Soc. 46. 409.) Pts. Pts. Pts. t MgSC>4 t MgSO* t MgSO4 MgSO 4 +Aq with sp. gr. 1.50 contains 44.4 % MsSO 4 ; sp. gr. 1.42, 39%; sp. gr. 1.30, 30% MgSOi. 26.9 37 44.2 74 61.4 (Dalton.) 1 27.4 38 44.7 75 61.9 2 3 27.9 28.3 39 40 45.2 45.6 76 77 62.3 62.8 Sp. gr. of MgSO 4 +Aq sat. at 15 = 1.275 (Michel and Krafft); at 8 = 1.267 (Anthon); 4 28.8 41 46.1 78 63.2 at 18.75 = 1.293 (Karsten.). 5 29.3 42 46.5 79 63.7 6 29.7 43 47.0 80 64.2 7 30.2 44 47.5 81 64.6 Sp. gr. of MgSO 4 +Aq at 15. 8 30.6 45 48.0 82 65.1 9 31.1 46 48.4 83 65.6 % MgS04 Sp. gr. % MgSO4 Sp. gr. in 01 K 47 4.0 Q 04. fifi j.\J 11 Ol . O 32.0 T: * 48 ^O . i) 49.3 OT: 85 oo . u 66.5 5 1.054 30 1.326 12 32.4 49 49.8 86 67.0 10 1.108 35 1.384 13 32.9 50 50.3 87 67.5 15 1.161 40 1.446 14 33.4 51 50.7 88 68.0 20 1.215 45 1.511 15 33.8 52 51.2 89 68.4 25 1.269 50 1.580 16 .4- . CO ci 7 on AQ q -LU 17 18 OT: . O 34.7 35.2 oo 54 55 O-L . t 52.2 52.7 7H 2 O), ZnSO 4 , 7H 2 O and MgSO 4 , 7H 2 O, ZnSO 4 . 7H 2 O. (Hollmann, Z. phys. Ch. 1901, 37. 212, and 1902, 40. 577. Magnesium sulphate potassium chloride, MgSO 4 , KC1+3H 2 O or MgSO 4 , K 2 SO 4 , MgCl 2 +6H 2 O. Min. Kainite. 100 pts. H 2 O dissolve 79.56 pts. at 18. (Krause, Arch. Pharm. (3) 6. 326.) Not sol. in a mixture of abs. alcohol and ether, which dissolves out MgCl 2 . (Lehmann, J. B. 1867. 416.) Alcohol dissolves out MgCl 2 , also little H 2 O. Much H 2 O dissolves completely. (Zincken, Miner. Jahrb. 1866. 310.) Magnesium sulphate potassium chromate, 2MgSO 4 , K 2 CrO 4 +9H 2 O. Sol. in H 2 O. (fitard, C. R. 86. 443.) 990 SULPHATE, MANGANOUS, BASIC Manganous sulphate, basic, 3MnO. 2SO 3 + 3H 2 O. Insol. in H 2 O, but slowly decomp. therebv. (Gorgeu, C. R. 94. 1425.) Manganous sulphate, MnSO 4 . Anhydrous. Absorbs H 2 O from the air to form MnSO 4 +4H 2 O. l.pt. MnSO 4 is sol. in pts. H 2 O at t. 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +H 2 O at t. t Pts. MnSO 4 t Pts. MnSO 4 Pts. MnSO 4 48 53 65 72 87.98 86.10 84.33 82.73 78 90 100 106 79.13 1 75.63 1 71.27 70.14 15 69.78 17 68.81 t Pts. H 2 t Pts. H 2 O t Pts. H 2 (Linebarger.) Min. Szmikite. Solubility of MnSO 4 +H 2 O in H 2 O at t. 6.25 10 1.77 1.631 18.75 37.5 1.667 T457 75 101.25 1.494 2.031 Or 100 pts. H 2 O dissolve pts. MnSO 4 at t. t Pts. per MnSO 4 100 pts. H 2 t Pts. MnSO 4 per 100 pts. H 2 t 6.25 10 Pts. MnS0 4 t Pts. MnSO 4 t Pts. MnS0 4 41. 50. 67. 5 1 1 61.06 58.01 51.37 75 84.8 95 99.6 49.45 44.87 38.71 34.27 56.49 61.29 18.75 37.5 60.00 68.63 75 101.25 66 . 95 49.33 (Brandes, Pogg. 20. 575.) Sol. in 2.5 nts H^O at 18 75 nt (\9 Z it i rliffir-iilt to dissolve 1 pt. MnSO 4 in 3 pts. H 2 O, but the sat. solution at 62.5 does not become cloudy on heating to 100. (Jahn.) 100 pts. MnSO 4 +Aq sat. at 11-14 contain 37.5 pts. MnSO 4 . (v. Hauer, J. pr. 103. 114.) Sat. MnSO 4 +Aq contains at: 8 5 +5 18 22 30.0 31.0 34.1 38.3 38.2% MnSO 4 , 23 32 45 52 70 39.1 41.7 44.2 36.4 41.1%MnSO 4 , 83 110 115 123 130 140 36.3 18.4 21.5 16.7 13.6 9.4% MnSO 4 . (Etard, A. ch. 1894, (7) 2. 553.) Solubility in H 2 O increases from 0-55, and decreases from 55-145. The increasing solu- bility is that of MnSO 4 +5H 2 O, and MnSO 4 + 2H 2 O separates out at 35, and is completely insol. at 145. (fitard.) If solubility S=pts. anhydrous MnSO 4 in 100 pts. solution, S = 30.0+0.2828t from 8 to 57; S =48.0-0.4585t from 57 to 150. Practically insol. in H 2 O at 180. (fitard, C. R. 106. 208.) Solubility varies according to the hydrate used. Above results of Etard show the solu- bility of MnSO 4 +7H 2 O at 0, and MnSO 4 + 3H 2 O at 57. Anhydrous MnSO 4 is stable only above 117. (Linebarger.) 100 pts. H 2 O dissolve pts. anhydrous MnSO 4 att. t Pts. MnS0 4 t Pts. MnS0 4 t Pts. MnSO 4 120 132 67.18 63.16 141 146 41.18 38.83 155 170 26.49 16.15 (Linebarger, Am. Ch. J. 15. 225.) +H 2 O. Stable only between 57 and 117 C Av. of varying results. (Cottrell, J. phys. Ch. 1900, 4. 652.) Linebarger's determinations are inaccurate. (Cottrell.) +2H 2 O. Stable between 40 and 57. 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +2H 2 O at t. t Pts. MnSO 4 t Pts. MnSO 4 t Pts. MnSO 4 35 40 68.88 75.31 42 45 77.63 80.07 50 55 83.16 86.27 (Linebarger.) -f 3H 2 O. Stable between 30 and 40. 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +3H 2 O at t. t Pts. MnS0 4 t Pts. MnSO 4 t Pts. MnSO 4 5 12 16 19 54.68 60.56 63.41 65.12 25 30 35 40 66.85 67.38 68.31 70.63 68 53 57 71.89 72.81 73.17 (Linebarger.) +4H 2 O. SI. efflorescent. Less sol. in boil- ing than in cold H 2 O. 100 pts. H 2 O at 4.4 dissolve 31 pts. MnSO 4 +4H 2 O. (Jahn.) SULPHATE, MANGANOUS 991 100 pts. H 2 O at t dissolve pts. MnSO4+4H 2 O. Solubility of MnSO 4 +4H 2 O in H 2 O at t. Pts. t MnSO 4 + 4H 2 t % Pts. MnSO 4 + 4H 2 O Pts. MnSO 4 t per 100 pts. H 2 t Pts. MnSO 4 per 100 pts. H 2 6.25 113.22 10 123 18.75 122 37.5 75 101.25 149 144 93 16.0 63.97 17.7 64.16 18.5 64.19 25.0 65.32 30.0 66.43 32.2 66.83 35.0 35.5 39.9 49.9 50.0 67.87 68.09 68.81 72.48 72.62 (Brandes, Pogg. 20. 575.) Solubility of MnSO 4 in 100 pts. using MnSO 4 +4H 2 O. H 2 O at t, t Pts. MnSO4 t Pts. MnSO 4 t Pts. MnS0 4 (Cottrell, J. phys. Ch. 1900, 4. 651.) Linebarger's determinations are inaccu- rate. (Cottrell.) Solubility in H 2 O at t. 1 2 3 4 5 6 . 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 55.4 55.9 56.5 57.1 57.7 58.2 58.8 59.4 60.0 60.5 61.1 61.7 62.2 62.7 63.3 63.8 64.3 64.8 65.3 65.8 66.3 66.7 67.2 67.6 68.1 68.5 68.9 69.3 69.7 70.0 70.4 70.7 71.0 71.3 71.6 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 63.5 64 65 66 67 68 69 71.9 72.2 72.4 72.7 72.9 73.1 73.3 73.5 73.7 73.9 74.0 74.2 74.4 74.6 74.7 74.8 74.9 75.1 75.2 75.3 74.7 74.0 72.9 71.5 69.5 65.9 61.'3 61.5 61.5 61.5 61.5 61.5 61.5 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 87 88 89 90 91 92 93 94 95 96 97 98 99 100 101 102 102.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.5 61.4 61.3 61.2 61.0 60.8 60.6 60.3 60.0 59.6 59.2 58.6 57.9 57.2 56.3 55.4 54.3 52.9 51.2 49.3 47.4 t g. MnSOi for 100 g. H 2 O 30.15 35 66.38 68.22 (Richards and Fraprie, Am. Ch. J. 1901, 26. 77.) +5H 2 O. Sol. in 1 pt. H 2 O at 18.75. (Jahn, A. 28. 110.) Stable from 8 to 18. 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +5H 2 O at t. f o PtS. ,o MnS0 4 Pts. MnS0 4 t MnSO4 58.05 20 2.5 62.41 25 4 64.22 30 7 66.83 32 10 68.05 34 15 72.33 37 75.16 78.63 79.16 80.38 82.04 83.91 40 84.63 42 85.27 45 86.16 47.7 86.95 53 88.89 54 89.08 (Linebarger.) Stable in aqeous solution between 15 and 20. (Schieber, M. 1898, 19. 281.) Solubility of MnSO 4 +5H 2 O at t. (Mulder, Scheik. Verhandel. 1864. 137. 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +4H 2 O at t. Pts. MnSO 4 t per 100 pts. H 2 t Pts. MnSCU per 100 pts. H 2 t 2.2 7.3 11 15 20 Pts. MnS0 4 t Pts. MnS0 4 t Pts. MnSO 4 57.88 61.78 64.01 67.12 69.93 25 30 35.5 40 45 72.23 74.67 78.81 79.63 83.06 48 52 56 84.33 86.16 88.19 5 58.06 9 59.23 12 60.19 12.3 60.16 15 61.08 16 25 30 31.1 35.5 61.59 64.78 67.76 67.92 71.61 (Linebarger.) Stable in aqueous solution between 25 and 31. (Schieber, M. 1898, 19. 281.) (Cottrell, J. phys. Ch. 1900, 4. 651.) Linebarger's determinations are inaccurate. (Cottrell.) 992 SULPHATE, MANGANOUS Solubility in H 2 O at 25 =65.09 g. MnSO 4 Sp. gr. of MnSO 4 +Aq at 15. for 100 g. H 2 O. (Richards and Fraprie, Am. Ch. J. 1901, 26. 77.) % MnSCU +4H 2 Sp. gr. % MnS0 4 +4H 2 Sp. gr. +6H 2 O. Stable from- 5 to +8. 1 1.006 29 1.208 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +6H 2 O at t. 2 3 4 1.013 1.020 1.025 30 31 32 1.2150 .224 .231 t Pts. Pts. Pts. 5 1.0320 33 .244 t MnSO 4 t MnS0 4 t MnSO 4 6 7 1 1.038 1f\A A 34 O C .250 oc^rri 4 55.87 9 70.88 30 76.24 8 .U44 1.050 65 36 .2579 .268 64.21 15 72.45 34 77.02 9 1.056 37 1.276 3 66.87 20 74.35 35 77.23 10 1.0650 38 1.285 5 67.49 25 75.38 38 7.481 11 i n 1.072 1 H7Q 39 Af\ 1.295 1OPIQQ (Linebarger.) iz 13 14 i .u/y 1.085 1.093 4U 41 42 .oUoo 1.313 1.322 15 1 . 1001 43 1.331 16 1.106 44 1.340 +7H 2 O. Efflorescent. 17 .114 45 .3495 Sol. in less than 0.5 pt, H 2 O at 18.75. 18 .121 46 .360 (Jahn.) 19 .129 47 .370 Stable between - 10 and - 5. 20 .1363 48 .380 21 .144 49 .389 22 .150 50 .3986 100 pts. H 2 O dissolve pts. MnSO 4 from MnSO 4 +7H 2 O at t. 23 24 25 O .160 1.166 1.1751 1 1 Q'i 51 52 53 1.410 1.420 1.430 1 AA.f\ t Pts. MnS04 t Pts. MnSO4 t Pts. MnSO 4 ^O 27 28 I . loo 1.190 1.200 : 55 1 .'4U 1.4514 50.11 53.61 10 59.91 10 -8 50.93 5 54.83 15 64.34 (Gerlach, Z. anal. 8. 288.) 5 51.53 7 56.62 (Linebarger.) Stable in aqueous solution below O c (Schieber, M. 1898, 19. 281.) Solubility of MnSO 4 +7H 2 O in H 2 O at t. Sp. gr. of MnSO 4 +Aq at 23. a=no. of ^ mols. in grms. dissolved in 1000 g. H 2 O; b=sp. gr. if a is MnSO 4 +5H 2 O, K mol. wt. = 120.5; c = sp. gr. if a is MnSO 4 , V> mol. wt. =75.5. t Pts. MnSO 4 per 100 pts. H 2 t Pts. MnSO 4 per 100 pts. H 2 10 5 47.96 56.23 56.38 9 12 14.3 59.33 61.78 63.93 a b c a b c 1 2 3 4 5 1.068 1.128 1.181 1.227 1.269 1.071 1.139 1.202 1.262 1 .320 6 7 8 9 10 1.306 1.341 1.371 1.399 1.426 3.576 1.429 (Cottrell, I. c.) M.-pt. of MnSO 4 +7H 2 O is 54. (Tilden, Chem. Soc. 46. 409.) (Favre and Valson, C. R. 79. 968.) Above table recalculated by Gerlach (Z. anal. 28. 475.) % MnSO 4 +5H2O Sp. gr. % MnS0 4 +5H 2 40 50 Sp. gr. 1.2900 1.3800 10 20 30 1.0630 1 . 1325 1.2070 SULPHATE, MANGANOUS 993 Sp. gr. of MnSO 4 +Aq at 15. a = %; b = Sol. in about 20 pts. boiling H 2 SO 4 , and sp. gr. if a is MnSO 4 ; c = sp. gr. if a is MnSO 4 +4H 2 O; d = sp. gr. if a is MnSO 4 +5H 2 O; e = sp. gr. if a is MnSO 4 + more sol. in boiling H 2 SO 4 +Aq of 1.6 sp. gr. (Schultz, Pogg. 133. 137.) Completely pptd. from solution by HC 2 H 3 O 2 . 7H 2 O. (Persoz.) b c For solubility in (NH 4 ) 2 SO 4 , see under a d e (NH 4 ) 2 S0 4 . 5 10 15 1.0500 .1035 .1605 1.0340 1.0690 1 . 1055 1.0310 1.0630 1.0965 1.0270 .0545 .0830 MnSO 4 +Aq sat. at 10, then sat. with K 2 SO 4 at same temp, contains for 100 pts. H 2 O 16.7 pts. MnSO 4 and 44.3 pts. K 2 SO 4 (IVTiilcl.Gr ^ 20 .2215 1 . 1435 1.1315 .1130 25 .'2870 1 . 1835 1 . 1685 .1440 30 .3575 1.2255 1.2070 .1765 35 1.2695 1.2470 .2105 Solubility of MnSO 4 +Na 2 SO 4 in H 2 O at 35. 40 1.3155 1.2885 .2455 45 rr\ 1.3640 1.3315 1.2815 g. per 100 g. sat. solution 50 55 . . . 1 . 3760 1.3185 1.3565 MnSCU Na 2 SO4 Solid phase (Gerlach, Z. anal. 28. 475.) 39.45 33.92 5.23 MnS0 4 , H 2 Sp. gr. of MnSO 4 -(-Aq at 0. S = pts. MnSO 4 33.06 7.97 MnS0 4 , H 2 O+9MnSO 4 , in 100 pts solution. 10Na 2 SO 4 qo no 7 42 n S Sp. gr. S Sp. gr. O& t/ 31.05 1 * TZA 9.20 9MnS0 4)f 10Na 2 SO 4 16.7450 1 1834 ~~ 5.8295 1.0928 27.67 22.14 10.76 14.28 tt 14.0462 1 1519 6.0172 1.0622 14.58 20.01 u 11.5804 1 1239 3.0865 1.0315 13.96 21.91 f\*\ fT C1/"\ -1 *"k"VT C*/~\ 1 (Charpy, A. ch. Sp. gr. of MnSO 4 +Aq taming r (6) 29. 26.) at room temp, con- 12.19 10.45 7.43 5fiQ 22.49 23.41 26.58 OQ Q1 9MnSO 4 , 10Na 2 SO 4 + MnS0 4 , 3Na 2 S0 4 MnS0 4 , 3Na 2 S0 4 " 11.45 1.1469 18.8 1.2513 22.08 %MnSO 4 . 1.3082 . D7 5.11 2.96 >\J OX 30.52 31.33 MnSO 4 , 3Na 2 SO 4 +Na 2 SO 4 Na 2 S0 4 (Wagner, W. Ann. 1883, 18. 271.) 33 Sp. gr. of MnSO 4 +Aq at 25. (Schreinemakers and Provije, Proc. Ak. Wet. Concentration of +Aq MnSO.. Sp. gr. Amsterdam, 1913, 16. 326.) 1 normal 1.0728 Insol. in liquid NH 3 . (Franklin, Am. Ch. v- 1 . 0365 J. 1898, 20. 828. 1 /4 1 1 1.0179 Anhydrous MnSO 4 in insol. in absolute Vs- (t 1.0087 alcohol. Vie" " 1.0041 1000 pts. alcohol of 0.872 sp. gr. dissolve (Wagner, Z. phys. Ch. 1890, 6. 39.) 6.3 pts. MnSO 4 . Sol. in 50 pts. of 50% alcohol. Insol. in Sp. gr. at 16/4 of MnSO 4 -f Aq. contain- ng 30.819% -MnSO 4 = 1.36267. (Schonrock, 5. phys. Ch. 1893, 11,781.) absolute alcohol. (Brandes, Pogg. 20. 556.) 100 pts. solution saturated at 15 in dil. alcohol containing: Sat. MnSO 4 +Aq boils at 102.4; crust orms at 101.6, and solution contains 48.7 10 50 60 % alcohol, contain 56.25 51.4 2.0 0.66 pts. MnSO 4 +5H 2 O. >ts. MnSOj to 100 pts. H 2 O. .-pt. of MnSO 4 +Aq containing pts. MnSO 4 to 100 pts. H 2 O. i B.-pt. Pts. MnSO 4 B.-pt. Pts. MnSO 4 100.5 101.0 101 .-fr 17.1 32.1 46.2 102.0 102.4 58.9 68.4 (Gerlach, Z. anal. 26. 434.) (Schiff, A. 118. 365.) When MnSO 4 +7H 2 O is boiled with ab- solute alcohol none is dissolved, but MnSO 4 -H3H 2 O is formed. When MnSO 4 +7H 2 O is dissolved in 15-50% alcohol, the liquid separates into two layers, the lower containing less (12-14%) alcohol and more (47-49%) salt; the upper containing 994 SULPHATE, MANGANOUS more (50-55%) alcohol and less (1.3-2.2%) salt. If the alcohol has the above strength (15-50%) the separation takes place at ordin- ary temp., but with 13-14% or 60% or more alcohol, warming is necessary to effect the separation. (Schiff, A. 118. 363.) Solubility of MnSO 4 +H 2 O in alcohol +Aq att. Composition of the solutions sat. with espect to one another. solid mpo salt at t. 30 31 35 37 41 42 43 Alcohol layer % alcohol % MnSO4 45.20 43.90 41.71 38.26 34.01 32.37 31.42 2.49 2.74 3.44 4.84 5.86 6.89 8.51 Water layer % alcohol % MnSO 8.69 8.47 9.24 11.03 11.93 13.57 14.33 30.15 30.10 28.61 26.47 24.97 23.09 22.01 (Schreinemakers and Deuss, Z. phys. Ch 1912, 79.. 559.) Composition of alcohol solutions sat. with MnSO 4 +H 2 O at t. 50 35 30 % H 2 63.74 65.21 65.23 64.83 59.41 61.4 62.13 62.06 62.01 *62.15 *54.85 50.69 50.16 61.4 61.43 61.25 60.78 *61.16 *52.31 44.83 30.95 9.19 % alcohol 6.67 16.02 22.63 36.47 5.50 6.46 7.48 9.24 41.71 47.73 48.27 2.26 5.09 5.96 8.69 45.20 54.19 68.97 90.80 MnSO 4 36.26 28.12 18.75 12.54 4.12 38.6 32.37 31.48 30.51 28.61 3.44 1.58 1.57 38.6 36.31 33.66 *33.26 30.15 2.49 0.98 0.08 0.01 *The solutions also sat. with respect to one another. (Schreinemakers and Deuss.) 50 35 30 water layer % alcohol % MnSO f5.68 17.69 t8.70 fll.85 18.38 *9.24 10.75 15.09 f7.60 *8.69 10.46 11.86 16.18 34.95 30.99 29.20 24.84 29.52 28.61 26.33 21.85 32.40 30.15 27.58 25.75 20.86 alcohol layer % alcohol % MnSO t53.64 145.83 J41.93 f35.15 f42.38 *41.71 36.89 30.06 t50.97 *45.20 40.71 37.54 29.89 0.97 2.19 3.11 5.95 * 3.07 3.44 5.19 9.03 1.74 2.49 3.93 5.20 9.64 (Schreinemakers and Deuss.) fMetastable solutions. *Solutions also sat. with respect to MnSO< H 2 O. Solubility of MnSO 4 +4H 2 O in alcohol +Aq g. H 2 55.86 52.25 49.41 45.34 42.56 g. alcohol 30.03 43.59 47.66 53.00 56.24 MnSO 4 , 4H 2 O 14.11 4.16 2.94 1.66 1.20 (Linebarger, Am. Ch. J. 1892, 14. 380.) Solubility of MnSO 4 +5H 2 O in alcohol+Ac Composition of the solution sat. wit MnSO 4 +5H 2 O. 10 15 17.6 21 25 alcohol layer alcohol MnSO4 37.06 44.56 47.11 53.55 53.09 5.44 2.79 2.22 1.10 1.23 water layer lcohol MnSO4 13.78 9.25 8.53 6.10 6:81 25.25 29.79 30.88 35.05 33.72 Composition of solution sat. with soli substance at 25. % H 2 % alcohol % MnSO4 Solid phase 60.7 *59.47 *45.68 42.05 23.30 6.81 53.09 57.39 76.70 39.3 33.72 1.23 0.56 0.0 MnSO 4 +5H 2 11 a ii MnSO 4 +H 2 *The two liquids are sat. with respect to o another. SULPHATE CUPRIC OXIDE, MANGANOUS 995 Composition of the two solutions sat. with respect to one another at 25. Manganous hydrazine sulphate, MnH 2 (SO 4 ) 2 , 2N 2 H 4 . 1 pt. is sol. in 60 pts. H 2 O at 18. Stable in the air at 100. (Curtius, J. pr. 1894, (2) 50. 331.) Manganous nickel potassium sulphate, MnSO 4 , NiSO 4 , 2K 2 SO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 57.) Water layer Alcohol layer % alcohol % MnS0 4 % alcohol % MnSQ 4 *8.81 8.48 15.02 *33.72 31.51 22.61 *53.09 49.76 32.75 1.23 1.83 8.01 *Also sat. with MnSO 4 , 5H 2 O. (Schreinemakers and Deuss.) Insol. in absolute ether between 5 and 7, and no crystal H 2 O is removed thereby. Insol. in boiling oil of turpentine, but 1 mol. crystal H 2 O is removed from MnSO 4 +4H 2 O (Brandes, Pogg. 20. 568.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.); ethyl acetate. Naumann, B. 1910, 43. 314); acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C.C. 1899, II. 1014.) 100 g. sat. solution in glycol contain 0.5 g. MnSO 4 (de Coninck, Bull. Ac. roy. Belg. 1905. 359.) MnSO 4 +7H 2 O occurs as the min. Mallar- dite. Manganomanganic sulphate, MnO, MnO 2 , 4S0 3 +9H 2 0. Deliquescent. Decomp. by H 2 O. Sol. in little dil. H 2 SO 4 +Aq. (Fremy, C. R. 82. 475.) Manganic sulphate, Mn 2 (SO 4 ) 3 . Extremely deliquescent. Sol. in H 2 O with evolution of heat, and decomposition into a basic sulphate. Behaves similarly with dilute acids . Sol . in traces in cold cone . H 2 SO 4 . Insol. in cold cone. HNO 3 +Aq. Sol. in cone. HCl-f-Aq. Decomp. by absolute alcohol. (Carius, A. 98. 53.) Manganyl sulphate, MnO 2 , SO 3 . Sol. in H 2 SO 4 but solution decomp. if below 40-60 Baume. Solubility in 40 Baume acid = 15%: 55, 4-5%. Solution can be heated to 60-80 without decomp. (Bad. Anilin u. Sodafabrik, C. C. 1905, II. 1398.) Manganous hydrogen sulphate. MnSO 4 is sol. in 20 pts. boiling cone. H 2 SO 4 ; more sol. in boiling H 2 SO 4 +Aq of 1.6 sp. gr. (Schultz.) MnH 2 (SO 4 ) 2 , and+H 2 O. Sol. in H 2 O with deoomp. (Schultz.) MnH 6 (SO 4 ) 4 . Sol. in H 2 O with decomp. (Schultz.) Manganic hydrogen sulphate, Mn 2 H 2 (SO 4 ) 4 + 8H 2 0. Deliquescent. Decomp. by H 2 O. Sol. in dil. H 2 SO 4 +Aq. (Francke, J. pr. (2) 36. 251.) Manganous potassium sulphate, K 2 SO 4 , MnSO 4 +2H 2 O. +4H 2 O. Efflorescent. (Pierre, A. ch. (3) 16. 239.) 2MnSO 4 , K 2 SO 4 . (Mallet, C. N. 1899, 80. 301.) Manganic potassium sulphate, K 2 Mn 2 (S0 4 ) 4 +24H 2 O. Decomp. by dissolving in H 2 O. (Mitscher- lich.) Manganomanganic potassium sulphate, Mn 5 (SO 4 ) 3 , 5K 2 S0 4 = 3Mn(SO 4 ) 2 , 2MnSO 4 , 5K 2 SO 4 . Decomp. by much H 2 O. Sol. in dil. or cone. H 2 SO 4 . Insol. in alcohol or ether. (Francke, J. pr. (2) 36. 166.) Manganous potassium zinc sulphate, MnS0 4 , 2K 2 SO 4 , ZnSO 4 +12H 2 0. Sol. in H 2 O. (Vohl.) Manganous rubidium sulphate, MnSO 4 , Rb 2 SO 4 +6H 2 O. Sol. in H 2 O. (Tutton, Chem. Soc. 63. 337.) 1 1. H 2 O dissolves 357 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27, 459.) +2H 2 O. (Wyrouboff, Bull. Soc. Min. 1891, 14. 242.) 2MnSO 4 , Rb 2 S0 4 . (Wyrouboff.) Manganic rubidium sulphate, Mn 2 (S0 4 ), Rb 2 SO 4 +24H 2 O. Deliquescent. (Christensen, Z. anorg. 1901, 27. 333.) Manganous sodium sulphate, MnSO 4 , Na 2 SO4. +2H 2 O. Deliquescent in moist air. (Geiger.) +4H 2 O. Sol. in 1.2 pts. boiling H 2 O. (Geiger.) Manganous sulphate ammonia, MnSO 4, 4NH 8 . Decomp. by H 2 O. (Rose, Pogg. 20. 148.) Manganous sulphate cupric oxide, MnSO 4 , 2CuO+3H 2 O. (Mailhe, A. ch. 1902, (7) 27. 392.) MnSO 4 . 3CuO+zH 2 O. (Recoura, C. R. 1901, 132. 1415.) MnSO 4 , 24CuO-fzH 2 O. (Recoura.) 996 SULPHATE HYDRAZINE, MANGANOUS Manganous sulphate hydrazine, MnSO 4 , 2N 2 H 4 . Very unstable. Somewhat sol. in NH 4 OH+Aq. (Franzen, Z. anorg. 1908, 60. 285.) Manganous sulphate hydroxylamine, MnSO 4 , NH 2 OH+2H 2 O. Insol. in H 2 O. (Feldt, B. 1894, 27. 405.) Mercurous sulphate, basic, 2Hg 2 O, S0 8 + H 2 O. Sol. in 25,000 pts. H 2 O at 20. (Gouy, C. R. 1900, 130. 1401.) Mercurous sulphate, Hg 2 SO 4 . Sol. in 500 pts. cold, and 300 pts. hot H 2 O. (Wackenroder, A. 41. 319.) Solubility in H 2 O at 18 = 7.8X10- 4 g. mol. per liter. (Wilsmore, Z. phys. Ch. 1900, 36. 305.) 1 1. H 2 O dissolves 11.71 XHH g.-mol. Hg 2 SO 4 at 25. (Drucker, Z. anorg. 1901, 28. 362.) Solubility in H 2 O at t. t In 100 pts. of the solution Hg 2 SO4 . H 2 S0 4 16.5 33 50 75 91 100 0.055 0.060 0.065 0.074 0.084 0.092 0.008 0.018 0.037 0.063 0.071 0.071 (Barre, A. ch. 1911, (8) 24. 203.) Solubility in H 2 at 25 is 20% greater than at 18 and = 11.71X10- 4 g. mol. per 1. By addition of increasing amts. of H 2 S0 4 the solubility is somewhat, but not regularly, decreased, K 2 SO 4 lowers solubility less than H 2 SO 4 . (Drucker, Z. anorg. 1901, 28. 362.) Easily sol. in dil. HNOs+Aq, from which solution it is separated by dil. H 2 SO 4 +Aq. (Wackenroder, A. 41. 319.) Abundantly sol. in hot, less sol. in cold dil. H 2 SO 4 +Aq. (Berzelius.) Solubility in H 2 SO 4 +Aq at 25. H 2 SO4 normality g.-mol. Hg 2 SO4 per litre 0.0400 0.1000 0.2000 8.31 X 10- 4 8.78 X 10-* 8.04 X 10-* (Drucker, Z. anorg. 1901, 28. 362.) Partially .decomp. by hot NH 4 salts +Aq. (Miahle, A. ch. (3) 6. 179.) . 5 times more sol. in sat. CdSO 4 +Aq than in H 2 O. (Hulett, Phys. Rev. 1907, 26. 16.) Sat. ZnSO 4 or CdSO 4 +Aq attack much less than pure H 2 O, yet the solubility of Hg 2 SO 4 in these solutions is greater, i. e- , 0.8 g. in 1 1. ZnSO 4 +Aq and 1.1 g. in 1 1. CdSO 4 + Aq at 20. (Gouy, C. R. 1900, 130. 1402.) Solubility in 0.2N K 2 SO 4 +Aq = 9.05X10- 4 g. mol. per 1. at 25. (Drucker, Z. anorg. 1901, 28. 362.) Solubility of Hg 2 SO 4 in K 2 SO 4 +Aq. t g. per 100 g. sat. solution K 2 SOi Hg 2 S04 free H 2 SO 4 15 2.90 5.70 8.22 8.77 9.44 0.0475 0.0703 0.0912 0.0994 0.1080 0.0080 0.0093 0.0098 o'.oiio 33 2.94 5.68 8.30 10.70 11.90 0.0677 0.1015 0.1364 0.1724 0.1902 0.0250 0.0350 0.0441 0.0438 0.0420 75 3.10 5.75 8.50 13.20 17.30 0.1344 0.2120 0.2951 0.4610 0.6440 0.1681 0.2135 0.2514 0.2503 0.2225 (Barre, A. ch. 1911, (8) 24. 202.) About 3 times as sol. in sat. ZnSO 4 +Aq as in distilled H 2 O. (Wright, Phil. Mag. (5) 1885, 19. 29.) Mercuric sulphate, basic, 2HgO, SO 3 . (Mailhe, A. ch. 1902, (7) 27. 394.) 3HgO, SO 3 . (Mineral turpeth.} Sol. in 2000 pts. cold and 600 pts. boiling H 2 O. (Fourcroy, A. ch. 10. 307.) Sol. in 43,478 pts. H 2 O at 16 when pptd. cold, and in 32,258 pts. at 16 when pptd. at 100. (Cameron, Z. anal. 19. 144.) SI. sol. in warm dil. H 2 SO 4 +Aq. (Rose.) Solubility in H 2 O is increased by addition of H 2 SO 4 up to an acid content of 4.3 mol. S0 3 to 93.7 mols. H 2 O. (Hoitsema, Z. phys. Ch. 1895, 17. 665.) Sol. in warm cone. HC1 or HBr+Aq. (Ditto.) Sol. in alkali chlorides +Aq. (Miahle.) Sol. in dil. HNO 8 or in HCl+Aq. More easily sol. in the warm acids. (R&y, Chem. Soc. 1897, 71. 1099.) 3HgO, 2SO 3 +2H 2 O. (Hoitsema, Z. phvs. Ch. 1895, 17. 659.) 4HgO, 3SO S . (Hopkins, Sill. Am. J. 18. Mercuric sulphate, HgSO 4 . Decomp. by H 2 O into 3HgO, SO 8 , and a sol. acid salt. Sol. in dil. H 2 SO 4 -f Aq. comp. by all acids. (Berzelius.) De- SULPHATE, MOLYBDENUM 997 Sol. in warm cone. HC1 or HBr+Aq; very si. sol. in boiling cone. HI+Aq. (Ditte, A. ch. (5) 17. 124.) Very si. sol. in hot cone. HF. (Ditte, A. ch. 1879, (5) 17. 125.) Sol. in HCN+Aq. (Mohr.) Sol. with decomp. in NaCl+Aq. (Miahle.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829. Insol. in cone, alcohol. Insol. in acetone. (Naumann, B. 1904, 37. 4329.); methyl acetate. (Naumann, B. 1909, 42. 3790.); ethyl acetate. (Naumann. B. 1910, 43. 314.) Insol. in benzonitrile. (Naumann, B. 1914. 47. 1370.) ' Insol. in pyridine. (Schroeder, Dissert. 1901.) +H 2 O. Decomp. by H 2 O. (Eisfeldt, Pharm. Centr. 1863. 812.) Mercuromercuric sulphate, Hg 2 0, 2HgO, S0 8 . Insol. in cold H 2 O; not decomp. by boiling H 2 O. Decomp. b^HCl+Aq. (Brooke, Pogg. 66. 63.) Hg 2 SO 4 , HgSO 4 . (Baskerville, J. Am. Chem. Soc. 1897, 19. 875.) Mercuric hydrogen sulphate, HgH 2 (SO 4 )2. (Braham, C. N. 42. 163.) Mercuric potassium sulphate, 3HgSO, K 2 SO 4 +2H 2 O. Sol. in H 2 O. (Hirzel, J. B. 1860. 332.) Mercuric sulphate chloride ammonium chloride, 2HgS0 4 , HgC] 2 , 2NH 4 C1. Decomp. with H 2 O. Ether dissolves out HgCl 2 . (Kosmann, A. ch. (3) 27. 238.) Mercuric sulphate cyanide, HgSO 4 , Hg(CN) 2 +5H 2 0. Decomp. by cone, or warm acids. (Rupp, Arch. Pharm. 1912, 260. 280.) Mercuric sulphate hydrazine, HgS0 4 , N 2 H 4 . Ppt. (Hofmann and Marburg, A. 1899, 306. 216.) Mercuric sulphate hydrobromide, HgSO 4 , 2HBr. Sol. in H 2 O without separation of basic sul- phate. (Ditte, A. ch. (5) 17. 122.) 3HgO, SO 3 , 6HBr. Sol. in H 2 O. (Ditte.) Mercuric sulphate hydrochloride, HgSO 4 , HC1. Not attacked by HC1. SI. sol. in HNO 3 . (Baskerville, J. Am. Chem. Soc. 1901, 23. 895.) HgSO*, 2HC1. Sol. in H 2 O without sep- aration of a basic salt. Very sol. in warm H 2 SO 4 , solidifying on cooling if very cone., or crystallising if dil. (Ditte.) Very deliquescent. Very sol. in H 2 O. (Baskerville, J. Am. Chem. Soc. 1901, 23. 895.) +H 2 O. (Baskerville, J. Am. Chem. Soc. 1901, 23. 895.) 3HgO, SO 3 , 6HC1. Sol. in H 2 O. (Ditte.) Mercuric sulphate hydroxylamine. HgSO 4 , 2NH 2 OH+H 2 0. Decomp. by cold H 2 O. (Adams, Am. Ch. J. 1902, 28. 209.) Mercuric sulphate iodate iodide, 6(3HgO, 2S0 8 ), 6HgI 2 , Hg(I0 3 ) 2 . Decomp. by H 2 O and acids. (Bruckner, M. 1907, 28. 961.) Mercuric sulphate iodide, basic, 3HgO, 2SO,, HgI 2 . 3(3HgO, 2SO 3 ), 2HgI 2 + 10H 2 O. 2(3HgO, 2SO 3 ), HgI 2 + 10H 2 O. Very sol. in hot cone. HNOs. 3HgO, 2S0 3 , HgS0 4 , HgI 2 + 10H 2 0. (Ditte, C. R. 1905, 140. 1167.) Mercuric sulphate iodide, HgS0 4 , HgI 2 . Decomp. by H 2 O, not by alcohol or ether. (Riegel, J. B. pr. Pharm. 11. 396.) 3HgSO 4 , HgI 2 . Decomp. by cold or hot H 2 O. Sol. in H 2 SO 4 +Aq. (Ditte, C. R. 1905, 140. 1165.) 4HgSO 4 , HgI 2 + 15H 2 O, and + 18H 2 O. De- comp. by cold or hot H 2 O. Sol. in H 2 SO 4 . (Ditte.) Mercuric sulphate phosphide. See Dimercuriphosphonium mercuric sul- phate. Mercuric sulphate sulphide, basic, 2HgO, S0 3 , HgS. Somewhat sol. in HC1, H 2 SO 4 and HNO 3 . (Jacobson, Pogg. 1846, 68. 412. 4HgO, 3SO 3 , 2HgS+4H 2 O. SI. sol. in H 2 SO 4 . (Estrup, Z. anorg. 1909, 62. 169.) Mercuric sulphate sulphide, 2HgSO 4 , HgS. SI. sol. in hot HC1, H 2 SO 4 , or HNO 3 +Aq. Easily sol. in hot aqua regia. (Jacobson, Pogg' 68. 410.) 2HgSO 4 , HgS. (Palm, C. C. 1863. 122.) HgSO 4 , 2HgS. (Barfoed, J. B. 1864. 282.) Sol. in aqua regia. (Deniges, Bull. Soc. 1915, (4) 17. 355.) HgSO 4 , 3HgS. Insol. in H 2 O. Easily sol. in aqua regia; decomp. by HNO 3 into 3HgSO 4 , HgS. Insol. in all acids except aqua regia. (Spring, A. 199. 116.) Molybdenum sesgwisulphate (?). Basic. Insol. in H 2 O. Neutral. Decomp. by H 2 O into acid and basic salts. Acid. Sol. in H 2 O. (Berzelius.) SULPHATE, MOLYBDENUM Molybdenum cfo'sulphate (?). Sol. in H 2 O. Molybdenum sulphate, Mo 2 O 5 , 2SO 3 . Very slowly sol. in cold, more quickly sol. in hot H 2 O. (Bailhache, C. R. 1901, 132. 476.) 7MoO 3 , 2MoO 2 , 7SO 3 +Aq. (Pechard, C. R. 1901, 132. 630. Molybdic sulphate, MoO 3 , SO 8 . Deliquescent. Sol. in H 2 O. (Schultz- SeUack, B. 4. 14.) MoO 3 , 3SO 3 +2H 2 O. Deliquescent. Par- tially sol. in H 2 O. (Anderson, Berz. J. B. 22. 161.) Does not exist. (Schultz-Sellack.) Molybdenum sulphate ammonia, 5NH 3 , MoO 2 SO 8 , 7MoO 3 +8H 2 O. 3NH 3 , MoO 2 SO 3 , 7MoO 3 + 10H 2 O. Both very sol. in water but less sol. in H 2 O containing ammonium salts. (Pechard, C. R. 1901, 132. 630.) Neodymium sulphate, basic, Nd 2 O 3 , SO 3 . Insol. in H 2 O. Nearly insol. in dil. acids. (Wohler, B. 1913, 46. 1730.) Insol. in H 2 O. (Matignon, C. R .1902, 134. 658.) Neodymium sulphate, Nd2(SO 4 ) 3 +8H 2 O. Solubility in 100 pts. H 2 O at t. t pts. Nd 2 (SO4)s 9.50 16 7.05 30 5.04 50 3.72 80 2.70 100 2.21 (Muthmann and Rolig, B. 1898, 31. 1728.) Neodymium hydrogen sulphate, Nd(S0 4 H) 3 . (Brauner, Z. anorg. 1904, 38. 331.) Neodymium potassium sulphate. Cryst. modification more sol. in cold than in hot H 2 O. (Boudouard, C. R. 1898, 126. 901.) (Berzelius.) (Athanasesco, C. R. Nickel sulphate, basic. Very si. sol. in H 2 O. 6NiO, 5SO 3 +4H 2 O. 103. 271.) 7NiO, 7H 2 O, SO 3 +3H 2 O. Nearly insol. in H 2 O. (Habermann, M. 5. 432.) 5NiO, SO 3 ; 5NiO, 2SO 3 ; and 5NiO, 3SO 3 . (Pickering, Chem. Soc. 1907, 91. 1985.) 6NiO, SO 3 . (Stromholm. C.C. 1906, 1. 1222.) Nickel sulphate, NiSO 4 . 100 pts. H 2 O dissolve pts. N1SO4 at t: 2 16 20 23 31 30.4 37.4 39.7 41 45.3 pts. NiSCh, 41 50 53 60 70 49.1 52 54.4 57.2 " 61.9 pts. NiSO 4 . (Tobler, A. 95. 193.) 100 pts. of sat. solution contain: at 11-14, 28.84; at 18-20, 30.77 pts. anhydrous salt. (v. Hauer, W. A. B. 53, 2. 221.) 100 pts. H 2 O at 112.5 dissolve 185.71 pts. NiSCU. (Griffiths.) NiSO4+7H 2 O is sol. in 3 pts. H 2 O at 12.5. (Tup- PU 100 pts. H 2 O at 15.5 dissolve 75.6 pts. NiSC>4 + 7H 2 0. Sat. NiSO 4 -f-Aq contains at: 3 +2 5 11 17 54 21.7 22.7 23.1 25.2 26.6 33.6% NiS0 4 . 68 74 92 97 110 117 119 38.2 38.7 42.4 44.2 46.5 48.8 49.4% NiSO 4 . (fitard, A. ch. 1894, (7) 2. 552.) See also below under hydrated salts. Sp. gr. of NiSO 4 '+Aq containing g. NiSO 4 + 7H 2 O in 1000 g. H 2 O at 23.5. 140.5 g. ( = Y* mol.) 281 421.5 562 1.073 1.136 1.190 1.238 602.5 1.280 843 1.317 983.5 1.349 1124 1.378 Containing NiSO 4 (anhydrous) : 77.5 g .( = i/ 2 mol.) 155 232.5 310 387.5 465 1.079 1.153 1.224 1.292 1.358 1.421 (Gerlach, Z. anal. 28. 468.) Sp. gr. of NiSO 4 +Aq at 0. S = pts. NiSO 4 in 100 pts. solution; Si = mols. NiSO 4 in 100 mols. solution. s Si Sp. gr. 4.2930 3.9591 3.2845 2.5043 1.6131 0.8327 0.581 0.476 0.392 0.297 0.189 0.097 .0522 .0431 .0357 .0271 .0173 .0089 (Charpy, A. ch. (6) 29. 26.) Sp. gr. of NiSO 4 +Aq at room temp, con- taining: 10.62 18.19 25.35% NiS0 4 . 1.0925 1.1977 1.3137 (Wagner, W. Ann. 1883, 18. 272.) Sp. gr. of NiSO 4 +Aq at 25. Concentration of NiSO4 +Aq Sp.gr 1-normal Vi- " l/ 4 _ l /g- " 1.0773 1.0391 1.0198 1.0017 (Wagner, Z. phys. Ch. 1890, 6. 39.) SULPHATE, NICKEL 999 For solubility of NiSO 4 +Na 2 SO 4 in H 2 O, see under NiSO 4 +7H 2 O and NiNa 2 (SO 4 ) 2 . 100 pts. sat. NiSO 4 +ZnSO 4 +Aq at 18-20 contain 35.45 pts. of the two salts, (v. Hauer.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) HC 2 H 3 O 2 precipitates it completely from aqueous solution. (Persoz.) 100 pts. absolute methvl alcohol dissolve 0.5 pt. NiSO 4 at 18. (de Bruyn, Z. phys. Ch. 10. 783.) Solubility of NiSO 4 , 3CH 4 O+3H 2 O in methyl . alcohol at 14. P = % anhydrous NiS0 4 in the sat. solu- tions. +6H 2 O. Two modifications. a-blue, tetragonal; /3-green, monoclinic. Solubility of a- NiSO 4 , 6H 2 O in H 2 at t. Salt used t g. N1SO4 in 100 g. H 2 O Salt remaining NiS04+6H 2 (blue) NiSO4+7H 2 O NiSO4+6H 2 NiSO4+7H 2 O NiS0 4 +6H 2 O (blue) 32.3 33.0 34.0 35.6 44.7 44.7 50.0 51.0 52.0 53.0 43.57 43.35 43.84 43.79 48.05 47.97 50.15 50.66 52.34 52.34 NiSO4 + 6H2O (blue) (Steele and Johnson.) Solubility of /3- NiSO 4 , 6H 2 O in H 2 O at t. Alcohol 1% by wt. P In 1000 mol. of the solution Mol. NiSO 4 Mol. CH 4 Mol. H 2 O Salt used t g. NiS0 4 per 100 g.H 2 Salt remaining 100 97.5 95 92.5 90 89 88 87 86 85 3.72 0.77 0.455 0.50 0.70 1.01 1.25 1.48 1.73 1.93 7.75 1.65 0.96 1.0 1.6 2.0 2.4 2.9 3.2 3.6 969 950 908 871 830 814 800 781 767 755 23.2 48.5 91 128 168 184 198 216 230 241 NiSO4+6H 2 O(blue) NiSO4+6H 2 O(blue) NiS0 4 +7H 2 NiSO4+6H 2 O(blue) NiS0 4 +7H 2 NiS04+7H 2 NiS0 4 +6H 2 0(blue) NiSO4+6H 2 O(blue) NiS0 4 +7H 2 N1SO4 +7H 2 O 54.5 157.0 jeo.o 69.0 70.0 73.0 80.0 89.0 99.0 52.50 53.40 54.84 58.38 59.44 60.72 63.17 67.90 76.71 NiSO4+6H 2 O (green) (de Bruyn, R. t. c. 1903, 22. 418.) This salt is more sol. in ethyl alcohol than in methyl alcohol. See also under hydra ted salts. For solubility of NiSO 4 in ethyl alcohol, see under hydrated salts. 100 g. sat. solution in glycol contain 9.7 g. NiSO 4 at ord temp, (de Coninck, Bull. Ac. Roy. Belg. 1906. 359.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethyl acetate, (Naumann, B. 1904, 37, 3602.) Very si. sol. in acetone. (Krug and M'Elroy.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014). +H 2 O. Very si. sol. in abs. methyl al- cohol. After standing in contact with it for 8-9 months, the solution contains 1.34% NiSO 4 . (de Bruyn. R. t. c. 1903, 22. 414.) +2H 2 O. Cryst. from sat. NiSO 4 -f Aq at 131. (Steele and Johnson.) +4H 2 O. Solubility in methyl alcohol + Aq at 10. Time = 24 hrs. P=% anhydrous salt in the sat. solutions. Alcohol of 100% 80% 50% 20% water P 7.38 0.66 1.43 14.8 25.1 (de Bruyn, R. t..c. 1903, 22. 414.) (Steele and Johnson, Chem. Soc. 1904, 86. 118.) Tr. point from a- to /3- salt = 53.3. (Steele and Johnson.) 100 pts. absolute methyl alcohol dissolve 31.6 pts, NiS0 4 +6H 2 Oat 17; 100 pts. 93.5% methyl alcohol dissolve 7.8 pts. NiSO 4 + 6H 2 O at 18; 100 pts. 50% methyl alcohol dissolve 1.9 pts. NiSO 4 +6H 2 O at 18. (de Bruyn, Z. phys. Ch. 10. 786.) a-Salt. Solubility in methyl alcohol +Aq at 14. Time = 5 to 6 hrs. Alcohol % by wt. N04 In 1000 mol. of the solution Mol. NiSO4 Mol. CH 4 O Mol. HaO 100 12.4 26 794 180 97.5 10.6 22.3 808 170 95 6.5 14 817 169 92.5 3.06 5.9 838 156 90 1.18 2.3 821 177 85 0.315 0.57 757 242 80 0.25 0.4 688 312 60 0.46 0.8 453 546 40 2.43 3.5 265 732 20 14.7 21 105 874 (water) 26.0 39 961 (de Bruyn, R. t. c. 1903, 22. 412.) 1000 SULPHATE, NICKEL /3-salt. Solubility in methyl alcohol +Aq at Solubility in 100 pts. H 2 O at t. Continued. 14. Time-24hrs. Pts Pts. Pts Alcohol O7 In 1000 mol. of the solution t NIS04 t NiSO 4 t NiS0 4 % by wt. % NiSCU Mol. Mol. Mol. 99 83.1 103 85.6 107 88.1 NiS0 4 CHiO H 2 100 83.7 104 86.2 108 88.7 100 15.7 33.8 763 203 101 102 84.3 84.9 105 106 86.8 87.5 108.4 88.7 97.5 12.4 26 781 193 95 92.5 90 89 10.0 5.61 2.35 1.79 20.3 11.1 4.5 784 800 810 196 189 185 (Mulder, calculated from his own and Tob- ler's determinations, Scheik. Verhandel. 1864. 70.) 88 1.29 87 97 t 86 0^73^ Solubility in H 2 O at t. OK OA1 10 *7K K C\A A oo 80 60 . Dl 0.41* 0.75 .0 ) 0.7 1.3 /GO 682 453 J44 317 546 Salt used t g. NiSO in 100 gH 2 Salt remaining 40 3 11 4 264 700 20 14! 1 2LO ^/l_r 105 i O ' 874 NiSO 4 +7H 2 O 5 25.74 NiSO 4+7H 2 (water) 27.2 40.0 960 tt 27.22 O1 Ct C (de Bruyn.) tt 15 ol .00 34.19 (( 22.6 37.90 _j_7jj 2 O tt 22.8 38.88 Solubility in 100 pts. H 2 O at t, using NiSO 4 +7H 2 O. NiSO NiSO tt 4 +6H 2 O 4 +7H 2 30.0 30.0 32.3 42.46 42.47 44.02 Pts Pts' Pts 33.0 45.74 t NiS0 4 t N1SO4 t NiS04 u 34.0 45.5 tt 29.3 33 45.5 66 63.6 (Steele and Johnson, Chem. Soc. 1904, 85. 1 29.7 34 46.0 67 64.1 116.) 2 30.1 35 46.5 68 64.7 3 30.5 36 47.0 69 65.3 4 5 6 7 8 9 10 31.0 31.5 32.0 32.5 33.0 33.5 34.0 37 38 39 40 41 42 43 47.5 48.0 48.5 49.0 49.6 50.1 50.6 70 71 73 72 74 75 76 65.9 66.5 67.0 67.6 68.2 68.8 69.3 M.-pt. of NiSO 4 +7H 2 O = 98-100. (Til- den, Chem. Soc. 45. 409.) Tr. point from a-6H 2 O salt to 7H 2 salt = 31.5. (Steele and Johnson.) Exists also in an unstable, more soluble modification. (Fedorow, C. C. 1903, II. f\f \ 11 34.5 44 51.2 77 69.9 95.) 12 35.0 45 51.7 78 70.5 13 14 35.5 36.0 46 47 52.3 52.8 79 80 71.1 71.7 Solubility of NiSO 4 .7H 2 O+Na 2 SO 4 .10H 2 O 15 1 C* 36.5 O^7 f\ 48 53.4 81 72.3 in 100 g. H 2 O at t. 16 17 37.0 37.5 49 50 53.9 54.5 82 83 72.9 73.5 .t grams N1SO4 grams NazSCh 18 19 20 21 38.0 38.5 39.0 39.5 51 52 53 54 55.0 55.6 56.1 56.7 84 85 86 87 74.1 74.6 75.2 75.8 5 10 22 25 28 .46 .28 .26 10.09 15.245 20.64 22 23 24 40.0 40.5 41.0 55 56 57 57.3 57.9 58.4 88 89 90 76.4 77.0 77.6 (Koppel, Z. phys. Ch. 1905, 52. 401.) See also under NiNa 2 (SO 4 ) 4 . 25 41.5 58 59.0 91 78.2 26 27 28 29 30 31 32 42.0 42.5 43.0 43.5 44.0 44.5 45.0 59 60 61 62 63 64 65 59.6 60.2 60.7 61.3 61.9 62.4 63.0 92 93 94 95 96 97 98 78.8 79.4 80.1 80.7 81.3 81.9 82.5 100 pts. absolute methyl alcohol dissolve 46 pts. NiSO 4 +7H 2 O at 17; 100 pts. absolute methyl alcohol dissolve 24.7 pts. NiSO 4 + 7H 2 O at 4; 100 pts. 93.5% methyl alcohol dis- solve 10.1 pts. NiSO 4 +7H 2 O at 4; 100 pts. 50% methyl alcohol dissolve 2 pts. NiSO 4 + 7H 2 O at 4. (de Bruyn, Z. phys. Ch. 10. 786.) SULPHATE, NICKEL ZINC 1001 Solubility in methyl alcohol +Aq at 14' Time, 5 to 6 hrs. A 1^_U 1 In 1000 mol. of solution Alcohol % by wt. NiS()4 Mol. Mol. Mol. NiSO 4 CH 4 O H 2 100 16.8 35.7 714 250 97.5 13.9 29 734 237 95 11.6 23.6 742 234.5 92.5 8.12 16.2 760 224 90 5.78 11.2 758 231 85 1.52 3 744 253 84 1.06 . . . . . 83 0.985 . 82 0.83 81 0.665 80 0.653 1^2 687 312 60 0.805 1.3 453 546 45 1.73 40 2.78 4 264 732' 35 4.55 30 6.33 20 13.7 20" 105 875' (water) 26.4 39.5 960.5 (de Bruyn, B. t. c. 1903, 22. 411.) * 100 g. absolute ethyl alcohol dissolve 1.3 g. NiSO 4 +7H 2 O at 4, and 2.2 g. at 17. (de Bruyn, Z. phys. Ch. 10. 786.) Min. Moreno site. Nickel hydrazine sulphate, NiH 2 (SO 4 ) 2 , 2N 2 H 4 . 1 pt. is sol. in 275.5 pts. H 2 O at 18. SI. sol. in hot H 2 O. Sol. in HNO 3 with decomp.; insol. in HC1. Sol. in NH 4 OH+Aq. (Cur- tius, J. pr. 1894, (2) 60. 331.) Nickel potassium sulphate, NiSO 4 , K 2 SO 4 + 6H 2 O. Sol. in 8-9 pts. H 2 O. (Tupputi.) 100 pts. H 2 dissolve at: 10 14 20 30 5.3 8.9 10.5 13.8 18.6 pts. anhydrous salt, 36 49 55 60 75 20.4 27.7 32.4 35.4 45.6 pts. anhydrous salt. (Tobler, A. 96. 193.) Saturated solution contains at: 20 40 60 80 8.7 12.3 17.6 22.0% anhydrous salt, (v. Hauer, J. pr. 74. 433.) Nickel rubidium sulphate, NiSO 4 , Rb 2 SO 4 -h 6H 2 0. Sol. in H 2 O. (Tutton, Chem. Soc. 63. 337.) 1 1. H 2 O dissolves 59.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Nickel sodium sulphate, NiNa 2 (SO 4 ) 2 +4H 2 0. Solubility of NiNa 2 (SO 4 ) 2 .4H 2 O in 100 g. H 2 O at t. t grams NiSO 4 grams Na2SC>4 20 25 30 35 . 40 29.31 27.33 24.64 23.66 21.88 26.87 25.33 22.58 21.67 20.65 (Koppel, Z. phys. Ch. 1905, 52. 401.) Solubility of NiNa 2 (SO 4 ) 2 .4H 2 O + NiSO 4 . 7H 2 O in 100 g. H 2 O at t. o grams N1SO4 grams , NaSO4 grams grams N1SO4 Na 2 SO4 18.5 30.70 20 31.59 25 33.11 25.805 30 25.355 35 23.07 40 34.98 19.825 36.01 16.435 37.935 14.295 (Koppel.) Solubility of NiNa 2 (SO 4 ) 2 .4H 2 O+Na 2 SO 4 . 10H 2 O in 100 g. H 2 O at t. t grams N1SO4 grams NaSO4 18.5 26.14 20 24.07 25 18.81 30 9.87 29.455 31.365 37.13 44.25 (Koppel.) Solubility of NiNa 2 (SO 4 ) 2 .4H 2 O+Na 2 SO 4 (anhydrous) in 100 g. H 2 O at t. t grams N1SO4 grams Na2SO4 35 40 7.13 7.245 49.595 49.03 (Koppel.) Nickel thallium sulphate, NiSO<, T1 2 SO 4 + 6H 2 O. Easily sol. in H 2 O. Can be recryst. from little H 2 O without decomp. (Werther, J. pr. 92. 132.) 1 1. H 2 O dissolves 46.1 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27, 459.) 1 1. H 2 O dissolves 68.8 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Nickel potassium zinc sulphate, 2K 2 SO 4 , ZnSO 4 +12H 2 O. Sol. in H 2 O. (Vohl, A. 94. 51.) Nickel zinc sulphate, NiSO 4 , ZnS0 4 +13H 2 0. Sol. in 3-4 pts. cold H 2 O. Insol. in alcohol. (Tupputi, 1811.) NiSO 4 , Completely sol. in NH 4 OH+Aq. 2NiSO 4 , 2ZnSO 4 , H 2 SO 4 . (Etard, C. R. 87. 602.) 1002 SULPHATE AMMONIA, NICKEL Nickel sulphate ammonia, NiS0 4 , 6NH 8 . Sol. in H 2 O with separation of hydroxide. (Rose, Pogg. 20. 151.) NiSO 4 , 5NH 3 +3^H 2 O. Deliquescent. (Andre, C. R. 106. 936.) NiSO 4 , 4NH 3 +2H 2 O. Easily sol. in H 2 O. Can be recrystallized out of little H 2 O. In- sol. even in dil. alcohol. (Erdmann.) Nickel sulphate cupric oxide, NiS0 4 , 2CuO+ 6H 2 O. (Mailhe, Bull. Soc. 1902, (3) 27. 172.) 2NiSO 4 , 3CuO + 10H 2 O, and +12H 2 O. (Mailhe.) 5NiSO 4 , 16CuO+zH 2 O. (Recoura, C. R. 1901, 132. 1415.) NiSO 4 , 20CuO+zH 2 O. (Recoura.) Nickel sulphate, hydrazine, NiSO 4 , 3N 2 H 4 . Ppt. (Curtius, J. pr. 1894, (2) 50. 343.) Nickel sulphate hydroxylamine, NiSO 4 , 6NH 2 OH. Decomp. by H 2 O. (Uhlenhut, A. 1899, 307. 334.) Nitrosyl sulphate, H(NO)SO 4 . See Nitrosulphonic acid. Osmious sulphate. Easily sol. in H 2 O and alcohol. Osmic sulphate. Sol. in H 2 O. (Berzelius.) Palladous sulphate, basic, PdS0 4 , 7PdO + 6H 2 O, and 10H 2 O. Insol. in H 2 O. Easily sol. in HCl+Aq. (Kane.) Palladous sulphate, PdS0 4 +2H 2 O. Deliquescent in moist air; very sol. in H 2 O, but decpmp. by much H 2 O, with separation of a basic salt. (Kane.) Phosphoryl sulphate, (PO) 2 (S0 4 ) (?). Possible composition of Weber's (B. 20. 86) P 2 O 6 , 3SO 3 (?). 3P 2 O 4 , 2SO. Immediately decomp. by H 2 O. (Adie, G. N. 1891, 63. 102.) Platinic sulphate, Pt(SO 4 ) 2 . Deliquescent. Sol. in H 2 O, alcohol, or ether; also in H 3 PO 4 , HC1, and HNO 3 +Aq. (Berzelius.) H 2 PtO 2 SO 4 . Sol.inH 2 0. (Blondel, A. ch. 1905, (8) 6. 109.) PtO 2 , SO 3 +4H 2 O. Ppt. Decomp. by H 2 0. Sol. in H 2 SO 4 . PtSO 4 (OH) 2 , 4Pt(OH) 4 +3H 2 O. Ppt. (Prost, Bull. Soc. (2) 46. 156.) Pt 8 SO 4 Oi 3 + 16H 2 O. As above. (Prost.) Platinum hydroxylamine sulphate, Pt(NH 2 OH) 4 SO 4 . Only si. sol. in H 2 O; sol. in dil H 2 SO 4 +Aq. (Uhlenhut, A. 1900, 311. 123.) Platinic potassium sulphate, basic. Insol. in boiling H 2 O, HNO 3 , H 2 SO 4 , HsPO^, HC 2 H 3 O 2 , or NH 4 OH+Aq. Easily sol. in boiling HCl+Aq. SI. decomp. by aqua regia. (E. Davy.) Ptio(SO 4 ) 2 Oio, 3K 2 SO 4 +34H 2 O. Insol. in H 2 O. (Prost, Bull. Soc. (2) 46. 156.) Pti 8 (SO 4 )O 22 , 5K 2 SO 4 +34H 2 O. As above. (Prost.) Platinum rubidium sulphate, Pt 6 Rb 6 (SO 4 ) 4 + 17H 2 O. Sol. in H 2 O. (Prost, Bull. Soc. (2) 46. 156.) Platinum sulphate sulphocarbamide, PtSO 4 , 4CS(NH 2 ) 2 . Insol. in H 2 O. Sol. in cone. H 2 SO 4 without decomp. (Kurnakow. J. pr. 1894, (2) 50, 489.) Potassium sulphate, K 2 S0 4 . Not hygroscopic in the ordinary sense of the word. 100 pts. K 2 SO 4 over H 2 O at 14-20 absorb 58 pts. H 2 in 22 days, and finally de- liquesce completely. (Mulder.) 12 pts. K 2 SO 4 mixed with 100 pts. H 2 O lower the temp. 3.3. (Riidorff, B. 2. 68.) 100 pts. H 2 O dissolve with absorption of heat at 0: 8.36 pts. K 2 SO 4 . (Gay-Lussac.) 8.46 " (Mulder.) 8.5 " (Gerardin.) 7.31 " (Moller, Pogg. 117. 386.) 7.3-7.9 " (Nordenskiold, Pogg. 136.314.) 100 pts. H 2 O at dissolve 8.36 pts. K 2 SC>4; at 12.72, 10.57 pts.; at 49.08, 16.91 pts.; at 63.90, 19.29 pts.; at 101.50, 26.33 pts. (Gay Lussac, A. ch. (2) 11. 311.) Solubility in 100 pts. H 2 O at t. t Pts. K 2 S04 t Pts. K 2 S0 4 15.65 28.1 7.8 10.3 12.8 - 47.0 70.2 98.0 16.0 20.3 23.9 (Nordenskiold, Pogg. 136. 341.) 100 pts. sat. K 2 SO4 at 101.7 contain 17.5 pts. K 2 SO4, or 100 pts. H 2 O at 101.25 dissolve 21.212 pts. K 2 SO4. (Griffiths.) 100 pts. H 2 O at 102.8 dissolve 29 pts. K 2 SO4 (Penny) ; at 15, 7.3-6.25 pts. (Ure's Diet.); at 100, 20 pts. (Ure's Diet.); at 100, 24.2 pts. (Wenzel). Sol. in 9.081 pts. H 2 O at 15 (Gerlach) ; in 16 pts. at 15, and 5 pts. at 100 (Bergmann) ; in 18 pts. cold, and 5 pts. boiling H 2 O (Fourcroy); in 15 pts. cold, and 5 pts. boiling H 2 O (Reid); in 12 pts. H 2 O at 0, and 4 pts. boiling H 2 O (M. R. and P.); in 12 pts. H 2 O at 18.75 (Abl) K 2 SO4 sat. at 15 has sp. gr. =1.0774, and contains 10.055 pts. K 2 SO 4 ip 100 pts. H 2 O. (Michel and Krafft, A. ch. (3) 41. 478.) 100 pts. H 2 O dissolve 9.26 pts. K 2 SO 4 at 15.6, and sat. solution has sp. gr. = 1.177. (Page and Keightley, Cheir. Soc. (2) 10. 566.) SULPHATE, POTASSIUM 1003 Solubility in 100 pts. H 2 O at t. 100 ccm. H 2 O dissolve 12.04 g. K 2 SO 4 at 25. (Trevor, Z. phys. Ch. 7. 468.) Sat. K 2 S0 4 +Aq contains at: 21 23 60 99 130 10.1 10.3 14.5 19.1 21.1%K 2 SO 4 , 130 152 175 195 220 21.3 22.8 24.5 23.8 24.6% K 2 S0 4 . (fitard, A. ch. 1894, (7) 2. 549.) Solubility of K 2 SO 4 in H 2 O at t. G. K 2 SO 4 per 100 g. H 2 O t Pts. K 2 S04 t Pts. K 2 S0 4 t Pts. KiS0 4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 8.5 8.6 8.7 8.8 9.0 9.1 9.2 9.3 9.4 9.5 9.7 9.8 9.9 10.0 10.2 10.3 10.4 10.5 10.7 10.8 10.9 11.1 11.2 11.3 11.5 11.6 11.7 11.9 12.0 12.2 12.3 12.5 12.6 12.8 13.0 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 13.1 13.3 13.4 13.6 13.8 14.0 14.2 14.3 14.5 14.7 14.9 15.1 15.3 15.5 15.6 15.8 16.0 16.2 16.4 16.6 16.8 17.0 17.2 17.4 17.6 17.8 18.0 18.2 18.4 18.6 18.8 19.0 1-9.2 19.4 19.6 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 87 88 89 90 91 92 93 94 95 96 97 98 99 100 101 102 102.25 19.8 20.0 20.2 20.4 20.6 20.8 21.0 21.2 21.4 21.6 21.8 22.0 22.2 22.4 22.6 22.8 23.0 23.2 23.4 23.6 23.9 24.1 24.3 24.5 24.7 25.0 25.2 25.5 25.7 25.9 26.2 26.4 26.6 26.75 t K 2 SO4 Sp. gr. 1 t KaSCU Sp.gr. 0.40 7.47 1.0589 58.95 18.01 1.1089 15.70 10.37 1.0770 74.85 20.64 1.1157 31.45 13.34 1.0921 89.70 22.80 1.1194 42.75 15.51 1 . 1010| 101 . 1* 24.21 1.1207 *=b.-pt. (Berkeley, Phil. Trans. Roy. Soc. 1904, 203. A, 189.) 100 g. H 2 O dissolve 0.133 gram-equivalent K 2 SO 4 at 25 (Van't Hoff and Meyerhoffer, Z. phys. Ch. 1904, 49. 315.) 1 1. sat K 2 SO/+Aq at 25 contains 0.617 mols. K 2 SO 4 . (Herz, Z. anorg. 1911, 73. 274.) Solubility of K 2 SO 4 in H 2 O at t. t % K 2 S0 4 4.78 7.82 30.05 11.43 54.20 14.77 68.90 16.40 (Le Blanc and Schmandt, Z. phys. Ch. 1911, 77. 614.) ( Mulder, calculated from his own and other If solubility S = pts. anhydrous salt in 100 pts. of solution, S = 7.5+0. 1070t from to 163. Solubility from 163 to 220 is constant at 25. (Etard, C. R. 106. 208.) 100 g. H 2 O dissolve 12.10 g. K 2 SO 4 at 25. (Amadori, Rend. Ace. Line. 1912, (5) 21. II. 667.) Solubility of K 2 SO 4 in H 2 O at various pres- sures. Figures denote pts. K 2 SO 4 con- tained in 100 pts. sat. K 2 SO 4 +Aq at t and A pressure in atmospheres. t Pts. K 2 S04 t Pts. K 2 S04 t Pts. K 2 S0 4 A 15 15.5 16.2 1 20 30 6.81 7.14 7.14 9.14 9.24 9.44 9.35 9.54 16 20 28 36 9.76 10.30 12.59 13.28 39 54 98 14.21 17.39 23.91 120 143 170 26.5 28.8 32.9 (MSller, Pogg. 117. 386.) (Tilden and Shenstone, Phil. Trans. 1884. 23.) Solubility of K 2 SO 4 in H 2 O. 100 pts. H 2 O dissolve at: 4.3 18.4 69.9 8.16 10.8 19.7 pts. K 2 SO 4 . (Andreae, J. pr. (2) 29. 456.) Sat K 2 SO 4 +Aq boils at 101.5, and con- tains 26.33 pts. K 2 SO 4 to 100 pts. H 2 O (Gay- ^ussac); at 101.7, and contains 21.2 pts. K 2 SO 4 to 100pts.H 2 O (Griffiths); at 102.25, and contains 26.75 pts, K 2 SO 4 to 100 pts. H 2 O Mulder); boils at 103 (Kremers). Crust forms at 101.7, and solution con- tains 25.3 pts. K 2 SO 4 to 100 pts. H 2 O; highest 1004 SULPHATE, POTASSIUM temp, observed, 102.1. (Gerlach, Z. anal. 26. 426.) B.-pt. of K 2 SO 4 +Aq containing pts. K 2 SO 4 to 100 pts. H 2 O. B.-pt. Pts. K 2 SO4 B.-pt. Pts. K 2 S04 100.5 101.0 101.5 7 14.5 22.1 102 102.1 30.0 31.6 (Gerlach, Z. anal. 26. 4300 Sp. gr. of K 2 SO4 at 19.5. K 2 S04 2.401 4.744 6.968 gr. 1.0193 1 . 0385 1 . 0568 K 2 S04 9.264 10.945 Sp. gr. 1.0763 1 . 0909 (Kremers, Pogg. 95. 120.) Sp. gr. and B-pt. of K 2 SO4+Aq at 12.5. Pts. K 2 SO to 100 pts. H 2 O Sp. gr. 1 . 0079 1.0151 1.0231 1.0305 1.0391 B.-pt. 100 . 38 100.63 100 . 75 100.88 101 2 SO to s. H 2 O Sp. gr. 1.0456 1.0524 1.0599 1.0676 1.0735 B.-pt. 101.12 101.25 101.25 101.38 101 . 5 (Brandes and Gruner, 1827.) K 2 SO 4 -f-Aq sat. at 8 has 1.072 sp. gr (Anthon, A. 24. 211.) K 2 SO 4 +Aq saturated at 12 contains 10.38% K 2 SO 4 and has sp. gr. 1.0716 (Struve Zeit. Ch. (2) 6. 323); saturated at 15 con- tains 11.01% K 2 SO 4 and has sp. gr. 1.0831 (Gerlach); saturated at 18.75 contains 10.74% K 2 SO 4 and has sp. gr. 1.0798 (Kars- ten). Sp. gr. of K 2 SO 4 +Aq at 15. Sp. gr. 1.0082 1.0163 1.0245 1.0328 Sp. gr. 1.0410 1.0495 1.0579 8 9 9.92 Sp. gr. 1.0664 1.0750 1.0830 (Gerlach, Z. anal. 8. 287.) Sp. gr. of K 2 SO 4 +Aq at 18. %K 2 S04 5 10 Sp. gr. 1.0395 1.0815 (Kohlrausch, W. Ann. 1879. 1.) p. gr. of K 2 SO 4 +Aq at 15/15. a = pts. K 2 SO 4 in 100 pts. of the solution; b = pts. K 2 SO 4 in 100 pts. H 2 O. 1 3 6 7 9 9.92 1.010 3.093 5.263 7.527 9.890 11.013 Sp. gr. 1.00808 1.02447 1.04091 1.05776 1.07499 1.08305 (Gerlach, Z. anal. 28. 493.) Sp. gr. of K 2 SO 4 +Aq at 20 containing 0.5 mol. K 2 SO 4 to 100 mols. H 2 O = 1.03758; :ontaining 1 mol. K 2 SO 4 to 100 mols. H 2 O = .06744. (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of K 2 SO 4 +Aq. at 25. Concentration of K 2 SO4 1-nonnal Vr- " Sp. gr. 1.0664 1.0338 1.0170 1.0084 (Wagner, Z. phys. Ch. 1890, 6. 37.) K 2 SO 4 +Aq. containing 6.7% K 2 SO 4 has sp. gr. 20/20 = 1.0549. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) Sp. gr. of K 2 SO 4 +Aq at 20.1, when p = per cent strength of solution; d = ob- served density; w = volume cone, in gr. per cc. /pd_ \ ^100 ~ w y p. 9.83 8.172 6.779 5.021 3.127 2.508 1.448 1.079 1.047 0.455 d. ,0800 ,0657 ,0539 .0394 .0238 .0186 .0100 .0070 .0066 1.0018 0.10615 0.08708 0.07144 0.05218 0.03202 0.02554 0.01463 0.01087 0.01053 0.00456 (Barnes, J. phys. Chem. 1898, 2. 543.) Sp. gr. of K 2 SO 4 +Aq at 18. Y4 44.40 TT . _|T: 3.36 \j& . O J. 52.24 phenol Mol/Liter Mol/Liter 47.30 2.92 49.78 0.000 0.016 0.021 0.032 0.6714 0.6650 0.6614 0.6598 62.82 70.28 80.36 85.26 2.00 1.75 1.40 1.08 35.18 27.97 18.24 13.66 0.040 0.047 0.6555 0.6522 Glycerol 8.96 1Q QA 8.87 7 fiQ 82.17 70 QK 0.064 0.6502 -LO . OvJ 20.34 t . \J\J 6.47 9 O . i/O 73.19 0.076 0.127 0.152 0.236 0.252 . 6494 0.6310 0.6251 0.6042 0.5956 24.15 33.73 40.40 43.52 50. 18 5.83 4.44 3.65 3.38 2 fiQ 70.02 61.83 55.95 53.10 47 13 0.308 0.5834 57^22 ^i . U*7 2.07 ^ * . J.O 40.71 0.409 0.464 0.486 0.495 . 5572 0.5480 0.5425 0.5389 67.94 78.18 98.28 1.53 0.98 0,73 30.53 20.84 0.99 0.498 (saturated) 0.5377 Mannitol 3.20 10.32 86.48 (Rothmund and Wilsmore, Z. phys. Ch. 1902 5.82 10.07 84.11 40. 619.) 8.35 9.61 82.04 100 g. 95% formic acid dissolve 36.5 g ' K 2 SO 4 at 21. (Aschan, Ch. Ztg. 1913, 37 1117.) 11.26 14.30 17.22 9.19 8.66 8.35 79.55 77.04 74.43 1008 SULPHATE, POTASSIUM HYDROGEN Solubility in organic substances +Aq at 25. Continued. Insol. in methyl acetate. (Naumann B. 1909, 42, 3790.) Min. Misinite. +5j^H 2 O. Deliquescent. (Senderens, Bull. Soc. (3) 2. 278.) Potassium cfthydrogen sulphate, K^^SO^s. Sol. in H 2 O. (Phillips, Phil. Mag. 1. 429.) Composition is 4K 2 0, 7SO 3 +3H 2 O, accord- ing to Berthelot (A. ch. (4) 30. 442). Potassium frihydrogen sulphate, KH 8 (SO 4 ) 2 . Sol. in H 2 O with rise of temperature. (Schultz, Pogg. 133. 137.) + 1HH 2 O. (Lesco3ur, C. R. 78. 1044.) Potassium cfo'sulphate (p?/rosulphate), K 2 S 2 7 . When dissolved in exactly the necessary amount of hot H 2 O for solution, it crystallises on cooling without decomp. Decomp. by excess of H 2 O. (Jacquelain, A. ch. 70. 311.) Insol. in methyl acetate. (Naumann, B. 1909. 42. 3790.) Organic substance Composition of the solutions % organic substance % K 2 S0 4 %H 2 Sucrose 9.56 18.55 28.16 37.24 47.55 57.00 9.65 8.65 7.42 6.35 5.21 4.24 80.79 72.80 64.42 56.41 47.24 38.76 Acetone 4.92 10.06 16.23 24.31 37.19 46.29 62.40 7.20 5.02 2.96 1.50 0.47 0.20 0.03 87.88 84.92 80.81 74.19 62.34 53.51 37.57 (Fox and Gage, Chem. Soc. 1910, 97. 381.) Sol. in 76 pts. glycerine of 1.225 sp. gr. at ordinary temp. (Vogel, N. Repert. 16. 557.) Insol. in acetone. (Krug and M'Elroy; Eidman, C. C. 1899, II. 1014.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6.257); benzonitrile. (Naumann, B. 1914, 47. 1370); methyl acetate. (Naumann, B. 1909, 42, 3790); ethyl acetate. (Naumann. B. 1904, 37, 3602.) 100 g. H 2 O dissolve 104 g.K 2 SO 4 +219.0 g. sugar at 31.25, or 100 g. sat. solution con- tain 3.8 g. K 2 SO 4 +66.74 g. sugar. (Kohler, Z. Ver. Zuckerind. 1897, 47. 447.) Min. Glaserite. + i^H 2 O. 100 pts. H 2 O dissolve 9.82 pts. (Ogier, C. R. 82. 1055.) Tn'potassium hydrogen sulphate, K 8 H(S0 4 ) 2 . Sol. in H 2 O. Potassium hydrogen sulphate, KHSO 4 . 1.07 pts. KHSO 4 ( = 1 pt. K 2 S 2 O 7 ) dissolve: at in 2.95 pts. H 2 O. " 20 "2.08 " " 40 " 1.59 " " 100 " 0.88 " (Kremers, Pogg. 92. 497.) Sp. gr. of KHSO 4 +Aq at 15 containing: 5 10 15 % KHSO 4 , 1.0354 1.0726 1.1116 20 25 27% KHS0 4 . 1.1516 1.1920 1.2110 (Kohlriiusch, W. Ann. 1879. 1.) Sat. solution boils at 105.5 (Griffiths); 108 (Kremers). Alcohol dissolves out H 2 SO 4 . K 2 SO 4 crystallises from dilute solutions. 100 g. 95% formic acid dissolve 14.6 g. KHSO 4 at 19.3. (Aschan, Ch. Ztg. 1913, 37. 1117.) Potassium hydrogen ^'sulphate, KHS 2 Oy. Sol. in fuming H 2 SO 4 without decomposi- tion. Potassium odosulphate, K 2 S 8 O 26 . Decomp. by H 2 O. (Weber.) Potassium praseodymium sulphate, 3K 2 S0 4 , Pr 2 (S0 4 ) 8 +H 2 0. SI. sol. in H 2 O. Sol. in cone. HC1 and HNO 3 . (Von Scheele Z. anorg. 1898, 18. 358.) Potassium rhodium sulphate, 3K 2 SO 4 , Rh 2 (S0 4 ) 8 . Does not exist. (Leidie, C. R. 107. 234.) K 2 SO 4 , Rh 2 (SO 4 ) 3 +24H 2 O. Very sol. in H 2 O. (Piccini, Z. anorg. 1901, 27. 66.) Potassium samarium sulphate, 9K 2 SO 4 , 2Sm 2 (S0 4 ) 8 +3H 2 0. SI. sol. in H 2 O. SI. sol. in sat. K 2 SO 4 +Aq. 1 1. sat. K 2 SO 4 +Aq dissolves 0.5 g. Sm 2 O 3 . (Cleve, Bull. Soc. (2) 43. 166.) Potassium scandium sulphate, 3K 2 S0 4 , Sc 2 (S0 4 ) 3 . Very slowly sol. in cold, more easily sol. in warm H 2 O. Insol. in sat. K 2 SO 4 +Aq. Sol. in H 2 O and in dil. K 2 SO 4 + Aq. (Meyer, Z. anorg. 1914, 86. 279.) 2K 2 SO 4 , Sc 2 (SO 4 ) 3 . Sol. in K 2 SO 4 +Aq. (Cleve.) Does not exist. (Nilson.) Potassium sodium sulphate, 3K 2 S0 4 , Na 2 SO 4 . 100 pts. H 2 O dissolve 40.8 pts. at 103.5. (Penny, Phil. Mag. (4) 10. 401.) 5K 2 SO 4 , Na 2 SO 4 . 100 pts. H 2 O at 100 dissolve 25 pts. ; at 12.7, 10.1 pts. ; at 4.4, 9.2 pts. (Gladstone, Chem. Soc. 6. 111.) SULPHATE, POTASSIUM YTTRIUM 1009 Potassium strontium sulphate, K 2 Sr 2 (SO 4 )2. Decomp. by (NH 4 ) 2 CO 3 +Aq. (Rose. Pogg. 93. 604.) K 2 SO 4 , SrSO 4 . This is the only double salt formed from these two components between and 100. 100 pts of the sat. solution in equilibrium with SrSO 4 and the double salt contain at: 17.5 50 75 100 1.27 1.88 2.71 3.9 pts. K 2 SO 4 . (Barre, C. R. 1909, 149. 292.) Potassium tellurium sulphate, KHS0 4 , 2TeO 2 , S0 8 +2H 2 0. (Metzner, A. ch. 1898, (7) 16. 203.) Potassium terbium sulphate. Easily sol. in H 2 O. SI. sol. in K 2 SO 4 +Aq. (Delafontaine, Zeit. Chem. (2) 2. 230.) Potassium thallic sulphate, KT1(SO 4 ) 2 + 4H 2 O. Decomp. by H 2 O. (Fortini, Gazz. ch. it. 1905. 36. (2) 453.) 2K 2 O, T1 2 O 3 , 4SO 3 . Insol. in H 2 O. Very difficultly sol. in warm dil. H 2 SO 4 +Aq. (Strecker, A. 135. 207.) Potassium thorium sulphate, K 2 S0 4 , Th(S0 4 ) 2 +4H 2 0. Sol. in hot H 2 O containing a few drops HC1. (Barre, A ch. 1911, (8) 24. 227.) 2K 2 SO 4 , Th(SO 4 ) 2 +2H 2 O. Slowly sol. in cold, easily and abundantly in hot H 2 O, and is gradually decomp. by boiling. Easily sol. in acids. Insol. in alcohol. (Berzelius.) 3.5K 2 SO 4 , Th(SO 4 ) 2 . Insol. in K 2 SO 4 +Aq of con2entrations above 4.5%. (Barre.) 4K 2 SO 4 , Th(SO 4 ) 2 +2H 2 O. (Chydenius.) Potassium tin (stannous) sulphate, K 2 SO 4 , SnS0 4 . (Marignac.) Potassium tin (stannic) sulphate, K 2 Sn(SO 4 ) 8 . Easily sol. in H 2 O with decomp. Sol. in HC1. (Weinland, Z. anorg. 1907, 64. 250.) Potassium tin (stannous) sulphate chloride, 4K 2 S0 4 , 4SnS0 4 , SnCl 2 . Can be recrystallised from H 2 O. (Marig- nac, Ann. Min. (5) 12. 62.) Potassium titanium sulphate, K 2 S0 4 , Ti(SO 4 ) 2 +3H 2 O. Difficultly sol. in H 2 O or HCl+Aq. De- comp. by much H 2 O. (Wallace, Pogg. 102. 453.) Potassium titanyl sulphate, 2K 2 SO 4 , 3TiO, SO 4 +10H 2 O. Very sol. in H 2 O with decomp. Insol. in cone. H 2 SO 4 . (Rosenheim, Z. anorg. 1901, 26. 251. K 2 S0 4 , Ti0 2 S0 4 +7H 2 0. Very hygro- scopic and sol. in H 2 O. (Mazzuchelli and Pontanelli, C. C. 1909, II. 420.) K 2 S0 4 ,(TiO)S0 4 . (Spence, C. C. 1901, II. Potassium uranous sulphate, K 2 SO 4 , U(S04) +H 2 0. Very si. sol. in H 2 O. (Rammelsberg.) Potassium uranyl sulphate, K 2 SO 4 , (U0 2 )S04 +2H 2 0. Sol. in 9 pts. H 2 O at 22 and in 0.51 pt. at 100. Insol. in alcohol. (Ebelmen, A. ch. (3) 5. 211.) 100 pts. of aqueous solution sat. at 25 contain 10.5 pts. salt; at 70.5 contain 23.93 pts. salt. (Rimbach, B. 1904, 37. 478.) +3H 2 O. (de Coninck, Chem. Soc. 1905, 88. (2) 394. 2K 2 SO 4 , (UO 2 )SO 4 +2H 2 O. Decomp. by H 2 0. Cannot be cryst. from rather cone. H 2 S0 4 , as it is completely decomp. by it. (Rimbach, B. 1905, 38. 1572.) K 2 O. 2UO 3 , 3SO 3 . Ppt. Identical with UO 2 , OK, SO 3 H of ScheUer, (A. 1867, 144. 238.) (Kohlschutter, A., 1900, 311. 11.) 2K 2 SO 4 , 3(UO 2 )SO 4 +H 2 O. Sol. in H 2 0. Insol. in alcohol. (Berzelius.) Does not exist. (Ebelmen.) Potassium vanadium sulphate, K 2 0, V 2 O, 2SO 3 +6H 2 O =K(VO 2 )SO 4 +3H 2 O. (Friedheim, B. 24. 1183.) =KVO 3 , K 2 SO 4 , V 2 O 5 , 2SO 3 +9H 2 O of Miinzing (Berlin, Dissert. 1889). K 2 S0 4 , VS0 4 +6H 2 0. Sol. in H 2 0. (Pic- cini, Z. anorg. 1902, 32. 61.) K 2 V 2 (SO 4 ) 4 +24H 2 O. 100 pts. H 2 O dis- solve 198.4 pts. salt, at 10. Sp. gr. of sat. solution at 4/20 = 1.782. (Piccini, Z. anorg. 1897, 13. 446.) Potassium vanadyl sulphate, K 2 S0 4 , (VO) 2 (S0 4 ) 3 . Very slowly sol. in H 2 O, still less sol. in dil. alcohol. (Gerland.) K 2 SO 4 , VOSO 4 +3H 2 O. Easily sol. in H 2 0. Sol. in alcohol+conc. H 2 SO 4 . (Koppel, Z. anorg. 1903, 36, 178.) K 2 SO 4 , 2VOSO 4 . Very hygroscopic. Very sol. in H 2 O but goes into solution slowly. (Koppel and Behrendt, B. 1901, 34. 3935.) Easily sol. in H 2 O. (Koppel, Z. anorg. 1903, 36. 174.) Potassium yttrium sulphate, 4K 2 S0 4 , Y 2 (S0 4 ) 8 . Sol. in 16 pts. cold H 2 O, and in 10 pts. sat. K 2 SO 4 +Aq, and more abundantly if the latter solution contains ammonium salts or free acid. (Berlin.) 3K 2 SO 4 , 2Y 2 (SO 4 ) 3 . 100 ccm. cold sat. 1010 SULPHATE, POTASSIUM ZINC K 2 SO 4 +Aq dissolve an amount of this salt corresponding to 4.685 g. Y 2 O 3 . (Cleve.) Potassium zinc sulphate, K 2 SOi. ZnSO 4 + 6H 2 0. Sol. in 5 pts. cold H 2 O. (Bucholz, N. J. Pharm. 9. 2. 26.) 100 pts. H 2 O dissolve at: 10 15 25 36 12.6 18.7 22.5 28.8 39.9 pts. hydrous salt, 45 50 58 65 70 51.2 54.0 67.6 81.3 87.9 pts. hydrous salt. (Tobler, A. 95. 193.) 100 pts. H 2 at 15 dissolve 14.8 pts. K 2 SO 4 , ZnSO 4 +6H 2 O; sp. gr. of sat. H 2 O solution at 15 = 1.0939. (Schiff, A. 109.326.) 1 1. H 2 O dissolves 131.9 g. anhydrous salt at 25. (Locke, Am. Ch. J. 1902, 27. 459.) Potassium zirconium sulphate, 2K 2 O, 6ZrO 2| 7S0 3 +9H 2 0. Decomp. by H 2 O. 3K 2 O, 3ZrO 2 , 7SO 3 +9H 2 O. Insol. in H 2 O. Zr 2 O 3 (KSO 4 ) 2 +8H 2 O. Ppt. (Rosenheim, B. 1905, 38. 815.) Potassium sulphate vanadate. Very difficultly sol. in H 2 O. alcohol. (Berzelius.) Insol. Potassium sulphate antimony Jn'fluoride. See Antimony Irifluoride potassium sul- phate. Praseodymium sulphate, basic, (PrO) 2 SO 4 . Insol. in H 2 O. (Matignon, C. R. 1902, 134. 660.) Insol. in H 2 O. Nearly insol. in dil. acids. (Wohler, B. 1913, 46. 1730.) Praseodymium sulphate, Pr 2 (SO 4 ) 8 . Sol. in H 2 O; very hydroscopic. 23.64 pts. are sol. in 100 pts. H 2 O at and 17.7 pts. at 20. (von Scheele, Z. anorg. 1898, 18. 357- 358.) +5H 2 O. Sol. in H 2 O. (von Scheele,, Z. anorg. 1898, 18. 357.) Difficultly sol. in H 2 O. (Kraus, Zeit. Kryst. 1901, 34. 400.) 1.50 pts. Pr 2 (SO 4 ) 3 are sol. in 100 pts. H 2 O at 85; 1.45 pts. at 90; and 1.02 pts. at 95. (Muthmann and Rolig, B. 1898, 31. 1729.) +8H 2 O. (Kraus, Zeit. Kryst. 1901, 34. 406.) Sol. in H 2 O. (von Scheele, Z. anorg. 1898, 18. 357.) Solubility in H 2 O at t. t Pts. Pr 2 (SO4)3 18 35 55 75 19.79 14.10 10.31 7.09 4.13 (Muthmann and Rolig, B. 1898, 31. 1727.) +15HH 2 O. Sol. in H 2 O. (von Scheele, Z. anorg. 1898, 18. 357.) Praseodymium hydrogen sulphate, Pr(S0 4 H) 8 . (Brauner, Z. anorg. 1904, 38. 330.) Solubility in boiling cone. H 2 SO 4 . 100 g, of the solution contain 1.02 g. of the acid sulphate. (Matignon, C. R. 1902, 134. 659.) Radium sulphate. Less sol. in H 2 O than corresponding Ba comp. (Curie, Dissert. 1903.) Rhodium sulphate, Rh 2 (SO 4 ) 8 +12H 2 0. Easily sol. in H 2 O. (Berzelius.) SI. sol. in, but not decomp. by H 2 O when not more than 16 pts. H 2 O are present to 1 pt. salt. Decomp. by hot H 2 O to Rh 2 (SO 4 ) 3 ,Rh 2 O 3 . Insol. in H 2 O. (Leidid, C. R.107. 234.) Rhodium rubidium sulphate, Rh 2 (S0 4 ) 3 , Rb 2 SO 4 +24H 2 O. Sol. in H 2 O; m.-pt., 108-109. (Piccini, Z. anorg. 1901, 37. 65.) Rhodium thallium sulphate, Rh 2 (S0 4 ) 3) T1 2 S0 4 +24H 2 O. Very sol. H 2 O. (Piccini, Z. anorg. 1901, 37. 69.) Rhodium sodium sulphate, Rh 2 Na 2 (S0 4 ) 4 . Insol. in H 2 SO 4 or aqua regia. (Seubert and Kobbe, B. 23. 2560.) Rubidium sulphate, Rb 2 S0 4 . 100 pts. H 2 O dissolve 42.4 pts. at 10. (Bunsen.) 100 cc. H 2 O at 17-18 dissolve 44.7 g. Rb 2 SO 4 . (Tutton, Chem. Soc. 1894, 65. 632.) Sat. Rb 2 SO 4 +Aq contains at: 3 20 27.4 32.5% Rb 2 S0 4 , 37 [97 170 37.3 43.9 " 49.2% Rb 2 SO 4 . (fitard, A. ch. 1894, (7) 2. 550.) SULPHATE, SAMARIUM 1011 SolubUity of Rb 2 SO 4 in H 2 O at t. Insol. in H 2 O. Sol. in HC1. Insol. in H 2 SO 4 . Decomp. by boiling with cone. H 2 S0 4 . (Stabler, B. 1905, 38. 2623.) Rubidium uranyl sulphate, Rb 2 (U0 2 )(S0 4 ) 2 + 2H 2 0. Somewhat less sol. in H 2 O than K salt. (Rimbach, B. 1904, 37. 479.) Rubidium vanadium sulphate. Rb 2 V 2 (SO 4 ) 4 + 24H 2 0. n 177 rrram mrla f\f a n Vi \rr\ rm l S0 4 K 2 S0 4 AgSO 4 Temp. =33 Temp. =51 (Swan, J. Am. Uhem. Soc. 1911, 33. 1814.) Solubility in HNO 3 +Aq at 25. 3.22 5.62 8.37 10.41 11.80 0.863 0.940 1.046 1.117 1.177 3.20 5.61 8.40 10.55 13.16 14.37 1.023 1.127 1.247 1.340 1.450 1.524 Normality HNOa Sp. gr. of the solution g. Ag 2 SO 4 dissolved per 1. 0.000 1.0046 2.0452 4.017 4.209 5.564 8.487 10.034 1.0054 1.061 1 . 1069 1.1871 1 . 1956 1.2456 1.3326 1.3676 8.350 34.086 49.010 71.166 73.212 84.609 94.671 90.806 Temp. =75 Temp. =100 3.12 5.73 8.43 10.55 13.17 17.06 1.273 1.406 1.554 1.665 1.806 2.021 3.23 5.60 8.45 11.30 15.07 18.58 1.488 1.675 1.890 2.115 2.410 2.677 (Hill and Simmons, Z. phys. Ch. 1909, 67. 603. Sol. in NH 4 OH, and (NH 4 ) 2 CO 3 +Aq. (Barre, A. ch. 1911, (8) 24. 149, 202, 210.) 1014 SULPHATE, SILVER Solubility in K 2 SO 4 +Aq at 25. solubility curves for various temp, all end at a concentration of 40% Na 2 SO 4 , that is, the mixed crystals formed at this concentration are equally sol. at all temp. (Barre, C. R. 1910, 160. 1323.) Solubility in Na 2 SO 4 +Aq at t. ^K 2 S04 +Aq Solubility of Ag2SCh Normality g.-mol. per litre 0.02 2.46X10- 2 0.04 2.36 X10- 2 0.10 2.31X10- 2 0.20 2.32X10- 2 t 100 pts. H 2 O dissolve (Drucker, Z. anorg. 1901, 28. 362.) . Solubility in Na 2 SO 4 +Aq at t. Na 2 S0 4 Ag 2 SO4 18 0.0 0.25 0.51 0.74 1.00 1.48 2.01 2.50 3.04 4.00 4.99 10.10 13.04 0.766 0.712 0.682 0.675 0.665 0.670 0.673 0.689 0.703 0.736 0.768 0.932 1.028 - AgzSCh in 100 pts: H 2 O Na 2 SO4 in 100 pts. H 2 O 14.5 0.741 0.904 1.003 5.278 10.103 13.045 33 0.972 1.150 1.320 1.448 1.548 1.570 1.549 1.462 1.199 0.932 5.345 10.056 15.185 20.093 25.412 29.556 34.732 39.447 44.693 46.976 33 0.0 0.25 0.51 0.75 0.98 1.50 2.01 2.48 3.00 0.917 0.861 0.835 0.825 0.816 0.820 0.832 0.849 0.867 51 .1.173 :1.377 1.572 1.705 1.787 1.302 ..,. t.,^27 1.540 1.188 0.882 5.407 10.116 15.146 20.247 25.196 29.230 34;25 39.302 42.914 44.464 51 0.00 0.25 0.49 0.68 1.02 1.51 1.90 2.46 2.92 3.95 1.081 1.032 1.010 0.000 0.995 1.002 1.017 .034 .053 .103 75 1.458 1.697 J..934 5.368 9.813 .15,260 19.978 25.556 29.662 35.278 38.944 41.365 - -- 2.075 2.161 2.138 1.910 1.603 1.156 75 0.00 0.20 0.47 0.80 0.98 1.52 1.96 2.50 2.98 4.08 .267 .215 1^210 1.222 1.238 1^494 100 1.651 2.012 2.312 2.351 2.260 2.012 1.687 1.158 5.336 10.153 15.532 25.451 29.714 34.718 38.635 40.160 100 0.00 0.50 1.01 1.44 1.94 3.02 Up to 33, the solubility of Ag 2 SO 4 in NajSCh+Aq increases with the concentration of Na 2 SO 4 ; above 33 the solubility of Ag 2 SO 4 rises* W "&" Maximum" at a certain concentra- tion of NaSO 4 .dependent on the temp. The (Barre, A. ch. 1911, (8) 24. 215.) SULPHATE ACETYLIDE, SILVER 1015 Solubility in salts +Aq at 25. C = concentration of salt in salt+Aq in milliequivalents per 1. di = sp. gr. 25/4 of salt+Aq. S = solubility of Ag 2 SO 4 in salt+Aq ex- pressed in milliequivalents per 1. d 2 = sp. gr. 25/4 of Ag 2 SO 4 +salt+Aq. Solubility in organic compds. +Aq at 25. Solvent Mol. Ag 2 SO4 sol. in 1 litre Water 0.5-N Methyl alcohol Ethyl alcohol Propyl alcohol Tert. amyl alcohol Acetone Ether Formaldehyde Glycol Glycerine Mannitol Glucose Sucrose Urea Dimethylpyrone Urethane Form amide Acetamide Acetonitrile Glycocoll Acetic acid Phenol Chloral Methylal Methyl acetate 0.0267 0.0249 0.0228 0.0218 0.0204 0.0220 0.0206 0.0227 0.0259 0.0263 0.0297 0.0283 0.0270 0.0303 0.0216 0.0227 0.0270 0.0253 0.0525 0.0433 0.0252 0.0379 0.0233 0.0205 0.0212 Salt C di S d 2 none 53.52 KNO 3 24.914 49.774 99.870 0.9986 1.0002 1.0034 57.70 61.13 67.93 1.0072 1.0092 1.0034 Mg(N0 3 ) 2 24.764 49.595 99.460 0.9985 0.9999 1.0026 59.44 64.32 72.70 1.0073 1.0094 1.0133 AgN0 3 24.961 49.86 99.61 1.0007 1.0044 1.0112 39.09 28.45 16.96 1.0065 1.0084 1.0137 K 2 S0 4 25.024 50.044 100.0 200.03 0.9989 1.0006 1.0041 1.0110 50.66 49.35 48.04 48.30 1.0064 1.0079 1.0112 1.0180 MgS0 4 20.22 50.069 100.04 200.05 0.9984 1.0002 1.0032 1.0092 52.21 50.93 49.95 49.60 1.0061 1.0079 1.0105 1.0164 (Rothmund, Z. phys. Ch. 1909, 69. 539.) Insol. in methyl acetate (Bezold, Dissert. 1906; Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601) ; liquid methylamine. (Franklin, J. Am. Chem. Soc. 1906, 28. 1420); acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Very sol. in a hot mixture of H 2 SO4 and monobrombenzene, less sol. in cold. (Couper, A. ch. (3) 62. 311.) (Harkins, J. Am. Chem. Soc. 1911, 33. 1813.) Solubility of Ag 2 SO 4 in salts +Aq at 25. C = concentration of salt in salt+Aq in milliequivalents per 1. S = solubility of Ag 2 SO 4 in salt+Aq in milliequivalents per 1. Salt C S KHSO 4 0.0 52.64 105.26 53.98 52.18 51.76 K 2 S0 4 0.0 27.18 54.34 53.98 50.90 49.30 (Swan, J. Am. Chem. Soc. 1911, 33. 1814.) Decomp. by alkali thiosulphates+Aq. (Herschell.) 100 ccm. Ag 2 SO 4 +AgC 2 H 3 O 2 +Aq sat. at 17 contain 3.95 g. Ag 2 SO 4 and 8.30 g. AgC 2 H 3 2 and solution has sp. gr. = 1.0094. (Euler, C. C. 1904, I. 1316.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898 20. 829.) Decomp. by H 2 O; sol. in H 2 SO 4 . (Stas.) A g2 0, 3H 2 0, 4S0 3 +2H 2 0=AgH 3 (S0 4 ) 2 + H 2 0. As above. (Schultz, Pogg. 133. 137.) 2Ag 2 O, 3H 2 O, 5SO 3 +2H 2 O=Ag 4 H 6 (SO 4 ) 6 +2H 2 O. As above. (Schultz.) Silver pyrosulphate, Ag 2 S 2 C>7. Decomp. by H 2 O. (Weber, B. 17. 2497.) SUver thallic sulphate, AgTl(SO 4 )j. (Lepsius, Chem. Ztg. 1890. 1327.) Saver tin (stannic) sulphate, Ag 2 Sn(SO 4 )-f 3H 2 0. Ppt. Decomp. by H 2 O. Sol. in HC1. (Weinland, Z. anorg. 1907, 64. 250.) Silver sulphate acetylide, Ag 2 S0 4 , 2Ag 2 C 2 . (Plimpton, Proc. Chem. Soc. 1892, 8. 109.) 1016 SULPHATE AMMONIA, SILVER Silver sulphate ammonia, Ag 2 SO4, 2NH 8 . Completely sol. in H 2 O. (Rose, Pogg. 20. 153.) Ag 2 SO 4 , 4NH 8 . Easily sol. in HjO or NH 4 OH+Aq without docomp. (Mitschor- lich.) Silver sulphate mercuric oxide, Ag 2 SO 4 , HgO. Insol. in HjO, but decomp. even in the cold. Sol. in JINOa and JI 2 H<) 4 . (Find, (J;i//. <-h. it. 1911, 41. (2) 548.) Silver sulphate sulphide, Ag>S0 4 , Ag 2 S. Decomp. by hot H 2 O or cold HCl+Aq. Sol. in boiling HNO 8 +Aq. (Poleck and Thttmmel, B. 18. 2435.) , and b pts. \ :. -s > .. +10HiO at t. t a b t a b 5.02 12.17 33.88 50.04 312.11 11. C.7 10.12 26.38 10. If, 1S.7S 291.44 i.ro 11.74 :u.:u 45.04 47.81 276.91 17.91 16.73 IS. US 50.40 4(5 ! 82 262 . 35 2r>.or, 2S . 1 1 '.'.) -IS 59.79 45.42 2X.7l 37.35 161.53 70.61 44.35 30.75 4S 05 215.77 84.42 42.96 :u.H4 47.37 270.22 103.17 42.65 : 7:1 50.65 322.12 (Gay-Lussac, A. ch. (2) 11. 312.) Maximum solubility is at 33 from experiment and theoretical considerations. At this temp. NatSO4 + lOHiO is converted into NaiSCh. (Kopp, A. 34. 271.) 100 pts. H-..0 at t. dissolve pts. Na,SO< f IOH.-0. if Pts. N a2 S04 t Pts. Na 2 SO4 17.9 4.53 16.28 24.1 33 25.92 50.81 t Pts. NinSO* -flOHiO t Pts. Massif -r-lOH-t) t Pts. NatSO4 -HlOHjO 2.5 7.5 1-2 .f> is.rr, LT. 31.25 11.39 ic. ;is iM . o;< :o . rs L48.88 170. W 37.50 4:1 7 r. 60 at; IT. 51! a <>s . :;> L>'.M 01 2ti\ IH i>s;,.of, IMS 11 2 J'J 2-2 242.SS 75 81.25 87.50 '.u ::> 100 241.68 217.20 220.65 225! 40 241.69 (Brandes and Firnhabor. 1884.) 1 pt. NjSO+10H 2 O is sol. in 6.1 pts. H 2 O at 7.5; 3.44 pts. at 12.5; 2.41 pts. at 18.75; and 1.724 pts. at .20. (Karsten.) 1 pt. NazSO4+10H 2 O is sol. in 2.86 pts. cold, and 0.8 pt. boiling HzO (Bergmann) ; in 3 pts. cold, and 0.5 pt. boiling HzO (Wittstein) ; in 4 pta. cold, and 1 pt. boiling H 2 O (Fourcroy) ; in 3 pts. H 2 O at 18.75 (Abl). 100 pts. H 2 O dissolve 12.494 pts. Na 2 SO 4 or 35.492 pts. Na 2 SO4-|-10H2O at 15, and sp. gr. of solution = 1.10847- (Michel and Krafft, A. ch. (3) 41. 478.) 100 pts. H 2 O dissolve 39.4 pts. cryst. salt at 15.5; 80 pts. cryst salt at 100. (lire's Diet.) 100 pts. H 2 O dissolve pts. Na 2 SO 4 at t. (Diacon, J. B. 1866. 61.) Solubility of Na 2 SO 4 in H 2 O at various pres- sures and temp. Pts. Na 2 SO 4 contained in 100 pts. sat. Na 2 SO 4 -f-Aq at A pressure in atmos. and t are given. A 1 20 15 15.4 A 15 4.40 4.53 11.32 10.78 11.4 10.74 30 40 10.05 10.33 (Mailer, Pogg. 117. 386.) The solubility of Na 2 SO 4 +10H 2 O increases with the temperature from to 34. At 34 and above, it is converted into the anhydrous salt, the solubility of which is least at 103.17, which is the boiling point of the saturated solution, and increases by cooling from that temp, down to 18-17. Below the latter temperature the anhydrous salt cannot exist in the presence of H 2 O, but is converted into Na 2 SO 4 -f7H 2 O, or Na 2 SO 4 +10H 2 O. The solubility of Na 2 SO 4 +7H 2 O increases with the temperature from 0-26, and at 27 it is converted into the anhydrous salt. Thus there are two different rates of solu- bility for Na 2 SO 4 for temperatures from 0-18, three different rates from 18-26, two from 26-34, and only one above 34. 1. By heating Na 2 SO 4 +10H 2 O to fusion and raising the heat until the liquid boils, placing in a closed vessel and cooling, the greater part of the anhydrous salt, which separates out on heating, redissolves on cool- ing, and the amount increases as the temp, falls until 18 is reached. Below 18 Na 2 SO< +7H 2 O is formed. Saturated Na 2 SO 4 +Aq thus obtained contains for 100 pts. HO at: 18 20 25 26 53.25 52.76 51.53 51.31 pts. Na 2 S0 4 , 30 33 34 36 50.37 49.71 49.53 49.27 pts. Na 2 SO 4 . j > 2. By allowing the boiling saturated solu tion free from undissolved salt to cool to SULPHATE, SODIUM 1017 with exclusion of air until crystals of Na 2 SO 4 +7H 2 O are formed, then removing the greater part of the mother liquor with a warm pipette, and warming the rest of the mother liquor with the excess of crystals, the crystals dissolve in increasing quantity between and 26-27, so that at 27 the solution contains 56 pts. Na 2 SO 4 to 100 pts. H 2 O. The remain- ing undissolved crystals of Na 2 SO 4 +7H 2 O be- gin to melt very slowly at 27, more quickly at higher temperatures, and cause the separa- tion of anhydrous crusts, and thus the strength of the solution is gradually lowered to the normal. Saturated solutions prepared in this way contain for 100 pts. H 2 O at: 13 34.27 pts. Na 2 SO 4 , 92.9 pts. Na 2 S0 4 +7H 2 O. 17 39.99 pts. Na 2 SO 4 , 111.0 pts. Na 2 SO 4 +7H 2 O, 20 44.73 pts. Na 2 SO 4 , 140.0 pts. Na 2 SO 4 +7H 2 0, 202.6 pts. Na 2 SO 4 +7H 2 O. 3. Solutions obtained by shaking H 2 with Na 2 SO 4 +10H 2 O contain for 100 pts. H 2 O at 10 19.62 30.49 or 44.89 78.9 15 16 37.43 38.73 or 105.8 117.4 18 19 41.63 43.35 or 124.6 133.0 25 26 52.94 54.97 or 188.5 202.6 5.02 or 12.16 18 16.80 or 48.41 26 30.00 or 109.81 33 50.76 or 323.1 10 9.00 23.04 20 19.40 5S.S5 15 13.20 pts. Na 2 SO 4 , 35.96 pts. 25 28.00 pts. Na 2 SO 4 , 98.48 pts. Na 2 SO 4 H-10H 2 O 30 40.00 pts. Na 2 SO 4 , 184.1 pts. Naz 34 55.0 pts. Na2SO 4 . 412.2 pts. NazSO.+lOHjO. 35 0.2 40 48.8 45 47.7 50 46.7 55 45.9 pts. Na 2 S0 4 , 60 45.3 65 44.8 70 44.4 75 44.0 80 43.7 pts. Na 2 S0 4 , 85 43.3 90 43.1 95 42.8 100 42.5 103.5 42.2 pts. Na 2 S0 4 . At 34, XajSO 4 +10H 2 O begins to melt in its crystal H 2 O. As long as there is a con siderable quantity of unchanged crystals present, the solution contains 55 pts. Na 2 SO for 100 pts. H 2 O, but as the hydrous salt de- creases in amount and becomes converted into the anhydrous salt, the solution becomes weaker and contains only 49.53 pts. N for 100 pts. HjO after warming for 6 or 8 hours at 34. In the same way temporary solutions can be obtained at 36-40 with 55-56 pts NajSO 4 to 100 pts. HjO, but this amoun sinks to the normal even more quickly than at 34 XajSO 4 dehydrated at 100-150, after the addition of 1 J '*-1H pts. H^, gives a solution between and 32 of the same strength as NaiSO 4 -f lOHjO, but at 34 a solution with 5 pts. Na 2 SO 4 to 100 pts. H 2 O cannot be btained, but one with 49.53 pts. is formed. Lowel, A. ch. (3) 49. 32.) 4. Solubility of anhydrous salt. Above 34, 00 pts. H 2 O dissolve at: (Mulder.) Solubility in 100 pts. H 2 O at t. t Pts. Na 2 SO4 t Pts. NH2SO4 t Pts. Na,SO 4.8 35 50.2 70 44.4 1 5.1 36 49.9 71 44.3 2 5.4 37 49.6 72 44.2 3 5.7 38 49.3 73 44.2 4 6.0 39 49.1 74 44.1 5 6.4 40 48.8 75 44.0 6 6.8 41 48.5 76 44.0 7 7.3 42 48.3 77 43.9 8 7.8 43 48.1 78 43.8 9 8.4 44 47.9 79 43.7 10 9.0 45 47.7 80 43.7 11 9.7 46 47.5 81 43.6 12 10.5 47 47.3 82 43.5 13 11.4 48 47.1 83 43.5 14 12.4 49 46.9 84 43.4 15 13.4 50 46.7 85 43.3 16 14.5 51 46.6 86 43.3 17 15.7 52 46.4 87 43.2 18 16.9 53 46.2 88 43.2 19 18.2 54 46.1 89 43.1 20 19.5 55 45.9 90 43.1 21 20.9 56 45.8 91 43.0 22 22.5 57 45.7 92 43.0 23 24.1 58 45.6 93 42.9 24 25.9 59 45.4 94 42.9 25 27.9 60 45.3 95 42.8 26 30.1 61 45.2 90 42.7 27 32.4 62 45.1 97 42.6 28 35.0 63 45.0 98 42.6 29 37.8 64 44.9 99 42.5 30 40.9 65 44.8 100 42.5 31 44.2 66 44.7 101 42.4 32 47.8 67 44.6 102 42.3 32.75 50.65 68 44.5 103 42.2 33 50.6 69 44.5 103.5 42.2 34 50.4 (Mulder, Scheik. Verhandel. 1864. 123.) 100 pts. dissolve at: 34 100 5 78.8(?) 42.7 120 41 95 pts. 140 160 42.0 42.9 (Tilden and 180 230 44.25 46.4pte.NaO. Loud. R. Soc. Proc. 1018 SULPHATE, SODIUM Solubility decreases above 230. (Etard C. R. 113. 854.) Sat. Na 2 SO 4 +Aq contains at: 7 13 24 28 30 4.1 6.2 9.9 19.3 25.2 29.5% Na 2 S0 4 49 62 83 99 134 150 32.8 31.3 30.0 29.7 29.4 29.8% Na 2 S0 4 190 240 279 320 29.9 30.0 24.5 17.8% Na 2 SO 4 . (Etard, A. ch. 1894, (7) 2. 548.) Solubility of Na 2 SO 4 in H 2 at t. G. per 100 g. H 2 O. t Na 2 S0 4 Sp. gr. "t Na 2 S04 Sp. gr. 0.70 4.71 .0432 33.5 49.39 1.3307 10.25 9.21 .0802 38.15 48.47 1.3229 15.65 14.07 .1150 44.85 47.49 1.3136 24.90 27.67 .2067 60.10 45.22 1.2918 27.65 34.05 .2459 75.05 43.59 1.2728 30.20 41.78 .2894 89.85 42.67 1.2571 31.95 47.98 .3230 101.9* 42.18 1.2450 * B.-pt. (Berkeley, Phil. Trans. Roy. Soc. 1904, 203. A, 189.) Transition point from Na 2 SO 4 +10H 2 O to Na 2 SO 4 = 32.5 (Berkeley); 32.383. (Rich- ards and Churchill, Z. phys. Ch. 1899, 28. 314.) 100 g. Na 2 SO 4 +Aq sat. at 15 contain 11.5 g. anhydrous Na 2 SO 4 ; 21.9 g. at 25. (Schreinemakers, Arch. Ne'er. Sc. 1910, (2) 16. 81.) 1 1. Na 2 SO 4 +Aq sat. at 25 contains 1.881 mols. Na 2 SO 4 . (Herz, Z. anorg. 1911, 70. 127.) Solubility in H 2 O at t. t Mol. % Na2SO4 Tl CO 62 5.39 n* 70 5.27 ar< 72 5.25 h 80 5.18 120 5.04 _5 190 5.25 Nf 192 5.27 as 208 5.39 Ot 241 5.39 10 250 5.04 i 279 4.12 Ch 319 2.56 r} n 252 4.9 ar 310 3.2 , 340 1.8 me 365 0.0 id (Wuite, Z. phys. Ch. 1913, 86. 364.) I* nc Supersaturated solutions of NaSO 4 are easily formed; when Na 2 SO 4 +Aq sat. at its b.-pt. is hermetically sealed, no crystals are deposited on cooling (Lowel). Supersat. Na 2 SO 4 +Aq may also be obtained by cooling hot sat. Na 2 SO 4 +Aq in flasks loosely stop- pered with cotton wool (Schroeder, A. 109. 45), or by covering the containing vessel with a glass plate, watch-glass, card, etc., or by covering the liquid itself with a layer of oil, and then allowing to cool. Hot Na 2 S0 4 +Aq containing 1 pt. H 2 O to 1 pt. Na 2 SO 4 +10H 2 O does not crystallise on slowly cooling or on being quickly cooled by immersion in cold water, if it is contained in a barometer tube freed from air by boiling, or in an exhausted well-closed vessel, or in an open vessel with a layer of oil of turpentine on it (Gay-Lussac) ; or in a vessel containing air, either well stoppered or furnished with a loose cover (Schweigger) ; or in an open vessel under a bell jar full of air and closed at the bottom with a water joint; or in open bottles placed in a quiet situation; or in an open glass enclosed in a stoppered vessel, contain- ing air and some KOH for drying; in this case Na 2 SO 4 +10H 2 effloresces from the solution, and when washed down again does not cause instant crystallisation, but redissolves. The crystallisation of a solution cooled in this way may often be brought about in- stantaneously, or often again after a short tune; (1) by agitation, when the solution has been cooled in an open vessel; (2) by access of air caused by opening the vessel, the crys- tallisation taking place the more rapidly the iarger the opening. In this case the crystallis- ation begins at the top, where the solution, the vessel and the air come in contact; when a eiOf dust falls in the liquid the crystal- isation begins a little under the surface. When the solution has been cooled in vacuo, a Bubble of air, hydrogen, carbonic acid, or litrous oxide is sufficient to set up the crystal- isation; (3) by contact with a solid body. The latter do not cause crystallisation when iooled in contact with the liquid, nor (except- ng a crystal of Na 2 SO 4 +10H 2 O) when they are moistened or warmed before contact with he solution. Supersat. Na 2 S0 4 -J-Aq is brought to xystallisation by addition of a crystal of Sfa 2 SO 4 + 10H 2 O, or an isomorphous substance is Na 2 SeO 4 +10H 2 O, or Na 2 CrO 4 + 10H 2 O. Other crystals, as MgSO 4 +7H 2 O, etc,, have no action. (Thomfeon, Chem. Soc. 35. 199.) See also Hartley, Jones and Hutchinson, ihem. Soc. 1908, 93. 825, on "Spontaneous rystallisation of sodium sulphate solutions," and de Cpppet (A. ch. 1907, (8) 10. 457) on ame subject. A more extended discussion of the pheno- mena and causes of supersaturation is not con- idered to the within the scope of this work. Na 2 SO4+Aq sat. at 15 has sp. gr. 1.10847 (Michel nd Krafft); at 15 has sp. gr. 1.119 (Stolba); at 16 SULPHATE, SODIUM 1019 has sp. gr. 1.1162 (Stolba) ; at 10 contains 29 pts. Na 2 SO4 to 100 pts. HzO (supersaturated?), and has sp. gr. 1.1259 (Karsten). Sp. gr. of Na 2 SO 4 +Aq at 19.5. % Na 2 SO4 Sp. gr. % Na 2 S04 Sp. gr. 2.894 5.589 7.995 1 . 0262 1 . 0509 1.0733 10.538 12.473 1.0977 1.1162 (Kremers, Pogg. 95. 120.) Sp.gr. of Na 2 SO4+Aq. +10H 2 O Sp. gr. Na 2 SO4 +10H 2 O Sp. gr. 1.262 .005 13.744 1.055 2.522 .010 14 . 975 1.060 3.780 .015 16.203 1.065 5.035 .020 17.426 1.070 6.288 .025 18.645 1.075 7.538 .030 19.860 1.080 8.786 1.035 21.071 1.085 10.030 1.040 22.277 1.090 11.272 1.045 23.478 1.095 12.510 1.050 24 . 674 1.100 (Schmidt, Pogg. 132. 132.) Sp. gr. of Na 2 SO 4 +Aq at 19. % Na 2 SO4 +10H 2 Sp. gr. % Na 2 SO4 +10H 2 O| Sp. gr. 1 1.0040 16 1.0642 2 1.0079 17 1.0683 3 1.0118 18 1.0725 4 1.0158 19 1.0766 5 1.0198 20 1.0807 6 .0232 21 1.0849 7 .0278 22 .0890 8 .0318 23 .0931 9 .0358 24 .0973 10 .0398 25 .1015 11 1.0439 26 .1057 12 1.0479 27 .1100 13 1.0520 28 .1142 14 1.0560 29 .1184 15 1.0601 30 .1226 (Schiff, A. 110. 70.) Sp. gr. of Na 2 SO 4 +Aq at 15. % Sp. gr. if Na 2 SO4 Sp. gr. if Na 2 S04 +10H 2 % Sp. gr. Naj8O< +10H 2 O % Sp. f gr. Na 2 SO4 +10H 2 O 1 1.0091 1.004 11 1.044 21 .086 2 1.0182 1.008 12 1.047 22 .090 3 1.0274 1.013 13 1.052 23 .094 4 1.0365 1.016 14 1.056 24 .098 5 1.0457 1.020 15 1.060 25 .103 6 1.0550, 1.024 16 1.064 26 .107 7 1.0644 1.028 17 1.069 27 1.111 8 1.0737 1.032 18 1.073 28 1.116 9 1.0832 1.036 19 1.077 29 1.120 10 1.0927 1.040 20 1.082 30 1.125 (Gerlach, Z. anal. 8. 287.) Sp. gr. of Na 2 SO+Aq at 24.8. a=no. of g., equivalent to 3^ mol. wt., dissolved in 1000 g. H 2 O; b = sp. gr. if a is Na 2 SO 4 + 10H 2 O, 3^ mol. wt. = 161; c = sp. gr. if a is Na 2 SO 4 , y> mol. wt.=71. 1.054 1.098 1.134 1.059 1.114 1.165 1.163 1.188 1.209 1.213 (Favre^and Valson, C. R. 79. 968.) Sp. gr. of Na 2 SO 4 +Aq at 18. % Na 2 SO 4 5 10 Sp. gr. 1.0450 1.0915 % Na 2 S0 4 15 Sp. gr. 1 . 1426 (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of Na 2 SO 4 +Aq at 20 containing 0.5 mol. Na 2 SO 4 to 100 mols. H 2 O = 1.03466; 1.0 mol. Na 2 SO 4 to 100 mols. H 2 O = 1.06744. (Nicol, Phil. Mag. (5) 16. 122.) Sp. gr. of Na 2 SO 4 +Aq at 25. Concentration of Na2SO4 +Aq Sp.jsr. 1-normal Vr- " V- " Vs " 1.0606 1.0309 1.0156 1.0079 (Wagner, Z. phys. Ch. 1890, 6. 39.) Sp. gr. at 16/4 of Na 2 SO 4 +Aq containing 9.4043% Na 2 SO 4 = 1.08655. (Schonrock, Z. phys. Ch. 1893, 11. 781.) Na 2 SO 4 +Aq containing 25.51% Na 2 SO 4 has sp. gr. 20/20 = 1.2527. Na 2 SO 4 +Aq containing 10.14% Na 2 SO 4 has sp. gr. 20/20 = 1.0938. (Le Blanc and Rohland, Z. phys. Ch. 1896, 19. 278.) Sp. gr. of Na 2 SO 4 +Aq at f.7.5, when p = per cent strength of solution; d = ob- served density; and w = volume cone, in grs. percc. (TT^ = p. d. w. 13.06 .1226 0.14662 11.75 . 1094 0.13043 10.68 .0990 0.11737 8.544 .0784 0.09214 6.762 .0615 0.07178 4.015 .0358 0.04159 2.599 .0225 0.02658 2.375 .0204 0.02423 1.818 .0154 0.01846 1.349 1.0109 0.01364 0.5204 1 .0037 0.00522 0.2921 1.0014 0.00293 (Barnes, J. phys. Chem. 1898, 2. 543.) 1020 SULPHATE, SODIUM Sp. gr. of Na 2 SO 4 +Aq at 20. B.-pt. of Na 2 SO 4 +Aq containing pts. Na 2 SO 4 to 100 pts. H 2 O. Normality of Na 2 SO4+Aq % Na 2 S04 Sp. gr. B.-pt. Pts. Na 2 SO 4 B.-pt. Pts. Na 2 S0 4 0.97 0.48 12.36 6.41 1.1138 1.0570 100.5 101.0 101.5 102.0 9.5 18.0 26.0 33.0 102.5 103.0 103.2 39.0 44.5 46.7 (Forchheimer, Z. phys. Ch. 1900, 34. 23.) Sp. gr. of sat. Na 2 SO 4 , 10H 2 O+Aq at t. t wt. of 1 ccm. of the solution 100 g. H 2 O dissolve g. Na 2 SO4+10H 2 .040 12.16 5 .058 10 .078 2i!o4 15 .109 35.96 18 .137 48.41 20 .156 58.35 25 .209 98.48 26 .222 109.81 30 .287 184.1 33 .312 323.1 34 .317 413.2 35 .317 (Tschernaj, J. Russ. Phys. Chem. Soc. 1914, 46. 8.) Sp. gr. and b.-pt. of Na 2 SO4+Aq. Na 2 SO 4 -r-Aq containing P pts. Na2SO4-flOH 2 O for every 100 pts. H 2 O has given sp. gr. and b.pt. P Sp. gr. B.-pt. P Sp. gr. B.-pt. 1 1.005 100.5 16 1.064 101.25 2 1.008 100.62 17 .067 101.25 3 1.014 100.62 18 .070 101.37 4 1.020 100.75 19 .072 101.37 5 1.021 100 . 75 20 .074 101.37 6 1.028 100.87 21 .076 101.37 7 1.030 100.87 22 .078 101.5 8 1.032 101.0 23 .080 101.5 9 1.036 101.0 24 .082 101.5 10 1.040 101.0 25 .084 101.5 11 1.043 101.12 26 .090 101.5 12 1.050 101.12 27 .092 101.63 13 1.055 101.25 28 1.095 101.63 14 1.060 101.25 29 1.098 101.63 15 1.062 101.25 30 1.100 101.75 (Brandes and Gruner, 1827.) Saturated solution boils at 103.17 (L6wel), 103.5 (Mulder), 105 (Kremers), 100.5 (Griffiths), 100.8 (Gerlach). Crust forms at 102.9; highest temp., 103.2, and solution contains 43.9 pts. Na 2 SO 4 to 100 pts. H 2 O. (Gerlach, Z. anal. 26. 426.) (Gerlach, Z. anal. 26. 430.) M.-pt. of Na 2 SO 4 +10H 2 O=34. (Tilden, Chem. Soc. 45. 409.) Sol. with decomp. in HCl+Aq. Solubility in H 2 SO 4 +Aq at 25. 1000 g. of the solution contain Solid phase Mols H 2 S0 4 Mols Na 2 S0 4 0.286 0.338 0.884 1.576 1.666 2.611 1.539 1.671 1.742 2.256 2.363 2.437 2.091 Na 2 S0 4 , 10H 2 a Na 2 SO 4 , 10H 2 O+Na 2 SO 4 Na 2 SO 4 +Na 3 H(SO 4 ) 2 (( Na 3 H(SO 4 ) 2 +Na 3 H(SO 4 ) 2 , H 2 O (D'Ans, Z. anorg. 1906, 49. 356.) Solubility of Na 2 SO 4 in H 2 SO 4 +Aq at 25. c 1000 g. of the solution contain Solid phase Mol. Na 2 S04 Mol. H 2 SO4 1.55 0.08 Na 2 SO 4 1.59 0.147 (C 1.85 0.60 Na 2 SO 4 , 10H 2 O 2.00 0.763 " 0.77 4.23 NaHSO 4 . H 2 O 0.47 4.96 0.32 6.61 Na 2 HSO 4 0.305 6.87 u 0.07 7.18 Na 3 H(S0 4 ) 2 0.79 8.78 (D'Ans, Z. anorg. 1909, 61. 92.) 10 ccm. of sat. Na 2 SO 4 + absolute H 2 S0 4 contain approx. 2.999 g. Na 2 SO 4 . (Bergius, Z. phys. Ch. 1910, 72. 355.) SULPHATE, SODIUM 1021 Solubility in H 2 SO 4 +Aq at 25. Solid Phase, Na 2 SO 4 -(-10H 2 O. Solubility in NaOH+Aq at 25. 1000 g. of the solution contair i Solid phase 4 Millimols H 2 SO4 in 10 ccm. Millimols Na 2 S04 in 10 ccm. Mols Mols (NaOH)'j Na 2 SC 18.81 1.54 Na 2 SO 4 , 10H 2 O 5.W 22.38 0.074 1.41 " 7.79 24.65 0.70 1.08 1 47 QO NfloSO,, lOHoO-J-NfloSfh (Herz, Z. anorg 1912, 73. 276.) J. . TZ f U . t/U .ii d>2fc3Vy4} Av/Xi2^-' |^-^ ct2^vy4 2.02 0.59 Na 2 SO 4 2.82 0.24 3.52 0.126 " 5.83 0.013 " Solubility in H 2 SO 4 +Aq at 25. 6.62 ... NaOH, H 2 O 1000 g. of the Solid phase (D'Ans and.Schreiner, Z. anorg. 1910, 67. 437.) solution contain Sol. in sat. NH 4 Cl+Aq. T"fc "11 11_ Jj.1 1' j. TT'/^ll I Mols SO 3 Mols Na 2 S04 Rapidly and abundantly sol. in sat. KC1+ Aq with pptn. of K 2 SO 4 . Na 2 SO 4 +10H 2 O is sol. in sat. NaCl+Aq 5.91 6.30 6.64 6.90 7.36 0.409 0.332 0.297 0.173 0.071 NaHS04 NaHSO4+NaH 3 (SO4)2, H 2 O NaH 3 (S0 4 ) 2 , H 2 without pptn. If effloresced Na 2 SO 4 is used, a ppt. of NaCl is caused at first, and subse- quently of Na 2 SO 4 +10H 2 O. (Karsten.) Sol. in boiling sat. NaCl+Aq with pptn. of NaCl, but from cold solutions the Na 2 SO 4 7.74 0.047 I separates out first. (Vauquelin.) 7.82 0^044 . Less sol. in NaCl +Aq than in H 2 O. (Hunt, 8.12 0.037 Am. J. Sci. (2) 25. 368.) 8.29 8.40 0.042 0.046 ,, Solubility in NaCl+Aq at t. 8.70 0]076 g. NaCl per g. Na 2 SO4 per 8.86 0.156 " t 100 g. H 2 Oj 100 g. H 2 O 8.93 8.93 0.259 0.269 M 10 0.00 4OQ 9.14 6Af) 8.93 0.273 .40 9 AH ._ . xv/ 33.69 34.08 O . "O 4.73 2.77 10.16 0.797 35*46 0.00 10.78 0.302 ? 25 C.OO 28.74 (D'Ans, Z. anorg. 1913, 80. 236.) 2.74 26.57 8.15 23.15 19.86 20.52 24.58 14.86 SI. sol. in cone. HC 2 H 3 O 2 . (Ure's Diet.) 31 21 9.95 Not pptd. by addition of glacial HC 2 H 3 O 2 to Na 2 SO 4 +Aq. (Persoz.) 32] 02 9^61 1022 SULPHATE, SODIUM Solubility in NaCl+Aq at t Continued. Solubility in NaCl+Aq at 15. t g. NaCl per 100 g.H 2 O g. Na2SO4 per 100 g. H 2 Composition of the sat. solution Solid Phase 27 0.00 2.66 5.29 7.90 16.13 18.91 19.64 20.77 32.33 31.10 28.73 27.17 26.02 24.83 21.39 20.11 19.29 9.53 % by wt. Na 2 S04 % by wt. NaCl 11.5 7.86 5.87 5.23 5.26 5.64 2.26 5.42 11.51 15.97 21.03 23.39 25.21 26.3 Na 2 SO 4 +10H 2 O u It u f( Na 2 SO 4 , 10H 2 O + NaCl NaCl a 30 0.00 2.45 5.61 7.91 10.61 12.36 15.65 18.44 20.66 32.43 39.70 38.25 36.50 35.96 31.64 29.87 25.02 21.30 19.06 9.06 (Schreinemakers and de Baat. Z. phys. Ch. 1909, 67. 554.) Sol. in sat. NH 4 NO 3 +Aq. (Margueritte, C. R. 38. 307.) Sol. in sat. KNO 3 +Aq with pptn. after several hours. (Karsten.) Na 2 SO 4 +10H 2 O is sol. in sat. NaNO 3 +Aq without pptn., but if effloresced Na 2 SO 4 is used, NaNO 3 is pptd. at first, and subse- quently Na 2 SO 4 +7H 2 O. The presence of CaSO 4 does not affect the solubility of Na 2 SO 4 in H 2 O to any great extent. (B.arre, A. ch. 1911, (8) 24. 160.) More sol. in K 2 SO 4 , CuSO 4 , MgSO 4 +Aq. than in H 2 O. (Pfaff. A. 99. 226.) 100 pts. H 2 O dissolve 20.7 pts. CuSO 4 and 15.9 pts. Na 2 SO 4 . (Rudorff, B. 6. 484.) Sol. in sat. MgSO 4 , K 2 SO 4 , CuSO 4 +Aq, but if more Na 2 SO 4 than can be dissolved is added to the CuSO 4 +Aq, a large quantity of a double sulphate separates out. (Karsten.) The solubility of Na 2 SO 4 in K 2 SO 4 +Aq has been determined at 15, 25, 40, 50, 60,, 70 and 80. From the results the conclusion is drawn that sodium and potassium sulphates form a double salt of the formula K 3 Na(SO 4 ) 2 . (Okada, Chem. Soc. 1915, 108. (2) 344.) See also under CuSO 4 , MgSO 4 , and K 2 SO 4 . Slowly but abundantly sol. in sat. ZnSO 4 + Aq, with separation of a double salt after a few days. 33 0.00 1.22 1.99 2.64 3.47 12.14 21.87 32.84 33.99 34.77 48.48 46.49 45.16 44.09 42.61 . 29.32 16.83 8.76 4.63 2.75 35 0.00 2.14 13.57 18.78 31.91 35.63 47.94 43.75 26.26 19.74 8.28 0.00 At 33 and above the values represent the solubility of Na 2 SO 4 in NaCl+Aq. At 10 the solid phase in contact with the solution is probably Na 2 SO 4 , 7H 2 O. Between 17 and 33 the solid phase is either Na 2 SO 4 , 10H 2 O or Na 2 SO 4 . An inversion of Na 2 SO 4 , 10H 2 O to Na 2 SO 4 takes place at various temp, below 33. depending on the amount of NaCl con- tained in the solution in contact with the solid sodium sulphate. (Seidell, Am. Ch. J. 1902, 27. 55.) Solubility of ZnSO 4 .7H 2 O+Na 2 SO 4 .10H 2 O in 100 g. H 2 O at t. t grams ZnSO4 grams Na2SOi 5 40.305 42.285 7.905 9.515 (Koppel, Z. phys. Ch. 1905, 62. 409.) See also under Na 2 Zn(SO 4 ) 4 +4H 2 O. SULPHATE, SODIUM 1023 Solubility of Na 2 SO 4 +Th(SO 4 ) 2 at 16. Solid phase Th(SO 4 ) 2 . Solubility of Na 2 SO 4 in alcohol +Aq at t, t 15 25 alcohol g. per 100 g. solution solid phase Pts. per 100 pts. H 2 O Pts. per 100 pts. H 2 O H 2 O alcohol Na2SO4 Na 2 S04 1.094 1.960 2.84 2.98 4.11 Th(S04) 2 Na 2 S04 Th(S0 4 ) 2 0.7 9.2 19.4 39.7 58.9 72.0 0.0 11.2 20.6 30.2 88.7 85.1 78.6 60.0 41.1 28.0 72.8 76.5 74.3 68.4 0.0 8.6 18.9 39.5 58.8 72.0 0.0 9.5 19.2 29.6 11.3 6.3 2.9 0.5 0.1 0.0 27.2 14.0 6.5 2.0 Na 2 SO 4 +10H 2 O (( (1 u Na 2 SO 4 +7H 2 O PI it 1 2 3 3 3 .743 .387 .800 .962 .375 5.79 9.35 12.24 15.36 2.136 1.379 1.169 1.048 (Barre, C. R. 1911, 160. 155.) Solubility in Na acetate +Aq at 25. Solid phase, Na 2 SO 4 +10H 2 O. 0.0 10.6 24.0 54.0 78.1 78.5 72.8 45.6 0.0 9.3 22.9 54.0 21.9 12.2 4.3 0.4 Na 2 SO 4 + 10H 2 O it C( 1C Composition of the solutions 36 45 0.0 8.8 12.8 17.9 18.1 28.9 48.7 67.0 70.0 71.2 71.1 71.0 66.5 50.9 0.0 6.8 10.5 15.5 15.7 28.4 48.3 33.0 22.6 18.3 13.4 13.3 5.1 0.8 Na 2 SO 4 tt it ^< (( (L (I % Na acetate % Na 2 S04 % H 2 J0 4.10 7.71 12.58 16.26 20.63 21 17 16 13 11 8 9 72 48 50 50 10 78.10 78.18 75.81 73.92 72.24 71.27 0.0 9.0 14.5 20.6 31.0 67.6 71.3 71.8 70.6 65.6 0.0 7.1 12.1 18.4 29.5 32.4 21.6 16.1 10.0 4.9 it It ie 2 t Pts. Th(S04) 2 0.88 1.02 1.25 30 40 1.85 2.83 50 55 4.86 6.5 aqueous solution. Sol. in about 88 pts. H 2 O atO. (Cleve.) Extremely slowly sol. in H 2 0. 100 pts. H 2 O dissolve pts. Th(SO 4 ) 2 +9H 2 0, calculated as Th(SO 4 ) 2 , at t. Above 55, Th(SO 4 ) 2 +4H 2 O separates out. (Demarcay C. R. 96. 1860, calculated by Roozeboom.) 100 pts. H 2 O dissolve pts. Th(SO 4 ) 2 +9H 2 0, calculated as Th(SO 4 ) 2 , at t. t Pts. Th (SO4)2 t Pts. Th(SO 4 ) 2 t Pts. Th(S0 4 ) 2 10 20 0.74 0.98 1.38 30 40 1.995 2.998 51 55 5.22 6.76 Above 60, Th(fcO 4 ) 2 +4H 2 O separates out. (Roozeboom, Z. phys. Ch. 6. 201.) For further data, see Roozeboom (Z.phys. Ch. 6. 198), where there is a full discussion of the subject. 100 g. sat. solution of Th(SO 4 ) 2 +9H 2 O in H 2 O at 25 contain 1.593 g. anhyd. salt. (Wirth, Z. anorg. 1912, 76. 174.) Solubility of Th(SO 4 ) 2 in H 2 SO 4 -(-Aq at t c t % H 2 S0 4 % ThS0 4 Solid phase 30 0.000 2.152 Th(S0 4 ) 2 +8H 2 0.466 2.055 0.72 2.085 1.468 2.267 (( 2.983 2.311 (C 4.38 2.367 4.97 2.323 H 9.95 1.961 <( 15.03 1.484 {( 18.95 1.078 u 23.64 0.7196 " 32.68 0.3364 Th(SO 4 ) 2 +4H 2 O 37.80 0.077 n 43.28 0.0213 u 45.69 0.0047 74.0 0.1208 C( 80.5. . 0.000 u 20 5 1.722 Th(SO 4 ) 2 +8H 2 O 15 0.9752 (C 25 0.3838 K 40 0.0103 Th(SO 4 ) 2 +4H 2 O Boiling 5 0.7407 ts temp. 10 0.4808 (t 15 0.3882 M (Koppel and Holzkampf, Z. anorg. 1910, 67. 274.) SULPHATE, TITANIUM HYDROGEN 1029 Solubility in H 2 SO 4 +Aq at 25' Per 100 g. of solution g. Th(SO4) 2 g. H 2 S04 1.722 0.000 1.919 1.072 2.017 1.941 2.060 2.821 2.061 3.843 2.035 5.212 1.863 8.055 1.702 10.105 (Barre, Bull. Soc. 1912, (4) 11. 647.) Solubility in H 2 SO 4 +Aq at 25. Normality H 2 S04 In 100 g. of the liquid are dissolved Solid phase g. oxide anhydrous sulphate 1.1 2.16 4.32 6.68 9.68 10.89 15.15 1.015 1.14 0.9265 0.545 0.2685 0.0651 0.0396 0.0192 1.593 1.831 1.488 0.8751 0.4312 0.1045 0.0636 0.0308 Th(S0 4 ) 2 +9H 2 a a <( Th(SO 4 ) 2 +8H 2 O Th(SO 4 ) 2 +4H 2 O (Wirth, Z. anorg. 1912, 76. 186.) Solubility of Th(SO 4 ) 2 in HCl+Aq at 30. %HC1 0.0 4.55 6.95 12.14 15.71 18.33 20 23.9 2.15 3.541 3.431= 2.811 2.360 2.199 2.13 1.277 Solid phase Th(SO 4 ) 2 +8H 2 O Th(S0 4 ) 2 +4H 2 (Koppel and Holzkampf, Z. anorg. 1910, 67 274.) Solubility of Th(SO 4 ) 2 in HNO 3 +Aq at 30 % HNOs % Th(S0 4 )2 Solid phase 0.0 5.17 10.04 16.68 21.99 28.33 28.51 33.17 38.82 2.15 3.68 4.20 4.84 4.47 3.96 3.88 3.34 2.51 Th(SO 4 ) 2 +8H 2 O ti ({ {( 11 Th(SO 4 ) 2 +4H 2 O (Koppel and Holzkampf, Z. anorg. 1910, 67. 274.) The presence of phosphoric acid increases ;he solubility of thorium sulphate in HC1 and HNO 3 . (Koppel and Holzkampf, Z. anorg. 1910, 67. 280.) For solubility of Th(SO 4 ) 2 in (NH 4 ) 2 SO 4 , i 2 SO 4 , and K 2 SO 4 , see respective sulphates. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Thorium hydrogen sulphate, ThH 2 (SO 4 ) 3 . Hydroscopic. Sol. in excess of hot H 2 SO 4 ; insol. in cold H 2 SO 4 . (Brauner, Z. anorg. 1904, 38. 333.) Thulium sulphate, Tm 2 (SO 4 ) 3 -f 8H 2 O. Insol. in alcohol. (James, J. Am. Chem. Soc. 1911, 33. 1343.) Tin (stannic) sulphate, basic, (SnO)SO 4 + H 2 O. Easily sol. in cold H 2 O, but quickly de- comp. with separation of stannic hydroxide. (Ditte, C. R. 104. 178.) 3SnO, SO 3 . Easily sol. in dil. acids. (Ditte, A. ch. 1882, (5) 27. 159.) LKH 2 O. Not decomp. by cold H 2 O. (Ditte.)" Tin (stannous) sulphate, SnSO 4 . Sol. in 5.3 pts. H 2 O at 19, and 5.5 pts. at 100. (Marignac.) Solution soon decomposes with separation of a basic salt. Sol. in. H 2 SO 4 +Aq. (Bouquet.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) . Tin (stannic) sulphate, Sn(SO 4 ) 2 +2H 2 O. Deliquescent. Easily sol. in H 2 O; decomp. by much H 2 O. Sol. in dil. H 2 SO 4 +Aq. Slowly sol. in HCl-(-Aq. Decomp. by abso- lute alcohol. (Ditte, C. R. 104. 178.) Titanium sulphate, Ti(SO 4 ) 2 +3H 2 O. Deliquescent, and sol. in H 2 O. The aque- ous solution is decomp. on boiling. (Glatzel, B. 9. 1833.) Titanium sesgm'sulphate, Ti 2 (SO 4 ) 8 . Very deliquescent, and easily sol. in H 2 O. Aqueous solution is decomp. by boiling. (Ebelmen.) Insol. in H 2 O, alcohol, ether and cone. H 2 SO 4 . Slowly sol. in dil. H 2 SO 4 .and HC1. (Stabler, B. 1905, 38. 2624.) Not sol. in alcohol. (Knecht, B. 1903, 36. 169.) +8H 2 O. Sol. in H 2 O. (Glatzel, B. 9. 1833.) Titanium hydrogen ses^uisulphate, 3Ti 2 (SO 4 ) j, H 2 SO 4 +25H 2 O. Gradually sol. in H 2 O. Insol. in 60% H 2 SO 4 , alcohol, ether and glacial acetic acid. (Stahler, B. 1905, 38. 2621.) 1030 SULPHATE, TITANYL Titanyl sulphate, (TiO)SO 4 . Decomp. by H 2 O. Slowly sol. in cold, rapidly in warm HCl+Aq. (Mer/, J. pr. 99. 157.) +2H 2 0. Sol. in H a O. (Blondel, Bull. Soc. 1899, (3) 21. 262.) 2TiO 2 , 3SO 3 +3H 2 O. Sol. in H 2 O acidified with HC1. (Blondel, Bull. Soc. 1899, (3) 21. 262.) 5Ti0 2 , SO 3 +5H 2 O. (Blondel.) 7TiO 2 , 2SO 3 +a;H 2 O. (Blondel.) 2TiO 2 , SO 3 +zH 2 O. (Blondel.) Uranous sulphate, basic, U(OH) 2 SO 4 +H 2 O. Insol. in H 2 O. H 2 O dissolves out H 2 SO 4 . (Ebelmen, A. ch. (3) 6. 217.) +5H 2 O. Sol. in alcohol. Pptd. by ether. (Rosenheim, Z. anorg. 1901, 26. 251. Uranous sulphate, U(SO 4 ) 2 +4H 2 O. Sol. in H 2 O with immediate decomp. Easily sol. in dil. H 2 SO 4 +Aq. (Kohl- schiitter, B. 1901, 34. 3629.) Decomp. by H 2 O into insol. basic, and sol. acid salt. Sol. in dil. H 2 SO 4 or HCl+Aq. Difficultly sol. in cone, acids. (Ebelmen, A. ch. (3) 6. 215.) Solubility of U(SO 4 ) 2 +4H 2 O in H 2 O at t. t %U(S04) 2 I t %U(S0 4 ) 2 29 37 9.8 8.3 8.1 7.3 (Giolitti and Bucci, Gazz. ch. it. 1905, 35. (2) 162.) 1 pt. is sol. in 4.23 pts. H 2 O at 13; 4.3 pts. at 11.3; 4.4 pts. at 9.1. (de Coninck, A. ch. 1903, (7) 28. 12.) +8H 2 O. Solubility of U(SO 4 ) 2 +8H 2 O in H 2 O at t. t %U(S0 4 ) 2 t % U(S0 4 )2 18 25.6 37 10.17 13.32 19.98 48.2 62 93 28.72 36.8 63.2 (Giolitti and Bucci, Gazz. ch. it. 1905, 35. (2) 162.) Sp.gr. of U(S0 4 ) 2 +Aq at t. t % salt Sp. gr. 16 1 1.0058 16.8 2 1.0107 16 3 1.0165 17.8 4 .0218 17.2 5 .0272 18 6 .0320 18.3 7 .0379 17.4 8 .0429 15.2 9 .0485 15.6 10 .0539 (de Coninck, A. ch. 1903, (7) 28. 11.) Solubility in acids +Aq. 1 pt. U(SO 4 ) is sol. in pts. acid at t. 9.7 9.2 11.2 10.3 11.4 10.7 15 14.2 15.5 14.4 16.5 15.9 11.7 10.9 10.1 9 Acid HC1 HNO 3 H 2 SeO 4 (sp. gr. 1.4) UBr HC 2 H 3 O 2 H 2 S0 4 Concentra- Pts. tion of acid acid 1:4 1:4 u 1:4 1:4 1:4.5 1:2 1:4 5.74 5.8 5.4 5.53 4.57 4.66 4 - 4.23 4.1 4.3 3.72 3.85 6.36 6.42 6.45 6.5 (de Coninck, Chem. Soc. 1902, 82. (2) 459.) Sp. gr. of U(SO 4 ) 2 +HCl(d = 1.046) at t. di = Sp. gr. referred to H 2 O. d 2 = Sp. gr. referred to HC1. t % salt d! d 2 16 17 18 18.4 17.6 1 2 3 4 5 1.0525 1.0572 1.0619 1.0667 1.0714 1.0063 1.0109 1.0154 1.0199 1 .0243 (de Coninck, A. ch. 1903, (7) 28. 11.) Sp. gr. of U(SO 4 ) 2 +H 2 SO 4 (d = 1.14) at t di = Sp. gr. referred to H 2 O. d 2 = Sp. gr. referred to H 2 SO 4 . 1 t %salt d! d 2 18.7 18.3 17.4 17.6 18.1 1 2 3 4 5 1 . 1442 . 1.1494 1.1539 1 . 1583 1.1626 1.0038 1.0083 1.0123 1.0162 1.0204 (de Coninck, A. ch. 1903, (7) 28. 11.) 1 pt. is sol. in 8, pts. alcohol (94) +Aq. (1:4) at 10.4. (de Coninck.) Solubility in glycol at 14.8 = 3.15%. (de Coninck, C. C. 1905, II. 883.) Min. Johannite. SI. sol. in H 2 O. Uranous hydrogen sulphate, U(SO 4 ) 2 , H 2 S0 4 + 10H 2 0. (Giolitti, C. C. 1905, II. 1226.) SULPHATE, VANADIUM 1031 Uranyl sulphate, basic, 3UO 3 , SO 8 +2H 2 O. (Athanasesco.) + 14H 2 O. Sol. in H 2 O. (Ordway, Sill. Am. J. (2) 26. 208.) 4UO 3 , SO 3 +7H 2 O. (Athanasesco, C. E. 103. 271.) UO 2 , 4UOSO 4 +8H 2 O. Less sol. in min. acids, especially dil. H 2 SO 4 +Aq, than UOSO 4 +2H 2 O. (de Coninck, C. C. 1901, II. 1038.) Sp. gr. of (UO 2 )SO 4 +H 2 SO 4 (d = 1.168) at t. di = Sp. gr. referred to H 2 O. d 2 = Sp. gr. referred to H 2 SO4. t % 8 alt ' di d2 20.6 22.2 21.1 22.7 22.3 1 2 3 4 5 .1738 .1775 .1880 .1872 .1918 .0050 .0082 .0129 .0165 .0204 +H 2 O. (de Coninck.) +3H 2 O. Efflorescent. Very sol. in H 2 O and alcohol. 1 pt. is sol. in 0.6 pt. cold H 2 O; in 0.45 pt. boiling H 2 O; in 25 pts. cold absolute alcohol; in 20 pts. boiling absolute alcohol. (Bucholz.) Sol. in 0.47 pt. H 2 O at 21, and 0.28 pt. boiling H 2 O. (Ebelmen.) 100 pts. H 2 O at 15.5 dissolve 160 pts., and at 100, 220 pts. (Ure's Diet.) 1 pt. is sol. in 5.3 pts. H 2 O at 13.2; 5.16 s. at 14.1; 4.96 pts. at 15.1; 4.88 pts. at .5. (de Coninck, A. ch. 1903, (7) 28. 8.) Sp. gr. of (UO 2 )SO 4 +Aq at t. t % (UO) 2 S0 4 Sp. gr. 14 1 1.0062 15.5 2 1.0113 11.3 3 1.0172 10.2 4 1.0229 10.2 5 1.0280 10 6 .0338 14 7 .0389 15.6 8 .0442 11 9 .0503 10.3 10 .0557 11.4 11 1.0612 11.6 12 1.0669 (de Coninck, A. ch. 1903, (7) 28. 7.) Solubility in acids +Aq. 1 pt. (UO 2 )SO 4 is sol. in: 3.4 ts. cone. HC1 at 12.8 " " " 13.6 HBr(d = 1.21) " 12.9 " 11.2 cone. HNO 3 " 12.3 " " " 10.8 H 2 SO 4 (d = l,38)"12.7 3.25 5.9 " 6.1 " 10.8 " 11.2" 4.3 " 4.1 " " " "14.0 5.6 " aqua regia (equal vol. HC1+ HNO 3 ) at 15.4 5.47 pts. aqua regia (equal vol. HC1+ HNO 3 ) at 16 4. 3.7 pts. selenic acid (d = 1.4) at 15.3. (de Coninck, A. ch. 1903, (7) 28. 8.) (de Coninck, A. ch. 1903, (7) 28. I.) 1 pt. is sol. in 37.9 pts. alcohol (85) at 16.7; 38.6 pts. at 15.8. (de Coninck, A. ch. 1903, (7) 28. 8.) Very si. sol. in formic and glacial acetic acids, (de Coninck, A. ch. 1903, (7) 28. 9.) Completely pptd. from (UO 2 )SO 4 +Aq by HC 2 H 3 O 2 . (Persoz.) Uranyl hydrogen sulphate, (UO 2 )SO<, H 2 SO<. Very deliquescent. (Schultz-Sellack.) 2(UO 2 )SO 4 , H 2 SO 4 +5H 2 O. Very deliques- cent. (Wyrouboff, Bull. Soc. Min. 1909, 32. 351.) Uranyl pyrosulphate, (UO 2 )S 2 O 7 . Very deliquescent. Hisses with H 2 O. (Schultz-Sellack.) Uranouranyl sulphate, USO,, (UO 2 )SO 4 . Sol. in H 2 O. (Ebelmen.) Decomp. boiling. (Berzelius.) Min. Voglianite. by Uranyl sulphate ammonia, (UO 2 )SO 4 , 2NH 8 . (v. Unruh, Dissert. 1909.) (UO 2 )SO 4 , 3NH 3 . (v. Unruh.) (UO 2 )SO 4 , 4NH 3 . (v. Unruh.) Vanadous sulphate, V 2 O 3 , 4S0 3 +9H 2 O. Sol. in H 2 O. (Brierley, Chem. Soc. 49. 882.) Vanadium sulphate, V 2 O 6 , 2SO 3 = (VO 2 ) 2 S 2 O 7 . Deliquescent. Easily sol. in H 2 O. V 2 O 6 , 3SO 3 . Deliquescent. Sol. in H 2 O and alcohol. +3H 2 O. Deliquescent. Very sol. in H 2 O, but decomp. by boiling. Sol. in alcohol; (Ditte, C. R. 102. 757.) VSO 4 +7H 2 O. Decomp. by air; very un- stable; sol. in H 2 O. (Piccini, Z. anorg. 1899, 19. 204.) Vanadium sesgmsulphate, V 2 (SO 4 )s. Anhydrous. Insol. in H 2 O. Insol. in cone. H 2 SO 4 , but slowly sol. in boiling dil. H 2 SO 4 . Sol. in HC1. Insol. in alcohol and ether. (Stahler, B. 1905, 38. 3979.) 1032 SULPHATE, ZINC, BASIC Vanadium hydrogen sulphate, V 2 (SO 4 ) 3 , H 2 SO 4 +12H 2 O. Sol. in H 2 O. Sol. in HC1. Insol. jn 60% H 2 SO 4 +Aq, alcohol, ether and acetic acid. (Stahler, B. 1905, 38. 3978.) Divanadyl sulphate, V 2 O 2 (SO 4 ) 2 . Insol. in H 2 O, HC1, or H 2 SO 4 +Aq, but on heating to 400 becomes sol. in H 2 O if heated to 130 therewith. (Gerland.) +4M 2 O. Very slowly sol. in H 2 O at 10, quickly at 60, and still more rapidly at 100. Deliquesces in warm moist air more quickly than it dissolves in H 2 O at 10. Insol. in absolute alcohol. Very sol. in alcohol of 0.833 sp. gr. (Berzelius.) +5H 2 O. (Koppel and Behrendt, Z. anorg. 1903, 36. 168.) +7H 2 O.andlOH 2 O. + 13H 2 O. Efflorescent. (Gerland.) 2V 2 O 4 , 5SO 3 + 18H 2 O. (Gain, C. R. 1906, 143. 1154.) V 2 O 4 , 3SO 3 + 10H 2 O. (G.) 2V 2 O 4 , 7SO 3 +20H 2 O. (G.) 2V 2 O 4 , 9SO 3 +22H 2 O. (G.) V 2 O 4 , 5SO 3 +12H 2 O. (G.) Wtttt Divanadyl hydrogen sulphate, (V 2 2 )H 2 (S0 4 ) 3 = V 2 4 , 3S0 3 +H 2 0. +2H 2 0. +3H 2 O. Deliquescent. Very slowly sol. in cold H 2 O or alcohol. Easily sol. in hot H 2 O. (Gerland.) +5H 2 O. Deliquescent. Insol. in ether. Scarcely sol. in alcohol. Slowly sol. in cold, easily in hot H 2 O, (Crow.) + 14H 2 O. Easily sol. in cold H 2 O or dil. alcohol. (Gerland.) 2VO 2 , 3SO 3 . SI. sol. in H 2 O. (Koppell and Behrendt, Z. anorg. 1903, 35. 163.) 2VOSO 4 , H 2 SO 4 +H 2 O. Very slowly sol. in H 2 O. (Koppel and Behrendt, Z. anorg. 1903, 36. 163.) 2VOSO 4 , 3H 2 SO 4 +15H 2 O. (Gain, C. R. 1906, 143. 1156.) 2VOSO 4 ,4H 2 SO 4 +16H 2 O. (G.) 2VOSO 4 , 5H 2 SO 4 +15H 2 O. (G.) 2VOSO 4 , 7H 2 SO 4 +15H 2 O. (G.) 2VOSO 4 , 8H 2 SO 4 + 16H 2 O. (G.) Ytterbium sulphate, Yb2(SO 4 ) 3 +8H 2 O. Quite slowly sol. in H 2 O even at 100. Anhydrous salt is easily sol. in much H 2 O, but if little H 2 O is used the hydrous salt is formed, which only slowly dissolves. Sol. in K 2 SO 4 +Aq. 100 pts. H 2 O dissolve at: 15.5 35 55 60 44.2 34.6 19.1 11.5 10.4 pts. Yb 2 (SO 4 ) 3 , 70 80 90 100 7.22 6.93 5.83 4.67 pts. Yb 2 (SO 4 ) 3 . (Cleve, Z. anorg. 1902, 32. 143.) Yttrium sulphate, basic, Y 2 O 3 , SO 3 = (YO) 2 S0 4 . Insol. in H 2 O. (Berzelius.) 2Y 2 O 3 , SO 3 +10H 2 O. (Cleve.) Yttrium sulphate, Y 2 (SO 4 ) 3 . Anhydrous. More sol. in H 2 O than the hydrous salt, and more sol. in cold than hot H 2 O. Solution sat. at separates Y 2 (SO 4 ) 3 + 8H 2 O at 50. 100 pts. H 2 O dissolve 15.2 pts. anhydrous salt, at ord. temp. 5.38 pts. are sol. in 100 pts. H 2 O at 25. (James and Holden, J. Am. Chem. Soc. 1913, 35. 561.) Easily sol. in large amount of sat. K 2 SO 4 + Aq, from which 3K 2 SO 4 , 2Y(SO 4 ) 3 is pptd. on warming. (Cleve and Hoglund, Sv. V. A. H. Bih. 1. No. 8.) Solubility of Y 2 (SO 4 ) 3 in Na 2 SO 4 +Aq at 25 Pts. Y 2 (S04)3 per 100 pts. H 2 O Pts. Na 2 S0 4 per 100 pts. H 2 Solid phase 5.61 1.29 6.38 7.40 3.85 6.21 Y 2 (S0 4 ) 3 8.43 8.53 5.86 7.57 4.75 7.72 3.42 10.14 2.36 11.36 - 2.02 13.42 1.90 14.89 1.79 1.86 16.51 18.44 Y 2 (SO 4 ) 3 ,Na 2 SO 4 +2H 2 O 2.99 19.96 3.04 21.05 2.27 27.14 1.52 28.22 1.61 28.13 5.38 0.0 Na 2 S0 4 -flOH 2 O (James and Holden, J. Am. Chem. Soc. 1913, 36. 560.) +8H 2 O. 100 pts. H 2 O dissolve 9.3 pts. of cryst. salt at ord. temp., and 4.8 pts. at 100. (Cleve, Bull. Soc. (2) 21. .344.) Less sol. in H 2 O containing H 2 SO 4 than in pure H 2 O. (Berzelius.) Completely pptd. by HC 2 H 3 O 2 +Aq. In- sol. in alcohol. Yttrium hydrogen sulphate, Y 2 (SO 4 H) 3 . (Brauner, Z. anorg. 1904, 38. 332.) Zinc sulphate, basic, 8ZnO, SO 3 +2H 2 O. Insol. in H 2 O. (Schindler, Mag. Pharm. 31. 181.) 6ZnO,SO 3 +10H 2 O. Insol. in H 2 O. (Kane, A. ch. 72. 310.) 4ZnO, SO 3 +2H 2 O. Scarcely sol. in hot or cold H 2 O. Sol. in ZnSO 4 +Aq. (Kiihn, Schw. J. 60. 337.) SULPHATE, ZINC, BASIC 1033 +3H 2 O. (Werner, B. 1907, 40. 4443.) Solubility of ZnSO 4 in 100 pts. H 2 O at t. +5H 2 O. Nearly insol. in H 2 O. (Haber- mann, M. 6. 432.) Pts Pts Pts. +6H 2 O. (Kraut, Z. anorg. 1897, 13. 5.) + *TTT r\ / A j.l~ /~i T> -i r\'t r>Ti \ t ZnS04 t ZnS0 4 t ZnSO< 7H 2 (J. (Athanasesco, C. R. 103. 271.) -f-8H 2 O. Extremely slowly decomp. bv H 2 O. (Reindel, J. pr. 1869, (1) 106. 373.') 1 44.0 44.6 14 15 52.8 53.5 '27 28 62.1 62.8 + 10H 2 O. (Schindler.) 2 45.2 16 54.2 29 63.6 3ZnO, SO 3 . Insol. in cold, si. sol. in hot .3 45.8 17 54.9 30 64.3 H 2 0. (Vogel.) 4 46.4 18 55.6 31 65.1 2ZnO, SO 3 . (Athanasesco.) 5 47.0 19 56.3 32 65.8 5ZnO, SO 3 . (Pickering, Chem. Soc. 1907, 6 47.6 20 57.0 33 66.6 91. 1986.) 7 48.3 21 57.7 34 67.3 +4H 2 O. (Moody, Am. J. Sci. 1906, [4] 8 48.9 22 58.4 35 68.1 22. 184.) 9 49.5 23 59.2 36 78.8 9ZnO, 2SO 3 + 12H 2 O. (Reindel, J. pr. 1869, 10 50.2 24 59.9 37 69.3 (1) 106. 374.) 11 50.8 25 60.7 38 70.4 Zinc sulphate, ZnSO 4 . Sol. in HoO with evolution of heat. 12 13 51.5 52.2 26 61.4- 39 71.2 Sol. in HCl+Aq. +H 2 O. (Etard.) +2H 2 O. Insol. in alcohol. (Kuhn.) +33^H 2 O. (Anthon.) +5H 2 O. Insol. in boiling alcohol of 0.86 sp. gr. (Kuhn.) +6H 2 O. (Marignac.) +7H 2 O. Slowly efflorescent. M.-pt. of ZnSO 4 +7H 2 O=50. (Tilden, Chem. Soc. 45. 409.) For solubility data on hydrated salts, see below. Sol. in 2 + pts. H 2 O at ord. temp., and in less at 100. (Bergmann.) 100 pts. H 2 O at 104.4 dissolve 81.81 pts. ZnSO*. (Griffiths.) 100 pts. H2O at ord. temp, dissolve 140 pts. ZnSO4 + 7H 2 O. (Dumas.) Sol. in 2.29 pts. H 2 O at 18.75. (Abl.) 100 pts.H 2 O at 15.56 dissolve 140 pts. ZnSO4+7H 2 O. Ure's Diet.) 100 pts. H 2 O at 15 dissolve 140.53 pts. ZnSO 4 + 7H 2 O, and has sp. gr. =1.4442. (Michel and Krafft.) 1 pt. of the crystals dissolves in 0.923 pt. H 2 O at 17.5, and forms a solution of 1.4353 sp. gr. (Karsten.) 100 pts. ZnSO 4 +Aq sat. at 18-20 contain 35.36 pts. ZnSO 4 . (v. Hauer, J. B. 1866. 59.) 100 pts. H 2 O dissolve at: 20 50 75 41.3 53.0 66.9 80.4 pts. ZnSO 4 . (Tobler, J. B. 1865. 309.) 100 pts. H 2 O at 20.5 dissolve 163.2 pts. ZnSO 4 +7H 2 O. (Schiff, A. 109. 336.) 100 pts. H 2 O at t dissolve pts. anhydrous ZnSO 4 , and pts. ZnSO 4 +7H 2 O. t Pts. ZnSO 4 Pts. ZnSO 4 + 7H 2 t Pts. ZnS0 4 Pts. ZnSO4 + 7H 2 O 43.02 115.22 60 74.20 313.48 10 48.36 138.21 70 79.25 369.36 20 53.13 161.49 80 84.60 442.62 30 58.40 190.90 90 89.78 533.02 40 63.52 224.05 100 95.03 653.59 50 68.75 263.84 ...' (Poggiale, A. ch. (3) 8. 467.) Decomp. into basic salt above 40. (Mulder, Scheik. Verhandel. 1864. 74.) If solubility S represents number of pts. anhydrous salt in 100 pts. of solution, S = 27.6+0.2604t from 5 to +81; S = 50.0 0.2244t from 81 to 175. (fitard, C. R. 106. 207.) Sat. ZnSO 4 +Aq contains at: 1 13 20 41 49 29.1 32.6 34.8 40.2 40.9%ZnSO 4 , 55 62 70 77 100 43.4 45.0 47.0 46.5 44.7%ZnSO 4 , 111 12. 137 144 169 171 43.0 40.7 38.0 37.4 30.0 29.0%ZnSO 4 . (fitard, A. ch. 1894, (7) 2. 551.) Transition point from +6H 2 O to +1H 2 O is 70. (fitard.) Solubility of ZnSO 4 +6H 2 O in H 2 O at t. t g. ZnS0 4 in 100 g. H 2 O 5.0 47.08 +0.1 49.48 9.1 54.20 15.0 57.15 25.0 63.74 30.0 65.82 35.0 67.99 39.0 70.08 (Cohen, Z. phys. Ch. 1900, 34. 182.) 1034 SULPHATE, ZINC, BASIC Solubility of the hepta-and hexa-hydrates of ZnSO 4 at t. p=wt. of salt expressed in percent of solu- tion. Sat. ZnSO 4 +Aq at 8 has sp. gr. = 1.421, (Anthon.) t P Sp. gr. of ZnSO 4 +7H 2 O at 20.5. % = %ZnS0 4 +7H 2 0. ' 15.00 15.88 30.70 39.92 39.95 40.73 41.49 46.40 49.97 49.99 50.00 50.02 29.43 29.53 29.49 33.66 33.85 38.46 41.36 41.37 41.43 41.70 42.68 43.51 43.41 43.50 43.51 % Sp. gr. % Sp. gr. % Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 1.0057 1.0115 .0173 .0231 .0289 .0348 .0407 .0467 .0527 .0588 .0649 .0710 .0772 .0835 1,0899 1.0962 1 . 1026 1.1091 1.1156 1 . 1222 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 1 . 1288 1 . 1355 1 . 1423 1 . 1491 1 . 1560 1 . 1629 1 . 1699 1.1770 1 . 1842 1.1914 1 . 1987 1 . 2060 1.2134 1.2209 1.2285 1.2362 1.2439 1.2517 1.2595 1.2674 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 1.2754 1.2834 1.2917 1.3000 .3083 .3167 .3252 .3338 .3424 .3511 .3599 .3688 .3779 .3871 .3964 1.4057 1.4151 1 . 4246 1.4342 1.4439 Transition point from +7H 2 O to +6H 2 O is 39. The formula representing the change of solubility between and 39 is p = 29 . 5 +0 . 270t +0 . 00068t 2 while the expression for the hexahydrate above 40 is p=41.35+0.210t+0.00070t 2 . (Barnes, J. phys. Chem. 1900, 4. 19.) Solubility of ZnSO 4 +7H 2 O in H 2 O at t. (Schiff, A. 110. 72.) Sp. gr. of ZnSO 4 +Aq at 15. % = %ZnS0 4 +7H 2 0. t g. ZnSO 4 in 100 g. H 2 O 5 +0.1 9.1 15.0 25.0 35.0 39.0 39.30 41.93 47.09 50.88 57.90 66.61 70.05 % Sp. gr. % Sp. gr. % Sp. gr. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 .006 .013 .019 .024 .0288 .035 .041 .047 .053 .0593 .066 1.073 1.079 1.085 .0905 .097 .103 .110 .116 .1236 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 .37 38 39 40 1.130 1.137 1.143 .150 .1574 .164 .171 .179 1.185 1 . 1933 1.200 1.209 1.216 1.224 1.231 1.240 1.246 1.255 1.263 1.2709 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 1.280 1.288 1.295 1.304 1.3100 1.320 1.330 1.337 1.346 1.3532 1.362 1.380 1.370 1.390 1 . 3986 1.408 1.416 1.425 1.435 1.4451 (Cohen, Z. phys. Ch. 1900, 34. 182.) Solubility in H 2 O at high pressures: Pressure . in atm. g. ZnSO 4 in 100 g. H 2 O Solubility at 25 1 26 500 26 500 25.8 1000 25.8 1000 25.8 57.95 58.43 58.32 57.95 57.95 57.95 57.92 57.91 57.55 57.55 (Cohen and Sinnige, Z. phys. Ch. 1909, 67. 444.) Liable to form supersaturated solutions. (Gerlach, Z. anal. 8. 288.) SULPHATE, ZINC, BASIC 1035 Sp. gr. of ZnSO 4 +A equivalent to } 1000 g. H 2 O;b 7H 2 O, Yi mol. \ is ZnSO 4 , Y>. me q at 2c 4 mol. = sp. gi 1.5. a = no. of g., wt., dissolved in . if a is ZnSO 4 + 3.5; c = sp. gr. if a =80.5. Sp. gr. of ZnSO 4 +Aq. g. salt in 100 g. solution Sp. gr. vt. = 14 1. wt. = 24.7170 21.4444 17.7573 14.0307 9.7426 5.1110 1.3152 1.2665 1.2145 1 . 1645 1.1106 1.0565 a b c a b 1 2 3 4 5 6 1.077 1.143 1.199 1.249 1.294 1.333 .084 .162 .236 .307 .376 .443 7 8 9 10 11 1.368 1.400 1.428 1.453 1.476 (Charpy, A. ch. 1893, (6) 29. 27.) Sp. gr. of ZnSO 4 +Aq. (Favre and Valson, C. K Sp. gr. of ZnSO 4 +Aq . 79. 968.) at 18. g. equivalents ZnSO4 per liter t Sp. gr. t/t 0.001309 0.002616 0.005212 0.01039 0.09818 0.18842 0.1890 2.493 13.59 13.575 13.573 13.585 13.621 13.642 16.11 15.88 .0001126 .0002258 .0004451 .000886 .008189 .015587 .01550 . 19385 o 1 N tf 5 10 Sp. gr. N & Sp. gr. 1 N Sp. gr. 1.0509 1 . 1369 15 20 1 . 1675 1.2313 32 50 1.3045 1.3788 (Kohlrausch and Hallwachs, W. Ann. 1894, 63. 27.) (Kohlrausch, W. Ann. 1879. 1.) Sp. gr. of ZnSO 4 +Aq at room temp, con taining : 7.12 16.64 23.09%ZnSO 4 . 1.1064 1.1953 1.2814 Sp. gr. of ZnSO 4 +Aq at 18.5, when p = percent strength of solution; d= ob- served density; and w = volume cone. in grams per cc. (Wagner, W. Ann. 1883, 18. 271.) Sp. gr. of ZnS0 4 +Aq at 19.5. p d W 29.22 25.14 21.28 17.08 11.20 8.44 6.65 3.82 3.18 1.46 0.577 1.3718 1.3091 1.2528 1 . 1957 1 . 1220 1.0894 1.0696 1.0387 1.0318 1.0138 1.0045 0.40057 0.32910 0.26659 0.20422 0.12567 0.09195 0.07112 0.03968 0.03281 0.01480 0.00580 Mass of salt per unit mass of solution Density of solution. (g. per cc.) 0.00186 0.00371 0.00556 0.00740 0.01106 0.01469 0.01829 0.02187 0.02542 0.02895 .00179 .00356 .00530 .00711 .01065 .01410 .01753 .02112 .02446 1.02798 (Barnes, J. phys. Chem. 1898, 2. 542.) Sp. gr. of dil. ZnSO 4 +Aq at 20.004. Cone. =g. equiv. per 1. at 20.004. Sp. gr. compared with H 2 O at 20.004 = 1 (McGregor, C. N. 1887, 65. 4.) Sp. gr. of ZnSO 4 +Aq at 25. Cone. Sp. gr. 0.0000 0.0001 0.0002 0.0005 0.0010 0.0020 0.0050 0.0060 1.0100 1.000,000,0 1.000,008,6 1.000,017,2 1.000,043,2 1.000,086,3 1.000,172,3 1.000,429,1 1.000,514,3 1.000,853,9 Concentration of ZnSCh +Aq Sp. gr. 1 normal i / (t 1.0792 1.0402 1.0198 1.0094 1.0047 (Lamb and Lee, J. Am. Chem. Soc. 1913, 35. 1690.) (Wagner, Z. phys. Ch. 1890, 5. 40.) 1036 SULPHATE, ZINC HYDROGEN Sat. ZnSO 4 +Aq boils at 104.4, and solu- tion contains 45 pts. ZnSO 4 to 100 pts. H 2 O. (Griffiths.) Crust forms at 103.5, the solution contain- ing 68 pts. ZnSO 4 to 100 pts. H 2 O. Highest temp, observed, 105. (Gerlach, Z. anal. 26. 426.) B.-pt. of ZnSO 4 +Aq containing pts. ZnSO 4 to 100 pts. H 2 O. B.-pt. Pts. ZnSO4 B.-pt. Pts. ZnSO4 100.5 13.1 103.0 61.0 101.0 25.0 103.5 68.0 101.5 37.7 104.0 74.9 102.0 45.4 104.5 80.7 102.5 53.9 105.0 85.7 (Gerlach, Z. anal. 26 432.) B.-pt. of ZnSO 4 +Aq. g. ZnS0 4 in Rise of the Barometric 100 g. H 2 b. -pt. pressure mm. 2.886 0. 080 743.0 6.647 0. 169 10.139 0. 266 13.389 0. 372 17.713 0. 461 22.202 0. 591 25.199 0. 690 28.249 0. 811 30.470 0. 899 742.0 32.89 0. 995 35.18 1. 122 37.36 1. 240 39.83 1. 381 41.30 1. 459 44.56 1. 671 (Kahlenberg, J. phys. Chem. 1901, 6. 370.) 1 1. absolute H 2 SO 4 dissolves 0.0021 mols. ZnSO 4 at 25. (Bergius, Z. phys. Ch. 1912, 72. 353.) Completely pptd. from ZnSO 4 +Aq by HC 2 H 3 O 2 . (Persoz.) Solubility of ZnSO 4 in KOH+Aq. Mols. KOH to 1 mol. ZnSO4 per cent ZnO in ppt. ,0.25 0.50 1.00 1.62 2.00 3.00 5.00 7.00 13.20 17.11 35.10 68.08 100.00 98.49 96.79 89.76 68.87 0.00 (Linebarger, J. Am. Chem. Soc. 1895, 17. 360.) Difficultly and slowly sol. in sat. NH 4 C1 + Aq, with separation of a double sulphate. Sol. in considerable quantity in sat. NaCl +Aq, without pptn. at first, but finally Na 2 SO 4 separates out. See under NaCl. Sol. in sat. NaNO 3 +Aq as in NaCl+Aq. See under NaNO 3 . Sol. in sat. KNO 3 +Aq with immediate pptn. of double sulphate. (Karsten.) See under KNO 3 . Very rapidly sol. in sat. K 2 SO 4 +Aq, with separation of a double salt. (Karsten.) See under K 2 SO 4 . Abundantly, in sat. CuSO 4 +Aq. Slowly sol. in sat. MgSO 4 +Aq. Very rapidly and abundantly sol. in sat. NaSO 4 +Aq. For solubility of ZnSO 4 +Na 2 SO 4 see under Na 2 SO 4 and Na 2 Zn(SO 4 ) 2 +4H 2 O. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Insol. in alcohol of 0.88 sp. gr. ; 1000 pts. alcohol of 0.905 sp. gr. dissolve 2 pts. (Anthon.) 100 pts. of a saturated solution in 40% alcohol contain 3.48 pts. ZnSO 4 +7H 2 O; 20%, 39 pts.; 10%, 51.1 pts. (Schiff, J. B. 1861. 87.) 100 pts. absolute methyl alcohol dissolve 0.65 pt. ZnSO 4 at 18. (de Bruyn, Z. phys. Ch. 10. 783.) 100 pts. absolute methyl alcohol dissolve 59 pts. ZnSO 4 +7H 2 O at 17. 100 pts. 50% methyl alcohol dissolve 15.7 pts. ZnSO 4 +7H 2 O at 17. (de Bruyn.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) 100 pts. glycerine dissolve 35 pts. ZnSO 4 at ord. temp. (Klever, Bull. Soc. 1872, (2) 18. 372.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790); ethvl acetate. (Naumann, B. 1904, 37. 3601.) Min. Gosslarite. Zinc hydrogen sulphate, ZnH 2 (SO 4 ) 2 +8H 2 O. Somewhat difficultly sol. in cold, easily in hot H 2 O. (v. KobeU, J. pr. 28. 492.) Zinc sulphate ammonia, basic. 4NH 3 . 4ZnO. S0 3 +4H 2 0. Ppt. (Schindler.) Zinc sulphate ammonia, ZnSO 4 , 2NH 3 . +H 2 O. Decomp. by H 2 O into basic zinc sulphate. ZnSO 4 , 4NH 3 +4H 2 O. Sol. in H 2 O. (Kane, A. ch. 72. 304.) +3H 2 O. (Andre, C. R. 100. 241.) ZnSO 4 , 5NH 3 . Sol. in H 2 O with partial decomp. (Rose, Pogg. 20. 149.) Zinc sulphate cupric oxide, ZnSO,, 2CuO-f 5H 2 O. (Mailhe, A. ch. 1902, (7) 27. 169.) ZnSO 4 , 3CuO+sH 2 O. (Recoura, C. R. 1901, 132. 1415.) SULPHURIC VANADIC ACID 1037 +5H 2 0. 2ZnSO 4 , 3CuO + 12H 2 O. (Mailhe, A. ch. Solubility of Zr(SO 4 ) 2 -f-4H 2 O in H 2 SO 4 + Aq at t. Continued, 1902, (7) 27. 169.) 7ZnS0 4 , 24Cu6+zH 2 O. (Recoura, C. R. 1 rw"v~l ! oo i A 1 er \ t g. ZrO 2 g. S0 3 1901, 132. 1415.) 0.33 42.1 Zinc sulphate hydrazine, ZnSO 4 , 2N 2 H 4 . 0.14 46.8 Sol. in NH 4 OH+Aq. (Franzen, Z. anorg. 1908, 60. 278.) 0.13 0.15 47.1 56.7 Sol. in NH 4 OH+Aq without decomp. (Curtius, J. pr. 1894, (2) 60. 345.) ZnH 2 (SO 4 ) 2 , N 2 H 4 . - 1 pt. is sol. in 185 pts. H 2 O at 12. SI. sol. in dil. acids. Decomp. by cone. HNO 3 and by hot cone. H 2 SO 4 . Very sol. in NH 4 OH+Aq. (Curtius, J. pr. 1894, (2) 50. 331.) 0.20 0.27 0.50 0.60 2.00 3.25 4.40 56.8 57.1 57.5 57.8 59.5 60.4 61.4 Zirconium sulphate, basic, 3ZrO 2 , 2SO 3 . 22, 0.10 0.13 56.1 46 ^ Insol. in H 2 O. Sol. in HCl+Aq. (Pay- 0*21 rrU . O 57.2 kull, B. 12. 1719.) 4ZrO 2 , 3SO 3 +14H 2 O. Ppt. Difficulty sol. in H 2 O. (Hauser, B. 1904, 37. 2024.) 3ZrO 2 , SO 3 . Insol. in boiling H 2 O. (Franz, B. 3. 58.) 7ZrO 2 , 6SO 3 . Insol. in H 2 O. (Endemann, J. pr. (2) 11. 219.) ZrO 2 , SO 3 . Sol. in very little H 2 O. More H 2 O decomp. into 3ZrO 2 , 2SO 3 and Zr(SO 4 ) 2 . (Berzelius.) 3ZrO 2 , 4SO 3 + 15H 2 O. Sol. in H 2 O. (Pay- kull.)- 6ZrO 2 , 7SO 3 + 19H 2 O. Sol. in H 2 O. (Pay- kull.) (Hauser, Z. anorg. 1907, 64. 197.) Zirconium hydrogen sulphate, Zr(S0 4 ) 2 , H 2 SO 4 +H 2 0. Solubility in H 2 SO 4 +Aq. at 39.5. 100 g. of the solution contain: 0.11 0.10 0.10 g. ZrO 2 81.4 81.6 81.5 g. S0 3 . (Hauser, Z. anorg. 1907, 54. 200.) +3H 2 O. Solubility in H 2 SO 4 +Aq at t. Zirconium sulphate, Zr(SO 4 ) 2 . 100 g. of the solution contain: Anhydrous. Slowly but completely sol. t g. ZrOa g. S0 3 Sol. in warm H 2 SC>4, but separates on cool- 39.5 4.55 61.5 ing. Precipitated from aqueous solution by 3.25 62.5 alcohol. 3.33 63.8 +4H 2 O. Easily sol. in H 2 O. 3.35 63.8 100 pts. of the solution contain 59.3 pts. 1.80 64.2- of the hydrated salt at 39.5. (Hauser, B. 1.60 64.6 1904, 37. 2025. 1.55 65.0 1.12 66.8 Solubility of Zr(SO 4 ) 2 +4H 2 O in H 2 SO 4 + 0.96 68.4 Aq at t. 100 g. of the solution contain: 22 0.80 66.4 0.65 67.5 t g. ZrO 2 g. S0 3 0.60 68.1 39.5 19.5 25.46 (Hauser, Z. anorg. 1907, 64. 200.) 19.3 25.6 19.6 25.99 Fersulphuric acid, HSO 4 19.3 18.8 26.5 27.0 See Persulphuric acid. 18.15 17.3 27.6 25.3 Pt/rosulphuric acid and pT/rosulphates. 16.2 29.1 See under Sulphuric acid and sulphates. 9.6 - 32.3 5.3 34.7 Sulphuric boric acid. 3.51 1.03 36.01 38.2 See Borosulphuric acid. 0.46 001 39.8 49 Sulphuric vanadic acid, V 2 O 6 , 3SO 8 +3H0 2 . . O -I- ^. . \J See Sulphate, vanadium. 1038 SULPHUROUS ACID, ANHYDROUS Sulphurous acid, anhydrous, SO 2 . See Sulphur efo'oxide. Sulphurous acid, H 2 SO 3 . Known only in aqueous solution, from which SO 2 is given off upon heating. Crys- tallizes in cold, with various amounts of water, forming compounds which approxi- mate H 2 SO 3 +8H 2 O (Pierre, A. 68. 228); H 2 SO 3 +10H 2 O (Dopping, Bull. Ac. St. Petersb. 7. 100); H 2 SO 3 + 14H 2 O (Schon- feld, A. 95. 22); H 2 SO 3 +6H 2 O (Roozeboom, R. t. c. 3. 29, 59, 75, 84; Geuther, A. 224. 218). Crystals are sol. in 2 pts. H 2 O at 10. (Pierre.) For sp. gr. of solutions, etc., see sulphur dioxide. Sulphites. Normal. Only the alkali sulphites are sol. in H 2 O, and they are insol. or only si. sol. in alcohol. Insol. in liquid NH 3 . (Franklin, Am. ch. J. 1898, 20. 824.) Acid. All the acid sulphites are sol. in H 2 O. In general it is rarely possible to determine whether the compd. described is a pure chemical compound or not. It is probable that many substances described by Svenssen and others are isomorphic mixtures whose composition depends upon the temp, and cone, of the solution in which it was pptd. (Rosenheim, Z. anorg. 1900, 25. 72.) Aluminum sulphite, basic, A1 2 O 3 , SO 2 -f 4H 2 O. Insol. in H 2 O; sol. in H 2 SO 3 +Aq. (Four- croy and Vauquelin.) 6A1(OH) 3 ,A1 2 (SO 3 ) 3 +9H 2 O. Ppt. (Seubert, Z. anorg. 1893, 4. 66.) Ammonium sulphite, basic, (NH 4 ) 2 SO 3 , NH 3 + 3 / 2 H 2 0. Sol. in H 2 O. Pptd. from aqueous solution by alcohol. (Muspratt.) Does not exist. (Marignac.) Ammonium sulphite, (NH4) 2 SOs. Very hydroscopic. (Divers, Chem. Soc. 1900, 77. 336.) Insol. in acetone. (Eidmann, C.C. 1899, II. 1014.) +H 2 O. Slowly sol. in H^O. (Muspratt, A. 50. 268.) Sol. in 1 pt. H 2 O at 12. (Fourcroy and Vauquelin, Crell. Ann. 1800. 2. 415.) More sol. in hot H 2 O with evolution of NH 3 . SI. sol. in absolute alcohol. (Mus- pratt.) , Much more sol. in alcohol than K 2 SO 3 . (Pierre.) Loses NH 3 in the air. Sol. in H 2 O. Cone, solution charged with NH 3 will deposit salt on evaporation over KOH. Dil. solution decomp. on evaporation. (Divers, Chem. Soc. 1900, 77. 335.)- Insol. in acetone. 37. 4329.) (Naumann, B. 1904, Ammonium hydrogen sulphite, NH 4 HSO 3 . Insol. in acetone. (Eidmann, C.C. 1899, II. 1014; Naumann, B. 1904, 37. 4329.) Ammonium p?/rosulphite, (NH 4 ) 2 S 2 O 5 . Deliquescent. Very sol. in H 2 O and alcohol. Insol. in ether. (Fock and Kliiss, B. 23. 3149.) Very sol. in H 2 O; very hydroscopic. Aq. solution is si. decomp. on evaporation. (Divers, Chem. Soc. 1900, 77. 336.) Ammonium cadmium sulphite, (NH 4 ) 2 SO 3 , CdSO 3 . Nearly insol. in H 2 C. Partly sol. in excess of H 2 SO 3 +Aq, but separates out on boiling. (Schuler, A. 87. 34.) Ammonium cobaltous sulphite, (NH 4 ) 2 SO 3 , CoSO 3 +o;H 2 O. Decomp. on air. (Berglund, B. 7. 469.) Ammonium cobaltocobaltic sulphite. See Cobaltisulphite, ammonium cobalt. Ammonium cuprous sulphite, (NH 4 ) 2 SO 3 , 2Cu 2 SO 3 +2H 2 0. (Bottinger, A. 51. 411.) (NH 4 ) 2 SO 3 , Cu 2 SO 3 . Insol. in cold, de- comp. by boiling H 2 O. (Rogojski, J. B. 1851. 366.) Decomp. by warming with H 2 O, in which it is insol. Sol. in acids with evolution of SO 2 . (Rosenheim and Steinhauser, 'Z. anorg. 1900, 25. 99.) +2H 2 O. (Commaille, J. B. 1867. 300.) 2(NH 4 ) 2 SO 3 , Cu 2 SO 3 +3H 2 O. Very sol. in H 2 O. Solution decomp. on standing. De- comp. by acids. (Rosenheim and Stein- hauser.) 5(NH 4 ) 2 SO 3 , Cu 2 SO 3 +2H 2 O. Decomp. on air. Sol. in H 2 O with decomp. (Svensson.) 6(NH 4 ) 2 SO 3 , Cu 2 SO 3 +4H 2 O. Easily de- comp. (Rosenheim and Steinhauser.) 7(NH 4 ) 2 SQ 3 , Cu 2 SO 3 +4H 2 O. Very sol. in H 2 O. Solution soon decomp. (Rosenheim and Steinhauser.) + 10H 2 O. Decomp. on air. 81. sol. in warm, less sol. in cold H 2 O.(de Saint-Gilles.) -)-14H 2 O. Decomp. on air. Sol. in H 2 O, but solution decomp. Very easily sol. in mother liquor. (Svens- son, Acta Lund. 1899. 13 .) Ammonium cuprocupric sulphite, (NH 4 ) 2 SO 3 , 2Cu 2 SO 3 ,CuS0 3 +5H 2 O. , Insol. in H 2 O and weak acids. Sol. in NH 4 OH+Aq. (de Saint-Gilles, A. ch. (3) 42. 31.) +6^H 2 O. Ppt. (Rosenheim and Stein- hauser, Z. anorg. 1900, 25. 98.) SULPHITE, ANTIMONY 1039 Ammonium glucinum sulphite, (NH 4 ) 2 O, 2G1O, 3SO 2 +4H 2 O. Ppt. Very unstable in the air. (Rosen- heim, Z. anorg. 1897, 15. 310.) Ammonium gold (aurous) sulphite, 3(NH 4 ) 2 SO3,Au 2 SO3. Very easily sol. in H 2 O. Insol. in alcohol. (Haase, Z. Ch. 1869. 535.) Ammonium gold (aurous) sulphite ammonia, (NH 4 ) 2 SO 3 , 3Au 2 SO 3 , 6NH 3 +H 2 O. Decomp. by H 2 O. Sol. in warm NH 4 OH + Aq, but decomp. by boiling. (NH 4 ;Au 3 (SO 3 ) 2 , 3NH 3 +4H 2 O. Decomp. by H 2 O: (Rosenheim, Z. anorg. 1908, 69. 201.) Ammonium indium sulphite. See Iridosulphite, ammonium. Ammonium iron (ferrous) sulphite, (NH 4 ) 2 SO 3 , FeSO 3 +zH 2 O. (Berglund.) Ammonium iron (ferric) sulphite sulphate, FeSO 3 SO 4 NH 4 +H 2 O. SI. sol. in cold H 2 O. Decomp. by cold dil. HC1. (Hofmann, Z. anorg. 1897, 14. 287.) Ammonium magnesium sulphite, (NH 4 ) 2 Mg 3 (SO 3 ) 4 +18H 2 0. Very si. sol. in H 2 O. (Fourcroy and Vau- quelin.) Sol. in H 2 SO 3 +Aq. +5H 2 O. Much more sol. in H 2 O than MgSO 3 . (Rammelsberg.) Ammonium manganous sulphite, (NH 4 )2SO 3 , MnSO 3 . Relatively easily decomp. by H 2 O. (Berg- lund, Bull. Soc. (2) 21. 213.) Not easily decomp. (Gorgeu, C. R. 96 376.) Ammonium mercuric sulphite, (NH 4 ) 2 SO 3 , HgS0 3 . Very easily sol. in H 2 O, but H 2 O solution gradually decomp., even in the cold. Ammonium nickel sulphite, (NH 4 ) 2 SO 3 , 3NiSO 3 + 18H 2 O. Sol. in H 2 O. (Berglund, B. 7. 469.) Ammonium platinous sulphite. See Platosulphite, ammonium. Ammonium potassium sulphite, 10(NH 4 ) 2 SO 3 , K 2 SO 3 +HH 2 O. Decomp. by H 2 O, etc. (Hartog, C. R 109. 221.) Ammonium scandium sulphate, (NH 4 ) 2 SO 3 , Sc 2 (SO 3 ) 3 +7H 2 O. Insol. in H 2 O. Difficulty sol. in H 2 SO 3 + Aq. (Meyer, Z. anorg. 1914, 86. 281.) Ammonium silver sulphite, (NH 4 ) 2 SO 3 , A g2 S0 3 . Insol. in H 2 O, but gradually decomp. hereby. (Svensson, B. 4. 714.) 6(NH 4 ) 2 SO 3 , Ag 2 SO 3 + 19H 2 O. Sol. in H 2 O without decomp. (Svensson.) 3(NH 4 ) 2 SO 3 , 4NH 4 HSO 3 , Ag 2 SO 3 + 18H 2 O. Easily sol. in H 2 O, but decomp. by warming. Ammonium sodium hydrogen sulphite, NH 4 Na 2 H(SO 3 ) 2 +4H 2 O. Not deliquescent. (Marignac, Ann. Min. 5) 12. 29.) 100 pts. H 2 O dissolve 42.3 pts. salt at 12.4, and 48.5 pts. at 15. (Schwicker, B. 22. 1732.) +5H 2 O =2Na 2 SO 3 , (NH 4 ) 2 S 2 O 5 +H 2 O. ^Tauber, Techn. J. B. 1888. 444.) Ammonium tellurium sulphite, (NH^SOs, TeSO 3 +zH 2 O. Sol. in H 2 O. (Berglund, B. 7. 469.) Ammonium uranyl sulphite, NH 4 (UO 2 )(OH)SO 3 . Insol. in pure H 2 O More sol. in H 2 SO 3 + Aq than the K salt, and less than the Na salt. (Scheller, A. 144. 240.) (NH 4 ) 2 O, 2UO 3 , 3SO 2 . (NH 4 ) 2 O. 4UO 3 , 5SO 2 . (NH 4 ) 2 O', 3UO 3 , 2SO 2 . (NH 4 ) 2 O, UO 3 , 2SO 2 . (Kohlschiitter, A. 1900, 311. 10.) Ammonium vanadium sulphite. See Vanadiosulphite, ammonium. Ammonium vanadyl sulphite, (NH 4 ) 2 SO 3 , VOS0 3 +2H 2 O. Sol. in H 2 O with decomp. (Koppel, Z. anorg. 1903, 36. 184.) (NH 4 ) 2 O, 3VO 2 , 2SO 2 +H 2 O. Sol. in cold H 2 O without decomp. Easily sol. in mineral acids and alkalies. SI. sol. in alcohol and ether. (Koppel Z. anorg. 1903, 36. 182.) Ammonium zinc sulphite, (NH 4 ) 2 SO 3 , ZnSO s . Sol. in H 2 O. (Berglund, B. 7. 469.) Ammonium sulphite mercuric chloride, 2(NH 4 ) 2 SO 3; HgCl 2 . SI. sol. in cold, decomp. by boiling H 2 O. (de St-Giles, A. ch. (3) 36. 95.) Antimony sulphite, Sb 2 O 3 , 3SO 2 (?). Insol. in H 2 O. (Berzelius.) Could not be obtained. (Rohrig, J. pr. (2) 37. 241.) 1040 SULPHITE, BARIUM Barium sulphite, BaSO 3 . Very si. sol. in H 2 O. (Fourcroy and Vau quelin, A. ch. 24. 301.) Sol. in about 46,000 pts. H 2 O at 16 (Autenrieth, Z. anal. 1898, 37. 204.) Sol. in H 2 SO 3 +Aq. Insol. in acetone. (Naumann. B. 1904, 37 4329); methyl acetate. (Naumann, B. 1909 42. 3790.) Solubility in sugar +Aq at t. Solvent t 100 ccm. of solution con- tain g. BaSOs water sucrose +Aq 10 Brix 20 " 30 " 40 " 50 " (sat.)" 60 " 20 0.01974 0.01040 0.00968 0.00782 0.00484 0.00298 0.00223 water sucrose +Aq 10 Brix 20 " 3 o u " 40 " 50 " (sat.)" 60 " 80 0.00177 0.00335 0.00289 0.00223 0.00158 0.00149 0.00112 (Rogowicz, C. C. 1905, II. 1223.) Barium cobaltic sulphite. See Cobaltisulphate, barium. Barium gold (aurous) sulphite, 3BaSO 3 , Au 2 SO 3 +:rH 2 O. Ppt. (Haase.) Barium mercuric sulphite, BaSO 3 , HgSO 3 + H 2 0. Ppt. (Earth, Z. phys. Ch. 9. 196.) Barium mercuric sulphite chloride, BaSO 3 , BaCl 2 , 2HgSO 3 +3^H 2 O. (Earth, Z. phys. Ch. 1892, 9. 208.) Bismuth sulphite, basic, Bi 2 O 3 , 3SO 2 +5H 2 O. Insol. in H 2 O, alcohol, or ether. SI. sol. in H 2 SO 3 +Aq. (Rohrig, J. pr. (2) 37. 241.) (BiO) 2 S0 3 , 3(BiOH)S0 3 +H 2 0. (Seubert and Elten, Z. anorg. 1893, 4. 72-5.) 2(BiO) 2 SO 3 , 3(BiOH)SO 3 +2H 2 O. (S. and E.) 3(BiO) 2 SO 3 , 7(BiOH)SO 3 + 10H 2 O. (S. and E.) 4(BiO) 2 SO 3 , (BiOH)SO 3 +5H 2 O. (S. and E.) 9(BiO) 2 S0 3 , (BiOH)SO 3 +2H 2 O. (S. and E.) Bismuth cobaltic sulphite. See Cobaltisulphite, bismuth. Cadmium sulphite, CdSO 3 . Difficultly sol. in H 2 O. Easily sol. in dil. acids. (Rammelsberg, Pogg. 67. 256.) +2H 2 O. Difficultly, sol. in H 2 O. Sol. in H 2 SO 3 +Aq. Sol. rnNH 4 OH+Aq. Insol. in alcohol. (Muspratt, Phil. Mag. (3) 30. 414.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Contains 2>E 2 O. (Deniges, Bull. Soc. (3) 7. 569.) Cadmium sodium sulphite, 3CdSO 3 , Na 2 SO 8 . Sol. in H 2 O. (Berglund, B. 7. 469.) Cadmium sulphite, ammonia, CdSO 3 , NH 8 . Decomp. by H 2 O. Pol. without decomp. in hot NH 4 OH+Aq. (Rammelsberg, Pogg. 67. 256.) Caesium sulphite, Cs 2 SO 3 . Easily sol. in H 2 O. SI. sol. in alcohol. (Chabrid, C. R. 1901, 133. 297.) Caesium hydrogen sulphite, CsHSO 3 . Easily sol. in H 2 O. SI. sol. in alcohol. (Chabrie", C. R. 1901, 133. 297.) Calcium sulphite, basic, Ca 6 S 6 O 16 = 6CaO, 5SO 2 . (Schott, Dingl. 202. 52.) Calcium sulphite, CaSO 3 +2H 2 O. Slowly effloresces. Sol. in 800 pts. cold H 2 O. (Berzelius.) Insol. in H 2 O. (Rohrig, J. pr. (2) 37. 230.) 0.043 g. is sol. in 1 1. H 2 O at 18. (Weis- berg, Bull. Soc. 1896, (3) 16. 1249.) CaSO 3 equiv. to 78 mg. CaO is sol. in 1 1. H 2 O at 100. (Robart, C. A. 1913. 2500.) Very sol. in H 2 SO 3 +Aq. See CaH 2 (SO 3 ) 2 . InsoL in liquid NH 3 . (Franklin, Am. Ch. J. 898, 20. 827.) CaSO 3 equiv. to 37 mg. CaO is sol. in 1 1. 2% cane sugar +Aq at 100. (Robart, C. A. 1913. 2500.) 0.0825 g. is sol. in 1 1. 10% stigar +Aq. at 8; 0.0800 g. is sol. in 1 1. 30% sugar +Aq. at 8.( Weisberg, Bull. Soc. 1896, (3) 16. 1249.) Insol. in acetone. (Krug and M'Elroy.) Insol. in methyl acetate. (Naumann, B. 909, 42. 3790; ethyl acetate. (Naumann, B. 1904, 37. 3601.) + KH 2 O. (Rammelsberg.) Calcium hydrogen sulphite, CaH 2 (SO 3 ) 2 . Know only in solution. 100 ccm. H 2 O containing 9 g. SO 2 dissolve .553 g. CaSO 3 to form a solution of 1.06 sp. r. (Gerland, J. pr. (2) 4. 119.) Calcium cobaltic sulphite. See Cobaltisulphite, calcium. SULPHITE, CUPROUS POTASSIUM 1041 Cerous sulphite, Ce 2 (SO 8 )j+3H 2 O. More sol. in cold than hot H 2 O. Solution gradually decomposes. (Berthier, A. ch. (3) 7. 77.) Chromous sulphite, CrSO 3 . Precipitate. Insol. in H 2 O. (Moberg.) Chromium sulphite, basic, Cr 2 O 3 , SO 2 . Colloidal modification. Sol. in H 2 O. 2Cr 2 O 3 , SO 2 . Ppt. (Recoura, Bull. Soc. 1898, (3) 19. 169.) Chromic sulphite. Known only in aqueous solution, which pre- cipitates a basic salt on boiling. 2Cr 2 O 3 ,3SO 2 + 16H 2 O. Precipitate. (Dan- son, Chem. Soc. 2. 205.) Chromic potassium sulphite, K 2 O, Cr 2 O, 2SO 2 +zH 2 O. Precipitate. (Berglund, B. 7. 470.) Cobaltous sulphite, basic. Ppt. Decomp. by H 2 O. (Berthier.) Co(OH) 2 , 5CoSO 3 + 10H 2 O. Ppt. (Seu- bert and Elten, Z. anorg. 1893, 4. 89.) Co(OH) 2 , 10CoSO 3 + 15H 2 O. (Seubert and Elten.) Cobaltous sulphite, CoSO 3 . +3H 2 O. Nearly insol. in H 2 O. Sol. in H 2 SO 8 + Aq. (Rammelsberg. ) Partly sol. in NH 4 OH+Aq. +5H 2 O. Insol. in H 2 O. Sol. in H 2 SO 3 + Aq. (Muspratt, A. 30. 282.) Cobaltocobaltic sulphite. See Cobaltisulphite, cobaltous. Cobaltic sulphite with 3M 2 SO 8 . See Cobaltisulphite, M. Cobaltous potassium sulphite, CoSO 8 , K 2 SO 3 +zH 2 0. Insol. in H 2 O; easily sol. in HCl+Aq. (Schultze, J. B. 1864. 270.) Cobaltic potassium sulphite, Co 2 (SO 8 )s, K 2 SO 8 . SI. sol. in H 2 O; easily sol. in H 2 SO 3 +Aq or HCl+Aq. (Schultze.) Cobaltous sodium sulphite, 3CoO, Na 2 O, 3S0 2 . Insol. in H 2 O. Easily sol. in HCl+Aq. (Schultze.) Cobaltic sodium sulphite, Co 2 8 , Na 2 O 3S0 2 . SI. sol. in H 2 O. (Schultze.) Cuprous sulphite, Cu 2 SO 8 +H 2 0. (a) Red. SI. sol. in H 2 O. Sol. in NH 4 OH or HCl+Aq. (Rogojski, J. B. 1861. 366.) Could not be obtained by St. Gilles or Svensson (B. 4. 713). Insol. in H 2 O, alcohol, or ether. (Etard, C. R. 95. 38.) Composition is (Cu 2 ) 8 Hi6(SO 4 ) 8 , "Cuprous isosulphite," according to fitard. + }^H 2 O. Etard's formula, Cu 2 SO 8 +H 2 O s incorrect. The salt 'is almost colorless. (Ramberg I. phys. Ch. 1909, 69. 512.) (j8) White. Normal salt. Insol. in H 2 O, alcohol, or ether. (Etard.) Cupric sulphite, basic, 4CuO, SO 2 +7H 2 O. Insol. in H 2 O, and decomp. by washing therewith. (Millon and Commaille.) 7CuO, 4SO 2 +8H 2 O. Sol. in dil. H 2 SO 4 . (Seubert and Elten, Z. anorg. 1893, 4. 48.) 3CuO, 2SO 2 + 1^H 2 O. SI sol. in H 2 O. (Newbury, Am. Ch. J. 14. 232.) 7CuO, 4SO 2 +8H 2 O, or 4CuSO a , 3Cu(OH) 2 +5H 2 O. Sol. in dil. H 2 SO 4 +Aq. (Seubert and Elten, Z. anorg. 1893, 4. 50.) Cuprocupric sulphite, CuSO 8 , Cu 2 SO 8 +2H 2 O. Nearly insol. in cold H 2 O. Decomp. by boiling. Sol. in H 2 SO 3 +Aq, HC1, or NH 4 OH+Aq. (Berthier.) Sol. in very dil. HNO 3 +Aq. (Dopping, J. B. 1861. 365.) Insol. in H 2 SO 3 , HC 2 H 3 O 2 , or Cu salts +Aq. (de St. Gilles.) +5H 2 O. Insol. in H 2 O. Easily sol. in H 2 SO 3 +Aq, HC 2 H 3 O 2 +Aq, in cupric salts +Aq, NH 4 OH+Aq, or HCl+Aq. (de St. Gilles, A. ch. (3) 42. 34.) Composition is ((^CugHiiiiSO^B^aiHiO, acid cuproso cupric octosulphite." (Etard, C. R. 96. 1475.) Cuprous ferroferric sodium sulphite, Cu 2 O, 2FeO, Fe 2 O 3 , Na 2 O, 6SO 2 +16H 2 O. Sol. in about 1000 pts. H 2 O. Sol. in cold dil. H 2 SO 4 +Aq; sol. in cold dil. HCl+Aq with a residue of Cu 2 Cl 2 . (Stromeyer, A. 109. 237.) Cuprous lithium sulphite, Cu 2 SO 8 , Li 2 SO 3 + 2H 2 0. Insol. in H 2 O, but gradually decomp. thereby. (Etard, C. R. 96. 138.) Cupric mercuric sulphite, CuSOj, HgSO 8 . Sol. in H 2 O in all proportions, but decomp. on boiling. Cuprous potassium sulphite, Cu 2 SO t , K 2 S0 8 (?). (Vohl, J. pr. 95. 219.) +2H 2 O. Sol. in H 2 O with decomp. 1042 SULPHITE, CUPROCUPRIC POTASSIUM (Rosenheim and Steinhauser, Z. anorg. 1890, 25. 96.) Cu 2 SO 3 , 2K 2 SO 3 . (Chevreul, Graham, etc.) Does not exist. (Svensson.) Cu 2 O, 3K 2 O, 6SO 2 +7H 2 O=4KHSO 3 , K 2 SO 3 , Cu 2 SO 3 +5H 2 O. Decomp. by H 2 O. (Svensson, B. 4. 713.) Could not be obtained. (Rosenheim and Steinhauser.) Cu 2 O, 4K 2 O, 8S0 2 +3H 2 O=6KHSO 3 , K 2 SO 3 , Cu 2 SO 3 . Decomp. by HzO. (Svens- son.) Could not be obtained. (Rosenheim and Steinhauser.) Cu 2 SO 3 , 8K 2 SO 3 + 16H 2 O. Sol. in H 2 O with decomp. (Rammelsberg, Pogg. 57. 391.) Does not exist, according to Svensson. Cuprocupric potassium sulphite, 3Cu 2 S0 3 , 3CuSO 3 , K 2 SO 3 . Properties as cuprous potassium sulphite. (Rogojski, J. B. 1851. 367.) 2Cu 2 SO 3 , CuSO 3 , K 2 SO 3 +5H 2 O. Insol. in H 2 O and weak acids, (de St-Gilles.) Cu 2 SO 3 , 4CuSO 3 , JK 2 SO 8 +16H 2 0. De- comp. by H 2 O. (Rosenheim and Steinhauser. Cuprous sodium sulphite, Cu 2 SO 3 , Na 2 SO 3 . +2H 2 O. Decomp. by H 2 O. (Svensson, 1870.) + 11H 2 O. Insol. in cold H 2 O, but decomp. by excess. (Etard, C. R. 95. 138.) 2Cu 2 SO 3 , 3Na 2 SO 3 +29H 2 O. Insol. in H 2 O. (Rosenheim and Steinhauser, Z. anorg. 1900. 25. 94.) Cu 2 SO 3 , 5Na 2 SO 3 +38H 2 O. Decomp. by H 2 O. (Svensson.) Cu 2 SO 3 , 7Na 2 SO 3 -|-19H 2 O. Completely sol. in H 2 O, but solutions decomp. on stand- ing. (Svensson.) ' ' Cuprous sodium oc/osulphite, ' ' (Cu 2 ) 3 Hi Na 16 S 8 O 32 +43H 2 O. (Etard.) 5Cu 2 SO 3 , 2Na 2 SO 3 +30H 2 O. Easily de- comp. (Rosenheim and Steinhauser, Z. anorg. 1900, 25. 94.) Cuprocupric sodium sulphite. Cu 2 SO 3 , 2CuSO 3 , 2Na 2 SO 3 +6H 2 O. Nearly insol. in cold, decomp. by hot H 2 O. (Rosenheim and Steinhauser. Z. anorg. 1900. 25. 95.) +8H 2 O. Decomp. by H 2 O. (Rosenheim and Steinhauser.) Cuprocupric sodium hydrogen sulphite. Na 8 Cu? I (CuDH 2 (S0 4 )8,6H 4 (S04) + 5H 2 O. Insol. in H 2 O. (Etard, C. R. 94. 1422.) (Cu!)CuNa 8 H 18 (S04)8. (Etard.) Copper sodium sulphites. Doubtless many of the compds. described in this class are in reality isomorphic mixtures whose composition depends upon the temp, and cone, of the solution in which pptd. (Rosenheim and Steinhauser, Z. anorg. 1900, 25. 92-95.) Didymium sulphite, Di 2 (SO 3 ) 3 +3H 2 O, or 6H 2 O. Precipitate. Insol. in H 2 O. Sol. in H 2 SO 3 +Aq, from which it is reprecipitated by heating, redissolving on cooling^ (Marignac, A. ch. (3) 38. 167.) Erbium sulphite, Er 2 (SO 3 ) 3 -|-3H 2 O. Precipitate. Glucinum sulphite, basic, 2G1SO 3 , 9G1(OH) 2 +6H 2 O. Ppt. (Seubert, Z. anorg. 1893, 4. 52.) G1SO 3 , G1O. Decomp. by H 2 O or alcohol. (K. and M.) 3G1SO 3 , G1C. Sol. in alcohol. (K. and M.) Glucinum sulphite, G1SO 3 . Decomp. by H 2 O or alcohol. (Kruss and Moraht, B. 23. 734.) Glucinum potassium sulphite, 2G1SO 3 , K 2 SO 3 +9H 2 O. Unstable in the air. (Rosenheim, Z. anorg. 1897, 15. 310.) Gold (aurous) potassium sulphite, Au 2 S0 3 , 3K 2 SO 3 . Very sol. in H 2 O; insol. in alcohol. (Haase.) Gold (auric) potassium sulphite, Au 2 O 3 , 5K 2 O, 8SO 2 +5H 2 O=5K 2 SO 3 , Au 2 (SO 3 ) 8 +5H 2 O. Sol. in H 2 O with decomp. Decomp. by acids; insol. in alkalies. (Fremy, A. 79.* 46.) Gold (auric) potassium sulphite, Au 2 (SO 3 ) 3 , 5K 2 SO 3 +10H 2 O. (Rosenheim and Hertzmann, Z. anorg. 1908. 59. 199.) Gold (auric) potassium sulphite ammonia, Au 2 (SO 3 ) 3 , 3K 2 SO 3 , 4NH 3 +4H 2 O. As the corresponding NH 4 salt. (Rosen- heim and Hertzmann, Z. anorg. 1908, 59. 202.) Gold (aurous) sodium sulphite, Au 2 SO 3 , 3Na 2 SO 3 +3H 2 O. Sol. in less than 1 pt. H 2 O. Insol. in alcohol (Hasse.) +5H 2 O. (Himly.) Gold (auric) sodium sulphite, Au 2 (SO 3 )^, 5Na 2 SO 3 +28H 2 O. As K salt. (Rosenheim and Hertzmann, anorg. 1908, 59. 199.) SULPHITE, MANGANOUS 1043 Gold (aurous) sulphite ammonia, 3Au 2 O, 4S0 2 , 8NH 3 +4H 2 0. SI. sol. in H2O with decomp. Decomp. by acids. SI. sol. in cold, more easily in hot NH 4 OH + Aq. Decomp. by boiling. (Hasse. Zeit. Ch. 1869. 535.) Gold (auric) sulphite ammonia, Au 3 (S0 3 ) 2 , 4NH 3 +4H 2 0. Ppt. Decomp. in moist air and in neutral solution (Herzmann, Z. anorg. 1908. 59. 198.) Indium sulphite, 2In 2 O 3 , 3S0 2 +8H 2 O. Insol. in H 2 O. (Bayer, A. 168. 372.) Iridium sulphite, Ir 2 (SO 3 ) 3 +6H 2 O. Scarcely sol. in H 2 O; easily sol. HCl+Aq. (Birnbaum, A. 136. 179.) Iridyl sulphite, (IrO)SO 3 +4H 2 0. Insol. in H 2 O. Sol. in HC1 or H 2 SO 4 +Aq. (Birnbaum.) Iridous potassium sulphite, IrO, .3K 2 O, 5SO,(f). SI. sol. in H 2 O, more sol. in KOH+Aq. Easily sol. in HCl+Aq. (Glaus, J. pr. 42. 359.) Iridous sulphite potassium chloride. See Iridosulphite, potassium. Iridium sulphite with M 2 SO 3 . See Iridosulphite, M. Iron (ferrous) sulphite, FeSO 3 +2^H 2 O. Very si. sol. in H 2 O. Easily sol. in H 2 SO 3 + Aq. Insol. in alcohol, but sol. therein in presence of SO 2 . (Muspratt.) Iron (ferric) sulphite, Fe 2 O 3 , S0 2 +6H 2 O. Very si. sol. in H 2 Q. Sol. in acids. (Koene.) 2Fe 2 O 3 , 3SO 2 . Deliquescent; decomp. by H 2 O into SO 2 and above comp. 3Fe 2 O 3 , SO 2 +7H 2 O. Ppt. Iron (ferroferric) potassium sulphite, FeSO 3 , (FeO) 2 SO 3 , 2K 2 SO 3 . Ppt. (Berglund.) Iron (ferric) potassium sulphite, K 2 O, Fe 2 O 3 , 3SO S +2H 2 0. Sol. in H 2 SO 3 +Aq. (Koene, Pogg. 63. 453.) Fe 2 O 3 , 2K 2 Q, 3SO 2 +5H 2 O. Ppt. (Mus- pratt, Phil. Mag. (3) 30. 414.) Iron (ferric) potassium sulphite sulphate, FeS0 3 S0 4 K. SI. sol. in cold H 2 O. Sol. in 20% HC1; decomp. on boiling. (Hofmann, Z. anorg. 1897, 14. 286.) Fe(SO 3 ) 2 SO 4 K 3 . Almost insol. in cold H 2 O. Decomp. by boiling with dil. acids. (Hofmann.) Fe 2 (SO 3 ) 4 SO 4 K 4 +5H 2 O. Insol. in cold H 2 O; sol. in cold 20% HCl+Aq; decomp. on boiling with H 2 O. (Hofmann.) Iron (ferric) sodium sulphite sulphate, Fe(SO 3 ) 2 SO 4 Na 3 +6H 2 O. Almost insol. in H 2 O. Decomp. by boiling with dil. acids. (Hof- mann, Z. anorg. 1897, 14. 289.) Iron (ferric) sodium hydrogen sulphite sul- phate, FeSO 4 (SO 3 ) 4 H 2 Na 2 +2H 2 O. Only very si. sol. in H 2 O. (Hofmann.) Lanthanum sulphite, La 2 (SO 3 ) 3 +4H 2 O. Precipitate. (Cleve.) Lead sulphite, PbSO 8 . Insol. in H 2 O. Decomp. by acids. SI. sol. in H 2 SO 3 +Aq. (Rohrig, J. pr. (2) 37. 233.) Lithium sulphite, Li 2 SO 3 +6H 2 O. Sol. in H 2 O; precipitated from aqueous solution by abs. alcohol. (Danson, Chem. Soc. 2. 205.) Sol. in H 2 SO 3 +Aq. +H 2 O. SI. sol. in alcohol, and still less sol. in ether. (Rohrig, J. pr. (2) 37. 225.) +2H 2 O. (Rohrig.) Lithium potassium sulphite, LiKSO+^H 2 O. Easily sol. in H 2 O. (Rohrig, J. pr. (2) 37. 251.) Lithium sodium sulphite, 6Li 2 SO 3 , Na 2 S0 8 + 8H 2 O. Sol. in H 2 O. (Rohrig.) Magnesium sulphite, MgSO 3 +6H 2 0. Sol. in 20 pts. cold, and in less hot H 2 O. (Fourcroy and Vauquelin.) Sol. in 80 pts. cold, and in 120 pts. boiling H 2 O. (Hager, C. C. 1875. 135.) More easily sol. in H 2 SO 3 +Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 828.) Precipitated from aqueous solution by alcohol. +3H 2 O. (Rohrig, J. pr. (2) 37. 234.) Manganous sulphite, MnSO 3 +2H 2 0. Insol. in H 2 O, alcohol, or ether. Easily sol. in acids, also in H 2 SO 3 +Aq. Insol. in acetone. (Naumann, B. 1904, 37. 4329.) +2HH 2 O. (Rammelsberg.) . +3H 2 O. Sol. in 10,000 pts. cold, and 5000 pts. hot H 2 O; more sol. in cone. Mn salts+Aq; sol. in 1000 pts. H 2 CO 3 +Aq. 100 pts. H 2 SO 3 +Aq dissolve 15-17 pts. (Gorgeu, C. R. 96. 341.) 1044 SULPHITE, MANGANOUS POTASSIUM Salt with 2^H 2 O is the only one -which exists. (Rohrig, J. pr. (2) 37. 2.) Manganous potassium sulphite, 2MnSO 3 , K 2 SO. Insol. in H 2 O, even when boiling. (Gorgeu, C. R. 96. 376.) MnSO 3 , K 2 SO 3 . Sol. in H 2 O. (Gorgeu.) Manganous sodium sulphite, MnSO 3 , Na 2 SO 3 +H 2 0. Insol. in hot H 2 O, but decomp. by cold H 2 0. (Gorgeu.) 4MnSO 3 , Na 2 SO 3 . Insol. in H 2 O. (Gor- geu.) Mercuric sulphite, 2HgO, SO 2 . Insol. in H 2 O. Sol. in HC1, alkali sul- phites with subsequent decomp., and in KCN +Aq. (de St-Gilles, A. ch. (3) 36. 80.) HgSO 3 . Decomp. by cold H 2 O. (de St- Gilles.) Does not exist. (Divers and Shimidzu, Chem. Soc. 49. 553.) HgO, 2SO 2 +H 2 O. Sol. in H 2 0, but de- comp. by boiling, (de St-Gilles.) Exists only in aqueous solution. (Divers and Shimidzu.) Mercuromercuric sulphite, Hg 3 (SO 3 ) 2 + 2H 2 O = Hg 2 SO 3 , HgS0 3 . Very efflorescent. Insol. in H 2 O. Decomp. by hot H 2 O. Insol. in dil. HNO 3 or H 2 SO 4 + Aq. +4H 2 O. Very efflorescent. Ifypomercurosic sulphite, Hg 4 (S0 3 ) 2 +H 2 O. Insol. in H 2 O, but easily decomp. on stand- ing therewith. Almost absolutely insol. in dil. HNO 3 or H 2 S0 4 +Aq. (Divers and Shimidzu.) Mercuric orn/sulphite, Hg(SO 2 OHgO) 2 Hg+ H 2 O. Insol. in H 2 O. Decomp. by hot H 2 O. In- sol. in dil. HNO 3 or H 2 SO 4 +Aq. Sol. in H 2 SO 3 -|-Aq. (Divers and Shimidzu.) Mercuric potassium sulphite, basic, K 2 O, 2HgO, 2SO 2 . (Earth. Z. phys. Ch. 1892, 9. 210.) K 2 O, 3HgO, 3SO 2 . Insol. in H 2 O. Partly sol. in KOH+Aq. (Barth.) Mercuric potassium sulphite, HgSO 3 , K 2 SO 3 +H 2 0. SI. sol. in cold H 2 O. Decomp. on boiling, (de St-Gilles, A. ch. (3) 36. 90.) Mercuric potassium sulphite mercuric chloride, K 2 Hg(S0 3 ) 2 , HgCl 2 . Decomp. by H 2 O. (Barth, Z. phys. Ch. 1892, 9. 206.) Mercuric silver sulphite, HgSO 3 , Ag 2 SO 3 + 2H 2 O. Decomp. rapidly; insol. in H 2 O. (Barth,, Z. phys. Ch. 9. 195.) Mercuric sodium sulphite, HgS0 3 , Na 2 SO 8 + H 2 O. Sol. in H 2 O. (de St-Gilles.) Sol. in 25 pts. cold H 2 O, and decomp. on heating. (Divers and Shimidzu.) +2H 2 O = Na 2 (SO 3 ) 2 Hg+2H 2 O. (Barth, Z. phys. Ch. 9. 193.) 2HgSO 3 , Na 2 SO 3 +H 2 O. Much more sol. in H 2 O than the above comp. especially on heating, (de St-Gilles.) Does not exist. (Divers and Shimidzu.) Mercuric strontium sulphite, HgS0 3 , SrSO 8 + 2H 2 O. Ppt. (Barth.) Mercuric sulphite ammonium bromide, HgSO 3 , NH 4 Br. As NH 4 C1 comp. (Barth, Z. phys. Ch. 1892, 9. 215.) Mercuric sulphite ammonium chloride, HgS0 3 , NH 4 C1. As K salt. (Barth.) Mercuric sulphite potassium chloride, HgSO 3 , KC1. Sol. in H 2 O. (Barth.) Mercuric sulphite sodium chloride, HgSO, NaCl+H 2 0. Sol. in H 2 O. (Barth.) Nickel sulphite, basic, 2NiSO 3 , Ni(OH) 2 + 6H 2 O. Ppt. (Seubert and Elten, Z. anorg. 1893, 4.91.) Nickel sulphite, NiSO 3 +4H 2 0. Insol. in H 2 O. Sol. in HCl+Aq. with evolution of SO 2 . (Muspratt, A. 60. 259.) +6H 2 O. Insol. in H 2 O. Sol. in H 2 SO 3 + Aq. (Rammelsberg, Pogg. 67. 391.) Nickel sulphite ammonia, NiSO 3 , 3NH 8 + 3H 2 0. Sol. in little H 2 O. Decomp. by much H 2 or heat. (Rammelsberg, Pogg. 67. 245.) Osmious sulphite, OsSO 8 . Insol. in H 2 O. Easily sol. in HCl+Aq without evolution of SO 2 . Very slowly de- comp. by KOH+Aq. (Claus.) Osmious potassium sulphite, OsS0 8 , 2K 2 SO, 2KHSO 3 +4H 2 O. Nearly insol. in H 2 O. SULPHITE, SCANDIUM 1045 Osmious potassium sulphite chloride, OsO, 2S0 2 , 6KC1. Easily sol. in H 2 O. PaUadous sodium sulphite, PdSO 3 , 3Na 2 S0 3 Na6Pd(SO 3 ) 4 +2H 2 O. Sol. in hot H 2 O. Sol. in NaOH+Aq or H 2 SO 3 +Aq. (Wohler and Frerichs, A. 174. 199.) Platinous sulphite, PtO 2 , 2SO 2 . Easily sol. in H 2 O or alcohol. (Dobereiner, J. pr. 16. 315.) Formula is PtSO 3 . (Gmelin.) PtSO 3 , H 2 SO 3 . (Birnbaum, A. 139. 172.) Platinic potassium sulphite, PtO 2 , S0 2 , K 2 S0 3 +H 2 0. Sol. in KOH+Aq. (Birnbaum, A. 139. 173.) Platinic sodium sulphite, PtO 2 , SO 2 , 2Na 2 SO 3 +2H 2 0. Sol. in H 2 O. (Birnbaum.) Platinous sulphite with M 2 SO 3 . See Platosulphite, M. Platinum sulphite ammonium chloride. See Chloroplatosulphite, ammonium. Potassium sulphite, K 2 SO 3 -f2H 2 O. Somewhat deliquescent. Sol. in 1 pt. cold, and still less hot H 2 O. (Fourcroy and Vau- quelin, A. ch. 24. 254.) Insol. in liquid NH 3 . (Franklin. Am. Ch. J. 1898, 20. 829.) Very slightly soluble in alcohol. Insol. in ethyl acetate. (Casaseca, C. R. 30. 821.) Potassium hydrogen sulphite, KHSO 3 . Sol. in H 2 O. Insol. in absolute alcohol. Potassium p^/rosulphite, K 2 S 2 O 6 . Slowly sol. in H 2 O. Very si. sol. in alcohol; insol. in ether. (Muspratt, A. 50. 259.) Potassium rhodium sulphite, 3K 2 SO 8 , Rh 2 (SO 3 ) 3 +6H 2 O. See Rhodosulphite, potassium. Potassium ruthenium sulphite, O[Ru(S0 3 ) 4 K6J 2 +2H 2 O. Ppt. (Miolati, C. C. 1901, 1. 501.) Potassium sodium sulphite, KNaSO 8 . Sol. in H 2 O. (Spring, B. 7. 1161.) + 1, and 2H 2 O. (Schwicker, B. 22. 1731.) Isomeric salts, KSO 3 Na and NaSO 3 K. (Earth, Z. phys. Ch. 9. 176.) Potassium sodium hydrogen sulphite, KNa 2 H(SO 3 ) 2 +4H 2 0. Easily sol. in H 2 O; 100 pts. H 2 O dissolve 69 pts. salt at 15. (Schwicker, B. 22. 1731.) K 2 NaH(SO 3 ) 2 +3H 2 O. (Schwicker.) Potassium uranyl sulphite, K(UO 2 )(OH)SO 8 . Insol. in H 2 O, but sol. in H 2 SO 3 +Aq. (Scheller.) K 2 O, 2UO S , 3SO 2 . (Kohlschiitter, A. 1900, 311. 10 et sea.) K 2 O, 4UO 3 , 5SO 2 . (K.) K 2 O, 3UO 3 , 2SO 2 . (K.) K 2 O, U0 3 , 2SO 2 . (K.) Potassium vanadium sulphite. See Vanadiosulphite, potassium. Potassium vanadyl sulphite, K 2 SO 3 , Sol. in H 2 O without decomp. and can be recryst. therefrom. (Koppel and Behrendt, B. 1901, 34. 3932.) K 2 O, 3VO 2 , 2SO 2 . Sol. without decomp. m cold and hot H 2 O.' Insol. in alcohol and ether. (Koppel, Z. anorg. 1903, 36. 182.) Potassium zinc sulphite, K 2 SO 3 , 3ZnS0 3 + Sol. in H 2 O with decomp. (Berglund, Acta Lund. 1872.) Rhodium sulphite, Rh 2 (SO 3 ) 3 +6H 2 O. Sol. in H 2 O. Insol. in alcohol. (Claus.) Rhodium sodium sulphite. See Rhodosulphite, sodium. Ruthenium sulphite, Ru 2 (S0 3 ) 8 . Colloidal substance, sol. in a large quantity of H 2 O. (Lucchesi, Gazz. ch. it. 1900, 30. (2) 71.) Ruthenium sodium sulphite, Na 7 Ru(SO 3 ) 5 +2H 2 0. Ppt. (Miolati, C. C. 1901, I. 501. Samarium sulphite, Sm 2 (SO 3 ) 3 . Amorphous precipitate. (Cleve.) Scandium sulphite, Sc 2 (SO 8 )3. Insol. in cold H 2 O. SI. sol. in hot H 2 O. Sol. in excess of sodium sulphite when heated. (Crookes, Phil. Trans. 1910, 210. A. 363.) +6H 2 O. Very si. sol. in H 2 O. Decomp. by boiling with H 2 O' with separa- tion of H 2 SO 3 . (R. J. Meyer. Z. anorg. 1914, 86.281.) 1046 SULPHITE, SELENIUM Selenium sulphite, SeS0 3 . Correct composition for "selenium sulph- oxide." (Divers, Chem. Soc. 49. 583.) Silver sulphite, Ag 2 SO. Very si. sol. in cold H 2 O. Decomp. on heating. Solubility in H 2 O is < 1:20,000. (Bau- bigny, C. R. 1909, 149. 858.) Easily sol. in NH 4 OH+Aq, and alkali sulphites+Aq. Insol. in H 2 SO 3 +Aq. .De- comp. by strong acids, but not by acetic acid. (Berthier, A. ch. (3) 7. 82.) _ Easily sol. in alkali thiosulphates+Aq. (Herschel.) Cold NaHSOs+Aq dissolves a considerable amount of Ag 2 SO 3 . ('Rosenheim and Stein- hauser, Z. anorg. 1900, 25. 78.) Practically insol. in HNO 3 +Aq or dil. AgNOs+Aq, also in H 2 SO 3 +Aq. (Divers, Chem. Soc. 49. 579.) Silver sodium sulphite, Ag 2 SO 3 , Na 2 SO 8 -f- H 2 0. Decomp. by H 2 O. (Svensson, B. 4. 714.) Sodium sulphite, Na 2 SO 8 . 100 pts. dissolve at 0, 14.1 pts.; at 20, 25.8 pts. ; at 40, 49.5 pts. Na 2 SO 3 . (Kremers, Pogg.,99. 50.) Maximum solubility is at 33. (Mitscherlich.) Solubility in 100 pts. H 2 O at t. t Pts. NazSOs 37.2 44.08 33.5 39.64 29.0 34.99 23.5 29.92 18.2 25.31 10.6 20.01 5.9 17.61 2.0 14.82 1.9 13.09 t Pts. Na 2 SO 3 60.4 59.8 59.8 59.8 28.29 28.29 28.65 28.75 37.0 37.0 47.0 47.0 55.6' 84.0 28.01 28.07 28.19 28.07 28/21 28.26 The temp, at which Na 2 SO 3 +7H 2 O changes into Na 2 SO 3 is about 21.6. (Hartley and Barrett, Chem. Soc. 1909, 95. 1183.) See also +7H 2 O. Sp. gr. of sat. solution at 15 = 1.21. (Greenish and Smith, Pharm. J. 1901, 66. 774.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. Insol. in ethyl acetate. (Casaseca, C. R. 30. 821.); methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in benzonitrile. (Naumann, B. 1914, 47. 1370.) -f-7H 2 O. Decomp. slowly on air. Sol. in 4 pts. H 2 O at 15 with absorption of heat (Dumas), and in 1 pt. boiling H 2 O (Fourcroy) . Solubility in 100 pts. H 2 O at t. Supersolubility curves have also been plotted for ice and Na 2 SO 3 +7H 2 O. (Hartley a'nd Barrett, Chem. Soc. 1909, 95. 1181.) +10H 2 O. Efflorescent. Somewhat less sol. than above salt. (Muspratt.) Sodium hydrogen sulphite, NaHSO 3 . : More difficulty sol. in H 2 than NaHCO 3 , and is precipitated by alcohol from aqueous solution. (Muspratt.) Insol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4329) methyl acetate. (Naumann, B. 1909, 42. 3790.) +4H 2 O. (Clark.) Sodium pyrosulphite, Na 2 S 2 6 . Decomp. gradually on the air. Sodium uranyl sulphite, Na(U0 2 )(OH)SO 3 . SI. sol. in H 2 O. More sol. in H 2 S0 3 +Aq than the K salt. (Scheller.) Na 2 O, 2UO 3 , 3SO 2 . : Na 2 O, 3UO 3 , 2SO 2 . (Kohlschutter; A. 1900, 311. 10 et seq.) Sodium vanadyl sulphite, Na 2 O, 2SO 2 , V0 2 +5H 2 0. Sol. in H 2 O with decomp. Na 2 O, 2SO 2 , 3VO 2 +4H 2 O. Sol. in cold H 2 O; decomp. on heating. (Koppel, B. 1901, 34. 3933.) Sodium zinc sulphite, Na 2 S0 3 , 3ZnS0 3 -f Sol. in H 2 O with decomp. (Berglund. Acta Lund, 1872.) Sodium sulphite silver chloride, 3Na 2 S0 8 , AgCl+21H 2 (X Sol. in H 2 O. (Svensson.) SULPHURYL TITANIUM CHLORIDE 1047 Strontium sulphite, SrSO 3 . Precipitate. Almost insol. in H 2 O. Sol. in H 2 SO 3 +Aq. (Muspratt.) Sol. in about 30,000 pts. H 2 O at 16-18. (Autenrieth, Z. anal. 1898, 37. 293.) Abundantly sol. in H 2 SO 3 +Aq. (Rohrig.) Tellurium sulphite, TeSO. Correct composition of "tellurium sulph- oxide." (Divers, Chem. Soc. 49. 583.) Thallous sulphite, T1 2 SO 3 . SI. sol. in cold, easily in hot HjSOs+Aq. (Rohrig, J. pr. (2) 37. 229.) 100 pts. H 2 O dissolve 3.34 pts. at 15.5. Easily sol. in hot H 2 O; insol. in alcohol. (Seubert and Elten, Z. anorg. 2. 434.) Thallous vanadyl sulphite, 2T1 2 SO 8 , V 2 3 S0 3 +4H 2 0. (Gain, A. ch. 1908, (8) 14. 278.) T1 2 SO 3 , 3V 2 O 3 SO 3 +8H 2 O. (Gain.) Thorium sulphite, Th(SO 3 ) 2 +H 2 O. Precipitate. (Cleve.) Tin (stannous) sulphite, 5SnO, 2SO 2 -fzH 2 O. Ppt. Partly sol. in H 2 SO 3 +Aq. (Rohrig, J. pr. (2) 37. 249.) +20HoO. (Rohrig.) 8SnO, 2SO 2 +20H 2 O. HSnO, 2SO 2 +20H 2 O. (Rohrig.) Uranous sulphite, basic, U(OH) 2 SO 8 +H 2 0. Insol. in H 2 O. Easily sol. in acids. Sol. in H 2 SO 3 +Aq, but is, soon decomp. (Ram- melsberg.) Uranyl sulphite, basic, 3UO 2 (OH) 2 , 5(UO 2 )SO 3 +10H 2 0. (Seubert and Elten, Z. anorg. 1893, 4. 80.) Uranyl sulphite, (UO 2 )SO 8 +4H 2 O. Insol. in H 2 O. Sol. in H 2 SO 3 +Aq or alco- holic solution of SO 2 . (Rohrig, J. pr. (2) 37. 240.) Vanadyl sulphite, 3VO 2 , 2SO 2 +4^H 2 O. Decomp. slowly on standing. Sol. in H 2 O without apparent decomp. (Koppel, Z. anorg. 1903, 35. 186.) 2V 2 O 4 , 3SO 2 -MOH 2 O. Sol. in H 2 O; aq. sol. decomp. on boiling giving off SO 2 and forming V 2 O 4 , 2H 2 O. (Gain, C. R. 1906, 143. 824.) Vanadyl zinc sulphite, ZnO, 3VO 2 , 2SO 2 . Decomp. slowly in the air. Sal. in H 2 O without decomp. (Koppel, Z. anorg. 1903, 35. 183.) Ytterbium sulphite, Yb 2 (SO 3 ) 8 +9H 2 O. Insol. in H 2 O. (Cleve, Z. anorg. 1902, 32. 143.) Yttrium sulphite, Y 2 (SO 3 ) 3 +3H 2 O. SI. sol. in H 2 O. (Cleve.) Zinc sulphite, basic, 2ZnSO 3 , 3Zn(OH) 2 . (Seubert, Arch. Pharm. 229. 321.) ZnSO 3 , Zn(OH) 2 +H 2 O. (Seubert.) Zinc sulphite, ZnSO 3 +2, and 2V 2 H 2 O. Very si. sol. in H 2 O. 100 pts. H 2 O dissolve 0,16 pt. ZnSO 3 +2H 2 O. (Henston and Tich- borne, Brit. Med. J. 1890. 1063.) Easily sol. in H 2 SO 3 +Aq. (Koene.) Sol. in NH 4 OH+Aq. Insol. in alcohol. Decomp. into basic salt by boiling H 2 O. (Seubert, Arch. Pharm. 229. 1.) Zinc sulphite ammonia, ZnSO 8 , NH 8 . Decomp. by H 2 O. Sol. in NH 4 OH+Aq, (Rammelsberg, Pogg. 67. 255.) Zirconium sulphite. Insol. in H 2 O. Somewhat sol. in H 2 SO 3 -f Aq, from which it is repptd. on boiling. Sol. in (NH 4 ) 2 SO3+Aq, from which Zr hydroxide is pptd. on boiling. (Berzelius.) Zr(SO 3 ) 2 +7H 2 O. Ppt. (Venable, J. Am. Chem. Soc. 1895, 17. 449.) Sulphuryl bromide, S0 2 Br 2 . (Odling, Chem. Soc. 7. 2.) Does not exist. (Sestini, Bull. Soc. 10. 226; Melsens, C. R. 76. 92; Michaelis.) ' ' ^*i^BI^HHHp^*^' ^^ Sulphuryl chloride, SO 2 C1 2 . Decomp. by H 2 O and alcohol. Decomp. by moist air, water, or abs. alcohol; more rapidly by alkalies, HC1, SO 2 , etc. '(Schiff, A. 102. 111.) +H 2 O. Only si. sol. in H 2 O at with slow decomp. (Baeyer, B. 1901, 34. 737.) -f-15H 2 O. SI. sol. in H 2 O at and stable therein for several hours. (Baeyer.) ZH'sulphuryl chloride (P?/rosulphuryl chlor- ide), S 2 O 6 C1 2 . Decomp. slowly with H 2 O. (Rose, Pogg. 44. 291.) Sol. in CC1 4 and CHC1 8 ; miscible with h'quid SO 8 . Sulphuryl hydroxyl chloride, SO 3 HC1=QSO 2 . Decomp. on moist air, and violently with H 2 O. Not miscible with CS 2 . Decomp. with alcohol. Sulphuryl titanium chloride, SO 8 . TiCl4 = TiCl 3 OSO 2 Cl. Slowly deliquescent. (Clausnitzer, B. 11* 2011.) 1048 SULPHURYL CHLORIDE STANNIC OXYCHLORIDE ZH'sulphuryl chloride stannic oxychloride, 5S 2 O 5 C1 2 , 4SnOCl 2 . Sol. in a little H 2 O, but decomp. by more H 2 O. (Rose, Pogg. 44. 320.) Sulphuryl fluoride, SO 2 F 2 . 1 pt. is sol. in 10 pts. H 2 O at 9. 3 vol. are sol. in 1 vol. alcohol at 9;insol. in cone. H 2 SO 4 at 66; sol. in aq. solution of KOH, Ca(OH) 2 , Ba(OH) 2 and in alcoholic solution of alkalies. (Moissan, C. R. 1901, 132. 377.) Sulphuryl hydroxyl fluoride, HSOF. Violently decomp. by H 2 O. (Thorpe and Kirwan, Z. anorg. 3. 63.) Sulphuryl peroxide, S0 4 . See Sulphur heptoxide. Sulphydric acid. See Hydrogen Sulphide. Sulphydroxyl. See Sulphhydroxyl. Tantalic acid, H 4 Ta 2 O 7 (?). Sol. in HF (Rose), and KH 3 (C 2 O 4 ) 2 +Aq (Gahn, Schw. J. 16. 437). At the instant of precipitation is sol. in various acids. (Rose.) Aluminum tantalate. Insol. in H 2 O. (Berzelius.) Ammonium fozatantalate, (NH 4 )tH7Ta 7 Oi 9 +H 2 0. Somewhat, sol. in H 2 O. (Rose, Pogg. 102. 57.) Barium fozatantalate, Ba 4 Ta80 19 +6H 2 O. SI. sol. in H 2 O. (Rose.) Cajsium tantalate, 4Cs 2 O, 3Ta 2 O 6 +14H 2 O. Completely sol. in a small amount of hot H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1908, 30. 1666.) 7Cs 2 O, 6Ta 2 O 6 +38H 2 O. Pptd. from its aqueous solution by alcohol. (Smith.) Ferrous tantalate, Fe(TaO). Min. Tantalite. 5FeO, 4Ta 2 O 6 . Min. Tapiolite. Magnesium ftezatantalate, Mg 4 TaeOi+ 9H 2 O, Ppt. (Rose, Pogg. 102. 61.) 4MgO, Ta 2 O 5 . Insol. in H 2 O. (Joly, C. R. :81. 266.) Mercurous tantalate, 5Hg 2 O, 4Ta 2 Q 6 -f-5H 2 O. Decomp. by warm HNO 3 -f-Aq (1.21 sp. gr.) -with separation of Ta 2 O 5 . (Rose, Pogg. 102. Potassium tantalate, KTaO 8 . Insol. in H 2 O. Sol. in KOH+Aq. (Marig- nac, A. ch. (4) 9. 249.) Potassium fcezatantalate, K 8 Ta 6 O 19 +16H 2 0. Sol. without decomp. in moderately warm H 2 O. Decomp. by boiling. (Marignac, A. ch. (4) 9. 259.) Rubidium tantalate, 4Rb 2 O, 3Ta 2 O 5 + 14H 2 O. Sol. in H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1908, 30. 1666.) Silver tantalate, 4Ag 2 O, 3Ta 2 O 6 .. Completely sol. in NH 4 OH+Aq. HNO 3 + Aq dissolves Ag 2 O, and Ta 2 Os separates out. (Rose, Pogg. 102. 64.) Sodium tantalate, NaTaO 8 . Insol. in H 2 O. (Rose.) Sodium Aezatantalate, Na 8 Ta6O 19 +25H 2 O. 1 pt. salt, dissolves in 493 pts. H 2 O at 13.5, and in 162 pts. at 100. Very slightly sol. in alcohol. Insol. in alkaline solutions. (Rose.) Pertantalic acid. See Pertantalic acid. Tantalum, Ta. Not attacked by HC1, HNO 3 , aqua regia, or hot cone. H 2 SO 4 . Easily sol. in a mixture of HNO 3 and HF (Berzelius, Pogg. 4. 6; Rose). Also sol. in HF alone (Berzelius.) Not attacked by alkali hydrates +Aq. Insol. in single acids and in aqua regia. Oxidized by a mixture of HF and aqua regia. (Moissan, C. R. 1902, 134. 211.) Pure Ta is insol. in boiling H 2 SO 4 , HNO 8 , HC1, aqua regia or mixtures of these acids; slowly sol. in HF-f Aq. (v. Bolton, Zeit. Elektrochem. 1905, 11. 45.) Tantalum bromide, TaBr 6 . Decomp. by H 2 O. (Rose.) Tantalum ^chloride, TaCl 2 +2H 2 O. Sol. in H 2 O when freshly prepared, brie", C. R. 1907, 144. 805.) (Cha- Tantalum pewfczchloride, TaCl 6 . Takes up H 2 O from the air without deli- quescing. Decomp. by H 2 O. Sol. in H 2 SO 4 . Sol. in cold HCl-fAq to a cloudy liquid, which gelatinises after a time. Not com- pletely sol. in boiling HCl+Aq, and the solution does not gelatinise by the subsequent addition of water, but all goes into solution. Partly sol. in KOH +Aq. Insol. in K 2 SO 3 + Aq. Sol. in absolute alcohol. TELLURATE, CAESIUM HYDROGEN 1049 Tantalum pentofluoride, TaF 6 . Solubility in H 2 O. Very hydroscopic; sol. in H 2 O. (Ruff, B. * >r _!_, 1909, 42. 494.) Mols TT (~\ 4. MOlS H 2 TeO4 Solid phase Temp. % JC12U tO Iw.^1 to 100 Tantalum fluoride with MF. H 2 TeO4 . mol H 2 TeO4 mols H 2 O See Fluotantalate, M. Tantalum hydroxide, Ta a O 6 , zH,O. H 2 TeO 4 +6H 2 O tc 5 13.92 17.84 66.2 49.2 1.51 2.03 See Tantalic acid. 11 10 26.21 30.2 3.31 . tf 15 32.79 21.9 4.55 Tantalum nitride, TaN. H 2 TeO 4 .2H 2 O 10 25.29 31.7 3.15 Not sol. in any acids, except a mixture of HF and HNO 3 . (Rose, Pogg. 100. 146.) i 18 30 28.90 33.36 26.2 21.4 3.82 4.67 Ta 3 N 5 . (Joly, Bull. Soc. (2) 26. 506.) t 40 60 36.38 43.67 18.8 14.2 5.33 7.04 Tantalum dioxide, Ta 2 O 2 (?). 1 80 51.55 10.07 9.93 Sol. in HF with evolution of hydrogen. i 100 60.84 6.89 14.52 (Hermann, J. pr. (2) 6. 69.) (Mylius, B. 1901, 34. 2211.) Tantalum tefr-oxide, Ta 2 O 4 . Not attacked by any acid, not even a mix- ture of HNO 3 and HF. (Berzelius, Pogg. 4. 20.) Decomp. by HC1. (Smith, Z. anorg. 1894, 7. 98.) Tantalum pen toxide, Ta a 8 . Insol. in any acid, even boiling H 2 SO 4 or in HF. (Berzelius.) Sol. in fused KHSO 4 ,, 10 pts. being necessary to dissolve 1 pt. Ta 2 O 5 . Tantalum silicide, TaSi 2 . Insol. in most inorganic acids. Sol. in HFandinHF+HNO 3 . Decomp. by fused alkali hydroxides. (Hon- igschmid, M. 1907, 28. 1027.) Tantalum sulphide, Ta 2 S 4 . Not attacked by HCl+Aq. Oxidised by boiling with HNO 3 +Aq,- more rapidly with aqua regia. Attacked by H 2 SO 4 on heating. Not completely sol. in HF or a mixture of HF and HN0 3 . Telluretted hydrogen, TeH 2 . See Hydrogen telluride. Telluric acid, H 2 TeO 4 . Insol. in H 2 O, cold cone. HC1, hot HNO 3 , or boiling KOH+Aq, but when heated with H 2 O is gradually converted into H 2 TeO 4 + 2H 2 O and dissolved. +2H 2 O. Very slowly sol. in cold H 2 O, but sol. in hot H 2 O in every proportion. Insol in absolute alcohol; sol. in dil. alcohol ac- cording to the amount of H 2 O present. Sol in acids and alkalies. Insol. in alcohol or Insol. in alcohol; sol. in NaOH+Aq (Mylius, B. 1901, 34. 2216.) Stable in the air. Sol. in H 2 O; pptd. by HNO 3 . (Stauden maier, Z. anorg. 1895, 10. 191.) +6H 2 O. Obtained from solutions at 0. Staudenmaier, Z. anorg. 1895, 10. 191.) AKotelluric acid, H 2 TeO 4 . Miscible with H 2 O. Sol. in alcohol; pptd. by NaOH+Aq but sol. in excess. (Mylius, B. 1901, 34. 2216.) Tellurates. Neutral alkali salts are sol. in H 2 O; the acid salts are only si. sol. therein, but dissolve in HCl+Aq. Aluminum tellurate. Ppt. Sol. in excess of aluminum salts +Aq. (Berzelius.) Ammonium tellurate, (NH 4 ) 2 TeO 4 . Slowly but completely sol. in H 2 O. SI. sol. in NH 4 OH+Aq or NH 4 Cl+Aq. SI. sol. in alcohol. (Berzelius.) (NH 4 ) 2 O, 2TeO 3 . SI. sol. in H 2 O, but more sol. than the corresponding K salt. (NH 4 ) 2 O, 4TeO 3 . Very si. sol. in H 2 O. Insol. in alcohol. (Berzelius.) Barium tellurate, BaTeO 4 +3H 2 O. SI. sol. in cold, more in boiling H 2 O. Easily sol. in HNO 3 +Aq. (Berzelius.) BaH 2 (TeO 4 ) 2 +2H 2 O. More sol. in H 2 O than BaTeO 4 . Decomp. by H 2 O. (Ber- zelius.) BaO, 41eO 3 . More sol. in H 2 O than either BaTeO 4 or BaH 2 (TeO 4 ) 2 . (Berzelius.) Bismuth tellurate, Bi 2 TeO 8 +2H 8 O. Min. Montanite. Sol. in HCl+Aq with evolution of Cl. Cadmium tellurate, CdTeO 4 . Ppt. Sol. in HCl+Aq. (Oppenheim.) Caesium hydrogen tellurate, CsHTeO 4 + M>H 2 0. 1 pt. is sol. in 30 pts. H 2 O. (Norris, Am. Ch. J. 1901, 26. 321.) 1050 TELLURATE, CALCIUM Calcium tellurate, CaTeO 4 . Ppt. Sol. in hot H 2 O. (BerzeliusV) Chromic tellurate, Cr 2 (TeO 4 ) 3 . Ppt. Sol. in excess of Cr salts +Aq. Cobaltous tellurate. Ppt. (Berzelius.) Cupric tellurate, CuTeO 4 . Ppt. (Berzelius.) CuO, 2TeO 3 . Ppt. (B.) Cu 3 TeO 6 . Insol. in H 2 O. Sol. in HC1, HNO 3 ,. NH 4 OH, KCN and acetic acid. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1181.) Glucinum tellurate, GlTeO 4 . Insol. in H 2 O. Iron (ferrous) tellurate, FeTeO 4 . Ppt. Min. Ferrotellurate. Iron (ferric) tellurate, Fe 2 (TeO 4 ) 3 . Ppt. Sol. in ferric salts +Aq. (Berzelius.) Lead tellurate, basic. Not completely insol. in H 2 O. Lead tellurate, PbTeO 4 . Somewhat sol. in H 2 O. PbO, 2TeO 3 . More sol. than PbTeO 4 . PbO, 4TeO 3 . SI. sol. in H 2 O. Sol. in HNO 3 +Aq, less sol. in HC 2 H 3 2 +Aq. (Ber- zelius.) Lithium tellurate, Li 4 TeO 6 +sH 2 O. SI. sol. in H 2 O with decomp. (Mylius, B. 1901, 34. 2209.) Magnesium tellurate, MgTeO 4 . Ppt. More sol. in H 2 O than the Ba, Sr. or Ca salts. MgTe 2 O 7 . More sol in H 2 O than MgTeO 4 . Manganous tellurate. Ppt. Mercurous tellurate, basic, 3Hg 2 O, 2Te0 3 . Ppt. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1178.) Mercurous tellurate, Hg 2 TeO 4 . Ppt. Min. Maqnolite. Mercuric tellurate, HgTe0 4 . Ppt. Very easily decomp. by H 2 O. (Hut- chins, J. Am. Chem. Soc. 1905, 27. 1179.) +2H 2 0. Slowly decomp. by cold H 2 (X Rapidly decomp. by boiling H 2 O. (Hut- chins.) Hg 3 TeO 6 . Insol. in H 2 O. Unchanged by boiling with H 2 O. Sol. in HNO 3 , but more readily sol. in HC1. (Hutchins.) Mercuric tellurate. Ppt. (Berzelius.) Mercurous hydrogen tellurate, HgHTeO 4 +3H 2 O. Stable in the air if protected from the light 'Insol. in H 2 O. Decomp. by boiling H 2 or by an excess of cold cone. HgNO 3 +Aq. Sol. in dil. HNO 3 or dil. acetic acid. (Hut- chins, J. Am. Chem. Soc. 1905, 27. 1177.) Nickel tellurate. Ppt. Potassium tellurate, K 2 Te0 4 +5H 2 O. Deliquesces. Sol. in H 2 O. Very si. sol. in H 2 O containing KOH. 100 g. H 2 dissolve at: 20 30 8 . 82 27 . 53 50 . 42 g. K 2 TeO 4 . (Rosenheim and Weinheber, Z. anorg. 1911, 69. 264.) Insol. in alcohol. (Berzelius.) K 2 O ; 2TeO 3 . Insol. in H 2 O, acids, or alkalies. (B). KHTeO 4 +HH 2 O. SI. sol. in cold, more sol. in hot H 2 O. (Berzelius.) K 2 O, 3TeO 3 +5H 2 O. Much more sol. in hot than in cold H 2 O. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1174.) K 2 O, 4TeO 3 . Insol. in H 2 O, HC1, or HNO 3 -fAq. Sol. by long heating with cone. HNO 3 +Aq. KHTeO 4 , H 2 TeO 4 +KH 2 O.- SI. sol. in H 2 0. Rubidium tellurate, Rb 2 TeO 4 +3H 2 O . Sol. in about 10 pts. H 2 O. (Norris, Am. Ch. J. 1901, 26. 322.) Rubidium hydrogen tellurate, RbHTeO 4 Sol. in about 20 pts. cold H 2 O. SI. more sol. in hot H 2 O. (Norris, Am. Ch. J. 1901, 26. 320.) Silver tellurate, 3Ag 2 O, TeO 8 . Sol. in NH 4 OH+Aq. 3Ag 2 O, 2TeO 3 . Insol. in boiling H 2 O. +3H 2 O. Ppt. Unchanged by cold H 2 O. Gradually decomp. by boiling H 2 O. (Hut- chins, J. Am. Chem. Soc. 1905, 27. 1169.) Ag 2 TeO 4 . Decomp. by H 2 O into 3Ag 2 0, TeO 3 . Sol. in NH 4 OH+Aq. +2H 2 O. Insol. in hot and cold H 2 O. Sol. in NH 4 OH, KCN, Na 2 S 2 O 3 , HNO 3 , H 2 SO 4 and HC 2 H 3 O 2 +Aq. Decomp. by cone. HNO 3 H 2 SO 4 or acetic! acid. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1165.) TELLURIUM CHLORIDE SULPHUR OXIDE 1051 Ag 2 TeO 7 . Ppt. Ag 2 O. 4TeO 3 . Ppt. Could not be obtained. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1168.) Sodium tellurate, Na 2 TeO 4 +2H 2 O. Very si. sol. in hot or cold H 2 O. When heated to drive off 2H 2 O becomes insol. in H 2 Q, but sol. in dil. HNO 3 +Aq. (Berzelius.) 1 pt. is sol. in about 130 pts. H 2 O at 18; 50 pts. H 2 at 100. +4H 2 O. 1 pt. is sol. in about 70 pts. H 2 O at 18; 40 pts. H 2 O at 50. (Mylius, B. 1901, 34. 2209.) Na 2 Te 2 O 7 +4H 2 O = NaHTeO 4 + 1 ^H 2 O . Slowly but completely sol. in H 2 O. SI. sol. in NaC 2 H 3 O 2 +Aq. Insol. in alcohol. (Ber- zelius.) Na 2 O, 4Te0 3 . Insol. in H 2 O, acids, or alkalies, except by long boiling with HNO 3 + Aq. +zH 2 O. (a)' Slowly sol. in H 2 O. (/3) Insol. even in boiling H 2 O. Na 4 TeO 5 +8H 2 O. Very sol. in H 2 O but with decomp. (Mylius.) Strontium tellurates. Resemble Ca salts. Thallous teUurate, Tl 2 TeO 4 . SI. sol. in H 2 O. (Dennis. J. Am. Chem. Soc. 1898, 18. 975.) Thorium tellurate. Ppt. Insol. in excess of thorium salts +Aq. Uranium teUurate, U 2 (Te 4 O) 3 (?) . Ppt. Insol. in H 2 O or UO 2 (NO 3 ) 2 +Aq. Yttrium teUurate. Ppt. Insol. in H 2 O or Yt salts +Aq. Zinc teUurate, Zn 3 TeO 6 . Insol. in H 2 0. Sol. in HNO 3 , HC1, H 2 SO 4 and acetic acid. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1181.) Zirconium tellurate. Ppt. (Berzelius.) Tellurium, Te. Insol. in H 2 O or HCl+Aq. SI. sol. in hot cone. H 2 SO 4 , but separates out on cooling. Sol. in boiling cone. H 2 SO 4 . Easily oxidised by HNO 3 or aqua regia. Sol. in boiling very cone. KOH+Aq, separating out again on cooling. Not attacked by boiling cone. HNO 3 +Aq, according to Hartung-Schwartzkoff (Ann. Min. (4) 19. 345). Sol. in warm cone. KCN+Aq. Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) 100 pts. methylene iodide dissolve 0.1 pt' Te at 12. (Retgers, Z. anorg. 3. 343.) Ya, com. oleic acid dissolves 0.0014 g. Te in 6 days. (Gates, J. phys. Ch. 1911, 15. 143.) A colloidal solution of Te in H 2 O can be obtained. It exists in two modifications, a brown and a blue-gray. Both can be diluted with H 2 O or concentrated by boiling without decomp. They are, however, de- comp. by electrolytes, especially NH 4 G1. (Gutbier, Z. anorg. 1902, 32. 53.) TeUurium cfabromide, TeBr 2 . Decomp. on air or by H 2 O. (Rose, Pogg. Cone, tartaric acid dissolves partly with- out decomp. (Brauner, M. 1891, 12. 34.) TeUurium tetrabromide, TeBr 4 . Sol. in a little, but decomp. by much H 2 O. Completely sol. in tartaric acid+Aq (1:1). (Brauner, M. 1891, 12. 34.) TeUurium hydrogen >romide, TeBr 4 , HBr-f- 5H 2 O. Fumes in the air. Deliquescent. Stable in an atmos. of HBr. (Metzner, C.; R. 1897, 124. 1951.) TeUurium ^'chloride, TeCla., Decomp. on air, or by H 2 O or HCl+Aq. (Ros-e, Pogg. 21.443.) TeUurium fctfrachloride, TeCl<. Extremely deliquescent. Decomp. by cold H 2 O, with separation of oxychloride and tellurous acid. Sol. in hot H 2 O with decomp. Sol. in dil. HC1 +Aq without decomp. (Rose. Pogg. 21. 443.) Insol. in sulphur chloride and in CS 2 . (Lenher, J. Am. Chem. Soc. 1902, 24. 188.) TeUurium hydrogen chloride, TeCl 4 , HC1+ 5H 2 O. Easily decomp. (Metzner. C. R. 1897, 125. 4.) TeUurium chloride with MCI. See Chlorotellurate, M. TeUurium fetfrachloride ammonia, TeCl 4 , 3NH 3 . Decomp. by H 2 O. (Metzner, C. R. 1897, 124. 33.) TeCl 4 , 4NH 3 . Not deliquescent. Decomp. by H 2 0. (Espenschied, J. pr. 80. 480;) TeUurium tefrachloride sulphur ^n'oxide, x TeCl 4 , S0 3 . Ppt. ((Prandtl, Z. anorg. 1909, 62. 247.) TeCl 4 ,2SO 3 . Decomp. by moisture. On heating at 120, it gives TeCl 4 ,SO 3 . (Prandtl.), 1052 TELLURIUM FLUORIDE Tellurium teJrafluoride, TeF 4 . (Metzner, C. R. 1897, 126. 25.) +H 2 O. (Hogbora, Bull. Soc. (2) 35. 60.) Tellurium Aezafluoride, TeF fl . Decamp, by H 2 O slowly but completely. (Prideaux, Chem. Soc. 1906, 39. 322.) Tellurium zirconium fluoride, See Fluozirconate, tellurium. Tellurium diodide, Telj. Insol. in H 2 O. (Rose, Pogg. 21. 443.) Tellurium tefraiodide, TeI 4 . Insol. in cold, decomp. by hot H 2 or alcohol. Sol. in HI, but only sol. in MI + Aq. (Berzelius.) Data on solubility of TeI 4 in HI+I+Aq are given by Menke (Z. anorg. 1912, 77. 283.) Tellurium hydrogen iodide, TeI 4 , HI+ 8H 2 O, and +9H 2 0. Deliquescent. (Metzner, A. ch. 1898, (7) 16. 203.) Tellurium nitride, Two forms. a. Stable at ord. temp. b. Unstable at ord. temp. (Franz Fischer, B. 1910, 43. 1472.) TeN. Not attacked by H 2 O or dil. acetic acid. Insol. in liquid NH 3 . Decomp. by KOH+ Aq. (Metzner, A. ch. 1898, (7) 16. 203.) Tellurium monoxide, TeO. SI. sol. in cold dil. HC1 or H 2 S0 4 +Aq. Easily oxidised by HN0 3 +Aq or aqua regia. Decomp. immediately by boiling cone. HC1+ Aq. Slowly decomp. by KOH+Aq. (Divers and Shimose", Chem. Soc. 36. 563.) Tellurium dioxide, TeO 2 . Very si. sol. in H 2 O. SI. attacked by acids. SI. sol. in NH 4 OH or alkali carbonates -f Aq. Easily sol. in NaOH or KOH+Aq. Not sol. in less than 150,000 pts. H 2 O. Easily sol. in warm dil. HNO 8 +Aq. Sol. in warm H 2 SO 4 +Aq. (Klein and Morel, Bull. Soc. (2) 43. 203.) 20% H 2 SO 4 +Aq. dissolves on warming about 0.7%; 30% H*SO 4 +Aq, about 0.85%: 50% H 2 SO 4 +Aq, about 4.4%. These solutions are supersat. and TeO 2 separates from the more dil. acids on stand- ing. (Brauner, M. 1891, 12. 34.) Min. Tellurite. Tellurium dioxide hydrobromic acid, TeOo 3HBr. (Ditte, C. R. 83. 336.) Tellurium dioxide hydrochloric acid, TeO 2 , 2HC1. (Ditte, C. R. 83. 336.) Te0 2 , 3HC1. (Ditte.) Tellurium tfn'oxide, TeO 3 . Insol. in cold or hot H 2 O, cold HCl+Aq, or cold or hot HNO 3 -fAq. Insol. in moderately cone. KOH+Aq, but, when the KOH+Aq is very cone., is sol. if boiling. Tellurium oxide, 2TeO 2 , TeO 3 . " Tellurium tellurate." (Metzner, A. ch. 1898, (7) 16. 203.) Tellurium oxybromide. Insol. in H 2 O. (Ditte. A. ch. (5) 10. 82.) Tellurium oxybromide sulphur in'oxide, TeOBr 2 , 2SO 3 . Deliquescent. (Prandtl, Z. anorg. 1909, 62. 247.) Tellurium oxychloride, TeOCl 2 . Insol. in H 2 O. (Ditte.) Tellurium oxyfluoride, TeF 4 , TeO 2 +2H 2 O. Sol. in H 2 O containing HNO 3 . Decomp. by H 2 O. 2TeF 4 , 3Te0 2 +6H 2 O. Decomp. by H 2 O. (Metzner, C. R. 1897, 125. 25.) Tellurium sulphide, TeS. Insol. in CS 2 ; very unstable. (Snelling, J. Am. Chem. Soc. 1912, 34. 802.) Tellurium di'sulphide, TeS 2 . Insol. in H 2 O or dil. acids. Sol. in alkali hydrates or sulphides +Aq. CS 2 dissolves out S, so that the substance is probably a mixture. (Becker, A. 180. 257.) Tellurium bisulphide, TeS 3 . Insol. in H 2 O. Sol. in K 2 S+Aq. Tellurium sulphoxide, Te&O 8 . Decomp. by H 2 O. - Sol. in H 2 SO 4 . (Weber, J. pr. (2) 26. 218.) Is tellurium sulphite. (Divers, Chem. Soc. 49. 583.) Tellurous acid, H 2 TeO 8 . Appreciably sol. in H 2 O and acids, in alkali hydrates or carbonates +Aq. Tellurites. The neutral and acid tellurites of the alkali metals are sol. in H 2 O. Ba, Sr. Ca, and Mg tellurites are si. sol., and the other salts yjsol. in H 2 O. Most tellurites are sol. in -tld+Aq. TERBIUM ior>;t Aluminum tellurite. Ppt. Insol. in Al salts +Aq. (Berzelius.) Ammonium tellurite, (NH 4 )HTeO 8 , H 2 TeO 3 + 3/iHjO. Sol. in H 2 O, from which it is precipitated by NH 4 Cl+Aq or alcohol. (Berzelius.) Barium tellurite, BaTe0 8 . SI. sol. in H 2 O when prepared in the moist way. (Berzelius.) BaO, 4TeO 2 . Cadmium tellurite. Ppt. Sol.inHNO 3 ,andHCl+Aq. (Oppen- heim.) Calcium tellurite, CaTeO a . SI. sol. in cold, more sol. in hot H 2 O. (Berzelius.) CaO, 4TeO 2 . Chromium tellurite. Ppt. Sol. in excess of chromic salts -fAq. Cobaltous tellurite. Ppt. Cupric tellurite. Insol. in H 2 O. (Berzelius.) Glucinum tellurite. Insol. in H 2 O. Indium teUurite, In 2 (TeO 3 , 2In(OH),. Ppt. (Renz, Dissert. 1902.) Ferrous tellurite. Ppt. Ferric tellurite. Ppt. Lead tellurite, PbTeO,. Ppt. Easily sol. in acids. (Berzelius.) Lithium tellurite, Li 2 TeO,. Sol. in H 2 O. (Berzelius.) LijO, 2TeOj. Decomp. by cold H,O into LijTeOs and LijO, 4TeO 4 . (B.) LijO, 4TeOj. Sol. in hot, much less in cold H,0. (B.) Magnesium tellurite, MgTeO*. Precipitate. Much more sol. in HjO than the Ba, Sr, or Ca salt. (Berzelius.) Manganous tellurite. Ppt. Mercurous tellurite. . Ppt, Mercuric tellurite. Ppt. Nickel tellurite. Ppt. Potassium tellurite, K 2 TeO,. Not deliquescent. Slowly sol. in cold. more quickly in boiling H 2 O. (Berzelius.) K 2 O, 2TeOz. Completely sol. in boiling H 2 O, from which K 2 O,4TeO 2 crystallises. (B.) K 2 O. 4TeO 2 +4H 2 O. Decomp. by cold HjO 4 nto K 2 O, TeO 2 , and K 2 O, 2TeO 2 , which dissolve, and H 2 TeO 3 , which is insol. (B.) Potassium Aezatellurite, K 2 0, 6TeO 2 +2H 2 O. Notdecomp. by, but si. sol. in JI 2 O. (Klein and Morel, C. R. 100. 1140.) SUver tellurite, Ag 2 TeO,. Ppt. Sol. in NH4OH+Aq. (Berzelius.) The freshly pptd. salt is insol. in HjO; sol. in HNO 3 . H2iSO 4 , acetic and tartaric and; decomp. by HC1. (Lenher, J. Am. Chem. Soc. 1913, 35. 727.) AgHTeOa. Insol. in HjO. Sol. in HNO 8 +Aq. (Rose, Pogg. 18. 60.) Sodium tellurite, NaaTeO,. Slowly sol. in cold, more quickly in hot Precipitated from aqueous solution by alcohol. (Berzelius.) Na 2 O, 2TeO s . Decomp. by H/> as K salt. (B.) , 4TeO 2 +5HjO. As above. (B.) Strontium tellurite, SrTeO. Resembles Ba salt. SrHtlWV Very sL sol. in HO, more easily in HNOa+Aq. Thorium tellurite* Precipitate. Insol. in HjO or Th salto+Aq. Stannous tellurite. Pptd. in presence of 60,000 pte. HjO. (Fischer.) Uranium teHwite, U,(TeO,)^ Ppt. InsoL in U salte+Aq. Yttrium teUurite. Precipitate. lurite. Ppt. Ppt. Terbium, *H>. Metal baa not been isolated. Has been decomp. into two or more ele- ments by Krttas (Z. anorg. 4. 27). 1054 TERBIUM CHLORIDE Terbium chloride, TbCl 3 -f-6H 2 O. Sol. in H 2 O; very hydroscopic; sol. in al- cohol. (Urbain, C. R. 1908, 146. 128.) Terbium hydroxide. Sol. in dilute acids. Decomposes NH4 salts +Aq. Terbium oxide, T 2 O 3 . Sol. in dil. acids, even after ignition. Terbium peroxide, Tb 4 7 . Sol. in HNO 3 and in hot HC1. (Urbain, C. R. 1907, 146. 127.) Tetramine chromium compounds. See Bromotetramine chromium compounds. Chlorotetramine chromium compounds. lodotetramine chromium compounds. Tetramine cobaltic compounds, See Bromotetramine cobaltic compounds. Carbonatotetramine cobaltic compounds. Chlorotetramine cobaltic compounds. Croceocobaltic compounds. Fuscocobaltic compounds. Flavocobaltic compounds. lodotetramine cobaltic compounds. Nitratotetramine cobaltic compounds. Praseocobaltic compounds. Roseotetramine cobaltic compounds. ~" ; Sulphatotetramine cobaltic compounds. See also under octamine cobaltic saltslfor many tetramine salts as yet unclassified. "" Tetramine cobaltic nitrite with MNO 2 , Co,(NH,) 4 (NO,)., 2MN0 2 . See Diamine cobaltic nitrite. Tetrathionic acid, H 2 S 4 O 6 . Known only in aqueous solution. Dil. solution can be boiled without decomp. Cone, solution decomp. by boiling. Addition of H 2 SO 4 or HC1 makes solution more stable. (Fordos and Gelis, C. R. 15. 920.) Tetrathionates. Tetrathionates are all easily sol. in H 2 O, but insol. in alcohol Barium tetrathionate, BaS 4 O 6 -f2H 2 O. Very sol. in H 2 O, but precipitated by addi- tion of alcohol Cadmium tetrathionate. Deliquescent. Solution in H 2 O gradually decomposes. (Kessler, Pogg. 74. 249.) Caesium tetrathionate, Cs 2 S 4 O 6 . (J. Meyer, B. 1907, 40. 1361.) Cuprous tetrathionate, Cu 2 S 4 O 6 . Decomp. by H 2 O. (Chancel and Diacon, C.R. 1863, 56. 711.) Cupric tetrathionate, CuS 4 Oe. Sol. in H 2 O. Decomp. by long boiling. (Curtius and Henkel, J. pr. 1888, (2) 37. 148.) Lead tetrathionate, PbS 4 O 6 +2H 2 O. Sol. in H 2 O. Manganous hydrogen tetrathionate, MnH 2 (S 4 6 ) 2 . Deliquescent. Very sol. in H 2 O and al- cohol. (Curtius and Henkel, J. pr. (2) 37. 148.) Nickel tetrathionate ammonia, NiS 4 O 6 , 6NH 3 . Ppt. Decomp. by H 2 O. Insol. in alcohol. (Ephraim, B. 1913, 46. 3109.) Potassium tetrathionate, K 2 S 4 O 6 . Soluble in H 2 O. Insol. in alcohol. Difficultly sol. in H 2 O. (Kessler, Pogg. 1847, 74. 254.) Rubidium tetrathionate, Rb 2 S 4 O 6 . Not hydroscopic. (J. Meyer, B. 1907, 40. 1356.) Sodium tetrathionate, Na 2 S 4 O 6 . Sol. in H 2 O. Precipitated therefrom by a great excess of alcohol. (Kessler, J. pr. 96. 13.) +2H 2 O. (Berthelot, A. ch. (6) 17. 450.) Strontium tetrathionate, SrS 4 6 +6H 2 O. Sol. in H 2 O. (Kessler, Pogg. 74. 255.) More sol. in H 2 O than Ba salt. Zinc tetrathionate. Sol.inH 2 O. (Fordos and Gelis.) Zinc hydrogen tetrathionate, ZnH 2 (S 4 O 6 ) 2 . Extremely sol. in H 2 O and alcohol. (Cur- tius and Henkel, J. pr. (2) 37. 147.) Zinc tetrathionate ammonia, ZnS 4 O 6 , 3NH 3 . Ppt. (Ephraim, B. 1915, 48. 641.) Thallic acid. Potassium thallate. Known only in aqueous solution. (Car- stanjen, J. pr. 101. 55.) Does not exist. (Lepsius, Chem. Ztg. 1890, 1327.) THALLOUS CHLORIDE 1055 Thallium, Tl. Not attacked by pure H 2 O. Easily sol. in dil. H 2 SO 4 or HNO 3 +Aq. Difficultly sol. in HCl+Aq. Absolute alcohol dissolves considerable quantity in a short time, also methyl alcohol, and acetic ether. (Bottger.) Not easily attacked by HF+Aq. (Kiihl- mann.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) l /z ccm. oleic acid dissolves 0.0424 g. Tl in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Thallium arsenide, TIAs. Decomp. by H 2 SO 4 . (Carstanjen.) Thallous azoimide, T1N 3 . SI. sol. in H 2 O. 0.1712 pt. is sol. in 100 pts. H 2 O at 0; 0.1965 pt. is sol. in 100 pts. H 2 O at 5; 0.3 pt. is sol. in 100 pts. H 2 O at 16. Insol. in abs. alcohol and ether. (Curtius, J. pr. 1898, (2) 58. 284.) Thallothallic azoimide, T1N 3 , T1N 9 . Explosive. Decomp. bv hot H 2 O and by acids. (Dennis, J. Am. Chem. Soc. 1896, 18. 973.) Thallous bromide, TIBr. Nearly insol. in cold, si. sol. in boiling H 2 O. (Willm, Bull. Soc. (2) 2. 89.) 1 1. H 2 O dissolves 0.00869 g. mol. TIBr at 68.5. (Noyes, Z. phys. Ch. 6. 248.) SI sol. in H 2 O. 0.48 X 10~ 2 g. is dissolved in a liter of sat. solution at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) 1 1. H 2 O dissolves 420 mg. TIBr at 18. (Kohlrausch, Z. phys. Ch. 1904, 50. 356.) 238 mg. TIBr are contained in 1 1. sat. solution at 0.13; 289 mg. at 9.37; 423 mg. at 18; 579 mg. at 25.68. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Solubility of TIBr in T1(NO 3 ) +Aq at 68.5. g. mola. per 1. g. mols. per 1. TINOs TIBr TiNOs TIBr 0.0163 0.0294 0.0955 0.00869 0.00410 0.00289 0.00148 4.336 7.820 25.400 2.469 1.164 0.821 0.420 (Noyes, Z. phys. Ch. 1890, 6. 248.) Insol. in acetone (Naumann, B. 1904, 37. 4329) ; pyridine (Naumann, B. 1904, 37. 4610) ; acetone (Eidmann, C. C. 1899, II. 1014). Thallic bromide, TlBr 3 . Deliquescent. Easily sol. in H 2 O and alcohol. (Willm.) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +H 2 O. Very unstable. Sol. in H 2 O, alcohol and ether. (Meyer, Z. anorg. 1900, 24. 353.) +4H 2 O. Very sol. in H 2 O. (Thomas, C. R. 1902, 134. 546.) Thallothallic bromide, TIBr, TlBr 3 . Decomp. by H 2 O. (Mever, Z. anorg. 1900, 24. 354.) STIBr, TlBr 3 . Decomp. by H 2 O into TIBr and TlBr 3 . Thallic hydrogen bromide, TlBr 3 , HBr. Very sol. in H 2 O. (Thomas, C. R. 1902, 134. 546.) Thallic bromide ammonia, TlBr s , 3NH 3 . Decomp. by H 2 O. Thallium bromochloride, TIClBr. Decomp. by H 2 O. (Thomas, C. R. 1901, 132. 1489.) " . TlClBr 2 +4H 2 O. Ppt. TlCl 2 Br+4H 2 O. Ppt. Decomp. by H 2 O. (Thomas, C. R. 1902, 134. 546.) Tl 3 Cl 2 Br 4 . Decomp. by H 2 O, H 2 SO 4 or HNO 3 . (Thomas, C. R. 1900, 131. 894; C. R. 1901, 132. 1489.) Tl 4 Cl 3 Br 3 . Sol. in H 2 O. (Thomas, C. R. 1901, 132. 82.) TlClBr 2 , 3T1C1. Cryst. from H 2 O con- taining HNO 3 . (Cushmann, Am. Ch. J. 1900, 24. 222.) T1C1 3 , 3TlBr. Sol. in H 2 O without decomp. (Cushmann.) "TlBrs', 3T1C1. Decomp. by H 2 O. (Cush- mann.) TlBr 3 , TlCl. Sol. in H 2 O with decomp. (Cushmann.) TlCls, 2TlBr, 11C1. Sol. in H 2 O. (Meyer, Z. anorg. 1900, 24.. 355-360.) TlBrs, 2T1C1, TIBr. Ppt. Decomp. by 2(TlBr 3 , TIBr). Ppt. (Meyer.) 2(T1C1 3 , TlCl), (TlBrs, TIBr). Ppt. De- comp, by hot H 2 O. (Meyer.) Thallium bromofluoride, TlFBr 2 . Decomp. in moist air. Sol. in abs. alcohol. (Gewecke, A. 1909, 366. 233.) Thallium bromofluoride ammonia, TlFBf 2 ,4NH 3 . Decomp. by moisture. Difficultly sol. in abs. alcohol. (Gewecke, AM909, 366. 234.) Thallous chloride, TlCl. Solubility in pts. H 2 O at t, according to H=Hebberling; C = Crookes; L = Lamy. 15 16 16.5 504 283.4 377 359 pts. H 2 O, H C H H 100 P about 50 L 100 52 . 5 C 100 63 pts. H 2 O. H 1056 THALLOUS CHLORIDE 1 1. H 2 O dissolves 0.0161 g. mol. T1C1 at 25. (Noyes, Z. phys. Ch. 6. 249.) 3.26 X 10 2 grams are dissolved in 1 liter of sat. solution at 20. (Bottger, Z. phvs. Ch. 1903, 46. 603.) 1 1. H 2 O at 25 dissolves 0.01606 g. mol. T1C1. (Geffcken, Z. phys. Ch. 1904, 49. 296.) Solubility in H 2 O at t. 100 cc. sat. solution contain at: t 10 20 30 40 50 g. T1C1 0.17 0.24 0.34 0.46 0.60 0.80 t 60 70 80 90 99.3 g. T1C1 1.02 1.29 1.60 1.97 2.41 (Berkeley, Trans. Roy. Soc. 1904, 203, A, 208.) 1 1. H 2 O dissolves 3.040 T1C1 at 18. (Kohlrausch, Z. phys. Ch. .1904, 50. 356.) 2.27 g. are dissolved in 1 1. of sat. solution at 9.54; 3.05 g. at 17.7; 3.97 g. at 25.76. (Kohlrausch, Z. phys. Ch. 1908/64. 168.) 0.01629 mol. is sol. in 1 1. H 2 at 25. (Hill, J. Am. Chem. Soc. 1910, 32. 1385.) 0.01607 g. equiv. is sol. in 1 1. H 2 O at 25. (Bray and Winninghoff, J. Am. Chem. Soc. 1911, 33. 1665.) Much less sol. in H 2 O containing HC1 or HN0 3 . Solubility in HCl+Aq at 25. 1 1. dissolves g. mol. T1C1. g. HCl added T1C1 g. HCl added T1C1 0.0283 0.0560 0.01610 0.00836 0.00565 0.1468 1.000 0.00316 0.00200 (Noyes, Z. phys. Ch. 6. 249.) Solubility in HCl+Aq. at 25. Concentration of HCl, equivalents per liter 0.025 0.05 0.10 0.20 Solubility of T1C1, equivalents per liter 0.01612 0.00869 0.00585 0.00384 0.00254 (Noyes, Z. phys. Ch. 1892, 9. 614.) Solubility in HNO 3 +Aq at 25. Normality HNOs 0.000 0.4977 1.0046 2.0452 4.017 Sp. gr. of the solution 0.996 1.0184 1.0359 1.0705 1 . 1362 g. T1C1 dis- solved per 1. 3.952 5.937 6.883 8.143 9.926 (Hill and Simmons, Z. phys. Ch. 1909, 67. 605.) Concentration of KNOs milliequivalents per 1. Solubility of TIC1. milliequivalents per 1. 10 20 50 100 300 1000 16.07 17.16 18.26 19.61 23.13 30.72 Nearly insol. in NH 4 OH+Aq. More sol. in K 2 CO 3 +Aq than in H 2 O. 3.86 g. T1C1 are sol. in 1 1. H 2 O at 25. 21.84 g. T1C1 are sol. in 1 1. 5N-K 2 CO 3 +Aq at 25. (Spencer and Le Pla, C. C. 1908, II. 198.) Solubility in KNO 3 +Aq at 25. (Bray and Winninghoff, J. Am. Chem. Soc. 1911, 33. 1670.) Solubility in K 2 SO 4 +Aq at 25. Concentration of K 2 SO-i milliequivalents per 1. 10 20 50 100 300 1000 Solubility of T1C1 milliequivalents per 1. 16.07 17.79 19.42 21.37 26.00 34.16 (Bray and Winninghoff, J. Am. Chem. Soc, 1911, 33. 1670.) Solubility in Tl 2 SO 4 +Aq at 25. Concentration of TlnSCi milliequivalents per 1. Solubility of T1C1 milliequivalents per I. 10 20 50 1 100 16.07 10.34 6.77 4.68 (Bray and Winninghoff, J. Am. Chem. Soc. 1911, 33. 1670.) Solubility of T1C1 in salts +Aq at 25. Salt Concentration of salt g. equiv. per 1. T1C1 dissolved g. equiv. per 1. NH 4 C1 - 0.025 0.05 0.2 0.00872 0.00593 0.00271 CaCl 2 0.025 0.05 0.10 0.20 0.00899 0.00624 0.00417 0.00284 THALLIUM TUNGSTEN CHLORIDE 1057 Solubility of T1C1 in salts +Aq Continued. at 25. Solubility of T1C1 in HC 2 H 3 O 2 +Aq at 25, (g. equiv. per 1.) Salt Concentration of salt g. equiv. per 1 T1C1 dissolved g. equiv. per 1. Acid T1C1 0.000 0.01629 0.5134 0.01580 1.013 0.01495 2.016 0.0132 4.180 0.0099 8.130 0.0054 11.49 0.0026 14.31 0.0012 16.01 0.0005 CdCl 2 0.025 0.05 0.10 0.20 OOOO 01040 0078 00578 00425 CuCl 2 0.025 0.05 0.10 0.20 oooo 00905 00614 00422 00291 (Hill, J. Am. Chem. Soc. 1910, 32. 1189.) Insol. in pyridine. (Naumann, B. 1904, 37. 4610); acetone. (Naumann, B. 1904, 37. 4329.) Thallic chloride, T1C1 3 . Anhydrous. Easily sol. in H 2 O and in most ord. sol- vents. In contact with moist air, it rapidly be- comes hvdrated. (Thomas, C. R. 1902 136. 1053.) Difficultly sol. in methyl acetate. (Nau- mann, B. 1909, 42. 3790.) Very sol. in acetone. (Renz, B. 1902, 35. 1110.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) +H 2 O. Deliquescent, and very easily sol. inH 2 O. (Werther.) Deliquescent, and very easilv sol. in H 2 O. (Werther.) -f 4H 2 O. 86.2 pts. are sol. in 100 pts. H 2 O at 17. Sp. gr. of sat. aq. solution at 17 = 1.85. (Thomas, C. R. 1902, 136. 1052.) Very hydroscopic. (Meyer, Z. anorg. 1900, 24. 336.) Very sol. in alcohol and ether. (Meyer, Z. anorg. 1900, 24. 338.) +7^H 2 O. Deliquescent. (Werther.) MgCl 2 0.025 0.05 0.10 0.20 oooo 00904 00618 00413 00275 MnCl 2 0.025 0.05 0.10 0.20 oooo 00898 00617 00412 00286 KC1 0.025 0.05 0.1 . 0.2 oooo 00872 00593 00399 00265 NaCl 0.025 0.05 0.10 0.20 0. 0. 0. 0. 00869 00592 00395 00271 ZnCl 2 0.025 v - 0.05 0.10 0.20 oooo 00899 00627 00412 00281 T1C1O 3 0.025 0. 00897 T1NO 3 0.025 0.05 0.10 pop 00883 00626 00423 (Noyes, Z. phys. Ch. 1892, 9. 609.) Solubility of T1C1 in salts -f Aq at 25. Salt Mols T1C1 sol. in 1 liter of O.5-N solution N solution 2-N solution 3-N solution 4-N solution NH 4 NO 3 KNOs NaNOs LiNOs KClOa NaClOs 0.02587 0.02566 . 02564 0.02542 . 02370 02320 0.03121 0.03077 . 03054 0.03035 . 02687 0.03966 0.03904 0.03851 0.03785 . 03060 . 04544 0.04438 0.03303 0.05128 . 03850 (Geffcken, Z phys. Ch. 1904, 49. 295.) Insol. in alcohol. Easily sol. in hot HgCl 2 +Aq. (Carstanjen.) Thallothallic chloride, 3T1C1, T1C1 8 . 1 pi. dissolves in pts. H 2 O at t, according to C=Crookes; H = Hebberling; L = Lamy. 15 17 100 100 380.1 346 52.9 20-25 pts. H 2 O. C H C L SI. decomp. by dissolving. (Lamy.) Thallic hydrogen chloride, T1C1 8 , HC1+ 3H 2 0. Very hygroscopic. Decomp. by H 2 O. (Meyer, Z. anorg. 1900, 24. 337.) Thallium tungsten chloride, T1 S W 2 C1 9 . Nearly insol. in H 2 O. Sol. in a hot mixture of equal pts. H 2 O and cone. HC1. 1058 THALLIC ZINC CHLORIDE SI. sol. in cone. HC1. Solubility of T1OH in H 2 O at t. Nearly insol. in most organic solvents. (Olsson, B. 1913, 46. 575.) t g. equiv. 1 1OH per 1 Sp. gr. 15/4 1 1 C1 1 9Q1 ThaUic zinc chloride, 2T1C1 3 , ZnCl 2 +6H 2 O. 18.5 i . i ') i 1.554 J- . _ ) 1 1.317 Can be cryst. from H 2 O. (Gewecke, A. 19.5 1.582 1.322 1909, 366. 224.) 29 1.803 1.342 23.1 1.861 . 1.377 Thallic chloride ammonia, T1C1 8 , 3NH,. 33.1 36 1.967 2.075 1.400 1.417 Decomp. by H 2 O. Sol. in HCl+Aq (Willm.) 40 2.240 1.446 44.5 2.442 . Thallium chlorofluoride, T1FC1 2 . 54.1 59.4 2.940 3.281 Very hydroscopic. 64.6 3.601 Decomp. by moist air. 78.5 4.673 Easily sol. in abs. alcohol. (Gewecke, A. 90.0 5.705 1909, 366. 230.) 99.2 6.708 +3H 2 O. Not hydroscopic. Decomp. by H 2 O, alcohol and ether. (Bahr, Z. anorg. 1911. 71. 87.) (Gewecke.) Thallium chlorofluoride ammonia, T1FC1 2 , 4NH 3 . Decomp. by H 2 O. Difficultly sol. in abs. alcohol and in ether. (Gewecke, A. 1909, 366. 232.) Thallium chlorofluoride potassium chloride, 2T1FCU, KC1. Ppt. (Gewecke, A. 1909, 366. 231.) Thallous fluoride, T1F. Sol. in 1% pis. H 2 O at 15, and in much less hot H 2 O. Difficultly sol. in alcohol. (Buchner, W. A. B. 62. 2. 644.) Deliquescent. (Willm.) ThaUic fluoride, T1F 8 . Insol. in H 2 O and cold HCl+Aq. (Willm.) Cannot be obtained in pure state. (Ge- wecke, A. 1909, 366. 218.) Thallous hydrogen fluoride, T1F, HF. Sol. in 1 pt. H 2 O. (Buchner.) Thallous tungstyl fluoride, See Fluoxytungstate, thallous. Thallous vanadium fluoride. See Fluovanadate, thallous. Thallous vanadyl fluoride. See Fluozyvanadate, thallous. Thallous hydroxide, T1OH. Sol. in H 2 O and alcohol. The solubility of T1 2 O in H 2 O at these temperatures is the same as that of T1OH. +H 2 O. (Willm, Bull. Soc. (2) 6. 354.) ThaUic hydroxide, T1 2 O 3 , H 2 O=T1O(OH). Insol. in H 2 O. Sol. in dil. acids and am- monium salts +Aq. Insol. in caustic alkali solutions. T1(OH),. Easily sol. in dil. HC1 or H 2 SO 4 +Aq. (Carnegie, C. N. 60. 113.) Thallous iodide, Til. Very si. sol. in H 2 O. 1 pt. Til is sol. in pts. H 2 O at t. C = ac- cording to Crookes; H = according to Hebber- ling; L = according to Lamy; W = according to Werther. 35 15, 16 16-17 19.4 20,0004450 16,000 11,676 14,654 pts. H 2 0, W C L H W 20 23.4 45 100 100 11,954 10,482 5407 842 804 pts. H 2 O. W W W C -H Sol. in 17,000 pts. H 2 O at 20. (Long, Z. anal. 30. 342.) Sat. solution at 20.15 contains 63.6 mg. or 1.92X10 4 g. mol. Til per 1. (Bottger, Z. phys. Ch. 1903, 46. 603.) 1 1. H 2 O dissolves "56 mg. Til at 18. (Kohlrausch, 2. phys. Ch. 1904, 60. 356.) 36.2 mg. are dissolved in 1 1. of sat. solution at 9.90; 56 mg. at 18.1; 84.7 mg. at 26. (Kohlrausch, Z. phys. Ch. 1908, 64. 168.) Solubility in H 2 O at 25 = 1.76X10 4 mol. per litre. (Spencer, Z. phys. Ch. 1912, 80. Not decomp. by dil. H 2 SO 4 , HC1. or alkalies +Aq. Decomp. by hot dil. HNO 3 +Aq, and cold cone. HNO 3 . Sol. in aqua regia. Also less sol. in acetic acid than in H 2 0. (Carstanjen.) THALLIUM TELLURIDE 1059 Insol. in NH 4 OH+Aq. (Werther.) Not wholly insol. in NH 4 OH+Aq. and solubility is increased by presence of (NH 4 ) 2 SO 4 or NH 4 C1. (Baubigny, C. R. 113. 544.) Sol. in 13,000 pts. NH 4 OH+Aq (6^ or NH 3 ). Sol. in 17,000 pts. NH 4 OH+Aq 1NH 3 ). (Long.) Insol. in dil. KI+Aq (1% KI). (Bau- bigny.) Much more insol. in KI+Aq than in H 2 0; 1 pt. dissolves in 75,000 pts. dil. KI+Aq. (Lamy.) Nearly insol. in Na 2 S 2 O 3 +Aq, and abso- lutely insol. therein in presence of Pb salts. (Werner. C. N. 63. 51.) Sol. in 56,335 pts. 85% alcohol at 13. (Werther.) Sol. in 18,934 pts. 98% alcohol at 19. (Hebberling.) When Til is shaken with alcohol of 78B (1 vol. H 2 O+3 vols. 98% alcohol) at 22, and let stand with Til for 24 hours, and then evaporated to Vs vol., there is shown no ppt. by NH 4 SH+Aq. (Baubigny.) Sol. in 260,000 pts. 90% alcohol, and 37,003 pts. 50% alcohol at 20. (Long.) Insol. in methylene iodide. (Retgers, Z. anorg. 3. 343.) Insol. in acetone. (Naumann, B, 1904, 37. 4329; Eidmann, C. C., 1899, II. 1014.) Insol. in pyridine. (Naumann, B. 1904, 37. 4601.) Thallic iodide, TlI 3i Sol. in alcohol. Decomp. slowly in the air. (Wells, Z. anorg. 1894, 6. 313.) Sol. in ether. Thallothallic iodide, T1 3 I 4 = 5T1I, T1I 3 . Sol. in H 2 O. (Jorgensen, J. pr. (2) 6* 82.) Thallium nitride. Very unstable. (Franz Fischer, B. 1901, 43. 1470.) Thallous oxide, T1 2 O. Deliquescent. Sol. in H 2 O. See Thallous hydroxide. Thallic oxide, T1 2 O 8 . Insol. in H 2 O. Not attacked by cold H 2 SO 4 . Sol. in hot H 2 SO 4 . Sol. in cold HC1 +Aq. Insol. in alkalies +Aq. (Werther, J. pr 91. 385.) Black modification. Less sol. in dil. acids than the brown modification. Solution is accompanied by a slight reduction to thallous salt. More sol. in 10% HC1 than in 10% H 2 SO 4 or HNO 3 . More sol. in cone, than in dil. acids. (Rabe Z. anorg. 1906, 48. 431.) Brown modification. Easily sol. in dil. mineral acids on warm- ng, with slight reduction to thallous salt. More sol. in cone. acid. (Rabe.) Thallium dioxide, T1O 2 . Insol. in H 2 O. (Piccini, Gazz. ch. it. 17. 450.) Thallic oxide ammonia, T1 2 O 3 , 6NH 3 . Decomp. by much H 2 O. Insol. in alcohol. (Carstanjen.) Thallic oxyfluoride, T1OF. Insol. in H 2 O. Slowly decomp. by boiling with H 2 O. Sol. in mineral acids. Almost insol. in HF. (Gewecke, A. 1909, 366. 226.) Thallium phosphide (?). Ppt. (Crookes.) Thallous selenide, Tl 2 Se. Insol. in H 2 O. Scarcely attacked by cold dil. H 2 SO 4 +Aq, but dissolves when heated. (Carstanjen.) Thallothallic selenide. Not attacked by cold cone, or boiling dil. H 2 SO 4 +Aq. Cone. H 2 SO 4 decomposes. (Car- stanjen.) Thallous sulphide, T1 2 S. Insol. in H 2 O, (NH 4 ) 2 S+Aq, NH 4 OH+Aq KCN+Aq, and in alkali carbonates, and hydrates +Aq. Difficultly sol. in a solution of oxalic acid or acetic acid. (Crookes.) Easily sol. in HNO 3 , and H 2 SO 4 +Aq. Diffi- cultly sol. in HCl+Aq. (Willm.) SI. sol. in H 2 O. 0.21 X10- 4 g. is dissolved in 1 1. sat. solu- tion at 20. (Bottger, Z. phys. Ch. 1903, 46. 603.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Thallic sulphide, T1 2 S 3 . Insol. in H 2 O. Insol. in cold, sol. in warm dil. H 2 SO 4 +Aq without separation of S. Sol. in other dilute acids with separation of S. (Carstanjen.) Thallium pentasulphide, T1 2 S 6 . Ppt. (Hofmann, B. 1903, 36. 3092.) Thallothallic sulphide, 5T1 2 S, 3T1 2 S 3 . Very slowly decomp. by cold dil. [2804+ T1 2 S 3 . (Carstanjen.) T1 2 S, 2T1 2 S 3 . Decomp. by dil. acids. (Schneider, J. pr. (2) 10. 55.) Thallium teUuride, Tl 2 Te. (Fabre, C. R. 105. 673.) 1060 THIOANTIMONIC ACID Thio- For compounds with prefix thio-, see also under sulpho-. Thioantimonic acid. See Sulphantimonic acid. Thioarsenic acid. See Sulpharsenic acid. Thiomolybdic acid. See Sulphomolybdic acid. Thionamic acid, NH 3 S0 2 = NH 2 SO(OH). Very deliquescent, and sol. in H 2 O. H 2 O solution decomp. gradually. (Rose, Pogg. 33. 275; 42. 425.) Ammonium thionamate, NH 2 SO(ONH 4 ). Deliquescent. Sol. in H 2 O; easily decomp. when in solution. (Rose.) Very sol. in alcohol with decomp. SI. sol. in dry ether. (Divers and Ogawa, C. C. 1900, I. 1259.) Dtthionic acid. See Dithionic acid. TVtthionic acid. See Trithionic acid. Tetraihiomc acid. See Tetrathionic acid. Penlathiomc acid. . See Pentathionic acid. Thionyl bromide, SOBr 2 . Unstable. . Decomp. by H 2 O. (Besson, C. R. 1896, 122. 322.) Thionyl bromochloride, SOClBr. Decomp. slowly in the cold, rapidly at 115. Deccmp. by H 2 O. (Besson C. R. 1896, 122. 321.) Thionyl chloride, SOC1 2 . Sol. in CHC1 3 , and CeHe. (Oddo, Gazz. ch it. 1899, 29. (2) 318.) Thionyl fluoride, SOF 2 . Decomp. by H 2 O. Sol. in AsCl 3 , CeH, ether and oil of turpen- tine, (Moissan, C. R. 1900, 130. 1439.) Thiophosphamic acid, H 2 PNH 2 O 2 S (?). Known only in its salts. (Gladstone and Holmes, Chem. Soc. (2) 3. 1.) Cadmium thiophosphamate, CdPNH 2 2 S. Sol. in dil. acids.* and NH 4 OH+Aq. (G. and H.) Lead , PbPNH 2 2 S. Ppt. Sol. in dil. HNO 3 +Aq. (Gladstone and Holmes, Chem. Soc. (2) 3. 1.) Thiophosphocfa'amic acid, H 2 PN 2 H 4 OS. Known only in solution, which soon de- composes. (G. and H.) Cadmium thiophosphocfo'amate, Cd(PN 2 H 4 OS) 2 . Insol. in H 2 O; sol. in dil. acids, and NH 4 OH H-Aq. (G. and H.) Cupric , Cu(PN2-H 4 OS) 2 . Insol. in H 2 O, dil. HC1, or NH 4 OH+Aq. Sol. in KCN+Aq. (Gladstone and Holmes. Chem. Soc. (2) 3. 1.) Lead , Pb(PN 2 H 4 OS) 2 . Insol. in H 2 O. Sol. in dil. HNO 3 +Aq. Nickel , Ni(PN 2 H 4 OS) 2 . Sol. in dil. acids, and NH 4 OH+Aq. (Glad- stone and Holmes, Chem. Soc. (2) 3. 1.) Zinc , Zn(PN 2 H 4 OS) 2 . Ppt. Sol. in dil. acids, and NH 4 OH+Aq. (Gladstone and Holmes.) Thiophosphonitrile, PSN. Not decomp. by cold H 2 O. Slowly decomp. by boiling H 2 O. Easily decomp. by boiling dil. HC1. (Stock, B. 1906, 39. 1974.) Thiophosphoric acid," H 3 PSO 3 =PS(OH) 3 . Known only in its salts. Ammonium magnesium thiophosphate, NH 4 MgPS0 3 +9H 2 0. SI. sol. in cold H 2 O. (Kubierschky, J. pr. (2) 31. 100.) Barium , Ba 3 (PSO 3 ) 2 . Insol. in H 2 O. (Wurtz, A. ch. (3) 20. 473.) Cobalt . Insol. in H 2 O, but partially decomp. when boiled therewith. (Wurtz.) Cupric . Insol. in H 2 O ; very easily decomp. (Wurtz.) Ferric . Insol. in H 2 O. (Wurtz.) Magnesium , Mg 3 (PSO 3 ) 2 +20H 2 O. SI. sol. in cold H 2 O. (Kubierschky, J. pr. THIOPHOSPHORYL CHLORIDE 1061 Nickel thiophosphate. Insol. in H 2 O, but decomp. when boiled therewith. (Wurtz.) Potassium , K 3 PSO 8 . Very sol. in H 2 O. Known only in aqueous solution. (Wurtz.) Sodium , Na 3 PSO 3 +12H 2 O. Easily sol. in boiling H 2 O. Cryst. out on cooling. (Wurtz, A. ch. (3) 20. 472.) Insol. in alcohol. Strontium . Insol. in H 2 O. (Wurtz.) Dithiometaphosphoric acid. Ammonium cfo'thioraetaphosphate, NH 4 PS 2 O. Decomp. by H 2 O. (Stock, B. 1906, 39. 1990.) Monothioorthophosphoiic acid. woriothioor^ophosphate, O:P(SNH 4 )(OH) 2 . Sol. in H 2 O. Insol. in alcohol. (Stock, B. 1906, 39. 1990. Tnammonium monothioortAophosphate, SNH 4 .PO.(ONH 4 ) 2 . (Stock.) IH'thioortAophosphoric acid. Ammonium ^'thiophosphate, (NH 4 ) 3 PS 2 O 2 -{- 2H 2 0. 81. efflorescent. Sol. hi H 2 O. (Kubier- schky, J. pr. (2) 31. 93.) Ammonium magnesium , NH 4 MgPS 2 2 +6H 2 0. 81. sol. in cold, H 2 O. (Kubierschky.) Barium , Ba 3 (PS 2 O 2 ) 2 +8H 2 O. Precipitate. (Kubierschky, J. pr. (2) 31. 103.) + 18H 2 O. As the Zn'thio compound. (Ephraim, B. 1910, 43. 287.) Calcium . Very easily decomposed. (Kubierschky.) Sodium , Na 3 PS 2 O 2 +llH 2 O. Very sol. in H 2 O. (Kubierschky, J. pr. (2) 31. 93.) Tn'thioortAophosphoric acid. Ammonium /n'thioor^Aophosphate, (NH 4 ) 3 PS 3 0+H 2 0. (Stock, B. 1906, 39. 1985.) Barium /nthioor^ophosphate, Ba 3 (PS 8 O) 2 + 20H 2 0. Decomp. by H 2 O and dil. acids. Sol. in cone. HNO 3 with oxidation of the sulphur to H 2 SO 4 . (Ephraim, B. 1910, 43 e sulp . 286. Magnesium , Mg 8 (PS 3 0) 2 +20H 2 0. Decomp. by H 2 O and dil. acids. (Ephraim. Thiophosphorous acid. Ammonium thiophosphite (?), (NH 4 ) 4 P 2 S 2 0| +3H 2 0. Sol. in H 2 O. (Lemoine, C. R. 98. 45.) +6H 2 0. Sodium thiophosphite (?), Na 4 P 2 S 2 O 3 +5H 2 O = P 2 O 3 , 2Na 2 S+5H 2 O. Sol. in H 2 O. (Lemoine. C. R, 98. 45.) Na 6 P 2 S 2 O 4 +4H 2 O = P 2 3 , 3Na 2 O, 2H 2 S+ 2H 2 O. Sol.inH 2 O. (Lemoine, I.e.) Thiophosphoryl tfn'amide, PS(NH 2 ) 3 . Rapidly decomp. by H 2 O. Scarcely sol. in alcohol, ether, or CS 2 . (Chevrier, C. R. 66. 748.) Metathiophosphoryl bromide, PS 2 Br. Decomp. by H 2 O. Insol. in ether. (Mich- aelis, A. 164. 9.) On'Aothiophosphoryl bromide, PSBr 8 . Slowly decomp. by cold, rapidly by hot H 2 O but volatile with only partial decomp. with steam. Easily sol. in ether, CS 2 , PC1 8 , PBr a . Decomp. by cold alcohol. Forms hydrate PSBr 3 +H 2 O. (Michaelis, A. 164. 9.) Pi/rothiophosphoryl bromide, P 2 S 8 Br 4 . Decomp. by H 2 O and alcohol. Sol. hi CSf and ether. (Michaelis.) Thiophosphoryl phosphorus bromide, PSBr 3 , PBr 3 . Decomp. by H 2 O into PSBr 3 . (Michaelis.) Thiophosphoryl cfabromochloride, PSClBr 2 . Decomp. by H 2 O and alkalies. Fumes in the air. (Besson, C. R. 1896, 122. 1059.) Thiophosphoryl bromoofo'chloride, PSCl 2 Br. Decomp. by H 2 O and alkalies. Reacts violently with HNO 8 . (Besson, C. R. 1896, 120. 1058.) Thiophosphoryl chloride, PSC1 8 . Very slowly decomp. by H 2 O, and may be distilled with steam without much decomp. Decomp. by alcohol. Miscible with CS 2 . (Baudrimont, J. pr. 87. 301.) Sol. in CC1 4 and C 6 H 6 . (Oddo, Gazz. ch. it. 1899, 29. (2) 318.) 1062 THIOPHOSPHORYL CHLORIDE Thiophosphoryl pentachloride, PS 2 C1 5 (?). Decomp. by H 2 O. Sol. in alkalies with residue of S. Attacked violently by HNO 3 , alcohol, ether, oil of turpentine. Miscible with CS 2 . (Gladstone, Chem. Soc. 3. 5.) Thiophosphoryl fluoride, PSF 3 . Slowly sol. in H 2 O with decomp. SI. sol. in ether. Insol. in H 2 SO 4 , CS^ or benzene. (Thorpe and Rodger, Chem. Soc. 66. 306.) More sol. in KOH or NaOH+Aq than in H 2 0. Thiophosphoryl iodide, P 2 SI 2 . Very sol. in CS 2 . Unstable when heated. Fumes in the air. (Besson, C. R. 1896, 122. 1201.) Thiosulphuric (formerly Hyposulphur- ous) acid, H 2 S 3 O 3 . Known only in aqueous solution, which is extremely unstable, and decomposes very quickly after its formation. The time before decomposition is exactly proportional to the ratio, of the weight of H 2 O to the weight of H 2 S 2 O 3 present; i. e., if one solution contains twice as much H 2 O for a given amt. of H 2 S 2 p 3 as a second solution, the first solution will decompose in twice the length of time. The length of time is about 20 sees, at 10, and 2 sees, at 50 for cone, solutions, to 120 sees, at 10 and 12 sees, at 50 for very dilute solu- tions. (See Landolt (B. 16. 2958) for further figures; also Winkelmann (B. 18. 406). Thiosulphates. The thiosulphates of the alkalies and of Ca and Sr are easily sol. in H 2 O; Ba and Sr salts are si. sol. and the other salts insol. The salts of the metals dissolve in alkali thiosul- phates + Aq. All are insol. in alcohol. Double Salts of Thiosulphuric acid. It is impossible to determine whether substances of this class are true chem . individuals. Many described by Svensson and others are doubt- less isomorphic mixtures, whose comp. de- pends on the temp, and cone, of the solution in which pptd. (Rosenheim, Z. anorg. 1900 25.72.) Ammonium thiosulphate, (NH 4 ) 2 S 2 03. Very deliquescent. Very sol. in H 2 O. Not deliquescent. (Fock and Kliiss, B. 1889, 22. 3099.) Crystallises with VsH^O. (Rammelsberg, Pogg. 66. 298.) Anhydrous. (Arppe, A. 96. 113.) Insol. in alcohol. (Arppe.) Sol. in acetone. (Eidmann, C. C. 1899. II. 1014.) Difficultly sol. in acetone. (Naumann, B. 1904, 37. 4328.) Ammonium cadmium thiosulphate, 3(NH 4 ) 2 S 2 O 3 , CdS 2 O 3 +3H 2 O. Can be recryst. from warm H 2 O. and Kliiss, B. 23. 1758.) +H 2 O. (F. and K.) (NH 4 ) 2 S 2 3 , CdS 2 O 3 . (F. and K.) (Fock Ammonium cuprous thiosulphate, (NH 4 ) 2 S 2 O 3 , Cu 2 S 2 O 3 +2H 2 O. Less sol. in H 2 O than 2(NH 4 ) 2 S 2 O 3 , Cu 2 S 2 O 3 + l^H 2 O. (Rosenheim and Stein- hauser, Z. anorg. 1900, 26. 91.) 2(NH 4 ) 2 S 2 3 , Cu 2 S 2 3 +l^H 2 0. Very sol. in H 2 O. Insol. in alcohol. (Rosenheim and Steinhauser.) Ammonium cuprous thiosulphate cuprous iodide, 7(NH 4 ) 2 S 2 3 , Cu 2 S 2 O 3 , 8CuI+ 4H 2 O. Insol. in H 2 O. (Brun, C. R. 1892, 114. 668.) Could not be obtained. (Rosenheim and Steinhauser, Z. anorg. 1900, 26. 107.) Ammonium cuprous sodium thiosulphate ammonia, 3Cu 2 S 2 O 3 , 4Na 2 S 2 O 3 , (NH 4 ) 2 S 2 3 , 6NH 3 . Ppt. When dry is fairly stable in the air. Partially decomp. by H 2 O. Sol. in dil. H 2 SO 4 or acetic acid. (Shinn, J. Am. Chem. Soc. 1904, 26. 948.) Ammonium lead thiosulphate, 2(NH 4 ) 2 S 2 O 8 , PbS 2 O 3 +3H 2 O. Easily and completely sol. in cold H 2 O, but deposits PbS 2 O 3 by standing or warming. (Rammelsberg, Pogg. 66. 312.) Ammonium magnesium thiosulphate, rNH 4 ) 2 Mg(S 2 O 3 ) 2 +6H 2 O. Very deliquescent, and sol. in H 2 O. (Kess- ler, Pogg. 74. 283.) Not deliquescent. (Fock and Kliiss, B. 23. 540.) Ammonium mercuric thiosulphate, 4(NH 4 ) 2 S 2 3 , HgS 2 3 +2H 2 0. Sol. in H 2 O, from which it is precipitated by alcohol. Extremely easily decomp. (Ram- melsberg, Pogg. 56. 318.) Ammonium potassium thiosulphate, NH 4 KS 2 O 3 . Sol. in H 2 O. (Fock and Kliiss, B. I. 536.) Ammonium silver thiosulphate, 2(NH 4 ) 2 S 2 O 3 , Ag 2 S 2 O 3 +zH 2 O. Easily sol. in H 2 O. Somewhat sol. in alco- hol. (Herschel, Edinb. Phil. J. 1. 398.) (NH 4 ) 2 S 2 O 3 , Ag 2 S 2 O 3 +xH 2 O. Nearly in- sol. in H 2 O; sol. in NH 4 OH+Aq, from which it is repptd. by an acid. (Herschel.) THIOSULPHATE, BISMUTH POTASSIUM 1063 Ammonium zinc thiosulphate, 3, ZnS 2 O 3 +H 2 O. Very sol. in H 2 O. (Rosenheim and David- sohn, Z. anorg. 1904, 41. 238.) Ammonium thiosulphate ammonium cuprous bromide, CuBr, NHiBr, 4(NJI 4 ) 2 S 2 O 3 . Sol. in H 2 O. (Rosenheim, Z. anorg. 1900, 26. 107.) The double salts of ammonium thiosul- phate with silver and copper haloids are true chemical compounds and may be recryst. from H 2 O without decomp. (Rosenheim, Z. anorg. 1900, 25. 100.) Ammonium thiosulphate ammonium silver bromide, AgBr, NH 4 Br, 4(NH 4 )2S 2 O 3 . Sol. in H 2 O. (Rosenheim.) Ammonium thiosulphate ammonium cuprous chloride, CuCl, NH 4 C1, 4(NH 4 ) 2 S 2 O 3 . Sol. in H 2 O and in NH 4 OH+Aq. (Rosen- heim.) Ammonium thiosulphate ammonium silver chloride, AgCl, NH 4 C1, 4(NH 4 ) 2 S 2 O 3 . Sol. in cold H 2 O and NH 4 OH+Aq. Decomp. by boiling with H 2 O and by dil. acids. (Rosenheim.) Ammonium thiosulphate ammonium cuprous cyanide. Composition not constant. (Rosenheim.) Ammonium thiosulphate ammonium silver cyanide. Composition not constant. (Rosenheim.) Ammonium thiosulphate ammonium cuprous iodide, Cul, NHJ, 4(NH 4 ) 2 S 2 3 . Sol. in H 2 O. (Rosenheim.) Ammonium thiosulphate ammonium cuprous iodide, 4(NH 4 ) 2 S 2 O 3 , NHJ, Cul. Very sol. in H 2 O. Decomp. by boiling. (Brun, C. R. 1892, 114. 668.) Ammonium thiosulphate ammonium silver iodide, Agl, NH 4 I, 4(NH 4 ) 2 S 2 O 3 . Sol. in H 2 O. (Rosenheim.) Ammonium thiosulphate ammonium cuprous sulphocyanide, CuSCN, NH 4 SCN, 4(NH 4 ) 2 S 2 3 . Sol. in H 2 O. (Rosenheim.) Ammonium thiosulphate ammonium silver sulphocyanide, AgSCN, NH 4 SCN, 4(NH 4 ) 2 S 2 3 . Sol. in H 2 O. (Rosenheim.) Ammonium thiosulphate cuprous iodide, (NH 4 ) 2 S 2 3 , 2CuI+H 2 0. Insol. in H 2 O. (Brun, C. R. 1892, 114. 668.) Could not be obtained. (Rosenheim and Steinhauser.) Barium thiosulphate, BaS a 3 +H 2 O. SI. sol. in H 2 0. (Rose, Pogg. 21. 437.) Insol. in alcohol. 1 pt. cannot be dissolved in 2000 pts. H 2 0. Sol. in dil. HCl+Aq without decomposition. (Herschel, 1819.) Pptd. from BaS 2 O 3 +Aq by dil. alcohol. (Sobrero and Selmi, A. ch. (3) 28. 211.) Insol. hi acetone. (Naumann, B. 1904, 37. 4329.) Barium bismuth thiosulphate, Ba 3 [Bi(S 2 0) l ]j. Sol. in H 2 O with decomp. (Hauser, Z. anorg. 1903, 36. 9.) Barium cadmium thiosulphate, 2BaS 2 O 8 , CdS 2 3 +8H 2 0. SI. sol. in H 2 O. (Fock and Kliiss, B. 23. 1761.) 3BaS 2 O 3 , CdS 2 O 3 +8H 2 O. SI. sol. in H 2 O. Barium cuprous thiosulphate. Easily sol. in hot, difficultly sol. in cold H 2 O. (Cohen, Chem. Soc. 61. 38.) 2BaS 2 O 3 , Cu 2 S 2 O 3 -t-7H 2 O. Nearly insol. in H 2 O. (Vortmann, M. 9. 165.) Barium gold thiosulphate. SI. sol. in H 2 O. Insol. in alcohol (Fordos and Gelis.) Barium lead thiosulphate. Difficultly sol. in H 2 O. (Rammelsberg, Pogg. 66. 313.) Barium thiosulphate chloride, BaS 2 O 8 , BaCl 2 +2H 2 O. Sol. in H 2 O. (Fock and Kliiss, B. 23. 3001.) Bismuth caesium thiosulphate, Cs 3 Bi(S 2 O 8 ) 8 . Sol. in H 2 O. Insol. in alcohol. (Hauser, Z. anorg. 1903, 36. 8.) Bismuth potassium thiosulphate, Solubility in H 2 0. 100 cc. of the sat. solution contain 3.5 g. at 2; 7.0 g. at 18. At 18 the solution decomposes. More sol. in Na 2 S 2 O 3 +Aq than in pure TT r\ Insol. in alcohol. (Hauser, Z. anorg. 1903, *+H 2 O Sol. in H 2 O. Insol. in alcohol. (Carnot, C. R. 83. 390.) 1064 THIOSULPHATE, BISMUTH RUBIDIUM Bismuth rubidium thiosulphate, Rb 3 Bi(S 2 3 ) 3 +^H 2 0. Sol. in H 2 O. Insol. in acid alcohol. (Hauser. Z. anorg. 1903, 36. 7.) +H 2 O. Sol. in H 2 O. (Hauser, Z. anorg. 1903, 36. 8.) Bismuth sodium thiosulphate, Very sol. in H 2 O, and also in alcohol. (Carnot, C. R. 83. 338.) Na 3 Bi(S 2 O 3 ) 3 . Decomp. by H 2 O. Easily sol. in 50% alcohol. (Hauser, Z. anorg. 1903, 35. 3.) Cadmium thiosulphate, CdS 2 O 3 +2H 2 O. Sol. in H 2 O. Insol. in alcohol. (Vortmann and Padberg, B. 22. 2638.) Cadmium potassium thiosulphate, 3CdS 2 3 , 5K 2 S 2 O 3 . Cannot be recryst. without decomp. (Fock and Kluss, B. 23. 1753.) CdS 2 O 3 , 3K 2 S 2 O 3 +2H 2 O. Can be crystal- lised from H 2 O without decomp. (F. and K.) Cadmium sodium thiosulphate, CdS 2 O 3 , 3Na 2 S 2 O 3 +16H 2 O. Not deliquescent. Sol. in H 2 O. (Jochum, C. C. 1885, 642.) +9H 2 O. (Vortmann and Padberg, B. 22. 2639.) +3H 2 O. Deliquescent. (Fock and Kluss, B. 23. 1157.) 2CdS 2 O 3 , Na 2 S 2 O 3 +7H 2 O. (V. and P.) 3CdS 2 O 3 , Na 2 S 2 O 3 +9H 2 O. (V. and P.) Cadmium strontium thiosulphate. CdS 2 O 3) 3SrS 2 O 3 +10H 2 O. (Fock and Kluss, B. 23. 1763.) Caesium' thiosulphate, Cs 2 S 2 O 8 . Easily sol. in H 2 O. (Chabrie", C. R. 1901, 133. 297.) +2H 2 O. Very hydroscopic. (J. Meyer, B. 1907, 40. 1360.) Caesium cuprous thiosulphate, Cs 2 S 2 O 3 , Easily sol. in H 2 O with decomp. Meyer, B. 1907, 40. 1361.) (J. Caesium lead thiosulphate, Cs 2 S 2 O 3 , PbS 2 3 +2H 2 0. Not hydroscopic. 2Cs 2 S 2 O 3 , PbS 2 O 3 +3H 2 O. (J. Meyer.) Hydroscopic. Caesium magnesium thiosulphate, Cs 2 S 2 O 3 , MgS 2 8 +6H 2 0. Easily sol. in H 2 O. (Meyer.) Caesium silver thiosulphate, 2Cs 2 S 2 O 3 , Ag 2 S 2 3 +3H 2 0. Not hydroscopic. Decomp. by hot H 2 O. (J. Meyer.) Calcium thiosulphate, CaS 2 O 3 +6H 2 O. Sol. in 1 pt. H 2 O at 3. Aqueous 'solution saturated at 10 has sp. gr. 1.300. Solution with sp. gr. 1.11437 at 15.5 contains 0.2081 of its weight in CaS 2 O 3 . Decomp. on heating. Insol. in alcohol (sp. gr. 0.8234). (Herschel, A. ch. 14. 355.) 100 g. sat. solution contains 29.4 g. CaS 2 3 at 9, and 34.7 g. CaS 2 O 3 at 25. (Kremann and Rodemund, M. 1914, 35. 1065.) Solubility of CaS 2 O 3 +Na 2 SO 3 in H 2 O. t o/ NfttfiOi % CaS2Os Solid phase 9 11.04 25.21 31.01 29.4 22.64 15.84 7.70 CaS 2 O 3 , 6H 2 O (e " +Na 2 S 2 O 3 , 5H 2 O Na 2 S 2 3 , 5H 2 25 9.24 15.67 18.34 28.24 30.19 31.24 35.04 34.7 29.69 21.41 25.18 21.14 20.33 18.43 11.61 CaS 2 3 , 6H 2 O (i u (C (( " +Na 2 S 2 3 , 5H 2 O Na 2 S 2 O 3 , 5H 2 O a (Kremann and Rodemund, M. 1914, 35. 1065.) Calcium lead thiosulphate, 2CaS 2 O 3 , PbS 2 O 3 +4H 2 0. Decomp. by H 2 O. (Rammelsberg.) Calcium potassium thiosulphate, CaS 2 O 8 , 3K 2 S 2 3 +5H 2 0. Sol. in H 2 O. (Fock and Kluss, B. 24. 3016.) Calcium silver thiosulphate, 2CaS 2 O 3 , Ag 2 S 2 3 Easily sol. in H 2 O; less sol. in alcohol. CaS 2 O 3 , Ag 2 S 2 O 3 +.rH 2 O. SI. sol. in H 2 O, abundantly in NH 4 OH+Aq. (Herschel, 1819.) Calcium sodium thiosulphate nitrate, . CaNa 3 (S 2 O 3 ) 2 NO 3 +llH 2 O. (Kremann and Rothemund, M. 1914, 35. 1065.) Cobaltous thiosulphate, CoS 2 O 8 +6H 2 O. Sol. in H 2 O. (Rammelsberg.) Cobaltous sodium thiosulphate, 2CoS 2 8 , 5Na 2 S 2 3 +25H 2 0. Efflorescent. Sol. in H 2 O. (Jochum.) Could not be obtained by Vortmann and Padberg. THIOSULPHATE, CUPRIC SULPHIDE, CUPRIC SODIUM 1065 CoS 2 O 3 , 3Na 2 S 2 O 3 + 15H 2 O. Sol. in H 2 O. (Vortmann and Padberg, B. 22. 2641.) Cuprous thiosulphate, Cu 2 O, 3S 2 O 2 +2H 2 O = Cu 2 H 4 (S 2 3 ) 2 . SI. sol. in H 2 O. Abundantly sol. in Na 2 S 2 O 3 + Aq, NH 4 C1 + Aq, NH 4 OH + Aq, or (NH 4 ) 2 CO 3 +Aq. Sol. in HC1 or HNO 3 +Aq. (v. Hauer, W. A. B. 13. 443.) Cuprous hydrazine thiosulphate, Cu 2 S 2 3 , (N 2 H 4 ) 2 H 2 S 2 Insol. in H 2 O; sol. in NH 4 OH+Aq and in dU. acids. (Ferratini, C. C. 1912, I. 1281.) Cupric lead thiosulphate, Pb(CuS 2 O 3 ) 2 +3H 2 0. (?) Very sol. in H 2 O and quickly decomp. (Girard, C. C. 1904, I. 253.) Cuprous mercurous thiosulphate, 5Cu 2 S 2 O 3 . 3Hg 2 S 2 O 3 . Insol. or si. sol. in cold, decomp. by boiling H 2 O. HNO 3 +Aq dissolves out Cu. (Ram- melsberg, Pogg. 66. 319.) Cuprous potassium thiosulphate, Cu 2 S 2 O 3 , K 2 S 2 O 3 +2H 2 O. SI. sol. in H 2 O; decomp. on heating with pptn. of CuS. Easily sol. in K 2 S 2 O 3 +Aq. (Rammelsberg, Pogg. 56. 321.) Cu 2 S 2 O 3 , 2K 2 S 2 O 3 . Very sol. in cold H 2 O; insol. in K 2 S 2 O 3 +Aq. (Cohen, Chem. Soc. 61. 39.) +3H 2 O. Scarcely sol. in cold, sol. with si. decomp. in hot H 2 O. Sol. in HCl+Aq with evolution of SO 2 . Cu 2 S 2 O 3 , 3K 2 S 2 O 3 +3H 2 O. More sol. in H 2 O than Cu 2 S 2 O 3 , K 2 S 2 O 3 +2H 2 O. Solution is not decomp. by boiling. Sol. in excess of NH 4 OH+Aq. (Rammelsberg.) Cuprous rubidium thiosulphate, Rb 2 S 2 O 3 , Cu 2 S 2 3 +2H 2 0. Ppt. (J. Meyer, B. 1907, 40. 1357.) 2Rb 2 S 2 O 3 , Cu 2 S 2 3 +2H 2 O. Ppt. (J. Meyer.) 3Rb 2 S 2 O 3 , Cu 2 S 2 O 3 +2H 2 O. Meyer.) Ppt. (J. Cuprous saver sodium thiosulphate am- monia, Cu 2 S 2 O 8 , 2Ag 2 S 2 O 3 , 5Na 2 S 2 O 3 , 6NH 3 . Ppt. Becomes dark when exposed to light. Decomp. by H 2 O. Sol. in NH 4 OH+Aq. (Shinn, J. Am. Chem. Soc. 1904, 26. 949.) Cuprous sodium thiosulphate, 2Cu 2 S 2 O 3 , 7Na 2 S 2 8 +2H 2 0. Ppt. from aqueous solution by alcohol. (Jochum, C. C. 1886. 642.) + 12H 2 O. Sol. in very dil. HCl+Aq. (Jochum-.) Cu 2 S 2 O 3 , 3Na 2 S 2 O 3 +2H 2 O. Sol. in H 2 O; insol. in alcohol. (Rammelsberg.) +6H 2 O. (Jochum.) 3Cu 2 S 2 O 3 , 2Na 2 S 2 O 3 +8H 2 O. Decomp. by H. 2 O. (Vortmann.) +5H 2 O. (Lenz, A. 40. 99.) Formula ac- cording to Jochum is 5Cu 2 S 2 O 3 , 4Na 2 S 2 O 3 +8H 2 O. Insol. in H 2 O or alcohol. Sol. in HCl+Aq without evolu- tion of SO 2 , also in dil. H 2 SO 4 or HNO 3 +Aq. Sol. in NH 4 OH+Aq. (Jochum.) +6H 2 O. As above. (Jochum.) Cu 2 S 2 O 3 , Na 2 S 2 O 3 +H 2 O. Insol. in H 2 O; sol. in Na 2 S 2 O 3 +Aq. (Russell, Ch. Ztg. 9. 233.) +2H 2 O. Insol. in H 2 O and alcohol. Decomp. by dil. acids. (Rosenheim and Steinhauser, Z. anorg. 1900, 25. 84.) +2^H 2 O. Sol. in H 2 O. Pptd. by alcohol. (Bhaduri, Z. anorg. 1898, 17. 1.) +3H 2 O. Decomp. by H 2 O. (Vortmann, M. 1888, 9. 168.) 3Cu 2 S 2 O 3 , 2Na 2 S 2 O 3 . (Gerard, C. C. 1904, I. 253.) +5H 2 O. Sol. in 352 pts. H 2 O. (Russell, Ch. Z. 1885, 9. 223.) 100 cc. 5% Na 2 S 2 3 +Aq dissolve 12.28 g. " " 7.5% " " 17.46g. " "10% " " 22.54g. (Russell, Ch. Z. 1885, 9. 223.) 4Cu 2 S 2 O 3 , 3Na 2 S 2 O 3 +6H 2 O. Insol. in H 2 O and alcohol. Decomp. by dil. acids. (Rosenheim and Steinhauser, 7. anorg. 1900, 26. 84.) +9H 2 O. Sol. in H 2 O. Pptd. by alcohol. (Bhaduri, Z. anorg. 1898, 17. 1.) 7Cu 2 S 2 O 3 , 5Na 2 S 2 O 3 + 16H 2 O. Decomp. by H 2 O and by alcohol. (Bhaduri, Z. anorg. 1898, 17. 1.) It is impossible to determine whether any of these compds. are complex or double salts. As a class they are not easily sol. and decomp. in solution. They may therefore be mixtures whose comp. depended upon the temp, and cone, of the solution in which they were pptd. (Rosenheim, Z. anorg. 1900, 26. 81.) Cuprocupric sodium thiosulphate ammonia, Cu 2 S 2 O 3 , CuS 2 O 8 , 2Na 2 S 2 O 3 , 4NH S . Insol. in, but decomp. by hot H 2 0. Sol. in HC 2 H 3 O 2 +Aq. Sol. in~NH 4 OH+Aq or Na 2 S 2 O 3 +Aq. (Schutte, C. R. 42. 1267.) Cuprous sodium thiosulphate cuprous chlor- ide, Cu 2 S 2 O 8 , 2Na 2 S 2 O 3 , 2CuCl. (Rosenheim and Steinhauser, Z. anorg. 1900, 26. 86.) Cupric sodium thiosulphate cupric sulphide, Cu 2 S 2 O 3 , Na 2 S 2 O 3 , CuS+4H 2 O. ; SI. sol. in H 2 O; easily sol. in Na 2 S 2 O 3 +Aq, and NH 4 OH+Aq; insol. in alcohol. (Lenz, A. 40. 99.) Cu 2 S 2 O 3 , Na 2 P 2 O 3 , 2CuS. Sol. in H 2 O or dil. HCl+Aq. (Kessel, B. 11. 1585.) 1066 THIOSULPHATE SODIUM CHLORIDE, CUPROUS SODIUM Cuprous sodium thiosulphate sodium chlor- ide, 3Cu 2 S 2 O 3 , 2Na 2 S 2 O 3 , 4NaCl+8H 2 O Sol. in Na 2 S 2 O 3 +Aq. (Siewert, Zeit. ges Naturwiss. 26. 486.) Ppt. (Bhaduri, Z. anorg. 1898, 17. 3.) Cupric thiosulphate ammonia, CuS 2 O 3 , 4NH 3 . 100 pts. H 2 O dissolve 21.79 pts. at 25 (Pudschies, Dissert.) Cuprocupric thiosulphate ammonium chlor- ide, Cu 2 O, CuO, 3S 2 O 2 , 2NH 4 C1. Sol. in HNO 3 +Aq with separation of S. (v. Hauer, W. A. B. 13. 447.) Glucinum thiosulphate, G1S 2 O 3 +11H 2 O. (Faktor, C. C. 1901, II. 878.) Gold (aurous) hydrogen thiosulphate, Au 2 S 2 3 , 3H 2 S 2 O 3 . Known only in solution. (Fordos and Gelis, A. ch. (3) 13. 394.) Gold (aurous) sodium thiosulphate, Au 2 S 2 3 , 3Na 2 S 2 3 +4H 2 0. Sol. in H 2 O; solution decomp. on heating. Insol. in absolute, si. sol. in dil. alcohol. (Fordos and Gelis.) Au 2 S 2 O 3 , 6Na 2 S 2 O 3 +10H 2 O. Very sol. in H 2 O, but decomp. by boiling. (Jochum, C. C. 1885. 642.) Iron (ferrous) thiosulphate, FeS 2 O 3 +5H 2 O. Deliquescent. Very sol. in H 2 O or alcohol. (Koene,- Pogg. 63. 241.) Iron (ferrous) sodium thiosulphate, FeS 2 O 3 , 3Na 2 S 2 O 3 +8H 2 O. Very sol. in H 2 O, and easily decomp. (Vortmann and Padberg, B. 22. 2641.) Lead thiosulphate, PbS 2 O 3 . k Sol. in 3266 pts. H 2 O. Sol. in alkali thio- sulphates +Aq. (Rammelsberg, Pogg. 66. 308.) Lead lithium thiosulphate, PbS 2 3 , Li 2 S 2 O 3 . Very hydroscopic. Decomp. by H 2 O with separation of PbS. (J. Meyer, B. 1907, 40. 1355.) Lead potassium thiosulphate, PbS 2 O 3 , 3K 2 S 2 3 +2H 2 0. Sol. in H 2 O with partial separation of PbS 2 O 3 . Sol. in K 2 S 2 O 3 +Aq. (Rammels- berg, Pogg. 56. 310.) Lead rubidium thiosulphate, 2Rb 2 S 2 O 3 , PbS 2 3 +2H 2 0. Difficultly sol. in cold H 2 O. Decomp. by H 2 O. (J. Meyer, B. 1907, 40. 1358.) Lead sodium thiosulphate, PbS 2 O 3 , 2Na 2 S 2 O 8 . SI. sol. in H 2 O. Very easily sol. in NaC 2 H 3 O 2 and Na 2 S 2 O 3 +Aq. (Lenz, A. 40. 98.) Insol. in alcohol. 2PbS 2 O 3 , 5Na 2 S 2 O 3 +60H 2 O. Easily de- comp. (Jochum, C. C. 1885. 642.) PbS 2 O 3 , 3Na 2 S 2 O 3 + 12H 2 O. Decomp. in boiling aqueous solution. (Vortmann and Padberg, B. 22. 2637.) Lead strontium thiosulphate. Sol. in H 2 O. Precipitated as a syrup by alcohol. (Rammelsberg.) ;, Lithium thiosulphate, Li 2 S 2 O 3 +3H 2 O. Very deliquescent, and sol. in H 2 O and absolute alcohol. (Fock and Kluss, B. 22. 3099.) Lithium silver thiosulphate, Li 2 S 2 3 , Ag 2 S 2 O 8 +H 2 O. Hygroscopic. Decomp. by boiling H 2 O and by acids. (Meyer and Eggeling, B. 1907, 40. 1355.) Magnesium thiosulphate, MgS 2 O 3 +6H 2 O. Very easily sol. in H 2 O. Precipitated from cone, solution by alcohol. (Rammelsberg, Pogg. 56. 303.) Magnesium potassium thiosulphate, MgK 2 (S 2 3 ) 2 +6H 2 0. Deliquescent, and sol. in H 2 O. Less sol. than K 2 S 2 O 3 . (Rammelsberg, Pogg. 56. 304.) Not deliquescent. (Fock and Kluss, B. 23. 539.) Magnesium rubidium thiosulphate, MgS 2 O 8 , Rb 2 S 2 3 +6H 2 0. Easily sol. in H 2 O.- (Meyer. B. 1907, 40. 1358.) Manganous thiosulphate, MnS 2 O 3 . Sol. in H 2 O, from which it is pptd. by alcohol. (Rammelsberg, Pogg. 56. 305.) +5H 2 O. Decomp. very easily. (Vort- mann and Padberg, B. 322. 2641.) Manganous sodium thiosulphate, MnS 2 O 8 , 2Na 2 S 2 3 +16H 2 O. Sol. in H 2 O. Insol. or but si. sol. in alcohol. (Jochum, C. C. 1885. 642.) Mercuric potassium thiosulphate, 3HgS 2 O 8 , 5K 2 S 2 3 . Sol. in 10 pts. H 2 O at 15, and Y^ pt. at 100. Aqueous solution decomp. on stand- ing or heating. Insol. in alcohlol. (Kirchhoff, Scher. J. 2. 30.) HgS 2 O 3 . 3K 2 S 2 O 3 +3H 2 O. (Fock and Kluss, B. 24. 1353.) HgS 2 Q 3 , 5K 2 S 2 3 +H 2 0. (F. and K.) THIOSULPHATE, SILVER SODIUM 1067 Nickel thiosulphate, NiS 2 O 3 +6H 2 O. Permanent. Sol. in H 2 O. (Rammelsberg, Pogg. 66. 306.) Nickel sodium thiosulphate, 2NiS 2 O 3 , 5Na 2 S 2 O 3 -f25H 2 O. Efflorescent. Sol. in H 2 O. (Jochum.) Nickel thiosulphate ammonia, NiS 2 O 8 , 4NH 3 +6H 2 0. Decomp. on air. Sol. in NH 4 OH+Aq. ' 306.) (Ephraim, B. 1913, (Vortmann and (Rammelsberg, Pogg. 66. 306.) NiS 2 O 3 , 5NH 3 +H 2 O. 46. 3108.) NiS 2 O 3 , 6NH 3 +3H 2 O. Padberg, B. 22. 2641.) Platinous sodium thiosulphate. See Platothiosulphate, sodium. Potassium thiosulphate, K 2 S 2 O 3 +V3, 1, 1 2 /3H 2 O, and 2H 2 O. Very deliquescent. Very sol. in H 2 O with absorption of heat. Solution is stable on the air. Insol. in alcohol. 100 pts. H 2 O dissolve pts. K 2 S 2 O 3 at t. t Pts. K 2 S 2 03 Solid phase 96.1 K 2 S 2 O 3 .2H 2 O 17 150.5 3K 2 S 2 O 3 .5H 2 O 20 155.4 " 25 165.0 " 30 175.7 " 35 202.4 3K 2 S 2 O 3 .5H 2 O+K 2 S 2 O 3 .H 2 O 40 204.7 K 2 S 2 O 3 .H 2 O 45 208.7 u 50 215.2 a 55 227.7 u 60 238.3 n 56.1 234.5 K 2 S 2 O 3 .H 2 O+3K 2 S 2 O 3 .H 2 O 65 245.8 3K 2 S 2 3 .H 2 70 255.2 a 75 268.0 it 78.3 292.0 3K 2 S 2 O 3 .H 2 O+K 2 S 2 O 3 80 293.1 K 2 S 2 3 85 298.5 [( 90 312.0 (i (Inohiko lo, Mem. Coll. Sc. Kioto, 1911, 3. 212.) Sol. in dil. HC 2 H 3 O 2 +Aq without decomp. (Mathieu-Plessy, C. R. 101. 59.) Insol. in ethyl acetate. (Casaseca, C. R. 30. 821.) Potassium silver thiosulphate, 2K 2 S 2 O 3 , Ag 2 S 2 3 . Sol. inH 2 O. (Cohen.) K 2 S 2 O 3 , Ag 2 S 2 O 3 . SI. sol. in H 2 O. (Her- schel.) 3K 2 S 2 O 3 , Ag 2 S 2 O 3 +2H 2 O. Rather si. sol. in H 2 O. (Rosenheim and Steinhauser, Z. anorg. 1900, 26. 76.) SI. sol. in H 2 O. (Rosenheim.) Potassium silver thiosulphate ammonia, KAgS 2 O 3 , 2NH 3 . Very si. sol. in H 2 O. Easily sol. in hot NH 4 OH+Aq. (Schwicker, B. 22. 1735.) 5K 2 S 2 O 3 , 3Ag 2 S 2 O 3 , NH 3 . Difficultly sol. in H 2 O with decomp. Sol. in hot NH 4 OH+Aq with partial de- comp. (J. Meyer, B. 1907, 40. 1359.) Potassium sodium thiosulphate. (a) KNaS 2 O 3 +2H 2 O. Very sol. in H 2 O. 100 pts. H 2 O dissolve 213.7 pts. salt at 15. (Schwicker, B. 22. 1733.) (6) NaKS 2 O 3 +2H 2 O. 100 pts. H 2 O dis- solve 205.3 pts. salt at 15. (Schwicker.) Potassium strontium thiosulphate, K 2 S 2 O 3 , SrS 2 O 3 +5H 2 O. Sol. in H 2 O. (Fock and Kliiss, B. 24. 3017.) Potassium zinc thiosulphate, K 2 S 2 O 3 , ZnS 2 O 3 +H 2 O. Very sol. in H 2 O. (Rosenheim and David- sohn, Z. anorg. 1904, 41. 238.) Potassium thiosulphate sodium chloride, K 2 S 2 3 , NaCl. Sol. in H 2 O. (Pape, Pogg. 139. 238.) Rubidium thiosulphate, Rb 2 S 2 O 3 +2H 2 O. Very hydroscopic; easily sol. in H 2 O. (J. Meyer, B. 1907, 40. 1356.) Rubidium silver thiosulphate, 2Rb 2 S 2 3 , A g2 S 2 3 +2H 2 0. Ppt. Not hydroscopic. Difficultly sol. in cold H 2 O. Decomp. by warm H 2 O. (J. Meyer.) Rubidium silver thiosulphate ammonia, Rb 2 $ 2 O 3 , Ag 2 S 2 O 3 , NH 3 . Ppt. (J. Meyer.) 3Rb 2 S 2 O 3 , 4Ag 2 S 2 O 3 , NH 3 . Ppt. Decomp. in the air. (J. Meyer.) Samarium thiosulphate. (Cleve.) Scandium thiosulphate, basic, Sc(OH)S 2 O 3 . Ppt. (R.. J. Meyer, Z. anorg. 1914, 86. 282.) Silver thiosulphate, Ag 2 S 2 O 8 . SI. sol. in H 2 O. Sol. in NH 4 OH or alkali thiosulphates-{-Aq. (Herschel, Edinb. Phil. J. 1. 26.) Silver sodium thiosulphate, Ag 2 S 2 O, Na 2 S 2 O 3 +H 2 O. SI. sol. in H 2 O. Easily sol. in NH 4 OH + Aq, also in Na 2 S 2 O 3 +Aq to form Ag 2 S 2 O 3 , 2Na 2 S 2 O 3 +2H 2 O. Easily sol. in H 2 O or NH 4 OH+Aq; somwehat sol. in*al- 1068 THIOSULPHATE ACETYLIDE ACETYLENE, SILVER SODIUM cohol, especially if warm or dilute. (Lenz, A. 40. 94.) Ag 2 S 2 O 3 , 6Na 2 S 2 O 3 +21H 2 O. Sol. in H 2 O. (Jochum, C. C. 1885. 642.) SUver sodium thiosulphate acetylide acety- lene, 2Na 2 S 2 O 3 , 7Ag 2 S 2 O 3 , 18Ag 2 C 2 , 32C 2 H 2 . Decomp. by H 2 O. Sol. in NH 4 OH+Aq. Insol. in alkalies. (Bhaduri, Z. anorg. 1913, 79 356 ) 7Na 2 S 2 O 3 , 5A g2 S 2 O 3 , 86Ag 2 C 2 , 13C 2 H 2 . (Bhaduri.) Silver sodium thiosulphate ammonia, NaAgS 2 O 3 , NH 3 . Very unstable. (Schwicker, B. 22. 1736.) Silver strontium thiosulphate, Ag 2 S 2 O 3 , SrS 2 O 3 . Nearly insol. in H 2 O. Very si. sol. in SrS 2 O 3 +Aq; easily sol. in NH 4 OH+Aq. (Herschel.) Sodium thiosulphate, Na 2 S 2 O 3 and +1, 2 and 5H 2 O. 100 pts. H 2 O dissolve: At 16, 65 pts. Na 2 S 2 O 3 . "20, 69 "25, 75 "30, 82 "35, 89 "40, 98 " 45, 109 "47, 114 (Mulder.) 100 pts. H 2 O dissolve at 0, 47.6 pts. Na 2 S 2 O 3 ; at 20, 69.5 pts. ; at 4~0*, 104 pts. ; at 60, 192.3 pts. (Kremers, Pogg. 99. 50) 100 pts. H 2 O dissolve 171 pts. cryst. ( = 108.9 pts. anhydrous )salt at 19.5 to form a solution of 1.3875 sp. gr. (Schiff, A. 113. 350.) By supersaturation 100 pts. H 2 O may dis- solve 217.4 pts. Na 2 S 2 O 3 at 0. (Kremers.) Solubility in H 2 O. t % Na 2 S 2 O3 Solid phase 34.43 Na 2 S 2 O 3 +5H 2 O 10 37.89 tt 20 41.17 (i 30 45.86 tt 40 50.65 a 45 54.49 t( 50 62.92 Na 2 S 2 O 3 +2H 2 O 60 67.39 te 72 70.39 {( 80.5 71.33 tt 90.5 71.76 it 100 72.68 it (Taylor, Proc. Edinburgh Soc. 1898, 22. 49.) Solubility of anhydrous Na 2 S 2 O 3 in H 2 O at t c t g. Na S 2 O 3 per 100 g. Solution HO 40 67.40 206.70 45 67.60 208.60 50 67.76 210.20 55 68.15 214.00 60 68.48 217.30 65 68.80 220.50 70 69.05 223.10 75 69.35 226.30 80 69.80 231.80 (Young and Burke, J. Am. Chem. Soc. 1906, 28. 327.) The solubility of the hydrates of Na 2 S 2 O 3 are exceedingly complicated. There are five groups of hydrates, (I) primary, (II) second- ary, (III) tertiary, (IV) quaternary, and (V), quintary, and transitions occur between mem- bers of the same and different groups. Na 2 S 2 O 3 +5H 2 O(I) is the commercial thio- sulphate. The relations and solubility of the various hydrates is shown in the following akj^o^/r Solubility of Na 2 S 2 3 in H 2 O at t. I. Primary hydrates. g. Na2S2Os per t 100 g. Solid phase Solution H 2 O 33.40 50.15 Na 2 S 2 3 , 5H,0(I) 5 35.33 54.64 " 10 37.37 59.69 (C 15 39.11 64.22 {{ 20 41.20 70.07 (( 25 43.15 75.90 It 30 45.19 82.45 11 35 47.71 91.24 " 40 50.83 105.37 a 45 55.33 123.87 a 48.17 " +Na 2 S 2 3 , 2H,0(I) 52.73 111.60 Na 2 S 2 3 , 2IT 2 0(I) 5 53.45 114.90 R 10 53.94 117.10 t( 20 55.15 122.68 ii 25 56.03 127.43 tt 30 57.13 133.27 ( 40 59.38 146.20 ( '45 60.73 154.70 t 50 62.28 165.11 c 55 63.85 176.60 t 60 65.68 191.30 ( 65 68.04 212.90 t 66.5 ... " +Na 2 S 2 3 THIOSULPHATE, SODIUM 1069 Solubility of Na 2 S 2 O 3 in H 2 O at t . Continued. II. Secondary hydrates. Solubility of Na 2 S 2 O 3 in H 2 O at t Continued. IV. Quaternary hydrate. t g. NaiSzOs per 100 g. Solid phase t g. NaaS2O3 per 100 g. Solid phase Solu tion H 2 Solu- tion H 2 5 10 15 20 25 30 30.22 41.96 43.56 45.25 47.27 49.38 52.15 56.57 72.30 77.17 82.65 89.36 97.55 108.98 130.26 Na 2 S 2 O,, 5H 2 O(II) t t . i t " Na 2 S 2 O 3 , 4H 2 O(II) 5 10 15 20 25 30 35 40 45 50 55 58 57.63 58.08 58.49 59.00 59.57 50.35 61.03 61.94 62.95 64.22 65.45 67.07 136.00 138.60 140.90 143.90 147.30 152.30 156.60 162.80 169.90 179.50 189.50 203.70 NaAO,, 4 ViH,0(IV) 1C (( It It tt (t tl 11 tt tt ," +Na 2 S 2 3 33.5 36.2 38.6 40.65 58.59 60.51 62.80 141.48 153.23 168.82 Na 2 S 2 3 , 4H 2 O(II) t( u " +Na 2 S 2 3 , H,0(II) 5 10 15 20 25 30 35 40 45 50 55 56.5 60.47 60.74 61.04 61.57 62.11 62.73 63.56 64.32 65.22 66.02 66.82 67.90 153.00 154.70 156.70 160.20 163.90 168.30 174.40 180.20 187.60 194.30 201.40 211.50 Na 2 S 2 3 , ( H 2 0(lI) a n a (i ft 1C (I tl (( (I " +Na 2 S 2 3 V. Quintary hydrates. 5 10 15 20 25 30 35 27.5 57.63 58.23 59.05 60.02 61.02 62.30 63.56 65.27 136.00 139.40 144.20 150.10 156.50 165.30 174.40 188.00 Na 2 S 2 3 , ( 2H 2 0(V) < i < i ( 11 +Na 2 S 2 3 , H 2 0(V) 30 35 40 45 50 55 43 63.34 64.07 64.75 65.58 66.58 67.59 172.80 178.40 183.70 190.50 199.20 208.50 Na 2 S 2 3/( H 2 0(V) ti ti it "+Na 2 S 2 3 , VH,0(V) III. Tertiary hydrates. 5 10 13 14.35 14.3 46.14 48.44 51.66 54.96 85.67 93.95 106.80 122.00 Na 2 S 2 O 3 , 6H 2 O (III and IV) u n ti "+Na,S,0,, 4 / 3 H 2 0(IV) "+Na 2 S 2 O 3 , 3 / 2 H 2 O(lII) 25 35 40 45 50 55 60 65 70 70 64.21 64.60 64.99 65.61 66.02 66.57 67.40 68.24 69.06 179.40 182.50 185.60 190.82 194.30 199.10 206.70 214.90 Na 2 S 2 3 , ^H 2 0(V) tt ti i t i i t " Na 2 S 2 8 5 10 15 20 25 30 35 40 45 47.5 48.5 57.42 57.84 58.28 58.80 59.28 60.18 60.78 61.57 62.60 63.97 64.68 134.80 137.20 139.70 142.70 145.60 151:10 155.00 160.20 167.40 177.50 183.00 Na 2 S 2 3 , yH,0(III) n K . tt a (( te (t n " +Na 2 S 2 3 , H,0(III) (Young and Burke, J. Am. Chem. Soc. 1906, 28. 321.) Heat is absorbed bv dissolving in H 2 O. 110 pts. Na 2 S 2 O 3 +5H 2 O + 100 pts. H 2 O lower temp, from 10.7 to 8. (Riidorff, B. 3. 68.) -f i^H 2 O. (Young and Burke, J. Am. Chem. Soc. 1906, 28. 321.) +H 2 0. + 4 / 3 H 2 O. (Young and Burke.) + 3 / 2 H 2 O. (Young and Burke.) 47.5 50 52.5 55 60 61 64.78 65.30 65.89 66.45 68.07 183.90 188.20 193.20 198.10 213.10 Na 2 S 2 O 3 , H 2 OaiI) tt a (t it " +Na 2 S 2 3 1070 THIOSULPHATE, SODIUM THALLOUS +2H 2 O. +4H 2 O. M.-pt. 41.60. (Young and Burke.) +5H 2 O. M.-pt. 45 (Kopp); 48 (Krem- ers), 50 (Mulder); 48.5 (Tilden, Chem. Soc. 46. 409); 47.9 (Taylor, Proc. Edinburgh, Soc. 1898, 22. 249); 48.09 (Richards and Churchill, Z. phys. Ch. 1899, 28. 314); 48.45 (Young and Burke, J. Am. Chem. Soc. 1906, 28. 324.) Labile modification melts at 32. (Parmen- tier and Amat, C. R. 98. 735.) Sp. gr. of Na 2 S 2 O 3 +Aq at 19. % = %Na 2 S 2 O 3 +5H 2 O. Sodium thallous thiosulphate, 3Na 2 S 2 3 , 2T1 2 S 2 Q 3 +10H 2 O. Sol. in H 2 O. (Werther.) +8H 2 O. (Jochum.) 2Na 2 S 2 O 3 , T1 2 S 2 O 3 +8H 2 O. (Vortmann ind Padberg, B. 22. 2638.) Sodium zinc thiosulphate, Na 2 S 2 O 3 , 2ZnS 2 O 3 +23H 2 O. Sol. in H 2 O. (Jochum, C. C. 1885. 642.) 3Na 2 S 2 O 3 . 2ZnS 2 O 3 '+10H 2 O. Deliques- cent. (Vortmann and Padberg, B. 22. 2640.) Sodium thiosulphate mercuric iodide, % Sp. gr. % Sp. gr. % Sp. gr. ^ixj* 2 02vy 3 , iigj. 2 . Decomp. by H 2 O and by alcohol. (Eder 1 1.0052 18 1.0975 35 1.1986 and Ulm, M. 1882, 3. 197.) 2 3 1.0105 1.0158 19 20 1.1031 1 . 1087 36 37 1.2048 1.2110 Strontium thiosulphate, SrS 2 O 3 +5H 2 O. 4 1.0211 21 1.1145 38 1.2172 Permanent. Sol. in 6 pts. cold H 2 O (Gay- 5 1.0264 22 1 . 1204 39 1.2234 Lussac); in 4 pts. H 2 O at 13, and 1.75 pts. 6 1.0317 23 1.1263 40 1.2297 boiling H 2 O (HerscheL 1819). 7 1.0370 24 1.1322 41 1.2362 1 g. is sol. in 3.7 cc. H 2 O at room temp. 8 1.0423 25 1 . 1381 42 1.2427 Antenrieth, Z. anal. 1898, 37. 293.) 9 1.0476 26 1 . 1440 43 1.2492 Gradually efflorescent. Insol. in alcohol. 10 1.0529 27 1.1499 44 1.2558 HerscheL) 11 1.0584 28 1 . 1558 45 1.2624 12 13 14 15 16 1.0639 1.0695 1.0751 1.0807 1.0863 29 30 31 32 33 1.1617 1 . 1676 1 . 1738 1 . 1800 1 . 1862 46 47 48 49 50 1.2690 1.2756 1.2822 1.2888 1.2954 Thallous thiosulphate. Ppt. SI. sol. in cold, easily sol. in hot H 2 O. Crookes.) Easily sol. in Na 2 S 2 O 3 +Aq. (Jochum.) 17 1.0919 34 1 . 1924 Tin thiosulphate (?). (Schiff, A. 113. 118.) Sol. in H 2 O. B.-pt. of Na 2 S 2 O 3 +Aq. P = pts. Na 2 S 2 O 3 to 100 pts. H 2 O. Uranyl thiosulphate, (UO 2 )S 2 O 3 . Ppt. (Faktor. C. C. 1901, II. 878.) B.-pt. 1 P B.-pt. p B.-pt. P 101 14 102 27 103 39 110 111 112 104 113 122 119 201 120 214.5 121 229 Zinc thiosulphate, ZnS 2 O 3 +zH 2 O. Very deliquescent, and very sol. in H 2 O and alcohol. (Rammelsberg.) 104 49 . 5 113 131.5 122 244 105 59 114 141.5 123 262 Zinc thiosulphate ammonia, ZnS 2 O 3 , 2NH 3 . 106 68 115 152 124 283 Decomp. by H 2 O. Sol. in NH 4 OH+Aq, 107 77 116 164 125 311 from which it is pptd. by alcohol. (Rammels- 108 86 117 175.75 126 348 berg, Pogg. 66. 62.) 109 95 118 188 (Gerlach, Z. anal. 26. 436.) Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) 100 pts. absolute ethyl alcohol dissolve at room temperature 2.5 mg. Na 2 S 2 O< (Bodtker, Z. phys. Ch. 1897, 22. 410.) 100 pts. absolute ethyl alcohol dissolve at room temperature 3.4 mg. Na 2 S 2 O 3 5H 2 O. (Bodtker, Z. phys. Ch. 1897, 22. 510.; Sol. in oil of turpentine (Edison, Am Chemist, 7. 127). Insol. therein (Techn J. B. 27. 1003). Insol. in ethyl acetate. (Casaseca, C. R 30. 821.) Decamp. H 2 O and alkalies. Stable in the air. (Muthmann, B. 1897, 30. 630.) Thkx&thiazyl ^'chloride, S 3 N 2 C1 2 . See Nitrogen sulphochloride. ThioZnthiazyl chloride, S 4 N 3 C1. See Nitrogen sulphochloride. Thio^nthiazyl iodide, N 3 S 4 I. Decomp. spontaneously in the air. unstable. (Muthmann, B. 1897, 30. Very 631.) THORIUM HYDRIDE 1071 ThioZnthiazyl nitrate, S 4 N 8 NO 8 . Sol. in H 2 O with decomp. Sol. in HNO 3 + Aq. (Demargay, C. R. 91. 1066.) Sol. in cold H 2 O with decomp. Completely insol. in organic solvents, as CS 2 , CHC1 3 , acetone, and acetic ether. (Muthmann and Seitter, B. 1897, 30. 629.) ThioZhthiazyl sulphate (S 4 N 8 )HSO 4 . Stable on air. Sol. in H 2 O with decomp. (Demarcay, C. R. 91. 854. 1066.) ThioJn'thiazyl sulphocyanide, N 3 S 4 CNS. Stable in the air. Sol. in benzene and chloroform. (Muth- mann and Seitter, B. 1897, 30. 631.) Dithiotefrathiazyl bichloride, S 6 N 4 C1 2 . See Nitrogen sulphochloride. Thorium, Th. Not oxidised by boiling H 2 O. Quickly sol. (Chydenius, Pogg. 119. 43), very slowly sol. by long boiling (Berzelius, Pogg. 16. 385) in HNO 3 +Aq. Insol. in cold, easily sol. in warm dil. H 2 SO 4 +Aq. Slowly sol. in cold, rapidly in hot HCl+Aq. Easily oxidised by aqua regia. Insol. in KOH+Aq or HF+Aq. ' SI. sol. in dil. H 2 SO 4 +Aq; decomp. by cone. H 2 SO 4 . Very si. sol. in dil., and less in cone. HNO 3 +Aq. Easily sol. in cone. HC1 + Aq, and aqua regia. (Nilson, B. 16. 2521.) Thorium B. Somewhat sol. in hot H 2 O, which dissolves 70% in an hour. More rapidly sol. in dil acids or hot KI-f-Aq. Somewhat sol. in organic solvents. Insol. in CS 2 and in methy lene iodide. (Hogley, Phil. Mag. 1913, (6 26. 331.) Thorium C. Somewhat sol. in hot H 2 O. More rapidly sol. in hot KI+Aq. and in dil. acids. More sol. in organic solvents than thorium B 20% sol. in CS 2 or methylene iodide in 1< minutes. (Hogley, Phil. Mag. 1913, (6) 25 331.) Thorium teZraboride, ThB 4 . Sol. in cold cone. HNO 3 and HC1 and in ho cone. H 2 SO 4 . (Jassonneix, C. R. 1905, 141 192.) Thorium fozaboride, ThBr 6 . Sol. in hot dil. or cone. HNO 3 ; insol. ic H 2 SO 4 , HC1, HF and aq. alkalies. (Jasson neix, C. R. 1905, 141. 193.) Thorium cfabromide, ThBr2. Sol. in H 2 O with partial decomp. (Troos and Ouvrard, A. ch. (6) 17. 227.) Thorium teirabromide, ThBr 4 . Sol. in H 2 O. (Berzelius.) Very hygroscopic, and sol. in H 2 O with artial decomp. (Troost and Ouvrard. A. h. (6) 17. 229.) SI. sol. in organic solvents. (Matthews, . Am. Chem. Soc. 1898, 20. 840.) +7H 2 O. Sol. in alcohol. (Rosenheim, B. 900, 33. 979.) +8H 2 O. Very sol. in alcohol and H 2 O. nsol. in chloroform and light petroleum. Lesinsky, Z. anorg. 1897, 15. 82.) Thorium feZrabromide ammonia, ThBr 4 , 3NH 3 . Insol. in organic solvents. (Matthews, J. Am. Chem. Soc. 1898, 20. 840.) Thorium carbide, ThC 2 . Almost insol. in cone, acids; decomp. by H 2 O and by dil. acids. (Moissan, C. R. 1896, 122. 577.) Thorium fefrachloride, ThCl 4 . Anhydrous. Extremely deliquescent, and sol. in H 2 O with evolution of heat. Sol. in alcohol. Sol. in ether. (Matthews. J. Am. Chem. Soc. 1898, 20. 824.) +7H 2 O. Deliquesces in the air. Very sol. in H 2 O and alcohol. Insol. in ether. (Kriiss, Z. anorg. 1897, 14. 368.) +8H 2 O. Hydroscopic. Easily sol. in H 2 O and absolute alcohol. Not pptd. from solution in alcohol by ether. +9H 2 O. As above. (Rosenheim, Z. anorg. 1903, 36. 426.) Thorium tefrachloride ammonia, ThCl 4 , 6NH 8 . Insol. in ether. Decomp. by H 2 0. ThCl 4 , 8NH 3 . Fumes in moist air. De- comp. by H 2 O. (Matthews, J.'Am. Chem. Soc. 1898, 20. 824.) The compds. of ThCl 4 with NH 3 are of the type ThCh, nNH 3 and may be classified into three groups. (1) n = 4, 6, 7, 12, 18. Compds. are de- comp. by H 2 O. (2) n =4, 6, 7. Compds. are not decomp. by H 2 O. (3) n = 6, 7, 12, 18. The first two compds. of this series are identical with the last two of group (2). ThCl 4 , 4NH 3 of group (2) is the only one in the whole series stable above 120. (Chauve- net, C. R. 1910, 151. 387.) Thorium fluoride, ThF 4 +4H 2 O. Insol. in H 2 O or HF+Aq. Thorium hydride, ThH 2 . Decomp. by dil. HCl+Aq. 24. 873.) (Winkler, B. 1072 THORIUM HYDROXIDE Thorium hydroxide, Th(OH) 4 . Insol. in H 2 O. Sol. in acids, except oxalic, molybdic, and hydrofluoric acids. Insol. in alkali hydroxides, but easily sol in alkali carbonates +Aq. More sol. in NH 4 OH+(NH 4 ) 2 CO 3 + Aq thanin (NH 4 ) 2 CO 3 +Aq. alone. (Berzelius.) Not pptd. in presence of tartaric and citric acids. (Chyde- nius, Pogg. 119. 43.) 4ThO 2 . H 2 O. Insol. in water and acids at boiling temp. Thorium hydroxybromide, Th(OH) 2 Br 2 + 11H 2 O. Sol. in alcohol. (Rosenheim, B. 1900, 33. 979.) Thorium hydroxychloride, (OH)ThCl 3 + 11H 2 O. Sol. in alcohol. (Rosenheim, B. 1900, 33. 978.) Th(OH) 2 Cl 2 +5H 2 O. Slowly takes up H 2 O from the air. Sol. in H 2 O without decomp. Sol. in alcohol. Pptd. from solution in alcohol by ether. (Rosenheim, Z. anorg. 1903, 36. 425.) +8H 2 0. Hydroscopic; sol. in alcohol. (Rosenheim, B. 1900, 33. 978.) Thorium hydroxyiodide, Th(OH)I 8 +10H 2 O. Evolves iodine in the light. (Rosenheim, Z. anorg. 1903, 35. 430.) Thorium iodide. Sol. in H 2 O. Thorium nitride, Th,N 4 . Decomp. by H 2 O. (Matignon, C. R. 1901, 132. 37.) Thorium oxide, ThO 2 . When ignited is insol. in HC1, and HNO 3 + Aq. Sol. in H 2 SO 4 by heating to boiling and subsequent addition of H 2 O. Insol. in alkali hydrates or carbonates +Aq. Thorium wetoxide, Th 3 6 +H 2 O. SI. sol. in HC1. (Locke, Z. anorg. 1894, 7. 348.) +2H 2 O. Loses 1 H 2 O at 100. Sol. in H 2 O; insol. in NH 4 OH+Aq. (Locke.) Metathorium oxide. Sol. in H 2 O after having been treated with cone. HNO 3 or HCl+Aq, even if previously ignited. ThO 2 ,zTh(OH) 4 . Compare Th 3 O 5 . (Locke) (Stevens, Z. anorg. 1901, 27. 42.) Thorium peroxide, Th 2 O 7 . Precipitate. (Cleve, C. R. 100. 605.) Thorium oxychloride. Decomp. by H 2 O into ThCl 4 and ThO 3 . ThOCla. Sol. inH 2 O. Insol. in abs. alcohol. (Matignon, A. ch. 1907, (8) 10. 133.) +3H 2 O. +5H 2 O. (Matignon, A. ch. 1907, (8) 10. 135.) Metothorium oxychloride, ThO 2 , zThC! 4 . Hydroscopic; sol. in H 2 O; insol. in abs. alcohol. (Stevens, Z. anorg. 1901, 27. 47.) Thorium oxyfluoride, ThOF 2 . Insol. in H 2 O. Sol. in H 2 SO 4 with decomp. (Chauvenet, C. R. 1908, 146. 974.) Thorium oxysulphide, ThS 2 , 2ThO 2 . (Chydenius.) Thorium phosphide. Insol.. in H 2 O. (Berzelius.) Thorium silicide, ThSi 2 . Sol. in aq. min. acids; insol. in aq. alkalies-. Decomp. by fusion with NaOH or KOH. (Honigschmid, C. R. 1906, 142. 158.) Thorium sulphide, ThS 2 . Insol. in warm H 2 SO 4 . Very slightly at- tacked by HNO 3 or HCl+Aq. Sol. in hot aqua regia. (Berzelius.) Thoromolybdic acid. Ammonium thoromolybdate, (NH 4 ) 8 Th(Mo 2 7 ) 6 +8H 2 0. Insol. in H 2 O; sol. in dil. acids. (Barbieri, C. A. 1913. 372*.) (NH 4 ) 6 H 2 Th(Mo 2 O 7 ) 6 +llH 2 O. Insol. in H 2 O; sol. in dil. acids. (Barbieri.) Silver thoromolybdate, Ag8Th(Mo 2 O 7 ) 6 . Insol. in H ? O; si. sol. in HNO 3 +Aq, but nearly insol. in presence of AgftO 3 . (Bar- bieri.) Sodium thoromolybdate, Na 8 Th(Mo 2 7 ) 6 + 15H 2 O. Insol. in H 2 O; sol. in dil. acids. (Barbieri.) Na6H 2 Th(Mo 2 O 7 ) 6 +17H 2 O. Insol. in H 2 0; sol. in dil. acids. (Barbieri.) Thulium, Tm. Thulium chloride, Tm 2 Cle+14H 2 0. Very sol. in H 2 O and in alcohol. (James, J. Am. Chem. Soc. 1911, 33. 1342.) Thulium hydroxide. Easily sol. in dil. acids. (James, J. Am. Chem. Soc. 1911, 33. 1342.) TIN BROMIDE, BASIC 1073 Thulium oxide, Tm 2 O 3 . Slowly sol. in hot cone, acids. (James, J. Am. Chem. Soc. 1911, 33. 1342.) Tin, Sn. Insol. in H 2 O. Tin is not atacked by dis- tilled H 2 O when air is passed through it for a week. Slowly sol. in dil. cold HCl+Aq, but rapidly sol. if hot and cone. Slowly sol. in hot dil. H2SO4+Aq, but decomp. by hot cone. H 2 SO 4 . Readily sol. in cold aqua regia. Attacked violently by cone. HNO 3 +Aq with pptn. of SnO 2 . Completely sol. in dil. cold HNO 3 + Aq (1 pt. HNO 3 : 1 pt. H 2 O) at 22. (Hay, C. N. 22. 298.) Not attacked by pure cone. HNO 3 +Aq of 1.512-1.419 sp. gr., but vio- lently attacked by less cone. acid. Also at- tacked by most cone, acid if it contains NO 2 . (Millon, A. ch. (3) 6. 95.) If Sn is placed in dil. HNO 3 +Aq of 1.15 sp. gr. it is si. dissolved, but soon pptd. again as SnO 2 . If a small amt. of NH 4 C1 is added, the Sn remains permanently in solution; HC1+ Aq has a similar action. (Ordway, Am. J. Sci. (2) 23. 220.) Easily sol. in the cold in mixture of 1 vol. H 2 SO 4 , 2 vols. HNO 3 , and 3 vols. H 2 O. (Basset, C. N. 63. 172.) HNOs+Aq containing less than 12% HNO 3 attacks Sn and forms a stannous salt, which decomposes, giving a turbid solution. HNO 3 +Aq (12-45% HNO 3 ) completely dissolves Sn, but solution becomes turbid on standing. HNO 3 +Aq containing more than 45% HNO 3 does not dissolve Sn, but forms a white sub- stance, which is sol. in H 2 O if over 70% acid is used; this solution soon becomes turbid. (Montemartini, Gazz. ch. it. 22. 384.) Sn dissolves in HNO 3 +Aq at low temps. (0-21). When very dil. HNO 3 +Aq (14% HNO 3 ) is used, the amount of stannous salt formed decreases only slightly with increase of temp, while with 30-40% acid it falls to zero at 21. (Walker, J. Soc. Chem. Ind. 1893. 845.) In presence of Fe, Cr or Al, HNO 8 +Aq acts on Sn to form soluble products, from which cone. HNO 3 ppts. all Sn as meta- stannic acid, (van Leent, C. C. 1899, 1. 101.) Much more sol. in acids when small quanti- ties of metallic salts have been added. This is most noticeable when PtCl 4 or tartar emetic is added to HCl+Aq. HCl+Aq with tartar emetic exerts 11 times, and with PtCl 4 13 times the action exhibited by pure acid. (Millon, C. R. 21. 47.) Sol. in 2N HClOs+Aq. (Hendrixson, J. Am. Chem. Soc. 1904, 26. 755.) Pyrosulphuric acid dissolves Sn on warm- ing. (Divers, Chem. Soc. 1885, 47. 639.) Hot telluric acid attacks Sn. (Hutchins, J. Am. Chem. Soc. 1905, 27. 1183.) Sn is attacked by 17% HN 3 +Aq. (Cur- tius and Rissom, J. pr. 1898, (2) 58. 299.) Sol. in a solution of Na in liquid NH 3 . (Kraus, J. Am. Chem. Soc. 1907, 29. 1562.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Sol. in boiling alum+Aq (1 pt. alum to 4 pts. H 2 0). Sol. in KHSO 3 , NH 4 C1 (1 :4), and K 2 C 4 H 4 O 6 +Aq. SI. sol. in KC 2 H 3 O 2 +Aq, but not at- tacked by MgSO 4 , K 2 SO 4 , KNO 3 , or Na 2 SO 4 +Aq. (Cludius, J. pr. 9. 161.) Sol. in alkalies +Aq. Attacked easily by cone. NaCl, KC1, or NH 4 NO 3 +Aq; not attacked by NH 4 Cl+Aq. (Hallock, Am. Ch. J. 6. 52.) Sol. in Fe(NO 3 ) 3 +Aq in presence of HNO 3 +Aq in proportion of 1 atom Sn to 1 atom Fe. (Lepez and Storch, W. A. B. 98, 2t>. 268.) Solubility in dil. saline solutions. 100 ccm. H 2 O containing 0.5 g. NaCl or KC1 dissolve 6 mg. Sn from 11.8 sq. cm. in one week when air without CO 2 is passed through the solution, but none at all when the air con- tains CO 2 . 100 ccm. H 2 O containing 1 g. NH 4 C1 dis- solve 5 mg. Sn under above conditions with- out CO 2 , and none with CO 2 . With 1 g. MgCl 2 , 1 mg. Sn was dissolved without CO 2 , and none wijth CO 2 . With 1 g. K 2 SO 4 , 2 mg. Sn were dissolved without CO 2 , and none with CO 2 . With 1 g. KNO 3 , 3 mg. Sn were dissolved without CO 2 , and 1 mg. with CO 2 . With 1 g. Na 2 C0 3 , 7 mg. Sn were dissolved without CO 2 . With 1 g. NaOH, 220 mg. Sn were dis- solved without CO 2 . CaO 2 H 2 +Aq did not dissolve. (Wagner, Dingl. 221. 260.) Not attacked by sugar +Aq. (Klein, C. R. 102. 1170.) % ccm. oleic acid dissolves 0.0134 g. Sn in 6 days. (Gates, J. phys. Chem. 1911, 15. 143.) Tin antimonide, SnSb. (Stead, J. Soc. Chem. Ind. 1897, 16. 205.) Tin arsenide, Sn 3 As 2 . (Stead, J. Soc. Chem. Ind. 1897, 16. 206.) Tin (stannous) bromide, SnBr 2 . Sol. in H 2 O. Sol. in pyridine. (Naumann, B. 1904, 37. 4609.) Mol. weight determined in pyridine and ethyl sulphide. (Werner, Z. anorg. 1897, 16. 23.) Tin (stannic) bromide, basic, SrBrOH+ 3H 2 0. Sol. in H 2 0. Decomp. in aq. solution when warmed. Sol. in ether, methyl alcohol, ethyl alcohol, acetone, acetic acid and esters of organic acids. Nearly insol. in benzene, ligroin and CHC1 3 . (Pfeiffer, Z. anorg. 1914, 87. 242.) 1074 TIN BROMIDE Tin (stannic) bromide, SnBr 4 . Deliquescent. Sol. in H 2 O without evolu- tion of heat. (Balard.) Decomp. by H 2 O much more quickly than SnCl 4 . (Lorenz, Z. anorg. 1895, 9. 378.) Easily sol. in AsBr 3 . (Walden, Z. anorg. 1902, 29. 374.); PC1 3 , PBr 3 and S 2 C1 2 . (Wal- den, Z. anorg. 1900, 26. 217.) Sol. in acetone. (Naumann, B. 1904, 37. 4328.) +4H 2 O. (Preis and Raymann, C. C. 1882. 773.) Stannic hydrogen bromide, SnBr 4 , 2HBr. See Bromostannic acid. Stannic bromide with MBr. See Bromostannate, M. Tin (stannic) bromochloride, SnClBr 3 . Fumes in moist air; decomp. by H 2 O. (Bes- son, C. R. 1897, 124. 685.) SnCl 2 Br 2 . Fumes in moist air. Decomp. by H 2 O. (Besson.) SnCl 3 Br. Fumes in moist air. Decomp. by H 2 O. (Besson.) Tin (stannic) bromoiodide, SnBr 2 I 2 . Sol. in cold H 2 O. Decomp. in aq. solution at 80. SnBr 3 I. SnBrI 3 . (Lenormand. C. C. 1899, II. 521 J. Pharm. 1899, 10. 114.') Tin (stannous) chloride, SnCl 2 , and +2H 2 O. Not deliquescent. 100 pts. H 2 O dissolve 83.9 pts. SnCl 2 at 0. (Engel, A. ch. (6) 17 347.) 100 pts. H 2 O dissolve 269.8 pts. SnCl 2 at 15, and sat. solution has sp. gr. 1.827 (Michel and Krafft, A. ch. (3) 41. 478.) Sol in a certain amount of H 2 O without decomp. but more H 2 O causes pptn. of SnO, SnCl 2 . SnCl 2 +Aq absorbs O from air. Melts in crystal H 2 O at 46. (Ordway. Sat. solution boils at 121.7. Sp. gr. of SnCl 2 +Aq at 15 containing: 5 10 15 20 % SnCl 2 +2H 2 1.0331 1.0684 1.1050 1.1442 25 30 35 40 % SnCl 2 +2H 2 O 1.1855 1.2300 1.2779 1.3298 45 50 55 60 % SnCl 2 +2H 2 O 1.3850 1.4451 1.5106 1.5823 65 70 75 % SnCl 2 +2H 2 0. 1.6598 1.7452 1.8399 (Gerlach, Dingl. 186. 131.) SnCl 2 HCl Sum of Sp. gr. of solu- jj 2 O 2 equiv. tion 74 74 .532 8.33 66.7 6.6 73.3 .489 8.35 63.75 13.54 77.29 .472 8.198 68.4 24.8 93.2 .524 7.869 81.2 34.9 116.1 .625 7 . 305 94.2 40.0 134.2 .724 6.880 117.6 44 161.6 1.883 6.108 147.6 49.4 197.0 2.114 5.387 156.4 66 222.4 2.190 4.715 157 78 235 2.199 4.309 Solubility of SnCl 2 in HCl+Aq. SnCL Yz molecules SnCl 2 in milligrammes in 10 com. solution; HC1 = molecules HC1 in milligrammes in ditto; H 2 O = amt. H 2 O present in grammes. (Engel, A. ch. (6) 17. 347.) Solubility is thus diminished by HCl+Aq, while there are less than 8-10 mols. HC1 for mol. SnCl 2 . When that limit is passed the solubility rapidly increases. (Engel.) Sol. in very dil. HC1 or tartaric acid +Aq. Sol. in KOH+Aq. Sol. in cone. SnOCl 2 +Aq. (Gerlach.) Sol. in NH 4 Cl+Aq. Anhydrous SnCl 2 is partially sol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Sol. in absolute alcohol. Insol. in oil of turpentine. 11.41 pts. SnCl 2 are sol. in 100 pts. ether at 0. 11.38 pts. SnCl 2 are sol. in 100 pts. ether at 16. . 11.38 pts. SnCl 2 are sol. in 100 pts. ether at 35.5. (Laszczynski, B. 1894, 27. 2286.) Anhydrous SnCl 2 is sol. in ether. (de Jong, Z. anal. 1902, 41. 596.) 1 g. anhydrous SnCl 2 is sol. in 1.8 g. acetone at 18. Sp. gr. of sat. solution 18 /4 = 1.6. (Naumann, B. 1904, 37. 4336.) Sol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Anhydrous SnCl 2 is sol. in methyl acetate to the extent of 15.7%. (Schroder and Steiner, J. pr. 1909, (2) 79. 63.) 31.20 pts. SnCl 2 +2H 2 O are sol. in 100 pts. ethyl acetate at 2. 35.53 pts. SnCl 2 +2H 2 O are sol., in 100 pts. ethyl acetate at +22. 73.44 pts. SnCl 2 +2H 2 O are sol. in 100 pts. ethyl acetate at 82. (Laszczynski, B. 1894, 27. 2286.) 1 pt. anhydrous SnCl 2 is sol. in 22.40 pts. ethyl acetate at 18. D18/4 =0.9215. (Naumann, B. 1910, 43. 319.) Insol. in ethyl amine (Shinn, J. phys. Ch. 1907, 11. 538); pyridine (Naumann, B. 1904, 37. 4609): benzonitrile (Naumann, B. 1914, 47. 1369.) TIN CHLORIDE 1075 Insol. in CS. (Arctowski, Z. anorg. 1894 6. 257.) Sol. in urethane. (Castoro, Z. anorg. 1899 20. 61.) Mol. weight determined in pyridine am ethyl sulphide. (Werner, Z. anorg. 1897 15. 22.) . Tin (stannic) chloride, basic, SnCl 3 OH+3H 2 O Hydroscopic. Sol. in H 2 O. Sol. in ether, alcohol, acetone, acetic acid Nearly insol. in ligroin and benzene. (Pfeiffer Z. anorg, 1914, 87. 241.) Tin (stannic) chloride, SnCl 4 . (a) Ordinary modification. Deliquescent Sol. in H 2 O. On diluting SnCl 4 +Aq and boiling, SnO 2 separates out. SnCl 4 +Aq is not pptd. by HNO 3 , HC1, or H 2 SO 4 +Aq H 3 PO 4 +Aq ppts. in a few days, and H 3 AsO 4 + Aq in a short time. No ppt. is formed by K 2 SO 4 , Na 2 SO 4 , KC1, NaCl, NH 4 C1, KNOl etc. + Aq. Sol. in S 2 C1 2 . (Walden, Z. anorg. 1900, 25. 217.) Easily sol. in PC1 3 and PBr 3 . (Walden, Z. anorg. 1900, 25. 211.) Very sol. in liquid NH 3 . (Gore, Am. Ch. J. 1899, 20. 830.) Very sol. in absolute alcohol, from which it is pptd. by H 2 O. Easily sol. in ether; de- comp. by oil of turpentine. Miscible with CS 2 and Br 2 . Sol. in acetone. (Naumann, B. 1904, 37. 4328.) Sol. in acetone and in methylal. (Eid- mann, C. C. 1899, II. 1014.) Sol. in ethyl acetone. (Naumann, B. 1904, 37. 3601.) Distribution of SnCl 4 between H 2 O and xylene. n = pts. by wt. of Cl in 100 pts. of H 2 O layer. m = pts. by wt. of Cl in 100 pts. of xylene layer. k = partition coefficient. 50 cc. xylene+60 g. SnCl 4 .5H 2 O. n m k SnCl 4 +5H 2 O Sp. gr. SnCU +5H 2 Sp. gr. SnCU +5H 2 Sp. gr. 66 40.35 0.08 504.4 80 QQ QK 175 228 5 2 1.012 34 1.226 66 .538 97.5 40.24 0.33 122.1 4 1.024 36 00 1.242 1 OCQ 68 .563 jro'r 111 40.27 0.68 59.3 8 .048 OO 40 1.276 72 .614 (Smirnoff, Z. phys. Ch. 1907, 68. 377.) 10 059 42 1.293 74 .641 12 .072 44 1.310 76 .669 50 cc. xylene+60 g. SnCl 4 .4H 2 O. 14 .084 46 1.329 78 1.698 16 .097 48 1.347 80 1.727 t 18 20 22 .110 .124 .137 50 52 54 1.366 1.386 1.406 82 84 86 1.759 1.791 1.824 66 80 100 41.905 41.915 41 845 0.925 1.555 2 515 45.3 27.0 16 7 24 26 1.151 1.165 56 58 .426 .447 88 90 1.859 1.894 111 41.68 3.235 12.9 28 1.180 60 .468 92 1.932 (Smirnoff.) 30 1.195 62 .491 94 1.969 32 1.210 64 .514 95 1.988 50 cc. xylene+60 g. SnCl 4 .3H 2 O. (Gerlach, Dingl. 178. 49.) t n m k Sp. gr. of SnCl 4 +Aq. 80 43.205 9.95 4-4 Deg. Baum6 % Sn Deg. Baum6 % Sn Deg. Baum % Sn 94 100 42 . 545 42.645 .325 10.56 .6 5.1 111 42 31 10.03 4.2 65.7 65 29.45 29.12 55 54 24.47 24.02 34 33 14.90 14.45 (Smirnoff.) 64 63 62 28.64 28.17 27.70 53 52 51 23.56 23.11 22.65 32 31 30 14.00 13.56 13.11 +2H 2 O. Sol. inH 2 O. +3H 2 O. Tr. pt. 83. (Meyerhoffer, Bull. 61 60 59 58 57 56 27.24 26.77 26.30 25.84 25.38 24.93 50 49 48 47 46 22.20 21.74 21.29 20.83 20.38 29 28 27 26 25 12.67 12.23 11.79 11.35 10.91 oc. 1891 (3) 6, 85.) +4H 2 O. Tr. pt. 63. (Meyerhoffer.) +5H 2 O. Very deliquescent, and sol. in [ 2 O. Decomp. by alcohol. Sol. in HCl+Aq. Tr. pt. 56. (Meyerhoffer.) +8H 2 O. More deliquescent than the 5H 2 alt. Tr. pt. 19. (Meyerhoffer.) (Heermann, Ch. Z. 1907, 31. 680.) +9H 2 (Nollner, Z. Ch. 1865. 45.) 1076 TIN HYDROGEN CHLORIDE (6) Metastannic chloride. Sol. in cold H 2 O; solution coagulates on boiling. Cone. HC1+ Aq ppts. from SnQ 4 +Aq. When solution does not contain HC1, the addition of HC1 + Aq causes a ppt., which dissolves in H 5 O. HNO 3 , and H 2 SO 4 +Aq also ppt. K 2 SO 4 , Na 2 SO 4 , and NaCl+Aq produce ppts,. insol. in H 2 O, but sol. in HCl+Aq. NH 4 C1 or KCl+Aq do not ppt. KNO 3 +Aq ppts. slowly. (Rose.) Tin (stannous) hydrogen chloride, SnCl 2 , HC1+3H 2 0. Decomp. by H 2 O. Melts at -25. (Engel, C. R. 106. 1398.) Tin (stannic) hydrogen chloride. See Chlorostannic acid. - n Tin (stannous) hydrazine chloride, SnCl 2 , 2N 2 H 4 , HC1. Very hydroscopic. Sol. in H 2 O and abs. alcohol. (Curtius. J. pr. 1894, (2) 60. 341.) Tin (stannic) chloride with MCI. See Chlorostannate, M. Tin (stannous) chloride ammonia, SnCl 2 , NH 3 . (Berzelius.) SnCl 2 , 4NH 3 . Ppt. (Naumann. B. 1904, 37. 4336.) Tin (stannic) chloride ammonia, SnCL, 2NH 3 . Sol. in cold H 2 O without decomp., but decomposes by heating. Tin (stannous) chloride arsenate. See Arsenate chloride, stannous. Tin (stannic) chloride cyanhydric acid. SnCL, 2HCN. Decomp. on moist air or with H 2 O. (Klein. A. 74. 85.) Tin (stannous) chloride hydrazine, SnCl 2 2N 2 H 4 . Decomp. by H 2 O. Insol. in NH 4 OH+Aq. (Franzen, Z anorg. 1908, 60. 286.) Tin (stannic) chloride nitrogen sulphide SnCl 4 , 2N 4 S 4 . Insol. in most solvents. Decomp. by warm NH 4 OH+Aq. Decomposes in the air. (Wolbling, Z anorg. 1908, 67. 284.) Decomp. by H 2 O. (Davis, Chem. Soc 1906, 89. 1576.) Tin (stannic) chloride phosphine, 3SnCl 4 , 2PH 3 . Decomp. by H 2 O. (Rose, Pogg. 24. 159.) Tin (stannous) chloride potassium stannous sulphate. See Sulphate, potassium stannous stannous chloride. Tin (stannic) chloride sulphur teZrachloride, SnCl 4 , 2SC1 4 . Very hygroscopic. Sol. in CHC1 3 , ligroin, petroleum ether, CS 2 , POC1 3 ; very sol. in completely dry absolute ether, in benzene, acetacetic ester and in SC1 2 . (Ruff, B. 1904, 37. 4517.) Tin (stannic) chloride sulphide, 2SnCl 4 , SnS 2 . See Stannic sulphochloride. Tin (stannic) chlorobromide, SnClBr 3 . Decomp. by H 2 O. (Ladenburg, A. suppl. 8. 60.) SnCl 2 Br 2 . Decomp. by H 2 O. (Laden- burg.) Tin (stannous) chloroiodide, SnClI. Decomp. immediately by H 2 O. (Henry, Phil. Trans. 1845. 363.) Tin (stannic) chloroiodide, SrCl 2 l2. Fumes in the air. Decomp. by H 2 O. (Lenormand, J. Pharm. 1898. 8.) SnClIa. (Lenormand, J. Pharm. 1899, 10. 114.) Tin (stannous) fluoride, SnF 2 . Easily sol. in H 2 O. (Berzelius, Pogg.; 1. 34.) Tin (stannic) fluoride, SnF 4 . Very hydroscopic. Sol. in H 2 O. Slowly decomp. in aq. solu- tion with separation of Sn0 2 . (Ruff, B. 1904, 37. 681.) Tin (stannic) fluoride with MF. See Fluostannate, M. Tin (stannous) hydroxide, 2SnO, H 2 O. Decomp. to SnO when boiled with H 2 O. More easily sol. in acids than Sn or SnO. Sol. in NaOH, and KOH+Aq, even when dil. Insol. or very si. sol. in NH 4 OH, (NH 4 ) 2 CO 3 , and K 2 CO 3 +Aq; sol. in cold CaO 2 H 2 , and BaO 2 H 2 with decomposition on boiling. (Fremy, A. ch. (3) 12. 460.) Only si. sol. in NH 4 Cl+Aq hot or cold. (Brett.) SI. sol. in NaC 2 H 3 O 2 +Aq. (Mercer.) TIN IODIDE 1077 Solubility in NaOH+Aq. G. Na in 20 ccm. G. Sn in 20 ccm. 0.2480 0.3680 0.6394 0.8326 0.9661 2.1234 0.1904 0.2614 0.4304 0.5560 . 0.7849 1.8934 (Rubenbauer, Z. anorg. 1002, 30. 335.) Not pptd. in presence of Na citrate. (Spiller.) Sol. in water-glass +Aq. (Ordway.) SnO 2 H 2 . Solubility in 1 1. H 2 O = 0.0000135 g. mol. at 25. (Goldschmidt, Z. phys. Ch. 1906, 66. 389.) Tin hydroxide, SnO, 6SnO 2 +5H 2 O. +9H 2 O. (Schiff, A. 120. 153. Tin sesg^uhydroxide, Sn 2 O 3 , xH 2 O. Insol. in H 2 O. Sol. in NH 4 OH+Aq. (Fuchs, J. pr. 6. 318.) Tin (stannic) hydroxide. "a" modification. Obtained by pptn. by alkali in stannic chloride solution. Freshly pptd. substance when air dried contains 73.5% H 2 O; when dried over H 2 SO 4 or in a vaccum for 1 month 12.6% H 2 O. Heated to glowing loses all H 2 O and passes into the anhydride. The "a" form is capable of existing in all degrees of hydration. (Lorenz, Z. anorg. 1895, 9. 372-375.) "a" stannic hydrate is a white amor- phous substance which is very sol. in HNO 3 when moist; sol. in H 2 SO 4 even dil.; sol. in HC1 and not pptd. by an excess. Very sol. in NaOH+Aq. and is not pptd. by an excess. A solution of a stannic acid in HC1 is iden- tical with a solution of freshly prepared aque- ous stannic chloride and gives no ppt. with dil. HC1, H 2 Sp 4 , HNO 3 or arsenic acid even on long standing;. " ft " modification. Obtained by oxiding and dissolving Sn hi HNO 3 , and from solution of sodium stannate by pptn. Freshly pptd. from HNO 3 when air dried contains 21.3% H 2 O, and when dried over H 2 SO 4 or in a vacuum 11.3%, corre- sponding to Sn(OH) 4 and SnO (OH) 2 respec- tively. Freshly pptd. from sodium stannate solu- tion and air dried contains 22.5% H 2 O and when dried over H 2 SO 4 or in a vacuum con- tains 12.1%, corresponding to Sn(OH) 4 and SnO (OH) 2 . Passes into the anhydride when heated to glowing. The "/3" form is capable of existing in all degrees of hydration. It is a white amor- phous substance which is insol. in HN0 3 ; in- sol in H 2 SO 4 even when cone.; insol. in HC1 changed by contact with the acid in ;hat when the acid has been removed the ppt. is readily sol. in H 2 O, though pptd. again from solution by addition of HC1. hen freshly prepared the "ft" form is sol. n NaOH+Aq. but is pptd. by an excess of NaOH. A solution of "ft" stannic acid in HC1 be- haves quite differently from an aq. solution of stannic chloride in that it ppts. metas- tannic sulphate when treated with H 2 SO 4 . This ppt. dissolves when heated with dilute HNO 3 or HC1, but the solution on standing spontaneously forms another ppt. A solution of "ft" stannic acid in HC1 gives a ppt. when treated with arsenic acid. (Lorenz, Z. anorg. 1895, 9. 372.) See also Stannic acid. Tin hydroxyl chloride, SnO(OH)Cl. See Chlorostannic acid. Tin (stannous) iodide, SnI 2 , and +2H 2 O. SI. sol. in cold, more abundantly in hot H 2 O, without decomp. Solubility in H 2 O. t Pts. SnI 2 in 100 pts. solution t Pts. SnI 2 in 100 pts. solution 98.5 3.43 97.3 3.70 84.9 3.05 87.4 3.24 73.9 2.56 77.6 2.75 60.1 2.09 67.5 2.34 51.5 1.79 59.7 2.03 41.0 1.50 49.5 1.72 30.5 1.21 39.4 1.38 20.8 1.03 29.6 1.11 19.8 0.96 (Young, J. Am. Chem. Soc. 1897, 19. 846.) Solubility of SnI 2 in HI+Aq at t. Pts. SnI 2 per 100 pts. solvent. t 20 30 40 50 60 70 80 90 100 ^M SSw ^ S3 0> ? o*-* ^M 2 ? 1 s > SB X s i i w 0.98 1.16 1.40 1.69 2.07 2.48 2.95 3.46 4.03 0.20 0.23 0.33 0.46 0.66 0.91 1.23 1.65 2.23 0.60 0.64 0.71 0.82 1.11 1.37 1.83 2.40 3.63 1.81 1.81 1.90 2.12 2.51 2.92 3.70 4.58 5.82 4.20 4.06 4.12 4.34 4.78 5.43 6.38 7.82 9.60 10.86 10.28 10.06 10.35 11.03 11.97 13.30 15.52 25.31 23.46 23.15 23.76 24.64 25.72 27.23 29.84 34.05 (Young, J. Am. Chem. Soc.fl897, 19. 851.) 1078 TIN OXIDE Solubility of SnI 2 at low temp, in 29.95% Solubility in organic solvents at t. HI+Aq. G. Snl4 in 100 Sp gr of the Temp. Pts. in 100 pts. solution Pts. in 100 pts. solvent Solvent t g. of the sat. solution sat. solution 1.5 1.5 6.0 10.5 12.96 13.15 12.35 11.01 14.89 15.14 14.09 12.36 CC1 4 CC1 4 CHC1 3 C 6 H 6 22.4 50.0 28.0 20.2 5.25 12.50 8.21 12.65 1.59 1.63 1.50 0.95 15.2 24.8 10.48 9.36 11.70 10.33 (McDermott, J. Am. Chem. Soc. 1911, 33. 1964) 30.7 8.78 9.62 04 o o 70 9 50 40 3 9 51 10.50 Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) (Young, J. Am. Chem. Soc. 1897, 19. 854.) Solubility of SnI 2 at low temp, in 39.6% HI+Aq. Temp. Pts. in 100 pts. of solution Pts. in 100 pts. of solvent I II 5.7 10.5 15.7 20.3 13.52 16.44 19.47 23.56 25.50 13.56 16.37 19.60 23.68 25.60 15.66 19.71 24.27 30.92 34.30 (Young, J. Am. Chem. Soc. 1897, 19. 852- 853.) Sol. in SnCl 2 +Aq. Sol. in warm alkali chlorides or iodides + Aq; also in dil. HC1+ Aq. Very si. sol. in CHC1 3 , CS 2 , or C 6 H 6 . (Personne, C. R. 54. 216.) Sol.inKOH+Aq. (Rose.) Sol. in acetone. (Naumann, B. 1904, -37. 4328.) Tin (stannic) iodide, SnI 4 . Decomp. by H 2 O into SnO 2 and HI. Very sol. in PC1 3 . (Beckmann, Z. anorg. 1906, 51. 110.) Sol. in POC1 3 , (Walden, Z. anorg. 1900, 25.212.). Easily sol. in PC1 3 and PBr 3 . (Walden, Z. anorg. 1900, 25. 211.) Sol. in liquid AsBr 3 forming a solution with sp. gr. =3.731 at 1. (Retgers, Z. phys. Ch. 1893, 11. 342.) Sol. in SOC1 2 , S 2 C1 2 and SO 2 C1 2 . (Walden, Z. anorg. 1900, 26. 215.) Sol. in SnCl 4 . (Walden.) Sol. in anhydrous alcohol, ether, and benzene. 1 pt. CS 2 dissolves .1.45 pts. SnI 4 at ordinary temp. (Schneider, Pogg. 127. 624.) 100 pts. methylene iodide, CH 2 I 2f dissolve 22.9- pts-. -Sftlr a4- 10-. -Sfh- gr^-ef solution = 3.481. (Retgers, Z. anorg. 3. 343.) (Eidman, C. C. 1899, 'Ut7, ' Sol. in acetone. II. 1014.) Solubility in CS 2 . 100 g. of the sat. solution contain at: 58 84 89 94 114.5 16.27 10.22 9.68 10.65 9.41 g. SnI 4 . (Arctowski, Z. anorg. 1896, 11. 274.) Sol. in allyl mustard oil. ph ys : Ch. 1905, 9. 647.) (Mathews, J. Tin (stannous) hydrogen iodide, SnI 2 , HI. Not obtained in pure- state. (Young, J. Am. Chem. Soc. 1897, 19. 856.) Tin (stannous) iodide ammonia) SnI 2 , 2NH 3 . (Ephraim and Schmidt, B. 1909, 42. 3857.) SnI 4 , 8NH 3 . (Ephraim and Schmidt.) Tin (stannic) iodide ammonia, SnI 4 , 3NH 3 . (Personne, C. R. 54. 218:) SnI 4 , 4NH 3 . (Personne.) SnI 4 , 8NH 3 . (Rammelsberg, Pogg. 48. 169.) Tin iodosulphide, See Tin sulphoidide. Tin monoxide (Stannous oxide), SnO. Insol. in H 2 O. Sol. in acids. Very si. sol. in boiling NH 4 Cl+Aq. (Rose.) Insol. in NaOH or KOH+Aq. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Insol. in acetone. (Naumann, B. 1904, 37. 4329.) Tin dioxide (Stannic oxide), SnO 2 . Insol. in H 2 O or cone, acids except cone H 2 SO 4 . Insol. in cone, alkalies or NH 4 OH+ Aq. Not absolutely insol. in dil. HNO 3 +Aq. (Mulder.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Mia. Cassiterite (Tin ^tone). Not attacked by acids. TIN SULPHIDE 1079 Tin sesquioxide, Sn 2 O 3 . While moist, easily sol. in NH 4 OH+Aq. SI. sol. in dil., more easily in cone. HCl+Aq. (Berzelius.) Tin (stannic) oxybromide, Sn 3 Br 6 O + 12H 2 O. Decomp. by H 2 O into SnBr 2 and H 2 SnO 3 . Sn 3 Br 8 O 2 . As above. (Preis and Ray- mann, C. C. 1882. 773.) Tin (stannic) oxybromide nitrogen pent- oxide, SnO 2 , 3Br 2 , N 2 O 6 . Decomp. by H 2 O. (Thomas, C. R. 1896, 122. 33.) Tin (stannous) oxychloride, SnO, SnCl 2 + 3H 2 O. Insol. in H 2 O. Sol. in HC1, HC 2 H 3 O 2 , and dil. HNO 3 , or H 2 SO 4 +Aq. (J. Davy, Schw. J. 10. 325.) Sn 8 Cli 4 O 8 + 10H 2 O. Easily sol. in H 2 O or alcohol. Can be recrystallized from alcohol but not from H 2 O. (Tschermak, W. A. B. 44. 2. 736.) 3SnO 2 , 2SnCl 2 +6H 2 O. Very si. sol. in H 2 O. Sol. in dil. acids. (Ditte, A. ch. 1882, (5) 27. 146.) 4SnO, SnCl 2 +6H 2 O. (Ditte.) Tin (stannic) oxychloride, SnO 2 , SnCl 4 . Sol. in H 2 O. (Scheurer-Kestner, A. ch. (3) 47. 6.) ' Tin (raetostannic) oxychloride, 3SnO 2 , SnCl 4 +3H 2 O. Sol. in little, decomp. by much H 2 O. (Weber, Pogg. 122.368.) 4SnO 2 , SnCl 4 +7H 2 O. (Weber.) "Metastannyl chloride ft," Sn 6 O 9 Cl 2 . De- liquescent. Sol. without decomp. in a small amount of H 2 O or in a large amount of H 2 O containing a few drops HC1. Sol., in abs. alcohol. (Engel, C. R. 1897, 124. 767.) +4H 2 O and +9H 2 O. Sol. in H 2 O acidified with one drop of HC1. Pptd. by excess HC1. (Engel, C. R. 1897, 124. 768.) "Pamstannyl chloride," Sn 6 O 9 Cl 2 +2H 2 0. Decomp. by excess H 2 O. Sol. in H 2 O; pptd. by HC1. (Engel, C. R. 1897, 126. 465.) Tin (stannic) oxychloride nitrogen pent- oxide, SnOCl 2 , 3SnCl 4 , N 2 O 6 . Hydroscopic; sol. in H 2 O. Decomp. by heat. (Thomas, C. R. 1896, 122. 32.) Tin (stannous) oxyiodide, SnO, 3SnI 2 2SnO, 3SnI 2 ; SnO, SnI 2 ; and 2SnO, SnI 2 . Decomp. by much H 2 O. (Personne, C. R 54. 216.) Tin oxysulphide, Sn 2 S 3 O+llH 2 0. Very sol. in (NH 4 ) 2 CO 3 +Aq; slowly sol. n H 2 0. (Schmidt, B. 1894, 27. 2739.) Tin phosphide, Sn 2 P. (Ragg, C. C. 1898, II. 170.) SnP. Sol. in HCl+Aq. Insol. in HNO 3 +Aq. SnP 2 . Not attacked by HC1. Easily at- tacked by aqua regia. (Emmerling, B. 1879. 12. 155.) SnP 3 . Insol. in HC1. Slowly attacked by dil. HNO 3 at 50. Oxidized by fuming HNO> with ignition. (Jolibois, C. R. 1909, 148. 638.) Sn 3 P 2 . Insol. in mercury. Decomp. by HC1. (Stead, J. Soc. Chem. Ind. 1897, 16. 206.) Sn 4 P 3 . Attacked by HC1, HNO 3 and al- kalies. (Jobilois, C. R. 1909, 148. 637.) The only true compounds are Sn 4 P 3 and SnP 3 . (Jolibois, C. R. 1909, 148. 637.) Tin phosphochloride, Sn 3 P 2 Cl. (Mahn, Jena. Zeit. 5. 1660.) Tin (stannous) selenide, SnSe. Decomp. by boiling HCl+Aq. Slowly oxidised by boiling HNO 3 +Aq, and easily dissolved in aqua regia (Schneider, Pogg. 127. 624.) Easily sol. in alkalies +Aq (Uelsmann, A. 116. 122), or scarcely even on boiling (Schneider), according to method of preparation. Sol. in alkali sulphides or selenides +Aq. Tin (stannic) selenide, SnSe 2 . Not attacked by H 2 O or dil. acids; scarcely attacked by boiling cone. HCl+Aq; gradu- ally decomp. by hot HNO 3 +Aq; easily dis- solved by warm aqua regia, and hot cone. H 2 S0 4 . Sol. in cold, more easily in warm KOH, NaOH, or NH 4 OH+Aq. (Uelsmann, A. 116. 122.) Tin (stannous) sulphide, SnS. 1 1. H 2 O dissolves 0.14X10- 6 mols. SnS at 18. (Weigel, Z. phys. Ch. 1907, 68. 294.) Insol. in dil., sol. in cone. HCl+Aq. SI. sol. in hot cone. HNO 3 +Aq. Insol. in KOH +Aq. +H 2 O. Insol. in H 2 O, H 2 S+Aq, or dil. acids; sol. with decomp. in cone, acids; easily sol. in hot cone. HCl+Aq. Insol. in H 2 SO 3 +Aq. Insol. in NH 4 OH+Aq. Insol. in NH 4 C1, or NH 4 NO 3 +Aq. Scarcely sol. in (NH 4 ) 2 S+Aq, but easily sol. in the same on addition of S. (Rose.) 10% NaOH+Aq dissolves SnS by violent boiling. Insol. in cold, si. sol. in hot Na 2 SO 3 +Aq. (Materne, C. C. 1906, II. 557.) Sol. in alkali polysulphides+Aq. Insol. in acetone. (Eidmann, C. C. 1899, 1080 TIN SULPHIDE II. 1014); (Naumann, B. 1904, 37. 4329.); ethyl acetate. (Naumann, B. 1910, 43. 314.) Tin (stannic) sulphide, SnS 2 . Anhydrous. (Mosaic gold.) Insol. in HC1 or HNO 3 +Aq, but decomp. by aqua regia. Sol. in hot KOH+Aq or K 2 CO 3 +Aq; also in hot K 2 S, Na 2 S+Aq, and (NH 4 ) 2 S+Aq. 1 1. H 2 O dissolves 1.13X10- 6 mols. SnS 2 at 18. (Weigel, Z. phys. Ch. 1907, 58. 294.) +zH 2 O. SI. sol. in NH 4 OH+Aq, but readily in KOH, KssS, or Na 2 S+Aq; also in hot cone. HCl+Aq. Decomp. by hot HNO 3 +Aq. Insol. in KHSOa+Aq. Sol. in K 2 GO 3 +Aq. Insol. in NH 4 C1, and NH 4 NO 3 +Aq. (Brett.) Pptd. SnS 2 is insol. in cold, sol. in hot Na 2 B 4 O 7 +Aq. Sol. in Na 2 CO 3 +Aq. Very sol. in NaOH+Aq. (Materne, C. C. 1906, II. 557.) Sol. in boiling cone. H 2 C 2 O 4 +Aq. (Clarke, C. N. 21. 124.) Insol. in methyl acetate (Naumann, B. 1909, 42. -3790); ethyl acetate (Naumann, B. 1910, 43. 314.); acetone (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Tin sesg-w'sulphide, Sn 2 S 3 . Sol. in moderately cone. HC1. (Antony and Niccoli, Gazz. eh. it. 1892, 22. (2) 408.) Tin sulphochloride, SnS 2 , 2SnCl 4 . H 2 O dissolves out SnCl 4 . (Dumas, Schw. J. 66. 409.) SnS 2 Cli 2 = SnCl 4 , 2SC1 4 . Sol. in H 2 O with separation of S. Gradually sol. in dil. HNO 3 +Aq. Sol. in POC1 3 . (Casselmann, A. 83. 267.) Tin sulphoiodide, SnS 2 l4. Decomp. by H 2 O into SnO 2 , S, and HI; by cold cone. HCl+Aq with separation of S, also by aqua regia, and HNO 3 +Aq. Cold KOH+Aq separates S and SnO 2 . Completely sol. in hot KOH+Aq. Sol. in cold, more easily in hot CS 2 or CHC1 3 . Decomp. by alcohol. (Schneider, Fogg. III. 249.) Tin sulphophosphide, Sn 3 P 2 S. Insol. in HC1, HNO 3 and aqua regia. Sol. in aq. alkali hydroxides, containing C1 2 or Br 2 in solution. (Granger, C. R. 1896, 122. 322.) Tin (stannous) telluride, SnTe. Not attacked by cone. HCl+Aq. (Ditte, C. R. 97. 42.) Titanic acid, TiO 2 , xH 2 O. a-Titanic add. Insol. in H 2 O or alcohol. When dried in the cold, is completely sol. in acids, especially HC1, or dil. H 2 SO 4 +Aq, but when the solution in acids is boiled, it is con- verted into /3- titanic acid. Very si. sol. even when moist in H 2 SO 3 +Aq. (Berthier.) SI. sol. in alkali carbonates +Aq. A complete solution in an alkali carbonate +Aq can only be obtained by adding a Ti salt drop by drop to the alkaline solution, and allowing the ppt. to dissolve entirely before adding more Ti salt. On boiling the solution in (NH 4 ) 2 CO 3 +Aq (or in K 2 CO 3 or Na a CO 3 +Aq with NH 4 C1) the titanic acid is pptd. Relatively easily sol. in mineral acids, de- creasing in the following order HC1, HNO 3 , H 2 SO 4 . Insol. in perchloric acid. (Lan- decker, Z. anorg. 1909, 64. 67.) Sol. in dil. H 2 SO 4 . 40 g. H 2 O + 70 g. H 2 SO 4 (sp. gr. 1.145) dissolves 0.33 g. TiO 2 in 15 min. (Hall and Smith, Proc. Am. Phil. Soc. 1905, 44. 193.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) p-Titanic acid, Metatitanic acid. Insol. in H 2 O, acids except HF, or alkali hydrates or carbonates +Aq. When digested with cone. H 2 SO 4 until acid is evaporated, the residue is sol. in H 2 O. (Berzelius.) y-Titanic acid. Sol. in pure H 2 O, but /3-acid is pptd. by boiling. (Knop, A. 123 351.) Colloidal TiO 2 :rH 2 O+Aq has been pre- pared by Graham (Chem. Soc. 17. 325.) Barium titanate, 2BaO, 3TiO 2 . (Bourgeois, C. R. 103. 141.) Barium pertitanate peroxide. See Pertitanate, barium peroxide. Calcium titanate, CaTiO 8 . (Ebelmen, C. R. 32. 711.) Min. Perofskite. Scarcely attacked by HC1 +Aq or other acids, except hot H 2 SO 4 , which decomposes it. CaO, 2TiO 2 . Min. Tilanomorphite. Par- tially decomp. by HCl+Aq, completely by H 2 SO 4 . Cobaltous titanate, CoTi0 3 . (Bourgeois, C. C. 1893, I. 226.) Ferrous ortfotitanate, Fe 2 TiO 4 . (Hautefeuille, C. R. 69. 733.) Ferroferric titanate, FeTiO 3 , zFe 2 O 3 . Min. Menaccanite. Very si. sol. in HC1 or aqua regia with separation of TiO 2 . Ferric titanate. Not attacked by boiling H 2 SO 4 or cone. HCl+Aq. (Wohler and Liebig, Pogg. 21. 578.) TITANIUM CHLORIDE 1081 Magnesium titanate, MgTiO 3 . Insol. in H 2 O and acids. (Hautefeuille, A. ch. (4) 4. 169.) Min. Geikielile. When finely powdered, is easily sol. in hot HC1, or in cold HF in a few hours. (Dick, Miner, Mag. 1894, 10. 146.) Mg 2 TiO4. Slowly decomp. by boiling with HNO 3 +Aq. (Hautefeuille, A. ch. (4) 4. 169.) Potassium titanate, K 2 TiO|. Anhydrous. Decomp. with H 2 O. +4H 2 O. Deliquescent. Very sol. in H 2 O. Precipitated from aqueous solution by alcohol. (Demoly, Compt. chim. 1849. 325.) Potassium titanate, acid, K 2 O, 3TiO 2 +2H 2 O Insol. in H 2 O. (Demoly.) K 2 O, 6TiO 2 +2H 2 O. (Demoly.) K 2 O, 3TiO 2 +3H 2 O. Insol. in H 2 O. Com- pletely sol. in HCl+Aq if only cold H 2 O is used for washing. When heated to 100, no longer completely sol. in HCl+Aq. (Rose, Fogg. 74. 563.) K 2 O, 12TiO 2 . (Rose, Gilb. Ann. 73. 78.) Sodium titanate, Na 2 TiO 3 . Anhydrous. Decomp. by H 2 O into NaOH, and an acid titanate, insol. in H 2 O. +4H 2 O. Deliquescent. Very sol. in H 2 O. Precipitated from aqueous solution by alcohol (Demoly.) Sodium titanate, acid, 2Na 2 O, 9TiO 2 +5H 2 O If not heated to 100, is sol. in cold HC1+ Aq. (Rose, Gilb. Ann. 73. 78.) 2Na 2 O, 3TiO 2 . Insol. in H 2 O; slowly sol in cold, easily in hot HCl+Aq. (Cormim- bceuf, C. R. 115. 823.) Na 2 O, 2TiO 2 . As above. (C.) Na 2 O, 3TiO 2 . Insol. in H 2 O, and nearly so in boiling HCl+Aq. (C.) Strontium titanate, 2SrO, 3TiO 2 . (Bourgeois, C. R. 103. 141.) Zinc titanate, ZnO, TiO 2 (?). (Uvy, A. ch. (6) 24. 456.) 2ZnO, TiO 2 (?). '(L4vy.) 3ZnO, 2TiO 2 . Slowly attacked by warn H 2 SO 4 or HNO 3 +Aq, and by H 2 SO 4 +HF Wholly sol. in cold HCl+Aq. (Le"vy.) - 4ZnO, 5TiO 2 . Not attacked by cold cone acids, but sol. by boiling except in HCl+Aq (Levy.) ZnO, 3TiO 2 . Insol. in H 2 O, alcohol, o ether. Dil. HNO 3 , H ? SO 4 , or HCl+Aq do not attack even on boiling; boiling H 2 SO 4 dis solves with difficulty; not attacked by cone boiling alkalies +Aq. (L6vy, A. ch. (6) 26 471.) Pertitanic acid. See Pertitanic acid. Itanium, Ti. Decomp. H 2 O even under 100 (Wohler); lot attacked by H 2 O under 500. (Kern, C. N. 3. 57). Does not decomp. H 2 O at 100. Schneider, Z. anorg. 1894, 8. 85.) Sol. in HCl+Aq if warmed. Rapiclly sol. n HF+Aq. Sol. in cold dil. H 2 SO 4 +Aq, HNO 3 +Aq, or HC 2 H 3 O 2 +Aq. Dissolves almost instantaneously in HF+Aq. (Merz.) Sol. in molten lead and iron; sol. in HC1, HNO 3 and aqua regia. (Moissan, C. R. 1895, 120. 293.) Amorphous. Loses its spontaneous in- lammability when left for a time in contact with H 2 O. (Schneider, Z. anorg. 1895, 8. 85.) Titanium amide, Ti(NH 2 ) 4 . Violently attacked by H 2 O. (Stahler, B. 1905, 38. 2629.) Titanium fribromide, TiBr 3 +6H 2 O. Very hydroscopic. (Stahler, B. 1904, 37. 4409.) Titanium teJrabromide, TiBr 4 . Deliquescent. Decomp. by H 2 O. (Duppa, R. 42. 352.) Sol. in absolute alcohol and in dry ether. (Rosenheim and Schiitte, Z. anorg. 1900, 24. 238.) Titanium bromonitride, TiNBr. Decomp. by a small amount of H 2 O. On addition of more H 2 O, a part dissolves form- ing a solution which decomp. on warming with separation of titanic acid. It behaves similarly toward dil. HNO 3 , dil. HC1 and dil. H 2 SO 4 . Completely sol. in warm dil. H 2 SO 4 . (Ruff, B. 1908, 41. 2262.) Titanium carbide, TiC. Sol. in HNO 3 +Aq. (Shinier, C. N. 66. 71.) Insol. in HC1. Slowly sol. in aqua regia. (Moissan, C. R. 1895, 120. 295.) Titanium carbide nitride, Ti 10 C 2 N 8 =Ti(CN) 2 , 3Ti 3 N 2 . Insol. in, and not attacked by boiling HNO S or H 2 SO 4 (Wollaston), but sol. in HNO 3 +HF (Berzelius) . Titanium bichloride, TiCl 2 . Very deliquescent. Decomposes H 2 O with violence. Insol. in ether, CS 2 , or CHC1 3 . Decomp. by 99.5% alcohol. Titanium trichloride, TiCl 8 . Deliquescent. Sol. in H 2 O with evolution of heat. +4H 2 O. (Glatzel, B. 9. 1829.) +6H 2 O. Very sol. in H 2 O. (Polidori, Z. anorg. 1898, 19/307.) 1082 TITANIUM CHLORIDE Titanium tefrachloride, TiCl 4 . Anhydrous. Sol. in H 2 O with evolution of much heat. +5H 2 O. Deliquescent. Titanium sulphuryl chloride, TiCl 4 SO 3 = TiCl 3 OSO 2 Cl. Deliquesces gradually in moist air. (Claus- nitzer, B. 11. 2011.) Titanium chloride ammonia, TiCl 4 , 4NH 3 . Deliquescent. Solution in H 2 O is not quite clear. (Rose.) According to Persoz (A. ch. 46. 315), is TiCU, 6NH 3 . TiCl 4 , 6NH 3 and TiCl 4 , 4NH 3 . Both compds. are unstable in moist air; insol. in ether. (Rosenheim, Z. ahorg. 1901, 26. 245.) TiCl 4 , 8NH 3 . Violently decomp. by H 2 O. (Stabler, B. 1905, 38. 2627.) Titanium te/rachloride cyanobromide, TiCl 3 , NCClBr. (Schneider, Z. anorg. 1894, 8. 92.) Titanium chloride cyanhydric acid, TiCl 4 , 2HCN. Deliquescent. Sol. in H 2 O with evolution of heat. (Woliler, A. 73. 226.) Titanium bichloride nitrogen sulphide. 2TiCl 3 , N 4 S 4 . Decomp. rapidly in air. (Davis, Chem. Soc. 1906, 89. (2) 1576.) Titanium te^rachloride nitrogen sulphide, TiCl 4 , N 4 S 4 . Hydroscopic. Decomp. by H 2 O, HNO 3 , HC1, KO& and alcohol. (Wolbling, Z. anorg. 1908, 57. 282.) Titanium chloride phosphine. Decomp. by H 2 O, HCl+Aq, KOH+Aq, K 2 CO 3 +Aq, or (NH 4 ) 2 CO 3 +Aq. (Rose.) Titanium trichloride phosphoryl chloride, TiCl 4 , 2POC1 3 . '(Ruff, B. 1903,36. 1783.) Titanium chloronitridej TiNCl. Decomp. by small amount cold H 2 O. On the addition of more H 2 O it is only partially decomp. v For complete solution, the addition of dil. HC1 or a mixture of warm dil. H 2 SO 4 1 and HF is necessary. Easily sol. in cone. HNO 3 and in cone. H 2 SO 4 . (Ruff, B. 1908, 41. 2259.) Titanium cfofluoride. . (Hautefeuille, C. R. 67. 151.) Probably sesquiftuoride. Titanium ses4 and HF. When less strongly ignited (by heating ortho or metatitanic acid to 700) it is easily sol therein. (Bornemann and Schirrmeister C. C. 1910, II. 1870.) Ignited TiO 2 is very difficultly sol. in HF (Pennington, J. Am. Chem. Soc. 1896, 18 56 ) The solubility of ignited TiO 2 in H 2 SO is helped by H 2 O 2 . (Weiss and Landecker Z.anorg. 1909,64.71.) The solubility in H 2 SO 4 is increased addition of H 2 O 2 . H 2 O 2 brings TiO 2 quickly and completely into solution in the presenc of NH 4 OH, NH 4 C1, NaOH, Na 2 CO 3 am Na 2 HPO 4 . (Weiss and Landecker, m anorg 1909,64.71.) Insol. in liquid NH 3 . (Gore, Am. Ch. , 1898, 20. 830.) Crystalline. Min. Rutile, Brookite, an Anatase. Solubility as above. See also Titanic acid. itanium oxide, Ti 3 O 5 . (Deville, C. R. 53. 163.) True formula is Ti 7 O ]2 . (v. der Pfordten, L 237. 201.) Titanium peroxide, TiO 3 . Sol. in acids. Solution in H 2 SO 4 is very table, but the HC1 solution decomposes very asily. (Weber, B. 16. 2599; Piccini, B. 15. !221; Classen, B. 21. 370.) Titanium oxychloride, TiO 2 , TiOCl 2 +8H 2 O. Sol. in much H 2 O. (Merz, Bull. Soc. 1867. 401.) Ti 2 O 2 Cl 2 . Insol. in H 2 O. Sol. in NH 4 OH + A.q with separation of TiO 2 . See also Titanium hydroxychloride. Titanium oxyfluoride. Insol. in H 2 O. (Berzelius.) Titanium oxyfluoride with MF. See Fluoxypertitanate, M. Titanium phosphide, TiP. SI. sol. in boiling aqua regia. Insol. in dil. or cone, acids and alkalies. SI. attacked by fuming HNO 3 in sealed tube at 250-300 6 . (Gewecke, A. 1908, 361. 84.) Titanium phosphochloride. See Phosphorus titanium chloride. Titanium silicide, TiSi 2 . Sol. in HF; insol. in other n?in. acids. Slowly sol. in 10% KOH+Aq. (Honig- schmid, C. R, 1906, 143. 226.) Titanium wonosulphide, TiS. Insol. in alkalies. Difficultly sol. in nitric acid and aqua regia. Insol. in HF. (v. der Pfordten, A. 234. 257.) Titanium bisulphide, TiS 2 . Decomp. slowly on moist air. Insol. in HC1 or dil. H 2 SO 4 +Aq. (Ebelmen.) Sol. in aqua regia or HNO 3 +Aq. Decomp. by KOH+Aq or NaOH+Aq. Insol. in KSH+Aq. (Rose.) Sol. in HF at 100. (v. der Pfordten, A. 234. 257.) Titanium sesgwisulphide, Ti 2 S 3 . Insol. in caustic alkalies +Aq. Sol. in HF at a high temp. Insol. in aqua regia. (v. der Pfordten, A. 234. 257.> Titanomolybdic acid, TiO 2 , 12Mo0 3 +22H 2 O. Very sol. in H 2 O. Sol. in ether. (Pechard, C. ft* 1893, 117. 790.) 1084 TITANOMOLYBDATE, AMMONIUM Ammonium titanomolybdate, 2(NH 4 ) 2 O, TiO 2 , 12MoO 3 +10H 2 O. Sol. in H 2 O and acids; completely insol. in solutions of ammonium salts. (Pechard.) Potassium titanomolybdate, 2K 2 O, TiO 2 , 12Mo0 3 +16H 2 O. Efflorescent. Sol. in H 2 O. (Pechard.) Titanodfdtungstic acid, H 8 TiWi O 3 6+ zH 2 0. (Lecarme, Bull. Soc. (2) 36. 17.) Titanotungstic acid or TitaTioduodeci- tungstic acid, H 8 TiW 12 O 42 +zH 2 O (Lecarme, Bull. Soc. (2) 36. 17.) Titanous acid. Sodium titanite, Na 3 TiO 3 = 3Na 2 O, Ti 2 3 . Sol. in dil. acids. (Koenig and v. der Pfordten, B. 22. 2075.) Titanyl compounds. See Titanium oxy- compounds. Triamine cobaltic compounds. See Dichrocobaltic compounds. Trithionic acid, H 2 S 3 O 6 . Known only in aqueous solution. Solution in H 2 O gradually decomposes in the cold, rapidly at 80. Not decomp. if very dilute or in presence of acids, except HNO 3 , HC1O 3 , and HIO 3 . (Fordos and Gelis, A. ch. (3) 28. 451.) Trithionates. The trithionates are all sol. in H 2 O, and very easily decomposed. Ammonium trithionate, (NH 4 ) 2 S 3 O 6 . Very deliquescent and unstable. Very sol. in H 2 O. Insol. in abs. alcohol. (Divers and Ogawa, Chem. Soc. 1900, 77. 337.) Barium trithionate, BaS 3 O 6 +2H 2 O. Very sol. in H 2 O. Precipitated from aqueous solution by large excess of alcohol. Aqueous solution is very unstable. (Kessler Pogg. 74. 250.) Lead trithionate, PbS 3 O 6 . Very si. sol. in H 2 O. Sol. in Na 2 S 2 O 3 +Aq (Fogh, C. R. HO. 524.) Potassium trithionate, K 2 S 3 O 6 . Sol. in H 2 O. Insol. in alcohol. (Kessler, Pogg. 74. 270.) Sol. in H 2 O with decomp. Insol. in alcohol. (Langlois, A. 1841, 40. 102.) Sodium trithionate, Na 2 S 3 O 6 . Very sol. in H 2 O. +3H 2 O. (Villiers, C. R. 106. 1356.) Thallous trithionate, T1 2 S 3 O 6 . Sol. in H 2 O. (Bevan, C. N . 38. 294.) Zinc trithionate. Sol. in H 2 O, but decomposes upon warming the solution. (Fordos and Gelis, C. R. 16. 1070.) Tungsten, W. Metallic. Not attacked by heating with fuming HNO 3 , aqua regia. or other acids, or by boiling KOH + Aq. Sol. in KOH + Aq and NaClO+Aq. (v. Uslar, A. 94. 255.) Not easily acted upon by moist air, if no CO 2 present. Sol. in a mixture of HF and HNO 3 . Very slowly sol. in H 2 SO 4 , HC1 and HF. (Moissan, C. R. 1896, 123. 15.) Very slowly attacked by HNO 3 , H 2 SO 4 , HC1 and even CrO 3 . A mixture of CrO 3 and H 2 SO 4 dissolved 1.67 g. in 16 hrs. from a fine wire and 1.36 g. in 14 hours. (Fink, Met. Chem. Eng. 1910, 8. 341.) Compact tungsten is not attacked by dil., and only si. dissolved by cone. H 2 SO 4 . Not attacked by dil. or cone. HC1. HNO 3 and HNO 3 +HC1 attack slowly by long heating, forming thin layer of WO 3 . Slowlv sol. in HNO 3 +HF. (Weiss, Z. anorg. 1910, 65. 339.) Aluminothermic tungsten is insol. in acids and in aqua regia. Sol. in fused KOH. (Stavenhagen, B. 1899, 32. 1515.) Insol. in HC1 of any concentration at room temp, and only very si. sol. at 110. After being in contact with hot cone. HC1 (sp. gr. 1.15) for 175 hrs. the metal lost 0.5% of its weight. SI. sol. in dil. HC1 at 110. Insol. in cone. H 2 SO 4 at room temp, and in dil. H 2 SO 4 at 110 J . Somewhat sol. in cone. H 2 S0 4 at high temp. Insol. in cone. HNO 3 , and hot or cold HF. SI. sol. in aqua regia. Very sol. in HF+HNO 3 . (Ruder, J. Am. Chem. Soc. 1912, 34. 387.) Insol. in aqua regia and acids; sol. in fused KOH. (Stavenhagen, B. 1899, 32. 1514.) Insol. in KOH-f-Aq. Sol. in fused KOH. Slowly sol. in fused Na 2 CO 3 , K 2 CO 3 or mixture of the two. Somewhat sol. in NaOCl+Aq. (Ruder, J. Am. Chem. Soc. 1912, 34. 388.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, .20. 830.) Crystalline. Insol. in H 2 O, HC1, or H 2 SO 4 . Oxidised by HNO 3 or aqua regia. (D'Elhu- jar.) Sol. in boiling KOH+Aq. (Riche, A. ch. (3) 50. 5.) Amorphous. Easily oxidised by HNO 3 + Aq. (Zettnow.) Tungsten amide. See Tungsten nitride. TUNGSTEN IODIDE 1085 Tungsten arsenide, WAs 2 . Insol. in H 2 O and other solvents. Not attacked by boiling HF or HNO 3 . Sol. in cold HF+HNO 3 and in hot aqua regia. Not attacked by hot KOH+Aq or NaOH+Aq. Decomp. by fused KOH or NaOH. (De- facqz, C. R. 1901, 132. 139.) Tungsten boride, WB 2 . Slowly attacked by cone, acids; vigorously attacked by aqua regia. (Tucker and Moody. Chem. Soc. 1902, 81. 16.) Tungsten ^'bromide, WBr 2 . Partly sol. in H 2 O, the rest decomposing to W0 2 and HBr. Tungsten pentdbromide, WBr 5 . Decomp. by moist air or H 2 O. Sol. in caustic alkalies +Aq. Very hydroscopic. Fumes in the air. Decomp. by H 2 O. Sol. in HF, or cone. HC1. SI. sol. in fuming HBr. Decomp. by dil. HC1, cone. HNO 3 or dil. H 2 SO 4 . Readily attacked by fused alkalies or alkalies +Aq. Sol. in CC1 4 , CHC1 3 , CHBr 3 , abs. alcohol, ether, essence of tere- benthine and benzene. (Defacqz, C R 1899, 128. 1232.) Tungsten /lezabromide, WBr 6 . Decomp. by H 2 O and in the air. Sol. in NH 4 OH+Aq. (Smith, J. Am. Chem. Soc. 1897, 18. 1100.) Tungsten bromochloride, WC1 6 , WBr 6 . Decomp. by H 2 O. Sol. in HF. Decomp. by HNO 3 or H 2 SO 4 . Violently attacked by fused alkali or alkali +Aq. Sol. in most organic solvents. WC1 6 , 3WBr 6 . Properties like those of WC1 6 , WBr 6 . (Defacqz, C. R. 1899, 129. 516.) Decomp. by H 2 O. Sol. in 40% HF+Aq. 22 B. HC1 +Aq gives a si. ppt. of WO 3 . Decomp. by HNO 3 and by H 2 SO 4 . Sol. in abs. alcohol, ether, CS 2 , C 6 H 6 and glycerine. Sol. in CC1 4 only on warming. Nearly insol. in oil of turpentine. (Defacqz.) Tungsten bronze. See Tungstate Tungstate slum. Tungstate Tungstate slum. Tungstate Tungstate Tungstate slum. Tungstate Tungstate tungsten oxide, barium, tungsten oxide, barium potas- tungsten oxide, barium sodium, tungsten oxide, calcium potas- tungsten oxide, calcium sodium, tungsten oxide, lithium, tungsten oxide, lithium potas- tungsten oxide, potassium, tungsten oxide, potassium so- Tungstate tungsten oxide, potassium stron- tium. Tungstate tungsten oxide, sodium. Tungstate tungsten oxide, sodium stron- tium, Tungsten carbide, W 2 C. Sol. in boiling HNO 3 ; very slowly acted upon by other acids. (Moissan, C. R. 1896, 123. 16.) WC. Insol. in dil. acids; only si. sol. in H 2 SO 4 and cone. HNO 3 ; sol. in fused KC1O 3 and KNO 3 . (Williams, C. R. 198, 126. 1724.) Tungsten bichloride, WC1 2 . Decomp. on the air or with H 2 O. (Roscoe.) Tungsten fefrachloride, WC1 4 . Deliquescent. Partly sol. in H 2 O, with sub- sequent decomposition. (Roscoe.) Tungsten pentachloride, WC1 6 . Very deliquescent. Decomp. with H 2 O with hissing and evolution of heat and separa- tion of W 2 O 5 . Very si. sol. in CS 2 . (Roscoe.) Tungsten Aermchloride, WC1 6 . Not decomp. by moist air or H 2 O. De- comp. by alcohol. Very sol. in CS 2 . (Ros- coe.) Easily sol. in PGC1 3 . (Teclu, A. 187. 255.) Tungsten chloride nitrogen sulphide, WC14, (Davis, Chem. Soc. 1906, 89. (2) 1575.) Tungsten chloroarsenide, W 2 AsCl 9 . Hydroscopic; decomp. by H 2 Q and acids; sol. in aq. solution of alkalies; insol. in an- hydrous organic solvents. (Defacqz, C. R. 1901, 132. 139.) Tungsten chlorosulphide, W 2 S 7 C1 8 . Decomp. by H 2 O. Sol. in S 2 C1 2 . (Smith and Oberholtzer, Z. anorg. 1894, 5. 68.) WC1 C , 3WS 3 . Decomp. by H 2 O. Insol. in CS 2 , alcohol and C 6 H 6 . (Defacqz, A. ch. 1901, (7) 22. 266.) Tungsten /z&rafluoride, WF fl . Fumes in the air. Decomp. by H 2 O. Easily sol. in aq. alkalies. (Ruff, B. 1905, 38. 747.) Tungsten duodide, WI 2 . Not decomp. by H 2 O. (Roscoe, A. 162. 366.) Insol. in H 2 O, CS 2 and alcohol. Decomp. by boiling H 2 O, HNO 3 , H 2 SO 4 and aqua regia; sol. in fused KOH, and alkali carbon- ates. (Defacqz, C. R. 1898, 126. 936.) 1086 TUNGSTEN IODIDE Tungsten Zdraiodide, WI 4 . Insol. in H 2 O, ether, chloroform and tur- pentine; sol. in abs. alcohol; decomp. when boiled with H 2 O; sol. with decomp. in dil. HC1 and H 2 SO 4 , in HNO 3 and aqua regia, and in alkali hydroxides and carbonates fused or in aq. solution. (Defacqz, C. R. 1898, 127. 511.) Tritungsten nitride, W 3 N 2 . (Uhrlaub.) W 2 N 3 . Insol. in HNO 3 , dil. H 2 SO 4 and NaOH+Aq. (Rideal, Chem. Soc. 1889, 55. 44.) Tungsten nitride amide, W 3 N 6 H4 W(NH 2 ) 2 . Not attacked by acids or caustic alkalies + Aq. (Wohler, A. '73. 191.) Tungsten nitride amide oxide, W 7 N 8 H 4 O 4 = 3WN 2 , W 2 (NH 2 ) 2 , 2WO 3 . Not attacked by acids or alkalies. (Woh- ler.) Tungsten worzoxide, WO. Insol. in H 2 O. Not attacked by HC1, HF, H 2 SO 4 , or KOH+Aq. HNO 3 +Aq or aqua regia convert it into WO 3 . (Headden, Sill. Am. J. 146. 280.) Tungsten dioxide, WO 2 . (a) When prepared in the dry way, is at- tacked only by aqua regia, which oxidises to WO 3 . (6) When moist, is sol. in HC1 or H 2 SO 4 + Aq, also in KOH+Aq. Insol. in NH 4 OH+ Aq. (Riche, A. ch. (3) 60. 5.) Cryst. Insol. in HC1, H 2 SO 4 and cone. aq. alkalies; sol. in HNO 3 . (Hallopeau, C. R. 1898, 127. 135.) Tungsten oxide, blue. W 2 O 6 (Riche, A. ch. (3) 60. 33); W 3 O 8 (v. Uslar); W 4 O n (Gmelin). All are probably the same substance. Not attacked by boiling HNO 3 or aqua regia. Slowly sol. in boiling KOH+Aq. Tungsten inoxide, WO 3 . Insol. in H 2 O or acids. SI. sol. in dil. KOH +Aq, NaOH+Aq, Na 2 CO 3 +Aq, or H 2 CO 3 + Aq, but easily sol. in cone, boiling solutions of same. NH 4 OH+Aq when boiling has a solvent action. Insol. in cone, and dil. H 2 SO 4 . (Desi J Am. Chem. Soc. 1897, 19. 214.) Min. Tungstite. Insol. in acids. Sol. in NH 4 OH+Aq. Tungsten oxide, W 2 O 8 . Sol. in alkalies. (Desi, J. Am. Chem. Soc. 1897, 19. 214.) W 3 O 8 . Insol. in acids and alkalies. (Desi, J Am. Chem. Soc. 1897, 19. 228.) +H 2 O. Like W 5 O 14 +H 2 O. (Allen and Gottschalk, Am. Ch. J. 1902, 27. 336.) W 4 O 3 . (Desi, J. Am. Chem. Soc. 1897, 19. 219.) W 5 O 9 . (Desi.) W 5 Oi 4 +H 2 O. Insol. in H 2 O containing a little HC1. Slowly attacked by cold, cone. MOH+Aq. (Allen 'and Gottschalk, Am. Ch. J. 1902, 27. 333.) Tungsten tfn'oxide ammonia, WO 3 , 3NH 3 . (Rosenheim and Jacobsohn, Z. anorg. 1906, 50. 306.) Tungsten oxybromide, etc. See Tungstyl bromide, etc. Tungsten rao/iophosphide, WP. Not attacked by HF or HC1. Sol. in warm HNO 3 +HF. Slowly attached by hot HNO 3 . Not attacked by KOH+Aq or NaOH+Aq. (Defacqz, C. R. 1901, 132. 34.) Tungsten efo'phosphide, WP 2 . Insol. in H 2 O and in most organic solvents; insol. in HC1 and HF; sol. in a mixture of HF and HNO 3 in the cold, and in aqua regia on warming. (Defacqz, C. R. 1900, 130. 916.) Tungsten phosphide, W 4 P 2 . Not attacked by any acid, not even by aqua regia. (Wohler and Wright, A. 79. 244.) W 3 P 4 . (Wohler and Wright.) Tungsten cfo'selenide, WSe 2 . (Uelsmann.) Tungsten iriselenide, WSe 3 . Easily sol. in alkali sulphides or selenides +Aq. (Uelsmann, Jahrb. f. Ch. 1860. 92.) Tungsten silicide. Sol. in HF. Only very si. sol. in other acids. (Warren, C. N. 1898, 78. 319.) WSi 2 . Not attacked by ordinary acids and scarcely by warm aqua regia, but violently attacked by HNO 3 +HF. SI. attacked by 10% alkalies +Aq. (Honigschmid, M. 1907, 28. 1017.) Not attacked by dil. or cone. HC1, HF, HNO 3 or H 2 SO 4 , nor by not aqua regia. . Attacked by HNO 3 +HF or by fused alkalies. (Defacqz, C. R. 1907, 144. 850.) WSi 3 . Violently attacked by HNO 3 +HF. Not attacked by HNO 3 , H 2 SO 4 , HC1 or HF. (Frilley, Rev. Me*t. 1911, 8. 509.) W 2 Si 3 . Insol. in acids including HF; sol. in a mixture of HF and HNO 3 ; sol. in fused alkali hydroxides and carbonates. (Vigour- oux, C. R. 1898, 127. 394.) TUNGSTATE,. ALUMINUM AMMONIUM 1087 Tungsten ^sulphide, WS 2 . Oxidised by HNO 3 +Aq. (Berzelius.) Insol. in min. acids. Sol. in a mixture of HF and HNO 3 and in fused alkalies and alkali carbonates. (De- facqz, C. R. 1899, 128. 611.) Tungsten Znsulphide, WS 3 . Somewhat sol-, in cold, abundantly in hot H 2 O, but separated out by the addition of salts, especially NH 4 C1, or acids. Sol. in alkali sulphides, and hydrosulphides+Aq. Sol in caustic alkalies, and alkali carbonates +Aq. Slowly sol. in NH 4 OH+Aq in the cold. Tungstic acid, H 2 WO 4 . Insol. in H 2 O. Sol. in HF. Insol. in tung- states +Aq. 44.7% H 2 WO 4 is sol. in 50% HF+Aq at 25. 55.3% H 2 WO 4 is sol. in 50% HF +Aq at 50. 100 g. sat. H 2 WO 4 +HCl+Aq contain 0.68 g. H 2 WO 4 at 80. 9.8 % H 2 WO 4 is sol. in sat. alcoholic HC1 at 75. Insol. in alcoholic solutions of HBr and HI. (Rosenheim, Chem. Soc. 1911,. 100. (2) 402.) Freshly pptd. tungstic acid dissolves in H 2 O 2 . (KeUner, Dissert. 1909.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) H 4 WO 5 . Precipitate. SI. sol. in H 2 O and aqueous solutions of the tungstates. Sol. in 250-300 p'ts. H 2 O. When freshly pptd., sol. in alkali hydrates or carbonates +Aq. (An- thon, J. pr. 9. 6.) Metatungstic acid, H 2 W 4 O 18 +9H 2 O. Sol. in H 2 O. Solution may be boiled and evaporated to a syrupy consistency, when it suddenly gelatinises and ordinary tungstic acid is precipitated. Sol. in H 2 0. When heated to 50, it be- comes insol. in H 2 O. (SobolefT, Z. anorg. 1896, 12. 28.) Solubility in H 2 O at t. t 100 ccm. ether dissolve g. of the cryst. acid 7.8 18.2 24.3 83.456 88.389 99.66 110.76 t 100 ccm. H 2 O dis- solve g. of the cryst. acid Sp. gr. of the solution 22 43.5 41.46 88.57 111.87 1.6025 2.5239 3.6503 (Soboleff.) Sp. gr. of solution of metatungstic acid at 17.5 containing: 2.79 12.68 27.61 43.75% WO 8 . 1.0257 1.1275 1.3274 1.6343 (Scheibler, J. pr. 83. 273.) Sp. gr. of aqueous solution calculated by M = Mendelejeff, and G = (Gerlach (Z. anal. 27. 300), containing: 5 10 15 20 25% W0 3 , M 1.047 1.098 1.153 1.214 1.285 G 1.0469 1.0980 1.1544 1.2172 1.2873 30 35 40 45 50% W0. M 1.366 1.458 1.555 1.581 (?) G 1.3660 1.4540 1.5527 1.6630 1.7860 Solubility in ether at t. (Soboleff, Z. anorg. 1896, 12. 32.) Colloidal. Sol. in H 2 O. Not precipitated by acids or alcohol. Can be evaporated to dryriess and heated to 200, and still remains sol. in H 2 O. Sol. in J^pt. of H 2 O. Sp. gr. of aqueous solution containing: 5 20 50 66.5 79.8% WO,. 1.0475 1.2168 1.8001 2.596 3.243 (Graham, Chem. Soc. 17. 318.) Perhaps paratungstic acid, Hi Wi 2 O 4 i. (Klein, Bull Soc. (2) 36. 547.) Tungstates. Few normal tungstates are sol. in H 2 O, even some of the K and NH 4 salts are very si. sol. Most of the metatungstates, however, are easily sol. in H 2 O. Tungstates insol. in H 2 O are usually insol. in dil. acids. Aluminum tungstate, Al 2 (WO 4 ) 8 -f 8H 2 O. Precipitate. Insol. in H 2 O and Na 2 WO 4 + Aq. Sol. in (NH 4 ) 2 Al 2 (SO 4 ) 4 +Aq, NaOH + Aq, NH 4 OH+ Aq. Easily sol. in H 3 PO 4 , H 2 C 2 O 4 , and H 2 C 4 H 4 O 6 +Aq. (Lotz, A. 83. 65.) Sol. in 1500 pts. H 2 O at 15. (Lefort, C. R. 87. 748.) Al 2 O a , 4WO 3 +9H 2 O. Sol. in 400 pts. H 2 O at 15. (Lefort, C. R. 87. 748.) A1 2 O 3 , 5WO 3 +6H 2 O. Sol. in H 2 O, from which it is pptd. by alcohol. (Lefort.) Formula according to Lefort is A1 2 O 3) 3WO 8 +3H 2 0, 2W0 3 . See also Aluminicotungstic acid. Aluminum paratungstate, 5A1 2 O 3 , 36WO-f 46H 2 0=A1 2 3 , 7W0 8 +9H 2 (?). Easily sol. in an alum solution. (Lotz, A. 83. 65.) Aluminum ammonium tungstate, 3(NH 4 ) 2 O, A1 2 O 8 , 9WO 8 +4H 2 O. Sol. in cone. HNO 3 and in cone. HC1. (Balke and Smith, J. Am. Chem. Soc. 1903, 25. 1230.) 1088 TUNGSTATE, ALUMINUM AMM.ONIUM ANTIMONY Aluminum ammonium antimony tungstate. See Aluminicoantimoniotungstate, ammon- ium. Aluminum antimony tungstate. See Aluminicoantimoniotungstic acid. Aluminum zinc tungstate. A1 2 O 3 , ZnO, 9WO 8 +20H 2 0. Very sol. in H 2 O. (Daniels, J. Am. Chem. Soc. 1908, 30. 1850.) 2A1 2 O 8 , 3ZnO, 18WO 3 + 16H 2 O. Sol. in much H 2 O. Sol. in very dil. mineral acids or in acetic acid. (Daniels.) Ammonium tungstate, (NH 4 ) 2 WO 4 . Known only in solution. (NH 4 ) 4 W 3 9n+3H 2 O = 2(NH 4 ) 2 O, 3WO 3 -f- 3H 2 O. Sol. in H 2 O with decomp. Decomp. on air with evolution of NH 3 , and formation of paratungstate. Sol. in NH 4 OH+Aq. (Marignac, A. ch. (3) 69. 23.) (NH 4 ) 4 W 6 17 +5H 2 = 2(NH 4 ) 2 0, 5WO.+ 5H 2 O. Sol. at ordinary temp, in 26-29 pts. H 2 O with partial decomposition. (Marignac.) +2y 2 K 2 0, +3H 2 0, +4H 2 0, +4^H 2 O, and +5H 2 O. (Pinagel, Dissert, 1904.) (NH 4 ) 6 W 3 27 +8H 2 = 3(NH 4 ) 2 0, 8WO 3 -f 8H 2 O. Sol. in H 2 O. (Marignac.) Colloidal. (NH 4 ) 2 O, 6WO 3 +4 or 6H 2 O. Miscible with water in nearly all propor- tions. (Taylor, J. Am. Chem. Soc. 1902, 24. 632.) Ammonium raetatungstate, (NH 4 ) 2 W 4 Oi 8 . +6H 2 O. (Marignac, A. ch. (4) 3. 74.) +8H 2 O. Efflorescent. Very sol. in H 2 O. 1 pt. dissolves at 15 in 0.84 pt. H 2 O. (Lotz.) 1 pt. dissolves at ordinary temp, in 0.35 pt. H 2 O. (Riche.) Solubility increases rapidly with the tem- perature. Saturated solution at 40 is solid on cooling. SI. sol. in ordinary, insol. in absolute alcq- hol. (Lotz.) Insol. in ether. (Riche.) [(NH 4 ) 2 W 3 Ou>+5H 2 O of Margueritte.j (NH 4 ) 6 Wi 6 O 6 i + 17H 2 O = 3(NH 4 ) 2 O, 16WO 3 + 17H 2 O. Very efflorescent. Decomp. by dis- solving in pure H 2 O. (Marignac, A. ch. (4) 3. 75.) Ammonium paratungstate, (NH 4 )ioWi2O 4 i = 5(NH 4 ) 2 0, 12W0 8 . (Marignac, A. ch. (3) 69. 25.) According to Lotz (A, 91. 49) and Scheibler (J. pr. 80. 208), formula is (NH 4 ) 6 W 7 O 24 = 3(NH 4 ) 2 0, 7W0 3 . +5H 2 O. (Scheibler. J. pr. 48. 232.) + 11H 2 O. Sol. in 25-28 pts. cold H 2 O (Anthon.) Sol. in 26.1 pts. H 2 O at 10.7, and 5.8 pts at 100. (Lotz.) Sol. in 33.3 pts. cold H 2 O, and 9.6 pts at 100. (Riche.) Sol. in 22-38 pts. H 2 O at 15-18. The solution gradually decomposes, with the "ormation oi a more soluble salt. (Marignac.) Not much more sol. in NH 4 OH+Aq than n H 2 O. Insol. in alcohol. (Anthon.) Sol. in H 2 O 2 . (Kellner. Dissert, 1909.) Ammonium bismuth tungstate. See Bismuthicotungstate, ammonium. Ammonium cadmium para tungstate, 3(NH 4 ) 2 0, 12CdO, 35WO 3 +35H 2 O. Ppt. Sol. in H 2 O acidulated with HNO 3 . (Lotz, A. 91. 49.) Ammonium cerium tungstate. See Cericotungstate, ammonium. Ammonium cobaltous tungstate, 8(NH 4 ) 2 O, 2CoO, 15WO 3 +3H 2 O. (Carnot, C. R. 109. 147.) Ammonium hydroxylamine tungstate, NH 4 OWO 4 NH 4 . Sol. in H 2 O. (Hofmann, Z. anorg. 1898, 16. 465.) Ammonium iron (ferric) tungstate, 5(NH 4 ) 2 O, Fe 2 O 3 , 5WO 3 +5H 2 O. Sol. in H 2 O. (Borck.) Ammonium lanthanum tungstate. See Lanthanicotungstate, ammonium. Ammonium magnesium p7ratungstate, 2(NH 4 ) 2 O, 3MgO, 12WO 3 +24H 2 O. Very slightly sol. in H 2 O. (Marignac, A. ch. (3) 69. 58.) (NH 4 ) 2 0, 2MgO, 7WO 3 +10H 2 O. Very si. sol. in H 2 O ; sol. in H 2 O acidulated with HNO 3 . (Lotz.) Ammonium mercuric tungstate, (NH 4 ) 2 W0 4 , HgW0 4 +H 2 0. Insol. in H 2 O. Decomp. by acids or al- kalies. (Anthon.) Ammonium neodymium tungstate. See Neodymicotungstate, ammonium. Ammonium nickel tungstate. See Nickelicotungstate, ammonium. Ammonium potassium paratungstate. 5K(NH 4 )0, 12W0 3 +HH 2 0. Sol. in boiling H 2 O; si. sol. in cold H 2 O. (Hallopeau, C. R. 1896, 123. 180.) Ammonium potassium sodium paratungstate, 5(K, Na, NH 4 ) 2 0, 12WO 3 +13H 2 O, where K:Na:NH 4 =3:3:4. 10(K, Na, NH 4 ) 2 O, 24WO 3 +26H 2 O, where K :Na:NH 4 = 3:3 : 14. (Laurent.) TUNGSTATE, CADMIUM 1089 Ammonium sodium psr?atungstate, 4(NH 4 ) 2 O, Na 2 O, 12WO 3 +5H 2 O. Can be crystallised from H 2 O without decomp. (Lotz, A. 91. 57.) + 14H 2 O. Sol. in warm H 2 O. (Hallopeau, C. R. 1896, 123. 181.) (NH 4 ) 2 O, 4Na 2 O, 12WO 3 -f 25H 2 O. SI. sol. in H 2 O. (Hallopeau, C. R. 1895, 120. 1344.) 5Na 2 O, 15(NH 4 ) 2 O. 48WO 3 +48H 2 O. (Marignac, A. ch. (3) 69. 53.) 2Na 2 O, 3(NH 4 ) 2 O, 12WO 3 + 15H 2 0. (Marignac.) 3(NH 4 ) 2 O, 2Na 2 O, 12WO 3 +15H 2 O. 3(NH 4 ) 2 O, 3Na 2 O, 16WO 3 +22H 2 O. Sol. in H 2 O without decomp. (Hallopeau, C. R. 1896, 123. 181.) 3Na 2 O, 4(NH 4 ) 2 O, 16WO 3 +18H 2 O. (Gibbs, Am. Ch. J. 7. 236.) Is 2Na 2 O, 3(NH 4 ) 2 O, 12WO 3 + 13H 2 O, ac- cording to Knorre (B. 19. 823). Very sol. in hot H 2 O. (Knorre, B. 1886, 19. 823.) (NH 4 ) 2 O, 3Na 2 O, 16WO 3 +38H 2 O. (Wy- rouboff, Bull. Soc. Min. 1892, 16. 85.) 6(NH 4 ) 2 O, 2Na 2 O, 20WO 3 +24H 2 O. Can be cryst from boiling H 2 O. (Baragiola, Dis- sert, '1902.) 4Na 2 O, 16(NH 4 ) 2 O, 50WO 3 +50H 2 0. SI. sol. in cold H 2 O. (Gibbs, Proc. Am. Acad. 15. 12.) Ammonium zinc paratungstate, (NH 4 ) 2 O, 2ZnO, 7WO 3 +13H 2 O. SI. sol. in boiling H 2 O, but more easily on addition of oxalic, tartaric, phosphoric, or dil. nitric acids, or of ammonium tungstate. (Lotz, A. 91. 49.) Ammonium zirconium tungstate. See Zirconotungstate, ammonium. Ammonium wetatungstate nitrate. See Nitrate raetatungstate, ammonium. Ammonium tungstate vanadate. See Vanadiotungstate, ammonium. Antimony tungstate, Sb 2 O 3 , 5WO 3 +4H 2 O. Sol. in H 2 O without decomp. (Lefort.) Sb 2 O 3 , 6WO 3 +8H 2 O. Ppt. See also Antimoniotungstic acid. Barium tungstate, BaWO 4 . Anhydrous. Insol. in H 2 O. Decomp. by boiling HNO 3 +Aq. (Geuther and Forsberg, A. 120. 270.) + 3^H 2 O. Insol. in H 2 O or boiling H 3 PO 4 + Aq. Sol. in boiling, less sol. in cold H 2 C 2 O 4 + Aq. (Anthon.) +2^H 2 O. Insol. precipitate. (Scheibler.) Pptd. BaWO 4 is attacked by dil. acids More sol. in NH 4 NO 3 +Aq than in H 2 O (Smith and Bradbury, B. 24. 2930.) Barium ^tungstate, BaW 2 O 7 +H 2 O (?). Nearly insol. in H 2 O. 100 ccm. H 2 O dis- solve about 0.05 g. at 15. (Lefort, A. ch. (5) 16. 325.) Barium /ntungstate, BaW 3 Oi -|-4H 2 O (?). Sol. in about 300 pts. H 2 O at 15. Decomp. by boiling H 2 O into an insol. salt. (Lefort, ^ R. 88. 798.) +6H 2 O. (Scheibler.) Barium me/atungstate, BaW 4 O 18 +9H 2 O. Efflorescent. Quite sol. in hot H 2 O. Partly decomp. by cold H 2 O into BaW 3 Oio and WO 3 , which recombine on heating. (Schei- bler, J. pr. 80. 204.) Barium tungstate, BaW 8 O 26 +8H 2 O. Insol. in H 2 O or HCl+Aq. (Zettnow.) BaW 6 Oi 6 . Barium bronze. ( Hallopeau, A. ch. 1900, (7) 19. 121.) Barium paratungstate, Ba 6 Wi 2 O 4 i+14H 2 O, or Ba 3 W 7 O 24 +8H 2 O. Insol. in cold H 2 O; when freshly pptd. is si. sol. in HNO 3 +Aq. (Lotz, A. 91. 60.) Sol. in NH 4 Cl+Aq. (Wackenroder.) +27H 2 O=Ba 3 W 7 O 24 +16H 2 O. Insol. in cold, si. sol. in hot H 2 O. (Knorre, B. 18. 327.) Barium potassium tungstate tungsten oxide, BaW 4 Oi 2 , 5K 2 W 4 O 12 . (Engels, Z. anorg. 1903, 37. 136.) Barium silver metotungstate. (Scheibler.) Barium sodium para tungstate, 2BaO, 3Na 2 O, 12 WO 3 +24H 2 O. (Marignac), or BaO, 2Na 2 O, 7WO 3 + 14H 2 O (Scheibler). Insol. in H 2 O. Barium sodium tungstate tungsten oxide, 2BaW 4 12 , 3Na 2 W 6 15 . BaW 4 O 12 , 5Na 2 W 3 O 9 . (Engels, Z. anorg. 1903, 37. 131.) Bismuth tungstate, Bi 2 O 3 , 6WO 3 +8H 2 O. Very sol. in H 2 O with decomp. Pptd. by alcohol from aqueous solution. (Lefort, C. R. 87. 748.) Cadmium tungstate, CdWO 4 . Anhydrous. +H 2 O. Sol. in about 2000 pts. H 2 O. (Lefort.) +2H 2 0. Insol. in H 2 O. Sol. in hot phos- phoric or oxalic acids, or in NH 4 OH+Aq. (Anthon, J. pr. 9. 341.) Sol. in KCN+Aq. (Smith and Bradbury, B. 24. 2390.) 1090 TUNGSTATE, CADMIUM Cadmium cfttungstate, CdW 2 O 7 +3H 2 O (?). Sol. in about 500 pts. H 2 O at 15. (Lefor A. ch. (5) 15. 346.) Cadmium fritungstate, CdW 3 10 +4H 2 O (?). (Lefort.) Cadmium metotungstate, CdO, 4W> 3 - 10H 2 O. Not efflorescent. (Scheibler, J. pr. 83. 273. Somewhat less sol. in HjO than the Mn sah (Wyrouboff. Bull. Soc. Min. 1892, 16. 84. Cadmium para tungstate, Cd 3 W 7 O 24 -H6H 2 O Ppt. (Gonzalez.) Insol. in H 2 O. Sol. in NH 4 OH+Aq, an hot H 3 PO 4 , H 2 C 2 O 4 . or HC 2 H 3 O 2 +Aq. Cadmium sodium paratungstate, 2CdO, Na 2 7W0 3 +18H 2 0. Difficultly sol. in cold H 2 O. (Knorre, B 19. 824.) Calcium tungstate, CaWO 4 . Insol. in H 2 O or dil. acids. Sol. in aboui 500 pts. H 2 O. (Lefort.) Decomp. by KOH+Aq. (Anthon.) When freshly pptd., sol. in NH 4 Cl+Aq (Wackenroder.) Sol. in Mg, and NH 4 salts, also Na 2 WO +Aq. (Sonstadt, C. N. 11. 97.) Min. Scheelite. Decomp. by HC1 or HNO ; +Aq. with separation of WO 3 . Calcium ditungstate, CaW 2 O 7 -f 3H 2 O (?). Sol. in 30 pts. H 2 O at 15. (Lefort, A. ch (5) 15. 328.) Calcium Zntungstate, CaW 3 Oi +6H 2 O (?). Sol. in cold H 2 O. (Lefort.) Calcium wetatungstate, CaW 4 Oi 3 +10H 2 O. Easily sol. in H 2 O. (Scheibler.) Calcium paratungstate, Ca 3 W 7 O 24 +18H 2 O (or Ca 6 Wi 2 O 41 +30H 2 O). Much more sol. than Sr or Ba salt. (Knorre B. 18. 328.) Easily sol. in H 2 O 2 . (Knorre, B. 1885, 18. 326.) Calcium potassium tungstate tungsten oxide, CaW 4 O 12 , 5K 2 W 4 O 12 . (Engels, Z. anorg. 1903, 37.149.) Calcium sodium paratungstate, 2CaO, 3Na 2 O 12W%+3H 2 0. (Gonzalez, J. pr. (2) 36. 44.) Calcium sodium tungstate tungsten oxide, CaW 4 12 , 5Na 2 W 6 16 . Engels, Z. anorg. 1903, 37. 145.) Cerium tungstate, Ce 2 (WO 4 ) 3 +H 2 O. Precipitate. (Cossa and Zecchino, Gazz. ch. it. 10. 225.) Cerium raetatungstate, Ce 2 O 3 , 12WO 3 + 30H 2 O. Permanent. Sol. in H 2 O. (Scheibler.) Cerium sodium tungstate, Ce 2 Na 8 (WO 4 ) 7 . Insol. in H 2 O. Slowly sol. in dil. acids, easily in HCl+Aq. (Hogbom, Bull. Soc. (2) 42. 2.) Ce 2 (WO 4 ) 3 , 3Na 2 WO 4 . (Didier, C. R. 102. 823.) Cerium tungstate chloride, 3Ce 2 (WO 4 ) 8 , 2CeCl 3 . (Didier, C. R. 102. 823.) Chromic tungstate, basic, Cr 2 O 3 . 2WO 3 + 5H 2 0. Sol. in 400 pts. H 2 O at 15. (Lefort, C. R. 87. 748.) Chromic tungstate, Cr 2 (W0 4 ) 3 +7, and 13H 2 O. Sol. in CrCl 3 +Aq, and in phosphoric, oxalic, or tartaric acids +Aq. (Lotz.) +3H 2 O. (Lefort, C. R. 87. 748.) Cr 2 O 3 , 4WO 3 +6H 2 O. Sol. in about 50 pts. H 2 O at 15. (Lefort.) Cr 2 O 3 , 5WO 3 . Not attacked by aqua regia. (Smith and Oberholtzer, Z. anorg. 5. 63.) Chromic yaratungstate, Cr 2 W 7 O 24 +9H 2 O. Insol. in H 2 O or NH 4 paratungstate+Aq; sol. in CrCl 3 +Aq. (Lotz.) Cobaltous tungstate, CoWO 4 . Anhydrous. Insol. in H 2 O and acids. +2H 2 O. Insol. in H 2 O and cold HNO 3 + Aq. SI. sol. inH 2 C 2 O 4 +Aq. Completely sol. n warm H 3 PO 4 , HC 2 H 3 O 2 , or NH 4 OH+Aq. Anthon, J. pr. 9. 344.) Sol. in about 500 pts. H 2 O. (Lefort.) Cobaltous dztungstate, CoW 2 O 7 (?). +3H 2 O. Insol. in H 2 O. SI. sol. in I 2 C 2 O 4 +Aq. Completely sol. in H 3 PO 4 , HC 2 H 3 O 2 , or NH 4 OH+Aq. (Anthon.) +5H 2 O. Sol. in about 100 pts. H 2 O. (Le- ort.) +8H 2 0(?). (Lefort.) Cobaltous ^tungstate, CoW 3 O 10 +4H 2 O (?). Sol. in H 2 O. (Lefort, C. R. 88. 798.) Cobaltous wetatungstate, CoW 4 Oi 3 +9H 2 O. Sol. in H 2 0. (Scheibler, J. pr. 83. 317.) obaltous paratungstate, Co 3 W 7 O 24 +25H 2 O. (Gonzalez, J. pr. (2) 36. 44.) TUNGSTATE, LANTHANUM SODIUM 1091 Cobaltous sojiium paratungstate, 2CoO 3Na 2 O, 12WO 3 +30H 2 O. (Gonzalez.) Cupric tungstate, CuWO 4 . +2H 2 0. Insol. in H 2 O. Sol. in H 3 PO 4 HC 2 H 3 O 2 , or NH 4 OH+Aq. Insol. in H 2 C 2 O +Aq. (Anthon.) 100 ccm. H 2 O at 15 dissolve 0.1 g. (Le fort.) Cupric ditungstate, CuW 2 7 (?). +4H 2 O. Insol. in H 2 O and HNO 3 . Sol in NH 4 OH+Aq. (Anthon, J. pr. 9. 346. +5H 2 O. Sol. in about 300 pts. H 2 O. (Le- fort.) Cupric raetatungstate, CuW 4 Oi 3 +llH 2 O. Sol. in H 2 O. (Scheibler.) Cupric paratungstate, Cu3W 7 O 24 +19H 2 O. Insol. in H 2 O. (Knorre, B. 19. 826.) Cuprocupric tungstate, Cu 2 W0 4 , 2CuW0 4 . Insol. in H 2 O. (Zettnow, Pogg. 130. 255.) Cupric sodium paratungstate, Cu 3 Na 6 (W 7 O 24 ) 2 +32H 2 O. Ppt. (Knorre, B. 19. 826.) CuO,4Na 2 0, 12WO 3 +32H 2 O. Ppt. (Gon- zalez, J. pr. (2) 36. 52.) Cupric tungstate ammonia. CuWO 4 . 2NH 3 + H 2 0. (Schiff, A. 123. 39.) CuWO 4 , 4NH 3 . Gives off NH 3 at ord. temp. Sol. in H 2 O. Sol. in dil. NH 4 OH + Aq. (Briggs, Chem.. Soc. 1904, 85. 676.) CuO, 4WO 3 , 6NH 3 +8H 2 O. Insol. in H 2 O. Nearly insol. in dil. NH 4 OH+Aq. (Briggs, Chem. Soc. 1904, 85. 676.) Didymium tungstate, Di 2 (WO 4 ) 3 . Precipitate. (Frerichs and Smith, A. 191. 355.) Didymium wetotungstate. Sol. in H 2 O. (Scheibler.) Didymium sodium tungstate, DiNa 3 (WO 4 ) 3 . Insol. in H 2 O. Slowly sol. in dil. acids. Sol. in cone. HCl+Aq. DiNa(WO 4 ) 2 . As above. (Hogbom, Bull. Soc. (2) 42. 2.) Erbium sodium tungstate, Na 6 Er 4 (W0 4 ) 9 . Insol. in H 2 O. (Hogbom.) Glucinum metatungstate. Very sol. in H 2 O. Indium tungstate, In 2 (WO 4 ) 3 +8H 2 O. Insol. in H 2 O. Decomp. by acids. (Renz, Dissert. 1902.) Iron (ferrous) tungstate, FeW0 4 . Min. Ferberite, Reinite. +3H 2 O. Insol. in H 2 O. Sol. in cold H 2 SO 4 , HC1, or HNO 3 +Aq. Decomp. by boiling acids with separation of WO 3 . Sol. in boiling H 3 PO 4 +Aq or warm H 2 C 2 O 4 +Aq. (Anthon, J. pr. 9. 343.) +zH 2 O. Very unstable. (Lefort, A. ch. (5) 15. 314.) Iron (ferrous) ditungstate, FeW 2 O 7 (?). Insol. in H 2 O. Sol. in hot H 3 PO 4 +Aq or H 2 C 2 O 4 +Aq. Decomp. by dil. HCl+Aq or by KOH+Aq. (Ebelmen, C. R. 17. 1198.) +zH 2 O. Very unstable. (Lefort.) Iron (ferrous) Zn'tungstate, FeW 8 Oi + Ppt. Decomp. by cold, more rapidly by hotH 2 O. (Lefort.) Iron (ferrous) raetatungstate. Sol. in H 2 O. (Scheibler, J. pr. 83. 315.) Iron (ferric) tungstate, basic, Fe 2 O 3 , 2W0 3 + Sol. in about 50 pts. H 2 O. (Lefort.) 2Fe 2 O 3 , 3WO 3 +6H 2 O. Sol. in about 300 pts. H 2 O at 15. (Lefort.) Iron (ferric) ^ntungstate (?), Fe 2 O 3 , 4WO 3 + 4H 2 O = Fe 2 O 3 , 3WO 3 +WO 3 , 4H 2 O (?). Sol. in H 2 O without decomp. (Lefort.) Iron (ferric) wetotungstate. Sol. in H 2 O. (Scheibler, J. pr. 83. 273.) Iron (ferrous) manganous tungstate, 7FeWC>4, MnWO 4 . (Geuther and Forsberg, A. 120. 277.) 4FeW0 4 , MnWO 4 . (G. and F.) 3FeWO 4 , MnWO 4 . Partially sol. in cone. HCl+Aq. (G. andF.) 3FeWO 4 , 2MnWO 4 . (G. and F.) FeWO 4 , MnWO 4 . (Zettnow, Pogg. 130. 250.) FeWO 4 , 2MnWO 4 . (G. and F.) FeWO 4 , 7MnWO 4 . (G. and F.) .rFeWO 4 , ?/MnWO 4 . Min. Wolframite. Sol. n HCl+Aq, and boiling H 3 PO 4 +Aq. Lanthanum tungstate, La 2 (WO 4 ) 3 . Precipitate. Lanthanum metotungstate. Sol. in H 2 O. (Scheibler.) Lanthanum silver tungstate. See Lanthanicotungstate, silver. Lanthanum sodium tungstate, Na 8 La 2 (WO 4 ) 7 . Insol. in H 2 O. Slowly sol. in dil. acids. Sol. in HCl+Aq. La 4 Na 6 (WO 4 ) 9 . As above. (Hogbom, Bull. Soc. (2) 42.2.) 1092 TUNGSTATE, LEAD Lead tungstate, PbWO 4 . Insol. in H 2 O or cold HNO 3 +Aq. Sol. in KOH+Aq. Decomp. by hot HNO 3 +Aq. (Anthon, J. pr. 9. 342.) Sol. in about 4000 pts. H 2 O. (Lefort.) Min. Scheelenite, Stolzite. Sol. in KOH + Aq; decomp. by HNO 8 . Absolutely insol. in NH 4 NO 3 +Aq. (Smith and Bradbury, B. 24. 2930.) Lead ditungstate, PbW 2 O 7 +2H 2 O (?). Sol. in about 80 pts. H 2 O at 15. (Lefort.) Lead Zntungstate, PbW 3 O 10 +2H 2 O (?). Ppt. (Lefort.) Lead metotungstate, PbW 4 Oi 3 +5H 2 O. SI. sol. in cold, more in hot H 2 O. Sol. in hot HNOg+Aq. (Scheibler, J. pr. 83. 318.) Lead paratungstate, Pb 3 W 7 O24. Insol. in H 2 O, dil. HNO 3 +Aq, (NH 4 ) 2 WO 4 +Aq, or Pb(NO 3 ) 2 +Aq. Sol. in NaOH + Aq or boiling H 3 PO 4 +Aq. (Lotz, A. 91. 49.) Lead sodium paratungstate, PbO, 4Na 2 O, 12WO 3 +28H 2 O. (Gonzalez.) Lithium tungstate, Li 2 WO 4 . Rather easily sol. in H 2 O. (Gmelin.) Lithium wetotungstate, Li 2 W 4 Oi 3 . Insol. in H 2 O. (Knorre, J. pr. (2) 27. 94.) +rcH 2 O. Syrup. (Scheibler.) Lithium paratungstate, Lii Wi 2 O 41 +33H 2 O (orLi 6 W 7 O 24 +19H 2 O). According to Scheibler, more sol. than the paratungstates of the other alkali metals. Lithium tungstate tungsten oxide, Li 2 WsOi5. Lithium bronze. Insol. in H 2 0. Lithium potassium tungstate tungsten oxide, Li 2 W 5 15 , 3K 2 W 4 12 . Lithium potassium bronze. Insol. in H 2 O. (Feit, B. 21. 135.) Lithium sodium tungstate, Li 2 WO 4 +3H 2 O, 3(Na 2 WO 4 +3H 2 O). (Traube, N. Jahrb. Miner, 1894, I. 190.) Magnesium tungstate, MgWO 4 . Anhydrous. Insol. in H 2 O. Gradually de- comp. by boiling cone. HNO 3 +Aq. (Geuther and Forsberg, A. 120. 272.) +3H 2 O. Very sol. in H 2 O; nearly insol in alcohol. (Lefort, A. ch. (5) 16. 329.) +7H 2 O. Slowly sol. in cold, very easily in hot H 2 O. (Ullik, W. A. B. 56. 2. 152.) Magnesium ^'tungstate, MgW 2 O 7 +8H 2 O (?). Sol. in about 100 pts. H 2 O. (Lefort.) Magnesium Zntungstate, MgW 3 Oio+4H 2 O(?). Easily sol. in H 2 O with gradual decomp. Lefort.) Magnesium rae.'atungstate, MgW 4 Oi 3 +8H 2 O. Sol. in H 2 O. (Scheibler.) esium paratungstate, Mg 3 W 7 O 24 4- 24H 2 0. Very difficultly sol. in cold, somewhat sol. n hot H 2 O. (Knorre, B. 19. 825.) Magnesium potassium tungstate, MgWO 4 , K 2 WO 4 . +2H 2 O. Very si. sol. in H 2 O. (Ullik.) +6H 2 O. Precipitate. Magnesium potassium paratungstate, 5( 2 / 3 K 2 0, ViMgO), 12W0 3 +24H 2 0. Insol. in cold, sol. in hot H 2 O. (Hallo- peau, C. R. 1898, 127. 621.) Magnesium sodium paratungstate, 3MgO, 3Na 2 O, 14WO 3 +33H 2 O. Nearly insol. in H 2 O. (Knorre, B. 19. 825.) Manganous tungstate, MnWO 4 . Min. Hubnerite. Partially sol. in HC1+ . +2H 2 O. Insol. in H 2 O; sol. in warm H 3 P0 4 and H 2 C 2 O 4 +Aq; si. sol. in HC 2 H 3 O 2 +Aq. Insol. in cold HCl+Aq. (Anthon.) +H 2 O. Sol. in about 2500 pts. H 2 O at 15. (Lefort.) Manganous ^tungstate, MnW 2 O 7 +3H 2 O (?). Sol. in about 450 pts. H 2 O at 15. (Lefort, A. ch. (5) 15. 333.) Manganous Zntungstate, MnW 3 Oio+5H 2 O(?). Decomp. by H 2 O into MnW 2 O 7 and MnW 4 O ]3 . (Lefort, A. ch. (5) 17. 480.) Manganous metotungstate, MnW 4 Oi 3 + 10H 2 O. Very sol. in H 2 O. (Wyrouboff, Bull. Soc. Min. 1892, 15. 82.) Manganous paratungstate, 5MnO, 12WO 3 + 34H 2 O. (Gonzalez, J. pr. (2) 36. 44.) Mn 3 W 7 O 24 +llH 2 O. When recently pptd., sol. in a small amt. of H 2 O acidulated with HNO 3 . (Lotz.) Manganous potassium tungstate, 2MnO, 3K 2 O, 12WO 3 +16H 2 O. Completely insol! in H 2 O. (Hallopeau, Bull. Soc. 1898, (3) 19. 955.) TUNGSTATE, POTASSIUM 1093 Manganous sodium paratungstate, 3Na 2 O, 3MnO, 14W0 3 +36H 2 0. Sol. in H 2 O. (Knorre, B. 19. 826.) Manganic sodium tungstate. See Permanganotungstate, sodium. Mercurous tungstate, Hg 2 WO 4 . Insol. in H 2 O. (Anthon.) Impossible to obtain pure, as it is decomp. into 2Hg 2 O, 3WO 3 +8H 2 O. Sol. in 100 pts. H 2 O at 15. (Lefort.) Mercurous metatungstate. Hg 2 W 4 Oi 3 -f- 25H 2 0. Ppt. (Scheibler, J. pr. 83. 319.) Mercuric tungstate, HgWO 4 . SI. sol. in H 2 O and very unstable. (Lefort, A. ch. (5) 15. 356.) 3HgO, 2WO 3 . Insol. in H 2 O. (Anthon.) 2HgO, 3WO 3 . Insol. in H 2 O. (Anthon.) 3HgO, 5WO 3 +5H 2 O. Sol. in about 250 pts. H 2 O at 15. (Lefort.) 2HgO, 5WO 3 +7H 2 O. Decomp. by hot or cold H 2 O. (Lefort, C. R. 88. 798.) Mercuric Zntungstate, HgW 3 O 10 +7H 2 O (?). Sol. in about 120 pts. H 2 O at 15. (Lefort, A. ch. (5) 15. 360.) Molybdenum tungstate. Easily sol. in H 2 O. Insol. in NH 4 Cl+Aq or in alcohol of 0.87 sp. gr. (Berzelius.) Neodymium tungstate, Nd 2 (WO 4 ) 3 . Very si. sol. in H 2 O. 1 pt. is sol. in 52630 pts. H 2 O at 22; 59580 pts. at 65; 66040 pts. at 98. (Hitchcock, J. Am. Chem. Soc. 1895, 17. 532.) Nickel tungstate, NiWO 4 . +3H 2 O. Sol. in about 1000 pts. H 2 O at 15. (Lefort.) +6H 2 O. Insol. in H 2 O or H 2 C 2 O 4 +Aq. Sol. in boiling H 3 PO 4 +Aq, HC 2 H 3 O 2 +Aq, or in warm NH 4 OH+Aq. (Anthon.) Nickel ^tungstate, NiW 2 O 7 +5H 2 O (?). Sol. in about 250 pts. H 2 O. (Lefort.) Nickel ^ntungstate, NiW 3 Oio+4H 2 O (?). Sol. in H 2 O. Pptd. by alcohol. Decomp. by cold or warm H 2 O after above pptn. (Le- fort.) Nickel wetatungstate, NiW 4 O 13 +8H 2 O. Sol. in H 2 O. (Scheibler, J. pr. 83. 273.) Nickel paratungstate, Ni 3 W 7 O 24 -fl4H 2 O. Insol. in H 2 O. SI. sol. in H 2 C 2 O 4 +Aq. Completely sol. in warm H 3 PO 4 or HC 2 H 3 O 2 -|- Aq. (Anthon.) Potassium tungstate, K 2 WO 4 . Anhydrous. Rather deliquescent. Easily sol. in H 2 O. +H 2 O. Easily sol. in H 2 O. Insol. in alcohol. +2H 2 O. Very sol. in H 2 O with absorption of heat. 1 pt. dissolves in 1.94 pts. cold, and 0.66 pt. boiling H 2 O. Alcohol does not mix with cone. aq. solution, but slowly separates out the salt from it. Acids, even H 2 SO 3 , HC 2 H 3 O 2 or H 2 C 2 O 4 , separate out WO 3 from solution. (Riche, A. ch. (3) 50. 45.) Potassium ditungstate, K 2 W 2 O7+2H 2 O. Sol. in about 8 pts. H 2 O at 15, but on heat- ing is converted into +3H 2 O. 100 pts. H 2 O dissolve only 2-3 pts. at 15. (Lefort, A. ch. (5) 9. 102.) Potassium ^n'tungstate, K 2 W 3 O 10 +2H 2 O. Sol. in 5-6 pts. H 2 O at 15. Can be re- cryst. from hot H 2 O. (Lefort, A. ch. (5) 9. 105.) Potassium metatungstate, K 2 W 4 Oi 3 +5H 2 O. Not efflorescent. Easily sol. in H 2 O. (Marignac.) (K 4 W 5 Oi 7 +8H 2 O of Margueritte.) +8H 2 O. Extremely efflorescent. (Scheib- ler.) Potassium odotungstate, K 2 W 8 O 26 . Insol. in H 2 O. (Knorre, J. pr. (2) 27. 49.) Potassium tungstate, K 8 Wi O 34 +9H 2 O = 4K 2 O, 10WO 3 +9H 2 O. Properties resemble the para tungstate. (Gibbs, Proc. Am. Acad. 16. 11.) +8H 2 O = K 4 W 6 O 17 -HH 2 O. Sol. in 15 pts. H 2 O at 15, but decomposed by heating into K 2 W 2 O 7 and K 2 W 3 Oi . (Lefort, A. ch. (5) 9. 104.) Ki W H O 47 . Very difficulty sol. in cold, appreciably sol. in hot H 2 O, probably with decomposition. (Knorre.) Potassium paratungstate, K 10 Wi 2 p 4 i+llH 2 O (or K 6 W7O 24 +6H 6 O, according to Lotz and Scheibler.) Much more sol. in hot than cold H2O. (Anthon.) Sol. in 100 pts. H 2 O at 16, in 8.5 pts. at 100. (An- Sol. in 46.5 pts. cold, and 15.15 pts. boiling EhO. (Riche.) By shaking the crystals several days at 20, 1 pt. dissolves in 71 pts. H 2 O. If the salt is treated with boiling water, more goes into solution the Ipnger it is boiled, until after several days' boiling 1 pt. of the salt dissolved in 5.52 pts. H 2 O at 18. Kept in a closed flask, this solution contained after 26 days 1 pt. of salt to 11.9 pts. H 2 O; after 153 days, 1 pt. of salt to 15.6 pts. H 2 0; after 334 days, 1 pt. of salt to 15.6 pts. H 2 O. In- sol. in alcohol. (Marignac.) +8H 2 O. 1094 TUNGSTATE, POTASSIUM SODIUM Potassium sodium tungstate, K 2 WO 4 , Easily sol. in hot and cold H 2 O. (Ullik, W. A. B. 66, 2. 150.) Deliquescent. Sol. in 1 pt. cold, and YI pt. hot H 2 O. (Anthon.) Potassium sodium paratungstate, Na 2 O, 4K 2 0, 12WO 3 +15H 2 O. Sol. in H 2 O-. (Marignac.) 8 /nNa 2 O, 3 /nK 2 O, 12WO 3 +25H 2 O. Sol. in H 2 O. (Marignac.) Potassium strontium tungstate tungsten oxide, 5K 2 W 4 Oi 2 , SrW 4 Oi 2 . (Engels, Z. anorg. 1903, 37. 143.) Potassium uranous tungstate. See Uranosotungstate, potassium. Potassium zirconium tungstate. See Zirconotungstate, potassium. Potassium tungstate tungsten oxide, K 2 WO 4 , W 2 6 . Potassium tungsten bronze. (Scheibler, J. pr. 83. 321.) Formula is K 2 W 4 Oi 2 . Not attacked by acids, and only very si. by alkalies. (Knorre, J. pr. (2) 27. 49.) K 2 WO 4 , 4WO 2 . Not attacked by acids, even HF, or bv alkalies +Aq. Insol. in alcohol. (Zettnow, Pogg, 130. 262.) Does not exist. (Knorre.) Potassium sodium tungstate tungsten oxide, 5K 2 W 4 Oi 2 +2Na 4 W 6 Oi5. Potassium sodium tungsten bronze. Prop- erties as potassium bronze. 3K 2 W 4 Oi 2 , 2Na 2 W 3 O 9 . As above. (Knorre, J. pr. (2) 27. 49.) Praseodymium tungstate, Pr 2 (WO 4 ) 3 . Very si. sol. in H 2 O. Insol. in H 2 O at 20; at 75, 1 pt. is sol. in 23,300 pts. H 2 O. (Hitchcock, J..Am. Chem. Soc. 1895, 17. 529.) Rubidium wetotungstate, Rb 2 O, 4WO 3 + 8H 2 0. Sol. in about 10 pts. cold H 2 O. Moderately sol. in warm H 2 O. (Wyrou- boff, Bull. S6c. Min. 1892, 15. 69.) Rubidium pentotungstate, Rb 2 W 6 O 16 . Almost insol. in hot H 2 O. When finely powdered, it is sol. in alkali carbonates +Aq. (Schaeffer, Z. anorg. 1904, 38. 163.) Rubidium octotungstate, Rb 2 W 8 O 26 . Insol. in H 2 O, acids, and alkalies. (Schaef- fer, Z anorg. 1934, 38. 103.) Rubidium paratungstate, 5Rb 2 O, 12WO 3 + 18H 2 0. Very si. sol. in H 2 O. (Schaeffer, Z. anorg. 1904, 38. 173.) Samarium metotungstate, Sm 2 O 3 , 12WO 3 + 35H 2 O. Easily sol. in H 2 O. (Cleve.) Samarium sodium tungstate, Na 6 Sm 4 (WO 4 )9. Insol. in H 2 O. Slowly sol. in dil. acids, easily in cone. HCl+Aq. (Hogbom, Bull. Soc. (2) 42. 2.) Silver (argentous) tungstate, Ag 4 O, 2WO 3 . HNOs+Aq separates WO 3 . KOH+Aq dissolves out WO 3 and separates Ag 4 O. (Wohler and Rautenberg, A. 114. 120.) Does not exist. (Muthmann, B. 20. 983.) Silver tungstate, Ag 2 WO 4 . Sol. in about 2000 pts. H 2 O at 15. Easily decomp. by NaCl+Aq or BNO 3 +Aq. (Lefort.) Ag 2 W 2 7 . Insol. in H 2 O. Nearly insol. in HC 2 H 3 2 or H 3 PO 4 +Aq. More sol. in KOH, NH 4 OH+Aq, or H 2 C 2 O 4 +Aq. (An- thon, J. pr. 9. 347.) +H 2 O. Sol. in about 5000 pts. H 2 O at 15. (Lefort.) Silver wetotungstate, Ag 2 W 4 Oi 3 +3H 2 O. SI. sol. in H 2 O. (Scheibler, J. pr. 83. 318.) Nearly insol. in H 2 O. (Rosenheim, Z. anorg. 1911, 69. 250.) Silver paratungstate, Ag 10 Wi 2 O 4 i+8H 2 O. (Gonzalez, J. pr. (2) 36. 44.) Silver tungstate ammonia, Ag 2 WO 4 , 4NH 3 . Sol. in H 2 O with rapid decomp. (Wid- mann, Bull. Soc. (2) 20. 64.) Sodium tungstate, Na 2 WO 4 +2H 2 O. Sol. in 4 pts. cold, and 2 pts. boiling H 2 0. (Vauquelin and Hecht.) Sol. in 1.1 pts. cold, and 0.5 pt. boiling H 2 O. (Anthon.) Sol. in 2.44 pts. H 2 O at 0; 1.81 pts. at 15; 0.81 pt. at 100. (Riche.) Solubility in H 2 O at t. t % Na 2 WOi Mols. H 2 O to 1 mol. Na 2 WO 4 Mols. of anhydrous salt to 100 mo Is. H 2 -3.5 +0.5 21.0 43.5 80.5 100.0 41.67 41.73 42.27 43.98 47.65 49.31 22.87 22.80 22.30 20.80 17.95 16.79 4.37 4.39 4.48 4.81 5.57 5.95 (Funk, B. 1900, 33. 3701.) See also -flOH 2 O. TUN GST ATE, SODIUM 1095 Sp. gr. of Na 2 WO 4 +Aq at 24.5 containing: Solubility in H 2 O at t. 5 10 15 % Na 2 WO 4 +2H 2 O, 1.036 1.075 1.119 t % Mols. H 2 O to 1 mol Mols. anhy- drous salt to 20 25 30 % Na 2 WO 4 +2H 2 O, 11 ftft 1 91 f 1 97 d. Na 2 WO4 Na 2 WO 4 100 mols. H 2 O .1OO 1.Z1O c.f 35 40 44 % Na 2 WO 4 +2H 2 O. -5. 30.60 37.04 2.70 1.349 1.430 1.492 4.0 31.87 34.92 2.86 (Franz, J. pr. (2) 4. 238.) -3.5 -2.0 32.98 34.52 33.19 30.90 3.01 3.23 0.0 36.54 28.37 3.52 +3.0 39.20 25.33 3.95 Sp. gr. of Na 2 WO 4 +Aq at 25. +5.0 41.02 23.48 4.26 (Funk, B. 1900, 33. 3701.) Sp. gr. at 20 Per cent Na 2 WO4 fer cent a 2 4, 2 Sodium rfituncstatc NTn.W.0.. 1.02016 2.21 2.48 Sol. in H 2 O by heating several hours to 1.03915 4.26 4.78 130-150. (Knorre, J. pr. (2) 27. 80.) 1.04292 4.59 5.15 +6H 2 O Sol. in 13 pts. H 2 O at 15. (Le- 1.05831 6.25 7.01 fort, C. R. 88. 798.) 1.07449 7.83 8.79 1.08209 1.09687 1.12114 1 . 13036 1.14392 1 . 16896 1.19154 8.61 10.08 12.30 13.16 14.44 16.56 18.52 9.66 11.31 13.81 14.77 16.21 18.62 20.79 Sodium Zntungstate, Na 2 W 3 Oio+4H 2 O. Sol. in 1 pt. H 2 O. Decomp. on standing into sol. tetratungst&te and insol. cfo'tung- state. (Lefort, C. R. 88. 798.) Neither this nor the other fritungstates of Lefort exist, according to Knorre (J. pr. (2) 1 . 19938 19.10 21.44 27. 49.) 1 . 20787 19.74 -22.16 1.21720 20.59 23.11 Sodium wefatungstate, Na 2 W 4 Oi 3 . 1.25041 23.16 25.99 Anhydrous. Insol in H 2 O. 1.25083 23.30 26.15 +10H 2 O. Sol. at 13. in 0.935 pt. H 2 O to 1.26234 24.05 27.00 form a solution of 3.02 sp. gr. (Scheibler.) 1.28143 25.46 . 28.58 Sol. at 19 in 0.195 pt. H 2 O. (Forcher.) 1.33993 29.50 33.11 Precipitated by alcohol. 1.38826 32.68 36.68 1.41072 33.91 38.06 Sodium pentatungstate, Na 2 W 6 Oi 6 . 1.47193 1.48481 1.48595 37.30 38.20 38.43 41.87 42.87 43.14 SI. sol. in H 2 O by heating 3 hours at 150. (Knorre, J. pr. (2) 27. 49.) C\ j j_.i^ _-.!. x "VT^ TIT f\ (Pawlewski, B. 1900, 33. 1224.) Na 2 WO 4 +Aq is pptd. by HC1, HNO 3 , or H 2 SO 4 +Aq, but not by H 2 SO 3 , HI, HCN, oxalic, or tartaric acids +Aq, but pptn. by the former acids is not prevented by presence of the latter, but when heated with HC 2 H 3 O 2 + Aq, or in presence of H 3 PO 4 +Aq, mineral acids cause no ppt. (Zettnow, Pogg, 130. -I f* \ Much more sol. in H 2 O 2 than in H 2 0. (Kellner, Dissert, 1909.) SI. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 829.) Insol. in alcohol. (Riche, A. ch. (3) 60. 52 ) Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) +10H 2 0. Insol. in H 2 O. Very difficultly attacked by acids and alkalies. (Knorre.) + 12H 2 O. Easily sol. in cold H 2 O, and can be recryst. without decomp. (Ullik, W. A. B. 66, 2. 157.) 3Na 2 O, 8WO 3 +17H 2 0. Very efflorescent. Very sol. in hot H 2 O. (Wells, J. Am. Chem. Soc. 1907, 29. 112.) Sodium tungstate, Na 6 W 7 O 27 (?). + 16H 2 O (?). (Marignac, A. ch. (3) 69. 51.) +21H 2 O (?). Much more sol. and much more rapidly than the paratungstate. (Ma- rignac.) Na 4 W 3 On+7H 2 O(?). Mixture of Na 2 W 4 O 13 and Na 2 WO 4 . (Knorre, J. pr. (2) 27. 49.) Na 4 W 6 Oi7 + lLH 2 O. Efflorescent. Sol. in H 2 O. (Marignac.) 100 pts. H 2 O dissolve 16 pts. at 15. (Le- fort, A. ch. (5) 9. 97.) Formula is 4Na 2 O, 10WO 3 +23H 2 O, ac- cording to Gibbs (Proc. Am. Acad. 15. 5.) 1096 TUNGSTATE, SODIUM Sodium paratungstate, Nai Wi 2 O 4 i+21H 2 O. +25HoO. +28H 2 O = 3Na 6 W 7 O 24 + 16H 2 O. according to Lotz and Scheibler. Sol. in 8 pts. cold H2O (Anthon) ; in 12.6 pts. at 22. (Forcher). Sol. in about 12 pts. H 2 O. (Marignac.) The aqueous solution saturated at 35-40 contained to 1 pt. of the salt, after: 1 12 77 227 410 days, at 18 18 18 16 20 9.25 11.26 10.92 11.90 11.74 pts. H 2 0. The solution saturated by very long boiling, after a part of the salt had crystallised out, contained, after: 1 2 12 days, . 68 0.91 2 . 59 pts. H 2 O to 1 pt. salt, 72 222 405 days, 6 . 88 9 . 75 ' 8 . 80 pts. H 2 O to 1 pt. salt. (Marignac.) Decomp. by boiling with" H 2 O. (Knorre, B. 18. 2362.) Sodium strontium paratungstate. Na 2 O, 4SrO, 12W0 3 +29H 2 0. (Gonzalez, J. pr. (2) 36. 44.) Sodium strontium tungstate tungsten oxide. 5NaW 5 O 15 , SrW 4 12 . 12Na 2 W 3 O 9 , SrW 4 O 12 . (Engels, Z. anorg. 1903, 37. 138.) Sodium thorium tungstate, Na 4 Th(WO 4 ) 4 . Insol. in H 2 O. Slowly sol. in dil. acids, easily in cone. HCl+Aq. (Hogbom, Bull. Soc. (2) 42. 2.) Sodium ytterbium tungstate, Yb 2 3 , 9Na 2 O, 12WO 3 . Insol. in H 2 O. (Cleve, Z. anorg. 1902, 32. 154.) 2Yb 2 3 , 4Na 2 0, 7WO 3 . Ppt. '(Cleve.) Sodium yttrium tungstate, Na 8 Y 2 (WO 4 ) 7 . Insol. in H 2 O, and very slowly attacked by dil. acids. (Hogbom, Bull. Soc. (2) 42. 2.) Sodium zinc paratungstate, Na 2 O, 2ZnO, 7WO 3 +15H 2 O. Difficultly sol. in cold, more sol. in hot H 2 O (Knorre, B. 19. 823.) +21H 2 O. (Knorre.) Sodium tungstate tungsten oxide, Na 2 W0 4 , W 2 O 6 . Yellow tungsten bronze. Gradually de- liquesces on air. Not decomp. by any acid, even aqua regia, except HF, or by alkalies' (Wohler, Pogg. 2. 350.) Correct formula is NasWeOig. according to Phillip (B. 16. 499). Sol. in ammoniacal silver solution with separation of Ag. Easily sol. in boiling alkaline potassium ferricyanide-f Aq. (Phillip, B. 12. 2234.) Na 2 WO 4 , 2W 2 O 6 . Blue tungsten bronze. Not attacked by acids or alkalies. (Scheibler.) Correct formula is Na 2 W 5 Oi 5 , according to Phillip (B. 16. 506). Sol. in ammoniacal silver solution with separation of Ag. Na 4 W 6 Oi 5 . Properties as above. (Phillip, B. 16. 499.) Na 2 \fy 3 O 9 . Properties as above. (Phillip.) Strontium tungstate, SrWO 4 . Precipitate. (Schultze.) Sol. in about 700 pts. H 2 O. (Lefort.) Strontium ditungstate, SrW 2 O 7 +3H 2 O (?). 100 ccm. H 2 O dissolve 0.35 g. at 15. (Le- fort, A. ch. (5) 15. 326.) Strontium ^ntungstate, SrW 3 O 10 +5H 2 O (?). Sol. in H 2 O with decomp. into SrW 2 O 7 and SrW 4 Oi 3 . (Lefort, A. ch. (5) 17. 477.) Strontium mefotungstate, SrW 4 Oi 3 +8H 2 O. Solubility as calcium meta tungstate. (Scheiblert) Extraordinarily sol. in H 2 O. (Wyrouboff, Bull. Soc. Min. 1892, 16. 63.) Strontium paratungstate, Sr 3 W 7 O 24 +16H 2 O, orSr 5 W 12 O 41 +27H 2 O. Insol. in cold, si. sol. in hot H 2 O. (Knorre, B. 18. 327.) Thallous tungstate, T1 2 WO 4 . Very si. sol. in H 2 O. Sol. in hot Na 2 CO 3 + Aq. (Flemming, J. B. 1868. 250.) Thallous raetatungstate, T1 2 W 4 O 13 +3H 2 O. Nearly insol. in H 2 O. (Rosenheim, Z. anorg. 1911, 69. 251.) Thallous paratungstate, 5T1 2 O, 12WO 3 . Insol. in H 2 O. Sol. in Na 2 CO 3 +Aq. and K~OH+Aq. decomposed bv mineral acids. (Schaeffer, Z. anorg. 1904, 38. 171.) Thallous hydrogen tungstate, T1HWO 4 . Insol. in H 2 O. Difficultly sol. in NH 4 OH + Aq. Easily sol. in boiling alkali carbonates or hydrates +Aq. (Oettinger, J. B. 1864. ^)T:. ) Thorium tungstate. Precipitate. (Berzelius.) Insol. in H 2 O. Tin (stannous) tungstate, SnWO 4 +6H 2 O. Insol. in H 2 O. Sol. in oxalic acid and in KOH+Aq. Slowly sol. in hot H 3 PO 4 +Aq. (Anthon, J. pr. 9. 341.) TUNGSTOCYANIDE, MANGANOUS 1097 Tin (stannic) tungstate, 9SnO 2 , 13WO 3 . Insol. in ammonium tungstate -|-Aq. Sol. in tin salts +Aq, also in phosphoric, oxalic, or tartaric acids +Aq. (Lotz, A. 91. 49.) Tungsten tungstate, WO 2 , WO 3 = W 2 O 5 . See Tungsten oxide, W 2 O 5 . Uranous tungstate, UO 2 , 3WO 3 +6H 2 O. Decomp. by NaOH+Aq or HNO 3 +Aq. Sol. in HCl+Aq, but not in H 2 SO 4 . (Ram- melsberg.) Uranyl tungstate, UO 3 , WO 3 +2H 2 O. Sol. in about 100 pts. H 2 O. (Lefort, C. R. 87. 748.) UO 3 , 3WO 3 +5H 2 O (?). Sol. in about 200 pts. H 2 O. (Lefort.) Vanadium tungstate. SI. sol. in H 2 O. Ytterbium tungstate basic, (YbO) 2 WO 4 . Ppt. (Cleve, Z. anorg. 1902, 32. 153.) Ytterbium raetatungstate, Yb 2 O 3 , 12WO 3 + 35H 2 0. Very sol. in H 2 O. (Cleve.) Yttrium tungstate, Y 2 (WO 4 ) 3 +6H 2 O. Very si. sol. in H 2 O, but more sol. in Na 2 WO 4 +Aq. (Berlin.) Zinc tungstate, ZnWO 4 . Insol. in H 2 O. (Geuther and Forsberg, A. 120. 270.) +H 2 O. Sol. in 503 pts. H 2 O. Zinc efttungstate, ZnW 2 O 7 +3H 2 O (?). Sol. in 10 pts. H 2 O at 15, but solution soon decomposes. (Lefort.) Zinc in'tungstate, ZnW 3 Oio+5H 2 O. Insol. in boiling H 2 O. Sol. in ZnSO 4 -f-Aq, or Na 4 W 6 17 +Aq. (Gibbs.) Zinc metatungstate, ZnW 4 O 13 +10H 2 O. Easily sol. in H 2 O. Loses crystal H 2 O by ignition, and becomes insol. in H 2 O. (Scheib- ler, J. pr. 83. 273.) -j-8H 2 O. More sol. in H 2 O than mag- nesium com p. (Wyrouboff, Bull. Soc. Min. 1892, 16. 72.) Zinc tungstate, Zn 4 W 10 O 34 +18H 2 O=4ZnO, 10WO 3 +18H 2 O. Insol. in H 2 O. Sol. in excess of zinc sul- phate or of sodium tungstate +Aq. (Gibbs, Proc. Am. Acad. 15. 14.) +29H 2 O. (Gibbs.) Zinc paratungstate, 5ZnO, 12WO 3 -r-37H 2 O. (Gonzalez, J. pr. (2) 36. 44.) Zinc tungstate, Zn 9 W 22 O 76 +66H 2 O=9ZnO, 22WO 3 +66H 2 O. . Insol. in H 2 O. (Gibbs.) Zinc tungstate -ammonia, ZnWO 4 , 4NH,+ 3H 2 O. Decomp. in the air. (Briges, Chem. Soc. 1904, 85. 677.) Pertungstic acid. See Pertungstic acid. Tungstoarsenic acid. See Arseniotungstic acid. Tungstoboric acid. See Borotungstic acid. Tungstocyanhydric acid, H 4 W(CN) 8 + Hydroscopic. Sol. in H 2 O and abs. alcohol. Insol. in ether, benzene etc. (Olsson. Z. anore. 1914, 88. 71.) Ammonium tungstocyanide, (NH 4 ) 4 W(CN) 8 . Easily sol. in H 2 O. Aqueous solution de- comp. slowly. Insol. in organic solvents. (Olsson. Z. anorg. 1914, 88. 62.) Cadmium tungstocyanide, Cd 2 W(CN) 8 -f- 8H 2 O. Nearly insol. in H 2 O. SI. sol. in dil. HC1. Sol. in cone. NH 4 OH-f Aq. Insol. in organic solvents. (Olsson, Z. anorg. 1914, 88. 68.) Caesium tungstocyanide, Cs 4 W(CN) 8 . Easily sol. in H 2 O forming stable solutions. Insol. in alcohol and other organic solvents (Olsson.) Calcium tungstocyanide, Ca 2 W(CN) 8 -|-8H2O. Easily sol. in H 2 O. Aqueous solution de- comp. slowly. Insol. in organic solvents. (Olsson.) Lead tungstocyanide, Pb 2 W(CN) 8 +4H 2 O. Sol. in H 2 O. Solution decomp. after short time. Insol. in organic solvents. (Olsson.) Magnesium tungstocyanide, Mg 2 W(CN) 8 -f 6H 2 0. Easily sol. in H 2 O. Aqueous solution decomp. on heating. Insol. in organic solvents. (Olsson.) Manganous tungstocyanide, Mn 2 W(CN) 8 + iganou 8H 2 O. Insol. in H 2 O and in acids. Insol. in organic solvents. (Olsson.) 1098 TUNGSTOCYANIDE, POTASSIUM Potassium tungstocyanide, K 4 W(CN) 8 + 2H 2 O. Easily sol. in H 2 O from which it can be cryst. 10 ccm. H 2 O dissolve 13-14 g. salt at 18. Insol. in alcohol, ether and other organic solvents. (Olsson.) Rubidium tungstocyanide, Rb 4 W(CN) 8 + 3H 2 O. Easily sol. in H 2 O. Can be cryst. from H 2 O. Insol. in alcohol and other organic solvents. (Olsson.) Silver tungstocyanide, Ag 4 W(CN) 8 . Insol. in H 2 O. Insol. in acids. Decomp. by dil. HC1. Sol. in hot cone. hH 4 OH+Aq. Insol. in organic solvents. (Olsson.) Sodium tungstocyanide, Na 4 W(CN) 8 + Hydroscopic. Easily sol. in H 2 O. Insol. in organic solvents. (Olsson.) Strontium tungstocyanide, Sr 2 W(CN) 8 + 8H 2 O, +9H 2 O. Easily sol. in H 2 O. Aqueous solution de- comp. on standing. Insol. in organic solvents. (Olsson.) Thallium tungstocyanide, T1 4 W(CN) 8 . Difficultly sol. in cold H 2 O, more sol. in hot H 2 O. Insol. in organic solvents. (Olsson.) Zinc tungstocyanide, Zn ? W(CN) 8 +4H 2 O. Insol. in H 2 O, and acids. Sol. in cone. NH 4 OH+Aq. (Olsson.) Metotungstoiodic acid. Ammonium wetotungstoiodate, 2(NH 4 ) 2 O, 2I 2 O 6 , 4WO 3 +12H 2 O. Very si. sol. in H 2 O. (Chretien, A. ch. 5, (7) 15. 431.) Potassium tungstoiodate, K 2 H 3 WIO 8 . (Blomstrand, J. pr. (2) 40. 327.) 2K 2 O, 2I 2 O 6 , 4WO 3 +8H 2 O. 5.13 g. are sol. in 1 1. H 2 O at 15; 8.25 g. at 100. (Chretien, A. ch. 1898, (7) 16. 431.) Tungstoperiodic acid. Ammonium sodium tungstoperiodate, 2(NH 4 ) 2 O, Na 2 O, I 2 7 , 2WO 3 +16H 2 O. Ppt. (Rosenheim, A. 1899, 308. 64.) Barium tungstoperiodate, 5BaO, I 2 O 7 , 12WO 3 +12H 2 0. Ppt. (Rosenheim.) Potassium tungstoperiodate, 5K 2 O, I 2 O 7 , 12WO 3 +8H 2 O. Sol. in H 2 O. (Rosenheim.) Sodium tungstoperiodate, 3Na 2 O, I 2 O 7 , 2WO 3 +4H 2 O. Ppt. 5Na 2 O. I 2 O 7 , 12WO 3 +16H 2 O. Sol. in H 2 O. (Rosenheim.) Strontium tungstoperiodate, 5SrO, I 2 7 , 12W0 3 +28H 2 0. Sol. in H 2 O. (Rosenheim.) Tungstophosphoric acid, See Phosphotungstic acid. Tungstosilicic acid, See Silicotungstic acid. Tungstotungstic acid. Lithium tungstotungstate, Li 2 O, WO 8 + WO 2 , 3WO 3 . Insol. in boiling H 2 O and cone. HC1. (Hallopeau, C. R. 1898, 127. 514.) Potassium tungstotungstate, K 2 O, WO 3 + W0 2 , 3W0 3 . Insol. in hot H 2 O, and cone. HC1. (Hallo- peau, Bull. Soc. 1899, (3) 21. 267.) Tungstous acid. Sodium tungstite, Na 2 W 2 5 . See Tungstate tungsten oxide, sodium. Tungstovanadic acid. See Vanadiotungstic acid. Tungstyl dibromide, WO 2 Br 2 . Not decomp. by cold H 2 O. (Roscoe.) Tungstyl ^rabromide, WOBr 4 . Extremely deliquescent. Decomposes at once in moist air or with H 2 O. Tungstyl bichloride, WO 2 C1 2 . Not decomp. by cold, and but slowly by boiling H 2 O.. Sol. in alkalies and ammonia. Tungstyl ^rachloride, WOC1 4 . Easily decomp. by H 2 O or moist air. Very sol. in CS 2 and S 2 C1 2 . SI. sol. in ben- zene. (Smith, J. Am. Chem. Soc. 1899, 21. 1008.) Tungstyl ^rafluoride, WOF 4 . Sol. in H 2 O with decomp. Very hydro- scopic. Insol. in carbon tetrachloride. URANATE, POTASSIUM 1099 SI. sol. in carbon bisulphide, dry benzene and ether. Easily sol. in chloroform and absolute alcohol. (Ruff, Z. anorg. 1907, 62. 265.) Tungstyl teirafluoride ammonia, 2WOF 4 , NH 3 . Sol. in H 2 O with decomp. Insol. in liquid NH 3 . (Ruff, Z. anorg 1907, 52. 266,) Ultramarine blue, 2Na 2 Al 2 Si 2 O 8 , Na 2 S 2 (?) Not attacked by solutions of alkalies or NH 4 OH+Aq. Decomp. by acids or acid salts +Aq. Decomp. by alum+Aq. Ultramarine green, Na 2 Al 2 Si 2 O 8 , Na 2 S (?). Decomp. by mineral aqids. Not attacked by alkalies. Decomp. by alum +Aq. Ultramarine white, 2Na 2 Al 2 Si 2 O 8 , Na 2 S (?). Uranic acid, H 2 UO 4 . Insol. in H 2 O. Sol. in acids. Very sol. in cold dil. HNO 3 +Aq. SI. sol. in boiling NH 4 Cl+Aq. Insol. in KOH, NaOH, or NH 4 OH+Aq. Easily sol. in (NH 4 ) 2 CO 3 , KHCO 3 , and NaHCO 3 +Aq; less in K 2 CO 3 + Aq. (Ebelmen.) Easily sol. in malic and tartaric acids to form complex compds. (Itzisr, B. 1901, 34. 3822.) H 4 UO 5 . Insol. in H 2 O; sol. in acids. (Ebelmen.) Uranates. Insol. in H 2 O; sol. in acids. Ammonium uranate. SI. sol. in pure H 2 O; insol. in H 2 O contain- ing NH 4 C1 or NH 4 OH. Sol. in (NH 4 ) 2 CO 3 +Aq. (Peligot, A. ch. (3) 6. 11.) (NH 4 ) 2 O, 4UO 3 +7H 2 O. (Grubler, Dis- sert, 1908.) (NH 4 ) 2 O, 6UO 3 + 10H 2 O. Insol. in cold and hot H 2 O and alkalies +Aq. Very sol. in H 2 SO 4 , HC1 and acetic acid +Aq. (Zehenter, M. 1900, 21. 235.) Barium uranate, BaU0 4 . Insol. in H 2 O. Sol. in dil. acids. BaU 2 O 7 . As above. (Ditte, C. R. 95. 988.) BaU 3 Oio+4^H 2 O. Nearly insol. in H 2 O, KOH+Aq. and alcohol. Easily sol. in cold dil. HC1 or HNO 3 and in hot acetic acid. (Zehenter, M. 1904, 26. 200.) Ba 2 U 6 Oi 7 +8H 2 O. Nearly insol. in hot or cold H 2 O, KOH+Aq. and alcohol. Easily sol, in cold dil. HC1 or HNO 3 and in hot acetic acid. (Zehenter.) Ba 2 U 7 O 23 + llH 2 O. Same properties as BaU 3 O 10 . (Zehenter.) Bismuth uranate, Bi 2 O 3 , UO 3 -f-H 2 O. Min. Uranosphaerite. Calcium uranate, CaUO 4 . Insol. in H 2 O; sol. in dil. acids. (Ditte, C. R. 96. 988.) CaU 2 O 7 . Insol. in H 2 O; sol. in dil. acids (Ditte.) Cobalt uranate. Insol. in H 2 O; sol. in Pb(C 2 H 3 O 2 ) 2 -|-Aq. (Persoz, J. pr. 3. 216.) Sol. in HNO 3 +Aq; insol. in KNO 3 +Aq. (Ebelmen, A. ch. (3) 5. 222.) Cupric uranate, CuU 2 O 7 . Insol. in H 2 O. (Debray, A. ch. (3) 61. 451.) Lead uranate, PbUO 4 . If ignited, very difficultly sol. in HC 2 H 3 O 2 + Aq. (Wertheim, J. pr. 29. 228.) Insol. in Pb(C 2 H 3 O 2 ) 2 +Aq. (Persoz.) 3PbO, 2UO 3 . Sol. in dil. HNO 3 +Aq. (Ditte, A. ch. (6) 1. 338.) PbU 3 Oio. Insol. in H 2 O. Sol. in HNO 3 Insol. in KOH+Aq, NH 4 OH and cold acetic acid. Sol. in hot acetic acid. (Zehen- ter, M. 1904, 25. 215.) Pb 4 U 6 O 19 +4H 2 O. Insol. in hot or cold H 2 O. Sol. in HNO 3 . Insol. in KOH+Aq, NH 4 OH, alcohol and ether. SI. sol. in cola, more easily sol. in hot acetic acid. (Zehenter.) Lithium uranate, Li 2 UO 4 . Insol. in H 2 O', but decomp. thereby. Sol. n dil. acids. Magnesium uranate, MgUO 4 . Insol. in H 2 O. Nearly insol. in cold HC1 + Aq. Slowly sol. in HCl+Aq on warming, and more rapidly by addition of a little HNO 3 +Aq. (Ditte.) MgU 2 O 7 . Ppt. (Berzelius.) Neodymium uranate, Nd 2 (U 3 Oio) 3 +18H 2 O. Ppt. (Orloff, Ch. Z. 1907', 31. 1119.) Potassium uranate, K 2 UO 4 (?). Insol. in H 2 O; sol. in dil. acids, etc., exactly as Na 2 UO 4 . (Ditte.) K 2 U 2 O 7 +6H 2 O. Insol. in H 2 O. Sol. in dil. acids, even acetic acid. (Zimmermann, B. 14. 440.) Insol. in K 2 CO 3 +Aq. but easily sol. in alkali hydrogen carbonates +Aq. Sol. in HCl+Aq. (Ebelmen, A. ch. (3) 6. 220.) K 2 O, 4UO 3 +5H 2 O. (Zehenter, M. 1900, 21. 235.) K 2 O, 6UO 3 +6H 2 O. Insol.. in H 2 O. Drenckmann, Zeit. ges. Nat. 17. 113.) + 10H 2 O. Nearly insol. in cold and hot :E 2 O. Easily sol. in hot acetic acid, dil. H 2 SO 4 HC1 and HNO 3 . Insol. in KOH+Aq, alco- 10! and ether. ((Zehenter, M. 1900, 21. 235.) 1100 URANATE, POTASSIUM HYDROXYLAMINE Potassium hydroxylamine uranate, UO 4 (NH 4 O)(NH 3 OK) +H 2 O. SI. sol. in H 2 O ; insol. in alcohol. (Hofmann, A. 1899, 307. 318.) Rubidium uranate, RbUO 4 . Insol. in H 2 O. (Ditte,. A. ch. (6) 1. 338.) Silver uranate, Ag 2 U 2 O 7 . Insol. in H 2 O. Easily sol. in acids. (Alibe- goff, A. 233. 117.) Sodium uranate, Na 2 UO 4 (?). Insol. in H 2 O; sol. in dil. acids. Sol. in alkali carbonates +Aq. (Ditte.) Na 2 U 2 O 7 +6H 2 O. Insol. in H 2 O. Sol. in dil. acids. (Stolba, Z. anal. 3. 74.) Na 2 O, 3UO 3 . Insol. in H 2 0. Easily sol. in very dil. acids. (Drenckmann.) Na 2 O, 5UO 3 +5H 2 O. Insol. in H 2 O, alco- hol, NH 4 OH. KOH+Aq. Sol. in HC1, HNO 3 , H 2 SO 4 . SI. sol. even on boiling in cone, acetic acid. (Zehenter, M. 1900, 21. 235.) Sodium hydroxylamine uranate, UO 4 (NH 4 O)(NH 3 ONa) +H 2 O. Sol. in H 2 O. (Hofmann, A. 1899, 307. 319.) UO 4 (NH 3 ONa) 2 +6H 2 O. Very sol. in H 2 O. (Hofmann.) Strontium uranate, SrUO 4 . Insol. in H 2 O. Sol. in dil. acids. SrU 2 O 7 . As above. (Ditte, C. R. 96. 988.) Very si. sol. in H 2 O. Sol. in all acids especially oxalic. +H 2 O. Very si. sol. in H 2 O. Sol. in all acids especially oxalic. (J, C. C. 1896, II. 512.) Thallous uranate. Ppt. (Bolton, Am. Chemist, 1872, 2. 456.) Zinc uranate. Insol. in H 2 O; sol. in Pb(C 2 H 3 O 2 ) 2 +Aq. (Persoz, J. pr. 3. 216.) Sol. in HNO 3 +Aq; insol. in KNO 3 , and NH 4 NO 3 +Aq. (Ebel- men. A. ch. (3)6.221.) Pmiranic acid. See Peruranic acid. Uranium, U. Not attacked by H 2 O. Slowly decomp. by cold dil. H 2 SO 4 +Aq, rapidly on warming. Easily sol. in dil. or cone. HCl+Aq. Fused U is slightly attacked by cone, or fuming HNO 3 , or cone. H 2 SO 4 . Amorphous U, how- ever, is easily attacked thereby. Not at- tacked by acetic acid, KOH, NaOH, or NH 4 OH+Aq. (Zimmermann, B. 16. 849.) When finely divided, it is decomp. by H 2 O slowly at ordinary temps, and rapidly at 100. (Moissan, C. R. 1896, 122. 1091.) Uranium antimonide, U 3 Sb 2 . Violently attacked by cone. HNO 3 . (Co- lani, C. R. 1903, 137. 383.) Uranium arsenide, U 3 As 2 . Violently attacked by cone. HNO 3 . (Co- ani, C. R. 1903 137. 383.) Uranium boride, UB 2 . Sol. in HNO 3 and HF. Deiomp. by fused alkalies. (Wedekind, B. 1913, 46. 1204.) Uranium ^n'bromide, UBr 3 . Very hygroscopic. Sol. in H 2 O with hiss- ing. (Alibegoff, A. 233. 117.) Uranium terabromide, UBr 4 . Anhydrous. Very deliquescent. Sol. in H2O with hissing. (Hermann.) Insol. in alcohol, (v. Unruh, Dissert, 1909.) Sol. in acetone. (Eidmann. C. C. 1899, II. 1014); methyl acetate (Naumann, B. 1909, 42. 3790); ethyl acetate. (Naumann, B. 1904, 37. 3601.) +8H 2 O. Very deliquescent, and sol. in H.O. (Rammelsberg.) Uranium carbide, UC 2 . (Ruff and Heinzelmann, Z. anorg. 1911, 71. 72.) Attacked slowly by H 2 O. Slowly attacked by cold dil. HC1, H 2 SO 4 or HNO 3 +Aq. Cone, acids, except HNO 3 , react si. in the cold, violently on heating. (Moissan, Bull. Soc. 1897, (3) 17. 12.) Sol. in fused KNO 3 and KC1O 3 ; sol. in dil. acids in the cold and in cone, acids on heating; decomp. by H 2 O. (Moissan, C. R. 1896, 122. 276.) Uranium /nchloride, UC1 3 . Very sol. in H 2 O. (Peligot.) Very unstable. (Zimmermann.) Very hygroscopic. Sol. in H 2 O with de- comp. Sol. in cone. HC1 and solution is much more stable than aqueous one. (Rosen- heim and Loebel, Z. anorg. 1908, 57. 234.) Uranium te^rachloride, UC1 4 . Anhydrous. Extremely deliquescent. Sol. in H 2 O with evolution of heat. De- comp. on boiling. Sol. in NH 4 Cl+Aq with- out decomp. HC1 increases its solubility in H 2 O. (Aloy, Dissert. 1901.) Sol. in alcohol, acetone, acetic ether, ben- zoic ether. Insol. in ether, CHC1 and C 6 H 6 . (Loebel.) Sol. in ethyl acetate. (Naumann, B. 1904, 37. 3601.) Uranium pentochloride, UC1 5 . Deliquescent. Sol. in H 2 O with evolution of heat and decomposition. .Roscoe, B. 7. 1131.) URANOURANIC OXIDE 1101 Sol. in acetic acid, acetic ether, benzalde- hyde, glycerine, benzyl alcohol (trace), nitrobenzene (trace), xylidine and p-toluidine (on warming). Insol. in aniline, ligroin, pyridine, quinoline, thioethyl ether, thioamyi ether and CS 2 (Pimmer, Dissert. 1904.) Sol. in abs. alcohol. Insol. in ether, C 6 H 6 , nitrobenzene, ethylene bromide. SI. sol. in CC1 4 and CHC1 3 . Sol. in benzoic ethsr, acetone and trichloracetic acid. Best solvents are ethyl acetate and benzonitrile. Sol. in many organic compounds containing oxygen. (Loebel, Dissert. 1907.) Uranium ^'fluoride, UF 2 +2H 2 O. Ppt (Giolitti and Agamennone, C. C. 1905, I. 1130.) Uranium tefrafluoride, UF 4 . Insol. in H 2 O. Very si. sol. in dil. acids. Sol. in hot cone. HaSO-t, and slowly in warm cone. HNO 3 +Aq. (Bolton, J. B. 1866. 209.) Uranium Aezafluoride, UF 6 . Very sol. in H 2 O. (Ditte, A. ch. (6) 1. 339.) Fumes in the air. Very hydros^opic; sol. in H 2 O. (Ruff, B. 1909, 42/495.) Very hygrosoopic. Sol. in H 2 O. Nearly insol. in CS 2 . Insol. in paraffine oil. Sol. in symmetrical tetrachlorethane (best solvent), CHC1 3 , CC1 4 , and nitrobenzene, (v. Unruh, Dissert. 1909.) Decomp v by H 2 O, alcohol and ether. Nearly insol. in CS 2 . Sol. in CHC1 3 , CC1 4 , nit obenzene and C 2 H 2 C1 4 . (Ruff, Z. anorg. 1911, 72. 81.) Uranium hydrogen fluoride, UF 6 , 8HF (?). Sol. in H 2 O. (Ditte.) Is U0 2 F 2 , HF+H 2 0. (SmitheUs ) Uranous hydroxide, UO 2 , zH 2 O. Easily sol. in dil. acids. Insol. in alkali hydrates and carbonates +Aq. (Berzelius.) Sol. in alkali carbonates +Aq. (Rammels- berg.) U(OH) 4 . Sol. in dil. acids. (Aloy, Bull. Soc. 1899, (3) 21. 613.) Uranouranic hydroxide, U 3 O 8 , 6H 2 O (?). Easily sol. in acids. Decomp. by (NH 4 ) 2 CO 3 +Aq, which dis- solves out UO 3 . (Berzelius.) Uranic hydroxide. See Uranic acid. Uranium te^raiodide, UI 4 . Sol. in H 2 O. (Guichard, C. R. 1907, 145. 921.) Uranium iodide. Sol. in ethyl acetate.. (Naumann. B. 1904 37. 3601.) Uranium nitride, U 3 N 4 . (Colani, C. R. 1903. 137. 383.) Uranium sw&oxide, UO (?). (Guyard, Bull. Soc. (2) 1. 89.) Does not exist. (Zimmermann, A. 213. 301.) U 2 O 3 (?). Ppt. Decomp. by H 2 and in the air. (Peligot.) Uranium dioxide (Uranous oxide), UO 2 . Insol. in dil. HC1 or H 2 SO 4 +Aq. Sol. in cone. H 2 SO 4 , and easily in HNO 3 + Aq. (Peligot.) Insol. in NH 4 Cl+Aq. (Rose.) Only si. sol. in H 2 SO 4 , but a considerable amount is converted into the sulphate which is nearly insol. in H 2 SO 4 . Slowly sol. in HC1, the amount dissolved in a given time varying widely with the method of preparation of the oxide. (Colani, C. R. 1912,, 155. 1251.) SI. more sol. in HNO 3 than in aqua regia. (Raynaud, Bull. Soc. 1912, (4) 11. 802.) Very sol. in cone. HNO 3 ; less sol. in dil. HNO 3 . 1 gram is sol. in 3100 grams HC1 (1.17) at 17; 4650 grams HBr(1.52) at 17; 2200 grams H 2 SO 4 (1.79) at 17; 12,000 grams acetic acid at 19. (Raynaud, C. R. 1911, 153. 1481.) SI. attacked by liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) Min. Uraninite. Easily sol. in warm HNO 3 +Aq. Not attacked V HCl+Aq. Uranium dioxide (Uranic oxide), UO 3 . Sol. in HNO 3 +Aq. (Peligot.) Insol. in boiling K tartrate +Aq. (Kah- lenberg and Hijlyer, Am. Ch. J. 1894, 16. 102.) Sol. in oleic acid. (Gibbons, Arch. Pharm. 1883, 221. 621.) See Uranic acid. Uranium te.!roxide, UO 4 . Decomp. by HCl+Aq. (Fairley, Chem. Soc. 31. 133.) -f 2H 2 O. Very hygroscopic. (Zimmer- mann.) +3H 2 O. Uranium pentoxide, U 2 O 6 . Sol. in acids. (Peligot.) Mixture of UO 3 and U 3 O 8 . (Ramrnels- berg, Pogg. 59. 5.) Mixture of UO 2 and U 3 O 8 . (Zimmermann, A. 232. 273.) Uranouranic oxide, U 3 O 8 . Green uranium oxide. Very slowly and slightly sol. in dil. HC1 or H 2 SO 4 +Aq; more easily when cone. Completely sol. in boil- ing H 2 SO 4 . Easily sol. in HNO 3 +Aq. 1102 URANOUS OXYCHLORIDE Uranous oxychloride, U0 2 , UC1 4 +H 2 O. Moderately sol. in H 2 O. (Aloy, Dissert. 1901.) 2U0 2 , UC1 4 +H 2 0. Very sol. in H 2 and alcohol. (Orloff, C. C. 1903, II. 484.; + 13H 2 O. Very sol. in H 2 O and alcohol (Orloff.) 4UO 2 , UC1 4 . Very sol. in H 2 O and alcohol (Orloff.) 5UO 2 , UC1 4 + 10H 2 O. Insol. in H 2 O (Aloy, Dissert, 1901.) Uranous oxyfluoride, UOF 2 +2H 2 O. (Giolitti and Agamennone, C. C. 1905, I 1130.) Uranous oxysulphide, U 3 O 2 S 4 =U0 2 , 2US 2 . Slightly attacked by dil., easily by cone. HCl+Aq. Sol. in cold HNO 3 +Aq. (Her- mann, J. B. 1861. 258.) Uranic oxy-compounds. See Uranyl compounds. Uranium phosphide, U 3 P 2 . Violently attacked by cone. HNO 3 . (Colani, C. R. 1903, 137. 383.) U 3 P 4 . Slowly attacked by H 2 O, not by dil. HCl+Aq. More easily attacked by cone. HCl+Aq. Quickly decomp. by boil- ing cone. HNO 3 and HNOs+HCl. (Colani, A. ch. 1907, (8) 12. 59.) Uranium selenide, USe. Spontaneously inflammable. Sol. in fum- ing HNO 3 . (Colani. C. R. 1903, 137. 383.) USe 2 . As US 2 . (Colani. C. C. 1903, II. 707.) U 2 Se 3 . (Colani.) Uranium cKsilicide, USi 2 . Sol. in cold or hot cone. HF; insol. in HC1, HNO 3 , H 2 SO 4 and aqua regia. (Defacqz, C. R. 1908, 147. 1051.) Uranium monosulphide, US. (Alibegoff, A. 233. 117.) Uranium sesgwsulphide, U 2 S 3 . Not attacked by HC1 or dil. HNO 3 +Aq. Oxidised by fuming H 2 SO 4 or aqua regia. (Alibegoff, A. 233. 117.) Uranium cfo'sulphide, US 2 . Insol. in cold or boiling dil. HCl+Aq. Sol. in cold cone. HCl+Aq. Decomp. by HNO 3 +Aq. (Hermann. J. B. 1861. 258.) Uranium telluride, U 4 Te 3 . Violently attacked by cone. HNO 3 . (Colani, C. R. 1903, 137. 383.) Uranosotungstic acid. Potassium uranosotungstate, 9K 2 O, 6UO 2 , 8WO 3 +34H 2 O. Insol. in H 2 O and in HC1. (Gibbs, Am. Ch. J. 1895, 17. 175.) Sodium uranosotungstate, 12Na 2 O, 6U0 2 , 8WO 3 +25H 2 O. Insol. in cold H 2 O. (Gibbs.) Uranyl bromide, UO 2 Br 2 . Sol. in H 2 O. (de Coninck, C. C. 1903, I. 693.) Sol. in ether, (v. Unruh, Dissert. 1909.) +7H 2 O. Deliquescent. Sol. in H 2 O. Uranyl bromide ammonia, UO 2 Br 2 , 2NH 8 . (v. Unruh, Dissert. 1909.) UO 2 Br 2 , 3NH 3 . (v. Unruh.) UO 2 Br 2 , 4NH 3 . (v. Unruh.) Uranyl chloride, UO 2 C1 2 . Anhydrous. Very deliquescent. Sol. in H 2 O, alcohol, and ether. Very sol. in H 2 O. Sp. gr. of UO 2 Cl 2 +Aq at t. t % U0 2 C1 2 Sp. gr. 14.6 1 1.0056 16.3 2 1.0112 13.7 3 1.0161 13.1 4 1.0215 14.2 5 1.0260 15.2 6 1.0313 14.3 7 1.0366 14.5 8 1.0418 15.0 9 1.0469 14.8 10 1.0517 (de Coninck, A. ch. 1904, (8) 3. 500.) Sol. in cone. HC1, cone. HNO 3 and in selenic acid. Decomp. by H 2 SO 4 . (de Coninck. A. ch. 1904, (8) 3. 504.) Sol. in methyl acetate (Naumann, B. 1909, 42. 3790) ; acetone. (Naumann, B. 1904, 37. 4328.) +H 2 O. Sol. in H 2 O, alcohol, and ether. +3H 2 O. Deliquescent. Very sol. in H 2 O. 1 pt. is sol. in 0.134 pts. H 2 O at 18 and solution, which is saturated, contains 76.2% UO 2 C1 2 or 88.2% UO 2 C1 2 + 3H 2 O. Sp. gr. of solution = 2.740. The solubility increases with rise in temp. Sol. in alcohol and in ether. (Mylius and Dietz, B. 1901, 34. 2775.) Uranyl hydrogen chloride,. UO 2 C1 2 , HC1+ 2H 2 O. Cryst. at - 10 from sat. solution of UO 2 C1 2 n HCl+Aq. VANADATE, AMMONIUM 1103 Fumes in the air. (Aloy, Bull. Soc. 1901, (3) 25. 154.) Uranyl chloride ammonia, U0 2 (NH 3 C1) 2 . Decomp. by H 2 O. (Regelsberger, A. 227. 119.) UO 2 (NH 3 .NH 3 C1)NH 3 C1. Decomp. by H 2 O. (Regelsberger.) UO 2 (NH 3 .NH 3 C1) 2 . Decomp. by H 2 O. (Regelsberger.) Uranyl fluoride, UO 2 F 2 . Very sol. in H 2 O. (Smithells, Chem. Soc. 43. 125.) Insol. in H 2 O or dil. acids. Very si. sol. in HF+Aq. Sol.inH 2 SO 4 +aquaregia. (Ditte, A. ch. (6) 1. 339.) Insol. in ether and amyl alcohol. (v. Unruh, Dissert, 1909.) UOF 4 . Very sol. in H 2 O. (Ditte, C. R. 91. 115.) True composition is U0 2 F 2 . (Smithells.) Uranyl hydrogen fluoride, UO 2 F 2 , HF+H 2 O. Very sol. in H 2 O. (Smithells, Chem. Soc. 43. 131.) Uranyl fluoride ammonia, UO 2 F 2 , 2NH 8 . (v. Unruh, Dissert. 1909.) UO 2 F 2 , 3NH 3 . (v. Unruh.) UO 2 F 2 , 4NH 3 . (v. Unruh.) Uranyl iodide, UO 2 I 2 . Ppt. Deliquescent. (Aloy, A. ch. 1910, (7) 24. 417.) Deliquescent. Sol. in alcohol, ether and benzene. (Aloy, Dissert. 1901.) - uy Sol. in acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328); methyl acetate. (Naumann, B. 1909, 42. 3790.) Uranyl iodide ammonia, U0 2 I 2 , 2NH 3 . (Aloy, Dissert. 1901.) UO 2 I 2 , 3NH 3 . (Aloy.) UO 2 I 2 , 4NH 3 . (Aloy.) Uranyl selenide, UO 2 Se. Very slowly decomp. by H 2 O. Easily sol. in cold HC1. Violently attacked by cold HNO 3 . Not attacked by dil. alkalies. (Milbauer, Z. anorg. 1904, 42. 450.) Uranyl sulphide, UO 2 S. SI. sol. in pure H 2 O. Sol. in dil., insol. in absolute alcohol. Sol. in cone. HCl+Aq, also in dil. acids. Decomp. by caustic al- kalies +Aq. . Partly sol. in (NH 4 ) 2 S+Aq. Afetavanadic acid, HVO 3 . Insol. in H 2 O; sol. in acids and alkalies. Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) See Vanadium pentoxide. Pyrovanadic acid, H4V 2 O 7 . Insol. in H 2 O. Sol. in acids and alkalies. Vanadates. The alkali, Ba, and Pb metavanadates are si. sol. in H 2 O, the others are more easily sol. Insol. in alcohol. Aluminum we.'avanadate. Very si. sol. in H 2 O. (Berzelius.) Aluminum cfo'vanadate. Very si. sol. in H 2 O. (Berzelius.) Ammonium rae/avanadate, (NH 4 )V0 3 . (a) Very slowly and sparingly sol. in cold H 2 O. Easily sol. in hot H 2 0. (Berzelius.) Easily sol. in H 2 O at about 70. Very si. sol. at above and below that temperature. (Guyard, Bull. Soc. (2) 25. 355.) 10 g. dissolve in 1 litre cold, and 63 g. in 1 litre hot H 2 O with partial decomp. (Ditte, C. R. 102. 918.) Solubility in H 2 O at t. t Solubility, mol. per litre 18 0.03715 25 0.05189 35 0.08980 45 0.13406 55 0.17041 70 0.25994 (Meyer, Z. Elektrochem, 1909, 16. 266.) Solubility in NH 4 OH+Aq at t. NH 4 OH+Aq t Solubility, mol. per litre 0.0677-N 0.2452-N 0.5872-N 18 0.04763 0.06798 0.1029 0.0677-N 0.2452-N 0.5872-N 25 0.06026 0.07303 0.1080 (Meyer, Z. Elektrochem, 1909, 15. 268.) Extremely si. sol. in sat. NH 4 Cl+Aq. (v. Hauer.) Insol. in sat. NH 4 Cl+Aq. 1104 VANADATE, AMMONIUM Solubility in salts +Aq at t. HVO 3 , 3NH 3 O, 2NH 3 = VO 6 N 5 H 16 . Rap- idly decomp. by H 2 O. (Hofmann and Kohlschutter.) Ammonium potassium vanadate, K 2 V 4 O n , (NH 4 ) 4 V 6 17 +9H 2 0. Sol. in H 2 O. (Ditte, C. R. 104. 1844.) Ammonium sodium vanadate, Na 2 V 4 O n , (NH 4 ) 4 V e 17 + 15H 2 0. Sol. in H 2 O. (Ditte, C. R. 104. 1841.) Ammonium uranyl vanadate, (NH 4 ) 2 O, 2UO 3 , V 2 5 +H 2 0. Insol. in H 2 O, NH 4 OH+Aq, or dil. HO 2 H 3 O 2 +Aq. (Carnot, C. R. 104. 1850.) Barium raetavanadate, Ba(VO 3 ) 2 +H 2 O. Somewhat sol. in H 2 O before ignition Sol. in cone. H 2 SO 4 . (Berzelius.) Salt solution t Solubility, mol. per litre 0.05-NNH 4 Cl+Aq 18 25 35 45 55 0.01419 0.02246 0.04445 0.07575 0.09544 0.1-NNH 4 Cl+Aq 18 25 85 45 55 0.00356 0.00995 0.02347 0.04507 0.06314 0.05-NNH 4 NO 3 +Aq 18 25 0.01433 0.02364 0.1-NNH 4 N0 3 +Aq 18 25 0.00497 0.01050 (Meyer, Z. Elektrochem, 1909, 16. 267.) Insol. in alcohol, (v. Hauer.) (6) Sol. in cold H 2 O, from which it is pptd. by alcohol. (Berzelius.) Ammonium ^vanadate, (NH 4 ) 2 V 4 On+4H 2 0. Sol. in H 2 O, from which it is precipitated by sat. NH 4 Cl+Aq or alcohol, (v. Hauer, W. A. B. 21. 337.) Correct formula is "(NH 4 ) 3 V 7 G,o+2H 2 O, accorcling to Rammelsberg (B. A. B. 1883. 3.) +3H 2 O. Very sol. in H 2 O. (Ditte, C. R. 102. 918.) Ammonium rfn'vanadate, (NH 4 ) 2 V 6 Oi 6 . Anhydrous. Nearly insol. in hot or cold H 2 O. (Norblad,B. 8. 126.) 1.5 g. dissolve in 1 litre of boiling H 2 O (Ditte, C. R. 102. 918.) +5H 2 O. Very si. sol. in H 2 O. (Ditte.) +6H 2 O (?). Very sol. in H 2 0. (v. Hauer, W. A. B. 39. 455.) Could not be obtained. (Norblad: also Rammelsberg, B. A. B. 1883. 3.) Ammonium vanadate, (NH 4 ) 3 V 7 Oi +2H 2 O. Correct formula of v. Hauer's ^vanadate, according to Rammelsberg (B. A. B, 1883. 3) SI. sol. in H 2 O. Ammonium sesgiuvanadate, (NH 4 ) 4 V 6 On+ 4 or 6H 2 O. Very sol. in H 2 O. (Ditte, C. R. 102. 918.) Ammonium penta vanadate, (NH 4 ) 4 Vi O 27 + 10H 2 O. Sol. in H 2 O. (Rammelsberg, B. A. B. 1883. 3.) Ammonium hydroxylamine vanadate. V0 6 N 3 H 10 . Rapidly decomp. by H 2 O. (Hofmann and Kohlschutter, Z. anorg. 1898, 16. 472.) Barium pyro vanadate, Ba 2 V 2 O 7 . Somewhat sol. in H 2 O. (Roscoe.) Barium vanadate, Ba 2 V 6 Oi 7 +14H 2 O. (Ditte, C. R. 104. 1705.) Ba 3 VioO 28 + 19H 2 O. 1 pt. is sol. in 5200 pts. H 2 O at 20-25. Much more sol. in hot, but decomp. by boiling H 2 O. (v. Hauer, W. A. B. 21. 344.) Sol. in about 5000 pts. H 2 O. (Manasse, C. C. 1886. 773.) Ba 4 VioO 29 +2H 2 O. (Norblad.) Bismuth vanadate, Bi,2(VO 4 ) 2 . Min. Pucherite. Sol. in HCl+Aq with evolution of Cl. Cadmium vanadate, Cd(VO 3 ) 2 . (Ditte, C. R. 102. 918.) CdV 6 O 16 +24H 2 O. SI. sol. in H 2 O. (Ditte, C. R. 104. 1705.) Cadmium potassium vanadate, CdK 2 V 6 Oi 7 + +9H 2 O. (Radau, A. 251. 148.) Cd 3 yioO 28 , K 6 Vi O 28 +27H 2 O. 1000 pts. H 2 O dissolve 5.4 pts. at 18. (Radau.) Cadmium vanadate bromide, 3Cd 3 (VO 4 ) 2 , CdBr 2 . Very sol. in dil. acids, (de Schulten, Bull. Soc. 1900, (3) 23. 160.) Cadmium vanadate chloride, 3Cd 3 (VO 4 ) 2 , CdCl 2 . Very sol. in dil. acids, (de Schulten, Bull. Soc. 1900, (3) 23. 159.) Caesium raetavanadate, CsVO 3 . (Chabrie", A. ch. 1902, (7) 26. 228.) VANADATE, LEAD ZINC 1105 Calcium wetavanadate, Ca(VO 3 ) 2 +4H 2 O. Much more sol. than Sr(VO 3 ) 2 , and solu tion is not precipitated by alcohol. (Ber zelius.) +3H 2 O. Sol. in H 2 O 2 ; insol. in alcohol (Scheuer, Z. anorg. 1898, 16. 304.) Calcium p^/rovanadate, Ca 2 V 2 O 7 +5H 2 O. Precipitate. +2H 2 O. Very sol. in dil. acids. (Ditte C. R. 104. 1705.) +2^H 2 O. (Roscoe.) Calcium eftvanadate, CaV 4 On+9H 2 O. Easily sol. in H 2 O. (v. Hauer.) When fused is nearly insol. in H 2 O. (v. Hauer.) +6H 2 O. (Manasse, A. 240. 23.) Calcium frivanadate, CaV 6 Oi 7 + 12H 2 O. Very sol. in H 2 O. (Ditte, C. R. 104. 1705.) Calcium vanadate, Ca 3 V 8 O 23 +15H 2 O. Sol. in H 2 O. (Manasse, A. 204. 23.) Ca 3 V 14 O 38 +7H 2 O (?). SI. sol. in H 2 O. Probably a mixture. (Manasse, A. 240. 23.) Ca 3 Vi*8O43+26H 2 O. Sol. in H 2 O. (Man- asse, A. 240. 23.) Calcium copper vanadate, (Ca, Cu) 4 V 2 O 9 + H 2 O. Min. Volborthite. Sol. in HNO 3 +Aq. Calcium potassium vanadate. CaK 8 V 20 O 6 5 + 22H 2 0. Sol. in H 2 O. (Manasse, A. 240. 23.) Calcium vanadate chloride, Ca 3 (VO 4 ) 2 , CaCl 2 . (Hautefeuille, C. R. 77. 896.) Chromium vanadate, CrVO 4 . Absolutely insol. in H 2 O containing NH 4 C 2 H 3 O; and HC 2 H 3 O 2 . (Carnot, C. R. 104. 1850.) Cobaltous raetavanadate, Co(VO 3 ) 2 +3H 2 O. Easily sol. in H 2 O. (Ditte, C. R. 104. 1705.) Cobaltous potassium vanadate, CoKV 6 Oi 4 + +8H 2 O. 1000 pts. H 2 O dissolve 4.8 pts. of this salt. \ (Radau, A. 251. 140.) Co 3 K 2 Vi 4 O 39 +21H 2 O. (Radau.) Cupric wetavanadate. Sol. in H 2 O. (Berzelius.) Cupric p?/r0vanadate, Cu 2 V 2 O 7 +3H 2 O. Sol. in hot H 2 O. (Ditte, C. R. 104. 1705.) Could not be obtained. (Radau, A. 251. 150.) Cupric lead vanadate, 5(Cu. Pb)O. V 2 O 6 + 2H 2 O. Min. Mottramite. 3CuO, V 2 5 , 3(3PbO, V 2 5 ), 6CuO 2 H 2 + 12H 2 O. Min. Psittacinnite. Cupric potassium vanadate, CuKV 9 O 24 + 171*20. Moderately sol. in warm H 2 O. 100 pts. H 2 O dissolve 11.1 pts. at 18. (Radau, A. 251. 151.) Didymium vanadate, Di 2 (VO 4 ) 2 . Precipitate. (Cleve.) Di 2 Vi O 30 +28H 2 O. Precipitate. (Cleve, Bull. Soc. (2) 43. 365.) Glucinum metovanadate (?). Difficultly sol. in H 2 O. (Berzelius.) Glucinum cfo'vanadate (?). Difficultly sol. in H 2 O. (Berzelius.) Indium metovanadate, In(VO 3 ) 3 +2H 2 O. Ppt. (Renz,. Dissert. 1902.) Iron (ferrous) wetavanadate. Ppt. Sol. in HCl+Aq. (Berzelius.) Iron (ferric) wetovanadate. Somewhat sol. in H 2 O. (Berzelius.) Lead wefovanadate, Pb(VO 3 ) 2 . SI. sol. in H 2 O. Easily sol. in warm dil. HNO 3 +Aq. Not completely decomp. by H 2 SO 4 or by boiling with K 2 CO 3 +Aq/' (Ber- zelius.) Min. Dechenite. Easily sol. in dil. HNO 3 + Aq, and decomp. by HCl+Aq. Lead p?/rovanadate, basic, 2Pb 2 V 2 O 7 , PbO. Insol. in boiling H 2 O or HC 2 H 3 O 2 . De- comp. by HN0 3 +Aq with separation of V 2 O 5 , which dissolves on warming. (Roscoe.) Lead p?/rovanadate, Pb 2 V 2 O 7 . Sol. in warm dil. HNO 3 +Aq. (Ditte, C. R. 104. 1705.) Min. Descloizite. Sol. in cold dil. HNO 3 + Lead ^vanadate, PbV 4 On. (Ditte, C. R. 104. 1705.) Lead or^ovanadate, Pb 3 (VO 4 ) 2 . Insol. in H 2 O. (Roscoe,, A. suppl. 8. 109.) Lead zinc ortho vanadate, 4Pb 3 (VO 4 ) 2 , 3Zn 3 (V0 4 ) 2 . Min. Eusynchite. Easily sol. in HNO 3 + Aq. 1106 VANADATE, LEAD ZINC Lead zinc vanadate, (Pb, Zn) 4 V 2 O 9 +H 2 O. Min. Descloizite. Sol. in excess of HNO 3 + Aq. Lead vanadate chloride, SFb.fVO,),, PbCl 2 . Min. Vanadinite. Easily sol. in HNO 3 + Aq. Lithium vanadate, basic, Li 6 V 2 O 8 +6H 2 O. Sol. in H 2 O. (Ditte, C. R. 104. 1168.) Li 8 V 2 O s +H 2 O, and 14H 2 O. Sol. in H 2 O. (Ditte.) Lithium metovanadate, LiV0 8 . Easily sol. in H 2 O. (Berzelius.) +2H 2 O. Quite easily sol. in H 2 O. (Ram- melsberg, B. A. B. 1883. 3.) Lithium divanadate, Li 2 V4O n +9H 2 O. Very sol. in H 2 O. (Norblad.) Correct formula is Li 3 V 5 Oi 4 +12H 2 O. (Rammelsberg.) +8, or 12H 2 O. (Ditte, C. R. 104. 1168.) Lithium or^ovanadate, Li 3 VO 4 . Insol. in H 2 O. (Rammelsberg, B. A. B. -1.3.) Lithium p*/rovanadate, Li 4 V 2 O 7 -HH 2 O. Very sol. in H 2 O. (Rammelsberg, B. 16. 1676.) +3H 2 O. (Ditte, C. P. 104. 1168.) Lithium vanadate, Li 3 V6O 14 +7H 2 O. Difficultly sol. in H 2 O. (Rammelsberg.) + 12H 2 O. Very efflorescent. Correct for- mula for v. Hauer's cfo'vanadate. (Rammels- berg.) Li 4 V 6 O 17 + 16H 2 O. Sol. in H 2 O. (Ditte, C. R. 104. 1168.) + 15H 2 O. (Rammelsberg.) + 11H 2 0. (R.) +3H 2 O. (R.) Li 6 V 4 Oi3 + 15H 2 O. Not very easily sol. in H 2 O. (Rammelsberg.) Li 6 V 8 O 2 3 + 12H 2 . Moderately sol. in H 2 O. (Rammelsberg . ) Lii Vi 2 O 35 +30H 2 O. Efflorescent. Very sol. in H 2 O. (Rammelsberg.) Magnesium metovanadate, Mg(VO 3 ) 2 . Very easily sol. in H 2 O. (Berzelius.) +6H 2 O. Very sol. in H 2 O. (Ditte, C. R. 104. 1705.) lesium divanadate, MgV 4 O u +8H 2 O. Difficultly sol. in H 2 O, but much more sol. than barium di vanadate. (v. Hauer.) +9H 2 O. (Ditte, C. R. 104. 1705.) Magnesium fnvanadate, Mg 2 V 6 Oi 7 +4^H 2 O. Very si. sol. in H 2 O. (Manasse, A. 240. 23.) Magnesium vanadate, Mg 3 Vi O 28 +28H 2 O. Sol. in H 2 O. (Suguira and Baker, Chem. Soc. 35. 715.) M ous raetavanadate, Mn(VO 3 ) 2 + Very si. sol. in cold, somewhat more sol. in hot H 2 O. Easily sol. in dil. acids. (Radau, A. 251. 125.) SI. sol. in H 2 O 2 ; insol. in alcohol. (Scheuer, Z. anorg. 1898, 16. 304.) Manganous pyrovanadate, Mn 2 V 2 O 7 . SI. sol. in hqt dil. HNO 3 +Aq. (Ditte, C. R. 96. 1048.) Manganous potassium vanadate, MnKV 6 Oi 4 +8H 2 O. 100 pts. H 2 O dissolve 1.7 pts. salt at 18. Easily sol. in acids. (Radau, A. 251. 129.) 3Mn 3 V 8 O 23 , K 6 V 8 O 23 +54H 2 O. (Radau.) 7Mn(VO 3 ) 2 , 2KVO 3 +25H 2 O. (Radau.) HMn(VO 3 ) 2 , 2KVO 3 +48H 2 O. (Radau.) Mercuric vanadate. SI. sol. in H 2 O. Nickel vanadate, Ni(VO 8 ) 2 . Sol. in H 2 O. (Ditte, C. R. 104. 1705.) Nickel or^ovanadate, Ni 3 (VO 4 ) 2 . Insol. in H 2 O; sol. in HN0 3 +Aq. (Ditte, C. R. 96. 1049.) Nickel (fcvanadate, NiV 4 On+3H 2 O. Sol. in H 2 O. (Ditte, C. R. 104. 1705.) Nickel potassium vanadate, 5Ni(V0 3 ) 2 , 2KV0 3 +25H 2 O. Ni 3 K 2 Vi O 29 +17H 2 O. Very si. sol. in hot H 2 O. NiKV 5 O 4 +8H 2 O. 2Ni 4 V 14 O 39 , K 8 Vi 4 O 39 +69H 2 O. 1000 pts. H 2 O dissolve 1.7 pts. of salt at 17.5. (Radau, A. 251. 137.) Potassium vanadate, basic, K 8 V 2 O 9 +20H 2 O. Sol. in H 2 O. (Ditte, C. R. 104. 902.) Potassium metovanadate, KV0 3 . Anhydrous. Slowly sol. in cold, more easily in hot H 2 O. Insol. in alcohol. (Ber- zelius.) Completely sol. in a little cold H 2 O. (Nor- blad.) +H 2 O. Sol. in H 2 O. (Rammelsberg.) + 1^H 2 O. (Ditte.) + 1^H 2 O. (Ditte.) +2H 2 O. (Ditte.) +3H 2 O. (Ditte, C. R. 104. 902.) +7H 2 O. (Rammelsberg.) VANADATE, SODIUM 1107 Potassium (ftvanadate, K 2 V 4 Oii+4H 2 O. Sol. in cold or lukewarm H 2 O. Decomp. by hot H 2 O. (Rammelsberg.) +3H 2 O. (Berzelius.) +3>iH 2 O. Sol. in warm H 2 O. (Norblad.) +8 or 10H 2 O. (Ditte, C. R. 104. 902.) +6H 2 O. (Ephraim, Z. anorg. 1903, 35. 76.) Potassium Znvanadate, K 2 V 6 Oi 6 . Anhydrous. Nearly insol. in H 2 O. (Nor- blad.) +6H 2 O. Insol. in cold or hot H 2 O. (Nor- blad.) + 1, and 5H 2 O. (Ditte, C. R. 104. 902.) Potassium or^ovanadate. K 3 VO 4 +4^ or 6H 2 0. Deliquescent. Sol. in H 2 O. (Ditte, C. R. 104. 902.) Decomp. by H 2 O into K 4 V 2 O 7 and KOH. (Rammelsberg, B. A. B. 1883. 3.) Potassium pyrovanadate, K 4 V 2 O 7 +3H 2 0. Deliquescent Easily sol. in H 2 O. Insol. in alcohol. (Norblad.) +4H 2 O. (Ditte, C. R. 104. 902.) Potassium vanadate, K 3 V5O 14 -f-5H 2 O. 100 pts. H 2 O dissolve 19.2 pts. at 17.5. (Radau, A. 251. 120.) -f-4^H 2 O. (Radau.) K 4 V 6 O ]7 +2H 2 O. Slowly sol. in H 2 O. (Rammelsberg.) +6H 2 O. (Ditte, C. R. 104. 902.) +7H 2 O. (Friedheim. B. 23. 1526.) K 4 VioO 27 + 12H 2 O. Very sol. in H 2 O. (Manasse, A. 240. 42.) K 10 V 8 O 25 +7H 2 O. Sol. inH 2 O. (Rammels- K 2 V 8 O 21 +1^H 2 O. Very si. sol. in H 2 O. (Ephraim, Z. anorg. 1903, 35. 75.) K 4 Vi 8 O 47 . (Ephraim, Z. anorg. 1903, 35. 78.) Potassium sodium vanadate, 2(2K 2 O,3V 2 5 ), 3(2Na 2 O, 3V 2 O 5 )+30H 2 O. (Friedheim, Z. anorg. 1894, 5. 442.) 2K 2 O, 3V 2 O 6 , 4(2Na 2 O, 3V 2 O 5 )+35H 2 O. Efflorescent. (Friedheim, Z. anorg. 1894, 5. 441.) Potassium strontium vanadate, K 2 Sr 3 Vi 4 O 3 9+ 20H 2 O. Sol. in H 2 O. (Manasse, A. 240. 23.) K 2 Sr 3 Vi 4 O 3 9+30H 2 O. As above. (Man- asse.) K 4 Sr 2 Vi 4 O 39 +18H 2 O. As above. (Man- asse.) Potassium zinc vanadate, KZnV 6 Oi 4 +8H 2 O. 1000 pts. H 2 O dissolve 4.1 pts of the salt. (Radau, A. 251. 145.) 2K 8 V 14 O 39 , 3Zn 4 V 14 O 39 +90H 2 O. (Radau.) Potassium vanadate cyanide, K 4 V 2 O 7 , 4KCN +14H 2 O. Easily decomp. Insol. in alcohol. (Petersen. Z. anorg. 1904, 38. 343.) Samarium vanadate, Sm 2 O 3 , 5V 2 O 6 +28H 2 O. (Cleve.) +24H 2 O. (Cleve.) Samarium or^ovanadate. Precipitate. Silver raetavanadate, AgVO 3 . Sol. in HNO 3 or dil. NH 4 OH+Aq. (Ber- zelius.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 829.) Silver or^ovanadate, Ag 3 VO 4 . Ppt. Easily sol. in HNO 3 or NH 4 OH+Aq. (Roscoe, Proc. Roy. Soc. 18. 316.) Silver pyrovanadate, Ag 4 V 2 O 7 . Ppt. (Roscoe.) Sol. in NH 4 OH+Aq. (Ditte, C. R. 104. 1705.) Silver vanadate, Ag 6 V 4 Oi 3 . Sol. in 21,414 pts. H 2 O at 14, and 13,617 pts. at 100. (Carnelley, A. 166. 155.) Silver vanadate ammonia, 6AgVO 3 , 4NH 3 -f- 8H 2 0. (Ditte, C. R. 104. 1705.) Sodium vanadate, basic, Na 8 V 2 O 9 +26 or 30H 2 O. Very sol. in H 2 O. (Ditte.) Sodium raetavanadate, NaVO 3 . Anhydrous. Slowly sol. in cold, very easily in hot H 2 O. (Norblad.) 100 g. H 2 O dissolve at: 25 40 60 75 21.10 26.23 32.97 38.83 g. NaVO 8 . (McAdam and Pierle, J. Am. Chem. Soc. 1912, 34. 606.) +2H 2 O. Easily sol. in H 2 O. 100 g. H 2 O dissolve at: 25 40 60 15.23 29.93 68.36 g. NaV0 3 . At 75 a value was obtained which showed that the solid phase had changed into the less sol modification. (McAdam and Pierle, J. Am. Chem. Soc. 1912, 34. 607.) + ^H 2 O. (Ditte, C. R. 104. 1061.) +3, 4, and 5H 2 O. (Ditte.) Sodium efo'vanadate, Na 2 V 4 On. Anhydrous. SI. sol. even in warm H 2 O, but easily sol. on addition of acids. 1108 VAN ABATE, SODIUM +9H 2 O. Easily sol. in cold H 2 O. Insol. in alcohol. (Norblad.) +5H 2 O. (Ditte, C. R. 104. 1061.) Not obtained by Rammelsberg (B. A. B. 1883. 3.) Sodium Jrivanadate, Na 2 V 6 Oi 6 +9H 2 O. Insol. in cold or hot H 2 O. (Norblad.) Composition is Na6V 16 O 43 +24H 2 O. (Ram- melsberg.) +3H 2 O. (Ditte, C. R. 104. 1061.) Sodium ori/wvanadate, Na 3 VO 4 +16H 2 O. Easily sol. in H 2 O, but decomp. into Na 4 V 2 O 7 and KOH. Precipitated by an ex- cess of alcohol. (Roscoe, A. suppl. 8. 102.) +7H 2 O. (Hall, Chem. Soc. 61. 96.) + 10., and 12H 2 O. Less sol. in dil. NaOH +Aq than in H 2 O. (Baker, A. 229. 286.) Sodium p?/rovanadate, Na 4 V 2 O 7 -f-18H 2 O. Easily sol. in H 2 O. Insol. in alcohol. (Norblad.) Spl. in alcDhol. (Ditte, C., R. 104. 1061.) +8H 2 O. (Ditte.) Sodium sesgmvanadate, Na 4 V 6 Oi 7 . Anhydrous. Insol. in H 2 O or NH 4 OH+Aq. (Rammelsberg.) + 10H 2 O. (Norblad.) + 16H 2 O. Efflorescent. (Rammelsberg.) + 18H 2 O. (Ditte.) Sodium pentavanadate, Na 4 Vi O 27 +3V2H 2 O. Scarcely sol. in H 2 O. (Rammelsberg.) Sodium vanadate, Na 6 V 4 Oi3-j-6H 2 O. Difficultly sol. in cold H 2 O. (Carnelley, A. 166. 155.) +2H 2 O. (Carnelley.) Na 6 Vi 6 O 43 +24H 2 O. Correct formula for Norblad' s ^nvanadate. (Rammelsberg.) Na 2 O, 4V a O+7^H 2 O: (Baragiola, Dis- sert. 1902.) +8MH 2 O. (Baragiola.) 3Na 2 O ; 5V 2 O 6 +22H 2 O. (Prandtl and Lustig, Z. anorg. 1907, 53. 405.) 4Na 2 O, 7V 2 O 5 +33H 2 O. (Friedheim, Z. anorg. 1894, 6. 443.) 5Na 2 O, 8V 2 O 6 +39H 2 O. Sol. in H 2 O (Friedheim, Z. anorg. 1894, 5. 441.) Sodium vanadate fluoride, 2Na 3 VO 4 , NaF+ 19H 2 0. Sol. in H 2 0. (Rammelsberg, W. Ann. 20. 928.) Stontium metavanadate, Sr(VO 3 ) 2 +4H 2 O. Difficultly sol. in cold H 2 O. (Norblad.) Strontium divanadate, SrV 4 O n +9H 2 O. SI. sol. in H 2 O, but much more sol. than barium di'vanadate. (v. Hauer.) Sol. in H 2 O 2 +Aq free from H 2 SO 4 . Insol. in alcohol. (Scheuer, Z. anorg. 1898, 16. 303.) Strontium nvanadate, SrV 6 Oi 6 +14H 2 O. Sol. in H 2 O, but decomposes slowly on boiling. Easily sol. in hot H 2 O acidified with HC 2 H 3 O 2 , and crystallizes therefrom without decomp. (v. Hauer, J. pr. 76. 156.) Strontium fctfravanadate, SrV 8 O 2 i + llH 2 0. Sol. in hot H 2 O with partial decomposition. (Manasse, A. 240. 34.) Strontium vanadate, Sr 3 V 8 O 23 +14H 2 O. Sol. in H 2 O. (Manasse, A. 240. 23.) Sr 4 V 14 O 3 9+30H 2 O. Sol. in H 2 O. (Nor- blad.) Thallous metovanadate, T1VO 3 . Sol. in 11,534 pts. H 2 O at 11, and 4756 pts. at 100. (Carnelley.) Thallous or^ovanadate, T1 3 VO 4 . SI. sol. in H 2 O. Sol. in 999 pts. H 2 O at 15, and 574 p s. at 100. (Carnelley, Chem. Soc. (2) 11. 323.) Thallous p2/rovanadate, T1 4 V 2 O 7 . Sol. in 4996 pts. H 2 O at 14, and 3840 pts. H 2 O at 100. (Carnelley.) Thallous vanadate, Tli 2 V 8 O 26 . Sol. in 3406 pts. H 2 O at 14, and 533 pts. at 100. (Carnelley.) Tl 12 V 10 O 3 i. Sol. in 9372 pts. H 2 O at 11, and 3366 pts. at 100. (Carnelley.) Tl 12 Vi 4 O 4 i. Ppt. (Carnelley) Thorium vanadate, Th 3 O 12 (VO) 4 , 16V 2 O 6 -f 24H 2 O (?). Sol. in H 2 O. (Cleve.) ThO 2 ,V 2 O 5 +6H 2 O. Sol. in acids. (Volck, Z. anorg. 1894 6. 167. Uranyl vanadate, 2UO 3 , V 2 O 6 , (UO 2 ) 2 V 2 O 7 . Insol. in H 2 O. "(Garnet, C. R. 104. 1850.) Vanadium vanadate, 2VO 2 , V 2 O6=V 4 O9. Insol. in H 2 O. Sol. in dil. H 2 SO 4 or HNO 3 Aq. (Rammeslberg.) Slowly oxidised by HNO 3 +Aq. Slowly sol. in NH 4 OH+Aq. Reasily sol. in HCl+Aq (Ditte, C. R. 101. 1487.) +2 2 / 3 H 2 O. (Brierley.) 2VO 2 , 2V 2 O 6 +8H 2 O. Insol. in H 2 O. (Brierley, Chem. Soc. 49. 31.) Ytterbium vanadate, 3Yb 2 O 3 , 5V 2 O 6 +3H 2 O. Yb 2 O 3 , 15VoO 6 . Ppt. (Cleve, Z. anorg. 1902, 32. 150.) Yttrium vanadate. Precipitate. (Berzelius.) VANADIOMOLYBDATE, AMMONIUM 1109 Zinc vanadate, Zn(VO 3 ) 2 -f 2H 2 O. Sol. in H 2 O. (Ditte, C. R. 104. 1705.) Zinc pyrovaaadate, Zn 2 V 2 O 7 . Appreciably sol. in H 2 O. (Ditte, C. R. 96. 1048.,) Pervanadic acid. See Pervanadic acid. Vanadicotungstic acid. Ammonium vanadicotungstate, 3(NH 4 ) 2 O, V 2 O 3 , 8WO 3 +10H 2 O. Very sol. in H 2 O. Insol. in organic solvents. (E. F. Smith, J. Am. Chem. Soc. 1903, 26. 1227.) Vanadicovanadic acid. Ammonium vanadicovanadate, (NH 4 ) 2 O, 2VO 2 , 4V 2 O 6 +8H 2 O. SI. sol. in cold and warm H 2 O. (Gibbs, Am. Ch. J. 7. 209.) (NH 4 ) 2 O, 2V 2 O 4 , 2V 2 O 6 +14H 2 O. Sol in H 2 O. (Brierley, Chem. Soc. 49. 30.) 3(NH 4 ) 2 O, 2V 2 O 4 , 4V 2 O 8 +6H 2 O. Insol. in H 2 O. (Brierley.) Potassium , 2K 2 O, 2V 2 O 4 , V 2 O 5 +6H 2 O. Sol. in hot H 3 O. (Brierley, Chem. Soc. 49. 30.) 5K 2 O, 2V 2 O 4 , 4V 2 O 5 +H 2 O. Insol. in H 2 O. .(Brierley.) K 2 O, V 2 O 4 , 8V 2 O 5 . Insol. in H 2 O. Sol. in cone. H 2 SO 4 . (Prandtl, B. 1905, 38. 660.) Sodium , 2Na 2 O, 2V 2 O 4 , V 2 O 6 +13H 2 O. Easily sol. in H 2 O. Insol. in cone, solu- tions of salts, especially acetate. (Brierley, Chem. Soc. 49. 30.) 2Na 2 O, V 2 O 4 , 5V 2 O 6 . Insol. in H 2 O. Sol. in cone. H 2 SO 4 . Not attacked by boiling with cone. HNOg. Slowly attacked by hot dil. NH 4 OH-fAq. (Prandtl, B. 1905, 38. 659.) Vanadioarsenic acid. See Arseniovanadic acid. Vanadioiodic acid. See lodovanadic acid. Vanadiomolybdic acid, 8MoO 3 , V 2 O 6 + 5H 2 O. Very si. sol, -in H 2 O, and si. sol. in boiling HNO 3 +Aq. (Ditte, C. R. 102. 757.) Could not be obtained. (Friedheim, B. 24. 1173.) Ammonium vanadiomolybdate, (NH 4 ) 2 O, V 2 O 5 , 2MoO 3 +4H 2 O. Nearly insol. in H 2 O. (Friedheim and Castendyck, B. 1900,. 33. 1615.) (NH 4 ) 2 0, 2V 2 6 , 2Mo0 3 +8H 2 0. Nearly insol. in H 2 O. (Friedheim and Castendyck.) 2(NH 4 ) 2 O, V 2 O 5 , 3MoO 3 +6H 2 O. (Euler- Chelpin, Dissert, 1896.) (NH 4 ) 2 0, V 2 5 , 3Mo0 3 +17H 2 0. (Euler- Chelpin.) 2(NH 4 ) 2 O, V 2 O 5 , 4MoO 3 +7H 2 O and + 8H 2 O. (Euler-Chelpin,) 3(NH 4 ) 2 0, 2V 2 5 , 4Mo0 3 +7H 2 0. (Milch, Dissert. Berlin, 1887.) +9H 2 O. Sol. inH 2 O. (Ditte, C. R. 102. 1019.) + 11H 2 O. Easily sol. in H 2 O. Correct composition of above compounds is = (NH 4 ) 2 O, 2V 2 O 5 +2[NH 4 ) 2 O, 2MoO 3 ]+llH 2 O. (Friedheim, B. 24. 1173.) Moderately sol. in H 2 O and can be re- cryst. therefrom. (Euler-Chelpin, Dissert, 1895.) 2(NH 4 ) 2 O, 3V 2 O 5/ . 4MoO 3 fllH 2 O. Near- ly insol. in H 2 O. (Friedheim and Casten- dyck, B. 1900, 33. 1615.) 2(NH 4 ) 2 O, 2V 2 O 5 , 5MoO 3 . Nearly insol. in cold H 2 O. (Euler-Chelpin, Dissert. 1896.) +8H 2 O. Nearly insol. in H 2 O. (Fried- heim and Castendyck, B. 1900, 33. 1615.) 3(NH 4 ) 2 O, 2V 2 O 5 , 5MoO 3 +8>iH 2 O. Very easily sol. in H 2 O. (Liebert, Dissert. 1891.) 4(NH 4 ) 2 O, 12V 2 O 5 , 5MoO 3 +24HiO. Prac- tically insol. in H 2 O. (Friedheim and Casten- dyck, B. 1900, 33. 1615.) 2(NH 4 ) 2 O, V 2 O 6 , 6MoO 3 +5H 2 O. Sol. in a large amount of H 2 O. (Gibbs, Am. Ch. J. 6. 361.) +6H 2 O. Rather si. sol. in H 2 O. Easily sol. in acids. (Liebert, Dissert, 1891.) Composition is double the above formula, r 4(NH 4 ) 2 O, 2V 2 O 5 , 12MoO 3 +12H 2 O. Rather difficultly sol. in H 2 O. Composition is (NH 4 ) 2 O, 2V 2 O 6 +3[NH 4 ) 2 O, 4MoO 3 ]. (Friedheim.) 3(NH 4 ) 2 O, V 2 O 5 , 6MoO 3 +7H 2 O. (Isen- burg, Dissert, 1901.) 5(NH 4 ) 2 O, 4V 2 O 5 , 6MoO 3 +12H 2 O and + 14H 2 O. (Euler-Chelpin, Dissert, 1896.) 5(NH 4 ) 2 O, 3V 2 O 6 , 7MoO 3 +13H 2 O and + 16H 2 O. Sol. in H 2 O and can be recryst. therefrom. (Toggenburg, Dissert, 1902.) 5(NH 4 ) 2 O, 3V 2 O 6 , 8MoO 3 +14H 2 O. (Stamm, Dissert, 1906.) 5(NH 4 ) 2 O, 2V 2 O 5 , 12MoO 3 flOH 2 O. Quite easily sol. in H 2 O. Composition is (NH 4 ) 2 O, 2V 2 O 5 +4[(NH 4 ) 2 O, 3MoO 3 ] + 10H 2 O. 6(NH 4 ) 2 0, 3V 2 5 , 12Mo0 3 +21H 2 0. Sol. in H 2 O. Composition is (NH 4 ) 2 O, 3V 2 O 5 + 5(NH 4 ) 2 O, 12MoO 3 . (F.) 8(NH 4 ) 2 O, 4V 2 O 6 , 13MoO 3 +21H 2 O. Sol. in H 2 O. (Isenburg, Dissert, 1901.) 8(NH 4 ) 2 O, V 2 O 6 , 18MoO 6 + 15H 2 O. De- comp. by hot H 2 O. (Gibbs.) Could not be obtained. (Friedheim.) 10(NH 4 ) 2 O, 3V 2 O 6 , 24MoO 3 +10H 2 O. Sol. in H 2 O. (Milch.) Could not be obtained. (Friedheim.) 1110 VANADIOMOLYBDATE, AMMONIUM BARIUM Ammonium barium vanadiomolybdate, 5(NH 4 ) 2 O, 15BaO, 6V 2 5 , 36MoO 3 . (Milch.) (NH 4 ) 2 O, BaO, V 2 O 5 , MoO 3 +6H 2 O. (Euler-Chelpin, Dissert, 1895.) 3(NH 4 ) 2 O, BaO. 3V 2 O 6 , 5MoO 3 +9H 2 O. SI. sol. in oold and hot H 2 O. (Euler-Chelpin.) Ammonium potassium , (NH 4 )aO, 3K 2 0, 2V 2 O 6 , 4Mo0 3 +5H 2 O. Decomp. by H 2 O. (Euler-Chelpin,) (NH 4 ) 2 O. 3K 2 O, 3V 2 5 , 5MoO 3 +9H 2 O. (Euler-Chelpin.) K(NH 4 ) 2 O, 3KK 2 O, 3V 2 O 6 , 5Mo0 3 + 16H 2 O. Sol. in H 2 O. (Jacoby, Dissert. 1900.) Ammonium sodium , (NH 4 ) 2 O, Na 2 O, 2V 2 O 6 , 6Mo0 3 +12H 2 0. (Euler-Chelpin, Dissert, 1896.) Barium , BaO, V 2 6 , MoO 3 +7H 2 O. (Euler-Chelpin.) Barium , 3BaO, 2V 2 O 6 , 6Mo0 3 . (Milch.) +8H 2 O. (Euler-Chelpin.) 5BaO, 4V 2 O 5 , 6MoO 3 +28H 2 O. Sol. in hot H 2 O. (Euler-Chelpin.) 3BaO, V 2 O 5 , 8MoO 3 +2BaO, H 2 O, V 2 O 5 , 8MoO 3 +28H 2 O. Sol. in hot H 2 O. (Gibbs, Am. Ch. J. 6. 361.) 7BaO, 3V 2 O 5 , 18MoO 3 +16H 2 O = BaO, 3V 2 O 5 +6(BaO, 3MoO 3 ) + 16H 2 O. SI. sol. in H 2 O. +36H 2 O and +48H 2 O. (Liebert, Dis- sert. 1891.) Potassium , K 2 O, V 2 O 5 , 3Mo0 3 +15H 2 O. Nearly insol. in cold H 2 0. (Euler-Chelpin, Dissert, 1896.) 3K 2 O, 2V 2 O 5 , 4MoO 3 +8H 2 O=K 2 O, 2V 2 5 -t-2(K 2 O, 2MoO 3 )+8H 2 O. Very sol. in H 2 O. (Friedheim.) +7H 2 O. Easily sol. in cold H 2 O. (Euler- Chelpin.) +9H 2 O; Easily sol. in cold H 2 O. (Euler- Chelpin.) 2K 2 O, 2V 2 O 6 , 5MoO 3 +10H 2 O. Nearly insol. in cold, very si. sol. in hot H 2 O. (Euler- Chelpin.) 3K A V 2 O S , 6MoO 3 +5H 2 O. (Euler-Chel- pin.) 2K 2 O, V 2 O 5 , 6MoO 3 +6H 2 O. Very si. sol, in cold, easily sol. in hot H 2 O. (Liebert.) 4K 2 0, 2V 2 O 8 , 12MoO 3 +12H 2 O=K 2 O, 2V 2 O 5 +3(K 2 O, 4Mo0 3 )-f-12H 2 O. SI. sol, in H 2 O. (Friedheim.) 5K 2 0, 2V 2 O 5 . 12MoQ 3 + 12H 2 O=K 2 0, 2V 2 O+4(K 2 O, 3MoO 3 ) + 12H 2 O. Rather si, sol. in H 2 0. (Friedheim.) SI. sol. in cold, easily sol. in hot H 2 O. (Liebert, Dissert, 1891.) 3K 2 O, V 2 O 6 , 12MoO 3 + 15H 2 0. (Liebert.) Potassium sodium vanadiomolybdate, K 2 O, 4Na 2 O, 2V 2 O 6 , 12Mo0 3 + 18H 2 O. (Euler-Chelpin. Dissert 1895.) Sodium , 2Na 2 O, V 2 O 5 , 6MoO 3 +16H 2 O. (Euler-Cheipin, Dissert, 1895.) Vanadiophosphoric acid. See Phosphovanadic acid. Vanadioselenious acid, 3V 2 O 6 , 4SeO 2 -f- 4H 2 0. +6H 2 O. Difficultly sol. in H 2 O. Can b< cryst. from H 2 O. + 10H 2 O. Difficultly sol. in H 2 0. Can b< cryst. from H 2 O. (Prandtl, B. 1905, 38 1307.) Ammonium vanadioselenite, 4(NH 4 ) 2 O, 6V 2 O 6 , 5SeO 2 +13H 2 O. SI. sol. in H 2 O. Decomp. by boiling H 2 O 3(NH 4 ) 2 O. 3V 2 O 5 . 6SeO 2 +2H 2 O. Ppt (Prandtl, B. 1905, 38. 1309.) (NH 4 ) 3 HV 6 O 17 , 12SeO 2 +2H 2 O. Ppt. +4H 2 O. Ppt. (Prandtl, Z. anorg. 1911 73. 231.) Ammonium silver ^2 2 /3(NH 4 ) 2 O, li/ 3 Ag 2 O 6V 2 O 6 , 5SeO 2 +12H 2 O,+16H 2 O am +22H 2 O. (Prandtl, Z. anorg. 1907, 63. 402.) Lithium , 4Li 2 0, 6V 2 O 5 , 5SeO 2 +30H 2 O Very. sol. in H 2 O. (Prandtl.) Potassium , 4K 2 O, 6V 2 O 5 , 5SeO 2 -f 13H 2 0. 3K 2 O, 3V 2 O 5 , 6SeO 2 . (Prandtl, B. 1905 38. 1309.) Sodium , 4Na 2 O, 6V 2 O 5 , 5SeO 2 +20H 2 Very. sol. in H 2 O. (Prandtl, Z. anore 1907, 63. 403.) Vanadiosulphuric acid, V 2 6 , 3S0 3 +3H 2 Deliquescent. Sol. in H 2 O, but is decomp by boiling. (Ditte, C. B,. 102. 757.) See Sulphate, vanadium. Vanadiosulpurous acid. Ammonium vanadiosulphite, 3(V 2 4 ,S0 2 ), (NH 4 ) 2 0, S0 2 +4H 2 0. (Gain, C. R. 1907, 144. 1158.) Caesium , (V 2 O 4 ,SO 2 ), 3(Cs 2 0,S0 2 ) + 8H 2 O. (Gain.) Lithium , (V 2 4 ,S0 2 ), 5(Li 2 0,S0 2 ) + 8H 2 O. (Gain.)' VANADIOTUNGSTATE, SODIUM 1111 Potassium vanadiosulphite, SO 2 ,(K 2 O)+5H 2 O. (Gain.) 3S0 2 ,(V 2 4 ), -, (V 2 4 ,S0 2 ), 2(Rb 2 0,S0 2 ) Rubidium 2H 2 O. (Gain.) Sodium , 5(V 2 4 ,S0 2 ), (Na 2 0,SO 2 ) + 2H 2 O. (Gain.) Thallium , 3(V 2 O 4 ,SO 2 ), (T1 2 0,SO 2 ) + 8H 2 O. (Gain.) Vanadiotungstic acid, 6H 2 0, V 2 O 6 , 10WO 8 +16H 2 O. Very si. sol. in cold, more easily in hot H 2 O. (Gibbs, Am. Ch. J. 6. 361.) 6H 2 O. V 2 O 5 , 16WO 3 +30H 2 O. Readily sol. in H 2 O. (Gibbs.) 17H 2 O. 4V 2 O 5 , 16WO 3 +24H 2 O. SI. sol. in cold, easily in hot H 2 O. (Rosenheim, A. 251. 228.) Aluminum sodium vanadiotungstate, 7A1 2 O 3 , 27Na 2 0, 36V 2 6 , 144WO 3 +504H 2 O= 3(A1 2 3 , 9Na 2 0, 48W0 3 ), 4(A1 2 O 3 , 9V 2 O 5 ) +504H 2 O. Sol. in H 2 O. (Rothenbach, B. 23. 3055.) -, (NH 4 ) 2 0, 3V 2 5 , W0 3 + Ammonium 6H 2 O. Sol. in H 2 O. (Rammelsberg, B. 1. 158.) 2(NH 4 ) 2 O, V 2 O 6 , 4WO 3 +4H 2 O. (Friedheim and Lowy, Z. anorg. 1984. 6. 24.) 4(NH 4 ) 2 O. 2H 2 0. V 2 O 5 , 5WO 3 + 11H 2 O. Sol. in H 2 0. (Gibbs. Am. Ch. J. 6. 361.) 2(NH 4 ) 2 O. V 2 O 6 , 5WO 3 +10H 2 O. Sol. in H 2 0. (Ditte, C. R. 102. 1019.) 31(NH 4 ) 2 0, 14V 2 5 . 60W0 3 +58H 2 = 5[5(NH 4 )0, 12WO,], 2[3(NH 4 ) 2 0, 7V 2 8 )]. Sol in H 2 O. (Rothenbach, B. 23. 3051.) 7(NH 4 ) 2 O, 4V 2 O 5 , 14WO 3 + 16H 2 O. Sol. in H 2 O. (Rosenheim, A. 261. 197.) 8(NH 4 ) 2 O, 4V 2 O 5 , 16WO 3 , 9H 2 O+4H 2 O. Efflorescent. Very sol. in H 2 O. (Rosenheim, A. 251. 216.) Barium , 19BaO, 10V 2 O 6 , 36WO 3 + 94H 2 = 3(5BaO, 12WO 8 ), 2(2BaO, 5V 2 5 )+94H 2 0. SI sol in H 2 O. (Rothenbach, B. 23. 3052.) 8BaO,' 4V 2 5 , 16WO 3 , 9H 2 O+44H 2 O. Efflorescent. Not very sol. in H 2 O. (Rosen- hC Com^oStion 2 is' 6BaO, 12WO 3 , 3V 2 O 6 + 39H 2 O. (Friedheim.) 6BaO 3V 2 5 ,- 12WO 3 +34H 2 O. Not easily sol. in H 2 O. (Friedheim and Lowy, Z. anorg. 1894, 6.7 18.) 4BaO, 4V 2 O 6 , 12WO 3 -f41H 2 O. Less sol. than preceding salt. Decomp. by boiling or by mineral acids. (Rosenheim.) Composition is 4BaO, 12WO 3 , 3V 2 O 6 + 30H 2 O. (Friedheim.) Calcium vanadiotungstate, 2CaO, V 2 O 6 . 2W0 8 + 12H 2 0. (Friedheim and L6wy, Z. anorg. 1894, 6. Magnesium sodium , MgO, 6Na 2 0, 3V 2 6 , 12W0 8 +42H 2 0=5Na 2 0, 12W0 8 +MgO, Na 2 0, 3V 2 O 6 +42H 2 O. Sol. in H 2 O. (Rothenbach, B. 23. 3054. Potassium , 4K 2 O, 3V 2 6 , 12WO 8 + 30H 2 O. Sol. in H 2 O. Composition is potassium metatungstate vanadate, 3(K 2 O, 4WO 3 )+K 2 O, 3V 2 O 6 + 30H 2 O. (Friedheim, B. 23. 1515.) SKA 4V 2 O 6 , 16WO 3 , 9H 2 O +24H 2 O. Very efflorescent. Easily sol. in H 2 O, (Rosen- heim, A. 251. 214.) Formula is 6K 2 O, 12WO 3 , 3V 2 O 5 +24H 2 O, which is a double salt, 5K 2 O, 12WO 3 +K 2 O, 3V 2 O 5 . (Friedheim, B. 23. 1505.) Potassium sodium , (5Na 2 O, 3V 2 6 , 6WO 3 +22H 2 O), 4(5K 2 O, 3V 2 6 , 6WO 8 +22H 2 O) or Na 2 O, 4K 2 O, 3V 2 O 6 , 6WO, +22H 2 0. (Friedheim and Lowy, Z. anorg. 1894, 6. 22.) 4(5Na 2 O, 3V 2 O 5 , 6WO 3 +24H 2 O), 3(5K 2 0, 3V 2 O 6 , 6W0 3 +24H 2 O.) (Friedheim and Lowy.) 5(5Na 2 O, 3V 2 O 5 , 6WO 3 +24H 2 O), 5K 2 O, 3V 2 O 5 , 6WO 3 +24H 2 Q. (Friedheim and Lowy.) Silver , 8Ag 2 O, 4V 2 O 6 , 16WO 8 , 9H 2 O. Somewhat sol. in cold H 2 O, more easily upon addition of little HNO 3 . Decomp. by warm H 2 O. (Rosenheim, A. 251. 224.) 3Ag ? O, 2V 2 O 5 , 6WO 3 +3H 2 O. Nearly insol. in cold H 2 O. Decomp. by addition of HNO 3 or upon warming. (Rosenheim.) Sodium , 5Na 2 O, 3V 2 O 6 , 6WO 8 +36H 2 O. Sol. in H 2 O. Composition is 3(Na 2 O, 2WO 3 )+2(Na 2 O, 3V 2 O 5 )+36H 2 O. (Friedheim, B. 23. 1527.) +38H 2 O. Sol. in 1.25 pts. H 2 O at 13.8. (Friedheim and Lowy.) 2Na 2 O, 2V 2 O 6 , 3WO 3 +2QH 2 O. Very sol, in H 2 O. Composition is Na 2 O, 3WO 3 -j-Na 2 O, 2V 2 O 6 +20H 2 O, double salt of sodium ^ntungstate and divanadate. (Friedheim, B. 23. 1523.) 4Na 2 0, 3V 2 5 , 12WO 3 +38H 2 O=3(Na 2 O, 4WO 3 )+Na 2 O, 3V 2 O 6 +38H 8 Q. Sol. in H 2 O. (Rpjbhenbach, B. 23. 3050.) aO, 4V 2 6 , 16W0 3 , : 9K 2 O+48H 2 O. 1112 VANADIOTUNGSTATE, STRONTIUM Efflorescent. Easily sol. to H 2 O. (Rosen- heim, A. 251. 210.) Formula is 6Na 2 O, 12WO 3 , 3y 2 O 6 +42H 2 0, and is a double salt of sodium paratungstate, 5Na 2 O, 12WO 3 , and sodium ^nvanadate. Na 2 O, 3V 2 O 6 . (Friedheim, B. 23. 1505.) 7Na 2 0, V 2 5 , 12W0 3 +29H 2 0. Easily sol. in H 2 O. (Friedheim and Lowy, Z. anorg. 1894, 6. 15.) 8Na 2 O, V 2 O 5 , 14WO 3 +60H 2 O and +66H 2 O (Friedheim and Lowy.) Strontium vanadiotungstate, 19SrO, 36WO 3 , 10V 2 O 6 +122H 2 O = 3(5SrO, 12WO 3 ), 2(2SrO, 5V 2 6 )+122H 2 0. Sol. in H 2 O. (Rothenbach, B. 23. 3053.) Vanadious acid. See Hypovanadic acid. Vanadiovanadicomolybdic acid. Ammonium vanadiovanadicomolybdate, 11(NH 4 )A 4V 2 5 , V0 2 , 28Mo0 3 + 48H 2 O. SI. sol. in cold, sol. in hot H 2 O without decomp. (Gibbs, Am. Ch. J. 5. 391.) Barium , 14BaO, 2V 2 O 5 , 3VO 2 , 3QMoO 3 +48H 2 0. Precipitate. Very si. sol. in cold, decomp. byhotH 2 O. (Gibbs.) Vanadiovanadicotungstic acid. Ammonium vanadiovanadicotungstate, 6(NH 4 ) 2 0, 2V 2 6 , 3V0 2 , 12WO 3 + 12H 2 O. Sol. in H 2 O. (Gibbs, Am. Ch. J. 5. S91.) Silver , 6Ag 2 0, 2V 2 O 6 , 3VO 2 , 12WO 3 + 8H 2 0. Precipitate. Very si. sol. in cold, sol. in much warm H 2 O. (Gibbs.) Sodium , 6Na 2 0, 2V 2 O 6 , 3V0 2 , 12WO 3 . Very sol. in H 2 O. (Gibbs.) Vanadium, V. Insol. in H 2 O, HC1, dil. H 2 SO 4 +Aq, and cold cone. H 2 SO 4 . Sol. in hot cone. H 2 SO 4 . Slowly sol. in HF+Aq. Easily sol. in dil. or cone. HNO 3 +Aq. Not attacked by hot or cold NaOH or KOH+Aq. (Roscoe, A. suppl. 7. 85.) Does not alter in the air; not acted upon by HC1 and very slowly by H 2 SO 4 . (Moissan, C. R. 1896, 122. 1299.) Vanadium boride, VB. Sol. in HF and HNO 3 . Decomp. by fused alkalies. (Wedekind, B. 1913, 46. 1203.) Vanadium ^bromide, VBr 3 . Very deliquescent; quickly decomposes. (Roscoe, A. suppl. 8. 99.) +6H 2 O. Sol. in H 2 with decomp. (Locke and Edwards Am. Ch. J. 1898, 20. 600.) Sol. in H 2 O, alcohol and ether. Insol. in HBr. (Piccini, Z. anorg. 1899, 19. 398.) Vanadium carbide, VC. Insol. in HC1 and H 2 SO 4 . Sol. in HNO 3 in the cold, and in fused KNO 3 and KC1O 3 . (Moissan, C. R. 1896, 122. 1300.) Vanadium ^chloride, VC1 2 . Very deliquescent. Sol. in H 2 O, alcohol, and ether. (Roscoe, A. suppl. 7. 79.) Vanadium bichloride, VC1 3 . Deliquescent. Sol. in H 2 O, absolute alco- hol, and ether. +6H 2 O. Sol. in H 2 O; si. sol. in cone. HC1+ Aq. Sol. in alcohol and ether. (Piccini, Z. anorg. 1899, 19. 395.) Vanadium ^rachloride, VC1 4 . Sol. with decomp. in H 2 O, alcohol, and ether. (Roscoe.) Sol. in H 2 Q with decomp. Sol. in fuming HC1 with decomp. Sol. in anhydrous CHC1 3 or glacial acetic acid apparently without chemical change. (Koppel, Z. anorg. 1905, 46. 346.) Vanadium cfo'fluoride, VF 2 . Sol. in HF with evolution of H 2 and forma- tion of VF 3 . (Manchot, A. 1907, 367. 135.) Vanadium Znfluoride, VF 3 . Nearly insol. in H 2 O and organic solvents. (Ruff, B. 1911, 44. 2544.) +3H 2 O. Efflorescent. Easily sol. in cold, extremely sol. in hot H 2 O with decomp. Can be recryst. from HF+Aq. Insol. in strong alcohol. (Petersen, J. pr. (2) 40. 48.) Vanadium teirafluoride, VF 4 . Very hydroscopic. Easily sol. in H 2 O. Difficultly sol. in SO 2 C1 2 and SiCl 4 . Sol. in POC1 3 with evolution of gas. Sol. in acetone and acetic acid. Difficultly sol. in alcohol and CHC1 3 . (Ruff, B. 1911,44.2545.) Vanadium pe/Uafluoride, VF 5 . Easily sol. in H 2 O. Easily sol. in alcohol, CHC1 3 , acetone, and ligroin. Insol. in CS 2 . Decomp. toluene and ether. (Ruff, B. 1911, 44. 2549.) Vanadium Zrifluoride with MF. See Fluovanadate, M. VANADIUM SULPHOCHLORIDE SULPHUR CHLORIDE 1113 Vanadium hydride, Stable. Does not react with boiling H 2 O. Not attacked by boiling HC1. but oxidized by hot H 2 SO 4 . Sol. in boiling HNO 3 . (Muthmann, A. 1907, 356. 86.) Vanadium ^hydroxide, VO, zH 2 O. Insol. in KOH or NaOH+Aq. V(OH) 2 . Sol. in HC1. (Locke and Ed- wards, Am. Ch. J. 1898, 20. 598.) Vanadium tfnhydroxide, V 2 O 3 , zH 2 O. Easily sol. in all acids. (Petersen, J. pr. (2) 40. 49.) Vanadium te^rahydroxide (Hypovanadic hy- droxide), V 2 O 2 (OH) 4 +5H 2 O. Easily sol. in acids or alkalies. (Crow, Chem. Soc. 30. 453.) Vanadium Jniodide, VI 3 +6H 2 O. Very hydroscopic; sol. in H 2 O. Only si. sol. in cold cone. HI+Aq. Sol. in alcohol. (Piccini, Z. anorg. 1899, 19. 399.) Vanadium nitride, V 2 N. Insol. in H 2 O, HC1, and KOH+Aq. Sol. in HN0 3 +H 2 S0 4 . Decomp. by fusing with KOH. (Muth- mann, A. 1907, 366. 93.) Insol. in liquid NH 3 . (Gore, Am. Ch. J. 1898, 20. 830.) VN. (Roscoe, A. suppl. 6. 114.) VN 2 . Not attacked by cold HNO 3 +Aq. (Uhrlaub, Pogg. 103. 134.) Vanadium dioxide, VO. Insol. in H 2 O; easily sol. in dil. acids. (Roscoe, A. suppl. 6. 95.) Vanadium Zrioxide, V 2 O 3 . Oxidized in H 2 O in contact with air and then dissolves. Insol. in acids, except HNO 3 , and in alkalies +Aq. (Roscoe, A. suppl. 6. 99 ) Easily sol. in HF. (Petersen, J. pr. (2) 40. 48.) Vanadium te^roxide, VO 2 . Sol. in acids and alkalies +Aq. Vanadium pentoxide, V 2 O 6 . Sol. in about 1000 pts. H 2 O. (Berzelius.) Sol. in acids, alkali hydrates, and carbon- ates +Aq. Insol. in absolute, very si. sol. in dil. alcohol. Insol. in glacial HC 2 H 3 O 2 . Sol. in cone. KF+Aq. (Ditte, C. R. 106. 1067.) Sol. in H 2 C 2 O 4 +Aq and alkali oxalates + Aq. (Halberstadt, Z. anal. 22. 1.) Three modifications. (a) Forms hydrates with 2. and 5H 2 O. Sol. in H 2 O. 1 1. of sat. solution contains 8 g. V 2 O 5 . (/3) V 2 O 6 , 2H 2 Q. Very si. sol. in H 2 O. 1 1. of sat. solution contains 0.5 g. V 2 O 6 . (7) V 2 O 5 , 5H 2 O. Less sol. in H 2 O than 11. H 2 O contains 0.05 g. V 2 O 5 when sat- urated. (Ditte, C. R. 101. 698.) See Vanadic acid. Vanadium oxide, V 4 O 9 =2VO 2 , V 2 O 5 . See Vanadate, vanadium. V 2 O 4 , V 2 6 + 8 / 3 H 2 0. (Brierley, Chem. Soc. 49. 30.) See also Vanadiovanadic acid. V 2 O<. 2V 2 O 5 +8H 2 0. See Vanadate, vanadium. Vanadium pentoxide with MF. See Fluoxyvanadate, M. Vanadium oxy compounds. See Vanadyl compounds. Vanadium silicide, V 2 Si. Insol. in H 2 O. Not attacked by HC1, HNO 3 or H 2 SO 4 . Readily attacked by HF. Not attacked by KOH+Aq, NaOH+Aq or NH 4 OH. Decomp. by fused KOH. Insol. in alcohol, ether and benzene. (Moissan, C. R. 1902. 135. 496.) VSi 2 . Sol. in HF; insol. in acids and al- kalies. Decomp. by fused KOH. (Moissan, C. R. 1902, 135. 78.) Vanadium ^sulphide, V 2 S 2 . Insol. in boiling dij. or cone. HC1, dil. H 2 SO 4 +Aq, or cold cone. H 2 SO 4 . Easily sol. in hot dil. or cone. HNO 3 +Aq, or in boiling cone. H 2 SO 4 . Insol. in alkalies +Aq. SI. sol. in KSH+Aq; sol. in NH 4 SH+Aq. (Kay, Chem. Soc. 37. 728.) Vanadium bisulphide, V^a. Insol. in cold HC1 or dil. H 2 SO 4 +Aq. Very si. sol. in hot HC1 or dil. H 2 SO 4 +Aq. More sol. in HNO 3 +Aq or cone. H 2 SO 4 . SI. sol. in NaOH or NH 4 QH+Aq. Easily sol. in (NH 4 ) 2 S or NH 4 SH+Aq, also in K 2 S+Aq. (iCay, Chem. Soc. 37. 728.) Vanadium pen to sulphide, V 2 Se. SI. attacked by hot cone. HC1 or hot dil. H 2 SO 4 +Aq; sol. in hot cone. H 2 SO 4 . Sol. in hot dil. HNO 3 +Aq. SI. sol. in NH 4 OH+Aq, but easily dissolved by NaOH+Aq. SI. sol in Na 2 S+Aq. Sol. in NH 4 SH+Aq. (Kay.) Vanadium sulphochloride sulphur chloride, 4VSC1 3 , S 2 C1 2 . Decomp. in the air. (Koppel, Z. anorg. 1905, 46. 357.) 1114 VANADOUS ACID Vanadous acid. Ammonium vanadite, basic. 2(NH 4 ) 2 O, V 2 4 . SI. sol. in cold, easily in hot H 2 O. (Ditte, C. R. 102. 1310.) Ammonium vanadite, (NH 4 ) 2 V 4 O 9 +3H 2 O. Sol. in H 2 O. (Crow, Chem. Soc. 30. 460.) +sH 2 O. Sol. in H 2 0. Insol. in alcohol, ether and ammonia. (Koppel, Z. anorg. 1903. 36. 297.) +3H 2 O. Easily sol. 'in H 2 O. (Mawrow, Z. anorg. 1907, 66. 150.) Barium vanadite, BaV 4 O 9 +4H 2 O. Ppt. (Koppell, Z. anorg. 1903, 36. 300.) +5H 2 O. Precipitate. Easily sol. in HNO 3 , or HCl+Aq. (Crow, Chem. Soc. 30. 460.) Lead vanadite, PbV 4 9 . .Ppt. (Crow.) Potassium vanadite, K 2 V 4 O 9 +4H 2 O. Sol. in H 2 O. Insol. in alcohol, ether and ammonia (Koppel, Z. anorg. 1903 ; 36. 300.) +7H 2 O. Easily sol. in H 2 O. Insol. in cold, sol. in hot KOH+Aq. Insol. in alcohol. (Crow.) +H 2 O. (Ditte. C. R. 102. 1310.) Silver vanadite, Ag 2 V 4 O 9 . Ppt. (Crow.) Sodium vanadite, Na 2 V 4 O 9 -f4H 2 O. Sol. in H 2 O. Insol. in alcohol, ether and ammonia. (Koppel, Z. anorg. 1903, 36. 299.) +7H 2 O. Easily sol. in H 2 O. (Crow, Chem. Soc. 30. 459.) Vanadosotungstic acid. Ammonium vanadosotungstate, 5(NH 4 ) 2 O, 2V 2 O 4 , 14WO 8 +13H 2 O. Very sol. in H 2 O. (E. F. Smith, J. Am. Chem. Soc. 1903, 26. 1228.) Vanadous acid. See Hypovanadic acid. Vanadovanadic acid. See Vanadicovanadic acid. Vanadyl bromide, VOBr. Very si. sol. in H 2 O, acetic anhydride, ethyl acetate, and acetone. Insol. in alcohol, ether, acetic acid, CHC1 3 , toluene and CC1 4 . (Ruff, B. 1911, 44. 2537.) Vanadyl ^bromide, VOBr 3 . Very deliquescent, and sol. in H 2 O. (Ros- coe.) Vanadyl /n'bromide, VOBr 3 . Very deliquescent, and quickly decomposes .n moist air. Sol. in H 2 O. (Roscoe.) Vanadyl bromide, V 2 O 3 Br 2 , 2HBr+7H 2 O. Very deliquescent. (Ditte, C. R . 102. 1310.) Vanadyl seraichloride, V 2 O 2 C1. Insol. in H 2 O. Easily sol. in HNO 8 +Aq. (Roscoe, A. suppl. 6. 114.) Vanadyl raonochloride, VOC1. Insol. in H 2 O. Easily sol. in HNO 3 +Aq. (Roscoe.) Vanadyl ^chloride, VOC1 2 . Deliquescent. Slowly decomp. by H 2 O. Easily sol. in HNO 3 +Aq. (Roscoe.) Vanadyl ^chloride, VOC1 8 . Deliquescent. Sol. in H 2 O and alcohol with decomp. (Bedson, A. 180. 235.) Sol. in ether with combination. Divanadyl chloride, V 2 4 C1 2 +5H 2 O. Deliquescent, and sol. in H 2 O, fuming HC1. or alcohol. (Crow; Chem. Soc. 30. 457.) Vanadyl chloride, V 2 O 3 C1 2 +4H 2 0. Very deliquescent. (Ditte. C. R. 102. 1310.) Vanadyl platinum chloride. See Chloroplatinate, vanadyl. Vanadyl inchloride ammonia, VOC1 3 , #NH 8 . Decomp. by H 2 O. (Roscoe.) Vanadyl ^fluoride, VOF 2 . Insol. in H 2 O. Insol. in alcohol, ether, CHC1 3 . SI. sol. in acetone. (Ruff, B. 1911, 44. 2546.) Vanadyl Znfluoride, VOF 3 . Very hydroscopic. Easily sol. in H 2 O. Sol. in POC1 3 with evolution of gas. Diffi- cultly sol. in PC1 3 and AsCl 3 . Sol. in hot CHC1 3 and acetic anhydride. (Ruff, B. 1911, 44. 2547.) Vanadyl fluoride wilh MF. See Fluoxyvanadate, and Fluoxhypovana- date, M. Vanadyl iodide, V 2 O 3 I 2 , 3HI+10H 2 O. Very deliquescent, and sol. in H 2 O. (Ditte, C. R. 102. 1310.) V 2 3 I 2; 2HI+8H 2 O. As above. Vanadyl sulphide, VOS (?). (a) Insol. in H 2 O, alkalies, alkali sulphides +Aq. Sol. in acids, except nitric acid and aqua regia. (Berzelius.) XANTHOCOBALTIC MERCURIC CHLORIDE 1115 (6) Sol. in alkalies, alkali carbonates, and sulphides+Aq. Insol. in acids. (Berzelius.) Water, H 2 O. Water is the most universal solvent. It absorbs all gases, usually with an increase of volume, seldom, as in the case of NH 3 , with a diminution of volume. It dissolves almost all solids in greater or less quantity, and mixes with or dissolves considerable amounts of many liquids. Miscible with alcohol. Sol. in 36 pts. ether. Sol. in 30-33 vols. ethyl acetate. (Becker.) Sol. in 5 vols. iodhydrin. SI. sol. in most of the fatty oils. Solubility in organic solvents at t. G. H 2 O in Solvent t 100 g. of the solution Benzene +3 0.030 23 0.060 40 0.114 55 0.184 66 0.255 77 0.337 Petroleum -2 0.0012 bpt. 190-250 + 18 0.005 at atmos. pressure 23 0.007 30 0.008 36 0.012 53 0.026 59 0.031 61 0.035 66 0.043 79 0.063 85 0.075 94 0.097 Paraffin oil + 16 0.003 bpt. 200-300 50 0.013 at 10 mm . pressur 65 0.022 73 0.030 77 0.035 94 0.055 (Groschuff, Z. Elektrochem, 1911, 17. 350.) White precipitate, fusible. See Mercuricfo'ammonium chloride. White precipitate, infusible. See Mercuric chloramide. Xanthochromium bromide, Cr(NO 2 )(NH 3 )5Br 2 . Sol. in H 2 O. Resembles the chloride (Christensen, J. pr,.' (2) 24. 74.) carbonate, dr(Kp 2 )(NH,)6CO,. Easily sol. in H 2 O. -(Christensen.) Xanthochromium chloride, Cr(N0 2 )(NH 3 ) 6 Cl 2 . More sol. in H 2 O than the roseo, but less than the purpureo salt. Solution decomp. by light or boiling. De- comp. by dil. acids. Sol. in NaOH+Aq and n NH 4 OH+Aq (sp. gr. 0.91). Insol. in alcohol. (Christensen, J. pr. (2) 24. 74.) chloroplatinate, Cr(NO 2 )(NH 3 )5PtCl6. Insol. in pure H 2 O, but sol. when warmed with H 2 O containing HC1, with formation of a new double salt. (Christensen.) mercuric chloride, Cr(NO 2 )(NH3) 6 Cl 2j 2HgCl 2 . Precipitate. Decomp. by long contact with H 2 O. (Christensen.) chromate, Cr(N0 2 )(NH 8 ) 6 CrO 4 . Difficultly sol. in H 2 O. (Christensen.) bichromate, Cr(N0 2 )(NH 3 ) 6 Cr 2 O7. Difficultly sol. in H 2 O. (Cliristensen.) dithioriate, Cr(NO 2 )(NH 3 ) 6 S 2 O 6 . Insol. in cold H 2 O. (Christensen.) hydroxide, Cr(N0 2 )(NH 3 ) 6 (OH) 2 . Known only in solution. (Christensen.) iodide, Cr(NO 2 )(NH 3 ) 5 I 2 . Quite difficultly sol. in H 2 O. (Christensen.) nitrate, Cr(NO 2 )(NH 3 ) 6 (N0 3 ) 2 . Sol. in about 150 pts. H 2 O. (Christensen.) sulphate, Cr(NO 2 )(NH 3 )5SO 4 +H 2 O. Sol. in H 2 O and (NH 4 ) 2 SO 4 +Aq. (Chris- tensen.) Xanthocobaltic bromide, Co(NH 3 ) 6 (NO 2 )Br 2 . Easily sol. in cold H 2 O. (Werner and Miolati, Gazz. ch. it. 23, 2. 140.) bromonitrate, Co(NO 2 )(NH 3 ) 6 (NO 3 )Br. SI. sol. in cold, more easily in hot H 2 O. (Gibbs.) chloride, Co(NO 2 )(NH 3 ) 6 Cl 2 . SI. sol. in cold H 2 O, and decomp. by boiling therewith. Insol. in HCl+Aq and alkali chlorides +Aq. Easily decomp. by boiling with acids, even dilute. (Gibbs and Genth.) Sol. in 50 pts. cold H 2 O. (Jorgensen, Z. anorg. 6. 172.) . mercuric chloride, Co(NO 2 )(NH 3 ) 6 Cl 2 , 2HgCl 2 +H 2 0. Insol. in cold, sL sol. in hot H 2 O without decomp. More sol. in acidified H 2 O. (Gibbs and Genth.) 1116 XANTHOCOBALTIC CHLORAURATE Xanthocobaltic chloraurate, Co(NO 2 )(NH 3 ) 5 Cl 2 , AuCl 3 +H 2 O. Can be easily crystallised out of hot H 2 O. (Gibbs and Genth, Sill. Am. J. (2) 24. 90.) chloronitrate, Co(NO 2 )(NH3)5(NO 3 )Cl. SI. sol. in cold;, more easily in hot H 2 O. chloronitrate gold chloride, Co(N0 2 )(NH 3 )5(N0 3 )Cl, AuCl 3 . chloronitrate platinic chloride, 2Co(NO 2 )(NH 3 ) 6 (NO 3 )Cl, PtCl 4 . chloroplatinate, Co(NO 2 )(NH 3 ) 6 Cl 2 , PtCl 4 +H 2 0. Scarcely sol. in hot or cold H 2 0. Can be recryst. from dil. HNQa+Aq. Sol. in hot dil. HCl+Aq. (Gibbs and Genth, Sill. Am. J. (2) 24. 91.) chromate, Co(NO 2 )(NH 3 ) 6 CrO 4 +H 2 O. Very si. sol. in cold, and but slightly sol. in hotH 2 O. (Gibbs.) bichromate, Co(NO 2 )(NH 3 ) 5 Cr 2 O 7 . Easily sol. in hot H 2 O. ferrocyanide, [Co(NO 2 )(NH 3 ) 6 ] 2 Fe(CN) 6 +7H 2 0. Nearly insol. in cold, decomp. by warm H 2 O. +6H 2 O. (Braun, A. 132. 47.) iodide, Co(N0 2 )(NH 3 ) 5 I 2 . Sol. in H 2 O. (Gibbs.) iodosulphate, [Co(NO 2 j(NH 3 ) 5 ] 2 (SO 4 )I 2 . Sol. in H 2 O. periodosulphate, [Co(N0 2 )(NH 3 ) 6 ] 2 (S0 4 )l4. Easily decomp. by hot H 2 O. nitrate, Co(NO 2 )(NH 3 ) 6 (NO 3 ) 2 . SI. sol. in cold, moderately sol. in hot H 2 O. Decomp. by boiling. Much less sol. than NH 4 C1 or (NH 4 ) 2 SO 4 in cold H 2 O. Insol. in HNO 3 . (Gibbs and Genth.) nitrite, Co(N0 2 )(NH 3 ) 5 (N0 2 )2+2H 2 0. Sol. inH 2 O. (Gibbs.) cobaltic nitrite, Co(NO 2 )(NH 3 ) 5 (NO 2 ) 2 +2H 2 0. SI. sol. in H 2 O. (Gibbs, Proc. Am. Acad. 11. 8.) Is nitratopurpureocobaltic cobaltic nitrite, [(NO 3 )Co(NH 3 ) 8 j3[Co(NO 2 )6] 2 +2H 2 O. (Jor- gensen, Z. anorg. 6. 175.) [Co(NO 2 )(NH 3 )5]3[Co(NO 2 ) 6 ] 2 . Not so difficultly sol. as the luteo salt. (Jorgensen.) Xanthocobaltic famine cobaltic nitrite, Co 2 (N0 2 ) 2 (NH 3 )io[Co 2 (NH 3 ) 4 (NO 2 ) 8 ] 2 . Can be recryst. from hot H 2 0. (Gibbs, Proc. Am. Acad. 11. 8.) = (N0 2 )Co(NH 3 ) 6 [(Np 2 ) 2 (NH 3 ) 2 Co(N0 2 ) 2 ] 2 . Xanthocobaltic famine cobaltic nitrite. Very si. sol. in cold H 2 O. (Jorgensen, Z. anorg. 5. 180.) oxalate, Co(NO 2 )(NH 3 ) 6 C 2 O 4 , Nearly insol. in cold, si. sol. in hot H 2 O. _ sulphate, Co(NO 2 )(NH 3 ) 5 SO 4 . Moderately sol. in hot, much less in cold H 2 O. Sol. without decomp. in H 2 SO 4 +Aq. (Gibbs and Genth.) Sol. in 25 pts. hot H 2 O acidified with HC 2 H 3 O 2 . (Jorgensen, Z. anorg. 6. 172.) 4Co(NO 2 )(NH 3 ) 5 SO 4 , 3H 2 SO 4 . Decomp. by H 2 O, not by absolute alcohol. (Jorgensen.) Xanthorhodium bromide, (NO 2 )Rh(NH 3 ) 5 Br 2 . Moderately sol. in H 2 O. (Jorgensen, J. pr. (2) 34. 394.) -chloride, (NO 2 )Rh(NH 3 ) 6 Cl 2 . Much more sol. in' H 2 O than the nitrate. - chloroplatinate, (NO 2 )Rh(NH 3 ) 5 PtCl 6 . Ppt. Extremely si. sol. in cold H 2 O. dithionate, (NO 2 )Rh(NH 3 ) 5 S 2 O 6 +H 2 O. Nearly insol. in H 2 O. fluosilicate, (NO 2 )Rh(NH 3 ) 5 SiF 6 . Ppt. hydroxide, (NO 2 )Rh(NH 3 ) 5 (OH) 2 . nitrate, (N0 2 )Rh(NH 3 ) 6 (NO 3 ) 2 . Moderately sol. in cold, easily in hot H 2 O. Insol. in alcohol. Less sol. in cone. NH 4 OH + Aq than in H 2 O. Insol. in dil. HNO 3 +Aq; sol. in HNO 3 +Aq of 1.4 sp. gr. oxalate, (NO 2 )Rh(NH 3 ) 6 C 2 O 4 . Nearly insol. in cold H 2 O. Very si. sol. in warm H 2 0. Easily sol. in dil. HC 2 H 3 O 2 +Aq. sulphate, (NO 2 )Rh(NH 3 ) 6 SO 4 . Slowly sol. in cold, quite easily in hot H 2 O. 4(NO 2 )Rh(NH 3 )5SO 4 , 3H 2 SO 4 . SI. sol. in cold, easily in hot H 2 O. Can be recrystal- lized from dil. H 2 SO 4 +Aq. ZINC 1117 Xenon, Xe. Absorption by H 2 O at t. t Absorption -coefficient 10 20 30 40 50 0.2189 0.1500 0.1109 0.0900 0.0812 0.0878 (Antropoff, Roy. Soc. Proc. 1910, 83. A, 480.) Ytterbium, Yb. Ytterbium bromide, YbBr 3 +8H 2 O. Very sol. in H 2 O. Hydroscopic. (Cleve, Z. anorg. 1902, 32. 135.) Ytterbium chloride, YbCl 3 +6H 2 O. Very sol. in H 2 O. (Cleve, Z. anorg. 1902, 32. 134.) Mpt. 150-155. Anhydrous salt is sol. in H 2 O and in alcohol. (Matignon, A. ch. 1906, (8) 8. 442.) Ytterbium oxide, Yb 2 O 3 . Slowly attacked by cold or warm acids, but easily sol. at 100. Ytterbium oxychloride, YbOCl. Ppt. (Cleve, Z. anorg. 1902, 32. 135.) Yttrium, Y. Decomposes H 2 O. (Cleve, Bull. Soc. (2) 21. 344.) Decomp. H 2 O slightly at ord. temp., more rapidly by boiling. Easily sol. in dil. acids, even acetic acid. Slightly acted upon by cone. H 2 SO 4 . Decomposes hot KOH-f-Aq and cold NH 4 Cl+Aq. Not attacked by NH 4 OH+Aq. (Popp, A. 131. 179.) Popp's yttrium contained erbium. Yttrium bromide, YBr 3 . Sol. in H 2 O with evolution of heat. (Du- boin, C. R. 107. 243.) +9H 2 O. Deliquescent. Easily sol. in H 2 O and alcohol. Insol. in ether. (Cleve.) Yttrium carbide, YC 2 . Decomp. by H 2 O and by dil acids; very slowly attacked by cone, acids. (Moissan, C. R. 1896, 122. 575.) Decomp. by H 2 O and dil. acids. (Petters- son, B. 1895, 28. 2421.) Yttrium chloride, YC1 3 . Anhydrous. Sol. in H 2 O with evolution of heat. (Cleve.) +6H 2 O. Deliquescent. Very sol. in H 2 O. SI. sol. in alcohol. Insol. in ether. (Cleve.) Mpt. 156-160; sol. in alcohol. 60.1 grams anhydrous salt are sol. in 100 grams of abs. alcohol at 15. 6,5 grams are sol. in 100 grams pyridine. (Matignon, A. ch. 1906, (8) 8. 437.) Yttrium fluoride, YF 3 +^H 2 O. Nearly insol. in dil. acids. (Cleve.) Yttrium hydroxide, Y 2 O 3 , 6H 2 O or Y 2 O 6 H 6 -f 3H 2 O. Insol. in H 2 O. Insol. in KOH or NaOH+Aq. Easily sol. in acids. Sol. in alkali carbonates +Aq. When freshly pptd., easily sol. in NH 4 C1+ Aq. Yttrium iodide, YI 3 . Very deliquescent. Easily sol. in H 2 O and alcohol. SI. sol. in ether. (Cleve.) Yttrium oxide, Y 2 3 . Insol. in H 2 O. SI. sol. in cold HC1, HNO 3 , or dil. H 2 SO 4 +Aq, but gradually completely sol. on warming. Insol. in NH 4 OH and si. sol. in KOH+Aq. Sol. in HC 2 H 3 O 2 +Aq. Somewhat sol. in K 2 CO 3 +Aq. Yttrium peroxide, Y 4 O 9 . (Cleve, Bull. Soc. (2) 43., 53.) Yttrium oxychloride, Y 2 O 2 C1 2 . Insol. in H 2 O. (Popp.) Yttrium sulphide, Y 2 S 3 . Not prepared in pure state. Impure is insol. in H 2 O, and partially decomp. thereby. Easily sol. in acids with decomp. (Popp.) Zinc, Zn. Not attacked by pure cold H 2 O. Slowly oxidised by boiling H 2 O. Pure H 2 O free from O dissolved nothing from 2500 sq. mm. Zn. Presence of air containing CO 2 caused a solu- tion of 3.5 mg. Zn, which maximum was reached in 2 days. Air without CO 2 also caused a slight action. (Snyders, B. 11. 936.) 100 ccm. distilled H 2 O dissolved 14 mg. Zn from 11.8 sq. cm. in one week, during which air free from CO 2 was passed through the liquid, and 19 mg. when air containing CO 2 was used. (Wagner, Dingl. 221. 260.) Filtered rain water was found to contain 20 mg. Zn per 1. (Burg, Isis, 1873. 119.) Very pure H 2 O, when conducted through a great length of galvanized iron pipe, con- tained 1.7 pts. Zn to 100,000 pts. H 2 O. (Davies, J. Soc. Chem. Ind. 1899, 18. 102.) Action of H 2 O on Zn in galvanized pipes is caused by electrolysis. (Smetham, C. N. 1879, 39. 236.) All kinds of H 2 O attack Zn, rain water the least. In distilled H 2 O exposed to air Zn is abun- 1118 ZINC dantly coated with ZnCO 3 , 2ZnO+3H 2 O. By allowing 32 g. Zn to stand in 270 cc. distilled H 2 O in a flask loosely stoppered with filter paper, 1.2 pts. Zn to 100,000 pts. H 2 O was found in solution in 1-2 days. (Smith, J. Soc. Chem. Ind. 1904, 23. 475.) Sol. in all acids. Very slowly sol. in dil, HC1 or H 2 SO 4 +Aq in glass vessels if Zn is pure. According to Jacquelain, 24 hours were necessary to dissolve 6 g. pure tfinc. When fused at the lowest possible temperature, it is much more slowly sol. than when heated to a red heat. In both cases it is much more rapidly dissolved if cooled quickly. (Bolley, A. 96. 294; Rammelsberg.) Dil. H 2 SO 4 +Aq dissolves given % zinc in the same length of time (B= according to Bolley, R according to Rammelsberg) Slowly cooled Rapidly cooled B R B R Cast at the melt- ing point 42 . 5 74 . 1 13 . 0.9 Cast at a red heat 100.0 69.4 85.5 9.5 50 ccm. H 2 SO 4 +Aq dissolved in 2 hours the following amts. from 1 sq. cm. Zn at t. t Strength of acid Grms. dissolved 20 H 2 SO 4 0.000 130 n 0.075 150 a 0.232 20 H 2 SO 4 +H 2 O 0.002 130 u 0.142 150 0.345 20 H 2 SO 4 +2H 2 0.002 130 4.916 150 " 5.450 20 H 2 SO 4 +3H 2 O 0.005 130. 3.080 20 H 2 SO 4 +4H 2 O 0.049 130 u 0.456 20 H 2 SO 4 +5H 2 O 0.027 130 u 0.337 20 H 2 SO 4 +6H 2 O 0.018 100 " 3.16 (Calvert and Johnson, Chem. Soc. 19. 437.) C. P. zinc is more quickly sol. in dil. acids in vacuo than under normal pressure, the ratio being about 1 : 6.5. The rate of solubil- ity increases slowly with rise of temp, from to 98, when it amounts to about 4 times that at 0, but from 98-100 the increase is thirteenfold. Thus, as an average of 6 ex- periments,, dil. H 2 SO 4 +Aq (1:20) dissolves in 30 minutes 2.1 mg. Zn at 0; 4.9 mg. at 20 7.4 mg. at 60; 9.3 mg. at 98; but 122.1 mg! at 100. If, however, the acid was prevented from boiling by increasing the pressure, the sudden increase between 98 and 100 does not take place. The rate of solubility in dil. H 2 SO 4 +Aq (1 : 20) is also increased 175 times by the addi- tion of CrO 3 and 306 times by the addition of H 2 2 . The above phenomena are ex- plained by assuming the formation of a condensed hydrogen atmosphere around the metal, which prevents the further action of the acid. (Weeren, B. 24. 1785.) Not attacked by HNO 3 +Aq of 1.512 to 1.419 sp. gr. at a temp, of 18 or less, but violently attacked if temp, is raised. HNO 3 + Aq of 1.419-1.401 sp. gr. does not attack Zn at temp, of a freezing mixture, but violently at 0. More dil. HNO 3 +Aq attacks Zn even at 20. (Millon, A. ch. (3) 6. 99.) Sol. in H 2 CO 3 +Aq. (Berzelius.) Solubility of Zn in acids is very much affected by the presence of small quantities of various metallic salts. Small amts. of PtCl 4 +Aq accelerated the action of H 2 SO 4 + Aq 149 times, and As 2 O 3 123 times. HgCl 2 has a strong retarding action owing to pptn. of Hg on the Zn. The rate of solution of Zn in acids and the effect of changes in concentration and tem- perature and of the presence of inorganic salts and organic substances on this rate has been studied. 26 Tables are given. (Ericson- Aure*n, Z. anorg. 1901, 27. 209-253.) . Speed of solution in H 2 SO 4 and in HC1. (Centnerszwer, Z. phys. Ch. 1914, 87. 692.) Various saline solutions have a strong sol- vent power in presence of PtCl 4 , i.e. KC1, NaCl, Na 2 S0 4 , K 2 SO 4 , MgSO 4 +Aq. PtCl 4 also causes Zn to decompose distilled H 2 O. CuSO 4 hae a similar but less energetic effect. In all the above cases the disengagement of hydrogen is slower in the dark than in the light. (Millon, C. R. 21. 37.) According to Barreswill (C. R . 21. 292) the above reactions are all caused by galvanic action due to pptd. metal, and a piece of Pt in contact with the Zn causes the same action as the PtCl 4 in solution. Easily sol. in alkalies +Aq, even NH 4 OH+ Aq, especially when the Zn is in contact with Fe. Sol. m"NaCl-fAq with pptn. of ZnO. (Siersch, J. B. 1867. 257.) Sol. in sat. alkali and alkali-earth chlorides +Aq. (Post, 1872.) Sol. in NH 4 salts+Aq. (Lorin, J. B. 1865. 124.) Sol. in sat. Na 2 SO 4 , K 2 SO 4 , MgSO 4 , NaNO 3 , KNO 3 , Ba(NO 3 ) 2 , CaCl 2 , MgCl 2 , and NH 4 NO 3 +Aq. Chlorides and sulphates (especially Na 2 SO 4 and MgCl 2 ) have strong- est action, MgSO 4 and nitrates the least. The action was greatly increased by heat. (Sny- ders, B. 11. 936.) Sol. in boiling NH 4 Cl+Aq. Sol. in neutral FeCl 2 +Aq with pptn. of Fe, especially easily at 100. (Capitaine, C. R. 9. 737.) Sol. in NiSO 4 +Aq with pptn. of NiO. (Tupputi.) Sol. in cone, hot ZnCl 2 +Aq, but Zn oxy- ZINC BROMIDE 1119 chloride is pptd. on diluting. (Ordwav, Am. J. Sci. (2) 23. 222.) Sol. in GlSO 4 +Aq. (Debray.) Solubility of Zn in dilute solutions of salts: 100 ccm. of solutions of the given salts were allowed to act one week on 11.8 sq. cm. Zn while a current of air with or without CO 2 was passed through the solution. Salt G. salt in 100 ccm. solution Mg. Zn dissolved without CO2 Mg. Zn dissolved with COz NaCl } or 0.5 7 38 KC1 J NH 4 C1 1.0 51 36 MgCl 2 0.83 18 54 K 2 SO 4 1.0 30 53 KNO 3 1.0 9 37 Na 2 CO 3 1.0 13 NaOH 0.923 60 CaO 2 H 2 Sat 3 (Wagner, Dingl. 221. 260.) Action of dil. salt solutions (1%) on Zn. The following amts. of Zn in mg. were dis- solved from 2500 sq. mm. Zn in 14 days by 400 ccm. 1% solution of the given salts : Violently decomp. by dil. HC1 or H 2 SO 4 +Aq, also by HNO 3 +Aq. Completely sol. in HC1 +Aq mixed with a little HNO 3 . (Cooke.) Zinc azoimide, basic, Zn(OH)N 8 . Very si. sol. in H 2 O. Decomp. by hot H 2 O. (Curtius, J. pr. 1898, (2) 68. 293.) Zinc azoimide ammonia, ZnN 6 , 2NH 8 . Insol. in H 2 O, but gradually decomp. thereby. (Dennis, J. Am. Chem. Soc. 1907 29. 20.) Zinc bromide, ZnBr 2 . Very deliquescent, and sol. in H 2 O. Sat. ZnBr 2 +Aq contains at: 20 +4 22 97 66.3 68.8 77.5 83.6%ZnBr 2 , 107 170 210 375 (mpt.) 83.8 85.0 89.3 100% ZnBr 2 . (Etard, A. ch. 1894, (7) 2. 541.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 35 40 60 80 100 85.45 85.53 86.08 86.57 87 . 05 g. ZnBr 2 . (Dietz, Z. anorg. 1899, 20. 250.) Salt Mg. Zn Salt Mg. Zn Sp. gr. of ZnBr 2 +Aq at 19. 5 containing NaCl . KC1 . . CaCl 2 . . 11.2 14.8 15.2 NaNO 3 Ba(NO,), . . NH 4 C1 . . 6 8 24.0 18.3 1 . 1849 ] 31.7 .3519 43.2 % ZnBr 2 , 1.5276 MgCl 2 . . BaCl 2 . . K 2 SO 4 MgSO 4 . 17.2 13.2 12.0 8.8 (NH 4 ) 2 SO 4 ... NH 4 N0 3 . . NaHCO, . . K 2 CO 3 . . 31.6 26.0 52.6 59.1 68 % ZnBr 2 . 1.7082 1.8525 2.1027 (Kremers, Pogg. 108. 117.) KNO 3 6.8 Na 2 CO 3 . . Sn jrr. of ZnBr 9 +Aa at 19.5. SI attacked by H 2 O at 80, bv hot cone. NH 4 OH; attacked by H 3 PO 4 or NaCl+Aq; ZnBr 2 Sp. gr. ZnBr 2 Sp. gr. % ZnBr2 Sp. gr. very si. attacked by NaNO 3 +Aq or KNO 3 + Aq at 100. (Smith, J. Soc. Chem. Ind. 1904, 23 476 ) 5 10 1.045 1.093 25 30 1.265 1.330 45 50 1.560 1.650 % ccm. oleic acid dissolves 0.0210 g. Zn 15 1.196 35 1.400 55 1.755 in 6 days. (Gates, J. phys. Chem. 1911, 16. 20 1.204 40 1.475 60 1.875 Attacked by cane sugar +Aq at 115 (Kremers, calculated by Gerlach, Z. anal. 8. (Klein and Berg, C. R. 102. 1170.) 285.) Zinc amide, Zn(NH 2 ) 2 . Decomp. by H 2 O and alcohol. Insol. in ether. (Frankland, Phil. Mag. (4) 15. 149.) Zinc antimonide, ZnSb. Does not decomp. boiling H 2 O except slightly. Not attacked by dil. mineral acids but decomp. by cone. HC1 or HNO 3 +Aq (Cooke, Proc. Am. Acad. 6. 348.) Zn 3 Sb 2 . Decomp. H 2 O rapidly at 100 Sol. in cone. HC1 or HC 2 H 3 O 2 +Aq, also in NH 4 OH+Aq. Sol. in AlBr 3 . (Isbekow, Z. anorg. 1913. 84 27 ) Very si. sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Sol in alcohol and ether. (Berthemot, J. Pharm. 14. 610.) Sol in methyl acetate. (Naumann, B. 1909, 42. 3790.) 1120 ZINC BROMIDE AMMONIA Insol. in ethyl acetate. (Naumann, B. 1910, 43. 314.) More sol. in anhydrous ether than in abs. alcohol. Insol. in CS 2 . (Hampe, Ch. Z. 1887, 11. 846.) Sol. in quinoline. (Beckmann and Gabel. Z. anorg. 1906, 61. 236.) Mol. weight determined in pyridine. (Werner, Z. anorg. 1897, 16. 22.) +H 2 O. (Lescoeur, A. ch. 1894, (7) 2. 78.) -j-2H 2 O. Very hygroscopic. Solubility in H 2 O. 100 g. of the sat. solution contain at: 8 13 25 30 37(mpt.) 79.06 79.55 80.76 82.46 84.08 86.20 g. ZnBr 2 . (Dietz, Z. anorg. 1899, 20. 250.) +3H 2 O. Solubility in H 2 O. 100 g. of the sat. solution contain at: 15 10 5 (mpt.) 77 .13 78 . 45 80 . 64 g. ZnBr 2 . (Dietz, Z. anorg. 1899, 20. 250.) ammonia, Zinc bromide Decomp. by H 2 O easily in berg, Pogj ZnBr 2 , 2NH 3 . SI. sol. in cold, more warm NH 4 OH+Aq. (Rammels- ;. 65. 240.) ). Decomp. by H 2 O with separa- tion of ZnO. (Andre ; C. R. 96. 703.) +H 2 O. Above salt of Rammelsberg's has this composition. (Andre*.) 3ZnBr 2 , 8NH 3 +2H 2 O. Decomp. by H 2 O. (Andre".) 3ZnBr 2 , 10NH 3 +H 2 O. Decomp. by H 2 O. (Andre-.) 2ZnBr 2 . 10NH 3 . Efflorescent. Decomp. by H 2 O. ' (Andre*.) Zinc bromide cupric oxide, ZnBr 2 , 3CuO-f 2H 2 O. +4H 2 O. (Mailhe, C. R. 1901, 133. 227.) Zinc bromide hydrazine, ZnBr 2 , 2N 2 H 4 . Decomp. by H 2 O. Sol. in NH 4 OH+Aq. (Franzen, Z. anorg. 1908, 60. 277.) Zinc chloride, ZnCl 2 . Very deliquescent, and sol. in H 2 O. Sol. in 0.333 pt. H 2 O at 18.75. Abl.) ZnCh+Aq sat. at 12.5 contains 78.5% ZnCl 2 . (Hassenfratz, A. ch. 28. 291.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 15 20 41 60 100 79.12 81.19 82.21 83.51 86.01 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) ZnCl 2 +Aq containing 1 pt ZnCl 2 in 1.8205 pts. H 2 O at 18 has sp. gr. = 1.3666. (Hit- torf, Z. phys. Ch. 1902, 39. 628.) Solubility in H 2 O at t. 100 g. H 2 O dissolve g. ZnCl 2 . t Solid phase ZnCl 2 5 ice 14 10 25 40 " 83 -62 50 ice:4aq ZnCl 2 +4H 2 104 113 ' cryohydrate point 40 127 30 4aq:3aq 160 transition point -10 ZnCl 2 +3H 2 189 " 208 +5 " 230 6.5 " 252 mpt. 5 " 282 3aq:lKaq 309 eutectic point ZnCl 2 +2 J^H 2 O 235 6.5 2>aq:3aq 252 transition point 10 ZnCls +2^H 2 O 272 12.5 " 303 mpt. 11.5 2^aq:l^aq 335 eutectic point 9 2^aq:laq 360 eutectic point 6 ZnCl 2 +2^H 2 O 385 -6 ZnCl 2 +lHH 2 O 298 + 10 " 330 20 M 368 26 13^aq:laq 423 transition point 26.3 l>iaq:ZnCl 2 433 transition point ZnCl 2 +H 2 342 10 364 20 " 396 28 laq:ZnC! 2 436 transition point 31 ZnCl 2 +H 2 477 25 ZnCh 432 40 " 452 60 " 488 80 " 543 100 . ' " 615 262 mpt. (Mylius and Dietz, Z. anorg. 1905, 44. 217.) See also below under hydrated salts. Sp. gr. of ZnCl 2 +Aq at 19.5. % ZnCl 2 Sp. gr. % ZnCh Sp. gr. 1.3859 1.5551 13.8 25.8 1 . 1275 1.2466 37.5 49.2 CKremers, Fogg. 106. 360.) Sp. gr. of ZnCl 2 +Aq at 19.5. % ZnCh 1 5 10 15 20 Sp. gr. 1.010 1.045 1.091 1.137 1.186 7o ZnCh Sp. gr. % ZnCh Sp. gr. 25 30 35 40 1.238 1.291 1.352 1.420 45 50 55 60 1.488 1.566 1.650 1.740 (Gerlach, Z. anal. 8. 283, calculated from Kremers.) Sp. gr. of ZnCl 2 +Aq at t. t 15 15 15 15 ZnCl 2 2.5 4.89 10.0 20.0 p.gr. 1.024 1.046 1.094 1.190 t 15 15 15 %ZnCl 2 29.86 40.0 58.88 Sp.gr. 1.297 1.423 1.728 (Long, W. Ann. 1880, 11. 38.) ZINC HYDRAZINE CHLORIDE 1121 Sp. gr. of ZnCl 2 +Aq at room temp, con- taining: 15 . 334 23 . 487 33 . 752% ZnCl 2 . 1.1459 1.2288 1.3431 (Wagner, W. Ann. 1883, 18. 267.) / Sp.gr. ofZnCl 2 +Aqat25. Concentration of ZnCh +Aq Sp. gr. 1 normal V* " '/4 " Vs " 1.0590 1.0302 1.0152 1 . 0077 (Wagner, Z. phys. Ch. 1890, 5. 40.) Sp. gr. of ZnCl 2 +Aq. Yi ZnCh g. in 1000 g. of solution Sp. gr. 16/16 1.000000 0.5994 1.000560 2.3163 1.002163 5.0406 1.004708 9.8988 1.009243 19.4914 1.018228 (Dijken, Z. phys. Ch. 1897, 24. 108.) Insol. in SbCl 3 . (Klemensiewicz, C. C. 1908, II. 1850.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Easily sol. in hot absolute alcohol, and ether. Sol. in 1 pt. strong alcohol at 12.5. (Wenzel.) Sol. in 0.35 pt. absolute alcohol. (Graham .) Sol. in butyl (Wurtz), and hexyl (Bouis) alcohol at ord. temp., but decomp. on heating. Very sol. in acetic ether with evolution of heat. (Cann, C. R. 102. 363.) Easily sol. in acetone. (Krug and M'El- roy, J. Anal. Ch. 6. 184.) 1 g. ZnCl 2 is sol. in 2.3 g. acetone at 18. Sp. gr. of sat. solution 18/4 = 1.14. (Nau- mann, B. 1904, 37. 4338.) Sol. in acetone and in methylal. (Eidmann, C. C. 1899, II. 1014.) Sol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Sol. in hot benzonitrile, also in other aro- matic nitriles. Sol. in methyl sulphide and in ethyl sul- phide. Very sol. in piperidine. (Werner, Z. anorg. 1897, 16. 7.) Sol. in benzyl alcohol, furfurol, methyl- propylketone, acetophenone, ethyl mono- chloracetate, ethyl cyanacetate, ethyl aceto- acetate, ethyl benzoate, ethyl oxalate, amyl nitrite, pyridine, piperidine, and quinoline. Insol. in salicylic aldehyde, ethyl nitrate, and nitrobenzene. (Lincoln, J. phys. Chem. 1899, 3. 460.) Sol. in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 51. 236.) Sol. in 2 pts. glycerine at ord. temp. (Clever, Bull. Soc. 1872, (2) 18. 372.) 100 g. glycerol dissolve 50 g. ZnCl 2 at 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) Insol. in CS 2 . (Arctowski, Z. anorg. 1894, 6. 257.) Sol. in urethane. (Castoro, Z. anorg. 1899, Mol. weight determined in piperidine; pyridine and methyl sulphide. (Werner, Z. anorg. 1897, 16. 18.) +H 2 O. Very deliquescent. Contains 1 1 A H 2 O. (Engel, C. R. 102. 1111.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 11 27 (mpt.) 74.33 78.25 84.61 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) . Solubility in H 2 O. 100 g. of the sat. solution contain at: 10 20 26 (mpt.) 67.45 73.65 80.08 83.43 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) +2H 2 O. Sat. aq. solution contains at: 20 14 10 4 1 54.7 55.4 56.5 57.4 57.9% salt, +5 9 15 33 42 59.1 60.2 62.0 66.8 68. 3% salt. (Etard, A. ch. 1894, (7) 2. 536.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 10 19 (mpt.) 67 .56 73 . 70 79 . 07 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) . Solubility in H 2 O . lOd g. of the sat. solution contain at: 8 13 (mpt.) 67.42 71.96 75. 14 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) +3H 2 O. Sol. in 12.5 pts. H 2 O at 0. (Engel.) Solubility in H 2 O. 100 g. of the sat. solution contain at: 5 +7 (mpt.) 64.5 67.58 71 . 57 g. ZnCl 2 . (Dietz, Z. anorg. 1899, 20. 245.) Zinc hydrogen chloride, 2ZnCl 2 , HC1+2H 2 0. Deliquescent. (Engel, C. R. 102. 1068.) ZnCl 2 , HC1+2H 2 O. (Engel.) Zinc hydrazine chloride, ZnCl 2 , N 2 H 4 , HC1. Very hydroscopic. Sol. in H 2 O. (Curtius, J. pr. 1894, (2) 60. 338.) 1122 ZINC CHLORIDE AMMONIA ZnCl-2. 2(N 2 H,, HC1.) Hydroscopic; very sol. in H 2 O. Sol. in hot alcohol and NH 4 OH+Aq. (Cur- tius, J. pr. 1894, (2) 50. 338.) Zinc chloride ammonia, ZnCl 2 , 5NH 3 +H 2 0. Easily sol. in little, but decomp. by much H 2 O. Still more sol.' in ZnCl 2 +Aq with de- comp. (Divers, C. N. 18. 13.) ZnCl 2> 4NH 3 +H 2 O. (Kane.) ZnCl 2 , 2NH 3 . Not completely sol. in H 2 O can be recryst. from hot NH 4 Cl+Aq. (Ritt- hausen, J. pr. 60. 473.) Insol.inH 2 O. Sol. in NH 4 C1 or NH 4 OH+ Aq. (Thomas, B. 20. 743.) +VAO. + 2 / 6 H 2 0. +V 2 H 2 0. +H 2 0. (Andre", C. R. 1882, 94. 964.) Decomp. by H 2 O. ZnCl 2 , NH 3 . ch. 72. 290.) Decomp. by H 2 O. (Kane, A*. Zinc chloride cupric oxide, ZnCl 2 , 3CuO + 4H 2 O. (Mailhe, C. R. 1901,. 134. 226.) Zinc chloride hydrazine, ZnCl 2 , 2N 2 H 4 . Ppt. (Franzen, Z. anorg. 1908. 60. 275.) ZnCl 2 , 2N 2 H 4 . Insol. in H 2 O. Easily sol. in NH 4 OH-f Aq. (Curtius, J. pr. 1894, (2) 60. 345.) Zinc chloride hydroxylamine, ZnCl 2 , 2NH 2 OH. SI. sol. in cold, somewhat more in warm H 2 O. Very sol. in NH 2 OH+Aq. Very si. sol. in alcohol and other organic solvents. (Crismer, Bull. Soc. (3) 3. 116.) 1 pt. is dissolved in 100 pts aq. solution sat. at 20. (Antonoff, C. C. 1906,, II. 810.) Zinc fluoride, ZnF 2 . SI. sol. in cold, more easily in ho,t H 2 O. Insol. in 95% alcdhpl. Sol. in boiling HNO 3 , HC1, or H 2 S0 4 . (Poulenc, C. R. 116. 581.) Contrary to older statements, ZnF 2 is quite sol. in H 2 O. CKohlrausch, Z. phvs. Ch. 1903, 44. 213.) Insol. in liquid NH 3 . (Gore, Amy Ch J 1898, 20. 830.) Insol. in methyl acetate. (Naumann. B. 1909, 42. 3790.) +4H 2 O. Difficultly sol. in H 2 O. Some- what more sol. in H 2 O containing HF, HC1, or HNO 3 . Easily sol. in NH 4 OH+Aq. (Berzelius, Pogg. 1. 26.) 1 1. H 2 O dissolves 16 g. at 18. (Dietz) Zinc hydrogen fluoride. Known only in solution. Zinc zirconium fluoride. See Fluozirconate, zinc. Zinc hydrophosphide, Zn 2 H 2 P 2 . Decomp. by cold H 2 O and by dil. HCl+Aq. (Drechsel and Finkelstein, B. 1871, 4. 353.) Zinc hydroxide, Zn0 2 H 2 . Insol. in H 2 O. Sol. in acids. Sol. in KOH. NaOH, NH 4 OH, or (NH 4 ) 2 CO 3 +Aq. 1 1. H 2 O dissolve 0.01 g. ZnO 2 H 2 at 25. (Bodlander, Z. phys. Ch. 1898, 27. 66.) Solubility in H 2 O is calculated to be 2.6 X 10:, 5 g. mols. per 1. (Herz, Z. anorg. 1900, 23. 227.) 1 1. H 2 O dissolves 0.0042 g. ZnO 2 H 2 at 18. (Dupre and Bialas, Z. angew. Ch. 1903, 16. 55.) See also Zinc oxide. Solubility in NH 4 OH+Aq at 25. ZnO 2 H 2 used NHs norm. G. ZnO per 1. prepared from 1.287 7.28 ZnSO 4 0.825 3.84 0.311 0.85 prepared from Zn(N0 3 ) 2 0.321 0.643 0.34 0.845 1.215 2.70 1.928 5.07 2.570 7.01 3.213 10.16 (Bonsdorff, Z. anorg. 1904, 41. 189.) Solubility of ZnO 2 H 2 in NH 4 OH and am- monium bases +Aq at 17-19. Normality of the base G. ZnO in 20 cc. of the solution 0.0942NH 3 0.00185 0.236 NH 3 0.01795 0.707NH 3 0.0959 0.0944NH 2 CH 3 0.0008 0.472NH 2 CH 3 0.01325 0.944NH 2 CH 3 0.0484 0.068NH 2 C 2 H 5 0.0005 0.51NH 2 C 2 H 5 0.0074 0.68NH 2 C 2 H 5 0.01605 NH(C 2 H 5 ) 2 insol. NH(CH 3 ) 2 a (Herz, Z. anorg. 1902, 30. 280.) Solubility in NH 4 OH+Aq increases with ncreasing concentration of NH 4 OH. (Euler, B. 1903, 36. 3401.) 2 pts. ZnO 2 H 2 dissolve in 5 pts. KOH+Aq. sp.gr. = 1.3.) (Bonnet.) ZINC IODIDE 1123 Solubility of ZnO 2 H 2 in NaOH+Aq. Zinc iodide, ZnI 2 . Deliquescent. Easily sol. in H 2 O. Sat. ZnI 2 -f Aq contains at: 18 5 +17 47 62 73 70.9 74.0 80.4 80.3 81.3 81.2%ZnI 2 , 97 100 107 138 140 82.1 83.0 82.6 83.8% ZnI 2 . (Etard, A. ch. 1894, (7) 2. 544.) Solubility in H 2 O. G. Na in 20 ccm. G. Zn in 20 ccm. 0.1012 0.1978 0.4278 0.6670 0.9660 1.4951 2.9901 0.0040 0.0150 0.0442 0.1771 0.9630 0.2481 0.3700 When zinc hydroxide is treated with alkali, more dissolves .at first than corre- sponds with the true equilibrium under the prevailing conditions, for such solutions spontaneously deposit more or less zinc hydroxide according to the concentration. (Rubenbauer, Z. anorg. 1902, 30. 333.) Solubility of ZnO 2 H 2 in NaOH+Aq at 25 C G. mol. per 1. 1.234 Sp. 5 1.045 30 1 . 368 Na Zn 0.2636 0.3871 0.5414 0.9280 0.00311 0.0057 0.0129 0.0425 (Wood, Chem. Soc. 1910, 97. 884.) Freshly pptd. ZnO 2 H 2 is easily sol. in KOH+Aq, but it gradually goes over into a stable form which is difficultly sol. in KOH+ Aq. (Herz, Z. anorg. 1901, 28. 474.) Freshly pptd. ZnO 2 H 2 is sol. in dil. salt solutions (1 %) as follows. The given amts. in mg. (calculated as Zn) were disolved per 1. at t. Salt Mg. Zn t NaCl KC1 CaCl 2 MgCl 2 BaCl 2 . KoSO* 51 43 57.5 65 38 37.5 18 20 16 16 18 20 MgSO 4 KNO 3 NaNO 3 27 17.5 22 21 15 15 Ba(NO 3 ) 2 K 2 CO 3 NH 4 C1 NH 4 NO 3 25 95 77 21 15 20 20 (NH 4 ) 2 SO 4 88 20 (Snyders, B. 11. 936.) +H 2 0. See also Zinc oxide. Zinc hydrosulphide, Zn(SH) 2 . Very unstable. Decomp. by H 2 O. (Zotta, M. 10. 807.) Sol. in NaSH+Aq. 2044.) Zn 3 H 2 S 4 . (Zotta.) (Thomsen, B. 11. 100 g. of the sat. solution contain at: 18 40 60 80 100 81.11 81.20 81.66 82.37 83.05 83.62 g. Znl,. (Dietz, Z. anorg. 1899, 20. 251.) See also under +2H 2 O. Sp. gr. of ZnI 2 +Aq at 19.5 containing: 23.1 42.6 56.3 63.5 76.0%ZnI 2 . 1.2340 1.5121 1.7871 1.9746 2.3976 (Kremers, Pogg. 111. 61.) Sp. gr. of ZnI 2 +Aq at 19.5 containing: 10 15 20 25 %ZnI 2 , 1.045 1.091 1.140 1.196 1.255 35 1.390 40 1.420 45 1.560 50 %ZnI 2 , 1.650 75 2.360 ZnI 2 . 55 60 65 70 1.754 1.8?5 2.020 2.180 (Rremers, calculated by Gerlach, Z. anal. 8. 285.) Sol. in (NH 4 ) 2 CO 3 -f Aq. Moderately sol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Sol. in alcohol. 100 pts. glycerine disolve 40 pts. at ord. temp. (Klever, Bull. Soc. 1872, (2) 18. 372.) 100 g. glycerol dissolve 40 g. ZnI 2 at 15.5. (Ossendowski, Pharm. J. 1907, 79. 575.) More sol. in anhydrous ether than in abs. alcohol. Insol. in CS 2 . (Hampe, Ch. Z. 1887, 11. 846.) Sol. in methyl acetate (Naumann, B. 1909, 42. 3790); acetone. (Eidmann, C. C. 1899, II. 1014; Naumann, B. 1904, 37. 4328.) Sol. in quinoline. (Beckmann and Gabel, Z. anorg. 1906, 61. 236.) Mol. weight determined in methyl sul- phate. (Werner, Z. anorg. 1897, 15. 25.) +2H 2 O. Solubility in H 2 O. 100 g. of the sat. solution contain at: __!0 5 +10 22 27(mpt.) 80.50 80.77 81.16 82.06 83.12 89.52 g. ZnI 2 . (Dietz, Z. anorg. 1899, 20. 251 .) +4H 2 O. (Lubarski, Z. anorg. 1898, 18. 387.) , Znl4. Known only in aqueous solution. (Baup, Repert. 14. 412.) Sol. in fenchone. (Rimini and Olivari, C. 1907, II. 241.) 1124 ZINC IODIDE AMMONIA Zinc iodide ammonia, ZnI 2 , 4NH3. Decomp. by cold H 2 O. Easily sol. in acids and NH 4 OH+Aq. (Rammelsberg, Pogg. ZnI 2 ,'5NH 3 . Decomp. by cold H 2 O. Sol. in NH 4 OH+Aq. (Rammelsberg.) 3ZnI 2 . 5NH 3 +3H 2 O. (Tassily, C. R. 1896, 122. 324.) Zinc iodide hydrazine, ZnI 2 , 2N 2 H 4 . Decomp. by H 2 O. Sol. in NH 4 OH+Aq. (Franzen, Z. anorg. 1908, 60. 277.) Zinc nitride, Zn 8 N 2 . Decomp. by H 2 O with the greatest violence. (Frankland, Phil. Mag. (4) 16. 149.) Easily decomp. by H 2 O when finely pow- dered. (Rossel, C. R. 1895, 121. 942.) Sol. in HC1. (Fischer, B. 1910, 43. 1468.) Zinc oxide, ZnO. Insol. in H 2 O. Some preparations of ZnO are si. sol. in H 2 O, never, however, in less than 1 million pts. H 2 O. (Bineau, C. R. 41. 510.) Calculated from electrical conductivity of ZnO+Aq. 1 pt. ZnO is sol. in 236,000 pts. H 2 O at 18. (Dupre and Bialas, Zeit. angew. Ch. 1903, 16. 55.) See also Zinc hydroxide. Easily sol. in acids, even after ignition. Easily sol. in acids, even H 2 SO 3 , or H 2 CO 3 + Aq. Solubility of ZnO in CrO 3 +Aq at 25. 1 1. of the solution contains: G.CrOs 0.010 0.010 0.010 0.604 2.14 4.19 11.4 11.5 22.2 31.4 43.1 57.5 66.5 66.7 70.6 93.3 G. ZnO 0.013 0.013 0.013 0.409 1.16 2.24 5.84 5.89 10.7 14.9 20.1 26.7 30.3 30.4 32.2 41.5 G. CrO 3 101 151 192 192 285 392 450 461 463 475 574 660 769 879 970 G.ZnO 44.9 66.1 83.8 83.6 123 168 193 196 197 202 240 274 318 354 389 (Groger, Z. anorg. 1911, 70. 136.) When moist is easily sol. in KOH, NaOH, and NH 4 OH+Aq. but only si. sol. therein after ignition. Partially repptd. from solu- tion in NH 4 OH+Aq by dilution with H 2 O. Anhydrous ZnO is insol. in dil., but sol in cone, alkali hydrates +Aq, but the hy- droxide is easily sol., even in dil. alkalies +Aq (Fremy, A. ch. (3) 23. 390.) Very si. sol. in NH 4 OH+Aq. After igni- ton its solubility is greatly increased by :races of K and NH 4 salts. Phosphates have strongest action, then, in the following order: arsenates, chlorides, sulphites, ni- brates, acetates, carbonates, tartrates, cit- rates, and sulphates. Succinates and ben- zoates increase the solubility in NH 4 OH + Aq, only when it is very dil.; borates, iodides, chlorates, arsenites, gallates, and oxalates do not increase the solubility. (Schindler.) ZnO is sol. in NH 4 OH+Aq. only in pres- nce of NH 4 salts. (Brandhorst, Zeit. an- gew. Ch. 1904, 17. 513.) Solubility in KOH, NaOH, and NH 4 OH + Aq. An excess over 4 mols. KOH to 1 mol. ZnO is necessary for solution, but that excess may be neutralised after solution, until only 4 mols. are left, without pptn. of ZnO. Solu- tion is pptd. by addition of 12 vols. H 2 O. KOH+Aq containing 16.5 g. KOH to a litre H 2 is the weakest solution which will dis- solve ZnO. Three times as much alkali are necessary for solution at 50 as at 16-17. Less excess of NaOH than of KOH is neces- sary. 3 mols. NH 4 OH will dissolve 1 mol. ZnO, and the temp, and dilution are in this case of little influence. (Prescott.) 100 cc. of 20% NaOH+Aq dissolve in many hours at most 2.97 g. ignited ZnO. Pptd. ZnO is more quickly dissolved but the action becomes very slow after 100 cc. of the solution contain 3.87 g. of Zn. (Forster and Giinther, Z. Elektrochem. 1900, 6. 301.) Solubility of ignited ZnO in NaOH+Aq gradually decreases, (Kunschert, Z. anorg. 1904, 41. 343.) Sol. in hot NH 4 Cl+Aq, either when moist [>r dry. Somewhat less sol. in NH 4 NO 3 +Aq. Somewhat sol. in water glass -f Aq. (Ord- way.) Slowly sol. in cold, easily in hot NaCl+Aq. (Siersch, J. B. 1867. 255.) Solubility of ZnO in ZnCl 2 +Aq at room temp. . ZnCl 2 per 100 g. H 2 O G. ZnO per 100 g. H 2 O 8.22 23.24 45.95 51.50 56.90 62.85 96.00 124.70 144.80 203.00 0.0137 0.138 0.497 0.604 0.723 0.884 1.792 3.213 2.640 1.590 The solubility curve has a maximum at a point corresponding to about 125 g. ZnCl 2 per 100 g. H 2 O. On the first branch of the curve the solid phase in equilibrium with the solu- tion is ZnCl 2 , 4ZnO, 6H 2 O; on the second branch it is ZnCl 2 , ZnO, 1.5H 2 O. (Driot, C. R. 1910, 160. 1427.) ZINC PHOSPHIDE 1125 Sol. in boiling Fe(NO 3 ) 3 , and Pb(NO 3 ) 2 + Aq with pptn. of oxides. Not attacked by Co(N0 3 ) 2 , Ni(NO,),, and Ce(NO,),+Aq. (Persoz.) Sol. in boiling KCN+Aq. Insol. in boiling K tartrate +Aq. (Kah- lenberg and Hillyer, Am. Ch. J. 1894, 16. 101.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) Tartar ic acid somewhat hinders the pptn. of ZnO 2 H 2 . Insol. in methyl acetate. (Naumann, B. 1909, 42. 3790.) Insol. in acetone. (Naumann, B. 1904, 37. 4329; Eidmann, C. C. 1899, II. 1014.) Sol. in methyl amine, but insol. in amyl amine+Aq. (Wurtz.) 1 1. solution containing 174.4 g. sugar and 14.1 g. CaO dissoolves 0.24 g. ZnO. (Bodenberider, J. B. 1865, 600.) Min. Zincite. Sol. in acids. Zinc peroxide. 1 pt. sol. in 45,000 pts. H 2 O. Very sol. in acids. (Foregger and Philipp, J. Soc. Chem. Ind. 1906, 25. 300.) Zn0 2 (?). Ppt. Decomp. by acids with evolution of H 2 O 2 . (Haass, B. 17. 2249.) ZnO, H 2 O, H 2 O 2 . (de Forcrand, A. ch. 1902, (7) 27. 58.) 3ZnO, 2H 2 O 2 . (de Forcrand.) 3ZnO, H 2 O, 2H 2 O 2 . (de Forcrand.) 4ZnO, H 2 O, 3H 2 O 2 . (de Forcrand.) ZnO 2 , ZnO 2 H 2 . Insol. in NH 4 OH+Aq (Kouriloff, A. ch. (6) 23. 431.) 3Zn0 2 , Zn(OH) 2 . Sol. in NaOH +Aq with evolution of O. (Eijkman, C. C. 1906, I. 1628.) Zii 4 O 7 , 3ZnO+4H 2 O. Completely sol. in dil. H 2 SO 4 . (de Forcrand.) 10ZnO 2 , 4ZnO+5H 2 O. Ppt. (Teletow C. C. 1911, I. 1799.) Zinc oxybromide, ZnBr 2 , ZnO+13H 2 O. ZnBr 2 , 4ZnO + 10, 13, and 19H 2 O. De- comp. by H 2 O into ZnBr 2 , 6ZnO+35H 2 O. (Andre".) ZnBr 2 , 5ZnO+6H 2 O. (Andre*.) All oxybromides are sol. in KOH anc NH 4 OH+Aq. (Andr6, C. R. 96. 703.) Zinc oxybromide ammonia, ZnBr 2 , 3ZnO 2NH 3 +5H 2 O. Decomp. by H 2 O. (Andre*, C. R. 96. 703. Zinc oxychloride, ZnO, 3ZnCl 2 +H 2 O. Decomp. by H 2 O. Very sol. in dil. acids. (Ephraim, Z. anorg 1908, 59. 67.) +4H 2 O. SI. sol. in H 2 O; more sol. IE ZnCl 2 +Aq. Easily sol. in acids, or NH 4 OH, or KOH + Aq. (Schindler, Mag. Pharm. 36. 45.) +5H 2 O and 8H 2 O. (Andre", A. ch. (6) 3 94.) ZnO, ZnCl 2 + lMH 2 O. (Driot, C. R. 1910, 50. 1427.) 3ZnO, ZnCl 2 +2H 2 O. SI. sol. in H 2 O, nore easily sol. in ZnCl 2 +Aq. Easily sol. n acids and in NH 4 OH or KOH+Aq. Schindler, Mag. Pharm. 36. 45.) +3H 2 O. (Werner, B. 1907, 40. 4443.) +5H 2 O. (Mailhe, A. ch. 1902, (7) 27. 367.) 3ZnO, 2ZnCl 2 +llH 2 O. (Andre*, C. R. 888, 106. 854.) 4ZnO, ZnCl 2 +6H 2 O. (Andre*, C. R. 1888, 106. 854.) + 11H 2 O. (Andre, A. ch. (6) 3. 94.) 5ZnO, ZnCl 2 +6H 2 O. (Perrot, Bull. Soc. 1895, (3) 13. 976.) +8H 2 O. (Andre", C. R. 1882, 94. 1524.) 5ZnO, 2ZnCl 2 +26H 2 O. Sol. in KOH or NH 4 OH+Aq. Decomp. by H 2 O into 5ZnO, ZnCl 2 +26H 2 O. Sol. in KOH or NH 4 OH+Aq. Decomp. by H 2 O into 6ZnO, ZnCl 2 +6H 2 O. Insol. in H 2 O. :Kane, A. ch. 72. 296.) 8ZnO, ZnCl 2 + 10H 2 Q. (Mailhe, A. ch. 1902, (7) 27. 367.) 9ZnO, ZnCl 2 +3H 2 O. Insol. in H 2 O. Less sol. in NH 4 OH+Aq than ZnCl 2 , 3ZnO + 2H 2 O, but easily sol. in +14H 2 O. 9ZnO, 2ZnCl 2 + 12H 2 O. Insol. in hot or cold H 2 O. (Habermann, M. 6. 432.) Zinc oxychloride ammonia, 6ZnCl 2 , ZnO, 12NH 3 +4H 2 O. Decomp. by H 2 O and boiling alcohol. (Andre", A. ch. (6) 3. 90.) ZnCl 2 , 3ZnO, 2NH 3 +5H 2 O. Decomp. by H 2 O. (Andre*.) ZnCl 2 , 2ZnO, 2NH 3 +3H 2 O. (Andre".) 6ZnCl 2 , 3ZnO, 10NH 3 + 13H 2 O. (Andre.) 4ZnCl 2 , ZnO, 8NH 3 +2H 2 O. - (Andre.) Zinc oxyiodide, ZnI 2 , 3ZnO+2H 2 O. Insol. in cold, si. sol. in boiling H 2 O. (Muller, J. pr. 26. 441.) ZnI 2 , 9ZnO+24H 2 O. Insol. in cold H 2 O. ZnI 2 , 5ZnO + llH 2 O. Decomp. by H 2 O. (Tassilly, C. R. 1896, 122. 324.) Zinc oxyphosphide, ZnP 2 O. (Renault, A. ch. (4) 9. 162.) Probably is a mixture of zinc phosphate and phosphorus. (Vigier, Bull. Soc. 1861. 5.) Zinc oxysulphide, ZnO, ZnS. Sol. in HCl+Aq. (Arfvedson, Pogg. 1. 59.) 4ZnS, ZnO. Not decomp. by boiling HC 2 H 3 O 2 +Aq. (Kersten, Schw. J. 57. 186.) Min. Volzite. Sol. in HCl+Aq. Zinc phosphide, ZnP. Less easily attacked by HCl+Aq than ZnP 2 . Not attacked by hot HCl+Aq. (Hvoslef, A. 100. 99.) ZnP 4 . Insol. in dil. HCl+Aq. (Renault.) 1126 ZINC SELENIDE Zn 3 P 2 . Insol. in H 2 O. Sol. in dil. HC1, H 2 SO 4 , or HNO 3 +Aq, with evolution of PH 3 . (Renault, A. ch. (4) 9. 162.) Zn 3 P 4 . Insol. in HCl+Aq. (Renault.) Zinc selenide, ZnSe. Cold dil. HNO 3 +Aq dissolves out Zn, and Se separates out, which dissolves on warming as H 2 SeO 3 . (Berzelius.) +zH 2 0. Insol. in H 2 O. (Berzelius.) Zinc sulphide, ZnS. Anhydrous. Insol. in H 2 O. Sol. in HC1+ Aq; insol. in HC 2 H 3 O 2 +Aq. (Ebelmen, A. ch. (3) 26. 97.) Sol. in H 2 S+Aq under pressure in a sealed tube. (Senarmont, A. ch. (3) 32. 168.) Min. Blende, Sphalerite. SI. attacked by acids, expecting aqua regia. 1 1. H 2 O dissolves 6.65 X10- 6 mols. zinc blende at 18. 1 1. H 2 O dissolves 6.63 Xlp- 6 mols. arti- ficial cryst. ZnS at 18. (Wiegel, Z. phys. Ch. 1907, 68. 294.) Sol. in an alkaline solution of NaClO. (Sadtler, Trans. Am. Electrochem. Soc. 1902, 1. 142.) Insol. in liquid NH 3 . (Franklin, Am. Ch. J. 1898, 20. 830.) +1/2, 2 /3, or 1H 2 O. Pptd. ZnS. 1 1. H 2 O dissolves 70.60 XKH 5 mols. pptd. ZnS at 18. (Wiegel, Z. phys. Ch. 1907, 58. 294.) Insol. in alkali hydrates, carbonates, and sulphides +Aq. Insol. in NH 4 OH, HC1, or (NH 4 ) 2 CO 3 +Aq. Easily sol. in very 'dil. HC1 and HNO 3 +Aq, but H 2 S ppts. ZnS in pres- ence of very dil. HCl+Aq, or H 2 S0 4 +Aq. (Eliot and Storer.) More easily sol. in HNO 3 +Aq than in HCl+Aq. (Fresenius.) Only si. sol. in acetic acid. (Wackenroder.) When still moist is sol. in H 2 S0 3 +Aq. Insol. in NH 4 C1 or NH 4 NO 3 +Aq. K 2 S+Aq when added to ZnS0 4 +Aq pro- duces a ppt. in presence of fO,000 pts. H 2 O, and a slight opalescence with 20,000 pts. (Lassaigne.) Slowly sol. in cone. KCN+Aq. (Halm, J. B. 1870. 1008.) SI. sol. in Na 2 S+Aq; sol. in NaSH+Aq. (Becker, Sill. Am. J. (3) 33. 199.) Zinc peratasulphide, ZnS 5 . Sol. in acids, with separation of S. (Schiff, A. 116. 74.) Zinc sulphosilicide, ZnSiS. Decomp. by acids and by alkalies. (Fraen- kel, Metall, 1909, 6. 683.) Zinc telluride, ZnTe. Decomp. by acids. Sol. in Br 2 +Aq. (Fabre, C. R. 105. 277.) Zincic acid. Zinc hydroxide shows weak acid properties, and forms the following salts. Ammonium zincate, 3ZnO, 4NH 3 +12H 2 O = 3ZnO, 2(NH 4 ) 2 O+10H 2 O. Decomp. by much H 2 O. . Barium zincate, BaH 2 Zn 2 O 4 +7H 2 O. Decomp. by H 2 O. (Bertrand, C. R. 116. 939.) Calcium zincate, CaH 2 Zn 2 O 4 +4H 2 O. Decomp. by H 2 O. Sol. in NH 4 OH+Aq. (Bertrand, C. R. 115. 939.) Cobaltous zincate, rcCoO, ?/ZnO. Rinman's green. Sol. in acids. H 2 CO 3 +Aq dissolves out ZnO. (Comey.) Potassium zincate, ZnO, K 2 O. Easily sol. in H 2 O, but decomp. by boiling. (Laux, A. 9. 183.) 2ZnO, K 2 O. Decomp. immediately by cold H 2 O. (Fremy, C. R. 15. 1106.) Sodic zincate, Na 2 O, 2ZnO+8H 2 O, or 2NaHZnO 2 +7H 2 O. Decomp. by H 2 O or alcohol. (Comey and Jackson, Am. Ch. J. 11. 145.) +7H 2 O. (Forster and Gunther, Z. Elek- trochem, 1899, 6. 301.) 2Na 2 O, 3ZnO + 18H 2 O or Zn 3 O 6 Na 4 H 2 + 17H 2 O. Decomp. by H 2 O or alcohol. Insol. in ether. (Comey and Jackson.) Strontium zincate, SrH 2 Zn 2 O 4 +7H 2 O. Decomp. by H 2 O. (Bertrand.) Zirconic acid. See Zirconium hydroxide. Barium zirconate, BaZrO 3 . Insol. in acids. (Ouvrard, C. R. 113. 80.) Calcium zirconate, CaZrO 3 . Insol. in acids. (Ouvrard, C. R. 113. 80.) Calcium zirconate, acid. Inscl. in H 2 O or HCl+Aq. (Hiordthal, A. 137. 237.) Calcium potassium zirconate, (Ca,K)LaO 3 (small quantity of CaO substituted by K 2 0). Sol. in HC1. (Venable, J. Am. Chem. Soc. 1896, 18. 444.) Cupric zirconate. (Berthier, A. ch. 59. 195.) ZIRCONIUM IODIDE 1127 Lithium zirconate, Li 2 ZrO 3 . Easily attacked by acids. (Ouvrard, C. R 112. 1444.) Magnesium zirconate. Insol. in H 2 O or HCl+Aq. (Hiordthal C. R. 61. 215.) Potassium zirconate. Decomp. by HCl+Aq. (Knop, A. 169. 44. Sodium zirconate, Na 2 ZrO 3 . Decomp. by H 2 O. Na 4 ZrO 4 . Decomp. by HCl+Aq, and is dissolved by subsequent addition of H 2 O Na 2 O, 8ZrO 2 + 12H 2 O. (Hiordthal.) Strontium zirconate, SrZrO 3 . As CaZrO 3 . (Ouvrard.) Zirconium, Zr. Crystallized. Attacked by cone. HCl+Aq above 50, but very slowly even at 100 rapidly by hot aqua regia. Sol. in cold cone HF+Aq. (Troost, C. R. 61. 109.) Very violently attacked by a mixture of HNO 3 and HF. (Berzelius, Pogg. 4. 117.) Amorphous. Slowly attacked by boiling aqua regia, H 2 SO 4 , or cone. HCl+Aq. (Ber- zelius.) Easily sol. in HF or HNO 3 +HF. Zirconium bromide, ZrBr 4 . Very hygroscopic. Violently decomp. by H 2 O to form oxybromide. (Melliss, Zeit. Ch. (2) 6. 296.) SI. sol. in organic solvents. (Matthews, J. Am. Chem. Soc. 1898, 20. 840.) Zirconium bromide ammonia, ZrBr 4 , 4NH 3 . Ppt. Insol. in organic solvents. (Mat- thews, J. Am. Chem. Soc. 1898, 20. 840.) ZrBr 4 , 10NH 3 . Very hydroscopic. Decomp. by H 2 O. (Stabler, B. 1905, 38. 2612.) Zirconium carbide, ZrC. Insol. in H 2 O and NH 4 OH+Aq and HC1 Aq even when heated. Sol. in HNO 3 , HaSO 4 and fused alkali nitrates, chlorates, or hy- droxides. (Moissan, C. R. 1896, 122. 653.) Zirconium chloride, ZrCl 4 . Sol. in H 2 O with evolution of much heat to form ZrOCl 2 . Sol. in alcohol. (Hinsberg, A. 239. 253.) Very unstable. Probably substances so described in the literature by Nylander and others were oxy- chlorides. (Venable, J. Am. Chem. Soc. 1894, 16. 471.) Sol. in ether. (Matthews, J. Am. Chem. Soc. 1898,20.821.) Zirconium chloride ammonia, ZrCl 4 , 2NHL Fumes in the air. Decomp. by H 2 O. (Matthews, J. Am. Chem. Soc. 1898, 20. 821.) ZrCl 4 , 3NH 3 . (Stabler, B. 1905, 38. 2611.) ZrCl 4 , 4NH 3 . Decomp. by H 2 O. (Pay- kull.) Unstable. Decomp. by H 2 O. (Matthews, J. Am. Chem. Soc. 1898, 20. 821.) ZrCl 4 , 8NH 3 . Stable in the air. Decomp. by H 2 O. Insol. in ether. (Matthews, J. Am. Chem. Soc. 1898, 20. 821.) Very hydroscopic. Decomp. by H 2 O. (Stabler, B. 1905, 38. 2611.) Zirconium fluoride, ZrF 4 . Anhydrous. Insol. in H 2 O and acids. (De- ville, A. ch. (3) 49. 84.) Only si. sol. in H 2 O. 1.388 g. dissolve in 100 cc. H 2 O without hydrolysis. On warming the solution, zir- conium hydrate begins to ppt. out at about 50. (Wolter, Ch. Z. 1908, 32. 606.) +3H 2 O. Sol. in H 2 O, but solution decom- poses on diluting, with pptn. of an insol. basic salt. Sol. in dil. HF+Aq. (Berzelius.) Zirconium fluoride ammonia, 5ZrF 4 , 2NH 8 . (Wolter, Ch. Z. 1908, 32. 607.) Zirconium hydride, ZrH 2 . Not attacked by acids. (Winkler, B. 24. < 873.) Zirconium hydroxide, Zr(OH) 4 . Insol. in H 2 O or alcohol. Sol. in 5000 pts. H 2 0. (Melliss.) Sol. in acids, even oxalic or tartaric acid, when precipitated cold. If precipitated hot, t is slowly dissolved upon heating with cone, acids. Sol. in dil. or cone. min. acids except HI. Readily sol. in oxalic, only si. sol. in acetic acid. Much less sol. when pptd. from hot splu- ion than when pptd. from cold solution. Venable, J. Am. Chem. Soc. 1898, 20. 274.) SI. sol. in (NH 4 ) 2 CO 3 +Aq. Insol. in 2 CO 3 and Na 2 CO 3 +Aq. Insol. in NaOH, OH, and NH 4 OH+Aq. Sol. in (NH 4 ) 2 C 4 H 4 O 6 +NH 4 OH+Aq. In- sol. in NH 4 salts +Aq. Zirconium iodide, ZrI 4 . Fumes in the air. Sol. in H 2 O and acids with violent re- .ction. Decomp. by alcohol. Sol. in abs. ether. SI. sol. in benzene and CS 2 . (Stabler, B. 904, 37. 1137.) Insol. in H 2 O, HNO 3 , HC1, aqua regia, ,nd CS 2 . Sol. in H 2 SO 4 with decomp; unchanged >y boiling H 2 O. (Dennis, J. Am. Chem. *oc. 1896, 18. 678.) 1128 ZIRCONIUM IODIDE AMMONIA Zirconium iodide ammonia, ZrI 4 , 6NH 3 ; ZrI 4 , 7NH 3 ; ZrI 4 , 8NH 3 ; ZrI 4 , 10NH 3 . All above comps. are hydroscopic and lose NH 3 in the air. (Stabler, B. 1905, 38. 2615.) Zirconium nitride. Scarcely attacked by acids, aqua regia, and caustic alkalies. Slowly -decomp. by long contact with H 2 O. (Mallet, Sill. Am. J. (2) 28. 346.) Zr 2 N 3 . Decomp. when heated in the air; sol. in HF; insol. in other min. acids. (Mat- thews, J. Am. Chem. Soc. 1898, 20. 844.) ZrsNp. Decomp. when heated in the air. Sol. in HF; insol. in other min. acids. (Mat- thews, J. Am. Chem. Soc. 1898, 20. 844.) Zirconium oxide, ZrO 2 . When ignited, is insol. in all acids except HF and H 2 SO 4 . SI. sol. in HF; sol. in H 2 SO 4 only when very finely powdered and heated with a mixture of 2 pts. H 2 SO 4 and 1 pt. H 2 O until the H 2 SO 4 volatilises. (Berzelius.) Zirconium peroxide, ZrO 3 . (Cleve, Bull. Soc. (2) 43. 53), or Zr 2 5 ac- cording to Bailey (Chem. Soc. 49. 150). Not attacked by cold dil. H 2 SO 4 +Aq. (Bailey.) Zirconium silicon oxide. Min. Zircon. See Silicate, zirconium. Zirconium oxy-compounds. See Zirconyl compounds. Zirconium phosphide, ZrP 2 . Insol. in dil. or cone, acids and alkalies. SI. sol. in aqua regia. (Gewecke. A. 1908. 361. 85.) Zirconium silicide, ZrSi 2 . Sol. in HF, insol. in other min. acids. Not acted upon by 10% KOH+Aq or NaOH+Aq. Decomp. by fusion with KOH. (Honigs- chmid, C. R. 1906, 143. 225.) Zirconium sulphide. * Insol. in H 2 O. Sol. in HF; slowly sol. in aqua regia. Insol. in HNO 3 , HC1, H 2 S0 4 , or KOH+Aq. (Berzelius.) Insol. in dil. acids. Sol. in cone. HN0 3 + Aq (perhaps an oxysulphide) . (Fremy.) Zirconomolybdic acid. Ammonium zirconomolybdate, 2(NH 4 ) 2 O, ZrO 2 , 12MoO 3 +10H 2 O. Sol. in H 2 O. (Pechard, C. R. 1893, 117. 790.) Potassium zirconomolybdate, 2K 2 O, ZrO 2 , 12MoO 3 + 18H 2 O. Sol. in H 2 O. (Pechard.) Zirconotungstic acid. Ammonium zirconoofecatungstate, 3(NH 4 ) 2 O, ZrO 2 , 10WO 3 + 13H 2 O. Very sol. in H 2 O. Efflorescent. (Hallopeau, Bull. Soc. 1896, (3) 15. 921.) 3(NH 4 ) 2 O, H 2 O, ZrO 2 , 10WO 3 +13H 2 O. Sol. in H 2 0; unstable; effloresces in the air. (Hallopeau.) Potassium zirconotungstate, 4K 2 O. ZrO 2 , WO 3 +20H 2 O. Sol. in hot H 2 O. (Hallopeau.) 4K 2 O, ZrO 2 , 10WO 3 +15H 2 O. More sol. in hot than in cold H 2 O. Sol. in fused alkali carbonates. (Hallo- peau.) Potassium cKzirconocfecatungstate, 4K 2 O, 2ZrO 2 , 10WO 3 +20H 2 O. More sol. in hot than in cold H 2 O. Sol. in fused alkali carbonates. (Hallopeau.) Zirconyl bromide, ZrOBr 2 +3H 2 O. Deliquescent. Decomp. in moist air. Very sol. in H 2 O. .(Venable, J. Am. Chem. Soc. 1898, 20. 324.) +7H 2 O. Sol. in H 2 O. (Melliss.) +8H 2 0. Deliquescent. Decomp. in moist air. Very sol. in H 2 O. (Venable, J. Am. Chem. Soc. 1898, 20. 324.) + 13H 2 O. Deliquescent. Decomp. in moist air. Very sol. in H 2 O. (Venable.) + 14H 2 O. Deliquescent. Decomp. in moist air. (Venable.) Very sol. in H 2 O. (Venable.) ZrBr(OH) 3 +H 2 O, and +2H 2 O. Deliques- cent, and decomp. in moist air. (Venable.) Zirconyl chloride, ZrOCl 2 . Sol. in H 2 O; insol. in HC1. (Venable, J. Am. Chem. Soc. 1894, 16. 475.) +2H 2 Q. (Chauvenet, C. R. 1912, 164. 822.) +3H 2 O. Sol. in H 2 O. (Venable.) d-3.5H 2 O. (Chauvenet, C. R. 1912, 154. 822.) +6H 2 O. (Chauvenet.) Sol. in H 2 O. Insol. in HC1. (Venable.) +4^H 2 O, 6^H 2 O, and 8H 2 O. Efflorescent. Easily sol. in H 2 O and alco- hol. Very si. sol. in cone. HCl+Aq. (Ber- zelius.) +8H 2 O. Sol. in H 2 O. (Venable, J. Am. Chem. Soc. 1898, 20. 321.) Effloresces in the air. ZIRCONYL SULPHIDE 1129 Sol. in H 2 O. Less sol. in HCl+Aq. and nearly insol. in cone. HC1. (Chauvenet, C. R. 1912, 154. 822.) Zr 2 OCl 2 . Sol. in H 2 O and alcohol. (Ende- mann, J. pr. (2) 11. 219.) Not decomp. by H 2 O. Sol. in dil. HC1. (Chauvenet, C. R. 1912, 154. 1236.) +H 2 O. (Chauvenet, C. R. 1912, 154. 1236.) -f 3H 2 O. Decomp. by H 2 O. Sol. in dil HC1. (Chauvenet.) 8ZrO 2 , 7HC1. Sol. in H 2 O. (E.) Zr 2 OCl 6 . (Troost and Hautefeuille, C. R. 73. 563.) Zr 3 OCl 4 =ZrCl 4 , 2ZrO 2 . Insol. in H 2 O. (Hermann.) Zirconyl iodide, ZrOI 2 +8H 2 O. Very sol. in H 2 O and alcohol. Very hydroscopic. ((Stabler, B. 1904, 37. 1138.) ZrI(OH) 3 +3H 2 O. Easily sol. in H 2 O. (Hinsberg, A. 239. 253.) Ppt. SI. sol. in HI+Aq. (Venable, J. Am. Chem. Soc. 1898, 20. 328.) Zirconyl sulphide (?) Decomp. by HNO 3 with separation of S. (Fremy, A. ch. (3) 38. 326.) APPENDIX FORMULAE FOR CONVERTING AREOMETER DEGREES INTO , SPECIFIC GRAVITY. n =no. of degrees on the areometer scale; sp. gr. = specific gravity. Areometer Temp. Liquids heavier than HaO Liquids lighter than HzO 1. Baume. (a) According to Baume' s original directions. For Kquids heavier than H 2 O. Sp. gr. of a solution of 15 pts. NaCl dissolved in 85 pts H 2 O 15 SD - 149 ' 5 s - 145 ' 56 (12 5 \ dj7^ = 1.1118988j = 15; H 2 O = 0. For liquids lighter than H 2 O. Sp. gr. of 10% NaCl+A*q at 12.5 / 12 5 \ fep< gr> " 149.05-n Sp>gr " -135.56+n I 12 5 ~ I " i H 2 O = 10. 145.88 145.88 (6) Old Form. Liquids heavier than H 2 O, 10%NaCl -f Aq-at 15 ( 4JL = 1.073350') 12.5 1^ bp ' gr - 145. 88 -n - 146 ' 3 bp - gr - 135.88+n 146.3 \ 15 1 = 10; H 2 O = 0. Liquids lighter than H 2 O, 10% NaCl fep ' gr - 146. 3-n 146.78 ^^"136.3+71 Sp r 146 ' 78 +Aq ,M 2 O 10 . (c) New Form. So-called " Rational Scale." Liquids heavier than H 2 O, H 2 SO 4 + 1 ^ 17.5 1 K ^^' 146. 78 -n p er 144 ' 3 hp>gr ' 136.78+n Aq-^j = 1.842 = 66; H 2 O = 0. JLo 15 bp>gr ' 144. 3 -n 2. Beck. H 2 O = 0; liquid of 0.850 /I o eo\ 1 - ^O ^r>ala 170 Sn - 17 f- & l '\ 12 5/ ocaie continued above and below. 12.5 . Sp ' gr - 170-n Sp.gr. - 170+n 3. Twaddle. H 2 O = 0. Each degree cor- responds to an increase of 0.005 in the sp. gr. Given on the instru- ment Sp.gr. = 1.000+0.005 1132 APPENDIX TABLES FOR THE CONVERSION OF BAUMfi DEGREES INTO SP. GR. Since the original directions of Baume there have been many slight modifica- tions suggested, so that there are several varieties of Baume hydrometers with somewhat varying readings, tables for the two principal ones of which are here- given. 1. According to Baume's original directions. For liquids heavier than H 2 O. Sp. gr. of 15 % NaCl+ Aq (^ps) = 1.1118988 = 15; H 2 O = 0. 149.05 Calculated according to the formula, sp. gr. = 149.05 -n. Deg. Baum6 Sp. gr. Deg. Baume Sp. gr. Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. .00000 20 . 15497 39 1.35438 58 1.63701 1 .00675 21 . 16399 40 1.36680 59 1.65519 2 .01360 22 1.17316 41 1.37945 60 1.67378 3 .02054 23 . 18246 . 42 1.39234 61 1.69279 4 .02757 24 1.19192 43 1.40547 62 1.71223 5 .03471 25 1.20153 44 1.41885 63 1.73213 6 .04194 26 1.21129 45 1.43248 64 1.75250 7 .04927 27 1.22122 46 1.44638 65. 1.773'35 8 .05671 28 .23131 47 1.46056 66 1.79470 9 1.06426 29 .24156 48 1.47501 67 1.81657 10 1.07191 30 .25199 49 .48971 68 1.83899 11 1.07968 31 .26260 50 .50479 69 1.86196 12 1.08755 32 .27338 51 .52014 70 1.88551 13 1.09555 33 .28436 52 .53580 71 1.90967 14 1.10366 34 .29522 53 .55179 ' 72 1.93446 15 1.11189 35 .30688 54 .56812 73 1.95989 16 1.12025 36 1.31844 55 .58471 74 1.98601 17 1.12873 37 1.33621 56 .60182 75 2.01283 18 1.13735 38 1.34218 57 .61923 76 2.04038 19 1 . 14609 APPENDIX 1133 For liquids lighter than H 2 O. Sp. gr. of 10 % NaCl (12 c i o \ jj^ j = 1.0737665 = 0; H 2 = 10. Calculated according to the formula, sp. gr. = 145.56 135.56+n' Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. 10 1.00000 30 0.87919 50 0.78443 65 0.72577 15 0.96679 35 0.85342 55 0.76385 70 0.70811 20 . 0.93571 40 0.82912 60 0.74432 75 0.69130 25 0.90657 45 0.80616 ; 2. According to the so-called Rational Scale. Sp. gr. of H 2 S0 4 +Aq(j^) = 1.842 = 66 ; H 2 O = 0. 144.3 Calculated according to the formula, sp. gr. 144.3 -n Deg. Baume Sp. gr. Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. Deg. Baum6 Sp. gr. 1 1.007 18 1.142 35 1.320 51 1.547 2 1.014 19 1.152 36 1.332 52 1.563 3 1.021 20 1.161 37 1.345 53 1.580 4 1.029 21 1.170 38 1.357 54 1.598 5 1.036 22 1.180 39 1.370 55 1.616 6 1.043 23 1.190 40 1.384 56 1.634 7 1.051 24 1.200 41 1.397 57 1.653 8 1.059 25 1.210 42 1.411 58 1.672 9 1.066 26 1.220 43 1.424 59 1.692 10 1.074. 27 1.230 44 1.439 60 1.712 11 1.082 28 .241 45 1.453 61 1.732 12 1.091 29 .251 46 1.468 62 1.753 13 1.099 30 .262 47 1.483 63 1.775 14 1.107 31 .274 48 1.498 64 1.797 15 1.116 32 .285 49 1.514 65 1.820 16 1.125 33 .296 50 1.530 66 1.842 17 1.133 34 .308 s 1134 APPENDIX SYNCHRONISTIC TABLE OF CHEMICAL AT*f>V Ch. Year A. A. ch. Am. J. Sci. Ann. Min. Ann. Phil. rcn. Pharm. Gaz. C.R. Dingl. 1800 (1) 32-34 1801 35-39 . .^ 1802 40-43 . . . 1803 44-47 . . . 1804 48-51 1805 52-55 1806 56-60 . . . 1807 61-64 , . . . 1808 65-68 . . . 1809 69-72 1810 73-76 1811 77-80 . . . . . . 1812 81-84 . . . . . . . . . 1 O 1 O OK OO (1} 1 2 1813 oO oo {*-/ *j " QO QO 3 4 1815 93-96 5, 6 1816 (2) 1-3 7, 8 1817 4-6 1 2 9, 10 1818 7-9 3 11, 12 1819 10-12 (ij V 4 13, 14 1820 13-15 2 5 15, 16 1-3 1821 16-18 3 6 (2) 1, 2 4-6 1822 19-21 4, 5 7 3, 4 1 2 . . . 7-9 1823 22-24 6 8 5, 6 3-6 10-12 1824 25-27 7,/8 9 7, 8 7-10 . . . 13-15 1825 28-30 9 10, 11 9, 10 11-14 16-18 1826 31-33 10, 11 12, 13 11, 12 16-19 19-22 1827 34-36 12 (2) 1, 2 20-23 23-26 1828 37-39 13, 14 3, 4 24-26 27-30 40-42 15 16 5 6 27-30 31-34 1830 ^r\J TC^ 43-45 17^ 18 / 7,' 8 31-34 35-38 1831 46-48 19, 20 35-39 39-42 1832 1-4 49-51 21, 22 (3) 1 2 N 40-43 43-47 1833 5-8 52-55 23, 24 Si 4 44-47 48-50 1834 9-12 56-57 25-27 5 6 48-50 51-54 1835 13-16 58-60 28, 29 7; 8 (2) 1-4 1 55-58 1836 17-20 61-63 30, 31 9, 10 5-8 2, 3 59-62 1837 21-24 64-66 32, 33 11, 12 9-12 4, 5 63-66 1838 25-28 67-69 35, 35 13, 14 13-16 _ .6, 7 67-70 1839 29-32 70-72 36, 37 15, 16 17-20 8 9 71-74 1840 33-36 73-75 38, 39 17, 18 21-24 10, 11 75-78 1841 37-40 (3) 1-3 40, 41 19, 20 25-28 12, 13 79-82 1842 41-44 4 7 6 42, 43 (4) 1, 2 29-32 14, 15 83-86 1843 45-48 7-9 44, 45 3, 4 . 33-36 1 16, 17 87-90 1844 49-52 10-12 46, 47 5, 6 37-40 2 18, 19 91-94 1845 53-56 13-15 48-50 7, 8 41-44 20, 21 95-98 1846 57-60 16-18 (2) 1, 2 9, 10 45-48 3 22, 23 99-102 1847 61-64 19-21 3, 4 11, 12 49-52 4 24, 25 103-106 APPENDIX 1135 AND OTHER SCIENTIFIC PERIODICALS Part I. Gilb. Ann. J. Chim. med. J. Pharm. J. pr. N Phil. Mag. Pogg. Proc. Am. Acad. Proc. Roy. Soc. Q. J. Sci. Scher. J. Schw. J. 4-6 6-8 3,4 7-9 9-11 . 5, 6 10-12 12-14 7, 8 . 13-15 15-17 9, 10 16-18 18-20 12, 12 19-21 21-23 13, 14 22-24 . ... 24-26 15, 16 25-27 . . 27-29 . 17, 18 . 28-30 30-32 19, 20 31-33 (1) 1 33, 34 21, 22 34-36 \^/ 2 35, 36 23, 24 37-39 _ 3 37, 38 Cont. as d)'i-3 40-42 4 39, 40 Schw. J. 4-6 43-45 5 41, 42 7-9 46-48 6 43, 44 10-12 49-51 (2) 1 45, 46 . * . 13-15 52-54 2 47, 48 I i 16-18 55-57 3 49, 50 2, 3 19-21 58-60 4 51, 52 4, 5 . . 22-24 61-63 5 53, 54 6, 7 . . . 25-27 64-66 6 55, 56 . . 8, 9 28-30 67-69 7 57, 58 10, 11 (2) 1-3 70-72 8 59, 60 12, 13 4-6 73-75 9 61, 62 t 14, 15 7-9 76 10 63, 64 i,"2 16, 17 10-12 Cont. as (i) i ,11 65, 66 3-5 . '. '. 18, 19 13-15 Pogg. 2 12 67, 68 6-8 20, 21 16-18 3 13 (2) 1, 2 9-11 . . 19-21 4 14 3, 4 12-14 22-24 5 15 5 6 15-17 25-27 6 16 7, 8 18-20 28-30 7 17 9. 10 21-23 (3) 1-3 8 18 11, (3) 1 24-26 'i' 4-6 9 19 2, 3 27-30 'i' 2 7-9 10 20 1-3 4, 5 31-33 Cont. as (2) 1 21 4-6 6, 7 34-36 . . . . . J. pr. 2 22 7-9 8, 9 37-39 . . . . 3 23 10-12 10, 11 40-42 '3' . . . 4 24 13-15 12, 13 43-45 . . . 5 25 16-18 14, 15 46-48 6 26 19-21 16, 17 49-51 . 7 27 22-24 18, 19 52-54 8 (3) 1, 2 25-27 20, 21 55-57 4 3 4 28-30 22, 23 58-60 t7 10 o, < 5 6 31-33 24 ? 25 61-63 J-vJ (3) 1 J, U 7, 8 34-36 26, 27 64-66 . . . . . . 2 9, 10 37-39 28, 29 67-69 2' . . . . Q ni2 40-42 30, 31 70-72 o 7 1136 APPENDIX SYNCHRONISTIC TABLE OF CHEMICAL AND Year A. A. ch. Am. Ch. J. Am. J. Sci. Analyst. Ann. Min. Arch. Pharm. A. suppl B. Bull. Soc. 1848 65-68 22-24 5, 6 13, 14 53-56 1849 69-72 25-27 7, 8 15, 16 57-60 1850 73-76 28-30 9, 10 17, 18 61-64 1851 77-80 31-33 11, 12 39, 20 65-68 1852 81-84 34-36 13, 14 (5) 1, 2 69-72 1853 85-88 37-39 15, 16 3,4 73-76 1854 89-92 40-42 17, 18 5, 6 77-80 1855 93-96 43^5 19, 20 7, 8 81-84 1856 97-100 46-48 21, 22 9, 10 85-88 1857 101-104 49-51 23, 24 11, 12 89-92 1858 105-108 52-54 25, 26 13, 14 93-96 1859 109-112 55-57 27," 28 15, 16 97-100 i 1860 113-116 58-60 29, 30 17, 18 101-104 2 1861 117-120 61-63 31, 32 19, 20 105-108 1 3 1862 121-124 64-66 33, 34 (6) 1, 2 109-112 2 4 1863 125-128 67-69 35, 3(5 3; 4 113-116 5 1864 129-132 (4) 1-3 37,^ 38 5, 6 117-120 3 (2) 1, 2 1865 133-136 4-6 39, 40 7, 8 121-124 4 3, 4 1866 137-140 7-9 41, 42 9, 10 125-128 5, 6 1867 141-144 10-12 43, 44 11, 12 129-132 5 7, 8 1868 145-148 13-16 45, 56 13, 14 133-136 6 1 9, 10 1869 149-152 16-18 47, 48 15, 16 137-140 2 ' 11, 12 1870 153-156 19-21 49, 50 17, 18 141-144 y 3 13, 14 1871 157-160 22-24 ... (3) 1, 2* 19, 20 145-148 4 15, 16 1872 161-164 25-27 3, 4 (7) 1, 2 149, 150 's 5 17, 18 (3) It 1873 165-170 28-30 5, 6 3, 4 2,3 6 19, 20 1874 171-174 (5) 1-3 7, 8 5, 6 4,5 7 21, 22 1875 175-179 4-6 9, 10 7, 8 6,7 8 23, 24 1876 180-183 7-9 11, 12 d 9, 10 9 8,9 9 25, 26 1877 184-189 10-12 13, 14 2 11, 12 ^Jy *J 10, 11 10 27,' 28 1878 190-194 13-15 . . 15, 16 3 13, 14 12,13 11 29, 30 1879 195-199 16-18 1 17, 18 4 15, 16 14,15 12 31, 32 1880 200-205 19-21 2 19, 20 5 17, 18 16, 17 13 33, 34 1881 206-210 22-24 3 21, 22 6 19, 20 18, 19 14 35, 36 1882 211-215 25-27 4 23, 24 7 8) 1, 2 20 15 37, 38 1883 216-221 28-30 5 25, 26 8 34 21 16 39, 40 1884 222-226 (6) 1-3 6 27, 28 9 5, 6 22 17 41, 42 1885 227-231 4-6 7 29, 30 10 7, 8 23 18 43, 44 1886 232-236 7-9 8 31, 32 -11 9, 10 24 19 45, 46 1887 237-242 10-12 9 33, 34 12 11, 12 25 20 47 J 48 1888 243-249 13-15 10 35, 36 13, 14 13, 14 26 21 49' 50 1889 1890 250-255 256-260 16-18 19-21 11 12 37, 38 39, 40 15, 16 17, 18 15, 16 17, 18 27 228 22 23 3) 1, 2 3 4 1891 1892 1893 1894 261-266 267-271 272-277 278-283 22-24 25-27 28-30 7) 1-3 13 14 15 16 41, 42 43, 44 45, 46 47, 48 19, 20 21, 22 23, 24 25, 26 19, 20 9)1, 2 3, 4 5, 6 229 '230 231 232 24 25 26 27 9 5, 6 7, 8 9, 10 11, 12 1895 284-289 4-6 17 49, 50 27, 28 7, 8 233 ... 28 13', 14 * Also cited as whole series, 101, 102, 103, etc. F AJso cited as 201, 202, etc. APPENDIX 1137 OTHER SCIENTIFIC PERIODICALS Part II. c. c. Chem. Ind. Chem. Soc. Ch. Gaz. Ch. Ztg. Cim. C. N. C. R. Dingl. Gazz. ch. it. J. Am. Chem. Soc. J. Anal. Ch. ... ... 5 ... ... 26, 27 107-110 . ' V 6 . . 28, 29 111-114 . . . 2 7 30, 31 115-118 . . 3 8 32, 33 119-122 . . . . . 4 9 1,'2 34, 35 123-126 . 5 10 3, 4 36, 37 127-130 . . . 6 11 5, 6 38, 39 131-134 . . 7 12 Cont. . 40, 41 135-138 1 . 8 13 . asN. . 42, 43 139-142 2 9 14 Cim. 44, 45 143-146 3 10 15 46, 47 147-150 4 11 16 48, 49 151-154 5 12 17 . i, 2 50, 51 155-158 6 . . 13 Cont. . . . 34 52, 53 159-162 . . 7 14, 15 as 5, 6 54, 55 163-166 8 ie* C. N. 7,- 8 56, 57 167-170 9 17 . 9, 10 58, 59 171-174 10 . 18 . . . 11, 12 60, 61 175-178 . . 11 . 19 . 13, 14 62, 63 179-182 . 12 20 15, 16 64, 65 183-186 13 21 17, 18 66, 67 187-190 14 22 . .9, 20 68, 69 191-194 15 . 23 . . . . 21, 22 70, 71 195-198 . . . 16 24 . 23, 24 72, 73 199-202 "i 17 ... 25 25, 26 74, 75 203-206 2 ... ... 18 26 ,...( ... ... 27, 28 76, 77 207-210 3 19 27 . . 29, 30 78, 79 211-214 4 . . 20 28 31, 32 80, 81 215-218 5 21 29, 30 33, 34 82, 83 219-222 6 22 31, 32 . i . . . 35, 36 84, 85 223-226 7 23 i 33, 34 . 2 37, 38 86, 87 227-230 8 24 2 35, 36 3 39, 40 88, 89 231-234 9 "l 25 3 37, 38 4 41, 42 90, 91 235-238 10 2 26 4 39, 40 5 . . 43, 44 92, 93 239-242 11 3 27 5 41, 42 . 6 . . . 45, 46 94, 95 243-246 12 4 28 6 43, 44 7 47, 48 96, 97 247-250 13 5 29 7 45, 46 8 49, 50 98, 99 251-254 14 6 30 8 47, 48 9 51, 52 100, 101 255-258 15 7 31 9 49, 50 . 10 . . . 53, 54 102, 103 259-262 16 8 32 10 51, 52 11 55, 56 104, 105 263-266 17 9 i 33 11 53, 54 12 57, 58 106, 107 267-270 18 10 2 34 12 55, 56 13 59, 60 108, 109 271-274 19 11 3 35 13 57, 58 14 . . 61, 62 110, 111 275-278 20 12 4 36 14 59, 60 . . 15 . . . 63, 64 112, 113 279-282 21 13 5 37 15 61, 62 16 65, 66 114, 115 283-286 22 14 6 38 16 63, 64 17 67, 68 116, 117 287-290 23 15 7 39 17 65, 66 . 18 . . 69, 70 118, 119 291-294 24 16 40 18 67, 68 19 71, 72 120, 121 295-298 25 17 ... * Also cited as (2) 1, 2, 3, etc. 1138 APPENDIX SYNCHRONISTIC TABLE OF CHEMICAL AND Year J. Chim med. Jena. Zeit. J. Pharm. J.pr. J. Russ Soc. J. Soc Chem Ind. M. Ch Monit Sclent N. Cim. N.Rep Pharm Pharm J. Trans Phil. Mag. 1848 4 13 14 43-45 32 33 1849 5 ***> * * 15 16 ' . J-vj 46-48 34, 35 1850 6 17 18 49-51 36, 37 1851 7 j. i , j.t> 19 20 52-54 (4)1 2 1852 8 21 22 -i , 55-57 1 \*/"f ** 3 4 185< 9 23 24 58-60 2 o, i 5 6 185^ 10 AM, ^^t 25, 26 61-63 3 J, U 7 8 1855 (4)1 27, 28 64-66 . . . ' 1,2 4 , 9, 10 1856 2 29,30 67-69 y ... . ' m ' t " 3,4 5 11, 12 1857 3 31,32 70-72 d)i 5,6 6 13, 14 1858 4 33,34 73-75 2 7,8 7 15, 16 1859 5 35,36 76-78 . 3 9, 10 8 17, 18 1860 6 37, 38 79-81 s3 . ;.-.' . . 4 11, 12 9 19, 20 1861 7 39, 40 82-84 13 14 10 21 22 1862 8 41, 42 85-87 j-o, x ^ 11 23' 24 1863 9 **J ** 43, 44 88-90 5 12 25^26 1864 10 1 45, 46 91-93 (2)6 13 27,28 1865 (5)1 . (4)1, 2 94-96 7 14 29, -30 1866 2 2 3,4 97-99 v ? ! 8 15 31, 32 1867 3 3 5,6 100-102 ' * J. . 9 16 33, 34 1868 4 4 7,8 103-105 ~'f ! ' 10 17 35,36 1869 5 9,10 106-108 1 11 18 37,38 1870 6 5 11,12 2)1,2 2 12 19 39,40 1871 7 6 13, 14 3,4 3 3)13 20 (3) 1 41, 42 1872 8 15, 16 5,6 4 flfi-l- '. 14 21 2 43,44 1873 9 7 17, 18 7, 8 5 15 22 3 45,46 1874 10 8 19,20 9, 10 6 16 23 4 47,48 1875 11 9 21, 22 11, 12 7 17 24 5 49,50 1876 12 10 23,24 13, 14 8 18 6 5)1, 2 1877 110 25,26 15, 16 9 19 7 3, 4 1878 12 27,28 17, 18 10 20 8 5, 6 1879 13 29,30 19, 20 11 g 21 9 7, 8 1880 14 5)1,2 21, 22 12 "l 22 10 9, 10 1881 15 3,4 23, 24 13 2 23 11 11, 12 1882 5,6 25, 26 14 i 3 24 12 13, 14 1883 16 7,8 27, 28 15 2 4 25 13 15, 16 1884 17 9, 10 29, 30 16 3 5 26 14 17, 18 1885 18 11, 12 31, 32 17 4 6 27 15 19, 20 1886 19 13, 14 33, 34 18 5 7 28 16 21, 22 1887 20 15, 16 35, 36 19 6 8 29 17 23, 24 1888 21 17, 18 37, 38 20 7 9 30 18 25, 26 1889 22 19,20 39, 40 21 8 10 31 19 27, 28 1890 23 21,22 41, 42 22 9 11 32 20 29, 30 1891 24 23, 24 43, 44 23 10 12 33 21 31, 32 1892 25 25,26 45, 46 24 11 13 34 22 33, 34 1893 26 27,28 47 > 48 25 12 14 35 23 35, 36 1894 27 29, 30 49, 40 26 13 15 36 24 37, 38 1895 28 6)1,2 51, 52 27 14 16 37 25 39, 40 APPENDIX 1139 OTHER SCIENTIFIC PERIODICALS Part II. Continued. Pogg. Proc. Am. Acad. Proc. Roy. Soc. Rep. Anal. Ch. R. t. c. 'echn. J.B. W. A. B. w. Ann. Z. anal. Z. an c g r Z. anorg. Zeit. Ch. z. p c r 73-75 76-78 79-81 82-84 85-87 88-90 91-93 94-96 97-99 100-102 103-105 106-108 109-111 112-114 115-117 118-120 121-123 124-126 127-129 130-132 133-135 136-138 139-141 142-144 145-147 148^150 151-153 154-155 157-159 160 Cont. as W.Ann 3 4 ... 1 2,3 4, 5 5 6,7 8,9 10, 11 12-14 15-18 19-21 22-27 28-33 34-38 39-42 43 44, 45 46-48 49 50-52 53,54 55,56 57,58 59, 60 61,62 63,64 65, 66 67,68 69,70 71,72 73, 74 75,76 77,78 79,80 81, 82 83,84 85,86 78," 88 89,90 91, 92 93,94 95,96 97,98 99, 100 101, 102 103, 104 105, 106 107, 108 109, 110 111 "5 6 "7 8 6 '- 8 9 10 'll 12 13 14 . . . ... (i) i 2 3 4 5 6 7 8 9 10 11 12 13 14 15 (2)1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 (1)1 2 3 4 5 ... ... 1 2 3 4 5 6 7 ... ... 6 (2)1 2 3 4 ... 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 15 16 17 18 19 20 21 22 23 24 25,26 27 28,29 30 31,32 33 34, 35 36,37 38,39 40,51 42,43 44,45 46,47 48,49 50 51, 52 53, 54 55,56 57,58 1 2 3 4 5 6 7 Cont. as Z. angew 1 2 3 4 5 6 7 8 9 10 11 12 13 14 1,'2 3-5 6-8 9-11 12-14 15-17 18-20 21-23 24-26 27-29 30-32 33-35 36-38 39-41 42-44 45-47 48-50 51-53 54-56 8 9 10 11 12 13- 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 5 6 7 iii . ... 1 2 3 4 5 6 7 8 6 -i 2 3,4 5,6 7,8 9,10 11, 12 13, 14 15, 16 1,2 3, 4 5^-7 8-10 . . . 1140 APPENDIX SYNCHRONISTIC TABLE OF CHEMICAL AND Year A. A. ch. Am. Ch. J. Am. J. Sci. Arch. Phann. B. Bull. Soc.